摘要:

J O U R N A LH. E. ARMSTRONG, Ph.D., F.R.S.DAVID HOWARD.F. R. JAPP, MA., Ph.D.HERBERT MCLEOD, F.R.S.R. MELDOLA.OFF. J. N. PAGE, B.Sc.W. H. PEBKIN, Ph.D., P.R.S.R. T. PLIMPTON, Ph.D.W. J. RUSSEGL, Ph.D., F.R.S.J. MILLAR Taonrsos.THE CHEMICAL SOCIETY.t% bitm :C. E. GROVES, F.R.S.%eab-Qbitar :A. J. GREENAWAY.H. BAKER.P. P. BEDSON, D.Sc.D. BENDIX.A. BLAIKIE.C. H. BOTIIAMLEP.B. BBAUNER.B. H. BBOUGH.C. F. CROSS.J. K. CROW, DSc.WYNDEAM R. DUNSTAN.JOSEPH FLETCHER.P. F. FUANKLAND, Ph.D., B.Sc.J. P. LAWS.D. A. LOUIS.A. K. MILLER, Ph.D.N. H. J. MILLER, Ph.D.J. M. H. MUNRO, D.Sc.A. PHILIP.E. W. PREVOST, Ph.D.S. RIDEAL.R. ROUTLEDGE, B.Sc.Jaxxs TAYLOR, B.Sc.A. THILLOT.L. T. THORXE, Ph.D.V. H. VELEY, M.A.H. P.WHITE.'CV. C. WILLIAMS, B.Sc.Vol. XLVIII. Part 11.1885. ABSTRACTS.L O N D O N :J. V A N VOORST, 1, P A T E R N O S T E R ROW.1885LONDON :ST. MARTIN’S LANE.EARRTSON AND SONS, PRINTERS IN ORDINARY TO HER MAJESTYC 0 N T E N T S.ABSTRACTS O F PAPERS PUBLISHED I N OTHER JOURNALS :-General and Plzysical Chemistry.PAGESIENENS (W.). A Unit for the Measurement oFLight . . . . . 1EANNONIKOFF (J.). Specific Refractive Energy . . . . . . 1Electrical and Optical Units . . . . . . . . . . 2BEETZ (W. v.). Constant Element for Electrical Measurements . . 2KOLLERT (J.). Electricity of Flames . . . . , . . . 2HANEEL (W.). Electricity Developed in the Disengagement of Gases . . 2KOOSEN (J. H.). Depolarisation of a Electric Cell by Bromine .. . 3MEEGES (C. L. R. E.). Apparatus for Breaking Electric Circuit in an Atmo-sphere of Hydrogen . . . . . . . . . . 3OSTWALD (W.). Electrical Conductivity of Acids . . . . . 3KUNDT (A.). Electromagnetic Rotation of the Plane of Polarisation ofLight by Iron, Nickel, and Cobalt . . . . . . . . 5LOMMEL (E.). A Freezing Apparatus . . . . . . . . 5STENGER (F.). Thermal Conductivity of Tourmaline . . . . . 5XONTGEN (W. C.). Absorption of Heat by Water Vapour . . . . 5THOELET (J.) and H. LAGAEDE. New Method of Determining SpecificHeats . . . . . . . . . * , . . 6BERTHELOT and VIEILLE. Specific Heat of Gaseous Elements at HighTemperatures . . , . . . . . . . . 7BERTHELOT and VIEILLE. Specific Heat of Steam and Carbonic AnhydrideBLUYCEE (A.).Influence of Concentration on the Specific Heat of Aqueousand Alcoholic Solutions of Metallic Chlorides . . . . .BOILLOT (A.). Heat of Combination of Hydrogen with Oxygen. . . 8TOMMASI (D.). Heat of Formation of some Soliible Compounds and theLaw of Thermal Substitution Constants . . . . . . 8WARBERG (L.) and J. SACHS. Relation between the Density and Viscosityof Liquids . . . . . . . . . . . . 9KLOBUKOFF (N. v.). Apparatus for the Determination of Tapour Densitiesa t Low Teinperatures . . . . . . . . . . 9KLOBEKOFF (N. v.). Estimation of Vapour Densities of Liquids of HighWINEELXANN (A.). Diffusion of Gases and Vapoms . . . . . 10WINEELMANN (A.). Diffusion of Homologous Ethereal Salts . . . 10BENDER (C.). Saline Solutions . . . . . .. . . 12EREBS (G.). An Elementary Hemonstration of A4v0gadr0'5 Law. . . 13CARNELLEY (T.).Nature . . . . . . . . . . . . 13New Apparatus for Laboratory Use . . . . . . . . 13SORET (C.). Refractive Indices of Crystallised Alums. . . . . 109LE Roux (F. F.).Junction a t a High Temperature . . . . . . . . 110GORE (G.). Electrolysis of Silver Fluoride, Chlorate, and Perchlorate . 110GORE (G.). Electro-depasition of Carbon and Silicon . . . . . 110BARBIER (E.)Thermometer. . . . . . . . * . . . 111a t High Pressures . . . . . . . . . . 7Roiling Point . , , , . . . . . . 9The Periodic Law and the Occurrence of the Xlements inInversion of the Electromotive Force of a Copper-ironRelation bebween the Ordinary Thermometer and the Weighta i V CONTENTS.SCHALL (C.). Attraction of Homogeneous Molecules .. . . .SCHALL (C.). Relation between Molecular Weight and Velocity of Evapo-ration of Liquids . . . , . . . . . . .BRUGELMANN (G.). On Crystallisation . . . . . .ALEXBEFF (W.). Stability of Compounds . . . . , . .MENDEL~EFF (D.). Phenomena of Condensation. . . . . .NICOL (W. W. J.). Connection between Pseudo-solution and True Solution.GOLDSTEIN (M.) and A. DAMSKI. .TRAUBE (J.) . Capillary Phenomena in Relation to Constitution and Mole-cular Weight . . . . . . . . . . . .FRITZ (H.). Mutual Relations of the Physical Properties of the Elements.LE CHATELIER (H.). A General Statement of the Laws of Chcmical Equi-librium . . . . . . . . . . . . .SANTIRI (s.). Coloration of the Hydrogen Flame .. . . .KRUSS (G.). Influence of Temperature on Spectroscopic Observations ,NASINI (R.). Specific Refraction in Refereuce to the Double Bond . .ALBITZKY (A.). Refractive Power of the Hydrocarbon C,2Hpo . . .11-YROUIIOFF (G.). Dispersion of Sodium Chromate . . . . .WEBEE (C. L.). Electric Conductivity of Amalgams . . . . .PFEIPPER (E.) . Electric Conductivity of Solutioiis of Carbonic Anhydride .NEESEN (F.). Influence of Magnetisation on the Resistance of MagneticLiquids . . . . . . . . . . . . .WESENDONCK (K.). Diathermaacy of ,Zsculin . . . . . .MULLER-ERZBACH (W.). Tension of Aqueous Vapoum of Hydrated Salts .KAYSER (H.). Condensation of Carbonic Anhydride on Glass . . .SCHLEGEL (G.) . Combustion of Hydrocurbous and their Derivatives withMixtures of Ox: gen and Chlorine .. . . . . . .BLUMCKE (A.). Determination of the Specific Gravity of Carbonic AcidSolutions . . . . . . . . . . . .MARIGNAC (C.) and also 0. LEXMANN. Crystallisation . . . .VALENTINI (A.). Lecture Experinleiits . . . . . . .ITASSELBERG (B ). The Second Spectrum of Hydrogen . , . .LI~TING (G. D.) and J. DBWA~~. Spectml Ljnes of Metals Developed byExploding Gases . . . . . . . . . . .PARRY (J.). Spectroscopic Examination of the Vapours evolved on HeatingIron, &c. . . . . . . . . . . . .FLEISCHL (E. v ) . Double Refraction of Liquids . . . . .LANGLEY (S. P.). Amount of Atinospheric Absorption . . . .OLIVIER (L.). .CROVA (A). A Diffusion Photometer . . . . , . . .GOKHAM (J.). The Pupil Photometer .. . . . , . .MCLEOD (I€.). Sunshine Recorder . . . . . . . .PREECE (W. H ) . New Standard of Illumination . . , . .SCHMIDT and HANSCE. Disturbing Phenomena observed in Polarising Opera-tions . . . . . . . . . . . . .CARHART (H. S.). Electromotive Force of a Daniell’s Cell . . . ,DE LA RUE (W.) and H. W. MULLER. Electric Discharge with the Chlorideof Silver Hattery . . . . . . . . . . .MICHAELIS (C.). Electric Conductivity of Impure %rcury . . .IC ~MEMSICY (G.). Electric Conductivity of Coppw Antimony Alloys . .KOHLEAUSCH (F.). Electric Conductivity of Water . . . . .OSTWALD (W). Electric Conducti-oity of Acids . . . . . .GORE (G.). Some New Phenomena of Electrolysis . . . . .GORE (G.). Unequal Electric Conduction R e d a n c e at Cathodes , .UOEB (G.).Relation of Chemical Corrosion to Voltaic Current , . .IIaaTLEY (w. N.). On the Use of Moist Electrodes . . . . .WRIGHT (C. R. A) and C. TIIOMPSOX. Determination of Chemical A5nityin Terms of Electromotive Force . . . . . . . .ABNEY (W. DE W.) and R. FESTING. Relation between Energy and Radia-tion in the Spectrum of Incandescelice Lamps . . . . .Rise of Solutions in Capillary TubesMethod of Measuring the Chemical Effect of RadiationPAGCB11111211%11411 411511511611711726920921021 L2112112122132132132142142152 1521531731731831831931932032032032132 L32132232632336332332432432432532532 COh‘TEKTS .GORE ((3.).RAYLEIOH (Lord) .Relation of Heat to Voltaic and Thermo-electric Action ofMetals in Electrolytes .. . . . . . . . .The Constant of Electromagnetic Rotation of Light inCarbon Bisulphide . . . . . . . . . . .FROIILICH ( G ) . Measurement of Solar Heat . . . . . .BERTHELOT and VIEILLE . Heats of Combustion of Charcoal and OrganicCompounds . . . . . . . . . . . .LOUGUININE (W.). etty Acids .LOUGUININE (W.). Heats of Combustion of certain Carbon C ipounds .Heats of Combustion of Ethereal Salts ofBERTHELOT . Thermochemistry of Phosphorus Trifiuoride . . .RUBNER (M.). Thermal Eqnivalent of a Solution of Urea .GUTHRIE (F.). Eutexia . . . . . . . . .. .MILLS (E . J.). Melting Points and Boiling Points as related t ChemicalComposition . . . . . . . . .. . .LEHMANN (0.). Melting Poiuts of Substances in Contact . . . .CLAUDON (E.). Employment of Condensation in Fractionating Apparatus .ANDREAE (J . L.). Method for Estimating the Specific Gravity of SolidSubstances soluble in Water . . . . . . . . .DOBBIF: ( J . J.) and J . B . HUTCHESON . Easy Method of Determining theSpecific Gravity of dolitls . . . . . . . . .GROSHANS (J . A.). Specific Gravity of Substances in the Solid State andin Aqiieous Solution . . . . . . . . . .AXDREAE (6 . L.). Specific Gravity of Saturated Solutions of Solid Sub-stances a t Various I’emperatures . . . . . . . .FLEURY (G.). Density of Porous Bodies . . . . . . .NICOL (1%’. W . J.). Molecular Volume of Saline Solutions . . . .BEZOLD (W . v.). Cohesion Fignres .. . . . . . .HENRY (L.). Solubility and Fuvibility in the Oxalic Acid Series . . .GZTTHRIE (F.). Salt Solutions and Attached Water . . . . .GUTHRIE (F.). Thermal and Volume Changes attending Mixture . .ILLINGWORTH (B.) and A . HOWARD . Thermal Relationship between Waterand Certain Salts . . . . . . . . . . .LE CHATELIER (H.). Laws of Solution . . . . . . .NICOL (W . W . J.). Saturation of Salt Solutions . . . . . .ALEXBEFF (W.). Reciprocal Solution of Liquids . . . . .MILLS (E . J.) and \V . M . MACEEY . .AMAGAT (E . H ) . Correction of the Results given in ti Paper on CompressedGas Manometers . . . . . . . . . . .THOMSON (J . J.). Combination of Gases . . . . . . .MILLS (E . J.). The Numerics of the Elements . . . . . .CARNELLEY (T.). The Periodic Law .. . . . . . .NICOL (W . W . J.). Boiling Points of Saline SolutionsDEWAR (J.). Critical Voluqes of Liquids . . . . . . .. . . .Lines of no Chemical Change .HOOD (J . J.). Rate of the Chemical Absorption of Gases . . . .SANTINI (S.). Coloration of the Hydrogen Flame . . . . .DEMAR~AY (E.). Methods of Spectrum Analysis . . . . . .LIVEIIW (G . D.) and J . DEWAR . Spectroscopic Studies on Gaseous Explo-sions . . . . . . . . . . . . .HARTLEY (W . N.). Delicacy of Spectrum Photography . . . .BURCH (G . J.). Experiments on Flame . . . . . . .BLEEERODE (L.). Indices of Refraction of Liquefied Gases . . . .NICHOLS (E . L.). Duration of Colour Impressions on the Retina . . .JABLOCHKOFF (P.). New Form of Voltaic Battery . .. . .BOTTOMLEY (J . T.). Daniell‘s Cell of Small Internal Resistance . . .RAYLEIUH (Lord) and Mrs . SIDGWICE . Electro-chemical Equivalent ofSilver . . . . . . . . . . . . .BOSTWICE (A . E.). Influence of Light on the Electrical Rejistance of MetalsHUBION . Variation in the Electric Resistance of Bismuth when placed in aMagnetic Field . . . . . . . . . . .FRIEDEL iC.1 and J . CURIE . Pvrolectricitr of the Tonaz . . . .VPAQE3253253263163273273283 283393393303313313313323323333343343343353353373393393403403403413413413413443444.6 54654654%466467468468469469469413946vi CONTEXTS.GRAY (T.), A. BRAY, and J. J. DOBBIE. Electric Qualities of Glass , .CHEESMAN (L.M.). Measurement of rapidly alternnting Electric Currents .BAUMIIAUER (E. H. v.). Simple Form of Thermo-regulator and RegisteringThermometer . . . . . . . . . . . .FORCEAND. Heat of Formation of Ammonium Sulphite , . , .GUSTATSON (G.). Thermic Data for the Cornpounds of Aluminium Bromidewith Hydrocarbons . . . . . . . . . . .WITZ (A.). Ca!orific Power of Coal-gas . . . . . . ,BERTHELOT. Chemical Neutrality of Salts , . . . . . .LE CHATELIER (H.). Laws of Dissolution . . . . . . .TOMLINSON (C.). Boiling of Liquids in a Vessel contained in a Water-bath .LE CHATELIER (H.). Dissociation of Chlorine Hydrate . . , .OLSZEWSKI (K.). Solidification of Pu'itrogen and Carbonic Oxide . . .THOULET (J.). Attraction between a Dissolved Salt and a Substanceimmersed in the Solution ., . . . . . . .BOTTOMLEY (J. T.). Condensation of Gases on the Surf'ace of Glms . .LLOYD (J. U.). Separation by Capillary Attraction . . . . .BERTHELOT. Rate of Propagation of Detonation in Solid and Liquid Explo-sives . . . . . . . . . . . . .DIXON (€I. B.). Conditions of Chemical Change in Gases . . . .URECH (F.). Influence of the Diluent on the Rate of Chemical Action .BETAD ('J.). Rate of Formation of the Carbonates of the Alkaline Earths inRelation to Time, Mass, &c. . . . . . . . . .LORIN. A Particular Case of Catalytic Action . . . . . .MORSE (H. N.) and E. II. KEISER. Apparatus to determine the Equivalentsof Certain Elements . . . . . . . . . .LANDOLT (H.) . Laboratory Apparatus . . . . .. .HART (E.). New Forms of Laboratory Apparatus . , . . .WALTER (J.). Use of Steam in Chemkal Laboratories . . . .BOISBAUDRAN (L. DE), Spectrum of Samarium . , . . . .DECIIANT (J.). Refractive Indices of Condensed Gases . . . .VOIGT (W.). Colour Phenomena of Pleochroic Crystals . . . .MICHEL-LBvY. Determination of the Double Refraction of Minerals . .LIEBISCH'(T.). .KLEIN (W.). Optical Modifications produced in Crystals by the Action ofHeat , . . . . . . . . . . . .BREMER((a. J. w.). Change of Specific Rotatory Power under the Influenceof Various Solvents. . . . . . . . . . .VIOLLE (J.). Absolute Unit of Light . . . . . . . .MOLLER (W.). Law of Emanation of Light from Incandescent Substances .PIRANI (E.) . Galvanic Polarisation . . .. . . . .RICHARZ (F.). Products of the Electrolysis of Dilute Sulphuric Acid . .BARTOLI (A), Electrical Conductivity of Carbon Compounds . . .BLUMCEE (A.). SpecXc Heat of Uranium . . . . . . .EHRHARDT (0.). Specific Heat and Latent Heat of Fusion. . . .KEELER (J. X.). .TRUCHOT (C.). Thermochemistry of Ammonium Fluosilicates . . .DE FORCRAND. Formation of Glyoxal Ammonium Hydrogen Sulphite .BERTHELOT and WERNER. Bromine Substitutions . . . . .BERTHELOT and WERNER. Isomerism in the Benzene Serie~: Heat ofNeutralisation of Polyhydric Phenols . . . . . . .RAMSAY (W,) and S. YOUSG. Influence of Change from Liquid to SolidState on Vapour-pressures . . . . . . . . .LE CHATELIER (En). Decomposition of Salts by Water . . . .CHANCEL (G.) and I?.PARMENTIER. Solubility of Carbon Disulpliide andChloroform in Water . . . . . . . . . .EBNER (V. v.). Difference between Crystalline and Anisotropic Structures .LFDEBUR. Oxidation and Reduction . . . . . . . .WALTER (J.). Apparatus for Chemical Laboratories . . . . .&RING (W.). Action of Mass . . . . . . . .Apparatus for Measuring the Angle of the Optic AxesAbsorption of Radiant Heat by Carbonic Anhydride.PAGE47047147147147247247247347447447547647747747847948045048045148148148148 262162162 L62162262262262262362362462462562562662662762762862963063063163 163CONTENTS. v iiWILL (W. W.) . Apparatus for Continual Percolation with Boiling LiquidsALLIHN (F.).Apparatus for Filtering in a Vacuum . . . . .SCIIOENE (E.). Spectrum of Ozone . . . . . - . .DESLANDRES (H.) . Relation between the Ultra-violet Spectrum of Waterand the Telluric Bands A, B, a . . . . . . . ,TIMIBIAXEFF (C.). Chemical Action of Light on Chlorophyll . . .CARPENTIER (J.). Battery with a Circulating Liquid . . . . .ROSESPELD (M.). New A-pparatus for Electrolysis . . . . .WROBLEWSKI (S. v.). Production of Low Temperatures by Means of LiquidOxygen, Nitrogen, &c. . . . . . . . . . .TOMASBI (D.). Heats of Formation of Hydrogen Compounds . . .MULLER (A.). Heats of Formation of Salts of the Amines . . . .LAZARUS (M. J.). Fractional Distillation in a Current of Steam . . .NAUMANN (A.). Kahlbaum's so-termed " Specific Remission " .. .SHALFBEFF (11.). Specific Volumes of Chlorine, Bromine, and IodiNe inCarbon Compounds . . . . . . . . . .SCHIFF (R.), Constants of Capillarity of Liquids . . . . .VOLKMANN (P.). Remarks on Schiff 's Paper on the Capillarity Constants ofLiquids . . . . . . . . . . . . .WRIGHT (C. R. A.) and C. THOMPSON. Deiermination of Chemical Affinityin Terms of Electromotive Force . . . . . . . .DULK (L.). Gravitation and Atomic Weight . . . . . .LAAB (C.). Possibility of Several Structural Formulre for the same ChemicalCompound . . . . . . . . . . . .TISSANDIER ((3.). Apparatus for the Constant Production of Gas . .CORNU (A.). Spontaneously Reversible Lines in Spectra . . . .DEAPEE (H.). Use of Carbon Bisulphide in Prisms . . . , .VOHWINKEL (E.).New Constant Galvanic Element . . . . .DUPRB (A.). Battery with Two Liquids . . . . . . ,D'AESONVAL (A.). Suppression of Nitrous Fumes from the BumenBattery . . . . . . . . . . . . .CLAMOND and J. CABPENTIER. New Arrangement of the Thermo-electricPile . . . . . . . . . . . . .JABLOCHKOFF. New Pile or Auto-accumulator . . . . . .CAILLETET and BOUTY. Electrical Conductivity of Solid Mercury and otherMetals . . . . . . . . . . . .BARTOLI (A.). Conductivity of Cetyl Alcohil . . . . . .TROWBRIDGE (J.). Measurement of Strong Electric Currents . . .OSTWALD (W.). Trustworthiness of Alternating Currents for MeasuringElectrical Resistances . . . . . . . . .GOCKEL (A.). Relation of " Peltier's Heat Effect'" to the Available Energyof a Galvanic Element .. . . . . . . . .OSMOND. Calorimetric Study Qf .the Effect of Tempering and Hammering onCast Steel . . . . . . . . . . . .WITZ (A.). Combustion of Mixtures of Coal-gas and Air . . . .STOHMANN (F.). Calorimetric Investigations . . . . . .XAOULT (F. M.). Influence of Uilution on the Reduction of the FreezingPoint of Aqueous Solutions . . . . . . . . .BARTOLI (A.). Relation between Critical and Boiling Points . , .BARTOLI (A.) and E. ST~ACCIATI. Nendel6effs Formula for the Expansionof Liquids . . . . . . . . . . . .BARTOLI (A.) and E. STRACCIATI. Critical Temperatures and Vslumes ofParaffins . . . . . . . . . . . .ERCKMANN (G.). Dissociation Tension of Ammonium Carbamate . .NAWMANN (A.). Dissociation Tension of Ammonium Carbamate .. .CAILLETET (L.). Liquefaction of Oxygen . . . . . . .OLZEWSKI (K.). Liquefaction and Solidification of Methane and NitricOxide . . . . . . . . . . . . .VINCENT (C.) and J. CHAPPUIS. Tensions and Critical Poi& af someVapoura . . . . . . . . . . . * .PAGE63163 171371371471471571571671671671771771772172172272272285385385385385485485485585585585685685685785785885985985985985985986086 ... Vlll CONTENTS.PAGEWROBLEWEW (S.).Permanent Gases in a Vacuuni , . . . . . . . 861NATANSON (E. and L.). Dissociation of Nitrogen Peroxide , . . . 862TAMUANN ((3.). Tension of Aqueous Vapour of Salt Solutions . . . 862GOODWIN (W. L.). Nature of Solution .. , . . . . a65RUDORFF (F.). Solubility of Mixtures of Salts , . . . . . 865THOULET (J.). Attraction between Dissolved Substances and Solids Immersedin the Solutions . . . . . . . . . . . 866TRAUBE (J.). Capil'ary Constants of Certain Aqueous and Alcoholic Solu-tions . . . . . . . . . . . . . 866BARTOLI (A.). Capillary Constants of Liquids and Cohesion of Solids . . 866BUNSEN (R. W.). Capillary Gas Absorption . . . . . . 867PFAUNDLER (L.). Action of Compressed Carbonic Anhydride on Glass , 868BERTHELOT. Principle of Maximum Work . . . . . . . 868BARTOLI (A.). Impermeability of Glass to Gases . , . . . 869XUDORFF (F.). Lecture Experiment . . . . . . . . 869BOISBAUDRAN (L. DE). New Order of Metallic Spectra . . . . 949BELL (L.). Absorption Spectrum of Nitrogen Peroxide .. . . 949KR&S ((3.).Organic Compounds . . . . . . . . . . 949KANONNIEOFP (J.). Refractive Power of Chemical Compounds . . . 949RUBNER (M.). Calorimetric Researches . . . . . , . 949MULLENBOFF (R,). Heat of Formation of Ferrous Sulphide . . . 950GORBOFP (A.) and A. KESSLEE.Reduced Pressure . . , . . . . . . , . 950FOCK (A.). New Therrno-regulator . . . . . . . . 950RasI%sKI (I?.). Fractional Distillation in a Current of Steam . . . 950LAEQER (C.) and V. METEB.Heat . . . . . . . . . . . . . 950SCHIFF (R.).Temperatures ' . . . . . . , . . 950HART (I?.). Motions of Camphor on the Surface of Water . . . . 951BELLAMP (F.). 951EXNER (F.), New Method for Determining the Size of Molecules . . 951HEMPEL (W.).951BALMER (J. J.). Spectrum Lines of Hydrogen . . . . . . 1025BOISBAUDEAN (L. DE). Spectrum of Ammonia . . . . . . 1025CROO~;CES (W.).rium . . . . . . . . . . . . . 1025EDER (J. M.). 1026VOIGT (W.). Optical Pr0perti.s of Thin Metallic Layers . . , , 1026STRECKER (K.). Reproduction of 8iernens' Mercu1.y Unit . . . 1027LODGE (0,). Seat of the Electromotive Force in the Voltaic Celi . . 1027STENGER (F.). Electric Conductivity of Gases . . . . . . 1028WEBER (C. L.).Mercury. . . . . . . . . . . . . 1028PFEIFFER (E.). Electric Conductivity of Aqueous Alcohol . . . . 1029JAHN (El.). Validity of Joule's Law for Electrolytes . . . . . 1029TOMASSI (D.). Electro-pseudolysis . . . . . . , . 1029OSTWALD (W.). Electro-chemical Studies . .. . , . . 1029XLEMENFIF (I.). Dielectric Constant of certain Gases and Vapours . . 1030RONQTEN (W. C.). Electromagnetic Action of Dielectric Polarisation. . 1030BLUXCKE (A.), Specific Heat of Aqueous Alcohol . . . . . 1031WIEDEMANN (E.) and C. LUDEEING. Thermal Phenomena of Collo'ids . 1031DE FOECRAND. Sodium Methoside . . . . . , . . 1031BERTHELOT and WERNER. Heat of Neutralisation of Hydroxyhenzoic Acids 1032LEHMANN (0.).stance~ . . . . . . , . . - . . . 1038MEPER (V.) and a. (3. POND. Physioo-ohemical Experiments . . . 1033TRAUBE (J.). 1035Phenomena which L4ccornpany the Evaporation of theRelation between the Composition and Absorption Spectra ofApparatus for Fractional Distillation underDensity of Sulphurous Anhydride a t a WhiteEstimation of the Bpecific Gravity of Liquids at HigherAction of some Metals on Mixtures of Acetylene and Air .Apparatus and Arrangements of the Laboratory at DresdenMutual Extinction of the Spectra of Yttrium and Sama-Spectrographic Investigation of Different Standards of LightElectric Conductivity and Temperature Coefficient of SolidSpontaneous Change of Porm of Homogeneous Solid Sub-Influence of Temperature ~n tho Capillary Aleniscus Angle CONTENTS.ixWILLGERODT (C.). Application of Various Substances as Halogen Carrierg.REICHER (L.). Velocity of Saponification . . . . . . .BROWN (tJ.). Formation of a Stnlactite by Vapour . . . . .SCHIFF (H.). Lecture Experiments on the Occlusion of Hydrogen by Palla-dium . . . . . . . . . . . . .CLEMINSHAW (E.).Lecture Experiments on Spectxm Analysis . . .ANSCHUTZ (R.) and A. KEKUL~. Useful Apparatus . . . . .WALTER (D. J.). Apparatus for Chemical Laboratories . . . .SORET (C.). Refractive Indices of Alums . . . . . . .NASINI (R.) and 0. BERNHEIMER. Relation between Refractive I’m t’r andChemical Constitution . . . . . . . , . .MESSERSCHMITT (J. B.). Spectro-photometric Observations . . .~ I E A R D (C.) and PABST. Absorption-spectra of some Colouring >ratters .BECQUEREL (E.). Spectroscopic Stud? of Compounds rendel ecl Phos- .ELSTER (J.) and H. GEITEL. .HEMPEL (W.). Influence of the Chemical Nature and the Pressure ofGases on Electric Induction Machines . . . . . . .CROVA and GARBE. Charge and Discharge of Secondary Batteries ..GAIFFE (A.). A Standard Volt . . . . . . . . .STRECKER (K.). Reproduction of Siemens’ Electric Mercury Unit . .WROBLEWSKI (S.). Electrical Resistance of Copper a t very Low Tempera-tures. Inhidating Properties of Liquid Oxygen and Nitrogen . .FOUSSEREAU (G.). Electrical Resistance of Alcohol . . . . .JAEN. Work done in the Decomposition of Electrolytes . . . .OLSZEWSKI (K.). Production of very Low Temperatures . . . .OLSZEWSKI (K ). The Use of Boiling Oxygen, Nitrogen, Carbonic Oxide,and Atmospheric Air for Producing Cold . . . . . .ARONS (L.). Heat of Dilution and Specific Heat of Saline Solutions . .BLUMCKE (A.). Specific Heat of Concentrated Soda Solutions . . .BUNTZ.RECOURA. Heat of Transformation of Chromous Chloride into ChromicChloride .. , . . . . . . , . .DE FORCRAND. Heat of Formation of Alkaline Alcoholates . . .TSCHELTZOW. Heat of Formation of Picrates . . . . . .BERTHELOT and WERNER. Heats of Formittion and Transformation of theHydroxybenzoic Acids . . , . . . . . . .COLSON. Heats of Formation of Phthalates . . . . . .VINCENT (C.) and J. CHAPPUIS. Critical Temperatures and Pressures ofsome Vapours. . . . , . . . . . . .CHERVET (A). Constants of Capillarity of Saline Solutions . . .MINNIGERODE (B.). The Symmetry rrnd Xlasticity of Crystals . . .KAHLBAUM (G. W. A.). Refractive Indices of the Three Methyl AcrylatesKLOBUKOFF (K.) . Relation between Molecular Structure and Absorptionof Light. . . . . . . . . . , . .EDER (J. M.). Chemical Action of Light . .. , . . .LINXEMANN (E.). Absorption Phenomena of Zircons . . . . .HARTLEY (W. N.). Absorption-spectra of Alkalo‘ids . . . . .BOISBAUDRAN (L. DE). Fluorescence of Rare Earths . . . . .STOKES ((3. (3.). Crystalline Reflection in Potassium Chlorate Crystals .PREECE (W. H.). Charging Secondary Batteries . . . . .ANDREWS (T.) . Electromotive Force between Metals a t High TemperaturesABNEP (W. de W.) and R. FESTING. Abuorption-spectra Thermograms .EAHLBAUM (GI. W. A.). Dependence of Boiling Point and Pressure . .SCHUMANN (0.). Boiling Point and Pressure . . . . . .STOEMAN (F.) and P. RODATZ. Heat of Combustion of Laurie and MyristicAcide , , . . . . . . . . . . .STORMAN (F.) and 11. WXLSING. Specific and Latent Heats of Mprietic andLaurio Adds .. . . . , . , . . . .phorescent by the Action of Light or the Electrical Discharge .The Simplest Form of Induction IllachineLOMMEL (E.). Variation of Induction Machines . . . . .Heat of Formation of Antimony Bromide and IodidePAGE10341034103410351035103510351097109’710971098109810981098109810991n991u991099110011001101110111911101110111021102110311031104110411051105117311’7311731173117411741175117511’76117511’7611761176l l i X CONTENTS.PAGEBERTHELOT. Isomerismin the Benzene Series . . . . . .RAMSAY (W.) and 8. YOUNG. Thermal Properties af Ethyl Alcohol , .SCHALL (C.). Relation of Expansion of Substances in Gaseous, Vaporous,and Liquid States to Absolute Temperature .. .SCHALL (C.). Modification of Petterson and Ekstrand's Method of Vapour-density Determinations . . . . . . . . . .IJA COSTE (W.). Estimation of Vapour-densities a t a Diminished Pressure.SCHALL (C.). Relation between Specific Gravity, Capillarity, and Cohesion .SCHALL (C.). Relation between Capillarity and Specific Grayity of Membersof Homologous Series . . , . . . . . . .TOMLINSON (C.). Motions of Camphor on Water . . . . .REYER (E.). On Solidification . . . . , . . . .RAUPENSTBAUCH (G. A.). Solubility of Salts in Water at Various Tempera-tures . . . . . . . . . . .VAN'T HOFF (J. He.). .SPOHR (J.). Action of Neutral Salts and of Temperature on the Inrersionof Cane-sugar . . . . . . . . . . . .METER (L.) and A.SCHENFEUEN. Chlorine and Bromine Carriers . .SCtiALL (C.). Relation of Diameters of Molecules . . . . .The "Critical Point" in Chemical DecompositionsInorganic Chemistry.SCHRAUF (A.). Dispersion Equivalent of tfhe Diamand . . . .GLSZE WSKI (V.) . Liquid Cmbonic Oxide , . . . . . .MOISSAX (H.). Phosphorus Trifluoride . . . , . , .HOFMANN (A. W.). Phosphorus Chloronitride . . . . . .KLEIN (0.) and J. MOREL. Action of Kitric Acid on Tellurium . . .KLEIN (D.) and J. MOREL. Action of Water and Nitric Acid on BasicTellurium Nitrate . . . . . . . . . . .MUSPRATT (E. K.) and G. ESCHELLMANN. Preparation of Potassium Chlo-rate . . . . . . . . . . . .MUSPRATT (E. K.) and G. ESCHELLMANN. Preparation of Sodium ChlorateTERREIL. Crystallised Argentammonium Chloride and Bronlide ., .WIDMANN (0.). Argeiitammonium Phosphate . . . . , .REYCHLEE (A,). Argentammonium Compounds . . . . . .WACKEBRODER. Preparation of Strontium and Barium Chlorides . .DREYFUS (E.). Constitution of Bleaching-powder . . . . .HAASS (R.). Peroxides of the Zinc Magnesium Group . . . .DEBRAY and JOSNBIS. Decomposition of Cupric Oxide by Heat . . .DEBRAY and JOANNIS. Oxidation of Copper . . . . . .QUANTIN. Some Reactions of Chromyl Dichloride . . . . .J~RGENSEN (S. M.). Chromammonium Compounds, Luteochromium Salts .HOCIBOM. Double Tungstates of Rare Metals . . . . . .MUNTZ (A.) and E. AUBIN. Combustible rganic Mat,ter in the Air . .GORE (G.). Reactions with Carbon and s g e of its Compounds . . .HAUTEFEUILLE (P.) and J.MARGOTTEK Polymorphism of Silicon Phos-phate . . . . . . . . . . . . .CABELL (5. M.). Crystalline Phosphorous Anhydride . . . . .MOISSAN (H.). Arsenic Trifluoride . . . . . , . .MEIVDEL~EPF (D.). Specific Gravity of Sulphuric Acid . . . .WEBER (R.). Octosulphates. . . . . . . . . ,RAOULT (F. M.). Action of Water on Double Salts . . . . .GORE (G.). Magnesium Suboxide. . . . . . . . .KRUSS ((2.). Copper Peroxide . . . . . . . . .MAUMEN~ (E. J.). Decomposition of Cupric Oxide by Heat . . .CABELL (J. M.). Action of Hydrogen Sulphide on Metallic Silver . .BRUCE (J. D.). Silver Hjdroxide. . . . . . . . .DELACHARLONNY (P. M.). Xvdrated Aluminium Sulphate . . . .FBONME (C.). The Tempering of Steel . . . . . .1.17'11178117911791180118011801180118011811181118111821182141415151617171718181819192021222323252611811912012112112112112212312412412412412COSTEXTS .xiSCHEURER.KESTNER . Reaction between Ferric Oxide and certain Sulphatesa t High Temperatures . . . . . . . . . .A~OISSAN (H.). Action of the Tnduction Spark on Phosphorus Trifluoride .LUNGE ((3.). Density of Sulphuric Acid . . . . . . .REESE (C . L.). Comparative Oxidation of Solutions of Sulphurous AcidSCHULZE (H.). Pyrosulphates . . . . . . . . .and of Sodium Sulpliite . . . . . . . . . .XOBTXSON (H.). Atomic Weight of Cerium . . . . . .GEUTHER (A.). Action of Lead HJdroxide and Silver Oxide on AqueousSolutions of Sodium Pentasulphide and Sodium Thiosulphate ..CAYAZZI (A.). Action of Hydrogen Phosphide on Bismuth ‘hichloride .KLEIN (D.). .HANRIOT . Hydrogen Peroxide . . . . . . . . .WEHSARG (K.) . Iodic Anhydride . . . . . . . .REPS (J . M.). Allotropic Transformation of Sulphur at very Low Tempera-tures . . . . . . . . . . . . .REICHER (L . T.). The Temperature of Allotropic Transformation of Sul-phur . . . . . . . . . . . . .DRAPXR (H . N.). Preparation of IIydrogen Sulphide . . . . .PFORDTEN (0 . v . D.). Purification of Hydrogen Sulphide frcm Arsenic .Action of Tellnrous and Telluric Acids on ParatungstatesYOLLACCI (E.). Spontaneous Oxidattion of Sulphur . . . . .MANECK (I?.). Electrolytic Preparation of Nitrogen Chloride . . .HUSKISSON ( P . L.). Crystallisation of Phosphoric Acid .. . .JOLY (A.) . Saturation of Phosphoric A&d by Bases . . . . .VAN DER PLAATS (J . U.). Atomic Weights of Carbon, Phosphorus, Tin,and Zinc . . . . . . . . . . . .DAMOISEAU (A.). Preparation of Sodium Sulphide . . . . .DE YITTEURS . Molecular Xodifications of Silver Bromide . . . .CAREY LEA (M.). Combination of Silver Chloride, Bromide, and IodideCLARK (J . W.). .BOUEGOIN (E.). .WELSBACH (A . v.). The Rare Earths . . . . . . . .GRATANA (U.). Double Sulphide of Aluminium and Potassium . . .GORGEU (A.). Tricobalt Tetroxide . . . . . . . .HABERMANN (J.) . Basic Salts . . . . . . . . .GODEFROY (L.). Hydrates of Chromic Chloride . . . . . .MULLER (M.). Purple of Cassius . . . . . . . .SCHNEIDER (It.) Atomic Weight of Bismuth .. . . . .HAGER . Nitric Peroxide in Bismuth Subnitrate . . . . . .HALBEESTADT (W.). Atomic Weight of Platinurn . . . . .WILM . New Rhodium Salts . . . . . . . . .VINCENT (C.). New Compounds of Iridium . . . . . .REXSEN (I.) and E . H . KEISEP . Estimation of Carbon in Ordinary Phos-phorus . . . . . . . . . . . . .MOEBAN (H.). Preparation of Phosphorous Triflnoride . . . .JOLF (A.). Crystallised Hjdrate of Phosphoric Acid . . . . .ISAHBERT (l?.). Action of Sulphur on Amorphous Phosphorus . . .TONMASI (D.). Non-existence of Ammonium Hydroxide . . . .REED (L.). Action of Boric Acid on Calcium Carbonate . . . .H a R T m Y (w . N.). Atomic Weight of Beryllium . . . . .ENGEL (R.). Solubility of Magnesium Carbonate in Carbonic Acid ..ANI)R$ (G.). Ammonio-zinc Sulphates . . . . . . . .OSMOND and WERTH . Cellular Structure of Fused Steel . . . .KNORRE (G . v.). Tungstates of Barium, Strontium, and Calcium . .GRIPPITHS (A . B.). Platinum Carbides formed at Low Temperatures . .AMAGAT (E . H.). Density and Atomic Volumes of Oxygen and Hydrogen .POPPER (A.). Decompositicn of Aqueous Solutions of I-Iypoclilorous Acidwith Colouring Matters . . . . . . . . . .Purification of Mercury by Distillation in a VacuumSolubility of Mercuric Iodide in Water and Alcohol .CLOEZ ((3.). Apparatus for preparing Hydrogen . . . . . .and of Chlorine in Sunlight . . . . . . . . .PAQE12521521621621721721 721821834.43463463463463473473473473483483493493503 503503503503613513523523543543553553564824524824834844844894844854864876316314a563Xii CONTEXTS .BERTEELOT .Action of Bromine on Chlorides . . . . . .~UBIERSCHPY (C.). Thiophosphoric Acid . . . . .MCCAY (L . W.). Reduction of Arsenic Acid Solutions by means of Sul:phurous Anhydride . . . . . . . . . .MUENCEE (A.). Apparatus for preparing Pure Carbonic Anhydride . .BETADE . Solubility of Lithium Carbonate . . . . . . .WILLIAMS (G.). Occlusion of Hydrogen by Zinc-dust . . . . .ANDR~ (J.). Basic and Ammoniacal Nitrates . . . . . .BOISBAUDRAN (L . DE) . Action of Hydrogen Peroxide on Cerium and. Thorium . . . . . . . . . . . . .C L ~ E (P . T.). Action of Hydrogen Peroxide upon the Rare Earths ..C L ~ E ( P . T.). Samarium Compounds . . . . . . . .BOISBAVDRAN (L . DE) . Alloys of Indium and Gallium . . . .MOISSAN (H.). Chromyl Chloride . . . . . . . .REOELSBEROER (F . F.) . Ammoniacal Compoun:ls of Uranyl Chloride . .DEVAR~AY (E.) . Separation of Titanium from Niobium and Zirconium .WINKELLMANN (4.). Time of Existence of Thiosulphuric Acid in AqueousSolution . . . . . . . . . . . . .ISAMBERT . Preparation of Ammmia Ga4 . . . . . . .h D O F F (A.). Formation of Hjdroxylninine . . . . . . .SCHIFF (H.) and R . SRSTINI . Compounds of Arsenious Anhydride withPotassium Bromide and Jodide . . . . . . . .WEIGLE (T.). Presence of Chlorine in Potassium Bromide . . . .MANZONI (G . S.). Preparation of Sodium Hyposulphite .. . .PELLIZZAXI (G.). Coinbiuations of Ammonia with Ammonium Salts . .SCHULTEN (A . DE) . New Crystallised Magnesium Phosphate and Arsenate .ENGEL (R.) . Magnesium Hydrocarbonate . . . . . . .Basic Nitrates of Lead . . . . . . . .MANZONI (G . S.). Chromium and Aluminium Sulphates . . . .EEMPEL (W.). Behaviour of the Different Modifications of Carbon towardsIron . . . . . . . . . . . . .JORGENSEN (S . M.), Roseocobalt Salts . . . . . . . .New Tin Salts . . . . . . . . . .TIrroLr (I).). Compounds of Platinum and Arsenic . . . . .THONSEN (J.). Molecular Weight of Fluid Water . . . . .MUNTZ (A.). Oxidatioii of Iodine during NitrScation . . . . .KLEIN (D.) and J . MOREL . Tellurous Anhydride . . . . .WINELER (C.). Change of Arsenious Oxide from the Amorphous to theCrystalline Condition .. . . . . . . . .JOLY (A.). Preparation of Arsenic Acid . . . . . . .HAUTEFEUILLJIB (P.) and A . PERRLEY . Apparent Volatilisation of Silicon at440' . . . . . . . . . . . . .Combination of Magnesium and Potassium Hydrogen Car-bonates . . . . . . . . . . . . ..LYTE (F . M.). Sodium dlnminate . . . . . . . .SYOLEA (A.).BENAS (T.).TREY (H.). Basicity of Hyposulphuric Acid . . . . . .GEANDEAU (H.). Phosphates . . . . . . . . .JOANNIS . aopper Oxides . . . . . . . . . .HAUTBFRUILLE (P.) and A . PERREY . Aluniinium Oxychlorides . . .JGROEN-EN (S . M.). Cobaltammonium Cdmpounds . . . . .Hydrochloride of Chromous Chloride . . . . . .GIBBS (W.). New Complex Inorganic Acids . . .. . .CATAZZI (A.). Bismuth Antimoniates . . . . . . . .DEBRAY (H.). Purple of Cas;ius . . . . . . . . .ENGRL (It.).ANDRE ((3.).FRIEDEL (C.) and L . ROUX .RECOURA .Arnmoiiio-cupric Sulphate and a Basic Cupric Sulpbate .Action of Aluminium on Aluminium ChlorideCAVAZZI (A.), Action of Phosphine on Auric Chloride . . . .SABATIER (I?.). Composition of Hydrogen Persulphide : a Nacreow VarietyGERNEZ (D.). Rate of Transforniation of Prismatic into OAahedral S&hurof Sulphur . . . . . . . . . .PAGE632632634634634634634G33635636638t1386386.78639722722762723723$723723$72472417257257257%72872887087087087087187187287287287287387487487587587'5875876a7395295CONTESTS .... XlllBERTHELOT . Volatility of Sulphur and Mercury . . . . . .WITZ (G.). Sulphurous Anhydride in the Air of Towns . . . .RATHEE (R.). Nature of Selenium Sulphide and of Alloys . . . .RUDORFF (F.). Compounds of Arsenious Oxide . . . . . .DIDIER (P.). Sulphides of Cerium and Lanthanum . . . . .NEWBURY (8 . B.). Action, of Light on Silver Chloridesulphate . . . . . . . . . . . . .MARTINON . Reducing Action of Hydrogen Peroxide . . . . .bonk Oxide by Carbon . . . . . . . . . .VAN’T HOFF (J . H.). Transformations of Sulphur . . . . .sulphide . . . . . . . . . . . . .GERNEZ (D.). Nacreous Crystals of Sullphur . . . . . .SABATIER (P.) . Hydrogen Persulphide . . . . . . .LUNGE ((3.). Solubility of Nitric Oxide in Sulphuric Acid .. . .MOISSAN (H.). Combination of Bromine with Phosphorus Trifluoride .YFORDTEN (0 . v . D.) . .GLASER (M.). Action of Potassium Permanganate on Sodium Thio-Formation of Red Silver Solutions by Reduction . . . .NAUNAXN (A.) and C . PISTOR . Reduction of Carbonic Anhydride to CarsMAQUENNE . Sulphur Liberated by the Decomposition of Hydrogen Per-MATHIEU-PLESSY (E.). Acetic Acid and Alkaline Thiosulphates . .GIRAUD (11.). Action of Ammonia on Solutions of Potassium Salts . .MULLER (A) . Action of Carbonic Anhydi-ide on Potassium Chloride inPresence of Various Amines . . . . . . . . .ARTH (G.). Action of Anhydraus Ammoniacal Ammonium Nitrate onRle tals . . . . . . . . . . . . .BIOBIX (H.). Action of Cadmium on Ammonium Nitrate .. . .Cr&E (P . T.). Didymium Compounds . . . . . . .VORTNANN ((3.). Cobalt-ammonium Compounds . . . . . .Extraction of Zirconia and the Qualitative Compositionof Zircon . . . . . . . . . . . .Co-operation of Water in the slow Oxidation of Zinc, Led,Slow Oxidation of Copper in Presence of Dilute SulphuricCo-operation of Water in the Combustion of Carbonic Oxide,aud Formatioil of Hydrogen Peroxide during such Combmtion . .Formation of Hydrogen Peroxide during the Combustion ofHydrogen . . . . . . . . . . . .Action of Direct Sunlight on Nitric Acid mixed with CarbonLINKEN ~ X N (E.).TRATJBE (M.).TRAUBE @I.) .TRAUBE (31.).TRAUBE (31.).Iron, and Palladium-hydrogen . . . . . . . .Acid, or ofa Solution of Ammonium Carbonate . . .. .GERNEZ (U.). Transformations of Sulphur . . . . . . .GAT (J.). Absorption of Nitric Oxide by Ferrous Salts . . . .B isulphide . . . . . . . . . . . .KLOBUKO w (N . v-) . Alkaline Tetrathionates . . . . . .TIFFEREAU .HONIG (31.). Action of Potassium Permanganate on Sodium Thioaulphate .BOHLIG (E.). Action of Silver Nitrate on Pure Potassium Monocarbonate .PUTTNER . Preparation of MagnesiumGORE ((3.). Reducticn of Metallic Solutions by Means of Gases, &c . . .CAVALZI ( A ) . Dissolution of Alurnii?ium i n Alkaline Hydroxides . .. . . . . . . .VILLE (J.) . Crystallised Zinc Hydroxide . . . . . . .WILSBACH (C . v.). Separation of Didymium into its ElementsTROOST (L.). Vapour-density of Thorium ChIoride . . . . .TROOST (L.). Thorium Metaphosphate .. . . . . .PICKEBING (53.1. Crystalline Basic Copper Sulphate . . . . .GUILLEMIN (G.). Alloys of Copper with Cobalt . . . . . .I~OUSSEAU ((3.). Manganites of the Alkaline Earths . . . . .VINCEXT (C.). New Rhodium Compounds . . . . . . .. . .WOOD (J.) and J . L . BORDEN . Action of Ammonia on the Haloger, Salts ofLend . . . . . . . . . . . . .GOXE (G.). Effect of Heat on Ammonium and Potassium Fluorchromates .LINDET (L.) . Gold Pliosphobromide~ aiid Phosphochlorobromides . .PAGE95395395495a955955955955933957103610361037103710371037105810381038103910391039104110421105110711081108110911091110111 i)1111111111121112111211 13111311131113111311141114111411141115111xiv CONTENTS .P.9GF:BRAME (C.).Pseudo-quadratic Octahedrons of Sulphur . . . . 1182MICHAELIS (A.) and W . LA COSTE . Valency of Phosphorus . . . 1182TILDEN (W . A.) and W . A . SHENSTONE .Saline Solutions . . . . . . . . . . . 1183SCHULTEN (A . DE) . Crystallised Magnesium and Cadmium Hydroxides . 1183HUMPIDGE (T . S.). Atomic Weight of Beryllium . . . . . 1184KNORRE ((3 . v.). Paratungstates . . . . . . . . . 1184KNORRE (a . v.) and P . OLSCHEWSKY .Antimonic Acid . . . . . . . . . . 1184Solubility of Calcium Sulphate inPotassium and Sodinm Salts ofB1inerctt.l og ical Chemistry .DOELTER ((7.) . .ARZRUNI (A.). Sulphur from Zielenzig . . . . . . .KRENNER (A.). Minerals of the Cryolite Group from Greenland .. .CATHREIN (A.). Microscopic Association of Magnetite with Titanite andRutile . . . . . . . . . . . . .Lasamx (A . v.). Pseudomorphs after Rutile . . . . . .VIVIER (A.). Apatite from Logrozan (Spain) . . . . . .DIEULAFAIT . .GCYRCEIX (H.). Minerals from the Metamorphic Rocks of Ouro Preto,Brazil . . . . . . . . . . . . .BEuTELr. (A.). The Potash Soda Felspars of Silesia . . . . .ARZRUNI (A.). Minerals €rom a Chromite Deposit . . . . .DAMOUR and DES.CLOIZEAUX . Msgnesian Epidote . . . . .Effect of Heat on Vesuvian. Apatite. and TourmalineRAMMELSBERG (C.). Xatural Borates . . . . . . . .Origin of the Phosphorites in the South-west of Fmnce .IGELSTROM (L . J.). Empholite . . . . . . . . .STARKL (G.). Schuchardtite . . . . . . . . .AEZRUNI (A.).Groddeckite, a New Zeolite . . . . . . .SCRARIZER (R.) . Constitution of the Amphiboles containing Alumina .SOXMERLAD (H.). Leucite- and Nepheline-basalt from the Vogelsberg .GONNARD (I?.). A Pegmatite containing large Crystals of Chlorophyllite .MANN (P.). Chemical Composition of dugites from Phonolites and SimilarRocks . . . . . . . . . . . . .LODIN . The Brown Coal of Tstria and Dalmatia . . . . . .BRUCE (J . D.). Analysis of Cassiterite from King Go., N . Carolina . .ROWAN (G . H.). Apatite from Amelia Co., Virginia . . . . .DIEULAFAIT . Origin and Formation of Masses of Calcium Phosphate inDE GASPARIN (P.). Phosphatic Deposits of the Souhh-east of France . .LJUBAVIN (N.). Investigation of a Haltpetre-earth from Turkestan ..REESE (C . L.). Analysis of Pinite from Madison Co., N . Carolina . .PAGE (C . C.). . . . .ROBERTSON (R.). Albite from Amelia Co., Virginia . . . . .ROBERTSON (R.). Analysis of Chrpocoila from Gila Co., Arizona . .GONNARD (F.). The Pegmatite on the Borders of VizBzy, new Montbrison .TIIOULET (J.). Determination of the Coefficient of Cubic Dilatation ofMinerals . . . . . . . . . . . . .FOULLON (H . v.). Crystallised Copper from Schneeberg . . . .DITTE (A.). Fluor-apatites . . . . . . . . . .Sedimentary Rocks . . . . . . . . . . .ROBERTSON (R.). Blue Quartz from Nelson Co., Virginia . . . .Amazon Stone froin Amelia Go., VirginiaROSCOE (H . E.). Diamond-bearing Rocks of South Africa . . . .DECHEN (v.). Silver Amalgam from Oberlahnstein .. . . .KLINQER (H.) and R . PITSCHKI . Siegburgite . . . . . .DEWALQUE (G.). Hatchettine from Seraing . . . . . .DOLL (E.) . Pseudomorphs . . . . . . . . . .KRENNER (J . A.). Stibnite from Japan . . . . . . .B R ~ N (A.). A Crystal of Stibnihe from Japan . . . . . .GONNARD (F.). Mineralogizal Notes on the Environs of Pontgibaud . .2627272728293030303131313132323233343412512612612612712712812913013013013013113121821922022022022022122122COPU'TENTS . xvWADA . Japanese Minerals . . . . . . . . . .Twin Crystals of Zircon . . . . . . . . .FOULLON (H . v.). Products of the Alteration of Pitchblendenear Nischne-Tagilsk . . . . . . . . . .RATH (G . v.). Colemanite .. . - . . . . . .DITTE (A.). Fluorapatites . . . . . . . . . .LACROIX (A.). Artificial Gypsum Crystals . . . . . . .Sevier Co., Tennessee . . . . . . . . . .DUDGEON (P.). Occurrence of Linarite in Slag . . . . . .LACROIX (A.). Wulfenite from Beaujolais . . . . . . .FRANZENAU (A.). Amphibole from the Aranyer Mountain . . . .LEWIS (1% . C.). An American Locality for Helvine . . . . .IGELSTROM (L . J.). Hyalophane from Jakobsberg . . . . .ROWAN (G . H.). Kaslinite from Calhoun Co., Alabama . . . .GFYOT (3f.). Description of a Crystal of Euclase . . . . .EONIG ((3 . A.). Orthite from Virginia . . . . . . .DOBBIE (J . J.). Variety of Saponite . . . . . . . .DOELTER (C.). Relation between the Optical Properties and ChemicalComposition of Pyroxene .. . . . . . . .LODIN . New Mineral from Godemas . . . . . . . .WOLFF (J . E.). Xepheline Rocks of the United StatesHAPEE (L.). Meteorite from Durango . . . . . . .MAUGINI (F.), Meteoric Sand . . . . . . . . .SABATIER (P.). Mineral Water of Salies-du-Salat . . . . .LEFORT (J.). Arsenic in Mineral Waters . . . . . . .SMITH (F . S.). Ozokerite . . . . . . . . . .BRUCE ( J . D.). Marmalite from Hinimelfahrt Mine, Freiburg . . .FOOTE .MIKLVCHO-MACLAY (3% . v.). Listwaenite from the Poroschnaja Mountain,LACROIX (A.). Accidental Formation of Cerussite Crystals on Roman Coins. . .BROWN (W . (3.). A new Hydrous Mangancse Aluminium Sulphate fromBRADBURY (C . M.). .CABRLL ( J . M.). Infusorial Earth from Richmond, Virginia . . .CHAPPELL (L .N.). .Garnet (Tar . Spessarite) from Amelia Co., VirginiaVariety of Chloropal from Albemarlc Co., Virginia. . . .SOUBEIRAN (L.) and Gt . MASSOL . Water from the Red Spring of Zucaune(Tarn, France) . . . . . . . . . . .DERBY (0 . A.). Occurrence of Gold in Brazil . . . . . .KIMEALL ( J . P.). Specular Iron Ores of Cuba . . . . . .LANG (J.). Bauxite from Langsdorf . . . . . . . .MIERB (H . A.). Hemiliedrism of Cuprite . . . . . . .EWING (A . L.). Erosion of Limestone . . . . . . .JACESON (A . W.). Colcmanite . . . . . . . . .SACC . Saltpetro Deposit . . . . . . . . . .HIDDEN (W . E.) and J . B . MACKINTOSH . Herderite from Oxford Co.,Maine . . . . . . . . . . . . .SCHAEFFER (C . A.). A New Tantalite Locality . . . . . .BLAEE (W .P.). Columhite in the Black Hills of Dakota . . . .DANA (J . D.). Sand and Kaolin from Qvlartzite . . . . . .MCKELVEY (J . W.). Siliceous Earth from Morris Co., New Jersey . ISMITH (E . G.). Chrysotile from Shipton, Canada . . . . .TRAUBE (It.). Nephrite from Jordansmuhl, in Silesia . . . . .DERBY (0 . A.). The Santa Catherina Meteorite . . . . . .PTSTOR (C.). Mineral Spring " Romerbrunnen. .. a t Echzell, Wetteran . .BLAEE (W . P.). Crystallised Gold in Prismatic Forms . . . .GRABOWSKI . Ozokeriteand Ceresine of Galicia . . . . . .PECKHAM (8 . F.). Origin of Bitumens . . . . . . .BROWK (W . G.). .GENTH (F . A.). Herderitc . . . . . . . . .NEWBERRY (S . B.). . . .BLAEE (F . H.). Vanadinite in Arizona . . . . . . .GORCEIX (H.) .Cassiterite from Irish Creek, Rockbridge Co., VirginiaSpecimens of Nickel Ore from NevadaMonazite Sands from Caravellas, Proxkce of Balsia, BrazilPAGE22122222222222422422422522622622622622622722722722822822832822922922923023023023123123223235635635635735535835835935935936036036136136136136248748748848848848948948x vi CONTENTS .TERRETL (A.).Analysis of Chrysotile . . . . . . . .PEXFIELD (S . L.). Occurrence of Alkalis in Beryl . . . . .CLARKE (F . W.) and T . M . CHATARD . Mineralogical Notes . . . .WILLIAXS (G . H.), Paramorphosis of Pyroxene to Hornblende in Rocks .DILLER (J . S.). Fulgurite from Mt . Tliielson, Oregon . . . . .MALLET (J .IV.). Meteoric Iron from Wichita Co., Texas . . . .BERTON (G.). Mineral Water of Acquarossa . . . . . .LORENZEN . Analyses of Metallic Iron from Greenland . . . .CARNOT (A.) . The Composition of Coal in Relation to the Plants from whichit is Derived . . . . . . . . . . . .EASTMANN (I . R.). New Meteorite . . . . . . . .SCHMIDT (A.). Isomorphism of Jordanite and Meneghinite . . .GORCEIX (H.), Hydrated Titanium Oxide from DiaInantina . . .DIEULAFAIT . Concentration of Zinc Carbonate in Dolomites . . .DAXOUR (A) . New Alumina Lime Phosphate . . . . . .SANDBEROER (F.). Fairfieldite from Rabenstein . . . . . .SANDBERGER (I?.). Manganese in Apatite . . . . . . .DORING (A.) and others . Vanadntes from the Argentine Republic . .ZEPHAROVICH (V .v.). Mineralogical Kotes . . . . . .DESCLOIZEAUX . Eudnophite . . . . . . . . .FOUQUB . Triclinic Felspar from Quatre Ribeiras . . . . . .SANDBERGER (J?.). Boric Acid in Mica . . . . . . .FREDA (G) . Clirysocolla from Etna . . . . . . . .Secondary Linrestones . . . . . . . . . .WEUNIER (S.). Deposit from a Spring at Carmnux . . . . .BECPENKSMP (J.). The Ooeflicients of Elasticity of Crystals . . .ILOWAY (L.). Conditions for the Formation of Native Sulphur . . .JANNASCH (P.). The Percentage of Water in Clinoclilore . . . .DAMOUR (A.). New Mineral from the Environs of Nantes . . . .COHEN (R.). Labradorite Rock of the Coasts of Labrador . . . .DIEULAFAIT . Origin of Iron, Manganese, and Zinc Minerals in the OlderSCHAFARZIK (F.). Native Mercury, Cinnabar, and Chromium Ores fromPAGE49049049149249349349449a639639639640640640640640641641641642648643643643644641!644!729729Serria . .. . . . . .KRENYER (J . A.). Orpiment and Realgar from Bosnia .LOCZKA (J.). Smithsmite from Yelsocz drd6 . . .IiroRTDAHL (T.). Colemanite . . . . . .XRENNEB (J.). Optical Properties of Allactite . . .RAMMELSBERG (C.). Cuprorlescloizite . . . . .STRUVER (J.). Columbite from Craveggia, Piedmont . .KOCH (A) . New Locality for Vivianite . . . .ICINTZE (C.). Microlite . . . . . . .MARKOWNIKOFF (V.). dstraaanite . . . . .Busz (C.). Barytes from Mittelagger . . . . .FBNYES (I).). Barytes from PBsey . . . . .PRANZENAU (A.). Anglesite from Felso-Viss6 .. .YRIMICS ((3.). Mineralogical Notes from Transylvania .BODEWIO (C.). Nephrite from Tasmania . . . .LOCZEA (J.). Wollastonite from RQzbBitya . . . .7 ~OLTEE (C.). iirigites . . . . . . . .MALY (R.). Andesite from Trifuil in Styria . . . .REINSCH ( P . I?.). Chemical Composition of Coal . . .JACKSON (A . W.). Colemanite . . . . . .KXOP (A.). Augites of the Kaiserstuhl Mountains . .Kocn (F.). Analyses of Transylvanian Minerals . . .SENHOFER (C.). Sericite from the Quartz-phyllite of WiltauWILEINSON (E.) .DIEITLAPAIT . Non-volcanic Origin of Boric Acid . . .DIEULAFAIT . Origin of Boric Acid . . . . .STOCKLASA (J.). Distribution of Phosphates in Bohemia .CEBARO ((3.). Koninckite . . . . . . .Occurrence of Native Mercury in Louisiana.....\ ,. 730 . 730 . 730 . 730 . 731 . 731 . 731 . 732 . 732 . 732 . 733 . 733 . 733 . 733 . 733 . 734 . 734 . 735 . 735 . 735 . 736 . 876 . 876 . 876 . 876 . 876 . 877 . 87CONTENTS .MACKINTOSH (J . B.). Analysis of Titanic Iron Sand from Brazil . .HIDDEN (W . E.). Mineralogical Notes . . . . . . .HILLEBRAND (W . F.). New Minerals from Colorrtdo . . . . .LUPTON (N . T.). Meteoric Iron from Coahnila, Mexico . . . .FISCHER (E.). Chemical Examination of Nocerine . . . . .Borax Deposits in California and Nevada . . . . . . .HAXKS (€3 . (3.). Borax Deposits . . . . . . . .BODEWIQ (C.) and G . v . RATH . . . .MOORE (G . E.) and V . v . ZEPHABOVICH . Calaite, Pseudomorphous afterApatite, from California . . . . . . . . .~ J O G R E N (H.) .Manganese Arsenates from Nordmarken in Wermland .SNITH (E . F.). Mineralogical Notes . . . . . . . .MEUNIER {S.). Synthesis of Anorthite . . . . . . .WERVEKE (L . v.). Ottrelith Rocks of Ottr6 and Viel-Salm . . . .MIJKTZ (A.) and V . MARCANO . Formation of Deposits of Nitrates in Tropi-SCHULTEN (A . DE) . Artificial Production of Strengite . . . . .FOULLON (H . v.). Native Tellurium from FaFzebaja . . . . .LEWIS (J . W.). Crystalline Form of Miargyrite . . . . . .WELCH (J . C.). Limonite . . . . . . . . . .KENIWOTT (A.). Priceite, Coiemanite, and Pandermite . . . .STAUTE (H.). Pinnoite. a New Borate from Stassfurt . . . . .ATANASESCO . Analysis of Artificial Brochantite . . . . . .BAREOIS . Chloritoi'd from Morbilian . . . . . .. .DESCLOIZEAUX . Crystalline Form and Optical Characters of Sismondine .KENNGOTT (A.). Nephrite from Jordansmiihl in Silesia . . . .NORDENSPJOLD (A . E.). Uranium Silicate from Garta . . . .DIEITLAFAIT . Origin of Manganese Minerals . . . . . .VEBBEEE (R . D . M.). Pyroxene-andesites from the Dutch Indian Archi-pelago . . . . . . . . . . . . .MALLET (F . R.). Native Lead and Chromite from the Andaman Islands .LuP~ors (N . T.). Analyses of Bituminous Coals from Alabama, Tennessee,MIKLUCHO-MACLAY (M . v.). Rutile and Cassiterite in the GriefensteinWEINBERG (A . M.). Kaolin Deposits of South-west Russia . . . .Colenianite from Californiacal Regiom . . . . . . . . . . . .STRENG (A.), Diopside from Zermatt . . . . . . . .and Kentucky . .. . . . . . . . . .XV iiPAGE8788788'788798809579579579579589599609609611042104<3111611161116111711171117111811181118111911191119112011851185Granite . . . . . . . . . . . .RINNE (F.). Rutile from Imfeld . . . . . . . .J E R E ~ E F F (P . W.). Russian Caledonite and Linarite . .SCHNEIDER (L.). Wolfram . . . . . . . .HANKEL (W.). Thermo- and Actino-electricity of Rock Crystal .LEMBERG (K.). Formation and Alteration of Silicates . . .RINNE (F.). Milarite . . . . . . . . . .TSCHERMAK ((3.1. Proportion of Chlorine in Scapolites . .LACROIX (A.). Diagnosis of Zeolites . . . . . .EOLENKO (B.). Pseudomorphs of Hornblende after Olivine .MEYER (A . B.). Unwrought Jadeite from Switzerland ..TEAUBE (H.). Nephrite from Jordansmuhl in Silesia . . .BATCH (F . H.). Hypersthene Andesite from €'em . . .HUSSACK (E.). Distribution of Cordierite in Rocks . . .HOOD (W.). Nickel Ore from Piney Mountain, Oregon . .BATJMHAUER (E . H . v.). The Ngawi Meteorite . . . .. 1185 . 1186 . 1186 . 1187 . 1187 . 1187 . 1187 . 1187 . 1187 . 1188 . 1188 . 1189 . 1189 . 1190 . 1190 . 1190Organic C F, emis try .BRIX (R.).EOHNLEIN (B.).Exchange of Chlorine. Bromine. and Iodine between OrganicExchange of Chlorine. Bromine. and Iodine between Inor-and Inorganic Compounds . . . . . . . . . 34ganicand OrganicCompounds . . . . . . . 35VOL . XLFIIT . CONTENTS.PAGEPAGE (A. (2.1. Action of Chlorine on Organic Compounds in Preeence ofNAUDIN (L.).Anthememe, a Hydrocarbon from Roman Chamomile . .GREENE (W. H.). Diethoxymethane j and Prepamtion of Methylene Dichlo-ride , . . . . . . . . . . . .EHRENBJCRG (A.). Mercury Fulminate . . . . . . .SCHOLVIEN (TJ.). Merniry Tulminate . . . . . . . .NENCEI (M.) and BOURQUIN. Rhodanic acid . . . . . .TOLLENS (B.). Circular Polarisation of Dextrose . . . . .LIPPMANN (E. 0. T.). Non-identity of Arabinose and Galactose . . .URECR (F.). Influence of Temperature and Concentration of HydrochloricAcid on the Rate of Inversion of Saccharose . . . . . .ZABOUDSKY. “Hydrate of Carbon” from Cast-iron . . , . .BEILSTEIN (I?.) and E. WIEGAND. Angelic and Tiglic Acids . . .CONRAD (M.) and M. GUTHZEIT. Halogen Derivatives of Ethyl Levulinate.DIETERLE (W.) and C.HELL, Adipic Acid . . . . . . .HELL (C.) and G. LUMPP. Normal But,ylmalonic Acid, a New IsomericPimelic Acid . . . . . . . . . . . .GANTTER (F.) and C. HELL. Occurrence of Pimelic Acid amongst theOxidation-products of Castor-oil . . . . . . . .HAITINGER and A. LIEBEN. Chelidoni’c Acid . . . . . .OST (H*). Nitrogenous Derivatives of Meconic Acid . . , . .RITTHAESEN and 3’. WEGCER, Betake in Cotton-seed . . . . .VERNEUIL (A.). Seleniocarbamide . . . . . . . .NAHNSEN (R.). The Thiophene Group , . . . . . .NAHNSEN (R.). /3-Thiophenic Acid . , . . . . . .SCHUPPHAUS (R.). Action of Chlorine on Boiling Benzene . . .MEUNIER (J.). Isomeride of Benzene Hexachloride . . . . .PYIOLTING (E.). Orthonitrobenzyl Chloride . . . . . . .GUMBERT (F.).Decomposition of Benzonitrile by Burning Sulphuric Acid .GREENE (W. H.). New Synthesis of Saligenin . . . . . .FISCHER (E.). Compounds of Glucoses and Sucroses with PhenylhydrazineGRIESS (P.). Action of Potassium Cyanate on Metanitmmidobenzoic Acid .GREENE (W. H.). Action of Hydrochloric Acid and of Chlorine on Aceto-benzoic Anhydride . , . . . . . . . . .ZEHENTER (J.). Action of Phenol and Sulphuric Acid on Hippuric Acid .WIDMANN (0.). Nitrocumenylacrylic Acids and their Derivatives . .PEGHMANN (H. v.) and J. B. COHEN. Compounds of Phenols with EthylAcetoacetate . , . . . . . . . . . .WISLICENUS (J.). Reduction of Phthalic Anhydride by Zinc and GlacialAcetic Acid . , . . . . . . , . . .KOLBE (H.). Ieatin , . . . . . . . . . .UREENE (W.H.). Formation of Dibenzyl from Ethylene Dichloride andBenzene in Presence of Aluminium Chloride. . . . . .CAZENETJVE (P.). Trichlorocamphor . . . . . . . .KACHLER (J.) and 3’. V. SPITZER. Camphoronic Acid . . . .ETTI (C.). Eino’in in Malabar Kin0 . . . , , . . .EAYSEB (R.). Substances obntained in Saffron . . . . . .MICHAEL (R.). Carboxylic Acids from Synthetically Prepared PyridineBasm . . . . , . . . . . . . .HANSSEN (A.). Brucine . . . . . . . . . ,HEssE (0.). Alkaloi’ds from the Bark of Rernijia Pzcrdieana . . ,MIRAILOFF (W.). Preparatiop of Albumin . , . . . . ,NESCEI (M.) and N. SIEBER , . . . . . . . .STRUTE (H.). Studies on Blood . . . . . . . . .BLOXAM (C. L.). Some Reactions of Silver Cyanide . . . . ,CAMELS (G.). .~~CEMITY (C.) and.J. ROBENBEE. . Gallisin . , . , , . .Inorganic Chlorides . . . . . . . . .LERCH (J. U.). Chelidonic Acid , . . . . . .HABERMANN (S.). Acetonequinol . . * . . . . .Action of Primary Alcoholic Iodides on Silver Fulminate36373888394.Q4.Q414142424243M44454’748505050515252525253535354555555565758585859595960636469697113313313CONTENTS.RARBAGLIA (a. A.). Thiovabraldehyde . . . . ,RUBENCAMP (R.,). Aldehyde and Etliylidene Derivatives , . . .CHANCEL (G.) and F. PARNENTIER. Some Reactions of Carbon Bisulphide,and its Soluhility in Water . . . . . . . . .JUSLIN (W.). Normal a-Hjdroxyvalerie Acid . . , . .PECHBCANN (H. v.). Acetonedicarboxylic Acid .. . . ._ .BEHRMANN (A.) and A. W. HOFMANN. Amidee of Cit'ric Acid and theirConversion into Pyridine-derivatives . . . . . . .MEYER (E. 7.). Aetion of Ethyl Ghlorocarbonate on Nitrogenous OrganicCompounds . . , . . . . . . . . .KULZ (E.). Cptine . . . . . . . . . . .MEYER (V.). Prepadion of Pure Thiophene . . . . . .MEYER (V.) and 0. STADLER. Nitration of Thiophene. . . . .PETER (A.). Acetothienone and eome of its Derivatives . . . .PIKNER (A.). Decomposition of Benzonitrile by Fuming Sulphuric Acid .STAEDEL (W.) Dinityotoluene . . . . . . . . .JACOBSEN (0.). Bromo-substitution Derivatives of Ortho-xylene. . .GREVINGK (E.). Nitro- and Amido-derivatives of Metaxylene . .SCHALL (C.) and C . DRALLE. Action of Chlorine, Bromine, and Iodine onSodium Paracresolnte .. . . . . . . . .COLSON (A.). Saponification of Halond Ethers of the Benzene Series byNeutral Substanaes . . . . . . . . . . ,BUCR (K.). Conversion of Phenols into Amines . . . . . .BERLINERBLAU (J.). The Action of Cyanogen Chloride on Ortho- and Par-TRAUB (M. C.) and C. HOCK. A iakmo'id . . . . . . ,SAXDMEYER (T.). Substitution of the Amido-group in Aromatic nerivativjsby Chlorine, Bromine, and Cyanogen . , . . . . .HAGE~. (H.). Action. of Ethyl Chlorocarbonate on Paranitraniline . .KLINQER (H.) and R. PITscHxE. Oxidation of Paratoluidine . . .EFFEONT (J.). Two Isomeric Isobutylortliamidotoluenes . , , ,FROERLIC~ (E.). Derivatives of Benzoylpseudocumidine . , . .PHILIP (M.) and A. CALM. Derivatives of Parahydcoxydiphenylain~ .GUCCI (P.)..Action of Carbon Bisulphide on $Ietrtphenylenediamiine . .BAMBEROES. (E.). Mixed Am-compounds . . . . . . .PINNER (A,). Action of Acetic Anhydride on Bemamidine. . . .PINNER (A.). Action of Ethyl Acetoacetate on the Amidines , . ,ROSER (W.). So-called Phthalylacetamide . . . . . , ,KOLBE (€1.) Preparation of Anthranilic Acid . . . . . ,SILBERSTEIN (H.). Betaines . . . . . . . . ,PRIEBS (B.). Action of Benzaldehyde on Nitxornethane and Nitroethane .NORDMANN (E.). Pltracarvacrotic Aldehyde. . . . . .BLUNZEIN (F. 0.). Action of Bromacetophenone on Amides . , .Ppeparatios of Salicyljc Acid. . . . . . . . . .BJLUYGEIN (F. 0,). grominated Phthalic Acids . . . . . ,GABRIEL (S,). Constitution of Phthalylacetic Acid .. . . .RQSER (W.). Phthalyl Derivatives ; Conversion of Eetonic Acids intoLactones. . . . .GRAEBE (C.). Reductiin of 'Phthalimihe and Phihalide . . , .JACOBSEN (0.) Constitution of the Benzenetetracarboxylic Acids . .GABRIEL (S.) Action of Sulphuric Acid on AcetophenoneorthocarboxylicAcid . . . . . . . . . . . . .LIPP (A.) Methylated'hdoiee . . . . . . . . .GATTERNANN (I; ) Tolane Tetrachloride . . . , . . .EENRIQUES (R.). A New Method of Preparing Secondary Aniidoazo-derivatives . . . . - . . . . . . .ILINSKI (M.). Nitrosonaphthol and its Derivatives . . . . .MYLIUS (F.). a- and p-Hydrojugione . . . . . . . .EKSTBAND (A. (3.). A Sulphowde of Naphthalene , . . . ,amido-phenetoyl . . . . . . . . . .Preparation of Isatin . . .. . . * . .b 2xixPAGE136136137137138138144)14014114114114121421421M145&461471 . 73 4814@14916115115415515615715815815915916016016216216216216416516516616616716716716816916917xx CONTENTS .PAGEOSTERMAYER (E. ) and J . ROSIENHEK . Derivatives of the Isomeric Di-naphthols . . . . . . . . . . . . .WALLACH (0.). Ethereal Oils . . . . . . . . .WALLACH (0.) and W . BRASS . Oleum Cynsc . . . . . .HELL (C.) and A . RITTER . Aotion of the Halogen Acid0 on Wormseed Oil .EACHLER (J.) and F . V . SPITZER . The so-called Campholenic Acid . .'I'RAUB (M . C.) and C . SCHARGFXS . Coal-tar Quinoline . . . . .CLAUS (A.) and P . STEOELITZ . a-Diquinohe from Azobenzene .. .OSTERMAYER (E.) aud W . HENRICESEN . .PECHMANN (H . v.) and W . WELSH . Formation of Ppridine Derivatives .Condensation-products from Malic Acid . . . . . . .PECHIVUNN i(H . v.). Synthesis of Pyridine Derivatives . Coumalinic Acid .SCHOTTEN (C.). Oxidation of Piperidine . . . . . . .SCHOTTEN (C.) and J . BAUM . A New Oxidation-produet of Conine . .BARBAGLIA (U . A.) . Parabuxinidine, a Fourth AlkaloYd from BUXWsempervirens . . . . . . . . . . . .BAUMERT (G.). Lupinidine from Lupinus luteus . . . . .NENCKI (M.). Albumin of the Splenic Fever Bacilla . . . . .REFORMATSKY (S.) . The Hydrocarbon, CBHI4, prepared from AlIy1-diekhylCarbinol . . . . . . . . . . . . .HABEL (L.). A Reddish Colomtion of Cyanide Solutions . . . .BTARD (A.) and G . B$MONT .Hjdroferrocyanic Acid and its Derivatives .SCHATZKY (E.) . Action d Ally1 and Isobutyl Iodides on Zinc and Acetone .SCHESTAKOFP (W.). Composition of a Bye-product obtained in the Prepara-tion of Diallyl Carbinol . . . . . . . . . .GEUTHER (A.). Derivatives of Symmetrical Isodichlorethyl Ether . .'B~CHAMP (A.) . Optical Inactivity of Cellulose and the Rotatory Power ofPyroxylin . . . . . . . . . . . .FLEBRY (G.). Grwillea Gum . . . . . . . . .NORDMANN (E.). Ethenylamidoxime and its Derivatises . . . .PRATESI (L.). Trioxymethylene . . . . . . . . .LOBRY DE BRUYN (C . A.). Action of Hydrocyanic Acid and of Dilute Sul-phuric Acid on Aldol . . . . . . . . . .LOV~N (J . M.). Some New Sulpho-derivatives of the Fatty Acids ..ALBITZKY (A.). P-Dipropjlacrylic Acid . . . . . . .LOBRY DE BWYN (C . A.). Propenylglycollic Acid . . . . .ANSCH~~TZ (R.). Formation of the Anhydrides of Mono- and Di-basic AcidsANSCHUTZ (I%.). Racemic Acid and the Calcium Salts of the Four IsomericTartaric Acids . . . . . . . . . . .HJELT (E.). Ethylidinethenyltrimrboxylic Acid . . . . . .BISCHOFP (C . A.) and C . RACR . Ethyl Acetylenetetracarboxylate . .CANZONERI (F.) and V . OLIVERI . Monobromo- and Dibromo-pyromucicAcids . . . . . . . . , . . . .ESSNER (J . C.). Action of Hydrogen on Aeetamide . . . . .LIPPMANN Occurrence of Leucine and Tyrosine in Beet-Nolasses . . . . . . . . . . . .BEHREND (R.). Derivatives of Carbamide . . . . . . .CIAMICIAX (G . L.) and M . DENNSTEDT .Action of Hydroxylamine onPyrroline . . . . . . . . . . . .KNORR (L.) . Synthesis of Furfurane-derivatives from Ethyl Diaceto-succinate . . . . . . . . . . . .PAAL (C.). Derivatives of Ethyl Acetophenoneacetoacetate and of EthylMEYER (V.) and 0 . STADLER . The Thiophene Group . . . . .SCHULZE (K . E.). A Simple Method of obtaining Thiotolene and ThioxyleneLELLMANN (E.). The Benzene Theory . . . . . . . .ISTRATI . Monochlorethylbenzene . . . . . . . .JANNASCH (P.). Monobromoparaxylene . . . . . . .Synthesis of a-Diquinoline .RIESS (C.). Derivatives of Cyanethine . . . . . . .(E . 0 . v.).CIAMICIAN ((3 . L.) and P . SILBER . Pyrroline a-Carboxylic Acid . . .Acetonylacetoacetate . . . . . . . . . .1711v11711721'731731731731741751761761771771772322332332352372372372372382382443241)24124224224324324324424!4!24524524624624624724825025125125125CONTENTS .ESSNES (J .C.) and E . GOSSIN . AcetyltolueneWALLACE (M.). Carbonates of Bivalent Alcohols and Phenols . . .PAUCKSCH (H.). Derivatives of Amidoethylbenzenes . . . . .BLADIN (J . A.). Action of Cyanogen on Aromatic DiamiiiesFISCHER (E.). Constitution of the Hydrazines . . . . . .BERNTHSEN (A.). Methylene-blue and Allied Dyes . . . . .FISCHER (0.) and at . KORNEB . Chrysaniline . . . . . .OTTO (R.) and H . DAMK~HLEB . Disulphones . . . . . .of .Anhydrous Oxalic Acid . . . . . . . . .. . . . . .C'OLSOW (A.) .ESSNER ( J . C.) and E .GOSSIN .JACKSON (C . L.) and A . E . MENKE .Action of Phosphoric Chloride on Ethers of the BenzeneSeries . . . . . . . . . . . . .Action of Benzoio Chloride on Isodurene .Action of Phosphorous Trichloride onAniline . . . . . . . . . . . . .. . .WROBLEWSEP (E.). Decomposition of Diazo-compounds by Alcohol . .ZINCKE (T.) and A . HEBEBRAND . . Action of Quinones on AmidophenolsKUHN (B.). Action of Pllenyl Isocyanate on Amido-compounds . . .ELBS (B.) and E. LARSEN . Paraxylylphenyllietone . . . . .ANSCHUTZ (R.). Replacement of two Chlorine-atoms in Chlorides bp meansBISCHQFF (C . A.) and C . RACH . .VALENTINI (A.). Parmethoxyphenoxycinnamic Acid . . . . .LELLMANN (E.) and R . GROTHMANN . Deriratires of Salicylic Acid . .SCHIFF (H.) and C .PARENTI . Ethyleneamidobenzamic Acid . . .Derivatives of Whonitrobenzoic AcidBERCHFM (P . D E ) ~ . Ditolylphthalide . . . . . . . .GRAEBE (C.) and P . GUYE . Diphthalyl . . . . . . .ROSER (W.). Phthalyl-derivatives . . . . . . . .FRIEDEL (C.) and J . M . CRAFTS . Decomposition of Sulphonic Acids . .BEYER and BEQEL . Preparation of Ihnitruphenolsulpho~c Acid . . .ANSCH~TZ (R. ) and H . IUMENDOEFF . Action of Alaminium Chloride . .ZINCKE (T.) and A . BEEUER . The Hydrocarbon C16Hi2 from StyroleneAlcohol . . . . . . . . . . . . .OISHI (H.). Japaneee Camphor Oil . . . . . . . .CAZENFUTE (P.). Bromonitro.camphor . . . . . . . .GOLDSCHMIDT (H.). The so-called Oxycamphor of Kachler and] Spitzer .LANQLEBERT (A.). Convallaria majalis (Lily of &he Valley) .. .JACKSON (C. L.) and A . E . MENKE . Substances obtained from Turmeric .CONINCK (0 . DE) . Decomposition of PyPidine Methiodides and EthiodidesCONINCK (0 . DE) . Pgridine-deyivrttives from Brucine . . . . .KNORR (L.) and 0 . ANTRICK . Constitution of Quinoline . . . .ROSEE (W.). Diquinoline from Benzidene . . . . . . .GAUTIBR (A.). New Method for the Synthesis of Nit. mgensus OrganicHESSE. (0.). Synthesis of Homoquinine . . . . . . .HUFNER (G.). Crystalline Metahsmoglobin from the Dog . . . .H~?FNER (G. ) and M . BUCHELER . Oxyhaenioglobin of the Horse . . .KUHNE (W.) and R . CHITTENDEN . . . .BRIEGER (L.). Basic Products (Ptonia'ines) from Human Corpses . .COPPOLA (F.). Genesis of Ptoma'ines . . . . . . . .GUSTAVSON ..CHANCEL (e.) and F . PARMENTIER . Chloroform Hydrate . . . .KIESEL Constitution of Nitroparaffins . . . . . . .&ARD (A.) and G . B$MONT . Alkaline Ferrocyanides and their Compoundswith Ammonium Chloride . . . . . . . . .JAMES (J . W.). Action of Chlorine on Ethyl Thiocyanate . . . .MILLER . Preparation of Canarine . . . . . . . .SARDO . Catalpic Acid . . . . . . . . . . .by the Action of Alkalis . . . . . . . . . .BERENP (L.). Dimethylquinoline I1 . . . . . . . .Compounds . . . . . . . . . . . .SHENSTONE .( W. A.). Biwcine . . . . . . . . .EANSSFN (4.). Brucine . . . . . . . . . .New Forms of AlbumoseReactions of Aluminium Salts with Organic Compounds .XXiPAQE25225225325425425525625725725725926026026126126326326426.526626626726726826926926927C27e2702712712722722732 732;'42732752762762?627627727727827836336336436436536x xii COPU’TENTS,NATTERER (E.).Dichlorether . . . . . . . . .WISLICEEUS (J.). Reactions of Dichlorether . . . . . .LIPMANN (E.). Actioa of Benzoic Peroxide on Amylene . . . .MCGOWAN (G.) . Trichloromethylsulphorrie Chloride and the Derivatives ofSOKOLOBOFF . New Anhydride of Mannitol . . . . . . .TOLLENS (B.). Raffinose (Melitose 3) from Molasses . . . . .SCHUBERT (S.). Action of Heat on Starch Granules . . . . .SCHOOR (W . K . J.). . . .LRVALLOIS (A.). Optical Activity of Cellulose . . . . . .BBCHAHP (A.). Rotatory Power of Solutions of Cellulose in Schweim’sReagent .. . . . . . . . . . . .FREMY (E.) and URBAIN . Cutose . . . . . . . . .WILLIAMS ((3.). Trimethylamine and Pyrolline from Coal Gas . . .QOVILLIER (E.) and H . MALBOT . Tetramethylammonium Nitrate . .WaaNEn (E.). Action of Zinc Organo-metallic Compounds on Aldehydes .COTTOK (M . S.). . . . .PETER (J.) and 0 . DE ROCHEFONTAINE . Crystalliaed Anhydrous ZincAcetate . . . . . . . . . . .LE CANU (J . A.). Compound of Ethyi Acetate witch c‘alcium Chloride .HENRY (L.). Halord Substitution Derivatives of Propionic Acid . . .DUVILbIEn (E.). a-Ethylamidopropionic Acid . . . . . .KRAFFT (F.) and T . BRUNNEE . Residue obtained by the Distillation ofCastor-oil in a Vacuum . . . . . . . . . .COSLIB (J . N.). Action of Ammonia on Ethyl Acetoacetate .. . .MOEHSIN BEG CHANLAROFF . Butyrolaclone and a-Ethylbutyrolactone .FITTIG- (R.) and M . RUHLMANN . Action of Water and Hydriodic Acid onValerolwtone and Isocaprolactone . . . . . . . .FITTIGF (R.). Condensation-products of the Lactones . . . . .JONES (E . J.). Decomposition of a-Me~hylpropyl-P-hydroxybutyric Acidby Heat . . . . . . . . . . . .ULSCH (K.). Decomposition of Ethyl Chlorocarbonate by Zinc Chloride .VERNEUIL (A.). SeleniocaPbamide . . . . . . . .SCHIFF (H.). Aspartic Acid . . . . . . . . . .MICHAEL (A.) and J . F . WING . Optically Inactive Aspartic Acid . .FIscHmt (0 . W.). Two Tin Organic Compounds . . . . . .CIAMIOIAN ((3.) and M . DENNSTEDT . Action of Organic Anhydrides onPyrroline . . . . .. . . . . . .SCHBAYM (J.). Formation of Parabromobenzyl Bromide by the Action ofBromine on Parabrornotoluene . . . . . . . .Methylsulphonic Acid . . . . . . . . . .Action of Certain Substances on DestrinAction of Metals on Chloral HydrateAUWERS (K.). Pseudocumenol . . . . . . . . .SPITZ (G.). Mixed Ethers of Resorcinol . . . . . . .NOLTINGF and WEINGFARTNER . Colouring Matter from Paramidophenol .GASTIBER . Ethyl Paratolplnitrosamine . . . . . . .NOLTINGF and FOREL . Xylidines . . . . . . . . .NOLTINGF and KOHN . New Cumidine . . . . . . . .GEBHARDT (W.). Secondary Amines . I1 . . . . . . .NOLTING and WEINQARTNEB . Ethenyldiphenyldiamine . . . .NOLTIKGF and BAUMANN . Derivatives of Cnmidine and Amidoazobenzene .NOLTING and BAUMANN .Azo-derivatives . . . . . . .N O L T I N G ~ ~ ~ BINDER . Diazoamido-derivatives . . . . . .ZIMMERMANN (J.) and A . MULLER . . NOLTING and KOHN . Tetramethylazyline . . . . . . .BENEDICT (R.) and P . JULIUS . A New Resorcinol BlueBERBER (F.). Action of Acetamide on Phenylcyanamide . . . .CALM (A.). A Reaction of Aldehydes . . . . . . . .New Synthesis of Pararosaniline . . . . .GmHanDT (W.). Action of Ammonia and Amines on Thiocarbamides .ROSSLNQ (A.) . Condensation-products of the Derivatives of SalicylaldehydeNOLTING and KOHN . Terephthalophenone . . . . . . .NOLTING and BAUMANN . Quinones . . . . . . . .PAGE3653663663673673683683693693693693693703703713’7137137237337337337437537537637637637737737737837938038138138138138338338438438538538638638638’738738738838939CON 'I'ENTS.xxiiiALEXBEFF (P.). Derivat. ives of Azocumic Acid . . . . . .HOCESTETTEB (H.). Melilotic Acid and Anhydride . . . . .EBEBT (G-.). Action of Hydrobromic Acid and Bromine on Coumarin.Coumarone. and Orthocoumaric Acid . . . . . . .PERL (J \ . Thiosulphonic Acids and Sulphinic Acids of Toluene . . .ZINCKE (T.) and H . BINDEWALD . Phenylhydraeine Derivatives of a- and,B.Naphthaquinone . . . . . . . . . . . .KORN (0.). Dinaphthyldiquinone . . . . . . . .SKRAUP (2 . H.) and 0 . W . FISCHER . . . .SKRAUP (Z . H.). New Method of Preparing Phenantholine . . . MethylphenanthrolineFROST (B.). Constitution of Terebic and Teraconic Acids .. . .L~oN-SOUBEIRAN (J.). Wood-oil from Cochin China . . . . .MATSCH (H . C . C.). Stearopten from Essence of Patchouli . . . . JAHNS (E.). Eucalyptole . . . . . . . . . .BREDT.(J.). Camphoronic Acid . . . . . . . . .GUIGNET (E.). Existence of Glycyrrhiein in several Vegetable Families .DUNSTAN (W . R.) and F . W . SHOET . Glucoside from Strychnos nzcxvomicaPAGB390390391391391392392393393394394394395395395GERRARD (A . W.). Crystalline Substance from Jambosa Root . .FRIDOLIN . Chebulinic Acid . . . . . . . . .GREENISH (T.). Pipitzahoic Acid . . . . . . .BELOHOUBEK (A.). Colouring Matters of Ebony Wood . . .HANTZSCH (A.). Decomposition-products of Pyridine Derivatives .VULPIUS (G.) . Thallin Preparations .. . . . . .Flavaniline . . . . . .FISCHER (0 . W.). Diquinolines . . . . . . . .FOURNEAUX (E.). Nitroparatoluquinoline . . . . . .FISCHER (0.) and E . TAUBER .SPALTEHOLZ (W.). Quinoline DTes . . . . . . .HOFMANN (A . W.). Conhydrine Derivatives . . . . .SALOMON { (3.1. Paraxanthine . . . . . . . .SCHULTZ (J . J.). Alkaloi'ds of Copt& trrolia . . . .EIJEMAN (J . F.). The Poisonous Constituents of Skopoliajaponica .VILLIERS (A.). E" ormation of Ptoma'ines in Cholera . . . .KRUKENBERG (C . F . W.). Chemical Constitution of Cartilage . .CHICHPOFF . Composition of Albuminoyds . . . . . .REGECZY (E . v.)* Diffusion of Albumin Solutions . . . .DRA~ENDORPF and SPOHN . Alkaloi'ds of Aconitum lycoctonum . .EIJKMAN (J .F.). The Alkalond of Macleya cordatct . . . .. 396 . 396 . 396 . 396 . 397 . 398 . 399 . 400 . 400 . 400 . 401 . 403 . 443 . 4Q3 . 404 . 404 . 404 . 405 . 405 . 405ROSENBER~ (A.j. Comparative Experiments with Alkalidbuminate. Acid-albumin. and Albumin . . . . . . . . . .LIDOFF . Solubility of FibroYn . . . . . . . . .JADEEHOLM (A.). Study of Metahsemoglobin . . . . . .CHECHOUEOFF (M.1. Separation of Butylenes . . . . . .SABANEIEFF (A.). Diallyl . . . . . . . . . .PERKIN (W . H., jun.). Trimethylene Iodide . . . . . .STEIN (S . v.). Method of obtaining Haemoglobin Crystals . . . .WILKES (J . F.). Decomposition of Potassium Cyanide . . . .~ T A E D (A.) and G- . BSMONT . Green Ferrocyanides or Glaucoferrocyanides .RADZISZEWSKI (B.). Oxidations by Hydrogen Peroxide .. . .NORTON (L: M.) and C . 0 . PEESCOTT . Continuous Etherification . .LOPATKIN (M.). Action of Ally1 Iodide and Zinc on Epichlorhydrin . .NATTEREB (K.). Action of Zinc Ethyl on a-y-Dichlorocrotonaldehyde .GERLACH (4% . T . ) . Specific Gravity. Boiling Point. and Vapour-tension ofKONONOWITZ (N.). Isopropylallyldimethylcarbinol . . . . .BOWHARDAT (G.). Glycol and Glycolmonochlorhydrin . . . .Aqueous Glycerol . . . . . . . . . . .WILEY (H . W.). Maple Sugar . . . . . . . . .BBCEAMP (A.). Optical Inactivity of Cellulose . . . . . . BRASSE (L.).LEVALLOIS (A.).Action of the Diastase of Malt on Crude Starch . . .Rotatory Power of Solutions of cellulose in Schweizer's8olution . . . . . . . . . . . . . . . . . . .44354%40640749549549549549649649649749749749849949949950050xxiv CONTENTS .BAUER @ .W.). Sugar from Agar-Agar . . . . . . .MULLER (A.). Extraction of Amines from Commercial Methylamine . .ANTRICK (0.). Compounds of Diacetonamine with Aldehydes . . .POSSEK (W.). Hydroxyphosphinic Acids . . . . . . .PRATESI (L.). Formation of Oxymethylene from Ethyl Nitrate . . .CHANCEL (G.). Isomeric Ketones . . . . . . . .PAAL (C.). Acetonyla.cetone . . . . . . . . .KLEEMANN (S.). Method of preparing Diacetyl Cyanide . . . .BECKVRTS (H.) and R . OTTO . Action of Heat and Water on the Halogen-substituted Acids of the C,H2n0 2.series . . . . . . .MABERY (C . F.) and H . H . NICHOLSON . P-Dibromo-dichloropropionic Acidand P-Bromodichloracrjlic Acid .. . . . . . .MABERY (C . I?.). P-Bromotetrachloropropionic Acid . . . . .CHITTENDEN (R . H.) and H . E . SMITH . Palmitic Acid m d the Palmitins .SCHWEIZEB (A.). Arachidic Acid and Nondecjlic Acid . . . .BUISINE (A.). Constituents of Wool Grease . . . . . .BECPURTS (H.) and R . OTTO . .MABERY (C . F.) and R . LLOYD . .SHATZKY (E.). Diallyloxalic Acid . . . . . . . .SCHONE (H.). Chlorocarbonylsulphamyl . . . . . . .SHATZEY (E.). Preparation of Ethglic Oxalate . . . . . .JUST (F.). Method for Introducing Nitrogenous Radicles into Ethyl MaIo-nate . . . . . . . . . . . . .~CHEXPS (E.). Hydroxymaleic and Hydroxycitraconic Acids . . .BAUYANN (E.). Deriyatives of Pyruvic Acid . . . . . .PERKIN (W . H., jun.). Dehydracetic Acid .. . . . . .MEYER (V.). Syntheses of Thiophen . . . . . . . .PAAL (C.). Synthesis of Tbiophen and Pyrolline-derivatives . . .JACOBSEN (0.). Formation of Hydrocarbons by the Reversal of Friedel andCraft’s Reaction . . . . . . . . . . .ESSNER (J . C.) and E . GOSSIN . Action of Amy1 Chlorides and Amylene onTduene . . . . . . . . . . . . .ELBS (K.) and 0 . WITTICH . Action of Chloropicrin and Chloroform onToluene . . . . . . . . . . . . .METJNIER (J.). Benzene B-Hexachloride . . . . . . .SCHRAMM (J.) . Influence of Sunlight on the Bromination of Aromatic Com-pounds . . . . . . . . . . . . .WEBER (A.] and A . N . WOLFF . Perchlorophenol from Perchlorobenzene .WILLGERODT (C.). Paranitrophenyl Mercaptan and Paranitrophenyl Disul-pbide .. . . . . . . . . . . .WILLQERODT (C.). a-Dinitrophenyl Thiobenzoate and the Ethers of Dinitro-phenyl Mercaptan . . . . . . . . . . .BARTH (J.) and I; . SCHPEDER . Substances Formed by the Fusion of Quinolwith Soda . . . . . . . . . . . .MICHAEL (A.). The Gliicoside-group . . . . . . . .LOSANSITCH (5 . M.) . Direct Replacement of the Amido-group in AromaticAmines by Halogens . . . . . . . . . .T H ~ L (A.). Symmetrical Metaxylidine and Symmetrical Xylenol . . .HALLER (S.). Pseudocumidine . . . . . . . . .BERAN ( A.) . Paramidoctylbenzene, Paramidocaprylbenzene, and Amidoctyl-toluene . . . . . . . . . . . . .SMITH (E . G.). Action of Bromine on Propenylphenylenediamine . .BARZILOVSKY (J.). Oxidation of Aromatic Amines . . . . .REMSEN (I.). Action of Alcohol on Diazo-compounds .. . . .GASIOROWSEI (K.). and A . WATSS . Diazo-compounds . . . .BRUNNER (H.) and W . ROBERT . Colouring Matters from Phenols . .WESELSEY (P.) and R . BENEDIPT . Resorcinol Dyes . . . . .MICHAEL (A.) and 8 . M . PALMER . Conversion of Organic Isoeganates intoThiocarbimides . . . . . . . . . . ,Monohalogen-derivatives of Acrylic Acida- and P-Chlorodibromacrylic Acids .JACOBSEN (0.). Bromosubstitution-derivatives of Metaxylene . . .PAQE50050150250450450550550550650750850850850950951051151251251351351351551551651651751751851851851951961952052152152252252352452552552552552652CONTENTS . SYVMICHAELIS (A.) and U .PABTOW . Benzylarsines . . . . . .GOERINC~ (0 . F.). Action of Aldehyde on Paranitrobenzaldehyde . .ELBERS (A.) . Compounds of Benzaldehyde with Aniline Hydrochloride andStannic Chloride . . . . . . . . . . .ERDMANN (H.) . .TRINIUS (P.). Derivatives of Hydratropic Acid . Artificial Formation ofPhloretic Acid . . . . . . . . . . .BALBIANO (L.). Derivatires of Bromanisic Acid . . . . . .EOSTANECEI (5 . v.) and S . NIEMENTOWSPI . Synthesis of NitrococcusicAcid . . . . . . . . . . . . .HILL (H . B.) and E . E . STEVENS . . . .WISLICENUS (W.). Action of Potassium Cyanide on Phthalide . . .SCHERES (E.). Hydrindonaphthenecarboxylic Acid . . . . .PELLIZZARI (G.) . Amidobenzoic Acid Derivatives of Succinic, Sebacic, andPhthalic Acids .. . . . . . . . . .ELBERS (A.). Compounds of Hydrazines with Ketonic and AldehydicAcids . . . . . . . . . . . . .NIETZKI (R.) and T . BENCKISER . Orthonitranilineadphonic Acid ; NewOTTO (R.). New Synthesis of Aromatic Sulphones . . . . .MICHAEL (A.) and Gt . M . PALMER . Action of Sodium Phenylsulpliinate onMethylene Iodide . . . . . . . . . . .OTTO (R.). Formation of Sulphonea from Alkykilphonated Acids of theSeries C,Hz, O2 . . . . . . . . . . .OTTO (R.) and H . DAMEOHLEE Disulphones . . . . . .MABERY (C . F.) and G . H . PALMER . .CURATOLO (T.). Phenylcoumarinsulphonic Acids . . . . . .REMSEN (I.). .FISCHER (E.) and J . TAFEL . . . .DTJISBERG (C.) . Formation of P~ratolylparamethylimesatin from Dichlor-acetic Acid and Paratoluidine .. . . . . . .FITTIGF (R.) and H . ERDMANN . Synthesis of a-Naphthol . . . .HOFFMANN (0.). Nitrosonaphthol and its Derivatives . . . .NIETZKI (R.) and 0 . GOLL . Azonaplithalene . . . . . .MABGFARY (L.). Derivatives of a- and /?-Naphtholazobenzene . . .BERNTHSEN (A.) and A . SEMPER . Juglone . . . . . . .EESTRAND (A . E.). Mononitro-a-naphthoic Acids . . . . .ELLIOTT (A . H.). Anthracene from Water-gas Tar . . . . .WALLACH (0.). Terpenee and Ethereal Oils . . . . . .GTJIGFNET (E.). Chlorophyll and its Compounds . . . . . .EIJKNANN (J . I!.). Active Constituents of Skimmia Japonica . . .BENEDIKT (R.) and C . HAZTJRA . Morin . . . . . . .KNORR (L.). Action of Ethylic Diacetosuccinate on Ammonia and PrimaryAmines . . . . . . . . . . .. .KNORR (L.) and A . BLANK . Action of Ethylic Benzoylacetate on Phenyl-hydrazine . . . . . . . . . . . .WEIDEL (H.) and B . PICE . Compounds from Animal Tar . . . .LADEXBURG (A.) and C . F . ROTH . . . . .PECHMANN (H . v.) . Constitution of Pyridine-derivatives derired fromCoumalinic Acid . . . . . . . . . . .BEREND (L.). Trimethylquinoline . . . . . . . .BERNTHSEN (A.) and W . HESS . Quinolineammonium Bases . . .MOHLATJ (R.). Diphenylpseudoamphiphenacylizitrile . . . . .OE STERMAY E R (F, . ) . Diquinolines . . . . . . . .CLAUS (A.) and T . MUCHALL . Quinojinecarboxylic Acid . . . .Action of Sulphuric Acid on the Phenylcrotonic AcidsPETTIGREW (H . P.). Oil of Gaultheria . . . . . . .Phmoxymucobromic AcidMet hod of Preparing Orthonitraniline .. . . . . .Orthiodotoluenesulphonic Acid .New Class of Compounds Analogous to the Phthale'ins .STOKES (H . N.). Phthalic Sulphinide . . . . . . . .ANTRICK (0.). Benzylindole . . . . . . . . . Hydrazines of Cinnamic AcidBAMBERGER (E.). Retene . . . . . . . . . .TANBET (C.). Vincetoxin . . . . . . . . . .Commercial PicolinePAGE526527528528528529530531531532533533534535535536536537538539539539544)54354354554554554654654854954955055155255355355455555655755855855856056056xxvi CONTENTS .UENTIL (C.), p-Naphthoquinolinesulphonic Acid . . . .WEIDEL (H.) and K . HAZURA . .PAUL (.B . H.) and A . J . COWNLEY . New Aikalo'i& of Cuprea Bark .CONINCK (0 .DE) . Brucine . . . . . . . . . .HANSSEN (A.). Brucine . . . . . . . . . .LADENBURG (A.). Derivatives of Dimethylpiperidine . . . . .MERCK (E.), Coca'ine . . . . . . . . . . .NAYLOB (W . A . H.). Hymenodictyonine . . . . . . .EIJKMAN (J . F.). Active Constituents of Nalzdina Domestics . . .KOSSEL (A.). New Base occurring in the Animal Organism . . .BOCKLISCH (0.). Ptoma'ines from Fish . . . . . . .SHALFEIEF (M.). Preparation of Haemin . . . . . . .LAGORIO (A) . Crystallographic Form of Haemin . . . . .RUNEBERG (J . W.). Filtration of Albumin Solutions . . . . .SSLEOWSKI (E . and H.). Putrefaction of Albumin ard Formation of Skatoleand Indole . . . . . . . . . . . .SALEOWSKI (E . and H.). Skatolecarboxylic Acid. . . . . .CHECHOUKOFF .Action of Chlorine on Butylenes . . . . . .FAVORSKY . Condensation of Crotonylenes . . . . . . .ILOTJPOTSKY . Action of Chlorine on Tetramethylethylene . . . .GOSSIN (E.). Action of Sulphuric Acid on Cyanogen Iodide . . .RIESS (C.) and E . T . MEYER . Cyanmethethine . . . . . .HENRY (L.). Pyrotartaronitrile and Succinonitrile . . . . .CHANCEL (Gt.). Characteristic Reaction of Secondary Alcohols . . .LWOFF and CH~CHOUKOFF . Action of Hydrochloric Acid on IsopropenylCarbinol . . . . . . . . . . . . .KABLOUEOFF . Gi-lycide of Hexylic Glycerol . . . . . . .KENT (W . H.) and B . TOLLENS . . . .EOLOTOFF . Action of Amines on Methaldehyde . . . . . .DE FORCRAND . Glyoxal-ammonium Hydrogen Sulphite . . . .CLERMONT (I? . DE) and P .CHAUTARD . . . . . .WILLOEBODT (C.) and A. MULLER . Acetonechloroform, Acetonebromo-form, and Acetoneiodoform . . . . . . . . .RAMMBLSBERG (C.). Double Uranium Acetates . . . . . .SCHNEEOANS (A.). Perkin's Reaction in the Paraffin Series . . .MELIKOFF . Homologues of Glycidic Acid . . . . . . .NEUGEBAUER (Ed L.) . Ethylic y-Hydroxyvalerate and y-Hydroxpler-arnide . . . . . . . . . . . . .KATJDEB (E.). Action of Phosphoric Chloride on Succinyl Compounds, andon Tartaric Acid . . . . . . . . . . .RODER.(F.). Vinaconic Acid . . . . . . . . .FITTIG (R.). Constitution of Vinaconic Acid . . . . . .CAVAZZI (A) . New Compounds of Bismuth . . . . . .WIEDERHOLD (B%) . Levonic Acid . . . . . . . .FRIEDEL (C.) and J . M . CRAFTS . Decomposing Action of AluminiumHydro-compounds of Cinchonic Acid ..HOFMANN (A . W.). The Conine-group . . . .Milk-sugar and GalactoseIodacetoneSAVARY (W.). Atripaic Acid . . . . . . . . .Chloride on Hydrocarbons . . . . . . . . .COLSON (A.). Xylenes . . . . . . . . . .ERRERA (G.). Action of Chlorine on Cymene . . . . . .GUYPERT (F.). Phenyl Cyanate . . . . . . . . . ALLEN (W.) and .A . K~LLIKER .LOBRY DE BRUYN (C . A.).LOBBY DE BBUYN (C . A.).Derivatives of Triphenylcarbinyl Bromide .Action of PotasEium Cyanide on Metadinitro-benzene . . . . . . . . . . . . .Replacement of the NO2 group by an Oxy-dkyl( ~ I I I ' " 'LOBRY DE BRUYN (C . A.). Action of Potassium Cyanide on OrtLo- andPara-dinitrobenzene . . . . . . . . . . . .MARTINON . Action of Hydrogen Peroxide on the Phenols .. . .WERNER (E.), Bromoxytribromophenol b . . . . . .PAGEbtjl5615625635645655655655655655665665665676676675696456456456456466466466476476476476486486M64864965065165165365365365365365465465565565865665765865B~~TTCHER (W.). Migrations in Benzene Ortho-di-derivatives . . .POLEK and LUSTI~ . Derivatires of Carvacrol . . . . . .VAX ROMBURGH (P.). Non-existence of Pentanitrodimethylaniline . .BERJTJ ((3.). Derivatives of Amidoazobenzene . . . . . .GOLOUBEFP . Reduction of Isodinitrobenzene . . . . . .WEDDIGE (A.). Derivatives of Orthamidobenzamide . . . . .WITTENBERG . Azophenylacebic Acid . . . . . . . .HERZBERO (M.) .Cinnamic and Bydrocinnamic Acid : Paranitrobenzalde-hyde . . . . . . . . . . . . .ERDMANN (H.). Nitration in the Side-chains in Aromatic Compounds .SLOCTJM (F . L.). Phenylangelic, Phenylmethacrylic, and EthylphenyllacticAcids . . . . . . . . . . . . .OTT (P.) . Phenylhydroxypivalic Acid . . . . . . .FITTIO (R.). Perkin’s Reaction . . . . . . . .LUDWIG (R.). Hydroxybenzaldehyde and Ooumaric Acid . . . .WEINSTEIN (L.). a- and P-Hydropiyeric Acids . . . . . .WILLBERODT (C. ) and P . MOHL . Unsvmmetrical Metadinitrobenzene Sd-phonic Acid . . . . . .. . . . . . .EOLBE (H.). Chemical Constitution of Isatin . . . . .MEYEB (E . v.). Isatoic Acid . . . . . . . .PAXA~-TOVIG (W.). Paramethylisatoic Acid . . . . .SCHULZE (9 . E.). Phenols of High Boding Point oontaiined in Coal-tarMILLER .a-Naphhquinone . . . . . . . .TERRISSE . Naphtholfluorescein and Naphtholeosin . . . .LE NOBEL ((3.). A New Terpene . . . . . . . .CAZENEUVE (P.). Monochlorobromommphor . . . . .WARINQER (L.). Camphanic Acid . . . . . . .BUTLEROW (A.) and B . RIZZA . Asarone . . . . . .POLECK and SAMELSON . Jalapin . . + . . . . .SACHSSE (E.). A New Colouring Matter from Chlorophyll . . .ABNAUD (M.). Colouring Matter s f Leaves . . . . . .CONINCK ( 0 . DE) . a.Picoline, ylutidine, and Pyridine . . .CONINCK (0 . DE) . Homonicotic Acid . . . . . . .OSTEBMAYER (E.). Action of Phosgene Gas on Quinoline . . .BEYER (C.). A Homologue of Quinoline . . . . . .OSTERNAYER (E.1. .SACHSSE (R.). Chlorophyll . . .. . . . .OSTERMAYER (E.). Methochlorides of the Quinolim Series . . .Action of Iodine Chloride on Q.uinolines, &c .OSTERMAYER (E.). Iodated Azo-colouring Matters- . . . . .HOOGISWERFF (8.) and W . A . VAN DORP . Colouring Matters fromLepidine . . . . . . . . . . . .ERUCKENBERB (C.) and H . WAGNER . Carnine . . . . . .HCHILLINO (E.). Caffei’ne Methylhydroxide . . . . . .BECKUBTS (H.). Strvchnine . . . . . . . . .BAUMERT ((3.). Behaviour of Lupinidine with Ethyl Iodide . . .HABERMANN (J.). Fagine . . . . . . . . . .GAUTIER (A) . Leucomai‘nes . . . . . . . . .MAAS (H.), BUCHMANN, and WASMUND . Putrefaction Alkalolds in BoiledM-eat . . . . . . . . . . . . .MIHALLOFF . Animal Colouring Matters . . . . . . .HAMMARSTEN (0.). The Mucin Group .. . . . . .LEBEDEFF . Reduction of Cetyl Todide . . . . . . . .HENRY (L.). Trimethylene Iodide . . . . . . . .KONDAEOFF (T.). Action of Chlorine on Trimethylethylene . . .FATORSKY (A.) . Isomerism of Acetylene Hydrocarbons . . . .CHRISTENSEN (0 . T.). Chromium and Manganese Compounds analogous toFerro- and Ferri-cyanides . . . . . . . . .MOISSAN (H.) . ;Potassium Chromocvanide . . . . . . . .H ESSE (0.). Dicinchonicine . . . . . . . . . .POWER (F . B.). Hyhrastine . . . . . . . . .PAGE6586596606606606616616616626626636636636646656656666666676676676686686686696696706706706716716726726726726’13673674674675675675676676676676676677736736736736737738GONTEKTS .xxriiY . . . . . . . xxviii CONTENTS .JENSEN (H . 0.). Formation of Nitroprussides without the Use of NitricAcid . . . . . . . . . . . . .WEDDIGE (A.) and M . KORNEE . Polynieric Dickrloracetonitriles . . .TRAUBE (J.). Preparation of Cyanamide . . . . . . .BEILSTEIN (F.) and E . WIEGAND . Unsaturated Compounb of the FattySeries . . . .SOLONINA (V.). Action'of Dilute 'Bcids' on b y 1 h c o i o l . . . .PRZYBYTEE (S.). Didlyl Dioxide . . . . . . . .NEMIROWSKY (J.). Action of Caybony1 Chloride on Glycol CMorhydrin .HAY (M.) and 0 . MASSON . Composition of Nitiroglycerol . . . .HAY (M.). Chemistry of Nitroglycerol .. . . . . . .SNOLKA (A.). Mannitol Lead Nitrate . . . . . . . .FAUCONNIER (A.). Reduction of Mannitol .. . . . .ALEEHINE (A.). Anhydrides of Mannitol . . . . . . .SCHEIBLER (C.). Nomenclature of Sugar& . . . . . . .EILIANI (H.). Isoswcliarin . . . . . . . . . .EILIANI (H.). Metasaccharin . . . . . . . . .CONRAD (M.) and M . GUTHZEIT . Demmposition of Sugar when Heatedwifh Dilute Acids . . . . . . . . . . .TBOOST (L.). Remarks on some Criticisms of Friedel's concerning ChloralHydrate . . . . . . . . . . . . .FBIEDEL . Reply to Remarks by Troost concerning Chloral Hydrate . .CANZONERI (F.) and G . SPICA . Reaction of Acetone with Amides of theAcetic Series . . . . . . . . . . .MICHAELIS (A.). Acetone Phoaphorslls Compounds . .. . . .BAUNANN (E.). Compound8 of Mercaptans with Uehydes, Kebnes, andKetonic Acids . . . . . . . . .. .DUVILLIER (E.). Diethyl-amido-a-butSric Acid . . . . . .CANZONERI (F.) and G . SP~CA . Ethyl Acetyl-B-imidobutyrate . . .KUCKERT (0.). Action of . Alkylamines on Ethyl Acetoacetate . . .CANZONERI (F.) and CX . S ~ C A . .PINNER (A.) . .FIELINSPY (N.) . Additive Products of Methylamine and /3-MethylglycidicAcid . . . . . . . . . . . .ARISTOPF (V.). Oxidation of Acids of the Lactic Series . . . .BOTTIBGER (C.). Preparation of Thiolactic Acid . . . . .BIRNIE (S.), Decomposition of FeTrous Oxalate . . . . . .OTTO (R.) and H . BECPURTS . Pyrocinchonic and Bchloradipic Acids froma-Dichloropropionic Acid . . . . . . . . .HELL (C.) and R . REXPEL . Derivatives OB NormaJ Suberic Acid . .HEMPEL . Derivatives of Snberic Acid . . . . . . . .HELL (C.) and G .SCHULE . Normal Pentyimalonic Acid . . . .HOMOLKA (B.) . Condensation-products of a-Ketonic Acids . . . .PINNER (A.). Preparation of Tartronic Aeid . . . . . .SCHULZE (E.) and E . BOSSHARD . Occurrence sf Glutamine in the SugarBeet . . . . . . . . . . . .SCHULZE (E.) and E . BOSSHARD . Optical Behviour of some Amido-acids .BAEYER (A.) . Polyacetylene Compounds . . . . . .SCEIFF (H.) Oxaldiamidopropionic Acid . . . . . . .PONOMAREPF (J.). Synthesis of Allantoxanic Acid from Parabanic Acid .HA IT INGE R (L . ) . D eh y drace tic Acid . . . . . . . .PERKIN (W . H.), jun. Action of Aniline on Methyl Dehydracetate . .HAITLNGIER (L.). Remarks on Perkin's Note em the Action of Aniline onMathyl Dehydracetate . . . . . . . . . .MEYER (V.).Constitution of Thiophen Compounds . . * . .Action of Amides on Ethyl AcetoacetateAction of Ethyl Acetoacetate on Amidines : PyrimidinesERLENMEYER (E.). Formation of Pyrotarbaric Acid . . . . .REICHER (L . T.). Rate of Formation of Maleic Anhydride . . . .BOTTINGER (C.). Condensation-product:ts ef Pyruwic Acid . . . .HILL (H . B.) and Gt . T . HARTSHORN .VOLHARD (J.) and H ..EBDXAN N. Synthesis of Thiophen . . . .Furfumne-derivatives . . .PAQE73973973974074174174174274274374374474474474574574674674674774875075075175175175275275275275375375575675775775575875975975975976076076176176276276376COXTENTS . XSiXSCRULZE (K . E.). Method of obtaining Thiophen and its HomologuesPAAO (C.) and J .TAPEL ..Thiophen from Mucic Acid . . . . . PAAI, (C.) and J . TAFEL . Thiophen from ErythriteSTADEEX (0.). Nitrothiophens . . . . . . . . .PETER (A.). @-Acetothienone and its Derivatives . . . . .PETER (A.) . Isomeric Thiaphenic Acids . . . . . . .LANGER (J.) Isomeric Thiophensdphonic Acids . . . . .E ~ L I (K) . Isomeric Thiotolens . . . . . . . . .BONZ (R.). Derivat. ives of B-Ethylthiophen . . . . . . .MESSINGER (J.). Thioxylen from Coal-tar . . . . . . .Aromatic Compounds . . . . . . . . . .. . . . .ScHRax&c (J.) Influence of Light on the Aetion of the Halogens onANSCHWTZ (R.) and E . ROMIG . Action of Aluminium Chloride on Mixturesof Ethylidene Chloride with Benzene, Toluene, or Metaxylene ..ANWHUTZ (R.) and H . IMMENDORFF . Preparation of Homologues ofBenzene by Aid of Aluminium Chloride . . . . . .SEELIG (E.) . Trichlorotoluenes . . . . . . . . .PELLIZZARI ((3.). Reduction of Nitrobenzyl Chloride . . . . .ERRERA ((3.). n-Phenylpropylene and a-Paratolylpropylene . . .LEUCKART (R.). Reactions of Aromatic Cyanates . . . . .ZIE~MEEMANN (J.) and A . MULLER . Paranitrobenzylidene Chloride . .EDLER (E) . 1, 3, 4, 5 Nitropseudocumene, Pseudscumidine, and Pseudo-cumenol . . . . . . . . . . . . .GASIOROWSKI (K.) and V . NERZ . .TESSMER (H.). Compounds of Polyhydric Alcohols with Phenyl Cyanate .HOPMANN (A . W.). Conversion of Phenyl Cyanate into Phenyl Cyanurate .LINDNER (J) . Bromnitrophenols and their Amido-derivatives .. .Nitriles from Aromatic FomamidesGOLDBOHMIDT (H.) andH . SCHMID . Nitrosophenols . . . . .E RRE EA ((3.). E t h ylphen ol . . . . . . . . . .FIrJETI (M.). Cumyl Ether . . . . . . . . . .BRUNNER (H.). Azoresorcinol and Azoresorufin . . . . . .ANSCH~~TZ (R.). Pipitzahoic Acid . . . . . . . .ANSCHUTZ (R.) and W . LEATHER . Derivatives of Pipitzahoic Acid . .MYLIUS (F.). Pipitzahoic Acid or Perezone . . . . . .CEIASANOWITZ (L.) and C . HELL . Action of Bromine on Eugenol . .NIETZEI (R.) and T . BENCKISER . Hexshydroxybenzene-derivatives mdtheir Relations to Croconic and Rhodizonic Acids . . . . .OLIPERI (V.). Action of Nitrous Anhydride on Parabrommiline Nitrate .WITT (0 . N.). Nitroso-derivatives of Aromatic Amines . . . .PRATESI (L.).Action of Porrrialdehyde on Aniline . . . . .PIUTTI (A.). Derivatives of Diphenylaminephthalek . . . . .NUTH (GI.). Action of Paramidodimethylaniline on Aldehydes . . .BZADIN (J . A.). Cyanogen Compounds of the Aromatic Diamines . .LEYMANN (H.). Action of p-Chlorethylene Sulphonic Chloride on Aniline’.ZINCKE (T.). Action of the Amines on Quinones . . . . . .JANOVSKY (J . V.). Reduction of Nitroazo-compounds and AzonitrolicAcids . . . . . . . . . . . . .TIEMANN (F.) and P . RRUGER . Relation8 of Benzenylamidoxime-deriva-PIUTTI (A.). Diphenylamine-derivatives of Succinic Acid . . . .HEss (0.). Benzoyl-derivatives of Aromatic Amines . . . . .ECKENROTB (H.). Mixed Observations . . . . . . .GRIESO (P.). Diazo-compounds . . . . . . .. .tives to the Benzhydroxamic Group . . . . . . .HOFNANN (A . W.) . Crystallised Methyl-violet . . . . . .EINEELIN (F.). Preparation of Metanitrocinnamaldehyde . . . .GOHRING (C . F.). Action of Aldehyde on Metanitrobenzaldehyde . .SCHULZE (K . 1.). Occurrence of Benzoic Acid in Coal-tar Oils . . .HENTSCREL (W.) . Conversion of Ethyl Carbanilate into Amidobenzoic AcidPAGE763763764764764765765766766767767768769769770771171772772773774774774775775’77677677677777777977978178278278278378378478478678678778878979079179179151925’92LA COSTE (W.j and J . BODE WIG . . MethylformylorthamidochlorobenzoicAcid and Methylpseudochlorisatin . . . . . . . . 79xss CONTENTS.WELTNER (A.). Action of Phenylbromacetic Acid on Ethyl Acetate .ALEXCRFF (P.).Action of Light on Nitrocumic Acid . . . .PEREIN (W. H.), jun., and G. BELLENOT.SCHIFF (H.) and E. PONS. An Amide b Gallic Acid . . , .PIUTTI (A.). Phthaljlaspartic Acid . . . , . . ,GRAERE (C.) and H. SCEINALZJGATJU. Diplithalyi . . , .SCHREDER (J.). The Constitution of Isuvitic Acid . - , ,ESCALES (R.) . Action of Phenylhydrazine on Sulphinie Acids , .EULI (K.). Dry Distillation of Ammoninm Benzenesulphonate . ,Low (W.). Indiaocarboxylic Acid . . . . . . .Paranitrobenzoglacetic AcidSCHIFF (H.). Phosphorsellinic Acid L . . .ROSER (W.). Phthalgl-derivatives . . . C . .ANSCHUTZ (R.) aid C. R~MIU.MAZZARA (G.). Action of Potassium Nitrite and Phenols on Diamidotri-phen ylmethane .. . . . , . . . . .HESS (W.) and A. BEENTHSEN. Amido- and Hyboxy-derivatives of Phenyl-acridine . . , . . . . . , . . . .HEWRIQTJIW (B.) and M. ILINSKI. Preparation of bhe Nitrosonaphthols .LIEBERMANN (C.). . Behaviour of a-Naphthaquinone and Benaoquinonetowards Sulphuric Acid , . . . . . . . , ,LAWSON (T. A.). Action of Diazo-compounds or P-Naphthylamine . .MYLIUS (F.) . Hydroxyjuglone . . . . . . , , .XOHLER (H.). Formation of Anthracene . . . . . . ,BRUNNER (H.) and E. CEUARD. P-Amidoalizarin . . . . .CAZENEWE (P.) An Isomeric Chlorobromocamphor . . . . .BAMREWER (E.). Coloar Reactions of Orthodiketones , . . .KACHLXR (J.) and F. V. SPITZEB. Camphoroaic Acid. . . . .DOBBIE (J. J.) and G. G. HENDERSON.Red Resin from Draccama Cin-lzabari . . . . . . . . . . . . .FRIDOLIN (A.). Tannin from Vaiious Plants . . . . . ,PLENUE (H. C.). Aloitn . . . . . . , . , .CIAMICIAN CG.) and P. SILBER. Acetylpyrroline . . . . . .CIAMICIAN (G.) and P. MAGXAQHI. Action of Carbonyl Chloride onPatassium Pyrroline . . . . . . . . . .CIAMICIAN (G.) and P. MAGNAUHI. Action Qf Nascent Hydrogen onMethylp y rroline . . . . . . . . ,CIAMICIAN ((3.) and P. SILBEB. Action of Nitric Acid on Pyxryl MethyiKetone . . . . . . . . . . . , .CIAMICIAN (G.) and P, SILBER. Pyrrylmethylketonesulphinic Aoid . .KNORR (L.) and A. BLANK. Action of Ethylic Acetoacetate on Yhenylhy-drazine . . , . . . . . . . . . .CIAMICIAN (G.) and €!. SILBER. Monobrornopyridine . . . . .HAITINGER (L.) and A.LIEBEN. Nitrogenous Derivatives of ChelidonioAcids . . . . , . . . . . . .HBSEKIEL (A.). New Methylpiperidine : P-Pieoline Hexahydride . .VOIUT (R ). PPyridinetricarboxylic Acid . . . . . . .OSTERMAYEB (E.). Methochlorides of Pyridine and Quinoline Bases . ,CLATJS (A.). Alkylquinoline-deriratives . . . . . . .BEBNTHSEN (A.). Ammonium Rases derived from Quinoline . . .LA COSTE (W.) . Quinoline Iodides . , . . . . .EPSTEIN (W.) Synthetical Lutidine . . . . . . . .LADENBURG (A.) and C. F. BOTH. . DURKOPF (C.) . Reduction and Oxidation-products of Aldehydecollidine .HALLER (S.). Trimethylquinizine-derivatives , . . . . .KONINCK (0. DE). Reactions of Alkaloi'ds . . . . , . .DUVILLIER (E.). Creatines and Creatinines. . , . ..HANSSEN (A.). Brucine . . . . . . . . . .HARTZ (J. D. A.). .FISCHER (0.) and E. TAUBER. Harmine and Harmaline , . . .EOBERF (R-). Constituents of Ergot of Rye , , . . . .Nitration-products of DiphenyletlianeIsolation of the so-termed a-LutidinePreparation of Daturine from Stralnonium Seeds .8008008018028328038068068068078078088088088088098098108108108118118128128138148148148158158178 1881 8819819820820821PAGE . 793 . 794 . 794 . 795 . 796 . 796797 . 797 . 798 . 798 . 799 . 799 . 80CONTENTS . xxxiTANRET ((2.). Cornutine and Ergotinine . . . . . . .EMICH (F.). Behaviour of the Bile Acids with Gelatin and Gelatin Pep-tones . . . . . . . . . . . . .MAUTHNER (J.).Cystine . . . . . . . . . .SZYMANSKI (F.). Malt Feptone . . . . . . . . .AMTHOR (C.). Nucle’in of Grape Stones . . . . . . .LOEW (0.). Albumin and its Oxidation . . . . . . .MALY (R.). Oxidation of Albumin . . . . . . . .ZALESRI (S.). New Reaction of Carbonic Oxide-hemoglobin . . .HOPPE-SEYLER (F. ) . Decomposition-products of the Colouring Matters ofthe Blood . . . . . . . . .KRTJKENBERG (C . F . W.) . Conchiolin . . . . . . .JACQUEXIN (Gt.) . Preparation of Cyanogen Gas . . . . . .NRNCEI (M.) and N . SIEBER . Colouring Matter of the Blood . . .HHNRY (L.). Volatility of Cyano-derivaiives containing Oxygen . . .SAYTZEFF (A.). Synthesis of Tertiary Alcohols from Ketones . . .REFORMATSKY (S.). Preparation of Polyhydric Alcohols . . . .OSTWALD (W.).Inversion of Cane-sugar . . . . . . .HENRY (L.). Primary HaloYd Derivatives of Ethyl Ether . . . .CANZONERI (F.) and B . SPICA . Products of Reduction of Dehydrotri-aceton amine . . . . . . . . . . . .HENTSCHEL (W.). Preparation of Methyl Chloroformate . . . .GROGER (M.). Oxidation of the Fattv Acids of Tallow . . . .CURTIUS (T.). Diazoacetic Acid : Diazoacetamide : Pseudodiszoacetarnde .BISCHOFF (C . A.) and C . RACH . Symmetrical Dimethglsuccinic Acid . . Derivatives of Diazosuccinic Arid . . .CURTIUS (T.). Formation of Ethyl Azinsuccinate from Ethyl Dizzoacetute .HENRY (L.). Anfides of the Oxalic Series . . . . . . .MEYER (V.). Thiotolen and Thiophen . . . . . . .LANGER (J.). Isomeric Thiophensulphonic Acids . . . . . .HENTSCHEL (W.).Phenyl Cyanate and Hydrogen Chloride . . .SCRRAXM (J.). Influence of Light on the BronLination af Aromatic Com-pounds . . . . . . . . . . . . .CLATJS (A.) and F . MANN . Ortho-ethyltoluene . . . . . .RADZISZEWSKI (B.) and P . WISPEK . Derivatives of the Xylenes . .DACCOMO (G.) . Trichloraphenol : Trichloronitro- and Amido-phenols :Tribromonitro- and Amido-phenols . . . . . . .GUARESCHI (J.) and GF . DACCOMO . Chloronitro- and Bromonitro-quinones .N~LTING (E.) and T . BAUMAN . Formation of Quinones . . . .HIRSCE (R.) . Paranitro-ort.hocreso1 and Toluquinoneclilorimide . . .Derivatives of Pseudocumidine . . .MAZZABA ((3.) and Gl . POSSETTO . . . .JANovSBY (J . W.) and L . ERB . Intermediate Reduction-products ofthe Nitroazo-compounds .. . . . . . . . .WICHELHAUS (H.). Crystalline Bases from Methyl-violet . . . .NOLTING (E.). Azylines . . . . . . . . . . .LOSSEN (W.). Structure of Hydroxylamine-derivatives . . . .TIEMANN (F.) . Amidoximes and Azoximea . . . . . . .TIEMANN (F.) and E . NAGELI . Action of Sodium Amalgam on AqueousSolutions of Benzenylamidoxime . . . . . . . .SC~OPF (M.). Metanitrobenzenylamidoxime . . . . . .SCHULZ (0.). Action of Acetic, Prapionic, and Butyric Acids, &C., onKNTJDSFN (P.) . Phenplethenylamidoxime . . . . . . .GROSS (F.). Phenylhydroxyethenylaulidoxime . . . . . .PL~~cHI; (J.) and L . WOLFRUM . Condensation of Balicylaldehyde withHippuric Acid . . . . . . . . . . .PLOCHL (J.) and W . Loi . n’itra- and Sulpho-derivatives of Phenylamido-acetic Acid .. , . . . . . . . .CUXTIUS (T.) and F . KOCH .NOLTING (E.) and T . BAUWAN .Azo-derivatives of ThpmolKEUGER (F.). Derivatives of Benzenylamidoxime . . . . .Benzenylarnidoxime . . . . . . . . . .PAQE821822822822823823824825825826828880880881882882882883883883.88388588588688688788788888888888988989189289289389389489589589589589589589689789789889889x xxii CONTENTS .SCHILLER-WECESLEE (M.). Anilidopyrotartaric Acid . . .SCACCHI (E.) . Crpstallogmphy of Phenylcoumarin and CoumarinAction of Plithalic Anhydride on Benzyl CyanideBIZZARRI (D . ) . Hydroxycoumarm . . . . . .GRAEBE (C.). P-Sulphophthalic Acid . . . . . .GABRIEL (S.).Benzenylidenephthalide . . . . .CLAUS (A.) and L . TONN . Cumenesulphonic Acid . . .MAZZARA (Gt.). Diamidotriphenylmethane . . . . .MAZZARA (G) . Azo-derivatives . . . . . . .BAMBERGER (E.) and S . C . HOOKER .WILL (W.). Narlngn . . . . . . . . .OLIVERI (V.) and A . DENARO . Quassin . . . . .BTJCHKA (K.) and A . ERCK . Brazilin . . . . . .GABRIEL (S.).EKSTRAND (A . G.). Mononitro-p-nsphthoic Acids . . .Retene . . . .CLATJS {A.) . Quinoline . . . . . . . . .HINSBERG (0.). Quinoxalines . . . . . . .BECKURTS (H.). Strychnine and Brucine . . . . . .MAXDELIN (K . F.). Aconitine . . . . . . I . .CLATJS (A.) and T . CRAMER .COMSTOCK (W . T.) and W . KONIGS . Cinchona bkalo'ids . . .Nitro- and Amido-derivatives of QuinolineCALMELS ((3.) and E .GOSSIN . Constitution of Cocai'ne . . .PAGE . 900 . 901 . 901 . 909 . 902 . 902 . 903 . 904, . 904 . 9n4r . 905 . 906 . 907 . 907908 . 908 . 909 . 910 . 911 . 911 . 912 . 913 COPPOU (F . j . Pt. omaynes . . . . . . . . .HAMMARSTEN (0.). The Sulphur of Casein . . . . . .SCHTJLZE (E.). Amido-acids formed from Albumin . . . . .KELLER (P.). Cyanmethine . . . . . . . . . .SCHWALBE (F.). Non-acid Constituents of Beeswax . . . . .Sugar . . . . . . . . . . . . .~OHANSSON (J . E.). Behaviour o€ Serum Albumin towards Acids andNeutral Salts . . . . . . . . . . . .BOQTJILLON (H.). Action of Chlorine on Isobutyl Alcohol . . . .HERRMAXN (P.) and B . TOLLENS . Reactions of Saccharin . . . .SCHEIBLER (C.). Separation of Raffinose from the Molasses of Beet-rootSIIFERT (R.). Formation of Amines from the Amidee of the Fatty Series .FRANCHIMONT (A .P . N.). Reduction of Nitrodimethylamine . . .MICHAEL (A.) and J . I? . WING . Additive Compound of Propionitrile andHydrogen Chloride . . . . . . . . . .LAXG (E.). Di-isobutylketine . . . . . . . . .LOBBY DE BRTJYN (C . A.). .ERDMAKN (H.) . Conversion of Lactonic Acids into Lactones . . .VRIES (H . DE) . Decomposition of Organic Acids under the Influence ofBRANCHIMORT (A . P . N.). Action of Nitric Acid on certain DibasicAcids . . . . . . . . . . . .Formation of Methyl Racemate from Methyl Dextro- andL8evo-tartrates . . . . . . . . . . .Propionic Acid and some of its DerivativesLight . . . . . . . . . . . .EAITINGER (L.) and A .LIEBEN . Cheklonic Acid . . . . .ANSCHUTZ (R.).KILIANI (H.) Trihydroxyadipic Acid . . . . . . . .KILIANI (H.). Galactonic Acid . . . . . . . . .VERWETJIL (A.).MICHAEL (A.) and J . F . WING .WTJRTZ and HENNINGER .FRANCHIMONT (A . P . N.).Simultaneous Action of Oxygen and Hydracids on Selenio-.Action of Ethyl Chlorocarbonate on PotassiumAction of Nitric Acid on Methylsulphonamides .. . . . . . . . . . . . carbamideAction of Methyliodide on AsparagineCyanate . . . . . . . . . . . . .MONARI (A.). New Sulphonic Acids . . . . . . . .PEIEBS (B.). Nitro-derivatives of Furfurane . . . . . .SCHIFF (R.) . Physical Properties of Thiophen . . . . . .MEYER (V.) and 0 . STADLER . Direct Preparation of Dibromthiophen fromCoal-tar Benzene .. . . . . . .STADLER (0.). Reduction of' Nitrb- to Amdo-thiophen . . . .91391491696196196296296296396396396396396396496496596696796796796896896997097197197197CONTENTS. xLOBBY DE BRUYN (C. A.). Identity of the two Ortho-positions in theBenzene Nucleus . . . . . . . . . . .WISPEK and ZUBER. Formation of Normal Propylbenzene . . .SILVA (R. D.). Formation of Normal Propylbenzene . . . . .CLAUS (A.) and H. KAUTZ. Chloro-derivatives of Orthoxylene . . .LELLMAYN (E.). Constitution of Dinitroparaxylenes . . . . .YOLIS (4.). Aromatic Silicon Compounds . . . . . . .NOLTING (E.) and E. WILD. Preparation of Mononitrophenols from theirPrimary Amines . . . . . . . . . . .LELLXANN (E.) and E. WURTHNEB.New Nitrotoluidine . . . .LIMPBICHT (H.). Nitrotoluidines . . . . . , . .GATTERYANN (L.). Derivatives of Metanitroparatoluidine . . . .BOESSNECK (P.). Condensation of Chloral Hydrate with Tertiary Amines .LELLYANU (E.). General Method for Determining the Constitution ofAromatic Diamines . . . . . . . . . . .LmLxANN (E.). New Toluylenediamine . . . . . . .LELLMANN (E.) and E. WUBTHNEP. Chemical Behaviour of Aromatic andPatty Diamines . . . . . . . . . . .NOLTING (E.) and E. WEINGARTNEE. Decomposition Products of Acet-anilide Hydrochloride . . . . . . . . . .KURN (B.). Action of Phenyl Isocyanate on Amido-compounds . . .GRAEBE ((2.). Phthalimidine . . . . . . . . .BLADIN (J. A.). Derivatives of Dicyanphenylhyd-azine . . . .TIEMANN (F.).GIucovanillim and Glucovanillyl Alcohol . . . .SANDNEYER (T.). Conversion of the Three Nitranilines into NitrobenzoicA c i d s . . . . . . . . . . . . .SANDYEPER (T.). Conversion of the ThrM Nitrobenzoic Acids into PhthalicAcids . . . . . . . . . . . . .BAUM (J.). Simple Method for preparing Hippuric Acid and Allied Cotu-FCHMITT (R.). Kilbe’s Synthesis of Salicylic Aeid . . ‘ . . .BEPEE (C.) Derivatives of Mandelic Acid . . . . . . .SEIFERT (R.). Action of Carbonic Anhydride on Sodium Bioetanilide : NewSynthesis of Dicaxboxylic Acids . . . . . . . .LIMPRICHT (H.). Oxidation of Amidobenzenesulphonic Acids . . ,LINPBICHT (H.) . Azobenzen,e-thiosulphonic and -sulphinic Acids . .R~ICHAEL (A.) and G. N. PALMER. Properhies of Phenylsulphonacetates .SPIEGEI, (A).New Class of Aromatic Sulphonic Acids . . . .JOURDAN (F.). New Synthesis of Derivatives of Hydroacridine and Acri-dine . . . - . . . . . . . . .FRIEDLANDER (P.) and A. WEINBERG. Carbostyril . . . . .KBLLIKER (A.). Derivatives of Triphenylcarbinyl Bromide . . .I i ~ o ~ s c n (R.). Benz-P-naphthylamide and /?-Dinaphthylamine . . ,’I’ANRET (C.). Terpinol . . . . . . . . . .JACKSON (C. L.). Reduation of Camphor to Borneo1 . . . . .HALLIBURTON (W.). Chitin . . . . . . . . .STOCKMAN (R.). Active Principle of Senna Leaves . . . . .REihKE (J.). Destruction of Chlorophyll Solutioil by Light . . ,LADEXBURQ (h.). Synthetical Yyridiue and Piperidine Bases . .CIAXICIAN (G.) and P. SILBER. Action of Nitric Acid on Pyrryl MethyiKetone .. . . . . . . . . . . .CrAmIcIm (G.) and P. SILBER. qywylene Dimethyl Diketone . . .I,ADEXBUBQ (A) and C. F. ROT=. New Lutidine . . . . .KNOBR (L.). Action of Ethyl Diacetosuccinate on Ammonia . . .KKORB (L.). Action of Ethyl Diacetosuccinate on Phenylhydrazine . .C‘LAUS ( I.) and E. HUETLIN. Yapaverine . . . . . . .(’LLUS (A,) and C. RITZFELD. Narceine . . . . . . .PAUL (B. H.) and A. J. COWNLEY. Cupreine and Homoquinine. . .MERCK (W.) . Benzoylecgonine . , , , . . . , .VOL. XLVIII. Cpounds . . . . . . . . . . . .SCHMIDT (E.) and E. SCHILLINQ. Caffeine , . . . . . .xxiiiPAGE9729729729729739739739749749759769769769279789199799799809819819819829829839849849869879879899909909.909919919919919929929939:!499499592559699699799xxxiv CONTENTS .VILLIEES .Curarine from Strychmos toxgera . . . . . .SZYMANSKI (F.). Hemialbumose from Vegetable Albumin . . . .SALEOWSKI (E.). Decomposition of Prote'ids by Permentat. ion . . .VILLIERS (A.). Nitro-derivatives of Ethylene . . . . . .LINNEMANN (E.). Oxidation of Propylene Oxide . . . . .HENRY (L.). Volatility of Chloronitriles . . . . . . .SANDMEYER (T.). Ethyl Hypochlorite . . . . . . . .LIEBERMANN (C.). The Wax and Fat of Cochineal . . . . .ZIKES (H.) . Butenylglycerjl Chlorhydrins . . . . . . .LE BEL (J . A.) and M . WASSERMANN . Reduction of Hexahydric Alcohols .SCHEIBLER (C.). Raffinose . . . . . . . . . .TANRET (C.). AlktrloYds produced by the Action of Ammonia on Glucose .COTTON (S.).Action of Oxidising Agents on Chloral Hydrate . . .SAYTZEFF (A.). Oxidation of Oleic Acid . . . . . . .ANSCHUTZ (R.) and C . HINTZE . Diammonium Chloride . . . .PERKIN (W . H., dun.). Trimethy1enedicarbox)lic Acid . . . .ANCHUTZ (R.) and F . KLINQEMANN . Preparation of Malic Acid from CitricAcid . . . . . . . . . . . . .HORBACZEWSKI (J.). Artificial Uric and Methyluric Acids . . . .MEYER (V.). The Thiophen-group . . . . . . . .ROSENBERG (J.). Tribromothiophen and Double Compounds of Dinitro-MESSINGER (J.). Thioxylen from Coal-tm . . . . . . .J ACOBSEN (0.). Monochlorometaxylene . . . . . . .KRUGER (A.). Monochloro-xylenes and their Oxidation-products . .SCHULTZ (R.), Oxidation-products of Solid Dibromo-paraxylene .. .SILVA (R . D.). Aromatic Hydrocarbons . . . . . . .KREYSLER (E.). Phosphates of the Phenols . . . . . .KREYSLER (E.). .HERTKORN (J.). Silicates of the Phenols . . . . . . .SEIFERT (R.). Action of Sodium Mercaptide on Phenyl Salts . . .GOLDSCHMIDT (H.) and R . ZURRER . Camoxime-derivatives . . .MEUNIER (J.). New Mode of Formation of Catechol . . . .CAZENEUVE (P.) and G . LINOSSIER . Action of Pyrogallol on Copper andIron Salts . . . . . . . . . . . .SIEGFRIED (M.). Oxidation of Phenol by Nitrobenzene . . . .BASIOROWSKI (H.) and A . F . WAYSS . Chlorinated and Brominated Hydro-carbons from Aromatic Aminep . . . . . . . .SENF (A.). Cyananiline and some of its Derivatives . . . . .TAFEL (J.). Benzoyl-derivatives of Phenylhydrazine .. . . .ANSCHUTZ (R.). Action of Phosphoric Chloride on Salicylic Acid . .RBE (A.) . a-Sulphophthalic Acid . . . . . . . .CLAUS (A.) and C . WITT . Dinitro- and Dittmido-amarine . . . .CLAW (A.). An Allotropic Modification of Amarine . . . . .ANSCHUTZ (R.) and Q . WIBTZ . Decomposition of Aromatic Pumarates byHeat . . . . . . . . . . . . .ANSCHUTZ (R.). New Method of Preparing Arvmatic Hydrocarbons . .CLAUS (A.) and K . ELBS . Alkylated Diphenylketones . . . . .NIEMEYER (M.). Chlorinattd Quinones and Quinols . . . . .VOIGT (K.). Benzoihanilide and its Derivatives . . . . . .ANSCHUTZ (R.) and P . MEYER . Amido- and Hydroxy-phenanthraquinones .ANCHUTZ (R.). Malic Acids . . . . . . . . . .thioph en . .. . . . . . . . . .Reactions of the Phosphates of the Aromatic Series .GAUTIEB (H.). Paramonochloracetophenone . . . . .HENIES (M.). Benzyl-derivatives . . . . . . . .ROENER (H.). p-Amidoalizarin . . . . . . . . .BAMBERGER (E . E.) and J . KRANZFELD . Chryeene . . . . .BAMBERGER (E.) and 5 . C . HOOKER . . . .GOLDSCIIMIDT (H.) and R . KOREFF . Camphor . . . . . .T~EMANN (F.) and A . KEES . Reactions of the Glucosides, IIelicin andGlucovanillin . . . . . . . . . . . .Constitution of RetenePAGE99799799810441044lo&10451045104610461046104710481049104910491049105010501051105110521052105310531054105410551056105710581059105910601060106010601061106110621062106310641064106510651067106710671068106910701071107CONTENTS .xxxvPAGETIEMANN (F.) and A . KEES . Glucosides prepared from Helicin . . .LIEUERMANN (C.). Oxyquinoterpene . . . . . . . . 10751073HESSE (0.). Opionin . . . . . . . . . . . 1074HESSE (0.). So-called Fat or Wax from Cinchona-bark . . . . 1075LIEBERMANN (C.). Cochineal and Carmine . . . . . . . 1076BISTRZYCKI (A.) and S . v . EOSTANECKI . New Isomeride of Euxnn-thone . . . . . . . . . . . . . 10’77CIAYICIAN (8.) and P . SILBER . Action of Halogens on Pyrroline . . 1077HANTSCH (A.) . Constitution of Synthetical Pyridine-deri~aticcs and ofIsocinchomeronic Acid . . . . . . . . . . 10781079KOSSEL (A.). Adenine . . . . . . . . . . 1080(XOLDSCBMIEDT (G.). Papaverine .. . . . . . . 1030KRAKAU (A.).lords . . . . . . . . . . . . . 1081CHASTAINQ . 1081DOEBNER (0.) and W . v . MILLER . Methyluqinolines . . . . .Action of Alkalis on Cinchonine and other Cinchona Alkn-Act. ion of Chlorine and Iodine on Pilocarpine . . . .SOSTEONI (L.). Examination of Humus from Peat . . . . . 1085GAUTIER (A.). Constitution of the Albumino‘ids . . . . . . 1082PFORDTEN (0 . v . D.). Condensation of Hydrocyanic Acid . . . . 1120BAUER (H.).their Derivatives . . . . . . . . . . . 1120DE GIRARD (J.). Action of Phosphonium Iodide on Ethylene Oxide . . 1121HENRY (L.). Physical Properties of Chloracetates . . . . . 1121EBERT (H.). Constitution of Ethyl Succinosuccinate . . . . . 1122WOLFP (L.). Derivatives of Levulinic Acid .. . . . . . 1123JOWANOWITSCH (E.).Glycerol . . . . . . . . . . . . . 1125SCHACHERL ((3.).Aconitic Acid . . . . . . . . . . . 1125HILL (H . B.). Monobromo- and Dibromo-pyromucic Acid . . . . 1125CANZONERI (F.) and V . OLIVERI .Acid . . . . . . . . . . . . . 1125MILLOT (A.).Ammonia . . . . . . . . . . . . 1125THOYSEN (J.). Constitutionof Thiophen . . . . . . . 1126PAWLEWSKI (B.). Paraxylene in Galician Petroleum . . . . . 1126MEUNIER (J.). Benzene Hexabromide . . . . . . . 1126NIETZKI (R.) and T . BENCKIBER .1127LEVINSTEIN (I.). Preparation of Nitro-derivatives of Aromatic Amines . 1127GRAEFF (F.). Action of Reducing Agents on Nitrotoluidines . . . 1127HOPYANN (A . W.). Pentamethylaniline . . . . . . . 1125FRAENKEL (N.). Derivatives of Thiodiphenylamine .. . . . 1130LANGE (M.). Formation of Rosaniline by the Nitrobenzene Process . . 1130JANOVSKY (J.) . Products of the Reduction of Nitrazo-compounds in NitrolicAcids . . . . . . . . . . . . . 1131MAZZARA (G.). Constitution of Phenylazothymol . . . . . 1131MAZZARA (G.). Phenylazocarvacrol and Diphenj lazocarvacrol . . . 1132CLAUS (A) and H . KOHLSTOCK . Amarine . . . . . . . 1136MICHAELIS (A.) and H . v . SODEN . Anilides of Orthophosphoric Acid . 1134MICHAELIS (A.) and H . v . SODEN . 1136Preparation of Metachlorobenzaldehyde . . . . . . . 1136CLAUS (A.) and R . WOLLNEB . Methyl Paraxylyl Ketone . . . . 1136REBUFFAT (0.). Phenylcinnamylacrylic Acid and Diphenyldiethylene . . 1137FRIEDLANDER (P.). Nitration of Cinnnmic Acid Derivatives .. . 1137FRIEDLANDER (P.) and J . MAHLY . Nitration of Paranitrocinnamic Acid . 1137FRIEDLANDER (P.) and M . LAZARUS .cinnamic Acids, &c . . . . . . . . . . . 1138MILONE (H.). Salts of Salicylic Acid . . . . . . . . 1139Boiling Point Anomalies of the Chlorinated Acetonitriles andDecomposition of Tartaric Acid in the Presence ofSynthesis of a New Tetrabasic Acid and an 1somer:de ofMonobromo- and Dibromo-pyromucicOxidation of Carbon in the Electrolysis of a Solution ofMENDINI (D.). Monobromo- and Dibromo-citraconimide . . . . 11 2tjBenzene-derivatives obtained by theAction of Carbonic Oxideon Potassium . . . . . . .Triphenylphosphine and its DerivativesNitration of Meta- and Ortho-nitro-c xxxvi CONTENTS .BAUER (R.) .Azobenzenethiosulphonic Acid. Azobenzenesulphinic Acid .MAZZARA (G.) and G . POSSETTO . Diamidomethoxytriphenylmethane . .BODCHARDAT (G.) and J . LAPONT . Essence of Lemon . . . . .CAZENEUVE (P.) and J . MOREL . Crystallographic PropertieB of Camphor-derivatives . . . . . . . . . . . .SPICA (P.). Barosrna CYrenata . . . . . . . . .SCHIFF (H.). So-called Isophloridzin . . . . . . . .PIXIPSON (T . L.). Identity of Regianin and Juglone . . . . .TERREIL . The Red Colo~ring Matters of Wine and Vegetables . . .C~AMICIAN ((3.) and P . MAGNAGHI . Action of Heat on Acetopyrroline andCANZONERI (F.) and V . OLIVERI . Reciprocal Transformation of the Pyrro- . . . . . .BGTTINGER (C.). P~~idiwtricarboxylic Acid . . . . . .MILLBR (W . v.) and F .KINKELIN . . . . .HANSSEN (A.). Relation of Brucine to Strychnine . . . . .BOC~CLISCH (0.). Ptoma'ines from Fish . . . . . . .CRIMAUX {E.). Albumino'ids and the Coagulation of ColloIds . . .ROBIN (M.). Ferric Peptonate . . . . . . . . .ERRENBERG (A.) . Sodium Fulminate . . . . . . . .EHRENBERG ( A.). Chloro- and Bromo-fulminuric Acids . . . .SCHNEIDER (R.). Action of Silver Cganide on Sulphur Chloride . . .BOFXANN (A . W.). Thiocyaauric Acid . . . . . . .STRIEGLER (M.) . Ammelide . . . . . . . . .LAUCH (R.). Preparation of Additive Products of Hypochlorous Acid .GUBBE (0.). Optical Rotatory Power of Invert Sugar . . . .RASCHIGF (F.). Action of Bromine on Dimethylamine . . . . .STOJENTIN (M.). Action of Ethyloxalic Chloride on Derivatives of Car-bamide and Guanidine .. . . . . . . . .NATTERER (K.). Parachloraldehyde . . . . . . . .Oxidation of Ketones . . . . . . . .Carbonylpyrroline . . . . . . . . . . .line. Furfuryl, and Thiophene Groupingsa-MetadiquinolinesEHRENBERG (A.). Fulminuric Acid . . . . . . . .WAGNER ((3.).PFUNGST (A.). Reactions with Nitromethane . . . . . .REINER (C . L.). Fat of the Fruit of Myristica Szcri?zamensis . . .HOMOLKA (B.) and F . STOLZ . lodopropargylic Acid . . . . .BAEYER (A.) . Polyacetylene Compounds . . . . . . .BUCEEA (K.). .THORNE (L . T.). Conversion of Ketonic Acids into Unsaturated Lactones .LEUCKART (R.). Symmetriral and Unsymmetrical Dimethylsuccinic Acids .ERHAXT (F.). Glycide Pyroracemate . . . . . . . .PAN'T HOFF (H., jun.). Malic Acid .. . . . . . .~~JNSCHMANN (M.) and H . v . PECHMANN . Suhstitution-products of Acetone-PECHXANN (H . v.) and H . STOXES . Action of Ammonia on Ethyl Acetone-dicarbos ylate . . . . . . . . . . . .KBECKELER (K ) and B . TOLLENS . Methylhydroxyglutaric Acid fromLevulinic Acid . . . . . . . . . . .HILSEBEIN (E.). Action of Phosphoric Chloride on Meconic Acid . .Action of Sulphur Chloride on Ethyl Sodacetoacetate .dicarboxylic Acid . . . . . . . . . . .MENNEL (E.). Nitrogenous Derivatives of Comenic Acid . . . .HILL (H . B.) and A . W . PALMER . dulphopyromucic Acid . . . .STADLER (0.). Compounds of Thiophen . . . . . . .MESSINGER (J.). Thioxjlen from Coal Tar . . . . . . .PAAL (C.), Synthesis of Thioxylen- and Pyrroline-derivatives . ..BONZ (R.). Bromination of n- and PThiophenic Acids . . .NAHXSEN (R.), Action of Ethyl Ohlorocarbonate and Sodium Amalgam onDiiodothiophen . . . . . . . . . . .BONZ (R.). Synthesis of Thiophendicarboxylic Acid . . . . .PAAL (C.). Action of Phosphoric Selenide on Acetony1a.etone . . .BUCIINER (E.) and T . CURTIUS . Action of Ethyl Diazoaeetate on AromaticHydrocarbons . . . . . . . . . . . .PAGB113911411141114111421142114211421143114411441144114611461146114711911192119211931193119411941194119511951196119711971197119811981200120012001201120112011202120212021203120412041205120512061207120'7120'7120CONTENTS . xxxviiLow (W.).Action of Fuming Nitric Acid on Paraxylylene Bromide . .EN~LER (C.). Presence of Pseudocumene and Mesitylene in DifferentMineral Oils . . . . . . . . . . . .LIEBERMANN (C.) and s . v . KOSTANECKI . Reactions Dependent on PositionROLL ((3.) and 0 . HOLZ . .Carvoxime . . . . . .KLUQE (P.). Mono- and di-Chloroxylene : Chloroparaxylidine . . .Benzyl Ethers of Brominated Nitrophenols .GOLDSCHMIDT (H.) and R . ZURRER .LEVY (9.). Constitution of Chioranilic Acid . . . . . .HOLZ (0.). Bromamidophenols . . . . . . . . .SCHUTT (F.). Parabrom-orthamidophenol . . . . . . .WAQNER (P.). Metamido-phenetoil . . . . . . . .HEYDRICH (C.). Triphenylamine . . . . . . . .LEUCPART (R.) . Tribenzylamine . . . . . . . . .ENQEL (W.). New Cumidine . . . . . .. . .LIMPRICHT (H.). U ydrazine Compounds . . . . . . .TIEMANN (F.). Readions of Aniidoximes . . . . . . .SCHOPF (M.). Derivatives of Metanitrobenzenylamidoxime, &c . . . .KNUDSEN (P.). Derivatives of Phenylethenylanidoxime . . . .GROSS (F.). Derivatives of Phenylhydroxye thenylamidoxinie . . .GRIESS (P.). Acidammonium Bases . . . . . . . .HOTTE (B.). Phenylparamide . . . . . . . . .LIPPMANN (E.) and F . FLEISSNER . .LOEB (M.). Action of Carbonylchloride on Ethenyldiphenyldiamine . .NORTON (L . M.) and W . ALLEN . Action of Dilute Nitric Acid on Anilidea .MICHAELIS (A.) and W . LA COSTE . Phenoxydiphenylphosphine . .Cyanhydrins of Nitroso-compoundsFALCP (E.). Action of Ethyl Chlorocarbonate, &c., on Benzenylamidoxime .SCHULZ (0.).Action of Anhydrides of Bibasic Acids on BenzenylamidoximeDIEHL (L.) and A . EINHORN .DIEHL (L.) and A . EINHORN .DIEHL (L.) and A . EINHORN .Condensation-products of Cinnamaldehydewith Acetone . . . . . . . . . . . .Preparation of Ortho- and Para-nitrocinnam-Condensation-products of Orthonitrocinnam-aldehyde . . . . . . . . . . . . .aldehyde with Acetone . . . . . . . . . .ENQLER (C.). Direct Nitration of Acetophenone . . . . . .ENGLEB (C.) and E . HASSENKAMP . .JACKSON (C . L.) and (3 . T . HARTSHORN . Action of Chromium Hexafluorideon Benzoic Acid . . . . . . . . . . .LEUCKART (R.) and M . SCHXIDT . Action of Phenyl Cyanate on Phenols .GRIESS (P.) . Derivatives of Cyanocarbimidoamidobenzoic Acid, &c . . .MULLER (G.). Benzenylamidoximecarboxylic Acid .. . . .Derivatives of DibromacetophenoneSALOMONSON (H . W.). Nitrophenylparaconic Acids . . . . .HUNT (B.). Synthesis of Tannin . . . . . . . . .GABRIEL (S.). Methglenephthalide . . . . . . . .GABRIEL (S.) . Ben zylidenephthalide . . . . . . . .LIMPRICHT (H.). Sulphonic and Disulphonic Acids . . . . .ULLMANN ((3.). Derivatives of Triphenylmethane . . . . .PISCHER (E.) and C . BULOW . Benzoylacetone . . . . . .and Ethyl Diazoacetate . . . . . . . . . .LAWSON (T . A.). a-/+Diamidonaphthalene . . . . . . .PRAGER (A.). Derivatives of Naphthalene . . . . . . .anthraquiiioiies . . . . . . . . . . .OTTO (R.) and A . ROSSING . Constitution of the Sulphinic Acids . . .WILLGFERODT (C.). Trinitrobenzenesulphonic Acid .. . . .ZEHENTER (J.). Action of Phenol and Sulphuric Acid on Hippuric Acid .FEER (A.) and W . KONIGS . . . . .GEIGFY (R.) and W . KONIGS . Derivatives of Benzophenone . . . .BTJCHNER (E.) and T . CURTIUS . Synthesis of Ketonic Acids from AldehydesGOLDSCHYIDT (H.) and H . SCHMID . Nitrosophenols . . . . .Derivatives of CarbostyrilKLEEMANN (9.) and W . WENSE . a-Diamidophenanthraquinol . . .KOSTANECKI (S . v.) and S . NIEMENTOWSKI . Isomeric Dihydroxydimethyl-PAGE12081205120912093 20912101210121112111212121212131213121312141215121512161216121612171218121812191220122012211221122212231223122412241224122512271228122812291231123212321235123512361236123712381238123812391240124xxxviii COSTENTS .LIEBERNANN (C.).Constitution of Alkylhydroxanthranols . . . .LEVI (L.) Benzylhydroxanthranol . . . . . . . .ZURRER (R.). Campholcnic Acid . . . . . . . . .HALLER (S.). Sylvic and Pimaric Acids . . . . . . .WIESNER (J.). The Gum Ferment . . . . . . . .SCHUNCK (E.). Chlorophyll . . . . . . . . . .MACMUNN (C . A.). Entero-chlorophyll . . . . . . .CIAMICIAN (G.) and P . MAGNAGHI . Bases derived from Pyrroline . .KRIPPENDORFF (F.). Hydroxpcomazine . . . . . . .MICHAEL (R.). Syntheses of Pyridine-derivatives from Ethyl Acetoacetate,Aldehydes, and Ammonia . . . . . . . . .FEER (A.) and W . KONIQS . Derivatives of Methylliydroquinoline . .BEYER (C.). a- y-Dimethylquinoline . . . . . . . .ENQLER (a) and P .RIEHM . Action of Acetone on Aniline . . . .PFITZINGER (W.). Trimethylpinoline . . . . . . .FISCHER (0 . W.). niquinolines . . . . . . . . .KNORR (L.) and F . JODICKE . Action of Ethylic NitrobenzoylacetoacetateCOMSTOCK (W . J.) and W . 6 1 6 ~ 1 ~ . Cinchona Alkaloi'ds . . . .MERCK (W.). Artificial Coca'ine . . . . . . . . .SKRAUP (2 . H.). Benzoylecgoiiine and its Conversion into Coca'ine . .CHASTAING . Alkyl-derivatives of Pilocarpine . . . . . .OSTERMAYER (E.). Caffe'ine Chloriodido . . . . . . .POUCHET (A . G.). Alkalo'id in Koch's Cultivating Fluids . . . .LACHOWICZ (B.) and M . NENCKI . Parahcmoglobin . . . . .MACMUNN (C . A.). Chromatology of the Actinise . . . . .HALLIBURTON (W . D.). Composition of trhe Cartilage of Certain Inverte-brates .. . . . . . . . . . . .on Phenplhydrazine . . . . . . . . .Physiological Chemistry .WOLPF (E.) and others . Digestibility of Potatoes and Carrots with Hay . . . . . . . . . .LAILLEB (A.). Elimination of Phosphoric Acid in the Urine in InsanityandANDOUARD (A.) and V . DBZAIJNAY . Influence of Exhausted Beetroot Pulpon Cow'sMilk . . . . . . . . . .EGGELING and PASTEUR . Various Cattle Diseases . . . . .ELLENBERGEB and HOFMEISTER . Effects of Lead on Ruminants . .ELLENBERGER and HOFFMEISTER .TAPPEINER (H.). Rescarcbes on the Fermentation of Cellulose, especiallywith reference to its Solution in the Alimentary Canal . . . .NICATI (W.) and RIETSCH . Odour and Poieonous Effects of the Productsof the Fermentation produced by the Comms Baciiius .. . .COHN . Value of Disinfectants in Chicken-cholera . . . . .LERYANN (C.). Effects of Alkalis and Acids on Respiration . . .JAWORSKI (W.). Behaviour of Carbonic Anhydride, Oxygen, and Ozone inthe Human Stomach . . . . . . . . . .CHANIEWSKI (S.). Formation z6f Fat from Carbohydrates i n the AnimalOrganism . . . . . . . . . . . .MUNTZ (A.) and C . GIRARD . . . . .MUNTZ (A.) and C . GIRARD . Food forHorses . . . . . . . . . . . .LEEDS (A . R.j. .POLITIS (G.). Relation of Phosphoric Acid to Nitrogen in the Urine duringFeeding with Brain . . . . . . . . . .K m z (E.) . Action of Trichlorethyl- and Trichlorbutyl-alcohol in theAnimal Organism . . . . . . . . . . .and Oats by the HorseEpilepsy . . . . . .. . . . . .Experiments on Digestion in the HorseVIUIER (P.). Digestive Ferments . . . . . . . . .Alimentary Value of OatsDigestibility of Substances usedCornposit-ion and Methods of Analysis of Human MilkPAUE12i01244)124112411241122.1124212421243124412451246124612461246124712p812491249125012501250125112511251727393737417817518018027927928028028128228928328CONTENTS . xxxixPAGEKIJLZ (E.) . A New LEcrorotatory Substance (Pseudohydroxybutyric Acid) .BOHM (L.) and 0 . SCHWENK . Putrefaction of Albumin in the AlimentaryCanal of Herbivora . . . . . . . . . .GRASSET (J.). Anaesthetic Action of Cocai’ne . . . . . .REONAULD (J.) and VILLEJEAN . Physiological Action of Dichloromethanecompared with that of Chloroform .. . . . . . .GUINOCHET . Analysis of the Contents of a Cyst formed under the Tongue .BAGINSKY (A.). Occurrence of Xanthine, Guanine, and Hyposanthine .KOSSEL (A.). Guanine . . . . . . . . . . .F R ~ D ~ C Q (L.). Influence of Changes in the Composition of the Air onRespiratory Changes . . . . . . . . . .BOURQTJELOT (E.). Differences between Pepsin and Trypsin . . . .CAMERER (W.). Metabolism of Five Children . . . . . .RUBNER (M.). Influence of Meat Extract on the Temperature of the Body .WEISKE (H.) and B . SCHULZE . Influence of Certain Amides on the AnimalOrganism . . . . . . . . . . . .WOLFF (E.) and others . Digestibility of Lucerne acd Clover Hay by theHorse and Sheep . . . .. . . . . . .WOLFF (E.) and others . Digestibility of Clover and Meadow Hay by theHorse and Sheep . . . . . . . . . . .SEEGEN (J.). Sugar in Blood : its Source and Signification . . . .&1UNK (J.) and C . v . VOIT . Influence of Asparagine on the Elimination ofAlbumin . . . . . . . . . . . . .NORTH (W.). .GRUNDLER (J.). Iodine in Human Urine after the External Application ofIodoform . . . . . . . . . . . .MINKOWSKI (0.). Occurrence of Hydroxybutyric Acid in the Urine in casesof Diabetes Mellitus . . . . . . . . . .MINKOWSKI (0.). Hydroxybutyric Acid in Diabetic Urine . . . .WEYL (T.). Nitrates in Urine . . . . . . . . .SALEOWSKI (E.). Phenaceturic Acid in the Urine of the Horse . . .SALOMON (G.). Chemical Composition of Pig’s Urine .. . . .GARROD (A . B.). Physiology of Uric Acid . . . . . . .RIEDE H. (€1.). Nitrogen in Faeces . . . . . . . . .GLAUSE (A.) and B . LUCHS~NQER . Physiological Action of some AmmoniumBases . . . . . . . . . . . . .GRA~SET (J.). Anaesthetic Action of Cocaine Hydrochloride . . .FOEKER ( A . P.). Hygienic Importance of the Detection of Carbonic OxideRABOT . Poisoning by Nicotine . . . . . . . . .CHITTENDEN (R . H.) and G . W . CUNMINS . Relative Digestibility of Fishin Gastric Juice . . . . . . . . . . .GRASSET and JEANEEL . Physiological Action of Coca’ine . . . .SBE (G.) and BOCHEPONTAIRE . Yhysiological Effect of Cinchonamine Sul-phate . . . . . . . . . . . . .WOOLDRIDGE (L . C.). Origin of the Fibrin Ferment . . . . .HAYCRAFT ( J .B.). Action of a Secretion obtaiued from the MedicinalLeech . . . . . . . . . . . . .HALLIBUBTOX (W . D.). The Proteids of Serum . . . . . .KOSSEL (A.). d Pectone-like Constituent of the Cell Nucleus . . .BUNGE (G.). Inorganic Constituents of Muscle . . . . . .HOPPE-SEYLER (F.}. .BUNGE ((3.). Assimilation of Iron . . . . . . . .HOPPE-SEYLEE (G.). Effects of Phenylhjdrazine on the Organism . .HERMANS (L) . Action of Trichloracetio Acid . . . . . .SALEOWSKI (E.). Behaviour of Skatolecarboxylic Acid in the Organism .POUCHET ((3.). Changes in the Composition of Certain Secretions duringCholera . . . . . . . . . . . .RIETSCH . Biliary Acids . . . . . . . . . .Influence of Bodily Labour on the Discharge of NitrogenSoaps as Constituents of Blood Plasma and ChyleELIASSOR (W.).Fate of Morphine in the Organism . . . . .O G ~ T A (M.). Poisonous Nature of Sulphurous Anhydride . . . .284284285285285286286p0740840940940941041141141241241341341341341341341441441541 541 54165695715715715’715715725735735745745755755’1657757757X l CONTENTS.EL (0.). Action of Potassium and Sodium Salts on Unstriated Muscle .HESS (E.) and B. LUCHSINQER. Toxicological Contributions . . .SUCHOILSKY (N.). Respiration in Compressed Air . . . . .QIRARD (A.). Alimentary Value of the different parts of the Wheat GrainBAGINSKP (A.). Use of Milk preserved by High Temperatures for Chil-dren's Food . . . . . . . . . . . .ELLENBERGER and HOFMEISTER.Digestion in the Horse . . . .KRATSCHMER. Carbohydratesin Human Liver . . . . . .URIFFITHS (A. B.). Uric Acid from the Green Glands of Astacws JEuvia-tizis . . . . . . . . . . . . JACKSCH (R. v.) Acehonuria . . . . . . . . .STOKVIS (H. J.). Turbidity of Albuminous Urine on Heating . . .SHITH (W. (3.). Composition of the Precipitate obtained on HeatingUrine . . . . . . . . . . . . .GUREENS (F.). Physiological Action of Nickel Salts . . . . .HAY (M.). Physiological Action of Nitroglycerol . . . . .BOCHEFONTAINE and 0. DE CONINGK. Physiological Action of P-Collidine-hexahydride . . . . . . . . . . . .s&E ((u.) and BOCHEFONTAINE. Physiolqgical Action of Cinchonamine .ANREP (B. v.). Physiological Action of Ptoma'ines .. . . .H~NOQUE (A.). Action of Potassium Nitrite on Blood . . . .ALBERTONI (K.). Action and Metamorphosis of some Substances in theOrganism in Relation t o Diabetes . . . . . . . .LOEW (0.). Different Degrees of Resistance in Protoplasm. . . .PFEIFER (E.). Influence of Salts on certain Digestive Processes . . .STUTZER (A.). Nitrogenous Substances Insoluble in Gastric Juice . .MUNK (J.). Absorption, Formation, and Storage of Fat in Animals . .OTTO (J. G.). Amount of Sugar and Reducing Substances in Blood . .GRIFPITES (A. B.). Pancreatic Function of the Cephalopod Liver . .GENTH (C.). Excretion of Carbamide . . . . . , . .DEICHMULLER (A.), F. SZYMANSKI, and B. TOLLENS. B-HydroxybutyricAcid in Diabetic Urine . . . * . . . . . .STADTEAGEN. Cystine not Present in Normal Urine .. . . .LOEW (0.)- Poisonous Action of Hydroxylamine . . , . .HQFMEISTEB (V.). Digestion of Cellulose by the Horse . . . .KNIEREM (W. v.). Assimilation of Cellulose . . . . . .BA~MSTARZ (F.). New Method of Proximate Reaolution of the BrainSabstance . . . . . . . . . . .BBIWKENBERG (C. F. W.) and II. WAGNER. Composition of the Con-tmdile Tissues . . . . . . . . . . .QRIFFITHS (A. B.) and H. FELLOWS. Examination of the Organ of Bojanusin Anodonta . . . . . . . . . . . .SALOMON (W.). Distribution of Ammonium Salts and Formation of Urea .SUNDBERG (C.). The Pepsin Ferment . . . . . . . .BIEDERT (F.). Albumino'ids of Human Milk . . . . . .GOLDMANN (E.) . Fate of Cystei'n and Formation of Sulphuric Acid in theAnimal Body.. . . . . . . . . . .DRESER (H.). .STADELMANN (E.). Pat,hological dcid in Diabetic Urine . . . .FLUCKIQER (M.). The Copper Oxide Reducing Constituent of NormalUrine . . . . . . . . . . . . .SALKOWSKI (E.). Composition of Horses' Urine . . . . . .CEPVELLO (V.). Physiological Action of Trimethylhydroxyethyl- and Tri-methylvinyl-ammonium Hydroxide. . . . . . . .RE~NAULD (J.) and VILLEJEAN. Inhalation of Methane and Monochloro-methane. . . . . . . . . . . . .REQNAULD (J.) and VILLEJEAN. Inhalation of Dichloromethane and Tetra-chloromethane . . . . . . . . . . .VILLIERS. Formation of Alkalolds in Disease . . . . . .LANDWEHB (H. A.). Assimilation (Reabsorption) of F a t . . , .Histological Chemistry and Physiology of the Kidney .PAGE5785786776786796796796806806806816816316816826826826%82782782782982982983083083083091691rj91892092192192192292292392492498 492592691692699COSTEXTS. xliCHITTENDEN (R.H.) and C. W. CUMMIPI'S. Tnfluence of Bile, Bile Salts,and Bile Acids on Amylolytic and Proteolgtic Accion . . . .SEBBLIEN (J.). The Prote'ids of Com' Milk . . , . . .SCHMOGER (M.). Milking of Cows . . . . . . . .TICHOMIROFF (A.). Chemical Changes attending the Development of theEmhryo in the Eggs of Bombyx mori . . . . . . .MERING (J. v.). Physiological Action of Potassium Chlorate . . .THIERFELDER (H.) and J. v. MERING. Physiologicil Action of the TertiaryAlcohols . . . . . . . .. . . .RICHARD. Action of Coca'ine on the Invertebrales . . . . .LEO (H.). ,EVULINU (W.). Case'in in Milk, and on the Action of ltennet . . .CHAUVEAU (A.). Preventive Inoculation for Splenic Fever . , . .VILLIERS f A.). Pathological Urinee . . . . . . . .MAIRET (A,), PILATTE, and COMBEMALE. Action of Antiseptics on HigherOrganisms : Thymol . . . . . . . . . .L~PIKE (R.) and P. AUBERT. Relative Toxic Effect of the Organic andSaline ConfAituents of Urine . . . . . . . . .SCHETZ (E.). Quantitative Relationship of Pepsin to Peptones . . .MUNE (I.). Assimilation of Fats . . . . . . . .ELLENBERQER and HOFYEISTER. Researches on the Digestion of 1 he HorseMULLER. Feeding with Dry and Steeped Maim . . . . . .ROSE. Maize Ensilage for Cows . . .. . . . . .MARCKER (M.). Value of Sugar BK) Food for Stock . . . . ,DOQIEL (A.), The Albumino'ids of Milk . . . . . . .TICHOMIROFF (A.). Chemical Changes in the Eggs of Bomlyz mori duringDevelopmeri t . . . . . . . . . . . .SRSTINI (F.). Relations between Atomic Weight and Physiological FunctionBROUARDEL (P.) and P. LOPE. Poisoning by Hydrogen Sulphide . .RUBNER. Calorimetric Inve: tigations . . . . . . . .CHANDELON (T.). Studies on Peptonisation. . . . . . .KLENZE. Digestibility of Cheese . . . . . . . . .HENNEBERG (W.). Feeding Sheep with Sugar . . . . . .MEYER (F.). Earthnut- and Rye-meals as Food for Milch Cows. . .WOOLDRIDQE (L. C.). Fibrin Ferment in Blood. . . . . .PURDIE (T.). Composition of the Milk of the Porpoise . . . .POULTON (E.B.). Essential Nature of the Colouring of PhytophagousLarve, &c. . . . . . . . . . . . .MAIRET, PILATTE, and COYBEMALE. Action of Antiseptics on HigherOrganisms . . . . . . . . . . . .Formation and Migration of Fat in Phosphorus Poisoning.Chemistry of Vegetable Physidogy and Agriculture.THAEE. Nitrogen necessary for Cultivated Plants . . . I .GIRARD (A.). Formation of Sugar in Beets . . . . . .GRIFPITHS (A. €3.) and E. C. CONRAD. Salicylic Acid in the CultivatedPansy . . . . . . . . . . . . .ELEIN ((3.). Experiments with Mauures containing Thiocyanates . .KONIG (J.). Poisonous Effects of Ammonium 'l'hiocyanate on Vegetation .SCHROXDEB (J. v.) and another. ,PEEREY (A.). Use of Copper Sulphate to Destrsv Mildew . . . .PELIUOT (E.).Carbon Bisulphide in Aqueous Solution as a Remedy forPhylloxera . . . . . . . . . . . .WOLLNY (E.), Protective Influence of Growing Plants on the UndergrowthVOELCKER (A). Four-course System at Woburn . . . . .Growth of Breadstuffs in Various Latitndes. . . . . . .v. PFUEL. Cultivation of two Varieties of Sorghum, and Preparation ofSugar therefrom . . . . . . . . . , .Influence of Acid Smoke on Vegetation999100010001000100210021002100210831084108410%10851147114811 49114911491149114911501150115112521252125212521852125312531253125.375757576767677'777778787xlii CONTENTS .PAGEMINANGOIN (N.). Cultivation of Sorghum in France . . . . .Tobacco Culture . .. . . . . . . . . .FERRARI (C.). Influence of the Weather on Crops . . . . .HEINRICH . Dependence of Cultivation on the Depth of the Soil . .ESER (C.). Influence of Physical and Chemical Properties of the Soil onEvaporation . . . . . . . . . . . .WOLLNY (E.). Influence of the Soil and its Cultivation on the Temperatureand Moisture in the Air . . . . . . . . . .RAMANN (E.). Result of Removing DBbris from the Surface of Sandy SoilMARCEER (M.) and others . Drying of Diffusion Cuttings . . . .PARSEP (F.): Fine and Coarse-graLed Superphosphates . .VOELCKER (A.). Action of Soluble and Insoluble Phosphates . .HEIDEN (E.). Superphosphatic Gypsum as an Absorbent of AmmoniaLECHARTIER ((3.). Employment of Potash Manures in Brittany .MARCKEX . Potash Manures for Potatoes .. . . . .FARSKY (F.). Sulphuric Acid as Manure . . . . . .IJADUREAU (A.), The Aminoniacal Ferment . . . . .MARCANO (V.). Pept. onic Fermentation . . . . . .JORISSEN (A.). Germination of Linseed and Sweet Almonds . .EEINLE (J.) .BRASSE (L.). Presence of Amylase in Leaves . . . . .MUNRO (J . M . H.). Ash of Stranberries . . . . . .KOXIQ (J.) and others . .~ V I L D T (E.). Removal of the Bitter Principle from Lupines . .FITTBOGRN (J.) arid 0 . FOERSTER . .DEHBRAIN (P . P.). Cultivation of Sugar-beet . . . . .FLEISCHEE (M.). Hop Culture in Peat Soils . . . . .DEHBRAIN (P . Y.). On Rotations . . . . . . .DRECHSLER (G.). Manuring Experiments . . . . . .DRECHSLER (G.). Notes on Manuring . . . . . .TROSCHEE . Preservatioti of Ammonia in Stable Manure .. .REDER (l’.). Experiments on the Nitrogen of Peat . . . .GAGNAIRE . Effects of Fresh Stable Manure on Potatoes . . .QAUTIER (A.) . .CAZENEUVL (P.). Plaster Filters to Sterilise Liauids . . . .Chlorophjll in the Living Cell and Assimilation of CarbonPLANTA (A . v.). Chemical Composition of Hazel Pollen . . .Ensilage and Acidification of Green FodderEnsilage of Prozen Potatoes .KOCH (L.). Manuring Experiments with Chili Saltpetre . . .VANDEVXLDE (G.). Chemistry of Bacillus subtilis . . . .Sterilisation of Fermentable Liquids in the Cold .CHAIRY . Aition of Various Compounds on Bacteria of the Genus Tyro-thrix . . . . . . . . . . . . .SACHS (J.) Activity of Assimilation by Leaves . . . . . .EMMERLING (A.).Formation of Albumin in Green Plants . . . .~ V I L M (V . v.). Fat in Palm Nuts . . . . . . . . .REGKAULD (J.) and VILLEJEAN . Oleaginous Seeds of the Symphonia fasci-culata . . . . . . . . . . . .PASCHKIS (K.j. Occurrence of Phytosterin . . . . . .MORQEN (A.). Composition of Inferior Hay . . . . . .LEPLAP (H.). Vegetation of the Sugar Beet in the Second Year . .HUEPPE (F.) . Changes which Milk undergoes through the Agency of Micro-SCRICHOWSKY . Composition of Maize . . . . . . .KINCH (E.). Composition of the Food of Scotch Hill SheepKRECHEL (G.). Analysis of White Carrot Fodder . . . . .organisms . . . . . . . . . . . .BBCHAMP (A.). Origin of Microzymas and Vibrioles . . . . .BUNGENER (H.). Degeneration of Brewer’s Yeast .. . . .DUCLAUX (E.). Vitality of Gerins of Microbes . . . . . .DIETZELL (B . E.). . . .ICONIC+ (J.). A New Germinator . . . . . . . . .CIESLAR (A.). Infliience of Light on the Germination of SeedsSCHUBELEB . Aotion of Long Days on Vetmation . . . . . .. . .Source of the Nitrogen of the Leguminosre. . .9.97979808080818182828383838318118118118218218218318318418418418518518718718718818928’72872882892892892902902912912 3129229829341641741741’741841941 941918CONTEXTS . xliiiPAGELIEBENBERQ (A. v.), Influence of Intermittent Heat on the Germination ofSeeds . . . . . . . . . . . . .J~NSSON (B.) . Effects of Running Water on Plants . . .. .TROSCHEE . Water Culture of Lupines . . . . . . .WEISKE . Water Culture of Lupines . . . . . . . .PRIPSON (T . L.). Chemical Phenomena of the Respiration of Plants . .HELLRIEGEL (H.). Evaporative Surfaces of Plants, and Influence ofMoisture in Soils on Plant Growth . . . . . . . .MATJMENE ( E . J.). Existence of Manganese in Plants and Animals . .RISLEE (E.). .LTEBSCFIER (G.). Cultivation of Swedish and German Cereals . . .MARX (L.). Comparison of the Barleys of Different Countries . . .MARCKER (At.). Loss of Weight in the Ensilage of Beet-leavesInfluence of Temperature on the Development of WheatKIRCHNER and others . Ensilage Experiments with Various Fodders . .DEHBRATR (P . P.). Cultivation of Sugar-beet at Grignon in 1884 . .LIEBSCHER (G.).Cultivation of Various Sugar-beets . . . . .PELLET (H.). Sugar-beet Seed as Fodder for Cattle . . . . .KLEIN (G.). Adulteration of Linseed Cake and Rape Cake . . . .SACO . . . . . .KONIG (F.). Analysis of Cot. ton Seeds . . . . . . .KREMSER (W.). Variations in Rainfall . . . . . . .WOLLNP (E.). Micro-organisms in Soil . . . . . . .I)UCLAUX (E.). Germination in Soil rich in Organic Matter, but free fromMicrobes . . . . . . . . . . .&fARCKER . SOlUtiOn of' Wool-dust . . . . . . . .SCHREINER . Peat as Manure . . . . . . . . .MAQNIER (H.). Straw, Pcat, and Sawdust as Litter . . . . .LOBBECKE . Manuring Experiments with Precipitated Phosphate . . .LIEBSCHER (8.). Manuring Sugar-beet . . . . . . .KUNTZE {L.). Parallel Experiments on Peat Compost and Chili Saltpetreas Manures for Sugar-beet .. . . . . . . .WILLIAMS (C . T.). Influence of Culture Fluids and Reagents on tho Growthof Bacillus tuberculosis . . . . . . . . . .BEIEGER (L.). Bacteria . . . . . . . . . .BBCHAMP (A.). Organisms which produce Zymases . . . . .BONNIER (G.) and L . MANGIN . Exchange of Gases between Lichens and theAtmosphere . . . . . . . . . . . .BERTHELOT and ANI)RB . Formation of Nitrates in Plants . . . .SCHULZE (E ) . Acid Amides from the Decomposition of Albumin . .THRESH (J . C.). Proximate Constituents of Hedychium spicatum . .3: LBO RNE (W . ) . English Rhubarb . . . . . . . .TAKAYAMA (J.). Japanese Teas and Tobaccos . . . . . .UUNSTAN (W . R.) and F . W . SHORT . Stvychnos Nux-vowica Indigenous toCeylon .. . . . . . . . . . . .DIEITLAFAIT . Composition of the Aph of the Equisetaceee . . . .LAWES (Sir J . B.) and J . H . GILBERT . Continuous Growth of Wheat a tRothamsted from 1864-1883 . . . . . . . . .RICHARDSON (C.). Chemical Composition of Wheat and Maize as Influencedby Environment . . . . . . . . . . .RUFIN (A.). First Grass and Aftermath . . . . . . .WOLLNP (E.). .CIXBAL (0.) and others . Cultivation of Potatoes . . . . . .KNATJER (F.) and others . .1 ) ~ GASPARIN (P.). Phosphoric Acid in the Soil . . . . . .HENSCH (A.). Influence of Cultivation on the Moisture of the Soil . .ZOLLA (U.). Use of Potassium Chloride in Agriculture . . . .GOESSMANN (C . A.). Manurial Value of Tobacco Stems . . . .. . .Composition of the Seeds of the Cutton Tree'IHUMEN (F .v.). Fairy Rings . . . . . . . . .MARCEER . Sidney Guano . . . . . . . . . .Influence of the Position of the Set on the Potato CropPeculiarities and Cultivation of the Beet SeedDF E R (B.) . Manuring Turnips . . . . . . . . .4194194204204204214214224224224324834234244254254.854254254254264284284284294294294294295785785805805815815825825825836835835855865865875 8758858856858958xliv CONTENTS .ZWILLINQ (3.). Correct Time for the Eoney Harvest . . . . .YICHARD (P.). Removal of Mildew in Vines . . . . . .DETMER (W.). Formation of Hjdrochloric Acid in Plants . . . .WOLLNY (E.). Micro-organisms in the Soil .. . . . . .CARBONI (G.). Formatron of Stamh in Vine Leaves . . . . .TROSCHKE . Composition of Furze QULex Buropeus) . . . . .CORENWINDER (B.). Growth of Sugar-beet . . . . . .BOTJSSINGAULT . Temperature of Hailstones . . . . . .QUANTIN (H.), Soil of Tanis . . . . . . . . .SACHS (T.). Metastasis in Leaves . . . . . . . .MOLLBR (H.). Respimtion of Plants . . . . . . . .CAMPANI (G.). Existence of Manganese in Plants . . . . .CEBUELLO (V.). Adonis Cupaaiaaa . . . . . . . .SZECHENYI (E . v., jun.). Cultivation of Sorghum saccharaturn . . .AUDOYNAUD (A.) and E . ZACHAEEWICZ . Farmyard Manure . . .MUXRO (J . M . H.).Conposition of Wood Ashes . . . . . . . .BOURQVELOT (E.). Diastase . . . . . . . . .and Absorption of Oxygen by Leaves in the Dark .. . . .GODLEWSKI (E.). Circulation of the Sap in Plants . . . . .FRANK (A . B.). Formation and Phyeidogical Significance of Gum . .HECKEL (E.) and F . SCHLAQDENRAUFFEN . Chemical Composition ofAdemisia Gallica . . . . . . . . . . .HELLRIEGEL (H.) . Preservation of Dried Washed Sugar-beet MarkSections . . . . . . . . . . . . .EMMERLING and others . Manurial Value of Freshly Fallen Leaves . .MARCKER . Manurial Value of Peat Waste . . . . . . .KUDELKA (F.) and M . HOLLRIJN~ . Large and Bmall Hulled Beetroot Seed .HILLER (E.). Percatage of Alkaloids in Lupines . . . . .SCHRODT (M.) and H . HANSEN . Feeding Milch Cows with Ensiled Sugar-beet Sections . . . . . . . . . . . .STREBEL and others . Cultivation and Preservation of certain Cereals ..BOURSIER and ST . ANDR~L Manuring Potatoes with Potash Salts . .LECHARTIER (G.). .Black Soil from Manitoba . . . . . .RITTER (A.). Improvement of Sheep Manure by Kainite . . . .WAGNER .DEHBRAIN (P . P.) and L . MAQUENNE .Employment of Cider Mark as Manure and E’odderEvolution of Carbonic AnhydrideHECKEL (E.) and F . SCHLABDENHAUPFEN . Chaulmoogra Seeds . . .Analysis of Tobacco . . . . . . . . . . .HANAMANN (J.). Composition of Horse Chestnuts . . . . .BRIEM (H.). Ahsorption of Water by Beetroots . . . . .DEH~BAIN (P . P.). .EIJCILINU (W.). Composition of Alpine and Valley Hay . . a . .PETERSEN . . . .SCHRODT (M.) and H . HANSEN . Ihfluenee of Malt Coombs on the Yield ofMilk . . . . . . . . . . . . .EUQLING (W.).Experiments with Nitrogenous and Peaty Soils . .FLEISCHER (M.) and others . Action of Sea-sand on Peaty and Sandy Soils .Experimental Culture of Wheat at Grignon in 1884Nutzitive Value of Hay grown on Marsh LandsDE GASPARIN . Complementary Manures . . . . . . .DANGUY (R.). Nitrogen in Leather Waste . . . . . . .BUCHNER (E.). Intluence of Oxygen on Fermentation . . . .BOURQUELOT (E.).TAMMANN (G.). Fate of Sulphur in Germination . . . . .CUBONI ((3.). Formation of Starch in Vine Leaves . . . . .Selective Alcoholic Fermentation . . . . .ATWATER (W . 0.). Acquisition of Atmospheric Nitrogen by Plants . .SCHULZE (E.) and E . BOSSHARD . Allant o h , Asparagine, Hypoxanthine,B ~ H M (R.) . Chemical and Toxicological Relations of Certain Fungi ..WOLLNY (E.). Absorptive and Evaporative Powers of Various Litters .BESELEL (0.) and M . MARCKER . Cultivation of Varieties of Oats . .and Guanine as Plant Constiterents . . . . . . .HANAMANN (J.). Keeping of Topped and Untopped Beet . . . .PA6 R5905906836836P3684684684685655685686ti86687831832832838832833833833833833834834834834834927927927927927928928928929929929929829930930100210031004100410051007100810081008100COXTEXTS . xJ vSCHLABDENHIUFFEN and GARNIER . .WAQ-XER . Manuring with Peat . . . . . . . . .FITTBOQ-EN . Action of Various Forms of Phosphoric Acid . . . .UNIQ- (J.) . Manuring Experiments . . . . . . . .MAUMEYE . Alleged Elective Fermentation .. . . . . .BOURQUELOT (E.). Fermentation of Invert Sugar . . . . .BGCHSMP (J.) and A . DUJARDIN . The Zymase of JequirityCarbonates in Living Plants . . . . .Arsenic in the Soil of Cemeteries. . .BERTHELOT and ANDRB .HORNBERGER (R.). Composition of f3isileapus alba during various Stages ofGrowth . . . . . . . . . . . . .KELLNER (0.) and J . SAWANO . Changes in Fodder during Ensilage . .MuNm (A.). Oxidation and Reduction under the Influenee of MicroscopicLEHMANN (V.). Self-fermentation of Yeast . . . . . . .LEPLAY (H.). Selective Fermentation of Invert Sugar . . . .TEIXEIRA (J . F.3. The Saccinic Acid Ferment and its Action onCane-sugar . . . . . . . . . . . .HOLDEFLEISS . Electrical Researches . . . . .. . .MOLI~CH (EL) . Deviation of Roots from the Normal Direetion of Growth .GE%HANT (N.) and J . PEYROU . Gas contained in Floating and SubmergedLeaves . . . . . . . . . . . .SCHULZE (E.). Fermation of Sulphates in Germination . . . .PORTELE (K.). So-called Sour-rot sE Grapes . . . . . .FITTBOGEN (J.) and others . .EUGFLINB (W.). . . . .SCHINDLER (F.). Valuation of Hay . . + . . . . .JENSEN (J . L.). Protection of Potatoes against Disease . . . .ANDRZ . Desiccation of Seed Potatoes . . . . . . . .LACE (B.). Shaded and Unshaded Sugar-beets . . . . . .TROSCHKE . Cultivation and Composition of Sorghum . . . . .SAARE (0.). Starch Refuse as Fodder . . . . . . .TAUTPEOUS (C . T.) and E . WOLLWY . Influence of Different Systems ofSESTINI (F.) and A .D~cocco .LAWES (Sir J . B.). Ensilage . . . . . . . . .Organisms in the Soil . . . . . . . . . .ERRERA (L.). Glycogen in Beer Yeast . . . . . . .Maize-heads as Fodder . . . .Influence of Calcium Sulphide on Barley .Effeet of Rain on the Quality of HayPAGE100910091009101010851085108510861087108710871088115111511151115211521152115311531153115311541154115411541155115511551155Applyin$ Manures . . . . . . . . . . .Various Slanure Materials . . . .MARCKER (34.). Chili Saltpetre or Amm mium Sulphate ? . . .LADUREAU (A.). Sugar-beet and Phosphates . . . . .EBREEA (L.). Glycogen in Ferments . . . . . . .CLAASSEN (E.). Bitter Principle of the Comberry . . . .WAGKEB (P.) and others .VENABLR (F .P.). Leaves of Illex cassine . . . . . .TSCHIRCH (A) . Hyacinthus orientaEis . . . . . .LAWES (Sir J . B.). Ensilage . . . . . . . .MAYER (A) . Feeding Value of Various Roots . . . . .MASURE (F.). Evaporation of Water into the Atmosphere . . .YHIPSON (T . L.). Caffetannic Acid, &c., in Virginia Creeper . .HORNBERGER (It.). .AITKEN (A . P.). Report on Ensilage and Manuring Beans and BarleyMineral Mabter in the Seeds of Forest TreesAUDOYNAUD (A.) and E . ZACHAREWLCZ . Farmjard Manure . .Analytical Chemistry.LITACHE (A.) .FOHR (C . F.).Preparat. ion of Standard Solutions of Carbon BisulphideEstimation of Minute Quantities of Silrer . . .B L O X A ~ (C.'L.).'E/IACKINTO-H (5 . B.).HUFSCHUIDT (I?.). Separation of Arsenic from Antimoiij aud Tin .. 86Estimation of Manganese in Cast Iron or SpiegeleisenVolumetric Estimation of Manganese ; Influence OfOrganic Matter and Iron . . . . . . . . . 85. 1156 . 1156 . 1156 . 1157 . 1254 . 1254 . 1254 . 1254 . 1255 . 1255 . 1255 . 1257 . 1259 . 1260 . 1260. 84 . 84 . 8xlvi CONTENTS .SMITH (ANGUS R.). Examination of Water . . . . . .MULLER-JACOBS (A.). Determination of the Nature of the Crude Oil inEILOART (A.). .REMONT (A.). Estimation of the Wool. Silk. and Cotton in Tissues . .JOHNSON (G . S.). Modification of Dumas' Method for the Estimation ofNitrogen. . . . . . . . . . . . .BRITO (P . S.). Method of Testing for Iodine in Presence of Large Quan-tities of Bromine . . . . . . . . . . .PRATT ( J . W.).Rapid Estimation of Fixed Ammonia . . . .CLASSEN (A.). Quantitative Analysis by Xlertrolysis . . . . .VALENTA (E.). Testing Mineral Oils . . . . . . . .Turkey-red Oil . . . . . . . . . . .Bromine as'% Test for Quinine, Narcotine, and MorphineCLASSEN (A.). Electrolytic Estimations . . . . . . .ILES (M . W.). Decomposition and Analysis of Slags . . . . .KNOP (W.). Remarks on the Analysis of Soils . . . . . .MOORE (T.). Separation of Zinc from Nickel . . . . . .GORE ((3.). Estirnat. ion of Ammonia in Potable Water . . . .MASON (W . P.). Viscosity of Oils . . . . . . . .LEFFMANN (H.). Examinations of Butter . . . . . . .MICHAILOFF (W.). New Reaction for Albuminoyds . . . . .STRENG (A4.). Microscopic Chemical Reactions . . . . . .HART (E.).Detection of Iodine. Bromine . and Chlorine . . . .HARNACK (E.). Estimation of Iodine in Urine . . . . . .REESE (C . L.). Estimation of Sulphurous Anhydride . . . . .CHATARD (T . M.). Estiniation of Alkalis in Silicates . . . . .DOUGHERTY (G . T.). Estimation of Antimony . . . . . .VOGEL (A.). Detection of Cyanogen . . . . . . . .GREINERT .PONCY (C . DE) .Ethyl Alcohol . . . . . . . . . . .JAY .KROEN (L . M.). Analysis of Red Wine by Means of Electrolysis . .RICHARD (L.). Estimation of St'arch in Gluten Bread . . . .ANDOUARD ( A . ) . Estimation of CIum Arabic in Syrup . . . .SAMBUC . Milk Adulteration . . . . . . . . .MOORE (R . W.) Koettstorfer's Method for the Examination of Biitter forForeign Fats . . . . . . . . . . . .BECHI .Detection of Cotton Seed Oil in Olive OilLEVALLOIS (A.). Estimation of Fragrant Essential Oils . . . .VRIJ (J . E . DE) . Assay of Commerciul Quinine SulphateRABY (L.). New Reactions for Codebe and Zsculine . . . .CARLES (I?.). Estimation of Tannin . . . . . . . .RABOURDIN (H.). Adulteration of Pepper . . . . . . .oxide. . . . . . . . . . . . . .MARTIKQN . Estimation of Hydrogen Peroxide . . . . . .FOURMONT . New Method of Testing for Chlorates . . . . .KRETJSLER (K.). Quantitative Estimation of Nitrogen . . . . .WAGNER (P.). Estimation of Nitrogen in Chili Saltpetre, &c . . . .OSTERSRTZER (J.). Nitrogen in Artificial Manures . . . . .Eetimation of Phosphoric Acid in ManuresGUCCI (P.). New Method for Separating Copper from Cadmium ..PETERSON (H.). Determination of Iron and Chromium in Alloys . .TAYLOR (W . J.). Detection of Cyanides in Presence of Compound CyanidesMCCAY (L . W.). Notes on Reichcrt's Method of Butter Analysis . .HANSSEN (A.) and C . E . SCHNITT . Methods of Butter Analysis . . .PRUNIER . Volumetric Estimation of Calcium Oxide and Carbonate . .HOOD (J . J.). . . . Estimation of Iron by Potassium PermanganateAmmonia. Nitrous Acid. and Nitric Acid in Potable Waters .Separation and Estimation of Methyl Alcohol in presence of. . . . . . Detection of Coal Tar Colours in Wines. . . . .. . . .CAMERER (W.). Estimation of Nitrogen in the Urine and Faxes . .CARPENTER (H . S.) and W . 0 . NICHOLSON . Estimation of HSdrogen Per-SPENCER (G . L.). New Method of Determinlng Phosphoric Acid in Manures .. . . . . .PAGE869395969G189189190190190192193193103194194196196196197197198294295296296296296297297297297298298298299299299300302301 .308302302303303430430430435436436437433BONQARTZ (J.). Volumetric Estimation of Phosphoric Acid . . .BECEURTS (H.). Hydrochloric Acid in Marsh's AppaPatus . . . .BECKURTS (H.). Preparation of Hydrochloric Acid free from Arsenic . .JOLY (A.). . . .Estimation of Potassiiim in ManuresHAGER (H.). New Reaction for Sodium, Ammonium, and Lithium Salts .QUESSAUD (J.). Determination of Silver and Copper in the same Solntion .PRUNIER (H.). Volumetric Determination of Alumina in Lime and CementSCHLAQDENHAUFFEN .Volumetric Determination of Manganese . . .WIELAND (J.) . Electrolytic Estimations . . . . . . .CABPENTER (H . S.) and \V . 0 . NICHOLSON . Examination of Water €orSTUTZEB (A.). Phosphoric Acid Soluble in the Soil . . . . .BECKURTS (H.). Estimation of Arsenic in Judicial Cases . . . .Action of Boric Acid on some Colouring Mattem . . . . . . . .Organisms . . . . . . . . . . . .Analysis of Wines . . . . . . . . . . . .ENDEMANN (H.). Examination of Glycerol . . . . . . .BISNAMINI . Estimation of Saccharose, Glucose, and Lactoee . . .RUBNER (M.). Action of Lead Acetate on Glucose and Lactose . . .BISHOP (W.). Analysis of Honey . . . . . . . .HEHNER (0.). Analysis of Honey . . . . . . . .ARCHBUTT (L.).Free Acid in Oils . . . . . . . .MALLAT (A.). Determination of Starch in Gluten Bread . . . .PUSCH (T.). Test for the Presence of Tartaric Acid in Citric Acici . .KINGZETT (0 . T.). . . .DECHAN (M.) and T . MABEN . Milk Analysis . . . . . .Fox (W.) and J . A . WANKLYN . . . . . .WILLIAMS (R.). Testing Aniline Hydrochloride . . . . . .NOTTA and G . LUSAN . Detection of Morphia in the Urine . . . .PETIT (A.). Assay of Cinchona Bark . . . . . . . .DUNSTAN (W . R.) and F . RANSON . Detection of Alkaloids in t'he Root ofLINDT (0.). Microchemical Test for Brucine and Strychnine . . .CHLOPINSKY . .LE NOBEL ((3.). Testing for Acetone in Acetonuria . . . . .PFEIFFER (T.). Titration of Urea . . . . . . . .HAMBURGER (H . J.). Estimation of Urea by Bromine .. . .OTT (A.). Estimation of AlbuminoYds in Urine . . . . . .MSHU (C.) Exaniination of Urine for Albnmose and Peptone . . .LANDRIN (E.). Adulteration of Pepper with Olive Residnes . . .STBOHMER (F.). Testing of Cayenne Pepper . . . . . .MEYER (0.). Simple Method of Examining Yeast . . . . .WOLLNY (R.). Analytical Operations and Apparatus . . . . .ZULKOWSKY (C.) and C . LSPBZ . Estimation of the Halogens in OrganicFURRY (F . E.). Iodic Acid as an Indicator . . . . . . .HEMPEL (W.). Estimation of Oxygen in Air . . . . . .DABNEY (C . W.) and B . v . HERFF . Determination of Nitrogen by theUAWALOVSKI (A.). M3dification of Zulkowsky's Azotimeter . . .WARINSTON (R.). Detection of Nitrous and Nitric Acid . . . .LONSI (A.). Volumetric Estimation of Nitric Acid .. . . .FLECK (H.). Recognition of Nitric Acid Stains on Textures . . . . .OSBORNE (T . B.). Separation of Zinc in Ores . . . . . .OSBORNE (T . B.). Separation of Zinc and Nickel . . . . .WHEELER and LUDEKINB . New Blowpipe Reagent . . . . .ROESSLER ((3.). Lead Assaying in the Wet Way . . . . . .FOOTE (H . (3.). Apparatus used for Precipitating Copper by Electrolysis .BARnEs (J.). SeDaration of Metals Preciuitated bv Hvdrochloric Acid .Rape Oil, Beef Fat, and Mutton DrippingButter AnalysisCASTHELAZ (C.). Commercial Phenols . . . . . . . .SCHWEISSINGER Detection of Atropine . .Atropa belladonna . . . . . . . . . . .. . . . .Detection of Picrotoxine in Animal Liquids and TissuesCompounds . . . . . . . . . .. .Copper Oxide Met'iod . . . . . . . . . .COXTENTS . xl\Tii\ I L I " 597PAGE438439439440440441)44144 14414414-224424424434434434444444444454454464464464464 644744744744844844944.941.945045045145 145 145245259159159259259359359359559559559559659659XI viii CONTENTS.CLASSEN (A). Electrolytic Estimations . . . . . . .TROILIUS (M.). Estimation of Manganese and Phosphorus in Iron andSteel . . . . . . . . . . . . .JAY. Ash Determinations . . . . . . , . . .LENZ (W.). Titrations with Potassium Permanganate Solutions . . .HEPPE ((3.). Adulteration of Petroleum with Solar Oil . . . .LANGBECE (H. W.). Detecdion of Adulterated Essential Oils .. .VAN DE VYVERE. Estimation of Methyl Alcohol in Ethyl Alcohol .ROSE (B.). Detection of Pusel Oil in Spirituoug Liquors . . . ,LASCH (K.). Sodium Nitroprusside as a Reagent for Sugars . . .WILEY (H. W.). Determinations of Lactose in Milks by Optical Methods .JAY. “ Dry Extract” . . . . . . , . . . .WEIGELT ((3.). Estimatim of Wine Extract . . . . . .SILLPOWSKI (H.). Me1t)ing Points and Separation of Mixtms of Phenyl-acetic and Hyrlroxycininamic Acids . . .. , . . . .MACEWAN (P.). Testing Peruvian Balsam . , . . . . ISCHMOGER (M.). Soxhlet’s Armmetric Butter-fat Estimations . . .BRADFORD (S. S.). Basic Lead Acetate as a Test for Olire Oil . . .GLADDIN@ (T.), Quantitative Separation of Rosins and Fats . . .AMTHOH. (C.). Caramel . . . .. . . . . .SCHEFFER (E.). Estimation & Nicotine . . . . . . .CHANDELON (T.). Deteotion of Stqdinirie and other Alkalo?ds . . .JOHANNSON (E,). Detection of Colocynthin, Elaterin, and Brymin . .~~IBSCHEIAUSEN (L. v.) . Detection of Berberine, Hydrastine, and Oxyacan-t h i n e . . . . . . .. . . . .RWGELQEN (A. v.). Detection of Sangiiinarine and Chelidonine . . .ZUELZEU (W.). Estimakion of Chlorine in Human Urine . . .PFLUUER (E.) and K. BOHLAND. Simple Method of Estimating Nitrogenin Urine. . . . . . . . . . . . .BOHLAND (K.). Estimation of Nitrogen in Drilae . . . . .LEHMANN (T.). Estimation of Alkalis in Urine . . . . . .GERRARD (A. W.). Apparatus for Estimating Carbamide . . . .LUZZATTO (&I.). Liebig’s Method for the Estimation of Carbamido ..1 . 0 ~ ~ (B.). Microchemieal Detection of Nucle’in, &c. . . . .HANYARSTEN (0.). Separation of Serum-albumin and Globulin by meansof Magnesium Sulphate . . . . . . . . . .HESSE (W.). Quantitative Estimation of Micro-organisms in the Air. .SCHYITZ (Y.). Modification of the Calcium Chloride Drying Tube used inElementary Analysis . . . . . . . . . .HOLTHOF (C.). A S;mple Fusion Salt . . . . . . . .BOHLIG (E.). Solubility of Glass . . . . . . . .OSMOND. Determination of Srr.al1 Quantities of Hydrogen Sulpliide . .CZECZETEA ((3.). Nitrogen Determinations by Kjeldahl’a Method .MACEINTOSIX (J. B.). Estimation of Graphite in Minerds . . . .HAUSHOFER. Microscopic Analysis . . . . . . . .VIGNON (P.). Separation of Aluminium and Iron .. . . .HOLTEIOF (C.). Precipitation of Manganese with Bromine . . .OSMOND. Colorimetric Estimation of Manganese. . . . . ,XAHLMANN (W.) and A. SMOLKA. Estimation of Manganese in Spiegeleisen,Ferromanganese, &c. . . . . . . . . . .RAMNELSBERG (C.). Analysis of Uranium Compounds . . . .SCHWEISSIX’GEB (0). Iodiscd Tannic Acid as a Reagent . . . .THORNER (W.). Apparatus for Collecting and Analysing the Gases DL-solved in Water . . . . . . . . . . .MAYREOFER. Estimation of Nitric Acid in Potable Water . . . .SCHWACKHOFER (I!.). Calorimetric Estimation of Fuels . . . .FERRARI (I).). Detection of Sulphuric Acid in Wine . . . . .ULBEICHT (R.). 71 ine Analysis . . . . . . . . ,SIEBOLD (L.). Estimation of Hydroeyanic Acid . . . . . .MOHR (C.).Estimation of Reverted Phosphoric Acid . . .PAUE59769759859859969960060060060060160260260260260360360360460460560660660860860860960961061061061 161168768768868868868868968968969069069069069169169169169269CONTENTS .PETER (J.). Determination of Non-volatile Residue in Wine . . .MEDICUS . Detection of Saccharose in Wine . . . . . .BATTUT (L.). Estimation of Sugars and Glucoses . . . . .CASAMAJOR (P.). The 4 Method of Sugar Analysis . . . . .SIEBEN (J.). Composition of Starch Syrup and of Honey . . . .PCHMOQEB (M.). Polarimetric Estimation of Sugar in Milk . . .SACHS (I?.) and R . DE BARBIERI . Influence of the Lead Precipikhte onPolarisation .. . . . . . . . . . .Trannin's New Saccharimeter . . . . . . . . .IHL (A.). Phenols as Reagents for Carbohydrates . . . . .CASALI . Detection of Chloral . . . . . . . . .LIEBERMANN (L.). Estimation of Milk-fat . . . . . . .ZANNI (J.). Tests for Butter . . . . . . . . .HORSLEY (J.). Tests for Butter and Butterine . . . . . .VALENTA (E.). Toilet Soap Analysis . . . . . . . .HEPPE (G.). Testing Oil of Cassia . . . . . . . .RAWSON (C.). Valuation of Indigoes . . . . . . . .MAYER (A.). Valuation of Hay by Chemical Analysis . . . .BECKTJRTS (H.). Separation of Alkalofds in Forensic Analysis . . .LENZ (W.). Pepper Fowder . . . . . . . . .MULLER (W.). .BRAUN (H.). Titration of Carbamide with Mercuric Nitrate . . .WOLLNY (R.). Analytical Operations and Apparatus .. . . .LOWE (J.). €Tse of Lime-water in Zinc Gasometers . . . . .GAWALOVSKI (A.). Bottles for Reagents . . . . . . .G~AWALOVSKI (A.). New Form of Burette . . . . . . .THRESH (J . C.). New Form of Apparatus for Continuous Percolation withBoiling Liquids . . . . . . . . . . .LONG (J . H.). PhenolphthaleYn as an Indicator . . . . . .KRUSS ((3.). Quantitative Spectrum Analysis . . . . . .ARNOLD (C.). Estimation of Chlorides in Urine . . . . . .BERQLUND (E.). Vortmann's Method for Estimating Chlorine in thePresecce of Bromine . . . . . . . . . .BERQLUND (E.). Separation of Chlorine and Bromine . . . . .PFORDTEN (0 . v . D.) . New Reagent for the Absorption of Oxygen .DIVERS (E.) and T . SHIMIDZU . Use of Sulphuric Acid to Oxidise MetallicSulphides in Analysis .. . . . . . . . .ARNOLD (0.). Estimation of Nitrogen . . . . . . . .WXLFARTH (H.) . Modifioation of Kieldahl's Method of Estimating NitrogenBOSSHARD (E.). Kjeldahl's Method of Estimating Nitrogen . . .GLASER (C.). Estimation of Phosphoric Acid . . . . . .PETERMANN (A.) and C . GLASER . Estimation of Reverted Phosphoric Acid .GLASER ((2.). Estimation of Reverted Phosphoric Acid by the OxalateQIICOMO (C.). Detection of Sugar in Urine . . . . .SPIET~HOFF (H.). Chemistry of Urine . . . . . . . . .Estimation of Dextrose in Urine by the Polarimeten ..xlixPAGE69269369369369369369469469469569569569669669769'7609701701702702702703835835835835835835835835836836836836837837837837837Method. .. . . . . . . . . . . .AUDOUARD . Analyses of Phosphatic Manures . . . .WARTHA (V.). Alkaline Reaction of Glass . . . . .LUNDIN (E.). .HAGER (H.). Detection of Arsenic in Presence of Antimony .BERGLUND (E.). Separation of Tin. Antimony, and Arsenic .BENAS (T.). Volumetric Determination of Tin . . . .RAIMOND (E.). Volumetric Estimation of Manganese . .LINOSSIER (G.). Volumetric Estimation of Iron . . . .ILINSKI (M.) and G . v . KNORRE .SCHNEIDER (L.) and I? . LIPP . Analyses of Tungsten Steel. . .PETIT (A.). Titration of Organic Matter in Watw . . .GUNNING (J . W.). Examination of Potable Water . . .UNGEB (B.). Analysis of Vulcanised CaoutcBouc . . .FREYERY (J .L . DE) . Analysis of Two Californian Wines . .Estimation of Arsenic in Iron and Eon OresSeparation of Nickel and'GobaltVOL . XLF'III .. . 838 . . 838 . . 838 . . 838 . . 838 . . 839 . . 839 . . 840 . . 840 . . 840 . . 840 . . 841 . . 841 . . 841 . . %21 COXTENTS .EGGER (E.). Testing Wine for added Water . . . . . .DYMOND (T . S.). .PELLET (H.). Direct Estimation of Sugar in Beet . . . . .LECHARTIER (G.). Application of the Demimeter to Cider Must . .OLIVIERI (V.). Estimation of Tartaric Acid in Wine Lees . . . .MANN (C.). Test for Citric Acid . . . . . . . . .DUBOIS (C.) and L . PAD& Natural Fats . . . . . . .A . v . T . . . . . . . .PICKERING (S . U.). Estimation of Oil in Cattle Cake . . . . .SHIMOYAMA (Y.). Estimation of the Quinine Alkalo’ids .. . .HOPPE-SEYLER (I?.). Separation of Case‘in from Albumin . . . .JOHNSON ((3.). Tests for Albumin in Urine . . . . . .NIKITINSPP (T.). Determination of the Quantity of Ash in Tea . .DABNEY (C . W.) and B . TON HERFF . Determination of Nitrogen by theCopper Oxide Method, &c . . . . . . . . . .JOKJLIE (H.). Estimation of Phosphoric Acid in Commercial Products .HAMMARSTEN (0.). Determination of Sulphur in Prote‘ids . . . .ENQEL (R.) and J . VILLE . Estimation of Hydroxides in Presence of Car-bonates . . . . . . . . . . . . .L~GER (E.). Phenolphthale’in as an Indicator . . . . . .DRAPER (H . N.). .HAMPE (W.). Separation of Zinc from Metals of the same Group . .HEMPEL (W.). Titration of Iron Ores . . . . . . ..CLASSEN (4.) and R . LUDWTQ . .Estimation of Ethyl Nitrite in Spirit of Nitrous EtherBKJCHNBR (G.). Detection of Sugar in Urine . . . . . .REMPEL (R.). Apparatus for the Estimation of Starch . . . .GAWALOVSKI (A.). S o a ~ Analysis . . . . . . .Estimation of Butter in CreamPOOL (F . V.). New Dropping Flask . . . . . . . .ARNOLD (C.). Kjeldahl‘s Method of Nitrogen Estimation . . . .MOULTON (C . W.). Estimation of Nitric Acid . . . . . .Lakmo’id and Carminic Acids as Reagents for AlkalisQuantitative Analysis by Electrolysis .JACQUEMIN (G.). Estimation of Cyanogen in Gaseous Mixtures . . .VITALI and TORNANI . Detection of Chloral Hydrate . . . . .PLUCKIQER (F . A.). Testing Oil of Roses . . . . . . .HINSBERG (0.). Reagent for Aromatic Diamines .. . . .RAU (H . M.). Indigo Testing . . . . . . . . .BECKER (F.). Estimatinn of Tannin . . . . . . . .SCHULZE (E.). Determination of Asparagine and Gtlutamine . . .SCHIMOYAMA (Y.). Estimation of Quinine . . . . . . .KOHNSTEIN (B.). Determination of Free Sulphuric Acid in Vinegar . .HEINER ((3.). Estimation of Resin in Soap . . . . . . .ULBETCHT (R.).KOHNSTEIN (B.) and F . SIMAND . Determination of the Free Acids conEstimation of Tannins by Lowenthal’s Method . . .tained in Tannin Liquor . . . . . . . . .FRENZEL (J.) and T . WEYL . .MORSE (H . N.). Apparatus for the Correct Reading of Gas Volumes overWater . . . . . . . . . . . . .SCHNEIDER (R.). Precipitation of Halogen Salts of Silver . . . .KINNICUTT (L . P.) and H . C .SWEETSER . Schulze’s Process for the Determi-HAGER (H.) . Reactions for Distinguishing Chlorides, Bromides, and Iodideswhen Mixed Together . . . . . . . . . .CARLES (P.). Titration of Potassium Iodide . . . . . .FALI~RES (E.). Titration of Potassium Iodide . . . . . .HUFSCHMIDT (F.). Volumetric Estimation of Nitrogen . . . .HOUZEAKJ (A.). Estimation of Nitrogen . . . . . . .EYSTER (G . H.). Qualitatire Determination of the Bases without HydrogenSulpliide . . . . . . . . . . . .DECHAN (M.). Gallei’n as an Indicator . . . . . . . .BELL (L.). Spectroscopic Determination of Lithium . . . . .MORSE (H . N.). Deterniintltion of the Value of Zinc-dust . . . .Determination of Case‘in in Cows’ Milk .nation of the Halogens in Aromatic Compounds .. . . .PAGE84284284284284384384384384484484484484584584584593093093093093193193193193193293293293393393393393493493493493493593593593610101010101010101011101110111011101210121012101CONTENTS . liPAQEB ~ H A L (A.). Separation of Copper and Cadmium . . ’ . . 1012S M I T ~ (J . L.). Methods of Estimating Columbates containing EarthyOxides . . . . . . . . . . . . . 1012XBUSS ((3.). Standardising Solutions of Potassium Permanganate . . 101310131013CAXTER (0 . C . S.). Delicate Test for Antimony . . . . . .RIDEAL (S.). Delicate Test for Antimony, Arsenic, and Tin . . . .Ether. Brc . . . . . . . . . . . . . 1013DOTT (D . B.). Estimation of Spirit of Nitrous Ether .. . . .MCEWAN (P.). Detection of Phenol i n Creasote . . . . . . 1013KRUIS (C.). Reducing Power of Certain Sugars . . . . . . 1013FREAR (W.). The Time Element in Gluten Determinations . . . 1014BLAIR (A . A.). Valuation of Acetate of Lime . . . . . . 1014ALLEN (A . H.). Estimation of Ethyl Nitrite in Spirit of Nitrous1013TRIES (H . DE) . Estimibtion of the Combined Acids in Plant Sap . . 1014MOORE (R . W.). Hubl’s Method for the Examination of Oils and Fsts . 1014GEISSLER (E.). Estimation of Fat in Milk . . . . . . . 1014LAFON (P.). New Reaction of Digitaline . . . . . . . 1014KERT~SZ (A) . 1015RAWSON ((2.). Indigo Testing . . . . . . . . . 1015CRIPPS (R . A.) and T . S . DYMOFD . Detection of Aloes in Mixtures .. 1015HOPPE-SBPLER (F.). 1015HEMPEL (W.). Percentage of Oxygen in ttte Air . . . . . 1091LONGCI (A.). Estimation of Nitrogen in Saps, &c . . . . . . 1092GRANDVAL (A.) and H . LAJOUX .in the Air, Water, Soils, &c . . . . . . . : . . 1093AUBIN (E.). Estimation of Phosphoric Acid . . . . . . 1093CARNOT (A.) and P . M . PROROMANT . Estimation of Cadmium . . . 1094CLASSEN (A) . Quantitative Analjsis by Electrolysis . . . . . 1094LAFON (P.). New Reaction for Cod&e . . . . . . . 1095Laboratory Apparatus for the Production of Uniform Temperatures . . 1157G‘ASAMAJOR (I?.). Silver Iodide as a Blowpipe Reageut . . . . 1157THOMSON (R . ‘J!.). Lalimo’id and other Indicators . . . . . 1157FISCHER is.) and 0 . PHILKPP .Alkalime try . .. . . . . . . . . . 1159KLOBUEOW (N . v.). Volumetric Estimation of Sulphur . . . . 1159Examination of Iron and Steel . . . . . . . . . 1160TUENER (T.). 1161P~TER (J.j. 1161LUNGE (G.).1162CHARPENTIER (P.). Valuation of Manganese Peroxide . . . . 1162ZULEOWSKY (C.). Estimation of the Halogens iri Organic Compounds . . 1162HEPPE ((3.). Adulteration of Lemon Oil with Oil of Turpentine . . 1163PELLET (H.). Simple Estimation of Sugar in Beet . . . . . 1163GIRARD (C.).the Municipal Laboratory in Paris . . . . . . . 1169SONNENSCHEIN (A.). Behaviour of Tannin with Felaling’s Solution . . 1163BERTHELOT and ANDRB . Oxalic AcidinYlants . . . . . . 1164WILM (V.). Estimation of Fat in Palm-nut Meal . . . . . 1164FLUCKIGER (F . A.). Estimation of Morphine in Opium .. . . 1165EHBENBERQ (A.). Analmis of Gases by Combustion . . . . . 1261TEED (F . L.). Estimatiin of Iodides in Presence of Bromides and Chlorides 1261REINHARDT (C.). Modified Kipp’s Hydrogen Sulphide Apparatus . . 1261WARINGCTON (R.). Behaviour of Nitrates in Kjeldahl’s Method for theDetermination of fiitrogen . . . . . . . . . 1261DUBERNARD . Volumetric Estimation of Potassium . . . . . 1262QUANTIN . Determination of Soluble Potash in Soils . . . . . 1262ROTTQER (F.) and H . PRECHT .of Yotasaium Chloride . . . . . . . . . . 1263Detection of Magentain Extract of Archil . . . .Separation of Case’in from Albumin in Human Milk .Detection and Estimation of n’itric AcidDimethylamidoazobenzene as Indicator inEstimation of Carbon in Iron and Steel .. . . .Estimation of Sulphur in Steel and Iran . . . . .Kstimation of Potassium Permanganate and of Pjrolusite byMeans of Hydrogen Peroxide . . . . . . . . .Estimation of Sugar by Fehling’s Solution, as conducted a tPhotometry . . . . . . . . . . . . . 1260Estimation of Sodium Chloride in Presenclii CONTENTS .PAGEBLOXAM (C . L.). -Detection of Iron. Aluminium. &c . . . . . . 1264Estimation. of Manganese . . . . . . . . . . 1264GOOCH (F . A.). 'Separation of Titanium from Aluminium and Iron . . 1265LEPsrns (B.). Dissolved Oxygen in Deep-well Waters . . . . . 1266WARDEN (C . J . H.). Biological Examination of Water . . . . 1266LACH (B.). Valuation of Ozokerite . . . . . . . . 1266WEINREB (C.) and S . BONDI .Titration of Phenol with Bromine . . 1266Determination of the Strength of 'Vinegar and Acetic Acid . . . . 1267HASLAM (A . R.). Action of Lime on Quinine . . . . . . 1267LUNGE (G.). Modscation of the Nitrometer for Use as a Ureometer, &c . . 1267Technical Chemistry .CPIANDI.BEY . Antiseptic Pxoperties of Carbon Bisulphide . . . 9'1Preparation of Potassium Magnesium Sulphate . . . . . . 98Manufacture of Aluminium . . . . . . . . . . 98Utilisation of Zinciferom Burnt Pyxites . . . . . . . 98JUNGCK (M.). The Siemens-Martin Process . . . . . . 98ABCRE (A.) and C . HASSACK . Analysis of aome Indian Bronzes and theirPatina . . . . . . . . . . . .CHEMIN (C . 0.). Process for Bleaching Ozokerite . . . .HOLZAPFEL (J.). Dari as 8 Source of Alcohol .. . . .JACOBSEN (J . C.). Degeneration of Yeast . . . . . .WIETERSHEIW and others . Loss of Sugar in Beetroots when Stored .LIPPMANN (E.) v . and others . Preparatisn of Sugar from Molasses .GANS (J.). Purification of Molasses . . . . . . .Extracting Sugar from Molasses . . . . . . . .ENDEMANN (H.). Formation of Grape Sugar from Starch . . .GORING (T.). Preparation of Concentrated Acetic Acid . . .FLEISCEMANN (W.). .LIEBSCHER . Bitter Milk . . . . . . . . .SCHRODT (M.). Quality of Butter made by different Processes . .Preparation of Quinaldine . . . . . . . . .DELORY . DSeing with Alzarin Cdaurs on Indigo-blue Cloth . .SCHEURER (A.). History of Alzarin-blue . . . . . .GOPPELSROEDER (F.) .LONGMORE (J.). Preparation of a Dyeduff' from Cotton-seed Oil .CECH (C .0.). Manufacture of Santonin in Turkestan . . .C . Thiel's Pasteurising Apparatus for Milk .Preparation .of Persulphocyanogen by ElectrolysisLAUBER (E.).GOPPELSROEDER (F.) . Bleaching Indigo-blue and Turkey-red by Electro-chemical Means . . . . . . . . . . .LUEGER . Clarification of Turbid River Water . . . . . .GRUBER (0 . v.). Preparation of Sulphuric Anhydride from Nitrosyl Sul-phate . . . . . . . . . . . . .SCEEURER.KESTNER . Composition of the Gases produced in the Combustionof Pyrites . . . . . . . . . . . .MOND (L.). Recovery of Hydrochloric Acid as Bye-product in the Ammonia-Poila Process . . . . . . . . . . . .Consumption of Fuel in Blast Furnaces . . . . . . .MANHBS (P.). . . .MARQUARD (G.). Japanese Bronzes .. . . . . . .Nitrogenous Contents of American Beers . . . . . . .ROMMIER (A.). Cultivated Wine Yeast . . . . . . .DEBPEISSIS (L . H.). Treatment of Syrups by Electricity . . . .PELLET (H.). Animal Charcoal in Sugar-refining . . . . .CUISJNER (L.). Manufacture of Maltose by Dubrunfaut's Method . .BARKER (G . F.) and others . Report on Qlucose . . . . . .ROSE (B.) and E . SCHULZE . Some Constituents of Emmenthaler Cheese .PRUDEOMME . Action of Bisulphites on Chlorates . . . . ." Red Spots " in Light Rose Dye . . . . .Extraction of Nickel and Cobalt from its Ores199200204204204205205205205206207207. 100 . 101 . 102 . 102 . 102 . 102 . 103 . 103 . 104 . 105 . 105 . 105 . 105 . 106 . 106 . 106 .107 . 108 . 108 . 10810819819919CONTENTS . liiiKOECHLIN (H.). New Chrome-mordanting Process . . . . .Preparation of the Sulphonic Acids of Methyl VioletCLAW (C . I?.). Recovery of Sulphur from Hydrogen SulphideMENZIES (W . J.). Purification of Sulphuric Acid . . . . .GOPPELSROEDER (F.) . Formation of Hydroxy- and Chloro-cellulose Electro-chemically . . . . . . . . . . . . . . . . . . . .BEILBY (G.) . Preparation of Ammonia from Nitrogenous Minerals . .TORSTEB and GRUNEBERG . Working up the Mother-liquors from SchoeniteLE CHATELIER (H.). Chemical Reactions in the Setting of HydraulicMortars . . . . . . . . . . . . .LAUTE (C.). Moulding of Porcelain . . . . . . . . SCHWARZ (C.). Roman Alunite . . . . . . . . .L’HOTE . Purification of Zinc containing Arsenic .. . . .GAUTIER (F.). Manganese Steel . . . . . . . .STEINER (E.). Formation of Patina . . . . . . . .DIETRICH (E.). Manufacture of Asphalt . . . . . . .JAY . A Substance Employed to Colour Wines . . . . . .Separation of Soap from the Leys by Centrifugal MeansPreparakion of Malleable Nickel and CobaIt . . . . . . .MULLER (X.). Weiller’s Silicon Bronze . . . . . . .ROTE (L.) . Process for Solidifying Mineral Oils . . . . . .SCHMITT (E.). Composition of Butter from Cow’s, Goat’s, and Ewe’s MilkMACHENHAUER (F.). Preparation of a Yellow Rosaniline Dye . . .Preparation of New Colouring Matters . . . . . . .Benzaldehyde-green . . . . . . . . . . .Preparation of Dyes from Alizarin and other Anthracene Colouring MattersLAXDSHOFP (L.).Preparation of Naphthylamine Compounds . . .Preparation cjf Naphthol-green . . . . . . . . .MULLER-JACOBS (A.). Turkey-red Oil . . . . . . .SCHMID (H.). Turkey-red Oil . . . . . . . . .LIECHTI (L.) and W . SUIDA . Composition of Turkey-red Oil . . .LIECHTI (L.) and W . SUIDA . Behaviour of Different Ferric Oxide Mordantswith Silk . . . . . . . . . . . .GACON (A.). Blasting Powder . . . . . . . . .HERRE (W.). Preparation of Waterproof and Incombustible Paper . .SPONNAQEL (3’. (3.). Enamelling Casks . . . . . . .SCHMELCK (L.). Investigation of Petroleum Lamps . . . . .TENABLE (F . P.). Zinc in Drinking Water . . . . . . .FISCHER (E.). Naphthalene as an Insecticide . . . . . . .ANDEER (J.). Phloroglucinol as an Antiseptic .. . . . .LUNGE (G.). Recovery of Sulphur from Hydrogen Sulphide . . .Methodsfor obtaining Phosphates . . . . . . . .Progress made in the Soda Industry . . . . . . . .MOODY (W.). Celestine . . . . . . . . . .REUSS (C.). Density of Solutions of Pure and Commercial Aluminium Sul-EWER (E.). Action ol! Dilite Acids on Boitle Glass . . . . .Gilding Earthenware Goods . . . . . . . . . .IWABUCHI (K.). Japanese Materials for the Manufacture of Ultramarine .PITKIN (L.). Action of Concentrated Sulphuric Acid on Lead and itsAlloys . . . . . . . . . . . . .Proportion of Cadmium in Zinc-dust . . . . . . . .STOLBA (F.). Preparation of Zinc free from Arsenic . . . . .Manufacture of Metallic Alloys . . . . . . . . .Preparation of Malleable Ferronickel and Ferrocobalt .. . . .BOOTH (J . C.). Toughening Gold, Silver, dtc., in the Crucible . . .PERRY (N . W.). Fusion, Casting, Dephosphorising, and Plating of IridiumGALLOWAY (W.). Influence of Coal-dust in Colliery Explosions . . .DUEIN . Recovery of Paraffln and Heavy Oils from Petroleum-residues .. . . .Suitable for Calico Printing . . . . . . . . .phate . . . . . . . .d 2PAQR20820820830430430430630630730730730730830830830930930930931031031031131231231231331331531531531531645245345445445445445545845845945946046046146146146146246246346liv CONTENTS .Preparation of Iodoform. Bromoform. and Chloroform . . . . .NOLTING (E.). Presence of Isocyanates in the First Runnings of the Distilla-tion of Crude Benzene .. . . . . . . . .REBOUX (E.). Manufacture of Sugar without Bye-products . . .BURY and 0 . PROTIUS . . . .DEHBRAIN (P . P.). Butyric Fermentation in the Diffusion Vessels of SugarFactories . . . . . . . . . . . .Potassio-antimonic Oxalate. a Substitute for Tartar Emetic . . . .DE PITTEURS . Molecular Modifications of Silver Bromide . . . .CAREY LEA (M.). .LOHSIE (0.). Isochromatic Gelatin Plates . . . . . . .PAVLOFFXKI (V.). Transferring Photographs to Porcelain or Wood . .REICHARDT (E.) . Drinking Water Supplies . . . . . . .RATIMOPF . Antiseptics . . . . . . . . . . .VIGIER (F.). Orthophenolsulphonic Acid, a New Antiseptic . . .SCHRODT (M.). New Conserving Agent for Milk and Butter .. .CAZENEUVE (P.). Preparation of Nitrous Oxide . . . . . .BLATTNER (G.). Decomposition of Ammonium Sulphate by means of SodiumSulphate . . . . . . . . . . . . .LOFASZ (J . F.). Separation of Kainite from Rock Salt . . . . .BROUVEN (H.). Recovery of Sulphur from Soda Waste . . . .HASENCLEVER (R.). Manufacture of Phosphate from Basic Slags . .PHILLIPS (W . B.). Reversion of Phosphoric Acid by Heat . . . .FRESENIUS (R . and W.). Portland Cement and its Adulteration . . .BOOTH (J . C.). Graphite Crucibles . . . . . . . .JAMES (F . L.). Deposition of Silver on Glass . . . . . .LEDEBUR (A.). Crucible Steel . . . . . . . . .HILGENSTOCK (G.). Phosphorus in the Blast Furnace . . . .BEHREND (P.). Changes occurring in Barley during Xalting .. .SENFF (M.). Dry Distillation of Wood . . . . . . .POETSCH (W.). Recovering the Waste Acids from Nitroglycerol Works .HIRSCHSOHN (E.). Siamese Benzoih . . . . . . . .BRUNIG (A.). Yield of Butter from Fresh and Stale Cream . . . .ROSSMASSLER ( F . A.) . Manufacture of Lubricating Oil from Baku Naphtha .Purree or Indian Yellow . . . . . . . . . .ROUSSEAU (L.). Flesh Meal . . . . . . . . . .EDER (J . M.). Behaviour of the Halo’id Compounds of Silver to the SolarNew Process of Extraction of BeetCombinations of Silver Salts with Colouring MattersSAARE (0.) and others . Preparation and Investigation of Starch . . .PAGE46346346446446446461161161261261261261261261361361461461 5615616616616616616617618619619620620620620620Spectrum .. . . . . . . . . .FLECK (H.). Oxidation of Ammonia in Spring Water . . .LAUJORROIS . Potassium Dichromate as an Antiseptic . . . .SCHMIDT (A.). Water Vapour in Gas Generators . . . .SOLVAY (E.) . Obtaining Hydrochloric Acid from Calcium Chloride .SCHEUREB.KESTNER . Composition of the Gas from Pyrites Burners .JULIE . Method of Hardening Plaster . . . . . . .Improvements in Metallurgy . . . . . . . . .HAXLAM (A . R.). .QUTZKOW (F.). .MENDEL~EFF . Distillation of American Petroleum . . . .TiuNaE (G.), V . MEYER, and E . SCHULZE . .BATTUT (L.) . Sulphurous Anhydride in Sugar Refining . . .FROMENTIN (A.) and MANOURY . Recovery of Beet-juice by Lime, &c .SCHMITT (R.).Preparation of Salicylic Acid . . . . .BAKKER (Ji . P.). Tengkawang Bat or Vegetable Tallow . . .JOBST (J . v.). Preparation and Utilisation of Grape-seed Oil . .MARG~ARY (L.). Synthesis of Dyes on Tissues . . . . .Preparation of Violet Colouring Matters . . . . . .JAY . Vinicolore . . . . . . . . . . .Obtaining Iodine in Peru . . . . . . . . .Volatilisation of Zinc from German Silver AIloysReynolds’ Process for Parting Bold from Bars .Fuse1 Oil in Spirit .Bleaching Tallow . . . . . . . . . . .. 703 . 704 . 704 . 705 . 705706 . 706 . 707 . 707 . 707 . 708 . 708 . 708 . 709 . 709 . 909 . 710 . 710 . 710 . 710 . 711 . 91CONTENTS .SCHEURER (A.). Dyeing with Alizarin on Indigo . . . . .HACQ (G.) and C . HOFFMANN . . . .ROTHER (R.). Bismuth and Pepsin .. . . . . . .NATTOX . Eola Nuts, Sterczclia Aczcminata . . . . . . .VOQEL (H . W.). Modifications of dilver Bromide . . . . .ENICH (F.). Natural Purification of Waters . . . . . .FISCHER (B.) and B . PROSKAUER . Disinfection with Chlorine and BromineWACHTEL (G.). Manufacture of Potassium Dichromate . . . .WITTING (F.) . Chilian Boronatrocalcite . . . . . . .KNAPP (F.). Preparation of Ultramarine Blue from Silica . . . .SCHEURER.~~ESTNER . .TROBACH (E.). New Method of Sugar Extract. ion . . . . .KUNZ (J.). Manufacture of Milk-sugar in Switzerland . . . .FLEISCHMANN (W.). Notes on Milk . . . . . . . .VIETH (P.). Composition of Mares’ Milk m d Eoumiss . . . .KAXNITZER (I.). Medicinal Properties of the Root Bark of the Pome-granate . . . . . . . . . . . . .Preparing Yellow Azo-colouring Matters . . . . . . .MULLER (H.). Preparation of Indigo . . . . . . . .KONIG (J.). Inrestfigation of Bone-meal . . . . . . .BAUER (M.), L . BROUAED, and 6 . ANCEL . . . .Harmless Soldering Mixture . . . . . . . . . .EDER (J . M.). Behariour of the HaloYd Salts of Silver in the SolarSpectrum . . . . . . . . . . . .AUSTEN ( P . T.) and F . A . WILBEB . Purification of Drinking Water byAlum . . . . . . . . . . . . .LUNGE (G.). Reducing Action of Coke on Nitric Acid . . . .Obtaining Sulphur from Hydrogen Sulphide . . . . . .CLAUS (C . F.). Manufacture of Strontium Hydroxide . . . . .TSCHEUSCHNER (E.). Calculation of Glass Batches . . . . .Q-RAETZEL . Preparation of Magnesium . . . . . . .Novelties in Metallurgy . . . . . . . . . .SCH~CHTERMANN (H.). Working up Bask Slag . . . . . .Application of Electricity in Chemical Industry . . . . . .FISCHER (F.). Electrolytic Praduction of Metals and Chlorine . . .Production of Platinum in Russia . . . . . . . .BARTH (N.). Specific Influence of Acetic Acid on the Fermentation ofMust . . . . . . . . . . . . .BARTH (M.). Abnormal Fermentation under Unfavourable Circumstances .HACCIUS (C.). Kephir . . . . . . . . . .DAIX and POSSOZ . Extraction of Sugar from Molasses . . . .MARKOWNIKOFF (V.) . Turkestan Manna . . . . . . .Preparation of Organic Anhydrides . . . . . . . .FLEISCHMANN (W.) and J . BEBENDEB . Creaming of Milk . . . .EICHBAUM (F.). Preparation of Cheap Toilet Soaps . . . . .EICHBAUM (F.). Curd Soaps . . . . . . . . .Preparation of New Colouring Matters . . . . . . . .WITT (0 . N.). Xew Series of Dyes . . . . . . . .REBER ((2.). Fixing Artificial Dyes by Ferro- and Ferri-cyanides . .COUNCLER (C.) and others . Tannin-yielding Substances and their Appli-cation . . . . . . . . . . . . .DUGQAN (J . R.). Relation of Antiseptic Power to Chemical Constitution .SERRANT (E.). Orthohydroxybeuzenesulphonic Acid . . . . .JOHNSON (J . (3.). Poisoning by Canned Goods . . . . . .WELDON (W.1. Preparation of Chlorine from Magnesium Oxychloride .TAQUET ((3.). PreDaration of Chlorine . . . . . . . .ANDBS (L . E.) . Preparation of Wood Stains in the Solid Form . . .A Substitute for CaoutchoucBOTTGER . Silvering of Glass . . . . . . . .Heat of Combustion of the Coal of Ronchamp .GURKE (0.). Preparation of Galkin . . . . . . .Vegetable LeakherNovelties in Explosives . . . . . . . .lvPAQ E711$1171271271284684684684684684784784884884884984985085085083085185185285293693693693793793794094094094094194294294294294394394394494494!49449459469461016101610161016. . . . . 1017 . . lvi CONTENTS .FELUNANN (A.) . Preparation of Ammonia . . . . . . .KEMP (W . J.). Decomposition of Soda Waste hy Means of CarbouicAnhydride . . . . . . . . . . . .NOBEL (A . B.) and C . FEHRENBACH . Preparation of Sulphuric Anhydride .WILLIAM-s (W . J.). Treatment of “Redonda” Phosphate . . . .Xecovery of Sulphur from Alkali Waste . . . . . . .WEINREB (C.). Cryolite Glass . . . . . . . . .KOSXANN . Clays . . . . . . . . . . . .HERZOG (&I.). Silvering of Glnss and Mirrors . . . . . .Natural Gas . . . . . . . . . . . . .SCEEURER.KESTNER . Colnposibion of Heat of Combustion of Coal fromRuhr . . . . . . . . . . . . .JUNEMANN . Manufacture of Sugar and Purification of Beet-juice by Meansof Magnesia and Alumina . . . . . . . . .KOHLRAUSCH (0.). Preparation of Sugar from Sorghum sacchamtuna .R~CHARDSON (C.) . Chemical Composition of the Products of Roller MillingSIEWART (M.). Creaming by Cenhifugals on Various Systems . . .WUST and KIRCHNER . Oberbockstruck’s Milk Refrigerator . . . .DAVIES (R . H.). Three Chinese Fixed Oils . . . . . . .HOLMES (E . M.). Japanese Oils . . . . . . . . .SEEMAN (B.). Preparation of Soaps from Oil Seeds . . . . .Preparation of Thallin . . . . . . . . . . .COSTOBADIE (H . A.), Goods Psinted with Artificial Indigo . . . .WITT (0 . N.), . . .KAYSER (R.). Caseiin Glue, a Substitute for Gum Arabic . . . .NOLTINQ (E.) and 0 . N . WITT . Liquid Bje-product in the Preparation ofDinitrotoluene . . . . . . . . . . .New Colouring Matters . . . . . . . . . . .COLLIN~II~ BENOIST . Reducing Vat for Indigo . . . . . .DALIYIOX (J.). Arbutin . . . . . . . . . .Manufacture of Cellulo’id . . . . . . . . . .Utilisation of Coal Gas for IIeating and Cooking PurposesSERRANT (E.). Aseptol . . . . . . . . . .SCHLOESING (T.) . Magnesia Industry . . . . . . . .MULLEE and others . Progress in Metallurgy . . . . . .HANSEN (E . C.).MARCKER (M.). Frot. hy Fermentation . . . . . . .MARCKER (M.). Properties of Malting Barley . . . . . .Progress in Brewing . . . . . . . . . . .EHRENSTEIN (S . v.). Lime in the Separation of Beet Juice . . . .HUEPPE (F.) and others . Lactic Ferment in Milk . . . . .HUEPPE (F.) and W . EUOLING . Blue Milk . . . . . .EUGLING (W.). Melted Butter . . . . . . . . .Preparation of Violet Dyes . . . . . . . . . .Azo-colours . . . . . . . . . . . . .Use of Magnesium for Bengal LightsSMITH (A.). Preparation of Carbons for Electric Lamps . . . .Electric Accumulators . . . . . . . . . . .MULLER (A.). Filtration of Sewage through Peat . . . . .Nanufacture of Chlorine from Calcium ChlorideCAREY (E.) and F . HURTER . Preparation of Ammonia from AmmoniumSulphate . . . . . . . . . . . . .MULLEB (H.). Prepmation of Potassium Sulphate . . . . .LARKIN (T.). New “ Sulphate” Furnace . . . . . . .Improi ements in the Soda IndustryTannin Method of Fixing Colours on Cotton. . . .SCHEURER.KESTNER . The Eniploynient of Korting’s Apparatus for ForcingGases through Sulphuric Acid Chambers . . . . . .Alcoholic Ferments . . . . . . . .A New Alcoholic Ferment which does not Invert Sugar TEIXBIRA (J . F.).DEUENER (P.) and J . LACE .HEEPPE (F.) and W . EEGLINQ .Treatment of Animal Charcoal . . .. . . . Preservation of Milk. . . . . . . .. . . . . .. . . . . . . .PAGE101710171017101810181019102010201020102010211021102110221022102210231023102310231024102410951095109610961096116611661166116611671168116811681169116911701170117011701171117111711172117212671268126812681268126812G8126CdNTEWTS . lviiMEBUS (E . 8.) and J . W . DECASTRO . Preparation of Strontium Carbonate .HASSACK (C.). Behaviour of Basic Copper Carbonate with NascentGLASER (F . C.). Manufacture of Zinc Oxide . . . . . .Hydrogen . . . . . . . . . . . .BECKER (F.). Aluminium Sulphate . . . . . . . .Improvements in Metallurgy . . . . . . . . . . HONIGMANN (M.). .LAUBER (E.) and C . WEINREB . Chromium Chlorate . . . . .HUNTINGTON (A . K.). Preparation of Tungatic Acid . . . . .BERNREUTHEP (0.). Steeping of Barley . . . . . . .AUBERT (L.) and V . GIRARD . .Preparation of Tetrachlorophthalic Acid . . . . . . .ROTONDI . Saponification of Fats by Electricity . . . . . .LACH (B.). Treating Vegetable Tallow . . . . . . . .Cultivation of the Star Anise Tree and the Preparation of the Oil in AnnamNew Coal Tar Colouring Matters . . . . . . . . .ZURCHER (K.). Formation of Aniline Black . . . . . .JACQUET (E.). Use of Antimony Oxalate in Printing . . . . .SCHEUREB (A.). .Producing a Coating of Ferrosoferric Oxide on IronThe Sorghum Sugar Industry in the United States . . . .Manufacture of Cane-sugar from StarchFixation of Alumina as a Discharge on Indigo Blue .PAGE126912701270127112711271127212721273127312741274127412751275127512761276127

ISSN:0368-1769    

DOI:10.1039/CA88548FP001

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

14 ABSTRACTS OF CHEhIICAIi PAPERS.In o r g a n i c C h e mi s t r y .Dispersion-equivalent of the Diamond. By A. SCHRAUF(Ann. Phys. Chern., 22, 4 2 6 4 2 9 ) .-The dispersion-equivalen t of a,Brazilian diamond, determined by the author, was 0.03286. He dis-cusses the extreme smallness of this number as compared with thesame constant in some series of organic bodies, which show anincrease of its value with increase of the proportion of carbon.XI. R.Liquid Carbonic Oxide. By V. OLSZEWSKI (Compt. rend., 99,706--707).-Carbonic oxide carefully purified from carbonic anhy-dride forms a transparent colourless liquid under pressure between- 139.5" and - 190°, but in a vacuum it solidifies a t - 21 1" to a snow-like mass, if the pressure has been reduced rapidly, but to a compactopaque mass if the pressure has been reduced slowly. If the pressure isreduced so gradually that the liquefied gas does not boil but evaporatesonly from the surface, the liquid forms a transparent solid. Whenthe pressure rises to one atmosphere the solid melts to a colourlessliquid. The following table shows the relation between the pressureand the boiling point of liquid carbonic oxide :-Pressure inatmos.Temp.35.5 - 139.5" (critical point)25.7 - 145.323.4 - 147.721.5 - 148.820.4 - 150.018.1 - 152.0Pressure inatmos. Temp.16.1 - 154.4"14-8 - 155.76-3 - 168.24.6 - 172.61.0 - 190.0Vacuum - 211.0 (solidifies)Although, in the gaseous state, carbonic oxide resembles nitrogen inmany of its properties, the two substances behave somewhat differ-ently a t very low temperatures.The critical point of carbonic oxide,and its boiling point under atmospheric pressure, are several degreeshigher than those of nitrogen. Carbonic oxide solidifies in a vacuum,but a low temperature alone is not sufficient to solidify nitrogen.Moreover, the temperature obtained by the evaporation of liquid car-bonic oxide in a vacuum is higher than that obtained by the evapora-tion of liquid nitrogen under the same conditions. The differenceIX'ORGAK'JC CHEMISTRY 1 5are doubtless due to the presence of a solid element in the carbonicoxide. C. H. B.Phosphorus Trifluoride. By H. MOISSAN (Cm7pt. rend., 99,6jr;-657).-Phosphorus trifluoride is obtained by heating carefullydried copper phosphide with lead fluoride free from silica, in a brasstube, and drying the product over pumice moistened with sulphuricacid.It is a colourless gas which does not liquefy under a pressureof 180 atmos. at 24", but under a pressure of 40 atmos. at -10" formsa colourless very mobile liquid, which does not attack glass. Thesp. gr. of the gas is 3.022 (calculated 3.0775).Phosphorus trifluoride is incombustible when mixed with air, but ex-plodes when it is mixed with b.alf its volume of oxygen and brought incontact with a flame or electric spark. When pure, it does not fumein the air, but it is decomposed slowly in presence of water at theordinary temperature, with formation of hydrofluoric and phosphorousacids, PI?, + 3H,O = H,PO, + 3HTp.When mixed with steam at loo",the decomposition of the fluoride is mnch more rapid. Solutions ofsodium o r potassium hydroxide rapidly absorb the trifluoride, withelevation of temperature and formation of a fluoride and a phosphite.Solutions of barium hydroxide o r potassium carbonate absorb the gasmore slowly. Phosphorus trifluoride is immediately decomposed bysolutions of chromic acid or potassium permangannte, and is instantlyahsorbed by bromine. It is also absorbed by alcohol with developmentof heat, and is not given off again when the liquid is boiled. Whenpassed over boron or silicon at a dnll red heat, it yields boron or siliconfluoride, and it is rapidly decomposed by melted sodium, more slowlgby heated copper. It combines with ammonia gas, forming a verylight, woolly, white compound, which is decomposed by water.When mixed with half its volume of oxygen and subjected t o theaction of an electric spark, phosphorus trifluorids explodes violently,and the compound formed fumes in the air and is instantly absorbedby water with formamtion of phosphoric acid, but no trace of phos-phorous acid.The gas thus produced seemed to be phosphorus ox)--fluoride, PF,O.When heated in contact with glass, phosphorus trifluoride is de-composed with separation of phosphorus and formation of siliconfluoride, and the volume of the silicon fluoride thus formed furnishesa means of estimating the amount of fluorine in the phosphorusfluoride. C. El. B.Phosphorus Chloronitride. By A.W. HOFJIANN (Bey., 17,1909-1912) .-The formula for this body has long been established asP3N3CIS, but Iittle work has been done on the subject. The aut,horhas made experiments to determine whether the chlorine-atoms canbe replaced by other radicals.Aniline dissolves this chloroni tride to a clear solution, which, how-ever, soon solidifies to a, crystalline mass. The principal products area crystalline substance, very sparingly soluble in alcohol, and anamorphous compound, easily soluble. The crystalline substance isbest purified by solution in glacial acid. It yields well-formed needle16 ABSTRACTS OF CHEMICAL PAPERS.melting at 268", a,nd has the formula P3N3(NHPh),.would be expressed by the equation-Its formationP3N3CL + 12NHPh = P,N,(NHPh), + 6NHSPhCl.Paratoluidine yields a similar crystalline compound, melting a t 243".Piperidine acts stron gly with the chloronitride, producing piperidinechloride and an amorphous substance, easily soluble in alcohol, insolu-ble in water.The author is inclined to look upon the group P3N3 as playing animportant part, and to consider that the formula of phospham shouldbe trebled, and would then become P,N,(NHj",. This would beanalogous to an aniline compound, P3N3( NPh)",.The substance,I',N,(NHPh), described above gives off aniline when heated, and leavesa resinous mass, which mag contain the compound, P,N3(NPh) "3.It is also probable that other ammonio-derivatives might be pre-pared somewhat according to the following equations :-3PC& + 3NH3 = P,N,Clp, + 9HC1SPCI, + 9NH3 = P3N,(NH,)6 + 15HC1.3PC15 + 6NH3 = P3N3(WH)", + 15HClL.T. T.Action of Nitric Acid 011 Tellurium. By D. KLEIN and J.MOREL (Compt. rend., 99, 540-542).-Pulverulent tellurium, obtainedby precipitation with sulphurous acid, dissolves readily in dilute nitricacid, with evolution of nitrogen oxides. The temperature at whichsolution takes place is lower the higher the concentration of the acid ;with acid of sp. gr. 1-25 the action begins a t - 11". At a low tem-perature solution is not complete, and a greyish curdy residue is left,which afterwards turns white, and forms long flexible microscopicneedles containing both nitric and telluric acid. The solution,when diluted with water, deposits " tellurous hydrate " or telluronsanhydride, a certain quantity of basic tellurium nitrate (Abstr., 1884,p.1256) always remaining in solution. " Tellurous hydrate " isformed when the nitric acid is dilute (sp. gr. 1.1-1.2) and the actiontakes place a t a low temperature. It is a white curdy substancewhich gradually changes to a yellowish-white mass of microscopicrectangular lamella of tellurous anhydride ; these act strongly onpolarised light. When the reaction takes place a t a higher tempera-ture, or if stronger nitric acid is used, tellurous anhydride is formedi n microscopic quadratic octahedra. The nitric acid solution spon-taneously deposits octahedral crystals of tellurous anhydride, and ifthe nitric acid employed is somewhat dilute (sp.gr. about lee), andthe temperature has not risen above 30" during the reaction, the pre-cipitntion of tellnrons anhydride is accelerated by heat. Under theseconditions, about half the tellurium remains in solution in the form ofnitrate, which crystnllises out when the liquid is concentrated andcooled. When the octahedral crystals of teilurous anhydride areboiled with nitric acid of sp. gr. 1.35, they yield a solution of thebasic nitrate.Tellurous anhydride requires 150,000 parts of water for solution.C. H. BINORGANIC CHEMISTRY. 17Action of Water and Nitric Acid on Basic TelluriumNitrate. By D. KLEIN and J. MOREL (Compt. rend., 99, 567-569).-Basic tellurium nitrate (Abstr., 1884,1256) is slowly decomposed bywater in the cold, nitric acid and a very small quantity of telliirousanhydride being dissolved, whilst tellurous anhydride is left undis-solved in rectangular lamella At a higher temperature, decompositionis almost instantaneous ; the solution becomes strongly acid, and thegreater part of the tlellurous anhydride remains undissolved in theform of microscopic octahedra.These facts explain the commonlyaccepted statement that tellurous anhydride is slightly soluble i nwater, but does not redden blue litmus. Tellurous nitrate does notact on moistened litmus in the cold until after several hours, andwhen decomposition takes place the solution of a small quantity oftellurous anhydride is due to the presence of the free nitric acid.Basic tellurium nitrate dissolves in nitric acid and crystallisesreadily when the solut\ion is concentrated and cooled. It seems to bemuch more soluble in the dilute than in the concentrated acid. Solu-tions in nitric acid of sp.gr. 1.1-1-4 are stable a t all temperatures,and solutions in acid of sp. gr. about 1-35, are not decomposed onaddition of 100 vols. of water. On the other hand, solutions in nitricacid of sp. gr. 1.1 are decomposed by water with precipitation of tel-lurous anhydride, decomposit'ion being more rapid the greater theproportion of water. The limit of decomposition appears to be reachedwhen the solution is mixed with 5 vols. of water; under these con-ditions, the precipitation of tellurous anhydride is very slow, and witha smaller proportion of water no decomposition takes place.Thetellurous anhydride deposited when the nitric acid solutions arediluted, does not crystallise in octahedra, but in some perfectly dis-tinct form.Basic tellurium sulphate, (TeOJ2S0,, decomposes in a similarmanner. C. H. B.Preparation of Potassium Chlorate. By E. K. MCSPRATT andG. ESCHELLMANN (Dingl. polyt. J., 254, 90).-Chlorine is passed intomagnesia mixed with water, and the solution is evaporated to 35-50" B., so that, on cooling, sorne magnesium chloride crystnllises out.The product is now treated with potassium chloride, when potassiumchlorate and magnesium chloride are formed ; the greater portion ofthe former may then be obtained by crystallisation. The mother-liquor, which retains 5-10 per cent. of the total potassium chlorate,is treated with hydrochloric acid and steam, by which potassiumchloride is formed and chlorine is evolved; the latter may be ab-sorbed by lime or magnesia.The solution containing an excess ofacid is now neutrnlised with magnesium carbonate, and a solution ofmagnesium chloride containing potassium chloride is formed. Thisis evaporated to 45" B., and allowed to cool, when it sets. In thisstate, it may go into commerce, or magnesia may be obtained from itby heating, and thi,s can again be employed in the process. J. T.By E. R. MUSPRATT andG. ESCHELLMANN (Dingl. polyt. J., 254, 47).-Chlorine is pused toPreparation of Sodium Chlorate.YOL. XLT~II. 18 ABSTRACTS O F CHEMICAL PAPERS.saturation into water holding magnesia in snspension, so that oneequivalent of magnesium chlorate to 5-54 equivalents of chloride gointo solution.This solution can be concentrated by evaporation to35-40' B., so that on cooling a part of the chloride crystallises out.The solution, now containing four equivalents of chloride to one ofchlorate, or the original solution if preferred, is treated with sodiumlivdroxide or carbonate, or a mixture of the two. Magnesia, mag-nesium carbonate, 013 a mixture of t-he two, as the case mav be, isprecipitated whilst sodium chloride and chlorate remain in solution.On concentrating by evaporation to 48-50' B., and cooling, thechlorate separates out. The magnesia residue is employed againdirectly, o r if it contains carbonate, after being calcined. J. T.Crystallised Argentammonium Chloride and Bromide.ByTERREIL (Bu71. SOC. Chim., 41, 597).-Argentammonium chloride andbromide were obtained in a cr-ystalline form by heating the dry salts,saturated w i t h ammonia gas, with a strong aqueous solution of ammo-nia in sealed tubes. The method, as well as the properties of thecrystals, have been described in a former Abstract (Abstr., 1884, $90).Note by Ahsfmetor.-The author states that the argentammoninmchloride and bromide have never before been crystallised. This,however, is incorrect. Faraday, in 1818 (Journ. Science arzd Arts, 5,74), obtained a crystalline argentamnionium chloride by dissolvingsilver chloride in strong solution of ammonia and allowing the liquidto stand. Transparent crystals $inch wide were deposited in flatrhombohedra, i n some of which two acute angles were missing, whichcaused them to appear like hemihedra.The crystals lost ammoniaand became opaque when exposed to air, and were similarly decnm-posed by water with separation of silver chloride. An argentammo-niuru bromide having analogous properties, was prepared in the sameway by Liebig (Schweig. Journ., 48, 103).-W. R. n.W. R. D.Argentammonium Phosphate. By 0. WIDMANN (Bey., 17, 2284-228.5) .-With reference to Reychler's communication on this sub-ject (Abstr., 1884, l261), the author states t h a t in 18'14 he described(Oej'ers. of Konyl. Vet. Ahad. F6i-handlingar, Stockliolm, 1874, No. 4,p. 41), a crystalline cliammonio-silver phosphate, AgjP04,4NH,. It wasobtained by evaporating an amznoniacal solution of silver phosphatein a desiccator over quicklime with which a little ammonium chloridehad been mixed.It formed coloiirless prismatic needlps resemblingthe arsenate. The probable constitution is AgO.PO(ONH,.NH,Ag),.The crystals turn yellow on exposure to the air, and give up all theirammonia over sulpliuric acid. With ammonia and dry silver phos-phate, the author obtained results similar to Reychler's.L. T. T.Argentammonium Compounds. By A. R EPCHLER (Rer., 17,2263 -22G6).-Ammonia is rapidly absorbed by silver citrate withconsiderable development O E heat and a discoloration of the salt :about 4-5 mols. NH, are thus absorbed. Silver citrate dissolveINORGANIC CHEMISTRY. 19readily in ammonia, and alcohol precipitates from this solution hex-immoizio-silver citrate as a thick syrup, easily soluble in water. Silverbenzoate absorbs dry ammonia to form diammonio-sihter benzoate, awhite substance insoluble in water.Carey-Lea has described (Chein.News, 1861) a yellow crystalline diammonio-silver picrate. Thepower of the picrate to absorb ammonia is probably due to its nitro-groups. Ammonium picrate absorbs 1 mol. NH, at 0" to form ~"IZOH-ammonio-ammonium picrate, C6H2(N03) 3.0NH,NH3 : a t summer heat(about 26") scarcely a trace of ammonia is absorbed.The author considers the constitution of the diammonio-comnouncls I R--.of the organic acids to be probably Okg > C < g z : , and of the mono-nmmonio-compounds, where he considers the nitro-group to be thedetermining agent, to be (taking AgN0,,NH3 as an example)Agoammonia united to the silver.L. T. T.0 >N<gg2 or Ago>N\A 0 pH, , and that in neither case is thePreparation of Strontium and Barium Chlorides. ByWACKENRODER (Dingl. poZyt. J., 253, 440).-The author proposes toadd to a solution of str.ontium o r barium sulphide an equivalentamount of calcium chloride, and pass- carbonic anhydride into themixture. Hydrogen sulphide is disengaged and a solution of strontiumor barium chloride obtained, whilst calcium carbonate is precipitated ;the latter is removed by filtration, and the solution evaporated andallowed to crystallise. D. B.Constitution oP Bleaching Powder. By E. DBKYFUS ( B d l .Xoc. Clzim., 41, 600-609) .-The formula proposed by Stahlschmidt(2CaHC10, + CaCI, + 2H,O) alone accounts-for the excess of calciumhydroxide that is invariably present in this compound.Assumingthis formula, bleaching powder should contain 39.01 per cent'. ofavailable chlorine, but experiment sliows that it often contains morethan 40 per cent., which appears to militate against the nssamption.But the use of moist lime in the maiinfaeturing process explains thisresult. The water acts on the bleaching compound CaHClO,, pro-ducing calcium hypochlorite, together with free calcium hydroxide,2CaHC102 = Ca(OH), + Ca(CIO),. The calcium hydrovide thenagain combines with chlorine. According t o this, the active cornpoundir! bleaching powder is CaHClO, with' more or less calcium hypo-chlorite.Stahlschmidt's formula also supposes the existence of cal-cium chloride in bleaching powder. This has been considered to beincorrect, as bleaching powder is said not to yield calcium chloridewhen treated with alcohol. The author dispute8 this assertion, andstates that calcium chloride is always diwolved from the compound byalcohol, in quantity which increases with the time during which thoalcohol is in contact. Lunge and Schappi (Abstr., 1880, 789),a:guing from the action of carbonic anhydride on bleaching powder,whereby nearly the whole of the chlorine is evolved, have also arrivedat the conclusion that calcium chloride is not a constituent of bleachingc 20 ABSTRACTS OF CHEMICAL PAPERS.powder. The author points ouk that this conclusion is erroneous ; foralthough carbonic anhydride does not act on calcium chloride alone,yet in presence of hypochlorous anhgdride (from the action of car-bonic anhydride on CaHC102), the following reaction occurs eitherwith dry calcium chloride or with its aqueous solution: CaCl, + CO, + C1,O = CaC03 4- 2CL.In order to determine that the calciumhydroxide precipitated by water from bleaching powder is an essentialconstituent, the following expeyiments were made :-Solid bleachingpowder was treated with ammonia and alcohol ; the liquid was boiled,filtered, diluted with water, and the calcium estimated as oxalate. Inanother experiment, dry bleaehing powder was melted at a red heatto expel oxygen and chlorine ; the residue, treated with alcohol andwater, was filtered, and the calcium estimated in the filtrate as oxa-late.The results of these two experiments, which determine t8heamount of calcium as chloride, were identical. It is further shownthat with two carefully prepared specimens of bleaching powder, thecalcium obtained as chloride by the ammonia method is just half ofthe total calcium combined with available Chlorine, the other halfhaving been precipitated as hydroxide. This is in accordance withthe following equations :--2[2(CaHC10,) + CaC12] + 2NH,.OH= 8NH4C1 t 3CaCL + 3Ca(OH), + 202, and at a red heat2[2(CaHC10,) + CaCl,] + H20 = 3CaC1, + 3Ca(OH)2 + C1, + 30.The author concludes, therefore, that the formuala of bleachingpowder should be written 2CaHC10, + CaCl, + 2&0.Peroxides sf the Zincmagnesium Group.By R. HAASS(Ber., 17, 2249-22.55).-Th&-1ard (Ann. Chim. Phys., 1818, 9, 53,and Mdm. d e l’L4cad. des Sciences, 3, 429) described the formation of a“deutoxide de zinc” by (A) solution of zinc hydroxide in a hydro-chloric solution of hydroxyl, and reprecipitation with potash or soda,and (B) by acting directly on gelatinous zinc hydroxide with hydroxyl.On estimating the excess of oxygen in his compounds, Thenard foundthat the additional oxygen taken up was rather more than half thatoriginally present in the monoxide ; and concluded from this that theperoxidation was incomplete. These results appear to 11ave been verygenerally overlooked, o r when noticed (as in Gmelin-Kraut’s Hand-book), mistrusted. The author has therefore repeated ThBnard’sexperiments and fully confirms his results.The author employed the methods used by ThBnard, but modified(A) so far as t o mix a solution of a pure zinc salt, with an aqueoussolution of hydroxyl, and then precipitate with ammonia.The authorwas not able to obtain the pure peroxide, the precipitate always con-taining unosidised zinc hydroxide, The composition of the preci-pitate dried a t 110”, varied between Zn,08 and Zn,O,. By numerousmodifications of the mode of preparation, the author endeavoured toobtain the peroxide free from the hydroxide, but in every case wherethe precipitation of hydroxide was avoided, no formation of peroxidetook place, so that the author is inclined to eonsider the presence ofhydroxide as essential to such formatioaAs rightly described hy Thdnard, zinc peroxide (or rather its mix-ture with the monoxide) is a white, odourless, tasteless, and neutralW.R. DINORGANIC CEEMISTRT. 21gelatinous mass. This substance is tolerably stable towards wat3r,acids, and heat. A sample which had been heated a t 120" for 12 hours,and subsequently more strongly heated in a test-tube, still gave thehydroxyl reaction very strongly when dissolved in hydrochloric acid.The author has also obtained similar results with cadmium, the com-pounds obtained varying between Cd50s and Cd305, Manganese,which in other ways may be easily converted into the dioxide,yielded by t,he above treatment results almost exactly agreeing withthose obtained with zinc and cadmium.The composition of the pre-cipitates varied between Mn,O, and &iInsOe. Magnesium appears toform a similar peroxide, but with more dif€iculty, the highest stage ofoxidation yet obtained being expressed by MgO : Op = 93 : 7, whereOp represents the additional oxygen. Up to the present, no evidenceof the existence of a peroxide of beryllium could be obtained.By DEBRAY andJOANNIS (Compt. ~ e u d . , 99, 533--587).-1t is well known that cupricoxide is decomposed when strongly heated, and it is generally believedthat the product of decomposition is an oxide, Cuj03, or Cu50p, inter-mediate between euproua and cupric oxides.If cupric oxide yields the oxide CujOI when heated, it aught t ohave a constant tension of dissociation until one-fifth of the oxygenhas been expelled, a t which point the tension will change to'bhat ofthe intermediate oxide ; but if, on the other hand, the cupric oxide isdecomposed simply into cuprous oxide and oxygen, and the se-calledintermediate oxide is really a iniature of these two bodies, khetensioriof dissociation of the cupric oxide should remain constant until halfthe oxygen is expelled, a t which point it will change to that of thecuprous oxide.Direct expeyiments show that when cupric oxide is heated in a,vacuum, it begins t o decompose at a dull red heat, and if the tempera-ture is so regulated that the oxide does not fuse, the tension of disso-ciation of the latter remains constant until very nearly half of theoxygen is expelled.If the apparatus is allowed t o cool, any oxygenremaining within i t is cowzpletely absorbed by the cuprons oxide, andwhen the residue is cold, it is found to consist of cuprous oxide i nthose parts which have been most strongly heated, and of cupricoxide in those parts which have been somewhat cooler, the line ofseparation of the two oxides being perfectly sharp and distinct. Thesame results are obtained with various samples of cupric oxide pre-viously partially decomposed by fusion. It follows, therefore, thatwhen cupric oxide is heated under these conditions, it is decomposedinto oxygen and cuprous oxide only, without forming any inter-mediate oxide.If the cupric oxide is heated to fusion, it is decomposed somewhatrapidly, b u t the tension of dissociationt-aries with the state of decom-position of the oxide, and diminishes rapidly as the residue becomesmore completely converted into cuprous oxide. When the partiallydecomposed oxide is allowed to cool slowly in the apparatus, the pres-sure of the oxygen diminishes until the moment of solidification,when it suddenly increases, quickly attains a maximum, and then, asL. T.T.Decomposition of Cupric Oxide by Heat22 ABSTRACTS OF CHEMICAL PAPERS.cooling continues, diminishes again, finally becoming nil if theabsorbing sureace is sufficiently large. These phenomena are easilyexplained if it is admitted that the dissolution of a dissociable body ina liquid incapable of combining with it lowers the tension of dissocia-tion of that body in the same way as the vapour-tensions of liquidsare modified when certain liqnids are mixed.On this assiimption, thetension of dissociation of cupric oxide, fused with an increasing pro-portion of cuprous oxide, diminishes as the proportion of cuprousoxide increases ; but when the residue solidifies and forms a mixtureof the two oxides which do not act on one another, tbe cupric oxideregains its original properties, and more especially its true tension ofdissociation, hence the sudden increase of pressure at this point.By DEBRAY and JOANNIS (Compt. rend.,99, 688--692).-When copper is heated in presence of air, it is con-verted in to cupric oxide without intermediate dormation of cuprousoxide, at all temperatures between that a t which oxidation begins(about 350"), and that a t which the tension of dissociation of theoxide formed amounts to one-fifth of the atniospheric pressure, i.e.,the pressure of the oxxgen in the air.Beyond this temperature, thecupric oxide a t first formed is partially decomposed, and when themixture of cuprous and cupric oxide melts, decomposition ceases assoon as the variable and diminishing tension cf the oxygen in themixture amounts to one-fifth of the atmospheric pressure. The com-position of the mixture will depend on the temperature. A similarresult is obtained by direct oxidation of copper at these high tem-peratures ; a fused product is always obtained consisting of a mixtureof cuprous and cupric oxides, in proportions varying with the tem-perature.If the partially decomposed oxide is allowed to cool in the air, it iscompletely reoxidised if sufficiently porous ; but if it has been fused,oxidation takes place only on the surface, and the solidified residuehas practically the same composition as the liquid.It is evident thatin determinations of copper as cupric oxide the temperature must notbe suEcient t,o melt the oxide.When the copper is present in large excess, the product of oxida-tion is cupric oxide alone, if the temperature is below redness ; but ift,he t,emperature is sufficiently high to partially dissociate the cupricoxide, t,he latter is decomposed into cuprous oxide and oxygen, andthe oxygen thus given off a t once combines with the excess of copper,forming a further quantity of cuprous oxide. A mixture of cupricoxide and metallic copper cannot in fact exist at a temperature atwhich the oxide begins to dissociate, for the oxygen given off is atonce absorbed by the metallic copper, and thus is prevented fromacquiring a tension sufficiently high to arrest decomposition.I n cases where the amount of oxygen is not sufficient to oxidisethe copper completely, but is more than sufficient to convert it intocuprous oxide, the product is a mixture of the cuprous and cupricoxides (preceding Abstract).Cuprous oxide absorbs oxygen evenmore readily than metallic copper ; hence if the preceding mixture isallowed to cool in air or in oxSgen, the cuprous oxide is completelyC. H.B.Oxidation of CopperINORGANIC CHEMISTRY. 23oxidised. The readiness and completeness with which cuprons oxideabsorbs oxygen when moderately heated may be used as a means ofobtaining a very perfect vacuum.Some Reactions of Chrornyl Dichloride. By QUANTIN (Compt.rend., 99, 707-7'09) .--Chromic chloride, Cr,CI,, can be prepared bypassing a mixture of chlorine and carbonic oxide over chromiumsesquioxide, heated to redness ; and is readily obtained in violet crys-tals by passing vapour of chromyl dichloride, chlorine, and carbonicoxide through a glass tube heated a t 500-600" ; 'LCrO,Cl, + 4CO +Cl, = 4c02 + CrzC16. I n this reaction, the chromyl dichloride is notfirst reduced to chromous chloride by the carbonic oxide, for if a mix-ture of chromyl dichloride with carbonic oxide alone is passed throughthe hot tube, vivid combustion takes place with formation of greenchromium sesquioxide and violet chromic chloride.The progress ofthe first reaction may be represented by the following equations :-C. H. B.(1) CO + 2CrO2Cl2 = Cr,O, + CO, + 2C1,( 2 ) Cr,O, + 3CO + 3C1, = Cr,C16 + 3c0,.The carbonic oxide combines only with the oxygen which wouldhave been liberated by the action of heat alone, and does not reducethe sesquioxide which is formed, but the latter is convei-ted intochromyl dichloride by the action of the chlorine which is liberatedand the excess of carbonic oxide. The same results are obtained withany mixture which will give off chromyl dichloride. Dry hydro-chloric acid gas acts slightly on chromyl dichloride a t a red heat, acertain quantity of chlorine, water-vapour, and black chromium oxidebeing formed, but no violet oxychloride is produced.When chromyldichloride is decomposed by heat, the only products are chlorine,oxygen, and black chromium oxide. C. H. B.Chromamrnonium Compounds. Luteochromium Salts. ByS. M. J~RGEKSEN (J.ppr. Chem., 30,1--32).--In a former communication(this Journal, Abstr., 1882, 1167), the author pointed out that a solu-tion of chromammonium chloride i n ammonic chloride undergoesoxidation in absence of air, heat is produced and hydrogen evolved,and the chief product is the roseo-chloride. If the mixture is cooledand the oxidation takes place slowly, then luteochrornium chloride isthe chief product. To prepare this compound, a solution of chromouschloride, prepared by Christenskn's method, is forced by hydrogenpressure into a vessel containing a mixture of 700 grams of ammoniumchloride and 750 C.C.solution of ammonia (sp. gr. 0.91). The vessel,entirely filled with this mixture, is closed by a stopper, through whichpasses a delivery tube opening under water. The vessel is surroundedby cold water to moderate the reaction. The evolution of hydrogentakes place slowly and ceases in about 94 hours, the undissolvedammonium chloride is covered with the lutcocbromium chloride, a.portion of which is also contained in the solution, from which it, maybe obtained by precipitation with alcohol ; the precipitate after beingwashed with alcohol is dried, dissolved in warm water, and the FO~U-t i v i i filtered into nitric acid (sp.gr. 1.39) ; in this manner a precipitat24 ABSTHACTS OF CHEMICAL PAPERS.of luteochromium nitrate is obtained. The nitrate is washed withdilute nitric acid (1 vol. of nitric acid to 2 vols. of water), and theacid removed by washing with dilute alcohol.The luteochromium chloride mixed with the ammonium chloride isseparated by repeated treatment with water, the aqueous extracts areprecipitated by nitric acid, and thus further quantities of luteochro-mium nitrate are obtained.Blomstrand’s method of preparing luteocobalt salts may be appliedfor the preparation of luteochromium salts.L?cteoch.romium nitrate, Cr212NH3,6N03, is obtained from dilutesolutions on addition of concentrated nitric acid in long narrowprisms ; from concentrated solutions, dilute nitric acid precipitates itin orange-yellow, lnstrous, quadratic tables. It may be crystallisedfrom wclrm water containing nitric acid, and then forms small quad-ratic pyramids.Luteochroiriium ititrate sulphate, CrJ 2NH3,2NO,.2SO4, obtained byadding dilute sulphnric acid to a solution of the nitrate, or by addi-tion of ammonium sulphate and ammonia, forms yellow, lustrous,quadratic octahedra.L~iteoehromium nitrate ylatinochloride, Cr212NH3,2NO,,2PtCl6 +2H20, an orange-yello w crystalline precipitate, formed when hydrogenplatinochloride is added to a solution of the luteo-nitrate.Luteochromizcm chloride, cr212NH3,cl6 + 2H,O, is best obtained byfirst treating a, saturated solution of the nitrate with concentratedhydrochloric acid and mercuric chloride, a yellow precipitate of thecompound Cr212NH3,C1,,2HgC1, is obtained. This mercury conipoundsuspended in water, and decomposed by sulphuretted hydrogen, givesa solution from which, on evaporation, the luteochromium chlorideseparates in large yellow crystals.It is converted by concentratedhydrochloric acid into the chloropurpureo-chloride.Luteochromaum platinoclilorides ; three such compounds have beenobtained : ( a ) Cr,12NH3,3PtC1, + 6H20 is formed as .an orange-yellow crystalline precipitate when sodium platinochloride is added toa dilute solution of the neutral luteo-chloride ; (6) Cr,12NH3C12,2PtCl~ + 5H,O is produced when an acid solution of the luteo-chloride isprecipitated by a solution of platinic chloride ; it forms long orange-yellow needles ; by cold water, it is resolved into luteo-chloride and thesalt G.When the salt ( b ) is washed with dilute hylrochloric acid, itis converted into the componnd Cr2l2NH3C1,,PtC~, + 2H20.lhteochromium bromide, Cr,12NH3,Br6, prepared by the action ofhydrobromic acid on a half-saturated solution of the nitrate ; i t formsan orange-yellow crystalljne precipitate, and is less soluble than thechloride.Luteochromium p latinobromide, CrJ 2NH3, 3P tBr6 + 4H20, preparedby adding a dilute solution of sodium platinobromide t o a dilute solu-tion of the luteo-bromide. It forms a precipitate consisting of deepvermillion, lustrous, quadratic, and eight-sided tables.When lessdilute solutions are employed, or the above precipitate is allowed tostand, a change takes place, and a compound similar to the luteo-chromium platinochloride with 6H20 is formed.Luteochrornium iodide, Crz12NH3,T6, is formed by treating a solutioINORGANIC CHEMISTRY. 25of the nitrate with solid potassic iodide: the yellow precipitate iswashed with hydriodic acid, dissolved in water, and filtered intohydriodic acid. It crystallises i n lustrous rhombic tablets, and isisom orphous with the bromide.Luteochrorniurn iodide sulyhate, CrJ2NH3,T2,2 SO4, is formed bytreating an ammoniacal solution of the chloride with ammoniumiodide and ammonium snlphate.L uteocliromium sulphate, Crz12NH,,3SOa + 5H20, is prepared byneutralising luteochromium hydroxide (formed by rubbing togetherthe luteo-bromide and moist silver oxide) with sulphuric acid, and pre-cipitating the solution with alcohol ; it crystallises in long, yellow,lustrous crystals.Luteochromiunz sulphate platinochloride, Cr212NH3,2S01,PtC16, isobtained as an orange-yellow precipitate.Luteochromiurn orthophosphate, Cr212NH3,2POd + 8H20, obtainedby treating a solution of the nitrate with sodium phosphate andammonia, as a yellow precipitate consisting of yellow shining needle-shaped crystals.Luteochronzium oxdate, Cr212NH3,3C20r + 4H20, obt'ained as acrystalline precipitate by decomposing the nitrate with ammoniumo xalat e .T'he following salts have been prepared in a simiiar manner : thepyrophosphate, Cr212NH3,2 (P207Na) + 23H20 ; the ferricyanide,It crystallises in octahedra.Crz12NH3,FezCy12 ;the cobalticyanide, Cr212NH,CozCy12 ; and the chromicyanide,Cr212NH3,Cr2Cylz.P. P. I).Double Tungstates of Rare Metals. By HOGBOM (BUZZ. XOC.Chim., 42,2--6).-By methods of fusion, a large number of compoundsof sodium tungstate with the metals of the rare earths were obtained ;these crystallised in the same form as the simple tungstntes describedby Cossa. The salts may be prepared by dissolving the oxides withtungstic acid, in fused sodium tungstate, or in fused sodium chloride,or still better in a fused mixture of the two. The mixture is liquefiedat a bright red heat, and maintained in a semi-liquid condition a t lowredness.Microscopic crystals of the salts are formed and separatedby treating the product with water, in which they are insoluble.Weak acids attack them orily slowly in the cold, but they are com-pletely decomposed by repeated treatment, in a finely powdered condi-tion, wiDh concentrated hydrochloric acid. It was in this way thatthe analyses of the greater number were made ; the others were fusedwith a mixture of alkaline carbonates, and the tungstic acid precipi-tated by mercuric nitrate. Notwithstanding the difference in compo-sition, the salts bear it great resemblance to one another in crystallineform, which is generally that of a tet(ragona1 octahedron. Thesewere not obtained large enough to measure the angles exactly, but anapproximate measurement was made with the aid of the microscope.The salts described may be arranged under the following types :2G ABSTRACTS OF CBEMICAL PAPERS.I. { 4gr;y} ~wo,; R = La, Ce, or G.11. { 'g:,:} 6W03; R = Di.IV. { grh:} 4W0, ; R = Di.V. { 'FG;} 4W0,;. R = Th.The salts of the types I, 11, and V are formed in presence of excessof sodium tunstate, and those of t4he types 111 and IV in presence ofexcess of sodium chloride. I n a note appended to this paper, Clevecomments on the remarkable fact of t,he similarity in crystallineform of t,hese different salts, all of which either crystallise i n the Eameform or in that of scheelite, which is isomorphous with fergusonite.Other cases of apparently anomalous isomorphism occnr with the rareearths and oxides of the formula RO. Thus titanite is isomorphouswith yttrotitanite, and according to Nordenskiold, cerite, 2CZO3,3SiO2,with peridote, 2Mg0,Si02. It) would thus appear that' isomorphism ispossible between compounds of the rare earths and of the oxides ofthe form RO when the total proportion of oxygen is the same in thebasic and acid oxides which const'itute the compounds. The formula?of the metallic oxides of the cerium and yttrium groups have beenso firmly established in other ways, that it is undesirable to changethem solely on account of the isomorphism of certain of their tung-states with scheelite. W. R. D.The Tempering of Steel. By C. FROMME (Anrt. Phys. Chem.,22, 371--S87).-The changes of density and of hardness in iron orsteel heated, and either slowly cooled or suddenly quenched in water,are the subjects investigated in the author's experiments. I n temperedsteel the density and hardness by 110 means go together, for increaseddensit'y more often corresponds with diminished hardness and aicevers&. The results recorded in the paper support the theory that intempering there takes place not only the mechanical and purelyphysical process of sudden contraction, but also another process of achemical nature consistino; chiefly in the combination of the ironwith the free carbon distributed through its mass. R. R

ISSN:0368-1769    

DOI:10.1039/CA8854800014

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

26 ABSTRACTS OF CBEMICAL PAPERS.Min er a1 o g i c a1 C h e m i s t r y.Effect of Heat on Vesuvian, Apatite, and Tourmaline, ByC. DOELTER (Juhrb. f. M h . , 1884, 2, Mem., 217--221).--The authorhas elaborately investigated the effect of heat on the optical propertiesof vesuvian, apatite, and tourmaline. H e finds that the optical proBIINERALOGIUAL CHEMISTRY. 27perties of vesuvian are very variable, not only in crystals fromdifferent localities, but also in those from the same locality. Manyvesurians are quite normal and exhibit the black cross in all positionsof the plate ; this is the case with the light-green variety from Ala.Much more frequent is the case in which a distinct separation of thearms of the cross occurs. CrystaIs from Vesuvius present a smallaxial angle of 4" to So, and other crystals may be mentioned whichexhibit a considerable axial angle.Thus, an axial angle of 34Q" forred light was measured on a light-brown crystal from Vesuvius, 24"on a yellowish-brown crystal from Piedmont, and 12" on a browncrystal from Zermatt. The vesuvians differing optically also presentdifferences on being heated. With the vesuvians which have a verysmall axial angle, this usually increases with increase of temperature,whilst with those which have a large axial angle: i t decreases.Apatite, according to Mallard, exhibits optical anomalies. This theauthor found to be the case with the violet apatites from Schlaggen-wald and Elirenfriedersdorf, and with coloured apatites generally ;whilst the colourless crystals from Pfitsch, and the pale-green crystalsfrom Salzbach, were perfectly normal.A yellowish-brown crystal oftourmaline from Lower Drauhurg, in Carintliia. exhibited an axialangle of 9" for red light. With a slight increase of temperature, nochange could be detected ; and a t a red heat the arms of the h-j-per-bola came nearer together, but did not even at the highest tempera-ture join completely.Sulphur from Zielenzig. By A. ARZRUKI (Juhrb. f. &tin., 1884,2, Ref., 307).-Rhombic crystals of sulphur occur in fissures in thelignite at the Phoenix Mine, near Zielenzig, in Brandenburg. Thecrptals have been formed by sublimation. The following forms wereobserved: P, OP, Pij, WP, P e , +P, +P, +P.Minerals of the Cryolite-group from Greenland. By A.KRENNER(Jahrb. f. illin., 1884, 2, Ref., 308-310).-This paper contains anaccount of the morphological and optical properties of the cryoliteminerals : cryolite, thomsenolite, pachnolite, arksutite, and ralstonite.Microscopic Association of Magnetite with Titanite andRutile. By A. CxrHmm (Julwb. f. &in., 1884, .2, Ref., 306-307).--Magnetite surrounded by tihnite, disseminated through a mixtureof chlorite and actinolite, occurs in remarkably fine examples in rocksfrom the Alpsbnch and Wildschonau valleys in the Tyrol. A mixtureof magnetite, with actinolite and a little titanite, was obtained afterrepeated washing and extraction with the magnet. This mixture,in very fine powder, after a quarter of an hour's treatment withhydrochloric acid, left a residue consisting of rutile and some actino-Zite.The acid solutionexhibited the composition given under I, 0.3565 gram being employed,with 0.1215 insoluble residue containing 0.11 SiOz, 0.017 Ti02, and0.093 pure actinolite-B. H. B,B. H. B.B. H. B.The latter was isoIated and analysed (11)28 ABSTRACTS O F CHEMICAL PAPERS.I.SiO,. ..... 4.67l’i02. ..... 5.07A120, .... -Cr203 .... 3-65Fe203 .... 52-94FeO.. .... 29.75CaO .... 2.27MgO .... 2.41H,O.. .... -Total .. 100.76The 90.02 per cent. ofing results :-Ti02. Cr,O,.3.22 4-06Magnetite.-2-903-6552.9429.251.28--- -90.02Titanite.1.632.1 7----1.52-- --5-32Actinolite.3.04 ----0.500.751-13- -5-4255.38--0-509.1613.6520.620.2799-58-magnetite calculated to 100 gave the follow-Fe203.FeO. MgO. To kal.58.81 32-49 1-42 100.00From the author’s observations, it follows that the so-calledleucoxene surrounding magnetite is a product of alteration. I n themagnetite, Fe,Os is replaced by FeTiO,, and leucoxene, which isnothing other than titanite, is formed. The microscopic investigationsupports this theory. B. H. B.Pseudomorphs after Rutile. By A. v. LASAULX (Juhrb. f. Mi%.,1884, 2, Ref., 299).-Pseudomorphs after rutile occur in the graniteof Morbihan. Rutile crystals are of frequent occurrence, but theyare often altered to a considerable depth into ilmenite. Betweenthe layer of ilrrienite and the rutile, yellow titanic hydrate is fre-quently met with.In other crystals, a product resembling titano-morphito occurs in the immediate neighbourhood of the ilmenite.Other rntile crjstals were altered into a mixture of ferric oxide,minute crystals of anatase, titauite, and rutile. In this case, theanatase is paramorphous after rutile. B. H. B.Natural Borates. By C. RAMMELSBERG (Jahrb. f. Mirz., 1@84, 2,Mem., 158--163).-0n the banks of a salt lake in the Argentine pro-vince of Jujuy, Brackenbusch collected a white mud which hardenedto a solid mass, on exposure to the atmosphere. This substance isboronatrocalcite (Dana’s ulexite), and contains rJodium chloride and alittle clay. It is Free from sulphates, but several of the harderparticles appear to be glauberite.When heated, the powder fuses toa cloudy green glass. Analysis gave the following results :-B203. CaO. Na20. H2O. Total.42.06 15.91 8.90 33.48 100.35from which the author calculates the formula to be : Na4Ca4Bl8033 +27H20 ; this requires :MIXERALOGICAL CHEMISTRY. 29BZO,. CaO. Na,O. €120. Total.43.03 15.30 8.47 33.20 100*00Na4B,01, + 9H,O{2(C aB60t, 2 + 9Hz0)’and if the borate R’BOz = R”B,04, the oxgen ratio for bases and acidis 2 : 3.In conclusion the author gives a summary of the natural borates,assuming that R’BO, = R“B20+A. Oxygm Ratio for Bases and Acid, 3 : 4.-1. Priceite (a mineralfrom Oregon identical with pandermite from Panderma on the BlackSea)-If the formula is written-CSBSO,, + 5HzO = { igz6y4} + 4&O.2.Boracite (and Stassf urtite)-B. OxygeN Ratio f o r Bases and Acid, 2 : 3.-1. Hodroboracite.2. Boronatrocalcite-3. Franklandite (.Phil. Mag., 1877, 284)-NGJ%Oll + 8&O} = {[?zlz]] Ca B204 { Ca*BsOl, + 8HDHBO,+ 7H20.C. Oxygen Ratio for Bases and Acid, 1 : 2.-1. %orax (Tinkal) ;-NazB& + 10HzO = 2 ~ ~ ~ ~ + 9&O.2. Borocnlcite (Hayesine, Tiza of Atacama)-CaBa07 + 6H20 = 2g:b: + 5H,O. 0D. Oxygen Ratio for Bases and Acid, 1 : 4.--1. Larderellite.AmBO,AmzBbO13 + 4H20 = 2 { 3HB0, } + HZO30 ABSTRACTS OF CHENICBL PAPERS.I n addition to the above are two basic borates.1. Sussexite-R = Mn, Mg.2. Spaibelyite-MgdMA1 i 3H20 =I n ludwigite, datolite, danburi te, tourmaline, and axinite, boronmust beregarded as replacing A1 or Fe.€3. H. B.Apatite from Logrozan (Spain). By A. VIVIER (Compt. refzd.,99, 709-71 l).-Apatite from Logrozan occurs in regular hexagonalprisms, the bases of which are modified by pyramidal faces. Thecrystals are enclosed in an altered trachyte, and are generally more orless opaque, and yellowish or greenish in colour, with an unevenvitreous fracture. They contain numerous enclosures of lamellai=specular hematite. Some of the crystals are as much as 25 mu]. inlength, but the apatite is also disseminated through the rock in micro-scopic crystals. The larger crystals, free from specular hematite,have the composition :-Aluminium and berjlliuni phosphates ........Calcium phosphate ........................ 89.54Cdcium fluoride (by diff .) ..................5.234.46Calcium chloride .......................... 0.77100~00C. H. B.Origin of the Phosphorites in the South-West of France.By DIKVLBFAIT (Corn@ rend., 99, 440--443).-1t has been urged thatthe author's theorF of the formation of phosphorites, partially, if notentirely, by the action of percolating saline waters of the tertiary age,is not applicable to the phosphorites in the south-west of France,because this district was never covered by the sea during the tertiaryperiod. In this district, however., there are many deposits of gypsumwhich undoubtedly belong to the tertiary period, and they contain innotfable quantity lithium, strontium, manganese, zinc, copper, .andboric acid, substances which the author has previously shown to becharacteristic of the saline deposits and saliferous marls formed inmodern seas.In all probability, therefore, the gypsums of the south-west of France, like those of the middle, and of the Paris basin, areproducts of the evaporation of saline waters.If the excavation of the phospboritic caverns and the deposition ofphosphorites has been the work of saline waters of the tertiary period,it follows that a calcareous tract may only be expected to containphosphorites when it is covered with deposits of tertiary age.Brazil.C. H. B.Minerals from the Metamorphic Rocks of Ouro Preto,By H. GORCEIX (JLchrb. f. $!in+, 1884, 2, Ref., 302-303).BlISERhLOGICXL CHEMISTRY. 311. Crystals planted on quartz with cobalt oxide. The crystals are ofa white colour, H.= 2-3, sp. gr. 2.3. They are soluble withdifficulty in warm nitric acid, and have the following composition :-A1203. H,O . Total.65.2 34.8 100.0correspoading to the formula A1203,H20.Thecrystals are white or pale-green, acicular, with distinct cleavage.H. = 4.P206. F. A1,03. CaO. MgO. H20. Total.33.0 3.6 36.1 0.3 0 2 26.2 99.42. Crystals of zuauellite in small geodes in black slate.Sp. gr. 2.34. The analysis gave the following results :-2. Pyrophy7Zite. With the above minerals, acicular white, greenishTheSp. gr. 2.76. Theor bluish crystals occur ; sometimes accompanied by disthene.mineral has a pearly lustre and low hardness.analyses gave the following results :-Si02. Al,03. FeO. CeO. H20. Total.65-3 28.0 1.7 0-4 5.5 100.9B.H. B.Empholite. By L. J. IGELSTRON (Jahrb. .f. A!&., 1884, 2, Ref.,317--318).-The new mineral from Horrsjoberg, Sweden, formerlyregarded as diaspore, gave oli analysis the folloning results :-Si02. A1,03. MgO.CaO.Fe0. H,O.53.3 30.5 3.4 13.8The mineral is insoluble in acids, H. = 6. It is found in thequartzose, disthene, and muscovite schists.The Potash-soda-felspars of Silesia. By A. BEUTELL ( J ~ h r b . f.Afin., 1884, 2. Ref., 319--324).-1n an exhaustive paper on thissnbject, the author gives crystallographical descriptions and chemicalanalyses of the following felspars : microcline from the granitite ofSchwarzbach and Griinbusch in the Riesengebirge, albite froni thegranitite of Schwarzbach, microcline from the granitite of Striegau,albite from the same locality, microcline from the granite vein ofIlampersdorf and Leutmannsdorf in the Eulengebirge, and alhite fromReichen bach.B. H. B.B. H. B.Minerals from a Chromite Deposit. By A. ARZRTJEI ( J n h ~ b . f.Nin., 1884, 2, Ref., .303--304.)-The minerals were found near theKassli smelting-works in the Ural. I n fissures in the chromik,crystals of kammererite occur ; they are not violet, but of a bluish-green colour. Crystals of perowskite and rutile also occur, the lattercontaining chromium. This is probably due to enclosed kammererite.B. I€. B.Magnesian Epidote. Bg DAMOUR and DES-CLOIZEAUX (Jdwb. f.ilfin., 1884, 2, Ref ,317).-On lapis lazuli from the Haikal Lake, mixedwith dolomite and iron pyrites, small white or yellowish transparen32 ABSTRACTS OF CHENICAL PAPERS.crystals were observed, the optical and crystallographical propertieso€ which are those of epidote.The crystals scratch glass, are iufusiblebefore the blowpipe, and contain silica, alumina, magnesia, and tracesof lime. The name picro-epidote is suggested for this epidote.B. H. B.Schuchardtite. By G. STARKL (Jakrb. f. M ~ N . , 1884, 2. Ref,,305).--This mineral is of an apple-green colour, soft, and is disinte-grated by water. Heated at 300" it loses 4.477 per cent. of water;in the desiccator i t loses 1.6 per cent. Sp. gr. 2.339. The analysisgave the following results :-SiO.2. A1,0,. Fe,O,. NiO. FeO. CaO.I. 33.281 14.616 3.825 5.678 3.561 1.47211.33% 14.882 3.905 5.t82 3.617 1.49911. 33-214 15.C93 2.605 6.106 3.517 1.824I. 23.723 13907 100*06311. 24.155 12.366 100.092111. 24.747 12.894 100*000MgO. H,O. Total.I is the analysis of fresh material ; I1 that of the substance driedFrom the at loo", and 111 the calculated percentage composition.azalysis is deduced the empirical formula-A1,,Fe,Si,,050 + Fe3Ni,CazMg,Si,,0,, + 44H,O.B. H. B.Groddeckite, a new Zeolite. By A. ARZRUNX (Jalzrb. f. Mi%.,1884, 2, Ref., 318--319).-The groddeckite crystals cover calcitecrystals which are planted on a breccia of a greenish-grey siliceousrock. I n addition to calcite, quartz crystals, galem, and magneticpyrites were observed. Only one specimen from St. Andreasberg hasbeen met with, this is in the collection of the Clausthal School of Mines.The cryetals are colourless and have a glassy lustre, H.= 2-3.Cleavage indistinct, prismatic. The crystals are very similar to thoseof gmelinite. The chemical composition is-SiO,. A1,03. Fe,03. CaO. MgO. N%O. H20. Total.51-53 12.0 7.7 1.1 3.3 4.5 20.2 100.0corresponding with the formula-Constitution of the Amphiboles containing Alumina. By R.SCHARIZER (Jahrb. .f. 2&z., 1884, 2, Mem., 143--157).-Schrauf pub-lished (Juhrb. f. Min., 1883, 2, 84) an account of the action of heaton the hornblende from Jan Mayen, in which he stated that thethermal constants were different from those of actinolite, Theauthor's chemical investjigation now proves that the chemical consti-tntion of actinolite is totally different from that of this hornblende.The analysis gave the following results :hlINERhLOGlCXL CHEMISTRY. 33FiO,.A1,03. Fe,O,. FeO. MnO. MgO.39.167 14.370 12.423 5.856 1.505 10.521CaO. K20. Na,O. HzO. Total.11.183 2.013 2.478 0.396 99.912corresponding with the formula (R’,,R”),(Al,Fe),Si,012, the usualformula for amphiboles, free from alumina, being (Mg,Fe)&aSiSi3Ol2.All amphiboles containing alumina must, according to the author,be mixtures of two terminal members, one being represented by thehornblende, rich in Al2O3 and Fe-03, from Jail Mayen, the otherbeing actinolite free from alumina. For the monoclinic substance,R3RzSi3012, the author adopts Breithaupt’s name, syntogmatife, becausethe hornblende from Vesuvius, so termed, closely resembles the terminalmember of this series of isomorphous mixtures, the hornblende fromJan Mayen.In order to prove the hypothesis that in the monoclinicdivision of the amphiboles t,wo terminal members exist differing inchemical composition, actinolite of the type (Mg,Fe),CaSiSi,Ol2, ainetasilicate and syntagmntite of the type R3R”2Si30,2, an orthosilicate,wliich mixed in variable proportions yields the hornblendes containingAl,O, and Fe,O,, a number of recent analyses were calculated. Theresults were distinctly in favour of the above hypothesis, and provethat three groups of amphiboles may be distinguished : the opticallynegative metasilicate, actinolite ; the optically negative orthosilicate,syntagmatite ; and the optically positive orthosilicate, pargasite, thecomposition of which may be expressed by the formula(~,Ca),(Mg,Fe)3(A1,Fe),Si,01G.B. H. B.Leucite- and Nepheline-basalt from the Vogelsberg. ByH. SOMMERLAD (Jahrb. f. Mi~z., 1884, 2, Mem., 221-223).-In thecollection belonging to the University of Giessen, the mthor foundtwo interesting rocks in which the presence of leucite and nephelinehad not previously been detected.The leucite-basalt from Ulrichstein presented a compact greenish-black ground-mass, containing olivine and augite crystals. Underthe microscope a finely crystalline ground-mass is seen, formed ofminute augite crystals and magnetite grains, accompanied by occa-sional patches of leucite. Olivine, augite, and brown mica formprophyritic crystals.An analysis of the rock gave the followingresults :-SiO,. 81.203. Fe20,. FeO. CaO. MgO.41.13 18.18 4.71 7.64 13.20 10.59K2O. NaO,. HzO . Total.1.59 2.00 1-74 100.i8The nepheline-basalt from the Ziegenstuck near Herbstein is of agreyish-black colour. In the ground-mass, olivine grains and augitemay be observed. Under the microscope, the principal mass is seen toconsist of black angites, with magnetite grains and irregular patchesof nepheline. The rock is a nepheline-basalt resembling the Taufsteinrock. B. H. B.VOL. XLFITI. 34 ABSTRACTS OF CHEN ICAL PAPERS.A Pegmatite containing Large Crystals of Chloropl?.yllite.By I?. GONNARD (Comnpt. rend., 99, 711-712).-A vein of pegmatitecutting through granite, about 10 kilorn. from Montbrison, Loire.onthe road between that place and St. Bonnet-le-Courreau, containscrystals of chlorophyllite as much as 6 cm. in length aiid about 3 ctn.in diameter. Some are very dark-green, with a fracture which isvitreous in some parts, dull in others. These crystals seem to passinto fahlunite. Others are greenish, greenish-grey, or pearly-grey,and cleave very easily along the basal plane ; sp. gr. 2.77. The peg-matite also contains crystals of white microcline, which have the rareface h. very well developed. These crystals have a reddish tinge, andconsist of thin Iarnin~ united along the direction h, but covered witha thir, layer of the same substance which masks the s t r i aChemical Composition of Augites from Phonolites andSimilar Rocks. By P. MANN (Jahrb. f. &fin., 1884, 2, nilem., 172-205).-The author has isolated and analysed the auqites from a num-ber of phonolites and other rocks pith in alkalis. The rocks employedwere phonolite from Elfdalen, leucitophyre from Rieden, hauynophprefrom Melfi. Of these rocks, the two latter contain augite onlp, whilstin the two former some hornblende also occurs, but in such smallquantity that sufficient material f o r analysis could not be obtained.The aagites from all the rocks examined were proved to contain alkalis,those from the phonolites proper to a much grea,ter extent than thosefrom the leucite and hauyn rocks. All the analyses give a percentageof silica much too low f o r the amount of alkalis present, thus renderingvery probable the presence of the silicate R2R”’Si06, as suggestedby Doelter. The extinction angle increases in direct proportion tothe percentage of iron and alkalis. This is shown in the followingtable :-C. H. B.Fe20,. IMelfi ................Rieden ..............Elfdalen ..............Hohektwiel ..........12.6’719 -5222.4426 -35Total alkalis.1.993 -359.3613 *33Extiiiction angle.39”301210~~ B. H. B

ISSN:0368-1769    

DOI:10.1039/CA8854800026

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

34 ABSTRACTS OF CHEN ICAL PAPERS.Organic C h e m i s t r y .Exchange of Chlorine, Bromine, and Iodine between Organicand Inorganic Compounds. By R. BRIX (Awnalen, 225, 146-170).-These experiments were made to ascertain the iufluenceexerted by the nature of the element contained in any inorganichaloid compound on the exchange of halogens with a n orgauic haloiOHGAICIC CHEJIISTRT. 35derivative. The organic compounds employed were ethyl iodidtl,isobiityl chloride, benzyl chloride, and ethyl monochloracet ate, theinorganic compounds were selevted from tlhe lialogen compoundsof the alkaline earths, of the heavy metals, and of arsenic, antiinon!-,and bismuth. The mixtures were heat,ed i n vessels provided witha reflux apparatus, except when otherwise mentioned.Calcium chloride and ethyl iodide do not react at the boiling point'.Barium chloride and ethyl iodide react very slightly a t 14f~".Barium iodide and isobutyl chloride do not, react on boiling.Bariumiodide and ethyl monochloracetate exchange their halogens completelyat the temperature of the water-bath. Barium iodide and benzylchloride give a partial interchange. Cupric chloride and ethj-1 iodidedo not react when boiled together, but on heating with alcohol a t1.50-160" complete interchange is effected. Zinc iodide arid ethFlmonochloracetnte react readily and nearly completely at 90 -100".Zinc iodide and benzyl chloride react on mixing, the interchangebecoming complete a t 43-50". Zinc iodide and isobutyl chloride donot react when boiled together.Cadmium chloride and ethyl iodide d onot react when boiled together, but partial interchange is effected byheat#ing a t 130-140" in sealed tubes with alcohol. Cadmium broriiitlesueers partial interchange when boiled with either benzyl chloride ore1,hj-l monochloracetate, but does not react with ethyl iodide. Cad-mium iodide gives but a slight interchange with ethyl monochlor-acetate, reacts readily but not completely with beuzyl chloride, and doesnot react with isobutyl chloride except in sealed tubes a t 135", whendecomposition-products are formed. Tlialli uin chloride and ethyliodide do not reaet. Thallium iodide and ethyl mono2hloracet;tte givea partial reaction in presence of alcohol. Lead chloride and ethyliodide do not react, but in sealed tmbes a t 1.?0-160" in presence ofalcohol, nearly complete interchange is erected.Lend iodide andbenzyl chloride do not react unless heated a t 150-160" in presenceof alcohol, when a partial reaction occurs. Arsenious bromide re-acts completely with either benzyl chloride or ethyl monochloracetatea t 140-145" in presence of alcohol, ALnCiinonious bromide gives a,complete intrrchange with either ethyl iodide or ethjl monoelllor-acetate a t 140-145" in pi*esence of alcohol. Bismuth bromide andethyl iodide give a partial intuerchnge ah 150-160" in pyesence ( J €alcohol. Bismuth bromide and ethyl monochloracetate heated withalcohol a t 140" give decomposibion-products.Exchange of Chlorine, Bromine, and Iodine between Inor-ganic and Organic Compounds.By B. KOHNLEIN ( A n n d c ~ ,A. J. G.225, 171-1' 5).-This paper is essentially a continuation of Biix's(preceding Abstract), from which it differs in the use of a much laryernumber of metallic compounds ; in the employment, as far as possible,of the same temperature (145-150" for four hours) in all cases, so 8sto obtain comparable results; and in the avoidance of the use ofalcohol, which in many c'ctses vitiates the results.Lead iodide and isobutyl chloride react to a very slight extent ; withlead chloride and ethyl iodide, on the contrary, nearly complete inter-change occurs. Antimonious chlori l e and et!iyl iodide exchange theird 3ii ABSTRACTS OF CHEMICAL PAPERS.halogens completely. Antimonious bromide and ethyl m onochlor-ticketate react partially ; antimonious bromide and ethyl iodide reactcompletely. Antimonious iodide and isobutyl chloride react withdecomposition, butylene being formed.Arsenious chloride and ethyliodide undergo complete interchange. Arsenious bromide does notreact with isobntyl chloride ; it reacts partially with ethyl monochlor-acetate ; it does not react with ethyl iodide unless the temperature israised to 150-160", when complete interchange takes place ; it reactscompletely with isopropyl iodide. Arsenious iodide scarcely reactswith ethyl monochloracetate, and does riot react with isobutyl chloride.Phosphorous chloride and ethyl iodide do not react. Phosphorousiodide does not react with ethyl monochlorncetate in open vessels a t143", although complete decomposition occurs in sealed tubes at 1FiO" ;it dces not react with isobutyl chloride at 140°, but complete decomposi-tion occurs a t 160-170" ; it reacts with propyl chloride with decompo-sition a t 1,50".Stannous chloride, or stannic chloride, and propyliodide react nearly completely, whilst stannous iodide scarcely reactswith propyl chloride. Zinc chloride, or cadmium chloride, and propyliodide give a nearly complete reaction. Propyl iodide suffers decom-position if heated with titanium chloride. Yerrous iodide or chloridegives practically no reaction with the corresponding propyl compounds.Manganous iodide and propyl chloride exchange their halogens nearlycompletely ; manganous chloride and propyl iodide do not exchange,but the propyl compound suffers partial decomposition.Cobaltchloride and propgl iodide react slightly ; cobalt iodide and propylchloride scarcely react. Nickel chloride and propyl iodide, and nickeliodide and propyl chloride respectively are practically without actionon one another. Thallium chloride and propyl iodide react partially.Magnesium chloride and propyl iodide do not react. Calcium iodideand prop~-l chloride give a complete interchange. Strontium iodide2nd propyl iodide exchange partially, whilst strontium chloride andpropyl iodide do not react. Barium chloride and propyl iodide arewithout4 action on one another.The author draws the following conclusions as t'o these reactions :-K, Mg, Ca, Sr, Ba, Al, Mn, and Co unite by preference with chlorinerather than with bromine and iodine, and with bromine rather thanwith iodine (under some circumstances Sr, Ba, and Co gives light inter-changes in the opposite direction).Zn, Cd, T1, Bi, Fe, and Ni showno constant rule of interchange. Cu, Ag, Hg, Sn, Pb, As, and S bunite by preference with iodine rather than with bromine or chlorine,and with bromine rather than with chlorine. A. J. G.Action of Chlorine on Organic Compounds in Presence ofInorganic Chlorides. By A. G. PAGE ( A m d e n , 225, 196-211).-Some years ago Arouheim showed that the presence of molybdenumpentachloride greatly facilitated the chIorination of aromatic com-pounds, but, from some preliminary experiments, did not appear tohave the same effect on the chlmination of fatty bodies (this Journnl,1876, i, 309).The author has continued this investigation andextended it to the emplojment of other inorganic chlorides.Chlorine does not act on acetic chloride, even in presence of molybORGASIC ClIE-\IIST RT. s7dennm pentachloride. The chlorination of butyric chloride atid ofethylene chloride is actually hindered by the presence of molybtleiiuiiichloride. Molybdenum trichloride does not assist chlorination belowt,he temperature (70') at which it is converted into pentachloride.Of the numerous other chlorides experimented with, the following onlywere found to assist chlorination : Fe2C16, Al2CI6, TlCI, and TICI, ;the chlorinating action of MoC1, and SbCl, is already well known.As regards the action of these bodies in assisting chlorination, theauthor regards the view that a molecular compound is formed betweenthe metallic chloride and the substance being chlorinated, whichcompound is i n the second place decomposed by chlorine with forma-tion of hydrochloric acid and a chlorinated product, as being moreprobable than that which is based on an alternate reduction andchlorination of the inorganic chloride.Chlorine has no action on nitrobenzene, but in presence of ferricchloride a t ordinary temperatures it converts it into the dichloronitro-benzene [Cl : C1 : NO, = 1 : 4 : 3j, and a t 100" into the tetrachloro-nitrobenzene [Cl : C1 : NO, : C1 : C1 = 1 : 2 : 3 : 4 : 51, whilst athigher temperatures it converts it completely into perchlorobenzene.Whilst chlorine acting alone on alcohol converts it chiefly intochloral alcoholate ; in the presence of ferric chloride, it converts it intoa mixture of chloral and (very little) chloral hydrate. A.J. G.Anthemene, a Hydrocarbon obtained from Roman Chamo-mile. By L. NAUDIN (Bzdl. SOC. C'hiln., 41, 483--$88).--From theflowers of ch2momile (Ant11,emis nobilis), the author has obtained twowhite crystalline substances, one of which appears to be a hydro-carbon. The flowers are exhausted completely with light petroleum,the solution thus obhained is evaporated to one-ninth of its bulk, andthe liquid residue allowed to stand. I n a few days, groups of whitecrystals of the new substance separate out, and in the mother-liquidare substances previously described by Demarpy, Fittig, and Kopp.The crystals were purified by recrystallisation from ether and lightpetroleum, and were found to consist of two substances.9 s oneof them is twenty-four times as soluble in absolute cold alcohol asthe other, they were separated by dissolving in hot alcohol, boilingwith animal charcoal, and filtering. Anthemene crystallises out o! Lcooling, and the second substance melting a t 188-189", the investigil-tion of which has not yet been completed, remains in solution. Theprocess of separation was yepeated twelve times. The yield is verysmall, for from 1 kilo. of t,he flowers the author only obtainetl1.5 grams of anthemene and 4.5 grams of the second substance.Anthemene crystallises in sleiider microscopic needles melting at63-64", and boiling a t about 440" without much decomposition ;sp.gr. 0.942 a t 15". It is insoluble in water, but soluble in ether,petroleum, carbon bisulphide, and chloroform, and soluble in hotabsolute alcohol, but almost iiisoluble in cold (at 25", 1 litre dissolves0.333 gram). The vapour-density by V. Mepx's method in thevapour of sulphur was 127 (theor. 131). The results of analysis givethe percentage of carbon 83.80, and of hydrogen 14.40, showing a lossof 1-80. Scliiitzenberger, who repeated the analyses, obtained simila38 ABSTRACTS O F CHEMICAL PAPERS.rcsults, and the author cannot account for this loss, as the compoundappears to be pure and to contain no oxygen. It appears to be of theser:es CnHIZn, and to be a p-octadecene (C 85-82? H 1418).Diethoxymethane, and Preparation of Methylene Dichloride.R.y W.H. GREENE (Chem. News, 50, 75--76).-The author has madecliethoxymethane from sodium ethylate and methylene dichloride.S ,dium, in equal molecular proportion, is added gradually to a mixtureof methylene chloride with excess of absolute alcohol contained in aflask fitted with reflux condenser ; when all the sodium has been added,the mixture is heated for an hour, and then distilled. The product isfractioned, and all which passes over below 78' is shaken with calciumchloride solution, the uppep layer separated, dried, and rectified, whenpure diethoxymethane is obtained boiling a t 86-89'. It is an etherealliquid with penetrating mint-like odour, boiling at @go under 769 mm.pressure.I t is slightly soluble in water,and miscible in all proportions with alcohol and ether.The following is recommended as the most convenient process forpreparing methylene chloride. A mixture of zinc and chloroformwith much alcohol is treated with a small quantity of hydrochloricacid in a flask fitted with a condenser ; heat is developed and chloro-form aiid methylene chloride distil over. When the reaction subsides,more hydrochloric a'cid is added, and a gentle heat is applied untilnear the completion of the operation, which is stopped when thealcohol commences to come over in large quantities. The distillateis rectified, the portion coming over below 53" being retained, whilstthe rdsidue is again treated with zinc, $c.This operation is repeatedseverd times, and ul timntely, by numerous careful rectifications ofthe product boiling below 53", pure methylene. chloride boiling at40-41" is obtained.A. B.Its sp. gr. at 0" is 0.851.D. A. L.Mercury Fulminate. By A. EHRENBERG ( J . pr. Chew., 30,38-G8).-Cnrstanjen and the author have shown (Abstr., 1882, 816) thatwhen mercury fulminate is decomposed with aqueous hydrochloricacid, it yields its nit'rogen as hydroxylamine lipdrochloride. A furtherexamination of this reaction bas proved that both carbonic oxide andcarbonic anhydride are formed. The quantit'y of t,hese compoundsproduced is but small, more especially when the decomposition iseI"fectcd in absence of air ; and it appears that they owe their originto the decomposition of formic acid, which the autbor has shown isproduced by the action of aqueous hydrochloric acid on mercuryfulminate. Tlie reaction taking place may be represented as follows :-C2HgNz02 + 2HC1+ 4HzO = 2H.COOH + 2NH1.OH + HgCI,.I n the hope of realising the following decomposiiion, and thusobtaining fulminic acid, C,HgN,O, + 2HC1 = HgCl, + C,H,N2O,, bheauthor passed dry hydrochloric acid gas into perfectly dry ether con-taining mercury fulminate in suspension.Mercuric chloride is pro-duced, and the ether holds in solution a compound which undergoesspontaneous decomposition, most probably fulminic acid. If thisethereal solution is carefully added to aqueous ammonia, and thORGAINIC CHEMISTRY.39ethereal solution separated from the aqueous solution, the lattercontains a yellow solid which is sparingly soluble in cold water, butsoluble in hot water, from which it may be obtained in yellowishneedles. The analysis of this compound shows it to be C3H,N,02 ; itforms with silver nitrate a cornpound, (C9H4N,0,),AgN03, insoluble incold water, and with an ammoniacal solution of copper oxids thecompound (C3H4N,02)2CuO(NH3)2, which is obtained as a light bluegranular precipitate. From the ammoniwal solution from which theabove compound was obtained, the author has isolated an acid isomericwith fulminuric acid, to which the name Isofulminuric acid is given.It is easily soluble in water, from which it separates in ill-definedcrystals ; absolute alcohol dissolves it easily, and by cooling the hotsaturated solution it is obtained as a white powder. With silvernitrate, its aqueous solution gives a white amorphous precipitate ofC3H,N303Ag, but yields no precipitates with ammoniacal solutionsof copper oxide, lead acetate, or mercuric chloride.The silver,ammonium, and barium ealts of this acid are described.Together with this acid, there is formed a small quantity of a com-pound more easily soluble in ether than isofulminuric acid, which ismost probably the ammonium salt of amidofulminuric acid,C3H (NH,)N,Os.NH,.Its aqueous solution gives precipitates with silver nitrate, lead acetate,and copper sulphate, and a blood-red to brownish-red coloration withferric chloride.Thiocyanic acid reacts with merciiry fulminate in a manner ana-logous to aqueous hydrochloric acid, mercuric thiocyanate, ammoniumthiooyanate, and carbonic anhydride are produced.the productionof the ammonium salts arising from the instability of hydroxylaminethiocj anate. The reaction may be represented thus :-C2HgNZ02 + 4H.CNS + 2HzO = 2CO? + Hg(CNS), + 2NHd.CNS.The action of ammonium thiocyanate on mercury fulminate isanalogous to the action of the chlorides of the alkali metals, but ismore energetic ; it may be expressed as follows :-2(CJT,OzHg) + 2HzO + 2NHk.CNS = C,H,N,O,.NH, + Hg(CNS), + HgO + CO, + 2NH3.Mercury Fulminate. By L. SCHOLVIEN ( J . pr. Chem., 30, 91-Y2).-A solution containing sodium fulminate is formed by treatingmercury fulminate suspended in water with sodium amalgam.Whenthis solution is decomposed with dilute sulphuric acid and shaken upwith ether, the ethereal solution is found to contain two acids of thecomposition HCNO. The less soluble of these crystallises from etherin colourless needles melting at 85" ; it is soluble in lukewarm watei,but is decomposed by boiling water. It forms a red insoluble silversalt, a dark yellow mercuric salt, and light yellow lead salt. Itssolutions yield a deep red coloration with ferric chloride. Decom-posed by hydrochloric acid, it yields hydroxylamine. The moresoluble isomeride may be crystnllised from hot water, jields noP. P. B40 ABSTRACTS OF CHENICAL PAPERS.coloration with ferric chloride, and forms no insoluble metallicsalts.The aqueous solution of sodium fulminate gives a precipitate clfsilver fulminate with silver nitrate, which when treated with metallic:chlorides and aniline hydrochloride forms double salts.It is decom-posed by ethyl iodide, and with potassium sulphide yields an easilyexplosive compound.Mercury fulminate and thiocarbamide yield carbonic anhydride,mercuric sulphide, carbamide, a compound thiocarbamide and mer-curic thiocyeuate. P. P. B.Rhodanic Acid. By M. NENCKI and BOURQUIN (Ber., 17, 2277-2282).-10 grams of rhodanic acid, C3H3NSz0, dissolved in 50 C.C. of90 per cent. alcohol, were mixed with 30 grams of strong sulphuricacid and heated on a water-bath ; 15 grams of benzaldehyde werethen added gradually. On cooling, or on the addition of water,BenzyZidene-~hod~iiic acid, C,oH7NSz0, crystallises out.When purifiedthis acid forms yellow needles, melting a t 200" (uncorr.). It givescrystalline salts with the alkalis, very easily soluble in alcohol andwater, less so in concentrated alkalis. It forms a yellowish-greensilver salt, CloH6AgNSz0, and an amorphous lead salt. The reactiontakes place according to the equationC3HJYS,O + C,H,.COH= CJT7NS20 + HZO.Acetaldehyde or its ammonia-compound similarly yields ethylidene-rhodanic acid, C,H,NS,O. This substance forms small yellow needles,melting a t 147-148". It is very sparingly soluble in water, easily inalcohol. Both of these com-pounds are decomposed when heated with alkalis, the aldehydesbeing reformed and the rhodanic acid further decomposed.Salicy 1-aldehyde and parahydroxybenzaldehyde also form similar condensa-t.ion-compounds, but these have not been investigated.When heated with water a t 200' in closed tubes, rhodanic acidis split up into carbonic anhydride, sulphuretted hydrogen, andammonium thioglycollate. When warmed with alkalis, it is readilydecomposed, potassium thiocyanate and a crystalliiie potassium (orsodium) salt sparingly soluble in alcohol being the products. Theacid or' which this is the salt appears to have the composition of ananhydride of thioglycollic acid, and to be of the formula(SH. CH2. CO),O.This acid is now undergoing investigation.As this formation of thiocyanic acid by the action of alkalis takesplace a t so low a temperature, there can be little doubt that the thio-It gives a yellow amorphous lead suZt.Ljanic group is already present in rhodanic acid.The formulaS 1 C<:$zF>CO, proposed by Liebermann, is therefore very im-probable, and that originally proposed by Nencki, SH.CH,.CO.S.CN,is in all probability the correct one.Circular Polarisation of Dextrose. By R. TOLLENS (Bey., 17,22%--2238).-1n continuation of his investigations with cane- sugarL. T. TOItGANIC CHEMISTRY. 41(Abstr., 1884,1285), the aut'hor has now examined very dilute soIutionsof dextrose. He finds that here, as in the case of cane-sugar, no increaseof rotation takes place, but that the same formula may be employecifor calcnlaiing the rotation whatever the degree of concentration ofthe solution.The dextrose employed was very carefully purified bythe method recommended by Soxhlet, and was purer than that pre-viously used. The author has therefore slightly amended his oldi'orrnuke, which now become-A (for anbydrous dextrose) [ a ] D = 52.50" + 0.018796P +B (for dextrose hjdrate) [%ID = 47.73" + 0.015534P +The following table gives a comparison between the results actually0-00051tXGP2.0.0003883P2.found with a Landolt-Laurent polarimeter and those calculated :-Weight of sugar in Rotation for [~ID.1.49 78 5 2*4( I 7 52.53d0 - 0.125"1.7933 52.289 52,537 - 0.2482.7533 52.370 52.556 - 0.1867.6042 52.691 52.673 + 0.01810.0992 52.738 52.742 + 0.00410,2567 5 2- 63 ti 52.747 - 0.11117.5982 52.991 52391 - 0~000100 grains solution.7--- -7 P. Found. Calculnt ed. Difference.L. T. T.Non-identity of Arabinose and Galactose. By E. 0. v. LIYP-MANN (Ber., 17, 2238-2240).-The author confirms Scheibler'sresults as to the non-identity of these two compounds. Galactoseforms large, hard, well-formed prisms melting a t 148" ; arabinoselong, fragile needles melting a t 160'. Arabinose has a sweetertaste than galactose. The rotation of arabinose in a 10 per cent.solution is [@ID = +105*4", [ a ] j = +lB" of galactose, +81*5" and + 92" respectively. Arabinose shows no birotation, galactose does ;a fresh solution having given [a],, = 134.5". Fermentation is easilyset up in solutions of galactose by means of yeast, but arabiriosecannot be fermented.When oxidised with nitric acid, arabinoseyields only oxnlic acid, while galactose forms mucic acid. Thereducing power of arabinose for E'ehling's solution is also greater thanthat, of galactose.With regard to the existence of the four arabinoses described byC. O'Sullivan (Trans., 1884, 41, et q.), the author calls attention tothe existence of unstable intermediate products (such as cerasinose,which is gradually converted, even in the crystalline form, into arabin-ose) analogous to these compounds, and suggests that the variousarabinoses may actually exist, and not be mere mixtures of arabinoseInfluence of Temperature and Concentration of Hydrochlo-By I?,with galactose as Scheiblei- believes. L. T. 1'.ric Acid on the Rdte of Inversion of Saccharose.(11)42 ABSTRACTS OF CHEIIICAL PAPERS.UKECH (Bey., 17, 2165-2178). The author refers to his previousexperiments (Abstr., 1883, 174), t,he results of which he now repre-sents byv means of ciirves and tables. A. K. M.'' Hydrate of Carbon '* from Cast Iron. By ZABOUDSKT (BdZ.ROC. Chim., 41,424-4%3).-A very pure specimen OF Swedish specularcast iron, free even from traces of graphite, phosphorus, or sulphur,but containing 0.23 per cent. of silicon and 4.1 per cent. of combinedcarbon, when treated with a mixture of copper sulphate and sodiumchloride yielded 5.72-5-79 per cent. of a *' hydrate of carbon," whichcontained C 71.6 ; H,O 86.9 ; siliceous ash 1.25 per cent,. These resultsapproximate to the formula C,,H,O,. Treatment of the steel withother reagents, silver nitrate, mercuric chloride, atmospheric air, andby Weyl's method, gave rise to the formation of an analogous sub-stance.The hydrate is not changed when heated in a closed tube to15C)", and although it gradually loses weight when further heated, at325" losing carbon a s well as water, it retains hydrogen and oxygeneven after being heated in a ba6h of metallic antimony. Heated in acurrent of hjdrogen, the compound lost considerabl7 in weight, butafter prolonged action the residue still contained hydrogen to theextent of nearly 3 per cent. The compound is insoluble in water,alcohol, ether, sulptiuric and hydrochloric acids. It is completelydissolved by warm nitric acid, forming a substance which probablyhas the formula C,,H,,(NO,) O1,.This body dissolves easily inalcohol and in nitric acid. It is insoluble in ether, but is dissolvedby alkalis, forming a, dark brown solution, from which hydrochloricacid precipitates the original compound apparently unchanged. Thisnitro-compound gives an odour of hydrogen cjanide when heated.Chlorine, bromine, and iodine also act on the hydrate of carbon ; theiodo-derivative probably has the formula C6aH2,10,5. W. R. D.Angelic and Tiglic Acids. By F. BEILSTEIN and E. WIEGAND(Bey., 17, 2261-2263) .-The authors have examined the productsproduced by the oxidation of these acids with potassium permanganate,in the hope of learning something of their respective constitutions.Aldehyde and acetic acid were formed in both cases ; the only differ-ence being that with angelic acid a very small quantity of a non-volatile acid yielding an amorphous barium salt was formed.The acids were prepared by Kopp's process from roman oil of chamo-mile (Abstr., 1879, 454), and their ethers were also made.Ethyl angelate is an aromatic liquid boiling a t 141.5" and having asp.gr. of 0.9347 at 0".3:tlzyZ tiglate boils at 152" and has a sp. gr. of 0.9425 at 0".Halogen-derivatives of Ethyl Levulinate. By M. CONRAD and31. GU'I'HZEIT (Bey., 17, 2285-2237).-With reference to the com-munication of Hell and Kebrer (Abstr., 1884, 1297), on the action ofbromine on levulinic acid, the authors publish this account of somesimilar work carried out simultaneously and independently by them-selves.Bth y 1 monobromoleculinate, CsHllBrOs, was obtained by graduallyL.T. TORGANIC CHEMISTRT. 43adding 16 grams of bromine to 14.4 grams of ethyl levulinatetLlutcd with 2.5 C.C. of ether, the whole being kept cool by means ofice. T t boils with partial decomposition at 240", and has a sp. gr. of1.430 at 1.5" compared with H,O at the same temperature. It entersinto reaction with ethgl sodomalonate, forming a colourless oil of thefor mu In ( C: 0 0 E t) ,C H. CIH,O. C: 00 E t, boiling at 280--285", a11 d havingthe sp. gr. 1.097 at 15". Ethyl monobromolevulinate absorbs morebromine and, as end-product, the authors obtained a mixture of thed i- and t ri- bromo- derivatives. E t h y 1 monoc hlorolevuli n ate, preparedi n R similar manner, is a colourless oil insoluble in water.It boils at225--230°, and has the sp. gr. 1.196 at 15". L. T. T.Adipic Acid, By W. DIETFRLE and C. BELL (Bey., 17, 2221-22&3).-1n continuation of the researches of Gantter and Hell 00suberic arid azelaic acids, t'he authors have investigated adipic acid,the third of the higher dibasic 2cids obtained in the oxidation of fats.The adipic acid was prep:ired from the mother-liquors obtained inthe preparation of suberic acid from castor-oil and other fats.Adipic acid is much less solublc in ether than suberio acid, butmuch more soluble in water. Tlre two acids can be therefore easilyseparated by successive crystallisations from these two solveuts. Theadipic acid thus obtained is still slightly yellow, and is purified bycrystallisation from strong aitric acid or by conversion into its salts.Adipic acid melts at 148-149", aiid solidifies to a crystalline fibrousmass.At 15", 1VO parts of water dissolve 1.44 parts of acid; 100parts of ether, 0.633 part of acid. Adipic acid has a very greattendency to form supersaturated solutions. It is not t-olat'ile insteam, but can be distilled alone withont decomposition. It is onlyattacked by bromine above 15U0, but i! about 0.3 per cent. amorphousphosphorus is added, broniiriation takes place at the temperature ofthe water- ba th.The potassium salt. K,C,H,O,, forms deliquescent crystals ; thesodium salt, mother-3f-pearl-liLe scales contaiuirrg +HzC), and easilysoluble in water. l'he ammonium salt is much more stable than thecorresponding salts of ;Juberic and azelaic acids, and may be evapo-rated without decomposition.I t crystallises in scales, and at 14", 100parts of water dissolve 39-97 of the salt : at, loo", it loses half its ammo-nia, the acid salt beiiig formed, and at 120-150", the rest of theammonia escapes and the puve ;reid is left. The bt-crium salt is lesssoluble in hot tharl in cold water, 100 parts of water dissolving 12-04!parts of salt at, 1jo, and only 7.47 at 100". The strontium salt formsprismatic prisms containing +H20 : 100 parts of water dissolve 13.61])arts of the anhydrous salt, at 14", and 2.r2 at 100". The cnlciumsaltc.rystallises with 1H20 : 100 parts of water dissolve 4.02 parts of theanhydrous salts at 13", 4.09 at li'", and 1.20 at 100".The mngnesiurn. d t crystallises with 4H,O : 100 parts of water dissolve 25.01 parts at15", and 21.71 at 100". The aluminium and ferric salts form volu-minous and a1 most insoluble precipitates. The 7nanJanese snlf mica-c'eous crystals containing 2H20, or, i f deposited at, high temperatures,IH,O : 100 parts of water dissolve 12.63 parts of the anhydrous salta t 18", and 2.71 at 100". The nic7ceZ salt yields apple-green scale44 ABSTRACTS OF CHEMICAL PAPERS.containing 4H20, and only loses the last. molecule completely a t 140" :100 parts of water dissolve 0.65 part of anhydrous salt a t 15", 4.07parts a t 100". The cobalt salt forms pale red prisms containing 4H02,which it loses a t 110": the anhydrous salt is of an intense bluish-violet colour: 100 parts of water dissolve 1.56 parts a t 15", 3.09 a t100".The zinc salt crptallises with 2H20 : 100 parts of water dis-solve 0.261 part a t 10" and 0.217 at 100". The copper salt forms itvoluminons bluish-green precipitate : when this is quickly pressedand dried, it, contains 1 mol. H20, but if allowed to remain undeywater takes up another mol. H20 and then forms small deep bluecrystals: 100 parts of water dissolve 0.024 part of the anhydroussalt a t 15", 0.089 a t 17", and 0.063 a t 100". The lead salt forms ananhydrous white precipitate : 100 parts of water dissolve 0.0206 partat l2*5", 0.0217 at 16", and 0-0217 at 100". The wereuric salt formsa n anhydrous crystalline precipitate : 100 parts of water dissolve0.0287 part at 11", 0.0125 at 1OU".The silver salt is stable towardslight, and forms sninll glittering scales : 100 parts of water dissolve0.0166 part a t 14";and 0.0491 a t 100".The sa?ts OP the heavier metals were mostly prepared by doubledecomposition. Precipitation often takes place very slowly in thecold, but is accelerated by stirring or heating the solution. The saltsof adipic acid resemble those of suberic acid in many respects, butthey are all more soluble than the latter. IJ. T. T.Normal Butylmalonic Acid : a New Isomeric Pimelic Acid.By C. HELL and G. LUMPP (Ber., 17, 2217-22PO).-To prepare thisacid, normal caproic acid is heated with bromine at 130", the mono-bromocaproic acid obtained is converted into the ethyl salt, and thisis boiled for one and a half to two days with a dilute alcoholic sol-u-tion of pure potassium o r sodium cyanide, the nitrile thus formed beingsaponified by boiling witah aqueous potash.Bufy ZmaZoriir, acid,C,81204, crystallises from water in thick prisms, melts a t 101*5", andis readily soluble in water, alcohol, and ether. On warming it or itssalts with concentrated sulphuric acid, they assume a red to violetcoloration. When butylmalonic acid is heated, it readily splits upinto carbonic anhydride and caproic acid, the decomposition beginninga t st little below 140", and being complete a t 150" ; the readiness withwhich this acid is decomposed distinguishes it from the pimelic acidobtained from fats, which may be distilled without decornposition.The barium salt, C7HIU04Ba, crystallises in white anhydrous scales ;solubility at 24", 2.98 parts salt in 100 parts water, and apparentlyless solnble in hot than in cold water.The Zead salt, C7HJI4Pb, isprecipitated in lustrous white crystalline scales, 100 parts of waterdissolving a t 20" only 0.0112 part salt. The si2ver salt, C,H,,O4Ag2,forms a voluminons pulverulent precipitate, 0.1 19 part dissolving in100 parts water at 23". The cqper. salt, C,H,,O,Cu, forms blue scalescontaining 1 rnol. H,O.Occurrence of Pimelic Acid amongst the Oxidation-productsof Castor-oil. By F. GAKTTER and C. HELL (Ber., 17, 2212--2217).-Arppe showed that the so-called pimelic acid obtained by the actiouA. K. MORGASIC CXEMISTE1T. 45of nitric acid on oleic acid and fatty bodies was a mixture of adipicaud suberic acids.The author has obtained it, however, in consider-able quantity by the oxidation of castor-oil by nitric acid. The moresparingly soluble acids are first separated, and the syrupy mother-1 iquor is largely diluted with water, nen tralised with chalk, filtered,and concentrated. The calcium salt obtained is decomposed with acid,when a partly oily and partly crystalline product separates, and maybe purified by alternate treatment with ether and water. Pimelicacid, which may also be obtained by the oxidation of earth-nut oil,crystallises from water in clusters of large flat plates, which melt a t105*5-106", and solidify t o a crystalline mass, which suddenly falls topieces with the slightest touch.The blxrium salt, C7Hl,04Ba,H,0,crystallises in white indistinct scales ; the Zeud salt, C,H,,O,Pb, andt,he silrer salt, C7Hl0O4Ag2, form white pulverulent precipitates ; andthe coyper saZt, CjH-loOICu, a green precipitate. The pimelic acidappears to be distinct from all the acids of the composition CjH1,O6hit,herto described ; its properties approximate most to those of Banerand Schuler's isopimelic acid (from amyleno bromide), but a moreextended comparison of the two is necessary to decide the question ofidentity. A. K. &I.Chelidonic Acid. By J. U. LERCH (Xonatsh. Chem., 5, 367-$l$)--The author refers to his previous work, and claims prioritybefore Haitiiiger and Lieben (see next Abstract).The ethyl salts were prepared by the usual methods; the diethy;!saZt, CjEf,O,Et,, melts a t 62"; the wtouetliyl salt, also formed bydecomposition of the preceding, melts a t 182-184"; its lead andsilver salts, C7H,0GEtAg, are cyystalline.The diethyl salt, dissolvedin alcohol, gives with ammonia a yellow solution, and then whitecrystals, probably the amide of chelidonic acid, C,H,O,(NH,),. Theyellow solution obtained by adding excess of potash to chelidonicacid is gradually decomposed, even at ordinary temperatures, intooxalic acid and acetone ; the acid is also decomposed by bromine andchlorine, oxalic acid and substituted acetones being formed. Potashgradually added to water containing calcium chelidonate in suspen-sion converts the whole into a stiff yellow jelly, without the forinationof oxalic acid and acetone ; it is a potassium calcium salt of che&hydronic acid (xanthochelidonic acid of Haitinger and Lieben), and ismore applicable for further preparation work than the easily decom-posable potassium salt.The free acid can only be prepared withgreat difficulty ; the gelatinous potassium calcium salt is treated withsulphuric acid, and fractionally extracted from ether ; from the secondand following ethereal extracts it is obtained as a pale yellow amorphousmass. By neutralising the gelatinous potassium-calcium salt wit13acetic acid, the calcium salt, C7H20,Ca2, is obtained as a citron-yellowprecipitate. Chelihydronic acid neutralised with ammonia givesa red solution, from which a crystalline arnmouiurn salt may beobtained.This red solution gives, with silver nitrate, a yellowprecipitate, CJl307AgS + 4N20, which by boiling is converted into abrown precipitate, C;H207Ag+ If in the above the chelihydronicacid be replaced by the gelatinous calcium potaasium salt, silve46 ABSTRACTS OF CHEMICAL PAPERS.precipitates having the same colour are obtained; but they aredouble salts, viz., yellow, (C7H307Ag),Ca + 4H20, and brown,(C7H307Ag3)2Ca, whilht lead and barium solutions also produceyellow precipitates of tlie composition (C7H207)4Pb5Ca3 + 6H,O andC7H,O7BaCa ; the calcium potassium salt precipitated from its solu-tion by alcohol has the composition (C7H2O7),Ca,R2 + 2H20. Cheli-hydronic acid has therefore the composition C7H6O7, and containsthree or four hydrogen-atoms that may be replaced by metals.Chelidonic acid evaporated with ammonia gives the ammonium saltof chelidammic acid, whose salts are also formed by the action ofammonia on the clielidonates. Hydrochloric acid added to a solution ofthe ammonium salt produces a precipitate of tlie formula CI,H,,N30,, ;this is a compound of the free acid with its ammonium salt, C7H,N0, + C7H,N0,.NH4 ; i t seems to be monoclinic, and dissolves in 1576 partsof cold water.By boiling this substance with potash, and then acidify-i n g , the cornpourid C7H7NO6 separates; this is a hydrate of the freeacid, C,H5N0, + H,O ; i t crystdlises in rhombic prihms, and dissolr-esi n 637 parts of cold water. Ethyl chelidnnzniate, C,H,N05Et, + H,O,melts a t 80- -81", and becomes anhydrous in a vacuuxn.Although theacid coutains only two acid hydroxyl-groups, i t forms three classes ofsalts ; the following are described :-C7H2N0,Pb(NH,) ; (C,H,XO,),Pb,;+ 3H20 ; C,H,NO,Ags ; C7HANOSC& + 2H20 ; (C7H2N05)2Ca, ;C,H,N05Ca (NTIJ + 2H20.When chelidammic acid is treated -with the halogens, i t yields hi-substitution-products. Bro,nocheZidummic acid, C7H,Br2N0, + 2H20,forms large efflorescent crystals ; its silver salt is C7HBr,N05Sg,.ChZorocheZiJammic mid, C7H3C12N05 + H 8 , forms long fibrous cr-j-stals ;i t s silver and lead salts are C7Cl,N0,Ag, and (C7C12N05),Pb3. Iodo-chelidanimic acid is obtained by dissolving chelidammic acid in analkali, saturating with iodine, and then acidifying; its formula isChelidammic acid at 250" loses carbonic anhydride, and there remainsa crystalline mass of chelmnide ( h y d r o z ~ p y r i d t n e ) , C,H,NO, melting at95-96', and therefore different from the hydroxypyridines of Ost,of Fischer and Korner, and of Konig and Geigy, which melt at 14b",123.5", and 107".When crystallised from water: it has the formulaC5H5NO + H,O. Heated with zinc-dust, i t yields pyridine. Thedouble salts ( C5H5NO)?,H2P~C16 + H,O ; C5HJV0,N03H,AgN0, ;C,H,N 0,HgC12 ; and the hydrochloride, C5H5N0,HCI, are described.Chelidonic acid is also acted on by aniline, producing a crystallinebody. Aniline chelidonate when heated evolves carbonic anhydride,and leaves a crystalline residue which after recrystnllisation from wateim,has the cornposition CIIHSNO + 2H20 ; this anilide, bowever, does notform eitlier single or double salts.Following is a discussion of the constitution of these bodies ; thefollowing forniuk are aclvocat ed :-C7H3N0,Pb; C7H:,NOjPbAg; (C7H,N05)2Pb$a+ 3H20; CTH2NO5PbKc7 H 312N 0 5 .0 Chelidonic acid, C00H.CH : CChelihydronic acid, COOH.CH : CCH.C(COOH)<Cd>.CH.C(OH)(COOH),ORGANlC CHEJIISTRY.47Chelidammic acid, C00H.CH : C : CH.C(COOH)/ Ii'C.OHH. R.Chelidonic Acid. Bg HAITINGER and A. LIEBEN (Nonatsh.Chem., 5, 339-3GG).-Reference is made to all previous work on thesubject. Lietzenmayer's method for isolating the acid was used.The free acid suspended i n alcohol and hydrochloric acid gas passedthrough, the solution evaporated and the residue dissolved in alcoholdeposits monethyl chelidonate, the diethyl salt remaining in solution.The diethyl saZt, C7H,06Et2, forms crystals melting at 62.7".Thenzon~thyl salt, C7H,0,Et, is crystalline, melts a t 223--224O, and itsalcoholic solution has an acid reaction. Chelidonic acid is dibasic,and not tribasic.It has been previously shown t h a t when chelidonic acid is heatedwith x l k a h or, much better, alkaline earths, it yields acetone andosalic acid. This has been rigorously confirmed, and it is alsoshown that the reaction proceeds exactly according to the equationC7H,06 + 3H,O = 2C,04H2 + C3H60.When chelidonic acid is treated with potash solution, a transientyellow coloration is produced with each addition, until two molecularproportions of the potassium salt have been addtd, i.p., until the neutralsalt of the bibasic chelidonic acid has been formed.Further addition ofpotash produces a permanent yellow coloration, hiit the solution doesnot remain alkaline until more than three molecular proportionsof potassium hydroxide hare been added. This pellnw soluiion con-tains the potassium salt of a new acid, zccnfhocheZidorric arid. If thissolution is acidified with acetic acid, it gives a yelluw precipitate,C,H,Pb2O5 + H20, with lead acetate ; tetrabasic calcium and silversalts could not be prepared. BJ acidifying a solution of chelidonicacid in excess of caustic potash with nitric acid, a light yellowcrjstalline deposit of an acid potassium salt, CiH5EOi, was obtained.The free acid cannot be isolated from its salts, since by the additionof an acid i t is at o ~ c e partly converted into chelidonic acid, and stiilmore so on standing.If chelidonic acid is treated with hydriodic acid, it yields pimelicacid (probably the normal acid).When it is heated with zinc andacetic acid, and the zinc removed by sulphuretted hydrogen, a n acid,hydrochelidork acid, C7H1,,O5, is obtained. This is colourless, crys-ta,iline, melts a t 142", and can be distilled unchanged. The zinc salt,CiH,OjZn + 2H20, is hut slightly soluble in cold water, and crys-tallises in small monoclinic tables,a: b : c = 1.0292: 1 :1*737; ,8 = 89" 7.5'; O P . 032m. m$2.also - Pa. Pm .322.The calcium salt, C7H,05Ca -+ H20, is indistinctly crystalline.Thesilver salt is C7H805Ag2 ; the copper, lead, and mercurous salts arealso mentioned.An alkaline solution of hydrochelidonic acid was treated mithpotassium permanganate, and oxalic and succinic acids obtained, i48 ABSTRACTS OF CHEMICAL PAPERS.accordance with the equation C,H,,05 + 60 = C204H2 + C,H,O, +COZ + H2O.Hydrocheliclonic acid heated with a saturated solution of hydriodicacid a t 200-210" is in greatest part reduced topirnclic acid, C,Kl2O4,which is obtained by simple evaporation ; it melts a t 1029- 103*9",and forms monoclinic crystals,a : b : c = 3.691 : 1 : 2.058 ; p = 103" 33' ; mPm . OP . mP . P .It is probably the normal acid. During the reduction, a smallquantity of a hydrocarbon is also formed.An alkaline solution of sodium xanthochelidonate was reduced withsodium amalgam, and the new sodium salt precipitated from theconcentrated solution by alcohol.The silver salt was found to havethe formula Ag,C7Hlo07, hence hydroxa,nthoclzelidonic acid must havethe composition C7H12a ; it is a syrupy liquid. Heated with hydriodicacid, it also acts like hydrochelidonic acid and chelidonic acid,I f chelidonic acid is heated a t 240" it loses 2 mols. CO,, and gives asdistillate a body melting at 32.5", and boiling a t 215". With aqueousammonia it gives hydroxypjridine (Mormtsh. Chem., 1883, 339),and tliere is no doubt that it is identical wit>h Ost's pyroconiene( J . pr. Chem., 29, 63), thus showing a connection between chelidonicand meconic acids.Chelidonic acid is certainly dibasic ; the pimelic acid referred to isprobably the normal acid, and by boiling with an alkali chelidonicacid jields oxalic acid and acetone.These and other facts are explained11;- the constitutional formulae :-CO0H.C-0-C.CO0HI-IC I1 . C 0. CH II COOH.CH<~~>CH(CEI,),.COOHChelidonic acid. Hydrochelidonic acid.CO[CH: C(OH).COOH], 0 H . C H[ Cl H,. C H ( OH). C 0 OH]H. B.Xanthochelidonic acid. Hydroxant.hochelidonic acid.Nitrogenous Derivatives of Meconic Acid. By H. OST (J. pr.Ch~m. [2], 29, 57--69).-1n previous papers (Abstr., 1879, 708, and1883, 791), the author has described those nitrogenous compoundswhich are readily obtainable from meconic acid, as substitutedproducts of a hypothetical pyridoue :-Pyridone, C5HSNO.Pyromecazonic acid, C,H,NO(OH),.Comenamic acid, C5H3NO(OH) (COOH).The author now shows that pyridone is hydroxypyridine, thatpyromecazonic acid is a trihydroxypyvridine, and comenamic acid adihydroxypyridinecarboxylic acid.BJthyl dkcetylcomenamale, C5HzN( O?G),.COOEt, was prepared byboiling ethyl comenamate with excess of acetic anhydride and thenevaporating- The diacetyl-compound melts at 38', whilst thORQANIC CHEMISTRY.49monacetyl-derivative, which is formed when the above mixture is onlywarmed, melts a t 152". Both compounds are decomposed by water oralcohol in the cold, with liberation of acetic acid.The ethyl dibenxoyZcomennmate, which is ohtained by boiling ethylconienamate with benzoic chloride, melts a t 102", and is more stablethan the acetpl-compounds.Since the existence of these diacetyl- and dibenzoy 1-compoundsdoes not conclusively prove that comenamic acid contains twohydroxyl and not one hydroxyl and one imido-group, the isolation ofpyridone was next proceeded with and accomplished by means of thea c ~ d C6H2C1202, to which the author gives the nnme of dichlorocomanicacid, comanic acid, C5H302.COOH, being comenic acid in which thehydroxyl is replaced by hvdrogen.Dichlomconzanic acid, C,HCl,O,.COOH, is prepared by heatingcomenic acid with 4 mols.of phosphorus pentacliloride and oxy-chloride, using a reflux condenser, until no more hydrochloric acid isevolved; on then distilling to 150" an oil remains behind whichyields the acid when decomposed with warm water.When purified,by crystallisation from alcohol, the acid forms voliiminous needlesmelting a t 217". A small quantit,y of monochlorocomanic acid isformed a t the same time; this crystallises in needles, and melts a t247".Coma& acid, C5H,02.COOIT, is obtained by boiIing the dichlor-iiiated acid for several hours with rather more than the theoreticalproportion of aqueous hydriodic acid (b. p. 1 2 i 0 ) ; the iodine is thendriven off in a current of steam, and on evaporating the solution theacid crystallises out in small nodules. The pure acid forms smalloblique prisms melting at 250" with violent evolution of gas. It givesno coloration with ferric chloride. The barium, silver, and ethylsalts are described ; the latter melts a t 103", and is not acted on byacctic anbydride or chloride.This shows that comanic acid is nota hydroxy acid, although barium hydroxide precipitates a basic salt,which, however, is derived from another acid into which comanicacid is readily converted by strong bases, and which gives a darkbrown-red coloration with ferric chloride. On heating it with excessof barium hydroxide, the precipitate formed is rapidly converted intobarium oxdate: acetone being formed also ; in this respect, comanicresembles chelidonic acid (Abstr., 1883, 8'70). When comanic acidis heated, carbonic anhydride is evolved, arid it is converted intorocomane, C5H402, a neutral body soluble in water, melting a t :go, and boiling a t 210-215".On gently heating comanic acid withstrong ammoilia, i t is readily converted into P-hydroxypicolinicacid, C,H,N( OH).COOH, which has already been described (Abstr.,1883, 791). Since this acid can also be obtained from pentachloro-picoline, there is no doubt that i t is hydroxypyridinecarboxSlicacid. I n a similar manner, although less readily, ammonia acts oncornenic acid, jielding comenamic acid, C,H,N( OH),.COOH, and onhydroxjcoinenic acid, yielding hjdroxycomenarriic acid,C,HN(OH),.COOH ;this proves that cornenamic acid is a dihydroxy-, and hydroxF-VOL. X L ~ X l : . 50 ABSTRACTS O F CHEJIICAL PAPERS.comenamic acid a trihydroxy-pyridinecarboxylic acid ; both theseacids, moreover, belong to the a-pyridinecarboxylic series.Hydroxypyridine, C5H4N.0H, is obtained from p-hydroxypicolinicacid by heating it above its melting point, carbonic anhydride beingevolved.It crystallises in small grains melting a t 148", is easilysoluble in water and alcohol. has a neutral reaction, combines withacids, and forms a platinocbloride crystallising in large rectangularprisms. This hydroxypyridine is identical with t,hat obtained byLieben and Haitinger (Abstr., 1883, 870). The following is a list ofthe nitrogenous derivatives of meconic acid :-E y drmjpyridines.C,H,N 0 H, h y drox yp yri dine.C5HtE,N(OH)?, dihydroxypyridine, pyrocomenamic acid.C,H,N (0 H) 3, trihy drox ypyridine, pyromecazonic acid.C5H2N02.0H, hydroxypyridinequinone, pyromecazone.C,HN(OH),, tetrahydroxypyridine (?), hydroxypyromecazonic acid.C,H,NMe(OH)a, dihydroxypicoline, methyldihydroxypyridonc(Abstr., this vol., p.$40).H ~ d r o x ~ p ~ r i d i e ~ ~ ~ o x y l ~ c Acids.C5K3N( OH).COOH, /3-hydroxypicolir1ic acid (and the isomeric a- andC5H,N(OH),.COOH, dihydroxypieolinie acid, comenamic acid.C,HN(OH),.COOH, trihydroxypicolinic acid, hydroxycomeriamicC,HNO,(OH).COOH, hydroxypicolinic acid quinone, azonecar-yacids).acid.hoxylic acid. P. F. F.Beta'ine in Cotton Seed. Bey H. RLTTHATJSEN and F. WEGEB ( J .pr. Cllem., 30, 32-37) .-The authors have succeeded in obtainingbetn'ine from the cotton seed, by trcatment of the mothcr-liquors fromwhich melitose had been separated (J. pr. Chew,., 29, 351). Theauthors have not, as yet determined in what form the betaine occursin t h e cotton seed.P. P. B.Seleniocarbarnide. By A. VERNEUIL (BUZZ. Xw. CIiem., 41, 599).-This compouud may be prepared by the action of hydrogenselenide on cyanamide. The latter dissolved in ether absorbs thegas completely in the cold, and after a short time crystals are depositedand finally the liquid becomes solid. The react,ion is facilitated bythe presence of a small quantity of ammonia. The compoundpurified by two crystallisations from boiling water forms whitecrystals which assnme a rose tint when exposed to light. Selenio-carbamide is very soluble in hot water, less so in cold, which dissolves10 7 per cent. at 19". Absolute alcohoI dissolves 28 per cert. a t 18",and ether 0.56 per cent. a t the same temperature, When rapidlyheated, the compouud melts without any apparent decomposition, butif slowly heated it melts at about 200" with decomposition.W.R. D.The Thiophene Group. By R. NAHXSEN ( B e y . , 17, 2197-219s).-The author has prepared larger quantities of dithiertSl (Abstr.ORGANIC CHEMISTRY. 511884, 1132), and has submitted it to a more thorough examinationthan was previously possible. It crystallises from hot alcohol 01'glacial acetic acid in silky scales, melts at 83", and boils at, 266".I t s solution in concentrated sulphuric acid is reddish-brown intrnnsmitt'ed and deep-green by reflected light, and in pouring thesolution into water dithienyl separates unchanged. Dith ienyl-sdpholzic acid. C8H5S2.S0,3H, is obtained by heating dithienyl with20 times its weight of sulphuric acid.(C,H,S,.SO,),Ba,is obtained as a ci-ystalline mass and is hygroscopic ; the potassi?lmsn7t is deliquescent arid yields dithienyl when distilled with ammoniumchloride. Perbroinodithienyl, CeBr& is prepared by beating a solu-tion of ditbienyl in glacial acetic acid with an excess of bromine.It, is very sparingly soluble in hot alcohol and i n cold benzene,~eadily in boiling benzene, from which it crjstdlises in small needlesmelting a t 235" (uncorr.).The bariutn saltA. K. 3f.p-Thiophenic Acid. By R. NAHNSEN (Ber;, 17, 2192-2196).-A thiophenic acid was prepared by Meyer and Kreis from thio-phenesulphonic acid by Merz's method (Abstr., 1884, 46). I n theliopes of obtaining larger quantities of this acid, tlie author submitteda mixture of iodotliiophene and ethyl chlorocarbonate to the action ofsodium amalgam. The reaction takes place much more readily thanin the case of Wurtz's synthesis of benzoic acid.The product issteam-distilled, the distillate extracted with ether, and the oilobtained is boiled for five hours with concentrated aqueous potash : thesolution is diluted, separatJed from the uiiattacked iodothiophene,supersaturated with sulphuric acid, and extracted with ether. Thethiophenic acid, C*H,S.COOH, obtained is, however, isomeric miththat obtained by Meyer and Kreis, and melts constantly a t 129". Theacid prepared from the sulphonate is assumed to be all a-derivative, inwhich case the new acid would be /j-thiophenic acid, thus:CH- CH CH- CH>S.I 1s.C(CO0H) : CH/ IC'H : C(CO0H)a-Thioplienic acid. a-Thiophenic acid.B-Thiophenic acid closely resembles benzoic acid. It crystallises incolourless needles, can be sublimed, and distils at, 260" ; it yields ablue solution when heated with sulphuric acid and isatin. It giveswhite precipitates with silver nitrate, lead acetate, and mercurousnitrate, and a very bulky yellow precipitate with ferric chloride;ivliilst copper, cadmium, zinc, ferrous, cobal t, nickel, mercuric,barium, calcium, and magnesium salts produce no precipitate. Thesilver salt, C,H,S.COOAg, foiwms lustrous transparent scales 01-l~eedles somewhat soluble i n hot, sparingly in cold water; the c u l c i u p ~s(11t, (C,H,S COO)LCa,3H,0, is readily soluble in water, and separatesin clusters of lanceolate crjstals ; the barizlm s d t ,(C4R$3.COO)2Ba,2H20,€ 52 ABSTRACTS OF CHEXICAL PAYERS.forms small lustrous crystals readily soluble in water. The chloride,C,H,S.COCl, is a colourless liquid boiling a t 190" (uncorr.), and hasthe same penetrating odour as benzoic chloride ; the ethyl salt,is a colourless, strongly refracting liquid, boils a t 218" ( o r r .) , andhas an odour closely resembling that of ethyl benzoate. P-Thiophen-amide, C4B3S.CON H,, forms dense prisms melting a t 180" (uncorr.).When /iI-thiophcnic acid is nit'rated and the product crystallised fromwater, dense yellow prisms, CIH2S(NOr).COOH, first crystallise out,,and afterwards long needles.A. K. M.Action of Chlorine on Boiling Benzene. By R. SCHUPPHAUS(Ber., 17, 2256--2260).--Meunier (Abstr., 1884, 733) has describeda compound obtained in the preparation of benzene hexachloride, andhas ascribed the formula xC6H6Cl6 to it. The author also discoveredthis substance independently about two years ago. Meunier noticedthe presence of this substance a f t e r sublimation of his crude product,and it has been thought it might have been formed a t the high tem-perature of sublimation. The author obtained it, however, amongstthe first crude crystals deposifed after the action of the chlorine onthe benzene. From the results of his analysis, and the general cha-racter of the compound, the autlior believes the formula of this com-pound to be C,,H&l,,, and not zC6H6C16) and that it is thus diphsqtyZdodecachloride.The crystals are brittle and become highly elect,rified when powderedin a mortar. Contrary to the statements of Mennier, the crystals arestrongly double refracting.By J.MEC'NIER (Bull.SOC. Chim., 41, 5 3 0 4 3 2 ) .-The rapour-density of this compound,the preparation and properties of which have previously beendescribed (Abstr., 1884, 733), has been defermined, and found to be9.365 and 9.207 a t 260" (theor. 10.03). The vapour-density ofordinary benzene hexachloride a t 22W was found to be 10.139. Thisdifference is probably due to partial decomposition of the isomeride a tthe temperature of the determination- The formula of this isomerideis therefore C6H6C16, and its melting point is about 3310°, that of ordi-nary benzene hexachloride being 157".By E.XLTING ( B ~ l l . BOC. Chin$.,41, 502--504).-Since the oil obtained its a bye-product in the pre-paration of paranitrobenzyl chloride (Abstr., 18%, 1005) consistscliiefly of orthonitrobenzyl chloride, it may, perhaps, serve as a meansof preparing orthonitrobenzaldehyde, the starting point in Baeyer'ssynthetical preparation of indigo, but the author has not j e t succeededin preparing the aldehyde from the oil.Decomposition of Benzonitrile by Fuming Sulphuric Acid.By F. GUMPERT ( J . pr. (%ern., 30, 87-90).-1n preparing cyaphewi~teaccording to Pinner and Klein's method (Abstr., 1878, t64), theThey belong to the regular system.L. T. T.Isomeride of Benzene Hexachloride.A. B.Orthonitrobenzyl Chloride.A.BORGANIC CHEMISTRY. 53author did not obtain this compound, but dibenzamide, NHBz,, identi-cal with that prepared by Barth and Senhofer (Bey., 9, 975), and byFischer and Troschke (Abstr., 1881, 51). Dibenzamide melts a t 148".When heated with alkalis, i t is converted into benzoic acid and ammo-nia; heated with alcoholic ammonia in sealed tubes, it is convertedinto benzamide. The compound' described by Pinner and Klein asdibenzimide oxide is formed along with the above compound ; whentreated with dilute hydrochloric acid it is converted into dibenzamide,and the author regards it as benzimidobenzamide, NHBz.CPh : NH.P. P. B.Acetonequinol. By S. HABERMANN (.iWonntsh. Chem., 5, 329-331).-Quinol dissolves easily in acetone and, on cooling, very fine crystalsof acetonequinol, C3He0,C6H602, separate out.When exposed to theair, they soon become opaque, and then consist only of quinol. I n com-position and easy decomposition, it resembles quinhydrone, and itsexistence is an argument in favour of the formnla for quinone,recently advocated by Kekule (AnnaZen, 223,170), showing two car-bonyl-groups. H. B.By W. H. GREENE (Chm. News,50, 76).-A mixture of methylene chloride (30 grams), phenol(30 grams), sodium hydroxide (40 grams), and water (50 grams), isheated in a sealed tube a t 100" for six hours; the contents of thetube are then neutralised with hydrochloric acid, extracted withether, and the ether distilled 08. The residue is repeatedly treatedwith boiling water, the aqueous solution is concentrated, the drops ofphenol which separate are removed, and the strong solution then leftto crystallise over sulphuric acid ; the product, when recrystallisedfrom boiling water, is pure saZigenin.Compounds of Glucoses and Sucroses with Phenylhydrazine.By E. FISCHER (Ber., 17, 579--584).-When an aqueous solution ofphenylhydrazine hydrochloride, to which sodium acetate has beenadded, is heated on the water-bath with the aqueous solution of asugar, combination takes place and an insoluble compound is formed.I n many cases, the production of these compounds may be used as ameans of detecting the presence of a sugar and of identifying thesame.They may, as a rule, be easily purified by crystallisationfrom alcohol. Of the sugars experimented with, inosite and trebaloseare the only two which have not the property of unitirrg with phenyl-liydrazine.PhenyZgZucosazone, C,sH2,N404, is the name given by the author tothe compound formed when dextrose or 1e-i-dose is treated with phenyl-hydrazine in the manner described. This compound is insoluble inwater, but soluble in boiling alcohol, from which it is precipitated bywater in slender yellow needles melting at 204-205".It is not actedon by aqueous solutions of caustic alkalis, but is decomposed by stronghydrochloric or sulphnric acids, with the production of dark red solu-tions. This compound is formed even when dilute solutions of dex-trose are employed, and it would appear that its production may beused as a means of detecting grape-sugar in urine.New Synthesis of Saligenin.D. A.L54 ABSTRACTS OF CHEAlICXL PAPERS.Phenylgalactosnzone, ClsHa2N404, is tlie product of the combinationof phenylhydrazine and galactose ; in properties, it resembles phenyl-glucosazone, differing from it in melting a t a lower temperature,namely, 182 O .Sorbin also unites with phenylhydrazine, forming a compoundwhich is easily soluble in hot alcohol, and may be precipitated from thesolution by water, in the form of fine yellow needles melting a t 164".When cane-sugar is warmed with the solution of phenylhydrazinehydrochloride, it is first inverted, and subsequently phenylglucosazoneis produced. Milk-sugar and maltose both unite with phcnylhydrazine,forming pheny lactosnzone and y h e y lmcdtosazone respectively.Thesecompounds have tlie same composition, viz., CZ4HJV4O9, are svluble inhot water, and crystallise in yellow needles ; the former melts a t 200",the latter a t 190- 191". P. P. B.Action of Potassium Cyanate on MetanitramidobenzoicAcid. By P. GRIESS (Ber., 17, 2184--2187).-Five: isomeric nramido-iiitrobenzoic acids have been described, in three of which the groupsNO, and NH.C0.NH2 occupy the ortho-position to one another, aridin the remaining two, the para-position. With the object of obtain-i n g an acid containing these groups in the meta-position, the authorhas submitted metanitramidobenzoic acid (Abstr., 1884, 314) to theaction of potassiuni cyanate.The nitramidobenzoic acid is graduallyadded to a cold aqueous solution of crude potassium cyanate, themixture heated for some hours at 50-60", and then tyeated with ailexcess of acetic acid. The product is allowed to stand for severalhours, a large excess of hydrochloric acid is added, and the precipitateseparated and washed, The product consists of two acids : urarnido-nitrobewoic acid, NH~.CO.NH.C~H~(PO~).COOH [I : 3 : 51, and di-urarnidonitrobe~~zoie acid, (NH~.CO)~N.C~H~(NO~).COOH [l : 3 : 51,which may be separated either by treatment with boiling wateror by means of the barium salts. Uramidonitrobenzoic acid,C,H7N3O5,H2O, is moderately soluble in boiling water, from which itcrystallises in bright yellow needles ; is much more readily soluble inhot alcohol, but very sparingly in ether ; it has a strong bitter taste.When heated, it detonates, producing a yellow smoke and leaving alarge carbonaceous residue.The barii~m salf,[NHz.CO.NH.C&&(NOZ) .C00]2Ba,5H,07forms yellow nodules, readily soluble in hot, moderately in cold water.On dissolving uramic3onitroberlzoic acid in nitric acid (sp. gr. 1.5), itis converted into uramidodinitrobenzoic acid,N Hz. C 0. N ( NOz) . C, H3 (N 0 2 ) . C 0 OH.Diuramidonitrobenzoic acid crystallises from alcohol w i t h 2 mols. H,O.It forms almcst white microscopic needles or scales generally unitedin tufts, is very sparinglv soluble even in boiling water, andsparingly also in hot aIcotol and in ether. It has a st,rong bitkertaste, and also resenibles the last acid in its behaviour when heated.By the action of tin and hydrochloric acid, it is converted into a newamido-acid, crjstallising from boiling water in slender white needlesORGIhNlC CHEMISTRY. 55The harium salt, [ (NH,.CO),N.C,H3(NO,).COO],Ba,7~H2O, is verysparingly soluble even in boiling water, and crystallises from it insmall yellow nodules when the solution is rapidly cooled, and in needlesby slow crptallisation ; it is insoluble in alcohol.Action of Hydrochloric Acid and of Chlorine on Aceto-benzoic Anhydride.By W. H. GBEEKE (Chew,. News, 50, 61-62).-It has been stated (Loir, Abstr., 1880, 31) that acetobenzoicanhydride prepared from beiizoic chloride and sodium acetate, differsfrom the anhydride prepared from acetic chloride and sodium benzoatein its reactions with hydrochloric acid and with chlorine.The authorshows that this is not the case, but that scetobenzoic anhydride, which-ever way prepared, behaves always in the same manner with hydro-chloric acid and chlorine. When dry hydrochloric acid is passed intot tie anhydride a t ordinary temperatures, acetic chloride and benzoicacid are the principal products, whiist a t higher temperatures, 130" tolW0, acetic and benzoic chlorides, and acetic and benzoic acids, areproduced in about equivalent proportions. With chlorine a t about 150",the products are acetic and benzoic chlorides, chloracetic and (1 : 2)uhlorobenzoic acids, whilst at lower temperatures the reaction yieldschiefly acetic chloride and chlorobenzoic acid.A.K. &I.D. A. L.Action of Phenol and Sulphuric Acid on Hippuric Acid.By J. ZEHENTER (Monatsh. Chern., 5, 33.2-338) .- Experimentswere made to obtain condensation-products of phenol with glycocolland alanine, but with negative results. But by heating hippuric acidwith phenol and sulpliuric acid a t 140", the nascent glycocoll does unitecompletely with the phenol. The product of the reaction is dissolvedin water, the berizoic acid removed by ether, and then neutraliseciwhile hot with lead carbonate. The solution of the lead salt is decom-posed with sulphuretted hydrogen, and the filtrate evaporated finallyin a vacuum and allowed to crysfallise. The substance, C,H,O,NS +H,O, melts a t 153-185", and is an acid forming salts, It is probablysulplio~heny Tgl~cocoZI, its formation being expressed by the equationXH2.CHz.COOH + C6H5.0H + H,S04 = C8H905NS + 2Hz0.Thesilver salt, C8H80,NSAg + 3H2U, the barium salt, (C,H,05NS)2Ba +H20, and also the copper and potassium salts are described.When the free acid is heated t o 200", it gives a distillate of phenol.Treated wihh aqua regia, a, yellow crystalline substance is formed.Wo satisfactory clue to the constitution of the acid is obtained byfusing it with alkalis. Phenol and hippuric acid do not act on eachother if heated with water under pressure.By. 0.WIDMANN (Ber., 17, 2282--2284).-As Einhorn and Hess have justpublished a communication containing some work on this subject, theauthor now gives a preliminary note of the results of a research whichhe has been carrying on of late.He has at present prepared andexamined the following compounds :-H. 13.Nitrocumenylacrylic Acids and their Derivatives5F ABSTRACTS OF CHEMICAL PAPERS.A. From orthonitrocumenylacrylic acid-Ethyl orthonitroc umenylacrylate ........Orthonitrocnmenylacrylic acid dibroniide. . m.p.Acetamidocumenylacrylic acid .......... ,,Cumostyril (isopropylcarbostyril) ........ ,,Orthoxycumenylacrylic acid ............ , .Orthamidocumenylacrylic acid .......... ,?Hydrocumostyril ...................... 5 ,B. From cumenylnitroacrylic acid-Cumen ylamidoacrylic acid .............. , ,C. From metanitrocumenylncrylic acid-Metanitrocumenylacrylic acid. ..........., ,Metanitrocumenylacrylic acid dibromide . . 9 ,Ethyl metanitrocumenylacrylate ........ 7 7Metamidocumenylacrylic acid ........... ,,Acetamidocumenylacrylic acid .......... 7Metamidocumenylpropionic acid ........ 7 7Acet'amidocumenylpropionic acid ........ 9Liquid.171"16522016 7-- 16813.5176154-15514158-59184I65240168L. T. T.103-105Compounds of Phenols with Ethyl Acetoacetate. 111. ByH. V. PECHYANN and J. B. COHEN ( B e y . 17, 2187-2191). I n continu-ation of their experiments on the substituted coumarins (Abstr., 1884,66, 1331) the authors give further evidence of the general applicationof the reaction for their formation. A comparison of the coumarinsobtained from ethyl acetoacetate with the ordinary coumarins shows astriking analogy in the properties and especially in the colour reactionsof those members of both series which are derived from the samephenol.The coumarin obtained from paracresol and ethyl acetoacetate (Zoc.cit.) may (in accordance with Baeyer's notation, Abstr., 1884, 998) benamed b-5-dimethylcoumarin ; it melts a t 148".p-Methyldaphnetin, C6H2( OH),< '?de :'">GO [l : 2 : 3 : 43, ob-tained from pyrog,zllol and ethyl acetoacetate (Zoc.cit.), closelyresembles daphnetin ; after boiling with bisuiphite, both compoundsyield an intense blue coloration with ferric chloride and a reddish-yellow reaction with ammonia and potassium ferricyanide. The actionof sulphuric acid on orcinol and ethyl acet'oacet'ate hss been examinedby Wittenberg ( J .pr. Chwn. [2], 26, 69), but his results disagreewith the authors'. The product is termed /3-6-dimethylumbelliferolie,C o H , M e ( O H ) < ~ ~ ~ > C O [CMe : 0 OH : Me -= 1 : 2 : 4 : 61.It melts at 248-250", crystallises in needles, dissolves readily in alcoholand glacial acetic acid, sparingly in benzme and chloroform, and isalmost insoluble in water. It yjelds yellow solutions with concen-trated sulphuric acid and with dilute alkalis. The solution obtainedby boiling i t with bisulphite yields (like homo-umbelliferone) a redcoloration. The ace$-derivative, CIJHl,Or, crystallises in white needlasORGANIC CHEJIISTRT. 57melting at 195", dissolves readily in alcohol, glacial acetic a d ,benzene, and chloroform, sparingly in ether, and is insoluble inwater.4- 6-Dihydroxy-P-~~zet?~ ylcoumnrin,C6H2( OH)2<-O-- CMe:CH>CO [CXe: 0 : OH: OH =1: 2 : 4 :6],from phloroglucol and ethyl acetoacetate is isomeric with /3-methyl-daphnetin. I t crystallises in colourless needles, melts ati 282-5284',dissolves readily in alcohol and glacial acetic: acid, sparingly in water,benzene, and chloroform, is almost insoluble in ether, and is readilydissolved by dilute alkalis. Its aqueous solution gives no reactionwith ferric chloride, and yields a yellow precipitate with lead acetate.It yields no colour reaction with bisulphite. The ncetyl-derivative,CI4Hl2O6, crystallises from alcohol in white glistening needles, melts at138-140°, is insoluble in water, sparingly soluble in ether, readily inalcohol, glacial acetic acid, and chloroform. /'3-Methylcounzarifi of>CO, from P-naphthol and ethyl aceto- naphthalene, C1OH6<acetate, forms white glistening needles, melting at 161-162" ; it dis-solves in alcohol, benzene, and chloroform, but is nearly insoluble inwater and ether.Sulphuric acid dissolves it with green fluorescence.Reduction of Phthalic Anhydride by Zinc and GlacialAcetic Acid. Bg J. WISLICENUS (Bey., 17, 2178--2183).--Whenphthalic anhydride (200 grams) is dissolved in glacial acetic acid(1 kilo.), heated on a water-bath, and zinc-dust (about 300 grams)added in small quantities a t a time, the latter at first dissolves rapidly,with considerable evolution of heat but without generating hydrogen ;when the reaction becomes sluggish, heat is applied, and hydrogen isthen seen to escape.The hot filtered solution deposits needles ofdiphthnZyZ, C16H804, on cooling ; this melts above 32U" and can be sub-limed in a current of carbonic anhydride. @n diluting the moiher-liquor with water, a flocculent precipitate is obtained, containinghyclrodiphthalyl, C16H1004, and hyc~rod~~hthalluctorlic acid, C16H1204,separable by means of sodium carbonate solution. Hydrvdiphthallyl,CO <yf:>CH.CH<Cf:>CO, crystnllises from boiling alcohol inslender colourless needles, melting between 228" and 229" ; it dissolvesextremely readily in boiling glacial acetic acid. Hydrodiphthal-lactonic acid, cO<yf:> CH. CH,. C6H4. COOH, dissolves very readilyin hot, sparingly in cold alcohol, and crystallises in short thick four-sided, vitreous prisms, melting a t 198.5" ; the potassium salt is readilysoluble, the silver salt, C1,H1,O4Ag, forms a white very stable pre-cipitate. On boiling the acid with excess of potash, two molecules ofthe latter become neutralised, and on then acidifying with hydro-chloric acid, ~ i ~ d r o h ~ i d r o x ~ ~ i p h t ~ a l y ~ ~ c acid,COOH.C6H,.CH2.CH( OH) .C6K4.COOH,is obtained, crjstallising in colourless prisms ; this melts a t 170" wirhseparation of water, then solidifies and melts again at 198.5". When hy-drodiphthallactonic acid is boiled with hydriodic acid and phosphorus,CMe CHA. K. M5 8 ABSTRACTS OF CIIEMICAL PAPERS.the acid, Cl6HI40.i, obtained by Or-aebe from diphthalyl, is formed, andis named by the author dib(!nayEdiorthocnrbo~~l~c acid,COOH.CcH4.CH,.CH,.C6H,.COOH.The dilnteci mother-liquor from the diphthalyl and diphthallactonicacid contains phthulicle which can be separated by extraction withether; i t crgstallises from warm ether and alcohol in densc stronglyrefracting prisms, and from boiling water in needles ; i t melts at 73",arid is volatile without decomposition, its boiling point being 281.5" a t:t pressure of 750 mm. (286.5" cow.). The residual solution freedfrom phthalide still cont ains zinc salts of acetic, phthalic, and hydro-diphthallactonic acids.The formation of diphthalyl from phthalic anhydride and zinc takesplace thus: 4C80,0, i 2Zn = 2C8H404Zn + C16H,04, this beingproved by heating fused plithalic anhydride at 130-140" with zinc-dust (free from oxide), wheu a mixture of zinc phthalate anddiphthalyl is obtained. A.K. M.Isatin. (Preliminary Note.) By H. KOLBE (J. pr. Chern., 30,S4--87).-Isatin is converted by chromic acid, dissolved in glacialacetic acid, into an acid which the author styles iscntoic acid, and whichhe regards as ~~itrogen-~eiza~~lcarboxylic acid, c6 { $} CO.COOH.It is sparingly soluble in cold water and alcohol, but easily in hotivater, from which it crystallises in yellow rhonibic tables. Thissitme acid is obtained by oxidising indigo with chromic acid.IVhen isatoic acid is heated above its melting point, or when itsayneons solution is boiled, it is decomposed, water and carbonic anhp-dride being formed.When boiled with baryta-water, a new acid isproduced, which is easily soluble in water, and seems t o be formedwhen isatoic a.cid is heated with sulphuric acid. In attempting toprepare th5 ethyl salt of this acid, a liquid was obtained, probablyC6H4N.COOEt, and an acid, which is probablyc { Ei} c { gHH} COOH. P. P. B.Formation of Dibenzyl from Ethylene Dichloride andBenzene in Presence of Aluminium Chloride. By W. H. GREENE(Chem. News, 50, 61).-By a,pplying Friedel and Crafts' reaction to amixture of benzene and ethylene dichloride, the author has obtaineddibenzyl (boiling point, according to present determination, 279" at'767 mm.), in nearly tbeoretical quantities, along with oily condensa-tion-products, which can neither be completely distilled, even a t 200"in a V~CUUIII, nor fractioned, nor solidified in a freezing mixture.D.A. L.Trichlorocamphor. By P. CAZENEUVE (Cornpi. rend., 99, 609-Gill).-Monochlorocamphor (melting a t 83-84") is heated on a water-bath and saturated with chlorine gas. The product is washedrepeatedly with water in order to remove hydrochloric acid, then dis-solved in alcohol, and the solution placed in a rnixtuie of ice anORGASIC CIIEXISTRII'. 59salt, when it separates into two layers, the lower of which is a mole-cular combination of the trichlorocainphor with alcohol, solidifyingbelow 0". This compound is decomposed by waler, ihe product com-pressed in order co expel a liquid substance, which is in all proba-bility a more highly chlorinated derivative, and then purified byrepeated solution in alcohol and precipitation by water.The trichloro-camphor thus obtained has the composition CloH,,C1,O, and formswhite microscopic crystals, which have w r y little odour, and resembleterebenthene derivatives. It is insoluble in water, but dissolveseasily in cold alcohol, ether, chloroform, carbon hisulphide, and theother solvents for camphor, It melts and solidifies at + 5 4 O , liquefiesin the vapours of ether and chloroform, like the mono- and di-deriva-tires, and in alcoholic solution has a dextrorotatory power [a] = + 64".When boiled, it decomposes with evolution of hydrochloric acid andformation of a carbonaceous residue.Prom its appearance, solubilities, and crystalline form, this deriva-tive seems to belong to the /3-series of chlorocamphors.C.H. B.Camphoronic Acid. By J. KACHLER and F. V. SPITZER (Monatsli.Clienz., 5, 415-416) .-The formula C9H,,05,H,0 has been previouslygiven to this acid (A7waZen7 159, 286), which Kissling (Inuuq. Diss.,Wurtzburg, 1878) believes to be an anhydride, the true acid beingC9H1406. The authcrs are studying the action of aqua regia a'ndpotassium permangsnate OII the acid.Kinoin in Malabar Kino. By C. ETTI ( B e y . , 17, 2241-2244).-Kremler (Vienna yl~ul.mnceutisclie Post, 16, 117) and A. Bergholz(Inauy. Dissert., Dorpat, 1884) deny the presence of kino'in in Malabarkino, and state that they have found protocatechuic acid therein.The authoi' proves the methods employed by these investiptors to bevery faulty, and fully sustains the comectness of his own earlierinvestigations on this subject (Abstr., 1879, 159).Substances contained in Saffron. By R.KAYSER (L'er., 17,'2228--8234~).--I(ouillon, Vogel, Qnadrat, Rochleder and &layer, andWeiss have a t various times worked at this subject, but the infoima-tion at present available is unsatisfactory. The author has thereforecarefully investigated a sample of saffron from Crocus eZectus, Qutin.Essential Oil of Safron.-This was obtained from saffron by steam-distillation in a current of carbonic anhydride. It is an almostcolourless mobile liquid, with an intmse odour of saffron. Whenexposed to the air, it becomes oxidised and turns brown and syrupy.Aiialysis showed its composition to be C,,H,,, so that it belongs to theclass of terpenes.Crocin.-Saffron was first freed from fatty matters, &c., by etherand then extracted with water at the ordinary temperature.Theaqueous solution was shaken up with bone-charcoal. which absorbednearly all the colouring matter. The charcoal was filtcrcd of, and thecrocin extracted from i t by washing with pure water. This solutionwas evaporated to dryness, and the residue treated with 90 per cent.alcohol. On evapordting the alcoholic solution, a yellowish-brownH. B.L. T. T60 ABSTRACTS OF CIIE31ICAL PAPERS.brittle mass is left, which yields zt yellow powder. Crocin is easilysoluble in water and dilute alcohol, less so in absolute alcohol, andalmost insoluble in ether.Strong sulphuric acid dissolves it to adeep blue solution, which turns first violet, then cherry-red, andlastly brown. Nitric acid (sp. gr. 1.4) gives a similarly colourad sola-tion, b u t the colour immediately changes to brown. Hydrochloricacid yields a yellow solution. Load acetate, and lime- and baryta-water give no precipitate, but, on heating, they decompose crocin intocrocetin and a sugar. Alkalis cause the same decomposition in thecold. Crocin is thus a glucoside, and analysis shows its cornpositionto be CalH7,02,.Crocetin is best obtained by the action of hydrochloric acid oncrocin. It is precipihted in the form of yellow flocks, which whendried yield a red powder. It is almost insoluble in pure water, butis rendered soluble by the addition of a small quantity of an alkali.Acids reprecipitate it from such solutions in orange flocks.It iseasily soluble in alcohol. An alcoholic solution gives bright red preci-pitates with lead acelate, and with lime- or baryta-water ; the com-pounds so formed, however, are not definite, but vary in composition.Snlphuric and hydrochloric acids behave with it as with crocin. Itscomposition is C,4H,60,. The decomposition appears to take placeaccording to the equation ~ C J ~ H ~ O O ~ S f 7H20 = C:,J€&, + 9C6H&.0rocose.-The sugar mentioned above yields rhombic crystals. Itsfiolution has a, sweet taste and strong dextrorotatory action. Itsreducing power for Fehling’s solution is only half that of dextrose.The quantities of crocetin and crocose obtained by the decompositionagree very closely with those required by the above equation.Picl.ocroci.n.-Su~~un-bitter.-l’his substance crystallises out in theether-extracting apparatus if the extraction be continued for a longtime.It forms colourless prismatic needles, very sparingly solublein ether. It dissolves easily in water and alcohol, less so in chloro-form. It has a, characteristic bitter taste, which is very persistent.It melts a t 75” to a colourless liquid. Its formula is C38H6S017. Leadacetate, lime-water, and baryta-water give no precipitate in the cold,but decompobition takes place on warming, crocose and the terpenedescribed above being formed, Picrocrocin is thus a glucoside likecrocin, and the decomposition may be expressed by the equation-C.>EIHFI~OI~ HzO = 3C6H1206 + ~CIOHI,.L. T. T.C arboxylic Acids from Synthetically Prepared PyridineBases. By R. MICHAEL (AmaZe.n, 225, 121--146).-Hantzsch hasrecently described the synthesis cjf a ppridiDe-derivative, ethyl hydro-collidinecarboxylate, by the action of ethyl acetoacetate on aldeliyde-ammonia, the formation from it of collidinedicarboxylic acid, andfurther, the limited oxidation of this latter substance by which it isconverted into lutidinetricarboxylic acid, pisoliaetetracarboxylic acid,and pyridinepentacarboxylic acid (Abstr., 1883, 82). The presentpaper deals with the formation of a collidinemonocarboxylic acid andits oxidation into a series of acids each containing a COOH-group lehsthan those above mentionedORQANIC CHEBIISTRP.61ColIidinemoriocni.boaylic acid is formed by heating collidinedicarbo-xylic acid, but in such small quantity that a more satisfactory methodfor its preparation had to be found.Hydrogen ethyl coZZidined i c a r b o q Zate, C5NMe3 (C 0 OE t) . C 0 0 H, isprepared by heating the diethyl salt with the quantity of alcoholicpotash necessary to saponify o d y one COOEt-group ; any undecom-posed diethyl salt m7as then removed by shaking with ether, the solu-tion of the potassium ethyl salt evaporated to dryness with the equiva-lent amount of hydrochloric acid, and the hydrogen etliyl salt sepa-rated from potassium chloride by solution in absolute alcohol. Itcrystallises (+ ;?H,O) from water in rosettes of long prisms or in thickwell-formed prisms, apparently of the monoclinic system ; from alcoholin stellate groups of needles.It melts, when anhydrous, at 157", isreadily soluble in alcohol and water, sparingly soluble in ether. Thefollowing salts were prepared from it. The acld silver salt,AgEtC,,H,NO, + HEtCioH,NO* + H20,forms small monoclinic prisms, and is not blackened by exposure tolight. The zinc salt, (EtC,,K,NO,),Zn + 5H20, crystallises in rosettesof colourless prisms, sparingly soluble in cold, readily in hot water.The cadmium salt, ( EtC,oH,N04),Cd + 4H20, crystallises in striatedprisms, and is readily soluble in hot water. The copper salf,(EtC,,H,NO,),Cu, forms an indigo-blue powder consisting of micro-scopic plates. It is anhydrous and insoluble in water.The caZciurnsaEt, (EtC1,H,NO,),Ca + 3H20, forms crusts of fine needles, and isreadily soluble in water and alcohol. The baritm salt,(EtC&gN0,)2Ba + 3H20,is sparingly soluble in water, insoluble in alcohol. It can also beobtained with only 1 mol. H20. The potassizcnz salt crystallises with1 mol. H,O in fibrous masses. The niclcel salt crystallises in pale greenprisms, the mezerc~~roi~s salt in thick tables. The hydrogen ethyl salt,like the free acid, combines with acids : the hydrochlode,C,NMe,(COOEt) .COOH,HCl,prepared by the action of hydrochloric acid on an ethereal solution ofthe salt, crystallises in thick transparent cube-like forms, melts a t1%" with decomposition, is very readily soluble in water, readilysoluble in alcohol.The platirudiloride,[ C5NMe3( C OOE t) . C 0 0 HI,, HzPt CI,,crystallises in red rhombic (?) tables, or with 2 mob, R,O in large,broad prisms, is sparingly soluble in cold alcohol, readily soluble inwater ; i t melts with decomposition a t 219".Ethyl collidi.nemonocarboxylate, C5NHMe3.COOEt, was obtained illvery small quantity by Hantzsch (Zoc. cz't.) by heating ethyl hydro-collidinemonocarboxylate with hydrochloric acid ; it is readily obtainedby heating hydrogen ethyl collidinedicarboxylnte, when it passes overbetween 230" and 260°, and can be purified by continued fractiona-tion. The yield is 56--.58 per cent. of the theoretical. It is a colour-less oil, distils at 256", has a sp.gr. = 1.0315 a t l5", and is readilG2 ABSTRACTS 01'' CHEMICAL PAPEHS.soluble in ether, alcohol, benzene, chloraform, and dilute acids. Crys-talline compounds with acids could not be obtained. The platinochlo-Tide, (C,NH~~e,.COOEt),,H~PtCl~, crystallises in thick reddish-yellowprisms, and melts a t 193"; i t is sparirlgly soluble in alcohol, readilysol iible in water.C,NHMe,.COOEt,MeI,formed by the union of its components at ordinary temperatures,crystallises in silky needles, melts a t 128", is readily soluble in alcoholand water, insoluble in ether.CoZZidinemonocarbox~Zic &7, C5NHMe3.COOH + 2H20, is preparedfrom the ethyl salt by saponification with alcoholic potash, and evapo-ration to dryness of t'he potassium salt formed with the equivalentamount of hydrochloric acid. It crystallises in short tetragonal (3)prisms o r in cube-like forms, and melts at l l O o , or, when anh-j-drous,a t 155".It is extraordinarily soluble in water and alcohol. It haseither a, very faint acid reaction or none at all, and unites with acidsand bases. The potassium salt, C5NHMeJ.COOK, is obtained as ayellowish powder, but can be crystallised from alcohol, when it formstufts of needles. It is very readily soluble in water and deliquesceson exposure t o the air. The calcium salt, (C9HloN0,),Ca + H,O,forms a crystalline powder soluble in water.ELhy I co Zlidiitecarhozy 1 ate met hiodide,The hydrochloride,C5NHMe3.COOH,HC1,crystallises in wart-like groups of needles or prisms, and is readilysoluble in water or alcohol.(C5NHMe3.COOH)2,H',PtC16 + H20,ciytallises in thick yellowish-red tables, melts at 198" with decompo-sition, is readily soluble in water, sparingly soluble in alcohol.Lu,tidinedicai.bo~,~lic acid, C5NHMe2(COOH)2 + l$H,O, is preparedhy heating on the water-bath a mixture of an aqueous solution ofpotassium collidinecarboxylate with the amount of potassium per-manganate necessary to oxidise one methyl-group, filtering off theinanganic oxide separated, neutralising with nitric acid, and precipi-tating with lead nitrate, the lead salt being then suspended in waterand decomposed with hydrogen salphide.It crystallises in colourless,lustrous pyisms, melts, when anhydrous, at 245", is sparingly solublein cold, more readily in hot water, and nearly insoluble in alcoholor ether.With silver nitrate, a solution of the ammonium salt givesa gelatinous precipitate, becoming crystalline on boiling ; with leadnitrate a, thick white precipitate, or from dilute solutions, after a time,rhonibic tables separate, which on being boiled become transformed intofihort prisms. The calcium salt, (15NHMez(C00)2C;. forms indis-tinctly crystalline crusts readily soluble in water. The magnesiuinFalt, C,NH&fe3( COO),Mg + 3H,O, resembles the calciuni sait. ThehydrochZoride crystallism in slender needles. The pZatl'nochloridP,[C,NHbIe,( COOH),],,H,PtCI, + 6H20, crjstallises in golden rhombictables or in reddish-yellow prisms, does not melt at 290", and isreadily soluble in water and alcohol.PicrJZinetl.icarbozyZic acid, C,NHMe(COOH), + 2H20, is obtainedThe platirtochlorideORGAXIC CHEJIISTRP.63in a manner similar to the abo-re, but with use of sufficient potassiumpermanganate to oxidise two of the methyl-groups in the potassiunzcollidineearboxj-late ; it is separated from any 1 utidinedicarboxglic acidformed a t the same time by repeated crystallisation from water, inwhich it is the more readily soluble of the two. I t crystallises inflocculent groups of slender needles, on heating becomes yellow below2C)O0, brcwn or black a t 210-22507 and melts with much frothing a t238'. A solution of the ammonium salt gives a gelatinous precipitatewith silver nitrate ; witb barium chloride a voluminous precipitate ;with lead and mercnry salts heavy white precipitates; and mit,hferrous salts a yellow coloration not altered by acetic acid.Thesilver saZt, C5NHMe( COOAg),, i s not crgstallinc. The bariwn salt,[C,NHMe(COO)3],Ba3, forms a hard sand-j- powder. Picolinetricar-boxylic acid does not combine with mineral acids nor yield a platino-chloride. A picolinetricarboxylic acid was obtained by Besthorn andFisher (Abstr., 1883,600) by the oxidation of flavenol, but it is doubt-ful whether it is identical with the acid abore described; the differencein the colour-reaction with ferrous salts and i i i the solubilities of thebarium and calcium salts seem to indicate tbat it is not.Pyridinetetl.acar7)ox?/Zic acid, C5NH( COOH), + 2H20, is preparedfrom potassium collidinecarboxylate by oxidation with a quantity ofpotassium permanganate slightly less than that necessary for theoxidation of the three methyl-groups. Its preparation is somewhatdifficult, the oxidation readily proceeding further with formation ofoxalic acid and carbonic anhydride.The solution, after filtering offthe manganic oxide, is neutralised with nitric acid, evaporated, andmixed with cupric sulphate, when cupric ~.'yridinetetracarboxSl,zte isprecipitated, whilst cupric lutidinedicarboxylate and picolinetricar-boxylate remain in solution. The free acid is obtained by decomposingthe copper salt with hydrogen sulphide ; it is still far from pnre, tbeanalytical numbers bcing very unsatisfactory. It crystsllises inslender needles, melts with decomposition a t 188", and is sparinglysoluble in alcohol and water.A solution of the ammonium salt giveswith cadmium sulphate a pulveriilerit precipitd e insoluble in hotwater, with silver nitrate it gelatinous precipitate blackened by expo-sure to light. A solution of the acid gives with copper sdts anamorphous bluish-green precipitate ; with ferric chloride a yellowishflocculent precipitate ; and with ferrous salts a brownish-red colora-tion, turning to dark cherry-red on addition of acetic acid.A. J. G.Brucine. By 9. RANSSEEN ( B e y . , 17, 2266--2267).-On heatingbrucine with hydrochloric acid, methyl chloride is given off and a sub-stance formed which crystallises in yellowish needles melting at 284".This when freshly precipitated dissolves readily in alkalis, and is re-precipitated by carbonic anhydride.With ferric chloride, it gives abluish-violet, with potassium dichromate and snlphuric acid a blood-red colour, and with nitric acid a brownish-yellow precipitate. Itforms a platinochloride crystallieing in bronze-coloured flakes. Boththe free base and its platinochloride, on analysis, yield numbers agree-ing with the loss of one methyl-group from brucine. If this com-pound is treated with potassium hydroxide and metllJl iodide, brucinG4 ABSTRACTS OF CHEMICAL PAPERS.methiodide, melting at 270", is formed identical with that obtaineddirectly from brucine. It is thus probable that brucine contains butone methoxy -group.Alkaloids from the Bark of Remijia, Purdieana.By 0.HESSE ( A n n u l e n , 225, 211-262) .-A preliminary notice of some ofthe results contained in this paper has already appeared (Abstr.,1883, 601). A description is given of the structure and properties ofthe bark. The alkalo'ids of this bark have been previously examinedby Arnaud, who found about 0.2 per cent. of cinchonamine, and0.8-1.0 per cent. of cinchonine. The author confirms the presenceof these bases, but finds that several other alkaloi'ds are present, andthat the amount of cinchonine is only 0.1-0.2 per cent. Theseparation of the alkaloids is effected as follows : the finely dividedbark is extracted with hot alcohol, the solution evaporated, and theresidue after treatment with excess of caustic soda, extracted withether.The ethereal solution is treated with excess of dilute sulphuricacid, and shaken, when the sulpbates of concusconine, chairamine,conchairamine, chairamidine and conchairamidine are precipitated,(A) whilst the sulphates of cinchonine and cinchonamine with smallquantities of the other bases remain in solution (B). By addition ofvery dilute nitric to the solution (B) cinchonamine is precipitated asnitrate and cinchonine is left in solut>ion. The precipitate A is di-gested with dilute soda, and the separated nlkalo'ids, after washing, aredried in the air, dissolved in hot alcohol, and sulphuric acid diluted withalcohol, added in the proportion of 1 part H2SOJ to 8 parts of thealkaloids. Nearly the whole of the concusconine separates as sulphate,a fnrther very small quantity separating on cooling.On adding con-centrated hydrochloric acid to the cold alcoholic filtrate, c7zairamineseparates as hydrochloride. The mother-liquor from this is heated,and small quantities of ammonium thiocyanate added as long as acrystalline precipitate is formed of conchuircrrnitie thiocyanate.After cooling and filtering, the liquid is again treated with am-monium thiocyanate, when a dark-coloured pit eh-like mass separates ;the filtrate from this is treaked with ammonia, and the resultingprecipitate shaken up with brnzene. The benzene solution is shakenwith dilute acetic acid, and the solution of the acetates so obtainedmixed with a saturated aqueous solution of ammonium sulphate,when %I precipitate of chairamidine aid conchairamidine siilphates isobtained.These are separated by dissolving them in boiling water andcooling, when the whole gelatinises ; on standing, crystals appear,the crystallisation being complete after some days ; on now heating to40°, the chaii*a?~iidl:ne sulphate dissolves, whilst conchairamidinesulphate is left. The process must be repeated several times on thesolution to obtain a pure product.Cinchonamine and its salts have been to some extent described byArnaud (Ahstr., 1884, 87)) whose results the author in generalConfirms, although differing in some details. Cinchonamine, ClsH2eNa0,crystallises in brilliant colourless needles, melts when anhydrous a t184-185" (194", Amaud), is readily soluble in hot alcohol, ether,chloroform, carbon bisulphide, and benzene, sparingly soluble i nL.T. TORGANIC CHEMlSTRP. 65light petroleum and water. I t s adcoholic solution has a strong bittertaste, and an alkaline reaction, and is dext'rorotary : [m]D = + 121.1"at p. = 2 and t . = 15". It dissolves in concentrated sulphuric acidwith reddish-yellow colour, which slowly darkens ; in nitric acidwith an intense yellow. It is soluble in concentrated hydrochloricacid, but it is decomposed when heated with it in sealed tubes at150". It,gields two series of salts, normal and monacid. Theh@oc7~ lorzde, C19H24N20,HC1, crystallises in anhydrous colourlessplates, readily soluble in alcohol, very sparingly soluble in water(according to Arnnud it contains 1 mol. H,O). The plntinochloride,( ClgH,,N20),,H,PtC1,, is obtained as a yellow flocculent precipitate,apparently becoming crystalline after a time. The hydwbrornide,C19H2aN20,HBr, crystallises in long flat needles, sparingly soluble incold water.The 2, ydrioditle, CIYH24N20rHI, forms long colourlessflat needles. The thiocynnatn, CI9HZ4N,O,CNSH, forms colourlessplates or short prisms, and is very sparingly soluble in coldwater. The nitrate, C19€€21N20,HNOJ, forms short colourlessprisms, melts a t about 195", is sparingly soluble in cold water,readily in boiling water and hot alcohol. The normal suZp7iafe,(C,9H,,N,0)2H,S04, crystallises in colourless prisms, is readilysoluble in hot or cold water, very sparingly soluble in cold alcohol.Its aqueous solution is dextrorotary : [ a ] D = + 36.7" a t p.= 2 andt. = 15 ; [O]D = f 39.8"atp. = 6 ; and [OC]D = -l- 39.6" a t p. = 2 and2 mol. H2S04. The arcid sulphnte, C19H2iN20,Hk30J, crystallisesin anhydrous prisms and shows the rotary power = + 34.9" atp. = 2.4 and t. = 15" and [ 1 ] D = + 37.4" a t p . = 6. The th;osuZplm,ts,C19H24N20,S203H2, forms anhydrous prisms sparingly soluble in water.Acet?lZainchonantine, CI9H2,AcN,O, prepared by heating cinchonaminewith acetic anhydride for some hours a t 85", is amorphous, sinterstogether a t 65", and melts a t 89-90", is readily soluble in ether,alcohol, chloroform, and acetic acid. DinitrociiLchonamine,c 19H22 (PU'O,) 2x20,is best prepared by dissolving cinchonamine in nitric acid of sp. gr.1.06, and pouring the intensely yellow solution into an excess of verydilute ammonia.It forms yellow flocks, melts a t 118", is readilysoluble i n ether, chloroform, alcohol, and acetic acid. A solution inhydrochloric acid gives with platinic chloride a yellow flocculentprecipitate of thephtiizoch Zoride, [ C,,H,,(N0,),N,0]2,H[,PtCl~ + 3H20.Cinchonninine rnethiodide, C19H,,N,0,MeI + HzO, prepared byadding methyl iodide to a solution of cinchonamine in methylalcohol, crystallises in hard colourless prisms, readily soluble inalcohol, sparingly soluble in water. The chloride. C19H,4N,0,MeCl~ isamorphous. The pZntinoc7doride7 ( CI,H,,N,OMeC1),PtCI4, is obtainedas a yellow crystalline precipitate. The h?ydroxide, obtained by theaction of silver oxide on an aqueous solution of the chloride, formsan aniorphous mass, readily soluble in water and alcohol, sparinglysoluble in chloroform and ether.It has an intemely bittev taste,and is a powerful base, eagerly absorbing carbonic anhydride fromthe air.VOL. XLVIIT. 66 ABSTRACTS OF CHEMICAL PAPERS.Methylcinchonnmine, C,,H,,MeN,O, is prepared by boiling cinchon-amine methiodide, chloride, or hydroxide, with caustic soda. Itforms an amorphous white powder, melts a t 139", is readily solublein alcohol, ether, and chloroform, insoluble in water. The chloride isamorphous, the p7ntinuchZoride7 (C,,H2,MeN2O),,H2PtC1, + 4H20, isobtained as a reddish-yellow flocculent precipitate.Cifichortaniine ethiodide, C19H24N20, EtI, forms a colourless varnish,readily soluble in alcohol, nearly insoluble in water.The eldorideforms colourless prisms, readily soluble in alcohol and hot water.The plahnochloride, (Cl,Hz4N20,EtCI),,PtC14 + 2Hz0, forms orange-colouretl crystals. The sdphate, (C,,H,,N,OE t),SO,, is colourless andamorphous. The hydroxide resembles the corresponding methylcompound.Ethz~7ci~~echoizanziize, ( C19H2,EtN20)3 + H20, forms a white powder,melts at. 75-i8", or when anhydrous at 140", aild is readily soluble inether and alcohol. The platinochlnride, (C,,H,,EtN,O),,H,PtCl, +3Hz0, forms a reddish-yellow flocculent precipitate.Conczwonhie, C,7H26N,04 + H,O.-This alkaloid is obtained as thenormal siilphate as already described, and is obtained in the free stateby decomposition of the snlphate with dilute soda, and recrystal-lisation from alcohol to which a little ammonia has been added.It forms colourless or pale-yellow compact prisms.It is readilysoluble in ether, chloroform, and benzene, sparingly soluble in boilingalcohol, insoluble in water. It is optically dextrorotary, giving forC,,H2,N204 + H20, p. = 2, t. = 15" ; in 97 vol. per cent. alcohol= 40.8" The hydrate melts at 144", becomes anhydrous, and thenmelts again a t 206-208"; a t 140-150" it becomes dark-browncoloured, being in small part converted in to amorphous concusconine.(This amorphous concusconine is readily separated by conversion ofthe fused mass into the normal sulphates, treatment with alcohol inwhich the sulphate of the a!morphouu base is readily soluble, andprecipitation with ammonia, when it separates in dark-brown, amor-phous, readily fusible flocks.) Concusconine dissolves readily inacetic anhydride apparently withoiit formation of an acetyl-derivative ;from t h i s it seems that no hydroxyl-groups are present.Nitricacid converts it into a dark-green mass ; addition of nitric acid to itssolution in acetic o r hydrochloric acids gives the dark-green colorationcharacteristic of this group of alkalo'ids. Concentrated sulphuricacid dissolves concuscoiiine with bluish-green colour, becomingolive-green on beating. With chromic acid and sulphuric acid, itgives a coloration at first dark reddish-brown, then intensely dark-green. Although concusconine is tasteless, its solutions in acidshave a bitter taste.The platino-nhloridp, ( ~ , , H , 6 N , ~ 4 ) , . ~ 2 P t c ~ 6 + 5H20, is obtained as a voluminousyellow flocculent precipitat'e.The salts are as a rule gelatinous.The nornzaZ sulphate,forms small white prisms nearly insoluble in water and alcohol in thecold, sparingly soluble on heating. The acid sulphnts is a gelatinousmass readily soluble in hot water. By mixing an alcoholic solutionwith methyl iodide, and allowing it to stand 21 hours, there iORGANIC CHEMISTRY. 67obtained a mixture of two iodides in about equal quantities ; they canbe separated by the difference of their solubilities in hot alcohol.The less soluble a-compound forms microscopic hexagonal prisms ofthe formula C23H,fiN201,MeI, very sparingly soluble in hot alcohol,moderately poluble i n boiling water.By trextmdnt with silverchloride, i t is converted into the chlorid~, C2,H,,N,0,,hfeCI, crystallisingin microscopic needles, readily soluble in water and alcohol. ThepZa,tiuiochloride, ((=,,H,,M~N,OIC1),,PtClI + 4 H 2 0 , forms a yellowish-red flocculent, prccipitate, and is insoluble in water. The aurochlorideforms a dirty gellow flocculent precipitate, from which gold soonseparates. The sulplmte, (C2,H,,MeN,0J)2S04, formed by the action ofsilver sulphate on the iodide, is amorphous arid very readily soluble inwater and alcohol. I t s rotarg power in aqueous solution at p. = 3.764and t. = 15" is [%ID = + 73". The hydroxide, C2,H,,N,04Xe.0H +5H20, obtained by the action of baryta-water on the sulphate, cr.ystal-lises in colourless cubes, melts at 203", is rea3ily soluble in alcohol andboiling water, insoluble i n ether.The iodide of the /3-co)npoud,C27H26N101MeI, is gelatinous and dries in air to a horcy mass ; is some-whak soluble in boiling water, readily soluble in alcohol. The chlorideis amorphous. The platinochloride, ( C,,Hz,N,O,MeCl)?,PtCZ1 + 5H,O,is a reddish-yellow flocculent precipitate. The sulphate,( C23H2GN204Me)2S0i,is a brown amorphous mass, and has no action on polaiised light.The hydroxide, Cn3H,,NZO4Me.OH + 2$H,O, forms a brown amor-phous mass, readily soluble in cold water and alcohol.Chairamine, C,,H,,N20, + H,O, crystallises in white needles orthick colourless prisms, and melts at 140", or when anhydronq, at233.It is readily soluble i n ether and chloroForm, 1 part of t h ebase dissolves in 540 parts o€ 97 per cent. alcohol. The alcoholicsolution is strongly dextrorotary ([a]? = about looo). Dissolved insulphuric acid containing molybdic acid, the solution a t first colour-less becomes after a tiqie an intense dark-green. The hyrZroclJoride,C22HJY?0,,HCl + H,O, crystallises in colourless needles, sparinglysoluble in boiling water and alcohol, insolulde i n dilute hydrochloricacid. The pZci,tinochlo.ride, (C,2H2,N,04),,H,PtCIs + 2H20, formsyellow needles insoluble i n water and alcohol. The ??orrrrci/ suI/iJL,ite,(C22H26N204)2,H2SO~ + 8H,O, forms concentric gi-oups of colourlessneedles, sparingly soluble in cold water or alcohol. The fhicrcyanateforms white needles insoluble in water.Conchairlnmine, crysta!lises with both water and alcohol of crystal-lisatiori in thick colourless prisms of the formula C,,H,N,O, +H,O + CzH60, the compound showing three meltinq poiiits, namely,82-86" for the whole compound, 108-110" after expulsion of thealcohol, and about 120" for t h e anhydrous compound, the massresolidifying between each temperature.A small portion is convertedby the heating into amorphous conchairamine. Conchairailline isreadily soluble in hot alcohol, in ether, and chloroform, sparinglysoluble in cold alcohol. Its solution i n 97 per cent. :ilco+ol has arotary power [ a ] ~ = + 68.4" a t p. = 2 and t. = 15". The alcoholatedissolves in sulphuric acid containing molybdic acid, qivin? a brownf 68 ABSTRACTS OF CHEMICAL PAPERS.colorat.ion that soon becomes intensely dark-green.With potassiumchromate and sulphuric acid, i t gives a coloration at first reddish-brown, then dark-green, and reddish-yellow if boiled with excess,The hydrocldoride, C,,H,,N204,HC1 + 2H20, crystallises in colourlessplates, readily soluble in hot water and alcohol, spwingly solublein cold water, nearly insoluble in ether. The platinochloride,(C72H282O4)2,H2PtCI6 + 5&0,forms it dark-yellow flocculent precipitate. The hydroiodide, +crystallises in colourless needles, sparingly soluble in cold water.The tlLiocyanate crystallises in colourless needles, very sparinglysoluble in hot water. The sulphate, (C,,H26N204),,H2S0, + 9H20,crystallises in long lustrous prisms, soluble in boiling water.Then i t r a t e forms satiny plates o r needles very sparingly soluble in water.Conchnira.mine rnethiodide, C2,H2,N204,MeI, is obtained either in redcrystals containing 1 mol. H20, or in colourless crystals with 3H20.The ch7oride, C22&N204,MeC1 + 2H,O, crystallises in large colourlessrhombohedrons, readily soluble in water and alcohol. The pZnti?~o-chloride has the coEplex formula (C20,H2,N20JMeC1),,PtCil +( C,,H,6N,01MeHCl,),PtC1, + 14H20 ; it crystallises in orange-colouredneedles, and is insoluble in cold water. The nitrate forms colourlesssatiny plates. The hydro.cide formed by the action of moist silveroxide on the chloride, forms an amorphous brown mass of bittertaste, readily soluble in water, insoluble in ether.Chairamidine, C2,H,,NZO4 + H20, fornis an amorphous whitepowder, melts a t 126-128", and is readily soluble in ether, alcohol,benzene, and chloroform, insoluble in water.Its alcoholic solutionRhows the rotary power [ a ] D = + '7.3" at p. = 3and t. = 15". Itdissolves in roncentrated sulphuric acid with yellowish colour, whichlater turns dark green. The platinochloride, ( C22H,N,04),,H,PtC16 +5H&, forms yellow amorphous flocks insoluble i n water. The normalsulphafe and liydrochloride are gelatinous, the acetate forms a slimymass.Conchairamidine, C2,Ho,,N20a + H,O, crystallises in white needles,melts at 114-115", and is very readily soluble in ether, chloroform,alcohol, benzene, and acetone. Its solution in alcohol (97 per cent.)is levorotary, [a]= = - 60" a t p.= 3 (anhFdrous) and t. = 15". Itdissolves in concentrated sulphuric acid with an intense dark-greencolour. With chromic: and sulphuric acids, it gives a solution at firstbrown, then dark-green. The hydrnchlo~ide, C,,H,,N,O,,HCl + 3Hz0,crystallises in long colourless needles. The pZatinochloride,( C,,H~~NZOI),,HZ?~CI~ + 5Hz0,forms a yellow flocculent precipitate. The normal sulphate,(C,,H,,N,Od),HzSOI + 14H20,crystallises in long colourless needles, sparingly soluble in cold water.The tli iocynnate is amorphous, readily soluble in alcohol, and spar-ingly soluble in cold waterORGANIC CHEMISTRY. 69The substance described under the name of concusconidine in theauthor's earlier communication (Zoc.cit.) has been found to be a,mixture of alkaloids. A. J. G.Preparation of Albumin. By W. MIHAILOFF (BUZZ. SOC. Chim.,41, 547--548).-The author describes a new method for obtainingpure albumin. White of egg, filtered through muslin, is treated withthree times the quantity of a saturated solution of ammoniumsulphate, and to this as much more solid ammonium sulphake isadded as will dissolve. The tillnuminoid substances (globulins, glo-bulinates, and albumin) are thus precipitated. The precipitate iswaslied wit,h a saturated solution of ammonium sulphate, and, havingbeen rendered slightly alkaline with ammonia, is dialpsed. The waterwhich replaces the excess of sulphate and the alkalis of the precipi-tated ai buminoids, leaves the whole of the globulins and globulinatesin the precipitate, and the pure albumin i s obtained in solution.Thissolution map be boiled without coagulation taking place, is almostneutral in its reaction (slightly acid): and gives no precipitate withbarium salts. By means of' ammonium sulphate, all albuminoids andtheir derivatives may be precipitated. A. B.Colouring Matter of the Blood. By M. NENCRI and N. SIERER(Ber,, 17, 2267-2276).-The authors find that tlie use of amyl alcoholas a solvent forms a very good method for obtaining hcemin fromblood. Freshly defibrinated blood is mixed with a solution of saltand allowed to stand for 2 4 4 0 hours in shallow dishes. It is thenmixed with double its volume of 99 per cent. alcohol, and stirred welluntil thoroughly coagulated.The coagulated mass is allowed to standanother 24 hours, and then filtered off and spread on blotting-paper.It should not be allowed to get too dry, and is usually dry enoughafter exposure to the air for about 24 hours, when it should still loseabout 60-65 per cent. of water if dried a t 110". This partly driedmass is then powdered i n a mortar, 400 grams n e introduced into itflask with 1600 grams of amyl alcohol, and the whole heated toboiling; 25 C.C. of pure hydrochloric acid of sp. gr. 1.12 are thenadded, and the whole boiled for 10 minutes and filtered. As it cools,the amyl alcohol deposits the hcemin as hydrochloride in thinglittering rhombic plates. These should be washed with alcohol andether, and dried a t 105". 1.5-3 grams of pure crystals are obtainedfrom 3 litres of blood.I n this way, haemin was prepared andanalysed from human blood, the blood of the ox, horse: and dog. Ineach case some of the crystals were converted into haematin by solu-tion in caustic soda and precipitation with hydrochloric acid. Allthese specimens of hEmatin from different sources mere also analysed.In all cases when tlie hiemin crystals were dissolved in alkali, amyl:ilcohol was liberated, and i t was found that when prepared as aboveIit~min alwap contains amyl alcohol of crystallisation, which it losesiieither by digestion with alcohol nor by drying a t 110". Thecrystals do not change in composition even when digested with diiutehydrochloric acid.The analyses of the samples from various sourcesgave numbers agreeing very closely, and leading t o tlie formuli70 ARSTRACTS OF CHEMICAL PAPERS.(C32H3,N4Fe03,HC1)2,C5H,,0 for haemin hydrochloride crystals, andCR2H3,N,Fe04 for haematin ; so that the latter is produced from heminby the addition of the constituents of water. The properties of thehaematin obtained as above agree with those ascribed to this compoundby Hoppe-Seyler. From the ease with which haemin forms doublecompounds with indifferent bodies such as amyl alcohol, t h e authorsthink it probable that its composition varies according to the methodof preparation ; and that the various hzenioglobins are possibly suchdouble compounds of haemin with albumins.Concentrated sulphuric acid deprives hematin of its iron, andHoppe-Seyler, who named the resulting compound haematoporphyrin,ascribed t o it the formula, C6sH,4N4012-a more highly hydrogeriisedformula than that which he ascribed to hzematin.The authors findthat the real formula of haematoporphyrin is CnHJ2N4O5, and that it isformed according t o the equation-C32H,,N404Fe + H2S04 + 0, = C'aH32N,05 + FeSO, + H,O.Haematoporphyrin is obtained much more easily by treating hemincrystals with conceiitrated sulphuric acid. Hydrocliloric acid isevolved, the crystals dissolve, and the solution deposits hEmatopor-phyrin. Haematolin, which is the product of tlie action of strongsulphuric acid on hEmatin out of contact with t h e air, is neithersolnble in acids nor in alkalis, and has not been further investigated.When subjected to the action of reducing agents, hmnin andhze-eiatin yield various reduction-products according to the nature of thereducing agent, the temperature employed, &c.With t i n and hydro-ch I o ric R ci cl , th e chief p rod uct i s heaah y d 1'0 h mnntop o r p h y r in , C ,H,,N,O,,which is formed from hemin crystals, according to the equationC3,H30N40,Fe,HC1 + 2H20 + HCI + H, = C32H3PN40j + FeCLIt is a brownish-red pigment, easily soluble in ;tlcohol, eparingly i ndilute hydrochloric acid, insoluble in water and alkalis. Whenboiled with alcoholic potash, i t is converted into a product easilysoluble in aqueous alkalis, and very closely resembling urobilin inproperties. The authors are now investigating this compound, whichalso appears t o be formed in stnall quantities during the redoction ofhaemin with tin and hydrochloric acid.By long-continued boilingwith tin arid liydrochloric acid, a soliltion of hmnin becomes qaitecolourless, volatile siibstaiices with odonrs resembling pyricline heirigformed. Attempts to obtain oxidation-products of hematin provedfruitless, nothirig bn t oxalic and carbonic acids being obtained.Leyer and Koller state ( B e y . , 7, 1064) that hRn1iitin is split up bydilute sulphuric acid into lucine and tyrosine. When fused withcaustic potash-towards which it is very stable--haematin gives offammonia and pyrroline, b u t no lucine is formed. Leyer and K611erwere probably dealing with impure hzematin.The colouring matter of the hlood is undoubtedly allied to thecolouring matter of the bile, and the conversion may be expressed bythe equationC,,H,,N,O,Fe + 2H,O = CJ2HEI:,.N106 + Fe.1-I mnat in.Uilir~binORGANIC CHEMTSTRY. 7 1Whether hasmatin is converted in the liver into bilirubin or bilirubiiiinto hsrnatin and hmmin is at present very doubt’ful, but the authorsare much inclined, from analogy with the formation of glycogen fromdextrose, &c., to think the latter more likely. L. T. T.Studies on Blood. By H. STRUVE (J. pr. Chem. [2], 29, 305-350).-The author contests the hitherto accepted riew of the com-position of blood-crystals, which according to Preyer are oxyhsmo-globin, of the formula C6,H,,N,5rFeS30,,,. The author finds thatthese crystals are rendered insoluble by treatment with alcohol, with-out changing their form, and that, they can then be further decolorisedby treatment with alcoholic ammonia, glacial acetic acid, strongsulphuric acid, or chlorine water, and therefore regards them ascrystals of a colourless albuminous subshnce accompanied by aniiuute quantity of one or more blood colouring matters. By extract-ing with ether, water, and alcohol respectively, the author hasobtained from the blood-corpuscles three distinct groups of com-pounds. The portion soluble in ether is, at ordinary temperatures, abrcJwn mass, which is generally soapy but sometimes crystalline. Whenheated, it melts and burns, emitting an odour of fat and acraldehyde ;the ash contains traces of phosphoric acid but no iron. Its solutiongives an absorption-band in the red, and it contains cholesterin,lecithin, cerebrin, and glycerides. The aqueous extract, on the otherhand, leaves on evaporation an amorphous mass of dark colour, readilysoluble in alcohol and water, but only slightly so in ether. Itssolution gives a strong absorption- band corresponding with Preyer’soxyhmmatin alkali; it gives no precipitate with lead acetate OYmercuric chloride in the cold, but the colouring matter is completelyprecipitated on boiling. Acids produce a precipitate even in the cold ;this is readily soluble in alkalis and alkaline carbonates withoutevolution of ammonia. It gives no hEmin-crystals ; the ash containsferric oxide, phosphoric acid, and silica. Elementary analyses of thecoloiiring matter point distinctly to its being a mixture of severalsubstances. The author regards the colouring matter as a feebleacid, which is probably combined in the blood with soda or someorganic base, and proposes to name it hcematic acid. The thirdgroup of SII bstsnces is obtained from the corpuwles by extractionwith alcoholic ammonia, and is represented by a single crystallinecolouring matter, which is quite insoluble in water, alcohol, ether,and dilute acids, sparingly soluble in dilute ammonia ; the ashconsists almost wholly of ferric oxide. The alkaline solutions of thecolouring matter exhibit the spec truin of Preyer’s oxyhaematin-alkali : on adding an acid, the colouring matter is precipitated quanti-tatively in an amorphous state ; this colouying matter yieldshmrintin-crystals. The elementary analysis corresponds with theempirical formula C,,&N8Fe,~lo, which agrees very closely withHoppe-Seyler’s formula for hematin, C68H70N8Fe2010. The author isof opinion that the hematin analysed by Hoppe-Seyler was impure,and that the carbon and hydrogen were coiisequently low. Owing toits behaviour with alkalis, the author regards this crystallinecolouring matter as a feeble acid, and proposes for it thc name o72 ABSTRACTS OF CIIEUICAL PAPERS.lrcrmic acid. The blood-crystals are thus to be considered as crystalsof a blood-albumin (globulin-crystals) free from iron, which arecoloured by a definite quantity of hematic and haemic acids. Thequantitative determiuation 9f these two acids is a t present impossible,but’ supposing the colouring matter to be entirely hEmic acid, and ifthe proportion of iron in the blood-crystals be -42 per cent., and inliemic acid 8*71 per cent., then the blood-crystals are composed ofglobulin-crystals 95.18 per cent., haemic acid 4.82 per cent. More-over, since tbe above empirical formulq both of the blood-crystals andof hemic acid, are calculated from the proportmion of iron they contain,the difference between the two must be the empirical formula ofthe globulin-crystals-ClsSHw9N50S058, taking Preyer’s formula,and C200H331Nj9SOS2, from Hufner’s formula.It is at present impossible to decide between the above formulae,but i t is especially interesting that the percentage compositionindicated by either of them corresponds in a remarkable mannerwith that given by Gorup-Besanez for the albuminoids in general.According to the author’s theory, all the spectroscopic phenomenaexhibited by solutions of blood are due exclusively to the colouring-matters, haematic and heemic acids ; he has not, however, succeededin attificially producing by means of mixtures of these two bodies, thebands a and p, which are characteristic of oxyhemoglobulin, andwhich are exhibited by all fresh solutions of blood. All the otherspectroscopic phenomena of blood solutions, e.g., the spectra ofhemoglobin, metahemoglobin, and haernochromogen, are to be re-garded as spectra of certain definite products of oxidation, reduction,or decomposition of hematic and hEmic acids. P. F. F

ISSN:0368-1769    

DOI:10.1039/CA8854800034

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

72 ABSTRACTS OF CIIEUICAL PAPERS.P h y s i o l o g i c a l C h e m i s t r y .Digestibility of Potatoes and Carrots with Hay and Oatsby the Horse. By E. WOLFF and others (Bied. Centr., 184,615-617).-The following are digestive coefficients of potatoes and carrots con-sumed by two horses, the second having received only the carrots inconjunction with hay and oats, for the first died from colic during the‘‘ potato ” period :-Dry Organic Non-nit rogen.matter. matter. Albumin. Fibrin. matter.Potatoes.. . , 90.46 93.28 88.01 9-14 99.36Carrols . . . . 84.86 87.23 99.31 - 93.81Compared m-ith the digestive coefficients of sheep and pigs forpotatoesPHYSIOLOGICAL CHEMISTRY. 73Organic Nun-nitrogen.matter. Albumin. matter.Sheep.. ...... 87.5 65.1 92.8Pig .........93.3 52.5 98.0the comparison is much in favour of the horse.Referring again to the experiments, we find that carrots greRtlyassist the digestion of the fibre of hay, and that oats rather reducethe digestion of hay fibre, viz., 44.65-38.42, but, that the percentageagain rises when the carrots are consumed with the oats and hay.E. W. P.Elimination of Phosphoric Acid in the Urine in Insanityand Epilepsy. By A. LATLLER (Cow@. rend., 99, 572--573).-Theaii thor’s results, obtained from many hundred analyses made whilstresident officer in a large asylum, agree with those of Mairet. I nacute delirium, phosphoric acid and urea are eliminated in notableexcess; in excitable mania, the phosphoric acid is in slight excess,whilst the amciunt of urea is normal ; and in simple insanity the urinehas the normal composition. I n acute or excitable lypemnnia, theamount of urea eliminated is abnormally high, whilst that of phos-phoric acid is abnormally low.I n simple lypemania, the compositionof the urine is normal. I n general paralysis, the elimination of bothphosphoric acid and urea is related to the general morbid conditionsof the patient. A t or immediately after epileptic seizures, the urinecontains a high proportion of phosphoric acid and a low proportion ofurea. If the seizures succeed one another rapidly, the proportion ofboth phosphoric acid and urea is increased; but in the intervalbetween seizures the urine has the normal composition.C . H. B.Influence of Exhausted Beetroot Pulp on Cow’s Milk.ByA. ANDOUARD and V. DBZAUNAY (Con@. rend., 99, 443--445).-Whenbeetroot pulp, exhausted by diffusion and preserved i n silos, isemployed as part of the food of cows, the yield of milk is con-siderably increased, and the animals themselves gain in weight, theincrease in both cases depending on the particular animal and thenature of the other constituents of its food. The proportion of butteris likewise augmented, and apparent’ly its qiiality is not affected. Onthe other hand, if the pulp is given in large quantity without admix-ture of a sufficient proportion of green food, the milk has a disagree-able taste, and is much more liable to spontaneous coagulation. ‘l’hesedefects are probably shared by other easily fermentable foods, and itfollows t’hat such substances are to be avoided if the milk is requiredfor drinking or cooking purposes, but are advantageous when theproduction of butter or the fattening of the beast is the main object.C.H. B.Various Cattle Diseases. By EGGELING and PASTEUR (Ried.Ceittr., 1884, 540 -544) .-Eggeling describes two diseases to whichswine are liable ; both are of the nature of erysipelas, one contagious,the other not. He throws no light, on their origin, prevention, orcure. He also draws attention to a disease to vchich horned cattl74 ABSTRACTS OP CHEMICAL PAPEHS.are subject on farms attached to distilleries of potato-spirit, due toover-eating the refuse and its fermentation.P;lst,eur gives further information respecting his experiments onhydrophobia. When the virus from a mad dog is communicated t oan ape, from this to another, arid so on, the poison becomes soweakened that when again injected hypodermically into another dogi t is incapable of producing madness, and even when introduced intot'he brain by trepanning, an operation which hitherto has always beenfollowed by madness, it failed and, on the other hand, rendered theanimal invulnerable against the disease.Wheil, however, the virusis passed into the bodies of rabbits or guinea-pigs, its intensity isincreased bg each inoculation, and after a few such, when again corn-municaked t o the dog produces madness of a very much more dreadfultype, arid death invariably follows. Although the virus is weakenedwhen passed into the bodies of monkeys, it can be made to resumeits virulence by inoculating rabbits or guinea-pigs from the monkey,and so on until it is again passed to a dog, producing madness anddeath.Pasteur suggests a means of utilising the action of the virus onrabbits-from a dead rabbit he inoculates a live one, from that asecond, and so on ; but from each of these animals he inoculates adog (the same dog), the poison increases in virulence at each opera-tion, but the dog has passed through the previous stage and is notharmed, so that when the intensity of the virus is a t its maximumthe dog bea,rs it without hurt, although it would madden and killmother not so prepared.J. P.Physiological Effect of Lead on Ruminants. By ELLENRERGEBand HOFNIEISTER (Died.Centr., 1884, 536-540) .-The chronic effectsof repeated doses of lead on domestic animals has not been muchstudied ; lead salts, as is well known, have a strong affinit]y foralbumin, and when taken even in yery small quantities the accumula-tion of lestd albnminate in the systetn produces serious effects.Sheep were the animals experimented on, and the salt of leademployed was the acetate, in doses of 0.5 to 3 grams per day, gradu-ally illcreasing from the smaller quantity. The symptoms of leadsickness in the sheep are not remai*kuble, loss of appetite, apathy,disturbed rumination, muscular weakness, dry dull wool, diminntionof urine and of urea, disappenraiice of hippuric acid, presence ofalbumin in the urine, and protruding bowel.To determine the presence of lesd in the organs, the author in-cinerates, extracts with nitric acid, and precipitates with sulphnrettedhydrogen. The quantity contairied by different organs varies con-siderably, as much was found in the kidneys as in the liver, contraryto expectation-oiie would expect most in the liver, the metal comingearlier into contact with it by means of the portal vein. After thekidneys and liver, most metal is found in the salivary glands andpancreas, then follow the bones and nervous system ; the blood andmusculai- system were poor in lead, but the spleen held a compara-tivrly large quantity. The author thinks the poison attacks thenerrous system first, and then the muscular. Excretion takes placYEGETABLE PHTSIOLOQY AND AGRICKLTURE. 75h-y the kidneys, liver, pancreas, and saliva, according t o the prepnra-tion of lead emplojed ; it is perceptible in the urine in about 40 hours.J. F

ISSN:0368-1769    

DOI:10.1039/CA8854800072

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

TT,GETAULE PHYSIOLOGY AND AQRICELTURE.Chemistry of Vegetable Physiology and Agriculture.75Nitrogen necessary for Cultivated Plants. By THAER (Bied.Centr., 1884, 546--549).-The author in 1879 reported to R congress ofnnt~uralists a t Freibury, as the result of eleven years' experimerlts, thatthe nitrogen contained in the crops on which lie experimented, grownon sandy loem, was derived from the soil, t o half its amount. He hascontinued his experiments since then on potatoes, rye, barley, andpeas, and now arrives a t the conclusion that tbere is an unmistakablerelation between the quantity of nitrogen supplied by the soil and thatput into it by man.If man supplies nitrogen freely in t,he manure, nature respondsfreely in the crop ; if man is sparing, so is nature ; and he formulatesthe rule that in a year of fairly productive weather, if the farmersupplies in the form of manure one-half the nitrogen which he oughtto receive from the crop, that nature will supply the remainder. Heexcepts specially adverse seasons when, for example, exceptionaldryness prevents decomposition of nitrogenous substances ; in suchcases, sulphate of ammonia and Chili saltpetre, if used, are a completeloss, as they are never available after the first year.J. 1'.Formation of Sugar in Beets. By A. GIRARD (Bied. Centr., 1884,545--.546, and CYowpt. ?wL(/., 99, 808).-The author being of opinionthat light takes a very great part in the production of cane-suger inthe beet, undertook a series of experiments, extending over severalmonths. He had leaves gathered daily about four o'clock in the after-noon and three in the morning, and analysed them ; he found that theleaves gathered after the enjoyment of the whole day's light invari-ably contained considerably more cane-sugar than those pluckedafter passing through the night, the amount in the former being inall cases more than double that of the latter ; the glucose and reduc-ing sugars did not vary in anything like the same proportion.Heconsiders the leaves t,o be the place where the sugar is formed, fromwhence it passes t o the roots, and that a double process of osmose iscontinually being carried on within the cells of the plant, one carry-ing the mineral matters derived from the plant t o the leaves, theother bringing the completed saccharose to the Foots.Tollens agreeswith him in this view, which he says has long been accepted as true.In a paper recently published in the Conzptes renclus, the authorgives additional experiments confirming these results.Salicylic Acid in the Cultivated Pansy. By A. B. GRIFFITHSatid E. C. COXKAD (C'ILL'IIL. A-ews, 50, 10d).--Various pnrt,s of theJ. F7 6 ABSTRACTS OF CHEMICAL PAPERS.garden pansy were found to contain the following percentage of sali-cylic acid :-I. 11.Leaves ............ 0.1329 0.1 930Stems 00852 0.0856Roots.. ............ 0.0531 0.0521,..............D. A. L.Experiments with Manures containing Thiocyanates. ByG. KLEIN (Bied. Csntr., 1884, 519-520).-Three plots mere sown withbarley and oats, one remained unrnanured, the second was manuredwith ammoniacal superphosphate, the third was manured with thesame, receiving in addition 0.8 per cent.of ammonium thiocyanate.In the last plot, the plants were developed slowly, and the points ofthe leaves became brown ; this lasted two weeks, when rain came on,and the plants recovered their normal strength and appearance, andthey flourished as well as those in the other plots ; evidently the rainhad caused decomposition of the thiocyanate. With water culture, thenulritive liquid used contained 0 . ~ 1 gram of ammotlium thiocyanate tothe litre; old plants with six to eight leaves bore this without injury, butwhen the quantity was doubled they sickened a t once, and 0.1 gramper litre proved fatal almost immediately.In view of the decidedlypoisonous effects of the thiocyanate, the author cautions farmersagainst using manures containing it.Poisonous Effects of Ammonium Thiocyanate on Vegetation.By J. K ~ N I G (Bled. C‘entr., 1881, 520-522),-Foar flower-pots werefilled with loamy soil, each was manured with 8 grams ammoniacalsuperphosphate. No. 1 was left so, No. 2 received 0.05 gram, No. 30.10 gram, and No. 4 0.25 gram of ammonium thiocyanate; theywere put aside for five weeks, a t the end of which No. 1 had aplentiful crop of weeds; No. 2 only a, few, and the other t w o none.‘The weeds were removed, and the pots sown with barley and oats.The growth was good in all of the pots, and the pots containingthiocyanate surpassed the others, owing probably to the excess ofammonia and deconiposition of the thiocyanate.Similar experimentswere made, sowing milnure and seeds together; the results weresimilar, and were confirmed by others in which the plants werewatered n-ith solutions containing varying quantities of thiocyanate.The author csutioiis buyers of manures apainst the use of certainsuperphosphates now being actively pushed, and if they are usedadvises them to be sown some days before the seed; if possiblerainy weather should intervene.J. F.J. E’.Influence of Acid Smoke on Vegetation. By J. v. SCHROEDERand another ( R i e d . Ce7~tr., 1884, 555-556).-The damage done togrowing plants by smoke containing acid gases shows itself first by theleaves becoming yellow or yellowish-brown and spotted-in leaves ofthe pine family the points become yellow.Such parts on analysisyield larger proportions of sulphuric or hydrochloric acid, as the casemay be, than the healthy leaves. Schroeder says that 5.L$ab of sulVEGETABLE PHTSIOLOGY AND AGRICULTURE. 57phurous anhydride in the air will quickly injure plants, but plants areriot so sensitive t o hydrochloric acid. The most sensitive to snlphurousgas are conifel-011s trees, the least so agricultural plants and vegetables.Fruit trees are very liable to damage, plums and cherries more sothan apples o r pems.The author made a large number of analyses of affected trees inthe neighbuurhood of four different fqctories, in t w o of which zincblende was roasted, a bronze foundry, and a general chemical worksfor producing sulphuric and hydrochloric acids, chloride of lime, &c.;he found that all the plants whose leaves showed they had beenattacked, contained throughout their substance more of the acidsthan healthy plants. To meet the suggestion that the supplycame from the soil, he made several examinations of it also, theresults of which confirm his views. On examination of the ash forcarbonic acid, less was found than in healthy plants; the authortliinks it proved that the acid gases penetrating from the exterior tothe interior of the plant neutralise the inorganic and organic basesnecessary to growth, and substitute those of a hurtful character.J. F.Use of Copper Sulphate to Destroy Mildew.By A. PERREY(Compt. r e n d . , 99, 543--545).-When vine poles are steeped in Rstrong solution of copper snlphate, and vines of from four to sixyears old are carefully trained round them, the vines are protectedfrom mildew (Peronospoyn viticokn), but the efficacy of the coppersulpliate does not extend beyond a cylindrical space 0.2-0.25 metrei n diameter, having the vine pole for its axis. C. H. B.Carbon Bisulphide in Aqueous Solution as a Remedy forPhylloxera. By E. PELIGOT (Conzpt. rend., 99, 587-Nl) .-Theauthor confirms Ckiandi-Bey's observations respecting the an tjsepticproperties of carbon bisulphide. He finds that when carbon bisul-phide is briskly agitat,ed with water a t the ordinary temperature,100 C.C. of water dissolve 0.3: c.c., or 0.452 gram of carbon bisul-phide.The solution has no action on lead paper, but when boiled1-upidly for some t i m e it gives off its carbon hisnlphide, and the con-densed water contailis small quantities of hydrogen sulphide. Theauthor recommends the application of an aqueous solution of carbonbisulphide to vines instead of the liquid itself.Protective Influence of Growing Plants on the Undergrowth.By E. WOLLKY (Bird. Centr., 1884, 550--551).--The distribution ofwater in the soil, and the temperature, depend very much on whether itis in a state of cultivation or not; in fallow ground, the higher strata arethe drier, and the lower the more moist. When covered by vegetation,the contrary is the case, as the roots of the plants withdraw moisturefrom the subsoil, and the leaves, fruit, &c., of the growing plantspr,ltect the upper layer from the drying influences of sun and wind.Small seeds tyhich are near the surface fare badly in fallow ground,but when sown where they are protected by vegettction they growwell. As soon as their roots reach the lower layers occupied by theC.H. B78 ABSTRACTS OF CHEMICAL PAPERS.roots of the covering plants, these must be removed, as well onaccount of the exhaustion of moisture as of excess of shade.J. F.Four-course System at Woburn. By A. VOELCKER (Bled. Centr.,1882,623-626 ; Jour. A y i . Xoc., 19, 348--35ti).-This report refers tothe seaqon 1883, and is an account of experiments conducted in thesame manner as has been previously reported on and referred to inthis Journal.The highest yield of purple top swedes was obtainedfroni the plot (plot 3 ) manured with farmyard manure of knowncomposition mixed with Chili saltpetre, bone-ash, superphosphate,and snlphates of magnesium and potassium, the lowest yield(plot 1) from the plot which had received farmyard manure(cotton cake added to the food); on the second plot, grew Dutchwhite clover, and it was fed off by sheep which on plot 1 receivedalso cotton cake, and on plot 2 maize-meal ; the sheep on plot 1 in-creased in weight the most rapidly of all the flock, and this greaterincrease is due to the cake. The clover on 3 was of least value, theaction of the saltpetre showing itrelf by diminishinp the value ofthe succeedinq season.The wheat was lowest on plot 3, but thestraw was highest; bnt the barley was highest of plot 2, which hadreceived only farmyard manure made with maize-meal. E. W. P.Growth of Breadstuffs in Various Latitudes. (Rid. Centr.,1884, 626--628.)-In Europe, barley (and potatoes) can be grown asf a r north as 70". but, east and wedwards the limit, falls southwards.In the Faroe Islands (61-43") but little grain is grown, whilst inGreenland and Iceland none a t all. I n East America the limit is SO",which rises to 57--'43" on the western coast, whilst on the east coastof Asia it again sinks to SO", gradually rising to 60" (Obi river.), 67"Archangel, and finally i n Sweden to 70". I n the southern hemi-spheres, the regions of limited growth are not ascertained.Thelatitude does not wholly determine the limit, height above the seamust also be taken iiote of. I n Sweden, cereals will not grow a t aheight above R few metres, whilst in Switzerland they flourish at, aheight of 625-1250 metres ; wheat requires a higher temperaturethan rye or barleg, oats require least warmth. There are many dis-tricts in the Alps were by reason of the cold no winter corn can besown, yet the summers are hot enough for maize to grow well. I nthe Himalayas, maize is grown a t 933 metres, wheat a t 3125 metres,barley, oats, and rye a t 3750 metres, and in Thibet wheat ripens a t5625 metres. The chanqe in the temperature IS remarkable. Pro-ceeding eastwards, wheat again hecomes more nitrogenous, which factis accounted for by the harder winters, the hotter summers, and thesmaller amount of rain than is experieiiced in Europe.The followingfigures represent the percentages of nitrogen in several samples ofwheat :-Scotch, 2.01 ; North of France, 2.08 ; Lille, 2-18 ; Chemnitz, 2.42 ;Bavarian, 2.20 ; Eldena, 2.18 ; Moraviau, 2.36 ; Polish, 2-68 ; Odessa,3.12 ; Tayanzog, 2 54 ; Rjgsan, 2.47 ; Samaya, 3.47 ; European Russia,3.58 ; Wilna, 1.95 ; Cedtrilt Provir~ces, 3.57 ; South-eastern Provinces,3-72 ; Siberia, 2.65 ; Tobolsk, 2.74. The nitrogen in rye and barleTWGETABLE PHY SIOLOOT ASD AGRICULTURE. 79also varies : Scotch rye, 0.90; German, 2.12 ; Scotch barley, 1.42 ;Cultivation of two Varieties of Sorghum, and Preparation ofSugar therefrom.By V. PFUEL and another ( B i e d . Centr., 1884,628-GW) .--HO~C?LC sorghum and H. sacch.nratum were sown thin and011 the flat ; the method of cultivation is the same as for niaizP, and afterautumn cutting it throws u p a good feed for sheep. As regards thevalue of t,his crop as a source of sugar, i t has been found t,hat a t theperiod when the seed ripens there is 15 per cent. of saccharose present ;before that time the qnantity is only 1-3 per cent. That the yieldof sugar may be as high as possible, the rows strould be 4 feet apart,the seeds (six together) one inch deep, and each plant left a t 4 to 6inches apart from its neighbour. The rows should run north andsouth, and the land be kept well hoed until the plants are 3 to 4 feetCultivation of Sorghum in France. By N.MINAKGOIN (Bied.Certtr., l884,634).-The cultivation of sorghum is less costly than thatof beet, and the yield of molasses is less. By the use of Champonnois’apparatus, good brandy can be prepared, and the residue makes goodfodder, but the brandy must be .thoroughly rectified, which can beaccomplished without difficulty.Drying of Diffusion Cuttings. By M. M~RCKER and others(Bied. Cei~tr., 1884,630-632).-Hellriegel states that i t is advisable todry these cuttings thoroughly ata high temperature, after which theyahaorh but a relatively small amount of moisture, and keep better.Marcker thinks that the digestibleness is impaired by the high heating ;he also recomniends $ per cent. of lime to be added, and then pressureapplied before drying ; this prevents swelling, and renders thepressing more easy of accomplishment. Cunze and Stammer considerthat, this addition renders the fodder unpalatable ; moreover, thisper cent.is equivalent to 10 per cent. of calcium carbonate when thesections are dry. Marcker, on the other hand, says cattle eat thefodder with vigour, and that the lime only amounts to 4.4 per cent.,as part is removed by pressing-of the remainder 1.1 per cent. onlyis as carbonate, the rest being present as organic salt ; also clover-hayfrequently contains 3 4 per cent. of lime. Marcker gives the lossof organic matter occasioned by his process as 5-32 per cent.Bavarian, 1.72. E. w. P.high. E. w. P.E. W. P.I!!. w. P.Tobacco Culture.(Hied. Centr., 1884, 5Fi2.)--This paper containsnotes relative to the growth of tobacco in Gnadenthal, Switzerland.Three descriptions are cultivated-Virginia, Maryland, and Cuban.It is found that a soil rich in humus gives good results ; heavy soilsyield greater weight, but inferior quality; newly broken, warm soilproduces fine, nicely perfumed leaves. As the roots do not penetratethe soil deeply, the condition of the subsoil is not of much importance.Ttle best irianiire to use is well rotted, easily assimilable, strong cow-dung ; fresh horse and cow-dung mitke the tobacco sharp, heavy, andbititig. Irrigation with liquid manure is also advised. J. 880 ABSTRACTS OF CHEMICAL PAPERS.Influence of the Weather on Crops. By C. FERRARI (Bied.Cemtr., 1884, 589).-Rcgarding wheat, rye, and barley, the crop isless the more cloudy are the months March to June, the greaterthe number of wet days during spring, and the lower the temperatureof April to June.FrGm data collected in the valley of the Po, tjhecrop on irrigated rice fields is higher when the skies in July andAugust are unclouded; maize yields best when the summer isshowerg. During 1880, and by reason of the cold winter of 1879-80,the crop of grapes was reduced 75 per cent. when the mean wintertemperature was -40°, and the reduction is 50 per cent. when themean temperature is - 2". E. W. P.Dependence of Cultivation on the Depth of the Soil. ByHEINRICH (Bied. CerLtr., 1884, 591-593) -Vegetation is largelydependent on the state of concentration of the plant-food in the soil ;the fertility of the soil is not a t all measured by the total quantity ofnourishment present, for a deep soil may contain the same absolutequantity of plant-food as a shallow one, but there the concentrationis much lower.Consequently, if there is a want of manure, the soilmust be cultivated shallow, so as to keep up the concentration,nnd deep cultivation without a corrcsponding increase in manure isprejudicial to the yield ; deep cultivation, however, ensures thewelfare and certainty of the crop during hard weather, but a t theexpense of the yield.Influence of Physical and Chemical Properties of the Soilon Evaporation. By C. ESER (Bied. Centr., 1884, 505-519).-Although the amount of moisture in the soil depends greatly onmeteorological conditionfl, yet its physical and chemical state exercisesmuch influence, and as this is capable of arbitrary alteration, it is amatter of much practic(L1 importance.The author has therefore nladean exhaustire series of experiments with soils of various composition,details of which accompany the paper. The general conclusions a twhich he arrives are as follows :-The amount' of evaporation of a soil depends principally on theamount of water contained when thoroughly wet. All soils appear toyield aqiieous vapour a t the same rate. Evaporation proceeds so longas the upper layer of soil continues moist, the loss being repaired bycapillary attraction from the subjacent layers. When capillary attrnc-tion ceases to act, the upper layer dries, and evaporation ceases.This drying diminishes the effects of the ordinary agents of evapora-tion, wind, &c., and if the upper layer be broken up mechanically itinterposes a still deeper shield between the moist snbsoil and thedrying influences of the atmosphere ; the same effect is produced bya top dressing, or covering of the soil.The phvsical state of thesurface is also of great importance, the evaroration from a lumpycoarse surface being considerably greater than from a smooth and well-tilled one, but a too finely powdered soil yields water more readilythan that which is in a moderately gra,nnlnr state. Under naturalconditions, soil containing humus dries quickest, sand slowest, andclay stands intermediate.The amount of evaporation is greaterE. W. PVEGETABLE PHYSIOLOGY AND AGRICULTURE. 81in proportion as the surface soil is dark in colour ; when there issubsoil-water, the amount of evaporation depends on the thickness anddensity of the intermediate layers of earth. The position of the groundalso affects the question, land exposed to the south losing most. Theangle at which ground rises from the level is also important, theloss of moisture being nearly in proportion to the inclination.Influence of the Soil and its Cultivation on the Tempera-ture of and Moisture in the Air. (Part I.) By E. Womm( Bied. Cent?.., 1884, 58%-588) .-Employing thermometers, the bulbsof which were protected from direct radiation by conical paper shades,suspended at different heights over various classes of soils, the authorfound that the air over quartz sand was the warmest, followed by darkyellow clay, then chalky sand, and lastly peat ; but that the surface ofthe peat was the warmest, then the quartz sand, clay, and chalky sand.The probable cause for the higher temperature of the peat, whilst theair above it is cooler, is the amount of moisture which it retains, butwhich, when evaporated, removes much heat, On the other hand,the light-coloured quartz sand reflects much heat ; consequently theheat absorbed and employed to evaporate the water is at a minimum,and the heating of the air is the most intense.Chalky sand beinglight-coloured reflects much heat, but much water is also retained ;therefore much heat is retained, and the air temperature falls close tothat of the air over the peat.Generalising, we have-soils which arelight-coloured and dry commu~iicate most heat to the air, whichis reduced when the soil is moist; the minimum of the air tempera-ture is reached when the soil is dark-coloured, and the heat renderedlatent by water. Another set of experiments was made on bare soil,and on soil carrying C ~ O F ~ ~ P , the heights of the thermometer above thesurface being 58 cm., 90 cm., and 200 cm., and the results were :-(1) that the air over a field bearing a crop is cooler than it would bewere there nothing growing ; (2) the variation of temperatures underthe first conditions is less than under the second. The first resultis brought about by the fact that so much heat is absorbed for theevaporation of the water by the leaves, and direct insolation of thesoil is prevented ; moreover the absorptive capacity for heat exerted byplants is much higher than that of the stones on the surface.Whenthe plants were moistened, the temperature fell below that of the airabove the same class of plant which was kept dry.To observe the influence of orientation, a pyramid of earth (4 squaremetres) was constructed, the four faces of which were directed respec-tively to the four cardinal points, at an angle of 30" to the horizon. Aswas to be expected, the air over the southern side was the warmest,over the northern side the coldest, whilst the western was warmerthan the eastern in the evening, and vice uersd.Result of Removing Debris from the Surface of Sandy Soil.By E.RAMANX (Bied. Centr., 1884, 59&596).-The soil under obser-vation was sandy, and was covered with the dead needles of pine treesgrowing on it. A plot from which these needles were regularlyremoved by a rake was compared with another kept in its naturalFOL. m v m .J. F.E. W. P.82 ABSTRACTS OF CBEMICAL PAPERS.state. The second plot was covered with moss and coarse grass,these had been removed from the experimental plot ; as regards themoisture present in both plots, it was only in May that the unrakedplot was the moister, whilst during June to September the raked plotcontained most water down to a depth of 80 em. ; this is because, asthe year proceeds, the surface becomes more thickly covered by theleaves which, together with the moss, prevent the penetration of therain.By keeping the surface of this class of soil bare a considerableloss of mineral matter occurs, by reason of the rain falling on the baresurface, arrd carrying with it much soluble matter into the lower strata ;whilst at the same time decomposition of the silicates proceeds morerapidly than in the covered soil, because of the greater variation ofheat and cold. This statement is in opposition to that of otherobservers on the same subject, but in support of his theory the authorstates that there is 4.6 percent. of insoluble mineralsin the undisturbedsoil, whilst in the raked soil there is 3.6 per cent, ; also there is a greaterloss of sulphuric acid and potassiizm.Moreover, as he finds that thereis more nitrogen removed in the rubbish than is accounted for by theloss experienced by the soil, he considers that this class of soil canabsorb nitrogen from the a i r ; the quantity of total solids removedfrom the surface is much less than what is lost by solution in thewater passing through. E. W. P.Fine and Coarse-grained Superphosphates. By F. FARSKY(Bied. Centr., I 684, 601-604) .-In his earlier communications(Abstr., 1882,90, 550,653), Farsky found that sometimes fine-grained,at others coarse-grained superphosphates were most satisfactory. I nthese experiments, he has attempted to decide the question by experi-ments made under glass, giving in addition to the superphosphate,sodium nitrate, and watering the plants (buckwheat) once and fourtimes a day ; the result thus obtained was in favour of the fine super-phosphate and the more frequent watering.I n another series, thesodium nitrate was replaced by ammonium sulphate, and the water wasgiven (1) in four equal quantities during the day; (2) one half in themorning, the other half in the afternoon ; (3) one quarter morning andthree quarters in the evening ; (4) the same quantity as in the previousexperiment, but given after the soil was much dried. It was found thatthe regular watering was best on plots manured with the finely dividedsuperphosphate, whilst the irregular watering was more adapted for thecoarse-grained manu re. On the whole, the finely divided superphos-phate is to be recommended for agricultural purposes.E. W. P.Action of Soluble and Insoluble Phosphates. By A. VOELCKER(Bied. Centr., 1884, 599; Jour. Roy. Agri. Xoc., 39, 357).--This isthe report of the action of the above manures on the experimentalplots at Woburn, during 1880-81-82-53, i.e., during a whole rotationunder the four-course system. The report in 1880-81 has already beenreferred to in a previous volume, and as the clover in 1882 failed, wehave only to remark the results obtained in 1883, when the crop wasoats. The best yield was obtained on that plot previously manuredwith Redonda phosphate, which gave the worst results in 1881 ; disVEGETABLE PBY SIOLOGY AND AGRICULTURE. 83solved and raw bone-meal is advanta'geous, and the plots producedmore than the unmanured plot ; the lime plot ranks high, in all pro-bability because of the paucity of lime in the soil (I per cent.).E.W. P.Superphosphatic Gypsurn as an Absorbent of Ammonia.By E. HEIDEN (Bied. Centr., 1884, 606) .-Coprolites from Helmstad tand Goslar were treated with sulphuric acid, the resulting solublephosphate pressed out, and the residue again treated with acid ; theresidue now consisted of calcium sulphate, with 4-5 per cent. 8olublr,and 1-2 insoluble phosphate. Compared with other ammoniumabsorbents as to its action on farmyard manure containing 0.2 percent. of ammoniacal nitrogen, it was found to be vastly superior.E. W. P.Employment of Potash Manures in Brittany.By G.LECHARTIER (Oompt. rend., 99, 658--661).-The crops grown on thereclaimed soils of Brittnny after the application of phosphatic manure,rapidly use up the reserve stores of potassium compounds in the soil,and although the grmitic rocks fi-om which the soils have been formedcontain a notable proportion of potassium, the latter can only bebrought into an assimilable form by continual tillage and exposure tothe atmosphere. I t therefore becomes necessaSy to employ manuresrich in potassium compounds, and the use of such manures is attendetlwith highly beneficial results, especially if they also contain phosphatesand nitrogen. C. H. B.By MXRCKER (Bied. Centr., 1884,607-609).-With the exception of potassium sulphate on good loam,which raised the percentage of starch 3.5 per cent., all other potashmanures depressed it 1.5 per cent. ; nor was a good result obtained withthese manures (kainite, kieserite, &c.) as regards total yield. Thisstatement, however, only applies to spring manuring, for potassiumsalts, especially on light soils, are necessary for potatoes, but they mustbe applied at some other period than the spring. The effect of potas-sium salts on the nitrogen is remarkable ; they raise the total nitrogen,but the percentage of albumino'id nitrogen is lowered, the amidq-nitrogen being correspondingly raised, pointing to the conclusion thatthe manured tubers were less ripe than the unmanured, but whethcrthis retardation of ripeness was occasioned by the potassium, by thechlorine, or by the magnesia present, is not as yet proved.Potash Manures for Potatoes.E. W. P.Sulphuric Acid as Manure. By F. FARSKY (Bied. Centr., 1884,642).-A plot manured with a compost t o which sulphuric acid hat1been added, was less productive than another but unmnnured plot.This result was probably due t o free acid in the compost, as shoti-11by analysis, E. W. Y

ISSN:0368-1769    

DOI:10.1039/CA8854800075

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

84 ABSTRACTS OF CHEXICAL PAPERS.An a1 y t i c a 1 Chemistry,Preparation of Standard Solutions of Carbon Bisulphide.By A. LIVACHE (Compt. rend., 99, 697-698).-When carbon bisul-phide is agitated for a short time with a solution of soap in whichpetroleum has been incorporated by the method previously described(Compt. rend., 97, 249), the bisulphide will dissolve to the extentof 200 grams per litre, although only 150 grams of soap are present,and this solution can be diluted to any extent wit,hout precipitatingthe bisulphide. Resin soaps and various intermediate solvents, suchas petroleum, essence of terebenthene, he., can also be employed,and in this way solutions of different composition, containing definiteamounts of carbon bisulphide, can readily be prepared.Estimation of Minute Quantities of Silver.By C. F. F ~ H R(Cliem. News, 50, 114--115).--For the determination of very smallquantities of silver, the author proceeds as follows :-I0 grams of sub-stance mixed in the crucible with 20 grams of a mixture of eqnaIparts of flour and potash, are fused with 30 grams of proof lead andsalt in a muffle a t a bright red heat for about three hours. The leadregulus is scorified once, then, cupelled ; when it is the size of a poppyseed, i t is removed to a fresh cupel for completion, and is finallyfinished before the blowpipe. The silver bead, which should be per-fectly bright and white, is carefully removed, wiped with blotting-paper, and its diameter measured on a scale, which consists of twoconverging lines, graduated so as to show the amount of silver ; thebead is moved along until it touches both lines, and the reading istaken two or three times, with the aid of a lens.By this method abead may be measured which represents 0*00005 per cent. of silver,when 10 grams of substance are taken.Estimation of Manganese in Cast Iron or Spiegeleisen. ByC. L. BLOXAM (Chem. News, 50, 112--113).--Tht! following process isrecommended for the determination of manganese in presence of largequantities of iron :-The metal is dissolved in hydrochloric acid, and after the removalof carbon and silica in the usual way, the solution is heat'ed with afew crystals of potassium chlorate, diluted, nearly neutralised withammonia, the iron converted into acetate by means of ammonia mixedwith excess of acetic acid, and excess of sodium phosphate is thenadded.The precipitated iron phosphate is separated, redissolved, re-precipitated, &c. The combined filtrates from these two precipitationsare mixed with excess of ammonia and boiled (or, better, kept near theboiling point for one hour, and left standing over night). Manganeseainnionium phosphate is precipitated, filtered off, washed, ignited, andweighed as pyrophospbate, Mn2P2O7. Good results are quoted, andcompsre iavourably with some obtained by the bromine method.C. H. B.D. A. L.D. A. LANALTTKAL CEIEXISTRY. 85Volumetric Estimation of Manganese ; Influence of OrgmicMatter and Iron. By J. B. ~IACKINTOSH (Chem. News, 50, 75)-I n reply to a previous communication (Abstr., 1884, 220) of the author,it was suggested (ibid., 499) tlint the conditions under which hcworked were not the same as are encountered in the analysis ofspiegeleisen, and on this basis the author’s views were contested.111repudiation of this the author has now made seven experiments withspiegeleisen, using the method described in his previous paper (Zoc. cit.),and 0.5 gram for each experiment : in the 1st and 2nd, it was dissolvedin hydrochloric acid ; in the 3rd, 25 C.C. of standard potassium perman-ganate was added ; in the 4th, 35 C.C. permanganate and a considerablequantity of a mixture of various kinds of organic matter, which mereadded to the manganese solution after the hydrochloric acid wasreplaced by nitric3 acid, the heating being then continued until theorganic matter had disappeared ; in the 5th, the spiegeleisen was dis-solved in nitric acid, the 6th was the same as the 5th, with the addi-tion of organic matter, and in the 7th hydrochloric acid was thesolvent, 35 C.C.of permanganate being added without first evaporatingoff the hydrochloric acid. From the results of these experiments, it 13evident that neither the iron nor the carbonaceous matter of thcspiegeleisen, nor the extraneous organic matter, haye any practicaleffect on the result ; but that hydrochloric acid has the effect of lowey-ing the results, presumably from its action on the manganic oxide ;hence it is important that the potassium chlorate employed should befree from chloride.Expt.-25352535-Other substances present.I- ---Organic matter .. . . . . . .Organic matter . . , . . . . .Hydrochloric acid . . . . . .Oxidising power ofprecipitate, in terms ofC.C. permanganate.13 *1513.1523 -0526.9013 .I523.1026 -55Expt.Oxidising powerof precipitate less Mn inspiegel taken, in termsof C.C. permanganate.-9.9013.759 -9513.408G ABSTRACTS OF CHEMICAL PAPERS.The results were as in Table, p. 85, 0.5 gram of spiegeleisen beingtaken in each case. D. A. L.Separation of Arsenic from Antimony and Tin. By F.HUFSCHMIDT (Bw., 17, 2245-2248) .-When experimenting withRunsen’s and with E. Fischer’s (Abstr., 1881,191) methods, the authorfound that when the arsenic was present in the pentad state, it wasvery difficult to drive it all over by distillation with hydrochloric acid.He finds, however, that the following modification of this methodyields very accurate results.The solution containing arsenic is made up to about 250 C.C. by theaddition of concentrated hydrochloric acid.This liquid is thensaturated with hydrochloric acid and distilled, a rapid current ofh~-drochloric acid being passed through the solution during the wholeof the distillation. Almost every trace of arsenic passes over in thefirst 50 C.C. of distillate, but for perfect safety the author advises thecollection of about 100 C.C. of distillate. The results are equally goodwith arsenic as with arsenious salts. The very volatile arseniouschloride fclrmed should be condensed by passing into a Woulff bottlecontaining potash.Theauthor gives numerous test estimations of arsenic, both alone and inthe presence of antimony and tin, the results being very close andconcordant. The arscnic found was almost always within 0.3 percent. of that employed, when from 0.07 to 0.15 gram arsenic wasused. L. T. T.No trace of tin or antimony is volatilised.Examination of Water. By R. ANGUS SMITH (Second Report(1883) to the Local Government Board as Iuspector under the RiversPollutiort PreveiEtion Act).-This posthumous report consistsIof aninquiry into certain characteristics of potable and other waters, andespecially of new methods proposed by the author for examining theorganic suhtances found in them which are of such a character asmay be supposed to affect health.The first, which promised to bethe most important, indicates a method for measuring the amount oforganic activity, or animal or vegetable vitality, amongst the microbes(at least of a certain class) which exist in the waters. The secondpart of the report continues the proof, formerly given in the author’sfirst report (1882), of the natural purification of rivers, now, in hisopinion, beyond dispute, as it can be shown in the laboratory. Thethird part’ is an account of a method for examining water by means ofKocli’s gelatin process. This part the author considered to be onlypartly worked out, but its general character, he says, may be seen,and the novelty of photographic proofs is a valuable addition t oordinary chemical analysis.Part I.The Vydrogert Process.-This process depends on the factthat most natural waters when treated with sugar and allowedt o stand, after a certain time give off hydrogen gas. The for-mation of hydrogen during the decomposition of sugar by vibrioshas already been observed, and also its formation in very smallquantities from organic matter in some decompositions. The author,however, was unaware t h a t Heinsch, who first used sugar as ANALYTICAL CHEMISTRY. 81C.C. ofnitrogenfrom50 C.C. ofn7ater.evolvedtrst for water, observed that hydrogen gas was liberated, and hetherefore has brought forward the action ol sugar on the organicmatter in water, as a method for measuring the amount of organiclife existing in the water, by means which may be considered aspurely chemical.Tubes 7+ inches long, 3 inch diameter, and holding 50 c.c., werefilled with the water t o be examined, and 1 per cent.of grape-sngarwas added. These tubes were then inverted, sealed a t the bottomwith mercury, and allowed to stand f o r some weeks. If the purestdistilled water be used no gas is evolved, nor is gas evolved if thenatural water be first boiled. From most of the waters experimentedwith, gases commenced to collect in five days, and for purposes ofcomparison, the gases were collected and analysed after 21 days inthe whole series of results given in this report. The total amount ofgas obtained in that time varied from 0 O.C.to 14c.c. The amount ofgas remaining dissolved in the water after the evolution in the coldwas not considered, but it was the author's intention to have includedthis in his investigations. The presence of carbonic anhydride wasproved by absorption with caustic potash, the absence of oxygen bypyrogallol, and the presence of hydrogen by adding oxygen andexploding the mixture. Thepresence of carbonic anhydride was to be expected, the author beforewnalj sis having presumed that all the gas evolved was carbonic anhy-dride. Nitrogen had come partly from the nitrogenous compoundsdecomposed, and partly from nitrogen in solution, and it also was theauthor's intention to have investigated this decomposition. Thequestion considered in this report is the production of hydrogen, andas neither carbonic anhydride nor nitrogen has ever appeared in suchwses without hydrogen, the author considers that gas to be thecharacteristic of the decomposition.The results of the analysis of the gases evolved from a large numberof waters collected from various parts of the country are given in full.They are grouped iu 21 tables, of which the following are examples :-The following is a description of the process.The residue was found to be nitrogen.c.c* Ofcarbonicevolved50 C.C.ofwater.anhSdrideTABLE Il.-London Waters; received May 8, 1883. Sugar alone added,ABCL'.C of gasevolvedfrom50 C.C. ofwater.7-095-758.31C.C. ofhydrogenevolvedfrom5oc.c. ofa-ater.4.403 -745 *470.93 1-761-40 I 0.612-07 0.77Percentage composition ofgases.II I62-04! 13.16 24.8063-00 24-44 10.5663.21 1 24.90 1 9.200.Z l00.000.0T9- 'PIon. 000.000.060. Vl$6*'Z108.9118- €1ZT. EZ79.800.0oc). 080.01:00.000.000.006. 990.609.468. OTES. 689. I:00.000- 092.100.000.000.096. Z49.189.145- 0 'Po. TTZ. T:00.000- 048.000.000- 000.0'PZ- I:01. 1:94.099. 0 zv- 011. TI:00.000. 000.000.000.000.008- 919P- 64s. L11- 8 'Po. E00.F6r: 700.0 x00.0 P69.8 I00-0 H00.0 000.0 ic0 o . n 300.01 3EC*V 809.v B''SI:.ZT a94.091.1:6E. T0v.v 84.9 39.8 bZ-8 899.9 LE.01 'Bzo. oz00.0196.609.4 309.9 800.8 Bi I61:- 9z4. z28.ANALYTICAL CHEMISTRY.89The names of the London water companies to which the letters A, B, and C referare omitted in the report. The letters in Table 15refer to the following samples :-A. Fountain below Hadfield, Woodhead.B. Paradise Well, village of Tintwhistle.C. 1st Reservoir, Tintwhistle.D. 2nd Reservoir.E. Scum from 2nd Reservoir.F. Stream, mountain eide, between Tintwhistle and Woodhead.G. Mountain stream.H. Mountain stream, near Crowden Station.I. 3rd Reservoir.J. Mountain stream, near Woodhead.K. Mountain stream, 1 mile from Woodhead Station.L. 5th Reservoir.The following table gives the werage amount of hydrogen from allthe waters examined, and the number of samples in each table :-Derbyshire waters (Buxton and neighbourhood),Sugar done added to the waters ..............April 19th, 1883-Sugar and sodium phosphate added.. ..........Flintshire waters (Mostyn, Holywell, St. Asaph)-Sugar alone added to the waters ..............Sugar and sodium phosphate added.. ..........Sugar alone added to the waters ..............Sugar and sodium phosphate added,. ..........Sugar alone added to the waters ..............Sugar and sodium phosphate added.. ..........The waters were allowed to stand for 48 hours:then the clear water was syphoned off, andsugar added to the clear water .. ., ..........The waters were allowed to stand fGr 48 hours:then the clear water was syphoned off, andsngar added to the deposit.. ................London waters ; received Feb.13th, 1883-London waters ; received April 12th, 1883-London waters; received May 8th, 1883-Table 11 (see page 87) ......................Table 12 ( .. 88) ......................Table 13 ( .. 88) ......................Table 14 ( .. 88) ......................Lancashire waters ; collected October, 1883-Table 15 ..................................Sewage rivers: Irk, Irwell, Medlock, and canalWith sugar addotl .......................... waters-Averageamount ofhydrogenevolved in C.C.from 50 C.C.water.1 *091 *561 -952 -012 -692.592 -853 *202 5 43 *5'74 -543 -913 -004.843 -718 *88Numberofsamples.9977565555333311190 ABSTRACTS OF CHEMICAL PAPERS.amount ofhgdrogenevolved in C.O.from 50 C.C.OfAverage 1----------Salford sewage water-Scum from reservoir a t Woodhead ................IMud from a stream at Buxton-With sugar added ..........................Sugar alone added .........................Sugar and sodium phosphate added.. ..........5 -0416 -804 -495 *53water.4111The author considered his results-when it is remembered that theyare first experiments of a very delicate nature-as fairly uniform,although in certain instances unexpected results were obtained. Fromthe analyses it is found that the higher waters in Derbyshire giveout less hydrogen than the lower waters where sewage enters thebrooks, and also give out less gas than the lower waters of thedrainage of the Thames Valley, or any other place. The waters ofLongdendale and neighbourhood, which form the supply of Man-Chester, as a rule are very free from hydrogen, and in some trials ofManchester water no hydrogen was obtaiiied, showing the greatpurity a t times of the water so far as this test is capable of illus-trating it.A seyies of experiments was also made to test the effect of bacteriaon the evolution of hydrogen, and to find if they were the actual causeof the evolution.The microbes used were obtaine3 from the surfaceof gelatin which had been dissolved in water containing more or lessbewage, and allowed to stand for a time. The liquid portion at thesurface contained countless numbers of bacteria; and in each case asmall drop was all that was required.The results showed (for fullparticulars the original paper must be consulted) that Medlock waterwhich contains sewage and chemicals, gave out its hydrogen mcchmore quickly when bacteria mere added : that the addition of bac-teria to distilled water produces results such as are found in less purewater ; that Mnnchester water when boiled and thus renderedincapable of producing gas from sugar, gave out hydrogen when bac-teria were added ; and that by adding more sugar and bacteria to awater which had given oxit a great deal of hydrogen, gases con-sisting of hydrogen and carbonic anhydride, with little or no nitrogen,were again evolved.The author, in discussing the value of this method, considered thatin many natural waters sugar is made to ferment and give outhydrogen gas, and that the amount of this gas, which in some is verysmall, increases in proportion to the impurity in the water.Thatthe kind of microbes is such, that if present in large numbersthey render the water impure to the senses, and that decompoANALYTIC IL CHEMISTRY. 91sition is caused by organisms i n this way is shown by the absence ofhydrogen on treating boiled water by sugar.That this method of estimation deals with bodies of an offensivecharacter we have the fact of their increase from the purest water ofthe moiintain t o the worst sexage. As far as the hydrogen is con-cerned, there seems to be a regular gradation. According to Pasteur,it appears that microzymes may be various in activity without changingtheir appearance, that they may be attenuated to any extent, and thattheir power may be virulent to any extent.To say that a certainclass of microbes is present is not to have a ver-y definite idea, theimportance lies in the activity. The author could not say whetherthis method is a real measurement of the amount of organic life, oronly a measurement of the vitality of certain organisms? but ifmicrobes when very active decompose sugar and produce hydrogen ingreater abundance than when inactive, then the hydrogen becomes themeasure of their power.The author has further discussed and speculated as t o the value ofthis method a t great length, but finally says that whether it measuresthe activity, quantity, or other characteristics of the organisms in thewater, is a matter yet to be decided.Part 11.The Eliininutioii of h‘itrogen during Putrefaction of Water.-This is a continuation of the author’s work published in his firstreport on water (1882). From the first report he quotes largely, andhas shown (1) that bodies containing protei’n compounds when inabundance of water and in common air may be oxidised and form nitricacid ; (2) that the same organic bodies in a state of decomposition,and in water, may be oxidised a t the expense of the nitrates, and giveoff nitrogen. In the first case, a certain qnantity of sewage is in thewater, b u t is overpowered by the air, in the second the sewage is inexcess, and overpowers the nitrates. He has shown also that thepurification of sewer river water is effected in nature first by putre-faction, and secondly by thorough oxidation.He gives some furtherresults which show the escape of free nitrogen from sewer river waterwhen treated with potassium nitrate.(1.) 1150 C.C. of Medlock water when treated with 1 gram of nitregave off 103.3 C.C. nitrogen in 39 days (1 gram potassium nitratecontains 110.2 C.C. nitrogen).(2.) Bridgewater Canal water and Manchester water, when treatedwith potassium nitrate, gave off no nitrogen after 46 days’ observation.(3.) Salford sewage water when treated with 0.1 per cent. of iiitregave off the whole of the nitrogen contained in the potassium nitrate,in 22 to 28 days ; in some cases a little more was given off afterwards.The remainder of this part, contains Lauth’s results (Conzpt.Tend.,84, 417) on the same subject.Part 111. The Gelatin Pmcess.-The use of gelatin as an indicatorof the amount of rital matter in water was suggested by Koch’swork. The chief advantage in the method is that the gelatin preventsthe water from moving, and that every point which has vitality in i tis able to assert itself, the number existing in the water being seen a ta glance.A solution containing 6 per cent. of solid thin leaf gelatin wasThe following is the method employed by t8he author :9-2 ABSTRACTS OF CHEMICAL PAPERS.heated to loo", clarified with fresh albumin, and filtered. This solu-tion melts a t about 27". 25 C.C. of this solution, at a little over 27",were mixed with 25 C.C.water in a test-tube, about 8 inches long and1 iuch diameter, closed with a stopper of cotton-wool, and kept for a,few minutes a t 27". Along with the waters to be tested, distilledwater and Manchester water were thus treated for the sake of com-parison. The rest of the process consists in observing day by daythe changes in the gelatin. The number of spheres or centres ofmicrobes is one measure, the depth to which the surface becomesliquid is a second, and the number of days before putrescence sets inis a third. I n the case of most waters, the gelatin is completelydecomposed in about 7 days, but much depends on the temperature,and in the case of pure distilled water it may keep for a much longertime ; a photograph of a gelatin solution with distilled water is shownwhich at the end of 15 days is still quite undecomposed.The resulhs seem to show that in sewer waters, and in very impurewaters, the gelatin is rendered liquid a t the surface, and this fluidityincreases until the whole becomes liquid.The liquid is alive with bac-teria. I n the case of potable waters, such as the Manchester water, thewhole tube becomes in two or three days filled with perfectly formedtranspa4rent spheres at the bottom of which is a little white line.These are fonnd to be liquid and to contain a great mass of activeand inactive bacteria. Also a number of minute white specks appearwhich seem to indicate the number of points of vitality; they arealso filled with bacteria, but of a different kind, as they do not formliquid spheres around them.In some cases, gases are evolved, andform globules or discs in the gelatin. The effects, or rate of effects,depends mnch on the temperature, and, without comparison withknown waters, conclusions should not be drawn.Of all the forms of change, that which seems to be connectedwith the most offensive water, is the liquefying of the surface. Theother changes are more or less objectionable, according to the numberof points of activity which the author considers are measures ofimpurity. Whether these germs are to be sixpposed as productive ofdisease, or productive of it by their multiplication, the author wasunable to say, but in those cases where they are most numerous, thewater is not so good to the senses, and therefore the method is clearlyan independent measure of excellence.The hydrogen method agreed well with the results obtained withgelatin, but the gelatin sometimes showed minute impurities whenhydrogen did not appear.Whether the microbes which transformgelatin also produce hydrogen, the author was unable to decide, but asthe results correspond very fairly, the probability is in favour of theaffirmative.The author had prepared photographs of 125 samples of watertreated with gelatin (in some cases with sugar, or sodium phosphate,or both, in addition), and has minutely described many of them.Unfortunately the whole of the photographs could not be included inthe report, but those selected by the author are very good examples ofthe appearance of the gelatin after 3, 5, or 7 days.A few of themare comparable. The photographs of a series of London waters w i t ASALTTICAL CHEJIISTRY. 93gelatin may be compared with those of a series of Derbyshire andFlintshire waters-the London waters seem to be inferior to the others.Manchester water was always found superior by this test to Londonwater. For t#he description of the changes, the original paper and thephotographs themselves must be referred to. The following is adescription of a few :-October, 1883.--Distilled water : No alteration during 8 days’observation.Manchester water (from laboratory tap) : After 3 days, innumerablesmall spheres appeared. After 4 days, these spheres had increasedin size, the surface of the gelatin remaining firm.After 5 days, adeposit had formed at the bottom of the spheres, and transformationof the gelatin was taking place very rapidly.Samples of vater taken from the reservoirs for the supply ofManchester, between Woodhead and Hatfield, gave similar results tothe Manchester tap water. Samples of water, taken from the moun-tain sides at Woodhead, developed a large number of “ points ” after3 days. After 4 days, discs of gas appeared, but spheres were absent.“Dots” or small “specks,, were observed, but they did not increasein size.Scum taken from one of the reservoirs showed after three daysinnumerable dots dispersed throughout the gelatin, and a large numberof discs of gas also appeared. The gelatin gradually softened, andthe development of the germs was far more advanced than in any ofthe other specimens of water under examination.April 2Oth, 1883.--DistiIled water : No alteration after 15 days’observation.Manchester water : On the second day a number of mimite spheresappeared, which had enlarged on the third day, the surface of thegelatin being unaltered.On the fourth day the spheres had increasedin size and number, and a deposit was forming at the bottom of thespheres.Water from below Buxton receiving sewage, although lookingclear: On the second day, a distinct band of minute spheres appearedat the surface of the gelatin. On the third day, the surface of thegelatin was quite liquid to a depth of 5 mm., and of a greenish colour.On the fourth day, a few discs of gas appeared, the surface of thegelatin being liquid to a depth of 7 mm.In the same way, London water collected from the various com-panies’ supply in February, April, and May, 1883, are described bythe aid of photographs, and compared with distilled and Manchesterwater. A.B.Testing Mineral Oils. By E. VALENTA (Dhtgl. potyt. J., 253,418-421) .-Referring to the adulteration of mineral oils with resinoils the author, in a previous communication (Abstr., 1884, 1079)ziientioned that by the aid of glacial acetic acid at a certain tempera-ture, it is possible to detect adulterations of mineral oils with resinoils with compayative ease. He has cont,inued his researches in thisdirection, and now gives the results of some experiments which hehas obtained in conjunction with Feigerle94 ABSTRACTS OF CHERIICAL PAPERS.-NO.-12345678910-flolubility Values of D$eren,t Mineral Oils.i3p. gr. of GlncialAcetic Acid at 15" = 1.0562.Name ofmineral oil.Lubricating oilDitto , . . . , . . .Engine oil e e l -low)Machine oil(yellow)Heavy mineraloil (thin)Light mineraloil (thin)Fatty mineraloil (thick)Green oil . . . .Blueoil.... ..Vulcan oil., . .0 -90900 -90900 *91390 *91090 *90900.88800 *90700 -91050 -90160 *9259Oil dis-solved by100 gramsglacialacetic acida t 50".grams.5 -7648- --5 -77895 *73334 "77784 *28104 5'0092 *67296 -49886 *01703.3451Oil dis-solved by10 C.C.glacialicetic acida t So^.-grams.0 '60890.61040 *60560 *50460 -45227I0*4965 I 0 -2823 J0 -68490 *63420 *3525Remarks.---Pale yellow, clear, highlyfluorescent oil, almostcolourless.Dark orange colour,odourless, highly fluor-escent, and clear.Pale ydQW, highly fluor-escent, and odourless.Oils having a pale ytl-low to orange-yellowcolour, fluorescent,perfectly neutral, andodourless.Blackish - brown non -transparent oil, having6 tarry odour.Dark brownish - red,opaque, highly fluor-escent, tarry odour.Almost black - brown,opaque, thin liquid oil,t,arry odour, highlyfluorescent.For quantitative estimation, the method adopted is as follows :-2 C.C.of the oil are treated with 10 C.C. glacial acetic acid, and heatedfor five minutes in a loosely corked test-tube in a water-bath. Themixture is then passed tlhrough a small filter, and the middle part ofthe filtrate collected.A weighed quantity of this solution is titratedwith standard alkali and the weight of glacial acetic acid containedin the solution calculated. The difference in the weight between thesolution and the glacial acetic acid gives the aniount of oil containedin the former. It has been found, however, by experiment that thesolubility does not increase with the percentage of resin oil containedin a mineral oil, hence this method is not suitable for the quantitativedetermination of the amount of resin oil in such mixtures. The sub-joined table gives the numbers which were obtained for the solubilityof different mixtures of oils containing a known amount of resinoilANALYTICAL CHEMISTRY.95Amount ofresin oil in themixture.Solubility of Diferent Micctures of Yellow Engine Oil and Crude ResinSp. gr. at 15": Glacial Acetic Acid = 1.0562, Mineral Oil at 50".Oil = 0.9139, and Resir, Oil = 1.0023.Oil dissolved Oil dissolvedby 100 gramsglacial acetic , glacial aceticacid. acid.Remarks. by 10 C.C.--Per cent. by vol.0255075100-------grams. grams.5 -7333 0 -6056 The crude resin oil was obtained7 -3973 0 3'796 from Wagenmann, of Vienna.8 *3653 0 -8816 I t had a dark brown colour,12 -5601 1 * 3237 tarry odour, high viscosity,16 -8782 1 .'ips8 and resinified in the air.The rotatory power of resin oils may be employed for the recogni-tion of the purity of a mineraI oil, the latter being optically inactive.For this purpose, the author recommends the use of &Iitscherlich'spolarising apparatus, with the modification that in the case of highlycolonred oils, they are first subjected to a treatment with potassiumferrocyanide and filtered.A further difference between resin andmineral oils is their behaviour with iodine. The author adopted themethod recently described by Hub1 (ibid., 253, 284), and found thatmineral oils fail to absorb more than 140 mgrms. iodine per gramof oil, whilst the iodine number for resin oils ranged between 430 and480 mgrms. D. B.Determination of the Nature of the Crude Oil in Turkey-red Oil. By A. M~LLER-JACOBS (Ding].polyt. J., 253, 473).-Onrendering a very dilute solution of Turkey-red oil alkaline withaqueous ammonia, the mixture shoiild remain perfectly clear on stand-ing. The formation of a precipitate indicates the presence of solidfats or their corresponding natural glycerol ethers (palmitin andstea,rin), and shows that for the manufacture of the Turkey-red oileither impure castor oil or other crude oils, such as rape oil, sesam6oil, train oil, cotton-seed oil, olive oil, or mixtures of both were used.The separation takes place only in very weak solutions, in which thesolvent action of sodium sulpholeate fails t o prevent the precipitationof the solid fats.To recognise the purity of Turkey-red oil, Beusemann recommeiidsthe determination of the melting point of the fatty acids separatedtherefrom.On decomposing Turkey-red oil by boiling it with diluteacids, and determining the melting point of the resulting mass, whichconsists of unaltered oil and liquid and solid acids, it is possible also tojudge of the nature of the crude oil employed in the manufacture.Finally, the behaviour of the separated mass with alcohol affordsvaluable indications of the purity of Turkey-red oil ; that from thepure oil, obtained from castor oil, forming a clear solution, whilst themass separated from other crude oils gives a turbid solution wit96 ABSTRACTS OF CHEMICAL PAPERS.alcohol, and this, on standing, deposits oily particles consisting of un-a1 t ered t riglyc erides. D. B.Bromine as a Test for Quinine, Narcotine, and Morphine.By A.EILOART (Chew. News, 5O7102-l03).-The following note refersto the delicacy of various modes of employing bromine for the detectionof certain alkalo’ids. QzzLinjne.-mlm part can be detected in solu-tion by the red colour produced by the successive addition of brominewater, mercuric cyanide, and precipitated chalk; & by usingbromine water, potassium ferrocyanide, and borax, Vogel’s test ;by employing petroleum instead of mercuric cyanide, or withBloxam’s test (Abstr., 1883, 1175), when chalk is added before thebromine, or Iny the green fluorescence produced wheri a neutral solu-tion of quinine is mixed with excess of bromine, boiled to expel theexcess, and then cooled ; dm when bromine (without debrominat-ing agent) and chalk are used ; in such cases, neutralising agents, weakammonia, zinc oxide, &c., produce a crimson colour ; drn can alsobe detected with Bloxnm’s test, as described (Zoc.cit.). Narcotirm-ing a slight excess of bromine, is neutralised with calcium carbonate ;with more than mlm of narcotine, the red is followed by violet andblue. This is the case even after the solution bas been brominatedfor some time, whereas quinine gives no colour with chalk afterfitanding. Tartaric or acetic acid impedes the production of the colour.Morphine.--&$.5 part produces a red colour, when a solution contain-ing it is boiled with excess of bromine water, neutralised with chalk, andagain boiled ; smaller quantities give rise to an orange or brown colora-tion, which is bleached by bromine water ; & can be detected bythe bleaching effect of bromine water on the subdivided neutralisedsolution.Strychnine, cinchonine, and c a f e h e give no characteristicreaction with bromine and chalk.A-_ 6$oo part gives a red colour if its hydrochloric acid solution, contain-D. A. L.Estimation of the Wool, Silk, and Cotton in Tissues. By A.REMONT (Chem. News, 50, 123--124).--Four portions of the materialto be examined are taken, each weighing 2 grams. One is reserved,the other three are boiled for a quarter of an hour in 3 per cent.hydrochloric acid, and if the liquid is very much coloured the boilingis continued for half an hour longer with fresh acid ; this operationremoves the dressing; one of these three samples is reserved. Toremove the silk from the other two, they are dipped for one or twominutes into a boiling solution of basic zinc chloride (60” B.), which isprepared by heating a mixture of 1000 parts of fused zinc chloride,850 parts of water, and 40 parts zinc oxide, until the lather is dis-solved. The two samples are then washed, first in acidulated and thenin pure water ; one is reserved, the other is gently boiled €or a quarterof an hour in 60 to 80 C.C. of soda solution (sp. gr. 1.020) to removewool ; the residue is washed as in the last case.The four samples are now heated in distilled water for a quarter ofan hour, left to dry spontaneously, and are then weighed. The firstshould weigh 2 grams, if it does not, any considerable loss must betaken into account, the difference between the weights of samples TECHNICAL CHEMISTRY. 97and 2 is the weight of the dressing, between 2 and 3 that of the silk,between 3 and 4 the wool: the residue being the vegetable fibre ; thelast two are only approximate, as the vegetable fibre is somewhatattacked by the soda solution.Boiling with dilute acid removes dyes readily from cotton, lessreadily from wool, and only imperfectly from silk. Dark-colouredsilks are most heavily weighted, and sometimes the weighting is soheavy that the colour is not sufliciently removed ; it is then necessaryto determine the amount of iron present in the ash of a few threads ofthe treated sample, and if it exceeds 5 per cent., it must be taken intoaccount . D. A. L

ISSN:0368-1769    

DOI:10.1039/CA8854800084

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

TECHNICAL CHEMISTRY. 97T e c h n i c a1 C h e m i s t r y.Antiseptic Properties of Carbon Bisulphide. By CKIAND~-B EY(Compt. rend., 99, 509--511).-Carbon bisulphide is soluble inwater to the extent of from 2 to 3 parts per million at 18-20". Byagitat,ing carbon bisulphide with water in a flask completely filled, asolution can be obtained containing approximately as much as0.5 gram of carbon bisulphide per litre. Carbon bisulphide alone andin aqueous solution arrests all fermentations, kills microbes, and isone of the most energetic of antiseptics. It moreover possesses con-siderable penetrating power. A solution of carbon bisulphide inalcohol of 96" decomposes slowly and gives rise to various products,notably hydrogen sulphide.During 20 years' experience amongst work men continually exposedto the vapours of carbon bisulphide, the author has never observedany paralysis of lower or upper limbs, nor any destructlion ofmasculine faculties.When breathed in certain proportions, thevapour of carbon bisulphide produces effects similar to those ofetherisation, the only disagreeable after-effect being heaviness of thehead, which soon passes off. When applied to the skin, carbon bisul-phide acts almost instantly as an energetic revulsive, the pain pro-duced being similar to that caused by boiling water. The pain,however, ceases as soon as the carbon bisulphide is volatilised, andno ulceration is produced.The author recommends the use of carbon bisulphide both externallyand internally, in aqueous solution and in the form of spray, in casesof cholera, typhoid, and other diseases resulting from the action ofmicrobes.It may also be used to disinfect the evacuations, clothes,&c., of cholera patients and others, and an aqueous solution may beemployed to water the streets and to wash out rooms in cases ofepidemics. Dr. Dujardin-Baumetz finds that the internal administra-tion of an aqueous solution in cases of typhus arrests the diarrhoea,and disinfects the breath and the excretions of the patient.When the aqueous solution is swallowed, it has a sweet, warm taste,VOL. XLVIII. 98 ABSTRACTS OF CHEMICAL PAPESS.nnd.produces a sensation of warmth in the stomach, followed aftersome time by irritation of the nose similar to that produced by snl-phurous anhydride.These sensations are followed by slight heavinessof the head, which soon passes away.For medicinal use, the carbon bisulphide must be carefully purifiedby agitating i t with mercury until no further formation of mercuricsulphide takes place. C. H. B.Preparation of Potassium Magnesium Sulphate. (Din$.polyi. J., 254, 48.)-The Cornsolidirten Alkaliwerke of Westeregelnfirst prepare the criide salt as artificial carnallite, which is thendecomposed by t.reatment with schonite mother-liquor. By thistreatment, the amount of potassium chloride is doubled, whilst themother-liquor becomes praportionally richer in magnesium chloride.The product is then warmed with a corresponding amount of magne-sium sulphate solution. On cooling, schonite, amounting to 65-70per cent.of the potassium chloride employed, separates out, the restremaining in solution, which is applied as above, to decompose thewtificial carnallite. The solution can be evaporated so that artificialcarnallite crystallises out, or it may be employed as solvent forcrude salt. J. T.Manufacture of Aluminium. (Dinql. polyt. J., 253, 426. j-(+adsden (Ger. Pat. 27,572, August, 1883) proposes to preparealuminium by subjecting aluminium chloride to the vapour of sodiumevolved from retorts in which a mixture of sodium carbonate withcharcoal is intensely heated.For the manufactdre of aluminium-bronze, Webster (Ger. Pat.28,117, January, 1884) prepares (1) an alloy consisting of 15 partsaluminium and 85 parts tin, and (2) an alloy composed of 17 partsnickel, 17 parts copper, and 66 parts tin.He then fuses equal partsof these alloys witlh copper, the best result being obtained with84 parts copper to 8 parts of ea8ch alloy. The resulting bronze issuitable for the preparation of castings of various kinds, tubes, guns,plates, wires, hydraulic apparatus, boiler-plates, domestic utensils, &c.(Diqzgl. polyt. J.,254, 89-90.)-The mining and smelting directors of Konigshuttepropose to roast burnt pyrites containing zinc with sodium chloride,and then to extract with water acidified with hydrochloric acid. Thesolution is freed from copper when necessary, and freed from sodiumsulphate by concentration and cooling. The zinc solution is thentreated for metallic zinc or for zinc preparations, by known methods.J.T.D. B.Utilisation of Zinciferous Burnt Pyrites.The Siemens-Martin Process. By M. JUNGCE (Difigl. polyt. J.,253, 509-514).-The author gives a detailed account of the mode ofworking this process at the Phenix Iron Works in Ruhrort. The gasgenerator consists of eight chambers, which are charged at intervalsof three hours with about 600 kilos. of coal having the followingcomposition :TECHNICAL CHEMISTRY. 99OxygenCarbon. Hydrogen. and nitrogen. Ash.7 1-10 4.24 11.92 12i4The g a s from two chambers is sufficient for the working of one rever-bwatorg furnace. Each furnace is provided with four regeneratingchambers. The charge consists of about 400 kilos. grey pig iron,150 kilos.spiegeleisen, 1500 kilos. steel scrap, and 25 to 50 kilos.wrought-iron scrap, from 20-43 kilos. spiegeleisen being addedtowards the end of the heating. A charge is worked off in from8-9 hours. The author has investigated the working of a chargeconsisting of spiegeleisen, English grey pig iron (Mnryport), andBessemer pig iron, which was produced at the Phoenix Works. Thepig iron used had the follmving composition :-CombinedGraphite. carbon. Mn. Si. P.Bessemer pig iron . . 3.09 0.97 2-55 1.59 0.116English pig iron . . , . 3.45 0.71 0.12 2-37 0.059Bessemer pig iron.. .. 0.249 0.018 91.417English pig iron .... trace trace 93.291After fusing this mixture, - some ends of Ressemer steel railswere added, and finally spiegeleisen. The steel when tested wasfound to fulfil the requirements of good Martin steel.It gave byanalysis-CU. 5. Fe.Mn. C. Si. P. S. Fe.0-304 0536 0.035 0.160 0.006 99.159The slag had the following composition :-SiO,. P20s, S. FeO. Al,03. MnO. CaO. MgO.50.18 0.02 0,014 25.75 2.61 20.44 0.62 0.17The aathor then describes a second process, in which the fumasewas worked too cold. The steel produced was too soft, and had t o bereworked with an additional quantity of spiegeleisen until the desireddegree of hardness was obtained.The following analysis gives the compauitiuu of the gas from thegenerator, tested in accordance wikh Stockmaan's method :--Pet. cent. Per cetlt.by volume. by weight.Nitrogen ................ 61.49 64-83Carbonic oxide ............23.24 24.50Carbonic anhydride. ....... 4.45 7-36Hydrocarbons ............ 2.07 1-24Hydrogen ................ 6.49 0.55Steam.. .................. 2-26 1.52The gas contained 13.61 per cent. (by weight) of lamp-black an100 ABSTRACTS OF CHEMICAL PAPERS.ash, and 0.9 per cent. tar. Since, in addition to the 15-61 per cent. ofsoot and ash, only aboxt 27 per cent. of calorific substances were con-tained in the gas, the decrease of the temperature in the furnace iseasily explained. D. B.Analysis of some Indian Bronzes and their Patina. Bg A.ARCHE and C. HASSACK (Biizgl. poZyt. J., 253, 514--519).-The inves-tigation which forms the subject of the present paper refers to twoIndo-Chinese ceremonial drums, placed at the disposal of the authorsby Count Hans Wilczek.One of these was recently bought for theNatural History Museum of Vienna, whilst the other belongs t o CountWilczek, and was shown at, the Bronze Exhibition in Austria in 1883.The first drum (marked A) is perfectly sound, but the second drum(marked B) has lost its pedestal, an3 has been repaired witch bronzeplates in one or two defectire places, otherwise both instruments aresimilar in form, size, and design. It was found that the pieces usedfor repairing the drum B did not belong to the missing pedestal, astheir composition differed considerably from that of the metal B.The authors therefore subjected this patchwork to a separate exami-nation, so that three Indian bronzes and their patina were analysed.Analysis of the three alloys :-Cu.Pb. Sn. Sb. As. Fe. CaO. SiO,.A . . . . . . . . 60.82 13-68 10.88 1.16' traces 0.91 0.38 1-13EL.. . . . . . '70.79 14-25 4.90 3.21 0.79 0.30 0.12 1.26Fatchrrork 68.i8 17-55 6.88' - - 0-85 traces 0.29S. C. HSO. 0.A.. , . . . .. .. 1.37 1.05 2-92 3.13 = 99.43Patchwork,. 1.49 0.70 1-89 0'66 = 99.09B.. . . , . . . . . 2.20 0.94 0.89 - = 99.65The patchwork had been fastened with iron rivets. Small pieces ofsolder were detected also. The iron rivets gave by analysis iron 97.43,carbon 2.20, and traces of sulphur and phosphorus. The solder wascomposed of-Cu. Pb. Sn. Zn. Fe. SiOP As, S,Co,Ni. H,O, C02, loss.66.70 3.78 0.55 23.97 0.82 0.12 traces 4.06Analysis of the patina :-CuO. PbO. SnO,. Fe20,+Al,0,. CaO. MgO. SiOPA , .. . . . . . 28.08 4.95 0.45 2.82 1.19 traces 45.29I3 . . . . . . . 11.00 0.59 0.05 1.11 0.31 traces 77.51Patchwork 26-11 12-96 10.52 4.46 5.66 0.27 15.24WaterSO3. COz. C. of hydration. Water.A , . .. .. .. traces 6.33 2.16 4.2 7 3 9 2 = 99.46B.. .. . . .. traces 1.60 0.75 1-90 3.18 = 98%0Patchwork 0.97 5.14 3.88 6.15 7.04 = 98.4TECHNICAL GHEMlYTRY. 101Patina A. The numbers obtained by analysis agree with theformula CuCOs,2Cu02H2 and 2PbCO3,PbO2H2 :-28-08 CuO require for CuCO3,2CuO2H, .... 535 GO2.4.95 PbO ,, 2PbC03,PbOJfj .... 0.65 ,,Total. ..... 6.00 .. Found .... 6.33 ..Patina €3 contain8 a copper cai-bonate poorer in carbonic anhydrideand the same lead carbonate as patina A :-11.00 CuO require for CuC03,3Cu02H, .... 1.53 CO,.0.59 PbO ..2PbC03,Pb02H, .... 0.03 ..Total. ..... 1-61 .. Found .... 1.60 ..The patina of the patchwork contains the same carbonates as B :--26.11 CuO require for CuCO3,3CuO2H2 .... 3-63 CO,.12.98 PbO .. 2PbCO,PbO2LE, .... l * i O ..Total. ..... 5-33 ,,Found .... 5.14 ,,By taking the essential constituents of each patina, ie., the stannichydroxide and basic carbonates, and calculating them on 100, thecomposition of the pure patina without admixture with foreignimpurities is obtained, thus :-Patina ofPatina 8. Patina B. patchwork.CuC03,2Cu0,H2. . 85.83 CUC~~,~CUO,H,. . 95.1 1 56-08BPbCO,,PbOZH,. . 13.01 2PbCO3,PbO,H,. 4.49 24.62Sn03H2 ........ 1.16 SnO,lla ........ 0.40 19.30I). B.Process for Bleaching Ozskerite. By C. 0.CHEXIN (Diqzgl.polyt. J., 253, 413-415). The object of this process is to preventthe darkening of ozokerite during bleaching. The author proposesto melt the material in water kept at a temperature of 70". Afterallowing the impurities to settle, the melted matter is decanted into aretort, treated with 5-15 per cent. flowers of sulphur, and distilledby tbe aid of superheated steam. The distillation, which is not frac-tional, gives m yellow crystalliue product. The action of the sulphuris partly mechanical and partly chemical. The product of the distil-lation may be treated in either of two ways (1) by subjecting cakes ofthe distillate to pressure, the plates of the press being a t a temperatureof 35" to 50', thus expressing the oils and hydroca>rbons melting atlow temperatures ; (2) by reducing the distillate to powder, and sub-jecting it to a spray of water at a temperature of 45" to GO", so as towash away the oils and readily fusible hydrocarbons.Instead of water,amyl alcohol or other solvent of hydrocarbon oils may be employed a tIl 102 ABSTRACTS OF CHEMICAL PAPERS.the ordinary temperature. The product obtained according to eitherof these modes of treatment is melted on a water-bath a t 35-70',and 20 per cent. amyl alcohol added. It is then mixed intimately,and cast into moulds. The resulting cakes after being subjected topressure are melted, digested for four hours in agitation with bone-black, and filtered through animal charcoal. On cooling, the product,amounting to 79-80 per cent.of the crude material treated, is white,hard, and sonorous. The residue resulting from the last treatment isdistilled so as to recover the solvents employed. It is then mixedwith the crude material to be subsequently treated. From 25 to40 per cent. of residue from treatment of petroleum or naphtha maybe mixed with the ozokerite, which is said to facilitate the working ofthis process. D. B.Dari as a Source of Alcohol. By J. HOLZAPFEL (Bied. Centr.,1884, 569-570).--Dari is the commercial name of the seeds ofSorghum nigrum, cafrorzim, and saccharaturn, containing on an average64 to 72 per cent. of starch. The author recommends the use of thisseed in brewing and distilling. Steamed under a pressure graduallyincreasing to 3 atmospheres, it yields a clear brown fluid mash.Usedin the proportion of 2351 grams to 52 kilos. malt, the results are highin spirit of good flavour, tasting better than maize spirit; at thepresent prices of dari and maize, there is also an economy in its use.Degeneration of Yeast. By J. C. JACOBSEN (Bied. Centr., 1884,638-640) .-Brewers' yeast deteriorates and grows wild if no change ismade ; the beer made loses quality and assumes an unpleasant taste.To prevent this, fresh yeast must be introduced from elsewhere, orelse cultivated by the manuf:wturers.By WIETERSHEIMand others (Bied. C'ent?.., 1884, 565--566).-When sugar-beets arestored they lose, between October and January, up to 1& per cent. inpolarisation, which it is calculated amounts to an annual loss of84 millions of marks on the beetroot production of Germany.It isfound that the loss is greater in proportion as the outside temperatureis high, and much more so when the temperature of the interior ofthe heap is high. A common mode of storing is in large pits, inwhich the roots are heaped up and covered with earth ; it is advisedthat they should not be stored underground, but on the ground, andlightly covered with peat fibre, damp being almost as injurious aswarmth. The loss of sugar is also influenced by the quality of thebeet, its mode of culture, manuring, and other causes.By E. V. LIPPMANNand others (Bied. Centr., 1884, 635-638) .-The composition of limesaccharate precipitatled by alcohol is C12H22011,Ca0 + 2H,O, the crys-talline water being lost at 100". If lime be added to the solution ofthe saccharate, the anhydrous dicalcium salt is precipitated ; and ifthe precipitation occurs at a high temperature, 2-3 mols.HzO arefound in combination. The tricalcium salt with 3Hz0 is produced ifJ. F.E. W. P.Loss of Sugar in Beetroots when Stored.J. F.Preparation of Sugar from MolassesTECHNICAL CHEXISTRY. 103well dried finely powdered lime is stirred up for a long time with thesaccharate ; this compound is soluble in 200 parts of cold water. Thetricalcium salt loses 2 mols. CnO when mixed with sugar solution,part of the lime being then precipitated ; the sugar crystals obtained byprecipitation of the lime by carbonic anhydride are somewhat differentin form from the normal crystals, being proportionally somewhatlonger, although the angles remain the same.Harperath’s patent con-sists in the employment of dolomite in place of strontium, &c. ; whenthe burnt mineral is introduced into the sugar solution, monocalciumand magnesium saccharates are first formed, also some soluble “ bisac-charate,” the i.mpurities are thus carried down by the lime andmagnesia, and a further addition of the ignited dolomite results inthe formation of insoluble tricalcium and magnesium saccharates ; thetricalcium and magnesium saccharate is absolutely insoluble in water,thus a gain over the calcium salt is obtained, which latter salt is thesource of loss in sugar to the extent of 6 per cent. Moreover a hightemperature is unnecessary, neither does the compound spontaneouslydecompose so readily as the pure calcium saccharate ; the composi-tion is said to be X[=~’?H,,O~~(C~O)~,(H,C))~ + yCl,H,,Oll(MgO),H,O,.Boivin’s and Loiseau’s patent for the separation of grape-sugar con-sists of the following processes : 700 grams of slaked lime is mixedwith 1 kilo.molasses which has previously been diluted to 12-15”BaumC! ; this mixture is cooled, saturated with carbonic anhydride,and the resulting mass is then pressed through a perforated cylinderinto threads 3-5 mm. thick ; afterwards the impurities are removedby stirring up with lime-water, and the washed calcium compoundis then decomposed by carbonic anhydride, the carbonate removed,and the sugar solut,ion evaporated.Scholvien publishes a patent tr,modify the osmotic process; by this method the molasses is to beheated to looo, and the sugar precipitated as the tricalcium corn-pound ; the filtrate, heated to 60°, is then submitted to osmosis.E. W. P.Purification of Molasses. By J. GANS (Bied. Centr., 1884, 645).-Gans has patented a process in which he employs aluminium hydr-oxide and dialyses at 60” ; to prevent the gelatinous separation of thealumina, a small quantity (0.001 per cent.) of tartaric acid is added.E. w. P.Extracting Sugar from Molasses. (DingZ. poZt~t. J., 253, 421-426 and 519--529.)-In extracting the sugar from molasses and syrups,according t o Scheibler’s strontia process, the formation of stroutixmbisnccharate may be prevented by introducing fresh quantities ofmolasses and strontium hydroxide into the mother-liquor resultingfrom the filtration of t h e monosaccharate originally produced.Thistreatment is repeated several times until the consistency of themother-liquor renders the process impracticable in consequence ofthe accumulation of non-saccharine matter. After repeating thisoperation 6 or 8 times, the residue contained only 3 per cent. of thesugar present in the molasses when attacked.Dureas gives a description of the ammonium chloride osmose pro-cess, as worked at the Haussy sugar refinery in France. The syrupobtained from product I is treated with about 1 per cent. ammoniu106 ABSTRACTS OF OHEMICAL PAPERS.ehloride, and heated to boiling. It is then run into collecting tanks,heated to loo", and purified by osmose with 10 to 12 parts of waterat 70-75".The resulting syrup is added to fresh juice.According to Stutzer, the recovery of sugar from molasses by theprecipitation process depends on the separation of calcium sacchamtefrom an alcoholic solutioa of molasses. It has been ascertained byexperiment that the precipitation of the sugar is best effected in analcoholic solution of molasses by previously slaking the lime withalcohol. The separation of calcium saccharate by the addition ofground lime to an alcoholic solution of molasses is not only slow butalso uncertain, a circumstance which proves that calcium hydroxidecombines more readily with sugar than the oxide, especially in alka-line saccharine solution (molasses).Barium and strontium hydrox-ides behave in a similar manner.Referring to Steffen's defecation process, the following methodshave been patented by the Brunswick Engineering Works :-Onmixing an aqueous solution of sugar with a compound of calciumfiaccharate containing more lime than the quantity required to formmonosaccharate, in such proportions that the total amount of sugarpresent in the mixture contains more than 15 parts calcium oxide to100 parts sugar in the solution, i t is possible to separate the sugar bytreating the solution with lime a t a temperature not exceeding 25"'the resulting compound of calcium saccharate being sparingly solublein water at that temperature. On adding to a solution of calciumsaccharate, a t a temperature not exceeding 35", a compound of calciumsaccharate of a higher degree of saturation than the quantity of limenecessary to form the monobasic salt, almost the whole of the sugarcontained in the mixture is separated in the form of a calcium sac-charate compound, insoluble in water at a temperature below 35".Biirthlein has worked the defecation process a,t the Sarstedt SugarRefinery with molasses of different composition, and obtained satisfac-tory results even with Indian molasses.He found that a solutioncontaining 7 per cent. sugar gave the best yield.Frost has recovered the sugar from 300 tons molasses according tothe defecation process. This quantity was worked up in four weekswith a yield of 52-52.5 per cent.of filling substance.Scholvien recommends the purification of calcium saccharate solu-tion by osmosis. For this purpoae the hot solution of molasses istreated with lime so that 1 mol. sugar equals 3 mols. lime. Themixture is then filtered, and the filtrate purified by osmosis at 60" andadded to freah juice.Hiittgen iises two osmose apparatus. He places one apparatus35 cm. above the other. The liquor from the former passes throughheating apparatus interposed between both apparatus, and isbrought to a temperature of 97" before it is purified by passingthrough the second osmose apparatus. It is said that a saving in fuelis effected, as only half the usual quantity of wash-water has to beevaporated. D. B.By H. ENDEMANN(Bied. Centy., 1884, 568-569) .-Endemann employs phosphoric in-Formation of Grape-sugar from StarchTECHNICAL CHEMISTRY. 105stead of sulphuric acid in the process of inversion.1000 kilos. air-dried starch, 2000 kilos. water, and 50 kilos. of phosphoric acid afreheated in a closed vessel at 140" ; the addition of a small quantity ofnitric acid assists the reaction. The acid is removed by addition of ah s e forming insoluble combinations, preferably lime ; the presenceof gypsum in the glucose is thereby avoided. J. F.Preparation of Concentrated Acetic Acid. By T. G ~ R ~ N G(Diwgl. poZyt. J., 254, 90--01j.-The author proposes to treat solu-tions of acetic acid with ethyl ether, ethyl acetate, amjl alcohol, orother similar liquid, insoluble or only slightly soluble in water ; saltsmay or may not be added at the same time.By systematic treatment,tthe whole of the acetic acid is concentrated in the liquid so added.The extract may be treated with a suitable base, as lime, by whichacetate is formed, and the extracting medium is ready for application:\fresh. If concentrated acetic acid be required, an ether of lowboiling point is employed, which is separated from the extracted acidby distillation. For very concentrated acid, the extract is firsttreated with Borne substance capable of removing the small quantityof water taken up, such as magnesium or calcium chloride, $c. Ifpure acid is required, the extract is subjected to an inverse process,the acid is washed out with water in a second apparatus, whilst theextracting medium retains certain impurities taken up along with theacetic acid.J. T.C. Thiel's Pasteurising Apparatus for Milk. By W. FLEISCH-MANN ( B i e d . Centr., 1884, 632-633) .-T hiel's apparatus consists of ahollow double-walled cylinder, the division between the two wallsbeing filled with water at 74-80" ; the inner division is covered by aperforated lid which admits of the milk flowing in streams down theoutside of the inner and heated wall ; from there the milk passes to aLaurence's refrigerator. Milk may thus be heated from 6" to 25-60'to the amount of 750 kilos. per hour. E. W. P.Bitter Milk. By LIEBSCHER ( B i d Centr., 1884, 561--562).-1na well-managed farm in Thiiringia, the butter which had hithertofound a ready sale became repulsively bitter, and consequently uu-saleable ; this led to strict examination, and it was eventually foundthat a number of the cows in the earliest portion of their milkingyielded a bitter milk, and that when this was taken in a separatevessel the remainder was sweet.It was therefore suspected that the stalls had in some mannerbecome infected with bacteria, which had commenced their progressinto the udders of the cows without having made much advance.Both stalls and cattle were thoroughly disinfected.Carbolic acid wassprinkled about frequently, and the cow's udders washed twice dailywith lukewarm water and then with dilute carbolic acid ; in three daysthe bitterness had disappeared, and the milk and butter tasted sweet.Quality of Butter made by different Processes.By &I.SCHRODT ( B i d Centr., 1584, 562-565).-1t has been said that butterJ. 3'106 ABSTRACTS OF CHEMICAL PAPERS.made by the centrifugal process is deficient in keeping properties, andnot of so good quality as hand-made butter; the aut,hor thereforecollected numerous samples of both descriptions from different locali-ties, and submitted them to the judgment of experts who classifiedthem into seven classes; the resnlts are tabulated, and show thatall processes when carefully conducted give equally good butters, andthat the centrifugal method can produce butters which are quiteas good as hand made, both in respect of their quality and keepingproperties. J. F.Preparation of Quinaldine. (Dingl.pdyt. J., 254, 91-92.)-According to the Actierzgesellschaft fiir Anilinfabrikation of Berlin, if3 mols. of aldehyde be allowed t o act on an aqueous or alcoholicsolution of 2 mols. aniline hydrochloride at the ordinary temperature,there is produced not the salt of the liquid quinaldine, CloH9N, butthe salt of a new fixed base, C18H20N2. The mixture must be keptcool with ice, and the reaction requires two or three days for its com-pletion. By evaporation, the hydrochloride of the new base is ob-tained as a brownish-red mass easily soluble in water. Alkalis pre-cipihate the base from a solution of the salt, in white flakes which,when dried, form a white amorphous powder insoluble in water, onlydightly soluble in boiling alcohol, but easily ih hot benzene or amylalcohol.On heating the hydrochloride of this base alone or in pre-sence of metallic chlorides, e.g., ferric chloride, quinaldine hydrochlo-ride is produced. By fusing it with zinc chloride, the double chlorideof zinc and quinaldine is produced. Instead of ordinary aldehyde,corresponding quantities of paraldehyde, aldol, or acetal can be em-ployed, and other aniline salts in place of aniline hydrochloride. Bp the action of aldehyde, &c., on the salts of other primary aromaticbases, such as orthotoluidine or naphthylamine, compounds are ob-tained analogous to the base CleHzoN2, and similarly convertible intoquinaldine. J. T.Dyeing with Alizarin Colours on Indigo-blue Cloth. (DinqZ.polyt. J., 253, 474.)-According to Delory of Rouen, calico dyedwith indigo is mordanted with aluminium acetate or sodium aluminate,and dyed with alizarin in the presence of Turkey-red oil.A smallamount of alizarin suffices to produce the desired effect of impartingto the blue a slight purple cast, and adding considerably to thestrength of the colour and its power to withstand the action of alkalis.The mordant used for darker blues is iron acetate or a mixture of thelatter with aluminium acetate. The alizarin employed is always ofthe purest blue shade.By A. SCHEUHER (Dirtgl. polyt. J.,253, %97-299).-1n September, 1875, Schaeffer drew the attentionof the Conzite' de Chemie t o an observation made by Strobel, that onexposing goods dyed red with alizarin to the fumes of nitrous anhy-d r d e an orange colour was obtained, which is not attacked by soapsolution. Rosenstiehl recognised this new chemical compound asmononitroalizarin, and its mannfactnre on a large scale was soonD.B.History of Alizarin-blueTECHNICAL CHEMISTRY. 1Q7commenced. Two years later he was engaged in the formation of anew dye, viz., alizarin-blue.On the 27th June, 1871, Prudhomme, in a communication laidbefore the Socie'tk Ihdustrielle de Mzclhouse, described the simul-taneous discovery of two colouring-matters, a blue and a brown dye,obtained by heating mononitroalizarin (alizvrin-orange) with glyceroland sulphuric acid. These colours were prepared on a large scalewithin a few months of their discovery.Brunk, of the BadidLen Aniliiz Fabrik, recognised the brown dyeas amidoaliza.rin, formed as a bye-product of the reaction. He isolatedtjhe blue colouring matter and studied its properties.In December,1877, the Baden Aniline Works brought this colour into commercein the form of a 10 per cent. paste. Its insolubility in water andacetic acid, however, prevented it from being used extensively.Dollfus proposed to dye alizarin-blue on cloth mordanted withnickel, the result being the production of permanent and brightshades. Kochlin and Prudhomme recommended to fix the blue oncotton with chromium acetate. The colour was found to resist theaction of chlorine and similar substances, but assumed a grey tingeon exposure to the light. Brunk then made a further improvemenbby bringing the blue into the market in a soluble form.For thispurpose alizarin-blue is treated with hydrogen sodium sulphite. Theresulting compound is soluble in water, and is fixed with chromiumacetate, a pure blue colour being obtained, which is said to resist theinfluence of light even better than indigo.Graebe assigned to alizarin-blue the formula C1,H9N04, and itmust therefore be regarded as the quinoline of alizarin. The bluemarked S, sold by the Radischen Fabrik, contains 2 mols. hydrogensodium sulphite to 1 mol. alizarin-blue, thus : C1,H,NO4,2NaHSO3.D. B.Preparation of Persulphocyanogen by Electrolysis. By F.GOPPELSROEDER (Dingl. poZyt. J., 254, 83).-On passing a galvaniccurrent through an aqueous soluiion of potassium thiocyanate, ayellow amorphous body appears a t the positive electrode, whichbehaves exactly like persulphocynnogen.I n the cold there isscarcely any reaction, but on heating the conversion is rapidlyeffected, and the orange-yellow flocculent precipitate merely requiresto be collect'ed and washed with cold water. The liquid at thepositive electrode is strongly acid, and a t the negative one stronglyalkaliue. Much gas is evolved a t tlhe negative electrode, the natureof which has not yet been investigated. The author will also furtherinvestigate the yellow product, which so far appears to be the dye men-tioned by Schutzenberger in his work Traite' de Chemie ge'ndral, ii, 620.Schutzenberger gives the probable formula afi C3N3HS,. The authorhas also produced the dye and fixed it on vegetable and animal fibresby the same process.The author cites Prochoroff's method of produc-ing the yellow dye kanarim, and ascribes the application of it to calico-printing to H. Schmidt. In an appendix, the author acknowledgesthat A. Lidow formed the same compound from ammonium thio-cyanate by electrolysis. J. T108 ABSTRACTS OF CHEMICAL PAPERS.Prepsration of a Dye-stuff from Cotton-seed Oil. By J.LORGSIORE: (DingZ. polyt. J., 253, 535).--The author proposes to meltthe precipitate thrown down in the refining of cotton-seed oil, andsaponify it with pulverised caustic soda or a solution of soda. Thesolut,ion which contains the colouring matter of cotton-seed oil isallowed to settle, and the resulting soap dissolved in water and saltedout with canstic soda or soda-lev.This treatment is rmeated severaltimes until the soap has attaimd at sufficient degree of ;urity.D. B.Manufacture of Santonin in Turkestan. By C. 0. CECH(DingZ. poZyt. J., 253, 474--476).-The author mentions that inTschemkeut, a town in the province of Syr-Daria, in Turkestan, itlarge factory is in course of erection, for the purpose of extractingsantonin from worm-seed (Artenaisia satonica and maritima). Thisplant is cnltivated in some parts of South America, and in the valleyof the River Arissi, in the Tschemkeut district. It contains from1% to 2.3 per cent. of santonin, and is called “Darmena” by thenatives. About 1600 tons of seeds are collected annually by theKirghiz-Kazaks during the month of August, and sent on caravansinto the interior of Russia, whence the product is forwarded toMoscow. In medicine, worm-seed is either employed per se, or istreated by chemical means, to extract the santonin therefrom, whichis used as a remedy for ascarides. Santonin is considered a valuablepreparation, 1 kilo. being sold at from 40 to 60 shillings. D. B.‘(Red Spots” in Light Rose Dye. By E. LAUBER (Din$.poZyt. J., 254, 41-42).-The author finds that these “ rcd spots ’’cannot be prevented, however finely the alizarin may be powdered,neither are they prevented if the thickeniiig paste is stirred into thealizarin paste, as recommended by the Badischen Aniline und Sodafirm. He finds the cause of this defect to be the employment of anunnecessary excess of mordant. The measured amount of mordantshould be first mixed with a small amount of thickening, to this therest of the thickening is then added by degrees, and finally thealizarin. J. T.Bleaching Indigo-blue and Turkey-red by ElectrochemicalMeans. By P. GOPPELSROEDER (DingZ. poZyt. J., 253,430) .-Scheurerhas recently laid before the Gomite’ de Chimie of the Xociete’ Industri-eZZe de Jfdhoztse, an interesting communication on the bleaching ofindigo and Turkey-red by the aid of gaseous chlorine. He showedthat on printing a thickened solution of caustic alkali on cerlainparts of indigo-blue or Turkey-red cloth, the printed places could bebleached with chlorine gas very readily. The author therefore madea series of hials, the object being to ascertain whether this processcould be applied to the bleaching of indigo or Turkey-red by elec-trolysis. He found that on saturating indigo-blue or Turkey-redcloth wibh a solution of potassium nitrate or sodium chloride, pre-viously treated with caustic alkali, and placing the cloth betweenplatinum plates, forming bhe two elecbrodes, it was possible to destroyboth colours. D. B

ISSN:0368-1769    

DOI:10.1039/CA8854800097

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

109General and Physical Chemistry,Refractive Indices of Crystallised Alums. By C. SORET(Compt. rend., 99, 867,-869).-By means of the instrument pre-viously described (Compt. rend., 95), the author has determined therefractive indices OE many alums for the lines a, B, C, D, E, b, I?, G,of the solar spectrum. He has also determined the specific gravitiesof the alums by means of the hydrostatic balance. In the followingtable, only the refractive indices for 13 and the specific gravities aregiven :-?D. Sp. gr.Ammonium aluminium alum.. . . 1.45939 1.631Sodium 9 ,Methylamine ,,Pohssium 9 1Rubidium 9,CEsium 9 ,Thallium 9 7Ammonium indium,, galliumPotassium ,,Ammonium chromiumPotassium 9 9Rubidium Y 9Thallium 3,Ammonium ironPotassium ,,Rubidium ,,CEsium ,,Thallium ,,,, ....7 ' * * ..9 9 *...,, ....,, ....,, ....,, ....,, ....,, ....,, ....,, ....,, ....,) ....,, ....,, ....,, ....,, ....,, ....3.438841.454101.456451.456601.458561.497481.466361.465581 *464991-484181.48 13 71.481511.484821-481691.482391.483781.523651.522801.6671.S681.7351.85219112.2572.0111.7451-7191.81 71.9462.2361.7131.8061.9162.0612.385-The molecular volume is not constant for the different terms of thesame series, but it seems to vary in a definite manner for the corre-sponding terms of the aluminium, chromium, and iron series.In passing from one alum to another, the variation in the refractiveindex is sensibly the same in the three series, thus following a lamwhich has been observed in other series of compounds.It is worthyof note, however, that the refractive index of sodium alum is muchless tbau that of potassium alum, whilst in the case of the chloridesthe sodium salt is intermediate between the potassium and ammoniumcompounds.The author's value for the refractive index of thallium alum ismuch higher than that obtained by Fock.Methylamine alum is intermediate between the sodium and potas-sium compounds, and it would seem as if, in the aluminium series, therefractive index varied continuously with the molecular weight of thealkaline radicle. C. H. B.VOL. xr,vm. 110 ABSTRACTS OF CHEMICAL PAPERS.Inversion of the Electromotive Force of a Copper IronJunction at a High Temperature.By F. F. LE ROUX (Compt.rend., 99, 842-84A).-A bar of iron was bent in the form of a horsn-shoe, and attached a t each end to a copper bar. This couple wasplaced in a furnace and heated nearly to the melting point of copper,a current of about 330 amphres being passed through the couple. Anychange in the temperature of the junction was detected by observinga change in the relative luminosity of the junction, the results ofocular observation being confirmed by the action of the radiation on agehtino-bromide plate.It was found that a t about 1000” a current passing from the copperto the iron raises the temperature of the junction, whilst at the ordi-nary temperature a current in the same direction cools the junction.C.H. B.Electrolysis of Silver Fluoride, Chlorate, and Perchlorate.By G. GORE (Chem. News, 50, 150).-A moderately strong solutionof silver fluoride acidified with hydrochloric acid is a very good con-ductor of electricity, and is very readily decomposed by means of silvereltctrodes and a current from a cell containing zinc and platinum indilute sulphuric acid. Crystals of silver are rapidly deposited a t thecathode, Fhilst the anode soon becomes rough, grey i n coiour, andvery friable. In special experiments, no evidence could be obtainedto show that this loss of cohesion was due to the diffusion of liberatedfluorine through the silver.When a solution of silver chlorate is electroljsed by sheet silverelectrodes and a current from two Smee’s cells charged with verydilute sulphuric acid (1 vol.of acid to 50of water), conduction is good,and silver is freely deposited only at first; the deposit being loose,and not very white. The anode also is soon coated with a black film,presumably silver peroxide, which seems to stop the current ; it ispermanently blackened, although but slowly corroded. With oneSmee’s cell, the deposit is formed slowly, and is more coherent,, Thissolution requires a feeble current, a large cathode, and a much largeranode.When silver perchlorate is similidy electrolysed, conduction is verygood, and loose, bulky, silky crystals of silver are soon deposited a t thecathode, whilst the anode quickly becornes black, the current a t thesame time becoming much diminished. With one cell and a moredilute solution, conduction is free, the deposit is smaller, and the anodebecornes less dark.A silver wire anode soon becomes corroded andloosely coated with a black substance ; this falls off and is ultimatelyreplaced by a thick green coating ; no gas is evolved. The solutionrequires a large cathode and a rather small anode. D. A. L.Electro-deposition of Carbon and Silicon. By G. GORE (Ckenz.Xews, 50, 113--114).--Carbon, silicon, and boron have each beendeposited during the eleccrolysis of certain fused mixtures.C‘irrbon is dfyosl’ted when a current from 10 Bmee’s elements ispaswd through a fused mixture of 200 grains of sodium hydroxide,170 grains precipitated silica, and 610 grains of mixed anhydroussodium and potassium carbonates, the anode being sheet platinumGENERAL ASD PHYSICAL GHEMISTRY. 111tlhe cathode a wire of the same metal; the deposition of carbon is,however, probably due to a secondary reaction of this character:silicon i s first deposited and &is reacts with the alkaline carbonates,and causes the separation of carbon.The same phenomenon occurswhen a mixture of 475.2 grains of 97.1 per cent. sodium carbonate and217.4 grains sodium borofluoride is similarly treated, and apparentlyalso in the electrolysis of aqueous or alcoholic oxalic acid. The de-posited carbon is not crystalline.Carbon is not deposited either during the electrolysis of sodium andpotassium carbonates, using eight Smee's cells and platinum electrodesa t a red heat, or when boric acid is included in the mixture, or bythe electrolysis of any of the following : potassium cyanide, oxalic acidin solution in hydrochloric or nitric: acid, sodium formate or formicacid, carbonic oxide and anhydride, pyrogallol, liquid hydrocynnicacid saturated with carbonic oxide, fuming sulphuric or syiwpyphosphoric acids saturated with dry carbonic anhydride ; or fromdilute sulphnric acid over which coal-gas was passing during the14 days the electrolysis was continued.Carbon tetrachloride does notyield carbon undcr t h e influence of an electric current. These experi-ments were conducted under different conditions a8 t o strength ofcurrent, length of time, temperature, and composition of electrodes.Xilicon is deposited when a fused mixture of 300 grains of 97.1 percent.potassium carbonate and 442 grains of potassium silicoflnorideis electrolysed, as described above i n the carbon-deposition experi-meats. D. A. L.Relation between the Ordinary Thermometer and the WeightThermometer. By E. BARBIER (Compt. rend., 99, 752-753).-Ademonstration of the theorem that if the ordinary thermometer andthe weight thermometer agree at the two fixed points, they agree atall temperatures. C. H. B.Attraction of Homogeneous Molecules. By C. SCHALL (BPI-.,17, 2555--?577).-In order to interpret experiments on the rela-tion between the rates of evaporation of liquids and their molecularweights and heats of expansion, the author has more particularlystudied the phenomena of cohesion and adhesion of liquids, a subjectof interest to the chemist as dealing witoh the attraction of homo-geneous and heterogeneous molecules.The method of investigationwas based on that of the so-called adhesion plates, which consists, inoutline, in suspending a plate of glass from one pan of a balance, andcounterpoising i t ; the plate being adjusted to a level, a dish contain-ing the liquid to be examined is placed under it, and then raised untilthe surfaces of the liquid and glass are in contact. To the oppositepan of the balance, weights are added until the glass is severed fromtlie liquid ; this excess of weight is then toted. The apparatus used,toget'her with devices for levelling the plate and for the complete sever-ance of the liquid and glass, are described in detail in the paper, Asthe attractive force between two contingent molecules within a liquidis proportional to their mass and inversely proportional to the squareoE the distance between them, and as increase of distance is correla-tive with decrease of specific gravity and also with that of cohesion, i 112 ABSTRACTS OF CHEMICAL PAPERS.it follows that a decrease of the latter caused by warming the liquidis proportional to tihe square of the former. But the superficial expan-sion, which is equal to the $j power of the cubical, is inversely propor-tional to the specific gravity.As the superficial expansion increases,the number as also the mass of molecules under the plate and theircorrelative cohesion diminishes, and therefore the latter diminishes indirect proportion to the Hence if sand s1 be the specific gravities for any two degrees of temperature, Gand G' the excess of weight necessary for the disruption of the plate,thenpower of the specific gravity.Experimental results are tabulated which demonstrate the validityof the formula, and of the law deduced therefrom, that the force bywhich homogeneous molecules are attracted varies in direct proportionto the square of the specific gravity, and also to the mass of the mole-cules.From the experimental results can be deduced the diminutionof cohesion for each degree of temperature, and thus the critical pointat which the cohesion is nil.Rut the results obtained with some of the liquids examined, espe-cially water, benzene, and its derivatives, are not in strict accordancewith the law enunciated above, so that it would appear that theforce of cohesion is dependent to some extent on the chemical consti-tuttion of the liquid.I n the case of t w o liquids, it is further de-monstrated that the relation between the respective cohesions and alsotheir specific gravities at boiling points within restricted limits ofpressure are approximately identical.These experiments are also of importance in regard to the pheno-menon of capillary attraction, a force which depends on the differ-ence between the force of cohesion of the molecules of the liquidwith one another, and of adhesion to the molecules of the glass.If the force of attraction as represented by the capillary height = h,that of the adhesion of the liquid to the glass = a, and of the cohe-sion of the liquid = c, then-1~ = a - c.The form of the meniscus is concave if a > c.but convex if a < c.B u t from the above formula, = (i)2(:)', then if the capillaryheights are h and h' at two different temperatures, then h = a-c,a-c I1 and h' = a'-c', it follows that h' = ~- , or 72' =Experimental results are also adduced in support of these formule,although water and liquid sulphur offer instances of marked exception ;it is thus probable that the molecular constitution of these liquids isthe cause of the discrepancy.Relation between Molecular Weight and Velocity of Evapo-ration of Liquids.By C. SCHALL (Bey., 17, 2199--2212).-ThisV. H. VGENERAL AND PHYSICAL CHEMISTRY. 113paper contains a description of the apparatus nnd method of workingemploged by the author in his experiments with benzene, carbonbisulphide, and water (Abstr., 1884, 551).Experiments with substances of nearly coincident molecular weightand boiling point :-Calculated.Phenol ................ wb = 94Aniline ................ rn = 93Toluene ................ m = 92Valeraldehyde .......... m = 86AIonochl(lrobenzene ...... m = 112.5Acetic anhydride m = 102Benzoic chloride ........ nz = 140.5Ethyl benzoate 112 = 150{{ ..................Found.95.57, 95.11, 95.1191.48, 91.91, 91.9193.8584.3108.2106144-:3, 144.5145.7, 145.2Experiments with substances of nearly equal molecular weights,but of different boiling points :-Calculated. Found.Ethyl acetate............. m = 88 86.32, 87.76Amyl alcohol(fermentation) m = 88 89.71, 87.76Benzddehyde .......... m = 106 104.7, 110Acetic anhydride ........ m = 102 103.3, 98.27{{{{{{{{ Amyl alcohol (fermentation) nz = 88Experiments with substances of unequal molecular weights, but ofnearly coincident boiling points :-Calculated. Found.Acetic chlori~le .......... m = Z3.5 78.06Acetone ................ WL = 58 58.33Alcohol ................ m = 46Benzene nz = 78 87.12, 87-12Toliiene ................ m = 92 94.28Phosphorus oxychloride . . m = 153.5 149-841.2, 41.2 ................Substances with different boiling points and different molecularweights :-Calculated.Found.Benzene ................ m = 78 75..5, 75.5Toluene ................ m = 92 95.04, 95.04Methyl alcohol’ .......... rn = 32 30.66Propyl alcohol nz = 60 62.63Ethyl alcohol.. .......... m = 46 45.48Isobutyl dcohol. N L = 74 74 84Isobutyl alcohol ......... m = 74 65.6599,19...................Recent determinations of heats of vaporisation show thst these areproportional to the time of vaporisation. I n the followiug table, t isthe boiling point a t which the heat of vaporisation L was determined,DL the product of the latter niultiplied by the theoreiical density, 112the calculated, and nz’ the found molecular weight :11 4 ABSTRACTS OF CHEMICAL PAPERS.---Water.. . .. . . . .. . .Wood spirit . . . . . , .Ethjl alcohol.. . . . .Amy1 alcohol . . . . , .litliyl acetate.. . . . .Metlijl butyrate.. . .Oil of lemon . . . . . .0 1 1 of turpentine.. .Hutjric acid . . . . . .Ethjl valerate . . . . .t.100"66 -5"7.81317493165156164113 *5L.---538 -0 cal.261 -7 ,)206 *4 ),120 -0 ,,105 .o ,,86.0 ,,69.5 ),68-5 ) )114 0 ,,68.4 ,,DL.--331 3'290.1328 ' 8368 *7320 *O31 13 .8327 * 4322.7347 -5308 .Om.---3246888810213613688130m'.---36.646 -489 .o91 - 2111.2138 *3139.884 -0140 -0The author has further compared the velocity of evaporation ofacetic acid with that of toluene, amyl alcohol, and isobutyl alcohol,and the results obtained show that the molecular weight of aceticacid a t its boiling point is 89.8 This may also be calculated fromF'avre and Sil bermann's determinations of its heat of vaporisation,arid likewise for formic acid, the molecular weight 69.A.K. M.On Crystallisation. Observations and Conclusions. By G.Stability of Compounds. By W. ALEXBEFF (Jour. XUSS. Chem.SOC., 16, 641-642) .-The author communicates his researches as tothe conditions determining the stability of a compound ill the presenceof an excess of one or the other of its constituents. The results agreewith what he found with regard to the stability of hydrates of alco-hols in their aqueous and alcoholic solutions. The difl'erence in thestability of hydrates determines the difference of the vapour-tensions,at one and the same temperature, for two solutions, which areformed by water, and a liquid capable of yielding a hydrate.More-over, in an aqueous solution, this tension is always smaller when thejormula of the hydrate is A + nH,O, n being generally greater thanunity. With solutions formed by water and ether, a difference intemperature of 8" corresponds with equal tensions.Phenomena af Condensation. By D. MENDEL~EFF (Jour. Russ.Clwm. rSoc., 16, 643--644).--The author remarks that the phenomenaof condensation, as shown in the case of the formation of solutions or ondiluting some liquids, is analogous to what takes place when sphericalbodies of different diameters, sach as samples of differentl seeds (peaseand millet), are niixeci together.When spherical bodies are mixed, ASmay be shown b-y experiment or by geometrical analysib, the weightof a measure containing a large numberof such small spheres of bothkinds is greater than the mean calculated from the weight of bothkinds taken alone. I n the same manner, the sp. gr. of a solution isgreater than it should be, when calculated from the sp. gr. and theynantity of the constituent liquids. The analogy in the change ofvolumes which takes place in both the above cases shows that when aI~R~GELMAKN (Ber., 17, 235942372).B. BQEKERAL AND PHYSICAL CHE3fISTRT. 115small bulk of light spheres of small diameter is added to heavierspheres of large diameter, the sp. gr. of a cubic: measure of the lastmay become greater, exactly as the firsf addition of water to normalsulphuric acid raises its sp.gr. The above geometric question is,unfortunately, up to the present inaccessible for full geometricanalysis, and the experimental investigation is rendered very di ficultby the impossibility of obtaining the neeessary balls of regular sizeand equal diameters.Experiments with mixtures of millet, and gunpowder, however, haveconvinced the author t h a t the above phenomenon exists, but it is onlya statical representation of a dynamical phenomenon which takes placein the case of dissolution as a simple act of chemical association ofheterogeneous particles. B. B.Connection between Pseudo-solution and True Solution.By ITT. W. J. NICOL (Chem. News, 50, 124).-Arguing from themolecular theory of solution, according to which the dissolution of asalt in water is the result of the attraction of the water molecules fora single salt molecule exceeding that of the attraction of the saltniolecules for one another, the author demonstrates that the differencebetween .pseudo-solution and true solution lies only in the degree ofsubdivision of tlie solid.For by this theory dissolution dependsgreatly upon cohesion, and where cohesion is small dissolution is easy,and vice we?-& ; taking barium sulphate as an example, the cohesionis great, the solubility almost nil ; if, however, the cohesion is dimin-ished by any means, then tlie finely-divided salt will remain suspendedin water for a long time, that is, in a state of pseudo-solution, whichshows that the water molecules alone were not able to overcome thecohesion, but this being to a certain extent overcome, pseudo-soh~tionis the result.Supposing now the insoluble salt could be resolvedinto its molecules, t h a t is, further subdivided, then it is easy tfo con-ceive that it would be possible to dissolve it to a great extent in water,and produce a trite soZuticJw, from which the solid would separatebut slowly, owing to the solid molecules seldom comiug in contact insuiiicient numbers for their niutual attraction to overcome that of thewater for them. As examples of such cases, the author refers to thefact that many almost insoluble compounds are precipitated withextreme slowness from cold dilute solutions.D. A. L,Rise of Solutions in Capillary Tubes. By M. GOLDSTEIN andA. DAMSKI (Juuy. Buss. Chew. Soc., 16, 642-643).-According toValson, the rise of a large number of solutions of salts in capillarytubes is inversely proportional to their specific gravities. Thiserroneous conclusion is explained by the fact that Valson workedwith solutions showing no great diffei-ences in sp. gr. and, therefore,in the rise. Very different results are obtained on using solutions ofgreat concentration (2 or 3 gram-mols. of salt to 1 litre of water) andnarrower tubes ; here the specific gravities and rise in the tubes differconspicuously from those of pure water, and the regularity, shown byValson, does not existi, e.g. :116 ABSTRACTS OF CEEMlCAL PAPERS.Height of rise.h.118.2117.49 ) # 9 7 ,, ..117-3,, . . 116.4 :: f :: ,, . . 11.5.3,, 2 9 , ,, . 114.17 2 3 9 , ,, . . 112.4Pure water. . . . . . . . . . .KCl $ mol. wt. to 1 litre-Sp. gr.d.1.0001.0091.0161.0251-0481.1001-155h . d.118.2118.4119.1119.31120.8125.5199.8The value h . d equals that for water only for very dilute solutions.The determinations of the above values for pot,assium chloride,bromide, and iodide have shown that the rise of solutions of potassiumbromide of different degrees of conceiitration is the mean of the riseof corresponding soh tions of potassium iodide and chloride, themolecular weight of KBr being t,he mean between those of KC1 andKI :-Height of rise.KC1.KI. KBr.w-calc. fromSolutions. a. 6. cc+b = c*2 2 mol. in 1 litre.. 117.4 - -9 , .. 117.3 114.5 115.57 9 . . 116.4 113.0 114.797 , . 115.3 108.5 111-92 7, .. 114.1 100.2 107.13 ?, .. 112.4 93-5 lu2-917 -foullaC.115-911 5.2114.6111.310 7.1102.8B. B.Capillary Phenomena in Relation to Constitution andMolecular Weight. By J. TRAUBE (Bw., 17, 2294-2316).-Allthe experiments described in this paper were made with aqueous solu-tions of organic substances : the advantages of the use of such solu-tions over organic liquid compounds, being the much greater heightat which the former stand in capillary tubes, and the much greaterdifferences in capillary height shown in the case of closely relatedsubstances. Voluminous tables are given, a t once showing the dif-ference in capillary height caused by difference in the concentration ofsolutions of the same substance, and comparing the capillary heightsof unlike substances in solutioris of the same degree of concen-tration. The following are amongst the more important conclusionsdrawn from these experiments :-1.The capillary height of the solu-tion of an orgariic body decreases with increasing concentration.Equnl differences of height are not, however, caused by equal incre-ments of concentration, the rate of difference first attaining a maxi-mum, and then diminishing. 2. I n a homologous series, the capillaryheivht diminishes with increasing molecular weight. The differencereaches its maximum sooner in more concentrated than in moredilute solutions.8. Isomeric Substances, although of related consti-tutions, have not necessarily equal capillary heights. With regardto the capillary relatlions of different organic series, the author giveGENERAL AND PHYSICAL CHEXISTRT. 117the following as the result of his observations:-An increase incapillary height is observed in passing, 1, from the fatty alcohols tothe correspoiiding aldehydes or acids ; 2, from the fatty acids to thehydroxy-acids; 3, from the monohydric to the di- and tri-hydricalcohols ; 4, from the normal and iso-alcohols to the tertiary alcohols ;5, from the ethereal salts of formic acid t o isomeric ethereal salts ofthe higher fatty acids; 6, from compounds of the propyl series tothose of the ally1 series.Probably an increase in capillary heightalso occurs in passing from aldehydes to isomeric ketones, and fromfatty acids to their monosubstituted halogen-derivatives, although onfurther substitution a decrease occurs ; f iirther observations arerequired on these two points. Aldehydes show a lower ca,pillaryheight than the corresponding fatty acids in concentrated solutions,but in dilute solutions the reverse is observed. Normal alcoholsshow a lower capillary height than iso-alcohols in concentrated solu-tions. A. J. G.Mutual Relations of the Physical ,Properties of the Ele-ments. By H. FRITZ (Ber., 17, 2160-2165).-This paper contains atable of most of the heavy metals, with their melting points, specificgravities, atomic weights, and specific heats ; from these, it may beshown by calculation that the product of the atomic heat b,y the relativeheat i s equal to the cube root of the product of the melting point mul-tiplied by the spec$% heat, As .Ds = V%; A being the atomicweight, s the specific heat, D the sp. gr., and t the melting point.The elements are arranged in groups in which different values aresubstituted for t. In the case of lithium, sodium, and potassium, thevalue ’ - i- 50 is substituted for t ; in the case of magnesium and2.50aluminium the value tG, and in that of strontium and barium7.4t + f;o30 *If the metals be arranged I, according to the amount of heatliberated by their union with oxygen aud chlorine, and IT, accordingto their conductivity for heat, the one series will be found to bethe revarse of the other.A. I(. M.A General Statement of the Laws of Chemical Equilibrium.By H. LE CHATELIER (Compt. rend., 99, 786--789).-The authorextends and modifies Van tl’Hoff’s general statement of the chemicalequilibrium of a system by including in it t,he “ condensation ” of thesystem, that is, pressure, concentration, number of molecules in unitvolume, &c., and by giving it a form similar to that of the lawsrelating to changes of equilibrium which effect mechanical work.Reversible chemical changes are thus brought into the class ofreciprocal phenomena.When a system in stable chemical equilibrium is acted on by anexternal cause which tends to alter the temperature or condensationeither of the whole system or of some of its parts, the system can onlIlls ABSTRACTS OF CHEMICAL PAPERS.undergo such inLerna1 modifications as would, if they had taken placespontaneously, have produced a change of temperature or con-densation of the contrary sign to that resulting from the action of theexternal cause.These modifications are generally progressive and incomplete.They are, however, sudden and complete if they can take place with-out changing the individual condensation of the different homo-geneous parts of the system, whilst a t the same time they alter thecondensation of the system as a whole,They are nil when their occurrence cannot, produce changesanalogous to those due to the external cause.Although modifications may be possible, they do not necessarilytake place. I n cases where no change occurs arid the system remainsunaltered, the original stable eqnilibr*ium becomes unstable, and thesystem can then only undergo such modifications as tend to bring itback t o stable equilibrium. Many well-known reactions, includingthe phenomena of fusion, evaporation, solution, &c., are cited asexamples. C. H. B

ISSN:0368-1769    

DOI:10.1039/CA8854800109

出版商:RSC    

年代:1885

数据来源: RSC

摘要:

Ills ABSTRACTS OF CHEMICAL PAPERS.I n o r g a n i c Chemistry,Combustible Organic Matter in the Air. By A. MUNTZ andE. AUBJN (Compt. rend., 99, 871--874).-The amount of combustibleorganic matter in the air was determined by two methods. In thefirst, a known volume of air, carehlly filtered from suspended matterand purified from carbonic anhydride, was passed over heated cupricoxide, and the volume of carbonic anhydride produced by the com-bustion of the organic matter was measured. In the second, theamount of carbonic auhydride in 1000-1500 litres of air was deter-mined by the method previously described (Le., by passing the airthrough a tube containing potash pumice), and an equal volume ofair taken a t the same place and a t the same time was passed overheated cupric oxide, and the amount of carbonic anhydride formedwas estimdted.The difference between this amount and that alreadyexisting in the air is the aruonrit produced bay the combustion of theorganic matter, Both methods gave identical results.At Paris, the amount of carbonic anhydride formed by the combus-tion of the atmospheric organic matter varies between 3 and 10 vols.per 1,000,000 vols. of air. At Vincennes the volume varies from2-0 to 4.7 per million, the mean result for October, November, andDecember, 1882, being 3.3 vols. It would seem, therefore, that theamount of organic matter in the air is represented by a volume ofcarbonic anhydride equal to one-hundredth part of the volume ofcarbonic anhydride existing as such in the atmosphere.If it is assumed that all the combustible carbon is present in theair as methane, the volume of the hydrogen contained in the latterwill be 16 per million of air, or, in Paris, 33 vols.per million, a num-ber which agrees well with the lower values foutld by BoussingaultINORGANIC CHEMISTRY. 119When electric discharges are passed through the air, the com-bustible organic matter is more or leas completely burnt, and there islittle doubt that the electric discharges which take place in the loaerregions of the atmosphere destroy a considerable proportion of thecombustible organic matter which the latter contains. C. H. B.Reactions with Carbon and some of its Compounds. ByG. GORE (Chem. News, 50, 124--126).-When white or red phos-phorus, or powdered arsenic or antimony or sodium, are added toiused poiassium cyanide ; or when aluminium or sodium phosphide,or‘ a mixture of sodium phosphide with zinc, is added to fused potassiumand sodium carbonates ; or when sodium carbonate is decomposed ata low red heat by phosphorus vapour ; or wlien a mixture of red phos-phorus and ammonium carbonate is dropped into a red-hot porcelaincrucible, a black substance separates, which i n some cases is found tobe carbon.Carbon is also obtained when coal-gas is passed over red-liot finely-powdered ferric oxide, or over just fused argentic fluorideor chloride, or over chloride of lead or copper. Arsenic and anti-mony do not visibly decompose fused sodium and potassium carbo-nates ; neither is carbon set free when ammonium carbonate is addedto fused sodium; nor when cod-gas is passed over fused cadmiumchloride or silver iodide ; nor in several experiments wherein nume-rous hydrocarbons, in various solvents, were exposed to metals andmetallic couples.Several unsuccessful attempts a t deoxidising car-bonic anhydride are also described along with many experimeotswherein many substances alone and in contact were immersed invarious solutions of metallic salts contaiiiing carbon in combination,and in these solutions when exposed t o carboniferous yapours, but inall cases without any deposition of carbon. The chlorides of carbonproved equally useless as sources of carbon, even resisting the influeuceof potassium, which however fornied an alkaline salt with carbon t’etra-chloI ide ; potassium or sodium, dissolved in anhydrous liquid ammoniaat 60” F., behaved in a similar manner with carbon bromide and sul-phide, and with anhydrous sodium carbonate or formate, or ammoniumoxalate. On passing dry ammonia gas into liquid carbon dichloridecontaining potassium, gas was evolved, and a red powder formed ; withnaphtha instead of the chloride, the potassium only became red.Carbonis insoluble in anhydrous liquid cyanogen, sulyhuric chloride, phos-phorus trichloride, antimony pentachloride, anhydrous liquid hydro-fluoric and hydrochloric acids : chlorides of carbon and bisulphide ofcarbon were also found to be insoluble in the last two acids, but theyare soluble in liquid cyanogen.Many experiments with carbon bisul-phide are described ; for example, when silver and platilium in con-tact are immersed in it, after some time the silver blackens ; in thesame way lead and mercury yield a black powder soluble in nitric:acid. Thallium also blackens, but no action could be observed withtin, or magnesium and platinum, or with boron fluoride; tin tetra-chloride, thallium chloride, and cyanogen are dissolved by it, and itprecipitates mercuric chloride from its solution in ether. The solutionsof sulphur and phosphorus in carbon bisulphide give no reaction whenexposed in an atmosphere of carbonic anhydride; zinc remains brigli120 ABSTRACTS OF CHEMICAL PAPERS.in the sulphur solution and potassium and platinum in contact causeno free carbon to separate from i t ; aluminium and magnesiumbecome dull, but are not corroded by prolonged exposure in thephosphorus solution.When a solution of silver nitrate with a pieceof platinum partly immersed in it was exposed to carbon bisulphidevapour continuously for seven weeks, all the silver was precipitated ;magnesium, aluminium, or silver partly immersed in water exposed tothe same vapour, were unaltered ; when, however, the silver was incontact with plabinum, the liquid became dark and the silver abovei t blackened. A liquid which dissolved selenium was obtained bypassing the vapour of selenium over charcoal powder kept at a fullred heat. D. A. L.Polymorphism of Silicon Phosphate. Ry P. HAUTEFEUILTBand J. MARGOTTET (Compt.rend., 99, 789--792).-Hydmted silicadissolves readily when heated with orthophosphoric acid, and thesolution deposits crystallised silicon phosphate in forms varying withthe temperature at which the deposition takes place. When an in-timate mixture of phosphoric acid and hydrated silica is graduallyheated to 260°, about 5 per cent. of silica is dissolved, and a stiillarger proportion can be obtained in solution by gradually heating amixture of phosphoric acid with silicon chloride.When the solution of silica in phosphoric acid is allowed to coolbelow 260", it deposits crystals having the appearance of flatteneddiscs. Similar crystals are obtained when the solution is mixed withstrong sulphuric acid and heated for some time at a temperaturesomewhat above the boiling point of the latter. These crystals arehexagonal prisms, frequently macled in the same manner as lamellarhmmatite.They act strongly on polarised light, and are somewhatrapidly attacked by water, but do not alter in contact with alcohol.If the temperature of the solution of silica is gradually raised from260" to about 360", it deposits an abundance of very thin hexagonallamellm, which act feebly on polarised light and resemble tridyniite inappearance. They are, however, distinguished from the latter by thefact that they yield silver pbosphate when fused with silver nitrate.These Iamelle are not altered by alcohol, but are slowly attacked bywater with formation of phosphoric acid and sohxble silica.If the solution of silica is heated rapidly, it remains limpid up toabout 700", but between 700" and 800" it deposits regular octahedrawhich are almost always modified by cubical faces.This form ofsilicon phosphate has already been described (Abstr., 1883, 782).When phosphoric acid containing only a small proportion of silica,is rapidly heated to about 900-1000", the crystals obtained are mono-clinic prisms which act strongly on polarised light. A t a high tempe-rature, these prisms are more sfhble than the other forms. If phos-phoric acid saturated with silica is slowly heated to lOOO", a mixtureof all four forms is obtained; but if the temperature is maintainedthe lamella3 and octahedra are quickly attacked, whilst the prismscontinue to increase.They allhave the composition P20,,Si02.The hexagonal crystals are formedThe crystals were analysed by fusion with silver nitrateINOROANIC CHENISTRY. 121below 300°, the lamellae resembling tridymite at about 360", the regu-lar octahedra between 700" and 800°, and the monoclinic prismsbetween 800" and 1000". This polymorphism is not due to differentgroupings of the same crystalline elements, for the hexagonal crystalsare attacked by water, which has no action on the octahedra, orprisms.Other phosphates behave in a similar manner. C. H. B.Crystalline Phosphorous Anhydride. By J. M. CABELL (Chew.News, 50,209).-The mixture of oxides obtained by burning phosphoruswith a limited supply of air was placed at both ends of a long tube,the intervening space being empty ; carefully dried and purifiedhydrogen was then passed through the tube and the foremost portionof the oxides gently heated. At about 350' F.crystals were depositedin the empty portion of the tube, whilst the residue became semi-fused. The crysfals, apparently monoclinic, could not be measured ;when quickly transferred to litmns-paper they did not redden it forsome seconds. Their solution did not give phosphoric acid reactionswith either ammonium molybdate or magnesia mixture; but afterwarming with nitric acid both reactions were obtained. It is henceinferred-that these are crystals of phospltorous anhydride.D. A. L.Arsenic Trifluoride. By H. MOBSAN (Comnpt. rend., 99,874-876).-A rsenic trifluoride was obtained by heating calcium fluoride andarsenious oxide with sulphuric acid.It forms a colourless, verymobile liquid, which boils at 63" under a pressure of 752 mm., andfumes in the air ; sp. gr. = 2,734. It dissolves a certain quantity ofiodine, acquiring a purple-red colour, and combines with bromine atR gentle heat, forming a crystalline compound. When heated to dullredness in a glass vessel, i t yields silicon fluoride and arsenious oxide,but no metallic arsenic is liberated: 4AsF3 + 3sio2 = 2As20, +3SiF4. When the arsenious fluoride is electrolysed in a platinumvessel by means of 25 Bnnsen elements arranged in series, metallicarsenic is deposited, and a gas is given off at the positive electrodewhich, although made of platinum, is superficially attacked.C. H.B.Specific Gravity of Sulphuric Acid. By D. MENDELLEFF (Bey.,17, 2536-2541).--8 reply to Lunge (Abstr., 1884, 1256), in whichthe author upholds the correctness of his density 1.8371 at 1 5 O __ asagainst that of 1.8384 found by Lunge.4 OL. T. T.Octosulphates. By R. WEBER (Bey., 17, 2497--2503).-By heat-ing carefully dried sulphates with excess of sulphuric anhydride, theauthor has obtained a series of well characterised salts of the generalformula M'20,8S03. The product while still hot consists of twolayers, the upper one being unchanged anhydride. The salt solidifiesas it cools, and the still liquid anhydride may be poured off, andthe last traces caref ullg distilled off at about 60"122 ABS L'RACTS OF CRE'MICAL PAPERS.The ptassium salt, K20,8S03, melts in the presence of excess ofsulphuric anhydride a t 80" : when isolated, it is slowly decomposed a tthe boiling point, of the anhydride, yielding first K20,2S03, and finallyK,SO,.Ruhidiuw andc ~ s i z i m behave exactly like potassium, but no corresponding sodiumor lithium compound could be obtained. The nmmoniurn salt,(NH4),0,8S0,, is formed even more easily than the potassium salt.Of the heavy metds, thaZZium alone seems capable of forming anoctosulphnte. Its crystals seem to be isomorphous with those of thepot,assium compound, and, like the latter, i t yields a disulphate,Tl2O,2SO,, when heated. 8iltwr yields a disulpkate, AmO,BSO,, underthis treatment, but no higher sulphate could be obtained. Theanalogy of thallium to potassium, and the dissimilarity therefrom ofsodium and lithium, are noticeable.It crystnllises from the fused mass in prisms.L.T. T.Action of Water on Double Salts. Rg F. M. RAOULT (Compt.rend., 99, 914-916).--.The author has dekermined the molecularreduction of the freezing point produced by various double saltscontaining more than one molecule of the acid radicle, with the resultsgiven in the following table, where A is the observed molecularreduction and S the sum of the molecular rednctions producedseparately by each of the simple salts of which the double salt iscomposed : --K2SOa,MgS04 . . 57.7 58.2K,SO,,Zn<O, .. 58.1 57.2K,SOo,FeSOI . . 56.5 58.0A. S.RZSO1,CuSOI .. 58.3 57.0K2SO~,A1,3SO~ . 82.4 83.4K,S04,Fe23S04.85.0 82.1K2SOa,Cr23S04 . 83.2 84.4A.2KCl,MqCl, . . 117.22KCI,CuC11, .. 116.82AmCl,H~:Cl,. 68.42NaC1,PtC14 . . 54.22KI,HgT, . . . . 50.82KCy,HgCy?. . 57.3KCy,AgCy .. 31.1It is evident that many double salts, espec:ially the alums and thedouble sulphates and double chlorides of the magnesium group ofmetals, produce a molecular reduction of the freezing point practicallyidentical with the sum of the molecular reductions produced separatelyby each constituent salt. In other words, thev behave in sohitioii asif the constituent salts were merely mixed and not in actual combilia-tion, a result which agrees perfectly with therrnochemical observa-tions. In the case of the last five salts in the table, however, thisdoes not hold good, and i t follows that these double salts ar'e notcompletely decomposed by wa! er, a result agreeing with therrno-chemical observatAms, which show that the formation of each of thelast three is accompanied by the development of a considerableamount of heat.From these results, i t follows that a comparison of the observdmolecular reduction of the freezirig point produced by a given doublesalt wilh the sum of the partid reductions produced by each con-stituent, will show whether the double salt is or is not compleit.lydecomposed when it is dissolved in water.If it is assumed that the molecular reduction produced by a givcISORGANIC: CHEMISTRY.123double salt is equal to the mean molecular reduction of the potassinrnsalts containing the same number of atoms in the molecule (a sup-position which is supported by the known beh,iviour of silver potas-sium cyanide), it is possible to calculate the amonnt of decompositionwhich each salt experiences when dissolved.Some of the numbersthus obtained are given in the following table. They represent thatfraction of the molecule of the double salt which is decomposed bywater :-KCy +2KCy +2KI +2AmCl+2XaCl +2KC1 +KYSO, +K&Oi +AgCy + water (2 litres) . . . . . . . .HpCx. + mater (10 litres). . . . . . . .HgI, + water (4 litres) . . . . . . . .HgCI, + u-ater (10 litres). . . . . . . .PIC1, + water (4 litres) . . . . . . . .MgCl, and analogous chlorides . . . .MgSO4 ,, sulphates . . . .A123SOd .... 1 ) ?,0.000.380.380.590.261.001.001.00C. H.B.Magnesium Suboxide. By G. GORE (Chem. Nezus, 50, 157).--Beet2 (Phil. JIag., 1866, 269) observed, when magnesium elec-trodes were used for the electrolysis of a solution of sodium chloride,that a black substance was formed on the positive pole, and from thefact that it evolved hpdrogen in contact with certain aqueous solutions,he concluded that i t was magnesium suboxide.The author has observed a similar phenomenon under the followingconditions :-When magnesium alone is partly immersed in water and exposedto coal-gas, carbonic anhydride, vapour of CCI, or CpC14, or when it i simmersed in a mixture of absolute alcohol with glacial acet,ic acid ;the deposition is slight with magnesium in liquefied glacial acetic acidalone, or in a solution of toluene or formic acid in absolute alcohol, orin a mixtiire of glacial acetic, with either sulphuric acid or vegetablenaphtha.On the. other hand, the deposition is more rapid in all thesecases when the magnesium is in contact with either platinum, gold,silver, or iron, and most rapid with palladium. Magnesium andplatinum in contact, produce it' when they are immersed in a solution ofeither creosote, toluene, or xylene in vegetable naphtha, or in a solutioncontaining 1.25 mm. of hydrochloric acid per ounce of water. Theblack deposit is also formed when magnesium alone is immersed insolutions of the following salts containing 5 grains of salt per ouilce ofwater :-potassium, sodium, ammonium, lithium, barium, stront;um,calcium, and magnesium chlorides, bromides of the first thyee, andpotassium iodide, the sodium chloride solution giving the largestamount.I n all cases it appeared within the first few daJs, sub-sequently disappearing with the simultaneous formation of whitemagnesium hydroxide. From all these facts, i t is evident that theblack substance comes from the magnesiiim. It turns white whenheated t= a temperature below redness. I t is soluble in dilute nitricacid, yielding a green solution owing tlo reduetion ; hjdrochluric aridsulphuric acids dissolve it with effervescelice. Its hydrochloric acaidsolution contains magnesium chloride only. These results confirn124 ABSTRACTS OF CHEMICAL PAPERS.Beetz's conclusion, namely, that this substance is magnesium szhb-oxide.D. A. L.Copper Peroxide. By G. R R ~ S S (Ber., 17, 259:3-2597).-Theexperiments by Thknard seemed to indicate the formation of a copperperoxide by the agitation of cupric oxide with a dilute solution ofhydrogen peroxide. In this paper, a description is given of a repeti-tion of this work, and it is shown that if very finely divided cupricoxide is agitated for several days with hydrogen peroxide there isgradually formed an olive-green precipitate of composition C uOz,H,O.It is decomposed at a temperature of 6" when moist, but is far morestable when dry. The formation of this compound points to thetetratomicity of copper. From other experiments, it would appear thatan oxide can be obtained intermediate in composition between cupricoxide and peroxide, formed by heating cupric oxide with caustic potash,or potassium or sodium chlorides.Decomposition of Cupric Oxide by Heat.By E. J. MAUMEN~(Cornpt. rend., 99, 757-759).-A criticism on the papers by Debrayand Joannis (this vol., pp. 21 and 22).V. H. V.C. H. B.Action of Hydrogen Sulphide on Metallic Silver. By J. M.CABELL (Chem. News, 50, 208--209).-The author has made fourexperiments in which very carefully cleaned pure silver was exposedunder certain varying conditions to a current of pure hydrogen sul-phide, which was first carefully dried. The results tend to show that,in absence of water, hydrogen sulphide does not act on silver at theordinary temperature. D. A. L.Silver Hydroxide. By J.D. BRUCE (Chem. News, 50, 208).-When dilute solutions of silver nitrate and potassium hydroxide, in90 per cent. alcohol, are mixed at the ordinary temperature, in quan-tities containing equivalent amounts of the two substances (AgNO,and KHO), the usual granular brown precipitate of silver oxide isformed, When, however, the mixing is effected at very low tempera-tures, the precipitate which forms is flocculent, and has less and lesscolour as the temperature is lowered, until at about -50" F. the precipi-tate is almost white. This white precipitate soon becomes coloured,and a t -440" F. is already pale brown. The white precipitate ispresumably silver hydroxide, and is but slightly soluble in water.Hydrated Aluminium Sulphate.By P. M. DELACHARLONNY(Compt. rend., 99,800--801).-When a moist mass of crystals of normalaluminium sulphate, Alz3S0,,l6H,O, is cooled to 6--8", crystals of anew hydrate, A1,3SO4,27H,O, are gradually formed. These crystalsare hexagonal prisms modified by faces of the rhombohedron in the samemanner as crystals of dioptase. They are formed only below 9*5", andwhen exposed to the air a t ordinary temperatures they give off waterand are reconverted into t'he hydrate Al23SO4,16H2O. The samechange is brought about by mechanical disturbance, such .as crushiiigthe crystals with a pestle. The crystals can, however, be preserved inn. A. LNINERALOQICXL CHXMISTRY. 125closed flasks without undergoing any alteration. The forniation of thishydrate from the ordinary hydrate is much facilitated by mixing thelatter with some ready-formed crystals of the former.Reaction between Ferric Oxide and certain Sulphates atHigh Temperatures. By SCHEURER-KESTNER (Compt. rend., 99,876--877).-When a mixture of t w o parts of calcium sulphate and onepart' ferric oxide is heated to bright redness, it fuses, the whole of thesulphur is expelled, and a residue of ferric and calciuni oxides is left,soluble in dilute acids. Even acetic acid gradually removes thecalcium in the cold. During the decomposition, sulphuric anhydrideis first evolved, and afterwards, as the temperature rises, sulphurousanhydride and oxygen. Probably the mixture fuses and calciumoxide and ferric sulphats are Eormed, the latter being afterwardsdecomposed. By adding a fl~ix, such a9 calcium chloride or fluoride,decomposition takes place at a lower temperature, but the crucible ismuch corroded.Lead sulphate is decomposed in the same way a t a somewhat, lowertemperature, The residue dissolves in dilute nitric acid withoutevolution of nitrogen oxides, and acetic acid gradually dissolves outthe lead in the cold. Magnesium sulpllate behaves in a similarmanner, but does not fuse, and only sulphurous anhydride and oxygenare given off without any sulphuric anhydride.C. H. B.C. H. B

ISSN:0368-1769    

DOI:10.1039/CA8854800118

出版商:RSC    

年代:1885

数据来源: RSC