摘要:

J O U R N A L H. BAKER. CHICHESTEB H. BELL, M.B. D. BENDIX. C. H. BOTHAMLEY. B. H. BBOUBH. C. F. CROSS. A. H. FISON. J. FLETCHER. W. D. HALLIBUBTON, M.D., B.So. J. P. Laws. D. A. LOUIS. T. MAXWELL, M.D., B.Sc. N. 'IT. J. MILLER, Ph.D. G. H. MORRIS, Ph.D. OF J. M. H. MUNBO, D.Sc. A. PHILIP. E. W. PREVOST, Ph.D. R. ROUTLEDBE, B.Sc. M. J. SALTER. C. SPURGE, B.A. JAMES TAYLOR, B.Sc. A. THILLOT. L. T. THOBNE, Ph.D. H. I(. TOMPKINS, B.Sc. V. H. VELEY, M.A. W. 0. WILLIAMS, B.Sc. W. P. WYNNE, B.Sc. THE CHEMICAL SOCIETY. H. E. ARMSTBONG, Ph.D., F.R.S. W. CBOOKES, F.R.S. F. R. JAPP, M.A., Ph.D., F.R.S. A. I(. MILLER, Ph.D. HUGO MULLEB, Ph.D., F.R.S. W. H. PERKIN, Ph.D., F.R.S. S. U. PICKERINB, M.A. R. T. PLIMPTON, Ph.D. W. J. RUSSELL, Ph.D., F.R.S. J. MILLAR THOMSON, F.R.S.E. T. E.THOBPE, Ph.D., F..R.S. &bitrrr : C. E. GROVES, F.R.S. Sttb-6bitar : A. J. GBEENAWAY. VOl. LII. I 8 8 7. ABSTRACTS. LONDON: J. V A N V O O R S T , 1, P A T E R N O S T E R ROW. 1887.LONDON : HARRISON AND SONS, PBINTERS IN ORDINARY TO HER MAJESTY, ST. MARTIN’S LAKE.C 0 N T E N T S. ABSTRACTS OF PAPERS PUBLISHED IN OTHER JOURNALS :- General and Physical Chemistry. PAGE STROUXBO. Production of White Light by E x i n g the Colour~ of the Spectrum . LIEBEPMANN (C.) and S. v. KOSTANECKI. Spectra of the Methyl-derivatives of Hydrox anthraquinone . VERNEUIL (AJ. Preparation of Calcium Sulphide with a Violet Phos- ' phorescence . BOISBAUDRAN (L. DE). Fluorescence of Manganese Compounds . BOISBAUDRAN (L. DE). Fluorescence of Bismuth Compounds . LUVINI (J.).Electrical Conductivity of Gases and Vapours . WINKELMANN (A,). Relation of the Conductive Capacity of Gases to Tem- perature. GRAETZ (L.). Electrical Conductivity of Solids at High Pressures . SCHIFF (R.). Speciflc Heats of Homologous Series of Liquid Organic Com- pounds . BLAREZ (C.). Saturation of Normal Arsenic Acid with Barium Hydroxide . BLAREZ (C.). Saturation of Arsenic Acid with Calcium and Strontium Oxides . , . DE FORCRAND. Sodium Glycerolate . SCHIFF (R.). Heat of Evaporation of Homologous Carbon Compounds . MEISSNER (F.). Heat evolved when Powders are Moistened . ZEHNDER (L.). Determination of the Sp. Gr. of Soluble Substances . BERTHELOT and ANDR~. Tension of Dissociation of Ammonium Hydrogen Carbonate . BERTHELOT and ANDRS. Decomposition of Ammonium Hydrogen Carbo- nate by Water, &c.DUCLAUX (E.). Chemical Changes produced by Sunlight . EDER (J. M.). Practical Methods of Photographing the Spectrum . HABERMA" (J.). Electrolysis of Carbon Compouuds . BERTHELOT. Thermochemistryof Phosphates . GAL (H.) and E. WEBNEB. Heat of Neutralisation of Homologous and Isomeric Acids . GAL (H.) and E. WERNER. Heats of Neutralisation of Malonic, Tartronic, and Mdic Acids . BERTHELOT. Thermochemistry of Reactions between Magnesia Salta and Ammonia . . STOHMANN (F.), P. RODATZ, and H. HERZBEPG. Heats of Combustion and Formation of Homologous Phenols . DE LANDERO and R. PRIETO. Some Laws of Chemical Combination . HUNT (T. S.). Law of Volumes in Chemistry . LESCCEUR (H.). Velocity of Dissociation . RAMSAY (W.) and S. YOUNQ.Nature of Liquids . TBAUBE (J.). Capillary Constants and Meniscus Angle . GUIGNET (C. E.). Crystallisation by Diffusion . TREY (H.). Influence of some Normal Salts on the Hydrolysis of Methyl Acetate . DIXON (H. B.). Preservation of Gases over Mercury . a 2 1 1 2 3 4 a 5 5 6 9 8 8 9 9 9 10 11 93 93 94 94 95 96 96 98 99 99 100 100 101 101 102 105iv CONTENTS. BECKMANN (E.). Cracking Glass with Certainty. WALTER (J.). Apparatus for Chemical Laboratories . DUCLAUX (E.) . Actinometr? . BOISBAUDRAN (L. DE). Fluorescence of Manganese and Bismuth . BECQUEREL (E.). Effect of Manganese on the Phosphorescence of Calcium Carbonate . BOISBAUDRAN (L. DE). Red Fluorescence of Alumina. BECQUEREL (E.). Phosphorescenee of Alumina . BRUHT, (J. W.). Molecular Refraction of Liquid Organic Compounds of High Dispersive Power .BRUHL (J. W.). Experimental Examination of the Older and More Recent Dispersion Formuh . THOMSEN (J.). Supposed Influence of Multiple Bonds of Union on the Molecular Refraction of the Hydrocarbons . BRUHL (J. W.) . Thomsen’s Supposed Explanation of Molecular Refraction Relations . PELLAT (H.). Absolute Electrodynamometer . ELOBUKOFF (N. v.). New Appamtus for Electrochemical Investigations . PIONCHON. JOLY (A.). Thermochemistry of Bibasic Phosphates and their Congeners . BERTHELOT. Ammoilium Magnesium Phosphate. BLAREZ (C.). Saturation of Arsenic Acid by Magnesia. Formation of Ammonium Magnesium Arsenate . , . DE FORCRAND. Heat of Formation of Potassium Methoxide and Ethoxide . GAL (H) and E. WERNER. Heats of Neutralisation of Glyceric and Camphoric Acids .GAL (H.) and E. WERNER. Heats of Neutralisation of Malic and Citric Acids . GAL (H.) and E. WEXNER. Heats of Neutralisation of Meconic and Mellitic Acids. KAHLBAUM (G. W. A.). Temperature Regulator. EAHLBAUM ((3. W. A.). Influence of Atmospheric Pressure on Boiling KAHLBAUM (G. W. A:). Boiling Points of t i e Fa’tty Acids C,H,O, td. RAOULT (E.). Vapour-tensions of Ethereal Solutions . EAHLBAUM (GI.. W. A.). Apparatus for measuring the Tension of Vapours . MULLER-ERZBACH (W.). Dissociation of Salts containing Water of Crystal- lisation . MULLER-ERZBACH (W.). Dissociation of Copper Sulphate . LESC~UR (H.). The Relation between the Efflorescence and Deliquescence of Salts and the Maximum Vapour-tensions of their Saturated Solutions .MCGREGOR (J. G.j. Density of Weak Aqueous Solutions of Salts . TOMLINSON (C.). Cohesion and Submemion Figures . TEAUBE (J.). Weight of Drops and their Relation to Capillarity . DELACHABLONNY (P. M.). Tolatillsation of Dissolved Substances during the Evaporation of the Solvent . SPRING (W.). The Periodic Law. COBNU (M. A.). Distinction been Spectral Lines of Solar and Terrestrial Origin . KOBB (G.). Spectrum of Germanium . WEISS (A.). Fluorescence of the Pigments of Fungi . EALISCHER (M.). New Secondary Element . LAURIE (A. P.). Electromotive Force of a Constant Cell with Moving Plates LAURIE (A. P.) . Electromotive Force of a Voltalc Cell having an Aluminium Plate as Electrode . MENDENHALL (T. C.). Electrical Resistance of Soft Carbon under Pres- sure .I . Specific Heats and Changes of State a t High Temperatures Point . CSHlo02. - . - . PAGE 105 105 189 189 190 191 191 191 195 198 200 200 200 201 202 202 204 204 205 205 206 206 206 207 207 207 207 208 208 209 209 210 21 1 211 313 313 314 314 314 315 315COSTENTS. GRAY (T.). Electrolysis of Silver and Copper : Application of Electrolysis to the Standardising of Electric Current and Potential Meters . FROMME (C.) . Electrolytic Polarisation produced by Small Electromotive Forces . AYRTON (W. E.) and J. PERRY. Expansion of Mercury between 0" and -39" . DE FORCRAND. Heats of Formation of Potassium Alkyl Oxides. DE FORCRAND. Heat of Formation of Sodium Alkyl Oxidea . DE FOECRAND. Potassium Glycerolate. RAMSAY (W.) and S. YOUNG. Thermal Properties of Ether .NICOL (W. W. J.). Vapour-pressures of Water from Salt Solutions . LESC(EUR (H.). Vapour-tension of Sodium Acetate . STEFAN (J.). Relation between the Theories of Capillarity and of Evaporrt- tion . OSTWALD (W.), Coefficients of Affinity of Bases. LEMOINE ((3.). Influence of Heat on the Decomposition of Oxalic Acid by Ferric Chloride . HOOD (J. J.). Theory of Fractional Precipitation . MEYER (L.). Halogen Carners . WILLGEEODT (C.). Halogen Carriers .. WILLGERODT (C.). Indium and Gallium as Halogen Carriers . AYRTON (W. E.) and J. PERRY. BOISBAUDRAN (L. DE). Red Fluorescence of Alumina. BECQKTEBEL (E.). Phosphorescence of Alumina . LOMMEL (E.). Phosphorescence . DUCLAUX (E.). Comparative Action of Heat and Solar Radiation . ROWLAND (H. A.). Water Battery . HARDING (5.L.). Sodium Uichromate Cell. WARREN (H. N.). Ferric Chloride as an Exciting Agent for Voltaic Batteries . NEGREANO. Specific Inductive Yower of Liquids. EBELING (A.). Electromotive Force of some Thermo-elements . STREINZ (F.). Galvanic Polarisation of Aliiminium . ARBHENIUS (5.). Conductivity of Mixtures of Aqueous Solutions of Acids. BLOWN (J.). Theory of Voltaic Action . DRAKE (D.) and J. M. GRAHAM. Electric Accumulators . JANEEEK (G.). LANGCLOIS (M.). Specific Heats of Liquids . COLSON (A.). Isomerism of Position . ARMSTRONG (H. E.). Determination of the Constitution of Carbon Com- pounds from Therrno-chemical Data . PICKERING (S. U.). Determination of the Constitution of Carbon Compounds from Thermo-chemical Data . BLUHL (J. W.). Criticism of Thomsen's Theory of the Heat of Formation of Organic Compounds .STOHMANN (F). Thomsen's Investigations . DE FORCRAND. Alcoholates of Sodium Glyceroxide . DE FORCRAND. Alcoholates of Potasbium Glyceroxide. STORMANN (B'.), P. RODATZ, and w. HEXzlsERG. Heat Equivalent of the Homologues of Benzene. STOHMANN (F.), P. RODATZ, and W. HERZBERG. Heat Equivalent of Ethers of the Phenol Series . THORPE (T. E.) and A. W. RUCKER. Relation between the Critical Tem- peratures of Substances and their Thermal Expansion as Liquids . BABTOLI (A.) and E. STRACCIATI. Relation between the Critical Tempera- tures of Siibstances and their Thermal Expansion as Liquids . THRELFALL (R.). Specific Heate of the Vapours of Acetic Acid and Nitrogen Tetroxide . , . RAMSAY (W.) and S. YOUNG. Influence of Change of Condition from the Expansion produced by Amalgamation Determination of Atomic Weight from Specific Heat .v PAGE 316 317 317 318 319 320 320 321 322 3 23 324 324 325 326 326 326 327 409 409 410 41 1 412 412 413 413 414 41 5 41 5 417 418 419 419 420 420 42 3 423 425 426 427 427 428 429 429 429 Liquid tb the Solid State on Vapour-pressure " . 430vi ONTENTS . RAMSAY (W.) and S . YOUNQ . Nature of Liquids aa shown by a Study of the Thermal Properties of Stable and Dissociable Substances . DYSON ((3.). Apparatus for Determining Vapour-densities . LE CHATELIER (H.). Thermodynamics and Chemistry . WROBLEWSKI (S . v.). BLUMCKE (A.). Specific Gravities of Mixtures of Ethyl Aicohoi and Carbonic Anhydride . MULLER-ERZBACH (W.). Dissociation of Sodium Phosphate .BEAUN (F.)- Solubility of Solid Substancee arid the Changes in Volume and Energy accompanying Solution . COLEMAN (J . J.). Liquid Diffusion . LOEW (0.). Catalytic Actions . THOMSEN (T.). Conditions of Equilibrium in Aqueous Solutions : Action of Aqueous Soda on some Normal Sodium Salts . VALENTINI (A.). Lecture Experiments . DEMARQAY (E.). Spark Spectra from Coils at Low Tension . BECQUEREL (H.). Variations in the Absorption Spectrum of Didymium . BOISBAUDRAN (L . DE) . Red Fluorescence o€ Alumina . VERNEUIL (A.). Phosphoreswnce of Calcium Sulphide . BECQUEREL (E.) Phosphorescence of Calcium Sulphide . GERNEZ (D.). Rotatory Power of Compounds formed in Solutions of Tartaric Acid . BOROHERS (W.). Galvanic Element . GOUY . Standard Galvanic Cell . FEOMIKE (C.).Galvanic Polarisation produced by Feeble Electromotive Forces . DE FORCRAND . Action of Ethylene Bromidi on kkyl'Metklic dxides . GUNTZ . Heat of Formation of Tartar Emetic . HORSTMANN (A.). Molecular Volumes . ENGEL (R.). Solubility of Sulphates . PARMENTIER (F.). A Particular Case of Solution . CHANCEL (G.) and F . PAEMENTIER . Solubility of Calcium Orthobutyrate LE CHATELIER (H.). Laws of Solution . CHROUSTCHOFF (P.) and A . MARTINOFF . Coe5cients of Chemical Affinity . OLSZEWSKI (K.). Absorption Spectrum of Liquid Oxygen and of Atmo- spheric Air . BOISBAUDRAN (L . DE) . Red Fluorescence of Alumina . NASINI (R.). Molecular Refraction of Carbon Compounds . MANEUVRIEB ((3.). Formation of the Electric Arc without Contact OE the Electrodes . GRIMALDI ((3 . P.).Thermic Expansions of Liquids at Various Pressures . CHAPPUIS (J.). Latent Heat of Vaporisation of certain Volatile Sub- stances . BEETHELOT and RECOURA . The Calorimetric Bomb . MVLLEB-ERZBACH (W.) . Dependence of Chemical Affinity on Temperature ROOZEBOOM (H . W . B.). Thermal Study of Hydrobromic Acid Solutions ROOZEBOOM (H . W . B.). Conditions of Equilibrium of Two Substances in the Solid, Liquid, and Gaseous Stakes . Isopyknics . and Isobutyrate . and Hydrate . ROOZEBOOM (H . W . B.). ROOZEBOOM (H . W . B.). New Hydrate of Hydrobromic Acid The Hydrate HBr, 2H20 . ROOZEBO?M (H . W . B.). Combination of Ammonium Bromide with Am- monia . RAOULT (F . M.). Influence of Concentration on the Vapour-tension of Ethereal Solutions . BOTT (W.) and D . S . MAONAIR .Apparatus for Determining Vapour- densities . CHANCEL (G.) and F . PAEMENTIEX . Variation of Solubility with Variation of Heat of Solution . PAGB 430 431 431 432 435 436 436 440 44-43 440 442 537 53'7 538 539 540 54.4) 541 541 541 544 544 645 546 547 547 548 548 625 625 626 626 626 62'7 627 628 628 629 630 631 631 631 632 632CONTENTS . v ii ENGCEL (R.). Effect of Nitric Acid on the Solubility of Nitratm . HAGEMANN (G . A.) . Aviclity-formula . ROSENFELD (M.). Lecture Experiment : Electrolysis oi? Hydrochloric Acid . SCHALL (C.). Lecture Experiment : SpecXc Heat of Zinc . Constant Gas Generator . STENGEB (F.). Absorption-bands of Chlorophyll . EALISCHER (S.). Electromotive Force produced by Light in Selenium . OLSZEWSKI (K.). Density of Liquefied Methane, Oxygen, and Nitrogen .THOMSEN (J.) . Avidity-formula . SLEENBUCH ((3.). WARREN (T . T . P . B.). Vapour-density Apparatus SCHALL (C.). Determination of Vapour-densities . AMAGAT (E . H.). Expansion and Compressibility of Water . SCHUMANN (M.). Compressibility of Aqueous Chloride Solutions . MULLEE-EBZBACH (W.). Rate and Vapour-tension of Diseociation . FOUSSEREAU ((3.) Effect of Pressure on the Decomposition of Chloridea . RUGHEIMEE (L.) . Practical Thermo-regulator . . Refractive Index of Ice . CHAPPUIS (J.) and C . RIVI~BE . Refractive Index and Compressibility of Cyanogen . NASINI (R.) and A . SCALA . Molecular RefracOive Energies o€ Derivatives of NASINI (R.) and A . SCALA . Molecular Refractive Energies of Thiocyanates and Thiocarbimides . BOISBAUDBAN (L . DE) .Red Fluorescence of Chromiferous Gallium . PRIBRAM (R.). Specifh Rotation of Optically Active Substances in very Dilute Solution . TOMASSI (D . and RADIGUET . Electric Couple with Carbon Element8 . KROUCHKOLL . BOUTY (E.). Conductivity of Acids and Salt6 in Dilute Solutions . BOCK (0.). Conductivity of Compounds of Potassium and Sulphur in Solu- tion. of Sodium Sulphide. and of Boric Acid . ECSAS (A.). Nobili’s Rings and Allied Electrochemical Phenomena . FA^ ((3.). Variations in the Electrid Resistance of Antimony and Cobalt in a Magnetic Field . NICOL (W . W . J.). Expansion of Salt Solutions . BEBTHELOT and C . FABEE . Tellurium . THOMSEN (J.). Heats of Combustion of Organic Substances . BERTHELOT and RECOUBA . Heats of Combustion . BEBTHELOT and LOUQUININE .Heats of Comhustion . RAMSAY (W.) and S . YOUNG . Continuous !lhansition from the Liquid to CHAPPUIS (J.) and C . RIVI~RE . Vapour-tension of Liquid Cyanogen . MACNAIB (D . S.). Apparatus for Vapour-density Determinations . MULLER-EEZBACH (W.). Hydrates of Barium and Strontium Hydroxides . SCHULZE (C . R.). Amount of Water of Crystallisation contained in some Salts . FOUSSEREAU (G.). Decomposition of Acetates by Water . REICHER (L . T.). Velocity of 8aponification . MILLS (E . J.). Action of Heat on Potassium Chlorate and Perchlorate . UBECH (F.). Influence of Temperature on the Rate of Inversion of Cane- sugar . UBECH (F.). Velocity of Chemical Reactions . SCHALL (C.) Demonstration of Avogadro’s Hypothesis . MEYER ((3.). Carbon Bisulphide . EETTELER (E.). Dispersion in Rock Salt .NEUMANN (2 . v.). Nickel and Carbon Elements . EISENMANN (R.) . Galvanic Element . Polarisation of Copper . WEBER (C . L.). Conductivity of Amalgams . the Gaseous State at all Temperatures . EMDEN (R.). Vapour-tensions of Saline Solutions . LESCGCUR (H.). Hydrates of Barium Chloride . PAGE 632 633 633 633 634 634 693 693 6% 695 695 695 696 696 697 697 698 698 753 163 753 754 754 155 755 756 757 757 957 757 158 158 159 760 760 761 761 761 762 763 764! 764 765 765 766 166 767 767 767 768viii CONTENTS. GOSSART. The Spheroidal State . BRAUN (F.) . Decrease of Compressibility of Ammonium Chloride Solutions with Increase of Temperature, . M~RMET (A.). Lecture Experiments . BOISBAETDRAN (L. DE). Fluorescence of Manganese and Bismuth . BECQU~EL (18.).Variations in the Absorption-spectra of Didymium Salts. BOTHAMLEY (C. H.). Orthochromatic Photography . BOUTY (E.). Conductivity of Mixtures . BERTHBLOT. Phosphates of the Alkaline Earths . JOLY (A). Trimetallic Phosphates . STOHMANN (F.). Heats of Combustion of Organic Compounds . STOHMANN (F.), P. RODATZ, and W. HERZBERG. Heat Equivalents of Benzyl-compounds . FLAWITEEY (F.). Relation between the Boiling Points of the Monatomic Alcohols and their Constitutions . EOLA~BE (F.) . Alteration of Freezing Points . NATANSON (E.). Cooling of Carbonic Anhydride on Expansion . SKINNER (S.). Phosphonium Chloride . . SCHALL (C.) . Vapour-density Apparatus . SCHALL (C.). Determination of the Vapour-density of High Boiling Sub- stances under Reduced Pressure . SPRING (W.).Influence of Temperature on the Rate of Action of certain Acido on Marble . BOUTY (B.). Application of the Electrometer to the Study of Chemical Reactions . FOUSSEREAU ((3.). Decomposition of Thiosulphates by Acids . MEYEB (L.). Apparatus for Fractional Distillation under Reduced Pressure BRUHL (J. W.). Influence of Single and Double Union on the Refractive Power of Compounds : Constitution of Benzene and Naphthalene . BOISBAUDRAK (L. DE). Fluorescence of Spinel . CROOKES (W.). Crimson Line of Phosphorescent Alumina . BOISBAUDRAN (L. DE). Fluorescences of Manganese and Bismuth . BOISBAUDRAN (L. DE). New Fluorescences with well-defined Spectra. DEMAE~AY (E,). Spectra of Didymium and Samarium . WRIQHT (C. R. A.) and C. THOMPSON. Development of Voltaic Electricity DEBRAY (H.) and €'&CHARD.Alteration of the Carbon Electrodes used for the Electrolysis of Acids . RIQHI (A.). Conductivity of Bismuth for Heat in a Magnetic Field . VIOLLE (J.). Comparative Radiation of Fused Platinum and Fused Silver . BERTHELOT and FABRN. Heat of Formation of Hydrogen Telluride . FABRE (C). Heat of Formacion of Crjstallised Tellurides . STOHMAN (F.). Heats of Combustion of Organic Compounds as Determined by Different Methods . BERTHELOT and RECOURA. Passage from the Benzene to the Acetic Series . GERLACH (G. T.). Boiling Points of Salt Solutions . AMAQAT (E. EL). Solidification of Liquids by Pressure . THOMSON (J. J.). Dissociation of some Gases by the Electric Discharge . GOUY and 8. CHAPERON. Osmotic Equilibrium and the Concentration of Solutions by Gravitation .SCHIFF (R.). Demonstration of the Coefficient of Expansion as a Lecture Experiment . REYCHLER (A.). Estimation of Pressure in Closed Tubes . TROWBRIDQE (J.) and C. C. HUTCHINB. Oxygen in the Sun . TROWBRIDGE (J.) and C. C.HUTCHINS. Carbon in the Sun. HUTCHINS (C. C.) and E. L. HOLDEN. Existence of certain Elements and Discovery of Platinum in the Sun . SUNDELL (F.). Spectrum Analysis . CROOKES (W.). Radiant Matter Spectroscopy : Examination of the Residual Glow . by Atmospheric Oxidation . PAGB 768 768 769 873 873 874 877 877 877 878 879 879 880 882 882 882 882 am 883 884 1005 1005 1006 1006 1008 1008 1008 1009 1009 1010 1010 1010 1011 101 1 1012 1013 1013 1013 1023 1014 1065 1065 1065 1066 1066CONTENTS . CBOOKES (W.). SharpLine Spectrum of Phosphorescent Aluminium .CROOKES (W.). Sharp Line Spectra of Phosphorescent Yttris and Lan- thana . GRUNWALD (A.). Chemical Structure of Oxygen and Hydrogen and their Dissociation in the Sun’s Atmosphere . STAATS (G.). Photochromatic Properties of Silver Nitrate . MOORE (T.). Modification of the Ferric Chloride Cell . BUCEANAN (J.). Electrical Conductivity of Hot Gases . MIESLER (J.). Electromotive Dilution Constants of Silver and Copper Salts . BOLTZMANN (L.). Thermochemical Law conjectured by Pebal respecting Non-reversible Electrolytic Actions . BOYS (C . V.). Bunsen’s Ice Calorimeter . KEISER (E . B.). New Pyrometer . BEKETOFF (N . N.). Change in Volume during the Formation of Metallic Oxides . SPRING (W.) and E . PAN AUBEL . Action of Acids on Zinc containing Lead .HUNT (T . S.). Integral Weights in Chemistry . Inorganic Chemistry . LUNGE ((3.). Conversion of Calcium Hypochlorite into Calcium Chlorate . RAMMELSBERG (C.). Crystalline Silicocarbonate from Soda Liquors . Sodium Calcium Carbonate . ROSENBLADT (F.). Double Nitrites of Cesium and Rubidium . BUNSEN (R.) Decomposition of Glass by Carbonic Anhydride condensed on its Surface . REIDEMEISTER ((2.). BOISBAUDRAN (L . DE) . Purification of Yttria . OSMOND . Heating and Cooling of Cast Steel . KNIESCIIE (l?.). Tungsten . PFORDTEN (0 . v . d.). Titanium . BOISBAUDRAN (L . DE) . Atomic Weight of Germanium . , . KRUSS (G.). Gold Oxides . BASSETT (H.) and E . FIELDINQ . Action of Hypochloroue Anhydride on Iodine Trichloride . BLAREZ (C.). Saturation of Selenious Acid by Bases .KAPPEL (S.). Formation of Nitrites . RUDORFF (I!.). Compound of Arsenious Oxide with Halogen Salts . . PLINGLE (A.). Some Probable New Elements . CASTNER (H . Y.). Production of Alkali Metals . LEIGHTON (G . W.). Crystalline Scale formed in the Manufacture of Sodium Hydrogen Carbonate . HEYER (C.). Strontia Dihydrate . BLOUNT (B.). Calcium Borate . BLOXAN (C . L.). WHEELER (H . A.). NORDENSKIOLD (A . E.). Eqnivalent of Gadolinium Oxide . KNAPP (F.). Formation of Ultramarine in the Wet Way . STANLEY (A.) . Sodium Dichromate . &Uss (G.) and H . SOLEREDEL . Reduction of Inorganic Sulpho-salts by Hydrogen . WADDELL (J.). Atomic Weight of Tungsten . RASCHIG (F.). Compounds of Gold with Nitrogen . GIBBS (W . ) . Complex Inorganic Acids .JORGENSEN (9 . M.). Roseo-rhodium Salts . JORGENSEN (S . M.). Nitratopurpureo-rhodium Salts . ROSENIXADT (T.). Solubility of some Gold Compounds . Calcium Ammonium Arsenate and Calcium Arsenate Artificial Lead Silicate from Bonne Terre, Montana ix PAGE 1069 10’70 1070 1071 1071 1071 1072 10’72 1073 1073 1073 10’74 1077 11 12 12 12 13 13 14 14 14 15 15 16 106 106 106 107 107 107 108 108 108 108 109 109 110 110 111 111 112 113 113 114 JORQENSEN (S . M.j. XanthoIrhddium Salts . 114X CONTENTS. PAB'E WURSTER (C.). Active Oxygen in the Atmosphere . 211 WURSTER (C.). Formation of Active Osygen in Paper . 211 MOISSAX (H.). Phosphorus Pentafluoride . 212 WEBER (R.). SCHNEIDER (R.). sulphide. 213 MCCAY (L. W.). Arsenic Pentasulphide . 213 BLOCHMANN (R.). Carbonic Anhydride in the Atmosphere.214 JOLP (A.). Bimetallic Phosphates . 214 JOLP (A.). Silver Phosphates and Arsenates . 215 CARPENTER (R. F.). Solubility of Silver Chromate in Ammonium Nitmte . 216 JENSCH (I%). Tetracalcium Phosphate and Basic Converter Slag. 216 SCHEIBLER (0.). Determination of Water in the Hydrates of Strontium Oxide . 217 FINKENER (R.). Actio; of Carbokc Ahhydride on the Dihydrate of Stron- tium Oxide . 217 HEYER (C.). Estimation of Water in Btrontia DihSdrate . 217 MENSCHING (J.) and V. MEYER. Vapour-density of Zina . 218 HENSGEN (0.). Ammonio-mercuric Chromates . 218 MAUXEK~ (E.). Water of Crystallisation of Alums . 218 JENSCH (E.). Composition of some Ancient Ceramics from Brandenburg . 218 OSMOND. Heating and Cooling of Fused Steel . 219 GAUTIER (F.).Influence of Silicon on the Condition of Carbon in Cast- won. 2 2 0 XEHRMANN (F.). k Ndw Clks of'Cobktic Ekts . 220 BLOMSTRAND (C. W.). Oxy-acids of Iodine. 327 THOMSON (J. J.) and R. THRELFALL. Production of Ozone. 32'7 SENDERENS (J. B.). Action of Sulphur on Ammonia and Metallic Bases in Presence of Water . 327 WEBER (R.). Combinations of Sulphuric Anhydride with 'Phosphonc and Iodic Anhydrides . 328 TEONSON (J. J.) and R. THBELFALL. Passage of Electric Discharges through Pure Nitrogen . 328 HAUTEFEUILLE (P.) and J. MARGOTTET. Hydrated Silicon Phosphate . 329 DEMAR~AP (E.). Action of Carbon Tetrachloride on Metallic Oxides . 929 QUANTIN (H.). Ferric Phosphate . , . 330 SHITH (W.) and W. B. HART. Sodium Carbonate . , 330 RAMMELSBEBQ (C.). Occasional Products in the Soda Manufacture .331 GOTTIG (C.). Water of Crystallisation of Sodium Monosulphide . 331 DRAPER (H. N.). Silver Ammonio-nitrate . 331 SEKDERENS (J. B.). Copper Nitrates . 331 SPRING (W.). under the Influence of Pressure . 332 BOURGEOIS (L.). Calcium Yilico-stnnnate . 333 COEN (S.). Solubility of Gypsum in Solutions of Ammonium Salts . 333 LINCK ((3.). Crystallography of Cadmium Borotungstate . 334 OSBOBNE (T. B.). Higher Oxides of Copper . 334 CROOEES (W.). New Elements in Gdolinite and Samarskite . 334 CHRISTENSEN (0. T.). Chemistry of Manganese and Fluorine . 335 GLASER (M.). Action of Potassium Permanganate on Sodium Thiosulphate 336 DITTE (A.). Compounds of Stannic Oxide . 336 PFORDTEN (0. V. D.). Titanium . 337 MANASSE (0.). Vanadates of the Alkaline Eaxthe .339 MICHAELIS (A.). Valency of Bkmuth. . 3.410 HASEBROEK (K.). Action of Hydrogen Peroxide on Bismuth Salts . 3410 KRUSS (G.). Atomic Weight of Gold . 340 ERUSS ((3.) SublimedAuricChbride. 341 Compounds of Selenious and Arsenious Anhydrides with Behaviour of Iodine with Reallgar and Arsenic Iodo- Sulphuric Anhydride . 212 Action of Carbon Tetrachloride on Chromyl Dichloride and Action of Non-metals on Solutions of Silver and Reaction between Barium Caxbonate and Sodium SulphateCONTENTS . xi WINCKLER (C.). Preparation of Chlorine from Bleaching Powder . STOLBA (F.). Action of Hydrochloric: Acid on Sphalerite . BERTHELOT . Metals and Minerals of Ancient Chaldea . WARREN (H . N.). Decomposition of Ammonium Chloride by an Alloy of Zinc and Iron .SHAW (W . N.). Atomic Weights of Silver and Copper . PREIS (X.) and B . RAYMANN . Decomposition of Sodium Sulpharsenate with Silver Nitrate . OTTO (H.). Tetracalcium Phosphate and Basic Slag . ENGEL (R.). Effect of Hydrochloric Acid on the Solubility of Chlorides . DIXON (W . A ) . Constitution of Acids . MEYEE (V.). Properties of some Metals . BIRD (G . B.). Purification of Zinc . HARDAWAY (H.). Analysis of Shot KUBEL (W.). Preparation of Lead Carbonate . BERRY (N . A.). Copper Slag HARRISON (GI.. ). Mirror Amalgam . BIRD (GI.. B.). Mercurous Hydroxide . BAYER (9 . J.). Rasic Aluminium Sulphate . . Sulphide . ANDR& (GI.. ). Action of Lead Oxide on Soluble Chlorides . ANDRS ((3.). Action of Mercuric Oxide on Dissolved Chlorides . CERISTENSEN (0 . T.). Fluorine and Manganese Compounds .CLAASSEN (E.). Solubility of Manganese Sulphide in Fused Potassium HOOD (J . J.). Preparation of Ammonium Dichromate . CLAASEN (E.). Extraction of Vanadium and Chromium from Iron Ores . KRUSS (G.). Gold . MILES (F . P.). Formation of Potaesium Silicate . RASCHI~ (F.). Action of Nitrous Acid on Bulphurous Acid . VAN NUYS (T . C.), and B . F . ADAMS . MENSCHINQ (3.) and V . MEYER . WTTIG (C.) New Hydrate of Sodium Hydroxide . SENDERENS ( J . B.) Action of Metals on Solutions of Silver Nitrate . WARREN (H . N.). Zinc-eisen . THOMS (H.) Ammonio-zinc Chlorides . MABERY (C . F.) Products from the Cowles Electrical Furnace . MEYER (L.), Action of Carbon Tetrachloride on Oxides . DONATR (E.) Barium Manganate . ROUSSEAU (G.). Formation of Manganites from Permanganates .BENDER (G.). Non-existence of Chromium Heptasulyhide . MUTEMANN (W.). Lower Oxides of Molybdenum . SEUBERT (K.) and SCHURMANN . Bromostannic Acid . KR~JSS ((3.). Gold . EREUSLER (U.). Amount of Oxygen in the Atmosphere . OLSZEWSKI (K.). RASCHIQ (F.). Reaction of Nitrous Acid with Sulphurous Acid . KRAUT (K.). Oxidation of Ammonia in presence of Platinum or Palla- dium . FRANKE (B.). Hyhroxylated Solii Hyirogen Phosphide . GOTTIG (C.). Hydrates of Potassium Hydroxide . MUTHMANN (W.) . Argentous Compounds . JOLY (A.). ANDR& ((3.). Ammoniacal Compounds of Cadmium Chloride . ANDRI~ ((3.). Ammoniacal Compounds of Cadmium Sulphate and Nitrate . OSMOND (F.). Effect of Manganese, &c., on the Properties of Steel . KNOP (A.). Crystallised Niobic Anhydride .Carbonic Anhydride in the Air Vapour-density of Potassium Iodide DEMARCAY (E.) Cerite Earths . SEUBERT (E.). Chlorostannic Acid . Boiling Point of Ozone : Solidification of Ethylene . Double Phosphates and Arsenates of Strontium and Sodium DITTE (A.). Alkaline Vanadates . COSSA (A.). Animoniacal Platinum Compounds . PAGE 442 442 44.3 443 443 44A 444 445 445 445 446 446 446 446 447 447 447 447 447 448 449 449 449 450 450 549 549 550 550 550 550 551 651 551 552 552 552 553 553 554 554 554 634 634 635 635 635 636 636 637 637 638 639 639 642 642xii CONTEXTS . MACIVOR (R . W . E.). Perbromic Acid . CURTIUS (l‘.). Diamidogen or Hydrazine . DRECHSEL (E.). Nitrous Acid . LESC(EUR (H.) Hydrates of Sodium Arsenate . DE MOND~SIR (P.). Particular Case of the Formation of Sodium Hypo- bromite .DRAPER (C . N.). Solubility of Lithium Carbonate . DRECHSEL (E.). Argentous Componnds . PFORDTEN (0 . v . D.). WANKLYN (J . A.). Specific Gravity of Lime-water . LUNGE (G.) and R . SCHOCH . VILLIERS (A.). Barium Phosphates . WARREN (H . N.). Thallium in Platinum . WARREN (H . N.). Preparation of Anhydrous Metallic Chlorides . WARREN (H . N.). Action of Nitrogen on Certnin Metals . MENKE (A . E.). SHIMER ( P . W.). Titanium Carbide in Pig-iron . DRECHSEL (E.). Formation of Complex Inorganic Acids . KBUSS (G.) and L . F . NILSON . Equivalent and Atomic Weight of Thorium . KRUSS (G.) and L . F . NILSON . Potassium Germanium Fluoride . DITTE (A.). Alkaline Vanadates . KRUSS (G.) and L . F . NILSON . Reduction of Potassium Niobium Fluoride with Sodium .KBUSS (G.) and L . F . NILSON . Earths and Niobic Acid from Fergusonite . NEUMANN (G.) . Preparation of Oxygen and of Sulphurous Anhydride with Kipp’s Apparatus . MICHAELIS (A.) . Vapour-density of Tellurium Tetrachloride : Valency of Tellurium . WAR~EN (H . N.). Nitrogen Fluoride . ALLARY (E.). Regeneration of Acid Residues in the Manufacture of Gun- cotton . MULLEB (J . A.). Influence of Temperature and Pressure on the Action of DE MONDBSIR (P.). Artificial Production of Trona or Urao . BAILEY (G . H.). Silver Suboxide . ENGEL (R.). Solubility of Calcium and Magnesium Chlorides in Water atOo . FORM~NEK (J.). Solubility of Lead Chloride in Solutions of Mercuric Chloride . The Lowest Compounds of Silver Action of Ammonia on Bleaching-powder Action of Ferric Sulphate on Iron Potassium Chloride on Crude Methylamine Carbonate .SAGLIEB (A.). Ammonium Copper Iodides . ~ T A R D (A.). Solubility of Copper Sulphate . BAUBIGNY (H.). Schweizer’s Reagent and “Eau Celeste” . MEYER (V.). Stability of Corrosive Sublimate Solution . BUCHNER (E.). Action of Carbonic Anhydride on Ulti.amarine . CLAASSEN (E.). Manganese Sulphate . LAUGIEB (P.). Action of Selenious Acid on Manganese Dioxide . JORGENSEN (a . M.). Cobaltammonium Compounds . KEHRMANN (F.). Structure of Complex Inorganic Acids . KEHRMANN (F.). Phosphotnngstic Acids . WEIBULL (M.). Crystallised Compounds of Zirconium . MAUMENR (E.). Alloys of Platinum, Iron, and Copper . DEBBAY (H.). Action of Acids on Alloys . THUMMEL (K.). Behaviour of Mercuric Chloride with Hydrogen Ammo- nium Carbonate .BERG (A.). Chromiodates . NILSON (L . F.) and 0 . PETTERSON . Physical Constants of Germanium and Titanium and their Compounds . KEUSS (G.). Gold . DEBRAY (H.). Crystalline Alloys of Tin and the Platinum Metals . PAGE 698 698 698 698 699 699 699 699 700 700 701 702 702 702 703 703 703 704 704 705 706 706 769 770 770 770 771 771 771 771 772 772 772 773 774 774 774 774 775 775 776 777 777 778 778 $78 778 779 779CONTENTS ... xu1 PAGE CHILO~STCHOFF . Precipitation of Mixtures of Iodates and Sulphates by Barium Salts . FILESENIUS (R.). Preparation of IIydrogen Sulphide free from Arsenic . JACOBSEN (0.). Purification of Hydrogen Sulphide from Hydrogen Arsenide FINE (R.). Affinity of certain Bivalent Metals for Sulphuric Acid .DACCOMO ((3.) and V . MEYER . Density of Nitric Oxide at -100’ . MENSCHING (J.) and V . MEYER . Behaviour of Phosphorus, Arsenic, and . HEMPEL (W.). Percentage of Oxygen in the Air . HARTOG (P . J.). Sulphites . Antimony a t a White Heat GEUTHER (A.). Arsenic . FOSSEE (W.). Carbonic Anhydride in the Air of School-rooms . GOTTIQ (C.). Crystallisation of Alkalis from Alcohol . PBEIS (C.) and B . RAYMAN . FISHER (J . H.). EBUSS (G.) and L . F . NILSON . Decomposition of Sodium Thioarsenate by Silver Nitrate . Corrosion of Zinc by Ammonium Chloride and Potassium Nitrate . . Components of the Rare Earths yielding Absorption-spectra . DE BOISSIEU (P.). Water of CrystalliQation of Alums . CHRISTENSEN (0 . T.). Chemistry of Manganese and Fluorine . ROUSSEAU ((3.).Potassium Manganites . ENGEL . Hydrochloride of Ferric Chloride . SABATIER (P.). Hydrochloride of Ferric Chloride . FRANEE (B.). Action of Sulphuric Acid on Potassium Permanganate . OSMOND and WERTE . Residues obtained from Steel and Zinc by the Action of Acids . GONZALEZ (C.). Paratungstates . HINSBERQ (0.). Zirconium . CARNOT (A.). Reactions of Vanadic Acid . DITTE (A.). Metallic Vanadates . DITTE (A.). Ammoniacal Vanadates . MATTHEY (E.). Metallurgy of Bismuth . DEBRAY (H.) . Products of the Action of Acids on Alloys of the Platinum Metals . FABRE (C.). Selenium Alums . DES CLOIZRAU . Monoclinic Form and Optical Properties of Arsenious Anhydride . ELASON (P.). Action of Chlorine in Carbon Bisulphide and of Sulphur on Carbon Tetrachloride . FEANKE (B.) .Manganese Compounds . TROOST (L.) and L . OUVEAILD . Thorium Silicates . TBOOST (L.) and L . OUVBARD . Thorium Sodium and Zirconium Sodium Phosphates . HOFFMANN (L.) and G . KRUSS . Gold Sulphides . KEISEB (E . H.). Combustion of Weighed Amounts of Hydrogen : Atomic Weight of Oxygen . FISCHER (F.) . MICHAELIS (A.) . Tellurium Dichloride . FISCHER (H.). Working up of Stassfurt Potash Liquors containing a . SCHOTTLANDER (P.). Crystalline Form of Potassium Aurobromide . WARREN (H . N.). Phosphorised Silver . FRIPDHEIM (C) . “ Silver Suboxide ” . WELLS (H . L.). Basic Zinc and Cadmium Nitrates . WAEEMANN (A . J.) and H . L . WELLS . COUSTNS (A. C.). Relation of Mkrcury to other Metals . KLASON (P.) Carbon Oxysulphide . CAILNOT (A . > . Vanadates . KILUSS ((3.).Atomic Weight of Gold . Composition of Generator Gas and Water Gas large Excess of Sodium Chloride Basic Lead Nitrates 884 8‘35 as5 885 885 886 887 888 888 888 889 889 889 890 892 892 a92 a93 894 894 894 895 896 898 900 a96 a99 900 1014 1015 1015 1015 1016 1016 1017 1018 1019 1019 1078 1078 1078 1039 1039 1079 1039 1080 1080 ioaoxiv CONTENTS . BOISBAUDRAN (L . DE) . Gallium . WARREN (T . T . P . B.) . Metallic Manganese Compound of Manganese Sesquioxide with Cupric Oxide . MOORE (T.) Peculiar Formation in Nickel Regulus . WINKLER (C.). Germanium . SCHNEIDER (E . A.). BETTEL (W.). Separation of Gold from the Platinum Met& . M;irteralogical Chemistry . BRAND (A.). Artificial Breithauptite from the Mecherniah Lead Furna,ce s . MACADAM (W . I.). Butyrellite .SCACCHI (E.). Minerals fr9m Vesuviua . BECKER (A.). Chemical Constitution of Barytocalcite and Alstonite . DES CLOIZEAUX (A.) and A . DAYOUR . Chemical Composition of Herderite BUSATTI (L.). Minerals from Tuscany . MACKENZIE (G . S.). Rare Copper Minerals from Utah . DANA (E . S.). Columbite . CHROUSTSCBOFF (K . v.) . Plagioclase . DES CLOIZEAUX (A.) and F . PISANI . Oligoclase . HOCKAUF (J.). Botryogene . . SPEZIA (Gt ) . Flexibility of Itacolumite . STRUVER (G.) Volcanic Fragments from the Lake of Bmcciano . NORDENSKIOLD (A . E.). DAUBR~E . DAMBREGIS (A . K.). Cosmical Powder from San Fernando, Chile . GURLT . Meteorite in a Tertiary Lignite . Note on a Meteorite in a Tertiary Lignite . HIDDEN (W . E.). Twin Crystals of Molybdenite . MEEM (J . G.). Limonite-pseudomorphs after Iron Pyrites .DANA (E . S.). Brookite from Magnet Cove, Arkansas . HIDDEN (W . E.). A Remarkable Crystal of Herderite . Analysis of Mineral Springs in Aegina and Andros . CLARKE (F . W.) and J . 8 . DILLER . PENFIELD (5 . L.) and F . L . SPERRY . Pseudomorphs of Garnet . HIDDEN (W . E.). Phenacite from Colorado . EIDDEK (W . E.) and A . DES CLOIZEAUX . North Carolha &finer81 Lo- calities . Turquoise from New Mexico . LEIGETON ((3 . W.). Mica from Leon Co., Texas . STROHECKER (J . R.). Ceriferous Hainstadt Clays . . HUNTINQTON (0 . W.). Crystalline Structure of Iron Meteorites . HIDDEN (W . E.). New Meteorite Iron from Texas . KUNZ ((3 . F.). Meteoric Iron from Glorieta Mt., New Mexico DANA (E . S.) and S . L . PENFIELD . Two Hitherto Undescribed Meteoric Stones .WANKLYN (J . A.). Occurrence of Free Iodine in a Mineral Water . ROMANIS (R.). Gold from Burmah . BOURGEOIS (L.). Crystallised Insoluble Carbonates . SANDBERGER (F.). Occurrence of Iodine in Phosphorites and of Lithium in Psilomelane . MEYER (A . B.). Nephrite from Alaska . BEUTELL (A.). Prehnite from Silesia . STEQER (V.). Porphyry from Horka in Prussia . DRASCHE (E.). Analyses of Persian Eruptive Rocks . SANDBERGER (F.). Investigations on Ore-veins . Recent Alluvial Deposits in the Ij and Zuyder Zee . MEUNIER (S.). Mineral Waters from Java . VAN BEYYELEN ( J . M.). SAUER [A.) . Amorphous Carbon (Graphito'id) in the Saxon Erzeebirm " V DANA (E . S.). Cryitallisation of NatiGe Copkr . BROWN (W . G.). Crystallographical Notes . 342 PAGE 1081 1081 1081 1081 1081 1 W 17 17 17 18 19 19 19 20 20 20 21 21 21 22 22 22 23 116 116 116 116 117 117 118 118 119 119 119 119 120 120 221 221 221 222 222 223 223 223 2% 224 224 341 341CONTENTS .GENTH (A.) . Mineralogical Notes . LINDSTROY (G.). Copper Mineral from Sunnerskog. Sweden . CROSS (W . J.) and W . F . HILLEBBAND . PENFIELD (S . L.) and D . N . HARPER . DANA (E . S.). Mineralogical Notes . WEIBULL (M.). Galenobismuthite from the Falun Mine . HILLEBRAND (W . F.). Emmonsite. an Iron Telluride . NORDENSKIOLD (A . E.). Gearksutite from Ivigtut. Greenland . Chemical Comr>oaition of Ralstonite . Elpasolite. a New Mineral . LOSCH (A . k.). 'Brucite from the Ural . A . GORQEU (A.). Artificial Zincite and Willemite . PEARCE (R.). Goslarite from Montana .SJOQREN (A.). Place of Spodiosite in the Mineral System . SJOQREN (A.). Sarkinite, a New Manganese hsenate . IQELSTROM (L . J.). Polyarsenite . PENFIELD (5 . L.). Vanadinite from Arizona and New Mexico . HEADDEN (W . P.). Columbite from Colorado . LINDSTROM (G.). Phosphoric Anhydride in Felspar . CLARKE (F . W.). Lithia Micas . CHATARD (T . M.). Lucasite, a New Variety of Vermiculite . LACROIX (A.) . Lamellar Thomaonite . LACROIX (A.). White Epidote from the Beagle Canal, Terra del Fuego LACROIX (A.). Critical Examination of some Minerals . ARZRUNI (A.). Paragonite Schist from the Ural . ANSDELL (G.) and J . DEWAR . FRESENIUS (R.). Hot Springs a t Wiesbaden . STELZNER (A.) and A . SCHERTEL . HOLLAND (P.). Quartzite . EINCH fE.). Plattnerite . Gaseous Constituents of Meteorites Black Zinc Blende of Friberg KINCH '(E.).F . H . BUTLER. and H . A . MIERS . New Vaziety of Dufrenite from Cornwall . MACADAM (W . I.). Talc used in Paper-making . PENPIELD (5 . L.), Phenacite from Colorado . SMITH (W . B.). Crystal Beds of Topaz Butte . ALLINQ (A . N.). Topaz from Thomas Range. Utah . JANNASCH (P.). Strontia in Heulandite . BISCHOP . Sodium Felspar from Krageroe. Norway . MALLET (J . W.). Silver in Cotopaxi Volcanic Ash . VOGDT (C . v.). Diabase-porphyrite from Petrosawodsk . EUNZ (a- . F.). Meteoric Iron from Augusta Co., Virginia HUNTINGTON (0 . W.) . Coahuila Meteorites . MILES (F . P.). Supposed Meteorite from Highland Co., Virginia . the Spring a t Oued Ref . ROMBURGH (P . v.). MCIVOR (R . W . E.). New Zealand Graphite . BECKER (G .F.). Natural Solutions of Cinnabar. Gold, and Associated Sulphides . FREMY . Artificial Formation of Rubies . FREYY and VERNEUIL . Action of Fluorides on Alumina . GORQEU (A.). Zinc Ferrite : Artificial Formation of Branklinite . LACROIX (A.). Plumbocalcite from Wenlock Head . OCHSENIUS (C.). Phosphoric Acid in Chili Saltpetre . DARAPSKY (L.). Chilian Alums . RATH (G v.). Cristobalite from Mexico . FUNARO (A.). Felspars from Elba . TSCH E RM AK (G.) . S capolite Series . . DE LESSEPS . Water from Artesian Well in the Tunisian Chotts and from Water from the Wells of Zemzem . DE CHBOUSTCHOFF (K.). Artificial Production of Quartz and k d y m i h . DE CHROUSTCHOFF (K.) . Artificial Production of Quartz and Orthoclme . HAUTEFEUILLE (P.) and L . P . DE SAINT.GILLES .Artificial Production of Micas . XV PAGB 342 543 343 343 3444 344 344 345 345 345 346 346 346 346 347 347 347 347 349 350 350 350 351 351 352 45 1 451 451 451 452 452 452 453 453 453 454 454 454 455 455 455 455 555 655 556 556 557 557 558 558 559 559 559 560 560 560xvi CONTENTS . COHEN (E.). Talc. Pseudophite. and Muscovite from South Africa . DATHE (E.). Kersantite from Wustewaltersdorf. in Silesia . GOTZ (J.). Andalusite from Marabastad. Transvaal . JANNASCH (P.). New Analyses of Norwegian Rocks . KOTG (B.). Japanese Rocks . HIDDEN (W . E.). The Mazapil Meteoric Iron . KUNZ (G . F.). Meteorites from Kentucky and Mexico . ZUBER (R.). Eruptive Rocks from Krzeszowice. near Cracow . RICCIARDI (L.). Origin of Hydrogen Chloride, Sulphurous Anhydride. and Iodine in the Gases of Volcanoes .KONIG (Gt . A.). Stromeyerite from Mexico . IGELSTROM (L . J.). Braunite from Jakobsberg. Wermland . JANNETTAZ (E.). Buratit. e from Laurium . ERBEN (B.). Bohemian Minerals . DEBY (J.). Cyprusite . IGELSTROM (L . J.). HEematostibite from Orebo . COSSA (A.). Columbite from Graveggia, Val Vigezzo . YOUNG (J.). Pectolite from Kilsyth . KONIG (G . A.). RNOP (A.). Biotite . Manganese-zinc Serpentine from Franklin, New Jersey KNOP (A.). Pseudobiotite . DAMOUR (A.). A Pink Clay . MEUNIER (S.). FREsENIus (H.). Analysis of the Schutzenhof Quelle, Wieibade6 LosaNITscH (S . M.). Mineral Waters from Servia . BULITSCH (P.). Analysis of the Water of a Saline Lake . MEUNIEP (S.). GORGETJ (A.). Artificial Production of Magnetite . XACIVOR (R .W . E.). BUSATTI (L.). Wollastonite from Sardinia . BOSSCHA (J.). Meteorite of Karang-Modjo or Magetan in Java . WILLM (E.). Sulphuretted Waters of Olette . KALECINSZKY (A.). Native Gold from Thibet . HUSSAK (E.). Granular Limestone of Stainz, in Styria . WEIBULL (M.). Manganese Apatite : Composition of Apatite . STAHL (W.). Celestine in Nautilus aratus . BAUBIGNY (H.) . Artificial Bormation of Alabandine . BOURQEOIS (L.). Artificial Production of Crocoisite . FLINK (G.). Lingbanite . CHESTER (A . H.). Mineralogical Notes . WARTHA (V.). Minerals of the Serpentine-chlorite Group . SCHLTJTTIQ (E.). Imperfectly known Silicates . TEALL ( J . J . H.). Plagioclase from the Tynemouth Dyke . LE CHATELIER (H.). Action of Heat on Clays . LE CHATELIER (H.). Constitution of Clays .SCHOELLEB (R.). River-waters of La Plata . SANDBERGER (F.). Graphitefrom Ceylon . PULA (E.). Recent Formation of Marcasite a t Marienbad . SANDBERGER (F.). IGELSTROM (L . J.). Minerals from the Sjo Mine, Sweden . ZEPHAROVICH (V . v.). Pyroxene : Scheelite . ARZRUNI (A.). Dipyr from Connecticut . JANNASC EI (P.). Heulandlte . TRAUBE (H.). Laubanite : Laumontite . Meteoric Iron a t Fort Duncan, Texas . MACIVOR (R . W . E.). Bismutlzic Gold . SEMMONS (W.). Enargite from.Montana . Artificial Formation of Rose-spinel or Balas Ruby Minerals occurring in Australian Bat Guano CES~RO (G.). Destinezite . HEPBTJRN (Gt.). Griqualandite . . Percylite, Caracolite, and Phosgenite from Chili EIGEL (F.). LEDROIT (J . M.1 .. So.-called Trachvte-dolerites of the Voeelaberg .Trachytic Rocks from the Island of San Pietro . PAGE 561 562 562 662 563 564 564 564 643 643 644 644 644 645 645 645 646 646 646 647 647 cj; 47 648 707 707 707 708 708 709 709 709 710 710 780 980 781 781 781 781 782 782 783 4 89 785 785 786 901 90 L 902 902 902 903 903 903 909 904 643 648 Z84CONTENTS . xv ii COHEP (IT.). Pallasite from Campo de Pucarii . ZEPHaRovrcH (v . v.). Trona. Idrialite. and Zinc Bloom . KOKSCHAROFF (N . J . v.). Turquoise from the Kirghis Steppes . ZGLENITZEIJ (W . K.). Epsomite from Poland . TEALL ( J . J . H.). Augite from the Whin Sill . TEALL ( J . J . H.). Andesine from Sutherlandshire . COLLINS ( J . H.). Minerals from Porthalla Core, Cornwall . LORY (C.). Microscopic Crystals of Albite in Calcareous Rocks of the RICCIARDI (L.).Composition of Volcanic Rocks . DAUBR~E . Meteorite a t Djati Pengilon, Java . LUZZATTO (E.) . Antimonite from Valdagno . DE LANDERO (C . F.) Tellurium Silver Bismuth from Jalisco, Mexico . LUEDECKE (0.). Minerals from the Stassfurt Salt Mines . PLUG+ (K . K.). PICCINI (A.). A Mineral associated with the Columbite of the Vai KNOP (A.). The Peridote of Schelinger Matten . KOTO (B.). Glaucophane . SCACCHI (E.). Altered Cordierite from Rocaa Tederighi in Tuscany . RICCIARDI (L.). Composition of Rocks and Minerals from Vulture and Melfi LUDWIG (E.) and G . TSCHERMAE . Meteorite from Angra dos Reis . Western Alps . Ignatieffite, a New Variety of Aluminite Vigezzo . JOHNSTONE (W.). Flitwick Water . Organic Chemistry . HENRY (L.). Volatility of Methane-derivatives .BERTHELOT . Sugars . KLASON (P.). Sugar formed in the Inversion of Lichens . CONRAD (M.) and M . UUTHZEIT . Action of Dilute Acids on Grape-sugar and Fruit-sugar . CONRAD (M.) and M . GUTHZEIT . Decomposition of Milk-sugar by Dilute Hydrochloric Acid . LANDWEHR (H . A.). Animal Gum . W o HL (A . ) . Thio f ormalde h y de-derivatives . MAGNAXINI (0.). Chloro-derivatives of Acetals . PECHXANN (H . v.) and K . WEHSARG . CECONOMIDES (L.). Ketines . BANNOW (A.). Pure Butyric Acid . MELIKOFP (P.). Derivatives of Tiglic Acid . MELIKOPP (P.). Constitution of C hlorohydroxybutyric Acid and Dichloro- butyric Acid . SAYTZEPP (A . C . and M.). Hydroxystearic Acids of Different Series . PEREIN (W . H., Jun.). Action of Trimethylene Bromide on Ethylaceto- PERKIN (W . H., Jun.), and P .C . E'EEER . Ethylacetotrimethplenecarboxg- late . CUBTIUS (T.) and I? . KOCH . Derivatives of Diazosuccinic Acid . JACOBSEN (0.). WALLACH (0.). Carbohydrates . Di-isonitroPoacetone acetate, Benzoylacetate, and Acetone Dicarboxglate . DRNARO (A.) . Dichloropyromucic Acid . WIDMAN (0.). Constitution of Glycoluril . ERREBA ((3.). Chloropropylbenzene . MAYER (I?.). Reduction of Trinitro-+-cumene . JAWBSEN (0.). Hemellithene . Hydrocarbons from Tar Oils boiling between 170" and 200" FILETI (M.) . Reciprocal Transformation of Cymene and Cumene-deri- vativeu . FILETI (M.) and F . CROSA . Chlorocymene and Bromocymene from Thymol JACOBSEN (0.). Ethylxylenes . VOL . LII . b PAGE 904 1021 1021 1021 1022 1022 1022 1023 1023 1024 1084 1084 1085 1085 1085 1086 1086 1086 1087 lo87 1087 24 24 25 25 26 26 26 27 28 28 29 29 29 30 30 32 33 33 34 344 35 35 36 36 36 37 37xviii OONTENTS .BENDER (Gt ..) . Ethereal Carbonates . B~EDERMANN (J.). Parahydroxybenzil Alcohol . KOSTAXECEI (S . v.). Synthesis of Betorcinol @-Orcinol) . CURTIUS (T) and (3 . LEDEBER . Benzylamine . CAUSSE . Acetal-resorcinol . GILL (J . M.). Citric Acid Derivatives of Paratoluidine . - . WALLACH (0.). Azo- and Diazo-eompounde . SUTKOWSEI (J.). Quinone-oximes . LOEB (M.). Amidine-derivatives . REIMARUS (0.). Action of Alkyl Iodides on Dibenzilthiocarbamide . STOLTE (H.) . Phenylseleniocarbimide and Diphenylse~eniocarbamid~ . BENDER ((3.). Substituted Nitroeen Chlorides . FILETI (M.). Preparation of Aromatic Amides . TSCHACHER '(0.). Condensation Gf Nitrobenzaldehyde with Hydrocarbons .HOFFMANN (A.). Compound of Pyrotartaric Acid with Hippuric Acid . ERLENMEYER (E ) and J . ROSENHEE . Phenyliodohydracrylio Acid . WENDE (H.). Cyesolcarboxylic Acid . L~EBERMANN (C.). Opianio Acid Derivatives . LIEPERXANN (C.) and S . KLEEMANN . Opianic Acid Derivatives . G R ~ N E (H.). Azo-opianic Acid . ELBEL (K.). Derivatives of Normethylnitro-opianic Acid . GABRIEL (S.). Homo-orthophthalamide . E~ERTENS (E.). Action of Amines on Shthalylacetic Acid . FILETI (M.). Bronioterephthalic Acid . SCHNAPAUFF (E.). Cumidic Acids . ERRERA ((3.). Reaction of Stilbene . ZINCKE (l'.). P-Naphthaquinone . ZINCKE (T.) and F . RATHQEN .. Benzene- and Toluene-azonaphthols and their Isomeric Hydrazine Derivatives . JULIUS (P.). New Diamidodinaphthyl .NOAH (E.) . Tetrahydroxyanthraquinones . CAHN (E . L.) . Methylanthragallols . CANNIZZARO (5.) and Gt . FABRIa . Acid from SanLonin : Isophotosantonic Acid . HESSE (0.). 'Cinchol . CONTNCK (0 . DE) . Alkaloyds . CIAMICIAN (G . L.) and M . DRNNSTEDT . Extraction of Pyrroline from Animal Oil . LADENBURG (A.). Ppidine Bases . CLAUS (A.) and F . COLLTSCHONN, Quinoliae . GABRIEL (S.). Isoquinolinsand its Derivatives . LIPPMANN (E.) aud F . FLEIGSNER . Synthesis of Hydroryquinolinecarboxylic Acid . LADENBERG ( A.). Piperidhe Bases . LTPSKI (A . A ) . Comparative Estimation of Preparations of Pepsin . REMSEN (T.) and H . W . HILLYER . Methods for Determining the Relative FISCHER (0.j and H . VAN Loo . Formation of P-Diquinoline . PODWYSSOZKI (W.). Method of Preparing Extrects of Pepsin .Stability of Alkgl Bromides . MANSFELD (W.). Derivatives of Diethylene Disulphide . ESCALES (R .) and E . BAUMANN . Disulphones BAUMANN (E.). Disulphones . LANDWEHR (H . A ) . Reagent for the Hydroxyl-group SCEWALB (F.) . Non-acid Constituents of Reeswax . HARVEY (S.) . HSRKIQ (M.) and S . SCHUTBERT . Carbohydrates . PETERS (K.). Linoleic Acid . Conversion of Starch into Glucose by means of Hydrochloric Acid . LADENBURG (A.) . Identity of Cadaverine with Pentamethylenediamirie . BAUMANN (E.). Compounds of Aldehydes and Ketones with Mercaptan . PAQE sa 38 39 443 44 40 4x3 41 42 $2 43 43 44 4.4 44 45 45 4!5 47 48; 49 50 61 52 52 53 53 54 66 66. 57 57 58 58 59 59 60 61 63 63 64r 65 66 122 122 123 323 124 124 125 125 125 126 126OONTENTS.BXEDT (J.). Acetyl-levulinio Acid : ConstituticHlr af pXetonic Acide . COXBES (A.). New aertction of Alumihm Chloride : Bpthesee in & Acetic Series .. VO~PEBT (F.). Gluconic Acids - . LIST (R). Actidn of Thi-kdeon' Ethil Aeelioaoehte . K~HLEE (A.) . Nitro-derivatives of Methylmil . B~PHRE~TD (R). l?ormation.of Dibromo- and Dichloro-kbiDc Acib . WER (V.)* Relation of a-Thiophsmc Acid t;o the Nomad Thiophnear- boxylic Acids . WILM~ERODT (C.). H&gm 0arriel.e . WALLACH (0.). Preparation of Organic Fhddea BAMBEILGER.(E.). Reaction of Potsssim Cyanide wik &&&xy'EE Chloride . $BEERSON (W. H.). Oidatdn oS'Ni&itylene . WEDMAX (0,). Intramolecrmlas Chsngee in the Pmpyl-gmapob the Cumene SeEies . , . W ~ M A N (Or). Reciprocal Transformations of Cymene- and .Cumenederiva- tivea ., . FHTICA (F.). A Fourth Monobromophenol and a &mnd Monobrmoben- NISTZKI (R.j. Cknstiktion of N'itranilic Acid . (LJ. Aniline and its Homnlogues . CLAUS (A.) and H. HIBZBL. Alkyl-derivatives of Aniline . ~ X D M E Y E R (T.). Action of Ethyl Imidoombonate on Armmtio dythd compounds .. -. BIEMSEBT (I.) and A. Gt. PALMER, Decomposition of -0-ompounds by Alcohol: Pmdiazotolueneorthos?.zlthoaic Acid . ~ R N B (F.). Ocklbenzene . - . c * zene -. * . WXLLACH (0.). Diazo- and Diamamid6-compounde . &WERE (E.). Hydrasines . Bwmw (C.). Phenyi3~ydrezine-compollnds . BUDIN (J. A.). Dicyrulphenylhy~~ne-compoPnds . &tkNTHSEN (A.) and H. SCE.ppre2TZZle'R. PhenaAd&atives . B~~NTHSEN (A). Conetitution of the S W n e a . W X N E ~ (A.).Metanitromethylsa~cylaldehyde and its Derivataves . EREKEUUB (E.). Action of Sulphuric Acid on h m s t i c Kkones . J~LENLTEYEB (E 9, juu. Pliichl'e Phenylglycidio Acid .. EXPP (A.). Para- and Ortho-nitrophenylosyacrylic Aeid . HENTSCHBL (W.). Derivatives of' Metkl C'8laadilate + . USEX (I.) and A. Gt, PALMER. Benaoic &lphihide . Ilar#as~~ I.) and A. Gd PALMEB. Pamthorybenzoic BdpWde . -SEN {I.) and W. 5. BAYLEY. Yambromobemic 8dphinide. ~WJTIEB (EL.). Chlorine-derivativea of Acetophenme . -HAS (R.). dmido-auids . m o w (C.) - Ethylphthdylacetoaetate . BWSEBT (I.) and C. S. PALXBR. Benzo~1taluenesulphcun;lmide . SCHNEE~VSS (E, A). Sepmtion of the two Leomeric 'Ibluidinesul-phunic Acids . &OPNEIDEE 6. A$ A&m-if Sulph&c A& on kph!kwtoluenesulphoni~ Acids .~ E ~ ~ s E N (1.j and W. H. EMEBSON. Oxidation by mmnu of Pcitasaium Permanganate . KELBE (W.) and N. v. CZAZLNOMSZL Aebion of Bromine and Water on a-Metaisocymenesulphonic Acid : Constitution of u+ and @-Metaim- FIsCHEB (E ). Syathesie af Indde-de&&vm . BMXEB (E,). Indolee from Phenylhydraaine . WER (A.). Indolbs from Medydmzinebenzoic Acid . oymeneeulphonic Acids . WEN (J.). Indoles from Meth lphenylhydrsaine . mCHUTZ (B.).blumini\l91~BlQlide&&C&a . 5 2 XiX PAQB 126 1W I* lzf 128 129 129 130 130 131 iae 18% 130 138 134 184 134 184 1% 136 . 137 138 . 138 . 189 . 139 . 146 . 141 . 141 . 142 . $la . 14% . 143 . 144 . 1 4 . 144 . 1% . 145 i38,lM 146 1-43 146 147 148 1443 149 149 156xx JONTENTS . LIPPMANN (E.). Dehydrogenation by means of Benzoic Peroxide .ELBS (K.). Formation of Substituted Stilbenes . EI. BS (K.) and F . BAUER . Substituted Stilbenes . GRAEBE (C.) and A . PEER . Euxanthone-group . MELDOLA (R.) . Preparation of Dinitronaphthylamine : Metanitrophenyl- azodimethylamidobenzene . WITT (0 . N.). Eurhodines and Laurent’s Naphthase . SCHLIEPER (A.). Indoles from P-Naphthylhydrazine . HECHT (H.). Action of Monamines on Citric Acid . STOKES (H . W.I and H . T . PECHMANN . Action of Ammonia 011 Ethvl Acetone- dicLrboxyiate . Synthesis of Pyridine-derivatives . : LADENBURG (A.) and C . F . ROTH . SEYFFERTH (E.). Derivatives of Picolinic and Nicotinic Acids * CLAUS (A.) and F . COLLISCHONN . Bromoquinoline . XNORR (I,.). Synthetical Experiments with Ethyl Acetoacetate .SKRAUP ( Z . H.) and P . BRUNNER . Metaquinolinecarboxylic Acid LADENBURG (A). Synthesis of Active Conine . LIEBRECHT (A.). Reductionof Nicotine . BAMBERGER (E.) . Sparteine . H ES BE (0.). Pseudomorphine . GOLDSCHYIEDT ((3.). Papaverine . JAHODA (R.). Papaverine Salts . SKRAUP ( Z . H.). Constitution of Cinchonine . LADENBURG (A.). Specific Rotatory Power of Yiperidine Bases . MERLING ((3.). Action of Bromine on Dimethylpiperidine . BIKFALVI (K.). HEmin Crystals . LINTNER (C . J.). Diastase . MUELLER (H.). Action of Diastase and Invertin . LE BEL (J . A.). Russian Petroleum . Bases from Animal Oil . NORTON (L . M.) and A . A . NOPES . OTTO (R.) and A . ROSSING . LINDET (L.). ROMBURGH (P . v.). Action of Heat on Ethylene . Reaction of Organic Bisulphides with Potas- sium Sulphide .Action of Alcohols on Aurophosphorous Chloride . Dextrorotatory Hexylic Alcohol . Formation and Composition of Humous Substances . Action of Hydrogen Chloride on Mixtures of MEYRR (V.). Thiodiglycol Compounds . BAUMANN (E.). Preparation ofBenzoic Ethers . KILIANI (H.). Arabinose . Aldehyde with Alcohols . MIXTER (W . (3.). Acid Propionates and Butyrates . MEYER (V.). Preparation of /3-Iodopropionic Acids . ROMBIJRGH (P . v.). Methylisopropylacetic Acid . REIMER (C . L.) and W . WILL . methylenecarboxylate with Lime . OST (H.) and A . MENTE . Oxalimide . WISLICENUS (W.). Ethyl Oxalacetate . THIERFELDER (H.) . Glycuronic Acid . WATTS (F.). Fermentation of Citric Acid . Decomposition of h i d e s by Water and Dilute Acids . BRUNSWIGF (H.). Derivatives of Acetothienone .DAMSKY (A.). Isomerism of the Thiophenic Acids : Derivatires of P-Thio- phenic Acid . ERNST (F.). Reduction of aa-Thiophendicarboxylic Acid . CONRAD (M.) and M . GUTHZEIT . ROMBURGH (P . T.). CLAUS (A.) and E . TRAINER . Decomposition by Heat of the Nitrates of Amines Erucic and Brassic Acids . COLMAN (H . G.) and W . H . PERKIN, Jun . Distillation of Calcium Tetra- BERTHELOT and ANDRB . EENST iF.\. Svnthetical Investica6ons in the ThioDhen Series . PAUE 151 151 151 152 152 153 153 154 155 157 157 158 159 160 160 161 162 163 163 164 164 164 164 165 165 166 225 236 226 227 228 228 228 229 229 230 231 231 232 232 233 234 234 234 235 235 235 236 23’1 237 238 KUES (iV.j and‘C . PAAL . SynthYesis of a-Phenylthiiphen . 238CONTENTS . xxi KPEKELEB (K.).Pentathiophen-group . CIAMICIAN (G.) and P . SILBER . Action of Light on Nitrobenzene . CuUs (A.) and E . PIESZCEK . Orthoethpltoluene . HEYMANN (€3.) and W . KOaras . BLAU (F.). Action of Sodium Methoxide 011 Bromobenzene . OTTO (R.) and A . ROSSING . JACKSON (C . L.) and A . M . COMEY . Action of Silicon Fluoride on Organic Bases . MERZ (V.) and P . MULLER . FISCHER (0.) and E . HEPP . Action of Alcoholic Hydrogen Chloride on Nit*rosamines . HOOGEWERFZ (S.) and ,W . A . VAN DORP . Benzylamine and Phenethyl- amine . ROWBURGH (P . v.). Isodinitrodimethylaniline . BERNTHSEN (A.). New Synthesis of Thiodiphenylamine . BENDER (G.). Ethereal Carbonates . WALDER (F.). Benzyl-derivatives of H-$.roxylamine . KNORR (JJ.). Correction . WITT (0 . N.), Action of Ethyl Acetoacetate on Aroniatic Diamines .DAHM (C.) and K . GASIOROWSKI . Condensation Products from Carbo- imides and Orthodiamines . MENTHA (E.) and K . HEUMANN . Parachlorazobenzene-derivatives . MENTHA (E.) arid K . HEUMANN . Cyanazobenzene and Yarazobenzenecar- Oxidation of Homologues of Phenol . Bisulphides with Mixed Organic Radirles Aniline and Diphenylamine from Phenol . boxylic Acid . MENTHA (E.). Chloroparazotoluene . GOLDSCHMIDT (H.). Reduction of Aldoximes and Acetoximes . BERNTHSEN (A.). Pyrogeniu Formation of Phenazine . NIETZKI (R.). Safranine Dyes . WITT (0 . N.). Constitution of the Safraninee . NIETZKI (R.). Constitution of Ssfranine . OSBORN (T . B.) and W . C- . MIXTER . Paranitroformanilide . Action of Concentrated Sulphuric Acid on Aromatic Eetones .MATTHIESSEN (C . H.) and W . G . MIXTER . DYER (J . 0.) and W . G . MIXTER . CLATJS (A.). Orthazoparabromacetanilide Halogen-derivative of Oxanilide . PAMPEL (0.) and G . SCHMIDT . Aromatic Ketones . ERAFFT (F.). Benzene-derivatives of High Molecular Weight . CLAUS (A.) and E . FICKERT . Paraxylyl Ethyl Ketone . NEUMANN (G.). Nitrophenyl Benzoates and Nitrobenzoates . Hydrocarbons . PL~CHL (J.). Phenylglycidio Acid . NEP (J . U.). Benzoquinonecarboxylic Acids . LIEBERMANN (C.). Constitution of Azo-opianic Acid . LIEBERMANN (C.). An Isomeride of Hemipinimide . ELKAN (T.). Isomeric Aldehydophenoxyacetic Acids . ELKAN (T.). Vanillinoxyacetic Acid . GERSON (G.). Derivat.ives of Pyruvic Acid . EUES (W.) and C . PAAL . Diketonic Acids . HANTZSCH (A.). Furfurane-derivatives from Resorcinol .OTTO (R.) and A . ROSSING . Sulphobenzidedisulphonic Acid . VALLIN (K.) . Metatoluenesulphonic Acid . ELASON (P.). Toluenedisulphonic Acids . LELLMANN (E.) and 0 . BONHOFFER . Introduction of Lhrboxyl into Aromatic LANG (E.). Action of Zinc Alkyl Compounds on Ethyl Malonate . LANG (E.). Furfurane-derivatives from Phloroglucinol . OTTO (R.) and E . ENGELHARDT . Phenylsulphinacetic Acid . CLAUS (A) and J . A . SCHTJLTE IM HOF . FISCHER (E.) . Cumene-orthosulphonic Acid and Orthocumic Acid . Action of Aldehydes, Anhydrides, and Diazo-compounds on the three Methylindoles . BEINITZEB (F.), Hydrocarrotene and Carrotene . PAGE 239 244 240 241 242 242 243 243 244 245 245 245 245 2% 247 247 247 247 218 258 249 249 249 250 250 250 251 251 251 252 252 253 254 254 254 255 257 258 259 260 261 261 262 262 263 263 263 264 258 264 265 265x xii CONTENTS PAGE EEMILTAX m.).Diphepylmetaxylylmethaneand Diphenylorfho-xyly~methane 266 CLATJS (A.) and M . ERLER . 268 CLAUS (A.) and 0 . SCHMIDT . @-Naphthol-@-disulphonic Acid . 269 CLAISEN (L.). Action of Aldehydes on Phenols . 270 CLAVS .( A.) and P . FEIST . a-Naphthyl Methyl Ketone . 271 BAMBERGER (E.) and M . PHILIP . Pyrene . 271 PESCI and BETTELLI . Terebenthene-derivatives . 272 KOSTANECEI (S . v.). Bormation of Euxanthic Acid . 272 CIAMICIAN (G.) and P . SILBER . Synthesis of Ygrroline . 273 CIAMICIAN (G.). Behrlviour of Methyl Ketole : Conetitution of P.yrroline . 273 PAAL (C.) and C . w . T . SCBNEIDER . 2'73 EITORR (L.). Syntheses by Means of Ethyl Acetoacetate .275 KEISER (E . H.). 272 LIPP (A.). Tetrahydropiwline . 277 CLAUS (A.) and P . KUTTNEP . Quinolinesulphonic Acids . 278 XNORR ~~ . (L.) and C . KLOTZ . 2'78 BENDER (F.) and G . SCQTJLTZ . Diamidostilbene . 268 Bromo-derivatives of Diphenic Acid . PEREIN (A . G.) and W . H . PERPIN, Jun . Kamda . 272 Synthesis of Pyrroline derivati~es Action of Chlorine on Pyridine . Reduction of HgdrosylepiYdine and Mothyl- lepidone . ;REHER (L.). a- and y-Ethyl Quinolines . BRUCKE (E. v.). Colour Reaction of Guanine . PLUGQE (P . C.). Opium Alkalo'ids . COMSTOCE (W . J.) and W . KOENIGS . Cinchona Alkalo'ids . LOEBISCH (W . F.) and P . SCHOOP . Strychnine . LADENBURG (A.). Specific Rotation of Pigeridine Bases . HESSE (0.). Alkaloids of the Berberidese . BRIEGER (L.).A New Ptoma'ise producing Tetanus . NEUMEISTER (R.). AJbumoses . NETJMBISTER (R.). Vitelloses . GRIMAUX (E.) and C . CLOEZ . Erythrene-derivatives . BARATAEFF (S.) and A . SAYTZEFF . Trimethyl Carbinol . USTINBFF (D.) and A . SAYTZEFF . Dipropyl Carbinol . DIEFF (W.). Action of Silver Acetate on Tetrabromodiellyl Cstrbiuol . CUISINIER ( L . ) . Glucose and the SWc harification of Starch . BOCRQTJELOT (E.). Action of Saliva on Starch . BOURQUELOT (E.). Starch Granules . MAQTJENNE . Inosite . MALBOT (H.). Preparation of Tsobutylamiaes . MALBOT (8.). Senaration of Mono- and Di-isobutylamines . ZEISEL (5.). Colchicipe . MERCK (C . E.). EcgQnine . Co~sop (A.). Erythrol . 279 . 280 . 280 . 281 . 282 . 282 . 283 . 204 . 284 . 284 . 286 . 352 . 353 . 353 . 353 .354 . 354 . 355 . 355 . 356 . 357 . 357 . 285 . 8% BAMBERQER'(E.). Synthesis of Guanylcarbarnide . GATTERMANN (L.) and Gt . SCHMIDT . Preparation of Alkylamidoformic MICHAEL (A.) . Convenient Method of Preparing Brominated Fatty Acids . MICHAEL (A.). Behaxiour of Acetic Acid and its Derivatives to Phosphorus Pentachloride . Chlorides and Alkyl Isocvanates . USTINOFF (D.). p-Dimethacrylic Acid . HAZTJRA (K.). Acids from Drying Oils . BARATAEFF (S.). Methoxydidylacetic Acid . FLICEHINGER (EL) . Oxalic Acid from the Residue of S@ritlss atheris IVitrosi . SCHATZEY (E.). Preparation of Ethyl Acetate . DAIMLER (C.). Action of Ethyl lodide and Zinc on Ethyl Malonate . BARATAEFF (S.). Action of Ally1 and Ethyl Iodides on Ethyl OsaIate . FITTIG (R.) and C . DAIMLER .Action of Ethyl Chloracetete a i d Zinc on Ethyl Oxalate . ROME& (M.). Nitration of a-Tbiophenic Acid . SCHATZEY (E.) . Diallyloxalic Acid . 358 358 359 359 359 359 360 360 360 361 361 361 362CONl’EN ‘1’S xxiii BAEYEB (A.) . Constitution . of Benzene . LADENBURG (A) . Constitution of Benzene . SEPLIG [E.). Chlorination of Toluene . GOLDSCHMIDT (H.) and M . HONIQ . Nitrochlorotolueiie and Clilorotoluidine THOMSEN (J.). Constitution of Benzene . KLABON (P.). Synthesis of Cyanphenin . MEYEE (E . v.) . Synthesis of Cyanphenin . BAESSLER (A.). ‘&in01 and its Derivatives . MICHAELIS (A.) and F . SCHMIDT . Isomeric Mono- and Di-benzoylphenyl- h ydrazines . BILLETEP (0.) aud A . STEINEB . Thiocarbimides of Bibasic Aromatic Radicles . MICHAELIS (A.) and L . WEITZ .Trianisylarsine and its Derivatives . MICHAELIS (A.). Organo-bismuth Compounda . MICHAELIS (A.) and A . POLIS . Triphenylbismuthine and its Derivatives . S~EULZE (E.) and E . N h m r . Phenylamidopropionic Acid obtained from Q~IBAUD (H.). Physical Peculimity of Triphenylguanidine . HOTTER (E.). Synthesis of Phenylaceturic Aoid . the Decomposition of Prote’ids . BAEYER (A.). Reduction of the Phthalic Acids . Action of Potassium Hydroxide on Mixed Alkyl Bisulpliides . Action of Sulphurous Anhydride onJ3enzene . * . Action of Potassium Hydroxide on Phenylene- MUNCHYEYE? (F.). Action of Hydroxylamine on Diketones . EKSTBAND (A . Gt.). Naphthoic Acids . RICHTER (E.). a- and /3-Naphthenylamidoxime . CLEVE (P . T.). Chloronaphthdenesalphonic Acids . FOBSLIKG (S.).Bronner’s j3-Naphthylaminesulphonic Acid . O T ~ O (JL) and A . ROSSING . COLBY (C . E.) and C . 5 . MCLOUBHLIN . OTTO (8.) and A . ROSSINQ . mefadiphenylwlphone . GOSKE (A.). Bynthesis of Carbazole . SOLTSIEN (P.). Essential Oils . HALLER (A.). Isomeric Camphols and Oamphora . LEUCKART (R.). Carveol, Borneol, and Menthol . LETJCKAPT (R.) and E . BACH . Bornylamine . . GEAM (C.). Active Principles of Asckpias currmsavica, A . incarnata, and CIAMICIAN (Gt.) and P . SILBEP . Conversion of Pyrroline ink0 Pyridine- derivatives . ALTAR (S.). Oxidation ot Symmetrical Triallylpyridines . LA COSTE (W.) and F . J7ALEUR . Quinoliiiedisulphonic Acid and its Derira- tives . HOFMANN (A . W.). Quinoline-red . CLEVE ( P . T.). Compound of Qninoline with Formamide . PANAJOTOW ((3.).1 : 3 Dimethylquinnldinc . HINSBERG (0.). Nomenclature of the Quinoxaline Series . LETJCKART (R.) and A . HEI~RMA” . Nitrotolylglycine and Oxydihydrotolu- Yilzcetoxicum ofleinalis . LIWEH (T.). 2 : 6 Dimethylpyridine Platinochloride . quinoxaline . LIWEH (T.). Conyrine Platinochloride . FREUND (M.) and W . WILL . Hydrastine . BECKUXTS (H.). Ptomaines . GRAM (C.). Origin of Ptoma‘ines . LOEW (0.). Diastase . . EKGLER (V.) and iM . BOEAM . Veaelin . MAGNAMINI ((3.). Piperilene . PISANELLO (Gt.). Hydrogenation of Propionitrile . WALLACH (0.) and F . LEHMANN . Atation of Phosphorus Pentachloride on Substituted Pormamides and on Piperidine-derivatives . PAGE 362 362 362 362 363 363 363 364 365 366 366 367 868 368 368 369 370 371 371 372 312 373 373 374 374 375 375 375 376 376 377 378 378 378 3’79 380 381 381 382 383 383 883 384 385 387 .387 456 457 457xxiv CONTENTS .BERTONI ((3.). Ethereal Salts of Nitrous Acid . POMEY (E.). Compound of Propyl Alcohol and Phosphopletinous Chloride . LOEW (0.). Formose . SELIWANOFF (T.). Reaction for Fruit-sugar . MACQUENNE . Inosite . HORVAT (V.). Dry Distillation of Starch with Lime . MAYER (A.). Nature of Niigeli’s Starch.cellu1ose . SCHULZE (E.) and E . STEIGER . Paragalactin . LANGELI (T.) . Trimethylpropylammonium Iodide and Hydroxide . MALBOT (H.) . Salts of Di-isobutylamine . BARBAGLIA (Gt . A.). Isobutaldehyde and its Polymerides . BARBAGLIA (G . A.). Action of Sulphur on Aldehydes . FASBENDER (H.). Compounds of Aldehydes and Ketones with Mercaptan . CLAISEN (L.). Action of Nitrous Acid in Ketones .AUTENRIETH (W.). Dimethylene Disulphone-derivatives . TAFEL (J.). y-Amidovaleric Acid . STADELMANN (E.). Hydroxybutyric Acid in Diabetic Urine . WOLFF (L.). p-Bromovderic Acid . KILIANI (H.). Axabinosecarboxylic Aoid and Arabinoee . FRANCHIMONT (A . P . N.). Action of Nitric Acid on Bibasic Acids . BE RGREEN (H.). Isonitroso-compounds . BURTON (B . S.) and H . v . PECHMANN . Action of Phosphoric Chloride on Ethyl Acetonedicarboxylate . HENTSCHEL (W.). Aconitic Acid . TAFEL (J.). Reduction of Dihydroxytartaric Acid Diphenylhydrazide . BGUTROUX (L.). Gluconic Acid . MICHAEL (A.). Constitution of Trimethylenetricarboxylic Acid . FRANCHIMONT (A . P . N.) and E . A . KLOBBIE . Amides of Ethylsulphonic Acid . DEL~PIN (S.). Calcium Urate . HILL (H .B.) and L . L . JACKSON . Chloropyromucic Acid . CANZONERI (F.) and V . OLIVERI . Transformation of Furfuran mto Pyrroline . TAFEL (J.). Furfurylamine . LEKO (M . T.). Thioplien in Aniline . EXNST (F.). Reduction of a-Thiophenic Acid . SCHULZE (K . E.). Constituents of Coal-tar . FILETI (M.). Reciprocal Transformation of Cumene and Cymene . PERATONER (A.). Oxidation of the Methyl Ethers of Mono- and Di-brom- orthoisopropylphenols . PONEY (E.) . Compound of Orthotoluidine with Cupric Chloride . POMEY (E.). Compound of Paratoluidine with Cupric Chloride . NIETZKI (R.) and F . KEHRMANN . TBUHL~R (J.) . Thioparatoluidine . SCHOOP (P.). Preparation of Dimethylaniline . HEIDLBERG (T.). Ortho- and Para-chlorodimethylaniline . GOLDSCHMIDT (H.) and E . EISSER . Carvole-derivatives .HINSBERG (0.). Action of Orthotoluylenediamine on Dextrose . Secondary and Tertiary Qninones . QRIESS (P.) and G . HARROW . NIETZKI (R.) and E . HAGENBACH . Tetramidobenzene and its Derivatives . CHETMICKI (’3 . v.) . Carbonylorthamidophenol and Thiocarborthamido- phenol . KLASON (P.). Substitution of Amidogen by Hydrothionyl and Oxjsul- JANOVSKP (J . V.) and L . ERB . Halogen-derivatives of Azobenzene and JANOVSKY (J . V.) and L . ERB . Direct Substitution-products of Parazo- ENGLER (C.) and C . SCIIESTOPAL . Action of Acetone on Pnramidoazoben- zene . Action of Aromatic Iliamines on Sugars phuryl Groups . Hydrazobenzene . toluene : Hydrazobromvbenzenes : Hydrazobromotoluenes . PAGE 468 468 469 459 459 460 460 460 461 461 461 462 462 463 463 463 464 464 465 466 466 467 467 467 468 468 468 469 469 470 4’70 471 471 471 47 1 472 47 2 472 4’72 473 474 474 475 475 476 476 477 478 478 479 479CONTENTS .HEUMANN (K.) and L . (ECONOMIDES . Action of Phenol on Diazoamidoben- zene . BERNTHSEN (A.). Constitution of the Safranines . M~~HLHAUSER (0.). Manufacture of Methylene-blue . LEVI (L . E.). Thiophen-green . MICHAEL (A.) . Action of Phosphorus Pentachloride on Acetanilide . MUNCHMEPER (F.) . Action of Hydroxylamine and Phenylhydrazine on Dialdehydes and Ketones . LANDSBERG *(L.). Preparation of Vanillin . BUCHKA (K.) and P . H . IRISH . Action of Potassium Ferricyanide on Aceto- phenone . BROMME (W.). Metacyanobenzoic Acid . BROMME (W.). GRIESS (P.). Meta- and Para-hydroxynitrobenzoic Acids . DIEHL (L.) and A .EINHOBN . Derivatives of Orthamidophenylvalerk Acid . PERATONER (A.). Substituted Mono- and Di-bromosalicylic Acids . PERATONER (A.). Constitution of Dibromosalicylic Acid . BUCHKA (K.). Formation of Phenylglyoxylic Acid from Benzoic Cyanide . VALENTINI (A.). Methyl ?VIethyldibromoparacoumarate . REQEL ((2.). Oxidation of a- and P-Hydroxypiperic Acids . MOIN~ (F.). Action of Bibasic Acids on Thiocarbltmide . WISLICENUS (W.). Action of Phenylhydrazine on Lactones . LELLMANN (E.) and C . SCHLEICH . Nitrobenzyl-derivatives of Ethyl Malo- nate . PIUTTI (A.). Synthesis of Ethereal Salts of Trimesic Acid . KLASON (P.) . Toluenedisulphonic Acids . GOLDSCRMIDT (H.) and N . POLONOWSKA . Diphenylhydroxyrthglamine . MASON (A . T.). Condensation-derivatives of Ethjlendiamine .CLAISEN (L.). Condensation of Aldehydes with Phenols and Aromatic Amines . CLEVE ( P . T.). Action of Cblorine on Acet-a-naphthalide . SPTCA (M.). Naphthoxyacetic Acids . BAMBERGER (E.) and M . PHILIP . BAMBERGER (E.) and M . PHILIP . Pyrene . GOLDSCHMIDT (H.). Camyhoroxime-derivatives . WILL (W.). Naringin . EIJKMAN (J . F.). Substances from Illiciurn Teligiosum . DE ZAAIJER (H . G.). Andromedotoxim . JAWEIN (L.). Crystalline Compound from Kamala . HURST (G . H.). Algaborilla . KULZ (E.). Indian-yellow and Glycuronic Acid . LADENBURG (A.) . Yjrrolidine . DURKOPF (E.). Preparation of Pyridine Basw . LUNGE (G.) and J . ROSENBERG . Coal-tar Lutidines . CANZONEBI (F.) and G . SPICA . Ethoxglutidine . CONEAD (M.) and M . GUTHZEIT . Action of Ammonia and Primary Amines on EthylDimethylpyronedicarboxylate .CONRAD (M.) and W . EPSTEIN . Lutidine-derivatives from Lutidonecar- boxylic Acid . COLLIE (N.). Condensation-product of Ethyl Amidoacetoacetate with Hydro- chloric Acid . CONRAD (M.) and M . GUTHZEIT . Ethyl Dimethylpyronedicarboxylate . LELLMANN (E.) and H . ALT . Quinolhe . TORTELLI (M.). Synthesis of Metaquinolinecarboxylic Acid . DOEBNER (0.). a-Alkylcinchonic Acids . HOOGEWERFF (S.) and W . A . VAN DORP . Isoquinoline and its Derive- tives . DOTT (D . B.). Acid Morphine Acetate . Behaviour of Cyanobenzoic Acids on Dry Distillation . Acenaphthene and Naplithalic Acid XSV PAGE 480 480 480 481 481 482 483 483 484 484 485 485 486 487 487 488 488 489 489 490 491 491 492 493 494 494 495 495 496 496 497 497 497 498 498 498 499 499 499 499 500 501 501 502 502 503 504 505 505 HANSENN (A.). Constitufiion of Brucine .505XXVi CONTENTS . EIJKMANN (J . F.). Hpdrastine . ANTRICK (0.). Optical Behaviour of Coca'ine . KOSTIEILINA (S.). Action of Pepsin on AmyloYd . MARTIN (8 I-I . C.). Vegetable Globulins . RENARD (A.). Action of Heat on Heptine . BENDER ((3.). Bismuth Thiocyanate . SMOLKA (A.). Action of Potassium Permanganate on Dextrose in Neutral Solution . FISCHER (E.). Compounds of Phenplhydrazine with Sugars . MAUMEN~ (E.}. Action of Nitric Acid on Sugar . MYLIUS (F.L Iodide of Starch . GOLDSCPMIPT (H.). Reduction of Aldoximes and Acetoximes . SANDMEYER (T.). Action of Nitrous Acid on Acetone . ENGEL (R.). Corrdensation of Acetone and Chloroform . GATTERMANN (L.) and G .SCHMIDT . Chloroformamide : Synthesie of Aro- matic Acids . WILLGERODT (C.) and F . DURR . Tertiary Trichlorbutil Choride and Ether . MABERY (C . F.). Substituted Acrylic and Propionic Acids . GLADYSZ (T.) . Preparation of Calcium and Potnssium Tartrates . HCHIFF .(H.) .. FQrfuraldehyde . METER (V.). Negative Nature of the Phenyl-group . FERKO (P.). Pyrogenic Reactions . POLIS (A.). Aromatic Lead Compounds . NEUMAPN (G . S.). Sylphuric Acid as an 1odine.Carrier . PURGOTTI (A) . Tribromophenol . MULHAUSER (0.). Manufacture of Resorcinol . NIETZEI (R.) and J . PREESSER . Constitution of Dinitroquinol : Formation of Nitranilic Acid . CLAISEN (L.). Action of Sodium Alkoxides on Benzaldehyde . NIETZEI (R.) and F . KEHRYANN . Quirionedioxinie and Dinitrosobenzene .CLAISEN (L ..} . Iptroduction of Acid Radicles into Ketonen . WULFING (A.). Separation of Ortho- and Para-toluidine . MUHLHAUSER (0.). Manufacture of Dimethylaniline . MERZ (V.) and P. MULLER . Coiiversion of Phenols into Amines . Moos (I?.). Condensation Products of Ethylene-aniline with Aldehydes . HANSSEN (A.). Action of Carbonjl Chloride on Ethylene- and Trimethylcne- diphenyldiamine . ZIEGLER (J . H.) and M . LOCHER . The Tartrazines ; a New Class of Dyes . ZIEGLEK (J . H.) and M . LOCHER . Condensation Products of Secondary Hydrazines with Dihydroxytwtaric Acid . DAHL (A) . Preparation of ~enzylrosaa~linedisulphonic Acids . MUHLHAUSER (0.). Manufacture of Benzaldehyde-greens . LIEBERMANN (C.) and P . SIEDLER . Opiaurin . BRODSEY (L.). Action of Aldehydes on Ammonium Thiocganate .HELMERS (0.). Additive Products of Aromatic Thiocarbimidea . BEUBERT (K.). Manganese Benzoate . MICHAEL (A.) and G . M . BBOWNE . Isomerism in the Cinnamic Acid Series EDELEANO (L.). Derivatives of Phenylmethacrylic Acid and of Yhenyliso- butyric Acid . CLAISEN (L.) and 0 . LOWMAN . LIEBEWANN (C.) and S . KLEEMANN . Preparation of Ethyl Benzoylscetate . Etherification of Opianic Acid . BOTTINQER (C.). Oak Tannin . KLEEMLNN (S.) Reduction of Nitrio-opianic Acid . SALOMON (0,) . J/-Meconine . BOWMAN (W.). Action of Potassium Cyanide on Meconine . EUHARA (M.). Orthotoljlphthalimide . WISLICENUS (W.). Synthesis of Ethyl Salts of Ketouic Acids . PIETTI (A ) . Synthesip of Ethyl Trirnesate . FISCHEB (E.) and P . WAGNER . Rosiadoles . PAGE 605 506 506 507 565 566 566 667 667 568 568 568 669 569 570 670 671 671 672 572 572 573 673 674 574 574 575 575 576 576 576 577 577 578 579 579 579 580 580 581 682 582 5&3 583 584 584 584 585 586 586 587 587 588CONTENTS .X FIsHEB (E.) and A . STECHE . Methylation of Indole-derivatives . ADAM (P.). Diphenyl-derivatives . GBAEBE (C.) and C . AUBIN . Condensation of Diphenic and Orbhodiphenyl- carboxylic Acids . GPAEBE (C.). Formula of Diphenic Acid . LELLMANN (E.). Preparation of B-.Nitronaphtlialene . NIETZKI (R.) and J . GOTTIC: . B-a-Azonaphthalene . WITT (0 . N.). New Method of Preparing Azines . WITT (0 . N.). Constitution of Isomeric Tolunaphthazincs . B IRU K OFF ( W . ) . D imet hy lan thragallol WEND E (H . ) . Trimet h y lanthragallol . Chloride on Anthracene Dihpdride .BRAE BE (C.) . Acenaphthene . QUINCKE (F.). Derivatives of Acenaplithene . LIEBERMANN (C.) and W . WENSE . Hydroxyanthraquinone Dyes . BEHLA (G.). Substituted Anthracene-carboxylic Acids : Action of Carbonyl TANRET (C.). Nitrogen-derivatives of Tehebenthene . WALLACH (0.). Terpenes and Ethereal Oils . WEBER (E.). Ethereal’ Oils . BOUCHARDAT (G.) and J . LAFONT . Active Camphelie and Ethylborneol . CIAMICIAN ((3.) and I? . SILBER . Determimtion of Positions in the Yyrro- line Series . CIAMICIAN (G.). Tetriodopyrroline . DENNSTEDT (M.) and J . ZIMMERMANN . Reactiqn of Acetone with Pyrdine PLOCHL (J.). Synthesis of Pjridine Bases . MUTHMANN (W.) aud J . U . Nef . RIEHM (P.). Condensation Products of Acetone and Acetoplienone with Aniline and Ammonia .KOENIGS (W.) and J . LJ . NEF . 4’-Phenylquinoline and the Derived Di- quinolyls . FISCHER (0.). Ortho- and Meta-quinolinesulphonic Acids . HNORR (L.). Synthetical Experiments by Means of Ethyl Acetoacetate . CONINCK (0 . DE) . Alkaloids . LELLMANN (E.). Phenylpiperidine . SCIXILBACH (C.). Berberine Salts . SCHMIDT (E.) and 0 . SCHILBACH . Ac ion of Potassium Permangauate on Berberine . KASSNER ((3.). Lactucerin . MYLIUS (F ) . Cholic Acid . YCHOTTEN (C.). Bile Acids . \VT-BSTER (C.). Behaviour of Hydrogen Perolide to Albumin . BOURQUELOT (E.). Deterioration of Diastase by the Action of Heat . KRAMER (G.) and W . BOTTCHEB . The Relation between Petroleum and the Hydrocarbons of Coal tQr and Shale-tar . MULLER (J . A.). New Class of Ferrscjanides and Ferricymidee .RATHKE (B.). Nelamines . RATHKE (B.). Thiammeline . LIEBERMANN (C.) and 0 . BERBAMI . Coccerjl Alcohol and Coweqlic Acid . FISCHER (E.) and J . TAPEL . Oxidation of Polyatomic Alcohols . kPPMANN (E . 0 . v.). A New Galactan : Properties of Galactose . MALBOT (H.). Preparation of Norm3 Propplamines and Isoamylamines . COMBES (A.). Homologues of Acetylacetone . LWOFF (J.). Fatty Acids in Resin . GEHRINB (G.). Octyl Mono., Di., and Tri-chloracetates . RENARD (A.). Metallic Propionates . WISLICENUS (J.). Chloro-derivatives of Crotonic Acid . MICHAEL (A.) and (3 . M . BROWNE . Isomerism in the Crotouic Acid Series . Cinchonic Acid STOEHR (C.). Strychnine . PAGE 588 559 589 589 590 590 590 591 592 592 592 693 593 593 595 596 596 5Y6 597 597 598 598 598 599 599 601 601 603 604 604 604 604 605 606 606 607 608 648 649 650 650 650 651 652 652 653 653 653 654 655 656xxviii CONTEZVTS .COMBES (A.). Synthesis in the Para5n Series by Means of Aluminium Chloride . SMOLKA (A.). Action of Bromine on Carbamide . UUNTZ . Antimony Tartrate . PAAL (C.). Constitution of Pyrotritartaric Acid . DIETRICH (F.) and C . PAAL . Pyrotritartaric Acid-derivatives . CANZONERI (F.) and V . OLIVEEI . /?-Bromofurfuran . JACOBSEN (0.) and W. DEIKE . Synthesis of Hemellithene . MAYER (F.). Reduction of Trinitro-+-cumene . JACOBSEN (0.). Action of Sulphuric Acid on Pentamethylbenzene . WILL (W.) and W . PUKALL . Resorcinol-derivatives . PUKALL (W.) . Resorcinol-derivatives . RATHKE (B.) . Triphenylthiammeline and a Third Triphenylammeline .MULLER (P.). Primary and Secondary Xylsmines from Xylenols . MICHAEL (A.) and Gt. M . BROWNE . JANOWKY (J . V.). Azo-compounds . HEUMANK (K.) and L . OECONOMIDES . Reaction of Diazoamido-compounds with Phenols . . ENORR (L.) . Cinnamylhydrazine . BERNTHSEN (A.). Phenazoxine . ZELINSKY (N.) . Action of Dehydrating Agents on Benzylideneacetoxime . BEEGNTHSEN (A.) and A . GOSKE . Methyl-orange and Ethyl-orange . WEDDIQE (A.) and H . FINGER . Action of Nitrous Acid on Orthamido- benzamide . SULKOWSKI (J.). Oximes of Paraxyloquinone . NOERRISON (C.). Bromorthotoluic and Bromorthophthalie Acids . MICHAEL (A.). Reduction of the Isomeric Bromocinnainic Acids . WEINREICH (S.). Mono- and Di-hydroxvtoluic Acids . ZELINSKY (N.). Ethyl Phthalate Chloride . HOTTE (B.). HENDERSEN ((3 .(3.). Ethyl Triphenylcarbinylmalonate : /I-Triphenyl- MICHAEL (A.). Action of Ethyl Sodacetoacetate and Sodomalonate on the MICHAEL (A.). Formation of Indigo-blue from Ortho-nitrophenylpropiolic Acid . BRERNER (P.) and 0 . N . WITT . HEUMANN (K.) and J . WIERNIK . Diphenylethane-derivatives . BERNTHSEN (A.) and A . SEMPER . BAMBERGEE (E.) and 0 . BOEKNANN . /3-Naphthyl-derivatives . TANRET (C.). Action of Hydrogen on Nitro-derivatives of Terebcnthene . Manufacture of Santonin . CIAMICIAN ((3.). Conversion of Pyrroline into Pyridine-derivatives . ENORE (L ) Yyrazole-derivatives CONRAD (M.) and L . LIMPACH . Synthesis of Quinoline-derivatives by Means Aromatic Hydroxylamines Action of Phenylhydrazine on Anhydrides of Bibasic Acids propionic Acid . Ethyl Salt8 of Unsat.urated Acids . Benzidine-derivatives ZIEOLER (J . H.). Tetramethylamidobenzophenone . URBAN (C.). I, 3, Naphthylenediamine . GIMBEL (A.). Nitrosoanthrone . BOUCEIARDAT ((3.) aed R . VOIRY . Terpinol . BUSCH (A.). Synthesis of Juglone . of Ethyl Acetoacetate : y-Hydroxyquinaldine . REED (J . H.). Methylnaph tliaquinolines and ,8 .Naphthacridine . STOEHR (C.). Skatole from Strychnine . GINTL (W.) and L . STORCH . Ecgonine . LATSCHINOFF (P.). Bile Acids . LATSCHINOFP (P.). Crystalline Form of Chole’ic Acid . WTJRSTER (C.). Action of Oxidising Agents on Albumin . WTJRSTER (C.). Behaviour of Sodium Nitrite towards Albumin and Hsemoglobin . HENRY (L.). Determination of the Relative Value of the Four Units of Activity in the Carbon-atom . P A QE 656 656 657 657 658 658 659 659 660 660 661 662 663 663 663 664 665 6f15 666 666 667 667 668 668 669 669 669 671 672 672 672 673 674 674 674 675 675 675 677 677 678 678 679 681 682 682 683 683 683 711 682CONTENTS .xxix NORTON (L . M.) and H . J . WILLIANS . Action of Bromine on Isobutylene . DE LACRE (N.). Dichlorethyl Alcohol . HENRY (L.). Synthetical Acetonitrile . CLAUDON (E.) and E . C . MORIN . Alcohols in Brandy KILIANI (H.). Action of Sodium Amalgam on Arabinove . WILL (W.). Sugars from Hesperidin and Naringin . CURTIUS (T.). Hydrazine (Diamidogen) . MICHAEL (A.) Reactions with Ethyl Sodacetoacetate . NETTLEFOLD (F.). Sodium Nitrate in Gun-cotton . DIEFF (W.) and A . REFORMATSKY . Oxidation of Ricinoleic and Liiioleic Acids . HANTZSCH (A.) and 0 . WOHLBRUCK . Ethyl Propiopropionate .REFORMATSKY (S.). Synthesis of Diatomic Monobasic Acids . LANQ (E.). Decomposition of Ethyl Acetomalonate and its Homologaes . (XOLDSCHMIDT (H.) and W . SCHULTHESS . Thienethylamine . Constitution of Benzene . THIERFELDER (H.) . Glycuronic Acid . CLAUS (A.). BAMBERGER (E.) and W . LODTER . Aromatic Nitriles . HANTZSCH (A.). Constitution of Quinone-derivatives . matic Compounds . SCHNITEB (K.). Isomeric Chloro- and Bromo-thymoqninones . SANDMEPER (T.). Substitution of the Amido- by the Nitro-group in Aro- LLOYD (R.), Conversion of the Higher Homologues of Phenol into Amines JACKSON (C . L.) and J . F . WING . Dimethylbenzylamine . MEEZ (V.) and C . RIS . Action of Ethylenedkmine on Catechol . HOLZMANN (E.) Thio-derivatives of Diethylaniline and Dimethylaniline .MICHAEL (A.) and J . P . RYDER . Action of Aldehydes on Phenols . MULLER (W.). Metamethylcinnamic Acid and its Derivatives . CHASANOWITSCH (J.). Action of Phosphorus Pentachloride on Salicylic Acid . Derivatives of Ethyl Quinoneparadi- carboxylate . Conversion of Aromatic Sulphonates into Amido-compounds . Oxidation of Benzene-derivatives with Potassium F'erricyanide . Conversion of p-Naphthaquinone into Indonaphthene-deriva- tives . ROSER (W.). Synthesis of Indonaphthene-derivatives . FISCHER (0.) and E . HEPP . Ritrosamines . WITT (0 . N) . Azonium Bases . ZINCKE (T.) and A . T . LAWSON .. Azo-derivatives of Phenyl-/3-naphthyl- amine . ZINCKE (T.) and A . T . LAWSON . Orthamidoazo- and Hydrazindo-deriva- tives . NIETZKI (R.) and A . L . GUITEBMANN .Naphtholcarboxylic Acids . BAYER (F.) and C . DUISBEXG . P-Naphthylaminesulphonic Acid . NIETZKI (R.) and T . STEINMANN . Purpurogallin . BARR (A.). Nitrophenols and Phenylhydwzine . LIMPRICHT (H.). Sulphazides . GABRIEL (S.). Homophthnlimide . HANTZSCH (A.) and A . ZECGENDOBF . JACKSON (C . L.) and J . F . WING . NOYES (W . A.) and C . WALKER . ZINCKE (T.) . WAGNER (H.). Oxidation of Santonin . VESTERBERG (A.) . Amyrin . SCHMIDT (R . E.). Composition of Lac-dye . OLDBACH (H.) . BAUNANN (J.). LADENBURG (A.). DUREOPF (E.) and M . SCHLAUQK . BBRKTHSEN (A.) and H . METTEGANG . 8-Methyltetramethylenediamine and P-Methylpyrrolidine . Action of Amines on Ethylenedibenzoylorthocarboxylic Acid . The Cinnamene of the Pyridine Series . Constitution of Aldehyde-collidine Reactions of Quinolinic Acid .PAGE 712 712 713 714 714 715 715 715 716 716 717 717 717 717 718 719 719 719 720 720 721 721 722 722 723 '723 723 724 725 725 327 727 727 728 729 729 729 730 731 732 732 733 733 733 734 735 735 737 737 737XXS CONTENTS . PAGE RUGHEIMER- (L.) .and C . G .SCHBAMM. Quinoline-derivatives . 738 SCHMITr (R.) and F . ENGELMANIT . Orthohydroxyquinolinecnrboxylic Acid 738 LELLMANN (E.) and Ct . LANGCE . Quinoline . 737 UABRIEL (S.). Homologue of Isoquinoline . 739 SALOMON (Gt.). Xanthine-derivatives in Urine . 739 LADENBURG (A.), The Piperidine Series . 741) LADENBUSG.(A.) and F . PEFERSON . Duboisine . 740 LADENBURQ (A.). Constitution of Tropine . 740 JOLIN (S.). The-Acids of Pig's Bile . 742 GUNTHER (F.). Iodoform and Bromoform .787 &HAL (A.). Caprylidene : Constitution of Capraldehyde . 788 EINHORN (A.). Ecgonine . 741 BOCKLESCH (0.). Ptomaines from Pure Cultivations of Vibrio proteus . 742 COLSON (A.). Products from the Residues of Compressed Gas . 787 GRIMAUX (E.) and C . CLOEZ . Ergthrene Bromides . 789 KLASON (P.). with Ethers end Alcohols . 789 ~ E H N (C.). FPee Thiocyanic and ayanuric Aoids and their Compounds Action of . Polyatomic Alcohols on Solutions of Boric Acid and Hydrogen Sodium Cartknate . ~TROM.EYER (W.)h Sugar-compounds . HAEDICKE (J.) and B . TOLLENS . HAEDIQKE (J.), R . W . BAUBR. and B . TOLLENS . Galactose from Canragheen Moss . SBYBERLICH -(A.) and H . TBAMPEDACH . Saccharification of Starch by R'itric Acid . Formation of Ualactose and RaiEnoae NETTLEFOLD (F.).Nitrocellulose . BUISINE (A.). Amines in Suint . DUVILLIER (E.). Trimethyl-a-amidobutyrobetaine . mmia with Unsaturated Compounds . LERCH (J . 2.). Red Dye from Chloral Hydrake . GRIMAVX (E.). Glyceraldehyde . ENGEL .( R.) .. Action of Ammonia on Chlorethanes : Direct Union of Am- RAUPENSTRMJCH (Gt . A.). Condensation of Normal Butyraldehpde . MO~ILAU (R.) and C . HOFFNANN . Alkyl Hypochlorites from Isonitroso- compounds . . HENRY (L.). Cyanacetic Acid . BALLEB (A.). Ethyl Cyanacetate . MENOZZI (A.) and C . BELLONI . a-Methylamidovaleric Acid . AUTENRIETH (W.3. Substibuted Crotonic Acids- . KOBERT . Croton Oil . HAZURA (K.) and.A. FBIEDREICH . Acids from Drying Oils . RAZURA (K.). Acid from Hempsced Oil . HALLER (A.) and A . HELD . Ethyl Cyltnacetoacetate .RISCHBIETH (P.). Preparation of Levulinic Acid . BLOCK (J.) and B . TOLLENS . &ALA (A.). Propylxanthic Acid. KEHRMANN (F.). Potassium Manganic Oxalate . KOERNER ((3.) and A . MENOZZI . BEHRINB ((3.). Butyl.Sebacate . B ~ K A L (A.). Capraldoxime and Methylhexylacetoxime . REWRY .(I,. ). Synthetic Acetic Acid and its Deriratires . Salts of Levulinic Acid . CLAISEN (L.). GEHRING f (3.). Addition of Ethyl Malonate to Unsatur&ted Compounds a-Amidoisosuccinic Acid . Perchloramvl and Perchlorobutrl Pe~chlorosebaea.tes . PIUTTI (A:> . ' Reciproctll Transformation of the Optically Active Aspms- gines . MARQUAEDT (A.). Alkyl Compounds of Bismuth . RUTH (U.). Furfuran-deriyatives . Thiophen Series . R U F ~ I fH.) . Normal Propylthiophen-derivatives : Ulyoxylic Acids of the MEYEB.(V.) and K .NEUBE . Bm-Droducts of the Thioghen Manufacture . m 791 791 791 792 792 793 792 793 793 '794 794 795 795 796 796 797 797 797 798 798 799 $99 799 800 800 800 800 801 801 801 802 802 803 804 806CONTENTS . xxxi NIETzKr (R.) . WZLLUERODT (C.). WIZLUERODT (C.) . V~SET (R.) and G . TIENNIL SCERAMM (J.). Format. ion of Croconic Acid from Eenaene-derivatives . The Ealogen Carriers in the Natural Groups of the Elements . Halogen Benzene HaloYds . a-Trichlorobenzene Hexa- chloride . Action of Acetylene on Benzene in Presence of Aluminium Chloride . Influence of Light on the Action of Halogens on Aromatic Compounds . MYLIUS (E.). Phenol . TASSINARI (a.). Action of . Sulphur Dicbloride on Phenol . ZINCKE (T.). Derivatives of Orthobenzoquinone .GOLDSCHMIDT (H.) and J . STRAUSS . Dinitroso-orcinol and Dinitrosores- orcinol . CAUSSE (H.). Action of Acetaldehyde . on Polyvalent Phenols . Formation of Haloid Substitution-derivatives of Amido-corn- pounds by the Reduction of Nitro-derivatives of Hydrocarbons . CLAUS (A.) and A . STIEBBL . Metanitropamhloradine . MATZUDAIRA (C.). Dibenzylaniline and its Derivatives . WALDER (F.). Benzyl-derivatives of Hydroxylaruine . KOCK (E.) . GBAEBE (C.). Boiling Points of piphenylamine and its Homologues . BERJJNERBLAU (J.) and H . POLIKIEV . Intermediate Products in the Formation of Indoles from Dichlorether and Aromatic Amines . ASCHAN (0.). Action of Chloracetic Chloride on Orthamidophenol . AUQER (V.). Action of CEnanthaldehyde and Heptyl Chloride on Di- BEENTESEN (A.).Action of Cinnamic Acid on Diphenylamine . methylaniline . BAITHER (0.). Tetramethyldiamidobenzophenone . Metaparatoluy leneaamine . GRIESS- (P.) Diazo-compounds . b . MELDOLA (R.). Constitution of Diazoamido-compounds . FIWHER (B.) and H . WIMMER . Diazoamido-compounds . FISCHER (B.) and H . WIMMER . Hydroxyazo-compounds . MUELHAUSER (0.). Manufacture of Methyl-violet . WITT (0 . N.). Induline of Azophenine . ZI~GLER (J . H.). Roshydrazine and a New Class of Dyes Q-EHRING (G.). Aniline Sebacate and Diphenylsebacamide . HOFMANN (A . W.). Orthamidophenol Mercaptan . WZLLER (J.), Xylyl Phosphorous Compounds . MICHA~L (A.). Condensation of Aldehydes with Phenols . BUCHEA (K.) and.P . H . IRISH . HALLXR (A.) . Cyanacetophenone . BECKMANN (E.). Isonitroso-compounds .Aromatic Ethylene Di- . (J~aus (A.) and A . W . BUCHER . Chlorobenzoic Acids . %RNEMANN (E.). Metamethylcinnamic Acid . HANTZSCH (A.) and H . ZUECHER, Polycoumarins . KIRCEER ((3.). Tetrachlororthobe~~zoylbenzoic Acid . LE ROPER (A . ). p-Dichlorophthalic Acid . GRAEBE (C.). Tetrschlorophthalic Acid . QLEVE (P . T,) . @.dphimido-compounda . HINSBERQ (0.). Action of Monatomic Aldehydes of the Fatty Series on MICHAELIS (A.) and E . SCHMIDT . Unsymmetrical BenzylphenylhSdrszine . BILLETER (0.). Action of Thiocarbonyl Chloride on Secondary Amines . Oxidation of Ketones . CLAUS (A.), WERNER, SCHLARB, and MURTPELD . ketones and Alkylated Benzoyl-p-Propionic Acids ANscHUTz (R.) and W . BERNS . ~ N B C H U T Z (R.) and C . C . SELDEN . ROSER (W.) and E . H~ELOFF .Phenylacetic Acid and Desoxybenzoins Glaser's Monobromochnsmic Acids Iromerism in the Cinnamic Acid Series VILLE (J.). Action of Cyanamide on Benzenesulphonic Acids . HIRSCE (R.). Chloronitroderivatives of the Aromatic Series . PAQE 805 806 806 806 807 807 807 808 808 809 810 810 812 812 813 813 814 814 814 816 816 817 818 819 819 820 82.1 821 822 822 823 823 824 826 826 826 8.27 828 829 829 829 830 830 881 831 83% 833 834 83 8.26xxxii CONTENTS . FAHLBERQ (C.) and R . LIST . Ethyl Benzoic Sulphinide and Ethyl Ortho- sulphaminebenzoate . MAUMEN~ (E.). " Saccharin " . BERLIKERBLAU (J.). Indole from Dichlorether and Aniline . ROSER (W.). Synthesis of Indonaphthene-derivatives . ROSER (W.). Preparation of Paradinitrodibenzyl . KOCK (E.). Triphenjlmethane-derivatives .GUARESCHI (I.). y-Dichloronaphthalene and Chloronaphthdlic Acid . ZINCEE (T.) and C . GERLAND . Action of Bromine on Diamido-a-naphthol . MASCHKE (L.). /3-Naphthylamine-derivatives . ANNAHEIM (J.). Substituted Naphthylenediamines . HOFMANN (A . W.). Amidonaphthyl Mercaptans . EESTRAND (A . G.). Naphthoic Acids . BAMBERGER (E.) and 0 . BOEEMANN . Action of Sodium on Alcoholic /3-Naphthonitrile . MASCHEE (L.). Trimethylnaphthalene . ELBS (K.) and H . EURICH . 2 : 3 Dimethylanthmqninone . ELBS (K.) and M . GUNTHER . BALBIANO (L.). Camphor-derivatives . CAZENEUVE (P.). Isomeric Nitrocamphors . HANBIOT . Anemonim . CIAMICIAN ((3.) and P . SILBER . Action of Acetic Anhydride on Mkthyl: DENNSTEDT (M.) and J . ZIMMEBMANN . Action of Propionic Anhydiide on Pyrroline .PPEIFFER (G.) . Preparation of Halogen-derivatives of Pyridine Bases from EINHORN (A.) and A . LIEBRECHT . Action of Chloral on a-Picoline . LEPETIT (R.). Reaction of Nitrobenzaldehydes with Ethyl Acetoacetate and Ammonia . 1 : 3 Dimethylanthraquinone pyrroline and Benzylpyrroline . the Pyridinecarboxylic Acids . CLAUS (A.) and M . KICKELHAYN . Cinchonic Acid . ENORR (L.). Synthesis of Quinoline.derivatives . WEIDEL (H.). Reactions of Quinoline . MUHLERT (F.). Action of Acetamide on Orthochloroquinoline . BEYEB (C.). Quinoline-derivatives from B-Diketones . BERNTHSEN (A.) and F . MUHLEBT . Acridaldehyde and Acridinecarb- oxylicAcid . DUVILLIER (E.). Creatines and Creatinines . DE CONINCK (0.). AlkaloYds . PLUGQE (P . C.). Opium AlkaloYde . PLUGGE (P .C.). Composition of Papaverine . GUARESCHI (I.). Strychninesulphonic Acids . HENSCHKE (A.). Chelidonine, Chelerythrine, and Sanguinarine . DRAGENDORFF (G.) and H . N . ROSEN . Hsemoglobininto Albumin andHEematin . LINOSSIER ((3.). Compound of HEematin with Nitric Oxide . MIUBA (M.). Melanin . BBHAL (A.). Preparation of Ally1 Iodide and Ally1 Alcohol . DEMUTH (R.) and V . MEYER . Sulphuranes . HERZIGF (J.). Isodulcitol . RAYMAN (B.) . Isodulcitol . MAQUENNE . Derivatives of Inosite . MAQUENNE . Identity of Dambose with Inosite . VINCENT (C.) and DELACHANAL . Carbohydrates from Acorns . GEUTHEB (A.) . Polyiodides . LUDECEE (0.). Crystallography of some Polyiodides . HOFFMANN (C.). Action of Hydroxylamine on Acetamide . HOLST and BECKURTS . Strychnine and Brucine Ferro- and Ferri-cyanides .Alkaloids of Lobelia . LEBENSBAUM (M.). Amount of Oxygen taken up in the Decomposition of HOLAND (R.). Subatitution-derivatives from Methylene Chloride . PAGE 835 836 836 836 836 836 837 838 838 839 839 840 840 841 844 Wl 842 842 84!3 843 89.4 84A 845 845 8443 847 847 848 849 849 850 851 851 852 852 853 854 854 854 854 855 905 905 906 906 906 908 909 909 910 910 911KARCZ (M.). Glyoxalaenanthyline and its Derivatives . ARNHOLD (M.). Triethylformate and various Methylals . ZELINSKF (N.) . Preparation of Ethyl a-Bromopropionate . FROMNE (G.) and R . OTTO . B-Dichloropropionic Acid . BENEDIKT (R.) and F . ULZER . GEUTHER (A.). Constitution of Ethyl Propiopropionate . LESCCEUR (H.). Dissociation of Hydrated Oxalic Acid . Ethyl Sodomalonate .ANSCHUTZ (R.). Isomerism of Fumaric and Maleic Acids . normal-butyric Acid . FLSCHER (E.). Carbamide-derivatives of Dibromopyruvic Acid . LASSER.COHN . Sodium and Potassium Ethyl Tartrates . HORBACZEWSEI (J.). Synthesis and Constitution of Uric Acid . BLAREZ (C.) and Gt . DENIQES . Solubility of Uric Acid HAZURA (K.). Acids from Drying Oils . DELISLE (A.). Action of Sulphur Dichloride on Ethyl Acetoacetate . ANSCHUTZ (R.) and A . R . HASLAM . Action of Phosphoric Chloride on Chloralide . BISCHOFF (C . A.) and A . HAUSDORFER . Action of Iodine on Derivatives of Turkey-red Oil . ENGEL . FROYME (G.) and R . OTTO . Synthesis of Xeronic Acid from a-Dibromo- CLAISEN (L.) and N . STYLOS . Action of Ethyl Acetate on Acetone . Conversion of Fumaric and Malei’c Acids into Aspartic Acid .BEIEREND (R.). Synthesis of Compounds of the Uric Acid Series . GUTHZEIT (M.) and W . EPSTEIN . Action of Phosphoric Sulphide on Ethyl Dimethylpyronedicarboxylate . ZELINSEY (N.) . Thiophen-group . MAREOWNIKOFF and J . SPADY . Constitution of the Hydrocarbon C,H, from Caucasian Petroleum . GAUTIER (H.). SCHRAUF (A.). Molecule of Crystalline Benzene . Influence of Light and Temperature on Chlorination . OTTO (R.). Synthesis of Aromatic Polysulphides . HUGOUNENQ (L.). Chlorine-derivatives of Anisoyl . GOLDSCHMIDT (H.) and E . KISSER . Carvole-derivatives . ZEHENTER (J.). Bromine-derivatives of Resorcinol . Pyrogallol . . HANTZSCH (A.) and K . SCHNITEB . Action of Chlorine and Bromine on SALZMANN (S.). Anilic Acids . NET (J . U.). Nitranilic Acid from Chloranil .RAYMAN (B.). Cholesterin . GIRARD (C.) and L . L’HOTE . Combination of Aniline with Chromic Acid . BONNA (A.) . Phenylparatoluidine . SENP (A.) . Cyananiline, Cyanphenylhjdrazine, &c . NIETZEI (R.). Hexa-derivatives of Benzene . GRIESS (P.) and G . HARROW . BLocnMANN (R.). Action of Aniline Hydrochloride on Ethyl Cyanide . BECKER (P.). Chlorination by Means of Acetic Chloride . GUITERMANN (A . L.). Orthazoxytoluene . FISCHER (E.). Hydrazines . FISCHEE (E.) and 0 . KNOEVENAGEL . Compounds of Phenylhydrazine with . PFULF (A.). Hydrazinehenzenesulphonic Acids . ANSCHUTZ (R.) and Q . WIRTZ . Anilides of Fumaric and Malei‘c Acids: . GEHRIRG (G.) . Sebaceodinitranilide . NIEMENTOWSEI (S.) and M . OBREMSKI . Metaformotoluide and its Deriva- tives .LELLMANN (E.) and 0 . BONHOFFER . Introduction of Carboxyl into Aromatic Derivatives by the Action of Diphenylcarbamide Chloride . BERGREEN (H.). Carbon Thiodichloride . NIEMENTOWSKI (S.). Anhydro-compounds . Action of Aromatic Diamines on Sugars Acraldehyde, IUesityl Oxide, and Ally1 Bromide P hen ylas p artic Acid PAGE 911 911 912 912 913 914 915 915 915 1315 916 916 917 917 917 918 918 918 919 919 920 921 922 922 922 923 923 923 924 925 926 926 926 927 927 928 929 930 931 932 932 932 932 933 934 935 935 935 937 937 CONTENTS . d i i VOL . L I I . Cxxxiv CONTENTS. MILLER (W. v.). Nitrosalicaldehydes . MILLER (W. v.) and F. KINKELIN. Nitrocoumaraldehydes . TAEGE (C.). Nitrosalicaldehyde and Nitrocoumarin . CLAISSEN (L.) and L. FISCHER. Benzoylaldehyde .ELBS (K.). Aromatic Eetones . BEYER (C.) and L. CLAISEN. Introduction of Acid Radicles into Ketones . CLAISEN (L.) and 0. MANASSE. Nitrosoketones . RACINE (S.). Derivatives of Orthotoluic Acid . ANSCHUTZ (R.) and W. 0. EMERY. Action of Phosphorus Chloride on Salicylic Acid and Phenol . ANSCHUTZ (R.) and G. D. MOORE. Action of Phosphoric Chloride on ANSCHUTZ (R.) and Q. D. MOORE. Action of Phosphoric Chlorido on ENBLER (C.) and E. WOHRLE. Preparation of Mandklic Acid and its De- rivatives . DUPARC (L.) . Reduction of Orthonitrophenylglycollic Acid . CLAUS (A.) and K. EROSEBERB. Parutolylglyoxylic, Paratolylhydroxyacetic, and Paratolylacetic Acids . BUCHKA (K.). Paratolylglyoxylic Acid . , . MICHAEL (A.). Behaviour of Ethyl Oxalate with Resorcinol . VINCENT (C.) and DELACHANAL.RAYMAN (B.). Action of Arsenious Sulphide on Acid Chlorides . RACINE (S ). Phthaldehydic Acid . BISCHOFF (C. A.) and H. SIEBERT. Benzyl and Benzoyl Compounds . WISLICENUS (W.). Combination of Lactones with Ethereal Salts . MAYER (I?.). Nitro-+-cumidinesulphonic Acid . OTTO (R.) and A. Ros SING. Aromatic Sulphonates containing Bivalent Alcohol Radicles . OTTO (R.) and A. ROSSING. Reduction of Aromatic Thiosulphonates con- taining Alkyl Radicles by means of Hydrogen Sulphide . XINCKE (T.) and C. FROLICH. Halogen-derivatives of Phenylene Dichlor- acetylene Ketone . PFULF (A.). Indoles . RASCHEK (J.) . Indoles from Tolylhydrazine . WENZING (M.). Methylindoles . MILLER (W. v.) and F. KINEELIN. Condensation of Isobutaldehyde and Methylal with Aniline . ARHEIDT (R.).Diphenylenedihjdrazine . DOBREFF (N.). Orthodibenzgldicarboxylic Acid . BAMBERQER (E.) and R. MULLER. So-called Carbonylcarbazole (Carbazole- ZINCKE (T.). Hydrocarbon C16H12 from Styrolene Alcohol . ZINCKE (T.). Action of Chlorine on Phenols . CLEVE (P. T.). Action of Chlorine on Aceto-p-naphthylamine . JACOBSEN (P.). Orthamidated Aromatic Ketones . CAHN (E.) and M. LANGE. Action of Aldehydes on Amidosulphonic Acids FORSLINQ (S.). &Naphthylaminesulphonic Acids . WOLFFENSTEIN (R.). Action of Phosphorus Pentachloride on a-Hydroxy- naphthoic Acid . SCHLIEPER (A.). Indoles from a-Waphthylhydrazine . JANDRIER (E.). Nitroacetonaphthene . BIRUKOFF (W.) . Naphthylerythrohydroxyanthraquinone . LIEBERMANN (C.) and A. GIMBEL. Preparation of Anthranol and Di- anthryl .WALLACH (0.). Terpenes and Ethereal Oils . *. FUWITZKY (F.) . Conversion of Dextrorotatory Terpenes from Russian Turpentine by means of Hydration and Dehydration . MEYER (V.). Isophthalaldehyde . VARNHOLT (L.). Chlorosalicylic Acids. Salicylic Acid . Meta- and Para-hydroxybenzoic Acids . Tannic Acid in Mountain Ash Berries blue) . " . PAGB 938 939 939 940 94Q 940 943 944 945 945 946 94'7 94'7 948 948 948 949 94 9 950 950 951 951 952 953 953 954 955 956 956 957 957 9 58 958 959 959 960 961 962 962 962 963 963 964 964 965 YG5 968CONTENTS. XXXV LAFONT (J.). Action of Glacial Acetic Acid on Lsevogyrate Camphor . EBERHARDT (L. A.). Black-pepper Oil . CAZENEUVE (P.). @-Chloronitrocamphor . GERRARD (A. W.). Strophanthus andStrophantin . SCHRAR (E.). Cubebin.CAZENEU~E (P.) and HUGOUNENQ. Pterocarpin and B omopterocarpin . GEUTHER (A.). Bitter Principle of Calalnus Root . SCHUNCE (E.) . Chlorophyll . LA COSTE (W.) and F. VALEUR. Derivatives of a-Quinolinedisulphonic Acid . LELLMANN (E.). Existence of Two Series of 4- (am) Derivatives of Quino- line . MILLER (W. v.). Action of Aniline on Mixtures of Fatty Aldehydes . RHODE ((3.). Action of Aniline on a Mixture of Acetaldehyde and Prop- aldehyde . MILLER (W. v.) and F. EINEELIN. Action of Aniline on a Mixture of Propaldehyde and Acetal . MILLER (W. v.). Condensation of Quinaldine with Aldehydes . BRUNNEB (J. C. A.). Action of Isobutaldehyde on Quinaldine . EISELE (17.). Action of Paraldehyde on Quinaldine . SRPEK (J. 0.). Action of Furfuraldehyde on Quinaldine . BULACH (W.).Action of Paranitrobenzaldehyde on Quinaldine . FISCHER (E.) and A. STECHE. Methylation of Indole . FRIEDLANDER (P.) and F. M~LLER. Derivatives of Pseudocarbostyril . MILLER (W. v.) and F. EINEELIPI’. a-Metanitrophenylparamethoxyquino- line and its Derivatives . WEIDEL (H.) and J. WILHELM. Oxidation Products of 2’ : 2’ Diquinoline BANDROWSKI (F. S.). Bases in Galician Petroleum . WELLER (A.). Occurrence of AlkaloYd-like Bases in Paraffin Oil . CLERMONT (A.). Normal Quinine Hydrochloride . STOCKMAN (R.) . Amorphous CocaYne . KUNZ (H.). Emetine . THOMPSON (F. A.). Alkaloi’ds of Gelseminum Root . MYLIUS (F.). Cholic Acid . OTTO (R.) and K. VOIGT. Solid a-Dichlorethyl Cyanide and its Conversion into Triethyl Cyanuride . . KLASON (P.). Action of Acids on Thiocyanic Acid .FRIEDEL (C.). Crystalline Form of Quercin. SCHMIDT (T.). Comparative Sweetness of Cane- and Starch-sugar . NIEDSCHLAG (W.) . EHRENBERG (A,). Substituted Methylenediamines . HENTSCHEL (W.). Derivatives of Chlorinated Methyl Formate . SPICA (M.). Derivatives of Isopropyl Formamide . SPICA (A.) and G. DE VARDA. Derivatives of Isopropyl Chlorocarbonate . DUCLAUX (E.). Preparation of Valerie Acid . MICHAEL (A.) and G-. M. BROWNE. Isomerism in the Crobnic Acid Series. HALLER (A.) and A. HELD. Ethyl Acetocyanacetate . ELASON (P.). Thio-derivatives of Ethyl Carbonate . WILLGERODT ( C . ) . Acids from Acetone-chloroform . REIMER (C. L.) and W. WILL. Constituents of Rape-seed Oil . HAILER (A.). Preparation of Ethyl Cyanomalonate and Ethyl Benzoyl- cyanacetate .EOERNER (G.) and A. MENOZZI. Action of Ammonia on Ethyl Bromo- succin ate . HALLER (A,) and GF. ARTH. Ethyl Succinimido-acetate and Camphorimido- acetate . PINNER (A.) and J. LIFSCHUTZ. Action of Carbamide on the Chlorai C yanh y drins . LLOYD (J. U.). Asiminine . MACMUNN (C. A.). Myohsematin . Decomposition of Saccharose by Boiling with Lime c 2 PAGE 969 969 970 970 970 971 972 972 973 973 974 974 975 975 975 975 976 9’76 976 977 978 979 979 979 980 980 980 981 981 982 983 1024 1025 1026 1026 1026 1026 1027 1028 1028 1028 1029 1029 1029 1030 1030 1030 1031 1031 1032xxxvi OONTENTS . JAFFB (M.) and R . COHN . Behaviour of Furfuraldehyde in the Animal Organism . GRINER (G.). Isomcride of Benzene . OTTO (R.). Action of Cyanuric Chloride and Chlorocyanuric Diamide on Phenols .HONIQ (M.). Nitrochlorotoluenes and Chlorotoluidines . GABRIEL (8.) and R . OTTO . Orthocyanotoluene . HEYMANN (B.) and W . KOENIQS . Oxidation of Homologues of Phenol . HANTZSCH (5.) and I( . SCHNITER . Constitution of Chlor- and Brom-anilic Acids . SCHNITER (K.). Preparation of Quinones . Halogen-derivatives of Tolu- quinone . GABRIEL (S.). Formation of Primary Amines from the Corresponding NORTON (L . M.) and W . D . LIVERMORE . Action' of Dilute Nitric Acid on HEUMANN (K.) and J . WIERNIK . Phenpl-derivatives of Ethane . GOLDSCHMIDT (H.) and A . GESSNER . Cumylamine . HOFMANN (A . W.). Orthamidophenyl Mercaptan . GOLDSCHMIDT (H.) and N . POLONOWSKA . Anisamine . EOCH (E.). Behaviour of Tertiary Amines towards Nitrous Acid . REYCHLER (A.).Preparation of Phenylhydrazine . MEYER (E . v.). Preparation of Iodobenzene from Phenylhydrazine . PINNER (A.). Action of Carbamide on Phenylhydraziiie . WEDDIQE (A.). Derivatives of Acetylorthamidobenzamide . EORNER (M.). Derivatives of Benzoylorthamidobenzaniide . WILLQERODT (C.). Action of Yellow Ammonium Sulphide on Ketones and Quinones . TUST (P.). Tetrachlorobenzoic Acid . ERLENMEYER (E.,jun.). Constitution of Phenyl-a- and Phenyl-n-B-hydroxy- propionic Acids . LOPATINE (N.). Action of Aniline on Ethyl Dibromosuccinate . OTTO (R.) and A . ROSSINQ . Behaviour of Aromatic Sulphinic Acids WITT (0 . N.). Manufacture of a-Naphthylamine . Halogen-derivatives . Subs ti tu ted Amid o . compounds . MARSHALL (J.) . Glycosuric Acid . towards Hydrogen Sulphide . GOLDMANN (F.).Action of Bromine on Anthranol . BIRUKOFF (W.) . Erythrohydroxyanthraquinonecarboxylic Acid . BIMBEL (A.). Derivatives of Dianthryl . LIEBERMANN (C.) and 0 . N . WITT . Azines of Chrysoquinone BALBIANO (L.). Derivatives of Camphor . HALr. ER (A.). Racemic Camphol and its Derivatives . LIEBERMANR (C.) and M . R ~ M E B . Alkannin . LIEBERMANN (C.) and 0 . BERGAMI . Ruberythric Acid . LADENBURG) (A.). Formation of Pyrrolidine . PINNER (A.). Pyrimidines . BALBIANO (L.). Derivatives of Pyrazole . AHRERS (F.). Sparte'ine . COLASANTI ((3.). Reactions of Creatinine . BOWMAN (W.). Acetylhydrocotarnineacetic Acid . FREUND (M.) and W . WILL . Hydrastine and its Derivatives MEISSLER (A.) Ethyl Isobutyl Ether . HALLER (A.). Inactive Borneols yielding Active Camphors .DENNSTEDT (M.) and J . ZIMMERMANN . LEPETIT (R.) . Pyridine-derivatives from Metanitrobenzaldehyde . Action of Acetone on Pyrroline PINNER (A.) and J . LIFSCHUTZ . Action of Carbamide on Cyanhydrins . LADENBURG (A) . Identity of Cadaverine with Pentamethylenediamine . HARDY and CALMELS . Synthesis of Pilocarpine . WARREN (H . N.). Detection of certain Hydi-ocarbons in Alcohols . NASINI (R.), and A . SCALA . So-called Ally1 Trisiphiie PAQE 1032 1033 1033 1034 1035 1035 1036 1036 1037 1038 1039 1039 1039 1041 1041 1042 1042 1042 1043 1044 1045 1046 1046 1046 104'7 1047 1048 1049 1049 1049 1049 1049 1050 1050 1051 1051 1052 1052 1053 1053 1054 1054 1056 1056 1056 1057 105'7 1057 1088 1088 1088CONTENTS . xxxvii SEMMLER (F . W.). Ethereal Salts of Alliurn ursinium .FICE (R.). Formation of Inosite . VIETH (P) . Alcoholic Fermentation of Milk-sugar . PUCHOT (E.). Aldehyde Resin . CLOEZ (C.) . Chloracetones . HENTGCHE; (W.). Chlorinated Methyl Formates . WOHLBRUCE (0.) Action of Sodium on Ethyl Salts of the HigherGFatty Acids . KOERNER (G.), and A . MENOZZI . Transformation of Fumaric and Male'ic Acids into Aspartic Acid and Asparagine . PELLIZZARI ((3.1. Oxidising Action of Alloxan . PAAL (C.), and A . PUSCHEL . 1 : 3-Methylphenylthiophen and 1 : 2-Thioxen FRIEDEL (C.), and J . M . CRAFTS . Action of Methyl Chloride on Orthodi- chlorobenzene in presence of Aluminium . FRIEYEL (C.) , and J . M . CRAFTS . Action of Methylene Chloride on Methyl- benzenes in Presence of Aluminium Chloride . ERRERA ((3.). Decomposition of Mixed Ethers by Heat a n i Nit& Acid .PECHMANN (H . v.). Isonitroso-derivatives . PHILIPS (B.). Unsymmetrical Secondary Hydrazines . FISCHER (O.), and E . HEPP . Azophenines and Indulines . COLLIE (N.). Action of Heat on Triethylbenzylphosphonium Salts . LEVY (S.), and K . JEDLICKA . Action of Bromine on Bromanilic and Chlor- anilic Acida . BOHN (R.), and C . GRAEBE . Galloflavin . ERRERA (G.) . Ethyl Parabromobenzoate and Parabromobenzoic Acid . REBUFFAT (0.). Derivatives of Phenylamidoacetic Acid . BONDZYNSEI (S.). Deriratives of Hydrothiocinnamic Acid . EIQEL ((3.). Paracoumaric acid . PULVERMACHER (G.). Homo-orthophthalimide . GABRIEL (S.) . Homo-orthophthalimide and the Homologues of Isoquinoline XAGNANINI (G.) Transformation of Homologues of Indole into those of Quinoline .GUARESCHI (J.), and P . BIQIKELLI . Chlorobromonaphthalenes . FISCHER (O.), and E . HEPP . Nitrosamines . BALBIANO (L.) . Derivatives of Camphor . . FRASER (T . R.). Strophanthin . MERCK (E.). StrophanthusandStrophanthin . ELBOBNE (W.). Strophanthus and Strophanthin . Ts CH IR CH (A . ) . Chlorophyll . GEDOLST (L.). Preparation of Picrocarmine . S CH ARTLER (L.) . Diastase . WEBER (J.). Pyridinepolycarboxylic Acids . GOLDSCHMIEDT (G.). Dimethoxyquinoline . LIPPMANN (E.), and F . FLEISSNER . Synthesis of Hydroxyquinolinecarb- oxylic acid . KNORR (L.), and C . KLOTZ . Pyrazoline-derivatives from Ethyl Benzoyl- acetate . GUARESCEI (J.). Weyl's Reaction for Creatinine . COMSTOCK (W . J.) and W . KOENIGS . Cinchona Alkalo%ds . WILLIAMS (J.). Preparation of Aconitine .BOEHM (R.). Curare . HESSE (0.). Alkalo'ids of Coca Leaves . SCHESTOPAL (C.). Tetramethyldiquinolyline . KAUDER (E.). Cryptopine and its Salts . HOWARD (W . C.). Separation of Hygrine from Cocaine . Novv (F . G.). Higher Homologues of Coca'ine . KRUGER (F.). Absorption of Light by Oxyhsemoglobin . LE NOBEL (C.). Action of Reducing Agents on Haematin, and Occurrence . AXENFELD . HEemialbumose . of the Products of Reduction in Pathological Urine PAGE 1089 1089 1090 1090 1091 1099 1099 1100 1100 1101 1101 1102 1103 1103 1104 1105 1106 1106 1107 1107 1108 1108 1109 1111 1112 1113 1113 1114 1115 1115 1116 1116 1116 1117 1117 1117 1119 1119 1120 1121 1122 1122 1122 1125 1125 1125 1126 1126 1126 1127 1127xxxviii CONTENTS . Physiological Chemistry .SEEGEN (J.). Sugar in the Blood with reference to Nutrition . SEEGEN (J.). Power of the Liver to form Bugar from Fat . ROHMAKN (F.). EELLNER (0.). E’eeding and Development of Silkworms . SALKOWSKI (E.). Isethionic Acid in the Body and Thiosulphuric Acid in the Urine . PFEXFFER (!I.). Natural and Artificial Digestion . DEMANT (B.). Glycogen in the Liver of New-born Dogs . MORNEB (K . A . H.). Importance of Ammonia for the Formation of Glycogen LEO (H.). Trypsin in Urine . HIRSCHLER (A.). Lactic Acid in Animals . WARDEN (C . J . H.). Cobra Poison . MILLS (T . W.). Urine of the Tortoise . EIJLZ (R.). Gases of Parotid Saliva . Pigments of Uelanotic Sarcomata LANDWEHR (H . A.). Pree Hydrochloric Acid of the Gastric Juice . MILLER (N.). Ferment Organisms of the Alimentary Canala .MUNE (J.). Formation of Eat in the Dog from Carbohydrates . CHAUVEAU (A.) and KAUPYANN . Relation between the Destruction of Glucose and the Production of Animal Heat and Work . STERN (H.). Origin of the Bile Colouring Matters . DRAQENDORFF (G.). Physiological Action of Convolvulin and Jalapin . STUTZER (A.). Artificial Digestion . GARROD (A . B.). BIEDERT . Albuminoi’ds of Human Milk and of Cow’s Milk KULZ (E.). Active P-Hydroxybutyric Acid . Place of Origin of Uric Acid in the Animal Organism . FIRTH (R . H.). Poisonous Ptomai’ne in Milk . GOSSELS (W.). MARSHALL (.J.). Huffner’s Reaction in Bile . POSNEZ (C.). Albumin in Normal Urine . CITRON (H.). Mucin in Urine . Nitrates in Animals and Plants . BOCEAL (A.). Physiological Action of Paraldehyde .MAIRET (A.) and COMBEMALE . Physiological Action of Methylal . KOCH (E.) Butylchloral Hydrate and Chloral Hydrate as Antidotes for BELKY (J.). Action of Gaseous Poisons . EHRENBERQ (A.) . Sausage Poisoning . HANRIOT (M.) and C . RICHET . Estimation of the Carbonic Anhydride MARCEUSE (W.). Formation of Lactic Acid during Muscular Activity . EOWALEWSKY (N.) . Formation of Methsemoglobin in Blood by the Action of Alloxantin . EULZ (E.). FFEIFFER (T.) and F . LEHMANN . ELLENBERGER and HOFMEISTER . Digestion in the Pig . BAHLMANN (P.). Amido-compounds in the Animal System . Strychnine and Picrotoxin . expired and the Oxygen absorbed in Respiration . Decomposition of Bromides and Iodides by the Stomach . Addition of Sugar to Cattle-foods . ARNSCHINK (L.). Nutritive Value of Glycerol .CONSTANTINIDI (A.). Wheat Gluten as a Food . LUDD (E . F.). Pepsin versus Animal Digestion . GRBHANT and QUINQUAIJD . Formates in the Organism . LEO (H.). Reducing SubstanceinDiabeticUrine . Gltocco (P.) . Creatinine in Urine . ANRAEFF (A . N.). MULLER (F.). Aniline Poisoning . MAIRET (A.) and COMBEMALE . Toxic Action of Colchicine . JONES (E . I,.). Specific Gravity of Human Blood . BBCHAMP (A.) . Causes of the Alteration of Blood in Contact with Air, Oxygen, and Carbonic Anhydride . Behaviour of Quinol with Urine and Urea PAGE 66 6’7 68 68 68 69 167 167 167 168 170 170 287 287 288 288 289 290 290 291 388 388 388 389 389 390 390 390 391 391 391 392 392 50’7 508 508 508 509 511 511 512 512 513 513 513 513 514 514 515 608 609CONTENTS .xxxix HASEBROEE (K.). A First Product of Gastric Digestion . GOLDSCHMIDT (H.). Intestinal Digestion in the Horse . WURSTER (C.). Oxidation in the Animal Body . KAST (A.). Fate of Certain Chlorine Compounds in the Organism . MONARI (A.). Formation of Xanthocreatinine in the Organism . MACMUNN (C . A.) . Invertebrate Chromatology . STUTZER (A.). Analysis of Nitrogenous Metabolites in Feces . HALLIBURTON (W . D.). Proteids of Cerebrospinal Fluid . MAIRET (A.) and COMBEMALE . Therapeutic Action of Colchicine . ELLENBERBER and HOFPYEISTER . Period required for Digestion in the Pig . SIEBER (N.) and A . SYIRNOW . Behaviour of the three Tsomeric Nitro- MAIRET (A.) and COYBEYALE . Therapeutic Action of Methylal . GOLDSCHXIDT (H.). Absorption in the Stomach of the Horse .ELLENBERBER and HOFYEISTER . IXgestion and Digestive Secretions in the Horse . KAISER and SCHMIEDER . Changes in Milk by Freezing . . HENZOLD (0.). Frozen Milk . RICHARDSON (B . W.). Action of Oxygen on Animals . WEISKE (H.) and others . Composition of Blood, Liver, and Flesh under varying Conditions. SANBORN (J . W.). Animal Nutrition . ANDOUARD (A.). Variations in the Proportion of Phosphoric Acid in Milk . MARES . WmrE . Hydroxybutpic Acid in Diabetic Urine . MEYER (V.) . Physiological Action of Chlorinated Ethyl Sulphides . SHAPIROFF (B . M.), Physiological Action of Tertiary Alcohols . DEAGENDORFF (G.) and S . SALOMONOWITSCH . Myoctonine . FISCHER (E.) and F . PENZOLDT . Sensitiveness of the Sense of Smell . WOOLDRIDQX (L . C.). New Constituent of Blood Serum .HALLIBURTOPF (IT . D.). Muscle Plasma . FOKKER . Fermentation by Protoplasm from Recently-killed Animals . BRUNTON (T . L.) and J . T . CASH . Action of Caffe'ine and The'ine on Volun- tary Muscle . BRUNTON (T . L.) and J . T . CASH . Chemical Constitution and Physiological Action . RANSOM (W . B.). Diabetes and Glycerol . HUBOUNENQ (L.). Laevorotatory P-Hydroxybutyric Acid in the Blood of a Diabetic Patient . BRUCKE (E.). Does Human Urine contain Free Acid ? . HANRIOT (M.) and C . RICHET . Relation between Muscular Activity and the Chemical Effect of Respiration . CHAUVEAU (A.) and KAUFYAKN . Heat Developed by the Activity of the Muscles . VIQNAL (W.). Action of Micro-organisms from the Mouth and from Faeces on Food-stuffs . MBHU (C.). Sugar in Urine .RANVIER (L.). Per-ruthenic Acidin Histology . CRAMER (A.). Glycogen . WEYL (T.). Chemical Studies on the Torpedo . ELLENBERBEB and HOFMEISTER . Nitrogenous Contents of the Digestive Juices . STUTZER (A.). Relation of Prote'ids to Digestive Ferments . ATWATER (W . 0.). Comparative Absorption of Fish and Meat in the Alimentary Canal . HERRMANN (A.) Digestion of Fibyin by Trypsin . TAPPRINEE (H.). Fermentation of Cellulose . benzaldehydes in the Animal Body . Excretion of Urea and Uric Acid from the System PAGH 609 610 610 612 613 613 613 614 614 684 684 684 743 744 745 745 855 855 856 856 856 857 857 857 858 983 983 984 984 985 985 985 986 986 1058 1059 1059 1060 1060 1127 1128 1129 1129 1130 1130 1131 EAST (A.). 'Arbmatic Products of Putrefaction in Human Sweat .1132xl CONTENTS . BAAS (K.). Relation of Tyrosine to Hippuric Acid . UDR~NSKY (L . v.). Urinary Pigments . Chemistry of Vegetable Physiology and Agriculture . LAURENT (E.). The Bacillus of Panary Fermentation . DENARO (A.). Decomposition of Silicic Acid by Leaves . EREUSLER (U.). Observations on the Growth of Potatoes . BATTUT (L.). Ammonia in Beetroots . HENKE (G.). Milky Juice of Certain Euphorbiacese . KLIEN . Composition of Barley and Pease . EELLEER (0.). Composition of Tea-leaves . HESSE (0.). China Bicolor . SACHS (J . v.). Chlorosis in Plants . KELLNEB (0.). Absorption by Soils . EELLNER (0.). Estimation of Absorbed Bases in Soils . STUTZER (A.). Chdi Saltpetre as Manure . MAGERSTEIN (v.). Comparative Manurial Values of Chili Saltpetre and QUANTIN (H.) .Reduction of Copper Sulphate during Alcoholic'Fermenta- tion . GAYON (V.) and E . DUBOURG . Alcoholic Fermentation of Dextrin and Starch . GAYON (V.) and Gt . DUPETIT . Method of Preventing Secondary Fermenta- tion . EHRENBEEG (A) . Is Free Nitrogen formed during Putrefaction ? . DEHBRAIN (P . P.) and MAQUENNE . Absorption of Carbonic Anhydride by Leaves . MUNTZ (A) . Ripening of Seeds . KRAUS (J.) . So-called Soluble Starch . FREUND (M.) and W . WILL . Substances contained in the Roots of Hydrastis Cumadensis . DEHBRAIN ( P . P.). Valuation of Manures . MUNTZ (A.) and C . QIRARD . Production of Farmyard Manure . WRIGHTSON (J.) and J . M . H . MUNRO . Manurial Value of Basic Steel MUNRO (J . M . H.). Influence of the Ferric Oxidc in Basic Cinder on the Growth of Plants .LIBORIUS (P.). Bacterial Life in Relation to Oxygen . ROMMIER (A.). Wine and Brandy from Raspberries and Strawberries . ARLOING (S.). Zymotic Virus and Fermentation . ATWATER (W . 0.) and E . W . ROCKWOOD . Loss of Nitrogen during Clermination and Growth . RICHARDSON (C.). Variations in the Chemical Composition and Physical GRASSMAN (P.). Loss occasioned by Improper Methods of Pickling Wheat BERTHELOT and ANDR~ . Nitrogen Compounds in Vegetable Soils . SIEVERT (M.). Manuring Rye with Thomas Slag, &c . RIMPAU and others . Thomas Slag and other Phosphates as Manure for Moorlands . NAUTIER (A.). Superphosphate Manuring for Sugar-beet . VINCENZI (L.). Chemical Constituents of Bacteria . SOHNKE (J.). Behaviour of Micro-organisms in Artificial Mineral Water .BRIEGER (L.). Source of Trimethylamine in Ergot of Rye . PAUL (R . H.) and A . J . COWNLEY . Amount of Caffei'ne in Various Kinds M~LLER (C . 0.). Formation of Albumino'ids in Placts . Ammonium Sulphate . MAGERSTEIN (v.). Experiments with Chili Saltpetre . Slag . Properties of American Oats . of' Coffe;! . HOOPER (D.). Ash of Cinchona Barks . 394 PA QE 1133 1133 70 70 70 71 71 72 73 73 76 76 76 77 71 77 78 171 171 171 172 172 173 173 174 174 175 176 178 291 292 292 292 293 293 293 294 294 295 393 393 394 394CONTEXTS . xh JODIN (V.). Action of Mercurial Vapour on Leaves . BEPTHELOT . Direct Absorption of Nitrogen from the Atmosphere by Vege- table Soils . ATWATER (W . 0.). Acquisition-of Atmospheric Nitrogen by Plants . NAGAMATSZ (A.). Functions of Chlorophyll .VOGEL (A.). Influence of Ozone on Germination . MULLER . Formation of Sugar in Grapes . EIJKMAN (F . J.). Cinnamic Acid in Plants of the Ericacese Family . TROSCHPE . Composition of Lupines . K~NIG (J.). MEUSEL (E.). Effects of Tfiiocyanates on Vegetation and Fermentation . BORDAS . Grain of Holcus sorgho . LECHARTIER (G.). Cider Ash . SCHULZE (B.). Silage of Maize . SCHULZE (E.). Silage of Vegetable Matter . MARCEER . Diffusion Residues . WOLLNY (E.). Influence of the Physical Properties of a Soil on the Amount . WARINGTON (R.). Nature of the Nitrogenow Organic Matter of Soils . WOLLNY (E.). Decomposition of Organic Matter in Soils . KELLNER (0.) and others . FLEISCHER (M.), BRINCKMAN, and others . Manuring with Thomas Slag and other Phosphates . FITTBOGEN and SALFELD .Manuring with Thomas Slag . WAGNER (P.). Manurial Value of Thomas Slag . LEONE (T.). Changes Induced in Water by the Development of Bacteria . EMMEPLINB (A.). Fermentation of AJbumin in Plants . RICHARDSON (C.) American Barley . GIRARD (A.). Destruction of the XematoYds of Beetroot . BERTHELOT . Direct Absorption of Nitrogen by Vegetable Soils . ANDOUARD (A.). Incompatibility of Nitrates and Superphosphates . PRINGSHEIH . Decomposition of Carbonic Anhydride by Chlorophyll . MUELLER (H.). Physiological RBle of Vine Leaves . KREUSLER (U.). I s Nitric Acid formed in the Organism of Higher Plants ? GRIESSMAYER . True Natureof Starch-cellulose . MORAWSEI (T.) and J . STINGJ. Sugars of the Soja Bean . MORAWSEI (T.) and J . STINGL . Fat of the Soja Bean .BRUCKNER (E.). Russian Black Earth . MARCPER (M.). Value of the Phosphoric Acid in Thomas Slag . CLAUDON (E.) and E . C . MORIN . Fermentation of Sugar with Elliptical Yeast . EHRENBERB (A.). Formation of Nitrogen during Putrefaction . ; PFXFFER (W.). Absorption of Aniline Colours by Living Cells . SCHULZE (E.). Presence of Clioline in Germinating Plants . SCOVELL (M . A. ) and A . E . MEXKE . Composition of Potatoes . STOSSNER (E.). Effects of Deep or Shallow Sowing on Cereals . PAGNOUL (A.). Manurial Experiments with Sugar Beets . CELLI (A.) and F . MARINO.ZUCO . Nitrification . MARCACCI (A.). Action of AlkaloPds in the Animal and Vegetable King- doms . SCHULZE (E.). Are Nitrates formed in the Organisms of Higher Plants ? . LIST (E.). Organic and Inorganic Constituents of Grapes .BERTHELOT and ANDRB . JOFFPE (J.). Agricultural Value of Retrograde Phosphates . GREEN (J . R.). Composition of the Inner Brown Skin of the Earth-nut . of Free Carbonic Anhydride present Beliaviour of Urea in Soils JENTYS (S.). Intramolecular Respiration . ARNAUD (A.). Carrotene in Leaves . EASSNEB ((3.). Solanine . QUANTIN (H.). Tunisian Soils . BOKORNY (T.). Reduction of Silver Salts by Living Protoplasm . Evolution of Ammonia from Vegetable Soils Changes in the Proteids of Seeds during Germination PAGE 395 395 515 516 516 517 517 518 519 519 519 520 521 521 521 521 523 523 524 52% 524 525 615 615 616 617 617 61 7 685 685 686 686 686 686 687 687 687 746 746 747 747 747 747 748 858 859 859 859 860 860 860 860 861 987 987xlii gONTENTS .DIAKONOFF (N . W.). Molecular Respiration of Plants . MAYER (A.). Exhalation of Oxygen by Fleshy-leaved Plants in Absence of MOLISCH (H.). Relations between Inorganic Salts containing Nitrogen, and Plants . MARTIN (S . H . C.). Prote'ids of the Seeds of Jequirity . FLUCKIGER . Safrole . ELBORNF (W.) Strophanthus . GAUNERSDORFER (J.). Poisoning of Plants by Lithium Salts . WAAGE (R.). Composition of some Leguminous Seeds . AITKEN . Experiments on Potatoes a t Harelam . DEH~EAIN ( P . P.). Production of Nitrates in Arable Soil . WEILANDT (M.). Free Phosphoric Acid and Superphosphate . AITKEN . Carbonic Anhydride . Basic Cinder and other Finely-ground Phosphatic Manures . AITPEN . Ground Pelspar as a Potash Manure . DUCLAUX (E.). Butter from Various Districts .ALVAREZ (E.). Microbe of the Indigo-fermentation . TSCHIRCH (A.). Aleurone-grains in the Seeds of Myristica Swrinamensis . BERGAMI (0.). Examination of Caucasian Madder Root . THIEL (H.). Experiments with Ensilage in Holland . GRUBER (M.). Culture of Anaerobic Bacteria : Morphology of Butyric Fermentation . MUNTZ (A.). Distribution of the Nitric Ferment and its Function in the HOPPE-SETTLER (F.). Methane Fermentation of Acetic Acid . BELLUCI (G.). Formation of Starch in the Chlorophyll Granules . LEITGEB (H.). Crystalline Deposits in Dahlia Tubers . MILES (M.) . Nitrifying Microbes . Disintegration of Rocks . WIPPRECHT (W.). Absorption of Ammonia by Clay . GOESSMANN (C . A.). Analysis of Onions . ROBERTS (W.). Manuring with Various Phosphates . KREMP . Manurial Experiments with Various Phosphates .Analytica 1 Chemistry , ARNOLD (C.). Kjeldahl's Method of Estimating Nitrogen . ZAMBELLI and LUZZATO . Separation of Arsenic and Antimony . BBENSTEIN . Detection of Thiosulphate in Sodium Hydrogen Carbonate . SALZER (T.). Detection of Thiosulphate in Sodium Hydrogen Carbonate . THILO (E.). BARNES (J.). Valuation of Zinc Powder and Testing of Carbonates . WEBTMOBELAND (J . W.). Determination and Valuation of Copper in BAUMANN (A.). Estimation of Ammoniacal Nitrogen in Soils . Estimation of Small Quantities of Silver in Burnt Pyrites Ores, &c . WRIGHT (L . T.). Analysis of Gas Coal . LUNGE (G.). Analysis of Explosives . SAMUELSON . Estimation of Glycerol in Wine . BOUILHON (E.). Estimation of Solid Matter in Wines . PBIOR (E.).Estimation of the Acidity of Malt . ALLEN (A . H.). Examining Fixed Oils . ELLIS (C . J.). Maumene's Test for Oils . JULIUS (P.). Employment of Congo-red in Titrating Aniline . with Sodium Hypobromite . HEW (J.). Detection of Artifxially Coloured Red Wine . SCHBODT (M.). Presence of Nitrites and Nitrates in Milk as Proof of Adulteration . PFLUGER (E.) and K . BOHLAND . PFLUGER (E.) and K . BOHLAND . Estimation of Urea in Human Urine WITT (0 . N.). Qualitative Test for the Dyes found in Commerce . Hufner's Method of Estimating Urea PAQE 988 988 989 990 990 991 991 991 992 993 995 995 996 996 1061 1061 1061 1062 1134 1135 1135 1135 1136 1136 1136 1137 1137 1137 78 78 79 79 79 a0 80 82 84 86 86 87 87 87 88 89 90 90 90 91 91CONTENTS . xliii PETTERSSON (0.).Apparatus for Gas Analysis . OETTEL (F.). Volumetric Method for determining Fluorine . PETTERSSON (0.). Air Analysis on a New Principle . WELCH (J . C.). WILSING (H.). Volumetric Determination of Sulphuric Acid . QUANTIN (H.). Volumetric Determination of Sulphatm . MORSE (H . N.) Land A . F . LINN . Determination of Nitric Acid . HOLLAND (P.). Determination of Alkalis in Silicates . BERG ( P . v.). Separation of Zinc from Iron, Cobalt, and Nickel . THOYFON (R . T.). Determination of Aluminium in Presence of much Iron DEANE (L . M.). Estimation of Manganese and of Phosphorus in Iron and Steel . Detection of Stannic Sulphide in Presence of Antimonious Sulphide . HERZFELD (A.). Estimation of Carbon in the Organic Constituents of Water . HARVEY (S.). Estimation of Nitrates in Water .EARTH (M.). Estimation of Glycerol in Wines . HERZFELD (A.). Estimation of Invert Sugar . BECKMANN (E.). Titration with Fehling’s Solution . CURTMAN (C . 0.). Detection of Salicylic Acid . ALLEN (A . H.). Specific Gravity, &c., of Waxes, &c . ALLEN (A . H.) and W . CHATTAWAY . Adams’ Method for Milk Analysis . THOMSON (W.). Adams’ Method for Milk Analysis . FOCPE . SAMUELSON . Detection of Artificial Colouring in Red Wine . GEORGES . Peptones in the Blood and Urine . Filters . CHAPMAN (A.). Method for Estimating Fluorine . WURSTEE (C.). Reagents for Active Oxygen . BRUGHAN (W . F.). Influence of Copper on the Estimation of Sulphur . MOLLER (G.). Eggerzt’s Method of Estimating Sulphur in Iron . ATKINSON (A . J.). FAIRLEY (T.). Estimation of Sulphur and Impurities in Coal-gas .DE KONINCP (L . L.). New Reaction of Thiosulphates . DE KONINCP (L . L.). Detection of Ammonia, Nitric or Nitrous Acids, and ENOP (W.). Determination of Ammonia in Arable Soil . WURSTER (C.). Griess’s Reaction for Nitrous Acid . ARYSBY (H . P.) and F . G- . SEORT . Apparatus for Nitrogen Determination . VORWERK (P.). Determination of Phosphorus in Iron and Steel . ROSENBLADT (!I.). Determination of Boric Acid . GOOCH (F . A.). Separation and Estimation of Boric Acid . VAN NUYS (B‘. C.). HAUSHOFER (E.). Microscopical Analysis . HAUSHOFER (K.) . Microchemical Tests . BERG (P . v.). ATNSN (A.). Detection of Mercury in Organic Liquids . ROSENBLADT (T.). Separation of Mercury and Palladium . THONSON (R . T.). MOORE (T.). Estimation of Nickel in Ores, Mattes, and Slags .KRUSS (G.). Universal Spectroscope . Assay of Iron Pyrites for Available Sulphur HUTCHINGS (W . M.). Analysis of Silicates . HAGER (H.). Testing Aluminium Sulphate . BLUY (L.). Separation of Manganese from Iron . GOZDORF ((3 . A.). Assay of Minute Quantities of Gold GRIFFITH (A.). . ALLEN (A . H.). Assay of Carbolic Soap . ALLEN (A . H) . Saponification of Fixed Oils . Separation of Morphine and Strychnine from Fatty Matters . DIEIJDONN~ (H.) Estimation of Tannin . G-AWAL o vs K I (A.) . Estimation of Sulphur in Coal and Coke Thiosulphuric Acid . Estimation of Carbonic Anhydride in Air Titration of Zinc and Cadmium Sulphides with Iodine . WEIL (F.). Valuation of Zinc-dust . Estimation of Alumina and Iron Oxide in Manures PAGE 179 179 179 180 180 181 181 181 181 181 182 182 182 183 183 183 184 184 184 184 185 185 185 1b5 186 1 S6 186 186 187 187 187 188 295 295 295 296 296 296 29’7 297 297 297 298 298 299 299 299 300 300 301 301 301 302 302 302 303xliv CONTENTS .SELL (W . J.). Volumetric Determination of Chromium . BROWN ( W . L.). Analysis of Chrome Paints . MCCULLOCR (N.). Estimation of Chromate in the Presence of Dichromete . WACHSMUTH (0.). Estimation of Tin and Lead in Alloys . LEVY (L.). Colour Reactions of Titanic, Niobic. Tantalic. and Stannic Anhydrides . LEVY (L.) . Colour Reactions of Arsenic. Arsenious. Vanadic. and Molybdic Anhydrides. and of Antimony and Bismuth Oxides . LUEDEKING (C.). Post-mortem Detection of Chloroform . SKALWEIT . Estimation of Glycerol in Wine and Beer .SCHEIBLER (C.). Separation and Estimation of Melitose in Cane-sugar . CREYDT (R.). Estimation of Melitose . PALM (R.). Detection and Determination of Lactic Acid . WATTS (F.). Titration of Citric Acid . SCHULZE (B.). Determination of Fatty Acids in Soap . CRONANDER (A.) . New Method of Estimating Fat in Milk . SKALWEIT (J.). Butter Testing . . HAGER (H.). Butter Testing . WOLL (F . W . A.). Butter Analysis . CORNWALL (H . B.) and S . WALLACE . Reichert's Method of Butter Analysis MOORE (R . W.). Carrot Coiour in Butter . MARSHALL (J.). New Ureometer . HIRSCHLER (A.). Separation of Nitrogenous Substances by Means of Phosphomolybdic Acid . DIETRICH (E.). Opium Testing . MOLL (J . W.). Microchemical Detection of Tannin . B . (E.). Tannin Determination .MYLIUS (E.). Thale'ioquinine Reaction . HEISCH (C.). Analysis of Pepper . H~NOCQUE . Heematoscopy ; a New Method of Blood Analysis . KOCHS (W.). Determination of Sulphur in AlbuminoYds . FRIEDHEIM (C.). Weil's Method for the Volumetric Estimation of Sul- phides . GREEN (A . G.) and F . EVERSHED . Volumetric Estimation of Nitrous Acid MEINEKE (C.). Determination of Phosphorus in Steel and Iron . BENTE (F.) Determination of Phosphoric Acid . HAGER (H.). Detection of Arsenic . EAGER (H.). Use of Copper containing Arsenic for the Dearsenification of BAUER (R.). Apparatus for Estimating Carbonic Anhydride and all similar Gases . GRAVILL (E . D.). Estimation of Ammonium Carbonate in Spim'tus Ammonia Aromaticus. B.P. Determination of Cadmium and its Separation from Copper Volumetric Determination of Manganese .Hydrochloric Acid : Reinsch's Test for Arsenic . BRAGARD (M.). Estimation of Zinc as Pyrophosphate . ATKINSON (R . W.). Estimation of Manganese . INCE (W . H.) Ferric Chloride as a Test for Organic Substances . CANDWEHR (H . A.). Precipitation of Dextrin by Iron . BAUER (R.). Estimation of F a t t j Acids as Fats . NICKEL (0.). Quantitative Estimation of Oxalic Acid in Urine . ERETZSCHMAR (M.). Estimation of Fat . MILLER (A . R.). Preserving Standard Tartar Emetic Solutions . STILWELL (C . M.). Opium Analysis . VULPIUS (G.). Estimation of Quinine Sulphate . DF: VRIJ (J . E.). Quinine Chromate in Analysis . HESSE (0.) Normal Quinine Chromate . KOBNER (A.) . SCHOFFEL (R.) and E . DONATH . GIRAUD (H.). Volumetric Estimation of Antimony in Presence of Tin ARCHBUTT (L.). Analysis of Oils .FINPENER . Distinction of Castor Oil from other Fatty Oils . PAGE 303 3041 304 3 M 304 305 305 306 306 306 307 307 307 308 308 309 309 309 310 310 310 310 311 311 311 312 312 396 396 396 396 397 397 397 398 398 398 398 399 399 MO 400 401 401 401 M.2 402 402 403 4!03 404 404 4Q4CONTENTS . JUNGPLEISCH (E.). Quinine Sulphate . LIEBMANN (A.) and STUDER . Detection of Rosaniline Salts . DE REGO (J . H.). Detection of Acid Coal-tar Colours in Wine . HOPPE-SEYLER (G.) . Discriminating between Chrysophanic Acid and San- tonin Colouring Matters in Urine . SCHMIDT (M . v.) and P . ERBAN . SAUL (J . E.). Test for Tannin . PALM (R.). Detection of Traces of Albumin . ERASSER (I?.). Presence of Albumin in Vegetable Tissues : Microchemical Test for AlbuminoYds .DANNENBERG (E.). Detection of Blood Stains in Presence of Iron Rust . Separation of Resins OTT (A.). Separation of Globulin from Albumin in Urine . AMTHOR (0.). Dannenberg's Hsemidin Crystals . HUGHES (J.). Analysis of Hoofs and Horns . CAMPBELL (E . D.). Estimation of Sulphur in Soluble Slags WHITFIELD (J . E.). Indirect Determination of Chlorine, Bromine, and Iodine . NETTLEFOLD (F.). Absorption of Nitric Oxide by Sulphuric Acid . MANPIEWICZ . Detection of Phosphorus . THILO (E.). Estimation of Phosphoric Acid from the Weight of the Mo- lybdate Precipitate . ISBERT (A.) . Estimation of Phosphoric Acid . LAIBLE . Estimation of Phosphoric Acid . SCHNEIDER (L.). Determination of Phosphorus in Iron and Steel .BRUNNEMANN (C.). Determination of Phosphorus in Basic Slag . LOQES (G.). Determination of Phosphoric Acid in Basic Slag . STRICK (a . H.). Estimation of Silicon in Iron . MARCET (W.). Volumetric Estimation of Carbonic Anhydride . KUHLMANN (E.). Determination of Normal Carbonates in " Bicarbo- nate~.~' . GOOCH ( F . A.). Separation of Sodium and Potassium from Lithium, Mag- nesium, and Calcium . LUCPOW (C.). Separation of Metals by Oxalic Acid . STAHL (IT.). Analysis of Copper . KNORRE ((3 . v.) . Employment of Nitroao-a-naphthol in Quantitative Analysis . HERZ (J.). Detection of Alum in Flour . BAYEE (K . J.). Detection of Free Sulphuric Acid and of Aluminium MEINECPE (C.). Volumetric Determination of Manganese . WARREN (H . N.). Use of Electro-dissolution in Analysis .WARREN (T . T . P . B.). Detection of Adulteration in Metallic Nickel and other Metals by the Magnet . DONATH (E.) and R . JELLER . Detection and Determination of Traces of Chromium . VENATOR (W.) and E . ETIENNE . Analysis of Chrome Iron Ore . CARNELLEY (T.) and W . MACPIE . Determination of Organic Matter in Air . ZAMBELLI (L.). Colorimetric Determination of Nitrites in Water . EOBRICH (A.). Determination of Organic Matter in Natural Water . AGOSTINI ( C . ) . Detection of Dextrose . IHL (A.). Colour Reactions of Beet-sugar . TOLLENS (B.). Behaviour of Sugar towards Acids and Phenol . IHL (A.). Colour Reactions of Starch and Gum . VOLCPER (0.). Determination of Hippuric Acid in Urine . LEVALT~IS (A.). Characteristics of Olive Oil . LEONE (T.) and A .LONGI . DRAPER (H . N.). and C . DRAPER . Behaviour of Alkaline Solutions of . HOPPE-SEYLEB (F.). Estimating Hvdrogen in the Presence of Methane . Hydroxide in Aluminium Sulphate . Properties of Olive, Sesame, and Cotton Oils PhenolphthaleYn in Presence of Alcohol x1 v PAGE 405 405 m5 406 406 406 40'7 407 408 408 408 525 526 526 526 526 526 526 527 527 527 527 528 528 528 5 29 520 530 530 530 531 531 531 531 532 532 533 533 534 534 534 534 535 535 536 618 618 4406 . V Y Vxlvi CONTENTS . KALMANN (W.) . Standardising Iodine Solutions : estimating Sulphurous WEIL (F.). Vclumetric Estimation of Sulphides . BABBITT (1% . C.). Manganese in Steel and Iron . DONATH (E.). Decompoeition of Chrome Iron Ore . FOLKARD (C . W.). Bacteriological Examination of Water .BURQHARDT (C . A.). Determination of Organic Carbon and Nitrogen in Waters . LAUBE (G.). Decolorisiiig Power of Bone-black . WUESTER ((3.). Quantitative Estimation of Wood in Paper . BENEDIKT (R.) and F . ULZEB . Investigation of Acetyl Compounde, : New Acid in Presence of Thiosulphuric Acid . Method for the Analysis of Fats . ROSE (B.). Analysis of Fats . CORNWALL (H . B.). Examination of Butter Colours . BLAREY (C.) and Gt . DENIG~S . Estimation of Uric Acid by Potassium Per- PLUGGE (P . C.). Volumetric Estimation of Acids in Salts of the Alka- loids . ADRIAN and E . GALLOIS . Assay of Opium . SCHLICKUM (0.). Estimation of Morphine . SCHAFER (L.). Estimation of Cinchonidine in Quinine Sulphate . SCHLICEUM (0.). Testing Quinine Sulphate . FLECK (H.) Colour Reactions of Picric Acid and Dinitrocresol .MACAQNO (J.). Determination of Tannin in Bumach . FRANCEE (B.). New Gas Burette . LEYBOLD (W.). Burette J e t . BRAND (A.). Use of “ Solid Bromine ’’ in Analysis TOPF ((3.). Iodometric Studies . FLUCEIGER (F . A.). Reaction of Thiosulphates . BRAGARD (M.). Zinc Determination . DITTE (A.). Estimation of Vanadic Acid . SPIEGEL (L.). Determination of Nitrates in Well Waters . TONY.GABCIN . Detection of Cane.sugar, Glucose, and Dextrin in Wines . MOLISCH (H.). New Test for Conferin . FRIEDHEIM (C.). Weil’s Method of Determining Sulphides . VILLIERS (A.). Detection of Sulphites in Presence of Thiosulphates . JACKSON (C . L.) and GF . W . ROLFE . Quantitative Determination of Hy- manganat e . L’EOTE (L.). Detection and Estimation of Aluminium in Wine and in Grapes .droxvl . DIEZ (R.\. Quantitative Estimation of Glycerol . LINDO (D.). New Sugar Reactions . CRAMPTOB (C . A.). Analyses of Sugar-cane and Beet Juices . MACNAIB (D . S.). Separation of Acetic and Formic Acids . SHORT ( F . (3.). Analysis of Milk . MORSE (H . N.) and C . PIGGOT . Determination of Butter in Milk . BLOXAM (C . L.). Colour Tests for Strychnine and other AlkaloYds . HAGER (H.). Guaiac Resin . THOMAS (H.). Estimation of Hydrogen Peroxide . SALZER (‘T.). Volumetric Estimation of Iodine . Determination of Sulphuric Acid in Water . RAULIN . Estimation of Nitrogen in Organic Substances . ULSCH (K.). Kjeldahl’s Method. for Estimating Nitrogen . GARNIER (L.). Estimation of Nitrogen in Urine . GASBAUD . Organic Nitrogen in Chemical Manures .MOHB (C.) Estimation of Phosphoric Acid . KRETZSCHMAR (M.). Detection of Boron in Milk, &c . HOLDERMA.” (E.). Estimation of Sodium and Lithium . BERNARD (A.). Cdcimetry . FRICEE . KRETZSCHMAR (M.). Estimation of Potassium in Ashes and Minerals . PAGE 618 618 619 619 619 619 619 620 620 621 621 621 621 622 622 623 623 624 624 687 688 688 688 689 689 690 691 691 692 692 749 749 749 750 751 751 751 751 752 752 752 862 862 862 862 863 863 863 864 864 864 864 865CONTENTS . xlvii STOLBA (E.). Determination of Calcium and Magnesium in presence of Man- ganese . KUPFERSCHLBGER . Titration of Zinc Powder . GATENBY (R.). Volumetric Estimation of Alumina . WEDDINQ . Estimation of Phosphorus inIron . BRAND (C.). Determination of Combined Carbon in Iron .KEHRMANN (F.). Separation of Phosphoric Acid from Tungstic Acid . DBAGENDOEFF (G.) and €I . TIENSENHAUSEN . Ciloral Hydrate . DRAQEWDORFF (G.) and W . JACOBSON . Isolation and Detection of Pheuol . EPFRONT (J.). Estimation of Starch and Sugars . ASBOTH (A . v.). Estimation of Starch . UIRARD (A.). Estimation of Starch in Potatoes . SONNENSCHEIN (A.). Estimation of Acetic Acid in Acetates by Direct Titration . GOEBEL (H.). Estimation of Morphine . VULPIUS (G.). Morphine Reaction . DRAGENDORFF (G.) and E . BLUMENBACH . Thallin . RENARD (A.). Estimation of Indigo in Textile Fabrics . KOCH (R.). Determination of the Free Acid in Tannin Liquor by Titra- tion . VILLON . New Method €or the Estimation of Tannin . GARNIER (L.). Escimrttion of Albumino’ids in Liquids from Cysts, &c .JTLUCEIGER (F . A.). Iodine Determination in Laminaria . TOPF (G .. ). Iodometric Studies . WEIL (F.). Estimation of Sulphides . LUNGE (G) . Detection of Nitrogen Compounds in Seleniferous Sulphuric Acid . BLUNT (T . P.). A Simple Nitrometer . OSMOND (F.). Colorimetric Estimation of Phosphorus . SIDERSEY . Apparatus for Determining Carbonic Anhydride in Carbo- nates . PETTERSON (0.) and A . PALMQUIST . Portable Apparatus for the Estima- tion of Carbonic Anhydride in the Atmosphere . FLUCKIQER (I? . A.) . Lithium Carbonate . WEIL (F.). Titration of Zinc Powder . , . SCHAND (A.). Electrolysis of Copper and Zinc . KLEIN (J.). Estimation of Formic Acid and of Organic Matter in Water . TOLEER (0.). Determination of Hippuric Acid in Urine .GAWALOWSEI (A.) . FEDERER (E . C.). Test for Oil of Peppermint . HELBING (H.). Reaction of Strophanthin . BIRD (F . C . J.). A Filter Tube for Use in the Estimation of Alkaloi‘ds by Mayer’s Reagent . LOSCH (A.). The’ine Estimation . PAUL (B . H.) and A . J . COWVNLEY . Coffee . PADB (L.). Analyses of Coffee . BLUM (L.). Detection of Albumin in Urine . PALM (R.). Determination of Milk Constituents . HEMPEL (W.). Source of Error in Gas Analysis . HEMPEL (W.). A Gas Burette which is Independent of Atmospheric Pres- sure and Temperature . MALOT . Estimation of Phosphoric Acid . KALMANN (W.) and J . SPULLER . Examination of Crude Soda Lyes and Red Liquors . LEVY (L.). Estimation of Titanic Acid . JOLLES (A.). New Chloroform Reaction . PLUGGE (P . C.). Test for Narce‘ine .Separation of Mineral Oils from Sapodable Fats MEHU (C.). Urea Estimation . MACKINTOSH (J . B.). Bas Apparatus . PAGE 865 865 865 865 866 866 866 866 867 867 868 868 869 869 870 870 871 871 871 872 872 996 997 998 998 998 999 999 999 1000 1000 1000 1000 1001 1001 1001 1001 1001 1002 1002 1002 1002 1003 1003 1062 1062 1063 1063 1064 1137xlviii CONTENTS . BREAL (E.). New Method of Testing for Nitrates . PAULY (C.). Detection of Potassium . FOCKE (H.). Determination of Alkaline Chlorides in Crude Potash . BAUDOIN . Testing Copper Sulphate . MEINEKE (C.). Analysis of Clay . MEINEKE (C.). Determination of Manganese . NEUMANN (G.). Determination of Metallic Iron in Slags . MORGAN (J . J.). Rapid Estimation of Silicon, Sulphur, and Manganese in Iron and Steel .TURNER (T.). Estimation of Silicon in Iron and Steel . PLATZ (P.). Determination of Sulphur in Iron . MCCKJLLOCH (N.). Volumetric Estimation of Cobalt in Presence of Nickel . MACINTOSH (J . B.). Separation of Nickel and Cobalt from Iron . MOORE (T.). Precipitation of Nickel in Presence of Iron . Water Analysis . HEHNER (0.). Eitimaiion ok Methyl Alcohol in Presence of Ethyl AIcobol . FISCHER (B.) . Dimethyl Ethyl Carbinol . LEGLER (L.). Estimation of Glycerol . HEHNER (0.). Estimation of Glycerol and its Non-volatility with Aqueous DAFERT (F . W.). Determination of Moisture in Starch . YOUNG (W . C.). Logwood Test for Alum in Bread . LINDE (0.). Estimation of Hydrocyanic Acid . ELASON (P.). Estimation of Thiocyanic Acid . CRAMPTON (C . A.) and T . C . TRESCOT .Estimation of Carbonic Acid in Beer . KOCH (R.). Estimation of Free Acid in Tannin Liquor . FARER (H.). Determination of Fat in Milk . ALLEN (A . H.). Reichert’s Distillation Process . CAMPANI ((3.). Volumetric Estimation of Urea . HESSE (0.). Estimation of Quinine Sulphate . ALLEN (A . H.). Detection of Hop-substitutes in Beer . RANSOM (F.) . Estimation of Ipecacuanha . Detection of Aniline Colours iii Wine MANNLEY (G.). Estimation of Indigo . LENZ (W.). Testing Indigo Dyes on Fabrics . MARTIN (E . W.). MYLIUS (F.). Pettenkofer’s Reaction . Vapour . EERNER (G.) and A . WELLER . Testing Quinine Sulphate . CURTMAN (C . 0.). Detection of Artificial Colouring Matters in Butter . LIEBERMANN (L.). Detection of Albumin in Urine . PAGE 1138 1138 1138 1139 1139 1139 1140 1140 1140 1141 1141 1141 1141 1141 1142 1142 1142 1143 1143 1143 1143 1144 1144 1144 1144 1145 1145 1145 1146 1146 1147 1147 1147 1147 1149 1149 1149J O U R N A LH.BAKER.CHICHESTEB H. BELL, M.B.D. BENDIX.C. H. BOTHAMLEY.B. H. BBOUBH.C. F. CROSS.A. H. FISON.J. FLETCHER.W. D. HALLIBUBTON, M.D., B.So.J. P. Laws.D. A. LOUIS.T. MAXWELL, M.D., B.Sc.N. 'IT. J. MILLER, Ph.D.G. H. MORRIS, Ph.D.OFJ. M. H. MUNBO, D.Sc.A. PHILIP.E. W. PREVOST, Ph.D.R. ROUTLEDBE, B.Sc.M. J. SALTER.C. SPURGE, B.A.JAMES TAYLOR, B.Sc.A. THILLOT.L. T. THOBNE, Ph.D.H. I(. TOMPKINS, B.Sc.V. H. VELEY, M.A.W. 0. WILLIAMS, B.Sc.W. P. WYNNE, B.Sc.THE CHEMICAL SOCIETY.H. E. ARMSTBONG, Ph.D., F.R.S.W. CBOOKES, F.R.S.F. R. JAPP, M.A., Ph.D., F.R.S.A.I(. MILLER, Ph.D.HUGO MULLEB, Ph.D., F.R.S.W. H. PERKIN, Ph.D., F.R.S.S. U. PICKERINB, M.A.R. T. PLIMPTON, Ph.D.W. J. RUSSELL, Ph.D., F.R.S.J. MILLAR THOMSON, F.R.S.E.T. E. THOBPE, Ph.D., F..R.S.&bitrrr :C. E. GROVES, F.R.S.Sttb-6bitar :A. J. GBEENAWAY.VOl. LII.I 8 8 7. ABSTRACTS.LONDON:J. V A N V O O R S T , 1, P A T E R N O S T E R ROW.1887LONDON :HARRISON AND SONS, PBINTERS IN ORDINARY TO HER MAJESTY, ST. MARTIN’S LAKEC 0 N T E N T S.ABSTRACTS OF PAPERS PUBLISHED IN OTHER JOURNALS :-General and Physical Chemistry.PAGESTROUXBO. Production of White Light by E x i n g the Colour~ of theSpectrum .LIEBEPMANN (C.) and S. v. KOSTANECKI. Spectra of the Methyl-derivativesof Hydrox anthraquinone .VERNEUIL (AJ.Preparation of Calcium Sulphide with a Violet Phos- 'phorescence .BOISBAUDRAN (L. DE). Fluorescence of Manganese Compounds .BOISBAUDRAN (L. DE). Fluorescence of Bismuth Compounds .LUVINI (J.). Electrical Conductivity of Gases and Vapours .WINKELMANN (A,). Relation of the Conductive Capacity of Gases to Tem-perature.GRAETZ (L.). Electrical Conductivity of Solids at High Pressures .SCHIFF (R.). Speciflc Heats of Homologous Series of Liquid Organic Com-pounds .BLAREZ (C.). Saturation of Normal Arsenic Acid with Barium Hydroxide .BLAREZ (C.). Saturation of Arsenic Acid with Calcium and StrontiumOxides . , .DE FORCRAND. Sodium Glycerolate .SCHIFF (R.). Heat of Evaporation of Homologous Carbon Compounds .MEISSNER (F.).Heat evolved when Powders are Moistened .ZEHNDER (L.). Determination of the Sp. Gr. of Soluble Substances .BERTHELOT and ANDR~. Tension of Dissociation of Ammonium HydrogenCarbonate .BERTHELOT and ANDRS. Decomposition of Ammonium Hydrogen Carbo-nate by Water, &c.DUCLAUX (E.). Chemical Changes produced by Sunlight .EDER (J. M.). Practical Methods of Photographing the Spectrum .HABERMA" (J.). Electrolysis of Carbon Compouuds .BERTHELOT. Thermochemistryof Phosphates .GAL (H.) and E. WEBNEB. Heat of Neutralisation of Homologous andIsomeric Acids .GAL (H.) and E. WERNER. Heats of Neutralisation of Malonic, Tartronic,and Mdic Acids .BERTHELOT. Thermochemistry of Reactions between Magnesia Salta andAmmonia .STOHMANN (F.), P. RODATZ, and H.HERZBEPG. Heats of Combustion andFormation of Homologous Phenols .DE LANDERO and R. PRIETO. Some Laws of Chemical Combination .HUNT (T. S.). Law of Volumes in Chemistry .LESCCEUR (H.). Velocity of Dissociation .RAMSAY (W.) and S. YOUNQ. Nature of Liquids .TBAUBE (J.). Capillary Constants and Meniscus Angle .GUIGNET (C. E.). Crystallisation by Diffusion .TREY (H.). Influence of some Normal Salts on the Hydrolysis of MethylAcetate .DIXON (H. B.). Preservation of Gases over Mercury .a 211234 a55698899910119393949495969698999910010010110110210iv CONTENTS.BECKMANN (E.). Cracking Glass with Certainty.WALTER (J.). Apparatus for Chemical Laboratories .DUCLAUX (E.) . Actinometr? .BOISBAUDRAN (L.DE). Fluorescence of Manganese and Bismuth .BECQUEREL (E.). Effect of Manganese on the Phosphorescence of CalciumCarbonate .BOISBAUDRAN (L. DE). Red Fluorescence of Alumina.BECQUEREL (E.). Phosphorescenee of Alumina .BRUHT, (J. W.). Molecular Refraction of Liquid Organic Compounds ofHigh Dispersive Power .BRUHL (J. W.). Experimental Examination of the Older and More RecentDispersion Formuh .THOMSEN (J.). Supposed Influence of Multiple Bonds of Union on theMolecular Refraction of the Hydrocarbons .BRUHL (J. W.) . Thomsen’s Supposed Explanation of Molecular RefractionRelations .PELLAT (H.). Absolute Electrodynamometer .ELOBUKOFF (N. v.). New Appamtus for Electrochemical Investigations .PIONCHON.JOLY (A.). Thermochemistry of Bibasic Phosphates and their Congeners .BERTHELOT.Ammoilium Magnesium Phosphate.BLAREZ (C.). Saturation of Arsenic Acid by Magnesia. Formation ofAmmonium Magnesium Arsenate . , .DE FORCRAND. Heat of Formation of Potassium Methoxide and Ethoxide .GAL (H) and E. WERNER. Heats of Neutralisation of Glyceric andCamphoric Acids .GAL (H.) and E. WERNER. Heats of Neutralisation of Malic and CitricAcids .GAL (H.) and E. WEXNER. Heats of Neutralisation of Meconic andMellitic Acids.KAHLBAUM (G. W. A.). Temperature Regulator.EAHLBAUM ((3. W. A.). Influence of Atmospheric Pressure on BoilingKAHLBAUM (G. W. A:). Boiling Points of t i e Fa’tty Acids C,H,O, td.RAOULT (E.). Vapour-tensions of Ethereal Solutions .EAHLBAUM (GI.. W. A.).Apparatus for measuring the Tension ofVapours .MULLER-ERZBACH (W.). Dissociation of Salts containing Water of Crystal-lisation .MULLER-ERZBACH (W.). Dissociation of Copper Sulphate .LESC~UR (H.). The Relation between the Efflorescence and Deliquescenceof Salts and the Maximum Vapour-tensions of their SaturatedSolutions .MCGREGOR (J. G.j. Density of Weak Aqueous Solutions of Salts .TOMLINSON (C.). Cohesion and Submemion Figures .TEAUBE (J.). Weight of Drops and their Relation to Capillarity .DELACHABLONNY (P. M.). Tolatillsation of Dissolved Substances duringthe Evaporation of the Solvent .SPRING (W.). The Periodic Law.COBNU (M. A.). Distinction been Spectral Lines of Solar and TerrestrialOrigin .KOBB (G.). Spectrum of Germanium .WEISS (A.).Fluorescence of the Pigments of Fungi .EALISCHER (M.). New Secondary Element .LAURIE (A. P.). Electromotive Force of a Constant Cell with Moving PlatesLAURIE (A. P.) . Electromotive Force of a Voltalc Cell having an AluminiumPlate as Electrode .MENDENHALL (T. C.). Electrical Resistance of Soft Carbon under Pres-sure . I .Specific Heats and Changes of State a t High TemperaturesPoint .CSHlo02. - . - .PAGE10510518918919019119119119519820020020020120220220420420520520620620620720720720720820820920921021 121131331331431431431531COSTENTS.GRAY (T.). Electrolysis of Silver and Copper : Application of Electrolysisto the Standardising of Electric Current and Potential Meters .FROMME (C.) .Electrolytic Polarisation produced by Small ElectromotiveForces .AYRTON (W. E.) and J. PERRY. Expansion of Mercury between 0" and-39" .DE FORCRAND. Heats of Formation of Potassium Alkyl Oxides.DE FORCRAND. Heat of Formation of Sodium Alkyl Oxidea .DE FOECRAND. Potassium Glycerolate.RAMSAY (W.) and S. YOUNG. Thermal Properties of Ether .NICOL (W. W. J.). Vapour-pressures of Water from Salt Solutions .LESC(EUR (H.). Vapour-tension of Sodium Acetate .STEFAN (J.). Relation between the Theories of Capillarity and of Evaporrt-tion .OSTWALD (W.), Coefficients of Affinity of Bases.LEMOINE ((3.). Influence of Heat on the Decomposition of Oxalic Acid byFerric Chloride .HOOD (J. J.). Theory of Fractional Precipitation .MEYER (L.).Halogen Carners .WILLGEEODT (C.). Halogen Carriers ..WILLGERODT (C.). Indium and Gallium as Halogen Carriers .AYRTON (W. E.) and J. PERRY.BOISBAUDRAN (L. DE). Red Fluorescence of Alumina.BECQKTEBEL (E.). Phosphorescence of Alumina .LOMMEL (E.). Phosphorescence .DUCLAUX (E.). Comparative Action of Heat and Solar Radiation .ROWLAND (H. A.). Water Battery .HARDING (5. L.). Sodium Uichromate Cell.WARREN (H. N.). Ferric Chloride as an Exciting Agent for VoltaicBatteries .NEGREANO. Specific Inductive Yower of Liquids.EBELING (A.). Electromotive Force of some Thermo-elements .STREINZ (F.). Galvanic Polarisation of Aliiminium .ARBHENIUS (5.). Conductivity of Mixtures of Aqueous Solutions of Acids.BLOWN (J.). Theory of Voltaic Action .DRAKE (D.) and J.M. GRAHAM. Electric Accumulators .JANEEEK (G.).LANGCLOIS (M.). Specific Heats of Liquids .COLSON (A.). Isomerism of Position .ARMSTRONG (H. E.). Determination of the Constitution of Carbon Com-pounds from Therrno-chemical Data .PICKERING (S. U.). Determination of the Constitution of Carbon Compoundsfrom Thermo-chemical Data .BLUHL (J. W.). Criticism of Thomsen's Theory of the Heat of Formationof Organic Compounds .STOHMANN (F). Thomsen's Investigations . DE FORCRAND. Alcoholates of Sodium Glyceroxide .DE FORCRAND. Alcoholates of Potasbium Glyceroxide.STORMANN (B'.), P. RODATZ, and w. HEXzlsERG. Heat Equivalent of theHomologues of Benzene.STOHMANN (F.), P. RODATZ, and W. HERZBERG. Heat Equivalent of Ethersof the Phenol Series .THORPE (T.E.) and A. W. RUCKER. Relation between the Critical Tem-peratures of Substances and their Thermal Expansion as Liquids .BABTOLI (A.) and E. STRACCIATI. Relation between the Critical Tempera-tures of Siibstances and their Thermal Expansion as Liquids .THRELFALL (R.). Specific Heate of the Vapours of Acetic Acid and NitrogenTetroxide . , .RAMSAY (W.) and S. YOUNG. Influence of Change of Condition from theExpansion produced by AmalgamationDetermination of Atomic Weight from Specific Heat .vPAGE3163173173183193203203213223 2332432432532632632632740940941041 141241241341341441 541 541741841941942042042 3423425426427427428429429429Liquid tb the Solid State on Vapour-pressure " .43vi ONTENTS .RAMSAY (W.) and S . YOUNQ . Nature of Liquids aa shown by a Study ofthe Thermal Properties of Stable and Dissociable Substances .DYSON ((3.). Apparatus for Determining Vapour-densities .LE CHATELIER (H.). Thermodynamics and Chemistry .WROBLEWSKI (S . v.).BLUMCKE (A.). Specific Gravities of Mixtures of Ethyl Aicohoi andCarbonic Anhydride .MULLER-ERZBACH (W.). Dissociation of Sodium Phosphate .BEAUN (F.)- Solubility of Solid Substancee arid the Changes in Volume andEnergy accompanying Solution .COLEMAN (J . J.). Liquid Diffusion .LOEW (0.). Catalytic Actions .THOMSEN (T.). Conditions of Equilibrium in Aqueous Solutions : Action ofAqueous Soda on some Normal Sodium Salts .VALENTINI (A.).Lecture Experiments .DEMARQAY (E.). Spark Spectra from Coils at Low Tension .BECQUEREL (H.). Variations in the Absorption Spectrum of Didymium .BOISBAUDRAN (L . DE) . Red Fluorescence o€ Alumina .VERNEUIL (A.). Phosphoreswnce of Calcium Sulphide .BECQUEREL (E.) Phosphorescence of Calcium Sulphide .GERNEZ (D.). Rotatory Power of Compounds formed in Solutions ofTartaric Acid .BOROHERS (W.). Galvanic Element .GOUY . Standard Galvanic Cell .FEOMIKE (C.). Galvanic Polarisation produced by Feeble ElectromotiveForces .DE FORCRAND . Action of Ethylene Bromidi on kkyl'Metklic dxides .GUNTZ . Heat of Formation of Tartar Emetic .HORSTMANN (A.). Molecular Volumes .ENGEL (R.). Solubility of Sulphates .PARMENTIER (F.).A Particular Case of Solution .CHANCEL (G.) and F . PAEMENTIER . Solubility of Calcium OrthobutyrateLE CHATELIER (H.). Laws of Solution .CHROUSTCHOFF (P.) and A . MARTINOFF . Coe5cients of Chemical Affinity .OLSZEWSKI (K.). Absorption Spectrum of Liquid Oxygen and of Atmo-spheric Air .BOISBAUDRAN (L . DE) . Red Fluorescence of Alumina .NASINI (R.). Molecular Refraction of Carbon Compounds .MANEUVRIEB ((3.). Formation of the Electric Arc without Contact OE theElectrodes .GRIMALDI ((3 . P.). Thermic Expansions of Liquids at Various Pressures .CHAPPUIS (J.). Latent Heat of Vaporisation of certain Volatile Sub-stances .BEETHELOT and RECOURA . The Calorimetric Bomb .MVLLEB-ERZBACH (W.) . Dependence of Chemical Affinity on TemperatureROOZEBOOM (H .W . B.). Thermal Study of Hydrobromic Acid SolutionsROOZEBOOM (H . W . B.). Conditions of Equilibrium of Two Substances inthe Solid, Liquid, and Gaseous Stakes .Isopyknics .and Isobutyrate .and Hydrate .ROOZEBOOM (H . W . B.).ROOZEBOOM (H . W . B.). New Hydrate of Hydrobromic AcidThe Hydrate HBr, 2H20 .ROOZEBO?M (H . W . B.). Combination of Ammonium Bromide with Am-monia .RAOULT (F . M.). Influence of Concentration on the Vapour-tension ofEthereal Solutions .BOTT (W.) and D . S . MAONAIR . Apparatus for Determining Vapour-densities .CHANCEL (G.) and F . PAEMENTIEX . Variation of Solubility with Variationof Heat of Solution .PAGB43043143143243543643644044-4344044253753'753853954054.4)54154154154454464554654754754854862562562662662662'762762862862963063163163163263CONTENTS .v iiENGCEL (R.). Effect of Nitric Acid on the Solubility of Nitratm .HAGEMANN (G . A.) . Aviclity-formula .ROSENFELD (M.). Lecture Experiment : Electrolysis oi? HydrochloricAcid .SCHALL (C.). Lecture Experiment : SpecXc Heat of Zinc .Constant Gas Generator .STENGEB (F.). Absorption-bands of Chlorophyll .EALISCHER (S.). Electromotive Force produced by Light in Selenium .OLSZEWSKI (K.). Density of Liquefied Methane, Oxygen, and Nitrogen .THOMSEN (J.) . Avidity-formula .SLEENBUCH ((3.).WARREN (T . T . P . B.). Vapour-density ApparatusSCHALL (C.). Determination of Vapour-densities .AMAGAT (E .H.). Expansion and Compressibility of Water ..SCHUMANN (M.). Compressibility of Aqueous Chloride Solutions .MULLEE-EBZBACH (W.). Rate and Vapour-tension of Diseociation .FOUSSEREAU ((3.) Effect of Pressure on the Decomposition of Chloridea .RUGHEIMEE (L.) . Practical Thermo-regulator .Refractive Index of Ice .CHAPPUIS (J.) and C . RIVI~BE . Refractive Index and Compressibility ofCyanogen .NASINI (R.) and A . SCALA . Molecular RefracOive Energies o€ Derivatives ofNASINI (R.) and A . SCALA . Molecular Refractive Energies of Thiocyanatesand Thiocarbimides .BOISBAUDBAN (L . DE) . Red Fluorescence of Chromiferous Gallium .PRIBRAM (R.). Specifh Rotation of Optically Active Substances in veryDilute Solution .TOMASSI (D . and RADIGUET .Electric Couple with Carbon Element8 .KROUCHKOLL .BOUTY (E.). Conductivity of Acids and Salt6 in Dilute Solutions .BOCK (0.). Conductivity of Compounds of Potassium and Sulphur in Solu-tion. of Sodium Sulphide. and of Boric Acid .ECSAS (A.). Nobili’s Rings and Allied Electrochemical Phenomena .FA^ ((3.). Variations in the Electrid Resistance of Antimony and Cobaltin a Magnetic Field .NICOL (W . W . J.). Expansion of Salt Solutions .BEBTHELOT and C . FABEE . Tellurium .THOMSEN (J.). Heats of Combustion of Organic Substances .BERTHELOT and RECOUBA . Heats of Combustion .BEBTHELOT and LOUQUININE . Heats of Comhustion .RAMSAY (W.) and S . YOUNG . Continuous !lhansition from the Liquid toCHAPPUIS (J.) and C . RIVI~RE . Vapour-tension of Liquid Cyanogen .MACNAIB (D .S.). Apparatus for Vapour-density Determinations .MULLER-EEZBACH (W.). Hydrates of Barium and Strontium Hydroxides .SCHULZE (C . R.). Amount of Water of Crystallisation contained in someSalts .FOUSSEREAU (G.). Decomposition of Acetates by Water .REICHER (L . T.). Velocity of 8aponification .MILLS (E . J.). Action of Heat on Potassium Chlorate and Perchlorate .UBECH (F.). Influence of Temperature on the Rate of Inversion of Cane-sugar .UBECH (F.). Velocity of Chemical Reactions .SCHALL (C.) Demonstration of Avogadro’s Hypothesis .MEYER ((3.).Carbon Bisulphide .EETTELER (E.). Dispersion in Rock Salt .NEUMANN (2 . v.). Nickel and Carbon Elements .EISENMANN (R.) . Galvanic Element .Polarisation of Copper .WEBER (C .L.). Conductivity of Amalgams .the Gaseous State at all Temperatures .EMDEN (R.). Vapour-tensions of Saline Solutions .LESCGCUR (H.). Hydrates of Barium Chloride .PAGE6326336336336346346936936%695695695696696697697698698753163753754754155755756757757957757158158159760760761761761762763764!76476576576616676776776776viii CONTENTS.GOSSART. The Spheroidal State .BRAUN (F.) . Decrease of Compressibility of Ammonium Chloride Solutionswith Increase of Temperature, .M~RMET (A.). Lecture Experiments .BOISBAETDRAN (L. DE). Fluorescence of Manganese and Bismuth .BECQU~EL (18.). Variations in the Absorption-spectra of Didymium Salts.BOTHAMLEY (C.H.). Orthochromatic Photography .BOUTY (E.). Conductivity of Mixtures .BERTHBLOT. Phosphates of the Alkaline Earths .JOLY (A). Trimetallic Phosphates .STOHMANN (F.). Heats of Combustion of Organic Compounds .STOHMANN (F.), P. RODATZ, and W. HERZBERG. Heat Equivalents ofBenzyl-compounds .FLAWITEEY (F.). Relation between the Boiling Points of the MonatomicAlcohols and their Constitutions .EOLA~BE (F.) . Alteration of Freezing Points .NATANSON (E.). Cooling of Carbonic Anhydride on Expansion .SKINNER (S.). Phosphonium Chloride .SCHALL (C.) . Vapour-density Apparatus .SCHALL (C.). Determination of the Vapour-density of High Boiling Sub-stances under Reduced Pressure .SPRING (W.). Influence of Temperature on the Rate of Action of certainAcido on Marble .BOUTY (B.).Application of the Electrometer to the Study of ChemicalReactions .FOUSSEREAU ((3.). Decomposition of Thiosulphates by Acids .MEYEB (L.). Apparatus for Fractional Distillation under Reduced PressureBRUHL (J. W.). Influence of Single and Double Union on the RefractivePower of Compounds : Constitution of Benzene and Naphthalene .BOISBAUDRAK (L. DE). Fluorescence of Spinel .CROOKES (W.). Crimson Line of Phosphorescent Alumina .BOISBAUDRAN (L. DE). Fluorescences of Manganese and Bismuth .BOISBAUDRAN (L. DE). New Fluorescences with well-defined Spectra.DEMAE~AY (E,). Spectra of Didymium and Samarium .WRIQHT (C. R. A.) and C. THOMPSON. Development of Voltaic ElectricityDEBRAY (H.) and €'&CHARD. Alteration of the Carbon Electrodes used forthe Electrolysis of Acids .RIQHI (A.).Conductivity of Bismuth for Heat in a Magnetic Field .VIOLLE (J.). Comparative Radiation of Fused Platinum and Fused Silver .BERTHELOT and FABRN. Heat of Formation of Hydrogen Telluride .FABRE (C). Heat of Formacion of Crjstallised Tellurides .STOHMAN (F.). Heats of Combustion of Organic Compounds as Determinedby Different Methods .BERTHELOT and RECOURA. Passage from the Benzene to the Acetic Series .GERLACH (G. T.). Boiling Points of Salt Solutions .AMAQAT (E. EL). Solidification of Liquids by Pressure .THOMSON (J. J.). Dissociation of some Gases by the Electric Discharge .GOUY and 8. CHAPERON. Osmotic Equilibrium and the Concentration ofSolutions by Gravitation .SCHIFF (R.). Demonstration of the Coefficient of Expansion as a LectureExperiment .REYCHLER (A.).Estimation of Pressure in Closed Tubes .TROWBRIDQE (J.) and C. C. HUTCHINB. Oxygen in the Sun .TROWBRIDGE (J.) and C. C.HUTCHINS. Carbon in the Sun.HUTCHINS (C. C.) and E. L. HOLDEN. Existence of certain Elements andDiscovery of Platinum in the Sun .SUNDELL (F.). Spectrum Analysis .CROOKES (W.). Radiant Matter Spectroscopy : Examination of the ResidualGlow .by Atmospheric Oxidation .PAGB768768769873873874877877877878879879880882882882882am8838841005100510061006100810081008100910091010101010101011101 11012101310131013102310141065106510651066106CONTENTS .CBOOKES (W.).SharpLine Spectrum of Phosphorescent Aluminium .CROOKES (W.). Sharp Line Spectra of Phosphorescent Yttris and Lan-thana .GRUNWALD (A.). Chemical Structure of Oxygen and Hydrogen and theirDissociation in the Sun’s Atmosphere .STAATS (G.). Photochromatic Properties of Silver Nitrate .MOORE (T.). Modification of the Ferric Chloride Cell .BUCEANAN (J.). Electrical Conductivity of Hot Gases .MIESLER (J.). Electromotive Dilution Constants of Silver and CopperSalts .BOLTZMANN (L.). Thermochemical Law conjectured by Pebal respectingNon-reversible Electrolytic Actions .BOYS (C . V.). Bunsen’s Ice Calorimeter .KEISER (E . B.). New Pyrometer .BEKETOFF (N . N.). Change in Volume during the Formation of MetallicOxides .SPRING (W.) and E .PAN AUBEL . Action of Acids on Zinc containingLead .HUNT (T . S.). Integral Weights in Chemistry .Inorganic Chemistry .LUNGE ((3.). Conversion of Calcium Hypochlorite into Calcium Chlorate .RAMMELSBERG (C.). Crystalline Silicocarbonate from Soda Liquors .Sodium Calcium Carbonate .ROSENBLADT (F.). Double Nitrites of Cesium and Rubidium .BUNSEN (R.) Decomposition of Glass by Carbonic Anhydride condensedon its Surface .REIDEMEISTER ((2.).BOISBAUDRAN (L . DE) . Purification of Yttria .OSMOND . Heating and Cooling of Cast Steel .KNIESCIIE (l?.). Tungsten .PFORDTEN (0 . v . d.). Titanium .BOISBAUDRAN (L . DE) . Atomic Weight of Germanium . , .KRUSS (G.). Gold Oxides .BASSETT (H.) and E . FIELDINQ . Action of Hypochloroue Anhydride onIodine Trichloride .BLAREZ (C.).Saturation of Selenious Acid by Bases .KAPPEL (S.). Formation of Nitrites .RUDORFF (I!.). Compound of Arsenious Oxide with Halogen Salts .PLINGLE (A.). Some Probable New Elements .CASTNER (H . Y.). Production of Alkali Metals .LEIGHTON (G . W.). Crystalline Scale formed in the Manufacture of SodiumHydrogen Carbonate .HEYER (C.). Strontia Dihydrate .BLOUNT (B.). Calcium Borate .BLOXAN (C . L.).WHEELER (H . A.).NORDENSKIOLD (A . E.). Eqnivalent of Gadolinium Oxide .KNAPP (F.). Formation of Ultramarine in the Wet Way .STANLEY (A.) . Sodium Dichromate .&Uss (G.) and H . SOLEREDEL . Reduction of Inorganic Sulpho-salts byHydrogen .WADDELL (J.). Atomic Weight of Tungsten .RASCHIG (F.). Compounds of Gold with Nitrogen .GIBBS (W .) . Complex Inorganic Acids .JORGENSEN (9 . M.). Roseo-rhodium Salts .JORGENSEN (S . M.). Nitratopurpureo-rhodium Salts .ROSENIXADT (T.). Solubility of some Gold Compounds .Calcium Ammonium Arsenate and Calcium ArsenateArtificial Lead Silicate from Bonne Terre, MontanaixPAGE106910’701070107110711071107210’7210731073107310’741077111212121313141414151516106106106107107107108108108108109109110110111111112113113114JORQENSEN (S . M.j. XanthoIrhddium Salts . 11X CONTENTS.PAB'EWURSTER (C.). Active Oxygen in the Atmosphere . 211WURSTER (C.). Formation of Active Osygen in Paper . 211MOISSAX (H.). Phosphorus Pentafluoride .212WEBER (R.).SCHNEIDER (R.).sulphide. 213MCCAY (L. W.). Arsenic Pentasulphide . 213BLOCHMANN (R.). Carbonic Anhydride in the Atmosphere. 214JOLP (A.). Bimetallic Phosphates . 214JOLP (A.). Silver Phosphates and Arsenates . 215CARPENTER (R. F.). Solubility of Silver Chromate in Ammonium Nitmte . 216JENSCH (I%). Tetracalcium Phosphate and Basic Converter Slag. 216SCHEIBLER (0.). Determination of Water in the Hydrates of StrontiumOxide . 217FINKENER (R.). Actio; of Carbokc Ahhydride on the Dihydrate of Stron-tium Oxide . 217HEYER (C.). Estimation of Water in Btrontia DihSdrate . 217MENSCHING (J.) and V. MEYER. Vapour-density of Zina . 218HENSGEN (0.). Ammonio-mercuric Chromates . 218MAUXEK~ (E.). Water of Crystallisation of Alums .218JENSCH (E.). Composition of some Ancient Ceramics from Brandenburg . 218OSMOND. Heating and Cooling of Fused Steel . 219GAUTIER (F.). Influence of Silicon on the Condition of Carbon in Cast-won. 2 2 0XEHRMANN (F.). k Ndw Clks of'Cobktic Ekts . 220BLOMSTRAND (C. W.). Oxy-acids of Iodine. 327THOMSON (J. J.) and R. THRELFALL. Production of Ozone. 32'7SENDERENS (J. B.). Action of Sulphur on Ammonia and Metallic Bases inPresence of Water . 327WEBER (R.). Combinations of Sulphuric Anhydride with 'Phosphonc andIodic Anhydrides . 328TEONSON (J. J.) and R. THBELFALL. Passage of Electric Dischargesthrough Pure Nitrogen . 328HAUTEFEUILLE (P.) and J. MARGOTTET. Hydrated Silicon Phosphate . 329DEMAR~AP (E.). Action of Carbon Tetrachloride on Metallic Oxides .929QUANTIN (H.).Ferric Phosphate . , . 330SHITH (W.) and W. B. HART. Sodium Carbonate . , 330RAMMELSBEBQ (C.). Occasional Products in the Soda Manufacture . 331GOTTIG (C.). Water of Crystallisation of Sodium Monosulphide . 331DRAPER (H. N.). Silver Ammonio-nitrate . 331SEKDERENS (J. B.).Copper Nitrates . 331SPRING (W.).under the Influence of Pressure . 332BOURGEOIS (L.). Calcium Yilico-stnnnate . 333COEN (S.). Solubility of Gypsum in Solutions of Ammonium Salts . 333LINCK ((3.). Crystallography of Cadmium Borotungstate . 334OSBOBNE (T. B.). Higher Oxides of Copper . 334CROOEES (W.). New Elements in Gdolinite and Samarskite . 334CHRISTENSEN (0. T.). Chemistry of Manganese and Fluorine . 335GLASER (M.).Action of Potassium Permanganate on Sodium Thiosulphate 336DITTE (A.). Compounds of Stannic Oxide . 336PFORDTEN (0. V. D.). Titanium . 337MANASSE (0.). Vanadates of the Alkaline Eaxthe . 339MICHAELIS (A.). Valency of Bkmuth. 3.410HASEBROEK (K.). Action of Hydrogen Peroxide on Bismuth Salts . 3410KRUSS (G.). Atomic Weight of Gold . 340ERUSS ((3.) SublimedAuricChbride. 341Compounds of Selenious and Arsenious Anhydrides withBehaviour of Iodine with Reallgar and Arsenic Iodo-Sulphuric Anhydride . 212Action of Carbon Tetrachloride on Chromyl Dichloride andAction of Non-metals on Solutions of Silver andReaction between Barium Caxbonate and Sodium SulphatCONTENTS . xiWINCKLER (C.). Preparation of Chlorine from Bleaching Powder .STOLBA (F.). Action of Hydrochloric: Acid on Sphalerite .BERTHELOT .Metals and Minerals of Ancient Chaldea .WARREN (H . N.). Decomposition of Ammonium Chloride by an Alloy ofZinc and Iron .SHAW (W . N.). Atomic Weights of Silver and Copper .PREIS (X.) and B . RAYMANN . Decomposition of Sodium Sulpharsenatewith Silver Nitrate .OTTO (H.). Tetracalcium Phosphate and Basic Slag .ENGEL (R.). Effect of Hydrochloric Acid on the Solubility of Chlorides .DIXON (W . A ) . Constitution of Acids .MEYEE (V.). Properties of some Metals .BIRD (G . B.). Purification of Zinc .HARDAWAY (H.). Analysis of ShotKUBEL (W.). Preparation of Lead Carbonate .BERRY (N . A.). Copper SlagHARRISON (GI.. ). Mirror Amalgam .BIRD (GI.. B.). Mercurous Hydroxide .BAYER (9 . J.).Rasic Aluminium Sulphate .Sulphide ..ANDR& (GI.. ). Action of Lead Oxide on Soluble Chlorides .ANDRS ((3.). Action of Mercuric Oxide on Dissolved Chlorides .CERISTENSEN (0 . T.). Fluorine and Manganese Compounds .CLAASSEN (E.). Solubility of Manganese Sulphide in Fused PotassiumHOOD (J . J.). Preparation of Ammonium Dichromate .CLAASEN (E.). Extraction of Vanadium and Chromium from Iron Ores .KRUSS (G.). Gold .MILES (F . P.). Formation of Potaesium Silicate .RASCHI~ (F.). Action of Nitrous Acid on Bulphurous Acid .VAN NUYS (T . C.), and B . F . ADAMS .MENSCHINQ (3.) and V . MEYER .WTTIG (C.) New Hydrate of Sodium Hydroxide .SENDERENS ( J . B.) Action of Metals on Solutions of Silver Nitrate .WARREN (H . N.). Zinc-eisen .THOMS (H.) Ammonio-zinc Chlorides .MABERY (C .F.) Products from the Cowles Electrical Furnace .MEYER (L.), Action of Carbon Tetrachloride on Oxides .DONATR (E.) Barium Manganate .ROUSSEAU (G.). Formation of Manganites from Permanganates .BENDER (G.). Non-existence of Chromium Heptasulyhide .MUTEMANN (W.). Lower Oxides of Molybdenum .SEUBERT (K.) and SCHURMANN . Bromostannic Acid .KR~JSS ((3.). Gold .EREUSLER (U.). Amount of Oxygen in the Atmosphere .OLSZEWSKI (K.).RASCHIQ (F.). Reaction of Nitrous Acid with Sulphurous Acid .KRAUT (K.). Oxidation of Ammonia in presence of Platinum or Palla-dium .FRANKE (B.). Hyhroxylated Solii Hyirogen Phosphide .GOTTIG (C.). Hydrates of Potassium Hydroxide .MUTHMANN (W.) . Argentous Compounds .JOLY (A.).ANDR& ((3.).Ammoniacal Compounds of Cadmium Chloride .ANDRI~ ((3.). Ammoniacal Compounds of Cadmium Sulphate and Nitrate .OSMOND (F.). Effect of Manganese, &c., on the Properties of Steel .KNOP (A.). Crystallised Niobic Anhydride .Carbonic Anhydride in the AirVapour-density of Potassium IodideDEMARCAY (E.) Cerite Earths .SEUBERT (E.). Chlorostannic Acid .Boiling Point of Ozone : Solidification of Ethylene .Double Phosphates and Arsenates of Strontium and SodiumDITTE (A.). Alkaline Vanadates .COSSA (A.). Animoniacal Platinum Compounds .PAGE44244244.344344344A44444544544544644644644644744744744744744844944944945045054954955055055055055165155155255255255355355455455463463463563563563663663763763863963964264xii CONTEXTS .MACIVOR (R .W . E.). Perbromic Acid .CURTIUS (l‘.). Diamidogen or Hydrazine .DRECHSEL (E.). Nitrous Acid .LESC(EUR (H.) Hydrates of Sodium Arsenate .DE MOND~SIR (P.). Particular Case of the Formation of Sodium Hypo-bromite .DRAPER (C . N.). Solubility of Lithium Carbonate .DRECHSEL (E.). Argentous Componnds .PFORDTEN (0 . v . D.).WANKLYN (J . A.). Specific Gravity of Lime-water .LUNGE (G.) and R . SCHOCH .VILLIERS (A.). Barium Phosphates .WARREN (H . N.). Thallium in Platinum .WARREN (H . N.). Preparation of Anhydrous Metallic Chlorides .WARREN (H . N.). Action of Nitrogen on Certnin Metals .MENKE (A . E.).SHIMER ( P .W.). Titanium Carbide in Pig-iron .DRECHSEL (E.). Formation of Complex Inorganic Acids .KBUSS (G.) and L . F . NILSON . Equivalent and Atomic Weight ofThorium .KRUSS (G.) and L . F . NILSON . Potassium Germanium Fluoride .DITTE (A.). Alkaline Vanadates .KRUSS (G.) and L . F . NILSON . Reduction of Potassium Niobium Fluoridewith Sodium .KBUSS (G.) and L . F . NILSON . Earths and Niobic Acid from Fergusonite .NEUMANN (G.) . Preparation of Oxygen and of Sulphurous Anhydride withKipp’s Apparatus .MICHAELIS (A.) . Vapour-density of Tellurium Tetrachloride : Valency ofTellurium .WAR~EN (H . N.). Nitrogen Fluoride .ALLARY (E.). Regeneration of Acid Residues in the Manufacture of Gun-cotton .MULLEB (J . A.). Influence of Temperature and Pressure on the Action ofDE MONDBSIR (P.). Artificial Production of Trona or Urao .BAILEY (G .H.). Silver Suboxide .ENGEL (R.). Solubility of Calcium and Magnesium Chlorides in WateratOo .FORM~NEK (J.). Solubility of Lead Chloride in Solutions of MercuricChloride .The Lowest Compounds of SilverAction of Ammonia on Bleaching-powderAction of Ferric Sulphate on IronPotassium Chloride on Crude Methylamine Carbonate .SAGLIEB (A.). Ammonium Copper Iodides .~ T A R D (A.). Solubility of Copper Sulphate .BAUBIGNY (H.). Schweizer’s Reagent and “Eau Celeste” .MEYER (V.). Stability of Corrosive Sublimate Solution .BUCHNER (E.). Action of Carbonic Anhydride on Ulti.amarine .CLAASSEN (E.). Manganese Sulphate .LAUGIEB (P.). Action of Selenious Acid on Manganese Dioxide .JORGENSEN (a .M.). Cobaltammonium Compounds .KEHRMANN (F.). Structure of Complex Inorganic Acids .KEHRMANN (F.). Phosphotnngstic Acids .WEIBULL (M.). Crystallised Compounds of Zirconium .MAUMENR (E.). Alloys of Platinum, Iron, and Copper .DEBBAY (H.). Action of Acids on Alloys .THUMMEL (K.). Behaviour of Mercuric Chloride with Hydrogen Ammo-nium Carbonate .BERG (A.). Chromiodates .NILSON (L . F.) and 0 . PETTERSON . Physical Constants of Germanium andTitanium and their Compounds .KEUSS (G.). Gold .DEBRAY (H.). Crystalline Alloys of Tin and the Platinum Metals .PAGE698698698698699699699699700700701702702702703703703704704705706706769770770770771771771771772772772773774774774774775775776777777778778$7877877977CONTENTS ...xu1PAGECHILO~STCHOFF . Precipitation of Mixtures of Iodates and Sulphates byBarium Salts .FILESENIUS (R.). Preparation of IIydrogen Sulphide free from Arsenic .JACOBSEN (0.). Purification of Hydrogen Sulphide from Hydrogen ArsenideFINE (R.). Affinity of certain Bivalent Metals for Sulphuric Acid .DACCOMO ((3.) and V . MEYER . Density of Nitric Oxide at -100’ .MENSCHING (J.) and V . MEYER . Behaviour of Phosphorus, Arsenic, and .HEMPEL (W.). Percentage of Oxygen in the Air .HARTOG (P . J.). Sulphites .Antimony a t a White HeatGEUTHER (A.). Arsenic .FOSSEE (W.). Carbonic Anhydride in the Air of School-rooms .GOTTIQ (C.). Crystallisation of Alkalis from Alcohol .PBEIS (C.) and B .RAYMAN .FISHER (J . H.).EBUSS (G.) and L . F . NILSON .Decomposition of Sodium Thioarsenate bySilver Nitrate .Corrosion of Zinc by Ammonium Chloride and PotassiumNitrate .Components of the Rare Earths yieldingAbsorption-spectra .DE BOISSIEU (P.). Water of CrystalliQation of Alums .CHRISTENSEN (0 . T.). Chemistry of Manganese and Fluorine .ROUSSEAU ((3.). Potassium Manganites .ENGEL . Hydrochloride of Ferric Chloride .SABATIER (P.). Hydrochloride of Ferric Chloride .FRANEE (B.). Action of Sulphuric Acid on Potassium Permanganate .OSMOND and WERTE . Residues obtained from Steel and Zinc by the Actionof Acids .GONZALEZ (C.). Paratungstates .HINSBERQ (0.). Zirconium .CARNOT (A.).Reactions of Vanadic Acid .DITTE (A.). Metallic Vanadates .DITTE (A.). Ammoniacal Vanadates .MATTHEY (E.). Metallurgy of Bismuth .DEBRAY (H.) . Products of the Action of Acids on Alloys of the PlatinumMetals .FABRE (C.). Selenium Alums .DES CLOIZRAU . Monoclinic Form and Optical Properties of ArseniousAnhydride .ELASON (P.). Action of Chlorine in Carbon Bisulphide and of Sulphur onCarbon Tetrachloride .FEANKE (B.) . Manganese Compounds .TROOST (L.) and L . OUVEAILD . Thorium Silicates .TBOOST (L.) and L . OUVBARD . Thorium Sodium and Zirconium SodiumPhosphates .HOFFMANN (L.) and G . KRUSS . Gold Sulphides .KEISEB (E . H.). Combustion of Weighed Amounts of Hydrogen : AtomicWeight of Oxygen .FISCHER (F.) .MICHAELIS (A.) .Tellurium Dichloride .FISCHER (H.). Working up of Stassfurt Potash Liquors containing a .SCHOTTLANDER (P.). Crystalline Form of Potassium Aurobromide .WARREN (H . N.). Phosphorised Silver .FRIPDHEIM (C) . “ Silver Suboxide ” .WELLS (H . L.). Basic Zinc and Cadmium Nitrates .WAEEMANN (A . J.) and H . L . WELLS .COUSTNS (A. C.). Relation of Mkrcury to other Metals .KLASON (P.) Carbon Oxysulphide .CAILNOT (A . > . Vanadates .KILUSS ((3.). Atomic Weight of Gold .Composition of Generator Gas and Water Gaslarge Excess of Sodium ChlorideBasic Lead Nitrates8848‘35 as5885885886887888888888889889889890892892a92a93894894894895896898900a96a999001014101510151015101610161017101810191019107810781078103910391079103910801080 ioaxiv CONTENTS .BOISBAUDRAN (L .DE) . Gallium .WARREN (T . T . P . B.) . Metallic ManganeseCompound of Manganese Sesquioxide with CupricOxide .MOORE (T.) Peculiar Formation in Nickel Regulus .WINKLER (C.). Germanium ..SCHNEIDER (E . A.).BETTEL (W.). Separation of Gold from the Platinum Met& .M;irteralogical Chemistry .BRAND (A.). Artificial Breithauptite from the Mecherniah Lead Furna,ce s .MACADAM (W . I.). Butyrellite .SCACCHI (E.). Minerals fr9m Vesuviua .BECKER (A.). Chemical Constitution of Barytocalcite and Alstonite .DES CLOIZEAUX (A.) and A . DAYOUR . Chemical Composition of HerderiteBUSATTI (L.). Minerals from Tuscany .MACKENZIE (G . S.). Rare Copper Minerals from Utah .DANA (E .S.). Columbite .CHROUSTSCBOFF (K . v.) . Plagioclase .DES CLOIZEAUX (A.) and F . PISANI . Oligoclase .HOCKAUF (J.). Botryogene .SPEZIA (Gt ) . Flexibility of Itacolumite .STRUVER (G.) Volcanic Fragments from the Lake of Bmcciano .NORDENSKIOLD (A . E.).DAUBR~E .DAMBREGIS (A . K.).Cosmical Powder from San Fernando, Chile .GURLT . Meteorite in a Tertiary Lignite .Note on a Meteorite in a Tertiary Lignite .HIDDEN (W . E.). Twin Crystals of Molybdenite .MEEM (J . G.). Limonite-pseudomorphs after Iron Pyrites .DANA (E . S.). Brookite from Magnet Cove, Arkansas .HIDDEN (W . E.). A Remarkable Crystal of Herderite .Analysis of Mineral Springs in Aegina and Andros .CLARKE (F . W.) and J . 8 . DILLER .PENFIELD (5 .L.) and F . L . SPERRY . Pseudomorphs of Garnet .HIDDEN (W . E.). Phenacite from Colorado .EIDDEK (W . E.) and A . DES CLOIZEAUX . North Carolha &finer81 Lo-calities .Turquoise from New Mexico .LEIGETON ((3 . W.). Mica from Leon Co., Texas .STROHECKER (J . R.). Ceriferous Hainstadt Clays .HUNTINQTON (0 . W.). Crystalline Structure of Iron Meteorites .HIDDEN (W . E.). New Meteorite Iron from Texas .KUNZ ((3 . F.). Meteoric Iron from Glorieta Mt., New MexicoDANA (E . S.) and S . L . PENFIELD . Two Hitherto Undescribed MeteoricStones .WANKLYN (J . A.). Occurrence of Free Iodine in a Mineral Water .ROMANIS (R.). Gold from Burmah .BOURGEOIS (L.). Crystallised Insoluble Carbonates .SANDBERGER (F.). Occurrence of Iodine in Phosphorites and of Lithium inPsilomelane .MEYER (A .B.). Nephrite from Alaska .BEUTELL (A.). Prehnite from Silesia .STEQER (V.). Porphyry from Horka in Prussia .DRASCHE (E.). Analyses of Persian Eruptive Rocks .SANDBERGER (F.). Investigations on Ore-veins .Recent Alluvial Deposits in the Ij and ZuyderZee .MEUNIER (S.). Mineral Waters from Java ..VAN BEYYELEN ( J . M.).SAUER [A.) . Amorphous Carbon (Graphito'id) in the Saxon Erzeebirm " V DANA (E . S.). Cryitallisation of NatiGe Copkr .BROWN (W . G.). Crystallographical Notes . 342PAGE108110811081108110811 W17171718191919202020212121222222231161161161161171171181181191191191191201202212212212222222232232232%22422434134CONTENTS .GENTH (A.) .Mineralogical Notes .LINDSTROY (G.). Copper Mineral from Sunnerskog. Sweden .CROSS (W . J.) and W . F . HILLEBBAND .PENFIELD (S . L.) and D . N . HARPER .DANA (E . S.). Mineralogical Notes .WEIBULL (M.). Galenobismuthite from the Falun Mine .HILLEBRAND (W . F.). Emmonsite. an Iron Telluride .NORDENSKIOLD (A . E.). Gearksutite from Ivigtut. Greenland .Chemical Comr>oaition of Ralstonite .Elpasolite. a New Mineral .LOSCH (A . k.). 'Brucite from the Ural . A .GORQEU (A.). Artificial Zincite and Willemite .PEARCE (R.). Goslarite from Montana .SJOQREN (A.). Place of Spodiosite in the Mineral System .SJOQREN (A.). Sarkinite, a New Manganese hsenate .IQELSTROM (L . J.). Polyarsenite .PENFIELD (5 .L.). Vanadinite from Arizona and New Mexico .HEADDEN (W . P.). Columbite from Colorado .LINDSTROM (G.). Phosphoric Anhydride in Felspar .CLARKE (F . W.). Lithia Micas .CHATARD (T . M.). Lucasite, a New Variety of Vermiculite .LACROIX (A.) . Lamellar Thomaonite .LACROIX (A.). White Epidote from the Beagle Canal, Terra del FuegoLACROIX (A.). Critical Examination of some Minerals .ARZRUNI (A.). Paragonite Schist from the Ural .ANSDELL (G.) and J . DEWAR .FRESENIUS (R.). Hot Springs a t Wiesbaden .STELZNER (A.) and A . SCHERTEL .HOLLAND (P.). Quartzite .EINCH fE.). Plattnerite .Gaseous Constituents of MeteoritesBlack Zinc Blende of FribergKINCH '(E.). F . H . BUTLER. and H . A . MIERS . New Vaziety of Dufrenitefrom Cornwall .MACADAM (W .I.). Talc used in Paper-making .PENPIELD (5 . L.), Phenacite from Colorado .SMITH (W . B.). Crystal Beds of Topaz Butte .ALLINQ (A . N.). Topaz from Thomas Range. Utah .JANNASCH (P.). Strontia in Heulandite .BISCHOP . Sodium Felspar from Krageroe. Norway .MALLET (J . W.). Silver in Cotopaxi Volcanic Ash .VOGDT (C . v.). Diabase-porphyrite from Petrosawodsk .EUNZ (a- . F.). Meteoric Iron from Augusta Co., VirginiaHUNTINGTON (0 . W.) . Coahuila Meteorites .MILES (F . P.). Supposed Meteorite from Highland Co., Virginia .the Spring a t Oued Ref .ROMBURGH (P . v.).MCIVOR (R . W . E.). New Zealand Graphite .BECKER (G . F.). Natural Solutions of Cinnabar. Gold, and AssociatedSulphides .FREMY . Artificial Formation of Rubies .FREYY and VERNEUIL .Action of Fluorides on Alumina .GORQEU (A.). Zinc Ferrite : Artificial Formation of Branklinite .LACROIX (A.). Plumbocalcite from Wenlock Head .OCHSENIUS (C.). Phosphoric Acid in Chili Saltpetre .DARAPSKY (L.). Chilian Alums .RATH (G v.). Cristobalite from Mexico .FUNARO (A.). Felspars from Elba .TSCH E RM AK (G.) . S capolite Series ..DE LESSEPS . Water from Artesian Well in the Tunisian Chotts and fromWater from the Wells of Zemzem ..DE CHBOUSTCHOFF (K.). Artificial Production of Quartz and k d y m i h .DE CHROUSTCHOFF (K.) . Artificial Production of Quartz and Orthoclme .HAUTEFEUILLE (P.) and L . P . DE SAINT.GILLES . Artificial Production ofMicas .XVPAGB342543343343344434434434534534534634634634634734734734734935035035035135135245 145145145145245245245345345345445445445545545545555565555655655755755855855955955956056056xvi CONTENTS .COHEN (E.).Talc. Pseudophite. and Muscovite from South Africa .DATHE (E.). Kersantite from Wustewaltersdorf. in Silesia .GOTZ (J.). Andalusite from Marabastad. Transvaal .JANNASCH (P.). New Analyses of Norwegian Rocks .KOTG (B.). Japanese Rocks .HIDDEN (W . E.). The Mazapil Meteoric Iron .KUNZ (G . F.). Meteorites from Kentucky and Mexico .ZUBER (R.). Eruptive Rocks from Krzeszowice. near Cracow .RICCIARDI (L.). Origin of Hydrogen Chloride, Sulphurous Anhydride. andIodine in the Gases of Volcanoes .KONIG (Gt .A.). Stromeyerite from Mexico .IGELSTROM (L . J.). Braunite from Jakobsberg. Wermland .JANNETTAZ (E.). Buratit. e from Laurium .ERBEN (B.). Bohemian Minerals .DEBY (J.). Cyprusite .IGELSTROM (L . J.). HEematostibite from Orebo .COSSA (A.). Columbite from Graveggia, Val Vigezzo .YOUNG (J.). Pectolite from Kilsyth .KONIG (G . A.).RNOP (A.). Biotite . Manganese-zinc Serpentine from Franklin, New JerseyKNOP (A.). Pseudobiotite .DAMOUR (A.). A Pink Clay .MEUNIER (S.).FREsENIus (H.). Analysis of the Schutzenhof Quelle, Wieibade6LosaNITscH (S . M.). Mineral Waters from Servia .BULITSCH (P.). Analysis of the Water of a Saline Lake .MEUNIEP (S.).GORGETJ (A.). Artificial Production of Magnetite .XACIVOR (R . W .E.).BUSATTI (L.). Wollastonite from Sardinia .BOSSCHA (J.). Meteorite of Karang-Modjo or Magetan in Java .WILLM (E.). Sulphuretted Waters of Olette .KALECINSZKY (A.). Native Gold from Thibet .HUSSAK (E.). Granular Limestone of Stainz, in Styria .WEIBULL (M.). Manganese Apatite : Composition of Apatite .STAHL (W.). Celestine in Nautilus aratus .BAUBIGNY (H.) . Artificial Bormation of Alabandine .BOURQEOIS (L.). Artificial Production of Crocoisite .FLINK (G.). Lingbanite .CHESTER (A . H.). Mineralogical Notes .WARTHA (V.). Minerals of the Serpentine-chlorite Group .SCHLTJTTIQ (E.). Imperfectly known Silicates .TEALL ( J . J . H.). Plagioclase from the Tynemouth Dyke .LE CHATELIER (H.). Action of Heat on Clays .LE CHATELIER (H.). Constitution of Clays .SCHOELLEB (R.).River-waters of La Plata .SANDBERGER (F.). Graphitefrom Ceylon .PULA (E.). Recent Formation of Marcasite a t Marienbad .SANDBERGER (F.).IGELSTROM (L . J.). Minerals from the Sjo Mine, Sweden .ZEPHAROVICH (V . v.). Pyroxene : Scheelite .ARZRUNI (A.). Dipyr from Connecticut .JANNASC EI (P.). Heulandlte .TRAUBE (H.). Laubanite : Laumontite .Meteoric Iron a t Fort Duncan, Texas .MACIVOR (R . W . E.). Bismutlzic Gold .SEMMONS (W.). Enargite from.Montana .Artificial Formation of Rose-spinel or Balas RubyMinerals occurring in Australian Bat GuanoCES~RO (G.). Destinezite .HEPBTJRN (Gt.). Griqualandite .Percylite, Caracolite, and Phosgenite from ChiliEIGEL (F.).LEDROIT (J . M.1 .. So.-called Trachvte-dolerites of the Voeelaberg .Trachytic Rocks from the Island of San Pietro .PAGE561562562662563564564564643643644644644645645645646646646647647cj; 476487077077077087087097097097107107809807817817817817827827834 8978578578690190 L902902902903903903909904643648Z8CONTENTS . xv iiCOHEP (IT.). Pallasite from Campo de Pucarii .ZEPHaRovrcH (v . v.). Trona. Idrialite. and Zinc Bloom .KOKSCHAROFF (N . J . v.). Turquoise from the Kirghis Steppes .ZGLENITZEIJ (W . K.). Epsomite from Poland .TEALL ( J . J . H.). Augite from the Whin Sill .TEALL ( J . J . H.). Andesine from Sutherlandshire .COLLINS ( J . H.). Minerals from Porthalla Core, Cornwall .LORY (C.).Microscopic Crystals of Albite in Calcareous Rocks of theRICCIARDI (L.). Composition of Volcanic Rocks .DAUBR~E . Meteorite a t Djati Pengilon, Java .LUZZATTO (E.) . Antimonite from Valdagno .DE LANDERO (C . F.) Tellurium Silver Bismuth from Jalisco, Mexico .LUEDECKE (0.). Minerals from the Stassfurt Salt Mines .PLUG+ (K . K.).PICCINI (A.). A Mineral associated with the Columbite of the VaiKNOP (A.). The Peridote of Schelinger Matten .KOTO (B.). Glaucophane .SCACCHI (E.). Altered Cordierite from Rocaa Tederighi in Tuscany .RICCIARDI (L.). Composition of Rocks and Minerals from Vulture and MelfiLUDWIG (E.) and G . TSCHERMAE . Meteorite from Angra dos Reis .Western Alps .Ignatieffite, a New Variety of AluminiteVigezzo .JOHNSTONE (W.). Flitwick Water .Organic Chemistry .HENRY (L.).Volatility of Methane-derivatives .BERTHELOT . Sugars .KLASON (P.). Sugar formed in the Inversion of Lichens .CONRAD (M.) and M . UUTHZEIT . Action of Dilute Acids on Grape-sugarand Fruit-sugar .CONRAD (M.) and M . GUTHZEIT . Decomposition of Milk-sugar by DiluteHydrochloric Acid .LANDWEHR (H . A.). Animal Gum .W o HL (A . ) . Thio f ormalde h y de-derivatives .MAGNAXINI (0.). Chloro-derivatives of Acetals .PECHXANN (H . v.) and K . WEHSARG .CECONOMIDES (L.). Ketines .BANNOW (A.). Pure Butyric Acid .MELIKOFP (P.). Derivatives of Tiglic Acid .MELIKOPP (P.). Constitution of C hlorohydroxybutyric Acid and Dichloro-butyric Acid .SAYTZEPP (A . C . and M.). Hydroxystearic Acids of Different Series .PEREIN (W .H., Jun.). Action of Trimethylene Bromide on Ethylaceto-PERKIN (W . H., Jun.), and P . C . E'EEER . Ethylacetotrimethplenecarboxg-late .CUBTIUS (T.) and I? . KOCH . Derivatives of Diazosuccinic Acid .JACOBSEN (0.).WALLACH (0.). Carbohydrates .Di-isonitroPoacetoneacetate, Benzoylacetate, and Acetone Dicarboxglate .DRNARO (A.) . Dichloropyromucic Acid .WIDMAN (0.). Constitution of Glycoluril .ERREBA ((3.). Chloropropylbenzene .MAYER (I?.). Reduction of Trinitro-+-cumene .JAWBSEN (0.). Hemellithene .Hydrocarbons from Tar Oils boiling between 170" and 200"FILETI (M.) . Reciprocal Transformation of Cymene and Cumene-deri-vativeu .FILETI (M.) and F . CROSA . Chlorocymene and Bromocymene from ThymolJACOBSEN (0.).Ethylxylenes .VOL . LII . bPAGE904102110211021102210221022102310231024108410841085108510851086108610861087lo871087242425252626262728282929293030323333343443535363636373xviii OONTENTS .BENDER (Gt ..) . Ethereal Carbonates .B~EDERMANN (J.). Parahydroxybenzil Alcohol .KOSTAXECEI (S . v.). Synthesis of Betorcinol @-Orcinol) .CURTIUS (T) and (3 . LEDEBER . Benzylamine . CAUSSE . Acetal-resorcinol .GILL (J . M.). Citric Acid Derivatives of Paratoluidine . - .WALLACH (0.). Azo- and Diazo-eompounde .SUTKOWSEI (J.). Quinone-oximes .LOEB (M.). Amidine-derivatives .REIMARUS (0.). Action of Alkyl Iodides on Dibenzilthiocarbamide .STOLTE (H.) .Phenylseleniocarbimide and Diphenylse~eniocarbamid~ .BENDER ((3.). Substituted Nitroeen Chlorides .FILETI (M.). Preparation of Aromatic Amides .TSCHACHER '(0.). Condensation Gf Nitrobenzaldehyde with Hydrocarbons .HOFFMANN (A.). Compound of Pyrotartaric Acid with Hippuric Acid .ERLENMEYER (E ) and J . ROSENHEE . Phenyliodohydracrylio Acid .WENDE (H.). Cyesolcarboxylic Acid .L~EBERMANN (C.). Opianio Acid Derivatives .LIEPERXANN (C.) and S . KLEEMANN . Opianic Acid Derivatives .G R ~ N E (H.). Azo-opianic Acid .ELBEL (K.). Derivatives of Normethylnitro-opianic Acid .GABRIEL (S.). Homo-orthophthalamide .E~ERTENS (E.). Action of Amines on Shthalylacetic Acid .FILETI (M.). Bronioterephthalic Acid .SCHNAPAUFF (E.). Cumidic Acids .ERRERA ((3.).Reaction of Stilbene .ZINCKE (l'.). P-Naphthaquinone .ZINCKE (T.) and F . RATHQEN .. Benzene- and Toluene-azonaphthols andtheir Isomeric Hydrazine Derivatives .JULIUS (P.). New Diamidodinaphthyl .NOAH (E.) . Tetrahydroxyanthraquinones .CAHN (E . L.) . Methylanthragallols .CANNIZZARO (5.) and Gt . FABRIa . Acid from SanLonin : IsophotosantonicAcid .HESSE (0.). 'Cinchol .CONTNCK (0 . DE) . Alkaloyds .CIAMICIAN (G . L.) and M . DRNNSTEDT . Extraction of Pyrroline fromAnimal Oil .LADENBURG (A.). Ppidine Bases .CLAUS (A.) and F . COLLTSCHONN, Quinoliae .GABRIEL (S.). Isoquinolinsand its Derivatives .LIPPMANN (E.) aud F . FLEIGSNER . Synthesis of HydroryquinolinecarboxylicAcid .LADENBERG ( A.). Piperidhe Bases .LTPSKI (A .A ) . Comparative Estimation of Preparations of Pepsin .REMSEN (T.) and H . W . HILLYER . Methods for Determining the RelativeFISCHER (0.j and H . VAN Loo . Formation of P-Diquinoline .PODWYSSOZKI (W.). Method of Preparing Extrects of Pepsin .Stability of Alkgl Bromides .MANSFELD (W.). Derivatives of Diethylene Disulphide .ESCALES (R .) and E . BAUMANN . DisulphonesBAUMANN (E.). Disulphones .LANDWEHR (H . A ) . Reagent for the Hydroxyl-groupSCEWALB (F.) . Non-acid Constituents of Reeswax .HARVEY (S.) .HSRKIQ (M.) and S . SCHUTBERT . Carbohydrates .PETERS (K.). Linoleic Acid ...Conversion of Starch into Glucose by means of HydrochloricAcid .LADENBURG (A.) . Identity of Cadaverine with Pentamethylenediamirie .BAUMANN (E.).Compounds of Aldehydes and Ketones with Mercaptan .PAQEsa383944344404x34142$24343444.44445454!54748;49506152525353546666.5757585859596061636364r656612212212332312412412512512512612OONTENTS.BXEDT (J.). Acetyl-levulinio Acid : ConstituticHlr af pXetonic Acide .COXBES (A.). New aertction of Alumihm Chloride : Bpthesee in &Acetic Series ..VO~PEBT (F.). Gluconic Acids - .LIST (R). Actidn of Thi-kdeon' Ethil Aeelioaoehte .K~HLEE (A.) . Nitro-derivatives of Methylmil .B~PHRE~TD (R). l?ormation.of Dibromo- and Dichloro-kbiDc Acib .WER (V.)* Relation of a-Thiophsmc Acid t;o the Nomad Thiophnear-boxylic Acids .WILM~ERODT (C.). H&gm 0arriel.e .WALLACH (0.).Preparation of Organic FhddeaBAMBEILGER.(E.). Reaction of Potsssim Cyanide wik &&&xy'EEChloride .$BEERSON (W. H.). Oidatdn oS'Ni&itylene .WEDMAX (0,). Intramolecrmlas Chsngee in the Pmpyl-gmapob the CumeneSeEies . , .W ~ M A N (Or). Reciprocal Transformations of Cymene- and .Cumenederiva-tivea . , .FHTICA (F.). A Fourth Monobromophenol and a &mnd Monobrmoben-NISTZKI (R.j. Cknstiktion of N'itranilic Acid . (LJ. Aniline and its Homnlogues .CLAUS (A.) and H. HIBZBL. Alkyl-derivatives of Aniline .~ X D M E Y E R (T.). Action of Ethyl Imidoombonate on Armmtio dythdcompounds .. -.BIEMSEBT (I.) and A. Gt. PALMER, Decomposition of -0-ompounds byAlcohol: Pmdiazotolueneorthos?.zlthoaic Acid .~ R N B (F.).Ocklbenzene . - . c *zene -. * .WXLLACH (0.). Diazo- and Diamamid6-compounde .&WERE (E.). Hydrasines .Bwmw (C.). Phenyi3~ydrezine-compollnds .BUDIN (J. A.). Dicyrulphenylhy~~ne-compoPnds .&tkNTHSEN (A.) and H. SCE.ppre2TZZle'R. PhenaAd&atives .B~~NTHSEN (A). Conetitution of the S W n e a .W X N E ~ (A.). Metanitromethylsa~cylaldehyde and its Derivataves .EREKEUUB (E.). Action of Sulphuric Acid on h m s t i c Kkones .J~LENLTEYEB (E 9, juu. Pliichl'e Phenylglycidio Acid ..EXPP (A.). Para- and Ortho-nitrophenylosyacrylic Aeid .HENTSCHBL (W.). Derivatives of' Metkl C'8laadilate + .USEX (I.) and A. Gt, PALMER. Benaoic &lphihide .Ilar#as~~ I.) and A. Gd PALMEB. Pamthorybenzoic BdpWde .-SEN {I.) and W. 5. BAYLEY.Yambromobemic 8dphinide.~WJTIEB (EL.). Chlorine-derivativea of Acetophenme .-HAS (R.). dmido-auids .m o w (C.) - Ethylphthdylacetoaetate .BWSEBT (I.) and C. S. PALXBR. Benzo~1taluenesulphcun;lmide .SCHNEE~VSS (E, A). Sepmtion of the two Leomeric 'Ibluidinesul-phunicAcids .&OPNEIDEE 6. A$ A&m-if Sulph&c A& on kph!kwtoluenesulphoni~Acids .~ E ~ ~ s E N (1.j and W. H. EMEBSON. Oxidation by mmnu of PcitasaiumPermanganate .KELBE (W.) and N. v. CZAZLNOMSZL Aebion of Bromine and Water ona-Metaisocymenesulphonic Acid : Constitution of u+ and @-Metaim-FIsCHEB (E ). Syathesie af Indde-de&&vm .BMXEB (E,). Indolee from Phenylhydraaine .WER (A.). Indolbs from Medydmzinebenzoic Acid .oymeneeulphonic Acids .WEN (J.). Indoles from Meth lphenylhydrsaine .mCHUTZ (B.).blumini\l91~BlQlide&&C&a .5 2XiXPAQB1261WI*lzf128129129130130131 iae18%1301381341841341841%136 .137138. 138 . 189 . 139 . 146 . 141 . 141 . 142 . $la . 14% . 143 . 144 . 1 4 . 144 . 1% . 145i38,lM1461-43146147148144314914915xx JONTENTS .LIPPMANN (E.). Dehydrogenation by means of Benzoic Peroxide .ELBS (K.). Formation of Substituted Stilbenes .EI. BS (K.) and F . BAUER . Substituted Stilbenes .GRAEBE (C.) and A . PEER . Euxanthone-group .MELDOLA (R.) . Preparation of Dinitronaphthylamine : Metanitrophenyl-azodimethylamidobenzene .WITT (0 . N.). Eurhodines and Laurent’s Naphthase .SCHLIEPER (A.). Indoles from P-Naphthylhydrazine .HECHT (H.).Action of Monamines on Citric Acid .STOKES (H . W.I and H . T . PECHMANN . Action of Ammonia 011 Ethvl Acetone-dicLrboxyiate . Synthesis of Pyridine-derivatives . :LADENBURG (A.) and C . F . ROTH .SEYFFERTH (E.). Derivatives of Picolinic and Nicotinic Acids *CLAUS (A.) and F . COLLISCHONN . Bromoquinoline .XNORR (I,.). Synthetical Experiments with Ethyl Acetoacetate .SKRAUP ( Z . H.) and P . BRUNNER . Metaquinolinecarboxylic AcidLADENBURG (A). Synthesis of Active Conine .LIEBRECHT (A.). Reductionof Nicotine .BAMBERGER (E.) . Sparteine .H ES BE (0.). Pseudomorphine .GOLDSCHYIEDT ((3.). Papaverine .JAHODA (R.). Papaverine Salts .SKRAUP ( Z . H.). Constitution of Cinchonine .LADENBURG (A.). Specific Rotatory Power of Yiperidine Bases .MERLING ((3.).Action of Bromine on Dimethylpiperidine .BIKFALVI (K.). HEmin Crystals .LINTNER (C . J.). Diastase .MUELLER (H.). Action of Diastase and Invertin .LE BEL (J . A.). Russian Petroleum .Bases from Animal Oil .NORTON (L . M.) and A . A . NOPES .OTTO (R.) and A . ROSSING .LINDET (L.).ROMBURGH (P . v.).Action of Heat on Ethylene .Reaction of Organic Bisulphides with Potas-sium Sulphide .Action of Alcohols on Aurophosphorous Chloride .Dextrorotatory Hexylic Alcohol .Formation and Composition of HumousSubstances ..Action of Hydrogen Chloride on Mixtures ofMEYRR (V.). Thiodiglycol Compounds .BAUMANN (E.). Preparation ofBenzoic Ethers .KILIANI (H.). Arabinose .Aldehyde with Alcohols .MIXTER (W .(3.). Acid Propionates and Butyrates .MEYER (V.). Preparation of /3-Iodopropionic Acids .ROMBIJRGH (P . v.). Methylisopropylacetic Acid .REIMER (C . L.) and W . WILL .methylenecarboxylate with Lime .OST (H.) and A . MENTE . Oxalimide .WISLICENUS (W.). Ethyl Oxalacetate .THIERFELDER (H.) . Glycuronic Acid .WATTS (F.). Fermentation of Citric Acid .Decomposition of h i d e s by Water and DiluteAcids .BRUNSWIGF (H.). Derivatives of Acetothienone .DAMSKY (A.). Isomerism of the Thiophenic Acids : Derivatires of P-Thio-phenic Acid .ERNST (F.). Reduction of aa-Thiophendicarboxylic Acid .CONRAD (M.) and M . GUTHZEIT .ROMBURGH (P . T.).CLAUS (A.) and E . TRAINER . Decomposition by Heat of the Nitrates of AminesErucic and Brassic Acids .COLMAN (H .G.) and W . H . PERKIN, Jun . Distillation of Calcium Tetra-BERTHELOT and ANDRB .EENST iF.\. Svnthetical Investica6ons in the ThioDhen Series .PAUE15115115115215215315315415515715715815916016016116216316316416416416416516516622523622622722822822822922923023123123223223323423423423523523523623’1237238KUES (iV.j and‘C . PAAL . SynthYesis of a-Phenylthiiphen . 23CONTENTS . xxiKPEKELEB (K.). Pentathiophen-group .CIAMICIAN (G.) and P . SILBER . Action of Light on Nitrobenzene .CuUs (A.) and E . PIESZCEK . Orthoethpltoluene .HEYMANN (€3.) and W . KOaras .BLAU (F.). Action of Sodium Methoxide 011 Bromobenzene .OTTO (R.) and A .ROSSING .JACKSON (C . L.) and A . M . COMEY . Action of Silicon Fluoride on OrganicBases .MERZ (V.) and P . MULLER .FISCHER (0.) and E . HEPP . Action of Alcoholic Hydrogen Chloride onNit*rosamines .HOOGEWERFZ (S.) and ,W . A . VAN DORP . Benzylamine and Phenethyl-amine .ROWBURGH (P . v.). Isodinitrodimethylaniline .BERNTHSEN (A.). New Synthesis of Thiodiphenylamine .BENDER (G.). Ethereal Carbonates .WALDER (F.). Benzyl-derivatives of H-$.roxylamine .KNORR (JJ.). Correction .WITT (0 . N.), Action of Ethyl Acetoacetate on Aroniatic Diamines .DAHM (C.) and K . GASIOROWSKI . Condensation Products from Carbo-imides and Orthodiamines .MENTHA (E.) and K . HEUMANN . Parachlorazobenzene-derivatives .MENTHA (E.) arid K . HEUMANN . Cyanazobenzene and Yarazobenzenecar-Oxidation of Homologues of Phenol .Bisulphides with Mixed Organic RadirlesAniline and Diphenylamine from Phenol .boxylic Acid .MENTHA (E.).Chloroparazotoluene .GOLDSCHMIDT (H.). Reduction of Aldoximes and Acetoximes .BERNTHSEN (A.). Pyrogeniu Formation of Phenazine .NIETZKI (R.). Safranine Dyes .WITT (0 . N.). Constitution of the Safraninee .NIETZKI (R.). Constitution of Ssfranine .OSBORN (T . B.) and W . C- . MIXTER . Paranitroformanilide ..Action of Concentrated Sulphuric Acid on Aromatic Eetones .MATTHIESSEN (C . H.) and W . G . MIXTER .DYER (J . 0.) and W . G . MIXTER .CLATJS (A.).OrthazoparabromacetanilideHalogen-derivative of Oxanilide .PAMPEL (0.) and G . SCHMIDT . Aromatic Ketones .ERAFFT (F.).Benzene-derivatives of High Molecular Weight .CLAUS (A.) and E . FICKERT . Paraxylyl Ethyl Ketone .NEUMANN (G.). Nitrophenyl Benzoates and Nitrobenzoates .Hydrocarbons .PL~CHL (J.). Phenylglycidio Acid .NEP (J . U.). Benzoquinonecarboxylic Acids .LIEBERMANN (C.). Constitution of Azo-opianic Acid .LIEBERMANN (C.). An Isomeride of Hemipinimide .ELKAN (T.). Isomeric Aldehydophenoxyacetic Acids .ELKAN (T.). Vanillinoxyacetic Acid .GERSON (G.). Derivat.ives of Pyruvic Acid .EUES (W.) and C . PAAL . Diketonic Acids .HANTZSCH (A.). Furfurane-derivatives from Resorcinol .OTTO (R.) and A . ROSSING . Sulphobenzidedisulphonic Acid .VALLIN (K.) . Metatoluenesulphonic Acid .ELASON (P.). Toluenedisulphonic Acids .LELLMANN (E.) and 0 .BONHOFFER . Introduction of Lhrboxyl into AromaticLANG (E.). Action of Zinc Alkyl Compounds on Ethyl Malonate .LANG (E.). Furfurane-derivatives from Phloroglucinol .OTTO (R.) and E . ENGELHARDT . Phenylsulphinacetic Acid .CLAUS (A) and J . A . SCHTJLTE IM HOF .FISCHER (E.) .Cumene-orthosulphonic Acid andOrthocumic Acid .Action of Aldehydes, Anhydrides, and Diazo-compounds onthe three Methylindoles .BEINITZEB (F.), Hydrocarrotene and Carrotene .PAGE2392442402412422422432432442452452452452%24724724724721825824924924925025025025125125125225225325425425425525725825926026126126226226326326326425826426526x xii CONTENTSPAGEEEMILTAX m.). Diphepylmetaxylylmethaneand Diphenylorfho-xyly~methane 266CLATJS (A.) and M .ERLER . 268CLAUS (A.) and 0 . SCHMIDT . @-Naphthol-@-disulphonic Acid . 269CLAISEN (L.). Action of Aldehydes on Phenols . 270CLAVS .( A.) and P . FEIST . a-Naphthyl Methyl Ketone . 271BAMBERGER (E.) and M . PHILIP . Pyrene . 271PESCI and BETTELLI . Terebenthene-derivatives . 272KOSTANECEI (S . v.). Bormation of Euxanthic Acid . 272CIAMICIAN (G.) and P . SILBER . Synthesis of Ygrroline . 273CIAMICIAN (G.). Behrlviour of Methyl Ketole : Conetitution of P.yrroline . 273PAAL (C.) and C . w . T . SCBNEIDER . 2'73EITORR (L.). Syntheses by Means of Ethyl Acetoacetate . 275KEISER (E . H.). 272LIPP (A.). Tetrahydropiwline . 277CLAUS (A.) and P . KUTTNEP . Quinolinesulphonic Acids .278XNORR ~~ . (L.) and C . KLOTZ .. 2'78BENDER (F.) and G . SCQTJLTZ . Diamidostilbene . 268Bromo-derivatives of Diphenic Acid .PEREIN (A . G.) and W . H . PERPIN, Jun . Kamda . 272Synthesis of Pyrroline derivati~esAction of Chlorine on Pyridine .Reduction of HgdrosylepiYdine and Mothyl-lepidone .;REHER (L.). a- and y-Ethyl Quinolines .BRUCKE (E. v.). Colour Reaction of Guanine .PLUGQE (P . C.). Opium Alkalo'ids .COMSTOCE (W . J.) and W . KOENIGS . Cinchona Alkalo'ids .LOEBISCH (W . F.) and P . SCHOOP . Strychnine .LADENBURG (A.). Specific Rotation of Pigeridine Bases .HESSE (0.). Alkaloids of the Berberidese .BRIEGER (L.). A New Ptoma'ise producing Tetanus .NEUMEISTER (R.). AJbumoses .NETJMBISTER (R.). Vitelloses .GRIMAUX (E.) and C .CLOEZ . Erythrene-derivatives .BARATAEFF (S.) and A . SAYTZEFF . Trimethyl Carbinol .USTINBFF (D.) and A . SAYTZEFF . Dipropyl Carbinol .DIEFF (W.). Action of Silver Acetate on Tetrabromodiellyl Cstrbiuol .CUISINIER ( L . ) . Glucose and the SWc harification of Starch .BOCRQTJELOT (E.). Action of Saliva on Starch .BOURQUELOT (E.). Starch Granules .MAQTJENNE . Inosite .MALBOT (H.). Preparation of Tsobutylamiaes .MALBOT (8.). Senaration of Mono- and Di-isobutylamines .ZEISEL (5.). Colchicipe .MERCK (C . E.). EcgQnine .Co~sop (A.). Erythrol .. 279 . 280 . 280 . 281 . 282 . 282 . 283 . 204. 284 . 284. 286 . 352 . 353 . 353 . 353. 354 . 354 . 355 . 355. 356 . 357 . 357. 285. 8%BAMBERQER'(E.). Synthesis of Guanylcarbarnide .GATTERMANN (L.) and Gt .SCHMIDT . Preparation of AlkylamidoformicMICHAEL (A.) . Convenient Method of Preparing Brominated Fatty Acids .MICHAEL (A.). Behaxiour of Acetic Acid and its Derivatives to PhosphorusPentachloride .Chlorides and Alkyl Isocvanates .USTINOFF (D.). p-Dimethacrylic Acid .HAZTJRA (K.). Acids from Drying Oils .BARATAEFF (S.). Methoxydidylacetic Acid .FLICEHINGER (EL) . Oxalic Acid from the Residue of S@ritlss atherisIVitrosi .SCHATZEY (E.). Preparation of Ethyl Acetate .DAIMLER (C.). Action of Ethyl lodide and Zinc on Ethyl Malonate .BARATAEFF (S.). Action of Ally1 and Ethyl Iodides on Ethyl OsaIate .FITTIG (R.) and C . DAIMLER . Action of Ethyl Chloracetete a i d Zinc onEthyl Oxalate .ROME& (M.).Nitration of a-Tbiophenic Acid .SCHATZEY (E.) . Diallyloxalic Acid .35835835935935935936036036036136136136CONl’EN ‘1’S xxiiiBAEYEB (A.) . Constitution . of Benzene .LADENBURG (A) . Constitution of Benzene .SEPLIG [E.). Chlorination of Toluene .GOLDSCHMIDT (H.) and M . HONIQ . Nitrochlorotolueiie and ClilorotoluidineTHOMSEN (J.). Constitution of Benzene .KLABON (P.). Synthesis of Cyanphenin .MEYEE (E . v.) . Synthesis of Cyanphenin .BAESSLER (A.). ‘&in01 and its Derivatives .MICHAELIS (A.) and F . SCHMIDT . Isomeric Mono- and Di-benzoylphenyl-h ydrazines .BILLETEP (0.) aud A . STEINEB . Thiocarbimides of Bibasic AromaticRadicles .MICHAELIS (A.) and L . WEITZ . Trianisylarsine and its Derivatives .MICHAELIS (A.).Organo-bismuth Compounda .MICHAELIS (A.) and A . POLIS . Triphenylbismuthine and its Derivatives .S~EULZE (E.) and E . N h m r . Phenylamidopropionic Acid obtained fromQ~IBAUD (H.). Physical Peculimity of Triphenylguanidine .HOTTER (E.). Synthesis of Phenylaceturic Aoid .the Decomposition of Prote’ids .BAEYER (A.). Reduction of the Phthalic Acids .Action of Potassium Hydroxide on MixedAlkyl Bisulpliides .Action of Sulphurous AnhydrideonJ3enzene . * .Action of Potassium Hydroxide on Phenylene-MUNCHYEYE? (F.). Action of Hydroxylamine on Diketones .EKSTBAND (A . Gt.). Naphthoic Acids .RICHTER (E.). a- and /3-Naphthenylamidoxime .CLEVE (P . T.). Chloronaphthdenesalphonic Acids .FOBSLIKG (S.). Bronner’s j3-Naphthylaminesulphonic Acid .O T ~ O (JL) and A .ROSSING .COLBY (C . E.) and C . 5 . MCLOUBHLIN .OTTO (8.) and A . ROSSINQ .mefadiphenylwlphone .GOSKE (A.). Bynthesis of Carbazole .SOLTSIEN (P.). Essential Oils .HALLER (A.). Isomeric Camphols and Oamphora .LEUCKART (R.). Carveol, Borneol, and Menthol .LETJCKAPT (R.) and E . BACH . Bornylamine .GEAM (C.). Active Principles of Asckpias currmsavica, A . incarnata, andCIAMICIAN (Gt.) and P . SILBEP . Conversion of Pyrroline ink0 Pyridine-derivatives .ALTAR (S.). Oxidation ot Symmetrical Triallylpyridines .LA COSTE (W.) and F . J7ALEUR . Quinoliiiedisulphonic Acid and its Derira-tives .HOFMANN (A . W.). Quinoline-red .CLEVE ( P . T.). Compound of Qninoline with Formamide .PANAJOTOW ((3.). 1 : 3 Dimethylquinnldinc .HINSBERG (0.).Nomenclature of the Quinoxaline Series .LETJCKART (R.) and A . HEI~RMA” . Nitrotolylglycine and Oxydihydrotolu-Yilzcetoxicum ofleinalis .LIWEH (T.). 2 : 6 Dimethylpyridine Platinochloride .quinoxaline .LIWEH (T.). Conyrine Platinochloride .FREUND (M.) and W . WILL . Hydrastine .BECKUXTS (H.). Ptomaines .GRAM (C.). Origin of Ptoma‘ines .LOEW (0.). Diastase .EKGLER (V.) and iM . BOEAM . Veaelin .MAGNAMINI ((3.). Piperilene .PISANELLO (Gt.). Hydrogenation of Propionitrile .WALLACH (0.) and F . LEHMANN . Atation of Phosphorus Pentachloride onSubstituted Pormamides and on Piperidine-derivatives .PAGE3623623623623633633633643653663663678683683683693703713713723123733733743743753753753763763773783783783’79380381381382383383883384385387.38745645745xxiv CONTENTS .BERTONI ((3.).Ethereal Salts of Nitrous Acid .POMEY (E.). Compound of Propyl Alcohol and Phosphopletinous Chloride .LOEW (0.). Formose .SELIWANOFF (T.). Reaction for Fruit-sugar .MACQUENNE . Inosite .HORVAT (V.). Dry Distillation of Starch with Lime .MAYER (A.). Nature of Niigeli’s Starch.cellu1ose .SCHULZE (E.) and E . STEIGER . Paragalactin .LANGELI (T.) . Trimethylpropylammonium Iodide and Hydroxide .MALBOT (H.) . Salts of Di-isobutylamine .BARBAGLIA (Gt . A.). Isobutaldehyde and its Polymerides .BARBAGLIA (G . A.). Action of Sulphur on Aldehydes .FASBENDER (H.). Compounds of Aldehydes and Ketones with Mercaptan .CLAISEN (L.).Action of Nitrous Acid in Ketones .AUTENRIETH (W.). Dimethylene Disulphone-derivatives .TAFEL (J.). y-Amidovaleric Acid .STADELMANN (E.). Hydroxybutyric Acid in Diabetic Urine .WOLFF (L.). p-Bromovderic Acid .KILIANI (H.). Axabinosecarboxylic Aoid and Arabinoee .FRANCHIMONT (A . P . N.). Action of Nitric Acid on Bibasic Acids .BE RGREEN (H.). Isonitroso-compounds .BURTON (B . S.) and H . v . PECHMANN . Action of Phosphoric Chloride onEthyl Acetonedicarboxylate .HENTSCHEL (W.). Aconitic Acid .TAFEL (J.). Reduction of Dihydroxytartaric Acid Diphenylhydrazide .BGUTROUX (L.). Gluconic Acid .MICHAEL (A.). Constitution of Trimethylenetricarboxylic Acid .FRANCHIMONT (A . P . N.) and E . A .KLOBBIE . Amides of EthylsulphonicAcid .DEL~PIN (S.). Calcium Urate .HILL (H . B.) and L . L . JACKSON . Chloropyromucic Acid .CANZONERI (F.) and V . OLIVERI . Transformation of Furfuran mtoPyrroline .TAFEL (J.). Furfurylamine .LEKO (M . T.). Thioplien in Aniline .EXNST (F.). Reduction of a-Thiophenic Acid .SCHULZE (K . E.). Constituents of Coal-tar .FILETI (M.). Reciprocal Transformation of Cumene and Cymene .PERATONER (A.). Oxidation of the Methyl Ethers of Mono- and Di-brom-orthoisopropylphenols .PONEY (E.) . Compound of Orthotoluidine with Cupric Chloride .POMEY (E.). Compound of Paratoluidine with Cupric Chloride .NIETZKI (R.) and F . KEHRMANN . TBUHL~R (J.) . Thioparatoluidine .SCHOOP (P.). Preparation of Dimethylaniline .HEIDLBERG (T.).Ortho- and Para-chlorodimethylaniline .GOLDSCHMIDT (H.) and E . EISSER . Carvole-derivatives .HINSBERG (0.). Action of Orthotoluylenediamine on Dextrose .Secondary and Tertiary Qninones .QRIESS (P.) and G . HARROW .NIETZKI (R.) and E . HAGENBACH . Tetramidobenzene and its Derivatives .CHETMICKI (’3 . v.) . Carbonylorthamidophenol and Thiocarborthamido-phenol .KLASON (P.). Substitution of Amidogen by Hydrothionyl and Oxjsul-JANOVSKP (J . V.) and L . ERB . Halogen-derivatives of Azobenzene andJANOVSKY (J . V.) and L . ERB . Direct Substitution-products of Parazo-ENGLER (C.) and C . SCIIESTOPAL . Action of Acetone on Pnramidoazoben-zene .Action of Aromatic Iliamines on Sugarsphuryl Groups .Hydrazobenzene .toluene : Hydrazobromvbenzenes : Hydrazobromotoluenes .PAGE4684684694594594604604604614614614624624634634634644644654664664674674674684684684694694704’7047147147147 147247 24724’7247347447447547547647647747847847947CONTENTS .HEUMANN (K.) and L .(ECONOMIDES . Action of Phenol on Diazoamidoben-zene .BERNTHSEN (A.). Constitution of the Safranines .M~~HLHAUSER (0.). Manufacture of Methylene-blue .LEVI (L . E.). Thiophen-green .MICHAEL (A.) . Action of Phosphorus Pentachloride on Acetanilide .MUNCHMEPER (F.) . Action of Hydroxylamine and Phenylhydrazine onDialdehydes and Ketones .LANDSBERG *(L.). Preparation of Vanillin .BUCHKA (K.) and P . H . IRISH . Action of Potassium Ferricyanide on Aceto-phenone .BROMME (W.).Metacyanobenzoic Acid .BROMME (W.).GRIESS (P.). Meta- and Para-hydroxynitrobenzoic Acids .DIEHL (L.) and A . EINHOBN . Derivatives of OrthamidophenylvalerkAcid .PERATONER (A.). Substituted Mono- and Di-bromosalicylic Acids .PERATONER (A.). Constitution of Dibromosalicylic Acid .BUCHKA (K.). Formation of Phenylglyoxylic Acid from Benzoic Cyanide .VALENTINI (A.). Methyl ?VIethyldibromoparacoumarate .REQEL ((2.). Oxidation of a- and P-Hydroxypiperic Acids .MOIN~ (F.). Action of Bibasic Acids on Thiocarbltmide .WISLICENUS (W.). Action of Phenylhydrazine on Lactones .LELLMANN (E.) and C . SCHLEICH . Nitrobenzyl-derivatives of Ethyl Malo-nate .PIUTTI (A.). Synthesis of Ethereal Salts of Trimesic Acid .KLASON (P.) .Toluenedisulphonic Acids .GOLDSCRMIDT (H.) and N . POLONOWSKA . Diphenylhydroxyrthglamine .MASON (A . T.). Condensation-derivatives of Ethjlendiamine .CLAISEN (L.). Condensation of Aldehydes with Phenols and AromaticAmines .CLEVE ( P . T.). Action of Cblorine on Acet-a-naphthalide .SPTCA (M.). Naphthoxyacetic Acids .BAMBERGER (E.) and M . PHILIP .BAMBERGER (E.) and M . PHILIP . Pyrene .GOLDSCHMIDT (H.). Camyhoroxime-derivatives .WILL (W.). Naringin .EIJKMAN (J . F.). Substances from Illiciurn Teligiosum .DE ZAAIJER (H . G.). Andromedotoxim .JAWEIN (L.). Crystalline Compound from Kamala .HURST (G . H.). Algaborilla .KULZ (E.). Indian-yellow and Glycuronic Acid .LADENBURG (A.) . Yjrrolidine .DURKOPF (E.).Preparation of Pyridine Basw .LUNGE (G.) and J . ROSENBERG . Coal-tar Lutidines .CANZONEBI (F.) and G . SPICA . Ethoxglutidine .CONEAD (M.) and M . GUTHZEIT . Action of Ammonia and Primary Amineson EthylDimethylpyronedicarboxylate .CONRAD (M.) and W . EPSTEIN . Lutidine-derivatives from Lutidonecar-boxylic Acid .COLLIE (N.). Condensation-product of Ethyl Amidoacetoacetate with Hydro-chloric Acid .CONRAD (M.) and M . GUTHZEIT . Ethyl Dimethylpyronedicarboxylate .LELLMANN (E.) and H . ALT . Quinolhe .TORTELLI (M.). Synthesis of Metaquinolinecarboxylic Acid .DOEBNER (0.). a-Alkylcinchonic Acids .HOOGEWERFF (S.) and W . A . VAN DORP . Isoquinoline and its Derive-tives .DOTT (D . B.). Acid Morphine Acetate .Behaviour of Cyanobenzoic Acids on Dry Distillation .Acenaphthene and Naplithalic AcidXSVPAGE480480480481481482483483484484485485486487487488488489489490491491492493494494495495496496497497497498498498499499499499500501501502502503504505505HANSENN (A.).Constitufiion of Brucine . 50XXVi CONTENTS .EIJKMANN (J . F.). Hpdrastine .ANTRICK (0.). Optical Behaviour of Coca'ine .KOSTIEILINA (S.). Action of Pepsin on AmyloYd .MARTIN (8 I-I . C.). Vegetable Globulins .RENARD (A.). Action of Heat on Heptine .BENDER ((3.). Bismuth Thiocyanate .SMOLKA (A.). Action of Potassium Permanganate on Dextrose in NeutralSolution .FISCHER (E.). Compounds of Phenplhydrazine with Sugars .MAUMEN~ (E.}.Action of Nitric Acid on Sugar .MYLIUS (F.L Iodide of Starch .GOLDSCPMIPT (H.). Reduction of Aldoximes and Acetoximes .SANDMEYER (T.). Action of Nitrous Acid on Acetone .ENGEL (R.). Corrdensation of Acetone and Chloroform .GATTERMANN (L.) and G . SCHMIDT . Chloroformamide : Synthesie of Aro-matic Acids .WILLGERODT (C.) and F . DURR . Tertiary Trichlorbutil Choride andEther .MABERY (C . F.). Substituted Acrylic and Propionic Acids .GLADYSZ (T.) . Preparation of Calcium and Potnssium Tartrates .HCHIFF .(H.) .. FQrfuraldehyde .METER (V.). Negative Nature of the Phenyl-group .FERKO (P.). Pyrogenic Reactions .POLIS (A.). Aromatic Lead Compounds .NEUMAPN (G . S.). Sylphuric Acid as an 1odine.Carrier .PURGOTTI (A) .Tribromophenol .MULHAUSER (0.). Manufacture of Resorcinol .NIETZEI (R.) and J . PREESSER . Constitution of Dinitroquinol : Formationof Nitranilic Acid .CLAISEN (L.). Action of Sodium Alkoxides on Benzaldehyde .NIETZEI (R.) and F . KEHRYANN . Quirionedioxinie and Dinitrosobenzene .CLAISEN (L ..} . Iptroduction of Acid Radicles into Ketonen .WULFING (A.). Separation of Ortho- and Para-toluidine .MUHLHAUSER (0.). Manufacture of Dimethylaniline .MERZ (V.) and P. MULLER . Coiiversion of Phenols into Amines .Moos (I?.). Condensation Products of Ethylene-aniline with Aldehydes .HANSSEN (A.). Action of Carbonjl Chloride on Ethylene- and Trimethylcne-diphenyldiamine .ZIEGLER (J . H.) and M . LOCHER . The Tartrazines ; a New Class of Dyes .ZIEGLEK (J .H.) and M . LOCHER . Condensation Products of SecondaryHydrazines with Dihydroxytwtaric Acid .DAHL (A) . Preparation of ~enzylrosaa~linedisulphonic Acids .MUHLHAUSER (0.). Manufacture of Benzaldehyde-greens .LIEBERMANN (C.) and P . SIEDLER . Opiaurin .BRODSEY (L.). Action of Aldehydes on Ammonium Thiocganate .HELMERS (0.). Additive Products of Aromatic Thiocarbimidea .BEUBERT (K.). Manganese Benzoate .MICHAEL (A.) and G . M . BBOWNE . Isomerism in the Cinnamic Acid SeriesEDELEANO (L.). Derivatives of Phenylmethacrylic Acid and of Yhenyliso-butyric Acid .CLAISEN (L.) and 0 . LOWMAN .LIEBEWANN (C.) and S . KLEEMANN .Preparation of Ethyl Benzoylscetate .Etherification of Opianic Acid . BOTTINQER (C.). Oak Tannin .KLEEMLNN (S.) Reduction of Nitrio-opianic Acid .SALOMON (0,) . J/-Meconine .BOWMAN (W.).Action of Potassium Cyanide on Meconine .EUHARA (M.). Orthotoljlphthalimide .WISLICENUS (W.). Synthesis of Ethyl Salts of Ketouic Acids .PIETTI (A ) . Synthesip of Ethyl Trirnesate .FISCHEB (E.) and P . WAGNER . Rosiadoles .PAGE6055065065075655665666676675685685686695695706706716716725725725736736745745745755755765765765775775785795795795805805816825825&358358458458458558658658758758CONTENTS . XFIsHEB (E.) and A . STECHE . Methylation of Indole-derivatives .ADAM (P.). Diphenyl-derivatives .GBAEBE (C.) and C . AUBIN . Condensation of Diphenic and Orbhodiphenyl-carboxylic Acids .GPAEBE (C.).Formula of Diphenic Acid .LELLMANN (E.). Preparation of B-.Nitronaphtlialene .NIETZKI (R.) and J . GOTTIC: . B-a-Azonaphthalene .WITT (0 . N.). New Method of Preparing Azines .WITT (0 . N.). Constitution of Isomeric Tolunaphthazincs .B IRU K OFF ( W . ) . D imet hy lan thragallolWEND E (H . ) . Trimet h y lanthragallol .Chloride on Anthracene Dihpdride .BRAE BE (C.) . Acenaphthene .QUINCKE (F.). Derivatives of Acenaplithene .LIEBERMANN (C.) and W . WENSE . Hydroxyanthraquinone Dyes .BEHLA (G.). Substituted Anthracene-carboxylic Acids : Action of CarbonylTANRET (C.). Nitrogen-derivatives of Tehebenthene .WALLACH (0.). Terpenes and Ethereal Oils .WEBER (E.). Ethereal’ Oils .BOUCHARDAT (G.) and J .LAFONT . Active Camphelie and Ethylborneol .CIAMICIAN ((3.) and I? . SILBER . Determimtion of Positions in the Yyrro-line Series .CIAMICIAN (G.). Tetriodopyrroline .DENNSTEDT (M.) and J . ZIMMERMANN . Reactiqn of Acetone with PyrdinePLOCHL (J.). Synthesis of Pjridine Bases .MUTHMANN (W.) aud J . U . Nef .RIEHM (P.). Condensation Products of Acetone and Acetoplienone withAniline and Ammonia .KOENIGS (W.) and J . LJ . NEF . 4’-Phenylquinoline and the Derived Di-quinolyls .FISCHER (0.). Ortho- and Meta-quinolinesulphonic Acids .HNORR (L.). Synthetical Experiments by Means of Ethyl Acetoacetate .CONINCK (0 . DE) . Alkaloids .LELLMANN (E.). Phenylpiperidine .SCIXILBACH (C.). Berberine Salts .SCHMIDT (E.) and 0 . SCHILBACH . Ac ion of Potassium Permangauate onBerberine .KASSNER ((3.).Lactucerin .MYLIUS (F ) . Cholic Acid .YCHOTTEN (C.). Bile Acids .\VT-BSTER (C.). Behaviour of Hydrogen Perolide to Albumin .BOURQUELOT (E.). Deterioration of Diastase by the Action of Heat .KRAMER (G.) and W . BOTTCHEB . The Relation between Petroleum andthe Hydrocarbons of Coal tQr and Shale-tar .MULLER (J . A.). New Class of Ferrscjanides and Ferricymidee .RATHKE (B.). Nelamines .RATHKE (B.). Thiammeline .LIEBERMANN (C.) and 0 . BERBAMI . Coccerjl Alcohol and CoweqlicAcid .FISCHER (E.) and J . TAPEL . Oxidation of Polyatomic Alcohols .kPPMANN (E . 0 . v.). A New Galactan : Properties of Galactose .MALBOT (H.). Preparation of Norm3 Propplamines and Isoamylamines .COMBES (A.). Homologues of Acetylacetone .LWOFF (J.).Fatty Acids in Resin .GEHRINB (G.). Octyl Mono., Di., and Tri-chloracetates .RENARD (A.). Metallic Propionates .WISLICENUS (J.). Chloro-derivatives of Crotonic Acid .MICHAEL (A.) and (3 . M . BROWNE . Isomerism in the Crotouic AcidSeries ..Cinchonic AcidSTOEHR (C.). Strychnine .PAGE5885595895895905905905915925925926935935935955965965Y659759759859859859959960160160360460460460460560660660760864864965065065065165265265365365365465565xxviii CONTEZVTS .COMBES (A.). Synthesis in the Para5n Series by Means of AluminiumChloride .SMOLKA (A.). Action of Bromine on Carbamide .UUNTZ . Antimony Tartrate .PAAL (C.). Constitution of Pyrotritartaric Acid .DIETRICH (F.) and C .PAAL . Pyrotritartaric Acid-derivatives .CANZONERI (F.) and V . OLIVEEI . /?-Bromofurfuran .JACOBSEN (0.) and W. DEIKE . Synthesis of Hemellithene .MAYER (F.). Reduction of Trinitro-+-cumene .JACOBSEN (0.). Action of Sulphuric Acid on Pentamethylbenzene .WILL (W.) and W . PUKALL . Resorcinol-derivatives .PUKALL (W.) . Resorcinol-derivatives .RATHKE (B.) . Triphenylthiammeline and a Third Triphenylammeline .MULLER (P.). Primary and Secondary Xylsmines from Xylenols .MICHAEL (A.) and Gt. M . BROWNE .JANOWKY (J . V.). Azo-compounds .HEUMANK (K.) and L . OECONOMIDES . Reaction of Diazoamido-compoundswith Phenols .ENORR (L.) . Cinnamylhydrazine .BERNTHSEN (A.). Phenazoxine .ZELINSKY (N.) .Action of Dehydrating Agents on Benzylideneacetoxime .BEEGNTHSEN (A.) and A . GOSKE . Methyl-orange and Ethyl-orange .WEDDIQE (A.) and H . FINGER . Action of Nitrous Acid on Orthamido-benzamide .SULKOWSKI (J.). Oximes of Paraxyloquinone .NOERRISON (C.). Bromorthotoluic and Bromorthophthalie Acids .MICHAEL (A.). Reduction of the Isomeric Bromocinnainic Acids .WEINREICH (S.). Mono- and Di-hydroxvtoluic Acids .ZELINSKY (N.). Ethyl Phthalate Chloride .HOTTE (B.).HENDERSEN ((3 . (3.). Ethyl Triphenylcarbinylmalonate : /I-Triphenyl-MICHAEL (A.). Action of Ethyl Sodacetoacetate and Sodomalonate on theMICHAEL (A.). Formation of Indigo-blue from Ortho-nitrophenylpropiolicAcid .BRERNER (P.) and 0 . N . WITT .HEUMANN (K.) and J .WIERNIK . Diphenylethane-derivatives .BERNTHSEN (A.) and A . SEMPER .BAMBERGEE (E.) and 0 . BOEKNANN . /3-Naphthyl-derivatives .TANRET (C.). Action of Hydrogen on Nitro-derivatives of Terebcnthene .Manufacture of Santonin .CIAMICIAN ((3.). Conversion of Pyrroline into Pyridine-derivatives .ENORE (L ) Yyrazole-derivativesCONRAD (M.) and L . LIMPACH . Synthesis of Quinoline-derivatives by MeansAromatic HydroxylaminesAction of Phenylhydrazine on Anhydrides of Bibasic Acidspropionic Acid .Ethyl Salt8 of Unsat. urated Acids .Benzidine-derivativesZIEOLER (J . H.). Tetramethylamidobenzophenone .URBAN (C.). I, 3, Naphthylenediamine .GIMBEL (A.). Nitrosoanthrone .BOUCEIARDAT ((3.) aed R . VOIRY . Terpinol .BUSCH (A.).Synthesis of Juglone.of Ethyl Acetoacetate : y-Hydroxyquinaldine .REED (J .H.). Methylnaph tliaquinolines and ,8 .Naphthacridine .STOEHR (C.). Skatole from Strychnine .GINTL (W.) and L . STORCH . Ecgonine .LATSCHINOFF (P.). Bile Acids .LATSCHINOFP (P.). Crystalline Form of Chole’ic Acid .WTJRSTER (C.). Action of Oxidising Agents on Albumin .WTJRSTER (C.). Behaviour of Sodium Nitrite towards Albumin andHsemoglobin .HENRY (L.). Determination of the Relative Value of the Four Units ofActivity in the Carbon-atom .P A QE6566566576576586586596596606606616626636636636646656f1566666666766766866866966966967167267267267367467467467567567567767767867867968168268268368368371168CONTENTS .xxixNORTON (L . M.) and H . J . WILLIANS . Action of Bromine on Isobutylene .DE LACRE (N.). Dichlorethyl Alcohol . HENRY (L.). Synthetical Acetonitrile .CLAUDON (E.) and E . C . MORIN . Alcohols in BrandyKILIANI (H.). Action of Sodium Amalgam on Arabinove .WILL (W.). Sugars from Hesperidin and Naringin .CURTIUS (T.). Hydrazine (Diamidogen) .MICHAEL (A.) Reactions with Ethyl Sodacetoacetate ..NETTLEFOLD (F.). Sodium Nitrate in Gun-cotton .DIEFF (W.) and A . REFORMATSKY . Oxidation of Ricinoleic and LiiioleicAcids .HANTZSCH (A.) and 0 . WOHLBRUCK . Ethyl Propiopropionate .REFORMATSKY (S.). Synthesis of Diatomic Monobasic Acids .LANQ (E.). Decomposition of Ethyl Acetomalonate and its Homologaes .(XOLDSCHMIDT (H.) and W .SCHULTHESS . Thienethylamine .Constitution of Benzene .THIERFELDER (H.) . Glycuronic Acid .CLAUS (A.).BAMBERGER (E.) and W . LODTER . Aromatic Nitriles .HANTZSCH (A.). Constitution of Quinone-derivatives .matic Compounds .SCHNITEB (K.). Isomeric Chloro- and Bromo-thymoqninones .SANDMEPER (T.). Substitution of the Amido- by the Nitro-group in Aro-LLOYD (R.), Conversion of the Higher Homologues of Phenol into AminesJACKSON (C . L.) and J . F . WING . Dimethylbenzylamine .MEEZ (V.) and C . RIS . Action of Ethylenedkmine on Catechol .HOLZMANN (E.) Thio-derivatives of Diethylaniline and Dimethylaniline .MICHAEL (A.) and J . P . RYDER . Action of Aldehydes on Phenols .MULLER (W.). Metamethylcinnamic Acid and its Derivatives .CHASANOWITSCH (J.).Action of Phosphorus Pentachloride on SalicylicAcid .Derivatives of Ethyl Quinoneparadi-carboxylate .Conversion of Aromatic Sulphonatesinto Amido-compounds .Oxidation of Benzene-derivatives withPotassium F'erricyanide .Conversion of p-Naphthaquinone into Indonaphthene-deriva-tives .ROSER (W.). Synthesis of Indonaphthene-derivatives .FISCHER (0.) and E . HEPP . Ritrosamines .WITT (0 . N) . Azonium Bases .ZINCKE (T.) and A . T . LAWSON .. Azo-derivatives of Phenyl-/3-naphthyl-amine .ZINCKE (T.) and A . T . LAWSON . Orthamidoazo- and Hydrazindo-deriva-tives .NIETZKI (R.) and A . L . GUITEBMANN . Naphtholcarboxylic Acids .BAYER (F.) and C . DUISBEXG . P-Naphthylaminesulphonic Acid .NIETZKI (R.) and T . STEINMANN .Purpurogallin .BARR (A.). Nitrophenols and Phenylhydwzine .LIMPRICHT (H.). Sulphazides .GABRIEL (S.). Homophthnlimide .HANTZSCH (A.) and A . ZECGENDOBF .JACKSON (C . L.) and J . F . WING .NOYES (W . A.) and C . WALKER .ZINCKE (T.) .WAGNER (H.). Oxidation of Santonin .VESTERBERG (A.) . Amyrin .SCHMIDT (R . E.). Composition of Lac-dye .OLDBACH (H.) .BAUNANN (J.).LADENBURG (A.).DUREOPF (E.) and M . SCHLAUQK .BBRKTHSEN (A.) and H . METTEGANG .8-Methyltetramethylenediamine and P-Methylpyrrolidine .Action of Amines on EthylenedibenzoylorthocarboxylicAcid .The Cinnamene of the Pyridine Series ... Constitution of Aldehyde-collidineReactions of Quinolinic Acid .PAGE712712713714714715715715716716717717717717718719719719720720721721722722723'72372372472572532772772772872972972973073173273273373373373473573573773773XXS CONTENTS .PAGERUGHEIMER- (L.) .and C .G .SCHBAMM. Quinoline-derivatives . 738SCHMITr (R.) and F . ENGELMANIT . Orthohydroxyquinolinecnrboxylic Acid 738LELLMANN (E.) and Ct . LANGCE . Quinoline . 737UABRIEL (S.). Homologue of Isoquinoline . 739SALOMON (Gt.). Xanthine-derivatives in Urine . 739LADENBURG (A.), The Piperidine Series . 741)LADENBUSG.(A.) and F . PEFERSON . Duboisine . 740LADENBURQ (A.). Constitution of Tropine . 740JOLIN (S.). The-Acids of Pig's Bile . 742GUNTHER (F.). Iodoform and Bromoform . 787&HAL (A.). Caprylidene : Constitution of Capraldehyde .788EINHORN (A.). Ecgonine . 741BOCKLESCH (0.). Ptomaines from Pure Cultivations of Vibrio proteus . 742COLSON (A.). Products from the Residues of Compressed Gas . 787GRIMAUX (E.) and C . CLOEZ . Ergthrene Bromides . 789KLASON (P.).with Ethers end Alcohols . 789~ E H N (C.).FPee Thiocyanic and ayanuric Aoids and their CompoundsAction of . Polyatomic Alcohols on Solutions of Boric Acid andHydrogen Sodium Cartknate .~TROM.EYER (W.)h Sugar-compounds .HAEDICKE (J.) and B . TOLLENS .HAEDIQKE (J.), R . W . BAUBR. and B . TOLLENS . Galactose from CanragheenMoss .SBYBERLICH -(A.) and H . TBAMPEDACH . Saccharification of Starch by R'itricAcid .Formation of Ualactose and RaiEnoaeNETTLEFOLD (F.). Nitrocellulose .BUISINE (A.).Amines in Suint .DUVILLIER (E.). Trimethyl-a-amidobutyrobetaine .mmia with Unsaturated Compounds .LERCH (J . 2.). Red Dye from Chloral Hydrake .GRIMAVX (E.). Glyceraldehyde .ENGEL .( R.) .. Action of Ammonia on Chlorethanes : Direct Union of Am-RAUPENSTRMJCH (Gt . A.). Condensation of Normal Butyraldehpde .MO~ILAU (R.) and C . HOFFNANN . Alkyl Hypochlorites from Isonitroso-compounds .HENRY (L.). Cyanacetic Acid .BALLEB (A.). Ethyl Cyanacetate .MENOZZI (A.) and C . BELLONI . a-Methylamidovaleric Acid .AUTENRIETH (W.3. Substibuted Crotonic Acids- .KOBERT . Croton Oil .HAZURA (K.) and.A. FBIEDREICH . Acids from Drying Oils .RAZURA (K.). Acid from Hempsced Oil .HALLER (A.) and A . HELD . Ethyl Cyltnacetoacetate .RISCHBIETH (P.). Preparation of Levulinic Acid .BLOCK (J.) and B .TOLLENS .&ALA (A.). Propylxanthic Acid.KEHRMANN (F.). Potassium Manganic Oxalate .KOERNER ((3.) and A . MENOZZI .BEHRINB ((3.). Butyl.Sebacate .B ~ K A L (A.). Capraldoxime and Methylhexylacetoxime .REWRY .(I,. ). Synthetic Acetic Acid and its Deriratires .Salts of Levulinic Acid .CLAISEN (L.).GEHRING f (3.).Addition of Ethyl Malonate to Unsatur&ted Compoundsa-Amidoisosuccinic Acid .Perchloramvl and Perchlorobutrl Pe~chlorosebaea.tes .PIUTTI (A:> . ' Reciproctll Transformation of the Optically Active Aspms-gines .MARQUAEDT (A.). Alkyl Compounds of Bismuth .RUTH (U.). Furfuran-deriyatives .Thiophen Series . R U F ~ I fH.) . Normal Propylthiophen-derivatives : Ulyoxylic Acids of theMEYEB.(V.) and K .NEUBE . Bm-Droducts of the Thioghen Manufacture .m791791791792792793792793793'794794795795796796797797797798798799$9979980080080080080180180180280280380480CONTENTS . xxxiNIETzKr (R.) .WZLLUERODT (C.).WIZLUERODT (C.) .V~SET (R.) and G . TIENNILSCERAMM (J.).Format. ion of Croconic Acid from Eenaene-derivatives .The Ealogen Carriers in the Natural Groups of theElements .Halogen Benzene HaloYds . a-Trichlorobenzene Hexa-chloride .Action of Acetylene on Benzene in Presenceof Aluminium Chloride .Influence of Light on the Action of Halogens on AromaticCompounds .MYLIUS (E.). Phenol .TASSINARI (a.). Action of . Sulphur Dicbloride on Phenol .ZINCKE (T.).Derivatives of Orthobenzoquinone .GOLDSCHMIDT (H.) and J . STRAUSS . Dinitroso-orcinol and Dinitrosores-orcinol .CAUSSE (H.). Action of Acetaldehyde . on Polyvalent Phenols .Formation of Haloid Substitution-derivatives of Amido-corn-pounds by the Reduction of Nitro-derivatives of Hydrocarbons .CLAUS (A.) and A . STIEBBL . Metanitropamhloradine .MATZUDAIRA (C.). Dibenzylaniline and its Derivatives .WALDER (F.). Benzyl-derivatives of Hydroxylaruine .KOCK (E.) .GBAEBE (C.). Boiling Points of piphenylamine and its Homologues .BERJJNERBLAU (J.) and H . POLIKIEV . Intermediate Products in theFormation of Indoles from Dichlorether and Aromatic Amines .ASCHAN (0.). Action of Chloracetic Chloride on Orthamidophenol .AUQER (V.).Action of CEnanthaldehyde and Heptyl Chloride on Di-BEENTESEN (A.). Action of Cinnamic Acid on Diphenylamine .methylaniline .BAITHER (0.). Tetramethyldiamidobenzophenone .Metaparatoluy leneaamine .GRIESS- (P.) Diazo-compounds . b .MELDOLA (R.). Constitution of Diazoamido-compounds .FIWHER (B.) and H . WIMMER . Diazoamido-compounds .FISCHER (B.) and H . WIMMER . Hydroxyazo-compounds .MUELHAUSER (0.). Manufacture of Methyl-violet .WITT (0 . N.). Induline of Azophenine .ZI~GLER (J . H.). Roshydrazine and a New Class of DyesQ-EHRING (G.). Aniline Sebacate and Diphenylsebacamide .HOFMANN (A . W.). Orthamidophenol Mercaptan .WZLLER (J.), Xylyl Phosphorous Compounds .MICHA~L (A.). Condensation of Aldehydes with Phenols .BUCHEA (K.) and.P .H . IRISH .HALLXR (A.) . Cyanacetophenone .BECKMANN (E.). Isonitroso-compounds .Aromatic Ethylene Di- .(J~aus (A.) and A . W . BUCHER . Chlorobenzoic Acids .%RNEMANN (E.). Metamethylcinnamic Acid ..HANTZSCH (A.) and H . ZUECHER, Polycoumarins .KIRCEER ((3.). Tetrachlororthobe~~zoylbenzoic Acid .LE ROPER (A . ). p-Dichlorophthalic Acid .GRAEBE (C.). Tetrschlorophthalic Acid .QLEVE (P . T,) . @.dphimido-compounda .HINSBERQ (0.). Action of Monatomic Aldehydes of the Fatty Series onMICHAELIS (A.) and E . SCHMIDT . Unsymmetrical BenzylphenylhSdrszine ..BILLETER (0.). Action of Thiocarbonyl Chloride on Secondary Amines .Oxidation of Ketones .CLAUS (A.), WERNER, SCHLARB, and MURTPELD .ketones and Alkylated Benzoyl-p-Propionic AcidsANscHUTz (R.) and W . BERNS .~ N B C H U T Z (R.) and C .C . SELDEN .ROSER (W.) and E . H~ELOFF .Phenylacetic Acid and DesoxybenzoinsGlaser's Monobromochnsmic AcidsIromerism in the Cinnamic Acid SeriesVILLE (J.). Action of Cyanamide on Benzenesulphonic Acids .HIRSCE (R.). Chloronitroderivatives of the Aromatic Series .PAQE80580680680680780780780880880981081081281281381381481481481681681781881981982082.18218228228238238248268268268.2782882982982983083088183183%833834838.2xxxii CONTENTS .FAHLBERQ (C.) and R . LIST . Ethyl Benzoic Sulphinide and Ethyl Ortho-sulphaminebenzoate .MAUMEN~ (E.). " Saccharin " .BERLIKERBLAU (J.).Indole from Dichlorether and Aniline .ROSER (W.). Synthesis of Indonaphthene-derivatives .ROSER (W.). Preparation of Paradinitrodibenzyl .KOCK (E.). Triphenjlmethane-derivatives .GUARESCHI (I.). y-Dichloronaphthalene and Chloronaphthdlic Acid .ZINCEE (T.) and C . GERLAND . Action of Bromine on Diamido-a-naphthol .MASCHKE (L.). /3-Naphthylamine-derivatives .ANNAHEIM (J.). Substituted Naphthylenediamines .HOFMANN (A . W.). Amidonaphthyl Mercaptans .EESTRAND (A . G.). Naphthoic Acids .BAMBERGER (E.) and 0 . BOEEMANN . Action of Sodium on Alcoholic/3-Naphthonitrile .MASCHEE (L.). Trimethylnaphthalene .ELBS (K.) and H . EURICH . 2 : 3 Dimethylanthmqninone .ELBS (K.) and M . GUNTHER .BALBIANO (L.). Camphor-derivatives .CAZENEUVE (P.). Isomeric Nitrocamphors .HANBIOT .Anemonim .CIAMICIAN ((3.) and P . SILBER . Action of Acetic Anhydride on Mkthyl:DENNSTEDT (M.) and J . ZIMMEBMANN . Action of Propionic Anhydiideon Pyrroline .PPEIFFER (G.) . Preparation of Halogen-derivatives of Pyridine Bases fromEINHORN (A.) and A . LIEBRECHT . Action of Chloral on a-Picoline .LEPETIT (R.). Reaction of Nitrobenzaldehydes with Ethyl Acetoacetate andAmmonia .1 : 3 Dimethylanthraquinonepyrroline and Benzylpyrroline .the Pyridinecarboxylic Acids .CLAUS (A.) and M . KICKELHAYN . Cinchonic Acid .ENORR (L.). Synthesis of Quinoline.derivatives .WEIDEL (H.). Reactions of Quinoline .MUHLERT (F.). Action of Acetamide on Orthochloroquinoline .BEYEB (C.). Quinoline-derivatives from B-Diketones .BERNTHSEN (A.) and F .MUHLEBT . Acridaldehyde and Acridinecarb-oxylicAcid .DUVILLIER (E.). Creatines and Creatinines .DE CONINCK (0.). AlkaloYds .PLUGQE (P . C.). Opium AlkaloYde .PLUGGE (P . C.). Composition of Papaverine .GUARESCHI (I.). Strychninesulphonic Acids .HENSCHKE (A.). Chelidonine, Chelerythrine, and Sanguinarine .DRAGENDORFF (G.) and H . N . ROSEN .Hsemoglobininto Albumin andHEematin .LINOSSIER ((3.). Compound of HEematin with Nitric Oxide .MIUBA (M.). Melanin .BBHAL (A.). Preparation of Ally1 Iodide and Ally1 Alcohol .DEMUTH (R.) and V . MEYER . Sulphuranes .HERZIGF (J.). Isodulcitol .RAYMAN (B.) . Isodulcitol .MAQUENNE . Derivatives of Inosite .MAQUENNE . Identity of Dambose with Inosite .VINCENT (C.) and DELACHANAL .Carbohydrates from Acorns .GEUTHEB (A.) . Polyiodides .LUDECEE (0.). Crystallography of some Polyiodides .HOFFMANN (C.). Action of Hydroxylamine on Acetamide .HOLST and BECKURTS . Strychnine and Brucine Ferro- and Ferri-cyanides .Alkaloids of Lobelia .LEBENSBAUM (M.). Amount of Oxygen taken up in the Decomposition ofHOLAND (R.). Subatitution-derivatives from Methylene Chloride .PAGE835836836836836836837838838839839840840841844Wl84284284!384389.484A845845844384784784884984985085185185285285385485485485485590590590690690690890990991091091KARCZ (M.). Glyoxalaenanthyline and its Derivatives .ARNHOLD (M.). Triethylformate and various Methylals .ZELINSKF (N.) .Preparation of Ethyl a-Bromopropionate .FROMNE (G.) and R . OTTO . B-Dichloropropionic Acid .BENEDIKT (R.) and F . ULZER .GEUTHER (A.). Constitution of Ethyl Propiopropionate .LESCCEUR (H.). Dissociation of Hydrated Oxalic Acid .Ethyl Sodomalonate .ANSCHUTZ (R.). Isomerism of Fumaric and Maleic Acids .normal-butyric Acid .FLSCHER (E.). Carbamide-derivatives of Dibromopyruvic Acid .LASSER.COHN . Sodium and Potassium Ethyl Tartrates .HORBACZEWSEI (J.). Synthesis and Constitution of Uric Acid .BLAREZ (C.) and Gt . DENIQES . Solubility of Uric AcidHAZURA (K.). Acids from Drying Oils .DELISLE (A.). Action of Sulphur Dichloride on Ethyl Acetoacetate .ANSCHUTZ (R.) and A . R . HASLAM . Action of Phosphoric Chloride onChloralide .BISCHOFF (C .A.) and A . HAUSDORFER . Action of Iodine on Derivatives ofTurkey-red Oil .ENGEL .FROYME (G.) and R . OTTO . Synthesis of Xeronic Acid from a-Dibromo-CLAISEN (L.) and N . STYLOS . Action of Ethyl Acetate on Acetone .Conversion of Fumaric and Malei’c Acids into Aspartic Acid ..BEIEREND (R.). Synthesis of Compounds of the Uric Acid Series .GUTHZEIT (M.) and W . EPSTEIN . Action of Phosphoric Sulphide on EthylDimethylpyronedicarboxylate .ZELINSEY (N.) . Thiophen-group .MAREOWNIKOFF and J . SPADY . Constitution of the Hydrocarbon C,H,from Caucasian Petroleum .GAUTIER (H.).SCHRAUF (A.). Molecule of Crystalline Benzene .Influence of Light and Temperature on Chlorination .OTTO (R.). Synthesis of Aromatic Polysulphides .HUGOUNENQ (L.).Chlorine-derivatives of Anisoyl .GOLDSCHMIDT (H.) and E . KISSER . Carvole-derivatives .ZEHENTER (J.). Bromine-derivatives of Resorcinol .Pyrogallol . HANTZSCH (A.) and K . SCHNITEB . Action of Chlorine and Bromine onSALZMANN (S.). Anilic Acids .NET (J . U.). Nitranilic Acid from Chloranil .RAYMAN (B.). Cholesterin .GIRARD (C.) and L . L’HOTE . Combination of Aniline with Chromic Acid .BONNA (A.) . Phenylparatoluidine .SENP (A.) . Cyananiline, Cyanphenylhjdrazine, &c .NIETZEI (R.). Hexa-derivatives of Benzene .GRIESS (P.) and G . HARROW .BLocnMANN (R.). Action of Aniline Hydrochloride on Ethyl Cyanide .BECKER (P.). Chlorination by Means of Acetic Chloride .GUITERMANN (A . L.). Orthazoxytoluene .FISCHER (E.).Hydrazines .FISCHEE (E.) and 0 . KNOEVENAGEL . Compounds of Phenylhydrazine with .PFULF (A.). Hydrazinehenzenesulphonic Acids .ANSCHUTZ (R.) and Q . WIRTZ . Anilides of Fumaric and Malei‘c Acids: .GEHRIRG (G.) . Sebaceodinitranilide .NIEMENTOWSEI (S.) and M . OBREMSKI . Metaformotoluide and its Deriva-tives .LELLMANN (E.) and 0 . BONHOFFER . Introduction of Carboxyl into AromaticDerivatives by the Action of Diphenylcarbamide Chloride .BERGREEN (H.). Carbon Thiodichloride .NIEMENTOWSKI (S.). Anhydro-compounds .Action of Aromatic Diamines on SugarsAcraldehyde, IUesityl Oxide, and Ally1 BromideP hen ylas p artic AcidPAGE9119119129129139149159159151315916916917917917918918918919919920921922922922923923923924925926926926927927928929930931932932932932933934935935935937937CONTENTS .d i iVOL . L I I . xxxiv CONTENTS.MILLER (W. v.). Nitrosalicaldehydes .MILLER (W. v.) and F. KINKELIN. Nitrocoumaraldehydes .TAEGE (C.). Nitrosalicaldehyde and Nitrocoumarin .CLAISSEN (L.) and L. FISCHER. Benzoylaldehyde .ELBS (K.). Aromatic Eetones .BEYER (C.) and L. CLAISEN. Introduction of Acid Radicles into Ketones .CLAISEN (L.) and 0. MANASSE. Nitrosoketones .RACINE (S.). Derivatives of Orthotoluic Acid .ANSCHUTZ (R.) and W. 0. EMERY. Action of Phosphorus Chloride onSalicylic Acid and Phenol .ANSCHUTZ (R.) and G. D. MOORE. Action of Phosphoric Chloride onANSCHUTZ (R.) and Q. D. MOORE.Action of Phosphoric Chlorido onENBLER (C.) and E. WOHRLE. Preparation of Mandklic Acid and its De-rivatives .DUPARC (L.) . Reduction of Orthonitrophenylglycollic Acid .CLAUS (A.) and K. EROSEBERB. Parutolylglyoxylic, Paratolylhydroxyacetic,and Paratolylacetic Acids .BUCHKA (K.). Paratolylglyoxylic Acid . , .MICHAEL (A.). Behaviour of Ethyl Oxalate with Resorcinol .VINCENT (C.) and DELACHANAL.RAYMAN (B.). Action of Arsenious Sulphide on Acid Chlorides .RACINE (S ). Phthaldehydic Acid .BISCHOFF (C. A.) and H. SIEBERT. Benzyl and Benzoyl Compounds .WISLICENUS (W.). Combination of Lactones with Ethereal Salts .MAYER (I?.). Nitro-+-cumidinesulphonic Acid .OTTO (R.) and A. Ros SING. Aromatic Sulphonates containing BivalentAlcohol Radicles .OTTO (R.) and A.ROSSING. Reduction of Aromatic Thiosulphonates con-taining Alkyl Radicles by means of Hydrogen Sulphide .XINCKE (T.) and C. FROLICH. Halogen-derivatives of Phenylene Dichlor-acetylene Ketone .PFULF (A.). Indoles .RASCHEK (J.) . Indoles from Tolylhydrazine .WENZING (M.). Methylindoles .MILLER (W. v.) and F. KINEELIN. Condensation of Isobutaldehyde andMethylal with Aniline .ARHEIDT (R.). Diphenylenedihjdrazine .DOBREFF (N.). Orthodibenzgldicarboxylic Acid .BAMBERQER (E.) and R. MULLER. So-called Carbonylcarbazole (Carbazole-ZINCKE (T.). Hydrocarbon C16H12 from Styrolene Alcohol .ZINCKE (T.). Action of Chlorine on Phenols .CLEVE (P. T.). Action of Chlorine on Aceto-p-naphthylamine .JACOBSEN (P.). Orthamidated Aromatic Ketones .CAHN (E.) and M.LANGE. Action of Aldehydes on Amidosulphonic AcidsFORSLINQ (S.). &Naphthylaminesulphonic Acids .WOLFFENSTEIN (R.). Action of Phosphorus Pentachloride on a-Hydroxy-naphthoic Acid .SCHLIEPER (A.). Indoles from a-Waphthylhydrazine .JANDRIER (E.). Nitroacetonaphthene .BIRUKOFF (W.) . Naphthylerythrohydroxyanthraquinone .LIEBERMANN (C.) and A. GIMBEL. Preparation of Anthranol and Di-anthryl .WALLACH (0.). Terpenes and Ethereal Oils . *.FUWITZKY (F.) . Conversion of Dextrorotatory Terpenes from RussianTurpentine by means of Hydration and Dehydration .MEYER (V.). Isophthalaldehyde .VARNHOLT (L.). Chlorosalicylic Acids.Salicylic Acid .Meta- and Para-hydroxybenzoic Acids .Tannic Acid in Mountain Ash Berriesblue) ." .PAGB93893993994094Q94094394494594594694'794'794894894894994 99509509519519529539539549559569569579579 58958959959960961962962962963963964964965YG596CONTENTS. XXXVLAFONT (J.). Action of Glacial Acetic Acid on Lsevogyrate Camphor .EBERHARDT (L. A.). Black-pepper Oil .CAZENEUVE (P.). @-Chloronitrocamphor .GERRARD (A. W.). Strophanthus andStrophantin .SCHRAR (E.). Cubebin.CAZENEU~E (P.) and HUGOUNENQ. Pterocarpin and B omopterocarpin .GEUTHER (A.). Bitter Principle of Calalnus Root .SCHUNCE (E.) . Chlorophyll .LA COSTE (W.) and F. VALEUR. Derivatives of a-QuinolinedisulphonicAcid .LELLMANN (E.). Existence of Two Series of 4- (am) Derivatives of Quino-line .MILLER (W.v.). Action of Aniline on Mixtures of Fatty Aldehydes .RHODE ((3.). Action of Aniline on a Mixture of Acetaldehyde and Prop-aldehyde .MILLER (W. v.) and F. EINEELIN. Action of Aniline on a Mixture ofPropaldehyde and Acetal .MILLER (W. v.). Condensation of Quinaldine with Aldehydes .BRUNNEB (J. C. A.). Action of Isobutaldehyde on Quinaldine .EISELE (17.). Action of Paraldehyde on Quinaldine .SRPEK (J. 0.). Action of Furfuraldehyde on Quinaldine .BULACH (W.). Action of Paranitrobenzaldehyde on Quinaldine .FISCHER (E.) and A. STECHE. Methylation of Indole .FRIEDLANDER (P.) and F. M~LLER. Derivatives of Pseudocarbostyril .MILLER (W. v.) and F. EINEELIPI’. a-Metanitrophenylparamethoxyquino-line and its Derivatives .WEIDEL (H.) and J.WILHELM. Oxidation Products of 2’ : 2’ DiquinolineBANDROWSKI (F. S.). Bases in Galician Petroleum .WELLER (A.). Occurrence of AlkaloYd-like Bases in Paraffin Oil .CLERMONT (A.). Normal Quinine Hydrochloride .STOCKMAN (R.) . Amorphous CocaYne .KUNZ (H.). Emetine .THOMPSON (F. A.). Alkaloi’ds of Gelseminum Root .MYLIUS (F.). Cholic Acid .OTTO (R.) and K. VOIGT. Solid a-Dichlorethyl Cyanide and its Conversioninto Triethyl Cyanuride .KLASON (P.). Action of Acids on Thiocyanic Acid .FRIEDEL (C.). Crystalline Form of Quercin.SCHMIDT (T.). Comparative Sweetness of Cane- and Starch-sugar .NIEDSCHLAG (W.) .EHRENBERG (A,). Substituted Methylenediamines .HENTSCHEL (W.). Derivatives of Chlorinated Methyl Formate .SPICA (M.).Derivatives of Isopropyl Formamide .SPICA (A.) and G. DE VARDA. Derivatives of Isopropyl Chlorocarbonate .DUCLAUX (E.). Preparation of Valerie Acid .MICHAEL (A.) and G-. M. BROWNE. Isomerism in the Crobnic Acid Series.HALLER (A.) and A. HELD. Ethyl Acetocyanacetate .ELASON (P.). Thio-derivatives of Ethyl Carbonate .WILLGERODT ( C . ) . Acids from Acetone-chloroform .REIMER (C. L.) and W. WILL. Constituents of Rape-seed Oil .HAILER (A.). Preparation of Ethyl Cyanomalonate and Ethyl Benzoyl-cyanacetate .EOERNER (G.) and A. MENOZZI. Action of Ammonia on Ethyl Bromo-succin ate .HALLER (A,) and GF. ARTH. Ethyl Succinimido-acetate and Camphorimido-acetate .PINNER (A.) and J. LIFSCHUTZ. Action of Carbamide on the ChloraiC yanh y drins .LLOYD (J.U.). Asiminine .MACMUNN (C. A.). Myohsematin .Decomposition of Saccharose by Boiling with Limec 2PAGE9699699709709709719729729739739749749759759759759769’76976977978979979979980980980981981982983102410251026102610261026102710281028102810291029102910301030103010311031103xxxvi OONTENTS .JAFFB (M.) and R . COHN . Behaviour of Furfuraldehyde in the AnimalOrganism .GRINER (G.). Isomcride of Benzene .OTTO (R.). Action of Cyanuric Chloride and Chlorocyanuric Diamide onPhenols .HONIQ (M.). Nitrochlorotoluenes and Chlorotoluidines .GABRIEL (8.) and R . OTTO . Orthocyanotoluene .HEYMANN (B.) and W . KOENIQS . Oxidation of Homologues of Phenol .HANTZSCH (5.) and I( .SCHNITER . Constitution of Chlor- and Brom-anilicAcids .SCHNITER (K.). Preparation of Quinones . Halogen-derivatives of Tolu-quinone .GABRIEL (S.). Formation of Primary Amines from the CorrespondingNORTON (L . M.) and W . D . LIVERMORE . Action' of Dilute Nitric Acid onHEUMANN (K.) and J . WIERNIK . Phenpl-derivatives of Ethane .GOLDSCHMIDT (H.) and A . GESSNER . Cumylamine .HOFMANN (A . W.). Orthamidophenyl Mercaptan .GOLDSCHMIDT (H.) and N . POLONOWSKA . Anisamine .EOCH (E.). Behaviour of Tertiary Amines towards Nitrous Acid .REYCHLER (A.). Preparation of Phenylhydrazine .MEYER (E . v.). Preparation of Iodobenzene from Phenylhydrazine .PINNER (A.). Action of Carbamide on Phenylhydraziiie .WEDDIQE (A.). Derivatives of Acetylorthamidobenzamide .EORNER (M.).Derivatives of Benzoylorthamidobenzaniide .WILLQERODT (C.). Action of Yellow Ammonium Sulphide on Ketones andQuinones .TUST (P.). Tetrachlorobenzoic Acid .ERLENMEYER (E.,jun.). Constitution of Phenyl-a- and Phenyl-n-B-hydroxy-propionic Acids .LOPATINE (N.). Action of Aniline on Ethyl Dibromosuccinate .OTTO (R.) and A . ROSSINQ . Behaviour of Aromatic Sulphinic AcidsWITT (0 . N.). Manufacture of a-Naphthylamine .Halogen-derivatives .Subs ti tu ted Amid o . compounds .MARSHALL (J.) . Glycosuric Acid .towards Hydrogen Sulphide .GOLDMANN (F.). Action of Bromine on Anthranol .BIRUKOFF (W.) . Erythrohydroxyanthraquinonecarboxylic Acid .BIMBEL (A.). Derivatives of Dianthryl .LIEBERMANN (C.) and 0 .N . WITT . Azines of ChrysoquinoneBALBIANO (L.). Derivatives of Camphor .HALr. ER (A.). Racemic Camphol and its Derivatives .LIEBERMANR (C.) and M . R ~ M E B . Alkannin .LIEBERMANN (C.) and 0 . BERGAMI . Ruberythric Acid .LADENBURG) (A.). Formation of Pyrrolidine .PINNER (A.). Pyrimidines .BALBIANO (L.). Derivatives of Pyrazole .AHRERS (F.). Sparte'ine .COLASANTI ((3.). Reactions of Creatinine .BOWMAN (W.). Acetylhydrocotarnineacetic Acid .FREUND (M.) and W . WILL . Hydrastine and its DerivativesMEISSLER (A.) Ethyl Isobutyl Ether ..HALLER (A.). Inactive Borneols yielding Active Camphors .DENNSTEDT (M.) and J . ZIMMERMANN .LEPETIT (R.) . Pyridine-derivatives from Metanitrobenzaldehyde .Action of Acetone on PyrrolinePINNER (A.) and J .LIFSCHUTZ . Action of Carbamide on Cyanhydrins .LADENBURG (A) . Identity of Cadaverine with Pentamethylenediamine .HARDY and CALMELS . Synthesis of Pilocarpine .WARREN (H . N.). Detection of certain Hydi-ocarbons in Alcohols .NASINI (R.), and A . SCALA ..So-called Ally1 TrisiphiiePAQE103210331033103410351035103610361037103810391039103910411041104210421042104310441045104610461046104'7104710481049104910491049104910501050105110511052105210531053105410541056105610561057105'7105710881088108CONTENTS . xxxviiSEMMLER (F . W.). Ethereal Salts of Alliurn ursinium .FICE (R.). Formation of Inosite .VIETH (P) . Alcoholic Fermentation of Milk-sugar .PUCHOT (E.).Aldehyde Resin .CLOEZ (C.) . Chloracetones .HENTGCHE; (W.). Chlorinated Methyl Formates .WOHLBRUCE (0.) Action of Sodium on Ethyl Salts of the HigherGFattyAcids .KOERNER (G.), and A . MENOZZI . Transformation of Fumaric and Male'icAcids into Aspartic Acid and Asparagine .PELLIZZARI ((3.1. Oxidising Action of Alloxan .PAAL (C.), and A . PUSCHEL . 1 : 3-Methylphenylthiophen and 1 : 2-ThioxenFRIEDEL (C.), and J . M . CRAFTS . Action of Methyl Chloride on Orthodi-chlorobenzene in presence of Aluminium .FRIEYEL (C.) , and J . M . CRAFTS . Action of Methylene Chloride on Methyl-benzenes in Presence of Aluminium Chloride .ERRERA ((3.). Decomposition of Mixed Ethers by Heat a n i Nit& Acid .PECHMANN (H .v.). Isonitroso-derivatives .PHILIPS (B.). Unsymmetrical Secondary Hydrazines .FISCHER (O.), and E . HEPP . Azophenines and Indulines .COLLIE (N.). Action of Heat on Triethylbenzylphosphonium Salts .LEVY (S.), and K . JEDLICKA . Action of Bromine on Bromanilic and Chlor-anilic Acida .BOHN (R.), and C . GRAEBE . Galloflavin .ERRERA (G.) . Ethyl Parabromobenzoate and Parabromobenzoic Acid .REBUFFAT (0.). Derivatives of Phenylamidoacetic Acid .BONDZYNSEI (S.). Deriratives of Hydrothiocinnamic Acid .EIQEL ((3.). Paracoumaric acid .PULVERMACHER (G.). Homo-orthophthalimide .GABRIEL (S.) . Homo-orthophthalimide and the Homologues of IsoquinolineXAGNANINI (G.) Transformation of Homologues of Indole into those ofQuinoline .GUARESCHI (J.), and P .BIQIKELLI . Chlorobromonaphthalenes .FISCHER (O.), and E . HEPP . Nitrosamines .BALBIANO (L.) . Derivatives of Camphor .FRASER (T . R.). Strophanthin .MERCK (E.). StrophanthusandStrophanthin .ELBOBNE (W.). Strophanthus and Strophanthin .Ts CH IR CH (A . ) . Chlorophyll .GEDOLST (L.). Preparation of Picrocarmine .S CH ARTLER (L.) . Diastase .WEBER (J.). Pyridinepolycarboxylic Acids .GOLDSCHMIEDT (G.). Dimethoxyquinoline .LIPPMANN (E.), and F . FLEISSNER . Synthesis of Hydroxyquinolinecarb-oxylic acid .KNORR (L.), and C . KLOTZ . Pyrazoline-derivatives from Ethyl Benzoyl-acetate .GUARESCEI (J.). Weyl's Reaction for Creatinine .COMSTOCK (W . J.) and W . KOENIGS . Cinchona Alkalo%ds .WILLIAMS (J.). Preparation of Aconitine .BOEHM (R.).Curare .HESSE (0.). Alkalo'ids of Coca Leaves .SCHESTOPAL (C.). Tetramethyldiquinolyline .KAUDER (E.). Cryptopine and its Salts .HOWARD (W . C.). Separation of Hygrine from Cocaine .Novv (F . G.). Higher Homologues of Coca'ine .KRUGER (F.). Absorption of Light by Oxyhsemoglobin .LE NOBEL (C.). Action of Reducing Agents on Haematin, and Occurrence .AXENFELD . HEemialbumose . of the Products of Reduction in Pathological UrinePAGE10891089109010901091109910991100110011011101110211031103110411051106110611071107110811081109111111121113111311141115111511161116111611171117111711191119112011211122112211221125112511251126112611261127112xxxviii CONTENTS .Physiological Chemistry .SEEGEN (J.). Sugar in the Blood with reference to Nutrition .SEEGEN (J.).Power of the Liver to form Bugar from Fat .ROHMAKN (F.).EELLNER (0.). E’eeding and Development of Silkworms .SALKOWSKI (E.). Isethionic Acid in the Body and Thiosulphuric Acid inthe Urine .PFEXFFER (!I.). Natural and Artificial Digestion .DEMANT (B.). Glycogen in the Liver of New-born Dogs .MORNEB (K . A . H.).Importance of Ammonia for the Formation of GlycogenLEO (H.). Trypsin in Urine .HIRSCHLER (A.). Lactic Acid in Animals .WARDEN (C . J . H.). Cobra Poison .MILLS (T . W.). Urine of the Tortoise .EIJLZ (R.). Gases of Parotid Saliva .Pigments of Uelanotic SarcomataLANDWEHR (H . A.). Pree Hydrochloric Acid of the Gastric Juice .MILLER (N.).Ferment Organisms of the Alimentary Canala .MUNE (J.). Formation of Eat in the Dog from Carbohydrates .CHAUVEAU (A.) and KAUPYANN . Relation between the Destruction ofGlucose and the Production of Animal Heat and Work .STERN (H.). Origin of the Bile Colouring Matters .DRAQENDORFF (G.). Physiological Action of Convolvulin and Jalapin .STUTZER (A.). Artificial Digestion .GARROD (A . B.).BIEDERT . Albuminoi’ds of Human Milk and of Cow’s MilkKULZ (E.). Active P-Hydroxybutyric Acid .Place of Origin of Uric Acid in the Animal Organism .FIRTH (R . H.). Poisonous Ptomai’ne in Milk .GOSSELS (W.).MARSHALL (.J.). Huffner’s Reaction in Bile .POSNEZ (C.). Albumin in Normal Urine .CITRON (H.). Mucin in Urine .Nitrates in Animals and Plants .BOCEAL (A.).Physiological Action of Paraldehyde .MAIRET (A.) and COMBEMALE . Physiological Action of Methylal .KOCH (E.) Butylchloral Hydrate and Chloral Hydrate as Antidotes forBELKY (J.). Action of Gaseous Poisons .EHRENBERQ (A.) . Sausage Poisoning .HANRIOT (M.) and C . RICHET . Estimation of the Carbonic AnhydrideMARCEUSE (W.). Formation of Lactic Acid during Muscular Activity .EOWALEWSKY (N.) . Formation of Methsemoglobin in Blood by the Actionof Alloxantin .EULZ (E.).FFEIFFER (T.) and F . LEHMANN .ELLENBERGER and HOFMEISTER . Digestion in the Pig .BAHLMANN (P.). Amido-compounds in the Animal System .Strychnine and Picrotoxin .expired and the Oxygen absorbed in Respiration .Decomposition of Bromides and Iodides by the Stomach .Addition of Sugar to Cattle-foods .ARNSCHINK (L.). Nutritive Value of Glycerol .CONSTANTINIDI (A.). Wheat Gluten as a Food .LUDD (E . F.). Pepsin versus Animal Digestion .GRBHANT and QUINQUAIJD . Formates in the Organism .LEO (H.). Reducing SubstanceinDiabeticUrine .Gltocco (P.) . Creatinine in Urine .ANRAEFF (A . N.).MULLER (F.). Aniline Poisoning .MAIRET (A.) and COMBEMALE . Toxic Action of Colchicine .JONES (E . I,.). Specific Gravity of Human Blood .BBCHAMP (A.) . Causes of the Alteration of Blood in Contact with Air,Oxygen, and Carbonic Anhydride .Behaviour of Quinol with Urine and UreaPAGE666’76868686916716716716817017028728728828828929029029138838838838938939039039039139139139239250’750850850850951151151251251351351351351451451560860CONTENTS .xxxixHASEBROEE (K.). A First Product of Gastric Digestion .GOLDSCHMIDT (H.). Intestinal Digestion in the Horse .WURSTER (C.). Oxidation in the Animal Body .KAST (A.). Fate of Certain Chlorine Compounds in the Organism .MONARI (A.). Formation of Xanthocreatinine in the Organism .MACMUNN (C . A.) . Invertebrate Chromatology .STUTZER (A.). Analysis of Nitrogenous Metabolites in Feces .HALLIBURTON (W . D.). Proteids of Cerebrospinal Fluid .MAIRET (A.) and COMBEMALE . Therapeutic Action of Colchicine .ELLENBERBER and HOFPYEISTER . Period required for Digestion in thePig .SIEBER (N.) and A . SYIRNOW .Behaviour of the three Tsomeric Nitro-MAIRET (A.) and COYBEYALE . Therapeutic Action of Methylal .GOLDSCHXIDT (H.). Absorption in the Stomach of the Horse .ELLENBERBER and HOFYEISTER . IXgestion and Digestive Secretions in theHorse .KAISER and SCHMIEDER . Changes in Milk by Freezing .HENZOLD (0.). Frozen Milk .RICHARDSON (B . W.). Action of Oxygen on Animals .WEISKE (H.) and others . Composition of Blood, Liver, and Flesh undervarying Conditions.SANBORN (J . W.). Animal Nutrition .ANDOUARD (A.). Variations in the Proportion of Phosphoric Acid inMilk .MARES .WmrE . Hydroxybutpic Acid in Diabetic Urine .MEYER (V.) . Physiological Action of Chlorinated Ethyl Sulphides .SHAPIROFF (B . M.), Physiological Action of Tertiary Alcohols .DEAGENDORFF (G.) and S .SALOMONOWITSCH . Myoctonine .FISCHER (E.) and F . PENZOLDT . Sensitiveness of the Sense of Smell .WOOLDRIDQX (L . C.). New Constituent of Blood Serum .HALLIBURTOPF (IT . D.). Muscle Plasma .FOKKER . Fermentation by Protoplasm from Recently-killed Animals .BRUNTON (T . L.) and J . T . CASH . Action of Caffe'ine and The'ine on Volun-tary Muscle .BRUNTON (T . L.) and J . T . CASH . Chemical Constitution and PhysiologicalAction .RANSOM (W . B.). Diabetes and Glycerol .HUBOUNENQ (L.). Laevorotatory P-Hydroxybutyric Acid in the Blood of aDiabetic Patient .BRUCKE (E.). Does Human Urine contain Free Acid ? .HANRIOT (M.) and C . RICHET . Relation between Muscular Activity andthe Chemical Effect of Respiration .CHAUVEAU (A.) and KAUFYAKN .Heat Developed by the Activity ofthe Muscles .VIQNAL (W.). Action of Micro-organisms from the Mouth and from Faeceson Food-stuffs .MBHU (C.). Sugar in Urine .RANVIER (L.). Per-ruthenic Acidin Histology .CRAMER (A.). Glycogen .WEYL (T.). Chemical Studies on the Torpedo .ELLENBERBEB and HOFMEISTER . Nitrogenous Contents of the DigestiveJuices .STUTZER (A.). Relation of Prote'ids to Digestive Ferments .ATWATER (W . 0.). Comparative Absorption of Fish and Meat in theAlimentary Canal .HERRMANN (A.) Digestion of Fibyin by Trypsin .TAPPRINEE (H.). Fermentation of Cellulose .benzaldehydes in the Animal Body .Excretion of Urea and Uric Acid from the SystemPAGH609610610612613613613614614684684684743744745745855855856856856857857857858983983984984985985985986986105810591059106010601127112811291129113011301131EAST (A.).'Arbmatic Products of Putrefaction in Human Sweat . 113xl CONTENTS .BAAS (K.). Relation of Tyrosine to Hippuric Acid .UDR~NSKY (L . v.). Urinary Pigments .Chemistry of Vegetable Physiology and Agriculture .LAURENT (E.). The Bacillus of Panary Fermentation .DENARO (A.). Decomposition of Silicic Acid by Leaves .EREUSLER (U.). Observations on the Growth of Potatoes .BATTUT (L.). Ammonia in Beetroots .HENKE (G.). Milky Juice of Certain Euphorbiacese .KLIEN . Composition of Barley and Pease .EELLEER (0.). Composition of Tea-leaves .HESSE (0.).China Bicolor .SACHS (J . v.). Chlorosis in Plants .KELLNEB (0.). Absorption by Soils .EELLNER (0.). Estimation of Absorbed Bases in Soils .STUTZER (A.). Chdi Saltpetre as Manure .MAGERSTEIN (v.). Comparative Manurial Values of Chili Saltpetre andQUANTIN (H.) . Reduction of Copper Sulphate during Alcoholic'Fermenta-tion .GAYON (V.) and E . DUBOURG . Alcoholic Fermentation of Dextrin andStarch .GAYON (V.) and Gt . DUPETIT . Method of Preventing Secondary Fermenta-tion .EHRENBEEG (A) . Is Free Nitrogen formed during Putrefaction ? .DEHBRAIN (P . P.) and MAQUENNE . Absorption of Carbonic Anhydride byLeaves .MUNTZ (A) . Ripening of Seeds .KRAUS (J.) . So-called Soluble Starch .FREUND (M.) and W . WILL . Substances contained in the Roots ofHydrastis Cumadensis .DEHBRAIN ( P .P.). Valuation of Manures .MUNTZ (A.) and C . QIRARD . Production of Farmyard Manure .WRIGHTSON (J.) and J . M . H . MUNRO . Manurial Value of Basic SteelMUNRO (J . M . H.). Influence of the Ferric Oxidc in Basic Cinder on theGrowth of Plants .LIBORIUS (P.). Bacterial Life in Relation to Oxygen .ROMMIER (A.). Wine and Brandy from Raspberries and Strawberries .ARLOING (S.). Zymotic Virus and Fermentation .ATWATER (W . 0.) and E . W . ROCKWOOD . Loss of Nitrogen duringClermination and Growth .RICHARDSON (C.). Variations in the Chemical Composition and PhysicalGRASSMAN (P.). Loss occasioned by Improper Methods of Pickling WheatBERTHELOT and ANDR~ . Nitrogen Compounds in Vegetable Soils .SIEVERT (M.).Manuring Rye with Thomas Slag, &c .RIMPAU and others . Thomas Slag and other Phosphates as Manure forMoorlands .NAUTIER (A.). Superphosphate Manuring for Sugar-beet .VINCENZI (L.). Chemical Constituents of Bacteria .SOHNKE (J.). Behaviour of Micro-organisms in Artificial Mineral Water .BRIEGER (L.). Source of Trimethylamine in Ergot of Rye .PAUL (R . H.) and A . J . COWNLEY . Amount of Caffei'ne in Various KindsM~LLER (C . 0.). Formation of Albumino'ids in Placts .Ammonium Sulphate .MAGERSTEIN (v.). Experiments with Chili Saltpetre .Slag .Properties of American Oats .of' Coffe;! .HOOPER (D.). Ash of Cinchona Barks . 394PA QE1133113370707071717273737676767771777817117117117217217317317417417517617829129229229229329329329429429539339339439CONTEXTS .xhJODIN (V.). Action of Mercurial Vapour on Leaves .BEPTHELOT . Direct Absorption of Nitrogen from the Atmosphere by Vege-table Soils .ATWATER (W . 0.). Acquisition-of Atmospheric Nitrogen by Plants .NAGAMATSZ (A.). Functions of Chlorophyll .VOGEL (A.). Influence of Ozone on Germination .MULLER . Formation of Sugar in Grapes .EIJKMAN (F . J.). Cinnamic Acid in Plants of the Ericacese Family .TROSCHPE . Composition of Lupines .K~NIG (J.).MEUSEL (E.). Effects of Tfiiocyanates on Vegetation and Fermentation .BORDAS . Grain of Holcus sorgho .LECHARTIER (G.). Cider Ash .SCHULZE (B.). Silage of Maize .SCHULZE (E.). Silage of Vegetable Matter .MARCEER .Diffusion Residues .WOLLNY (E.). Influence of the Physical Properties of a Soil on the Amount .WARINGTON (R.). Nature of the Nitrogenow Organic Matter of Soils .WOLLNY (E.). Decomposition of Organic Matter in Soils .KELLNER (0.) and others .FLEISCHER (M.), BRINCKMAN, and others . Manuring with Thomas Slagand other Phosphates .FITTBOGEN and SALFELD . Manuring with Thomas Slag .WAGNER (P.). Manurial Value of Thomas Slag .LEONE (T.). Changes Induced in Water by the Development of Bacteria .EMMEPLINB (A.). Fermentation of AJbumin in Plants .RICHARDSON (C.) American Barley .GIRARD (A.). Destruction of the XematoYds of Beetroot .BERTHELOT . Direct Absorption of Nitrogen by Vegetable Soils .ANDOUARD (A.). Incompatibility of Nitrates and Superphosphates .PRINGSHEIH .Decomposition of Carbonic Anhydride by Chlorophyll .MUELLER (H.). Physiological RBle of Vine Leaves .KREUSLER (U.). I s Nitric Acid formed in the Organism of Higher Plants ?GRIESSMAYER . True Natureof Starch-cellulose .MORAWSEI (T.) and J . STINGJ. Sugars of the Soja Bean .MORAWSEI (T.) and J . STINGL . Fat of the Soja Bean .BRUCKNER (E.). Russian Black Earth .MARCPER (M.). Value of the Phosphoric Acid in Thomas Slag .CLAUDON (E.) and E . C . MORIN . Fermentation of Sugar with EllipticalYeast .EHRENBERB (A.). Formation of Nitrogen during Putrefaction . ;PFXFFER (W.). Absorption of Aniline Colours by Living Cells .SCHULZE (E.). Presence of Clioline in Germinating Plants .SCOVELL (M . A.) and A . E . MEXKE . Composition of Potatoes .STOSSNER (E.). Effects of Deep or Shallow Sowing on Cereals .PAGNOUL (A.). Manurial Experiments with Sugar Beets .CELLI (A.) and F . MARINO.ZUCO . Nitrification .MARCACCI (A.). Action of AlkaloPds in the Animal and Vegetable King-doms .SCHULZE (E.). Are Nitrates formed in the Organisms of Higher Plants ? .LIST (E.). Organic and Inorganic Constituents of Grapes .BERTHELOT and ANDRB .JOFFPE (J.). Agricultural Value of Retrograde Phosphates .GREEN (J . R.).Composition of the Inner Brown Skin of the Earth-nut .of Free Carbonic Anhydride presentBeliaviour of Urea in SoilsJENTYS (S.). Intramolecular Respiration .ARNAUD (A.). Carrotene in Leaves .EASSNEB ((3.). Solanine .QUANTIN (H.). Tunisian Soils .BOKORNY (T.).Reduction of Silver Salts by Living Protoplasm .Evolution of Ammonia from Vegetable SoilsChanges in the Proteids of Seeds during GerminationPAGE39539551551651651751751851951951952052152152152152352352452%52452561561561661761761 768568568668668668668768768774674674774774774774885885985985986086086086086198798xlii gONTENTS .DIAKONOFF (N . W.). Molecular Respiration of Plants .MAYER (A.). Exhalation of Oxygen by Fleshy-leaved Plants in Absence ofMOLISCH (H.). Relations between Inorganic Salts containing Nitrogen, andPlants .MARTIN (S . H . C.). Prote'ids of the Seeds of Jequirity .FLUCKIGER . Safrole .ELBORNF (W.) Strophanthus .GAUNERSDORFER (J.).Poisoning of Plants by Lithium Salts .WAAGE (R.). Composition of some Leguminous Seeds .AITKEN . Experiments on Potatoes a t Harelam .DEH~EAIN ( P . P.). Production of Nitrates in Arable Soil .WEILANDT (M.). Free Phosphoric Acid and Superphosphate .AITKEN .Carbonic Anhydride .Basic Cinder and other Finely-ground Phosphatic Manures .AITPEN . Ground Pelspar as a Potash Manure .DUCLAUX (E.). Butter from Various Districts .ALVAREZ (E.). Microbe of the Indigo-fermentation .TSCHIRCH (A.). Aleurone-grains in the Seeds of Myristica Swrinamensis .BERGAMI (0.). Examination of Caucasian Madder Root .THIEL (H.). Experiments with Ensilage in Holland .GRUBER (M.). Culture of Anaerobic Bacteria : Morphology of ButyricFermentation .MUNTZ (A.).Distribution of the Nitric Ferment and its Function in theHOPPE-SETTLER (F.). Methane Fermentation of Acetic Acid .BELLUCI (G.). Formation of Starch in the Chlorophyll Granules .LEITGEB (H.). Crystalline Deposits in Dahlia Tubers .MILES (M.) . Nitrifying Microbes .Disintegration of Rocks .WIPPRECHT (W.). Absorption of Ammonia by Clay .GOESSMANN (C . A.). Analysis of Onions .ROBERTS (W.). Manuring with Various Phosphates . KREMP . Manurial Experiments with Various Phosphates .Analytica 1 Chemistry ,ARNOLD (C.). Kjeldahl's Method of Estimating Nitrogen .ZAMBELLI and LUZZATO . Separation of Arsenic and Antimony .BBENSTEIN . Detection of Thiosulphate in Sodium Hydrogen Carbonate .SALZER (T.). Detection of Thiosulphate in Sodium Hydrogen Carbonate .THILO (E.).BARNES (J.).Valuation of Zinc Powder and Testing of Carbonates .WEBTMOBELAND (J . W.). Determination and Valuation of Copper inBAUMANN (A.). Estimation of Ammoniacal Nitrogen in Soils .Estimation of Small Quantities of Silver in Burnt PyritesOres, &c .WRIGHT (L . T.). Analysis of Gas Coal .LUNGE (G.). Analysis of Explosives .SAMUELSON . Estimation of Glycerol in Wine .BOUILHON (E.). Estimation of Solid Matter in Wines .PBIOR (E.). Estimation of the Acidity of Malt .ALLEN (A . H.). Examining Fixed Oils .ELLIS (C . J.). Maumene's Test for Oils .JULIUS (P.). Employment of Congo-red in Titrating Aniline .with Sodium Hypobromite .HEW (J.). Detection of Artifxially Coloured Red Wine .SCHBODT (M.).Presence of Nitrites and Nitrates in Milk as Proof ofAdulteration .PFLUGER (E.) and K . BOHLAND .PFLUGER (E.) and K . BOHLAND . Estimation of Urea in Human UrineWITT (0 . N.). Qualitative Test for the Dyes found in Commerce .Hufner's Method of Estimating UreaPAQE988988989990990991991991992993995995996996106110611061106211341135113511351136113611361137113711377878797979a080828486868787878889909090919CONTENTS . xliiiPETTERSSON (0.). Apparatus for Gas Analysis .OETTEL (F.). Volumetric Method for determining Fluorine .PETTERSSON (0.). Air Analysis on a New Principle .WELCH (J . C.).WILSING (H.). Volumetric Determination of Sulphuric Acid .QUANTIN (H.).Volumetric Determination of Sulphatm .MORSE (H . N.) Land A . F . LINN . Determination of Nitric Acid .HOLLAND (P.). Determination of Alkalis in Silicates .BERG ( P . v.). Separation of Zinc from Iron, Cobalt, and Nickel .THOYFON (R . T.). Determination of Aluminium in Presence of much IronDEANE (L . M.). Estimation of Manganese and of Phosphorus in Iron andSteel .Detection of Stannic Sulphide in Presence of AntimoniousSulphide .HERZFELD (A.). Estimation of Carbon in the Organic Constituents ofWater .HARVEY (S.). Estimation of Nitrates in Water .EARTH (M.). Estimation of Glycerol in Wines .HERZFELD (A.). Estimation of Invert Sugar .BECKMANN (E.). Titration with Fehling’s Solution .CURTMAN (C . 0.). Detection of Salicylic Acid .ALLEN (A .H.). Specific Gravity, &c., of Waxes, &c .ALLEN (A . H.) and W . CHATTAWAY . Adams’ Method for Milk Analysis .THOMSON (W.). Adams’ Method for Milk Analysis .FOCPE .SAMUELSON . Detection of Artificial Colouring in Red Wine .GEORGES . Peptones in the Blood and Urine .Filters .CHAPMAN (A.). Method for Estimating Fluorine .WURSTEE (C.). Reagents for Active Oxygen .BRUGHAN (W . F.). Influence of Copper on the Estimation of Sulphur .MOLLER (G.). Eggerzt’s Method of Estimating Sulphur in Iron .ATKINSON (A . J.).FAIRLEY (T.). Estimation of Sulphur and Impurities in Coal-gas .DE KONINCP (L . L.). New Reaction of Thiosulphates .DE KONINCP (L . L.). Detection of Ammonia, Nitric or Nitrous Acids, andENOP (W.).Determination of Ammonia in Arable Soil .WURSTER (C.). Griess’s Reaction for Nitrous Acid .ARYSBY (H . P.) and F . G- . SEORT . Apparatus for Nitrogen Determination .VORWERK (P.). Determination of Phosphorus in Iron and Steel .ROSENBLADT (!I.). Determination of Boric Acid .GOOCH (F . A.). Separation and Estimation of Boric Acid .VAN NUYS (B‘. C.).HAUSHOFER (E.). Microscopical Analysis .HAUSHOFER (K.) . Microchemical Tests .BERG (P . v.).ATNSN (A.). Detection of Mercury in Organic Liquids .ROSENBLADT (T.). Separation of Mercury and Palladium .THONSON (R . T.).MOORE (T.). Estimation of Nickel in Ores, Mattes, and Slags .KRUSS (G.). Universal Spectroscope .Assay of Iron Pyrites for Available SulphurHUTCHINGS (W . M.). Analysis of Silicates .HAGER (H.).Testing Aluminium Sulphate .BLUY (L.). Separation of Manganese from Iron .GOZDORF ((3 . A.). Assay of Minute Quantities of GoldGRIFFITH (A.)..ALLEN (A . H.). Assay of Carbolic Soap .ALLEN (A . H) . Saponification of Fixed Oils .Separation of Morphine and Strychnine from Fatty Matters .DIEIJDONN~ (H.) Estimation of Tannin .G-AWAL o vs K I (A.) .Estimation of Sulphur in Coal and CokeThiosulphuric Acid .Estimation of Carbonic Anhydride in AirTitration of Zinc and Cadmium Sulphides with Iodine .WEIL (F.). Valuation of Zinc-dust .Estimation of Alumina and Iron Oxide in ManuresPAGE1791791791801801811811811811811821821821831831831841841841841851851851b51861 S618618618718718718829529529529629629629’729729729729829829929929930030030130130130230230230xliv CONTENTS .SELL (W .J.). Volumetric Determination of Chromium .BROWN ( W . L.). Analysis of Chrome Paints .MCCULLOCR (N.). Estimation of Chromate in the Presence of Dichromete .WACHSMUTH (0.). Estimation of Tin and Lead in Alloys .LEVY (L.). Colour Reactions of Titanic, Niobic. Tantalic. and StannicAnhydrides .LEVY (L.) . Colour Reactions of Arsenic. Arsenious. Vanadic. and MolybdicAnhydrides. and of Antimony and Bismuth Oxides .LUEDEKING (C.). Post-mortem Detection of Chloroform .SKALWEIT . Estimation of Glycerol in Wine and Beer .SCHEIBLER (C.). Separation and Estimation of Melitose in Cane-sugar .CREYDT (R.).Estimation of Melitose .PALM (R.). Detection and Determination of Lactic Acid .WATTS (F.). Titration of Citric Acid .SCHULZE (B.). Determination of Fatty Acids in Soap .CRONANDER (A.) . New Method of Estimating Fat in Milk .SKALWEIT (J.). Butter Testing .HAGER (H.). Butter Testing .WOLL (F . W . A.). Butter Analysis .CORNWALL (H . B.) and S . WALLACE . Reichert's Method of Butter AnalysisMOORE (R . W.). Carrot Coiour in Butter .MARSHALL (J.). New Ureometer .HIRSCHLER (A.). Separation of Nitrogenous Substances by Means ofPhosphomolybdic Acid .DIETRICH (E.). Opium Testing .MOLL (J . W.). Microchemical Detection of Tannin .B . (E.). Tannin Determination .MYLIUS (E.). Thale'ioquinine Reaction .HEISCH (C.).Analysis of Pepper .H~NOCQUE . Heematoscopy ; a New Method of Blood Analysis .KOCHS (W.). Determination of Sulphur in AlbuminoYds .FRIEDHEIM (C.). Weil's Method for the Volumetric Estimation of Sul-phides .GREEN (A . G.) and F . EVERSHED . Volumetric Estimation of Nitrous AcidMEINEKE (C.). Determination of Phosphorus in Steel and Iron .BENTE (F.) Determination of Phosphoric Acid .HAGER (H.). Detection of Arsenic .EAGER (H.). Use of Copper containing Arsenic for the Dearsenification ofBAUER (R.). Apparatus for Estimating Carbonic Anhydride and all similarGases .GRAVILL (E . D.). Estimation of Ammonium Carbonate in Spim'tus AmmoniaAromaticus. B.P.Determination of Cadmium and its Separation from CopperVolumetric Determination of Manganese .Hydrochloric Acid : Reinsch's Test for Arsenic .BRAGARD (M.).Estimation of Zinc as Pyrophosphate .ATKINSON (R . W.). Estimation of Manganese .INCE (W . H.) Ferric Chloride as a Test for Organic Substances .CANDWEHR (H . A.). Precipitation of Dextrin by Iron .BAUER (R.). Estimation of F a t t j Acids as Fats .NICKEL (0.). Quantitative Estimation of Oxalic Acid in Urine .ERETZSCHMAR (M.). Estimation of Fat .MILLER (A . R.). Preserving Standard Tartar Emetic Solutions .STILWELL (C . M.). Opium Analysis .VULPIUS (G.). Estimation of Quinine Sulphate .DF: VRIJ (J . E.). Quinine Chromate in Analysis .HESSE (0.) Normal Quinine Chromate .KOBNER (A.) .SCHOFFEL (R.) and E . DONATH .GIRAUD (H.). Volumetric Estimation of Antimony in Presence of TinARCHBUTT (L.).Analysis of Oils .FINPENER . Distinction of Castor Oil from other Fatty Oils .PAGE30330413043 M304305305306306306307307307308308309309309310310310310311311311312312396396396396397397397398398398398399399MO400401401401M.24024024034!034044044QCONTENTS .JUNGPLEISCH (E.). Quinine Sulphate .LIEBMANN (A.) and STUDER . Detection of Rosaniline Salts .DE REGO (J . H.). Detection of Acid Coal-tar Colours in Wine .HOPPE-SEYLER (G.) . Discriminating between Chrysophanic Acid and San-tonin Colouring Matters in Urine .SCHMIDT (M . v.) and P . ERBAN .SAUL (J . E.). Test for Tannin .PALM (R.). Detection of Traces of Albumin .ERASSER (I?.).Presence of Albumin in Vegetable Tissues : MicrochemicalTest for AlbuminoYds .DANNENBERG (E.). Detection of Blood Stains in Presence of Iron Rust .Separation of ResinsOTT (A.). Separation of Globulin from Albumin in Urine .AMTHOR (0.). Dannenberg's Hsemidin Crystals .HUGHES (J.). Analysis of Hoofs and Horns .CAMPBELL (E . D.). Estimation of Sulphur in Soluble SlagsWHITFIELD (J . E.). Indirect Determination of Chlorine, Bromine, andIodine .NETTLEFOLD (F.). Absorption of Nitric Oxide by Sulphuric Acid .MANPIEWICZ . Detection of Phosphorus .THILO (E.). Estimation of Phosphoric Acid from the Weight of the Mo-lybdate Precipitate .ISBERT (A.) . Estimation of Phosphoric Acid .LAIBLE . Estimation of Phosphoric Acid .SCHNEIDER (L.). Determination of Phosphorus in Iron and Steel .BRUNNEMANN (C.). Determination of Phosphorus in Basic Slag .LOQES (G.). Determination of Phosphoric Acid in Basic Slag .STRICK (a . H.). Estimation of Silicon in Iron .MARCET (W.). Volumetric Estimation of Carbonic Anhydride .KUHLMANN (E.). Determination of Normal Carbonates in " Bicarbo-nate~.~' .GOOCH ( F . A.). Separation of Sodium and Potassium from Lithium, Mag-nesium, and Calcium .LUCPOW (C.). Separation of Metals by Oxalic Acid .STAHL (IT.). Analysis of Copper .KNORRE ((3 . v.) . Employment of Nitroao-a-naphthol in QuantitativeAnalysis .HERZ (J.). Detection of Alum in Flour .BAYEE (K . J.). Detection of Free Sulphuric Acid and of AluminiumMEINECPE (C.). Volumetric Determination of Manganese .WARREN (H . N.). Use of Electro-dissolution in Analysis .WARREN (T . T . P . B.). Detection of Adulteration in Metallic Nickel andother Metals by the Magnet .DONATH (E.) and R . JELLER . Detection and Determination of Traces ofChromium .VENATOR (W.) and E . ETIENNE . Analysis of Chrome Iron Ore .CARNELLEY (T.) and W . MACPIE . Determination of Organic Matter inAir .ZAMBELLI (L.). Colorimetric Determination of Nitrites in Water .EOBRICH (A.). Determination of Organic Matter in Natural Water .AGOSTINI ( C . ) . Detection of Dextrose .IHL (A.). Colour Reactions of Beet-sugar .TOLLENS (B.). Behaviour of Sugar towards Acids and Phenol .IHL (A.). Colour Reactions of Starch and Gum .VOLCPER (0.). Determination of Hippuric Acid in Urine .LEVALT~IS (A.). Characteristics of Olive Oil .LEONE (T.) and A . LONGI .DRAPER (H . N.). and C . DRAPER . Behaviour of Alkaline Solutions of .HOPPE-SEYLEB (F.). Estimating Hvdrogen in the Presence of Methane ..Hydroxide in Aluminium Sulphate .Properties of Olive, Sesame, and Cotton OilsPhenolphthaleYn in Presence of Alcoholx1 vPAGE405405m540640640640'74074084084085255265265265265265265275275275275285285285 295205305305305315315315315325325335335345345345345355355366186184406. V Y xlvi CONTENTS .KALMANN (W.) . Standardising Iodine Solutions : estimating SulphurousWEIL (F.). Vclumetric Estimation of Sulphides .BABBITT (1% . C.). Manganese in Steel and Iron .DONATH (E.). Decompoeition of Chrome Iron Ore .FOLKARD (C . W.). Bacteriological Examination of Water .BURQHARDT (C . A.). Determination of Organic Carbon and Nitrogen inWaters .LAUBE (G.). Decolorisiiig Power of Bone-black .WUESTER ((3.). Quantitative Estimation of Wood in Paper .BENEDIKT (R.) and F . ULZEB . Investigation of Acetyl Compounde, : NewAcid in Presence of Thiosulphuric Acid .Method for the Analysis of Fats .ROSE (B.). Analysis of Fats .CORNWALL (H . B.). Examination of Butter Colours .BLAREY (C.) and Gt . DENIG~S . Estimation of Uric Acid by Potassium Per-PLUGGE (P . C.). Volumetric Estimation of Acids in Salts of the Alka-loids .ADRIAN and E . GALLOIS . Assay of Opium .SCHLICKUM (0.). Estimation of Morphine .SCHAFER (L.). Estimation of Cinchonidine in Quinine Sulphate .SCHLICEUM (0.). Testing Quinine Sulphate .FLECK (H.) Colour Reactions of Picric Acid and Dinitrocresol .MACAQNO (J.). Determination of Tannin in Bumach .FRANCEE (B.). New Gas Burette .LEYBOLD (W.). Burette J e t .BRAND (A.). Use of “ Solid Bromine ’’ in AnalysisTOPF ((3.). Iodometric Studies .FLUCEIGER (F . A.). Reaction of Thiosulphates .BRAGARD (M.). Zinc Determination .DITTE (A.). Estimation of Vanadic Acid .SPIEGEL (L.). Determination of Nitrates in Well Waters .TONY.GABCIN . Detection of Cane.sugar, Glucose, and Dextrin in Wines .MOLISCH (H.). New Test for Conferin .FRIEDHEIM (C.). Weil’s Method of Determining Sulphides .VILLIERS (A.). Detection of Sulphites in Presence of Thiosulphates .JACKSON (C . L.) and GF . W . ROLFE . Quantitative Determination of Hy-manganat e ..L’EOTE (L.). Detection and Estimation of Aluminium in Wine and inGrapes .droxvl .DIEZ (R.\. Quantitative Estimation of Glycerol .LINDO (D.). New Sugar Reactions .CRAMPTOB (C . A.). Analyses of Sugar-cane and Beet Juices .MACNAIB (D . S.). Separation of Acetic and Formic Acids .SHORT ( F . (3.). Analysis of Milk .MORSE (H . N.) and C . PIGGOT . Determination of Butter in Milk .BLOXAM (C . L.). Colour Tests for Strychnine and other AlkaloYds .HAGER (H.). Guaiac Resin .THOMAS (H.). Estimation of Hydrogen Peroxide .SALZER (‘T.). Volumetric Estimation of Iodine .Determination of Sulphuric Acid in Water .RAULIN . Estimation of Nitrogen in Organic Substances .ULSCH (K.). Kjeldahl’s Method. for Estimating Nitrogen .GARNIER (L.). Estimation of Nitrogen in Urine .GASBAUD . Organic Nitrogen in Chemical Manures .MOHB (C.) Estimation of Phosphoric Acid .KRETZSCHMAR (M.). Detection of Boron in Milk, &c .HOLDERMA.” (E.). Estimation of Sodium and Lithium .BERNARD (A.). Cdcimetry .FRICEE .KRETZSCHMAR (M.). Estimation of Potassium in Ashes and Minerals .PAGE61861861961961961961962062062162162162162262262362362462468768868868868968969069169169269274974974975075175175175175275275286286286286286386386386486486486486CONTENTS . xlviiSTOLBA (E.). Determination of Calcium and Magnesium in presence of Man-ganese .KUPFERSCHLBGER . Titration of Zinc Powder .GATENBY (R.). Volumetric Estimation of Alumina .WEDDINQ . Estimation of Phosphorus inIron .BRAND (C.). Determination of Combined Carbon in Iron .KEHRMANN (F.). Separation of Phosphoric Acid from Tungstic Acid .DBAGENDOEFF (G.) and €I . TIENSENHAUSEN . Ciloral Hydrate .DRAQEWDORFF (G.) and W . JACOBSON . Isolation and Detection ofPheuol .EPFRONT (J.). Estimation of Starch and Sugars .ASBOTH (A . v.). Estimation of Starch .UIRARD (A.). Estimation of Starch in Potatoes .SONNENSCHEIN (A.). Estimation of Acetic Acid in Acetates by DirectTitration .GOEBEL (H.). Estimation of Morphine .VULPIUS (G.). Morphine Reaction .DRAGENDORFF (G.) and E . BLUMENBACH . Thallin .RENARD (A.). Estimation of Indigo in Textile Fabrics .KOCH (R.). Determination of the Free Acid in Tannin Liquor by Titra-tion .VILLON . New Method €or the Estimation of Tannin .GARNIER (L.). Escimrttion of Albumino’ids in Liquids from Cysts, &c .JTLUCEIGER (F . A.). Iodine Determination in Laminaria .TOPF (G .. ). Iodometric Studies .WEIL (F.). Estimation of Sulphides .LUNGE (G) . Detection of Nitrogen Compounds in Seleniferous SulphuricAcid .BLUNT (T . P.). A Simple Nitrometer .OSMOND (F.). Colorimetric Estimation of Phosphorus .SIDERSEY . Apparatus for Determining Carbonic Anhydride in Carbo-nates .PETTERSON (0.) and A . PALMQUIST . Portable Apparatus for the Estima-tion of Carbonic Anhydride in the Atmosphere .FLUCKIQER (I? . A.) . Lithium Carbonate .WEIL (F.). Titration of Zinc Powder . , .SCHAND (A.). Electrolysis of Copper and Zinc .KLEIN (J.). Estimation of Formic Acid and of Organic Matter in Water .TOLEER (0.). Determination of Hippuric Acid in Urine .GAWALOWSEI (A.) .FEDERER (E . C.). Test for Oil of Peppermint .HELBING (H.). Reaction of Strophanthin .BIRD (F . C . J.). A Filter Tube for Use in the Estimation of Alkaloi‘ds byMayer’s Reagent .LOSCH (A.). The’ine Estimation .PAUL (B . H.) and A . J . COWVNLEY . Coffee .PADB (L.). Analyses of Coffee .BLUM (L.). Detection of Albumin in Urine .PALM (R.). Determination of Milk Constituents .HEMPEL (W.). Source of Error in Gas Analysis .HEMPEL (W.). A Gas Burette which is Independent of Atmospheric Pres-sure and Temperature .MALOT . Estimation of Phosphoric Acid .KALMANN (W.) and J . SPULLER . Examination of Crude Soda Lyes andRed Liquors .LEVY (L.). Estimation of Titanic Acid .JOLLES (A.). New Chloroform Reaction .PLUGGE (P . C.). Test for Narce‘ine .Separation of Mineral Oils from Sapodable FatsMEHU (C.). Urea Estimation .MACKINTOSH (J . B.). Bas Apparatus .PAGE86586586586586686686686686786786886886986987087087187187187287299699799899899899999999910001000100010001001100110011001100110021002100210021003100310621062106310631064113xlviii CONTENTS .BREAL (E.). New Method of Testing for Nitrates .PAULY (C.). Detection of Potassium .FOCKE (H.). Determination of Alkaline Chlorides in Crude Potash .BAUDOIN . Testing Copper Sulphate .MEINEKE (C.). Analysis of Clay .MEINEKE (C.). Determination of Manganese .NEUMANN (G.). Determination of Metallic Iron in Slags .MORGAN (J . J.). Rapid Estimation of Silicon, Sulphur, and Manganese inIron and Steel .TURNER (T.). Estimation of Silicon in Iron and Steel .PLATZ (P.). Determination of Sulphur in Iron .MCCKJLLOCH (N.). Volumetric Estimation of Cobalt in Presence of Nickel .MACINTOSH (J . B.). Separation of Nickel and Cobalt from Iron .MOORE (T.). Precipitation of Nickel in Presence of Iron .Water Analysis .HEHNER (0.). Eitimaiion ok Methyl Alcohol in Presence of Ethyl AIcobol .FISCHER (B.) . Dimethyl Ethyl Carbinol .LEGLER (L.). Estimation of Glycerol .HEHNER (0.). Estimation of Glycerol and its Non-volatility with AqueousDAFERT (F . W.). Determination of Moisture in Starch .YOUNG (W . C.). Logwood Test for Alum in Bread .LINDE (0.). Estimation of Hydrocyanic Acid .ELASON (P.). Estimation of Thiocyanic Acid .CRAMPTON (C . A.) and T . C . TRESCOT . Estimation of Carbonic Acid inBeer .KOCH (R.). Estimation of Free Acid in Tannin Liquor .FARER (H.). Determination of Fat in Milk .ALLEN (A . H.). Reichert’s Distillation Process .CAMPANI ((3.). Volumetric Estimation of Urea .HESSE (0.). Estimation of Quinine Sulphate .ALLEN (A . H.). Detection of Hop-substitutes in Beer .RANSOM (F.) . Estimation of Ipecacuanha .Detection of Aniline Colours iii WineMANNLEY (G.). Estimation of Indigo .LENZ (W.). Testing Indigo Dyes on Fabrics .MARTIN (E . W.).MYLIUS (F.). Pettenkofer’s Reaction .Vapour .EERNER (G.) and A . WELLER . Testing Quinine Sulphate .CURTMAN (C . 0.).Detection of Artificial Colouring Matters in Butter .LIEBERMANN (L.). Detection of Albumin in Urine .PAGE113811381138113911391139114011401140114111411141114111411142114211421143114311431143114411441144114411451145114511461146114711471147114711491149114

ISSN:0368-1769    

DOI:10.1039/CA88752FP001

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

INORGAXIC CHEMISTRY. I n or g a n i c C h e m i s t r y . 11 Conversion of Calcium Hypochlorite into Calcium Chlorafe. By G. LUNGE (J. SOC. Chem. h d , 4, 722--724).-1t has already been shown by the author that the reaction 6Ca0C12 = 5CaC12 + Ca(C10& does not take place completely and without considerable loss of oxygen, except in presence of an excess of chlorine, idthough that chlorine does not appear in the equation. The author’s experiments point to the following conclusions :-The most13: ABSTRAOTS OF CHEMICAL PAPERS. favourable way of converting hypochlorite into chlorate is t o raise the temperature of the solution, and simultaneously have an excess of chlorine present therein. A large excess of chlorine is useless, perhaps i-sjurions, for the yield of chlorate.On the large scale, it is not necessary to raise the temperature by artificial means, the heat produced by the reaction being sufficient to complete it. The con- version at the ordinary temperature proceeds almost at once to the limit of about 70 per cent., but subsequently makes very slow pro- gress, so that it is impracticable to wait for its completion without heating. D. B. A Crystalline Silico-carbonate from Soda Liquors. By C. RAMMELSBERG (CYhem. Id., 9, 110-11 l).-Two specimens of crystals removed from the pump of a carbonating tower at the " Hermannia " Chemical Works at Schonebeck had the following composition :- COz. Si02. AlZO3. CaO. Na,O. HzO. I. 22.75 14-99 7.38 13.28 22-37 19.23 = 100 11. 21.50 15-00 8.03 12.41 21.66 21.40 = 100 Allowing for adhering soda liquor, these numbers lead to the formula Na18Ca6A12(Si,C)210R3 + 3oH20, or the substance is a, com- pound of the isomorphous normal carbonates and silicates 3 [3Nh( Si, C) 0,,2Ca (Si, C) Oy ],2A1( Si, C),O,,.The crystals are rhombic, exhibiting the form of the primary pyramid with its acuter terminal edges truncated, or frequently a tabular form due to the development of the end face ; the ratio of the axes is 0.5295 : 1 : 1.73. These crystals were first observed in 1880, but the specimen then analysed contained an admixture of gay-lussite, and the silica and alumina were not recognised as essential constituents. X. J. $. Sodium-calcium Carbonates from the Soda, Manufacture. By C. REIDEMEISTER (Chem. Ind., 9, lll).-In the Chemische Iyadustrie for 1884 the author described the rhornbic crystals analysed by Ram- melsberg (see preceding Abstract) as a hydrated sodium calcium carbonate.They are now found to occur in both the crude and car- bonated liquors. In the former, in which formerly only gay-lussite had been recognised, they have now been observed with crystals of gay-lussite deposited on their surfaces. The gay-lussite crystals are chiefly deposited from liquors in process of cooling; the silico- carbonate from those undergoing slow evaporation. M. J. S. Double Nitrites of Caesium and of Rubidium. By T. ROSEN- BLADT (Bey., 19, 2531-2535).-The double nitrite of cesium and eobalt, ~CSNO,CO(NO~)~ + H20! is formed by boiling equal parts of cvbztlt nitrate and sodium acetate in water (15 parts), filter- ing, and adding to the cold solution first acetic acid (20 parts), and then a, strong solution of sodium nitrite until tho liquid has an orange cdour, it irs then filtered, and treated with a solution of aINORGANIC OHEMISTRT.13 eaesium salt. The double salt 3RbN02,Co(N02), + HzO is prepared in a similar manner. They are both lemon-coloured crystalline salts, and resemble in their behaviour Fischer's potassium-compound, except in their solubility in water, the czesium salt dissolving only in 20,100 parts of water at 17", and the rubidium salt in 19,800 parts of water. The method employed in analysing these compounds is described. Thallium also yields a double salt with cobalt nitrite ; it is a red crystaliine compohd, soluble in 23,810 pai.ts of water. . N.H. M. Decomposition of Glass by Carbonic Anhydride condensed on its Surface. By R. BUNSEN (Ann. Phys. Chem. [2], 29, 161- 165) .-Formerly the author attributed the absorption of carbonic anhydride by glass-wool rather to an interpenetration of the glass by the molecules of the liquefied gas rather than to any chemical change (Abutr., 1884, 146). This view would also be confirmed by the obser- vations on the stability of glass towards the most concentrated hydro- chloric acid. However, if the glass-wool be damp, whereby the absorption of the gas is remarkably increased (Abstr., 1885, 867), the possibility of a chemical change is not precluded. Accordingly the glass (49.453 grams) used in the experiment was exhausted with water, and a residue obtained from it corresponding to the decompo- sition of 2.882 grams of glass, or 5-83 per cent.of the whole. Even if the chemical change consists in the production at first of sodium carbonate, which would take up a further quantity of carbonic anhydride, corresponding with the formation of sodium hydrogen carbonate, which on subsequent heating would again be driven off, yet all the carbonic anhydride absorbed caunot be accounted for in this way. The phenomenon is thus not only one of chemical change, but also of absorption, the particular degree of each of which cannot be estimated. If, then, carbonic acid can decompose glass, the same is to be expected of water. Observations in the course of experiments on the determination of the tension of aqueous vepour at high temperatures are quoted to show that glass tubes containing water-vapour when heated at 88" are converted into n white porcelain-like mass, and that their inner diameter is diminished by one-tenth.Note.-On the decomposition of glass by carbonic anhydride under high pressures compare Pfaundler (Abstr., 1885, 868). Purification O f Yttria. By L. DE BOISBAUDRAN (Compt. rend., 103, 627-629).-A comparatively very pure sample of yttria was sub- jected to 32 series of fractionations by means of ammonia. The product of the last precipitation of the thirty-second series showed 8 less brilliant fluorescence than the original earth, and the bands of Za and 2/3 in the spectrum had diminished considerably in intensity, whilst the bands of samarium retained their original vigour. The colour of the fluorescence had changed from y ellowish-green to orange- yellow.This last precipitate was submitted to 26 series of fractionations by meam of oxalic acid. The brilliancy of the fluorescence continu- V. H. V. V. H. V.14 ABSTRACTS OF CHEMICAL PAPERS. ally diminished, but, contrary to the phenomena observed during the first fractionation, the samarium bands diminished in intensity much more rapidly than the bands of Za and ZP. The earth from the oxalate precipitated at the end of the fifth fractionation showed very faintly the citron band and the double green band of Za and ZP, with a trace of the red bands of samarium. The oxalate from the twenty-sixth fractionation yielded a very white earth which showed a trace of the citron band of Za, but none of the red, green, blue, and violet bands in the spectrum described by Crookes.This yttria gave no fluorescence when mixed with lime, but its hydrochloric acid solution gave a brilliant spark spectrum of yttrium. The sulphate prepared from the last precipitate f ~ o m the fractiona- tion with oxalic acid gave a rose-coloured fluorescence due to the presence of a trace of bismuth. Heating and Cooling of Cast Steel. By OSMOND (Compt. rend., 103, 743-746) .-The phenomena which accompany the heating and cooling of cast steel were investigated by means of a thcrmo- electric couple connected with an aperiodic galvanometer. Barrett observed that when a bar of hard iron is cooled from a white heat there is a sudden development of heat at dull redness, and the magnetic properties of the iron change abruptly.He distin- guished this phenomenon by the name recalescence. Chatelier and Yinchon found that at about 700" a molecular modification of pure iron is formed. The author's experiments show that as the proportion of carbon increases from 0.16 to 1-25 per cent. the temperature at which the molecular alteration takes place falls, whilst the point of recalescence rises, until in hard steel the t v o points coincide. The rate at which heating takes place has no influence on the temperature at which the two changes take place, but these temperatures are affected by the rate of cooling, and are lower the greater the rapidity with which cooling takes place. In quick tempering, no such phenomena are observed ; the heat corresponding with the non-effected changes remains in the iron.The two critical points also fall somewhat if the initial tem- perature of heating is raised. During annealing after tempering, the latent heat of tempering is liberated gradually and not abruptly. By T. KNIESCHE (Chenz. Zeit., 10, 1067--1068).-1n treating tungsten ores, sodium tungstate is first obtained, then from this tungstic acid, which i n its turn is reduced at a temperature of 1600" to metallic tungsten. The preparation of the chemically pure metal is simply a question of time; any way, as obtained at present, it is useful in steel making. It must be added only when the irou is in it perfectly fluid state. Sodium tungstate is used for rendering inflam- mable materials fireproof. C. H. B. C. H. R. Tungsten. D.A. L. Titanium. By 0. v. PFORDTEN (AnnuZen, 234, 257--299).-The sulphides of those metals which have a strong affinity for oxygen cannot be obtained in the pure date by passing carbon bisulphide over the metallic oxides at a red heat, but they can be prepared by theINORGANIC CEEMISTRY. 15 action of pure sulphuretted hydrogen on the metallic chlorides. The gas must be passed through chromons chloride to remove traces of oxygen, and is then dried by means of phosphoric oxide. The author disputes Thorpe's statement (Trans., 1885, 492) that sulphuretted hydrogen can be dried by passing thegas through sulphuric acid. At the ordinary temperature, sulphure tted hydrogen reduces titanic chloride to titanous chloride ; at a higher temperature, a compound is precipitated, which is probably a sulphochloride.Crystals of titanium disulphide, TiS2, are deposited when sulphuretted hydro- gen and the vapour of titanium tetrachloride are passed through a red-hot tube from which atmospheric air has been carefully expelled. The bisulphide is not attacked by hydrogen at a red heat in the presence of an excess of sulphuretted hydrogen. A t a red heat, it is oxidised completely by carbonic anhydride, and it splits up into the sesquisulphide, Ti2&, and sulphur in an atmosphere of hydro- gen or nitrogen. The sequisulphide is a metallic grey substance, insoluble in sodium hydroxide solution; it dissolves in nitric and strong sulphuric acids with a green coloration. The author is of opinion that the sesquisulphide described by Thorpe (Zoc.cit.) is an impure Rubstance, and that its green colour is due to the presence of vanadium. The sesquisulphide is reduced to monosulphide by hydrogen a t a higher temperature than that at which refractory glass softens. The crystals of the monosulphide are dark red. Dilute nitric acid attacks the monosulphide with difficulty ; in other respects, this substance Atomic Weight of Germanium. By L. DE BOISBAUDRAN (Corn@. rend., 103, 452--453).-Winkler's recent determination of the atomic weight of germanium, 72.32 (hbstr., 1886, 985), agrees perfectly with the value calculated by the author from the wave-lengths of the lines in the germanium spectrum (Abstr., 1886, 768). The law of proportionality between the variations in the atomic weights of the elements, and the variations in the wave-lengths of the lines in their respective spectra, thus receives further confirmation.resembles the sesquisulphide. w. c. w. C . H. B. Gold Oxides. By G. K R ~ S S (Bey., 19, 2541--9549).-Aurons oxide, Au20, could not be obtained in the pure state by any of the known methods. It is prepared by treating the double bromide of gold with aqueous sulphurous acid at 0" until the intense red colour of the bromide has disappeared. The colourless solution of aurous bromide so formed is warmed with potash, which causes a separation of aurous hydroxide. The oxide is dark violet when moist, greyish- violet when dry ; when freshly precipitated, it dissolves in cold mater, yielding an indigo-coloured solution with a brownish fluorescence ; it is insoluble in hot water.The solution has a characteristic absorp- tion spectrum showing a band at X = 587.0. Hydrochloric and hydrobromic acids convert it into gold and the corresponding auric compounds ; other acids have no action. The hydroxide parts with water at 200", and at 2.50" gives up its oxygen. Aurosoauric oxide, Autoz (compare Schottlander, Abstr., 1883,853),16 ABSTRACTS OF C€€EMICAL PAPERS. 70". -- 81-0 31'0 12.0 - is prepared by gradually heating pure auric hydroxide up to 160" until the weight remains constant. It is a fine dark yellowish- brown powder, is very hygroscopic, and can only be kept over phosphoric anhydride. When heated above 173", it gives off oxygen. Auric oxide, AuZ03, is conveniently obtained by treating auroauric chloride (1 part) with water (50 part's), boiling the solution, and adding finely powdered magnesia nlba, stirring the whole time, until the red colour of the auric chloride has disappeared.The gold trihydroxide is filtered, mixed with water (20 parts), treated with nitric acid, sp. gr. 1.4 (10 parts), and left for 24 hours. The residue, after filtering, is mixed with an equal amount of water and nitric acid, and heated for six hours at 100". The undissolved portion is now free from magnesia, and is washed with water to remove nitric acid. The pure auric hydroxide has a yellowish-brown colour when moist, and is rather readily soluble in nitric acid. When kept for weeks over phosphoric anhydride, it is converted into aurylic hydroxide, AuO*OH, and when carefully heated yields auric oxide.The so-called " purple oxide of gold " appears to be gold in a finely divided state. The author was unable to obtain Prat's gold siiperoxide and Figuier's auric acid (Compt. rend., 70, 844), or any other oxide of gold than the three described. This behaviour of gold is in accord- ance with the position (between platinum and mercury) assigned to it in the periodic arrangement of the elements. Solubility of some Gold Compounds. By T. ROSEKBLADT (Bw., 19, 2535--2538).-The following table shows the amounts of the anhydrous double salts contained i n 100 pnpts by weight of aqueous solution at the given temperatures :- N. H. M. 80". - I 85.7 35.3 16.3 -- 1 10". 60.2 57'7 38.2 9.0 0 - 8 NaAuC1, LiduC4 RbAuC1, KAuC14 CsAuCl4 64.0 62.5 48-7 13.4 1.7 69.4 67.3 59'2 17'2 3.2 20".1 30". 7'7-5 72.0 70.0 22.2 5.4 1 40". 1 50". 58 '2 53 -1 27 -7 4 . 6 0 . 5 60". 90 *o 76 -4 80 *2 26 -6 8 - 2 90". - 39 -7 21 -7 looo. - 44.2 2'7 -5 ~~~~ ~ ~ ~ ~~~~~~~~~~~ The solubilities of the double salts (with exception of the lithium salt) are inversely proportional to the molecular weights of the salts. N. EL. M.INORGAXIC CHEMISTRY.I n or g a n i c C h e m i s t r y .11Conversion of Calcium Hypochlorite into CalciumChlorafe. By G. LUNGE (J. SOC. Chem. h d , 4, 722--724).-1t hasalready been shown by the author that the reaction 6Ca0C12 =5CaC12 + Ca(C10& does not take place completely and withoutconsiderable loss of oxygen, except in presence of an excess ofchlorine, idthough that chlorine does not appear in the equation.Theauthor’s experiments point to the following conclusions :-The mos13: ABSTRAOTS OF CHEMICAL PAPERS.favourable way of converting hypochlorite into chlorate is t o raise thetemperature of the solution, and simultaneously have an excess ofchlorine present therein. A large excess of chlorine is useless,perhaps i-sjurions, for the yield of chlorate. On the large scale, it isnot necessary to raise the temperature by artificial means, the heatproduced by the reaction being sufficient to complete it. The con-version at the ordinary temperature proceeds almost at once to thelimit of about 70 per cent., but subsequently makes very slow pro-gress, so that it is impracticable to wait for its completion withoutheating. D. B.A Crystalline Silico-carbonate from Soda Liquors.By C.RAMMELSBERG (CYhem. Id., 9, 110-11 l).-Two specimens of crystalsremoved from the pump of a carbonating tower at the " Hermannia "Chemical Works at Schonebeck had the following composition :-COz. Si02. AlZO3. CaO. Na,O. HzO.I. 22.75 14-99 7.38 13.28 22-37 19.23 = 10011. 21.50 15-00 8.03 12.41 21.66 21.40 = 100Allowing for adhering soda liquor, these numbers lead to theformula Na18Ca6A12(Si,C)210R3 + 3oH20, or the substance is a, com-pound of the isomorphous normal carbonates and silicates3 [3Nh( Si, C) 0,,2Ca (Si, C) Oy ],2A1( Si, C),O,,.The crystals are rhombic, exhibiting the form of the primarypyramid with its acuter terminal edges truncated, or frequently atabular form due to the development of the end face ; the ratio of theaxes is 0.5295 : 1 : 1.73.These crystals were first observed in 1880, but the specimen thenanalysed contained an admixture of gay-lussite, and the silica andalumina were not recognised as essential constituents.X. J. $.Sodium-calcium Carbonates from the Soda, Manufacture.By C. REIDEMEISTER (Chem. Ind., 9, lll).-In the Chemische Iyadustriefor 1884 the author described the rhornbic crystals analysed by Ram-melsberg (see preceding Abstract) as a hydrated sodium calciumcarbonate. They are now found to occur in both the crude and car-bonated liquors. In the former, in which formerly only gay-lussitehad been recognised, they have now been observed with crystals ofgay-lussite deposited on their surfaces. The gay-lussite crystals arechiefly deposited from liquors in process of cooling; the silico-carbonate from those undergoing slow evaporation.M. J. S.Double Nitrites of Caesium and of Rubidium. By T. ROSEN-BLADT (Bey., 19, 2531-2535).-The double nitrite of cesium andeobalt, ~CSNO,CO(NO~)~ + H20! is formed by boiling equal partsof cvbztlt nitrate and sodium acetate in water (15 parts), filter-ing, and adding to the cold solution first acetic acid (20 parts),and then a, strong solution of sodium nitrite until tho liquid has anorange cdour, it irs then filtered, and treated with a solution of INORGANIC OHEMISTRT. 13eaesium salt. The double salt 3RbN02,Co(N02), + HzO is preparedin a similar manner. They are both lemon-coloured crystalline salts,and resemble in their behaviour Fischer's potassium-compound, exceptin their solubility in water, the czesium salt dissolving only in20,100 parts of water at 17", and the rubidium salt in 19,800 parts ofwater.The method employed in analysing these compounds isdescribed.Thallium also yields a double salt with cobalt nitrite ; it is a redcrystaliine compohd, soluble in 23,810 pai.ts of water..N. H. M.Decomposition of Glass by Carbonic Anhydride condensedon its Surface. By R. BUNSEN (Ann. Phys. Chem. [2], 29, 161-165) .-Formerly the author attributed the absorption of carbonicanhydride by glass-wool rather to an interpenetration of the glass bythe molecules of the liquefied gas rather than to any chemical change(Abutr., 1884, 146). This view would also be confirmed by the obser-vations on the stability of glass towards the most concentrated hydro-chloric acid.However, if the glass-wool be damp, whereby theabsorption of the gas is remarkably increased (Abstr., 1885, 867),the possibility of a chemical change is not precluded. Accordinglythe glass (49.453 grams) used in the experiment was exhausted withwater, and a residue obtained from it corresponding to the decompo-sition of 2.882 grams of glass, or 5-83 per cent. of the whole.Even if the chemical change consists in the production at first ofsodium carbonate, which would take up a further quantity of carbonicanhydride, corresponding with the formation of sodium hydrogencarbonate, which on subsequent heating would again be driven off, yetall the carbonic anhydride absorbed caunot be accounted for in thisway.The phenomenon is thus not only one of chemical change, butalso of absorption, the particular degree of each of which cannot beestimated.If, then, carbonic acid can decompose glass, the same is to beexpected of water. Observations in the course of experiments on thedetermination of the tension of aqueous vepour at high temperaturesare quoted to show that glass tubes containing water-vapour whenheated at 88" are converted into n white porcelain-like mass, and thattheir inner diameter is diminished by one-tenth.Note.-On the decomposition of glass by carbonic anhydride underhigh pressures compare Pfaundler (Abstr., 1885, 868).Purification O f Yttria. By L. DE BOISBAUDRAN (Compt.rend., 103,627-629).-A comparatively very pure sample of yttria was sub-jected to 32 series of fractionations by means of ammonia. Theproduct of the last precipitation of the thirty-second series showed8 less brilliant fluorescence than the original earth, and the bands ofZa and 2/3 in the spectrum had diminished considerably in intensity,whilst the bands of samarium retained their original vigour. Thecolour of the fluorescence had changed from y ellowish-green toorange- yellow.This last precipitate was submitted to 26 series of fractionationsby meam of oxalic acid. The brilliancy of the fluorescence continu-V. H. V.V. H. V14 ABSTRACTS OF CHEMICAL PAPERS.ally diminished, but, contrary to the phenomena observed during thefirst fractionation, the samarium bands diminished in intensity muchmore rapidly than the bands of Za and ZP.The earth from the oxalateprecipitated at the end of the fifth fractionation showed very faintlythe citron band and the double green band of Za and ZP, with a traceof the red bands of samarium. The oxalate from the twenty-sixthfractionation yielded a very white earth which showed a trace of thecitron band of Za, but none of the red, green, blue, and violet bands inthe spectrum described by Crookes. This yttria gave no fluorescencewhen mixed with lime, but its hydrochloric acid solution gave abrilliant spark spectrum of yttrium.The sulphate prepared from the last precipitate f ~ o m the fractiona-tion with oxalic acid gave a rose-coloured fluorescence due to thepresence of a trace of bismuth.Heating and Cooling of Cast Steel.By OSMOND (Compt. rend.,103, 743-746) .-The phenomena which accompany the heating andcooling of cast steel were investigated by means of a thcrmo-electric couple connected with an aperiodic galvanometer.Barrett observed that when a bar of hard iron is cooled from awhite heat there is a sudden development of heat at dull redness, andthe magnetic properties of the iron change abruptly. He distin-guished this phenomenon by the name recalescence. Chatelier andYinchon found that at about 700" a molecular modification of pureiron is formed.The author's experiments show that as the proportion of carbonincreases from 0.16 to 1-25 per cent. the temperature at which themolecular alteration takes place falls, whilst the point of recalescencerises, until in hard steel the t v o points coincide.The rate at whichheating takes place has no influence on the temperature at which thetwo changes take place, but these temperatures are affected by the rateof cooling, and are lower the greater the rapidity with which coolingtakes place. In quick tempering, no such phenomena are observed ;the heat corresponding with the non-effected changes remains in theiron. The two critical points also fall somewhat if the initial tem-perature of heating is raised. During annealing after tempering, thelatent heat of tempering is liberated gradually and not abruptly.By T. KNIESCHE (Chenz. Zeit., 10, 1067--1068).-1ntreating tungsten ores, sodium tungstate is first obtained, then from thistungstic acid, which i n its turn is reduced at a temperature of 1600"to metallic tungsten.The preparation of the chemically pure metalis simply a question of time; any way, as obtained at present, it isuseful in steel making. It must be added only when the irou is in itperfectly fluid state. Sodium tungstate is used for rendering inflam-mable materials fireproof.C. H. B.C. H. R.Tungsten.D. A. L.Titanium. By 0. v. PFORDTEN (AnnuZen, 234, 257--299).-Thesulphides of those metals which have a strong affinity for oxygencannot be obtained in the pure date by passing carbon bisulphideover the metallic oxides at a red heat, but they can be prepared by thINORGANIC CEEMISTRY.15action of pure sulphuretted hydrogen on the metallic chlorides. Thegas must be passed through chromons chloride to remove traces ofoxygen, and is then dried by means of phosphoric oxide. The authordisputes Thorpe's statement (Trans., 1885, 492) that sulphurettedhydrogen can be dried by passing thegas through sulphuric acid. Atthe ordinary temperature, sulphure tted hydrogen reduces titanicchloride to titanous chloride ; at a higher temperature, a compoundis precipitated, which is probably a sulphochloride. Crystals oftitanium disulphide, TiS2, are deposited when sulphuretted hydro-gen and the vapour of titanium tetrachloride are passed througha red-hot tube from which atmospheric air has been carefullyexpelled. The bisulphide is not attacked by hydrogen at a red heatin the presence of an excess of sulphuretted hydrogen.A t a redheat, it is oxidised completely by carbonic anhydride, and it splits upinto the sesquisulphide, Ti2&, and sulphur in an atmosphere of hydro-gen or nitrogen. The sequisulphide is a metallic grey substance,insoluble in sodium hydroxide solution; it dissolves in nitric andstrong sulphuric acids with a green coloration. The author is of opinionthat the sesquisulphide described by Thorpe (Zoc. cit.) is an impureRubstance, and that its green colour is due to the presence ofvanadium.The sesquisulphide is reduced to monosulphide by hydrogen a t ahigher temperature than that at which refractory glass softens. Thecrystals of the monosulphide are dark red.Dilute nitric acid attacksthe monosulphide with difficulty ; in other respects, this substanceAtomic Weight of Germanium. By L. DE BOISBAUDRAN (Corn@.rend., 103, 452--453).-Winkler's recent determination of the atomicweight of germanium, 72.32 (hbstr., 1886, 985), agrees perfectly withthe value calculated by the author from the wave-lengths of thelines in the germanium spectrum (Abstr., 1886, 768). The law ofproportionality between the variations in the atomic weights of theelements, and the variations in the wave-lengths of the lines in theirrespective spectra, thus receives further confirmation.resembles the sesquisulphide. w. c. w.C . H. B.Gold Oxides. By G. K R ~ S S (Bey., 19, 2541--9549).-Auronsoxide, Au20, could not be obtained in the pure state by any of theknown methods.It is prepared by treating the double bromide ofgold with aqueous sulphurous acid at 0" until the intense red colourof the bromide has disappeared. The colourless solution of aurousbromide so formed is warmed with potash, which causes a separation ofaurous hydroxide. The oxide is dark violet when moist, greyish-violet when dry ; when freshly precipitated, it dissolves in cold mater,yielding an indigo-coloured solution with a brownish fluorescence ; itis insoluble in hot water. The solution has a characteristic absorp-tion spectrum showing a band at X = 587.0. Hydrochloric andhydrobromic acids convert it into gold and the corresponding auriccompounds ; other acids have no action. The hydroxide parts withwater at 200", and at 2.50" gives up its oxygen.Aurosoauric oxide, Autoz (compare Schottlander, Abstr., 1883,853)16 ABSTRACTS OF C€€EMICAL PAPERS.70".--81-031'012.0-is prepared by gradually heating pure auric hydroxide up to 160"until the weight remains constant. It is a fine dark yellowish-brown powder, is very hygroscopic, and can only be kept overphosphoric anhydride. When heated above 173", it gives off oxygen.Auric oxide, AuZ03, is conveniently obtained by treating auroauricchloride (1 part) with water (50 part's), boiling the solution, andadding finely powdered magnesia nlba, stirring the whole time, untilthe red colour of the auric chloride has disappeared. The goldtrihydroxide is filtered, mixed with water (20 parts), treatedwith nitric acid, sp. gr. 1.4 (10 parts), and left for 24 hours. Theresidue, after filtering, is mixed with an equal amount of water andnitric acid, and heated for six hours at 100". The undissolvedportion is now free from magnesia, and is washed with water toremove nitric acid. The pure auric hydroxide has a yellowish-browncolour when moist, and is rather readily soluble in nitric acid. Whenkept for weeks over phosphoric anhydride, it is converted into aurylichydroxide, AuO*OH, and when carefully heated yields auric oxide.The so-called " purple oxide of gold " appears to be gold in a finelydivided state.The author was unable to obtain Prat's gold siiperoxide andFiguier's auric acid (Compt. rend., 70, 844), or any other oxide ofgold than the three described. This behaviour of gold is in accord-ance with the position (between platinum and mercury) assigned toit in the periodic arrangement of the elements.Solubility of some Gold Compounds. By T. ROSEKBLADT (Bw.,19, 2535--2538).-The following table shows the amounts of theanhydrous double salts contained i n 100 pnpts by weight of aqueoussolution at the given temperatures :-N. H. M.80".- I85.735.316.3--1 10".60.257'738.29.00 - 8NaAuC1,LiduC4RbAuC1,KAuC14CsAuCl464.062.548-713.41.769.467.359'217'23.220". 1 30".7'7-572.070.022.25.4140". 1 50".58 '253 -127 -74 . 60 . 560".90 *o76 -480 *226 -68 - 290".-39 -721 -7looo.-44.22'7 -5~~~~ ~ ~ ~ ~~~~~~~~~~~The solubilities of the double salts (with exception of the lithiumsalt) are inversely proportional to the molecular weights of the salts.N. EL. M

ISSN:0368-1769    

DOI:10.1039/CA8875200011

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

MINERALOGICAL CHEMISTRT. M i n e r a1 o g i c a1 C h em i s t ry. 17 Artificial Breithauptite from the Mechernich Lead Fur- naces. By A. BRAND (Zeit. Kryst. M ~ N . , 12, 234-239).-1n 1885 the author found a number of peculiar crystals in the clay used for stopping the tap-holes of the lead furnaces in which antimonial lead was smelted. They occur in all the furnaces ; the clay being pulverised and used again. It is therefore impossible to determine whether they were originally formed in the smelting of hard lead. The crystals were columnar, hexagonal prisms, 0.1 to 0.5 mrn. thick, and 5 to 26 mm. long. They were brittle, had an uneven fracture, adamantine lustre, steel-grey to copper-red colour, and greyish-brown streak. The hardness was 5 to 5.5, and the sp. gr. about 8.Analysis of carefully purified material gave the following results :- Sb. Ni. co. Pb. cu. Fe. Tntal. 65.46 29.67 1.12 1.39 0.16 1.45 99-25 The formula of the mineral ia thus NiSb. B. H. B. Chemical Composition of Butyrellite. By W. I. MACADAM (Min. Mag., 6, li5-180; Zeit. Kryst. Min., 12, 182).-Tn the in- vestigation of ten samples of bog-butter or butyrellite (Dana) from various localities in the peat bogs of Scotland and Ireland, the author found that the portion of the butyrellite soluble in ether corresponded in all respects with the substance obtained under like conditions from ordinary butter. This portion varies in the ten analyses from 91.52 to 98.94 per cent. The portion insoluble in ether, 0.38 to 4a.56 per cent., was slightly soluble in water, and gave evidence of the presence of milk-sugar.The portion insoluble in water contained nitrogen, and gave on combustion the peculiar odour of burning cheese. The ash or mineral portion, 0.01 to 0.36 per cent., contained traces of phos- phoric acid. These results, and the fact that a number of cow’s hairs were found in the samples, show that butyrellite has no claim to be called a mineral. It cannot be discussed how these masses found their way into the positions from which they are now obtained. It is, however, obvious that the material is not of mineral or even of resinous origin, but of undoubted animal derivation, and should therefore be erased from the list of minerals. B. H. B. Minerals from Vesuvius. By E. SCACCHI (Zeit. Rryst. Min., 12, 202-203).-1. Hydrogiobertite is the name given by the author to a new hydrated magnesium carbonate, which occurs in the form of grey, compact masses 2 to 15 mm.in diameter. With the lens, minute magnetite crystals are observed enclosed in the mass. The sp. gr. is 2.149 to 2,174. The loss on ignition amounted to 53.07 per cent. Of the sample, 0.507 gram contained 0.0025 gram of magnetite, and 0.022 gram of ferric oxide which was subtracted as limonite with the mag- netite. The results of the analysis were as follows :- VOL. LII. C18 ABSTRACTS OF OHEMICAL PAPERS. coz. MgO. H20. Total. 28-16 44.91 29.93 100~00 The formula of the new mineral is MgzCOa + 3H20. The? hydrogiobertite was discovered near Polleiia in a block of angitophyre very closely resembling lava. In the interior, the structnre was crystalline. On this Tock was a compact mixture of silicates (plagioclase, augite, and magnetite) with which the hydrogiobertite was associated.2. AZtered Aragonite.-In the mother-rock of the hydrogiobertite, described above, hexagonal prisms, 3-4 mm. long and 1-1.5 mm. broad were found. They are white and opaque, and for the most part soluble in acids ; the insoluble portion frequently preserving the original form of the crystal, or becoming divided longitudinally into prismatic fragments. On heating at 170", there wag a loss of 6.81 per cent. I n hydrochloric acid, 11.78 per cent. was insoluble; this portion was found to c6ntain 58.97 per cent. of silica with ferric oxide, alumina, and lime ; whilst the soluble portion consisted essentially of lime.The insoluble substance also occurs in the interior of the crystals. 3. Fluorspar.-A number of minute octahedral crystals occurring on a' lava from Pollena (187'3) were found to be fluorspar. This mineral has hitherto +en unknown in the lavas of Vesuvins and other volcanoes. Associated with the fluorspar are minute aciculw crystals of apatite. B. H. B. Chemical Constitution of Barytocalcite and Alstonite. By A. BECKER (Zeit. Kryst. Min., 12,222-227) .-The monoclinic baryto- calcite and the rhombic alstonite have hitherto been regarded as having the same chemical composition (BaC03 + CaCO,). The question now arises whether they should both be considered isomorph- ous mixtlures of BaCOs and CaCO,, or whether one of them is not a molecular compound of the two carbonatea with the formula BaCaC20s. Qroth regards barytocalcite as a moleciilar compound of this kind, whilst alstonite, he thinks, is an isomorphous mixture of equal amounts of the two salts.This view is confirmed experimentally by the author, who gives the following results of a series of analyses of the two minerals in question :- BaO. I. 30.09 11. 50.36 111. 51.59 IV. 44-69 V. 37.42 VI. 50.97 VII. 51.45 cso. 19.77 19.22 18-61 23.40 29.06 19 83 19.89 MnO. GOz. 0.35 29.52 0.25 29.44 0.35 29.39 0.29 31.71 0.30 32.21 - 29-65 0.20 29-52 Insol. ma. Total. - 99.73 0.30 99-37 0.28 103.22 - 100.09 - 98.98 0.25 100.70 I 101.06 All the specimens analysed were from Alston Moor. calcite, purchased from Pech of Berlin. I. Barytocalcite, purchased from Sturtz of Bonn.11. Baryto- 111. Bargtocalcite from theMINERALOGTCAL CHEMISTRY. 19 minem~ogica,l miasearn of the University of Leipziq. These three analpee correspond with the formula BaCO, + CaC03. IV. Alstonite from Pech of Berlin; formula, 3BaC0, + 4CsC0,. V. A second specimen of the same, formula BaCO, + 2CnCO3. VI. Alstonite, purchased from Gregory of London, formula BaC0, + CaCO,. VII. Alatonite from the mineralogical museum of the Uni- versity of Leipzig, formula BaC03 + CaC03. For the three specimens of barytocalcite analysed, the same formula (BaCO, + CaC03) is obtained; so that this mineral must be regarded as a, molecular compound ; whilst of the four specimens of alstonite analysed, two had the same formula (BaC03 + CaCO,), and the other two the formule 3BaCO3 + 4CaC0, and BaC03 + 2CaC03.Alston- ite, consequently, is undoubtedly an isomorphous mixture of the two carbonates. B. EL B. Chemical Composition of Herderite. By A. DES CLOIZEAVX and A. DAMOUR (Zeit. R y s t . Rfin., 12, ‘204).-Since Des Cloizeaux (Abstr., 1889, 827) establiahed the optical identity of the herdcrite crygtals from Sfoneham, Maine, and from Ehrenfriedersdorf, Saxony, C. Winkler (Abstr., 1884, 1102) bas given an analysis of the crystals from both localities, attributing tho loss to water, and not to fluorine. $ubseqnently F. A. Genth (Abstr., 1885, 488) found 8.93 per cent. of fluorine in the Stoneham herderite. These discordant rmults have induced the authors to make a fresh investigation, and their analysis ahowa the presence of a considerable amount of fluorine.The sp. gr. of the mineral examined was 2.98 (compare Abstr., 1885, 359). B. H, B. Minerals from Tuscany. By L. BUSATTI (Zeit. Kryst. Min., 12, 200-202) .-At Caprillone, near Montecatini, fine, large crystals of barytes are found in geodes in conglomerate and miocene marl-lime- stone. The crystals are opaque, porcelain-white at the edges, and reddish-yellow in the middle. In appearance, the crystals resemble *hose of celestine. Analysis gave the following results :- &. Ca. SO4. Total. 13p. gr. 37-82 0.24 41.09 99.15 4-38 The author also describes a twin-crystal of hsmatite from Rio in Elba, in the Pisa Museum, exhibiting the planes R, )R, -+R, gR3, +F2. The twinning axis is perpendicular to mR. Descriptions are also given of crystals of chlorite from Bottino in the Apnan Alps; quartz from the Cala, dell’ Allume ore-bed in the island of Giglio ; g p m m from the same locality ; pyrolusite from the manganese ore- bed of the Campese in the island of Giglio; and magnetite and epidofa from Romito.Rare Copper Minerals from Utah. By G. S. MACKENZIE (itfin. Mag., 6, 181-182; Zeit. Kryst. Mi%., 12, 182--183).-The author gives analyas of two minerals from the American Eagle Mine, Utah Territopy, occurring in intimate msociation with olivenite and other mppr compounds. B. H. B. The resnlts-of the analpes were as follows :- c 220 ABSTRACTS OF CHEMICAL PAPERS. CuO. CaO. MgO. ZnO. Ag. Fez03 AI2O3. As20,. I. 28.59 19.67 0.61 2.75 0.29 0.45 - 39.80 11. 26.88 0.55 0.23 - - 26.94 1.17 34.62 P,O;. H20. COz. Quartz.Total. I. 0.20 5.55 (0.98) 1-11 100.00 11. - 9.25 - 0 - i l 100.35 I. Conichabiie in emerald-green globules. 11. Cheneviaite scat- tered in patches throughout such parts of the ore as occur in hard lumps, in a greenish opaque body with no lustre (compare Abstr., 1886, 516). B. H. B. Columbite. By E. S . DANA (Zeit. Kryst. Min., 12, 266-274).- I n 1861 Schrauf published his monograph on this mineral, in which the axial ratio is stat,ed tlo be a : b : c = 0.40744 : 1 : 0.33467. The aut,hor has now made an exhaustive investigation of the recently dis- covered crystals from Stnndish in Maine. He gives a list of the 13 planes observed, and finds the axial ratio to be a : b : c = 0.40234 : 1 : 0.35798. The angles calculated from this ratio, on the whole, agree better with those given by Dana (1837) and Des Cloizeaux (1851) than with those given by Schranf.The frequently repeatled question whether columbite does not belong to the mono- symmetric system like wolfram, is answered by the author in the negative. There can be no doubt that columbite crystallises in the rhombic system. B. H. B. Plagioclase from California. By I(. YON CHROUSTSCHOFF (Zeit. Kryst. Min., 12, 204-205) .-The felspar examined forms lmge dark tabular crystals in a hypersthenite from San-Diego. The angles made by tbe directions of extinction wit)h the edge formed by the faces OP and mPm, on clearage_plates taken parallel to OP is + 1" to + 2", on plates parallel to mPm +12". Analysis gave the following results :- SO2. A1203. CaO. Fe,03. MgO. K20. N%O. 65.17 21.04 1.20 0.74 0.04 1-70 9.20 Loss on ignition.Total. SP. gr. 0.80 99.89 2*6:)9 B. H. B. Oligoclase. By A. DES CLOIZEAUX and F. PISANI (Zeit. K y s f . Mil?,., 12, 204) .-A flesh-ccloured felspar from Telemarken (Norway) with a cleavage angle ~ P U O : OP, equal to 86" 30', proves to be an oligoclase of the first class (Abstr., 1886, 776). The extinction on plates parallel to OP is +I" to 2i0, parallel to OoPw +loo to 120. Analysis gave the following result,s (I) :- Loss on SiOz. AlL03. F~203. CaO. NafzO. E20. ignition. Total. Sp. p. I. 65.30 23.00 - 2.42 9.65 0.70 0.20 101.27 2.610 11. 62.25 24.80 0.25 4.90 7.80 0.80 0.20 101.00 2.628&IINERALOGFICA L CHEMISTRY. 21 For comparison, an analysis (It) of sunstone from Frederiksvarn (Zeit. Kryst. Min., 11, 648) was made.As in the sunstone from Tvedestrand, the percentage of ferric oxide is very small in spite of the large amount of hsmatite particles intermingled. Botryogene. By J. HOCKAUF (Zeit. R y s t . Min., 12, 240-254).- The author gives the results of two analyses of botryogene from the Vienna Museum. The specimen examined formerly belonged to Haidinger, and probably supplied the material for his original in- vestigations. The analytical resuits were as follows :- B. H. B. Fe,03. MnO. SO3. L,-v-- FeO. CaO. MgO. H20. Residue. Total. I. 37.1’2 18.31 2.24 0.75 7.91 34.10 0.34 100.77 Ii. 37.00 16-69 1.93 2-24! 1.06 7-40 34-10 0.30 100.72 The formula adopted by the author is 5R”S04 + 2(Fe,S,09) + 38H20. A mineral is frequently soId by the dealers as hotryagene, which is not identical with it.There is a specimen thus obtained in the Vienna Museum, an analysis of which gave the following results :- SO3. A1203. Fe20,. FeO. MnO. CaO. MgO. H20. Total. 33.53 4.52 1-93 2-09 2.34 0.79 5-44 48-68 99-32 B. H. B. (Compare Blaas, Abstr., 1884, 269, 1103 .) Flexibility of Itacolumite. By G. SPEZIA (Zeit. Kryst. Min., 12, 202).-The author was induced to test the accuracy of the general theory as t o the cause of tlhe flexibility of itacolumite by the fact that the flexible mica-like mineral occurs but spsrsely in the itacolumite of North Carolina. His observations show that the rock is flexible when it is composed exclusively of quartz-grains. Under the micro- scope each separate grain is seen to be distinctly flexible. This may also be observed in the coarsely granular itacolumite from Mariaiia in Brazil.The itacolumite examined is also Fery porous, as is shown by the rapid absorption of liquids. A prism weighing 186.444 grams absorbed 5.825 grams of distilled water, and had a volume of 73.5 c.c., of which 5.825 C.C. were of course taken up by the absorbed water, and thus represent the intergranular space. The tenacity of this itaco- lumite is also remarkable. The fracture of a prism 6-29 square cm. in section, by tension in the direction of the plane of cleavage and longi- tudinal axis of the flexible mica-like lamells, was effected with a load of 29.66 kilos. (= 67.06 lbs. per square inch). This tenacity is obviously due t o the twisting of the quartz-grains, whilst the porosity is due to their power of moving. Consequently, the flexibility of itacolumite may be explained mechanically from the form and relative position of the quartz-grains, without assuming a flexible mineral, This conclusion is in accordance with the author’s observations t h a t rectangular prisms cut in different directions exhibit uniform flexibility. R.H. €3. Volcanic Fragments from the Lake of Bracciano. By G. STR~VER (Zeit. Kryst. Mln., 12, 197-2OO).--Numerous volcanic22 ABSTRACTS OF OHEMICAL PAPERS. fragments have recently been discovered in the district between I’Anguillara and the Lake of Martignano, in the midst of an enormous heap of angular fragments of limestones, leucitio and tephritic lavas, leucite phonolites, and trachytes. Similar materials have been found at Monte S.Anqelo and near Cesano, in grey tuff. In these volcanic fragments, the following minerals have been found :-Pleonast, magne- tite, limonite, wollas tonite, pyroxene, hornblende, garnet, idocrase, humboldtilite, meroxene, sai-kolite, nepheline, hauyn, leucite, anor- thite, sanidine, titanite, apatite, and calcite. Of tbese minerals, sarkolite is the most interesting, as it has hitherto only been observed as a rare mineral in the Somma volcanic bombs. The crystals are 10 mm. long, 10 mm. broad, and 5 mm. deep. The combinations ob- served are OP. mPm. P, and OP. mPm. P. Ym. +P. mP. SP3. Frw- ture conchoidal, vitreous lustre, flesh colour or colourless, trnnslucen t to transparent, streak white, hardness 6, optically uniaxial, double refraction positive.B. H. B. Cosmical Powder which fell on the Cordilleras, near San Fernando, Chili. By A. E. NoRDENsmora (Compt. rend., 103, 686 -686).--This powder fell for about half an hour on the surface of fresh fallen snow on the Cordilleras, in November, 1883. During this month ~t peculiar red glow was observed in the sky in the evening, and the atmosphere was highly charged with electricity. The powder was collected by C. Stolp and forwarded to the author. It consists mainly of irregularly rounded reddish-bro wn grains, frequently agglomerated in somewhat large masses, which showed no signs of fusion, and dissolved, though slowly, in hydrochloric acid. The powder also contained a small quantity of annular scales, probably felspar and green hexagonal plates, which consisted chiefly of mica.No metallic iron as present. The powder had the following corn- position :-Fe203, 74.59 ; NiO, with traces of COO, 6.01 ; CuO, traces ; Y205, 0.63: SO,, 0.37; SiOz, 7.57: AlzOj, 2.90; CaO, 0.31; MgO, :3.88; loss on heating, 2.61 = 98-87. A small quantity of alkali is probably also present. The composition of the powder shows that it is not a product of the Krakatoa eruption, and is not of terrestrial origin. It is evidently of cosmical origin, but there is no proof that tlie red glow in the sky was in any way connected with the fall of the powder. C. H. B. Meteorite in a Tertiary Lignite. By GURLT, with Note by DAUBR~E (Conzpt. rend., 103, 702-703).--The meteorite was found in a block of tertiary lignite from Wolfsegg. It formed a rectangular parallelopiped 67 mm.by 62 mm. by 47 mm., and weighed 783 grams. The surlace showed cnpules similar to those observed on meteorites, and was covered with a thin layer of magnetic oxide of iron. The meteorite is a holosiderite, and contains carbon with a trace of nickel, but no quantitative analysis was made. It showed cubical cleavage, but a polished surface did not show Widmanstatt’s figures when treated with acid. Utiubde cousiders that the position of the meteorite and otherMINERALOGICAL CHEMISTRY. 23 evidence proves that the '' meteorite " was deposited in the lignite during the formation of the latter. C . H. B. Note by Abstractor.-Lawrence Smith has shown (Abstr., 1879, 892) that the native iron found in the miocene lignites of Greenland is really of terrestrial origin.C. H. B. Andysis of Mineral Springs in Aegina, and Andros. By A. K. DAMBERGIS (Ber., 19, 2538-254O).-The water from Aegina springs from a calcareous rock, has a salt taste, and a temperature of 26"; sp. gr. at 12" = 1.009635; 10,000 C.C. of the water contain- Calcium sulphate .................. Sodium carbonate. ................. ,, chloride .................. Potassium chloride ................ Magnesium bromide. ............... ,, chloride.. .............. Calcium carbonate ................ Magnesium carbonate .............. Iron carbonate .................... Alumina.. ........................ Silica ............................ Carbonic anhydride (half combined) . Free carbonic anhydride ............ 12,3757 grams. 4-2400 ,) 84.0915 ,, 1,9455 ,, 0-3050 ,, 15.4679 ,, 0.8501 ,, 3.4391 ,, 0-0160 ,, 0.0200 ,, 0*1600* ,, 41004 ), 1.4150 ,, Traces of strontia, fluorine, iodine, nitric and phosphoric aoids, ammonia, lithia, and organic substances are also present in the water.The water of Andros has an agreeable taste, is colonrless and with- out odour ; it is used on account of its medicinal properties ; 10,000 C.C. of the water contain- &odium carbona te.................. Calcium ,, .................. Magnesium carbonate .............. Calcium sulphate .................. Sodium chloride .................. Potassium chloride ................ Magnesium ,, ................ Alumina, ......................... Silica ............................ Carbonic anhydride (half combined). . .......... 7, ,, (free) 0-12M6 gram.0.83000 ,, 0.25140 ,, 0.24010 ,, 1.11996 ,, 0.09586 ,, 0.18192 ,, 0 otjooo ,, 0.14400 ,, 0.54680 ,, 0.15640 ,, Traces of iron carbonate, ammonia, nitric and phosphoric acids, and organic substances were also found to be present. N. H. M.MINERALOGICAL CHEMISTRT.M i n e r a1 o g i c a1 C h em i s t ry.17Artificial Breithauptite from the Mechernich Lead Fur-naces. By A. BRAND (Zeit. Kryst. M ~ N . , 12, 234-239).-1n 1885the author found a number of peculiar crystals in the clay used forstopping the tap-holes of the lead furnaces in which antimonial leadwas smelted. They occur in all the furnaces ; the clay being pulverisedand used again. It is therefore impossible to determine whether theywere originally formed in the smelting of hard lead.The crystalswere columnar, hexagonal prisms, 0.1 to 0.5 mrn. thick, and 5 to26 mm. long. They were brittle, had an uneven fracture, adamantinelustre, steel-grey to copper-red colour, and greyish-brown streak. Thehardness was 5 to 5.5, and the sp. gr. about 8. Analysis of carefullypurified material gave the following results :-Sb. Ni. co. Pb. cu. Fe. Tntal.65.46 29.67 1.12 1.39 0.16 1.45 99-25The formula of the mineral ia thus NiSb. B. H. B.Chemical Composition of Butyrellite. By W. I. MACADAM(Min. Mag., 6, li5-180; Zeit. Kryst. Min., 12, 182).-Tn the in-vestigation of ten samples of bog-butter or butyrellite (Dana) fromvarious localities in the peat bogs of Scotland and Ireland, the authorfound that the portion of the butyrellite soluble in ether correspondedin all respects with the substance obtained under like conditions fromordinary butter.This portion varies in the ten analyses from 91.52 to98.94 per cent. The portion insoluble in ether, 0.38 to 4a.56 per cent.,was slightly soluble in water, and gave evidence of the presence ofmilk-sugar. The portion insoluble in water contained nitrogen, andgave on combustion the peculiar odour of burning cheese. The ashor mineral portion, 0.01 to 0.36 per cent., contained traces of phos-phoric acid. These results, and the fact that a number of cow’s hairswere found in the samples, show that butyrellite has no claim to becalled a mineral. It cannot be discussed how these masses foundtheir way into the positions from which they are now obtained.It is,however, obvious that the material is not of mineral or even ofresinous origin, but of undoubted animal derivation, and shouldtherefore be erased from the list of minerals. B. H. B.Minerals from Vesuvius. By E. SCACCHI (Zeit. Rryst. Min., 12,202-203).-1. Hydrogiobertite is the name given by the author to anew hydrated magnesium carbonate, which occurs in the form ofgrey, compact masses 2 to 15 mm. in diameter. With the lens, minutemagnetite crystals are observed enclosed in the mass. The sp. gr. is2.149 to 2,174. The loss on ignition amounted to 53.07 per cent. Ofthe sample, 0.507 gram contained 0.0025 gram of magnetite, and 0.022gram of ferric oxide which was subtracted as limonite with the mag-netite.The results of the analysis were as follows :-VOL. LII. 18 ABSTRACTS OF OHEMICAL PAPERS.coz. MgO. H20. Total.28-16 44.91 29.93 100~00The formula of the new mineral is MgzCOa + 3H20.The? hydrogiobertite was discovered near Polleiia in a block ofangitophyre very closely resembling lava. In the interior, the structnrewas crystalline. On this Tock was a compact mixture of silicates(plagioclase, augite, and magnetite) with which the hydrogiobertitewas associated.2. AZtered Aragonite.-In the mother-rock of the hydrogiobertite,described above, hexagonal prisms, 3-4 mm. long and 1-1.5 mm.broad were found. They are white and opaque, and for the mostpart soluble in acids ; the insoluble portion frequently preserving theoriginal form of the crystal, or becoming divided longitudinally intoprismatic fragments.On heating at 170", there wag a loss of 6.81 percent. I n hydrochloric acid, 11.78 per cent. was insoluble; thisportion was found to c6ntain 58.97 per cent. of silica with ferric oxide,alumina, and lime ; whilst the soluble portion consisted essentially oflime. The insoluble substance also occurs in the interior of thecrystals.3. Fluorspar.-A number of minute octahedral crystals occurringon a' lava from Pollena (187'3) were found to be fluorspar. Thismineral has hitherto +en unknown in the lavas of Vesuvins andother volcanoes. Associated with the fluorspar are minute aciculwcrystals of apatite. B. H. B.Chemical Constitution of Barytocalcite and Alstonite. ByA. BECKER (Zeit.Kryst. Min., 12,222-227) .-The monoclinic baryto-calcite and the rhombic alstonite have hitherto been regarded ashaving the same chemical composition (BaC03 + CaCO,). Thequestion now arises whether they should both be considered isomorph-ous mixtlures of BaCOs and CaCO,, or whether one of them is nota molecular compound of the two carbonatea with the formulaBaCaC20s. Qroth regards barytocalcite as a moleciilar compound ofthis kind, whilst alstonite, he thinks, is an isomorphous mixture ofequal amounts of the two salts. This view is confirmed experimentallyby the author, who gives the following results of a series of analysesof the two minerals in question :-BaO.I. 30.0911. 50.36111. 51.59IV. 44-69V. 37.42VI. 50.97VII. 51.45cso.19.7719.2218-6123.4029.0619 8319.89MnO.GOz.0.35 29.520.25 29.440.35 29.390.29 31.710.30 32.21- 29-650.20 29-52Insol. ma. Total. - 99.730.30 99-370.28 103.22 - 100.09- 98.980.25 100.70I 101.06All the specimens analysed were from Alston Moor.calcite, purchased from Pech of Berlin.I. Barytocalcite, purchased from Sturtz of Bonn. 11. Baryto-111. Bargtocalcite from thMINERALOGTCAL CHEMISTRY. 19minem~ogica,l miasearn of the University of Leipziq. These threeanalpee correspond with the formula BaCO, + CaC03.IV. Alstonite from Pech of Berlin; formula, 3BaC0, + 4CsC0,.V. A second specimen of the same, formula BaCO, + 2CnCO3.VI. Alstonite, purchased from Gregory of London, formula BaC0, +CaCO,. VII.Alatonite from the mineralogical museum of the Uni-versity of Leipzig, formula BaC03 + CaC03.For the three specimens of barytocalcite analysed, the same formula(BaCO, + CaC03) is obtained; so that this mineral must be regardedas a, molecular compound ; whilst of the four specimens of alstoniteanalysed, two had the same formula (BaC03 + CaCO,), and the othertwo the formule 3BaCO3 + 4CaC0, and BaC03 + 2CaC03. Alston-ite, consequently, is undoubtedly an isomorphous mixture of the twocarbonates. B. EL B.Chemical Composition of Herderite. By A. DES CLOIZEAVXand A. DAMOUR (Zeit. R y s t . Rfin., 12, ‘204).-Since Des Cloizeaux(Abstr., 1889, 827) establiahed the optical identity of the herdcritecrygtals from Sfoneham, Maine, and from Ehrenfriedersdorf, Saxony,C.Winkler (Abstr., 1884, 1102) bas given an analysis of the crystalsfrom both localities, attributing tho loss to water, and not to fluorine.$ubseqnently F. A. Genth (Abstr., 1885, 488) found 8.93 per cent. offluorine in the Stoneham herderite. These discordant rmults haveinduced the authors to make a fresh investigation, and their analysisahowa the presence of a considerable amount of fluorine. The sp. gr.of the mineral examined was 2.98 (compare Abstr., 1885, 359).B. H, B.Minerals from Tuscany. By L. BUSATTI (Zeit. Kryst. Min., 12,200-202) .-At Caprillone, near Montecatini, fine, large crystals ofbarytes are found in geodes in conglomerate and miocene marl-lime-stone. The crystals are opaque, porcelain-white at the edges, andreddish-yellow in the middle.In appearance, the crystals resemble*hose of celestine. Analysis gave the following results :-&. Ca. SO4. Total. 13p. gr.37-82 0.24 41.09 99.15 4-38The author also describes a twin-crystal of hsmatite from Rio inElba, in the Pisa Museum, exhibiting the planes R, )R, -+R, gR3,+F2. The twinning axis is perpendicular to mR. Descriptions arealso given of crystals of chlorite from Bottino in the Apnan Alps;quartz from the Cala, dell’ Allume ore-bed in the island of Giglio ;g p m m from the same locality ; pyrolusite from the manganese ore-bed of the Campese in the island of Giglio; and magnetite andepidofa from Romito.Rare Copper Minerals from Utah. By G. S. MACKENZIE (itfin.Mag., 6, 181-182; Zeit. Kryst. Mi%., 12, 182--183).-The authorgives analyas of two minerals from the American Eagle Mine, UtahTerritopy, occurring in intimate msociation with olivenite and othermppr compounds.B.H. B.The resnlts-of the analpes were as follows :-c 20 ABSTRACTS OF CHEMICAL PAPERS.CuO. CaO. MgO. ZnO. Ag. Fez03 AI2O3. As20,.I. 28.59 19.67 0.61 2.75 0.29 0.45 - 39.8011. 26.88 0.55 0.23 - - 26.94 1.17 34.62P,O;. H20. COz. Quartz. Total.I. 0.20 5.55 (0.98) 1-11 100.0011. - 9.25 - 0 - i l 100.35I. Conichabiie in emerald-green globules. 11. Cheneviaite scat-tered in patches throughout such parts of the ore as occur in hardlumps, in a greenish opaque body with no lustre (compare Abstr.,1886, 516). B. H. B.Columbite. By E. S . DANA (Zeit. Kryst. Min., 12, 266-274).-I n 1861 Schrauf published his monograph on this mineral, in whichthe axial ratio is stat,ed tlo be a : b : c = 0.40744 : 1 : 0.33467.Theaut,hor has now made an exhaustive investigation of the recently dis-covered crystals from Stnndish in Maine. He gives a list of the13 planes observed, and finds the axial ratio to be a : b : c =0.40234 : 1 : 0.35798. The angles calculated from this ratio, on thewhole, agree better with those given by Dana (1837) and DesCloizeaux (1851) than with those given by Schranf. The frequentlyrepeatled question whether columbite does not belong to the mono-symmetric system like wolfram, is answered by the author in thenegative. There can be no doubt that columbite crystallises in therhombic system.B. H. B.Plagioclase from California. By I(. YON CHROUSTSCHOFF (Zeit.Kryst. Min., 12, 204-205) .-The felspar examined forms lmge darktabular crystals in a hypersthenite from San-Diego. The anglesmade by tbe directions of extinction wit)h the edge formed by the facesOP and mPm, on clearage_plates taken parallel to OP is + 1" to + 2",on plates parallel to mPm +12". Analysis gave the followingresults :-SO2. A1203. CaO. Fe,03. MgO. K20. N%O.65.17 21.04 1.20 0.74 0.04 1-70 9.20Loss onignition. Total. SP. gr.0.80 99.89 2*6:)9 B. H. B.Oligoclase. By A. DES CLOIZEAUX and F. PISANI (Zeit. K y s f .Mil?,., 12, 204) .-A flesh-ccloured felspar from Telemarken (Norway)with a cleavage angle ~ P U O : OP, equal to 86" 30', proves to be anoligoclase of the first class (Abstr., 1886, 776).The extinction onplates parallel to OP is +I" to 2i0, parallel to OoPw +loo to 120.Analysis gave the following result,s (I) :-Loss onSiOz. AlL03. F~203. CaO. NafzO. E20. ignition. Total. Sp. p.I. 65.30 23.00 - 2.42 9.65 0.70 0.20 101.27 2.61011. 62.25 24.80 0.25 4.90 7.80 0.80 0.20 101.00 2.62&IINERALOGFICA L CHEMISTRY. 21For comparison, an analysis (It) of sunstone from Frederiksvarn(Zeit. Kryst. Min., 11, 648) was made. As in the sunstone fromTvedestrand, the percentage of ferric oxide is very small in spite ofthe large amount of hsmatite particles intermingled.Botryogene. By J. HOCKAUF (Zeit. R y s t . Min., 12, 240-254).-The author gives the results of two analyses of botryogene from theVienna Museum.The specimen examined formerly belonged toHaidinger, and probably supplied the material for his original in-vestigations. The analytical resuits were as follows :-B. H. B.Fe,03. MnO.SO3. L,-v-- FeO. CaO. MgO. H20. Residue. Total.I. 37.1’2 18.31 2.24 0.75 7.91 34.10 0.34 100.77Ii. 37.00 16-69 1.93 2-24! 1.06 7-40 34-10 0.30 100.72The formula adopted by the author is 5R”S04 + 2(Fe,S,09) +38H20. A mineral is frequently soId by the dealers as hotryagene,which is not identical with it. There is a specimen thus obtained in theVienna Museum, an analysis of which gave the following results :-SO3. A1203. Fe20,. FeO. MnO. CaO. MgO. H20. Total.33.53 4.52 1-93 2-09 2.34 0.79 5-44 48-68 99-32B. H. B. (Compare Blaas, Abstr., 1884, 269, 1103 .)Flexibility of Itacolumite. By G.SPEZIA (Zeit. Kryst. Min., 12,202).-The author was induced to test the accuracy of the generaltheory as t o the cause of tlhe flexibility of itacolumite by the fact thatthe flexible mica-like mineral occurs but spsrsely in the itacolumiteof North Carolina. His observations show that the rock is flexiblewhen it is composed exclusively of quartz-grains. Under the micro-scope each separate grain is seen to be distinctly flexible. This mayalso be observed in the coarsely granular itacolumite from Mariaiia inBrazil. The itacolumite examined is also Fery porous, as is shown bythe rapid absorption of liquids. A prism weighing 186.444 gramsabsorbed 5.825 grams of distilled water, and had a volume of 73.5 c.c.,of which 5.825 C.C.were of course taken up by the absorbed water, andthus represent the intergranular space. The tenacity of this itaco-lumite is also remarkable. The fracture of a prism 6-29 square cm. insection, by tension in the direction of the plane of cleavage and longi-tudinal axis of the flexible mica-like lamells, was effected with a loadof 29.66 kilos. (= 67.06 lbs. per square inch). This tenacity isobviously due t o the twisting of the quartz-grains, whilst the porosityis due to their power of moving. Consequently, the flexibility ofitacolumite may be explained mechanically from the form and relativeposition of the quartz-grains, without assuming a flexible mineral,This conclusion is in accordance with the author’s observations t h a trectangular prisms cut in different directions exhibit uniform flexibility.R.H. €3.Volcanic Fragments from the Lake of Bracciano. By G.STR~VER (Zeit. Kryst. Mln., 12, 197-2OO).--Numerous volcani22 ABSTRACTS OF OHEMICAL PAPERS.fragments have recently been discovered in the district betweenI’Anguillara and the Lake of Martignano, in the midst of an enormousheap of angular fragments of limestones, leucitio and tephritic lavas,leucite phonolites, and trachytes. Similar materials have been foundat Monte S. Anqelo and near Cesano, in grey tuff. In these volcanicfragments, the following minerals have been found :-Pleonast, magne-tite, limonite, wollas tonite, pyroxene, hornblende, garnet, idocrase,humboldtilite, meroxene, sai-kolite, nepheline, hauyn, leucite, anor-thite, sanidine, titanite, apatite, and calcite.Of tbese minerals,sarkolite is the most interesting, as it has hitherto only been observedas a rare mineral in the Somma volcanic bombs. The crystals are10 mm. long, 10 mm. broad, and 5 mm. deep. The combinations ob-served are OP. mPm. P, and OP. mPm. P. Ym. +P. mP. SP3. Frw-ture conchoidal, vitreous lustre, flesh colour or colourless, trnnslucen tto transparent, streak white, hardness 6, optically uniaxial, doublerefraction positive. B. H. B.Cosmical Powder which fell on the Cordilleras, near SanFernando, Chili. By A. E. NoRDENsmora (Compt. rend., 103, 686-686).--This powder fell for about half an hour on the surface offresh fallen snow on the Cordilleras, in November, 1883.Duringthis month ~t peculiar red glow was observed in the sky in theevening, and the atmosphere was highly charged with electricity.The powder was collected by C. Stolp and forwarded to the author.It consists mainly of irregularly rounded reddish-bro wn grains,frequently agglomerated in somewhat large masses, which showed nosigns of fusion, and dissolved, though slowly, in hydrochloric acid.The powder also contained a small quantity of annular scales, probablyfelspar and green hexagonal plates, which consisted chiefly of mica.No metallic iron as present. The powder had the following corn-position :-Fe203, 74.59 ; NiO, with traces of COO, 6.01 ; CuO, traces ;Y205, 0.63: SO,, 0.37; SiOz, 7.57: AlzOj, 2.90; CaO, 0.31; MgO,:3.88; loss on heating, 2.61 = 98-87.A small quantity of alkali isprobably also present.The composition of the powder shows that it is not a product ofthe Krakatoa eruption, and is not of terrestrial origin. It is evidentlyof cosmical origin, but there is no proof that tlie red glow in the skywas in any way connected with the fall of the powder.C. H. B.Meteorite in a Tertiary Lignite. By GURLT, with Note byDAUBR~E (Conzpt. rend., 103, 702-703).--The meteorite was foundin a block of tertiary lignite from Wolfsegg. It formed a rectangularparallelopiped 67 mm. by 62 mm. by 47 mm., and weighed 783 grams.The surlace showed cnpules similar to those observed on meteorites,and was covered with a thin layer of magnetic oxide of iron. Themeteorite is a holosiderite, and contains carbon with a trace of nickel,but no quantitative analysis was made.It showed cubical cleavage,but a polished surface did not show Widmanstatt’s figures whentreated with acid.Utiubde cousiders that the position of the meteorite and otheMINERALOGICAL CHEMISTRY. 23evidence proves that the '' meteorite " was deposited in the ligniteduring the formation of the latter. C . H. B.Note by Abstractor.-Lawrence Smith has shown (Abstr., 1879,892) that the native iron found in the miocene lignites of Greenlandis really of terrestrial origin. C. H. B.Andysis of Mineral Springs in Aegina, and Andros. ByA. K. DAMBERGIS (Ber., 19, 2538-254O).-The water from Aeginasprings from a calcareous rock, has a salt taste, and a temperature of26"; sp. gr. at 12" = 1.009635; 10,000 C.C. of the water contain-Calcium sulphate ..................Sodium carbonate. .................,, chloride ..................Potassium chloride ................Magnesium bromide. ...............,, chloride.. ..............Calcium carbonate ................Magnesium carbonate ..............Iron carbonate ....................Alumina.. ........................Silica ............................Carbonic anhydride (half combined) .Free carbonic anhydride ............12,3757 grams.4-2400 ,)84.0915 ,,1,9455 ,,0-3050 ,,15.4679 ,,0.8501 ,,3.4391 ,,0-0160 ,,0.0200 ,,0*1600* ,,41004 ),1.4150 ,,Traces of strontia, fluorine, iodine, nitric and phosphoric aoids,ammonia, lithia, and organic substances are also present in thewater.The water of Andros has an agreeable taste, is colonrless and with-out odour ; it is used on account of its medicinal properties ; 10,000C.C. of the water contain-&odium carbona te..................Calcium ,, ..................Magnesium carbonate ..............Calcium sulphate ..................Sodium chloride ..................Potassium chloride ................Magnesium ,, ................Alumina, .........................Silica ............................Carbonic anhydride (half combined). . .......... 7, ,, (free)0-12M6 gram.0.83000 ,,0.25140 ,,0.24010 ,,1.11996 ,,0.09586 ,,0.18192 ,,0 otjooo ,,0.14400 ,,0.54680 ,,0.15640 ,,Traces of iron carbonate, ammonia, nitric and phosphoric acids, andorganic substances were also found to be present. N. H. M

ISSN:0368-1769    

DOI:10.1039/CA8875200017

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

24 ABSTRACTS OF CHEMlCAL PAPERS. Organic Chemistry. Volatility of Methane-derivatives. By L. HENRY (Compt. rend., 103, 603-606) .-The volatility of methane-derivatives follows the same order as that of the substituted elements when the latter are arranged in natural families in the order of their atomic weights. The boiling point rises as the molecular weight increases, but the differences between the volatility of the methane-derivatives are much less than those between the boiling points of the electronegative elements which they contain. B. p. Diff. cl, gas ...... - 35") 96" Br, liquid .... + 63 I, solid . . , . . + 250 } O , ~ R S ........ - 181 N, gas. ...... - 193 S, solid ...... + 448) 629 P, solid ...... + 287}480 B. p. Diff. MeC1, gas .... - 23" } 27.5 Me20, gas .....- 23 } 60.0 4- } 50.0 Me3N, gas MeBr, gas .... + 4.5 MeI, liquid ... Me,S, liquid. .. + 37 Me3P, liquid.. . + 41 44 } 39'5 ..... The differences show that electronegative elements in the same natural family are far from being comparable in the free state, whilst ip methane-derivatives they may be regarded as existing under analogous physical conditions. I n each of the groups of methane-derivatives, the rise of the boiling point is not proportional to the increase in the molecular weight ; in fact the greater the increase in the molecular weight resulting from substitution, the less proportionally is the rise of the boiling point. The substitution of sulphur causes proportionally less rise in the boil- ing point than the substitution of oxygen, and the snbstitution of phosphorus less than the substitution of nitrogen, although sulphur and phosphorus are solids, whilst oxygen and nitrogen are gases.The atomic weights being nearly equal, the diminution of volatility resulting from substitution is greater the more strongly marked the electronegatire character of the substituted element, or, in other words, the more distinctly its properties differ from those of hydro- gen. This is well seen in the case of the nitrogen- and boipon-deriva- tives. Me3N, mol. wt. 59, a liquid boiling at 9.3". Me3B, mol. wt. 36, a gas which liquefies at -10" under a pressure of 3 atmos. This phenomenon is doubtless connected with the fact that the heat of combination of carbon with electronegative elements diminishes as the atomic weight of the latter increases.Sugars. By BERTHELOT (Compt. rend., 103, 533-537).--8 soh- tioh of invert sugar which had been kept for nearly 30 years, deposited spheroidal groups of radiating crystals, which when care- C. H. B.ORGANIC CHEMISTRY. 25 fully dried on filter-paper resembled purified glucose. The crystals have the composition C6H,,0e when anhydrous ; their reducing power is equal to that of glucose, and they are completely fermentable, but their rotatory power is only [a]= = + 32.2, or little more than half that of glucose. The crystals are a compound of glucose and levu- lose, in which one constituent behaves like water of crystallisation. The compound is decomposed by solvents ; its rotatory power shows that the ratio of levulose to glucose is 1 : 5.A similar compound prepared by G6lis has the rotatory power of +15O, which corresponds with a ratio of levulose to glucose of 1 : 3. The compound formed as an intermediate product in alcoholic fer- mentation is most probably formed by the union of one molecule of levulose with two of glucose, but it does not seem to have been ob- tained in crystals. In the process of extracting raffinose from cotton-seed cake, crys- tals were obtained which when dried on filter-paper without treatment with any solvent had all the properties of mellitose from the manna of eucalyptus. When the aqueous solution of this substance is treated with yeast, only half the sugar undergoes fermentation, and the liquid contains a non-fermentable sugar with the properties of eucalpe. If the mellitose is treated with boiling alcohol, it splits up into rafflnose, which crystallises after some time, and eucalyne, which remains in solution.An alcoholic solution of ra5nose and eucalyne when allowed to remain, deposits crystals which seem to be formed by the recom- bhation of the rnffinose with the eucalyne. Mellitose, which is widely diffused in the vegetable kingdom, is the result of the association of raffinose, a true saccliarose, with eucdyne, a non-fermentable carbohydrate. This association bears no resemblance to the union of glucoses to form saccharoses, and the constitution of mellitose is analogous to that of hydrates and alco- holates rather than to that of ethereal salts. C. H. B. Sugar formed in the Inversion of Lichens. By P. KLASON (Ber., 19, 2541).-Bauer showed (Abstir., 1886, 869) that dextrose is formed by inverting lichens.The author previously obtained the same results (Lund’s Pysiogr. Sallskops Minneskr., 1878, 61). Appa- rently no other sugar is formed in the inversion. N. H. M. Action of Dilute Acids on Grape-sugar and Fruit-sugar, By M. CONRAD and &I. GUTHZEIT (Ber., 19, 2569-2574).-According to Tollens and v. Grote (Annnnlen, 175, 181, and 206, 207), dextrose as well as levulose when boiled with sulphuric, or better with hydro- chloric acid, .Fields acetopropionic acid in very small quantity. Quantitative experiments on the decomposition of cane-sugar by hydrochloric acid, made by the authors (Abstr., 1885, 743), pointed to the formation of a small amount of acetopropionic acid from dex- trose.Experiments described in the present paper show that this view (the formation of acetopropionic acid chiefly from levulose) only holds good for the decomposition of cane-sugar with dilute sulphuric acid, and not with hydrochloric acid. Quantities of dextrose and levulose corresponding with 20 grams of26 ABSTRACTS OF OHEMICAL PAPERS. cane-sugar were heated for 17 hours with the same amounts of acid and water as those previously used (Zoc. cit.). 1. Decomposition with dilute sulphuric acid- Aceto- Humic propionic Formio substances. Dextrose. acid. acid. Dextrose.. .... 52.6 0.83 43-70 2.78 1.21 Levulose.. .... 32.6 13.78 - 16.78 6.46 Cane-sugar.. .. 100.0 = 14.61 43.70 19.56 7-87 2. Decomposition with dilute hydrochloric acid- Aceto-. Humic propionic Formic Dextrose., ....52.6 4-76 14-52 15.53 6-51 Levulose.. .... 52.6 10.65 - 16.28 8-78 substances. Dextrose. acid. acid. Cane-sugar, , . . 100.0 = 15.41 14-52 31.81 15.29 Decomposition of Milk-sugar by Dilute Hydrochloric Acid. By M. CONRAD and M. GUrHZElT (Bey., 19, 2575--2576).-The follow- ing results were obtained froni three experiments, in which 21, 21, and 10.5 grams of milk-sugar were heated with 50 C.C. of water and 4.87, 5.0, and 487 grams of hydrochloric acid respectively :- substances, (unchanged). acid. acid. N. H. M. Humic Milk-sugar Acetopropionic Pormic 1 ...... 3.68 5.54 6-29 2.39 2 ...... 3.94 - 5-80 2.24 3 ...... 1-60 L 3.32 1.33 In 2 and 3, the milk-sugar was not determined. N. H. M. Carbohydrates. By 0. WALLACE (Annalea, 234, 364-375).- The rhizome of the water lily, Iris pseudacorw, contains a peculiar Carbohydrate, called " irisin " by the author.Irkin, CaHl0O5 + HzO, closely resembles inulin, but is distinguished from the latter by its more powerfal action on polarised light; [dc]D = -49' 90 for a 2 per cent. solution of irisin, and [ a ] D = - 37" 27' for a soIution of inulin of the same strength. Fehling's Rolution is not reduced by irisin, but the carbohydrate is easily attacked by dilute acids, yielding levulose as the chief product. Irisin is four times as soluble as inulin in water s t 22". Under the microscope, the globules of irisin resemble the minute globules of inulin in size, but they do not exhibit double refraction. w. c. w. Animal Gum. By H. A. LANDWEHR ( P f t i i g ~ ' ~ arc hi^, 39,193- 204) .--The animal carbohydrates may be arranged in parallel groups with those occurring in the vegetable kingdom, and animal gum resembles vegetable gum in yielding oxrzlio acid after treatment with nitric acid.Mwiin was prepared It is obtained readily from m u c hORGANIC CHEMISTRY. 27 by precipiktion with acetic acid from an extract of submaxillary glands, made with a 1 per cent. sodium carbonate solution. The pre- oipitate was washed with weak acetic acid, and then dissolved in weak hydrochloric acid by the aid of heat. On neutralising with soda, a white flocculent preciFitate is obtained, which is increased in amount on the addition of sodium sulphate and boiling. The precipitate is collected and freed from salt by dialysis; i t consists of an ordinary proteid.The filtrate contains no nitrogen, biit contains animal gum. From tendon mucin, the same carbohydrate is obtained, in spite of what Loebisch (Abstr., 1886, 166) says to the contrary; it may also be obtained from synovia, collo'id cysts, and from the mucin of the snail's mnntle. nilucin and animal gum both yield lsvulic acid when treated with hydrochloric acid. By long boiling with water, chondrin splits into gelatin, animal gum, and possibly a third substance not yet further investigated. Pure chondrin is soluble in hot water, and its solutions gelatinise when cold, if not too dilute ; this power of gelatinising is lost after prolonged boiling. A dilute solution gives the following reactions :-Dilute mineral acids cause a precipitate soluble in excess ; acetic acid gives a precipitate insoluble in excess ; acetic acid and potassium ferrocyanide give a precipitate, soluble in excess of the latter reagent.Sodium chloride solution gives no cloud, but hinders the precipitation by acetic acid. Metaphos- phoric acid gives a cloudiness disappearing on warmth. Alum gives a cloudiness, disappearing on adding excess. Lead acetate gives a preci- pitate, soluble in excess. Basic lead acetate gives a precipitate, partially soluble in excess. Lead acetate and ammonia give a flocculent preci- pitate, insoluble in excess. Tannin and acetic acid give a precipitate, insoluble in excess. Copper sulphate and sodium hydroxide colour the liquid violet, which becomes red on boiling. Boiling the solution for fire or six hours with 1 per cent.mlphuric acid gives it the power of reducing copper salts, this being due to the formation of a reducing sugar from animal gum. Animal gum may be separated from chondrin in the same way as from mucin. Metalbumin and paralbumin may also be used as sources of animal gum. It is also found in small quantities, but constantlly in the red blood corpuscles, brain, kidney, spleen, liver, and pancreas. Prote'ids pi-opor do not yield it. Another source of animal gum is chondrin. W. D. H. Derivatives of Thioformaldehyde. By A. WOHL (Rw., 19, 23444347) .-Thiometaforrnaldehyde, (CH,S),, is obtained when an aqueous or alcoholic solution --of hexamethyleneamine saturated with hydrogen sulphide is heated on a water-bath. It separates as a, white, amorphous substance, which is washed with water and hydro4 chloric acid, and extracted with boiling glacial acetic acid and alcohol.It is insoluble in all the usual solvents, and has a peculiar odour ; it melts at 175-176", and decomposes at a high temperature. It dissolves unchanged in strong sulphuric acid. Methy Zthi~formuldine, S2(CH2)sNMe, is prepared by diluting 50 C.O. of a 20 per cent.. solution of formaldehyde with an equal volume of wa&er, 8nd saturating with hydrogen sulphide; 200 C.C. of wafer are28 ABSTRACTS OF CHEMICAL PAPkXS. then added, the whole filtered and stirred with 20 C.C. of a 30 per cent. solution of methylamine. In 24 hours crystals separate. More hydrogen sulphide i s then passed through the solution until it is no longer turbid ; the crystals are collected, washed with water, and dis- solved in ether.I t crystallises in needles melting at 65", and is insoluble in water, soluble in dilute mineral acids, alcohol and glacial acetic acid. It distils with steam, boils at about 185", being at the same time converted into a compound melting at 130-140". The hydrochloride forms needles readily soluble in water ; it melts at 188" with decomposition. Dimeth ylthioformuldinium iodide, SL(CH,),NMe,1, is formed by treating the compound with methyl iodide. In two to three days the liquid solidifies to a mass of slender, lustrous needles. It melts at 161- 163O, and dissolves readily i n water, sparingly in alcohol. The platino- chloride, [ Sz( CH2)3NMe]zMezPtC16, is a bright yellow, crystalline sub- stance.The iodide dissolves in hot aqueous potash and separates unchanged on cooling. When boiled with silver oxide, it yields an ammonium base, which, however, could not be isolated. Chloro-derivatives of Acetals. By 0. MAGNAMINI (Gazxetta, 16, 330-3333) .-Trichlorometh y let hylacetal, CC13*C €3 (OMe) OEt, is ob- tained by heating tetrachlorether with methyl alcohol in sealed tubes. The reaction is as follows: CCI,*CHCI*OEt + MeOJ3 = HCl + CCl,GH(OMe)*OEt. It is a colourless liquid of camphor-like odour ; it boils at 193.4; sp. gr. = '1.32. Trichlorodimethylacetal, UCI3*CH(CMe)?, obtained from tetrachlor- ethyl methyl ether, is a liquid of similar characters. It boils at 183.2" ; sp. gr. = 1.28. The tetrachlorethyl methyZ ether, CC13*CHC1*OMe, prepared by the action of phosphoric chloride on chloral methylate, is a colourless liquid boiling at 178"; sp.gr. at 0" = 1.84. I t does not appear to have been previously isolated. Diisonitrosoacetone. By H. v. PECHMANN and R. WEHSARG (Ber., 19, 2465-2467).-V. Meyer and Zublin have shown that when accto- acetic acid is treated with nitrous acid, carbonic anhydride is evolved, and isonitrosoacetone formed. The authors find that when, in like manner, acetonedicarboxylic acid is treated with water and sodium nitrite, a rapid evolution of carbonic anhydride takes place, and diiso- nitrosoacetone, CO (CH-NOH),, is produced. This forms glistening prismatic crystals, meltiug with decomposition at 143-144". It is easily soluble in alcohol and ether, sparingly in cold water, chlorofoim, and benzene.Its aqueous solution when heated decomposes into hydrocyanic acid, car- bonic anhydride, and water. Acids cause a similar decomposition, but hydroxylamine is also among the products. It is more stable in nlka- line solutions, and forms alkali saEts, which crystallise in orange-yellow needles. Its salts, especially the red crystalline silver salt, explode when heated. When warmed with phenol and Rulphuric acid, the nitroso-compound gives a red coloration, with ferric chloride a brown. The authors are further investigating the subject. N. H. M. V. H. V. I t is very unstable, and detonates when heated. L. T. T.ORGANIC CHEMISTRY. 29 Hetines. By L. CON OM IDES (Ber., 19, 2524--2527).-When a very dilute solution of diethylketine, CloH,,N2, is treated with the theoretical amount of potassium permanganate, a ketinedicarboxylic acid is obtained, identical with that prepared by Wleugel by reducing ethyl isonitrosoethylacetate (Abstr., 1882, 949).If the oxidation takes place in a warm solution, other and more unstable acids are formed. When 5 grams of ethyl imidoisonitrosobutyrate are care- fully warmed with powdered zinc chloride at 60-70" for a long time, and the product saponified with alcoholic potash, a small quantity of an acid melting at l90-195", identical with Wleugel's acid (Zoc. c i t . ) , is formed. The above reactions, together with the fact that the ketine- acid does not yield an anhydride, point to the following constitutional formulae for methylketiiie and the ketine-dicarboxylic acid :- CMe*CH CMe* C (C 0 OH) NeCH: CMeyN and NeC(COOH): CMeyN* N. H.M. Pure Bntyric Acid. By A. BANNOW (Ber., 19, 2552-2554).- Pure butyric acid is best prepayed by converting the commercial acid into the ethyl salt, which is then fractionally distilled. The fraction boiling at 120-121" is reconverted into acid. N. H. M. Xoc., 1886, 287-297).--Tiglic (methylcrotonic) acid, Derivatives of Tiglic Acid. By P. MELIKOFF (J. RUSS. C h m ~ CHBle: CNeCOOH, was prepared either by the saponification of the oil of Roman chamo- mile (Kopp, Abstr., 1879, 454), or by heating a-methyl-p-hydroxy- butyric acid (Rohrbeck, Abstr., 1878, 136). The acid was treated under water with an aqueous solution of hypochlorous acid, the pro- duct of the reaction extracted with ether, and the solvent; distilled off.The residue, after remaining for some time over sulphuric acid, solidified to a crystalline mass, which was found to consist of two isomeric chlorhydroxyvaleric acids, C5H9C103. A concentrated aqueous solu- tion of this mixture was neutralised with zinc carbonate : a crystalline zinc salt was precipitated, and the mother-liquor on being evaporated left another salt in the form of an amorphous humoid substance, The two acids obtained by decomposing these salts with sulphuric acid are both easily soluble in water, alcohol and ether ; the one forming a crgstalline sparingly soluble zinc salt, melts at 75", and crjstallises from ether in thin prisms; the other isomeride melts at 111*5", and is obtained from its ethereal solution in the form of large, translucent prisms.When a mixture of these acids, or each of them separately, is treated with alcoholic potash, the potassium salt of an anhydro-acid, CHMe <--,- >CMe*COOH, is formed. The free acid forms silky, crystal- line needles having the odour of butyric acid, easily soluble in water, alcohol, and ether, melting at 62". The energy with which i t enters into direct combination is in the main the same as that shown by p-rnethylglycidic acid : a-methj lglj cidic acid in this respect exhibiting30 ABSTRACTS OF CHEMICAL PAPERS. much greater energy. This circumstance, established by experiments on the hydration of the potassium salt by heating with water, is in accordance with the results obtained by the author in a former work on glycidic and a- and p-methylglycidic acids (Abstr., 1885, 650).The energy of direct combination is diminished with increasing molecular- weight in acid8 of analogous constitution ; at the same time among isomeric acids the greatest energy is exhibited by the one containing tertiarily united carbon in its molecule. a-p-Dimethylglycidic acid contains one CH,-group more than a- and P-methylglycidic acids, but, on the other hand, one of its carbon-atoms combined with oxygen is in tertiary union. By the action of hydrochloric acid on a-P-dimethylglycidic acid, a-methy E-P-clLZor-a-hydroaybzLtyric acid, OH*CHMe*CMeCI*COOH, is formed ; it melts at 75", and is identical with one of the chlorhydroxg- valeric acids above described, the other isomeride being therefore a-methtyl-a-clLZoro-~-~~~droxyLUt~r~c acid, CHMeCl*CMe(OH)-COOH.An aqueous solution of a-/3-dimethylgl@dic acid, when heated during 6-10 hours at 99", is converted into a-P-dimethyZqlycidic acid, OHCHMe*CMe(OH)*COOH, melting at lo?", readily dissolving in water, alcohol, .and ether. A. T. Constitution of Chlorhydroxybutyric and Dichlorobutyric Acid. . By E. MELIKOFF (J. Buss. Chem. SOC., 1886, 227-303).- Chlorhydroxybutgric acid (formed by the combination of crotonic with hypochlorous acid, Abstr., 1884, 1302, and 1885, 650), when heated with concentrated sulphuric acid, yields monochlorocrotonic acid, crys- .fallising in long, thin prisms, melting at 98", sparingly soluble in cold, more readily in hot water, easily soluble in alcohol and ether. This acid yields normal crotonic acid (m. p. 72") ou reduction by zinc and sulphuric acid.The chlorocrotonic acid above mentioned is an a-chlorinated product, the isomeric &derivative being obtained, amongst other methods, by the action of phosphorus pentachloride on ethyl acetoacetate; hence, the chlorhydroxybutyric acid in question must be a-chloro-P-hydroayB?~tyric acid. This acid was heated with hydrochloric acid, and a-/%diChloTObUt?/riC acid was obtained; it crystallises in long prisms and melts at 69". An alcoholic solution of the latter compound, when treated with alcoholic potmh, gives a-monochlorocrotonic acid. a-p-Dichlorobutyric acid is formed in like manner when a-monochlorocrotonic acid is heated with hydrochloric acid. A. T. Hydroxystearic Acids of Different Origin. By A. C. and M. SAYTZEFF (J.RUM. Chem. Xoc., 1886, 328--348).-A hydroxp- stearic acid was prepared by one of the authors some time ago in his work on the oxidation of oleic acid (Abstr., 1886, 140). Another acid of this composition was discovered by Fr6my (AnnuZen, 19, 296 ; 20, 50; 33, lo), who obtained it by the action of concentrated sulphuric acid on oleic acid, and described it under t,he name of hydro- rnargaritic acid. Although the main points of the reaction had been satisfactorily explained by FrBmy's work, yet subsequent work on this question has mostly led to unsatisfactory results. SnbaneieffORGANIC CHEMISTRY. 31 (Qbst?., 1886, 442) ha4 at last succeeded in throwing some new light on the processes involved, but the authors do not in all cases obtain results in agreement with his.Oleic acid was obtained by the saponification of oil of almonds, and purified in the ordinary way by conversion into its lead salt. The action of sulphuric acid was regulated in such a manner as to prevent the temperature rising above 35". The mixture was then allowed to remain 20 hours a t a temperature below O", and decomposed by water. In order to increase the yield of hydroxystearic acid, the fatty layer, separated by the action of water and solidifying a t the ordinary temperature to a crystalline mass, was treated with alcoholic potash, whereby the anhydrides of this acid are decomposed. The saponified product was then converted into the acid by boiling with sulphuric acid. When the products of the action of sulphuric acid on oleic acid are left for some time even at low temperatures, the quantity of hydroxystearic acid is diminished, whilst the quantity of its anhydrides increases.Hydroxpstearic acid was extracted from the above-mentioned crystalline mass by repeated recry stallisation from ether and alcohol. So obtained, hydroxystearic acid, CH,. ( C H,) 13-CH,.CH( 0 H) CH2*C 0 OH, melts at 83-85", and resolidifies a t 68-65". At 20" alcohol (99p Ti-.) dixsolres 8.78 per cent., ether 2.3 per cent. of the acid. Tlydroxy- stearic acid does not absorb bromine. The free acid and the hydroxy- stearates of sodium, calcium, barium, copper, zinc, and silver, were analysed, and the formula of the acid shown to be C18H,0,. With hydriodic acid, hydroxystearic acid yields iodostenric acid. CH,*(CH,)13 CH,*CHI*CH2*COOH ; the latter can be converted into ordinary stearic acid by reducing its alcoholic solution with zinc and hydrochloric acid.When hydroxystearic acid is heated at 100" in sealed tubes with fuming hydrochloric acid, a syrupy liquid is formed, soluble in ether, insoluble in alcohol m d water, and having the composition of oleic acid. It does not show acid properties, nor give additive products with bromine or iodine (in Hubl's solution); it is therefore considered to be a complete anhydride of hydroxystearic acid, formed by elimination of 2 mols. of water from 2 mols. of the acid (analogous to glycolide or lactide). The anhydride is decomposed into hydroxystearic acid by treatment with alcoholic potash a t tem- peratures above 150". Heated with dilute sulphuric acid (in sealed tubes at looo), hydroxystearic acid yields the same anhjdride, but when concentrated salphnric acid is iised a t ordinary temperature, two other products of non-saturated character are formed, one corn bining with 17 per cent., the other with 33 per cent., of iodine, when heated with it on the water-bath.These substances bear a great resemblance to FrBmy 's metoleic acid, and will be further investigated. It wag shown that the hydroxystearic acid prepared by $he action32 ABSTRACTS OF CHEMICAL PAPERS. of moist silver oxide on iodostearic acid was identical with that described above. Finally, the authors have studied the action of alcoholic potash on iodostearic acid. After heating the mixture in a reflux apparatus, and expelling the alcohol by distillation, the product of the reaction was decomposed by sulphuric acid.An acid was obtained, solidifying ak ordinary temperatures to a crystalline mass, and consequently not identical with oleic acid. It was purified by converting it into the sodium salt, recrystnllising this salt from alcohol, precipitating with zinc sulphate, recrystallising from boiling alcohol, and decompodng the zinc salt by sulphuric acid. Thus purified, the substance crys- tallises from ether in translucent, rhombic tables, easily soluble in alcohol, sparingly in ether, and melts at 40-45". The composition of this acid was found to be the same as that of oleic and elaidic acids. It is a non-saturated compound, taking up two atoms of bromine 01' iodine. When oxidised by potassium permanganate i n alkaline solution, it yields dihydroxystearic acid, melting a t 78".The authors intend to continue the investigation of this solid oZeic acid. Another acid, melting a t 20-25", simultaneously formed by the action of potash on iodost,earic acid, was found to be a mixture of ordinary and solid oleic acids. The constitution of solid oleic acid is CH,*( CH2) Is*CH2*CH : CH*COOTJ, ordinary oleic acid being repre- sented by CH3*(CH2)13*CH : CH*CH,-COOH. A. T. Action of Trimethylene Bromide on Ethyl Acetoacetate, Benxoylacetate, and Acetonedicarboxylate. By W. H. PKRKIN, Jun. (Ber., 19, 2.557-2561 ; comp. Abstr., 1886, 689).-When the acid C7Hl0O3 (from trimethylene bromide and ethyl sodacetoacetate) is boiled with aaker, carbonic anhydride is evolved, and Lipp's acetobutyl alcohol (Abstr., 1886, 218) is formed. When the acid is distilled, the anhydride of acetobutyl alcohol, CH2<cCH2.C,2-->0, CH : CHMe is obtained; it is a mobile oil.The same compound is also formed when acetobu tyl is heated. Strong hydrobromic acid dissolves the ethyl salt C9Hla03, and decomposes it into bromobntyl methyl ketone ( Lipp, Zoc. cit.) and carbonic anhydride. Benzoyltetramethylene- carboxylic acid is decomposed by hydrobromic acid in a similar manner, with formation of the compound COPh*CH2*CHz*CH2*CHzBr ; this cyystallises in plates melting a t 61". The instability towards hydrobromic acid of the products obtained by the action of tri- methylene bromide on etbyl acetoacetate and benzoylacetate respec- tively, distinguishes them sharply from tetramethylenedicarboxylic acid.Trimethylene bromide acts on the sodium compound- CO(CHNa*COOEt)2 (from ethyl acetonedicarboxglate and sodium ethoxide), yieiding the compound C O O E t * C H ~ ~ ~ , ~ ~ C > O . The latter is a colour- less oil boiling at 238-240-(under 150 mm. pressure). The mon- et/t,yl salt melts at 114"; the free acid at 185--190" with decom-ORGANIC CHEMISTRY. 33 position. When the monethyl salt is distilled, a subtance is obheined apparently identical with the product of the reaetion between tri- methylene bromide and ethyl acetoacetate. The dicarboxylic acid is decomposed by boiling water into acetobutyl alcohol and carbonic anhydride. N. H. M. Ethyl Acetotrimethyleneearboxylatk By W, H. PERBIN, Jun., and P.C. FREER (Ber., 19, 2561--2569).-The fact that trimethyleno bromide reacts with ethyl malonate, yielding a tetramethykne- derivative, and with ethyl acetoacetate with formation of an ether, sugges6ed the possibility that the product of the reaction between ethylene bromide and ethyl acetoacetate (Trans, 1885, 801) is not a trimethylene-derivative bdt an ether. The aesults of determinations of the magnetic circular polarisation, and the optical properties point, however, to the trimethylene formula first ascribed to the compound, E t h yZic brometh y Zucetoacetate, CH2Br+H2-CHAc*C00Et, is obtained by dissolving ethyl acetyltrimethylenecarboxylate, well cooled., in hydrobromic acid, sp. gr. 1.85 (3 parts) ; after being left for 10 minutes at the ordinary temperature, it is poured into ice water..It is a yellowish oil, having an odour of camphor ; when exposed to air it becomes brown, and gives off hydrobromic aeid.. When reduced by means of zinc-dust and acetic acid, it is converted into ethyl aceto- acetate. Acetopropy I aZcohoZ, COMe*CHz-CH2-CH2-OH, is prepared by boiling 20 grams of the above homo-compound for two hours with 5 grams of hydrochloric acid and 20 grams of water. The reaction is analo- gous to that by means of which Lipp obtained acetobutyl alcohol from ethyl bromopropylaeetoacetate (Abstr., 1886, 216). It i s a colourless oil, very soluble in water; the solution very readily reduces ammoniaeal silver solution but not Yehling's solution. It is very unstable. A phenylhydrazine-compound was prepared. When the alcohol is heated, it is converted with evolution of water into a mobile oil, having an ekhereal odour ; it is probably an anhydride, CMe- cHqCH2* CH2>0 (comp.A'bstT., 1886, 219). y-PeNty Zeme glycol, OH-CHMe*CH2-CR2.CH2-OH, is obtained by reducing acetopropyl alcohol with sodium amalgam. I t is a very thick, colourless oil, extremely soluble in water. It boils a t 210- 220" with partial decomposition. When heated above its boiling Doint. or with 50 to 60 Der cent. of sulDhuric acid at 100'. it is con- I ' CHM - verted into the anhydride, CH2< CH,. &,>O, boiling at 78- 83". - - Pentylene glycol dissolves in hydrobromic acid (sp. gr, 1-85) with considerable development of heat ; when the solution is heated at W", the momobromohydrin of the glycol, C5HI13&, is formed, This is a colourless oil, which boils (under 150 man.pressure) at 144-145". N. H. M. Derivatives of Diaxosuccinic Acid. By T. C m r m and F. KOCH (Ber., 19, 2460--2462).--This is a continuation of the authors' previous work on this subject (Abstr., 1885, 885). Aspartic acid wsls VUL. LIr. d34 ABSTRACTS OF CF-IElIICAL PAPERS. obtained by the reduction of ethyl diazosuccinate with zinc-dust and acetic acid, thus proving the correctness of the formula formerly ascribed to diazosuccinic acid. NHz* CO* CN,*CHz*CO ONe (from the action of ammonia on methyl dia zosuccinnte), crystallises in long, golden-yellow prisms soluble in ether and alcohol, and melting at 84". When ethyl diaeosuccinate is acted on by cold slightly acidified water, mulamic and f umalramic acids are produced.Malamic acid, NH,*CO*CH ( OH)*CH2*COOH, crystallises in colourless prisms easily solnble in water, alcohol, and ether, and melts a t 146" ; its methyl salt yields silky sca1e.s soluble in alcohol, ether, and water, and melting a t 105". illethyl furnuramate, NHz*CO*CzH,*COOMe, crystallises in colourless plates, soluble in alcohol, and melts at 160-162". EihyZ benzoyZmaZamute, NH,*CO~CH(OBz)~CH,~COOEt, was obtained by heating together equal molecular proportions of benzoic acid and ethyl diaxosuccinamate a t 140-150". It forms colourless clinorhombic crystals soluble in water, alcohol, and ether, and melts at 96-97". It decomposes easily when heated. The corresponding methyl salt form8 colonrless crystals, melting at 78-80".By the action of iodine on an ethereal solution of ethyl diazosuccinamate an unsymmetrical ethyl diiodowxinamate, NH,*CO*CI,*CH,* COOEt, is formed. This crystallises in long, greenish-white needles which darken at 110", melt a t 132", and decompose at 150". The methyl salt and come- sponding methyl and ethyl hromo-salts are oils. Dichloropyromucic Acid. By A. DENARO (Gazzetta, 16, 333- 335).-1f a current of dry chlorine gas is passed into the ethyl salt of pyromucic acid, a thick oil is at first obtained, probably consisting of the tetrachloride of the acid. This on decomposition with alcoholic potash and subsequent acidification, yields a dichlorqyromucic acid which crystallises in white needles, melting at 167". Its barium salt crystallises with 3 mols. HzO i n prisms, the calcium salt with 3$ mols. H,O in scales; both become completely anhydrous when heated to 110".v. 1%. v. By 0. WIDMANN (Ber., 19, 2477- 2$82).-As the mode of formation and reactions of this substance are best explained by the formula CO' /GO, which 1111- doubtedly belongs to acetylenecarbamide, the author has carefully re-examined these two compounds with the view of determining whether they are isomeric or identical. He finds that the latter is the case, and that the apparent differences in their reactions are due to erroneous observation. When boiled with concentrated baryta-water, acetylenecarbamide does not, as previously asserted, yield carbonic anhydride, but, like glycoluriI, is decomposed into hydantoic acid and carbamide. The solubility of acetylenecarbamide i 3 given by Schiff as 1 in 333 parts of water a t 15".The author fiads that pure acetylenecarbamide requires 1090 parts of water for solution, whilst a similar determination af the solubility of glycoluril showed a Methyl diazosuccinumate, L. T. T. Constitution of GIycoluriI. NH*CH*NH, I \NH.CH*NHORUA'NlC CHENISTRY. 35 ratio of 1 : 1060. Similar agreement was also found in the siher sdts, crystalline form, &c., both compounds crystallising variously in needles, prisms, or octahedra according to the solvent employed. Glycoluril and acetylenecarbamide are therefore identical, and the author pro- pofies the adoption of the latter name as the more suitable. Hydrocarbons from Tar-oils Boiling between 170" and 200". By 0. JACOBSEN (Ber., 19, 2511--2515).-The author has examined a sample of coal-tar oil free from thiophen, of boiling point 170-200".By combined fractional distillation, conversion into sulphonic acids, sulphonic salts, and sulphonamides, he succeeded in isolating naph- thalene, pseudocumene, hemellithene, and another hydrocarbon, boiling like the last-named at 175-175*5", but yielding a very soluble mi+mwnide melting a t about 122-123". On oxidation, the hydro- carbon yields an acid which crystallises in needles melting at 119- 121" and volatile in steam, aud also small quantities of a second acid melting at 90". The acid of higher melting point yields isophthalio acid when oxidised with permanganate. Chloropropylbenzene.. By G. ERRERA (Gazzzetta, 16,310-325) .- I n order to determine the constitution of the chloropropylbenzene obtained by the action of chlorine on the boiling hydrocarbon, the three alcohols derivable from propylbenzene have been prepared and converted into tbe corresponding chloro-derivatives.Phenylpropyl oloohoJ, C&Ph*CH2*CH20H, obtained from crude fitorax by Rugheimer's process, is not altered by gaseous hydrogen chloride, but when heated in a sealed tsbe with saturated hydro- chloric acid solution, it yields tbe chloro-derivative CH,Ph-CH,-CH,Cl. This compound i s a pale-yellow liquid, boiling at 219", and resembling cymene in odour; when pure, it is very stable, being unaltered by prolonged treatment with fused xinc chloride or, silver acetate. Heated with alcoholic potttsh, it yields phenylpropyl ethyl ether, CH2Ph*CHe*CH20Et, a colourlem liquid boiling a t 220", insoluble in water.NethyZ benzykd carbinoE, CHePh*CHMe*OH, obtained together with, allylbenzene and stilbene by the reduction of methyl henzyl ,ketone with sodium amalgam, is a, liquid boiling at 215", of, a pale-yellow colour and agreeable odour. Heated with hydrochloric acid in sealed tubes, it yields the chloro-derivative, CH,Ph*CHClMe, a yellowish liquid, boiling at 204-2Q7" with partial decomposition into allyl- benzene and hydrogen chloride. A similar reaction occurs with alGQ- holic potash, metallic zinc or its chloride. EthyZphenyZ carhino& CHPhEt-OH, prepared by prolonged reduction of the corresponding ketone with sodium amalgam, as described by Barry, is a liquid boiling at 215-217'. It is converted by gaseous hydrogen chloride, even at ordinary temperatures, into the chloride CHPhEtCl, a yellow liquid.bailing about 200-205", but with con- siderable decomposition into bydrogen chloride and allylbenzene, 8 change which takes place even on distillation in a vacuum. It is distinguished from the two preceding chloro - derivatives by the readimss with which it reacts with silver acetate, .xielding tbe itcetyl- L. T. T. L, T. T. d P36 ARSTRACTS OF CHEMICAL PAPERS. derivative, CIAPh'EkOAc, a liquid %oiling trt 227", of fruity odonr, and imsolixble in water. The chloropropylbenaene obtained by the direct dhlorination of the hydrocarbon is identical with the second of the above chloro-compounds, i n that it is decomposed by distillaticm and by alcoholic potash, as also by its stability towards silver aoebate.Iu these properties, the chloro-derivatives of propylbenzene are directly comparable to those of ethylbenzene. Reduction-of Trinitro-+-cumene. By F. MAYER (Ber., 19,2312 -2314) .-In preparing nitrocnmidine by passing hydrogen sulphide through a boiling alcoholic solution of trinitro-+xmene, the chief product is a new acid, CgH12N&305. T t is insoluble in alcohol, ether, glacial acetic acid, '&c., soluble in' hot water, from which it crystallises on the addition of a few drops of hydrochloric acid in splendid, white or yellowish plates. Salts were prepared. 'N. H. M. Hemellithene. By 0. JAUOBSEN (Ber., 19, 2517-2520).--The author has investigated this compound, which he has now isolated from the fraction of coal-tar oils boiling between 170-200" (see p.35). Hemellithene, CsH3M, [ 1 : 2 : 31, boils at T75-175.5", and does not solidify a t - 20". Tribrow~ohenl,ellithene, C9H9Br3, forms long needles melting at 245", and is very sparingly soluble in alcohol ; trinitrdhenzelli- tliene forms prisms melting at 209". The monnosulphonic acid crys- tallises in hydrated rhombic or hexagonal plates, and yields crys- talline salts ; its sulphonamide melts at 99tL-196". Hemellithehenol, C,H,,*OH [Me : Me : Me : OH = 1 : .2 : 3 : 51, is obtained by fusing the mlphonic acid with alkali. It is soluble in dcohol and ether, and crystallises in needles melting at 81". Hemelli- thy& acid, C,H,Me,*COOH [Me : Me: COOH = 1 : 2 : 31. is furmed by the oxidation of the hydrocarbon by dilute nitric acid.It is volatile in steam, and crystallises in wales melting a+ 144". Its 8aZcim salt is described. Distilled with lime, it yields mthoxylene. a - Sz~~rph.aminehemellithy1ic acid [Me : Me : COOH : SO,NH, = 1 : 2 : 3 : 51, is formed by the oxidation of the above sulphonamide. It melts art Z W , and with hydrochloric acid yields a sulphohemelli- thylic acid melting at 180-190". ~-Szclprphaminehemellithylic acid [Me : "Me :COOH : SOZNHz = 1 : 3 : 2 : 51, formed a t the same time as the-a-ackl, is more solhble, and melts a t 174". It yields avery soluble sulphonic acid when ' hwted with hydrochloric acid. Both acidR when fused with potash yielded an easily soluble hydroxyhemellithylic acid, which does not give a blue coloration with ferric chloride.Hemellithene may be readily extracted from the tar oil by means of the sparing solubility of its barium sulphonate. Reciprocal Transformations Of Cymene and Cumenederi- vatives. By M. FILETI (Guzzetta, 16, 300-310).-In this paper are collected the hitherto observed transformations of cumene and cymene- derivatives, the one into the other, and from them is drawn the following generalisation :--A propy1-poup in the para-position rela- tively to a carbon-atom combined with other elements or with non- oxygenated groupings, is transformed into the isopropyl-group, if this V. H. V. It melts at 240" and carbonises. L. T. T.ORGANIC CHEJIISTRT. 37 element or grouping is displaced by an oxygenated radicle whose oxygen is directly united to the carbon-atom compound, and conversely ail isopropyl, is converted into a propyl-group when these substitutions are reversed.(Compare Widman, Abstr., 1886, 453.) Chlorocymene and Bromocymene from Thymol. By M. FILETI and F. CROSA (Gazzetta, 16, 287 - 300). - Chlorocymene (parapropylmetachlorotohene), C6H3MePrC1, is obtained almost in theoretical proportions by heating in a reflux apparatus 4 mols. of thymol with 1 mol. phosphoric chloride. On oxidation with nitric acid, Gerichten (Abstr., 1879, 238) obtained an acid, believed to be a hydrochlorocinnamic acid, C,H,n/Ie~1*Cil2.CH2*C0OH. It is here, however, shown that under these conditions three acids are formed, namely, chlorocumic, orthochloroparatoluic, and chloroterephthalic acids. Sixty per cent. of the theoretical quantity of bromocymene, calcu- hted according to the equation 4C,HI3*OH + PBr5 = CloH13Br + PO(OCloHlJ3 + 4HBr, can be obtained by the gradual addition of 26 grams of bromine to 45 grams of phosphorus tribromide, and heat- i n g the resulting perbromide with 100 grams of thymol.On oxidn- tion with nitric acid of sp, gr. 1.2, bromocymene yields bromocumic acid ; with acid of sp. gr. 1.29, bromonitrocymene with bromocumic, bromonitrotoluic, and bromoterephthalic acids, whilst nitric acid of sp. gr. 1.39 yields the same acids without the bromonitrocy- mene. The bromcumic acid is identical with that obtained by the direct bromination of cumic acid ; it has, therefore, the constitution C6H,PrBr*COOH. The broinoizdrotoluic acid crys tallises in laminae, which melt at 200" without decomposition; it is isomeric with the acid obtained by the nitration of bromotoluic acid ; its barium salt crystallises in long, yellow needles.The brornoterephthalic acid is identical with that obtained by Fischli by the oxidation of bromopara- toluic acid. V. H. V. V. H. V. Ethylxylenes, By 0. JACOBSEN (Ber., 19, 2515--2516).-For the purposes of comparison with hydrocarbons obtained from the fraction of coal-tar oils boiling between 170" and 200" (this vol., p. 35), the author prepared the three isomeric ethylxylenes from the three corre- sponding xylenes, using Fittig's method. Etlzylorthoxyle~~e yields a crystalline sulphonic acid, giving a sulphonamide crystallising in needles melting at 126". Ethylmetaxylene boils a t 184-186", and is still liquid a t - 15" ; its sulpphonic acid is crystalline, and yields crystal- line barium and sodiwm salts; its sulphoibamide melts at 148".Jbhyl- paraxylene boils at 185", and is still liquid a t - 20"; its suZphonic acid crystallises in rhombic scales, forms crystalline barium and sodium salts, and yields a crystalline suZpphonamide which melts at 117". Ethereal Carbonates. By. G. BENDER (Ber., 19, 2265-22.71 ; compare Abstr., 1881, 48). -When naphthyl ethyl carbonate, OCloH,*CO-OEt, is boiled f o r some time, carbonic anhydride and alcohol are given off, and the residue consists of a, mixture of a-naphthol and a, compound C2,H1202 (Zoc. cit.). The formation of L. T. T.38 ABSTRACTS OF OHEJIICAL PAPERS. diphenylene ketone oxides from salicylic acid (Perkin, Tmna, 1883, 35) and the intermolecular change of sodium phenyl carbonate to sodium salicylate, suggest that Ohe naphthyl ethyl carbonafe may have become changed to the ethyl salt, OHCl,H6~COOEt, and that 2 mols.of the latter have condensed with formation of the compound CZ1H1",2 ; this would then be dinaphthylene ketone oxide, ClOH6<CO>ClO'Il6* 0 The isonaeride obtained by boiling P-dinapht hyl diethyl orthocarbonate (loc. cit.) crystallises from benzene in thin prisms melting a t 194". When phenyl ethyl carbonate is heated a t 300" for 3-4 hours diphenylcarbonate is formed. Paraditoly 1 carbonate is obtained by heating paratolyl ethyl carbo- nate at 300"; it is insoluble in water, moderately soluble in hot alcohol, and melts at 115". Tlynayl ethyl carbonate is a thick liquid boiling at 260"; a t 300" it decomposes into dithyrnly 1 carbonate, melting a t 60".Orthoaitrophenyl ethyl carbonate is prepared by the action of ethyl chlorocarbonate on potassium orthonitrophenoxide. It is a heavy yellow oil which boils with decomposition a t 275-285". The arnido- salf, NHE,*C6HrO*C0.0Et, melts a t 95"; it is soluble in alcoho!, moderately soluble i n boiling water. When distilled, it gives off alcohol with formation of ar~hydro-orthamid~~7~e~~yl carbonate, C,H,NO, ; the latter dissolves in alkalis. The silver salt, C7H4AgN02, forms an amorphous, colourless precipitate. The ethyl salt is obtained by boiling the compound with alcoholic potash and ethyl iodide. When heated with fuming hydrochloric acid, it yields ethyl orthamido- phenol and carbonic anhydride ; the constitution of the substance is therefore c6H,<~~~>co.Tbe phenylhydrazine compound of anhy- dro-orthamidophenyl carbonate, C6&<-O->C : N*NHPh, crys- tallisee in yellow needles, which melt at 208". The acetyZ-derivative melts at 97-98". A InorLonrtro-co~npound was prepared ; it forms long yellow needles melting at 256". Bromine acts on the anhydro-corn- pound with formation of a nzonobromo-derivative ; this crystallises from water in plates melting at ,196". When treated with phosphoric chloridc, the compound C7H4ClN02 is .formed. Parahydroxybenzyl Alcohol. By J. BIEDERMANN (Ber., 19,2373- 2376).-Parahydroxybenzt~l alcohol, OH*C6H4*CH20H, is prepared by dissolving parahydroxybenzaldehyde (I part) in a mixture of water (10 parts) and alcohol (5 parts) ; it is then acidified with dilute sulphuric acid and gradually treated with 3 per cent.sodium amalgam (40 parts). Grey crystals of diparahydroxyhydrobenzoin and oily drops of dipnra- hydroxyisohydrobenzoh separate. When hydrogen is no longer evolved, the solution is made strongly acid and left for 12 hours, it is then filtered, the filtrate extracted with ether, and the ethereal extract treated with hydrogen sodium sulphite. On evaporating the ether, the alcohol separates in needles ; these are purified by dissolving tlhem in hot chloroform and precipitating with light petroleum. It forms slender N H N. H. M.ORG AKIU CHEMISTRY. 39 white needles, readily soluble in water, alcohol, and ether, sparingly in benzene and chloroform; sulphuric acid dissolves it, yielding a splendid 1-ed-violet solution.It melts a t 110". The alcohol is also formed when parahydroxybenzaldehyde is kept dissolved in aJcoholic potash for several weeks, but the reaction is still very incomplete. The acety I-derivative, OH*C6H4*CH,.0Ac, is prepared by heating the alcohol with a mixture of glacial acetic acid and sulphuric acid. It crystallises from water in small yellow needles, melting at 84", and is readily soluble in alcohol and ether, spariiigly in water, benzene, chloroform, &c. The diucetyl - derivative, OAc*CcH4*CH2*OAc, is obtained by heating pnrahydroxybenzyl alcohol with an excess of acetic anhydride a t 160" for 5-6 hours. It forms yellowish needles melting a t 75", readily soluble in alcohol and ether, sparingly in benzene, &c.Br~isic alcohol, OMe*C6H4*CHI,0H[ = 1 : 41, is formed when para- hydroxybenzyl alcohol is dissolved in methyl alcohol and digested with potash and methyl iodide for some hours at 100". The product is treated with wzter, heated to expel methyl alcohol and iodide, and extracted with ether. On evaporating the ether, it is obtained as an oil which gradually solidifies when kept over sulphuric acid. It crp- tallises from water in needles melting a t 45" (compare hbstr., 1888, 460). N. H. 11. Synthesis of Betorcinol (p-Orcinol). By S. V. KOSTANECKI (Bey., 19, 22 18-2324 ; comr are Abstr., 1886, 242) .-Z'araxylorcinol [Me2 : (OH), = 1 : 4 : 3 : 51 was prepared from metadinitroparaxylene by rcplacing the nitro-groups successively by amido- and hydroxyl- groups ; it is identical with Stenhouse and Groves's betorcinol (Trans., 1880, 396).The crude product obtained by nitrating paraxylene is crystallised from alcohol to remove most of the orthodinitroparaxylene, dissolved in hot alcoholic ammonia, and treated with hydrogen sul- phide for about one hour; i t is then evaporated to dryness. The paradinitro-compound, being more readily reduced than the meta- compound, is thus converted into paranitroparaxylidine, which is extracted by means of hydrochloric acid. The residue, insoluble in acid, was extracted with boiling alcohol, and yielded crystals of pure metadinitroparaxylene. This was reduced by dissolving in alcoholic ammonia and treating for two hours with hydrogen sulphide, and the nitroxylidine [ Me2 : 50, : NH2 = 1 : 4 : 3 : 51 so obtained was converted into the corresponding nitroxylenol. The latter crystallises in yellow plates melting at 91".It was reduced with tin and hydrochloric acid, and the amidoparaxylenol diazotised ; to 1 gram of the hydrochloride 10 grams of sulphuric acid and 100 grams of water were used, and the whole kept cold by means of ice and salt. Paraxylorcinol so prepared has all the properties ascribed to it by Stenhouse and Groves (Zoc. cit.), except that it yields a green fluo- rescent solution when treated with dilute soda and chloroform. Metaxylorcinol (Pfaff, Abstr., 1883, 918) crystallises from chloro- form in white monocliniccrystals, a : b : c = 1.7237 : 1 : ? ; p = 38" 21'. It boils a t 276-279". When heated with sodium carbonate solution a t lSO", metaayZol.ci,rLoZcurborylic acid, CsHMe2( OH),*COOH, is formed.40 ABSTRACTS OF OHEMICAL PAPERS.The latter crystallises from dilute alcohol in well-formed prisms which nielt with decomposition at 196", and give a deep blue coloration with ferric chloride. N. H. M. AcetalsesoscinoL By - CAUSSE (J, Pharm. [ 5 ] , 13, 354-358). -The author has examined the action of sulphuric acid and heat on a solution containing acetaldehyde and resorcinol. The crystals obtained are insoluble i n water, ether, chloroform, and ben- zeue. They are soluble in alcobol, which yields them again partly changed. Anhydrous ether dehydrates them, converting them in to II powder, which in time aggregates to yellow, translucent crystals. Thus purified, the compound decomposes on fusing with regenera- tion of resorcinol.Its composition is indicated by the formula c14Hl404 = C2H40 + 2C6H602 - H20. The action of heat on the compound apparently removes the elements of water. Heated a t 120°, a reddish powder was formed which could be obtained in large brown crystals. These had the composition CzeE,60, = 2CI4H,,O4 - The reactions indicate that the yellow crystals are st molecular combination of aldehyde and resorcinyl ether, C,l&O,O( C6Ha*OH)2. Benzylarnine. By T. CURTIUS and G. LEDERER (Rer., 19, 2462- 2463) .-When benzaldehyde and amidoacetic acid are heated together a t 130", carbonic anhydride is evolved and benzylamine formed. Similar reactions seem to take place when cinnamaldehgde, salicylaldehyde, or orthonitrobenzaldehyde, are substituted for the Benzaldehyde, but the products are not so easily isolated.Citric Acid Derivatives of Paratoluidine. By J. M. G:LL H2O. The diacetyl compound, C36H1B012, melts a t 28'2". J. T. L. T. T. (Ber., 19, 2352-2354) -Citroparatoluidide, C6H,04(NH.C7H7),, is obtained by heating citric acid (1 rnol.) and' paratoluidine (3 mols.) at, 140-145" for 10 hours. It crystallises from alcohol, in which it is sparingly soluble, in lustrous, microscopic needl'es, melting a t 189". Citrodlparatoluide, C6H504(NH*C7B7) N.C7H,, is formed when citric acid (1 mol.) and paratoluidine (2 mols.) are heated at 160-170" for three hours. . It melts at 205", is insoluble in water, rather readily soluble i n ether and alcohol, and separates from the latter solvent in small, yellow, well-formed crystals. When heated with citric acid at 140-145", it is converted into citroparatoluidide. Ammonia acts on it, yielding a salt of citrTaraditoluidic acid, C6H,04(NHC7H7)2*OH. The latter crystallises from alcohol in groups of needles, melting at 161".NC7H,, is prepared by adding paratoluidine (1 mol.) to a hot concentrated alcoholic solution of citric acid (1 mol.). On cooling, the solution yields clear prismatic crystals; these are heated for two hours at 160-170", and crystal- lised from water. It melts a t 172*5", and dissolves readily in alcohol, ether, and hot water. N. H. M. By 0: WALLACH (Annalen, 234, 350-364) .- Paxace tometatoluylenediamine, obtained by the action It is soluble in water, insoluble in alcohol and ether.Citroparafoluidic acid, C6H5O4(0H) Azo- and Diazo-compounds.ORGANIC OHEMISTRY. 41 of acetic anhydride on metatoluylenediamine (Abstr., 1883, 329) can also be prepared by converting nitrotoluidine (m. p. 77.5") into the aceto-compound (m. p. L44-5"), and reducing this substance with iron filings and acetic acid. By means of the diazo-reaction, the aceto- metatoluylenediamine is converted into acetamidocresol (m. p. 225"), proving t hatl the acetyl-group occupies the para-position. Parucetamidotolueneorthazodimethy lanild-ne, NHBc*C6H~e.N,*C6H4*N~e2, is formed when a, solution of the diazo-csmpound is poured into an ice-cold alcoholic solution of dimethylaniline. The substance crystal- lises in golden plates and melts at 200". It unites withacids to form salts, which dissolve in water, yielding deep-red solutions. The acetyl-group can be eliminated by boiling with dilute sulphuric acid.P(rramidoto1ueneorthazodimethy Ianilins mystallises in golden scales. It melts a t 145", and dissolves in hot alcohol, chloroform, and ben- zene. The diazo-compound unites with phenol, fomning totueneazo- dirnethy l a d b eparawphenol, NMe2.C6~*N,*C6H3Me.N2*CsH4*OH. . This substance dissolves in dilute solutions of the alkalis, and is reprecipitabed by carbonic acid. It also dissolves in strong acids, and is reprecipitated by the addition of water. It dissolves freely in alcohol, ether, chloroform, and benzene. It is insoluble in water, sparingly soluble in alcohol, b u t dissolves in strong sulphuric acid, with a red coloration.Pai.acRt~idotoluensorthazodiethzJlaniEine crystallises in needles of a reddish-brown colour. It melts at 159", and dissolves freely in alcohol, ether, chloroform, and in acids. The sdts are decom- posed by large quantities of water. Orthacetometatoluylenediamine, NHAc*C6H&le*NH, [Me : NHAc : NH, = I : 2 : 41, prepared from orthoamidoparanitrotoluene (m. p. 107"), crystallises in white needles, and melts at l4W. It is soluble in alcohol, in ether, and in hot water. Orthacetamidotolzceneljarazodintethylamili,ne melts at 192", and dissolves freely in almhol, chloroform, benzene, and ether. Orthamidotoluene- parazodirnethyllanili~~e melts at 215P, and is freely soluble in chloroform, Acetnmido b ,onZen emet azodimet h y landhe, NH Ac*C,H,*&*C,H,*NMe,, crystallises in plates, and melts at 184".Amidobenzenmzodimeth?yl- aniline forms golden scale% soluble in alcohol, which melt at. 165- 166". w. c. w. The corresponding P-naphthol-compound melts about 24". Quinone-oximes. By 3;. SUTKOWSKI (Ber., 19, 2314-2317).- When thymoquinone-oxime is dissolved in cold, fuming hydrochloric acid, a yellow precipitate is formed, consisting of dichlorothymo- quinone and monochlbramidothymol (Andresen, Abstr., 1881, 590). When the precipitate is boiled with glacial acetic acid, a splendid red dye is formed. The reaction is of interest, as itl d ~ o a s the analogy between the Beactions of thymoquinone and of thymoquinone-oxime with fuming hydrochloric acid. Andresen also obtained the same products from thymoquinonechlorimide. The oxime is therefore the hydroxyl-derivative corresponding with the quinonechlorimide.42 ABSTRACTS OF CHEMICAL PAPERS.When chloramidothyrnd hydrochloride and chloranil are hmted in glacial acetic acid solution, the red dye above mentioned is formed. Tetrachloroquiriol is formed in the reaction ; it crystallises in long colourless needles melting at 832". Analyses of the dye point to the formula C30H35C13N203. In a similar manner, a dye was obtained by the action of parsmido- thymol on chloranil in glacial acetic acid solution. It has the cam- position expressed by the formula C,H38N203. (It dissolves in acetic acid, alcohol, ether, and benzene, but not in water. Ammonia dissolves it with formation of a blue solution. Lead acetate gives a blue preoi- pitate.N. H. M. By M. LOEB (Ber., 19, 2340-2344) .-- When the compound Cl6Hl2N2CI2O2, prepared by the action of car- bony1 chloride on ethenyldiphengldiamine (Abstr., 1885, ,1213), is treated with alkalis or acids, it is reconverted into the amidine. Boiling water has no action on it ; 'boiling alcohol converts it into carbanilide, ethyl acetate, and ethyl chloride. The ethyl salt, OEt*CO*NPh*CMe : N*C6H4-COOEt, separates from its ethereal solp- tion in hard, lustrous, rhombic crystals which melt at 90.5". When the chloride is dissolved in benzene and treated with dry ammonia, i t is converted into ethenyldiphenyldiamine and ammonium chloride ; aniline acts like ammonia. Amidine-derivatives. Ethenylimidobenzanilide, CMe<,,,>CO, N.CeH4 is prepared by the action of carbonyl chloride dissolved in benzene on an excess of ethenyldiphenyldiamine ; i t crystallism from benzene in large, lustrous plates melting at 118".It is identical with the compound to which the formula CO( C11H13N2)P was previou-sly ascribed (Zoc. cit.). Dilute hydrochloric acid decomposes it wihh formation of aniline and phengl cyanate. When a saturated ethereal solution of ethenyldiphenyldiamine is treated with two or three drops of water and then with cyanogen until it has a wine-red colour, and allowed to remain for 16 hours, a black crust is formed which yields a compound, C16H16W40; the latter forms a white, crystalline powder very sparingly soluble in ether and benzene, and cannot be recrystallised, as it at once resinifies when heated with solvents.It becomes violet at ;120", and melts with decomposition at 165". Its constitution is probably analogous to that of Griess' cyanocarbimidoamidobenzoic acid, as shown in the formula NPh : CMe*NPh*C(NH)CN + H20. Ethyl allophanate is formed when urethane (7 partsl) and carbonyl chloride (1 part) are dissolved in benzene and heated at 75". N. H. M. Preparation of Aromatic Amides. By 34. FEILETII (Gaxzei%a, 16, 281--284).-The method, proposed by Letts, for the preparation of the nitriles by heating the carboxylic acids with potassium thio- cyanate, has been shown to yield the amides, if ammonium thio- cyanate be substituted for the potassium mlt. The former chaiige is attributed by Keku16 to the greater dehydrating action of the potassium salt, an interpretation confirmed by the observation ofORGANIC CIIEMISTRY.48 Muller that in the above method benzamide is formed if the process is conducted quickly, but phenyl nitrile if slowly. In the course of the preparation of cumonitrile, a small quantity of cuminamide is obtained from the crude product of the reaction, if the aqueous solution, prerioudy rendered alkaline by ammonia, is agitated with benzene. This amide crystallises .in glittering lamins melting a t 153*5", insoluble in cold, sparingly goluble in hot water, soluble in alcohol. It is not decomposed by boiling with hydrochloric acid or potash of moderate concentration. With mercuric oxide, i t yields a derivative, ( CsH4Pr*CONH),Hg + 1+H,O ; this crystallises in needles melting a t 190", insoluble in water, soluble in alcohol.V. H. V. Action of Alkyl Iodides on Dibenzylthiocarbamide. By C. REIMARUS (Ber,, 19, 2348--2349).-Will has shown (Abstr., 1882, 723) that alkyl iodides react with diphenyl- and dibenzyl-thiocarb- amide, with formation of hydriodides of bases in which the alkyl- group is directly combined with sulphur. The author has found that the isomeric dibenzykthiocarbamide behaves analogously. Brnzy Zimidobei,zyZcarbuminethiomefhg I, SMe-C (NHCTH,) : NC7H7, is formed when methyl iodide and dibenzylthiocarbamide are heated for 2-3 hours at 100". Thelproduct is dissolved in water, treated with sodium carbonate, and extracted with ether. The suZphate of the base crystallises in lustrous needles readily soluble in water and alcohol ; i t melts a t 145". The hydrochloride forins large rhombic plates melting a t 125" ; the h!jdriodide crystallises in splendid octahedrii melting at 99", readily soluble in hot water.Benzy ZimidlJbelzzy Zcarbaminethioet~i yl, SEt.C(NHC&) NGTH,, crys- tallises in wide prisms, apparentlF monoclinic, which melt at 93" ; it dissolves readily in alcohol, sparingly in water. %he suZphate forms large rhombic plates readily soluble in water and alcohol ; the plutiiio- chloride crystallises in needles. Corresponding compouuds were also prqpared from propyl iodide and amyl iodide. Phenylseleniocarbimide and Diphenylseleniocarbamide. By H. STOLTE (Ber., 19, 2350-2352).--Yh enyZseZeniocarbimide, CSe*NPh, is prepared by passing hydrogen selenide into aqueous soda, evapo- rating, and adding isocyanophenyl chlolride diluted with ether to prevent the reaction becoming too violent.After a day, the product is filtered, the ether evaporated, and the residue steam-distilled and dried in a vacuum over sulphuric acid. It is.a yellowish-red oil, insoluble in water, readily soluble in alcohol and ether, and has only a slight odour. When the ethereal solution of the substance is treated with ammonia, it is converted into monophenylseleniocarb- amide (Abstr., 1886, 781). Di13heiayZseleniocurbur)aide, CSe (NHPh),, is prepared from phenyl- seleniocarbimide by treating its ethereal solution with aniline. The product is washed with ether, and crjstallised from alcohol. It melts at 1M3 with decomposition. N. H. M. N. H. 31.44 ABSTRACTS OF CHEMICAL PAPERS. Substituted Nitrogen Chlorides.By G. BENDER (Ber., 19, 2272--2274).-When the compound C,H4<-5H> CO (this vol., p. 38) is treated with bleaching powder and hydrochloric acid the cowpomzd C7H,N02C12 separates in colourless needles. When the latter is brought into contact with quinol, an odour of quinone is given off, and on cooling crystals of quinhydrone separate. The componnd is decomposed by alcohol, alkalis, aniline, &c., into the =TTT compound C,H,Cl<f~>CO (Zoc. cit.) . Acetanilide, when treated with bleaching powder in presence of acetic acid, yields the compound NPhCl*COMe. The latter has the properties of the compound described above. It melts at 91' ; when heated to.l72", it becomes yellow, effervesces violently and is converted into its isomeride, parachloracetanilide, melbing at 172".The same change takes place when the substance is treated wibh cold hydro- chloric acid or when warmed with absolute alcohol; if more t,han 2 grams be employed, a violent explosion takes place. The compound reacts with paranitranibine, yielding acetanilide and ort bochloropara- nitrani line. The comPound <C&CO cH2*co >NC1 was prepared from succinimide : it crystallises from benzene in large colourless crystals melting at 148". Ihnaamide yielded the cornpzclzd COPh*N€€Cl. This crystallises fPom water in long prisms melting at 116". Condensation of Nitrobenzaldehyde with Hydrocarbons. By 0- TSCHACHER (Ber., 19; 2463-2464).-Baeyer has shown that fatty aldehydes, in the presence of concentrated sulphuric acid, form condenmtion products with aromatic hydrocarbons, whilst aromatic aldehydes do not.The author finds that the ilbtroduction of a nitro- group into the phenyl-ring gives to aromatic aldehydes the power of forming such condensation products With benzene, metanitrobenzaldehyde yields metanitrotripheny2;- methane, forming crystals melting at 90". With toluene, rnstanitro- phenydditoly ZmethaNe is formed. N. H. M. L. T. T. Compound of Pymvic Acid with Hippuric Acid. By A. HOFFMBNN (Ber., 19, 2554--2557).-6 grams of pyrnric acid were di esCed with 11 grams of sodium hippurate and 25 grams of acetic aniydride on a water-bath. In a short time, a vigorous reaction takes place and the temperature of the mixture rises to 108". The producf is dissolved in alcohol, the solution diluted with water, evaporated, and the brownish crgstala recvystallised from petpoleurn. Analyses of the compound point to the formula CJ&NO4; the sub- stance is therefore formed by the iinion of its two constituents (equal mols.) with elimination of the elements 0% water (2 mds.).I t forms colourless, flat needles melting at 157"'; iD is very readily soluble i n alcohol, ether, and acetic acid; insoluble in water. It yields salts corresponding with a, bibasic acid, C1'LHllNOO. The barium salt, Cl2HEN'O5Br + 2H20, was prepared; when treated with acid, itORGANIC CHEMISTRY. 45 yields the anhydride, ClzH9NOa, the acid not being capable of existing in the free state. When the anhydride is heated with hydrochloric acid at 140°, benzoic acid is formed. N. H. N. Phenyliodohydracrylic Acid.By E. ERLENMEXER and J. ROSENHEK (Ber., 19, 246&2465).-Ph eny l i o d ~ h y d r u ~ m ~ l ic (a-iodo- 6-pheny Zh ydroxypropionic) acid, OH-CHPh-CH I*COOH, was obtained by theaction of iodine chloiPide on cinnamic acid. A chloriodophenyl- propionic acid is probably fimt formed, whieh is then converted into the hydroxy-acid by the action of water. The acid forms large crystals which melt with decomposition at 137-139", and are soluble in benzene. When treated with hydrochloric acid, this acid yields a compound C18H16CI104, which the author believes to have the formula n CHPh : CHG (OH) <g>C(OH) *CHI. CHClPh. L. T. T. Creasolcarboxylie Acid. By H. WENDE (Ber., 19, 2324-2327). -CreosoZcarbozylk acid, OH*C6H2&fe(O?Y1e).COOH [= 4 : 1 : 3 : 51, is prepared by gradually adding 4 grams of sodium to 50 grams of creosol through which a current of dry carbonic anhydride is being passed.The reaction takes place slowly with evolution #of hydrogen and slight development of heat, and is assisted by gently warming; much heat is then developed, and the reaction becomes rather violent. The product, when cold, is treated with dilute hydrochloric acid, extracted with ether, and the ethered solution extracted with sodium carbonate solution. It erystallises in needles melting at lHO-lX'i', dissolves sparingly in water, readily in alcohol, ether, and chloroform, and is almost insoluble in benzene and light petroleum. It sublimes unchanged when carefully heated, and aequires a deep blue colous when trea%ed with ferric chloride.The ammonium saIt crystallises in globular groups of needles ; the potassium salt forms small, readily soluble needles ; the barium salt is sparingly soluble ; the copper salt is a yellow powder; it is very electric when dry. The inethyl salt forms small, rhomhic crystals, a : 'b : c = 0.5285 : 1 : 0.7334 ; it melts at 92", and gives a bluish-green coloration with ferric chloride. The ethyl salt crystallises in s m d l needles or prisms melting at 77". N. H. M. Derivatives of Op'ianic Acid. By C. LIEBERMAWN (Ber., 19, 2275 - 2287 ; compare Abstr., 1886, 550). - Amidohemipinphenyl- ,C : N -- NPh hydrazide (az~ianpheny lhydrnzide), NH( I I , is prepared C6H ( OMe) 2mc 0 by the action of phenylhydrazine on azopianic acid. It separates from its solution in benzene in small, honey-coloured, tetragonal crystals, having a glassy lustre, a : c = 1 : 0.5947. It melts at 222", and dissolves in strong sulphuric acid and in fuming hydrochloric acid.Amido-opianpheny7hydrazide, NH2*C6H(OMe)2<-CH CO-NPh N->, is ob- tained by reducing the nitro-compound (Zoc. cit.) with tin and fuming46 ABSTRACTS OF CHEMICAL PAPERS. hydrochloric acid, care being taken t o prevent the reaction from becoming too violent from the heat developed. On adding water to its alcoholic solution, it crystallises in slender needles melting at 157 -143". is formed when nitro-opianphenylhydrazide is boiled with alcoholic potash, and the potassium salt thus obtained' treated with hydro- ehloric acid. It crystallises in Fellow, glittering, rbombic plates melt- ing at 191". The potassium salt is a carmine-red powder.Oyianoxime anliydride (hemipiniinize), CJ&NO,, is prepared by boil- ing opianic acid (1 mol.) dissolved in nine times its weight of 80 per cent. alcohol with, hydroxylamine hydrochloride ( I t mol.) for two to three hours. It crystallises from alcohol in long, very slender needles melting at7 228-230". An aqueous or alcoholic solution con- taining only a trace of the subdance has a fine blae fluorescence. It sublimes unchanged, and can be heated with strong sulphuric acid without decomposition. Cold aqueous a1 kali dissolves it, forming a, yellow solution which soon ldecomea colourless. When heated with alkali, it, yields hemipinic acid and ammonia. The compound was alm prepred by heating ammonium hemipinate.The potassium salt, CloH80NK, is a white compound almost insoluble in cold absolute alcohol. Hemipinethyl imide, ClnH804 : NEt,.is obtained by heating potassium hcmipinimide with ethyl iodide at 150". It crystallises from boiling water in colourless- needles resembling hemipiuimide ; the solution shows the same fluorescence. It diksolveR very readily in alcohol, acetone, and benzene, and melts a t 96-98". The formation of hemipinimide is interesting on account of its complete analogy with observations lately made in the phthalic acid series. The author a,ssigns to the compounds phthalimide and hemi- pinimide the respective constitutional formulae. CO<-O'>C : NH 0- and Co<G,(OMe), Anilido-opianic acid, Cl6HI5NOd, is obtained by boiling a solution of equal weights of opianic acid and aniline, dissolved in gIacial acetic acid, for 10 minutes.On cooling, the whole solidifies to a, white mass, which is washed with water, dissolved in benzene, and precipitated with ether. It dissolves only in Btrong alkali solution. Artilidonitropianic acid, C16H14N20s, is prepared from ni tr- opianic acid in a manner similar t o the above compound. It, cr-ystal- lises in needles melting a t 183-184". When treated with alkali, it yields n sparingly soluble potassiwn salt. Nitrohemipinic acid, K02*CsH(OXe)2(COOH)o, is very readily p1.e- pared by boiling nitropianic acid with fuming nitric acid (4 parts) for one hour. It melts a t 166" (not 155"), but has all the other properties ascribed to it by Prim (Abstr., 1882, 402).Wben heated above its melting point, it gives up water and yields a yellowish compound, probably the anhydride. The silver s@Zt was also prepared. c6H4 >C : NH. It melts at 186-187'.ORGANIC CHEMISTRY. 43 Opianic anhydride, [ CHO*C,H,(OMe),*CO],O, is formed when opianic acid is heated at 160" in a current of dry air. It crystallises well from acetone and melts at 234". It is identical with the coni- pound described by Wegscheider (Ahstr., 1883, 996) as triopiarnide, 0,H,aO14. When boiled with alkali, it, is gradual17 transformed into opianic acid. Strong nitric acid converts it into nitropiauic acid. Opianic Acid Derivakives. By C. IJTEBERMANN and S. KLEEMAKN N. H, M. (Ber., 19, 2287-2299).-AcetyZupinnic acid, is prepared by heating opianic acid and dry sodium acetate with acetic anhydride.The excess of. acetic anhydride is then removed by contact with cold watey for 24 hours, and the remaining compound crptallised from boiling water. It is inso- luble in cold aqueous alkali, and when boiled with it, is decomposed into opianic and acetic acids. >CH*OAb, is prepared Acetylnitropianic acid, < in a manner similar to acetylopianic acid. I& is a yellow substance insoluble in cold sodium carbonate solution. Propiony lopa'anic acid, C13H1406, crystallises in needles melting at 111". An hyaraceta nt id oh emip inic acid, G ,,H,AcN O,, and trhe pi-opion y 1- compound, C,,H,( C3H,0)N0,, melt at 164" and 139" respectively ; they ape very unstable. )CH*CH,*COO@ is obtained by heating opianic acid (3 parts), rnalonic acid @+ part), glacial acetic acid (2 park), and sodium acetate (li Rart) for five hours at 100" ; the colourless, crystalline product IS crystallised from water.It forms lustrous needles melting at 167" ; it has an aoid reaction and dissolves i n ammonia. The silver, calciunz, &c., salts were prepared. The ethyl salt crystallises in plates soluble in alcohol, ether, and hot water; it melts at 82.5". The reactions of the acid are analogous to those of phthalylacetic acid. When boiled with baryta, and the excess of baryta afterwards removed by means of carbonic anhydride, barium opianylacetate" is obtained ; it forms lustrous prisms. The free acid is not capable of existence. When the silver salt is treated with methyl iodide, it yields, not methyl opianjlacetate, but methyZ m ecoiline-acetate ; the latter crystallises in lustrous plates melting at 124".It melts at 120-121". (JO--- C6H(N0,) @Me), co- CsH2(0Me)2 Necouiw-acetic acid, < >CH*CH,*COOH, is pre- co--0 Normecortine-acetia acid, <C,H,(OH), pared by heating rneconine-acet& ahd with hydriodic acid and phos- phorusi ; the product is diluted with water and filtered. It crystal- lises from water in long plates melting a t 218". The calcium and buriuwt saZts form white crystalline precipitates. When the acid is * The fmmtda slnd azalp:s given in the original do not agree.48 ABSTRACTS OF CHEMICAL PAPERS. heated with ferric chloride, it acqfiires a characteristic blue colour, which changes to green in presence of an excess of ferric chloride, The ethyl salt separates from its solution in boiling water as an oil, which then solidifies and melts at 131".Its solution is fluorescent and reduces silver solution, but to a smaller exbenltthan the free acid. I t has an acid reaction and precipitates from baryta solution a yellow barium salt of the ether. This acid property and the power of reducing silver solutions is due t o the presence of pylrocatechol- hydroxyl. Ort h onitrom econine- acetic acid, co -o>CH.CH2*COOH [NO2 : CH*CH2*COOH=1 : 21, <C,H(N02) is obtained by dissolving meconine-acetic ncid in fuming nitric acid and afterwards precipitating with water. It forms colourless crystals melting at 176". The ethyl salt crystallises in lustrous needles, rcadily soluble in alco'hol and benzene ; it melts at 129".Nitromeconine-acetic acid dissolves in sulphnric acid, forming a. yellow solution ; this, when warmed, acquires a cherry-red colour, characteristic of compounds containing a nitro- group in the ortho-position to a long side-chain (Baeyer, Abstr.. 1882, 620). When the nitro-compound is reduced with tin and hydro- c hloric acid, dimethox y hy drocarbostyril- lactone, The calcitwt saZt forms yellow needles. is formed. This crystallises from water in colourIess needles, melt- inq with evolution of carbonic anhydride at 256". It is readily soln'ble in alcohol and glacial acetic acid, insoluble in ether and benzene. It dissolves in baryta; when the solution is boiled and treated with carbonic anhydride and evaporated down, Iastrous needles of barium dimethoxyhydrocarbostyrilcarboxylate are ob- tained.Dilnetliox~IddihydrochZoroquinoline lactone, 6C12Hl0N Clod, is prepared by heating the lactone just described with phosphorus pentachloride and some phosphorus oxychloride for two hours at 165-170"; the product is poured into iced water, and the precipitate crystallised froni alcnhol, from which it separates in needles ; these melt at 218" with evolutim of carbonic anhydride. The barium) salt, obtained by boiling the lactone with baryta, and the silver salt were prepared. Dihydroxydihydroquinoli?ie lactone, CloH,IIU'O,, is obtained by heating the above chloro-derivative dissolved in glacial acetic add for one hour at 120" with hydriodic acid. It melts at 220" with decomposition. By H. GRCNR (Ber., 19, 2299-23@5).- Azo-opianic acid, prepared from nitropianic acid, melts at 200" with decomposition (not 184" as given by Prim, Abstr., 1888, 404).The pofassium salt is a white crystalline powder. The et?iyl salt crystal- 1ises in needles melting at 98" ; the methyl salt melts at 127". The author confirms the statement of Prinz ( ZOC. cit.) that azopianic acid, when boiled with barytzt in excess, yieIdrJ barium amidohemipinate N. H. M. Azo-opianic Acid.ORQAXIC CHEMISTRY. 49 The yield is almost quantitative. Sodium amidohenzipinate crystallises from alcohol with 3 mols. H,O, in long, almort white needles ; it is very readily soluble in water. The copper salt (with i mols. H,O) erystallises in stellate groups of slender, green needIes. The aqueous solution of the free acid has a fine green fluorescence which disappears when alkalis or acids (except acetic acid) are added. It reduces a cold animoniacal silver solution, and Fehling's solution when warmed.ob- tained when a cooled solution of sodium amido-hemipinate is treated with sodium nitrate and hydrochloric acid. It is a bright yellow, micro- crystalline powder which becomes superficially red when exposed to light, and explodes at 140-150" or when struck. It dissolves readily in alkalis and acids ; when boiled with water, it gives off nitrogen and yields a hydroxy-acid, which gives an intense blue-violet colour with ferric chloride. The hydrochloride, COOH*CsH( OMe),( COOH)*N,Cl + H20, crystallises in long, colourlew needles ; in presence of water, it decomposes into hydrochloric acid and free anhydroazohemipinic acid.When the diazohemipinic acid is boiled with alcohol undsr slight pressure, it is converted, with evolution of nitrogen, into hemi- pinic acid. Nitrohemipinic acid was prepared by Liebermann's method (this vol., p. 46). The potacsium sult crystallises in deep yellow prisms, readily soluble in water and alcohol, the silver saZt is also yellow. 21Titrohen2ipinic rcnhydride, NO,*CsH( OMe) <co > 0, is prepared by heating the acid at 160-165" for two hours ; it crystallises from benzene in bright yellow prisms melting a t 145". When nitrohemi- pinic acid is reduced with ferrous sulphate and soda, amidohemipinic acid is formed identical with the acid obtained by boiling azo-opianic acid with baryta. The results of the experiments above described confirm the view brought forward by Liebermann (loc cit.) that Prinz's so-called azo- opianic acid is not an azo-derivative of opianic acid but an internal anhydride of orthamidohemipinic acid.When nitrohemipinic acid is reduced with tin and hydrochloric acid, the compound COOH.C6H,( OMe)2*NH2,HC1 is formed. N. H. M. Derivatives of Normethylnitropianic Acid. By K. ELBEL (Ber., 19,2306-2312) .-Normethylnitropianic acid COH* C6H ( C 0 OH) (OH) ( OMe) *NO,, is best prepared by heating finely powdered nitropianic acid with fuming hydrochloric acid (10 parts) for 15 hours at loo", with a reflux condenser, hydrogen chloride being passed in all the time. The product is evaporated down, when the normethyl-compound sepa- rates ; the yield is 80 per cent.of the theoretical. Normethylorthanhyd~-lzmidohemipinic acid (normethylazo-opianic acid), OMe*C6H(OH)(COOH)<~~> [OMe: OH : COOH : CO : NH = 4 : 3 : 2 : I : 61, is obtained by treating a boiling saturated aqueous N,-0 Anhydrodiazohenzipinic acid, COOH*C6H(O~e)2< co >, is co VOL. LII. e50 ABSTRACTS OF CHEMICAL PAPERS. fiolution of normethylnitropianic acid with tin and hydrochloric acid. It is dissolved in alcohol and precipitated with water. It crystallises i n colourless, lustrous needles which melt at 174-175" with decom- position ; i t is readily soluble in alcohol, sparingly in benzene, and insoluble in ether. When boiled with baryta, crystals of barium normet h ylamido hemi pinate are formed. The diacety I-d erivative, O&fe*C6H(OAc) (COOH)<NA:>, co oMe*C,H(oAc)(CooH)<,,>, co melting at 198'.is obtained by boiling normethyl- anhydramidohemipinic acid with sodium acetate and acetic anhydride (10 parts) for one hour. It melts a t 205", dissolves readily in ben- zene; the alcoholic solution has a fine blue fluorescence. It is very unstable and changes when kept into the monacetyl compound, Normethy/nit?.opianic acid phenylh ydrazine crystallises in red needles which melt a t 178-179" with decomposition. When boiled with glacial acetic acid, it parts with the elements of water and yields norrnethy Znitropiaxide, No2*C6H(0Me) (OH) < ca: : N->. The latter crystallises in lustrous, lemon-coloured, rhombic plates melting at 191". I t dissolves unchanged in dilute potash solution.The potassium salt is very readily soluble in water, almost insoluble in absolute alcohol. Normethy Zamido-opiaxide is obtained by boiling the nitro-compound suspended in ammonia with ferrous sulphate. It crystallises from alcohol in short, almost colourlesv prisms. CO*NPh Normethy1rritro~'anoximic acid, NO2*CsH(OMe) (OH)(COOH)*CH :NOH [ = 6 : 4 : 3 : 2 : 11, is formed b;j- mixing a boiling solution of normethylnitropianic acid in water (40 parts) with an aqueous solution of hydroxylamine hydro- chloride and sodium acetate. It crystallises from alcohol in lustrous yellow needles which become brown when warmed, and melt at 252". It has a slight reducing action on Fehling's solution. It dissolves in alkali with SL deep-red colour, and the solution gives off ammonia, when boiled, with formation of normethylnitrohemi~inic acid, NO,*C,H(OMe) (OH)(COOH), [ = 6 : 4 : 3 : 2 : 11.The latter crys- tallises from alcohol in almost white, silky needles, readily soluble in water and alcohol; it melts at 220". The hydrogen potassium salt forms bright yellow prisms. The same acid is formed when nor- methylhemipinic acid is nitrated with dilute nitric acid, Normethylnitrohemipinimide, N02*C6H( OMe) (OH) <C CO.0- H)>, is obtained by boiling an alcoholic solution of normethylnitropianic acid with hydroxylamine hydrochloride, or better by boiling normethyl- nitropianoximic acid with glacial acetic acid. It crystallises in bright yellow needles which melt a t 252" with decomposition. Homo-orthophthalimide. By S. GABEIEL (Ber., 19,2363-2367 ; compare Abstr., 1886, 812, and this vol., p.61).-When a solution of homo-orthophthalimide (2 grams) and potash (1 gram) in methyl alcohol (15 c.c.) is digested with methyl iodide (4 grams) at loo", N. H. M.ORQANIC CHEMISTRY. 51 dimethylhomo-orthophthalimide, CgH5Me2NO2. is formed. The latter crystallises from water in flat needles melting at 119-120"; it is readily soluble in the usual solvents and in alkali. When heated with potash and methyl iodide a t loo", it yields the trimethyl- derivative, CDHaMe3NO2 ; this cry stallises in long needles melting at 102-103" : it is readilv soluble. Alkali does not dissolve it. CH G O Howio- ort hophthalmeth y limide, C&< .kMe > , is formed by evaporating a mixture of homo-orthophthalic acid and methylamine, arid distilling the residue.It forms long, colourless needles, which melt a t 123" and boil at 314-318". I t is readily soluble in the usual solvents and dissolves in alkalis. When heated with methyl iodide and potash, it yields trimethylhomophthalimide melting at 102-103". In the latter compound, therefore, one of the methyl-groups is attached to nitrogen. Trimethylhomophthalimide is hardly attacked by fuming hydrochloric acid at 100", and so cannot contain methoxyl; when heated with the fuming acid a t 230-240", the anhydride of a co This crystallises in flat crystals melting at, 82.5-83" ; the silver salt, Cl1HI6OkAg2, was pre.. pared. The anhydride is also formed when dimethylhomophthalide (fi-om homophthalide, potash, and methyl iodide) is heated a t 230" with fuming hydrochloric acid; ammonia is formed in the reaction.Tri- and di-methylhomophthalimide and the anhydride (m. p. 82.5433") have probably the constitution expressed in the formula- , bibasic acid, C,H,Me,<CO>O, is obtained. Action of Amines on Phthalylacetic Acid. By E. MERTENS (Bey., 19, 2367--2373).--Pure phthalylacetic acid is stiriaed with water and treated with a 33 per cent. solution of ethylamine until it is dissolved ; it is then filtered and saturated with hydrogen chloride, being kept cold the whole time. A white crystalline substance gradually separates with ,slight evolution of carbonic anhydride, Analyses show the compound to have the formula C~~&,O~NZ. It melts at 129", dissolves readily in warm alcohol, ether, and chloro- form, more sparingly in benzene ; boiling water decomposes it.2Methylei~eyphthalethimidine, CO< z g i > C CHz, is formed when the compound C,H,,O,N, is heated above its melting point ; carboriio anhydride and water are evolved. It has a carrot-like odour, distils with steam, and is readily soluble in alcohol, ether, and chloroform, &c. It strongly resembles Gabriel's methylenephthalomethimidine (Abstr., 1885, 1228). Phthalethimidylacetic acid, C@< %g(>C : CH-COOH, is obtained by keeping a solution of the compound C,H24N205 in sulphuric acid (10 parts) for 24 hours, and then pouring it into water. The white crystalline precipitate is crystallised from dilute alcohol, from which it eCL52 ABSTRACTS OF CHEMICAL PAPERS. separates in yellow needles melting a t 180" with effervescence.It is readily soluble in hot water, alcohol, and ether, less soluble in benzene. The silver salt forms a flaky crystalline precipitate; the barium saZt crystallises in yellow lustroufi needles. Propylamine and phthalylacetic acid yield the compound C,,H,,O,N,. It forms large well-formed prismatic crystals which melt with effervescence a t 103". It behaves similarly to the ethylamine compound. Acetophenone-orthocarboxa.,7iZideJ COMe*C6H4*CO*NHPh, is obtained by warming phthalylacetic acid with aniline. After the evolution of carbonic anhydride has ceased, the whole is left for 24 hours, when the substance separates in white crystals. It crystallises from benzene in large, well-formed cubes which melt at 189- 192", and dissolve readily in warm alcohol, ether, or chloroform.When heated a t 204" and afterwards a t 2.30". it is converted with evolution of aniline and water into rnethylene~hthal~~enimiLJine, CO<::~>C CH,. The latter crystallises in yellowish prisms readily soluble in alcohol, ether, and chloroform; it melts at 100". When acetophenonecarboxanilide is kept dissolved in strong sol- sulphuric acid for 24 hours, it is converted into a compound, C16H11N0, isomeric with the compound just described. It is sparingly soluble in alcohol and ether, readily in benzene, chloroform, and light petroleum ; it melts at 265". N. H. M. Bromoterephthalic Acid. By M. FILETI (Gaxzetta, 16, 284- 287).--Pischli (Abstr., 1879, 639) states that the monobromotere- phthalic acid obtained by the oxidation of bromotoluic acid retains 1 mol.H,O, even after drying a t 120". As the same acid obtained from bromocymene was found to be anhydrous, the author has repeated Pischli's experiments. The analytical results obtained for the proportion of carbon and bromine show that this acid is also anhydrous. Its silver salt is precipitated as a white, gelatinous mass, somewhat soluble in water. The methyl saZt, C6H,Br(COOMe)2, obtained from the said chloride (Fischli), as also from the acid itself (Fileti), crystal- lises in acicular prisms, melting at 5 2 " ; it presents a well-marked chromatic polarisation. V. H. V. It melts a t 296", and at the same time sublimes. Curnidic Acids. By E. SCHNAPAUFF (Ber., 19, 2508--2511).-The author prepared a-cumidic acid, C6H&fez(GOf)H,), [Me : Me : COOH : COOH = 1 : 3 : 4 : 61, by a modification .of Wurtz's process, by the action of efhyl chloro- carbonate and sodium amalgam on dibromometaxylene, This acid forms glittering prisms melting much above 320"' and subliming with only slight decomposit,ion.It is easily soluble in boiling alcohol, very sparingly in boiling water. Its barium salt crystallises with 1+ mol. H,O, and is very soluble in water: the methyl salt forms long needles or plates and melts a t 76". Cumidic acid, obtained as described by Jannasch (this Journal, 18'71, 240) by the oxidation of durene, was converted into the methylORQANIC CHEMISTRY. 53 salt, and this by crystallisation from alcohol was separated into two parts, the one melting a t 76" the other crystallising in needles and.melting at 114". The former was the methyl salt of the a-acid j u s t described. The ether melting a t 114" yielded @-cur/lidic acid [Me : Me : COOH : COOH = 1 : 4 : 2 : 51 on hydrolysis. This acid is easily soluble in boiling alcohol, very sparingly in boiling water ; it rr\-stnllises in hexagonal prisms, and sublimes at high temperatures without previous fusion. Its barium salt crystallises with 24 mols. H20; its methyZ salt melts at 114" and boils at about 297" (corr.). When the barium salt is distilled with excess of lime, paraxylene is formed, so that the above formula may be regarded as established. Jannasch's acid is, therefore, a mixture of two isomeric cumidio acids. L. T. T. Reaction of Stilbene. By (3.ERRERA (Cazzetta, 16, 325).-Kade (Abstr., 1880, 46) states that stilbene in alcoholic solution gives a red coloration when heated with a solution of ferric chloride. It is here shown that this change is in reality due to the presence of water in the alcohol, which causes a partial decomposition of the ferric chloride into hydrochloric acid and some stable form of ferric hydroxide. Stilbene is not even necessary for the reaction ; if absolute alcohol is used no colour-change ensues. By T. ZINCKE (Ber., 19, 2493-25Q2) .-In the hope of elucidating the constitution of the two compounds, C3,H,,N,0s and CB1HP2NCOG (Abstr., 1882, 736, and 1883, 210), ob- tained by the action of nitrous acid on P-naphthaquinone-anilide and -toluide respectively, the author has undertaken similar investigations with phenanthraquinone.I n the present communication, the author details some preliminary experiments as to the action of alkalis on halogen-derivatives of /I-naphthaquinone, which were made to deter- mine whether @-naphthaquinone-deriva tives undergo changes similar t o the conversion, by the action of alkalis, of phenanthraquinone into di phenyleneglycollic acid. the action of bromine in acetic solution on p-naphthaquinone, and crystal- lising in red prisms melting at 177-178", dissolves readily in cold tlilute alkalis. From these solutions, acids precipitate hjdroxybromo- /3-naphthaquinone, described by Merz and Baltzer. Aniline and am- monia also act on bromo-/j-naphthaquinone, forming corn pounds analogous to naphthaquinoneanilide. Dibrorno - /3 - naphthayuino,he, [0 : 0 : Br : Br = 1 : 2 : 3 : 41, could not be obtained directly from naphthaquinone, but was formed by the action of excess of bromine on an acetic solution of the monobromo-derivative.It is best ob- tained, however, by the action of bromine on a-amido-p-naphthol. It crystallises in red: rhombic scales or tables, sparingly soluble in ;~lcohol and ether, and melts a t 172-174". With ammonia and aniline, it yields the same compounds as the monobromo-derivative. It dissolves in cold dilute alkalis, and from these solutions acids Irecipitate a substance, crystallising in small white needles ; this has not beeu further investigated. V. H. T. p-Naphthaquinorre. Rro.rrLo-@-nuphthaqIcinone, [0 : 0 : Br = 1 : 2 : 31, obtained54 ABSTRACTS OJ!' CHENICAL PAPERS.ChEoro-P-naphthaphone, [0 : 0 : C1 = 1 : 2 : 31, is formed when chlorine is passed through a solution of p-naphthaquinoiie in ten times its weight of glacial acetic acid, until a precipitate begins to be formed. It crystallises in red needles, soluble in alcohol, glacial acetic acid, and benzene, ahd melts a t 172". It gives an additive product with hydrochloric acid which forms white cr,ystals. It dissolves in dilute alkalis, and this solution when acidified yields hydroxychloro-a-naphthaquinone. The unstable p- hydroxy-compound undoubtedly first formed passes into the more stable a-derivative. When chloro-P-naphthzquinone is reduced with sulphurous acid i n acetic solution, chloro- p - naphthapuinol, C,H,Cl(OH),, is formed, and crystallises in long, colourless needles melting a t 116-117".The anilide and imide of chloro-p-naphthaquinone both crystnllise in dark-coloured scales having a metallic lustre, the former substance melting a t 253", the latter at 260". Dichloro-p-naphthczpi~inzone, [0 : 0 : C1 : C1 = 1 : 2 : 3 : 41, may be obtained directly from the quinone, but is best prepared by the action of chlorine on a-amido-p-naphthol. It crystallises i n red scales, needles, or tables, easily solnble in chloroform and boiling benzene, sparingly in alcohol, melts a t 184", and sublimes without decom- position. With ammonia or aniline, it forms the imide or anilide respectively. When reduced with sulphurous acid in acetic solution, it yields dichloro-/3-naphthaquinone, crystallising in white needles which melt a t 125". Ik dissolves in cold dilute alkali, and this Eolution when heated becomes cloudy, and deposits a greyish-white precipitate.If the cold alkaline solution be treated with excess of acid, an acid of the formula C,H,Cl?03 is liberated. This acid crys- tallises with 1 mol. H20 in small white needles, melts a t 98-100", and is easily soluble in alcohol, sparingly so in water. Its methyZ smZt forms colourless scales or hexagonal plates melting a t 13'7-138". The action of the alkali on the dichloroquinone appears to take place according to the equation C,oH4Cl,0, + H,O = CloH,Cl,O,. The author considers the action to be similar to the action of alkalis on phenanthrsquinone, and the most probable constitution of the acid t o he CCl<ccl:> C6 I3 C( OH)-COOH.The acid forms an ncety Z-dericative, melting at 75-76'. Boiling baryta-water or alkalis cause a separa- aion of carbonic anhydride. When a solution of the acid in glacial acetic acid is treated with concentrated sulphuric acid at 120", hydrogen chloride is evolved, and a yellow crystalline compound melting at 224-226" is produced. The acid is decomposed on heating its aqueous solution, a yellow compound of intense odour and volatile in steam being amongst the products of reaction. The experiments on the bromo-derivatives were carried out in conjunction with Weltner, those on the chloro-derivatives with C. Frolilich. L. T. T. Benzene- and Toluene-azonaphthols and their Isomeric Hydrazine-derivatives. By T. ZINCKE and I?. RATHGEN (Ber., 19, 2482 - 2493).- W $en the two position-isomerides, benzeneazo-p- naphthol and P-napl -thaquinonehydrazide (see Zinckc and Bindewald,ORGANIC CHEJIlSTRY. 55 Abstr., 1%35, 391), are reduced by means of stannous chloride, the former yields a-amido-@-naphthol, the latter P-amido-a-naphthol. When a-amido-/I-naphthol is oxidised, P-naphthaquinone is formed, but the authors find that p-amido-a-naphthol yields under similar conditions P - diriaphthaquinone (/3 - dinaphthadiquinone). Both quinones yield with bromine dibromo-p-naphthaquinone. When heated with nitric acid, benzeneszo-P-naphthol yields dinitro- P-naphthol, CloH5(OH)(N0,), [NO, : OH : NO, = 1 : 2 : 41, whilst p-naphthaquinonehydrazide yields dinitro-a-naphthol [OH : NOz : NO, = 1 : 2 : 41. When the above isomeric hydraside and azo-compound are reduced in alkaline solution, they are both decomposed into aniline and amido-naphthol. The author disputes the correctness of Denaro's assertion (Abstr., 1886, 246) that two isomeric benzeneazonaphthols can be obtained from p-naphthol.The authors have also investigated the corresponding toluene-deriva- tives. Pitratolueneazo-a-naphthol, OH*CloH6*Nz*C7H7 [OH : N, = 1 : 41, was prepared like the similar benzene-compound. It crys tallises in dark-red flakes having a metallic lustre, aud melts with decomposition a t 208". It is easily soluble in acetone, aniline, and alkalis, sparingly so in alcohol and acetic acid. No bromo-derivative could be obtained. Nitric acid yields dinitro-a-naphthol (b. p. 139"). The hydrochlorida and hydrobromide form bluish-green scales, which are slowly decom- posed by water, rapidly by alcohol.It also Eorms metallic derivatives. The ethoxide crystallises in red needles, which appear yellow by transmitted light, and melt a t 126-127"; the methoxide melts a t 103-104" ; the acetyl-derivative crystallises in yellow needles melting a t 101-102". Orthotolueneazo-a-naphthol, [OH : N, = 1 : 41, forms red needles melting a t 144-146', soluble in alcohol, benzene, and ncetic acid. It forms dinitro-a-naphthol with nitric acid, and yields salts resembling those of the para-compound. The sthoxide crys- tsllises in red scales melting at 94", the methoxide in reddish- brown needles melting a t 93". Para- and ortho-tolylhydrazides of a-naphthaquinone are identical with the corresponding azo-com- pounds.Parato Zuene-@naphthol, ClOH~ON,H*C,H7, or C10H6 (0 H) *Nz*C7R7 [0 : N, : : 2 : 11, forms red crystals with green flnorescence, is soluble in alcohol, benzene, and acetone, and melts a t 134-135". It forms very unstable salts with acids. The dibrorno-derivative forms intensely red needles melting at 190". Nitric acid converts the azo-componnd into dinitro -P-napht hol (m. p. 194"). 0 rthotol ueneazo +-nap ht h ol, [O : N, = 2 : 11, crystalliscs in small red needles or scales which melt a t 131". With nitric acid, it yields a dinitro-p-naphthol melting a t 167". The tolylhydrazides of P-naphthaquinone are, like the similar phenylhydrazide, isomeric and not identical with the nzo-compounds. They resemble them, however, very closely, the chief difference being their greater solubility i n alkalis. P-Naphfhaquinone-iuaratolylhydr- azide, CIOH60*N2H*C7H7 [0 : NP = 1 : 21, crystallises in small, red, glistening needles which melt at 145".The dibromo-dericative, CliH12B~-20, forms red, sparingly soluble needles melting at 236". B-NallhthapuinrJne-o~t~iotol~~li y draxide crystallises in red scales with a The P-derivative melts at 1!34", the a- a t 138".56 ABSTRACTS OF CHEMICAL PAPERS. golden-yellow fluorescence. It is easily soluble i n the usual solvents and melts at 156". Its dibromo-derivative melts at 254". Besides these hydrazides, the product of the action of the tolylhydrazinc on the p-naphthaq uinone always contained considerable quantities of di- naphthyldiquinol. L. T. T. New Diamidodinaphthyl.By P. JULIUS (Ber., 19,2549-2552). -am-Dinaphthyl is best prepared by distilling a-dinaphthol with zinc- dust (10-15 parts) : the distillate is re-distilled in a vacuum and recrgstallised from glacial acetic acid. Mononitrodinaphthyl, C10H7*C10H6*N02, is obtained by adding nitric acid, of sp. gr. 1.3 (20 grams), to a solution of dinaphthyl (10 grams) in 150 C.C. of glacial acetic acid. It crystallises in lustrous, orange- coloured plates melting at 188". It dissolves easily in hot benzene and glacial acetic acid, less readily in alcohol and ether. Dinitrodinaphthyl, N02*C10H6*C10~6*N01, is prepared by treating a solution of 10 grams of dinaphthyl in 150 C.C. of glacial acetic acid with 80 grams of nitric acid, and then heating at 60". It crystallises in bright yellow, volumiiious needles which melt at 280°, it dissolves very sparingly in benzene, xylene, and glacial acetic: acid, and is practically insoluble in other solvents.Uiczmidodinaphthyl hydrochloride, ~H,*C,oH6~C,oH60NHz,2H~l, is prepared by treating 10 grams of the dinitro-compound, suspended in 200 C.C. of glacial acetlic acid, with hydrochloric acid, and50 grams of zinc-dust. It is readily soluble in water, sparingly in strong hydro- chloric acid ; when exposed to the air, it quickly becomes green. The free base could not be isolated. The diacety 1-derivatiue crystallises in almost colourless needles which melt above 300" ; it is insoluble. When the hydrochloride is treated with ferric chloride, dark-brown, lustrous needles of diimidodinaphthyl h?ydrochloride, CZoH,,N,C1,, .are obtained ; this is reconverted by reducing agents into the diamido- compound.N. H. M. Tetrahydroxyanthraquinones. By E. NOAH (Ber., 19, 2337- 2340) .-When metahydroxybenzoic and gallic acids (equal mols.) are heated with sulphuric acid (10 parts) for 20 hours at 170", two tetrahydroxyanthrapuinones, ClaHa( OH),O,, are formed, together with hexahydroxjanthraquinone. The product is extracted with alcohol, the solution evaporated to dryness, and the residue extracted with benzene. The solution contains +now only one tetrahydroxyant hra- quinone. This crystallises in long, slender, red, lustrous needles, which do not melt at 350", and sublime with difficulty, becoming partly carbonised. I t is readily soluble in alcohol, acetone, and glacial acetic acid, sparingly in benzene, xylene, &c.The solutions in sulphuric acid and in caustic alkali are violet and emerald coloured respectively. The tetracety 1-derivative crystallises in yellow micro- scopic needles, which melt with decomposition at 207-2U9". The second tetrahydroxpnthraquinonc is extracted by means of dilute alcohol from the residue undissolved by benzene. It crystallises in small, red needles which do not melt at 380" ; it sublimes in small, yeilow needles, but is mostly decomposed. It dissolves readily inORGANIC CHXMISTRT. 57 alcohol, glacial acetic acid, and acetone, sparingly in ether and ~ a t e r . The solution in sulphuric acid is brownish-yellow; that in caustic alkali emerald-coloured. The tetracetyl-compound crystallises in lemon- coloured prisms, which are very readily soluble in glacial acetic acid, alcohol, and chloroform ; it melts at 189".N. H. M. Methylanthragallols. By E. L. CAHN (Ber., 19, 2333-2336 ; compare Abstr., 1886, 556).-l-~Methylanthragallol, is prepared by heating orthotoiuic acid (3 parts) with gallic acid (2 parts) for 12 to 15 hours up to 130-135". It crystallises from alcohol in gold-coloured flakes consisting of microscopic needles. It sublimes in long, orange-coloured needles, and melts at 297-298" with decomposition. It is readily soluble in hot alcohol and glacial acetic acid, sparingly in benzene ; it also dissolves in hot water, yield- i n g a red solution. The triacety 1-derivative crystallises in sulphur- coloured microscopic plates melting at 208-210", readily soluble in chloroform, acetone, hot alcohol, &c.When methylanthragallol is distilled with zinc-dust, a hydrocarbon, crystallising in white plates and melting at 197", is formed. When oxidised, it is converted into a quirione melting at 278-2279". 3-~etl~ylanthragallol is prepared in a manner similar to the above compound from paratoluylic acid. It melts at 275', and sublimes in orange-coloured needles. It resembles its isomeride. The triacetyl- derivative crystallises in well-formed, lustrous, golden prisms melting at 203-208' with decomposition. 2- Methyl- and 4-methy l-anthragallol are formed simultaneously from metatoluylic and gallic acids. The separation of the isomerides is difficult, and is best performed by converting the mixed product into the acetyl-derivative and recrystallising repeatedly from glacial acetic acid.The one methylanthragallol has a slight golden lustre, and melts at 31 2-313" ; the other crystallises in small, well-formed prisms melting at 235-5240". The acetyl-derivatives melt at 188-190" and at 217-218" respectively. The four methylanthragallols closely resemble one another and anthragallol. They are readily soluble in alcohol, and dissolve in strong and in dilute alkalis, yielding green and violet solutions respec- tively. The solution in hot ammonia has a fine blue colonr, in sul- phuric acid it is red; the latter changes to green on addition of a trace of nitric acid. The absorption-spectra of the red solutions of anthragallol and of the methylanthragallols in sulphuric acid are almost the same.N. H. M. Acid from Santonin : Isophotosantonic Acid. By S. CANNIZ- ZARO and G. FABRIS (Ber., 19, 2260-2265) .-Isophotosantonic acid, C15H3206, is obtained by exposing 1 kilo. of santonin dissolved in 52 litres of acetic acid to the action of light for several months ; one-ninth of the acetic acid is then boiled off under diminished pressure, and the58 ABSTRACTS OF CHEMICAL PAPERS. residue filtered from the photosantonic acid which separates on cool- ing. A further quantity of photosantonic acid is precipitated by adding water. The solution is then nearly free from photosantonic acid and still contains almost the whole of the isorneride. It is treated with sodium carbonate (which dissolves the photosantonic acid alone) and extracted with ether.It separates from its alcoholic solution in thick, triclinic crystals, rather soluble in ether, and sparingly in water. When heated a t loo", it is converted into the lactone, C,,H,,O*. It is dextrorotatory, [a]= = f 3 24" 17'. Photosantonic acid has nearly the same specific rotatory power, but is lsevorotatory. Isophotosan- tonic acid dissolves in alkalis and in warm solutions of alkaline carbonates ; the solutions are orange-red. The barium salt, (C15H,106)2Ra + H,O, is an amorphous powder, readily soluble i n alcohol and in water. The monacetyl-compoimd crystallises from alcohol in transparent needles which melt a t 183" ; it is dextrorotatory, [ a ] D = + 58" 16'. The diacetyl-cowpound is very sparingly soluble ; it melts a t 163-166".It is very unstable, and when often recrys- tallised changes to the monacetyl-derivative. The results ahove described point to the following constitutional formule for the lactones of isophotosantonic and photosantonic acids respectively :- CH : CH*CH-CHMe*C(OH)z CH 1 CH*CH*CHMe*CH*CH<;?>CO I I and CH : CH*CH*CHMe*COOH CH CH* C H*C HMe*CH2*CH < :?> C 0. N. H. M. I I Cinchol. By 0. HESSE (Annulen, 234, 375--379).-A further comparison of i he properties of cinchol and Liebcrmann's oxyquino- terpene or cliolestole (Abstr., 1885, 1075) confirms the author's pre- viously expressed opinion (Abstr., 1885, 1076) that these two substances are identical. They both melt at 115", and are identical in crystalline form. The acetates melt at 1 2 4 O , and also exhibit identical crystalline forms.w. c. w. Alkaloids. By 0. DE CONINCK (Contpt. rend., 103, 640-641.)- Piperidine methiodide gives no colour reaction with potassium hydr- oxide (Abstr., 1886, 897), and this difference furnishes a means of distinguishing between a pyridic base and its hexhydyide. Cicutine methiodide also gives no colour reaction, but the solution acquires an amber tint. The reaction is always obtained with colli- dines, and therefore will most probably be given by conyrine, the collidine of which cicutine is the hexhrdride. No similar colour reaction is obtained with the methiodides of aniline, orthotoluidine, or metaxylidine. When methiodides of pyridic bases are mixed with a fragment of solid potassium hydroxideORGANIC CHEMISTRT. 59 and sn6cient water to form a paste, and then heated, a peculiar odour is developed owing to the formation of pyridic dihydrides.No similar reaction is given by methiodides of pyridic hexhydrides, nor by the methiodides of aniline and its homologues. C. H. 33. Extraction of Pyrroline from Animal Oil. By G. L. CIAMICIAN and M. DENNSTEDT (Gazzetfa, 16,356) .-Pyrroline may be extracted as the potassium-derivative by using caustic potash instead of the metal as heretofore practised. The reaction is probably CIH,NH + KOH = C,H,NK + H,O; the excess of potash serving as a dehydrating agent. The fraction of the oil, freed previously from nitriles, which passes over at 125-140", is heated in an oil-bath with an excess of fused pofash, using a reflux apparatus. At the conclusion of the rcaction, the liquid separates into three layers, the heaviest of which is the excess of potash, the next the potassium compound, and the lightest the unaltered hydrocarbons.On cooling, the potassium com- pound solidifies, and is washed with anhydrous ether. The substance thus obtained, distilled in a current of steam, yields pyrroline of boil- ing point 130-138' ; with chloroform, it yields chloropyridine (Abstr., 1881, 820). V. H. V. Pyridine Bases. By A. LADENBURG (Compt. rend., 103? 692- 695 ; see also Abstr., 1884 and 1885).--a-MetlzyZ~yridine (picoline), C6NH7, is obtained in the form of hydriodide by heating p-j-ridine methiodide at 300". The base boils at 138-129", and is miscible with alcohol and water ; sp. gr. a t 0' = 0.9656. It forms a characteristic mercuriochloride, C,NH7,HCI,HgC12, by means of which i t can be isolated in a state of purity; this compound is very soluble in hut water, but only slightly soluble in cold water.p-MethyZpyridine is best prepared by Zanoni's method of heating glycerol and acetamide with phosphoric anhydride. I t boils a t 142" ; sp. gr. at 0" = 0.9771. The platinochloride crystallises with 1 mol. H,O and melts at 214" ; the aurochloride is anhydi-ous and melts a t 183" ; the mercuriochloride is also anhydrous, melts a t 143", and forms slender needles which can be crystallised from water. .y-iWethy@yridi?~e is formed only in small quantity by the action of heat on pyridine mdhiodide; it boils a t 144-145" ; sp. gr. at 0" = 0.9708. The platinochloride is anhydrous, melts a t 225", and is only slightly soluble in water.aa'-Dimethyl- pyridiite is isolated from the fraction of animal oil boiling a t 138- 145" by means of the mercuriochloride, C7NH9,HCI,HgCl2, which can he crystallised from water, and melts a t 183". When decomposed, it yields lutidine boiling at 142-143"; .sp. gr. at 0" = 0.9924. The aurochloride forms yellow needles which melt at 124" ; the platino- chloride crptalliees in large monoclinic crystals isomorphous with /3-picoline platinochloride, although the former is anhydrous, whilst the latter contains 1 mol. H,O. The picrate is only slightly soluble in water and melts a t 159". When the base is oxidised, it yields a bibasic acid, C5NH3( COOH),, crystallising in beautiful needles which melt a t 226", and at the same time decompose into pyridine and carbonic ttnbjdride.oc-y-Dimefk$pyridine exists in large quantity in Dippel's60 ABSTkACTS OF CHEMICAL PAPERS, oil, and can be isolated from the fraction which boils at 1S5--160" by acidifying with hydrochloric acid and adding mercuric chloride. The precipitated mercuriochloride, 2(C,NHg,HC1,2HgC12) + HzO, is re- peatedly recrystallised, and forms beautiful needles which melt at 129'. When decomposed, it, yields the base ; this boils at 157", and is only slightly soluble in cold water, still less soluble in hot water. The platinochloride is somewhat solnble, crystallises readily, and melts at 219-220'. The aurochioride, C7HgN,HL4uC11, is less soluble and does not crystallise so well. This lu tidine is identical with the lutidine prepared synthetically by Hantzsch.When oxidised, it yields lutidinic acid, which crystallises in plates which melt at 235". a-Ethy7pyridine is the principal product of the action of a, high temperature on pyridine ethiodide ; it boils at 150", is miscible with alcohol, but is only slightly soluble in water. The platinochloride is somewhat soluble in water, and melts at 168-170" ; the aurochloride melts at 120" and crystallises readily from hot water; the picrate melts at 110". When the base is oxidised, it yields picolinic acid only. y-Ethykym'dine is also formed in smaller quantity by the action of heat on pyridine ethiodide, and is separated from its isomeride by taking advantage of the comparative insolubility of its salts, especially the platinochloride or ferrocyanide.The base boils at 163'; sp. gr. at 0" = 0.9522. The plstinochloridie melts at 208", the picrate at 163", the aurochloride at 138". The ferrocyanide is precipitated even from very dilute solutions. When the base is oxidised, it yields isonico- tinic acid. a-y-DietkyZpyridine is also obtained in small quantity by the action of heat on pyridine ethiodide ; it boils at 187-188", has a, disagreeable odour, and is only slightly soluble in water. When care- f u l ! ~ oxidised, it yields lutidinic acid which melts at 235". a-lsopropylpyridine, obtained by heating pyridine with propyl or isopropyl iodide at SOO", boils at 158-159", is slightly soluble in water, and has a very disagreeable odour ; sp. gr. at 0" = 0.9342. The platinochloride, (C8Hl,N),,HZPtCI6, is somewhat soluble and melts at 168" ; the aurochloride crystallises from dilute solutions in yellow plates which melt at 9l"and are only slightly soluble in water; the picrate forms yellow needles which melt at 116".When the base is oxidised by potassium permanganate, it yields picolinic acid. y l s o - propyZppidipLe is obtained in smaller quantity by the same reaction, arid is separated by means of the platinochloride, which is only slightly soluble in water, and melts at 203". The base boils at 177-178"; sp. gr. at 0" = 0.9439. The picrate melts at 180". When oxidised, it yields isonicotinic acid. C. H. B. Quinoline. By A. CLAUS and F. COLTJSCHONN (Bey., 19, 2502- 2508).-The authors describe a number of halogen additive products of the propio-haloid compounds of quinoline.Quinoline propio- bromide is easily formed when its constituents are heated alone, or better, with alcohol, at 90-100". It is easily soluble in alcohol and water, and crystallises from water in colourless plates containing 2 mols. H,O, and melting at 66" ; from absolute alcohol, it separates in anhjdrous crystals melting at 148". It is easily soluble in chloro- form, and horn this solutiou crystallises with 1 mol. CHC1, in quadraticORGANIC CHEMISTRY. 61 prisms which cradually lose chloroform and become opaque, soften at 65", and melt with evolution of chloroform a t 128-129". Quinoline propiodide forms yellow anhydrous ctptals me1 ting at 145", and becoming rapidly discoloured in the light. This also crystallises with 1 mol. CHCI, in quadratic prisms which begin to evoke chloroform at 92".Quinoline propiochloride cannot be easily prepared directly from its constituents, but is best obtained by acting on the corre- sponding bromide with silver chloride. It is very soluble in water, and crystnllises in colourless prisms or plates containing 1 mol. H,O and melting a t 95". The hygroscopic anhydrous salt melts at 135" ; it also crystallises with 1 mol. CHCI, in quadratic prisms melting a t 79". The additive products were obtained by treating a chloroform solu- tion of the propiohaloid salt with the halogen. Quinoline propiobroinide dibromide, CgNH,*PrBr?, forms glistening, red, triclinic crystals melting at 93". The di-iodide forms brown metallic needles melting a t 60". The dichloride forms yellow scales melting at 60".The tetriodide, CgH,N*PrBrId, yields small, almost black needles having a green fluorescence and melting at 49". Quinoline propiodide dibromide forms orange triclinic crystals melt- ing a t 77". The di-iodide forms thin, bronze-coloured scaleq melting at 62". The dichloride forms yellow needles melting a t 87". The tetrabromide, C9NH7*PrIBr4, is a very unstable orange-red powder which evolves bromine a t the ordinary temperature, and gave no con- stant malting point (48-58"). The tetriodide forms iodine-coloured plates melting a t 50'. The tetrachloridp crystallises in needles which show the high melting point 1 4 ~ 1 4 . 5 " . It is also formed when quinoline propiochloride is treated with iodine trichloride, and may therefore really he quinoline propiochloride iodide trichloride.When boiled with water, it is gradually decomposed into quinoline propio- chloride. Similar migmtion of the halogen-atoms may also very likely take place in others of the mixed halo'id compounds. Qziinoline propiochloride dibromide forms orange crystals melting at 84-85'. The &iodide melts a t 61-W. The dichloride is very unstable and could not be obtained in a pure state. A tetriodide is easily formed, but could not be obtained in a pure state. All these additive compounds decompose when heated a t 250-200", prop91 haloid salts, quinoline haloid salts, and halogenispd and alkglated quinolines being amonget the products of decomposition. These decompositions are being studied. All the above temperatures are uncorrected.L. T. T. Isoquinoline and its Derivatives. By S . GABRIEL (Ber., 19, 2354--2363 ; compare Abstr., 1886, 812) .-Dichlorisopuinoline, CH: CC1 C"""&y: N 2, is prepared by heating homo-orthophthalimide (8 grams) with phos- phorus oxychloride (24 grams) for three hours a t 150-170". The product is poured into alcohol ( 5 vols.), the mass of crystals so obtained treated with soda until alkaline, filtered. and recrystallised from alcohol. It is readily soluble i n hot alcohol, cold chloroform,62 ABSTRACTS OF CHEMICAL PAPERS. ether, and benzene; it boils at 305-307". The alkaline mother- liquor obtained in the preparation of this compound, when treated CCl : N >' with hydrochloric acid, yielded the cldoro-derivutive C6H4< CH,*CO or C6H4<~CH1_C"0H'> ; this crystallises from boiling alcohol in long needles melting at 195-197" with evolution of gas.It is rather soluble in hot alcohol, sparingly in hot benzene and in chloroform ; it dissolves in alcohol, but not in ammonia. The methyl-cornpoun,d, C,H5MeClN0, is obtained by dissolving half a gram of the substance in methylalcohol (10 c.c.), adding methyl iodide (2 grams), and heat- i n g a t 100". It forms slender, white crystals, readily soluble in alcohol, ether, benzene, &c., insoluble in alkali. It melts at 66-67', and has an odour of fruit. Chlorisopuinoline, C6H1< CH CH:N ' '">, - is obtained by reducing the dichloro-compound with phosphorus and hydriodic acid at 150- 170", or with tin and hydrochloric acid. It melts at 47-48', and boils at 280-281" under 753 mm.pressure, and is readily soluble. Methoxy pheiilJlclzloriso quinoline, C"H4<C(oMe) : N>, is formed when phenyldichlorisoquinoline (1 gram) and sodium methoxide are heated for three hours at 100". I t crystallises from alcohol in needles melting a t 76", readily soluble in ether, benzene, &c. It dissolves also in strong hydrochloric acid, but is precipitated by water. When heated with fuming hydrochloric acid at loo', it is conyerted, with evolution of methyl chloride, into the compound C16H&1N0, probably ch!orisobenzuZ phthliinidine, C6HH'<Co.~H->. It crystallises from alcohol in slender, lustrous needles, melting at 211-212", moderately soluble in ether and cold alcohol, readily in glacial acetic acid, ben- ztae, &c.The formation of this compound is analogous to that of isobenzslphthalimidine from phenylethoxyisoquinoline (Abstr., 1886, 631). Ethozychlorisoquiil.oline, CeH4<g$YgCk>, is prepared by heating dichloroisoquinoline with alcoholic soda at 100". It forms readily soluble needles melting at 37-37.5". The methoxy-derivative, CloH8XOC1, is prepared in a, similar manner. It melts a t 73-74", and is isomeric with the methyl-compound obtained from chloroxy quinoline. When heated at 150" in a current of dry hydrogen chloride, it is converted into oxychlorisoguinoline, C,H4<gt.&!!>. This crystallises from dilute alcohol in slender needles melting at 218-220' ; i t dissolves rather readily in ether, easily in alcohol and chloroform ; it is also readily soluble in dilute aqueous soda.The methylderivative, c6H4<gg.&z:>, crydxdlises in long, broad needles which melt at 111-112" ; it is readily solnble. c)xy chlorisoquinoline is formed in small quantities in the preparation of ethoxychlorisoquinolhe. CC1: CPh - CC1' CPhORGANIC CHEMISTRY. 63 Isoquinoline is conveniently prepared by heating dichlorisoquinoline (3 grams), and hydriodic acid, sp. gr. 1.96 (18 c.c.) for five hours at 230". The product is treated with alkali, and steam distilled ; the distillate being treated with hydrochloric acid and again steam dis- tilled to remove the unchanged chloro-base. Isoquinoline melts at 20-22", and boils at 236-236.5". The ethiodide crystallises in gold- coloured plates melting at 147-148", readily soluble in water and in warm alcohol. N.H. M. Synthesis of Hydroxyquinolinecarboxylic Acid. By E. ,LIPP- MANN and F. FLEISSNER (Ber., 19, 2467-2471) .-Unlike ordinary phenol-derivatives, the potassium compound of orthohydroxyquinoline is not acted on by carbonic anhydride even at 300". When, however, nascent carbonic anhydride (obtained by the action of potash on carbon tetrachloride) is employed, action takes place. Orthohydroxy- quinoline, carbou tetrachloride, and caustic potash are mixed in alco- holic solution in the proportions necessary for the equation C9NH7U + CCI, + 6KHO = 4KC1 + C9NH5(OK)*COOK + 4H20, and the ~ h o l e boiled for 12 hours. The product contains hydroxyquinoZine- ccirboxylic acid, OH.C,NH,*COOH, which when purified crystallises in yellow prisms melting at 280".?'his acid agrees in its salts and in all its properties, save melting point and oxidatiou products, with the a-hydroxycinchonic acid (m. p. 254-256") obtained by Weidel and Cobenzl from sulphocinchonic acid (Abstr., 1881, 742). The acid is sparingly soluble in the ordinary solvents. It dissolves in dilute hydrochloric acid to form a hydrochloride, which is precipitated on the addition of concentrated hydrochloric acid in the form of glistening needles. The platinochloride forms unstable, bright yellow needles. The acid forms a normal barium salt, the pale yellow solution of which, on the addition of baryta-water, yields white needles of the bask barium salt CloNH,BaO3 + H,O ; these only part with their water of crystallisation at 140-150". The silver salt is precipitated in the form of pale lemon-yellow flocks, which soon change to microscopic needles.The aqueous solution of the acid gives a green coloration with ferric chloride, but none with ferrous sulphate. When subjected t o dry distillation, the acid yields orthohydroxyquinoline. When oxidised by potassium permanganate in alkaline solution, the acid yields a pyridinedicarboxylic acid, C,NEIQ04, forming bright yellow crystals melting at 234-235". With ferrous sulphate, it give8 a blood-red coloration, and forms a silver salt which is gelatinous when first precipitated, but soon becomes crystalline. This acid is probably identical with Bottinger's pyridiuedicarboxylic acid, and isomeric with Weidel's isocinchomeronic acid. Weidel and Cobenzl's a-hydroxyvcinchonic acid, when similarly oxidised, yields a-pyridinetricarboxylic acid.The authors are further investigating this subject. By 0. FISCHER and H. VAN Loo (Ber., 19, 2471--2476).--This is a continuation of the authors' previous work (Abstr., 1884, 1372). When P-diquinoline is heated with ethyl iodide in closed tubes at 90-loo", P-diquinolirbe L. T. T. Peculiar Formation of 6-Diquinoline.64 ABSTRACTS OF CHEMICAL PAPERS. ethiodide, Cl,N2H12EtI, is formed in long, ruby-red crystals. It is very unstable, and is decomposed by water and by boiling alcohol. Ro diethiodide could be obtained. When bromine is allowed t o act on P-diqiiinoline in chloroform solution, a tetrabromc-additive product, CI,N2H,,Br4, is produced. This crystallises in pale yellow needles melting at 192", and is decomposed at once by sulphurous acid, diquinoline sulphnte being formed./3- DiquinolinedisuZphonic acid, ClsN2H,,(S03H)2, is produced when P-diquinoline is heated with a large excess of fuming sulphuric acid. It is very soluble in water, and is precipitated from this solution by a mixture of alcohol and ether in yellowish flocks. Its potassium salt crystallises from 50 per cent. alcohol in glistening white prisms containing 3 mols. HzO. The anaquinolinecarboxylic acid described in the former paper (loc. cit.), as obtained by the oxidation of the base by chromic acid in acetic solution, is undoubtedly identical with that lately obtained by Skraup and Brunner (m. p. 247"). The melting. point previously given by the authors was obtained from a sample crystallised from benzene ; when crystallised from water, it melts at 248-249".The author con- siders this acid to be metaquinolinecarboxylic acid, and that the name anaquinolinecarboxylic acid should be transferred to the acid melting at 357O, and hitherto designated metaquinolinecarboxylic acid. If chromic acid is dissolved in sulphuric acid in place of acetic acid, the oxidation takes place in quite a different way. Under these circumstances p yridy 7quinolinecarbon: y Zic acid, C,NH,*C,NH,.C OOH, i8 formed. This crystallises in glistening needles, which melt with decomposition at 271-273". It is sparingly soluble in water, easily in alcohol, and forms salts both with acids and bases. The silver saIt, when heated, yields a p y r i d y lqzcinohe, C14N2H10, which crystaliises in white needles melting at 104", and gives a reddish-yellow crystalline platinoch lorid e.Piperidine Bases. By A. LADENBURG (Compt. rend., 103, 747- 74{9).-The bases are obtained by treating boiling alcoholic solutions of the corresponding pyridine bases with a large excess of sodium. Piperidine obtained in thh way is identical with the base prepared from piperine. a-Methylpiperidine or a-pipecoliqe boils at 118-119", has the same odour as piperidine, and dissolves readily in water; sp. gr. at 0" = 0.860. The hydrochloride is very soluble, but not deliquescent, and melts at 189". The hydrobromide is less soluble, and forms confused needles which melt at 182" ; the platinochloride is very soluble. With carbon bisulphide, the base yields a thiocarbamate, CS2,'2C6HI3N, which crystallises readily, melts at 118", and is analogous to that! formed from piperidine.p-Methylpiperidine or P-pipecoline boils at 125", and dissolves readily in water; sp. gr. at 0" = 0.8684. The hydriodidc crystallises in beautiful, non-deliquescent needles, which melt at 131". It combines with cadmium iodide, forming the compound Cd12,2C6H13NHI, a wbite precipitate soluble in warm water, from which it crystallises in white tables melting at 145". The platinochloride is somewhat soluble, and forms orange prisms melting at 192" ; the aurochloride is very soluble, and melts at 231" ; the picrate nielts at 136". aoc'-Dimethy~~peridinR or aa'-lupetidine boils at 128- L. T. T.ORGANIC CHE_1IISiTlZI'. 6 5 130", and is very soluble in water and alcohol ; sp.gr. at 0" = 0.8492, The hydrochloride and hydrobromide crystallise in non-deliquescent needles ; the platinochloride forms large orange crystals which melt a t 212". ay-Dirnethypip~ridz'ne boils at 141", has an odour of piperi- dine, and dir,solves readily in water, though not in all proportions : sp. gr. a t 0" = 0.8615. The hydrochloride crystallises in beautiful needles which melt a t 235" ; the hydrobromide is even more soluble ; the platinochloride is not very soluble, and crystallises in nodules ; the aurochloride is an oil. a-Ethylpiperidine boils at 143", and dis- solves slightly in water, but separates from the solution on heating, and has an odour resembling that of piperidjne and coniciiie ; sp. gr. a t 0" = 0.8674.The hydrochloride forms non-deliqiiescent crystals ; the platinochloride cryst,aliises in large tablea which melt a t 178". The methyl-derivative boils at 143-152"; sp. gr. at 0" = 0.8495. ~,-.E&yZpiperitline boils at 1 -57", has a disagreeable odour, is only s,lghtly soluble in cold water, and still less soluble in warm water ; sp. gr. a t 0" = 0.8795. The hydrochloride is deliquescent ; the platino- chloride forms yellow tables which meltl at 170-173" ; the auro- chloride crystallises from warm water in lamella which melt a t 105". a- IsopropyZpiperiditLe boils at 160-162", and is slightly soluble in water, but separates from the solution when gently heated ; sp. gr. a t 0" = 0.8676. Its odour and its properties generally resemble those of its isomeric-le, conicine, but it is much less poisonous.The platinochloride is much less soluble in water. and is not soluble in alcohol or ether ; i t melts a t 193" ; the hydrochloride melts a t 240", the hydrobromide a t 230", the hydriodide at 24 Lo. All these derivatives crgstallise readily. The iodide combines with cadmium iodide, forming a slightly soluble double salt, which crystallises readily and melts at 132". The picrate and aurochloride crystaUise readily, and are only slightly soluble. With carbon bisulphide, the base yields a crystalline compound, CS (C,H,,N)SH,C,H1,N, which melts a t 105", dissolves readily in alcohol, but is only slightly soluble i n water. The methrl-dvivative of or-isopropy~piperidine boils a t 166" ; sp. gr. at 0" = 0 85P3. Its hydrochloride is extremely soluble in water ; the aurochloride forms shining lamellae, and is also very soliihle in water ; the platinochloride is somewhat soluble, and melts a t 100" ; the picrate crystallises readily, and nielts a t 149".ry-Isop,.opyZpiperi~~//e boils at 168-171", dissolves slightly in water, and has a very disagreeable odour. The hydro- chloride crystallises, but is not stable in moist air ; the platinochloride is crystalline, and is only slightly soluble in water, but dissolves in alcohol and ether, arid melts at 172"; the aurochloride is also crgstal- line, and only slightly soluble. Method of Preparing Extracts of Pepsin. By W. PODWYSSOZKI ( P J ~ g p r ' . c A T C ~ L ~ U , 39, 62-74). -If the gastric mucous membrane of carnivora and herbivora be placed in glycerol almost immediately after death, very little pepsin is extracted.Ebstein and Grutzner state that glycerol dissolves pepsin only, but the author finds that a certain amonut of pepsin precursor, or as he t,c.rmq it " propepsin," is dissolved also. Mucous membrane exhausted with glycerol still yields an important C. H. B. VOL. 1.11 f66 ABSTRACTS OF CHEMICAL PAPERS. amount of pepsin when treated with hydrochloric acid or hydrochloric acid and glycerol. It appears, therefore, that gastric mucous mem- brane contains two propepsins, one soluble in glycerol, the other insoluble. I f the mucous membrane is kept in a warm place for 24 hours before it is extracted, a much larger yield of pepsin is obtained, provided no putrefaction has set in. Hydrogen and carbonic anhydride have no influence on the forma- tion of pepsin, but oxygen, on the other hand, appears to favour its development ; more pepsin is formed when the mucous membrane is allowed to remain in contact with oxygen than when it is in contact with air.Chlorine gas passed through any extract entirely destroys the ferment. J. P. L. Comparative Estimation of Preparations of Pepsin. By .A. A. LIPSKI (Russlcayrc Medifsiiza, 35,583-584).-The powdered pepsins were examined by digesting 0.2 gram of the preparation with 10 grams of white of egg and 100 C.C. of hydrochloric acid (0.25 per cent.) for four hours at 40". The undissolved albumin being then determined, the weight of this in grams was :-Perret acidifih 8.756, Marquart 8 577, Lamatch 8.557, Merck 7.213, Boudault neutre (No.4) 2 62, Witte 2.195, Boudault acidifit5 1.2, Russicum solubile (of the Russian Ph.) 0.721, do. do. recent 0.47, do. do. without the sugar contained in the official preparation 0.157. The Russian pepsin is, therefore, far more active than any of the German or French pre- parations tested. The same holds good for the pepsin wines.24 ABSTRACTS OF CHEMlCAL PAPERS.Organic Chemistry.Volatility of Methane-derivatives. By L. HENRY (Compt.rend., 103, 603-606) .-The volatility of methane-derivatives followsthe same order as that of the substituted elements when the latterare arranged in natural families in the order of their atomic weights.The boiling point rises as the molecular weight increases, but thedifferences between the volatility of the methane-derivatives are muchless than those between the boiling points of the electronegativeelements which they contain.B.p. Diff.cl, gas ...... - 35") 96"Br, liquid .... + 63I, solid . . , . . + 250 }O , ~ R S ........ - 181N, gas. ...... - 193S, solid ...... + 448) 629P, solid ...... + 287}480B. p. Diff.MeC1, gas .... - 23" } 27.5Me20, gas ..... - 23 } 60.04- } 50.0 Me3N, gasMeBr, gas .... + 4.5MeI, liquid ...Me,S, liquid. .. + 37Me3P, liquid.. . + 4144 } 39'5.....The differences show that electronegative elements in the samenatural family are far from being comparable in the free state, whilstip methane-derivatives they may be regarded as existing underanalogous physical conditions.I n each of the groups of methane-derivatives, the rise of the boilingpoint is not proportional to the increase in the molecular weight ; infact the greater the increase in the molecular weight resulting fromsubstitution, the less proportionally is the rise of the boiling point.The substitution of sulphur causes proportionally less rise in the boil-ing point than the substitution of oxygen, and the snbstitution ofphosphorus less than the substitution of nitrogen, although sulphurand phosphorus are solids, whilst oxygen and nitrogen are gases.The atomic weights being nearly equal, the diminution of volatilityresulting from substitution is greater the more strongly marked theelectronegatire character of the substituted element, or, in otherwords, the more distinctly its properties differ from those of hydro-gen. This is well seen in the case of the nitrogen- and boipon-deriva-tives.Me3N, mol.wt. 59, a liquid boiling at 9.3".Me3B, mol. wt. 36, a gas which liquefies at -10" under a pressureof 3 atmos.This phenomenon is doubtless connected with the fact that the heatof combination of carbon with electronegative elements diminishes asthe atomic weight of the latter increases.Sugars. By BERTHELOT (Compt. rend., 103, 533-537).--8 soh-tioh of invert sugar which had been kept for nearly 30 years,deposited spheroidal groups of radiating crystals, which when care-C. H. BORGANIC CHEMISTRY. 25fully dried on filter-paper resembled purified glucose. The crystalshave the composition C6H,,0e when anhydrous ; their reducing poweris equal to that of glucose, and they are completely fermentable, buttheir rotatory power is only [a]= = + 32.2, or little more than halfthat of glucose.The crystals are a compound of glucose and levu-lose, in which one constituent behaves like water of crystallisation.The compound is decomposed by solvents ; its rotatory power showsthat the ratio of levulose to glucose is 1 : 5. A similar compoundprepared by G6lis has the rotatory power of +15O, which correspondswith a ratio of levulose to glucose of 1 : 3.The compound formed as an intermediate product in alcoholic fer-mentation is most probably formed by the union of one molecule oflevulose with two of glucose, but it does not seem to have been ob-tained in crystals.In the process of extracting raffinose from cotton-seed cake, crys-tals were obtained which when dried on filter-paper without treatmentwith any solvent had all the properties of mellitose from the manna ofeucalyptus. When the aqueous solution of this substance is treatedwith yeast, only half the sugar undergoes fermentation, and the liquidcontains a non-fermentable sugar with the properties of eucalpe.Ifthe mellitose is treated with boiling alcohol, it splits up into rafflnose,which crystallises after some time, and eucalyne, which remains insolution. An alcoholic solution of ra5nose and eucalyne when allowedto remain, deposits crystals which seem to be formed by the recom-bhation of the rnffinose with the eucalyne.Mellitose, which is widely diffused in the vegetable kingdom, isthe result of the association of raffinose, a true saccliarose, witheucdyne, a non-fermentable carbohydrate. This association bearsno resemblance to the union of glucoses to form saccharoses, and theconstitution of mellitose is analogous to that of hydrates and alco-holates rather than to that of ethereal salts.C. H. B.Sugar formed in the Inversion of Lichens. By P. KLASON(Ber., 19, 2541).-Bauer showed (Abstir., 1886, 869) that dextrose isformed by inverting lichens. The author previously obtained thesame results (Lund’s Pysiogr. Sallskops Minneskr., 1878, 61). Appa-rently no other sugar is formed in the inversion. N. H. M.Action of Dilute Acids on Grape-sugar and Fruit-sugar,By M.CONRAD and &I. GUTHZEIT (Ber., 19, 2569-2574).-Accordingto Tollens and v. Grote (Annnnlen, 175, 181, and 206, 207), dextroseas well as levulose when boiled with sulphuric, or better with hydro-chloric acid, .Fields acetopropionic acid in very small quantity.Quantitative experiments on the decomposition of cane-sugar byhydrochloric acid, made by the authors (Abstr., 1885, 743), pointedto the formation of a small amount of acetopropionic acid from dex-trose. Experiments described in the present paper show that thisview (the formation of acetopropionic acid chiefly from levulose) onlyholds good for the decomposition of cane-sugar with dilute sulphuricacid, and not with hydrochloric acid.Quantities of dextrose and levulose corresponding with 20 grams o26 ABSTRACTS OF OHEMICAL PAPERS.cane-sugar were heated for 17 hours with the same amounts of acidand water as those previously used (Zoc.cit.).1. Decomposition with dilute sulphuric acid-Aceto-Humic propionic Formiosubstances. Dextrose. acid. acid.Dextrose.. .... 52.6 0.83 43-70 2.78 1.21Levulose.. .... 32.6 13.78 - 16.78 6.46Cane-sugar.. .. 100.0 = 14.61 43.70 19.56 7-872. Decomposition with dilute hydrochloric acid-Aceto-.Humic propionic FormicDextrose., .... 52.6 4-76 14-52 15.53 6-51Levulose.. .... 52.6 10.65 - 16.28 8-78substances. Dextrose. acid. acid.Cane-sugar, , . . 100.0 = 15.41 14-52 31.81 15.29Decomposition of Milk-sugar by Dilute Hydrochloric Acid.By M. CONRAD and M. GUrHZElT (Bey., 19, 2575--2576).-The follow-ing results were obtained froni three experiments, in which 21, 21,and 10.5 grams of milk-sugar were heated with 50 C.C.of water and4.87, 5.0, and 487 grams of hydrochloric acid respectively :-substances, (unchanged). acid. acid.N. H. M.Humic Milk-sugar Acetopropionic Pormic1 ...... 3.68 5.54 6-29 2.392 ...... 3.94 - 5-80 2.243 ...... 1-60 L 3.32 1.33In 2 and 3, the milk-sugar was not determined. N. H. M.Carbohydrates. By 0. WALLACE (Annalea, 234, 364-375).-The rhizome of the water lily, Iris pseudacorw, contains a peculiarCarbohydrate, called " irisin " by the author. Irkin, CaHl0O5 + HzO,closely resembles inulin, but is distinguished from the latter byits more powerfal action on polarised light; [dc]D = -49' 90 for a2 per cent.solution of irisin, and [ a ] D = - 37" 27' for a soIution ofinulin of the same strength. Fehling's Rolution is not reduced byirisin, but the carbohydrate is easily attacked by dilute acids, yieldinglevulose as the chief product. Irisin is four times as soluble asinulin in water s t 22". Under the microscope, the globules of irisinresemble the minute globules of inulin in size, but they do not exhibitdouble refraction. w. c. w.Animal Gum. By H. A. LANDWEHR ( P f t i i g ~ ' ~ arc hi^, 39,193-204) .--The animal carbohydrates may be arranged in parallel groupswith those occurring in the vegetable kingdom, and animal gumresembles vegetable gum in yielding oxrzlio acid after treatment withnitric acid. Mwiin was prepared It is obtained readily from m u c ORGANIC CHEMISTRY. 27by precipiktion with acetic acid from an extract of submaxillaryglands, made with a 1 per cent.sodium carbonate solution. The pre-oipitate was washed with weak acetic acid, and then dissolved in weakhydrochloric acid by the aid of heat. On neutralising with soda, a whiteflocculent preciFitate is obtained, which is increased in amount on theaddition of sodium sulphate and boiling. The precipitate is collectedand freed from salt by dialysis; i t consists of an ordinary proteid.The filtrate contains no nitrogen, biit contains animal gum. Fromtendon mucin, the same carbohydrate is obtained, in spite of whatLoebisch (Abstr., 1886, 166) says to the contrary; it may also beobtained from synovia, collo'id cysts, and from the mucin of thesnail's mnntle. nilucin and animal gum both yield lsvulic acid whentreated with hydrochloric acid.By long boiling withwater, chondrin splits into gelatin, animal gum, and possibly a thirdsubstance not yet further investigated.Pure chondrin is soluble inhot water, and its solutions gelatinise when cold, if not too dilute ;this power of gelatinising is lost after prolonged boiling. A dilutesolution gives the following reactions :-Dilute mineral acids cause aprecipitate soluble in excess ; acetic acid gives a precipitate insolublein excess ; acetic acid and potassium ferrocyanide give a precipitate,soluble in excess of the latter reagent. Sodium chloride solutiongives no cloud, but hinders the precipitation by acetic acid.Metaphos-phoric acid gives a cloudiness disappearing on warmth. Alum gives acloudiness, disappearing on adding excess. Lead acetate gives a preci-pitate, soluble in excess. Basic lead acetate gives a precipitate, partiallysoluble in excess. Lead acetate and ammonia give a flocculent preci-pitate, insoluble in excess. Tannin and acetic acid give a precipitate,insoluble in excess. Copper sulphate and sodium hydroxide colour theliquid violet, which becomes red on boiling. Boiling the solution forfire or six hours with 1 per cent. mlphuric acid gives it the power ofreducing copper salts, this being due to the formation of a reducingsugar from animal gum. Animal gum may be separated fromchondrin in the same way as from mucin.Metalbumin and paralbumin may also be used as sources of animalgum. It is also found in small quantities, but constantlly in the redblood corpuscles, brain, kidney, spleen, liver, and pancreas.Prote'idspi-opor do not yield it.Another source of animal gum is chondrin.W. D. H.Derivatives of Thioformaldehyde. By A. WOHL (Rw., 19,23444347) .-Thiometaforrnaldehyde, (CH,S),, is obtained whenan aqueous or alcoholic solution --of hexamethyleneamine saturatedwith hydrogen sulphide is heated on a water-bath. It separates as a,white, amorphous substance, which is washed with water and hydro4chloric acid, and extracted with boiling glacial acetic acid and alcohol.It is insoluble in all the usual solvents, and has a peculiar odour ; itmelts at 175-176", and decomposes at a high temperature.Itdissolves unchanged in strong sulphuric acid.Methy Zthi~formuldine, S2(CH2)sNMe, is prepared by diluting 50 C.O.of a 20 per cent.. solution of formaldehyde with an equal volume ofwa&er, 8nd saturating with hydrogen sulphide; 200 C.C. of wafer ar28 ABSTRACTS OF CHEMICAL PAPkXS.then added, the whole filtered and stirred with 20 C.C. of a 30 per cent.solution of methylamine. In 24 hours crystals separate. Morehydrogen sulphide i s then passed through the solution until it is nolonger turbid ; the crystals are collected, washed with water, and dis-solved in ether. I t crystallises in needles melting at 65", and isinsoluble in water, soluble in dilute mineral acids, alcohol and glacialacetic acid. It distils with steam, boils at about 185", being at thesame time converted into a compound melting at 130-140".Thehydrochloride forms needles readily soluble in water ; it melts at 188"with decomposition.Dimeth ylthioformuldinium iodide, SL(CH,),NMe,1, is formed bytreating the compound with methyl iodide. In two to three days theliquid solidifies to a mass of slender, lustrous needles. It melts at 161-163O, and dissolves readily i n water, sparingly in alcohol. The platino-chloride, [ Sz( CH2)3NMe]zMezPtC16, is a bright yellow, crystalline sub-stance. The iodide dissolves in hot aqueous potash and separatesunchanged on cooling. When boiled with silver oxide, it yields anammonium base, which, however, could not be isolated.Chloro-derivatives of Acetals. By 0.MAGNAMINI (Gazxetta, 16,330-3333) .-Trichlorometh y let hylacetal, CC13*C €3 (OMe) OEt, is ob-tained by heating tetrachlorether with methyl alcohol in sealedtubes. The reaction is as follows: CCI,*CHCI*OEt + MeOJ3 = HCl + CCl,GH(OMe)*OEt. It is a colourless liquid of camphor-likeodour ; it boils at 193.4; sp. gr. = '1.32.Trichlorodimethylacetal, UCI3*CH(CMe)?, obtained from tetrachlor-ethyl methyl ether, is a liquid of similar characters. It boils at 183.2" ;sp. gr. = 1.28.The tetrachlorethyl methyZ ether, CC13*CHC1*OMe, prepared by theaction of phosphoric chloride on chloral methylate, is a colourlessliquid boiling at 178"; sp. gr. at 0" = 1.84. I t does not appear tohave been previously isolated.Diisonitrosoacetone.By H. v. PECHMANN and R. WEHSARG (Ber.,19, 2465-2467).-V. Meyer and Zublin have shown that when accto-acetic acid is treated with nitrous acid, carbonic anhydride is evolved,and isonitrosoacetone formed. The authors find that when, in likemanner, acetonedicarboxylic acid is treated with water and sodiumnitrite, a rapid evolution of carbonic anhydride takes place, and diiso-nitrosoacetone, CO (CH-NOH),, is produced. This forms glisteningprismatic crystals, meltiug with decomposition at 143-144". It iseasily soluble in alcohol and ether, sparingly in cold water, chlorofoim,and benzene. Itsaqueous solution when heated decomposes into hydrocyanic acid, car-bonic anhydride, and water. Acids cause a similar decomposition, buthydroxylamine is also among the products. It is more stable in nlka-line solutions, and forms alkali saEts, which crystallise in orange-yellowneedles.Its salts, especially the red crystalline silver salt, explodewhen heated. When warmed with phenol and Rulphuric acid, thenitroso-compound gives a red coloration, with ferric chloride a brown.The authors are further investigating the subject.N. H. M.V. H. V.I t is very unstable, and detonates when heated.L. T. TORGANIC CHEMISTRY. 29Hetines. By L. CON OM IDES (Ber., 19, 2524--2527).-When avery dilute solution of diethylketine, CloH,,N2, is treated with thetheoretical amount of potassium permanganate, a ketinedicarboxylicacid is obtained, identical with that prepared by Wleugel by reducingethyl isonitrosoethylacetate (Abstr., 1882, 949). If the oxidationtakes place in a warm solution, other and more unstable acids areformed.When 5 grams of ethyl imidoisonitrosobutyrate are care-fully warmed with powdered zinc chloride at 60-70" for a long time,and the product saponified with alcoholic potash, a small quantity ofan acid melting at l90-195", identical with Wleugel's acid (Zoc. c i t . ) ,is formed. The above reactions, together with the fact that the ketine-acid does not yield an anhydride, point to the following constitutionalformulae for methylketiiie and the ketine-dicarboxylic acid :-CMe*CH CMe* C (C 0 OH)NeCH: CMeyN and NeC(COOH): CMeyN*N. H. M.Pure Bntyric Acid. By A. BANNOW (Ber., 19, 2552-2554).-Pure butyric acid is best prepayed by converting the commercial acidinto the ethyl salt, which is then fractionally distilled.The fractionboiling at 120-121" is reconverted into acid. N. H. M.Xoc., 1886, 287-297).--Tiglic (methylcrotonic) acid,Derivatives of Tiglic Acid. By P. MELIKOFF (J. RUSS. C h m ~CHBle: CNeCOOH,was prepared either by the saponification of the oil of Roman chamo-mile (Kopp, Abstr., 1879, 454), or by heating a-methyl-p-hydroxy-butyric acid (Rohrbeck, Abstr., 1878, 136). The acid was treatedunder water with an aqueous solution of hypochlorous acid, the pro-duct of the reaction extracted with ether, and the solvent; distilled off.The residue, after remaining for some time over sulphuric acid, solidifiedto a crystalline mass, which was found to consist of two isomericchlorhydroxyvaleric acids, C5H9C103. A concentrated aqueous solu-tion of this mixture was neutralised with zinc carbonate : a crystallinezinc salt was precipitated, and the mother-liquor on being evaporatedleft another salt in the form of an amorphous humoid substance, Thetwo acids obtained by decomposing these salts with sulphuric acidare both easily soluble in water, alcohol and ether ; the one forming acrgstalline sparingly soluble zinc salt, melts at 75", and crjstallisesfrom ether in thin prisms; the other isomeride melts at 111*5", and isobtained from its ethereal solution in the form of large, translucentprisms.When a mixture of these acids, or each of them separately, istreated with alcoholic potash, the potassium salt of an anhydro-acid,CHMe <--,- >CMe*COOH, is formed.The free acid forms silky, crystal-line needles having the odour of butyric acid, easily soluble in water,alcohol, and ether, melting at 62". The energy with which i t entersinto direct combination is in the main the same as that shown byp-rnethylglycidic acid : a-methj lglj cidic acid in this respect exhibitin30 ABSTRACTS OF CHEMICAL PAPERS.much greater energy. This circumstance, established by experimentson the hydration of the potassium salt by heating with water, is inaccordance with the results obtained by the author in a former workon glycidic and a- and p-methylglycidic acids (Abstr., 1885, 650). Theenergy of direct combination is diminished with increasing molecular-weight in acid8 of analogous constitution ; at the same time amongisomeric acids the greatest energy is exhibited by the one containingtertiarily united carbon in its molecule.a-p-Dimethylglycidic acidcontains one CH,-group more than a- and P-methylglycidic acids, but,on the other hand, one of its carbon-atoms combined with oxygen is intertiary union.By the action of hydrochloric acid on a-P-dimethylglycidic acid,a-methy E-P-clLZor-a-hydroaybzLtyric acid, OH*CHMe*CMeCI*COOH, isformed ; it melts at 75", and is identical with one of the chlorhydroxg-valeric acids above described, the other isomeride being thereforea-methtyl-a-clLZoro-~-~~~droxyLUt~r~c acid, CHMeCl*CMe(OH)-COOH.An aqueous solution of a-/3-dimethylgl@dic acid, when heated during6-10 hours at 99", is converted into a-P-dimethyZqlycidic acid,OHCHMe*CMe(OH)*COOH, melting at lo?", readily dissolving inwater, alcohol, .and ether.A. T.Constitution of Chlorhydroxybutyric and DichlorobutyricAcid. . By E. MELIKOFF (J. Buss. Chem. SOC., 1886, 227-303).-Chlorhydroxybutgric acid (formed by the combination of crotonic withhypochlorous acid, Abstr., 1884, 1302, and 1885, 650), when heatedwith concentrated sulphuric acid, yields monochlorocrotonic acid, crys-.fallising in long, thin prisms, melting at 98", sparingly soluble incold, more readily in hot water, easily soluble in alcohol and ether.This acid yields normal crotonic acid (m. p. 72") ou reduction byzinc and sulphuric acid. The chlorocrotonic acid above mentionedis an a-chlorinated product, the isomeric &derivative being obtained,amongst other methods, by the action of phosphorus pentachloride onethyl acetoacetate; hence, the chlorhydroxybutyric acid in questionmust be a-chloro-P-hydroayB?~tyric acid.This acid was heated with hydrochloric acid, and a-/%diChloTObUt?/riCacid was obtained; it crystallises in long prisms and melts at 69".An alcoholic solution of the latter compound, when treated withalcoholic potmh, gives a-monochlorocrotonic acid.a-p-Dichlorobutyricacid is formed in like manner when a-monochlorocrotonic acid isheated with hydrochloric acid. A. T.Hydroxystearic Acids of Different Origin. By A. C. andM. SAYTZEFF (J. RUM. Chem. Xoc., 1886, 328--348).-A hydroxp-stearic acid was prepared by one of the authors some time ago in hiswork on the oxidation of oleic acid (Abstr., 1886, 140).Anotheracid of this composition was discovered by Fr6my (AnnuZen, 19, 296 ;20, 50; 33, lo), who obtained it by the action of concentratedsulphuric acid on oleic acid, and described it under t,he name of hydro-rnargaritic acid. Although the main points of the reaction had beensatisfactorily explained by FrBmy's work, yet subsequent work onthis question has mostly led to unsatisfactory results. SnbaneiefORGANIC CHEMISTRY. 31(Qbst?., 1886, 442) ha4 at last succeeded in throwing some new lighton the processes involved, but the authors do not in all cases obtainresults in agreement with his.Oleic acid was obtained by the saponification of oil of almonds, andpurified in the ordinary way by conversion into its lead salt.Theaction of sulphuric acid was regulated in such a manner as to preventthe temperature rising above 35". The mixture was then allowedto remain 20 hours a t a temperature below O", and decomposed bywater. In order to increase the yield of hydroxystearic acid, thefatty layer, separated by the action of water and solidifying a t theordinary temperature to a crystalline mass, was treated with alcoholicpotash, whereby the anhydrides of this acid are decomposed. Thesaponified product was then converted into the acid by boiling withsulphuric acid. When the products of the action of sulphuric acidon oleic acid are left for some time even at low temperatures, thequantity of hydroxystearic acid is diminished, whilst the quantity ofits anhydrides increases.Hydroxpstearic acid was extracted fromthe above-mentioned crystalline mass by repeated recry stallisationfrom ether and alcohol. So obtained, hydroxystearic acid,CH,. ( C H,) 13-CH,.CH( 0 H) CH2*C 0 OH,melts at 83-85", and resolidifies a t 68-65". At 20" alcohol (99p Ti-.)dixsolres 8.78 per cent., ether 2.3 per cent. of the acid. Tlydroxy-stearic acid does not absorb bromine. The free acid and the hydroxy-stearates of sodium, calcium, barium, copper, zinc, and silver, wereanalysed, and the formula of the acid shown to be C18H,0,.With hydriodic acid, hydroxystearic acid yields iodostenric acid.CH,*(CH,)13 CH,*CHI*CH2*COOH ; the latter can be converted intoordinary stearic acid by reducing its alcoholic solution with zinc andhydrochloric acid.When hydroxystearic acid is heated at 100" in sealed tubes withfuming hydrochloric acid, a syrupy liquid is formed, soluble in ether,insoluble in alcohol m d water, and having the composition of oleicacid.It does not show acid properties, nor give additive productswith bromine or iodine (in Hubl's solution); it is therefore consideredto be a complete anhydride of hydroxystearic acid,formed by elimination of 2 mols. of water from 2 mols. of the acid(analogous to glycolide or lactide). The anhydride is decomposedinto hydroxystearic acid by treatment with alcoholic potash a t tem-peratures above 150". Heated with dilute sulphuric acid (in sealedtubes at looo), hydroxystearic acid yields the same anhjdride, butwhen concentrated salphnric acid is iised a t ordinary temperature, twoother products of non-saturated character are formed, one corn biningwith 17 per cent., the other with 33 per cent., of iodine, when heatedwith it on the water-bath.These substances bear a great resemblanceto FrBmy 's metoleic acid, and will be further investigated.It wag shown that the hydroxystearic acid prepared by $he actio32 ABSTRACTS OF CHEMICAL PAPERS.of moist silver oxide on iodostearic acid was identical with thatdescribed above.Finally, the authors have studied the action of alcoholic potash oniodostearic acid. After heating the mixture in a reflux apparatus,and expelling the alcohol by distillation, the product of the reactionwas decomposed by sulphuric acid.An acid was obtained, solidifyingak ordinary temperatures to a crystalline mass, and consequently notidentical with oleic acid. It was purified by converting it into thesodium salt, recrystnllising this salt from alcohol, precipitating withzinc sulphate, recrystallising from boiling alcohol, and decompodngthe zinc salt by sulphuric acid. Thus purified, the substance crys-tallises from ether in translucent, rhombic tables, easily soluble inalcohol, sparingly in ether, and melts at 40-45". The compositionof this acid was found to be the same as that of oleic and elaidicacids. It is a non-saturated compound, taking up two atoms ofbromine 01' iodine. When oxidised by potassium permanganate i nalkaline solution, it yields dihydroxystearic acid, melting a t 78".The authors intend to continue the investigation of this solid oZeic acid.Another acid, melting a t 20-25", simultaneously formed by theaction of potash on iodost,earic acid, was found to be a mixture ofordinary and solid oleic acids.The constitution of solid oleic acid isCH,*( CH2) Is*CH2*CH : CH*COOTJ, ordinary oleic acid being repre-sented by CH3*(CH2)13*CH : CH*CH,-COOH. A. T.Action of Trimethylene Bromide on Ethyl Acetoacetate,Benxoylacetate, and Acetonedicarboxylate. By W. H. PKRKIN,Jun. (Ber., 19, 2.557-2561 ; comp. Abstr., 1886, 689).-When theacid C7Hl0O3 (from trimethylene bromide and ethyl sodacetoacetate)is boiled with aaker, carbonic anhydride is evolved, and Lipp'sacetobutyl alcohol (Abstr., 1886, 218) is formed. When the acid isdistilled, the anhydride of acetobutyl alcohol, CH2<cCH2.C,2-->0, CH : CHMeis obtained; it is a mobile oil.The same compound is also formedwhen acetobu tyl is heated. Strong hydrobromic acid dissolves theethyl salt C9Hla03, and decomposes it into bromobntyl methyl ketone( Lipp, Zoc. cit.) and carbonic anhydride. Benzoyltetramethylene-carboxylic acid is decomposed by hydrobromic acid in a similarmanner, with formation of the compound COPh*CH2*CHz*CH2*CHzBr ;this cyystallises in plates melting a t 61". The instability towardshydrobromic acid of the products obtained by the action of tri-methylene bromide on etbyl acetoacetate and benzoylacetate respec-tively, distinguishes them sharply from tetramethylenedicarboxylicacid.Trimethylene bromide acts on the sodium compound-CO(CHNa*COOEt)2(from ethyl acetonedicarboxglate and sodium ethoxide), yieiding thecompound C O O E t * C H ~ ~ ~ , ~ ~ C > O .The latter is a colour-less oil boiling at 238-240-(under 150 mm. pressure). The mon-et/t,yl salt melts at 114"; the free acid at 185--190" with decomORGANIC CHEMISTRY. 33position. When the monethyl salt is distilled, a subtance is obheinedapparently identical with the product of the reaetion between tri-methylene bromide and ethyl acetoacetate. The dicarboxylic acid isdecomposed by boiling water into acetobutyl alcohol and carbonicanhydride. N. H. M.Ethyl Acetotrimethyleneearboxylatk By W, H. PERBIN, Jun.,and P.C. FREER (Ber., 19, 2561--2569).-The fact that trimethylenobromide reacts with ethyl malonate, yielding a tetramethykne-derivative, and with ethyl acetoacetate with formation of an ether,sugges6ed the possibility that the product of the reaction betweenethylene bromide and ethyl acetoacetate (Trans, 1885, 801) is not atrimethylene-derivative bdt an ether. The aesults of determinationsof the magnetic circular polarisation, and the optical properties point,however, to the trimethylene formula first ascribed to the compound,E t h yZic brometh y Zucetoacetate, CH2Br+H2-CHAc*C00Et, is obtainedby dissolving ethyl acetyltrimethylenecarboxylate, well cooled., inhydrobromic acid, sp. gr. 1.85 (3 parts) ; after being left for 10minutes at the ordinary temperature, it is poured into ice water..Itis a yellowish oil, having an odour of camphor ; when exposed to airit becomes brown, and gives off hydrobromic aeid.. When reducedby means of zinc-dust and acetic acid, it is converted into ethyl aceto-acetate.Acetopropy I aZcohoZ, COMe*CHz-CH2-CH2-OH, is prepared by boiling20 grams of the above homo-compound for two hours with 5 gramsof hydrochloric acid and 20 grams of water. The reaction is analo-gous to that by means of which Lipp obtained acetobutyl alcoholfrom ethyl bromopropylaeetoacetate (Abstr., 1886, 216). It i s acolourless oil, very soluble in water; the solution very readily reducesammoniaeal silver solution but not Yehling's solution. It is veryunstable. A phenylhydrazine-compound was prepared.When thealcohol is heated, it is converted with evolution of water into a mobileoil, having an ekhereal odour ; it is probably an anhydride,CMe-cHqCH2* CH2>0(comp. A'bstT., 1886, 219).y-PeNty Zeme glycol, OH-CHMe*CH2-CR2.CH2-OH, is obtained byreducing acetopropyl alcohol with sodium amalgam. I t is a verythick, colourless oil, extremely soluble in water. It boils a t 210-220" with partial decomposition. When heated above its boilingDoint. or with 50 to 60 Der cent. of sulDhuric acid at 100'. it is con- I ' CHM - verted into the anhydride, CH2< CH,. &,>O, boiling at 78- 83".- -Pentylene glycol dissolves in hydrobromic acid (sp. gr, 1-85) withconsiderable development of heat ; when the solution is heated at W",the momobromohydrin of the glycol, C5HI13&, is formed, This is acolourless oil, which boils (under 150 man.pressure) at 144-145".N. H. M.Derivatives of Diaxosuccinic Acid. By T. C m r m and F.KOCH (Ber., 19, 2460--2462).--This is a continuation of the authors'previous work on this subject (Abstr., 1885, 885). Aspartic acid wslsVUL. LIr. 34 ABSTRACTS OF CF-IElIICAL PAPERS.obtained by the reduction of ethyl diazosuccinate with zinc-dust andacetic acid, thus proving the correctness of the formula formerlyascribed to diazosuccinic acid.NHz* CO* CN,*CHz*CO ONe(from the action of ammonia on methyl dia zosuccinnte), crystallisesin long, golden-yellow prisms soluble in ether and alcohol, and meltingat 84". When ethyl diaeosuccinate is acted on by cold slightlyacidified water, mulamic and f umalramic acids are produced. Malamicacid, NH,*CO*CH ( OH)*CH2*COOH, crystallises in colourless prismseasily solnble in water, alcohol, and ether, and melts a t 146" ; its methylsalt yields silky sca1e.s soluble in alcohol, ether, and water, and meltinga t 105".illethyl furnuramate, NHz*CO*CzH,*COOMe, crystallises incolourless plates, soluble in alcohol, and melts at 160-162". EihyZbenzoyZmaZamute, NH,*CO~CH(OBz)~CH,~COOEt, was obtained byheating together equal molecular proportions of benzoic acid and ethyldiaxosuccinamate a t 140-150". It forms colourless clinorhombiccrystals soluble in water, alcohol, and ether, and melts at 96-97". Itdecomposes easily when heated. The corresponding methyl salt form8colonrless crystals, melting at 78-80".By the action of iodine onan ethereal solution of ethyl diazosuccinamate an unsymmetricalethyl diiodowxinamate, NH,*CO*CI,*CH,* COOEt, is formed. Thiscrystallises in long, greenish-white needles which darken at 110",melt a t 132", and decompose at 150". The methyl salt and come-sponding methyl and ethyl hromo-salts are oils.Dichloropyromucic Acid. By A. DENARO (Gazzetta, 16, 333-335).-1f a current of dry chlorine gas is passed into the ethyl saltof pyromucic acid, a thick oil is at first obtained, probably consistingof the tetrachloride of the acid. This on decomposition with alcoholicpotash and subsequent acidification, yields a dichlorqyromucic acidwhich crystallises in white needles, melting at 167". Its barium saltcrystallises with 3 mols.HzO i n prisms, the calcium salt with 3$ mols.H,O in scales; both become completely anhydrous when heated to110". v. 1%. v.By 0. WIDMANN (Ber., 19, 2477-2$82).-As the mode of formation and reactions of this substanceare best explained by the formula CO' /GO, which 1111-doubtedly belongs to acetylenecarbamide, the author has carefullyre-examined these two compounds with the view of determiningwhether they are isomeric or identical. He finds that the latteris the case, and that the apparent differences in their reactionsare due to erroneous observation. When boiled with concentratedbaryta-water, acetylenecarbamide does not, as previously asserted,yield carbonic anhydride, but, like glycoluriI, is decomposed intohydantoic acid and carbamide.The solubility of acetylenecarbamidei 3 given by Schiff as 1 in 333 parts of water a t 15". The author fiadsthat pure acetylenecarbamide requires 1090 parts of water for solution,whilst a similar determination af the solubility of glycoluril showed aMethyl diazosuccinumate,L. T. T.Constitution of GIycoluriI.NH*CH*NH,I \NH.CH*NORUA'NlC CHENISTRY. 35ratio of 1 : 1060. Similar agreement was also found in the siher sdts,crystalline form, &c., both compounds crystallising variously in needles,prisms, or octahedra according to the solvent employed. Glycoluriland acetylenecarbamide are therefore identical, and the author pro-pofies the adoption of the latter name as the more suitable.Hydrocarbons from Tar-oils Boiling between 170" and 200".By 0.JACOBSEN (Ber., 19, 2511--2515).-The author has examined asample of coal-tar oil free from thiophen, of boiling point 170-200".By combined fractional distillation, conversion into sulphonic acids,sulphonic salts, and sulphonamides, he succeeded in isolating naph-thalene, pseudocumene, hemellithene, and another hydrocarbon, boilinglike the last-named at 175-175*5", but yielding a very solublemi+mwnide melting a t about 122-123". On oxidation, the hydro-carbon yields an acid which crystallises in needles melting at 119-121" and volatile in steam, aud also small quantities of a second acidmelting at 90". The acid of higher melting point yields isophthalioacid when oxidised with permanganate.Chloropropylbenzene.. By G.ERRERA (Gazzzetta, 16,310-325) .-I n order to determine the constitution of the chloropropylbenzeneobtained by the action of chlorine on the boiling hydrocarbon, thethree alcohols derivable from propylbenzene have been prepared andconverted into tbe corresponding chloro-derivatives.Phenylpropyl oloohoJ, C&Ph*CH2*CH20H, obtained from crudefitorax by Rugheimer's process, is not altered by gaseous hydrogenchloride, but when heated in a sealed tsbe with saturated hydro-chloric acid solution, it yields tbe chloro-derivative CH,Ph-CH,-CH,Cl.This compound i s a pale-yellow liquid, boiling at 219", and resemblingcymene in odour; when pure, it is very stable, being unaltered byprolonged treatment with fused xinc chloride or, silver acetate.Heated with alcoholic potttsh, it yields phenylpropyl ethyl ether,CH2Ph*CHe*CH20Et, a colourlem liquid boiling a t 220", insoluble inwater.NethyZ benzykd carbinoE, CHePh*CHMe*OH, obtained together with,allylbenzene and stilbene by the reduction of methyl henzyl ,ketonewith sodium amalgam, is a, liquid boiling at 215", of, a pale-yellowcolour and agreeable odour.Heated with hydrochloric acid in sealedtubes, it yields the chloro-derivative, CH,Ph*CHClMe, a yellowishliquid, boiling at 204-2Q7" with partial decomposition into allyl-benzene and hydrogen chloride. A similar reaction occurs with alGQ-holic potash, metallic zinc or its chloride.EthyZphenyZ carhino& CHPhEt-OH, prepared by prolonged reductionof the corresponding ketone with sodium amalgam, as described byBarry, is a liquid boiling at 215-217'.It is converted by gaseoushydrogen chloride, even at ordinary temperatures, into the chlorideCHPhEtCl, a yellow liquid. bailing about 200-205", but with con-siderable decomposition into bydrogen chloride and allylbenzene, 8change which takes place even on distillation in a vacuum. It isdistinguished from the two preceding chloro - derivatives by thereadimss with which it reacts with silver acetate, .xielding tbe itcetyl-L. T. T.L, T. T.d 36 ARSTRACTS OF CHEMICAL PAPERS.derivative, CIAPh'EkOAc, a liquid %oiling trt 227", of fruity odonr, andimsolixble in water. The chloropropylbenaene obtained by the directdhlorination of the hydrocarbon is identical with the second of the abovechloro-compounds, i n that it is decomposed by distillaticm and byalcoholic potash, as also by its stability towards silver aoebate.Iuthese properties, the chloro-derivatives of propylbenzene are directlycomparable to those of ethylbenzene.Reduction-of Trinitro-+-cumene. By F. MAYER (Ber., 19,2312-2314) .-In preparing nitrocnmidine by passing hydrogen sulphidethrough a boiling alcoholic solution of trinitro-+xmene, the chiefproduct is a new acid, CgH12N&305. T t is insoluble in alcohol, ether,glacial acetic acid, '&c., soluble in' hot water, from which it crystalliseson the addition of a few drops of hydrochloric acid in splendid, whiteor yellowish plates. Salts wereprepared. 'N.H. M.Hemellithene. By 0. JAUOBSEN (Ber., 19, 2517-2520).--Theauthor has investigated this compound, which he has now isolatedfrom the fraction of coal-tar oils boiling between 170-200" (see p. 35).Hemellithene, CsH3M, [ 1 : 2 : 31, boils at T75-175.5", and does notsolidify a t - 20". Tribrow~ohenl,ellithene, C9H9Br3, forms long needlesmelting at 245", and is very sparingly soluble in alcohol ; trinitrdhenzelli-tliene forms prisms melting at 209". The monnosulphonic acid crys-tallises in hydrated rhombic or hexagonal plates, and yields crys-talline salts ; its sulphonamide melts at 99tL-196". Hemellithehenol,C,H,,*OH [Me : Me : Me : OH = 1 : .2 : 3 : 51, is obtained byfusing the mlphonic acid with alkali. It is soluble in dcoholand ether, and crystallises in needles melting at 81".Hemelli-thy& acid, C,H,Me,*COOH [Me : Me: COOH = 1 : 2 : 31. is furmedby the oxidation of the hydrocarbon by dilute nitric acid. It isvolatile in steam, and crystallises in wales melting a+ 144". Its8aZcim salt is described. Distilled with lime, it yields mthoxylene.a - Sz~~rph.aminehemellithy1ic acid [Me : Me : COOH : SO,NH, =1 : 2 : 3 : 51, is formed by the oxidation of the above sulphonamide.It melts art Z W , and with hydrochloric acid yields a sulphohemelli-thylic acid melting at 180-190". ~-Szclprphaminehemellithylic acid[Me : "Me :COOH : SOZNHz = 1 : 3 : 2 : 51, formed a t the same time asthe-a-ackl, is more solhble, and melts a t 174". It yields avery solublesulphonic acid when ' hwted with hydrochloric acid.Both acidRwhen fused with potash yielded an easily soluble hydroxyhemellithylicacid, which does not give a blue coloration with ferric chloride.Hemellithene may be readily extracted from the tar oil by means ofthe sparing solubility of its barium sulphonate.Reciprocal Transformations Of Cymene and Cumenederi-vatives. By M. FILETI (Guzzetta, 16, 300-310).-In this paper arecollected the hitherto observed transformations of cumene and cymene-derivatives, the one into the other, and from them is drawn thefollowing generalisation :--A propy1-poup in the para-position rela-tively to a carbon-atom combined with other elements or with non-oxygenated groupings, is transformed into the isopropyl-group, if thisV. H. V.It melts at 240" and carbonises.L.T. TORGANIC CHEJIISTRT. 37element or grouping is displaced by an oxygenated radicle whoseoxygen is directly united to the carbon-atom compound, and converselyail isopropyl, is converted into a propyl-group when these substitutionsare reversed. (Compare Widman, Abstr., 1886, 453.)Chlorocymene and Bromocymene from Thymol. By M.FILETI and F. CROSA (Gazzetta, 16, 287 - 300). - Chlorocymene(parapropylmetachlorotohene), C6H3MePrC1, is obtained almost intheoretical proportions by heating in a reflux apparatus 4 mols. ofthymol with 1 mol. phosphoric chloride. On oxidation with nitricacid, Gerichten (Abstr., 1879, 238) obtained an acid, believed to be ahydrochlorocinnamic acid, C,H,n/Ie~1*Cil2.CH2*C0OH. It is here,however, shown that under these conditions three acids are formed,namely, chlorocumic, orthochloroparatoluic, and chloroterephthalicacids.Sixty per cent.of the theoretical quantity of bromocymene, calcu-hted according to the equation 4C,HI3*OH + PBr5 = CloH13Br +PO(OCloHlJ3 + 4HBr, can be obtained by the gradual addition of26 grams of bromine to 45 grams of phosphorus tribromide, and heat-i n g the resulting perbromide with 100 grams of thymol. On oxidn-tion with nitric acid of sp, gr. 1.2, bromocymene yields bromocumicacid ; with acid of sp. gr. 1.29, bromonitrocymene with bromocumic,bromonitrotoluic, and bromoterephthalic acids, whilst nitric acidof sp. gr. 1.39 yields the same acids without the bromonitrocy-mene. The bromcumic acid is identical with that obtained by thedirect bromination of cumic acid ; it has, therefore, the constitutionC6H,PrBr*COOH. The broinoizdrotoluic acid crys tallises in laminae,which melt at 200" without decomposition; it is isomeric with theacid obtained by the nitration of bromotoluic acid ; its barium saltcrystallises in long, yellow needles.The brornoterephthalic acid isidentical with that obtained by Fischli by the oxidation of bromopara-toluic acid. V. H. V.V. H. V.Ethylxylenes, By 0. JACOBSEN (Ber., 19, 2515--2516).-For thepurposes of comparison with hydrocarbons obtained from the fractionof coal-tar oils boiling between 170" and 200" (this vol., p. 35), theauthor prepared the three isomeric ethylxylenes from the three corre-sponding xylenes, using Fittig's method. Etlzylorthoxyle~~e yields acrystalline sulphonic acid, giving a sulphonamide crystallising inneedles melting at 126".Ethylmetaxylene boils a t 184-186", and isstill liquid a t - 15" ; its sulpphonic acid is crystalline, and yields crystal-line barium and sodiwm salts; its sulphoibamide melts at 148". Jbhyl-paraxylene boils at 185", and is still liquid a t - 20"; its suZphonic acidcrystallises in rhombic scales, forms crystalline barium and sodiumsalts, and yields a crystalline suZpphonamide which melts at 117".Ethereal Carbonates. By. G. BENDER (Ber., 19, 2265-22.71 ;compare Abstr., 1881, 48). -When naphthyl ethyl carbonate,OCloH,*CO-OEt, is boiled f o r some time, carbonic anhydride andalcohol are given off, and the residue consists of a, mixture ofa-naphthol and a, compound C2,H1202 (Zoc.cit.). The formation ofL. T. T38 ABSTRACTS OF OHEJIICAL PAPERS.diphenylene ketone oxides from salicylic acid (Perkin, Tmna, 1883,35) and the intermolecular change of sodium phenyl carbonate tosodium salicylate, suggest that Ohe naphthyl ethyl carbonafe mayhave become changed to the ethyl salt, OHCl,H6~COOEt, and that2 mols. of the latter have condensed with formation of the compoundCZ1H1",2 ; this would then be dinaphthylene ketone oxide,ClOH6<CO>ClO'Il6* 0The isonaeride obtained by boiling P-dinapht hyl diethyl orthocarbonate(loc. cit.) crystallises from benzene in thin prisms melting a t 194".When phenyl ethyl carbonate is heated a t 300" for 3-4 hoursdiphenylcarbonate is formed.Paraditoly 1 carbonate is obtained by heating paratolyl ethyl carbo-nate at 300"; it is insoluble in water, moderately soluble in hotalcohol, and melts at 115".Tlynayl ethyl carbonate is a thick liquid boiling at 260"; a t 300" itdecomposes into dithyrnly 1 carbonate, melting a t 60".Orthoaitrophenyl ethyl carbonate is prepared by the action of ethylchlorocarbonate on potassium orthonitrophenoxide.It is a heavyyellow oil which boils with decomposition a t 275-285". The arnido-salf, NHE,*C6HrO*C0.0Et, melts a t 95"; it is soluble in alcoho!,moderately soluble i n boiling water. When distilled, it gives offalcohol with formation of ar~hydro-orthamid~~7~e~~yl carbonate, C,H,NO, ;the latter dissolves in alkalis.The silver salt, C7H4AgN02, formsan amorphous, colourless precipitate. The ethyl salt is obtainedby boiling the compound with alcoholic potash and ethyl iodide.When heated with fuming hydrochloric acid, it yields ethyl orthamido-phenol and carbonic anhydride ; the constitution of the substance istherefore c6H,<~~~>co. Tbe phenylhydrazine compound of anhy-dro-orthamidophenyl carbonate, C6&<-O->C : N*NHPh, crys-tallisee in yellow needles, which melt at 208". The acetyZ-derivativemelts at 97-98". A InorLonrtro-co~npound was prepared ; it forms longyellow needles melting at 256". Bromine acts on the anhydro-corn-pound with formation of a nzonobromo-derivative ; this crystallises fromwater in plates melting at ,196". When treated with phosphoricchloridc, the compound C7H4ClN02 is .formed.Parahydroxybenzyl Alcohol.By J. BIEDERMANN (Ber., 19,2373-2376).-Parahydroxybenzt~l alcohol, OH*C6H4*CH20H, is prepared bydissolving parahydroxybenzaldehyde (I part) in a mixture of water(10 parts) and alcohol (5 parts) ; it is then acidified with dilute sulphuricacid and gradually treated with 3 per cent. sodium amalgam (40 parts).Grey crystals of diparahydroxyhydrobenzoin and oily drops of dipnra-hydroxyisohydrobenzoh separate. When hydrogen is no longerevolved, the solution is made strongly acid and left for 12 hours, it isthen filtered, the filtrate extracted with ether, and the ethereal extracttreated with hydrogen sodium sulphite. On evaporating the ether, thealcohol separates in needles ; these are purified by dissolving tlhem in hotchloroform and precipitating with light petroleum.It forms slenderN HN. H. MORG AKIU CHEMISTRY. 39white needles, readily soluble in water, alcohol, and ether, sparinglyin benzene and chloroform; sulphuric acid dissolves it, yielding asplendid 1-ed-violet solution. It melts a t 110". The alcohol is alsoformed when parahydroxybenzaldehyde is kept dissolved in aJcoholicpotash for several weeks, but the reaction is still very incomplete.The acety I-derivative, OH*C6H4*CH,.0Ac, is prepared by heating thealcohol with a mixture of glacial acetic acid and sulphuric acid. Itcrystallises from water in small yellow needles, melting at 84", and isreadily soluble in alcohol and ether, spariiigly in water, benzene,chloroform, &c.The diucetyl - derivative, OAc*CcH4*CH2*OAc, isobtained by heating pnrahydroxybenzyl alcohol with an excess ofacetic anhydride a t 160" for 5-6 hours. It forms yellowish needlesmelting a t 75", readily soluble in alcohol and ether, sparingly inbenzene, &c.Br~isic alcohol, OMe*C6H4*CHI,0H[ = 1 : 41, is formed when para-hydroxybenzyl alcohol is dissolved in methyl alcohol and digestedwith potash and methyl iodide for some hours at 100". The productis treated with wzter, heated to expel methyl alcohol and iodide, andextracted with ether. On evaporating the ether, it is obtained as anoil which gradually solidifies when kept over sulphuric acid. It crp-tallises from water in needles melting a t 45" (compare hbstr., 1888,460).N. H. 11.Synthesis of Betorcinol (p-Orcinol). By S. V. KOSTANECKI(Bey., 19, 22 18-2324 ; comr are Abstr., 1886, 242) .-Z'araxylorcinol[Me2 : (OH), = 1 : 4 : 3 : 51 was prepared from metadinitroparaxyleneby rcplacing the nitro-groups successively by amido- and hydroxyl-groups ; it is identical with Stenhouse and Groves's betorcinol (Trans.,1880, 396). The crude product obtained by nitrating paraxylene iscrystallised from alcohol to remove most of the orthodinitroparaxylene,dissolved in hot alcoholic ammonia, and treated with hydrogen sul-phide for about one hour; i t is then evaporated to dryness. Theparadinitro-compound, being more readily reduced than the meta-compound, is thus converted into paranitroparaxylidine, which isextracted by means of hydrochloric acid.The residue, insoluble inacid, was extracted with boiling alcohol, and yielded crystals of puremetadinitroparaxylene. This was reduced by dissolving in alcoholicammonia and treating for two hours with hydrogen sulphide, and thenitroxylidine [ Me2 : 50, : NH2 = 1 : 4 : 3 : 51 so obtained was convertedinto the corresponding nitroxylenol. The latter crystallises in yellowplates melting at 91". It was reduced with tin and hydrochloric acid,and the amidoparaxylenol diazotised ; to 1 gram of the hydrochloride10 grams of sulphuric acid and 100 grams of water were used, and thewhole kept cold by means of ice and salt.Paraxylorcinol so prepared has all the properties ascribed to it byStenhouse and Groves (Zoc.cit.), except that it yields a green fluo-rescent solution when treated with dilute soda and chloroform.Metaxylorcinol (Pfaff, Abstr., 1883, 918) crystallises from chloro-form in white monocliniccrystals, a : b : c = 1.7237 : 1 : ? ; p = 38" 21'.It boils a t 276-279". When heated with sodium carbonate solution a tlSO", metaayZol.ci,rLoZcurborylic acid, CsHMe2( OH),*COOH, is formed40 ABSTRACTS OF OHEMICAL PAPERS.The latter crystallises from dilute alcohol in well-formed prisms whichnielt with decomposition at 196", and give a deep blue coloration withferric chloride. N. H. M.AcetalsesoscinoL By - CAUSSE (J, Pharm. [ 5 ] , 13, 354-358).-The author has examined the action of sulphuric acid andheat on a solution containing acetaldehyde and resorcinol.Thecrystals obtained are insoluble i n water, ether, chloroform, and ben-zeue. They are soluble in alcobol, which yields them again partlychanged. Anhydrous ether dehydrates them, converting them in toII powder, which in time aggregates to yellow, translucent crystals.Thus purified, the compound decomposes on fusing with regenera-tion of resorcinol. Its composition is indicated by the formulac14Hl404 = C2H40 + 2C6H602 - H20. The action of heat on thecompound apparently removes the elements of water. Heated a t120°, a reddish powder was formed which could be obtained in largebrown crystals. These had the composition CzeE,60, = 2CI4H,,O4 -The reactionsindicate that the yellow crystals are st molecular combination ofaldehyde and resorcinyl ether, C,l&O,O( C6Ha*OH)2.Benzylarnine.By T. CURTIUS and G. LEDERER (Rer., 19, 2462-2463) .-When benzaldehyde and amidoacetic acid are heatedtogether a t 130", carbonic anhydride is evolved and benzylamineformed. Similar reactions seem to take place when cinnamaldehgde,salicylaldehyde, or orthonitrobenzaldehyde, are substituted for theBenzaldehyde, but the products are not so easily isolated.Citric Acid Derivatives of Paratoluidine. By J. M. G:LLH2O.The diacetyl compound, C36H1B012, melts a t 28'2".J. T.L. T. T.(Ber., 19, 2352-2354) -Citroparatoluidide, C6H,04(NH.C7H7),, isobtained by heating citric acid (1 rnol.) and' paratoluidine (3 mols.)at, 140-145" for 10 hours. It crystallises from alcohol, in which itis sparingly soluble, in lustrous, microscopic needl'es, melting a t 189".Citrodlparatoluide, C6H504(NH*C7B7) N.C7H,, is formed when citricacid (1 mol.) and paratoluidine (2 mols.) are heated at 160-170" forthree hours.. It melts at 205", is insoluble in water, rather readilysoluble i n ether and alcohol, and separates from the latter solvent insmall, yellow, well-formed crystals. When heated with citric acidat 140-145", it is converted into citroparatoluidide. Ammonia actson it, yielding a salt of citrTaraditoluidic acid, C6H,04(NHC7H7)2*OH.The latter crystallises from alcohol in groups of needles, melting at161".NC7H,, is prepared by addingparatoluidine (1 mol.) to a hot concentrated alcoholic solution ofcitric acid (1 mol.).On cooling, the solution yields clear prismaticcrystals; these are heated for two hours at 160-170", and crystal-lised from water. It melts a t 172*5", and dissolves readily in alcohol,ether, and hot water. N. H. M.By 0: WALLACH (Annalen, 234,350-364) .- Paxace tometatoluylenediamine, obtained by the actionIt is soluble in water, insoluble in alcohol and ether.Citroparafoluidic acid, C6H5O4(0H)Azo- and Diazo-compoundsORGANIC OHEMISTRY. 41of acetic anhydride on metatoluylenediamine (Abstr., 1883, 329) canalso be prepared by converting nitrotoluidine (m. p. 77.5") into theaceto-compound (m. p. L44-5"), and reducing this substance with ironfilings and acetic acid. By means of the diazo-reaction, the aceto-metatoluylenediamine is converted into acetamidocresol (m.p. 225"),proving t hatl the acetyl-group occupies the para-position.Parucetamidotolueneorthazodimethy lanild-ne,NHBc*C6H~e.N,*C6H4*N~e2,is formed when a, solution of the diazo-csmpound is poured into anice-cold alcoholic solution of dimethylaniline. The substance crystal-lises in golden plates and melts at 200". It unites withacids to formsalts, which dissolve in water, yielding deep-red solutions. Theacetyl-group can be eliminated by boiling with dilute sulphuric acid.P(rramidoto1ueneorthazodimethy Ianilins mystallises in golden scales.It melts a t 145", and dissolves in hot alcohol, chloroform, and ben-zene. The diazo-compound unites with phenol, fomning totueneazo-dirnethy l a d b eparawphenol, NMe2.C6~*N,*C6H3Me.N2*CsH4*OH.. This substance dissolves in dilute solutions of the alkalis, and isreprecipitabed by carbonic acid. It also dissolves in strong acids, andis reprecipitated by the addition of water. It dissolves freely inalcohol, ether, chloroform, and benzene.It isinsoluble in water, sparingly soluble in alcohol, b u t dissolves in strongsulphuric acid, with a red coloration.Pai.acRt~idotoluensorthazodiethzJlaniEine crystallises in needles ofa reddish-brown colour. It melts at 159", and dissolves freely inalcohol, ether, chloroform, and in acids. The sdts are decom-posed by large quantities of water. Orthacetometatoluylenediamine,NHAc*C6H&le*NH, [Me : NHAc : NH, = I : 2 : 41, prepared fromorthoamidoparanitrotoluene (m. p. 107"), crystallises in white needles,and melts at l4W.It is soluble in alcohol, in ether, and in hot water.Orthacetamidotolzceneljarazodintethylamili,ne melts at 192", and dissolvesfreely in almhol, chloroform, benzene, and ether. Orthamidotoluene-parazodirnethyllanili~~e melts at 215P, and is freely soluble inchloroform,Acetnmido b ,onZen emet azodimet h y landhe, NH Ac*C,H,*&*C,H,*NMe,,crystallises in plates, and melts at 184". Amidobenzenmzodimeth?yl-aniline forms golden scale% soluble in alcohol, which melt at. 165-166". w. c. w.The corresponding P-naphthol-compound melts about 24".Quinone-oximes. By 3;. SUTKOWSKI (Ber., 19, 2314-2317).-When thymoquinone-oxime is dissolved in cold, fuming hydrochloricacid, a yellow precipitate is formed, consisting of dichlorothymo-quinone and monochlbramidothymol (Andresen, Abstr., 1881, 590).When the precipitate is boiled with glacial acetic acid, a splendid reddye is formed.The reaction is of interest, as itl d ~ o a s the analogybetween the Beactions of thymoquinone and of thymoquinone-oximewith fuming hydrochloric acid. Andresen also obtained the sameproducts from thymoquinonechlorimide. The oxime is therefore thehydroxyl-derivative corresponding with the quinonechlorimide42 ABSTRACTS OF CHEMICAL PAPERS.When chloramidothyrnd hydrochloride and chloranil are hmted inglacial acetic acid solution, the red dye above mentioned is formed.Tetrachloroquiriol is formed in the reaction ; it crystallises in longcolourless needles melting at 832".Analyses of the dye point to theformula C30H35C13N203.In a similar manner, a dye was obtained by the action of parsmido-thymol on chloranil in glacial acetic acid solution. It has the cam-position expressed by the formula C,H38N203. (It dissolves in aceticacid, alcohol, ether, and benzene, but not in water. Ammonia dissolvesit with formation of a blue solution. Lead acetate gives a blue preoi-pitate. N. H. M.By M. LOEB (Ber., 19, 2340-2344) .--When the compound Cl6Hl2N2CI2O2, prepared by the action of car-bony1 chloride on ethenyldiphengldiamine (Abstr., 1885, ,1213), istreated with alkalis or acids, it is reconverted into the amidine.Boiling water has no action on it ; 'boiling alcohol converts it intocarbanilide, ethyl acetate, and ethyl chloride.The ethyl salt,OEt*CO*NPh*CMe : N*C6H4-COOEt, separates from its ethereal solp-tion in hard, lustrous, rhombic crystals which melt at 90.5". Whenthe chloride is dissolved in benzene and treated with dry ammonia,i t is converted into ethenyldiphenyldiamine and ammonium chloride ;aniline acts like ammonia.Amidine-derivatives.Ethenylimidobenzanilide, CMe<,,,>CO, N.CeH4 is prepared by theaction of carbonyl chloride dissolved in benzene on an excess ofethenyldiphenyldiamine ; i t crystallism from benzene in large, lustrousplates melting at 118". It is identical with the compound to whichthe formula CO( C11H13N2)P was previou-sly ascribed (Zoc. cit.). Dilutehydrochloric acid decomposes it wihh formation of aniline and phenglcyanate.When a saturated ethereal solution of ethenyldiphenyldiamine istreated with two or three drops of water and then with cyanogenuntil it has a wine-red colour, and allowed to remain for 16 hours, ablack crust is formed which yields a compound, C16H16W40; thelatter forms a white, crystalline powder very sparingly soluble in etherand benzene, and cannot be recrystallised, as it at once resinifies whenheated with solvents.It becomes violet at ;120", and melts withdecomposition at 165". Its constitution is probably analogous to thatof Griess' cyanocarbimidoamidobenzoic acid, as shown in the formulaNPh : CMe*NPh*C(NH)CN + H20. Ethyl allophanate is formedwhen urethane (7 partsl) and carbonyl chloride (1 part) are dissolvedin benzene and heated at 75". N.H. M.Preparation of Aromatic Amides. By 34. FEILETII (Gaxzei%a, 16,281--284).-The method, proposed by Letts, for the preparation ofthe nitriles by heating the carboxylic acids with potassium thio-cyanate, has been shown to yield the amides, if ammonium thio-cyanate be substituted for the potassium mlt. The former chaiige isattributed by Keku16 to the greater dehydrating action of thepotassium salt, an interpretation confirmed by the observation oORGANIC CIIEMISTRY. 48Muller that in the above method benzamide is formed if the processis conducted quickly, but phenyl nitrile if slowly. In the course ofthe preparation of cumonitrile, a small quantity of cuminamide isobtained from the crude product of the reaction, if the aqueoussolution, prerioudy rendered alkaline by ammonia, is agitated withbenzene.This amide crystallises .in glittering lamins melting a t153*5", insoluble in cold, sparingly goluble in hot water, soluble inalcohol. It is not decomposed by boiling with hydrochloric acid orpotash of moderate concentration. With mercuric oxide, i t yields aderivative, ( CsH4Pr*CONH),Hg + 1+H,O ; this crystallises in needlesmelting a t 190", insoluble in water, soluble in alcohol.V. H. V.Action of Alkyl Iodides on Dibenzylthiocarbamide. By C.REIMARUS (Ber,, 19, 2348--2349).-Will has shown (Abstr., 1882,723) that alkyl iodides react with diphenyl- and dibenzyl-thiocarb-amide, with formation of hydriodides of bases in which the alkyl-group is directly combined with sulphur.The author has found thatthe isomeric dibenzykthiocarbamide behaves analogously.Brnzy Zimidobei,zyZcarbuminethiomefhg I, SMe-C (NHCTH,) : NC7H7, isformed when methyl iodide and dibenzylthiocarbamide are heated for2-3 hours at 100". Thelproduct is dissolved in water, treated withsodium carbonate, and extracted with ether. The suZphate of the basecrystallises in lustrous needles readily soluble in water and alcohol ;i t melts a t 145". The hydrochloride forins large rhombic plates meltinga t 125" ; the h!jdriodide crystallises in splendid octahedrii melting at99", readily soluble in hot water.Benzy ZimidlJbelzzy Zcarbaminethioet~i yl, SEt.C(NHC&) NGTH,, crys-tallises in wide prisms, apparentlF monoclinic, which melt at 93" ; itdissolves readily in alcohol, sparingly in water.%he suZphate formslarge rhombic plates readily soluble in water and alcohol ; the plutiiio-chloride crystallises in needles.Corresponding compouuds were also prqpared from propyl iodideand amyl iodide.Phenylseleniocarbimide and Diphenylseleniocarbamide. ByH. STOLTE (Ber., 19, 2350-2352).--Yh enyZseZeniocarbimide, CSe*NPh,is prepared by passing hydrogen selenide into aqueous soda, evapo-rating, and adding isocyanophenyl chlolride diluted with ether toprevent the reaction becoming too violent. After a day, the productis filtered, the ether evaporated, and the residue steam-distilledand dried in a vacuum over sulphuric acid. It is.a yellowish-red oil,insoluble in water, readily soluble in alcohol and ether, and has onlya slight odour. When the ethereal solution of the substance istreated with ammonia, it is converted into monophenylseleniocarb-amide (Abstr., 1886, 781).Di13heiayZseleniocurbur)aide, CSe (NHPh),, is prepared from phenyl-seleniocarbimide by treating its ethereal solution with aniline.Theproduct is washed with ether, and crjstallised from alcohol. It meltsat 1M3 with decomposition.N. H. M.N. H. 3144 ABSTRACTS OF CHEMICAL PAPERS.Substituted Nitrogen Chlorides. By G. BENDER (Ber., 19,2272--2274).-When the compound C,H4<-5H> CO (this vol., p.38) is treated with bleaching powder and hydrochloric acid thecowpomzd C7H,N02C12 separates in colourless needles. When thelatter is brought into contact with quinol, an odour of quinone isgiven off, and on cooling crystals of quinhydrone separate.Thecomponnd is decomposed by alcohol, alkalis, aniline, &c., into the=TTTcompound C,H,Cl<f~>CO (Zoc. cit.) .Acetanilide, when treated with bleaching powder in presence ofacetic acid, yields the compound NPhCl*COMe. The latter has theproperties of the compound described above. It melts at 91' ; whenheated to.l72", it becomes yellow, effervesces violently and is convertedinto its isomeride, parachloracetanilide, melbing at 172". The samechange takes place when the substance is treated wibh cold hydro-chloric acid or when warmed with absolute alcohol; if more t,han2 grams be employed, a violent explosion takes place. The compoundreacts with paranitranibine, yielding acetanilide and ort bochloropara-nitrani line.The comPound <C&CO cH2*co >NC1 was prepared from succinimide : itcrystallises from benzene in large colourless crystals melting at 148".Ihnaamide yielded the cornpzclzd COPh*N€€Cl.This crystallisesfPom water in long prisms melting at 116".Condensation of Nitrobenzaldehyde with Hydrocarbons.By 0- TSCHACHER (Ber., 19; 2463-2464).-Baeyer has shown thatfatty aldehydes, in the presence of concentrated sulphuric acid, formcondenmtion products with aromatic hydrocarbons, whilst aromaticaldehydes do not. The author finds that the ilbtroduction of a nitro-group into the phenyl-ring gives to aromatic aldehydes the power offorming such condensation productsWith benzene, metanitrobenzaldehyde yields metanitrotripheny2;-methane, forming crystals melting at 90".With toluene, rnstanitro-phenydditoly ZmethaNe is formed.N. H. M.L. T. T.Compound of Pymvic Acid with Hippuric Acid. By A.HOFFMBNN (Ber., 19, 2554--2557).-6 grams of pyrnric acid weredi esCed with 11 grams of sodium hippurate and 25 grams of aceticaniydride on a water-bath. In a short time, a vigorous reactiontakes place and the temperature of the mixture rises to 108". Theproducf is dissolved in alcohol, the solution diluted with water,evaporated, and the brownish crgstala recvystallised from petpoleurn.Analyses of the compound point to the formula CJ&NO4; the sub-stance is therefore formed by the iinion of its two constituents (equalmols.) with elimination of the elements 0% water (2 mds.).I t formscolourless, flat needles melting at 157"'; iD is very readily soluble i nalcohol, ether, and acetic acid; insoluble in water. It yields saltscorresponding with a, bibasic acid, C1'LHllNOO. The barium salt,Cl2HEN'O5Br + 2H20, was prepared; when treated with acid, iORGANIC CHEMISTRY. 45yields the anhydride, ClzH9NOa, the acid not being capable of existingin the free state. When the anhydride is heated with hydrochloricacid at 140°, benzoic acid is formed. N. H. N.Phenyliodohydracrylic Acid. By E. ERLENMEXER and J.ROSENHEK (Ber., 19, 246&2465).-Ph eny l i o d ~ h y d r u ~ m ~ l ic (a-iodo-6-pheny Zh ydroxypropionic) acid, OH-CHPh-CH I*COOH, was obtainedby theaction of iodine chloiPide on cinnamic acid.A chloriodophenyl-propionic acid is probably fimt formed, whieh is then converted intothe hydroxy-acid by the action of water. The acid forms largecrystals which melt with decomposition at 137-139", and are solublein benzene. When treated with hydrochloric acid, this acid yields acompound C18H16CI104, which the author believes to have the formulanCHPh : CHG (OH) <g>C(OH) *CHI. CHClPh. L. T. T.Creasolcarboxylie Acid. By H. WENDE (Ber., 19, 2324-2327).-CreosoZcarbozylk acid, OH*C6H2&fe(O?Y1e).COOH [= 4 : 1 : 3 : 51,is prepared by gradually adding 4 grams of sodium to 50 grams ofcreosol through which a current of dry carbonic anhydride is beingpassed. The reaction takes place slowly with evolution #of hydrogenand slight development of heat, and is assisted by gently warming;much heat is then developed, and the reaction becomes rather violent.The product, when cold, is treated with dilute hydrochloric acid,extracted with ether, and the ethered solution extracted with sodiumcarbonate solution.It erystallises in needles melting at lHO-lX'i',dissolves sparingly in water, readily in alcohol, ether, and chloroform,and is almost insoluble in benzene and light petroleum. It sublimesunchanged when carefully heated, and aequires a deep blue colouswhen trea%ed with ferric chloride. The ammonium saIt crystallises inglobular groups of needles ; the potassium salt forms small, readilysoluble needles ; the barium salt is sparingly soluble ; the copper saltis a yellow powder; it is very electric when dry.The inethyl saltforms small, rhomhic crystals, a : 'b : c = 0.5285 : 1 : 0.7334 ; it meltsat 92", and gives a bluish-green coloration with ferric chloride. Theethyl salt crystallises in s m d l needles or prisms melting at 77".N. H. M.Derivatives of Op'ianic Acid. By C. LIEBERMAWN (Ber., 19,2275 - 2287 ; compare Abstr., 1886, 550). - Amidohemipinphenyl-,C : N -- NPhhydrazide (az~ianpheny lhydrnzide), NH( I I , is preparedC6H ( OMe) 2mc 0by the action of phenylhydrazine on azopianic acid. It separatesfrom its solution in benzene in small, honey-coloured, tetragonalcrystals, having a glassy lustre, a : c = 1 : 0.5947. It melts at 222",and dissolves in strong sulphuric acid and in fuming hydrochloricacid.Amido-opianpheny7hydrazide, NH2*C6H(OMe)2<-CH CO-NPh N->, is ob-tained by reducing the nitro-compound (Zoc.cit.) with tin and fumin46 ABSTRACTS OF CHEMICAL PAPERS.hydrochloric acid, care being taken t o prevent the reaction frombecoming too violent from the heat developed. On adding water toits alcoholic solution, it crystallises in slender needles melting at 157-143".is formed when nitro-opianphenylhydrazide is boiled with alcoholicpotash, and the potassium salt thus obtained' treated with hydro-ehloric acid. It crystallises in Fellow, glittering, rbombic plates melt-ing at 191". The potassium salt is a carmine-red powder.Oyianoxime anliydride (hemipiniinize), CJ&NO,, is prepared by boil-ing opianic acid (1 mol.) dissolved in nine times its weight of 80 percent.alcohol with, hydroxylamine hydrochloride ( I t mol.) for twoto three hours. It crystallises from alcohol in long, very slenderneedles melting at7 228-230". An aqueous or alcoholic solution con-taining only a trace of the subdance has a fine blae fluorescence. Itsublimes unchanged, and can be heated with strong sulphuric acidwithout decomposition. Cold aqueous a1 kali dissolves it, forming a,yellow solution which soon ldecomea colourless. When heated withalkali, it, yields hemipinic acid and ammonia. The compound was almprepred by heating ammonium hemipinate. The potassium salt,CloH80NK, is a white compound almost insoluble in cold absolutealcohol.Hemipinethyl imide, ClnH804 : NEt,.is obtained by heating potassiumhcmipinimide with ethyl iodide at 150".It crystallises from boilingwater in colourless- needles resembling hemipiuimide ; the solutionshows the same fluorescence. It diksolveR very readily in alcohol,acetone, and benzene, and melts a t 96-98".The formation of hemipinimide is interesting on account of itscomplete analogy with observations lately made in the phthalic acidseries. The author a,ssigns to the compounds phthalimide and hemi-pinimide the respective constitutional formulae. CO<-O'>C : NH0-and Co<G,(OMe),Anilido-opianic acid, Cl6HI5NOd, is obtained by boiling a solution ofequal weights of opianic acid and aniline, dissolved in gIacial aceticacid, for 10 minutes. On cooling, the whole solidifies to a, white mass,which is washed with water, dissolved in benzene, and precipitatedwith ether.It dissolves only in Btrong alkalisolution. Artilidonitropianic acid, C16H14N20s, is prepared from ni tr-opianic acid in a manner similar t o the above compound. It, cr-ystal-lises in needles melting a t 183-184". When treated with alkali, ityields n sparingly soluble potassiwn salt.Nitrohemipinic acid, K02*CsH(OXe)2(COOH)o, is very readily p1.e-pared by boiling nitropianic acid with fuming nitric acid (4 parts) forone hour. It melts a t 166" (not 155"), but has all the other propertiesascribed to it by Prim (Abstr., 1882, 402). Wben heated above itsmelting point, it gives up water and yields a yellowish compound,probably the anhydride.The silver s@Zt was also prepared.c6H4>C : NH.It melts at 186-187'ORGANIC CHEMISTRY.43Opianic anhydride, [ CHO*C,H,(OMe),*CO],O, is formed whenopianic acid is heated at 160" in a current of dry air. It crystalliseswell from acetone and melts at 234". It is identical with the coni-pound described by Wegscheider (Ahstr., 1883, 996) as triopiarnide,0,H,aO14. When boiled with alkali, it, is gradual17 transformed intoopianic acid. Strong nitric acid converts it into nitropiauic acid.Opianic Acid Derivakives. By C. IJTEBERMANN and S. KLEEMAKNN. H, M.(Ber., 19, 2287-2299).-AcetyZupinnic acid,is prepared by heating opianic acid and dry sodium acetate withacetic anhydride. The excess of. acetic anhydride is then removed bycontact with cold watey for 24 hours, and the remaining compoundcrptallised from boiling water.It is inso-luble in cold aqueous alkali, and when boiled with it, is decomposedinto opianic and acetic acids.>CH*OAb, is prepared Acetylnitropianic acid, <in a manner similar to acetylopianic acid. I& is a yellow substanceinsoluble in cold sodium carbonate solution.Propiony lopa'anic acid, C13H1406, crystallises in needles melting at111".An hyaraceta nt id oh emip inic acid, G ,,H,AcN O,, and trhe pi-opion y 1-compound, C,,H,( C3H,0)N0,, melt at 164" and 139" respectively ;they ape very unstable.)CH*CH,*COO@ is obtained byheating opianic acid (3 parts), rnalonic acid @+ part), glacial aceticacid (2 park), and sodium acetate (li Rart) for five hours at100" ; the colourless, crystalline product IS crystallised from water.It forms lustrous needles melting at 167" ; it has an aoid reaction anddissolves i n ammonia.The silver, calciunz, &c., salts were prepared.The ethyl salt crystallises in plates soluble in alcohol, ether, and hotwater; it melts at 82.5". The reactions of the acid are analogous tothose of phthalylacetic acid. When boiled with baryta, and the excessof baryta afterwards removed by means of carbonic anhydride, bariumopianylacetate" is obtained ; it forms lustrous prisms. The free acidis not capable of existence. When the silver salt is treated withmethyl iodide, it yields, not methyl opianjlacetate, but methyZm ecoiline-acetate ; the latter crystallises in lustrous plates melting at124".It melts at 120-121".(JO---C6H(N0,) @Me),co-CsH2(0Me)2 Necouiw-acetic acid, <>CH*CH,*COOH, is pre- co--0 Normecortine-acetia acid, <C,H,(OH),pared by heating rneconine-acet& ahd with hydriodic acid and phos-phorusi ; the product is diluted with water and filtered. It crystal-lises from water in long plates melting a t 218".The calcium andburiuwt saZts form white crystalline precipitates. When the acid is* The fmmtda slnd azalp:s given in the original do not agree48 ABSTRACTS OF CHEMICAL PAPERS.heated with ferric chloride, it acqfiires a characteristic blue colour,which changes to green in presence of an excess of ferric chloride,The ethyl salt separates from its solution in boiling water as an oil,which then solidifies and melts at 131".Its solution is fluorescentand reduces silver solution, but to a smaller exbenltthan the free acid.I t has an acid reaction and precipitates from baryta solution a yellowbarium salt of the ether. This acid property and the power ofreducing silver solutions is due t o the presence of pylrocatechol-hydroxyl.Ort h onitrom econine- acetic acid,co -o>CH.CH2*COOH [NO2 : CH*CH2*COOH=1 : 21, <C,H(N02)is obtained by dissolving meconine-acetic ncid in fuming nitric acidand afterwards precipitating with water. It forms colourless crystalsmelting at 176". The ethylsalt crystallises in lustrous needles, rcadily soluble in alco'hol andbenzene ; it melts at 129". Nitromeconine-acetic acid dissolves insulphnric acid, forming a.yellow solution ; this, when warmed, acquiresa cherry-red colour, characteristic of compounds containing a nitro-group in the ortho-position to a long side-chain (Baeyer, Abstr.. 1882,620). When the nitro-compound is reduced with tin and hydro-c hloric acid, dimethox y hy drocarbostyril- lactone,The calcitwt saZt forms yellow needles.is formed. This crystallises from water in colourIess needles, melt-inq with evolution of carbonic anhydride at 256". It is readilysoln'ble in alcohol and glacial acetic acid, insoluble in ether andbenzene. It dissolves in baryta; when the solution is boiled andtreated with carbonic anhydride and evaporated down, Iastrousneedles of barium dimethoxyhydrocarbostyrilcarboxylate are ob-tained.Dilnetliox~IddihydrochZoroquinoline lactone, 6C12Hl0N Clod, is preparedby heating the lactone just described with phosphorus pentachlorideand some phosphorus oxychloride for two hours at 165-170"; theproduct is poured into iced water, and the precipitate crystallised fronialcnhol, from which it separates in needles ; these melt at 218" withevolutim of carbonic anhydride.The barium) salt, obtained by boilingthe lactone with baryta, and the silver salt were prepared.Dihydroxydihydroquinoli?ie lactone, CloH,IIU'O,, is obtained by heatingthe above chloro-derivative dissolved in glacial acetic add for onehour at 120" with hydriodic acid. It melts at 220" with decomposition.By H. GRCNR (Ber., 19, 2299-23@5).-Azo-opianic acid, prepared from nitropianic acid, melts at 200" withdecomposition (not 184" as given by Prim, Abstr., 1888, 404).Thepofassium salt is a white crystalline powder. The et?iyl salt crystal-1ises in needles melting at 98" ; the methyl salt melts at 127". Theauthor confirms the statement of Prinz ( ZOC. cit.) that azopianic acid,when boiled with barytzt in excess, yieIdrJ barium amidohemipinateN. H. M.Azo-opianic AcidORQAXIC CHEMISTRY. 49The yield is almost quantitative. Sodium amidohenzipinate crystallisesfrom alcohol with 3 mols. H,O, in long, almort white needles ; it isvery readily soluble in water. The copper salt (with i mols. H,O)erystallises in stellate groups of slender, green needIes. The aqueoussolution of the free acid has a fine green fluorescence which disappearswhen alkalis or acids (except acetic acid) are added.It reduces acold animoniacal silver solution, and Fehling's solution when warmed.ob-tained when a cooled solution of sodium amido-hemipinate is treatedwith sodium nitrate and hydrochloric acid. It is a bright yellow, micro-crystalline powder which becomes superficially red when exposed tolight, and explodes at 140-150" or when struck. It dissolves readilyin alkalis and acids ; when boiled with water, it gives off nitrogen andyields a hydroxy-acid, which gives an intense blue-violet colour withferric chloride. The hydrochloride, COOH*CsH( OMe),( COOH)*N,Cl+ H20, crystallises in long, colourlew needles ; in presence of water,it decomposes into hydrochloric acid and free anhydroazohemipinicacid.When the diazohemipinic acid is boiled with alcohol undsrslight pressure, it is converted, with evolution of nitrogen, into hemi-pinic acid.Nitrohemipinic acid was prepared by Liebermann's method (thisvol., p. 46). The potacsium sult crystallises in deep yellow prisms,readily soluble in water and alcohol, the silver saZt is also yellow.21Titrohen2ipinic rcnhydride, NO,*CsH( OMe) <co > 0, is preparedby heating the acid at 160-165" for two hours ; it crystallises frombenzene in bright yellow prisms melting a t 145". When nitrohemi-pinic acid is reduced with ferrous sulphate and soda, amidohemipinicacid is formed identical with the acid obtained by boiling azo-opianicacid with baryta.The results of the experiments above described confirm the viewbrought forward by Liebermann (loc cit.) that Prinz's so-called azo-opianic acid is not an azo-derivative of opianic acid but an internalanhydride of orthamidohemipinic acid.When nitrohemipinic acid is reduced with tin and hydrochloricacid, the compound COOH.C6H,( OMe)2*NH2,HC1 is formed.N.H. M.Derivatives of Normethylnitropianic Acid. By K. ELBEL(Ber., 19,2306-2312) .-Normethylnitropianic acidCOH* C6H ( C 0 OH) (OH) ( OMe) *NO,,is best prepared by heating finely powdered nitropianic acid withfuming hydrochloric acid (10 parts) for 15 hours at loo", with a refluxcondenser, hydrogen chloride being passed in all the time. Theproduct is evaporated down, when the normethyl-compound sepa-rates ; the yield is 80 per cent.of the theoretical.Normethylorthanhyd~-lzmidohemipinic acid (normethylazo-opianicacid), OMe*C6H(OH)(COOH)<~~> [OMe: OH : COOH : CO : NH= 4 : 3 : 2 : I : 61, is obtained by treating a boiling saturated aqueousN,-0 Anhydrodiazohenzipinic acid, COOH*C6H(O~e)2< co >, iscoVOL. LII. 50 ABSTRACTS OF CHEMICAL PAPERS.fiolution of normethylnitropianic acid with tin and hydrochloric acid.It is dissolved in alcohol and precipitated with water. It crystallisesi n colourless, lustrous needles which melt at 174-175" with decom-position ; i t is readily soluble in alcohol, sparingly in benzene, andinsoluble in ether. When boiled with baryta, crystals of bariumnormet h ylamido hemi pinate are formed. The diacety I-d erivative,O&fe*C6H(OAc) (COOH)<NA:>, cooMe*C,H(oAc)(CooH)<,,>, co melting at 198'.is obtained by boiling normethyl-anhydramidohemipinic acid with sodium acetate and acetic anhydride(10 parts) for one hour.It melts a t 205", dissolves readily in ben-zene; the alcoholic solution has a fine blue fluorescence. It is veryunstable and changes when kept into the monacetyl compound,Normethy/nit?.opianic acid phenylh ydrazine crystallises in redneedles which melt a t 178-179" with decomposition. When boiledwith glacial acetic acid, it parts with the elements of water and yieldsnorrnethy Znitropiaxide, No2*C6H(0Me) (OH) < ca: : N->. Thelatter crystallises in lustrous, lemon-coloured, rhombic plates meltingat 191". I t dissolves unchanged in dilute potash solution.Thepotassium salt is very readily soluble in water, almost insoluble inabsolute alcohol. Normethy Zamido-opiaxide is obtained by boiling thenitro-compound suspended in ammonia with ferrous sulphate. Itcrystallises from alcohol in short, almost colourlesv prisms.CO*NPhNormethy1rritro~'anoximic acid,NO2*CsH(OMe) (OH)(COOH)*CH :NOH [ = 6 : 4 : 3 : 2 : 11,is formed b;j- mixing a boiling solution of normethylnitropianic acidin water (40 parts) with an aqueous solution of hydroxylamine hydro-chloride and sodium acetate. It crystallises from alcohol in lustrousyellow needles which become brown when warmed, and melt at 252".It has a slight reducing action on Fehling's solution. It dissolves inalkali with SL deep-red colour, and the solution gives off ammonia,when boiled, with formation of normethylnitrohemi~inic acid,NO,*C,H(OMe) (OH)(COOH), [ = 6 : 4 : 3 : 2 : 11.The latter crys-tallises from alcohol in almost white, silky needles, readily soluble inwater and alcohol; it melts at 220". The hydrogen potassium saltforms bright yellow prisms. The same acid is formed when nor-methylhemipinic acid is nitrated with dilute nitric acid,Normethylnitrohemipinimide, N02*C6H( OMe) (OH) <C CO.0- H)>, isobtained by boiling an alcoholic solution of normethylnitropianic acidwith hydroxylamine hydrochloride, or better by boiling normethyl-nitropianoximic acid with glacial acetic acid. It crystallises in brightyellow needles which melt a t 252" with decomposition.Homo-orthophthalimide. By S.GABEIEL (Ber., 19,2363-2367 ;compare Abstr., 1886, 812, and this vol., p. 61).-When a solutionof homo-orthophthalimide (2 grams) and potash (1 gram) in methylalcohol (15 c.c.) is digested with methyl iodide (4 grams) at loo",N. H. MORQANIC CHEMISTRY. 51dimethylhomo-orthophthalimide, CgH5Me2NO2. is formed. The lattercrystallises from water in flat needles melting at 119-120"; it isreadily soluble in the usual solvents and in alkali. When heatedwith potash and methyl iodide a t loo", it yields the trimethyl-derivative, CDHaMe3NO2 ; this cry stallises in long needles melting at102-103" : it is readilv soluble. Alkali does not dissolve it.CH G O Howio- ort hophthalmeth y limide, C&< .kMe > , is formed byevaporating a mixture of homo-orthophthalic acid and methylamine,arid distilling the residue.It forms long, colourless needles, whichmelt a t 123" and boil at 314-318". I t is readily soluble in the usualsolvents and dissolves in alkalis. When heated with methyl iodideand potash, it yields trimethylhomophthalimide melting at 102-103".In the latter compound, therefore, one of the methyl-groups isattached to nitrogen. Trimethylhomophthalimide is hardly attackedby fuming hydrochloric acid at 100", and so cannot contain methoxyl;when heated with the fuming acid a t 230-240", the anhydride of a co This crystallises in flatcrystals melting at, 82.5-83" ; the silver salt, Cl1HI6OkAg2, was pre..pared. The anhydride is also formed when dimethylhomophthalide(fi-om homophthalide, potash, and methyl iodide) is heated a t230" with fuming hydrochloric acid; ammonia is formed in thereaction.Tri- and di-methylhomophthalimide and the anhydride (m.p.82.5433") have probably the constitution expressed in the formula-, bibasic acid, C,H,Me,<CO>O, is obtained.Action of Amines on Phthalylacetic Acid. By E. MERTENS(Bey., 19, 2367--2373).--Pure phthalylacetic acid is stiriaed withwater and treated with a 33 per cent. solution of ethylamine until itis dissolved ; it is then filtered and saturated with hydrogen chloride,being kept cold the whole time. A white crystalline substancegradually separates with ,slight evolution of carbonic anhydride,Analyses show the compound to have the formula C~~&,O~NZ.Itmelts at 129", dissolves readily in warm alcohol, ether, and chloro-form, more sparingly in benzene ; boiling water decomposes it.2Methylei~eyphthalethimidine, CO< z g i > C CHz, is formed when thecompound C,H,,O,N, is heated above its melting point ; carboriioanhydride and water are evolved. It has a carrot-like odour, distilswith steam, and is readily soluble in alcohol, ether, and chloroform,&c. It strongly resembles Gabriel's methylenephthalomethimidine(Abstr., 1885, 1228).Phthalethimidylacetic acid, C@< %g(>C : CH-COOH, is obtainedby keeping a solution of the compound C,H24N205 in sulphuric acid(10 parts) for 24 hours, and then pouring it into water. The whitecrystalline precipitate is crystallised from dilute alcohol, from which iteC52 ABSTRACTS OF CHEMICAL PAPERS.separates in yellow needles melting a t 180" with effervescence.It isreadily soluble in hot water, alcohol, and ether, less soluble inbenzene. The silver salt forms a flaky crystalline precipitate; thebarium saZt crystallises in yellow lustroufi needles. Propylamine andphthalylacetic acid yield the compound C,,H,,O,N,. It forms largewell-formed prismatic crystals which melt with effervescence a t 103".It behaves similarly to the ethylamine compound.Acetophenone-orthocarboxa.,7iZideJ COMe*C6H4*CO*NHPh, is obtainedby warming phthalylacetic acid with aniline. After the evolutionof carbonic anhydride has ceased, the whole is left for 24 hours,when the substance separates in white crystals.It crystallisesfrom benzene in large, well-formed cubes which melt at 189-192", and dissolve readily in warm alcohol, ether, or chloroform.When heated a t 204" and afterwards a t 2.30". it is converted withevolution of aniline and water into rnethylene~hthal~~enimiLJine,CO<::~>C CH,. The latter crystallises in yellowish prismsreadily soluble in alcohol, ether, and chloroform; it melts at 100".When acetophenonecarboxanilide is kept dissolved in strong sol-sulphuric acid for 24 hours, it is converted into a compound, C16H11N0,isomeric with the compound just described. It is sparingly soluble inalcohol and ether, readily in benzene, chloroform, and light petroleum ;it melts at 265". N. H. M.Bromoterephthalic Acid. By M. FILETI (Gaxzetta, 16, 284-287).--Pischli (Abstr., 1879, 639) states that the monobromotere-phthalic acid obtained by the oxidation of bromotoluic acid retains1 mol.H,O, even after drying a t 120". As the same acid obtainedfrom bromocymene was found to be anhydrous, the author hasrepeated Pischli's experiments. The analytical results obtained forthe proportion of carbon and bromine show that this acid is alsoanhydrous. Itssilver salt is precipitated as a white, gelatinous mass, somewhatsoluble in water. The methyl saZt, C6H,Br(COOMe)2, obtained fromthe said chloride (Fischli), as also from the acid itself (Fileti), crystal-lises in acicular prisms, melting at 5 2 " ; it presents a well-markedchromatic polarisation. V. H. V.It melts a t 296", and at the same time sublimes.Curnidic Acids. By E.SCHNAPAUFF (Ber., 19, 2508--2511).-Theauthor prepared a-cumidic acid,C6H&fez(GOf)H,), [Me : Me : COOH : COOH = 1 : 3 : 4 : 61,by a modification .of Wurtz's process, by the action of efhyl chloro-carbonate and sodium amalgam on dibromometaxylene, This acidforms glittering prisms melting much above 320"' and subliming withonly slight decomposit,ion. It is easily soluble in boiling alcohol, verysparingly in boiling water. Its barium salt crystallises with 1+ mol.H,O, and is very soluble in water: the methyl salt forms long needlesor plates and melts a t 76".Cumidic acid, obtained as described by Jannasch (this Journal,18'71, 240) by the oxidation of durene, was converted into the methyORQANIC CHEMISTRY.53salt, and this by crystallisation from alcohol was separated into twoparts, the one melting a t 76" the other crystallising in needles and.melting at 114". The former was the methyl salt of the a-acid j u s tdescribed. The ether melting a t 114" yielded @-cur/lidic acid[Me : Me : COOH : COOH = 1 : 4 : 2 : 51 on hydrolysis. This acidis easily soluble in boiling alcohol, very sparingly in boiling water ; itrr\-stnllises in hexagonal prisms, and sublimes at high temperatureswithout previous fusion. Its barium salt crystallises with 24 mols.H20; its methyZ salt melts at 114" and boils at about 297" (corr.).When the barium salt is distilled with excess of lime, paraxylene isformed, so that the above formula may be regarded as established.Jannasch's acid is, therefore, a mixture of two isomeric cumidioacids.L. T. T.Reaction of Stilbene. By (3. ERRERA (Cazzetta, 16, 325).-Kade(Abstr., 1880, 46) states that stilbene in alcoholic solution gives a redcoloration when heated with a solution of ferric chloride. It is hereshown that this change is in reality due to the presence of water inthe alcohol, which causes a partial decomposition of the ferricchloride into hydrochloric acid and some stable form of ferrichydroxide. Stilbene is not even necessary for the reaction ; if absolutealcohol is used no colour-change ensues.By T. ZINCKE (Ber., 19, 2493-25Q2) .-Inthe hope of elucidating the constitution of the two compounds,C3,H,,N,0s and CB1HP2NCOG (Abstr., 1882, 736, and 1883, 210), ob-tained by the action of nitrous acid on P-naphthaquinone-anilide and-toluide respectively, the author has undertaken similar investigationswith phenanthraquinone.I n the present communication, the authordetails some preliminary experiments as to the action of alkalis onhalogen-derivatives of /I-naphthaquinone, which were made to deter-mine whether @-naphthaquinone-deriva tives undergo changes similart o the conversion, by the action of alkalis, of phenanthraquinone intodi phenyleneglycollic acid.theaction of bromine in acetic solution on p-naphthaquinone, and crystal-lising in red prisms melting at 177-178", dissolves readily in coldtlilute alkalis. From these solutions, acids precipitate hjdroxybromo-/3-naphthaquinone, described by Merz and Baltzer.Aniline and am-monia also act on bromo-/j-naphthaquinone, forming corn poundsanalogous to naphthaquinoneanilide. Dibrorno - /3 - naphthayuino,he,[0 : 0 : Br : Br = 1 : 2 : 3 : 41, could not be obtained directly fromnaphthaquinone, but was formed by the action of excess of bromineon an acetic solution of the monobromo-derivative. It is best ob-tained, however, by the action of bromine on a-amido-p-naphthol. Itcrystallises in red: rhombic scales or tables, sparingly soluble in;~lcohol and ether, and melts a t 172-174". With ammonia andaniline, it yields the same compounds as the monobromo-derivative.It dissolves in cold dilute alkalis, and from these solutions acidsIrecipitate a substance, crystallising in small white needles ; this hasnot beeu further investigated.V.H. T.p-Naphthaquinorre.Rro.rrLo-@-nuphthaqIcinone, [0 : 0 : Br = 1 : 2 : 31, obtaine54 ABSTRACTS OJ!' CHENICAL PAPERS.ChEoro-P-naphthaphone, [0 : 0 : C1 = 1 : 2 : 31, is formed whenchlorine is passed through a solution of p-naphthaquinoiie in tentimes its weight of glacial acetic acid, until a precipitate begins to beformed. It crystallises in red needles, soluble in alcohol, glacialacetic acid, and benzene, ahd melts a t 172". It gives an additiveproduct with hydrochloric acid which forms white cr,ystals. Itdissolves in dilute alkalis, and this solution when acidified yieldshydroxychloro-a-naphthaquinone. The unstable p- hydroxy-compoundundoubtedly first formed passes into the more stable a-derivative.When chloro-P-naphthzquinone is reduced with sulphurous acid i nacetic solution, chloro- p - naphthapuinol, C,H,Cl(OH),, is formed,and crystallises in long, colourless needles melting a t 116-117".The anilide and imide of chloro-p-naphthaquinone both crystnllisein dark-coloured scales having a metallic lustre, the former substancemelting a t 253", the latter at 260".Dichloro-p-naphthczpi~inzone, [0 : 0 : C1 : C1 = 1 : 2 : 3 : 41, may beobtained directly from the quinone, but is best prepared by the actionof chlorine on a-amido-p-naphthol.It crystallises i n red scales,needles, or tables, easily solnble in chloroform and boiling benzene,sparingly in alcohol, melts a t 184", and sublimes without decom-position.With ammonia or aniline, it forms the imide or aniliderespectively. When reduced with sulphurous acid in acetic solution,it yields dichloro-/3-naphthaquinone, crystallising in white needleswhich melt a t 125". Ik dissolves in cold dilute alkali, and thisEolution when heated becomes cloudy, and deposits a greyish-whiteprecipitate. If the cold alkaline solution be treated with excess ofacid, an acid of the formula C,H,Cl?03 is liberated. This acid crys-tallises with 1 mol. H20 in small white needles, melts a t 98-100",and is easily soluble in alcohol, sparingly so in water. Its methyZsmZt forms colourless scales or hexagonal plates melting a t 13'7-138".The action of the alkali on the dichloroquinone appears to take placeaccording to the equation C,oH4Cl,0, + H,O = CloH,Cl,O,.Theauthor considers the action to be similar to the action of alkalis onphenanthrsquinone, and the most probable constitution of the acid t ohe CCl<ccl:> C6 I3 C( OH)-COOH. The acid forms an ncety Z-dericative,melting at 75-76'. Boiling baryta-water or alkalis cause a separa-aion of carbonic anhydride. When a solution of the acid in glacialacetic acid is treated with concentrated sulphuric acid at 120", hydrogenchloride is evolved, and a yellow crystalline compound melting at224-226" is produced. The acid is decomposed on heating itsaqueous solution, a yellow compound of intense odour and volatile insteam being amongst the products of reaction.The experiments on the bromo-derivatives were carried out inconjunction with Weltner, those on the chloro-derivatives withC.Frolilich. L. T. T.Benzene- and Toluene-azonaphthols and their IsomericHydrazine-derivatives. By T. ZINCKE and I?. RATHGEN (Ber., 19,2482 - 2493). - W $en the two position-isomerides, benzeneazo-p-naphthol and P-napl -thaquinonehydrazide (see Zinckc and BindewaldORGANIC CHEJIlSTRY. 55Abstr., 1%35, 391), are reduced by means of stannous chloride, theformer yields a-amido-@-naphthol, the latter P-amido-a-naphthol.When a-amido-/I-naphthol is oxidised, P-naphthaquinone is formed,but the authors find that p-amido-a-naphthol yields under similarconditions P - diriaphthaquinone (/3 - dinaphthadiquinone). Bothquinones yield with bromine dibromo-p-naphthaquinone.When heated with nitric acid, benzeneszo-P-naphthol yields dinitro-P-naphthol, CloH5(OH)(N0,), [NO, : OH : NO, = 1 : 2 : 41, whilstp-naphthaquinonehydrazide yields dinitro-a-naphthol [OH : NOz : NO,= 1 : 2 : 41.Whenthe above isomeric hydraside and azo-compound are reduced in alkalinesolution, they are both decomposed into aniline and amido-naphthol.The author disputes the correctness of Denaro's assertion (Abstr.,1886, 246) that two isomeric benzeneazonaphthols can be obtainedfrom p-naphthol.The authors have also investigated the corresponding toluene-deriva-tives. Pitratolueneazo-a-naphthol, OH*CloH6*Nz*C7H7 [OH : N, = 1 : 41,was prepared like the similar benzene-compound. It crys tallises indark-red flakes having a metallic lustre, aud melts with decompositiona t 208".It is easily soluble in acetone, aniline, and alkalis, sparingly soin alcohol and acetic acid. No bromo-derivative could be obtained.Nitric acid yields dinitro-a-naphthol (b. p. 139"). The hydrochloridaand hydrobromide form bluish-green scales, which are slowly decom-posed by water, rapidly by alcohol. It also Eorms metallic derivatives.The ethoxide crystallises in red needles, which appear yellow bytransmitted light, and melt a t 126-127"; the methoxide melts a t103-104" ; the acetyl-derivative crystallises in yellow needles meltinga t 101-102". Orthotolueneazo-a-naphthol, [OH : N, = 1 : 41, formsred needles melting a t 144-146', soluble in alcohol, benzene, andncetic acid. It forms dinitro-a-naphthol with nitric acid, and yieldssalts resembling those of the para-compound. The sthoxide crys-tsllises in red scales melting at 94", the methoxide in reddish-brown needles melting a t 93".Para- and ortho-tolylhydrazides ofa-naphthaquinone are identical with the corresponding azo-com-pounds.Parato Zuene-@naphthol, ClOH~ON,H*C,H7, or C10H6 (0 H) *Nz*C7R7[0 : N, : : 2 : 11, forms red crystals with green flnorescence, is solublein alcohol, benzene, and acetone, and melts a t 134-135". It formsvery unstable salts with acids. The dibrorno-derivative forms intenselyred needles melting at 190". Nitric acid converts the azo-componndinto dinitro -P-napht hol (m. p. 194"). 0 rthotol ueneazo +-nap ht h ol,[O : N, = 2 : 11, crystalliscs in small red needles or scales which melta t 131".With nitric acid, it yields a dinitro-p-naphthol melting a t167". The tolylhydrazides of P-naphthaquinone are, like the similarphenylhydrazide, isomeric and not identical with the nzo-compounds.They resemble them, however, very closely, the chief difference beingtheir greater solubility i n alkalis. P-Naphfhaquinone-iuaratolylhydr-azide, CIOH60*N2H*C7H7 [0 : NP = 1 : 21, crystallises in small, red,glistening needles which melt at 145". The dibromo-dericative,CliH12B~-20, forms red, sparingly soluble needles melting at 236".B-NallhthapuinrJne-o~t~iotol~~li y draxide crystallises in red scales with aThe P-derivative melts at 1!34", the a- a t 138"56 ABSTRACTS OF CHEMICAL PAPERS.golden-yellow fluorescence. It is easily soluble i n the usual solventsand melts at 156".Its dibromo-derivative melts at 254". Besidesthese hydrazides, the product of the action of the tolylhydrazinc onthe p-naphthaq uinone always contained considerable quantities of di-naphthyldiquinol. L. T. T.New Diamidodinaphthyl. By P. JULIUS (Ber., 19,2549-2552).-am-Dinaphthyl is best prepared by distilling a-dinaphthol with zinc-dust (10-15 parts) : the distillate is re-distilled in a vacuum andrecrgstallised from glacial acetic acid.Mononitrodinaphthyl, C10H7*C10H6*N02, is obtained by adding nitricacid, of sp. gr. 1.3 (20 grams), to a solution of dinaphthyl (10 grams)in 150 C.C. of glacial acetic acid. It crystallises in lustrous, orange-coloured plates melting at 188". It dissolves easily in hot benzeneand glacial acetic acid, less readily in alcohol and ether.Dinitrodinaphthyl, N02*C10H6*C10~6*N01, is prepared by treating asolution of 10 grams of dinaphthyl in 150 C.C.of glacial acetic acidwith 80 grams of nitric acid, and then heating at 60". It crystallisesin bright yellow, volumiiious needles which melt at 280°, it dissolvesvery sparingly in benzene, xylene, and glacial acetic: acid, and ispractically insoluble in other solvents.Uiczmidodinaphthyl hydrochloride, ~H,*C,oH6~C,oH60NHz,2H~l, isprepared by treating 10 grams of the dinitro-compound, suspended in200 C.C. of glacial acetlic acid, with hydrochloric acid, and50 grams ofzinc-dust. It is readily soluble in water, sparingly in strong hydro-chloric acid ; when exposed to the air, it quickly becomes green.Thefree base could not be isolated. The diacety 1-derivatiue crystallisesin almost colourless needles which melt above 300" ; it is insoluble.When the hydrochloride is treated with ferric chloride, dark-brown,lustrous needles of diimidodinaphthyl h?ydrochloride, CZoH,,N,C1,, .areobtained ; this is reconverted by reducing agents into the diamido-compound. N. H. M.Tetrahydroxyanthraquinones. By E. NOAH (Ber., 19, 2337-2340) .-When metahydroxybenzoic and gallic acids (equal mols.)are heated with sulphuric acid (10 parts) for 20 hours at 170", twotetrahydroxyanthrapuinones, ClaHa( OH),O,, are formed, together withhexahydroxjanthraquinone. The product is extracted with alcohol,the solution evaporated to dryness, and the residue extracted withbenzene.The solution contains +now only one tetrahydroxyant hra-quinone. This crystallises in long, slender, red, lustrous needles,which do not melt at 350", and sublime with difficulty, becomingpartly carbonised. I t is readily soluble in alcohol, acetone, andglacial acetic acid, sparingly in benzene, xylene, &c. The solutionsin sulphuric acid and in caustic alkali are violet and emerald colouredrespectively. The tetracety 1-derivative crystallises in yellow micro-scopic needles, which melt with decomposition at 207-2U9". Thesecond tetrahydroxpnthraquinonc is extracted by means of dilutealcohol from the residue undissolved by benzene. It crystallises insmall, red needles which do not melt at 380" ; it sublimes in small,yeilow needles, but is mostly decomposed.It dissolves readily iORGANIC CHXMISTRT. 57alcohol, glacial acetic acid, and acetone, sparingly in ether and ~ a t e r .The solution in sulphuric acid is brownish-yellow; that in causticalkali emerald-coloured. The tetracetyl-compound crystallises in lemon-coloured prisms, which are very readily soluble in glacial acetic acid,alcohol, and chloroform ; it melts at 189". N. H. M.Methylanthragallols. By E. L. CAHN (Ber., 19, 2333-2336 ;compare Abstr., 1886, 556).-l-~Methylanthragallol,is prepared by heating orthotoiuic acid (3 parts) with gallic acid(2 parts) for 12 to 15 hours up to 130-135". It crystallises fromalcohol in gold-coloured flakes consisting of microscopic needles. Itsublimes in long, orange-coloured needles, and melts at 297-298"with decomposition.It is readily soluble in hot alcohol and glacialacetic acid, sparingly in benzene ; it also dissolves in hot water, yield-i n g a red solution. The triacety 1-derivative crystallises in sulphur-coloured microscopic plates melting at 208-210", readily soluble inchloroform, acetone, hot alcohol, &c. When methylanthragallol isdistilled with zinc-dust, a hydrocarbon, crystallising in white platesand melting at 197", is formed. When oxidised, it is converted intoa quirione melting at 278-2279".3-~etl~ylanthragallol is prepared in a manner similar to the abovecompound from paratoluylic acid. It melts at 275', and sublimes inorange-coloured needles. It resembles its isomeride.The triacetyl-derivative crystallises in well-formed, lustrous, golden prisms meltingat 203-208' with decomposition.2- Methyl- and 4-methy l-anthragallol are formed simultaneously frommetatoluylic and gallic acids. The separation of the isomerides isdifficult, and is best performed by converting the mixed product intothe acetyl-derivative and recrystallising repeatedly from glacial aceticacid. The one methylanthragallol has a slight golden lustre, andmelts at 31 2-313" ; the other crystallises in small, well-formedprisms melting at 235-5240". The acetyl-derivatives melt at 188-190"and at 217-218" respectively.The four methylanthragallols closely resemble one another andanthragallol. They are readily soluble in alcohol, and dissolve instrong and in dilute alkalis, yielding green and violet solutions respec-tively.The solution in hot ammonia has a fine blue colonr, in sul-phuric acid it is red; the latter changes to green on addition of atrace of nitric acid. The absorption-spectra of the red solutions ofanthragallol and of the methylanthragallols in sulphuric acid arealmost the same. N. H. M.Acid from Santonin : Isophotosantonic Acid. By S. CANNIZ-ZARO and G. FABRIS (Ber., 19, 2260-2265) .-Isophotosantonic acid,C15H3206, is obtained by exposing 1 kilo. of santonin dissolved in 52litres of acetic acid to the action of light for several months ; one-ninthof the acetic acid is then boiled off under diminished pressure, and th58 ABSTRACTS OF CHEMICAL PAPERS.residue filtered from the photosantonic acid which separates on cool-ing.A further quantity of photosantonic acid is precipitated byadding water. The solution is then nearly free from photosantonicacid and still contains almost the whole of the isorneride. It is treatedwith sodium carbonate (which dissolves the photosantonic acid alone)and extracted with ether. It separates from its alcoholic solution inthick, triclinic crystals, rather soluble in ether, and sparingly in water.When heated a t loo", it is converted into the lactone, C,,H,,O*. It isdextrorotatory, [a]= = f 3 24" 17'. Photosantonic acid has nearlythe same specific rotatory power, but is lsevorotatory. Isophotosan-tonic acid dissolves in alkalis and in warm solutions of alkalinecarbonates ; the solutions are orange-red.The barium salt,(C15H,106)2Ra + H,O, is an amorphous powder, readily soluble i nalcohol and in water. The monacetyl-compoimd crystallises fromalcohol in transparent needles which melt a t 183" ; it is dextrorotatory,[ a ] D = + 58" 16'. The diacetyl-cowpound is very sparingly soluble ;it melts a t 163-166". It is very unstable, and when often recrys-tallised changes to the monacetyl-derivative.The results ahove described point to the following constitutionalformule for the lactones of isophotosantonic and photosantonic acidsrespectively :-CH : CH*CH-CHMe*C(OH)zCH 1 CH*CH*CHMe*CH*CH<;?>CO I I andCH : CH*CH*CHMe*COOHCH CH* C H*C HMe*CH2*CH < :?> C 0.N. H. M.I ICinchol. By 0. HESSE (Annulen, 234, 375--379).-A furthercomparison of i he properties of cinchol and Liebcrmann's oxyquino-terpene or cliolestole (Abstr., 1885, 1075) confirms the author's pre-viously expressed opinion (Abstr., 1885, 1076) that these twosubstances are identical.They both melt at 115", and are identicalin crystalline form. The acetates melt at 1 2 4 O , and also exhibitidentical crystalline forms. w. c. w.Alkaloids. By 0. DE CONINCK (Contpt. rend., 103, 640-641.)-Piperidine methiodide gives no colour reaction with potassium hydr-oxide (Abstr., 1886, 897), and this difference furnishes a means ofdistinguishing between a pyridic base and its hexhydyide.Cicutine methiodide also gives no colour reaction, but the solutionacquires an amber tint. The reaction is always obtained with colli-dines, and therefore will most probably be given by conyrine, thecollidine of which cicutine is the hexhrdride.No similar colour reaction is obtained with the methiodides ofaniline, orthotoluidine, or metaxylidine.When methiodides of pyridicbases are mixed with a fragment of solid potassium hydroxidORGANIC CHEMISTRT. 59and sn6cient water to form a paste, and then heated, a peculiar odouris developed owing to the formation of pyridic dihydrides.No similar reaction is given by methiodides of pyridic hexhydrides,nor by the methiodides of aniline and its homologues. C. H. 33.Extraction of Pyrroline from Animal Oil. By G. L. CIAMICIANand M. DENNSTEDT (Gazzetfa, 16,356) .-Pyrroline may be extracted asthe potassium-derivative by using caustic potash instead of the metalas heretofore practised.The reaction is probably CIH,NH + KOH =C,H,NK + H,O; the excess of potash serving as a dehydratingagent. The fraction of the oil, freed previously from nitriles, whichpasses over at 125-140", is heated in an oil-bath with an excess offused pofash, using a reflux apparatus. At the conclusion of thercaction, the liquid separates into three layers, the heaviest of whichis the excess of potash, the next the potassium compound, and thelightest the unaltered hydrocarbons. On cooling, the potassium com-pound solidifies, and is washed with anhydrous ether. The substancethus obtained, distilled in a current of steam, yields pyrroline of boil-ing point 130-138' ; with chloroform, it yields chloropyridine(Abstr., 1881, 820).V. H. V.Pyridine Bases. By A. LADENBURG (Compt. rend., 103? 692-695 ; see also Abstr., 1884 and 1885).--a-MetlzyZ~yridine (picoline),C6NH7, is obtained in the form of hydriodide by heating p-j-ridinemethiodide at 300". The base boils at 138-129", and is miscible withalcohol and water ; sp. gr. a t 0' = 0.9656. It forms a characteristicmercuriochloride, C,NH7,HCI,HgC12, by means of which i t can beisolated in a state of purity; this compound is very soluble in hutwater, but only slightly soluble in cold water. p-MethyZpyridine isbest prepared by Zanoni's method of heating glycerol and acetamidewith phosphoric anhydride. I t boils a t 142" ; sp. gr. at 0" = 0.9771.The platinochloride crystallises with 1 mol.H,O and melts at 214" ;the aurochloride is anhydi-ous and melts a t 183" ; the mercuriochlorideis also anhydrous, melts a t 143", and forms slender needles which canbe crystallised from water. .y-iWethy@yridi?~e is formed only in smallquantity by the action of heat on pyridine mdhiodide; it boils a t144-145" ; sp. gr. at 0" = 0.9708. The platinochloride is anhydrous,melts a t 225", and is only slightly soluble in water. aa'-Dimethyl-pyridiite is isolated from the fraction of animal oil boiling a t 138-145" by means of the mercuriochloride, C7NH9,HCI,HgCl2, which canhe crystallised from water, and melts a t 183". When decomposed, ityields lutidine boiling at 142-143"; .sp. gr. at 0" = 0.9924. Theaurochloride forms yellow needles which melt at 124" ; the platino-chloride crptalliees in large monoclinic crystals isomorphous with/3-picoline platinochloride, although the former is anhydrous, whilstthe latter contains 1 mol.H,O. The picrate is only slightly soluble inwater and melts a t 159". When the base is oxidised, it yields a bibasicacid, C5NH3( COOH),, crystallising in beautiful needles which melt a t226", and at the same time decompose into pyridine and carbonicttnbjdride. oc-y-Dimefk$pyridine exists in large quantity in Dippel'60 ABSTkACTS OF CHEMICAL PAPERS,oil, and can be isolated from the fraction which boils at 1S5--160" byacidifying with hydrochloric acid and adding mercuric chloride. Theprecipitated mercuriochloride, 2(C,NHg,HC1,2HgC12) + HzO, is re-peatedly recrystallised, and forms beautiful needles which melt at129'.When decomposed, it, yields the base ; this boils at 157", and isonly slightly soluble in cold water, still less soluble in hot water.The platinochloride is somewhat solnble, crystallises readily, andmelts at 219-220'. The aurochioride, C7HgN,HL4uC11, is less solubleand does not crystallise so well. Thislu tidine is identical with the lutidine prepared synthetically byHantzsch. When oxidised, it yields lutidinic acid, which crystallisesin plates which melt at 235".a-Ethy7pyridine is the principal product of the action of a, hightemperature on pyridine ethiodide ; it boils at 150", is miscible withalcohol, but is only slightly soluble in water. The platinochloride issomewhat soluble in water, and melts at 168-170" ; the aurochloridemelts at 120" and crystallises readily from hot water; the picratemelts at 110".When the base is oxidised, it yields picolinic acid only.y-Ethykym'dine is also formed in smaller quantity by the action of heaton pyridine ethiodide, and is separated from its isomeride by takingadvantage of the comparative insolubility of its salts, especially theplatinochloride or ferrocyanide. The base boils at 163'; sp. gr. at0" = 0.9522. The plstinochloridie melts at 208", the picrate at 163",the aurochloride at 138". The ferrocyanide is precipitated even fromvery dilute solutions. When the base is oxidised, it yields isonico-tinic acid. a-y-DietkyZpyridine is also obtained in small quantity bythe action of heat on pyridine ethiodide ; it boils at 187-188", has a,disagreeable odour, and is only slightly soluble in water.When care-f u l ! ~ oxidised, it yields lutidinic acid which melts at 235".a-lsopropylpyridine, obtained by heating pyridine with propyl orisopropyl iodide at SOO", boils at 158-159", is slightly soluble inwater, and has a very disagreeable odour ; sp. gr. at 0" = 0.9342.The platinochloride, (C8Hl,N),,HZPtCI6, is somewhat soluble andmelts at 168" ; the aurochloride crystallises from dilute solutions inyellow plates which melt at 9l"and are only slightly soluble in water;the picrate forms yellow needles which melt at 116". When the baseis oxidised by potassium permanganate, it yields picolinic acid. y l s o -propyZppidipLe is obtained in smaller quantity by the same reaction,arid is separated by means of the platinochloride, which is only slightlysoluble in water, and melts at 203".The base boils at 177-178";sp. gr. at 0" = 0.9439.The picrate melts at 180".When oxidised, it yields isonicotinic acid.C. H. B.Quinoline. By A. CLAUS and F. COLTJSCHONN (Bey., 19, 2502-2508).-The authors describe a number of halogen additive productsof the propio-haloid compounds of quinoline. Quinoline propio-bromide is easily formed when its constituents are heated alone, orbetter, with alcohol, at 90-100". It is easily soluble in alcohol andwater, and crystallises from water in colourless plates containing2 mols. H,O, and melting at 66" ; from absolute alcohol, it separatesin anhjdrous crystals melting at 148".It is easily soluble in chloro-form, and horn this solutiou crystallises with 1 mol. CHC1, in quadratiORGANIC CHEMISTRY. 61prisms which cradually lose chloroform and become opaque, soften at65", and melt with evolution of chloroform a t 128-129". Quinolinepropiodide forms yellow anhydrous ctptals me1 ting at 145", andbecoming rapidly discoloured in the light. This also crystallises with1 mol. CHCI, in quadratic prisms which begin to evoke chloroform at92". Quinoline propiochloride cannot be easily prepared directlyfrom its constituents, but is best obtained by acting on the corre-sponding bromide with silver chloride. It is very soluble in water,and crystnllises in colourless prisms or plates containing 1 mol.H,Oand melting a t 95". The hygroscopic anhydrous salt melts at 135" ; italso crystallises with 1 mol. CHCI, in quadratic prisms melting a t 79".The additive products were obtained by treating a chloroform solu-tion of the propiohaloid salt with the halogen.Quinoline propiobroinide dibromide, CgNH,*PrBr?, forms glistening,red, triclinic crystals melting at 93". The di-iodide forms brownmetallic needles melting a t 60". The dichloride forms yellow scalesmelting at 60". The tetriodide, CgH,N*PrBrId, yields small, almostblack needles having a green fluorescence and melting at 49".Quinoline propiodide dibromide forms orange triclinic crystals melt-ing a t 77". The di-iodide forms thin, bronze-coloured scaleq meltingat 62".The dichloride forms yellow needles melting a t 87". Thetetrabromide, C9NH7*PrIBr4, is a very unstable orange-red powderwhich evolves bromine a t the ordinary temperature, and gave no con-stant malting point (48-58"). The tetriodide forms iodine-colouredplates melting a t 50'. The tetrachloridp crystallises in needles whichshow the high melting point 1 4 ~ 1 4 . 5 " . It is also formed whenquinoline propiochloride is treated with iodine trichloride, and maytherefore really he quinoline propiochloride iodide trichloride. Whenboiled with water, it is gradually decomposed into quinoline propio-chloride. Similar migmtion of the halogen-atoms may also verylikely take place in others of the mixed halo'id compounds.Qziinoline propiochloride dibromide forms orange crystals melting at84-85'.The &iodide melts a t 61-W. The dichloride is veryunstable and could not be obtained in a pure state. A tetriodideis easily formed, but could not be obtained in a pure state.All these additive compounds decompose when heated a t 250-200",prop91 haloid salts, quinoline haloid salts, and halogenispd andalkglated quinolines being amonget the products of decomposition.These decompositions are being studied. All the above temperaturesare uncorrected. L. T. T.Isoquinoline and its Derivatives. By S . GABRIEL (Ber., 19,2354--2363 ; compare Abstr., 1886, 812) .-Dichlorisopuinoline,CH: CC1C"""&y: N 2,is prepared by heating homo-orthophthalimide (8 grams) with phos-phorus oxychloride (24 grams) for three hours a t 150-170".Theproduct is poured into alcohol ( 5 vols.), the mass of crystals soobtained treated with soda until alkaline, filtered. and recrystallisedfrom alcohol. It is readily soluble i n hot alcohol, cold chloroform62 ABSTRACTS OF CHEMICAL PAPERS.ether, and benzene; it boils at 305-307". The alkaline mother-liquor obtained in the preparation of this compound, when treatedCCl : N >' with hydrochloric acid, yielded the cldoro-derivutive C6H4< CH,*COor C6H4<~CH1_C"0H'> ; this crystallises from boiling alcohol in longneedles melting at 195-197" with evolution of gas. It is rathersoluble in hot alcohol, sparingly in hot benzene and in chloroform ;it dissolves in alcohol, but not in ammonia. The methyl-cornpoun,d,C,H5MeClN0, is obtained by dissolving half a gram of the substancein methylalcohol (10 c.c.), adding methyl iodide (2 grams), and heat-i n g a t 100".It forms slender, white crystals, readily soluble inalcohol, ether, benzene, &c., insoluble in alkali. It melts at 66-67',and has an odour of fruit.Chlorisopuinoline, C6H1< CH CH:N ' '">, - is obtained by reducing thedichloro-compound with phosphorus and hydriodic acid at 150-170", or with tin and hydrochloric acid. It melts at 47-48', andboils at 280-281" under 753 mm. pressure, and is readily soluble.Methoxy pheiilJlclzloriso quinoline, C"H4<C(oMe) : N>, is formedwhen phenyldichlorisoquinoline (1 gram) and sodium methoxide areheated for three hours at 100". I t crystallises from alcohol in needlesmelting a t 76", readily soluble in ether, benzene, &c.It dissolvesalso in strong hydrochloric acid, but is precipitated by water. Whenheated with fuming hydrochloric acid at loo', it is conyerted, withevolution of methyl chloride, into the compound C16H&1N0, probablych!orisobenzuZ phthliinidine, C6HH'<Co.~H->. It crystallises fromalcohol in slender, lustrous needles, melting at 211-212", moderatelysoluble in ether and cold alcohol, readily in glacial acetic acid, ben-ztae, &c. The formation of this compound is analogous to that ofisobenzslphthalimidine from phenylethoxyisoquinoline (Abstr., 1886,631).Ethozychlorisoquiil.oline, CeH4<g$YgCk>, is prepared by heatingdichloroisoquinoline with alcoholic soda at 100".It forms readilysoluble needles melting at 37-37.5".The methoxy-derivative, CloH8XOC1, is prepared in a, similar manner.It melts a t 73-74", and is isomeric with the methyl-compoundobtained from chloroxy quinoline. When heated at 150" in a currentof dry hydrogen chloride, it is converted into oxychlorisoguinoline,C,H4<gt.&!!>. This crystallises from dilute alcohol in slenderneedles melting at 218-220' ; i t dissolves rather readily in ether,easily in alcohol and chloroform ; it is also readily soluble in diluteaqueous soda. The methylderivative, c6H4<gg.&z:>, crydxdlisesin long, broad needles which melt at 111-112" ; it is readily solnble.c)xy chlorisoquinoline is formed in small quantities in the preparationof ethoxychlorisoquinolhe.CC1: CPh -CC1' CPORGANIC CHEMISTRY.63Isoquinoline is conveniently prepared by heating dichlorisoquinoline(3 grams), and hydriodic acid, sp. gr. 1.96 (18 c.c.) for five hours at230". The product is treated with alkali, and steam distilled ; thedistillate being treated with hydrochloric acid and again steam dis-tilled to remove the unchanged chloro-base. Isoquinoline melts at20-22", and boils at 236-236.5". The ethiodide crystallises in gold-coloured plates melting at 147-148", readily soluble in water and inwarm alcohol. N. H. M.Synthesis of Hydroxyquinolinecarboxylic Acid. By E. ,LIPP-MANN and F. FLEISSNER (Ber., 19, 2467-2471) .-Unlike ordinaryphenol-derivatives, the potassium compound of orthohydroxyquinolineis not acted on by carbonic anhydride even at 300".When, however,nascent carbonic anhydride (obtained by the action of potash oncarbon tetrachloride) is employed, action takes place. Orthohydroxy-quinoline, carbou tetrachloride, and caustic potash are mixed in alco-holic solution in the proportions necessary for the equation C9NH7U + CCI, + 6KHO = 4KC1 + C9NH5(OK)*COOK + 4H20, and the~ h o l e boiled for 12 hours. The product contains hydroxyquinoZine-ccirboxylic acid, OH.C,NH,*COOH, which when purified crystallisesin yellow prisms melting at 280". ?'his acid agrees in its salts and inall its properties, save melting point and oxidatiou products, with thea-hydroxycinchonic acid (m. p. 254-256") obtained by Weidel andCobenzl from sulphocinchonic acid (Abstr., 1881, 742). The acid issparingly soluble in the ordinary solvents. It dissolves in dilutehydrochloric acid to form a hydrochloride, which is precipitated on theaddition of concentrated hydrochloric acid in the form of glisteningneedles. The platinochloride forms unstable, bright yellow needles.The acid forms a normal barium salt, the pale yellow solution ofwhich, on the addition of baryta-water, yields white needles of thebask barium salt CloNH,BaO3 + H,O ; these only part with their waterof crystallisation at 140-150". The silver salt is precipitated in theform of pale lemon-yellow flocks, which soon change to microscopicneedles. The aqueous solution of the acid gives a green colorationwith ferric chloride, but none with ferrous sulphate. When subjectedt o dry distillation, the acid yields orthohydroxyquinoline.When oxidised by potassium permanganate in alkaline solution, theacid yields a pyridinedicarboxylic acid, C,NEIQ04, forming brightyellow crystals melting at 234-235". With ferrous sulphate, it give8a blood-red coloration, and forms a silver salt which is gelatinous whenfirst precipitated, but soon becomes crystalline. This acid is probablyidentical with Bottinger's pyridiuedicarboxylic acid, and isomeric withWeidel's isocinchomeronic acid.Weidel and Cobenzl's a-hydroxyvcinchonic acid, when similarlyoxidised, yields a-pyridinetricarboxylic acid. The authors are furtherinvestigating this subject.By 0. FISCHER andH. VAN Loo (Ber., 19, 2471--2476).--This is a continuation of theauthors' previous work (Abstr., 1884, 1372). When P-diquinoline isheated with ethyl iodide in closed tubes at 90-loo", P-diquinolirbeL. T. T.Peculiar Formation of 6-Diquinoline64 ABSTRACTS OF CHEMICAL PAPERS.ethiodide, Cl,N2H12EtI, is formed in long, ruby-red crystals. It is veryunstable, and is decomposed by water and by boiling alcohol. Rodiethiodide could be obtained. When bromine is allowed t o act onP-diqiiinoline in chloroform solution, a tetrabromc-additive product,CI,N2H,,Br4, is produced. This crystallises in pale yellow needlesmelting at 192", and is decomposed at once by sulphurous acid,diquinoline sulphnte being formed. /3- DiquinolinedisuZphonic acid,ClsN2H,,(S03H)2, is produced when P-diquinoline is heated with alarge excess of fuming sulphuric acid. It is very soluble in water,and is precipitated from this solution by a mixture of alcohol andether in yellowish flocks. Its potassium salt crystallises from 50 percent. alcohol in glistening white prisms containing 3 mols. HzO. Theanaquinolinecarboxylic acid described in the former paper (loc. cit.),as obtained by the oxidation of the base by chromic acid in aceticsolution, is undoubtedly identical with that lately obtained by Skraupand Brunner (m. p. 247"). The melting. point previously given bythe authors was obtained from a sample crystallised from benzene ;when crystallised from water, it melts at 248-249". The author con-siders this acid to be metaquinolinecarboxylic acid, and that thename anaquinolinecarboxylic acid should be transferred to the acidmelting at 357O, and hitherto designated metaquinolinecarboxylic acid.If chromic acid is dissolved in sulphuric acid in place of aceticacid, the oxidation takes place in quite a different way. Under thesecircumstances p yridy 7quinolinecarbon: y Zic acid, C,NH,*C,NH,.C OOH,i8 formed. This crystallises in glistening needles, which melt withdecomposition at 271-273". It is sparingly soluble in water, easilyin alcohol, and forms salts both with acids and bases. The silver saIt,when heated, yields a p y r i d y lqzcinohe, C14N2H10, which crystaliises inwhite needles melting at 104", and gives a reddish-yellow crystallineplatinoch lorid e.Piperidine Bases. By A. LADENBURG (Compt. rend., 103, 747-74{9).-The bases are obtained by treating boiling alcoholic solutionsof the corresponding pyridine bases with a large excess of sodium.Piperidine obtained in thh way is identical with the base preparedfrom piperine. a-Methylpiperidine or a-pipecoliqe boils at 118-119",has the same odour as piperidine, and dissolves readily in water;sp. gr. at 0" = 0.860. The hydrochloride is very soluble, but notdeliquescent, and melts at 189". The hydrobromide is less soluble,and forms confused needles which melt at 182" ; the platinochloride isvery soluble. With carbon bisulphide, the base yields a thiocarbamate,CS2,'2C6HI3N, which crystallises readily, melts at 118", and is analogousto that! formed from piperidine. p-Methylpiperidine or P-pipecolineboils at 125", and dissolves readily in water; sp. gr. at 0" = 0.8684.The hydriodidc crystallises in beautiful, non-deliquescent needles,which melt at 131". It combines with cadmium iodide, forming thecompound Cd12,2C6H13NHI, a wbite precipitate soluble in warm water,from which it crystallises in white tables melting at 145". Theplatinochloride is somewhat soluble, and forms orange prisms meltingat 192" ; the aurochloride is very soluble, and melts at 231" ; the picratenielts at 136". aoc'-Dimethy~~peridinR or aa'-lupetidine boils at 128-L. T. TORGANIC CHE_1IISiTlZI'. 6 5130", and is very soluble in water and alcohol ; sp. gr. at 0" = 0.8492,The hydrochloride and hydrobromide crystallise in non-deliquescentneedles ; the platinochloride forms large orange crystals which melta t 212". ay-Dirnethypip~ridz'ne boils at 141", has an odour of piperi-dine, and dir,solves readily in water, though not in all proportions :sp. gr. a t 0" = 0.8615. The hydrochloride crystallises in beautifulneedles which melt a t 235" ; the hydrobromide is even more soluble ;the platinochloride is not very soluble, and crystallises in nodules ;the aurochloride is an oil. a-Ethylpiperidine boils at 143", and dis-solves slightly in water, but separates from the solution on heating,and has an odour resembling that of piperidjne and coniciiie ; sp. gr.a t 0" = 0.8674. The hydrochloride forms non-deliqiiescent crystals ;the platinochloride cryst,aliises in large tablea which melt a t 178".The methyl-derivative boils at 143-152"; sp. gr. at 0" = 0.8495.~,-.E&yZpiperitline boils at 1 -57", has a disagreeable odour, is onlys,lghtly soluble in cold water, and still less soluble in warm water ;sp. gr. a t 0" = 0.8795. The hydrochloride is deliquescent ; the platino-chloride forms yellow tables which meltl at 170-173" ; the auro-chloride crystallises from warm water in lamella which melt a t 105".a- IsopropyZpiperiditLe boils at 160-162", and is slightly soluble inwater, but separates from the solution when gently heated ; sp. gr. a t0" = 0.8676. Its odour and its properties generally resemble those of itsisomeric-le, conicine, but it is much less poisonous. The platinochlorideis much less soluble in water. and is not soluble in alcohol or ether ; i tmelts a t 193" ; the hydrochloride melts a t 240", the hydrobromide a t230", the hydriodide at 24 Lo. All these derivatives crgstallise readily.The iodide combines with cadmium iodide, forming a slightly solubledouble salt, which crystallises readily and melts at 132". The picrateand aurochloride crystaUise readily, and are only slightly soluble.With carbon bisulphide, the base yields a crystalline compound,CS (C,H,,N)SH,C,H1,N, which melts a t 105", dissolves readily inalcohol, but is only slightly soluble i n water. The methrl-dvivativeof or-isopropy~piperidine boils a t 166" ; sp. gr. at 0" = 0 85P3. Itshydrochloride is extremely soluble in water ; the aurochloride formsshining lamellae, and is also very soliihle in water ; the platinochlorideis somewhat soluble, and melts a t 100" ; the picrate crystallises readily,and nielts a t 149". ry-Isop,.opyZpiperi~~//e boils at 168-171", dissolvesslightly in water, and has a very disagreeable odour. The hydro-chloride crystallises, but is not stable in moist air ; the platinochlorideis crystalline, and is only slightly soluble in water, but dissolves inalcohol and ether, arid melts at 172"; the aurochloride is also crgstal-line, and only slightly soluble.Method of Preparing Extracts of Pepsin. By W. PODWYSSOZKI( P J ~ g p r ' . c A T C ~ L ~ U , 39, 62-74). -If the gastric mucous membrane ofcarnivora and herbivora be placed in glycerol almost immediatelyafter death, very little pepsin is extracted.Ebstein and Grutzner state that glycerol dissolves pepsin only, butthe author finds that a certain amonut of pepsin precursor, or as het,c.rmq it " propepsin," is dissolved also.Mucous membrane exhausted with glycerol still yields an importantC. H. B.VOL. 1.11 66 ABSTRACTS OF CHEMICAL PAPERS.amount of pepsin when treated with hydrochloric acid or hydrochloricacid and glycerol. It appears, therefore, that gastric mucous mem-brane contains two propepsins, one soluble in glycerol, the otherinsoluble.I f the mucous membrane is kept in a warm place for 24 hoursbefore it is extracted, a much larger yield of pepsin is obtained,provided no putrefaction has set in.Hydrogen and carbonic anhydride have no influence on the forma-tion of pepsin, but oxygen, on the other hand, appears to favour itsdevelopment ; more pepsin is formed when the mucous membrane isallowed to remain in contact with oxygen than when it is in contactwith air.Chlorine gas passed through any extract entirely destroys theferment. J. P. L.Comparative Estimation of Preparations of Pepsin. By .A.A. LIPSKI (Russlcayrc Medifsiiza, 35,583-584).-The powdered pepsinswere examined by digesting 0.2 gram of the preparation with 10grams of white of egg and 100 C.C. of hydrochloric acid (0.25 percent.) for four hours at 40". The undissolved albumin being thendetermined, the weight of this in grams was :-Perret acidifih 8.756,Marquart 8 577, Lamatch 8.557, Merck 7.213, Boudault neutre (No. 4)2 62, Witte 2.195, Boudault acidifit5 1.2, Russicum solubile (of theRussian Ph.) 0.721, do. do. recent 0.47, do. do. without the sugarcontained in the official preparation 0.157. The Russian pepsin is,therefore, far more active than any of the German or French pre-parations tested. The same holds good for the pepsin wines

ISSN:0368-1769    

DOI:10.1039/CA8875200024

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

66 ABSTRACTS OF CHEMICAL PAPERS. P h y s i o l o g i c a l Chemistry. Sugar in the Blood with Reference to Nutrition. By J. SEEGEN (PJliiger’s Archiu, 39, 121--131).-Experiments on dogs hare shown (Abstr., 1886, 382 and 411) that the percentage of sngar is always approximately twice as great in the blood of the hepatic as in the blood of the portal vein during various carbohydrate diets and during long periods of inanition, also that peptone is probably the chief constituent from which the liver forms sugar under normal conditions. The sugar formed in one day during starvation is far in excess of the total glycogen present in the body. Further experiments have been made on dogs fed with a diet of meat only, of fat with a minimal quantity of meat, and in some instances with fat only.The general result is the same as in previous experiments, namely, that the percentage of sugar in the blood leaving the liver is double that of the blood ou entering. The total amount of sugar in the blood as well as the difference between the percentages in the bloodPBTStOLOGI&iL CHEMISTRY. 67 oh cntering and leaving the liver is greater with a meat diet than arty other. The most striking result is the continued formation of sagar during an almost exclusively fat diet. It might be supposed that this is due to prote’id decomposition, but a determination of the nitrogen excreted during the feeding was quite insufficient to account for the increase. The amount of blood passing through the liver of dogs of 10 to 12 kilos is not less than 200 litres in the 24 hours.The mean difference in thk percentage of sugar of the blood on entering and leaving the liver is 0.1 per cent., consequently about 200 grams of sugar would he foi-med in 24 hours. During the f a t diet, the amount of nitrogen excreted daily was on an average 15 grams, corresponding to 100 grams of prote’id, a quantity quite insufficient to furnish 200 grams of sugar, even supposing that none of the carbon of the proteid be utilised for the formation of urea. The conclusion drawn from these experiments is that the liver has the power of forming sugar from fat. This would satisfactorily explain the constant formation of sugar during starvation, for Voit has shown that an animal during starvation loses 97 per cent. of its fat, and only 30 per cent.of its muscular substance. The chief results of the author’s experiments may be thus summed up :- 1st. The blood of the hepatic vein is without exception richer in sugar tlinn the blood of the portal vein. 2nd. The new formed sugar does not depend on the sugar and carbohydrates ingested with the food. 3rd. The glycogen of the liver is not concerned in the formation of sugar. 4th. Albumin and fat are the materials from which the liver forms sugar. J. P. L. Power of the Liver to Form Sugar from Fat. By J. SEEGEN (P’iiger’s Arcltiv, 39, 132--142).-1t has been previously shown that small pieces of freshly excised liver in the presence of defibriaated blood have the power of converting peptone info sugar (Abstr., 1886, 382). By a similar series of experiments, the author has proved that the liver cells can under the same conditions convert fat into sugar, thus confirming the conclusion he arrived at from his experi- ments on feeding dogs on a diet consisting exclusively of fat (pre- ceding Abstract).For each experiment, 50 grams of finely cut liver excised from a recently killed dog was mixed with 60 to 80 C.C. of freshly defibri- nated blood and placed in a, large flask; to this mixture various emulsions of vegetable oils were added. The flask and contents were maintained for 5 or 6 hours a t 35’ to 40°, and a constant stream of air was drawn through tJhe mixture of blood by means of an aspirator. The average increase in the percentage of sugar was found to be 50 per cent. A further series of experiments proved that both constitpnts of a fat, that is both glycerol and the fatty acid, are alike capable of beiug converted into sugar by the liver.Control experiments we1.e made in every instance. J. P. L. f 268 ABSTRACTS OF CHEMICAL PAPERS. hportance of Ammonia for the Format:on of Glycogen in tle Liver of the Rabbit. By F. ROHMANN (Pjiiger’s Archiv, 39, 21--53).-Aspmagine and glycocine given with a carbohydrate diet inorease the amount of glycogen formed in the liver to a marked extent ; this increase i8 more pronounced with asparagine than with glymcinc. On account of its slight solubility, asparagine is probably not absorbed unchanged, but undergoes decomposition with formation of ammonia. Ammonium carbonate given with the game diet increases the glycogenin a still more maked manner, but ammonia in the form of lactate seems t o be inert.As sodium carbonate and hydrogen carbonate have no effect, ammonium carbonate does not exert its influence by reason of its alkalinity. As a possible explanation, the author suggests that the ammonia arid a carbohydrate entming +he liver cells together may form a new compound which will split into glycogen on the one hand and a nitro- genised product on the other, for instance, urea. Feeding and Development of Silkworms. By 0. KFLLNER (Landw. Versuchs-Stat., 1886, 38€-392).-This article contailis an account of experiments which are a continuation of those previously detitilecl (Abstr., 1884, 1202). The research was commenced with the view of determining whnf quantity of food was necessary for the f u l l and healthy development of the worm, with the largest subsequent supply of silk.Without entering into the details of feeding, &c., all of which are fully given in tables, i t will be sufficient to give the find results. Every increase of growth requires an increase in the food, but this increase in food is not commensurate with the growth, being very much higher ; the weaker the illsect is before envelop- ment, the greater will be the loss during metamorphosis, by respira- tion, &c. A poorly fed and dereloped cakerpillar produces a lower yield of valuable silk than those which are well and largely fed, and will con- tain iiiore nitrogenous and mineral matter, whilst the well-fed in+ect will be richer in fat and other non-nitiaogenous matter.J. P. L. E. W. P. Isethionic Acid in the Body, and Thiosulphuric Acid in the Urine. By E SALKOWSKI (PJliig~r’s Archia, 39, 209--222).-1n a former paper (Virchow’s Archiv, 66, 31.5)’ the author stated that in the dog the admillistration of sodium isethionate produced an in- crease of sulphuric acid in the urine, but tbat thiosulphuric a d was under all circumstances absent. Heffter (P’iiger’s Archiu, 38, 476) states however, that sulphuric acid is not formed from isethionic acid, but that the greater part (78 per cent.) of the latter acid leaves the body as thiosalphuric acid, and a ~meller portion (22 per cent.) in Rome undiscovered manner. Heffter himself explains the discrepancy by supposing it to be due to the differerice in diet during the inyestiga- tion, Heffter using meat, not bread and milk as in Salkowski’s earlier e .periments.The present research is a, rehvestigation of the subject : a dog wauPIIY‘EIOLOGICAL CHEMISTRY. 69 fed on a fixed meat diet, and for three days 3 grams of sodium isethonate was given per diem. The results are shown inithe fullowing table :- Nitrogen Sulphurio wid ray. Diet. in urine. in urine. 1 Meat 12-22 3-20 2 Do. 12.49 3.15 3 Do. 12.49 2.9 7 4 3 gr. of drug added 12-49 3 83 5 Do. 12.23 4.65 6 Do. 12.25 4.99 7 Meat 12.04 3.40 8 Do. 11.63 2.89 9 Do. 11-49 3.16 This table shows that whereas the nitrogen output remains cou- stant, the amount of sulphates is increased ; the increase could there- fore not have been due to increased metabolism of protkds; it is therefore all due to the isethionic acid, and it is found from the foregoing numbers, that 30 per cent.of the isethionic acid must have become oxidised into sulphuric mid. By comparing the intensity of the sulphuretted hydrogen reaction, it was found also that the amount of thiosnlphnric acid in the urine was slightly increased. The amount of this acid in the urine was estimated also by its reducing action on potassium permanganate; the increase during the days when the drug was given, show theoretically that 13.4 per cent, of the sulphur of the isethionic acid pass out of the body in tohe form of thiosulphuric acid, a figure which is shown by control experiments to be too high, as the urine contains other easily oxidisable substances. The question as to what becomes of the re- mainder of thesulphur is not entered into.There seemsalso to be no way of reconciling the present results with those obtained by Heffter. The aromatic sulphonic acids pafis out unchanged in the urine, no thiosulphates being formed; this also is contradictory to the state- ments of Heffter. W. D. H. Trypsin in Urine. By H. LEO (Pjiigw’s Archiv, 39, 246- 264) .-Since the publication of the author’s paper (Abstr., 1886, 381) in which he showed that trypsin did not exist in the urine, Gehrig (P’iiger’s Archiv, 38, 35) states he has found trypsin in the urine ; pieces of fibrin stained with magdala-red, soaked in urine, and trailsferred to 1 per cent. soda solution undergo digestion in a few hours ; this cannot be due to putrefaction as it is so rapid ; it is how- ever prevented by the admixture of t h p o l mlth the digesting mixture; this is explained by saying that thymol hinders pancreatic digestion.The present research is a reinvestigation of the subject, the urine of healthy men and dogs being employed. I t is found that thymol does not hinder pancreatic digestion. A very weak solution of the trpptic ferment was prepared by adding a drop of glycerol extract of pancreas to a litre of water. This excited no digestive action on fibrin. After pieces of fibrin had been soaked in it for70 ABSTRACTS OF CHEMICAL PAPERS. 24 hours, however, and then transferred to a 1 per cent. soda solution they underwent digestion, as they had absorbed the ferment. With the urine, however, no such result ever occurred ; that is, urine, if it contains trypsin at all, contains a less amount than the weak solution of it obtained hy adding.a drop of extract of pancreas to a litre of water.W. I). H66 ABSTRACTS OF CHEMICAL PAPERS.P h y s i o l o g i c a l Chemistry.Sugar in the Blood with Reference to Nutrition. By J.SEEGEN (PJliiger’s Archiu, 39, 121--131).-Experiments on dogs hareshown (Abstr., 1886, 382 and 411) that the percentage of sngar isalways approximately twice as great in the blood of the hepatic as inthe blood of the portal vein during various carbohydrate diets andduring long periods of inanition, also that peptone is probably thechief constituent from which the liver forms sugar under normalconditions. The sugar formed in one day during starvation is far inexcess of the total glycogen present in the body.Further experiments have been made on dogs fed with a diet ofmeat only, of fat with a minimal quantity of meat, and in someinstances with fat only.The general result is the same as in previous experiments, namely,that the percentage of sugar in the blood leaving the liver is doublethat of the blood ou entering.The total amount of sugar in theblood as well as the difference between the percentages in the blooPBTStOLOGI&iL CHEMISTRY. 67oh cntering and leaving the liver is greater with a meat diet than artyother.The most striking result is the continued formation of sagar duringan almost exclusively fat diet. It might be supposed that this is dueto prote’id decomposition, but a determination of the nitrogen excretedduring the feeding was quite insufficient to account for the increase.The amount of blood passing through the liver of dogs of 10 to12 kilos is not less than 200 litres in the 24 hours.The mean differencein thk percentage of sugar of the blood on entering and leaving theliver is 0.1 per cent., consequently about 200 grams of sugar wouldhe foi-med in 24 hours. During the f a t diet, the amount of nitrogenexcreted daily was on an average 15 grams, corresponding to 100grams of prote’id, a quantity quite insufficient to furnish 200 gramsof sugar, even supposing that none of the carbon of the proteid beutilised for the formation of urea.The conclusion drawn from these experiments is that the liver hasthe power of forming sugar from fat.This would satisfactorilyexplain the constant formation of sugar during starvation, for Voithas shown that an animal during starvation loses 97 per cent. of itsfat, and only 30 per cent. of its muscular substance.The chief results of the author’s experiments may be thus summedup :-1st. The blood of the hepatic vein is without exception richer insugar tlinn the blood of the portal vein.2nd. The new formed sugar does not depend on the sugar andcarbohydrates ingested with the food.3rd. The glycogen of the liver is not concerned in the formation ofsugar.4th. Albumin and fat are the materials from which the liverforms sugar. J. P. L.Power of the Liver to Form Sugar from Fat. By J. SEEGEN(P’iiger’s Arcltiv, 39, 132--142).-1t has been previously shown thatsmall pieces of freshly excised liver in the presence of defibriaatedblood have the power of converting peptone info sugar (Abstr.,1886, 382).By a similar series of experiments, the author has provedthat the liver cells can under the same conditions convert fat intosugar, thus confirming the conclusion he arrived at from his experi-ments on feeding dogs on a diet consisting exclusively of fat (pre-ceding Abstract).For each experiment, 50 grams of finely cut liver excised from arecently killed dog was mixed with 60 to 80 C.C. of freshly defibri-nated blood and placed in a, large flask; to this mixture variousemulsions of vegetable oils were added. The flask and contents weremaintained for 5 or 6 hours a t 35’ to 40°, and a constant stream ofair was drawn through tJhe mixture of blood by means of an aspirator.The average increase in the percentage of sugar was found to be50 per cent.A further series of experiments proved that both constitpnts of afat, that is both glycerol and the fatty acid, are alike capable of beiugconverted into sugar by the liver.Control experiments we1.e made in every instance.J.P. L.f 68 ABSTRACTS OF CHEMICAL PAPERS.hportance of Ammonia for the Format:on of Glycogen intle Liver of the Rabbit. By F. ROHMANN (Pjiiger’s Archiv, 39,21--53).-Aspmagine and glycocine given with a carbohydrate dietinorease the amount of glycogen formed in the liver to a markedextent ; this increase i8 more pronounced with asparagine than withglymcinc.On account of its slight solubility, asparagine is probablynot absorbed unchanged, but undergoes decomposition with formationof ammonia.Ammonium carbonate given with the game diet increases theglycogenin a still more maked manner, but ammonia in the formof lactate seems t o be inert.As sodium carbonate and hydrogen carbonate have no effect,ammonium carbonate does not exert its influence by reason of itsalkalinity.As a possible explanation, the author suggests that the ammoniaarid a carbohydrate entming +he liver cells together may form a newcompound which will split into glycogen on the one hand and a nitro-genised product on the other, for instance, urea.Feeding and Development of Silkworms. By 0. KFLLNER(Landw. Versuchs-Stat., 1886, 38€-392).-This article contailis anaccount of experiments which are a continuation of those previouslydetitilecl (Abstr., 1884, 1202).The research was commenced with theview of determining whnf quantity of food was necessary for the f u l land healthy development of the worm, with the largest subsequentsupply of silk. Without entering into the details of feeding, &c., allof which are fully given in tables, i t will be sufficient to give the findresults. Every increase of growth requires an increase in the food,but this increase in food is not commensurate with the growth,being very much higher ; the weaker the illsect is before envelop-ment, the greater will be the loss during metamorphosis, by respira-tion, &c.A poorly fed and dereloped cakerpillar produces a lower yield ofvaluable silk than those which are well and largely fed, and will con-tain iiiore nitrogenous and mineral matter, whilst the well-fed in+ectwill be richer in fat and other non-nitiaogenous matter.J.P. L.E. W. P.Isethionic Acid in the Body, and Thiosulphuric Acid in theUrine. By E SALKOWSKI (PJliig~r’s Archia, 39, 209--222).-1n aformer paper (Virchow’s Archiv, 66, 31.5)’ the author stated thatin the dog the admillistration of sodium isethionate produced an in-crease of sulphuric acid in the urine, but tbat thiosulphuric a d wasunder all circumstances absent. Heffter (P’iiger’s Archiu, 38, 476)states however, that sulphuric acid is not formed from isethionic acid,but that the greater part (78 per cent.) of the latter acid leaves thebody as thiosalphuric acid, and a ~meller portion (22 per cent.) inRome undiscovered manner. Heffter himself explains the discrepancyby supposing it to be due to the differerice in diet during the inyestiga-tion, Heffter using meat, not bread and milk as in Salkowski’s earliere .periments.The present research is a, rehvestigation of the subject : a dog waPIIY‘EIOLOGICAL CHEMISTRY.69fed on a fixed meat diet, and for three days 3 grams of sodiumisethonate was given per diem. The results are shown inithe fullowingtable :-Nitrogen Sulphurio widray. Diet. in urine. in urine.1 Meat 12-22 3-202 Do. 12.49 3.153 Do. 12.49 2.9 74 3 gr. of drug added 12-49 3 835 Do. 12.23 4.656 Do. 12.25 4.997 Meat 12.04 3.408 Do.11.63 2.899 Do. 11-49 3.16This table shows that whereas the nitrogen output remains cou-stant, the amount of sulphates is increased ; the increase could there-fore not have been due to increased metabolism of protkds; itis therefore all due to the isethionic acid, and it is found fromthe foregoing numbers, that 30 per cent. of the isethionic acidmust have become oxidised into sulphuric mid. By comparingthe intensity of the sulphuretted hydrogen reaction, it was foundalso that the amount of thiosnlphnric acid in the urine was slightlyincreased. The amount of this acid in the urine was estimated alsoby its reducing action on potassium permanganate; the increaseduring the days when the drug was given, show theoretically that13.4 per cent, of the sulphur of the isethionic acid pass out of thebody in tohe form of thiosulphuric acid, a figure which is shown bycontrol experiments to be too high, as the urine contains other easilyoxidisable substances.The question as to what becomes of the re-mainder of thesulphur is not entered into. There seemsalso to be noway of reconciling the present results with those obtained by Heffter.The aromatic sulphonic acids pafis out unchanged in the urine, nothiosulphates being formed; this also is contradictory to the state-ments of Heffter. W. D. H.Trypsin in Urine. By H. LEO (Pjiigw’s Archiv, 39, 246-264) .-Since the publication of the author’s paper (Abstr., 1886,381) in which he showed that trypsin did not exist in the urine,Gehrig (P’iiger’s Archiv, 38, 35) states he has found trypsin in theurine ; pieces of fibrin stained with magdala-red, soaked in urine, andtrailsferred to 1 per cent. soda solution undergo digestion in a fewhours ; this cannot be due to putrefaction as it is so rapid ; it is how-ever prevented by the admixture of t h p o l mlth the digestingmixture; this is explained by saying that thymol hinders pancreaticdigestion. The present research is a reinvestigation of the subject,the urine of healthy men and dogs being employed. I t is found thatthymol does not hinder pancreatic digestion. A very weak solutionof the trpptic ferment was prepared by adding a drop of glycerolextract of pancreas to a litre of water. This excited no digestiveaction on fibrin. After pieces of fibrin had been soaked in it fo70 ABSTRACTS OF CHEMICAL PAPERS.24 hours, however, and then transferred to a 1 per cent. soda solutionthey underwent digestion, as they had absorbed the ferment. Withthe urine, however, no such result ever occurred ; that is, urine, if itcontains trypsin at all, contains a less amount than the weak solutionof it obtained hy adding.a drop of extract of pancreas to a litre ofwater. W. I).

ISSN:0368-1769    

DOI:10.1039/CA8875200066

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

70 ABSTRACTS OF CHEMICAL PAPERS. Chemistry of Vegetable Physiology and Agriculture. The Bacillus of Panary Xermentation. By E. LAURENT (Bied. Csntr., 1886, 648).-The author says that the surface of wheat, rye, and other food grains contains spores of bacilli which in grinding pass into the flour, asd when made into dough they germinate, evolve carbonic anhydride, and raise the bread. When cultivated on gelatin, it develops charactepistic cultures different from other bacilli, and has been given the name of Bacillus pwajicnns; it exists with or without oxygen, and renders albumin and gluten soluble; it also grows in saccharose and in a weak solution of boiled starch ; it withstands the heat of boiling water, if at a depth of 7 or 8 mm. in the bread ; it is abundant in bread which has been eaten, and is found freely in the faeces.It can attack starch after baking, if the medium is not Bufficiently acid, and causes a disease in bread which the author ha8 often observed, arid calls viscid or clammy bread ; the addition of a sufficient quantity of an organic acid prevents this. J. 3’. Decomposition of Silicic Acid by Leaves. By A. DENARO (Gazzetta, 16, 328--350).-A few years ago Grimaldi stated in a pamphlet that silica is decomposed by leaves exposed to sunlight, precisely as carbonic anhydride is, into the element and oxygen. It is probable, however, that sufficient care was not taken to exclude carbonic anhydride derived from the potassium carbonate, as an iin- purity in the silica. Accordingly the author has repeated the experi- ments with a sample of silicic acid obtained from a sodium silicate produced by the direct fusion of sodium oxide with silica.Compara- tive experiments were made with leaves of which some were pre- viously deprived of air, whilst others were introduced directly into the solution of silicic acid. In the former case, no oxygen was evolved, In the latter only a small quantity. Further, it is shown that no silica is absorbed by the leaves ; the proportion of silica in them was found to be the same, whether or not they had been treated by the silicic acid solution. V. H. V. Formation of Albuminoids in Plmts. By C. 0. M~LLER (Landw. Versuchs-Stat., 1886, 326--335).--From the experiment8 which have been made on many plants, it would appear that under normal conditions, planta contain asparagine, and this amide appearsVEGETABLE PHYSIOLOGY AND XQRIOULTURE. il if the growing parts are placed in darkness ; but in fully grown por- tions, asparagine is only exceptionally found, and then only in traces.If a portion of a plant is placed in darkness, by enveloping it in black paper, whereby it still remains connected with the parent, and the older portions are left undisturbed, then an accumulation of asparagine is formed, which when the light is admitted, is absorbed ; This does not occur in the fully grown parts, save exceptionally. This result seems to show that the formation of asparagine is inde- pendent of carbohydrates, and also that the amide formed is not it bye-product of the interchange of matter within the plant. It has also been found that even when a plant is growing under abnormal conditions, when all carbonic anhydride has been removed from the air, asparagine is formed in the young parts, but not in the matured por- tions.Consequently it appears as if light played as inconspicuous a part in the formation of asparagine as carbohydrates. The author considers that asparagine i s formed by the union of inorganic nitrogen compounds and malic acid within the plant, the acid being derived By U. KREUSLER (Bied. Centr., 1886,618-664). -The author has examined potatoes at different stages of their growth. At the time of sowing, large and small tubers were of the same specific gravity and composition ; taken up shortly after the sowing, there was but little change observable, there was more moisture, due to partial exhaustion of their substance.Glucose was not found before planting, but was present in the ger- minating tubers ; nitrogenous combinations diminished considerably in the growing roots. The young tubers gradually developed dry matter, principally starch, in proportion as they grew. Glucose was present at the beginning, but gradually decreased as they ripened, when it disappeared. Sub- stances which reduced copper were absent from the very young plants, but appeared at a later stage to disappear when fullyripe; the amount of carbohydrates in the sap was twice as much in the young as in the ripe tubers. In the stalks and leaves, cellulose and non-nitrogenous extract increased, raw prote’in and fat decreased ; the fruit is tolerably rich in fat ; the whole young foliage of the potato belongs to those vegetables which are richest in nitrogen, the proportion of the dry substance amounting to 7-5 per cent.= 47 per cent. crude protein ; the amount of nitrates in the non-protein portions is also very considerable, in the whole plant 3.5 per cent., in the stalks 5 per cent., calculated as N,06. This large quantity of nitrates leads the author to agree with And&, Berthelot, and Schulze, that it is not altogether supplied from external sources, but that a part is formed in the plant itself. from the carbohydrates. E. w. P. Observations on the Growth of Potatoes. J. F. Ammonia in Beetroots. By L. RATTUT (Bied. Centr., 1886, 604 --607).-The opinions of persons who interest themselves in this matter are divided, some asserting the presence of ammonia in the roots, others the contrary.Owing to the rapid decomposition of the organic constituents of beet-juice when heated with alkalis, the deter-72 ABSTRACTS OF CHEMICAL PAPERS. minations were made in the cold by Schlosing's method-in each of four dishes 100 C.C. of distilled water mas poured, in one normal beet- juice with 10 C.C. milk of lime, in two others milk of lime with two kinds of ammonium salts, the fourth milk of lime only-the dishes covered with glass plates to which were fixed moistened test-papers ; the three gave an immediate alkaline reaction. Attempts a t quanti- tative estimations were made witahout much success, but the author concludes from their results that an ammoniacal salt exists in the roots which is readily decomposed by caustic magnesia, and that there are two nitrogenous organic substances present, one, probably asparagirie, quickly decomposed by lime, the other by caustic potash solution.Milky Juice of Certain Euphorbiaceae. By G. HENKE (Arch. Pharm. [ 31, 24, 729--759).-Hitherto euphorbone had not been obtained in a pure state, even Fliickiger, who proposed the name, was unsuccessful. The author treated finely powdered euphorbium in the cold with light petroleum of 60-70" boiling point ; this treatment being repeated as long as anything was dissolved. The solutions obtained were mixed, filtered, and allowed to evaporate spontaneously. The sides of the evaporating vessel became coated with beautiful, tmnsparent, crystalline needles of euphorbone, whilst the remaiader of the residue consisted of a yellowish, crystalline, warty mass, Repeated treatment with light petroleum gives a pure product finally, but is wasteful ; it is better to dissolve the yellow mass in ether after remov- ing the petroleum by heating on the water-bath ; on adding alcohol until a faint turbidity appears, filtering and allowing to remain, a yellow, resinous mass separates.The liquid on evaporation leaves a snow-white, bntter-like mass which gives brilliant needles on crystal- lising from a sufficiently dilute solution of. light petroleum. Eccphorbone thus prepared melts a t 67-68", its composition was found to be GH,,O. Its rotatory power dissolved in chloroform was [a]= = + 15%". Its crystals are persistent in the air, tasteless, Hnd are neutral in solution.It is very soluble in light petroleum, chloroform, ether, alcohol, benzene, acetone, and 90" vol. per cent. alcohol, less soluble in more dilute alcohol. It is unaffected by dilute acids, sodium carbonate, ammonia, potash, and soda, and by alcoholic zinc chloride solution. It is soluble in 10,000 parts of hot water. Cold anhydrous acetic acid does not affect it ; when heated a t 150-200" a solutiori is obtained from which a yellowish precipitate is thrown down on diluting with much water, this precipitate has the properties of unchanged euphorbone. Bromine acts violently on the compound, producing a yellow, resin-like, non-crystallisable mass. Hot nitric acid -'_issolves euphorbone, and from the solution an amorphous, nitroge- nous compound can be obtained.A granular oxidation product was obtained by long boiliitg with potassium dichromate and sulphuric acid. On heating euphorbone with phosphoric anhydride, heptane, octane, xylene and small quantities of other aromatic hydrocarbons were obtained. The residue from the preparation of euphorbone, when extracted with alcohol, yielded two resins, one soluble and the other insoluble in ether; their reactions are detailed. The detection of malic acid, gum, and other substances in the residue and the extrac- J. F.VEGETABLE PHYSIOLOGY ASD AGRICULTURE. 73 tion therefrom are described. The pure euphorborium was found to contain :-Euphorbone, 34.60 ; resin soluble in ether, 26.95 ; resin insoluble i n ether, 14.25; caoutchene, 1.10; malic acid, 1.50; gum and salts precipitated by alcohol, 8.10 ; gum and salts not precipitated by alcohol, 12.30 ; salts and organic substances soluble in ammonia, 1.20 per cent.Somewhat similar results were obtained in the case of juices of other plants of the euphorbia class. J. T. Composition of Barley and Pease. By KLIEN (Ried. C'enfr., 1886, 644-645) .-The author's experiments show that in soils con- taining but little lime, large quantities of superphosphate diminish the protei'ds contained in the grain, whilst soils rich in lime bear very heavy manuring with those substances without damage to the ciop ; precipitated phosphate, a neutral combination of phosphoric acid, was applied in considerable excess without reducing the protei'ds ; evc n in a soil composed of phosphorite containing 20 per cent.of phosphoric acid, the protejid was not lower in the case of pease than in norinally manured soils. Wagner has found that an increase in prote'id by heavy manuring with phosphates can only be obtained in straw and green crops, not in grain and seeds, the percentage being diminished in the latter by large applications of phosphatic manures ; the author thinks Wagner's conclusions are true only when the soil is poor in lime and has traces of mineral acids present, in such cases he recom- mends the application of neutral, that is, precipitated phosphate. J. F. Composition of Tea-leaves. By 0. KELLNER (Landw. Versuclis- Stat., 1886, 370--380).-The chid interest in this research lies in the fact that it is almost the only case in which an evergreen plant has been systematically examined throughout the year.The leave8 were dried at 60--F30°, and the " total nitrogen " estimated by soda-lime, whilst the albumino'id nitrogen was determined by a modification of Stutzer's process, because the'ine- tannate is only decomposed with difficnlty and a t 100"; also the filtration of the solution is attended with great difficulty. The method employed was to boil 2 grams of the sub- stance with 100 C.C. water, to add 20 C.C. of a 10 per cent. copper sulphate solution, and then to precipitate the copper by a titratetl solution of sodium hydroxide, still leaving a small quantity of copper in solution ; after washing with hot water, the precipitate was washed with 95 per cent. alcohol. The filtrate ran rapidly through the paper and was free from albuminoids, nhich were found t o be rather lower than the original process showed.The total soluble matter was estimated indirectly, in that 3 grams were repeatedly boiled with water, the residue being dried and weighed. Theme was estimated in 5 to 7 grams which were boiled in water, the solution evaporated, and magnesia usta added ; after gently drying, the residue was extracted with ether, and the alkaloid obtained by evaporation. To obtain the tannic acid, which by reason of the presence of pectin could not be filtered in the usual way, the leaves were extracted with alcohol acidified with a few drops of acetic acid, the solution thus obtained evaporated and the residue dissolved in water, and filtered through asbestos: in calculating the results, 63 parts of oxalic acid were takenDate.May 15 . . . . . . . . ,, 30 .. .. .. .. June 15 . . . . . . . . ,, 30 .. .. .. . July 15 ... .. .. .. 30. .. .. .. .. August 15 . . . . . . ,, 30 .. .. .. September 15.. . . ,, 30.. .. October 15 . . . . . . ,, 30.. .. .. November 15 . . . ,, 30 .... Yay 15 .. .. .. .. ,, (old leaves). Water in fresh leal es. 76 *83 75-78 78 -61 70 *85 72 -67 70-54 64.21 67 * 75. 65 *26 64 -20 64 -66 64 -11 59.43 60.97 60 -03 -1 ?P Percentage OE Dry Matter. Crude prote'in. 30 -64 24 -25 22 *83 21 '02 20.06 19-96 19 -05 18 * 58 18 -27 18 '15 17 *91 17 -98 17 -70 17 -14 16 -56 Crude fibre. -- 9 -10 17 *25 17 *38 18.69 19 el6 17 *56 17 -72 17 -95 19 *13 19 -17 18 -66 18 -40 18 *26 18 -34 17 '62 - Ethereal extract.-- 6 -48 6 -42 6 -65 6 '83 7 -00 8 -59 10 -85 12'14 13 -40 14 -16 17 -23 19 '50 20 -38 22-19 14'18 Cellu- lose, BLc. 49 -09 47 *32 48 -26 48 '50 49 *49 49 -43 4'7 -80 46 -35 44 * 35 43 -41 41 *14 39 -05 38 *66 37 -31 46 *50 -. Ash. 4 69 4 -76 4 -88 4 '96 4 -29 4 -46 4 -58 4.98 4-85 5 -11 5 -06 5 -07 5.00 5 -04 5 -14 Th e'ine. --. 2 *85 2 *80 2.77 2 -59 2 -51 2 -30 2 -30 2'22 2 -05 2 -06 1 -83 1 -79 1-30 1 -00 0 *84 Tannin. 8 -53 9 *67 10 '10 10 -25 9 -4Q 10.44. 13 -75 11 -09 11 -32 10 *91 11 *21 11 '27 11 -34 12 *16 11 -11 Soluble in hot water. -- 36 -18 37 -17 36 -12 36 '06 31 "72 33 *77 32 -70 34 -00 30 -01 33 -05 34 -76 36 '80 38 -21 37.91 36 -45 - Total N. 4 -91 3 -88 3 *65 3 '37 3 '21 3 -19 3 *05 2.91 2 *93 2.91 2 -87 2 *88 2 -83 2 *74 2 *67 - Album.N. -- 3 *44 2 *77 2 '73 2 *43 2.31 2 *25 2.28 2.19 2 -27 2 -39 2.45 2 -35 2 -30 2 35 2-43 - The'ine N. -- 0 -81 0 -79 0 -78 0 '73 0 -71 0 -65 0 -65 0 *63 0 *59 0 *58 0 -52 0-51 0 -37 0-28 0 *23 Anlido N. + % 0-66 0.32 0 14 0.21 0 L4 0'21 Q 0-29 z 0.16 + r 0.08 v - b- a M - s c3 0.12 i; 0.02 ? 0.16 0.11 0 -01VEGETABLE PHYSIOLOGY ASD AGRICULTURE . Date . May 15 ............ .. 30 ............ June 15 ............ .. 30 ............ July 15 ............ .. 30 ............ August 15 .......... .. 30 .......... Eleptumber 15 ........ .. 30 ....... October 15 .......... .. 30 .......... November 15 ........ .. 30 ........ May 15 (old leaves) ... In 100 parts of Pure Ash . K20 . -. 49 *06 46 '33 41 '37 37 '09 35 -76 32 -84 31.01 29 *15 23 -72 22-28 20 *97 19.75 18 67 17.31 14 -20 Na20 .1 '07 2 -00 1 *23 1 *59 1.58 0 80 1 *08 1-14 4 -77 2 '06 2.76 2 *72 2.76 2 -02 3 -21 Date . May 15 ............ .. 30 ............ June 15 ............ .. 30 ............ July 15 ............ .. 30 ............ August 15 .......... .. 30 .......... September 16 ........ .. 30 ........ October 15 .......... .. 30 .......... November 15 ........ .. 30 ........ May 15 (old leaves) ... Fe203 . 3 '80 4 -30 6.55 7 -25 8-48 9 -75 12 -14 11 *@A 11 -64 12 *11 11 -83 11 -63 11.37 11 '02 11 -93 p20. . .- 16 *67 15 '63 13 -76 18 -85 12 *41 12 *33 12 -00 11 *71 11-25 11 -52 10 -71 10 *23 10 -70 10 -96 10 *64 CaO . 11 -95 14 -93 17.70 21 -95 22 04 22 '88 23 *24 22 -20 23 *44 27.71 27 *90 28 -75 29-60 30 '37 30 -46 MgO . 8 *69 9 00 11 '72 11 '67 12 *21 12 *91 13 -71 14 -79 14 -74 15 *80 15 *88 17 '19 17 -39 17.99 18 -49 .- 75 Mn.04 .1-64 1-79 1.98 1-30 1*58 1-75 1-21 1'57 1-72 1-63 1.37 1*53 2*06 2-48 2 '82 -- SO, . 3 *75 3 *61 3'21 3 -56 3-37 8 *83 3 -43 3 81 4 -74 4 -03 4 37 4 -01 3.84 4 -02 4 '41 .- Si02 . 2 -34 1 '24 1-60 1 *41 1-62 1'35 1 '02 2 -72 1 *69 2.17 2 -61 2 -44 1 -75 2-70 2 -13 .- c1 . .. 1*04 1'39 1-06 1-18 1-17 1-22 1-14 1'13 1*58 1-35 1.11 1-38 1.09 1-19 1 *32 to be equivalent to 34-23 gallotannic acid; the ;annin in tea being identical with tliat acid . The composition of the leaves is shown in the accornpanying tables . The fluctuation in the percentage of water is less than that observed in leaves of deciduous trees ; the percentage of ash lies between that found in the needles of pines and in ordinary leaves .It will be noticed that the non-albuminoyd nitrogen is almost wholly absent, during the later stages of growth. being found as theine . Connecting this with the fact that albumin bas increased. and that no theine is found in the seeds. the author believes that positive proof is afforded that the alkaloid. like glutamine and asparagine. is a decompositior~ product of albumiu. and is capable of again forming albumin . A8 regards the ash. we have here a regular increase. whilst in deciduous trees is found both diminution and increase . I3 . W . P .76 ABSTRACTS OF CREMICAL PAPERS. China bicolor. By 0. HESSE (Annulen, 231, 380-384) .-The author is of opinion that the small quantities of quinine and other dkaloids which Hodgkin (Phnrm.Jour., 15, 217) found in the bark of China bicolor, are probably due to the presence of a small quantity of the bark of Remijiapsdunculata in the China bicolor bark. Chlorosis in Plants. By J. v. SACHS (Ried. Centr., 1886, 602- 604).-When attacked by this disease, the leaves pale and turn perfectly white ; weak plants succumb quickly. Stronger ones are attacked year after year until their reserve material is exhausted; they then die. Tho touching of a diseased leaf with a dilute solotion of an iron salt often causes the production of chlorophyll and cures the disease. However, from extended observations the author does not think that i t is altogether the absence of iron that causes the disease, as plants growing on the same soil are irregularly attacked, some escaping altogether.His experience leads him to think that the roots or leading vessels suffer some alteration which prevents the minute quantities of iron contained in the sap from reaching the leaves. A too rapid and luxuriant growth favours the disease. I n the winters of certain years, thonsands of trees and shrub3 were heavily pruned; the energy divided betwcen numerous growths was concentrated on a much less number; they grew rapidly and luxuriantly; the first leaves were green, but the later were quite white. Trenches 20 to 30 cm. deep and wide were dug round the diseased trees at a distance of 80 to 100 cm. ; in these trenches ferrons sulphate in lumps was placed, in quantities varying from 1 to 5 kilos., accordiiig to the size of the tree. Water was then freely admitted and the trenches filled up with earth.Within three to six days the smaller bushes comnienced to green, within 14 days no sign of chlorosis was visible, and in the following spring all the growths were normal. An experiment of the author’s has, he considers, an important bearing on vegetable physiology. Certain acacia trees showed symp- toms of chlorosis, in particular the thick branches of a 20 year old tree. The author caused holes to be bored in the main stem, just beneath the bifurcation of the branch with the core of the tree. In these holes he placed corks fitted with funnels, charged afterwards with ferrous sulphate or ferric chloride in dilute solution. I n dry weather the tree absorbed the solutions so readily that the funnels had to be frequently refilled.‘1 he leaves in line of each funnel became quite green in 10 to 14 days, but those not in the line remained white. This the author thiuks a proof that each branch and twig has its own sap-ducts. J. F. Ey 0. KELLNER (Landw. Versuclis-Stat., 1886, 349-358).-After a detailed description of the modification of Pillitz’s method, which was employed to eqtimate the absurption of various solutions by soils, the author shows that the absorption of bases by the soils he employed is but slightly dependent on the composition of those soils ; that soils rich in zeolites and humus have not of necessity a higher absorptive capacity ; nor does absor- w. c. w. Absorption by Soils.VEGETABLE PHYSIOLOGY AND AGRlCULTUWE. 77 tion wholly depend on the quantity of the absorbing medium, but largely on the character of the surfaces with which the absorbable substances come in contact.It would appear also, that potash and ammonia are absorbed according to the ratio of their equivalents. E. W. Y. Estimation of Absorbed Bases in Soils, &c. By 0. K E r m E R (Lnndw. Versuchs-Stat., 1886, 359-369) .--From the analytical details given, it is concluded that the potash held in a soil by absorption only may be rezdily estimated by digestion of the soil in a concentrated solution of ammonium chloride. As regards the estimation of lime, the author has failed, as the soils he employed would not retain added lime. He attempted to saturate with calcium chloride aud then remove with ammonium chloride, but found more lime present i n the solu- tion than should have been, showing that other forms of lime (carbo- nate) had been attacked.I n a second series of experiments, he found that peas, when growing, only assimilated the potash and lime held in solution in the soil, and that the insoluble compounds (anhydrous silicates, &c.) were in no wise taken up by the roots. Chili Saltpetre as Manure. By A. STUTZER (Bied. Centr., 1886, 585-597).-The author was awarded the first prize offcred by the union of nitrate firms on the weAern coasts of South dnierica, for his essay on the value of Chili saltpetre as a manure. Wagner has condensed the contents of this essay and that of Damseaux, which obtained the second prize, into a compact form of questions and answers, which are of valce in agricultural science. Some of the answers follow :--Plants cannot grow under normal cocditions unless ,z supply of nitrogen is available for their roots, and a satisfactory crop cannot be obtained without the use of nitrogenous manures.Stable manure, in the quantities produced on a farm, does not provide sufficient nitrogen to produce good results ; high farming requires that nitrogen be procured as artificial manure. Manures contaiiiing nitrogen in the form of animal matter take a long time to alter into nitrates, whilst the Chili saltpetre is a t once available. The increase in weight of various crops tried was greater when the saltpetre was used than when ammonium sulphate was the manure. The application of phosphates and potassium salts increase materially the activity of the saltpetre. This manure does not unduly exhaust the soil ; it renders the mineral plant foods more assimilable, but no more of theni is removed than is accounted for in the increase of the crop.The crops which are most benefited by Chili saltpetre are all straw-growing plants ; next rape, mustard, &c. ; fodder, sugar- beets and potatoes come in the second rank ; meadow gras:,es in the third ; the least effect is produced 011 pease, vetches, lupines, clover, and liiiseed. Chili saltpetze should be applied as top-dressing only on sandy or porous soils, just before vegetation begins; the time of application should be in early spring. Comparative Manurial Values of Chili Saltpetre and Ammo- nium Sulphate. By v. MAGERSTEIN (Bied. Centr., 1886, 583-585).E. W. P. J. E'.78 ABSTRACTS OF CHEMICAL PAPERS. -The experiments were made on a sandy soil, with barley and oats. ZOO kilos. of Chili saltpehre and 300 kilos. of ammonium sulphate were used to the hectare ; the plots manured with the former salt showed a better result in grain, but a smaller yield of straw. Compared with unmanured plots, the increase obtained by manuring was- Barley. Oats. Chili saltpetre . * . . . . . . Ammonium sulphate.. . . 5.46 ,, 6.94 ,, Calculating the cost of the manures and the market prices of barley, oats, and straw, the author considers the Chili saltpetre the more paying of the two. Experiments with Chili Saltpetre. By v. MAGERSTEIN (Biecl. Centr., 1886, 581--583).-1n order to compare the effects of this manure when used as top-dressing and when dug in, the author pre- pared plots of 7 to 8 square metres all cultivated in the same way, except as regards the application of the manure.I n the cases of potatoes and oats, the top-dressing gave the better results, but the contrary was the case with barley: the difference is attributed to the dryness of tho season. The solution of the salt was slow and conceii- trated ; t.lierefore unfavourable to growth. The roots of barley came first i n contact with it, whilst the deeper roots of potatoes and oats received a more dilute solution and were stronger when it reached them. J. I?. 8.13 hcct. grain. 10.25 hect. grain. J. F.70 ABSTRACTS OF CHEMICAL PAPERS.Chemistry of Vegetable Physiology and Agriculture.The Bacillus of Panary Xermentation.By E. LAURENT (Bied.Csntr., 1886, 648).-The author says that the surface of wheat, rye,and other food grains contains spores of bacilli which in grindingpass into the flour, asd when made into dough they germinate, evolvecarbonic anhydride, and raise the bread. When cultivated on gelatin,it develops charactepistic cultures different from other bacilli, and hasbeen given the name of Bacillus pwajicnns; it exists with or withoutoxygen, and renders albumin and gluten soluble; it also grows insaccharose and in a weak solution of boiled starch ; it withstands theheat of boiling water, if at a depth of 7 or 8 mm. in the bread ; it isabundant in bread which has been eaten, and is found freely in the faeces.It can attack starch after baking, if the medium is not Bufficiently acid,and causes a disease in bread which the author ha8 often observed, aridcalls viscid or clammy bread ; the addition of a sufficient quantity ofan organic acid prevents this.J. 3’.Decomposition of Silicic Acid by Leaves. By A. DENARO(Gazzetta, 16, 328--350).-A few years ago Grimaldi stated in apamphlet that silica is decomposed by leaves exposed to sunlight,precisely as carbonic anhydride is, into the element and oxygen. Itis probable, however, that sufficient care was not taken to excludecarbonic anhydride derived from the potassium carbonate, as an iin-purity in the silica. Accordingly the author has repeated the experi-ments with a sample of silicic acid obtained from a sodium silicateproduced by the direct fusion of sodium oxide with silica.Compara-tive experiments were made with leaves of which some were pre-viously deprived of air, whilst others were introduced directly intothe solution of silicic acid. In the former case, no oxygen was evolved,In the latter only a small quantity. Further, it is shown that no silicais absorbed by the leaves ; the proportion of silica in them was foundto be the same, whether or not they had been treated by the silicicacid solution. V. H. V.Formation of Albuminoids in Plmts. By C. 0. M~LLER(Landw. Versuchs-Stat., 1886, 326--335).--From the experiment8which have been made on many plants, it would appear that undernormal conditions, planta contain asparagine, and this amide appearVEGETABLE PHYSIOLOGY AND XQRIOULTURE.ilif the growing parts are placed in darkness ; but in fully grown por-tions, asparagine is only exceptionally found, and then only in traces.If a portion of a plant is placed in darkness, by enveloping it inblack paper, whereby it still remains connected with the parent, andthe older portions are left undisturbed, then an accumulation ofasparagine is formed, which when the light is admitted, is absorbed ;This does not occur in the fully grown parts, save exceptionally.This result seems to show that the formation of asparagine is inde-pendent of carbohydrates, and also that the amide formed is not itbye-product of the interchange of matter within the plant. It hasalso been found that even when a plant is growing under abnormalconditions, when all carbonic anhydride has been removed from the air,asparagine is formed in the young parts, but not in the matured por-tions. Consequently it appears as if light played as inconspicuousa part in the formation of asparagine as carbohydrates.The authorconsiders that asparagine i s formed by the union of inorganic nitrogencompounds and malic acid within the plant, the acid being derivedBy U. KREUSLER(Bied. Centr., 1886,618-664). -The author has examined potatoes atdifferent stages of their growth. At the time of sowing, large andsmall tubers were of the same specific gravity and composition ; takenup shortly after the sowing, there was but little change observable,there was more moisture, due to partial exhaustion of their substance.Glucose was not found before planting, but was present in the ger-minating tubers ; nitrogenous combinations diminished considerablyin the growing roots.The young tubers gradually developed dry matter, principally starch,in proportion as they grew.Glucose was present at the beginning,but gradually decreased as they ripened, when it disappeared. Sub-stances which reduced copper were absent from the very young plants,but appeared at a later stage to disappear when fullyripe; the amountof carbohydrates in the sap was twice as much in the young as in theripe tubers.In the stalks and leaves, cellulose and non-nitrogenous extractincreased, raw prote’in and fat decreased ; the fruit is tolerably rich infat ; the whole young foliage of the potato belongs to those vegetableswhich are richest in nitrogen, the proportion of the dry substanceamounting to 7-5 per cent.= 47 per cent. crude protein ; the amount ofnitrates in the non-protein portions is also very considerable, in thewhole plant 3.5 per cent., in the stalks 5 per cent., calculated as N,06.This large quantity of nitrates leads the author to agree with And&,Berthelot, and Schulze, that it is not altogether supplied from externalsources, but that a part is formed in the plant itself.from the carbohydrates. E. w. P.Observations on the Growth of Potatoes.J. F.Ammonia in Beetroots. By L. RATTUT (Bied. Centr., 1886, 604--607).-The opinions of persons who interest themselves in thismatter are divided, some asserting the presence of ammonia in theroots, others the contrary.Owing to the rapid decomposition of theorganic constituents of beet-juice when heated with alkalis, the deter72 ABSTRACTS OF CHEMICAL PAPERS.minations were made in the cold by Schlosing's method-in each offour dishes 100 C.C. of distilled water mas poured, in one normal beet-juice with 10 C.C. milk of lime, in two others milk of lime with twokinds of ammonium salts, the fourth milk of lime only-the dishescovered with glass plates to which were fixed moistened test-papers ;the three gave an immediate alkaline reaction. Attempts a t quanti-tative estimations were made witahout much success, but the authorconcludes from their results that an ammoniacal salt exists in the rootswhich is readily decomposed by caustic magnesia, and that there aretwo nitrogenous organic substances present, one, probably asparagirie,quickly decomposed by lime, the other by caustic potash solution.Milky Juice of Certain Euphorbiaceae.By G. HENKE (Arch.Pharm. [ 31, 24, 729--759).-Hitherto euphorbone had not beenobtained in a pure state, even Fliickiger, who proposed the name, wasunsuccessful. The author treated finely powdered euphorbium in thecold with light petroleum of 60-70" boiling point ; this treatmentbeing repeated as long as anything was dissolved. The solutionsobtained were mixed, filtered, and allowed to evaporate spontaneously.The sides of the evaporating vessel became coated with beautiful,tmnsparent, crystalline needles of euphorbone, whilst the remaiader ofthe residue consisted of a yellowish, crystalline, warty mass, Repeatedtreatment with light petroleum gives a pure product finally, but iswasteful ; it is better to dissolve the yellow mass in ether after remov-ing the petroleum by heating on the water-bath ; on adding alcoholuntil a faint turbidity appears, filtering and allowing to remain, ayellow, resinous mass separates. The liquid on evaporation leaves asnow-white, bntter-like mass which gives brilliant needles on crystal-lising from a sufficiently dilute solution of.light petroleum. Eccphorbonethus prepared melts a t 67-68", its composition was found to beGH,,O. Its rotatory power dissolved in chloroform was [a]= = + 15%". Its crystals are persistent in the air, tasteless, Hnd areneutral in solution.It is very soluble in light petroleum, chloroform,ether, alcohol, benzene, acetone, and 90" vol. per cent. alcohol, lesssoluble in more dilute alcohol. It is unaffected by dilute acids,sodium carbonate, ammonia, potash, and soda, and by alcoholiczinc chloride solution. It is soluble in 10,000 parts of hot water.Cold anhydrous acetic acid does not affect it ; when heated a t 150-200"a solutiori is obtained from which a yellowish precipitate is throwndown on diluting with much water, this precipitate has the propertiesof unchanged euphorbone. Bromine acts violently on the compound,producing a yellow, resin-like, non-crystallisable mass. Hot nitric acid-'_issolves euphorbone, and from the solution an amorphous, nitroge-nous compound can be obtained.A granular oxidation product wasobtained by long boiliitg with potassium dichromate and sulphuricacid. On heating euphorbone with phosphoric anhydride, heptane,octane, xylene and small quantities of other aromatic hydrocarbonswere obtained. The residue from the preparation of euphorbone, whenextracted with alcohol, yielded two resins, one soluble and the otherinsoluble in ether; their reactions are detailed. The detection ofmalic acid, gum, and other substances in the residue and the extrac-J. FVEGETABLE PHYSIOLOGY ASD AGRICULTURE. 73tion therefrom are described. The pure euphorborium was found tocontain :-Euphorbone, 34.60 ; resin soluble in ether, 26.95 ; resininsoluble i n ether, 14.25; caoutchene, 1.10; malic acid, 1.50; gumand salts precipitated by alcohol, 8.10 ; gum and salts not precipitatedby alcohol, 12.30 ; salts and organic substances soluble in ammonia,1.20 per cent. Somewhat similar results were obtained in the case ofjuices of other plants of the euphorbia class.J. T.Composition of Barley and Pease. By KLIEN (Ried. C'enfr.,1886, 644-645) .-The author's experiments show that in soils con-taining but little lime, large quantities of superphosphate diminish theprotei'ds contained in the grain, whilst soils rich in lime bear veryheavy manuring with those substances without damage to the ciop ;precipitated phosphate, a neutral combination of phosphoric acid, wasapplied in considerable excess without reducing the protei'ds ; evc n ina soil composed of phosphorite containing 20 per cent.of phosphoricacid, the protejid was not lower in the case of pease than in norinallymanured soils. Wagner has found that an increase in prote'id byheavy manuring with phosphates can only be obtained in straw andgreen crops, not in grain and seeds, the percentage being diminishedin the latter by large applications of phosphatic manures ; the authorthinks Wagner's conclusions are true only when the soil is poor inlime and has traces of mineral acids present, in such cases he recom-mends the application of neutral, that is, precipitated phosphate.J. F.Composition of Tea-leaves. By 0. KELLNER (Landw. Versuclis-Stat., 1886, 370--380).-The chid interest in this research lies in thefact that it is almost the only case in which an evergreen plant has beensystematically examined throughout the year.The leave8 were driedat 60--F30°, and the " total nitrogen " estimated by soda-lime, whilstthe albumino'id nitrogen was determined by a modification of Stutzer'sprocess, because the'ine- tannate is only decomposed with difficnlty anda t 100"; also the filtration of the solution is attended with greatdifficulty. The method employed was to boil 2 grams of the sub-stance with 100 C.C. water, to add 20 C.C. of a 10 per cent. coppersulphate solution, and then to precipitate the copper by a titratetlsolution of sodium hydroxide, still leaving a small quantity of copperin solution ; after washing with hot water, the precipitate was washedwith 95 per cent.alcohol. The filtrate ran rapidly through the paperand was free from albuminoids, nhich were found t o be rather lowerthan the original process showed. The total soluble matter wasestimated indirectly, in that 3 grams were repeatedly boiled withwater, the residue being dried and weighed. Theme was estimated in5 to 7 grams which were boiled in water, the solution evaporated, andmagnesia usta added ; after gently drying, the residue was extractedwith ether, and the alkaloid obtained by evaporation. To obtain thetannic acid, which by reason of the presence of pectin could not befiltered in the usual way, the leaves were extracted with alcoholacidified with a few drops of acetic acid, the solution thus obtainedevaporated and the residue dissolved in water, and filtered throughasbestos: in calculating the results, 63 parts of oxalic acid were takeDate.May 15 .. . . . . . .,, 30 .. .. .. ..June 15 . . . . . . . .,, 30 .. .. .. .July 15 ... .. .. ..30. .. .. .. ..August 15 . . . . . .,, 30 .. .. ..September 15.. . .,, 30.. ..October 15 . . . . . .,, 30.. .. ..November 15 . . .,, 30 ....Yay 15 .. .. .. ..,,(old leaves).Waterinfreshleal es.76 *8375-7878 -6170 *8572 -6770-5464.2167 * 75.65 *2664 -2064 -6664 -1159.4360.9760 -03Percentage OE DryCrudeprote'in.30 -6424 -2522 *8321 '0220.0619-9619 -0518 * 5818 -2718 '1517 *9117 -9817 -7017 -1416 -56Crudefibre.--9 -1017 *2517 *3818.6919 el617 *5617 -7217 -9519 *1319 -1718 -6618 -4018 *2618 -3417 '62-Etherealextract.--6 -486 -426 -656 '837 -008 -5910 -8512'1413 -4014 -1617 -2319 '5020 -3822-1914'18Cellu-lose, BLc.49 -0947 *3248 -2648 '5049 *4949 -434'7 -8046 -3544 * 3543 -4141 *1439 -0538 *6637 -3146 *50-.Ash.4 694 -764 -884 '964 -294 -464 -584.984-855 -115 -065 -075.005 -045 -14Th e'ine.--.2 *852 *802.772 -592 -512 -302 -302'222 -052 -061 -831 -791-301 -000 *84Tannin.8 -9 *10 '1010 -9 -10.44.13 -11 -11 -10 *11 *11 '11 -12 *11 VEGETABLE PHYSIOLOGY ASD AGRICULTURE .Date .May 15 .............. 30 ............June 15 ............ .. 30 ............July 15 ............ .. 30 ............August 15 .......... .. 30 ..........Eleptumber 15 ........ .. 30 .......October 15 .......... .. 30 ..........November 15 ........ .. 30 ........May 15 (old leaves) ...In 100 parts of Pure Ash .K20 .-.49 *0646 '3341 '3737 '0935 -7632 -8431.0129 *1523 -7222-2820 *9719.7518 6717.3114 -20Na20 .1 '072 -001 *231 *591.580 801 *081-144 -772 '062.762 *722.762 -023 -21Date .May 15 ............ .. 30 ............June 15 ............ .. 30 ............July 15 ............ .. 30 ............August 15 .......... .. 30 ..........September 16 .......... 30 ........October 15 .......... .. 30 ..........November 15 ........ .. 30 ........May 15 (old leaves) ...Fe203 .3 '804 -306.557 -258-489 -7512 -1411 *@A11 -6412 *1111 -8311 -6311.3711 '0211 -93p20. ..-16 *6715 '6313 -7618 -8512 *4112 *3312 -0011 *7111-2511 -5210 -7110 *2310 -7010 -9610 *64CaO .11 -9514 -9317.7021 -9522 0422 '8823 *2422 -2023 *4427.7127 *9028 -7529-6030 '3730 -46MgO .8 *699 0011 '7211 '6712 *2112 *9113 -7114 -7914 -7415 *8015 *8817 '1917 -3917.9918 -49.-75Mn.04 .1-641-791.981-301*581-751-211'571-721-631.371*532*062-482 '82--SO, .3 *753 *613'213 -563-378 *833 -433 814 -744 -034 374 -013.844 -024 '41.-Si02 .2 -341 '241-601 *411-621'351 '022 -721 *692.172 -612 -441 -752-702 -13.-c1 ...1*041'391-061-181-171-221-141'131*581-351.111-381.091-191 *32to be equivalent to 34-23 gallotannic acid; the ;annin in tea beingidentical with tliat acid .The composition of the leaves is shown inthe accornpanying tables .The fluctuation in the percentage of water is less than that observedin leaves of deciduous trees ; the percentage of ash lies between thatfound in the needles of pines and in ordinary leaves . It will benoticed that the non-albuminoyd nitrogen is almost wholly absent,during the later stages of growth. being found as theine .Connectingthis with the fact that albumin bas increased. and that no theine isfound in the seeds. the author believes that positive proof is affordedthat the alkaloid. like glutamine and asparagine. is a decompositior~product of albumiu. and is capable of again forming albumin .A8 regards the ash. we have here a regular increase. whilst indeciduous trees is found both diminution and increase . I3 . W . P 76 ABSTRACTS OF CREMICAL PAPERS.China bicolor. By 0. HESSE (Annulen, 231, 380-384) .-Theauthor is of opinion that the small quantities of quinine and otherdkaloids which Hodgkin (Phnrm. Jour., 15, 217) found in the bark ofChina bicolor, are probably due to the presence of a small quantity ofthe bark of Remijiapsdunculata in the China bicolor bark.Chlorosis in Plants.By J. v. SACHS (Ried. Centr., 1886, 602-604).-When attacked by this disease, the leaves pale and turnperfectly white ; weak plants succumb quickly. Stronger ones areattacked year after year until their reserve material is exhausted;they then die. Tho touching of a diseased leaf with a dilutesolotion of an iron salt often causes the production of chlorophylland cures the disease. However, from extended observations theauthor does not think that i t is altogether the absence of ironthat causes the disease, as plants growing on the same soil areirregularly attacked, some escaping altogether. His experienceleads him to think that the roots or leading vessels suffer somealteration which prevents the minute quantities of iron contained inthe sap from reaching the leaves.A too rapid and luxuriant growthfavours the disease. I n the winters of certain years, thonsands oftrees and shrub3 were heavily pruned; the energy divided betwcennumerous growths was concentrated on a much less number; theygrew rapidly and luxuriantly; the first leaves were green, but thelater were quite white. Trenches 20 to 30 cm. deep and wide weredug round the diseased trees at a distance of 80 to 100 cm. ; in thesetrenches ferrons sulphate in lumps was placed, in quantities varyingfrom 1 to 5 kilos., accordiiig to the size of the tree. Water was thenfreely admitted and the trenches filled up with earth. Within three tosix days the smaller bushes comnienced to green, within 14 daysno sign of chlorosis was visible, and in the following spring all thegrowths were normal.An experiment of the author’s has, he considers, an importantbearing on vegetable physiology.Certain acacia trees showed symp-toms of chlorosis, in particular the thick branches of a 20 year oldtree. The author caused holes to be bored in the main stem, justbeneath the bifurcation of the branch with the core of the tree. Inthese holes he placed corks fitted with funnels, charged afterwardswith ferrous sulphate or ferric chloride in dilute solution. I n dryweather the tree absorbed the solutions so readily that the funnelshad to be frequently refilled. ‘1 he leaves in line of each funnel becamequite green in 10 to 14 days, but those not in the line remained white.This the author thiuks a proof that each branch and twig has its ownsap-ducts.J. F.Ey 0. KELLNER (Landw. Versuclis-Stat.,1886, 349-358).-After a detailed description of the modificationof Pillitz’s method, which was employed to eqtimate the absurptionof various solutions by soils, the author shows that the absorptionof bases by the soils he employed is but slightly dependent onthe composition of those soils ; that soils rich in zeolites and humushave not of necessity a higher absorptive capacity ; nor does absor-w. c. w.Absorption by SoilsVEGETABLE PHYSIOLOGY AND AGRlCULTUWE. 77tion wholly depend on the quantity of the absorbing medium, butlargely on the character of the surfaces with which the absorbablesubstances come in contact.It would appear also, that potashand ammonia are absorbed according to the ratio of their equivalents.E. W. Y.Estimation of Absorbed Bases in Soils, &c. By 0. K E r m E R(Lnndw. Versuchs-Stat., 1886, 359-369) .--From the analytical detailsgiven, it is concluded that the potash held in a soil by absorption onlymay be rezdily estimated by digestion of the soil in a concentratedsolution of ammonium chloride. As regards the estimation of lime,the author has failed, as the soils he employed would not retain addedlime. He attempted to saturate with calcium chloride aud then removewith ammonium chloride, but found more lime present i n the solu-tion than should have been, showing that other forms of lime (carbo-nate) had been attacked. I n a second series of experiments, he foundthat peas, when growing, only assimilated the potash and lime held insolution in the soil, and that the insoluble compounds (anhydroussilicates, &c.) were in no wise taken up by the roots.Chili Saltpetre as Manure.By A. STUTZER (Bied. Centr.,1886, 585-597).-The author was awarded the first prize offcred bythe union of nitrate firms on the weAern coasts of South dnierica, forhis essay on the value of Chili saltpetre as a manure. Wagner hascondensed the contents of this essay and that of Damseaux, whichobtained the second prize, into a compact form of questions andanswers, which are of valce in agricultural science. Some of theanswers follow :--Plants cannot grow under normal cocditions unless,z supply of nitrogen is available for their roots, and a satisfactorycrop cannot be obtained without the use of nitrogenous manures.Stable manure, in the quantities produced on a farm, does not providesufficient nitrogen to produce good results ; high farming requiresthat nitrogen be procured as artificial manure.Manures contaiiiingnitrogen in the form of animal matter take a long time to alter intonitrates, whilst the Chili saltpetre is a t once available.The increase in weight of various crops tried was greater when thesaltpetre was used than when ammonium sulphate was the manure.The application of phosphates and potassium salts increase materiallythe activity of the saltpetre. This manure does not unduly exhaustthe soil ; it renders the mineral plant foods more assimilable, but nomore of theni is removed than is accounted for in the increase ofthe crop. The crops which are most benefited by Chili saltpetre areall straw-growing plants ; next rape, mustard, &c. ; fodder, sugar-beets and potatoes come in the second rank ; meadow gras:,es in thethird ; the least effect is produced 011 pease, vetches, lupines, clover,and liiiseed. Chili saltpetze should be applied as top-dressing only onsandy or porous soils, just before vegetation begins; the time ofapplication should be in early spring.Comparative Manurial Values of Chili Saltpetre and Ammo-nium Sulphate. By v. MAGERSTEIN (Bied. Centr., 1886, 583-585).E. W. P.J. E'78 ABSTRACTS OF CHEMICAL PAPERS.-The experiments were made on a sandy soil, with barley and oats.ZOO kilos. of Chili saltpehre and 300 kilos. of ammonium sulphate wereused to the hectare ; the plots manured with the former salt showed abetter result in grain, but a smaller yield of straw. Compared withunmanured plots, the increase obtained by manuring was-Barley. Oats.Chili saltpetre . * . . . . . .Ammonium sulphate.. . . 5.46 ,, 6.94 ,,Calculating the cost of the manures and the market prices of barley,oats, and straw, the author considers the Chili saltpetre the morepaying of the two.Experiments with Chili Saltpetre. By v. MAGERSTEIN (Biecl.Centr., 1886, 581--583).-1n order to compare the effects of thismanure when used as top-dressing and when dug in, the author pre-pared plots of 7 to 8 square metres all cultivated in the same way,except as regards the application of the manure. I n the cases ofpotatoes and oats, the top-dressing gave the better results, but thecontrary was the case with barley: the difference is attributed to thedryness of tho season. The solution of the salt was slow and conceii-trated ; t.lierefore unfavourable to growth. The roots of barley camefirst i n contact with it, whilst the deeper roots of potatoes and oatsreceived a more dilute solution and were stronger when it reachedthem. J. I?.8.13 hcct. grain. 10.25 hect. grain.J. F

ISSN:0368-1769    

DOI:10.1039/CA8875200070

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

78 ABSTRACTS OF CHEMICAL PAPERS. An a 1 y t i c a 1 C h em i s t ry. Kjeldahl's Method of Estimating Nitrogen. By C. ARNOLD (Arch. Pharrn. [3], 24, 785--794).-The author shows that this method (Abstr., 1884, 364; 1885, 930) is also applicable to nitrates, nitro- and cyanogen-compounds, in the presence of beneoic acid, sugar, mercury, and copper sulphate ; further, in the case of alkaloids and otber compounds that can be treated by this method, oxidation by potassium permanganate is unnecessary if the boiling be continued until the warm liquid acquires a bluish-green tint, becoming colour- less on cooling ; this takes place tolerably quickly in the presence of mercury and copper. That the oxidation has been completed can readily be ascertained by adding a crystal of potassium permanganate, which should give a persistent violet or green coloration. A descrip- tion of tlie apparatus used by the author is given.J. 1'. Separation of Arsenic and Antimony. By ZAMBELLI and LUZZATO ( A ~ c h . Pharm. [ 3 ] , 24, 772).-These elements can be sepa- mted, even in foyensic cases, by treating the still moist sulphides with hydrogen peroxide at 40' for some hours, then heating to near 100"AKALYTICAL CHEMISTRY. 79 and filtering. The arsenic acid formed goes into the filtrate, whilst the insoluble antimony oxide remains on the filter. The method is said to be very delicate. Detection of Thiosulphate in Hydrogen Sodium Carbo- nate. By RRENSTEIN and T. SALZER (Arch. Yharm. [3], 24, 761).- According to Brenstein, the reaction given for thiosulphate by Mylius is not characteristic, as other oxygen-compounds of sulphur, such as sulphites, give rise to the formation of hydrogen sulphide.A bettar test for tJiiosu1phate is to add to a 5 per cent. solution of hydrogen sodium carbonate a few drops of silver nitrate solution, then excess of nitric acid, and heat to boiling; even minute traces of thiosulphate give an immediate dark precipitate of silver sulphide. According to Salzer, the absence of thiosulphate is easily ascer- tained by adding a few drops of iodine solution to about 20 C.C. of a saturated solution of hydrogen sodium carbonate ; the solution must have a yellowish tint. Decolorisation of the iodine solution does not necessarily imply the presence of thiosulphate, since normal carbo- nate, the most commonly occurring impurity, produces this effect.Both authors found thiosulphate to be a constant impurity of ordinary qualities of hydrogen sodium carbonate, whilst the better qualities were mostly free from it. Estimation of Small Quantities of Silver in Burnt Pyrites. By E. Trrrr,o (Cherrz. Zeit., 10, 822; 1065--1067).-The amount of silver in burnt pyrites is ordinarily 0*003--0.008 per cent., and to obtain trustworthy results material containing 0.01 gram of silver should be taken for analysis, or about 300 to 500 prams of pyrites. Many difficulties have been encountered in endeavouring to deal with these large quantities of material so as to get all the silver. Experiments show that the decomposition of the whole mass is out of the question, therefore methods for extracting the silver, &c., were tried ; treat- ment with nitric acid or with gaseous chlorine, and subsequent extraction of the silver chloride proved unsuitable. Digestion with chlorine-water was somewhat better ; but bromine or bromine-water gives the best results.The powdered burnt pyrites is passed through a 0.25-mm. mesh sieve, and about 300-500 grams of it is placed i n an acid-proof iron basin; it is well covered with water, and while vigorously stirred, bromine is added until present in excess. After 24 hours it is heated on a water-bath for one hour with frequent stirring, treated with excess of ammonia, then with 500 grams of ammonium chloride, and 1 litre of water. The mass is boiled for an hour, and filtered. The residue is dried, ignited at a low red heat, and again treated with arnmoniacal ammonium chloride, by which means all the silver is extracted.Inasmuch as copper is quite as difficult as silver to extract by means of bromine, and as theamount of copper i n the pyrites is reduced from 5 per cent. to a trace (0.01 per cent.) by the above treatment, this may be used as an indicator of the progress of the desilvering, and in practice when the copper is reduced to this amount it may be safely inferred that all the silver is removed. The solu- tion, about 4 litres, is made acid with hjdrochloric acid; it is not J. T. J. T.80 ABSTRACTS Ol!’ CHEMICAL PAPERS. affected by daylight either before or after acidifying. The silver, copper, and lead are then precipitated by means of chemically piire zinc.When the precipitation is complete, the solution is colourless (or rose-red if cobalt is present), and is not turned blue bv ammonia. As the precipitate contains, most liksly, silver chloride and bromide, and some iron oxide, it is fused with potassium cpnide, and sub- sequently with anhydrous borax, the temperature being raised to melt the copper, The regulus is dissolved in nitric acid, and the silver either precipitated by means of hydrochloric acid or determined electrolytically. Silver determinations may also be made in ordinary pyrites, which is first roasted carefnllp, and then treated in the above manner. Good results have been obtained by this method, with roasted copper schist, with spathic iron ore containing argentiferous tetrahedrite and pyrites, and with other ores.A determination can be complded iu three days. Comparative Gasometric Assaying with Especial Reference to the Valuation of Zinc Powder and the Testing of Car- bonates. By J. BARNES ( J . SOC. Chem. Ind., 5, 145--147).-1n a, previous communication (Trans., 1881, 462), the author described a method for the valuation of zinc powder, consisting in measuring the amount of hydrogen liberated on treatment with an acid. The author has since devised a method and constructed an apparatus for gasome tric assaying, contrived originally for the valuation of zinc powder, but applicable also to the estimation of other substances, which may be made to cause or control tlie evolution of gases. The method, which is described in detail in the paper, is a comparative one, and requires a t least two graduated instruments, each provided with a suitable gas evolving arrangement. A substance of known value, taken as the standard, is placed in one, and the sample to be examined in the other instrument.The value of the sample is then calculated by the following formula: - . W . R = x ; - whereV equals the volume of gas from standard, v the volume of gas from mmple, W the weight of standard, and ?u the weight of sample. R is the amount of pure substance or its equivalent in unit of standard, and x the amount of pure substance in unit of sample. Determination and Valuation of Copper in Ores and Products for Commercial Purposes, with some Remarks on the Assay of Gold in Bar Copper. By J. TV. WESTMORKLAND ( J . Soc.Chem. Ind., 5, 48--64).-Esfin?ation of Moisture.-This, although apparently a simple process, is conducted very differently by rarious assr,yers, and the author proposes that the temperature and niaiiner in which the moistnre is to be taken should be more clearly defined than it is at the present time. Wet Assay of Coppr.-Having examined a iarge number of samples of all kinds of copper ores aud products by several wet processes, the author has given the iodide process as modified by Brown the preference-being more trustworthy arid accurate than the electrolytio process. For cupreous pyrites, burnt ores, &c., the followiiig mctliod D. A. L. v 20 D. B.ANALYTICAL CEEMISTRY. 81 mny be used. From 50 to 150 grains of the sample is dissolved in acids, evaporated to dryness with excess of sulphuric acid, diluted with water arid filtered, From this solution, the copper is separated with sodium t'hiosulphate, the precipitate dried, ignited, dissolved in nitric acid, evaporated with sulphuric acid to separate Graces of lead, diluted with water and filtered, sodium carbonate added in excess, and then acetic acid to acid reaction. The solution is then titrated with potassium iodide.As 8n alternative method, the ore may be calciued, dissolved in hydrochloric acid, the ferric salt reduced by boiling with a solution of sodium sulphite, and hydrogen sulphide passed through the cold Rolution; the precipitated sulphides are then washed, and the process conducted as before. Richer copper ores, mattes, preci- pitates, &c., are dissolved in acids, and the solution precipitated either with sodium thiosulphate or hydrogen sulphide, the sulpbides being dissolved in acids, and treated 8s before.The accuracy of this process was tested by numerous experiments, in which known weights of pure electrotype copper, silver, arsenic, antimony, lead, cadmium, bismuth, tin, manganese, zinc, and iron salts were used. The solutions were made to represent cnpreons burnt ores, mattes, cupriferous lead regul us, second quality and rich precipitates, &c. Experiments were also made i n many cases with the metals separately. The electro- deposition method may be employed in cases where it is desir,thle to have resultti of two separate and distinct processes, it being noted that with pure solutions of copper, accurate results are obtained, whilst when silver or bismuth are present they are precipitated, and in one experiment tin was also deposited with the copper.In the presenoe of ferric salts, the deposition is retarded. It was found that whilst the results with refined or bar coppers and rich precipitates agree with those obtained by the iodide process, those obtained by electrolgsing sulphuric acid solutions of mattes, copper ores, $c., are generally slightly below the triie percentage. With burntl ores, cupreous pyrites, and ores containing but little COPPOI', the author first precipitates with hydrogen sulphide, dissolving the s u lphide in nitric acid, and evaporating this soliifion with excess of sulphuric acid, the sulphates dissolved in water give a solution from which copper (and bismuth) is readily deposited.The results by the battery process are generally from 0.01 to 0.04 per cent. higher than by the iodide process, this being cniised by a slight deposit of bismuth. The Cornish Yroce.9~ of Dry Assay.-This process is considered to be inaccurate and misleading, and is also liable to aerious variation even in the hands of experienced operators. The author is of opinion that in cases where the sulphur contents of pyrites are sold to alkali works, tbe burnt ores being returned to the vendors, an accurate wet assay forms the best# check on the copper contents of the ore delivered to and received from the alkali works. In the remaining part of the paper, the methods in vogue for fixing the prices payable for copper in pyrites, copper ores.&c., are discussed. Reftmnce is also made to the avsay of goltl in bar coppry, and the opinion is expressed that t>hese assays are not conducted as carefully aa they should be, taking the value of the metal into oonsideration. I). B. 9 VOL LU.82 ABSTRAOTS OF CREMICAL PAPERS. Estimation of Ammoniacal Nitrogen in Soils, and the Amount of Assimilable Nitrogen in Uncultivated Land. Ry A. BAUMAXN (Lmdw. Versuchs-Stat., 1886, 2$7--303).--The methods employed to estimate the ammonia in soils are nnsatisfactor-y. Schlosing’s method, whereby the ammonitt is freed by means of milk of lime or sodium hydroxide, gives results too high, probably owing to the formation of ammonia from other compounds during the period (2-3 days) required for the process. In Bonssingault’s process as modified by Sclilosing, a hydrochloric acid extract of the soil is treated with magnesia usta, but the ammonia collected in acid mu$ not be estimated by titIration, but must be azotometrically determined ; nor must cork nor caoutchouc be employed in the formation of the apparatus, The liquid in the evolution flask must be boiled for at least an hour, and the magnesia usta must be fresh.With these two processes, it is found that humous soils, when treated with sodium hydroxide, continuously yield ammonia ; if the soil, after treatment with magnesia, be further treated with sodium hydroxide, another supply of ammonia is obtained, b u t only in the case of soils rich in numus. Knop’s process, in which the ammonia is decomposed by brominated sodium hydroxide solution, is vitiated by the fact, noticed by Rnop and others, that in the presence of the soil itself a con- traction of the volume of gas enclosed in the apparatus occurs ; this contraction was stated by some to be due to absorption by the organic matter, whilst others considered the oxides of iron in the clay to be the real cause; also it had been stated that the presence of borax prevented this contraction.To ascertain the cause of the con- tract.ion, a sample of stiff soil poor in humus, was taken from uncul- tivated land a t a depth of 15-20 cm.; this sample seemed free from humus, although root-fibres were visible ; at a distance of 40 m. from this spot another sample was drawn from a depth of 2-10 cm., this was close to a pine SO years old.The sample showed humus, and when dry was grey. At another spot, close to a 100 year old pine, a third sample was taken, and this when dry wa8s dark-brown, These last two samples overlaid a soil similar to the first sample, Employing these samples, the author argued that if the contraction was due to the clay and the iron, and not to the humus, then identical contractions would be observed when equal quantities of all samples were subjected to like conditions. On the other hand, if the phe- nomenon is caused by the humus, then that sample richest in humus would produce the greatest effect on the volume of the gas, and when borax was employed no contraction should occur. It appears that the ferruginous soil poor i n humus produced no contraction, but rather an increase of volume after the first 2 hour ; this is explained by the probable presence of nitrogenous matter decomposable by the brominated alkali.The presence of borax assisted the evolution of gas. Experimenting with humous samples, it was found that the volume of gas evolved by Knop’s method stands in no ratio to the percent- age of ammonia present ; this remarkable result was most manifest in the case of the third sample, which contained most humus, for then the contraction was evident when only 5 grams were used,AXALP TlCXL CIIEMISTRY. 83 and in spite of borax the contraction amounted to 71 per cent. when 1UO grams was employed, This contraction is clearly due to oxida- tion of the organic matter of the soil, and consequent removal of part of the gaseous contents of the azotometer.Working with sandy and chalky Hoils, the author found that the results obtained by Knop’s method are quite as untrustworthy as in the case of humous samples. The following method is recommended for the estimation of am- monia in soils:--200 grams of the soil is mixed with 100 C.C. of hydrochloric acid (1 : 4), then diluted with 300 C.C. of distilled water and allowed to remain for two hours, with frequent shaking. Should much chalk be present, then more than 100 C.C. acid must be added, and the whole amount of liquid made up to 400 C.C. ; all heating must be avoided. Of the filtrate, 200 C.C. (= 100 grams soil) is placed in the evolution vessel of the azotometer together with 5 grams of freshly ignited magnesia usta, and the vessel closed by a doubly bored india-rubber stopper ; through one of the borings a glass tube passes to the bottom of the flask, whilst the other opens immediately below the stopper, and is connected with an aspirator, whilst the other tube supplies air ozonised by passing through potassium per- manganate and concentrated sulphuric acid.The passage of this gas for 10 minutes oxidises organic matter, so that no subsequent con- traction occurs, The rest of the process is conducted in the ordinary way. Percentage of Ammonia i n Soils.-Soils of various characters were examined, and the percent’ages as found by Schlosing’s and the other methods are given : there appears to be a, wide difference between the first and the other two methods. The percentages at different periods in summer and at different depths are recorded.The conclusions drawn are that the percentage of ammonia in uncultivated soils varies with the character of the soil, loams containing most, the quantity increasing with the increase of clay; chalks and sands are poor in ammonia, but in sands rich in hurnus there is a large supply of organic compounds which readily decompose and yield ammonia, although generally speaking, the percentage of organic matter is no indication of t$he amount of ammonia present, and the percentage of ammonia in a soil does not seem to vary with the weather, but does decrease with depth from the surface. Percenta>ge of Nitrates i ? ~ Urnnunured Soils.-Baumann employs Schlosing’s method of estimating nitrates if the solution of 1000 grams soil in water made up to 3000 C.C.shows the brucine reaction, even if the reaction is only obtained after evaporating the solution to one-half of its original volume. If this test should fail, then diphenylnniine is to be employed; this should indicate 1 in 1,500,000 or 0.6- 1 mgrm. per litre ; should this fail, so also will Schlosing’s method, and it will be necessary to evaporate 1 litre of extract with some alkali to dryness, add alcohol, boil, filter, and then evaporate the alcohol and dissolve in 40 C.C. water. The solution must be again tested by brucine and diphenylamine, and if indications of the presence of nitrates are visible, the Marx-Trommsdorf’s method (Zeit. anal. C‘lzem., 1868, 412, and 1870,171) is to be employed for the quantitative8 -1 ABSTRACTS OF CHElllICAL PAPERS.estimation ; this will indicate 0*00001 per 300-400 grams soil. Examination of many soils shows that when the soil is uncultivated the percentage of nitrates is very small, especially in forests, where i t only appears as traces. The author then reviews the work of Warington, Scliliisinp, and Miint>z on nitrification, and considers that the absence of nitrates in such soils as he refers to, is due to the normal temperature ( 5 > ) being so close to that a t which nitrification first occurs; also water is necessary for nitrification, and in forest soils, therefore little nitri- fication takes place, because of the great dryness of that soil in summer, due especially to the enormous transpiration continually occurring, which renders the soil almost "air-dry ; " a further cause for the absence of nitrification may be faund in the want of animal Analysis of Gas Coal.By L. T. WRIGHT (J. SOC. Chem. Ind., 4, 656-667) .-Proximate amZysis.-T he first determination is that of moisture. T'arious temperatures have been recommended at which the sample of coal shall be dried. Since ZOO' is a temperature easily Recured and maintained constant by means of a water-bath, the author has adopted it as the standard. The estimation of moisture by loss of weight in drjing a t 100" until the weight of the substance become9 constant is not, however, free from error ; as it has been noticed by different observers, that after a time the coal not only ceases to lose weight but actually gains. Hinrichs attributes this increase to the slow oxidation of pyrites and other substances in the coal ; the author.however, considers it to be due to the absorption of gases into the pores of t h e coals left vacant by the expelled moisture. He has also found that the increase of weight, which only exhibits itself when t h e con1 has been nearly dried, has been going on during the whole period of the drying process, SO that where accuracy is required it is preferable to weigh the water as such. According to Hinrichs the total volatile matter of coal is determined with accuracy by taking 1 to 2 grams of undried pulverised coal, heating for three and a half minutes over a Bunsen burner, and then immediately igniting without cooling, for the same period over a blast gas lamp (white heat).The greatest difference which Hinrichs obtained amounted to 0.29 per cent. The author has reFeated this method and obtained very fair results, although not quite so accurate as the above. The author adopts the following method:-Take about 2 grams of finely pulverised coal and let i t form an even layer on the bottom of a thin platinum crucible. Weigh without cover. place the crucible (with cover on) in an upright position, then apply a powerful gas flame. Note when the gases cease issuing from under the lid; allow one minute further heating, remove the gas flame, place the crncible and cover in a desiccator tor about five minutes to cool, and then weigh without cover as soon as possible. For the determination of ash in refractory cokes and such substances as gas carbon, heat to redness 2 grams of the coal or coke placcd on a piece of platinurnfoil, in R combustion tube through which ft gentle current of air is drawn.The ash should be saved for the determination of sulphuric acid. nutriment for the growth of the ferment. E. w. P.ASALFTIC hL C HENISTRT. 85 k'or the determination of the total sulphur, the best and eimplest method is that suggested by Nakamura, which consists in heating the coal below a red heat in contact with alkaline carbonates, when the coal whether bituminous or not rapidly undergoes complete oxidation. For the purpose of distinction hetween the sulphur which goes over into the volatile matter, the sulphur left in the coke and that which is finally left in the ash combined as sulphate, three determinations are required :-(1) Total sulphur by Nakamura's method.(2) Sulphur which is converted into sulphurous anhydride by combustion of the coke in air, obtained by roasting a quantity of coke representing a known quantity of the coal, and aspirating the gaseous products of combustion through a solution of iodine or bromine. (3) Sulphur in ash. This can be done either by boiling the ash with hydrochloric acid, filtering and determining the sulphuric acid in the filtrate, or by fusion with alkaline carbonates. Proximate Analysis of Australian Xhale. Sp. gr. = 1.0401. Water lost at 100" - .......... 0.44 Volatile matter ............ 77 69 Corrected for sulphur. Fixed carbon .............. 5.56 9, 7 9 Ash ...................... 15.83 Sulphur in volatile matter.. . . ? * . . . . 9 9 fixed carbon.. 9 , ash. ............. 100.00 The practical method of examining coal for gas-making purposes partakes of two forms : (1) a partial imitation of the process of gns manufacture on a small scale ; (2) analysis of coal by conducting a gas manufacture in a setting of clay retorts with large plant for exhausting, condensing, scrubbing, purifying, measuring the gas, and so on, as is in actual use. The laboratory practical analysis is undoubtedly of great value ; .it will, however, be necessary in interpreting the results, to recollect that the method of heating the coal is different to that used in practice with clay retorts. As far as quality and volume of gas are concerned, the best results are obtained with the small iron retort.The difference varies with the kind of coal employed. With the very finest cokinq coals the difference is very small, and as the coking quality of the coal increases so the difference between the two methods of testing increases. With coals (not cnnnels) which scarcely intumesce a t all, the difference becomes very high. Cannels also vary in tlie same manner, the difference in the results being always connected with differences in the qualities of the cokes. Since the gas from the iron retort is not scrubbed, a deduction of about 3 per cent. should be made from the results of the small apparatus to compensate for the small loss of illuminating power suffered by the qav 9 286 ABSTRACTS OF CHEMICAL PAPERS. of the large experimental works in the washing process.When this allowance is made there is but little difference between the two methodstof testing in the case of coking coals. Estimtion of Hydrogen XulphiJe mtd Carbonic A d ydTide in Crude Coal-gas.-The author prefers the use of a method admitting of the employment of a tolerably large quantity of gas collected regularly during an interval of )time sufficiently long to afford an idea of the average composition of the gas supply to be tested. The reagent used for absorbing the hydrogen sulphide is cupric phosphate. Absorption tubes charged with cupricLphosphate gain in weight under the action of pure coal-gas ; the increme of weight, however, soon reaches a limit, and the phosphatelmsby be saturated by passing 3 cubic feet of pure dry-coal gas slowly through tbe tubes.The carbonic anhydride is absorbed in soda-lime tubes, one half f u l l of soda-lime and one half of calcium chloride. To increase its absorptive power for carbonic anhydride the soda-lime is used in a moist condition. In cases where ammonia exists in the gas its removal is best effected by passing the crude gas before it is dried through a 12-inch U-tube filled with broken pumice saturated with syrupy phosphoric acid. Cyanogen.-This substance is estimated by paming a measured quantity of crude gas freed from ammonia through a (j-tube filled with soda’lirne, and then making a combustion of the residue as in an ordinary nitrogen determination. D. B. Analysis of Explosives. By G. LUNGE ( O h m . Ifid., 9, 273-274). -To render the author’s nitrometer suitable for the determination of nitrogen by Cmm’s method in substances like dynamite and gun-cotton, which cannot be introduced into the decomposition tube in the liquid form, and at the same time to avoid the error due to the evolution of carbonic.anhydride to which Hempel’s modification (this Journal, 40, 472) is liable, a small funnel-tube bent into a swan-neck is fitted by a rubber stopper to the cup in which the weighed substance has been placed. Through this the sulphuric acid required to dissolve the substance is poured. Any carbonic anhydride evolved can escape, but loss of nitrous fumes is prevented by the acid which remains in the bend of the swan-neck. When the substance has dissolved (which in the case of gun-cotton may take three-qnarters to one hour) the solution is drawn into the graduated tube.The acid in the funnel tube follows and rinses the cup. The stopper can now be removed and further rinsings given. The siliceous earth suspended in the acid has not been found to cause any inconvenience. Three analyses of gun-cotton reported agree very closely. M. J. S. Estimation of Glycerol in Wine. By SAMUELSON (Chem. Zeit., 10, 933-934) .-Great discrepancies are observed in the estimation of glycerol by different chemists; this is probably due to want of uniformity in working, therefore the following mode of procedure is recommended. After adding milk of lime, evaporate only as far as to leave the mass just moist, then add somewhat more than 50 C.C. of 96 per cent. alcohol, and evaporate the alcoholic extract to 5 c.c ;ASALYTICAL CHE3lISTRY.87 extract with absolute alcohol and ether, evaporate the extract until free from alcohol, then dry the residue for a t least an hour. Estimation of Solid Matter in Wines. By E. ROEILHON (Cornpt. rend., 103,498) .-When the total residue in wine is estimated by evaporation in a vacuum, the weight of the residue obtained is lower the greater the surface of the evaporating dish, owing to the loss of part of the glycerol. Three dishes each containing 10 C.C. o€ wine were placed under the same receiver and kept in a dry vacuum for 8-24 hours. The results axe given in grams of solid matter per litre of wine. Dilute alcohol D. A. L. Rousil- with 10 p. c. Bordeaux. Girs. lon. Coupage. glycerol. 28 sq. C.C. surface. 22.4 30.8 34.2 25% 34.8 70 7 9 ,, .. 22.0 30-3 33.0 25.1 33.2 with sand 5 mm. 21.2 .29.1 30.4 23.8 31.7 70 9 9 I n order to obtain comparable results, flat dishes of the same diameter should be uscd, arid these should contain equal quantities of wine and be placed ,in the same position in the receiver of the air- Pump. C. H. B. deep . . . . . ” . . . * * . . } Estimation of Acidity of Malt. By E. PRIOR ( B i d Ceiitr., 1886, 647).-The usual way to estimate the acidity of malt is to digest a weighed quantity of ground malt in water for two hours, with frequent agitation, to filter quickly, estimate acidity in an aliquotl part, and calculate as lactic acid ; the author found that half an hour’s digestion with water sufficed to show acidity; he recom- mends a 20 per cent. dilution by Folume of neutral alcohol as the fluid for extraction, the percentage of acidity when this is employed remaining constant €or 24 hours.His method is to dilute ordinary commercial absolute alcohcl with four volumes of water, 500 C.C. of this is used to 100 grams of ground malt, digested in the cold fcr four hours with frequent agitation, filtered, and 100 C.C. titrated with baryta-water. Freaence of Nitrites and Nitrates in Milk an Evidence of Adulteration. By M. SCHRODT (Bied. Centr., 1886, 629).-Nitrous or nitric acids are not norrnally found in milk, and when found in a, suspected sample should be taken as evidence of dilution, spring water which is often added to dilute it, generally containing either nitrites or nitrates. The objection may possibly be made that the cow’s fodder contained nitrates or nitrites ; to put this to the proof, the author fed two cows for five days on beets, to which he added 10 grams daily per head of potassium nitrate, notwithstanding which rio trace of nitrates, &c., was found in the milk ; he therefore thinks tlie evidence afforded by their presence is conclusive.The method used was that introduced by Soxhlet, the reagent being diphenylamine. J. F. J. F.88 ABSTRACTS OF CHEMICAL PAPERS. Further Notes on the Methods of Examining and Chemistry of Fixed Oils. By A. H. ALLEN (J. SOC. Chsm. Ind., 5, 65-72, and 288--283).-Speci$c Gravihy of Oils.-A convenient instrument for ascertaining the density of fixed oils is Westphal's hydrostatic balance. A counterpoised thermometer suspended from a piece of thin platinum wire is attached to one end of a graduated lever. On immersing the thermometer in a liquid, it loses a certain weight.The equilibrium is restored by hanging on the lever a series of riders, whlch are adjusted in weight so as to make the reading very simple. As t'he employment of a thermometer as a plummet renders the instrument unsuited €or determinations of density a t loo", or other high temperature, the author substitutes in such cases a plummet of thick gIass rod. For the determination of the density of fats the author some time ago recommended the use of a Sprengel tabe, and urged that the density should be taken at the boiling point of water. I n all cases, however, where there is snfficient substance a t disposal, the Sprengel tube has been abandoned in favour of the plummet.Coeflccients of Expansion of Oils.-A series of tables illustrating the rates of expansion of fats and oils are given, showing (1) that the rates of expansion of the fluid fixed oils are not sufficiently different to be of any value for their recognition; (2) that of the fluid fixed oils examined (sperm oil, bottle-nose oil, whale oil, porpoise oil, seal oil, menhaden oil, neats-foot oil, lard oil, olive oil, arachis oil, rape oil, sesame oil, cotton-seed oil, niger-seed oil, linseed oil, and castor oil) all with the exception of whale oil expand sensibly equally for the same increase of temperature; and (3) that with the exception of whale oil the correction in density for the fluid fixed oils examined may safely be taken at 0.64 for 1" C.(water a t 15.5" = lU00). Viscosity of Oils.-The author is of opinion that Redwood's new form of viscosimeter bids fair to become the recognised standard instrument of the future. For many purposes, however, and especially as a convenient test by oil merchants, the following instrument is likely to grow in favour. It consisks of a simple arrangement by which a small paddle-wheel (actuated by a falling weight) is caused to revolve in the sampla of oil maintained at a definite temperature by an outer ressel of water. The manipulation is very simple, Snd the results expressed by the number of seconds required by the weight to fall through a given space are very constant. Bromine and Iodine Absorptions of Oils.-In order to facilitate the comparison between the results of Mills (ibid., 2,435, and 3, 366) and Hub1 (Abstr., 1884, 1435), the author has multiplied the bromine absorptions obtained by Mills by -, so as to obtain the equivalent iodine absorptions, and has compared the results with * the experi- mental numbers for iodine absorptions obtained by Hiibl.The figures which are tabulated in the original paper indicate that the drying oils (containing linoleic acid) assimilate the largest proportions of the haloyds, alzd their capacity in this respect might probably be employed as a measure of their drying properties. The fish liver oils, however, fully eqiial the vegetable oils in their assimilating power for haloids. Hiibl's results in the main confirm those of Mills.127 80ANALYTICAL CHEJlIST RY. 89 Va7enfa’s Acetic Acid Test.-The author has tried this method (Abstr., 1884, 1018) on a number of oils and finds that a slight variation in the strength or proportion of the acid employed is not of importance, and that the temperature at which turbidity occurs with any particular specimen is readily observed and fairly constant. Concordant results have also been obtained from several samples of butter, and it appears probable that further experience may prove the method to afford a simple means of distinguishing butter from but terin e. Deferininnfion of Glycerol.-The difficulties attending the deter- mitiation of the glycerol produced by the saponification of fixed oils have recently been orercome by a method originally suggested by W a n k l p and Pox (Abstr, 1886, 395), and perfected by Benedikt and Zsigmondy.It depends on the saponification of the oil, and oxidation of the glycerol thus formed by potassium permanganate in alkaline solution, with formation of oxalic acid, carbonic anhydride, and water. The excess of permanganate is then destroyed by a sdphite, the solution filtered, the filtrate acidified with acetic acid, and pmcipitated with a calcium salt. As the precipitate contains calcium sulphate and silicic acid in addition to calciuni oxalate, the amourit of oxalic acid is determined either by titration of the pre- cipitate with permnnganate in acid solution, or by estimating the alkalinity of the ignited precipitate. For the determination of glycerol in fats, the author recomniends modifying the method in the jollowing manner :-5 grams of the sample of fixed oil is placed in a six-ounce bottle, together with a solution of 2 grams of caustic potrsh in 12 C.C.of water. The bottle is secnrely closed and heated in a water-oven or in boiling water for 8 or 10 hours, the contents being frequently agitated. When the product is perfectly homo- geneous and all oily globules have disappeared, tbe bottle is opened, and the soap diluted with hot water, when a perfectly clear solution should be obtained, except in cases of sperm oil, wax, and other sub- stances yielding insoluble alcohols on saponification. The soap solution is then treated with a moderate excess of acid in the usual way, and the liberated fatty acids are separated from the aqueous liquid con- taining the glycerol, ahich latter is then ready for oxidation with a1 kaline permanganate as above described.By C. J. ELLIS (J. SOC. Chenz. Id., 5, 150-152 and 361-362).-The author has made some experiments with the view of extending the application of Maumenk’s test to drying oils and fish oils, to which it caniiot be directly applied without some slight modification, owing to the violent action which ensues when these oils are mixed with concentrated sulphuric acid. To overcome this difficulty i t was found necessary to mix with a drying or fish oil some liquid which will moderate the action of the acid on the oil. The author employed a mineral lubricatiiig oil of 0.915 sp. gr. for this purpose, and as on mixing sulphuric acid with such an oil a certain increase of temperature takes place, it is necessary to deter- mine the rise due to each gram of the mineral oil.To accelerate the action of sulphuric acid on the mineral oil, a certain proportion of I). B. Maumen6’s Test for Oils.90 ABSTRACTS OF CHEMICAL PAPERS. colza oil was added, for which the standard number, when not mixed, was accurately determined and found to be 35.8”. Contrary to ex- pectation, it was found that the smaller the quantity of mineral oil iii the mixture the greater is the value representing the rise due to each gram of the mineral oil, providing the rise due t o each gram of the vegetable oil remains constant whatever the mixture. To calculate the rise in temperature due to each gram of the mineral oil the following formula is employed :--y = a + bz, iii which -y represents the rise in tempeiature due to each gram of mineral oil, x is the fraction of the mixture coiisisting of mineral oil, and cc and b are constants depending on the conditions of the experiment and the particular mineral oil employed.In order to obtain the most concordant and trustworthy results, the maximum temperature attained should not exceed 60”, and it is for this reason that the author prefers the use of a, mineral oil as the re- tarding reagent. D. B. Employment of Congo-red in Titrating Aniline. By P. JULIUS (C‘hein. I d , 9, 109-110).-CCongo-red, the compound of tetrazodiphenyl with naphtholsnlphonic acids, is turned blue by acids, and recovers its red colour with an excess of alkali. When used as an indicator i n titrating aniline or its homologues with a mineral acid, the point is taken at which a bluish-violet, not changed by small further additions OE acid, is produced.A much larger excess is required to produce a pure blue. The results do not vary more than 0.2 per cent. from the theoretical numbers. Hufner’s Method of Estimating Urea. Ry E. PFL~GER and K. BOHLAND (P’cger’s Archiv, 39, l-l7).-Pfliiger and Schenk pre- viously proved (ibid., 38, 385) that Hiifner’s method of estimating the nitrogen in urine gave results which were too low and variable to found a calculation of the total nitrogen on. Owing to the improve- ment made in Bunsen’s method, the authors have been able to ascertain whether Hufner’s method was sufficiently accurate for the determination of urea only.They find that the results are always too high and also very variable. The variatipn ranges from 1 per cent. to 10 per cent., and does not therefore admit of compensation. J. P. L. M. J. S. Estimation of Urea in Human Urine with Sodium Hypo- bromite. By E. PFL~~GER and K. BOHLAND (Pfliiger’s Archiv, 39, 143-158) .-Pfluger’s new method of estimating urea by hypobromite (PJliiger’s rlrchiv, 38, 503) can be applied to the estimation of urea in liunian urine provided the nitrogenous extractives are first removed. J?or this purpose, a given volume of urine acidified with hydrochloric acid (1 of acid to 10 of urine) is precipitated with sufficient phospho- tungstic acid to ensure the separation of all the extractives, the mixture made up to a known volume, and allowed to remain 24 hours a t least previous to filtration.The acid filtrate is carefully neutralised with powdered lime, and again filtered through a dry filter. Great stress is laid on the use of pure soda and bromine for theASALPTICAL CHEJIISTRT. 91 preparation of the hypobromite. of urine by this process was + 1.3 per cent. The mean error of several analyses J. P. L. Qualitative Tests for the Dyes Found in Commerce. By 9. N. WITT (Chem. Ind., 9, 1--7).-A table of reactions for the identi- fication of about 80 artificial colouring matters taken singly. Many commercial dyes are mixtures : in this case, the powder strewn upon wet filter-paper or colourless sulphuric acid will generally give streaks of more than on6 colour. Where the mixture is more intimate a solution must be made, and the colouring matters withdrawn frac- tionally by dyeing small pellets of wool or silk in it.The principal adulterant for azo-dyes is sodium sulphate. It is best detected after precipitating tlie colour by pure sodium chloride. M. J. S. Detection of Artificially Coloured Red Wine (Clarat). By J. HERZ (Chem. Zeit., 10, 968-969 ; 998).-To 30-50 C.C. of the wine, or if the quantity of colouring matter in the wine is small, 100 C.C. concentrated to 30 c.c., 20-30 C.C. of a saturated solution of magne- sium sulphate, and 10-20 C.C. of soda solution are added, stirring well; if necessary the treatment is repeated until the liquid is colourless, or nearly so. The filtrate is made acid with dilut,e sul- phuric acid (1 : 3), and if sulphonic acid colours are present the red colour reappears.The most commonly used member of this group, acid-magenta (rosanilinesulphonic acid), yields a, violet-red solution, and can be estimated by comparing the tint with magenta solutions of known strength. One mgram. of magenta per litre can be distinctly detected in 30 C.C. of wine without previous concentration. When archil (orseille) colours are present, the filtrate is bluish, and when made acid turns a litmus-red colour. To test for magenta under such circumstances, Blarez’ method of shaking with lead dioxide is used ; $his destroys the orseille and natural colour. Cazeneuve’s method is not recommended. To test for other colours in the magnesium hydroxide precipitate, the gelatinous mass is stirred up with hot water, allowed to settle, and the liquid decanted off.I f only the natural colour of the wine is present, or bilberry has been used, this liquid is yellow-brown ; if archil has been used, dark-violet,; if yonceau, onion or ponceau red ; if casskshe, pale-red or dark-yellow ; if cinicoline bcrdelaise, a yellow-red to yellow-brown liquid, which when poured on sulphuric acid gives a violet ring. By shaking the coloured liquid with ainyl alcohol, Tonceau yields an onion-red residue ; vinicoline, a dark-brown one ; ccmwsine, a dirt-y-green, violet at the edge, turned yellow by strong hydrochloric acid. The precipitate is a dark-grey or brownish-grey colour when the natural or vegetable colours only are present; with archil, it is violet; with magenta (acid o r ordinary), dirty white ; with cassissine, dirty yellow-brown ; with vinicoline, crimson-red.The precipitate is mixed with sand, dried, and extracted with ether ; the extract contains any ordinary magenta which can be identified in the usual manner by dyeing wool, or cassissine which dyes wool red-brown and leaves a yellow-brown residue in the dish. The dyed wool becomes yellow when treated with strong hydrochloric acid and colourless with ammonia. When92 ABSIL’RACTS OF CHEMICAL PAPERS. wine is shaken with amyl alcohol, and the coloured extract evaporated, the residue, if it contains tho gubstances named, behaves in the manner described below :- Wilh concentmted c-A 7 H:S0,. HCI. NaHO. Archil . . . . . . . . violet-red bl ue red bl 11 e Bordeaux, B... . oarmine carmine carmine carmine Ponceau, RRR.. dark-red crimson crimson brown Cassissirie.. . . . . violet-purple yellow yellow- red Vinicoline Bor- brown delaise . . . . . . cherry-red brown red brown whilst the wine after extraction i~ cherry-red with ordinary maqefcta, violet-red with acihmngenfu, dark-cherry with Bordeam, yellow-red with p o i z c m ~ . Wine coloured with magenta produces a violet froth. The detection of vegetable colouring matters in presence of the natural colour of wine or otherwise is a matter of great difficultg, and most of the known metliods are ineffectual ; it is, however, effected by the authorwith comparative facility in the following manner :-I0 15 C.C. of wine is shaken with 5 C.C. of a saturated solutiop of tartar emetic, and then examined by reflected and transmitted light either a t once or, if no immediate chanqe has taken place, after some time.This treatmelit produces with genuine red wine always a cherry. red colour, and with other substances as follows :-Red-poppy (Papaver r?iwus), dark cherry-red ; cherry, violet : commercial elder colonring matter, Ed-violet ; hilberry (Vaccin. niyrtill), blue-violet ; priret-berry, piire violet. White wines artificially colonred, and red wines mixed with artificial colours have been successfully examined in this manner ; in the latter case the wine some time after treatment is compared with a genuine red wine to distinguish more readily the change of colour. Old solutions of privet do not give the d o u r change. Sodium hydrogen carbonate produces with pure wine, brown-red ; with wine coloured with pure eldedwry, grey-violet ; and with hilberry, brown- green.Tartar emetic appcars to form an antimony lake with tho colouring matters. With practice, all the above-mentioned coloum cart be detected in 30-50 C.C. of wine. In the subsequent communication (loc. cit., 998), the author acknowledges the priority of Ambiihl and Elsner’s recommendation of the use of tartar emetic for the purpose in question. They, homver, recommend hot solutJions ; the author finds cold better. Fermented bilberries give the violet colour even better than unfermented berries, especially when fresh, innsrriuch as oxidation interl’eree with t,he delicacy after a time. The distinctness of this colour is increased by diluting the wine.D. A. L.78 ABSTRACTS OF CHEMICAL PAPERS.An a 1 y t i c a 1 C h em i s t ry.Kjeldahl's Method of Estimating Nitrogen. By C. ARNOLD(Arch. Pharrn. [3], 24, 785--794).-The author shows that thismethod (Abstr., 1884, 364; 1885, 930) is also applicable to nitrates,nitro- and cyanogen-compounds, in the presence of beneoic acid, sugar,mercury, and copper sulphate ; further, in the case of alkaloids andotber compounds that can be treated by this method, oxidation bypotassium permanganate is unnecessary if the boiling be continueduntil the warm liquid acquires a bluish-green tint, becoming colour-less on cooling ; this takes place tolerably quickly in the presence ofmercury and copper. That the oxidation has been completed canreadily be ascertained by adding a crystal of potassium permanganate,which should give a persistent violet or green coloration.A descrip-tion of tlie apparatus used by the author is given. J. 1'.Separation of Arsenic and Antimony. By ZAMBELLI andLUZZATO ( A ~ c h . Pharm. [ 3 ] , 24, 772).-These elements can be sepa-mted, even in foyensic cases, by treating the still moist sulphides withhydrogen peroxide at 40' for some hours, then heating to near 100AKALYTICAL CHEMISTRY. 79and filtering. The arsenic acid formed goes into the filtrate, whilst theinsoluble antimony oxide remains on the filter. The method is saidto be very delicate.Detection of Thiosulphate in Hydrogen Sodium Carbo-nate. By RRENSTEIN and T. SALZER (Arch. Yharm. [3], 24, 761).-According to Brenstein, the reaction given for thiosulphate by Myliusis not characteristic, as other oxygen-compounds of sulphur, such assulphites, give rise to the formation of hydrogen sulphide.A bettartest for tJiiosu1phate is to add to a 5 per cent. solution of hydrogensodium carbonate a few drops of silver nitrate solution, then excess ofnitric acid, and heat to boiling; even minute traces of thiosulphategive an immediate dark precipitate of silver sulphide.According to Salzer, the absence of thiosulphate is easily ascer-tained by adding a few drops of iodine solution to about 20 C.C. of asaturated solution of hydrogen sodium carbonate ; the solution musthave a yellowish tint. Decolorisation of the iodine solution does notnecessarily imply the presence of thiosulphate, since normal carbo-nate, the most commonly occurring impurity, produces this effect.Both authors found thiosulphate to be a constant impurity of ordinaryqualities of hydrogen sodium carbonate, whilst the better qualitieswere mostly free from it.Estimation of Small Quantities of Silver in Burnt Pyrites.By E.Trrrr,o (Cherrz. Zeit., 10, 822; 1065--1067).-The amount ofsilver in burnt pyrites is ordinarily 0*003--0.008 per cent., and toobtain trustworthy results material containing 0.01 gram of silvershould be taken for analysis, or about 300 to 500 prams of pyrites. Manydifficulties have been encountered in endeavouring to deal with theselarge quantities of material so as to get all the silver. Experimentsshow that the decomposition of the whole mass is out of the question,therefore methods for extracting the silver, &c., were tried ; treat-ment with nitric acid or with gaseous chlorine, and subsequentextraction of the silver chloride proved unsuitable.Digestion withchlorine-water was somewhat better ; but bromine or bromine-watergives the best results. The powdered burnt pyrites is passed througha 0.25-mm. mesh sieve, and about 300-500 grams of it is placed i nan acid-proof iron basin; it is well covered with water, and whilevigorously stirred, bromine is added until present in excess. After24 hours it is heated on a water-bath for one hour with frequentstirring, treated with excess of ammonia, then with 500 grams ofammonium chloride, and 1 litre of water.The mass is boiled for anhour, and filtered. The residue is dried, ignited at a low red heat, andagain treated with arnmoniacal ammonium chloride, by which meansall the silver is extracted. Inasmuch as copper is quite as difficult assilver to extract by means of bromine, and as theamount of copper i nthe pyrites is reduced from 5 per cent. to a trace (0.01 per cent.) by theabove treatment, this may be used as an indicator of the progress of thedesilvering, and in practice when the copper is reduced to this amountit may be safely inferred that all the silver is removed. The solu-tion, about 4 litres, is made acid with hjdrochloric acid; it is notJ. T.J. T80 ABSTRACTS Ol!’ CHEMICAL PAPERS.affected by daylight either before or after acidifying.The silver,copper, and lead are then precipitated by means of chemically piirezinc. When the precipitation is complete, the solution is colourless(or rose-red if cobalt is present), and is not turned blue bv ammonia.As the precipitate contains, most liksly, silver chloride and bromide,and some iron oxide, it is fused with potassium cpnide, and sub-sequently with anhydrous borax, the temperature being raised to meltthe copper, The regulus is dissolved in nitric acid, and the silvereither precipitated by means of hydrochloric acid or determinedelectrolytically. Silver determinations may also be made in ordinarypyrites, which is first roasted carefnllp, and then treated in the abovemanner. Good results have been obtained by this method, withroasted copper schist, with spathic iron ore containing argentiferoustetrahedrite and pyrites, and with other ores.A determination can becomplded iu three days.Comparative Gasometric Assaying with Especial Referenceto the Valuation of Zinc Powder and the Testing of Car-bonates. By J. BARNES ( J . SOC. Chem. Ind., 5, 145--147).-1n a,previous communication (Trans., 1881, 462), the author described amethod for the valuation of zinc powder, consisting in measuring theamount of hydrogen liberated on treatment with an acid. Theauthor has since devised a method and constructed an apparatus forgasome tric assaying, contrived originally for the valuation of zincpowder, but applicable also to the estimation of other substances,which may be made to cause or control tlie evolution of gases.Themethod, which is described in detail in the paper, is a comparativeone, and requires a t least two graduated instruments, each providedwith a suitable gas evolving arrangement. A substance of knownvalue, taken as the standard, is placed in one, and the sample tobe examined in the other instrument. The value of the sample isthen calculated by the following formula: - . W . R = x ; - whereVequals the volume of gas from standard, v the volume of gas frommmple, W the weight of standard, and ?u the weight of sample.R is the amount of pure substance or its equivalent in unit ofstandard, and x the amount of pure substance in unit of sample.Determination and Valuation of Copper in Ores andProducts for Commercial Purposes, with some Remarks onthe Assay of Gold in Bar Copper.By J. TV. WESTMORKLAND( J . Soc. Chem. Ind., 5, 48--64).-Esfin?ation of Moisture.-This,although apparently a simple process, is conducted very differentlyby rarious assr,yers, and the author proposes that the temperatureand niaiiner in which the moistnre is to be taken should be moreclearly defined than it is at the present time.Wet Assay of Coppr.-Having examined a iarge number of samplesof all kinds of copper ores aud products by several wet processes, theauthor has given the iodide process as modified by Brown thepreference-being more trustworthy arid accurate than the electrolytioprocess. For cupreous pyrites, burnt ores, &c., the followiiig mctliodD.A. L.v 20D. BANALYTICAL CEEMISTRY. 81mny be used. From 50 to 150 grains of the sample is dissolved in acids,evaporated to dryness with excess of sulphuric acid, diluted with waterarid filtered, From this solution, the copper is separated with sodiumt'hiosulphate, the precipitate dried, ignited, dissolved in nitric acid,evaporated with sulphuric acid to separate Graces of lead, dilutedwith water and filtered, sodium carbonate added in excess, and thenacetic acid to acid reaction. The solution is then titrated withpotassium iodide. As 8n alternative method, the ore may be calciued,dissolved in hydrochloric acid, the ferric salt reduced by boiling witha solution of sodium sulphite, and hydrogen sulphide passed throughthe cold Rolution; the precipitated sulphides are then washed, andthe process conducted as before.Richer copper ores, mattes, preci-pitates, &c., are dissolved in acids, and the solution precipitatedeither with sodium thiosulphate or hydrogen sulphide, the sulpbidesbeing dissolved in acids, and treated 8s before. The accuracy of thisprocess was tested by numerous experiments, in which known weightsof pure electrotype copper, silver, arsenic, antimony, lead, cadmium,bismuth, tin, manganese, zinc, and iron salts were used. The solutionswere made to represent cnpreons burnt ores, mattes, cupriferous leadregul us, second quality and rich precipitates, &c. Experiments werealso made i n many cases with the metals separately. The electro-deposition method may be employed in cases where it is desir,thle tohave resultti of two separate and distinct processes, it being notedthat with pure solutions of copper, accurate results are obtained,whilst when silver or bismuth are present they are precipitated, andin one experiment tin was also deposited with the copper.In thepresenoe of ferric salts, the deposition is retarded. It was found thatwhilst the results with refined or bar coppers and rich precipitatesagree with those obtained by the iodide process, those obtained byelectrolgsing sulphuric acid solutions of mattes, copper ores, $c., aregenerally slightly below the triie percentage. With burntl ores,cupreous pyrites, and ores containing but little COPPOI', the authorfirst precipitates with hydrogen sulphide, dissolving the s u lphide innitric acid, and evaporating this soliifion with excess of sulphuricacid, the sulphates dissolved in water give a solution from whichcopper (and bismuth) is readily deposited.The results by the batteryprocess are generally from 0.01 to 0.04 per cent. higher than by theiodide process, this being cniised by a slight deposit of bismuth.The Cornish Yroce.9~ of Dry Assay.-This process is considered to beinaccurate and misleading, and is also liable to aerious variation evenin the hands of experienced operators.The author is of opinion that in cases where the sulphur contentsof pyrites are sold to alkali works, tbe burnt ores being returned tothe vendors, an accurate wet assay forms the best# check on the coppercontents of the ore delivered to and received from the alkali works.In the remaining part of the paper, the methods in vogue for fixingthe prices payable for copper in pyrites, copper ores.&c., are discussed.Reftmnce is also made to the avsay of goltl in bar coppry, and theopinion is expressed that t>hese assays are not conducted as carefullyaa they should be, taking the value of the metal into oonsideration.I). B.9 VOL LU82 ABSTRAOTS OF CREMICAL PAPERS.Estimation of Ammoniacal Nitrogen in Soils, and theAmount of Assimilable Nitrogen in Uncultivated Land. RyA. BAUMAXN (Lmdw. Versuchs-Stat., 1886, 2$7--303).--The methodsemployed to estimate the ammonia in soils are nnsatisfactor-y.Schlosing’s method, whereby the ammonitt is freed by means of milkof lime or sodium hydroxide, gives results too high, probably owingto the formation of ammonia from other compounds during theperiod (2-3 days) required for the process.In Bonssingault’sprocess as modified by Sclilosing, a hydrochloric acid extract of the soilis treated with magnesia usta, but the ammonia collected in acid mu$not be estimated by titIration, but must be azotometrically determined ;nor must cork nor caoutchouc be employed in the formation of theapparatus, The liquid in the evolution flask must be boiled for atleast an hour, and the magnesia usta must be fresh. With thesetwo processes, it is found that humous soils, when treated with sodiumhydroxide, continuously yield ammonia ; if the soil, after treatmentwith magnesia, be further treated with sodium hydroxide, anothersupply of ammonia is obtained, b u t only in the case of soils rich innumus.Knop’s process, in which the ammonia is decomposed bybrominated sodium hydroxide solution, is vitiated by the fact, noticedby Rnop and others, that in the presence of the soil itself a con-traction of the volume of gas enclosed in the apparatus occurs ; thiscontraction was stated by some to be due to absorption by the organicmatter, whilst others considered the oxides of iron in the clay to bethe real cause; also it had been stated that the presence of boraxprevented this contraction. To ascertain the cause of the con-tract.ion, a sample of stiff soil poor in humus, was taken from uncul-tivated land a t a depth of 15-20 cm.; this sample seemed freefrom humus, although root-fibres were visible ; at a distance of 40 m.from this spot another sample was drawn from a depth of 2-10 cm.,this was close to a pine SO years old.The sample showed humus,and when dry was grey. At another spot, close to a 100 year oldpine, a third sample was taken, and this when dry wa8s dark-brown,These last two samples overlaid a soil similar to the first sample,Employing these samples, the author argued that if the contractionwas due to the clay and the iron, and not to the humus, then identicalcontractions would be observed when equal quantities of all sampleswere subjected to like conditions. On the other hand, if the phe-nomenon is caused by the humus, then that sample richest in humuswould produce the greatest effect on the volume of the gas, and whenborax was employed no contraction should occur.It appears thatthe ferruginous soil poor i n humus produced no contraction, butrather an increase of volume after the first 2 hour ; this is explainedby the probable presence of nitrogenous matter decomposable by thebrominated alkali. The presence of borax assisted the evolution ofgas.Experimenting with humous samples, it was found that the volumeof gas evolved by Knop’s method stands in no ratio to the percent-age of ammonia present ; this remarkable result was most manifestin the case of the third sample, which contained most humus, forthen the contraction was evident when only 5 grams were usedAXALP TlCXL CIIEMISTRY.83and in spite of borax the contraction amounted to 71 per cent. when1UO grams was employed, This contraction is clearly due to oxida-tion of the organic matter of the soil, and consequent removal of partof the gaseous contents of the azotometer.Working with sandy and chalky Hoils, the author found that theresults obtained by Knop’s method are quite as untrustworthy as inthe case of humous samples.The following method is recommended for the estimation of am-monia in soils:--200 grams of the soil is mixed with 100 C.C. ofhydrochloric acid (1 : 4), then diluted with 300 C.C. of distilled waterand allowed to remain for two hours, with frequent shaking. Shouldmuch chalk be present, then more than 100 C.C.acid must be added,and the whole amount of liquid made up to 400 C.C. ; all heatingmust be avoided. Of the filtrate, 200 C.C. (= 100 grams soil) isplaced in the evolution vessel of the azotometer together with 5 gramsof freshly ignited magnesia usta, and the vessel closed by a doublybored india-rubber stopper ; through one of the borings a glass tubepasses to the bottom of the flask, whilst the other opens immediatelybelow the stopper, and is connected with an aspirator, whilst theother tube supplies air ozonised by passing through potassium per-manganate and concentrated sulphuric acid. The passage of this gasfor 10 minutes oxidises organic matter, so that no subsequent con-traction occurs, The rest of the process is conducted in the ordinaryway.Percentage of Ammonia i n Soils.-Soils of various characters wereexamined, and the percent’ages as found by Schlosing’s and the othermethods are given : there appears to be a, wide difference between thefirst and the other two methods.The percentages at different periodsin summer and at different depths are recorded. The conclusionsdrawn are that the percentage of ammonia in uncultivated soils varieswith the character of the soil, loams containing most, the quantityincreasing with the increase of clay; chalks and sands are poor inammonia, but in sands rich in hurnus there is a large supply oforganic compounds which readily decompose and yield ammonia,although generally speaking, the percentage of organic matter is noindication of t$he amount of ammonia present, and the percentage ofammonia in a soil does not seem to vary with the weather, but doesdecrease with depth from the surface.Percenta>ge of Nitrates i ? ~ Urnnunured Soils.-Baumann employsSchlosing’s method of estimating nitrates if the solution of 1000 gramssoil in water made up to 3000 C.C.shows the brucine reaction, even ifthe reaction is only obtained after evaporating the solution to one-halfof its original volume. If this test should fail, then diphenylnniineis to be employed; this should indicate 1 in 1,500,000 or 0.6-1 mgrm. per litre ; should this fail, so also will Schlosing’s method, andit will be necessary to evaporate 1 litre of extract with some alkali todryness, add alcohol, boil, filter, and then evaporate the alcohol anddissolve in 40 C.C.water. The solution must be again tested bybrucine and diphenylamine, and if indications of the presence ofnitrates are visible, the Marx-Trommsdorf’s method (Zeit. anal.C‘lzem., 1868, 412, and 1870,171) is to be employed for the quantitativ8 -1 ABSTRACTS OF CHElllICAL PAPERS.estimation ; this will indicate 0*00001 per 300-400 grams soil.Examination of many soils shows that when the soil is uncultivatedthe percentage of nitrates is very small, especially in forests, where i tonly appears as traces.The author then reviews the work of Warington, Scliliisinp, andMiint>z on nitrification, and considers that the absence of nitrates insuch soils as he refers to, is due to the normal temperature ( 5 > ) beingso close to that a t which nitrification first occurs; also water isnecessary for nitrification, and in forest soils, therefore little nitri-fication takes place, because of the great dryness of that soil insummer, due especially to the enormous transpiration continuallyoccurring, which renders the soil almost "air-dry ; " a further causefor the absence of nitrification may be faund in the want of animalAnalysis of Gas Coal.By L. T. WRIGHT (J. SOC. Chem. Ind., 4,656-667) .-Proximate amZysis.-T he first determination is that ofmoisture. T'arious temperatures have been recommended at whichthe sample of coal shall be dried. Since ZOO' is a temperature easilyRecured and maintained constant by means of a water-bath, the authorhas adopted it as the standard.The estimation of moisture by lossof weight in drjing a t 100" until the weight of the substance become9constant is not, however, free from error ; as it has been noticed bydifferent observers, that after a time the coal not only ceases to loseweight but actually gains. Hinrichs attributes this increase to theslow oxidation of pyrites and other substances in the coal ; the author.however, considers it to be due to the absorption of gases into thepores of t h e coals left vacant by the expelled moisture. He has alsofound that the increase of weight, which only exhibits itself when t h econ1 has been nearly dried, has been going on during the wholeperiod of the drying process, SO that where accuracy is required it ispreferable to weigh the water as such.According to Hinrichs thetotal volatile matter of coal is determined with accuracy by taking1 to 2 grams of undried pulverised coal, heating for three and a halfminutes over a Bunsen burner, and then immediately igniting withoutcooling, for the same period over a blast gas lamp (white heat). Thegreatest difference which Hinrichs obtained amounted to 0.29 percent. The author has reFeated this method and obtained very fairresults, although not quite so accurate as the above. The authoradopts the following method:-Take about 2 grams of finelypulverised coal and let i t form an even layer on the bottom of a thinplatinum crucible. Weigh without cover. place the crucible (withcover on) in an upright position, then apply a powerful gas flame.Note when the gases cease issuing from under the lid; allow oneminute further heating, remove the gas flame, place the crncible andcover in a desiccator tor about five minutes to cool, and then weighwithout cover as soon as possible.For the determination of ash inrefractory cokes and such substances as gas carbon, heat to redness2 grams of the coal or coke placcd on a piece of platinurnfoil, inR combustion tube through which ft gentle current of air is drawn.The ash should be saved for the determination of sulphuric acid.nutriment for the growth of the ferment. E. w. PASALFTIC hL C HENISTRT. 85k'or the determination of the total sulphur, the best and eimplestmethod is that suggested by Nakamura, which consists in heating thecoal below a red heat in contact with alkaline carbonates, when thecoal whether bituminous or not rapidly undergoes complete oxidation.For the purpose of distinction hetween the sulphur which goes overinto the volatile matter, the sulphur left in the coke and that which isfinally left in the ash combined as sulphate, three determinations arerequired :-(1) Total sulphur by Nakamura's method. (2) Sulphurwhich is converted into sulphurous anhydride by combustion of thecoke in air, obtained by roasting a quantity of coke representing aknown quantity of the coal, and aspirating the gaseous products ofcombustion through a solution of iodine or bromine.(3) Sulphur inash. This can be done either by boiling the ash with hydrochloric acid,filtering and determining the sulphuric acid in the filtrate, or byfusion with alkaline carbonates.Proximate Analysis of Australian Xhale.Sp.gr. = 1.0401.Water lost at 100" - .......... 0.44Volatile matter ............ 77 69 Corrected for sulphur.Fixed carbon .............. 5.56 9, 7 9Ash ...................... 15.83Sulphur in volatile matter. . . . ? *. . . . 9 9 fixed carbon..9 , ash. .............100.00The practical method of examining coal for gas-making purposespartakes of two forms : (1) a partial imitation of the process of gnsmanufacture on a small scale ; (2) analysis of coal by conducting a gasmanufacture in a setting of clay retorts with large plant for exhausting,condensing, scrubbing, purifying, measuring the gas, and so on, as is inactual use.The laboratory practical analysis is undoubtedly of greatvalue ; .it will, however, be necessary in interpreting the results,to recollect that the method of heating the coal is different to thatused in practice with clay retorts.As far as quality and volume ofgas are concerned, the best results are obtained with the small ironretort. The difference varies with the kind of coal employed. Withthe very finest cokinq coals the difference is very small, and as thecoking quality of the coal increases so the difference between the twomethods of testing increases. With coals (not cnnnels) which scarcelyintumesce a t all, the difference becomes very high. Cannels also varyin tlie same manner, the difference in the results being alwaysconnected with differences in the qualities of the cokes.Since thegas from the iron retort is not scrubbed, a deduction of about 3 percent. should be made from the results of the small apparatus tocompensate for the small loss of illuminating power suffered by the qav9 86 ABSTRACTS OF CHEMICAL PAPERS.of the large experimental works in the washing process. When thisallowance is made there is but little difference between the twomethodstof testing in the case of coking coals.Estimtion of Hydrogen XulphiJe mtd Carbonic A d ydTide in CrudeCoal-gas.-The author prefers the use of a method admitting of theemployment of a tolerably large quantity of gas collected regularlyduring an interval of )time sufficiently long to afford an idea of theaverage composition of the gas supply to be tested.The reagent usedfor absorbing the hydrogen sulphide is cupric phosphate. Absorptiontubes charged with cupricLphosphate gain in weight under the actionof pure coal-gas ; the increme of weight, however, soon reaches a limit,and the phosphatelmsby be saturated by passing 3 cubic feet of puredry-coal gas slowly through tbe tubes. The carbonic anhydride isabsorbed in soda-lime tubes, one half f u l l of soda-lime and one half ofcalcium chloride. To increase its absorptive power for carbonicanhydride the soda-lime is used in a moist condition. In cases whereammonia exists in the gas its removal is best effected by passing thecrude gas before it is dried through a 12-inch U-tube filled withbroken pumice saturated with syrupy phosphoric acid.Cyanogen.-This substance is estimated by paming a measuredquantity of crude gas freed from ammonia through a (j-tube filledwith soda’lirne, and then making a combustion of the residue as in anordinary nitrogen determination.D. B.Analysis of Explosives. By G. LUNGE ( O h m . Ifid., 9, 273-274).-To render the author’s nitrometer suitable for the determination ofnitrogen by Cmm’s method in substances like dynamite and gun-cotton,which cannot be introduced into the decomposition tube in the liquidform, and at the same time to avoid the error due to the evolution ofcarbonic. anhydride to which Hempel’s modification (this Journal, 40,472) is liable, a small funnel-tube bent into a swan-neck is fitted by arubber stopper to the cup in which the weighed substance has beenplaced.Through this the sulphuric acid required to dissolve thesubstance is poured. Any carbonic anhydride evolved can escape, butloss of nitrous fumes is prevented by the acid which remains in thebend of the swan-neck. When the substance has dissolved (which inthe case of gun-cotton may take three-qnarters to one hour) thesolution is drawn into the graduated tube. The acid in the funneltube follows and rinses the cup. The stopper can now be removedand further rinsings given. The siliceous earth suspended in the acidhas not been found to cause any inconvenience. Three analyses ofgun-cotton reported agree very closely. M. J. S.Estimation of Glycerol in Wine. By SAMUELSON (Chem.Zeit.,10, 933-934) .-Great discrepancies are observed in the estimation ofglycerol by different chemists; this is probably due to want ofuniformity in working, therefore the following mode of procedure isrecommended. After adding milk of lime, evaporate only as far as toleave the mass just moist, then add somewhat more than 50 C.C. of96 per cent. alcohol, and evaporate the alcoholic extract to 5 c.c ASALYTICAL CHE3lISTRY. 87extract with absolute alcohol and ether, evaporate the extract untilfree from alcohol, then dry the residue for a t least an hour.Estimation of Solid Matter in Wines. By E. ROEILHON(Cornpt. rend., 103,498) .-When the total residue in wine is estimatedby evaporation in a vacuum, the weight of the residue obtained islower the greater the surface of the evaporating dish, owing to theloss of part of the glycerol.Three dishes each containing 10 C.C. o€wine were placed under the same receiver and kept in a dry vacuumfor 8-24 hours. The results axe given in grams of solid matter perlitre of wine.Dilute alcoholD. A. L.Rousil- with 10 p. c.Bordeaux. Girs. lon. Coupage. glycerol.28 sq. C.C. surface. 22.4 30.8 34.2 25% 34.870 7 9 ,, . . 22.0 30-3 33.0 25.1 33.2with sand 5 mm. 21.2 .29.1 30.4 23.8 31.770 9 9I n order to obtain comparable results, flat dishes of the samediameter should be uscd, arid these should contain equal quantities ofwine and be placed ,in the same position in the receiver of the air-Pump. C. H. B.deep .. . . . ” . . . * * . . }Estimation of Acidity of Malt. By E. PRIOR ( B i d Ceiitr.,1886, 647).-The usual way to estimate the acidity of malt is todigest a weighed quantity of ground malt in water for two hours,with frequent agitation, to filter quickly, estimate acidity in analiquotl part, and calculate as lactic acid ; the author found that halfan hour’s digestion with water sufficed to show acidity; he recom-mends a 20 per cent. dilution by Folume of neutral alcohol as thefluid for extraction, the percentage of acidity when this is employedremaining constant €or 24 hours.His method is to dilute ordinary commercial absolute alcohcl withfour volumes of water, 500 C.C. of this is used to 100 grams of groundmalt, digested in the cold fcr four hours with frequent agitation,filtered, and 100 C.C.titrated with baryta-water.Freaence of Nitrites and Nitrates in Milk an Evidence ofAdulteration. By M. SCHRODT (Bied. Centr., 1886, 629).-Nitrousor nitric acids are not norrnally found in milk, and when found in a,suspected sample should be taken as evidence of dilution, springwater which is often added to dilute it, generally containing eithernitrites or nitrates. The objection may possibly be made that thecow’s fodder contained nitrates or nitrites ; to put this to the proof,the author fed two cows for five days on beets, to which he added 10grams daily per head of potassium nitrate, notwithstanding which riotrace of nitrates, &c., was found in the milk ; he therefore thinks tlieevidence afforded by their presence is conclusive.The method usedwas that introduced by Soxhlet, the reagent being diphenylamine.J. F.J. F88 ABSTRACTS OF CHEMICAL PAPERS.Further Notes on the Methods of Examining and Chemistryof Fixed Oils. By A. H. ALLEN (J. SOC. Chsm. Ind., 5, 65-72, and288--283).-Speci$c Gravihy of Oils.-A convenient instrument forascertaining the density of fixed oils is Westphal's hydrostaticbalance. A counterpoised thermometer suspended from a piece ofthin platinum wire is attached to one end of a graduated lever. Onimmersing the thermometer in a liquid, it loses a certain weight. Theequilibrium is restored by hanging on the lever a series of riders,whlch are adjusted in weight so as to make the reading very simple.As t'he employment of a thermometer as a plummet renders theinstrument unsuited €or determinations of density a t loo", or otherhigh temperature, the author substitutes in such cases a plummet ofthick gIass rod.For the determination of the density of fats theauthor some time ago recommended the use of a Sprengel tabe, andurged that the density should be taken at the boiling point of water.I n all cases, however, where there is snfficient substance a t disposal,the Sprengel tube has been abandoned in favour of the plummet.Coeflccients of Expansion of Oils.-A series of tables illustrating therates of expansion of fats and oils are given, showing (1) that therates of expansion of the fluid fixed oils are not sufficiently differentto be of any value for their recognition; (2) that of the fluid fixedoils examined (sperm oil, bottle-nose oil, whale oil, porpoise oil, sealoil, menhaden oil, neats-foot oil, lard oil, olive oil, arachis oil, rapeoil, sesame oil, cotton-seed oil, niger-seed oil, linseed oil, and castoroil) all with the exception of whale oil expand sensibly equally forthe same increase of temperature; and (3) that with the exceptionof whale oil the correction in density for the fluid fixed oils examinedmay safely be taken at 0.64 for 1" C.(water a t 15.5" = lU00).Viscosity of Oils.-The author is of opinion that Redwood's newform of viscosimeter bids fair to become the recognised standardinstrument of the future. For many purposes, however, and especiallyas a convenient test by oil merchants, the following instrument islikely to grow in favour.It consisks of a simple arrangement bywhich a small paddle-wheel (actuated by a falling weight) is causedto revolve in the sampla of oil maintained at a definite temperatureby an outer ressel of water. The manipulation is very simple, Sndthe results expressed by the number of seconds required by theweight to fall through a given space are very constant.Bromine and Iodine Absorptions of Oils.-In order to facilitate thecomparison between the results of Mills (ibid., 2,435, and 3, 366) andHub1 (Abstr., 1884, 1435), the author has multiplied the bromineabsorptions obtained by Mills by -, so as to obtain the equivalentiodine absorptions, and has compared the results with * the experi-mental numbers for iodine absorptions obtained by Hiibl.Thefigures which are tabulated in the original paper indicate that thedrying oils (containing linoleic acid) assimilate the largest proportionsof the haloyds, alzd their capacity in this respect might probably beemployed as a measure of their drying properties. The fish liver oils,however, fully eqiial the vegetable oils in their assimilating power forhaloids. Hiibl's results in the main confirm those of Mills.1278ANALYTICAL CHEJlIST RY. 89Va7enfa’s Acetic Acid Test.-The author has tried this method(Abstr., 1884, 1018) on a number of oils and finds that a slightvariation in the strength or proportion of the acid employed is not ofimportance, and that the temperature at which turbidity occurs withany particular specimen is readily observed and fairly constant.Concordant results have also been obtained from several samples ofbutter, and it appears probable that further experience may prove themethod to afford a simple means of distinguishing butter frombut terin e.Deferininnfion of Glycerol.-The difficulties attending the deter-mitiation of the glycerol produced by the saponification of fixed oilshave recently been orercome by a method originally suggested byW a n k l p and Pox (Abstr, 1886, 395), and perfected by Benediktand Zsigmondy.It depends on the saponification of the oil, andoxidation of the glycerol thus formed by potassium permanganate inalkaline solution, with formation of oxalic acid, carbonic anhydride,and water.The excess of permanganate is then destroyed by asdphite, the solution filtered, the filtrate acidified with acetic acid,and pmcipitated with a calcium salt. As the precipitate containscalcium sulphate and silicic acid in addition to calciuni oxalate, theamourit of oxalic acid is determined either by titration of the pre-cipitate with permnnganate in acid solution, or by estimating thealkalinity of the ignited precipitate. For the determination ofglycerol in fats, the author recomniends modifying the method in thejollowing manner :-5 grams of the sample of fixed oil is placed ina six-ounce bottle, together with a solution of 2 grams of causticpotrsh in 12 C.C. of water. The bottle is secnrely closed and heatedin a water-oven or in boiling water for 8 or 10 hours, the contentsbeing frequently agitated.When the product is perfectly homo-geneous and all oily globules have disappeared, tbe bottle is opened,and the soap diluted with hot water, when a perfectly clear solutionshould be obtained, except in cases of sperm oil, wax, and other sub-stances yielding insoluble alcohols on saponification. The soap solutionis then treated with a moderate excess of acid in the usual way, andthe liberated fatty acids are separated from the aqueous liquid con-taining the glycerol, ahich latter is then ready for oxidation witha1 kaline permanganate as above described.By C. J. ELLIS (J. SOC. Chenz. Id., 5,150-152 and 361-362).-The author has made some experimentswith the view of extending the application of Maumenk’s test to dryingoils and fish oils, to which it caniiot be directly applied without someslight modification, owing to the violent action which ensues whenthese oils are mixed with concentrated sulphuric acid.To overcomethis difficulty i t was found necessary to mix with a drying or fish oilsome liquid which will moderate the action of the acid on the oil.The author employed a mineral lubricatiiig oil of 0.915 sp. gr. forthis purpose, and as on mixing sulphuric acid with such an oil acertain increase of temperature takes place, it is necessary to deter-mine the rise due to each gram of the mineral oil. To accelerate theaction of sulphuric acid on the mineral oil, a certain proportion ofI).B.Maumen6’s Test for Oils90 ABSTRACTS OF CHEMICAL PAPERS.colza oil was added, for which the standard number, when not mixed,was accurately determined and found to be 35.8”. Contrary to ex-pectation, it was found that the smaller the quantity of mineral oil iiithe mixture the greater is the value representing the rise due to eachgram of the mineral oil, providing the rise due t o each gram of thevegetable oil remains constant whatever the mixture. To calculatethe rise in temperature due to each gram of the mineral oil thefollowing formula is employed :--y = a + bz, iii which -y representsthe rise in tempeiature due to each gram of mineral oil, x is thefraction of the mixture coiisisting of mineral oil, and cc and b areconstants depending on the conditions of the experiment and theparticular mineral oil employed.In order to obtain the most concordant and trustworthy results, themaximum temperature attained should not exceed 60”, and it is forthis reason that the author prefers the use of a, mineral oil as the re-tarding reagent.D. B.Employment of Congo-red in Titrating Aniline. By P.JULIUS (C‘hein. I d , 9, 109-110).-CCongo-red, the compound oftetrazodiphenyl with naphtholsnlphonic acids, is turned blue by acids,and recovers its red colour with an excess of alkali. When used asan indicator i n titrating aniline or its homologues with a mineralacid, the point is taken at which a bluish-violet, not changed bysmall further additions OE acid, is produced. A much larger excess isrequired to produce a pure blue.The results do not vary more than0.2 per cent. from the theoretical numbers.Hufner’s Method of Estimating Urea. Ry E. PFL~GER andK. BOHLAND (P’cger’s Archiv, 39, l-l7).-Pfliiger and Schenk pre-viously proved (ibid., 38, 385) that Hiifner’s method of estimatingthe nitrogen in urine gave results which were too low and variable tofound a calculation of the total nitrogen on. Owing to the improve-ment made in Bunsen’s method, the authors have been able toascertain whether Hufner’s method was sufficiently accurate for thedetermination of urea only. They find that the results are alwaystoo high and also very variable. The variatipn ranges from 1 percent. to 10 per cent., and does not therefore admit of compensation.J.P. L.M. J. S.Estimation of Urea in Human Urine with Sodium Hypo-bromite. By E. PFL~~GER and K. BOHLAND (Pfliiger’s Archiv, 39,143-158) .-Pfluger’s new method of estimating urea by hypobromite(PJliiger’s rlrchiv, 38, 503) can be applied to the estimation of urea inliunian urine provided the nitrogenous extractives are first removed.J?or this purpose, a given volume of urine acidified with hydrochloricacid (1 of acid to 10 of urine) is precipitated with sufficient phospho-tungstic acid to ensure the separation of all the extractives, themixture made up to a known volume, and allowed to remain 24 hoursa t least previous to filtration. The acid filtrate is carefully neutralisedwith powdered lime, and again filtered through a dry filter.Great stress is laid on the use of pure soda and bromine for thASALPTICAL CHEJIISTRT.91preparation of the hypobromite.of urine by this process was + 1.3 per cent.The mean error of several analysesJ. P. L.Qualitative Tests for the Dyes Found in Commerce. By 9.N. WITT (Chem. Ind., 9, 1--7).-A table of reactions for the identi-fication of about 80 artificial colouring matters taken singly. Manycommercial dyes are mixtures : in this case, the powder strewn uponwet filter-paper or colourless sulphuric acid will generally givestreaks of more than on6 colour. Where the mixture is more intimatea solution must be made, and the colouring matters withdrawn frac-tionally by dyeing small pellets of wool or silk in it. The principaladulterant for azo-dyes is sodium sulphate.It is best detected afterprecipitating tlie colour by pure sodium chloride. M. J. S.Detection of Artificially Coloured Red Wine (Clarat). By J.HERZ (Chem. Zeit., 10, 968-969 ; 998).-To 30-50 C.C. of the wine,or if the quantity of colouring matter in the wine is small, 100 C.C.concentrated to 30 c.c., 20-30 C.C. of a saturated solution of magne-sium sulphate, and 10-20 C.C. of soda solution are added, stirringwell; if necessary the treatment is repeated until the liquid iscolourless, or nearly so. The filtrate is made acid with dilut,e sul-phuric acid (1 : 3), and if sulphonic acid colours are present the redcolour reappears. The most commonly used member of this group,acid-magenta (rosanilinesulphonic acid), yields a, violet-red solution,and can be estimated by comparing the tint with magenta solutionsof known strength.One mgram. of magenta per litre can be distinctlydetected in 30 C.C. of wine without previous concentration. Whenarchil (orseille) colours are present, the filtrate is bluish, and whenmade acid turns a litmus-red colour. To test for magenta under suchcircumstances, Blarez’ method of shaking with lead dioxide is used ;$his destroys the orseille and natural colour. Cazeneuve’s method isnot recommended. To test for other colours in the magnesiumhydroxide precipitate, the gelatinous mass is stirred up with hotwater, allowed to settle, and the liquid decanted off. I f only thenatural colour of the wine is present, or bilberry has been used, thisliquid is yellow-brown ; if archil has been used, dark-violet,; ifyonceau, onion or ponceau red ; if casskshe, pale-red or dark-yellow ;if cinicoline bcrdelaise, a yellow-red to yellow-brown liquid, whichwhen poured on sulphuric acid gives a violet ring. By shaking thecoloured liquid with ainyl alcohol, Tonceau yields an onion-red residue ;vinicoline, a dark-brown one ; ccmwsine, a dirt-y-green, violet at theedge, turned yellow by strong hydrochloric acid. The precipitate isa dark-grey or brownish-grey colour when the natural or vegetablecolours only are present; with archil, it is violet; with magenta(acid o r ordinary), dirty white ; with cassissine, dirty yellow-brown ;with vinicoline, crimson-red. The precipitate is mixed with sand,dried, and extracted with ether ; the extract contains any ordinarymagenta which can be identified in the usual manner by dyeing wool,or cassissine which dyes wool red-brown and leaves a yellow-brownresidue in the dish. The dyed wool becomes yellow when treatedwith strong hydrochloric acid and colourless with ammonia. Whe92 ABSIL’RACTS OF CHEMICAL PAPERS.wine is shaken with amyl alcohol, and the coloured extract evaporated,the residue, if it contains tho gubstances named, behaves in themanner described below :-Wilh concentmtedc-A 7H:S0,. HCI. NaHO.Archil . . . . . . . . violet-red bl ue red bl 11 eBordeaux, B.. . . oarmine carmine carmine carminePonceau, RRR.. dark-red crimson crimson brownCassissirie.. . . . . violet-purple yellow yellow- redVinicoline Bor-browndelaise . . . . . . cherry-red brown red brownwhilst the wine after extraction i~ cherry-red with ordinary maqefcta,violet-red with acihmngenfu, dark-cherry with Bordeam, yellow-redwith p o i z c m ~ . Wine coloured with magenta produces a violet froth.The detection of vegetable colouring matters in presence of the naturalcolour of wine or otherwise is a matter of great difficultg, and mostof the known metliods are ineffectual ; it is, however, effected by theauthorwith comparative facility in the following manner :-I0 15 C.C.of wine is shaken with 5 C.C. of a saturated solutiop of tartar emetic,and then examined by reflected and transmitted light either a t onceor, if no immediate chanqe has taken place, after some time. Thistreatmelit produces with genuine red wine always a cherry. red colour,and with other substances as follows :-Red-poppy (Papaver r?iwus),dark cherry-red ; cherry, violet : commercial elder colonring matter,Ed-violet ; hilberry (Vaccin. niyrtill), blue-violet ; priret-berry, piireviolet. White wines artificially colonred, and red wines mixed withartificial colours have been successfully examined in this manner ; inthe latter case the wine some time after treatment is compared with agenuine red wine to distinguish more readily the change of colour.Old solutions of privet do not give the d o u r change. Sodiumhydrogen carbonate produces with pure wine, brown-red ; with winecoloured with pure eldedwry, grey-violet ; and with hilberry, brown-green. Tartar emetic appcars to form an antimony lake with thocolouring matters. With practice, all the above-mentioned coloum cartbe detected in 30-50 C.C. of wine. In the subsequent communication(loc. cit., 998), the author acknowledges the priority of Ambiihl andElsner’s recommendation of the use of tartar emetic for the purposein question. They, homver, recommend hot solutJions ; the authorfinds cold better. Fermented bilberries give the violet colour evenbetter than unfermented berries, especially when fresh, innsrriuch asoxidation interl’eree with t,he delicacy after a time. The distinctnessof this colour is increased by diluting the wine. D. A. L

ISSN:0368-1769    

DOI:10.1039/CA8875200078

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

93 General and Physical Chemistry. Chemical Changes produced by Sunlight. By E. DUCLAUX (Compt. rend., 103, 881-882).-Many organic compounds are affected hy solar radiation in the same way as by microbes, the products of the change being water and carbonic anhydride, with other substances which are relatively stable in the conditions under which tEey are produced, and are identical with the products of the action of microbes. Cane-sugar in neutral or alkaline solution is not affected by pro- longed exposure to sunlight, but if slightly acidified even with an organic acid it is readily inverted by solar radiation. The solution of invert sugar undergoes no further change so long as it remains acid, but if made alkaline the glucose is rapidly decomposed with formation of water, carbonic anhydride, oxalic, formic, and acetic acids, and about 3 per cent. of alcohol.A similar change takes place, although less rapidly, out of contact with the air, and hence it is evident that the decomposition is due to internal combustion. Lactose and lactates also yield alcohol under similar conditions. The exact nature of the change in any case is modified by the nature’ of the source from which oxygen is absorbed (air, salts of platinum, gold, mercury) ; but the chief products are practically the same from all substances. These products are alcohol, oxalic acid, acids of the acetic series, leucine, carbamide, carbonic anhydride, water, &c. Certain differences are, however, observed. Tartaric acid gives aldehyde in place of alcohol, and the alcohols, if oxidation is regular, tend to produce the corresponding acid of the acetic series.Practical Methods of Photographing the Spectrum. By J. M. EDER (Monatsh. Chem., 7 , 429-454) .-This paper .contains a description of some practical methods of photographing the various parts of the spectrum by silver bromide gelatin plates sensitised by different dyes. The preparation of the plates and the processes used for the development are described in full, and accompanied by copies of photographs taken. For spectra from the ultra-violet to the yellow, about D, the best dyes are erythrosin, henzopurpurin 4B, and yuinoline-red ; from the ultra-violet to the red cyanin, is the best ; from the orange to the red, ccerulein with red glass, and “sensitive green,” R dye from para- hydroxybenzaldehyde and dimethylaniline, are recommended.These plates, sensitive to the green, yellow, or red part of the spectrum, are suitable for photography by petroleum and gas light, and for taking photographs of gilded documents and papyri, of microscopic prepam- tions. and of clouds on a blue sky, interposing yellow glass to subdue the blue. Excellent photographs of stars have been taken with tha C. H. B. aid of these plates. v. H. v. VOL. LII. h94 ABSTRACTS OF CHEMICAL PAPERS. Electrolysis Of Carbon Compounds. By .T. HABERhIANN (Monntslz. Chem., 7, 529-551).-1n continuation of former experi- ments on the electrolysis of carbon compounds (Abstr., 1881,215), the author describes the resalts which are obtained under various con- ditions with alcohol acidified with sulphnric acid, or rendered alkaline by soda, and with potassium acetate dissolved in methyl alcohol or its homologues.The sources of electrical energy used were a thermo- battery of 120 elements, a Smee’s battery of 16 elements, and a dynamo- machine of one horse-power. On electrolysis, alcohol acidified with sulphnric acid yields hydrogen evolved as gas at the negative pole, aldehyde, and after prolonged action aldehyde-resin together with ethyl hydrogen sulphate. The main reaction is therefore C2H,0 = C2H40 + H,. If the alcohol is rendered alkaline, or is in the form of sodium ethoxide, the products of decom- position are hydrogen, carbonic anhydride as sodium carbonate, an aldehyde-resin insoluble in ether and alcohol, together with a soluble modification, and a subshance allied to cinnamaldehyde.A concentrated solution of potassium acetate in ethyl alcohol yields a mixture of hydrogen and ethane together with potassium ethyl carbonate, by the mutual decomposition of the salt and acid. In fact, the process serves as a convenient method for the preparation of potassium ethyl carbonate in large quantities, as the salt separates in fine crystalline aggregates. It is quickly decomposed by water, but dissolves in absolute alcohol without change. The results obtained with solutions of potassium acetate in methyl and butyl alcohols were unsatisfactory. V. H. V. Phosphates. By BERTHELOT (Compt. rend,, 103, 911-917).- When ammonium chloride is added to a solution of trisodinm phos- phate there is an absorption of heat which varies with the proportion of ammonium chloride, being 5.96, 5.63, 4.84, and 2.62 cal. for 3, 2, 1 and 4 mols.of ammonium chloride respectively. Complete decom- pwition of the sodium phosphate would correspond with an absorption.of heat equal to -6.4 cal., and hence it is evident that t,he action of the ammonium chloride is almost complete, although the water exerts a greater dissociating effect on the ammonium pbosphate than on the sodium salt. I f trisodium phosphate is added to a solution of a magnesium, barium, strontium, calcium, or manganese salt,, a colloidal precipitate of the insoluble phosphate is at first formed, and there is considerable absorption of heat, but after some minutes the precipitate becomes crystalline and a large quantity of heat is developed.The heslts of formation of the colloidal and crystallised phosphates are given in the following table :- Colloidal. Crystallised. Magnesiuni hydrogen phosphate., 50.6 ,, 54.2 ,, Magnesium phosphate .......... 57.8 cal. 83.0 cal. Barium phosphate ............. 68.4 ,, 1008 ,, Strontium phosphate .......... 65.4 ,, 97.4 ,, Calcium phosphate 64.0 ,, - Manganw? phosphate .......... 45.8 ,, 53.5 ,, ............ 9 ,GENERAL AND PHYSICAL CHEMISTRY. 95 In the case of barium phosphate, the sodium phosphate must be added to the barium chloride, and not vice uers$, otherwise the change to the crystalline state is Loo rapid. The phenomena now described explain the discordant results obtained by Louguinine and the author for the heat of neutralisation of phosphoric acid by baryh, and also the differences observed by Blarez (this vol., p.7) between the heats of formation of barium phosphale and barium arsenate. In the case of strontium also, the change to the crystalline condition is extremely rapid, if the strontium solution is poured into that of the trisodium phosphate. Calcium phosphate was obtained only in the colloidal form. The heats of formation of the collo'idal insoluble phosphates do not differ to any great extent from the heat of formation of an equivalent quantity of trisodium phosphate, 33.6 x 2 cak. In other words, the precipitate in its initial condition corresponds clsseIy with the soluble salt from which it has been derived, a further example of the tendency of systems which are undergoing transformation to preserve their molecular type.On the other hand, the new phosphates may be dissociated by water to a greater extent than the sorubre phosphate from which they have been formed; and this dissociation ail1 be accompanied by an absorption of b a t , This absorption is practically wil with barium phosphate, which appmximates closely to the alkaline phosphates, but ib is very cfistinct wihh magnesium phosphate, which is more readily dissociated. In dissolved trisodium phosphate, the third and even the second equivalents of the base are less intimately combined with the acid than the first atom, and are partially separated from it by the dissociating action of the solvent. There can be little doubt that this imperfect state of combination also exists in- the colloidal insoluble phosphates, tlie formation of which is due b a polyalcoholic rather than an acid function of the phosphoric acid.The combination, however, soon becomes more intimate, and the alcoholic function changes to an acidic function comparable with that 04' ordinary tribasic acids, the change being accompanied by development of heat, and crystallisation of the phosphates. The actual development of heat is mnch greater than can be supposed to be due to the mere physical change from the colldidal to the crystalline condition, even if the change were accompanied by eombination with water. As a matter of fact, the erystallised phosphate contains less water than the colloidal phosphate. In their new condition, the heats of formation of the insoluble phos- phabes become practically treble that of the ordinary monophosphates, or in other words, the three acid functions become equivalent to one another, and to this change is due the greater proportion of the heat developed in the passage from ihe colloidal to the crystalline form.Heats of Neutralisation of Homologous and Isomeric Acids. By H. GAL and E. WERNER (Comyt. rend., 103, 806--809).-The author has determined the heats of neutralisation of isobutyric, isopropy la ce tic, t rime thy lace tic (pivalic) , caproic, isobu tylace tic. and sorbic acids, and his results, together with the heats of neutralisation of the lower acid8 of the acetic series, as determined by Berthelot, C. H. B. h 296 ABSTRACTS OF CHEMICAL PAPERS. Lougninine, and others, are given in the following table.Heat of solution of isobutyric acid, directly + 0973 cal., indirectly + 1.012 cal. ; isopropylacetic acid, directly + 1.167, indirectly + 1.030. Heat of Acid. neutralisation. Formic acid, H-COOH ........................ 13.3 Acetic acid, MeGOOH ........................ 13.4 Propionic acid, CH,Me*COOH .................. 14.3 Normal butyric acid, CHF,Me*CH2*COOH ........ 14.4 Isobutyric acid, CHMe,*COOH. ................. 13.9 Normal valeric acid, CH2Me*CR2*CH,*COOH.. .... 14.4 Tsopropylacetic acid, C HMe2*C H2* C 0 OH ......... 14.4 T rime thylace tic acid, CMe3*COOH .............. 13.6 74 Normal caproic acid, CH,Me*CH,*CH,*UH,*COOH . 14.689 Isobu tylilcetic acid, CHMe,*CH,*C 0 OH 14-5 i .......... { Omitting formic and acetic acids, the heat of neutralisation of the other acids, with the exception,of isobutyric and trimethylacetic acids, is practically constant, and varies between 14.3 and 14.6.Isobutyric acid is a secondary acid, and trimethylacetic acid is ft tertia1.y acid, and it would seem therefore that the heat of neutralisation of primary acids is greater than that of secondary acids, whilst that of tertiary acids is somewhat smaller atill. The heat of neutralisation of sorbic acid, which is regarded by Menschutkin as a tertiary acid, is 12.945. C. H. B. Heats of Neutralisation of Malonic, Tartronic, and Malic Acids. By H. GAL and E. WERNER (Compt. rend., 103, 871-873) .- MaZonic Acid.-Heat of solution at 10° = -4.573 cal. Heat of neutralisation by soda : 1st equivalent, 13.342 cal, ; 2nd equivalent, 13.778 cal.; total, 27.120 cal. Heat of neutralisation by soda : l e t equivalent, 13.71 1 cal. ; 2nd equivalent, 11.856 cal. ; 3rd equivalent, 0 0 cal. ; total, 25.567. Mulic Acid.-Heat of solution at 20" = -3,148 cal. Heat o€ neutralisation by soda : 1st equivalent, 12.730 cal. ; 2nd equivalent,, 12.189 cal. ; 3rd equivalent, 0.0 cal. ; total, 24.919. The heat of neutralisation of oxalic acid is 28.1 cal. (Berthelot and Thomsen) ; of succinic acid, 26.4 csl. (Chroutschoff) ; and tartaric acid, 25.3 cal. (Berthelot). I t is evident from these values that the heat of neiitralisation diminishes as the molecular weight increases. The intzodnction of the OH group into oxalic, malonic, and succinic acids lowers the heat of neutrdisation by about 2 cal. A similar difference has previouely been observed between propionic and lactic acids, and between benzoic and the hydroxybenzoic acids.Themnochemistry of Reactions between Magnesium Salts and Ammonia. By BERCHELOT (Compt. rend., 103, 844-848) .- When magnesium sulphate solution is mixed with an equivalent quantity of sodium hydroxide solution, there is an immediate develop-, Tartronic Acid.-Heat of solution at 12" = -4.331 cal. C. H. B.GENERAL Ah'l) PHYSICAL CWMBTRY. 97 ment of +0*18 cal., but the development of heat gradually slackma, and at the end of 10 minutes is + 1-14 cal. ThB successive develop- ments of heat are due to the fact that a basic srtlt is first formed, which is afterwards decomposed by the soda, and also to the hydra- tion, contraction, $c., of .the precipitate.Magnesium chloride m d sodium hydroxide behave in like manner. At first there is an absorp- +ion of -0.32 cal., and afterwards a development of 44-32 cal., the final result being nil. It is evident, &s the reseamhes of Thomsen, Favre and Silbermann, Ditjte, and othere have already indicated, that the heat developed by the action of acids on magnesium hydroxide approximates closely to thttt developed by their action on potash and soda. The action of ammonia on magnesium sulphate is accompanied by an absorption of -0.24 cal., whereas if the magnesium were com- pletely displaced, 3.0 cal. should be absorbed. The difference is due to the formation of double salts or oxides, the production of which is accompanied by a development of + 2.8, cal.With magnesium chlo- ride, the difference between the calculated and observed values is +2.2 cal. If magnesium sulphate is mixed with 2 mols. of ammonium chloride, +0.32 cal. is developed, and if an equivalent quantity of ammonia i q now added, there is a further development of +0.26 cal., the total de- velopment of +0*58 cal. being due to the formation of a complex oxide, the heat of neutralisation of which is 0.33 cal. higher than the sum of the heats of neutralisation of magnesium oxide and ammonia separate1.v. When magnesium chloride is mixed with ammonia, there is an absorption of -0.48 cal., and if ammonium chloride is then added there is a, development of +0*56 cal., the sum being 0.08 cd., from which it followa that the heat of neutralisation of the complex oxide by hydrochloric acid is practically identical with that of magne- aium oxide, If magnesium sulphabe OF chloride solution is mixed with sodinin hydroxide, and ammonk then added, the greater part of the precipi- tate redissolves, but there k no sensible $herma1 disturbance, a result which indicates that the heat of solution of the precipitate is idenfical with its heat of combination with the solvent. If, oa the other hand, magnesium sulphafe i s first mixed with ammonia, md the sodium hydroxide added afterwards, there is a development, a€ +Is90 cal., probably due to the facf that, the order *of admixture being reversed, the liquid requires a much longer time to attain the same condition.The differenee betweert the observed thermal d i s t n r b c e and the de- mb ment of heat resulting fmni the action of soda or magnesium mlp!ka alone ia a, fnrther proof of the formation of complex corn- peunds.I f magnesium snlphate is mixed with 2 mals. of ammonium chlo- ride and sodium hydroxide then added, +3.64 cal. are developed, and some permanent precipitate is formed. The thermal disturbance is greater than that which would colrwpond with the displacement of ammonium by sodium, rtnd the difference indicah the cornbination of magnesia and a;mmonia with formation of ammonio-magnesium sul- phate. If 4 mols. of ammonium chloride fire added at the begia-9s ABSTRACTS OF CHEMICAL PAPERS, ning, no precipitate is formed, and the heat developed is +3.90 cal. JVith magnesium sulphate, the excess of heat developed above that corresponding with the decomposition of the ammonium salt is + 1.2 cal., with the chloride it is +1*0 cal. From these results it follows that the complex ammonio-magnesium bases in uniting with sulphuric or hydrochloric acid, develop about + 1.8 cal.more than pure ammonia, and + 0.3 cal. mow. than magne- sium oxide. The association of ammonia with a metallic oxide such as magnesia would seem to result in the production of a complex alkali analogous to tetramethylammonium oxide, with an energy greater than that of metallic oxides, and approaching +ha& of the strongest alkalis. C. H. B. Heats of Combustion and Formatiun mf Homologous Phe- nols. By 3’. STOHMAKN, P. RODATZ, and H. HERZBERU (J. pr. Chem. [2], 34, 311-327).-1n this paper a series of determinations of the heats of combustion and formation of the homologous series of phenols are given in detail, as also their heats of liquefaction.The principal values obtained m e given in the following table :- Heat of combustion per gram-molecule. Phend (did), C,H,-OH. ..... .- .. 723659 Orhhocresol (liquid), CsH4Me-OH. .. 883008 Mehcresol (liquid) .............. 880956 Paracresol ................ 882900 Orcinol, C6H,Me(OH), (solid). ..... 824724 Orthoxylenol, C6H3.%fe2*OH (solid). . 1035434 Mehxylenol (liquid). ............. 1037499 9 araxylenol (solid) ........ -. ..... 1035638 Fseudocumenol, CBH,Me,-OH (solid) 119145 1 Carvacrol, CGH3MePr*OH (liquid). . 1354819 Thymol (liquid). ................. 1353750 .. (liquid) ................. 726002 ..(solid). ............. 879788 .. (solid) .............. 880441 .. (solid) .................. 1348982 Heat of formation. - 50992 53044 51100 109276 61566 5950 1 61362 68549 68181 69250 - - On a comparison of these numbers, it will be seen that every dis- g!acement of hydrogen bp a methyl-group corresponds with an incre- inent of 155356 cal. in the heat of combustion, a value praotically equal ta that obtained for the homologues oE methyl alcohol. Thus it follows that the displacement of‘ hydrogen by methyl, either in the so-called side-chain or i n the nucleus, corresponds with the same value for the heat-increment. Thus the value for ethylphenol will be equal t o that of xylenol. Similarly also, as the d u e s for carvacrol and thymol are approximately equal to that of pseudocumenol, namely, the introduction of the isopropyl-group produces the same effect as that of three single methyJ groups, then the heat values of the iso- are equal to those of normal-compounds.V. H. V.GENERAL AND PHYSICAL CHEIIISTKT. 99 Some Laws of Chemical Combination. By DE LANDERO and R. P R r E n , (Conzpt. rend., 103,934-935).-1f chemical combination is taken as the clashing together of the particles of the elements, and if each particle is regarded as possessing a constant velocity which is characteristic of the pctrticular element, the loss of energy resulting from the union of the non-elastic particles may be regarded as the equivalent of the quantity of heat developed by the combination. These considerations lead to the formula- (V + T q 2 , ee' = 2(a + e') in whichf = the heat of Combination expressed in calories, e, e' = the weights of the combining elements epuivaient to 1 gram of hydrogen, whilst V and V' are quantities which a m constant for each element and are proportional to the velocities of their particles.These quan- tities may be termed thermodynamic constants, or thermodynamic cquivdeuts, and their value is obtained by the €ormula- 9 * v'=y/2f--,,. e + e' Take the ease of the two copper bromida- Cuprous bromide: e + e' = 143.4; f = 25900 Cupric bromide: e + e' = 111.7; f = 17300 - + 38.269 cal.; V + V' = cal; v * V' = - + 39'039. Calculations with t i n bromides, mercury bromides, mercury iodides, &c., lead to similar results. Since V Ifi V' is the sum or difference of the thermodynamical equivalents of the two elements in each system ; i t is necessary to obtain the consfants of some of the elements from different sets of compounds, care being taken to use only thermo- chemical data referred to the solid state. The following table gives the thermodynamical equivalents of several elements, these values re- ferring in each case to that quantity of the element which is equivalent to 1 gram of hydrogen:- K ......45221 S ...... 47.874 A1 ...... 48.218 Nu.. .... 49.768 T1 ...... 5.223 Zn.. .... 13.073 Hg.. .... 9.079 Ag .... 12.i86 Bb ...... 5.155 B r . . .... 44.171 Cu .... 4.999 Si ...... 37.519 I ....... 32.416 Ca, ..... 50.309 C. H. B. The Law of Volumes in Chemistry. By T, S. HUNT (Chem. News, 54,206-207) .-The author advocates the universal application of the law of volumes to solids, liquids, and gases, which would render the application of the atomic hypothesis to explain the law of definite proportions wholly unnecessary.From this standpoint, the union of many volumes of vapour or gas to form a single volume of vapour or solid would be regarded as chemical combination; the reverse, namely raporisation, would be chemical decomposition, which wonld be without specific difference in the case of integral volatilisation, or100 ABSTRACTS OF CHEMICAL PAPERS. with definite changes, as in cases now regarded as dissociation. The difference between chemical and physical molecules would hence be quite evident. D. A. L. Velocity of Dissociation. By H. LESCCEUR (Compt. rend., 103, 931-933) .-The velocity of dissociation of acid sodium acetate, CzH,0zNa,2CzH40,, was determined by placing the compound in a small bell-jar which also contained soda-lime ; the temperature of the whole being kept a t 100".The mean velocity of dissociation during k i given interval is determined by dividing the time into the loss of weight of the compound. The results indicate the existence of a biacetate, CZH,O2Na,C2H1O2, and a sesquiacetate, 2C2H,02Na + Velocity of dissociation does not depend on the temperature alone, as Miiller-Erzbach siipposes, but also on the physical condition of the substance which is undergoing dissociation. In this particular case, the rate of dissociation increased fourfold when the acetate becttme solid, although the tension of dissociation did not change, and similar phenomena are observed with copper sulphate crystals, &c.CzHaOz. C. H. B. Nature of Liquids. By W. RAMSAY and S. YOUNG (Ohm. News, 54, 203-205).-1t is proved by various investigations that, above a eertain pressure and temperature, all liquids show an increase in the density of their saturated vapours beyond that deducible from the molecular formula, varying of course with the liquid. Some liquids, however, known to be dissociable, in addition show an increase also on fall of temperature and pressure below a certain tem- perature and pressure characteristic of the liquid. Reasoning from these facts, the following difference is suggested between stable and dissociable liquids :-In the former, the molecules exhibit physical but not chemical attraction ; in the latter both pliysical and chernical attraction are evident, inasmuch as, besides cohesion and surface ten- sion, there is evidence of molecular combination.The behaviour of .vapours at the moment the liquid is visible support this theory, for whereas vapours from dissociable liquids continue to rise in pressure i n spite of the decrease in volume and condensation of liquid (evidence of non-homogeneity of the vapour, owing in these instances to forma- tion of molecules of higher molecular weight), vapours from stable liquids do not behave in this manner, but the pressure in such case is the vapour-pressure corresponding with the temperature ; hence it may be concluded that the latter show no tendency to form complex molecular groups. With regard to the solvent action of a fluid above its critical point, the authors have worked with a solution of eosin in alcohol, taking the fluorescence as indicating solution.They find that solution existed at least for a short time at temperatures a little above the critical point, and at volumes smaller than the critical volume ; apparently, however, after some time the solid is wholly deposited as such on the walls of the tube. This is not conclusive, as the translucent red sub- starice deposited on the glass interfered with the detection of the fluorescence. According to the authors' view of the nature of liquids,GENERAL AND PH Y STCAL CHEMISTRY. 101 solution should be possible above the critical point provided the volume is sufficiently small. D. A.L. Capillary Constants and Meniscus Angle. By J. TKAUBE (J. pr. C'he?n. [2], 34, 292--31l).--l)eterminations are given for the value of the function a' cos 8 according to the formula rh = a2 cos 0, for aqueous solutions of. the alcohols of the paraffinoid series and acids of the acetic series at various degrees of concentration (comp. Abstr., 1885, 1033). The principal points to be noticed are that both propyl and isopropyl alcohols show a minimum value for tho function with mixtures of equal weights of the alcohol with water, and that the eurve for butyric acid at first decreases with increase of concentration up to 30 per cent., thence increases up to 50 per cent., and sub- sequently decreases. After a historical review of the literature on the magnitude of drops, an account is given of experiments, made with an apparatus previously described, permitting of the formation of drops from a capillary tube under constant or variable conditions of temperature and pressure.The weight of the drops was ascertained by deter- minations of the specific gravity and the number of drops in a constant volume. The results obtained with the above-mentioned alcohols and acids show that the volume of the drops is proportioual to the rise in height in the ca~illary tube, or their weight is proportiwrd to the product oj' the height and the specijiic gravzty. If then the mean weight of the drop is divided by the circumference -, then for all liquids examined this quotient is less than the capillary constant a cos0, and secondly this qnotient increases with decrease of radius of the tube.Both these statements are deducible from the previous observations of Hagen and Quincke. Again the diameter of the capillary tube determines the shape of the drop; thus with tubes of less than 3 4 mm. their form is more or leas spheroidal, with tubes of 1 mm. the form is cylindrical with a convex base, and with tubes of larger diameter it is para- boidal . V. H. V. C 2 r r Crystallisation by Diffusion. By C . E. GUIGNET (Compt. rend., 303, 8iS--875).-The experiments described in this paper are an extension of Becquerel's researches on electro-capillary reactions. The introduction of any solid into a saturated solution of another solid determines the crystallisation of the latter, provided that the solid introduced is soluble in the particular solvent.For example, solid paraffin introduced into a saturated solution of sulphur in carbon bisulphide causes the separation of crystals of sulphur, and vice versd ; sodium thiosulphate introduced into a saturated solution of ammonio-cupric sulphate yields violet needles of ammonio-cupric thiosulphate. If crystals of sodium sulphate are placed in a saturated solution of barium chloride, the crystals become opaque but retain their form, aud when the crystals are broken each one is found to be a sort of102 ABSTRACTS OF CIIEMICAL PAPERS. miniature lode with crystals of barium sulphate. Barium chloride iiitroduced into a saturated solution of sodium sulphate yields only amorphous barium sulphate, probably because the chloride dissolves too quickly.Ordinary sodium phosphate placed in magnesium sulphate solution produces crystallised magnesium phosphate. Ia order to observe these phenomena with two liquids, if the action is merely physical, a saturated solution of a solid is covered with a layer of the solvent, and on this is poured a second liquid in which the solid is somewhat less soluble than in the first. The liquids gradually mix by diffusion, and the solid separates in very distinct crystals. If a saturated solution of sulphur in carbon bisalphide is covered with a layer of the bisulphide, and on this is poured a layer of oil, alcohol, glacial acetic acid, benzene, petroleum, &c., octahedral crystals of sulphur are deposited. A saturated solution of lead chloride in hydrochloric acid covered in a similar manner with a layer of hydrochloric acid and a layer of water, yields fine crystals of lead chloride.Where chemical action takes place between the liquids, one is placed in a crgstallising dish which is 6lled nearly i~ the top, and this is placed inside another vessel which contains the second liquid. Water is then carefully poured into both dishes until it is just higher than the edge of the inner dish. Diffusion takes place through the super- natant water, and crystals are formed. Sodium snlphate and calcium chloride give long crystals of calcium sulphate ; sodium sulphate and barium chloride give crystallised barium sulphate ; sodium sulphate and lead acetate give crystals of lead sulphate ; and potassium ferro- cyanide and lead acetate yield long pale-yellow needles of lead ferro- cyanide.On a large scale, wooden vessels with a leaden partition which does not quite reach to the top are used. The liquids are poured one into each compartment, and &he latter are then tilled up with water until the water just, flows over the top of the partition. In this way very large crystals can be obtained. Influence of some Normal Salts on the Decomposition of Methyl Acetate by Hydrochloric and Sulphuric Acids. By H. TREY (J. pr. Chenz. [2], 34, 353--377).-Ostwald investigated (J. pr. Chem. [2], 23, 209) the difference in the action of acids caused by the presence of their normal salts; the author has repeated these experiments with a view to obtaining a satisfactory explanation of t h i s action. Tbe experiments were made with hydrochloric and sulphuric acids, and the salts of these acids with the alkalis and alkaline earths.The methyl acebate method was used, in the manner previously described, with normal acids ( I gram-equivalent in 1 litre) and normal acids to which 4, 4, 1, &c., equivalents of their normal salts had been added. These normal solutions were also used 29, 5, and l2g times diluted. The results were calculated according to the formulse given by Ostwald (this Journal, 1884, SSl), and are given in a series of tables. These values are not strictly comparable, but require correcting for the increase of volume caused by the addition of salt and the consequent decrease of the velocity of the reaction. The C. H. B.GENERAL AND PHYSICAL CHEMISTRY.103 mean values found are given below; the second line in each case gi yes the corrected value. 1.121 1.049 1.032 Normal . . . . . 1 - normal .. Z L 6 normal.. . . 1 - normal . . 12+ --- 1.426 1,167 1.005 Hydrochloric Acid and Alkaline Chlorides. 1 - normal . . 2 i 32 -76 32.87 11 -75 11 *82 6 -61 5 -68 2 -23 2 -24 1.000 HC1 (1 litre) t lNaCl 1 - normal. . 12.1- 36 -87 37 *49 12 '27 12 -35 5 -75 5 t85 2 -20 2 -24 1 .OOO HC1 (1 litre) t 4NaCl -- 52 -87 57 '62 13 -88 14 *88 6 -09 6 -64 2 *15 2 -34 - HCl :1 litre) + tKcL 31 -89 32 -16 11 -73 11 -83 5 *63 6-67 2 -21 2 -22 - - HCl (1 litre) + lKC1. 34 -66 35 -05 11 -89 12 -26 5 -63 5 -80 2 -15 2 -22 HCl (1 litre) + 3KU1. 40.83 44 -60 12-45 13 *64 5 -60 6 -14 2 '10 2 *30 -- Calculating the ratio in which the velocity of action of the hydro- chloric arcid is increased %y the addition of the &ove salts, the following numbers are obtained :- (1 litre).I + normal.. . . I 1 -000 - HCl (1 litre) + +N&l. 1 051 1.011 1.011 1.009 - HC1 (1 litre) + lNaCl --- 1 0199 1 -056 1 -041 1 -009 HCl (1 litre) + 4A aC1 1 '843 1 a73 1 -181 1-054 - HC1 (l. litre) + tKCl 1 *028 1 -012 1 -009 1 -000 HCl (1 litre) + 1KC1. HCl (1 litre) + 3KC1. For the stronger solutions, the increase of the action of the hydro- chloric acid is proportional to the amount of salt present; for the weaker solutions, the increase is so small as to fall within the errors of experiment. Hydrochloric acid and lithium, magnesium, calcium, strontium, and barium chlorides, gave the followiog numbers :-104 ABSTRACTS OF CHEMICAL PAPERS.Normal . . . . . + normal.. . . -- Normal .. . . 4 normal.. . . 1 *OOd 1 *961 1 '000 1 *146 56 *83 61.31 5 -97 6 -44 1.985 1.171 HCl (1 litre) + BMgCl,. 1.409 1.080 66 -56 69 -26 6 '33 6-59 HC1 (1 litre) + 2CaC1. -- 59 -43 62 *69 6 -24 6 5 6 HC1 (1 litre) + 2SrC1,. 68 *55 62 -06 6.20 6 -58 HC1 (1 litre) + 1BnC1,. 42 -46 44 -07 5 *84 6 -07 -- These numbers gave the following ratios for the accelerating action of the salts :- HC1 (1 litre) + 2MgC1,. HC1 (1 litre) + 2UaCI. HC1 HC1 (1 litre) (1 litre) + 2SrClj. + lBaCI,. 2 -215 1.173 2 *005 1 -167 From these results the author concludes that the accelerative influence of the chlorides stands in the inversive ratio to the atomic weights of the respective series. Thus, calculated for 1 equivalent of chloride, the numbers are :- .~ LiC1. 1 NaCl.1 KCE. 1 MgCk. 1- CaC1,. 1 SrC1,. 1 BaCIJ. 1.240 1 1.199 1 1.121 I 1.304 I 1.251 1 1.246 I 1.205 These results agree with those found by Reicher (Abstr, 1885, The action of eulphnric acid in the presence of normal salphates is The action is retarded to 1 equivalent salt, but in a less degree The following tables give the mean values for 1034) for the saponification of ethyl acetate by alkalis. the reverse of that of hydrochloric acid. nearly proportionally with with 2 equivalents. normal and + normal solutions :-QENERAL AND PHYSICAL CEENISTRY. #IlGrmlbl - Normal. +normal 105 3 -04 2 -68 2 -16 { 3L546 3 -04 2 -69 2 -19 -- -__I_ ------ 1.000 0.885 0 -760 0 * 578 1.000 0.910 0 -805 0 -656 frH$04 (1 litre) + )MgSO,.0.787 *HaSol (1 litre) + lNGO4. I__-- 6 8s' 7 -08 1 '62 1 -67 0 -426 0 -500 -- - &SO4 (1 litre) BH2S04 (1 litre) BH,SO, (1 litre) + +LizS04. f +Na&404. + +Kfi04. 0 -620 0 -579 0 *330 -------_I_-- With aulphuric acid, the retarding influence of the sulphates on the velocity of the action appears to inorease with the atomic weight of the elements of the series, thus :- Dithionic acid in the presence of its normal salts was in- fluenced in the same way as hydrochloric acid, so also was the bibasic methylenedisulphonic acid, whilst dichloracetic acid behaved like sulphuric acid. This method of investigation will therefore throw no light on the basicity of dithionic acid, but th0 author thinks the results show that it does not form acid salts in aqneoucil solution.Preservation of Gases over Mercury. By H. B. DIXON (Chem. News, 64, 227-228).-From the author's eqepiments, it is shown that, provided due precautions are taken t o prevent the formation of' a, film between the glass and the mercury, gases may be safely preserved over mercury for a considerable time. Cracking Glass with Certainty. By E. BECKXANN (Zeit. amE. &%em., 25, 530-531).-A scratch is made with a file ; at both sides of this, pads of wetted filter-paper are wrapped round the object,, leaving a, space of a few millirnetres between them. The flame of a Bunsen or gas blowpipe is applied to this space, when the crack will be carried round from the scratch midway between the two pads. Apparatus for Chemical Laboratories. By J. WALTER (J. PT.Chem. [23, 34, 427--432).-A new form of condenser, and flasks for use with it, both for ordinary and fractional distillation. G. H. M. D. A. L. M. J. S. G. H. M.93General and Physical Chemistry.Chemical Changes produced by Sunlight. By E. DUCLAUX(Compt. rend., 103, 881-882).-Many organic compounds are affectedhy solar radiation in the same way as by microbes, the products of thechange being water and carbonic anhydride, with other substanceswhich are relatively stable in the conditions under which tEey areproduced, and are identical with the products of the action ofmicrobes.Cane-sugar in neutral or alkaline solution is not affected by pro-longed exposure to sunlight, but if slightly acidified even with anorganic acid it is readily inverted by solar radiation.The solution ofinvert sugar undergoes no further change so long as it remains acid,but if made alkaline the glucose is rapidly decomposed with formationof water, carbonic anhydride, oxalic, formic, and acetic acids, andabout 3 per cent. of alcohol. A similar change takes place, althoughless rapidly, out of contact with the air, and hence it is evident thatthe decomposition is due to internal combustion.Lactose and lactates also yield alcohol under similar conditions.The exact nature of the change in any case is modified by the nature’of the source from which oxygen is absorbed (air, salts of platinum,gold, mercury) ; but the chief products are practically the same fromall substances. These products are alcohol, oxalic acid, acids of theacetic series, leucine, carbamide, carbonic anhydride, water, &c.Certaindifferences are, however, observed. Tartaric acid gives aldehyde inplace of alcohol, and the alcohols, if oxidation is regular, tend toproduce the corresponding acid of the acetic series.Practical Methods of Photographing the Spectrum. ByJ. M. EDER (Monatsh. Chem., 7 , 429-454) .-This paper .contains adescription of some practical methods of photographing the variousparts of the spectrum by silver bromide gelatin plates sensitised bydifferent dyes. The preparation of the plates and the processes usedfor the development are described in full, and accompanied by copiesof photographs taken.For spectra from the ultra-violet to the yellow, about D, the bestdyes are erythrosin, henzopurpurin 4B, and yuinoline-red ; from theultra-violet to the red cyanin, is the best ; from the orange to the red,ccerulein with red glass, and “sensitive green,” R dye from para-hydroxybenzaldehyde and dimethylaniline, are recommended.Theseplates, sensitive to the green, yellow, or red part of the spectrum, aresuitable for photography by petroleum and gas light, and for takingphotographs of gilded documents and papyri, of microscopic prepam-tions. and of clouds on a blue sky, interposing yellow glass to subduethe blue. Excellent photographs of stars have been taken with thaC. H. B.aid of these plates. v. H. v.VOL. LII. 94 ABSTRACTS OF CHEMICAL PAPERS.Electrolysis Of Carbon Compounds. By .T. HABERhIANN(Monntslz. Chem., 7, 529-551).-1n continuation of former experi-ments on the electrolysis of carbon compounds (Abstr., 1881,215), theauthor describes the resalts which are obtained under various con-ditions with alcohol acidified with sulphnric acid, or rendered alkalineby soda, and with potassium acetate dissolved in methyl alcohol or itshomologues.The sources of electrical energy used were a thermo-battery of 120 elements, a Smee’s battery of 16 elements, and a dynamo-machine of one horse-power.On electrolysis, alcohol acidified with sulphnric acid yields hydrogenevolved as gas at the negative pole, aldehyde, and after prolonged actionaldehyde-resin together with ethyl hydrogen sulphate. The mainreaction is therefore C2H,0 = C2H40 + H,.If the alcohol is renderedalkaline, or is in the form of sodium ethoxide, the products of decom-position are hydrogen, carbonic anhydride as sodium carbonate, analdehyde-resin insoluble in ether and alcohol, together with a solublemodification, and a subshance allied to cinnamaldehyde.A concentrated solution of potassium acetate in ethyl alcohol yieldsa mixture of hydrogen and ethane together with potassium ethylcarbonate, by the mutual decomposition of the salt and acid. In fact,the process serves as a convenient method for the preparation ofpotassium ethyl carbonate in large quantities, as the salt separates infine crystalline aggregates. It is quickly decomposed by water, butdissolves in absolute alcohol without change.The results obtained with solutions of potassium acetate in methyland butyl alcohols were unsatisfactory.V. H. V.Phosphates. By BERTHELOT (Compt. rend,, 103, 911-917).-When ammonium chloride is added to a solution of trisodinm phos-phate there is an absorption of heat which varies with the proportionof ammonium chloride, being 5.96, 5.63, 4.84, and 2.62 cal. for 3, 2, 1and 4 mols. of ammonium chloride respectively. Complete decom-pwition of the sodium phosphate would correspond with anabsorption.of heat equal to -6.4 cal., and hence it is evident thatt,he action of the ammonium chloride is almost complete, although thewater exerts a greater dissociating effect on the ammonium pbosphatethan on the sodium salt.I f trisodium phosphate is added to a solution of a magnesium,barium, strontium, calcium, or manganese salt,, a colloidal precipitate ofthe insoluble phosphate is at first formed, and there is considerableabsorption of heat, but after some minutes the precipitate becomescrystalline and a large quantity of heat is developed.The heslts offormation of the colloidal and crystallised phosphates are given in thefollowing table :-Colloidal. Crystallised.Magnesiuni hydrogen phosphate., 50.6 ,, 54.2 ,,Magnesium phosphate .......... 57.8 cal. 83.0 cal.Barium phosphate ............. 68.4 ,, 1008 ,,Strontium phosphate .......... 65.4 ,, 97.4 ,,Calcium phosphate 64.0 ,, -Manganw? phosphate .......... 45.8 ,, 53.5 ,,............ 9 GENERAL AND PHYSICAL CHEMISTRY. 95In the case of barium phosphate, the sodium phosphate must beadded to the barium chloride, and not vice uers$, otherwise the changeto the crystalline state is Loo rapid.The phenomena now describedexplain the discordant results obtained by Louguinine and the authorfor the heat of neutralisation of phosphoric acid by baryh, and also thedifferences observed by Blarez (this vol., p. 7) between the heatsof formation of barium phosphale and barium arsenate. In the caseof strontium also, the change to the crystalline condition is extremelyrapid, if the strontium solution is poured into that of the trisodiumphosphate. Calcium phosphate was obtained only in the colloidalform.The heats of formation of the collo'idal insoluble phosphates do notdiffer to any great extent from the heat of formation of an equivalentquantity of trisodium phosphate, 33.6 x 2 cak.In other words, theprecipitate in its initial condition corresponds clsseIy with the solublesalt from which it has been derived, a further example of the tendencyof systems which are undergoing transformation to preserve theirmolecular type. On the other hand, the new phosphates may bedissociated by water to a greater extent than the sorubre phosphatefrom which they have been formed; and this dissociation ail1 beaccompanied by an absorption of b a t , This absorption is practicallywil with barium phosphate, which appmximates closely to the alkalinephosphates, but ib is very cfistinct wihh magnesium phosphate, whichis more readily dissociated.In dissolved trisodium phosphate, the third and even the secondequivalents of the base are less intimately combined with the acid thanthe first atom, and are partially separated from it by the dissociatingaction of the solvent.There can be little doubt that this imperfectstate of combination also exists in- the colloidal insoluble phosphates,tlie formation of which is due b a polyalcoholic rather than an acidfunction of the phosphoric acid. The combination, however, soonbecomes more intimate, and the alcoholic function changes to an acidicfunction comparable with that 04' ordinary tribasic acids, the changebeing accompanied by development of heat, and crystallisation of thephosphates. The actual development of heat is mnch greater thancan be supposed to be due to the mere physical change from thecolldidal to the crystalline condition, even if the change wereaccompanied by eombination with water.As a matter of fact, theerystallised phosphate contains less water than the colloidal phosphate.In their new condition, the heats of formation of the insoluble phos-phabes become practically treble that of the ordinary monophosphates,or in other words, the three acid functions become equivalent to oneanother, and to this change is due the greater proportion of the heatdeveloped in the passage from ihe colloidal to the crystalline form.Heats of Neutralisation of Homologous and Isomeric Acids.By H. GAL and E. WERNER (Comyt. rend., 103, 806--809).-Theauthor has determined the heats of neutralisation of isobutyric,isopropy la ce tic, t rime thy lace tic (pivalic) , caproic, isobu tylace tic.andsorbic acids, and his results, together with the heats of neutralisationof the lower acid8 of the acetic series, as determined by Berthelot,C. H. B.h 96 ABSTRACTS OF CHEMICAL PAPERS.Lougninine, and others, are given in the following table. Heat ofsolution of isobutyric acid, directly + 0973 cal., indirectly + 1.012cal. ; isopropylacetic acid, directly + 1.167, indirectly + 1.030.Heat ofAcid. neutralisation.Formic acid, H-COOH ........................ 13.3Acetic acid, MeGOOH ........................ 13.4Propionic acid, CH,Me*COOH .................. 14.3Normal butyric acid, CHF,Me*CH2*COOH ........ 14.4Isobutyric acid, CHMe,*COOH. ................. 13.9Normal valeric acid, CH2Me*CR2*CH,*COOH...... 14.4Tsopropylacetic acid, C HMe2*C H2* C 0 OH ......... 14.4T rime thylace tic acid, CMe3*COOH .............. 13.6 74Normal caproic acid, CH,Me*CH,*CH,*UH,*COOH . 14.689Isobu tylilcetic acid, CHMe,*CH,*C 0 OH 14-5 i .......... {Omitting formic and acetic acids, the heat of neutralisation of theother acids, with the exception,of isobutyric and trimethylacetic acids,is practically constant, and varies between 14.3 and 14.6. Isobutyricacid is a secondary acid, and trimethylacetic acid is ft tertia1.y acid, andit would seem therefore that the heat of neutralisation of primary acidsis greater than that of secondary acids, whilst that of tertiary acidsis somewhat smaller atill. The heat of neutralisation of sorbic acid,which is regarded by Menschutkin as a tertiary acid, is 12.945.C.H. B.Heats of Neutralisation of Malonic, Tartronic, and MalicAcids. By H. GAL and E. WERNER (Compt. rend., 103, 871-873) .-MaZonic Acid.-Heat of solution at 10° = -4.573 cal. Heat ofneutralisation by soda : 1st equivalent, 13.342 cal, ; 2nd equivalent,13.778 cal. ; total, 27.120 cal.Heat ofneutralisation by soda : l e t equivalent, 13.71 1 cal. ; 2nd equivalent,11.856 cal. ; 3rd equivalent, 0 0 cal. ; total, 25.567.Mulic Acid.-Heat of solution at 20" = -3,148 cal. Heat o€neutralisation by soda : 1st equivalent, 12.730 cal. ; 2nd equivalent,,12.189 cal. ; 3rd equivalent, 0.0 cal. ; total, 24.919.The heat of neutralisation of oxalic acid is 28.1 cal. (Berthelot andThomsen) ; of succinic acid, 26.4 csl.(Chroutschoff) ; and tartaricacid, 25.3 cal. (Berthelot).I t is evident from these values that the heat of neiitralisationdiminishes as the molecular weight increases. The intzodnction ofthe OH group into oxalic, malonic, and succinic acids lowers the heatof neutrdisation by about 2 cal. A similar difference has previouelybeen observed between propionic and lactic acids, and between benzoicand the hydroxybenzoic acids.Themnochemistry of Reactions between Magnesium Saltsand Ammonia. By BERCHELOT (Compt. rend., 103, 844-848) .-When magnesium sulphate solution is mixed with an equivalentquantity of sodium hydroxide solution, there is an immediate develop-,Tartronic Acid.-Heat of solution at 12" = -4.331 cal.C.H. BGENERAL Ah'l) PHYSICAL CWMBTRY. 97ment of +0*18 cal., but the development of heat gradually slackma,and at the end of 10 minutes is + 1-14 cal. ThB successive develop-ments of heat are due to the fact that a basic srtlt is first formed,which is afterwards decomposed by the soda, and also to the hydra-tion, contraction, $c., of .the precipitate. Magnesium chloride m dsodium hydroxide behave in like manner. At first there is an absorp-+ion of -0.32 cal., and afterwards a development of 44-32 cal., thefinal result being nil.It is evident, &s the reseamhes of Thomsen, Favre and Silbermann,Ditjte, and othere have already indicated, that the heat developed bythe action of acids on magnesium hydroxide approximates closely tothttt developed by their action on potash and soda.The action of ammonia on magnesium sulphate is accompanied byan absorption of -0.24 cal., whereas if the magnesium were com-pletely displaced, 3.0 cal.should be absorbed. The difference is dueto the formation of double salts or oxides, the production of which isaccompanied by a development of + 2.8, cal. With magnesium chlo-ride, the difference between the calculated and observed values is+2.2 cal.If magnesium sulphate is mixed with 2 mols. of ammonium chloride,+0.32 cal. is developed, and if an equivalent quantity of ammonia i qnow added, there is a further development of +0.26 cal., the total de-velopment of +0*58 cal. being due to the formation of a complexoxide, the heat of neutralisation of which is 0.33 cal.higher than thesum of the heats of neutralisation of magnesium oxide and ammoniaseparate1.v. When magnesium chloride is mixed with ammonia, thereis an absorption of -0.48 cal., and if ammonium chloride is thenadded there is a, development of +0*56 cal., the sum being 0.08 cd.,from which it followa that the heat of neutralisation of the complexoxide by hydrochloric acid is practically identical with that of magne-aium oxide,If magnesium sulphabe OF chloride solution is mixed with sodininhydroxide, and ammonk then added, the greater part of the precipi-tate redissolves, but there k no sensible $herma1 disturbance, a resultwhich indicates that the heat of solution of the precipitate is idenficalwith its heat of combination with the solvent.If, oa the other hand,magnesium sulphafe i s first mixed with ammonia, md the sodiumhydroxide added afterwards, there is a development, a€ +Is90 cal.,probably due to the facf that, the order *of admixture being reversed,the liquid requires a much longer time to attain the same condition.The differenee betweert the observed thermal d i s t n r b c e and the de-mb ment of heat resulting fmni the action of soda or magnesiummlp!ka alone ia a, fnrther proof of the formation of complex corn-peunds.I f magnesium snlphate is mixed with 2 mals. of ammonium chlo-ride and sodium hydroxide then added, +3.64 cal. are developed,and some permanent precipitate is formed. The thermal disturbanceis greater than that which would colrwpond with the displacement ofammonium by sodium, rtnd the difference indicah the cornbination ofmagnesia and a;mmonia with formation of ammonio-magnesium sul-phate.If 4 mols. of ammonium chloride fire added at the begia9s ABSTRACTS OF CHEMICAL PAPERS,ning, no precipitate is formed, and the heat developed is +3.90 cal.JVith magnesium sulphate, the excess of heat developed above thatcorresponding with the decomposition of the ammonium salt is + 1.2 cal., with the chloride it is +1*0 cal.From these results it follows that the complex ammonio-magnesiumbases in uniting with sulphuric or hydrochloric acid, develop about + 1.8 cal. more than pure ammonia, and + 0.3 cal. mow. than magne-sium oxide. The association of ammonia with a metallic oxide suchas magnesia would seem to result in the production of a complexalkali analogous to tetramethylammonium oxide, with an energygreater than that of metallic oxides, and approaching +ha& of thestrongest alkalis.C. H. B.Heats of Combustion and Formatiun mf Homologous Phe-nols. By 3’. STOHMAKN, P. RODATZ, and H. HERZBERU (J. pr. Chem.[2], 34, 311-327).-1n this paper a series of determinations of theheats of combustion and formation of the homologous series ofphenols are given in detail, as also their heats of liquefaction. Theprincipal values obtained m e given in the following table :-Heat of combustionper gram-molecule.Phend (did), C,H,-OH. ..... .- .. 723659Orhhocresol (liquid), CsH4Me-OH. .. 883008Mehcresol (liquid) ..............880956Paracresol ................ 882900Orcinol, C6H,Me(OH), (solid). ..... 824724Orthoxylenol, C6H3.%fe2*OH (solid). . 1035434Mehxylenol (liquid). ............. 10374999 araxylenol (solid) ........ -. ..... 1035638Fseudocumenol, CBH,Me,-OH (solid) 119145 1Carvacrol, CGH3MePr*OH (liquid). . 1354819Thymol (liquid). ................. 1353750.. (liquid) ................. 726002 .. (solid). ............. 879788.. (solid) .............. 880441.. (solid) .................. 1348982Heat offormation.-509925304451100109276615665950 161362685496818169250--On a comparison of these numbers, it will be seen that every dis-g!acement of hydrogen bp a methyl-group corresponds with an incre-inent of 155356 cal.in the heat of combustion, a value praotically equalta that obtained for the homologues oE methyl alcohol. Thus it followsthat the displacement of‘ hydrogen by methyl, either in the so-calledside-chain or i n the nucleus, corresponds with the same value forthe heat-increment. Thus the value for ethylphenol will be equal t othat of xylenol. Similarly also, as the d u e s for carvacrol andthymol are approximately equal to that of pseudocumenol, namely,the introduction of the isopropyl-group produces the same effect asthat of three single methyJ groups, then the heat values of the iso-are equal to those of normal-compounds. V. H. VGENERAL AND PHYSICAL CHEIIISTKT. 99Some Laws of Chemical Combination. By DE LANDERO andR. P R r E n , (Conzpt.rend., 103,934-935).-1f chemical combination istaken as the clashing together of the particles of the elements, and ifeach particle is regarded as possessing a constant velocity which ischaracteristic of the pctrticular element, the loss of energy resultingfrom the union of the non-elastic particles may be regarded as theequivalent of the quantity of heat developed by the combination.These considerations lead to the formula-(V + T q 2 , ee'= 2(a + e')in whichf = the heat of Combination expressed in calories, e, e' = theweights of the combining elements epuivaient to 1 gram of hydrogen,whilst V and V' are quantities which a m constant for each elementand are proportional to the velocities of their particles. These quan-tities may be termed thermodynamic constants, or thermodynamiccquivdeuts, and their value is obtained by the €ormula-9 * v'=y/2f--,,.e + e'Take the ease of the two copper bromida-Cuprous bromide: e + e' = 143.4; f = 25900Cupric bromide: e + e' = 111.7; f = 17300- + 38.269cal.; V + V' =cal; v * V' =- + 39'039.Calculations with t i n bromides, mercury bromides, mercury iodides,&c., lead to similar results. Since V Ifi V' is the sum or difference ofthe thermodynamical equivalents of the two elements in each system ;i t is necessary to obtain the consfants of some of the elements fromdifferent sets of compounds, care being taken to use only thermo-chemical data referred to the solid state. The following table givesthe thermodynamical equivalents of several elements, these values re-ferring in each case to that quantity of the element which is equivalentto 1 gram of hydrogen:-K ......45221 S ...... 47.874 A1 ...... 48.218Nu.. .... 49.768 T1 ...... 5.223 Zn.. .... 13.073Hg.. .... 9.079 Ag .... 12.i86 Bb ...... 5.155B r . . .... 44.171 Cu .... 4.999 Si ...... 37.519I ....... 32.416 Ca, ..... 50.309C. H. B.The Law of Volumes in Chemistry. By T, S. HUNT (Chem.News, 54,206-207) .-The author advocates the universal applicationof the law of volumes to solids, liquids, and gases, which would renderthe application of the atomic hypothesis to explain the law of definiteproportions wholly unnecessary. From this standpoint, the union ofmany volumes of vapour or gas to form a single volume of vapour orsolid would be regarded as chemical combination; the reverse,namely raporisation, would be chemical decomposition, which wonldbe without specific difference in the case of integral volatilisation, o100 ABSTRACTS OF CHEMICAL PAPERS.with definite changes, as in cases now regarded as dissociation. Thedifference between chemical and physical molecules would hence bequite evident.D. A. L.Velocity of Dissociation. By H. LESCCEUR (Compt. rend., 103,931-933) .-The velocity of dissociation of acid sodium acetate,CzH,0zNa,2CzH40,, was determined by placing the compound in asmall bell-jar which also contained soda-lime ; the temperature of thewhole being kept a t 100". The mean velocity of dissociation duringk i given interval is determined by dividing the time into the loss ofweight of the compound.The results indicate the existence of abiacetate, CZH,O2Na,C2H1O2, and a sesquiacetate, 2C2H,02Na +Velocity of dissociation does not depend on the temperature alone,as Miiller-Erzbach siipposes, but also on the physical condition of thesubstance which is undergoing dissociation. In this particular case,the rate of dissociation increased fourfold when the acetate becttmesolid, although the tension of dissociation did not change, and similarphenomena are observed with copper sulphate crystals, &c.CzHaOz.C. H. B.Nature of Liquids. By W. RAMSAY and S. YOUNG (Ohm. News,54, 203-205).-1t is proved by various investigations that, above aeertain pressure and temperature, all liquids show an increase in thedensity of their saturated vapours beyond that deducible from themolecular formula, varying of course with the liquid.Some liquids,however, known to be dissociable, in addition show an increasealso on fall of temperature and pressure below a certain tem-perature and pressure characteristic of the liquid. Reasoning fromthese facts, the following difference is suggested between stable anddissociable liquids :-In the former, the molecules exhibit physicalbut not chemical attraction ; in the latter both pliysical and chernicalattraction are evident, inasmuch as, besides cohesion and surface ten-sion, there is evidence of molecular combination. The behaviour of.vapours at the moment the liquid is visible support this theory, forwhereas vapours from dissociable liquids continue to rise in pressure i nspite of the decrease in volume and condensation of liquid (evidenceof non-homogeneity of the vapour, owing in these instances to forma-tion of molecules of higher molecular weight), vapours from stableliquids do not behave in this manner, but the pressure in such case isthe vapour-pressure corresponding with the temperature ; hence itmay be concluded that the latter show no tendency to form complexmolecular groups.With regard to the solvent action of a fluid above its critical point,the authors have worked with a solution of eosin in alcohol, takingthe fluorescence as indicating solution.They find that solution existedat least for a short time at temperatures a little above the criticalpoint, and at volumes smaller than the critical volume ; apparently,however, after some time the solid is wholly deposited as such on thewalls of the tube.This is not conclusive, as the translucent red sub-starice deposited on the glass interfered with the detection of thefluorescence. According to the authors' view of the nature of liquidsGENERAL AND PH Y STCAL CHEMISTRY. 101solution should be possible above the critical point provided thevolume is sufficiently small. D. A. L.Capillary Constants and Meniscus Angle. By J. TKAUBE(J. pr. C'he?n. [2], 34, 292--31l).--l)eterminations are given for thevalue of the function a' cos 8 according to the formula rh = a2 cos 0, foraqueous solutions of. the alcohols of the paraffinoid series and acids ofthe acetic series at various degrees of concentration (comp.Abstr.,1885, 1033). The principal points to be noticed are that both propyland isopropyl alcohols show a minimum value for tho function withmixtures of equal weights of the alcohol with water, and that theeurve for butyric acid at first decreases with increase of concentrationup to 30 per cent., thence increases up to 50 per cent., and sub-sequently decreases.After a historical review of the literature on the magnitude ofdrops, an account is given of experiments, made with an apparatuspreviously described, permitting of the formation of drops from acapillary tube under constant or variable conditions of temperatureand pressure. The weight of the drops was ascertained by deter-minations of the specific gravity and the number of drops in aconstant volume.The results obtained with the above-mentionedalcohols and acids show that the volume of the drops is proportioual tothe rise in height in the ca~illary tube, or their weight is proportiwrd tothe product oj' the height and the specijiic gravzty. If then the meanweight of the drop is divided by the circumference -, then for allliquids examined this quotient is less than the capillary constanta cos0, and secondly this qnotient increases with decrease of radiusof the tube. Both these statements are deducible from the previousobservations of Hagen and Quincke.Again the diameter of the capillary tube determines the shapeof the drop; thus with tubes of less than 3 4 mm.their form ismore or leas spheroidal, with tubes of 1 mm. the form is cylindricalwith a convex base, and with tubes of larger diameter it is para-boidal . V. H. V.C2 r rCrystallisation by Diffusion. By C . E. GUIGNET (Compt. rend.,303, 8iS--875).-The experiments described in this paper are anextension of Becquerel's researches on electro-capillary reactions.The introduction of any solid into a saturated solution of anothersolid determines the crystallisation of the latter, provided that thesolid introduced is soluble in the particular solvent. For example,solid paraffin introduced into a saturated solution of sulphur incarbon bisulphide causes the separation of crystals of sulphur, andvice versd ; sodium thiosulphate introduced into a saturated solutionof ammonio-cupric sulphate yields violet needles of ammonio-cupricthiosulphate.If crystals of sodium sulphate are placed in a saturated solution ofbarium chloride, the crystals become opaque but retain their form,aud when the crystals are broken each one is found to be a sort o102 ABSTRACTS OF CIIEMICAL PAPERS.miniature lode with crystals of barium sulphate.Barium chlorideiiitroduced into a saturated solution of sodium sulphate yields onlyamorphous barium sulphate, probably because the chloride dissolvestoo quickly. Ordinary sodium phosphate placed in magnesiumsulphate solution produces crystallised magnesium phosphate.Ia order to observe these phenomena with two liquids, if the actionis merely physical, a saturated solution of a solid is covered with alayer of the solvent, and on this is poured a second liquid in whichthe solid is somewhat less soluble than in the first.The liquidsgradually mix by diffusion, and the solid separates in very distinctcrystals. If a saturated solution of sulphur in carbon bisalphide iscovered with a layer of the bisulphide, and on this is poured a layerof oil, alcohol, glacial acetic acid, benzene, petroleum, &c., octahedralcrystals of sulphur are deposited. A saturated solution of leadchloride in hydrochloric acid covered in a similar manner with a layerof hydrochloric acid and a layer of water, yields fine crystals of leadchloride.Where chemical action takes place between the liquids, one is placedin a crgstallising dish which is 6lled nearly i~ the top, and this isplaced inside another vessel which contains the second liquid. Wateris then carefully poured into both dishes until it is just higher thanthe edge of the inner dish.Diffusion takes place through the super-natant water, and crystals are formed. Sodium snlphate and calciumchloride give long crystals of calcium sulphate ; sodium sulphate andbarium chloride give crystallised barium sulphate ; sodium sulphateand lead acetate give crystals of lead sulphate ; and potassium ferro-cyanide and lead acetate yield long pale-yellow needles of lead ferro-cyanide.On a large scale, wooden vessels with a leaden partition which doesnot quite reach to the top are used.The liquids are poured one intoeach compartment, and &he latter are then tilled up with water untilthe water just, flows over the top of the partition. In this way verylarge crystals can be obtained.Influence of some Normal Salts on the Decomposition ofMethyl Acetate by Hydrochloric and Sulphuric Acids. By H.TREY (J. pr. Chenz. [2], 34, 353--377).-Ostwald investigated (J. pr.Chem. [2], 23, 209) the difference in the action of acids caused bythe presence of their normal salts; the author has repeated theseexperiments with a view to obtaining a satisfactory explanation oft h i s action. Tbe experiments were made with hydrochloric andsulphuric acids, and the salts of these acids with the alkalis andalkaline earths. The methyl acebate method was used, in the mannerpreviously described, with normal acids ( I gram-equivalent in 1 litre)and normal acids to which 4, 4, 1, &c., equivalents of their normalsalts had been added.These normal solutions were also used 29, 5,and l2g times diluted. The results were calculated according to theformulse given by Ostwald (this Journal, 1884, SSl), and are given in aseries of tables. These values are not strictly comparable, but requirecorrecting for the increase of volume caused by the addition of saltand the consequent decrease of the velocity of the reaction. TheC. H. BGENERAL AND PHYSICAL CHEMISTRY. 103mean values found are given below; the second line in each casegi yes the corrected value.1.1211.0491.032Normal . . .. .1 - normal .. Z L6 normal.. . .1 - normal . .12+---1.4261,1671.005Hydrochloric Acid and Alkaline Chlorides.1 - normal . .2 i32 -7632.8711 -7511 *826 -615 -682 -232 -241.000HC1(1 litre)t lNaCl1 - normal. .12.1-36 -8737 *4912 '2712 -355 -755 t852 -202 -241 .OOOHC1(1 litre)t 4NaCl--52 -8757 '6213 -8814 *886 -096 -642 *152 -34-HCl:1 litre) + tKcL31 -8932 -1611 -7311 -835 *636-672 -212 -22 --HCl(1 litre) + lKC1.34 -6635 -0511 -8912 -265 -635 -802 -152 -22HCl(1 litre) + 3KU1.40.8344 -6012-4513 *645 -606 -142 '102 *30--Calculating the ratio in which the velocity of action of the hydro-chloric arcid is increased %y the addition of the &ove salts, thefollowing numbers are obtained :-(1 litre).I+ normal.. . . I 1 -000-HCl(1 litre) + +N&l.1 0511.0111.0111.009 -HC1(1 litre) + lNaCl ---1 01991 -0561 -0411 -009HCl(1 litre) + 4A aC11 '8431 a731 -1811-054 -HC1(l. litre) + tKCl1 *0281 -0121 -0091 -000HCl(1 litre) + 1KC1.HCl(1 litre) + 3KC1.For the stronger solutions, the increase of the action of the hydro-chloric acid is proportional to the amount of salt present; for theweaker solutions, the increase is so small as to fall within the errorsof experiment.Hydrochloric acid and lithium, magnesium, calcium, strontium,and barium chlorides, gave the followiog numbers :104 ABSTRACTS OF CHEMICAL PAPERS.Normal .. . . .+ normal.. . .--Normal .. . .4 normal.. . .1 *OOd 1 *9611 '000 1 *14656 *8361.315 -976 -441.9851.171HCl(1 litre) + BMgCl,.1.4091.08066 -5669 -266 '336-59HC1(1 litre) + 2CaC1.--59 -4362 *696 -246 5 6HC1(1 litre)+ 2SrC1,.68 *5562 -066.206 -58HC1(1 litre) + 1BnC1,.42 -4644 -075 *846 -07--These numbers gave the following ratios for the accelerating actionof the salts :-HC1(1 litre) + 2MgC1,.HC1(1 litre) + 2UaCI.HC1 HC1(1 litre) (1 litre) + 2SrClj. + lBaCI,.2 -2151.1732 *0051 -167From these results the author concludes that the accelerativeinfluence of the chlorides stands in the inversive ratio to the atomicweights of the respective series. Thus, calculated for 1 equivalent ofchloride, the numbers are :-.~LiC1. 1 NaCl. 1 KCE. 1 MgCk. 1- CaC1,. 1 SrC1,. 1 BaCIJ.1.240 1 1.199 1 1.121 I 1.304 I 1.251 1 1.246 I 1.205These results agree with those found by Reicher (Abstr, 1885,The action of eulphnric acid in the presence of normal salphates isThe action is retardedto 1 equivalent salt, but in a less degreeThe following tables give the mean values for1034) for the saponification of ethyl acetate by alkalis.the reverse of that of hydrochloric acid.nearly proportionally withwith 2 equivalents.normal and + normal solutions :QENERAL AND PHYSICAL CEENISTRY.#IlGrmlbl -Normal.+normal1053 -04 2 -68 2 -16 { 3L546 3 -04 2 -69 2 -19 -- -__I_ ------1.000 0.885 0 -760 0 * 5781.000 0.910 0 -805 0 -656frH$04 (1 litre) + )MgSO,.0.787*HaSol(1 litre) + lNGO4.I__--6 8s'7 -081 '621 -670 -4260 -500---&SO4 (1 litre) BH2S04 (1 litre) BH,SO, (1 litre) + +LizS04. f +Na&404. + +Kfi04.0 -620 0 -579 0 *330-------_I_--With aulphuric acid, the retarding influence of the sulphates onthe velocity of the action appears to inorease with the atomic weightof the elements of the series, thus :-Dithionic acid in the presence of its normal salts was in-fluenced in the same way as hydrochloric acid, so also was the bibasicmethylenedisulphonic acid, whilst dichloracetic acid behaved likesulphuric acid. This method of investigation will therefore throwno light on the basicity of dithionic acid, but th0 author thinksthe results show that it does not form acid salts in aqneoucil solution.Preservation of Gases over Mercury. By H. B. DIXON (Chem.News, 64, 227-228).-From the author's eqepiments, it is shownthat, provided due precautions are taken t o prevent the formation of'a, film between the glass and the mercury, gases may be safelypreserved over mercury for a considerable time.Cracking Glass with Certainty. By E. BECKXANN (Zeit. amE.&%em., 25, 530-531).-A scratch is made with a file ; at both sidesof this, pads of wetted filter-paper are wrapped round the object,,leaving a, space of a few millirnetres between them. The flame of aBunsen or gas blowpipe is applied to this space, when the crack willbe carried round from the scratch midway between the two pads.Apparatus for Chemical Laboratories. By J. WALTER (J. PT.Chem. [23, 34, 427--432).-A new form of condenser, and flasksfor use with it, both for ordinary and fractional distillation.G. H. M.D. A. L.M. J. S.G. H. M

ISSN:0368-1769    

DOI:10.1039/CA8875200093

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

106 ABST tiACTS OF CHEMICAL PAPERS. In o r g a n i c C h e m i s t r y. Action of Hypochlorous Anhydride on Iodine Trichloride. Ry H. BASSETT and E. FIELDING (Chem. News, 54, 205--206).--Iodic anhydride is the main product of the reaction when solutions of iodine trichloride and’ hypochlorous anhydride in carbon tetrachloride are mixed, or when a current of bypochlorous anhydride is passed through a solution of iodine trichloride, or even over solid trichloride. In the last case, the action is very slow. D. A. L. Saturation of Selenious Acid by Bases. By C. BLAREZ (Conzpt. rend., 103, 804- 806). -With cochineal or helianthin (methyl- orange), selenious acid is monobasic. With litmus, it is monobasic to ammonia, lime, strontia, and baryta, but if soda or potash is used the litmus only becomes blue-violet when about 1.5 equivalent of alkali is added. With phendphthalein.and potash, soda, ammonia, lime or strontia, the colour change takes place when somexhnt more than 1.5 equivalent of alkali is added, but with phenolphthalein and baryta selenious acid is bihasic,, and the colour change is sharp and distinct. Selenious acid can be accurately titrated by means of standard barytn solution, using helianthin or phenolphthalein as indicator. The bavyta has double the value with the first indicator that i t has with the second. Both indicators can be used in the same solution ; the rose colour of the heliauthin disappears when the acid is half saturated, and the rose colour due to the change of the phenol- phthalein becomes visible when saturation ik complete.As no. basic barium selenite is formed when baryta is present in excess, an excess of baryta can be determined by means of phenol- phthaleh and a standard acid in the liquid containing the precipitated barium selenite. Selenious acid, like sulphurms acid, cant be estimated in presence of other acids by means of baryba, provided that the tofal basicity of these acids is indicated by helianthin. Helianthin and phenol- phthaleln are both a;dded to the same solution, and the amount of selenious acid is calculated from the quantity of bnryta solution required to produce the second colour change, this quantity being exactly half that which would be required to neutralise the selenious acid alone with phenolphthale’in as the indieator. C. H, B.Formation of Nitrites- By S. KAPPEL (Arch. Pkarm. [3], 24, 897--900).--The author has extended his observations made on the action of copper, iron, and zinc in contact with the air, and solutions of ammonia and the fixed alkalis (AbsBr., ’1883, 282, 286), employing in recent experiments magnesium, aluminium, and tin. Magnesium exposed to the a i r in contact with aqueous potash, gave small quan- tities of nitrous acid, ozone, and hydrogen peroxide. With ammonia solution, strong indications of nitrous acid were obtained. Alnmiriium in potassium hydrate produced nitrous acid readily, even in the cold,INORGAKIC CHEMISTRY. 107 nitric acid and hydrogen peroxide were also easily detected. With ammonia the action was much slower. Tinfoil gave scarcely any reaction ; nitrous acid was not produced, but hydrogen peroxide was perceptible.J. T. Compounds of Arsenious Anhydride with HaTogen Salts. By F. R~UORFF (Ber., 19,2668--2679).-1n this paper the preparation and properties of compounds of the halogen salts of the alkali metals with arsenious anhydride are described. These are best obtained by passing carbonic anhydride info a mixed solution of potassium arsenite and the halogen salt. These componnds separate either in the amor- phous form or in indistinct crystals, of the general formula MX,2As203, sparingly soluble in water, insoluble in alkaline carbonates, but very soluble in the free alkalis; when heated, they decompose with elimi- nation of arsenious anhydride, the compound KI, 2As,03 decomposing a t 350" ; KBr,2As20z a t 380" ; and KCI,As203 a t 240" ; a compound, KC1,2Asz0,, is also described.The ammonium compounds NH41,AsL03, NH4Br,2As,C3, and NH4Cl,As20,, are also described, those of sodium being reserved for a future communication. V. H. V. Some Probable New Elements. By A. PRINGLE (Chem. News, 54, 167-168).-TThe author claims to have discovered some new sub- stances, including five metals and a substance resembling selenium, called hesperisiztm, in some " Lower Silurian " rocks, situated in the county of Selkirk. One metal is said to be like iron, but gives neither the thiocyanate nor the tannic acid reaction ; one is Eke lead in appear- ance, is easily fused and volatilised, and yields yellow and green salts ; another which is charcoal-black, is called erebodium,; its equivalent is 95.4, and it forms several oxides.A fourth, g a d e n i m , with equivalent about 43.6, a light-grey powder, forms a red monoxide and a cream- coloured dioxide, yielding respectively white and yellow saltp. Another, polymnesturn (Pm), is a rather dark-coloured metal, with equivalent about 74. A preliminary description of four oxides, PmO, PmOs, PmO,, and (?)I Pm05, of two sulphides, PmS and PmSp, and of other compounds is given. D. A. L. Production of Alkali Metals. By H. Y. CASTXER (Chem. News, 54, 218--SlS).--Irou reduced by hydrogen or carbonic oxide is mixed with t a r in proper proportions, so that after the mixture is coked it has a composition about = FeCp The coke is finely ground, mixed with c a s t i c soda (or potash) in proportions = 3NaHO + E'eC,, or about 100 NaHO to 15 of coke.This mixture is introduced into a cast-iron crucible, and heated in a specially arranged furnace (described in the paper). The reduction and distillation commence at a temperatnre of 1000". When the operation is finished the crucible is removed, and another immediately put in its place. The residue consists of some sodium carbonate, and finely divided iron; the sodium carbonate is recovered, the iron used to make fresh reducing coke, aiid the crucible is used over and over again. The advantages over the old method are manifest. D. A. L.108 ABSTRACTS OF CHEMICAL PAPERS. Crystalline Scale formed in the Manufacture of Sodium Hydrogen Carbonate. By G. W. LKIGHTON (Amer. .J. Xci., 33, 318--.319).-This scale was formed in the manufacture of sodium hydrogen carbonate by the ammonia process, at Syracuse, New Pork.It was deposited on the inner surface of an iron tank, and had the appearance of boiler-scale, being 1 to 2 inches thick, with a vitreous lustre, and a greenish-grey colour. It is usually covered with crystal planes, proving to be the termination of prisms (probably monoclinic). Analysis gave the following results :- NaC1. Na2C0,. MgCOB. CaC0,. FeCO,. H20. CO,. Total. 22.23 40.62 31.57 3.56 0.08 0.63 0.64 99.33 The scale is evidently a triple sait, represented by the formula MgCO,,Na,?CO,,NaCl. It is, in fact, a definite crystalline product of an interesting constitution, not unlike that of several well -defined mineral species, in which an alkaline chloride appear8 to be in mole- cular combination with heterogeneous materials. By C .HEYER (Ber., 19, 2684-2690).- When strontium hydroxide is heated to bright redness, it is converted into strontium oxide. When the latter is exposed to air saturated with aqueous vapour, and then to dry air at the ordinary femperature, strontia dihydrate, Sr0,2H20, is obtained as a white, crystalline powder. I Dry strontia dihydrate, when heated with dry carhonic anhydride, is completely converted into carbonate ; the monohydrate, however, absorbs only traces of carbonic anhydride. The water in the dihy- drate was determined by passing dry carbonic anhydride over t h e substance for five hours at 26*5", and for 40 minutes at 121.5", and absorbing the water in sulphuric acid bulbs. These results are not in accordance with those obtained by Scheibler (Abstr., 1886, 927).N. H. M. B. H. B. Strontia Dihydrate. Calcium Borate. By B. BLOTJNT (Chem. News, 54,208-209).- The salt obtained by fusing freshly calcined lime with boric anhydride over a Bunsen burner is CaB,O,. I t is possible that t4he salt obtained on a platinum wire loop before the blowpipe, with large excess of boric anhydride, contains a larger proportion of boric acid. D. A. L. Calcium Ammonium Arsenate and Calcium Arsenates. By C. L. BLOXAM (Chem. News, 54, 268-170 ; 193--194).-1n a previous communication (Abstr., 1886, 920), mention is made of a calcium ammonium arsenate. Various observers differ as to the composition of this salt and as to the amount of water it contains. The amount' of water appears to vary somewhat with the state of the atmosphere, and hence, prohably, the cause of the difference of opinion on this point.It is now shown theoretically and experimentally that the* precipitate produced by arsenic acid in a solution of calcium chloride containing free ammonia hae the following composition :-INOROANI C CHEMISTRY. 109 Air-dried.. ........................ CaNHAsSOh + 7H20. Dried in a vacuum over sulphuric acid, Ca3NH4HZ(As04), + 3H20. Dried at 100". ..................... Ca6NH4H6(AsO& + 3H,O. Ignited ........................... CazAs,Oy. I t is suggested to use the precipitation of calcium as calcinm ammo- nium arsenate for quantitative purposes ; it ie convenipnt, the precipi- tate being crystalline and bulky, but is not susceptible of such great accuracy as the oxalate method.It is recommended for checking hardness determinations in water analysis. Its various advantages and disadvantages as a method aye discussed. On evaporating down a hydrochloric acid solution of calcium ammonium arsenate with platinic chloride, the platinochloride after ignition was observed t o be mixed with fine, white, opaque, prismatic crystals of the orthoarsenate Ca3(As04)2, insoluble in acids. A repetition of the experiment re- sulted in the production of a substance somewhat similar in appearance, namely the meta-arsenate C ~ ( A S O ~ ) ~ ; the same substance is formed when mixtures of arsenious anhydride and calcium carbonate are ignited, and is left as an insoluble, crystalline powder when the ignited mass is treated with hydrochloric acid.Artificial Lead Silicate from Bonne Terre, Missouri. By H. A. WHEELER (Amer. J. Sci., 32, 272--273).-E. S. Dana and S. L. Penfield hare given (Abstr., 1886, 317) some crystallographic deter- minations and apalyses of this artificial mineral from the Desloge Lead Co., of Boxine Terre. Since the publication of that paper, the author has examined some specimens in the metallurgical collection of Washington University. The results of his analysis are as follows :- D. A. L. Si02. PbO. Fe203. Al20,. CaO. MgO. I .... 17.11 73.66 0.80 0.53 2.35 0.22 I1 .... 18.51 '72.93 1.31 0.62 1.66 0.201 C1. Nn20. Ni0. Total. I .... 0.08 2.22 3.06 100.03 I1 .... undet. undet. undet. 95.23 I, coarse crystals; 11, fine crystals. The iron in these analyses was assumed to be in the form of ferric oxide.B. H. B. Equivalent of Gadolinium Oxide. By A. E. NORDENSKIOLD (Cowzpt. rend., 103, 795-798).-Gadolinium oxide is the mixture of jttrium, erbium. and ytterbium oxides, which was first obtained from the gadolinite found at Ytterby. It is precipitated by ammonia and ammonium oxalate as well as by potassium sulphate, and the three constituents cannot be separated quantitatively. The gadolinium oxide obtained from kainosite, the silicocarbonate of yttrium, erbium, and ytterbium, recently discovered at Hittero, in Norway, has the molecular weight 260 2 it 0 = 16 and the formula of the oxide is taken as &03. This number is practically identical with the molecular weight of the similar mixture of oxides obtained VOL.LII. i110 ABSTRACTS OF CHEMICAL PAPERS. by different observers (Nordenskiold, Lindstrom, Engstrom, Cl b e ) from gadolinite, kainosite, azzhenitc, xenotime, fergusonite, clevite, fluocerite, and eudialite. These minerals are found in different localities, and contain the oxides in combination with different acids, such as silicic, pbosphoric, niobic, or tantalic acid. Moreover, the oxides have been separated by somewhat different methods, and yet in all cases the greatest variation from the mean value for the mole- cular weight, 261.9, is one per cent., a variation which is within the error of experiment, and is not greatel. than the alterations which have been made in recent times in the atomic weights of some of the better known elements. It follows therefore that gadolinium oxide, although not thc ozide of a simple substance, but a, ?nixtwe of three isomorphous oxides, has a constant molecular weight, even whrrt obtained .from totally &#went minerals found in widely separated localities.This is the first instance of the coexistence of three isomorphous substances in constant DroDortions. The exdanation of this fact seems to be a problem andogius to that of the brigin of the minor planets. C. H. B. Formation of Ultramarine in the Wet Way. By I?. KNAPP ( J . 237'. Chem. [ d ] , 34, 328-340).-An account of some further ex- periments on the formation of ultramarine by the exposure of a heated mixture of kaolin, soda, and sulphur, to a damp atmosphere, or treat- ment of the same with liver of sulphur (Abstr., 1886, 306).The various conditions necessary for success are discussed in full, such as the degree of aggregation of the liver of sulphur and the form of silicate or silica used. Thus experiments with quartz were unsuc- cessful, and those with silicic acid jelly from soluble glass led to the production of it bluish-green material, which turned to a deep blue on warming. Pure alumina led to no result, but sodium aluminate gave a very satisfactory product. Salts of sodium, such as the thio- sulphate, or even calcium phosphate, produced very fine specimens of ultramarine-blue. V. H. V. Sodium Dichromate. By A. STANLEY (Chem. News, 54,194- 196).-Sodium dichromate crystallises wi1,h 2 mols. HzO, in prisms and plates belonging to the triclinic system; its sp. gr.is 2.5246 at 13"; i t is deliquescent. It loses 1 mol. H,O below 75", and all below loo", leaving a light brown, anhydrous salt, which fuses to a transparent dark red liquid a t 320°, and on cooling cr~stallises in the same forms as the hydrated salt, When treated with water, the anhydrous salt causes a rise, and the hydrated salt a fall in temperature. 100 parts of the saturated aqueous solution contain- Temperature.. 0" 15" 30" 80" 100" 139" Parts Na&r2O7 107.2 109.2 116-6 1428 162.8 209.7 The saturated solution boils at 139". A table of the sp. gr. of soh- tious of various strengths is given. Sodium dichromate is insoluble in ether, slightly soluble in alcohol. I t is very hygroscopic, in 48 hours an exposed sample absorbed one-third its weight of water ; a sample of calcinm ch1or:de under fiimilar circumstances absorbedINORGANIC CHEMISTRY.111. nearly its own weight of water. It decomposes slightly above its melting point, and a t a dull red heat leaves sodium chromate and chromic oxide, In its reactions generally it resembles potassium dicliromat e. By dissolving the dichromate in warm aqueous chromium trioxide, the trichromate separates on cooling in dark red crystals ; these a r e very solnble in water, and are deliquescent. By the action of sodium dichromate on freshly prepared cuprio hydroxide, a brown powder is formed, consisting of microscopic crystals of the composition Na2Cr04,CuCrz07,2Cu0 + 4H20- It is almost insoluble in water, and but slightly soluble i n alcohol. It loses all its water below loo", and partially decomposes a t higher tempera; tures, cupric oxide separating.Magnesium sodium chromate, prepared by neutmlising sodium dichromate with magnesia, crystallises with 3 mols. H20, in yellow four-sided prisms and plates. It is soluble in water and alcohol, but insoluble in ether. The 3 mols. H,O are driven off below 200°, leaving a dark reddish-brown powder, which fuses at a red heat with partial decomposition. D. A. L. Reduction of Inorganic Thio-salts by Hydrogen.. By G. K R ~ ~ S S and H. SOLEREDER (Bey., 19, 2729--2759).--By the reduction of molybdothio-salts by hydrogen at a red heat, salts of a lower molybdosulphide could not be obtained ; potassium thiomolybdate and ammonium dithiomolybdate are gradually redaced t o a mixturn of molybdenum and potassium sulphide and to molybdenum.I n the case of ammonium dithiomolybdate, no oxpulphide could be obtained. Potassium thallium sulphide, K2TlaS4, behaves k a similar manner, being reduced to potassium sulphide and thallium. The salts of such thio-acids as remain unchanged in a current of hydrogen are not reduced; for example : R2S,3ZnS ; K,S,SCdS, &3. If the thio-acid is merely reduced to -a lower stable sulphide, the corresponding thio-salt yields also the lower sulphide or its thio-salt in the case of its having the properties of a thio-acid. Examples : K2S,3Cu2S,Cu,S2, K2S,Fe2S3. Atomic Weight of Tungsten. By J. WADDBLL (Amer. Chem. J., 8, 280--288).--ScheeIite was decomposed by nitric acid, and the impure tungsten trioxide freed from silica as follows :-The mixture is fused with an equal weight of hydrogen potassium sulphate until in a state of limpid fusion; the cool mass is digested with water and filtered ; water containing ammonium carbonate must be used for the further washing to keep the fluid from running through turbid, and to assist in the solution of the tnngstate.If the silica is to be esti- mated it will probably require a second fusion, &c., with acid potas- sium sulphate. Another method of separating tungstic acid and silica is by means of ammonia, but here also the extraction is apt $0 be incomplete. Commercial metallic tungsten is but slowly attacked by acids, it cannot be fused with nitre without attacking the crucible, and is therefore best oxidised by a current of air a t ared heat.The product is fused with sodium carbonate, and after dissolution N. H. M. i 2112 ABSTRACTS OF CHEMICAL PAPERS. filtered from uaoxidised material. The filtrate boiled with ammonium carbonate gave a smail precipitate of alumina. To remove molyb- denum, tartaric acid is added (half the weight), then hydrochloric acid (no tungstic acid is precipitated), and sulphuretted hydrogen passed. The blue filtrate is decolorised by a current *of air, and the tungsten separated in 11 fractions by boiling with hydrochloric acid. Fractions 3, 7, and 10 were purified for determination of the atomic weight by solution in ammonia, reprecipitation by hydrochloric acid, and roasting of the precipitate in a current of air. The analysis was effected by heating gradually in a current of hydrogen, using a porcelain boat and tube, and a Fletcher’s blast furnace. No.3 gave W = 184.50, No. 7 184.00, and No. 10 183.67, when 0 = 16. The first number is to be considered most accurate, namely, W = 184.50, 0 = 16; or W = 184.G4, 0 = 15-96. The specific gravity of this sample of metal is 18.77. Compounds of Gold and Nitrogen. By I?. RASCHICI (Annnlen, 235, 341-368).--Aurous oxide, Au20, is most conveniently prepared by boiling a solution of mercurous nitrate with an excess of auric chloride, as descritled by Figuier (Ann. Chim. Phys. [3], 11, 336). The precipitate dried over phosphoric anhydride contains 2 11301s. HzO. When strong ammonia is added to water containing aurous oxide in suspension, a black explosive powder, NAu3,NH3, is obtained. Boiling with water, or with dilute acids, converts the sespui-auroamine into triauramine, NAu3.Met hylamine also acts on aurous oxide, forming diauromethy Zamine, NM eAuz. This compound also loses half its nitrogen when boiled in water for 15 minutes. Gold monoxide, AuO, was first obtained in a pure state by Schottlander (Abstr., 1883, 853). It is converted by strong ammonia into the very explosive compound sespu ihydrazhry Zamine, NH,,N( AuOH)~. Warm hydro- chloric acid dissolves two-thirds of the gold, but one-third is left in the metallic state. On boiling with water, half the nitrogen is expelled, and trihydraurylamine remains. Methylamine unites with gold monoxide, formirig the compound MeN(AuOH)a ; this loses half its nitrogen in the form of methylamine when boiled in water. The author confirmsthe accuracFof Dumas’s formula, (AuN + NH3)2+ 3H20, for the fiilminating gold prepared by the action of ammonia on auric oxide, Auz03 ; but he proves t h a t t<he substance which is precipitated by ammonia from a solution of auric chloride is a mixture of the preceding compound and auric imidochloride, NH : AuCl.The latter compound is obtained in an impure state when a, hew drops of ammonia are added to a large excess of auric chloride. Only a por- tion of the chlorine can be removed by digestion with ammonia. Fulminating gold is slowly attacked by boiling water, losing ammonia. Boiling with nitric acid renders the compound more explosive. Dilute sulphuric acid does not liberate ammonia, but forms a very explosive substance of the composition ( AuN2H3),,H28O4.The constitution of auric diamine is represented by the formula NH,*Au : NH. The decomposition it undergoes when boiled with water is probably 2NHzAuNH = NH : AuN Methylamine yields a, yellow precipitate with auric chloride, soluble H. B. AuNH2 -I- NHs.INORGAN10 UHEMISTRT. 113 in an exoess of the reagent. On warming the solution, a bibown pre- cipitate which contains a large quantity of chlorine is deposited. Auric oxide yields a red compound with methylamine. Complex Inorganic Acids. By W. GIBBS (Amer. Chem. J., 8, 289-290 j .-Compounds have been obtained comparable with the chlorplatinophosphoric acids of Schutzenberger. These compounds are to be regarded as phosphoric acid in which one atom of oxygen is replaced by platinous chloride, bromide or oxide, or the corresponding compounds of palladium, iridium, ruthenium, and osmium.More- over the phosphorus may be replaced by arsenic or antimony. The following formula? are given to the compounds so far studied :- w. c. w. As,0,3( As203,2Pt0),5 (NH4)aO + 7H20 ; fAs,O3,2PtCI,)K,O + 2HzO ; ~ ~ W O ~ , A S ~ ~ ~ , ~ ( A S ~ O ~ , ~ P ~ C ~ , ) , ~ ~ P ~ ( + 60R2O j 23 W O ~ , ~ A S ~ O ~ , ~ ( A S ~ O ~ , ' ~ P ~ O ) 6Pt (N&),O + 4OH2O ; ~~XOO~,AS~O~(AS~O~,~P~O)~P~(NH~)~O + 27H20. H. B. Roseo-rhodium Salts. By S. M. JORGENSEN (J. pr. Chem. [2], 34, 394-406 ; compare Abstr., 1883, 1058) .-Boseo-rhodium nitrate, ( Rh2,10XH,,2Hz0) (NO,), is obtained by adding moderately dilute nitric acid to a concentrated solution of roseo-rhodium hydroxide, when i t separates as a white precipitate consisting of microscopic, quadratic tables.It loses 2 mols. of water at loo", and is converted into nitratopurpureo-rhodium nitrate. Roseo-rhodiunz platinochloride witrate, ( Rh2,1 0NH3,2H,0)(N0,),PtC16 + 2H20, is obtained as a beautiful, orange-yellow, crystalline pre- cipitate on adding hydrogen platinochloride to a solution of the nitrate. It emily loses 2 mo1s. of water at 100°, the other 2 mols. are given off more slowly, and nitratopurpureo-rhodium platinochloride is formed; on treating this with dilute hydrochloric acid all the platinum is dissolved, leaving white nitratopurpurco-rhodium chloride undissolved. A solution of the latter in water give8 wit4 sodium dithionate a precipitate of the characteristic nitratopurpureo-dithionate.Roseo-rhodium bromide, ( Rh,,10NH3,2H20j,Br6, is prepared by adding concentrated hydrogen bromide to a solution of roseo-rhodium hydroxide. It forms a crystalline powder consisting of small octo- hedrons or six-sided tables. At loo", it loses 2 mols. H20 a.nd is converted into the bromopurpureo-bromide. It is easily soluble i n cold water, and its aqueous solution gives the same reactions as Che nitrate. Roseo-rhodium sutphate, ( Rhz,10NH3,2E20) (SO& + 2H20, is pre- pared by saturating the hydroxide with dilute sulphuric acid, and precipitating with alcohol. It forms a white precipitate of very small octohedral crystals. 'In contrast to the other roseo-rhodium salts, i t is not converted into the purpureo-salt by solution in boiling water ; i t crystallises in large, quadratic prisms, terminated by a quadratic pyramid, apparently isomorphous with roseocobalt sulphate.At looo, i t quickly loses 4 mols. H20, and then more slowly another 4 mol., undergoing a similar ahanga to the analogous roseooobitlt salt, form- It is easily soluble in water.114 ABSTRACTS OF CHEMICAL PAPERS. ing luteo-salts. Bn aqueous solution gives all the reactions of the nitrate ; with potassiiim iodide, it gives a white precipitate, consisting of microscopic octohedrons of the roseoiodide sulphate, (Rh,,lONH,,2HzO)I,(SO,)2. Roseo-rhod ium platinochloride sdyhnte, ( Rhz, 1 O?SH3,2H20)PtC16( SO,)?, is obtained as ti beautiful, silky, buff precipitate of very thin six-sided tables, by adding a solution of hydrogen platinochloride to a cold solution of the roseo-sulphate. It seems to be isomorphous with the corresponding roseo- and luteo-salts of cobalt and chromium.Roseo-rhodium orthophoyhzte, ( Rhz,10NH3,2H20) (PO4H)s + 4Hzo, is prepared by adding a 10 per cent. solution of phosphoric acid to a concentrated solution of the hydroxide. It forms a white, crystalline powder which behaves like the correFponding cobalt salt. Sodium roseo-rhodium pyrophosphate, ( Rhz,10NH3,2H,0),P20,Na + 23H20, is obtained by adding sodium pyrophosphate to a solution of the hydroxide iu dilute hydrochloric acid until the amorphous precipitate a t first formed is redissolved ; on shaking, the salt then separates as a silky, white crystalline precipitate. It agrees in all respects with the cobalt salt.Koseo-rhodium cobalticyanide, (Rh,,10NH3,2HzO),COzCyn, is obtained a s srnall pale-yellow crystals on adding a solution of potassium cobalti- cyanide to the hydroxide, neutralised with dilute sulphuric acid. Nitratopurpureo-rhodium Salts. By S . M. JORGEXSEN ( J . pr. G. H. M. C'hem. ['L], 34, 40 -109) .-Nitratopur~ureo-rhodiunz nitrate, is easily obtained by heating the roseonitrate or by dissolving this salt in hot water, adding an equal volume of Concentrated nitric acid, heating the mixture for some time on the water-bath and then allow- ing it to cool, when the salt separates in small, octohedral, white crystals with a greenish-yellow tinge. Heated over a flame, the salt explodes. Nitrat~urpureo-rhoa~u~n chloride, (K 0,) L( Rhp, 10NH,)Cl,, is obtained as a pale greenish-yellow precipitate on filtering a, cold solution of the nitrate into an ice-cold mixture of 3 vols.hydrochloric acid and 1 vol. water. Nitratopurpureo-rhodium dithionate, (NO,),( Rhz,10NH3)( Sz06)2 + 2H20, is prepared by precipitating a cold saturated solution of the nitrate or chloride with sodium dithionate. It forms white, silky X-shaped aggregations resembling the corresponding cobalt salt. The air-dried salt loses all its water a t 100". It is quite insoluble i n water. G. H. M. It is only slightly soluble in water. An aqueous solution gives all the reactions of the nitrate. Xantho-rhodium Salts. By S. M. J~SKGENSEN (J. pr. Chem. [2], 34, 410-423) .-Xantho-rhodium nitrate, (NOz),( Rhs, 10NH)(3N03)4, is pre- pared by dissolving the chloropnrpureochloride in dilute sodium hydroxide on the water-bath, and then adding pure sodium nitrite and dilute nitric acid ; the salt separates as a, white, crystalline powder which can be recrystallised from hot water.Heated over a flame, theINORWNIC CHEMISTRY. 115 salt explodes and leaves a voluminous residue of rhodium. The xanthonitrate is fairly soluble in cold, easily in hot water ; insoluble in alcohol. Its aqueous solution, unlike that of the nitratonitrate, is not converted into the roseonitrato by boiling. It is also unacted on by sodium hydroxide, ammonium sulphide, &c. Xantho-rhodium chloride. (NO,),(Rh,,lUNH,) C14, is prepared in the same way as the nitrate, adding dilute hydrochloric acid, however, instead of nitric acid after the sodium nitrite, when the salt separates RS a white powder ; or from the nitrate, by filtering a concentrated solution of the latter into dilute hydrochloric acid, the addition of alcohol then throws down a yellowiBh-white precipitate of small octa- hedrons.When heated, the salt is decomposed, and leaves a residue of pure rhodium. Treated with silver oxide and water, the chloride yields a solution oExantho-rhodium hydroxide, which behaves as a strong a1 kali. Xantho-rhodium platinochloride, (NO&( Rhz,10NH3) (PtC16)2, is ob- tained as a buff -colonred precipitate consisting of microscopic needles by adding hydrogen platinochloride to a solution of the nitrate. This salt is analogous to the corresponding cobalt and chromium salts. Xuntho-rhodium bromide, (NOz),( Rhz,10NH3)Rr4, is obtained as a white, crystalline preciphate on adding concentrated hydrobromic acid to a cold solution of the nitrate.I t is easily soluble in water, and the solution gives all the reactions of the nitrate. Xardho-rhodium dithionnte, (NO,),( Rh,,lONH,)(S,O,), + 2H20, is prepared by filtering a cold solution of the nitrate into an excess of sodium dithionate. It forms a white, crystalline precipitate consisting of microscopic prisms. Xuntho-rhodium sulphutes are prepared by treating the chloride with strong sulphuric acid, &c. (a) The normal salt, It loses all its water at 100". (NOz) 2 ( Rh2,10NH3) ( S O&, crystallises in Bat, brilliant, needles many centimetres long. It may also be obtained by precipitating a solution of the acid salt with alcohol.The salt explodes on heating. With a solution of iodine in potassium iodide, it yields a periodide. ( b ) The acid salt, 2[ (NO,),(€th,,lONH,)( SO&],( H2S04),, crystallises in long, white needles. The salt decomposes quietly on heating, leaving the rhodium in pseudomorphs of the crystals. Xuntho-rhodium siZicoJZuoride, (NO,),( Rh,,lONH,)( SiF6),, is obtained AS a snow-white, silky precipitate on adding a cold solution of the nitrate to an excess of hydrofluosilicic acid. Under the microscope, i t consists of small rhombic tables resembling the chloropurpureo- rhodium silicofluoride. Dilute nitric acid decomposes it, forming the nitrate and free acid. Xatztho-rhodium oxaZate, (NO,),( Rh2,10NH3) ( C,O,),, is obtained as a white precipitate consisting of microscopic prisms, by adding a solu- tion of the nitrate to excess oE ammonium oxitlate.Nitric acid decomposes it in the same way as the silicofluoride. The roseo- and purpureo- as well as the xantho-salts of rhodium show a most unmistakable resemblance to those of cobalt and chro- miurn. The xantho-rhodium salts are, however, much mom stable116 ABSTRACTS OF CHEMICAL PAPERS. than those of cobalt and chromium. The nitrate is especially so, showing that the xantho-salts are really nitritopurpureo-salts. The great stability of the nitrate is partly accounted for by the nature of the metal, and also probably partly by the fact that pentad nitrogen is combined with pentad nitrogen, thus :- 0 : N.0.106 ABST tiACTS OF CHEMICAL PAPERS.In o r g a n i c C h e m i s t r y.Action of Hypochlorous Anhydride on Iodine Trichloride.Ry H.BASSETT and E. FIELDING (Chem. News, 54, 205--206).--Iodicanhydride is the main product of the reaction when solutions ofiodine trichloride and’ hypochlorous anhydride in carbon tetrachlorideare mixed, or when a current of bypochlorous anhydride is passedthrough a solution of iodine trichloride, or even over solid trichloride.In the last case, the action is very slow. D. A. L.Saturation of Selenious Acid by Bases. By C. BLAREZ (Conzpt.rend., 103, 804- 806). -With cochineal or helianthin (methyl-orange), selenious acid is monobasic. With litmus, it is monobasic toammonia, lime, strontia, and baryta, but if soda or potash is used thelitmus only becomes blue-violet when about 1.5 equivalent of alkaliis added.With phendphthalein. and potash, soda, ammonia, lime orstrontia, the colour change takes place when somexhnt more than1.5 equivalent of alkali is added, but with phenolphthalein and barytaselenious acid is bihasic,, and the colour change is sharp and distinct.Selenious acid can be accurately titrated by means of standardbarytn solution, using helianthin or phenolphthalein as indicator.The bavyta has double the value with the first indicator that i t haswith the second. Both indicators can be used in the same solution ;the rose colour of the heliauthin disappears when the acid is halfsaturated, and the rose colour due to the change of the phenol-phthalein becomes visible when saturation ik complete.As no.basic barium selenite is formed when baryta is present inexcess, an excess of baryta can be determined by means of phenol-phthaleh and a standard acid in the liquid containing the precipitatedbarium selenite.Selenious acid, like sulphurms acid, cant be estimated in presenceof other acids by means of baryba, provided that the tofal basicity ofthese acids is indicated by helianthin. Helianthin and phenol-phthaleln are both a;dded to the same solution, and the amount ofselenious acid is calculated from the quantity of bnryta solutionrequired to produce the second colour change, this quantity beingexactly half that which would be required to neutralise the seleniousacid alone with phenolphthale’in as the indieator. C. H, B.Formation of Nitrites- By S.KAPPEL (Arch. Pkarm. [3], 24,897--900).--The author has extended his observations made on theaction of copper, iron, and zinc in contact with the air, and solutionsof ammonia and the fixed alkalis (AbsBr., ’1883, 282, 286), employingin recent experiments magnesium, aluminium, and tin. Magnesiumexposed to the a i r in contact with aqueous potash, gave small quan-tities of nitrous acid, ozone, and hydrogen peroxide. With ammoniasolution, strong indications of nitrous acid were obtained. Alnmiriiumin potassium hydrate produced nitrous acid readily, even in the coldINORGAKIC CHEMISTRY. 107nitric acid and hydrogen peroxide were also easily detected. Withammonia the action was much slower. Tinfoil gave scarcely anyreaction ; nitrous acid was not produced, but hydrogen peroxide wasperceptible. J.T.Compounds of Arsenious Anhydride with HaTogen Salts.By F. R~UORFF (Ber., 19,2668--2679).-1n this paper the preparationand properties of compounds of the halogen salts of the alkali metalswith arsenious anhydride are described. These are best obtained bypassing carbonic anhydride info a mixed solution of potassium arseniteand the halogen salt. These componnds separate either in the amor-phous form or in indistinct crystals, of the general formula MX,2As203,sparingly soluble in water, insoluble in alkaline carbonates, but verysoluble in the free alkalis; when heated, they decompose with elimi-nation of arsenious anhydride, the compound KI, 2As,03 decomposinga t 350" ; KBr,2As20z a t 380" ; and KCI,As203 a t 240" ; a compound,KC1,2Asz0,, is also described.The ammonium compoundsNH41,AsL03, NH4Br,2As,C3, and NH4Cl,As20,, are also described,those of sodium being reserved for a future communication.V. H. V.Some Probable New Elements. By A. PRINGLE (Chem. News,54, 167-168).-TThe author claims to have discovered some new sub-stances, including five metals and a substance resembling selenium,called hesperisiztm, in some " Lower Silurian " rocks, situated in thecounty of Selkirk. One metal is said to be like iron, but gives neitherthe thiocyanate nor the tannic acid reaction ; one is Eke lead in appear-ance, is easily fused and volatilised, and yields yellow and green salts ;another which is charcoal-black, is called erebodium,; its equivalent is95.4, and it forms several oxides. A fourth, g a d e n i m , with equivalentabout 43.6, a light-grey powder, forms a red monoxide and a cream-coloured dioxide, yielding respectively white and yellow saltp.Another, polymnesturn (Pm), is a rather dark-coloured metal, withequivalent about 74.A preliminary description of four oxides, PmO,PmOs, PmO,, and (?)I Pm05, of two sulphides, PmS and PmSp, andof other compounds is given. D. A. L.Production of Alkali Metals. By H. Y. CASTXER (Chem. News,54, 218--SlS).--Irou reduced by hydrogen or carbonic oxide ismixed with t a r in proper proportions, so that after the mixture iscoked it has a composition about = FeCp The coke is finely ground,mixed with c a s t i c soda (or potash) in proportions = 3NaHO +E'eC,, or about 100 NaHO to 15 of coke. This mixture is introducedinto a cast-iron crucible, and heated in a specially arranged furnace(described in the paper).The reduction and distillation commence ata temperatnre of 1000". When the operation is finished the crucibleis removed, and another immediately put in its place. The residueconsists of some sodium carbonate, and finely divided iron; thesodium carbonate is recovered, the iron used to make fresh reducingcoke, aiid the crucible is used over and over again. The advantagesover the old method are manifest. D. A. L108 ABSTRACTS OF CHEMICAL PAPERS.Crystalline Scale formed in the Manufacture of SodiumHydrogen Carbonate. By G. W. LKIGHTON (Amer. .J.Xci., 33,318--.319).-This scale was formed in the manufacture of sodiumhydrogen carbonate by the ammonia process, at Syracuse, New Pork.It was deposited on the inner surface of an iron tank, and had theappearance of boiler-scale, being 1 to 2 inches thick, with a vitreouslustre, and a greenish-grey colour. It is usually covered with crystalplanes, proving to be the termination of prisms (probably monoclinic).Analysis gave the following results :-NaC1. Na2C0,. MgCOB. CaC0,. FeCO,. H20. CO,. Total.22.23 40.62 31.57 3.56 0.08 0.63 0.64 99.33The scale is evidently a triple sait, represented by the formulaMgCO,,Na,?CO,,NaCl. It is, in fact, a definite crystalline product ofan interesting constitution, not unlike that of several well -definedmineral species, in which an alkaline chloride appear8 to be in mole-cular combination with heterogeneous materials.By C .HEYER (Ber., 19, 2684-2690).-When strontium hydroxide is heated to bright redness, it is convertedinto strontium oxide. When the latter is exposed to air saturatedwith aqueous vapour, and then to dry air at the ordinary femperature,strontia dihydrate, Sr0,2H20, is obtained as a white, crystallinepowder.I Dry strontia dihydrate, when heated with dry carhonic anhydride,is completely converted into carbonate ; the monohydrate, however,absorbs only traces of carbonic anhydride. The water in the dihy-drate was determined by passing dry carbonic anhydride over t h esubstance for five hours at 26*5", and for 40 minutes at 121.5", andabsorbing the water in sulphuric acid bulbs.These results are notin accordance with those obtained by Scheibler (Abstr., 1886, 927).N. H. M.B. H. B.Strontia Dihydrate.Calcium Borate. By B. BLOTJNT (Chem. News, 54,208-209).-The salt obtained by fusing freshly calcined lime with boric anhydrideover a Bunsen burner is CaB,O,. I t is possible that t4he salt obtainedon a platinum wire loop before the blowpipe, with large excess ofboric anhydride, contains a larger proportion of boric acid.D. A. L.Calcium Ammonium Arsenate and Calcium Arsenates. ByC. L. BLOXAM (Chem. News, 54, 268-170 ; 193--194).-1n a previouscommunication (Abstr., 1886, 920), mention is made of a calciumammonium arsenate. Various observers differ as to the compositionof this salt and as to the amount of water it contains.The amount'of water appears to vary somewhat with the state of the atmosphere,and hence, prohably, the cause of the difference of opinion on thispoint. It is now shown theoretically and experimentally that the*precipitate produced by arsenic acid in a solution of calcium chloridecontaining free ammonia hae the following composition :INOROANI C CHEMISTRY. 109Air-dried.. ........................ CaNHAsSOh + 7H20.Dried in a vacuum over sulphuric acid, Ca3NH4HZ(As04), + 3H20.Dried at 100". ..................... Ca6NH4H6(AsO& + 3H,O.Ignited ........................... CazAs,Oy.I t is suggested to use the precipitation of calcium as calcinm ammo-nium arsenate for quantitative purposes ; it ie convenipnt, the precipi-tate being crystalline and bulky, but is not susceptible of such greataccuracy as the oxalate method.It is recommended for checkinghardness determinations in water analysis. Its various advantagesand disadvantages as a method aye discussed. On evaporating downa hydrochloric acid solution of calcium ammonium arsenate withplatinic chloride, the platinochloride after ignition was observed t o bemixed with fine, white, opaque, prismatic crystals of the orthoarsenateCa3(As04)2, insoluble in acids. A repetition of the experiment re-sulted in the production of a substance somewhat similar in appearance,namely the meta-arsenate C ~ ( A S O ~ ) ~ ; the same substance is formedwhen mixtures of arsenious anhydride and calcium carbonate areignited, and is left as an insoluble, crystalline powder when the ignitedmass is treated with hydrochloric acid.Artificial Lead Silicate from Bonne Terre, Missouri.By H.A. WHEELER (Amer. J. Sci., 32, 272--273).-E. S. Dana and S. L.Penfield hare given (Abstr., 1886, 317) some crystallographic deter-minations and apalyses of this artificial mineral from the DeslogeLead Co., of Boxine Terre. Since the publication of that paper, theauthor has examined some specimens in the metallurgical collectionof Washington University. The results of his analysis are asfollows :-D. A. L.Si02. PbO. Fe203. Al20,. CaO. MgO.I .... 17.11 73.66 0.80 0.53 2.35 0.22I1 .... 18.51 '72.93 1.31 0.62 1.66 0.201C1. Nn20. Ni0. Total.I ....0.08 2.22 3.06 100.03I1 .... undet. undet. undet. 95.23I, coarse crystals; 11, fine crystals. The iron in these analyseswas assumed to be in the form of ferric oxide. B. H. B.Equivalent of Gadolinium Oxide. By A. E. NORDENSKIOLD(Cowzpt. rend., 103, 795-798).-Gadolinium oxide is the mixture ofjttrium, erbium. and ytterbium oxides, which was first obtainedfrom the gadolinite found at Ytterby. It is precipitated by ammoniaand ammonium oxalate as well as by potassium sulphate, and thethree constituents cannot be separated quantitatively.The gadolinium oxide obtained from kainosite, the silicocarbonateof yttrium, erbium, and ytterbium, recently discovered at Hittero, inNorway, has the molecular weight 260 2 it 0 = 16 and the formulaof the oxide is taken as &03.This number is practically identicalwith the molecular weight of the similar mixture of oxides obtainedVOL. LII. 110 ABSTRACTS OF CHEMICAL PAPERS.by different observers (Nordenskiold, Lindstrom, Engstrom, Cl b e )from gadolinite, kainosite, azzhenitc, xenotime, fergusonite, clevite,fluocerite, and eudialite. These minerals are found in differentlocalities, and contain the oxides in combination with different acids,such as silicic, pbosphoric, niobic, or tantalic acid. Moreover, theoxides have been separated by somewhat different methods, and yetin all cases the greatest variation from the mean value for the mole-cular weight, 261.9, is one per cent., a variation which is within theerror of experiment, and is not greatel.than the alterations whichhave been made in recent times in the atomic weights of some of thebetter known elements. It follows therefore that gadolinium oxide,although not thc ozide of a simple substance, but a, ?nixtwe of threeisomorphous oxides, has a constant molecular weight, even whrrt obtained.from totally &#went minerals found in widely separated localities. Thisis the first instance of the coexistence of three isomorphous substancesin constant DroDortions. The exdanation of this fact seems to be aproblem andogius to that of the brigin of the minor planets.C. H. B.Formation of Ultramarine in the Wet Way. By I?. KNAPP( J . 237'. Chem. [ d ] , 34, 328-340).-An account of some further ex-periments on the formation of ultramarine by the exposure of a heatedmixture of kaolin, soda, and sulphur, to a damp atmosphere, or treat-ment of the same with liver of sulphur (Abstr., 1886, 306).Thevarious conditions necessary for success are discussed in full, such asthe degree of aggregation of the liver of sulphur and the form ofsilicate or silica used. Thus experiments with quartz were unsuc-cessful, and those with silicic acid jelly from soluble glass led to theproduction of it bluish-green material, which turned to a deep blueon warming. Pure alumina led to no result, but sodium aluminategave a very satisfactory product. Salts of sodium, such as the thio-sulphate, or even calcium phosphate, produced very fine specimens ofultramarine-blue. V. H. V.Sodium Dichromate. By A.STANLEY (Chem. News, 54,194-196).-Sodium dichromate crystallises wi1,h 2 mols. HzO, in prisms andplates belonging to the triclinic system; its sp. gr. is 2.5246 at 13"; i tis deliquescent. It loses 1 mol. H,O below 75", and all below loo",leaving a light brown, anhydrous salt, which fuses to a transparentdark red liquid a t 320°, and on cooling cr~stallises in the same formsas the hydrated salt, When treated with water, the anhydrous saltcauses a rise, and the hydrated salt a fall in temperature. 100 partsof the saturated aqueous solution contain-Temperature.. 0" 15" 30" 80" 100" 139"Parts Na&r2O7 107.2 109.2 116-6 1428 162.8 209.7The saturated solution boils at 139". A table of the sp. gr. of soh-tious of various strengths is given.Sodium dichromate is insolublein ether, slightly soluble in alcohol. I t is very hygroscopic, in48 hours an exposed sample absorbed one-third its weight of water ;a sample of calcinm ch1or:de under fiimilar circumstances absorbeINORGANIC CHEMISTRY. 111.nearly its own weight of water. It decomposes slightly above itsmelting point, and a t a dull red heat leaves sodium chromate andchromic oxide, In its reactions generally it resembles potassiumdicliromat e.By dissolving the dichromate in warm aqueous chromium trioxide,the trichromate separates on cooling in dark red crystals ; these a r every solnble in water, and are deliquescent.By the action of sodium dichromate on freshly prepared cupriohydroxide, a brown powder is formed, consisting of microscopiccrystals of the composition Na2Cr04,CuCrz07,2Cu0 + 4H20- It isalmost insoluble in water, and but slightly soluble i n alcohol.It losesall its water below loo", and partially decomposes a t higher tempera;tures, cupric oxide separating.Magnesium sodium chromate, prepared by neutmlising sodiumdichromate with magnesia, crystallises with 3 mols. H20, in yellowfour-sided prisms and plates. It is soluble in water and alcohol, butinsoluble in ether. The 3 mols. H,O are driven off below 200°,leaving a dark reddish-brown powder, which fuses at a red heat withpartial decomposition. D. A. L.Reduction of Inorganic Thio-salts by Hydrogen.. By G.K R ~ ~ S S and H. SOLEREDER (Bey., 19, 2729--2759).--By the reductionof molybdothio-salts by hydrogen at a red heat, salts of a lowermolybdosulphide could not be obtained ; potassium thiomolybdate andammonium dithiomolybdate are gradually redaced t o a mixturn ofmolybdenum and potassium sulphide and to molybdenum.I n the caseof ammonium dithiomolybdate, no oxpulphide could be obtained.Potassium thallium sulphide, K2TlaS4, behaves k a similar manner,being reduced to potassium sulphide and thallium.The salts of such thio-acids as remain unchanged in a currentof hydrogen are not reduced; for example : R2S,3ZnS ; K,S,SCdS,&3. If the thio-acid is merely reduced to -a lower stable sulphide,the corresponding thio-salt yields also the lower sulphide or itsthio-salt in the case of its having the properties of a thio-acid.Examples : K2S,3Cu2S,Cu,S2, K2S,Fe2S3.Atomic Weight of Tungsten.By J. WADDBLL (Amer. Chem. J.,8, 280--288).--ScheeIite was decomposed by nitric acid, and theimpure tungsten trioxide freed from silica as follows :-The mixture isfused with an equal weight of hydrogen potassium sulphate until ina state of limpid fusion; the cool mass is digested with water andfiltered ; water containing ammonium carbonate must be used for thefurther washing to keep the fluid from running through turbid, andto assist in the solution of the tnngstate. If the silica is to be esti-mated it will probably require a second fusion, &c., with acid potas-sium sulphate. Another method of separating tungstic acid andsilica is by means of ammonia, but here also the extraction is apt $0be incomplete.Commercial metallic tungsten is but slowly attackedby acids, it cannot be fused with nitre without attacking thecrucible, and is therefore best oxidised by a current of air a t ared heat.The product is fused with sodium carbonate, and after dissolutionN. H. M.i 112 ABSTRACTS OF CHEMICAL PAPERS.filtered from uaoxidised material. The filtrate boiled with ammoniumcarbonate gave a smail precipitate of alumina. To remove molyb-denum, tartaric acid is added (half the weight), then hydrochloricacid (no tungstic acid is precipitated), and sulphuretted hydrogenpassed. The blue filtrate is decolorised by a current *of air, andthe tungsten separated in 11 fractions by boiling with hydrochloricacid. Fractions 3, 7, and 10 were purified for determination of theatomic weight by solution in ammonia, reprecipitation by hydrochloricacid, and roasting of the precipitate in a current of air.The analysiswas effected by heating gradually in a current of hydrogen, using aporcelain boat and tube, and a Fletcher’s blast furnace. No. 3 gaveW = 184.50, No. 7 184.00, and No. 10 183.67, when 0 = 16. Thefirst number is to be considered most accurate, namely, W = 184.50,0 = 16; or W = 184.G4, 0 = 15-96. The specific gravity of thissample of metal is 18.77.Compounds of Gold and Nitrogen. By I?. RASCHICI (Annnlen,235, 341-368).--Aurous oxide, Au20, is most conveniently preparedby boiling a solution of mercurous nitrate with an excess of auricchloride, as descritled by Figuier (Ann.Chim. Phys. [3], 11, 336).The precipitate dried over phosphoric anhydride contains 2 11301s.HzO. When strong ammonia is added to water containing aurousoxide in suspension, a black explosive powder, NAu3,NH3, is obtained.Boiling with water, or with dilute acids, converts the sespui-auroamineinto triauramine, NAu3. Met hylamine also acts on aurous oxide,forming diauromethy Zamine, NM eAuz. This compound also loses halfits nitrogen when boiled in water for 15 minutes. Gold monoxide,AuO, was first obtained in a pure state by Schottlander (Abstr., 1883,853). It is converted by strong ammonia into the very explosivecompound sespu ihydrazhry Zamine, NH,,N( AuOH)~. Warm hydro-chloric acid dissolves two-thirds of the gold, but one-third is left inthe metallic state.On boiling with water, half the nitrogen isexpelled, and trihydraurylamine remains. Methylamine unites withgold monoxide, formirig the compound MeN(AuOH)a ; this loses halfits nitrogen in the form of methylamine when boiled in water. Theauthor confirmsthe accuracFof Dumas’s formula, (AuN + NH3)2+ 3H20,for the fiilminating gold prepared by the action of ammonia on auricoxide, Auz03 ; but he proves t h a t t<he substance which is precipitatedby ammonia from a solution of auric chloride is a mixture of thepreceding compound and auric imidochloride, NH : AuCl. The lattercompound is obtained in an impure state when a, hew drops ofammonia are added to a large excess of auric chloride. Only a por-tion of the chlorine can be removed by digestion with ammonia.Fulminating gold is slowly attacked by boiling water, losingammonia.Boiling with nitric acid renders the compound moreexplosive. Dilute sulphuric acid does not liberate ammonia, butforms a very explosive substance of the composition ( AuN2H3),,H28O4.The constitution of auric diamine is represented by the formulaNH,*Au : NH. The decomposition it undergoes when boiled withwater is probably 2NHzAuNH = NH : AuNMethylamine yields a, yellow precipitate with auric chloride, solubleH. B.AuNH2 -I- NHsINORGAN10 UHEMISTRT. 113in an exoess of the reagent. On warming the solution, a bibown pre-cipitate which contains a large quantity of chlorine is deposited.Auric oxide yields a red compound with methylamine.Complex Inorganic Acids.By W. GIBBS (Amer. Chem. J., 8,289-290 j .-Compounds have been obtained comparable with thechlorplatinophosphoric acids of Schutzenberger. These compoundsare to be regarded as phosphoric acid in which one atom of oxygen isreplaced by platinous chloride, bromide or oxide, or the correspondingcompounds of palladium, iridium, ruthenium, and osmium. More-over the phosphorus may be replaced by arsenic or antimony. Thefollowing formula? are given to the compounds so far studied :-w. c. w.As,0,3( As203,2Pt0),5 (NH4)aO + 7H20 ;fAs,O3,2PtCI,)K,O + 2HzO ;~ ~ W O ~ , A S ~ ~ ~ , ~ ( A S ~ O ~ , ~ P ~ C ~ , ) , ~ ~ P ~ ( + 60R2O j23 W O ~ , ~ A S ~ O ~ , ~ ( A S ~ O ~ , ' ~ P ~ O ) 6Pt (N&),O + 4OH2O ;~~XOO~,AS~O~(AS~O~,~P~O)~P~(NH~)~O + 27H20.H.B.Roseo-rhodium Salts. By S. M. JORGENSEN (J. pr. Chem. [2],34, 394-406 ; compare Abstr., 1883, 1058) .-Boseo-rhodium nitrate,( Rh2,10XH,,2Hz0) (NO,), is obtained by adding moderately dilutenitric acid to a concentrated solution of roseo-rhodium hydroxide,when i t separates as a white precipitate consisting of microscopic,quadratic tables. It loses 2 mols. of water at loo", and is convertedinto nitratopurpureo-rhodium nitrate.Roseo-rhodiunz platinochloride witrate, ( Rh2,1 0NH3,2H,0)(N0,),PtC16 + 2H20, is obtained as a beautiful, orange-yellow, crystalline pre-cipitate on adding hydrogen platinochloride to a solution of thenitrate. It emily loses 2 mo1s. of water at 100°, the other 2 mols.are given off more slowly, and nitratopurpureo-rhodium platinochlorideis formed; on treating this with dilute hydrochloric acid all theplatinum is dissolved, leaving white nitratopurpurco-rhodium chlorideundissolved.A solution of the latter in water give8 wit4 sodiumdithionate a precipitate of the characteristic nitratopurpureo-dithionate.Roseo-rhodium bromide, ( Rh,,10NH3,2H20j,Br6, is prepared by addingconcentrated hydrogen bromide to a solution of roseo-rhodiumhydroxide. It forms a crystalline powder consisting of small octo-hedrons or six-sided tables. At loo", it loses 2 mols. H20 a.nd isconverted into the bromopurpureo-bromide. It is easily soluble i ncold water, and its aqueous solution gives the same reactions as Chenitrate.Roseo-rhodium sutphate, ( Rhz,10NH3,2E20) (SO& + 2H20, is pre-pared by saturating the hydroxide with dilute sulphuric acid, andprecipitating with alcohol.It forms a white precipitate of very smalloctohedral crystals. 'In contrast to the other roseo-rhodium salts, i t isnot converted into the purpureo-salt by solution in boiling water ; i tcrystallises in large, quadratic prisms, terminated by a quadraticpyramid, apparently isomorphous with roseocobalt sulphate. At looo,i t quickly loses 4 mols. H20, and then more slowly another 4 mol.,undergoing a similar ahanga to the analogous roseooobitlt salt, form-It is easily soluble in water114 ABSTRACTS OF CHEMICAL PAPERS.ing luteo-salts. Bn aqueous solution gives all the reactions of thenitrate ; with potassiiim iodide, it gives a white precipitate, consistingof microscopic octohedrons of the roseoiodide sulphate,(Rh,,lONH,,2HzO)I,(SO,)2.Roseo-rhod ium platinochloride sdyhnte, ( Rhz, 1 O?SH3,2H20)PtC16( SO,)?,is obtained as ti beautiful, silky, buff precipitate of very thin six-sidedtables, by adding a solution of hydrogen platinochloride to a coldsolution of the roseo-sulphate.It seems to be isomorphous with thecorresponding roseo- and luteo-salts of cobalt and chromium.Roseo-rhodium orthophoyhzte, ( Rhz,10NH3,2H20) (PO4H)s + 4Hzo,is prepared by adding a 10 per cent. solution of phosphoric acid to aconcentrated solution of the hydroxide. It forms a white, crystallinepowder which behaves like the correFponding cobalt salt.Sodium roseo-rhodium pyrophosphate, ( Rhz,10NH3,2H,0),P20,Na +23H20, is obtained by adding sodium pyrophosphate to a solution of thehydroxide iu dilute hydrochloric acid until the amorphous precipitatea t first formed is redissolved ; on shaking, the salt then separates as asilky, white crystalline precipitate.It agrees in all respects with thecobalt salt.Koseo-rhodium cobalticyanide, (Rh,,10NH3,2HzO),COzCyn, is obtaineda s srnall pale-yellow crystals on adding a solution of potassium cobalti-cyanide to the hydroxide, neutralised with dilute sulphuric acid.Nitratopurpureo-rhodium Salts. By S . M. JORGEXSEN ( J . pr.G. H. M.C'hem. ['L], 34, 40 -109) .-Nitratopur~ureo-rhodiunz nitrate,is easily obtained by heating the roseonitrate or by dissolving this saltin hot water, adding an equal volume of Concentrated nitric acid,heating the mixture for some time on the water-bath and then allow-ing it to cool, when the salt separates in small, octohedral, whitecrystals with a greenish-yellow tinge.Heated over a flame, the saltexplodes.Nitrat~urpureo-rhoa~u~n chloride, (K 0,) L( Rhp, 10NH,)Cl,, is obtainedas a pale greenish-yellow precipitate on filtering a, cold solution of thenitrate into an ice-cold mixture of 3 vols. hydrochloric acid and 1 vol.water.Nitratopurpureo-rhodium dithionate, (NO,),( Rhz,10NH3)( Sz06)2 +2H20, is prepared by precipitating a cold saturated solution of thenitrate or chloride with sodium dithionate. It forms white, silkyX-shaped aggregations resembling the corresponding cobalt salt.The air-dried salt loses all its water a t 100".It is quite insoluble i nwater. G. H. M.It is only slightly soluble in water.An aqueous solution gives all the reactions of the nitrate.Xantho-rhodium Salts. By S. M. J~SKGENSEN (J. pr. Chem. [2], 34,410-423) .-Xantho-rhodium nitrate, (NOz),( Rhs, 10NH)(3N03)4, is pre-pared by dissolving the chloropnrpureochloride in dilute sodiumhydroxide on the water-bath, and then adding pure sodium nitrite anddilute nitric acid ; the salt separates as a, white, crystalline powderwhich can be recrystallised from hot water. Heated over a flame, thINORWNIC CHEMISTRY. 115salt explodes and leaves a voluminous residue of rhodium. Thexanthonitrate is fairly soluble in cold, easily in hot water ; insolublein alcohol.Its aqueous solution, unlike that of the nitratonitrate,is not converted into the roseonitrato by boiling. It is also unactedon by sodium hydroxide, ammonium sulphide, &c.Xantho-rhodium chloride. (NO,),(Rh,,lUNH,) C14, is prepared in thesame way as the nitrate, adding dilute hydrochloric acid, however,instead of nitric acid after the sodium nitrite, when the salt separatesRS a white powder ; or from the nitrate, by filtering a concentratedsolution of the latter into dilute hydrochloric acid, the addition ofalcohol then throws down a yellowiBh-white precipitate of small octa-hedrons. When heated, the salt is decomposed, and leaves a residueof pure rhodium. Treated with silver oxide and water, the chlorideyields a solution oExantho-rhodium hydroxide, which behaves as a stronga1 kali.Xantho-rhodium platinochloride, (NO&( Rhz,10NH3) (PtC16)2, is ob-tained as a buff -colonred precipitate consisting of microscopic needlesby adding hydrogen platinochloride to a solution of the nitrate. Thissalt is analogous to the corresponding cobalt and chromium salts.Xuntho-rhodium bromide, (NOz),( Rhz,10NH3)Rr4, is obtained as awhite, crystalline preciphate on adding concentrated hydrobromic acidto a cold solution of the nitrate. I t is easily soluble in water, and thesolution gives all the reactions of the nitrate.Xardho-rhodium dithionnte, (NO,),( Rh,,lONH,)(S,O,), + 2H20, isprepared by filtering a cold solution of the nitrate into an excess ofsodium dithionate. It forms a white, crystalline precipitate consistingof microscopic prisms.Xuntho-rhodium sulphutes are prepared by treating the chloride withstrong sulphuric acid, &c. (a) The normal salt,It loses all its water at 100".(NOz) 2 ( Rh2,10NH3) ( S O&,crystallises in Bat, brilliant, needles many centimetres long. It mayalso be obtained by precipitating a solution of the acid salt withalcohol. The salt explodes on heating. With a solution of iodine inpotassium iodide, it yields a periodide.( b ) The acid salt, 2[ (NO,),(€th,,lONH,)( SO&],( H2S04),, crystallisesin long, white needles. The salt decomposes quietly on heating, leavingthe rhodium in pseudomorphs of the crystals.Xuntho-rhodium siZicoJZuoride, (NO,),( Rh,,lONH,)( SiF6),, is obtainedAS a snow-white, silky precipitate on adding a cold solution of thenitrate to an excess of hydrofluosilicic acid. Under the microscope,i t consists of small rhombic tables resembling the chloropurpureo-rhodium silicofluoride. Dilute nitric acid decomposes it, forming thenitrate and free acid.Xatztho-rhodium oxaZate, (NO,),( Rh2,10NH3) ( C,O,),, is obtained as awhite precipitate consisting of microscopic prisms, by adding a solu-tion of the nitrate to excess oE ammonium oxitlate. Nitric aciddecomposes it in the same way as the silicofluoride.The roseo- and purpureo- as well as the xantho-salts of rhodiumshow a most unmistakable resemblance to those of cobalt and chro-miurn. The xantho-rhodium salts are, however, much mom stabl116 ABSTRACTS OF CHEMICAL PAPERS.than those of cobalt and chromium. The nitrate is especially so,showing that the xantho-salts are really nitritopurpureo-salts. Thegreat stability of the nitrate is partly accounted for by the nature ofthe metal, and also probably partly by the fact that pentad nitrogenis combined with pentad nitrogen, thus :-0 : N.0

ISSN:0368-1769    

DOI:10.1039/CA8875200106

出版商:RSC    

年代:1887

数据来源: RSC

摘要:

116 ABSTRACTS OF CHEMICAL PAPERS. M in e r a1 o g i c a 1 C h em i s t r y. Twin Crystal of Molybdenite. By W. E. HIDDEN (Amer. J . Sci., 52, dlO).-This crystal was found near Redrew, Canada, with other remarkable crystals, some of which weighed nearly a pound. The method of twinning seems to prove that molybdcnite should be referred to the hexagonal system. B. H. B. Limonite-pseudomorphs after Iron Pyrites. By J. G. MEEM (Amer. J. Sci., 32, 274-276) .-These limonite pseudomorphs are found near Lexington, Rockbridge Co., Virginia, occurring in the soil. In colour they vary from light-brown to almost black. Most of the crystals have undergone a complete alteration, there being no iron pyrites visible to the naked eye. In some, the unaltered iron pyrites is found forming a nucleus at the centre, in others it forms the bulk of the crjstal.The most commun form of these pseudo- morphs is the octahedron ; this generally occurs combined with the cube. On nearly all the octahedral faces, striations. running at right angles to the edges of these faces are observed. (Compare Abstr., 1886, 992.) B. H. B. Brookite from Magnet Cove, Arkansas. By E. S. DANA (Amer. J. Sci., 32, 314-317).--5. L. Penfield (Abstr., 1H86, 989) described a crystal of brookite of unusual form,from Magnet Cove. The author has studied the large series of brookite crystals from this locality in the collection of C. S. Bement. The planes he has determined o_n these crystals are as follows :-Pinacoids, =Pa, OP ; prisms, wP2, w P, mP2, new ; brachydome, 2Pi6 ; pyramids, +€’, iP2, $Pi, 1P2.B. H. B. By I?. W. CLARKE and J. 8. DILLER (Amer. J. Sci., 32, 211-217).--ht Los Cerillos, New Mexico, about 22 miles south-west of Santa Fb, are mines of turquois which have been worked for centuries. The turquois has never been fully aaalysed. It occurs buried in its matrix, sometimes in nodules, often in veins. It varies in colour from pure sky-blue to dark-green. For aualyses, three typical samples were selected-1, bright blue, faintly translucent ; 2, pale-blue, opaque, earthy, sp. gr. 2.805 ; 3, dark-green, opaque. Turquois from New Mexico. The results were as follows :-MINERUOOIOAL OEEMISTRY 113 Al,O,. &&.. HaO, L V - d P30, CuO, SiO,. CaO. Total. 19.80 39.53 31.96 6.30 1.15 0-13 98-87 19.60 36.88 2-40 32.86 7-51 0.16 0.38 99.79 18.49 37.88 4.07 28.63 6.56 4.20 - 99.83 In discussing these results, it is advisable to compare them with the figures given by Church for the Persian variety (Chem. News, 10, 290), and with those given by Moore (Abstr., 1885, 958) for Cali- fornian turquois, pseudomorphous after apatite.These analyses, ignor- ing the dark-green variety (3), agree well with each other in their atomio ratios. The tnrquois is shown by these analyses to be a v&- able mixture of the salts, 2Al2O3,P2O6,5H20, and 2CuO,PzO6,4H~0. The former formnla may be regarded as that of normal turquois, and may be within A&HPO,jOH),. The copper salt to which the mineral owes its calour is to be considered as an impurity, a view confirmed by the analysis of the dark-green variety (3).A microscopic study of the turquois indicatea that the mineral may have been derived from the alteration of another substance (apatite) with which the vein was formerly filled. The turqaois-bearing rock appears to be eruptive, and probably of tertiary age. Under the microscope, it is seen to be composed of felspar, with a considerable amount of biotite, epidote, iron pyrites, limonite, and some amorphous substance. B. H. €3. A Remsrkable Crystal of Herderite. By W. E. HIDDEN (Amer. J. Sci., 32, 209).--This crystal was found at the locality near Stone- ham, Maine (Abstr., 1884, 827, 1102). Excepting YF2, mP2, and cnP& all the planes observed in the American crystals occur on thie crystal, and one new plane, Ps, is seen to be present. The crystal has a diameter of 25 mm., and in point of size and perfection is un- 6qualled.The planes occurring are 13 in number, with several others slightly indicated. The mean index of refraction for this species for yellow rays is found by Des Cloixeaux to be 1.609. Pseudornorphe of Garnet. By S . L. PENFIELD and F. L. SPEERT Amep. J. Xci., 32, 307--311).-Pseudomorphs of garnet occur in abundance in a bed of chloritie schist overlying the great magnetite bed of the S urr-Michigamme iron range. The crystals are invariably dodecahedra[ varying in sp. gr. from 4.11 to 3-22; the heaviest crystals being nearly pure garnet, and the lightest ones almost wholly the decomposition product. Analysis of the garnet and of the decom- position products gave the following results :- B. H. B. SiOs.&03. Fe20:,. FeO. MnO. MgO. CaO. 1. 38-03 20.83 - 36-15 2.14 0.97 11-73 11. 2 i . 4 19.53 6.26 29-42 - 6.04 - 111. 29.08 19.94 3.91 30.48 0.20 5-36 0-23 N%O. K20. HSO. Total. I. - - - 100.85 11. 0.42 2.64 7.30 99.26 111. 0.29 366 6-53 99.90118 ABSTRACTS OF CHEmCAL PAPERS. I, pure gamet ; 11, decomposition prodncf from a crystal having a sp. gr. of 3.281 ; 111, the same from a crystal having a sp. gr. of 3-22. The decomposition product appears to be closely related to Sand- berger's aphrosiderite. The material in which the garnets are embedded is a, ferriferous chlorite, differing from the alteration product of the garnet, and agreeing closely with thuringite. The pseudomorph garnets from Salida, Chaffee Co., Colorado, differ from the Lake Superior garnets in that the decomposition product forms only a coating, whilst the interior of the crystal is quite homo- geneous. The following are analyses (I) of the pure garnet, sp.gr. 4.163: and (11) of the decomposition product, after deducting 1.04 per cent. of garnet :- SiOa. Al,O,. FeO. MnO. MgO. CaO. I. 37.61 22.70 33-83 1-18 3.61 1.44 11. 28.20 22.31 19.11 - 17.68 0.48 Na,O. KaO. H20. Total. I. - I - 100.31 11. 0.72 1-03 10.90 100.43 The changes which have been previously noted in garnet, differ from those described bv the authors, in that they have been the alteration of pyrope into ri6dolite or serpentine-like kagnesium silicates. B. H. B. Phenacite from Colorado. By W. E. HIDDEN (Amer. J. Sci., 32, 21O--'Lll).-Since the original annoiincement of the discovery by the author, of phenacite a t Florissant (Abstr., 1885, 878), many additional crystals have been found ; the best of them being sent to Professor Des Cloizeaux for examination.He observed 12 planes, amongst which it'2 is new for this species. North Carolina Mineral Localities. By W. E. HIDDEN and A. DES CLOIZEAUX (Avner. J. Sci., 32, 204-208) .-8poduutelze has been discovered in Sharpe's Township, Alexander Co. Physically the emerald-green spodumene (hiddenite) found, is iden tical with the yellow spodumene (triphnne) of Brazil. The three indices of refrac- tion were found to be : a = 1.677 ; = 1.669 ; ty = 1.651 for yellow rays, Black tourrnnZine, noteworthy from the brilliancy and number of the planes prese~ited, occurs a t the same locality. Twelve planes have been identified.Xenotime was discovered about 3 miles east of the Emerald and Hiddenite Mine, in Alexander Co. The colour of the crystals is hair- brown, and some of them are perfectly transparent. Sp. gr. 4.45 to 4.52. Twin crystals of monazite occur with the xenotime. Few finer examples of this rare mineral have ever been found. The crystals are transparent, red, and highly polished. They vary in size from 4 to 20 mm. in length and thickness. They are prismatic from an nn- usual extension of + P and + Pm. 9 distinct but imperfect cleavage parallel to the clinopinacoid wits observed on several crystals, whilst B. H. B. The cleavage is prismatic, and the habit long prismatic.MINERALOGICAL CHEMISTRB. 119 the common b a d cleavage was absent. The fact that common monazite is described as having perfect basal cleavage suggests that the difference may be due to the thorium silicate often present as an impurity.Quartz crystals with h a 1 plane.-Genuine basal planes are of very rare occurrence in the so-called basal-plane quartz crystals from North Carolina. In most cases, the planes observed have been produced by compression or juxtaposition, and when carefully measured do not meet the requirements. Mica from Leon Co., Texas. By G. W. LErGmoN (Amer. J. Xci., 32, 317--318).-This mica attracted notice. as it presents characters intermediate between those of the vermiculites and the muscovites. B. H. B. Analysis gave the following results :- SiO,. Al,O,. FqO,. MgO. CuO. N%O. K20. H30. Total. 48.95 25.17 9.40 1.69 trace trace 11.08 4.31 100.60 This composition agrees very closely with that of the mica from Hirschburg.It appears to be an early stage in the alteration of muscovite to vermiculite. B. H. B. Ceriferous Hainstadt Clays. By J. R. STROHECKER (Chem. Nms, 54, 207-208).-The author replies to the criticisms of Blom- strand and of Schertel (Abstr., 1886, 678) and re-a6rms the correct- ness of his statements (Abstr., 1886,,314, 424) as to the presence of the cerium metals in these clays. Crystalline Structure of Iron Meteorites. By 0. W. HUNT- INGTON (Amer. J. Sci., 32, 284-3@3).-From an exhaustive study of the very large collection of meteorites at Hervard College, the author concludes that many of the masses of meteoric iron now known are cleavage crystals, broken off probably by the impact of the mass against the atmosphere.These masses show cleavages parallel to the planes of all the three fundamental forms of the isometric or regular system. The Widmanstatten figures and Neumann lines are sections of planes of crystalline growth parallel to the same three fundamental forms of the isometric system. On different sections of meteorites, Widmanstatten figures and Neumann lines can be exhibited in evei-y degree with no break where a natural line of division can be drawn, The features of the Widmanstftten figures are due to the elimination of incompatible material during the process of crystallisation. The results of this invest,igation confirm the theory that the process of crystallisation must have been very slow ; the most, probable theory of the origin of meteorites seems to be that these masses were thrown off from a sun among the fixed stars, and that they were slowly cooled, while revolving in a zone of intense heat.B. H. B. New Meteoric Iron from Texas. By W. E. HIDDEN (ATner. J. Xci., 32,30&306).-This meteorite was found in 1882, in Maverick Go., Texas. It weighs 97a lbs., and mtlasures 12 by 10 by 6 inches120 ABSTRAOTS OF OHEMlOAL PAPERS. in its three diameters ; its shape being a nearly symmetrical ovoid, somewhat flattened. Tho surface is quite smooth, and coated with the usual thin black crust. Whena small surface is etched a peculiar appearance was presented. There are no Widmanstatten figures, except in traces. There are, however, two series o€ fine lines, cross- ing each other at angles of 70" and 110".which the author concludes to be due to twinning lamella. The meta1 is of unusual whiteuess, and is very soft. Analpis gave the following results :-- Fe . P. Ni + Co. Total. SP. gr. 94 90 0.23 (487) 100~00 7.522 B. H. B Meteoric Iron from Glorieta Mt., New Mexico. By G. F. KUNZ (Amer. J. Sci., 32, 311--313).-Since the publication of the account of the three masses of meteoric iron from Glorieta Mt. (Abstr., 1886, 321), three more masses of the meteorite have been found by J. H. Bullock, and a small piece was found by a Mexican, but it dis- appeared before i t could be Recured. Seven fragments have thus far been obtained. No. 4 weighs 2.65 lbs. ; No. 5, 2.48 Ibs. ; and No. 6, 2.31 lbs. All these fragments are figured and described by the author. A meteorite wag reoently presented to the Colorado Scientific Society by the Boston and Colorado Silver Mining Company, who re- ceived it from Albuquerque, Mew Mexico, as silver bullion.Its weight before cutting was about 5 lbs. An analysis of the iron gave the following result8 :- Fe. Ni. 00. Cu. Zn. C. P. S. Si. Total. 88.76 9.86 0.51 0.03 0.03 0.41 0.18 0.01 PO4 99.83 The striking similarity between this analysis and that of the Glorieta, meteorite, leads the author to believe that this iron is the seventh fragment of the meteorite found by the Mexican, and mistaken by him for silver bullion, B. H. B. Two hitherto undescribed Meteorio Stones. By- E. S. DANA and S. L. PRNFIELD (Amer. J. Xci., 32, 226-231).-1. Meteoritefrom Utuh.-This was found in 1869, in the prairie between Salt Lake City and Echo, and is now in the Pale collection, Its weight is 875 grams.It is oblong in shape, about 12 cm. long, and 9 cm. in its greatest width. The surface is comparatively smooth ; the colour of the crust being reddish-black. The interior of the stone is of a dark bluish- grey colour, distinctly mottled by its chrondritic character, and showing a rather large proportion of iron irregularly distributed through it, with minute patches of troilite. Olivine is the most prominent constituent. Bronzite appears i n irregular crystal frag- ments scattered through the mas8, and plagiaclase felspar is sparingly present in crystalline fragments. The sp. gr. of the meteorite was found to be 3 66. Analysis gave 17.16 per cent.of nickeliferous iron, and 89-84 per cent. of the mineral put, including the troilite and silicates, The iron gave on analyak-MINERALOGICAL CHEMISTR P. 121 Fe. Ni. co. cu. Total. 91.32 8.04 0.60 0.04 100.00 The mineral portion was divided into :-Soluble in hydrochloric acid ; troilite, 6.70 per cent. with 0.62 of NiS ; silicates, 48.85 per cent. Insoluble in hydrochloric acid, including chromite, 45.97. Water, 1.14. Total, 100.66. Analyses of the soluble (I) and insoluble (11) portions gave :- Si02. AI2O3. FeO. MgO. CaO. Na,O. I. 40.33 0.51 21.33 35.15 1.66 0.33 11. 54.83 4.82 8.64 24.56 3.341 1.98 K20. P,O,. Chromite. Total. 100*00 11. 0.12 - 1.71 100~00 I. 0.04 0.65 - The composition of the insoluble part implies that it is made np of brorizite with a little plagioclase.The Chantonnay metborite seems to bear the closest resemblance to the new stone. 2. Neteorite from Cape Gimrdeazc, Missouri.-This stone fell at 3 B.M., on August 14, 1846, accompanied by a, loud report. It became the property of the Yale Museum several years ago. The stone in the museum consists of two parts fitted together, and weighing together 2058 grams. The general shape of the stone is roughly rectangular, with dimensions of 12 by 10 by 10 cm. The surface is smooth, and, where fresh, is of a light grey colour. The metallic particles me scattered uniformly through the mass. The chondritic character is distinct. The sp. gr. of the stone was found to be 3.67. The analysis showed a relation of native iron to troilite and silicates very near that of the Utah meteorite, namely, 17.90 to 82.10 per cent, The iron gave on analysis- Fe .Xi. co. cu. Total. 91-93 7.39 0.63 0.05 100.00 The analysis of the mineral portion gave !-Soluble in hydrochloric acid : troilite, 6.95 ; silicates, 42.68. Insoluble in hydrochlcric acid, including chromite, 50.19. Water, 0.58. Total 100*40. The soluble (I) and insoluble (11) parts gave- Si02. AI20,. FeO. MgO. CaO. N%O. I. 36.32 - 22.31 4023 - 0-28 11. 55.79 5.54 7.91 23-65 3.35 185 I. 0.04 0.82 - 100~00 11. 0.24 - 1.67 100.00 K20. P20,. Chromite. Total. The insoluble part is evidently bronzite, with some felspar. The stone belongs t o the light grey chondrite type of meteorites. B. H. B.116 ABSTRACTS OF CHEMICAL PAPERS.M in e r a1 o g i c a 1 C h em i s t r y.Twin Crystal of Molybdenite.By W. E. HIDDEN (Amer. J . Sci.,52, dlO).-This crystal was found near Redrew, Canada, with otherremarkable crystals, some of which weighed nearly a pound. Themethod of twinning seems to prove that molybdcnite should bereferred to the hexagonal system. B. H. B.Limonite-pseudomorphs after Iron Pyrites. By J. G. MEEM(Amer. J. Sci., 32, 274-276) .-These limonite pseudomorphs arefound near Lexington, Rockbridge Co., Virginia, occurring in thesoil. In colour they vary from light-brown to almost black. Most ofthe crystals have undergone a complete alteration, there being noiron pyrites visible to the naked eye. In some, the unaltered ironpyrites is found forming a nucleus at the centre, in others it formsthe bulk of the crjstal.The most commun form of these pseudo-morphs is the octahedron ; this generally occurs combined with thecube. On nearly all the octahedral faces, striations. running at rightangles to the edges of these faces are observed. (Compare Abstr.,1886, 992.) B. H. B.Brookite from Magnet Cove, Arkansas. By E. S. DANA (Amer.J. Sci., 32, 314-317).--5. L. Penfield (Abstr., 1H86, 989) describeda crystal of brookite of unusual form,from Magnet Cove. The authorhas studied the large series of brookite crystals from this locality inthe collection of C. S. Bement. The planes he has determined o_nthese crystals are as follows :-Pinacoids, =Pa, OP ; prisms, wP2,w P, mP2, new ; brachydome, 2Pi6 ; pyramids, +€’, iP2, $Pi, 1P2.B. H. B.By I?. W.CLARKE and J. 8.DILLER (Amer. J. Sci., 32, 211-217).--ht Los Cerillos, New Mexico,about 22 miles south-west of Santa Fb, are mines of turquois whichhave been worked for centuries. The turquois has never been fullyaaalysed. It occurs buried in its matrix, sometimes in nodules, oftenin veins. It varies in colour from pure sky-blue to dark-green. Foraualyses, three typical samples were selected-1, bright blue, faintlytranslucent ; 2, pale-blue, opaque, earthy, sp. gr. 2.805 ; 3, dark-green,opaque.Turquois from New Mexico.The results were as follows :MINERUOOIOAL OEEMISTRY 113Al,O,. &&..HaO, L V - d P30, CuO, SiO,. CaO. Total.19.80 39.53 31.96 6.30 1.15 0-13 98-8719.60 36.88 2-40 32.86 7-51 0.16 0.38 99.7918.49 37.88 4.07 28.63 6.56 4.20 - 99.83In discussing these results, it is advisable to compare them withthe figures given by Church for the Persian variety (Chem.News, 10,290), and with those given by Moore (Abstr., 1885, 958) for Cali-fornian turquois, pseudomorphous after apatite. These analyses, ignor-ing the dark-green variety (3), agree well with each other in theiratomio ratios. The tnrquois is shown by these analyses to be a v&-able mixture of the salts, 2Al2O3,P2O6,5H20, and 2CuO,PzO6,4H~0.The former formnla may be regarded as that of normal turquois, andmay be within A&HPO,jOH),. The copper salt to which the mineralowes its calour is to be considered as an impurity, a view confirmedby the analysis of the dark-green variety (3).A microscopic study of the turquois indicatea that the mineral mayhave been derived from the alteration of another substance (apatite)with which the vein was formerly filled. The turqaois-bearing rockappears to be eruptive, and probably of tertiary age.Under themicroscope, it is seen to be composed of felspar, with a considerableamount of biotite, epidote, iron pyrites, limonite, and some amorphoussubstance. B. H. €3.A Remsrkable Crystal of Herderite. By W. E. HIDDEN (Amer.J. Sci., 32, 209).--This crystal was found at the locality near Stone-ham, Maine (Abstr., 1884, 827, 1102). Excepting YF2, mP2, andcnP& all the planes observed in the American crystals occur on thiecrystal, and one new plane, Ps, is seen to be present. The crystalhas a diameter of 25 mm., and in point of size and perfection is un-6qualled.The planes occurring are 13 in number, with several othersslightly indicated. The mean index of refraction for this species foryellow rays is found by Des Cloixeaux to be 1.609.Pseudornorphe of Garnet. By S . L. PENFIELD and F. L. SPEERTAmep. J. Xci., 32, 307--311).-Pseudomorphs of garnet occur inabundance in a bed of chloritie schist overlying the great magnetitebed of the S urr-Michigamme iron range. The crystals are invariablydodecahedra[ varying in sp. gr. from 4.11 to 3-22; the heaviestcrystals being nearly pure garnet, and the lightest ones almost whollythe decomposition product. Analysis of the garnet and of the decom-position products gave the following results :-B. H. B.SiOs.&03. Fe20:,. FeO. MnO. MgO. CaO.1. 38-03 20.83 - 36-15 2.14 0.97 11-7311. 2 i . 4 19.53 6.26 29-42 - 6.04 -111. 29.08 19.94 3.91 30.48 0.20 5-36 0-23N%O. K20. HSO. Total.I. - - - 100.8511. 0.42 2.64 7.30 99.26111. 0.29 366 6-53 99.9118 ABSTRACTS OF CHEmCAL PAPERS.I, pure gamet ; 11, decomposition prodncf from a crystal having asp. gr. of 3.281 ; 111, the same from a crystal having a sp. gr. of 3-22.The decomposition product appears to be closely related to Sand-berger's aphrosiderite. The material in which the garnets areembedded is a, ferriferous chlorite, differing from the alteration productof the garnet, and agreeing closely with thuringite.The pseudomorph garnets from Salida, Chaffee Co., Colorado, differfrom the Lake Superior garnets in that the decomposition productforms only a coating, whilst the interior of the crystal is quite homo-geneous.The following are analyses (I) of the pure garnet, sp. gr.4.163: and (11) of the decomposition product, after deducting 1.04per cent. of garnet :-SiOa. Al,O,. FeO. MnO. MgO. CaO.I. 37.61 22.70 33-83 1-18 3.61 1.4411. 28.20 22.31 19.11 - 17.68 0.48Na,O. KaO. H20. Total.I. - I - 100.3111. 0.72 1-03 10.90 100.43The changes which have been previously noted in garnet, differ fromthose described bv the authors, in that they have been the alterationof pyrope into ri6dolite or serpentine-like kagnesium silicates.B. H. B.Phenacite from Colorado. By W. E. HIDDEN (Amer. J. Sci.,32, 21O--'Lll).-Since the original annoiincement of the discoveryby the author, of phenacite a t Florissant (Abstr., 1885, 878), manyadditional crystals have been found ; the best of them being sent toProfessor Des Cloizeaux for examination.He observed 12 planes,amongst which it'2 is new for this species.North Carolina Mineral Localities. By W. E. HIDDEN and A.DES CLOIZEAUX (Avner. J. Sci., 32, 204-208) .-8poduutelze has beendiscovered in Sharpe's Township, Alexander Co. Physically theemerald-green spodumene (hiddenite) found, is iden tical with theyellow spodumene (triphnne) of Brazil. The three indices of refrac-tion were found to be : a = 1.677 ; = 1.669 ; ty = 1.651 for yellowrays,Black tourrnnZine, noteworthy from the brilliancy and number ofthe planes prese~ited, occurs a t the same locality.Twelve planes havebeen identified.Xenotime was discovered about 3 miles east of the Emerald andHiddenite Mine, in Alexander Co. The colour of the crystals is hair-brown, and some of them are perfectly transparent. Sp. gr. 4.45 to4.52.Twin crystals of monazite occur with the xenotime. Few finerexamples of this rare mineral have ever been found. The crystals aretransparent, red, and highly polished. They vary in size from 4 to20 mm. in length and thickness. They are prismatic from an nn-usual extension of + P and + Pm. 9 distinct but imperfect cleavageparallel to the clinopinacoid wits observed on several crystals, whilstB. H. B.The cleavage is prismatic, and the habit long prismaticMINERALOGICAL CHEMISTRB. 119the common b a d cleavage was absent. The fact that commonmonazite is described as having perfect basal cleavage suggests thatthe difference may be due to the thorium silicate often present as animpurity.Quartz crystals with h a 1 plane.-Genuine basal planes are of veryrare occurrence in the so-called basal-plane quartz crystals from NorthCarolina. In most cases, the planes observed have been produced bycompression or juxtaposition, and when carefully measured do notmeet the requirements.Mica from Leon Co., Texas.By G. W. LErGmoN (Amer. J.Xci., 32, 317--318).-This mica attracted notice. as it presentscharacters intermediate between those of the vermiculites and themuscovites.B. H. B.Analysis gave the following results :-SiO,. Al,O,.FqO,. MgO. CuO. N%O. K20. H30. Total.48.95 25.17 9.40 1.69 trace trace 11.08 4.31 100.60This composition agrees very closely with that of the mica fromHirschburg. It appears to be an early stage in the alteration ofmuscovite to vermiculite. B. H. B.Ceriferous Hainstadt Clays. By J. R. STROHECKER (Chem.Nms, 54, 207-208).-The author replies to the criticisms of Blom-strand and of Schertel (Abstr., 1886, 678) and re-a6rms the correct-ness of his statements (Abstr., 1886,,314, 424) as to the presence ofthe cerium metals in these clays.Crystalline Structure of Iron Meteorites. By 0. W. HUNT-INGTON (Amer. J. Sci., 32, 284-3@3).-From an exhaustive study ofthe very large collection of meteorites at Hervard College, the authorconcludes that many of the masses of meteoric iron now known arecleavage crystals, broken off probably by the impact of the massagainst the atmosphere. These masses show cleavages parallel to theplanes of all the three fundamental forms of the isometric or regularsystem.The Widmanstatten figures and Neumann lines are sectionsof planes of crystalline growth parallel to the same three fundamentalforms of the isometric system. On different sections of meteorites,Widmanstatten figures and Neumann lines can be exhibited in evei-ydegree with no break where a natural line of division can be drawn,The features of the Widmanstftten figures are due to the eliminationof incompatible material during the process of crystallisation.The results of this invest,igation confirm the theory that the processof crystallisation must have been very slow ; the most, probable theoryof the origin of meteorites seems to be that these masses were thrownoff from a sun among the fixed stars, and that they were slowlycooled, while revolving in a zone of intense heat.B. H. B.New Meteoric Iron from Texas. By W. E. HIDDEN (ATner. J.Xci., 32,30&306).-This meteorite was found in 1882, in MaverickGo., Texas. It weighs 97a lbs., and mtlasures 12 by 10 by 6 inche120 ABSTRAOTS OF OHEMlOAL PAPERS.in its three diameters ; its shape being a nearly symmetrical ovoid,somewhat flattened. Tho surface is quite smooth, and coated withthe usual thin black crust. Whena small surface is etched a peculiarappearance was presented. There are no Widmanstatten figures,except in traces.There are, however, two series o€ fine lines, cross-ing each other at angles of 70" and 110". which the author concludesto be due to twinning lamella. The meta1 is of unusual whiteuess,and is very soft. Analpis gave the following results :--Fe . P. Ni + Co. Total. SP. gr.94 90 0.23 (487) 100~00 7.522B. H. BMeteoric Iron from Glorieta Mt., New Mexico. By G. F. KUNZ(Amer. J. Sci., 32, 311--313).-Since the publication of the accountof the three masses of meteoric iron from Glorieta Mt. (Abstr., 1886,321), three more masses of the meteorite have been found by J. H.Bullock, and a small piece was found by a Mexican, but it dis-appeared before i t could be Recured. Seven fragments have thus farbeen obtained.No. 4 weighs 2.65 lbs. ; No. 5, 2.48 Ibs. ; and No. 6,2.31 lbs. All these fragments are figured and described by theauthor.A meteorite wag reoently presented to the Colorado ScientificSociety by the Boston and Colorado Silver Mining Company, who re-ceived it from Albuquerque, Mew Mexico, as silver bullion. Itsweight before cutting was about 5 lbs. An analysis of the iron gavethe following result8 :-Fe. Ni. 00. Cu. Zn. C. P. S. Si. Total.88.76 9.86 0.51 0.03 0.03 0.41 0.18 0.01 PO4 99.83The striking similarity between this analysis and that of the Glorieta,meteorite, leads the author to believe that this iron is the seventhfragment of the meteorite found by the Mexican, and mistaken byhim for silver bullion, B. H. B.Two hitherto undescribed Meteorio Stones.By- E. S. DANAand S. L. PRNFIELD (Amer. J. Xci., 32, 226-231).-1. MeteoritefromUtuh.-This was found in 1869, in the prairie between Salt Lake Cityand Echo, and is now in the Pale collection, Its weight is 875 grams.It is oblong in shape, about 12 cm. long, and 9 cm. in its greatestwidth. The surface is comparatively smooth ; the colour of the crustbeing reddish-black. The interior of the stone is of a dark bluish-grey colour, distinctly mottled by its chrondritic character, andshowing a rather large proportion of iron irregularly distributedthrough it, with minute patches of troilite. Olivine is the mostprominent constituent. Bronzite appears i n irregular crystal frag-ments scattered through the mas8, and plagiaclase felspar is sparinglypresent in crystalline fragments.The sp. gr. of the meteorite wasfound to be 3 66. Analysis gave 17.16 per cent. of nickeliferous iron,and 89-84 per cent. of the mineral put, including the troilite andsilicates, The iron gave on analyakMINERALOGICAL CHEMISTR P. 121Fe. Ni. co. cu. Total.91.32 8.04 0.60 0.04 100.00The mineral portion was divided into :-Soluble in hydrochloric acid ;troilite, 6.70 per cent. with 0.62 of NiS ; silicates, 48.85 per cent.Insoluble in hydrochloric acid, including chromite, 45.97. Water,1.14. Total, 100.66.Analyses of the soluble (I) and insoluble (11) portions gave :-Si02. AI2O3. FeO. MgO. CaO. Na,O.I. 40.33 0.51 21.33 35.15 1.66 0.3311. 54.83 4.82 8.64 24.56 3.341 1.98K20. P,O,. Chromite. Total.100*0011. 0.12 - 1.71 100~00I. 0.04 0.65 -The composition of the insoluble part implies that it is made np ofbrorizite with a little plagioclase. The Chantonnay metborite seemsto bear the closest resemblance to the new stone.2. Neteorite from Cape Gimrdeazc, Missouri.-This stone fell at3 B.M., on August 14, 1846, accompanied by a, loud report. It becamethe property of the Yale Museum several years ago. The stone inthe museum consists of two parts fitted together, and weighingtogether 2058 grams. The general shape of the stone is roughlyrectangular, with dimensions of 12 by 10 by 10 cm. The surface issmooth, and, where fresh, is of a light grey colour. The metallicparticles me scattered uniformly through the mass. The chondriticcharacter is distinct. The sp. gr. of the stone was found to be 3.67.The analysis showed a relation of native iron to troilite and silicatesvery near that of the Utah meteorite, namely, 17.90 to 82.10 per cent,The iron gave on analysis-Fe . Xi. co. cu. Total.91-93 7.39 0.63 0.05 100.00The analysis of the mineral portion gave !-Soluble in hydrochloricacid : troilite, 6.95 ; silicates, 42.68. Insoluble in hydrochlcric acid,including chromite, 50.19. Water, 0.58. Total 100*40. The soluble(I) and insoluble (11) parts gave-Si02. AI20,. FeO. MgO. CaO. N%O.I. 36.32 - 22.31 4023 - 0-2811. 55.79 5.54 7.91 23-65 3.35 185I. 0.04 0.82 - 100~0011. 0.24 - 1.67 100.00K20. P20,. Chromite. Total.The insoluble part is evidently bronzite, with some felspar. Thestone belongs t o the light grey chondrite type of meteorites.B. H. B

ISSN:0368-1769    

DOI:10.1039/CA8875200116

出版商:RSC    

年代:1887

数据来源: RSC