摘要:

J O U R N A L C. F BAKER. H. BAKER. D. BENDIX. A. (3. BLOXAM. C. H. BOTHAMLEY. B. BRAUNEB. B. H. BROUQH. H. CBOYPTON. W. D. HALLIBURTON M.D. B.Sc. F. 5. KIPPINO Ph.D. D.Sc. J. W. LEATHER Ph.D. D. A. LOUIS. T. MAXWELL M.D. B.Sc. N. H. J. MILLER Ph.D. OF Q-. T. MOODY U.Sc. J. M. H. MUNRO D.Sc. T. (3. NICHOLSON. E. W. PEEVOST Ph.D. H. H. ROBINSON B.A. R. ROUTLEDBE B.Sc. M. J. SALTER. JAMES TAYLOR B.Sc. L. T. THORNR Ph.D. H. K. TOMPKINS B.Sc. Gt. W. DE TUNZELMANN B Sc. W. C. WILLIAMS B.Sc. W. P. WYNNE B.Sc. THE CHEMICAL SOCIETY. H. E. ARMSTBONG Ph.D. F.R.S. W. CROOKES F.R.S. WYNDHAM R. DUNSTAN. I?. R. JAPP M.A. Ph.D. F.R.S. H.MCLEOD F.R.S. A. K. MILLER Ph.D. HUGO MULLIPR Ph.D. F.R.S. 5. U. PICKERINU M A. W. RAMSAY Ph.D. F.R.S. W. J. RUSSELL Ph.D. F.R.S. J. MILLAR THOMSON F.R.S.E. T.E. THORPE Ph.D. l7.B.S W. P. WYNNE B.Sc. @bitm C. E. GROVES F.R.S. A. J. GREENAWAY. Vol. LVI 18 8 9. ABSTRACTS. LONDON GURNEY & JACKSON 1 PATERNOSTER ROW. 1889.LONDON TIAIiRISON AND SONS PRINTERS IN ORDINARY TO HER MAJESTY ST. MAILTIN’S LANE.J O U R N A L THE CHEMICAL SOCIETY. H. E. ARMSTRONG Ph.D. F.R.S. W. CROOKES F.R.S. WYNDHAM R. DUNSTAN. F. R. JAPP M.A. Ph.D. F.RS. H. MCLEOD F.R.S. A. I(. MILLER Ph.D. HUGO MULLER Ph.D. F.R.S. S. U. PICKERITGF &LA. W. RANSAY Ph D. F R.S W. J. RUSSELL Pli D F.R S. J. MILLAR TITOMSON F R S E T. E. THOEPE Ph.D P.B S. W. P. WYNNE B Sc. &;bitw C. E. GROVES F.R.8 Sjub-@/bitar a. J. GREENAWAY. 3Jbstrartoss C. F. BAKER. G. T. MOODY D.Sc. H. BAKER. J. M. H. MUNRO D.Sc. D. BENDIX. T. (3. NICHOLSON. A.G.BLOXAM. E. W. PREVOST Ph.D. C. H. BOTIIAMLEY. H. H. ROBINSON B A. B. BRAUNER. R. ROUTLEDQE B.Sc. B. H. BROUGH. M. J. SALTER. H. CROMPTON. JAMES TAYLOR B.Sc. W. D. HALLIBURTON M.D. B.Sc. L. T. THORNR P1i.D. F. S. KIPPINQ Ph.D. D.Sc. H. K. TOMPEIXS B.Sc. J. W. LEATHER Ph.D. G. W. DE TUNZELMAXN I3 Sc. D. A. LOUIS. W. C. WILLIAMS B.Sc. T. MAXWELL M.D. B.Sc. W. P. WYNNE B Sc. N. H. J. MILLER Ph.D. VOl. LVI. Part I. 1889. ABSTRACTS. LONDON GURNEY & JACKSON 1 PATERNOSTER RCW. 1889.LONDON HARRISON AND SONS PBINTEBS I N ORDINARY TO HER MAJESTY ST. MARTIN’S LANE.C 0 N T E N T S. ABSTRACTS OF PAPERY PUBLISHED IN OTHER JOURNALS :- General and Physical Chemistry. LIVEING (G. D.) and J. DEWAR. Absorption-spectrum of Oxjgen.TROWBRIDGE (J.) and W. C. SABINE.Metallic Spectra.BOISBAITDRAN (L. DE). Degree of Oxidation of Chromium and Manganese in Fluorescent Mixtures.LINDECK (S.). Electromotive Force of Amalgams. KALISCBER (S.). Electromotive Force of Selenium. GEE (W. W. H.) and H. HOT.DEN. Reciprocal Conductivity.OSTWALD (W.). Apparatus for Determining the Conductivity of Electro- lytes. STJTHEBLAND (W.). Specific Heats at High Temperatures.MATHIAS (E.). Specific Heats of Saline 8olutions. LOUQUININE (W.). Heat of Co.iibustion of Acids of the Oxalic :ind Lactic Series. OSSIPOFF (I.) Heats of Combustion of some Organic Substances.LOUGUININE (W.). Heat of Combustion of Camphorjc Acids.WALKER (J.). Method of Determining Vapour-tensions at Low rein- perat ures.RAOITLT (F. M.). Vapour-tensions of Alcoholic Solutions.LESC~EITR (H.) and D.MATHURIN. Water of Crystallisation of the Alums WARREN (H. N.). Electrolytic Method of Liquefying Gases.AMAQAT (E. H.). Compressibility of Hydrogen Oxygen Nitrogen and Air a t very High Pressures.DE VXIES (H.). Isotonic Coefficient of Glycerol. ROWLAND (H. A.) and L. BELL. Actior. of a Magnet on Chemical Action.MEYERHOFFER (W.).Accelerating and Retarding Influences in Chemical Processes.GIERSBACH (J.) and A. KESSLER. Nitration of Benzene.HUNT (T. S.). The Foundations of Chemistry. BECKMANN (E.). Determining Molecular Weights by Reduction of the JOFFRE (J.). NEWBURY (S. B.). Apparatus for Distillation in a Vavuum.LIVEINGC (a. D.) and J. DEWAR. Spectrum of Magnesium. LIVEING (G. D.) and J. DEWAR. Ultra-violet Spectra of Nickel and Cobalt WRIGHT (C.R. A.) and C. THOMPSON. Two-fluid Cells.GORE (G.). Effect of Chlorine on the Electromotive Force of a Voltaic Couple. WRIQHT (C. R. A.) acd C. THOMPSON. Development of Voltaic Electricity by Atmospheric Oxidation.WARBURQ (E.) and F. TEGETMEIER. Electrolytic Conductivit j of Rock Salt. MONCKMAR (J.). Effect of Occluded Gases on the Thermo-electric Proper- ties of Compounde.ANDHEWS (T.). Electzochemical E5ects of Magnetising Iron.HESS (H.). Specific Heat of some Solid Organic Compoiinde.VELEY (V. H.). Evolution of Gases from Homogeneous Liquids.Freezing Point.Resistance to Light of Colouring Matters fixed in l'issties g d PAQE 1 1 2 2 :? 3 1 4 4 5 5 6 c i 7 7 7 8 9 9 9 10 10 1 1 1% I:! S:) 89 h!) ! )O 90 91 98 92 92 94CONTENTS. V SCEALL (0.). Vapour-density Estimation under Diminished Pressure.MULLER-ERZBACH (W.).Water of Crystallisation of the Alums.BEEETOFF (N.). Selective Chemical A5nity. POTILITZIN (A.).Influence of Temperature on the Direction of Chemical Change. BONZ (A.). Formation of Amides from Ethereal Salts and Ammonia and the Reversal of the Reaction.WATSON (G.). Dead Space in Chemical Reactions. BRAUNER (B.). Standard of Atomic Weights. EYKMAN (J.F.). Apparatus for Determining the Reduction of the Freezing Point. GROSHANS (J.A.). Calculation of the Molecular Volume of Benzene Naphthalene Anthracene &c.CIAMICIAN ((3.). Lecture Experiment on Rnoult's Law.HAWKRIDGE (P.). Lecture Experiment Volumetric Composition of certain LEONABD (N.). Blue Flame produced by Sodium Chloride in a Coal Fire.KANONNIPOFF (I.).Relation between the Rotatory and Refractive Power SUTHERLAND (W.). Molecular Refraction. GRUNWALD (A.). Spectral Analysis of Cadmium. BOISBAUDRAN (L.DE).Gadolinium. EXNER (F.) and J.TUMA.PO IN CAR^ (L.). Electrical Conductivity of Fused Salts.HBRROUN (E.F.). Abnormal Electromotive Forces. QUINCKE (F.). Electrolysis of Copper Chloride. HENNEBERG (H.). Heat Conductivity of Mixtures of Ethyl Alcohol and Water. JOLY (J.). Specific Heats of Gases a t Constant Volume.OSSIPOFF (I.).Heats of Formation of Several Organic Acids.OSSIPOFF (I.). Heats of Combustion of Stilbene and the Isomeric Nono- napht henes.ANTOINE (C.). Dilatation and Compression of Air. JAEGER (W.). Velocity of Sound in Vapours and the Determination of the Vapour-density.RICHARDS (T.W.). Vapour-density Determinations.ETARD (A.). Relation between the Solubility of Salts and their Melting Points. HERITSCR (A.). General Law of the Diminution of Volume of Salts by Solution in Water.WINEELMANN (A.). Influence of Temperature on Evaporation and on the Diffusion of Vapours.PENDLEBURY (W.H.) and M.SEWARD.Gradual Chemical Change.URECH (F.). Reduction-velocity of Alkaline Copper Solutions.FUCHS (F.). A General Method of Estimatiiig the Basicity of Acids.GROSHANS (J.A.). Prout's Hypothesis especially in relation to the Atomic BRUHL (J.W.). Sublimalion Apparatus. BRUHL (J.W.). Apparatus for Urystallisiag at a Low Temperature.BECQUEREL (H.). Absorption-spectra of Epidote. WALTER (B.). Change of Fluorescence with Concentration.WALTER (B.). Evidence afforded by Fluorescence and Absorption of the Decomposition of Molecular Groups in Solutions.RIGHI (A.). Electromotive Force of Selenium. SOHNCEE (L.). Production of the Current in the Galvanic Circuit.BOUTY (E.). Electrical Conductivity and Electrolysis of Concentrated Solutions of Sulphuric Acid.WEBER (C.L.). Electric Conductivity of Solid Mercury.POTIEB (A.). Electrochemical Measurement of Currents.OSTWALD (W.) and W.NERNST.FreeIons. Gaseous Compounds.of Chemical Compounds.Chemical Theory of the Galvanic Element Weights of Carbon and Oxygen. PAGE 331 331 332 335 335 335 335 336 336 336 336 336 453 454 455 456 456 457 457 458 459 459 459 4.60 460 460 4t10 460 461 461 462 462 463 463 463 4 64 553 553 554 555 556 556 557 557 558CONTENTS. vii OSTWALD (W.). Dropping Electrodes.AUBEL (E.v.). Electrical Resistance of Bismuth. CHROUSTCHOFF (P.). Electrical Conductivity of Saline Solutions.CHROUSTCHOPF (P.).Electrical Conductivity of Saline Solutions. Re- ciprocal Displacement of Acids. CHROUSTCHOFF (P.). Electrical Conductivity of Saline Solutions.CHROUSTCHOFF (P.) and V. PACEKOFF. Electrical Conductivity of Saline Solutions.LUDEKINO (C.). Conductivity of Solutions of Zinc Sulphate containing Gelatin. BORE (G.). MULLER (J. A.). Heat of Formation of Alkaline Carbonates in v e v DilGte Solutions.BERTHELOT and PETIT. Heat OF Combustion of Carbon.BERTHELOT and PETIT. RETGERS (J. W.). Determination of the Specific Gravity of Salts which are Soluble in Water.GERLACH (G. T.). The Densitv Numbers of Groshans.LESCCEUR (H.). Dissociation of &line Hydrates and Analogous Compounds.MULLER (0.). Absorption of Carbonic Anhydride by Mixtures of Alcohol and Water.BRUGELMANN (G.). Crystallisation and Physical Union.VOIGTLANDER (F.). Diffusion in Agar Jelly. HALLOCK (W.). Chemical Action between Solids. OSTWALD (W.). Constants of Affinity of Organic Acids and their Relation to Composition and Constitution. MEPERHOFFER (W.). Reversible Transformation of Copper Potassium OSTWALD (W.). Unit of Atomic Weights. BRAUNER (B.). Basis of Atomic Weights. MEYER (L.) and K. SEUBERT. Unit of Atomic Weights.LADENBURQ (A.).Molecular Weight Determinations from Osmotic Pressure WILL (W.) and G. BREDIG. Xstirnation of the Molecular Weights of Dissolved Substances.KLOBUKOFF (N. v.). Cryoscopic Behwiour of Solutions of Iodoform in Benzene and Acetic Acid.STOEMANN (F.) C.ELEBER and H. LANOBEIN. Cornbustion of Organic Substances in Oxygen a t High Pressure. BERTFIELOT. Heat of Formation of Hgponitrites. ,.VANT’ HOFF (J. H.) and L. T. REICHER. Temperature of Transformation in Double Decomposition.ZETGERS (J. W.). Specific Gravity of Isomorphous Mixtures.HECRT (W.) and M. CONRAD. Determination of Affinits Constants.OSTWALD (W.) Dissociation of Electrolytes. VANT’ HOPF (J. H.). Relation between the Affinity in Absolute Measure and Ostwald’s Constant? of Affinity. OSTWALD (W.). Unit of Atomic Weight. TAMMANN (G.) Constitution of Alloys. SILOW (P.). Alloys.BECKMANN (E.). Estimation of the Molecular Weight from the Rise in the Boiling Point.KLOBUKOFF (N. v.). Cryoscopic Behaviour of Solutions of Morphine Com- pounds in Benzene Acetic Acid and Water.PATERN~ (E.). Molecular Depression of the Freezing Point of Benzene by Alcohols. TAFEL (J.). Apparatus for Shaking. BECEE (F.). Crystalline Form of Grape-sugar and of OpticallF Active Sub- stances in General.RICHARZ (F.). Electrical Behaviour of Platinum in Persulphuric Acid && the Galvanic Polarisation in the Formation of the Latter.Loss of Voltaic Energy of Electrolytes by Chemical Union Heats of Combustion and Formation of Nitriles Sulphate. PAGE 807 80 7 808 808 809 809 809 810 810 811 813 812 813 815 816 81’7 81 7 817 818 819 819 819 819 820 820 82 1 929 930 930 931 931 931 932 932 9.38 933 933 933 9$3 934 1041 1041CONTENTS.CHANTEMILLE (P.). Hydrogen Sulphide Apparatus. MAUMEN~ (E.J.). Chydrazine or Yrotoxide of Ammonia.Hydrogen.Methane. &c.COOKE (S.).Action of the Electric Spark on Mixtures of Nitric Oxide with COOKE (S.) Decomposition of Nitric Oxide in contact with Water and with Potash.MCCAY (L.W.). Action of Hydrogen SulphiJe on Arsenic Acid.HODGES (E.R.). Barium Sulphite. RAUPEYSTR4UCH (a.A.).Solubility of Gypsum. SPILLER (J.). Ancient Mortar from a Roman Wall in London.WELCH (J.C.). Analysis of Money. CHUARD (E.). New Hydrated Cupric Chloride. Csams (J.M.). Purification of Mercury. DUBOIN (A.). Yttrium-potassium and Yttrium-sodium Phosphates.LAUTH (C.) and G.DUTAILLY. BONGAETZ (J.) and A.CLASSEN. HODGKINSON (W.R.) and F.K.S.LowNDEs.Action of Incandescent. ENGEL (R.). Normal Platinum Chloride. MANN.Preparation of Chemically Pure Hydrogeu Peroxide.STORTENBEKER (W.).Compounds of Chlorine with Iodine.RASCHIG (F.). Theory of the Lead Chamber Process. LUNGE (G.). Theory of the Lead Chamber Process. CAMERON (C.A.) and J.MACALLAN.Compounds of Ammonia with Selenious Anhydride.WEDENSKY (V.). Constitution of Phosphorous Acid. RUDORPF (F.). Compounds of Arsenious Acitl with Sodium Iodide.HAMPE (W.). Preparation of Boron and Silicon by Electrolysis.HAUTEFEUILLE (P.) and A.PERREY.Beryllium Silicates.SORET (A.). Occlusion of Gas by Electrolytic Copper. ROBERTS-AUSTEK (W.C.). Mechanical Properties of Metals in Relation to the Periodic Law.ZIRNITB (G.). Solution of Iron in Aqueous Soda. MAURO (F.). Ammonium Fluoroxymolybdates. VIQNON (L.). Tin.PETERSEN (@.) Fluorine-derivatives of Vanadium. ELBERS (W.).Decomposition of Antimony Sulphide by Boiling Water.BURCHARD (0.). Oxidation of Hydrogen Iodide bj Oxy-acid4.HODGKINSON (w.R.) and F.I(.S.1.owNDEs.Action of Incandescent. UFFELMANN.Analysis of Atmospheric Air. BERTHELOT and FABRE.Hydrogen Telluride. MENTE (A.). Amides of Phosphorus and Sulphur. ENGEL.Allotropic Arsenic.LANDAU (W.). RAWSON (S.(3.). Preparation of Boron and Silicon. WARREN (H.N.). Preparation of Silicon. PARSONS (C.A.). GAUTIER (A.). Formation of Carbon Oxysulphide. BAYER (K.J.). Alkaline Aluminates. LAUTH (C.) and G.DUTAILLY.Porcelain Glazes. SPRING (W.). Cause of Railsrusting less quickly when inUse than when not MACKINTOSH (J.€3.). Crystalline Subsulphide of Iron and Nirkel.PICCINI (A) and G.GIORGIS.DIXON (H.B.) and H.W.SMITH.Imperfect Combustion in Gaseous Explosions.WARDEB (R.33.).Coefficients of Volatility for Auueous Hvdrochloric Acid JOHNSON (G.S.). Barium Sulphite. So-called Crackle China Atomic Weight of Tin Platinum on Gases and Vapours Platinum on Gases and Vapours Action of Ammania and Amines on Arsenious Bromide Effect of High Temperature and Pressure on Carbon New Fluorine Compounds of Vanadium ix PAGE 14 14 15 I5 15 16 16 16 16 17 17 17 18 18 19 20 20 101 102 103 103 103 103 103 103 104 105 105 105 106 107 107 108 207 208 209 210 210 211 211 211 212 212 212 213 214 2144 214 214 337 337 POTILITZI~ (A.). Rate of Decompositioi of t h e Salts oyf Halogen Oxy- acids by Heat andthe Products obtained. 338CONTENTS. xi 674 674 675 675 676 676 677 677 678 678 673 678 754 755 755 755 756 7 57 7 58 759 760 760 762 821 821 823 824 825 825 826 826 827 827 828 829 830 831 83 1 83 2 832 833 834 834 835 934 935 935 936 937 939 9-40 941 PAQE JAWEIN (L.) and A.THILLOT. Molecular Weight of some Metaphosphates. COMEP (A. M.) and C. L. JACKSON. Sodium Zinc Oxides.DENIG~S. Formation of Cuprous Chloride and Bromide from Cupric Sul- phate. BARFOED ((3.). Action of Ammonia on Mercurous Salts.HAXPE (W.). Electrolysis of Cryolite. HAMPE (W.). Aluminium Subfluoride.GAUTIER (A.) and L. HALLOPEAU. Metallic Sulphides.HURST (G. H.). Ochres Siennas and Umbers. CARNOT (A.). Peroxides of Nickel and Cobalt Estimation of Nickel and Cobalt. RAWBON (S. G.). Oxy-haloi'd Derivntires of Chromium.JOLY (A.). Nitroso-compounds of Ruthenium. MERZ (V.) and E. HOLZMANN. Formation of Hydrogen Bromide and Hydrogen Iodide.JOHNSON (G.54.). Solubility of White Precipitate in Solution of Ammonia containing Ammonium Carbonate. WILLIAMS (G. H.) and W. M. BURTON. Crystalline Form of Metallic Zinc MORSE (H. N.) and J. WHITE. Dissociation of the Oxides of Zinc and JOHNSON (I( R.). Some Phosphates of Yoljvalent Metals.Roux and E. LOUISE. Molecular Weights of Aluminium Compounds.SZILASI (J.). Green Ultramarine. WINKLER (C.). Atomic Weight of Nickel and Cobalt.COLORIANO (A.). Crystalline Metallic Molybdates. HUNDESHAGEN (F.). Phosphododecnmolybdic Acid. ROSENHEIM (A.). Vanadotungstic Acid. WINKLE& (C.). Chlorine from Bleaching Powder. OLSZEWSKI (K.). Determination of the Boiling Point of Ozone and of the Solidifying Point of Ethylene.BERTHELOT.Action of Alkdis on the Thionic Acids. BRRTHELOT. Action of Acids on Thiodphates. LE ROY (G. A.). Preparation of Alkaline Nitrites. AMAT (L.). Phosphorous Acid.PARMENTIER (F.). LEF~VRE. Action of Alkaline Arsenates on the Alkaline Eart!ts.FEIT (W.).Potassium Magnesium Bromide. ANDRB (G.). Formation of Mercurammonium Chlorides.MYLIUS (F.) and F. FOERSTER. GORGEU (A.). Formation of Manganese Oxides in the Wet Way.GORGEU (A.). Action of Air on Manganous Carbonate.GAUTIER (A.) and L. HALZOPEAU. Metallic Strlphides.BOURGEOIS (L.). Crystallised OrthosilicateP of Nickel and Cobalt.VOSMAER (A). Preparation of Chromic Chloride. PBCIIARD (E.). Metatungstic Acid. VIGNON (L.). Variations in the Acid Function of Stannic Oxide.BESSON (A.). Combination of Nitrogen Oxides with Metallic Chlorides.PIGEON (L).Platinirni Tetrachloride. JOLY (A.). Atomic Weight of Ruthenium. REMSEN (1.j. Double Halogen Salts. JOHNSON (G. S.). Atomic Weight of Oxygen. PETTERSSON (0.) and K. SOND~N. Absorptive Power of Water for Atmo- spheric Gases.WINKLER (L. W.). Solubility of Oxygen in Water. TRACBE (M.). Autoxidation.TRAUBE (M ). Constitution of Peroxides. TRAUBE (31.). Formation of Hydrogen Peroxide from Persulphuric Acid.TRAUBE (M.). Behaviour of Persulphuric Acid towards Nitrogen Evapora- DIEHL (W.). Ahiminium Subfluoride. Cadmium in the Vapours of their respective Metals.Presence of Sodium Siilphate in the Atmosphere.Solubility of alas3 in Water tion of Hydrogen Peroxide.CONTENTS . xu1 Mineralogical Chemistry.STAHL (W.). Hexagunal Crystals of Zinc Sulphide.SCHMIDT (A.). Arsenopgrite from Servirt. MICHEL (L.). Preparation of Pproniorphite and Mimetesits.JANNETTAZ (E.). Uranite from Madazascar. IGELSTROM (L.J.). Arseniopleite a new Swedish Miisera1.CATHREIN (A.). Minerals of the Tyrol. KUNZ (G.F.). Mineralogical Notes. DOELTER (C.). Artificial Formation of Mica. ROHRBACH (M.). Chiastolite.HOVEY (E.0.). Cordierite-gneiss. KOTO (B.). Piemontite.IDDINGS (J.P.). Origin of Primary Quartz i n Basalt.WOLLEMANN (A.). The Badenweiler Ore Deposit. GLASER (M.) and W.KALMANN.Analysis of Roncegno-water HOFFMAN (G.C.). Native Platinum from Canada. BARROIS ((7.). The Pyroxenites of Morbihan. RINNE (F.). The Dachberg a Volcano of the Rhone. STRENGE (A).Dolerite of Londorf. DE ROUVILLE (P.) and A.DELAGE.Porphyrites at Gtabian.MONTEMARTINI (C.).Composition of Serpentine Rocks.PREUSSNER.A Remarkable Bed of Sulphur. LOCKZA (J.). Arsenopyrite from dervia. LOCZKA (J.). Constitution of Arsenopyrite. SJOGREN (A.). Periclase from Nordmarken. LANBHAUS ((3.). Psilomelane.BLOMSTRAND (C.W.) Analyses of Monazite and Xenotime.HIDDEN (W.E.) and J.B.MACKINTOSH.Sulphohalite SJOGREN (A.). Allactite from LLngban. HOQBOM (A.G.). Pgrrhoarsenite and Berzelite. EAKINS (L G.). Thiantimonites from Colorado. WETBULL (M.). Hjelmite.NORDENSKIOLD (A.E.). Eudidymite. LINDSTEOM ((3.). Analysis of Natrolite. LINDSTROM ((3.). Hplotekite from Lgngban. RAMMELSBERG (C.). Gadolinite.NORDENSKIOLD (A.E.). Mineralogical Notes. BLOMSTRAND (C.W.). The so-called Cyrtolite of Ytterby.FLIKK (G.). Swedish Minerds.LADRI~RE (J.).Phosphatic Minerals a t Montay and Forest.DUNNINQTON (F.P.). BOURGEOIS (TJ.). Formation of Deposits of Oxides of Manganese.Artificial Production of Hydrocerusite it8 Composition. and the Constitution of White Lead HATLE (E.) and H.TAUSS.SCHNEIDER (E.A.). Treatment of Natural Silicates with Hydrochloric Baryto-celestine from Werfen in Salzburg Acid as a means of ascertaining their Structure. PENFIELD (S.L.). Bertrandite from Mt.Ontero Colorado.WADSWORTH (M.E.). Peridotite of Iron Mine Hill Cumbedand Rhodd bland. FRESENIUS (R.). Mineral Spring in the Admirals.garteabad Berlin.CHATARD (T.M.). Analyses of the Waters of some American Alkali Lakes.Riebeckite and the new Formation of Albite in Granite- orthoclase. SAUER (A.).IGELSTR~M (L.J.). Pyrrhoarsenite and other Swedish Antimoniates.HIDDEN (W.E.) and J.B.MACKINTOSH.Auerlite a New Thorium Mineral.FREDA ((3.). Composition of Piperno of the Collina del Vomero.HOWITT (A.W.). Metamorphic and Plutonic Rocks at Omeo PAGE 20 21 21 21 21 22 22 22 23 23 24 24 25 25 25 25 26 27 27 27 28 29 109 109 109 110 110 110 111 215 215 216 216 216 217 217 217 217 21Q 218 219 219 219 219 219 220 220 221 221 262 222 222 MONTEMARTINI (C.). Compbsition of some Rocks from the Shore at Nice.223CONTEXTS. XV PAGE 838 839 839 1054 1054 29 30 31 31 31 32 32 32 33 33 34 34 35 35 35 36 37 37 38 39 40 40 41 4 1 41 42 42 45 45 47 4!3 49 49 50 51 51 51 54 54 55 55 52 LACROIX ( A.).Barium Sulphate.MEPER (A. B.). So-called Jadeitz from Switzerland. COHEN (E.). Msteoric Iron from Portugal.LACBOIX (A.).Rock Containing Sodium-amphibole Astrophyllite Pj-ro- chlorite and Zircon.REICHARDT (E.). Mineral Water of the Ottili Spring Suhl Thuringia Orgal& ChemistnJ GUSTAVSON (G.) and M. DEMJANOFF. Isoallylene. CLAUS (A.) and 0. PTJTENSEN. Cyanurates. ASCHAN (0.). Preparation of a-dibromhydrin. PAAL (C.). Epichlorhydrin.FAUCONNIER (A.).Propylphycite. MAQUENNE. Molecular Weight and Valency of Perseite.R A ~ A N N (B.). Constitution of the Glucoses. KILIANI (H.). Oxidation of Arabinose with Nitric Acid.MAYER (F.). Action of Nitrous Acid on Hexamethylenamhe.UDR~NSKY (L. T.) and E. BAUMANN. Identity of Putresine and Tetra- methylenediamine.ORNDORPF (W. R.) and H. JESSEL. Deconjposition of Acetone with Bleaching Powder.PECHMANN (H. v.) and K. WEHSARG. Dinitrosoacetone.DE VARDA (G.).Sulphoisovaleric Acid. GRAF (P.). Constituents of Cocoa FLtt. MESSINGER (J.) and C. ENGELS. Action of Hydrogen Phosphide on'Alde hydes and Ketonic Acids.WEDARD (E. M.). LOUTSF. (E.) and L. ROUX. Freezing Points of Solutions of Aluminium Alkpls. HILL (H. B.) and A. W. PAXMER. Substituted Pyromucic Acids.Action of Heat on Tartaric Acid in Aqueous Solution VOSWINKEL (A.). Metadiethylbenzene. JACOBSEN (0.) Synthegis of Consecutive Tetramethylbenzene.JACOBSEN (0.). Tetrethylbenzene. CHABRIB (C.). Synthesis of Aromatic Selenium Compounds.JACOBSEN (0.). Comecutive Metaxylenol. RE LA HARPE (C.) and F. REVERDIN. Nitronitrosoresorcinol.BELZER (C.). Derivatives of Paramidoisobutylhenzene.JACOBSEN (0.). Pentethylbenzene and its Decomposition by Sulphuric Acid.PECHMANN (H. v.). Condensation Products of Quinone and Ethyl Aceto- acetate. ORNDORFF (W. R.). Decomposition of some Diazo-compounds with Formic and Acetic Acids.JENTZSCH (h.).Chrysoidincarbamide Amidophenylenecarbamide.PECHMANN (H. v.) and I(. WEHSARG. Hydrazoximes. DECKER (H.). Ethyl Phenylhydrazineacetylacrylate. KNECHT (E.). Theory of Dyeing. phenone.ARONSTEIN (L.) and A F. HOLLEMANN. Stilbene. KYM (0.). Thio-derivatives of P-J)inephthglamine. EKSTRAND (A. (3.). Naphthoic Acids. FORSLING (S.). P-Chloronaphthaleneaulphonic Acid. SCHALL (C.) and G. DRALLE. Brazilin. HOLLEMANN (A. F.). Product of the Action of Nitric Acid on Aceto- CLAUS (A.) and E. FOHLISCH. Consecutive Duryl ;Methyl Ketone.AUWERS (K.) and V. MEYER. Action of Heat on Benzildihydrazone.DACCOMO ((3.).Filicic Acid.KOBERT (R.) Quillajic Acid.CONTENTS.xv ii PAGE BISCHLER (A.). Condensation Products from Bases of the Para-series with Para- and Meta-nitrobenzaldehyde. ABENIUS (P.W.) and 0.WIDMAN.Halogen-substituted Acetamido-deriva- tives of the Aromatic Series.ABENIUS (P.W.) and 0.WIDMAN.Action of Bromine on Orthaceto- toluidide a t a High Temperature. JACOBSON (P.). Phenylenediazosulphide. NOLTING (E.) and T.STRICKER.Azo.xylenes Diamidodixylyls and the Colouring Matters derived therefrom. KOSTANECKI (S.v.).Nitroso-derivatives of Resorcinol-azo-dyes.KOSTANECEI (S.v.). Isomeric Phenyldiazoresorcinols.BURCHARD (0.) and A.MICHAELIS.a-Ethylenephenylhydrazine.BLADIN (J.A.). Diphenylmethyltriazole. DENIG~S (G.).Actiou of Sodium Hypobromite on Nitrogen-derivatives of the Benzene Series.MAUTHNER (J.) and W.SUIDA.Aromatic Derivatives of Oxamide and Oxamic Acid.GRAEBE (C.).Phthalimidine.GRAEBE (C.) and A.PICTET.Substituted Phthalimidines.VILLE (J.). Action of Hypophosphorous Acid on Benzaldehyde.RODSIANKO (A.). Mono- and Di-nitropmazobenzoic Acids.ANSCHUTZ (R.). Reissert’s Pgranilpyroic Acid. REISSERT (A.). Pyrsnilpyroic Acid. CLAUS (A.) and S.WYNDHAM.MAUTHNER (J.) and W.SUIDA.Phenylglycinorthocarboxylic Acid Glyco- cine-deriratives.NIETZKI (R.) and 2.LERCH.Orthonitranilineaulphonic Acid.NOLTING (E.). The Sulphonic Acid of Methyl Phenylcarbamate.GRAEBE (C.) and C.AUBIN.Diphenic Anhydride and Orthodiphenylene- ke tonecarboxylic Acid.VAN ROMBURGH (P.). Nitro-derivatives of Tetramethyldiamidodiphenyl- methane.BANDROWSKI (F.X.). EAPF (S.) and C.PAAL.HELLSTROM (P.). Derivatives of a-P-Dichloronaphthalene.ERDMANN (H.) and R.EIRCHOFF.Di-substituted Naphthalenes from the Isomeric Chlorophenylpamconic Acids. FBIEDL~NDER (P.) and P.WELMANS.Dimethyl-a-naphthylamine and Di- ethyl- a-Naphthylamine.EROHN (C.).a-Nsphtholdiazobenaene and a-Naphthylaminediazobenzene.EKSTRAND (A.G.). Naphthoic Acids. PALMAER (W.). Action of Sulphuric Acid on a-Nitronaphthalene.CLEVE (P.T.). y-Amidonaphthalenesulphonic Acid. CLEVE ( P.T.). 6-Amidonaphthalenesulphonic Acid. ERDMANN (H.). Constitution of Isomeric Naphthalene-derivatives.PESCI (L.). Dextrorotatory Terebenthene. KACHLER (J.) and F.V.SPITZER.Hydroxycamphoronic Acids.KORNER (G.). Syringin.COTTON (S.). Arganin.CAZENEUVE (P.) and L.HUGOUNENQ.Homopterocarpin and Pterocarpin from Red Sandal Wood.LADENBURG (A.).Dipicolylmethane. GARRET (J.C.). The Two Bidesyls. BACHBR (F.). Methylstilbazole and its Reduction-product8.PLATH ((3.). P-Ethyl-a stilbazo!e and its Derivatives. NOLTING (E.) and J.FRUHLING.Paraxyloquinolinesulphonic Acid.GOLDSCHMIEDT (G.). Isoquinoline. JOHNSON (G.S.). Creatinines.STRANSKY (A.). Bases formed by the Action of Potash on Additive Pro- ducts of Papaverine.Nitro-derivatives of Isophthalic Acid.Action of Primary Aromatic Amines on Benzil.Derivatives of Ethyl Phenacylbenzoylacetate VOL.LVI.b 133 134 134 135 135 137 138 138 138 139 139 140 141 141 141 142 142 142 143 144 144 145 146 147 147 149 150 150 152 152 153 154 155 156 157 158 159 160 160 161 162 162 163 164 165 165 166CONTENTS.xix BALBIANO (L.).Trimethylenephenylimine. RWGHEIMER (L.).Hippuroflavin.WEISE (W.G.M.). Derivative3 of Diphenjlacetaldehyde.HERZIG (J.) and S.ZEISEL.Passivity of certain Yolyketones towards Hydroxylamine and Phenylhydrazine. MILLER (J.A.). Nitriles.SBNKOWSKI (M.). Derivatives of Metamethylphenylacetic Acid.TAKAHASHI (D.). Scopoletin.LE BLANC (M.). Homo-orthophthalic Acid. KOTHE (R.). Syntheses of Dialhylphthalides. DITTR~CH (A.) and C.PAAL.y-Ketonic Acids. ANSCHUTZ (R.) and F.HENSXL.Reissert’s Deoxypyranilpyroic Dibromide and Bromodeoxypyranilpyroic Acid. FEEE (A.) and H.MULLER.Dyes from Diamidoethoxydiphenylsulphonic Acid. WOLFF (L.). Indolc-derivatives.TRENKLEE (B.). Indolee.PETIT (P.). Decomposition of Benzidine Hydrochlorides by Water.HOOKER (S C.).Similar R. eactions of Carbnzole and Pyrolline.MANNS (A.). Malachite-green and Derivatives of Paramidodiphenylme- thane. WISLICENUS (J.) and A.BLANK.Arrangements of the Atoms in Space Members of the Stilbene-group. KUNZE (E.). Nitroparadiphenols.ALBRECHT (K.). New Method of Formation of Benzhydrol-derivatives.JAPP ( F.R.) and F.KLINQEMANN.Formation of Henzaniarone.ERDMANN (H.). Constitution of certain Dichloronaphthalenes.ZINCKE (T.) and 0.KEGEL.Action of Chlorine on ,8 .Naphthol.WITT (0.N.). Reduction Products of the Azo-dyes of the Naphthalene Series. WITT (0.N.). Constitution of P-Naphthol-a-Sulphonic Acid.FORSLING (S.). Action of Fuming Sulphuric Acid on Bronner’s P-Naph- thyvltimine-~-Sulphonic Acid.LUCK (E.). Filicic Acid.BOUCHARDAT (G.) and J.LAFONT.Trantlformation of Terpilene into Xenthene.LANDSBERG (M.) Essential Oil of Daucus carota.OLIVERI (V.). Constitution of Quassin. POXERANZ (C.). Methysticin.PLUQGE (P.C.) and H.G.DE ZAAYEE.Andromedotoxin.QCHUNCK ( E ).Chlorophyll.HINS BERG (0.). Hydroxy quinoxalines. CLAUS (A.) and G.N.VIS.Metabromoquinoline. WILLIAMS (G.). Cerinm Quinoline Nitrate. SEUTTEB (E.v.). Additive Product of Pttpaverine with Orthonitrobenzyl Chloride.SKRAUP (Z.H.). Constitution of Cinchona-derivatives.JOHANNY ((3.) and S.ZEISEL.Colchicine. EINHORN (A.) and 0.KLEIN.Action of Acid Chlorides on the Methyl Salts of Ecgonine Hydrochloride. LIEBERMANN (C.). Cinnamylcocalne. FRAQNER (K.). Imperialine.H OPPE-SEYLEB (F. ).Humous S uhstances. PELLIZZARI ((3.). Cholamide and Hippuramide.LEHMARN (V.). Chinethionic Acid. VAEET (R.). Action of Mercuric Cyanide on Cupric Salte.MARLA (F.). New Compound of Potassium Iron and Cganogen.MEYER (E.v.). New Method of obtaining Cyanethine and similar Bases.FAVOESKY (A.). Action of Alcoliolic Potash on Allylene.BARBIER (P.). Phthaliniidine and Methylphthttlimidine.h 2 PAGE 252 252 253 253 254 254 255 255 256 257 257 258 258 259 259 260 260 261 261 262 263 265 265 265 270 275 2’75 276 276 277 278 278 278 279 280 280 281 281 281 292 283 283 234 285 286 286 359 359 360 360CONTENTS.xxi PAGCB KNORR (L.).Hydrolysis of Ethyl Diacetosuccinate. Acetonylacetone. and Diacetosuccinic Acid.HILL (H.B.) and W.PALMER.CIAMICIAN (G.). Physical Properties of Benzene and Thiophen.MEYER (L.). Nitration.VOSWINKEL (A.). Orthodiethylbenzene. WEYL (T.).Creolin.CLAUS (A.) and J.HIBSCH.Metacresols. SCHWEITZER (W.). Derivatives of Hydroxyquhob. LEVY (S.) and E.JEDLICKA.Products of Decomposition of Chlor. Brom. and Nitr-anilic Acids.PALNER (A.W.). Pentamidotoluene. HINRICHSEN (W.). Metaxylylamidomethane. RWGEEIMER (L.). Dibenzamidodihydroxytetrene. JANOVSKY (J. V.) and K.REIMANN.Two Isomeric Azoxytoluenee derived from Paranitroluene.MARCKWALD (L.). Derivatives of Phenylhydrazine. CUXTIUS (T.) and R.JAY.Condeneation Products of. Hydrazine with Alde- TRAUBE (W.). Additive Compounds of Cyanic Acid. NOYES (W.A.). Oxidation of Benzene-derivatives with Potassium Per- manganate.LIEBERMANN (C.) W.DROILY and 0.BERGFAMI.y- and 8-Isatropic Acids EINEORN (A.) and C.GEHRENBECK.Paranitrophenylbutinecarboxylic Acids.LIMPBICHT (H.).Hydrazinesulphonic Acids and Triazo-compounds.POLIS (A).Aromatic Lead Compounds.DENNSTEDT (M.).Conversion of Pyrroline-derivatives into Indole-deriva- tives. SCHUTZ (H.). Derivatives of Paradiphenol. AUWERS (K.) and V.MEYER.Isomerism of the Benzildioximes.ONUFBOWICZ (S.). &Naphthol Sulphide. MELDOLA (R.). Evidence as to the Quantivalence of Oxygen derived from. KLINGER (H.). Action of Sunlight on Organic Compounds.WEBSTEB (C.S.S.) and L.GI.HUNT.LIEBERMANN (C.) and L.SPIEQEL.Chrysene Hydrides.SHKATELOFF (V.). Chemical Composition of the Russian White Resin from Pinus sylvestris.CIAMICIAN ((3.) and P.SILBER.Apiole. ARNAUD.Crystalline Compound from glabrous Stmphantus.TANRET (C.). Ergosterin.MAGNANINI ((3.). Derivatives of Metadimethylpyrroline.KNORX (L.) and H.LAUBMANN.Pyrazole and Pyrazoline.DOBNER (0.1.a-Alkglcinchonic Acids and a-Alkplquinolines.DOBNER (0.) and P.KUNTZE.a-Phenylnaphthacinchonic Acids.PFITZINQER (W.1. Quinoline-derivatives of Isatinic Acid.HANTZSCH (A.). Azoles.ARAPIDES (L.). Conversion of Ketone Thiocyanates into Oxythiazoles.AEAPIDES (L.). Isothiocyanoacetic Acid. TEAUMANN (V.). Amidothiazoles and their Isomerides.CLAUS (A.) and A.EDINGIER.Isoquinoline. COLSON (A.). Base derived from Diqiiinoline. PAUL (B.H.) and A.J.COWNLEY. KNORR (L.). Morphine.HESSE (0.). Water of Crystallisation in Morphine. ROSER (W.). Narcotine.SEVI TER (E.v.). Additive Compound of Papaverine with Phenacyl Bromide. Substituted Pyromucic Acids hydes. the Study of the Azonsphthol Compounds Action of Halogens on Rufigallol WARDEN (C.J.H.).Embelic Acid. Alkaloid from Tea 385 386 387 387 388 389 389 389 390 390 391 391 392 392 393 393 394 395 396 397 400 400 402 403 404 404 405 405 405 406 407 407 407 408 408 409 41 0 41 1 412 413 41 3 414 414 415 416 416 417 417 417 418UONTENTS.xxiii POSP~CHOFF (V.). Some Derivatives of Orthazotoluene.BISCHLER (A.). Orthonitrophenylhydrazine. ZINCKE (T.) and H.ARZBEEQER.Azimido-compounds.HIRSCH (R.). Theory of the Formation of Aniline-blue.GATTERMANN (L.) and G.WICHMANN.Aldehyde-blue.REYNOLDS (J.E.). MICHAELIS (A.). Aromatic Boron and Silicon Compounds.HONIQ (M.). Preparation of Terephthalaidehyde. ENQLER ( C.) and 0.ZIELKE.Acetophenone-derivatives.HAUSENECHT (G.). Derivatives of Phenylacetic Acid and Phenylglyoxylic Acid.LUFF (G.). Nitrohydroxycinnamic Acids. CONRAD (M.) and F.ECKHARDT.Action of Methyl Iodide on Ethyl Phenyl- amidocrotonate.ENQLER ( C.) and 0.ZIELCKE.Preparation of Nitromaridelk Acid.NEF (J.U.). Tautomeric Compounds. ULZER (l?.). Derivatives of Resorcinolsulphonic Acid. NENCKI (M.).Preparation of Tetramethyldiamidotriphenylmethane.HIRSCH (R.). Diphenyl Ether and Dinitrodiphenyl Ether.BISCHOFF (E.). Action of Nitrous Acid on Tetramethyldiamidobenzophe- none and Analogous Compounds. BISCHOFF (E.). Derivatives of Deoxybenzo‘in. STIERLIN (R.). Benziles.NIETZKI (R.) and J.ZUBELEN.Nitration of Naphthionic Acid.RABE (H.). Action of Phosphoric Chloride on B-Hgdroxynaphthoic Acid.IMMERHEISER (C.).Constitution of P-Naphthplamine-a-sulphonic Acid.PFITZINQEB (W.) and C.DUISBERG.Constitition of p-Naphthol-a-sulpho- nic Acid and B-Naphthol-a-disulphonic Acid.NIETZKI (R.) and J.ZUBELEN.6-Naphthol-a-sulphonic Acid.KRAVKOFF (N.).Unorganised Ferments. MEYEE (V.). Ring-formation with Elimination of a Nitro-group from the Benzene-nucleus.PELLIZZARI (G.). Compounds of Alloxan with Pyrazolic Bases.BAMBERGFER (E.). Reduction of Quinoline-derivatives.BISCHOFF (C.A.). Quinoline-derivatives from Ethyl Orthonitrobenzoyl- malonate.CONRAD (M.) and F.ECKHARDT.Methylquinaldone and Methyllutidone.GERDEISSEN.Metamidoquinaldine. ECEHARDT (F.).Metayuinaldineacrylic Acid and Metaquinaldinealdehyde.RHODE (G.). 2’ 3’-Dimethylquinoline. ENQLER ( C.) and A.BAUEB.Action of Acetone on Ortho- and Pam-amido- phenol. SEITZ (I?.). B.NapEithaquinaldine.IMMERHEISER (C.).Oxidation of P-Naphthaquinolinesulphonic Acid.BULACH (W.). Condensation of Paranitrobenzaldehyde with Quinaldine.KRUQER (A).The Sulphur of Prote’ids. CHITTEXDEN (R.H.) and G.W.CuMmNs.Myosin. CHITTENDEN (R.H.) and others.Caseoaes Caseln Dyspeptone and Case‘in- peptone. HERMANN (L.). Reduced HRemoglobirr. LAMBLINGF (E.). Reducing Action of Indigo-white on Oxyheemoglobiil.MACMUNK (C.A.). Pigments of the Urine. HELL (C.) and C.HAQELE. MESLANS (M.). Propyl and Isopropyl Fluorides. HOLZ (0.). Brominated Derivatives of Pseudobutylene.PWCEERT (M.).Conversion of Crotonylene Hydrobromide into Bromopseudo- butylene. WISLICENUS (J.). Arrangement of the Atoms in Space.MEYER (E.v.). Constitution of Cyanethine and its Analogue6.MEYEP (E.v.). Polymerides of the Nitriles.Silico-organic Compound of a New Type The Hydrocarbon C60H1B PAQE 501 501 501 503 503 504 505 505 505 506 507 508 508 509 510 510 510 511 512 512 513 514 514 515 5 15 515 516 517 518 519 519 520 521 523 524 525 527 527 528 530 530 530 530 531 575 575 575 576 676 577 577CONTENTS.AUWERS (K.) and V.MEYER.Two Isomeric Benzilemonoximes.BRAIJN (E.). Aldine Formation.GTJDEMAN (E.). Aldine Formation. HELL (C.). Pichtelite.FRIEDLANDER (P.) and 0.BOCKXANN.Naphthaquinonedichlorodiimide.WOLFFENSTEIN (R.). Constitution of a-Hydroxynaphthoic Acid.Constitution of Filicic Acid. BARBCER (P.) and J.HILT.Australene. JAHNS (E.). Oil of Myrtle.CAZENEUVE (P.). Nitrocamphor.CAZENEUVE (P.). Nitrophenol Isomeric with a-Nitrocamphor.CLAISEN (L.) and 0.MANASSE.HALLER (A).Normal and Acid Ethereal Salts of Uamphols.HALLER (A.).Phthalates of Camphols. GRAF (B.). Dammara Resin.REYCHLER (A.). Artificial Diastase. SCHUTT (F.).Phycoerythrin.FEHRLIN (H.C.). Bidesyls.ENGLER (C.) and W.KIBY. WOHL (A.) and W.MARCKWALD.Condensation-prodncts from Amido- acetal. KNOLL (A.). Code’ine.SKRAUP ( Z.H.). Constitution of the Cinchona AlkaloYds Quinine.SCHNIDERSCHITSCH (H.).Constitution of the Cinchona Alkalo‘ids Cin- chonidine.WURSTL (J.). Constitution of the Cinchona AlkaloYds Quinidine.GARZAROLLI-THURNLACKH (K.v.). Strychnine. FREUND (M.). Hydrastine.MARFORI (P.).Berberine.EINHORN (A.). Alkalo’ids occurring with Cocabe. MALY (E.). Oxidation of Gelatin with Potassium Permanganate.SCHWARTZ (A.). Reciprocal Action between Hemoglobin and Protoplasm.HOLTZWART (R.).Dimolecular Methyl Cyanide. WACHE (R.). Polymerides of Nitriles. MEYER (E.v.). Cyanethine and its Derivatives. PALMER (C.). Constitution of Ally1 Cyanide. DROUIN (R.). Succinamonitrile.MALBOT (H.). Preparation of Alkyl Chlorides from Alcohols.REISS (R.). Seminose.PISCHER (E.) and J.HIRSCHBERGFER.Mannose. BAITER (R.W.). Sugar-like Compound from Laminaria.HOFMANN (A.W.). KRAFFT (N.) and A.MOPE.Conversion of Palmitonitrile into Hexadecyl- amine.DE PORCRAND.Combination of Chloral with Glycol. ATJWERS (K.). Preparation of Oximes. WILLGERODT (C.) and F.DURR.Derivatives of Solid Acetone-chloroform.GROGER (&I.). Dihydroxystearic Acid. ERAFFT (F.) and H.NOERDLINGER.Boiling Points in the Oxalio and Oleic Acid Series.MASSOL.Calcium and Strontium Malonates. ZELINSKY (N.) and S.KRAPIVIN.BALLO (M ).Reduction of Tartaric Acid.BUCHNER (E.). Action of Methyl Diazoacetate on Ethereal Salts of Un- saturated Acids.SELL (W.J.). Base containine Chromium and Carbamide.GUARESCHI (J.). /3.Chloro.a.Bromonaphthalene. PAT ERN^ (E.). PAPASOGLI (G.). Spontaneous Oxidation of Essential Oils.Nitrosocamphor and Camphorquinone BISCHOP (A.W.) and L.C‘LAISEN.Camphoraldehyde.&Methyl Pyridyl Ketone Amines of the Methyl and Ethyl Series Symmetrical Dimethylsuccinic Acids sxf PAGE 611 613 613 614 614 614 615 615 615 616 816 617 618 619 619 620 621 621 621 622 623 623 624 625 626 626 626 626 627 627 628 629 629 683 684 685 686 686 687 687 687 687 688 658 689 689 689 690 690 691 692 693 694 695 QUIN~KE (F:).Aluminium &&hide.695CONTENTS.xx vii HOFMANN ((3.). Selenazole Compounds Selenocyanogen.CLAMICIAN (G.) and C.M.ZANETTI.CIAMICIAN (Q.) and F.ANDERLINI.BUCHKA (K.) and C.SPRAGUE.Direct Synthesis of Homologues of Pyrroline.Adion of Methyl Iodide on a-Nethyl- Formstion of Pyridine from Amidoazo- naphthalene.pyrroline.CLAUS (A.) and H.DECKER.y-Bromoquinoline.MAGNANINI (G.) and H.ANGELI.Constitution of Lepidine COLSON (A.). Artificial and Natural Alkalolds.DRESER (H.). Acid Nicotine Tartrate.FISCHER (0.). Harmine and Harmaline.HEME (0.). Coca Bases.LIEBERMANN (C.). Hygriue.CONINCK (0.de).Ptomalnes.MALBOT (K.). Action of Hydriodic Acid on Ally1 Iodide.JAHN (K.). Synthetical Formation of Formaldehyde.POHL (0.). WISLICEKUS (W.).Ethyl Oxalosuccinate.RIDEAL (S.). Organic Boron Compounds.LIEBERMANN (C.).Coca Bases.LIEBERMANN (C.) and W.DRORY.F- and yJsatropylcocalne Action of Acid Chlorides on Arsenic Trioxide.KLINGBMANN (F.). Action of Aromatic Amines on Acetylcitric Anhj dride.NIETZKI (R.) and H.ROSEMIINN.Oximes of Leuconic Acid and their Reduction Products.MIXTER (W.G.) and Y.KLEEBERG.Nitro-derivatives of Oxalotoluidide.JACOBSON (P.) and E.NEY.Aromatic Ozthamidomercaptans.GOLDSCHMIDT (H.) and A.GESSNER.Cumylamine.GOLDSCHXIDT (H.) and V.BADL.Diazoamido-compounds.BERNTHSEN (A.). Methylene-blne Group.SCHULZE (W.). Derivatives of Metamidobenzamide.TKJMMELEY (E.). Azo-compounds of Salicaldehyde Salicyl Alcohol and Salicylamide. GEBEK (L.). Azo-compounds of Salicylic Acid.JACKSON (C.L.) and G.D.MOORE.Ethyl Bromodinitrophenylacetoacetate WICHELHAUS (H.).Diamidobenzophenone.BECKMANN (E.). Behaviour of Ketones and Aldehydes towards Sodium in presence of indifferent Solvents.BAMBERGER (E.) and J.HOSKYNS- ABRAITATXG.1 4'-Tetrahydronaphthylene- diamine. BAMBE KGER (E.) and J.BAMMANN.1 J 4'-Tetrahydronaphthylenediamine and a-Tetrahydronaphthylamine.RUHARA (M.). Specific Volumes of Camphor and Borneo1.HINSBERG (0.). Piaselenoles. LIMBWJRG (P.). Solution and Precipitation of ProteTds by Salts.HOPPE-SEPLER (F.). Blood Pigments.HIRSCHFELD (E.). Black Pigment of the Choroid.B ~ H A L (A.). Hydrocarbons of the C,H,,- 3 Series.HITZEMANN (C.) and B.TOLLENS.Hexyl Iodide from Sorbite.HANRIOT (M.) and L.BOUVEAULT.Products of the Polymerisation of Ethyl MALBOT (H.) and L.QENTIL.Action of Zinc Chloride on I'sobutyl i c o h o i SCHOPFF (&I.). Diphenylamine-derivat ives.THOISS (G.).Adenine. Cyanide. in Presence of Hydrochloric Acid.LIPP (A.). Normal Acetopropyl Alcohol.LAMBERT (A.).Action of Borax on Polyhydric Alcohols.HEFFTER (A.). Action of Chloral on Glucose.PBRIEB (L.).' Solubility of Sugar in Water.BEYTHIEN (A.) and B.TOLLENS.Compounds of Ra5nose with Bases.896 PAQ E 726 727 728 728 728 '729 729 730 730 '731 '732 '732 733 '733 '766 766 767 767 768 '769 769 '771 '771 772 773 774 775 778 779 780 '781 '781 781 782 782 785 785 '786 7u7 '787 788 839 841 841 842 843 845 845 846COXTENTS.xxix KOSTANECKI (S.v.). Nitroso- and Dinitroso-naphtharesorcinol.BAMBERGER (E.) and R.MULLEB.BAMBEEGER (E.) and H.HELWIU.BAMBERGEE (E.) and W.J.SCHIEFFELIN.Reduction of Alkjl-~-naphth-ylamines.Reduction of Secondary and Tertiary Alkyl-naphthylamines.Hy$rogenation of 1 2- and 1 4- Naphthylenediamine Preparation of 2 2 -Naphthylenediamine.RUEFF (L.). P.Dinaphthylparaphenylenedianiine.FORSLING (S.)./3-Bromonaphthalenesulphonic Acids.HALWARTEN (F.). Propyl-derivatives of Anthranol.BOUCHARDAT ((3.) and LAFONT.Action of Heat and Acetic Acid on French Essence of Terebenthene. F’LIEDEL (C.). Mesocamphoric Acid.KOWALEWSKY (N.). Action of Ozone on Guaiacum Resin.ARNAUD.Tanghinin from Tanghinia Yenenifera.MACCHIASI (L.). Xanthophjllidrin.MAGNANINI ((3.). Behaviour of Pyrroline and its Derivatives as regards Raoult’s Law. LELLM A NN (E.).ConiwYns. LEZLMANN (E.) and R.SCHWADERER.LXCLLMANN (E.). Pdyrnerisation of Compounds containing doubly-bound Carbon-atoms.BUNZEL (H.). Oxidation of a-Pipecoline.LELLMANN (E.) and C.SCHLRICH.Formation of Colouring Matters from Paradiamidodiphenylpiperazine.LELLMANN (E.) and H.REUSCH.ENORR (L.). Morphine. JUNGPLEISCH (E.) and E.LBGER.a-Hgdroxycinchonine.HESSE (0.). New Compounds of the Cinchona Alkaloids.FREUND (M.). Hydrastine. EINHOBN (A.). Conversion of Anhjdroecgonine into Pyridine.KRUGEE (A.). Chemistry of Gluten.NEUMEISTEE (x.). Products of the Action of Superheated Steam on Fibrin. ROMANIS (R.). Burmese Petroleum.Q-USTAVSON (G.) and N.DEMJANOFF.Pentamethylene and Tetramethylene Bromides. B~HAL (A.). Formation of Hexylacetylene from Methylvaleryl-Acetylene RAMMELSBERG (C.).Ferricyanides.WILM (T.). Derivatives of Potassium Platinocyanide.SMOLKA (A.) and A.FEIEDREICH.WILL (W.) and C.PETERS.Oxidation of Rhamnose (Isodulcitol).WEDENSKY (W.).PLATH ((3.). @Ethyl-ci-Stilbazole and its Derivatives.PipeTide‘ine and Dipiperide’ine Quinoline and Tetrahydroquinoliiie MERCK (E.). Meconarceihe and h’arce’ine Meconate.STOEHR (C.). Constitution of Ecgonine.OTTO (R.). Discovery of the Normal Tricyanides.KRAFFT (F.). Synthesis of Cpanphenin.GARZINO (L.). Bromotrimethyl Carbinol.EEWIG (E.) and W.KOENIGS.Pentacetyldextrose.SCHEIBLER (C.) and H MITTELYEIER.Melitose (Raffinose).VAN DEE ZAHDE (K.H.M.). Diisopropglamine.ZINCKE (T.) and 0.KEUEL.Symmetrical Tetrachloracetone.MAQTJENNE.Preparation of Concentrated Formic Acid.HAZTJRA (K.). Drying Oils. Derivatives of Cyanamide.Action of Ethyl Iodide and Zinc on Paraldehyde.GRUSSNEE (A.) and K.HAZURA.Oxidation of Unsaturated Fatty Acids.HELL (C.) and S.TWERDOMEDOFF.Derivatives of Myristic Acid.FEIST (F.).Dehydracetic Acid.OTTO (R.) and J.TROGER.Synthesis of ietonic Acids by the Action of Acid Chlorides on Propionitrile.CASTELAZ (J.). Manganese Oxalate.PAGE 887 888 891 892 894 894 894 895 898 900 900 900 901 901 901 901 903 904 904 9u5 905 906 906 908 908 908 909 910 910 949 950 950 950 950 951 351 951 951 931 932 952 953 953 954 955 955 956 9 56 956 957 957 967CONTENTS. xxxi ERWIB (E.) and W.KOENIGS.Acetyl-deriratives of Quinic Acid.REMSEN (I.) and A.R.L.DOHME.Orthosulphobenzoic Acid and its Derivatives OTTO (R ) and A.ROSSING.Behaviour of Alkyl-halogen Compounds towards KEHRMANN (F.). Iodophenolsulphonic Acid Iodophenone.Ethyl Sodophenylsulphonacetate.OTTO (R.) and A.ROSSINQ.Short Communications.JACOBSEN (0.). Action of Sulphuric Acid on Symmetrical Bromopseudo- cumene.KURZEL (C.). Action of Sulphuric Acid on Symmetrical Iodopseudo- rumene. NIEMENTOWSKI (S.) and B.ROZANSKI.Synthesis of Isatoic Acid.ELBS (K.) and 0.HOLRMANN.Diphenoltrichlorethane and Paradihydroxy- stilbene.BBHAL (A.). Conversion of Methylbenzylidene Chloride into Triphenyl- benzene. BICKEL (H.). Derivatives of Diphenylacetic Acid and of Benzilic Acid.HOOKER (5.C.) and W.H.GREENE.Constitution of Lapachic Acid and its Derivatives.BAMBERGER (E.) and S.WILLIAMSON.Hydrogenation of ,tl.l)iethylnap h. thy lamine. Camphor and Borneol of Rosemary Separation of Camphor and Borneol.Acetates and Benzoates of Active and Racemic Camphols.Preparation of a Dextro-borneol identical with Dryobalanops Borneol.BRUNNER (K.). Quinol and Quinone of Ditolyl.EKBOM (A.) and R.MAUZELTTJS.Fluoronaphthalenes. EHRLICH (h;.). Oxidation oi @-Naphthol. MauzELIUs (R.). 1 4-Fluornaphtl~alenesulphonic Acid.HALLEB (A.).HALLER (A.). LEUCKART (R.) and H.LAMPE.Dibornylaniine. BARTH (L.) and J.HERZIG.Constituents of Herniaria SCHALL (C.) and C.DBALLE.Brazilin. PINNER (A.). Amidinev and Pyrimidines. PINNER (A.). Pyrimidines (Metadiazines). BISCHOFF (C.A.) and 0.NASTVOGEL.Ketopiperazines BISCHOFF (C.A.) and 0.NASTVOQEL.a-y-Diketopiperazines NASTVOGEL (0.). Homologues of Dipheny1.a.y.diketopiperazine.HAUSDORFER (A.).Diphenyl-a-y- and -a-&diketopiperazines.BTSCHOFF (C.A.) and 0.NASTVOGEL.a-P-Diketopiperazinps.BISCHOFF (C.A.). Piperazines.BISCHOFF (C.A.).Hydrogenated Paradiazines of the Aromatic Series.BISCHOFP (C.A.). Characteristics of the Piperazines. TAFEL (J.) and A.NEUGEBAUER.Methglpyrrolidine. GOLDSCHMIEDT (G.) and H.STRACHE.Pyridineorthodicarboxylic Acid.KRAFFT (F.) and I.MAI.Myristic Aldehyde. VAN DER KOLF (A.P.) and P.H.VAN LEENT.Ethyl Cinchonate and Cin- chonamide.LEIPEN (R.). Caffei'ne.SKRAIJP (2.H.) and D.WIEGMANN.Morphine. EINHORN (A.). Ecgonine and Anhydroecgonine. OUDEMANS (A.C. jun.). Cupre'ine. LADENBURG (A.) and C.OELSCHLAGEL.Pseudephredine.LIEBEBMANN (L.). Nucle'in.SUILLIOT (H.) and H.RAYNAUD.Manufactureof Iodoform.OSSIPOFF (I.). Chlorination of Ethyl Acetoacetate. MICHAEL (A.). Geometrical Constitution of the Crotonic Acids and of their Halogen Substitution-products. NICHAEL (A.) and P.FREER.Action of Hydriodic Acid on thecrotonic Acids DBECHSEL (E.). Decomposition Products of Case'in.MONNET.Reduction of Copper Salts by Sugars. LASSAR-COHN.Electrolysis of Organic Potmsium Salts.PAQE 991 992 993 994 994 994 995 996 996 997 998 999 999 999 10cu) 1001 1001 1002 1002 1003 1003 1004 1004 1005 1009 1009 1010 101 1 1012 1013 1015 1015 1015 1016 1017 1017 1017 1018 1018 1018 1020 1021 1021 1055 1055 1056 1056 1057 1057CONTENTS. xsxiii PAQE FISCHER (E.) and J. MEYER. Oxidation of Maltose. 1132 BAUER (R. W.). Fehling’s and Sachsse’s Solutions. 1132 GUIGNET (C. E.). and Mannitols.,.1133 GABRIEL (S.). Bromethylamine. -. 1134 VILLE (J ). Dihydroxyphosphinic Acids.,.1134 KLINGER (H.) aud A. MAASSEN. Sulphines and the Valency of Sulphur.1135 BAUMANN (E.) and A.KAST. Disulphones. 1136 WEDENSKY (V.). Action of Ethyl Iodide and Zinc on Paraldehyde.1136 LEVY (S.) and A. CURCHOD. SymmetAcal Tehchloracetone.1136 PECHMANN (H. v.). Reduction of DiacetyE. 1137 PECHMANN (H. v.) and R. OTTE. Homologues of Diacetyl.1137 KNORR (L.). Preparation of Acetonylacetone from Ethyl Diacetosuccinate.1139 DUVILLIER (E.). Diethsmido-a-propionic Acid.,.1139 KOLOTOFP (U. C.). Nitro-compounds of the Fatty Series.1140 DE WILDE (P.) and A. REYCHLER Acid. 1140 REYCHLER (A.). Conversion of Erucic Acid into Behenic Acid.1140 SCHULZ (0.). Molecular Weight of the Acids of the Olerc Series.1140 MICHAEL (A.). saturated Acids.1140 HELD (A.). Derivatires of Ethyl Acetocyanacetate. 1141 OELKERS (L.). Oxamic Acid.1148 EPHRAIM (J.).Dithioxamide (Cyanogen Disulphydmte). 1142 TIENANN (F.). Amidoxime of Oxalic Acid. 1142 FEANCHIMONT (A. P. N.) and E. A. KXOBBIE. Organic Compounds.1143 FRANCHIMONT (A. P. N.). of Organic Compounds with Nitric Acid. 1145 AUWERS (K.) and V. MEYER. Tetramethylsuccink Acid.1145 SEMENOFF (V.). Fumaric and Male’ic Acids. 1146 FITTIG (R.) and G. PARKER. Acids. -. 1146 URWANTZOFF (L.). Osidation of Erucic Acid. 1146 GERNEZ (D.). Action of Malic Acid on Ammonium Molybdate.1147 DIEFF (V.). Oxidation of Ricinoleic Acid. 1147 BAEYER (A.) and W. A. NOYES. Succinosuccinic Acid ,.1147 MILLER (W. L.). Dihydroxytartaric Acid. 1149 FISCHER (E.). Reduction of Acids of the Sugar-group I.1149 HUQOUNENQ (L.).Perchlorination of Phenol. 1146 MESSINQER (J.) and G. VORTMANN. New Class 0-f Iodated Phenols.1150 COLSON (A.).Dyes derived from Benzidine. 1152 SKRAUP (2. H.). Benzoyl-compounds with Alcohols Phenols and Sugars.1152 MARQULIES (0.). Hexamethylphloroglucinol. 1153 BAEYER (8.) and E. KOCHENDOERFER. Cntecholphthalek.1153 VAN ROMBURQEI (P.).Tetranitrophenylmethylnitramine and its Conversion into Metaphenylenediamine-derivatives. 1154 KEHRMANN (F.). Oxidation of Aromatic Diamines. 1154 BECHHOLD (J.).Converaion of Phenylazoresorcinol Ethers into Hydroxy- quicol-derivatives.1155 CULMAN (C.) and I(. GASIOROWSPI. Action of Stannous Chloride on Salts of Diazo-hydrocarbons and some Reactions of Diazoimido-lijdrocarbons 1156 CTJRTIUS (T.). Substitution of the Azo-group for Ketonic Oxygen.1157 MICHAELIS (A.). Sodium Phenylhydrazine. 11 58 PHILIPS (B.).Action of Alkjl Bromides and of Benzyl Chloride on Preparation of Unsymmetrical Secondary Action of Acid Chlorides and Anhydrides on Sodium Birotation of Arabinose and its Reducing Value with Combinations of Cupric Oxide with Starches Sugars Conversion of Ole’ic Acid into Stearic Regularities in the Addition of Halogen-compounds to Un- Action of Nitric Acid on Influence of Certaim Groups on the Behaviour Condensation of Ketonic Acids with Ribasic Sodium Pheny lhy drazine. Phenylhydrazines.1158 Phen ylhydrctzine.115 9 SCHMIDT (F.). VOL. LVI. CCONTENTS.xxxv AUWERS (K.) and V.MEYER.CAZENEUVE (P.). Oxidation of Nitrocamphor in presence of Light.CAZENEUVE (P.). Nonochlorocamphor formed by the Action of Hypo- chloroua Acid.CAZENEUVE (P.). Isomeride of Bromocamphor.HALLER (A.).Camphor-deriratives. HALLEB (A.). Influence of Solvents on the Rotatory Power of Isocamphols GLADSTONE fJ.H.) and W.HIBBERT.Molecular Weight of Caoutchouc and Collojid Substances.LETELLIER (A.). Colouring-matter of Purpura lapillur.CIAMICIAN (G.) and C.U.ZANETTI.Conversion of Homolowes of Pyrro- Oximes of Phenanthraquinone VULPIUS (G.)- Terpin Hydrate.\ I . line into Tetramethvlenediamine. DENNSTEDT (M.) and A.LEHNE.DENNSTEDT (M.). Dimethylpprrolines. ~ E N N S T E D T (M.). Dimethylpyrrolines in Dippel’s Oil.RUGHEIMER (L.). KUHLING (0.). Derivatives of Pyrrolidone. BLAU (F.). Preparation of Mono- and Di-Bromopyridine.DOBNER (0.) and P.KUNTZE.2 6-Diphenylpyridine.BLAU (F.). Distillation of the Salts of Pyridinecarboxylic Acids.HERSTEIN (B.).ALT (H.).Quinoline.BUCHNER (E.). Isomeride of Glyoxaline. BALBIANO (L.).Monosubstituted-derivatives of Pyrazole.KNORR (L.). Syntheses in the Oxazine Series.FREUND (M.) and S.LACHMANN.Hydrastine.FREUND (M.).Hydrastine. AHRENS F.B.Mandragorine. WRAXPELMEYER (E.). Thc Existence of Avenine.MEYET.Crystallised Hemoglobin. SCEROTTER (H.). Ethereal-derivatives of Albuminoiids.2- and 3-Methylpyrrolines Action of Sodium I<thoxide on Ethyl Hippurate Truxillopiperidides and Truxillopiperididic Acids Physiological Chemistry.HALLIBURTON (W.D.). Nature of Fibrin Ferment.KRAUSS (E.). ’Glycogen in Muscle after Section of the Nerve and Tendon.SALOMON (G.). Lactic Acid in the Blood. HARRIS (V.D.) and H.H.TOOTH.Micro-organisms and Proteolytic Digestion.LEUBE (W.). (31 co en in Diabetic Urine.HALDANE (J.S.).’ Agromatic Substances in Febrile Urine.DUBOIS (R.) and L.VIQNON.Physiological Action of Yara- and Meta- phen ylenediamine.LOEB (J.). Influence of Light on Oxidation in Animals.MAYER (A.). Melting Point and Chemical Composition of Butter as affected by Xutrition.N EISSER (E.). Glycogen.PFLUGER (E.). Synthetical Processes in the Animal Organism.ELLENBERGEB and HOFMEISTEB.The Sugar-contents of the Horse’s Stomach. GIRARD (H.). Post-mortem Formation of Sugar in the Liver.KUHN.Aqueous Humour.GLEISS (W.). Lactic Acid in Pale and Red Muscle. SOXHLET Citric Acid in Caws’ Milk. NASSE (0.). Primary and Secondary Oxidation. HIRSCRFELD (F.). Protejid Metabolism in Man. c 2 the PAGE 1201 1202 1203 1203 1204 1205 1206 1207 1207 1208 1209 1209 1809 1210 1211 1212 1212 1212 1213 1214 1214 1215 1218 1220 1221 1222 1223 1223 1224 63 64 64 64 65 65 66 172 172 173 174 174 174 176 176 177 177 178CONTENTS.xxxvii CHITTENDEN (R.H.) and J.A.BLAKE.Influence of Arsenic and Antimony on the Glpcogenic Function of the Liver.CHITTENDEN (R.H.) and A.LAMBERT.Physiological Action of Uranium Salts.CHITTENDEN (R.H.) and C.NOERIS.Relative Absorption of Nickel and Cobalt Salts.WEYL (T.). Physiological Action of Antharobin and Chrysarobin.BROWN-SBQUARD and D’ARSONVAL.Poisonous Effect of Expired Air.BRASSE (L.). Influence of Temperature on the Tension of Dissociation of 0 xy herno globin.BRUNTON (T.L.) and T.J.BOKENHAM.Action of Hydroxylamine and Nitrite& on Blood-pressure.ZECHNISSEN (H.). Conversion of Starch in the Human Stomach.VOIT (E.).Formation of Glycogen from Carbohydrates.POPOFF (N.). BRINCK (J.). Synthetic Action of Living Cells. LUKJANOW (S.M.). Relation of Water and Solid Constituents in the Organs. LEVY (L.). Muscle Pigments.DE REY-PAILHADE (J.). Attraction of Animal Tissues for Sulphur.SOLDNER (F.). The Salts of Milk and their Relation to the Behaviour of Case’in. WERTHEIMER (E.) and E.MEYER.Oxyhaemoglobin in the Bile Spectro- scopic Characters of Bile.BAELDE (A.) and H.LAVRAND.Biliary Acids in Urine during Jaundice.ENGEL and KIENER.Urobilinuria and Icterus. JAKSCH (R.v.). The Urine in Melanuria. IJADD (E.F.). Artificial versus Animal Digestion. BOAS.Free Hydrochloric Acid in Gastric Juice. BOURQUELOT and TROISIER.Assimilation of Milk-sugar.FREAR (W.).Digestibility of Soiling Rye. TORRING (H.v.).Amount of Glycerol in the Residuary Liquors of Brandy Distillation.MORNER (C.T.). Chemical Composition of Cartilage. BAMBEROER (E.) and W.FILEHNE.Relations between the Physiological.BUNGE ((3.). Amount of Iron in Fcetal Tissues. SCHINDLEX (S.). Adenine Guanine and their Derivatives.COPEMAN (S.M.) and W.B.WINSTON. HALLIBTJRTON ( W.D.). Cerebrospinal Fluid. WALTER (G.). Cyst of Protopterns Aunectens. ZUNTZ (X.) c.LEHMANN and 0.HAGEMANN.Change of Substance in the. EWALD (A.). Digestion of Elastic Fibres and Allied Structures. JOXDAN (W.A.) J.M.EARTLETT and L.H.MERRIL.Composition and Digestibility of some Foods with Observations on the 1)etermination of Digestibility of Protei’n and Carbohydrates.GRBRANT and QUINQUAUD.Amount of Urea in Blood and Muclcle.VIETH (P.).Composition of Milk produced in English Dairy Farms.STIFT.Influenceof “Saccharin” on Digestion.PLANTA (A.v.). Food of the Larval Bee. LADD (E.F.). Influecce of Food on the Composition of Butter. ALBEELTONI (P.). Action of Carbohydrates on the Animal Organs.MIDDENDORFP (M.v.). HEemoglobin in Blood passing to and from the Formation of Serum Albumin in the Alimentary Canal and Tissues in Normal and Starving Animals Properties and Constitution of’ Hydrogenised Bases HumanBile Horse a t Rest and a t Work Liver and Spleen. MACMUNN (C.A.). Myoheematin. MARTIN (S.). Prote’id Poisons.UDRANSZKY (L.v.) and E.BAGMANN.Diamines (Ptomaynes) in Cjstinuria LUFF (A.P.). Relations of Ptoma’ines to Infectious Fevers. FJORD (N.J.). Feeding of Milch Cows.PAGE 537 537 538 539 629 630 630 63 1 631 632 632 632 633 63 3 634 636 637 637 637 7J4 734 ’735 735 735 736 737 789 790 792 793 793 y11 912 913 914 914 1028 10.2 1023 1023 1023 1024 1024 1026 1026 1076CONTENTS.xxxix L ~ V Y (A.). Composition of Rain-water .BELLUCCI (G.). Salt in Rain-water. FOBBE (F.). American Red Clover. HEIDEN (E.). Value o€ Basia Slag as a Manure compared with Soluble Phosphate and Bone-meal.HEIDEN (E.). Manuring Experiments in Hemy Soil.SEBELIEN (J.Influence of the Concenhration of the Cream in Butter Making.WEIGERT (L.). Influence exerted by Salicylic Acid on the Proportions of Glycerol and Alcohol formed in Wines. HECKEL (E.) and F.SCHLAGDENHAUFFEN.DE MONDESIR (P.). Legurninow in ,4 cid Soils.RATTLIN (J.). Phosphates and Ceredb. SCHNEIDEE (E.A.).Analysis of a Soil from Washington Territory.LADUBEAKJ (A.). Algerian Soils.DELACHARLONNY (P.M.) and L.DESTEEMX.Action of Ferrous Sulphst? in rarious Soils. BAESSLER.Comparative Manurid Value of the NitrageB in Sodium Nitrate and Ammonium Phosphate. PETERHANN (A.). Bat's Guano from Cuba. GR%HANT and QUINQUAUD.Disengagement of Carbonic Anhydride by Anaerobic Yeast. BWET (V.) Cornpositmion of the Bmillus from Erythema lzodosum.SCHULZE (E.).lteserve Materials especially Starch Tannin contained in Evergreen Leaves. SCHULZE (E.). Reserve Substances in Evergreen Leaves. RODEWALD (H.). Tramsformation of Force and of Material in Plant Respi- ration.POLLAK (E.). Absence of Nitric Acid in Wine Must.EBERMAYER (E.). Absence of Nitrates in Forest Trees.HOOPER (D.). Laurel-nut Oil.GANS (R.) and B.TOLLENS.Quince and Salep Mucus.LIDOFB (A.). Tmnic Acid in Caucasian Wild Sumach. DEHBRAIN (P.P.).Field Experiments. at Grignon in 1888-. DE MONDESIR (P.). Calcium in Soils. EGQERTZ (C.G.). Humous Compounds in Soil.BROWN (L.P.). Analysis of Tobacco Screenings.HAMMERSC ELAG (A.).Chemical Comqosition of Bacillus Tuberculosis.SCHLOESSING (T.). Loss of Nitrogen in the Decomposition of Organic Matter. SCHLOESSING (T.). Slow Combustion of Organic Substances-. HELLRIEOEL (H.) and H.WILPARTH.Sources of the Nitrogen of the Gramineae and Legurninow.PEYBOU (J.). Variations of the Internal Atmosphere of Plants. PALLADIN (W.). Products of Decomposition of Albrimino'ids in Plants.SCHULZE (E.) and E.KISSER.Decomposition of Prote'ids in Green Plants kept in the nark.SCHULZE (E.) and E.STEIGER.Oceurrence of an Insoluble Carbohydrate in Red Clover and Lucerne. MAXWELL (W.). Soluble Carbohydrates in the Seeds of Leguminous Plants BAUDET and ADRIAN.Morphine in E'scholtzia calzfwnira. MOLISCH (H.) and S.ZEISEL.PLUGGE (P.C.). Andromedotoxin in the Ericaccoe.SCHULZE (E.) and E.STEIGER.Lecithin in the Seeds of Plants. LINOSSIER (G.). Influence of Carbonic Oxide on Germination. MUNTZ (A.). Fertilising Properties of the Water of the Nile. GEORGESON (C.C.). Manuring of Rice. LTETGEB (H.). Asparagine and Tyrosine in Dahlia Bulbs. PARSONS (C.L.). Analysis of Fruits from the Southern States Juice of Bassia latzyolia. LOEW (0.). Rble of Formaldehyde in the Assimilation of Plants. New Source of Coumarin PAGE 299 299 299 299 300 300 433 433 43 4 434 434 435 435 436 436 436 436 539 539 540 5440 540 541 541 541 541 541 541 512 543 513 638 638 639 640 640 641 642 642 643 644 644 644 644 646 645 646 646CWTESTS.xli HECKEL (E.) and F. SCHLAGDENHAUFFEN. Oleo-gum-resin Secreted by Araucarias. TTMIRIAZEFF (C.). Protophyllin in Etiolated Plants.SCHLOESSING (T.). Atmospheric Nitrogen and Vegetable Soils. BERTHELOT. Absorption of Nitrogen by Clay Soils.SCHLOESSING (T.). The Relation of Atmospheric Nitrogen to Vegetable Soils.BERTHELOT. Influence of Electrification on the Absorption of Nitrogen by Vegetable Soils. BERTHELOT. Absorption of Atmospheric Nitrogen.BERTHELOT. Evolution csf Ammonia and Volatile Nitrogen-compounds from Vegetable Soils and from Plants.SCHLOESSING (T.).Nitrification of Ammonia.PBCIIABD. Influence of Calcium Sulphste and of Clay on the Absorption of Nitiwgen. HEBERT (A.) Formation of Ammonia in Arable Soils. MULLEX (A.). Sea Sludge and its Absorpthe Power €or Lime or Potash.RAULING (G.). Phosphates and Cereds. Analytical Chemistvy. GASTINE (G.). Preparation of Starch Solution for Use in Volumetric? Analysis.BORNTRAGEB (H-). Use o€ Salicylic Acid for Preserving aandard Solutions LAMBLING (E.). Application of Spectrophotometry to Chemical Physiology JOLLES (A.). Determination of Chlorine in Plant Ashes. GETZOW (F,]. Determination of Bromine in Sea Water. LASNE (H.). Determination of Fluorine. LINOSSIER ((3.). General Method for ithe Separation and Volumetric &timation of Acids.MCGLASCHAN (J.).Volumetric Estimation of Boric Acid and of Ammonia in Ammonium Salts.LrNDo (D.). Resorciriol as a Test for Nitrates.SHIMER (P. W.). Determination of Phosphorus in I,mn and Steel.HOGQ (T. W.). CLASSEN (A.) and R. SCHELLE. Quantitative Analysis by Electrolysis.KUPFFERSCHLAEGER. Separation of Calcium Barium and Strontium.KASSNER (G.). Volumetric Estimation of Mercuric Chloride. STRENG (A). Microchemical Reactihs. HAUSHOFER (K.). Detection of Small Quantities of Germanium.LBGER (E.). Characteristic Reaction for Bismuth.WINELER (L. W.). Determination of Oxygen dissolved in Water.FLUCKIGER (F. A). Ash Determination. ME~SINGER (J.). Wet Methods of Organic Analysis.NEWBURY (S. B.) and W. P. CUTTER. Safety of Comniercial Kerosene Oils PAWLEWSKI (B.) and J. FILEMONOWICZ.Solubility and Estimation of Paraffin.TEISSIER (J.). Analysis of a Mixture of Silver Chloride Cyanide Thio- cyanate Perriqanide and Ferrocyanide.REVERDIN (F.) and C. DE LA HARPE. Determination of Paranitrotoluene HABERMANN (J.). Detection of Methyl Alcohol in Wood Spirit. ROCQUES (X.). Composition of Natural Brandies the way of distinguishing thern. BISCHOP (R. W.). Determination of Sugar in Presence of Carbohydrates.SCHWARZ (C.). Determination of Sugar in Urine.SCHWARZ (C.). Detection of Chloral or Chloroform in Liquids. MANSFIELD (M.). Modification of the Reichert-Meissl Method of Butter Analpsi s.LONG (J. H.). Densities and Refractive Indices of Oils. Influence of Sulphur on Eggertz's Carbon Colour Test PAQE 1236 1236 1237 1237 1237 1237 1238 1238 1239 1239 1240 1241 1242 73 73 73 73 74 74 75 75 75 76 76 76 77 78 78 78 79 79 80 80 88 82 83 84 84 84 85 85 85 85 85CONTENTS.xliii PAQE ERRERA (C.) Separation and Estimation of Chlorine Bromine Iodine and Cy anogen. - WATSON (J.). Estimation of Sulphur in Burnt Pyrites. ENQ-EL. Volumetric Estimation of Acids. SIDERSKY (D.). Volumetric Estimatioii of Sulphates.QUANTIN. True Rdle of Soda-lime in the Estimation of Nitrogen.SMITI~ (J. H.). New Method for the Estimation of Pr’itrogen. CLARK (J.). Estimation of Phosphoric Acid with Silrer Kitrate. BRRTHELOT and G. ANDR~. SCOTELL (M. A.). Estimation of Nitrates by Kjeldahl’s Method.LINOSSIER (G.). Estimation of Phosphoric? Acid.HOGG (T. W.)- Estimation of Carbon in Iron Steel &c. BENEDIKT (R.) and M. CANTOR. WIKKLER (C.).Estimation of the Percentage of Lead in Tin-lead Alloys by takiiig the Specific Gravity.WILLIANS (R.). Estimation of Copper by the Iodide Process. MEINEKE (C.). Separation of Manganese and Allied Metals from the Sesqui- oxide Group and Phosphoric Acid. CARNOT (A.). Estimation of Chromium by Hydrogen Peroxide. RUSAG (K.). Analysis of Commercial Scherlite.JOLLES (A.). Volumetric Estimation of Antimonious and ArRenious Acids.ENORRE (G. v.). Volumetric Estimrttior of Antimonic Acid. HOOKER (S. C.). Estimation of Nitrates in Natural Waters. MESSINGER (J.). Estimation of Acetone in Methyl Alcohol. PABCUS (E.). SIDERSKY (D.). Indirect Analysis of the Sugar-beet.PELLET (L.). Estimation of Sugar in Beet by Digestion with Water.WEISBERG (J.). BATTUT (L.). Estimation of Sugar in Beet.CLERC (M.). Estimation of Sugar in Beet. V I E ~ H (P.). Estimation of Milk-sup in Milk by the Polariscope.LINTNER (C. J.). Compounds of Starch with the Alkaline Earths.PETERS (W.). Adulteration of Vegetable Fatty Oils.FAWSITT (C. A.). Action of Sulphur Ciiloride on Oils. PLANCHON (I7.). Detection of Margarin in Butter.WILLIAMS (R.). Iodine Absorptions Combining Weights and Melting Points of some Fatty Acids.ALLEN (A. H.). Detection of Cotton-seed Oil in Lard.HEHNEK. (0.). Mixed Lard and the Detection of Cotton-seed Oil.WILLIAMS (R.). Adulteration of Lard with Cotton-seed Oil. JOKES (E. W. T.). Lard Adulterated with Cotton-seed Oil. ALLEN (A. H.). Adulteration of Lard with Cocoanut Oil. ARCHBUTT (L.). Analvsis of Grease. RAESSLER (F.). Estimkion of the Oil and Water in Linseed Cake.BUCHNER (G.).Analysis of Wax. WILLIAMS (R.). Examination of Certain Gums and Resins.ALLEN (A. H.). Detection of “ Saccliarirt ” in Beer.KREMEL (A.). Estiniation of Aikaloids in Nux-vomica. XUDDIMANN (E. A.). Estimation of Quinine by Kerner’s Blethod.1,AGORCE (E.). Detection of Cochineal in Alimentary Substances.GRIMBERT. Detection of Urobilin in Urine.W~NKLER (C.). Draught Arrangement for Water-baths. BERINQER (C. and J. J.). Volumetric Estimation of Sulphur by means of Barium Chloride. DE KONIKCK (L. L.). Estimation of Hydrogen Sulphide. LHOTE (L.). Estimation of Nitrogen by Kjeldahl’s Method. GIUNTI (M.). SPIEGEL (L.). Estimation of Nitrates in Mineral Waters. MIELCKE (W.). Calculation of Phosphoric Acid Estimations. TZSCHUCKE (H.). Direct Estimation of Phosphoric Acid as Tricalcium Phosphate ,.Estimation of Nitrogen in Vegetable Soils Volumetric Estimation of Zinc Oxide Detection of Invert-sugar in the Presence of Cane-sugar Estimation of sugar in Beet by Digestion with Water Source of Error in the Estimation of Nitrates in Soils.304 306 306 306 306 307 307 307 308 308 308 309 309 309 309 311 311 311 312 312 31 3 313 814 314 314 314 314 315 316 316 317 318 318 319 319 320 320 320 32 1 321 322 322 322 323 323 324 324 437 437 4.3 7 438 438 438 439 439CONTENTS.xlv DROWN (T.M.). Loss on Ignition in Water Analysis.BORNTRAGER (H.). Examination of Commercial Alcohol. CRISMER (L.) Detection of Sugar in Urine. VINCENT (C.) and DELACHANAL.Estimation of Sorbite. LIST (K.). Detection of Nitrobenzene in Presence of Oil of Bitter Almonds EGGER (E.).REIS (M.A.v.). Estimation of Phosphorus and Sulphur in Tron.AUBIN (E.) and ALLA.ZECCHINI (M.) and A.VIGNA.Estimation of Nitrogen by Kjeldahl’s Method ZECCHINI (M.) and A.VIGNA.Estimation of ready formed Nitrogen in Manures. FLUCKIGER (F.A.). Detection of Minute Quantities of Arsenic. KATAYAMA (K.). Test for Carbonic Oxide Poisoning in Blood. J ~ G E R (E.) and 8.KRUSS.Volumetric Estimation of Carbonic Acid.Detection of Free Sulphuric Acid in Aluminium Sulphate Estimation of Nitrogen by Kjeldahl’s Method CONINCK (0.DE).Estimation of Total Nitrogen in Urine. FRAXK (B.). Detection of Nitrates in Soil. SCHYDLOWSKI (F.). Estimation of Carbonic Anhydride in Air. KLEIN (J.). Detection of Mercury. Magnesium.BAUBIGNY (H.). Separation of Zinc from Nickel.BAUBIGNY (H.). Separation of Zinc from Cobalt.FISCHER (R.). Separation of Nickel from Cobalt.KLEIN (J.). Detection of Manganese. BLUM (L.). Analysis of Substances containing Aluminium Calcium and MARINO-ZUCO (F.).Destruction of Organic Matter in Toxicological Investi- gations.PENDRII? (M.A.). Cyanogen and its Compounds in the Products of Coal Distillation. WEIGFERT (L.). Terreil’s Reaction for Testing the Colouring Matter of Wine.PALMIEBI (P.) and F.CASOEIA.Tests for Archil Cochineal and Magenta inWine.Estimation of Raffinose in the Products of Beet-sugar Manufacture. TRAUBE (J.). Examination of Spirituous Liquids.DENIG~S ((3.). Reagents for Mercapfans. VAN ITALLIE (L.). New Test for Thymol. BORNTRAGER (H.).Characteristic Reaction for Aldehyde. GUNNING (J.W.). HEIDENHAIN (H.) Goldenberg’s Method for Estimating Tartaric Acid.BESANA (C.). Methods for Detecting the Adulteration of Butter. HIPSCHSOHN (E.). Detection of Cotton-seed Oil in Olive Oil. Cotton-seed Oil and Beef Fat in Lard BIEL (J.). Detection of Cotton-seed Oil in Olive Oil WILSON (J.A.). AMBUHL ((3.). Adulteration of Lard. UMNEY ( J.C.). Oil of Anise.SCHRODER (J.). Detection of Antifebrin in Phenacetin. Oxyhsemoglobin. L’HOTE (L.). Estimation of Orgmic Nitrogen.EDWARDS (V.). Estimation of Insoluble Phosphates.DENIG~S.Reaction for Copper.MOORE (T.). Volumetric Estimation of Nickel.CARNOT (A.). Estimation of Nickel and Cobalt.CARNOT (A.). Separation of Nickel and Cobalt. MORAWSKI (T.). A Delicat. e Reaction for Pine-wood Resin.LAMBLING (E.). Estimation of Methaemoglobin in the Presence of LONG (J.H.). Behaviour of Phenolphthalein with Ammonia. FOERSTER (0.). Estimation of Nitrogen in Nitrates by Ejeldahl’s Method.TORRING (H.+.). Estimation o l Glycerol in the Residues of Brandy Distil- lation.LEWKOWITSCH (J.). Estimation of Glycerol in Crude Glycerol.PAQE 551 5 52 552 552 552 648 648 648 649 649 649 649 650 650 651 651 651 652 652 653 653 653 653 653 654 655 655 655 656 657 657 657 658 65 8 658 659 659 659 660 660 660 746 746 746 747 747 747 747 747 748 748COXTENTS.xlvii PAUE VIGNON (L.). for Technical Purposes.1035 BERTHELOT.Estimation of Benzene Vapoiir in Coal-gas. 1036 CAUSSE (H.). Estimation of Sugar by Fehling’s Solution. 1036 PHIPSON (L.T.). Tin in Sugar.1036 LOSEKANN (G.).Estimation of Formaldehyde.1036 WoLmY (R.). Estimation of Fatty Acids from Butter. 1037 SHORT (P.G.). Estimation of Fat in Milk. 1037 WILSON (J.A.). Free Alkali of Soap. 1037 REVERDIN (P.) and C.DE LA HARPE.aniline. 3038 LUTHER (R.). TCe Knop-Hufner Method of Estimating Urea,. 1039 CAMERER (W.). 1040 BRUCKE (E.37.). 1040 NENCKI (hl.v.). Testing of Reagents Eniplojed in Elementary Analysis.1085 FOERSTER (0.). Purification of Litmus. 10% HOLBLING (V.). Volumetric Apparatus. 1g86 BAWALOVSKI (A.). Separation of Ethereal Solutions from Aqueous Liquids 1086 STEIN (W.M.) and P.w.SCHWARZ.Rapid Metbod of Anaiysing Water prior to its Softening Estimation of Aniline and Methyl- Estimation of Uric Acid in Human Urine. Van Deen’s Test for Blood ar.d Vitali’s Tesl for Pus REICHARDT (E.) and UP-MEYER.Estimation of Iodine.1086 DE LA HARPE (C.) and F.REVERDIN.Analytical Notes. 1087 Estimhon of Ammonia by Distilla- tion.1087 Q~JANTIN (H.). Volumetric Estimation of Sulphates.1087 BLUM (L.).Precipitation of Magnesia. 1087 BLUM (L.). BLUM (L.). Determination of Carbon in Iron.1098 MARTINOTTI (F.). Estimation of Nitrogen by Kjeldahl’s Method.1088 REICHARDT (E.). Elementary Analysis of Volatile Liquida. 1088 POLITIS (J.E.). Rapid Estimation of Saccharine Compounds. 1088 STEIGER (E.). Estimation of Galactose. 1059 KONIG (J.) and M.KESENER.Discrimination of Fruit and Beet Syrups.1083 LUDY (E.). Detection of Carbamide. 1090 BODD~ (H.). Detection of Resorcinol. 1090 BOURCART (R.). Milk Analysis.1090 DE VRIJ (J.C.). Quinine Sulphate.1091 EWER (E.). Indirect Estimation of Extractive Matters in Wine.1091 SOSTEGNI (L.). Detection of Foreign Colouring Matters in Wine.1091 PALMER (T.C.). Testing Logwood Extracts.1091 WHITE (J.T.). Estimation of Tea Tannin. 1092 REICHL (C.). New Reaction for Albumino’ids.1c92 COPEXAN (S.M.). Detection of Human Blood.1092 WURSTER ((3.). Naphthylamine as a Reagent for Hydrogen Peroxide in Presence of Sodium Chloride. 1242 JAKSCH (R.v.). Estimation of Free Hydrochloric Acid in Gastric Juice.1242 WURSTBR (C.). Reaction. 1243 JANKASCH (P.). Decomposition of Sulphides by Air containing Bromine.1243 JANNASCH (P.). New Method of Analysing Pyrites.1243 JANNASCH (P.). Decomposition of Pyrites iii a Stream of Oxygen.1244 JANKASCH (P.). Estimation of Sulphnric Acid in Presence of Iron.1244 LUNGE (G.).1244 PAD$ i L.). Milk.1244 DROWN (T.M.). Silicon.1245 HUGHES (J.). dnttlysis of Concentrated Superphosphate. 1245 JONES (C.). Pjg.iron.1246 Source of Error in Separating Traces of Manganese from much Lime by Ammonium Sulphide. 1087 Potassium Chromate as a Reagent for the Purity of Use of Ammonium Acetate in Detecting Nitrites by Griess’ Estimation of Sulphuric Acid in Presence of Iron. Detection and Est. imation of Sodium Hydrogen Carbonate in Estimation of Phosphorus in Iron in the Presence of Method of Rapid Evaporation for the Estimation of Silicon inJ O U R N A LC. F BAKER.H. BAKER.D. BENDIX.A. (3. BLOXAM.C. H. BOTHAMLEY.B. BRAUNEB.B. H. BROUQH.H. CBOYPTON.W. D. HALLIBURTON M.D. B.Sc.F. 5.KIPPINO Ph.D. D.Sc.J. W. LEATHER Ph.D.D. A. LOUIS.T. MAXWELL M.D. B.Sc.N. H. J. MILLER Ph.D.OFQ-. T. MOODY U.Sc.J. M. H. MUNRO D.Sc.T. (3. NICHOLSON.E. W. PEEVOST Ph.D.H. H. ROBINSON B.A.R. ROUTLEDBE B.Sc.M. J. SALTER.JAMES TAYLOR B.Sc.L. T. THORNR Ph.D.H. K. TOMPKINS B.Sc.Gt. W. DE TUNZELMANN B Sc.W. C. WILLIAMS B.Sc.W. P. WYNNE B.Sc.THE CHEMICAL SOCIETY.H. E. ARMSTBONG Ph.D. F.R.S.W. CROOKES F.R.S.WYNDHAM R. DUNSTAN.I?. R. JAPP M.A. Ph.D. F.R.S.H.MCLEOD F.R.S.A. K. MILLER Ph.D.HUGO MULLIPR Ph.D. F.R.S.W. RAMSAY Ph.D. F.R.S.W. J. RUSSELL Ph.D. F.R.S.J. MILLAR THOMSON F.R.S.E.T. E. THORPE Ph.D. l7.B.S:W. P. WYNNE B.Sc.@bitm :C. E. GROVES F.R.S.A. J. GREENAWAY.Vol. LVI,LONDON:GURNEY & JACKSON 1 PATERNOSTER ROW.LONDON :TIAIiRISON AND SONS PRINTERS IN ORDINARY TO HER MAJESTY,ST.MAILTIN’S LANEJ O U R N A LTHE CHEMICAL SOCIETY.H. E. ARMSTRONG Ph.D. F.R.S.W. CROOKES F.R.S.WYNDHAM R. DUNSTAN.F. R. JAPP M.A. Ph.D. F.RS.H. MCLEOD F.R.S.A. I(. MILLER Ph.D.HUGO MULLER Ph.D. F.R.S.S. U. PICKERITGF &LA.W. RANSAY Ph D. F R.SW. J. RUSSELL Pli D F.R S.J. MILLAR TITOMSON F R S ET. E. THOEPE Ph.D P.B S.W. P. WYNNE B Sc.&;bitw :C. E. GROVES F.R.8,Sjub-@/bitar :C. F. BAKER. G. T. MOODY D.Sc.H. BAKER. J. M. H. MUNRO D.Sc.D. BENDIX. T. (3. NICHOLSON.A. G.BLOXAM. E. W. PREVOST Ph.D.C. H. BOTIIAMLEY. H. H. ROBINSON B A.B. BRAUNER. R. ROUTLEDQE B.Sc.B. H. BROUGH. M. J. SALTER.H. CROMPTON. JAMES TAYLOR B.Sc.W.D. HALLIBURTON M.D. B.Sc. L. T. THORNR P1i.D.F. S. KIPPINQ Ph.D. D.Sc. H. K. TOMPEIXS B.Sc.J. W. LEATHER Ph.D. G. W. DE TUNZELMAXN I3 Sc.D. A. LOUIS. W. C. WILLIAMS B.Sc.T. MAXWELL M.D. B.Sc. W. P. WYNNE B Sc.N. H. J. MILLER Ph.D.VOl. LVI. Part I.LONDON:GURNEY & JACKSON 1 PATERNOSTER RCW.LONDON :HARRISON AND SONS PBINTEBS I N ORDINARY TO HER MAJESTY,ST. MARTIN’S LANEC 0 N T E N T S.ABSTRACTS OF PAPERY PUBLISHED IN OTHER JOURNALS :-General and Physical Chemistry.LIVEING (G. D.) and J. DEWAR. Absorption-spectrum of Oxjgen .TROWBRIDGE (J.) and W. C. SABINE. Metallic Spectra.BOISBAITDRAN (L. DE). Degree of Oxidation of Chromium and Manganese inFluorescent Mixtures.LINDECK (S.). Electromotive Force of Amalgams.KALISCBER (S.).Electromotive Force of Selenium.GEE (W. W. H.) and H. HOT.DEN. Reciprocal Conductivity.OSTWALD (W.). Apparatus for Determining the Conductivity of Electro-STJTHEBLAND (W.). Specific Heats at High Temperatures.MATHIAS (E.). Specific Heats of Saline 8olutions.LOUQUININE (W.). Heat of Co.iibustion of Acids of the Oxalic :ind LacticSeries.OSSIPOFF (I.) Heats of Combustion of some Organic Substances .LOUGUININE (W.). Heat of Combustion of Camphorjc Acids.WALKER (J.). Method of Determining Vapour-tensions at Low rein-RAOITLT (F. M.). Vapour-tensions of Alcoholic Solutions.LESC~EITR (H.) and D. MATHURIN. Water of Crystallisation of the AlumsWARREN (H. N.). Electrolytic Method of Liquefying Gases.AMAQAT (E. H.). Compressibility of Hydrogen Oxygen Nitrogen and AirDE VXIES (H.).Isotonic Coefficient of Glycerol.ROWLAND (H. A.) and L. BELL. Actior. of a Magnet on Chemical Action .MEYERHOFFER (W.).Accelerating and Retarding Influences in ChemicalProcesses.GIERSBACH (J.) and A. KESSLER. Nitration of Benzene.HUNT (T. S.). The Foundations of Chemistry.BECKMANN (E.). Determining Molecular Weights by Reduction of theJOFFRE (J.).NEWBURY (S. B.). Apparatus for Distillation in a Vavuum.LIVEINGC (a. D.) and J. DEWAR. Spectrum of Magnesium.LIVEING (G. D.) and J. DEWAR. Ultra-violet Spectra of Nickel and CobaltWRIGHT (C. R. A.) and C. THOMPSON. Two-fluid Cells.GORE (G.). Effect of Chlorine on the Electromotive Force of a VoltaicCouple.WRIQHT (C. R. A.) acd C. THOMPSON. Development of Voltaic ElectricityWARBURQ (E.) and F.TEGETMEIER. Electrolytic Conductivit j of RockSalt.MONCKMAR (J.). Effect of Occluded Gases on the Thermo-electric Proper-ANDHEWS (T.). Electzochemical E5ects of Magnetising Iron.HESS (H.). Specific Heat of some Solid Organic Compoiinde.VELEY (V. H.). Evolution of Gases from Homogeneous Liquids .Freezing Point.Resistance to Light of Colouring Matters fixed in l'isstiesPAQE:?,10I:!S:)! )OANDREWS (T. the late). Properties of Matter in the Gaseous and LiquidState under various Conditions of Temperature and Pressure .FUCHS (F.). Behaviour of certain Gases at Low Pressures in Relation toRUDORFF (F ). Constitution of Solutions.LUDEEING (C.). Physical Properties of Colloid Solutions.NASSE (0.).Precipitation of Collo‘id Substances by Salts.UROSHAXS (J. A.). Formula for the Molecular Volumes of Compounds atPAT ERN^ (E.). Molecular Lowering of the Freezing Point of Benzene byPhenols.HASCHEK (A.). Refractive Indices of Turbid Media.EETTELER (E.). Refraction of Liquids within Wide Limits of TemperatureKNOPS (C.). Molecular Refraction of Fumaric Maleic Mesaconic Citra-BECQUEREL (E.).Preparation of Phosphorescent Calcium and StrontiumURIVEAUX (F.). Decomposition of the Halb’id Silts of Silver by the ActionBELLAMY (F.). Decoloration and Recoloration of Litmus Solution by LightGORE ((3.). Minimum Point of Change of Potential of a Voltaic Couple .GOZE ((3.). Change of Potential of a Voltaic Couple.GORE ((3.). Influence of the Chemical Energy of Electrolytes on theMinimum Point of Change of Potential.GORE (G.).Effects of Different Positive Metals on the Change of Poten-Ealtus (C.). Electrical Relations of the Alloys of Platinum.POHLRAUSCH (F.). Electrical Resistance of Mercury.GRUNMACH (L.). Influence of the State of Aggregation of Substances onULJANIN (W. v.). E.M.F. of Selenium.VAN’T HOPF (J. H.) and L. T. REICHER. Theory of the Dissociation ofElectrolytes.OSTWALD (W.). Electrochemical Studies.FABRE. Specific Heat of Tellurium.CAmERON (L.). Estimation of the Value of a Degree in Thermometers ofShort Range.TSCHERNAY (N.). Dilatation of Salt Solutions.ERRERA ((3.). Table of Vapour-tensions of Solutions of PotassiumHydroxide.LE CHATELIER (H.). Dissociation of Carbonic Anhydride.GOLDSTEIN (M.).Rise of Salt Solutions in Capillary Tubes.BERLINER (A.). Catalytic Action of Metals on Oxyhydrogen Bas .SPRING (W.). Metallic Lustre.BRUHL (J. W.).WEBER (R.). Ether Levels.LANGLEY (S. P.). Invisible Lunar and Solar Spectra.PITCHER (F. B.). Absorption-spectra of Blue Solutions.KANONNTKOPF (I.). Relation between the Rotatory and Refractive PowersKETTELER (E.). New Theory of Molecular Volume and Refraction .LOEB (M.) and W. NERNST. Kinetics of Substances in Solution.OSTWALD (W.). Estimation of the Basicity of Acids from the ConductivityLOUGUININE (W.).Heat of Combustion of Terpilene Terpin Hydrate andTerpin.LOEGCUININE (W.). Heat of Combustion of Camphors and Borneo18 .BODISCO (A.). Heat of Dissolution of Anhydrous Lithium Iodide .BREMER (G.J. W.). Density and Expansion by Heat of Saline Solutions .TSCHERNAP (N.). Dilatation of Salt Solutions.Boyle’s Law.Sulphides.Apparatus for Fractional Distillation in a Vacuiim .PAQE200207CONTENTS. VSCEALL (0.). Vapour-density Estimation under Diminished Pressure .MULLER-ERZBACH (W.). Water of Crystallisation of the Alums .BEEETOFF (N.). Selective Chemical A5nity.POTILITZIN (A.).Influence of Temperature on the Direction of ChemicalChange.BONZ (A.). Formation of Amides from Ethereal Salts and Ammonia andWATSON (G.). Dead Space in Chemical Reactions.BRAUNER (B.). Standard of Atomic Weights.EYKMAN (J.F.). Apparatus for Determining the Reduction of the FreezingPoint.GROSHANS (J.A.). Calculation of the Molecular Volume of Benzene,Naphthalene Anthracene &c.CIAMICIAN ((3.).Lecture Experiment on Rnoult's Law.HAWKRIDGE (P.). Lecture Experiment Volumetric Composition of certainLEONABD (N.). Blue Flame produced by Sodium Chloride in a Coal Fire .KANONNIPOFF (I.). Relation between the Rotatory and Refractive PowerSUTHERLAND (W.). Molecular Refraction.GRUNWALD (A.). Spectral Analysis of Cadmium.BOISBAUDRAN (L.DE).Gadolinium.EXNER (F.) and J.TUMA .PO IN CAR^ (L.). Electrical Conductivity of Fused Salts.HBRROUN (E.F.). Abnormal Electromotive Forces.QUINCKE (F.). Electrolysis of Copper Chloride.HENNEBERG (H.). Heat Conductivity of Mixtures of Ethyl Alcohol andWater.JOLY (J.). Specific Heats of Gases a t Constant Volume.OSSIPOFF (I.).Heats of Formation of Several Organic Acids.OSSIPOFF (I.). Heats of Combustion of Stilbene and the Isomeric Nono-ANTOINE (C.).Dilatation and Compression of Air.JAEGER (W.). Velocity of Sound in Vapours and the Determination of theVapour-density.RICHARDS (T.W.). Vapour-density Determinations.ETARD (A.). Relation between the Solubility of Salts and their MeltingPoints.HERITSCR (A.). General Law of the Diminution of Volume of Salts bySolution in Water.WINEELMANN (A.). Influence of Temperature on Evaporation and on theDiffusion of Vapours.PENDLEBURY (W.H.) and M.SEWARD.Gradual Chemical Change .URECH (F.). Reduction-velocity of Alkaline Copper Solutions.FUCHS (F.). A General Method of Estimatiiig the Basicity of Acids .GROSHANS (J.A.).Prout's Hypothesis especially in relation to the AtomicBRUHL (J.W.). Sublimalion Apparatus.BRUHL (J.W.). Apparatus for Urystallisiag at a Low Temperature .BECQUEREL (H.). Absorption-spectra of Epidote.WALTER (B.). Change of Fluorescence with Concentration.WALTER (B.). Evidence afforded by Fluorescence and Absorption of theDecomposition of Molecular Groups in Solutions.RIGHI (A.). Electromotive Force of Selenium.SOHNCEE (L.). Production of the Current in the Galvanic Circuit .BOUTY (E.). Electrical Conductivity and Electrolysis of ConcentratedSolutions of Sulphuric Acid.WEBER (C.L.). Electric Conductivity of Solid Mercury.POTIEB (A.). Electrochemical Measurement of Currents.OSTWALD (W.) and W.NERNST.FreeIons.Gaseous Compounds.Chemical Theory of the Galvanic ElementWeights of Carbon and Oxygen.PAGE456462VIOLLE and CHASSAGNY.Electrolysis.BARNLI (A.) and G.PAPASOGLI .SCH L F IE HMACHER ( A.).Heat. Conductivity of Mercury Vapour.GIR ~ R D (C.) and L.L’HOTE.Heat of Formation of Aniline Dichromate .DE TORCRAND.Alcohohtes of Monosodium Glycol.WROBLEWSKI (8.r.). Compressibility of Hydrogen.BEPERINCK (M.W.). Simple Diffusion Experiment.FABINYI (R.). Raoult’s Law of Freezing.EYILMAN (J.F.). Raonlt’s Law of Freezing.PAT ERN^ (E.). Molecular Depression of the Freezing Point of Benzene byIodoform.EOPP (H ).Molecular Volume of Liquids.STRANSKY (S.). Numerical Relations of the Atomic Weights.CONRADY (E.) .YELLAT (H.).SCHKEBER (K.). Electromotive Forces of thin Layers of Hydrated PeroxidesP~LTSCHIKOFF (N.).Initial Phase of Electrolysis.PILTSCHIKOFF (N.). Klectrolytic Polarisation by Metals.SCHGLTZE (W.H.). Electrolytic Behaviour of Mica at High Temperatures .GORE ((3.). Detection of the Combining Proportions of Compounds by theVoltaic Balance.EYKMAN (J.F ).Determination of the Latent Heat of Fusion from theTttouLxT and CHEVALLIER.Specific Heat of Sea-water of DifferentDen sit.ies.BERTHELOT and P.PETIT .LOUGUININE.Heats of Combustion of Metaldehyde Erythrol and Tricar-ANTOINE ((2.). Dilatation and Compression of Caybonic Anhydride .~ A N ’ T HOFF (J.H.) and L.T.RPICHER.Relation between Osmotic Presmre,Reduction of the Freezing Point and Electrical Conductivity .T.~MMANN (G.). Vapour-pressure of Aqueous Solutions.WOUKOLOFF .SABATIER (P.).Rate of Transformation of Metaphosphoric Acid.Electrolysis with Carbon ElectrodesTAMMANN (G.). Action ol’ Ferments.ALESSI (A).Lecture Experiments.Calculation of Atomic Refractions for Sodium Light .Contact Potential of a Metal and its SaltsGORE ((3.). Voltaic Energy of Electrolytes.CHASSY (A.). Electrical Transport of Dissolved Salts.Reduction of the Freezing Point.Heat of Formation of Antimony Hydride .BERTHELOT.Thermochemietry of the Thionic Acids.Solubility of Uases.LF CHATELrER (H.). Solubility O f Salts.TILINGSHEIM (E.). UnPtable Equilibrium of Atoilis.A USTEN (P.T.). Lecture Experiments with Nitric Acid.R~JLUDT (A.). Variation with Temperature of the Velocity of Light inMetals.MILTHALER (J.).Variation in the Specific Heat of Mercury with Tempe-BLUMCKW (A.). Isotherms of a Mixture of Sulphurous and CarbonicAnh ydridrs.MEYER (L.). Gas Eeating.Absorption and Condensation of Carbonic Anhydride onConditions of Equilibrium between Solid andKRAUSE (H.).ROOZEBOOM (H.W.B.).Liquid Compounds of Water with Salts.MEYER (L.) and K.SETJBERT.Unit of Atomic Weights.ANSCH~TZ (R.). Raoiilt’s Method of determining Molecular Weights asMEYER (L.). Air Baths.AUSTEN (P.T.). Lecture Experiments.BARBIER (P.) and L.Roux.Diqpersion in Organic Compoixndq.YASCH EN (F.).Relation bet. ween Potential Difference and Striking DistancePABR66 1672CONTENTS. viiOSTWALD (W.). Dropping Electrodes.AUBEL (E. v.). Electrical Resistance of Bismuth.CHROUSTCHOFF (P.).Electrical Conductivity of Saline Solutions .CHROUSTCHOPF (P.).Electrical Conductivity of Saline Solutions. Re-CHROUSTCHOFF (P.). Electrical Conductivity of Saline Solutions .CHROUSTCHOFF (P.) and V. PACEKOFF. Electrical Conductivity of SalineSolutions.LUDEKINO (C.). Conductivity of Solutions of Zinc Sulphate containingGelatin.BORE (G.).MULLER (J. A.). Heat of Formation of Alkaline Carbonates in v e v DilGteSolutions.BERTHELOT and PETIT. Heat OF Combustion of Carbon.BERTHELOT and PETIT.RETGERS (J. W.). Determination of the Specific Gravity of Salts which areSoluble in Water.GERLACH (G. T.). The Densitv Numbers of Groshans.LESCCEUR (H.). Dissociation of &line Hydrates and Analogous Compounds.MULLER (0.).Absorption of Carbonic Anhydride by Mixtures of AlcoholBRUGELMANN (G.). Crystallisation and Physical Union.VOIGTLANDER (F.). Diffusion in Agar Jelly.HALLOCK (W.). Chemical Action between Solids.OSTWALD (W.). Constants of Affinity of Organic Acids and their RelationMEPERHOFFER (W.). Reversible Transformation of Copper PotassiumOSTWALD (W.). Unit of Atomic Weights.BRAUNER (B.). Basis of Atomic Weights.MEYER (L.) and K. SEUBERT. Unit of Atomic Weights.LADENBURQ (A.).Molecular Weight Determinations from Osmotic PressureWILL (W.) and G. BREDIG. Xstirnation of the Molecular Weights ofDissolved Substances.KLOBUKOFF (N. v.). Cryoscopic Behwiour of Solutions of Iodoform inBenzene and Acetic Acid.STOEMANN (F.) C. ELEBER and H. LANOBEIN.Cornbustion of OrganicSubstances in Oxygen a t High Pressure.BERTFIELOT. Heat of Formation of Hgponitrites. ,.VANT’ HOFF (J. H.) and L. T. REICHER. Temperature of TransformationZETGERS (J. W.). Specific Gravity of Isomorphous Mixtures.HECRT (W.) and M. CONRAD. Determination of Affinits Constants .OSTWALD (W.) Dissociation of Electrolytes.VANT’ HOPF (J. H.). Relation between the Affinity in Absolute MeasureOSTWALD (W.). Unit of Atomic Weight.TAMMANN (G.) Constitution of Alloys.SILOW (P.). Alloys.BECKMANN (E.). Estimation of the Molecular Weight from the Rise in theBoiling Point.KLOBUKOFF (N. v.). Cryoscopic Behaviour of Solutions of Morphine Com-PATERN~ (E.). Molecular Depression of the Freezing Point of Benzene byAlcohols.TAFEL (J.).Apparatus for Shaking.BECEE (F.). Crystalline Form of Grape-sugar and of OpticallF Active Sub-RICHARZ (F.). Electrical Behaviour of Platinum in Persulphuric Acid &&Loss of Voltaic Energy of Electrolytes by Chemical UnionHeats of Combustion and Formation of NitrilesSulphate.PAGE81’7931ALLIHN (F.). The Rise in the Zero Point of Thermometers made of JenaSTOHMANN (F.) C. KLEBER and H. LANQBEIN. Heat of Combustion ofBenzene and of other Hydrocarbons of the Aromatic Series.SABATIER (P.). Heats of Dissolution and of Formation of Hydrated MetallicChlorides.KLOBUEOFF (N v.). Apparatus for Cryoscopical Investigations.GERLACH (8. T.). Specific Gravity of Aqueous Solutions.SETSCHENOFF (J.). Constitution of Salt Solutions inferred from theirBehaviour to Carbonic Anhydride.,.ARICHENIUS (S.).Heat of Dissociation of Electrolytes and Influence of Tem-MULLER-ERZBACE (W.).Statical and Dynamical Methods of MeasuringSTEFAN (J.). Diffusion of Acids and Bases into One Another.FEITLER (S,). Molecular Volumes of Aromatic Compounds. .BREYER (T.). Gas Generator with Continuous Removal of the ExhaustedSolution. ,ELIMENPO (E.) and (3. PEKATOBOS. Action oi? Hykroge'n Ch'loridk andMetallic Chlorides on the Photochemical Decompovition of ChlorineWater.ALTHAUSSE (k) and 8. KRUSS. Relationships between the CompositionKLOBUKOFF (N. v.). New Apparatus for Electrochemical Investigations .DUTER (E.). Electrolysis of Distilled Water ,. ,NERNST (W.). Electrolytic Activity of the Ions.WEBER (C.L.). Absolute Velocity of the Ions.BERTHELOT and MOISSAN. Heat of Combustion of Fluorine with Hydro-STOHMANN (F.) C. KLEBEB and H. LANBBEIN. Calorimetric Investiga-STOHMANN (F.) C. KLEBER and H. LANBBEIN. Thermochemistry ofAcids of the Oxalic Series and of Fumaric and Male'ic Acids .BODISCO (A.).BERTHELOT and P. PETIT. Thermochemistry of the Nitrocnmphors and ofCyanocamphor.VIGNON (L.). Thermochemistry of Phenylenediamines.ARRHENIUS (S.). Electroljtic Dissociation versus Hydration.YICKERING (a. U,). Nature of Solutions.RETQERS (J. W.). Determination of the Sp. Gtr. of Soluble Salts .TCHERNAY (N. A.). Dilatation of Salt Solutions.CHARPY. Contraction of Solutione. ,ARRHENIUS (S.). Rate of Change in the Inversion of Cane-sugar .LELLMANN (E.).Eataimation of the Coefficients of Affinity of OrganicBases.*.DELAUNEY. Atom'ic Wiights of theElements ,.MELDOLA (R.) and F. W. PTREATFEILD. Determination of the MolecularWeights of Polymeric Compounds by Raoult's Method.~ 1 a s s. ,.Heat of Dissolution of Anhydrsus Lithium Bromide .PAQB10951105Ifiorganiic Chemistry.BOLTON (H. C.).ALLARY (E.). Chlorine and Cyanogen. 13VOSMAEB (A.). Apparatus for a Constant Supply of Chlorine. 13WARREN (H. N.).Metal.13BTARD (A.). Preparation of Hydriodic Acid.14DAGGER (J. H. J.). Hydrogen Sulphide Appart~~us.14List of Elementary Substances announced from 1877 toDiesemination of Sulphur and Phosphorus in Masses oCONTENTS .CHANTEMILLE (P.). Hydrogen Sulphide Apparatus.MAUMEN~ (E.J.).Chydrazine or Yrotoxide of Ammonia.Hydrogen. Methane. &c.COOKE (S.).Action of the Electric Spark on Mixtures of Nitric Oxide withCOOKE (S.) Decomposition of Nitric Oxide in contact with Water and withPotash.MCCAY (L.W.). Action of Hydrogen SulphiJe on Arsenic Acid .HODGES (E.R.). Barium Sulphite.RAUPEYSTR4UCH (a.A.).Solubility of Gypsum.SPILLER (J.). Ancient Mortar from a Roman Wall in London.WELCH (J.C.). Analysis of Money.CHUARD (E.). New Hydrated Cupric Chloride.Csams (J.M.). Purification of Mercury.DUBOIN (A.). Yttrium-potassium and Yttrium-sodium Phosphates .LAUTH (C.) and G.DUTAILLY.BONGAETZ (J.) and A.CLASSEN.HODGKINSON (W.R.) and F.K.S.LowNDEs.Action of Incandescent.ENGEL (R.). Normal Platinum Chloride.MANN.Preparation of Chemically Pure Hydrogeu Peroxide.STORTENBEKER (W.).Compounds of Chlorine with Iodine.RASCHIG (F.). Theory of the Lead Chamber Process.LUNGE (G.). Theory of the Lead Chamber Process.CAMERON (C.A.) and J.MACALLAN.Compounds of Ammonia withSelenious Anhydride.WEDENSKY (V.). Constitution of Phosphorous Acid.RUDORPF (F.). Compounds of Arsenious Acitl with Sodium Iodide .HAMPE (W.). Preparation of Boron and Silicon by Electrolysis.HAUTEFEUILLE (P.) and A.PERREY.Beryllium Silicates.SORET (A.). Occlusion of Gas by Electrolytic Copper.ROBERTS-AUSTEK (W.C.). Mechanical Properties of Metals in Relation toZIRNITB (G.). Solution of Iron in Aqueous Soda.MAURO (F.). Ammonium Fluoroxymolybdates.VIQNON (L.). Tin.PETERSEN (@.) Fluorine-derivatives of Vanadium.ELBERS (W.).Decomposition of Antimony Sulphide by Boiling Water .BURCHARD (0.). Oxidation of Hydrogen Iodide bj Oxy-acid4.HODGKINSON (w.R.) and F.I(.S.1.owNDEs.Action of Incandescent.UFFELMANN.Analysis of Atmospheric Air.BERTHELOT and FABRE.Hydrogen Telluride.MENTE (A.). Amides of Phosphorus and Sulphur.ENGEL.Allotropic Arsenic.LANDAU (W.).RAWSON (S.(3.). Preparation of Boron and Silicon.WARREN (H.N.). Preparation of Silicon.PARSONS (C.A.).GAUTIER (A.). Formation of Carbon Oxysulphide.BAYER (K.J.). Alkaline Aluminates.LAUTH (C.) and G.DUTAILLY.Porcelain Glazes.SPRING (W.). Cause of Railsrusting less quickly when inUse than when notMACKINTOSH (J.€3.). Crystalline Subsulphide of Iron and Nirkel .PICCINI (A) and G.GIORGIS .DIXON (H.B.) and H.W.SMITH.Imperfect Combustion in GaseousExplosions.WARDEB (R.33.).Coefficients of Volatility for Auueous Hvdrochloric AcidJOHNSON (G.S.). Barium Sulphite.So-called Crackle ChinaAtomic Weight of TinPlatinum on Gases and VapoursPlatinum on Gases and VapoursAction of Ammania and Amines on Arsenious BromideEffect of High Temperature and Pressure on CarbonNew Fluorine Compounds of VanadiumPAGEI5103209POTILITZI~ (A.). Rate of Decompositioi of t h e Salts oyf Halogen Oxy-x CONTENTS .PAGBBILTZ (H.). Molecular Weight of Sulphur. 340CURTIUS (T.) and R.JAY.Hydrazine. 340MEYER (L.). Nitric Anhydride.341DRAWE (P.). Hypophosphoric Acid andits Salta.341MARSHALL (J.) and C.S.POTTS .GATTERMANN (L.).Silicon and Boron. 342WARREN (H.N.). Graphite from Various Metals.343HODGKINSON (W.R.) and F.K.S.LOWNDES.Decomposition of PotassiumChlorate in Contact with Metallic Oxides.343Extraction of Lithium from its Minerals. 344IRVINE (R.) and G.YOUNG .HILL (.J. R.). Solubility of Strontium Nitrate in Alcohol. 345WARREN (H.N.). Action of Ammonia on Metallic Magnesium. 345BAUBIGNY (H.). Action of Hydrogen Sulphide on Zinc Sulphate.346PRAFULLA CHANDRA RAY.Mixed Double Sulphates of the Copper-BARFOED (C.). Action of Sodium Hydroxide on Mercurous Salts.346RAMMELSBERG (C.). Ammoniacal Mercury Compounds. 347EREMIN (F.A.) .WARREN (H.N.). 348KRUSS (8.) and F.W.SCHMIDT.349BERTHELOT.Interaction of Chromic Acid and Hydrogen Peroxide.350VIGNON (L.).Oxidation of Tin.351RADAU (C.). Salts of Vanadic Acid. 351JORGENSEN (5.M.). Metallic Dianline Compounds.351PALVAER (W.). Iridio-ammonium Compounds.352JOLY (A.).Ruthenium Nitrosochlorides ; Atomic Weight of Ruthenium.352HABERYANN (J.). Preparation of Hydrogen.465OOHRING (C.F.). Preparation of Oxygen. 465BAKER (H.B.). Combustion in Dried Oxygen.465G~USTAVSON ((3.). Valency of Boron. 465BOTTINGER (C.). Formation of Carbon Oxysulphide.466MCCALEB ( J.F.). 466MCCALEB ( J.F.j. Hydration of Calcium Sulphate.466MCC~LEB ( J.F.). Specific Gravity of Calcium Sulphate. 467JARMAN (J.L.) and J.F.MCCALEB .SCHURMAXN (If.). Affinity of the Heavy Metals for Sulphur. 468BERTHELOT.Interaction of Chromic Acid and Hydrogen Peroxide.468BRANDHORST (C.H.) and K.KRAUT.Phosphotungstic Acid.469TBOMA (M.). Absorption of Hydrogen by Metals.588VILLIEES (A.). Action of Sulpliurous Acid on Sodium Thiosulphate.568CAMPAEI ((3.). Preparation of Nitrous Oxide.569LACHOWICZ (B.). Acid Character of the Salts of the Heavy Metals.569ANDRR (G.). Properties of the Mercurammonium Chlorides. 570COMBES (A.). Valency of Aluminium. 571BERTHELOT.Hydrogen PeroxideandChromicAcid.571LBVY (L.). Titanium Peroxide.57’2HBRARD (F.). Amorphous Bismuth. 572AUSTEN (P.T.). Hypochlorous Acid in Alkaline Solution. 672NOYEB (W.A.). Atomic Weight of Oxygen.672BERTHELOT.Abeorption of Nitrogen during slow Oxidation. 673LUCION (R.). Action of Chlorine on Carbonic Anhydride. 673BILTZ (H.) and V.MEFER.Vapour-density Determinations of someArsenic in Glass and in Alkali Hydr-Soliibility of various Forms of Calcium Car-Action of Concentrated Sulphuric Acid on Solutions ofSolution for depositing Metallic Cobalt.Nickel and Cobalt.Relative Rates of Dissolution of Gypsum and Anhydrite .A Red Copper Slag containing Arti-AYAT (L.).Sodium Phosphite.569PAILLARD (C.A.). Non-magnetisable Alloys of Palladium. 573Elementsand Compoundsat a White Heat.67CONTENTS. xi755827936PAQEJAWEIN (L.) and A. THILLOT. Molecular Weight of some Metaphosphates.COMEP (A. M.) and C. L. JACKSON. Sodium Zinc Oxides.DENIG~S. Formation of Cuprous Chloride and Bromide from Cupric Sul-BARFOED ((3.). Action of Ammonia on Mercurous Salts.HAXPE (W.). Electrolysis of Cryolite.HAMPE (W.).Aluminium Subfluoride.GAUTIER (A.) and L. HALLOPEAU. Metallic Sulphides.HURST (G. H.). Ochres Siennas and Umbers.CARNOT (A.). Peroxides of Nickel and Cobalt Estimation of Nickel andCobalt.RAWBON (S. G.). Oxy-haloi'd Derivntires of Chromium.JOLY (A.). Nitroso-compounds of Ruthenium.MERZ (V.) and E. HOLZMANN. Formation of Hydrogen Bromide andHydrogen Iodide.JOHNSON (G. 54.). Solubility of White Precipitate in Solution of AmmoniaWILLIAMS (G. H.) and W. M. BURTON. Crystalline Form of Metallic ZincMORSE (H. N.) and J. WHITE. Dissociation of the Oxides of Zinc andJOHNSON (I( R.). Some Phosphates of Yoljvalent Metals.Roux and E. LOUISE. Molecular Weights of Aluminium Compounds .SZILASI (J.). Green Ultramarine.WINKLER (C.). Atomic Weight of Nickel and Cobalt.COLORIANO (A.).Crystalline Metallic Molybdates.HUNDESHAGEN (F.). Phosphododecnmolybdic Acid.ROSENHEIM (A.). Vanadotungstic Acid.WINKLE& (C.). Chlorine from Bleaching Powder.OLSZEWSKI (K.). Determination of the Boiling Point of Ozone and of theSolidifying Point of Ethylene.BERTHELOT. Action of Alkdis on the Thionic Acids.BRRTHELOT. Action of Acids on Thiodphates.LE ROY (G. A.). Preparation of Alkaline Nitrites.AMAT (L.). Phosphorous Acid.PARMENTIER (F.).LEF~VRE. Action of Alkaline Arsenates on the Alkaline Eart!ts.FEIT (W.).Potassium Magnesium Bromide.ANDRB (G.). Formation of Mercurammonium Chlorides.MYLIUS (F.) and F. FOERSTER.GORGEU (A.). Formation of Manganese Oxides in the Wet Way .GORGEU (A.). Action of Air on Manganous Carbonate.GAUTIER (A.) and L.HALZOPEAU. Metallic Strlphides.BOURGEOIS (L.). Crystallised OrthosilicateP of Nickel and Cobalt .VOSMAER (A). Preparation of Chromic Chloride.PBCIIARD (E.). Metatungstic Acid.VIGNON (L.). Variations in the Acid Function of Stannic Oxide .BESSON (A.). Combination of Nitrogen Oxides with Metallic Chlorides .PIGEON (L). Platinirni Tetrachloride.JOLY (A.). Atomic Weight of Ruthenium.REMSEN (1.j. Double Halogen Salts.JOHNSON (G. S.). Atomic Weight of Oxygen.PETTERSSON (0.) and K. SOND~N. Absorptive Power of Water for Atmo-WINKLER (L. W.). Solubility of Oxygen in Water.TRACBE (M.). Autoxidation.TRAUBE (M ). Constitution of Peroxides.TRAUBE (31.). Formation of Hydrogen Peroxide from Persulphuric Acid .TRAUBE (M.).Behaviour of Persulphuric Acid towards Nitrogen Evapora-DIEHL (W.). Ahiminium Subfluoride.Cadmium in the Vapours of their respective Metals.Presence of Sodium Siilphate in the Atmosphere .Solubility of alas3 in Waterxii CONTEXTS .PICKERING (S.U.). New Hydrate of Sulphuric Acid.SCHWICKEB (A.).Sulphites and Thiosulphates.MAQUENNE.Hyponitrites.VAUBEL (W.). Behaviour of Sodium Thiosulphate with Acid0.CHODOUNSKY (K.). Solubility cf Arsenious Oxide and Sulphide.DELACHARLONNY (P.M.). Presence of Sodium Sulphate in the Atmo-MORSE (H.N.) and J.WHITE.Dissociation of the Sulphides of CadmiumELOBUKOFF (N.v.). Modifications of Precipitated Cadmium Sulphide .SORET (A.). Occlusion of Gases by Electrolytic Copper.GABBA (L.).New Reaction with Ferric Chloride.KOENIG (T.) and 0.v.D.PFORDTEN.Titanium CompoundsJOLY (A.). Ammoniacal Derivatives of Ruthenium.SABATIER (P.). Hydrated Metallic Chlorides.KASSNER (G.). Basic Zinc Ammonium Carbonate.NETJMAWN (G.). Halogen Mercuric Acids.THUMMEL (K.). Mercury Oxychlorides.KLEINSTUCK (0.). Specific Gravity and Composition of Tin-Lead Alloys .SPRING (W.). A New Tin Oxide.L E P ~ Z (C.) and L.STORCH.Behaviour of Metastannic Acid to BismuthSTORCH (L.). Stannic Sulphide and Thiostannic Acid.Libeixtion of Chlorine during the Decomposi-HOPPE-SEYLER (F.). Autoxidation.HARTOG (P.J.). Sulphites.Behaviour of Sodium Thiosulphate with Acids a n iMetallic Salts.BIRHANS (B'.). Solidification of Nitrous Anhydride.CROSS (C.I?.) and E.J.BEVAN .WOUKOLOFF.Solubility of Carbonic Anhydride in Chloroform.SPRING (W.) and J.DEMARTEAU.Constitution of Potassium Poly-CHAPMAN (A.S.).Cistern Deposits.VIARD ((3.). Zinc and Cadmium Chromites.BRUN (E.). Cupric Oxybromide analogous to Atacamite.BOECK (J.). Oriental Enamel on Tiles and its Imitations.SPRING (W.) and E.PROST .VORTMANN (G.).Conditions of Activity of Nitric AcidNILSON (L.F.) and 0.PETTERSSON .CARNEGIE (D.J.).Molecular Weight of AluminiumCbloride.Reaction between Solutions of Ferric Chloride andPotassium Iodide.SAINT-EDMB (E.). Passivity of Cobalt.KRUSS (G.) and F.W.SCHMIDT.Cobalt and Nickel.DF SCHULTEN (A.). Crystallised Cobalt and Nickel Hydroxides.ROUSSEAU (G.). Barium Cobaltite.Existence of a Cobalt Dioxide withAcidic Functions.CARNOT (A.).Ammonio-cobaltic Molybdate Tungstate and Vanadate .CARNOT (A.). Purpureo-cobaltic Tungstate and Vanadate.JAGER (E.) and G.KEUSS.Chromium.VIGNON (L.).KOENIG (T.) and 0.v.D.PFORDTEN .BEILSTEIN (F.) and 0.v.BLASE.Basicity of Antinionic Acid.Mercury.PBCHARD (E.). Phosphotungstic Acid.Action of Water on Stannic Chloride.Titanium.PETERSEN (E.). Pluorine-compounds of Val adium and its Analogues .WARREN (H.N.). Action of Silicon on Gold Silver Platinum andROUSSEAU ((3.). Platinates of the Alkalis and Alkaline Ear'ths.PAGE10511113CONTENTS . xu1Mineralogical Chemistry .STAHL (W.). Hexagunal Crystals of Zinc Sulphide.SCHMIDT (A.). Arsenopgrite from Servirt.MICHEL (L.). Preparation of Pproniorphite and Mimetesits.JANNETTAZ (E.).Uranite from Madazascar.IGELSTROM (L.J.). Arseniopleite a new Swedish Miisera1.CATHREIN (A.). Minerals of the Tyrol.KUNZ (G.F.). Mineralogical Notes.DOELTER (C.). Artificial Formation of Mica.ROHRBACH (M.). Chiastolite.HOVEY (E.0.). Cordierite-gneiss.KOTO (B.). Piemontite.IDDINGS (J.P.). Origin of Primary Quartz i n Basalt.WOLLEMANN (A.). The Badenweiler Ore Deposit.GLASER (M.) and W.KALMANN.Analysis of Roncegno-waterHOFFMAN (G.C.). Native Platinum from Canada.BARROIS ((7.). The Pyroxenites of Morbihan.RINNE (F.). The Dachberg a Volcano of the Rhone.STRENGE (A).Dolerite of Londorf.DE ROUVILLE (P.) and A.DELAGE.Porphyrites at Gtabian.MONTEMARTINI (C.). Composition of Serpentine Rocks.PREUSSNER.A Remarkable Bed of Sulphur.LOCKZA (J.).Arsenopyrite from dervia.LOCZKA (J.). Constitution of Arsenopyrite.SJOGREN (A.). Periclase from Nordmarken.LANBHAUS ((3.). Psilomelane.BLOMSTRAND (C.W.) Analyses of Monazite and Xenotime.HIDDEN (W.E.) and J.B.MACKINTOSH.SulphohaliteSJOGREN (A.). Allactite from LLngban.HOQBOM (A.G.). Pgrrhoarsenite and Berzelite.EAKINS (L G.). Thiantimonites from Colorado.WETBULL (M.). Hjelmite.NORDENSKIOLD (A.E.). Eudidymite.LINDSTEOM ((3.). Analysis of Natrolite.LINDSTROM ((3.). Hplotekite from Lgngban.RAMMELSBERG (C.). Gadolinite.NORDENSKIOLD (A.E.). Mineralogical Notes.BLOMSTRAND (C.W.). The so-called Cyrtolite of Ytterby.FLIKK (G.). Swedish Minerds.LADRI~RE (J.). Phosphatic Minerals a t Montay and Forest.DUNNINQTON (F.P.).BOURGEOIS (TJ.).Formation of Deposits of Oxides of Manganese .Artificial Production of Hydrocerusite it8 Composition.and the Constitution of White LeadHATLE (E.) and H.TAUSS .SCHNEIDER (E.A.). Treatment of Natural Silicates with HydrochloricBaryto-celestine from Werfen in SalzburgAcid as a means of ascertaining their Structure.PENFIELD (S.L.). Bertrandite from Mt.Ontero Colorado.WADSWORTH (M.E.). Peridotite of Iron Mine Hill Cumbedand RhoddFRESENIUS (R.). Mineral Spring in the Admirals.garteabad Berlin .CHATARD (T.M.). Analyses of the Waters of some American Alkali Lakes .Riebeckite and the new Formation of Albite in Granite-SAUER (A.)..IGELSTR~M (L.J.). Pyrrhoarsenite and other Swedish Antimoniates .HIDDEN (W.E.) and J.B.MACKINTOSH.Auerlite a New ThoriumMineral.FREDA ((3.).Composition of Piperno of the Collina del Vomero .HOWITT (A.W.).Metamorphic and Plutonic Rocks at OmeoPAGE25216221MONTEMARTINI (C.). Compbsition of some Rocks from the Shore at Nice.22PAGERICCIARDI (IJ.). Examination of the Rocks of the Vulsinian Volcanoes.224EROF~EFF (M.) and P.LATSCHINOFF.Meteorite from Novo-Ure'i.224MUNTZ (A.) and V.MARCAXO.Black Rivers in Equatorial Regions.226MACADAM (W.1.). 353SCHNEIDEE (R.).Artificial Copper Pyrites.354MEUNIEB (S.). Artificial Production of Chromite.364HIDDEN (W.E.). Edisonite a Fourth Form of Titanic Anhydride.354HAUTEFEUILLE (P.) and A.PEEEEY.Artificial Production of Zircon.355Fossil Resins from the Coal Measures.Action of Cuprous Chloride on Potassium Iron Sulphide :DANA (E.S.).Beryllonite.355HIDDEN (W.E.). Xenotime. 355PENFIELD (S.L.) and E.S.SPERRY.356HAUTEFETJILLE (P.) and A.PERREY.Ferric Orthoclase. 357KATZER (F.). Geology of the District of Riean.357KUNZ (G.I?.). Two New Masses of Meteoric Iron.358TICHONRAVOFF PETROFF and others.Meteorite from Ochansk. 358DICKIE (A.). Chemical Composition of the Water of the Clyde Sea Area.359JARMAN (J.L.). PFrolusite from Augusta Co. Virginia. 470DANA (E.S.) and H.L.WELLS.Beryllonite.470HANKS (H.G.).Occurrence of Hanksite in California. 471WELLS (H.L.) and S.L.PENFIELD.Sperrylite.471VRBA (C.). Bertrandite from Pisek. 471JANNASCH (P.) and G.CALB.Composition of Tourmalin. 472LINDGREN (W.). Minerals of the Pacific Coast.472KONIG (G.A).473ROBIKSON (W.C.). Spessartine.473VAN HISE (C.R.).BAYLEP (W.8 ).Rocks of Pigeon Point Minnesota.473DE LAPPARENT (A.).Rocks.474LOSSEN (K.A.).Palseopicrite from Stoppenberg in the Harz. 573FOTJLLON (H.B.v.). 574T)ILT.ER (J.S.). Peridotite of Elliot Co. Kentucky.680Mineralogical Notes.New Minerals from Franklin New Jersey.Iron Ores of the Penokee-Gogebic Series of MichiganRelation between Solfataras and Acidic EruptiveMeteorites of Slialka and Manbhoom.LATTRRMANN ((3.). Pseudo-brookite. RXOMFNTZ (A.) and V.MARCANO.Formation of Deposits of Nitrates.680DTLLER (J.S.). Gehlenite in a Furnace Slag.681DILLER (J.S ) and J.34.WHITFIELD .TRAUBE (H.). Eclogite from Frankenstein in Silesia.681THOULET (J.).Solutihty of Minerals in Sea-water.682GOOCH (F.A.) and J.E.WHITFIELD .Park.682BEOWNE (D.H.). Phosphorus in the Ludington Mine Michigan.763TRATJBE (H.). Zinc-bearing Aragonite horn Tarnowitz. 763SCHARIZER (R.). Tourmaline ctf Schuttenhofen.764WULFING (E.A.). Formula of Tourmaline. 765WEIBULL (M.). Fluocerite from Gsterby. 765MEUNIER (S.). Meteorite at Eagle Station Kentucky.765CLARKE (F.W.) and C.CATLETT.835COHEN (E.). Genesis of Alluvial Gold. 835Dumortierite from Harlem NewYork. and Clip Arizona.Waters of the Yellowstone NationalPlatiniferous Nickel Ore from Canada .SANDBEHGER (F.v.). ModTfications of Zinc Blende.P36VRBA (C.). Strontianite from Altahlen. 837VRBA (C.). Apatite from Pisek. 837SAPTZEFF (A.). Minerals from the Central Ural.837NANTIER (A*) .QCHSENIUS (C.).Minerals from the Douglashall Salt Mine. 838Enrichment of Phosphatic Chalk Origin of the Rich PhosCONTEXTS. XVPAGE3442LACROIX ( A.).Barium Sulphate.MEPER (A. B.). So-called Jadeitz from Switzerland.COHEN (E.). Msteoric Iron from Portugal.LACBOIX (A.).Rock Containing Sodium-amphibole Astrophyllite Pj-ro-REICHARDT (E.). Mineral Water of the Ottili Spring Suhl ThuringiaOrgal& ChemistnJGUSTAVSON (G.) and M. DEMJANOFF. Isoallylene.CLAUS (A.) and 0. PTJTENSEN. Cyanurates.ASCHAN (0.). Preparation of a-dibromhydrin.PAAL (C.). Epichlorhydrin.FAUCONNIER (A.).Propylphycite.MAQUENNE. Molecular Weight and Valency of Perseite.R A ~ A N N (B.). Constitution of the Glucoses.KILIANI (H.). Oxidation of Arabinose with Nitric Acid.MAYER (F.).Action of Nitrous Acid on Hexamethylenamhe.UDR~NSKY (L. T.) and E. BAUMANN. Identity of Putresine and Tetra-ORNDORPF (W. R.) and H. JESSEL. Deconjposition of Acetone withBleaching Powder.PECHMANN (H. v.) and K. WEHSARG. Dinitrosoacetone.DE VARDA (G.). Sulphoisovaleric Acid.GRAF (P.). Constituents of Cocoa FLtt.MESSINGER (J.) and C. ENGELS. Action of Hydrogen Phosphide on'Alde:WEDARD (E. M.).LOUTSF. (E.) and L. ROUX. Freezing Points of Solutions of AluminiumAlkpls.HILL (H. B.) and A. W. PAXMER. Substituted Pyromucic Acids .Action of Heat on Tartaric Acid in Aqueous SolutionVOSWINKEL (A.). Metadiethylbenzene.JACOBSEN (0.) Synthegis of Consecutive Tetramethylbenzene.JACOBSEN (0.).Tetrethylbenzene.CHABRIB (C.). Synthesis of Aromatic Selenium Compounds.JACOBSEN (0.). Comecutive Metaxylenol.RE LA HARPE (C.) and F. REVERDIN. Nitronitrosoresorcinol.BELZER (C.). Derivatives of Paramidoisobutylhenzene.JACOBSEN (0.). Pentethylbenzene and its Decomposition by SulphuricAcid.PECHMANN (H. v.). Condensation Products of Quinone and Ethyl Aceto-ORNDORFF (W. R.). Decomposition of some Diazo-compounds with FormicJENTZSCH (h.).Chrysoidincarbamide Amidophenylenecarbamide .PECHMANN (H. v.) and I(. WEHSARG. Hydrazoximes.DECKER (H.). Ethyl Phenylhydrazineacetylacrylate.KNECHT (E.). Theory of Dyeing.ARONSTEIN (L.) and A F. HOLLEMANN. Stilbene.KYM (0.). Thio-derivatives of P-J)inephthglamine.EKSTRAND (A. (3.). Naphthoic Acids.FORSLING (S.).P-Chloronaphthaleneaulphonic Acid.SCHALL (C.) and G. DRALLE. Brazilin.HOLLEMANN (A. F.). Product of the Action of Nitric Acid on Aceto-CLAUS (A.) and E. FOHLISCH. Consecutive Duryl ;Methyl Ketone .AUWERS (K.) and V. MEYER. Action of Heat on Benzildihydrazone .DACCOMO ((3.). Filicic Acid.KOBERT (R.) Quillajic Acid. PBOE w IDMAN (0.). Nomenclature of Compounds c6ntaining NitrogenbusNuclei. 56Q-LTXAUX (E.). Metapyrazolones. 56COMBES (A.).Action of Phenylliydrazine and Hydroxjlamine on Acetyl-DE VARDA (G.). Derivatives of Methylpyrroline.,. 57MAGNANINI ((3.). Derivatives of Unsymmetrical Dimethylpproline.57AXDERLINI (F.). Derivatives of Pyrrolinephthalide.,. 58CIAMICIAN ((3.) and F. ANDERLINI.Pyrroline-derivatives.58AHRENS (F.B.). Dipiperidyl and Dipicolyl.59HEBEBRAND (H.). Action of Chlorine on Hydroxyquinoline. 60SCHMIDT (E.). Papaveracese Alkalo’ids.,. 62HENSCHKE (A.). Chelidonine.62GAUTIER (A.) and L. MOURGUES. AlkaloYds from Cod-liver Oil,.63BEVAD (I.). Action of Zinc Et,hyl on Nitroethane.112KONDAKOFF (I.). Action of Ohlorine on Isopropylethyiene. 113HOLTZWART (R.). Polymeride of Methyl Cyanide.113MEYER (E. v.). Polymeride of Ethyl Cyanide. ,.114SYOLKA (A.) and A. FRIEDREICH. Ammeline.114NASINI (R.) and A. SCALA. Snlphines and the Valency of Sulphur.115KONDAKOFF (I.). Trimethylene Glycol from Methyl Isoproyengl Carbinol.115MAQUENNE. Combination of Benzaldeh yde with Polyhydric Alcohols.116KILIANI (H.) and c. SCREIBLER. constitution of Sorbinose.116ZULKOWSKI (K.). Changes suffered by Starch when Dissolved in HotUlycerol.116PAAL (C.). Derivatives of Allylamine. 116LOUYSE (E.).synthesis of Hydroxypropylenediisoamylamine. 118RIEGER (J.). Glyoxalbutyline and Glyoxalisobutyline.119BARBAGLIA (G. A). Action of Sulphur on Parisobut.ylaldehyde. 120HorPE (E.). Action of Ammonia on Methylethylacrrildehyde. 120LUDWIG (E*). Action of Sulphurous Acid on Methylethglacraldehyde.121ZELINSKY (N.) Action of Potassium Cyanide on Ethyl a-Bromopropionate 122KEPPICH (P.).Normal Caproicand Diethylacetic Acids. ,.122GENVRESSE (P.). Chloro-derivatives of Ethyl Acetoacetate. 128SPIRIDONOFF (N.).Oleic Acid. 123MATVBEFF (V.). Action of Ally1 lodide and Zinc on Ethyl Malonate.124OSSXPOPF (I.) Action of Maleic Acid on Aniline ,.124OSSIPOFF (I.). Ieomerism of Fumaric and Maleic Acids. 124FBANCRIMONT (A. P. N.) and E. A. KLOBBIE. Methyl and Ethyl Ethylene-FEANCHIMONT (A. P. N.) and E. A. KLOBBIE. Ure’idee and their Nitro-FITTIG (R.) and A. HANTZSCH. Identity of Methronic Acid wich Syivane-~CHRAYM (J.).Isomeric Changes on Synthesising Aromatic CompoundsCLAUS (A.) and U. A. JACKSON. Orthocresol.128NOLTING (E.) and B. PICK. Dinitrorthoxylenols.129KRAFFT (F.) and J. GOTTIG. Benzene-derivatives of High MolecularWeight.129KOSTANECKI (S.) and B. FEINSTEIN. Constitution of Stypbnic Acid.130WIERNIK (J.).NOLTING (E.) and B PICK.Wroblewsky’s Orthoxylidins. ,. 137HINRICHSEN (W.). Metaxylylamidomethane.131LACHOWICZ (B.). Action of Amines on Nitrogenous Organic Compounds.132Action of Methyl Iodide on someSoiubility of the Silver Calcium and Barirzm 8alts ofDihydroxystearic Acid obtained by the Oxidation ofAction of Carbon Bisulphide on Dimetliylaniline in pre-CONTENTS.xv iiPAGEBISCHLER (A.).Condensation Products from Bases of the Para-series withPara- and Meta-nitrobenzaldehyde.ABENIUS (P.W.) and 0.WIDMAN.Halogen-substituted Acetamido-deriva-ABENIUS (P.W.) and 0.WIDMAN.Action of Bromine on Orthaceto-JACOBSON (P.). Phenylenediazosulphide.NOLTING (E.) and T.STRICKER.Azo.xylenes Diamidodixylyls and theColouring Matters derived therefrom.KOSTANECKI (S.v.).Nitroso-derivatives of Resorcinol-azo-dyes.KOSTANECEI (S.v.). Isomeric Phenyldiazoresorcinols.BURCHARD (0.) and A.MICHAELIS.a-Ethylenephenylhydrazine .BLADIN (J.A.).Diphenylmethyltriazole.DENIG~S (G.).Actiou of Sodium Hypobromite on Nitrogen-derivatives ofMAUTHNER (J.) and W.SUIDA.Aromatic Derivatives of Oxamide andOxamic Acid.GRAEBE (C.). Phthalimidine.GRAEBE (C.) and A.PICTET.Substituted Phthalimidines.VILLE (J.). Action of Hypophosphorous Acid on Benzaldehyde.RODSIANKO (A.). Mono- and Di-nitropmazobenzoic Acids.ANSCHUTZ (R.). Reissert’s Pgranilpyroic Acid.REISSERT (A.). Pyrsnilpyroic Acid.CLAUS (A.) and S.WYNDHAM .MAUTHNER (J.) and W.SUIDA.Phenylglycinorthocarboxylic Acid Glyco-NIETZKI (R.) and 2.LERCH.Orthonitranilineaulphonic Acid.NOLTING (E.). The Sulphonic Acid of Methyl Phenylcarbamate.GRAEBE (C.) and C.AUBIN.Diphenic Anhydride and Orthodiphenylene-VAN ROMBURGH (P.).Nitro-derivatives of Tetramethyldiamidodiphenyl-BANDROWSKI (F.X.).EAPF (S.) and C.PAAL .HELLSTROM (P.). Derivatives of a-P-Dichloronaphthalene.ERDMANN (H.) and R.EIRCHOFF.Di-substituted Naphthalenes from theIsomeric Chlorophenylpamconic Acids.FBIEDL~NDER (P.) and P.WELMANS.Dimethyl-a-naphthylamine and Di-EROHN (C.).a-Nsphtholdiazobenaene and a-Naphthylaminediazobenzene .EKSTRAND (A.G.). Naphthoic Acids.PALMAER (W.). Action of Sulphuric Acid on a-Nitronaphthalene .CLEVE (P.T.). y-Amidonaphthalenesulphonic Acid.CLEVE ( P.T.). 6-Amidonaphthalenesulphonic Acid.ERDMANN (H.). Constitution of Isomeric Naphthalene-derivatives .PESCI (L.). Dextrorotatory Terebenthene.KACHLER (J.) and F.V.SPITZER.Hydroxycamphoronic Acids.KORNER (G.).Syringin.COTTON (S.). Arganin.CAZENEUVE (P.) and L.HUGOUNENQ.Homopterocarpin and PterocarpinLADENBURG (A.). Dipicolylmethane.GARRET (J.C.). The Two Bidesyls.BACHBR (F.). Methylstilbazole and its Reduction-product8.PLATH ((3.). P-Ethyl-a stilbazo!e and its Derivatives.NOLTING (E.) and J.FRUHLING.Paraxyloquinolinesulphonic Acid .GOLDSCHMIEDT (G.). Isoquinoline.JOHNSON (G.S.). Creatinines.STRANSKY (A.). Bases formed by the Action of Potash on Additive Pro-Nitro-derivatives of Isophthalic Acid .Action of Primary Aromatic Amines on Benzil .Derivatives of Ethyl PhenacylbenzoylacetateVOL.LVI.b142154GOLDSCHMIEDT (Gt.) and C.OSTERSETZER.Papaverine-derivatives .GOLDSCHMIEDT (G.). Constitution of Papaverine.LADENBURG (A.).Relations between Atropine and Hyosryamine .HOOGEWERF (S.) and W.A.VAN DORP.Constitution of Berberine .LIEBERMANN (C.) and F.GIESEL.Commercial Preparation and PartialSynthesis of Cocai'ne.EINHORN (11.). Coca'ine.G-AUTIER (A.) and L.MORQUES.CAMPANI (R.). Action of Phosphorus Oxychloride on Cholic Acid .MICHAILOFF (V.). Gelatinous State of Albuminoi'd Substances.LE BEL (J.A.).WAQNER (Gt.). Oxidation of the Hydrocarbons C,H2 -.B~HAL (A.). Hydration of Methylamylacetylene Ethyl Amy1 Ketone .FAUCONNIER (A.). Preparation of Ethylene Cyanide.ELASON (P.). Perthiocyanic and Dithiocyanic Acids.ENEBUSKE (C.). Platinum Compounds of Methyl Sulphide.DONATH (E.).BLOMSTRAND (C.W.). Platinum Compounds of Ethyl Sulphide .WAaNER (G.). Oxidation of Unsaturated Compounds.WAGNER (G.).Part played by Water in the Oxidation of UnsaturatedFAUCONNIER (A.). Preparation of Epichlorhydrin.MEUNIER (J.). Benzoic Acetltls of Mannitol.BAUER (R.W.). Sugar obtained from Plantago pyllium.WALLACH (C.). Amylene Nitrosate and its Derivatives.SCHIFF (H.). Aldehyde and Acetone Sulphites of Organic Bases .PATEIN ((3.). Sulphines.RJELT (E.) and V.0.SIVEN.HAMONET (J.). Prepamtion of Ketones.GRIMAUX (E.) and L.LEF$VRE.Diethoxyacetone.THOMAS and LEF~VRE .WISLICENUS (J.) E.TEISLER and H.LANGBEIN.Geometrical ConstitutionOSSIPOFF (I.). Action of Phosphorus Sulphides on DibromosuccinicAcids.OSSIPOFF (I.). Ethereal Salts of Fumaric and Malei'c Acids.NASTVOQEL (0.). Compounds of Dibromopyruvic Acid with Hydrazines .DAUMICHEN (P.).Tricarballylic Acid.KRUTWIQ (J.). Rate of Oxidation of Tartaric Acid.PELLIZARRI (G.). Alloxan Hydrogen Sulphites of Organic Bases .JAFFS (M.) and H.LEVY .SCHRAMM (J.). Influence of Light on the Action of Halogens on AromaticFRENTZEL (W.). Aromatic Cyanates and their Polymerides.PRIEDEL (C.) and J.M.CRAFTS.New General Method for the Synthesis ofKEHRMANN (F.).Influence of the Presence of Halogens and Alkyl-groupsgroup.TASSINARI ((3.). Dihydroxythiobenzenes.HERZIG (J.) and 8.ZEISEL.Desmotropy in Phenols.ERRERA (G.). Derivatives of Parabromo- and Parachloro-benzyl Alcohols .RUGHEIMER (L.).Derivatives of Tetrene and Synthesis of Tribenzamido-JANOVSEP (J.V.). Azotoluene.LOEBISCH (W.F.) and H.MALFATTI.Strychnine.An Acid from Cod-liver OilMineral Matter in Natural PetroleumActionof Hot Mangaiiese Dioxide on Alcohol Vapour .Compounds.Symmetrical DibromacetoneAction of Acetylacetone on Carbonyl ChlorideGlycocine-derivatives of a-Thiophenic AcidCompounds.Aromatic Compounds.MEYER (R.) and 0.OPPELT.Fluoresce'in.ERRERA ((3.).Nitrobenzyl Ethyl Ether.NEUFELD (A.). 'Halogen-derivatives of Phenylhydmzine.RUDOLPH (0.). Phenylhydrazonee. 251PAQE229237249CONTENTS.xixBALBIANO (L.). Trimethylenephenylimine.RWGHEIMER (L.).Hippuroflavin.WEISE (W.G.M.). Derivative3 of Diphenjlacetaldehyde.HERZIG (J.) and S.ZEISEL.Passivity of certain Yolyketones towardsHydroxylamine and Phenylhydrazine.MILLER (J.A.). Nitriles.SBNKOWSKI (M.). Derivatives of Metamethylphenylacetic Acid.TAKAHASHI (D.).Scopoletin.LE BLANC (M.). Homo-orthophthalic Acid.KOTHE (R.). Syntheses of Dialhylphthalides.DITTR~CH (A.) and C.PAAL.y-Ketonic Acids.ANSCHUTZ (R.) and F.HENSXL.Reissert’s Deoxypyranilpyroic DibromideFEEE (A.) and H.MULLER.Dyes from DiamidoethoxydiphenylsulphonicAcid.WOLFF (L.). Indolc-derivatives.TRENKLEE (B.). Indolee.PETIT (P.). Decomposition of Benzidine Hydrochlorides by Water .HOOKER (S C.). Similar R. eactions of Carbnzole and Pyrolline.MANNS (A.). Malachite-green and Derivatives of Paramidodiphenylme-WISLICENUS (J.) and A.BLANK.Arrangements of the Atoms in Space :Members of the Stilbene-group.KUNZE (E.). Nitroparadiphenols.ALBRECHT (K.). New Method of Formation of Benzhydrol-derivatives .JAPP ( F.R.) and F.KLINQEMANN.Formation of Henzaniarone.ERDMANN (H.).Constitution of certain Dichloronaphthalenes.ZINCKE (T.) and 0.KEGEL.Action of Chlorine on ,8 .Naphthol.WITT (0.N.). Reduction Products of the Azo-dyes of the NaphthaleneSeries.WITT (0.N.). Constitution of P-Naphthol-a-Sulphonic Acid.FORSLING (S.). Action of Fuming Sulphuric Acid on Bronner’s P-Naph-LUCK (E.). Filicic Acid.BOUCHARDAT (G.) and J.LAFONT.Trantlformation of Terpilene intoXenthene.LANDSBERG (M.) Essential Oil of Daucus carota.OLIVERI (V.). Constitution of Quassin.POXERANZ (C.). Methysticin.PLUQGE (P.C.) and H.G.DE ZAAYEE.Andromedotoxin.QCHUNCK ( E ).Chlorophyll.HINS BERG (0.). Hydroxy quinoxalines.CLAUS (A.) and G.N.VIS.Metabromoquinoline.WILLIAMS (G.).Cerinm Quinoline Nitrate.SEUTTEB (E.v.). Additive Product of Pttpaverine with OrthonitrobenzylChloride.SKRAUP (Z.H.). Constitution of Cinchona-derivatives.JOHANNY ((3.) and S.ZEISEL.Colchicine.EINHORN (A.) and 0.KLEIN.Action of Acid Chlorides on the MethylSalts of Ecgonine Hydrochloride.LIEBERMANN (C.). Cinnamylcocalne.FRAQNER (K.). Imperialine.H OPPE-SEYLEB (F. ).Humous S uhstances.PELLIZZARI ((3.). Cholamide and Hippuramide.LEHMARN (V.). Chinethionic Acid.VAEET (R.). Action of Mercuric Cyanide on Cupric Salte.MARLA (F.). New Compound of Potassium Iron and Cganogen .MEYER (E.v.). New Method of obtaining Cyanethine and similar Bases .FAVOESKY (A.). Action of Alcoliolic Potash on Allylene.BARBIER (P.). Phthaliniidine and Methylphthttlimidine.PAGE260278359FORTON (L.M.) and A. A. NOYES. Butines.MAQUENNE. Heptine from Perseitol.P~BYTEK (S.). Di-isocrotyl and its Derivatives.MULDEB (E.). Action of Iodine Iodoform and Methylene Iodide onSodium Ethoxide and of Iodine on Ethyl Sodium Carbamate .KLINUER (H.) and A. KREUTZ. Action ofLMethy1 Iodide on SodiumArsenite.MOISSAN (H.). Ethyl bluoiide.MOISSAN (H.) and M. MESLANS. Methyl and Isobutyl Fluorides .DUNSTAN (W. R.) and E. J. WOOLEY. Isobutyl Nitrite.DUNSTAN (W. R.) and W. L. WILLIAMS. The Metameric Amp1 Nitrites .SOKOLOFP (N.). Action of Alkalis on the Nitro-compounds of AlkylRadicles. ,.SOPOLOFF (N.). Action of Alkyl Iodides on Sodium Nitroethane .DEMUTH (R.) and MEYEB. Nitroethyl Alcohol.REBOUL (E.).Butyric Ethers.DE FORCEAND. Compound of Sodium Glycol with Glycol. .TOLLENS (B.) F. MAYEB and H. WHEELER. Molecular Weight of Arabi-RUDELIUS (C.). Platinum Compounds of Propyl and Isopropyl Sulphides .LONDAHZ (H.). Platinum Compounds of Butyl Isobutyl and BenzylBulphides.JORGENSEN (5. M.). Metallic Diamine Compounds.TOLLEKS (B.) and F. MAYER. Estimation of the Molecular Weight ofParaformaldehyde.-.CURTIUS (T.) and J. LANG. Triaco-derivatives.HELL (C.) and M. ROTHBERU. Action of finely-divided Silver on EthylBromopropionate.KORNER (T.). Derivatives of Phenyl a-/3-Dibromisobutyric Aeid .HANTZSCH (A.). Action of Sodiun; on Ethyl Isobutyrate.- .HELL (C.) and W. MAYER.KONDAKOFF (I,). Oxidation of Angelic and Tiglic Aoids.HAZURA (K.) and A.GRUSSNER. Olive Oil.HAZURA (K.) and A. GRUSSNER. Oxidation of Unsaturated Fatty Acids byCLMSEN (L.). Action of Ethyl Chlorocarbonate on Ethyl SodacetoacetateBUJARD (A.) and C. HELL. Bromazelai’c and Hydroxyazelak Acids .MULDER (E.) and C. WELLEMANN. Action of Ethyl Dibromosuccinate,Bromomaleate and Tartrate on Potassium Ethoxide.CURTIUS (T.) and F. KOCH. Diazosuccinic Diazosuccinamic and Diazo-ZELINSPY (N.) and A. BITSCHICHIN. Action of Potassium Cyanide onHELL (C.). Symmetrical Diethylsuccinic Acids.OSTWALD (W.). Immalic Acid.CLAISEN (L.) and W. ZEDEL. Action of Ethyl Chlorocarbonate on theSodium-derivatives of Acetglacetone Ethyl Acetoacetate and EthylMelonate.THIERFELDER (H.).Gtlycuronic Acid.P%BRAM (R.). Change in the Rotatory Power of Tartaric Acid in MixedSolutions.LONG (J. H.).Polarisation of Tartrate Solutions.MEYER (L.). Decomposition of lmides with Alcohols.PIUTTI (A). Synthesis of the Asparagines.PIUTTI (A.). Constitution of the Monethyl Aspartates and the AsparaginesCIAMICIAN (G.) and P. SILBER. Derivatives of Maleinimide.KNORR (I.,.). Constitution of Carbopyrotritartaric Acid.KNORR (L.) and W. CAVALLO. Carbopyrotritartaric Acid.KNORR (L.). Derivatives of Ethyl Discetosuccinate.Action of Silver on Ethyl BrornisovaleratePermanganate.PAGE367377CONTENTS.xxiPAGCBKNORR (L.).Hydrolysis of Ethyl Diacetosuccinate. Acetonylacetone. andDiacetosuccinic Acid.HILL (H.B.) and W.PALMER.CIAMICIAN (G.). Physical Properties of Benzene and Thiophen.MEYER (L.).Nitration.VOSWINKEL (A.). Orthodiethylbenzene.WEYL (T.). Creolin.CLAUS (A.) and J.HIBSCH.Metacresols.SCHWEITZER (W.). Derivatives of Hydroxyquhob.LEVY (S.) and E.JEDLICKA.Products of Decomposition of Chlor. Brom.,PALNER (A.W.). Pentamidotoluene.HINRICHSEN (W.). Metaxylylamidomethane.RWGEEIMER (L.). Dibenzamidodihydroxytetrene.JANOVSKY (J. V.) and K.REIMANN.Two Isomeric Azoxytoluenee derivedMARCKWALD (L.). Derivatives of Phenylhydrazine.CUXTIUS (T.) and R.JAY.Condeneation Products of. Hydrazine with Alde-TRAUBE (W.). Additive Compounds of Cyanic Acid.NOYES (W.A.). Oxidation of Benzene-derivatives with Potassium Per-LIEBERMANN (C.) W.DROILY and 0.BERGFAMI.y- and 8-Isatropic AcidsEINEORN (A.) and C.GEHRENBECK.ParanitrophenylbutinecarboxylicAcids.LIMPBICHT (H.).Hydrazinesulphonic Acids and Triazo-compounds .POLIS (A).Aromatic Lead Compounds.DENNSTEDT (M.).Conversion of Pyrroline-derivatives into Indole-deriva-SCHUTZ (H.).Derivatives of Paradiphenol.AUWERS (K.) and V.MEYER.Isomerism of the Benzildioximes.ONUFBOWICZ (S.). &Naphthol Sulphide.MELDOLA (R.). Evidence as to the Quantivalence of Oxygen derived from.KLINGER (H.). Action of Sunlight on Organic Compounds.WEBSTEB (C.S.S.) and L.GI.HUNT .LIEBERMANN (C.) and L.SPIEQEL.Chrysene Hydrides.SHKATELOFF (V.). Chemical Composition of the Russian White Resin fromPinus sylvestris.CIAMICIAN ((3.) and P.SILBER.Apiole.ARNAUD.Crystalline Compound from glabrous Stmphantus.TANRET (C.). Ergosterin.MAGNANINI ((3.).Derivatives of Metadimethylpyrroline.KNORX (L.) and H.LAUBMANN.Pyrazole and Pyrazoline.DOBNER (0.1. a-Alkglcinchonic Acids and a-Alkplquinolines.DOBNER (0.) and P.KUNTZE.a-Phenylnaphthacinchonic Acids.PFITZINQER (W.1. Quinoline-derivatives of Isatinic Acid.HANTZSCH (A.). Azoles.ARAPIDES (L.). Conversion of Ketone Thiocyanates into Oxythiazoles .AEAPIDES (L.). Isothiocyanoacetic Acid.TEAUMANN (V.). Amidothiazoles and their Isomerides.CLAUS (A.) and A.EDINGIER.Isoquinoline.COLSON (A.). Base derived from Diqiiinoline.PAUL (B.H.) and A.J.COWNLEY.KNORR (L.). Morphine.HESSE (0.). Water of Crystallisation in Morphine.ROSER (W.). Narcotine.SEVI TER (E.v.). Additive Compound of Papaverine with PhenacylBromide.Substituted Pyromucic Acidsthe Study of the Azonsphthol CompoundsAction of Halogens on RufigallolWARDEN (C.J.H.).Embelic Acid.Alkaloid from Tea393407417LIEBERMANN (C.). Cocai’nes.FRANKFELD (H.). Cinnamic Acid in the Products of Decomposition ofCoca’ine.EINEOHN (A.). A Metameric Cocai’ne and its Homologues.JAHNS (E.). Alkaloids of Areca Nut.CONINCK (0.DE).Ptoma‘ines.WYBORN (J.M.).JOLIN (S.). Acids of Pig’s Bile.CHITTENDEN (R.H.) and A.8.HART.Elastin and Elastoses.KUHNE (W.) and R.H.CHITTENDEN.Myosin and Myosinoses.LEWITH (S.).HOFMEISTER (F.). Action of Salts on Prote’ids.GUIQNET (C.E.). Soluble Prussian Blue.LENGFELD (F.). Relative Stability of the Alkyl Bromides.BORQMANN (E.) and W.FRESENIUS.~POLETBEFF (G.). Boiling Points of Secondary Alcohols containing Secon-REBOUL (E.).Butyl Ethers.FISCHER (E.) and J.TAFEL.VINCENT (C.) and DELACHANAL.Extraction of Sorbite.MEUNIER (J.) Dibenzoic Acetal of Sorbite.JUNQFLEISCH (E.) and L.GRIMBEBT.Invert Sugar.Fermentation of Galactose Arabinose,Sorbose and other Sugars.STONE (W.E.) and B.TOLLENS.ArabinoseF~SCHER (E.) and J.HIKSCHBERQER.Mannose.FISCHER (E.) and B.PASSMORE.Formation of Acrose from FormaldehydeFISCHEB (E.). Compounds of Phenylhydrazine with Sugars.FISCHER (E.) and J.TAFEL.Synthetical Experiments in the Sugar-RAPMANN (B.) and K.CHODCCNSKP.Rhamnodiazine.FISCHER (E.) and 3.MEYER.Oxidation of Milk-sugarGABRIEL (S.). Derivatives of Trimethylenediamine.FISCHER (E.) and W.J.LAYCOCK .KOLL (A.). Chlorocrotonic Acids.DELIST~E (A.).Ketosulphides a. nd Ketosulphide Acids.SEISSL (J.). Ketonic Acids.WAGNER (R.). Potassium Antimony Oxalate.(Ketipic Acid) and Diacetyl.VOSWINKEL (A.). Paradiethylbenzene.Hy drosulphides.STAEDEL (W.). Nitrometacresols.NEF ( J.U.). Constitution of the Anilic AcidsJACOBSON (P.). Dehydrothiotoluidine.LIJIPACH (L.). Metamidoparacresyl Methyl Ether.Ptoma’ines and their Genesis in Relation to SepsinePOHL (J.).Artificially prepared Nucle’ins.Action of Salts on the Prote‘ids of SerumAnalysis of Pure SherryOxidation of GlycerolSTONE (W.E.) and B.TOLLENS .HAYMANN (F.H.). Action of Sulphurous Anhydride on Tiglic Aldehyde .Metacetone.MOSCHELES (R.) and H.CORNELIUS.Molecular Weight of Pentic Acid .J~ISCHOFF (C.A.) and E.VOIT .FITTIQ (R.) C.DAIMLER and H.KELLER.Diacetyldicarboxylic AcidFRANCHIMONT (A.P.N.) and E.A.KLOBBIE.Some Nitramines and theirDerivatives.FILETI (M.) and F.CROSA.Nitrobromocvmene and Nitrochlorocymene .FILETI (M.) and F.CROSA.Oxidation of the Chlorocymene and Bromo-FUCRS (I?.).Behaviour of Phenols and Hydroxy-acids towards AlkaliSymmetrical Dimethylsuccinic AcidsMARGULTES (0.).IGIRARD (c.) and L.L’HOTE .Action of Methyl Iodide and Potash on Phloroglucinol .Aniline Chlorate and Perchlorate.FISCHER (0.) and E.HEeP.Oxidation of Orthophenylenedi~mine .BEHREND (R.) and K.LEUCXS.Benzyl-derivatives of HydroxylaminePAUE477487497UONTENTS.xxiiiPOSP~CHOFF (V.). Some Derivatives of Orthazotoluene.BISCHLER (A.). Orthonitrophenylhydrazine.ZINCKE (T.) and H.ARZBEEQER.Azimido-compounds.HIRSCH (R.).Theory of the Formation of Aniline-blue.GATTERMANN (L.) and G.WICHMANN.Aldehyde-blue.REYNOLDS (J.E.).MICHAELIS (A.). Aromatic Boron and Silicon Compounds.HONIQ (M.). Preparation of Terephthalaidehyde.ENQLER ( C.) and 0.ZIELKE.Acetophenone-derivatives.HAUSENECHT (G.). Derivatives of Phenylacetic Acid and PhenylglyoxylicAcid.LUFF (G.). Nitrohydroxycinnamic Acids.CONRAD (M.) and F.ECKHARDT.Action of Methyl Iodide on Ethyl Phenyl-ENQLER ( C.) and 0.ZIELCKE.Preparation of Nitromaridelk Acid .NEF (J.U.). Tautomeric Compounds.ULZER (l?.). Derivatives of Resorcinolsulphonic Acid.NENCKI (M.).Preparation of Tetramethyldiamidotriphenylmethane .HIRSCH (R.). Diphenyl Ether and Dinitrodiphenyl Ether.BISCHOFF (E.).Action of Nitrous Acid on Tetramethyldiamidobenzophe-BISCHOFF (E.). Derivatives of Deoxybenzo‘in.STIERLIN (R.). Benziles.NIETZKI (R.) and J.ZUBELEN.Nitration of Naphthionic Acid.RABE (H.). Action of Phosphoric Chloride on B-Hgdroxynaphthoic Acid .IMMERHEISER (C.).Constitution of P-Naphthplamine-a-sulphonic Acid .PFITZINQEB (W.) and C.DUISBERG.Constitition of p-Naphthol-a-sulpho-NIETZKI (R.) and J.ZUBELEN.6-Naphthol-a-sulphonic Acid.KRAVKOFF (N.).Unorganised Ferments.MEYEE (V.). Ring-formation with Elimination of a Nitro-group from theBenzene-nucleus.PELLIZZARI (G.). Compounds of Alloxan with Pyrazolic Bases.BAMBERGFER (E.). Reduction of Quinoline-derivatives.BISCHOFF (C.A.). Quinoline-derivatives from Ethyl Orthonitrobenzoyl-CONRAD (M.) and F.ECKHARDT.Methylquinaldone and Methyllutidone .GERDEISSEN.Metamidoquinaldine.ECEHARDT (F.).Metayuinaldineacrylic Acid and Metaquinaldinealdehyde .RHODE (G.).2’ 3’-Dimethylquinoline.ENQLER ( C.) and A.BAUEB.Action of Acetone on Ortho- and Pam-amido-SEITZ (I?.). B.NapEithaquinaldine.IMMERHEISER (C.). Oxidation of P-Naphthaquinolinesulphonic Acid .BULACH (W.). Condensation of Paranitrobenzaldehyde with Quinaldine .KRUQER (A).The Sulphur of Prote’ids.CHITTEXDEN (R.H.) and G.W.CuMmNs.Myosin.CHITTENDEN (R.H.) and others.Caseoaes Caseln Dyspeptone and Case‘in-HERMANN (L.). Reduced HRemoglobirr.LAMBLINGF (E.). Reducing Action of Indigo-white on Oxyheemoglobiil .MACMUNK (C.A.). Pigments of the Urine.HELL (C.) and C.HAQELE.MESLANS (M.).Propyl and Isopropyl Fluorides.HOLZ (0.). Brominated Derivatives of Pseudobutylene.PWCEERT (M.).Conversion of Crotonylene Hydrobromide into Bromopseudo-WISLICENUS (J.). Arrangement of the Atoms in Space.MEYER (E.v.). Constitution of Cyanethine and its Analogue6.MEYEP (E.v.). Polymerides of the Nitriles.Silico-organic Compound of a New TypeThe Hydrocarbon C60H1BPAQE510520576DITTMAX (W.) and C. A. FAWSITT. Physical Properties of Methyl AlcoholLEGLER (C.). Products of the Slow Combustion of Ethyl Ether.THYLMANN (V.) and A. HILGER. Products of Alcoholic Fermentation,MEUNIER (J.). Combination of Mannitol with' Aldehydes of the AceticSeries.VINCENT (C.) and DELACHANAL. Sorbite and its Occurrence in the FruitsKILIANI (A.) and C.SCHEIBLER. Quercitol.LINDET (L.). Saccharification of Dextrin by Diastase.LOEW (0.). Formation of' Baccharoses from Formaldehyde.LOEW (0.). Formose.CLAISEN (L.) and 0. MANASSE. Conversion of Ketones into NitrosoketonesENGLER (C.).CURTIUS (T.). Constitution of Diazo- and Azo-compounds of the FattySeries and of Hydrazine.PUCEERT (M.). Bromine Additive Products of Angelic and Tiglic Acids .HALLER (A.) and A. HELD. Ethyl Chloracetoacetates.BARTHE (L.). Synthesis by Means of Ethyl Cyanosuccinate.GUINOCHET (E.).KILIANI (H.). Oxidation of Galactosecarboxylic Acid.EILIA'NI (H.). Metasaccharic Acid.GABRIEL (S.) and K KROSEBERG. Preparation of Glycocine.PIUTTI (A.). Ethyl E'umarimide.PIUTTI (A.). Asparagines.PATERNB (E.) and A.PERATONER.FITTIG (R.). Condensation of Ethereal Salts of /3-Ketonic Acids withBibasic Acids.EYNERN (F. v.).FEIBT (P.). Salts of Uvic Carbuvic and Ethylcarbuvic Acids.DIETZEL (A.). Ethyl Acetoacetate and Pyruvic Acid.SCHLOESSEB (A.). Succinic Acid and Ethyl Benzoylacetate.BIDET (A.).MEYER (V.). Aromatic Nitriles Benzyl Cyanide and Hydrrttroponitrile .JANSSEN (H.). Replacement of the Methylene Hydrogen-atoms in BenzylCyanide.NEURE (K.). Replaced Benzyl Cyanides.FROST (H. V.). Condensation of Benzyl Cyanide and its Substitution-SEELIG (E.). Action of Chlorine and Bromine on Benzyl Acetate .ZINCKE (T.) and F. KUSTER. Action of Chlorine on Catechol and Orth-HEMPEL (A.). Orthonitroethylaniline and its Derivatives.HELL (C.) and T.ROCKENBACH. Last Runnings obtained in the Purifica-GATTERMANN (L.). Action of Sulphur on Toluidine.ANSCHUTZ (R.) and Gt. SCHULTZ. Behaviour of Primary Aromatic AminesWITT (0. N.) E. NOLTINB and S. FOREL. Preparation and Properties ofParaxy lidine.NIETZEI (R.) and E. MULLER. Symmetrical Tetramidobenzene.FRIEDLANDER (P.). Short Communications.BECEMANN (E.). Isomerism of Oximido-compounds Isomeric Monosub-BECKBZANN (E.). Isomerism of Oximido-compounds.AUWERS (E.) and V. MEYEB. Isomerism of Oximido-compounds .MUHLHAUSER (0.). Manufacture of Benzyl-violet.ABT (W.). Benzoglenecarbamide.STRASSMANN (H.). Action of Hydroxylamine on Bromacetophenone .NOLTINQ (E.) and 0. KOHN. Sulphonic Acids of Meta- and Para-xylidine .Decomposition of Fatty Acid by Heating under PressureAction of Bromine on Aconitic and Carballylic AcidsAttempts to prepare Titanium EthylCondensation of Ethyl Acetoacetate and Succinic AcidEffect of Thiophen on the Cblour of Benzene-derivatives58859761CONTENTS .AUWERS (K.) and V.MEYER.Two Isomeric Benzilemonoximes.BRAIJN (E.).Aldine Formation.GTJDEMAN (E.). Aldine Formation.HELL (C.). Pichtelite.FRIEDLANDER (P.) and 0.BOCKXANN.Naphthaquinonedichlorodiimide .WOLFFENSTEIN (R.). Constitution of a-Hydroxynaphthoic Acid .Constitution of Filicic Acid.BARBCER (P.) and J.HILT.Australene.JAHNS (E.). Oil of Myrtle.CAZENEUVE (P.). Nitrocamphor.CAZENEUVE (P.). Nitrophenol Isomeric with a-Nitrocamphor.CLAISEN (L.) and 0.MANASSE .HALLER (A).Normal and Acid Ethereal Salts of Uamphols.HALLER (A.).Phthalates of Camphols.GRAF (B.). Dammara Resin.REYCHLER (A.). Artificial Diastase.SCHUTT (F.).Phycoerythrin.FEHRLIN (H.C.). Bidesyls.ENGLER (C.) and W.KIBY.WOHL (A.) and W.MARCKWALD.Condensation-prodncts from Amido-KNOLL (A.). Code’ine.SKRAUP ( Z.H.). Constitution of the Cinchona AlkaloYds Quinine .SCHNIDERSCHITSCH (H.).Constitution of the Cinchona Alkalo‘ids Cin-WURSTL (J.). Constitution of the Cinchona AlkaloYds Quinidine .GARZAROLLI-THURNLACKH (K.v.). Strychnine.FREUND (M.). Hydrastine.MARFORI (P.).Berberine.EINHORN (A.). Alkalo’ids occurring with Cocabe.MALY (E.). Oxidation of Gelatin with Potassium Permanganate .SCHWARTZ (A.). Reciprocal Action between Hemoglobin and Protoplasm .HOLTZWART (R.). Dimolecular Methyl Cyanide.WACHE (R.).Polymerides of Nitriles.MEYER (E.v.). Cyanethine and its Derivatives.PALMER (C.). Constitution of Ally1 Cyanide.DROUIN (R.). Succinamonitrile.MALBOT (H.). Preparation of Alkyl Chlorides from Alcohols.REISS (R.). Seminose.PISCHER (E.) and J.HIRSCHBERGFER.Mannose.BAITER (R.W.). Sugar-like Compound from Laminaria.HOFMANN (A.W.).KRAFFT (N.) and A.MOPE.Conversion of Palmitonitrile into Hexadecyl-DE PORCRAND.Combination of Chloral with Glycol.ATJWERS (K.). Preparation of Oximes.WILLGERODT (C.) and F.DURR.Derivatives of Solid Acetone-chloroform .GROGER (&I.). Dihydroxystearic Acid.ERAFFT (F.) and H.NOERDLINGER.Boiling Points in the Oxalio and OleicAcid Series.MASSOL.Calcium and Strontium Malonates.ZELINSKY (N.) and S.KRAPIVIN .BALLO (M ).Reduction of Tartaric Acid.BUCHNER (E.).Action of Methyl Diazoacetate on Ethereal Salts of Un-SELL (W.J.). Base containine Chromium and Carbamide.GUARESCHI (J.). /3.Chloro.a.Bromonaphthalene.PAT ERN^ (E.).PAPASOGLI (G.). Spontaneous Oxidation of Essential Oils.Nitrosocamphor and CamphorquinoneBISCHOP (A.W.) and L.C‘LAISEN.Camphoraldehyde.&Methyl Pyridyl KetoneAmines of the Methyl and Ethyl SeriesSymmetrical Dimethylsuccinic AcidsPAGE620629690QUIN~KE (F:).Aluminium &&hide. 69PAQEHILL (H.B.). Methylfurfuraldehyde and the corresponding Methyl-JACKSON (C.L.) and W.D.BANCROFT.Tetrabromodinitrobenzene.696BUCHKA (K.). Preparation of Metanitrotoluene.696KRAFFT (F.) and A.v.HANSEN.Tricyanides.696WILLGERODT (C.) and A.KOLE~BSWM .Solution.607SCHALL (C.).Metamidoparacresyl Methyl Ether.698LIMPACH (L.). Amidoparacresyl Methyl Ether.698LIEBERMANN (C.) and 0.BERGAMI .LLOYD (R.).AUSTEN (P.T.) DiamidophenylThiocyanate.700XULLER (E.). Oxidation Prodnct of Triauiidobenzene. 700BUCHKA (K.) and F.SCHACHTEBECK.Reduction Products of Metanitro-FISOHEE (0.) and L.WACKER.Action of Nitroso-bases on Phenyl-BLADIN (A.J.). Compounds derived from Dicyanophenylhydrazine.702BEHREND (R.) and K.LEUCHS.Benzyl-derivatives of Hydroxylamine.$03PINNER (A.) and A.SPILKER.Eydantoyns. 704KEHRXANN (F.).ANSCHUTZ (R.). Reissert's Anilosuccinic Acid and Anilopropionic Acid.707ERLENMEYEE (E.) Jun.Substituted Q-lycine Anhydrides.708GLEDITSCH (A.) and H.MOELLER.Three Isomeric Toluric Acids.'708EGEL (E.).Derivatives of Paranitrometamidobenzenesulpbonic Acid.708FAHLBERQ (C.) and R.BARGE.Sulphobenzoic Acid and its Derivatives.709Iodation of Phenols in AmmoniacalAction of Sulphuric Acid on y- andConversion of some Homologues of Phenol into Primary andSecondary Amines. 700GIRAUD (H).Methyltlcetanilide.704Quinones. 707BARTHE (L.). Ethyl BenzplcTanosuccinate.708REYSEN (I.) and A.F.LINN.SulphonephthaleSns.710KASTLE (J.H.). Paranitro-orthosulphobenzoic Acid.711Potassium Ferricyanide.'711PECHMANN (H.v.). Diphenyltriketone. 712BAMBERGER (E.). Fichtelite.714CLAUS (A.). A New Dihydroxpaphthalene.714KRAFFT (F.) andR.SCHBNHERR.Thionaphthols.715BAMBERGER (E.) and P.BOXDT.a-Tetrahydronaphthylamine.715HINSBERG (0.). 1 1'-Naphthylenediamine.'717ANSELM (F.). Hydronaphthalic Acid. 717BENDER (F.). a-Naphtholsulphonic Acid. 717KBNIG (K.). Hydroxysulphonaphthoic Acids.'719SCHOELLER (A.). Hystazarin Compounds. 719Hydrocarbons. 719BECKMANN (E.). The Camphor Series. 721HOOPER (D.). Gymnemic Acid.723HANTZSCH (A.). Thiazoles from Thiamides.'723POPP ((3.) Thiazolee from Amidothiazoles. 724Ethyl Acetoacetate.725Action of Alkalis and Ammonia on Halogen-substitutedNOYES (W.A.) and W.B.WILEY .ZATTI (C.). Action of Acetic Anhydride on 2'-Indolecarboxylic Acid.712ELBS (K.) and H.FORSTEL.Diphenyltrichloroethane. 713AUWERS (K.) and V.MEYER.713Oxidation of Benzene-derivatives withThe Third Benziledioxime.BAMBERGER (E.).Relations between the Chemical Properties and Constitu-FORSLING (S.).Constitution of B-NaphthSlamine-a-Euphonic Acid.'718LIEBERMANN (C.) and L.SPIEGEL .CAZENEUVE (P.). Reduction of Nitrocamphor to Nitrosocamphor.720Perhydrides of the Higher AromaticZURCREB (H.).Action of Thiocyanates and Thiocarbamide on ChlorinateCONTENTS.xx viiHOFMANN ((3.). Selenazole Compounds Selenocyanogen.CLAMICIAN (G.) and C.M.ZANETTI .CIAMICIAN (Q.) and F.ANDERLINI .BUCHKA (K.) and C.SPRAGUE .Direct Synthesis of Homologues ofPyrroline.Adion of Methyl Iodide on a-Nethyl-Formstion of Pyridine from Amidoazo-pyrroline.CLAUS (A.) and H.DECKER.y-Bromoquinoline.MAGNANINI (G.) and H.ANGELI.Constitution of LepidineCOLSON (A.). Artificial and Natural Alkalolds.DRESER (H.).Acid Nicotine Tartrate.FISCHER (0.). Harmine and Harmaline.HEME (0.). Coca Bases.LIEBERMANN (C.). Hygriue.CONINCK (0.de).Ptomalnes.MALBOT (K.). Action of Hydriodic Acid on Ally1 Iodide.JAHN (K.). Synthetical Formation of Formaldehyde.POHL (0.).WISLICEKUS (W.).Ethyl Oxalosuccinate.RIDEAL (S.). Organic Boron Compounds.LIEBERMANN (C.). Coca Bases.LIEBERMANN (C.) and W.DRORY. F- and yJsatropylcocalneAction of Acid Chlorides on Arsenic Trioxide.KLINGBMANN (F.). Action of Aromatic Amines on Acetylcitric Anhj dride .NIETZKI (R.) and H.ROSEMIINN.Oximes of Leuconic Acid and theirReduction Products.MIXTER (W.G.) and Y.KLEEBERG.Nitro-derivatives of Oxalotoluidide .JACOBSON (P.) and E.NEY.Aromatic Ozthamidomercaptans.GOLDSCHMIDT (H.) and A.GESSNER.Cumylamine.GOLDSCHXIDT (H.) and V.BADL.Diazoamido-compounds.BERNTHSEN (A.).Methylene-blne Group.SCHULZE (W.). Derivatives of Metamidobenzamide.TKJMMELEY (E.). Azo-compounds of Salicaldehyde Salicyl Alcohol andSalicylamide.GEBEK (L.). Azo-compounds of Salicylic Acid.JACKSON (C.L.) and G.D.MOORE.Ethyl BromodinitrophenylacetoacetateWICHELHAUS (H.). Diamidobenzophenone.BECKMANN (E.). Behaviour of Ketones and Aldehydes towards Sodium inBAMBERGER (E.) and J.HOSKYNS- ABRAITATXG.1 4'-Tetrahydronaphthylene-BAMBE KGER (E.) and J.BAMMANN.1 J 4'-TetrahydronaphthylenediamineRUHARA (M.). Specific Volumes of Camphor and Borneo1.HINSBERG (0.). Piaselenoles.LIMBWJRG (P.). Solution and Precipitation of ProteTds by Salts .HOPPE-SEPLER (F.).Blood Pigments.HIRSCHFELD (E.). Black Pigment of the Choroid.B ~ H A L (A.). Hydrocarbons of the C,H,,- 3 Series.HITZEMANN (C.) and B.TOLLENS.Hexyl Iodide from Sorbite.HANRIOT (M.) and L.BOUVEAULT.Products of the Polymerisation of EthylMALBOT (H.) and L.QENTIL.Action of Zinc Chloride on I'sobutyl i c o h o iSCHOPFF (&I.). Diphenylamine-derivat ives.THOISS (G.). Adenine.Cyanide.LIPP (A.). Normal Acetopropyl Alcohol.LAMBERT (A.).Action of Borax on Polyhydric Alcohols.HEFFTER (A.). Action of Chloral on Glucose.PBRIEB (L.).' Solubility of Sugar in Water.BEYTHIEN (A.) and B.TOLLENS.Compounds of Ra5nose with Bases.896PAQ E'729'731'732'732'733'766'769'771'771'781'781'786'787WHEELER (H.J.) and B. TOLLENS. Xylose and Wood Uum.GUIGNET (C. E.). Colloidal Cellulose.GABRIEL (S.) Bromethylamine and its Derivatives.CLAISEN (L.) and E. F. EHRHARDT. Preparation of Acetylacetone and itsHomologues.COMBES (A.). Action of Diamines on Diketones. ~ FROMM (E.) and E. BAUYANN. Thio-derivatives of Eetones.HANTZSCH (A.). Products of the Action of Chlorine on Phenol in AlkalineSolution.-.HOFFMANN (C.). Trichlorodihydroxypenteneca&oxylic Acid.XILIANI (H.). Aldehydegalactonic Acid.HEFFTER (A.). Preparation 0% Gluconic Acid.MASSOL. Ammonium Malonates. .PBCHARD (E.). Oxalomolybdic Acid and its Salts.HALLER (A.). Ethereal Salts of Cpnomalonic Acid.GERNEZ (D.). Comhination of Normal Molybdates with TartaPic h i d .GUTHZEIT (M.) and 0.DRESSEL. Ethyl Ethoxy-a-pyronedicarboxybte ,HOTTER (E.). Aconitic Triamide.ROSSOLYMO (A.).Substitution 08 tihe Mathylene-Hydrogen Atoms inGATTERMANN (L.) MAISCH and EHRHARDT. Akline-de~vatives oiPhenylic Ethers.BEBTRAM (J.). and E. GILDMEISTER. Betei Oil.LAMBERT (A.). Action of Borax on Polyhydric Alcohols.LEUCKART (R.) and W. HOLTZILPFEL. Azobenzeneacetoacetamide .JANOVSKY (J. V.). Azoxytoluene.BANKIE WICZ (2.)” Reduction Products of Metanitroparacetotoluidide.WOHL (A.) and W. MARCKWALD. Condensation Products of Amidoacetal .PFITZINBER (W.) and L. GATTERUNN. Constitution of Primuliue .GATTERMANN (L.) and P. JACOBSON. History of Primuline.KOSTANECKI (S. v.). Substawes which form Coloured Compounds withMordants._.ENECHT (E.) and J.R. APPLEYARD. Tho Theory of Dyeing.GABRIEL (S.).Amidomercaptan.JEANRENAUD (A.). Action of Hydroxylamine on Ethereal Salts.HECTOR (D. S.).Action of Hydrogen Peroxide on Phenylthiocarbamide .BRADLEY (W. P.). Disalicaldehyde.HALLER (A.). Cyanacetophenone and its Denivatives Synthesis of a-Ke-STARTING (A.). Preparation of Benzoic Acid.JACOBSEN (0.). Pentamethylbenaoic Acid and Durenecarboxylic Acid .ARONSTEIN (L.) and A. F. HOLLEYAN. Conversion of Acetylene intoEthylene-derivatives by the Direct Addition of Hydrogen.BONIBER (M.). Ethyl Dihydroxyquinonedicarboxylate andita Hydro-deriva-JACKSON (0. L.). Constitution of Ethjlbromodinitrophenylmalonate .CLAUS (A.) and W. FAHRION.LERCH (J. 2.). Orthonitrosulphanilic Acid.REMSEN (I.).Orthosulphobenmic Acid and its Derivatives.HANEIOT (M.) and 0. SAINT-PIERRE. Action of Potassium on Triphenyl-AUWERS (K.) and V. MEPER. Tetraphenylsuccinonitrile.STRASSMANN (H.). Isomeric Methyldeoxybenzohs.LEUCKART (R.) and H. JANSSEN. Actionof Ammonium F m a t e on De-BOURCABT (E.). Bromo-derivatives of Dibenzyl Ketone.KLINGER (H.) and 0. STANDKE. Bendic Acid and its Derivatives .GRABBE (C.). Synthesis of Euxanthone.ZINCKE (T.). Action of Chlorine on ,%Naphthol.Benzyl Cyanide.CLAUS (A.) and A. D~REHER. Metacresol.Carvole and Carvacmlsulphonic Acid .Pk6&B8618 73886COXTENTS.xxixKOSTANECKI (S.v.). Nitroso- and Dinitroso-naphtharesorcinol.BAMBERGER (E.) and R.MULLEB .BAMBEEGER (E.) and H.HELWIU .BAMBERGEE (E.) and W.J.SCHIEFFELIN .Reduction of Alkjl-~-naphth-ylamines .Reduction of Secondary and TertiaryAlkyl-naphthylamines.Hy$rogenation of 1 2- and 1 4-Naphthylenediamine Preparation of 2 2 -Naphthylenediamine .RUEFF (L.).P.Dinaphthylparaphenylenedianiine.FORSLING (S.)./3-Bromonaphthalenesulphonic Acids.HALWARTEN (F.). Propyl-derivatives of Anthranol.BOUCHARDAT ((3.) and LAFONT.Action of Heat and Acetic Acid on FrenchEssence of Terebenthene.F’LIEDEL (C.). Mesocamphoric Acid.KOWALEWSKY (N.). Action of Ozone on Guaiacum Resin.ARNAUD.Tanghinin from Tanghinia Yenenifera.MACCHIASI (L.). Xanthophjllidrin.MAGNANINI ((3.). Behaviour of Pyrroline and its Derivatives as regardsRaoult’s Law.LELLM A NN (E.).ConiwYns.LEZLMANN (E.) and R.SCHWADERER .LXCLLMANN (E.).Pdyrnerisation of Compounds containing doubly-boundCarbon-atoms.BUNZEL (H.). Oxidation of a-Pipecoline.LELLMANN (E.) and C.SCHLRICH.Formation of Colouring Matters fromParadiamidodiphenylpiperazine.LELLMANN (E.) and H.REUSCH .ENORR (L.). Morphine.JUNGPLEISCH (E.) and E.LBGER.a-Hgdroxycinchonine.HESSE (0.). New Compounds of the Cinchona Alkaloids.FREUND (M.). Hydrastine.EINHOBN (A.). Conversion of Anhjdroecgonine into Pyridine.KRUGEE (A.). Chemistry of Gluten.NEUMEISTEE (x.). Products of the Action of Superheated Steam onFibrin.ROMANIS (R.). Burmese Petroleum.Q-USTAVSON (G.) and N.DEMJANOFF.Pentamethylene and TetramethyleneBromides.B~HAL (A.). Formation of Hexylacetylene from Methylvaleryl-AcetyleneRAMMELSBERG (C.).Ferricyanides.WILM (T.).Derivatives of Potassium Platinocyanide.SMOLKA (A.) and A.FEIEDREICH .WILL (W.) and C.PETERS.Oxidation of Rhamnose (Isodulcitol) .WEDENSKY (W.).PLATH ((3.). @Ethyl-ci-Stilbazole and its Derivatives.PipeTide‘ine and Dipiperide’ineQuinoline and TetrahydroquinoliiieMERCK (E.). Meconarceihe and h’arce’ine Meconate.STOEHR (C.). Constitution of Ecgonine.OTTO (R.). Discovery of the Normal Tricyanides.KRAFFT (F.). Synthesis of Cpanphenin.GARZINO (L.). Bromotrimethyl Carbinol.EEWIG (E.) and W.KOENIGS.Pentacetyldextrose.SCHEIBLER (C.) and H MITTELYEIER.Melitose (Raffinose).VAN DEE ZAHDE (K.H.M.). Diisopropglamine.ZINCKE (T.) and 0.KEUEL.Symmetrical Tetrachloracetone.MAQTJENNE.Preparation of Concentrated Formic Acid.HAZTJRA (K.).Drying Oils.Derivatives of Cyanamide.Action of Ethyl Iodide and Zinc on Paraldehyde .GRUSSNEE (A.) and K.HAZURA.Oxidation of Unsaturated Fatty Acids .HELL (C.) and S.TWERDOMEDOFF.Derivatives of Myristic Acid .FEIST (F.). Dehydracetic Acid.OTTO (R.) and J.TROGER.Synthesis of ietonic Acids by the Action ofAcid Chlorides on Propionitrile.CASTELAZ (J.). Manganese Oxalate.PAGE9019509 56B ~ H A L (A.) and V. AUGER. Action of Phosphorus Pentachloride onMalonic Acid.MASSOL. Barium Malonates.JOULOWSKY (8.).HELL (C ) and M. ROTHBERG.BISCHOFF (C. A.) and P. WALDEN. Disubstituted Succinic Acids .ZANETTI (C. U.). Thiosuccinic Anhydride.ANDREASCH (R.). Thiocarbimidacetic Acid and Rhodanic Acid.FREYDL (J.). New Synthesis of Rhodanic Acid.TAFEL (J.).y-Amidovaleric Acid.OEIXERS (L.). Oxamic Acid. ,VAN DEB ZANDE (I(. H. M.). Unsymmetrical Dialkylcarbamides .TI~ATJBE (W.). Derivatives of Allophanic Acid.WILLGEROT (C.) and R. WOLXIEN. Chlorobromoparaxylenes and theirDerivatives.REAUBRPAIRE. Preparation of Durene and of Benzyldurene.Heazrs (J.) and 8. ZEISEL. Desmotropp in Phenols.ZINCKE (T.) and 0. KEGEL. Action of Chlorine on PhloroglucinoI .NIETZKI (R.) and F. SCHMIDT. Derivatives of Symmetrical Dihydroxy-EEHRMANN (F.) and R. BRASCH. Tolunitranilic Acid Nitro-derivatives ofToluquinol.UEORGESCO and MINCOU. New Francei’n from 1 3 4 5-letrachloro-PICTET (A.) and R. BUNZL.VAN RONBURGH (P.). Trinitrophenylinethytnitramine.VAN ROMBURGH (P.). Action of Chromic Anhydrid on Alkylanilines .SODERBAUV (K.(3.) and 0. WIDNAN. Derivatives of OrthamidobenzylAlcohol. -.BANDROWSKI (E. v.). Oxidation of Paraphenylenediarnine and of Paramido-NIETZKI (R.) and L. SCHMIDT. Consecutive Tetramidobenzene .REMSEN (I.) and R. 0. Q-XAHAM. Decomposition of Diazo-compounds .TAFEL (J.). Reduction of Hydrazones.FREUND (M.).Conversion of Trinitrohydrazobenzene into Nitrosodinitro-BLADIN (J. A.). Amidoximes and Azoximes of the Triazole and TetrazoleSeries.BERREND (R.). Alkyl-derivatives of Hjdroxylamine. .BECKMANN (E.). Isomerism of the Benzaldoximes.EECKMANN (E.). Benzaldoximes.HOOOEWERFF (S.) and w. A. VAN 1)ORP. Action of Potassium HypobromiteHAFNER (A.). Compounds of the Benzyl Series.MOORE (I.) Condensation Products from Aromatic Carbodiimides andOrthodittlrnines.PINNEE (A.).Benzaldehyde.MILLER (W. v.) and G. ROHDE. Synthesis of Tndine-derivatives.BBHAL (A.). Action of Phosphorus Pent achloride on Acetophenone .WILLGERODT (C.) and H. SALZMA”. Halogen-derivatives of Toluene andALT (H.). Bromination of 0rthacetyl.imidobenzoic Acid.CLAW (A.) and H. KUNATH. Bromotoluic Acids.CLAUS (A.) and N. DAVIDSEN. Chloroparatoluic Acids.EELILNMEYER (E.). Behaviour of Ammonia and Organic Bases with SodiumPhenoxy acrylate.MILLER ( W. v.) and F. KINEELIN. Orthocoumaric and Orthocoumarinic SeriesMILLER (W. v.) and F. KINEELIN. Transition from the Coumaric to theQuinoline Series.ERLENMEYER (E.). Synthesis of Phenylpyruvic Acid.Action of Ethyl Iodide and Zinc on Ethyl MalonateFormation of Dimethylsuccinic Acid .Action of Zinc Chloride on Acetanilide .PAQE967980CONTENTS.xxxiERWIB (E.) and W.KOENIGS.Acetyl-deriratives of Quinic Acid .REMSEN (I.) and A.R.L.DOHME.Orthosulphobenzoic Acid and its DerivativesOTTO (R ) and A.ROSSING.Behaviour of Alkyl-halogen Compounds towardsKEHRMANN (F.). Iodophenolsulphonic Acid Iodophenone.Ethyl Sodophenylsulphonacetate.OTTO (R.) and A.ROSSINQ.Short Communications.JACOBSEN (0.). Action of Sulphuric Acid on Symmetrical Bromopseudo-KURZEL (C.). Action of Sulphuric Acid on Symmetrical Iodopseudo-NIEMENTOWSKI (S.) and B.ROZANSKI.Synthesis of Isatoic Acid .ELBS (K.) and 0.HOLRMANN.Diphenoltrichlorethane and Paradihydroxy-BBHAL (A.). Conversion of Methylbenzylidene Chloride into Triphenyl-BICKEL (H.).Derivatives of Diphenylacetic Acid and of Benzilic Acid .HOOKER (5.C.) and W.H.GREENE.Constitution of Lapachic Acid and itsDerivatives.BAMBERGER (E.) and S.WILLIAMSON.Hydrogenation of ,tl.l)iethylnap h.Camphor and Borneol of Rosemary Separation of CamphorAcetates and Benzoates of Active and Racemic Camphols .Preparation of a Dextro-borneol identical with Dryobalanops Borneol .BRUNNER (K.). Quinol and Quinone of Ditolyl.EKBOM (A.) and R.MAUZELTTJS.Fluoronaphthalenes.EHRLICH (h;.). Oxidation oi @-Naphthol.MauzELIUs (R.). 1 4-Fluornaphtl~alenesulphonic Acid.HALLEB (A.) .HALLER (A.).LEUCKART (R.) and H.LAMPE.Dibornylaniine.BARTH (L.) and J.HERZIG.Constituents of HerniariaSCHALL (C.) and C.DBALLE.Brazilin.PINNER (A.).Amidinev and Pyrimidines.PINNER (A.). Pyrimidines (Metadiazines).BISCHOFF (C.A.) and 0.NASTVOGEL.KetopiperazinesBISCHOFF (C.A.) and 0.NASTVOQEL.a-y-DiketopiperazinesNASTVOGEL (0.). Homologues of Dipheny1.a.y.diketopiperazine.HAUSDORFER (A.).Diphenyl-a-y- and -a-&diketopiperazines.BTSCHOFF (C.A.) and 0.NASTVOGEL.a-P-DiketopiperazinpsBISCHOFF (C.A.). Piperazines.BISCHOFF (C.A.).Hydrogenated Paradiazines of the Aromatic Series.BISCHOFP (C.A.). Characteristics of the Piperazines.TAFEL (J.) and A.NEUGEBAUER.Methglpyrrolidine.GOLDSCHMIEDT (G.) and H.STRACHE.Pyridineorthodicarboxylic Acid .KRAFFT (F.) and I.MAI.Myristic Aldehyde.VAN DER KOLF (A.P.) and P.H.VAN LEENT.Ethyl Cinchonate and Cin-LEIPEN (R.).Caffei'ne.SKRAIJP (2.H.) and D.WIEGMANN.Morphine.EINHORN (A.). Ecgonine and Anhydroecgonine.OUDEMANS (A.C. jun.). Cupre'ine.LADENBURG (A.) and C.OELSCHLAGEL.Pseudephredine.LIEBEBMANN (L.). Nucle'in.SUILLIOT (H.) and H.RAYNAUD.Manufactureof Iodoform.OSSIPOFF (I.). Chlorination of Ethyl Acetoacetate.MICHAEL (A.). Geometrical Constitution of the Crotonic Acids and of theirHalogen Substitution-products.NICHAEL (A.) and P.FREER.Action of Hydriodic Acid on thecrotonic AcidsDBECHSEL (E.). Decomposition Products of Case'in.MONNET.Reduction of Copper Salts by Sugars.LASSAR-COHN.Electrolysis of Organic Potmsium Salts.PAQE100110151057BENEDIET (R.) and K.HAZURA.Composition of Solid Animal and Veget-HAZURA (K.) and A.GRUSSNEE.Non-drying Oils.LANGER (A.).Oily Acids from Lycopodium.RJASANTZBFF.Action of Zinc Ethide Gn Succinic Chloride ; of Zinc Ethide .LUDY (E.). Aldehydic Condensation-products of Carbamide.EYICH (F.). Amides of Carbonic Acid.BREDT (J.) and W.BOEDDINGHOUS.Rischtieth’s y-Valeroximidolactone .CLAUS (A.). Constitution of Benzene.MICHAELIS (A.) and A.MARQUARDT .LAJOUX (H.) and A.GEANDVAL.Mercury Salicylates.PISANELLO ((3.). Sulphonic Derivatives of Salicylic Acid.MICHAEL (A.) and H.PENDLETON.Allo-isomerism in the Cinnamic AcidSeries.KUSSEROW (R.). Derivatives of Anilidosuccinic Acid.LOSSEN (W.). Structural Formulse of Hydroxylamine and its Deriva-NIEMEXTOWSEI (S.). Derivatives of Metatoluquinazoline and Metahomo-WEGERHOFF (P.). Intramolecular Change of the Oximes of Parachloro-GUNTHEX (E.).Intramolecular Change of a- and p-Benzildioxime andWISLICENUS (W.) and A.KOTZLE.Diketohydrindene.WISLICENUS (W.) and A.KOTZLE.Action of Ethyl Propionate on EthylPhthalate.MAUTHNER (J.) and W.SUIDA .WALLACH (0.) and E.CONRADY. Rotatory Power of Terpene-derivatives .COMBES (A.and C.). Synthesis of Hydropyridic Bases.SERAUP (Z.H.) and J.WURSTL.Constitutioii of the Cinchona Alkaloids .Meth y lsuccinimide.Aromatic Bismuth Compounds .SCHIFF (H.).Phloroglucinotannic Acid.Tndole from Phenylamidoacetic Acid .WALLACH (0.). Molecular Refraction of Camphene.WALLACE (0.). Isomerism in the Terpene Group.WALLACH (0.). Terpenes and Ethereal Oils.(Part 11.).MITTMANN (0.). Bay Oil.AHRENS (F.B.). AlkaloYds of Mandragora.DEL~ZINIER (A.M.).A New Ptomaine.CORIN (G.) and E.BERARD.Proteids of White of Egg.MAI (I.). Elimination of Carbonic Anhydride by the aid of SodiumMethoxide.MOLTSCHANOFFSKY (N.).Liquefaction of Propylene Allylene and Tri-KONDAKOFF (I.). Action of Hydrogen Chloride on Dimethylallylene .BEVAD (I.). Action of Zinc Ethyl on Primary and Secondary Nitro-com-BEVAD (I.). Preparation of Secondary and Tertiary Nitro-compounds fromKRAPIVIN (S.) and N.ZFLINSKY.Vapour-density of Ethyl IsocyanurateKRESS ((3.) and H.MORAHT.Double Thiocyanates of Iron and Potassium .EONDAKOFF (I.). Amylene from Tertiary Amy1 Iodide.Halogen-derivatives of Nitromethane.SABANPEFF (A.). Hexabromotetramethjlene.WARKEN (T.T.P.B.) Stability of Fatty GlyceridesSERAUP (Z.H.).Constitution of Glucose.SELIVANOFP (T.). Formation of Cane-sugar from Starch.ERWIG (E.) and W.KOENIGCS.Pentacetylgalactose and Pentacetyldex-PAGE10651126CONTENTS. xsxiiiPAQEFISCHER (E.) and J. MEYER. Oxidation of Maltose. 1132BAUER (R. W.).Fehling’s and Sachsse’s Solutions. 1132GUIGNET (C. E.).GABRIEL (S.). Bromethylamine. -. 1134VILLE (J ). Dihydroxyphosphinic Acids. ,. 1134KLINGER (H.) aud A. MAASSEN. Sulphines and the Valency of Sulphur.1135BAUMANN (E.) and A. KAST. Disulphones. 1136WEDENSKY (V.). Action of Ethyl Iodide and Zinc on Paraldehyde.1136LEVY (S.) and A. CURCHOD. SymmetAcal Tehchloracetone. 1136PECHMANN (H. v.). Reduction of DiacetyE. 1137PECHMANN (H. v.) and R. OTTE. Homologues of Diacetyl.1137KNORR (L.). Preparation of Acetonylacetone from Ethyl Diacetosuccinate.1139DUVILLIER (E.). Diethsmido-a-propionic Acid. ,.1139KOLOTOFP (U. C.). Nitro-compounds of the Fatty Series. 1140DE WILDE (P.) and A. REYCHLER,Acid.1140REYCHLER (A.). Conversion of Erucic Acid into Behenic Acid. 1140SCHULZ (0.). Molecular Weight of the Acids of the Olerc Series.1140MICHAEL (A.).HELD (A.). Derivatires of Ethyl Acetocyanacetate.1141OELKERS (L.). Oxamic Acid.1148EPHRAIM (J.). Dithioxamide (Cyanogen Disulphydmte). 1142TIENANN (F.). Amidoxime of Oxalic Acid. 1142FEANCHIMONT (A. P. N.) and E. A. KXOBBIE.Organic Compounds.1143FRANCHIMONT (A. P. N.).AUWERS (K.) and V. MEYER. Tetramethylsuccink Acid. 1145SEMENOFF (V.). Fumaric and Male’ic Acids.1146FITTIG (R.) and G.PARKER.Acids.-.1146URWANTZOFF (L.). Osidation of Erucic Acid.1146GERNEZ (D.). Action of Malic Acid on Ammonium Molybdate. 1147DIEFF (V.). Oxidation of Ricinoleic Acid.1147BAEYER (A.) and W. A. NOYES. Succinosuccinic Acid ,. 1147MILLER (W. L.). Dihydroxytartaric Acid. 1149FISCHER (E.). Reduction of Acids of the Sugar-group I. 1149HUQOUNENQ (L.).Perchlorination of Phenol.1146MESSINQER (J.) and G. VORTMANN. New Class 0-f Iodated Phenols.1150COLSON (A.). Dyes derived from Benzidine.1152SKRAUP (2. H.). Benzoyl-compounds with Alcohols Phenols and Sugars.1152MARQULIES (0.). Hexamethylphloroglucinol.1153BAEYER (8.) and E. KOCHENDOERFER. Cntecholphthalek. 1153VAN ROMBURQEI (P.).Tetranitrophenylmethylnitramine and its ConversionKEHRMANN (F.).Oxidation of Aromatic Diamines.1154BECHHOLD (J.).Converaion of Phenylazoresorcinol Ethers into Hydroxy-CULMAN (C.) and I(. GASIOROWSPI. Action of Stannous Chloride on SaltsCTJRTIUS (T.). Substitution of the Azo-group for Ketonic Oxygen.1157MICHAELIS (A.). Sodium Phenylhydrazine. 11 58PHILIPS (B.). Action of Alkjl Bromides and of Benzyl Chloride onPreparation of Unsymmetrical SecondaryAction of Acid Chlorides and Anhydrides on SodiumBirotation of Arabinose and its Reducing Value withCombinations of Cupric Oxide with Starches Sugars,Conversion of Ole’ic Acid into StearicRegularities in the Addition of Halogen-compounds to Un-Action of Nitric Acid onInfluence of Certaim Groups on the BehaviourCondensation of Ketonic Acids with RibasicSodium Pheny lhy drazine.Phenylhydrazines.1158Phen ylhydrctzine.115 9SCHMIDT (F.).VOL. LVI. PAGELEVY (S.) and F. 0. WITTE. Action of Phenylhydrazine on Tetrachlor-WIILGERODT (C.) and B. HERXANN. Orthoparadinitrophenyl-phenyl-MICHAELIS (A.) and C. CLAESSEN. Unsymmetrical Secondary AromaticHydrazines containing Unsaturated Alcohol Radicles. 1161BAEFRR (A.) and E. KOCHENDOERFEB. Action of Phenylhydrazine onPhloroglucinol and Resorcinol. 11 62MICHAELIS (A.). Inorganic Derivatives of Phenylhydrazine. 1163FISCHER (E.). Some Reactions of Phenylhydrazine and of Hydroxylamine. 1163TIEMANN (F.). Action of Hydroxplaniine on Thiocarhimides. 1165PAWLE WSKI (B.).Action of Chlorosulphonic Acid on Phenylthiocarb-GABRIEL (S.) Ethylene Bases.1166CHABRI~ (C.).Selenium-compounds of the Benzene Series. 1167~IrTRAuER (s.). dctioii of Phosphonium Iodide on Benzaldehyde.1168T~EMANN (F.) .Ethers.1168RIECAE (F.).The Four Isomeric Nitrometamethoxybenzaldehydes.11 69MULLER (H.) and H. v. PECHMANN. Mixed a-lXlietones. 1170PAWLEWSKI (B.). Orthotolyl-P-imidohutgric Acid.1171GABRIEL (S.) and J. HAL-SMANN. Action of Orthocyanobenzyl Chloride onE t hy 1 Sodacetoacet ate.1172HAUSMANX (J.). Action of Orthocyanobenzyl Chloride on Ethyl Sodo-SALKOWSKI (H.). Deriratives of Parahydroxyphenjlacet ic Acid. TheEthereal Oil of White Mustard. 1173REISSERT (A.). Pyranilpyroic Acid and Mesaconilic Acid. 1174BAEI ER (A. v.). Constitutioii of 3enzene. Reduction-products of Tere-LEVY (S.) and A.CURCHOD. Action of Phosphorus Pentachloride on EthylSuccicosuccinate.11'19BAEYER (A. v.) and F. TUTEIN. Reduction Products of Hydroxytere-WIDMAN (0,). Paracarboxyhydrocinnnmic Acid. 1181WIDMAN (0.). Constitution of Cumenylpropionic Acid. 1182DELISLE (A.). Reduction of Ortliosirlpliobenzoic Chloride. 1183LE CANIJ (J. A.). Ortliophenolsulphonic Acid.1183XEHRNANN (F.). Iodophenolsulphonic Acid and Iodoquinone ,.1184LE CANU (J. A.). Phenoldisulphonic Acid. 1185WIDITAN (0.). Isomeric Change in the Propyl-group. 1185OTTO (R.). Synthesis of Symmetrical Diphenylsulphoneacetone. 1186CIAMIcrAN (G) and C. BAYTI. Indole-derivatives.1187DIANIN (A. Y.). Condensation-products of Acetone and its Homologues.1187RUSSA~-OW (W.). Condensation-products of Benzaldehjde with Phenol?JATHAXS~;N (M.) and P.MULLER. Derivatives and Reactions of Tetra-AIJWE~S (K.) and M. DITTRICH. Structure of the Oximido-group in theIsomeric Benzilmonoximes.*.1192LIEBERMANN (C.). Isomeric Truxillic Acids.*.1194DRORY (W. L.). Salts and Derivatives of the Truxillic Acids. 1196KEHRMANN (F.) and 0. WEICHARDT.BAXBERGER (E.) and H. HELWIB. Hydronaphthabenzy!ainines.1198JOLLES (0.). a- and /3-Naphthylglycines and their Derivatives. 1199BRANDIS (E.). Condensation-derivatives of a-Naplithaldehyde. 1199FRIEDEL (C.) and J. RI. CRAFTS.Mononitrated b ydroxybenzaldehydes and their MethylGBOSSMANN (G.). Reduction uf Amarine.1191Derivatives of Nitrohydroxynaphtha-Decomposition of Sulphonic Acids iCONTENTS.xxxvAUWERS (K.) and V.MEYER.CAZENEUVE (P.).Oxidation of Nitrocamphor in presence of Light .CAZENEUVE (P.). Nonochlorocamphor formed by the Action of Hypo-CAZENEUVE (P.). Isomeride of Bromocamphor.HALLER (A.).Camphor-deriratives.HALLEB (A.). Influence of Solvents on the Rotatory Power of IsocampholsGLADSTONE fJ.H.) and W.HIBBERT.Molecular Weight of CaoutchoucLETELLIER (A.). Colouring-matter of Purpura lapillur.CIAMICIAN (G.) and C.U.ZANETTI.Conversion of Homolowes of Pyrro-Oximes of PhenanthraquinoneVULPIUS (G.)- Terpin Hydrate.\ I .,DENNSTEDT (M.) and A.LEHNE .DENNSTEDT (M.). Dimethylpprrolines.~ E N N S T E D T (M.). Dimethylpyrrolines in Dippel’s Oil .RUGHEIMER (L.).KUHLING (0.). Derivatives of Pyrrolidone.BLAU (F.). Preparation of Mono- and Di-Bromopyridine .DOBNER (0.) and P.KUNTZE.2 6-Diphenylpyridine .BLAU (F.).Distillation of the Salts of Pyridinecarboxylic Acids .HERSTEIN (B.) .ALT (H.). Quinoline.BUCHNER (E.). Isomeride of Glyoxaline.BALBIANO (L.).Monosubstituted-derivatives of Pyrazole .KNORR (L.). Syntheses in the Oxazine Series.FREUND (M.) and S.LACHMANN.Hydrastine.FREUND (M.).Hydrastine.AHRENS F.B.Mandragorine.WRAXPELMEYER (E.). Thc Existence of Avenine.MEYET.Crystallised Hemoglobin.SCEROTTER (H.). Ethereal-derivatives of Albuminoiids .Action of Sodium I<thoxide on Ethyl HippurateTruxillopiperidides and Truxillopiperididic AcidsPhysiological Chemistry .HALLIBURTON (W.D.). Nature of Fibrin Ferment.KRAUSS (E.). ’Glycogen in Muscle after Section of the Nerve andTendon.SALOMON (G.). Lactic Acid in the Blood.HARRIS (V.D.) and H.H.TOOTH.Micro-organisms and ProteolyticDigestion.LEUBE (W.).(31 co en in Diabetic Urine.HALDANE (J.S.).’ Agromatic Substances in Febrile Urine.DUBOIS (R.) and L.VIQNON.Physiological Action of Yara- and Meta-LOEB (J.). Influence of Light on Oxidation in Animals.MAYER (A.). Melting Point and Chemical Composition of Butter as affectedN EISSER (E.). Glycogen.PFLUGER (E.). Synthetical Processes in the Animal Organism.ELLENBERGEB and HOFMEISTEB.The Sugar-contents of the Horse’sStomach.GIRARD (H.). Post-mortem Formation of Sugar in the Liver.KUHN.Aqueous Humour.GLEISS (W.). Lactic Acid in Pale and Red Muscle.SOXHLET Citric Acid in Caws’ Milk.NASSE (0.).Primary and Secondary Oxidation.HIRSCRFELD (F.). Protejid Metabolism in Man.thePAGE121264FAGEBTJISINE (A.) and F.BUISINE.Glycollic Acid and Pyrotartaric Acid fromSuint.ROFMANN (H.). Fate of Certain Ferments in the Organism.HARLEY (G.) and H.S.HARLEY.Myxmdema.GREENWOOD (M.). Digestion in Hydra,.HENNEBERG (W.). Influence of the Consumption of Water on the Alimen-WOOLDRIDGE (L.C.). Coagulation of the Blood.XELLER (H.). Influence of Ethyl Alcohol on Metabolism in Man .MORNER (K.A.H.). Metabolism of Acetamide in the Human Body .JAFFB (M.) and R.KOHN.Metabolism of Forfuraldehyde in Fowls .JIJVAZTA (N.). Is the Benzene Nucleus destroyed in the Body ?.MARIN~-ZUCO (F.). Chemical Examination of tlie Suprarenal Capsules .MOSCATELLI (R.).Sugar and Allantoi'n in Ascitic Fluid.LIMBOURG (P.). Antiseptic Action of Bile Acids.WEDENsnr (N.). Carbohydrates in Normal Urine.LEUBE (W.). Glycogen in Diabetic Urine.SALOMON (G.). Physiological Action of Paraxanthine.DRECHSEL (E.). Can the Mucous Membrane of the Stomach decomposeBromides and Iodides ?.HUFNER (G.). Tension of Oxygen in Blood and in Solutions of Oxy-LOWIT (W.). Blood Tablets and Thrombosis.ALDEHOPF (G.). Influence of Starvation on the Glycogen of the Liver andMuscle.MANCHB (E.). Eflect of Muscular Work on the Glycogen in the Muscles .SCHMELZ (C.). Source of the Glycogen of Muscle.IRVINE (R.) and Gt.SIMS WOODHEAD .SEBELIEN (J.). Protei'ds in Milk.WEINLAND (C.). Guanine in the Excrement of Spiders.SHER (S.).Relation between the Total Sulphuric Acid of the Urine andRTADELMANN (E.). Pepsin in Normal and Pathological Urine.SaLItowsm (E.). Formation of Volatile Fatty Acids in the AmmoniacalPermentation of Urine.SAmowsm (E.). Evolution of Hydrogen Sulphide in Urine and the Beha-BRUNTON (T.L.) and T.J.BOKENHAM.Physiological Action of Amy1Nitrite.LEHMANN (I(.B.). Formation of Adipocere.GEOLL (S.) and L.HERMANN.Amount of Hzernoglobin in the Blood duringInanition.TORUP (S.). Production of the Prote'ids of the Blood.LOEWP (A.). Influence of Saline Materials on Gaseous Metabolism inMan.CHITTENDEN (R.H.) and C.W.STEWART.Influence of certain TherapeuticCHITTPNDEN (R.H.) and others.Influence of Urethane Paraldehyde Anti-Composition of PearlsSecretion of Lime by AnimalsRADZIWILLOWICZ.Cystin.LAHOUSSE.Gases of Peptone Blood.SANSON (A.).Digestion in Mules.Agents on Amylolytic aiid Proteolytic Digestion.STAMATI.Gastric Juice of Crayfish.LANGLEP (J.N.) and H.M.FLETCHER .GRUENHAGEN (A ).Aqueous Humour.Reducing Substances in Urine.HELWES (F.). Rennet in Human Urine.BOXLAND (K.). Nitrogenous Constituents of Urine.LAMBLING (E.). Waxy Degeneration of the Kidney.Secretion of Saliva.HAGEMANR .293493CONTENTS.xxxviiCHITTENDEN (R.H.) and J.A.BLAKE.Influence of Arsenic and AntimonyCHITTENDEN (R.H.) and A.LAMBERT.Physiological Action of UraniumSalts.CHITTENDEN (R.H.) and C.NOERIS.Relative Absorption of Nickel andCobalt Salts.WEYL (T.). Physiological Action of Antharobin and Chrysarobin .BROWN-SBQUARD and D’ARSONVAL.Poisonous Effect of Expired Air .BRASSE (L.).Influence of Temperature on the Tension of Dissociation ofBRUNTON (T.L.) and T.J.BOKENHAM.Action of Hydroxylamine andNitrite& on Blood-pressure.ZECHNISSEN (H.). Conversion of Starch in the Human Stomach .VOIT (E.). Formation of Glycogen from Carbohydrates.POPOFF (N.).BRINCK (J.). Synthetic Action of Living Cells.LUKJANOW (S.M.). Relation of Water and Solid Constituents in the Organs.LEVY (L.). Muscle Pigments.DE REY-PAILHADE (J.). Attraction of Animal Tissues for Sulphur .SOLDNER (F.). The Salts of Milk and their Relation to the Behaviour ofCase’in.WERTHEIMER (E.) and E.MEYER.Oxyhaemoglobin in the Bile Spectro-BAELDE (A.) and H.LAVRAND.Biliary Acids in Urine during Jaundice .ENGEL and KIENER.Urobilinuria and Icterus.JAKSCH (R.v.). The Urine in Melanuria.IJADD (E.F.).Artificial versus Animal Digestion.BOAS.Free Hydrochloric Acid in Gastric Juice.BOURQUELOT and TROISIER.Assimilation of Milk-sugar.FREAR (W.). Digestibility of Soiling Rye.TORRING (H.v.).Amount of Glycerol in the Residuary Liquors of BrandyDistillation.MORNER (C.T.). Chemical Composition of Cartilage.BAMBEROER (E.) and W.FILEHNE.Relations between the Physiological.BUNGE ((3.). Amount of Iron in Fcetal Tissues.SCHINDLEX (S.). Adenine Guanine and their Derivatives.COPEMAN (S.M.) and W.B.WINSTON.HALLIBTJRTON ( W.D.). Cerebrospinal Fluid.WALTER (G.). Cyst of Protopterns Aunectens.ZUNTZ (X.) c.LEHMANN and 0.HAGEMANN.Change of Substance in the.EWALD (A.).Digestion of Elastic Fibres and Allied Structures.JOXDAN (W.A.) J.M.EARTLETT and L.H.MERRIL.Composition andDigestibility of some Foods with Observations on the 1)etermination ofDigestibility of Protei’n and Carbohydrates.GRBRANT and QUINQUAUD.Amount of Urea in Blood and Muclcle .VIETH (P.). Composition of Milk produced in English Dairy Farms .STIFT.Influenceof “Saccharin” on Digestion.PLANTA (A.v.). Food of the Larval Bee.LADD (E.F.). Influecce of Food on the Composition of Butter.ALBEELTONI (P.). Action of Carbohydrates on the Animal Organs .MIDDENDORFP (M.v.). HEemoglobin in Blood passing to and from theFormation of Serum Albumin in the Alimentary CanalProperties and Constitution of’ Hydrogenised BasesHumanBileHorse a t Rest and a t WorkLiver and Spleen.MACMUNN (C.A.).Myoheematin.MARTIN (S.). Prote’id Poisons.UDRANSZKY (L.v.) and E.BAGMANN.Diamines (Ptomaynes) in CjstinuriaLUFF (A.P.). Relations of Ptoma’ines to Infectious Fevers.FJORD (N.J.). Feeding of Milch Cows.PAGE636’7351023PAGEWOOLDBIDCFE (L.0.). Coagulation of the Blood.PANOFF (M.). Nitrogen in Sputum.LENZ (L.). Home Fat.KARMENSKI (S.S.). Physiological Action of Acetophenone.HANDLER ( S.).Reduction of Oxyhaemoglobin in the Heart.RAUDNITZ (R.W.). Digestibility of Boiled Milk.PRAUSNITZ (W.).GIRARD (H.). Influences of Chlorides on the Composition of the GastricJuice.COHN (F.0.). Influence of Artificial Gastric Juice on the Acetous andLactic Fermentations.WURSTER (C.).Formation of Nitrous Acid and Nitric Acid in Saliva fromForrnaldehyde and Ammonia.HOPPE-SEYLER (F.). Muscle Pigmenf s.MACMUNR (C.A.).Animal Chromatology.BERGEAT (E.). Crystalline Acid from Pig’s Bile.HALLIBURTON (W.D.) and W.M.FRIEND.The Stromatn of Red Cor-GRI~HANT (N.).Physiological Action of Hydrocyanic Acid.BAUMANN (E.) and A.KAST.Relation between the Chemical Action and.DASTRE (A.) and M.ARTHUS.HANKIN (E.H.). Albumose Isolated from Anthrax Cultures.Digestion of Beans in the Human Alimentary CanalPhysiological Action of Certain SulplionesGlycogenesis i n ZcterusChemistry of Vegetable Physiology and Agriculture .RAELIN (J.). Action of Micro-organisms on certain Colouring Matters .DUBOIS (R.).BOKORNY (T.). Formation of Starch from Various Substances.MOLISCH (H.).Matter Excreted by Roots.GUTZEIT (H.). Occurrence of Solid Hydrocarbone in the VegetableKingdom.SCHWABE (P.). Constituents of the Bark of Rhamfiusfraayzgula.FESCA (M.) and H.IMAI.Japanese Tobaccos.FRABK (B.). Loss and Gain of Nitrogen in Agriculture.DEVARDA (A.). Action of Superphosphates on Nitrates.ENGELMANN (T.W.). Bacterio-purpurin.MARTINAND.Beer Yeast.SCHULZ (H.). Yeast Poisons.ENGELMANN (T.W.). Blood-pigment as a Gauge of Gaseous Exchange inPlants.BERTHOLD (B.). A Plant which Destroys the Taste of Sweets and Bitters .CHURCH (A.H.) .BAUMANN (A.). Formation of Nitric and Nitrous Acids by the EI aporationMARCKRR (M.). Composition of Spring Wheats grown in 1887.DIETRICH (T.).Composition of East Tndian Wheats.JENSCH (E.). Calcium Sulphite as a Preventive of Loss of Nitrogen inManure Heaps.BLOCK (H.). Constituents of Hedra heZix.LIPPMANN (E.0.v.). Rare Constituents of the Ash of Sugar-beet .BAUMERT ((3.).Decolorisation of Tincture of ‘i’urnesole in Closed VesselsOccurrence of Aluminium in Vascular Cryptogarus .MARCKER (M.). Composition and Nutritive Value of Oats.MODDERMAN (T.). Presence of Nitrites in Plants.JACOBSON (H.). Vegetable Fats.JOHANNSEN (W.). Gluten and its Presence in Wheat Brain.WARDEN (C . J. If.). Errithroxylon coca grown in IndiaOccurrence of Boric Acid in the Vine and in Wines ..JOHNS LONE (W.).Volatile Alkalond in Petmer.1232182CONTENTS.xxxixL ~ V Y (A.). Composition of Rain-water .BELLUCCI (G.).Salt in Rain-water.FOBBE (F.). American Red Clover.HEIDEN (E.). Value o€ Basia Slag as a Manure compared with SolublePhosphate and Bone-meal.HEIDEN (E.). Manuring Experiments in Hemy Soil.SEBELIEN (J.Influence of the Concenhration of the Cream in ButterMaking.WEIGERT (L.). Influence exerted by Salicylic Acid on the Proportions ofGlycerol and Alcohol formed in Wines.HECKEL (E.) and F.SCHLAGDENHAUFFEN .DE MONDESIR (P.). Legurninow in ,4 cid Soils.RATTLIN (J.). Phosphates and Ceredb.SCHNEIDEE (E.A.). Analysis of a Soil from Washington Territory .LADUBEAKJ (A.). Algerian Soils.DELACHARLONNY (P.M.) and L.DESTEEMX.Action of Ferrous Sulphst?BAESSLER.Comparative Manurid Value of the NitrageB in Sodium NitratePETERHANN (A.).Bat's Guano from Cuba.GR%HANT and QUINQUAUD.Disengagement of Carbonic Anhydride byAnaerobic Yeast.BWET (V.) Cornpositmion of the Bmillus from Erythema lzodosum .SCHULZE (E.).lteserve Materials especially Starch Tannin contained inEvergreen Leaves.SCHULZE (E.). Reserve Substances in Evergreen Leaves.RODEWALD (H.). Tramsformation of Force and of Material in Plant Respi-POLLAK (E.). Absence of Nitric Acid in Wine Must.EBERMAYER (E.). Absence of Nitrates in Forest Trees.HOOPER (D.). Laurel-nut Oil.GANS (R.) and B.TOLLENS.Quince and Salep Mucus.LIDOFB (A.). Tmnic Acid in Caucasian Wild Sumach.DEHBRAIN (P.P.).Field Experiments. at Grignon in 1888-.DE MONDESIR (P.). Calcium in Soils.EGQERTZ (C.G.). Humous Compounds in Soil.BROWN (L.P.).Analysis of Tobacco Screenings.HAMMERSC ELAG (A.).Chemical Comqosition of Bacillus Tuberculosis .SCHLOESSING (T.). Loss of Nitrogen in the Decomposition of OrganicMatter.SCHLOESSING (T.). Slow Combustion of Organic Substances-.HELLRIEOEL (H.) and H.WILPARTH.Sources of the Nitrogen of theGramineae and Legurninow.PEYBOU (J.). Variations of the Internal Atmosphere of Plants.PALLADIN (W.). Products of Decomposition of Albrimino'ids in Plants .SCHULZE (E.) and E.KISSER.Decomposition of Prote'ids in Green PlantsSCHULZE (E.) and E.STEIGER.Oceurrence of an Insoluble CarbohydrateMAXWELL (W.). Soluble Carbohydrates in the Seeds of Leguminous PlantsBAUDET and ADRIAN.Morphine in E'scholtzia calzfwnira.MOLISCH (H.) and S.ZEISEL.PLUGGE (P.C.). Andromedotoxin in the Ericaccoe.SCHULZE (E.) and E.STEIGER.Lecithin in the Seeds of Plants.LINOSSIER (G.).Influence of Carbonic Oxide on Germination.MUNTZ (A.). Fertilising Properties of the Water of the Nile.GEORGESON (C.C.). Manuring of Rice.LTETGEB (H.). Asparagine and Tyrosine in Dahlia Bulbs.PARSONS (C.L.). Analysis of Fruits from the Southern StatesJuice of Bassia latzyolia.LOEW (0.). Rble of Formaldehyde in the Assimilation of Plants.New Source of CoumarinPAGE43663864PAGECIRARD (A.) Cultivation sf Potatoes. 647PETERMANN.Assimilaticm ofsthe Phosphoric Acid in Basic Slag. 647PETERMANN.Manuring with Fish Guano. 647FRANKLAND (P.F.). Action of Gases on the Development of Micro-TACKE (B.). Disengagement of Free Nitrogen during Putrrefaotion .REISET (J.).Putrefaotion Formation of Manures.LINOSSIER ((3.). Effect of Carbonic Oxide on Germination .HARTIG (R.). Reserve Materials in T m s.BOURQUELOT (E.). Saccharine Substances in Fungi.GATELLIER (E.) and L.L'HOTE.Gluten ill Wheat.LANGER (A.). Constituents of Lycopodium Spores.CROSS (C F.) and E.J.BEVAN.Chemistry of Flax Fibre.SORAUER (P.). Failure of Oat Crops.JENKINS (E.H.) and others .HANAMAN (J.). Manuring of Barley.BERTHELOT.Absorption of Nitrogen by Soils.DEHBRAIN (P.P.).MEISSL (E.). Comparison of Basic Slag with Superphosphate .CRAMPTON (C.A.).WHITE [J.T.).Maize as Dry Food and at3 Silage .Loss and Gain of Nihrogen in SoilsBoric Acid as a Plant ConstituentAt3h of.the Indigo StemGREENE'(W.'H.) and S.C.H~OKEE.Occmrrence of Lapachic Acid inBethabarra Wood.JUST (L.) and H.HEINE .STOOD (A.).Action of Water containing Sodium Chloride on Soils andPlants.MARCANO t(V.). Almholic Fermentation of the Juice of the Sugw-cane .MARTINAN D. Alcoholic Fermentation of Milk.SCHULZE (E.). Gompmitisn of Vegetable Cell Membrane.KRAUS (G.). Physiology 04 Tannin.WASHBURN ( J.H.) and B.TOLLENS.Cane-sugar from MaizeARNDT (E. M.J.ZOPP (W.). Colouring Matters of Fiingi.GATELLIER (A.) and L.L'HOTE .MAYER (A.). Composition of Canary Seed.Damage done to Plants by Acid Vapours .Volatile Base from the Root of CephaBZis Ipecacuamha .Gluten in Wheat.LAWES (Sir J.B.).MUNTZ (A) and V.MARCANO .UDR~NSZKY (L.v.) .SALKOWSKI (E.) .PFEFFER .HELL (C.) and S.TWERDOMEDOFF.Fatty Oil of Cyprus escuZentzcs .SCHULZE (E.).Presence of Beta'ine an& Choline in the Seeds of Vicia sctioaWOLLNY (E ).Percentage of Carbonic Anhydride in the Air of Soils .WOLL (F.W.A.). Decomposition af Organic Arnmoniacal Compounds inEnsilage.-.WILSON (D.). Nutritive Value m d Produce of Grasses and Clovers .History of a Field newly laid down to PermanentGrass.Nitrates in the Rain of Tropical Districts.Formation of Glycerol in Alcoholic FermentationFormation of Sugar and other Substances in Yeast .PFEFFER.Oxidation in the Living Cell.MAXWELL (W.). Solubility of the Conetituenks of Sreds. Reduction of Silver Nitrate in the Lfving Cell.HARTIG (R.) and R.WEBER .MAYER (A.).Manurial Value of Several Marine Products.The Wood of the Beech.ROLLAND (C.).Comparative Manurial Values of Chili Saltpetre and Am-ENKLAAR (J.E.). Presence of Ammonia and Nitrous Acid in PotableWaters.TIMIRIAZEFF (C.). Relation between the Intensity of Radiation and theDecomposition of Carbonic Anhydride by Plants.PALLADIN ( W.).Carbohydrates as Oxidation-products of VegetableAlbumin.LANGE ((3.). Lignin.1027CWTESTS. xliHECKEL (E.) and F. SCHLAGDENHAUFFEN. Oleo-gum-resin Secreted byAraucarias.TTMIRIAZEFF (C.). Protophyllin in Etiolated Plants.SCHLOESSING (T.). Atmospheric Nitrogen and Vegetable Soils.BERTHELOT. Absorption of Nitrogen by Clay Soils.SCHLOESSING (T.). The Relation of Atmospheric Nitrogen to VegetableSoils.BERTHELOT. Influence of Electrification on the Absorption of Nitrogen byVegetable Soils.BERTHELOT.Absorption of Atmospheric Nitrogen.BERTHELOT. Evolution csf Ammonia and Volatile Nitrogen-compoundsSCHLOESSING (T.).Nitrification of Ammonia.PBCIIABD. Influence of Calcium Sulphste and of Clay on the Absorption ofNitiwgen.HEBERT (A.) Formation of Ammonia in Arable Soils.MULLEX (A.). Sea Sludge and its Absorpthe Power €or Lime or Potash .RAULING (G.). Phosphates and Cereds.Analytical Chemistvy.GASTINE (G.). Preparation of Starch Solution for Use in Volumetric?Analysis.BORNTRAGEB (H-). Use o€ Salicylic Acid for Preserving aandard SolutionsLAMBLING (E.). Application of Spectrophotometry to Chemical PhysiologyJOLLES (A.). Determination of Chlorine in Plant Ashes.GETZOW (F,]. Determination of Bromine in Sea Water.LASNE (H.).Determination of Fluorine.LINOSSIER ((3.). General Method for ithe Separation and Volumetric&timation of Acids.MCGLASCHAN (J.). Volumetric Estimation of Boric Acid and of AmmoniaLrNDo (D.). Resorciriol as a Test for Nitrates.SHIMER (P. W.). Determination of Phosphorus in I,mn and Steel .HOGQ (T. W.).CLASSEN (A.) and R. SCHELLE. Quantitative Analysis by Electrolysis .KUPFFERSCHLAEGER. Separation of Calcium Barium and Strontium .KASSNER (G.). Volumetric Estimation of Mercuric Chloride.STRENG (A). Microchemical Reactihs.HAUSHOFER (K.). Detection of Small Quantities of Germanium.LBGER (E.). Characteristic Reaction for Bismuth.WINELER (L. W.). Determination of Oxygen dissolved in Water .FLUCKIGER (F.A). Ash Determination.ME~SINGER (J.). Wet Methods of Organic Analysis.NEWBURY (S. B.) and W. P. CUTTER. Safety of Comniercial Kerosene OilsPAWLEWSKI (B.) and J. FILEMONOWICZ. Solubility and Estimation ofParaffin.TEISSIER (J.). Analysis of a Mixture of Silver Chloride Cyanide Thio-REVERDIN (F.) and C. DE LA HARPE. Determination of ParanitrotolueneHABERMANN (J.). Detection of Methyl Alcohol in Wood Spirit.ROCQUES (X.). Composition of Natural Brandies the way of distinguishingBISCHOP (R. W.). Determination of Sugar in Presence of Carbohydrates .SCHWARZ (C.). Determination of Sugar in Urine.SCHWARZ (C.). Detection of Chloral or Chloroform in Liquids.MANSFIELD (M.). Modification of the Reichert-Meissl Method of ButterAnalpsi s.LONG (J.H.). Densities and Refractive Indices of Oils.Influence of Sulphur on Eggertz's Carbon Colour TestPAQE7380BIZIO (G.). Bechi’s Newest Method for the Detection of Cotton-seed Oil inMixtures.ROLDE.Qualitative Test. for Resin Oil in Vegetable and Mineral Oils .LINDO (D.). Test for Saccharine.LENZ (W.). Recent Processes for Testing Quinine.GILLET.Detection of Ground Olive Stones in Pepper.KATAYANA (K.).SCRAUMANN (H.). Determination of Albumin in Urine.DREHSCHMIDT (H.). Gas Analysis.STORTENBEKER (W.). Estimation of Iodine.ZIPPERE~ (P.). Estimation of Nitrogen in Nitrate-superphosphate and inChili Saltpetre.STTTZER (A.). Estimation of Phosphoric Acid.JUPTNER (H.v.). Wiborg’s Gasometric Method for Estimating Carbon inIron and Steel.LONATSCHEFFSKY-YETRUNIAKA (T.).Absorption of Carbonic Oxide byLONATWHEFFSKY-PETPUNIAKA (T.).Action of Sulphuric and HydrorLUCION (M.). Precipitation of Bariutn Sulphate in the Presence of BromineTAUBER (G.). Precipitation af Barium Sulphate in the Presence of Bro-OPIFICIUS (L.). Analysis of Lead Peroxide.- .RUDORFF (F.). Electrolytic Estimation of Copper.STEIN (G.). Estimation of Manganese in Foods.KENNEPOHL (G.). Estimation of Iron azld Aluminium in the Presellce ofCalcium and Phosphoric Acid.BAUBIQNY.Separation of Kickel and Cobalt.JOLLES (A.). Volumetric Estimation of Stannous Chloride.JENNINQS.Estimation of Titanium and Phosphorus i c Iron Ores .OPIFICIUS (L.). Estimation of Noble Metals in Potassium Cyanide SolutionsDUDLEY (W.L.).TREADWZLL IF.P.) and H.N.STOEES.Source of Error in the EstimationEKMAN (F.L.).HEHLES (F.).Estimation of Sugar in Molasses.DAMMULLER (J.). Estimation of Saccliarose as well as Invert-sugar orRa5nose.LOTMAN (G.). Estimation of Raffinose in Beet-sugar.HARTWICH (C.). Detection of Foreign Starches in Chocolate.PAGNOUL and GRENET.Butter Analysis.BISCHOP (W.) and L.IN&.Detection of Cotton-seed Oil in Lard .SAMELSON.Estimation of Fatty Acids in Soap.ELION (H.).SNYDERS (A.J.C.).Kocn (R.). The Simand-Kohnstein Method of Estimating the Acids inTanning Liquors.CROSS (C.F.) and E.J.BEVAN.Apparatus for Estimating the Amount ofBERTHELOT.Graduation of Tubes for Gasometric Purposes.XILOART (A.). Calorimetric Bomb as a Combustion Furnace for UltimateEINQZETT (C.T.).Eslimation of Hydrogen Peroxide.LINOSSIER (G.) and M.LIGNON.Estimation of Chlorine.WHITE ( J.T.). Volumetric Estimation of Chlorine.SJOQVIST (J.). New Method of Estimating Free Hydrochloyic Acid in theStomach Contents.New Test for the Blood in Carbonic Oxide PoisoningCuprous Chloride.Modifications of the Methods of Organic Analysis .The Amount and Estimation of Pusel Oil in Spirits .Detection and Estimation of Salicylic Acid chiefly in BeerDetection of Salic-jlic Acid in BeerDENNER (C.). Testing Peru Balsam.Gas disappearing in a Reaction.MARCET (W.). A New Form of Eudiometer.Analysis.PAGE&18’7192CONTENTS. xliiiPAQEERRERA (C.) Separation and Estimation of Chlorine Bromine Iodine andCy anogen.-WATSON (J.). Estimation of Sulphur in Burnt Pyrites.ENQ-EL. Volumetric Estimation of Acids.SIDERSKY (D.). Volumetric Estimatioii of Sulphates.QUANTIN. True Rdle of Soda-lime in the Estimation of Nitrogen .SMITI~ (J. H.). New Method for the Estimation of Pr’itrogen.CLARK (J.). Estimation of Phosphoric Acid with Silrer Kitrate.BRRTHELOT and G. ANDR~.SCOTELL (M. A.). Estimation of Nitrates by Kjeldahl’s Method.LINOSSIER (G.). Estimation of Phosphoric? Acid.HOGG (T. W.)- Estimation of Carbon in Iron Steel &c.BENEDIKT (R.) and M. CANTOR.WIKKLER (C.). Estimation of the Percentage of Lead in Tin-lead Alloys byWILLIANS (R.). Estimation of Copper by the Iodide Process.MEINEKE (C.). Separation of Manganese and Allied Metals from the Sesqui-CARNOT (A.).Estimation of Chromium by Hydrogen Peroxide.RUSAG (K.). Analysis of Commercial Scherlite.JOLLES (A.). Volumetric Estimation of Antimonious and ArRenious Acids .ENORRE (G. v.). Volumetric Estimrttior of Antimonic Acid.HOOKER (S. C.). Estimation of Nitrates in Natural Waters.MESSINGER (J.). Estimation of Acetone in Methyl Alcohol.PABCUS (E.).SIDERSKY (D.). Indirect Analysis of the Sugar-beet.PELLET (L.). Estimation of Sugar in Beet by Digestion with Water .WEISBERG (J.).BATTUT (L.). Estimation of Sugar in Beet.CLERC (M.). Estimation of Sugar in Beet.V I E ~ H (P.). Estimation of Milk-sup in Milk by the Polariscope .LINTNER (C. J.). Compounds of Starch with the Alkaline Earths .PETERS (W.). Adulteration of Vegetable Fatty Oils.FAWSITT (C.A.). Action of Sulphur Ciiloride on Oils.PLANCHON (I7.). Detection of Margarin in Butter.WILLIAMS (R.). Iodine Absorptions Combining Weights and MeltingPoints of some Fatty Acids.ALLEN (A. H.). Detection of Cotton-seed Oil in Lard.HEHNEK. (0.). Mixed Lard and the Detection of Cotton-seed Oil .WILLIAMS (R.). Adulteration of Lard with Cotton-seed Oil.JOKES (E. W. T.). Lard Adulterated with Cotton-seed Oil.ALLEN (A. H.). Adulteration of Lard with Cocoanut Oil.ARCHBUTT (L.). Analvsis of Grease.RAESSLER (F.). Estimkion of the Oil and Water in Linseed Cake .BUCHNER (G.). Analysis of Wax.WILLIAMS (R.). Examination of Certain Gums and Resins.ALLEN (A. H.). Detection of “ Saccliarirt ” in Beer.KREMEL (A.). Estiniation of Aikaloids in Nux-vomica.XUDDIMANN (E.A.). Estimation of Quinine by Kerner’s Blethod .GRIMBERT. Detection of Urobilin in Urine.W~NKLER (C.). Draught Arrangement for Water-baths.BERINQER (C. and J. J.). Volumetric Estimation of Sulphur by means ofBarium Chloride.DE KONIKCK (L. L.). Estimation of Hydrogen Sulphide.LHOTE (L.). Estimation of Nitrogen by Kjeldahl’s Method.GIUNTI (M.).SPIEGEL (L.). Estimation of Nitrates in Mineral Waters.MIELCKE (W.). Calculation of Phosphoric Acid Estimations.TZSCHUCKE (H.). Direct Estimation of Phosphoric Acid as TricalciumPhosphate ,.Estimation of Nitrogen in Vegetable SoilsVolumetric Estimation of Zinc OxideDetection of Invert-sugar in the Presence of Cane-sugarEstimation of sugar in Beet by Digestion with WaterSource of Error in the Estimation of Nitrates in Soils .311318437REIS (M.A.v.). Estimation of Phosplioric Acid in Basic Slag.JOHNSTONE (A.).Decomposition of Insoluble Silicates.LUNGE (G.) and A.ZECKENDOBF.Estimation of Carbonic Anhydride inWOLFF (C.H.). Electrolytic Detection of Mercury.MEINEEE ( C.).Analysis of the Raw Materials and Products of the IronIndustry.MCCULLOCH (N.). Volumetric Estimation of Cobalt.CARNOT (A.). Estimation of Chromium Iron and Manganese by means ofHydrogen Peroxide.HOLLAND (P.). Estimation of Titaniiim in Natural Silicates.JOHNSTONE (A.). Detection of Antimony in Minerals.JOLLES (A.). Volumetric Estimation of Antimonic Acid.DUNSTAN (W.R.) and 1).E.BOOLE.Tartar Emetic.G-RESHOFF.Decomposition and Estimation of Iodoform by Silver Nitrate .GIRARD (C.) and X.ROCQUES.Analysis of Alcohols.HAOER (H.). Estimation of Alcohol in Essential Oils.WEIOERT (L.).Estimation of Glycerol in Wine.CRISMER (L.). Safranine as a Reagent for Graps-sugar.HOOBN (G.H.). Detection of Salicylic Acid in Beer.WEIGERT (L.). Estimation of Salicylic Acid.EWELL (E.E.) and A.B.PRESCOTT.Estimation of Foreign Acids in Arti-WARD (J.S.). Estimation of Citric and Tartaric Acids when mixed .RAWSOX (S.G.). Tests for Tannic and Gallic Acids.ENDE (D.). Detection of Iron in Oil.BESANA (C.). The Reichert-Meissel- Wollny Method of Analysis as appliedWILSON (J A.). Estimation of Free Caustic Alkali in Soap.HOOKER (S.C.). Detection of “Saccharin”.BORSSTEIN (E.). Detection of “Saccharin”.HAYCRAFT (J.B.) and R.T.WIILIAMSON.Estimation of the Alkalinity ofBlood.UDR~NSZKY (L.v.). Furfuraldehyde Reactions.GOSSAGE (A.M.).Volumetric Estimation of Uric Acid.SEBELIEN (J.).CHRISTENSEN (A.). Estimation of Albumin in Urine.BUNGE (N.A.). Kaolin Balls for Gas Analysis.REICHERT (E.).Quantitative Estimation by Measurement of ElectricalConductivity.JANNASCH (P.). Estimation of Water in Silicates.ZSIGMONDY (R.). Source of Error in the Determination of the Nitrogen inSubstances containing Halogens.VIOLLETTE ( C.).Estimation of Nitrogen by Kjeldahl’s Method.FOEBSTEB (0.). Estimation of Nitrogen in Nitrates by I( jeldahl’s Method .KBEUSLER.Detection of Nitrates in Soils.LANGE (0.). Estimation of Nitrogen and Phosphoric Acid in Organic Sub-FRESBNIUS (W.).Estimation of Phosphoric Acid in Sweet Wines .SEYPERT (F.). Estimation of Phosphoric Acid in the Presence of AmmoniumCitrate.MILLARD (E.J.). The Molybdate Test for Hypophosphites.FBESENIUS (H.). Arsenic in Bone Phosphate used for Cattle Feeding .LEVOIR (L.C.). Apparatus for the Electrolytic Estimation of Metals .YVON.Volumetric Estimation of Lead in Presence of Tin.MYLITJS (F.). Testing Glass by Colour Reactions.LALIETJ (A.). Direct Estimation of Oxygen and Nitrogen in NaturalWaters.Estimation of Prote’icls with special Reference to MilkDUBNINGTON (F.P.). Use of Hydrogen Peroxide in Analysis.NEUMANN (G.). Estimation of Zinc in Presence of Mercury.DAVIS (I.T.). Separation of Aluminium and Zirconium.- .PAGE446544549CONTENTS.xlvDROWN (T.M.). Loss on Ignition in Water Analysis.BORNTRAGER (H.).Examination of Commercial Alcohol.CRISMER (L.) Detection of Sugar in Urine.VINCENT (C.) and DELACHANAL.Estimation of Sorbite.LIST (K.). Detection of Nitrobenzene in Presence of Oil of Bitter AlmondsEGGER (E.).REIS (M.A.v.). Estimation of Phosphorus and Sulphur in Tron .AUBIN (E.) and ALLA .ZECCHINI (M.) and A.VIGNA.Estimation of Nitrogen by Kjeldahl’s MethodZECCHINI (M.) and A.VIGNA.Estimation of ready formed Nitrogen inManures.FLUCKIGER (F.A.). Detection of Minute Quantities of Arsenic.KATAYAMA (K.). Test for Carbonic Oxide Poisoning in Blood.J ~ G E R (E.) and 8.KRUSS.Volumetric Estimation of Carbonic Acid .Detection of Free Sulphuric Acid in Aluminium SulphateEstimation of Nitrogen by Kjeldahl’s MethodCONINCK (0.DE).Estimation of Total Nitrogen in Urine.FRAXK (B.).Detection of Nitrates in Soil.SCHYDLOWSKI (F.). Estimation of Carbonic Anhydride in Air.KLEIN (J.). Detection of Mercury.Magnesium.BAUBIGNY (H.). Separation of Zinc from Nickel.BAUBIGNY (H.). Separation of Zinc from Cobalt.FISCHER (R.). Separation of Nickel from Cobalt.KLEIN (J.). Detection of Manganese.BLUM (L.). Analysis of Substances containing Aluminium Calcium andMARINO-ZUCO (F.).Destruction of Organic Matter in Toxicological Investi-PENDRII? (M.A.). Cyanogen and its Compounds in the Products of CoalDistillation.WEIGFERT (L.). Terreil’s Reaction for Testing the Colouring Matter ofWine.PALMIEBI (P.) and F.CASOEIA.Tests for Archil Cochineal and MagentaEstimation of Raffinose in the Products of Beet-sugarManufacture.TRAUBE (J.).Examination of Spirituous Liquids.DENIG~S ((3.). Reagents for Mercapfans.VAN ITALLIE (L.). New Test for Thymol.BORNTRAGER (H.). Characteristic Reaction for Aldehyde.GUNNING (J.W.).HEIDENHAIN (H.) Goldenberg’s Method for Estimating Tartaric Acid .BESANA (C.). Methods for Detecting the Adulteration of Butter.HIPSCHSOHN (E.). Detection of Cotton-seed Oil in Olive Oil.Cotton-seed Oil and Beef Fat in LardBIEL (J.). Detection of Cotton-seed Oil in Olive OilWILSON (J.A.).AMBUHL ((3.). Adulteration of Lard.UMNEY ( J.C.). Oil of Anise.SCHRODER (J.). Detection of Antifebrin in Phenacetin.Oxyhsemoglobin.L’HOTE (L.).Estimation of Orgmic Nitrogen.EDWARDS (V.). Estimation of Insoluble Phosphates.DENIG~S.Reaction for Copper.MOORE (T.). Volumetric Estimation of Nickel.CARNOT (A.). Estimation of Nickel and Cobalt.CARNOT (A.). Separation of Nickel and Cobalt..MORAWSKI (T.). A Delicat. e Reaction for Pine-wood Resin.LAMBLING (E.). Estimation of Methaemoglobin in the Presence ofLONG (J.H.). Behaviour of Phenolphthalein with Ammonia.FOERSTER (0.). Estimation of Nitrogen in Nitrates by Ejeldahl’s Method .TORRING (H.+.). Estimation o l Glycerol in the Residues of Brandy Distil-LEWKOWITSCH (J.). Estimation of Glycerol in Crude Glycerol .PAQE657FILSINCIER (F.). Estimation of Glycerol in Crude Glycerol.GEROCK (J. E.). Separation of Strychnine from Brucine.LINOSSIER (G.). Volumetric Estimation of Acids.BUISINE (A. and P.). Alleged Reaction of Copper Salts.MARSH (C. W.). Detection of Chlorine Bromine and Iodine and SulphurGUNNING (J. W.). Modification of Kjeldhai's Mkthod.LEFFXANN (H.) and W. BEAM. Estimation of the Total Organic NitrogenHUNDESHAGEN (F.). Estimation of Phosphoric Acid by AmmoniumMoly bdate.JOHNSTONE (A.). Detection of Mercury in Minerals.SMITH (E F.) and L. K. FRANKEL. The Electrolytic Method applied toJOHNSTONE (A.).HOQG (l'. W.). Influence of Copper on the Determination of Iron in Ferro-JOLLES (A.). Use of Potassium Manganate in Analysis.PREUSSER (J.). Estimation of Tungsten in its Alloys.CHARPENTIER (P.). Errors iu the Assay of Fine Gold.KONIG (J.). Mode of Stating the Results of Wine Analyses.GRANVAL and VALSER.NOB:RDLINQER (H.). Free Fatty Acids in Oils.,.NILSON (L. F.). Butter Analysis.CRAMPTON (C. A.). Specific Gravity of some Fats and Oils.PopovicI (M.). Quantitative Estimation of Pu'icotine.SCHINDLRR (S.). Separation and Estimation of Adenine Guanine and theirDerivatives.LANDRIN (E.). Analysis of Cinchonas.LYONS (A.). Evaluation of Ipecacuanha.KONIG (J.) and W. KISCH. Examination of Commercial Peptones .WINELER (C.). Technical Gas Analysis.PREUSSER (J.) Substitute for the Calcium Chloride Tube in ElementaryAKJBIN (E.) and L. ALLA. Estimation of Nitrogen by Kjeldahl's Method .BAILHACHE. Estiniation of Nitric Nitrogen by Ferrous Sulphate .JANNASCH (P.) and T. W. RICHARDS. Estimation of Sulphuric Acid inPresence of Iron.SMITH (E. F.). Oxidation with the Galvanic Current.FEIT (W.) Estimation of Thallium and Mercury.FRESENIUS (R.) and E. HINTZ. Estimation of Silicon and Iron in CryoliteGEHIZENBECK (C.). Simultaneous Estitiration of Hydrogen and Nitrogen .NEUMANX (S ). Eudiometric Estimation with Mixtures of Ammonia andOxygen.FAUSER (G.). Estimation of Hydrogen Sulphide in Aqueous Solution.STOCKJ AS 1 (J.).Detection of Phosphoric Acid of Mineral Origin .SACK (E.). New Apparatus for the Indirect Estimation of Carbonic Anhy-MARSH ( C.W.). Reduction of Barium Sulphate to Barium Sulphide onIgnition M ith Filter-paper.SCUIERKING (H.). Estimation of Calcium and Magnesium in Gun-cotton .SMITH (E. F.) and L. I(. ERANKEL. Electrolytic Separation of CadmiumDEWEY (F. P.). Estimation o i Cuproirs Oxide in Metallic Copper .MooxE (T.). Volumetric Ebtimation of Nickel.PETTEItSSON (0.). Volumetric Estimation of Gases Dissolved in water .Detection of Minute Quantities of Iron in MineralsFalsifimtion of Oleic Acid by Linoleic Acid .IHL (A). Colour-reactions of some Ethereal Oils.Analysis.CAZEXEUVE (P.). Detection of Impurities in Alcohol.Natural Waters by Kjeldahl's Method. 103COXTENTS.xlviiPAUEVIGNON (L.).BERTHELOT.Estimation of Benzene Vapoiir in Coal-gas. 1036CAUSSE (H.). Estimation of Sugar by Fehling’s Solution. 1036PHIPSON (L.T.). Tin in Sugar.1036LOSEKANN (G.). Estimation of Formaldehyde.1036WoLmY (R.). Estimation of Fatty Acids from Butter. 1037SHORT (P.G.). Estimation of Fat in Milk. 1037WILSON (J.A.). Free Alkali of Soap. 1037REVERDIN (P.) and C.DE LA HARPE .LUTHER (R.). TCe Knop-Hufner Method of Estimating Urea,. 1039CAMERER (W.). 1040BRUCKE (E.37.). 1040NENCKI (hl.v.). Testing of Reagents Eniplojed in Elementary Analysis.1085FOERSTER (0.). Purification of Litmus. 10%HOLBLING (V.). Volumetric Apparatus. 1g86BAWALOVSKI (A.). Separation of Ethereal Solutions from Aqueous Liquids 1086STEIN (W.M.) and P.w.SCHWARZ .Rapid Metbod of Anaiysing Water prior to its SofteningEstimation of Aniline and Methyl-Estimation of Uric Acid in Human Urine.Van Deen’s Test for Blood ar.d Vitali’s Tesl for PusREICHARDT (E.) and UP-MEYER.Estimation of Iodine. 1086DE LA HARPE (C.) and F.REVERDIN.Analytical Notes. 1087Estimhon of Ammonia by Distilla-Q~JANTIN (H.). Volumetric Estimation of Sulphates.1087BLUM (L.).Precipitation of Magnesia. 1087BLUM (L.).BLUM (L.). Determination of Carbon in Iron.1098MARTINOTTI (F.). Estimation of Nitrogen by Kjeldahl’s Method.1088REICHARDT (E.). Elementary Analysis of Volatile Liquida. 1088POLITIS (J.E.). Rapid Estimation of Saccharine Compounds. 1088STEIGER (E.). Estimation of Galactose. 1059KONIG (J.) and M.KESENER.Discrimination of Fruit and Beet Syrups.1083LUDY (E.). Detection of Carbamide. 1090BODD~ (H.). Detection of Resorcinol. 1090BOURCART (R.). Milk Analysis.1090DE VRIJ (J.C.).Quinine Sulphate. 1091EWER (E.). Indirect Estimation of Extractive Matters in Wine.1091SOSTEGNI (L.). Detection of Foreign Colouring Matters in Wine.1091PALMER (T.C.). Testing Logwood Extracts.1091WHITE (J.T.). Estimation of Tea Tannin. 1092REICHL (C.). New Reaction for Albumino’ids.1c92COPEXAN (S.M.). Detection of Human Blood.1092WURSTER ((3.). Naphthylamine as a Reagent for Hydrogen Peroxide inPresence of Sodium Chloride. 1242JAKSCH (R.v.). Estimation of Free Hydrochloric Acid in Gastric Juice.1242WURSTBR (C.).Reaction. 1243JANKASCH (P.). Decomposition of Sulphides by Air containing Bromine.1243JANNASCH (P.). New Method of Analysing Pyrites.1243JANNASCH (P.). Decomposition of Pyrites iii a Stream of Oxygen.1244JANKASCH (P.). Estimation of Sulphnric Acid in Presence of Iron.1244LUNGE (G.). 1244PAD$ i L.).Milk.1244DROWN (T.M.).Silicon.1245HUGHES (J.). dnttlysis of Concentrated Superphosphate. 1245JONES (C.).Pjg.iron.1246Source of Error in Separating Traces of Manganese from muchLime by Ammonium Sulphide. 1087Potassium Chromate as a Reagent for the Purity ofUse of Ammonium Acetate in Detecting Nitrites by Griess’Estimation of Sulphuric Acid in Presence of Iron.Detection and Est. imation of Sodium Hydrogen Carbonate inEstimation of Phosphorus in Iron in the Presence ofMethod of Rapid Evaporation for the Estimation of Silicon iCAENOT (A.). Volumetric Estimation of Mercury. Thallium. and Silver .KRUSS (G.) and H.MORAHT.Spectro-colorimetric Estimation of Iron andThiocyanates.JONES (C).Reduction of Ferric Sulphate in Volumetric Analysis .LINDET (L.). Simultaneous Estimation of Saccharose and Raffinose .LIRDO (D.). Analyeis of GlassCARNOT (A.). Separation of Cobalt and Nickel.BLAU (F.). Elementary Analysis.ESCHWEILER (W.).SALKOWSEI (E.). Estimation of Uric Acid in Urine.PATRICK (G.E.).WRAMPELMEYER (E.). Estimation of Fat in Linseed-cake.BRULLE (R.). Reactions of Oils with Silver Pu’itrate.Psmm (C.). Error in the Detection of Albumin.VolumetricPAGE

ISSN:0368-1769    

DOI:10.1039/CA88956FP001

出版商:RSC    

年代:1889

数据来源: RSC

摘要:

INORGANIC CHEJIISTRY. 13 I n o r g a n i c Chemistry. List of Elementary Substances announced from 1877 to 1887. By H. C. BOLTON (Chem. News, 58, 188).-The names of 58 substances, announced as being elementary, together with their sources and the names of their discoverers, are given in tabular form. By E. ALLARY (Bull. XOC. Cliim., 49, 865-867) .-The author cites the isomorphism of potassium chloride and potassium cyanide as fresh evidence in support of the views of Brodie, Dumag, Lockyer, and others that chlorine is composed of two elements. If the atomic weight of chlorine is dirided into two parts proportioiial to the atomic weights of carbon and nitrogen, the two constituents of chlorine would have the atomic weights 19.1 and 16.4 respectively. From the study of certain series of organic com- pounds, Dumas came to the conclusion that chlorine consists of two elements, the atomic weights of which are 19 and 16.5 respectively. If this view were correct, chlorine would probably be composed of fluorine and oxygen, and the oxygen is perhaps intimately united H with --.Meyer’s observation that oxygen is produced when chlorine 2 is strongly heated, may be adduced in support of this theory. Apparatus for a Constant Supply of Chlorine. Chlorine and Cyanogen. F. S. K. By .A. VOSMAER ( Z a i t . anal. Chem., 27, 638-640).-The manganese dioxide is used in fragments of the size of peas, andis placed in a two-necked bottle, a t the bottom of which there is a layer of broken glass o r pumice. This stands in a water-bath. Hydrochloric acid is supplied irom a reservoir a t a higher level by a tube reaching to the bottom of the layer of glass, a T-piece and stopcocks allowing the same tube to Serve for the removal of the manganese solution.The corks should be soaked in paraffin. Suitable drying apparatus can be attached, and will not require replenishing for a long time. The chlorine begins to come oft’ when the temperature of the bath reaches 50°, and by means of a stopcock on the outlet its rate is completely under control. The evolution can speedily be arrested by closing t,he stop- cock a t the outlet of the d q i n g apparatus and emptying the water- bath. The apparatus is then left full of chlorine, and is ready a t any moment to give a supply of the gas completely free from oxygen. M. J .S. Dissemination of Sulphur and Phosphorus in Masses of Metal. By H. N. WARREN (Chenz. Ncws, 58, 177--178).--When sulphur is well mixed with excess of molten iron, and a rod cast from14 ABSTRACTS OF BHEMICAL PAPERS. the mass is made the positive electrode of an electriccircuit, in a bath of ferrous chloride, with a platinum 01- copper negative electrode, tile metallic iron is dissolred and is precipitated on the negative elec- irode, whilst ferrous sulphide, FeS, remains attached to the positive electrode. I n the same way, iron phosphide, Fe4P, may be separated from a mam of the metal. Other metals of the iron group behave in a similar manner. The author r e p r d s the above compounds, FeS, Fe4P, and the compound Fe,Si. obtained by him, as the lowest forms of the respective iron sulphides, phosphides, or silicides, although ordinary analytical results may indicate still lower forms, owing to the intimate dissemination of these compound< throughout the mass of the metal.The sulphides of the metals of the second group are not disseminated in this way ihrough the mass of the metal (compare Abstr., 1888, 555-556). Preparation of Hydrogen Iodide. By A. ~ A R D (Bdl. XOC. Cltim., 49, 742-743) .-In preparing- hydrogen iodide from iodine and amorphous phosphorus, the authw places the iodine in a flitsk provided with a bent, neck and connected with the vessel contailling the phosphorus and water by means of a bent tube. By turning the flask round the bent tube, fresh quantities of iodine can be added when requisite without admitting air into the apparatus.Hydrogen Sulphide Apparatus. By J. H. J. DAGGER (Chem. News, 58, 127).-The apparatus figured and described consists of two glass globes connected by india-rubber tubing. The acid is put in one of the globes, the ferroiis sulphide (zinc or marble) in the other ; they are fi.tted with tubes and corks and then fixed in a suit- able position. D, A. L. Apparatus for the Preparation of Hydrogen Sulphide. By P. CHANTEMILLE (Bzdl. Roc. Chim., 50,170-171).-The iron sulphide is contained i n an kpouvrette, and the acid in an ordiiiary flask fitted with a doubly-bored cork, through the one hole of which is passed a tnbe reaching to the bottom of the flask, and closed a t its upper end by an india-rubber tube and pinch-cock ; the second hole is fitted with x short# tube bent a t right angles and fitted to the lower end of the bpouvrette.The force of gas is increased or diminished by raising or lowering the flask. By E. J. MAUMENB (Bull. SOC. Chin?., 49, t350-85~).-Ch!/dr(iza~ne is evolved when a fiolntion of potassium permanganate (158 grams) and sulphuric acid (40 prams SO,) is added to dried, crystallised ammonium oxalate (141.2 grams), the whole well mixed and gently heated until it begins to boil. The gafeous product is absorbed in hydrochloric acid and a neutral solution of the salt can thus be obtained. The hyrl~o- chlwide is crystalline and very readily soluble in water, but only sparingly in alcohol. The sublimed salt has the composition N2H,O,2HC1, but the crystals dried by means of the anhydrous salt contain one-fifteenth of their weight of water.When a solution of D. A. L. F. S. K. The gas is purified in the usual manner. N. H. &I. Chydrazaine or Protoxide of Ammonia.INdRGANIC CHEJJISTRP. 35 the hydrochloride is mixed with platinic chloride, a pZatinochloride is obtained, the composition of which varies with the conditions of the experiment ; with excess of the hydrochloride, a yellow salt is formed, the composition of which is approximately NzH,0,H2PtC16, but if excess of platinic chloride is added, the proportion of platinum is sensibly increased. The suZpphate is crystalliiie and soluble in water, but only very sparingly so in absolute alcohol ; it forms a double salt with aluminium sulphate. The nitrate is crystalline. When a solu- tion of the nitrate is evaporated, nitric acid, nitric peroxide, nitrogen, and a compound having the composition NzHz are evolved.Action of the Electric Spark on Mlxtures of Nitric Oxide with Hydrogen, with Methane, &c. By S. COOKE ( C h e w News, 58, 130--131).-Under the influence of sparks (from a coil capable of giving a 4-inch spark), with the eudiometer wires half an inch apart, a mixture of hydrogen and nitric oxide always explodes, pro- vided the proportion of hydrogen to nitric oxide does not exceed 6 : 10 ; but with the wires closer together, or with a feeble coil, or if the pressure is diminished to 300 mm. of mercury, no explosion occurs. The carefully dried gases explode quite as readily as when they are not dried. The nature of the gaseous mixture after explosion varies very considerably, but there is little doulnt that much of the nitric oxide is converted into oxygen aiid nitrogen.Explosions have also been obtained with nitric oxide and hydrogen sulphide ; with nitric oxide and methane with the production of carbonic anhydride and oxygen : other hydrocarbons i n proper proportions and suitable spa1.k make an explosive mixture with nitric oxide. Carbonic and nitric oxides mixed do not explode under the influence of the spark, but combination goes on gradually with the production of carbonic anhy- dride and nitrogen. Decomposition of Nitric Oxide in Contact with Water and with Potash. By S. COOKE (Chem. News, 58, 155--156).--Nitric oxide exposed in tubes over water in the dark undergoes gradual decomposition with the production of nitrous acid, nitrogen, and a little nitrous oxide.The change is always slow, but is more active at the commencement than a t the end of an experiment; it is also accelerated by the presence of platinum and by heat, whilst admix- ture with hydrogen retards it. The actionof potassium hydroxide on nitric oxide is also aided by platinum and heat (oompare this Journal, 18i7, ii, 37). BJ- L. W. I?. S. K. D. A. L. D. A. L. Action of Hydrogen Sulphide on Arsenic Acid. MCCAY (Zeit. an/iZ. Chern., 27, 632-634; compare Brauner and Toinihek, Trans., 1888, 145).-When a slow stream of hydrogen sulphide is passed through an acidified solution of an arsenate a t 7u0, besides arsenic pentasulphide there is also formed Home free thioxy- arsenic acid, H,As03S.This, under the influence of mineral acids and heat, decomposes into free sulphur and arsenious acid, the latter of which then yields arsenic trisulphide with the hydrogen sulphide. A solution of thioxyarsenic acid may be obtained by passing hydro-16 ABSTRACTS OF CHEMICAL PAPERS. gen sulphide not in excess into a cold, dilute, acidified solution of potassium arsenate. If R larger quantity of hydrogen sulphide is employed, the excess may be removed either by immediate addition of copper sulphate or by a vigorous stream of air bubbles. An opalescence caused by free sulphur may be removed by shaking with asbestos. The clear, strongly acid liquid obtained, exhibits the fol- lowing pPoperties. It remains clear for a long time after addition of sulphuric or hydrochloric acid ; it gives no immediate precipitate with hydrogen sulphide, but ultimately yields one.When boiled, i t gives a precipitate of pure sulphur, without evolution of hydrogen sulphide or sulphurous anhydricle. With hydrogen sulphide, the boiled and cooled liquid gives an immediate precipitate of arsenic trisulphide ; it gives no precipitate with copper sulphate ; with mercuric chloride it gives immediately a heavy yellowish-white precipitate ; with silver sulphate it gives a heavy black precipitate, the filtrate from which contains no arsenious acid. The potassium thioxyarsenate of Bouquet and CloGz agrees with this solution in all the above particulars. M. J. S. Barium Sulphite. By E. R. HODGES (Chem. News, 58, 128); G. S. JOHNSON (ibid., 155).-Hodges' experiments led him to infer that barium sulphite is insoluble in hydrochloric acid ; but 3ohnsoii proves it to be readily and completely soluble in that solvent.He, moreover, shows that pure aqueous barium chloride is not precipitated by sulphrnrous acid, but that i n the presence of dissolved oxygen a precipitate of barinm sulphate forms. n. A. L. Solubility of Gypsum. By G. A. RAUPFNSTRAUCH ( C h ~ m . Cent?,, 1888, 891-822, from Pharin. Centrulhal., 29,229-233).-The author finds that a saturated solution of gypsum is readily obtained, but supersaturation of the solution can only be obviated by shaking the solution for some time. The solubility of gypsum increases up to the temperature of 32", between 32" and 38" it, remains almost constant, and at, higher temperatures than 38" decreases.Natural gypsum comports itself like artificial, provided it be pure. After heating, gypsum takes up water of crystallisation more or less rapidly, and shows the normal solubility again. J. W. L. Ancient Mortar from a Roman Wall in London. By J. SPILLER (Chem. News, 58, 189).-While examining some mortar from a Roman wall, exposed when sinking the foundations of the new Post Office buildings in St. Martin's-le-Grand, the author found, after extracting as much silica as possible by means of dilute hydro- chloric acid, that the residue yielded nearly 11 per cent. of silica to cold dilute sodium hydroxide. Under similar treatment with cold soda, builder's sand and pulverised flints yield a mere trace of silica in solution, whilst mortars 20, 160, and many hundreds of years old yielded quantities of silica increasingwith the age of the mortar.The author suggests that perhaps the Romans used a puzzuolana in com- pounding their mortar, or perhaps this soluble silica or silicate is the direct result of long contact of plain sand and lime. The mortarIN0 RGANIC CHEMISTRY. 17 from St. Martin's-le-Grand had the following composition per cent: :-Sand and brick, 46.48 ; acid-soluble, SiO, 0.52 ; alkali-solublt~, SiO, 10.44, A1,0, 3.00, Fez03 0.48, CaO 20.02, MgO 0.76, CO, 13-03, SO3 0.37,NaCl trace, H,O and loss 4.90. D. A. L. Analysis of Money. By 5. C. WELCH (Chem. News, 58, 164- 165) .-The author has analysed some specimens of " matlilla money'' made in Birmingham. It is yello wish-red, reddish-yellow, brass or bronze-like in colour, and in shape like a G.They proved to be variable alloys of lead and copper with small quantities of iron, tin, zinc, antimony, and arsenic. Some contained pieces of originally unmolten metal, and some had a semi-fused appearance. Another coin resembling gold in colour contained per cent. : Cu, 62-58 ; Zn, 37.26 ; Fe, 0.11 ; Pb, 0.013, and had been silvered to pass for a 6d.-piece. D. -4. L. New Hydrated Cupric Chloride. By E. CHUARD (Chem. Centr., 1888, 887, from Arch. sci. Phys. Nat. Gendve [3], 19, 477).-A hydrated cupric chloride of the formula CuCI, + 3H,O crystallises from the solution of the green hydrate when cooled down to 0". The existence of this compound explains the change in the colour of the solution which takes place when it suffers dilntion, for the chloride of the green hydrate contains only 2 mols. HzO, and by diluting or by cooling below O", the chloride with 3 mols.H,O is formed, and gives a blue colour to the solution. The latter chloride again loses 1 mol. H,O when the solution is boiled. J. W. L. Purification of Mercury. By J. M. CRAFTS (BuZ7. Xoc. Chim., 49, 856--860).-Mercury can be completely freed from lead, zinc, tin, and other impurities by placing it in a slightly inclined glass tube provided with a funnel at the lower extremity, and aspirating a gentle stream of air through the apparatus for about 48 honrs. The oxides of the metals collect at the upper end of the tube, and after about 24 hours, as a rule, the surface of the mercury is quite clean and the operation is finished. Large quantities can be treated in this way, but mercury which has been used for amalgamating zinc contains such a large amount of impurity that this method cannot be suitably employed.A stream of piire air was passed through pure mercury contained in the apparatus described above, but even after 10 days' time no appreciable quantity of oxide was formed. Platinum, in the form of thin foil, is not attacked by cold mercur-, but when the latter is boiled, air being excluded, the platinum is gradually acted on. Only a small quantit? is dissolved, as a large proportion separates in the form of a black powder, and almost the whole is simply held in suspension. The surface of the mercury remains bright, but when a stream of air is passed, the platinum collects at the surface aft,er some time as a black powder, and on dis- tilling the separated mercury only a very small quantity of platinum remains.F. S. K. Silver is not removed by this process. VOL. LVI. C18 ABSTRACTS OF’ CHEMICAL PAPERS. Yttrium-Potassium and Y ttrium-Sodium Phosphates. Bg A. DUBOIN (Compt. rend., 107, 622-624) .-YYtt&ma-pofassiurn pyro- phosphate, K2O,YZO3,2PzO5, is obtained by saturating potassium meta- phosphate with yttrium oxide a t a bright red heat, and then keeping the mixture a t a somewhat lower temperature for a considerable time. The cooled product is extracted with water, when the phosphate remains undissolved. It forms small, colourless, highly birefractive prisms. Yttrium-potassium orthophosphate, 3K20,YZO3,2P2O5, is obtained by adding excess of yttria to a fnsed mixture of potassium pyrophos- phate with nine times its weight of potassium chloride, and heating over a Bunsen burner f o r 20 minutes. It crystallises in brilliant, hexagonal lamellae; sp.gr. at 20” = 3.3. The same product is obtained on heating amorphous yttrium phosphate to redness, o r even to a much higher temperature, with excess of potassium sulphate. Another orthophosphate, 3Kz0,5Y20,,6P205, is obtained by heating potassium sulphate to a high temperature with a much larger propor- tion of yttrium phosphate. It forms brilliant, trausparent, colour- less, hexagonal prisms. If the mixture of yttrium phosphate and potassium sulphate con- tains 10 per cent. of the former, and is heated t o a very high tempe- rature for about 10 hours, yttrium phosphate is obtained i u a form identical with xenotime.C. H. B. So-called (( Crackle” China. By C. LAUTH and G. DUTATLLY (Bull. Xoc.. Chim., 49, 948--956).-The name crackle china is given to china, the glazing of which is cracked in a regnlai- manner so as to form a sort of network. If the appearance is similar to that of fish scales, the china is said to be “ troutod.” The Chinese colour the interstices by means of smoke or Indian ink, and the articles thus produced are valued very highly. The crackle effect is due to the unequal contraction of the glaze and of the paste. When the firing is continued for a certain time, the coefficients of expansion of the glaze and of the paste gradually become identical, and i f the firing is stopped at this point the crackle effect is not produced ; if, however, the burning is continued, the co- efficients of expansion again become different, and fracture of the glaze takes place on cooling.If the temperature which is required for a certain paste and a certain glaze to give perfect porcelain is known, and if the baking is always arrested a t this point, the crackle effect can be obtained by altering the composition of the paste or that of the glaze. The latter alternative is the more practical, but i t was found necessary to alter the degree of fusibility of the glaze at the same time. As, for various reasons, i t is disadvantageous to employ a readily fusible glaze, the temperature of fusion was raised by adding a larger pro- portion of silica.The paste experimented on is that employed at Sdvres ; its composition is- Silica, 66 ; alumina, 27 ; alkalis, 7 ; and the ordinary glaze employed a t Sbvres has the composition-INORQANIC CHEMISTRY. 19 Silica ................ 66-18 Alumina. ............. 14-55 Alkalis, .............. 3.55 Chalk.. .............. 15-90 The glaze which was found to give the best crackle effecb has the following composition :- Silica ................ 79.42 Alumina, ............. 11 -80 Alkalis. .............. 5-51 Chalk.. .............. 2-88 Crackle china is also produced if the pEoportion of alumina in the glaze is increased, for example with a glaze composed of- Silica, 69-92; alumina, 18.13 ; alkalis, 11.95, but the effects produced are not so good, and it seems that fracture more frequently occurs.Whichever method is adopted, it is always nnrticularly advantageous to substitute the chalk in the glaze for kknlis. If the propartion of alumina is increased, the necessary degree of fusibility is obtained by addimg other bases ; if the propor- tion of alumina is decreased, the quantity of other bases is diminished, and an additional quantity of silica is added. It was found that with a given glaze the crackle china can be pro- duced by making the paste more readily fusible. This can be done by increasing the quantity of felspar, and the results are better the smaller the proportion of quartz contained i n the paste. The extreme composition of the unbaked paste employed for these experiments was- Silica, 58.5 ; alumina, 28.0 ; alkalis, 5.5 ; water, 8.0.The glaze should be of medium thickness, and to obtain a close mesh it should have the composition given in one of the above two examples. If a larger mesh is required the " crackle " glaze is mixed with the ordinary glaze, and the mesh is larger the greater the pro- portion of the latter. It is advisable to make crackle china of sufficient thickness t o avoid all chance of fracture. F. S. K. Atomic Weight of Tin. By T. BONGARTZ and A. CLASSEN (Bey., 21, 2'300-2909) .-The authors made determinations of the atomic weight of tin (1) by oxidising the pure metal with nitric acid; (2) by the electrolysis of ammonium stannic chloride ; ( 3 ) by the electroljsls of potassium stannic chloride ; and (4) by the electrolysis of stannic bromide. The results are given in &he following table :- Number of Difference between experiments.Atomic weight. maximum and minimum. (1.) ...... 11 11 8,7606 u-459 (3.) ...... 10 118-7975 0.1 63 (4.) ...... 10 11 8.7309 0.144 ...... ( 2 . ) 16 118.8093 0.228 - Total ... 47 Average 118.7745 0 *;I 4s 5 c 220 ABSTRACTS OF CHEMICAL PAPERS. The average of the 26 results obtained by the electrolysis of the ammonium and potassium double salts is higher than the average of all the results. This is probably due to the fact that in oxidisinq the tin, the platinum vessel is always attacked to a slight extent, and that in dissolving the stannic bromide, a small portion may be lost by volatilisation. If, therefore, the average of the 26 experiments is taken as the most trustworthy result, the atomic weight of tin is 118.8034 (0 = 15.96) or 119.1 (0 = 16). Experiments in which it was sought to determine the atomic weight by converting pure tin into stannic sulphide, and estimating the sulphur in the latter, did not give satisfactory results (118.676 as the average of eight experiments). It was also found that when the oxide is reduced with pure hydrogen, it small quantity of tin is always volatilised.F. S. K. Action of Incandescent Platinum Wire on Gases and Vapours. By W. R. HODGKINSON and F. I(. S LOWNDES (Chern. News, 58, 187).-When a spiral of platinum wire is exposed to the action of chlorine in a glass globe and rendered incandescent by 2n electric current, a white glow is observed round the heated wire, the sides of the globe become covered with platinous chloride, arid very fine crystals of platinum are formed on the wire.With bro- mine or iodine vapour, the flame round the wire is greatly increased, but only a very small quantity of platinous bromide or a trace of the iodide is formed, and no crystalline metal is produced. With dry silicon fluoride, crystals of silicon are deposited, and the top of the globe is deeply corroded, presumedly by the liberated fluorine. D. A. I;. Normal Platinum Chloride. By R. ENGEL (BUZZ. HOG. Chi~z., 50, 100-102) .--Norm:tl platinum chloride, PtCla + 4H20, can be obtained by dissolving the calculated amount of platinum oxide in a solution of platinum chloride hydrochloride; the liquid is filtered and evaporated. The crystals are deliquescent like those of the hydro- chloride.When dry h j drogen chloride is passed over the crystals heated a t 50°, the hydrochloride is formed ; a t a lower temperature no combination takes place. N. H. M.INORGANIC CHEJIISTRY. 13I n o r g a n i c Chemistry.List of Elementary Substances announced from 1877 to1887. By H. C. BOLTON (Chem. News, 58, 188).-The names of 58substances, announced as being elementary, together with theirsources and the names of their discoverers, are given in tabular form.By E. ALLARY (Bull. XOC. Cliim., 49,865-867) .-The author cites the isomorphism of potassium chlorideand potassium cyanide as fresh evidence in support of the views ofBrodie, Dumag, Lockyer, and others that chlorine is composed oftwo elements.If the atomic weight of chlorine is dirided into twoparts proportioiial to the atomic weights of carbon and nitrogen, thetwo constituents of chlorine would have the atomic weights 19.1 and16.4 respectively. From the study of certain series of organic com-pounds, Dumas came to the conclusion that chlorine consists of twoelements, the atomic weights of which are 19 and 16.5 respectively.If this view were correct, chlorine would probably be composed offluorine and oxygen, and the oxygen is perhaps intimately unitedH with --. Meyer’s observation that oxygen is produced when chlorine 2is strongly heated, may be adduced in support of this theory.Apparatus for a Constant Supply of Chlorine.Chlorine and Cyanogen.F. S. K.By .A.VOSMAER ( Z a i t .anal. Chem., 27, 638-640).-The manganese dioxideis used in fragments of the size of peas, andis placed in a two-neckedbottle, a t the bottom of which there is a layer of broken glass o rpumice. This stands in a water-bath. Hydrochloric acid is suppliedirom a reservoir a t a higher level by a tube reaching to the bottom ofthe layer of glass, a T-piece and stopcocks allowing the same tube toServe for the removal of the manganese solution. The corks shouldbe soaked in paraffin. Suitable drying apparatus can be attached,and will not require replenishing for a long time. The chlorinebegins to come oft’ when the temperature of the bath reaches 50°, andby means of a stopcock on the outlet its rate is completely undercontrol. The evolution can speedily be arrested by closing t,he stop-cock a t the outlet of the d q i n g apparatus and emptying the water-bath.The apparatus is then left full of chlorine, and is ready a t anymoment to give a supply of the gas completely free from oxygen.M. J . S.Dissemination of Sulphur and Phosphorus in Masses ofMetal. By H. N. WARREN (Chenz. Ncws, 58, 177--178).--Whensulphur is well mixed with excess of molten iron, and a rod cast fro14 ABSTRACTS OF BHEMICAL PAPERS.the mass is made the positive electrode of an electriccircuit, in a bathof ferrous chloride, with a platinum 01- copper negative electrode, tilemetallic iron is dissolred and is precipitated on the negative elec-irode, whilst ferrous sulphide, FeS, remains attached to the positiveelectrode.I n the same way, iron phosphide, Fe4P, may be separatedfrom a mam of the metal. Other metals of the iron group behavein a similar manner. The author r e p r d s the above compounds,FeS, Fe4P, and the compound Fe,Si. obtained by him, as the lowestforms of the respective iron sulphides, phosphides, or silicides,although ordinary analytical results may indicate still lower forms,owing to the intimate dissemination of these compound< throughoutthe mass of the metal. The sulphides of the metals of the secondgroup are not disseminated in this way ihrough the mass of the metal(compare Abstr., 1888, 555-556).Preparation of Hydrogen Iodide. By A. ~ A R D (Bdl. XOC.Cltim., 49, 742-743) .-In preparing- hydrogen iodide from iodineand amorphous phosphorus, the authw places the iodine in a flitskprovided with a bent, neck and connected with the vessel contaillingthe phosphorus and water by means of a bent tube.By turning theflask round the bent tube, fresh quantities of iodine can be added whenrequisite without admitting air into the apparatus.Hydrogen Sulphide Apparatus. By J. H. J. DAGGER (Chem.News, 58, 127).-The apparatus figured and described consists oftwo glass globes connected by india-rubber tubing. The acid is putin one of the globes, the ferroiis sulphide (zinc or marble) in theother ; they are fi.tted with tubes and corks and then fixed in a suit-able position. D, A. L.Apparatus for the Preparation of Hydrogen Sulphide. ByP. CHANTEMILLE (Bzdl. Roc. Chim., 50,170-171).-The iron sulphideis contained i n an kpouvrette, and the acid in an ordiiiary flask fittedwith a doubly-bored cork, through the one hole of which is passed atnbe reaching to the bottom of the flask, and closed a t its upper endby an india-rubber tube and pinch-cock ; the second hole is fitted withx short# tube bent a t right angles and fitted to the lower end of thebpouvrette. The force of gas is increased or diminished by raising orlowering the flask.By E.J. MAUMENB(Bull. SOC. Chin?., 49, t350-85~).-Ch!/dr(iza~ne is evolved when afiolntion of potassium permanganate (158 grams) and sulphuric acid(40 prams SO,) is added to dried, crystallised ammonium oxalate(141.2 grams), the whole well mixed and gently heated until itbegins to boil.The gafeous product is absorbed in hydrochloric acidand a neutral solution of the salt can thus be obtained. The hyrl~o-chlwide is crystalline and very readily soluble in water, but onlysparingly in alcohol. The sublimed salt has the compositionN2H,O,2HC1, but the crystals dried by means of the anhydrous saltcontain one-fifteenth of their weight of water. When a solution ofD. A. L.F. S. K.The gas is purified in the usual manner.N. H. &I.Chydrazaine or Protoxide of AmmoniaINdRGANIC CHEJJISTRP. 35the hydrochloride is mixed with platinic chloride, a pZatinochloride isobtained, the composition of which varies with the conditions of theexperiment ; with excess of the hydrochloride, a yellow salt is formed,the composition of which is approximately NzH,0,H2PtC16, but ifexcess of platinic chloride is added, the proportion of platinum issensibly increased.The suZpphate is crystalliiie and soluble in water,but only very sparingly so in absolute alcohol ; it forms a double saltwith aluminium sulphate. The nitrate is crystalline. When a solu-tion of the nitrate is evaporated, nitric acid, nitric peroxide, nitrogen,and a compound having the composition NzHz are evolved.Action of the Electric Spark on Mlxtures of Nitric Oxidewith Hydrogen, with Methane, &c. By S. COOKE ( C h e w News,58, 130--131).-Under the influence of sparks (from a coil capableof giving a 4-inch spark), with the eudiometer wires half an inchapart, a mixture of hydrogen and nitric oxide always explodes, pro-vided the proportion of hydrogen to nitric oxide does not exceed6 : 10 ; but with the wires closer together, or with a feeble coil, or if thepressure is diminished to 300 mm.of mercury, no explosion occurs.The carefully dried gases explode quite as readily as when they arenot dried. The nature of the gaseous mixture after explosion variesvery considerably, but there is little doulnt that much of the nitricoxide is converted into oxygen aiid nitrogen. Explosions have alsobeen obtained with nitric oxide and hydrogen sulphide ; with nitricoxide and methane with the production of carbonic anhydride andoxygen : other hydrocarbons i n proper proportions and suitable spa1.kmake an explosive mixture with nitric oxide. Carbonic and nitricoxides mixed do not explode under the influence of the spark, butcombination goes on gradually with the production of carbonic anhy-dride and nitrogen.Decomposition of Nitric Oxide in Contact with Water andwith Potash.By S. COOKE (Chem. News, 58, 155--156).--Nitricoxide exposed in tubes over water in the dark undergoes gradualdecomposition with the production of nitrous acid, nitrogen, and alittle nitrous oxide. The change is always slow, but is more active atthe commencement than a t the end of an experiment; it is alsoaccelerated by the presence of platinum and by heat, whilst admix-ture with hydrogen retards it. The actionof potassium hydroxide onnitric oxide is also aided by platinum and heat (oompare this Journal,18i7, ii, 37).BJ- L.W.I?. S. K.D. A. L.D. A. L.Action of Hydrogen Sulphide on Arsenic Acid.MCCAY (Zeit. an/iZ. Chern., 27, 632-634; compare Brauner andToinihek, Trans., 1888, 145).-When a slow stream of hydrogensulphide is passed through an acidified solution of an arsenate a t 7u0,besides arsenic pentasulphide there is also formed Home free thioxy-arsenic acid, H,As03S. This, under the influence of mineral acidsand heat, decomposes into free sulphur and arsenious acid, the latterof which then yields arsenic trisulphide with the hydrogen sulphide.A solution of thioxyarsenic acid may be obtained by passing hydro16 ABSTRACTS OF CHEMICAL PAPERS.gen sulphide not in excess into a cold, dilute, acidified solution ofpotassium arsenate. If R larger quantity of hydrogen sulphide isemployed, the excess may be removed either by immediate additionof copper sulphate or by a vigorous stream of air bubbles.Anopalescence caused by free sulphur may be removed by shaking withasbestos. The clear, strongly acid liquid obtained, exhibits the fol-lowing pPoperties. It remains clear for a long time after addition ofsulphuric or hydrochloric acid ; it gives no immediate precipitatewith hydrogen sulphide, but ultimately yields one. When boiled, i tgives a precipitate of pure sulphur, without evolution of hydrogensulphide or sulphurous anhydricle. With hydrogen sulphide, the boiledand cooled liquid gives an immediate precipitate of arsenic trisulphide ;it gives no precipitate with copper sulphate ; with mercuric chlorideit gives immediately a heavy yellowish-white precipitate ; with silversulphate it gives a heavy black precipitate, the filtrate from whichcontains no arsenious acid.The potassium thioxyarsenate of Bouquetand CloGz agrees with this solution in all the above particulars.M. J. S.Barium Sulphite. By E. R. HODGES (Chem. News, 58, 128);G. S. JOHNSON (ibid., 155).-Hodges' experiments led him to inferthat barium sulphite is insoluble in hydrochloric acid ; but 3ohnsoiiproves it to be readily and completely soluble in that solvent. He,moreover, shows that pure aqueous barium chloride is not precipitatedby sulphrnrous acid, but that i n the presence of dissolved oxygen aprecipitate of barinm sulphate forms. n. A. L.Solubility of Gypsum. By G.A. RAUPFNSTRAUCH ( C h ~ m . Cent?,,1888, 891-822, from Pharin. Centrulhal., 29,229-233).-The authorfinds that a saturated solution of gypsum is readily obtained, butsupersaturation of the solution can only be obviated by shaking thesolution for some time. The solubility of gypsum increases up to thetemperature of 32", between 32" and 38" it, remains almost constant,and at, higher temperatures than 38" decreases. Natural gypsumcomports itself like artificial, provided it be pure. After heating,gypsum takes up water of crystallisation more or less rapidly, andshows the normal solubility again. J. W. L.Ancient Mortar from a Roman Wall in London. ByJ. SPILLER (Chem. News, 58, 189).-While examining some mortarfrom a Roman wall, exposed when sinking the foundations of thenew Post Office buildings in St.Martin's-le-Grand, the author found,after extracting as much silica as possible by means of dilute hydro-chloric acid, that the residue yielded nearly 11 per cent. of silica tocold dilute sodium hydroxide. Under similar treatment with coldsoda, builder's sand and pulverised flints yield a mere trace of silicain solution, whilst mortars 20, 160, and many hundreds of years oldyielded quantities of silica increasingwith the age of the mortar. Theauthor suggests that perhaps the Romans used a puzzuolana in com-pounding their mortar, or perhaps this soluble silica or silicate is thedirect result of long contact of plain sand and lime. The mortaIN0 RGANIC CHEMISTRY. 17from St. Martin's-le-Grand had the following composition percent: :-Sand and brick, 46.48 ; acid-soluble, SiO, 0.52 ; alkali-solublt~,SiO, 10.44, A1,0, 3.00, Fez03 0.48, CaO 20.02, MgO 0.76, CO, 13-03,SO3 0.37,NaCl trace, H,O and loss 4.90.D. A. L.Analysis of Money. By 5. C. WELCH (Chem. News, 58, 164-165) .-The author has analysed some specimens of " matlilla money''made in Birmingham. It is yello wish-red, reddish-yellow, brass orbronze-like in colour, and in shape like a G. They proved to bevariable alloys of lead and copper with small quantities of iron, tin,zinc, antimony, and arsenic. Some contained pieces of originallyunmolten metal, and some had a semi-fused appearance. Anothercoin resembling gold in colour contained per cent. : Cu, 62-58 ;Zn, 37.26 ; Fe, 0.11 ; Pb, 0.013, and had been silvered to pass for a6d.-piece. D.-4. L.New Hydrated Cupric Chloride. By E. CHUARD (Chem. Centr.,1888, 887, from Arch. sci. Phys. Nat. Gendve [3], 19, 477).-A hydratedcupric chloride of the formula CuCI, + 3H,O crystallises from thesolution of the green hydrate when cooled down to 0". The existenceof this compound explains the change in the colour of the solutionwhich takes place when it suffers dilntion, for the chloride of thegreen hydrate contains only 2 mols. HzO, and by diluting or bycooling below O", the chloride with 3 mols. H,O is formed, and givesa blue colour to the solution. The latter chloride again loses 1 mol.H,O when the solution is boiled. J. W. L.Purification of Mercury. By J. M. CRAFTS (BuZ7.Xoc. Chim.,49, 856--860).-Mercury can be completely freed from lead, zinc, tin,and other impurities by placing it in a slightly inclined glass tubeprovided with a funnel at the lower extremity, and aspirating agentle stream of air through the apparatus for about 48 honrs. Theoxides of the metals collect at the upper end of the tube, and afterabout 24 hours, as a rule, the surface of the mercury is quite cleanand the operation is finished. Large quantities can be treated inthis way, but mercury which has been used for amalgamating zinccontains such a large amount of impurity that this method cannot besuitably employed.A stream of piire air was passed through pure mercury containedin the apparatus described above, but even after 10 days' time noappreciable quantity of oxide was formed.Platinum, in the form of thin foil, is not attacked by cold mercur-,but when the latter is boiled, air being excluded, the platinum isgradually acted on.Only a small quantit? is dissolved, as a largeproportion separates in the form of a black powder, and almost thewhole is simply held in suspension. The surface of the mercuryremains bright, but when a stream of air is passed, the platinumcollects at the surface aft,er some time as a black powder, and on dis-tilling the separated mercury only a very small quantity of platinumremains. F. S. K.Silver is not removed by this process.VOL. LVI. 18 ABSTRACTS OF’ CHEMICAL PAPERS.Yttrium-Potassium and Y ttrium-Sodium Phosphates. BgA.DUBOIN (Compt. rend., 107, 622-624) .-YYtt&ma-pofassiurn pyro-phosphate, K2O,YZO3,2PzO5, is obtained by saturating potassium meta-phosphate with yttrium oxide a t a bright red heat, and then keepingthe mixture a t a somewhat lower temperature for a considerable time.The cooled product is extracted with water, when the phosphateremains undissolved. It forms small, colourless, highly birefractiveprisms.Yttrium-potassium orthophosphate, 3K20,YZO3,2P2O5, is obtained byadding excess of yttria to a fnsed mixture of potassium pyrophos-phate with nine times its weight of potassium chloride, and heatingover a Bunsen burner f o r 20 minutes. It crystallises in brilliant,hexagonal lamellae; sp. gr. at 20” = 3.3. The same product isobtained on heating amorphous yttrium phosphate to redness, o r evento a much higher temperature, with excess of potassium sulphate.Another orthophosphate, 3Kz0,5Y20,,6P205, is obtained by heatingpotassium sulphate to a high temperature with a much larger propor-tion of yttrium phosphate.It forms brilliant, trausparent, colour-less, hexagonal prisms.If the mixture of yttrium phosphate and potassium sulphate con-tains 10 per cent. of the former, and is heated t o a very high tempe-rature for about 10 hours, yttrium phosphate is obtained i u a formidentical with xenotime. C. H. B.So-called (( Crackle” China. By C. LAUTH and G. DUTATLLY(Bull. Xoc.. Chim., 49, 948--956).-The name crackle china is givento china, the glazing of which is cracked in a regnlai- manner so as toform a sort of network.If the appearance is similar to that of fishscales, the china is said to be “ troutod.” The Chinese colour theinterstices by means of smoke or Indian ink, and the articles thusproduced are valued very highly.The crackle effect is due to the unequal contraction of the glazeand of the paste. When the firing is continued for a certain time,the coefficients of expansion of the glaze and of the paste graduallybecome identical, and i f the firing is stopped at this point the crackleeffect is not produced ; if, however, the burning is continued, the co-efficients of expansion again become different, and fracture of the glazetakes place on cooling.If the temperature which is required for a certain paste and acertain glaze to give perfect porcelain is known, and if the baking isalways arrested a t this point, the crackle effect can be obtained byaltering the composition of the paste or that of the glaze.The latteralternative is the more practical, but i t was found necessary to alterthe degree of fusibility of the glaze at the same time. As, forvarious reasons, i t is disadvantageous to employ a readily fusibleglaze, the temperature of fusion was raised by adding a larger pro-portion of silica. The paste experimented on is that employed atSdvres ; its composition is-Silica, 66 ; alumina, 27 ; alkalis, 7 ;and the ordinary glaze employed a t Sbvres has the compositionINORQANIC CHEMISTRY. 19Silica ................ 66-18Alumina. .............14-55Alkalis, .............. 3.55Chalk.. .............. 15-90The glaze which was found to give the best crackle effecb has thefollowing composition :-Silica ................ 79.42Alumina, ............. 11 -80Alkalis. .............. 5-51Chalk.. .............. 2-88Crackle china is also produced if the pEoportion of alumina in theglaze is increased, for example with a glaze composed of-Silica, 69-92; alumina, 18.13 ; alkalis, 11.95,but the effects produced are not so good, and it seems that fracturemore frequently occurs. Whichever method is adopted, it is alwaysnnrticularly advantageous to substitute the chalk in the glaze forkknlis. If the propartion of alumina is increased, the necessarydegree of fusibility is obtained by addimg other bases ; if the propor-tion of alumina is decreased, the quantity of other bases is diminished,and an additional quantity of silica is added.It was found that with a given glaze the crackle china can be pro-duced by making the paste more readily fusible.This can be doneby increasing the quantity of felspar, and the results are better thesmaller the proportion of quartz contained i n the paste. The extremecomposition of the unbaked paste employed for these experimentswas-Silica, 58.5 ; alumina, 28.0 ; alkalis, 5.5 ; water, 8.0.The glaze should be of medium thickness, and to obtain a closemesh it should have the composition given in one of the above twoexamples. If a larger mesh is required the " crackle " glaze is mixedwith the ordinary glaze, and the mesh is larger the greater the pro-portion of the latter.It is advisable to make crackle china of sufficient thickness t oavoid all chance of fracture.F. S. K.Atomic Weight of Tin. By T. BONGARTZ and A. CLASSEN (Bey.,21, 2'300-2909) .-The authors made determinations of the atomicweight of tin (1) by oxidising the pure metal with nitric acid; (2) bythe electrolysis of ammonium stannic chloride ; ( 3 ) by the electroljslsof potassium stannic chloride ; and (4) by the electrolysis of stannicbromide. The results are given in &he following table :-Number of Difference betweenexperiments. Atomic weight. maximum and minimum.(1.) ...... 11 11 8,7606 u-459(3.) ...... 10 118-7975 0.1 63(4.) ...... 10 11 8.7309 0.144...... ( 2 . ) 16 118.8093 0.228-Total ... 47 Average 118.7745 0 *;I 4s 5c 20 ABSTRACTS OF CHEMICAL PAPERS.The average of the 26 results obtained by the electrolysis of theammonium and potassium double salts is higher than the averageof all the results. This is probably due to the fact that in oxidisinqthe tin, the platinum vessel is always attacked to a slight extent, andthat in dissolving the stannic bromide, a small portion may be lost byvolatilisation. If, therefore, the average of the 26 experiments istaken as the most trustworthy result, the atomic weight of tin is118.8034 (0 = 15.96) or 119.1 (0 = 16).Experiments in which it was sought to determine the atomic weightby converting pure tin into stannic sulphide, and estimating thesulphur in the latter, did not give satisfactory results (118.676 as theaverage of eight experiments). It was also found that when the oxideis reduced with pure hydrogen, it small quantity of tin is alwaysvolatilised. F. S. K.Action of Incandescent Platinum Wire on Gases andVapours. By W. R. HODGKINSON and F. I(. S LOWNDES (Chern.News, 58, 187).-When a spiral of platinum wire is exposed to theaction of chlorine in a glass globe and rendered incandescent by 2nelectric current, a white glow is observed round the heated wire,the sides of the globe become covered with platinous chloride, aridvery fine crystals of platinum are formed on the wire. With bro-mine or iodine vapour, the flame round the wire is greatly increased,but only a very small quantity of platinous bromide or a trace of theiodide is formed, and no crystalline metal is produced. With drysilicon fluoride, crystals of silicon are deposited, and the top of theglobe is deeply corroded, presumedly by the liberated fluorine.D. A. I;.Normal Platinum Chloride. By R. ENGEL (BUZZ. HOG. Chi~z., 50,100-102) .--Norm:tl platinum chloride, PtCla + 4H20, can be obtainedby dissolving the calculated amount of platinum oxide in a solutionof platinum chloride hydrochloride; the liquid is filtered andevaporated. The crystals are deliquescent like those of the hydro-chloride. When dry h j drogen chloride is passed over the crystalsheated a t 50°, the hydrochloride is formed ; a t a lower temperatureno combination takes place. N. H. M

ISSN:0368-1769    

DOI:10.1039/CA8895600013

出版商:RSC    

年代:1889

数据来源: RSC

摘要:

20 ABSTRACTS OF CHEMICAL PAPERS. M i n e r a l o g i c a1 C h e m i s t r y , Hexagonal Zinc Sulphide. By W. STAHL (Chem. Centr., 1888, 943, from Berg. Hutt. Zpit., 47, 207--208).-The naturally occurring mineral, wurtzite, which has also been artificially prepared, has been noticed by the author as a product of the blast furnace of the Sophia snielting work in the Lower Harz. It forms clear, wine-yellow, shining, hexagcnal crystals, mostly in tufts, wit,h the faces mP2, €2, 2P2, and OP. Cleavage in the direction R and WE. Hardness = 3-4, sp. gr. = 4.32 ; composition :-BII?r'ERALOGICAL CHEMISTRY. 21 Zn. Fe. Mn. Pb. 5. 66.08 0.55 trace 0.31 32.88 = 99.82 J. W. L. Arsenopyrite from Servia. By A. SCHMIDT (Zeit. Kryst. Mia., 14, 573-574) .--The specimen examined formed part of the collection of the Royal Hungarian Geological Survey at Budapest. It is stated to have come from the Luta Strana adit-level, Servia.The arseno- pyrite occurs, with iron pyrites and zinc blende, in small_prismtrtic crystals, on which were observed the forms mP, OP, $ z P ~ , $Pw, the two last being new for this mineral. The axial ratio is computed t o be a : b : c = 0.686 : 1 : 1.170. Analysis of this arsenopyrite gave the following results :- Fe. As. Sb. S. Zn. Insoluble. Total. 34.58 42.38 0.14 21-71 0.46 0.22 99-49 The percentage of zinc is evidently due to an unavoidable admixture of blende. B. H. B. Formation of Deposits of Oxides of Manganese. Ry F. P. DUNNINGTON (Amer. J. Sci., 36, 175--178).-1n view of the results of a series of 15 experiments, i t appears possible that many deposits of manganese ore in calciferous rocks have been formed by the action of solutions of sulphates rather than of bicarbonates. An illustration of such action is perhaps afforded by the maugnnese deposits of Crimora, Augusta Go., Virginia.Wherever pyrites has been deposited, the outcrop is gradually converted into limonite by weathering, and the acid solution of ferrous sulphate which sinks into the underlying deposits, must carry with it all the manganese in the pyrites itself, and in any disintegrating silicates. As this solution is exposed t o the air or meets with calcium carbonate, ferrous carbonate will be formed, whilst the manganese sulphate will aernain in solution until exposed to the action of both air and calcium carbonate at the same time.B. H. B. Artificial Production of Hydrocerusite. The Composition of this Mineral and the Constitution of White Lead. By L. BOURGEOIS (Bull. SOC. Chi/n., 5 0, 83-85) .-Hydrocerusite, 2PbC03, Pb(OH)z, is formed if a boiling solution of lead acetate (1 mol.) is treated with litharge (l$ mol.), and when cold, with carbamide (1 mol.). The liquid is then filtered and heated at about 130" for some hours, when a quantity of nacreous spangIes separate which are washed with water. These have a sp. gr. = 6.14 at 15", dissolve with effervescence in nitric and acetic acids, and give off water and carbonic anhydride at 400", leaving a residue of massicot slightly coloured by a, trace of minium. White lead consists of a mixture of hydrocerusite and cerusite.N. H. M. Preparation of Pyromorphite and Mimetesite. By L. MICHEL (Zeit. Kryst. Min., 14, 619, from Bull. SOC. franp. win., 10, 133).- The author mixes three equivalents of lead phosphate or arsenate, or a mixture of the two, with one equivaIent of lead chloride in a porcelain crucible. He covers the mixture with a thin layer of lead chloride,22 ABSTRACTS OF CHEMICAL PAPERS. and places the crucible in one of fireclay. Both are hermetically sealed, the intei*mediate space being filled with ignited magnesia. The crucibles are then heated to the melting point of gold, and slowly cooled. The cavities of the fused mass contain hexagonal prisms as much as 2 cm. in length and 1 mm. in width. The best results were obtained with the mixture coryesponding with kampylite (Analysis 4), the prisms being well developed and perfectly transparent.The crystalline productis obtained had the following compositions :- I .............. 2 .............. 3 .............. 4 .............. 5 .............. 6 .............. 7 .............. 8 .............. 9 .............. Pb,As,O,. 89 -75 84 '73 79'85 69.78 46.05 29 '37 19.43 10 *21 -~ -- Pb$?,O,. -- - 4 -9'7 10- 06 20 -0.2 44 -87 59 *24 68 +98 '79 -67 89 *87 PbC12. -- 9-92 10 * 03 8.98 10.07 9 9 9 10 -31 10.12 9 *71 10 * 14 Total. -- 99 -67 99 -73 98 -89 99 '8'7 l00*71 98 -92" 98 *53 99 -59 100 -01 Sp. gr. 7 -12 6 -93 6.97 6 -93 -- -- - - - -- On the addition of a small quaiitity of lead chromate, yellow or In rare cases, they are of a grass-green orange crystals are obtained.colour. B. H. B. Uranite from Madagascar. By E. JANNETTAZ (Zed. Rryst. Min., 14, 608, from Bull. SOG. frung. milt., 10, 47).-The mineral examined forms greenish-yellow aggregates of crystals exactly similar in ap- pearance to those of Autun. H,O. P20,. UO,. Fe,O,. CaO. Total. 22.08 14-93 55-08 1-33 651 99-96 Analysis gave the following results :- These results correspond with the formula (UO,,Fe,Ca),P,O, + 12H,O. Of the proportion of water, 9 per cent. is evolved at 65". B. H. B. Baryto-celestine from Werfen in Salzburg. By E. HATLE and H. TAUSS (Jahrb. f. Min., 1888, ii, Ref., 210, from Tschermak's min. Mitth., 9,227-231) .-The baryto-celestine accompanying the wagner- ite of Werfen has hitherto been regarded as barytes. It forms druses, crystals 1.5 cm. thick, and radiated or granular masses.It is of a pink coloui-, and translucent, with a hardness of 3.5 and a sp. gr. of 4-17. Analysis gave 84.80 per cent. of barium sulphate and 15.03 of strontium sulphate. Arseniopleite, a New Swedish Mineral. By L. J. IGELSTROM (Jahrb. f. &fin., 1888, ii, Mem., 117- 122).--Numerons rare and new minerals occur with braunite and hausmannite at the manganese mine, Sjtigrufvan, in the parish of Gryhyttan, Oerebro, Sweden. In November, 1887, the author discovered there another new mineral, # 99 *51 in the original paper. The formula is 4BaS04 + SrSO1. B. H. B.MXNERALOQTCAL CHEMISTRY. 23 which he names arsenioyZeite from the metal arsenic, and slrX&ov (more). The mineral occurs in intimate association with rhodonite in small veins in dolomite.It also occurs in the same rock in masses 0.5 to 1 cm. in thickness. NO crystals have been found. It is uniaxial and positive, and judging from the cleavage appears to crystallise in rhombohedra1 forms. Analysis gave the following results :- Its colour is cherry-red. A S , ~ , . MnO. Fe,O,. PbO. CaO. MgO. H20. Total. 44.98 28.25 3.68 4.48 8.11 3.10 5.67 98.27 Traces of Sb205 and C1 were observed. Arseniopleite is a basic arsenate, like olivenite. It resembles most closely dindelphite and synadelphite. It, however, contains no alumina. Its relation to the other hydrated arsenates occurring in Sweden may be seen from the following list :- Chondroarsenite.. . . (MnO)~SzO5 + 24Hz0. Xanthoarsenite . . . . (MnO)5As205 + 5H20 (Abstr., 1886, 25). HEmafjbrite .. . . . . (MnO),AsZO5 + 5H20. Polyarsenite . . . . . . (MnO)4Asz05 + HzO (Abstr., 1887, 347). Allactite . . . . . . . . . . (Mn0),As205 + 4H20. Diadelphite.. . . . . . . (MnO),As205 + AlZO3(Fe2O3) + 8H20. Synndelphite . . . . . . (MnO),As,O, + Al2O3(Fe2O,) + 5Hz0. Arseniopleite . . . . . . 3(Mn0,Ca0,Pb0,MgO)3As205 + (Compare Abstr., 1867, 902.) Treatment of Natural Silicates with Hydrochloric Acid as a means of Ascertaining their Structure. By E. A. SCENEIDER (Anwr. Chem. J., 10, 405--408).-Referring to the recent paper by Clarke (Abstr., 1888,659), the author remarks that the weathering of minerals may be used for drawing conclusions as to their constitution, and suggests the carrying out of a number of experiments, substi- tuting hydrochloric acid for the atmospheric carbonic anhydride, and accelerating its action by heating in sealed tubes in a water-bath, the mineral being finely powdered. Minerals of the Tyrol.By A. CATHRRTN (Jahrb. f. Min., 1888, ii, Ref., 2%0-221, from Tschernznk’s min. Mitth., 8,400-413).-1. The so-called Paragonite frona the Zillerthn1.-The composition of this mineral is found to be that of talc, and not that of mica. It is EM f0llOvr~S :- Mn,03(B’e203) + 3H20. B. H. B. H. B. SiO,. MgO. FeO. H,O. Total. 62-24 30.22 2.66 4.97 100.09 This talc is the matrix of the actinolite from this locality. 2. A New Pseudnmorph of Fasstcite.-This was found at Monzoni iu association with crystals of grossular remarkable for the occurrence of the rare plane 40+, first observed by Bauer on garnet from Oravicza.The composition of the fassaite is as follows :-24 ABSTRAUTS OF CHEMICAL PAPERS. Loss on Si02. A120,. Fe20B. FeO. CaO. MgO. ignition. Total. 44.22 12.37 3.83 1.14 27.31 11.26 0.73 100.86 The fassaite appears to be pseudomorphous after gehlenite. 3. Pseudonaorphs of Grossulnr after Geh1enite.-On a specimen from the Monzoni mountains, pseudomorphs after gehlenitc were found. Ana1.y sis gave the following results :- Si02. Al,O,. Fe,O,. FeO. CaO. MgO. Ignition. Total. 39.64 16.47 4-62 1-13 31.52 5.72 1-04 100.14 This composition is nearly that of the grossular from Wilui. B. H. B. Bertrandite from Mount Antero, Colorado. By S. L. PENFIELD (Amer. J. Sci., 36, 52-55) .-The rare mineral, bertrandite, identified in France and Bohemia, has been found in little rectangular blades, 5 mm.long, 2 mm. wide, and 0.3 mm. thick, at Mouut Antero. The crystals are associated with quartz and beryl, and have a curious hemimorphic aspect, which the author refers to the rhombic system with an axial ratio of 0.5953 : 1 : 0.5723. The hardness of the crystals is 6 to 7, and their sp. gr. 8.598. An analysis of 0.1259 gram gitve the following results :- Si02. BeO. CaO. H,O. Total. 51.8 39.6 1.0 8.4 100-8 B . H. B. Mineralogical Notes. BJ- G. F. KUNZ (Amer. J. Sci., 36, 222- 224).-1. Phenacite from Maine.-In May, 1888, crystals of ptienacite were found near Stoneham in R vein of coarse albitic granite, asso- ciated with crystals of smoky quartz, topaz, and muscovite. The crystals were lenticular, 3 to 12 mm. across, and 1 to 3 uim.in thickness. 2. Quartz Pseudomorphs after Spodumene.-These pseudomorphs were found a t Peru, Maine, and, with the exception of a white core of albite, were entirely composed of white quartz. The surface of the crystals was covered with a coating of damourite. 3. A remarkable Variety of Transparent 0ligoclase.-Faint green crystals of oligoclase of wonderful tIansparency were found in the Hawk Mica Mine, near Bakersville, North Carolina. The crystals contain a series of cavities surrounded by acicular microlites. Analysis gave the following results :- Si02. AI2O3. CaO. K20. NeO. Ignition. Fe,O,,MnO. Total. 62.92 25.32 4.03 0.96 6.18 0.23 trace 99-66 4. Apatite from Yonkers, New Yo&.-A fragment of an apatite crystal, found in tunnelling for the Croton Aqueduct, measures 10 by 15 mm.It is of a rich, oily green, and remarkable for its trans- parency. 5. Cyanite from North Caro2ina.-The ci*ystals occur in a vein of white, massive quartz near the summit of Yellow Mountain, Bakers-MINERALOGICAL CHEXISTRY. 25 ville. Some of the crystals were 2 inches in length, and in perfec- tion, depth of colour, and transparency, rival those from S t. Gothard. 6. Arngoiaile Pseudomorph.-A crystal from Pima Co., Arizona, originally consisted of aragonite, but had been almost entirely changed and impregnated by ferric and manganese oxides. It had an outer coating of white cacholong. Artificial Formation of Mica. By C. DOELTER (Juhrb. f. Min., 1888, ii, Mem., 178--180).-1n May, 1888, the author announced to the Royal Academy of Sciences of Vienna, that he had successfully pro- duced mica artificially.From alumina-hornblende and augite he obtained biotite, and from pennine and glaucophane he obtained phlogopite, when these minerals were fused with magnesium fluoride and sodium fluoride at a red heat. In the same manner, biotite is obtained on fusing the silicate, K2A12Si208 + Mg,Si04, with sodium and magnesium fluorides. When ferrous silicate is substituted for the magnesium silicate, ferriferous biotites are obtained. Recently the author has obtained very excellent results by fusing garnet and anda- lusite with fluorides. Biotite, closely resembling that from Vesuvius, is obtained by fusing pyrope or almandine with sodium and mag- nesium fluorides. Very beautiful crystals of muscovite are obtained by fusing andalusite with potassium fluoride, silicon fluoride, and aluminium fluoride in the proportion of 4 : 3 : 1 at a low red heat.Curiously enough, the artificial mica usually exhibits a smaller axial angle than the natural. Zinnwaldite is obtained by fusing, at a dull red heat, andalusite with 4 parts of potassium fluoride, 3 of silicon fluoride, 2 of aluminium fluoride, and 1 of lithium carbonate. B. H. B. B. H. B. Chiastolite. By M. ROHRBACH (Chem. Centr., 1888, 942, from Zed. deut. geol. ges., 39, 632-638).-The author again points out that the characteristic cross-like division of the coal-black substance has no connection with a twin-formation, but uiost probably with a crys- talline “ growth ” which, according to the author’s view, has been brought about as follows :-The primarily-formed black, prismatic crystals have grown on the cnP faces more than on the edges, and, consequently, appear notched ; the black, slate-like particles cover- ing the crystals are pressed back from the faces, but on the edges they become enclosed by the substance of the crystals.Cordierite-gneiss from Connecticut. By E. 0. HOVEY (Amer, J. Sci., 36, 57-58).- Cordierite (or iolite), which has hitherto been found in America only as an accessory constituent in rocks, has been found at Guildford, near New Haven, with biotite, quartz, and some plagioclase constituting a true gneiss. This is the first time cordierite- gneiss is reported from America. J. W. L. B. H. B. Occurrence of Piemontite. By B. KOTO (Zeit. Kryst. Min., 14, 599-600, from J.CoZZ. Xci. Tokyo, 1, 303).-In a former paper, the author described the occurrence of piemontite (manganese-epidote) with glaucophane-bearing rocks of the archean-schist series. The dark- violet rocks are developed most typically in the vicinity of the town26 ABSTRACTS OF CHEMICAL PAPERS. of Tokusima, on the island of Shikoku. Here piemontite occurs in association with fine quartz grains, forming a stratified rock, in which sericite, garnet, rutile, orthoclase, and specular iron ore occur as accessory constituents. I n the glaucophane-schists, piemontite also occurs as an accessory constituent. An analysis of piemontite, isolated by means of Thoiilet's solution, from Otakisan in the province of Awa, gave the following results :- SiO,. 61203.Fe,O,. Mn20,. CaO. MgO. Na,O. H20. Total. 36.16 22.52 9.33 6.43 22.05 0.40 0.44 3.20 100.53 Piemon tite-schist is widely distributed throughout Japan. Like glaucophane-schist, it occurs in the lowest portion of the chlorite- sericite gneisses of the archaean formation. Origin of Primary Quartz in Basalt. By J. P. IDDINGS (Amer. J. Xci., 36, 208--222).-The basalts i n the vicinity of the Rio Grande Caiion, Tewan Mountains, New Mexico, contain porphyritic rounded grains of crackled quartz, surrounded by light green shells of micro- scopic augites. Similar remarkable occurrences of free silica in a basic magma are met with in the lithophysae of the rhyolitic obsidian from Obsidian Cliff, Yellowstone National Park, and from Cerro de las Navajas, Mexico. This anomalous association of primary igneous materials was most probably brought about by great pressure and aqueo-igneous action, induced by the influence of water-vapour absorbed in the molten glass.In order to show that the chemical composition of quartz-bearing basalts is not characteristic of a par- ticular modification of rock magma, the author gives the following analyses :- B. H. B. Si0, ....... T I O ~ ....... A1203 ...... Fe203.. ..... FeO ........ M n 0 . ..... CaO ........ MgO ....... BLLO. ....... K@ ....... N%O ...... LIZ0 ....... H20 ....... coz ........ P,Oj ....... c1. ......... Total ....... I. 52 '27 1.49 17-68 2'51 5'00 0 -23 8-39 6.05 0 -06 1.58 4-19 0 *82 - trace trace 100 -27 - j-- 11. 52.37 1.60 17 '01 1 '44 5 -89 0 '32 7 '59 6 *86 0 -06 1.59 3.51 1 -29 0 '37 - -- trace 99.90 -- 111.51 -57 1 '43 17 9 2 6 *24 1.78 0 -45 8 -82 4 *91 0'16 1 -99 3.59 0 -64 0 -58 -- - - -- 99 *88 IV. -- 52 '38 1.22 18 -79 2 -88 4 a90 0.18 7 -70 4 -91 0 *11 1 -76 3 -99 0.53 0 56 - - - -- 99.91 V. 57 -25 0 '60 16.45 1 -67 4 "72 0 '10 7-65 6 74 1-57 3 '00 0 -40 0 -20 - - - - -- 100.35 VI. -- 56 '28 0 *84 14 -23 4 -69 4 -05 0.16 7 *94 6 '37 1 -23 2 -98 0 - C l O * F 3 0 -40 O * l ? 100.28 - - --- B. H. B.MINERALOGICAL CHEMISTRY. 27 Peridotite of Iron Mine Hill, Cumberland, Rhode Island. By 51. E. WADSWORTH (Jnhrb. f. Min., 1888: ii, Ref., 224-225, from Bull. Mas. Comp. Zool. Earvard, 7 , 183).--The mean of a number of analyses of the iron ore, peridotite, from Iron Mine Hill, Cumberland, Rhode Island, was as follows :- SiO,. A1,03.Fe,O, + FeO. MnO. CaO. MgO. TiOp. 22-87 10.64 44.88 2-05 0-65 5.67 9-99 Zn. HzO. Total. 0.20 ( 3 0 5 ) 100*00 Under the microscope, the ore is seen to consist of magnetic pyrites, oliyine, plagioclase, and actinolite. B. H. B. The Badenweiler Ore Deposit. By A. WOLLEMANN (Zeit. Kryst. Min., 14, 624-628, from Verh. phys. naed. ges. Wurxbzwg, 20, 39).- The ore deposit of Badenweiler traverses a highly siliceous sandstone, and is enclosed on the one side by granite and porphyry and on the other by Keuper marl, in which rocks numerous branches of the deposit are met with, After giving a geological sketch of the vicinity of Badenweiler, the author gives the results of his petrographical and chemical investigations of the crystalline rocks of the district. The somewhat coarse-grained granite of the Forstgarkchen contains oligo- clase, orthoclase, and mica, analyses of which minerals are given.As further macroscopic constituents, quartz, hornblende, and orthite are met with, whilst magnetite, apatite, zircon, rutile, anatase, and epidote occur microscopically. The minerals found in the ore deposit include barytes (analysis given), quartz, fluorspar, brown-spar, zinc- blende, zinc silicate, galena: anglesite, linarite, cerussite, pyro- morphite (three analyses given), yellow lead ore, and copper pyrites. From the last-named mineral, copper glance and copper indigo are produced in indistinct pseudomorphs. Other products of decompoei- tion are chrysocolla, malachite, and limonite. The quartz appears to be younger than the barytes and fluorspar, after which it forms pseudomorphs The memoir concludes with a discussion of the genesis of the ore deposit by lateral secretion.Mineral Springs in the Admirals-gartenbad, Berlin. By R. FRESENIUS (J. pr. Chem. [el, 38,236-240$.-0n 24th January, 1888, the spring delivered 12.8 litres per minute ; the temperature of the water was 15*2", the air temperature being 5". The water was perfectly clear, but deposited oxide and phosphate of iron on exposure to air; its sp. gr. at 17.5" was 1.021016; no micro-organisms were developed in the bacteriological research. The detailed analysis is as follows, all the carbonates being calculated as normal carbonate :- B. H. B.28 ABSTRACTS OF CHEMICAL PAPERS. In 1000 partR by weight. Sodium chloride . . . .. . . . . . . . . . . Potassium chloride . . . . . . . . . , . . . Lithium chloride . . . . . . . . , . . . . . A mmoni urn c 11 loride. . . . . . . . . . . . Calcium chloride. . . . . . . . . . . , . . . Magnesium chloride . . . . . . . . . . . . Sodium bromide. . . . . . . . . . . . . . . . Sodium iodide , . . . . . . . . . . . . . . . . Calcium sulphate . . . . . . . . . . . . . . Stxoiitium sulphate . . . . . . . . . . . , Barium sulphate . . , . . . . . . . . . . . . Magnesium carbonate . . . . . . . . . . Ferrous carbonate. . . . . . . . . . . . . . Manganous carbonate. . . . . . . . . . . Aluminium phosphate . . . . . . . , . . Aluminium silicate ( A1,0,,3SiOz). Calcium borate . . . . . . . . . . . . . . . . Silica, . . . . . . . . . . . . . . . . . . . .. . . . 26.715139 0.139062 0.0021 97 0.0 1 885 5 0.52r ,697 0.6441 99 0.020943 0*000398 0.297493 0.637129 trace 0.245551 0-00809 7 0.000160 0.0001 0 7 0.0021 73 0.005 80 7 0-013925 28.672132 0.131754 0-014010 the normal carbonates, to form Carbonic anhydride combined with bicarbonates . . . . . . . . . . . . . . . . Free carbonic anhydride . . . . . . . . 1 - 28.817896 The author compares this water with other waters as to its contents of sodium, calcium, and magnesium chlorides, sodium bromide, and sodium iodide. A. G. B. Analysis of Roncegno-water. By M. GLASER and W. KALMAXN (Be?-., 21, 2879--2881).-The quantity of water flowing from this medicinal spring, which has its source in the Tesobo Mountain, varies during the year. The analysis of a sample taken at the time of greatest flow is given below ; one litre at 18" containing- H3As0,.FeS04. Fe2(S04),. Fe2(P04)*. hl2('SOJ3. MnS04. 0.1531 0.0072 3.0980 0.0285 1.5572 0.1684 C0S04. NiS04. ZnSOg. CuW4, CaS0,. MgS04. 0.0353 0.0862 13.0121 0.0306 1.9072 0.3657 Organic &SO4. Na2S04. NaC1. Si02. matter. 0.0400 0.3009 0.0043 0.1274 0.2280 Total solids, by direct estimation, 8.1440 gramw A comparison with the analysis previously given (Ahstr., 1888, 796) shows that the quantity of arsenic acid has decreased consider- ably (38.1 mgrm. per litre), whilst the other cmstituents are present i n almost the same quantities as before. F. S. K.ORGANIC CHEMISTRY. 29 0.24 1-95 35.53 0.21 - 10*05 0'24 16.23 35 '41 0'14 100 -00 - - Analyses of the Waters of some American Alkali Lakes.By T. M. CHATARD (Amer. J. Sci., 36, 14.6--150).-Tbe four analyses given repi-esent the most important alkali lakes so far known. For deteitmining the boric acid, Gooch's method (Abstr., 1887, 299) was found to be the most accurate. Of the four lakes, the most northern is Albert Lake (I), in south-east Oregon. The sample analysed mas taken in September, 1887, 1 foot below surface, and 35 feet from the shore ; sp. gr. 1.03117 et 19 8". IT. Big Soda Lake, near Ragtown, Churchill Co., Nevada; sample taken in 1881 a t the depth of 1 foot; sp. gr., 1.0995 a t 19%". III. Mono Lake, California, although of a composition favourable to ntilisation, is practically inaccessible on account of its great altitnde. The sample was taken in 1882 a t the depth of 1 foot ; sp.gr. 1.045 a t 15.5". IV. Owen's Lake, Inyo Co., California, is 17 miles long and 9 miles wide, its greatest depth being 51 feet. It is estimated to contain 22 million tons of sodium carbo- nate. The manufacture of soda a t this point has been commenced. The sample was taken in September, 1886 ; spa gr. 1.062 a t 25". The analytical results were as follows, a being the composition in grams per litre, and b that per cent. of solid constituents :- 0.070 0 961 19.685 0 -020 0-055 } 0 '003 6'672 0.160 13.690 12 *104 0.052 53 -472 -- -- SiOz.. .. .. K . . . . * . * . N a . . . . . . , Ca . . . . . . . Mg ...... Pe,O, . . . . A1203 . . 504 ...... BJ07 . . . . COB .. .. .. c1 H . . . . . . . Totals . . . . . , . . . . . 0.59 1.3'7 37-51 - - - - 1.80 - 24.21. 34-67 0.15 100 '30" Ia.0'304 2.520 45.840 0 -270 12.960 0 *314 20.934 45.690 0.181 129 -013 - - - ~- 0 -232 0 -538 14.690 - - - - 0.706 9.486 13.462 0 -058 - 1.644 28*5(30 0.014 {t':;: 7.505 0'36'7 19 '398 19'344 0.063 77.098 0.005 39 *172 - 2 13 36.96 0.02 - 0 -02 0.03 9-33 0.49 25 -16 25.09 0.10 100 -01 -- - IIIb. -- 0 *12 1 -79 36 -81 0'04 0 -10 0 '01 12 *48 0 '30 25 '61 22 *64 0 -10 100 -00 IVa. 1 IVb. B. H. B.20 ABSTRACTS OF CHEMICAL PAPERS.M i n e r a l o g i c a1 C h e m i s t r y ,Hexagonal Zinc Sulphide. By W. STAHL (Chem. Centr., 1888,943, from Berg. Hutt. Zpit., 47, 207--208).-The naturally occurringmineral, wurtzite, which has also been artificially prepared, has beennoticed by the author as a product of the blast furnace of the Sophiasnielting work in the Lower Harz.It forms clear, wine-yellow,shining, hexagcnal crystals, mostly in tufts, wit,h the faces mP2, €2,2P2, and OP. Cleavage in the direction R and WE. Hardness= 3-4, sp. gr. = 4.32 ; composition :BII?r'ERALOGICAL CHEMISTRY. 21Zn. Fe. Mn. Pb. 5.66.08 0.55 trace 0.31 32.88 = 99.82J. W. L.Arsenopyrite from Servia. By A. SCHMIDT (Zeit. Kryst. Mia.,14, 573-574) .--The specimen examined formed part of the collectionof the Royal Hungarian Geological Survey at Budapest. It is statedto have come from the Luta Strana adit-level, Servia. The arseno-pyrite occurs, with iron pyrites and zinc blende, in small_prismtrticcrystals, on which were observed the forms mP, OP, $ z P ~ , $Pw,the two last being new for this mineral. The axial ratio is computedt o be a : b : c = 0.686 : 1 : 1.170.Analysis of this arsenopyrite gavethe following results :-Fe. As. Sb. S. Zn. Insoluble. Total.34.58 42.38 0.14 21-71 0.46 0.22 99-49The percentage of zinc is evidently due to an unavoidable admixtureof blende. B. H. B.Formation of Deposits of Oxides of Manganese. Ry F. P.DUNNINGTON (Amer. J. Sci., 36, 175--178).-1n view of the results ofa series of 15 experiments, i t appears possible that many deposits ofmanganese ore in calciferous rocks have been formed by the action ofsolutions of sulphates rather than of bicarbonates. An illustration ofsuch action is perhaps afforded by the maugnnese deposits of Crimora,Augusta Go., Virginia. Wherever pyrites has been deposited, theoutcrop is gradually converted into limonite by weathering, and theacid solution of ferrous sulphate which sinks into the underlyingdeposits, must carry with it all the manganese in the pyrites itself,and in any disintegrating silicates.As this solution is exposed t o theair or meets with calcium carbonate, ferrous carbonate will be formed,whilst the manganese sulphate will aernain in solution until exposedto the action of both air and calcium carbonate at the same time.B. H. B.Artificial Production of Hydrocerusite. The Compositionof this Mineral and the Constitution of White Lead. ByL. BOURGEOIS (Bull. SOC. Chi/n., 5 0, 83-85) .-Hydrocerusite,2PbC03, Pb(OH)z, is formed if a boiling solution of lead acetate (1 mol.)is treated with litharge (l$ mol.), and when cold, with carbamide(1 mol.).The liquid is then filtered and heated at about 130" forsome hours, when a quantity of nacreous spangIes separate which arewashed with water. These have a sp. gr. = 6.14 at 15", dissolve witheffervescence in nitric and acetic acids, and give off water and carbonicanhydride at 400", leaving a residue of massicot slightly coloured by a,trace of minium.White lead consists of a mixture of hydrocerusite and cerusite.N. H. M.Preparation of Pyromorphite and Mimetesite. By L. MICHEL(Zeit. Kryst. Min., 14, 619, from Bull. SOC. franp. win., 10, 133).-The author mixes three equivalents of lead phosphate or arsenate, or amixture of the two, with one equivaIent of lead chloride in a porcelaincrucible. He covers the mixture with a thin layer of lead chloride22 ABSTRACTS OF CHEMICAL PAPERS.and places the crucible in one of fireclay.Both are hermeticallysealed, the intei*mediate space being filled with ignited magnesia.The crucibles are then heated to the melting point of gold, and slowlycooled. The cavities of the fused mass contain hexagonal prisms asmuch as 2 cm. in length and 1 mm. in width. The best results wereobtained with the mixture coryesponding with kampylite (Analysis 4),the prisms being well developed and perfectly transparent. Thecrystalline productis obtained had the following compositions :-I ..............2 ..............3 ..............4 ..............5 ..............6 ..............7 ..............8 ..............9 ..............Pb,As,O,.89 -7584 '7379'8569.7846.0529 '3719.4310 *21-~--Pb$?,O,.---4 -9'710- 0620 -0.244 -8759 *2468 +98'79 -6789 *87PbC12.--9-9210 * 038.9810.079 9 910 -3110.129 *7110 * 14Total.--99 -6799 -7398 -8999 '8'7l00*7198 -92"98 *5399 -59100 -01Sp.gr.7 -126 -936.976 -93---- -----On the addition of a small quaiitity of lead chromate, yellow orIn rare cases, they are of a grass-green orange crystals are obtained.colour. B. H. B.Uranite from Madagascar. By E. JANNETTAZ (Zed. Rryst. Min.,14, 608, from Bull. SOG. frung. milt., 10, 47).-The mineral examinedforms greenish-yellow aggregates of crystals exactly similar in ap-pearance to those of Autun.H,O. P20,.UO,. Fe,O,. CaO. Total.22.08 14-93 55-08 1-33 651 99-96Analysis gave the following results :-These results correspond with the formula (UO,,Fe,Ca),P,O, +12H,O. Of the proportion of water, 9 per cent. is evolved at 65".B. H. B.Baryto-celestine from Werfen in Salzburg. By E. HATLE andH. TAUSS (Jahrb. f. Min., 1888, ii, Ref., 210, from Tschermak's min.Mitth., 9,227-231) .-The baryto-celestine accompanying the wagner-ite of Werfen has hitherto been regarded as barytes. It formsdruses, crystals 1.5 cm. thick, and radiated or granular masses. It isof a pink coloui-, and translucent, with a hardness of 3.5 and asp. gr. of 4-17. Analysis gave 84.80 per cent. of barium sulphateand 15.03 of strontium sulphate.Arseniopleite, a New Swedish Mineral.By L. J. IGELSTROM(Jahrb. f. &fin., 1888, ii, Mem., 117- 122).--Numerons rare and newminerals occur with braunite and hausmannite at the manganesemine, Sjtigrufvan, in the parish of Gryhyttan, Oerebro, Sweden. InNovember, 1887, the author discovered there another new mineral,# 99 *51 in the original paper.The formula is 4BaS04 + SrSO1.B. H. BMXNERALOQTCAL CHEMISTRY. 23which he names arsenioyZeite from the metal arsenic, and slrX&ov(more). The mineral occurs in intimate association with rhodonitein small veins in dolomite. It also occurs in the same rock inmasses 0.5 to 1 cm. in thickness. NOcrystals have been found. It is uniaxial and positive, and judgingfrom the cleavage appears to crystallise in rhombohedra1 forms.Analysis gave the following results :-Its colour is cherry-red.A S , ~ , .MnO. Fe,O,. PbO. CaO. MgO. H20. Total.44.98 28.25 3.68 4.48 8.11 3.10 5.67 98.27Traces of Sb205 and C1 were observed. Arseniopleite is a basicarsenate, like olivenite. It resembles most closely dindelphite andsynadelphite. It, however, contains no alumina. Its relation to theother hydrated arsenates occurring in Sweden may be seen from thefollowing list :-Chondroarsenite.. . . (MnO)~SzO5 + 24Hz0.Xanthoarsenite . . . . (MnO)5As205 + 5H20 (Abstr., 1886, 25).HEmafjbrite . . . . . . (MnO),AsZO5 + 5H20.Polyarsenite . . . . . . (MnO)4Asz05 + HzO (Abstr., 1887, 347).Allactite . . . . . . . . . . (Mn0),As205 + 4H20.Diadelphite.. . . . . . . (MnO),As205 + AlZO3(Fe2O3) + 8H20.Synndelphite .. . . . . (MnO),As,O, + Al2O3(Fe2O,) + 5Hz0.Arseniopleite . . . . . . 3(Mn0,Ca0,Pb0,MgO)3As205 +(Compare Abstr., 1867, 902.)Treatment of Natural Silicates with Hydrochloric Acid as ameans of Ascertaining their Structure. By E. A. SCENEIDER(Anwr. Chem. J., 10, 405--408).-Referring to the recent paper byClarke (Abstr., 1888,659), the author remarks that the weathering ofminerals may be used for drawing conclusions as to their constitution,and suggests the carrying out of a number of experiments, substi-tuting hydrochloric acid for the atmospheric carbonic anhydride, andaccelerating its action by heating in sealed tubes in a water-bath, themineral being finely powdered.Minerals of the Tyrol. By A.CATHRRTN (Jahrb. f. Min., 1888, ii,Ref., 2%0-221, from Tschernznk’s min. Mitth., 8,400-413).-1. Theso-called Paragonite frona the Zillerthn1.-The composition of thismineral is found to be that of talc, and not that of mica. It is EMf0llOvr~S :-Mn,03(B’e203) + 3H20.B. H. B.H. B.SiO,. MgO. FeO. H,O. Total.62-24 30.22 2.66 4.97 100.09This talc is the matrix of the actinolite from this locality.2. A New Pseudnmorph of Fasstcite.-This was found at Monzoni iuassociation with crystals of grossular remarkable for the occurrenceof the rare plane 40+, first observed by Bauer on garnet fromOravicza. The composition of the fassaite is as follows :24 ABSTRAUTS OF CHEMICAL PAPERS.Loss onSi02. A120,. Fe20B. FeO. CaO. MgO. ignition. Total.44.22 12.37 3.83 1.14 27.31 11.26 0.73 100.86The fassaite appears to be pseudomorphous after gehlenite.3.Pseudonaorphs of Grossulnr after Geh1enite.-On a specimen fromthe Monzoni mountains, pseudomorphs after gehlenitc were found.Ana1.y sis gave the following results :-Si02. Al,O,. Fe,O,. FeO. CaO. MgO. Ignition. Total.39.64 16.47 4-62 1-13 31.52 5.72 1-04 100.14This composition is nearly that of the grossular from Wilui.B. H. B.Bertrandite from Mount Antero, Colorado. By S. L. PENFIELD(Amer. J. Sci., 36, 52-55) .-The rare mineral, bertrandite, identifiedin France and Bohemia, has been found in little rectangular blades,5 mm. long, 2 mm. wide, and 0.3 mm. thick, at Mouut Antero. Thecrystals are associated with quartz and beryl, and have a curioushemimorphic aspect, which the author refers to the rhombic systemwith an axial ratio of 0.5953 : 1 : 0.5723.The hardness of thecrystals is 6 to 7, and their sp. gr. 8.598. An analysis of 0.1259 gramgitve the following results :-Si02. BeO. CaO. H,O. Total.51.8 39.6 1.0 8.4 100-8B . H. B.Mineralogical Notes. BJ- G. F. KUNZ (Amer. J. Sci., 36, 222-224).-1. Phenacite from Maine.-In May, 1888, crystals of ptienacitewere found near Stoneham in R vein of coarse albitic granite, asso-ciated with crystals of smoky quartz, topaz, and muscovite. Thecrystals were lenticular, 3 to 12 mm. across, and 1 to 3 uim. inthickness.2. Quartz Pseudomorphs after Spodumene.-These pseudomorphswere found a t Peru, Maine, and, with the exception of a white core ofalbite, were entirely composed of white quartz. The surface of thecrystals was covered with a coating of damourite.3.A remarkable Variety of Transparent 0ligoclase.-Faint greencrystals of oligoclase of wonderful tIansparency were found in theHawk Mica Mine, near Bakersville, North Carolina. The crystalscontain a series of cavities surrounded by acicular microlites.Analysis gave the following results :-Si02. AI2O3. CaO. K20. NeO. Ignition. Fe,O,,MnO. Total.62.92 25.32 4.03 0.96 6.18 0.23 trace 99-664. Apatite from Yonkers, New Yo&.-A fragment of an apatitecrystal, found in tunnelling for the Croton Aqueduct, measures 10 by15 mm. It is of a rich, oily green, and remarkable for its trans-parency.5. Cyanite from North Caro2ina.-The ci*ystals occur in a vein ofwhite, massive quartz near the summit of Yellow Mountain, BakersMINERALOGICAL CHEXISTRY.25ville. Some of the crystals were 2 inches in length, and in perfec-tion, depth of colour, and transparency, rival those from S t. Gothard.6. Arngoiaile Pseudomorph.-A crystal from Pima Co., Arizona,originally consisted of aragonite, but had been almost entirelychanged and impregnated by ferric and manganese oxides. It hadan outer coating of white cacholong.Artificial Formation of Mica. By C. DOELTER (Juhrb. f. Min.,1888, ii, Mem., 178--180).-1n May, 1888, the author announced to theRoyal Academy of Sciences of Vienna, that he had successfully pro-duced mica artificially. From alumina-hornblende and augite heobtained biotite, and from pennine and glaucophane he obtainedphlogopite, when these minerals were fused with magnesium fluorideand sodium fluoride at a red heat.In the same manner, biotite isobtained on fusing the silicate, K2A12Si208 + Mg,Si04, with sodiumand magnesium fluorides. When ferrous silicate is substituted for themagnesium silicate, ferriferous biotites are obtained. Recently theauthor has obtained very excellent results by fusing garnet and anda-lusite with fluorides. Biotite, closely resembling that from Vesuvius,is obtained by fusing pyrope or almandine with sodium and mag-nesium fluorides. Very beautiful crystals of muscovite are obtainedby fusing andalusite with potassium fluoride, silicon fluoride, andaluminium fluoride in the proportion of 4 : 3 : 1 at a low red heat.Curiously enough, the artificial mica usually exhibits a smaller axialangle than the natural.Zinnwaldite is obtained by fusing, at a dullred heat, andalusite with 4 parts of potassium fluoride, 3 of siliconfluoride, 2 of aluminium fluoride, and 1 of lithium carbonate.B. H. B.B. H. B.Chiastolite. By M. ROHRBACH (Chem. Centr., 1888, 942, fromZed. deut. geol. ges., 39, 632-638).-The author again points out thatthe characteristic cross-like division of the coal-black substance hasno connection with a twin-formation, but uiost probably with a crys-talline “ growth ” which, according to the author’s view, has beenbrought about as follows :-The primarily-formed black, prismaticcrystals have grown on the cnP faces more than on the edges, and,consequently, appear notched ; the black, slate-like particles cover-ing the crystals are pressed back from the faces, but on the edgesthey become enclosed by the substance of the crystals.Cordierite-gneiss from Connecticut.By E. 0. HOVEY (Amer,J. Sci., 36, 57-58).- Cordierite (or iolite), which has hitherto beenfound in America only as an accessory constituent in rocks, has beenfound at Guildford, near New Haven, with biotite, quartz, and someplagioclase constituting a true gneiss. This is the first time cordierite-gneiss is reported from America.J. W. L.B. H. B.Occurrence of Piemontite. By B. KOTO (Zeit. Kryst. Min., 14,599-600, from J. CoZZ. Xci. Tokyo, 1, 303).-In a former paper, theauthor described the occurrence of piemontite (manganese-epidote)with glaucophane-bearing rocks of the archean-schist series.The dark-violet rocks are developed most typically in the vicinity of the tow26 ABSTRACTS OF CHEMICAL PAPERS.of Tokusima, on the island of Shikoku. Here piemontite occurs inassociation with fine quartz grains, forming a stratified rock, in whichsericite, garnet, rutile, orthoclase, and specular iron ore occur asaccessory constituents. I n the glaucophane-schists, piemontite alsooccurs as an accessory constituent. An analysis of piemontite, isolatedby means of Thoiilet's solution, from Otakisan in the province ofAwa, gave the following results :-SiO,. 61203. Fe,O,. Mn20,. CaO. MgO. Na,O. H20. Total.36.16 22.52 9.33 6.43 22.05 0.40 0.44 3.20 100.53Piemon tite-schist is widely distributed throughout Japan.Likeglaucophane-schist, it occurs in the lowest portion of the chlorite-sericite gneisses of the archaean formation.Origin of Primary Quartz in Basalt. By J. P. IDDINGS (Amer.J. Xci., 36, 208--222).-The basalts i n the vicinity of the Rio GrandeCaiion, Tewan Mountains, New Mexico, contain porphyritic roundedgrains of crackled quartz, surrounded by light green shells of micro-scopic augites. Similar remarkable occurrences of free silica ina basic magma are met with in the lithophysae of the rhyoliticobsidian from Obsidian Cliff, Yellowstone National Park, and fromCerro de las Navajas, Mexico. This anomalous association of primaryigneous materials was most probably brought about by great pressureand aqueo-igneous action, induced by the influence of water-vapourabsorbed in the molten glass.In order to show that the chemicalcomposition of quartz-bearing basalts is not characteristic of a par-ticular modification of rock magma, the author gives the followinganalyses :-B. H. B.Si0, .......T I O ~ .......A1203 ......Fe203.. .....FeO ........M n 0 . .....CaO ........MgO .......BLLO. .......K@ .......N%O ......LIZ0 .......H20 ....... coz ........P,Oj ....... c1. .........Total .......I.52 '271.4917-682'515'000 -238-396.050 -061.584-190 *82-tracetrace100 -27-j--11.52.371.6017 '011 '445 -890 '327 '596 *860 -061.593.511 -290 '37---trace99.90--111.51 -571 '4317 9 26 *241.780 -458 -824 *910'161 -993.590 -640 -58---- --99 *88IV.--52 '381.2218 -792 -884 a900.187 -704 -910 *111 -763 -990.530 56--- --99.91V.57 -250 '6016.451 -674 "720 '107-656 741-573 '000 -400 -20------100.35VI. --56 '280 *8414 -234 -694 -050.167 *946 '371 -232 -980 - C lO * F 30 -40O * l ?100.28-----B. H.BMINERALOGICAL CHEMISTRY. 27Peridotite of Iron Mine Hill, Cumberland, Rhode Island.By 51. E. WADSWORTH (Jnhrb. f. Min., 1888: ii, Ref., 224-225, fromBull. Mas. Comp. Zool. Earvard, 7 , 183).--The mean of a number ofanalyses of the iron ore, peridotite, from Iron Mine Hill, Cumberland,Rhode Island, was as follows :-SiO,.A1,03. Fe,O, + FeO. MnO. CaO. MgO. TiOp.22-87 10.64 44.88 2-05 0-65 5.67 9-99Zn. HzO. Total.0.20 ( 3 0 5 ) 100*00Under the microscope, the ore is seen to consist of magnetic pyrites,oliyine, plagioclase, and actinolite. B. H. B.The Badenweiler Ore Deposit. By A. WOLLEMANN (Zeit. Kryst.Min., 14, 624-628, from Verh. phys. naed. ges. Wurxbzwg, 20, 39).-The ore deposit of Badenweiler traverses a highly siliceous sandstone,and is enclosed on the one side by granite and porphyry and on theother by Keuper marl, in which rocks numerous branches of thedeposit are met with, After giving a geological sketch of the vicinityof Badenweiler, the author gives the results of his petrographical andchemical investigations of the crystalline rocks of the district.Thesomewhat coarse-grained granite of the Forstgarkchen contains oligo-clase, orthoclase, and mica, analyses of which minerals are given. Asfurther macroscopic constituents, quartz, hornblende, and orthite aremet with, whilst magnetite, apatite, zircon, rutile, anatase, andepidote occur microscopically. The minerals found in the ore depositinclude barytes (analysis given), quartz, fluorspar, brown-spar, zinc-blende, zinc silicate, galena: anglesite, linarite, cerussite, pyro-morphite (three analyses given), yellow lead ore, and copper pyrites.From the last-named mineral, copper glance and copper indigo areproduced in indistinct pseudomorphs. Other products of decompoei-tion are chrysocolla, malachite, and limonite. The quartz appears tobe younger than the barytes and fluorspar, after which it formspseudomorphs The memoir concludes with a discussion of thegenesis of the ore deposit by lateral secretion.Mineral Springs in the Admirals-gartenbad, Berlin.By R.FRESENIUS (J. pr. Chem. [el, 38,236-240$.-0n 24th January, 1888,the spring delivered 12.8 litres per minute ; the temperature of thewater was 15*2", the air temperature being 5". The water wasperfectly clear, but deposited oxide and phosphate of iron on exposureto air; its sp. gr. at 17.5" was 1.021016; no micro-organisms weredeveloped in the bacteriological research. The detailed analysis is asfollows, all the carbonates being calculated as normal carbonate :-B.H. B28 ABSTRACTS OF CHEMICAL PAPERS.In 1000 partR by weight.Sodium chloride . . . . . . . . . . . . . . .Potassium chloride . . . . . . . . . , . . .Lithium chloride . . . . . . . . , . . . . .A mmoni urn c 11 loride. . . . . . . . . . . .Calcium chloride. . . . . . . . . . . , . . .Magnesium chloride . . . . . . . . . . . .Sodium bromide. . . . . . . . . . . . . . . .Sodium iodide , . . . . . . . . . . . . . . . .Calcium sulphate . . . . . . . . . . . . . .Stxoiitium sulphate . . . . . . . . . . . ,Barium sulphate . . , . . . . . . . . . . . .Magnesium carbonate . . . . . . . . . .Ferrous carbonate. . . . . . . . . . . . . .Manganous carbonate. . . . . . . . . . .Aluminium phosphate . . . . . . . , . .Aluminium silicate ( A1,0,,3SiOz).Calcium borate .. . . . . . . . . . . . . . .Silica, . . . . . . . . . . . . . . . . . . . . . . . .26.7151390.1390620.0021 970.0 1 885 50.52r ,6970.6441 990.0209430*0003980.2974930.637129trace0.2455510-00809 70.0001600.0001 0 70.0021 730.005 80 70-01392528.6721320.1317540-014010the normal carbonates, to formCarbonic anhydride combined withbicarbonates . . . . . . . . . . . . . . . .Free carbonic anhydride . . . . . . . . 1-28.817896The author compares this water with other waters as to its contentsof sodium, calcium, and magnesium chlorides, sodium bromide, andsodium iodide. A. G. B.Analysis of Roncegno-water. By M. GLASER and W. KALMAXN(Be?-., 21, 2879--2881).-The quantity of water flowing from thismedicinal spring, which has its source in the Tesobo Mountain, variesduring the year.The analysis of a sample taken at the time ofgreatest flow is given below ; one litre at 18" containing-H3As0,. FeS04. Fe2(S04),. Fe2(P04)*. hl2('SOJ3. MnS04.0.1531 0.0072 3.0980 0.0285 1.5572 0.1684C0S04. NiS04. ZnSOg. CuW4, CaS0,. MgS04.0.0353 0.0862 13.0121 0.0306 1.9072 0.3657Organic&SO4. Na2S04. NaC1. Si02. matter.0.0400 0.3009 0.0043 0.1274 0.2280Total solids, by direct estimation, 8.1440 gramwA comparison with the analysis previously given (Ahstr., 1888,796) shows that the quantity of arsenic acid has decreased consider-ably (38.1 mgrm. per litre), whilst the other cmstituents are presenti n almost the same quantities as before. F. S. KORGANIC CHEMISTRY. 290.241-9535.530.21-10*050'2416.2335 '410'14100 -00--Analyses of the Waters of some American Alkali Lakes. ByT. M. CHATARD (Amer. J. Sci., 36, 14.6--150).-Tbe four analysesgiven repi-esent the most important alkali lakes so far known. Fordeteitmining the boric acid, Gooch's method (Abstr., 1887, 299) wasfound to be the most accurate. Of the four lakes, the most northernis Albert Lake (I), in south-east Oregon. The sample analysed mastaken in September, 1887, 1 foot below surface, and 35 feet from theshore ; sp. gr. 1.03117 et 19 8". IT. Big Soda Lake, near Ragtown,Churchill Co., Nevada; sample taken in 1881 a t the depth of 1 foot;sp. gr., 1.0995 a t 19%". III. Mono Lake, California, although of acomposition favourable to ntilisation, is practically inaccessible onaccount of its great altitnde. The sample was taken in 1882 a t thedepth of 1 foot ; sp. gr. 1.045 a t 15.5". IV. Owen's Lake, Inyo Co.,California, is 17 miles long and 9 miles wide, its greatest depth being51 feet. It is estimated to contain 22 million tons of sodium carbo-nate. The manufacture of soda a t this point has been commenced.The sample was taken in September, 1886 ; spa gr. 1.062 a t 25".The analytical results were as follows, a being the composition ingrams per litre, and b that per cent. of solid constituents :-0.0700 96119.6850 -0200-055 } 0 '0036'6720.16013.69012 *1040.05253 -472----SiOz.. .. ..K . . . . * . * .N a . . . . . . ,Ca . . . . . . .Mg ......Pe,O, . . . .A1203 . .504 ......BJ07 . . . .COB .. .. .. c1H . . . . . . .Totals . . . .. , . . . . .0.591.3'737-51----1.80 -24.21.34-670.15100 '30"Ia.0'3042.52045.8400 -27012.9600 *31420.93445.6900.181129 -013---~-0 -2320 -53814.690 ----0.7069.48613.4620 -058-1.64428*5(300.014{t':;:7.5050'36'719 '39819'3440.06377.0980.00539 *172 -2 1336.960.02 -0 -020.039-330.4925 -1625.090.10100 -01---IIIb.--0 *121 -7936 -810'040 -100 '0112 *480 '3025 '6122 *640 -10100 -00IVa. 1 IVb.B. H. B

ISSN:0368-1769    

DOI:10.1039/CA8895600020

出版商:RSC    

年代:1889

数据来源: RSC

摘要:

ORGANIC CHEMISTRY. 29 Organic C h e m i s t r y . Isoallylene. By G. GUSTAVSON and N. DEMJANOFF (J. p r . Chem. [Z], 38, 201--207).-1soallylene may be prepared by the action of zinc-dust on an alcoholic solution of dibromopropylene. The latter, best obtained by the action of potassium hydroxide on tribromhydrin, is allowed to drop slowly into the warm mixture of zinc-dust and $0 per cent. alcohol, contained in a flask. The isoallylene evolved is * 100 00 in the original paper.80 ABSTRACTS OF CHEMICAL PAPERS. collected over water, in wliich it is very little soluble. 10 grams of dibromopropylene yield 900 to 1000 C.C. of the gas, IsozLZZyZene is ;I colourless gas, smelling like normal allylene; it burns with a skrongly luminous flame, and gives 110 precipitate with ammoniacal cuprous chloride or silver nitrate.With aqueous solu- tions of mercuric chloride or sulphate it gives a white precipitate. The gas from 10 grams of dibromopropylene was absorbed by 35 grams of bromine, the unaltered bromine dissolved in sodium hydroxide solution, and the colourless oil washed with water. It weighed 17 grams, the calculated yield being 18 grams, and had the formula C3H4Br4. IsoaZZyZene tetrabromide smells of camphor, and has the sp. gr. 2.729 at 0" and 2.658 a t 18" (water a t 0" = 1) ; it solidifies when cooled to -18", and melts below 0" ; a t the ordinary pressure it distils between 215" and 230" with partial decomposition. Normal allylene tetrabromide has the sp. gr. 2.690 a t 0" and 2.652 at It;", and does not solidify in a freezing mixture. That the two are not identical is conclusively proved by the fact that by the action of zioc- dust isoallylene is liberated from the one, and normal allylene from the other.On heating sodium with an ethereal solution of isoallylene in a sealed tube st loo", the sodium is converted into a white powder, which evolves normal allylene when treated with water. Pavorsky has shown that this conversion of iso- into normal hydro-carbons by the action of sodium, is characteristic of the homologues of acetylene. When passed into strong sulphuric acid, isoallylene is absorbed, and on dilution with water and addition of potassium hydroxide, acetone separates ; this is a strong argurnent in favour of isoallylene being dirnethyZenemethane, CH2:C:CH2, thus (1) CH2:C:CH2 + 2H2S04 + 2H2SOa.If this is the case, the dibromopropylene from which isoallylene is obtained must be CH2Br*CBr:CH2, and isoallylene tetrabromide must be CH2Br.CBr2*CH2Br. = CH,*C(HS0,)2*CH3; (2) CH,*C(HSO,)2*CH3 + H2O = CH,.CC)*CH, A. G. B. Cyanurates. By A. CLAUS and 0. PUTENSEN (J. pr. Chem. [2], 38, 20&-229).-The amethyst-coloured crystals, obtained when cyanuric acid is mixed with ammoniacal copper sulphate, have the composition ( C3N303H2),Cu,2NH3. By digesting them with dilute ammonia, violet needles of the composition ( C3N30,H2)2Cu,3NH3 are obtained, and if strong ammonia is used a deep blue compound, (C3N303H2)2C~,4NH3, is formed ; but this last is very unstable, rapidly losing ammonia in the ail.. When the first of these ammoniacal copper cyanurates is digested with water, a basic copper cyanurate, C,N,O,(Cu*OH), + 3H20, is formed.An acid copper cyanurate of the composition ( C3Nd03HL)2C~,C3N303H3,NH3 + H20 is formed when copper carbonate is digested with cpanuric acid and ammonia. The salt, C3N303HCu + 3H20, is precipitated when sodium cyanurate is added to copper sulphate ; and normal copper cyanurate, (C,N,O,),Cu, + H,O, crystallises when acid magnesium cyanurate is mixed with copper sulphate. The following cyanurates are also described : Acid magnesium cyanurate, ammoniacal cadmium cyanurate, ammoniacal zinc cyanurate, ammoniacal nickel cyanurate, cyanurates of nickel,ORGANIC OHEMISTHY. 31 cobalt, and manganese : tetramethylammonium cyanurate, and furhher, cyanurates of quinoline, quinine, cinchonine, strychnine, narc0 tine, and caff ehe.A. G. B. Preparation of a-Dibromhydrin. By 0. ASCHAN (Ber., 21, 2890-2892) .-a-Dibromhydrin is best prepared as follows :-Phos- phorus tribromide (650 grams) is dropped in quantities of from 10 to 20 grams at a bime into pure, warm glycerol (500 grams), the whole being well shaken and cooled after each addition of bromide, The operation is at an end in from three to four hours. After keeping for 24 hours, the mixture is heated on the water-bath for about three hours, cooled, diluted with water (3 to 4 vols.), extracted with ether, and the extract washed with sodium carbonate solution and dried. After evaporating the ether, the residual oil is heated at about 200°, and then fractionated ; the portion boiling at 208-218", which con- stitutes about two-thirds of the whole, is finally distilled under reduced pressure.500 gra'ms of glycerol yield 135 grams of pure a-dibromhydrin. The requisite quantities of yellow phosphorus and bromine can be employed instead of phosphorus tribromide. When a-dibromhydrin is treated with nitric acid of sp. gr. 1.48, the principal product is a liquid boiling at 78-79' (18 mm.), which con- tains bromine and nitrogen. It forms very stable, yellow, readily crystallisable salts. F. S. K, Epichlorhydrin. By C. PAAL (Ber., 21, 2971-2973) .-Chloriodo- hydrin methyl ether, C3H5CII*OMe, is obtained by heating epichlor- hydrin (1 mol.) with methyl iodide (1 mol.) at 190°, fractionating the product, and removing the free iodine wit,h finely divided si!ver.The yield is about 'LO per ceilt. of the theoretical quantity. I t is a colourless oil with a pungent smell, exceedingly sensitive to light, and miscible with the ordinary solrents excepting water, in which it is insoluble. I t boils at about 200" with partial decomposition, and is readily volatile with steam. Chloriodohydrin etlyl ether, C,H,CiI-@Et, is prepared by heating epichlorhydrin with ethyl iodide at 200-220", and purifying the product as described above. The yield is 30-50 per cent. of the theoretical quantity . It boils at 200-210" with slight decomposition and resembles the preceding compound. Chloriodohydrin isopropyl ether, C,H,ClI*OPrF, prepared in like manner, boils at 208-212" with partial decomposition and resembles the ethyl ether. The noymai propyZ ether boils at 200-210" with slight decomposition ; it is relatively stable and less sensitive t o light than the other ethers which, however, it resembles in other respects.F. 8. I(. Propyl-phycite. By A. 'FAUCONNIER (Compt. rend., 107,629-630). -The action of hypochlorous acid on epichlorhydrin results in the rtssimilation of water, most probably because of the acidity of the liquid, and the " propyl-phycite " obtained by Carius by saponifying the product of this reaction, and described by him as a lower homo- logue of erythrol, is in reality ordinary glycerol. C. H. B.32 ABSTRACTS OF CHEMICAL PAPERS. Molecular Weight and Valency of Perseite. By MAQTJENNE (Compt. rend., 107, 583-586) .-When perseite is treated with boil- ing hydriodic acid, it is partly converted into resinous products of indefinite composition, and partly into a volatile liquid which can be separated into two fractions boiling at 100-110" and 133-200" respectively.The first is a heptine, isomeric with oenanthylidene, which boils a t 102-105" after rectification over calcium oxide and over sodium ; sp. gr. at 20" = 0.78. The second fraction is a dense red oil with a slight ethereal odour. It boils at 192-196" under ordinary pressure, and at 02-35" under a pressure of 40-50 mm., but decom- poses to a considerable extent even when distilled in a vacuum. It consists mainly of heptyl iodide with a small quantity of heptine hydriodide. The dibenzok acefal of perseite, C,,H2,O7, is obtained by the action of benzaldehyde on perseite in presence of alcohol saturated with hydrogen chloride.It forms confused, slender, microscopic needles which soften at 215", but have no definite melting point, and are quite insoluble in water and almost insoluble in alcohol. ThePe results show that the formula previously attributed to per- seite (Abstr., 1888, 807) is incorrect, and that perseite is really the next higher homologue of mannitol, and has the formula C,H,,O,. It is the first instance of a heptahydric alcohol and of a sugar containing 7 carbon-atoms. C. H. B. Constitution of the Glucoses. By B. RA~MANN (Bey., 21, 2841- 2842).-The author considers that the aldehyde and ketone formulze explain the chief reactions of the glucoses, and that the reactions which Tollens mentions (KzLrzes Eandb. d. Kohlenhydrate), as incom- patible with the assumption that these compounds are aldehydes do not afford sufficient grounds for changing the formuls.N. H. If. Oxidation of Arabinose with Nitric Acid. By H. KILIANI (Ber., 21, 3006-3009) .--Calcium arabonat'e is obtained in consider- able.quantities when arabinose (1 part) is heated at 35" for about six hours with nitric acid of sp. gr. 1.2 (2 parts), the diluted solution boiled with excess of calcinm carbonate, filtered, enporated, and mixed with alcohol. This method can be suitably employed for the preparation of arabonic acid. Calcium trihydroxyglutarate is obtained from arabinose as follows :- Arabinose (1 part) is digested at 35" with nitric acid of sp. gr. 2.2 (2.5 parts) ; after the evolution of gas has ceased, the solution is evaporated until free from nitric acid, the residual syrup dissolved in water (25 parts), boiled with calcium carbonate, and the hot solu- tion filtered. The sparingly soluble, red calcium salt which separates is spread on porous plates, and by concentrating the mother-liquor, separating the salt, and repeating the process several times, 40-45 per cent.of the weight of the arabinose employed is obtained in the form of calcium trihydroxyglutarate. It is very similar to calcium sacchnrate in appearance and in its behaviour when heated with water. The potassium salt, C5H607K2, crystallises in large, colourless, monoclinic plates or prisms, is readily soloble, and is not convertedORGANIC CHEMISTRY. 33 into the acid salt when the aqueous soIuttion is evaporated with acetic acid.Lead acetate and silver nitrate produce white precipitates in an aqueous solution. TrihydrozyLglutzLric acid, C5H807, obtained by decomposing the calcium salt with oxalic asid, crystallises from alcohol in colourless, microscopic plates, melts a t 127", and does not reduce Fehling's solu- tion. The normal ammonium salt crystallises in slender needles and is very readily soluble. By F. MBYER (Ber., 21, 2883-2t390).-~rLnzeth~Zenetrinitrosamine, C3H6N6O3, is obtained when an ice-cold solution of hexamethyleneamine (1 part) in water (40 parts) is mixed with ice-cold, dilut,e (If per cent.) hydrochloric acid, and a solution of sodium nitrite ( 2 i parts) in a small quantity of water immediately added. After about, 15 minutes, the yellowish, crystalline substance which separates at the surface is tlirown on to a filter, washed with cold water, and dried on porous plates.The yield is 50 to 60 per cent., or more, of the aniine employed. It crystal!ises from boiling alcohol, in which it is moderately soluble, in small, yellowish, silky needles or prisms, melts at 105--106", and is readily soluble in cold acetone, but only moderately so in warm benzene, chloroform, and ether, and insoluble in light petroleum. It dissolves unchanged in cold glacial acetic acid, and the molecular weight determined by Raoult's method was found t o be 196. On exposure to moist air, the crystals lose their silky appearance, and when treated with cold water, a slight evolution of nitrogen occurs. It melts under boiling water to a yellowish oil which gradually dissolves with evolution of nitrogen, and the solution contains formaldehyde.The same decomposition takes place, but much more quickly, when it is warmed with glacial acetic acid or dilute acids, but the decomposition into formaldehyde and nitrogen is not quite quantitative, as traces of ammonia are formed a t the same time. When heated in a capillary tube, or when treated with con- centrated acids, i t is immediately decomposed with evolution of nitrous fumes, and when heated on platinum foil it explodes. It gives Liebermann's reaction. The filtrate obtained in the prepara- tion of this cornpound contains unchanged hexamethyleneamine ; if, however, the mixture is kept for R long time before separating the nitrosoamine, the latter is decomposed into formaldehyde and nitro- gen, and some of the hexamethylenearnine is converted into form- aldehyde and ammonia.Dinitrosopentamethylenetetramine was obtained by gradually add- ing dilute hydrochloric acid to a solution of hexamethyleneamine and sodium nitrite (compare Griess and Harrow, Abstr., 1888, 1268). It melts a t 202--203", arid gives Liebermann's nitroso-reaction. F. S. I(. Action of Nitrous Acid on Hexamethylenearnine. F. S. K. Identity of Putresine and Tetramethylenediamine. By L. V. UURBNSZKY and E. BAUMANN (Bey., 21, 2938-2941).-A direct com- parison of the dibenzoyl-derivatives of putresine (Brieger), tetra- rnetlhylenediamine, and the compound obtained by the authors from YOL. LVt. d34 ABSTHACTS OF GHEMICAL PAPERS. the urine of a patient suffering from cystinuria (compare Abstr., 1888, 1296), proved that these bases are identical. Concentrated solutions of guanidine, creatine, creatinine, and similar compounds give a precipitate with soda and benzoic chloride, whereas no separation occurs in solutions containing less than 0.5 gram of the bases ; it is therefore necessary that when benzoic chloride is used as a reagent for diamines (Zoc. cit.) only very dilute solutions of the latter should be employed.By W. R. ORNDORFF and H. JESSEL (Amer. Chern. J., 10, 363--367).-Liebig stated that acetone could advantageously be substituted for alcohol in the preparation of chloroform ; this statement has been contradicted by Siemerling,.yet chloroform is now largely made from acetone. In a number of trials, the yield was 166 to 173 per cent.of the weight of the acetone used, and the residual liquors contained considerable quan- tities of calcium acetate. The reaction is represented by 2CO(CH,)z + GCaOCl, = SCHCl, + 2Ca(OH), + XaCI, + Ca(CH,*COO),. Liebig states that calcium carbonate is precipitated during the reaction, but the precipitate is calcium hydroxide. Acetophenone similarly treated with blenching powder, yields chloroform, calcium hydrate, and calcium benzoate. H. B. F. S. K. Decomposition of Acetone with Bleaching Powder. Dinitrosoacetone. By H. v. PECHMANN and K. WEHSARG (Ber., 21, 2989-2993) .-When dinitrosoacetone (compare Abstr., 1887, 28) is boiled with water or acids, it is decomposed into carboiiic anhydride, hydrogen cyanide, water, and ammonium hydrogen oxalate ; but when it is heated with glacial acetic acid, oxamic acid, melting at 210°, and hydrogen cyanide are formed.Trinitrosopropnne, NOH:CH*C(NOH)*CH:NOH, prepared by heat- ing a, mixture of dinitrosoacetone (1 mol.), hydroxylamine hydro- chloride (1 mol.), sodium acetate (1 mol.), and water at 50-60' for 1 to 2 hours, separates from hot water in the form of a colourless, crystalline powder melting a t 171" with sudden decomposition. It is only sparingly soluble in ether, but readily solubIe in alcohol, from which it crystallises in needles, and it, dissolves slowly, but in con- siderable quantities, in hot water. It behaves like dinitrosoacetone when heated with dilute acids, but its aqueous solution can be boiled for a short time without decomposition taking place.Ferric chloride gives a brownish-red coloration with a dilute aqueous solution ; ferrous sulphate produces a wine-red colour, and the solution then gives a violet precipitate with soda. Dinitrosoacetone hydrazone, NOH: C H-C (N,HPh) CH :NOH, pre- pared by treating dinitrosoacetone (1 mol.) with phenylhydrazine (1 mol.) in hot, alcoholic solution, crystallises in yellow needles, melts a t 145" with decomposition, and is readily soluble in alcohol and ether, more sparingly in benzene and light petroleum, and insoluble in water. It dissolves in alkalis with a yellow, and in concentrated sulphuric acid with an orange-yellow coloration. The metyZ-deriv% tive, C9H9N4O2Ac, a light yellow, crystalline compound, melts a t 133", and is soluble i n dilute alcohol.It dissolves in alkalis with aORGIAKIC CHEMISTRY. 35 yellowish coloration, but the soliltion becomes colourless on boiling, md on adding acids, a compound, C,H8N*0, is precipitated in shining, colourless needles. This substance is also formed when the acetyl- derivative is boiled with water. A compound, C,,H,,N,, is obtained when dinitrosoacetone is beaked with excess of phenylhydrazine acetate. It crystallises from hot alcohol or benzene in shining, yellow plates melting at 122". It is not acted on when boiled with ferric chloride, and its solution in concentrated sulphuric acid does not give a coloration with this reagent. Sulphoisovaleric Acid. By G. DE VARDA (Chew,. Ceiztr., 1888, 587-888, from Rend. Acad. dei Lincei [4], 4, 1).-100 parts of isovaleric acid are mixed with 100 parts of chlorosulphonic acid, and, after the spontaneous reaction has ended, the mass is heated to 230" ; it is then diluted with several volumes of water, and distilled from the oil-bath until the distillate no longer has an acid reaction.The distil- late is then heated with plumbic carbonate for some time, filtered while hot, and the lead precipitated from the solution by hydrogen sul- pbide, the solution of the free acid being concentrated in a vacuum. The aqueous solution partly decomposes when heated on the water-bath. The lead salt, C6H,S0,Pb.'LHz0, crystallises from water in colourless, odourless, small plates, which taste sweet ; they are slightly soluble in water, and insoluble in alcohol, ether, and chloroform.The barium salt, containing 1 mol. HzO, forms small, tabular crjstals, without smell o r colour, and taste bitter. It is soluble in water, insoluble in alcohol, ether, and chloroform. F. S. K. Su7phoisowaZeric acid so obtained forms deliquescent crystals. J. W. L. Constituents of Cocoa Fat. By P. GRAF ( A d . Pharm. [3], 26, 830-846 ; comp. Kingzett, Trans., 1878, 38).-l1he melting point of various samples of commercial cocoa butter from widely different sources was determined both in open and closed glass tubes. In the open tube, the results varied from 29" to 33-44', whilst in the closed tube 11 samples gave 34.3" and one 33.5". The whole of the samples were mixed together for the further investigation. The €at was found to contain hardly any free acid. Two determinations of glycerol averaged 9-59 per cent.A little cholesterin and small quantities of formic, acetic, and butyric acids were detected. After the separation of oleic acid, the solid fatty acids were isolated by fractional crystallisation, followed by Heintz's method of fractional precipitation by means of magnesium and barium acetates. No acid with a higher molecular weight than arachidic acid was found ; this confirms Traub's statement that he was unable to find theohromic acid asserted to be present by Kingzett. The presence of oleic, stearic, and palmitic acids was confirmed ; and either lauric acid o r one of its isomerides was isolated : there was not sufficient material at hand to settle this point. J. T. Action of Hydrogen Phosphide on Aldehydes and Ketone Acids.By J. MEESINGER and C. ENGELS (Ber., 21,2919-2928).- The compound obtained by passing hydrogen phosphide and hy- d 236 ABSTRACTS OF CHEXICAL PAPERS. drogen chloride into an ethereal solution of pyruvic acid has the constitution P(CMe<C0>)3, and is named by the authors phos- iUhorus-trianhyd~o~yru~ic acid (compare Abstr., 1888, 441). It is in- soluble in cold acids, and on heating, decomposition takes place. It dissolves in warm, glacial acetic acid, and separates unchanged on cooling. It is not acted on by bromine even a t 150", but when boiled with water it is decomposed into pyruvic acid and hydrogen phosphide. 0 Phospho1.zks-trihydroplll.uvic acid hydrazide, P[ CMe(OH)*C(OH):N,HPh],, is formed when the preceding compound is warmed with phenyl- hjdrazine in alcoholic solution ; it is a colourless, crystalline com- pound, melts a t 132", and is moderately soluble in alcoholic ether, but only sparingly in cold alcohol, and almost insoluble in ether.Hy drazonepyruvic acid hydyazide, Cl5'EIZI6N40, is formed , together with hydrogen phosphide, when phosphorustrianhydropyruvic acid is heated with excess of phenylhydrazine, in which i t is readily soluble. It crys tallises from hot alcohol in colourless, shining plates, melts at 162", and is only sparingly soluble in cold alcohol and ether. Phosphorus-t,.ihyclro~yruvic acid dianilide, is obtained when aniline is gradually added to an alcoholic solution of phosphorus-trianhydropyruvic acid. It separates from warm alcohol in colourless crystals, melts a t 158", is very sparingly soluble in cold alcohol and insoluble in water or ether.It is completely decom- posed, with separation of phosphorus, when treated with hydrogen chloride in alcoholic or ethereal solution. Dihy dyazonepy rzsv ic acid hy drazide, NP h (C 0-CMe: X2H Ph), , is formed when the preceding compound is treated with phenylhydrazide. It crystallises from alcohol in small needles melting at 169". Phosphorus-trianhydropyruvio acid and toluylenediamine yield a crystalline compound, CQHgOGP 3- 2C6H3Me(NH2),, which melts at 178" with decomposition. Hydrogen phosphide, in presence of hydrogen chloride, has no action on ethyl acetoacetate or benzoylcarboxylic acid, but tribromo- pyruvic acid absorbs the gas in considerable quantities with evolution of hydrogen bromide and the ultimate formation of phosphorus-fri- anhydropyruvic acid.3'. S. K. Action of Heat on Tartaric Acid in Aqueous Solution. B.7 E. M. WEDARD (Chenz. Centr., 1888, 889, from Atti. R. Acad. Scz. Torino, 6, 65-67).-The author noticed that when tartaric acid had been heated for several days in sealed tubes with ferrous sulphate, several of the tubes exploded violently, and in the others a consider- able quantity OE carbonic anhydride was found. As the ferrous salt had not become oxidised a t all, the reaction had not been a simple reduction of the tartaric acid. Tartaric acid heated with water alone at 150" in sealed tubes also suffered a considerable loss of carbonicORQANIC CHEMISTRT. 37 anhydride. In one experiment, the author opened the tube after heating, allowed the carbonic anhydride to escape, then sealed it again, and submitted the contents to a further heating, and repeated the operation until no further evolution of carbonic anhydride took place, after which the resulting liquid was found to contain pyro- tartaric acid along with undecomposed tartaric acid. Freezing Points of Solutions of' Aluminium Alkyls.By E. LOUISE and L. Roux (Cowpt. rend., 107, 600--603).-Pure ethylene bromide was used as a solvent, the molecular reduction, T, with this liquid being 118. The number obtained with mercury propyl was 124.8 ; mercury isobutyl, 122.7 ; mercury isoamyl, 123.6 ; mercury phenyl, 120.4. Aluminium ethyl gave a molecular reduction of 115.6, which agrees with the formula A1,Et6.Alunzinium proyy2, obtained by the action of aluminium on mercury propyl, is a colourless, mobile liquid, which boils a t 250" and takes fire in contact with the air. Aluminium isoam!jl, obtained in a similar way, is a somewhat viscous, colourless liquid, with an odour of amyl compounds ; it boils at 250" under a pressure of 80-100 mm., and does not readily take fire in contact with the air. The molecular reduction with aluminium propyl is 92.8, and with aluminium iso- amyl 84.5. These values agree more closely with the formula A]&, than with AIRs, and hence confirm the conclusions deduced from J. W. L. vapour-density determinations (Abstracts, l8S8, 583). C. H. B. Substituted Pyromucic Acids. By H. B. HILL and A. W. PALMEK. (Amer. Chen?. J., 10, 375--391).-With the exception of a sulphopyromucic acid briefly described b r Schwanert, no furf uran- derivatives containing the sulplionic group are described ; yet the general behaviour of pyromucic acid is similar to that of benzoic acic1.6- Sulphopyromucic acid is readily formed bay treating pyromucic acid with fuming sulphuric acid. The acid itself is extremely soluble in water, but may be obtained in large, deliquescent crystals. The follow- ing salts are described : RnC,H2S06 + 4H20 ; Ba( C5&SO,)a + 4H20, and also with 6H,O; CaC,H,SO, + 3H20; PbC,H,SO, + 2H20, all readily soluble in hot water; Ag,C5H2S06 is sparingly soluble in water; K,C5H,S0, + 4x20 ; KC,H,so, ; Na,C5H,S06 4- 5H20, and NaC&SO, + H20, all very soluble, All these salts crjstallise readily. By treating the dry sodium salt with phosphorns penta- chloride. and the resulting viscous oil with ammonia, the crystalline 6-suZphopyromucal.riide, C,H,SO,(NH,),, is obtained ; it is readily soluble in hot water, and melts a t 213'.The dry acid is only decom- posed by bromine at loo", dibromosuccinic acid and other products being formed ; in aqueous solution the acid is mainly converted into fumaric acid. Dilute nitric acid oxidises i t slowly, and also produces fumaric acid and some oxalic acid ; concentrated nitric acid at 100" readily converts it into Klinkhardt's 8-nitropyrom ucic acid, and at t h e same time a neutral substance, in all probability aa-dinitro- furfuran, is formed. Although bro,nine-derivatives of 8-sulphopyromucic acid camot be38 ABSTRACTS OF CHEMICAL PAPERS.obtained by the action of bromine, they may be obtained by sul- phonating the corresponding bromopyromucic acids : P-Hromo- 6-sulyhopyromucic acid is extremely soluble in cold water, and forms deliquescent crystals. The salts- BaC5HBrSo6 + 4H20; CaC5HBrS06 + 6H,O ; PbC5HBrS06 + 4H,O ; K,C5HBrS0, + 1+H20 (2) are described ; they are all crystalline and soluble in water. That the acid is really a derivative of 6-sulphopyromucic acid is proved by obtaining this acid by treatment of the bromo-acid with zinc and ammonia. Bromive in aqueous solution readily converts the bromo- acid into monobromofumaric acid. Concentrated nitric acid readily yields P-bro.uno-~-nitropyronzucic acid, soluble in water, alcohol, &c., and melting at 159-160". 8-r-Dibromo-6-su~h(~~~omucic acid is prepared by dissolving /3-y-di- bromopyromucic acid in fuming sulphuric acid, b u t it is more advan- tageous to use the mixture of P-61- and /3-6-dibromopyromucic acids resulting from the decomposition of the tetrabromo-acid, as the p-8-dibromo-acid is but little acted on by the sulphuric acid.Tbe acid in question is very soluble in water, and is crystalline; the following salts are described: BaC,Br2S06 + 5H20 and also with 3&O; PbC,Br2S06 + 4H20 ; AgzC,Br,So6 4- HzO ; K2C5Br2SO6 + H,O. That the sulphoriic acid occupies the 8-position, the only pos- sible one, is proved by treatment of the above barium salt with zinc-dust and ammonia, when the a-sulphopyromucic acid first described is obtained. Bromine in aqueous solution readily oxidises the barium salt, giving barium sulphate and dibromonialeic acid.Dilute nitric acid oxidises it to dibroruosuccinic acid. Concentrated nitric acid yields a mixture of P-ri-dibromo-8-nitropyrornucic acid, crystallising from water in sparingly soluble, slender, yellow needles, that melt a t 204- 205", and /3/3-dibromo-aa-dinitrofurfuran, a substance melting at 150-151" and crystallising from benzene, as the compound C',Br2(NO,),O,C6H6, which readily gives off this benzene of cqstal- lisation. H. B. Metadiethylbenzene. By A. VOSWINKEL (Ber., 21,2829- 2831). i7.letudiethyZbeiizene, C6H4Et2, is obtained, together with the para- compound, by the action of ethyl bromide and aluminium chloride on benzene ; the two compounds are separated from each other by means of the barium sulphonates.It boils a t 181--182", and does not solidify a t -20", but bccomes thicker. Sp. gr.. = 0.8602 at 20" com- pared with water a t 4". When boiled with dilute nitric acid, ethyl- benzoic and isophthalic acids are formed. The barium sulphonate (with 3 mols. H,O) crystallises in hemispherical groups of prisms, rather sparingly soluble in cold water. The coppr saZt (with 4 mols. H,O) forms bright-blue plates of a satiny lustre ; the potussium salt (with 1 mol. H20) crystsllises in quadratic plates. The sulphor~arnide separates from the dilute alcoholic solution in long, flat needles, melting a t 101-102". The bromir~e-derivatii.e, C6H3Et2Br, boils at about 238". The teirnbromo-compciund, C6Et2Br4, crybtrcllises from alcohol in small, colourless prisms melting a t 74".Nat,ometuJ!iefhyZ- btlzneiie, C,B,Et,*NO2, is a pale yellow liquid, which boils atORGANIC CHEMISTRY. 39 280-285", with decomposition. The trirdro-compound, CsHEt,(NO,)-, crystallises from light petroleum in prisms melting at 62". A;mido- metadiethylbenzene, C6H3Et2.NHa, prepared by reducing the nitro- derivative, is a colourless liquid which distils readily with steam ; the hydrochloi-ide crystallises in groups of very long needles ; the acetyl- derivative forms stellate groups of needles melting at 104". Metadi- ethyZphenoZ, C6H3Et2*OH, is obtained by fusing the sulphonic acid with potash ; it boils at 225", and dissolves spariugly in water ; the solution gives a blue-violet colour (which changes to green on adding alcohol) with ferric chloride. Zeta-ethylbenzoic acid, C6H4Et.COOH, crystallises in long needles, melts a t 47", and is almost insoluhle in water.The calcium salt (with 4 mols. H,O) forms lustrous needles, readily soluble in water and alcohol. Synthesis of Consecutive Tetramethylbenzene. By 0. JACOBSEN (Ber., 2 1, 282 1-28 28) .-Dinitro bromopseudocumene, N. H. M. [(N02)2 : Br : Me3 = 5 : 6 : 2 : 1 : 3 : 41, obtained by the action of nitric and sulphuric acids on bromopseudo- cumene [Br : Mes = 2 : 1 : 3 : 41, crystdlises from hot alcohol in small, yellowish-white, lustrous prisms, melts a t 182", and dissolves readily in hot benzene, sparingly in hot alcohol. Bromopseudocumene, [Br : Me, = 2 : 1 : 3 : 41, has the same boiling point as the 5, 1, 3, 41 compound: 237-238" (not 226-229").The sulphonamide nielts at 185" (not 137-188"; compare Kelbe and Pathe, Her., 19, 1546). 1, 2, 3, 4-'l'ctramet,hylbenzene is prepared by heatiiig pure bromo- pseudocumene (25 grams), methyl iodide (40 grams), and sodium (14 grams), in presence of sufficient absolute ether to cover the latter. After two or three days, it is distilled. The yield of tetramethyl- benzene is 38 per cent. of the weight of the bromopseudocumene. Dibromonietnzylene, [Me, : Br2 = 1 : 3 : 2 : 41, is obtained in the preparation of spinietrical dibromometaxylene by brominating the hydrocarbon ; it is an oily liquid which, when cooled, solidifies to a hard crystalline mass melting a t -So, and boils a t 269" under 760 mm. pressure. The di~itro-deri~atiwe forms a1 rriost colourless, microscopic crystals, melts a t 191", and dissolves readily in toluene, very sparingly in alcohol.When exposed to light it becomes yellow. The sodium sulphowie, C6HNe,Br,*S03Na + H,O [= 1 : 3 : 2 : 4 : 61, crystallises in groups of needles; the potassium salt with 1 mol. H20 forms lustrous plates, sparingly soluble in cold water; the barium salt crystallises in small prisms. The amide separates from alcohol in small prisms, which melt with decomposition above 300". When the sodium salt is treated with zinc-dust and ammonia, the salt of ordinary unsymmetrical metaxylenesulphonic acid is formed. OrthoiZicLmidometaayZene, [Me, : (NH,), = 1 : 3 : 5 : 61, is obtained by very prolonged action of tin and hydrochloric acid on the dinitro- dibromo-compound, and is liberated from its hydrochloride by dry distillation with sodium carbonate in a stream of hydrogen.It crys- tallises from water in rhombic plates, melts a t 78.5", and dissolves readily in alcohol, ether, and hot water. When exposed to moist air,40 ABSTRACTS OF CHEMICAL PAPERS. it beeomes grey-violet. The constitution of this compound as given is proved by the synthesis of 1, 2, 3, 4-tetramethylbenzene from the liquid dibromometdxylene by the action of methyl iodide and sodium, using ether as a diluent. When symmetrical dibromometaxylene is heated with sulphuric acid (3 parts) at 240", it is converted into the liquid isomeride. Tetrethylbenzene. By 0. JACOBSEN (Ber., 21, 2819-2821). -Symnretrscal tetrethylbmzene, C,H.,Et, [Eta = 1 : 'L : 4 : 51, is obtained, together with a smaller amount of the isomeride [Et, = 1 : 2 : 3 : 41, by the action of ethyl bromide on benzene in presence of aluminium chloride, at a temperature not above the boiling point of the bromide ; the product is sulphonated in the cold and the sodium sulphonnte heated a t 170" with hydrochloric acid.It melts a t 13", and boils a t 250". When boiled with dilute nitric acid, and the product further oxidised with permanganste, pyromellitic acid is formed. Dibromotetrethylbenzene, C,Br,Et, [Et, = 1 : 2 : 4 : 51, crystallisea from hot alcohol in long, thin prisms melting a t 112.5". S o d i u m tetreth y1benzenesubphonate, C,H E t,*SO,Na + 4H20, crystal- lises from water in very large, lustrous plates, sparingly soluble in cold water, much more readily in alcohol, almost insoluble in cold dilute aqueous soda.The barium salt (with 9 mols. H20) is sparingly soluble in hot water. The sulphona?~~ide, C14H21.S02*NH2, crystallises from hot dilute alcohol in rhombic plates, melting at 122". Pentethylbenzene and its Decomposition by Sulphuric Acid. By 0. JACOBSEN (Ber., 21, 2814-2819 ; compare Abstr., 1887, 660 ; 1888, 137).-PentsthyZbenzene, C,HEt,, is prepared by the action of ethyl bromide on benzene in presence of aluminium chloride, and purified in a manner similar to the pentamethyl-compound (loc. cit.). I t forms a thick oil, which boils at 277", and does not solidify at -20". Brornopentethylbe?inene, C,BrEt,, obtained by brominating the hydro- carbon dissolved in glacial acetic acid, crystallises from alcohol in long needles, melts at 47*5", and boils a t about 315". It is readily soluble in hot alcohol.The suZphone, SO,( C6Ets),, crystallises from light petroleum con- taining some alcohol in large, transparent, hexagonal prisms of a glassy lnstre, melts a t 76", and is very readily soluble in alcohol, much less in light petroleum, and insoluble in water. Sodium perdeth y Zb enseisesulphonate, C,,H,,-S 0,Na + 4H,O, crystal - lises from water in thin, lustrous plates, moderately soluble in hot water, much more soluble in alcohol. The anhydrous salt crystallises froin 90 per cent. alcohol in groups of hair-like needles. The potccssium salt (with 2 mola. H,O) crystallises in thin plates, rather readily soluble in hot water, much more soluble in alcohol. The aniinonium (with 1 mol.H,O) and barium (with 9 mols. H20) saZfs crystallise respectively in large, thin plates and small scales. When pentethylbenzene is treated with an equal volume of sulpburic acid sy much fumiug sulphuric acid added to the cooled mixture that N. H. M. N. H. M. Sp. gr. = 0.8985 a t 19".ORGANIC CHEMISTRY. 41 a clear, brownish-yellow solution is obtained, and the whole kept for 4-5 days a t the ordinary temperature, hexethylbenzene and tetrethyl- benzene [Et, = 1 : 2 : 3 : 41 are formed. Hexethylbenzene melts at 229" and boils a t 298". Tetrethylbenzene [Et, = 1 : 2 : 3 : 41 boils a t 254", and does not solidify a t -20". It is probably identical with Galle's compound (Abstr., 1883, 109 1). The dibronzo-derivative, CsBi.,Et4, crystallises in prisms of a glassy lustre, melts at 77", and is sparingly soluble i l l boiling alcohol.Barium tetrethylbenxenesdphonate, (C,,EI,,*SO,),Ba + 6H20, crystal- lises from water in flat prisms OF a glassy lustre; the sodium saZt (with 5 mols. H,O) forms readily soluble rhombic plates. The amide sepa- rates from its solution in water and alcohol in well-formed crystals of a glassy lustre, and melts at 107". N. H. M. Synthesis of Aromatic Selenium Compounds. By C. CHABRIF: (Bull. SOC. Chlm., 50, 133-137) .-Phenyl selewide, SePh,, is obtained by adding aluminium chloride to selenium tetrachloride (I part) and benzene (3 parts), contained in a reflux apparatus, until no more hydrogen chloride is evolved. The temperature in the flask varies from 22' to 27", and the operation is finished in about 60 hours.It boils a t 227" under a few cm. pressure. Phenyl chloride and an oil boiling at 250" under a pressure of A few cm. are also formed. Selenium oxychloride in presence of aluminium chloride and selenious anhydride, also react with benzene. Consecutive Metaxylenol. By 0. JACOBSEN (Ber., 21, 2828- 2829) .-The author previously (Abstr., 1878, 412) ascribed t o con- secutive metaxylenol the melting point 74.5". Nolting isolated the compound from commercial xylidine, and found the melting pointl 49". This melting point is now confirmed by preparing metaxylenol by heating pure parahydroxymesitylic acid ; the product melted a t 47-48'. The xylenol previously obtained (Zoc. cit.) was paraxylenol. Nitronitrosoresorcinol. By C:. DE LA HARPE and F.REVERDIN N. H. M. N. H. M. (Bull. SOC. Chim., 49, 760-763).-Nitronitrosoresorcil/ol, [OH: NO,: 0 : NOH = I : 2 : 3 : 41, is obtained when a cooled mixture of nitroresorcinol (1 mol.), melting a t 85", with a solution of soda (1 mol.) in 10 parts of water and an aqueous solution of sodium nitrite (1 or 2 mols.) is gradually added t o excess of dilute and well-cooled sulphuric acid. The yellow, flocculent precipitate is washed with water, dried over sulphuric acid, and extracted with ether to ~emove traces of nitrosoresorcinol. It cvystallises from alcohol in brownish needles, and is readily soluble in water, acids, and alkalis, but only moderately soluble in alcohol, and insoluble in ether, benzene, and chloroform. It is not changed when heated to about 200", but at higher temperatures it deflagrates violently.It yields diamidoresorcinol (compare Bite, Ber., 8, 631) when reduced with tin and hydrochloric acid. The aqueous solutioii gives an intense green coloration with ferrous sulphate o r with iron filings, and a slightlly acid solution of the colouring matter, which can42 ABSTRACTS OF CHEXICAL PAPEkS. be precipitated from the aqueous solution by adding sodium chloride, dyes wool green (compare F h r e , Abstr., 1883, 733). Concentrated snlphuric acid added to a mixture of resorcinol and nitronitroso- resorcinol? produces a green colour, which changes to blue and t,hen to a dirty violet; from this solution water precipitates brown flocks, which dissolve in alkalis with a greenish-brown coloration. Nitroresorcinol, [(OH), : NO2 = 1 : 3 : 41, melting at 115", does not form a nitroso-derivative when treated as described above.Condensation-product of Quinone and Ethyl Acetoacetate. By H. V. PECHMANN (Ber., 21, 3OO5-WO6) .-A Condensation-product, C16H1606, is formed when quinone (1 gram) is heated a t 100" with ethyl acetoacetate (2.5 grams) and a 50 per cent. solution of zinc chloride (6 grams) in absolute alcohol. It melts a t 184", and is solu- ble i n boiling alcohol or glacial acetic acid, but insoluble in water. The solution in Concentrated sulphuric acid turns deep blue when heated. It yields crystalline derivatives when treated with bromine, but it is not acted on by phenylhydrazine, benzoic chloride, sodium ethoxide and alkyl iodides, or by boiling hydriodic acid.A crystalline bibasic acid, C14K1,06, is precipitated when the preceding compound is hydrolysed with alcoholic potash and the solution acidified with acetic acid. It sublimes without melting, and is insoluble in all ordinary solvents. The potassium salt, C,4HloK206 + 2H,O, is a colourless, crystalline, spariugly soluble compound, and loses its water at 125". F. S. I(. Derivatives of Paramidoisobutylbenzene. By C. GE LZER (Ber., 21, 2941-2949, and 2Y49-2961).-l?aracetarnidobromisobutyl- benzene, C4HS*C,H,Br.NHAc, prepared by brominating acetamidoiso- butylbenzene: crybtallises from hot dilute alcohol or benzene in large, shining scales or plates, and melts a t 1.53". It is readily soluble in alcohol, hot benzeoe, ether, carbon bisulphide, and chloroform, but only very sparingly soluble in boiling water.B~Iiir7obrumi.sobzctylbenzene, C4H,*C6H,Br*NH2, is a heavy,. yellowish, aromatic-smelling oil, boiling a t 264-265" (710 mm.) with decom- position, and volatile with steam ; i t is readily soluble in alcohol, ether, and benzene, b u t insoluble in water. The hydrochloride, CloHI4NBr,HCl, crystallises from benzene in moss-like needles, and is readily soluble in water, alcohol, and warm benzene, but almost insoluble in ether. The platinochloride, (CloH14NBr)2,B ZPtCI6, obtained by precipitating a cold alcoholic solution of the base with a hydrochloric acid solution of platinic chloride, crystallises in slender,. yellow needles, and is readily soluble in alcohol, but only sparingly in cold water, and insoluble in ether; it is decomposed when boiled with water.A light yellow, crystalline substance, ( CloH14NBr),PtCl,, is obtained when a cold alcoholic solution of the base is precipitated with a neutral solution of platinic chloride ; it; is sparingly soluble in cold alcohol, and is decomposed when the solution is heated. The picrate, CloH14NBr,CsH,N,07, separates from a mixture of warm benzene and light petroleum in slender, yellow, spear-shaped crystals, and is readily soluble in cold alcohol, ether, or liot water, but only sparingly in cold water or cold benzene, and moderately soluble in hot benzene. F. S. IC.ORQANIC CHEMISTRY. 43 Bi-onzisobutylbenzene, C4H,.C6H4Br, obtained by treating the amido- derivative with nitrous acid and distilling the product, is a heavy, slightly yellow, aromatic-smelling oil, boiling a t 231-232" (710 mm.), and only slightly volatile with steam.It is readily soluble in alcohol, ether, and benzene, but irisoluble in water. It yields metanitrobenzoic acid when heated a t 235-240" with nitric acid of sp. gr. 1.15. 17letanitroi-cobzLtylbenxene, C4HS*CqH4-NO2, obtained by treating the amido-derivative with nitrous acid, and fractionating the product in a partial vacuum, is a bright yellowish-red, aromatic-smelling oil, boil- ing a t 250-252" (740 mm.). It yields metanitrobenzoic acid when heated at 200" with nitric acid of sp. gr. 1.12. I~iti-oisobut2/l~henoZ, [C4Hg : NO, : OH = I : 3 : 41, prepared by boiling amidonitroisobntylbenzene with dilute potash and distilling the product, separates from alcohol in yellowish-red, deliquescent crystals, melts at 95", and boils at 289-290" (711 mm.) with only slight decomposition.It is readily soluble in alcohol, ether, benzene, light petroleum, alkalis, and hot water. Metainidoisobuty lbenzene, C4H9*Cj6H1*NH,, prepared by reducing the nitro-derivative with stannous chloride and hydrochloric acid, is a yellowish oil, boiling a t 229' (708 mm.), and moderately volatile with steam. It is readily soluble in alcohol, ether, and benzene, b u t only sparingly in water. It dissolves in a solution of bleaching powder with a bright riolet colour, and with potassium dichromate and sulphuric acid yields a reddish-violet coloration, which quickly changes to brown. The hydrochloride, ClOH,,N,HCl, crystallises from hot benzene in colouiless plates, and is readily soluble in aater and hot alcohol, but only sparingly soluble in benzene.The platino- chloride, ( C,oH,,N)2,H,PtCl,, crystnllises in bright yellow plates, and is readily soluble in boiling water and hot alcohol, but only sparm.gly in benzene and ether. The ozalate, CloH&,C2H204, crysthllises from hot water or dilute alcohol, in which it is readily soluble, in large white plates. The acetyl-derivative, C4Hg*C6H4*NHAc, crys- tallises from boiling water in colonrless, shining plates, melts at 101", and is readily soluble in alcohol, ether, and benzene. n~etacetamidonit,.oisobzctylbenzene, [C4Hg : NO, : NHAc = 1 : 2 : 31, obtained by nitrating the acetamido-derivative, crystallises from hot dilute alcohol in small, yellow needles, melts a t 105*5", and is readily soluble in alcohol, benzene, and ether, but very sparingly in boiling water.Ainidonitroisobut?lZbenzene, C4H9.C,H,(X0,)*NH2, separates from dilute alcohol in bright yellow crystals, melts at 1 2 4 , and is readily soluble in alcohol, ether, benzene, and boiling water, but sparingly soluble in cold water. It is only a feeble base, and the salts are readily soluble. Dia.r.lzidoisoEutyZbenzene, [CIHg : (NH,), = 1 : 2 : 31, prepared by reducing the preceding compound with stannous chloride and hydro- chloric acid, crystallises from alcohol in colourless plates, melts at log", is readily soluble in water, alcohol, ether, and benzene, and blackens on exposure to the air. The oaalate, (CloH16N,),,C2H204, crystallises in flat needles, and is readily soluble in boiling water, but only sparingly in cold, ahsolute alcohol, and almost insoluble in ether.44 ABSTRACTS OF CHEMlCAL PAPERS.an alcoholic solution of the dinmine is mixed with a glacial acetic acid solution of phenanthraquinone. It separates from hot dilute alcohol in yellow nodular crystals, melts a t 144" with previous soften- ing, and is readily soluble in warm alcohol, ether, and benzene, but only sparingly in boiling water. It dissolves in concentrated nitric acid with a brownish-red. in concentrated sulphuric acid with a scarlet coloration, and is precipitated unchanged from both solutions on adding water. U NCPh \N*CPhH Benzilisobuty@hennzitze, C,Hg*C6H,/ I \, prepared in like man- ner from the dinmine and benxil, crystallises in small, light-yellow prisms, melts a t 96", and is only sparingly soluble in cold alcohol, but readily in ether, benzene, and hot alcohol.It dissolves in concen- trated nitric acid or concentrated sulphuric acid, but is precipitated unchanged on adding water. AcefLt?nidobromonifroisobuf!llbenzene, C4Hg~C,H,Br(N0,)~NHAc, pre- pared by nitrating acetamidobromisobutylbenzene, crystallises from a mixture of ether and light petroleum in small, rhombic plates, melts at 144O, and is readily soluble in hot alcohol, ether, or benzene, but only very sparingly soluble i n boiling water. Amidobromonitroisobuty Zbenxene, C,Hg*c6H2Br( NO,) .NH2, crystallises in long needles, melts a t 69*5", boils a t 278-280" with partial decom- position, and is volatile with steam. It is very sparingly soluble in boiling water, but readily in alcohol, ether, and benzene.Diamidobromisobutylbenzene, c4Hg*C6~,Br(N&),, obtained by re- ducing the preceding compound with stannous chloride and hydro- chloric acid, crystallises from ether in slender, colourless needles, melts a t 85*5", and turns brown on exposure to the air. It sublimes with considerable decomposition, forming colourless needles which are stable in the air. It is readily soluble in alcohol, ether, and benzene, but only very sparingly in hot water. Ferric chloride produces a brownish-red coloration ; bleaching powder precipitates oily drops, and platinic chloride gives a brownish-black coloration in a hydrochloric acid solution of t.he base. The oxulate, C1oH15BrNzl CJLO4, crystallises in small needles, and is moderately soluble in boiling alcohol, but only sparingly in ether, benzene, and warm water.The picrate, CloHlbBrN2*2, C6H3N307, crystallises from hot water in yellow needles. and is readilv soluble in alcohol and ether. lises from boiling alcohol in slender? yellow needles, melts- at 153-5", and is readily soluble in benzene, ether, and boiling alcohol, b u t only sparingly in cold alcohol. It dissolves in concentrated mineral acids, forming red solutions, from which it is precipitated unchanged on adding water.ORGANIC CHEJIISTET. 45 X*C*Ph \N*C-Ph Beiizilbromisobuty ~ h e n a z i ~ e , C4Hg*C,H2BJ I II 3 crystallises from hot alcohol in colourless needles, melts at 172", and behares towards solvents similarly to the preceding compound ; it dissolves in (son- cen trated acids with a yellowish-red coloration.Dibi-oniisobutylbenzene, [C4Hg : BrP = 1 : 3 : 51, obtained by heating metabromisobutylbenzene with bromine in presence of iodine, and distilling the product with steam, is a light yellow oil, boils a t 376-277" (718 mm.), and is readily soluble in all ordinary solvents except water. When heated a t aboxt 250" with nitric acid, sp. gr. 1.20, i t is converted into symmetrical dibromobenzoic acid. F. S. K. Decomposition of some Diazo-compounds by Formic and Acetic Acids. By W. R. ORNDORFF (Amer. Che1.12. J., 10, 368-372). -The decomposition of diazo-compounds by formic acid might be expected to furnish an easier means of displacing the amido-group by hydrogen than the decomposition with alcohol.But the reaction proceeds otherwise and could not be followed out, a9 the phenyl formate that was probably formed could not be isolated. Substitut- ing acetic acid for formic acid, it is shown that phenyl acetate is pro- duced ; the yield is, however, small, as milch tar is also formed ; the reaction is analogous to the production of phenetnil by the action of alcohol. The boiling point of phenyl acetate has been variously stated; it has been redetermined as 195" at 733 mm. pressure. Similarly, paradiazotoluene sulphate, when boiled with acetic acid, yields paracresyl acetate, boiling a t 213", and identical with that pre- pared from paracresol. Paradiazobenzenesulphonic acid appears to undergo a similar change, and the reaction therefore seems to be general.H. B. Chryso'idincarbamide. Amidophenylenecarbamide. By A. JENTZSCH (J. pr. Chem. [ 2 ] , 38, 121-139). -When carbonyl chloride is passed into a moderately strong solution of chrysoidin in dry chloroform, it is rapidly absorbed with development of heat, and red-brown flocks separate which become of a darker brown as the action proceeds. The brown matter is collected, dried, powdered, heated with dilute hydrochloric acid, and filtered hot ; brilliant golden-yellow laminae crystallise out on cooling, together wit8h octo- hedral crystals of diamidoazobenzene hydrochloride. By dissolving the mixed crystals in alcohol and adding ammonia, golden-yellow needles of the correspoiiding bases are obtained, which may be separs ted by digestion with chloroform, the diamidoazobenzene being dlssolved.The residue, consisting of the new base, is purified by dis- solving in alcohol and passing hydrogen chloride through the solution to obtain the hydrochloride which is then decomposed by ammonia. Chrysozdincarbarnide, NPh:NC,H,:(NH)Z:CO, thus obtained, crys- tallises in brilliant, golden-yellow laminae, sparingly soluble in alcohol, nearly insoluble in water, ether, and chloroform. It does not meit at 300". I f the chloroform solution of diamidoazobenzene be satur;rted with carbonyl chloride and allowed to stand for some days, only46 ABSTRACTS OF OHEMMIGAL PAPERS. carbamide hydrochloride and unaltered chrysoi'din hydrochloride will be found on evaporating the chloroform. The hydrochloride crystallises in golden-yellow laniinse, sparingly soluble in water, more so in alcohol, insoluble in ether.The pZatiizochZoride, ( C13H11NaUC1)2PtC14, forms red-brown laminse. The nitrate crystal- lises in brilliant, golden-yellow scales, very sparingly soluble in water, sparingly soluble in alcohol, and insoluble in ether ; they decompose with slight explosion at above 200". The suZphate forms a yellowish- red powder ; it is very sparingly soluble in water, more so in alcohol. When heated with moderately strong hydrochloric acid in a sealed tuhe at 200" for eight hours, chrysoidincarbamide is decomposed, with the formation of carbonic anhydride and a dark-brown mass. The same dark-brown substance is obtained when chrysoidin is treated in the same way. It yields phenol when distilled with steam, and a reddish-brown residue which has not been identified.Inasmuch as chrysoidin splits up into aniline and triamidobenzene when reduced by hydrochloric acid and tin, it seemed probable that its carbamide would yield aniline and a new substance, by the same treatment, thus showing that both NH-groups are attached to the same benzene nucleus. 100 grams of the carbarnide were heated with 50 grams of tin aud 250 grams of hydrochloric acid (sp. gr. 1.2) in a flask. The solution became colourless at first, and subsequently brown, through oxidation ; after the action had ceased, the hydrochloric acid was evaporated, the residue dissolved in hot water, and hydrogen sulphide passed through the solution ; the filtrate from the tin sulphide was evaporated in a current of hydrogen sulphide, the crystalline residue dissolved in water, and made alkaline with barium hydroxide.This precipitated aniline, which was dis- tilled off; the excess of barium hydroxide was precipitated from the liquid remainisg in the retort by sulphuric acid, and the excess of the latter by barium chloride. From the filtrate, the hydrochloride of the new base did not crystallise well, so the solution was digested with ammonium oxala te and filtered hot. On cooling, amidophenyZene- arbamide oxalate crystallised out in nearly white minute needles, collected in spheres, freely soluble in hot, sparingly in cold water, nearly insoluble in alcohol. Amido~he?zyZerzecai.bnmide, NHz*C6H3: (NH),:CO, obtained from the oxalate by adding sodium carbonate to a hot solution of it in hydro- chloric acid, forms brilliant and nearly colourless, pointed laminm, sparingly soluble in cold, easily in hot water, freely soluble in hot alcohol, and decomposing at 220".The hydrochloride crystallises in minute needles, freely soluble in water, very sparingly so in alcohol. The sulphate also forms minute needles, having the same solubility. The triacetyZ-derivutzve, NHAc.C6H3:(NAc)z:C0, forms fine, white, silky needles, insoluble in water, fairly soluble in alcohol, and melting at 248'. NH,* CsH,: (NH),:CO, /NH*CO\ c 6 H 3 \ ~ ~ - ~ ~ / N 7 Dicarboity ltriainidobenzene, was obtained beating amidophenylene carbamide with liquid carbonyl chloride in aORGANIC CHEMISTRY. 47 sealed tube for eight hours at 130". The excess of carbonyl chloride was evaporated and the residue heated with water, which extracted the hydrochloride of the carbamide fo~med during the reaction, and left the carbonyl compound as a crystalline residue, insoluble in alcohol, ether, benzene, toluene, aniline, and acids, but very soluble in alkaline solutions, from which it is precipitated by acids.By passing nitrous acid through a cooled, acidified aqueous solution of the sulphate of amidophenylenecarbamide, yello wish-green crystals, giving the reactions of a diazo-compound of the carbamide, were obtained, but they were not pure. By dissolving them in hydro- bromic acid and adding a few drops of bromine, yellowish-red needles of the perbromide of the diazo-compound crystallised out- ; these lost bromine as they dried, and by digesting them with warm alcohol they weye converted into yellow crystalline laminm of the diazo- hroinide of amidophenylenecarbamide.By H. v. PECHMANN and I(. WEHSARG (Rer., 21, 2994 - 3004).-Nitrosoa~etonehydrazone (methylglyoxal-aw- hydrciz- oain2 e ) N,H Ph: CMe.CH:NO H, prepared by mixing nit rosoacetone (1 mol.) with phenylhydrazine (1 mol.) in alcoholic or ethereal solu- tion, crystallises from alcohol in yellowish prisms or needles, melts at 134", and is soluble in ether and benzene, but insoluble in hot water. It dissolves in concentrated sulphuric acid with a reddish-yellow colour which becomes deep blue on adding ferric chloride. Met hylglyoxalosnzone hydrochloride is obtained when the preceding compound is warmed with concentrated hydrochloric acid in alcoholic solution. It crystallises from boiling methyl alcohol, melts a t 197", and yields the free base (compare Abstr., 1888, 1287) when treated with ammonia.A. G. B. Hydrazoxirnes. Diacety Eli ydrazoxime (methylnitrosoacetone h ydraxone) , CMe(N,BPh)*CMe:NOR, prepared in like manner from nitrosometbylacetone, crystallises from dilate alcohol in large, colourless needles, melts at 158", and resembles nitrosoacetonehydrazone in its behaviour towards solvents. It dig- solves in concentrated sulphuric acid with a yellow coloration which changes to a bluish-violet on adding ferric chloride, and when heated with concentrated hydrochloric acid in alcoholic solution, yields a mixture of diacetylosazone melting at 241--242", and diacetyl- hydrazone melting at 13.3". Gl~/ox~Zcya?zide-a-hydrazone, CRO*C(N,HPh).CN, is formed, together with hydroxylamine, when dinitrosoacetonehytlrazone (com- pare this vol., p.34) is warmed with alcohol and hydrochloric acid. It crystallises from boiling alcohol in pale-yellow needles, melts at 161" with decomposition, and is dissolved on warming in most sol- vents except water. It is soluble in dilute alkalis, and dissolves in concentrated sulphuric acid with a yellow colour which is not changed by ferric chloride. When boiled with hydriodic acid, it yields the theoretical quantity of aniline. Glyoxy Zr y anideosazone, NZHP h:CH*C (N2HPh) *CN, prepared by mixing a hot, alcoholic solution of the preceding compound with48 ABSTRACTS OF CHEMICAL PAPERS phenyl hydrazine, cry stallises from alcohol in orange-red needles, melts at 161" with decomposition, and is soluble in alcohol and glacial acetic acid, but, only sparingly in most other solvents.The concentrated siilphnric acid solution is yellowish-red, and its colour is not changed bv ferric chloride. .I GlyoxylcyarLideosotetrazone, < ~ ~ ~ ~ ~ $ is formed when the preceding compound is m-armed with ferric chloride or with a solution of potassium dichromate and dilute acetic acid. It crystallises from acetone or alcohol in brownish-red, moss-like needles melting at 137" with decomposition. When heated with hydrochloric acid, a colour- less, crystalline product, probably an osotriazone (loc. cit.) volatilises. This compound, CgH6N@:N2Ph, is formed by the combination of glyoxylcyanidehydrazone with diazobenzene chloride ; it crystallises from alcohol in brownish plates, melts a t 162-163", and is insoluble in alkalis. Gll/ox?/lcZlanide-aw-hydrazox~~ne, NOH:CH.C(N,HPh).CN, prepared by boilicg an alcoholic solution of the hydrazone (1 mol.) with hydroxylamine hydrochloride (1 mol.) and a few drops of hydro.cliloric acid, crystallises from alcohol in citron-yellow, sparingly soluble needles melting a t 240" with decomposition. It dissolves in alkalis with a yellow coloration, but the yellow, concentrated sul- phuric acid solution is not changed on adding ferric chloride. A compound, C,H,N 4, is obtained when glyoxylcyanidehydrax- oxime is dissolved in phosphorus oxycbloride, heated with phosphoric chloride, the solution poured on to ice, the precipitated product ex- tracted with ether, dissolved in dilute alkali, and fractionally pre- cipitated with hydrochloric acid.It crystallises from a mixture of ether and light petroleum in yellowish needles, melts a t 135" with decomposition, and is soluble in hot water, alkalis, and most of the ordinary solvents. It dissolves in Concentrated sulphuric acid with a blood-red coloration which is not changed on adding ferric chloride. When warmed with concentrated hydrochloric acid or when boiled with alcoholic potash, it is converted into a ccmpouiid, C9H9N40, which crystallises in small, yellow needles melting a t 244-245". - A compound, C,,H,,N,, is formed i n the preparation of glyoxyl- cyanidehydrazone, and can also be obtained by heating the hydraz- oxime with alcohol ( 3 patbts) and cmcentrated hydrochloric acid (10 parts). I t crystallises from benzene in shining, orange-yellow plates melting a t 165", and does not give the osazone reaction (loc.cit.). MethylgZyoxal-ocw-met?~Zl~hen~~l~iy~~raz~~~~e, N,MePh:CMe*CH:NOH, prepared by mixing an aqueous solution of nitrosoacetone with a solution of methylpbenylhydrazine sulphate and sodium acetate, -crystallises from dilute alcohol in orange-yellow prisms melting at 118". Alkaline solutions are dark yellow, and the yellow, concen- trated sulphuric acid solution changes to violet on adding ferric chloride. Mesoxala7deh yde- a w w-n7 eth y lphen y lh ydrazonedioxim e (dinitrosoaceton e methylphenylhydruzolze), N OH:CH.C(N,MePh)*CH:NOH, prepared in like manner, crystallises from dilute alcohol in orange-yellow ueedlesORGANIC CHEMTSTRY.49 or plates, melts a t 137", and is soluble in alkalis and most of the ordinary solvents. It dissolves in concentrated sulphuric acid, forming a brownish-red solution in which ferric chloride produces a light violet coloration. When heated with hydrochloric acid, it yields decomposition products the nature of which varies according to the conditions of the experiment. Glyoxylcyanide-a-msfhyZphenylhydrnzone, CHO*C(N,MePh).CN, is obtained by dissolving the preceding compound in acetone ( 7 parts), adding concentrated hydrochloric acid (7 parts) and, after the first energetic reaction is a t an end, heating the mixture for about a minute and adding water to the cold solution. It crystallises from benzene, alcohol, or light petroleum in yellow, feathery needles, or thick, spear-shaped crystals, melts a t 113*5", and is insoluble in alkalis.When mixed with phenylhydrazine, it yields a compound, probably N,HPh:CH.C (N,MePh) CN, which crystalliseq from abso- lute alcohol in golden-yellow plates melting a t 181". The and, NPh:CH*C (X,MePh).CN, prepared by mixing the hpdrazone with aniline i n acetic acid solution, crystallises from alcohol in slender, yellow needles, melts a t 150-151°, and is reconverted into the hy$hzone when warmed with dilute hydrochloric acid. The hydrar- oxz112e, NOH:C H*C (N,MePh).CN, obtained by treating the hydrazone with hydroxylamine, crystallises in small, yellow needles melting at 178'. The acetyl-derivative, NOAc:CH*C(N,MePh).CN, of the hydrazoxime crystallises from alcohol in yellow needles, melts a t 122*5", and is reconverted into the hydrazoxime when boiled with soda.F. S. K. Ethyl Phenylhydraxineacetylacrylate. By H. D ECICER (Ber., 21, 2937-2938).-Tbe compound obtained by Bender (Abstr., 1888, 1188) by hydrolysing ethyl phenylhydrazineacetylacrylate, has already been fully described by L. Wolff (Abstr., 1887, 464). F. S . K. Theory of Dyeing. By E. KNECHT (Ber., 21, 2804-2805 ; com- pare Abstr., 1888, 832).-When wool is boiled with a mixture of sulphuric acid (2 parts) and water (3 parts) for two hours, it dissolves almost entirely ; when filtered, a clear, light-brown solution is ob- tained. If this is mixed with aqueous solutions of acid coal-tar dyes, intensely coloured precipitates are formed, which dissolve readily in alkalis, but not in water or dilute acids.A solution of silk in moderately dilute sulphuric acid behaves in like manner. Animal fibres, therefore, yield a substance which forms insoluble bases with acid coal-tar dyes; it has not yet been deter- mined whether this substance already exists in the fibres, or whether it is gradually formed by the action of the acid bath. N. H. M. Product of the Action of Nitric Acid on Acetophenone. By A. F. HOLLEMAR" (Bei-., 21, 2835-2840 ; compare Abstr , 1888, 275). -The molecular weight of the compound C,,H,,N,04. obtained by the actioii of nitric acid on acetophenone (Zoc cit.), was confirmed by a determination by Raoult's method (BPT., 21, 861). When the alco- holic solution is reduced with stannous chloride, benzoic and hydro- VOL.LVI. e50 ABSTRACTS OF CHEMICAL PAPERS. cyanic acids are formed. By qrolonged boiling with strong hydro- chloric acid, it is decomposed into benzoic and oxalic acids; am- monia and hydroxylamine are also formed. These reactions make it probable that the compound has the constitution <CBaiN.O>, CBz'N-0 which is further supported by the fact that the substance, which is named diphenyldi.nitrosacyl, can be prepared by oxidising nitroso- acetophenone. Diphenjldinitrosacyl reacts with aniline with formation of benz- anilide and a compound crystallising in lustrous, brown needles. When this is heated a t 100" €or some time, it gives an odour somewhat like that of carbylamine : when crystallised from dilute alcohol, it is nearly white, and melts a t 205".When diphenyldinitrosacyl is heated with acetic anhydride at 110-120" for six hours, the compound C,6H10N204 + OAc, is formed. This crystallises in stellate groups of needles melting at 149". The sparingly soluble compound melting at 177-179", which is also obtained by the action of nitric acid on acetophenone (loc. cif.), has the same empirical composition as diphenpldinitrosacyl ; it is, how- ever, much more stable than the latter. Boiling aqueous potash and hot sulphuric acid decompose it, yielding benzoic acid ; with potash, ammonia is evolved. N. H. M. Consecutive Duryl Methyl Ketone. By A. CLAUS and E. FOHLISCH ( J . pr. Chew. [a], 38, 230-235; compare Abstr., 1888, 275) .-The boiling point of consecutive dureno is 199-200" (uncorr.) and its melting point is -4".Consecutive duryl methyl ketone, C6HMe4*COMe [Me4 : COMe = 2 : 3 : 4 : 5 : 11, is prepared in the manner previously described, by which 80-90 per cent. of the durene used is couverted into the ketone ; it is a brown, strongly refractive oil, of agreeable aromatic odour, boiling a t 258-260" (uncorr.), and easily soluble in the nsual solvents, except water. The pkenylhydrazine compound forms,, colourless laminae melting a t 129" (uncorr.). 2 : 3 : 4 : 5 - 1 ' e t r a m e t h y ~ ~ ~ e n y ~ g l y o a y ~ i c acid, C6Hh!fe4*CO*COOH, is formed when the above ketone is oxidised with potassium perman- ganate in the cold. It is a bright yellow syrupy oil, very little soluble in cold, more so in hot water, very soluble in alcohol, ether, carbon bisulpliide, and chloroform ; it solidifies on prolonged cooling and decomposes when heated. The barium and calcium sa2ts (with 4 mols.H,O), the copper (with 3 mols. H,O), azd the silver salts are described. 2 : 3 : 4 : El-Tetramethylmandelic acid, C6H%~e4.CH(OH)*COOH, is obtained by reducing the foregoing acid with sodium amalgam. 'It crystallises from alcohol in colourless hexahedra, sparingly soluble in cold, readily in hot water and in alcohol, ether, and chloroform, and meits at 160" (uncorr.). The potassium (with 4 mols. H,O), barii~m (with 3 mols. H,O), calcium (with 24, mols. H,O), and silver salts are described. 2 : 3 : 4 : 5-Tetrainethy123herz2llacstic acid, C6HMep-CHz.COOH, is formed when either of the above described acids is reduced withORGANIC CHEMISTRY.51 hydriodic acid. It crystallises from hot water in slender, colourless needles, me1 ting a t 125" (uncorr.), and easily soluble in alcohol, ether, and chloroform. The calcium salt forms colourless, silky needles con- taining 3 mols. H,O. By oxidising consecutive duryl methyl ketone or the foregoing de- rivatives, with the calculated quantity of potassium permanganate, at a gentle heat, 2 : 3 : 4 : 5- tetramethylbenzoic acid is obtained as a thick, colourless oil, sparingly soluble in water, freely so in other sol- vents. When heated, it decomposes a t 270°, and an oil distils over, which solidifies and melts at 150" ; this contains 73.8 per cent. of carbon and 7.9 per cent. of hydrogen. The sodium (with 3 mols. H,O), calcium (with 3 mols.H,O), bariunc (with 6 mols. H,O), silver and coypel- salts are described. A. G. B. Stilbene. By I;. ARONSTEIN and A. F. HOLLEMANN (Ber., 21, 2831-%334) .-The experiments described were made with a vicw to obtain a geometrical isomeride of stilbene which should exist according to Wislicenus' theory. No definite results were obtained, but the investigation is being continued. Action of Heat on Benzildihydrazone. By I(. AUWERS and V. CPh'N M E ~ R (Ber., 2 1,2806 -2 80 7). --Tripheny losotriazone, < CPhiN >NPh, formed when benzilhydrazone is heated with alcohol at 200-210", crystallises in white, lustrous plates, melts a t 122O, and boils without decomposition. N. 13. M. Thio-derivatives of p-Dinaphthylamine. By 0. KYN (Ber., 21, 2807-28 13) .-When sulphur chloride dissolved in benzene is added to /3-dinaphthylamine, also dissolved in benzene, hydrogen chloride is evolved and two isomeric dithiudinaphth ylainines, C20H13NS2, are ob- tained.The one forms lustrous, brass-coloured plates melting a t 205O, whilst the other crystallises in reddish-yellow prisms melting a t 220". Both compounds are sparingly soluble. When the dithio-compounds are boiled with cumene or with aniline, they are both converted with evolution of carbon bisulphide into Ris's thio-P-dinaphthylamine (Abstr., 1886, 1036). A small quantity of the latter compound is formed in the reaction between dinaphthylamine and sulphur chloride. Acetylthio-p-dinnphthylainiwe, Cz2Hl5NOS, is obtained by the action of acetic anhydride on the dithio-compound (ni.p. 605") or on the monothio-compound. It crystallises in slender, lustrous, almost white needles, melts a t 211", and is readily soluble in hot alcohol or benzene. When the dithio-compound (m. p. 205O) is treated with an ammoniacal alcoholic silver solution, a compound free from sulphur is obtained, which melts a t 240°, and sublimes in slender, lemon- yellow needles. Sulphur dichloride acts on p-dinaphthylamine, yielding as chief product thio-p-dinaphthylamine, and a sparingly soluble isomeride which melts a t 303". Sometimes a small amount of a compound, probably thiotetranayhthylanline, S ( C,oH6*NH.CloH7)2, is obtained. This forms dark-yellow crystals melting at 307". N. H. M. N. H. M. e 252 ABSTRACTS OF CHEMICAL PAPERS. Naphthoic Acids. By A. G. EKSTRAND (J.pr.Chem. [2], 38, 139--285).-This paper is a summary of the author's work on the subject; much of it has already appeared. The following new corn- pounds are described :- Chloro-a-naphthoic arnide is obtained by heating chlopo-a-naphtho- nitrile (Abstr., 1884, 1361) with an alcoholic solution of potassium hydroxide ; it forms crystalline laminae, soluble in alcohol and melting a t 239". The chloro-a-naphthoic acid which melts a t %5" (Abstr., 1884, 1361) has the constitution [COOH : C1 = 1 : 4'1, as it is obtained by treating 1 : 4' amido-a-naphthoic acid by Sandmeyer's method (Abstr., 1884, 1312). Chloro-a-nayhthoic a,cid (1 : 1') is obtained when 1 : 1' amido-a- naphthoic acid (Abstr., 1885, 549) is dissolved in the calculated quantity of sodium hydroxide and potassium nitrite (1 mol.to 1 mol. of the amido-acid) added ; the mixture is cooled to 0" and treated with excess of hydrochloric acid. The hydrochloride of the diazonaphthoic acid thus obtained is added to a boiling solution of cuprous chloride in hydrochloric acid ; colourless crystals of the chloro-acid are formed ; they melt a t 167" and sublime as plates. The calcium salt crystallises with 2 mols. €LO in long tabular needles, soluble in 42 parts of water at the ordinary temperature. The ethyZ salt forms long needles melting at 50". Dichlor-a-naplithoic acid is obtained when the foregoing acid is dissolved in glacial acetic acid, some iodine added, and chlorine passed t o saturation ; crystalline scales separate, melting at 186-187". The calcium salt crystallises with 2 mols.H,O in long, colourless needles ; the ethyl salt forms fine needles melting at 61". It is possible to obtain this acid from chlornitro-a-naphthoic acid [COOH : NO, : C1 = 1 : 1' : 4'1 (Abstr., 1886, 156), consequently its constitution is [COOH : C1 : C1 = 1 : 1' : 4'1. Trichloro-a-nap hthoic acid, the mother-liquor from the preparation of chloro-a-naphthoic acid (1 : 4') by the action of chlorine on a-naph- thoic acid in acetic acid solution, is saturatedwith chlorine at the boiling point : dilution with water then throws down a crystalline precipitate, which is heated with calcium carbonate, filtered, and the filtrate pre- cipitated with acid ; when crystallised from alcohol and water, this precipitate forms small, colourless needles, melting at 163-164' and subliming in fine needles.The ethyl salt of monobromo-a-naphthoic acid, 1 : 4' (Abstr., 1886, 715), forms colourless tables melting a t 48-49'. Mononitro-a-naphthoic acid of meltiug point 215" (Abstr., 1885, 54$) is soluble in 21.5 parts of commercial alcohol, and in 2590 parts of water a t the ordinary temperature. During its formation a small quantity of a-mononitronaph.t//alene (melting point 60') is obtained. The calcium salt of amido-a-naphthoic acid (Absbr., 1885, 549) crystallises with 9.5 mols. H20 in fine needles, soluble in water. The hydroch Zoride, COOH.C,oH6*NH,,HC1, is precipitated in fine needles O n adding hydrochloric acid to a solution of the sodium salt. Nsphthostyril, C,,H,<ZE> (Abstr., 1886, 715), crystallises fromORGANIC CHEMISTRY.53 an alcoholic solution of the amido-a-naphthoic acid ; it is also formed when the acid is heated with water ; it melts a t 180-181". The benxoyl-derivative forms slender needles melting a t 170" ; the hydrochloride melts a t 178". a-Naphtlzoybz aph thostyri1.-When a-naphthoyl chloride and naph - thostyril are heated together, a gi-een product is formed, which is dissolved in alcohol and decolorised hy animal charcoal. A mixture of granular crystals (melting a t 110") and needles (melt- ing at 132") is obtained ; by recrystallking these, partly from alcohol and partly from glacial acetic acid, a mixture of the same crystals is obtained, melting a t 150". /3-Naphthoylnaphthostyril, is obtained in the same way tw tlie above, only a t a lower temperature, in slender colourless needles, melting at The calcium salt of chlornitro-a-naphlhoic acid, of melting point 225" (Abstr., 1886, 156), forms slender colourless needles, crystallising with 3 mols.H,O, and the ethyl salt tabular crystals melting at 121", and very soluble in alcohol. The question whether this acid has the constitution [COOH : NO, : C1 = 1 : 1' : 4' or 1 : 4 : 4') is settled in favour of the former, as chZoronaphthostyJriB (with C1 in position 4') is obtained in yellow needles melting at 670", by reducing the acid with ferrous sulphate in an ammoniacal solution. Nitronaphthostyril (1 : 4') is formed when nitric acid (sp. gr. 1.42) is added to a solution of naphthostyril in glacial acetic acid, and the mixture heated on the water-bath ; the crystalline mass thus obtained is partially soluble in alcohol, from which yellow needles, melting about 235", are obtained ; the greater part recrystallises from glacial acetic acid in orange-yellow needles melting a t 300".Both are nitro- nap hthostyrils. Arraidonuplzthostllril is formed when nitronaphthostyril is reduced with tin and hydrochloric acid. and the hydrochloride thus produced decomposed with ammonia ; it crystallises in red needles melting a t 239-240", and freely solable in alcohol and hot water: The hydro- chloride crystallises in yellow needles melting above 290". Dinitronaphthostyrd is obtained when the nitronaphthostyril is heated with nitric acid (1.43 sp. gr.) ; it forms yellow needles, or, when pre- pared by the action of nitric acid on naphthostyril, rhombic tables, melting above 290".Naphthostyrilpuinone, C,,H,O,<EE>, is obtained when a Bolution of naphthostyril in glacial acetic acid is mixed with chromic acid and then with water; fine red needles are precipitated, which, after re- crystallisation from glacial acetic acid, melt near 278". When it is dissolved in warm glacial acetic acid and an acetic acid solution of toluylenediamine added, a yellow, crystalline powder, consisting of nuphthostyriZtoZ~p~inoaali.ne, CllH5N30,C6H3CH3, is obtained ; it melts above 290". Nitronaphthosty1.ilquinone forms orange-red needles or tables, melt- ing near 685", soluble in alcohol and sparingly so in glacial acetic acid. A. G. B. 19 7-198". The acetyl-derivative melts above 290".54 ABSTRACTS OF C'HERIICAL PAPERR p-Chloronaphthalenesulphonic Acid.By S. FoRsrmG (Be?.., 21, 2802--2804).--When ,!3-amidonaphthalenesulphonic acid (Abstr., 1887, 962) is converted into the diazo-compound, and this is boiled with strong hydrochloric acid and neutralised with potassium carbonate, potassi um p-chloronapht h alenesulph onate separates. p- Chloronaph thalenesulphonic chloride, CloH6C1*SO2C1 (Arnell, Ahstr., 1886, Fj55), is prepared by mixing the well-dried potassium salt with phosphorus pentachloride and heating ; it crystallises from chloroform in broad needles melting a t 129". The brornide, CloH6C1*S 02Br, prepared by the action of phosphorus bromide on the potassium salt, crystallises from chloroform in small needles melting at 139". The amide, CIoH6C1.S02*NH,, is obtained by boiling the chloride with a mixture of equal parts of ammonia and alcohol, and crys- tallising the product from dilute alcohol, in which it is sparingly soluble; it melts at 235". p-Chloronaphthalenesulphonic acid has the constitution [Cl : SOsH = 2 : 4 o r 2 : 1 ] .N. H. M. Filicic Acid. By G. DACCOMO (Bey., 21, 2962-2970) .-Filicic acid, prepared by the method already described (Daccomo, Abstr., 1888,521) , has the composition Cl4H1,O6. It is a yellowish, odonrless, crystalline powder, melts at 179-180" (uncorr.), and. is insoluble in water, almost insoluble in absolute alcoho1,'moderately soluble in glacial acetic acid, ether, amyl alcohol, and toluene, and readily in chloroform, cwbon bisulphide, and benzene. The benzoyl-deriva tive, C2,H,,0,, separates from dilute alcohol in colourless crystals, melts a t 123", and is very readily soluble in ether, but insoluble in water.The ethyt salt, C,H,,O,, prepared by treating the acid with alcoholic potash and ethyl iodide, separates from dilute alcohol in reddish crystals, melts at 142", and is very readily soluble in ether and benzene, but insoluble i n water, The propyl salt melting at 158", and the ethylene salt melting at 165", resemble the ethyl salt in appearance and solu- bility. Bronzo$Zicic acid, Cl4HI5BrO6, prepwed by treating the acid with bromine in glacial acetic acid solution, crystnllises from alcohol in red prisms, meits a t 122", and is very readily soluble in absolute alcohol and ether, but insoluble in water. AniZidoJiZicic acid, C14HZ50,*NHPh, obtained by boiling a glacial acetic acid solution of the acid with aniline, separates from alcohol in reddish-violet crystals, melts a t 140°, and is soluble in alcohol and benzene, but insoluble in water.The hydraaide, C,Hl,O.( NZHPh),, prepared by boiling an ethereal solution of the acid with phenylhydrazine, crystallises from ether ill red needles, melts at 198", and is readily soluble in alcohol, but insoluble in waker. When the acid (100 parts) is heated above its melting point (compare Luck, AnnaZen, 54, 119), or heated with water at 170-190", it is decomposed into isobutyric acid (32.5 parts) and a compound, the composition of which is C?OH,AOI. Hydrochloric acid produces the same decomposition at 150-160". Filicic acid is completely oxidised when treated with chromic acidORGANIC CEIEMISTRT.55 in glacial acetic acid solution, but when a solution of the potassium salt is oxidised in the cold with a 2 per cent. solution of potassium permnnganate, isobutyric acid and oxalic acid are obtained. Tbe same products are formed when nitric acid of sp. gr. 1.48 is employed. When the acid is treated with zinc-dust in alkaline solution, i t is con- verted into an acid, the composition of which is probably Cl4Hz2011, and at the same time a small quantity of isobutyric acid is formed. When treated with sodium in amyl alcohol solution, it, yields butyric acid and resinous products. The compound CZOH,80,, referred to above, separates from ether or amyl alcohol as an amorphous, red powder, and has no well-detined melting point.It is soluble in most ordinary solvents, has an acid reaction, decomposes carbonates, and dissolves in alkalis, forming red solutions from which it is precipitated in red flocks on adding acids. It yjelds phthalic acid and small quantities of ovalic acid when oxidised with nitric acid of sp. gr. 1.40 in the cold. When reduced with zinc-dust in alkaline solution, it gives a colourless substance which rapidly oxidises, and is probably reconverted into the original compound. From the above results, it follows that filicic acid is probably an isobutyric acid derivative of hydroxynaplithaquinone. F. S. K. Quillajic Acid. By R. KOBERT (CYhesn. Centr., 1888, 927-928, from Arch. ex$. Path. Pharm., 23, 233).--The saponin of commerce, as all other specimens of saponin, is an almost inactive, non-poisonous modification of quillajic acid.The author precipitated the acid from the aqueous extract of the bark of Quillaja sapomaria with neutral lead acetate ; the precipitate was fresd from lead, the solution of the acid evaporated almost to dryness, and then taken up with hot absolute alcohol. The colouring matter was precipitated with chloroform ; the quillajic acid eventually crystallised out in pure white flakes. It is insoluble in ether, soluble in water and alcohol. On treatment with concentrated sulphuric acid, it becomes dark red. By boiling with dilui e mineral acids, it is split up into an unfermentable glucose and sapo- ginin ; this solution reduces Fehling's solution. Quillajic acid has the formula Cl,H,oOlo.The sodium salt acts as a very severe caustic on the tongue and throat, and the smallest particles coming in contact with the nose or throat cause violent sneezing and coughing. Brought on to the eye, it causes severe pain, flow of tears, and swelling of the lids. Injected into the blood, the sodium salt proves fatal, causing cramp arid paralysis of the respiratory organs and brain. On the other hand, it may be imbibed into the stomach without injury to the extent of 500 times the quantity which proves fatal when injected into the blood. J. W. L. Brazilin. By C. SCHALL and G. DRALLE (Bey., 21, 3009-3017, compare Abstr., 1888, 295) .-Tetramethylbrazilin is best prepared as follows:-A solution of brazilin (100 grams) in warm 98 per cent. alcohol is mixed with sodium ethoxide (30.26 grams sodium) and methyl iodide (206 grams), the mixture kept a t 60-70" for 40 to 50 hours, cooled and poured into cold water.The precipitate is collected,56 ABSTRACTS OF CHEMICAL PAPERS. washed with water, dissolved in ether, the solution shaken with soda ( 1 7 2 per cent.), washed with water, the ether evaporated, and the residue crystnllised from alcohol with addition of animal charcoal. The yield is 58.5 per cent. of the theoretical quantity. Trirnethylbrazilin, C16H1105Me3 + iH,O, is obtained by neutralising the alkaline washings from the tetramethyl-derivative, extracting with ether, washing the extract first with sodium hydrgen carbonate, then with sodium carbonate, and evaporating the ether a t the ordinary temperature. The residue is mixed with concentrated soda, the pre- cipitated sodium-derivative collected, washed with alcoholic ether, dissolved in water, and precipitated from the filtered solution by treat- ment with carbonic anhydride.If the product is pure, it is obtained in the crystalline condition containing about 1 mol. H,O, but the impure compound does not crystallise well even after keeping for months. It dissolves in dilute alcohol, and the solution gives a brown precipitate with ferric chloride ; the solution in soda is colourless, and does not alter on keeping. The acetyl-derivative, C16H,,05Me,Ac, is crystalline, and melts a t 95-97" with previous softening. Rrornotetrainethylbrazilin, C16H9BrMe40,, obtained by treating the tetramethyl-derivative (1 mol.) with bromine (1 mol.) in glacial acetic acid solution, crystallises from dil-cite alcohol in long, colourless prisms melting a t 180-181".A crystalline tetrabromo-derivative, C,,H,Br,Me,O,, is formed when a larger quantity of bromine (2-3 mols.) is employed ; this snbstance loses bromine (about 26 per cent.) when treated with dilute ammonia, or soda, and appears to be dibromotetramethylbrazilin dibromide. It is probable that other bromo-derivatives exist, and a crystalline iodo- additive product was also obtained. Tribrornobrazilin dibyomide, C16HllBr305,Br2 + 2H20, is obtained in reddish-brown needles when bromine (4-6 mols.) is added gradually to a boiling glacial acetic acid solution of brazilin. A compound, C20Hld09, is obtained when brazilin (2.7 grams) is dissolved in water (150 c.c.) and soda of sp. gr.1.37 (10 c.c.), and a stream of air passed through the solution for about 36 hours. It crystallises from alcohol in light brown, flat, microscopic needles, melts at &71", and is readily soluble in dilute soda, sparingly soluble in ether or sodium carbonate, and insoluble in sodium bicarbonate. The aqueous alcoholic solution gives a slight violet coloration with ferric chloride, and a citron-yellow coloration with concentrated nitric acid. When heated above its melting point, shining scales sublime, but considerable' decomposition takes place. F. S. K. Nomenclature of Compounds containing Nitmgenous Nuclei. By 0. WIDMAN ( J . pr. Chem. [a], 38, 185-20l).-A new system of nomenclature for the quinoxalines and compounds of allied structure.(Compare Mason, Proc., 1888, 109.) Metapyrazolones. By E. GRINAUX (BUZZ. SOC. C'him., 49, 739- 740) .-The compounds described by Pinner and Lifschutz, and named by them metapyrazolone-derivatives, are derivatives of glycolylcarb-ORGANIC CHE3IIISTRY. 57 amide or hydantojin, and the isomeric substances which Pinner and Lifschutz name metapyrazole-derivatives are simple ureides. P. S. K. Action of Phenylhydrazine and Hydroxylamine on Acetyl. acetone. By A. COMBES (Bull. SOC. China., 50, 145-146 ; compare ibid., 48, 471) .-Dimethy~hei.ly~yrazole, CMe<Nph,N>CMe, is formed by the action of phenylhydrazine on acetylacetone : it boils at 270.5". Derivatives of Methylpyrroline. By G. DE VARDA (Ber., 21, 28 7 1-28 74) .-MethyZtetrabromo~yrrol~ne, C4NBr4Me, obtained by digesting tetrabromopyrroline with caustic alkali and methyl iodide dissolved in methyl alcohol, crystallises from light petroleum in long, colourless needles, which melt at 154-155" to an intensely blue liquid.Dibromomaleinmethy limide, C4Br,0zNMe, is prepared by slowly adding tbe above t,etrabromide to fuming nitric acid (3 parts), cooled to 0", and pouring the product into water (10 parts). It crystallises from boiling water in long, light-yellow needles melting a t 121". It distils readily with steam ; the vapour has an irritating odour. N e t h y k y r r y lg Zy ozy Zic acid, CaNH,Me-CO*COOH, is obtained by treating a boiling solution of methylacetylpyrroline (5 grams) in alkaline water (500 c.c.) with a solution of potassium permanganate (15.5 grams) in water (500 c.c.).The whole is boiled, steam-distilled, and filtered ; it is then evaporated down, acidified, and extracted with ether. The acid is crystallised from benzene, from which it separates in light-yellow needles which melt a t 141-142.5' with decomposi- tion; it is sparingly soluble. The silver salt was prepared, The dibromo-derivatice, C4NHIMeBr2*CO*COOH, prepared by brominating the acid dissolved in acetic acid, crystallises from benzene in small, sulphur-coloured prisms melting a t 160". When the dibromo-acid is slowly added to fuming nitric acid (10 parts), dibromomalei'n- methvlimide is formed. The bromine-atoms and the --CO*COOH CH-- (Compare Claisen, Abstr., 1888, 692 ; and Zedel, 1051.) N. H. M. grou; have, therefore, the positions 3, 4, and 5 respectively.N. H. M. Derivatives of Unsymmetrical Dimethylpyrroline. By G. MAGNANINI (Ber., 21,2864-2868, 2874-2879) .-Ethy I diwethylasetyl- pyrrolinecnrboxylate, C4NHMe2Ac*COOEt [ 2 : 4 : 5 : 31, prepared by heating ethyl hydrogen dimethylpyrrolinedicarboxylate (Know, A n d e n , 236, 318) with acetic anhydride at 'LOO", crystallises in needles, melts at 142-143", dissolves very readily in alcohol, etlier, acetic acid, and benzene, &c., sparingly in light petroleum. The f r e e acid obtained by boiling the ethyl salt with aqueous potash, melts at about 152-158Owith formation of dimethylacet~I-pyrroZine and evolution of carbonic anhydride, is almost insoluble in boiling water, very sparirigiy soluble in ether, chloroform, and benzene, and readily soluble in hot acetic acid, from which it separates in long, lustrous needles.It gives a green coloration when heated with isatin and sulpbnric acid. DimethyZacety~yl.roZine, C4NH,MezAc [ = 2 : 4 : 51, is prepared by distilling dimethy lacetylcarbopyrrolic acid in a retort heated in a58 ABSTRACTS OF CHEMICAL PAPERS. metal-bath a t ZOO". It is first crystalliscd from water containing a little sodium carbonate, then from dilute alcohol, and lastly from light petroleum. It melts a t 122-123", sublimes a t loo", and is readily soluble in the usual organic solvents. Dimethylpyi-rolinedica.l.boxylic acid irnineanhydride, c O / y M e \c . c 0 OH, 'N*C Me/ is obtained by boiling Knorr's unsymmetrical dicarboxylic acid (Abstr., 1887, 275) with acetic anhydride (10 parts) in a reflux apparatus for three to four hours.The acetic anhydride is distilled off under diminished pressure, the residue washed with alcohol, dis- solved in aqueous sodium carbonate, filtered, and precipitated with acetic acid. It is almost insoluble in the usual solvents, becomes slightly brown a t 300", and decomposes a t a higher temperature into dimethylpyrroline and dimethylpyrocoll. It resists the action of mineral acids, but seems to be pastially decomposed by aqueous ammonia. The silver salt is a yellowish, amorphous substance ; the m a p e s i u m saZt forms lustrous needles. The ethyl salt crystallises in thread-like needles, melts a t 270", and is sparingly soluble. 2, 4-DiiizethylpyrocoZZ, C7H7N0, obtained by distilling the copper or silver salt of the above acid in a stream of carbonic anhydride, is light, yellow, melts a t 272--272*5", dissolves very readily in chloroform, readily in acetic acid, but only sparingly in ether, light petroleum, and cold alcohol ; it is insoluble in water.The crystals are rhombic ; cc : b : c = 0.788:-(4 : 1 : 0.94606. The compound is hardly attacked by aqueous potash. N. H. M. Derivatives of Pyrrolinephthalide. By F. ANDERLINI (Bey., 21, 2869-2870) .-Dibromopyrrolinephthalide, C,,H5Br,NO2, .prepared by treating a warm solution of pyrroliuephthalide (2 grams) in glacial acetic acid (15 grams) with bromine (8 grams), crystallises in small, yellow, lustrous needles, melts at 199", is insoluble in water, sparingly soluble in boiling alcohol and ether. Nitropyrroli.,iep7itAalide, C,,H6N2O4, is formed when the phthalide is dissolved in strong nitric acid ; it crystallises from alcohol in needles.When pyrrolinephthalide is treated with bromine in alkaline solution, tetrabromopyrroline and phthalic acid are formed. On similarly treating the dibromo- and nitro-derivatives, both compounds yield phthalic acid; the substituted radicles are therefore in the pyrroline nucleus. When potassium pyrrolinephenylcarbinolorthocarboxylate, CINH3:C (0 H) *c6H4.co~K, is distilled with potassium carbonate, it is decomposed into pyrroline and benzene. N. H. M. Action of Methyl Iodide on some Pyrroline-derivatives. By G. CIAMiCraN and F. ANDERLlNr (Bey., 21, 2855--2864).-Dihydro- tetl.ainethyl~,llridine, C9kI15N, is obtained, together with other bases,ORGAN I0 CHEMISTRY.59 when sodium carbopyrrolate (5 grams), methyl iodide (10 grams), and methyl alcohol (7 grams) are heated a t 120" for 12 hours. It boils a t about 160". The aurochloride, CgH15N,HAuC14, crystallises from very dilute solutions in long, flat, monoclinic needles ; a : b : c = 54: 10 : 5 i ; j? = 85%. When the base is reduced with sodium and alcohol, the compound C&HI9N is formed. This boils a t 150-152°. The azirochloride separates from its solution as an oil, which crystal- lises after some days in yellow needles melting a t 117-119". When the base C,HlgN is boiled with methyl iodide in a, reflux apparatus, and the product, freed from tlhe excess of methyl iodide, is dissolved in alcohol and precipitated with ether, the compound CI9Hl8NMeZI is obtained in colourless prisms which melt at 262".It is very readily soluble in water, insoluble in ether. The mother-liquor from the di- methyl compound contains a small amount of a buse, C9HI8NMe, which forms an oil. MetliyZL~il~yd70~2/0^roZine, CloHl7N, is prepared by heating methyl- pyrroline (3 grams), methyl iodide (7 grams), potassium carbonate (3 grams), and methyl alcohol ( 5 grams), for 10 hours ah 140". The oily product is heated with strong hydrochloric acid at, 125-130", and distilled with potash. The aurochloride, Cl7HI7N,HAuCI4, crystal- lises from dilute hydrochloric acid in flat, yellow needles, which melt at 100". N. H. M. Dipiperidyl and Dipicolyl. By F. B. AHRENS (Eey., 21, 2929- 2932).-Dipiperidyl is obtained when pi-dipyridyl is reduced with sodium and alcohol and the product purified by means of the nitroso- derivative.It crystallises in colourless needles, melts at 120-122" with previous softening, and is readily soluble in alcohol and ether, but insoluble in water. It absorbs carbonic anhydride when exposed to the air, and is only slighhly volatile with steam. The pkr,tiv,o- chloride, CloH,,M,,H,PtC16, forms microscopic crystals, is only sparingly soluble in water, and blackens when heated a t 195". The aurochloride, CloH,N2,HAuC14, crystallises in small, yellow needles, is readily soluble in hot, dilute hydrochloric acid, and is gradually decomposed when heated a t about 160". The p i c r a t e crystallises from hot water in needles ; it blackens when heated, and is completely decomposed at about 257".Mercuric chloride,. phosphomolybdic acid, and potas- sium ferroqanide produce precipitates in a solution of the hydro- chloride. DipicoZyZ, CI2Hl2N2, is obtained when picoline, boiling a t 128-1 34", is treated with sodium at 80-90". After washing the product with water, it is dissolved in ether, the solution filtered, and the base ex- tracted wit8h dilute hydrochloric acid. The extract is mixed with excess of soda, the treatment with ether and hydrocliloric acid repeated several times, and finally the ethereal solution is dried over potash and evaporated. The residual yellow oil is then distilled, and the portion passing at 270-300" collected ; this dist,illate solidi- fies to a mass of yellowish, very deliquescent needles. The platino- chloride, C12Hl,N2,H2PtC16, crystallises in small plates, and is very sparingly soluble in water, but readily in hydrochloric acid ; it, is only partially decomposed when heated at 2 75".The aurochloride,60 ABSTRACTS OF CHEMICAL PAPERS. C1,H,,N2,HAnC14, separates from warm, concentrated hydrochloric acid, in which it is readily soluble, in nodular crystals mixed with metallic gold ; it is completely decomposed when heated a t 200-201". The picrate forms yellow, moss-like crystals, and is readily soluble in hot water. An aqueous solution of the hydrochloride gives precipi- tates with mercuric chloride, phosphomolybdic acid, potassium iodide, and potassium ferrocyanide. Action of Chlorine on Hydroxyquinoline. By H. HERhRRAND (Ber., 21, 2977 - 2989).- Chlcrrhyd,.uxyqztinoline, CgNH,OCl, is formed in small quantities when chlorine is passed into a well-cooled solution of 1-hydroxyquinoline ( 5 grams) in glacial acetic acid. Dichlorhydroxyquinohne (see below) separates a t hst, and is further converted into the hydrochloride whilst a further portion of the hydr- oxyquinoline is oxidised t o the rnonochloro-derivative. As soon as the whole of the hydroxyquirioline 1s changed, the solution is filtered and the residue treated with absolute alcohol to dissolve the dichlorhydroxy- salt. The residue is dissolved in hot, dilute hydrochloric acid, the solution mixed with excess of sodium carbonate, and the precipitated monochlorh ydroxy-compound recrystallised fram methyl alcohol and light petroleum. It is thus obtained in colourless needles melting a t 129-130'.The hydrochloride crystallises in small, yellow needles, melts a t 253", and is moderately soluble in alcohol and hot, dilute hydrochloric acid ; it is very stable and sublimes in compact crystals. The platinochbride, (C9NH60C1)2,H2Pt C1, + 2H20, crystallises in yellow needles, and is readily soluble in hot but only sparingly in cold, dilute hydrochloric acid. DichZorhydroxyqzLinoZine, CgMH4C12*OH [OH : CI, = 1 : 2 : 41, is prepared by passing chlorine into a 10 per cent. glacial acetic acid solution of hydroxyquinoline until the colour changes to yellow, pouring the solution into water, and recrystallising the precipitated product from alcohol. It is also obtained when t~ichloroketoqu~noline (see below) is treated with hydrogen sodium snlphite or boiled w i t h alcohol or dilute acids.It crystallises in long, slender needles, melts at 179-180", and is readily soluble in warm alcohoi or glacial acetic acid, but only moderately in hot benzene and light petroleum. It dissolves readily in alkalis and acids, forming yellow solutions, but the salts are unstable and cannot be recrystallised, and acid solutions are precipitated by water. When treated with chlorine in chloroform solution, it is converted into trichloroketoquinoline, The h y d ~ o - chloride crgstallises in long, yellow needles, and in aqueaus solution gives a black precipitate with ferric chloride. The platircochloride, ( C9NH,0C1,),,H2PtC16 + 2H20, crystallises in long, orange needles, and loses its water a t 120"- The acety l-derivative, CgMH40C1,Ac, separates from light petroleum in small, colourless ci-ystals melting at 97-98"; it is very unstable, and is decomposed by water or when boiled for a long time with glacial acetic acid.Tricl~lorl2ydroxyyuinoZ~ne, [OH : C1, = 1 : 2 : 3 : 41, is formed when the mother-liquor from trichloroketoquinolitie is boiled or when the hydrochloric acid solution of pentachloroketoquinoline is treated witli hydrogen sodium sulphite or with water. It crystallises from glacial F. S . I(.ORGANIC CHEMISTRY. 61 acetic acid i n long, colourless, moss-like needles, melts a t 213-214", and is readily soluble in hot alcohol or glacial acetic acid, but only sparingly in the cold solvents and in dilute acids ; it is readily soluble in concentrated acids, but is reprecipitated on adding water.When treated with chlorine in chloroform solution, it yields a yellow powder, probably tetrachloroketoquinoline, which melts a t 175" with decomposition, and is recoiiverted into trichlorhydroxyquinoline when boiled with alcohol. When heated with sodium carbonate, it yields a sodium-derivative melting a t 270". The potassium-derimtive is c r p talline. The hydrochzoride crystallises in small, yellow needles. The p latinochzoride, ( C,NH4C130) %, H2Pt C1, + 2 H,O, crys t allises from dilute hydrochloric acid in long, orange needles and loses its water at 140-150". The acety2-derivative separates from a mixture of glacial acetic acid and acetic anhydride in thin, transparent, forked, efflore- scent crystals, melts a t 172-173", and is readily decomposed.Tricli Zoroketoquinoline hydrochloride, C,NH40C13,HC1 + 2H20, pre- pared by saturating a well-cooled glacial acetic acid solution of hydr- oxyquinoline with chlorine and washing the product with glacial acetic acid, is very unstable, hygroscopic, and sensitive t o light. When simply dried between blotting paper, it melts at 93-95" to a yellow liquid which decomposes a t 100-120" with evolution of gas and then solidifies, melting again at 170-1 80" with decomposition. When dried over sulpburic acid under reduced pressure, it does not begin to decompose until heated a t 160" and melts at 180". It is readily soluble in moderately dilute hydrochloric acid, but when the solution is evapo- rated under reduced pressure dichlorhydroxyquinoline separates.14, is decomposed when warmed with solvents, generally with forma- tion of the dichlorhydroxy-derivative, and this substance is formed very readily when the keto-derivative is reduced with hydrogen sodium sulphite. The platinochloride is very readily soluble, and when the solution is boiled or evaporated under reduced pressure, a mixture CO*CCl, of platinochlorides is obtained. The free base, C,NH,< CCl:CH >, obtained by decomposing the hydrochloride with water and extracting the precipitated oil with ether, crystallises in long, thin, yellow prisms or needles, melts a t 9So, turns brown a t 130", and is completely decomposed a t 170". It is readily soluble in benzene, alcohol, and glacial acetic acid, and does not decompose when kept.EthoxydichZor7~ydroxyqzlinoZine, OEt*C,NH,Cl,*OH [OH : C1, : OEt = 1 : 2 : 4: 1'3, is formed, together with dichlorhydroxyquinoline and a small quantity of the trichloro-derivative, when an alcoholic solution of freshly prepared trichloroketoqninoline is boiled for 1-2 hours. It crystallises from alcohol or benzene in long, thin, colourless needles, melts at 150-151", and dissolves sparingly in most ordinary solvents in the cold but readily on warming. It is soluble in acids, forming colourless solutions, from which i t is reprecipitated by water, and when warmed with alcoholic soda, it yields a solution from which a spongy sodium-derivative separates on cooling. Dihydroxydzchloroquiizoline, [(OH), : C1, = 1 : 1' : 2 : 41, is ob- tained, together with ethyl chloride, when the preceding compound is heated a t 110-120" with concentrated hydrochloric acid; it is also62 ABSTRACTS OF CHEMICAL PAPERS.formed when trichloroketoquinoline is boiled with methyl alcohol. It crystallises from alcohol in needles, melts atv 278", and is more sparingly soluble than the chloro-derivatives of hydroxyy uinoline. It crystallises from methyl alcohol in efflorescent needles containing alcohol. Anilidoquinolinequinoneani lide, C,NH,< C'O*C(NPh)- d (NH ,:cEI>, is ob- tained by treating an alcoholic solution of the ketochloro-derivative with excess of aniline. It crystallises in small, golden plates or long needles, melts a t 222", and shows all the properties of a feeble base. It is moderately soluble in glacial acetic acid, sparingly in alcohol, insoluble in water, and dissolves in dilute acids with a bluish-violet coloration.It is not changed by boiling with alcohol or concentrated potash, but is readily decomposed when heated with acids, yielding. a, yellow, crystalline substance which was not, obtained in the pure state. The hydrochZoride crystallises from acidified alcohol in small, dark- golden needles and is unstable. The yicrate crystallises from alcohol in dark, copper-red needles. The acetate crystallises in needles, melts a t 19Y", and is decomposed by water. Pentach loroketopuinoline platinochloride, (CJ H,Cl,O) 2, H,Pt Cl,, is formed when trichloroketoquinoline hydrochloride (5 grams) is heated at 140-150" for six hours with manganese dioxide (35grams) and concentrated hydrochloric acid (18 grams), the resulting solution filtered and mixed with platinic chloride.It is a yellow, crystalline compound, and when recrystallised or dried, it seems to lose hydro- gen chloride and be convei-ted into the salt of tetrachloroketoquinoliae. A solution of pentachloroketoquinoline hydrochloride yields trich lor- bydroxyquinoline when mixed with water or hydrogen sodium sulphite. F. S. I(. Alkaloids from Papaveraceae. By E. SCHMIDT (Arch. Pharm. [ 3 ] , 26, 622-623).-The following abstract is the first of a series on these alkaloids, giving the results of investigations undertaken a t the instance of the author. Schiel's conclusion that chelerythrine and sanguinarine are identical is not confirmed. The former appears to have the formula CI9Hl7N04, as deduced from the analysis of the small quantities obtained, whilst the latter, from the analysis of various compounds, has the formula, CI7Hl5NO4, thus confirming Naschold's result.Three more bases have recently been separated from Chelidonlum majus which are now the subject of research. Chelidonine. By A. HENSCHKE (Arch. Pharm. [3], 26,624-644 ; compare Abstr., 1887, 854) .--The alkaloi'd was obtained partly by recrystallisation of the commercial base, and partly by direct extrac- tion from the root of CheZidoriiunz rnajus. Probst's method of ex- traction was employed, the stamped root being boiled in water acidified with sulphuric acid, ammonia in excess added, and the filtrate dried. This was purified by treatment with acidified alcohol, and again with ether, and finally was repeatedly crystallised from boiling alcohol.Chel idonine, CzoH19N05 + HzO, forms vitreous, tabular, colour- less, monocliuic crystals of about 3 mm. diameter. The reactions of J. T.PHYSIOLOGICAL CHEMISTRT. ti3 the base are given in detail. Solutions of the salts of this base have an acid reaction, and tlie hydrochloride has the formula C,,H,,NO,-HCl ; the nitrate, C,,HlgN05,HN03; the sulphate, C20H19N05,H2SO~ + 2H20 ; the platinochloride, (C20H,9N05)2,H2PtC16 + 2H20 ; this was not, ob- tainable in a crystalline form ; the aurochloride, C2,,H,,N05,HAuC14, is easily obtained in crystals. Ethyl iodide combines with the base, and the compound is not acted on by potassium hydroxide ; these and less positive results lead to the conclusion that chelidonine is a tertiary base.By oxidation with potassium permanganate in alkaline solution, chelidonine yields oxalic acid, methylamine and ammonia, the latter resulting from the decomposition of methylamine. In acid solution, the oxidation goes further, carbonic anhydride and methyl- amine resulting. J. T. Alkaloids from Cod-liver Oil. By A. GAUTIER and L. MOURGUES (Compt. rmd., 107, 626-629 ; compare Abstr., 1888,1325) .-Aselline, C25H32N4, is an amorphous, colourless solid which becomes green on exposure to light. It melts to a viscom, yellowish liquid with an aromatic odour recalling that of the ptomaines, is very slightly soluble in water, to which it imparts a bitter taste and an alkaline reaction, but dissolves in ether and still more readily in alcohol ; sp.gr. about 1-0,5. The salts of aselline crystallise readily, but are partially de- composed by water. The mercurochloride crystallises from warm water ; the aurochloride is very easily reduced ; the platinochloride is orange-yellow, and dissolves in warm water, but is decomposed by boiling water. Aselline is feebly toxic, and produces fatigue and stupor; 3 mgrms. of the hydrochloride killed a greenfinch in 14 minutes. Morrhuivae, C19H2,N3, is separated from aselline by taking advantage of tlie greater solubility of its platinochloride. It is a thick, oily, amber-coloured liquid with an odour which recalls that of aselline, and is only slightly soluble in water, but more soluble in alcohol and ether. It is caustic and strongly alkaline, and absorbs carbonic anhydride from the air.The hydrochloride is very deliquescent ; the aurocbloride is yellow, and dissolves in warm water; the platino- chloride is somewhat soluble and crystallises in needles. Morrhuine constitutes one-third of the total bases in the oil, and an ordinary dose of one fluid ounce contains 2 milligrams. It excites the appetite and has remarkable diaphoretic and diuretic properties. In large doses it produces fatigue and stupor. C. H. B.ORGANIC CHEMISTRY. 29Organic C h e m i s t r y .Isoallylene. By G. GUSTAVSON and N. DEMJANOFF (J. p r . Chem.[Z], 38, 201--207).-1soallylene may be prepared by the action ofzinc-dust on an alcoholic solution of dibromopropylene. The latter,best obtained by the action of potassium hydroxide on tribromhydrin,is allowed to drop slowly into the warm mixture of zinc-dust and$0 per cent.alcohol, contained in a flask. The isoallylene evolved is* 100 00 in the original paper80 ABSTRACTS OF CHEMICAL PAPERS.collected over water, in wliich it is very little soluble. 10 grams ofdibromopropylene yield 900 to 1000 C.C. of the gas,IsozLZZyZene is ;I colourless gas, smelling like normal allylene; itburns with a skrongly luminous flame, and gives 110 precipitate withammoniacal cuprous chloride or silver nitrate. With aqueous solu-tions of mercuric chloride or sulphate it gives a white precipitate.The gas from 10 grams of dibromopropylene was absorbed by35 grams of bromine, the unaltered bromine dissolved in sodiumhydroxide solution, and the colourless oil washed with water.Itweighed 17 grams, the calculated yield being 18 grams, and had theformula C3H4Br4. IsoaZZyZene tetrabromide smells of camphor, and hasthe sp. gr. 2.729 at 0" and 2.658 a t 18" (water a t 0" = 1) ; it solidifieswhen cooled to -18", and melts below 0" ; a t the ordinary pressureit distils between 215" and 230" with partial decomposition. Normalallylene tetrabromide has the sp. gr. 2.690 a t 0" and 2.652 at It;",and does not solidify in a freezing mixture. That the two are notidentical is conclusively proved by the fact that by the action of zioc-dust isoallylene is liberated from the one, and normal allylene fromthe other.On heating sodium with an ethereal solution of isoallylene in a sealedtube st loo", the sodium is converted into a white powder, whichevolves normal allylene when treated with water. Pavorsky hasshown that this conversion of iso- into normal hydro-carbons by theaction of sodium, is characteristic of the homologues of acetylene.When passed into strong sulphuric acid, isoallylene is absorbed,and on dilution with water and addition of potassium hydroxide,acetone separates ; this is a strong argurnent in favour of isoallylenebeing dirnethyZenemethane, CH2:C:CH2, thus (1) CH2:C:CH2 + 2H2S04+ 2H2SOa.If this is the case, the dibromopropylene from whichisoallylene is obtained must be CH2Br*CBr:CH2, and isoallylenetetrabromide must be CH2Br.CBr2*CH2Br.= CH,*C(HS0,)2*CH3; (2) CH,*C(HSO,)2*CH3 + H2O = CH,.CC)*CH,A. G. B.Cyanurates.By A. CLAUS and 0. PUTENSEN (J. pr. Chem. [2],38, 20&-229).-The amethyst-coloured crystals, obtained whencyanuric acid is mixed with ammoniacal copper sulphate, have thecomposition ( C3N303H2),Cu,2NH3. By digesting them with diluteammonia, violet needles of the composition ( C3N30,H2)2Cu,3NH3 areobtained, and if strong ammonia is used a deep blue compound,(C3N303H2)2C~,4NH3, is formed ; but this last is very unstable,rapidly losing ammonia in the ail.. When the first of these ammoniacalcopper cyanurates is digested with water, a basic copper cyanurate,C,N,O,(Cu*OH), + 3H20, is formed. An acid copper cyanurate of thecomposition ( C3Nd03HL)2C~,C3N303H3,NH3 + H20 is formed whencopper carbonate is digested with cpanuric acid and ammonia. Thesalt, C3N303HCu + 3H20, is precipitated when sodium cyanurate isadded to copper sulphate ; and normal copper cyanurate, (C,N,O,),Cu, + H,O, crystallises when acid magnesium cyanurate is mixed withcopper sulphate.The following cyanurates are also described : Acidmagnesium cyanurate, ammoniacal cadmium cyanurate, ammoniacalzinc cyanurate, ammoniacal nickel cyanurate, cyanurates of nickelORGANIC OHEMISTHY. 31cobalt, and manganese : tetramethylammonium cyanurate, and furhher,cyanurates of quinoline, quinine, cinchonine, strychnine, narc0 tine, andcaff ehe. A. G. B.Preparation of a-Dibromhydrin. By 0. ASCHAN (Ber., 21,2890-2892) .-a-Dibromhydrin is best prepared as follows :-Phos-phorus tribromide (650 grams) is dropped in quantities of from 10 to20 grams at a bime into pure, warm glycerol (500 grams), the wholebeing well shaken and cooled after each addition of bromide, Theoperation is at an end in from three to four hours.After keepingfor 24 hours, the mixture is heated on the water-bath for about threehours, cooled, diluted with water (3 to 4 vols.), extracted with ether,and the extract washed with sodium carbonate solution and dried.After evaporating the ether, the residual oil is heated at about 200°,and then fractionated ; the portion boiling at 208-218", which con-stitutes about two-thirds of the whole, is finally distilled underreduced pressure. 500 gra'ms of glycerol yield 135 grams of purea-dibromhydrin. The requisite quantities of yellow phosphorus andbromine can be employed instead of phosphorus tribromide.When a-dibromhydrin is treated with nitric acid of sp.gr. 1.48, theprincipal product is a liquid boiling at 78-79' (18 mm.), which con-tains bromine and nitrogen. It forms very stable, yellow, readilycrystallisable salts. F. S. K,Epichlorhydrin. By C. PAAL (Ber., 21, 2971-2973) .-Chloriodo-hydrin methyl ether, C3H5CII*OMe, is obtained by heating epichlor-hydrin (1 mol.) with methyl iodide (1 mol.) at 190°, fractionatingthe product, and removing the free iodine wit,h finely divided si!ver.The yield is about 'LO per ceilt. of the theoretical quantity. I t is acolourless oil with a pungent smell, exceedingly sensitive to light,and miscible with the ordinary solrents excepting water, in which itis insoluble.I t boils at about 200" with partial decomposition, andis readily volatile with steam.Chloriodohydrin etlyl ether, C,H,CiI-@Et, is prepared by heatingepichlorhydrin with ethyl iodide at 200-220", and purifying theproduct as described above. The yield is 30-50 per cent. of thetheoretical quantity . It boils at 200-210" with slight decompositionand resembles the preceding compound.Chloriodohydrin isopropyl ether, C,H,ClI*OPrF, prepared in likemanner, boils at 208-212" with partial decomposition and resemblesthe ethyl ether. The noymai propyZ ether boils at 200-210" withslight decomposition ; it is relatively stable and less sensitive t o lightthan the other ethers which, however, it resembles in other respects.F. 8. I(.Propyl-phycite.By A. 'FAUCONNIER (Compt. rend., 107,629-630).-The action of hypochlorous acid on epichlorhydrin results in thertssimilation of water, most probably because of the acidity of theliquid, and the " propyl-phycite " obtained by Carius by saponifyingthe product of this reaction, and described by him as a lower homo-logue of erythrol, is in reality ordinary glycerol. C. H. B32 ABSTRACTS OF CHEMICAL PAPERS.Molecular Weight and Valency of Perseite. By MAQTJENNE(Compt. rend., 107, 583-586) .-When perseite is treated with boil-ing hydriodic acid, it is partly converted into resinous products ofindefinite composition, and partly into a volatile liquid which can beseparated into two fractions boiling at 100-110" and 133-200"respectively. The first is a heptine, isomeric with oenanthylidene,which boils a t 102-105" after rectification over calcium oxide andover sodium ; sp.gr. at 20" = 0.78. The second fraction is a dense redoil with a slight ethereal odour. It boils at 192-196" under ordinarypressure, and at 02-35" under a pressure of 40-50 mm., but decom-poses to a considerable extent even when distilled in a vacuum. Itconsists mainly of heptyl iodide with a small quantity of heptinehydriodide.The dibenzok acefal of perseite, C,,H2,O7, is obtained by the actionof benzaldehyde on perseite in presence of alcohol saturated withhydrogen chloride. It forms confused, slender, microscopic needleswhich soften at 215", but have no definite melting point, and arequite insoluble in water and almost insoluble in alcohol.ThePe results show that the formula previously attributed to per-seite (Abstr., 1888, 807) is incorrect, and that perseite is really thenext higher homologue of mannitol, and has the formula C,H,,O,. Itis the first instance of a heptahydric alcohol and of a sugar containing7 carbon-atoms.C. H. B.Constitution of the Glucoses. By B. RA~MANN (Bey., 21, 2841-2842).-The author considers that the aldehyde and ketone formulzeexplain the chief reactions of the glucoses, and that the reactionswhich Tollens mentions (KzLrzes Eandb. d. Kohlenhydrate), as incom-patible with the assumption that these compounds are aldehydes donot afford sufficient grounds for changing the formuls.N. H. If.Oxidation of Arabinose with Nitric Acid.By H. KILIANI(Ber., 21, 3006-3009) .--Calcium arabonat'e is obtained in consider-able.quantities when arabinose (1 part) is heated at 35" for aboutsix hours with nitric acid of sp. gr. 1.2 (2 parts), the diluted solutionboiled with excess of calcinm carbonate, filtered, enporated, andmixed with alcohol. This method can be suitably employed for thepreparation of arabonic acid.Calcium trihydroxyglutarate is obtained from arabinose as follows :-Arabinose (1 part) is digested at 35" with nitric acid of sp. gr. 2.2(2.5 parts) ; after the evolution of gas has ceased, the solutionis evaporated until free from nitric acid, the residual syrup dissolvedin water (25 parts), boiled with calcium carbonate, and the hot solu-tion filtered. The sparingly soluble, red calcium salt which separatesis spread on porous plates, and by concentrating the mother-liquor,separating the salt, and repeating the process several times, 40-45per cent.of the weight of the arabinose employed is obtained in theform of calcium trihydroxyglutarate. It is very similar to calciumsacchnrate in appearance and in its behaviour when heated withwater. The potassium salt, C5H607K2, crystallises in large, colourless,monoclinic plates or prisms, is readily soloble, and is not converteORGANIC CHEMISTRY. 33into the acid salt when the aqueous soIuttion is evaporated with aceticacid. Lead acetate and silver nitrate produce white precipitates inan aqueous solution.TrihydrozyLglutzLric acid, C5H807, obtained by decomposing thecalcium salt with oxalic asid, crystallises from alcohol in colourless,microscopic plates, melts a t 127", and does not reduce Fehling's solu-tion.The normal ammonium salt crystallises in slender needles andis very readily soluble.By F.MBYER (Ber., 21, 2883-2t390).-~rLnzeth~Zenetrinitrosamine, C3H6N6O3,is obtained when an ice-cold solution of hexamethyleneamine (1 part)in water (40 parts) is mixed with ice-cold, dilut,e (If per cent.)hydrochloric acid, and a solution of sodium nitrite ( 2 i parts) in asmall quantity of water immediately added. After about, 15 minutes,the yellowish, crystalline substance which separates at the surface istlirown on to a filter, washed with cold water, and dried on porousplates. The yield is 50 to 60 per cent., or more, of the aniineemployed.It crystal!ises from boiling alcohol, in which it ismoderately soluble, in small, yellowish, silky needles or prisms, meltsat 105--106", and is readily soluble in cold acetone, but onlymoderately so in warm benzene, chloroform, and ether, and insolublein light petroleum. It dissolves unchanged in cold glacial acetic acid,and the molecular weight determined by Raoult's method was foundt o be 196. On exposure to moist air, the crystals lose their silkyappearance, and when treated with cold water, a slight evolution ofnitrogen occurs. It melts under boiling water to a yellowish oilwhich gradually dissolves with evolution of nitrogen, and the solutioncontains formaldehyde. The same decomposition takes place, butmuch more quickly, when it is warmed with glacial acetic acid ordilute acids, but the decomposition into formaldehyde and nitrogen isnot quite quantitative, as traces of ammonia are formed a t the sametime.When heated in a capillary tube, or when treated with con-centrated acids, i t is immediately decomposed with evolution ofnitrous fumes, and when heated on platinum foil it explodes. Itgives Liebermann's reaction. The filtrate obtained in the prepara-tion of this cornpound contains unchanged hexamethyleneamine ; if,however, the mixture is kept for R long time before separating thenitrosoamine, the latter is decomposed into formaldehyde and nitro-gen, and some of the hexamethylenearnine is converted into form-aldehyde and ammonia.Dinitrosopentamethylenetetramine was obtained by gradually add-ing dilute hydrochloric acid to a solution of hexamethyleneamine andsodium nitrite (compare Griess and Harrow, Abstr., 1888, 1268).Itmelts a t 202--203", arid gives Liebermann's nitroso-reaction.F. S. I(.Action of Nitrous Acid on Hexamethylenearnine.F. S. K.Identity of Putresine and Tetramethylenediamine. By L. V.UURBNSZKY and E. BAUMANN (Bey., 21, 2938-2941).-A direct com-parison of the dibenzoyl-derivatives of putresine (Brieger), tetra-rnetlhylenediamine, and the compound obtained by the authors fromYOL. LVt. 34 ABSTHACTS OF GHEMICAL PAPERS.the urine of a patient suffering from cystinuria (compare Abstr.,1888, 1296), proved that these bases are identical.Concentrated solutions of guanidine, creatine, creatinine, and similarcompounds give a precipitate with soda and benzoic chloride, whereasno separation occurs in solutions containing less than 0.5 gram of thebases ; it is therefore necessary that when benzoic chloride is used asa reagent for diamines (Zoc.cit.) only very dilute solutions of thelatter should be employed.By W.R. ORNDORFF and H. JESSEL (Amer. Chern. J., 10, 363--367).-Liebigstated that acetone could advantageously be substituted for alcohol inthe preparation of chloroform ; this statement has been contradictedby Siemerling,.yet chloroform is now largely made from acetone. Ina number of trials, the yield was 166 to 173 per cent. of the weight ofthe acetone used, and the residual liquors contained considerable quan-tities of calcium acetate.The reaction is represented by 2CO(CH,)z + GCaOCl, = SCHCl, + 2Ca(OH), + XaCI, + Ca(CH,*COO),.Liebig states that calcium carbonate is precipitated during the reaction,but the precipitate is calcium hydroxide. Acetophenone similarlytreated with blenching powder, yields chloroform, calcium hydrate, andcalcium benzoate. H. B.F. S. K.Decomposition of Acetone with Bleaching Powder.Dinitrosoacetone. By H. v. PECHMANN and K. WEHSARG (Ber.,21, 2989-2993) .-When dinitrosoacetone (compare Abstr., 1887, 28)is boiled with water or acids, it is decomposed into carboiiic anhydride,hydrogen cyanide, water, and ammonium hydrogen oxalate ; but whenit is heated with glacial acetic acid, oxamic acid, melting at 210°, andhydrogen cyanide are formed.Trinitrosopropnne, NOH:CH*C(NOH)*CH:NOH, prepared by heat-ing a, mixture of dinitrosoacetone (1 mol.), hydroxylamine hydro-chloride (1 mol.), sodium acetate (1 mol.), and water at 50-60' for1 to 2 hours, separates from hot water in the form of a colourless,crystalline powder melting a t 171" with sudden decomposition.Itis only sparingly soluble in ether, but readily solubIe in alcohol, fromwhich it crystallises in needles, and it, dissolves slowly, but in con-siderable quantities, in hot water. It behaves like dinitrosoacetonewhen heated with dilute acids, but its aqueous solution can be boiledfor a short time without decomposition taking place. Ferric chloridegives a brownish-red coloration with a dilute aqueous solution ;ferrous sulphate produces a wine-red colour, and the solution thengives a violet precipitate with soda.Dinitrosoacetone hydrazone, NOH: C H-C (N,HPh) CH :NOH, pre-pared by treating dinitrosoacetone (1 mol.) with phenylhydrazine(1 mol.) in hot, alcoholic solution, crystallises in yellow needles, meltsa t 145" with decomposition, and is readily soluble in alcohol andether, more sparingly in benzene and light petroleum, and insolublein water.It dissolves in alkalis with a yellow, and in concentratedsulphuric acid with an orange-yellow coloration. The metyZ-deriv%tive, C9H9N4O2Ac, a light yellow, crystalline compound, melts a t133", and is soluble i n dilute alcohol. It dissolves in alkalis with ORGIAKIC CHEMISTRY.35yellowish coloration, but the soliltion becomes colourless on boiling,md on adding acids, a compound, C,H8N*0, is precipitated in shining,colourless needles. This substance is also formed when the acetyl-derivative is boiled with water. A compound, C,,H,,N,, is obtainedwhen dinitrosoacetone is beaked with excess of phenylhydrazineacetate. It crystallises from hot alcohol or benzene in shining, yellowplates melting at 122". It is not acted on when boiled with ferricchloride, and its solution in concentrated sulphuric acid does not givea coloration with this reagent.Sulphoisovaleric Acid. By G. DE VARDA (Chew,. Ceiztr., 1888,587-888, from Rend. Acad. dei Lincei [4], 4, 1).-100 parts ofisovaleric acid are mixed with 100 parts of chlorosulphonic acid, and,after the spontaneous reaction has ended, the mass is heated to 230" ;it is then diluted with several volumes of water, and distilled from theoil-bath until the distillate no longer has an acid reaction. The distil-late is then heated with plumbic carbonate for some time, filtered whilehot, and the lead precipitated from the solution by hydrogen sul-pbide, the solution of the free acid being concentrated in a vacuum.Theaqueous solution partly decomposes when heated on the water-bath.The lead salt, C6H,S0,Pb.'LHz0, crystallises from water in colourless,odourless, small plates, which taste sweet ; they are slightly soluble inwater, and insoluble in alcohol, ether, and chloroform.The bariumsalt, containing 1 mol. HzO, forms small, tabular crjstals, withoutsmell o r colour, and taste bitter.It is soluble in water, insoluble inalcohol, ether, and chloroform.F. S. K.Su7phoisowaZeric acid so obtained forms deliquescent crystals.J. W. L.Constituents of Cocoa Fat. By P. GRAF ( A d . Pharm. [3], 26,830-846 ; comp. Kingzett, Trans., 1878, 38).-l1he melting point ofvarious samples of commercial cocoa butter from widely differentsources was determined both in open and closed glass tubes. In theopen tube, the results varied from 29" to 33-44', whilst in the closedtube 11 samples gave 34.3" and one 33.5". The whole of the sampleswere mixed together for the further investigation. The €at wasfound to contain hardly any free acid. Two determinations ofglycerol averaged 9-59 per cent.A little cholesterin and smallquantities of formic, acetic, and butyric acids were detected. Afterthe separation of oleic acid, the solid fatty acids were isolated byfractional crystallisation, followed by Heintz's method of fractionalprecipitation by means of magnesium and barium acetates. Noacid with a higher molecular weight than arachidic acid was found ;this confirms Traub's statement that he was unable to find theohromicacid asserted to be present by Kingzett. The presence of oleic,stearic, and palmitic acids was confirmed ; and either lauric acid o rone of its isomerides was isolated : there was not sufficient materialat hand to settle this point. J. T.Action of Hydrogen Phosphide on Aldehydes and KetoneAcids.By J. MEESINGER and C. ENGELS (Ber., 21,2919-2928).-The compound obtained by passing hydrogen phosphide and hy-d 36 ABSTRACTS OF CHEXICAL PAPERS.drogen chloride into an ethereal solution of pyruvic acid has theconstitution P(CMe<C0>)3, and is named by the authors phos-iUhorus-trianhyd~o~yru~ic acid (compare Abstr., 1888, 441). It is in-soluble in cold acids, and on heating, decomposition takes place.It dissolves in warm, glacial acetic acid, and separates unchanged oncooling. It is not acted on by bromine even a t 150", but whenboiled with water it is decomposed into pyruvic acid and hydrogenphosphide.0Phospho1.zks-trihydroplll.uvic acid hydrazide,P[ CMe(OH)*C(OH):N,HPh],,is formed when the preceding compound is warmed with phenyl-hjdrazine in alcoholic solution ; it is a colourless, crystalline com-pound, melts a t 132", and is moderately soluble in alcoholic ether, butonly sparingly in cold alcohol, and almost insoluble in ether.Hy drazonepyruvic acid hydyazide, Cl5'EIZI6N40, is formed , togetherwith hydrogen phosphide, when phosphorustrianhydropyruvic acidis heated with excess of phenylhydrazine, in which i t is readilysoluble. It crys tallises from hot alcohol in colourless, shining plates,melts at 162", and is only sparingly soluble in cold alcohol and ether.Phosphorus-t,.ihyclro~yruvic acid dianilide,is obtained when aniline is gradually added to an alcoholic solution ofphosphorus-trianhydropyruvic acid.It separates from warm alcoholin colourless crystals, melts a t 158", is very sparingly soluble in coldalcohol and insoluble in water or ether.It is completely decom-posed, with separation of phosphorus, when treated with hydrogenchloride in alcoholic or ethereal solution.Dihy dyazonepy rzsv ic acid hy drazide, NP h (C 0-CMe: X2H Ph), , is formedwhen the preceding compound is treated with phenylhydrazide. Itcrystallises from alcohol in small needles melting at 169".Phosphorus-trianhydropyruvio acid and toluylenediamine yield acrystalline compound, CQHgOGP 3- 2C6H3Me(NH2),, which melts at178" with decomposition.Hydrogen phosphide, in presence of hydrogen chloride, has noaction on ethyl acetoacetate or benzoylcarboxylic acid, but tribromo-pyruvic acid absorbs the gas in considerable quantities with evolutionof hydrogen bromide and the ultimate formation of phosphorus-fri-anhydropyruvic acid.3'. S. K.Action of Heat on Tartaric Acid in Aqueous Solution. B.7 E. M. WEDARD (Chenz. Centr., 1888, 889, from Atti. R. Acad. Scz.Torino, 6, 65-67).-The author noticed that when tartaric acid hadbeen heated for several days in sealed tubes with ferrous sulphate,several of the tubes exploded violently, and in the others a consider-able quantity OE carbonic anhydride was found. As the ferrous salthad not become oxidised a t all, the reaction had not been a simplereduction of the tartaric acid. Tartaric acid heated with water aloneat 150" in sealed tubes also suffered a considerable loss of carboniORQANIC CHEMISTRT. 37anhydride. In one experiment, the author opened the tube afterheating, allowed the carbonic anhydride to escape, then sealed itagain, and submitted the contents to a further heating, and repeatedthe operation until no further evolution of carbonic anhydride tookplace, after which the resulting liquid was found to contain pyro-tartaric acid along with undecomposed tartaric acid.Freezing Points of Solutions of' Aluminium Alkyls.By E.LOUISE and L. Roux (Cowpt. rend., 107, 600--603).-Pure ethylenebromide was used as a solvent, the molecular reduction, T, with thisliquid being 118. The number obtained with mercury propyl was124.8 ; mercury isobutyl, 122.7 ; mercury isoamyl, 123.6 ; mercuryphenyl, 120.4.Aluminium ethyl gave a molecular reduction of 115.6, which agreeswith the formula A1,Et6.Alunzinium proyy2, obtained by the action of aluminium onmercury propyl, is a colourless, mobile liquid, which boils a t 250" andtakes fire in contact with the air.Aluminium isoam!jl, obtained in asimilar way, is a somewhat viscous, colourless liquid, with an odourof amyl compounds ; it boils at 250" under a pressure of 80-100 mm.,and does not readily take fire in contact with the air. The molecularreduction with aluminium propyl is 92.8, and with aluminium iso-amyl 84.5. These values agree more closely with the formula A]&,than with AIRs, and hence confirm the conclusions deduced fromJ. W. L.vapour-density determinations (Abstracts, l8S8, 583).C. H. B.Substituted Pyromucic Acids. By H. B. HILL and A.W.PALMEK. (Amer. Chen?. J., 10, 375--391).-With the exception of asulphopyromucic acid briefly described b r Schwanert, no furf uran-derivatives containing the sulplionic group are described ; yet thegeneral behaviour of pyromucic acid is similar to that of benzoic acic1.6- Sulphopyromucic acid is readily formed bay treating pyromucic acidwith fuming sulphuric acid. The acid itself is extremely soluble inwater, but may be obtained in large, deliquescent crystals. The follow-ing salts are described : RnC,H2S06 + 4H20 ; Ba( C5&SO,)a + 4H20,and also with 6H,O; CaC,H,SO, + 3H20; PbC,H,SO, + 2H20, allreadily soluble in hot water; Ag,C5H2S06 is sparingly soluble inwater; K,C5H,S0, + 4x20 ; KC,H,so, ; Na,C5H,S06 4- 5H20, andNaC&SO, + H20, all very soluble, All these salts crjstallisereadily.By treating the dry sodium salt with phosphorns penta-chloride. and the resulting viscous oil with ammonia, the crystalline6-suZphopyromucal.riide, C,H,SO,(NH,),, is obtained ; it is readilysoluble in hot water, and melts a t 213'. The dry acid is only decom-posed by bromine at loo", dibromosuccinic acid and other productsbeing formed ; in aqueous solution the acid is mainly converted intofumaric acid. Dilute nitric acid oxidises i t slowly, and also producesfumaric acid and some oxalic acid ; concentrated nitric acid at 100"readily converts it into Klinkhardt's 8-nitropyrom ucic acid, and att h e same time a neutral substance, in all probability aa-dinitro-furfuran, is formed.Although bro,nine-derivatives of 8-sulphopyromucic acid camot b38 ABSTRACTS OF CHEMICAL PAPERS.obtained by the action of bromine, they may be obtained by sul-phonating the corresponding bromopyromucic acids : P-Hromo-6-sulyhopyromucic acid is extremely soluble in cold water, and formsdeliquescent crystals. The salts-BaC5HBrSo6 + 4H20; CaC5HBrS06 + 6H,O ; PbC5HBrS06 + 4H,O ;K,C5HBrS0, + 1+H20 (2)are described ; they are all crystalline and soluble in water. That theacid is really a derivative of 6-sulphopyromucic acid is proved byobtaining this acid by treatment of the bromo-acid with zinc andammonia. Bromive in aqueous solution readily converts the bromo-acid into monobromofumaric acid.Concentrated nitric acid readilyyields P-bro.uno-~-nitropyronzucic acid, soluble in water, alcohol, &c.,and melting at 159-160".8-r-Dibromo-6-su~h(~~~omucic acid is prepared by dissolving /3-y-di-bromopyromucic acid in fuming sulphuric acid, b u t it is more advan-tageous to use the mixture of P-61- and /3-6-dibromopyromucic acidsresulting from the decomposition of the tetrabromo-acid, as thep-8-dibromo-acid is but little acted on by the sulphuric acid.Tbeacid in question is very soluble in water, and is crystalline; thefollowing salts are described: BaC,Br2S06 + 5H20 and also with3&O; PbC,Br2S06 + 4H20 ; AgzC,Br,So6 4- HzO ; K2C5Br2SO6 + H,O.That the sulphoriic acid occupies the 8-position, the only pos-sible one, is proved by treatment of the above barium salt withzinc-dust and ammonia, when the a-sulphopyromucic acid firstdescribed is obtained.Bromine in aqueous solution readily oxidisesthe barium salt, giving barium sulphate and dibromonialeic acid.Dilute nitric acid oxidises it to dibroruosuccinic acid. Concentratednitric acid yields a mixture of P-ri-dibromo-8-nitropyrornucic acid,crystallising from water in sparingly soluble, slender, yellow needles,that melt a t 204- 205", and /3/3-dibromo-aa-dinitrofurfuran, a substancemelting at 150-151" and crystallising from benzene, as the compoundC',Br2(NO,),O,C6H6, which readily gives off this benzene of cqstal-lisation. H. B.Metadiethylbenzene. By A. VOSWINKEL (Ber., 21,2829- 2831).i7.letudiethyZbeiizene, C6H4Et2, is obtained, together with the para-compound, by the action of ethyl bromide and aluminium chloride onbenzene ; the two compounds are separated from each other by meansof the barium sulphonates.It boils a t 181--182", and does notsolidify a t -20", but bccomes thicker. Sp. gr.. = 0.8602 at 20" com-pared with water a t 4". When boiled with dilute nitric acid, ethyl-benzoic and isophthalic acids are formed. The barium sulphonate(with 3 mols. H,O) crystallises in hemispherical groups of prisms,rather sparingly soluble in cold water. The coppr saZt (with 4 mols.H,O) forms bright-blue plates of a satiny lustre ; the potussium salt(with 1 mol. H20) crystsllises in quadratic plates. The sulphor~arnideseparates from the dilute alcoholic solution in long, flat needles,melting a t 101-102". The bromir~e-derivatii.e, C6H3Et2Br, boils atabout 238".The teirnbromo-compciund, C6Et2Br4, crybtrcllises fromalcohol in small, colourless prisms melting a t 74". Nat,ometuJ!iefhyZ-btlzneiie, C,B,Et,*NO2, is a pale yellow liquid, which boils aORGANIC CHEMISTRY. 39280-285", with decomposition. The trirdro-compound, CsHEt,(NO,)-,crystallises from light petroleum in prisms melting at 62". A;mido-metadiethylbenzene, C6H3Et2.NHa, prepared by reducing the nitro-derivative, is a colourless liquid which distils readily with steam ; thehydrochloi-ide crystallises in groups of very long needles ; the acetyl-derivative forms stellate groups of needles melting at 104". Metadi-ethyZphenoZ, C6H3Et2*OH, is obtained by fusing the sulphonic acidwith potash ; it boils at 225", and dissolves spariugly in water ; thesolution gives a blue-violet colour (which changes to green on addingalcohol) with ferric chloride.Zeta-ethylbenzoic acid, C6H4Et.COOH,crystallises in long needles, melts a t 47", and is almost insoluhle inwater. The calcium salt (with 4 mols. H,O) forms lustrous needles,readily soluble in water and alcohol.Synthesis of Consecutive Tetramethylbenzene. By 0.JACOBSEN (Ber., 2 1, 282 1-28 28) .-Dinitro bromopseudocumene,N. H. M.[(N02)2 : Br : Me3 = 5 : 6 : 2 : 1 : 3 : 41,obtained by the action of nitric and sulphuric acids on bromopseudo-cumene [Br : Mes = 2 : 1 : 3 : 41, crystdlises from hot alcohol insmall, yellowish-white, lustrous prisms, melts a t 182", and dissolvesreadily in hot benzene, sparingly in hot alcohol.Bromopseudocumene, [Br : Me, = 2 : 1 : 3 : 41, has the same boilingpoint as the 5, 1, 3, 41 compound: 237-238" (not 226-229").Thesulphonamide nielts at 185" (not 137-188"; compare Kelbe andPathe, Her., 19, 1546).1, 2, 3, 4-'l'ctramet,hylbenzene is prepared by heatiiig pure bromo-pseudocumene (25 grams), methyl iodide (40 grams), and sodium(14 grams), in presence of sufficient absolute ether to cover the latter.After two or three days, it is distilled. The yield of tetramethyl-benzene is 38 per cent. of the weight of the bromopseudocumene.Dibromonietnzylene, [Me, : Br2 = 1 : 3 : 2 : 41, is obtained in thepreparation of spinietrical dibromometaxylene by brominating thehydrocarbon ; it is an oily liquid which, when cooled, solidifies to a hardcrystalline mass melting a t -So, and boils a t 269" under 760 mm.pressure.The di~itro-deri~atiwe forms a1 rriost colourless, microscopiccrystals, melts a t 191", and dissolves readily in toluene, very sparinglyin alcohol. When exposed to light it becomes yellow. The sodiumsulphowie, C6HNe,Br,*S03Na + H,O [= 1 : 3 : 2 : 4 : 61, crystallisesin groups of needles; the potassium salt with 1 mol. H20 formslustrous plates, sparingly soluble in cold water; the barium saltcrystallises in small prisms. The amide separates from alcohol insmall prisms, which melt with decomposition above 300". When thesodium salt is treated with zinc-dust and ammonia, the salt of ordinaryunsymmetrical metaxylenesulphonic acid is formed.OrthoiZicLmidometaayZene, [Me, : (NH,), = 1 : 3 : 5 : 61, is obtainedby very prolonged action of tin and hydrochloric acid on the dinitro-dibromo-compound, and is liberated from its hydrochloride by drydistillation with sodium carbonate in a stream of hydrogen.It crys-tallises from water in rhombic plates, melts a t 78.5", and dissolvesreadily in alcohol, ether, and hot water. When exposed to moist air40 ABSTRACTS OF CHEMICAL PAPERS.it beeomes grey-violet. The constitution of this compound as given isproved by the synthesis of 1, 2, 3, 4-tetramethylbenzene from theliquid dibromometdxylene by the action of methyl iodide and sodium,using ether as a diluent.When symmetrical dibromometaxylene is heated with sulphuricacid (3 parts) at 240", it is converted into the liquid isomeride.Tetrethylbenzene.By 0. JACOBSEN (Ber., 21, 2819-2821).-Symnretrscal tetrethylbmzene, C,H.,Et, [Eta = 1 : 'L : 4 : 51, isobtained, together with a smaller amount of the isomeride [Et, =1 : 2 : 3 : 41, by the action of ethyl bromide on benzene in presence ofaluminium chloride, at a temperature not above the boiling point ofthe bromide ; the product is sulphonated in the cold and the sodiumsulphonnte heated a t 170" with hydrochloric acid. It melts a t 13",and boils a t 250". When boiled with dilute nitric acid, and theproduct further oxidised with permanganste, pyromellitic acid isformed.Dibromotetrethylbenzene, C,Br,Et, [Et, = 1 : 2 : 4 : 51, crystalliseafrom hot alcohol in long, thin prisms melting a t 112.5".S o d i u m tetreth y1benzenesubphonate, C,H E t,*SO,Na + 4H20, crystal-lises from water in very large, lustrous plates, sparingly soluble incold water, much more readily in alcohol, almost insoluble in cold diluteaqueous soda.The barium salt (with 9 mols. H20) is sparinglysoluble in hot water. The sulphona?~~ide, C14H21.S02*NH2, crystallisesfrom hot dilute alcohol in rhombic plates, melting at 122".Pentethylbenzene and its Decomposition by Sulphuric Acid.By 0. JACOBSEN (Ber., 21, 2814-2819 ; compare Abstr., 1887, 660 ;1888, 137).-PentsthyZbenzene, C,HEt,, is prepared by the actionof ethyl bromide on benzene in presence of aluminium chloride,and purified in a manner similar to the pentamethyl-compound (loc.cit.). I t forms a thick oil, which boils at 277", and does not solidifyat -20".Brornopentethylbe?inene, C,BrEt,, obtained by brominating the hydro-carbon dissolved in glacial acetic acid, crystallises from alcohol inlong needles, melts at 47*5", and boils a t about 315".It is readilysoluble in hot alcohol.The suZphone, SO,( C6Ets),, crystallises from light petroleum con-taining some alcohol in large, transparent, hexagonal prisms of aglassy lnstre, melts a t 76", and is very readily soluble in alcohol, muchless in light petroleum, and insoluble in water.Sodium perdeth y Zb enseisesulphonate, C,,H,,-S 0,Na + 4H,O, crystal -lises from water in thin, lustrous plates, moderately soluble in hotwater, much more soluble in alcohol. The anhydrous salt crystallisesfroin 90 per cent.alcohol in groups of hair-like needles. Thepotccssium salt (with 2 mola. H,O) crystallises in thin plates, ratherreadily soluble in hot water, much more soluble in alcohol. Theaniinonium (with 1 mol. H,O) and barium (with 9 mols. H20) saZfscrystallise respectively in large, thin plates and small scales. Whenpentethylbenzene is treated with an equal volume of sulpburic acidsy much fumiug sulphuric acid added to the cooled mixture thatN. H. M.N. H. M.Sp. gr. = 0.8985 a t 19"ORGANIC CHEMISTRY. 41a clear, brownish-yellow solution is obtained, and the whole kept for4-5 days a t the ordinary temperature, hexethylbenzene and tetrethyl-benzene [Et, = 1 : 2 : 3 : 41 are formed.Hexethylbenzene melts at 229" and boils a t 298".Tetrethylbenzene [Et, = 1 : 2 : 3 : 41 boils a t 254", and does notsolidify a t -20".It is probably identical with Galle's compound(Abstr., 1883, 109 1). The dibronzo-derivative, CsBi.,Et4, crystallisesin prisms of a glassy lustre, melts at 77", and is sparingly soluble i l lboiling alcohol.Barium tetrethylbenxenesdphonate, (C,,EI,,*SO,),Ba + 6H20, crystal-lises from water in flat prisms OF a glassy lustre; the sodium saZt (with5 mols. H,O) forms readily soluble rhombic plates. The amide sepa-rates from its solution in water and alcohol in well-formed crystals ofa glassy lustre, and melts at 107". N. H. M.Synthesis of Aromatic Selenium Compounds. By C. CHABRIF:(Bull. SOC. Chlm., 50, 133-137) .-Phenyl selewide, SePh,, is obtainedby adding aluminium chloride to selenium tetrachloride (I part) andbenzene (3 parts), contained in a reflux apparatus, until no morehydrogen chloride is evolved.The temperature in the flask variesfrom 22' to 27", and the operation is finished in about 60 hours. Itboils a t 227" under a few cm. pressure. Phenyl chloride and an oilboiling at 250" under a pressure of A few cm. are also formed.Selenium oxychloride in presence of aluminium chloride andselenious anhydride, also react with benzene.Consecutive Metaxylenol. By 0. JACOBSEN (Ber., 21, 2828-2829) .-The author previously (Abstr., 1878, 412) ascribed t o con-secutive metaxylenol the melting point 74.5". Nolting isolated thecompound from commercial xylidine, and found the melting pointl49". This melting point is now confirmed by preparing metaxylenolby heating pure parahydroxymesitylic acid ; the product melted a t47-48'.The xylenol previously obtained (Zoc. cit.) was paraxylenol.Nitronitrosoresorcinol. By C:. DE LA HARPE and F. REVERDINN. H. M.N. H. M.(Bull. SOC. Chim., 49, 760-763).-Nitronitrosoresorcil/ol,[OH: NO,: 0 : NOH = I : 2 : 3 : 41,is obtained when a cooled mixture of nitroresorcinol (1 mol.), meltinga t 85", with a solution of soda (1 mol.) in 10 parts of water and anaqueous solution of sodium nitrite (1 or 2 mols.) is gradually addedt o excess of dilute and well-cooled sulphuric acid. The yellow,flocculent precipitate is washed with water, dried over sulphuric acid,and extracted with ether to ~emove traces of nitrosoresorcinol.Itcvystallises from alcohol in brownish needles, and is readily solublein water, acids, and alkalis, but only moderately soluble in alcohol,and insoluble in ether, benzene, and chloroform. It is not changedwhen heated to about 200", but at higher temperatures it deflagratesviolently. It yields diamidoresorcinol (compare Bite, Ber., 8, 631)when reduced with tin and hydrochloric acid. The aqueous solutioiigives an intense green coloration with ferrous sulphate o r with ironfilings, and a slightlly acid solution of the colouring matter, which ca42 ABSTRACTS OF CHEXICAL PAPEkS.be precipitated from the aqueous solution by adding sodium chloride,dyes wool green (compare F h r e , Abstr., 1883, 733). Concentratedsnlphuric acid added to a mixture of resorcinol and nitronitroso-resorcinol? produces a green colour, which changes to blue and t,hen toa dirty violet; from this solution water precipitates brown flocks,which dissolve in alkalis with a greenish-brown coloration.Nitroresorcinol, [(OH), : NO2 = 1 : 3 : 41, melting at 115", doesnot form a nitroso-derivative when treated as described above.Condensation-product of Quinone and Ethyl Acetoacetate.By H.V. PECHMANN (Ber., 21, 3OO5-WO6) .-A Condensation-product,C16H1606, is formed when quinone (1 gram) is heated a t 100" withethyl acetoacetate (2.5 grams) and a 50 per cent. solution of zincchloride (6 grams) in absolute alcohol. It melts a t 184", and is solu-ble i n boiling alcohol or glacial acetic acid, but insoluble in water.The solution in Concentrated sulphuric acid turns deep blue whenheated.It yields crystalline derivatives when treated with bromine,but it is not acted on by phenylhydrazine, benzoic chloride, sodiumethoxide and alkyl iodides, or by boiling hydriodic acid. A crystallinebibasic acid, C14K1,06, is precipitated when the preceding compound ishydrolysed with alcoholic potash and the solution acidified with aceticacid. It sublimes without melting, and is insoluble in all ordinarysolvents. The potassium salt, C,4HloK206 + 2H,O, is a colourless,crystalline, spariugly soluble compound, and loses its water at 125".F. S. I(.Derivatives of Paramidoisobutylbenzene. By C. GE LZER(Ber., 21, 2941-2949, and 2Y49-2961).-l?aracetarnidobromisobutyl-benzene, C4HS*C,H,Br.NHAc, prepared by brominating acetamidoiso-butylbenzene: crybtallises from hot dilute alcohol or benzene in large,shining scales or plates, and melts a t 1.53".It is readily soluble inalcohol, hot benzeoe, ether, carbon bisulphide, and chloroform, butonly very sparingly soluble in boiling water.B~Iiir7obrumi.sobzctylbenzene, C4H,*C6H,Br*NH2, is a heavy,. yellowish,aromatic-smelling oil, boiling a t 264-265" (710 mm.) with decom-position, and volatile with steam ; i t is readily soluble in alcohol, ether,and benzene, b u t insoluble in water. The hydrochloride, CloHI4NBr,HCl,crystallises from benzene in moss-like needles, and is readily soluble inwater, alcohol, and warm benzene, but almost insoluble in ether. Theplatinochloride, (CloH14NBr)2,B ZPtCI6, obtained by precipitating a coldalcoholic solution of the base with a hydrochloric acid solution of platinicchloride, crystallises in slender,.yellow needles, and is readily solublein alcohol, but only sparingly in cold water, and insoluble in ether;it is decomposed when boiled with water. A light yellow, crystallinesubstance, ( CloH14NBr),PtCl,, is obtained when a cold alcoholic solutionof the base is precipitated with a neutral solution of platinic chloride ;it; is sparingly soluble in cold alcohol, and is decomposed when thesolution is heated. The picrate, CloH14NBr,CsH,N,07, separates froma mixture of warm benzene and light petroleum in slender, yellow,spear-shaped crystals, and is readily soluble in cold alcohol, ether, orliot water, but only sparingly in cold water or cold benzene, andmoderately soluble in hot benzene.F.S. ICORQANIC CHEMISTRY. 43Bi-onzisobutylbenzene, C4H,.C6H4Br, obtained by treating the amido-derivative with nitrous acid and distilling the product, is a heavy,slightly yellow, aromatic-smelling oil, boiling a t 231-232" (710 mm.),and only slightly volatile with steam. It is readily soluble in alcohol,ether, and benzene, but irisoluble in water. It yields metanitrobenzoicacid when heated a t 235-240" with nitric acid of sp. gr. 1.15.17letanitroi-cobzLtylbenxene, C4HS*CqH4-NO2, obtained by treating theamido-derivative with nitrous acid, and fractionating the product in apartial vacuum, is a bright yellowish-red, aromatic-smelling oil, boil-ing a t 250-252" (740 mm.).It yields metanitrobenzoic acid whenheated at 200" with nitric acid of sp. gr. 1.12.I~iti-oisobut2/l~henoZ, [C4Hg : NO, : OH = I : 3 : 41, prepared byboiling amidonitroisobntylbenzene with dilute potash and distillingthe product, separates from alcohol in yellowish-red, deliquescentcrystals, melts at 95", and boils at 289-290" (711 mm.) with onlyslight decomposition. It is readily soluble in alcohol, ether, benzene,light petroleum, alkalis, and hot water.Metainidoisobuty lbenzene, C4H9*Cj6H1*NH,, prepared by reducing thenitro-derivative with stannous chloride and hydrochloric acid, is ayellowish oil, boiling a t 229' (708 mm.), and moderately volatilewith steam. It is readily soluble in alcohol, ether, and benzene, b u tonly sparingly in water.It dissolves in a solution of bleachingpowder with a bright riolet colour, and with potassium dichromateand sulphuric acid yields a reddish-violet coloration, which quicklychanges to brown. The hydrochloride, ClOH,,N,HCl, crystallisesfrom hot benzene in colouiless plates, and is readily soluble in aaterand hot alcohol, but only sparingly soluble in benzene. The platino-chloride, ( C,oH,,N)2,H,PtCl,, crystnllises in bright yellow plates, andis readily soluble in boiling water and hot alcohol, but only sparm.glyin benzene and ether. The ozalate, CloH&,C2H204, crysthllisesfrom hot water or dilute alcohol, in which it is readily soluble,in large white plates. The acetyl-derivative, C4Hg*C6H4*NHAc, crys-tallises from boiling water in colonrless, shining plates, melts at 101",and is readily soluble in alcohol, ether, and benzene.n~etacetamidonit,.oisobzctylbenzene, [C4Hg : NO, : NHAc = 1 : 2 : 31,obtained by nitrating the acetamido-derivative, crystallises from hotdilute alcohol in small, yellow needles, melts a t 105*5", and is readilysoluble in alcohol, benzene, and ether, but very sparingly in boilingwater.Ainidonitroisobut?lZbenzene, C4H9.C,H,(X0,)*NH2, separates fromdilute alcohol in bright yellow crystals, melts at 1 2 4 , and is readilysoluble in alcohol, ether, benzene, and boiling water, but sparinglysoluble in cold water.It is only a feeble base, and the salts arereadily soluble.Dia.r.lzidoisoEutyZbenzene, [CIHg : (NH,), = 1 : 2 : 31, prepared byreducing the preceding compound with stannous chloride and hydro-chloric acid, crystallises from alcohol in colourless plates, melts atlog", is readily soluble in water, alcohol, ether, and benzene, andblackens on exposure to the air.The oaalate, (CloH16N,),,C2H204,crystallises in flat needles, and is readily soluble in boiling water, butonly sparingly in cold, ahsolute alcohol, and almost insoluble in ether44 ABSTRACTS OF CHEMlCAL PAPERS.an alcoholic solution of the dinmine is mixed with a glacial aceticacid solution of phenanthraquinone. It separates from hot dilutealcohol in yellow nodular crystals, melts a t 144" with previous soften-ing, and is readily soluble in warm alcohol, ether, and benzene, butonly sparingly in boiling water.It dissolves in concentrated nitric acidwith a brownish-red. in concentrated sulphuric acid with a scarletcoloration, and is precipitated unchanged from both solutions onadding water. U NCPh\N*CPhHBenzilisobuty@hennzitze, C,Hg*C6H,/ I \, prepared in like man-ner from the dinmine and benxil, crystallises in small, light-yellowprisms, melts a t 96", and is only sparingly soluble in cold alcohol, butreadily in ether, benzene, and hot alcohol. It dissolves in concen-trated nitric acid or concentrated sulphuric acid, but is precipitatedunchanged on adding water.AcefLt?nidobromonifroisobuf!llbenzene, C4Hg~C,H,Br(N0,)~NHAc, pre-pared by nitrating acetamidobromisobutylbenzene, crystallises froma mixture of ether and light petroleum in small, rhombic plates,melts at 144O, and is readily soluble in hot alcohol, ether, or benzene,but only very sparingly soluble i n boiling water.Amidobromonitroisobuty Zbenxene, C,Hg*c6H2Br( NO,) .NH2, crystallisesin long needles, melts a t 69*5", boils a t 278-280" with partial decom-position, and is volatile with steam.It is very sparingly soluble inboiling water, but readily in alcohol, ether, and benzene.Diamidobromisobutylbenzene, c4Hg*C6~,Br(N&),, obtained by re-ducing the preceding compound with stannous chloride and hydro-chloric acid, crystallises from ether in slender, colourless needles,melts a t 85*5", and turns brown on exposure to the air. It sublimeswith considerable decomposition, forming colourless needles whichare stable in the air. It is readily soluble in alcohol, ether, andbenzene, but only very sparingly in hot water.Ferric chlorideproduces a brownish-red coloration ; bleaching powder precipitatesoily drops, and platinic chloride gives a brownish-black coloration in ahydrochloric acid solution of t.he base. The oxulate,C1oH15BrNzl CJLO4,crystallises in small needles, and is moderately soluble in boilingalcohol, but only sparingly in ether, benzene, and warm water. Thepicrate, CloHlbBrN2*2, C6H3N307, crystallises from hot water in yellowneedles. and is readilv soluble in alcohol and ether.lises from boiling alcohol in slender? yellow needles, melts- at 153-5",and is readily soluble in benzene, ether, and boiling alcohol, b u tonly sparingly in cold alcohol.It dissolves in concentrated mineralacids, forming red solutions, from which it is precipitated unchangedon adding waterORGANIC CHEJIISTET. 45X*C*Ph\N*C-PhBeiizilbromisobuty ~ h e n a z i ~ e , C4Hg*C,H2BJ I II 3 crystallises fromhot alcohol in colourless needles, melts at 172", and behares towardssolvents similarly to the preceding compound ; it dissolves in (son-cen trated acids with a yellowish-red coloration.Dibi-oniisobutylbenzene, [C4Hg : BrP = 1 : 3 : 51, obtained by heatingmetabromisobutylbenzene with bromine in presence of iodine, anddistilling the product with steam, is a light yellow oil, boils a t376-277" (718 mm.), and is readily soluble in all ordinary solventsexcept water. When heated a t aboxt 250" with nitric acid, sp.gr.1.20, i t is converted into symmetrical dibromobenzoic acid.F. S. K.Decomposition of some Diazo-compounds by Formic andAcetic Acids. By W. R. ORNDORFF (Amer. Che1.12. J., 10, 368-372).-The decomposition of diazo-compounds by formic acid might beexpected to furnish an easier means of displacing the amido-group byhydrogen than the decomposition with alcohol. But the reactionproceeds otherwise and could not be followed out, a9 the phenylformate that was probably formed could not be isolated. Substitut-ing acetic acid for formic acid, it is shown that phenyl acetate is pro-duced ; the yield is, however, small, as milch tar is also formed ; thereaction is analogous to the production of phenetnil by the action ofalcohol.The boiling point of phenyl acetate has been variouslystated; it has been redetermined as 195" at 733 mm. pressure.Similarly, paradiazotoluene sulphate, when boiled with acetic acid,yields paracresyl acetate, boiling a t 213", and identical with that pre-pared from paracresol. Paradiazobenzenesulphonic acid appears toundergo a similar change, and the reaction therefore seems to begeneral. H. B.Chryso'idincarbamide. Amidophenylenecarbamide. By A.JENTZSCH (J. pr. Chem. [ 2 ] , 38, 121-139). -When carbonylchloride is passed into a moderately strong solution of chrysoidinin dry chloroform, it is rapidly absorbed with development of heat,and red-brown flocks separate which become of a darker brown as theaction proceeds. The brown matter is collected, dried, powdered,heated with dilute hydrochloric acid, and filtered hot ; brilliantgolden-yellow laminae crystallise out on cooling, together wit8h octo-hedral crystals of diamidoazobenzene hydrochloride. By dissolvingthe mixed crystals in alcohol and adding ammonia, golden-yellowneedles of the correspoiiding bases are obtained, which may besepars ted by digestion with chloroform, the diamidoazobenzene beingdlssolved. The residue, consisting of the new base, is purified by dis-solving in alcohol and passing hydrogen chloride through the solutionto obtain the hydrochloride which is then decomposed by ammonia.Chrysozdincarbarnide, NPh:NC,H,:(NH)Z:CO, thus obtained, crys-tallises in brilliant, golden-yellow laminae, sparingly soluble in alcohol,nearly insoluble in water, ether, and chloroform. It does not meit at300".I f the chloroform solution of diamidoazobenzene be satur;rtedwith carbonyl chloride and allowed to stand for some days, onl46 ABSTRACTS OF OHEMMIGAL PAPERS.carbamide hydrochloride and unaltered chrysoi'din hydrochloridewill be found on evaporating the chloroform. The hydrochloridecrystallises in golden-yellow laniinse, sparingly soluble in water,more so in alcohol, insoluble in ether. The pZatiizochZoride,( C13H11NaUC1)2PtC14, forms red-brown laminse. The nitrate crystal-lises in brilliant, golden-yellow scales, very sparingly soluble in water,sparingly soluble in alcohol, and insoluble in ether ; they decomposewith slight explosion at above 200". The suZphate forms a yellowish-red powder ; it is very sparingly soluble in water, more so in alcohol.When heated with moderately strong hydrochloric acid in a sealedtuhe at 200" for eight hours, chrysoidincarbamide is decomposed,with the formation of carbonic anhydride and a dark-brown mass.The same dark-brown substance is obtained when chrysoidin istreated in the same way. It yields phenol when distilled with steam,and a reddish-brown residue which has not been identified.Inasmuch as chrysoidin splits up into aniline and triamidobenzenewhen reduced by hydrochloric acid and tin, it seemed probable thatits carbamide would yield aniline and a new substance,by the same treatment, thus showing that both NH-groups areattached to the same benzene nucleus.100 grams of the carbarnidewere heated with 50 grams of tin aud 250 grams of hydrochloricacid (sp. gr. 1.2) in a flask. The solution became colourless at first,and subsequently brown, through oxidation ; after the action hadceased, the hydrochloric acid was evaporated, the residue dissolved inhot water, and hydrogen sulphide passed through the solution ; thefiltrate from the tin sulphide was evaporated in a current of hydrogensulphide, the crystalline residue dissolved in water, and made alkalinewith barium hydroxide. This precipitated aniline, which was dis-tilled off; the excess of barium hydroxide was precipitated from theliquid remainisg in the retort by sulphuric acid, and the excess ofthe latter by barium chloride. From the filtrate, the hydrochloride ofthe new base did not crystallise well, so the solution was digested withammonium oxala te and filtered hot.On cooling, amidophenyZene-arbamide oxalate crystallised out in nearly white minute needles,collected in spheres, freely soluble in hot, sparingly in cold water,nearly insoluble in alcohol.Amido~he?zyZerzecai.bnmide, NHz*C6H3: (NH),:CO, obtained from theoxalate by adding sodium carbonate to a hot solution of it in hydro-chloric acid, forms brilliant and nearly colourless, pointed laminm,sparingly soluble in cold, easily in hot water, freely soluble in hotalcohol, and decomposing at 220". The hydrochloride crystallises inminute needles, freely soluble in water, very sparingly so in alcohol.The sulphate also forms minute needles, having the same solubility.The triacetyZ-derivutzve, NHAc.C6H3:(NAc)z:C0, forms fine, white,silky needles, insoluble in water, fairly soluble in alcohol, and meltingat 248'.NH,* CsH,: (NH),:CO,/NH*CO\c 6 H 3 \ ~ ~ - ~ ~ / N 7Dicarboity ltriainidobenzene, was obtainedbeating amidophenylene carbamide with liquid carbonyl chloride in ORGANIC CHEMISTRY.47sealed tube for eight hours at 130". The excess of carbonyl chloridewas evaporated and the residue heated with water, which extractedthe hydrochloride of the carbamide fo~med during the reaction, andleft the carbonyl compound as a crystalline residue, insoluble inalcohol, ether, benzene, toluene, aniline, and acids, but very solublein alkaline solutions, from which it is precipitated by acids.By passing nitrous acid through a cooled, acidified aqueous solutionof the sulphate of amidophenylenecarbamide, yello wish-green crystals,giving the reactions of a diazo-compound of the carbamide, wereobtained, but they were not pure.By dissolving them in hydro-bromic acid and adding a few drops of bromine, yellowish-red needlesof the perbromide of the diazo-compound crystallised out- ; these lostbromine as they dried, and by digesting them with warm alcoholthey weye converted into yellow crystalline laminm of the diazo-hroinide of amidophenylenecarbamide.By H. v. PECHMANN and I(. WEHSARG (Rer., 21,2994 - 3004).-Nitrosoa~etonehydrazone (methylglyoxal-aw- hydrciz-oain2 e ) N,H Ph: CMe.CH:NO H, prepared by mixing nit rosoacetone(1 mol.) with phenylhydrazine (1 mol.) in alcoholic or ethereal solu-tion, crystallises from alcohol in yellowish prisms or needles, melts at134", and is soluble in ether and benzene, but insoluble in hot water.It dissolves in concentrated sulphuric acid with a reddish-yellowcolour which becomes deep blue on adding ferric chloride.Met hylglyoxalosnzone hydrochloride is obtained when the precedingcompound is warmed with concentrated hydrochloric acid in alcoholicsolution. It crystallises from boiling methyl alcohol, melts a t 197",and yields the free base (compare Abstr., 1888, 1287) when treatedwith ammonia.A. G.B.Hydrazoxirnes.Diacety Eli ydrazoxime (methylnitrosoacetone h ydraxone) ,CMe(N,BPh)*CMe:NOR,prepared in like manner from nitrosometbylacetone, crystallises fromdilate alcohol in large, colourless needles, melts at 158", and resemblesnitrosoacetonehydrazone in its behaviour towards solvents. It dig-solves in concentrated sulphuric acid with a yellow coloration whichchanges to a bluish-violet on adding ferric chloride, and when heatedwith concentrated hydrochloric acid in alcoholic solution, yields amixture of diacetylosazone melting at 241--242", and diacetyl-hydrazone melting at 13.3".Gl~/ox~Zcya?zide-a-hydrazone, CRO*C(N,HPh).CN, is formed,together with hydroxylamine, when dinitrosoacetonehytlrazone (com-pare this vol., p.34) is warmed with alcohol and hydrochloric acid.It crystallises from boiling alcohol in pale-yellow needles, melts at161" with decomposition, and is dissolved on warming in most sol-vents except water.It is soluble in dilute alkalis, and dissolves inconcentrated sulphuric acid with a yellow colour which is not changedby ferric chloride. When boiled with hydriodic acid, it yields thetheoretical quantity of aniline.Glyoxy Zr y anideosazone, NZHP h:CH*C (N2HPh) *CN, prepared bymixing a hot, alcoholic solution of the preceding compound wit48 ABSTRACTS OF CHEMICAL PAPERSphenyl hydrazine, cry stallises from alcohol in orange-red needles, meltsat 161" with decomposition, and is soluble in alcohol and glacial aceticacid, but, only sparingly in most other solvents. The concentratedsiilphnric acid solution is yellowish-red, and its colour is not changedbv ferric chloride..IGlyoxylcyarLideosotetrazone, < ~ ~ ~ ~ ~ $ is formed when thepreceding compound is m-armed with ferric chloride or with a solutionof potassium dichromate and dilute acetic acid. It crystallises fromacetone or alcohol in brownish-red, moss-like needles melting at 137"with decomposition. When heated with hydrochloric acid, a colour-less, crystalline product, probably an osotriazone (loc. cit.) volatilises.This compound, CgH6N@:N2Ph, is formed by the combination ofglyoxylcyanidehydrazone with diazobenzene chloride ; it crystallisesfrom alcohol in brownish plates, melts a t 162-163", and is insolublein alkalis.Gll/ox?/lcZlanide-aw-hydrazox~~ne, NOH:CH.C(N,HPh).CN, preparedby boilicg an alcoholic solution of the hydrazone (1 mol.) withhydroxylamine hydrochloride (1 mol.) and a few drops of hydro.cliloric acid, crystallises from alcohol in citron-yellow, sparinglysoluble needles melting a t 240" with decomposition.It dissolves inalkalis with a yellow coloration, but the yellow, concentrated sul-phuric acid solution is not changed on adding ferric chloride.A compound, C,H,N 4, is obtained when glyoxylcyanidehydrax-oxime is dissolved in phosphorus oxycbloride, heated with phosphoricchloride, the solution poured on to ice, the precipitated product ex-tracted with ether, dissolved in dilute alkali, and fractionally pre-cipitated with hydrochloric acid. It crystallises from a mixture ofether and light petroleum in yellowish needles, melts a t 135" withdecomposition, and is soluble in hot water, alkalis, and most of theordinary solvents. It dissolves in Concentrated sulphuric acid with ablood-red coloration which is not changed on adding ferric chloride.When warmed with concentrated hydrochloric acid or when boiledwith alcoholic potash, it is converted into a ccmpouiid, C9H9N40,which crystallises in small, yellow needles melting a t 244-245".- A compound, C,,H,,N,, is formed i n the preparation of glyoxyl-cyanidehydrazone, and can also be obtained by heating the hydraz-oxime with alcohol ( 3 patbts) and cmcentrated hydrochloric acid(10 parts).I t crystallises from benzene in shining, orange-yellowplates melting a t 165", and does not give the osazone reaction(loc. cit.).MethylgZyoxal-ocw-met?~Zl~hen~~l~iy~~raz~~~~e, N,MePh:CMe*CH:NOH,prepared by mixing an aqueous solution of nitrosoacetone with asolution of methylpbenylhydrazine sulphate and sodium acetate,-crystallises from dilute alcohol in orange-yellow prisms melting at118".Alkaline solutions are dark yellow, and the yellow, concen-trated sulphuric acid solution changes to violet on adding ferricchloride.Mesoxala7deh yde- a w w-n7 eth y lphen y lh ydrazonedioxim e (dinitrosoaceton emethylphenylhydruzolze), N OH:CH.C(N,MePh)*CH:NOH, prepared inlike manner, crystallises from dilute alcohol in orange-yellow ueedleORGANIC CHEMTSTRY. 49or plates, melts a t 137", and is soluble in alkalis and most of theordinary solvents. It dissolves in concentrated sulphuric acid,forming a brownish-red solution in which ferric chloride produces alight violet coloration.When heated with hydrochloric acid, it yieldsdecomposition products the nature of which varies according to theconditions of the experiment.Glyoxylcyanide-a-msfhyZphenylhydrnzone, CHO*C(N,MePh).CN, isobtained by dissolving the preceding compound in acetone ( 7 parts),adding concentrated hydrochloric acid (7 parts) and, after the firstenergetic reaction is a t an end, heating the mixture for about aminute and adding water to the cold solution. It crystallises frombenzene, alcohol, or light petroleum in yellow, feathery needles, orthick, spear-shaped crystals, melts a t 113*5", and is insoluble inalkalis. When mixed with phenylhydrazine, it yields a compound,probably N,HPh:CH.C (N,MePh) CN, which crystalliseq from abso-lute alcohol in golden-yellow plates melting a t 181".The and,NPh:CH*C (X,MePh).CN, prepared by mixing the hpdrazone withaniline i n acetic acid solution, crystallises from alcohol in slender,yellow needles, melts a t 150-151°, and is reconverted into thehy$hzone when warmed with dilute hydrochloric acid. The hydrar-oxz112e, NOH:C H*C (N,MePh).CN, obtained by treating the hydrazonewith hydroxylamine, crystallises in small, yellow needles melting at178'. The acetyl-derivative, NOAc:CH*C(N,MePh).CN, of thehydrazoxime crystallises from alcohol in yellow needles, melts a t122*5", and is reconverted into the hydrazoxime when boiled withsoda. F. S. K.Ethyl Phenylhydraxineacetylacrylate. By H. D ECICER (Ber.,21, 2937-2938).-Tbe compound obtained by Bender (Abstr., 1888,1188) by hydrolysing ethyl phenylhydrazineacetylacrylate, has alreadybeen fully described by L.Wolff (Abstr., 1887, 464). F. S . K.Theory of Dyeing. By E. KNECHT (Ber., 21, 2804-2805 ; com-pare Abstr., 1888, 832).-When wool is boiled with a mixture ofsulphuric acid (2 parts) and water (3 parts) for two hours, it dissolvesalmost entirely ; when filtered, a clear, light-brown solution is ob-tained. If this is mixed with aqueous solutions of acid coal-tar dyes,intensely coloured precipitates are formed, which dissolve readily inalkalis, but not in water or dilute acids.A solution of silk in moderately dilute sulphuric acid behaves inlike manner. Animal fibres, therefore, yield a substance which formsinsoluble bases with acid coal-tar dyes; it has not yet been deter-mined whether this substance already exists in the fibres, or whetherit is gradually formed by the action of the acid bath.N. H. M.Product of the Action of Nitric Acid on Acetophenone. ByA. F. HOLLEMAR" (Bei-., 21, 2835-2840 ; compare Abstr , 1888, 275).-The molecular weight of the compound C,,H,,N,04. obtained by theactioii of nitric acid on acetophenone (Zoc cit.), was confirmed by adetermination by Raoult's method (BPT., 21, 861). When the alco-holic solution is reduced with stannous chloride, benzoic and hydro-VOL. LVI. 50 ABSTRACTS OF CHEMICAL PAPERS.cyanic acids are formed. By qrolonged boiling with strong hydro-chloric acid, it is decomposed into benzoic and oxalic acids; am-monia and hydroxylamine are also formed.These reactions makeit probable that the compound has the constitution <CBaiN.O>, CBz'N-0which is further supported by the fact that the substance, which isnamed diphenyldi.nitrosacyl, can be prepared by oxidising nitroso-acetophenone.Diphenjldinitrosacyl reacts with aniline with formation of benz-anilide and a compound crystallising in lustrous, brown needles.When this is heated a t 100" €or some time, it gives an odour somewhatlike that of carbylamine : when crystallised from dilute alcohol, it isnearly white, and melts a t 205".When diphenyldinitrosacyl is heated with acetic anhydride at110-120" for six hours, the compound C,6H10N204 + OAc, is formed.This crystallises in stellate groups of needles melting at 149".The sparingly soluble compound melting at 177-179", which is alsoobtained by the action of nitric acid on acetophenone (loc.cif.), hasthe same empirical composition as diphenpldinitrosacyl ; it is, how-ever, much more stable than the latter. Boiling aqueous potash andhot sulphuric acid decompose it, yielding benzoic acid ; with potash,ammonia is evolved. N. H. M.Consecutive Duryl Methyl Ketone. By A. CLAUS and E.FOHLISCH ( J . pr. Chew. [a], 38, 230-235; compare Abstr., 1888,275) .-The boiling point of consecutive dureno is 199-200" (uncorr.)and its melting point is -4".Consecutive duryl methyl ketone, C6HMe4*COMe [Me4 : COMe =2 : 3 : 4 : 5 : 11, is prepared in the manner previously described, bywhich 80-90 per cent.of the durene used is couverted into theketone ; it is a brown, strongly refractive oil, of agreeable aromaticodour, boiling a t 258-260" (uncorr.), and easily soluble in the nsualsolvents, except water. The pkenylhydrazine compound forms,,colourless laminae melting a t 129" (uncorr.).2 : 3 : 4 : 5 - 1 ' e t r a m e t h y ~ ~ ~ e n y ~ g l y o a y ~ i c acid, C6Hh!fe4*CO*COOH,is formed when the above ketone is oxidised with potassium perman-ganate in the cold. It is a bright yellow syrupy oil, very little solublein cold, more so in hot water, very soluble in alcohol, ether, carbonbisulpliide, and chloroform ; it solidifies on prolonged cooling anddecomposes when heated. The barium and calcium sa2ts (with 4mols.H,O), the copper (with 3 mols. H,O), azd the silver salts aredescribed.2 : 3 : 4 : El-Tetramethylmandelic acid, C6H%~e4.CH(OH)*COOH, isobtained by reducing the foregoing acid with sodium amalgam. 'Itcrystallises from alcohol in colourless hexahedra, sparingly soluble incold, readily in hot water and in alcohol, ether, and chloroform, andmeits at 160" (uncorr.). The potassium (with 4 mols. H,O), barii~m(with 3 mols. H,O), calcium (with 24, mols. H,O), and silver salts aredescribed.2 : 3 : 4 : 5-Tetrainethy123herz2llacstic acid, C6HMep-CHz.COOH, isformed when either of the above described acids is reduced witORGANIC CHEMISTRY. 51hydriodic acid. It crystallises from hot water in slender, colourlessneedles, me1 ting a t 125" (uncorr.), and easily soluble in alcohol, ether,and chloroform.The calcium salt forms colourless, silky needles con-taining 3 mols. H,O.By oxidising consecutive duryl methyl ketone or the foregoing de-rivatives, with the calculated quantity of potassium permanganate, ata gentle heat, 2 : 3 : 4 : 5- tetramethylbenzoic acid is obtained as athick, colourless oil, sparingly soluble in water, freely so in other sol-vents. When heated, it decomposes a t 270°, and an oil distils over, whichsolidifies and melts at 150" ; this contains 73.8 per cent. of carbon and7.9 per cent. of hydrogen. The sodium (with 3 mols. H,O), calcium(with 3 mols. H,O), bariunc (with 6 mols. H,O), silver and coypel- saltsare described. A. G. B.Stilbene. By I;. ARONSTEIN and A.F. HOLLEMANN (Ber., 21,2831-%334) .-The experiments described were made with a vicwto obtain a geometrical isomeride of stilbene which should existaccording to Wislicenus' theory. No definite results were obtained,but the investigation is being continued.Action of Heat on Benzildihydrazone. By I(. AUWERS and V.CPh'N M E ~ R (Ber., 2 1,2806 -2 80 7). --Tripheny losotriazone, < CPhiN >NPh,formed when benzilhydrazone is heated with alcohol at 200-210",crystallises in white, lustrous plates, melts a t 122O, and boils withoutdecomposition. N. 13. M.Thio-derivatives of p-Dinaphthylamine. By 0. KYN (Ber., 21,2807-28 13) .-When sulphur chloride dissolved in benzene is addedto /3-dinaphthylamine, also dissolved in benzene, hydrogen chloride isevolved and two isomeric dithiudinaphth ylainines, C20H13NS2, are ob-tained.The one forms lustrous, brass-coloured plates melting a t 205O,whilst the other crystallises in reddish-yellow prisms melting a t 220".Both compounds are sparingly soluble. When the dithio-compoundsare boiled with cumene or with aniline, they are both converted withevolution of carbon bisulphide into Ris's thio-P-dinaphthylamine(Abstr., 1886, 1036). A small quantity of the latter compound isformed in the reaction between dinaphthylamine and sulphur chloride.Acetylthio-p-dinnphthylainiwe, Cz2Hl5NOS, is obtained by the actionof acetic anhydride on the dithio-compound (ni. p. 605") or on themonothio-compound. It crystallises in slender, lustrous, almostwhite needles, melts a t 211", and is readily soluble in hot alcohol orbenzene. When the dithio-compound (m.p. 205O) is treated with anammoniacal alcoholic silver solution, a compound free from sulphuris obtained, which melts a t 240°, and sublimes in slender, lemon-yellow needles.Sulphur dichloride acts on p-dinaphthylamine, yielding as chiefproduct thio-p-dinaphthylamine, and a sparingly soluble isomeridewhich melts a t 303". Sometimes a small amount of a compound,probably thiotetranayhthylanline, S ( C,oH6*NH.CloH7)2, is obtained.This forms dark-yellow crystals melting at 307".N. H. M.N. H. M.e 52 ABSTRACTS OF CHEMICAL PAPERS.Naphthoic Acids. By A. G. EKSTRAND (J.pr. Chem. [2], 38,139--285).-This paper is a summary of the author's work on thesubject; much of it has already appeared.The following new corn-pounds are described :-Chloro-a-naphthoic arnide is obtained by heating chlopo-a-naphtho-nitrile (Abstr., 1884, 1361) with an alcoholic solution of potassiumhydroxide ; it forms crystalline laminae, soluble in alcohol andmelting a t 239".The chloro-a-naphthoic acid which melts a t %5" (Abstr., 1884,1361) has the constitution [COOH : C1 = 1 : 4'1, as it is obtained bytreating 1 : 4' amido-a-naphthoic acid by Sandmeyer's method (Abstr.,1884, 1312).Chloro-a-nayhthoic a,cid (1 : 1') is obtained when 1 : 1' amido-a-naphthoic acid (Abstr., 1885, 549) is dissolved in the calculatedquantity of sodium hydroxide and potassium nitrite (1 mol. to 1 mol.of the amido-acid) added ; the mixture is cooled to 0" and treated withexcess of hydrochloric acid.The hydrochloride of the diazonaphthoicacid thus obtained is added to a boiling solution of cuprous chloridein hydrochloric acid ; colourless crystals of the chloro-acid areformed ; they melt a t 167" and sublime as plates. The calcium saltcrystallises with 2 mols. €LO in long tabular needles, soluble in 42parts of water at the ordinary temperature. The ethyZ salt formslong needles melting at 50".Dichlor-a-naplithoic acid is obtained when the foregoing acid isdissolved in glacial acetic acid, some iodine added, and chlorine passedt o saturation ; crystalline scales separate, melting at 186-187".The calcium salt crystallises with 2 mols. H,O in long, colourlessneedles ; the ethyl salt forms fine needles melting at 61".It is possible to obtain this acid from chlornitro-a-naphthoic acid[COOH : NO, : C1 = 1 : 1' : 4'1 (Abstr., 1886, 156), consequently itsconstitution is [COOH : C1 : C1 = 1 : 1' : 4'1.Trichloro-a-nap hthoic acid, the mother-liquor from the preparationof chloro-a-naphthoic acid (1 : 4') by the action of chlorine on a-naph-thoic acid in acetic acid solution, is saturatedwith chlorine at the boilingpoint : dilution with water then throws down a crystalline precipitate,which is heated with calcium carbonate, filtered, and the filtrate pre-cipitated with acid ; when crystallised from alcohol and water, thisprecipitate forms small, colourless needles, melting at 163-164' andsubliming in fine needles.The ethyl salt of monobromo-a-naphthoic acid, 1 : 4' (Abstr., 1886,715), forms colourless tables melting a t 48-49'.Mononitro-a-naphthoic acid of meltiug point 215" (Abstr., 1885,54$) is soluble in 21.5 parts of commercial alcohol, and in 2590 partsof water a t the ordinary temperature.During its formation a smallquantity of a-mononitronaph.t//alene (melting point 60') is obtained.The calcium salt of amido-a-naphthoic acid (Absbr., 1885, 549)crystallises with 9.5 mols. H20 in fine needles, soluble in water. Thehydroch Zoride, COOH.C,oH6*NH,,HC1, is precipitated in fine needlesO n adding hydrochloric acid to a solution of the sodium salt.Nsphthostyril, C,,H,<ZE> (Abstr., 1886, 715), crystallises froORGANIC CHEMISTRY. 53an alcoholic solution of the amido-a-naphthoic acid ; it is also formedwhen the acid is heated with water ; it melts a t 180-181".The benxoyl-derivative forms slender needles melting a t 170" ; thehydrochloride melts a t 178".a-Naphtlzoybz aph thostyri1.-When a-naphthoyl chloride and naph -thostyril are heated together, a gi-een product is formed, whichis dissolved in alcohol and decolorised hy animal charcoal. Amixture of granular crystals (melting a t 110") and needles (melt-ing at 132") is obtained ; by recrystallking these, partly from alcoholand partly from glacial acetic acid, a mixture of the same crystals isobtained, melting a t 150"./3-Naphthoylnaphthostyril, is obtained in the same way tw tlie above,only a t a lower temperature, in slender colourless needles, melting atThe calcium salt of chlornitro-a-naphlhoic acid, of melting point225" (Abstr., 1886, 156), forms slender colourless needles, crystallisingwith 3 mols. H,O, and the ethyl salt tabular crystals melting at 121",and very soluble in alcohol.The question whether this acid has theconstitution [COOH : NO, : C1 = 1 : 1' : 4' or 1 : 4 : 4') is settled infavour of the former, as chZoronaphthostyJriB (with C1 in position 4') isobtained in yellow needles melting at 670", by reducing the acid withferrous sulphate in an ammoniacal solution.Nitronaphthostyril (1 : 4') is formed when nitric acid (sp. gr. 1.42)is added to a solution of naphthostyril in glacial acetic acid, and themixture heated on the water-bath ; the crystalline mass thus obtainedis partially soluble in alcohol, from which yellow needles, meltingabout 235", are obtained ; the greater part recrystallises from glacialacetic acid in orange-yellow needles melting a t 300".Both are nitro-nap hthostyrils.Arraidonuplzthostllril is formed when nitronaphthostyril is reducedwith tin and hydrochloric acid. and the hydrochloride thus produceddecomposed with ammonia ; it crystallises in red needles meltinga t 239-240", and freely solable in alcohol and hot water: The hydro-chloride crystallises in yellow needles melting above 290".Dinitronaphthostyrd is obtained when the nitronaphthostyril is heatedwith nitric acid (1.43 sp. gr.) ; it forms yellow needles, or, when pre-pared by the action of nitric acid on naphthostyril, rhombic tables,melting above 290".Naphthostyrilpuinone, C,,H,O,<EE>, is obtained when a Bolutionof naphthostyril in glacial acetic acid is mixed with chromic acid andthen with water; fine red needles are precipitated, which, after re-crystallisation from glacial acetic acid, melt near 278".When it isdissolved in warm glacial acetic acid and an acetic acid solution oftoluylenediamine added, a yellow, crystalline powder, consisting ofnuphthostyriZtoZ~p~inoaali.ne, CllH5N30,C6H3CH3, is obtained ; it meltsabove 290".Nitronaphthosty1.ilquinone forms orange-red needles or tables, melt-ing near 685", soluble in alcohol and sparingly so in glacial aceticacid. A. G. B.19 7-198".The acetyl-derivative melts above 290"54 ABSTRACTS OF C'HERIICAL PAPERRp-Chloronaphthalenesulphonic Acid.By S. FoRsrmG (Be?.., 21,2802--2804).--When ,!3-amidonaphthalenesulphonic acid (Abstr., 1887,962) is converted into the diazo-compound, and this is boiled withstrong hydrochloric acid and neutralised with potassium carbonate,potassi um p-chloronapht h alenesulph onate separates.p- Chloronaph thalenesulphonic chloride, CloH6C1*SO2C1 (Arnell,Ahstr., 1886, Fj55), is prepared by mixing the well-dried potassiumsalt with phosphorus pentachloride and heating ; it crystallises fromchloroform in broad needles melting a t 129".The brornide, CloH6C1*S 02Br, prepared by the action of phosphorusbromide on the potassium salt, crystallises from chloroform in smallneedles melting at 139".The amide, CIoH6C1.S02*NH,, is obtained by boiling the chloridewith a mixture of equal parts of ammonia and alcohol, and crys-tallising the product from dilute alcohol, in which it is sparinglysoluble; it melts at 235".p-Chloronaphthalenesulphonic acid has the constitution [Cl : SOsH= 2 : 4 o r 2 : 1 ] .N. H. M.Filicic Acid. By G. DACCOMO (Bey., 21, 2962-2970) .-Filicicacid, prepared by the method already described (Daccomo, Abstr.,1888,521) , has the composition Cl4H1,O6. It is a yellowish, odonrless,crystalline powder, melts at 179-180" (uncorr.), and. is insoluble inwater, almost insoluble in absolute alcoho1,'moderately soluble in glacialacetic acid, ether, amyl alcohol, and toluene, and readily in chloroform,cwbon bisulphide, and benzene.The benzoyl-deriva tive, C2,H,,0,,separates from dilute alcohol in colourless crystals, melts a t 123", andis very readily soluble in ether, but insoluble in water. The ethytsalt, C,H,,O,, prepared by treating the acid with alcoholic potash andethyl iodide, separates from dilute alcohol in reddish crystals, meltsat 142", and is very readily soluble in ether and benzene, but insolublei n water, The propyl salt melting at 158", and the ethylene saltmelting at 165", resemble the ethyl salt in appearance and solu-bility.Bronzo$Zicic acid, Cl4HI5BrO6, prepwed by treating the acid withbromine in glacial acetic acid solution, crystnllises from alcohol in redprisms, meits a t 122", and is very readily soluble in absolute alcoholand ether, but insoluble in water.AniZidoJiZicic acid, C14HZ50,*NHPh, obtained by boiling a glacialacetic acid solution of the acid with aniline, separates from alcohol inreddish-violet crystals, melts a t 140°, and is soluble in alcohol andbenzene, but insoluble in water.The hydraaide, C,Hl,O.( NZHPh),, prepared by boiling an etherealsolution of the acid with phenylhydrazine, crystallises from ether illred needles, melts at 198", and is readily soluble in alcohol, butinsoluble in waker.When the acid (100 parts) is heated above itsmelting point (compare Luck, AnnaZen, 54, 119), or heated withwater at 170-190", it is decomposed into isobutyric acid (32.5 parts)and a compound, the composition of which is C?OH,AOI. Hydrochloricacid produces the same decomposition at 150-160".Filicic acid is completely oxidised when treated with chromic aciORGANIC CEIEMISTRT.55in glacial acetic acid solution, but when a solution of the potassiumsalt is oxidised in the cold with a 2 per cent. solution of potassiumpermnnganate, isobutyric acid and oxalic acid are obtained. Tbe sameproducts are formed when nitric acid of sp. gr. 1.48 is employed.When the acid is treated with zinc-dust in alkaline solution, i t is con-verted into an acid, the composition of which is probably Cl4Hz2011,and at the same time a small quantity of isobutyric acid is formed.When treated with sodium in amyl alcohol solution, it, yields butyricacid and resinous products.The compound CZOH,80,, referred to above, separates from ether oramyl alcohol as an amorphous, red powder, and has no well-detinedmelting point.It is soluble in most ordinary solvents, has an acidreaction, decomposes carbonates, and dissolves in alkalis, forming redsolutions from which it is precipitated in red flocks on adding acids.It yjelds phthalic acid and small quantities of ovalic acid whenoxidised with nitric acid of sp. gr. 1.40 in the cold. When reducedwith zinc-dust in alkaline solution, it gives a colourless substancewhich rapidly oxidises, and is probably reconverted into the originalcompound.From the above results, it follows that filicic acid is probably anisobutyric acid derivative of hydroxynaplithaquinone. F. S. K.Quillajic Acid. By R. KOBERT (CYhesn. Centr., 1888, 927-928,from Arch.ex$. Path. Pharm., 23, 233).--The saponin of commerce,as all other specimens of saponin, is an almost inactive, non-poisonousmodification of quillajic acid. The author precipitated the acid from theaqueous extract of the bark of Quillaja sapomaria with neutral leadacetate ; the precipitate was fresd from lead, the solution of the acidevaporated almost to dryness, and then taken up with hot absolutealcohol. The colouring matter was precipitated with chloroform ;the quillajic acid eventually crystallised out in pure white flakes. Itis insoluble in ether, soluble in water and alcohol. On treatment withconcentrated sulphuric acid, it becomes dark red. By boiling with dilui emineral acids, it is split up into an unfermentable glucose and sapo-ginin ; this solution reduces Fehling's solution.Quillajic acid hasthe formula Cl,H,oOlo. The sodium salt acts as a very severe causticon the tongue and throat, and the smallest particles coming in contactwith the nose or throat cause violent sneezing and coughing. Broughton to the eye, it causes severe pain, flow of tears, and swelling of thelids. Injected into the blood, the sodium salt proves fatal, causingcramp arid paralysis of the respiratory organs and brain. On theother hand, it may be imbibed into the stomach without injury to theextent of 500 times the quantity which proves fatal when injectedinto the blood. J. W. L.Brazilin. By C. SCHALL and G. DRALLE (Bey., 21, 3009-3017,compare Abstr., 1888, 295) .-Tetramethylbrazilin is best prepared asfollows:-A solution of brazilin (100 grams) in warm 98 per cent.alcohol is mixed with sodium ethoxide (30.26 grams sodium) andmethyl iodide (206 grams), the mixture kept a t 60-70" for 40 to 50hours, cooled and poured into cold water.The precipitate is collected56 ABSTRACTS OF CHEMICAL PAPERS.washed with water, dissolved in ether, the solution shaken with soda( 1 7 2 per cent.), washed with water, the ether evaporated, and theresidue crystnllised from alcohol with addition of animal charcoal.The yield is 58.5 per cent. of the theoretical quantity.Trirnethylbrazilin, C16H1105Me3 + iH,O, is obtained by neutralisingthe alkaline washings from the tetramethyl-derivative, extractingwith ether, washing the extract first with sodium hydrgen carbonate,then with sodium carbonate, and evaporating the ether a t the ordinarytemperature.The residue is mixed with concentrated soda, the pre-cipitated sodium-derivative collected, washed with alcoholic ether,dissolved in water, and precipitated from the filtered solution by treat-ment with carbonic anhydride. If the product is pure, it is obtained inthe crystalline condition containing about 1 mol. H,O, but the impurecompound does not crystallise well even after keeping for months. Itdissolves in dilute alcohol, and the solution gives a brown precipitatewith ferric chloride ; the solution in soda is colourless, and does notalter on keeping. The acetyl-derivative, C16H,,05Me,Ac, is crystalline,and melts a t 95-97" with previous softening.Rrornotetrainethylbrazilin, C16H9BrMe40,, obtained by treating thetetramethyl-derivative (1 mol.) with bromine (1 mol.) in glacialacetic acid solution, crystallises from dil-cite alcohol in long, colourlessprisms melting a t 180-181".A crystalline tetrabromo-derivative, C,,H,Br,Me,O,, is formed whena larger quantity of bromine (2-3 mols.) is employed ; this snbstanceloses bromine (about 26 per cent.) when treated with dilute ammonia,or soda, and appears to be dibromotetramethylbrazilin dibromide. Itis probable that other bromo-derivatives exist, and a crystalline iodo-additive product was also obtained.Tribrornobrazilin dibyomide, C16HllBr305,Br2 + 2H20, is obtained inreddish-brown needles when bromine (4-6 mols.) is added graduallyto a boiling glacial acetic acid solution of brazilin.A compound, C20Hld09, is obtained when brazilin (2.7 grams) isdissolved in water (150 c.c.) and soda of sp.gr. 1.37 (10 c.c.), and astream of air passed through the solution for about 36 hours. Itcrystallises from alcohol in light brown, flat, microscopic needles,melts at &71", and is readily soluble in dilute soda, sparingly solublein ether or sodium carbonate, and insoluble in sodium bicarbonate.The aqueous alcoholic solution gives a slight violet coloration withferric chloride, and a citron-yellow coloration with concentratednitric acid. When heated above its melting point, shining scalessublime, but considerable' decomposition takes place. F. S. K.Nomenclature of Compounds containing NitmgenousNuclei.By 0. WIDMAN ( J . pr. Chem. [a], 38, 185-20l).-A newsystem of nomenclature for the quinoxalines and compounds of alliedstructure. (Compare Mason, Proc., 1888, 109.)Metapyrazolones. By E. GRINAUX (BUZZ. SOC. C'him., 49, 739-740) .-The compounds described by Pinner and Lifschutz, and namedby them metapyrazolone-derivatives, are derivatives of glycolylcarbORGANIC CHE3IIISTRY. 57amide or hydantojin, and the isomeric substances which Pinner andLifschutz name metapyrazole-derivatives are simple ureides.P. S. K.Action of Phenylhydrazine and Hydroxylamine on Acetyl.acetone. By A. COMBES (Bull. SOC. China., 50, 145-146 ; compareibid., 48, 471) .-Dimethy~hei.ly~yrazole, CMe<Nph,N>CMe, isformed by the action of phenylhydrazine on acetylacetone : it boilsat 270.5".Derivatives of Methylpyrroline. By G.DE VARDA (Ber., 21,28 7 1-28 74) .-MethyZtetrabromo~yrrol~ne, C4NBr4Me, obtained bydigesting tetrabromopyrroline with caustic alkali and methyl iodidedissolved in methyl alcohol, crystallises from light petroleum in long,colourless needles, which melt at 154-155" to an intensely blueliquid.Dibromomaleinmethy limide, C4Br,0zNMe, is prepared by slowlyadding tbe above t,etrabromide to fuming nitric acid (3 parts), cooledto 0", and pouring the product into water (10 parts). It crystallisesfrom boiling water in long, light-yellow needles melting a t 121". Itdistils readily with steam ; the vapour has an irritating odour.N e t h y k y r r y lg Zy ozy Zic acid, CaNH,Me-CO*COOH, is obtained bytreating a boiling solution of methylacetylpyrroline (5 grams) inalkaline water (500 c.c.) with a solution of potassium permanganate(15.5 grams) in water (500 c.c.).The whole is boiled, steam-distilled,and filtered ; it is then evaporated down, acidified, and extracted withether. The acid is crystallised from benzene, from which it separatesin light-yellow needles which melt a t 141-142.5' with decomposi-tion; it is sparingly soluble. The silver salt was prepared, Thedibromo-derivatice, C4NHIMeBr2*CO*COOH, prepared by brominatingthe acid dissolved in acetic acid, crystallises from benzene in small,sulphur-coloured prisms melting a t 160". When the dibromo-acidis slowly added to fuming nitric acid (10 parts), dibromomalei'n-methvlimide is formed.The bromine-atoms and the --CO*COOHCH--(Compare Claisen, Abstr., 1888, 692 ; and Zedel, 1051.)N. H. M.grou; have, therefore, the positions 3, 4, and 5 respectively.N. H. M.Derivatives of Unsymmetrical Dimethylpyrroline. By G.MAGNANINI (Ber., 21,2864-2868, 2874-2879) .-Ethy I diwethylasetyl-pyrrolinecnrboxylate, C4NHMe2Ac*COOEt [ 2 : 4 : 5 : 31, prepared byheating ethyl hydrogen dimethylpyrrolinedicarboxylate (Know,A n d e n , 236, 318) with acetic anhydride at 'LOO", crystallises inneedles, melts at 142-143", dissolves very readily in alcohol, etlier,acetic acid, and benzene, &c., sparingly in light petroleum. The f r e eacid obtained by boiling the ethyl salt with aqueous potash, melts atabout 152-158Owith formation of dimethylacet~I-pyrroZine and evolutionof carbonic anhydride, is almost insoluble in boiling water, verysparirigiy soluble in ether, chloroform, and benzene, and readily solublein hot acetic acid, from which it separates in long, lustrous needles.It gives a green coloration when heated with isatin and sulpbnric acid.DimethyZacety~yl.roZine, C4NH,MezAc [ = 2 : 4 : 51, is prepared bydistilling dimethy lacetylcarbopyrrolic acid in a retort heated in 58 ABSTRACTS OF CHEMICAL PAPERS.metal-bath a t ZOO".It is first crystalliscd from water containing alittle sodium carbonate, then from dilute alcohol, and lastly from lightpetroleum. It melts a t 122-123", sublimes a t loo", and is readilysoluble in the usual organic solvents.Dimethylpyi-rolinedica.l.boxylic acid irnineanhydride,c O / y M e \c .c 0 OH,'N*C Me/is obtained by boiling Knorr's unsymmetrical dicarboxylic acid(Abstr., 1887, 275) with acetic anhydride (10 parts) in a refluxapparatus for three to four hours. The acetic anhydride is distilledoff under diminished pressure, the residue washed with alcohol, dis-solved in aqueous sodium carbonate, filtered, and precipitated withacetic acid. It is almost insoluble in the usual solvents, becomesslightly brown a t 300", and decomposes a t a higher temperature intodimethylpyrroline and dimethylpyrocoll. It resists the action ofmineral acids, but seems to be pastially decomposed by aqueousammonia. The silver salt is a yellowish, amorphous substance ; them a p e s i u m saZt forms lustrous needles.The ethyl salt crystallises inthread-like needles, melts a t 270", and is sparingly soluble.2, 4-DiiizethylpyrocoZZ, C7H7N0, obtained by distilling the copper orsilver salt of the above acid in a stream of carbonic anhydride, is light,yellow, melts a t 272--272*5", dissolves very readily in chloroform,readily in acetic acid, but only sparingly in ether, light petroleum,and cold alcohol ; it is insoluble in water. The crystals are rhombic ;cc : b : c = 0.788:-(4 : 1 : 0.94606. The compound is hardly attackedby aqueous potash. N. H. M.Derivatives of Pyrrolinephthalide. By F. ANDERLINI (Bey.,21, 2869-2870) .-Dibromopyrrolinephthalide, C,,H5Br,NO2, .preparedby treating a warm solution of pyrroliuephthalide (2 grams) in glacialacetic acid (15 grams) with bromine (8 grams), crystallises in small,yellow, lustrous needles, melts at 199", is insoluble in water, sparinglysoluble in boiling alcohol and ether.Nitropyrroli.,iep7itAalide, C,,H6N2O4, is formed when the phthalide isdissolved in strong nitric acid ; it crystallises from alcohol in needles.When pyrrolinephthalide is treated with bromine in alkaline solution,tetrabromopyrroline and phthalic acid are formed.On similarlytreating the dibromo- and nitro-derivatives, both compounds yieldphthalic acid; the substituted radicles are therefore in the pyrrolinenucleus.When potassium pyrrolinephenylcarbinolorthocarboxylate,CINH3:C (0 H) *c6H4.co~K,is distilled with potassium carbonate, it is decomposed into pyrrolineand benzene. N.H. M.Action of Methyl Iodide on some Pyrroline-derivatives.By G. CIAMiCraN and F. ANDERLlNr (Bey., 21, 2855--2864).-Dihydro-tetl.ainethyl~,llridine, C9kI15N, is obtained, together with other basesORGAN I0 CHEMISTRY. 59when sodium carbopyrrolate (5 grams), methyl iodide (10 grams),and methyl alcohol (7 grams) are heated a t 120" for 12 hours.It boils a t about 160". The aurochloride, CgH15N,HAuC14, crystallisesfrom very dilute solutions in long, flat, monoclinic needles ; a : b : c =54: 10 : 5 i ; j? = 85%. When the base is reduced with sodium andalcohol, the compound C&HI9N is formed. This boils a t 150-152°.The azirochloride separates from its solution as an oil, which crystal-lises after some days in yellow needles melting a t 117-119". Whenthe base C,HlgN is boiled with methyl iodide in a, reflux apparatus,and the product, freed from tlhe excess of methyl iodide, is dissolvedin alcohol and precipitated with ether, the compound CI9Hl8NMeZI isobtained in colourless prisms which melt at 262".It is very readilysoluble in water, insoluble in ether. The mother-liquor from the di-methyl compound contains a small amount of a buse, C9HI8NMe, whichforms an oil.MetliyZL~il~yd70~2/0^roZine, CloHl7N, is prepared by heating methyl-pyrroline (3 grams), methyl iodide (7 grams), potassium carbonate(3 grams), and methyl alcohol ( 5 grams), for 10 hours ah 140". Theoily product is heated with strong hydrochloric acid at, 125-130",and distilled with potash.The aurochloride, Cl7HI7N,HAuCI4, crystal-lises from dilute hydrochloric acid in flat, yellow needles, which meltat 100". N. H. M.Dipiperidyl and Dipicolyl. By F. B. AHRENS (Eey., 21, 2929-2932).-Dipiperidyl is obtained when pi-dipyridyl is reduced withsodium and alcohol and the product purified by means of the nitroso-derivative. It crystallises in colourless needles, melts at 120-122"with previous softening, and is readily soluble in alcohol and ether,but insoluble in water. It absorbs carbonic anhydride when exposedto the air, and is only slighhly volatile with steam. The pkr,tiv,o-chloride, CloH,,M,,H,PtC16, forms microscopic crystals, is only sparinglysoluble in water, and blackens when heated a t 195". The aurochloride,CloH,N2,HAuC14, crystallises in small, yellow needles, is readilysoluble in hot, dilute hydrochloric acid, and is gradually decomposedwhen heated a t about 160".The p i c r a t e crystallises from hot waterin needles ; it blackens when heated, and is completely decomposedat about 257". Mercuric chloride,. phosphomolybdic acid, and potas-sium ferroqanide produce precipitates in a solution of the hydro-chloride.DipicoZyZ, CI2Hl2N2, is obtained when picoline, boiling a t 128-1 34",is treated with sodium at 80-90". After washing the product withwater, it is dissolved in ether, the solution filtered, and the base ex-tracted wit8h dilute hydrochloric acid. The extract is mixed withexcess of soda, the treatment with ether and hydrocliloric acidrepeated several times, and finally the ethereal solution is dried overpotash and evaporated.The residual yellow oil is then distilled,and the portion passing at 270-300" collected ; this dist,illate solidi-fies to a mass of yellowish, very deliquescent needles. The platino-chloride, C12Hl,N2,H2PtC16, crystallises in small plates, and is verysparingly soluble in water, but readily in hydrochloric acid ; it, is onlypartially decomposed when heated at 2 75". The aurochloride60 ABSTRACTS OF CHEMICAL PAPERS.C1,H,,N2,HAnC14, separates from warm, concentrated hydrochloricacid, in which it is readily soluble, in nodular crystals mixed withmetallic gold ; it is completely decomposed when heated a t 200-201".The picrate forms yellow, moss-like crystals, and is readily soluble inhot water.An aqueous solution of the hydrochloride gives precipi-tates with mercuric chloride, phosphomolybdic acid, potassium iodide,and potassium ferrocyanide.Action of Chlorine on Hydroxyquinoline. By H. HERhRRAND(Ber., 21, 2977 - 2989). - Chlcrrhyd,.uxyqztinoline, CgNH,OCl, isformed in small quantities when chlorine is passed into a well-cooledsolution of 1-hydroxyquinoline ( 5 grams) in glacial acetic acid.Dichlorhydroxyquinohne (see below) separates a t hst, and is furtherconverted into the hydrochloride whilst a further portion of the hydr-oxyquinoline is oxidised t o the rnonochloro-derivative. As soon as thewhole of the hydroxyquirioline 1s changed, the solution is filtered andthe residue treated with absolute alcohol to dissolve the dichlorhydroxy-salt.The residue is dissolved in hot, dilute hydrochloric acid, thesolution mixed with excess of sodium carbonate, and the precipitatedmonochlorh ydroxy-compound recrystallised fram methyl alcohol andlight petroleum. It is thus obtained in colourless needles melting a t129-130'. The hydrochloride crystallises in small, yellow needles,melts a t 253", and is moderately soluble in alcohol and hot, dilutehydrochloric acid ; it is very stable and sublimes in compact crystals.The platinochbride, (C9NH60C1)2,H2Pt C1, + 2H20, crystallises inyellow needles, and is readily soluble in hot but only sparingly in cold,dilute hydrochloric acid.DichZorhydroxyqzLinoZine, CgMH4C12*OH [OH : CI, = 1 : 2 : 41, isprepared by passing chlorine into a 10 per cent.glacial acetic acidsolution of hydroxyquinoline until the colour changes to yellow,pouring the solution into water, and recrystallising the precipitatedproduct from alcohol. It is also obtained when t~ichloroketoqu~noline(see below) is treated with hydrogen sodium snlphite or boiled w i t halcohol or dilute acids. It crystallises in long, slender needles, meltsat 179-180", and is readily soluble in warm alcohoi or glacial aceticacid, but only moderately in hot benzene and light petroleum. Itdissolves readily in alkalis and acids, forming yellow solutions, butthe salts are unstable and cannot be recrystallised, and acid solutionsare precipitated by water. When treated with chlorine in chloroformsolution, it is converted into trichloroketoquinoline, The h y d ~ o -chloride crgstallises in long, yellow needles, and in aqueaus solutiongives a black precipitate with ferric chloride.The platircochloride,( C9NH,0C1,),,H2PtC16 + 2H20, crystallises in long, orange needles,and loses its water a t 120"- The acety l-derivative, CgMH40C1,Ac,separates from light petroleum in small, colourless ci-ystals melting at97-98"; it is very unstable, and is decomposed by water or whenboiled for a long time with glacial acetic acid.Tricl~lorl2ydroxyyuinoZ~ne, [OH : C1, = 1 : 2 : 3 : 41, is formed whenthe mother-liquor from trichloroketoquinolitie is boiled or when thehydrochloric acid solution of pentachloroketoquinoline is treated witlihydrogen sodium sulphite or with water.It crystallises from glacialF. S . I(ORGANIC CHEMISTRY. 61acetic acid i n long, colourless, moss-like needles, melts a t 213-214",and is readily soluble in hot alcohol or glacial acetic acid, but onlysparingly in the cold solvents and in dilute acids ; it is readily solublein concentrated acids, but is reprecipitated on adding water. Whentreated with chlorine in chloroform solution, it yields a yellowpowder, probably tetrachloroketoquinoline, which melts a t 175" withdecomposition, and is recoiiverted into trichlorhydroxyquinoline whenboiled with alcohol. When heated with sodium carbonate, it yields asodium-derivative melting a t 270". The potassium-derimtive is c r ptalline. The hydrochzoride crystallises in small, yellow needles.Thep latinochzoride, ( C,NH4C130) %, H2Pt C1, + 2 H,O, crys t allises from dilutehydrochloric acid in long, orange needles and loses its water at140-150". The acety2-derivative separates from a mixture of glacialacetic acid and acetic anhydride in thin, transparent, forked, efflore-scent crystals, melts a t 172-173", and is readily decomposed.Tricli Zoroketoquinoline hydrochloride, C,NH40C13,HC1 + 2H20, pre-pared by saturating a well-cooled glacial acetic acid solution of hydr-oxyquinoline with chlorine and washing the product with glacial aceticacid, is very unstable, hygroscopic, and sensitive t o light. When simplydried between blotting paper, it melts at 93-95" to a yellow liquidwhich decomposes a t 100-120" with evolution of gas and thensolidifies, melting again at 170-1 80" with decomposition. Whendried over sulpburic acid under reduced pressure, it does not begin todecompose until heated a t 160" and melts at 180". It is readily solublein moderately dilute hydrochloric acid, but when the solution is evapo-rated under reduced pressure dichlorhydroxyquinoline separates.14, is decomposed when warmed with solvents, generally with forma-tion of the dichlorhydroxy-derivative, and this substance is formedvery readily when the keto-derivative is reduced with hydrogensodium sulphite. The platinochloride is very readily soluble, and whenthe solution is boiled or evaporated under reduced pressure, a mixtureCO*CCl, of platinochlorides is obtained. The free base, C,NH,< CCl:CH >,obtained by decomposing the hydrochloride with water and extractingthe precipitated oil with ether, crystallises in long, thin, yellowprisms or needles, melts a t 9So, turns brown a t 130", and is completelydecomposed a t 170". It is readily soluble in benzene, alcohol, andglacial acetic acid, and does not decompose when kept.EthoxydichZor7~ydroxyqzlinoZine, OEt*C,NH,Cl,*OH [OH : C1, : OEt =1 : 2 : 4: 1'3, is formed, together with dichlorhydroxyquinoline and asmall quantity of the trichloro-derivative, when an alcoholic solutionof freshly prepared trichloroketoqninoline is boiled for 1-2 hours.It crystallises from alcohol or benzene in long, thin, colourlessneedles, melts at 150-151", and dissolves sparingly in most ordinarysolvents in the cold but readily on warming. It is soluble in acids,forming colourless solutions, from which i t is reprecipitated by water,and when warmed with alcoholic soda, it yields a solution from whicha spongy sodium-derivative separates on cooling.Dihydroxydzchloroquiizoline, [(OH), : C1, = 1 : 1' : 2 : 41, is ob-tained, together with ethyl chloride, when the preceding compound isheated a t 110-120" with concentrated hydrochloric acid; it is als62 ABSTRACTS OF CHEMICAL PAPERS.formed when trichloroketoquinoline is boiled with methyl alcohol.It crystallises from alcohol in needles, melts atv 278", and is moresparingly soluble than the chloro-derivatives of hydroxyy uinoline.It crystallises from methyl alcohol in efflorescent needles containingalcohol.Anilidoquinolinequinoneani lide, C,NH,< C'O*C(NPh)- d (NH ,:cEI>, is ob-tained by treating an alcoholic solution of the ketochloro-derivativewith excess of aniline. It crystallises in small, golden plates or longneedles, melts a t 222", and shows all the properties of a feeble base.It is moderately soluble in glacial acetic acid, sparingly in alcohol,insoluble in water, and dissolves in dilute acids with a bluish-violetcoloration. It is not changed by boiling with alcohol or concentratedpotash, but is readily decomposed when heated with acids, yielding. a,yellow, crystalline substance which was not, obtained in the pure state.The hydrochZoride crystallises from acidified alcohol in small, dark-golden needles and is unstable. The yicrate crystallises from alcoholin dark, copper-red needles. The acetate crystallises in needles,melts a t 19Y", and is decomposed by water.Pentach loroketopuinoline platinochloride, (CJ H,Cl,O) 2, H,Pt Cl,, isformed when trichloroketoquinoline hydrochloride (5 grams) isheated at 140-150" for six hours with manganese dioxide (35grams)and concentrated hydrochloric acid (18 grams), the resulting solutionfiltered and mixed with platinic chloride. It is a yellow, crystallinecompound, and when recrystallised or dried, it seems to lose hydro-gen chloride and be convei-ted into the salt of tetrachloroketoquinoliae.A solution of pentachloroketoquinoline hydrochloride yields trich lor-bydroxyquinoline when mixed with water or hydrogen sodiumsulphite. F. S. I(.Alkaloids from Papaveraceae. By E. SCHMIDT (Arch. Pharm.[ 3 ] , 26, 622-623).-The following abstract is the first of a series onthese alkaloids, giving the results of investigations undertaken a t theinstance of the author. Schiel's conclusion that chelerythrine andsanguinarine are identical is not confirmed. The former appears tohave the formula CI9Hl7N04, as deduced from the analysis of thesmall quantities obtained, whilst the latter, from the analysis ofvarious compounds, has the formula, CI7Hl5NO4, thus confirmingNaschold's result. Three more bases have recently been separatedfrom Chelidonlum majus which are now the subject of research.Chelidonine. By A. HENSCHKE (Arch. Pharm. [3], 26,624-644 ;compare Abstr., 1887, 854) .--The alkaloi'd was obtained partly byrecrystallisation of the commercial base, and partly by direct extrac-tion from the root of CheZidoriiunz rnajus. Probst's method of ex-traction was employed, the stamped root being boiled in wateracidified with sulphuric acid, ammonia in excess added, and the filtratedried. This was purified by treatment with acidified alcohol, andagain with ether, and finally was repeatedly crystallised from boilingalcohol. Chel idonine, CzoH19N05 + HzO, forms vitreous, tabular, colour-less, monocliuic crystals of about 3 mm. diameter. The reactions ofJ. TPHYSIOLOGICAL CHEMISTRT. ti3the base are given in detail. Solutions of the salts of this base have anacid reaction, and tlie hydrochloride has the formula C,,H,,NO,-HCl ;the nitrate, C,,HlgN05,HN03; the sulphate, C20H19N05,H2SO~ + 2H20 ;the platinochloride, (C20H,9N05)2,H2PtC16 + 2H20 ; this was not, ob-tainable in a crystalline form ; the aurochloride, C2,,H,,N05,HAuC14,is easily obtained in crystals. Ethyl iodide combines with the base, andthe compound is not acted on by potassium hydroxide ; these and lesspositive results lead to the conclusion that chelidonine is a tertiarybase. By oxidation with potassium permanganate in alkalinesolution, chelidonine yields oxalic acid, methylamine and ammonia,the latter resulting from the decomposition of methylamine. In acidsolution, the oxidation goes further, carbonic anhydride and methyl-amine resulting. J. T.Alkaloids from Cod-liver Oil. By A. GAUTIER and L. MOURGUES(Compt. rmd., 107, 626-629 ; compare Abstr., 1888,1325) .-Aselline,C25H32N4, is an amorphous, colourless solid which becomes green onexposure to light. It melts to a viscom, yellowish liquid with anaromatic odour recalling that of the ptomaines, is very slightly solublein water, to which it imparts a bitter taste and an alkaline reaction,but dissolves in ether and still more readily in alcohol ; sp. gr. about1-0,5. The salts of aselline crystallise readily, but are partially de-composed by water. The mercurochloride crystallises from warmwater ; the aurochloride is very easily reduced ; the platinochlorideis orange-yellow, and dissolves in warm water, but is decomposed byboiling water. Aselline is feebly toxic, and produces fatigue andstupor; 3 mgrms. of the hydrochloride killed a greenfinch in14 minutes.Morrhuivae, C19H2,N3, is separated from aselline by taking advantageof tlie greater solubility of its platinochloride. It is a thick, oily,amber-coloured liquid with an odour which recalls that of aselline,and is only slightly soluble in water, but more soluble in alcohol andether. It is caustic and strongly alkaline, and absorbs carbonicanhydride from the air. The hydrochloride is very deliquescent ; theaurocbloride is yellow, and dissolves in warm water; the platino-chloride is somewhat soluble and crystallises in needles.Morrhuine constitutes one-third of the total bases in the oil, andan ordinary dose of one fluid ounce contains 2 milligrams. It excitesthe appetite and has remarkable diaphoretic and diuretic properties.In large doses it produces fatigue and stupor. C. H. B

ISSN:0368-1769    

DOI:10.1039/CA8895600029

出版商:RSC    

年代:1889

数据来源: RSC

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J O U l t N A L C. F. BAKER. H. BAKER. D. BENDIX. A. Q.BLOXAM. C. H. BOTHAMLEY. B. BRAIJNER. B. H. BROUGH. H. CROMPTON. W. D. HALLIBURTON, M.D., B.Sc. F. 5. KIPPINB, Ph.D., D.Sc. J. W. LEATHER, Ph.D. D. A. LOUIS. T. MAXWELL, M.D., B.Sc. N. H. J. MILLER, Ph.D. OP G. T. MOODY, L).Sc. J. M. H. MMUNRO, D.Sc. T. G. NICHOLSON. E. W. PREVOST, Ph.D. H. H. ROBINSON, B.A. R. ROUTLEDGE, B.Sc. M. J. SALTER. JAMES TAYLOR, B.Sc. L. T. THORNE, Ph.D. H. I(. TOMPKINS, B.Sc. 8. W. DE TUNZELMANN, B.Sc. W. C. WILLIAMS, B.Sc. W. P. WYNNE, B.Sc. THE CHEMICAL SOCIETY. H. E. ARMSTRONG, Ph.D., F.R.S. W. CROOKES, F.R.S. WYNDHAM R. DUNSTAN. F. R. JAPP, M.A., Ph.D., F.R.S. H. MCLEOD, F.R.S. A. K. MILLER, Ph.D. HUGO MULLER, Ph.D., F.R.S. S. U. PICKERING, M.A. W. RAMSAY, Ph.D., F.R.S. W. J. RUSSELL, Ph.D., F.R.S.J. MILLAR THOMSON, F.R.S.E. T. E. THORPE, Ph.D., F.X.S. W. P. WYNNE, B.Sc. Gbiiar : C. E. GROVES, F.R.S. %b-&;bifar: A. J. GREENAWAY. VOl. LVI. Part 11. 18 8 9. ABSTRACTS. LONDON: GURNEY & JACKSON, 1, PATERNOSTER ROW. 1889.LONDON 2 HARRISON AND SONS, PRINTEBS IN ORDINARY TO HEB YAJESTY, 6T. NABTIN’S M E .J O U l t N A LC. F. BAKER.H. BAKER.D. BENDIX.A. Q.BLOXAM.C. H. BOTHAMLEY.B. BRAIJNER.B. H. BROUGH.H. CROMPTON.W. D. HALLIBURTON, M.D., B.Sc.F. 5. KIPPINB, Ph.D., D.Sc.J. W. LEATHER, Ph.D.D. A. LOUIS.T. MAXWELL, M.D., B.Sc.N. H. J. MILLER, Ph.D.OPG. T. MOODY, L).Sc.J. M. H. MMUNRO, D.Sc.T. G. NICHOLSON.E. W. PREVOST, Ph.D.H. H. ROBINSON, B.A.R. ROUTLEDGE, B.Sc.M. J. SALTER.JAMES TAYLOR, B.Sc.L. T. THORNE, Ph.D.H. I(. TOMPKINS, B.Sc.8. W. DE TUNZELMANN, B.Sc.W. C. WILLIAMS, B.Sc.W. P. WYNNE, B.Sc.THE CHEMICAL SOCIETY.H. E. ARMSTRONG, Ph.D., F.R.S.W. CROOKES, F.R.S.WYNDHAM R. DUNSTAN.F. R. JAPP, M.A., Ph.D., F.R.S.H. MCLEOD, F.R.S.A. K. MILLER, Ph.D.HUGO MULLER, Ph.D., F.R.S.S. U. PICKERING, M.A.W. RAMSAY, Ph.D., F.R.S.W. J. RUSSELL, Ph.D., F.R.S.J. MILLAR THOMSON, F.R.S.E.T. E. THORPE, Ph.D., F.X.S.W. P. WYNNE, B.Sc.Gbiiar :C. E. GROVES, F.R.S.%b-&;bifar:A. J. GREENAWAY.VOl. LVI. Part 11.18 8 9. ABSTRACTS.LONDON:GURNEY & JACKSON, 1, PATERNOSTER ROW.1889LONDON 2HARRISON AND SONS, PRINTEBS IN ORDINARY TO HEB YAJESTY,6T. NABTIN’S M E

ISSN:0368-1769    

DOI:10.1039/CA88956FP051

出版商:RSC    

年代:1889

数据来源: RSC

摘要:

PHYSIOLOGICAL CHEMISTRT. P h y s i o l o g i c a l C h e m i s t r y . ti3 The Nature of Fibrin Ferment. By W. D. HALLIBURTON (J. Physiol., 9, 227-286).-This paper gives a full account of the researches of which a preliminary account has already been published (Abstr., 1888, 974). W. D. H.64 ABSTRACTS OF CKERIICAL PAPERS, The Glycogen in Muscle after Section of its Nerve and its Tendon. By E. KRAIJSS ( V~TC~OW’S Archiv, 113,325-332). -The first part of this paper is devoted to the histological changes that occur in muscle after nenrotomy and tenotomy respectively. For the glycogen estimations, the tendo Achillis was divided in 21 rabbits, and the sciatic nerve in 16 others. The animals were then fed for 1 to 3 days before death with 15-30 grams of sugar dissolved in water.The glycogen was determined by Kiilz’ method (Abstr., 1886, 494). The animals were killed a t different periods varying from 2 to 124 days after the operation. The results of analysis, given in tabular form, show after neurotomy an increase of glycogen in 8, a normal amount in 3, and a decrease in 4 cases ; after tenotomy an increase in 6, a normal amount in 8, and a, decrease in 2 cases. The general result is therefore that in the pathologic81 condition of muscle produced by section of its nerve or of its tendon, metabolism is altered in such a way that glycogen is not got rid of so easily as in healthy muscle. Lactic Acid in the Blood. By G. SALOMON (Tirchow’s Archiu, 113, 356--36O).-Gaglio (Arch. Anat. Physiol., Phys. Abth., 1886, 400), and Berlinerblau (Abstr., 1888, 974) have described lactic acid as a constituent of blood.The author has for some years made similar observations in cases of disease. Thus in a specimen of leucaemic blood he found 0*05-0*06 per cent. of lactic acid ; in pleural exudation from a case of carcinoma, there was a percentage of 0.007. I n both cases, estimation of the water of crystallisation, and of the zinc in the zinc salt showed that sarcolactic acid was the particular form of lactic acid that was present. More extended observations, however, have shown that lactic acid in the blood is not characteristic of the diseases mentioned, but can be obtained from the blood of patients who have died from nearly every variety of disease. Observations on the blood removed from the vessels during life show, however, that lactic acid is then as constantly absent as it is present in the blood examined after death.If the blood is examined immediately it is drawn, lactic acid is found to be absent, but if the blood is allowed to stand a short time and then examined, the acid will then be found. Its formation is connected with the ferment actions that set in in shed blood, or in blood left in contact with dead tissues. If it is formed a t all during life, it must be rapidly oxidised, and so cannot be discovered in living blood. W. D. H. W. D. H. Micro-organisms and Proteolytic Digestion. By V. D. HARRIS and H. H. TOOTH (J. Physiol., 9, 220-‘L26).-The experiments of which this is a preliminary account gave the following results :- (1.) The general belief that micro-organisms need take no part in gastric digestion, and are generally absent was confirmed. (2.) Experiments to prove that micro-organisms are themselves competent to convert prote’ids into peptone were very unsatisfactory ; albumoses have been noticed, but never true peptone.Perhaps some special micro-organism is necessary.PEYSIOLOGICATI CHEMISTRY. 65 (3.) As i t was found exceedingly difficult to exclude micro- organisms in pancreatic digestions by employing strictly the principles of Listerian surgery in the removal of the pmcreas, the organisms were killed by the addition of antiseptic reagents, of which mercuric chloride and phenol were found to be the most effective. It was found that the tryptic ferment is able to convert proteids into peptone without the aid of micro-organisms, although that is no proof that the micro-organisms do not assist in the action in the intestine.Phenul, however, either prevents the pancreatic ferment from forming leucine and tyrosine, or else the formation of these substances depends in part a t all events on bacteria. (4.) With regard to the production of indole, it was found that the appearance of indole and its allies in alkaline pancreatic fluids is very capricious and can be easily prevented. I n plugged flasks, it may not appear for a considerable time, no other precaution being taken than that of simply plugging the flasks, micro-organisms being present in large numbers. The smallest amount of mercuric chloride or phenol, even if not sufficient to render the liquid aseptic, also prevents the for- mation of these substances.Indole appears moet readily in the difrec- tion of uncoagulnted (unboiled) proteids. Whenever it is present, lar: e numbers of all sorts of bacteria are there also, still it may be absent even if swarms of micro-organisms are present. I t thus appears that there are special indole-forming orga.nibms. Experiments with pure cultivations of the different forms of bacteria found are, however, at present incomplete. As a result of inoculation of solutions of pure peptone, and of solutions of leucine and tyrosiue with a mixture of bacteria potent to cause the formation of indole, it was found that indole is formed from the peptone, not from leucine or tyrosine. It seems, therefore, likely that the formation of indole and its allier in the alimentary canal below the stomach is ail alternative course for the excretion of nitrogen to that by the formation of leucine and ty rosin e .W. L). H. Glycogen in Diabetic Urine. By W. LEUBE (Vimhow’s Archiu, 113, 391-393).-E. Iteiuhardt (&it. anal. Chem., 1875) has de- scribed ‘. destiin ’’ as occurring in diabetic urine. Glycogen haq, however, never been detected before. Two cases were examinetl in the present research. A large amount of urine (3-5 litres) was precipitated with alcohol, the precipitate collected and washeii free from sugar. The precipitate was then dissolved in water, ant1 the solution gave a brown colour with iodine ; on boiling the solu- tion with 10 per cent. of sulphuric acid, the carbohydrate (probably glycogen) was converted into dextrose.In one of the two cases, the amount of glycogen present was very small. It is consideretl probable that the sugar in the blood is partly converted into glycogen a s it passes through the epithelium of the urinary tubules. W. D. H. Aromatic Substances in Febrile Urine. By J. S. HALDANF; (J. Yhysiol., 9, 213--219).-Diseases and conditions of the bod! where putrefactive changes are greater than normal, cause the a1)- VOL. LVI. f66 ABSTRACTS OF CHEMICAL PAPERS. pearance of an increased quantity of certain aromatic substances, phenol, cresol, indole, scatole, &c., in the urine. Brieger (Zeit. klin. -Wed., 3,465) classes, however, scarlet fever and diphtheria as putrefactive diseases with erysipelas and pyaemia i u which putrefactive processes no doubt often go on.It seemed advisable therefore to repeat these observations with regard to scarlet fever and diphtheria, especially as Brieger's method, which consisted in weighing the phenol as tribromophenol, was found to be wanting in accuracy. -It was found that the more concentrated the urine, the greater was the quantity of tribromopbenol obtainable from it, on account of the solubility of the bromine-water precipitate. In fact, on comparing Brieger's results with control experiments performed with a wine concentrated to different extents, it was found that the illcrease in phenol as described by Brieger i n scarlet fever and diphtheria, could be equally well explained by the rise of the specific gravity of the urine in those diseases.The method adopted was therefore that of estimating the proportion of sulphuric acid coiii- bined as ethereal hydrogen sulphates to that combined as ordinary sulphates. Taking the normal proportion as 1 to 10, it was found io 16 cases of scarlet fever in which the urinewas passed during the feyer to be 1 to 17, and in 13 cases in which the urine was passed during tlle first three days of convalescence to be 1 to 21 : so far as the chemical composition of the urine goes, there is thus no ground f o r regarding scarlet fever as analogous to a putrefactive process. The average of the ratio in five analyses made in cases of diphtheria was 1 to 13, hence in these cases also there was no increase in the elimination of aromatic substances. W. D. H. Physiological Action of Para- and Meta-phenylenedi- amine.By R. DLTBOIS and L. VIGNON (Conzpt. reud., 107, 533- 535).-i?Ieta- and para-phenylenediamines are similar in constitution to the ptomaines and leucoma'ines, and their physiological action is therefore of considerable interest. In doses of 8.1 gram per kilo. of body-weight, both compounds produce salivation, vomiting, diarrhea, excessive emission of uriiie, and coma. Death follows in two to three hours in the case of the pdra-derivative arid in 15 hours with the meta-derivative. The com- pounds remove oxygen from the blood and tissues in the same way as micro-organisms which are rapidly multiplying. and the brownish products thus formed impart a dark colour t o the blood and tissues. Metaphenylenedianiirie produces in the dog all the symptoms of agqravated influenza, with continual sneezing and a hoarse cough, which ends in coma and death.Paraphenyleiiediamine produces very remarkable exophthalmia, the tissues of the eye undergoing complete alteration. C. H. B.PHYSIOLOGICAL CHEMISTRT.P h y s i o l o g i c a l C h e m i s t r y .ti3The Nature of Fibrin Ferment. By W. D. HALLIBURTON (J.Physiol., 9, 227-286).-This paper gives a full account of theresearches of which a preliminary account has already been published(Abstr., 1888, 974). W. D. H64 ABSTRACTS OF CKERIICAL PAPERS,The Glycogen in Muscle after Section of its Nerve and itsTendon. By E. KRAIJSS ( V~TC~OW’S Archiv, 113,325-332). -The firstpart of this paper is devoted to the histological changes that occur inmuscle after nenrotomy and tenotomy respectively.For the glycogen estimations, the tendo Achillis was divided in21 rabbits, and the sciatic nerve in 16 others.The animals werethen fed for 1 to 3 days before death with 15-30 grams of sugardissolved in water. The glycogen was determined by Kiilz’ method(Abstr., 1886, 494). The animals were killed a t different periodsvarying from 2 to 124 days after the operation.The results of analysis, given in tabular form, show after neurotomyan increase of glycogen in 8, a normal amount in 3, and a decreasein 4 cases ; after tenotomy an increase in 6, a normal amount in 8,and a, decrease in 2 cases. The general result is therefore that in thepathologic81 condition of muscle produced by section of its nerve orof its tendon, metabolism is altered in such a way that glycogen isnot got rid of so easily as in healthy muscle.Lactic Acid in the Blood. By G.SALOMON (Tirchow’s Archiu,113, 356--36O).-Gaglio (Arch. Anat. Physiol., Phys. Abth., 1886,400), and Berlinerblau (Abstr., 1888, 974) have described lactic acidas a constituent of blood. The author has for some years madesimilar observations in cases of disease. Thus in a specimen ofleucaemic blood he found 0*05-0*06 per cent. of lactic acid ; in pleuralexudation from a case of carcinoma, there was a percentage of 0.007.I n both cases, estimation of the water of crystallisation, and of thezinc in the zinc salt showed that sarcolactic acid was the particularform of lactic acid that was present.More extended observations, however, have shown that lactic acidin the blood is not characteristic of the diseases mentioned, but can beobtained from the blood of patients who have died from nearly everyvariety of disease.Observations on the blood removed from thevessels during life show, however, that lactic acid is then as constantlyabsent as it is present in the blood examined after death.If the blood is examined immediately it is drawn, lactic acid isfound to be absent, but if the blood is allowed to stand a short timeand then examined, the acid will then be found. Its formation isconnected with the ferment actions that set in in shed blood, or inblood left in contact with dead tissues. If it is formed a t all duringlife, it must be rapidly oxidised, and so cannot be discovered in livingblood.W. D. H.W. D. H.Micro-organisms and Proteolytic Digestion. By V. D. HARRISand H. H. TOOTH (J. Physiol., 9, 220-‘L26).-The experiments ofwhich this is a preliminary account gave the following results :-(1.) The general belief that micro-organisms need take no part ingastric digestion, and are generally absent was confirmed.(2.) Experiments to prove that micro-organisms are themselvescompetent to convert prote’ids into peptone were very unsatisfactory ;albumoses have been noticed, but never true peptone. Perhaps somespecial micro-organism is necessaryPEYSIOLOGICATI CHEMISTRY. 65(3.) As i t was found exceedingly difficult to exclude micro-organisms in pancreatic digestions by employing strictly the principlesof Listerian surgery in the removal of the pmcreas, the organismswere killed by the addition of antiseptic reagents, of which mercuricchloride and phenol were found to be the most effective.It wasfound that the tryptic ferment is able to convert proteids into peptonewithout the aid of micro-organisms, although that is no proof that themicro-organisms do not assist in the action in the intestine. Phenul,however, either prevents the pancreatic ferment from forming leucineand tyrosine, or else the formation of these substances depends in parta t all events on bacteria.(4.) With regard to the production of indole, it was found that theappearance of indole and its allies in alkaline pancreatic fluids is verycapricious and can be easily prevented.I n plugged flasks, it maynot appear for a considerable time, no other precaution being taken thanthat of simply plugging the flasks, micro-organisms being present inlarge numbers. The smallest amount of mercuric chloride or phenol,even if not sufficient to render the liquid aseptic, also prevents the for-mation of these substances. Indole appears moet readily in the difrec-tion of uncoagulnted (unboiled) proteids. Whenever it is present, lar: enumbers of all sorts of bacteria are there also, still it may be absenteven if swarms of micro-organisms are present. I t thus appears thatthere are special indole-forming orga.nibms. Experiments with purecultivations of the different forms of bacteria found are, however, atpresent incomplete. As a result of inoculation of solutions of purepeptone, and of solutions of leucine and tyrosiue with a mixture ofbacteria potent to cause the formation of indole, it was found thatindole is formed from the peptone, not from leucine or tyrosine.Itseems, therefore, likely that the formation of indole and its allier inthe alimentary canal below the stomach is ail alternative course forthe excretion of nitrogen to that by the formation of leucine andty rosin e . W. L). H.Glycogen in Diabetic Urine. By W. LEUBE (Vimhow’s Archiu,113, 391-393).-E. Iteiuhardt (&it. anal. Chem., 1875) has de-scribed ‘. destiin ’’ as occurring in diabetic urine. Glycogen haq,however, never been detected before. Two cases were examinetlin the present research.A large amount of urine (3-5 litres)was precipitated with alcohol, the precipitate collected and washeiifree from sugar. The precipitate was then dissolved in water, ant1the solution gave a brown colour with iodine ; on boiling the solu-tion with 10 per cent. of sulphuric acid, the carbohydrate (probablyglycogen) was converted into dextrose. In one of the two cases, theamount of glycogen present was very small. It is consideretlprobable that the sugar in the blood is partly converted intoglycogen a s it passes through the epithelium of the urinary tubules.W. D. H.Aromatic Substances in Febrile Urine. By J. S. HALDANF;(J. Yhysiol., 9, 213--219).-Diseases and conditions of the bod!where putrefactive changes are greater than normal, cause the a1)-VOL. LVI.66 ABSTRACTS OF CHEMICAL PAPERS.pearance of an increased quantity of certain aromatic substances,phenol, cresol, indole, scatole, &c., in the urine.Brieger (Zeit. klin. -Wed., 3,465) classes, however, scarlet fever anddiphtheria as putrefactive diseases with erysipelas and pyaemia i uwhich putrefactive processes no doubt often go on. It seemedadvisable therefore to repeat these observations with regard toscarlet fever and diphtheria, especially as Brieger's method, whichconsisted in weighing the phenol as tribromophenol, was found tobe wanting in accuracy. -It was found that the more concentratedthe urine, the greater was the quantity of tribromopbenol obtainablefrom it, on account of the solubility of the bromine-water precipitate.In fact, on comparing Brieger's results with control experimentsperformed with a wine concentrated to different extents, it was foundthat the illcrease in phenol as described by Brieger i n scarlet feverand diphtheria, could be equally well explained by the rise of thespecific gravity of the urine in those diseases.The method adoptedwas therefore that of estimating the proportion of sulphuric acid coiii-bined as ethereal hydrogen sulphates to that combined as ordinarysulphates. Taking the normal proportion as 1 to 10, it was found io16 cases of scarlet fever in which the urinewas passed during the feyerto be 1 to 17, and in 13 cases in which the urine was passed duringtlle first three days of convalescence to be 1 to 21 : so far as thechemical composition of the urine goes, there is thus no ground f o rregarding scarlet fever as analogous to a putrefactive process.The average of the ratio in five analyses made in cases ofdiphtheria was 1 to 13, hence in these cases also there was no increasein the elimination of aromatic substances. W. D. H.Physiological Action of Para- and Meta-phenylenedi-amine. By R. DLTBOIS and L. VIGNON (Conzpt. reud., 107, 533-535).-i?Ieta- and para-phenylenediamines are similar in constitutionto the ptomaines and leucoma'ines, and their physiological actionis therefore of considerable interest.In doses of 8.1 gram per kilo. of body-weight, both compoundsproduce salivation, vomiting, diarrhea, excessive emission of uriiie,and coma. Death follows in two to three hours in the case of thepdra-derivative arid in 15 hours with the meta-derivative. The com-pounds remove oxygen from the blood and tissues in the same wayas micro-organisms which are rapidly multiplying. and the brownishproducts thus formed impart a dark colour t o the blood and tissues.Metaphenylenedianiirie produces in the dog all the symptoms ofagqravated influenza, with continual sneezing and a hoarse cough,which ends in coma and death. Paraphenyleiiediamine producesvery remarkable exophthalmia, the tissues of the eye undergoingcomplete alteration. C. H. B

ISSN:0368-1769    

DOI:10.1039/CA8895600063

出版商:RSC    

年代:1889

数据来源: RSC

摘要:

VEGETABLE PHYSIOLOGY AND XQRICULTURE. 67 Chemistry of Vegetable Physiology and Agriculture. Action of Micro-organisms on cert -tin Colouring Matters. By J. RAULIN (Corn@. rend., 107, 4B.;-447).-A.~1eergillus niger will grow in cultivation liquids containing ammonium nitrate, but not in similar liquids containing salts of aniline, rosaniline or indigo- carmine. Slightly acidified yeast solution, beer wort, and sugar solution tinted with indigocarmine, slowly decolorise in presence of air arid in absence of all organisms, but this change is due to oxidation and does not take place in an atmosphere of carbonic anhydride. Certain aikobic organisms retard or prevent decolorisation by pre- venting the access of oxygen. Active beer-y east also decolorises indigocarmine in absence of ;)xygen, but decolorisation is due to reduction and the colour returns if the liquid ir, exposed to air.I n this case, reduction is accompanied by the development of micro-organisms similar in ap- pearance to the lactic ferment. The change takes place most rapidly i f the yeast solution has been exposed to the air a t 2 4 O for several days ; it then acquires a putrid odour and is full of bacteria. The rate of decolorisation increases with an increase ill the number of orpanisms, and the addition of an antiseptic, or any other cause which destroys the organisms, prevents the changes. Reduction is due to changes connected with the vital processes of the organisms, and is not due to the liberation of hydrogen. It is not analogous to the reduction of indigocarmine by an alkaline solution of glucose, since in that case the presence of organisms is not essential.Similar reducing actions were observed with logwood, orchil, cochineal, safranin, and several artificial colouring matters. C. H. B, Decolorisation of Tincture of Turnesole in closed Vessels. By R. DUBOIS (Bull. Xoc. Chew., 49, 963-964).-Tbe decolorisation of turnesole kept in a closed vessel is entirely due to the action of wrnis, as when the solution is sterilised the blue colour is permanent. The colourless solution contains only one species of liring organisms ; this is a very small, completely spherical micrococcus, which can be cultivated in slightly alkaline peptonised gelatin. The liquid de- colorised by these micro-organisms a t once regains its blue colour on exposure to the air.Formation of Starch from Various Substances. Bg T. BOKORNY (Chem. Cenir., 1888, 858-4339, from Bey. deut. bot. Ges., 6, 116--120).-Since earlier experiments had proved that a l p can be fed with methylal, the author has shown, by means of further experi- ments, that starch is formed from methylal. Spirogyra were used as the material for the investigation. Whilst in the absence of light, the formation of starch could not be observed, its formation could be readily detected after the spirogyra had lain in 1-0-1 per cent. I?. S. K. f 268 ABSTRACTS OF CHEMICAL PAPERS. methylal in the sunlight. Spirogyra fed on solution of methvl alcohol of' the same strength, namely, 1-0.1 per cent., showed a t the end of 6 to 24 hours a very considerable new formation of starch.The author finds that glycol and glyeerol, like mannitol, are also able to form starch. J. W. L. By H. MOLISCH (Ann. Agronom., 14, 334--335).-1t is known that roots excrete an acid juice capable of attacking minerals. The author finds that the liquid has much more extensive powers, namely, it has both reducing and oxidising pro- perties; turns tiiicture of guaiacum blue ; oxidises tannins and humic substances, and consequmtly promotes the decomposition of hunius : transforms cane-sugar into reducing sugar, and acts feebly like diastase ; corrodes a plate of ivory ; and modifies the organic matter of soil. The root membranes are not simply permeated with this juice, it may sometimes 'be seen to exude in dnoplets. Matter Excreted by Roots.J. M. H. M. Occurrence of Solid Hydrocarbons in 'the Vegetable King- dom. By H. GUTZEIT (Rer., 21, 2881-2882. Compare Abbot and Trirnble, Abstr., 1888, 1329).-The author points out that he has already described solid hydrocarbons which were obtained from the fruit of Heracleum giganteurn, hfirt., Eeracleum spondylium, L., and Pastinnca sativa, L. (Beitrage zur Pflmueirchemie, Jena, 1879), and that others have already proved the presence of such compounds in the vegetable kingdom. F. S. K. Constituents of Bark of Rhamnus Frangula and R. Purshiana. By P. SCHWABE (Arch. P h ~ m . [3], 26, 569-594).- The coarsely powdered bark is freed from f a t by means of ether, and extracted with 98 per cent. alcohol ; the extract is mixed with several times its volume of water, and is shaken up by portions with ether.The first ethereal solutions are dark coloured, but on repeating the operation 10 or 1'2 times the ether remains colourless. The unit)ecl ethereal solutions are distilled, when a light-yellow deposit forms in thin layei s on the side of the vessel. The deeply coloured mother-liquor is filtered after remaining 24 hours. The residue on the filter is repeatedly washed with alcohol and ether, and finally crjstallised several times from boiling alcohol, until the microscope shows distinct crystallisation, undoubtedly due to frangulin. The mother-liquor filtered from frangulin was brcught to dryness, taken up with a little alcoliol, mixed with several times its weight of water and again shaken up with ether, but only once or twice ; in this way the beauti- fully crystalline body emodin (trihydroxjmethylanthraquinone) was srpalated.On distilling off the ether, tLe residue is readily seen under a lens to be permeated with crystals. This is heated with glacial acetic acid, in which it readily dissolves, and on cooling emodin crptallises out. Recrystallisation yields emodin as a light red crptalline mass, which melts at 254". The yield was fran- gulin 0.06 per cent., and emodin 0.10 per cent,. Fresh bark gaye no frai:gulin, thus confirming an observation previously made by Castelmann ; whilst bark a year and a-half old gave frangulin 0.04 perVEQETABLE PHTSIOLOOE. AND AQRICULTURE. 69 cent., and emodin 0.10 per cent. as before. Emodin, C15H1005 + HzO, gives red to brown-red amorphous precipitates with the alkaline earths and with lead, copper, and mercury salts.It dissolves in dilute alkalis to a splendid dark cherry-red colour, but gives no crystals on evaporation. A solution in alcoholic potash, heated at 100" in a sealed glass tube, showed fine needle-like aggregates after standing nilopened for 24 hours. FranguZin melts a t 228" to 230°, whilst, Casselmann puts it a t 249" and Faust a t 226", the differences being due to impurity in the last two cases. It is almost insoluble in water and ether, more easily in chloroform, benzene, and alcohol, and very soluble in liot acetic acid. When dry, it forms a beautiful, light- yellow, brittle mass, with somewhat silky lustre. Its composition is C,,H,,09. Four to five hours' boiling with 20 per cent.sulphnric acid converts it into emodin and glucose. If anywllere, frangulinic acid should make its appearance here, but the compound previously described under this name is identical with emodin. The coarsely powdered root of RhanawuspurshiaJna (Cascara sagrada) was extracted with ether, and then with 98 per cent. alcohol. After the addition of water, the ether extract' was shaken repeatedly with light petroleum until the oily extracts became almost colour- less. On removing the petroleum, the dark-coloured mother-liquor gave an immediate brown-red, flocculo-crystalline precipitate. As in the case of Rhamnus frangda bark, the alcoholic extract shaken up with ether after the addition of water afforded a crystalline product. The petroleum product which proved to be identical with this, was found to be emodin.Fraiigulin was not present, although i t may possibly occur in older bark. J. T. Japanese Tobaccos. By M. PESCA and H. IMAI ( B i d Cenfr., 1888,629-637).-The authors analysed the soils and the tobaccos produced in a locality in Opmada, and also one other Japanese tobacco. Permeability and a certain amount of humus are far more important as regards the soil than the amount of plant food, as the latter can be supplied by manuring. The best tobacco soil exhibited only a moderate absorptive power for bases. The manures applied are human and animal excreta, wood and straw ashes, and bath-water. As regards analysis as a means of judging the quality of a tobacco, the authors came to the following conclusions :-(1.) Just as an alco- holic drink should contain a certain percentage of alcohol, so a tobacco should contain a certain percentage of nicotine ; but that the quality of a tobacco depends on the percentage of the nicotine has not yet beenproved.(2.) Nitric acid is not contained in well-fermented tobaccos. ( 3 . ) The ammonia in the older analyses was too high, as it included some that came from amides. The ammonia, which only comes to some tenths of a per cent., cannot account for lowered quality. (4.) The amount of albumino'ids, reckoned as it formerly was, without allowing for the amide-iiitrogen present, affords no standard for judging tobacco. The worst tobacco analysed had the lowest total nitrogen, yet owing to the nicotine and amides being very low, it had the highest amount of albuminoids.( 5 . ) Arnide nitrogeii for the most part indicates the presence of compounds which do not injure and perhaps even enhance70 ABsTRACTS OF CHEMICAL PAPERS. the quality of the tobacco. One of the most important duties of the fermentation is to change albumino'ids into amides. (6.) The deter- mination of the amount of substances that ether extracts is of bnt little use. (7.) Carbohydrates, with the exception of cellulose, should not be present in well-fermented tobacco. A study of their decomposition, and of the formation and decomposition of organic acids and of amides should prove useful in determining the quality and guiding the culture and treatment of tobacco. (8.) Dis- tinctions as to quality can only be drawn when the differences in the amounts of the substances estimated are considerable, and they can only be made safely when the whole composition proves quite satis- factory or quite the reverse ; they can rarely be drawn from differences in the amounts of single substacces.Inferiority can be more safely inferred than superiority. In very bad tobacco, the albuminojids, the sulphuric acid, the clilorine and generally the mineral acids are high, whilst the amide nitrogen and the potash are low. (9.) To indicate good quality and especially combustibility, there should be a medium amount of bases, especially of potash and lime. Within certain limits these bases appear capable of replacing one another. The percentage of one or the other must fall very low before it is to be regarded as a bad indication.Magnesia, if exceptionally high, appears to injure the combustibility. (10.) Mineral acids if high indicate bad combustibility ; but they must be exceptionally high t'o surely indicate low value. Apart from silica, phosphoric acid appeal s to be the least injurious, chlorine considerably more, and sulphuric acid the most injurious to the quality and combustibility. (11.) 'l'hc bases soluble in water and either free or existing as carbonates, appear to have no important influence, but, the amount of carbonic anhydride up to a certain point indicates increased combustibility, and a large amount of carbonates in proportion to mineral salts indicates good value. (12.) A high proportion of bases in the ash, provided it is not caused by magnesia or iron, points especially to good combusti- bility.H. H. R. The remaining conclusions relate to the ash constituents. Formation of Nitrates in Soils of different Degrees of Fertility. By P. P. DEH~RATN (Ann. Agronom., 14, 289-320).-1t appears probable, from the researches of Lawes and Gilbert, War- ington, and others, that a soil exhausted by cropping contains only nitrogenous organic matter difficult to nitrify, and that the relative sterility which is produced by a number of successive crops without manure, is due not only to a decrease in the total amount of nitroqen, but also to the residual nitrogenous matter being less apt to nitrify than that in a fertile soil. To obtain confirmation of this, the author has studied the rate of nitrification in different soils, fertile and exhausted, manured and unmanured, under different conditions of humidity, temperature, division, &c.A few only of the results, most of which are provisional and require further elucidation, are given below. A saturated atmosphere is ultimately unfavourable to nitrifi- cation ; probably because monlds are encouraged which destroy the nitrate. Soil very 6nely sifted, placed in a funnel, and submitted toVEGETABLE PHYSIOLOGY AND AGRICULTURE. 71 frequent waterings, so as to alternate periods of comparative dryness and moistlure, is very favourably circumstanced for nitrification ; for example, in the 189 days from 1 7 t h May to 22nd November, there was formed per 1000 kilos. of soil, 880 grams nitric acid: reckoning the weight of the soil at 3600 tonnes per hectare, this would give 819.8 kilos.nitrogen per hectare nitrified in that space of time, a quantity infinitely superior to the requirements of the most exhausting crop. The waterings in this experiment were equivalent to five times the normal rainfall. The accumulation of nitrate i i i the soil, at any rate t o the extent of 700 mgrrns. per kilo., does not retard the rate of nitrification. The organic matter was more nitrifiable at the com- mencement of the experiment than afterwards, since much more nitrate was formed in the first 27 days than in any subsequent similar period, notwithstanding the lower temperature of this first month as compared with the two following. Again, in the December to January period more nitrogen was nitrified per diem than in the October +,o November period, in spite of the lower temperature ; from this the author infers that the organic matter of the soil is subject from time to time to changes rendering it more or less easy of nitrification.Trituration of the soil and elevation of temperature were both found to greatly accelerate nitrification. The addition of sodium nitrate t o the soil in quantities of 0.06 and 0.60 per cent. almost prevented nitri- fication for the first 40 days, and greatly retarded it during a subsequent like period, although eventually nitrification at something Iike the normal rate occurred; the addition of 1 : 1000 of common salt to the soil exercises little or no effect, 2.5 : 1000 is injurioua, and 5 : 1000 prevents nitrification. Three soils, long unmanured and poor in nitrogen, developed very little nitrate for some weeks after being placed in circumstances the most favourable for nitrification, but afterwards fairly rapid nitrifi- cation set in, which the author attributes to changes undergone by the organic matter under the new conditions.A fourth poor soil, unma.nured and equally poor in nit,rogen with the other three, proved, however, very nitrifiable, it developed from the first more nitrate than a fertile soil placed in the same conditions. J. M. H. M. Loss and Gain of Nitrogen in Agriculture. By B. FRANK (Bied. Cerh., 1888, 610-617) .-Among the sources of loss is the volatilisation of animonia from the soil. In some experiments in which ammonium sulphate solution was added to samples of soil, the author found that the ammonia thus added soon disappeared, being to a small extent converted into nitrates whilst the greater part volatilised.A light and pure sandy soil does not expel the ammonia and has only a feeble nitrifying power, so that the ammonium salt is retained nearly undiminished for a long time. Of the individual constituents, quartz grains and clay are inactive, whilst calcium carbonate causes both slow nitrification and also partial liberation of ammonia. Another source of loss was mentioned by Boussingault, namely, that when nitrates were given to plants growing in the dark, there was a libera- tion of free nitrogen, which be attributed to the action of some organic substance excreted by the roots. The author experimented72 ABSTRACTS OF CHEMICAL PAPERS.on the point, growing bean seeds in the dark in nutritive solutions, both with and without nitrogen compounds. As in every case there was a loss of nitrogen, it could not be due to reduction of nitrates, and he attributes it to the loss of nitrogen consequent on the decay of those parts of the seed not made use of by the germinating plant. Next, treating of the gain of nitrogen, he combats Hellriegel's view that the root nodules of the Leguminosae are concerned in rendering free nitrogen available to the plant. His own experiments lead him to the coriclusion that the land gains in combined nitrogen in some way besides that caused by lightning discharges, which at present is the only one undisputed. He found that the presence of vegetation raised the amount of this gain, that this could not be accounted for by the ammonia of the air, and that it must be derived from the free nitrogen of the air.The gain rises with increased plant development, and both the kind of soil and the species of plant have an influence. Lupines are very effective as compared with non-leguminous plants ; but the difference in the powers of increasing the combined nitrosen is one of degree, not one of kind ; hence it cannot be ascribed to the nodules. Further, nodules did not occur in lupines grown in sterilised soil, yet the plants developed better than in a pardlel experiment with unsterilised soil where the plants had nodules, and besides the nodules the legumes have no other organs to siipply nitrogen which other plants do not also possess.The next question is how soil unoccupied by a crop gains in combined nitrogen. This gain takes the form chieHy or entirely of organic nitrogen compounds, thus agreeing with Ber- thelot's experiments, and is explained by the growth in the soil of the cryptoganiic plants, algae containing chlorophyll and allied forms which the author discovered there. He next discusses the question whether these plants avail themselves of free nitrogen or of nitrogen oxidised in the soil by an inorganic process. He asserts that under the influence of calcium or magnesium carbonates free nitrogen can be oxidised to nitric acid, the action being distinct a t lOO", still apparent a t 45-50', and no longer apparent a t 15-22", but thinks that in the German climate this action can only very rarely occur.He con- cludes that it is not an inorganic process that makes the free nitrogen available, but that the combined nitrogen is due to a development of plant cells containing albumino'ids which is not to be connected with any process occurring in the soil. This power of assimilating free nitrogen is very different for different plants; the result is smallest in fallow land, where only the lower plant forms are at work; it is larger with hjghsr plant forms, and among these the lupines and probably other Leguminosae produce the greatest result. H. H. R. Action of Superphosphate on Nitrates. By A. DWARDA (Chew. Ceiztr., 1888, 899--900).-Experirnents by the author go to show that, at the ordinary temperature, the phosphoric acid, hydro- flouric acid, and readily decomposable organic compounds, as well as ferrous salts present in superphosphates, cause no loss of nitrogen from nitrates which may have been mixed with them.In those cases, however, where the mixtures are exposed to a moderately high temperature, the loss of nitrogen is considerable, although in thisANALYTICAL CHENIST RY. 73 case the ferrous compounds take no part in the reaction. The author also found that iii mixtures of superphosphate and nitrates the soluble phosphate becomes insoluble much more quickly than when the nitrate is omitted, and the mixing of nitrate with superphos- phate for any length of time is therefore not to be recommended. J. W. L.VEGETABLE PHYSIOLOGY AND XQRICULTURE. 67Chemistry of Vegetable Physiology and Agriculture.Action of Micro-organisms on cert -tin Colouring Matters.By J.RAULIN (Corn@. rend., 107, 4B.;-447).-A.~1eergillus nigerwill grow in cultivation liquids containing ammonium nitrate, but notin similar liquids containing salts of aniline, rosaniline or indigo-carmine.Slightly acidified yeast solution, beer wort, and sugar solutiontinted with indigocarmine, slowly decolorise in presence of air aridin absence of all organisms, but this change is due to oxidation anddoes not take place in an atmosphere of carbonic anhydride.Certain aikobic organisms retard or prevent decolorisation by pre-venting the access of oxygen.Active beer-y east also decolorises indigocarmine in absence of;)xygen, but decolorisation is due to reduction and the colourreturns if the liquid ir, exposed to air.I n this case, reduction isaccompanied by the development of micro-organisms similar in ap-pearance to the lactic ferment. The change takes place most rapidlyi f the yeast solution has been exposed to the air a t 2 4 O for severaldays ; it then acquires a putrid odour and is full of bacteria. Therate of decolorisation increases with an increase ill the number oforpanisms, and the addition of an antiseptic, or any other causewhich destroys the organisms, prevents the changes. Reduction isdue to changes connected with the vital processes of the organisms,and is not due to the liberation of hydrogen. It is not analogous tothe reduction of indigocarmine by an alkaline solution of glucose,since in that case the presence of organisms is not essential.Similar reducing actions were observed with logwood, orchil,cochineal, safranin, and several artificial colouring matters.C.H. B,Decolorisation of Tincture of Turnesole in closed Vessels.By R. DUBOIS (Bull. Xoc. Chew., 49, 963-964).-Tbe decolorisationof turnesole kept in a closed vessel is entirely due to the action ofwrnis, as when the solution is sterilised the blue colour is permanent.The colourless solution contains only one species of liring organisms ;this is a very small, completely spherical micrococcus, which can becultivated in slightly alkaline peptonised gelatin. The liquid de-colorised by these micro-organisms a t once regains its blue colour onexposure to the air.Formation of Starch from Various Substances.Bg T.BOKORNY (Chem. Cenir., 1888, 858-4339, from Bey. deut. bot. Ges.,6, 116--120).-Since earlier experiments had proved that a l p can befed with methylal, the author has shown, by means of further experi-ments, that starch is formed from methylal. Spirogyra were used asthe material for the investigation. Whilst in the absence of light,the formation of starch could not be observed, its formation could bereadily detected after the spirogyra had lain in 1-0-1 per cent.I?. S. K.f 68 ABSTRACTS OF CHEMICAL PAPERS.methylal in the sunlight. Spirogyra fed on solution of methvl alcoholof' the same strength, namely, 1-0.1 per cent., showed a t the end of6 to 24 hours a very considerable new formation of starch.Theauthor finds that glycol and glyeerol, like mannitol, are also able toform starch. J. W. L.By H. MOLISCH (Ann. Agronom., 14,334--335).-1t is known that roots excrete an acid juice capable ofattacking minerals. The author finds that the liquid has much moreextensive powers, namely, it has both reducing and oxidising pro-perties; turns tiiicture of guaiacum blue ; oxidises tannins and humicsubstances, and consequmtly promotes the decomposition of hunius :transforms cane-sugar into reducing sugar, and acts feebly likediastase ; corrodes a plate of ivory ; and modifies the organic matterof soil. The root membranes are not simply permeated with thisjuice, it may sometimes 'be seen to exude in dnoplets.Matter Excreted by Roots.J.M. H. M.Occurrence of Solid Hydrocarbons in 'the Vegetable King-dom. By H. GUTZEIT (Rer., 21, 2881-2882. Compare Abbot andTrirnble, Abstr., 1888, 1329).-The author points out that he hasalready described solid hydrocarbons which were obtained from thefruit of Heracleum giganteurn, hfirt., Eeracleum spondylium, L., andPastinnca sativa, L. (Beitrage zur Pflmueirchemie, Jena, 1879), and thatothers have already proved the presence of such compounds in thevegetable kingdom. F. S. K.Constituents of Bark of Rhamnus Frangula and R.Purshiana. By P. SCHWABE (Arch. P h ~ m . [3], 26, 569-594).-The coarsely powdered bark is freed from f a t by means of ether, andextracted with 98 per cent. alcohol ; the extract is mixed with severaltimes its volume of water, and is shaken up by portions with ether.The first ethereal solutions are dark coloured, but on repeating theoperation 10 or 1'2 times the ether remains colourless.The unit)eclethereal solutions are distilled, when a light-yellow deposit forms inthin layei s on the side of the vessel. The deeply coloured mother-liquoris filtered after remaining 24 hours. The residue on the filter isrepeatedly washed with alcohol and ether, and finally crjstallisedseveral times from boiling alcohol, until the microscope shows distinctcrystallisation, undoubtedly due to frangulin. The mother-liquorfiltered from frangulin was brcught to dryness, taken up with a littlealcoliol, mixed with several times its weight of water and againshaken up with ether, but only once or twice ; in this way the beauti-fully crystalline body emodin (trihydroxjmethylanthraquinone) wassrpalated. On distilling off the ether, tLe residue is readily seenunder a lens to be permeated with crystals.This is heated withglacial acetic acid, in which it readily dissolves, and on coolingemodin crptallises out. Recrystallisation yields emodin as a lightred crptalline mass, which melts at 254". The yield was fran-gulin 0.06 per cent., and emodin 0.10 per cent,. Fresh bark gayeno frai:gulin, thus confirming an observation previously made byCastelmann ; whilst bark a year and a-half old gave frangulin 0.04 peVEQETABLE PHTSIOLOOE. AND AQRICULTURE. 69cent., and emodin 0.10 per cent. as before. Emodin, C15H1005 + HzO,gives red to brown-red amorphous precipitates with the alkaline earthsand with lead, copper, and mercury salts.It dissolves in dilutealkalis to a splendid dark cherry-red colour, but gives no crystals onevaporation. A solution in alcoholic potash, heated at 100" in asealed glass tube, showed fine needle-like aggregates after standingnilopened for 24 hours. FranguZin melts a t 228" to 230°, whilst,Casselmann puts it a t 249" and Faust a t 226", the differences being dueto impurity in the last two cases. It is almost insoluble in waterand ether, more easily in chloroform, benzene, and alcohol, and verysoluble in liot acetic acid. When dry, it forms a beautiful, light-yellow, brittle mass, with somewhat silky lustre. Its composition isC,,H,,09.Four to five hours' boiling with 20 per cent. sulphnricacid converts it into emodin and glucose. If anywllere, frangulinicacid should make its appearance here, but the compound previouslydescribed under this name is identical with emodin.The coarsely powdered root of RhanawuspurshiaJna (Cascara sagrada)was extracted with ether, and then with 98 per cent. alcohol. Afterthe addition of water, the ether extract' was shaken repeatedlywith light petroleum until the oily extracts became almost colour-less. On removing the petroleum, the dark-coloured mother-liquorgave an immediate brown-red, flocculo-crystalline precipitate. Asin the case of Rhamnus frangda bark, the alcoholic extract shaken upwith ether after the addition of water afforded a crystalline product.The petroleum product which proved to be identical with this, wasfound to be emodin.Fraiigulin was not present, although i t maypossibly occur in older bark. J. T.Japanese Tobaccos. By M. PESCA and H. IMAI ( B i d Cenfr.,1888,629-637).-The authors analysed the soils and the tobaccosproduced in a locality in Opmada, and also one other Japanesetobacco. Permeability and a certain amount of humus are far moreimportant as regards the soil than the amount of plant food, as thelatter can be supplied by manuring. The best tobacco soil exhibitedonly a moderate absorptive power for bases. The manures appliedare human and animal excreta, wood and straw ashes, and bath-water.As regards analysis as a means of judging the quality of a tobacco,the authors came to the following conclusions :-(1.) Just as an alco-holic drink should contain a certain percentage of alcohol, so a tobaccoshould contain a certain percentage of nicotine ; but that the qualityof a tobacco depends on the percentage of the nicotine has not yetbeenproved.(2.) Nitric acid is not contained in well-fermented tobaccos.( 3 . ) The ammonia in the older analyses was too high, as it included somethat came from amides. The ammonia, which only comes to some tenthsof a per cent., cannot account for lowered quality. (4.) The amount ofalbumino'ids, reckoned as it formerly was, without allowing for theamide-iiitrogen present, affords no standard for judging tobacco.The worst tobacco analysed had the lowest total nitrogen, yet owingto the nicotine and amides being very low, it had the highest amountof albuminoids.( 5 . ) Arnide nitrogeii for the most part indicates thepresence of compounds which do not injure and perhaps even enhanc70 ABsTRACTS OF CHEMICAL PAPERS.the quality of the tobacco. One of the most important duties of thefermentation is to change albumino'ids into amides. (6.) The deter-mination of the amount of substances that ether extracts is of bntlittle use. (7.) Carbohydrates, with the exception of cellulose,should not be present in well-fermented tobacco. A study of theirdecomposition, and of the formation and decomposition of organicacids and of amides should prove useful in determining thequality and guiding the culture and treatment of tobacco. (8.) Dis-tinctions as to quality can only be drawn when the differences in theamounts of the substances estimated are considerable, and they canonly be made safely when the whole composition proves quite satis-factory or quite the reverse ; they can rarely be drawn from differencesin the amounts of single substacces.Inferiority can be more safelyinferred than superiority. In very bad tobacco, the albuminojids, thesulphuric acid, the clilorine and generally the mineral acids are high,whilst the amide nitrogen and the potash are low.(9.) Toindicate good quality and especially combustibility, there should be amedium amount of bases, especially of potash and lime. Withincertain limits these bases appear capable of replacing one another.The percentage of one or the other must fall very low before it isto be regarded as a bad indication.Magnesia, if exceptionally high,appears to injure the combustibility. (10.) Mineral acids if highindicate bad combustibility ; but they must be exceptionally high t'osurely indicate low value. Apart from silica, phosphoric acid appeal sto be the least injurious, chlorine considerably more, and sulphuricacid the most injurious to the quality and combustibility. (11.) 'l'hcbases soluble in water and either free or existing as carbonates,appear to have no important influence, but, the amount of carbonicanhydride up to a certain point indicates increased combustibility, anda large amount of carbonates in proportion to mineral salts indicatesgood value.(12.) A high proportion of bases in the ash, provided itis not caused by magnesia or iron, points especially to good combusti-bility. H. H. R.The remaining conclusions relate to the ash constituents.Formation of Nitrates in Soils of different Degrees ofFertility. By P. P. DEH~RATN (Ann. Agronom., 14, 289-320).-1tappears probable, from the researches of Lawes and Gilbert, War-ington, and others, that a soil exhausted by cropping contains onlynitrogenous organic matter difficult to nitrify, and that the relativesterility which is produced by a number of successive crops withoutmanure, is due not only to a decrease in the total amount of nitroqen,but also to the residual nitrogenous matter being less apt to nitrifythan that in a fertile soil.To obtain confirmation of this, the authorhas studied the rate of nitrification in different soils, fertile andexhausted, manured and unmanured, under different conditions ofhumidity, temperature, division, &c. A few only of the results, mostof which are provisional and require further elucidation, are givenbelow. A saturated atmosphere is ultimately unfavourable to nitrifi-cation ; probably because monlds are encouraged which destroy thenitrate. Soil very 6nely sifted, placed in a funnel, and submitted tVEGETABLE PHYSIOLOGY AND AGRICULTURE. 71frequent waterings, so as to alternate periods of comparative drynessand moistlure, is very favourably circumstanced for nitrification ; forexample, in the 189 days from 1 7 t h May to 22nd November, there wasformed per 1000 kilos.of soil, 880 grams nitric acid: reckoning theweight of the soil at 3600 tonnes per hectare, this would give 819.8kilos. nitrogen per hectare nitrified in that space of time, a quantityinfinitely superior to the requirements of the most exhausting crop.The waterings in this experiment were equivalent to five times thenormal rainfall. The accumulation of nitrate i i i the soil, at any ratet o the extent of 700 mgrrns. per kilo., does not retard the rate ofnitrification. The organic matter was more nitrifiable at the com-mencement of the experiment than afterwards, since much morenitrate was formed in the first 27 days than in any subsequentsimilar period, notwithstanding the lower temperature of this firstmonth as compared with the two following.Again, in the Decemberto January period more nitrogen was nitrified per diem than in theOctober +,o November period, in spite of the lower temperature ; fromthis the author infers that the organic matter of the soil is subject fromtime to time to changes rendering it more or less easy of nitrification.Trituration of the soil and elevation of temperature were both foundto greatly accelerate nitrification. The addition of sodium nitrate t othe soil in quantities of 0.06 and 0.60 per cent. almost prevented nitri-fication for the first 40 days, and greatly retarded it during asubsequent like period, although eventually nitrification at somethingIike the normal rate occurred; the addition of 1 : 1000 of commonsalt to the soil exercises little or no effect, 2.5 : 1000 is injurioua, and5 : 1000 prevents nitrification.Three soils, long unmanured and poor in nitrogen, developed verylittle nitrate for some weeks after being placed in circumstances themost favourable for nitrification, but afterwards fairly rapid nitrifi-cation set in, which the author attributes to changes undergone bythe organic matter under the new conditions.A fourth poor soil,unma.nured and equally poor in nit,rogen with the other three, proved,however, very nitrifiable, it developed from the first more nitrate thana fertile soil placed in the same conditions. J. M. H. M.Loss and Gain of Nitrogen in Agriculture. By B. FRANK(Bied. Cerh., 1888, 610-617) .-Among the sources of loss is thevolatilisation of animonia from the soil.In some experiments in whichammonium sulphate solution was added to samples of soil, the authorfound that the ammonia thus added soon disappeared, being to a smallextent converted into nitrates whilst the greater part volatilised. Alight and pure sandy soil does not expel the ammonia and has only afeeble nitrifying power, so that the ammonium salt is retained nearlyundiminished for a long time. Of the individual constituents, quartzgrains and clay are inactive, whilst calcium carbonate causes bothslow nitrification and also partial liberation of ammonia. Anothersource of loss was mentioned by Boussingault, namely, that whennitrates were given to plants growing in the dark, there was a libera-tion of free nitrogen, which be attributed to the action of someorganic substance excreted by the roots.The author experimente72 ABSTRACTS OF CHEMICAL PAPERS.on the point, growing bean seeds in the dark in nutritive solutions,both with and without nitrogen compounds. As in every case therewas a loss of nitrogen, it could not be due to reduction of nitrates,and he attributes it to the loss of nitrogen consequent on the decayof those parts of the seed not made use of by the germinating plant.Next, treating of the gain of nitrogen, he combats Hellriegel's viewthat the root nodules of the Leguminosae are concerned in renderingfree nitrogen available to the plant. His own experiments lead himto the coriclusion that the land gains in combined nitrogen in someway besides that caused by lightning discharges, which at present isthe only one undisputed.He found that the presence of vegetationraised the amount of this gain, that this could not be accounted forby the ammonia of the air, and that it must be derived from the freenitrogen of the air. The gain rises with increased plant development,and both the kind of soil and the species of plant have an influence.Lupines are very effective as compared with non-leguminous plants ;but the difference in the powers of increasing the combined nitrosenis one of degree, not one of kind ; hence it cannot be ascribed to thenodules. Further, nodules did not occur in lupines grown in sterilisedsoil, yet the plants developed better than in a pardlel experiment withunsterilised soil where the plants had nodules, and besides the nodulesthe legumes have no other organs to siipply nitrogen which other plantsdo not also possess.The next question is how soil unoccupied by acrop gains in combined nitrogen. This gain takes the form chieHyor entirely of organic nitrogen compounds, thus agreeing with Ber-thelot's experiments, and is explained by the growth in the soil of thecryptoganiic plants, algae containing chlorophyll and allied formswhich the author discovered there. He next discusses the questionwhether these plants avail themselves of free nitrogen or of nitrogenoxidised in the soil by an inorganic process. He asserts that underthe influence of calcium or magnesium carbonates free nitrogen can beoxidised to nitric acid, the action being distinct a t lOO", still apparenta t 45-50', and no longer apparent a t 15-22", but thinks that in theGerman climate this action can only very rarely occur. He con-cludes that it is not an inorganic process that makes the free nitrogenavailable, but that the combined nitrogen is due to a developmentof plant cells containing albumino'ids which is not to be connectedwith any process occurring in the soil. This power of assimilatingfree nitrogen is very different for different plants; the result issmallest in fallow land, where only the lower plant forms are atwork; it is larger with hjghsr plant forms, and among these thelupines and probably other Leguminosae produce the greatest result.H. H. R.Action of Superphosphate on Nitrates. By A. DWARDA(Chew. Ceiztr., 1888, 899--900).-Experirnents by the author go toshow that, at the ordinary temperature, the phosphoric acid, hydro-flouric acid, and readily decomposable organic compounds, as well asferrous salts present in superphosphates, cause no loss of nitrogenfrom nitrates which may have been mixed with them. In thosecases, however, where the mixtures are exposed to a moderately hightemperature, the loss of nitrogen is considerable, although in thiANALYTICAL CHENIST RY. 73case the ferrous compounds take no part in the reaction. The authoralso found that iii mixtures of superphosphate and nitrates thesoluble phosphate becomes insoluble much more quickly than whenthe nitrate is omitted, and the mixing of nitrate with superphos-phate for any length of time is therefore not to be recommended.J. W. L

ISSN:0368-1769    

DOI:10.1039/CA8895600067

出版商:RSC    

年代:1889

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ANALYTICAL CHEMISTRY. ‘73 A n a1 y t i c a1 C h e m i s t r y. Preparation of Starch Solution for Use in Volumetric Analysis with Iodine. By G. GASTINE (BUZZ. SOC. Chim., 50, 172 -173).-Five grams of potato-starch is mixed with 0.01 gram of mercury iodide, stirred with a little water, and poured into boiling water (1 litre). It is allowed to settle, and the clear liquid poured off. A solution prepared in this manner has been kept for more than a year without deteriorating. Use of Salicylic Acid for Preserving Standard Solutions. By H. BORNTRAGER ( Z e i t . and. Chem., 27, 641--642).-The addition of a pinch of salicylic acid to each litre of a thiosulphate solution greatly diminishes its tendelicy t o decompose. The author’s deter- minations show large variations, but not a progressive diminution in strength.M. J. S. Applications of Spectrophotometr y to Chemical Physiology. By E. LAMBLING (Arch. de Physiol., 4th Series, 12, 1--.34).-This 1)aper gives an historical account of the spectrophotometer, and of the principles upon which the spectrophotometric method depends. The practical application of the method for quantitative purposes in- xolves :-(1) The choice of a region of the spectrum; (2) the deter- mination of the coefficient of extinction of the coloured solution for that region ; and (3) the determination of the amount of absorption of the colouriig matter for the same region. When two colouring matters are mixed in a solution, they may also be estimated quantita- tively, provided the absorptive power of each of the two pigments for two regions of the spectrum be previously known.Finally, t,he application of such methods t o animal pigments (of the blood, bile, urine, &c.), is pointed out. Determination of Chlorine in Plant-ashes. By A. JOLLES ( Chem. Ceiztr., 1888, 863-864, from Zeit. Nahrunpnittel u. Hygiene, 2, 81).-The method the author proposes as the best is as follows:- The plant (10 grams) is incinerated gently in a platinum dish, moistened with an alcoholic solution of sodium carbonate, the alcohol burned off, aiid the process repeated; after this, the whole of the carbon may be burnt off without an1 fear of chlorine being lost, and N. H. M. W. D. H.74 ABSTRACTS OF CHEMICAL PAPERS. the ash may he extracted by means of water and the determination finished in the usual manner with silver nitrate.This deviation from the ordinary direct combustion of vegetable matter in the determina- tion of chlorine obviates the chance of a loss of this element which might otherwise take place. J. W. L. Method for the Determination of Bromine in Sea-water. By F. GUTZKOW (Chern. News, 58, 190-193).-25o C.C. of sea-water is mixed with a drop or two of sulphuric acid and with 100 C.C. of a solution containing about 25 grams of copper sulphate. It is then treated with sodium sulphite solution until the precipitate redissolves with difficulty, and heated until the blue colour returm; more sodium sulphite is now added, about one-third that already used, and the whole ag"n heated until blue, and then cooled. In this way, all the bromine is precipitated in a few minutes.After washing the precipitate, first with 100 C.C. of water containing 1 gram of sulplinric acid, then with a few drops of sodium carbonate solution, it is warmed with hydrochloric acid until all sulphurous anhydride is removed, and is finally treated with zinc. The filtrate and washings from the copper, which combined should not exceed 25 c.c., are titrated with sodium hypochlorite by a method of the author's which is described in detail in the original. The flask containing the liquid is fitted with a triple- bored cork ; through one hole passes a tube closed by a piece of india- rubber tubing and a clip, through the other holes two thistle-headed funnels reaching nearly to the bottom of the flask, one is roughly graduated. By blowing into the tube, a quantity of liquid is forced u p both funnels and is titrated in the graduated one, the other serving for comparing the colour ; in this way an indication of the quantity of hypochlorite required by the whole liquid is obtained, and so the operation can be finished with greater rapidity than by the ordinary mode of procedure.Determination of Fluorine in Substances Decomposable by Sulphuric Acid and especially in Natural Phosphates. Bg H. LASNE (BUZZ. Xoc. Chirn., 50, 167- liO).-Sufficient substance to yield 0.2 gram of calcium fluoride is put into a, flask containing strong sulphuric acid (50 c.c.) and pure sand (10 grams), and con- nected with two wash-bottles, the first of which contains 2.5 grams. and the second 0-5 gram of soda dissolved respectively in 25 C.C.of water. Dry air is passed into the flask, which is heated for an hour a t 180--260"; it is then allowed to cool, dry air being passed through. The soda solutions are united and boiled for a hour; phenolphthaleyn is added, and carbonic anhydride passed through the solution until it is colourless ; it is then heated for + hour at 50", and treated with ammonium carbonate, when the silica is almost com- pletely precipitated. The liquid is cooled quickly, diluted to 125 c.c., filtered through a large folded filter, and 100 C.C. collected. A few drops of tropeoline solution is added to the solution, which is carefully neutralised with dilute hydrochloric acid, It is then treated with pure sodium carbonate (equal to 0.5 gram of anhydrous carbonate), boiled until free from carbonic anhydride, and precipitated D.A. L.ANALYTICAL CHEMISTRY. 75 with a slight excess of calcium chloride. The precipitate is ignited, treated with acetic acid, evaporated to dryness, again treated with aretic acid, and the undissolved calciuni fluoride, washed, ignited, and weighed. N. H. M. General Method for the Separation and Volumetric Estima- tion of Acids : Application to Sulphuric Acid. By G. LINOSSIEI~ (BUZZ. SOC. Chin?., 50. 46-47).-The method is applicable to all acids which yield insoluble compounds when combined with metals which are precipitated by hydrogen sulphide in acid solution. The determinahn of sulphuric acid is carried out as follows :--The s o h - tion of the sulphate (containing 0.05 to 0.1 gram) contained iri a dish is treated with alcohol (2 vols.), heated almost to boiling, and precipitated with a slight excess of lead acetate.When cold it is maslied by decantation with a mixture of alcohol and water (0.5 to 1 vol.), passing the decanted liquid through a small filter. The trace of lead sulphate on the filter is washed with aqueous hydrogen sulphide into a flask ; the rest of the lead sulphate is shaken with a saturated solution of hydrogen sulphide, the liquid poured on to n filter, and the precipitate treated with a fresh amount of hydrogen sulphide and filtered. It is then washed with aqueous hydrogen sulphide until the filtrate gives no reaction with Poirrier’s orange. The whole of the sulphuric acid is then i n the filtrate, and is titrated with decinormal soda solution.N. H. 31. Volumetric Estimation of Boric Acid, and of Ammonia in Ammonium Salts. By J. MCGLASHAN (Chew. News, 58, 175- 176).-By using Poirrier’s oranges I and 11, boric acid and ammo- nium borate can be titrated directly with normal soda, but borax must first be made neutral to methyl-orange with aulphuric acid; boracite must be heated with dilute sulphuric acid, made neutral to methyl-orange with soda, and any carbonic anhydride eliminated before titrating. Ammonia is objectionable in any form except as borate or hydroxide, the latter when dilute is neutral to both orangeh. Therefore, with these indicators ammonia may be titrated with soda, in any ammonium salt, without distillation. With ammonium car- bonate and with arsenates, the end reaction is not distinct, but with hydrogen sulphide it is sharp. D.A. L. Resorcinol as a Test for Nitrates. By D. L~NDO (Chem. News, 58. 176--177).-For testing with resorcinol, 10 grams are dis- solved in 100 c . ~ . of water, and one drop of this solution, one drop of 15 per cent. hydrochloric acid, and 2 C.C. of concentrated sulphuric acid are added to 0.5 C.C. of the nitrate solution (compare Abstr., 1888, 1337) ; one in 500,000 gives a definite permanent purple colour after some time, whilst with increasing strengths of nitrate solution the colour becomes more intense, until with one in 10,000 the vivid purple- red colour is so intense as only to be distinctly seen i n the lower portion of the band. Resorcinol is valueless without hydrochloric acid, but with it, is a more delicate test for nitrates than ordinary phenol.Copper suiphate does not aid the reaction materially. The reagents76 ABSTRACTS OF CHEMICAL PAPERS. alone gave a band which, however, cannot be mistaken for the nitrate band. With nitrites, it is more delicate than with nitrates ; with chlorates it is no good, with dichromate (0.5 gram per litre) it gives a red to buff upper with a purplish lower band, the latter changing to pink or with hydrochloric acid to reddish-brown ; the colours are slightly different if the acid is run in at once, or after some delay. Perman- gsnate, N/10, with 4 vols. water, gives a, dark-orange upper and yellowish lower band ; with hydrochloric acid, these are respectively orange, red, and greenish. Hydrogen peroxide in dilute solution yields a green and brownish compound b;lnd.D. A. L. Estimation of Phosphorus in Iron and Steel. By P. W. SHIMER (Chem. News, 58, 165--168).-Dissolve 1 gram of iron in 20 C.C. of nitric acid, sp. gr. 1-20, and add to the boiling solution 10 c,c. of a solution of 20 grams of potassium permanganate in a litre of water, 2.5 C.C. a t R time, and after a few minutes 5 C.C. of hydro- cliloric acid, sp. gr. 1.12. When the action has ceased, add a mix- ture of 5 C.C. of concentrated sulphuric acid and 5 C.C. of water, and evaporate until fumes of sulphuric acid begin to come off. When cool, add 5 C.C. of nitric acid, sp. gr. 1.20, and sufficient water; boil to dissolve iron salts, filter, and wash with water. The residue serves well for the estimation of silicon. Heat the filtrate to 80" and add 5 C.C.of ammonium molybdate (5 grams of MOO,, 20 C.C. ammonia, sp. gr. 0.96, 30 C.C. nitric acid, sp. gi.. l a % ) , then keep at GO" until the liquid is clear, which occupies less than an hour when the solution is not too dilute. The yellow precipitate is washed with acid ammonium nitrate solution, dissolved in ammonia and pre- cipitated by magnesia mixture. The method gives good results both for silicon and phosphorus. A few experiments were made using sulphuric acid and ammonium sulphnte instead of nitric acid and ammonium nitrate for the molybdate precipitation, with satisfactory results. I). A. L. Influence of Sulphur on Eggertz's Carbon Colour-test. l 3 ~ T. W. HOGG (Chern. News, 58, 175).- When ordinary steels contain- ing say 0.05 per cent.of sulphur are dissolved in the usual manner, the sulphur separates out and produces a turbidity which interferes with the colour-test for carbon ; a fact easily proved by dividing such a solution into two portions, filtering one, and then comparing the colour produced in the filtered and unfiltered solutions. Conse- quently, if a common steel is compared with a standard of pure steel, the colour intensity is sure to be over-estimated, and vice versd. D. A. L. Quantitative Analysis by Electrolysis. By A. CLASSEN and R. SCHELLE (Ber., 21,2892-2899).-The current from two of Farbaky and Schenek's accumulators, fully charged by a dynamo giving R current of 20-25 amperes, was employed in making 50 analyses in the course of six days. Four to eight analyses were made simul- taneously, and the current was employed continuously day and night, except during the short intervals required for changing the platinumANALYTICAL CHEMISTRY.7 7 dishes, During this time the strength of the current decreased from 2.05 to 1.92 volt, so that one charge would be sufficient for 60 to 70 analyses. The condition of the accumulator can be ascertained from the specific gravity of the sulphuric acid, which is 1.240 when the accumulator is charged and 1.118 when i t is not charged. The pre- cipitated metal is in a more suitable condition than when a battery or dynamo is employed. Experiments which were made with Neumann’s (Abstr., 1888, 529) and Wolffs ( Z e i t . ung. Chem., 1888, 296) voltameters, employ- ing currents of various strengths, show the necessity of working under the same conditions when repeating electrolytic methods of analpis (compare Classen, Quantitative Analyse durch Electrolyse, 2nd ed., 43).In the separation of antimonyfroin tin in sodinm sulphide solution, the solution, freed from antimony, is boiled with ammonium pulphate, and the tin precipitated by electrolysis (compare Abstr., 1884, 932). A simpler and more convenient method is to convert the stannic sulphide into hydrogen stannic oxalate and electrolyse the solution. For this purpose, the solution is acidified with dilute sulphuric acid, and the sulphide oxidised with ammoniacal hydrogen peroxide, or the hot alkaline solution is treated a t once wi+h hydrogen peroxide until it becomes colourless, acidified with sulphuric acid, neutralised with ammonia, and more hydrogen peroxide added.The solution is then boiled, filtered, and the residual stannic acid washed off the filter with and dissolved in a hnt solution of oxalic acid. If there is a residue of sulphur, i t is separated by filtration, washed with a cold saturated solution of hydiwgen animonium oxalate, and the washings added to the filtrate. The solution, which should contain at least 50 C.C. of the hydrogen ammonium oxalate solution, is electrolysed with a current giving 8-10 C.C. of explosive gas per minute. The electroljtic deposition of copper from its salts, dissolved in a saturated solution of ammonium oxalate, is hastened very consider- ably if the solutian is kept acid, especially towards the end of the operation, by adding excess of a cold, saturated solution of oxalic acid.The smaller the quantity of copper, the more oxalic acid soln- tion may be added. A solution poor in copper can be mixed with the oxalic acid solution a t the commencemtnt of sthe process, but in concentrated solutions, the precipitation must be carried out in a solu- tion as nearly neutral as possible to avoid the separation of copper oxalate. If the copper solution is kept a t 40-50°, aLout two grams of copper are deposited in from 3 to 4 hours. A current giving 3-4 C.C. of explosive gas per minute mas employed, and quantitative experiments showed that the whole of the copper is deposited. Separation of Calcium, Barium, and Strontium. By KUPFFERSCHLAEGER (Bull. SOC. Clzim., 49, 854- 856).-A quantitative analysis of a mixture of the carbcnates of barium, strontium, and calcium can be carried out as follows :--The mixture is dissolved in a slight excess of very dilute nitric acid, the solution evaporated to dryness, the residue dissolved in distilled water, and the filtered solu- tion again evaporated to complete dryness, The residue of mixed nitrates is agitated with a small quantity of a mixture of absolute I?.s. I(.78 ACSTRACTS OF CHEMICAL PAPERS. alcohol and ether, and the solvent separated by filtration as soon as the solution becomes clear ; this process is repeated three times, the propor- tion of ether being gradually increased until the mixture contains equal volumes of the constituents. The residual mixture of the nitrates of barium and strontium is dried, dissolved in water, and treated with a cold saturated solution of potassium dichromate. The precipitated barium dichroniate is washed with cold, very dilute a,lcohol, and con- verted into sulphate by heating with sulphuric acid.The strontium in the filtrate is converted into sulphate by warming the solution with dilute sulphuric acid. A solution of strontium chloride is not precipitated by potassium dichrornate. F. S. K. Volumetric Estimation of Mercuric Chloride. By G. KASSRER (Arch. Phawn. [ 3 ] , 26, 595-604).-The method promises well for pharmaceutical practice. 50 grams of the organic compound contain- ing mercuric chloride is placed in a porcelain dish without previous division, 500 C.C. of water is added, and the mass is well kneaded with a pestle.500 C.C. of a solution of 0.4 gram of potassium anti- monions tartrate and 1 gram of sodium phosphate, or in place of the latter 1 to 2 grams of sodium acetate, is now added and the kneading continued. A very intimate mixture is thus obtained, and a milky liquid results from the decomposition of the mercuric chloride. About 500 C.C. is now filtered off, and titrated with decinormal iodine solution after the addition of freshly prepared starch solution, and a suffirient quantity of sodium hydrogen carbonate. The iodine employed corresponds to the amount' of unchanged tartrate remaining in the filtrate. The reaction is as follows :-4HgCI, + Sb,O, + 2H,O = 4KC1 + Sb,05 + 4HgC1. The presence of phosphoric and organic acids is admissible, but not of free hydrochloric acid.By A. STRENG (Jahrb. f. Mi%, 1888, ii, Mem., 142-152 ; continuation of Abstr., 1886, 4877.-For detect- ing tin under the microscope, t'he author avails himself of the brown colour produced on adding hydrochloric acid and platinum chloride. When the solution is effected, a drop of the liquid is transferred to an object-glass, and a grain of potassium chloride added, and the solution slightly evaporated. In this way, rhumbic crystals of pot'assinm stannous chloride (2KC1 + SnC1, + H,O) are form_ed. They-are mostly combinations of the forms mP, mPm, 03Pq Pm, Pm. When the staunous chloride has been thus detected, a drop of nitric acid is added, and the solution heated. The stnncous chloride is converted into stannic chloride, and the imperfectly soluble salt, K,SnCl, is formed.This crystallises in the regular system, and is perfectly isotropic. This reaction may be employed for detecting stannous and stannic oxides in compounds soluble in hydrochloric acid. Caesium chloride may be used instead of the isomorphous potassium salt. The author also describes methods for detecting potassium, caesium, and rubidium, sodium, and silicon. Detection of small Quantities of Germanium. By K. HAUSHOFER (Clrern. Centr., 1888, 867, from Xitzber. Akad. JIGnche~~, 1887, 133). J. T. Microchemical Reactions. B. H. B.AX ALP TIC AL C €1 ENIST R Y. 70 -By heating in an atmosphere of hydrogen snlphide, the germanium in the mineral argyrodite is converted into the sulphide GeS, which is crystalline, and may be detected and yecognised by means of ihe microscope.With concentrated sulphuric acid, it forms a white, non- crystalline substance, with concentrated nitric acid it is converted into the white, crystalline oxide, GeOz, which is soluble in dilute nitric acid and water, and crystallises out of the solution again on evapora- tion. Heated in a tube, it sublimes similarly to antimony oxide, but differs from this by its solubility in water, and also by melting t o clear colourless drops. It, is necessary to apply the potassium iodide test also, as a means of distinguishing it from the mercuric sulphide, which has also been found present in argyrodite. J. W. L. Characteristic Reaction of Bismuth. By E. L ~ G E R (BUZZ. XOC. Chi%., 50, (31-93) .-A solution of bismuth iodide and potassium iodide is sometimes used for detecting alkalo'ids, with which it gives orange-yellow precipitates.It is suggested that the reaction should be employed for detecting bismuth. A solution is prepared by dissolving cinchonine (1 gram) and potassium iodide (2 grams) in water (100 c.c.). Other alkaloids may be nsed instead of cinchonine, but thir seems to give the most sensitive reaction. The reagent must be added in excess ; the presence of too much nitric acid, and espe- cially the presence.of hydrochloric and sulphuric acids, is to be avoided. Bismuth may be detected in solutions containing only 1 part in 500,000 parts. Solutions which contain &her metals besides bismuth are precipitated with hydrogen sulphide, the sulphides of copper, lead, cadmium, mercury, and bismuth converted into nitrates, then in to carbonates, and the caiabonates of bismuth and lead separated by means of potnssium cyanide ; these carbonates are converted into clibrides, and the lead chloride separated by means of alcohol.The alcoholic solution is evaporated to dryness, c?issolved in a drop of nihric: acid and sorne C.C. of water, and treated with the rexgent. Solu- tions of the salts of mercury, cadmium, silver, copper, and lead also give precipitates of various colours with the cinchonine reagent. N. H. M. Determination of Oxygen dissolved in Water. By L. W. WINKLER (Ber., 21, 2846-2854) .-The method consists in oxidising :in excess of manganese hydroxide in presence of alkali by the oxygen present in a weighed amount of the water; potassium iodide and hydrochloric acid are then added, and the iodine which separates (which is equivalent to the amount, of dissolved oxygen) titrated with sodium thiosulphate.A solution of maiiganous chloride (free from iron) is made of such a strength that 100 C.C. contains 40 grams of the salt (MnC1, + 4H20). The soda must be free from nitrate, and the solution prepared of eight times the normal strength ; potassium iodide (10 grams) is dissolved in 100 C.C. of the soda solution, the rest of which is kept. A strong flask of about 2 litre capacity is filled with the water ; 1 C.C. of the potassium iodide soda solution is added by means of a pipette reaching nearly to the bottom of the flask, then 1 C.C. of the manganous chloride solution. The flask is closed, care being taken t h a t no bubble of air remains, and the contents mixed.80 ABSTRACTS O F CHEMICAL PAPERY.When the precipitate settles, fuming h~drochIoric acid (3 s.c.) is added by means of a pipette similar to those previously used. The flask is again closed, the contents mixed, and the yellow liquid titrated in the usual manner with sodium thiosulphate, the most convenient strength of which is 1/100 normal, so that each C.C. corresponds witli 0.055825 C.C. of' oxygen (at 0" and 760 mm. pressure). When the water to be analysed contains mucii carbonic anhydride, more of the reagent must be added, as manganous carbonate is not oxidised by the oxygen. In the case of waters containing nitrates, the process has to be modified : a soda solution containing no potassium iodide is first added, then hFdrochloric acid (twice the amount other- wise used), and after three minutes a solution of potassium iodide.A manganic chloride solution is then prepared as follows :--500 C.C. of distilled water is treated with the pure soda solution (1 c.c.), 5 to 10 drops of the manganous chloride solution, and then sufficient hydro- chloric acid is added to dissolre the precipitate. 100 C.C. of this solution is taken out and diluted with distilled water; to the rest, 100 C.C. of the water to be examined is added. After two to three minutes, both solutions are treated with potassium iodide and the iodine which separates determined as usual. From the difference in the amount of thiosulphate used, the correction for 100 C.C.of water is calculated. Concordant results obtained b j the new method are gil en. N. H. M. Ash Determination. By F. A. FL~~CKTGER (Zeit. anal. Chem., 27, 637-638).-The substance is heated in a roomy platinum capsule so gently that carbonisation takes place without combustion. It ir then cooled, a copious amount of water is added, and the whole eva- porated completely on the water-bath. On reheating the carbonaceous rebidue very gradually, it burns a t a low temperature, and very quickly. &I. J. S. Wet Methods of Organic Analysis. By J. MESSIKGER (Bey., 21, 2910-2919) .-Organic compounds, as Cross and Bevan have show11 (Proc., 1888, 76, and Trans., 1888, 889), are completely oxidised when warmed with chromic acid and concentrated sulphuric acid. I f nitrogen is present, it is evolved as such or as ammonia, whilst sulphur, phosphorus, and arsenic are converted into the corresFond- ing acids.Halogens are evolved in the free state, and metals remain as sulphate or, with a large excess of chromic acid, as chromates. To estimate the quantity of carbon, the substance (0*15-0*35 gra,m) is weighed in a small bulb or tube, and placed in the apparatus employed by Classen for the estimation of carbonic anhydride (Quudtative Analyse, 3rd ed., 239), together with chromic acid (?5--.6 grams) or powdered potassium dichromate. A gentle stream of air, free from carbonic anhydride, is passed throngh the appa- ratus to drive out the carbonic anhydride, the weighed potash bulbs and sods-lime tube are attached, and the latter connected with a calcium chloride tube to prevent absorption of moisture from the air.Concentrated sulphuric acid (30 c.c.) is then poured throughANALYTICAL CHEMISTRY. 81 tlle funnel, and the stream of air stopped. The flask is warmed very cautiously until the evolution of carbonic anhydride commences, and then the heating is immediately discontinued until the reaction is almost at an end. Pure air is passed through the apparatus for half an hour, and the tubes weighed. Tlie results obtained are very satisfactory, except in the case of substances which sublime readily, but great care must be taken when heat is first applied. I n analysing volatile substances, the bulb is broken by means of the funnel. If the substance con- tains halogens, a Dreschler’s flask of about 100 C.C.capacity, contain- ing 40 C.C. of concentrated potassium iodide solution, and a small U -tube filled with glass-wool, half of which is moistened with a solu- tion of silver nitrate and half with concentrated sulphuric acid, are interposed between the condenser and the potash bulbs. Quantitative experiments with compounds of the most varied nature gave satis- factory results (compare Cross and Bevan, Zoc. cit.). Sulphur can be estimated, except in the case of extremely volatile substances, as follows :-The substance (0.15-0.35 gram), together with potassium permanganate (1&2 grams), and pure potash (0.5 gram) is placed in a flask of 500 C.C. capacity provided with a con- denser, water (25-30 c.c.) poured down the condenser, and the mixture heated for 2-3 hours.Concentrated hydrochloric acid is then gradually poured down the condenser into the cold inixture, which should be of a reddish colour, mid after the evolution of gas has ceased, the whole is heated until the liquid beconies clear. The sulphuric acid is then precipitated with barium chloride. Potassium dichromate (2-3 grams) and hydrochloric acid (20-25 C.C. : 2 parts concentrated acid, 1 part water) may be employed instead of potas- sium permaiiganate and potash. The operation is carried out in the manner described, but after heating for about two hours a few drops of alcohol are added to determine whether all the dichromate has heen reduced; if the odour of aldehyde is perceptible, the mixture iuust be heated again and the test repeated. Both methods can also be employed for the detection of sulphiir.Numerous quantitative cbxperiments gave satisfactory results, but in the case of a few sul- phones i t was found that sulphur cannot be estimated by this method. Phosphorus, arsenic, and antimony in organic compounds can be estimated by placing the substance (0.3-0.4 gram) with chromic acid (4.-5 grams) in a flask provided with a condenser, pouring sulphuric acid (10 c.c., 2 parts concentrated acid, 1 part water) down the con- denser, and heating gently. After an hour’s time, sulphuric acid (10 c.c.) is added, and the heating continued for about an how. The mixture must always be heated very carefully, and the cold solu- tion should be perfectly clear. Some antimony compounds require only 1 gram of chromic acid and 10 C.C.of sulphuric acid. In the estimation of phosphorus, the solution is warmed with ammonium nitrste (3-4 grams) and ammoniuni molybdate solutior! (50 c.c.) for 2-3 hours, filtered, the precipitate washed 6 to 8 times by decantatioii with ammonium nitrate solution (20 grams in 100 C.C. of water), throan on to a filter, and dissolved in not more than 40- 50 C.C. of warm dilute (2 per cent.) ammonia ; a concentrated solution The process occupies about two hours. VOL. LVI. 982 ABSTRACTS OF OHEMIOAL PAPERS. of citric acid (4-5 drops) is added to the filtrate, and the phosphoric acid precipitated with magnesia mixture. In estimating arsenic, the solution is diluted to about 100 c.c., heated to about 70", and the arsenic precipitated with hydrogen sul- phide.The precipitate is washed with water containing hydroqen sulphide until free from chromium salts, and then converted into arsenic acid by means of ammoniacal hydrogen peroxide (compare Classen, Abstr., 18b3, 934). After boiling for an hour, ammonia is added to the filtered solution, and the arsenic precipitated with mag- nesia mixture. Antimony is estimated by adding potash and excess of sodium sulphide, boiling for half an hour, and precipitating the metal electrolytically. Metals are estimated by mixing the solution with excess of ammo- nium oxalate and precipitating electrolytically. Halogens can be detected by warming the substance (1-2 mgrms.) with chromic acid and sulphnric acid, and passing the gas evolved into a dilute solution of potassium iodide ; quantitative experiments gave unsatis- factory results.F. S. K. The Safety of Commercial Kerosene Oils. Bp S. B. NEWBURY and W. P. CUTTER (Amer. Chem. J., 356-362).-Although oils are regularly testea for their flashing points and conclusions drawn as to their being sa€e for burning in lamps, it is noteworthy that many modern lamps heat their reservoir of oil to temperatures above the legal flashing point, and that there are not sufficient experimental data to allow of the correct interpretation of the flashing point deter- minations into +terms expressing the inability of such oils to form explosive mixtures of vapour with air. All hydrocarbons up to and including octane, form at ordinary temperatures mixtures that can be exploded; nonane mixtures (b. p. 148-1.50") explode sharply at 79" F., and decane at 104" F.The addition of small quantities of low-boiling oils materially lowers the flashing point of another sample. Thus a sample flashing at 212" F. was made to flash at 145" F. by the addition of 5 per cent. of heptane; at 110" F. by the addition of 5 per cent. pentane or hexane, or 10 per cent. heptane; at 96" F. by the addition of 15 per cent. heptane ; and at ordinary temperatures by the addition of 10 per cent. pentme or hexane, or 20 per cent. heptane. The tem- peratures at which am oil may be kindled in an open vessel approaches the more nearly to the Bashing point the more homogeneous the oil is. The flashing point of an ordinary oil may be materially raised, with but little diminution of weight, by passing a current of air through it for several hours.H. B. Solubility and Estimation of Paraffin. By B. PAWLEWSKI and J. FILEMONOWICZ (Ber., 21, 2973-2976) -The following table gives the solubility at 20' of ozokerit paraffin of sp. gr. 0.9170 at 20°, melting at 64-65', and solidifying at, 61-63' :-ANALYTICAL CHE3lISTHY. - Solvent. Carbon bisulphide.. ................... Light petroleum, up to 75" G., sp. gr. 0'7233 ............................ Turpentine oil, sp. gr. 0 -857 ; b. p. 158- 186". .............................. Cumene (comm.), up to 160°, sp. gr. = 0 *867. ............................. Cumene (frac.), 150-160", sp. gr. = 0.849 Xylene (comm.), 138- 143",sp. gr. = 0.866 (frac.). 136-1383, sp. gr. = 0.864. . Toluene (comm.), l(B--llO",sp.gr. = 0.866 (frac ), 108.5-109 5", sp.gr. = 0-866 .............................. Chloroform .......................... Benzene ............................. Ethyl ether .......................... Isobutyl alcohol (comm.), sp. gr. = 0.804. 1l:tliyl acetate. ........................ Amy1 alcohol, 127-129", sp. gr. = 0813 . l'ropionic acid.. ...................... )'ropy I alcohol ........................ Met hpl alcohol, 65.5 - 66 5 O , ~ p . gr. = 0.798 JIetli! 1 forniate ....................... (fluci 11 acetic acid .................... ,, ,, Acetone, 55-5-56 5", sp. gr. = 0.797.. ... Ethyl alcohol, 99.5' Tr.. ............... Ethyl alcohol, 945" Tr. ................ Acetic anhydride.. .................... l?ormic acid (crjst.) ................... Ethyl alcohol, 75" Tr.. .................Paraffin (grams), dissolved by 100 grams 12 *99 11 '73 6.06 4.28 3 -99 3.95 4.s9 3 -83 3 -92 2 '42 1 -9Y 1 -95 0.288 0 '262 0 '238 0 * 819 0 -20% 0 -166 0 -141 0 ' o n 0 -060 0 -060 0 -046 0 -028 0 -013 0 *Wd03 -.- 100 C.C. - 8 *48 5 -21 3-72 3 -39 3 -43 3.77 3 -34 3 -41 3 -61 1 -75 0 -228 0 '209 0 '164 0 -056 0 -063 0 '015 - - - - - c - - Weight of solvent required to dis- solve completely 1 part d paraffin. 7.6 8'5 16 *1 23 -4 26-0 25 -1 22 -7 26 -1 25 *5 41 '3 60 '3 50.8 352 -9 378'7 419.0 453 -6 495 -3 595 -3 709 -4 l a 7 -5 1648 -7 1668 -6 2149 * 5 3856 -2 7689 -2 330000 *o The liquid constituents present in man-j- prodncts of the petroleum or ozokerit industry are soluble in glacial acetic acid, whereas vaselin, cerisin, ozokerit, and paraffln are almost insoluble.To estimate the quantity of solid paraffin in petroleum, lubricating oils, mineral oils, vaselin, &c., 5-20 C.C. of the mixture is well shaken with 100-200 C.C. of glacial acetic acid, the residual para& thrown on to a weighed filter, washed two or three times with glacial acetic acid, and then two or three times with alcohol of 75" Tr., dried and weighed, or the residual paraffin is washed, dissolved in benzene or ether, the solution evaporated, and the residue weighed. This method is quick and accurate, and can be carried out at the ordinary temperature, F. S. K. Analysis of a Mixture of Silver Chloride, Cyanide, Thio- cyanate, Ferricyanide, and Ferrscyanids. By J. TELSS~ER (BUZZ. Soc. Chim., 50, 10&106).-The mixture occurs in the analysis of materials used in the purification of coal-gas. Sodium carbonate is heated in a crucible until aahjiirous, the weighed substance and Borne81 ABSTRACTS OF CHEMICAL PAPERS.potassium nitrate are added, and the whole is heated. The product is extracted with water, which leaves a residue of pure silver and ferric oxide. In the solution, sulphur is determined as barium sul- phnte and chlorine as silver chloride. The residue is dissolved in nitric acid, the silver determined as chloride, and the iron as sesqui- oxide. Equations are given by means of which the amount of each salt present in the mixture is calculated. Estimation of Paranitrotoluene. By F. REVERDIN and C. DE LA HARPE (Bull. Xoc. Chim., 50, 44-46).-The method is based on the fact that paranitrotoluenesulphonic acid is readily converted by boiling with soda into dinitrosulphostilbene which yields a red colour when dissolred in alkali, whilst orthonitrotolnenesulphonic acid is not attacked by soda, and the alkaline solution is yellow.2 C.C. of pure orthonitrotoluene is heated in a water-bath with 6 C.C. of sul- phuric acid (containing 25 per cent. of anhydride) for three hoiirq, the product cooled and diluted to 1 litre. I n a similar manner a mixture of orthonitrotoluene (96 parts) and paranitrotoluene (4 parts) is sulphonated and the product diluted to 200 C.C. I n determining the amount of paranitrotoluene, the substance and nitrotoluene (con- taining 4 per cent. of the para-compound) are sulphonated, the pro- ducts diluted to 200 c.c., and the colours compared which are obtained by mixing 1 C.C.of each solution with 5 C.C. of aqueous soda. If the sample to be aiialysed gives a stronger colour, a measured quantity (50 to 50 c.c.) is progressively diluted with the solution of ortho- nitrotoluenesulphonic acid until 1 C.C. when heated with 5 C.C. of aqueous soda gives the same amount of colour as the solution con- taining 4 per cent. The percentage of paranitrotoluene can then be calculated. N. H. &I. Detection of Methyl Alcohol in Wood Spirit. By J. HABER- MAXN (Zcit. anal. Chem., 27, 663, from VerAandl. nut. Ver. Byutm, 26). -Commercial methyl alcohol contains impurities which reduce per- manganate energetically. Cazeneuve and Cotton shake 10 c c. of the spirit to be tested with 1 C.C. of a 0.1 per cent.solution of per- manganate a t 20'. If wood spirit is present. decolorisation takes place immediately ; with pure alcohol, 20 minutes is required. Ethereal oils, which may be present in spirit o r brandy, and would cause a similar reduction, may be removed by shaking the spirit twice with half its volume of the purest olive oil and then filtering through a well wetted filter. N. H. M. If sugar is present, the spirit must be distilled. M. J. S. Composition of Natural Brandies and the Way of Dis- tinguishing them. By X. ROCQUES (Bull. SOC. Chim., 50, 157- 164).-500 C.C. of the brandy is distilled in a, Le Bel-Henniger ap- paratus and nine fractioiis of 50 C.C. each collected, the temperatures being noted. Each fraction is subjected t o the following tests:- (1) Rosaniliue bisulphite, (2) aniline acetate, (3) sulpharic acid, (4) permanganate, (5) ammoniacal silver nitrate solution.The results of several analyses of brandies are given in tables. N. H. 31.ANALYTICAL CHEMISTRY. 85 Estimation of Sugar in Presence of Carbohydrates. By R. W. BISHOP (Chern. Centr., 1888, 952-953, from Msc. ,Won. Sci., 32, 558).-The author has carried out a number of experiments with a view to determine the conditions under which inversion may be completed without a t the same time damaging the accompanying carbohydrates. It was found that sulphuric acid has a greater power of inversion than hydrochloric acid, but it appears that hydro- chloric acid is the best for the conversion of starch into dextrose. Prolonged heating of inverted sugar with the acid seems to act on the lmvulose rather strongly, and the solution becomes less lmvo- rotatory and eventually dextrorotatory.For the inversion of cane- mgar, 0.5 C.C. of hydrochloric acid is snfficient, and the heating is con- tinued for 10 minntes at 95". For the conversion of dextrin, the solution should not contain more than 1-3 grams of carbohydrates i n 50 C.C. The inversion is performed by adding 2 C.C. of hydrochloric acid and heating for three hours at 95". J. W. L. Detection of Sugar in Urine. By C. SCHWARZ (Arch. Pharnz. [3], 26, 796, from Pharm. Zeit., 33, 465).-1 to 2 C.C. of lead acetate is added to 10 C.C. of urine and filtered ; 5 C.C. of the filtrate is mixed with 5 C.C. of normal potash solution and one or two drops of phenylhydrazine, well shaken and vigorously boiled ; in the presence of sugar, the liquid becomes lemon- to orange-yellow, and becomes opaque on adding an excess of acetic acid owing to the immediate formation of a finely divided yellow precipitate.In the absence of sugar, this precipitate never OCCUTS with urine. J. T. Detection of Chloral or Chloroform in Liquids. By C. SCHWARZ (Zeit. anal. Chem., 27, 668-669, from Pharm. Zeit., 33, 419).-Either of these substances when boiled with resorcinol and an excess of soda gives a red colour, which disappears on acidifying and is restored by alkalis. If, on the other hand, an excess of resorcinol and only a dropor two of soda solution is used, the product is n yellowish- red solution with intense yellowish-green fluorescence.0.0001 gram of chloral hydrate in 1 C.C. gives this reaction very diwtinctly when vigorously boiled with 0.05 gram of resorcinol and five drops of soda solution. Rf. J. S. Modification of the Reichert-Meissl Metho& of Butter Analysis. By M. MANSFELD (Chem. Centr., 1888, 870-871, from Milch Zeit., 17, 281-283).-1n order to obviate the possible error arising from the use of alcohol in the saponification of the butter-fat, theauthor has tried the use of alkali alone, the latter being added to the fat in a small flask and heated on the water-bath for two hours, a t the end of which time the saponification is complete, and the process is finished as Wollny prescribes. J. W. L. Densities and Refractive Indices of Certain Oils. By J. H. LONG (Amer. Chem. J., 10, 392--405).-The following values arc obtained-the densities a t 20" being compared with water at 4' as86 ABSTRACTS OF CHEMICAL PAPERS.unity, and the substance weighed in a vacuum; the refractive indices are for sodium light a t 20" :- Olive oil .......... 0.9130 Ref. index 1.4703 Cotton-seed oil. 0.9191 2.4732 Sesame oil ........ 0,9191 1.4740 Mustard oil.. 0.9121 1.4742 Castor oil.. 0.9589 1.4791 Lard oil 0.9122 1.4686 Peanut oil ........ 0.9173 1.4717 The densities and refractive indices are also given for other tempe- ratures than 20". In nearly all cases, the variations due to temperature are t,he same, namely, about -0.G0068 i n denpity and -0-0004 in refraction for each rise of 1". The author believes such determiuations may prove of value in the identification of other oils..... ...... ........ .......... H. B. Bechi's Newest Method for the Detection of Cotton-seed Oil in Mixtures. By G. Biz10 (Chem. Centr., 1888, 873, from Atti Inst. Veneto [ 6 ] , 6 ) .--The author finds that pure olive oil gives Bechi's new cotton-seed oil reaction with slightly acid silver nitrate, whilst, on the other hand, he finds that there are some cotton-seed oils which do not give the reaction at all. J. W. L. Qualitative Test for Resin Oil in Vegetable and Mineral Oils. By HOLDE (Chem. Centr., 1888, 952, from Pharna. Zeit., 33, %8).- Whereas Storch's reagent (concentrated sulphuric acid and arihjdrous acetic acid) for the detection of resin oil is not always admissible, the author recommends sulphuric acid of sp. gr. 1.53, which produces a violet coloration with resin oil.If the oil under examination becomes sc) dark-coloured with sulphuric acid as to interfere with the reaction, the resin oil may first be extracted with alcohol, when the colour test is readily performed. J. W. L. Test for Saccharin." By D. LINDO (Chem. News, 58,155).-The author modifies his test for " saccharin " (Abstr., 1888, 1350). After evaporating to dryness with nitric acid on a water-bath, a few drops of alcoholic potash is added to the cold residue ; when this is heated, a greater variety of colours is obtained than by following the original directions. D. A. L. Recent Processes for Testing Quinine. By W. LEKZ (Zeit. anal. Chenz., 2 7, 549-631) .-The foreign alkalojids in commercial quinine consist chiefly of cinchonidine and hydro-bases.Four principal methods are in use for the determination of these. In all these methods, a product (" Nebenalkaloide ") is obtained, containing the greater part of the impurities together with a certain quantity of quinine.', In this product, the cinchonidine is determined by the " tetrasulphate process." 1 gram of the mixture is dissolved in 9 grams of absolute alcohol and 3 grams of 50 per cent. sulphuric acid. The mixture is kept at 0" for 24 hours, the acid liquid isANALYTICAL CHEMISTRY. 87 removed by suction, the crystals are washed with a little absolute alcohol, and then air-dried. They are then dissolved in water, and the base is precipitated by excess of sodium carbonate. It is dried first over sulphuric acid, and then a t 115”.A correction (the amount of which depends on the percentage of cinchonidine found) must be applied. The author gives a curve for the purpose. The cinchonidine is very nearly pure. The hydro-bases are determined approximately by oxidising the quinine and cinchonidine in acid solution by a 1 per cent, solution of potassium permanganate, rendering alkaline, and shaking with ether, followed by chloroform. The residues from these solutions, although very impure, are regarded as hydroquinine. For the “chromate procew” of De Vrij see Abstr., 1887, 404; for the “ oxalate tesh” see Schaefer (Abstr., 1887, 623). The amount of oxalate prescribed is insufficient for samples containing less than 15 per cent. of water, and the cooling at 20” should be prolonged to one hour.Schaefer’s correction of 004 gram per 100 C.C. appears to be ltoo large. In Hesse’s ‘( bisulphate process” 5 grams of quinine sulphate is dissolved in 12 C.C. of normal sulphuric acid by warming, and the solution is allowed to erystallise in a naprow-necked funnel in a cold place. The mother-liquor is withdrawn by a filter-pump into a graduated cylinder, and the crystals washed with 3 C.C. of water. This solution is shaken with 16 C.C. of ether (0.721-0*728), then 3 C.C. of ammonia (0.96) added, again shaken, and left for 24 hours. The ether is removed by a pipette, the crystals are collected on a filter, washed with water saturated with ether, dried between filter- paper, washed again with ether, and dried. In the “ crystallisation process ” of Paul and Hewe, 5 ,mms of quinine sulphate is dissolved in boiling water, and crystallised out four times, using in the first case 150 c.c., next 130 c.c., and then twice 120 C.C.The united mother-liquors are evaporated at a low temperakmre almost to dryness, the residue dissolved in the smallest possible quantity of dilute sulphuric acid, made up to 20 c.c., and shaken with ether and excess of ammonia. The crystals which form are treated as in the bisulphate test. The hydro-bases crystallise in part with the quinine, therefore the mother-liquor should not be used for their determination. The chromate process gives very varying results, but on the average gives the highest yield of cinchonidine, especially with the purer samples The oxalate test gives the lowest numbers, but they are more concordant than those of the chromate process.The com- position of the bye-product is, however, variable. The bisulphate test gives results varying considerably. The alkaloids in the ethereal solution ought t o be submitted to the process a second and even a third time, but even with this improvement the whole of the cin- chonidine is not obtained, and the results vary much, but the com- position of the bye-product is more uniform than in the other processes. The crystallisation test has the same advantages as the bisulphate test if the crystallisation is repeated often enough, and is the process which i8 least influenced by the presence of hydro-bases. I t is, however, tedious. The process of the German Pharmacopoeia depends88 ABSTRACTS OF CHEMICAL PAPERS. on the fact that the precipitate produced by ammonia in solntionc: of the alkalo'ids is soluble i n excess of ammonia, but that much more ammonia is required for quinine than for the other alkalolds.The excess of ammonia required varies, however, very considerably with the temperature. M. J. S. Method for Recognising the Adulteration of Pepper by the Addition of Ground Olive Stones. By GILLET (BUZZ. XOC. chim., 50,173-174).-When 1 gram of olive stones is treated with 1 C.C. of a 5 per cent. iodine tincture, it acquires, after a quarter of an hour, a, J ellowish colour, whilst pepper is coloured brown or maroon. A series of mixtures of pepper with 5, 10, 15, and 20 per cent. of olive stones are prepared and coloured with iodine tincture. It is then easy to determine the amount of olive stones in samples of pepper by com- paring the colour obtained with these types.A New Test for the Blood in Carbonic Oxide Poisoning. By R. KATAYAMA (Virchow's Archiv, 114, 53-64).-When ammonium sulphide holding sulphur in solution and acetic acid are added to hlmd containing carbonic oxide, the result is a beautiful clear red or mse colour ; whereas normal blood becomes greenish-grey, or reddish- preen-grey on the addition of the same reagents. On examining these liquids spectroscopically, it is found that both in the case of normal and csrbonic oxide blood the absorption-spectrum indicates that a mixture of two substances is present. In the case of normal blood, there is a band between C and D and another between D and E ; this last becomes double on shaking up the mixture with air.In other words, there is a mixture of sulphur methaemoglobin (see Hoppe-Seyler, Physiol. Chem., 386) and reduced haemoglobin. I n the case of carbonic oxide there are three bands : one between C and D, due to sulphur methEmoglobin, and two between D and E, due to carbonic oxide hsemoglobin. That is to say, in spite of the pre- sence of sulphur methaemoglobin, the liquid does not become greenish, but remains red, the colour of carbonic oxide haemoglobin overpowering the olivegreen of the sulphur methaemoglobin. This test is stated to be more delicate than Hoppe-Seyler's (Abstr., 1888, 540), and is obtained with a mixture which contains one part of carbonic oxide blood to five parts of normal blood.Estimation of Albumin in Urine. By H. SCHACJMANN (Zeit. afial. Chent., 27, 635-636J-The estimation of albumin is much accelerated by collecting it, not on a paper filter, but in a filter-tube plugged with cotton-wool and connected with a filter-pump. When the washing with hot water is complete, a calcium chloride tube is connected, and dry air is drawn over the albumin whilst gradually raising its temperature to 110". N. H. M. W. D. H. M. J. S.ANALYTICAL CHEMISTRY. ‘73A n a1 y t i c a1 C h e m i s t r y.Preparation of Starch Solution for Use in VolumetricAnalysis with Iodine. By G. GASTINE (BUZZ. SOC. Chim., 50, 172-173).-Five grams of potato-starch is mixed with 0.01 gram ofmercury iodide, stirred with a little water, and poured into boilingwater (1 litre).It is allowed to settle, and the clear liquid pouredoff. A solution prepared in this manner has been kept for more thana year without deteriorating.Use of Salicylic Acid for Preserving Standard Solutions.By H. BORNTRAGER ( Z e i t . and. Chem., 27, 641--642).-The additionof a pinch of salicylic acid to each litre of a thiosulphate solutiongreatly diminishes its tendelicy t o decompose. The author’s deter-minations show large variations, but not a progressive diminution instrength. M. J. S.Applications of Spectrophotometr y to Chemical Physiology.By E. LAMBLING (Arch. de Physiol., 4th Series, 12, 1--.34).-This1)aper gives an historical account of the spectrophotometer, and of theprinciples upon which the spectrophotometric method depends.Thepractical application of the method for quantitative purposes in-xolves :-(1) The choice of a region of the spectrum; (2) the deter-mination of the coefficient of extinction of the coloured solution forthat region ; and (3) the determination of the amount of absorptionof the colouriig matter for the same region. When two colouringmatters are mixed in a solution, they may also be estimated quantita-tively, provided the absorptive power of each of the two pigments fortwo regions of the spectrum be previously known.Finally, t,he application of such methods t o animal pigments (of theblood, bile, urine, &c.), is pointed out.Determination of Chlorine in Plant-ashes. By A. JOLLES( Chem. Ceiztr., 1888, 863-864, from Zeit. Nahrunpnittel u.Hygiene,2, 81).-The method the author proposes as the best is as follows:-The plant (10 grams) is incinerated gently in a platinum dish,moistened with an alcoholic solution of sodium carbonate, the alcoholburned off, aiid the process repeated; after this, the whole of thecarbon may be burnt off without an1 fear of chlorine being lost, andN. H. M.W. D. H74 ABSTRACTS OF CHEMICAL PAPERS.the ash may he extracted by means of water and the determinationfinished in the usual manner with silver nitrate. This deviation fromthe ordinary direct combustion of vegetable matter in the determina-tion of chlorine obviates the chance of a loss of this element whichmight otherwise take place. J. W. L.Method for the Determination of Bromine in Sea-water.By F.GUTZKOW (Chern. News, 58, 190-193).-25o C.C. of sea-wateris mixed with a drop or two of sulphuric acid and with 100 C.C. of asolution containing about 25 grams of copper sulphate. It is thentreated with sodium sulphite solution until the precipitate redissolveswith difficulty, and heated until the blue colour returm; moresodium sulphite is now added, about one-third that already used, andthe whole ag"n heated until blue, and then cooled. In this way,all the bromine is precipitated in a few minutes. After washing theprecipitate, first with 100 C.C. of water containing 1 gram of sulplinricacid, then with a few drops of sodium carbonate solution, it is warmedwith hydrochloric acid until all sulphurous anhydride is removed, andis finally treated with zinc.The filtrate and washings from the copper,which combined should not exceed 25 c.c., are titrated with sodiumhypochlorite by a method of the author's which is described in detailin the original. The flask containing the liquid is fitted with a triple-bored cork ; through one hole passes a tube closed by a piece of india-rubber tubing and a clip, through the other holes two thistle-headedfunnels reaching nearly to the bottom of the flask, one is roughlygraduated. By blowing into the tube, a quantity of liquid is forced u pboth funnels and is titrated in the graduated one, the other servingfor comparing the colour ; in this way an indication of the quantityof hypochlorite required by the whole liquid is obtained, and so theoperation can be finished with greater rapidity than by the ordinarymode of procedure.Determination of Fluorine in Substances Decomposable bySulphuric Acid and especially in Natural Phosphates.BgH. LASNE (BUZZ. Xoc. Chirn., 50, 167- liO).-Sufficient substance toyield 0.2 gram of calcium fluoride is put into a, flask containingstrong sulphuric acid (50 c.c.) and pure sand (10 grams), and con-nected with two wash-bottles, the first of which contains 2.5 grams.and the second 0-5 gram of soda dissolved respectively in 25 C.C. ofwater. Dry air is passed into the flask, which is heated for an houra t 180--260"; it is then allowed to cool, dry air being passedthrough. The soda solutions are united and boiled for a hour;phenolphthaleyn is added, and carbonic anhydride passed through thesolution until it is colourless ; it is then heated for + hour at 50", andtreated with ammonium carbonate, when the silica is almost com-pletely precipitated.The liquid is cooled quickly, diluted to 125 c.c.,filtered through a large folded filter, and 100 C.C. collected. A fewdrops of tropeoline solution is added to the solution, which iscarefully neutralised with dilute hydrochloric acid, It is thentreated with pure sodium carbonate (equal to 0.5 gram of anhydrouscarbonate), boiled until free from carbonic anhydride, and precipitatedD. A. LANALYTICAL CHEMISTRY. 75with a slight excess of calcium chloride. The precipitate is ignited,treated with acetic acid, evaporated to dryness, again treated witharetic acid, and the undissolved calciuni fluoride, washed, ignited, andweighed. N.H. M.General Method for the Separation and Volumetric Estima-tion of Acids : Application to Sulphuric Acid. By G. LINOSSIEI~(BUZZ. SOC. Chin?., 50. 46-47).-The method is applicable to allacids which yield insoluble compounds when combined with metalswhich are precipitated by hydrogen sulphide in acid solution. Thedeterminahn of sulphuric acid is carried out as follows :--The s o h -tion of the sulphate (containing 0.05 to 0.1 gram) contained iri adish is treated with alcohol (2 vols.), heated almost to boiling, andprecipitated with a slight excess of lead acetate. When cold it ismaslied by decantation with a mixture of alcohol and water (0.5 to1 vol.), passing the decanted liquid through a small filter.The traceof lead sulphate on the filter is washed with aqueous hydrogensulphide into a flask ; the rest of the lead sulphate is shaken with asaturated solution of hydrogen sulphide, the liquid poured on to nfilter, and the precipitate treated with a fresh amount of hydrogensulphide and filtered. It is then washed with aqueous hydrogensulphide until the filtrate gives no reaction with Poirrier’s orange.The whole of the sulphuric acid is then i n the filtrate, and is titratedwith decinormal soda solution. N. H. 31.Volumetric Estimation of Boric Acid, and of Ammonia inAmmonium Salts. By J. MCGLASHAN (Chew. News, 58, 175-176).-By using Poirrier’s oranges I and 11, boric acid and ammo-nium borate can be titrated directly with normal soda, but boraxmust first be made neutral to methyl-orange with aulphuric acid;boracite must be heated with dilute sulphuric acid, made neutral tomethyl-orange with soda, and any carbonic anhydride eliminated beforetitrating.Ammonia is objectionable in any form except as borateor hydroxide, the latter when dilute is neutral to both orangeh.Therefore, with these indicators ammonia may be titrated with soda,in any ammonium salt, without distillation. With ammonium car-bonate and with arsenates, the end reaction is not distinct, but withhydrogen sulphide it is sharp. D. A. L.Resorcinol as a Test for Nitrates. By D. L~NDO (Chem.News, 58. 176--177).-For testing with resorcinol, 10 grams are dis-solved in 100 c .~ . of water, and one drop of this solution, one drop of15 per cent. hydrochloric acid, and 2 C.C. of concentrated sulphuric acidare added to 0.5 C.C. of the nitrate solution (compare Abstr., 1888,1337) ; one in 500,000 gives a definite permanent purple colour aftersome time, whilst with increasing strengths of nitrate solution thecolour becomes more intense, until with one in 10,000 the vivid purple-red colour is so intense as only to be distinctly seen i n the lowerportion of the band. Resorcinol is valueless without hydrochloric acid,but with it, is a more delicate test for nitrates than ordinary phenol.Copper suiphate does not aid the reaction materially. The reagent76 ABSTRACTS OF CHEMICAL PAPERS.alone gave a band which, however, cannot be mistaken for the nitrateband.With nitrites, it is more delicate than with nitrates ; withchlorates it is no good, with dichromate (0.5 gram per litre) it gives ared to buff upper with a purplish lower band, the latter changing to pinkor with hydrochloric acid to reddish-brown ; the colours are slightlydifferent if the acid is run in at once, or after some delay. Perman-gsnate, N/10, with 4 vols. water, gives a, dark-orange upper andyellowish lower band ; with hydrochloric acid, these are respectivelyorange, red, and greenish. Hydrogen peroxide in dilute solution yieldsa green and brownish compound b;lnd. D. A. L.Estimation of Phosphorus in Iron and Steel. By P. W.SHIMER (Chem. News, 58, 165--168).-Dissolve 1 gram of iron in20 C.C.of nitric acid, sp. gr. 1-20, and add to the boiling solution10 c,c. of a solution of 20 grams of potassium permanganate in a litreof water, 2.5 C.C. a t R time, and after a few minutes 5 C.C. of hydro-cliloric acid, sp. gr. 1.12. When the action has ceased, add a mix-ture of 5 C.C. of concentrated sulphuric acid and 5 C.C. of water, andevaporate until fumes of sulphuric acid begin to come off. Whencool, add 5 C.C. of nitric acid, sp. gr. 1.20, and sufficient water; boilto dissolve iron salts, filter, and wash with water. The residueserves well for the estimation of silicon. Heat the filtrate to 80"and add 5 C.C. of ammonium molybdate (5 grams of MOO,, 20 C.C.ammonia, sp. gr. 0.96, 30 C.C. nitric acid, sp. gi.. l a % ) , then keep atGO" until the liquid is clear, which occupies less than an hour when thesolution is not too dilute.The yellow precipitate is washed withacid ammonium nitrate solution, dissolved in ammonia and pre-cipitated by magnesia mixture. The method gives good results bothfor silicon and phosphorus.A few experiments were made using sulphuric acid and ammoniumsulphnte instead of nitric acid and ammonium nitrate for themolybdate precipitation, with satisfactory results. I). A. L.Influence of Sulphur on Eggertz's Carbon Colour-test. l 3 ~T. W. HOGG (Chern. News, 58, 175).- When ordinary steels contain-ing say 0.05 per cent. of sulphur are dissolved in the usual manner,the sulphur separates out and produces a turbidity which interfereswith the colour-test for carbon ; a fact easily proved by dividing sucha solution into two portions, filtering one, and then comparing thecolour produced in the filtered and unfiltered solutions.Conse-quently, if a common steel is compared with a standard of pure steel,the colour intensity is sure to be over-estimated, and vice versd.D. A. L.Quantitative Analysis by Electrolysis. By A. CLASSEN andR. SCHELLE (Ber., 21,2892-2899).-The current from two of Farbakyand Schenek's accumulators, fully charged by a dynamo giving Rcurrent of 20-25 amperes, was employed in making 50 analyses inthe course of six days. Four to eight analyses were made simul-taneously, and the current was employed continuously day and night,except during the short intervals required for changing the platinuANALYTICAL CHEMISTRY.7 7dishes, During this time the strength of the current decreased from2.05 to 1.92 volt, so that one charge would be sufficient for 60 to 70analyses. The condition of the accumulator can be ascertained fromthe specific gravity of the sulphuric acid, which is 1.240 when theaccumulator is charged and 1.118 when i t is not charged. The pre-cipitated metal is in a more suitable condition than when a battery ordynamo is employed.Experiments which were made with Neumann’s (Abstr., 1888,529) and Wolffs ( Z e i t . ung. Chem., 1888, 296) voltameters, employ-ing currents of various strengths, show the necessity of working underthe same conditions when repeating electrolytic methods of analpis(compare Classen, Quantitative Analyse durch Electrolyse, 2nd ed., 43).In the separation of antimonyfroin tin in sodinm sulphide solution,the solution, freed from antimony, is boiled with ammonium pulphate,and the tin precipitated by electrolysis (compare Abstr., 1884, 932).A simpler and more convenient method is to convert the stannicsulphide into hydrogen stannic oxalate and electrolyse the solution.For this purpose, the solution is acidified with dilute sulphuric acid,and the sulphide oxidised with ammoniacal hydrogen peroxide, or thehot alkaline solution is treated a t once wi+h hydrogen peroxide untilit becomes colourless, acidified with sulphuric acid, neutralised withammonia, and more hydrogen peroxide added.The solution is thenboiled, filtered, and the residual stannic acid washed off the filterwith and dissolved in a hnt solution of oxalic acid.If there is aresidue of sulphur, i t is separated by filtration, washed with a coldsaturated solution of hydiwgen animonium oxalate, and the washingsadded to the filtrate. The solution, which should contain at least50 C.C. of the hydrogen ammonium oxalate solution, is electrolysedwith a current giving 8-10 C.C. of explosive gas per minute.The electroljtic deposition of copper from its salts, dissolved in asaturated solution of ammonium oxalate, is hastened very consider-ably if the solutian is kept acid, especially towards the end of theoperation, by adding excess of a cold, saturated solution of oxalicacid. The smaller the quantity of copper, the more oxalic acid soln-tion may be added.A solution poor in copper can be mixed withthe oxalic acid solution a t the commencemtnt of sthe process, but inconcentrated solutions, the precipitation must be carried out in a solu-tion as nearly neutral as possible to avoid the separation of copperoxalate. If the copper solution is kept a t 40-50°, aLout two gramsof copper are deposited in from 3 to 4 hours. A current giving3-4 C.C. of explosive gas per minute mas employed, and quantitativeexperiments showed that the whole of the copper is deposited.Separation of Calcium, Barium, and Strontium. ByKUPFFERSCHLAEGER (Bull. SOC. Clzim., 49, 854- 856).-A quantitativeanalysis of a mixture of the carbcnates of barium, strontium, andcalcium can be carried out as follows :--The mixture is dissolved ina slight excess of very dilute nitric acid, the solution evaporated todryness, the residue dissolved in distilled water, and the filtered solu-tion again evaporated to complete dryness, The residue of mixednitrates is agitated with a small quantity of a mixture of absoluteI?.s. I(78 ACSTRACTS OF CHEMICAL PAPERS.alcohol and ether, and the solvent separated by filtration as soon as thesolution becomes clear ; this process is repeated three times, the propor-tion of ether being gradually increased until the mixture contains equalvolumes of the constituents. The residual mixture of the nitrates ofbarium and strontium is dried, dissolved in water, and treated witha cold saturated solution of potassium dichromate.The precipitatedbarium dichroniate is washed with cold, very dilute a,lcohol, and con-verted into sulphate by heating with sulphuric acid. The strontiumin the filtrate is converted into sulphate by warming the solutionwith dilute sulphuric acid. A solution of strontium chloride is notprecipitated by potassium dichrornate. F. S. K.Volumetric Estimation of Mercuric Chloride. By G. KASSRER(Arch. Phawn. [ 3 ] , 26, 595-604).-The method promises well forpharmaceutical practice. 50 grams of the organic compound contain-ing mercuric chloride is placed in a porcelain dish without previousdivision, 500 C.C. of water is added, and the mass is well kneadedwith a pestle. 500 C.C. of a solution of 0.4 gram of potassium anti-monions tartrate and 1 gram of sodium phosphate, or in place of thelatter 1 to 2 grams of sodium acetate, is now added and the kneadingcontinued.A very intimate mixture is thus obtained, and a milkyliquid results from the decomposition of the mercuric chloride.About 500 C.C. is now filtered off, and titrated with decinormal iodinesolution after the addition of freshly prepared starch solution, anda suffirient quantity of sodium hydrogen carbonate. The iodineemployed corresponds to the amount' of unchanged tartrate remainingin the filtrate. The reaction is as follows :-4HgCI, + Sb,O, + 2H,O= 4KC1 + Sb,05 + 4HgC1. The presence of phosphoric and organicacids is admissible, but not of free hydrochloric acid.By A. STRENG (Jahrb. f. Mi%, 1888,ii, Mem., 142-152 ; continuation of Abstr., 1886, 4877.-For detect-ing tin under the microscope, t'he author avails himself of the browncolour produced on adding hydrochloric acid and platinum chloride.When the solution is effected, a drop of the liquid is transferred to anobject-glass, and a grain of potassium chloride added, and the solutionslightly evaporated.In this way, rhumbic crystals of pot'assinmstannous chloride (2KC1 + SnC1, + H,O) are form_ed. They-aremostly combinations of the forms mP, mPm, 03Pq Pm, Pm.When the staunous chloride has been thus detected, a drop of nitricacid is added, and the solution heated. The stnncous chloride isconverted into stannic chloride, and the imperfectly soluble salt,K,SnCl, is formed. This crystallises in the regular system, and isperfectly isotropic.This reaction may be employed for detectingstannous and stannic oxides in compounds soluble in hydrochloricacid. Caesium chloride may be used instead of the isomorphouspotassium salt. The author also describes methods for detectingpotassium, caesium, and rubidium, sodium, and silicon.Detection of small Quantities of Germanium. By K. HAUSHOFER(Clrern. Centr., 1888, 867, from Xitzber. Akad. JIGnche~~, 1887, 133).J. T.Microchemical Reactions.B. H. BAX ALP TIC AL C €1 ENIST R Y. 70-By heating in an atmosphere of hydrogen snlphide, the germaniumin the mineral argyrodite is converted into the sulphide GeS, whichis crystalline, and may be detected and yecognised by means of ihemicroscope.With concentrated sulphuric acid, it forms a white, non-crystalline substance, with concentrated nitric acid it is converted intothe white, crystalline oxide, GeOz, which is soluble in dilute nitricacid and water, and crystallises out of the solution again on evapora-tion. Heated in a tube, it sublimes similarly to antimony oxide, butdiffers from this by its solubility in water, and also by melting t o clearcolourless drops. It, is necessary to apply the potassium iodide testalso, as a means of distinguishing it from the mercuric sulphide, whichhas also been found present in argyrodite. J. W. L.Characteristic Reaction of Bismuth. By E. L ~ G E R (BUZZ. XOC.Chi%., 50, (31-93) .-A solution of bismuth iodide and potassiumiodide is sometimes used for detecting alkalo'ids, with which it givesorange-yellow precipitates.It is suggested that the reaction shouldbe employed for detecting bismuth. A solution is prepared bydissolving cinchonine (1 gram) and potassium iodide (2 grams) inwater (100 c.c.). Other alkaloids may be nsed instead of cinchonine,but thir seems to give the most sensitive reaction. The reagent mustbe added in excess ; the presence of too much nitric acid, and espe-cially the presence.of hydrochloric and sulphuric acids, is to be avoided.Bismuth may be detected in solutions containing only 1 part in 500,000parts. Solutions which contain &her metals besides bismuth areprecipitated with hydrogen sulphide, the sulphides of copper, lead,cadmium, mercury, and bismuth converted into nitrates, then in tocarbonates, and the caiabonates of bismuth and lead separated bymeans of potnssium cyanide ; these carbonates are converted intoclibrides, and the lead chloride separated by means of alcohol.Thealcoholic solution is evaporated to dryness, c?issolved in a drop ofnihric: acid and sorne C.C. of water, and treated with the rexgent. Solu-tions of the salts of mercury, cadmium, silver, copper, and lead alsogive precipitates of various colours with the cinchonine reagent.N. H. M.Determination of Oxygen dissolved in Water. By L. W.WINKLER (Ber., 21, 2846-2854) .-The method consists in oxidising:in excess of manganese hydroxide in presence of alkali by the oxygenpresent in a weighed amount of the water; potassium iodide andhydrochloric acid are then added, and the iodine which separates(which is equivalent to the amount, of dissolved oxygen) titrated withsodium thiosulphate.A solution of maiiganous chloride (free fromiron) is made of such a strength that 100 C.C. contains 40 grams ofthe salt (MnC1, + 4H20). The soda must be free from nitrate, andthe solution prepared of eight times the normal strength ; potassiumiodide (10 grams) is dissolved in 100 C.C. of the soda solution, the restof which is kept. A strong flask of about 2 litre capacity is filledwith the water ; 1 C.C. of the potassium iodide soda solution is addedby means of a pipette reaching nearly to the bottom of the flask, then1 C.C. of the manganous chloride solution. The flask is closed, carebeing taken t h a t no bubble of air remains, and the contents mixed80 ABSTRACTS O F CHEMICAL PAPERY.When the precipitate settles, fuming h~drochIoric acid (3 s.c.) isadded by means of a pipette similar to those previously used.Theflask is again closed, the contents mixed, and the yellow liquid titratedin the usual manner with sodium thiosulphate, the most convenientstrength of which is 1/100 normal, so that each C.C. corresponds witli0.055825 C.C. of' oxygen (at 0" and 760 mm. pressure).When the water to be analysed contains mucii carbonic anhydride,more of the reagent must be added, as manganous carbonate is notoxidised by the oxygen. In the case of waters containing nitrates, theprocess has to be modified : a soda solution containing no potassiumiodide is first added, then hFdrochloric acid (twice the amount other-wise used), and after three minutes a solution of potassium iodide. Amanganic chloride solution is then prepared as follows :--500 C.C.ofdistilled water is treated with the pure soda solution (1 c.c.), 5 to 10drops of the manganous chloride solution, and then sufficient hydro-chloric acid is added to dissolre the precipitate. 100 C.C. of thissolution is taken out and diluted with distilled water; to the rest,100 C.C. of the water to be examined is added. After two to threeminutes, both solutions are treated with potassium iodide and theiodine which separates determined as usual. From the differencein the amount of thiosulphate used, the correction for 100 C.C. ofwater is calculated.Concordant results obtained b j the new method are gil en.N.H. M.Ash Determination. By F. A. FL~~CKTGER (Zeit. anal. Chem., 27,637-638).-The substance is heated in a roomy platinum capsule sogently that carbonisation takes place without combustion. It irthen cooled, a copious amount of water is added, and the whole eva-porated completely on the water-bath. On reheating the carbonaceousrebidue very gradually, it burns a t a low temperature, and veryquickly. &I. J. S.Wet Methods of Organic Analysis. By J. MESSIKGER (Bey., 21,2910-2919) .-Organic compounds, as Cross and Bevan have show11(Proc., 1888, 76, and Trans., 1888, 889), are completely oxidisedwhen warmed with chromic acid and concentrated sulphuric acid.I fnitrogen is present, it is evolved as such or as ammonia, whilstsulphur, phosphorus, and arsenic are converted into the corresFond-ing acids. Halogens are evolved in the free state, and metals remain assulphate or, with a large excess of chromic acid, as chromates.To estimate the quantity of carbon, the substance (0*15-0*35 gra,m)is weighed in a small bulb or tube, and placed in the apparatusemployed by Classen for the estimation of carbonic anhydride(Quudtative Analyse, 3rd ed., 239), together with chromic acid(?5--.6 grams) or powdered potassium dichromate. A gentle streamof air, free from carbonic anhydride, is passed throngh the appa-ratus to drive out the carbonic anhydride, the weighed potash bulbsand sods-lime tube are attached, and the latter connected with acalcium chloride tube to prevent absorption of moisture from theair.Concentrated sulphuric acid (30 c.c.) is then poured througANALYTICAL CHEMISTRY. 81tlle funnel, and the stream of air stopped. The flask is warmed verycautiously until the evolution of carbonic anhydride commences, andthen the heating is immediately discontinued until the reaction isalmost at an end. Pureair is passed through the apparatus for half an hour, and the tubesweighed. Tlie results obtained are very satisfactory, except in thecase of substances which sublime readily, but great care must betaken when heat is first applied. I n analysing volatile substances,the bulb is broken by means of the funnel. If the substance con-tains halogens, a Dreschler’s flask of about 100 C.C.capacity, contain-ing 40 C.C. of concentrated potassium iodide solution, and a smallU -tube filled with glass-wool, half of which is moistened with a solu-tion of silver nitrate and half with concentrated sulphuric acid, areinterposed between the condenser and the potash bulbs. Quantitativeexperiments with compounds of the most varied nature gave satis-factory results (compare Cross and Bevan, Zoc. cit.).Sulphur can be estimated, except in the case of extremely volatilesubstances, as follows :-The substance (0.15-0.35 gram), togetherwith potassium permanganate (1&2 grams), and pure potash (0.5gram) is placed in a flask of 500 C.C. capacity provided with a con-denser, water (25-30 c.c.) poured down the condenser, and themixture heated for 2-3 hours.Concentrated hydrochloric acid isthen gradually poured down the condenser into the cold inixture,which should be of a reddish colour, mid after the evolution of gashas ceased, the whole is heated until the liquid beconies clear. Thesulphuric acid is then precipitated with barium chloride. Potassiumdichromate (2-3 grams) and hydrochloric acid (20-25 C.C. : 2 partsconcentrated acid, 1 part water) may be employed instead of potas-sium permaiiganate and potash. The operation is carried out in themanner described, but after heating for about two hours a few dropsof alcohol are added to determine whether all the dichromate hasheen reduced; if the odour of aldehyde is perceptible, the mixtureiuust be heated again and the test repeated.Both methods can alsobe employed for the detection of sulphiir. Numerous quantitativecbxperiments gave satisfactory results, but in the case of a few sul-phones i t was found that sulphur cannot be estimated by this method.Phosphorus, arsenic, and antimony in organic compounds can beestimated by placing the substance (0.3-0.4 gram) with chromic acid(4.-5 grams) in a flask provided with a condenser, pouring sulphuricacid (10 c.c., 2 parts concentrated acid, 1 part water) down the con-denser, and heating gently. After an hour’s time, sulphuric acid(10 c.c.) is added, and the heating continued for about an how.The mixture must always be heated very carefully, and the cold solu-tion should be perfectly clear.Some antimony compounds requireonly 1 gram of chromic acid and 10 C.C. of sulphuric acid.In the estimation of phosphorus, the solution is warmed withammonium nitrste (3-4 grams) and ammoniuni molybdate solutior!(50 c.c.) for 2-3 hours, filtered, the precipitate washed 6 to 8 timesby decantatioii with ammonium nitrate solution (20 grams in 100 C.C.of water), throan on to a filter, and dissolved in not more than 40-50 C.C. of warm dilute (2 per cent.) ammonia ; a concentrated solutionThe process occupies about two hours.VOL. LVI. 82 ABSTRACTS OF OHEMIOAL PAPERS.of citric acid (4-5 drops) is added to the filtrate, and the phosphoricacid precipitated with magnesia mixture.In estimating arsenic, the solution is diluted to about 100 c.c.,heated to about 70", and the arsenic precipitated with hydrogen sul-phide.The precipitate is washed with water containing hydroqensulphide until free from chromium salts, and then converted intoarsenic acid by means of ammoniacal hydrogen peroxide (compareClassen, Abstr., 18b3, 934). After boiling for an hour, ammonia isadded to the filtered solution, and the arsenic precipitated with mag-nesia mixture. Antimony is estimated by adding potash and excessof sodium sulphide, boiling for half an hour, and precipitating themetal electrolytically.Metals are estimated by mixing the solution with excess of ammo-nium oxalate and precipitating electrolytically. Halogens can bedetected by warming the substance (1-2 mgrms.) with chromicacid and sulphnric acid, and passing the gas evolved into a dilutesolution of potassium iodide ; quantitative experiments gave unsatis-factory results.F. S. K.The Safety of Commercial Kerosene Oils. Bp S. B. NEWBURYand W. P. CUTTER (Amer. Chem. J., 356-362).-Although oils areregularly testea for their flashing points and conclusions drawn as totheir being sa€e for burning in lamps, it is noteworthy that manymodern lamps heat their reservoir of oil to temperatures above thelegal flashing point, and that there are not sufficient experimentaldata to allow of the correct interpretation of the flashing point deter-minations into +terms expressing the inability of such oils to formexplosive mixtures of vapour with air. All hydrocarbons up to andincluding octane, form at ordinary temperatures mixtures that can beexploded; nonane mixtures (b.p. 148-1.50") explode sharply at79" F., and decane at 104" F.The addition of small quantities of low-boiling oils materiallylowers the flashing point of another sample. Thus a sample flashingat 212" F. was made to flash at 145" F. by the addition of 5 per cent.of heptane; at 110" F. by the addition of 5 per cent. pentaneor hexane, or 10 per cent. heptane; at 96" F. by the addition of15 per cent. heptane ; and at ordinary temperatures by the additionof 10 per cent. pentme or hexane, or 20 per cent. heptane. The tem-peratures at which am oil may be kindled in an open vessel approachesthe more nearly to the Bashing point the more homogeneous the oil is.The flashing point of an ordinary oil may be materially raised, withbut little diminution of weight, by passing a current of air throughit for several hours.H. B.Solubility and Estimation of Paraffin. By B. PAWLEWSKI andJ. FILEMONOWICZ (Ber., 21, 2973-2976) -The following table givesthe solubility at 20' of ozokerit paraffin of sp. gr. 0.9170 at 20°,melting at 64-65', and solidifying at, 61-63' :ANALYTICAL CHE3lISTHY.-Solvent.Carbon bisulphide.. ...................Light petroleum, up to 75" G., sp. gr.0'7233 ............................Turpentine oil, sp. gr. 0 -857 ; b. p. 158-186". ..............................Cumene (comm.), up to 160°, sp. gr. =0 *867. .............................Cumene (frac.), 150-160", sp. gr.= 0.849Xylene (comm.), 138- 143",sp. gr. = 0.866(frac.). 136-1383, sp. gr. = 0.864. .Toluene (comm.), l(B--llO",sp.gr. = 0.866(frac ), 108.5-109 5", sp. gr. =0-866 ..............................Chloroform ..........................Benzene .............................Ethyl ether ..........................Isobutyl alcohol (comm.), sp. gr. = 0.804.1l:tliyl acetate. ........................Amy1 alcohol, 127-129", sp. gr. = 0813 .l'ropionic acid.. ......................)'ropy I alcohol ........................Met hpl alcohol, 65.5 - 66 5 O , ~ p . gr. = 0.798JIetli! 1 forniate .......................(fluci 11 acetic acid ....................,,,,Acetone, 55-5-56 5", sp. gr. = 0.797.. ...Ethyl alcohol, 99.5' Tr.. ...............Ethyl alcohol, 945" Tr.................Acetic anhydride.. ....................l?ormic acid (crjst.) ...................Ethyl alcohol, 75" Tr.. .................Paraffin (grams),dissolved by100 grams12 *9911 '736.064.283 -993.954.s93 -833 -922 '421 -9Y1 -950.2880 '2620 '2380 * 8190 -20%0 -1660 -1410 ' o n0 -0600 -0600 -0460 -0280 -0130 *Wd03-.-100 C.C.-8 *485 -213-723 -393 -433.773 -343 -413 -611 -750 -2280 '2090 '1640 -0560 -0630 '015-----c --Weight of solventrequired to dis-solve completely1 part d paraffin.7.68'516 *123 -426-025 -122 -726 -125 *541 '360 '350.8352 -9378'7419.0453 -6495 -3595 -3709 -4l a 7 -51648 -71668 -62149 * 53856 -27689 -2330000 *oThe liquid constituents present in man-j- prodncts of the petroleumor ozokerit industry are soluble in glacial acetic acid, whereas vaselin,cerisin, ozokerit, and paraffln are almost insoluble.To estimate thequantity of solid paraffin in petroleum, lubricating oils, mineral oils,vaselin, &c., 5-20 C.C. of the mixture is well shaken with 100-200 C.C.of glacial acetic acid, the residual para& thrown on to a weighed filter,washed two or three times with glacial acetic acid, and then two or threetimes with alcohol of 75" Tr., dried and weighed, or the residual paraffinis washed, dissolved in benzene or ether, the solution evaporated, andthe residue weighed. This method is quick and accurate, and can becarried out at the ordinary temperature, F.S. K.Analysis of a Mixture of Silver Chloride, Cyanide, Thio-cyanate, Ferricyanide, and Ferrscyanids. By J. TELSS~ER (BUZZ.Soc. Chim., 50, 10&106).-The mixture occurs in the analysis ofmaterials used in the purification of coal-gas. Sodium carbonate isheated in a crucible until aahjiirous, the weighed substance and Born81 ABSTRACTS OF CHEMICAL PAPERS.potassium nitrate are added, and the whole is heated. The productis extracted with water, which leaves a residue of pure silver andferric oxide. In the solution, sulphur is determined as barium sul-phnte and chlorine as silver chloride. The residue is dissolved innitric acid, the silver determined as chloride, and the iron as sesqui-oxide.Equations are given by means of which the amount of eachsalt present in the mixture is calculated.Estimation of Paranitrotoluene. By F. REVERDIN and C.DE LA HARPE (Bull. Xoc. Chim., 50, 44-46).-The method is basedon the fact that paranitrotoluenesulphonic acid is readily convertedby boiling with soda into dinitrosulphostilbene which yields a redcolour when dissolred in alkali, whilst orthonitrotolnenesulphonic acidis not attacked by soda, and the alkaline solution is yellow. 2 C.C. ofpure orthonitrotoluene is heated in a water-bath with 6 C.C. of sul-phuric acid (containing 25 per cent. of anhydride) for three hoiirq,the product cooled and diluted to 1 litre. I n a similar manner amixture of orthonitrotoluene (96 parts) and paranitrotoluene (4 parts)is sulphonated and the product diluted to 200 C.C.I n determiningthe amount of paranitrotoluene, the substance and nitrotoluene (con-taining 4 per cent. of the para-compound) are sulphonated, the pro-ducts diluted to 200 c.c., and the colours compared which are obtainedby mixing 1 C.C. of each solution with 5 C.C. of aqueous soda. If thesample to be aiialysed gives a stronger colour, a measured quantity(50 to 50 c.c.) is progressively diluted with the solution of ortho-nitrotoluenesulphonic acid until 1 C.C. when heated with 5 C.C. ofaqueous soda gives the same amount of colour as the solution con-taining 4 per cent. The percentage of paranitrotoluene can then becalculated. N. H. &I.Detection of Methyl Alcohol in Wood Spirit.By J. HABER-MAXN (Zcit. anal. Chem., 27, 663, from VerAandl. nut. Ver. Byutm, 26).-Commercial methyl alcohol contains impurities which reduce per-manganate energetically. Cazeneuve and Cotton shake 10 c c. of thespirit to be tested with 1 C.C. of a 0.1 per cent. solution of per-manganate a t 20'. If wood spirit is present. decolorisation takes placeimmediately ; with pure alcohol, 20 minutes is required. Etherealoils, which may be present in spirit o r brandy, and would cause asimilar reduction, may be removed by shaking the spirit twice withhalf its volume of the purest olive oil and then filtering through a wellwetted filter.N. H. M.If sugar is present, the spirit must be distilled.M. J. S.Composition of Natural Brandies and the Way of Dis-tinguishing them.By X. ROCQUES (Bull. SOC. Chim., 50, 157-164).-500 C.C. of the brandy is distilled in a, Le Bel-Henniger ap-paratus and nine fractioiis of 50 C.C. each collected, the temperaturesbeing noted. Each fraction is subjected t o the following tests:-(1) Rosaniliue bisulphite, (2) aniline acetate, (3) sulpharic acid,(4) permanganate, (5) ammoniacal silver nitrate solution. Theresults of several analyses of brandies are given in tables.N. H. 31ANALYTICAL CHEMISTRY. 85Estimation of Sugar in Presence of Carbohydrates.By R. W. BISHOP (Chern. Centr., 1888, 952-953, from Msc. ,Won.Sci., 32, 558).-The author has carried out a number of experimentswith a view to determine the conditions under which inversion maybe completed without a t the same time damaging the accompanyingcarbohydrates.It was found that sulphuric acid has a greaterpower of inversion than hydrochloric acid, but it appears that hydro-chloric acid is the best for the conversion of starch into dextrose.Prolonged heating of inverted sugar with the acid seems to act onthe lmvulose rather strongly, and the solution becomes less lmvo-rotatory and eventually dextrorotatory. For the inversion of cane-mgar, 0.5 C.C. of hydrochloric acid is snfficient, and the heating is con-tinued for 10 minntes at 95". For the conversion of dextrin, thesolution should not contain more than 1-3 grams of carbohydrates i n50 C.C. The inversion is performed by adding 2 C.C. of hydrochloric acidand heating for three hours at 95".J. W. L.Detection of Sugar in Urine. By C. SCHWARZ (Arch. Pharnz.[3], 26, 796, from Pharm. Zeit., 33, 465).-1 to 2 C.C. of leadacetate is added to 10 C.C. of urine and filtered ; 5 C.C. of the filtrateis mixed with 5 C.C. of normal potash solution and one or two dropsof phenylhydrazine, well shaken and vigorously boiled ; in the presenceof sugar, the liquid becomes lemon- to orange-yellow, and becomesopaque on adding an excess of acetic acid owing to the immediateformation of a finely divided yellow precipitate. In the absence ofsugar, this precipitate never OCCUTS with urine. J. T.Detection of Chloral or Chloroform in Liquids. By C.SCHWARZ (Zeit. anal. Chem., 27, 668-669, from Pharm. Zeit., 33,419).-Either of these substances when boiled with resorcinol and anexcess of soda gives a red colour, which disappears on acidifying and isrestored by alkalis.If, on the other hand, an excess of resorcinol andonly a dropor two of soda solution is used, the product is n yellowish-red solution with intense yellowish-green fluorescence. 0.0001 gramof chloral hydrate in 1 C.C. gives this reaction very diwtinctly whenvigorously boiled with 0.05 gram of resorcinol and five drops of sodasolution. Rf. J. S.Modification of the Reichert-Meissl Metho& of ButterAnalysis. By M. MANSFELD (Chem. Centr., 1888, 870-871, fromMilch Zeit., 17, 281-283).-1n order to obviate the possible errorarising from the use of alcohol in the saponification of the butter-fat,theauthor has tried the use of alkali alone, the latter being added tothe fat in a small flask and heated on the water-bath for two hours, a tthe end of which time the saponification is complete, and the processis finished as Wollny prescribes. J.W. L.Densities and Refractive Indices of Certain Oils. By J. H.LONG (Amer. Chem. J., 10, 392--405).-The following values arcobtained-the densities a t 20" being compared with water at 4' a86 ABSTRACTS OF CHEMICAL PAPERS.unity, and the substance weighed in a vacuum; the refractive indicesare for sodium light a t 20" :-Olive oil .......... 0.9130 Ref. index 1.4703Cotton-seed oil. 0.9191 2.4732Sesame oil ........ 0,9191 1.4740Mustard oil.. 0.9121 1.4742Castor oil.. 0.9589 1.4791Lard oil 0.9122 1.4686Peanut oil ........0.9173 1.4717The densities and refractive indices are also given for other tempe-ratures than 20". In nearly all cases, the variations due to temperatureare t,he same, namely, about -0.G0068 i n denpity and -0-0004 inrefraction for each rise of 1". The author believes such determiuationsmay prove of value in the identification of other oils........... ..................H. B.Bechi's Newest Method for the Detection of Cotton-seedOil in Mixtures. By G. Biz10 (Chem. Centr., 1888, 873, from AttiInst. Veneto [ 6 ] , 6 ) .--The author finds that pure olive oil gives Bechi'snew cotton-seed oil reaction with slightly acid silver nitrate, whilst,on the other hand, he finds that there are some cotton-seed oils whichdo not give the reaction at all.J. W. L.Qualitative Test for Resin Oil in Vegetable and Mineral Oils.By HOLDE (Chem. Centr., 1888, 952, from Pharna. Zeit., 33, %8).-Whereas Storch's reagent (concentrated sulphuric acid and arihjdrousacetic acid) for the detection of resin oil is not always admissible,the author recommends sulphuric acid of sp. gr. 1.53, which producesa violet coloration with resin oil. If the oil under examinationbecomes sc) dark-coloured with sulphuric acid as to interfere with thereaction, the resin oil may first be extracted with alcohol, when thecolour test is readily performed. J. W. L.Test for Saccharin." By D. LINDO (Chem. News, 58,155).-Theauthor modifies his test for " saccharin " (Abstr., 1888, 1350). Afterevaporating to dryness with nitric acid on a water-bath, a few dropsof alcoholic potash is added to the cold residue ; when this is heated,a greater variety of colours is obtained than by following the originaldirections.D. A. L.Recent Processes for Testing Quinine. By W. LEKZ (Zeit.anal. Chenz., 2 7, 549-631) .-The foreign alkalojids in commercialquinine consist chiefly of cinchonidine and hydro-bases. Fourprincipal methods are in use for the determination of these. In allthese methods, a product (" Nebenalkaloide ") is obtained, containingthe greater part of the impurities together with a certain quantity ofquinine.', In this product, the cinchonidine is determined by the" tetrasulphate process." 1 gram of the mixture is dissolved in9 grams of absolute alcohol and 3 grams of 50 per cent.sulphuricacid. The mixture is kept at 0" for 24 hours, the acid liquid iANALYTICAL CHEMISTRY. 87removed by suction, the crystals are washed with a little absolutealcohol, and then air-dried. They are then dissolved in water, andthe base is precipitated by excess of sodium carbonate. It is driedfirst over sulphuric acid, and then a t 115”. A correction (the amountof which depends on the percentage of cinchonidine found) must beapplied. The author gives a curve for the purpose. The cinchonidineis very nearly pure. The hydro-bases are determined approximatelyby oxidising the quinine and cinchonidine in acid solution by a 1 percent, solution of potassium permanganate, rendering alkaline, andshaking with ether, followed by chloroform.The residues from thesesolutions, although very impure, are regarded as hydroquinine.For the “chromate procew” of De Vrij see Abstr., 1887, 404;for the “ oxalate tesh” see Schaefer (Abstr., 1887, 623). The amountof oxalate prescribed is insufficient for samples containing less than15 per cent. of water, and the cooling at 20” should be prolonged toone hour. Schaefer’s correction of 004 gram per 100 C.C. appears tobe ltoo large.In Hesse’s ‘( bisulphate process” 5 grams of quinine sulphate isdissolved in 12 C.C. of normal sulphuric acid by warming, and thesolution is allowed to erystallise in a naprow-necked funnel in a coldplace. The mother-liquor is withdrawn by a filter-pump into agraduated cylinder, and the crystals washed with 3 C.C.of water.This solution is shaken with 16 C.C. of ether (0.721-0*728), then3 C.C. of ammonia (0.96) added, again shaken, and left for 24 hours.The ether is removed by a pipette, the crystals are collected on afilter, washed with water saturated with ether, dried between filter-paper, washed again with ether, and dried.In the “ crystallisation process ” of Paul and Hewe, 5 ,mms ofquinine sulphate is dissolved in boiling water, and crystallised outfour times, using in the first case 150 c.c., next 130 c.c., and thentwice 120 C.C. The united mother-liquors are evaporated at a lowtemperakmre almost to dryness, the residue dissolved in the smallestpossible quantity of dilute sulphuric acid, made up to 20 c.c., andshaken with ether and excess of ammonia. The crystals which formare treated as in the bisulphate test. The hydro-bases crystallise inpart with the quinine, therefore the mother-liquor should not beused for their determination.The chromate process gives very varying results, but on theaverage gives the highest yield of cinchonidine, especially with thepurer samples The oxalate test gives the lowest numbers, but theyare more concordant than those of the chromate process. The com-position of the bye-product is, however, variable. The bisulphatetest gives results varying considerably. The alkaloids in the etherealsolution ought t o be submitted to the process a second and even athird time, but even with this improvement the whole of the cin-chonidine is not obtained, and the results vary much, but the com-position of the bye-product is more uniform than in the otherprocesses. The crystallisation test has the same advantages as thebisulphate test if the crystallisation is repeated often enough, and is theprocess which i8 least influenced by the presence of hydro-bases. I t is,however, tedious. The process of the German Pharmacopoeia depend88 ABSTRACTS OF CHEMICAL PAPERS.on the fact that the precipitate produced by ammonia in solntionc: ofthe alkalo'ids is soluble i n excess of ammonia, but that much moreammonia is required for quinine than for the other alkalolds. Theexcess of ammonia required varies, however, very considerably withthe temperature. M. J. S.Method for Recognising the Adulteration of Pepper by theAddition of Ground Olive Stones. By GILLET (BUZZ. XOC. chim.,50,173-174).-When 1 gram of olive stones is treated with 1 C.C. ofa 5 per cent. iodine tincture, it acquires, after a quarter of an hour, a,J ellowish colour, whilst pepper is coloured brown or maroon. A seriesof mixtures of pepper with 5, 10, 15, and 20 per cent. of olive stonesare prepared and coloured with iodine tincture. It is then easy todetermine the amount of olive stones in samples of pepper by com-paring the colour obtained with these types.A New Test for the Blood in Carbonic Oxide Poisoning.By R. KATAYAMA (Virchow's Archiv, 114, 53-64).-When ammoniumsulphide holding sulphur in solution and acetic acid are added tohlmd containing carbonic oxide, the result is a beautiful clear red ormse colour ; whereas normal blood becomes greenish-grey, or reddish-preen-grey on the addition of the same reagents. On examining theseliquids spectroscopically, it is found that both in the case of normal andcsrbonic oxide blood the absorption-spectrum indicates that a mixtureof two substances is present. In the case of normal blood, there is aband between C and D and another between D and E ; this lastbecomes double on shaking up the mixture with air. In other words,there is a mixture of sulphur methaemoglobin (see Hoppe-Seyler,Physiol. Chem., 386) and reduced haemoglobin.I n the case of carbonic oxide there are three bands : one between Cand D, due to sulphur methEmoglobin, and two between D and E,due to carbonic oxide hsemoglobin. That is to say, in spite of the pre-sence of sulphur methaemoglobin, the liquid does not become greenish,but remains red, the colour of carbonic oxide haemoglobin overpoweringthe olivegreen of the sulphur methaemoglobin. This test is stated tobe more delicate than Hoppe-Seyler's (Abstr., 1888, 540), and isobtained with a mixture which contains one part of carbonic oxideblood to five parts of normal blood.Estimation of Albumin in Urine. By H. SCHACJMANN (Zeit.afial. Chent., 27, 635-636J-The estimation of albumin is muchaccelerated by collecting it, not on a paper filter, but in a filter-tubeplugged with cotton-wool and connected with a filter-pump. Whenthe washing with hot water is complete, a calcium chloride tube isconnected, and dry air is drawn over the albumin whilst graduallyraising its temperature to 110".N. H. M.W. D. H.M. J. S

ISSN:0368-1769    

DOI:10.1039/CA8895600073

出版商:RSC    

年代:1889

数据来源: RSC

摘要:

89 General and P h y s i c a l Chemistry. DEWAR formed by the Spectrum of Magnesium. By G. D. LIVEING and J. (Proc. &t~. ,!!oc., 44, 241-252) -When an electric arc is between magnesium electrodes,' most of the lines produced spark discharge are observed. The larger number of lines with an arc discharge may be due not to lowness of temperature, but to the greater mass of incandwcent matter, and to a wider range of tem- perature a t different portions of the discharge, recombinations occur- ing a t its edge. The electiic discharge itself may also give rise to vibrations distinct from those due to heat. The seven bands in the green are due to the oxide, as they are only prodiiced in the presence of oxygen or its compounds. If a piece of hurnt magnesium wire be heated in the oxphydrogen flame, the spectrum of magnesium is produced, the met:illic lines appearing if the hydrogen is in excess.The triplet near M which is produced when magnesium is burnt, is found t o be produced in the arc befween rnagnesium electrodes and in many other cahes when oxygen is present, but not in an atmosphere of nitrogeu o r hydrogen, hence it is due to the oxide. Vacuous tube8 are found to be very untrustworthy for the ultra-violet spectra, as the water-spectrum and lines of nitrogen are nearly always present, and the spectra sometinres vary unaccountably. A pump is described in which rubber connections and free contact of the mercury with air are avoided. H. K. T. Ultra-violet Spectra of Nickel and Cobalt. By G. D. LIVEING and J. DEWAR (Proc. Rot/.Xoc., 43,43O).-A comparison is made between a plane Rowland's grating with a goniometer and the concave grating (20 feet focal length) used by Bell. The results agree very closely, the concave grating gives more light, a i d is more suitable for com- plicated spectra, as the overlapping spectra of different orders are not all in focus at once. The coinci- dences are not greater than the theory of chances would allow, aud do not correspond with their chemical relationship. H. R. T. Ultra-violet lines of cobalt and nickel are compared. Two-fluid Cells. By C. R. A . WRIGHT and C. THOMPSON (Proc. Roy. Soc., 43, 489-493).-Cells are set up consisting of platinum plates in acid and alkaline solutions, with the further addition either of oxidising agents to the acid solution or of reducing agents to the alkaline solution.Currents are produced, in the first case with evolution of oxygen from the alkaline solution, in the second with evolution of hydrogen from the acid solution. The quantity of gas evolved was equivalent to the current. The acid and alkali were sul- phuric acid and potassium hydroxide respectively ; the oxidising agents being potassium permanganate, dichromatc, and ferricyanide, ferric chloride, and solutions of chlorine and bromine and the reducing VOL. LYI. 7b90 ABSTRACTS OF OHEMTCAL PAPERS. agents sodium hyposulphite, pyrogallol, cuprous chloride, and ferrous sulphate and ammonium chloride in nmmouiacal solution. Hydrogen was not evolved with sodium sulphite or hypophosphite, potassium ferrocyanide, or manganous hydroxide in ammoniacal ammonium chloride, nor was oxygen with barium dioxide and sulphuric acid, o r with hydrochloric acid and iodine.On the other hand, an aeration plate of platinum sponge gave a current four times as great. Plates of oxidisable metals in alkaline solution could be substituted for the reducing substance, hydrogen being evolved in the acid solution ; this was particularly the case when potassium cyanide was used. Gold, silver, and palladium in cyanide solution gave hydrogen, but platinum and iron were ineffective. When both oxidising and reducing agents are used, comparatively powerful currents are produced. Effect of Chlorine on the Electromotive Force of a Voltaic Couple. By G. GORE (Proc. Roy. Soc., 44, 151--152).-1f the electromotive force of a small magnesium-platinum couple in distilled water is balanced through a galvanometer and dilute chlorine-water is gradually added, the electromotive force does not alter a t first, but after a cert,aiii point has been reached (1 in 17,000 millions) it begins to increase rapidly.I n t h i s way, the one ten-thousand-millionth of a grain of chlorine in 0.1 C.U. of water can be detected. Other electrolytes give the same reaction, b u t require a larger quantity of dissolved substance. H. K. T. H. K. T. Development of Voltaic Electricity by Atmospheric Oxida- tion. By C. R. A. WRIGHT and C. THOMPSON (PYOC. RUy. Xoc., 44, 182- 2OO).-The electromotive force of cells in which aeration plates are used, falls off very rapidly if the current density exceeds a certain amount.When oxidisable liquids are used, it is difficult to determine, as it appears to vary with the nature of the aeration plate, and also with the incorrodible plate in the liquid to be oxidised. For determin- ing these electromotive forces, an arrangement is used in which t5e asration plate can be kept undisturbed, and in which the oxidisable substances are protected from alterations of temperature, impurities from the air, &c. After a few hours or days, the currents become constant. In these cells, variation of the asration plate produces a difference in the electromotive force independent of the oxidisable plate used ; similarly the effect of varying the metal is independent of the asration plate. The nature and strength of the liquid affects the results to some extent.The electro- motive force actually generated falls very considerably short of that corresponding with the chemical changa, especially when the current density is large. With silver as the oxidisable plate, however, the electromotive force is higher than the theoretical, this being due to the high negative value of the thermovoltaic constant of silver in contact with sulphurib acid. When oxygen was substituted for air over the aGration plate, a slight rise in the electromotive force was observed. With aeration plates immersed in coal-gas or hydrogen, and opposed to a platinum plate in alkaline permanganate or in sulph uric acid and potassium dichromate, very weak and variable Tables of results are given.GESERAL AND PHYSICAL CHEMISTRY.9 1 currents were observed. aGration plates in hydrogen and air respectively. The same was the case with cells formed of H. K. T. Electrolytic Conductivity of Rock Crystal. By E. WARBURG and I?. TEGETMEIER (Ann. Phys. Chem. [a], 35, 455-467).-Jn a, former paper (ibid. [2], 32, 447), the authors showed that a slice of rock crystal cut perpendicularly to the principal axis, and having its ends covered with layers of gold or plumbago, when subjected at a temperature of about 230" to a long-continued E.M.F. of considerable intensity, had its conductivity permanently reduced to a small Rztctioti of its original amoiint. In directions perpendicular to the axis, rock crystal, even at higher temperatures, has little or no conductivity. As the result of their further investigations, the authors have arrived at the conclusions that- (1.) The electrolytic conductivity of rock crystal in bhe direckion of the principal axis is, at high temperatures, about the same as that of ordinary glass.(2.) When a slice cut perpendicularly to the axis is electrolysed, sodium-amalgam being used as the anode, sodium migrates through the slice, its amount being in accordance with Faraday's law, and the weight of the slice remains unchanged. (3.) Even at high temperatures, rock crystal acts as a good insulator with respect to an E.M.F. in a direction perpedicular to the prin- cipal axis. When sodium-amalgam was used as the anode in am experiment lasting for three days, at a temperature of 250°, 88 milligrams of silver were deposited in a silver voltameter in the circuit, and the only substance which could be detected at the cathode was sodium.When potassium was used in the place'of sodium, it was found that after 40 hours the current had sunk to about the hundredth part of its original value, only 2 milligrams of silver were separated, and no potassium could be detected ah the cathode, even by means of the spectroscope. The authors therefore conclude that the conductivity is due to the presence of sodium, in the form of Na,SiO,, which was shown, by an analysis specially made by Baurnann, to be present in the crystal employed in the proportion of 1 part in 2300, so that the crystal might he regarded as a ver,y dilute solution of this salt. The electrolytic character of the conductivity was further COU- firmed by the fact that a cell giving an E.M.F.of from 1.2 to 2 volts could be formed of mercury, a slice of quartz at a temperature of 225", cut perpendicularly to the axis, and sodium-amalgam. According to Clausius's theory of electrolysis, the fact of electrolytic conduction only taking place in the directioa of the principal axie would tend to the inference that in the case of rock crystal not traversed by an electric current, the interchange of atoms between the molecules can only take place, at any rate to a sensible extent, in the direction of the principal axis. A confirmation of this inference is found in the fact first noted by Salm-Horstmar (Ann. Phys. Chem., 120, 334), that the action of hydrofluoric acid on rock crystal is much greater in the direction of the axis than perpendicular to this axis.The authors have themselves h 292 ABSTRACTS OF CHEMICAL PAPERS. made experiments to test the truth of this statement, and the results are in agreement with those of Salm-Horstmar. It would appear from the results obtained in the paper, tllnt the silicate Na2Si03 contained in the crystal must partake of its crystal- line structure. G. W. T. Effect of Occluded Gases on the Thermoelectric Properties of compounds. By J. MONCKMAN (Proc. Ro?y. SOC., 44, 220-236). -When a portion of platinum o r palladium wire is charged with hydrogen by electrolysis, and the wire afterwards heated, a cui-rent passes from ithe protected to the unprotected part. The same occurs with rods of carbon after charging and pressing together, the current passing from the hydrogen to the oxygen.The wires and rods are found to have an increased resistance, that of the oxygen rod being the greatest. The effect disappears after short circuiting. If the wires or rods be charged twice in opposite directions, the effect dis- appears, unless thc second charging is of very short durafion; in fhis case,'% reversal takes place. With carbon rods a t different tem- peratures in contact, reversal occurs a t 250" ; with a thermoelectric couple of carbon and pla,tinum, the thermoelectric line rises below 250', and falls above that temperature. The rate of decrease of resist- ance of carbon diminishes as the temperature rises to 250", but increases afterwards. The rate of evpansion increases as the tem- peratiirc rises to 250", but afterwards decreases.The specific hest increases fairly regularly up to 250°, but above that temperature falls to half. H. K. T. Electrochemical Effects on Magnetising Iron. By T. ANDREWS (Yroc. Roy. SOC., 44, 152-168).-A niagnetised and an nnmagne- tised bar of iron or steel are immersed in different reagents, and the current produced noted. The amount varies considerably, but is large in the case of bromine, salts of copper, and nitric acid. The result is dependent both on the strength of the solution and the degree of magnetisation. With powerful oxidisers, the magnetised bar is generally electropositive, but becomes electronegative with sulphuric acid, dilute hydrocbloric acid, and ferric chloride and chlorine. In the laut-named instances, the effect may be due to the diamagnetic properties of the solutions, or of the gases evolved. With ferric chloride alone, the magnetised bar is electropositive, with chlorine electronegative, with the two together, electronegative until the chlorine is exhausted, when it becomes electropositive.In the same bar, local currents are produced from the more magnetised portions to the less. These may cause the magnetised bar to be acted on to a greater extent than the unniagnetised. In strong nitric acid, a current is produced from the magnetised to the unmagnetised bar. Specific Heat of some Solid Organic Compounds. By H. HESS (Ann. Yhys. Chem. [Z], 35, 410--429).-The author states that, with the exception of some investigations by De Heen (Bull acnd. roy. brlg., 5) and A.Batt'elli (Atti R. Id. Veneto [GI, 3), he has not been able t o find any account of investigations of the specific heats of solid Experiments were also made with graphite rods. H. I(. T.GENERAL -4hTI.l PHYSICAL CHEMISTKY. 93 organic compounds, and he therefore undertook the present inresti- gation with a view especially of determining t>he manner in which the specific heats of solid organic substances depend on temperature. The author gives a number of curves showing the relation between specific heat and temperature in the substances exauiined, tempera- tiires being taken as ordinates, and the corresponding specific heats as abscissae. The curves he fiuds to be sensibly straight lines intersecting the specific heat axis above the zero point, so that the specific heat Name of substance.{ Oxalic acid.. . . Malonic acid . . Succinic acid . . Isosuccinic acid Glutaric acid (solid) (liquid) { Gtlutaric acid Py rot artaric acid nic acid { Dimethylmalo- { Sugar .. .. .. .. Benzoic acid (solid) (liquid) { Benzoic acid Phthalic acid . . {- ~~~ Mean specific heat. Tempera- ture limits. -- 0" to 50" 0 )7 75 0 7 7 94 0 77 50 0 7 7 94 0 7) 110 0 7 7 50 0 Y, 94 0 97 75 0 77 94 0 7, 50 0 7 ) 75 0 )) 94 0 ,) 99.3 0 7 , 50 0 >, 75 0 ,7 94 0 ), 105 0 7 7 50 0 7) 94 0 ,7 75 0 7, 94 0 ,, 150 J > 50 0 ,) 130 0 ), 113 0 ,) 130 0 9 , 50 0 ,, 94 0 7 7 130 0 ,) 122 0 ), 136 0 ., 75 0 7 . 119 0 ,7 150 C. 0 -3359 0 -3575 0 -3728 0 *2832 0 -3131 0.3262 0.2898 0 -3252 0 -3650 0 -3378 0.3500 0 *3ti36 0 *3081 0 *3207 0 *3461 0 * 7503 J 0 *3098 0 *3267 0 -3548 0-3575 0 -3996 I 0 34741 0 -3037 0 * 3197 0.3337 0.3511 0 *25? 1 0 -3118 0 *3319 0 '50'72 I 0-5256j 0 -2559 0 -2862 0 *3099 0 9285 1 Tempemtm coefficient.Cempeiature limits. 50" to 75" 50 77 94 50 ,) 94 94 ,, 110 50 ), 110 50 94 94 7 7 150 50 ,) 150 75 ,, 94 50 )) 75 75 ,7 94 75 y 7 94 50 7 7 94 50 ,, 75 50 7 7 94 99 7 7 130 50 7 7 75 75 ,) 105 50 7 7 94 50 7 7 106 50 77 94 75 7 ) 94 75 ,) 113 94 ,) 130 75 ), 130 50 7 7 94 50 ,) 110 122 ,) 136 94 ,) 110 75 ) ) 119 119 ,) 150 75 ,, 150 6. 0 *000864 0 -00801 0 *000839 0 *000680 0 *000771 0.000705 0 -000805 0 ~000711 0.0007ti2 0 *000512 0 -000716 0 *000600 0 -000504 0 '0913.3'7 0-000864 O~OoO7lO 0 so0676 0 *001027 0 - 000796 0 *000867 0 -000859 0 - 000842 0 *OW789 0 *OW872 0.000862 0 -00124 0.00126 0 -00165 0 -00131 0 -000689 0.000764 0 *000720 Means.b = 0 '000835 6 = 0 *000719 b = 0 *000759 i i 1 6 = 0 400609 b = 0 .000901 b = 0 *000;10 b = 0 '000842 1 b = 0*000859 I 6 = 0 *000841 I b = 0 '00125 b = 0 '00131 6 = 0 '000724 194 ABSTRACTS OF CHEMICAL PAPERS. can be represented by a formula of the form n + bt. The results obtained are given in tabular form (p. 93), c representing the mean spezific heat between tihe temperature limits indicated, and b the temperature coefficient. The values obtained by assuming the true specific heat to be repre- sented by a forniula of the form cc + bt are given in the second table, under the head of "observed specific heat," the column headed " calculated specific heat " being calculated from Kopp's law, that the molecular heat of a body i s equal to the sum of the atomic heats of its constituents.The atomic heats of carbon, hydrogen, and oxygen respectively are taken as 1.8, 2.3, and 4.0. The column headed t gives the temperature a t which the observed and calculated specific heats are equal, and it will be seen that with the exception of oxalic and isosuccinic acids, the different substances obey Kopp's law for some temperature within the limits 3-5" and 50". Kopp's law might be generalised if we could assume the specific heats of carbon, hydrogen, and oxygen to be functions of the tem- perature, but this would not lead to correct general formulae, for Regnault (Compt. rend., 26, 311) and E, Wiedemann ( A m . P h y s . Chem. 15 7, 1) have shown that the specific heats of hydrogen and oxygen are sensibly iudependeut of the temperature, and although H.P. Weber has shown (Ann. Phys. Chem., 147,362) that the specific: heat of carbon increases considerably with the temperature, this increase would not be sufficient to account for the observed increase in the temperature coefflcient. Name of substance. Oxalic acid.. ................. Malonic acid.. ................ Succinic acid ................. Isosuccinic acid ............... Gtlutaric acid (solid) ........... I? yrot art aric acid. ............. Dimethylmalonic acid ......... Sugar.. ...................... Rerizoic acid.. ............... Plithalic acid.. ............... Benzoic acid.. ................ Glutaric acid (liquid) .......... Specific heat. Calculated.0 *2689 0.2942 0 -3136 0 - 3 h 8 0 *3!!40 0 -2820 0 -2602 ¶) - - 0 bserved. 0-2941 + 0-00167t 0'2473 + 0.001445 0.2518 + 0-00152f 0.3067 + 0-00122t 0 -2620 + 0.00180t 0.2677 + 0'00168t 0.2666 + 0'001725 0.2387 + O'OCI173t 0.1946 + 0.002505 0.2016 + 0-00145~ 0 -6580 + 0 -00142t 0.3474 + 0.002625 t. - 15 -1' + 32 -6 + 40.7 + 5-7 f 37 -1 + 36 *4 + 36 *2 + 49 -3 + 35-0 +40*4 - - - The author's results show that there are often considerable differ- ences in the specific heats of different isomeric compounds. Evolution of Gases from Homogeneous Liquids. Ry V. H. VELEY (Proc. B o y . Xoc., 44, 239--240).-The addition of fineiy divided substances is found to increase the rate of evolution of gases from liquids in which they are formed. When the temperature G. W. T.GENERAL AND PHYSICAL CHEMISTRY.95 remains the same, the rake of evolution rises slowly until a maximum is reached, which is maintained for some time. The rate then decreases proportionally to the diminution in mass. The phenomenon repeats itself when the temperature is lowered and then raised t o its former point, and also when the pressure is suddenly increased. The reduction of the pressure to a fraction of an atmosphere produces no permanent effect. The rate of decomposition of formic acid into carbonic anhydride and water is also examined, and is found t o agree with the equation log (T + t ) + log r = log c, where T is the time from the Commencement of the observations, t the interval of time from the moment of commencement up to the moment at which the time required for unit change is mil, r the mass at the end of each observation, and c a constant.The curve of rate of change conforms with the law drld7 = - r2/c, which expresses the rate at which equivalent masses react on one another. Hence it is presumable that equivalent masses react, and that the change is represented by the equations HCOsOH + HCO*OH = HCO-OCHO + H,O and HCO.O*CHO = 2CO + H20, a reaction similar to the production of ethyl formate from formic acid and alcohol. Properties of Matter in the Gaseous and Liquid State under Various Conditions of Temperatura and Pressure. By the late T. ANDREWS (Ann. Chirn. Pl~ys. [GI, 13, 411-432).-Regnault (Xem. Acad. Sci., 26, 680-696) made a series of experiments to determine the tension of a mixture of a gas and a vapour, such as nitrogen or air, and the vapour of water or some more volatile liquid, and came to the conclusion that Dalton’s law of partial pressures may be con- sidered theoretically correct in the case of such mixtures, and that probably this law could be proved to be correct experimentally if the mixture of gas and vapour could be enclosed i n a vessel the interior surface of which was composed of the volatile liquid.He also found that, under pressures varying from + to 2 atmospheres, the com- pressibility of a mixture of ordinary gases, such as air and carbonio anhydride, hydrogen and sulphurous anhydride, was intermediate between that of each gas separately for the same variations of pres- sure (ibid., 258). The results of all experiments which had been carried out up to the time when the author’s investigations were commenced, had been to show that, with one exception, Dalton’s law i s true in all cases for mixtures of gases or vapours, or at any rate in the case of gases and vapours which exert no chemical action on one another.A mixture of the vapours of two mutually soluble liquids, in presence of the two lcquids mixed or dissolved, constitutes, however, an important exception to this law, because of the disturbing influence of the chemical affinity of the liquids. But as, up to this time, no experi- ments had been carried out, to prove the truth of Dalton’s law under pressures greater than 2 atmospheres, the author investigated the change in volume of a mixture of 3 vols. of pure carbonic anhydride and 4-05 1-01s.of nitrogen at temperatures above and below the critical temperature of carbonic anhydride, the pressure employeci vcrying between about 40 and 300 atmospheres. H. K. T.9 8 ABSTRACTS OF OH'EJllCAL PAPERS. From the results, which are given in tabular form, curves are drawn showing the volume of tlie mixture at the various temperatures and pressures. These curves are all very similar, showing no differ- ence in character for temperatures above or below 31". If it be granted t h a t Dalton's and Boyle's laws are true in the case of nitrogen under the pressures employed, the curves showing the change in volume of the carbonic anhydride in the mixture under tlie various conditions of temperature and pressure prove that below 31" t h i s gas tends to occupy the volume corresponding with the liquid state, although the curves are quite different from those of carbonic anhydride alone.It follows, therefore, that Dalton's l a w is no longer applicable in this case, and is only strictly true of a perfect gas. As no liquefaction took place in any of the above experiments, showing that the presence of nitrogen lowered the critical point OF the carbonic anhydride, the author investigated this phenomenon more fully. A mixture of 6.2 vols. of carbonic anhydride and 1 vol. of nitrogen was placed under a pressure of 48.3 atmospheres ; no con- densation occurred until the temperature was lowered to 3.5". As the pressure was increased the volume of the liquid augmented, and after each increase of pressure, the volume continued to augment slowly for some time; for example, under a pressure of 82 atmo- spheres the relative volumes of the gas and liquid were at first 8.5 and 5.8, but, the apparatus having been left for some time, thcb volume of the liquid slowly increased.The pressure having been then raised to 102 atmospheres, the volume of the gas which was a t first 1.7 diminished gradually until only a small globule remained, which finally disappeared entirely, the nitrogen dissolving in the liquid carbonic anhydride. In a second experiment, with the same mixture at a higher and constant temperature, the liquid had a t first its usual concave surface, and as the pressure was increased, the volume of the liquid also augmented without any noticeable change in the appearance of the concave surface ; on further increasing the pressure, the surfaca of separation appeared in section as a fine line, but when the pressure was again increased, i t disappeared entirely, the whole becoming homogeneous.The position in the tube, occupied by the surface of separation, depended on the temperature a t which the observation was made ; a t 14" the liquid filled about, two-thirds of the entire space a t the very moment when the surface of separation was about to disappear, The critical temperature of a mixture of 1 vol. of nitrogen and 3.43 vols. of carbonic anhydride was found to be 14", and the cor- responding pressure 98 atmospheres. Experiments with this mixture showed that at 6.3" no condensation took place until the pl:essure reached 68.7 atmospheres ; the liquid then disappeared under in- creased pressure, but reappeared when the pressure reached 113.2 atmospheres.At 9.Y0, the liquid first appeared when the pressure reached 77.6 atmospheres ; after having disappeared i t was again formed under a pressure of 107.8 atmospheres. At 13*2", the liquid appeared under a pressure of 91.6 atmospheres, disappeared as the pressure was increased, and reappeared when it attained 103.2 atmo- spheres, If the mean of the two pressures for each of the aboveGESERAL AXD PHYSICAL CHEMISTRY. 97 temperatures is taken, the critical pressure a t 6*3", 9*9", 13 2", and 14" is found to be 90.9, 92.7, 944, and 98 atmospheres respectively. I n the course of these experiments, the author found it convwient to employ a tube bent twice at right angles.When the gaseous mixture was compressed below the critical point, the liquid carbonic: anhydride collected in the lower portion of the tube, although part of the liquid was first formed a t the surface of the mercury ; but the whole of the liquid soon collected at the bottom of the tube. In some experiments, the carbonic anhydride liquefied a t temperatures above 20°, and sometimes no condensation took place even a few degrees below this temperature. This phenomenon was found to be owing to the fact that when liquefaction had taken place, if the pressure was diminished so that the mixture could become completely gaseous, the liquid separated into two portions, one rich, the other poor, in carbonic anhydride. The portions of the tube which had been previously occupied by the liquid then contained a large excess of carbonic anhydride, especially when the tube had been previously cooled to -lo", so that almost the whole of the carbonic anhydride had been liquefied. If the pressure was reduced so as to bring the whole of the liquid to the gaseous state, the temperature being a t the same time raised to 26", it was found that the carbonic anhydride could be liquefied by pressure alone (at 26"), provided that, the experiment was performed without loss of time.When, however, the mixture was left for some time in the gaseous state, diffusion gradually took place, and the temperature at which liquefaction wa9 possible decreased accordingly. Diffusion was not complete until after some hours, and then increased pressure caused no liquefaction until the temperature was reduced to 14".This method of separating the gases was employed to shorn the effect of diffusion as follows :-A mixture of carbonic anhydride and nitrogen was kept at 8.5" under a pressure of 46.4 atmospheres until diffnsion was complete ; the volume of the mixture was then 162.2, After liquefying the carbonic anhydride by employing great pressure and lowering the temperature to -12", the temperature was again raised to 8*5", and the pressure brouqht back to 46.4 atmospheres; the volume was then found to be 159.5, showing that a contraction of 2.7 ~01s. had taken place owing to the separation of the mixed gases. A t the end of 1+ hours the volume had increased to 161.5 in conse- quence of partial diffusion. In a second expeiiment at 16", under a pressure of 47.9 atmospheres, the original volume of the mixture was 164.6, but, after liquefaction, only 161.9 when brought back to the initial temperature and pres- sure ; after 1; hours the volume had increased to 164.1.I n a third experiment a t 20", under a pressure of 46.4 atmospheres, the volume decreased from 175.8 to 173.5 after the separation of the gases. These results show that when the two gases d i f i s e into one another under great pressure, an increase in volume ocmrs, and when they are separated the volume is diminished. This change in volume undoubtedly occurs also under ordinary pressures, but the variation would probably be so small that it would be dif€icult to detect experi- mentally. F. S. K.98 ABSTRACTS OF CHEMICAL PAPERS.The Behaviour in Relation to Boyle’s Law of certain Gases at Low Pressures. By F. FUCHS (AN%. Phys. Chem. [‘L], 35, 430- 450).-The author, from the results of a series of experiments on atmospheric air, carbonic and sulphurous anhydrides and hydrogen, arrives a t the following conclusions :- (1.) At ordinary temperatures, Boyle’s law does not represent a limiting state towards which a gas approaches indefinitely with increasing rarefaction, but a t pressures respectively above and below a certain amount, the deviations from Boyle’s law are respectively positive and negative. The limits of pressure within which Boyle’s law holds are indefinitely small, as any finite change in volume will alter the forces betweeii the gaseous molecules. (2.) I n the case of atmospheric air a t the temperature 0”’ a change of sign of this kind takes place at a pressure very slightly below the ordinary atmospheric pressure.If any similar change of sign occurs witb carbonic and sulphurous anhydrides, it must be a t pressures less than any at which the author’s observations were made. (3.) The deviations from Boyle’s law in the case of hydrogen at low pressures are so small that hydrogen under these circumstances may, without, sensible error, be regarded as a perfect gas. G. W. T. Constitution of Solutions. By F. R~DORFF (Ber., 21, 3044- 3050).-Snlts of the composition R2S04 t R“S04 + 6H20 and R,SOd + R,“’(S04)3 + 24H20 are partially decomposed into their constituents when dissolved in water (compare Abstr., 1888, 342).Hydrogen potassium sulphate behaves similarly, but hydrogen ethyl sulphate diffuses unchanged. 3KZCzO4,Fe2(C2O4), + 6H,O ; 3Na2CzOd,Fe,( C204), + 6Hz0 ; 3K,C,Oa,Cr,(C2O4), + 6H20 ; 2(NH4)HC2O4 + H,O ; PU’nHC4H406 + H20, and 2K(SbO)C4H40, + H20, diffuse unchanged, but (NHa)HC,04,C,H204 + 2H,O is partially de- composed into oxalic acid and hydrogen ammonium oxalate. Solutions of potassium chromate, potassium dichromate, and sodium dichromate diffuse unchanged, but the salt (NH4)2Cr04,MgCrOl + 6H20 The following salts :- is partially decomposed when dissolved in water. ‘l’he following salts :-2NaCl,PtCI, + 8H20 ; 2KCl,PtCIz ; 2NH4C1,HgC12 ; Ba(CN),,Pt(CN), + 4H20, and all double cyanides are true molecular compounds, but KCl,Hg( CN), is partially resolved into its constituents when dissolved in water (Zoc.cit.). NaH2POa and Na2HP04 diffuse unchanged: Na,P04, on the con- trary, is partially decomposed. The three sodium salts of citric acid are not decomposed in aqueous solution. F. S. K. Physical Properties of Colloi’d Solutions. By C. L~DEKING (Ann. Phys. Chenz. [2], 35, 552--557).--In a paper with Wiedemann (Abstr., 1885, 1032) it, was shown that the vapour-pressure of aGENERAL AND PHYSICAL CHEJIISTRY. 99 40 per cent. aqueous solution of gelatin was less a t a temperature of 40" than that of pure water. According to Guthrie (this Journal, 1877, i, 36), a 40 per cent. solut'ion of gnm boiled at 98", and a 45 per cent. solution of gelatin at 97.5": results which were in contra- diction to those above mentioned.With a view of discovering the reason of the discrepancy, the author made experiments on solutions of gum arabic, gum trngacan th, dextrin, starch, and agar-agar. He finds that a 40 per cent. solution of gum arabic boils at IOO", but carbonic anhydride begins to be given off a t a temperature of about go", and a t a somewhat higher temperature gives the appearance of boiling to the solution. The other solutions also boiled at loo", although in the case of gelatin boiling began with the thermometer a t 98", which, however, the author attributes to the liquid not rapidly assuming the same temperature throughout, owing to its viscidity preventing the forma- tion of convection currents, This opinion was based on the fact that the thermometer did not remain at 98", butpadually rose to 99.8", where it remained constant.The author found that the addition of the colloid in every case slightly lowered the vapour-pressure, and, as he points out, the presence of a solid i n solution could not possibly increase the vapour-pressure. For example, if the steam given off at 98" from a gelatin solution had a pressure of 760 mm., i t would necessarily re- condense to water and mix again with the solution. When solutions of gum or gelatin are cooled considerably below zero, the author finds that they do not solidify as a whole, as stated by Guthrie, but ice crystals gradually separate out. He finds that gelatin has a strong condensing action on the water of solution. G. W. T. Precipitation of Colloid Substances by Salts. By 0.NASSE (Pjiiyer's Archiv, 41, 504--514).-A11 prote'ids except peptone can be precipitat!ed by saturating a neutral solution with ammonium sul- phate, some more easily than others, for instance, globulins more easily than albumins. Other salts bave the same power, but none act so readily as ammonium sulphate. This property, however, is not characteristic of proteids : soaps, gelatin, and certain fioluble carbo- hydrates (glycogen, amidulin, inulin, &c.>, are similarly precipitated ; it in fact seems to be a property common to colloid substances. The question arises, on what does the difference in the concentra- tion of the salt necessary to produce precipitation depend ? Is the action of the salt simply due to a struggle of the molecule of proteid, gelatin, &c., with that of the salt for water, and t h a t the pre- cipitation of the colloid substance occurs as soon as its water-attract- ing power is exceeded by that of the salt? In order to determine whether this is the case, one m u d ascertain the amount of two or more different salts necessary to precipitat'e the same aniount of one colloid substance, the necessary concentration of the salt solutions corresponding with a : b : c, &c. The same ques- tion is then invebtigated €or another colloid substance, and the ratio100 ABSTRACTS OF CHEMICAL PAPERS.a' : b' : c', &c., found. for water, a : b : c, &c., will be found = a' : b' : c', &c. Tf hhen we have only to deal with attraction The following table illustrates the results obtained :- Collo'id substances.Gplatin ......... The solution contained in 100 C.C. the following amounts of salt w18cn precipitation began. L--v---J a. 6 . Ammonium Magnesium sulphate. sulphat e. a : b. 12.4 14.8 0.84 White of egg.. .... 20.2 19.6 1-03 9 3 ...... 18.5 19.3 0.95 Serum prote'rds .... 17.4 18.5 0.94 Albumose. ........ 12.7 13.6 0.9:3 ,, ......... 14.9 17.6 0.85 Amidulin. ........ 20.9 10.5 1-99 Glycogen-dextrin . . 44.7 23.7 1-99 The differences of the numbers in the last column show that water-attracting power is not the only influence at work, but some other relation must exist between the colloid and the salt. Still it is possible that it may explain some of the precipitations, especially that of gelatin. Gelatin loses many of its characteristic properties after the prolonged heating of its solutions; it, for instance, no longer gelatinises on cooling, and its water-holding power is greatly in- creased, yet, the ratio a : b = 0.84 remains constant for the gelatin in all the different stages of this change.With regard to the proteids, in which such wide differences occur, it is thought probable that the explanation lies in the fact that loose compounds with the salts are formed. The paper concludes with some remarks on the influence of tern- perature in determining precipitation by salts. New Formula for Calculating the Molecular Volumes of Chemical Compounds at the Boiling Points. By J. A. GROSHANS (Rac. l'rav. Chim., 7, 220--225).-The molecular volume of a sut)stance, CPH4Or, at the boiling point may be represented by t7, = a + 1O(p + q ) - 7.28 B for a fatty compound, or by the same expression miiius 15 for an aromatic compound, c1 being the number of' O.C.equal to the molecular weight of the compound, and B = p + q + Y. Both these formulte obey Kopp's rules, that homologous compounds differing in their composition by CH, should differ i u their molecular volumes by 22, and that a fatty compound should have approximately the same volume as an aromatic compound which differs in its formula by C2 - Hq. With hydrocarbons, since 7 = 0, the formula may also be written (us - a)/B = 2-72 for fatty compounds, or (u, - a -+- 15)/B = 2-72 for aromatic, both of which are fonnd t o agree well with experiment. For halogen-deiaivatives, an addition of 15 must be made for each atom of halogen oontained.H. C. W. D. H.ISORGANIC CHEMISTRY. 101 Molecular Lowering of the Freezing Point of Benzene by Phenols. By E. PAT ERN^ (Ber., 21, 3178-3180).--The author made a, number of experiments to ascertain whether the fact that certain substances containing the hydroxyl-group produce an abnormal lower- ing of the freezing point of benzene WRS true of all substances, and whether this abnormal behaviour was sufficient proof of the pi*esence of the hydroxyl-group (compare Raoult, Abstr., 1884, 959). The re- sults showed that although phenol behaves in an abnormal manner, the following compounds : ethyl phenol, acetylphenol, two isomeric nitrophenols, tribromophenol, picric acid, paracresol, methyl salicylate, thymol, nitrothymol, nitrosothymol, a-naphthol, /-3-naphthol, and benzylphenol, all produce the normal lowering of the freezing point of benzene and of acetic acid, either in dilute or moderately concentrated solutions, the variations caused Ey change in concentration of course being taken into consideration.The molecular weight of water determined by Raoult's method in acetic acid solution was found to be 18 (compare Rxonlt, lor. cit.), but the author points out that tlhis result is not by any means conclusive, as, even if the molecules were originally more complex, they would be simpli6ed by the act of solution. Hentschel's experiments with acetic acid (Zeit. phys. Chenz., 2, 308) seem to point to an opposite conclusion, but in this case the freezing point of the benzene solution was considerably below that of acetic acid.The fact that the molecular weight of water is found to be 36 when the freezing point of the solution lies below 0" shows that the temperature a t which the mixture freezes is a most important factor in the case. F. S. K.89General and P h y s i c a l Chemistry.DEWARformedby theSpectrum of Magnesium. By G. D. LIVEING and J.(Proc. &t~. ,!!oc., 44, 241-252) -When an electric arc isbetween magnesium electrodes,' most of the lines producedspark discharge are observed. The larger number of lines with anarc discharge may be due not to lowness of temperature, but to thegreater mass of incandwcent matter, and to a wider range of tem-perature a t different portions of the discharge, recombinations occur-ing a t its edge.The electiic discharge itself may also give rise tovibrations distinct from those due to heat. The seven bands in thegreen are due to the oxide, as they are only prodiiced in the presenceof oxygen or its compounds. If a piece of hurnt magnesium wire beheated in the oxphydrogen flame, the spectrum of magnesium isproduced, the met:illic lines appearing if the hydrogen is in excess.The triplet near M which is produced when magnesium is burnt, isfound t o be produced in the arc befween rnagnesium electrodes and inmany other cahes when oxygen is present, but not in an atmosphereof nitrogeu o r hydrogen, hence it is due to the oxide. Vacuous tube8are found to be very untrustworthy for the ultra-violet spectra, as thewater-spectrum and lines of nitrogen are nearly always present, andthe spectra sometinres vary unaccountably.A pump is described inwhich rubber connections and free contact of the mercury with airare avoided. H. K. T.Ultra-violet Spectra of Nickel and Cobalt. By G. D. LIVEING andJ. DEWAR (Proc. Rot/. Xoc., 43,43O).-A comparison is made betweena plane Rowland's grating with a goniometer and the concave grating(20 feet focal length) used by Bell. The results agree very closely,the concave grating gives more light, a i d is more suitable for com-plicated spectra, as the overlapping spectra of different orders are notall in focus at once.The coinci-dences are not greater than the theory of chances would allow, auddo not correspond with their chemical relationship. H.R. T.Ultra-violet lines of cobalt and nickel are compared.Two-fluid Cells. By C. R. A . WRIGHT and C. THOMPSON (Proc.Roy. Soc., 43, 489-493).-Cells are set up consisting of platinumplates in acid and alkaline solutions, with the further addition eitherof oxidising agents to the acid solution or of reducing agents to thealkaline solution. Currents are produced, in the first case withevolution of oxygen from the alkaline solution, in the second withevolution of hydrogen from the acid solution. The quantity of gasevolved was equivalent to the current. The acid and alkali were sul-phuric acid and potassium hydroxide respectively ; the oxidisingagents being potassium permanganate, dichromatc, and ferricyanide,ferric chloride, and solutions of chlorine and bromine and the reducingVOL. LYI.790 ABSTRACTS OF OHEMTCAL PAPERS.agents sodium hyposulphite, pyrogallol, cuprous chloride, and ferroussulphate and ammonium chloride in nmmouiacal solution. Hydrogenwas not evolved with sodium sulphite or hypophosphite, potassiumferrocyanide, or manganous hydroxide in ammoniacal ammoniumchloride, nor was oxygen with barium dioxide and sulphuric acid, o rwith hydrochloric acid and iodine. On the other hand, an aerationplate of platinum sponge gave a current four times as great. Platesof oxidisable metals in alkaline solution could be substituted for thereducing substance, hydrogen being evolved in the acid solution ; thiswas particularly the case when potassium cyanide was used. Gold,silver, and palladium in cyanide solution gave hydrogen, but platinumand iron were ineffective.When both oxidising and reducing agentsare used, comparatively powerful currents are produced.Effect of Chlorine on the Electromotive Force of a VoltaicCouple. By G. GORE (Proc. Roy. Soc., 44, 151--152).-1f theelectromotive force of a small magnesium-platinum couple in distilledwater is balanced through a galvanometer and dilute chlorine-wateris gradually added, the electromotive force does not alter a t first, butafter a cert,aiii point has been reached (1 in 17,000 millions) it beginsto increase rapidly. I n t h i s way, the one ten-thousand-millionth ofa grain of chlorine in 0.1 C.U. of water can be detected. Otherelectrolytes give the same reaction, b u t require a larger quantity ofdissolved substance. H.K. T.H. K. T.Development of Voltaic Electricity by Atmospheric Oxida-tion. By C. R. A. WRIGHT and C. THOMPSON (PYOC. RUy. Xoc., 44,182- 2OO).-The electromotive force of cells in which aeration platesare used, falls off very rapidly if the current density exceeds a certainamount. When oxidisable liquids are used, it is difficult to determine,as it appears to vary with the nature of the aeration plate, and alsowith the incorrodible plate in the liquid to be oxidised. For determin-ing these electromotive forces, an arrangement is used in which t5easration plate can be kept undisturbed, and in which the oxidisablesubstances are protected from alterations of temperature, impuritiesfrom the air, &c.After a few hours or days, the currents becomeconstant. In these cells, variation of the asration plate produces adifference in the electromotive force independent of the oxidisableplate used ; similarly the effect of varying the metal is independent ofthe asration plate. The nature and strength of the liquid affects theresults to some extent. The electro-motive force actually generated falls very considerably short of thatcorresponding with the chemical changa, especially when the currentdensity is large. With silver as the oxidisable plate, however, theelectromotive force is higher than the theoretical, this being due tothe high negative value of the thermovoltaic constant of silver incontact with sulphurib acid. When oxygen was substituted for airover the aGration plate, a slight rise in the electromotive force wasobserved.With aeration plates immersed in coal-gas or hydrogen,and opposed to a platinum plate in alkaline permanganate or insulph uric acid and potassium dichromate, very weak and variableTables of results are givenGESERAL AND PHYSICAL CHEMISTRY. 9 1currents were observed.aGration plates in hydrogen and air respectively.The same was the case with cells formed ofH. K. T.Electrolytic Conductivity of Rock Crystal. By E. WARBURGand I?. TEGETMEIER (Ann. Phys. Chem. [a], 35, 455-467).-Jn a,former paper (ibid. [2], 32, 447), the authors showed that a slice ofrock crystal cut perpendicularly to the principal axis, and having itsends covered with layers of gold or plumbago, when subjected at atemperature of about 230" to a long-continued E.M.F.of considerableintensity, had its conductivity permanently reduced to a small Rztctiotiof its original amoiint. In directions perpendicular to the axis, rockcrystal, even at higher temperatures, has little or no conductivity.As the result of their further investigations, the authors havearrived at the conclusions that-(1.) The electrolytic conductivity of rock crystal in bhe direckion ofthe principal axis is, at high temperatures, about the same as that ofordinary glass.(2.) When a slice cut perpendicularly to the axis is electrolysed,sodium-amalgam being used as the anode, sodium migrates throughthe slice, its amount being in accordance with Faraday's law, and theweight of the slice remains unchanged.(3.) Even at high temperatures, rock crystal acts as a good insulatorwith respect to an E.M.F. in a direction perpedicular to the prin-cipal axis.When sodium-amalgam was used as the anode in am experimentlasting for three days, at a temperature of 250°, 88 milligrams of silverwere deposited in a silver voltameter in the circuit, and the onlysubstance which could be detected at the cathode was sodium.When potassium was used in the place'of sodium, it was found thatafter 40 hours the current had sunk to about the hundredth part ofits original value, only 2 milligrams of silver were separated, and nopotassium could be detected ah the cathode, even by means of thespectroscope.The authors therefore conclude that the conductivityis due to the presence of sodium, in the form of Na,SiO,, which wasshown, by an analysis specially made by Baurnann, to be present inthe crystal employed in the proportion of 1 part in 2300, so that thecrystal might he regarded as a ver,y dilute solution of this salt.The electrolytic character of the conductivity was further COU-firmed by the fact that a cell giving an E.M.F.of from 1.2 to 2 voltscould be formed of mercury, a slice of quartz at a temperature of225", cut perpendicularly to the axis, and sodium-amalgam.According to Clausius's theory of electrolysis, the fact of electrolyticconduction only taking place in the directioa of the principal axiewould tend to the inference that in the case of rock crystal nottraversed by an electric current, the interchange of atoms betweenthe molecules can only take place, at any rate to a sensible extent, inthe direction of the principal axis.A confirmation of this inference is found in the fact first noted bySalm-Horstmar (Ann.Phys. Chem., 120, 334), that the action ofhydrofluoric acid on rock crystal is much greater in the direction ofthe axis than perpendicular to this axis. The authors have themselvesh 92 ABSTRACTS OF CHEMICAL PAPERS.made experiments to test the truth of this statement, and the resultsare in agreement with those of Salm-Horstmar.It would appear from the results obtained in the paper, tllnt thesilicate Na2Si03 contained in the crystal must partake of its crystal-line structure.G. W. T.Effect of Occluded Gases on the Thermoelectric Propertiesof compounds. By J. MONCKMAN (Proc. Ro?y. SOC., 44, 220-236).-When a portion of platinum o r palladium wire is charged withhydrogen by electrolysis, and the wire afterwards heated, a cui-rentpasses from ithe protected to the unprotected part. The same occurswith rods of carbon after charging and pressing together, the currentpassing from the hydrogen to the oxygen. The wires and rods arefound to have an increased resistance, that of the oxygen rod beingthe greatest. The effect disappears after short circuiting. If thewires or rods be charged twice in opposite directions, the effect dis-appears, unless thc second charging is of very short durafion; infhis case,'% reversal takes place.With carbon rods a t different tem-peratures in contact, reversal occurs a t 250" ; with a thermoelectriccouple of carbon and pla,tinum, the thermoelectric line rises below250', and falls above that temperature. The rate of decrease of resist-ance of carbon diminishes as the temperature rises to 250", butincreases afterwards. The rate of evpansion increases as the tem-peratiirc rises to 250", but afterwards decreases. The specific hestincreases fairly regularly up to 250°, but above that temperature fallsto half.H. K. T.Electrochemical Effects on Magnetising Iron. By T. ANDREWS(Yroc. Roy. SOC., 44, 152-168).-A niagnetised and an nnmagne-tised bar of iron or steel are immersed in different reagents, and thecurrent produced noted.The amount varies considerably, but islarge in the case of bromine, salts of copper, and nitric acid. Theresult is dependent both on the strength of the solution and the degreeof magnetisation. With powerful oxidisers, the magnetised bar isgenerally electropositive, but becomes electronegative with sulphuricacid, dilute hydrocbloric acid, and ferric chloride and chlorine. In thelaut-named instances, the effect may be due to the diamagnetic propertiesof the solutions, or of the gases evolved. With ferric chloride alone,the magnetised bar is electropositive, with chlorine electronegative,with the two together, electronegative until the chlorine is exhausted,when it becomes electropositive. In the same bar, local currents areproduced from the more magnetised portions to the less.These maycause the magnetised bar to be acted on to a greater extent than theunniagnetised. In strong nitric acid, a current is produced from themagnetised to the unmagnetised bar.Specific Heat of some Solid Organic Compounds. By H.HESS (Ann. Yhys. Chem. [Z], 35, 410--429).-The author states that,with the exception of some investigations by De Heen (Bull acnd. roy.brlg., 5) and A. Batt'elli (Atti R. Id. Veneto [GI, 3), he has not beenable t o find any account of investigations of the specific heats of solidExperiments were also made with graphite rods.H. I(. TGENERAL -4hTI.l PHYSICAL CHEMISTKY. 93organic compounds, and he therefore undertook the present inresti-gation with a view especially of determining t>he manner in which thespecific heats of solid organic substances depend on temperature.The author gives a number of curves showing the relation betweenspecific heat and temperature in the substances exauiined, tempera-tiires being taken as ordinates, and the corresponding specific heats asabscissae.The curves he fiuds to be sensibly straight lines intersectingthe specific heat axis above the zero point, so that the specific heatName ofsubstance.{ Oxalic acid.. . .Malonic acid . .Succinic acid . .Isosuccinic acidGlutaric acid(solid)(liquid) { Gtlutaric acidPy rot artaricacidnic acid { Dimethylmalo-{ Sugar .. .. .. ..Benzoic acid(solid)(liquid) { Benzoic acidPhthalic acid . . {-~~~Mean specific heat.Tempera-ture limits.--0" to 50"0 )7 750 7 7 940 77 500 7 7 940 7) 1100 7 7 500 Y, 940 97 750 77 940 7, 500 7 ) 750 )) 940 ,) 99.30 7 , 500 >, 750 ,7 940 ), 1050 7 7 500 7) 940 ,7 750 7, 940 ,, 150J > 500 ,) 1300 ), 1130 ,) 1300 9 , 500 ,, 940 7 7 1300 ,) 1220 ), 1360 ., 750 7 . 1190 ,7 150C.0 -33590 -35750 -37280 *28320 -31310.32620.28980 -32520 -36500 -33780.35000 *3ti360 *30810 *32070 *34610 * 7503 J0 *30980 *32670 -35480-35750 -3996 I0 347410 -30370 * 31970.33370.35110 *25? 10 -31180 *33190 '50'72 I0-5256j0 -25590 -28620 *30990 9285 1Tempemtm coefficient.Cempeiaturelimits.50" to 75"50 77 9450 ,) 9494 ,, 11050 ), 11050 9494 7 7 15050 ,) 15075 ,, 9450 )) 7575 ,7 9475 y 7 9450 7 7 9450 ,, 7550 7 7 9499 7 7 13050 7 7 7575 ,) 10550 7 7 9450 7 7 10650 77 9475 7 ) 9475 ,) 11394 ,) 13075 ), 13050 7 7 9450 ,) 110122 ,) 13694 ,) 11075 ) ) 119119 ,) 15075 ,, 1506.0 *0008640 -008010 *0008390 *0006800 *0007710.0007050 -0008050 ~0007110.0007ti20 *0005120 -0007160 *0006000 -0005040 '0913.3'70-000864O~OoO7lO0 so06760 *0010270 - 0007960 *0008670 -0008590 - 0008420 *OW7890 *OW8720.0008620 -001240.001260 -001650 -001310 -0006890.0007640 *000720Means.b = 0 '0008356 = 0 *000719b = 0 *000759ii1 6 = 0 400609b = 0 .000901b = 0 *000;10b = 0 '000842 1b = 0*000859I 6 = 0 *000841 Ib = 0 '00125b = 0 '001316 = 0 '000724 94 ABSTRACTS OF CHEMICAL PAPERS.can be represented by a formula of the form n + bt.The resultsobtained are given in tabular form (p. 93), c representing the meanspezific heat between tihe temperature limits indicated, and b thetemperature coefficient.The values obtained by assuming the true specific heat to be repre-sented by a forniula of the form cc + bt are given in the second table,under the head of "observed specific heat," the column headed" calculated specific heat " being calculated from Kopp's law, that themolecular heat of a body i s equal to the sum of the atomic heats ofits constituents. The atomic heats of carbon, hydrogen, and oxygenrespectively are taken as 1.8, 2.3, and 4.0.The column headed tgives the temperature a t which the observed and calculated specificheats are equal, and it will be seen that with the exception of oxalicand isosuccinic acids, the different substances obey Kopp's law forsome temperature within the limits 3-5" and 50".Kopp's law might be generalised if we could assume the specificheats of carbon, hydrogen, and oxygen to be functions of the tem-perature, but this would not lead to correct general formulae, forRegnault (Compt. rend., 26, 311) and E, Wiedemann ( A m . P h y s .Chem. 15 7, 1) have shown that the specific heats of hydrogen andoxygen are sensibly iudependeut of the temperature, and althoughH. P. Weber has shown (Ann. Phys. Chem., 147,362) that the specific:heat of carbon increases considerably with the temperature, thisincrease would not be sufficient to account for the observed increase inthe temperature coefflcient.Name of substance.Oxalic acid...................Malonic acid.. ................Succinic acid .................Isosuccinic acid ...............Gtlutaric acid (solid) ...........I? yrot art aric acid. .............Dimethylmalonic acid .........Sugar.. ......................Rerizoic acid.. ...............Plithalic acid.. ...............Benzoic acid.. ................ Glutaric acid (liquid) ..........Specific heat.Calculated.0 *26890.29420 -31360 - 3 h 80 *3!!400 -28200 -2602¶)--0 bserved.0-2941 + 0-00167t0'2473 + 0.0014450.2518 + 0-00152f0.3067 + 0-00122t0 -2620 + 0.00180t0.2677 + 0'00168t0.2666 + 0'0017250.2387 + O'OCI173t0.1946 + 0.0025050.2016 + 0-00145~0 -6580 + 0 -00142t0.3474 + 0.002625t.- 15 -1' + 32 -6 + 40.7 + 5-7f 37 -1 + 36 *4 + 36 *2 + 49 -3 + 35-0+40*4 - - -The author's results show that there are often considerable differ-ences in the specific heats of different isomeric compounds.Evolution of Gases from Homogeneous Liquids.Ry V. H.VELEY (Proc. B o y . Xoc., 44, 239--240).-The addition of fineiydivided substances is found to increase the rate of evolution of gasesfrom liquids in which they are formed. When the temperatureG. W. TGENERAL AND PHYSICAL CHEMISTRY. 95remains the same, the rake of evolution rises slowly until a maximumis reached, which is maintained for some time.The rate thendecreases proportionally to the diminution in mass. The phenomenonrepeats itself when the temperature is lowered and then raised t o itsformer point, and also when the pressure is suddenly increased. Thereduction of the pressure to a fraction of an atmosphere produces nopermanent effect. The rate of decomposition of formic acid intocarbonic anhydride and water is also examined, and is found t o agreewith the equation log (T + t ) + log r = log c, where T is the timefrom the Commencement of the observations, t the interval of timefrom the moment of commencement up to the moment at which thetime required for unit change is mil, r the mass at the end of eachobservation, and c a constant.The curve of rate of change conformswith the law drld7 = - r2/c, which expresses the rate at whichequivalent masses react on one another. Hence it is presumablethat equivalent masses react, and that the change is represented bythe equations HCOsOH + HCO*OH = HCO-OCHO + H,O andHCO.O*CHO = 2CO + H20, a reaction similar to the production ofethyl formate from formic acid and alcohol.Properties of Matter in the Gaseous and Liquid State underVarious Conditions of Temperatura and Pressure. By the lateT. ANDREWS (Ann. Chirn. Pl~ys. [GI, 13, 411-432).-Regnault (Xem.Acad. Sci., 26, 680-696) made a series of experiments to determinethe tension of a mixture of a gas and a vapour, such as nitrogen orair, and the vapour of water or some more volatile liquid, and cameto the conclusion that Dalton’s law of partial pressures may be con-sidered theoretically correct in the case of such mixtures, and thatprobably this law could be proved to be correct experimentally if themixture of gas and vapour could be enclosed i n a vessel the interiorsurface of which was composed of the volatile liquid.He also foundthat, under pressures varying from + to 2 atmospheres, the com-pressibility of a mixture of ordinary gases, such as air and carbonioanhydride, hydrogen and sulphurous anhydride, was intermediatebetween that of each gas separately for the same variations of pres-sure (ibid., 258).The results of all experiments which had been carried out up tothe time when the author’s investigations were commenced, had beento show that, with one exception, Dalton’s law i s true in all cases formixtures of gases or vapours, or at any rate in the case of gases andvapours which exert no chemical action on one another.A mixtureof the vapours of two mutually soluble liquids, in presence of thetwo lcquids mixed or dissolved, constitutes, however, an importantexception to this law, because of the disturbing influence of thechemical affinity of the liquids. But as, up to this time, no experi-ments had been carried out, to prove the truth of Dalton’s law underpressures greater than 2 atmospheres, the author investigated thechange in volume of a mixture of 3 vols. of pure carbonic anhydrideand 4-05 1-01s. of nitrogen at temperatures above and below thecritical temperature of carbonic anhydride, the pressure employecivcrying between about 40 and 300 atmospheres.H. K.T9 8 ABSTRACTS OF OH'EJllCAL PAPERS.From the results, which are given in tabular form, curves aredrawn showing the volume of tlie mixture at the various temperaturesand pressures. These curves are all very similar, showing no differ-ence in character for temperatures above or below 31". If it begranted t h a t Dalton's and Boyle's laws are true in the case ofnitrogen under the pressures employed, the curves showing thechange in volume of the carbonic anhydride in the mixture under tlievarious conditions of temperature and pressure prove that below 31"t h i s gas tends to occupy the volume corresponding with the liquidstate, although the curves are quite different from those of carbonicanhydride alone.It follows, therefore, that Dalton's l a w is no longerapplicable in this case, and is only strictly true of a perfect gas.As no liquefaction took place in any of the above experiments,showing that the presence of nitrogen lowered the critical point OF thecarbonic anhydride, the author investigated this phenomenon morefully. A mixture of 6.2 vols. of carbonic anhydride and 1 vol. ofnitrogen was placed under a pressure of 48.3 atmospheres ; no con-densation occurred until the temperature was lowered to 3.5". Asthe pressure was increased the volume of the liquid augmented, andafter each increase of pressure, the volume continued to augmentslowly for some time; for example, under a pressure of 82 atmo-spheres the relative volumes of the gas and liquid were at first 8.5and 5.8, but, the apparatus having been left for some time, thcbvolume of the liquid slowly increased.The pressure having beenthen raised to 102 atmospheres, the volume of the gas which was a tfirst 1.7 diminished gradually until only a small globule remained,which finally disappeared entirely, the nitrogen dissolving in theliquid carbonic anhydride. In a second experiment, with the samemixture at a higher and constant temperature, the liquid had a t firstits usual concave surface, and as the pressure was increased, thevolume of the liquid also augmented without any noticeable changein the appearance of the concave surface ; on further increasing thepressure, the surfaca of separation appeared in section as a fine line,but when the pressure was again increased, i t disappeared entirely,the whole becoming homogeneous.The position in the tube, occupiedby the surface of separation, depended on the temperature a t whichthe observation was made ; a t 14" the liquid filled about, two-thirds ofthe entire space a t the very moment when the surface of separationwas about to disappear,The critical temperature of a mixture of 1 vol. of nitrogen and3.43 vols. of carbonic anhydride was found to be 14", and the cor-responding pressure 98 atmospheres. Experiments with this mixtureshowed that at 6.3" no condensation took place until the pl:essurereached 68.7 atmospheres ; the liquid then disappeared under in-creased pressure, but reappeared when the pressure reached 113.2atmospheres.At 9.Y0, the liquid first appeared when the pressurereached 77.6 atmospheres ; after having disappeared i t was againformed under a pressure of 107.8 atmospheres. At 13*2", the liquidappeared under a pressure of 91.6 atmospheres, disappeared as thepressure was increased, and reappeared when it attained 103.2 atmo-spheres, If the mean of the two pressures for each of the abovGESERAL AXD PHYSICAL CHEMISTRY. 97temperatures is taken, the critical pressure a t 6*3", 9*9", 13 2", and14" is found to be 90.9, 92.7, 944, and 98 atmospheres respectively.I n the course of these experiments, the author found it convwientto employ a tube bent twice at right angles.When the gaseousmixture was compressed below the critical point, the liquid carbonic:anhydride collected in the lower portion of the tube, although part ofthe liquid was first formed a t the surface of the mercury ; but thewhole of the liquid soon collected at the bottom of the tube. Insome experiments, the carbonic anhydride liquefied a t temperaturesabove 20°, and sometimes no condensation took place even a fewdegrees below this temperature. This phenomenon was found to beowing to the fact that when liquefaction had taken place, if thepressure was diminished so that the mixture could become completelygaseous, the liquid separated into two portions, one rich, the otherpoor, in carbonic anhydride. The portions of the tube which hadbeen previously occupied by the liquid then contained a large excessof carbonic anhydride, especially when the tube had been previouslycooled to -lo", so that almost the whole of the carbonic anhydridehad been liquefied. If the pressure was reduced so as to bring thewhole of the liquid to the gaseous state, the temperature being a t thesame time raised to 26", it was found that the carbonic anhydridecould be liquefied by pressure alone (at 26"), provided that, theexperiment was performed without loss of time.When, however, themixture was left for some time in the gaseous state, diffusion graduallytook place, and the temperature at which liquefaction wa9 possibledecreased accordingly. Diffusion was not complete until after somehours, and then increased pressure caused no liquefaction until thetemperature was reduced to 14".This method of separating the gases was employed to shorn theeffect of diffusion as follows :-A mixture of carbonic anhydride andnitrogen was kept at 8.5" under a pressure of 46.4 atmospheres untildiffnsion was complete ; the volume of the mixture was then 162.2,After liquefying the carbonic anhydride by employing great pressureand lowering the temperature to -12", the temperature was againraised to 8*5", and the pressure brouqht back to 46.4 atmospheres;the volume was then found to be 159.5, showing that a contraction of2.7 ~01s.had taken place owing to the separation of the mixed gases.A t the end of 1+ hours the volume had increased to 161.5 in conse-quence of partial diffusion.In a second expeiiment at 16", under a pressure of 47.9 atmospheres,the original volume of the mixture was 164.6, but, after liquefaction,only 161.9 when brought back to the initial temperature and pres-sure ; after 1; hours the volume had increased to 164.1.I n a thirdexperiment a t 20", under a pressure of 46.4 atmospheres, the volumedecreased from 175.8 to 173.5 after the separation of the gases.These results show that when the two gases d i f i s e into oneanother under great pressure, an increase in volume ocmrs, and whenthey are separated the volume is diminished. This change in volumeundoubtedly occurs also under ordinary pressures, but the variationwould probably be so small that it would be dif€icult to detect experi-mentally. F.S. K98 ABSTRACTS OF CHEMICAL PAPERS.The Behaviour in Relation to Boyle’s Law of certain Gasesat Low Pressures. By F. FUCHS (AN%. Phys. Chem. [‘L], 35, 430-450).-The author, from the results of a series of experiments onatmospheric air, carbonic and sulphurous anhydrides and hydrogen,arrives a t the following conclusions :-(1.) At ordinary temperatures, Boyle’s law does not represent alimiting state towards which a gas approaches indefinitely withincreasing rarefaction, but a t pressures respectively above and belowa certain amount, the deviations from Boyle’s law are respectivelypositive and negative. The limits of pressure within which Boyle’slaw holds are indefinitely small, as any finite change in volume willalter the forces betweeii the gaseous molecules.(2.) I n the case of atmospheric air a t the temperature 0”’ a changeof sign of this kind takes place at a pressure very slightly below theordinary atmospheric pressure.If any similar change of sign occurswitb carbonic and sulphurous anhydrides, it must be a t pressures lessthan any at which the author’s observations were made.(3.) The deviations from Boyle’s law in the case of hydrogen atlow pressures are so small that hydrogen under these circumstancesmay, without, sensible error, be regarded as a perfect gas.G. W. T.Constitution of Solutions. By F. R~DORFF (Ber., 21, 3044-3050).-Snlts of the composition R2S04 t R“S04 + 6H20 andR,SOd + R,“’(S04)3 + 24H20 are partially decomposed into theirconstituents when dissolved in water (compare Abstr., 1888, 342).Hydrogen potassium sulphate behaves similarly, but hydrogen ethylsulphate diffuses unchanged.3KZCzO4,Fe2(C2O4), + 6H,O ; 3Na2CzOd,Fe,( C204), + 6Hz0 ;3K,C,Oa,Cr,(C2O4), + 6H20 ; 2(NH4)HC2O4 + H,O ;PU’nHC4H406 + H20, and 2K(SbO)C4H40, + H20,diffuse unchanged, but (NHa)HC,04,C,H204 + 2H,O is partially de-composed into oxalic acid and hydrogen ammonium oxalate.Solutions of potassium chromate, potassium dichromate, andsodium dichromate diffuse unchanged, but the salt(NH4)2Cr04,MgCrOl + 6H20The following salts :-is partially decomposed when dissolved in water.‘l’he following salts :-2NaCl,PtCI, + 8H20 ; 2KCl,PtCIz ;2NH4C1,HgC12 ; Ba(CN),,Pt(CN), + 4H20, and all double cyanidesare true molecular compounds, but KCl,Hg( CN), is partiallyresolved into its constituents when dissolved in water (Zoc.cit.).NaH2POa and Na2HP04 diffuse unchanged: Na,P04, on the con-trary, is partially decomposed. The three sodium salts of citric acidare not decomposed in aqueous solution. F. S. K.Physical Properties of Colloi’d Solutions. By C. L~DEKING(Ann. Phys. Chenz. [2], 35, 552--557).--In a paper with Wiedemann(Abstr., 1885, 1032) it, was shown that the vapour-pressure of GENERAL AND PHYSICAL CHEJIISTRY. 9940 per cent. aqueous solution of gelatin was less a t a temperature of40" than that of pure water. According to Guthrie (this Journal,1877, i, 36), a 40 per cent. solut'ion of gnm boiled at 98", and a 45 percent.solution of gelatin at 97.5": results which were in contra-diction to those above mentioned.With a view of discovering the reason of the discrepancy, theauthor made experiments on solutions of gum arabic, gum trngacan th,dextrin, starch, and agar-agar.He finds that a 40 per cent. solution of gum arabic boils at IOO",but carbonic anhydride begins to be given off a t a temperature ofabout go", and a t a somewhat higher temperature gives the appearanceof boiling to the solution.The other solutions also boiled at loo", although in the case ofgelatin boiling began with the thermometer a t 98", which, however,the author attributes to the liquid not rapidly assuming the sametemperature throughout, owing to its viscidity preventing the forma-tion of convection currents, This opinion was based on the fact thatthe thermometer did not remain at 98", butpadually rose to 99.8",where it remained constant.The author found that the addition of the colloid in every caseslightly lowered the vapour-pressure, and, as he points out, thepresence of a solid i n solution could not possibly increase thevapour-pressure. For example, if the steam given off at 98" from agelatin solution had a pressure of 760 mm., i t would necessarily re-condense to water and mix again with the solution.When solutions of gum or gelatin are cooled considerably belowzero, the author finds that they do not solidify as a whole, as statedby Guthrie, but ice crystals gradually separate out.He finds thatgelatin has a strong condensing action on the water of solution.G.W. T.Precipitation of Colloid Substances by Salts. By 0. NASSE(Pjiiyer's Archiv, 41, 504--514).-A11 prote'ids except peptone canbe precipitat!ed by saturating a neutral solution with ammonium sul-phate, some more easily than others, for instance, globulins moreeasily than albumins. Other salts bave the same power, but noneact so readily as ammonium sulphate. This property, however, is notcharacteristic of proteids : soaps, gelatin, and certain fioluble carbo-hydrates (glycogen, amidulin, inulin, &c.>, are similarly precipitated ;it in fact seems to be a property common to colloid substances.The question arises, on what does the difference in the concentra-tion of the salt necessary to produce precipitation depend ? Is theaction of the salt simply due to a struggle of the molecule ofproteid, gelatin, &c., with that of the salt for water, and t h a t the pre-cipitation of the colloid substance occurs as soon as its water-attract-ing power is exceeded by that of the salt?In order to determine whether this is the case, one m u d ascertainthe amount of two or more different salts necessary to precipitat'e thesame aniount of one colloid substance, the necessary concentrationof the salt solutions corresponding with a : b : c, &c.The same ques-tion is then invebtigated €or another colloid substance, and the rati100 ABSTRACTS OF CHEMICAL PAPERS.a' : b' : c', &c., found.for water, a : b : c, &c., will be found = a' : b' : c', &c.Tf hhen we have only to deal with attractionThe following table illustrates the results obtained :-Collo'id substances.Gplatin .........The solution contained in 100C.C.the following amounts ofsalt w18cn precipitation began.L--v---Ja. 6 .Ammonium Magnesiumsulphate. sulphat e. a : b.12.4 14.8 0.84White of egg.. .... 20.2 19.6 1-039 3 ...... 18.5 19.3 0.95Serum prote'rds .... 17.4 18.5 0.94Albumose. ........ 12.7 13.6 0.9:3,, ......... 14.9 17.6 0.85Amidulin. ........ 20.9 10.5 1-99Glycogen-dextrin . . 44.7 23.7 1-99The differences of the numbers in the last column show thatwater-attracting power is not the only influence at work, but someother relation must exist between the colloid and the salt.Still it ispossible that it may explain some of the precipitations, especially thatof gelatin. Gelatin loses many of its characteristic properties afterthe prolonged heating of its solutions; it, for instance, no longergelatinises on cooling, and its water-holding power is greatly in-creased, yet, the ratio a : b = 0.84 remains constant for the gelatin inall the different stages of this change.With regard to the proteids, in which such wide differences occur,it is thought probable that the explanation lies in the fact that loosecompounds with the salts are formed.The paper concludes with some remarks on the influence of tern-perature in determining precipitation by salts.New Formula for Calculating the Molecular Volumes ofChemical Compounds at the Boiling Points. By J. A.GROSHANS (Rac. l'rav. Chim., 7, 220--225).-The molecular volumeof a sut)stance, CPH4Or, at the boiling point may be represented byt7, = a + 1O(p + q ) - 7.28 B for a fatty compound, or by the sameexpression miiius 15 for an aromatic compound, c1 being the numberof' O.C. equal to the molecular weight of the compound, and B = p + q + Y. Both these formulte obey Kopp's rules, that homologouscompounds differing in their composition by CH, should differ i utheir molecular volumes by 22, and that a fatty compound shouldhave approximately the same volume as an aromatic compound whichdiffers in its formula by C2 - Hq.With hydrocarbons, since 7 = 0, the formula may also be written(us - a)/B = 2-72 for fatty compounds, or (u, - a -+- 15)/B = 2-72for aromatic, both of which are fonnd t o agree well with experiment.For halogen-deiaivatives, an addition of 15 must be made for each atomof halogen oontained. H. C.W. D. HISORGANIC CHEMISTRY. 101Molecular Lowering of the Freezing Point of Benzene byPhenols. By E. PAT ERN^ (Ber., 21, 3178-3180).--The author madea, number of experiments to ascertain whether the fact that certainsubstances containing the hydroxyl-group produce an abnormal lower-ing of the freezing point of benzene WRS true of all substances, andwhether this abnormal behaviour was sufficient proof of the pi*esenceof the hydroxyl-group (compare Raoult, Abstr., 1884, 959). The re-sults showed that although phenol behaves in an abnormal manner,the following compounds : ethyl phenol, acetylphenol, two isomericnitrophenols, tribromophenol, picric acid, paracresol, methyl salicylate,thymol, nitrothymol, nitrosothymol, a-naphthol, /-3-naphthol, andbenzylphenol, all produce the normal lowering of the freezing point ofbenzene and of acetic acid, either in dilute or moderately concentratedsolutions, the variations caused Ey change in concentration of coursebeing taken into consideration.The molecular weight of water determined by Raoult's method inacetic acid solution was found to be 18 (compare Rxonlt, lor. cit.), butthe author points out that tlhis result is not by any means conclusive,as, even if the molecules were originally more complex, they wouldbe simpli6ed by the act of solution.Hentschel's experiments with acetic acid (Zeit. phys. Chenz., 2, 308)seem to point to an opposite conclusion, but in this case the freezingpoint of the benzene solution was considerably below that of aceticacid. The fact that the molecular weight of water is found to be 36when the freezing point of the solution lies below 0" shows that thetemperature a t which the mixture freezes is a most important factorin the case. F. S. K

ISSN:0368-1769    

DOI:10.1039/CA8895600089

出版商:RSC    

年代:1889

数据来源: RSC

摘要:

ISORGANIC CHEMISTRY. 101 I n o r g a n i c C h e m i s t P y. Preparation of Chemically Pure Hydrogen Peroxide. By MANN (Chem. Zeit., 12, 857).-Hiydrogen peroxide of commerce con- tains many impurities ; it is niixed with a 4 per cent. of phosphoric acid and then, while stirring vigorously, barium hydroxide is added until the solution is exactly neutral to litnius. The clear solution is poured into a cold saturated aolution of barium hydroxide, and the precipitate of barium peroxide is well washed and may be kept for the preparation of pure hydrogen peroxide. For this purpose, i t i8 made into a thin magma and carefully decomposed by dropping steadily into dilute sulphuric acid containing 18 per cent. of con- centrated acid; any excess of sulphuric acid being removed by hydroxide, and vice verSd.Excess of barium peroxide must be avoided as it decomposes hjdrogen peroxide. D. A. L.2 02 ABSTRACTS OF CHEMICAL PAPERS. t. 1 P. Compounds Of Chlorine with Iodine. By w. STosTENBEKER ( R e c . Trav. Chinz., 7, 152-205).-The only compounds of iodine with chlorine which are capable of existing in the solid state are IC1 and ICI,. Two modifications of the first exist which the author terms a and /3. IC1 is best, prepared by passing dry chlorine over iodine and then distilling the product with a few grams of iodine. If the distillate is allowed to solidify at -25", the a-modification is obtained in long, dark-red needlcs, melting a t 27.2". If the crystal- lisation take place between +5" and -lo", modification p is usually, but not invariably, obtained.When slowly formed, it crystullises in dark-red plates meltirig a t 13.9'. It is unstable and readily converted into the a-modification, into which it is gradually changed. The most favourable temperatures for its existence are between 0" and -10". If cooled below -12" it changes into the a-modifica- tion. The trichloride ICl, is prepared by treating iodine, or the liquid IC1 with excess of chlorine. It sublimes very readily and settles on the sides of the apparatus in slender, yellow needles. It melts a t the ordinary pressure a t temperatures varying between 20" and GO", but under a pressure of 16 atmos. melts regularly at 101". After fusion, it solidifies in brownish-red crystals. The author further shows tbat every mixture of the two elements, chlorine and iodine, is possible in the liquid state above a certain temperature which depends on the proportion of the two elements.Below that temperature, one of the substances Iz, ICla, IClP, ICI,, or c1, will separate in the solid state. I€ on a diagram representing pressures and temperatures the two points be taken at which chlorine and iodine melt, corresponding wlth the temperatures - 102" and 114.3', then between these points will lie the curve which is the locus of the points a t which the various mixtures of chlorine and iodine exist in the liquid state. These t w o end points are triple points for the pure elements, and on the intermediate curve will be found three quadruple points, each corresponding to equilibrium between four phases (comp. Roozeboom, Abstr., 1888, 1151).Phases present. Complete solidification will only occw a t the three distinct tern- peratures of the quadruple points, when separation of a mixture of the solids I, + IC1, IC1 + Ic13 or ICI, + C1, will take place. A study of the compounds of iodine and chlorine in the gaseous state shows that molecules IC1 exist i n that condition, and only suiTey slight dissociation even a t 80°, whereas ICl3 cannot exist as gas, the molecules undergoing complete dissociation. H. C.INORGANIC CHEMISTRY. 103 Theory of the Lead Chamber Process. By F. RASCHIG (Anualen, 248, 123-140), and by G. LUNGE ( B e y , , 21, 3223-3240). -Controversial papers. Compounds of Ammonia with Selenious Anhydride. By C. A. CAMERON and J. MACALLAN (Proc. Boy. Soc., 44, 112-115).-Dry ammonia passed into an alcoholic solution of selenious anhydride forrris amrnoiLiurn seEenosamate, NH4*Se0,*NH2, which crys tallises in hexa- gonal prisms and pyramids. It loses ammonia very easily even on exposure to air or treatment with solvents and on heating.It is only partially converted into ammonium selenate by the action of water even after continued boiling. Potassium hydroxide a t once liberates ammonia. Sulphuric acid reacts violently with it, and chlorine oxidises it to ammonium selenate. Sulphurous anhydride and stannous chloride reduce it with separation of selenium. The acid salt formed from the above by loss of ammonia has the composi- tion (NH4)H(SeO2-NH2),, and is a deliquescent salt soluble in alcohol. It behaves like the normal salt, but is much more stable. When strongly heated, it is decomposed iiito ammonium selenite, ammonia, water, nitrogen and fused selenium.These compounds of selenious anhydride are more akin to the compounds of sulphuric anhydride with ammonia than to those of sulphurous anhydride. By V. WEDENSKY ( J . BUSS. Chem. Xoc., 1888, 20, 29--32).-When phosphorous acid is dis- solved in acetic anhydride, a colourless crystalline substance separates after a time. This is washed with ether and analysed ; the results agree with the formula of a monacetyl-derivative of phosphorous acid, (C,H,O) H2POs. When acetic anhydride acts on phosphorus trichloride, an analogous compound is obtained ; this, however, seems to be a mixture, and cannot be obtained free from chlorine.A H. K. 1’. Constitution of Phosphorous Acid. phosphorous triacetyl-derivative could not be obtained. B. l3. Compounds of Arsenious Acid with Sodium Iodide and Bromide. By F. R~~DORFF (Ber., 21, 30.51--305.3).-The compound NaEh,2As2O, is obtained when arsenious acid (20 grams) and sodium bromide (120 grams) are dissolved in boiling water (350 c.c.), and the filtered solution allowed to cool slowly (compare Abstr., 1887, 107). It crjstallises in hexagonal plates and is decomposed when warmed with water. The compound NaI, 2As203, prepai-ed by dissolving arsenious acid (22 grams) and sodium iodide (60 grams) in hot water (500 c.c.), cry stallises in hexagonal plates and is decomposed by hot water. Preparation of Boron and Silicon by Electrolysis. By W. HANPE (Chem.Zeit., 12, 841).-When fused borax is submitted to electrolysis in a gas-carbon crucible with a platinum positive and a gas-carbon negative electrode, oxygen is evolved from the platinum, whilst in the first instance sodium separates a t the negative electrode, but this by a secondary reaction liberates boron. The negative electrode is from time to time withdrawn from the crucible, and P. S. K.104 ABSTRACTS OF CHEJTICXL PAPERS. when cool, the slag carrying the boron i q carefully knocked off. Th;s is treated with hydrochloric acid and water, leaving pure amorphous boron mixed with a small quantity OF carbon and some isolated microscopic crystals of, a t present, anknown composition. Fused boric anhydride does not conduct. But amorphous silicon may be prepared in a similar manner from fused sodium silicate.Beryllium Silicates. By P. HAumFEuTLLF: and A. PERREY (Compt. rend., 107, 786-789) .-If the constituents of an aluminium or beryllium leucite are fused a t 600-800" with excess of potassium vanadate, mineralisation takes place rapidly, b u t the cornposition of the product varies as the vanadate gives up more or less of its alkali, and it is rarely homogeneous. The product is washed with water and very dilute potash, and tJhe crystalline constituents are separated by solutions of cadmium tungstoborate of varying specific gravity. I n the alum- inium compounds, the potassium and aluminium are always present in the proportion A1,03 : &O, whilst in the beryllium com- pounds the ratio of beryllia to potash varies from 1.25 to 0.5.The silicate containing Be,03,2K20 is obtained with r), mixture which always contains an excess of alkali, whilst the silicate containing Be,03,K20 is obtained with a neutral mixtme. In the aiuminium compounds, the ratio of silica to potash varies from 4 ko 5, whilst in the beryllium compounds the same ratio varies from 4.5 to 5.0, In the latter case, the product is always heterogeneous, and probably results from the simultaneous crgstallisation of silicates containing 4sio2 and 5Si02. The silicate 4SiO2,Re,O3,KZO is obtained in icosi- tetrahedrons by rapidly heating its constituents to st high temperature and cooling very gradually. Products were also obtained containing both alumina and beryllia. They are all fusible, and are homogeneous with respect to sp.gr. The following ratios were observed :-K,O : SiO, : : 1 : 4.5-4.8 ; K,O : R,O, : : 1 : 0*75-1*0 ; Be,O, : A120, : : 1 : 0.5-1.75. Silicates containing beryllia and ferric oxide are yellowiRh, crystallise in the same form, and are bomogeneoiis with respect to specific gravity. The following ratios were observed :-KzO : SiO, : : 1 : 4.59-5.0; K,O : R20, : : 1 : 0.6-1-3 ; Be203 : 'Fez03 : : 1 : 0.3-1.3. Alumina and silica in the proportion of 1 mol. of A1203 to 6 mols. of Si03, heated with potassium vanadate, yield orthoclase in macled, prismatic crystals ; but with beryllia in place of alumina, the crystals are always icositetrahedrons. With a mixture of alumina and I,eryllia, however, non-macled, prismatic, crystals, of the composition GSi02,Rz03,K20 are obtained, and are homogeneous with respect to bpecific gravity.The ratio SiO, : K,O remains constant, whilst the iatio A1203 : BezO, varies. The silicates obtained w i t h beryllium may be regarded as mixtures of the following compounds :- D A. L. All the products crystallise i n icositetrahedrons, a2. 8Si02,Be203,2K20 4Si02,Rez03, K 2 0 5Si02,Be203,K,0. 10 S i O,, Be203, 2K20, The fact that the beryllia can be replaced by alumina and ferricIN0 RGANIC CHEMl ST RY. 105 oxide in these compounds, and can replace alumina in orthoclase, combined with the well-known relations of beryllium to magnesium, would seem to indicate that beryllia has sometimes the functions of a monoxide and sometimes those of a sesquioxide. Occlusion of Gas by Electrolytic Copper.By A. SORET (Qompt. r e d . , 107, 733-734) .-With dilute copper solutions, unless the current is very weak, the precipitated metal is spongy, the nature of the deposit depending not only on the strength of the solution and the intensity of the current, but also on the proportion of free acid present. Lenz obtained 4.4 vols. of hydrogen from 1 vol. of deposited copper. The author finds that eleclroljtic copper always contains hydrogen, which, however, is simply occluded. There is a connection between the volume of gas occluded and the temperature and acidity of the soliltion. These conditions also affect the malleability of the metallic deposit. The occluded hydrogen sometimes contains small quantities of carbonic anhydride and traces of carbonic oxide. Mechanical Properties of Metals in Relation to the Periodic Law.By W. C. KOBERTS-AUSTEN (Proc. Roy. Xoc., 43, 425-428). -Very pure gold was alloyed with 0.2 per cent. of various metals, and the tensile strength determined. The tenacity was found to be affected by the elements in the order of their atomic volumes, those elements which have a higher atomic volume than gold diminishing its tenacity very considerably, whilst silver, which has nearly the same atomic volume as gold, hardly affects either its tenacity or extensibility. Hence it appears that Carnelley’s law-that ‘‘ the properties of compounds of the elements are a periodic function of their atomic weights,” may also be applied to alloys. Tenacity was chosen for examination, since those metals which are most tenacious liave the highest melting points, and the melting point, according to Pictet, is intimately connected with the lengths of the molecular oscillations.H. I(. T. Dissolution of Iron in Aqueous Soda. By G. ZIRNIT~ (Chem. Zeit., 12, 355).-When a strong current of air is blown into a hot, concentrated solution of soda containing about 34 per cent. of hydr- oxide, standing in an iron vessel, or to which finely divided hydrated ferric oxide has been added, perceptible quantities of iron are dis- solved without colouring the liquid. The solution remains clear and colourless for several days at tlhe ordinary temperature, but ultimately becomes turbid, yellow, and finally red, owing to the separation of the hydrated ferric oxide ; this colour, howerer, disappears again on heating.When the colourless solution is diluted, the ferric oxide is precipitated in about half an hour, but is redissolved by concentrating the diluted solution. Hydrogen sulphide a t first produces a deep, cherry-red coloration in the colourless liquid, and on continuing the action a greenish-black precipitate is formed, leaving a clear solution free from iron, but slightly yellow from sodium sulphide. It is suggested that the iron exists in solution as sodium perferrate, NaFe04. D. A. L. VOL. LVI. i C. B. B. C. H. B.106 ABSTRACTS OF CHEMICAL PAPERS. Ammonium Fluoroxymolybdates. By F. MAURO (Chsnz. CPntr., 1888, 1056-1057, from Hem. R. Acad. dei Lincei [4], 4, 481-488). - Triummonium Jluoroxyrnoly bd Ute, Mooz F2,3NH4F, prepared by evaporating a solution of ammonium molybdate in excess of am- monium fluoride solution acidified with hydrogen fluoride, is obtained in clear and colourless rhombic prisms.The faces (loo), (OlO), (120), and (011)-were observed, and the angles (100) : (110) = 28" 36', (011) : (011) = 82" 29', and (011) : (110) = 71" 36'. Axial ratio, a : b : c = 0.5452 : 1 : 0.8767. It is soluble in water, pro- ducing an acid solution. On heating, white fumes are evolved and anhydrous molybdic acid remains. It contains no water of crystal- lisat ion. Fluorurnmonium-moly bdic anhydride, Moo3, ZNH4F, prepared by adding ammonia to the solution of the last-named salt, and is thus obtained as a white, microscopic, crystalline precipitate. Larger crystals may be obtained by dissolving the compound in a hot solu- tion of ammonium fluoride and ammonia, and allowing to evaporate spontaneously by exposure to the air o r over sulphuric acid, when the salt crystallises out-at first as prisms, but later in octahedrons.If the precipitated salt is simply dissolved in ammonia and then allowed to evaporate, monoclinic crystals of hydrated ammonium mol ybdate separate first, then, later, the prisms and octahedrons of the new salt. The crystals appear usually in the form of twins, grown together in such a manner as to give the crystal the appearance of it hexagonal prism. They are shining, transparent, light-yellow, and belong to the rhombic system; u : h : c = 0.57464 : 1 : 0.67705. The faces (OlO), (Ool), (110), and (011) were ob,served. Twinning plane (110). The angles measured were: (110) : (110) = 59" 46'; (010) : (110) = 60" 7' ; (010) : (011) = 55" 54'; and (110) : (011) = 7 3 O 47". This salt is decomposed by water.It is anhydrous, and is decomposed on heating above looo, molybdic acid remaining. Normal ammonium Jluoroxy moly bda.te? Mo02F2,2NH4F, is prepared from the last-named salt by spontaneous evaporation of the aqueous solution, rendered acid with hydrogen fluoride. It consists of brightly shining, transparent, colourless plates or prisms belonging to the rhombic system; a : b : c = 0.8413 : 1 : 1.0164. The faces (OlO), (OOl), ( O l l ) , (eel), and (221) were observed. The angles measured were: (001) : (201) = 67" 31'; (001) : (011) = 45" 28'; (001) : (221) = 72" 26'; (291) : (011) = 74" 27' ; (011) : (221) = 49" 31' ; and (201) : (221) = 37" 52'.This salt is sparingly soluble in water, and is decomposed by heating above 100"; ammonium fluoride and hydrogen fluoride are evolved, leaving molybdic acid. Octahedric ammonium Jluoroxymolybdate, MoO~F~,~NH~F, (NH~)~MoO~, a double salt of ammonium flnoroxymolybdate with ammonium molyb- date, is prepared by allowing a solution of triammonium fluoroxy- molybdate i n ammonia to evaporate spontaneously in the air or over sulphuric acid. It forms small, colourless, transparent, lustrous octa- hedrons, which gradually disintegrate when exposed to the air. It is isomvrphous with the corresponding double salt of tungsten. It isINORQANIC CHENISTRY. 1 0 I soluble in water, and does not again crystallise out of the solution. It suffers decomposition, like the other salts, when heated above 100".Ammonium dimolybdate, 2Mo03,(NH&0 + H,O, prepared by dis- solving flnorammonium-molybdic anhydride in ammonia andC allowing ths solution to remain. It forms transparent, colourless, lwstwus, monoclinic crystals-usualiy pyramidal ; a : b : c = 0.99628 : 1 : 0'94497 ; /3 = 'IS0 47' 41". TJe faces observed were: (loo), (OlO), (Oll), (lOi), ( l l l ) , and (111) ; the ;t_ngles : (001) : (100) = 72" 48' ; (001) : (iOl) = 52'44' ; (100) : (101) = 5P" 28'. By heating above 100" this compound behaves exactly like the other members of the series, and leaves a residue of molybdic acid. By L. VIGRON (Compt. r m d . , 107, 734-'737).-When sheet zinc is immersed in a solution of a kin salt which contains no free acid, and the precipitated tin is washed with water and dried in coil- tact with air, the product is iafusible and burns like tinder wlieii heated in presence o€ air.If heated to redness in a porcelain tube in a current of carbonic anhydride for two hours, it separates into small globules of fused tin and a grey powder. These are separated by levigrttion, and atfter the powder has been dried, it burns readily when heated in the air. The infusible tin occurs in slender, denriritica forms of sp. gr. 6.910 to 7.198 at -15", and contains 96 to 97.3 p ~ r cent. of tin. I t dissolves readily in hydrochloric acid with evolutioir of hydrogen. The alteration in the properties of the tin does not, tako place during precipitation, but when the tin is dried in contact wlttl air it is partially converted into stannous oxide, the alteration taking place the more readily the less the proportion of free acid in the liquid from which the tin is precipitated.If much free acid is present, the tin does not oxidise when dried. The proportion of stannous oxide in the oxidised tin varies from 22.5 to 33.4 per cent., and when combustion takes place shannic oxide is formed. J. W. L. Tin. C. €I. B. Fluorine-derivatives of Vanadium and its Analogues. fiY E. PETERSEN (Ber., 21, 3257--3259).-The following compounds were prepared by treating the oxides dissolved in hydrofluoric wid, wibh a solution of the various fluorides. ( I . ) Compounds derived fyont the 8esgwioxide.-(1) V,F,, + 6Hz0, large, readily soluble, dark green rhombohedra; (2) V2Ffi,4KF + 2H20, bright green, sparingly soluble, crystalline powder ; (3) \T,F6,6AmF, small, grass-green, regular octahedra; (4) CrZF6,6AmF( Wagner, Abstr., 1886, 676), rather darker green octahedra ; (5) Ti,F',,GAmF (Picciiii, Comnpt. rend., 97), small, red-violet octahedra ; (6) A1,Ffi,6AmF, spay- ingly soluble, dazzling white, crystalline powder ; (7) V2F6,4AmF + 2Hz0, emerald-green, rather large crystals, like octahedra, but politr- king ; (8) V2F6,2AmF' + 4H20, darker green, laniellar aggregates ; (9) V2F6,5NaF + HJ), bright green, sparingly soluble.crystalline powder ; (10) VzF6,2CoF~ + 14H20, small, dark green, monoclinic prisms ; (11) CrzFfi,2CoPz + 1PH20, pure dark green, monochic prisms ; (la) V2J?6,2XiF2 + 14H20, grass-green, monoclinic prisms ; i 2LO8 ABSTRACTS OF CHEUICXL PAPERS.(13) Cr2F,,2NiF’, + 14H20. emerald-green, monoclinic prisms. last four compounds are isomorphous. (11.) Compounds corresponding with Vanadium Dioxide.- (14) VOF2,3AmF, small, blue, almost regular octahedra, but polar- ising; (15) VOF2,2AmF + H20 (Baker, Trans., 2878, 392), larger, dark blue prisms ; (16) 4VOF2,7AmP + FiH,O, still darker blue, lamellar aggregates ; (17) 4VF4,2AmF + zH,O, small, blue-green prisms, stable only in solutions, strongly acidified with hvdrogen fluoride; (18) 3VOF2,7KF ; ( 1 9 ) VOF,,SKF ; (20) 3VOF2,8NaF + 2H20. These three form bright blue, sparingly soluble, crystalline powders. (111.) Compourds derived from the Pentoaide.--(21) VOF,,ZKF, colourless, crystalline powder ; (22) 2VOF3,3KF,HF, white, lustrous prisms ; ( 2 3 ) VP5,VOB’,,4KF, colourless aggregates of very slender needles ; ( 2 4 ) VOZF,2KF, golden-yellow, lustrous, hexagonal prisms, (25) 2\T02F,3KF, bright yellow prisms ; (26) 5VOF3,9AmF,3HF, colourless, dull lustrous prisms ; (27) V02F,3AmF, larger, straw- coloured, probably rhombic crvstals ; (28) 4V02F,7AmF,HP, white, lustrous aggregates ; (29) 2Nb205,3KF + 5H20, lust’rous white, sparingly soluble, crystalline powder ; (30) Nb205,KF + 3H20, colourless prisms. The compounds 14, 19, and 27 seem to be identical with those prepared by Piccini and Giorgis (Atti d.R. Acc. d e i Lincei, 1888, 590, and GIaz., 18, 186). The thermochemical relation of hydrogen fluoride to the sesqui- oxides of iron, chromium, and vanadium was determined. The following numbers were obtained for the heat of neutralisation in dilute aqueous solutions:-(Fe,0,H6,6HF + Aq) = 47500 cal., (Cr2o6€T6,6AF + Aq) = 50330 cal., (VZ(J6H,,6HF + Aq) = 52240 cal.The N. H. M. Decomposition of Antimony Sulphide by Boiling Water. By W. ELBERS (Chelrz. Zeit., 12, 355-356).- When antimonious sulphide is boiled with water, it is decomposed with the evolution of hydrogen sulphide and the formation of antimonious anhydride. I n this way 0.05 gram of the sulphide was completely converted into the anhydride in 14 hours; the liquid then had a slightly alitaline reaction. D. A. L.ISORGANIC CHEMISTRY. 101I n o r g a n i c C h e m i s t P y.Preparation of Chemically Pure Hydrogen Peroxide. ByMANN (Chem. Zeit., 12, 857).-Hiydrogen peroxide of commerce con-tains many impurities ; it is niixed with a 4 per cent.of phosphoricacid and then, while stirring vigorously, barium hydroxide is addeduntil the solution is exactly neutral to litnius. The clear solution ispoured into a cold saturated aolution of barium hydroxide, and theprecipitate of barium peroxide is well washed and may be kept forthe preparation of pure hydrogen peroxide. For this purpose, i t i8made into a thin magma and carefully decomposed by droppingsteadily into dilute sulphuric acid containing 18 per cent. of con-centrated acid; any excess of sulphuric acid being removed byhydroxide, and vice verSd. Excess of barium peroxide must beavoided as it decomposes hjdrogen peroxide. D. A. L2 02 ABSTRACTS OF CHEMICAL PAPERS.t.1 P.Compounds Of Chlorine with Iodine. By w. STosTENBEKER( R e c . Trav. Chinz., 7, 152-205).-The only compounds of iodinewith chlorine which are capable of existing in the solid state areIC1 and ICI,. Two modifications of the first exist which the authorterms a and /3. IC1 is best, prepared by passing dry chlorine overiodine and then distilling the product with a few grams of iodine.If the distillate is allowed to solidify at -25", the a-modification isobtained in long, dark-red needlcs, melting a t 27.2". If the crystal-lisation take place between +5" and -lo", modification p is usually,but not invariably, obtained. When slowly formed, it crystullisesin dark-red plates meltirig a t 13.9'. It is unstable and readilyconverted into the a-modification, into which it is gradually changed.The most favourable temperatures for its existence are between0" and -10".If cooled below -12" it changes into the a-modifica-tion.The trichloride ICl, is prepared by treating iodine, or the liquidIC1 with excess of chlorine. It sublimes very readily and settles onthe sides of the apparatus in slender, yellow needles. It melts a t theordinary pressure a t temperatures varying between 20" and GO", butunder a pressure of 16 atmos. melts regularly at 101". After fusion, itsolidifies in brownish-red crystals.The author further shows tbat every mixture of the two elements,chlorine and iodine, is possible in the liquid state above a certaintemperature which depends on the proportion of the two elements.Below that temperature, one of the substances Iz, ICla, IClP, ICI,, or c1, will separate in the solid state.I€ on a diagram representingpressures and temperatures the two points be taken at which chlorineand iodine melt, corresponding wlth the temperatures - 102" and114.3', then between these points will lie the curve which is thelocus of the points a t which the various mixtures of chlorine andiodine exist in the liquid state. These t w o end points are triplepoints for the pure elements, and on the intermediate curve will befound three quadruple points, each corresponding to equilibriumbetween four phases (comp. Roozeboom, Abstr., 1888, 1151).Phases present.Complete solidification will only occw a t the three distinct tern-peratures of the quadruple points, when separation of a mixture ofthe solids I, + IC1, IC1 + Ic13 or ICI, + C1, will take place.A study of the compounds of iodine and chlorine in the gaseousstate shows that molecules IC1 exist i n that condition, and only suiTeyslight dissociation even a t 80°, whereas ICl3 cannot exist as gas, themolecules undergoing complete dissociation.H. CINORGANIC CHEMISTRY. 103Theory of the Lead Chamber Process. By F. RASCHIG(Anualen, 248, 123-140), and by G. LUNGE ( B e y , , 21, 3223-3240).-Controversial papers.Compounds of Ammonia with Selenious Anhydride. By C. A.CAMERON and J. MACALLAN (Proc. Boy. Soc., 44, 112-115).-Dryammonia passed into an alcoholic solution of selenious anhydride forrrisamrnoiLiurn seEenosamate, NH4*Se0,*NH2, which crys tallises in hexa-gonal prisms and pyramids.It loses ammonia very easily even onexposure to air or treatment with solvents and on heating. It isonly partially converted into ammonium selenate by the action ofwater even after continued boiling. Potassium hydroxide a t onceliberates ammonia. Sulphuric acid reacts violently with it, andchlorine oxidises it to ammonium selenate. Sulphurous anhydrideand stannous chloride reduce it with separation of selenium. Theacid salt formed from the above by loss of ammonia has the composi-tion (NH4)H(SeO2-NH2),, and is a deliquescent salt soluble in alcohol.It behaves like the normal salt, but is much more stable. Whenstrongly heated, it is decomposed iiito ammonium selenite, ammonia,water, nitrogen and fused selenium.These compounds of seleniousanhydride are more akin to the compounds of sulphuric anhydridewith ammonia than to those of sulphurous anhydride.By V. WEDENSKY ( J . BUSS.Chem. Xoc., 1888, 20, 29--32).-When phosphorous acid is dis-solved in acetic anhydride, a colourless crystalline substance separatesafter a time. This is washed with ether and analysed ; the resultsagree with the formula of a monacetyl-derivative of phosphorousacid, (C,H,O) H2POs. When acetic anhydride acts on phosphorustrichloride, an analogous compound is obtained ; this, however, seemsto be a mixture, and cannot be obtained free from chlorine. AH. K. 1’.Constitution of Phosphorous Acid.phosphorous triacetyl-derivative could not be obtained.B.l3.Compounds of Arsenious Acid with Sodium Iodide andBromide. By F. R~~DORFF (Ber., 21, 30.51--305.3).-The compoundNaEh,2As2O, is obtained when arsenious acid (20 grams) andsodium bromide (120 grams) are dissolved in boiling water (350 c.c.),and the filtered solution allowed to cool slowly (compare Abstr.,1887, 107). It crjstallises in hexagonal plates and is decomposedwhen warmed with water.The compound NaI, 2As203, prepai-ed by dissolving arseniousacid (22 grams) and sodium iodide (60 grams) in hot water (500 c.c.),cry stallises in hexagonal plates and is decomposed by hot water.Preparation of Boron and Silicon by Electrolysis. By W.HANPE (Chem. Zeit., 12, 841).-When fused borax is submitted toelectrolysis in a gas-carbon crucible with a platinum positive and agas-carbon negative electrode, oxygen is evolved from the platinum,whilst in the first instance sodium separates a t the negative electrode,but this by a secondary reaction liberates boron. The negativeelectrode is from time to time withdrawn from the crucible, andP.S. K104 ABSTRACTS OF CHEJTICXL PAPERS.when cool, the slag carrying the boron i q carefully knocked off. Th;sis treated with hydrochloric acid and water, leaving pure amorphousboron mixed with a small quantity OF carbon and some isolatedmicroscopic crystals of, a t present, anknown composition. Fusedboric anhydride does not conduct. But amorphous silicon may beprepared in a similar manner from fused sodium silicate.Beryllium Silicates.By P. HAumFEuTLLF: and A. PERREY(Compt. rend., 107, 786-789) .-If the constituents of an aluminiumor beryllium leucite are fused a t 600-800" with excess of potassiumvanadate, mineralisation takes place rapidly, b u t the cornposition ofthe product varies as the vanadate gives up more or less of its alkali,and it is rarely homogeneous. The product is washed with waterand very dilute potash, and tJhe crystalline constituents are separatedby solutions of cadmium tungstoborate of varying specific gravity.I n the alum-inium compounds, the potassium and aluminium are alwayspresent in the proportion A1,03 : &O, whilst in the beryllium com-pounds the ratio of beryllia to potash varies from 1.25 to 0.5. Thesilicate containing Be,03,2K20 is obtained with r), mixture whichalways contains an excess of alkali, whilst the silicate containingBe,03,K20 is obtained with a neutral mixtme.In the aiuminiumcompounds, the ratio of silica to potash varies from 4 ko 5, whilst inthe beryllium compounds the same ratio varies from 4.5 to 5.0, Inthe latter case, the product is always heterogeneous, and probablyresults from the simultaneous crgstallisation of silicates containing4sio2 and 5Si02. The silicate 4SiO2,Re,O3,KZO is obtained in icosi-tetrahedrons by rapidly heating its constituents to st high temperatureand cooling very gradually.Products were also obtained containing both alumina and beryllia.They are all fusible, and are homogeneous with respect to sp. gr.The following ratios were observed :-K,O : SiO, : : 1 : 4.5-4.8 ;K,O : R,O, : : 1 : 0*75-1*0 ; Be,O, : A120, : : 1 : 0.5-1.75. Silicatescontaining beryllia and ferric oxide are yellowiRh, crystallise in thesame form, and are bomogeneoiis with respect to specific gravity.The following ratios were observed :-KzO : SiO, : : 1 : 4.59-5.0;K,O : R20, : : 1 : 0.6-1-3 ; Be203 : 'Fez03 : : 1 : 0.3-1.3.Alumina and silica in the proportion of 1 mol.of A1203 to 6 mols. ofSi03, heated with potassium vanadate, yield orthoclase in macled,prismatic crystals ; but with beryllia in place of alumina, the crystalsare always icositetrahedrons. With a mixture of alumina andI,eryllia, however, non-macled, prismatic, crystals, of the compositionGSi02,Rz03,K20 are obtained, and are homogeneous with respect tobpecific gravity.The ratio SiO, : K,O remains constant, whilst theiatio A1203 : BezO, varies.The silicates obtained w i t h beryllium may be regarded as mixturesof the following compounds :-D A. L.All the products crystallise i n icositetrahedrons, a2.8Si02,Be203,2K204Si02,Rez03, K 2 0 5Si02,Be203,K,0.10 S i O,, Be203, 2K20,The fact that the beryllia can be replaced by alumina and ferriIN0 RGANIC CHEMl ST RY. 105oxide in these compounds, and can replace alumina in orthoclase,combined with the well-known relations of beryllium to magnesium,would seem to indicate that beryllia has sometimes the functions of amonoxide and sometimes those of a sesquioxide.Occlusion of Gas by Electrolytic Copper. By A. SORET(Qompt.r e d . , 107, 733-734) .-With dilute copper solutions,unless the current is very weak, the precipitated metal is spongy,the nature of the deposit depending not only on the strength of thesolution and the intensity of the current, but also on the proportionof free acid present. Lenz obtained 4.4 vols. of hydrogen from 1 vol.of deposited copper.The author finds that eleclroljtic copper always contains hydrogen,which, however, is simply occluded. There is a connection betweenthe volume of gas occluded and the temperature and acidity of thesoliltion. These conditions also affect the malleability of the metallicdeposit. The occluded hydrogen sometimes contains small quantitiesof carbonic anhydride and traces of carbonic oxide.Mechanical Properties of Metals in Relation to the PeriodicLaw. By W.C. KOBERTS-AUSTEN (Proc. Roy. Xoc., 43, 425-428).-Very pure gold was alloyed with 0.2 per cent. of various metals,and the tensile strength determined. The tenacity was found to beaffected by the elements in the order of their atomic volumes, thoseelements which have a higher atomic volume than gold diminishingits tenacity very considerably, whilst silver, which has nearly thesame atomic volume as gold, hardly affects either its tenacity orextensibility. Hence it appears that Carnelley’s law-that ‘‘ theproperties of compounds of the elements are a periodic function oftheir atomic weights,” may also be applied to alloys. Tenacity waschosen for examination, since those metals which are most tenaciousliave the highest melting points, and the melting point, according toPictet, is intimately connected with the lengths of the molecularoscillations.H. I(. T.Dissolution of Iron in Aqueous Soda. By G. ZIRNIT~ (Chem.Zeit., 12, 355).-When a strong current of air is blown into a hot,concentrated solution of soda containing about 34 per cent. of hydr-oxide, standing in an iron vessel, or to which finely divided hydratedferric oxide has been added, perceptible quantities of iron are dis-solved without colouring the liquid. The solution remains clear andcolourless for several days at tlhe ordinary temperature, but ultimatelybecomes turbid, yellow, and finally red, owing to the separation of thehydrated ferric oxide ; this colour, howerer, disappears again onheating.When the colourless solution is diluted, the ferric oxide isprecipitated in about half an hour, but is redissolved by concentratingthe diluted solution. Hydrogen sulphide a t first produces a deep,cherry-red coloration in the colourless liquid, and on continuing theaction a greenish-black precipitate is formed, leaving a clear solutionfree from iron, but slightly yellow from sodium sulphide. It issuggested that the iron exists in solution as sodium perferrate,NaFe04. D. A. L.VOL. LVI. iC. B. B.C. H. B106 ABSTRACTS OF CHEMICAL PAPERS.Ammonium Fluoroxymolybdates. By F. MAURO (Chsnz. CPntr.,1888, 1056-1057, from Hem. R. Acad. dei Lincei [4], 4, 481-488).- Triummonium Jluoroxyrnoly bd Ute, Mooz F2,3NH4F, prepared byevaporating a solution of ammonium molybdate in excess of am-monium fluoride solution acidified with hydrogen fluoride, is obtainedin clear and colourless rhombic prisms.The faces (loo), (OlO),(120), and (011)-were observed, and the angles (100) : (110) =28" 36', (011) : (011) = 82" 29', and (011) : (110) = 71" 36'. Axialratio, a : b : c = 0.5452 : 1 : 0.8767. It is soluble in water, pro-ducing an acid solution. On heating, white fumes are evolved andanhydrous molybdic acid remains. It contains no water of crystal-lisat ion.Fluorurnmonium-moly bdic anhydride, Moo3, ZNH4F, prepared byadding ammonia to the solution of the last-named salt, and is thusobtained as a white, microscopic, crystalline precipitate. Largercrystals may be obtained by dissolving the compound in a hot solu-tion of ammonium fluoride and ammonia, and allowing to evaporatespontaneously by exposure to the air o r over sulphuric acid, when thesalt crystallises out-at first as prisms, but later in octahedrons.Ifthe precipitated salt is simply dissolved in ammonia and then allowedto evaporate, monoclinic crystals of hydrated ammonium mol ybdateseparate first, then, later, the prisms and octahedrons of the new salt.The crystals appear usually in the form of twins, grown together insuch a manner as to give the crystal the appearance of it hexagonalprism. They are shining, transparent, light-yellow, and belong tothe rhombic system; u : h : c = 0.57464 : 1 : 0.67705. The faces(OlO), (Ool), (110), and (011) were ob,served.Twinning plane (110).The angles measured were: (110) : (110) = 59" 46'; (010) : (110) =60" 7' ; (010) : (011) = 55" 54'; and (110) : (011) = 7 3 O 47". Thissalt is decomposed by water. It is anhydrous, and is decomposed onheating above looo, molybdic acid remaining.Normal ammonium Jluoroxy moly bda.te? Mo02F2,2NH4F, is preparedfrom the last-named salt by spontaneous evaporation of the aqueoussolution, rendered acid with hydrogen fluoride. It consists of brightlyshining, transparent, colourless plates or prisms belonging to therhombic system; a : b : c = 0.8413 : 1 : 1.0164. The faces (OlO), (OOl),( O l l ) , (eel), and (221) were observed. The angles measured were:(001) : (201) = 67" 31'; (001) : (011) = 45" 28'; (001) : (221) =72" 26'; (291) : (011) = 74" 27' ; (011) : (221) = 49" 31' ; and(201) : (221) = 37" 52'.This salt is sparingly soluble in water, andis decomposed by heating above 100"; ammonium fluoride andhydrogen fluoride are evolved, leaving molybdic acid.Octahedric ammonium Jluoroxymolybdate,MoO~F~,~NH~F, (NH~)~MoO~,a double salt of ammonium flnoroxymolybdate with ammonium molyb-date, is prepared by allowing a solution of triammonium fluoroxy-molybdate i n ammonia to evaporate spontaneously in the air or oversulphuric acid. It forms small, colourless, transparent, lustrous octa-hedrons, which gradually disintegrate when exposed to the air. It isisomvrphous with the corresponding double salt of tungsten. It iINORQANIC CHENISTRY. 1 0 Isoluble in water, and does not again crystallise out of the solution.Itsuffers decomposition, like the other salts, when heated above 100".Ammonium dimolybdate, 2Mo03,(NH&0 + H,O, prepared by dis-solving flnorammonium-molybdic anhydride in ammonia andC allowingths solution to remain. It forms transparent, colourless, lwstwus,monoclinic crystals-usualiy pyramidal ;a : b : c = 0.99628 : 1 : 0'94497 ; /3 = 'IS0 47' 41".TJe faces observed were: (loo), (OlO), (Oll), (lOi), ( l l l ) , and(111) ; the ;t_ngles : (001) : (100) = 72" 48' ; (001) : (iOl) = 52'44' ;(100) : (101) = 5P" 28'. By heating above 100" this compoundbehaves exactly like the other members of the series, and leaves aresidue of molybdic acid.By L. VIGRON (Compt. r m d . , 107, 734-'737).-When sheetzinc is immersed in a solution of a kin salt which contains no freeacid, and the precipitated tin is washed with water and dried in coil-tact with air, the product is iafusible and burns like tinder wlieiiheated in presence o€ air. If heated to redness in a porcelain tubein a current of carbonic anhydride for two hours, it separates intosmall globules of fused tin and a grey powder. These are separatedby levigrttion, and atfter the powder has been dried, it burns readilywhen heated in the air.The infusible tin occurs in slender, denririticaforms of sp. gr. 6.910 to 7.198 at -15", and contains 96 to 97.3 p ~ rcent. of tin. I t dissolves readily in hydrochloric acid with evolutioirof hydrogen. The alteration in the properties of the tin does not, takoplace during precipitation, but when the tin is dried in contact wlttlair it is partially converted into stannous oxide, the alteration takingplace the more readily the less the proportion of free acid in theliquid from which the tin is precipitated.If much free acid ispresent, the tin does not oxidise when dried. The proportion ofstannous oxide in the oxidised tin varies from 22.5 to 33.4 per cent.,and when combustion takes place shannic oxide is formed.J. W. L.Tin.C. €I. B.Fluorine-derivatives of Vanadium and its Analogues. fiY E. PETERSEN (Ber., 21, 3257--3259).-The following compounds wereprepared by treating the oxides dissolved in hydrofluoric wid, wibh asolution of the various fluorides.( I . ) Compounds derived fyont the 8esgwioxide.-(1) V,F,, + 6Hz0,large, readily soluble, dark green rhombohedra; (2) V2Ffi,4KF + 2H20,bright green, sparingly soluble, crystalline powder ; (3) \T,F6,6AmF,small, grass-green, regular octahedra; (4) CrZF6,6AmF( Wagner, Abstr.,1886, 676), rather darker green octahedra ; (5) Ti,F',,GAmF (Picciiii,Comnpt. rend., 97), small, red-violet octahedra ; (6) A1,Ffi,6AmF, spay-ingly soluble, dazzling white, crystalline powder ; (7) V2F6,4AmF +2Hz0, emerald-green, rather large crystals, like octahedra, but politr-king ; (8) V2F6,2AmF' + 4H20, darker green, laniellar aggregates ;(9) V2F6,5NaF + HJ), bright green, sparingly soluble.crystallinepowder ; (10) VzF6,2CoF~ + 14H20, small, dark green, monoclinicprisms ; (11) CrzFfi,2CoPz + 1PH20, pure dark green, monochicprisms ; (la) V2J?6,2XiF2 + 14H20, grass-green, monoclinic prisms ;i LO8 ABSTRACTS OF CHEUICXL PAPERS.(13) Cr2F,,2NiF’, + 14H20. emerald-green, monoclinic prisms.last four compounds are isomorphous.(11.) Compounds corresponding with Vanadium Dioxide.-(14) VOF2,3AmF, small, blue, almost regular octahedra, but polar-ising; (15) VOF2,2AmF + H20 (Baker, Trans., 2878, 392), larger,dark blue prisms ; (16) 4VOF2,7AmP + FiH,O, still darker blue,lamellar aggregates ; (17) 4VF4,2AmF + zH,O, small, blue-greenprisms, stable only in solutions, strongly acidified with hvdrogenfluoride; (18) 3VOF2,7KF ; ( 1 9 ) VOF,,SKF ; (20) 3VOF2,8NaF +2H20. These three form bright blue, sparingly soluble, crystallinepowders.(111.) Compourds derived from the Pentoaide.--(21) VOF,,ZKF,colourless, crystalline powder ; (22) 2VOF3,3KF,HF, white, lustrousprisms ; ( 2 3 ) VP5,VOB’,,4KF, colourless aggregates of very slenderneedles ; ( 2 4 ) VOZF,2KF, golden-yellow, lustrous, hexagonal prisms,(25) 2\T02F,3KF, bright yellow prisms ; (26) 5VOF3,9AmF,3HF,colourless, dull lustrous prisms ; (27) V02F,3AmF, larger, straw-coloured, probably rhombic crvstals ; (28) 4V02F,7AmF,HP, white,lustrous aggregates ; (29) 2Nb205,3KF + 5H20, lust’rous white,sparingly soluble, crystalline powder ; (30) Nb205,KF + 3H20,colourless prisms. The compounds 14, 19, and 27 seem to beidentical with those prepared by Piccini and Giorgis (Atti d. R. Acc.d e i Lincei, 1888, 590, and GIaz., 18, 186).The thermochemical relation of hydrogen fluoride to the sesqui-oxides of iron, chromium, and vanadium was determined. Thefollowing numbers were obtained for the heat of neutralisationin dilute aqueous solutions:-(Fe,0,H6,6HF + Aq) = 47500 cal.,(Cr2o6€T6,6AF + Aq) = 50330 cal., (VZ(J6H,,6HF + Aq) = 52240 cal.TheN. H. M.Decomposition of Antimony Sulphide by Boiling Water.By W. ELBERS (Chelrz. Zeit., 12, 355-356).- When antimonioussulphide is boiled with water, it is decomposed with the evolution ofhydrogen sulphide and the formation of antimonious anhydride. I nthis way 0.05 gram of the sulphide was completely converted intothe anhydride in 14 hours; the liquid then had a slightly alitalinereaction. D. A. L

ISSN:0368-1769    

DOI:10.1039/CA8895600101

出版商:RSC    

年代:1889

数据来源: RSC