摘要:

J O U R N A LH. E. ARMSTRONG, Ph.D., F.R.S.A. DUPR~, Ph.D., F.R.S.C. GRAHAM, D.Sc.F. R. JAPP, M.A., Ph.D.HUGO MULLER, Ph.D., F.R.S.W. H. PERKIN, F.R.S.OFI€. E. ROSCOE, LL.D., F.R.S.W. J. RUSSELL, Ph.D., F.R.S.J. MILLAR THOMSON, F.C.S.R. WARINGTON, F.C.S.C. R. A. WRIGHT, D.Sc., F.R.S.THE CHEMICAL SOCIETY.Sub-Ghitar:C. E. GROVES, F.C.S.G. T. ATEINSON.P. P. BEDSON, D.Sc.H. BAKER.D. BENDIX.C. H. BOTRAMLEY.C. A. BURSHARDT, Ph.D.9’. CARNELLEY, D.Sc.FRANK CLOWES, D.Sc.A. J. COWNLEY.c. E‘. CROSS.J. K. CROW, D.Sc.JOSEPH FLETCHER.A. J. GREENAWAY.OTTO HEHNER.W. R. HODGEINSON, D.Sc.D. A. LOUIS.J. M. H. MUNRO, D.Sc.W. NORTH.E. W. PRE‘COST, Ph.D.6. ROBINSON.R. ROUTLEDGE, B.Sc.I,. T. O’SHEA.J. TAYLOR.F. L. TEED.V. H.VELEY, B.A.C. W. WATTS.JOHN WATTS, D.Sc.JOHN I. WATTS.W. C. WILLIANS.Vol. XL.18 8 1. ABSTRACTS.L O N D O N :J. VAN VOOXST, 1, PATERNOSTER ROW.1881LONDON :HARRISON AXD SONS, PRINTERS IN ORDINARY TO RE% XAJEJTY, ST. XBILTIN’S LANEC 0 N T E N T S.ABSTRACTS OF PAPERS PUBLISHED I N OTHER JOURNALS :-THOLLON (L.). Rays in the Solar Spectrum produced by AtmosphericAbsorption . . . . . . . . . . . .HUGGINS. Luminous Spectrum of Water . . . . . . .JLLNSSEN (J.). Inversion of Photographic Images by the Prolonged Actionof Light . . . . . . . . . . . .DUFET (H.) . Optical Properties of Mixtures of Isomorphow Salts . .CURIE (J. and P.). Development of Electric Polarity by Pressure in Hemi-hedral Crystals with lnclined Faces .. . . . . .HAUTEFEUILLE (P.) and J. CHAPPUIS. Researches on the Silent ElectricDischarge . . . . . , . . . . . .D’ARSONVAL (A.). Voltaic Cells . . . . . . . . .SNITH (E. F.). Electrolytic Experiments . . . . . . .CRAFTS (J. M.). Rise of the Zero Point in Mercury Thermometers . .PEENET (J.). .CRAFTS (J. M.). Defects of the Mercurial Thermometer . . . .SALLERON (J.). Changes in Glass by Heating . . . . . .SORET (G). Influence of Temperature on the Distribution of Salts in Solu-tion . . . . . . . . . . . . .BERTHELOT. Reciprocal Displacements of the Halogen Elements. . .BERTHELOT. Heats of Formation of tlie Oxides of Nitrogen and of SulphurPOTILITZIN. Action of Dry Hjdrogen on Anhydrous Haloid Salts . .BERTHELOT. Cuprous Chloride . . . .. . . . .BERTHELOT. Atttcalnite . . . . . . . . .BERTHELOT. Thermochemistry . . . . . . . . .BERTHELOT. Contributions to the History of the Ethers . . . .ALEX~JEFF (W.). Heat Phenomena of the Solution of Alcohols in Water,and of Water in Alcohols . . . . . . . . .LOUGUININE (W.). Heat of Combustion of some Compounds of the FattySeries . . . . . . . . . . . . .RECHENBERG (C. v.). Heat of Combustion of Carbon Compounds . .GOLDSCHNIDT (H.) . An Acoustic Method of Determining Vapour-densitiesAMAGAT (E. H.). Dilatation and Compressibility of Gases under HighPressures . . . . . . . . . . . .SCHROEDER (H.). “ Volume Constitution” of Liquids . . . .BRUHL (J. W.). Relations between the Physical Properties of Carbon Com-poundsand their Chemical Constitution .. . . . . .BERTHELOT. Stabilityof Hydrogen l’erosiile . . . . . .DITTE (A.). Decomposition of Salts by Liquids . . . . . .OSTWALD (W.). Chemical d5nity . . . . . . . .MERZ (V.) and W. WEITH. Lecture Experiments . . . . .FIEVEZ (C.). Relative Intensity of the Spectral Lines of Hjdrogen andNitroqen ; its Bearing on the Constitution of Nebuh . . . .LUBARSCH (0.). Fluorescence. . . . . . . . . .HOORWEG (J. L.). Therniic Theory of Electricity . . . . .NARR (F.) . Discharge of’ Electricity in Gases and High T’acua . . .LONG (J. H.). Electrical Conductiritr of Saline Solutions . . . .Variation of the Fixed Points in Mercury Thermometersct 2General and Physical Chemistry.PAGE1112233344+55556667889910I d12131516171718697070707i v CONTENTS.WINKELXAN (A.) .Vapour-tensions of Homologous Series and Kopp’a Lawof Constant Difference of Boiling Points . . . . . .DUHRING (U.). The Law of Corresponding Boiling Points . . .MULLER ERZBACH (W.). Volume Relations of some Haloyd Salts . .J’ETTERSSON (0.). L o t h r Meycr and the Latest biscavery in Physics. .HAASS (R.). Lecture Experiment . . . . . . . .POTILITZIN (M.) . Reciprocal Displacement of the Halogens in Absence ofWater . . . , , . . . . . . . .THOMSEN (J.). Heat of Conibustion of Benzene . . . . . .EECIIENBERG (C. v.). Heat of Coinbustion of Carbon Compounds . .MEYER (V.). Determination of the Densities of Permanent Gases . .SCHRODER (H.). Volume Constitution of Sulphates, Chromates, and Se-lenates .. . . . f . . . . .XESDELRJRFF (D.). History of Periodic Atomicity . . . . .SIEYER (L.). Periodic Atomicity. . . . . . . . .CIIAPPUIS (J.). Absorption Spectrum of Ozone . . . . . .GLADSTONE (J. H.). Specific Refraction and Dispersion of Isomeric Bodies.JANOWSPY (J. V.). Optical Constants . . . . . . . .LAMANSEY (S.). Fluorescence . . . . . . . . .THOMSEN (T.). Molecular Rotatory Poiwr of Carbon Compounds . .HANKEL (IT.). Photo- and Thermo-electyic Properties of Fluorspar . .HABERMANN. Electrolysis of Organic Substances in Aqueous Solutions .THOMSEN (J.). Chemical Energy and Electromotive Power of Various Gal-vanic Combinations. . . . . . . . . . .OFFER (H.). Guthrie’s Cryohydrates .. . . . . . .UELLATI (M.) and R. ROMANESE. Thermic Properties of some DoubleIodides . . . . . . . . . . . . ,OGTER (J.). Thermochemistry of the Bromides and Iodides of Phosphorus .BCXTIIELOT. Thermochemistry of certain Haljid Salts . . . .BEETHELOT. Magnetic Oxide of Iron . . . . . . . .‘CIIOMSEN (J.). Heat of Combustion of Carbon Compounds . . . .AM^^^^ (V.). Vapour-density of Chlorine . . . . . . .XWLLER-ERZBACH (W.). Volume Relations in the Formation and Decom-pxitiou of Salts . . . . . . . . . . .BRAUNER (B.) and J. I. WATTS. Specific Volumes of Oxides . . .SCHRODER (H.). Volume Constitution of Liquid Compounds . . .HALLON ON (L.). .GOUY. Measurement of the Intensity of some Obscure Rays in the SolarSpectrum . . . . . . . . . .. .GLADSTONE (J. H.). Refraction Equivalents of the Diamond and ofCarbon Compounds . . . . . . . . . .I’PAFF (F.). Influence of Change of Temperature and Preseure on DoubleRefraction . . . . . . . . . . .IJPPMANN. The Unit in Absolute Electrical hfeasurements . . .l<X?U’ER (F.). Theory of the )Galvanic couple . . . . . .HEPPERGER (J.). Influence of Concentration of the Solutions on the Electro-motive Force of a Daniell’s Cell . . . . . . . .BOUTP (E.) . Measure of the Thermoelectric Electromotive Forces Developedby the Contact of a Metal and a Liquid . . . . . . .HANKEL (G. W.) . Photoelectric and Thermoelectric Properties of FluorsparCURIE (J. and P.). Laws of the Development of Electricity by the Action ofPI essure on Tourmaline . .. . . . . . . .CURIE (J. and P.) , Polar Electricity of Hemihedral Crystals with InclinedFaces . . . . . . . . . . . . .CL-RIE (J. and P.). Electrical Phenomena of Tourmaline and HemihedralCrystals with Inclined Faces . . . . . . . . .WEINHOLD (A.). Preparation of Selenium Resistance Rods for PhotophonicPurposes . . . . . . . . . . . .BECCXEBEL (H.) SDecific Magnetism of Ozone . . . . . .MEYER (L.). Evaporation without Fusion . . . . . .Observations on a Group of Rays in the Solar SpectrumPAGE71717113313313 313413513513713713813821321321421421521521521 621621 721821921921921921921922033333333333433433533533633733833833933334CONTENTS. 7-BLAVITZKP (73.).Specific Heat of Gases and Vapours . . . .WITZ. Cooling Power of Gases and Vap011i.s . . . . . .CRAFTS (J. M.). Cause of Variation of the Fixed Points of Theiwometem .POTILITZIN (A.). Double Decomposition in Absence of Water . . .BERTHELOT. Reciprocal Replacement of the Halogens . .POTILITZIN (A.) . Displacement of Chlorine by Bromine in Potassium ChlorideSARRAU and VIELLE. Heat of Formation of Gun-cotton . . . .BERTHELOT. Thermal Formation of PFrogenic Hydrocarbons . . .TOMMASI (D.). Apparatus for Showing the Dissociation of Bmnionilun SaltsVARENNE (L.). Passive State of Iron . . . . . . . .KAJANDER. Rate of Solution of Nagnesium in different Acids . . .BERTHELOT. Part played by Time in the Formation of Salts . . .DOWNES (A.). A Simple Proress of Slow Actinometry .. . .HUGGINS (W.). Photographic Spectraof Stars . . . . . .RUSSELL (W. J.). Absorption Spectra of Cobalt Salts . . . .ABNEY (W. DE W.) and FESTIEG. Influence of the Molecular Grouping inOrganic Bodies on their Absorption in the Infra-red Region of theSpectrum . . . . . . . . . . . .MORTON (H.) . Displacement of the Absorption Bands of Purpurin in AlumSolutions . . . . . . . . . . . .RADZISZEWSKI (B.). Phosphorescence of Organic and Organised Bodies .KOYL (C. H.). Colours of Thin Blowpipe Deposits . . . . .BRUHL (J. W.). Chemical Constitution of Organic Compounds in Relationto their Refractive Power and Density . . . . . . .LECHER (E.). Absorption of Sun's Ra! s by the Carbonic Anhylricle of theAtmosphere .. . . . . . . . . . .HOLTZ (W.). Some Remarkable Phenomena with Flames . . . .BEETZ (W.). The Strict Meaning of Galvanic Polarisation . . . .PBOYME ((2.). Electromotive Power of Galvanic Combinations consisting ofZinc, Sulphuric Acid, and Platinum, with Copper, Gold, and Carbon .KITTLER (E.). Differences of Electric Tension between Liquids in Contact,with Special Reference to the State of Concentration . . . .ROWLAND (H. A.). The Mechanical Equident of Heat . . . .SABATIER. Thermochemicnl Researches on the Sulpliides . . . .NILSON (L. I?.) and 0. PETTERSSON. Molecular Heat and Volume of the RareEarths and their Sulphates . . . . . . . . .RODWELL (G. F.). Coefficients of Exp:~nsion of Leai Iodide and of SilverLead Iodide . . . . . . . . . . ..SCHRODER (H.). Specific Grai ity and Volume-constitution of Formates .OSTWALD (W.) Volumetric Determination of the Chemical Influence ofMass. Part 111. On the Mass Influence of Water , . . .SPRING (W.). Union of Bodies bv Pressure . . . . . .MEYER (L.) and 0. SCHUMAEN. Transpiration of Taponrs . . . .BODASZEWSKY (L. J.) . Smoke and Vttpour under the Microscope . .LOCKYER (J. N.). Spectrum of Iron in the Sun . . . . . .VIOLLE (J.) . Intensity of the Liuminous Radiation fi.om IncandescentPlatinum . . . . . . . . . . . .CHAPPUIS (J.). Phosphorescence. . . . . . . . .EDER (J. M.). Decomposition of Perric Chloride and some Ferric Salts ofOrganic Acids by Light . . . . . . . . . .REYNIER (E.). Faure's Secondary Electric Pile . . . . . .BLONDLOT (R.). Electric Conductivity of Heated Gages .. . .BOUTY (E.). Changes of Vohime Accompanying Elrctrolptic Deposition ofa Metal . . . . . . . . . . . . .OGIER (J.). Chloride, Bromide, and Iodide of Sulphur . . . .BERTHELOT. Heat of Formation of Sulphur Oxides . . . , .ISAMBERT. Vapour of Ammonium Dihydrosulphide . . . . .BERTHELOT and J. OGIER. Heat of Forination of Dinlljl, Chlorinated Com-THOWSEN (J.). Benzene and Propargyl . . . . .pounds, and Aldehyde . . . , . . . .PAGE34034234234234"34234.23433433433 44%34448 545;4864874884884894.894894H! 14904904.9 149149249 1.49 t54954964974'8504'50566967067167167167367367367vi CONTENTS .BERTHELOT . Chloral Alcoholate .. . . . . . . .CAILLETET (L.) and P . HAUTEFEUILLE . Liquefaction of Gaseous Mixtures .CAILLETET (L.) and P . HAUTEFEUILLE . Changes of State near the CriticalMEYER (L.). Evaporation without Fusion . . . . . . .CROOKES (W.). Viscosity of Gases . . . . . . . .CLAUS (A.). Quantivalence of Carbon . . . . . . . .LOSSEN (W.). The So-called Differences in the Quantivalence of a Multi-valent A tom . . . . . . . . . . .KLINGER (H.). Magnitudes of Affinity in Carbon . . . . .BROCH (0 . J.), H . ST . CLAIRE.DEVILLE, and J . STAS . Measure made of a10 Per Cent . Iridium-Platinum Alloy . . . . . . .VOGEL (H . W.). Sensitiveness of SilTer Bromide Dry Plates for DifferentPortions of the Solar Spectrum . . . . . . . .HEUMANN (K.). Action of the Air in Rendering the Flame of the BunsenLamp Non-luminous .. . . . . . . . .CROOKES (W.) . .EXNER (F.) . Galvanic Polarisation . . . . . . . .UEETZ (W.). Elasticity and Electric Conductivity of Carbon . . .HOORWEG ( J . L.). Tliermic Theory of Galvanism . . . . .HORSTYANN (A) . Application of the Second Proposition of the Theory ofHeat to Chemical Phenomena . . . . . . . . . .MAILLARD and LE CHATELIER . Temperature of Ignition of GaseousMixtures . . . . . . . . . . . . .WULLKER (A.). Supposed Heating of Ice . . . . . . .~ ‘ H A N (C . v.). Thermochemical Investigations . . . . . .BERTHELOT and VIE~LLE . Study of the Explosive Properties of MercuryFulminate . . . . . . . . . . . .SCHTJMANN (0.). Vapour-densities of Homologous Ethers .. . .MULLER-ERZBACH (W.). Tension of Aqueous Vapour in Presence of dif-ferent Hygroscopic Bodies . . . . . . . . .AMAGAT (E . H.). Compressibility of Oxygen . . . . . .NIES (F.) and A . WINKELMANIT . Changes in Volume of some Metals onPusion . . . . . . . . . . . . .DOUGLAS (J . C.). .OSTWALD (W.). Deterniination of Cheniicd Affinity . . . .YOUNG (J.) and G . FORBES .WESENDONCK (C.). Spectrum of Carbonic Anhydride . . . .ABNEY (W . DE W.). Spectrum of Sodium . . . . . . .JANOVSKY (J . V.) . Alteration of Molecular Weight and Molecular Refrac-tive Power . . . . . . . . . . . .NOEL (G.). Action of Light on Silver Bromide . . . . . .CL~MANDOT and others . Action of Light on Phosphorescent Bodies . .PHIPSON (T . L.) . Curious Actinic Phenomenon .. . . . .EXNER (F.). Production of Electricity by Contact of Heterogeneous MetalsTemperature . . . . . . . . . . . .Discontinuous Pliosphorescent Spectra in High Vacua .The Phenomenon commonly called the “Cry of Tin”Experimental Determination of the Velocity ofWhite and Coloured Light . . . . . . . . .EXNER (F.). Thecry of Inconstant GalvanicCells . . . . .REGEIER (E.). Efficiency of Secondary Piles . . . . . .GLADSTONE ( J . H.) and A . TRIBE . Therinal Electrolysis . . . .BERTHELOT . Action of the Halond Acids on Salts containing the same HaloldElements . . . . . . . . . . . . .BERTHELOT .YOTILITZIN (A.) . Thermochemistry of Double Decomposition in AqueousSolutions of Salts . . . . . . . . . .BERTHFLOT and OGIER . Heat of Formation of various Carbon CompoundsLOUGUININE .Heat of Combustion of Alcohols of the Ally1 Series . .METER (V.). Vapour-density of the Halogens . . . . . .~IANNAY (J . B.). Absorption of Gases by Solids . . . . . .KAMANN (E.1. Passive State of Iron . . . . . . . .Reciprocal Displacement of the Halo’id Acids . . . .PAQE675676677678678679679679680773773773775176777777778778779779782’782782783783180861861866862862863863864866868868868869869870871872872876i - nLOBIN . Reiction without the Intervention of a Solvent . . . . 87OONTENTS. viiLECHNER (E.). So-cnlbd Chemical Repulsion . . . . . .SXITH (R. A.). Measurement of the Actinism of the Sun’s Raps and ofDaylight .. . . . . . . . . - .FIEVEZ (C.). Widening of the Hydrogen Lines . . . . . .PIEVEZ (C.). Spectrum of Magnesium and Constitution of the Sun . .WROBLEWSKI (S.). Application of Photometry to the Study of DiffusionPhenomena in Liquids . . . . . . . . . .LOCKTER (J. N,). On a New Method of Spectrum Observation . . .LOCKYER (J. N.). Note on the Spectrum of Hydrogen . . . .HUGGINS (W.). On the Photographic Spectra of Stars . . . .ABNEY (W. de W.). On the Photographic Method of Mapping the LeastRefrangible End of the Solar Spectrum, with a Map of the Solar Spec-trum from 7,600 to 10,750 . . . . . . . . .LIVEING (G. D.) and J. DEWAR. On the Spectra of Magnesium andLithium . . . . . , . . . . . . .LIVEING (G. D.) and J. UEWAR.On the Spectra of the Compounds ofCarbonwith Hydrogenand Nitrogen . . . . . . .LOCKYER (J. N.). Note on the Spectrum of Carbon . . . . .LIVEING ((3. D.) and J. DEWAR. On the History of the Carbon Spectrum .HUGGINS (W.). On the Spectrum of the Flame of Hydrogen . . .LIVEING (G. D.) and J. DEWAR. On the Spectrum of Water . . .HARTLEY (W. N.) and A. K. HUNTINGTON. Researches on the Action ofOrganic Substances on the Ultra-violet Rays of the Spectrum. Part 111.An Examination of the Essential Oils . . I . . . .RUSSELL (W. J.). On the Absorption Spectra of Cobalt Salts . . .LIVEING (G. D.) and J. DEWAR. Reversal of the Lines of MetallicVapours. No. VIII. Titanium, Chromium, and Aluminium . .LOCKYER (J. N.). On the Iron Lines widened in Solar Spots .. .ABNEY (W. de W.) and R. FESTING. On the Influence of Molecular Group-ing in Organic Bodies on their Absorption in the Infra-red Region ofthe Spectrum. . . . . . . . . . . .LIVEINQ (G. D.) and J. DEWAR. Investigations on the Spectrum of Mag-nesium . . . . . . . . . . . . .CROOKES (W.). On Discontinuous Phosphorescent Spectra in High Vacua .LIVEING (G. D.) and J. DEWAR. On the Identity of Spectral Lines ofDifferent Elements . . . . . . . . . . .GLADSTONE (J. H.) . The Refractive Equivalents of Carbon, Hydrogen,Oxygen, and Nitrogen in Organic Compounds . . . . .MASCART. Absolute Measurement of Currents by Electrolysis . . .LE Roux (F. P.). Electromotive Force of the Electric Arc . . . .COHN (E.). Resistance of Polarised Cells . . .. . . .HANKEL (W.) . Development of Polar Electricity in Hemimorphous Crystalsby AIterPLtion of Pressure in the Direction of the Asymmetrical Axes .NIAUDET (A.). Sound of the Electric Arc . . . . . . .WRIGHT ( C . R. A.). Determination of Cliemical A5nity in Terms of Elec-tromotive Force . . . . . . . . . . .REMSEN (I.). Deposition of Copper on Iron in a Magnetic Field . . .GORE (G.) . Chemico-electric Relations of Metals on Solutions of PotassiumSalts . . . . . . . . . . . . .DEWAR (J.). Studies on the Electric Arc . . . . . . .DEWAR (J.). Notes on Electrolytic Experiments. . ’ . . . .STREINTZ (F.) . Decomposition of Water between Platinum Electrodes bythe Discharge of a Leyden J a r . . . . . . . .SIENENS (C. W.). On the Influence of Electric Light on Vegetation, and onCertain Physical Principles involved .. . . . . .GORE (G.). Effects of Electric Currents on the Surfaces of Mutual ContactPERRY (J.) and W. E. AYRTON. A Preliminary Account of the Reduction .ABNEY (W. de W.). Note on the Spectrum of Sodium . - . .ofAqueous Solutions . . . . . . . . .of Obserrations on Strained Material, Leyden Jars, and VoltametersPAGE87395595595595696695695695795’795795795793795795795795795795795795795795’795895895895895895995996296296 296296296296296viii CONTENTS .PAGF:HOPKINSON (J.). The Electrostatic Capacity of Glass . . . . 963GORE (G.) .Electrodes . . . . . . . . . . . . 963GORE (G.). Experiments on Electric Osmose .. . . . . 063GORE (G.). Electric Currents caused by Liquid Diffusion and Osmose . 963TRIBE (A.) .963HOPXINSON (J.). Dielectric Capacity of Liquids . . . . . . 963GORE (G.). Influence of Voltaic Currents on the Diffusion of Liquids . . 963LORD RAYLEIGH and A . SCHUSTER .Measure . . . . . . . . . . . . . 963TRIBE (A.). Refraction of Electricity . . . . . . . . 963REIS (M . S.).the Molecular Weight . . . . . . . . . . 963SABATIER (P.) . Iron Chlorides . . . . . . . . . 964ItODWELL (G . F.). Effects of Heat on the Chloride, Bromide, and Iodideof Silver, and on some Chlorobromiodides of Silver . . . . . 965RODWELL (G. F.). Expansion Coefficients of Lead Iodide, and of an Alloyof Lead Iodide with Silver Iodide . . . . . . .. 966CARNELLEY (P.). Preliminary Notice on the Existence of Ice and otherBodies in the Solid State at Temperatures far above their ordinaryThermoelectric Behaviour of Aqueous Solutions with PlatinumExperimental Researches into Electric Distribulion as mani-fested bp that. of the Radicles of ElectrolStes . . . . . .Determination of the Ohm in AbsoluteSpecific €€eat of Organic Compounds, and its Relation toMelting Points . . . . . . . . . . . 966BOTTOMLEY (5 . T.). On the Thermal Couductivity of Water . . . 966TYNDALL (J.). On Buff’s Experiments on the Diathermancy of Air . . 966CROOKES (W.). On Heat Conduction in Highly Rarefied Air . . . 966TYHDALL (J.). Action of an Intermittent Beam of Radiant Heat onGaseous Matter . . . . . . . . . .. 966LOUGUININE . Heat of Combustion of Certain Alcohols and Aldehydes ofBERTHELOT . Glycollic Ether and Ethylene Oxides . . . . . 967SARRAU and VIEILLE . Heat of Formation of Explosives . . . . 968SCERODER (H.). Density and Molecular Volume of Certain Acetates . . 969HILGARD (E.). Aggregation of Small Particles . . . . . . 970AITKEN (J.). Relations between Dust, Fog, and Clouds . . . . 970HANNAY (J . B.) and J . HOGARTH . . 970the Fatty Series . . . . . . . . . . . 966On the Solubility of Solids in GasesHANNAY (J . B.). On the Absorption of Gases by Solids . . . . 971CROOEES (W.). Viscosity of Gases at High Exhaustions . . . . 971RAMSAY (W.). On the Critical State of Gases . . . . . . 971HANNAY (J . B.). On the Limit of the Liquid State .. . . . 971CROOKES (W.). On a Fourth State of Matter . . . . . . 971MILLS (E . J.). On Chemiaal Repulsion . . . . . . . 971oils . . . . . . . . . . . . . 9’71Explosive Gaseous Mixtures . . . . . . . . . 9’71GOROFF (N . E.). Tellnric Rays of the Solar Spectrum . . . . 1091DE CHARDOENET . Absorption of the Ultra-violet Rays . . . . 1091PHIPSON (T . L.). A Curious Actinic Phenomenon . . . . . 1092LINDO (D.). Improvements in BatterieR . . . . . . . 1092and by EvaporationandCondensation . . . . . . . 1002XONOVALOFF (D.). Vapour-tension of Mixed Liquids . . . . . 1093Low Pressures and a t High Temperatures . . . . . . 1094riment . . . . . . . . . . . . 1095MAUBIEKI? (E . J.).MALLARD and LE CHATELIER .Action of Sulphuric Acid recently heated t o 320” onVelocity of Propagation of Inflammation inXOSER (J.).BERTHELOT .Specific Heat and Heat of Dilution of Perchloric Acid . . 1092BERTHELOT and VIEILLE . Heat of Formation of Potassium Perchlorate . 1093AXAGAT (E . H.).LEMOINE (G.) .The Circuit Produced by the Reaction Current of ElectrolysisCompressibility of Carbonic Anhydride and of Air underDissociation : Comparison of Formulse deduced from ExpeCONTENTS . isIn,orgartic Chemistry .BTARD (A.) and H . MOISSAN . Preparation of Hydrogen Selenide andHydrobromic Acid . . . . . . . . . .HAUTEFEUILLE (P.) and J . CHaPPuis . Liquefaction of Ozone, and its Colourin the Gaseous State . . . . . . . . . .SCHLOESING (T.) . Constancy of the Proportion of Carbonic Anhydride inthe Atmosphere .. . . . . . . . . .REISET (J.). Proportion of Carbonic Anhydride in the Atmosphere . .SCHONE (E.). Proofs of the Existence of Ozone in the Atmosphere . .SCHONE (E.). Observations on the Atmo>phere made with Thallium Papers~ T A R D (A.). Position of Boron in the Series of Elementary Bodies . .COLSON (A.). Action of Sulphur on Water . . . . . . .NAYEN~ON . .MOISSAN (H.). Sesquioxide of Chromium . . . . . . .BERTHELOT . Preparation of Chlorine . . . . . . . .ELEIN (D.). Boroduodecitungstic Acid . . . . . . .MEUNIER (M . S.). A Source of Atmospheric Carbonic Anhydride . .SCHULZE (H.) . Liquid Sulphur Phosphide . . . . . . .MARIGNAC (C.). The Earths of Samarskite . . . . . . .MOISSAN (H.). Metallic Oxides of the Iron Group .. . . .SCHNEIDER (R.). Atomic Weight of Antimony . . . . . .ZIMMERMANN (C.). Products of Decomposition and Metamorphosis of UranylKONINCE (L . L.). Preparation of Hydrochloric Acid Gas . . . .MOOT (C . G.). Action of Iodine on Phosphorus Trichloride . . . .KOBTER (A.). Impurities in Sodium Bicarbonate . . . . . .SILBER (P . G.). Action of Hydrochloric Acid a t High Temperatures cnUltramarine Rich in Silica . . . . . . . . .MEYER (L.). Atomic Weight of Glucinum . . . . . . .NILSON (L . F.). Atomic Weight of Glucinum . . . . . .SPRENGER (M.). Phosphotungstic Acid . . . . . . .FLEURY (G.). Sodium Arsenate . . . . . . . . .RICHE (A.). Bismuth Subnitrate . . . . . . . . .REINSCH (H.). Manganese Dioxide containing Antimony . . . .LEEDS (A .R.). Preparation of Ozone by Heating Substances containingHAUTEFEUILLE (P.) and J . CHAPPTTIS . Nitrification . . . . .HAUTEFEUILLE (P.) and J . CHAPPUIS . spectra of Compound Gases, and a . . . . . .DEMAR~AY (E.). New Derivative of Nitrogen Sulphide . . . .DAMOISEAU (A.). Action of Phosphorus on Hydriodic and Hydrobromic AcidsHOGBOM (A.). Fluosalts of Tellurium . . . . . . .DITTE (A.). Action of Hydrochloric Acid on Metallic Chlorides . . .SCHONACH (J.). Solubility of a Mixture of Sodium and Potassium ChloridesBARBAGTJA (a . A.) and P . Gucci . Action of Heat on Sodium HydrogenKLEIN (U.). Sodium Borotungstates . . . . . . . .BRAUNEB (B.). Atomic Weight of Glucinum . . . . . .Presence of Cerium in the Coal Measures of St . etienne .KLEIN (D.).Borodecitungstic Acid and its Sodium Salts . . . .Sulphide . . . . . . . . . . . .CRAFTS (J . M.) and F . MEIER . Density of Iodine Vapour . . . .Oxygen . . . . . . . . . . . . .New Compoundof Nitrogen and OxygenSulphite . . . . . . . . . . . . .COSSA (A.). Distribution of the Cerite Metals . . . . . .COSSA (A.). Didymium Tungstate . . . . . . . .GROGER (M.) . Chromium Sulphides . . . . . . . .SCHONE (E.). Atmospheric Ozone . . . . . . . .VARENNE CL.) . .WILLM (E ) . . . . .ENGEL (R.). Platinous Hypophosphite . . . . . . .SCHACHEBL (G.). Boiling Point of Chlorine Tetroxide . . . .Action of Hydrofluoric Acid on Ammonium DichromateSeparation of the Metals of Platinum OresPAGEI S18191920202 0212121222324727.27374757313813%13813813914014014114114.12212212212212222222232232232242242242242252252252262263453 4X CONTENTS.PAS EDENAR~AY (E.).Action of Chlorine on Nitrogen Sulphide . . . . 346FREIDEL (C.) and E. SARASIN. Artificial Production of CrystallisedQuartz . . . . . . . . . . . . . 346BERTRAND (A.) .Trichloride . . . . . . . . . . . . 34'7DITTE (A.). Action of Hydrochloric Acid on Metallic Chlorides . . . 347BBKBTOFF. Combination of Sodliim Oxide with Carbonic Anhydride, andAction of Sodium on Mercuric Oxide . . . . . . . 348RAOULT (F. M.). Action of Dry Carbonic Anhydride on Quicklime . . 348SORET (J. L.).Cerium Groups . . . . . . . . . . . 349THALBN (R.). Spectrum of Thulium .. . . . . . . 349CLEVE (P. T.). Erbium . . . . . . . . . . 350DUMAS. Gases Occluded in Aluminium and Magnesium . . . . 350MEUNIER (S.).Alkaline Silico-aluminates . . . . . . . . . 350HEUMANN (K.). Some Ultramarine Compounds . . . . . . 351MEUGEOT (A.). Formation of Permanently Green Crystals of ChromicChloride . . . . . . . . . . . . 352WYROUBOFF ((3.). Potassium and Ammonium Tetrachromates . . . 352BOURGEOIS (L.). Preparat,ion of Crystallised Chromates . . . . 352HANNAY (J. B.). Artificial Formation of Pgrolusite . . . . . 353E'UEST (E.). Action of Chlorine Tetroxide on Potassium Permanganate . 353BROGGER (W. C.). Two Furnace Products . . . . . . . 353BRAHAM (P.). Silver Sulphate . . . . . . . . . 354WINKLER (C.). Recrystallisation of Argentiferous Bismuth .. . 354KBUTWIG (J.). Action of Chlorine on Inorganic Silver Salts . . . 354DITTE (A.). Compounds of Hydrochloric Acid with Mercuric Chloride . 355BRAHAM (P.). Analysis of a Crystalline Mercury Salt . . . . . 355THURNLACKH (K. G.) . Chlorine Trioxide , . . . . . . 506LEEDS (A. R.) . The Invariable Production, not only of Ozone and HydrogenPeroxide, but also of Ammonium Nitrate, in the Ozonation of PurifiedAir by Moist Phosphorus . . . . . . . . . 506COLDSCHMIDT (H.) . Gay-Lussac's .Hypochloronitric Anhydride . . . 506HAMPTON (F). Existence and Properties of Phosphorus Yentiodide . . 50'7REINITZER (B.). Solid Compounds of Boron and Hydrogen . . . 507"ROOST (L.) and P. HAUTEFEIJILLE. Preparation of Silicon Oxychlorides .508BERNTHSEN (A.). Composition of Sodium Hyposulphite . . . . 508SMITH (W.) and W. T. LIDDLE. Nature of the lnsoluble Form of SodaExisting in the Residue left on Causticising Sodium Carbonate withLime . . . . . . . . . . . . 508FOLKARD (C. W.) . Crystallised Double Sulphata of Calcium and Sodium . 509BAKER (A. L.).Strontium . . . . . . . . . . . . 509ENDEMANN (H.). Composition of Ultramarine . . . . . . 509NILSON (L. F.) and 0 YETTERSSON. Properties and Chemical Characters ofGlucinum . . . . . . . . . . . . 511PHIPSON (T. L.). Rusting of Iron . . . . . . . . 512HOGLAN (P.). Stability of Calomel . . . . . . . . 512COOKE (J. P.). Atomic Weight of Antimony . . . . . . 512ALLEN (C. L.). Incaudescence of Cupric Antimonate when heated strongly 513COOKE (J.Y.). Oxidation of Hydrochloric Acid Solutions of Antimony in theAtmosphere . . . . . . . . . . . . 5 13SEUBERT (K.). Atomic Weight of Platinum. . . . . . . 514WILM (T.). Chemistryof the Platinum Metals . . . . . . 514MICHAELIS (A.) and P. BECKER. 682MARSDEN (R. S.). Preparation of Adamantine Carbon or Diamond . . 682SCH~TZENBERGER (P.). Sodium Hyposulphite . . . . . . 682XDER (J. M.). Ammonium Bromide . . . . . . . . 6821)ELB'rTRE (c.). Decomposition of Bicalcium Phosphate . . . . 683Combination o€ Titanium Tetrachloride with PhosphorusAbsorption Spectra of some Metals of the Yttrium andSynthetic Production of Native Silicates of Alumina andAmount of Water of Crystallisation of Hydrated Nitrate ofAttempts to Prepare Boron OxytrichloridCONTENTS .X1LE CHATELIER .SILBER (P . G.).MOISSAN (H.).Crystalline Hydrated Barium Silicate . . . . .Sodium Aluminium Silicates formed by the Action ofSodium Carbonate on Kaolin . . . . . . . . .Preparation and Properties of Chromous Chloride and Sul-phate . . . . . . . . . . . . .MOISSAN (H.). Chromous Bromide, Iodide. and Oxalate . . . .RAMMELSBERGF (C.). Molecular Properties of Tin and Zinc . . . .Temperatures . . . . . . . . . . . .Low (0.). Free Fluorine in Fluorspar . . . . . . . .DITTE (&4.). Action of Hydrochloric Acid on Metallic Chlorides . . .ZIMMERMANN (C.). Uranates . . . . . . . . .SCENEIDER (R.). Behaviour of Iodine and Arsenious Sulphide a t HighSTRECKER (K.). .BEBTHELOT .Solution of Chlorine in Water . . . . . . . Specific Heat of Chlorine, Bromine, and Iodine GasesHAUTEPEUILLE (P.) and J . CEAPPUIS . Liquefaction of Ozone in presence ofHART (P.). Sulphuretted Hydrogen Appwatus . . . . . .TOMMASI (D.). .DITTE (A.). Action of Chlorine and Hydrochloric Acid on Lead Chloride .MALLARD (E ) . Crystalline Form of Spiegeleisen . . . . . .PICKERIKG (S . U.). Oxides of DiIanganesz . . . . . . .BERTHELOT . Spontaneous Oxidation of Mercury and other Metals . .GUENOE . Isodimorphism of Arsenious and Antimonious Oxides . . .MATTHEY . Preparation of Platinum . . . . . . . .CAILLETET (L.) and P . HAUTEPEUILLE . Densities of Liquid Oxygen,MUNTZ (A.) and E . AUBIN . Propovtion of Carbonic Anhydride in the Air .MAUMENB (E .J.). . . . . .CASAXAJOR (P.). Sulphuretted Hydrogen . . . . . . .BERTHELOT . Heat of Vaporisation of dulphuric Anhydride . . .B ~ T H E L O T . Hydrochlorides of Metallic Chlorides, and the Reduction ofChlorides by Hydrogen . . . . . . . . . .LESCCEUR (H.). Hydrates of Calcium Chloride . . . . . .RAOULT (F . M.). Action of Carbonic Ariliydride on Barium and StrontiumOxides . . . . . . . . . . . . .LOIR (A.). Crystallisation of Alums . . . . . . . .RAMANN (E.). Decomposition of Water by Metallic Iron . . . .KLEIN (D.). Sodium Tungstoborate . . . . . . . .KLEIN (D.). Cadmium Tungstoborate . . . . . . . .KLEIN (D.) . Titanotungstates . . . . . . . . .YARMENTIER (F.) . Silico-molybdates . . . . . . . .RUYSSEN (F.). and E . VAREXNE . Solubility of Silver Chloride in Hydro-chloric Acid .. . . . . . . . . . .MERZ (V.) and W . WEITH . Amalgams . . . . . . .RUYSSEN (F.) and E . VARENNE . Solubility of Mercurous Chloride in Hydro-chloric Acid . . . . . . . . . . . .RESIONT (A.). Actioe of Flame on Platinum . . . . . .TROOST (L.). New Compounds of Hsdrobromic and Hydriodic Acidswit. h Ammonia . . . . . . .MALLET (J . W.). Molecular Weight oi Hytkofluoric Acid . . . .ARSISTEOSG (G . F.). Diurnal Variation of Carbonic Anhydride in the Air .YAPASOGLI ((2.). Action of Carbonic Acid on Potassium Iodide and onBERNTHSEN (A.) . Sodium Hyposulphite . . . . . . .SCH~TZENBEROER (P.). Hyposulphurous Acid . . . . . .DEMARQAY (E.). Some Compounds of Sulphur and Nitrogen . . .DITTE (A.). Action of Lead Peroxide on Alkaline Iodides .. . .NOBLE and F . A . ABEL . Note on the Existence of Potassium Thiosulphate . . . . . .Carbonic Aiihydride ; its Colour in the Liquid State . . . .Action of Potassium Nitrite on Ammonium Chloride .ILES (M . W.). Lead Chlorobromide . . . . . . . .Hydrogen, and Nitrogen in Presence of Inert Liquids . . . .Action of Nitric Acid on MetalsOzonoscopic Papers . . . . . . . . . .in the Solid Residue of Fired GunpowderPAGE68368468468568568668678478417857857867877887887897897897917917928748758768768768778788788788798798798808808808b18818829729%9749759769769769769'7xii CONTESTS.TOMMASI (D.). Decomposition of Sodium Salts by Cuprio Hydrate , .PRECHT (H.) and B.WITTJEN. Solubility of Mixtures of Salts of theAlkalis and Alkaline Earth Metals . . . . . . . .ANDRB. Strontium and Bari-inn Oxychlorides , . . . . .DELAFONTAINE. Decipium and Samarium . . . . . . .LIMOUSIN (S.). Esplosion in preparing Oxygen . , . . . .FILHOL (E.) and SENDERENS. Action of Sulphur on Certain Metallic Snlu-tions . . . . . . . . . . . . .WINKLER (C.). Amount of Sulphuric Anhydride in Fuming SulphuricAcid . . . . . . . , . . . . .CURTIUS (T.). Contribution to the Knowledge of the Poljthionic Acids con-tained in Wackenroder's Solution . . , . . . .CAMERON (C. A.) and E. W. DAIT. New Selenium Compounds . . .FILHOL (E.) and SENDERENS. A New Series of Phosphates and Arsenates .DITTE (A.).Solubility of Silver in Presence oi' Iodides . . . .ENGEL (M.) and J. VILLE. Solubility of Magnesium Carbonate in WaterCharged with Carbonic Acid . . , . . . . . .BOISBAUDRAN (L. DE). Anhydrous Gallium Chlorides. . . . .PHIPSON (T. L.). Actiniixm, a New Metal . . . . . . .REMSEN (I.). Conduct of Finely Divided Iron towards Nitrogen. . .CHRISTENSEN (0. T.). Chromammonium Compounds . . . . .PORUMBARU. Cobaltamines. . . . . . . . . .LEEORT (J.). Action of Arsenic and Phosphoric Acids on Sodium Tung-states . . . . . . . . . . . . .AXAGAT (E.) . Action of Oxygen on Mercury at the Ordinary Temperature .Min,eralogicab Chemistry.ROSIXI (B.). The Zundererz or Tinder Ore of Clausthrtl . . . .BUCKING (H.). Freislebenite from Hiendelaencina, Spain .. . .STRENG (A.). Quartz from the Eleanor0 Mine, on the Dunstberg nearGiessen . . . . . . . . . . . . .ERHAKD (T.) and A. STELZNER. Fluid Enclosures irn Topaz . . .BERTRAND (E.). Andalusite from Brazil . . . . . . .SCHULTEN (A. DE) . Artificial Analcime . . . . . . .ROTH (L.). A New Occurrence of Gismondine . . . . . .CORSI (A.). Occurrence of Prelinite in Tuscany , . . . . .DOLTEX (C.). Acmite and Aegerine . . . . . . . .LORETZ (H.). Dolomite of South Tyrol . . . . . . .WOLF (F. M.). Examination of Melaphyr from the neighbourhood ofKleinschmalkalden . . . . . . . . . . .HANSEL (V.). Petrographical Constitution of the Monzonite of Predrazzo .TORNEBOHN (A. E.). The Ferruginous Rocks of Ovifak and Assuk . .SMITH (J. L.). A New Meteoric Mineral .. . . . . .REICHARDT (E.). Examination of the Grossliider Mineral Spring at Salz-schlirf . . . . . . . . . . . . .HULWA (F.). Analysis of the Kanizer or Kainzen Spring . . . .BURI (E.). Analysis of the Mineral Water of Niederbronn in Unter-ElPass .DELACHANAL. The Hot Spring a t Bagnoles de l'Orne, and the DepositsFormed in the Conduits . . . . . . . . . .SCHMELCK (L.). Results of the Norwegian North Sea Expedition . .PRECHT (H.). .DAUBRBE. Conteinporaneous Production of Native sulphur in the Subsoil ofParis . . . . . . . . . . . . .HOCHSTETTER (F. v.). Covellin occurring as Encrusting Pseudomorph on aBronze Celtic Axe found on thesalzberg . . . . . .CLARKE (F. W.) and MARY E. OWENS. .BRAUN (J.1. Nickel Sueiss . .. . . . . . . .Formation of Hydrogen in the Stassfurt Potash Mines.A new Form of Tetrahedrite .PAGE91759789'79979109710971097109810991101110111021103110 E110411104411061107110CONTENTS .BRTXH (G . J.) and E . 8 . DANA . Two new Mineral Species from FairfieldCo., Comecticut . . . . . . . . . . .RAMMELSBERO (C.). Composition of Kjerulfin . . . . . .RATH ((3 . v.). Mineralogical Contributions . . . . . . .ZEPHAROVICH (V . v.). Mispickel, FeSAs. from Pribram . . . .ZEPHAROVICH (V . v.). Halotrichite and Melanterite from Idria . . .TSCIIERNAK (G.) and L . SIP~CZ . TheClintonite Group . . . .COSSA (A.). Green Garnet from Val Maleneo . . . . . .LINDSTROM (G.). Thaumasite, a New Mineral from Aareskutan . . .SCHRAUF (A.) . Eggonite .. . . . . . . . .LASSAULX (A . v.). Mineralogical Notices . . . . . . .Fall of Meteorites at Gnadenfrei, in Silesia . . . . . . .DAUBRBE . Products from a Crater . . . . . . . .DAUBRBE . Action of Mineral Waters on Metals . . . . . .PFAFF (F.). Variability of the Angles of Crystals . . . . .JANNETTAZ (E.). Colours of the Diamond in Polarised Light . . .INOSTRANZEFF (A.). A New Variety of Native Carhon . . . .DOLTER (C.). New Resin from Eoflach, in Styria . . . . .RICHARD (A.). Minerals of the Sarrabus Mine, Sardinia . . . .HIDEGH (K.). Chemical Analvsis of Hungarian Fahl-ores . . . .COLLINS (J . H.). Crystophite‘from St . Agnes. Cornwall . . . .MALLET (J . W.). Chemical Composition of Guanajuatite . . . .NORDENSTROM (G.).Occurrence of Anthracite in an Iron Mine in Norberg,Sweden . . . . . . . . . . . . .BRUSH (G . J.) and W . J . COMSTOCK . American Sulpho-selenides ofMercury . . . . . . . . . . . .WEISBACH (9.). Mineralogical Notices . . . . . . .SADEBECK (A.). The Crystal System of Manganite . . . . .ALLEN (0 . D.) and W . J . COMSTOCE . Bastnasite and Tponite fromColorado . . . . . . . . . . . .PENPIELD (S . I,.). Analyses of some Apatites containing Manganese . .BRUSH ( G . J.) and E . S . DANA . Relation between Childrenite andEosphorite . . . . . . . . . . . .DAMOUR and DES CLOIZEAUX . Hopeite . . . . . . .PRIEDEL C . and E . SARASIN .SCHRAUF (A.) . Phosphorised Copper Ores . . . . . . .LINGER (S.). Sulphates occurring in the Bauersberg, near Bischofsheim .COSSA (A.).Rutile in Gastaldite-Eclogite from Val Tournanche . .LASAULX (A . v.). Titanomorphite, a new Calcium Titanate . . .~)OLTER (C.). Constitution of the Pyroxene Group . . . . .BAUER (M.). Barsowite . . . . . . . . . .DAMOUR (A.). Xote on a Chromiferous Garnet, found on the Pic Posets,near the Maladetta (Pyrenees) . . . . . . . .BERWERTH (F.). Nephrite and Bowerite from New Zealand . . .GONNARD (F.). A new Locality of Szaboite . . . . . .I)AMOUR (A.). Note on yenasquite . . . . . . . .BAUER (M . 0.). .LASAULX (A . v.). Idocrase from Gleinitz and the Johnsberg, near Jordans-miihl . . . . . . . . . . . . .SIIEPARD (C . U.). Mineralogical Notices . . . . . . .If-4UGHTON (8.). .FUIEDEL (C.) and E . SARASIN .Artificial Production of a Felspatliic Sub-stance . . . . . . . . . . . . .COSSA (A.). Corundiferous Felspar of Biella in Piedmont . . . .~ICDDLE (M . F.). Hauzhtonite . a new Mica . . . . . .KRENNER ( J . L4.). Telluric Silver from BotAs, in Transylvania . . .YENFIELD (S . L.). Chemical Composition of Childrenite . . . .BAUEX (M.). Kjerulfin . . . . . . . . .Artificial Libethenite . . . . .GENTH (F . A.). P-jrophillites from Schuykill Co., Pennsylvania . . .Parallel Combination of different Varieties of EpidoteSJOGREN (H.). Pyroxene from Nordmark in Sweden . . . . .Mineralogy of the Counties of Dublin and Wicklow .... XlllPAGE2292302313593593593603603613613623643643643643653653663663673683693703’7137137537637737837837937938038138138238338438XiV CONTENTS .HAUSHOPER (K.).Oligoclase from Diirrmosbach . . . . .AN~ELBIS (C.). The Picrites of Nassau and the Labradorite Porphyries ofHAUGHTON (T . S.). . . .COSSA (A.) . . . .FOUQUB (F.). Hypersthene from the Pumice of Santorin . . . .HAUTEFEUILLE (P.) . A Potassio-ferric Silicate analogous to Leucite . .COLLINS (J . H.). Penwithite, a new Cornish Mineral . . . . .ATTWOOD (G.). A Contribution to South American Geology . . .GUMBEL (C . W.). Fossil Plants from the Carboniferous Strata of theTarentaise . . . . . . . . . . . .GUNBEL (C . W.) . Rocks of Kecgnelen’s Land and the neighbouring IslandsMARTIN (K.). Phosphoritic Limestones of the Island of Bonaire, WestIndies .. . . . . . . . . . . .COHEN (E.). .v . KOENER . Pumice from Launsbsch . . . . . . . .DAUBREE . Examination of the Material of some French “ Vitrified Forts ” .HIDDEN (W . E.). Meteorite from Cleborne Co., Alabama . . . .SEEPARD (C . U.). Meteoric Iron from Ivanpah, California . . . .SHEPARD (C . U.). Meteorite of Estherville, Emmet CO., Iowa . . .SMITH (J . L.). The Emmet Co . Meteorite . . . . . . .GALLE (J . (3.) and A . v . LASAULX . Pall of Meteorites a t Gnadenfrei inSilesia . . . . . . . . . . . . .HOUZEAU (A.) . Amount of Iron in the Mineral Waters of Rouen andSELIGMEN (G.). Crystallographic Notices . . . . . . .Westphalia . . . . . . . . . . . . .Note on an Olivine-gabbro from CornwallPeridotiferous Diabase of M osso in the BielleseLavas from Hawaii and other Islands of the Pacific OceanForges les Eaux .. . . . . . . . . .WEISBUCIT (R.). Crystalline Form of Leucite . . . . . .BAUMHAUER (R.). Artificial Calcspar Twins . . . . . .ZEPBAROVICH (V . v.). Enargite from the Muntzenkopf, near Brixlegg, inTyrol . . . . . . . . . . . . .SELLA (Q.). Crystalline Forms of the Anglesites of Sardinia . . .BSUMHAUER (H.) and E . MALLARD . Boracite . . . . . .DES CLOIZEAUX (A.). On the Monoclinic Form to which Epistilbite shouldbe referred . . . . . . . . . . . .ARZRUNI (A.) . Coquimbite . . . . . . . . . .SCEUSTER (M.). Optical Orientation of Plagioclases . . . . .RUMPF (J.). Crystalline Structure of Apophyllite . . . . .BAUMHAUER (H.). Perowskite .. . . . . . . .ZEPHAROVICH (V . v.). Crystalline Form of Silver Iodide . . . .ENOP (A.) . Artificial Production of Hollow Pseudomorphs . . .~ O H L E R (F.). Remarks on the Native Iron of Greenland . . . .HABERMEHL (H.). Composition of MngneticPgrites . . . . .CANENGE (E.). Gtuejarite: a New Mineral Species . . . . .FRIEDEL (C.) . Crystalline Form of Guqjarite . . . . . .BAHEX (A . L.). Artificial Production of Livingstonite . . . .PREDA ((3.). dntimonious Acid, a Vesuvian Product . . . . .LOVISATO (D.). The Kinzigites of Calabria . . . . . . .BECKE (F.). Twin-formation and Optical Properties of Chabasite . .LIEBISCII (T.) . Analytical Geometric Treatment of Crystallography . .PAGE (W . T.).PAGE (W . T.).Cox (E . T.).Examination of Livingstonite from a New Mexican LocalityExamination of an Altered Livingstonite from Guadalcizar ..Extensive Lodes of Antimony Oxide a t Sonora, Mexico .SCEULZE (H.) and A . STEINEIL . Conversion of the Distillation Vessels ofXOESCHAROW (N . VON) . Materials for the Mineralogy of Russia . .BABCOCK (S . M.). Celestine from the Musclielkalk of Jiihnde, nearOottingen . . . . . . . . . . . .Zinc Furnaces into Zinc-spinelle and Tridymite . . . . .PATERN& (E.). Analysis of Native Sodium Sulphute from Sicilp . . .BREZINA (A.). Herrengrundite, a New Basic Copper Sulphate . . .IIOFFMANN (C.). Canadian Apatite . . . . . . . .PAGE38638738838838838938939039039139139239339439439439539539539739739739739739739739739739730739839839539851551551651751751751751851851851052052352452452452CONTEXTS .ZiYPAGE(&men . . . . . . . . . . . . . 52.5MASSIE (F . A.). Composition of Dufrenite from Rockbridge. Co., Va . . 529BRUSH (G . J.) and E . S . DANA .Connecticut . . . . . . . . . . . . 529BREZINA (A.). Autunite . . . . . . . . . . 531LINDSTROM (G.). Hedyphane containing Baryta. from Laangban . . 531NIES (A.). Two New Minerals from the Eleonora Mine. on the Dunsberg. nearSTRENa (A.) . The Phosphates of Wddgirmes . . . . . . 525Two new Mineral Species from Fairfield.SCHRAUF (A.). Arsenates from Joachimsthal . . . . . . 532NORDSTROM (T.). Analyses of Minerals . . . . . . . 532RAMYELSBERG (C.).Chemical Composition of the Micas . . . . 533COSSA (A.). Euphotide of Elba . . . . . . . . . 53’7MASSIE (€7 . A.). Aiialyses of Amphibole from Amelia Co., Va . . . .LOSCH (A.). Lime Iron Garnet from Syssertzk in the Urals . . . 538BECKE (F.). Hypersthene from Bodenmais . . . . . . . 539HELMHACKER (R.). Minerals of the Clay Group . . . . . 540Ottawa Co., Quebec . . . . . . . . . . ,542,LASPEYRES (H.). Mineralogical Observations . . . . . . 543SCHARIZER (R.). Notices on Some Austrian Minerals . . . . . 544HOFFNANN (C.) . Canadian Minerals . . . . . . . . 545RATH (G . v.). Contributionq to Mineralogy . . . . . . 548538RAYMOND (R . W.). The lhnite of the Jenks Mine. Macon Co., N .Minerals of some of the Apatite-bearing Veins ofCarolina .. . . . . . . . . . . . 540EARRINGTON (B . J.).COHEN (E.). (( Eklogite” which occurs in the Diamond Mines of Jagers-fontain . . . . . . . . . . . . . 552DOLTEX (c.). Chemical Composition of Arfvedsonite and some AlliedMineral . . . . . . . . . . . . . 552BAEER (A . L.). Analysis of a Perruginous Mineral from Anihurst Co., Va . 554PAGE (W . T.). Analysis of a Highly Aluminous Pyroxene from AmhurstCo.,Va. . . . . . . . . . . . . . 554RATH (G . v.) and A . DAMOUR . Kentrolite. a New Mineral Species from Chili 554WIXKLER ((2.). Examination of the Iron Meteorite from Rittersgrun . . 560SMITH (J . L.). The Meteorite which fell a t Estherville. U.S.A. . . . 561~ILVESTRI (0.). Meteoric Dust containing Metallic Iron which fell atCatania. 29th March.1880 . . . . . . . . . 561ADAMS (F . D.). Analyses of the Waters of the Assiniboine and Red Rivers.Canada . . . . . . . . . . . . 562BOUSSINGAULT . The Hot Spring of the Littoral Chain of Venezuela . . 563564LIVERSIDQE (A.). Water from a Hot Spring. Fiji Islands . . . . 564CHAPER (M.).United States . . . . . . . . . . . . . 687PIESZCZEK (E.). New Fossil Resins from East Prussia . . . . 687BUCIINER (\I.). Boqhead Coal from Resiutta . . . . . . 688SJOGREN (H.). Some Bismuth Minerals from Nordmark in Wermland . 688BLAKE (W . P.). Occurrence of Cinnabar in California and Nevada . . 689FOUQUB (F.). Santorin and its Eruptions . . . . . . . 555LIVERSIDGE (A.). Water from a Hot Spring. New Britain . . . .LIVERSIDQE (A.). Formation of Moss-gold and Silver .. . . . 687Mode of Occurrence of Gold in Certain Minerals from theROLLAND ((3.). Occurrence of Mercury in California . . . . . 689URBA (K.). Analysis of Frieseite . . . . . . . . . 689THOULET (J.). Note on Chrome-iron . . . . . . . . 690MALLARD (E.) .690SJOGREN (H.). Manganese-calcium Carbonate containing Barium . . 690RAFFELT (R.). Aluminite from Muhlhausen. near Krulup in Bohemia . 691DES C ~ o ~ z s a u x and A . DAMOUR . Chalcomenite. 8 New Mineral . . 691DES CLOIZEAUX and A . DAXOCR . Note on Cabrerite from Laurium . . 691BAUNHAUER (H.). Note on Mica. more especially Zinnwaldite . . . 692Production of Crystallieed Iron Phosphide and of Anor-thite by the Fires in the Coal Beds at Commentry . . . . .FILHOL (E.). Felspars from the Valley of RagnBres-de-Luchon .. . 69xvi CONTENTS .VBLAIN (0.). Microscopical Study of the Glasses resulting from the Fusionof the Ashes of Grass. &c . . . . . . . . . .COSSA (A.). Serpentine from Verrayes. in the Valley of Aosta . . .DAXOUR (A.). Note on Titaniferous Peridote from Zermatt . . .JOIIN (K.). Halloysite from Tuffer . . . . . . . .SELIGMANN (G.). Russian Topaz and Enstatite from Snarum . . .DOELTER (C.). Spodumene and Petalite . . . . . . .GRENER (L.). Artificial Pyroxene (Diopside) . . . . . .LIVERSIDGE (A.). Stilbite from Kergueleii’s Island . . . . .HUSSAK (E.). The So-called “ H-jpersthene-Andesite” from St . Egidi, LowerStyria . . . . . . . . . . . . .FRESEKIES (W.). Phillipsite and its Relations to Harmotome and Desmin .DAMOER (A.).Note on Zinc-Spinelle from Brazil . . . . .WALLER (J.). Analysis of Demantoid from the Urals . . . . .BOEQU~ (F.) and A . M . LBVP . Artificial Production of Opbitic Structure .S ~ i i a REN (A.). Mineralogical Notes . . . . . . . .HJORTDAHL (T.). Mineral Anahses . . . . . . . .SCHUMACHER (E.). The Maintain Group of the Rummelsberg, nearStrehlen . . . . . . . . . . . . .DORLTEE (C.). Occiimence of Propylite in Transylvania . . . .KA LKOWS KY (E . ) . Pipern o . . . . . . . . . .ECKENBRECRER (C . v.). .LECEARTIER (G.). .DOELTER (C.). Products of the Volcano, Monte Ferru . . . . .HAWES (G . W.). A Group of Eruptive Rocks in Campton, New Hamp-shire . . . . . . . . . . . . .WICHMANN (A.). Some Lavas from the Island of Niuafou .. . .RICCIARDI (L.). Lavas from the Neighbourhood of Catania . . .Kocn (A.). Mineral and Rock Enclosures in the Basalt of the PersanyerGebirge . . . . . . . . . . . . .DAEBRBE . Examination of the Material of “Vitrified Forts” a t CraigPhadrick. Inverness . . . . . . . . . .SMITH (J . .L. ). Anomalous Magnetism of the Meteoric Iron a t Sainte-Catherine . . . . . . . . . . . .SMITH (J . L.). .111x0~ (W. A.). Inorganic Constituents of the Coals OP New SouthWales . . . . . . . . . : . . .DUDLEY (W . L.) and F . W . CLARKE . Graphite from Ducktown, in Ten-PISCRER (H.). Miscellaneous Contributions to Microscopical Mineralogy .Changes produced by Weathering of PhonolitePresence of Phosphorus in the Rocks of Brittany .Nodules of Chromite in Meteoric Iron from CohahnilaLIVERSIDGE (A.).Composition of New South Wales Coals . . .nessee . . . . . . . . . . . . .LIVERSIDGE (A.). New South Wales Minerals . . . . . .ZEPH~ROVICH (V.) . Mineralogical Notices . . . . . . .CORNWALL (H . B.). Gallium in American Blendes . . . . .DOMEPKO (I.). Bismuth Ores of Bolivia, Peru, and Chili . . . .DEWALQUE (F.). Diadochite from the VBdrin Mine . . . . .Pey chagnard . . . . . . . . . . . .GIRA~~DON (J.). Artificial Production of Vivianite . . . . .DOMEYKO (I.). Crystals of Metallic Copper from the Mines of Coro.Coro,Bolivia . . . . . . . . . . . . .Fredricite. a Mineral resembling the Fahlerz from Falu . SJOGREN (H.).LENZECARNOT (A.).. . . . . . Calcspar in Basalt Tufa from Oweiier BolleTwo Varieties of Diadochite found in the Coal Mine a tBERTRAN-D (E.) and A .E . NORDEBSKIOLD .RAMMELSBERG (C.) .WEBSKY .\\VEBSKP .Thaumasite and Melanophlo-gite . . . . . . . . . . . . .Composition of Descloizite and the Natural VanadiumConipo im ds in general . . . . . . . . . . . . . . . . . Crystalline Form of DescloiziteCrystalline Form of Vanadinite from Cordoba . . . .I)TTNNIKGTOX 1%’. P.). Microlite from Amelia Co., Virginia . . . .PAQE692693693693694694694695695695696697697697698698698699700700700701701701703’703704705980983989990991995997997998998998999999100010001000100110021002 ........... \ I . v COKTENTS. s viiSTRUVER (J.).Perowskite of Val Malenco . . . . . . .RICCIARDI (L.). On Flint . . . . . . . . . .RANNELSBERG ((3.). Composition of Pollucite from Elba . . . .MICHEL-LETT (A.). Sillinianite in the Gneiss of the Norvan . . .JULIEN (A. A.). Spodumene and its Alterations . . . . . .BLONSTRAKD (C. W.). Arctolite, a Mineral from Spit~bergen . . .LUEDECKE (0.). Mesolite and Scolecite . . . . . . .COLLIER (P.). Analysis of a Mineral resembling Thorite . . . .GRATTAROLA (G.). Rosterite, a New Variety of Beryl from Elba . . .LIVERSIDQE (.4.), Composition of some Coral Limestones, &c., from theSouth Sea Islands . . . . . . . . . . .COSSA (A). Composition of Tuscan Serpentines . . . . . .RCKENBRECRER (C.) Metamorphoses of Nepheline Rocks . .. .HOPFNER (C.1. The Rock of Monte Tajumbina, in Peru . . . .ARKOLD (A. 2.). .CARNOT (A.). A Volcanic Breccia . . . . . . . .HARRIS (W. E.). A New Meteoric Iron from North Carolina . . .DAUBRBE (A.). On a Meteorite which fell on Nov. 36, 1874, at Kerilis,CGtes-du-Nord . . . . . . . .MEUKIER (S.) . Litliological and Geological Examination of a Meteoritewhich fell 15th Oct., 1872, near Soko-Banya, Serria . . . .MEUNIER ( S . ) . Synthetic Imitation of Meteopic Nickel-iron . . .DIEULAFAIT. Law of the Formation of Saline Mineral Waters . . .MUGGE (0.). Felepar from the Rhombic Porphyry of Christiania . .HANNAT (J. B.). On the Artificial Formation of the Diamond . . .DIEULAFAIT. Esistence of Bormic Acid in Saline Lakes and NaturalSaline Waters .. . . . . . . . . . .ROMANIS (It.). .LIVERSIDGE (A.). Water of Hot Springs in New Britain and the FijiIslands . . . . . . . . . . . . .SILLIMAN (B .) . Mineralogical Notices . . . . . . . .HIDDEN (W. E.). Notes on Mineral Localities in North Carolina . .GENTH (F. A.) . ’ Spanish Minerals . . . . . . . .CAMPBELL (J. L.). Dufrenite from Rockbridge Co., Virginia . . .SHEPARD (C. U.). Meteoric Iron of Unknown Locality, in the SmithsonianMuseum . . . . . . . . . . . .JOHKSTOKE (W.). Chalybeate Spring, Kingstead, St. Edmunds . . .VILLE (J.). Ferruginous Carbonated Waters . . . . . .‘hCHERNAK and SIPOCZ. ZO’iSite . . . . . . . . .Note on a Crptallised Slag isomorphous with OlivineHot Spring at Nnbmoo, near Manlmnin, British Burmah0 rg anic Chemistry .VILLIERS (A.).Etherification of Hpdrobromic Acid . . . . .FORCRAND. Hydrate of Methyl Iodide . . . . . . .LIEBERXABN (C.) and L. LANDSHOFF. Compound of Ether with PhosphorusPentachloride. . . . . . . . . . .J~VILLIER (E.). and A. BUISINE. Action 0; Methyl Bromide and MethylIodide on Monomethylamine . . . . . . . . .PLIMPTON (R. P.) . Amylamines from Inactive Amy1 Alcohol . . .BARBAGLIA (G. A.) . Thiovaleraldehyde . . . . . . .BARBAGLIA (G. A.) and P. GUCCI. Action of Chlorine on Di-isopropyl-ketone . . . . . . . . . . . . .BREDT (J.). Constitution of Lactones . . . . . . . .GIRARD (J.). Propylacetal and Isobutylacetal . . . . . .BARBAGLIA (G. A.) and P. GUCCI. Dry Distillation of Calcium IsobutyrateANSCHUTZ (R.) and W.PETRI. Itaconic Anhydride . . . . .ANSCHUTZ (R.). Decomposition of Citric Acid by Distillation . . .HILL (H. B.). Mucobromic Acid. . . . . . . . .MEXSCHUTKIN (N.). Influence of Isomerism of Alcohols on the Formationof Ethereal Salts . . . . . . . . . . .VOL. XL. 2,PhQE1002100310031005100510051006100710091009101110121013101510161016101710171017101810181019101910191019101911081109111011111111111211123236333333343434344353535363xviii CONTENTS .PAGEMENSCHUTKIN (N.) . Influence of Isomerism of Monobasic Saturated Acidson Etherification . . . . . . . . . . .MABERY (C . I?.) and H . B . HILL . Oxidation-products of DimethyluricAcid . . . . . . . . . . .. .BRE~RE . Conversion of Terebenthene into Cymene . . . . .ARMSTRONG (H . E.) and W . A . TILDEN . Remarks on Kelbe’s Discovery ofa New Cymene in Light Rosin Oil . . . . . . . .FRIEDEL (C.) and J . M . CRAFTS . Synthesis of Hexmethylbenzene and ofMellitic Acid . . . . . . . . . . . .LEHNE (A.). Paraditolylnitrosamine . . . . . . . .LEHNE (A.). Paraditolylhydrazine . . . . . . . .STEBBINS (J . H.). Azo-derivatives . . . . . . . .SCHULEI~UD (L.). Action of Hydrochloric Acid on Organic Amides . .REIMER (C . L.) . Alphatoluylamide . . . . . . . .VOLTZKOW (M.) . Phenjl and Tolylthiocarbimide-glycollide . . .BAMBERGER (E.) . Guanylthiocarbamide and some Guanylguanidines . .LIEBERMANN (C.). Constitution of the Thiourethanes . . . . .LIEBERMANN (C.) and S .NATANSON . Para- and Ortho-tolylthiouretlianes .MEYER (R.) and A . BAEER . Introduction of the Hydroxyl Group by directOxidation . . . . . . . . . . . .FITTICA (F.) . A Fourth Mononitrophenol . . . . . . .FITTICA (F.). New Nitrophenols . . . . . . . .REIMER (C . L.) . Action of Bromine on Benzyl Cyanide and on PhenylaceticAcid a t High Temperatures . . . . . . . . .BENDER (G.). Action of Ethyl Chlorocarbonate on Phenols . . .LORENZ (C.) . Methyleuecaffeic and Methylenehomocaffeic Acids and theirDerivatives . . . . . . . . . . . .HARMSEN (W.). Bitrometaxylenesulphonic Acid . . . . .JACOBSEN (0.) and H . LONNIES . a-Isophthalosulphonic Acid . . .JACOBSEN (0.). Anhydrosulphonamine-isophthalic Acid . . . . LONNIES (H.) . 7-Isopl~thalosulphonic Acid and y .Hydroxyisophthalic AcidFISCHER (E.) and H . TROSCHKE . Amarine and Lophine . . . .GIRAUD (E.) . Indoline . . . . . . . . . .MCHOEL (D . A.) . Derivatives of Anthraquinonesulphonic Acid . .HARRIOT (M.) and E . DOASSANS . A Substance from Thalictrum macrocar-pum . . . . . . . . . . . . .LIEBERMANT (C.) and TAECHERT . Catechin . . . . . .Derivatives of Santonin . . .STILLMANN (J . M.). Gum Resin from Arizona and CaliforniaDOASSANS (E.). Thalictrine . . . . . . . . . .CARNELETTL (G.) and R . NASINI . Alkannin . . . . . .CANNIZZARO (S.) and J . CARNELUTTI .MEYER (E . v.). Cyanethine, and New Bases derived from itCONTWCK (0 . DE) . Bases of the Pyridine SeriesJOBST (J.). Crystalline Quinoydine Borate . . . . .. .LADENBURG (A.). Hyoscine . . . . . . . . .. . .. . . . . . . . .HESEMANN (T.). Ptoma’ines considered in relation to Forensic Chemistryand Toxicology . . . . . . . . . . .WURTZ (A ) . Papa% . . . . . . . . . . .TENABLE (F . P.). Derivatives of the Heptane from Pinus sahinia.raa . .HOPPE-SEYLER (F.). Fermentation of Glycerol . . . . . .KOLBE (H.). Di- and Tri-carbinole . . . . . . . .EISENBERG (L . J.) . Methylamine in Commercial Trimethylamine Hydro-chloride . . . . . . . . . . . . .LIPP (A.). Some DeriFatives of Tsobutaldehyde . . . . . .PLOCHL (J.). Lead Formacetate . . . . . . . . .DUVILLIER (E.). Amido-acids of n-Hydroxybutyric Acid . . . .SCHREINER (L.). Two Remarkable Cases of Metamerism in Carbon Com-pounds . . . . . . . .. . . . .SCHEIBE (E.). Borocitrates . . . . . . . . . .THOMSEN (J.). Constitution of Benzene . . . . . . .39393940404141414243434344454546474-74848495050515 15 1515252525253535456565657588282828384868788888CONTENTS .KOHLER (H.). Action of Phosphorus Trichloride on Benzene . . .POST (J.).HR~~CENER (A . ) .JAHNS (E.).Action of Sulphuric Acid on the Substituted Nitro- and Amido-benzenes . . . . . . . . . . . . .Oxidation of Nitrogenous Methplated Benzene Derivatit-esSome Constituents of the Essential Oil of Origanum vulgareAction of Resorcinol on Ureaand Thymus Serpyllum . . . . . . . . . .BIRNBAUM (K.) and G . LURIE .LINE ((3.). Phloroglucol-phthale'in and Diresorcinol-phthale'in .. .BEYER (B.). Some Derivatives of Isophthalic Acid . . . . .SCHWARZ (H.), Preparation of Orcinolcarboxylic Acid . . . .SPIEGEL (A.). Vulpic Acid . . . . . . . . . .ROSENSTIEHL . Bayer's Process for the Synthesis of Indigotin . . .. . .PECHMANN (H . v.). Compounds of Orthobenzoylbenzoic Acid with PhenolsKOHLER (H.). Action of Phosphenyl Dichloride on some Chlorides . .LUNGE (G.) End T . STEINKAULER . New Hydrocarbon from Sequoia giganteaLIEBERMANN (C.) and L . LINDEMANN . Combinations of Anthracene withthe Oxides of Nit. rogen . . . . . . . . . .LIEBERMANN ((2.). Derivatives of Anthraquinone . . . . .SCHROTTER (H.). Reduction-products of Camphor . . . . .CECH (C . 0.). Coffee Oil . . . . . . .. . .SAALFELD (E.) . Yalembang Benzo'in . . . . . . . .TILDEN (W . A.). Light Rosin Oil . . . . . . . .ISSLEIB (M.). The Bitter Principle and Resin of Hops . . . .LLOYD (J . U.). Resin of Leptandra . . . . . . . .WARDEN (C . J . H.). Gloriosa superba . . . . . . .ALLEN (H.) . Vibui*nztm prunifolium . . . . . . . .HOLZHAUER (W . C.). Eriodictyon californicum . . . . . .HOLDEN (L . H.). Aralia spinosa . . . . . . . .PARSONS (A . B.) . Analysis of Damiana . . . . . . .REINSCH (H.). Coal . . . . . . . . . . .WULFSBERG (N.). Aspidospermine and Paytine . . . . . .HARNACK (E.). DitaYne . . . . . . . . . .HOOGEWERFF (S.) and W . A VAN DORP . LepidineGERICHTEN (E . v.). Apophyllic Acid . . . . . . . .HUFNER (G.). Researches on the Phjsical Chemistrj of Blood .. .Hydrocarbons . . . . . . . . . . .LIEBERMANN (C.) and R . KNIETSCH . Composition of Aesculin and Aescu-letin . . . . . . . . . . . . .. . . . .CECH (C . 0.). Investigation of the Processes of Decomposition occurringduring the Rotting of Eggs . . . . . . . . .JAHN (H.). Decomposition of Simple Organic Compounds by Zinc-dust .])EMOLE (E.). Action of Oxygen on the Bromo-derivatives of UnsaturatedTANATAR (S.). Preparation of Sodium Ferrocyanide . . . . .BANNOW (A.). An Isomeric Potassium Cyanate . . . . . .MENSCHUTEIN (N.). Influence of Isomerism of Glycols on the Formation oftheir Acetates . . . . . . . . . . . .LIEBEK and ZEISEL . Synthesis of Glycerol . . . . . . .MORAWSEI (T.). Lead Glycerides, and the Quantitative Estimation ofFERNBACH (A.).Action of Soda on Glycerol . . . . . .nfARKOWNIKOFF (w.). A Six-carbon Gtlycerol . . . . . .R~ENSCHUTEIN (N.) . Polyhydric Alcohols . . . . . . .TXIOMSEN (T.). Multiples of the Optical Rotary Powers of Carbohydrates .VINCENT (C.). Sorbin arid Sorbite . . . . . . . .LIPPMANN (E . 0 . v.). Inversion of Raw Sugar by Carbonic Acid, and someProperties of Inverted Sugar . . . . . . . . .LJPPMANN (E . 0 . v.). Presence of Saccharin in Osmosed Sugar . . .SCHEIBLER (C.). Saccharin and Saccharinic Acid . . . . . .ALLIHN (F.). Conversion of Starch into Sugar by the Action of Dilute Sul-pfiuric Acid at High Temperatures . . . . . . . .Glycerol . . . . . . . . . . . . .b 2xixPAQE919193959595969696979798989910010010010110110110310310410510510610710710810910911011011114114214314414414514514514614614714814814814914xx CONTENTS.LEFRANC.Specific Identity of Jnulins and of Natural Levulins . . .MEISSL (E.). Specific Rotatory Power of Lactose. . , . . .ERDMANN (E. 0.). Anli~drous Nilk-sugar . . . . . . .SCHMOEGER (M.). A Hitherto Unobserved Property of Milk-sugar . .MORLEY (H. T.) . Isopropylene-neurine . . . . . . .RENOUF (E.) . Dimethylhgdrazine . . . . . . . .CAZENEUVE (P.). .CLAISEN (L.) and P. J. ANTWEILER. Some Derivatives of TrichloracctjlCyanide . . . . . . . . . . . . .MELIKOFF (P.). Formation of a- and P-Chlorolactic Acids . . . .CLAISEN (L.) and E. MORITZ.Propionylformic Acid . . . . .BOURGOIN (E.) Action of Bromine on Malonic Acid . . . . .HJELT (E.). .MARKOWNIKOFF (W.) . Itaconic Anhydride . . . . . . .BOTTINGER (C.). Behaviour of Glyoxglic Acid with Potash . . . .BOTTINGER (C.). Formation of Uvic (Pprotritartaric) Acid. . . .BISCHOFF (C. A.). Synthesis of Tri- and Tetra-basic Fatty Acids . .KEKUL~ (A.) and R. ANSCHUTZ. Tanatar’s Dioxyfuniaric Acid . . .CLARKE (F. W.) and H. STALLO. Constitution of Taytar-emetic . . .TANRET (C.). Ferrous Sucrocarbonate . . . . . . . .LATSCHINOFF (P.). On Cholic Acid containing Solid Patty Acids. . .MICHAELIS (A.). Ethyl Yhosphodicliloride, and its Homologues . . .TROMSEN (J.). Formula of Benzene . . . . . . . .BEILSTEIN (F.) and A. KURBATOW. Nature of Caucasian Petroleum ..BEILSTEIN (F.) and A. KURBATOW. IIydrocarbons from American Petro-leum . . . . . . . . . . . .SCHOOP (P.). Action of Dimethylaniline on Ethjlene ‘Bromide and Acetyl-ene Tetrabromide . . . . . . . . . . .STEBBINS (J. H.) . Action of Nitroso-dimet?iylaniline Hydrocliloride on thePhenolsulphonic Acids which do not contain the Methyl Group .LIPPMANN (E.) and R. LANGE. Condensation of Tertiary Bases by NitricOxide . . . . . . . . . . . . .FISCHER (E. and 0.). Rosaniline. . . . . . . . .HEUMANN (K.). Nomenclature of Some Azo-compounds . . . .LAUBENHEIMER (A.) and R. GORING. Hydrocyancarbocliphenylimide .HIRSCH (A.). Quinonechlorimide and Similar Substances . . . .ELANDER (S. U.). Action of Sulphonic Chlorides on Urea .. . .DOEBNER (0.). Compounds of Beazotrichloride with Phenols and TertiaryAromatic Bases . . . . . . . . . . .HANTZSCH (A.) . Parahydroxyphenol and Some Aldehydes and Alcoholsderived from Quinol . . . . . . . . . .TONNIES (P.). Action of Nitrous Acid on Anethol . . . . .LA COSTE (W.). Arsinobenzoic Acid . . . . . . . .PLOCIIL (J.). Phenylsmido-acetic Acid . . . . . . .CONRAD (M.). Synthesis of Cinnamic and Phenjl-lactic Acids from EthylMalonat e. . . . . . . . . . . . .CLAISEN (L.) and P. J. ANTWEILER. Cinnamyl Cyanide and Cinnamylfor-mic Acid. . . . . . . . . . . . .TIEMANN (I?.) and J. OPPERMANN. Three Isomeric Arnidocinnsmic AcidsLADENBURG (A.) and L: RUGHEIMER. Sycthesis of Tropic Acid. . .BO~TINGER ((3.). Preparation of a-Hydroxyuvitic Acid .. . .JACOBSEN (0.). Hydroxyuvitic Acid . . . . . . . .BOTTINGER (C.). Constitation of Uvitonic Acid . . . . . .SPIEGEL (A.). Vulpic Acid . . . . . , . . . .ANDREWS (L. W.). Bromorthamidoparabenzenesulphonic Acid . . .ANDREWS (L. W.). Bromorthonitrobenzenesulphonic Acids . . .CLAUS (A.) . Cymenesulphonic Acids . . . . . . . .SALKOWSKI (E. and H.). Skatole-forming Substance . . . . .ZIMNEBMANP (J.) . Azo-compounds of Paramononitrodiphenyl . . .Decomposition of Copper Acetate in Presence of WaterAction of Water on Ethyl Malonate at a High Temperature.and Carbostyril . . . . . . . . . .FAGE14.915015 115115115 11531531 <5415%1551551551551551551561561571581581591591591601611611621631631631641651661671681651681691691711731721731’7317417417417517CONTENTS .XXlZCMMEltMANN (J.). Derivatives of Paramidodiphenyl . . . . .STREIFF (J.). a- and P-Naphthylphenylamine . . . . . .GRAEBE ((2.). Reactions of Naplitliol . . . . . . . .HANTZSCR (A.) . Action of Commercial Trimethylamine on ?-Naphthol .KOELLE (G.). Derivatives of Naplithol . . . . . . .NIETZKI (R.). Biebrich Scarlet . . . . . . . . .GBIESS (P.). /3-Naphtholdisulphonic and Dihydroxynaphthalene-disulpho-nic Acids . . . . . . . . . . . .BURG (0.). Picene, a New Hydrocarbon from Peat-tar . . . .CAZENEUJ-E (P.) and IMBERT . Conibiiiation of Chloral Hydrate with Cam-phor . . . . . . . . . . . . .SCH~FF (I€.). Acetyl-derivatives of Aesculin and Aesculetin .. .HESSE (0.). Calycin . . . . . . . . . . .CARNELUTTI (J . ) and R . NASINI . Optical Rotary Powers of Sailtonin-deri-vat i B es . . . . . . . . . . . . .SOUBEIRAN (L.). Thapsia garganica . . . . . . . .HOTTINGER (C.). Synthetical Pyridinetricarboxylic Acid . . . .BOTTIXGER (C.). Synthesis of Quinoline . . . . . . .CLAUS (A.) and P . HIMNELNANN . Quinoline . . . . . .CLAUS (A.). Alkaloids of Peruvian Bark . . . . . . .CLAUS (A) and M . DANXENBAUM . .ULAUS (A.) and R . BOCK . .CLAUS ( A ) and C . BATCKE . Phenylhomocinchonidine . . . .~IESSE (0.). Relation of Echitamine to Dita'ine . . . . . .1)ANILEWSKY (A.) . Crystalline Decomposition-product of Albuminous Sub-stances . . . . . . . . . . .. .J~DERHOLM (A.). Metahaemoglobin . . . . . . . .UANOISEAU (A.). Chlorine and Bromine Derivatives of Methane . . .BNRTRAND (A.) and E . FINOT . Action of Ant. imony Pentachloride on CarbonBisulphide . . . . . . . . . . . .C'ONINCK (0 . DE) . Preparation of Ethyl-vinyl Hydrocyanide . . .YIWNIER (L.) and E . VARESNE . Products from Petroleum Coke . . .BANDROWSKI (E.). Potassium P r i p r g j l a t e . . . . . . .SBUBERLICH (K.). Preparation of Potassium Ferricyanide . . . .EICHARD (A.) and A . BERTRAND . Magnesium and Potassium Platino-'BERTRAND (A) . Combination of Titanium Tetrachloride with Ethyl Etlier .CLAESSON (P.) and C . F . LUNDVALL . Action of Amnionia and Amines onEtlijI and Methyl Sulplistes . . . . . . . . .Di-iodopropyl Alcoliol and i k o d - a l l y lAlcohol .. . . . . . . . . . . .~ J R E C H (P.). Inversion of Canc-sugar by Hydrochloric Acid a t the OrdinaryTOLLENS (B.). .KILIBNI (H.). .KILIANI (IT.). Identity of Arabinose and Lactose . . . . .KILIANI (H.). Inulin . . . . . . . . . . .SCHEIBLER (C.). Relation between Cqstalline Form and Rotatory Power ofcertain Carbohydrates . . . . . . . . . .Y'HONSEN (T.). Optical Rotatory Power of the Carbohjdrates and theirDerivatives . . . . . . . . . . . .BISENBERG (J . L.). Separation of Trimethylamine from the CoiiimercialEthjl-derivatives of Cinchonidine .Methyl-derivatives of Homocinchonidines .cyanide . . . . . . . . . . . . .BERTRAND (A) . Reduction of Ethyl Nitrate by Alcohol . . .VALENTE (L.). Supposed Synthesis of Glucose .. . .f l WBNER (H.) and LELLNARN .Temperature . . . . . . . . . . .Specific Rotation of Cane-sugar in Different Solvents .Oxidation of Lactose and Lactonic Acid by Siher O d eHydroch1or;de . . . . . . . . . . . .SCHULZ (H.). Action of Oxalethylin . . . . . . . .WURTZ (A) . An Oxygenated Basic Derivative of Aldol . . . .CIAMICIAX (G . L.). Aldehyde Resin . . . . . . . .SCHXIDT (J . G.). Action of Aldehyde on Furfuraldcli~tlc . . . .13yAssox (11.). Transformatiou of Chloral into Metaolilorul . . . .PAQE17517617717717717817817918018018018018118118218218318318418418418518523823923923923923924024024024224224224324324324324324524524624624624724724xxii CONTEXTS .HOERMAXN (J .v.). Symmetrical ,B .Dichloracetone . . . . .URECIJ (F.). Action of Bromine on Acetic Anhjdride, Acetic Bromide.UEUTHER (A) . .LUBAVIN . Conversion of Ethyl Acetate into Butyric Acid . . . .HELL (C.). Occurrence of a Fatty Acid in Beech-wood Tar Paraffin . .Ethyl Acetate. Etliyl Snccinate. &c . . . . . . . .Conversion of Chlorocarbonic Acid into Formic Acid .HELL (C.) arid 0 . HERMANN . Lignoceric Acid . . . . . .KAHLBAEM (G . w . A.). Polymerides of Methyl Acrylate . . . .COENCLER (C.) . Methyl Carbonate . . . . . . . . KILIANI (H.). Preparation of Glycollic Acid from Sugar . . . .ROSE (B ) . Ethereal Salts of Carbonic Acid . . . . . . .PIC~ET (A.) . Anhydride and Ethers of Isodibromosuccinic Acid .. .BOTTINGER (C.). Oxyethylideiiesuccinic Acid . . . . . .HUBXER (H.). Formulae of Maleic and Fumaric Acicls . . . . .CLAUS (A.) and F . VOELLER . Action of Ammonia on Ethyl Chloromaleate .DEMARFAY (E.). Tetrolic and Oxytetrolic Acids and their Homologues .CAYPANI (G.) and D . BIZZARRI . Tartronic Acid produced by the OxidationHJELT (E.). Dihydroxyadipic Acid . . . . . . . .KONIQ (F.). Fermentation of Tartaric Acid . . . . . . .EEKEL~ (A.). Synthesis of Citric Acid . . . . . . .ANDREASCH (R.). Carbamidttcetosulphonic Acid . . . . . .THOXSEN (T.). Miiltiples in the Optical Rotatory Power of Organic Com-pounds . . . . . . . . . . . . .LANDOLT (H.). Inversion of the Rotation of Optically Active Substances .MOLLER (H.). Cynnamido-compounds of Succinic Acid .. . .FRIEDEL (C.) and M . BALSOHN . Action of Ethylene Bromide on Toluene inHOFMANN (A . W.). Hexmethylbenzene . . . . . . .HEPP (P.). oxidation of Di- and Tri-nitrobenzene . . . . .EISENBERG (L . J.). Ferrocyanides of Amines . . . . . .MOHLAU (R.). Action of Primary Aromatic Amines on AcetophenoneBromide . . . . . . . . . . . . .ALEXEJEFF . Diazo-compounds . . . . . . . . .GABRIEL [S.). A Base from Phthalimide . . . . . . .Etherification of Phenols . . . . .Direct Introduction of Carboxjl intoPhenols and Aromatic Acids . . . . . . . . .of Glycerol with Potassium Permanganate . . . . . .FRIEDEL (C.) and M . BALSOHN . Oxidation of Triethylbenzene . . .presence of Aluminium Chloride . . . . . . . .SPICA (P.).Action of Nascent Hydrogen on ‘Nitrils . . . . .ROSENSTIEHL (A.). Existence of Three Isomcric Rosanilines . . .LADENBURG (A.). Constitution of Tropine . . . . . . .FLEISSNER (I?.). Tribenzylphosphine Oxide . . . . . . .MERZ (v.) and w . \vEITII .SUIDA (W.) and S . PLOHN . Orthoethylphenol . . . . . .CANZONERI (I?.). Oxidation of the Methyl Ether of Pnraxylenol . . .CONINCK (0 . DE) . Dimethylresorcinol . . . . . . . .KARIOF (K.). Dipropylresorcinol and some of its Derivatives . . .TIEMANN (I?.) and A . PARRISIUS . Resorcinol Derivatirev . . . .EARIOF (K.). Derivatives of Dimethylquinol . . . . . .GAUTIER (A.). Ieomerides of Phloroglucol . . . . . . .BURCKER (E ) . Synthesis of Benzoylpropionic Acid . . . . .SENHOFER (C.) and C . BRUNNER .BERTRAND (A.). Combination of Titanium Tetracliloride and BeilzoicChloride .. . . . . . . . . . . .FRIEDEL (C.) and M . BALSOHN . Synthesis of Diphenylacetic Acid . .GABRIEL (S.) and J . ZIYMERNANN . DinitroliSdrocinnamic Acid and itsDerivatives . . . . . . . . . . . .BAEYER (A.). Relation of Cinnamic Acid to the Indigo-group . . .LIPMANN (E . v.) and R . LANGE . IIydroxycumic Acid . . . . .OQLIALORO (A.) . Phenoxycinnamic Acid . . . . . . .SPIEQEL (A.). Synthesis of Tropic Acid from Acetophenone . . .PAQE24824482482492402492502512512512532542542542552562562562662572572372582592802602612612662662622632632632632642652682682692692702722722’7327327327427427627627CONTENTS .xxiiiETTI (C.). Quemitannic Acid . . . . . . . . .SCIEOOP (P.) . Sulphotereplithalic Acid . . . . . . .BOTTINGER (C.). Constitution of Aniluvitonic Acid . . . . .B~~TTINGER (C.). Dimethyl a-Hydroxyuvitste . . . . . .BAEYER (A.). Preparation of Skatole from Indigo . . . . .FRIEDEL (C.) and M . BALSOHN .FRIEDEL (C.) and M . BSLSOHN .Action of Ammonia on Nonobromodi-phenylniethane . . . . . . . . . . .Action of Sulphuric Acid on Phenyl-acetylene . . . . . . . . . . .CARNELUTTI (G.). Ethylnaphthaiene . . . . . . . .TASSINARI (GI.. ) Acetyl-a-naphthol . . . . . . . .HONIG (M.). Action of Oxalic and Sulphnric Acids on Naphthol . .RICHTER (M.), Dinaphthylniethane . . . . . . . . KNECHT (W.) and J . UNZEITIG .a- andp-Dinaphthylene Oxide . . .ARX (v . J.). u- and P-Nephthylenephenylene Oxides . . . . .SCHREDER (J.). Decomposition of Itufigallic Acid . . . . . .GOLDSCHMIDT (G.). Idryl . . . . . . . . . .GRAEBE (C.) and J . WALTER .VALENTE (L.). Essential Oil from Hemp . . . . . . . Picene . . . . . . . .Amidine Bases from Dibasic Acids .The Two Isomerides of Santonincalled Metasantonin . . . . . . . . . .Action of Phosphorus Pentachlorideon Santonic Acid . . . . . . . . . . .Picrotoxin . . . . . . .TERREIL (A.). Phytolaccic Acid . . . . . . . . .BERNHEIMER (0.). Products from the Roasting of Coffee . . . .KRAKAU (A.). Quinoline . . . . . . . . . .CLAUS (A.). Quinoline . . . . . . . . . .CONIKCK (0 . DE) . Lutidine Aurochloride .. . . . . .HESSE (0.). Cinchonine . . . . . . . . . .WALLACH (0.). and I . KAMENSKI .CANNIZZARO (S.) and G . CAENELUTTI .CANNIZZARO (S.) and G . CARNELUTTI .BARTII (L.) and M . KRETSCHY .SKRAUP (Z . H.). Synthesis of Qninoline . . . . . . .CAROURS (A.) and A . ETARD . Nicotine . . . . . . .CLAUS (A.) and H . M u u m . Methyl-derivatives of Cinchonine . . .CLAUS (A.) and KEMPERDICK . Ethyl-derivatives of Cinchonine . . .CLAUS (A. ) and W . TREUPEL . Benzjl-derivatives of Cinchonine . . .SKRAUP ( Z . H.). Cinchomeronic Acid . . . . . . . .HESSE (0.). Cinchonidine and Homocinchonidine . . . . .RICFIET (C.) and G . BOUCHARDAT . Chlorinated Derivatives of Strychnine .SCHNIDT (E.). Alkaldids from Belladonna and Datum Stramoniunz . .PESCI (L.).Atropine . . . . . . . . . . .SPICA (P.). .C L ~ E (P . T.). Oxidation-products of Cholic Acid . . . . .HOFNEISTER (F.). Chemical Structure of Collagen . . . . .TAWILDAROFF . Action of Chlorine and Bromine on Ethylidene Chloride andEthyl Bromide . . . . . . . . . . .GTJSTAVSON (G.) . Reactions of Aluminium Chloride and Bromide withOrganic Compounds . . . . . . . . . .GUSTATSON (G.). Action of the Alcoholic Bromides, and of Eesbrom-ethane on Para5ns in presence of Aluminium Bromide . . . .SABAN~EFF . Boiling Points of Ethylene and Ethane Derivatives . . .KEHRER (E . A. ) and B . TOLLENS . Hydrocarbons obtained as Bye-products . . .FiiRsr (E.). Chlorine Tetroxide and Ethylene . . . . . .LWOW (0.). Polpmerisation of Vinyl Bromide . .. . . .ELT~KOFF . Atomic Migration . . . . . . . . .HESSE (0.). The Bark of Aspidosprrma Quebracho . . . . .Some Alkaloids found in the Animal Organism during LifeWEIDEL (H.) and G . L . CIAMICIAN . Dry Distillation of Gelatin . . .Lwow (0.). Hexmethylethane . . . . . . . . .in the Decomposition of Levulic Acid by Hydriodic AcidKOKOVALOFP . Isobutylene . . . . . . . . .PAGE2772782782782782792792802802802812812822822832842842842852%28628628728728728728828828828928929029029129329329329429429429429539839839939939939939940040040xxiv CONTENTS.KONOVALOPF. Action of Kitric Acid on IsodibutSlene . . . .\~7ALITZKY (w. E). Cholestene (Cholesterilene) .. . . .DAVY (E. W.). Nitroprussides of the Alkaloids . . . . . .STCHERBAEOFF. Formation of a Secondary Alcohol . . . . .BOBOMOLETZ. Action of Zinc-methyl on Chloracetic Cliloride . . ,SENLJANITZIN (A.) . All~lmethylpropyl Carbinol and P-Methylpropj lethj 1-en elactic Acid . . . . . . . . . . . .YRZYBYTEK. Oxidation of Erythrol and Glycerol . . . . .COLIXY aiid VAKOVITCH. Preparation of Sucrose from Glacosc . . .A ~ O R I X (I€.). Gelose . . . . . . . . . . .PORUMBIRU. Gelose . . . . . . . . .LAXDOLT (H.). Mull iples in the Rotatorv Powers of Organic Componnds .RJABININ (I<.). Methyl and EthylEtheiek of Uialljlcarbinol . . .CLAISEN (L.). Condensation of Aldehjdes with Ethyl Acctnte and MalonateXEWBURY. Preparation of Crotonaldehyde .. . . . . .GRIMAUX (E.) and P. ADAM. Deri\atives of Acrole’a . . . . .FRIEDRICH (R.). Dichloraldrhyde Hydrate . . . . . . .ENGEL and MOITESSIER. Dissociation of But~lchloral IIydratc . . .WINOBRADCFF. Action of Aluminium Chloride on Acetic Cliloridc . .FRIEDRICH (R.). Dry Distillation of Potassium Dichloracetate . . .KABLOUKOFF. Triacetin . . . . . . .SAYTZEFF (A.). Calcium a n j Barium Salts of Dicthjl- and Methylpropyl-acetic Acids . . . . . . . . . .GUTHZEIT (M.). Cetgl- and Dicetjl-acetic and iiialonic Acids . . .WISLICENUS (J.1. Decomposition of l’olybasic Acetoacetates by Alkalis .GROTE (A. F.), E. KEIIRER, and B. TOLLENS. Preparation and Properties ofLevulic or @-Acetopropionic Acid . . . . . . . .GROTE (A. v.) and B. ‘~!oLI,E~s. Formation of Levulic Acid from DextroseRODEWALD (€1.) and B.TOLLUKS. Formation of Levulic Acid froin Milk-sngar . . . . . . . . . . . . .KEHBER (E. A.) and 13. TOLLEFS. Conrcrsion of Levulic Acid into KormalValeric Acid . . . . . . . . . . . .TOLLENS (13.). Oxidation of L,evulic Acid . . . . . . .BISCHOFF (C.). Two Homolsgues of Acetopropionic Acid . . . .FRIEDRICH (A. R.). Action of Potash on Bromomethacrylic Acid . .LAGERMARK (A.). Tetrolic Acid . . . . . . . . .KLIMENPO (11.). Isomerides of Lactic Acid. . . . . . ,SCHIROKOFF (A.). Conversion of Hydroxjraleric Acid from All? lcliniethylCarbinol into Isopropylacctic Acid . . . . . . . .MAUMEN~ (E. J.). Ammonium Carbonate . . . . . . .SOROKIN (B.) . Formation of P-Methosyglutaric Acid from DialljlmcthylCnrbinol .. . . . . . . . . . . .URECH (F.). Product of the Action of Bromiiie on Ethyl Succinate . .BOTTINGER (C.). Decomposition of Mesoxalie Acid . . . . .BALLO (M.) . Isobutylallylnialonic Acid . . . . . . .OSSIPOFF. Halogen Derivatives of Fumaric and Maleic Acids . . .KRUSEMARK (I?.). Citraconic and Mcsnconic Acids . . . . .FRANK (E.). .ERLENMEYER (E.). Action of DehFdrat ing Agcnts on Glyceiic and TartaricAcid . . . . . . . . . . . . .DOTT (D. B.). Meconic Acid . . . . . . . . .RENNIE (E. H.). Double Salts of Meconic Acid . . . . . .COOICE (J. P.). Argento-antimonious Tarti*ate . . . . . .DUVILLIER (E.) and A. BTTISNE. Separation of Trimethjlamiiic froni theCommercial Product . . . . . . . . . .HEINTZ (W.). Triacetonediamine. .. . . . . . .HEINTZ (W.). An Acetone Base containing Sulphur . . . . .LADENBERG ( A.) . Trone’ines . . . . . . . . .IIANRIOT. Action of Hydrochloric Acid on Aldehyde . . . .Synthesis of Glyceric Acid from Monochlorolactic Acid .BOTTINGER ((3.). Ethyl Pyroraceinate . . . . . . .PAO E40040140140140140240240240340340340440$40540540640740740740840840840840040941041041142141241 341341341441441441441541541641641641‘341841841841941942048042CONTENTS . XXYWBOBLEWSPY . Oxidation of Xitroxylene and Xylidine . . . .GOLOUBEFF . Dinitro-derivatives of Deoxybenzo'in . . . . .CLAISEN (L.) and A. CLAPAK~DE . Compounds of Acetone and MesitylPAT ERN^) (E.).and S . SCICHILONE . Synthesis of Aroinntic Aldehydes byGOLDSTEIN . Oxidation of Ketones . . . . . . . .PILETI (M.) . Two Modifications of Amidocumic Acid : Acet amidocumic AcidKRAUT (K.) and G . MERLING . .KAST (H.). Atrolactic, Phenpllactic, and Atroglj-eeric Acids . . .BOSLER (M.). Cumino'in and Anisoin . . . . . . . .Oxide with Benzaldehyde : Constitution of AcetophoroneMeans of Clironiyl Chloride . . . . . . . . .Preparation of Benzoic Acid and of Benzaldehyde . . . . . .FITTIG (R.). Isatropic Acid . . . . . . . . .GRIESS (P.). Benzidinedisulphonic Acid . . . . . . .CLAESSON (P.) . Tolucnetrisulplionic Acid . . . . . . .. . .Addition-compounds of L4tropic Acid .JACOBSEN (0.). Sulphamine- and Hydroxy-acids derived from Mesitylene .BORSILOWSKY (J.).Azo-derivatiues of Toluene . . . . . .WROBLEWSKY (E.). Isomeric Xylidines . . . . . . .SOMMARUGA (E . v.). Action of Aniniunia on Isatin . . . . .HEMILIAN . Diphenylpnraxylylnietliane and Diplzenylnaphthylmcthane .HEMILIAN . Diplienylenephenylmctl~ane and Dipheriylenetolylmetliane .S C H M I D T ~ ~ ~ S C H U L T Z . Oiphenylbenzenes . . . . . . .BEILSTEIN and KOURBATOFF . Oxidation of a- and p-Dinitronaphthalcne byNitric Acid . . . . . . . . . . . .REINGRUBER (F.) . Methylnaphthalene . . . . . . .bfELUoLA (R.). Nitroso-P-naphtholsulphonic Acid . . . . .FLAVITZKY (F.). Comniercial Lemon Oil . . . . . . .FLAVITZKY (F.). The Terebecthenes . . . . . . . .USLLO (M.). A New Property of Camphor . . . . . . .ALEXEJEFF (W.).Liquid Camphor . . . . . . . .BALLO (M.). Oxidation Products of Camphor . . . . . .SCHIFE (R.). Action of Bromine and Chlorine on Nitrocamphor . .SCH~FF (i3.). Decomposition of Glucosides by Heat . . . . .SCHIFP (H.). A Modification of Heliciu . . . . . . .VERNET (L.). Glucosjde irom the Ivy . . . . . . .PATERNZ, (E.) and A . OGL~ALORO . Kemarks on the Chemical Nature ofPicrot oxin . . . . . . . . . . . .TABRET (C.). TValdivin . . . . . . . . . .PATLEVSKY . Acid from P-iscum album . . . . . . .GREENISH (H . G.). Cape Tea . . . . . . . . .C'HUECH (A . 11.). Cape Tea . . . . . . . . .CONISCK (0 . cle) . Pyridine Bases . . . . . . . .CLAUS (A.) and P . IIIIKVIXLMANN . Reduction of Quinoline . . . .WICHNEGRADSKY . Reduction of Quinoline and Bthjlpyridine .. .GERICHTEN (E . v.). Cotarnine . . . . . . . . .FILETI (&I.). Distillation of Cinchonine with Zinc .LADENBDEG (A.). The Mydriatic or Pupil-dilating Alkaloihs : . :LLOYD (J . U.). Citrate of Caffeine . . . . . . . .POHL . Pilocarpine . . . . . . . . . . .IIESSE (0.). Bark of Alstonia spectabilis . . . . . . .DANSLEWSKI and P . BADENHAUSEN . Albumino'ids in Milk . . . .SCHAFFER (F.). Mgcoprote'in . . . . . . . . .BLEUNARD (A.). Legumin . . . . . . . . . .CATILLON (A.) . Preparation of Peptoncs . . . . . . .'L'IIOMSEN (J.). Ethane . . . . . . . . . .H~~CHAMP (A.) . Formation of Chloroform from Alcohol and Bleaching-powder . . . . . . . . . . . . .ZAGOUMENNY . Tetraphenykthane . . . . : . . .HESSE (0.).AIkalo'ids from Dita Bark . . . . . .H e s R Y (L.). Dipropargyl . . . . . . . .PAGE4204214224224234234.234244254254274284294294324334'3E43443443443;43543643643744374384384384384.394'31)4404404414. 4144144344344444.444544 644 64474.4744744844944944944956556556xxvi CONTENTS .ARONSTETN (L.) . .HENRY (L.) . Ally1 Iodide and RiIonobromallyl Alcohol . . . .BERTHELOT . The Saccharoses . . . . . . . . .KULZ (E.j. Maltose . . . . . . . . . . .YOSHIDA (H.). Maltose . . . . . . . . . .STEINER (J.). Remarks on Some Experiments with Maltose . * .KULZ (E.) and A . BORNTRAGER . .KULZ (E.). Specific Rotatory Power of Glycogen . . . . .KULZ (E.).Action of Mineral Acids on Glycogen . . . . .KULZ (E.). SchtscherbakoPs A, B, C, and D Glycogen . . . .MUSCULUS (F.) and A . MEYER . Conversion of Glucose into Dextrin . .MUSCULUS (F.) and A . MEYER . Erythrodextrin . . . . . .HOFMANN (A . W.). . . .GURKE (0.). Ethylhydroxylamine . . . . . . . .WALLACH (0.) and E . SCHULZE . Bases of the Oxalic Series . . . .SCHMIDT (J . G.) . Action of Furfuraldehyde on Aldehydes and Acetone inPresence of Sods . . . . . . . . . . .TBOOST (L.). The Vapour of Chloral Hydrate . . . . . .BECKURTS (H.) and R . OTTO . Action of Heat and Water on the Halogen- . . . . . .ARONSTEIN (L ) . Action of Ethyl Bromide on Ethyl Bromacctate . .ARONSTEIN (L.) and J . M . A . KRAXPS . Action of Methyl Iodide on MethylIodacetste .. . . . . . . . . . .LEGLER (L.). Etheric or Lampic Acid . . . . . . . .CLARKE (F . W.) and E . A . KEBLRR . .CONRAD (M.) . Ethyl Chloronialonate . . . . . . . .HJELT (E.). A Neutral Bromide from Diallylmalonic Acid . . . .SCHACHERL (G.). Preparation of Monobromo- and Dibromo-succinicAcids . . . . . . . . . . . . .CLAUS (h.) and J . HELPENSTEIN . Action of Ammonia on Ethyl Dibromo-succinate . . . . . . . . . . . .GANTTER (F.) and C . HELL . Azelaic Acid . . . . . . .BISCHOFF (A.) and M . GUTHZEIT . .BAYLEY (T.). Preparation of Potassium Hydrogen Saccharate . . .KILIANI (H.). Potassium Idactonate . . . . . . . .PAGE (W . T.). . . . .CLAESSON (P.). Dithioglycollic Acid . . . . . . . .CARL (F.). Zsethionic Acid . . . .. . . . . .LEEDS (A . R.). Action of Nitrogen Peroxide on Carbon Compounds . .CLAUS (A. ) and P . RAUTENBERG . Decomposition of DimethylanilineMetliiodide and Ethiodide by Potash, and Action of Amy1 Bromide onDimethylaniline . . . . . . . . . . .GURKE (0.). a- and p-Ethyl Dibenzoylhydroxamate and a- and j3-Ethylben-zoylhydroxamic Acid . . . . . . . . . .COHN (L.) . l’hthalylhydroxylamine : Conversioll of Phthalic into SalicylicAcid . . . . . . . . . . . . .FISCHER (0.). Condensation-products of Aromatic Bases . . . .ANDRESGN (AI.). Thymoquinonedichlorimide . . . . . .LANDAUER (J.) . Absorption Spectra of Chrysoi’din and Related Azo-colour-ing Matters . . . . . . . . . . . .Action of Glacial Acetic Acid on Phenyl-thiocarbiinide . . . . .. . . . . .Compounds of Monobasic and Dibasic Acidswith Phenols . . . . . . . . . . . .Cresol-derivatives . . . .Conversion of Normal into Isopropyl Bromide by HeatElementary Composition of GlycogenAction of Heat on the Ammonium Basessubstituted Acids of the CnHBn02 SeriesChromium Barium Osalate .j3~Methylethenyltricarboxylic Acid .Solubility of Carbon Bisulpliide in Water~CTARD . Chlorochromic Acid as an Oxidising Agent . . . . .RAU (H . M.). Benzolone and Benzostilbene . . . . . .CLAUS (A) and M . VOLTZKOW .NENCKI (ill.) and N . SIEBER .MICHAEL (11.). Action of Aromatic Hydroxy-acids on Phenols . . .I~OFMANN (A . W.) and w . 17 . MIrLER .PATERNZ) (E.) and F . CANZONERI . Synthesis of ThymolHALLOCK (E . J.). Bromonitro- and Chloronitro-phenetoi’ls .. . .. . . .PAGE5675675675675685685695695695705705705705’735735745765765765765775775775’775785795 8058058058058158158458458458558759059159159 159159259259359CONTENTS . xxviiMAGATTI (G.). A Derivative of Quinol . . . . . . .ZINCEE (T.). Action of dinines on Quinones . . . . . .VINCENT (C.). Benzhydryl Acetate . . . . . . . .HESSE (C.). Amidotoluene Sulphjdrates . . . . . . .~ I D N A N (0.). Cnmino’in . . . . . . . . . .PATERN& (E.). Organic Fluorine Compounds . . . . . .REBUFFAT (0.). Barium and Calcium Cinnamates . . . . .FISCHER (E.). Orthohydrazincinnamic Acid . . . . . .JACOBSEN (0.). Hydroxytoluic and Hydroxyphthalic Acids .. .JACOBSEN (0.). Hydrox~mesitylenic Acid from Xylenol . . . .RUGEEIMER (I,.) . Phenglsnccinic Acid . . . . . . .RUGHEIMER (L.). Etlijlatrolactic Arid . . . . . . .DOEBNER (0.). Formation of Aromatic Ketonic Acids . . . .LOEW (0.). Schizomycetic Fermentation of Quiiiic Acid . . . .ARATA (P . N.) . .SPICA (P.) . Cpmenesulphonic Acids . . . . . . . .SCHIAPARELLI (C.). Ethereal Salts of Phenyl and some of their Deri-vati1 es . . . . . . . . . . . . .SCHULTZ (G.) and H . STRASSER . .MERZ (v.) and W . WEITH . Mononaphthylamines from Naphthols . .COSINER ((2.). Derivatives of P-Naphthylamine . . . . . .LIEBERMANN (C.) and L . LANDSHOFF . Action of Nitric -4cid on AnthraceneDihydride and Ethylanthracene Dihydride . . . . . .PERQER (H .R.). Formation of Dihydroanthranol and of Anthracenc fromAn thmqui non e . . . . . . . . . . .SIMON (S . E.) . Dinitroxyanthraquinone . . . . . . .LIEBERMANN (C.). Alkyloxanthranols . . . . . . . .LIEBERMANN (C.) and L . LANDSHOFF . Derivatives of Ethyl, Amyl, andMethyl Oxanthranols . . . . . . . . . .LIEBERMANN (C.) and WALDER . Butyloxanthranol . . . . .SCHIFF (H.). Researches on Glucosides . . . . . . .LIEBBRMANN (C.) and H . MASTBAUM . Aesculetin . . . . .JACKSON (C . L.). Curcumin . . . . . . . . .HALBERSTADT (W.) and M . A . v . REIS . . . . . .HOOG-EWEEFF (S.) and W . A . v . DORP . Yyridine- and Methylpyridine-carboxylic Acids . . . . . . . . . . .BOTTINGER (C.). Synthetic Picoline-monocarboxj lie and Pyridine-dicar-CONINCK (0 DE) .Fractional Distillation of Crude Quinoline . . .BEDALL (K.) and 0 . FISCHER . Hydroxyquinoline . . . . .WILLIAMS (C . G.). Action of Sodium on Quinoline . . . . .BOTTINGER (C.). Forination of Pyrroline . . . . . . .FISCHER (E.). Caffeine . . . . . . . . . .HESSE (0.). Constitution of some Alknloi’ds of the Cinchona Barks . .CLATJS (4.) and F . MALLMANN . Methyl- and Ethyl-derivatives of Quinine .HESSE (0.). Propionylquinine . . . . . . . . .CLAUS (A.) and C . BOTTLER . Tolyl-quinines . . . . . .CLAUS (A.). Cinchonidine . . . . . . . . . .FORST (C.) and C . BOHRINGER . Cinchotine . . . . . .HOFMANN (A . W.). Action of Heat on Ainines . . . . . .ARATA (P . N.). Supposed Identity of Paptine and Aspidoapermine . .HESSE (0.). Alkaloids of Alstonia constpieta .. . . . .HAMMERSTEN (0.). A New Oxidstion-product of Cholic Acid . . .GRUBLER (G.). Crystallisable Albumin from Pumpkin Seeds . . .HUFNER ((2.). Crystalline Haemoglobin . . . . . . .SCHUTZENBERGER (P.) and N . IONINE . Con;position of Petroleum from theCaucasus . . . . . . . . . . .WILM (T.). .Chemical Extimination of Persea Liiigue and its TanninMICHAETJS (A.) and C . PAXEK . Benzophoephinic Acid . . . .CLATJS (A.) and E . RISLER .Diphenyline and 6-DiamidodiphenylReactions of Benzictine . . . . .Hremate’in. boxylic Acids . . . . . . . . . . . .Action of Palladium, Rhohium, and Platinum on Coal-gasPAGE5955955%59659759759559859959959960060060060260260260360460560560560650760860860860961061061061161161261261361361461461561962062062062062162265362462562570570xxviii CONTENTS .GOLDSCHMIDT (11.). .SCHOLTZ (R.).Double Platinocyanides . . . . . . .ETARD (A.). Action of Ammonium Chloride on Glycerol . . . .THOMSEN (‘T.). Rotatory Power of Carbon Compounds . . . .FRANCHIMONT . Acetic Derivatives of Cellulose . . . . . .BERTHELOT . Ethyl Peroxide . . . . . . . . .<ECONOMID~S (S.) . Action of Phosphorus Pentachloridc on Isobutaldeliyde.LIEBEN (A.) and S . ZIESEL . Condensation-products of Aldehj des and theirDerivatives . . . . . . . . . . . .(ECONOMIDBS (S.). Preparation of Isobutylal . . . . . .LIEBEN (A.) and S . ZIESEL . . . .SPRING (W.).Formation of Acetone and Tliiacetone . . . . .HELL (C.). New Method of Bronunating Organic Acids . . .LIEBEN (A.). .MELIKOFF . P-lodolactic Acid . . . . . . . . .DUVILLIER (E.). Amido-acids dcrived from Iso-hydroxyvaleric Acid . .EDEE ( J . M.) and E . VALENTA . Iron Oxalates and some of their DoubleSalts . . . . . . . . . . . . .XULDER (E.) and H . L . MEULEN . Action of Zinc-rthyl on Ethyl Tartrate .KEKUL% (A.) and R . ANSCHUTZ . . . .CLAESSON (P.) . A Compound of ‘I‘hiocyanacetic Acid and Cai.baiiiinctliiogly-collie Acid . . . . . . . . . . . .CLAESSON (P.). Thiocyanuracetic Acid . . . . . . .GABRIEL (8.). Sulphonacctic Acids . . . . . . . .BEHREND (R.). Action of Sulpliurjl Chloride on Dimethylamine . .LETTS (E . A.). Phosphorus-bcta‘ints .. . . . . . .WALLACH (0.). Substituted Oxamides, Formamidcs, and DiethyloxamicAcid . . . . . . . . . . . .LEEDS (A . R.j. Action of Ozone, Pu’ascent Oxygen, and Hydrogen Pcroxideon Benzene . . . . . . . . . . . .BERTHELOT and OGIER . Researches on Isomerism : Benzene and Dipro-Action of Molecular Silver on Carbon Chloride3 .Reduction of Crotonyl ChloralCompounds of Calciuni Chloride with the Fatty Acids .BOTTINGER (C.). Tartronic Acid . . . . . . . .WALLACH (0.). Derivatives of Pyromucic Acid . . . . . .Tanstar’s Trioxymaleic AcidFRANCHIMONT . Action of Sulphuric Acid on Arctic dnhydricic . . .pargyl . . . . . . . . . . . .RENARD (A.). Electrolysis of Toluene . . . . . . .YIENNE and STEINER . Preparation of Metatoluidine .. . . .LICHTENSrEIN (L.). Dry Distillntion of the Mucates of Aniline and Para-toluidine . . . . . . . . . . . .STAEDEL (W.) and 0 . SIEPERXANN . New Synthesis of Organic Bases con-taining Oxygen . . . . . . . . . . .LETTS (E . A.) and N . COLLIE . Salts of Tetrabenzylphosphonium . .MICHAELIS (A.) and C . SCHULTE . Arsenobenzene . . . . .ALEXEJEFF (W.). Preparation of Pure Phenol . . . . . .N~LTING (E.) and EL SALIS . Nitro-cresols . . . . . . .ZULKOWSKY (K.). Crystallisable Constituents of Corallin . . . .LORENZ (C.) . Derivatives of Piperonal . . . . . . .GABRIEL (S.) and R . NEYER . Dinitrophenylacetic Acid . . . .ROSER (I,.). Synthesis of Ketonic Acids . . . . . . .GABRIEL (S.). Phthnlic Anhydride Condensation-products . . . .BARTH (L.) and J .IIERZIG . Mesitylcnedisulphonic AcidJACKSON (0 . R.). Methylketolo . . . . . . . . ..T ACOBSEN (P.). @Derivatives of Naphthalenc . . . . . .CLSCS (h.) and ii . IIEWTEI. . lntliraquinone DerivativesSTAEDEL (W.) and others . Action of Nitric Acid on somc Phenol Ethers .WESELSKY (P.) and R . BENEDIKT . Resorcinol Colouyiiig Matters . .HALBERSTADT (W.). Action of Bromine on Paranitrobcnzoic Acid . .FRIEDEL (C.) and J . M . CRAFTS . Compounds of Phtlialic Bnhjdride withHydrocarbons of the Benzenc Series . . . . . . .. . . .LIEBERNANN (C.j and G . TOBIAS . Syntliesis of Homologncs of Anthracene . . . .PAUE70770770870970970970971071171 171171171272271371371471471471471571571s7 M71671771771971972172172172272272272372372572572672772972973173173373373473673673COXTEXTS .xxixMOBIN (H.). Essence of Linaloes . . . . . . . .RRNARD (A.). Products of the Distillation of Colophony . . . .TTEMANN (F.) and W . WILL . IIesperidin and its DerivativesLA COSTE (W.). Bromine-derivatives of Quinoline . . . . .JACKSON (0 . R.). Tetrahydromethyl-quinoline . . . . . .. . .SCHMIDT (E.) and E . LOWENHARDT . Constituents of the Seeds of CocculusIndicus . . . . . . . . . . . . .WIEDEL (H.) and A . COBENZL . Cinchonic Acid and Quinoline Deri-vatives . . . . . . . . . . . . .HOOQEWERPF (S.) and W . A . v . DORP . Pyridinecarboxylic Acids . .SKRAUP (Z . H.). Isomerism in the Pyridine and Quinoline Series ..SCHNIDT (E.). Caffeine . . . . . . . . . .HOFMANN (A . W.). Action of Heat on Ammoniuni BasesMALY (R.) and F . HINTEREBQER .CLAUS (A.) and K . GLASSNER . Strychnine . . . . . . .LEXTXAIT . A Coinpound of Strychnine with Iodoforrn . . . .CLAUS (A.) and R . ROHRE . Brucine . . . . . . .Vegetable Alkaloids . . . . . . . . . .C L ~ V E (P . T.). Oxidation of Cholic Acid . . . . . . .. . . .Caffeine and Theobromine . . .BROVARDFL (P.) and E . BOUTMY . Test to distinguish Ptoniajines fromWURTZ (A.). Papaine : a New Contribation to the History of Soluble Fer-ments . . . . . . . . . . . . .STRUVE (H.). Blood Crystals . . . . . . . . . .~ ~ C O I T O M I D E S (S.). Action of Ammonia on Isobntglidene Chloride . .PINNER (A.) and W .SCHATJMANN . Action of Sodium and Carbonic Anhy-dride on Allylene Chloride . . . . . . . . -MAUMES~ (E . J.). Decomposition of Mercury and Silver Cjanides . .HARTINB (E . C.). Oil of Wine . . . . . . . . .MULLER (W.) and J . HAGEN . Reduction of Cupric Hydrate in Keutral andAcid Mixtures by Grape-sugar . . . . . . . .MULLER (W.) and J . HABEN . Reduction of Cupric Hydrate in AlkalineLiquids . . . . . . . . . . . . .MULLER (W.) and J . IIABEN . Decompositions which occur in the Use ofTrommer’s Test . . . . . . . . . . .CLASSON (P.). Arabinose . . . . . . . . . .MEYER (V.) and F . P . TREADWELL . . . . . . .PINNER (A.). Condensation of Acetone . . . . . . .FITZ (A.) . Double Salts of the Lower Membm of the Acetic Acid Series .LANDOLT (H.).T . Thornsen’s Law of Multiple Rotations . . . .KetinesLUBAVIN (N.). Action of Ammonium Cysnate on Aldehydos . . .BOUNGUB (M.). Electrolysis of Formic and Mellic Acids . . . .CLAUS (A . ). Potassium Cyanide and Ethyl Dichloracetate . . . .FITZ (A.) . Ferrnciltation of Normal Valeric Acid . . . . .MICHAEL (A ) and L . M . NORTON . Monobromocrotonic Acids . . .C L A ~ S (A.) and G . LISCHKE . Action of Potassium Cyanide on Ethyl Clilor-isocrotonate . . . . . . . . . . .LIEBERMANN (C ) and A . LANGE . Lead Plumbothioglycollate . . .ALLARY (E.). Purification of Carbon Eisulphide . . . . . .LIPPMANN (E . 0.). Occurrence of Malonic Acid in the Manufacture ofKRESTOWNIKOFF (M ) . Homo-itaconic Acid . . . . . . .CIAMICIAN (C . L.) and M .DENNSTEDT . .MULDER (E.). Action of Bromine on Urarnil . . . . . .BECKE H. (A.) . Optical Rotatory Power of Asparagine and Aspartic Acid inDifferent Solvents . . . . . . . . . . .POMEY (E.) . Phosphoplatinic Compounds . . . . . . .JACKSON (C . L.) and A . W . FIELD . Yarachlorobenzyl Compounds . .JACKSON (C . L.) and J . F . WHITE . Parachlorobenzgi Compounds . .JANNASCH (P.) and C . STUNKEL . Crystallisation of a- and B-Dinitropua-xylenes . . . , . . . . . . . . .Beet-sugar . . . . . . . . . . . .Derivatives of Pyromucic AcidPAGE738$3873974074174.27437447447457467477477.48749749749750751793793794794795795795795795796796’796797798798798798 .80080080080080180180180180880380 680xxx CONTENTS.KELBE (W.).Occurrence o€ an Aromatic Hydrocarbon, CllHI6, in RosinOil. . . . . . I . . . . . . BERTHELOT and VIEILLE. Diazobenzene Nitrate . . . . . .NERGER (F.). Action of Acetainide on Phenyl Cyanamide . . . .PINNER (A.) and W. SCHAUMANN. Action of Hydrochloric Acid Gas onThiocarbimides and Thiocyanic Ethers in presence of Absolute Alrohol .NENCKI (M.) and N. SIEBER. Compounds of Mono- and Di-basic Acids withPhenols . . . . . . . . . . . . .KNAPP (H. v.). Action of Ammonia and Amines on Chloroquinones . .WIESER (H.). Pyroguajacol . . . . . . . . .BORODTN (A.). Action of Nitric Acid on Deoxxbenzoh . . . .R ~QOUMENNY (A.) . Benzopinacone and Benzopinacolin . . . .t LAUS (A.) and A. LADE. .L‘HoMPsoN (C.T.). .BOTTINGEX ((3.). Introduction of Aromatic Hydrocarbons into Ketonic andAldehydic Acids . . . . . . . . . . .OSER (J.) and W. KALXANX. A New Derivative of Gallic Acid . . .FAHLBERG (C.). a-Toluenedisulphonic Acid and its Derivatives . . .MEYER (R.) and H. BAEER. Oxidation of lsocymenesulphonic Acid . .REMSEN (I.) and W. BURNEY. Sulphoterephthalic Acid . . . .YLOCHL (J,). Action of Hydrocyanic Acid on Hydrobenzamide . . .IIALL (L. B.) and I. REXSEN. .GRAEFF (F.). Naphthalene Derivat ires. . . . . . . .JACKSON (C. L.) and J. F. WHITE. Synthesis of Anthracene and Phe-nanthrene from Orthobromobenzyl Bromide . . . . . .LIEBERMANN (C.) and S. E. SIMON. Hydroxyanthrauol . . . .ROEMER (C.). Deoxyalizarin. . , . . . . . . .GOLDSCHMIEDT (G.) and M.v. SCHIDT. Examiliation of “Stuppfett ” .MICHAEL (A.) and C. GUNDELACH. Synthesis of Methylconine and Consti-tution of Conine . . . . . . . . . . .C’AROURS (A.) and A. ETARD. Action of Selenium on Nicotine . . .CIAMICIAN (a. L.) and M. DENNSTEDT. Action of Chloroform on Potassiuml’yrroline . . . . . . . . . . . .KRETSCHY (M.) . Eya uric Acid . . . . . . . . .GRIMAUX (E.) . Transformation of Morphine into Code’ine and HomologousBases . . . . . . . . . . . . .FORST (C.) and C. BOHRINGER. Cinchotine and Hydrocinchonidine . .WEIDEL (H.). Tetrahydrocinchonic Acid . . . . . . .RAMMELSBERG (C.). Sttrychnine Sulphate . . . . . . .BAUMERT (G.). Lupinine . . . . . . . . . .TANRET (C.) . Peptones and Alkdonds . . . . . . . .RITTHAUSEN (H.).Crystalline AlbuminoTds from different Oil-seeds . .KUTSCHEROFF (M.). Monobromethylene . . . . . . .KUTSCHEROFF (M.). Direct Addition of Water to the Hydrocarbons of theAcetylene Series . . . . . . . . . . .EERNHEIMER (0.). Organic Nitroprussides . . . . . .~IENSCHUTKIN (N.). Influence of Isomerism on the Etherification of Alcoholsand Acids . . . . . . . . . . .BERTHELOT. Ethylene Chlorhydrin . . . . . . . .FOXHLET (F.) and others. Relation of various Sugars to Fehling’s Solution3fuscuLus (F.). Modifications of Starch . . . . . . .],IPPMANN (E. 0. v.). Lsevdan, LL New Species of Gum occurring in Beet-root Molasses . . . . . . . . . . . .GRIMAUX (E.) and P. ADAM. Chloropropaldehyde . . . . .SCHMIDT (J. G.). Action of Acetone on Furfuraldehyde and Benzaldchydein presence of Alkalis .. . . . . . . . .BranTHNER (J.) and w. SVTDA. Brominated Propionic and Acrylic Acids .&IEYER (P. J.). Ethyl Mono- and Di-chlorothiacetates : Action of Phospho-rus Pentasulphide on Chlorinated Acetic Acids . . . . .GANTTER (F.) and C. HELL. .Action of Bromine on Orthonitrobenzoic AcidNitration of Benzoyl Cyanide and its Derivatives.Oxidation of Mesitglenesulphonamide .Separation of Suberic and Azelaic AcidsPAGE809809e11081 181181281281381381481451481581681 881982082082282282382382382582582682782983083083 183183283388288388388388788788888888888988989089CONTENTS . sxxi1SCRNEIDER (Q .H ) .BAUER (A.) and M . GROGER .Rotatory Power of Malic Acid and its Salts .... HONIG (M.). New Isompride of Gluconic Acid . . . . . .TREADWELL (F . P.). A New Series of Volatile Organic BasesMEYER (V.) and E . J . CONSTAN . Ethylazaurolic AcidHERTH (R.). Synthesis of Biguanide . . . . . . . .Acids, and of Thio-cholestrophane . . . . . . . .CIAM~CIAN (G . L.) and M . DENNSTEDT . FurfurylamineSTUDER (A.). Butylation of Aniline . . . . . . . .Production of Hydrogen Peroxide by Hydrogenised Palla-dium.-Ozobenzene . . . . . . . . . .ZULKOWSEY (C.). Cryatallisable Constituents of Corallin . . . .LOWE (J.). Tannin of Oak-bark . . . . . . . . .Derivatives of Metachloronitrobenzene and Orthochloroben-zenesulphonic Acid . . . . . . . .. .LIMPRICHT (J.) Hydrazobenzenetetrasulphonic Acid . . . . .L A COSTE (W.). Benzarainic Acid and its Derivatives . . . .WILL (W.). Action of Carbonyl Chloride, and of Alcoholic Bromides, &c., onsubsti tilted Thiocarbamides . . . . . . . . .SCHTJLTZ (G.). Constitution of Diphenyl Derivatives . . . . .SCIIULTZ ((3.). Diphenyl Bases . . . . . . . . .SCHMIDT (H.) and G . SCHTJLTZ . Benzidine . . . . . . .SCHULTZ (G.) and others . Diphenyline . . . . . . .SCHWARZ (H.) . Preparation of Triphenylmethane, Tetraphenylethylene, andTetratolylethylene . . . . . . . . . . .SILTA (R . D.). Products accompanying Dibenzyl in the Alumiuium ChlorideReaction . . . . . . . . . . . .CLATJS (A.) and 0 . ZIMMERMANN . Action of Phosphorus Pentachloride onZINCKE (T.).Action of Amines on Quinones . . . . . .New Acid of the C,H, --4 O6 Series . . .. . . .ANDREASCH (R.) . Synthesis of Methylparabanic and Methyl-thioparabanic. . . .LEEDS (A . B.).ALLERT (R.) .P-Naphtholsulphonic Acid . . . . . . . . .FLUCKIGER (F . A.). Cananga Oil . . . . . . . .BATTR (J.). Hydrangea arborescens . . . . . . . .GREENISH (13 . (3.). Nerium odorum . . . . . . .EYKMAN (J . F.). Illiciurn religiosuin . . . . . . .SKRATJP (H.). Synthesis of the Quinoline Series . . . . .HOFMANN (A . W.). Pyridine Bases . . . . . . . .CHASTAIKG (P.). Constitution of Morphine . . . . . .HESSE (0.). Quinamine . . . . . . . . . .KUTSCHEROFF (M.). Oxidation of Cholic Acid . . . . . .TJANDOLT (H.). Optical Rotatory Power . . . .. . .MAUMENB (E . J.). Deciline . . . . . . . . .LE BEL (J . A.). Active Proppl Glycol . . . . . . .PRZYBYTEK . Oxidation of Glycerol by Nitric Acid . . . . .BOTTINGER (C.). Sugar from the Tannin of the Oak-bark . . . .TANRET and VILLIERS . Inosite . . . . . . . . .THOXSEN (T.). Optical Rotatory Power of Cane-sugar in Alkaline SolutionsTHOMSEN (T.). Rotation Constants of Cane-sugar . . . . .HERZFELD (A.). Effects of Diastase on Starch-paste . . . . .RDCHAMP (A.) . Viscose . . . . . . . . . .NASINI (R.). Specific Rotatory Power of Parasantonide . . . .HESSE (0.). New Platinochlorides of Cinchona Alkalosda . . . .THOXSEN (T.). Optical Rotatory Power of Organic Compounds . . .BEILSTEIN (F.) and A . KURBATOW . Caucasian Petroleum . . . .HEBOUL (E.). Action of Triethylamine on the Monohaloid Parafin Deriva-IhJVILLIER (E.) and A .BTJISINE . .HANTZBCH (H.) . Condensation-products from Aldehyde-ammonia andKetone Derivatives . . . . . . . . . .tives from Secondary and Tertiary Alcohols . . . . . .Separation of Compound AmnioniasCRIMATJX (E.) and P . ADAM . Dibromopropaldehyde . . . . .?AGB892893894895895896896897898898899901902903903905907907909911912913914915916916916918919919921921922922926102010201020102110211021102110221023102310241024102410251028102x xxii CONTENTS .HILL (I-I . 13.) and C . F . XABERY . Tetrasubstitution-dtu.iratives of Pro-HILL (H . B.). Structure of Disubstitiitrd Acrylic Acid .. . .HILL (H . B.) and C . W . ANDREWS . . . . .OTTO (R.) and H . HRCKURTS . . . .CLARKE (F . W.) and E . A . KEBLEB . Some I)ouLle and Triple Oxalates con-FUNARO (A.). l~econiposition of Calcium Succiijate by Heat . . .PETRI (W . ) . .BOTTINGER (C.). Pyroracemic Acid Compounds . . . . . .RENNIE (E . 13.). Acids of the Australian Currant . . . . .SCH~TZENBERGER (P.). Carboglucosic Acid . . . . . .CONRAD (M.) and M . GUTHZEIT . Barbituric Acid . . . . .SARRAU and VIEILLE . Decomposition of Potassium Picrste . . .SMITH (E . F.). Synthesis of Salicylic Acid . . . . . .BOTTIKGER ((2.). Introduction of Aromatic Hydrocarbons into Kctonic andPOST (J.) and C . G . MEYER . Metachloronitro- and Metachlommido-bcnzene-COALE (R .D.) and I . REMYEN . Oxidation of Sulphaniinemetatoluic Acid in . . . . . . . .MRYER (P . J.). A New Phenylthiohydantoic Acid . . . . .KUHARA (M.). Yhthalimide . . . . . . . . .MARCHETTI ((2.). Action of Aluminium Cliloyide on a Xixture of Naphtha-MILLER (0.). Naphthaquinone . . . . . . . . .kEBERMANN (C.) . Conversion of p-Naplltllaquinonei~nilide into a-Naphtha-. . . pionic Acid . . . .Dibromacrylic AcidConstitution of Glyoxylic Acidtaining Chromium . . . . . . . . . . .Derimtives of Itaconic, Mesaconic, and Citraconic AcidsMANN (W . ) . Methyldeoxybcnzoin . . . . . . . .Aldehjdic Acids . . . . . . . . . . .SPIEGEL (A.) . Vulpic Acid . . . . . . . .sulphonic Acids . . . . . . . . . .Alkaline and in Acid SolutionsBONDET (L.).Cork-tar . . . . . . . . . .lene and Ethyl Chloride . . . . . . . . .quinoneanilide . . . . . . . . . . .HALLER ( A.) . Cyano-camphor . . . . . . . . .SADTLER (S . P.) and W . L . ROWLAND . Colouring-matter from Beth-a-barrnU’ood . . . . . . . . . . . . .DEWAR (J.). Studies on the Quinoline Series . . . . . .BRIMAUX (E) . Some Reactions of Morphine and its Congeims . .GRIMAUX (E.). Ethereal Deri\ratires of Morphine . . . . .HESSE (0.). Cinchamidine . . . . . . . . . .ETARD (A.) . Homologue of Pelletieyine . . . . . . .CASALI ( A.) . Biliarp Acids in Toxicological Researches, and tlic ChcinicalNature of Selmi’s Ptomai’nes . . . . . . . .BLEUNARD (A.). Products of the Decomposition of Protei’n Compounds .GAMGEE (A.) and E . BLANKENIIDRN .The Existence of Liebreich’s Protagonin tlie Brain . . . . . . . . . . . .LOUGUININE IT.). E a t of Combustion of Heptane and HexhydrotolueneDOMAC (J.). Hexylene from Mannitol . . . . . . . .BOCCHARDAT (G.). Action of Sulpliuric Acid on Bromamylene . . .HAITINGER (L.). Nitro-olefines . . . . . . . . .Lead, Cadmium, and Mercury Oxycpanidcs . . . . . JOANNIS .MENSCHTJTKIN (N . ). Determination of the Reaction-values of the Com- . . . . . . . .HENRY (L.) . .MARKOWNIKOFF (W.). Dichlorhydrin and its Oxidation-products . .ponents of Alcohols and AcidsAction of Hypochlorous Acid on Propargylic CompoundsWILLIAMS (E.). Absorption of Moisture by GlScerol . . . . .HENRY (L.). Pyruvic Alcohol and its Derivatives . . . . .LEVALLOIS (A.). A Sugar present in the Grain of soja hispidrtBEVAN (E .T.) and C . F . Clzoss .REBOUL (E.). Action of Methylamine on Xpichlorhydrin . . . .SILVA (R . D.). Gljceric EtherMICHAEL (A.). Preparation of Formic Aldehyde . . . . .. . .Bast Fibres . I11 . . . . .. . . . . . . . .PAGE102910301030103010311031103210321033103310331033103410351035103610371038103910391040104110411041104110421043104.4.10451045104610461 04 7104’711131113111411141116111711201120112011211121112111221122112CONTEXTS . xsxiiiPAGECLARKE (F . W.) and MARY OWENS . Some New Cranium Salts . . .Substituted Acrylic Acids from Bromopro-Di-iodobromacrylic and Chloro-1124HILL (H.) and C . F .MABERY .MABERY (C . F.) and RACHAEL LLOYD .piolic Acid . . . . . . . . . . . . 1124bromacrylic Acids . . . . . . . . . . . 1125SCHMIDT (E.). Methylcrotonic and Angelic Acids . . . . . 1126Acids . . . . . . . . . . . . . 1126SENFP (M.). Substituted Glycollic Acids . . . . . . . 1127(Homoitaronic Acid) . . . . . . . . . . 1127MICHAEL FA.). A New Formation of Ethqlthiocarbimide . . . . 1128SCHMIDT (E.). Calcium Double Salt of MethJicrotonic and IsobutylformicMARKOWNIKOFF (W.) and A . KBEYTOWNIKOFF . Tetrylenedicarboxylic AcidSMITH (W.). Certain Volatile Products in Crude Coal-tar Benzenes . . 1128SADTLER (S . P.) and I€ . G . MCCARTER .Destrurtive Distillati011 of Petroleum . . . . . . . 1128MIXTER (W . G.) .Sulpliate . . . . . . . .. . . . . 1129TIUBNER ( H . ) . Anhydro-compounds . . . . . . . . 1130SARAUW (E.). Quitlone Derivatives . . . . . . . . 1135WEDDIGE (A.). Ethylenic Ethers of Phenol and Xitrophenol . . . 1136into Phenols and Aroniatic Acids . . . . . . . . 1140MERLIhCf (G.). Addition-products of Atropic Acid . . . . . 1143MICHAEL (A) . Sthylphthalic Acid . . . . . . . . 1147FISCHER (H ) . Reeorcinolsulphonates . . . . . . . . 1147LTTZGE ((3.). Preparation of Pure Naphthalene . . . . . . 1151BALLANT . Phytolacca dioi'ca . . . . . . . . . 1151BOWMAN (W . J.). Aspidiumrigidurn . . . . . . . 1152d R A T a (P . N.). Qiiebrachitannic Acid . . . . . . . 1162DUDLEY (W . L.) Spigeline, a New Volatile Alkaloid . . . . .HESSE (0.). Methyl Ether of Morphine . . . .. . . 1153DE VRIJ (J.). Quino'idine Borate, a New Febrifuge . . . . . 1154OUDEMANS (A . C.). Conquinamine . . . . . . . . 1154HESSE (0.). Conquinamine . . . . . . . . . . 1156LADXNBURGC (A.). Alcamines . . . . . . . . . 1157BODEEER (K.). Lycopodine . . . . . . . . . . 1158RITTHAUSEN (H.). Vicin and Convicin . . . . . . . 1158SPRINGER (A.). Ethjl Glycocholate . . . . . . . . 1160Pecrocene, a Product of theCompounds of Aromatic Amines with Silver Nitrate andBENEDIKT (R.) and A . v . HUBL . Dinitro- and Trinitro-resorcinol . . 1132WESELSKY [P.) and R . BESEDIKT . Ethers of Quinol and Orcinol . . 1139SEN~OFER (C.) and F . SARLAY . Direct Introduction of Carboxyl-groupsCURTIUS (T.). Action of Bmzoic Chloride on Glycocine-silver . . . 1144HART (E.).Nitrosulphohenzoic Acids and some of their Derivatires . . 1144MICHAE; (A.). 1150-VIGIEB (F.) and C . CLOEZ . Eeseilce of Zriywoa canadense . . . 1151A New Formation of Stilbene and some of its Derivatives .1163RITTHAUSEN (H.) . Action of Salt Solutioiis on Conglutin and Legumin . 1160Pli y siol ogicnl Chemistry .MUNK (E.) and others . Nutritive Value of Glycerol . . . . .KELLNER (0.). Relations between Work and the Decomposition of Food intheBody . . . . . . . . . . . .BROWN (I€ . T.) and J . HEBON . Hjdrolytic Action of the Pancreas andSmall Intestine . . . . . . . . . . .ENGEL (R.). Phenol in the Animal Economy . . . . . .XUBNER (M.). Decomposit. ion of Pease in the Intestine of Man . . .MOTT (H . A.). Effects of Alumina Salts on Digestion .. . . .CAMERER . Researches on Tissue Change in Children . . . . .VOlT (E.). Iniportance of Lime to the Animal Organism . . . .BORNTR~GER (A) . Urine after Administration of Quinine and Morphine I)VOL . XL . C1141141141141871f918919019sxxiv CONTENTS.DRECHSEL (E.). Formation of Urea in the Animal Organism . . .STUTZER (A.). Action of Acid Gastric Juice on the Nitrogenous Consti-tuents of Fodder . . . . . . . . . . .KELLNER (0.). Researches on the Digestion of Proteids . . . .SCHRODT (M.) and others. Feeding Cows with Rice Meal . . . .BECPHUSEN (H.). Results of Fattening Calves with Skimmed Milk . .LEPINE (R.) and FLAVARD. .MALY (R.). Formation of Free Sulphuric Acid in the Gasteropoda . .DONATH (J.) .Physiological and Physiologico-chemical Effects of QuinolirieKERN (E.) and H. WATTENBERG. Duration and Composition of the Increasein Li-oe Weight of Lambs when Fattening . , . . . .DARBY (S.). Fluid Meat . . . . . . . . . .RTJBNER. Fluid Meat . . . . . . . . . . .GRUBER. Elimination of Nitrogen from the Animal Body . . . .GRUBER. Influence of Borax on the Decomposition of Protei'ds . . .FEDER and VOIT. Formation of Urea from Ammonia Salts of Organic AcidsXULZ (E.). Formation of Glycogen in the Liver . . . . . .KULZ (E.). Influence of Severe Bodily Exercise on the Amount of Glycogenin the Liver . . . . . . . . . . . .XULZ (3.). Influence of Cold on the Amount of Glycogen in the Liver .KULZ (E). Does Injection of Sodium Carbonate into the Portal Vein causethe Disappearance of Glycogen from the Liver ? .. . . .KULZ (E.). Nature of the Sugar found in the Liver after rigor morfis .KULZ (E.). Amount of Glycogen in the Liver and Muscles after Death .KULZ (E.). Does Glycogen occur in the Blastoderm of the Chick ? . .KULZ (E.). Formation of Glycogen in Muscle . . . . . .KULZ (E.). Glycogen in the Livers of Hybernating Animals . . .BLAKE (J.) . Relation between the Molecular Properties of Inorganic Coin-pounds and t8heir Action on Living Animal Organisms . . . .WEITH (TIT.). Relation of the Number of Fish to the Lime present inWaters . . . . . . . . . . . . .FLEISCHMANN (IT.) and P. WEITH. Quantity and Quality of Milk yieldedby Different Races of Cows . . . . . . . . .FORSTER (J.).Composition of Human Milk . . . . . .DEMANT (B.). Serum Albumin in Muscle . . . . . . .XOSSEL (A.). Phenol Ethers in the Animal Body . . . . .SOTNISCIFEWSPY. Glycerolphosphoric Acid in R-ormal Human Urine . .SCHIFFER (J.) Occurrence and Origin of Methylamine and Illethylcarba-mide in Urine . . . . . . . . .NENCKI (M.) and P. GIACOSA. Oxidation of Aromatic Hydrocarbons in theAnimal Organism . . . . . . . . . . .FLEISCHER (R.). .EXKEN (F.). Influence of Malt Liquids on Digestion . . . . .I~OLRERG (L.). .MUNTZ (A.). Influence of Food on the Canstitution of the Fat of Animals .MOLESCHOTT and others. Influence of Light on Chemical Action inAnimals. . . . . . . . . . . . .WOLBERG (L.) . .Fattening of Shecp . . . . . . . . . . .MALY (R.).Changes of Temperature during Digestion . . . .Fattening Pigs with the Soja-bean . . . . . . . .Fattening Pigs with Fleshmeal . . . . . . . . .XELLNER (0.). Comparison of the Influence of Field Beans and Lupines onthe Production of Milk . . . . . . . . . .BBCHAMP (J.). Presence of Alcohol in the Aninid Tissues . . .CAZEXEUVE. Lactic Acid Fermeiitation in Urine. . . . . .SCHRODER JW.) and others. Formation of Hippuric Acid in the AnimalOrganism . . . . . . . . . . . .T ) ' A 4 ~ ~ ~ ~ ~ T ~ L (A.). Animal Heat . . . . . . . .Incompletelv Oxidised Sulphur in the UrineInfluence of Alcohol, Beer, and Wine on Digestion .Influence of Certain Salts and Alkalo'ids on DigestionInfluence of certain Salts and Alkalo'ids on Digestion .PAUE19229629629 729729829829845045045145145345362662666'76276286286296296296296306306:'063068 163163 16327557537524 0283 583483492691 792792792892892810.19*-'&&OM and D~TZEL. Nutritive Value of Gelatin .. . . . . 101'CONTENTS . xsxvPAGERUBNER (M.). Absorption of Food passin? through the Human Body . 1050LUNIN (N.). Importance of Inorganic Salts in Feeding Animals . . 1050D'ARSONVAL (A.) and COUTY . . 1051ROBERTS (W.).Pancreatic Extracts . . . . . . . . . . 1031MITSCHEE-COLLANDE (F.).Effect of Mat6 on the Gases of the BloodEstimation of the AniSloljtic and Proteoljtic Activity ofRelation of wool to Body Weight in MerinoSheep . . . . . . . . . .. . 1054of the Urine in Disease . . . . . . . . . 1055by Man at Rest . . . . . . . . . . . 1056NEELSOW (F.). Blue Milk . . . . . . . . . . 1055RUSSELL (W . J.) and S . WZST . Relation of the Urea t o the Total NityogenWEST (S.) and W . J . RUSSELL . Amount of'Nitrogen Excreted in the UrineMACMTJKN (C . A.). Researches on the Colouring-matters of Human Urine . 1056KENNEPOHL (G.). Nitrogcnous Constituents of Excrement . . . 10%PAVY (E . W.). 1058BRUNTON (T . L ) and T . CASH .Hydrocyanic Acid, on Muscle and Ncrve . . . . . . 1058WILLIAMS (C . G.). Physiological Action of B-Lutidine . . . . 1058DUBELIR (D.). Influence of the Continued Use of Sodium Carbonate on theComposition of the Blood . . . . . . . . . 1161BOUCHERON (F.). Abnormal Presence of Uric Acid in the Salira,Gastric Juice, and other Secretions .. . . . . . 1161DEICHM~LLEE (A.). Diabetic Urine . . . . . . . . 1162TOLLENS (B.). Diabetic Uriuc . . . . . . . . . 1162PORTELE (K.). Milk of Tyrolese Cows . . . . . . . 1163and their Artificial Production from Bilirubin and from HaenlatinPhysiology of Sugar in the Animal System . . . .Action of Ammonia and its Salts, and ofChemistry of Vegetable Physiology and Agriculture .BUCHNER (H.). Artificial Generation of Spleen Fungus . . . .LADUREAU (A.). The Function of Fat in Germination . . . .KEAUS (K.). Growth of Sprouts on Potatoes . . . . . .MAQUENNE . Vegetation of Oil-producing Plants . . . . . .MEUNIER (F.). Distribution of Sugar in Sorghum . . . . .OEHME and others .Successful Growth of Flax in Saxony . . . .WOLLNY (E.). Cultivation of Beet . . . . . . . .BRIER (C.) and L . JEIILE . Experiments with various kinds of Beet . .PAGNOUL (A.) . Cultivation of Beetroot . . . . . . .WOLLNY (E.). Influence of Trenching on the Temperature and Moisture ofSoil . . . . . . . . . . . . .RIEGLER (W.). Descent of Rain-water down Tree-steins . . . .DEHBRAIN (P . P.) and MEYER . Worthlessness of Phosphates as Manure forCertain Soils . . . . . . . . . . . .SCHTJMACHER (A.). Manuring Experiments on Arable Land . . .PO~~E-ROGGOW (H.) . Manuring Experiments with Mangold Wnrzel andBeet . . . . . . . . . . . . .HOLDEFLEISS . Analysis of Pond Slime . . . . . . .PATOW.LALENDORF . Best Method of Manuring Potatoes . . ..DUDOTTY (A.). Manuring of Beetroot . . . . . . . .TIEGHEM (P . v.). Alcoholic Fermentation in the Roots of an Apple Tree .EJELDAHL (M . J.). Fermenting Power of Diastase . . . . .PELLET (H.). Ammonia in Plants . . . . . . . .LADUREAU (A.) . Chemical Composition of Linseed . . . . .GRANDEAU (L.) and A . LECLERC . . . . .VOELCEER (A.). Fattening of Oxen . . . . . . . .SCHIRXER.NEUHANS . Cultivation of Furze . . . . . . .PUTTKAMMER and others . Use of Lupiiies as Fodder . . . . .BOHN (J.). Pressure in Plant Stems . . . . . . . .HULWA (F.). Curapao Guano . . . . . . . . .Composition of Oatsc 25959606060606060606060616161( i lc i l61616111531511611611611613611sxxvi CONTENTS .~IARZ (C .0.). Cultivation of Soja Bean . . . . . . .GODEFROY (J.) and A . DOUDOUP . .SCHILLER (R.). Drainage Water from Moorlands . . . . .ALBERT (H.) and R . WAGXER . Behaviour of Phosphates in Water chargedwith Carbonic Acid . . . . . . . . . .PITSCH (0.). Organic Matters in Soil ; Examination of Grandeau’s Theory .MORGEN (A.). Solubility of Certain Slaniire Materials . . . . .WEIN (E.). Experiments with Various Phosphates as Manure . . .3Ianure for Fruit Trees . . . . . . . . . . .~VAGNER (P.) and H . PRINZ . Manuring of Vines . . . . .~ A G E L I (v.) and 0 . LOEW . Nutrition of the Lower Orders of Fungi byCarbonaceous and Nitrogenous Matter . . . . . . .KRAUS (C.). Influence produced on the Growth of the Plant by previouslyFLEISCHER (M.). Injurious Effect of Kainite and Superphosphate on theGermination of Potatoes .. . . . . . . .RICCIARDI (L.). Comparison of Diseased and Sound Lemon Trees . .HEIHE (F.). Cultivation of several Varieties of Potatoes . . . .PETERXANN (A.). Analysis of Cocoa and Palm-meal . . . . .KLEIN (G.). Experiments on Sugar-beet . . . . . . .PETERMAKN (A.). .RELLR’ER (0.). Changes produced in Beet-leaves by Permentation . .KELLER-EDERSTADT (A.). Flesh-meal as Fodder . . . . . .MENDEL (H . J.). Preparation of Food for Pigs . . . . . .a 4 ~ ~ f o s (G.). Permeability of Soils to AirSEELI-IEIM (F.). Percolation of Wat. er through Soils . . . . .DUNKELBERG and others . Artificial Manures . . . . . .On Sandy Soils and Manuring with Artificial Manures . . . ..FITTBOGEN (J.). Manuring Potatoes . . . . . . . .Rendering Acid Gases Inactive . . . . . . . . .Spores . . . . . . . . . . . . .posed to Rain . . . . . . . . . . .Cultivation of various kinds of BeetWEIN (E.), Pigeons’ Dung . . . . . . . . . .WEIN (E.). Growth of Yellow Lupines . . . . . . .Steeping the Seed . . . . . . . . . . .Composition of “ Diffnuion” and “ Press” Residues. . . . . . .SCIIINDLER (F.).ENNERLING (A.).DBHBRAIN (P . P . and others) .KRAUS ((2.).Influence of Temperature on the Germination of BuntThe Loss which Newly Mown Grass Suffer8 when ex-Cultivation of Potatoes, Maize, Oats, andSainfoin . . . . . . . . . . . .The Influence on the Growth of Potato and Jerusalem Arti-choke Plants of allowing the ‘‘ Sets ’’ to Decay before Planting ..SCHIPIIDT (C.). Examination of various Soils and Subsoils . . . .KOSTITCHEFF . Phosphoric Acid in the Sail . . . . . .BELETZBY . Decomposition of Phosphorite by Peat . . . . .MEYER (L4.). Potassinin Salts as Manures . . . . . . .FIEDLER . Influence of Sodium Nitrate on Absorption of Phosphoric Acidand Potash . . . . . . . . . . . .ALBERT (H.) and SIEGFRIED . Manuring Cress with Dicalcium Phosphate onSoil free from Humus . . . . . . . . . .CRAPEISIS (E.). Action of Ozone on Germs contained in the &r . .Ronx (E.) . .BRIEM (I€.). .LrmENBmm . Fertilisation of Cereals . . . . . . . .COLLIER (I?.). Development of Sugar in Sorgho . . . . . .SCHULZE (E.). Decomposition of Albumin in Plants . . . . .ICUIIN (J.).Investigation into the Cause of Beet Sickness in SoilsComposition of Fodder . . . . . . . . . . .PRESSER (I<.). Cotton-seed Meal as Fodder for Milch Corns . . .~IOLDENFLEISS (I?.). Examination of Liiiqecd-cake and Meal . . .WARDEN (C . J . H.). Analysis of Forage BiscuitsMAYER (A.). Estimation of the Absorptive Power of Soils . . . .A Yeast incapable of Producing Invertive Fermentation .Influence of Heat on the Growth of Beets and Potatoes. .. . . . .PAGE1161171171171171201201211211212992993003003003013013013013023023023023033043043053054554554554564564574574574594<6263%63263 363363463463463663663663763PXTZ (C.). Removal of Iron from Newly Broken Soil .. . . .VOELCKER (A.). Continuous Cropping of Wheat and Barley . . .KONIG (J.). Action of Water in the Process of IrrigationVOELCKER (A.). Rotation of Crops . . . . . . . .GENAY (P.). Experiments with Artificial Manures . . . . .PETERXANN (A) . Composition of Two Samples of Peat . . . .PELT. ET (H.). Constancy in Composition of Plants . . . . .RODEWALD and J . REINKE . Coniposition of Protoplasm . . . .LADUREAU (A.). Chemical Composition of Linfeed . . . . .MEUKIER (F.). Composition of Wheat Ashes . . . . . .LINDE (S.). Clover-sickness . . . . . . . . .PIERRE (I.) and LEMETAYER . Spring Barley as Green FodderPELLET (H.) and M . L~EBSCEINITZ . Analysis of Beet-seeds . . . .DE LEEW . Composition of Brandy Distillery Residues .. . .. . . .FLEISCHER . Manure . . . . . . . . . . .VOELCKER (8.). Comparative Value of Soluble and Insoluble Phosphates .W . H . Potatoes Manured with Peat, “ Nitrophosphatc, ” and PodiumNitrate . . . . . . . . . . . . .. . .PHILIPPAR (E.). On Swedes . . . . . . . . .SIMON.LEGRAND . Comparison of “ Diffusion ” and “ Press ” Residues asFoods . . . . . . . . . . . . ..Comparative Experiments onthe Manurial Values of Soluble, Reduced, and Precipitated PhosphatesPETERMANN (A.). African Guano . . . . . . . .MIQUEL (P.) and L . BENOIST . Sterilisation of Animal and PegetableLiquids . . . . . . . . . . . . .DURST (0.). Microscopic Researches on Yeast . . . . . .MAYER (A.) and others . Fermentation in Presence of Organic Salts ..GAYON (W.). Influence of Succinic Acid on the Fermentation of Canc-sugar . . . . . . . . . . . . .BOUSSINGAULT . Dissociation of Nitric Acid by Vegetation . . . .SESTINI (I?.). Action of Vapours on Seeds . . . . . . .TIEGHEM (P . v.) and G . BONNIER . Torpid Condition of Seeds . . .VOGEL (A.). Ash of Various Parts of a Plant . . . . . .BREYMANN (E.). Crushed Oats as Fodder . . . . . . .OPPENAU ( F . v.). Stripping of Maize . . . . . . . .HABERLANDT (G.). Colour of Clover Seed . . . . . . .KELLNER (0.). Purification and Digestibility of Lupines . . . .ROMANIS (R.). Analysis of Rice Soils froni Burmsh . . . . .PITSCH (0.). The Humus extracted from Soil by Alkalis . . . .MARCKER (M.). Employmerit of Potassium Salts as Manure . . .MAYER (A.).Manuring with Potassium Salts . . . . . .Potassium Salts a8 Manure for Grass . . . . . . . .MAECKER (M.). Stable Dung as Manure for Beet . . . . .MULLEE (A.). Irrigation with Sewage . . . . . . . .ROUSSET and others . .COCHIN (D.). Nature of the Alcoholic Ferment . . . . . .Yeast. and Fermentation . . . . . . . . . .GRAWITZ (P.). Behaviour of Fungi in the Animal System . . . .WIESNER . Influence of Intermittent Light. on the Formation of Cliloro-BRIEM (H.). . . . .LEVY (A.). Influence of Light on the Ripening of Grapes . . . .MACCAGNO (J.). Influence of Atmospheric Electricity on the Growth ofMUNTZ . Cultivation of Hops . . . . . . . . .CAUVET . Evolution of Carbonic Anhvdride bv Plant Roots . . .SCHKODT (M.) and H . v . PE~EH .MULLEE (C.) and W .C . MULLFR.SCHEE~EL .American Fleshmeal for Milch Cowson Sandy Soils . . . . . . . . . . .CHAMBERLAND and ROUX . Non-existence of iWicrozymu &eta . . .Phylloxera vastutrix and Means of Destrojing itphyll . . . . . . . . . . . . .Influence of Light on the Growth of BeetGrapes . . . . . . . . . . . . .PAGE63863863863‘361‘16-1064.16-1161875375375375475575575675775775775s75875883583583583683683683783 i‘8378378378378388388398398408428428428 42925988930930930930931COKTESTS . xssv1s x x viii CONTENTS.NOBBE (F.). Gemination of Fir Seeds . . . . . . .LATOUR (E.). Analysis of Lichen esculentus . . . . . .DSHBRAIN (P . P.).Report on the Experimental Plots a t Grignon in 1879 .JACOBS (F.) and others . Experiments with Potatoes . . . . .FRESENIUS (H.). Specific Gravity of Potatoes . . . . . .MF.ISE . Chunnos Potatoes from Peru . . . . . . . .MARCKER (M.). Preservation of Diffusion Residues from Beet-sugar Manu-facture . . . . . . . . . . . . .PELLET (H.) and C . LE LAVANDIER . Nutritive Value of Diffusion Pulpand Pulp from the Hydraulic Press . . . . . . .KUHN (J.). Prevention of Lupine Sickness . . . . . . .BECQUEREG (E . and H.). Temperature of the Soil under Snow . . .WOOLNY (E.). Influence of Superficial Drying on the Temperature andMoisture of the Soil . . . . . . . . . .DBH~ERAIN (P . I?.) and KAYSER . The Form of Combination in which Phos-plioric Acid exists in the Soil .. . . . . . .ZALOMANOFX (R.). New Nethod of Ascertaining the Absorptive Power ofa s o i l . . . . . . . . . . . . .RADIANU (S . P.). .SCHAFFERT (F.) . Manuring Experiineiits on " Donaumoos " . . .Manuring Experiments at Lutter . . . . . . . . .MARI&DAVY (kf.). Experiments with Sewage . . . . . .SORAUER (P.). Manuring Xxperiments on Fruit Trees . . . .LAUCHE (W.) and A . ORTH . . . .MEDIC~S . Testing the Progress of Putrchction in Manure Heaps . .BIRSER and BEIMMER . Researches on the Changes occurring in StableManure when kept . . . . . . . . . . .Woo1 Waste as Manure . . . . . . . . . . .Preparation of a Maniire from Molasses Waste . . . . . .CHANCELLOX (H.). .WEIN (E.). Cultivation and Manuring uf Legurninom .. . .CILLMPONNOIS and PELLET . Manuring of sugar Beet . . . .NAGELI (C.). Nutrition of the Lower Fungi . . . . . .HAYDUCK (M.). .ATKINSON (R . W.). Diastase of Kbji . . . . . . . .RICHET (C.) Fermentation of Urea . . . . . . . .SOILA-~ER (P.). Studies on Evaporation . . . . . . .WOLLNY (E.). Amount of Water Appropriated by Agricultural Plants .YAJ~INTZIN (A) . Influence of Light 011 tlre Liberation of Carbonic Anhydrideby Plants . . . . . . . . . . . .NAYER (A.) . Infliiencc of an Increased Quantity of Carbonic Anhydride onthe Growth of Plants . . . . . . . . . .SCHIMPER (A . F . W.). Formation of Starch Grains . . . . .SCECIMPER (A . F . W.). Growkh of Starch Gr;iinsMechanical and Chemical Analyses of Roumanian SoilGarden 5Innuring ExperimentsRfanuring of Wheat, Barley, and Oats with SaltpetreInfluence of Rochelle dalts on the Activity of Yeast ... . . .STEBLER .MACH (E.) and K . PORTELE .SCEULZE (E.) and J . BARBIERI .Influence of Light on the Germination of Seeds . . . .Composition of Farious Parts of Grapes .Occurrence of Allantoin in Vegetable Or-ganisms . . . . . . . . . . . . .Injurious Effect of Furnace Gases on the Forests of the UpperHarz . . . . . . . . . . . . .. . . . . . . . .Experiments with Darnel and Lucerne as a Mixture forMeadows . . . . . . . . . . . .VINES (5 . H.). Chemicd Composition of Alewone-grains . . . .HXINE (2.). New English kinds of W'heat . . . . . . .K~AMER (E.). Feeding Value of Alpine Hay . . . . . .XUHN . The Sand Vetch, a New Fodder Plant .. . . . .KEOCKER . Analysis of Plantain Seeds . . . . . . .BIRNER . Effect of the Moisture in Soils on the Yield of Potatoes . .Utilisation of Diseased Potatoes . . . . . . . . .REUSS .Djugara, a New Kind of CornWITTMANN .PAUE931931.932932932932932933934934934934935935935935936936936937937937937938931593810581058105910591059106010601060106110611061106110611062106410651065106510651065106610661G6CONTENTS . xsxisROHL and 0 . HESS . Prevention of Rot in PotatoesDIXOX (W . A.). On Salt-bush and Native Fodder Plants of New South ’SVsles. . . . .KONIG (J.). Money Value of Feeding Stuffs . . . . . .SAMEK (J.). Cultivation of Various Agricultural Plants .. . .Rotation of Crops in Kitchen Gardens . . . . . . . .VALERY-MAYET and others . Researches on Phylloxera . . . .SCHIKIDT (C.). “ Black-earth ” of Russia . . . . . . .LIEBENBERQ . Investigations on Warintli in Soils . . . . .PARSKY (F.). Potash Salts as a &.lanure . . . . . . .RNDOYNAUD (A.) and B . CHAUZIT . Permeation of Water through the Soil .FITTBOGEN and others . Manuring Experiments with Phosphoric Acid inDifferent Combinations . . . . . . . . . .MARCKER (K) Relative Value of Soluble and Insoluble Phosphates asManure . . . . . . . . . . . . .WOLPF (E.) and others . Manuring Experiments to Determine the ValueNANQUETTE and others . Gypsum as Manure . . . . . .LECOUTEUX (E.). Money Value of Stable Nanure .. . . .Lake Mud and Marsh Earth as ManureGround Wood as Horse LitterGAUDICH (H.) and others . Manuring Experiments on Oats . . . .ZOEBL (A.) Manuring Experiments with Summer Barley . . . .TIEDE (H.). Manuring Potatoes . . . . . . . . .PETERS (J . F.) Manuring Experiments . . . . . . .of Phosphoric Acids Soluble in Citrate Solution . . . . .. . . . . . .. . . . . . . . .TAPPENTHAL (H.) and others . .MARCKER (M.). Manuring Experiments with Sugar-beets . . . .NERGER (C.). Comparative Manuring Experiments . . . . .TEAUB (C . G.). Bark of Sambucus canadensis . . . . . .LECHARTIER (G.). Analyses of Buckwheat . . . . . .FASSBENDER (G.) . Analyses of Fodder . . . . . . .TUXEN (C . F . A.). Absorption of Salts by the Soil . .. . .TUXEN (C . F . A.). Grandeau’s Theory of the Fertility of a Soil . . .KROCKER and H . CRAHL . 3Ianuring Experiments with various PhosphatesManuring Experiments with Potatoes .Arzaiytical C1temisti.y.SCEWARZ (H.). Apparatus for the Volumetric Estimation of Nitrogen .BOLTON (H . C.). . . . .GBUPE (A.) and others . Estimation of Retrograde Phosphoric Acid . .MILLOT (M . A.). Retrograde Phosphoric Acid . . . . . .LEPEL (B . v.). Alkanet Red as a Test for Magnesium Salts . . .LEPEL (F . v.). Vegetable Colouring Matters as Tests for Magnesium Salts .WILM (T.). Chromium Sesquioxide . . . . . . . .HEME (0.). The O5cinal Test of Quinine, and Water of Crystallisation ofQuinine Sulphste . . . . . . . . . . .KERNER (G.). Testing Commercial Sulphate of Quinine for Foreign Alka-londs .. . . . . . . . . . . .MEDICUS (L.) and others . Butter Analysis . . . . . . .DUPRB (A.) . On Accurate Perception of Colour-change in Titration . .ZIMMERMANN ((3.). Action of Uranyl Salts on Turmeric Paper . . .ZIMMERNAXN (C.). Separation of the Heavy Metals of the AmmoniumSulphide Group . . . . . . . . . . .BING (I.). Occurrence and Estimation of Nitrates in some Vegetable Sub-stances . . . . . . . . . . . . .OSSIKOVSZKY (J.). Arsenious Sulphide as a Poison, and its Importance inJudicial Cases . . . . . . . . . . .VANDERBURG (E . A.). Ash of Light-coloured Cod-liver Oil . . .SCHWARZ (€1.) and P . PASTROVICH . Elementary Analysis of 01.ganic Saltsof Alkalis and Alkaline Earths . . . . . . .Action of Organic Acids on MineralsPAGE1066106710671069106910691070107110711072107210731075107610761077107710771017107810181078107910791163116411651165116611676262626262636363636612112212212212312412Sl COSTEXTS .VANDERBURG (E .A.). Analysis of Iodine-iron Cod-livey Oil . . .FLUCKIGER (F . A.). Testing of Mustard Oil . . . . . .FLAVART . Apparatus for the Estimation of Nitrogen in Organic Com-pounds . . . . . . . . . . . . .STAEDEL (W.). Apparatus for the Collection of Nitrogen in ElementaryAnalysis . . . . . . . . . . . . .LUX (F.). Simp!e Aspirator . . . . . . . . . .KONINCK (L . L . DE) . Solution of Bromine as a Reagent . . . .Lux (F.). Flavescin, a New Indicator .. . . . . . .WAGXER (A.). Analysis of Gunpowder . . . . . . .LUNGE (G.). Determination of Sulphur in Pyrites . . . . .HASWELL (A . E.). Quantitative Determination of Phosphorus and Siliconin Iron and Steel . . . . . . . . . . .PEITZSCH (B.) and others . Estimation of Phosphoric Acid . . . .OTTO (R.). Detection of Zinc in Toxicological Cases . . . . .REICHEL (F.). Qualitative Separation of Cobalt from Nickel . . .FISCHER (E.). Separation and Estimation of Arsenic . . . . .REICHARDT (E.). Detection and Estimation of Arsenic . . . .MAYER (L.). New Method for the Estimation of Arsenious in presence ofArsenic Acid . . . . . . . . . . . .BAUDRINONT (E.). Analysis of Bismuth Subnitrate . . . . .WAGNER (A.). Deterniination ot’ Ash in Coal and Coke .. . .SMETHAM (A.). Estimation of Organic Carbon in Potable Waters . .PERKINS (F.). Determination of Carbon in Water Residues . . .CAZENEUVE and COTTON . .REBOUL . Wine from Raisins . . . . . . . . .KNIGHTS (J . W.). Estimation of the Insoluble Patty Acids in Butter . .CAEPENTIN . Estimation of Batty Acids in Oils . . . . . .RBYONT (A.). Analysis of Heavy Mineral Oils, of Rosin and Fatty Oils,and of Rosin in Oils of Commerce . . . . . . . .SCHACHT (C.). Estimation of the AlkaloYds in Quinine Wine . . .KAPOUSTIN (M.). Rapid Estimation of Atmospheric Carbonic Anhydride .WAGNER (A.). Limits of Error in Analysis of Combustion Gases . .FASSBENIIE K. (G.) . Quantitative Determiuatiou of Albumin by CupicHydrate . . . . .. . . . . . . .PIESSE (C . H.) and L . STANSELL . Analyses o€ Black and White Mustard .PELLIEUX (J.) and E . ALLAKY . . . . .WEYL (T.) and X . ZEITLER . Oxygen Absorption of Alkaline Pyrogdlate .HOFMANN (A . W.) . Estimation of Small Quantities of Carbon Uisulphide .MACAGNO (J.). Estimation of Carbon Bisulphide . . . . .SELMI (F.). Cliemical Toxicology of Phosphorus . . . . . .EMMERLING (A.). Determination of the Helative Values of Precipitatedand Soluble Phosphates . . . . . . . . . .BERNTHSEN (A.). Use of Sodium Hyposulphite, NaBS02, in the EstimationBEBNTHSEN (A.). and A . DREWS . Titration of Hjposulphite with IndigoCarmine . . . . . . . . . . . . .SELMI (B’.). Chemical Toxicology of Arsenic . . . . . .SCHULZE (E.) and J . BARBIERI .Estimation of Nitrogen-compounds inPlants . . . . . . . . . . . . .JAY (H.). Detection of Alcohol in Transparent Soaps . . . . .CASALI (A.). Testing for Sulphuric Acid in Wine and in Vinegar . .KONIG (F.). Detection of Rosaniline in Wine . . . . . .HESSE (0.). Optical Estimation of Cinchoiiidine in Commercial QuinineSulphate . . . . . . . . . . . .CARXELUTTI ((3.) and L . VALENTE . Estimation of Glucose in Urine . .ESBACH (G.). Urea, Sugar, and Sodium Hypobromite . . . .WaxandHoney . . . . . . . . . . . .PETERMANN (A.) . Presence of Corn-cockle Seeds in Meals . . . .PILETI (U.). Notes on Gas Analysis . . . . . . . .Detection of Methyl Alcohol in Ethyl AlcollolAn lodometric Processof Copper, of Indigo, and of Oxygen dissolved in Water . .. .rAa E12 412519219219219319319319319419419419419519519519619619619719719820120320220420420520520530’730730830830030931031031131231431431431531531631631746COKTESTS .POUCHET (A . G.). Destruction of Organic Matter when Searching forMetallic Poisons . . . . . . . . . . .MORGEN (A.) . .KONIG (A.) . Estimation of Retrograde Phosphoric Acid by iiieans of Ammo-nium Citrate . . . . . . . . . . . .DREWSEN (S.). Estimation of Soluble Phosphate in Superphosphates . .EGGERTZ . Determination of Phosphorus in Iron and Iron Ores . .P~REER (J . 8.). Varying Condition of Carbon in steel, and its Influence onEggertz’s Process . . . . . . . . . . .LARSEN (G.).Separation of Copper and Zinc by Precipitation with Sulphu-RHICHEL (F.). Estimation of Arsenic as Magnesium Pyroarsenate . .BRAME (C.). Use of Baryta to obtain Metallic Arsenic from ArseniousMARECK (F.). Quantitative Determination of Silver in Galvanic Silver-baths . . . . . . . . . . . . .MUNTZ (A.) aiid E . AUBIN . Estimation of Carbonic Anhydride in the Air .ENGLER (C.) and R . HAASE . Apparatus for Testing the Inflammability ofPetroleum . . . . . . . . . . . .BERT HELOT . Remarks on the Properties of Vapours of Chlorinated OrganicCompounds . . . . . . . . . . . .CLAUSNIZER (F.). Estimation of Glycerol in Beer . . . . .HEMPEL (W.). Estimation of Nitroglycerol in Dynamite . . . .BORNTRAGER (A.). Detection of Salicylic Acid in Urine .. . .Use of the Azotometer for Agricultural InvestigationsKONINCK (L . de) . Aluminium Phosphate . . . . . . .retted Hydrogen . . . . . . . . . . .Oxide and Arsenic Sulphides . . . . . . . .MARCHAND (E.). The Acidity of Milk . . . . . . .MASON (A . H.). Adulterated Linseed Oil . . . . . . .FRAUDE (G.) . Test for Quebracho Bark . . . . . . .LOWENTHAL (J.). Estimation of Tannin . . . . . . .RIMMINGTON (F . M.). Analysis of Coffee . . . . . . .PAWLEWSKI (B.). A Simple Method of Determining Boiling Points . .BOLTOK (H . C.). . . . .DALKOWSEI . Quantitative Estimation of Chlorides in Urine . . .FIELD (F.). Detection of Iodine in Urine . . . . . . .FIELD (F.). Laboratory Observations . . . . . . . .KONIG . Estimation of Small Quantities of Phosphoric Acid .. .FLEISCHER . Insoluble PhosphateEstimation . . . . . .PHIPSON (T . L.). Grains of Silica and Micrococci in the Atmosphere . .ILES (M . W.). Decomposition of Slags and Silicates . . . . .DROWX (T . M.). Determination of Sulphur in Sulphides and in Coal andCoke . . . . . . . . . . . . .CLAESSON (P.). Characteristic Colour Reactions with Sulphydmtes . .ARNOLD (J . 0.). Estimation of Phosphorus in Steel . . . . .ARNOLD (J . 0.). . . .DROWN (T . N.) and P . TiT . SHIMER . Estimation of Silicon and Titanium inPig Iron and Steel . . . . . . . . . . .BETTEL (W.). Determination of Basic Cinder and Oxides in Manufac-tured Iron . . . . . . . . . . . .CHITTENDEN (R . H.) and H . H . DONALDSON . Detection and Estimation ofArsenic in Organic Matter .. . . . . . . .FIELD (F.). Detection of Small Quantities of Platinum . . . .WEYL (T.) and X . ZEITLER . Relation between the Oxygen and OrganicMatter found in Natural WatersKOENIB (F.). Apparatus for Studying the Diffusion of Carbon Bisulphide inthe Ground . . . . . . . . . . . .SKALWEIT (F.). Examination of Petroleum . . . . . . .ALLEN (A . H.). Notes on Petroleum Spirit and Allied Liquids . . .BOTJSSINC+AULT (J.). Rapid Alcoholic Fermentation . . . . .ALLEN (A . H.). Specific Rotatory Power of Cane and Invert Sugar . .. Swecific Rotatory Power of Cane and Invert Sugar . . .Action of Organic Acids on MineralsEstimation of Chromium in Iron and Steel. . . . . . . .xliPAGE46346446446546546546646746 7a746846846947047047.24734734734736426-1264364864464q b64564564564664661664764864864965065065065 16526534472417364.xlii CONTENTS.CASAMAJOR (P.) .Detection of Starch-sugar Mechanically Mixed with Com-mercial Cane-sugar . . . . . . . . . .RULZ (E ). Quantitative Estimation of Glycogen . . . . .WALLER (E.). Testing of Phenol . . . . . . . .FENTON (H. J. H.). Tartaric Acid Reaction . . . . . ,KRAKAO (A.). Quinoline Reactions . . . . . . . .ST. CAPRANICA (S.). New Guanine Reaction . . . . . .HAXLET (W. M.). Estimation of Fat in Milk . . . . . .SOXHLET (F.). .CALDWELL ((3. C . ) . Milk-testing with the Lactobutyrometer . . .GEILBER (N.) and others. Milk Analysis . . . .. . .MACAGNO (H.). Detection of Aniline Colours in Red Wine . . .SPILLER (J.). Identification of Coal-tar Colours . . . . .STGTZER (A.). Quantitative Estimation and Separation of Protei’n Matter inPlants . . . . . . . . . . . . .GOTTWALT. Quantitative Analysis of the Albumino’ids of the Kidney Sub-stance . . . . . . . . . . . .HUGHES (J.). Analysis of Shoddy and Wool Waste . . . . .ZIXXRRMAXN (C.) . Use of Yotasaium Permanganate in VolumetricAnalysis . . . . . . . . . . . .KONIQ (A.). Influence of Ammonia on the Estimation of Bicalcium Phos-phate . . . . . . . . . . . . .GRUPE (A.) and B. TOLLENS. Action of Citric Acid on Phosphates . .DONATH (E.). Direct Estimation of Alumina in Presence of Iron . .DONATH (E.)* Volumetric Determination of Chromium and Manganese inPresence of Ferric Oxide and Alumina .. . . . . .DONATH (E.) Separation of Silver from Lead . . . . . .HESSE (W.). Quantitative Estimation of Dust in Workshops . . .PIZZI (L4.). Detection of Logwood in Wine . . . . . .MEUNIER (F.). Asparagine . . . . . . . . .HAUSAMANN (0.). Determination of Undecomposed Fat in Mixtures of FattyAcids . . . . . . , , . . . . .v. BORRIES ((3.). Composition of Milk from the same Cow on ConsecutiveDays . . , . . . . . . . . . .TISSANDIER ((3.). Dust in the Air . . . . . . . .TERREIL (A.). Volumetric Determination of Peroxides . . . .KESSLER (F.). Employment of Potassium Permanganate in QuantitativeAnalysis . . . . . . . . . . . . .REIS (M. A. v.). Use of Oxalates in Analysis .. . . .MAGAGNO (H.) . Strength of Solutions of Sulphur in Carbon Bisulphide, andits Application to the Analysis of Sulphur Ores . . . . .GRUPE (A) and B. TOLLENS. Action of Ammonium Citrate on Phos-Areometric Method for the Estimation of Fat in NilkPAGE6546.5565565565565565665665765765965966066166175075075576076076076176 176 1’762762843843843843844phates . . . . . . . . . . . . . .TERREIL (A.). Solubility of Tricalcium Phosphate in Ammoniacal andNeutral Alkaline Salts . . . . . . . . . .HERCHER (R.) and P. WAGNER. Employment of Ammonium Citrate inExamination of Phosphates in Manure . . . . . . .ANTZ (C.) and E. ERLENMEYER. Action of AmmoniumCitrate on Phos-WARDER (R. B.). Alkalimetry with Yhenolphthale‘in as Indicator ..MossE (H. N.). Estimation of Barium as Chromate . . . , .KUPFER-SCHLBGER. Separation of Zinc from Cadmium . . . .ROUX. Quick Method for the Estimation of Lead . . . . .HASWELL (E,). Titration of Iron with Sodium Thiosulphate . . .KNUBLAUCH (0.). Determination of Ethylene and Benzene Vapour in Coal-gas. . . . . . . . . . . . . .MULLER (W.) and J. HAGEN. Sensitiveness of Trommer’s Test and Fehling’sSolution as a Qualitative Test for Sugar . . . . . . .TOLLENS (B.). Scheibler’s Method of Estimating Sugar in Beet . . .KNAUER (I!.). Value Constant fOT Beet . . . . . . .phates . * . . * . . . . . . .84584584684784884884984984985085 1.85 185COXTENTS .SHARPLES (S . P.). Determination of Fat in Milk .. . . . .MACAGNO (H.). Detection of Artificial Colouring Matters in Red Wines byMeans of the Spectroscope . . . . . . . . .DITT-MAR (W.). Differential Method of Specific Gravity Determination .WANKLYN (J . A.) and W . J . COOPER . New Apparatus for Use in GasAnalysis . . . . . . . . . . . . .LOWE (J.). Note on Incineration . . . . . . . . .BUNTE (H.). Analyses of Furnace Gases . . . . . . .MULLER (C.). .SALZER (T.). Nessler’s Test for Ammonia . . . . . . .HERZFELD (A.) and G . FEUERLEIN . Estimation of Reduced and Precipi-tated Phosphates . . . . . . . . . . .ZUCESCEWERT and WEST . Estimation of Potassium as Platinochloride .FRESENIUS (B.). Solubility of Cadmium Sulphide in Ammonium Sulphide .ARBOLD (C.). Fehling’s Solution .. . . . . . . .MORSE (H . N.) and W . C . DAY . Determination of Chromium in ChromeIron Ore . . . . . . . . . . . .BARDP (C.). Wood Spirit for making Methylated Spirit . . . .HIRSCIISOHN (E.). Comparative Experiments on the Behaviour of ThymolEstimation of Phosphorus in Slag from Blast Furnaces .Determination of Sulphur . . . . . . . . . .and Phenol with Different Reagents . . . . . .HAYDUCK (M.). Determination ofv Starch in Pressed Yeast . . .GLADDING (T . S.). Estimation of Carbonic Anhydride . . .Mvsso ((3.). .R~MONT (A.). Estimation of Salicylic Acid in Beverages . . .PETIT (A.). Rapid Estimation of Uric Acid . . . . .MYLIUS (B.). Estimation of Morphine in Opium . . . . .CONROY (&I.). Adulteration of Olive Oil .. . . . .Examination of Milk . . . . . . . . . .BACHMEYER (W.) . Tannic Acid as Alkalimetric Indicator . . .GRIESMAYER (V.). Valuation of Barley . . . . . .FLUCEIQER (F . A.). Testing Peru Balsam . . . . . .PICCINI (A.). Separation and Estimation of Nitric and Nitrous AcidsCARNOT t A.) . SerJaration of Aluminium from Iron and ChromiumLactic Acid in, and Alcoholic Fermentation of MilkCECH (C . 0.). Valuationof Hops . . . . . . .GROVES (R . H.). Borntrager’s Alocs Test . . . . . .DEPRESNE . Estimation of Peptones . . . . . . ..CLASSEN ‘(A:) andlM . A . v . REIS .JOHWSON (S . W.) and R . H . CHITTENDEN .MAURO (F.) and L . DANESI .Elcctrolytir Estimations and SeparationsDistribution of Arsenic in theAnimal Body . . . . . . . . . ..New Method for the Volumetric EstimationDELVAUX (G.). Separation of Nickel and Cobalt . . . . .of Molybdenum . . . . . . . . . . .COUTTOLENC ((3.). Evaporation of Glycerul . . . . . .MAUMENB (E . J.). New Method of Anall-sing Oils . . . . .MACCAGKO (I.). Estimation of Tannin in Sumach . . . . . NINGER (F.). Influence of Frost on Bndjses of Sugar-beets . . .QUINQFAUD . Estimation of Urea by Means of Standard Sodium Hypobro-mite . . . . . . . . . . . . .ST . MARTIN (L.). Estimation of the Residues of Wines . . . .KLEIN (M . D.). A Solution of Density 3’28 suitable for the Analysis of MineralsGOOCII ( F . A.) . Estimation of Phosphoric Acid as Magnesium Pyrophos-pliate . . . . . . . . . . . . .LINDO (D.). Estimation of Potassium as Ylatinochloride .. . .REINHARDT (H.) and R . IHLE . Electrolytic Estimation of Zinc . . .BROWN (T . M.). Reduction of Iron-ores by Powdered Zinc . . . .MOORE (T.). Separation of Cobalt and Nickel from Iron . . . .COBENZL (A.). Separation of Tungsten from Antimony, Arsenic, and ITon .WIGNER (G . W.) and R . H . HARLAND . Action of Potassium PermanganatesliiiPAGE8518529389399399399399409.1094094194194294294694294394494494494594594694694694694694694794710801081108 I10821082108310F4108410841085108610861168116811691179117011711171.on Potable Waters a t Different Temperatures . . . . . 117sliv CONTENTS .WEST-KIJIGHTS (J.). Estimation of Nitrates in Potable Waters .. .PFJRKINS (F . P.). Estimation of Nitrates in River Water . . . .HARVEY (S.). Detection of Lead in Potable Waters . . . . .BARDY (C.j. Assay of Wood-spirit for the Preparation of MethylatedSpirit . . . . . . . . . . . . .MUTER (J.). Volumetric Estimation of Glycerol . . . . .LUDWIG (E.). and J . WAUSHNER . Detection of Hydrocyanic Acid . .CROSS (C . F.). .PELLET (H.) and J . DE GROBERT . Determination of Salicylic Acid in Food-New Demonstration of Carbonic Anhydride in the Breathstuff s by a Colorimetric Reaction . . . . . . . .HILL (A.). Estimation of Tannin in Tea . . . . . . .BLYTII (A . W.). Estimation of Quinine . . . . . . .ALLEN (A . H.). Isolation of Strychnine . . . . . . .DYER (B.). Analysesof Milk . . . . . . . ..CAMERON (C . A.). Analyses of Milk . . . . . . . .TUCKEX (J . XI.).Products on Alkaline Copper Oxide Solution . . . . .BBNARD and J . GIRARDIN . Estimation of Gluten in Flour . . .Action of Organic Matter, not Sugar, in Cane and Beet. .RIMMINGTON ( F . M.). Method for Examination of Coff‘ee . . .RBMONT (A.). Separation of Wool and Silk in Textile Fabrics . .Technical Chenzistry .VOIT . .BIRNBAUM (K.). Analpes of Gluten Bread . . . . .BRAGA (J . I?.). Hair-djes . . . . . . . . .THOMPSON (W.). Composition of Ink . . . . . . .QUAJAT (E.), Combustibility of Tobacco . . . . . .GERMAIN (R.). A Photo-electric Regulator for Painted-glass FurnacesCECH (C . 0.). Disinfecting Power of the Chlorophenols . . .STRUVE (€3.) and 0 . JACOBSBN ..BRUNCK (H ) and C . GRAEBE . Action of Soda on Cast-iron . . .DELBRUCK (M.) and G . HEINZELMANN . New Method of FermentationMACS (E.) and PORTELE . Nashingof Grapes . . . . .BOUSSINGAULT . .PELLET (H.). .DURIN . Inversion of Sugar during Manuhcture . . . . .JUNEXANN and C . SCHEIBLER . .WURM (E.). Manufacture of Vinegar by Means of Bacteria . .The Changes Undergone by Meat in the Process of PicklingWickerheim’s Preservative FluidSaccharine Matters in the Friiit of the Coffee PlantAction of Animal Charcoal in the Sugar ManufactureSeparation of Sugar from MolassesSTIMNEL (C.). Apparatus for Skimming Milk . . . . .CECH (C . 0.). Colouring Matter of Xlcbus chamcemorus . . .ROTHER (R.), Coccus Red . . . . . . . . .BELOIIOUBECK . Analysis of Bohemian Tea .. . . . .VALAENBURQ (S . D . von) . .RENOUAKD (A) . Steeping of Hemp . . . . . . .v . NORDLINGER . Hardness and Resistance of Wood . . . .WEITZ (M.). A Eakmg Powder . . . . . . . .SARAUER (P.). Preservation of Fruit in Winter . . . . .RUDIGER (A.). Analvsis of Ice . . . . . . . .Preparation of Iodine-iron Cod-liver OilPELLIEUX ‘( J.) and E . Y A ~ ~ ~ ~ ~ . Manufacture of Iodine . . .OTTO (R.) and G . GABLER . Comparative Examination of Samples of Mag-nesium Carbonate . . . . . . . . . . .Freiberg Lead Furnaces . . . . . . . . . . .Enamelling metals . . . . . . . . . . . .CECH (C . 0.). Russian Fruit Wines . . . . . . . .Margarine, a Substitute for Butter and Lard . . . . .Saponification of Fats . . . . . . . .. . .Use of Methyl Alcohol in preparing Colouring Matters . . . . .BONG (G.).RICHE .Residue from the Manufacture of Para5n Oil from Schists .PAGE11731173117311741174117511751175117611’761176117611761177117711771177666767676812512612612612612612712712712812812012913013113113213213213220720720820820820820920921021CONTENTS. xlvPAGE211212212-2123173183183193193 203213223233233243 243253263283283293293303 303313313313323323324744744764754754764774774784784794794804814814 24824824834834834834 83662WIGNER ( 0 . W.). Analysis of Tinned Foods . .: . . ,MASING (E.). Examination of Various Kinds of Gum Arabic and of Traga-canth . . . . . . . . . . . . .EDER (J. M.). Aqueous Varnish for Prints on Unglazed PaperKOLBE (H.). Destructive Action of Wood on Salicylic Acid . . . .EDER (J. M.).Carbonic Oxide in the Air of RoomsTHIERCELTN.ALLARY (E.) a d J. PELLIEUX.. . .New DeT elopers for Silver Bromide D1.y Plates . . . . . . . . .Incineration of Seaweeds in the Manufacture of Iodine . .Extraction of Potassium Iodide fromK e l p . . . . . . . . . . . . .ALLARY (E.). Analysis of Marine Algae . . . . . . .COLSON (A.). Extraction of Phosphoric Acid . . . . . .Novelties in the Soda IndustryLUNGE (G.). Technical Notes . . . . . . . . .JEZLER. Composition of Weldon-mud and Similar Substances .. .MULLER (M.). Technology of Glass . . . . . . . .SEGER (H.). Composition of Clay for Porcelain . . . . . .FISCHER (F.). Zinc Distillation . . . . . . . . .FISCHER (F.) . Derhosyhorising Pig Iron . . . . . . .. . . . . . . . .Contributions to the Knowledge of Clay and Earthenware Goods . , .POCHIN (W.). Slag obtained during the Dephosphorising of Iron . .Boiler Incrustation . . . . . . . . . . .KNUBLAUCH. Illuminating Power of Benzene, Toluene, Ethylene, and EtherRUDNEW (W.). Products irom the Manufacture of Petroleum Gas . .OGLOBLINE. Commercial Petroleums . . . . . . . .Use of Maize in the Preparation of Starch, Sugar, Spirit, and Beer .GRIMMER (H.). The Decrease of Nitrogen in Malt Wort during Fermenta-tion . . . . . . .. . . . . ..SEUCEER (P.).CECII (C. 0.). Wines from Cloudberry and Cranherry . . . . .GAYON (U.). Spontaneous Changes in Raw Sugar . . . . .FISCIIER (E.). Dry Distillation of Wood . . . . . . .Rendering Furnace Gases inactive . . . . . . . .MASON (A. H.). Hydrogen Peroxide . . . . . . . .KRAUT (It ). Inflammation by Nitric Acid . . . . . . .Treatment of Must in the Press-house . . . . .NESSLER (J.). Composition and Unwholesome Effects of a Potato-sugar ,E'LEKKEL. Extraction of Potash from Suint of Russian Wool . . .LASNE and BENKER. Loss of Oxides of Nitrogen in the Manufacture of . . . . .GIRARD (C.) and J. A. PABST. . Sulphuric Acid, and a Means of Preventing itApplication of Lead Chamber CrystalsSTOKLASA (J.). Bohemian Chalk Fossils .. . . . . .Clay and Earthenware Goods . . . . . . . . .upoii it . . . . . . . . . . . . .MAYER (A.). Oxygen and Alcoholic Fermentation . . . . .SADLOW (K.). Tanning . . . . . . . . . .HOCKXANN (F.). Celluloid . . . . . . . . . .EDER (J. M.). Aqueous Shellac Varnish . . . . . . .New Dyestuff . . . . . . . . . . . .TCHECH. Hops of Southern Europe . . . . . . . .DE LA BASTIE.Hoaa (T. W.).WARTH 9 (V.)Resistance of Toughened Glass to Flexure . . . .Condition ofcarbon in Steel and the Effect of HardeningOn an Explosion Produced while Heating Wine, and a NewProcess for the Estimationof Alcohol . . . . . .GAYON (U.) . Recovery of Cane-Sugar from Molasses by Fermentation .HAEDICKE (H.). Spontaneous Tgnitjon of Coal . . . . . .LAFAURIE (J.). .Solid Preparation of Risulpliide of Carbon for Vines .MARECK (F.). Pigment for Floors, Wood, Stone, and Brickwork . .MOLLEB (J.) and J. POHL. .SARRAU and VIEILLE. Decomposition of Explosives in Closed Vessels .THOHPE (T. E.) . .Seeds of Cawin occidentalbs from MartiniqnePreparation of Pyrogallol for Dry-plate Developmcnxlvi CONTENTS .WALLACE (W.). Chemistry of Sewage Precipitation . . . . .SUILLIOT (H.). Nitric Oxide a Disinfectant . . . . . .HARGREA~ES (J.). Manufacture of Soctinm Sulpliate by the Direct ProcessALLDRED (C . H.). Treatment of Mineral and other Substances containingSmall Quantities of Calcium Phosphate . . . . . .KYNASTON ( J . W.). Production of Aluminium Sulphate free from Ironfrom Aluminous Minerals containing €ron . . . . . .NAWOKICHI MATSUI . Examination of the Raw Materials used for AritaPorcelain . . . . . . . . . . . .KERN (S.). Note on Siemens-Martin Stecl . . . . . . .PARNELL (E . A.). Metallurgic Treatment of Complex Ores containing ZincEDER (J . M.). Photochemistry of Siller Bromide . . . . .Novelties in the Soda Industry . . . . . . . . .JURISCH (K . W.). Oxidation of Soda Liquors . . . . . .SCHEURER.KESTNER . New Methods for the Desulphurisation of AlkalineSolutions . . . . . . . . . . . .L'HOTE (L.). Phosphorite from the South of France . . . . .FORQU~~NON (L.). Malleable Cast-iron . . . . . . .DELESSE (M.). Removal of Earthy Matters from Poor Lead-ores by ineansof an Air-blast . . . . . . . . . . .Novelties in Metallurgv . . . . . . . . . .DOREMIJS (C . A.). Wilkinson's Process of making Illuminating Gas fromWood . . . . . . . . . . . . .NICKELS (B.). Removal of Carbon Bisulphide from Commercial Benzene .ALLIHN (I?.). Grape-sugar from Starch . . . . . . .XEDZIE (R . C.). Hurtful Action of Potato-sugar . . . . . .SCHRODT (M.). Creaming of Milk in Earthen Pans . . . . .trifugal Separator . . . . . . . . . . .NAYER (A.). American Preserved Meats . . . . . . .WATSON (W . H.). Action of Oils on Metals . . . . . .MULLER (A) . Purification of Foul Water . . . . . . .Chemical Technology of Alkalis . . . . . . . . .GRUNEBERG (H.). Preparation of Potassium Sulphate from the Salts of theStassfurt Deposits . . . . . . . . . . .VINCENT . Thiocsrbonates of Potassium and other Metals . . . .DONATH (E.). Occurrence of Arsenic and Vanadium in Commercial CausticSoda . . . . . . . . . . . . .ROBERTS (W . C.). Steel for the Manufacture of DiesSTaVELEY (w . m-.). A Pure Coke . . . . . . . .CECH (C . 0.). Preparation of Braga Beer . . . . . . .Preparation of Soap . . . . . . . . . . .Dialysis . . . . . . . . . . . . .EITNER (W.). Preparation of Leather . . . . . . . .RCHLUMBERQER . Applications of Salicylic Acid . . . . . .ABEL (F . A.). Colliery Explosions . . . . . . . .GALLOWAY (W.) . Influence of Coal-dust in Colliery Explosions . . .ALBERT (E.) and H . Preparation of Phosphates . . . . . .KERN (S.). Manganese in Steel . . . . . . . . .zene by Alcoholic Potash . . . . . . . . .DELBRUCK (M.). Souring of Yeast . . . . . . . .Action of Cold on Ropy WineNEALE (A.) and others . New Fermentation of Beet-root Molasses . .VOELCKER (A.). Composition of Cream and Skim-milk from De Laval's Cen-HAXS (R.).BIEFEL (R.) and T . POLECK .Inflamniability of Vegetable Substances with Nitric Acid .Poisoning by Choke-damp and Coal-gas .... . . . .JACKEL.HANDWERK . Prevention of the Occurrence of Lactic Acid inBeer . . . . . . . . . . . . .SCHRODT (M.) and v . PLOTHO . .KOHLRAUSCH (0.). New Process for Extracting Tannin by Means ofCreaming of Milk by Surface Cooling .NICKELS (B.). Eliinination of Carbon Bisulphide from Commercial Ben-. . . . . . . . .PAGE662664664665666667667668762764765766766766767765769770770'7707'io771771771.77177285385485485585585685655785785755785885E8508609489509509509509519:CBX’TENTS . xlviiInfluence of Temperature on the Composition and Amount of Extract obtainedfrom Malt . . . . . . . . . . . .HOLZBECKER (H.). ’Influence of Oxygen on the Clarif~ing of Beer . .SALOMON and M . HERTER . Method of Preserving Brewers’ Grains . .Sugar Manufacture . . . . . . . . . . .ECESTEIN (A.). Use of Parchment Paper in Osmose . . . . .BERGMANN (A.). Ziemann’s Process for the Manufacture of Butter andCheese . . . . . . . . . . . . .Milk. Butter, and Cheese . . . . . . . . . .Peculiar Property of Gutta-percha . . . . . . . .CAMERON (C . A.). Sewage in Oysters . . . . . . . .GRUBER (M.). Poisoning by Carbonic Oxide . . . . . .ENGEL (R.). Manufacture of Potassium Carbonate . . . . .BODENBENDER (H.) and others . Analpses of Beet Molasses . . .DOREMUS (C . A.). Wilkiason’e Process for the Manufacture of Gas fromwood . . . . . . . . . . . . .Relation betxeen Oxygen and Organic Matterin Various Waters . . . . . . . . . . .SCHLOESING (T.) . Magnesia Industry . . . . . . . .Contributions to our Knowledge of Cement . . . . . . .CASAMAJOR (P.) and others . .WLTTELSH~~FER (P.) . Disadvantages of Cooling-pans in Distilleries . .NESSLER . Fermentation of Italian Wines . . . . . . .MACH (JF.) and K . POBTELE . Influence of Acids on the Preservation ofWine . . . . . . . . . . . . .MORITZ (J.). Analyses of Wine and Must . . . . . . .LINTNER . Influence of Malt on the Quality and Keeping Properties of BeerALBERT (J.) . Coloured Photographs . . . . . . . .JANSSEN (J.). .REUSS . Injurious Effect of Furnace-gases in the Forests of the UpperHarz . . . . . . . . . . . . .LANGFELDT . Destruction of Microscopio Animals in Potable Water . .Production of Magnesia . . . . . . . . . .SCHLCESING (T.) . Magnesia Industry . . . . . . . .On Cement . . . . . . . . . . . . .Composition of some Cements . . . . . . . . .WEBER (R.). Explosion of Petroleiim nncl other Combustible Liquids .ASHBY (A.), Formula for Calculating tlie Quantity of Water added toDiluted Spirit . . . . . . . . . . .ULBRICHT (R.), Analyses of Wine and Must . . . . . .GEISSLER (E.). Esamination of Preped Yeast . . . . . .PETER (H.). Milk Analysis . . . . . . . . .ARNOLD (L . B.) Effect of Oxygen on the Quality of Butter . . . .MUSSO (G.) and others . Ripening of Cheese . . . . . .PORTELE (K.). Use of Salicylic Acid in the Dairy . . . . .BALLAUD . A Cause of Alteration of Textile Fabrics . . . . .Use of Cadmium in Calico-printing . . . . . . . .GLENCK (C.). Preparation of Aniliiie Black . . . . . .SADLON (K.). New Observations in Tanning . . . . . .WEYL (T.) and X . ZEITLER .Adulteration of Cane-sugar with GlucoseMARPXANN . Interference of Bacteria with Brewing . . . . .Changes of Photographs by the prolonged Action of LightSLOETEN (W . v.). Air of Hospitals dnring Yellow Fever . . . .MAYER (-4.). The Action of Rennet under mrious Conditions . . .PAaE95195195195195295295395395395410561087108710871088108910891089109010901090109010901175117911791179117911801180l l h O1181118111831182118311831184.118-41 1 8 h1185118511851186118

ISSN:0368-1769    

DOI:10.1039/CA88140FP001

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

18 ABSTRACTS OF CHEMICAL PAPERS.I n o rg a n i c C he m i s t r y.Preparation of Hydrogen Selenide and Hydrobromic Acid.By A. ETARD and H. MOISSAN (BUZZ. SOC. Chim. [2], 34, 69).-Theauthors prepare hydrogen selenide by a method analogous to thatemployed by Champion and Pellet for h-j-drobromic acid and hydrogensulphide, that is, by the action of bromine and sulphur respectivelyon paraffin. The hydrocarbon used in preparing hydrogen sulphidewas colophene, as its boiling point (300" C.) is considerably above thefusing point of selenium (250" C.). The reaction takes place in twostages : a t first a substituted product is formed, and this is subse-quently decomposed; at the end of the experiment nothing but amixture of unaltered colophene and carbon is left.Hydriodic acidmay be prepared by a similar proeess. V. H. V.Liquefaction of Ozone, and its Colour in the Gaseous State.By P. HAUTEFEUILLE and J. CHAPPUIS (Compt. Tend., 91, 522-525).-The authors obtained a mixture very rich in ozone by the action ofelectricity on oxygen at a very low temperature. This mixture wastransferred to the capillary tube of Cailletet's apparatus, and subINORGANIC CHEMISTRY. 19mitted to pressure, at a temperature of - 2.3". At the first fewstrokes of the piston an azure-blue colour was seen to fill the tubeand as the pressure increased the colour deepened, until when the gaswas under a pressure of several atmospheres, the colour had becomeindigo-blue. When the pressure was suddenly removed, a momentarywhite mist was observed within the tube, indicating a condensationinto the liquid, or perhaps solid state.The blue colour, being like itsodour, an essential property of ozone, may be seen whenever a suffi-cient thickness of a mixture containing it is viewed. Thus the oxygenissuing from Berthelot's silent-discharge apparatus exhibits a sky-bluecolour when viewed along a column 1 metre in length. I n a forth-coming communication, the author will discuss the agency of ozone asaffecting the colour of the atmosphere. R. R.Constancy of the Proportion of Carbonic Anhydride in theAtmosphere. By T. SCHLUESING (Cow@ rend., 90, 1410-1413) .-The author is of opinion that the sea plays an imporbnt part in regu-lating the quantity of carbonic anhydride present in.the atmosphere.He has shown (ibid., June and July, 1872) that water in contact withthe carbonate of an alkaline earth, and an atmosphere containing car-bonic anhydride, absorbs the latter, forming a quantity of bicarbonate,which increases with the tension of the carbonic anhydride in theatmosphere, according t o a given law. Moreover, if the water con-tains a neutral salt, the amount of bicarbonate formed is increased.Comparing this with the state of the sea and the atmosphere, it is seenthat the sea is in constant contact with air which contains carbonicanhydride, and with the earthy carbonates at its bottom. Fromanalyses of sea water, the author finds that I litre contains 98.3 mgrms.of carbonic anhydride, and a base combined with it equivalent to99.3 mgrms.sulphnric acid, so that the greater part exists in the formof bicarbonate. Now when the amount of carbonic anhydride in theatmosphere, which is proportionately very much less than that containedin sea water, increases beyond its norma1 amount, the surplus isabsorbed by the sea and a fresh portion of the earthy carbonates goesinto solution. On the other hand, when the quantity decreases, car-bonic anhydride escapes into the atmosphere. This action, togetherwith the continual motion of the atmosphere, tends greatly to equalisethe quantity of the gas present in the atmosphere. L. T. 0's.Proportion of Carbonic Anhydride in the Atmosphere. ByJ. REISET (Compt. rend., 90, 1457--1459).-This is a reply to Marie-Davy, in which the author maintains that the method of experimentused by the observer at Montsouris to determine the constancy ofthe proportion of carbonic anhydride in the air was not sufficientlyexact to eliminate all sources of erim : also that the experiments ofTruchot on the influence of altitude on the amount of carbonic anhy-dride require repetition, since no correction is made for the alterationin the standard sohtions due to evaporation a t such high altitudes,The author quotes his former remarks (this Journal, Abstr., 1880,605) * L.T. 07s.c 20 ABSTRACTS OF CHEMICAL PAPERS.Proofs of the Existence of Ozone in the Atmosphere. By E.SCHONE (Ber., 13, 1503-l508).-Hydrogen peroxide has been shownby the author (this Journal, 34, 552 and 703) to be a constituentof the atmosphere. This being the case, the evidence adduced bySchonbein and Honzeau to prove the existence of ozone in the atmo-sphere is of little value, for the results they obtained may have beenproduced by hydrogen peroxide.Little weight is to be attached tothe evidence brought forward hy Andrems (PhiZ. Mag. [4], 34, 312 ;and Nature, 8,347 and 364) ; or Fox (“ Ozone and Antozone,” London,1873, 48 and 216), in support of the existence of ozone in the atmo-sphere, these authors having ignored the presence of hydrogen per-oxide completely. The method of testing for ozone by exposing silverfoil is one to which many objections may be raised. The odourobserved after a flash of lightning and attributed by many to ozone,the author fails to recognise as resembling that of ozone.The author concludes that the evidence in favour of the existence ofozone in the atmosphere is by no means conclusive, yet in atmosphericelectricity we have power sufficient for its production.The existenceof hydrogen peroxide in the atmosphere does not exclude that ofozone, since these bodies decompose one another b u t slowly.P. P. B.Observations on the Atmosphere made with ThalliumPapers. By E. SCH~NE (Ber., 13, 1508--1514).-The observationsof the author and others show that the ozonometer of Schonbein(AnnuZen, 89, SZS), is too much influenced by the hygroscopic stateof the atmosphere to be of service in determining the combinedeffect of ozone and hydrogen peroxide present in the atmosphere.This ozonometer the author stigmatises as a crude hygrometer.Asthe oxidation of thallous hydrate by ozone or hydrogen peroxide isuninfluenced by the presence of moisture, the author has made aseries of daily and nightly observations by exposing to the atmo-sphere papers saturated with a 2 per cent. solution of thallous hydrate.A sca!e of numbers was made corresponding with the densities of thebrown colour produced by exposure. Observations were made simul-taneously with the ozonometer, the deductions from which were usuallythe opposite of those obtained from the thallous hydrate. The obser-vations with thallous hydrate show that the oxidation is greaterduring the day than during the night ; it is influenced by the directionof the wind.a southerly wind is attended with a stronger coloration ;clouds and rain have a marked influence, viz., the reduction of thecoloration of the thallium paper. Further allowance must be madefor the strength of the wind. The observations made with thalliumpapers agree with the results obtained by the author in the moreexact determination of the atmospheric hydrogen peroxide. Fromthis fact, the author thinks that atmospheric hydrogen peroxide issufficient to produce the observed oxidation, and that the presence ofatmospheric ozone is uncertain.ByA. ETARD (Comnyt. rend., 91, 627-629).-The author proposes toplace boron a t the head of the vanadium family of elements, formingP. P. B. .Position of Boron in the Series of Elementary BodiesINORGANIC CHEMISTRY.21a group intermediate between that of phosphorus and that of carbon.This juxtaposition of boron to the phosphorus group is supported bythe existence of the compounds BCl, and BOC13, recently discoveredby Councler, and by the existence of boric triethide or triethylborine,which is analogous to triethylphosphine in composition and properties.The relations of vanadium to the phosphorus group have been estab-lished by Roscoe, and the labours of Deville and Troost have doneas much for niobium and tantalum. Boron and vanadium areboth grey, pulverulent, carbon-like substances, combustible, and infusi-ble; both combine with chlorine, forming BCl, and VCl,, and theiroxychlorides, BOCI, and VOCl,, are yellow fuming liquids. Boronand vanadium, like the other members of the group, B, V, Nb, Ta,have also the somewhat rare property of directly absorbing nitrogen.The author will, in a subsequent communication, describe the proper-ties of an oxide of boron, U205, corresponding with V205 and Pz05.Action of Sulphur on Water. By A.COLSON (Bull. SOC. Ckim.[2], 34, 66-69).-The author was induced to study the action of sul-phur in the nascent state on boiling water, from difficulties whicharise in the determination of iron by the Marguerite process. Onadding a very dilute solution of sodium thiosulphnte to dilute hydro-chloric acid (1 : lo), the salt is completely decomposed, with forma-tion of hydrogen sulphide and sulphuric acid, the reaction beingS2OZ + H20 = SO, + HzS. In more concentrated solutions the de-composition is not so complete, part of the sulphur being deposited onthe sides of the flask.An experiment with sulphur dissolved in sodiumprotosulphide showed tha,t an amount of lead sulphide was obtainedgreater than that required by theory for the protosulphide employed.A comparison is drawn between the action of water on flowers of sul-phur and on sulphur liberated from the thiosulphate. The latter isenergetic, and takes place at once a t ordinary temperatures; theformer requires time, and the temperature of boiling water. The sul-phur deposited on the flask from the decomposition of the strongthiosulphate solution, was in the form of lemon-yellow grains, whlchhad no action on polarised light. The same form was obtained fromsulphur deposited from a benzene solution, and kept for some time incontact with boiling water.It would appear that sulphur loses itsPresence of Cerium in the Coal Measures of St. Etienne.By MAYENCON (Conzpt. reid., 91, 669).-The paper notes the author'sdiscovery of cerium in some mineralogical products of the miningdistrict of St. Etienne. The cerium is found particularly in certainhard nodules of carbonate of iron, where it appears to exist in thestate of carbonate. R. R.R. R.crystalline form before entering into combination. V. H. v.Sesquioxide of Chromium. By H. MOISSAN (BUZZ. SOC. Chin%.[2), 34, 70-73).-The author compares the action of various re-agents on ignited chromium sesquioxide and the oxide rendered anhy-drous by heating it a t 440" C.in a current of nitrogen or carbonicanhydride. Hydrogen sulphide and selenide, chlorine, bromine, an22 ABSTRACTS OF CHEMICAL PAPERS.oxygen have no action on the former modification. The actions ofsome of these substances on the &her modification are studied.Action, of Hydrogen Sz1bpl&ie.--By exposing the anhydrous oxide toa current .of hydrogen sulphide, whether dry or moist, at 140" C., it isconverted into the corresponding black sulphide, clr,S,. The substanceis not attacked by any acid except nitric acid and aqua regia. Byreducing it in hydrogen, a black protosulphide, CrS, is formed.Actiou of Oxygen.--The sesquioxide when heated in this gas is con-verted into the dark grey dioxide, CrOz, which resembles the corre-sponding manganese dioxide, MnOz, in its reactions.ktCtiO.12 of ChZoriwe.-By exposing the hydrated sesquioxide to acurrent of dry chlorine and gradually raising the temperature, redvapours of chlorochromic acid begin to be evolved at 440" C., butwith the anhydrous sesquioxide, dry chlorine forms the sesquichloride,the reaction being very incomplete : moist chlorine gives chlorochromicacid with the anhydrous sesquioxide or sesqnichloride.It mouldappear from these experiments that the presence of small quantities ofwater determine the formation of chlorochromic acid, the necessaryoxygen being furnished by the water. By stopping the reaction at acertain stage, the sesquioxide is converted into the brown oxychlorideof Moberg, an intermediat<e body less oxidisecl than chlorochromicacid, and decomposable by water.The sesquioxide of chromium isa type of those oxides in which a change of properties is accompaniedby an evolution of heat. V. H. V.Preparation of Chlorine. By BERTHELOT (Compt. rend., 91,252-256) .--The author's experiments were undertaken to elucidatethe first stage of the reaction which occurs in the preparation ofchlorine by the action of hydrochloric acid on manganese dioxide.When these subst'ances are mixed in the cold, a brown liquid isformed, which was supposed by Forchammer to contain a, sesquichlo-ride of manganese, by NicklAs and by Fisher (this Journal, 3, 409)t o contain manganese tetrachloride.Actim of Chlorine on Ma.lzgn~ious C1doride.- A concentrated solutionof manganous chloride, saturated with chlorine, and placed in contactwith an atmosphere of this gas, dissolves only about half the quantitydissolved under the same circumstances by pure water, and about thesame amount of heat is evolved in proportion to the chlorine dissolvedin the two cases.The liquid slowly deposits a precipitate of manganesedioxide, absorbing a t the same time an additional quantity of chlo-rine, but even after two months the ratio of chlorine absorbed tomanganous chloride taken did not exceed 1 : 55. By diluting theoriginal solution of manganous chloride saturated with chlorine withnine times its volume of water, an abundant precipitate OC manganesedioxide is formed a t once, which increases during a certain time.Atthe end of two months, the liquid still contained manganous chlorideand free chlorine, coexisting with the hydrochloric acid and manganesedioxide formed : there is in fact an equilibrium established.Action of Hydrochloric Acid OY& Manganese Dioxide.-Manganesedioxide mixed with a nearly equivalent quantity of a dilute (10 C.C. =0.16 gram) solution of hydrochloric acid, evolves chlorine, and IN ORGANIC CHEiIIISTRY. 23brown liquid is formed, but the reaction is very incomplete. If thesame mixture be heated in a sealed tube at 100" for 20 hours, the re-action proceeds further, but remains incomplete. After cooling, man-ganese dioxide slowly separates out on the wall of the tube, provingthat the equilibrium is dependent on the temperature.Action of Chlorine on Manganous Chloride and Hydrochlo& Acid-On passing a current of chlorine into a concentrated solution ofnianganous chloride mixed with its own volume of strong hydro-chloric acid, the liquid turns brown almost immediately, but depositsno precipitate even after three months.If the preceding solutionbe diluted ten times before saturating with chlorine, it absorbs aboutthe same quantity of that gas without any coloration or precipitatebeing at first, produced, but after some weeks a small quantity ofmanganese dioxide separates out on the walls of the flask. The heatevolved during the absorption of chlorine by manganous chloride inpresence of hydrochloric acid is several times as great as that evolvedin the absence of hydrochloric acid.The author concludes from these experiments that the brown colouris due to the formation of a compound perchloride, which may beconsidered as HCl.Cl, + nMnCl,, or as nHCl + MnC14.On the firstview, this perchloride is derived from the perchloride of hydrogen,HC1.Cl2, described by the author in a previous paper. This compounddissociates under the influence of heat, and the dissociation is renderedcomplete when the chlorine is removed as fast as it is liberated. Whenthe experiment is conducted in sealed tubes, reabsorption of the chlorinetakes place on cooling, attended with separation of manganese dioxide.The influence of dilut,ion is twofold ; in the first place the manganouschloride is partly decomposed by the water int,o oxide and free acid,and the oxide is peroxidised by the combined action of the five chlorineand water ; in the second place, absorption of energy takes place byt,he formation of definite hydrates of hydrochloric acid, and in con-sequence of this loss of energy, the mauganous chloride may bepartly transformed into dioxide even iu presence of hydrochloric acid,the equation MnC1, (dilute) + 2H,O + C1, (gas) = MnO, + 4HC1(dilute) corresponding with a disengagement of 3.7 thermal units.This reaction is never complete, on account of the secondary forma-tion of HC1, + nMnC1,.The equation MnO, + 4HCl = MnCl, (anhydrous) + 2C1 (gas) + 2H20 (gas), corresponds with a disengagement of 12.9 thermalucits, and this takes place to a greater or less extent in concentratedsolutions, in which a portion of the hydrochloric acid is not combinedwith the water as a stable hydrate, the heat of formation of which isfi*om 10 to 12 thermal units.J. M. H. M.Borodecitungstic Acid and its Sodium Salts. By D. KLEIN(Compt. rend., 91, 474-475 j.-When a solution containing boraxand boric acid in the proportion of 1 mol. of the former to 2 mols.of the latter is heated with an excess of tungstic acid (hydrated), aportion of the latter is dissolved. On cooling the filtered solutiondeposits crystals of boric acid and polyborates of sodium, and by con-tinuing the evaporation of the mother-liquor in vaczco crystals of bora24 ABSTRACTS OF CHEMICAL PAPERS.are first obtained, and then a salt excessively soluble in water, and verydifficult to purify by recrystallisation. This salt has the composition2Na20.2Hz0.10WO3.B2O3 + 11Aq.The crystals belong to the clino-rhombic system, but are ill-defined, with dull faces. The reaction isfaintly acid to litmus. On adding a trace of alkali, the acid reactionis changed to alkaline, but reappears after a time. By adding asmuch sods as is already present, and evaporating, a second crystallinesalt is obtained, which has not yet been analysed.Sodium borodecitungstate is precipitated by salts of mercury, andfr.om this precipitate the acid may be obtained. This acid and boro-duodecitungstic acid correspond with the silicodecitungstic and silico-duodecitungstic acids described by Marignac, and their salts have verysimilar properties.Boroduodecitungstie Acid. By D. KLEEIN (Cowpi. rend., 91,495--498).-When tungstic hydrate in large excess is added to a boil-ing solution of potassium pentametaborate, potassium boroduodecitnng-state is formed. The author ascribes to this compound the formula2K20.B20,.12W03.2H~0 + 15Aq. It is a very soluble salt, crystal-lising in needles resembling those of potassic tungstoborate. Themother-liquor yields white tabular crystals of another salt!, of theformula 4K2O.B,O3.12 WO, + 21Aq. By treating the insoluble mer-curous salt with the requisite quantity of hydrochloric acid, andevaporating the solution after removal of the mercurous chloride,boroduodecitungstic acid is obtained as a syrupy liquid.J. M. H. M.R. R

ISSN:0368-1769    

DOI:10.1039/CA8814000018

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

24 ABSTRACTS OF CHEMICAL PAPERS.M i n e r a 1 o g i c a1 C h e mi s t r y.The Zundererz or Tinder-ore of Clausthal. By B. ROSING(Juhrb. f. Min., 1879, 137).-An analysis of this mineral gave thefollowing results :-Pb. Cu. Ag. F1. Sb. 5.33.41 0.58 0.05 1.66 36.81 27.49 = 100.00From this analysis, the formula, appears to be Pb4Sb6SI7, and themineral an impure bournonite (bleispiessglanz), in which a part ofthe lead has been replaced by copper, silver, and iron. The authoris of opinion that ziindererz is the final product of the decompositionof an antimonial galena. C. A. B.Freislebenite from Hiendelaencina, Spain. By H. B~~CKING(Juhrb. f. Min., 1879, 161).-Some of. the crystals of this mineralattain a, size of 6 mm. Two new twin-laws were observed occurringon the crjstals from this locality, twins according to the well-knownlaw, ‘K the twin-plane &Pa’’ not having been observed.In conse-quence of repeated combination, the crystals exhibited the characteristiMINERALOGICAL CHEMISTRY. 25striation parallel to the zonal axes of the prisms and clinodromes. Thetwo new twin-laws are as follows, viz. :-(la) The twin-plane, a hemi-pyramid, probably - 3P4 ; the prisms observed were mP2 and mP,whilst the domes were +Fm and iym. (2.) The twin-plane, a faceof a prism, probably ms:. The same forms as those observed inNo. 1 occur also in combination in this case. In a,ddition, the follow-ing forms were observed, occupying a very secondary position, viz.,mq5, 0352, mF$, fym, and ism. Thirty forms have now been ob-served on freislebenite.C. A. B.Quartz from the Eleanore Mine, on the Dunstberge, nearGiessen. By A. STRENG (Jahrb. f. Min., 1879, 156).-The quartz inquestion occurs in isolated broken crystals or in druses, enclosed inbrown iron ore, the forms observed by him being R. -R. mP, and aprism having probably the symbol mPS1. The terminal edges of R.were modified by a semi-scalenohedron, but its faces were so smallthat no measurements could be made. The quartz from the EleanoreMine resembles closely that from Striegau, described by Websky(Jaltrb. f. Min., 1871, 732). C. A. B.Fluid Enclosures in Topaz. By T. ERHARD and A. STELZNER(Jahrb. f. Min., 1879, 158--159).--According to Vogelsang, the veryexpansive fluid which occurs in quartz, topaz, and other minerals isliquid carbonic acid, its "critical point" being 30" to 32" C.Theauthors conducted a very careful series of experiments, using a micro-scope which was kept at the same temperature as the object by meansof a water-bath. Two topaz crystals were examined, containing inall seven fluid enclosures. Each fluid enclosure contained two otherenclosures. The results of the investigation were briefly as follows,viz. :-1. For one and the same enclosure the globule disappeared andreappeared with intumescence at the same temperature. 2. The" critical points " of the fluid enclosures in different specimens are notquite identical. 3. As the " critical points '' were found to lie between28.745" and 29.18" C. the authors concluded that the fluid enclosurescould not be pure carbonic acid, as the "critical point" of thatsubstance is about 30.92" C.C. A. B.Andalusite from Brazil. By E. BERTRAND (Jahrb. f. Min., 1879,161-162) .-The author examined some rounded crystals from Brazilwhich were partly light coloured and partly opaque, and stronglydichroitic. They scratched quartz. Sp. gr. = 3.16 to 3.20.C. A. B.Artificial Analcime. By A. DE SCHULTEN (Compt. rend., 90,1453--1495).-0n heating a solution of sodium silicate or causticsoda a t 180-190" with an alumina glass for about 18 hours, smallcrystals covered with a lamellar layer of gelatinous silica are foundadhering to the sides of the tube. These, when examined micro-scopically, appear transparent, of the form of a trapezohedron of thefirst system.Hydrochloric acid acts but slowly on them. The analysisshows that the crystals are a silicate of sodium, aluminium, and cal26 ABSTRACTS OF CHEMICAL PAPERS.cium, of the same composition as natural analcime. Their action onpolarised light has been studied. L. T. 0’s.By L. ROTH (Jahrb. f.A f h . , 1879, 157) .-Crystals of this mineral occur in drusy cavities,accompanied by crystals of chabasite and phillipsite, in the basalt oftlhe Vogelsgebirge, between Gedern and Oberseemen. They are iden-tical with those found a t Schiffenberg and Rurkhards. The crystalsare rhombic pyramids, 2 to 8 mm. in size, partly simple, partly pene-tration twins, similar to those from Schiffenberg, described by Streng(Jcchrb.f. Min., 1874, 578). They are also often coated with a yellowcrust or with hyalite, but there is always a clear kernel.By A. CORSI (Julwb. f.Min., 1879, 161).-This mineral occurs-;-1. At Impruneta, in gabbro,of which it is a “ decomposition-product.” The crystals are sometimestabular, exhibiting the forms OP.mP*.mP&,mP in combinatipn (OPbeing strongly striated), arid sometimes colourless aggregates of crys-tals. The prehnitc is occasionally accompanied by analcime, whichdecomposes into prehnite. 2. At Figline in tabular crystals, notexhibiting many forms, and accompanied by albite and acicularzeolites. 3. At Moiztecatini, in the Cecina valley, in hollow spacesin gabbro ; prismatic crystals are found exhibiting the formsucrP.mPd;j.OP in combination, and accompanied by calcite and nativecopper.4. At Jlonte Perrone, on Elba, tabular crystals and crystal-line aggregates, in diorite, accompanied by epidote.By C. D~LTER (Jahrb. f. &fin., 1879,157-158) .-In the present paper the author continues his researchesinto the composition of these minerals, the previous results beingpublished in the Jahrb.f. E n . 1878, 657.Aegerine from Brevig.-Sp. gr. 3.501. Chemical composition asfollows, viz. :-51.74 26-17 3.48 0.47 0.46 5.07 1-79 0.34 11.02 = 100.54The small qnan-tity of potash found is the constitueut of orthoclase, which is presentin microscopical particles in the aegerine. Dolter considers the con-stitution of aegerine to be as follows, viz. :-A New Occurrence of Gismondine.C.A. B.Occurrence of Prehnite in Tuscany.C. A. B.Acmite and Aegerine.Si02. FezO3. FeO. A1,03. MnO. CaO. MgO. E20. N%O.This analysis agrees with those already published.Na2Fe,”‘Si4OI2 = 77.0 per cent.Ca,Mg,Si4012 = 9.9 ,,Ca,Fe,Si4012 = 11.6 ,,Ca2Mn2Si40u = 1.5 ,, --100.0Acn7de.-This mineral is crystallographically identical with aegerine.Chemical composition as follows, viz. :- Sp. gr. 3.520.SiO,. Fe203. FeO. Al,O,. MnO. CaO. MgO. K20. Na.0.51.35 32-11 2-59 1.59 0.37 - - 11.3MINERALOGICAL CHEMISTRY. 27Acmite is generally weathered, but the aut,hor selected fresh speci-He found a smaller intermixture of other silicatesThe constitution ofmens for analysis.in this mineral than was the case in aegerine.acmite, according to Dolter, is as follows, viz.:-Na2Fe9’”Si101z = 89.0 per cent.Fe2Fel”’Si201z = 6.0 ,,FezAl*’”SizOlz = 3.7 ,,CazMn2Si401a = 1.3 ,,100.0From the above it would appear that a silicate having the formulaNa2Fei”Si401z must be present in acmite and aegerine.C. A. R.Dolomite of South Tyrol. By H. LORETZ (Jahrb. f. 2&., 1879,175) .-On microscopical examination, the dolomite exhibited threekinds of structure, viz. :-1. Oolitic or oolithoidal structure. 2. Stra-tified str’ucture. 3. Breccia-like structure. The first is simply aspheroidal occurrence of the crystalline individuals which the authorbelieves to have been caused by movements taking place round aboutmicrolitic depositions of the dolomite substance, whilst’ the greaterpart of the surrounding mass was in a semi-fluid condition.Thesecond formation is caused by the occurrence of alternate layers orstrata of microcrystalline and macrocrystalline substance. The thirdformation is caused by the fragmentary occurrence of portions ofmicrocrystalline and macrocrystalline substance together.C. A. B.Examination of Melaphyr from the Neighbourhood ofKleinschmalkalden. By F. M. WOLF (Jahd. f. M~TL., 1879, 162-163) .-A very complete examination showed that all the specimenscontained as essential constituents (wesentliche Bestandtheile) plagio-clase, augite, and olivine embedded in a “ base ” of varying constitu-tion, from which it was evident that all the rocks examined were truemelaphyr. The author divides the melaphyrs of Kleiiischnialkaldeninto two groups, viz.:-1.The rocks from the Reisigenstein, theFinsterliete, and the Linsenkopf. 2. The rock from the Eberhaidekopf.Analyses made of the above rocks showed that those of the first groupcontain 43 per cent. of silica and compounds of iron, whilst that ofthe second group contains 5’2 per cent. The rocks of the first groupare characterised by a porphyritic occurrence of crystals of augite,olivine, and mica, which are surrounded by numerous small bands offelspar. These melaphyrs are augitz’c nzelaphyrs. The melaphyr fromthe Eberhaidekopf contains very little augite, no mica, and has a fine-grained structure. C. A. B.Petrographical Constitution of the Monzonite of Predrazzo.By V. HANSEL (Jahrb. f. J h ., 1879, 162).-Although monzonite be-longs to the trias formation, it exhibits externally the characteristicsof the old crystalline rocks, graoite and syenite. Its microscopicalenclosures make this resemblance a11 the more striking. On the otherhand, its connection with more recent rocks is shown by the occurrenc28 ABSTRACTS OF CHEMICAL PAPERS.of “glass enclosures ” in the felspars. The varieties of monzonitecan be arranged into two groups, in both of which plagioclase occurstogether with orthoclase. The first group includes basic rocks, which(mineralogically speaking) correspond with diabsse and gabbro, andcontain from 40 to 50 per cent. of silica. The second group includes acidrocks, corresponding with syenite or diorite, and containing from 50 to59 per cent.of silica. The last-mentioned group includes rocks consist-ing principally of hornblende, augite, and biotite, whilst those of thefirst group ‘consist principally of augite or diallagite. Thc monzoniteof Predrazzo is (mineralogically and geologically) almost identical withthe monzonite of Monzoni, the only difference between them being thelarge occurrence of biotite in the rock of Predrazzo. C. A. B.The Ferruginous Rocks of Ovifak and Assuk, in Green-land. By A. E. TORNEBOHM (Jah~b. f. Min., 1879, 173--175).-Therocks which furnished the famous iron masses of Ovifak appear t o beportions of a formation consisting principaily of basalt, in which areenclosed fragments or portions of a dolerite and an anorthite rockcontaining graphite. The aut.hor found the native iron to OCCUL’principally in the dolerite or other enclosures in the basalt; he didnot find ib in the basalt alone.The dolerite consisted of plngioclase,augite, olivine, titanic iron, and a glassy ‘‘ interpolation mass,” andnative iron occurs filling up the irregular interstices which existbetween the above-mentioned mineral constituents of the dolerite.The native iron occurs as ductile grains, having an almost silver-whitecolour, also as dull grey almost lustreless particles, and black opaquemasses (consisting probably of finely-divided iron, magnetite, andcarbon), accompanied always by magnetic iron pyrites and a ferru-ginous silicate. The shining metallic particles do not consist ofnative iron alone, but in all probability contain schreibersite.Themagnetic iron pyrites has a yellowish-grey colour, and containsparticles of a sulphide which is easily decomposed (probably calciumsulphide or troilite). The ferruginous silicate varies in appearance,according to its more or less decomposed condition. It is rarely foundfresh, and when it is in that condition it is isotropic, grass-green incolour, and is sharply defined from the “ glassy mass ” above men-tioned. I n the fresh condition, the silicate resembles chlorophaite,whilst in the decomposed state it resembles hisingerite. This silicateoccurs also in amygdaloidal nodules, analogous to the chlorophaitenodules found in basalt and melaphyr, so tha’t the mass filling up theirregular interstices between the various mineral constituents of therock of Ovifak differs only from the corresponding mass of the basalts ofother localities in containing native iron and magnetic iron pyrites.Theround cavities in the dolerite of Ovifak are often filled with native iron(exhibiting sometimes Widmannstatten’s figures) and magnetic ironpyrites, and it is quite evident that these globules of iron are notmechanical enclosures. The anorthite rock consists of a coarse-grainedmass of asymmetrical felspars (anorthite and labradorite), graphite,and spinelle. It occurs sometimes in fragments interspersed in thebasalt, and sometimes it is very intimately intermixed with the dole-rite. Iron is found in this rock also, filling up the breccia-like interMIKERALOGICAL CHEMISTRY.29stices. The rock of Assuk, in the Waigattet, consists of enstatite,a s p metrical felspar, and a glassy base. Between these constituentsare interspersed numerous small grains of native iron, lumps of anopaque substance (most probably graphite), and some magnetic ironpyrites, whilst here and there a greenish mass was observed (ansful-lungsmasse), also larger nodules filled up zonally with viridite, quartz,or garnet. The Assuk rock, therefore, does not resemble that ofOvifak, and it cannot be a basalt, as it contains 56 per cent. of silica ;it is probably a secondary molten mass.A New Meteoric Mineral. By J. LAWRENCE SMITH (Cow@. rend.,90, 1460--1462).-The author has made a further examination of themineral obtained from the meteoric shower at Iowa, 1879. Themineral forms projections on the surface of the stones.It has an easycleavage, and on breaking presents an opalescent fatty appearanceand a greenish-yellow colour. Its microscopic structure differs fromthat of olivine.C. A. B.Sp. gr. = 3.25.The results of the analyses are as follows :-I. 11. Oxygen.SiOz ........ 49.60 49.59 25-73FeO ......... 15.78 17.01 3.77MgO ........ 33.01 32-51 12.66Prom these numbers the formula BSiO,.RO + Si02.2R0 may bededuced, which represents 2 mols. of enstatite or bronzite with 1 ofolivine. For this mineral, the author proposes the name peckhamite.An account is also given of the meteoric shower. L. T. 0's.Chemical Examination of the Grossliider Mineral Springat Salzschlirf.By E. REICHARDT (Arch. Pharm. [3], 16, 208-216).-This spring is distinguished for its richness in carbonic anhydride,which constantly escapes; it discharges itself a t a depth of about1 metre from the surface, and therefore requires to be pumped. Thesamples received were slightly turbid, but became much more so afterthe escape of carbonic anhydride.The analysis was made in the usual way, the following analyticaldetails alone being noteworthy.The specz& gravity was taken after the escape of carbonic anhydrideat the ordinary temperature (13.5" C.) had ceased.Boric and nitric acids were absent.Silicic acid was chiefly present in the deposit formed by standing ;when hydrochloric acid in excess was added, this deposit entirely dis-solved after a time, and silicic acid was then estimated by evaporationin the usual way.Barium was detected in the sodium carbonate precipitate, but nostrontium was found.The direct results of analysis showed that 1,000 parts of water con-tained-c1.Br. P,O,. SiOB. SO3. COZ. Na. K.9.653 0.1186 0.0008 0.3176 1.852 2.776 6.619 0.31430 ABSTRACTS OF CHEMICAL PAPERS.Li. CaO. MgO. SrO. Pe,03. MnO. Al,03.0*005 1.5869 0.5582 0*0009 0,0326 0.0044 0.0045.Alkaline carbonates were absent, for the aqueous solution of thedried solid residue was not alkaline ; but some of the potassium andsodium were present as organic salts, as was proved by igniting t,heresidue, and also by permanganate. The following proportions ofsolid substances were calculated to have been present :-Sodium chloride ..........Potassium chloride ........Lithium chloride ..........Magnesium chloride. .......Sodium bromide ..........Sodium (organic salts) ....Calcium sulphate ..........Magnesium sulphate ......Strontium sulphate ........Calcium phosphate ........Calcium carbonate ........Magnesium carbonate.. ....Ferrous carbonate..........Manganous carbonatme ......Dissolved silica. ...........Alumina. .................In one litre.grams.15.68350.61020.00330.05270.155'70.50201.64021,38730.00160.00171.67300.21 730.04810-00730,32330.004622.3118I n 1,000 grams.grams.15 *41220.59960.003'20.05180.15500.49331.61181.36330.001 60,001 71.64410.21350-04730.00720.31 760.004521.9257Free carbonic anhydride at11.5" C.and 760 mm. .... 1656.24 C.C. 1627.59 C.C. = 3.107grams.Specific gravity = 1.0176.Subtracting from the total carbonic anhydride evolved on boilingthat which had been expelled from the ferrous and manganous car-bonates, the weight evolved from 1,000 grams of water would be3.0864 grams.The total solid residue from 1,000 grams of water dried at 100" C.weighed 21.860 grams, the loss on the weight calculated above beingdue to partial decomposition of the ferrous and manganous carbonatesduring evaporation and drying.The analytical numbers obtained from four other Salzschlirf medi-cinal springs are tabulated with those yielded by the Grossluder spring,The latter is remarkable as st saline spring, containing iron and muchcarbonic acid ; it also contains much magnesium sulphate, whoseunpleasant taste is masked by t,hat of the carbonic acid ; the watermost closely resembles that of the Hissingen Racoczy, but is fourtimes stronger.It remains clear for a considerable time after haringbeen bottled. F. c.Analysis of the Kanizer or Kainzen Spring. By F. HULWA(J. ,237. Clxm. [2], 22, 290-293).-This spring comes from the car-bonaceous and dolomitic rocks not far from Partenkirchen, in thePartnacht valley of the Bavarian highlands. Under these rocks lies MINERALOGICAL CHEMISTRY. 31stratum containing iron, lead pyrites, and different salts. The tem-perature of the water is 8” ; it is nearly clear, but a sediment formson standing.It does not effervesce, but carbonic anhydride is evolvedon heating. It has a distinct odour of sulphuretted hydrogeii, anda faint sulphurous taste. The sediment consists of remains of phanero-gams and cryptogams, together with organic detritus. The reactionis distinctly alkaline, especially on boiling. Sp. gr. 1.00074. Itcontains no free carbonic acid. Sulphuretted hydrogen is present onlyin minute quantities. Composition in 100,000 parts = 100 litres :-a. Changeable Constituents.Organic residue .................. 1.200 parts.Oxygen required for oxidation ...... 0.288 ,,Calculated for organic bodies ...... 5.683 :,Ammonium nitrate ................ 0.185 ,,b. Nineral Constituent$.Sum of solid constituents : total residue = 58.6 parts containing :-Sodium ..............31.303 parts.Potassium ............ 0.4915 ,,Lithium .............. 0.0023 ,,Lime.. ................ 0.5230 ,,Magnesia .............. 0.4967 ,,Strontia .............. 0.0042 ,,Baryta ................ traceFerric oxide. ........... 0.075 ,,Manganese dioxide. ..... 0*0008 ,,Lead oxide ............ 0.005 ,,Copper oxide .......... 0.0082 ,,Silicic acid ............ 1.0000 ,,S ulphuric acid. ......... 2.646 ,,Chlorine .............. 0.7472 ,,Bromine ............... 0.009 ,,Jodine ................ 0.0045 ,,Sodium carbonate ...... 51.7538 .,Lithium .............. 0.005 7 ,,Manganese carbonate.. , . 0.1090 ,,Manganous ,, .... 0.0124 ,,Potassium sulphate. ..... 0.9082 ,,Sodium ,, ...... 0.8675 ,,Calcium ,, ...... 1.2700 ,,Magnesium sulphate . . . . 1.4901 ,,Strontium ,, .... 0.0070 ,,Sodium chloride ........ 1.2315 ,,,, bromide ........ 04026 ,,,, iodide .......... 0.0053 ,,Lead oxide ............ 0.0050 ,,Copper oxide .......... 0.0082 ,,Silicic acid ............ 1.0000 ,,Total carbonic acid. ..... 3 1.9000 ,,As bicarbonates. ........ 0.3 7032 ABSTRACTS O F CHEMICAL PAPERS.The following points are characteristic of the Kainzen spring.(1.) The extreme softness of the water(2.) The relatively small quantity of mineral constituents.(3.) The occurrence of minute quantities of sulphuretted hydro-(4.) The absence of free carbonic acid.(5.) The combination of sodium carbonate, chiefly as monocar-(6.) The relatively large proportion of sodium carbonate to the othergen.bonate.constituents. G. T. A

ISSN:0368-1769    

DOI:10.1039/CA8814000024

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

32 ABSTRACTS O F CHEMICAL PAPERS.Organic Chemistry.Etherification of Hydrobromic Acid. By A.'VILLIERS (Colt@rend., 90, 1488-1491) .-The extent to which hydrobromic acid,when treated with absolute alcohol and ft mixture of alcohol and water,undergoes etherification varies greatly with the temperature. Absolutealcohol, with different proportions of h ydrobromic acid, and heated atdifferent temperatures, gives the following results :-Percentage of acid etherified.+HBr + C2H60. AHBr + C2H60.At ordinary temperature, limit 658 days 68.0 52-57: 44" 9 7 79.6 59-97 7 100" 9 7 88.7 80.0The percentage of acid converted into ether is not so great as thatof the carbon acids, moreover, it is not fixed, but increases with thetemperature.These results show that combinations of alcohol with hydrobromicacid are formed analogous to hydrates,The presence of water decreases the extent of etherification, and inlarge quantity prevents any action from kaking place ; the quantity ofwater required to prevent the action increases with the temperature.This is probably due to the formation of hydrat.es of hydrobromic acid,and the dissociation of these hydrates as the temperature is raised.Hydrate of Methyl Iodide. By FORCRAND (Compt.rend., 90,1491--1493).-When a few drops of methyl iodide are placed in atube and a strip of filter-paper is introduced, crystals a.re deposited onthe edge of the paper after a short time. When all the iodide hasdisappeared from the glass a drop of water is seen at the end of eachcrystal, which increases as the crystal diminishes, and is finally absorbedby the filter-paper.During the formation of these crystals the tem-perature falls from about 16" to 15". By passing a current of moistair through the iodide large quantities of the crystals are formed, butwhen dry air is used, no crystals are formed, notwithstanding the tem-perature sinks to a greater extent. The crystals melt at -4", andtherefore cannot be ice. The analyses show them to have the com-L. T. 0'sORGANIC CHEMISTRY. 33position (CH,I),H,O.been obtained by Berthelot (Ann. Chim. Phys. [3], 66, 490).Similar compounds of carbon bisulphide haveL. T. 0's.Compound of Ether with Phosphorus Pentachloride. ByC. LIEBERMANN and L. LANDSHOFF (Ber., 13, 690-691).-A whitecrystalline compound is slowly deposited when absolute ether andfinely-powdered phosphorus pentachloride are well shaken together.The composition of the crystals could not be ascertained with accuracyon account of their rapid decomposition by moisture ; the analysesapproximately agree with the formula 2C4H,,0 + 3PC1, orP,C1,,CsH,*02.This substance is not a simple addition-product, since on addingwater to it ether is not set free, but phosphoric and ethylphosphoricacids are produced.On distillation, it splits up into phosphorus tri-chloride and a mixture of chlorinated organic derivatives. w. c. w.Action of Methyl Bromide and Methyl Iodide on Mono-methylamine. By E. DUVILLIER and A. BUISINE (Cowpi. rend., 90,1426-1427) .-When equal molecular proportions of methyl bromideand monomethylamine, dissolved in methyl alcohol, are heated at loo",the products of the reaction consist of unaltered monomethylamine,small quant<ities of di- and tri-methylamine, and large quantities oftetramethylammonium bromide.A similar result is obtained bytreating methylamine with inethyl iodide, the reaction being veryviolent. These reactions are similar to that of methyl nitrate onmonomethylamine, and they are all comparable with the action ofmethyl iodide on ammonia. L. 2'. 0,s.Amylamines from Inactive Amy1 Alcohol. By R. P. PLIXPTON(Compt. rend., 91, 433435).-A quantity of inactive amyl chloridewas prepared by Le Bel's process (Compt. rend., 77, 1021) from themixture of active and inactive alcohols resulting from fermentation.The chloride prepared in this way (b.p. 100.5") was without action onpolarised light when examined in a tube 1 meter long. Heated at 150"in a digester for one or two hours with a little more than its own weightof a saturated solution of ammonia in alcohol, it was converted intoa crystalline mass. From this the amylamine wits separated in theusual manner, and purified by repeated rectification over potash. Itboils at 96.5" under a pressure of 766 mm. (Wurtz, 95" ; Brazier andGosleth, 93"; Custer, 92-93') : a trace of moisture lowers the boilingpoint 2-3".Awylumine hydrochloride (inactive) is very soluble in hot alcohol,insoluble in ether. The platinochloride separates from hot water inplates.The aurochloride is obtained by slow evaporation in clino-rhombic crystals, resembling those of augite. It is soluble in alcoholand ether. The residue from the distillation of the amylamine con-tains inactive diamylamine and triamylamine. These were separatedas far as possible by fractional distillation, converted into hydrochlo-rides, and treated with ether, which dissolves triamylamine hydro-chloride only.Sp. gr. a t 22.5" = 0.7517.VOL. XL. 34 ABSTRACTS OF CHEMICAL PAPERS.Dz'antylnrnine, prepared from the hydrochloride purified by crystal-lisation from water, boils at 185" (Hofmann, 176" ; Custer. 187", forthe product obtained from nitrosodiamylamine). The liydrochloricleforms splendid plates, sparingly soluble in hot water. The plntinochlo-r i d e crpstallises well, is soluble in alcohol, but not in water.Theanrochloride forms needles soluble in alcohol, insoluble in water.It is anoleaginous liquid, insoluble in water. The h ydroch loride separatesfrom ether in slender prisms. It is very soluble in etlher and alcohol,less soluble in water; melts below 100". The platinoch,loride is in-soluble in water. The aurochloride crystallises from alcohol in needles,insoluble in water.1 kilo. of inactive amylarnine chloride gave 15-20 grams of amyl-amine, 150 grams of diamylamine, and about 130 grams of t'riamyl-amine. J. M. H. M.TriumyZumirLe boils a t 237" (uncorr.) (Hofmann, 256").Thiovaleraldehyde. By G. A. BARBAGLTA (Ber., 13, 1574j.-Schroeder (Ber., 4, 402) describes a solid thiovaleraldehyde obtainedby acting on valeraldehyde with aulphuretted hydrogen.Ry heatingsulphur and valeraldehyde at 250" in sealed tubes, a liquid valeralde-hyde, CsH,,S, has been obtained. It is a clear liquid of exceedinglydisagreeable odour, resembling that of garlic. It boils at 114-115" ;is insoluble in water, and easily miscible with alcohol or ether. Vale-rianic acid is formed during the reaction, which may be expressed asfollows :-4CsHloO + S, = 2CSH1,S + 2C5Hl002. P. P. B.Action of Chlorine on Di-isopropylketone. By G. A. BAR-BAGLIA and P. GUCCI (Ber., 13, 1570--1571).-iM0tz0chZor0-~li-i~0p~~p~/l-katone, C,HLIC1O, is obtained by acting on dry di-isopropylketone withdry chlorine ; it is a liquid having an odour resembling that of cam-phor and turpentine, and boils a t 141-142'.Dichloro-di-isopropylketone, C7HI2C1,0, is obtained by passing chlo-rine into the ketone and water; it is a liquid having an odour ofturpentine, and boils a t 175-1 76".T~ichZoro-di-isopropyllcetoiie, C7HIIC130, is obtained by the action ofchlorine on the vapours of di-isopropylketone ; it is a colourless liquid,which blackens on standing, and has a penetrating odour ; it boils a tThe further action of chlorine on di-isopropylketone is attendedwith the production of resinous bodies.Constitution of Lactones.By J. BREDT (Ber., 13, 748-749).-The author finds that isocaproic acid is converted, by oxidation withpotassium permanganate, into the lactone, C6Hlo02, identical with thelactone obtained by heating terebic acid, and infers that the lactonesought to be regarded as the phthalides of the fatty series.228-229".P. P.B.w. c. w.Propylacetal and Isobutylacetal. By J. GCRARD (Coinpt. rend.,91, 629-631).-Propylacetal is obtained by passing a current of non-inflammable phosphoretted hydrogen for several hours info a mixturORQANIC CHEMISTRY. 35of aldehyde and propylic alcohol. After the products have beenmashed with water and dried by contact with calcium chloride, thepropylacetal is isolated by fractional distillation, Itr is a colourlessliquid, b. p. 146-148" ; iiisoluble in water, but soluble in alcohol andi n ether; sp. gr. a t 22.5" = 0.825. It does not reduce ammoniacalsilver nitrate, and is not acted on by potassium, or by a boiling solu-tion of potash.Concentrated hydrochloric acid dissolves it withoutcoloration ; strong sulphuric acid carbonises it in the cold.Isobutylacetal is obtained in a similar manner, and its propertiesare similar to those of propylacetal ; b. p. 168-170" ; density a t 22"= 0.816. R. R.Dry Distillation of Calcium Isobutyrate. By G. A. BAR-BAOLIA and P. GUCCI ( B e y . , 13, 1571--1572).-Amongst the productsobtained by the distillation of calcium isobutyrate, beside di-isopro-pylketone, the authors have fonnd water, isobutgric acid, isobutyl-aldehyde (Popoff, Ber., 6, 125?5), methylpseudobutylketone (describedby Butlerow, Ber., 7 , 729), and a compound having the empiricalformula C,H,,O. This compound is a liquid having an odour re- u sembling that-of peppermint,'and boils at 150-152".P.P. B.Itaconic Anhydride. By R. ANSCH~~TZ and W. PETRI (Ber., 13,1539--1540).--lt has been shown in former communications (Ber.,10, 325 and 1881) that dibasic acids are easily converted into theiranhydrides by the action of acetic chloride, and that whilst fumaricacid is not attacked by this reagent, maleic acid is converted into itsanhydride (Ber., 12, 2281). Itaconic acid heated in the water-bathwith acetic cbloride is also converted into the anhydride.Itaconic anhydride, C5H4O3, crystallises from glacial acetic acid incolourless, transparent, compact columnar crystals ; it melts at 68" anddistils a t 139-140" under a pressure of SO mm. If distilled underthe ordinary pressure, it is converted into citraconic anhydride.Itaconic anhydride, mixed with glacial acetic acid or citraconic anhy-dride, remains liquid for a considerable length of time when cooledbelow its melting point.When dissolved in warm water, it is con-verted into itaconic acid. It crystallises from chloroform in clearprismatic crystals, belonging to the rhornbic system, which becomedull on exposure to the air. It resembles maleic anhydride in ap-pearance, and in its behaviour with acetic acid and chloroform.P. P. B.Decomposition of Citric Acid by Distillation. By R. ANSCH~TZ(Rer., 13, 1541-1543) .-When citric acid is distilled, the portioncoming over between 200-215" separates into two layers. If thesebe separated, and the heavier portion fractionated under reducedpressure (30 mm.), the following three fractions are obtained :-(l), 180"; (2), 120-130"; (3), 130-140".The author finds thatfractions (2) and (3) consist chiefly oE itaconic anhydride, whilst thefirst fraction consists of citraconic and itaconic anhydrides. Theformation of these anhydrides is explained as follows :-d 36 ABSTRACTS OF CHEMICAL PAPERS.COOH.CH,.C(OH). (COOH).CH,.COOH - H,O =COOH.CH2 C(CO0H) : CH.COOH.Aconitic acid.COOH.CH2.C(COOH) : CH.COOH - H2O =COOH. CH,.C-CO-C0OH.CH: C-CO CH-COHypothetical aconitic anhydride. Hypothetical aconitic anhydride.The first aconitic anhydride loses CO, and gives citraconic anhy-CH,.CO.dride, having the formula I >O ; whilst the second wouldCH,: C-COyield CO, and itaconie anhydride, to which the constitutional formulaCH3.C-C 0-CH-GOII >O is attributed.The author bas shown (preceding abstract) that itaconic anhy-dride is converted by heat into citraconic anhydride.Its formation inthe above case is accounted for by its being carried over by the currentof carbonic anhydride produced in the above decomposition.P. P. B.Mucobromic Acid. By H. B. HILL (Ber., 13, 734-739).-Bythe action of dry bromine (1 mol.) on mucobromic acid (2 mols.) at130-140°, a mixture of bromomucobromic and dibromosuccinic acidswith dibromomaleic anhydride is produced. The acid which is formedby dissolving the anhydride in water is identical with Kekul6’sdibromomaleic acid. The dibromo-fumaric acid which Limpricht andDelbriick (Annalen, 165, 293) obtained by heating mucobromic acidwith bromine and water is also identical with dibromomaleic acid.Mucobromic acid also yields dibromomaleic acid on oxidation withdilute nitric acid.w. c. w.Influence of Isomerism of Alcohols on the Formation ofEthereal Salts. By MENSCHUTKIN (An?. Chim. Phys. [5], 20, 289-361).-The author has endeavoured to throw light on the relationsof isomeric alcohols by a quantitative study of the formation ofethereal salts by heating the various alcohols witrh the same acid. Ona future occasion he proposes to extend the research by heating thesame alcohol with various acids. The present paper has reference tothe reaction of acetic acid with primary, secondary, and tertiaryalcohols and with phenols, a short account of which has alreadyappeared (this Journal, 1879; Abstr., 36, 214, and 215). Similarexperiments were carried out by Berthelot and PQan de St.Gillesin 1862 and 1863, but at that time the isomeric alcohols were littleknown.M&od of Bxperiment. -A certain quantity of the alcohol wasweighed out, and the theoretical equivalent of acetic acid added froma dropping pipette. About 0.3 gram of the mixture was then weigheORGANIC CHEMISTRY, 37carefully into a tube of 5 mm. diameter, of such a, length that themixture occupied half t o two-thirds of the volume. The tube wasscaled and suspended in a glycerol-bath, kept constant a t 1543. A tthe end of a certain number of hours the tubes were withdrawn fromthe bath and broken into stoppered flasks, containing about 50 C.C.ofalcohol. A few drops of an alcoholic solution of rosolic acid wereadded, and the free acetic acid titrated with standard baryta-water.The observations were made with a view to obtaining two sets ofnumbers-(1) the initial rate of ethertjication, expressed by the per-centage of acid found combined with the alcohol a t the end of thefirst hour; and (2) the limit of etheriJcation, expressed by the per-centage of acid converted into an acetate when etherification ceased.The error of experiment for the former determination areraged0.4 per cent. from themean.Acetic Ethers of the Primary Alcohols.-The alcohols, first purified asfar as possible, were in all cases dried over caustic baryta.The fol-lowing mode of procedure was adopted, as it was the only one thatafforded a guarantee of the completeness of the desiccation :-Thewhole quantity of purified alcohol was dried over baryta, distilled, andan etherification assay made ; the remainder was treated a second timewith baryta and distilled, and another etherification essay made. Ifthe second really agreed with the first, the experiments were assumedto be correct; if not, the drying and testing were repeated until twosuccessive series of results showed no appreciable difference. Theresults obtained in this way have already been given (Zoc. cit.,p. 36).With regard to the limit of etherificntion, Berthelot and St. Gillesconcluded that “ the equivalent proportions of acid and alcohol thatenter into combination are almost independent of the special nature ofthe acid or alcohol.” The results obtained by the author are opposedto this conclusion, and show on the other hand that (1) methyl alcoholis distinguished from all other alcohols by its high limit; (2) for theother members of the CnH2,+,.H0 series, the limit increases with in-crease of molecular weight, but is not influenced by isomerism;(3) alcohols of the unsaturated series have a considerably lower limitthan those OF the C,H2n+l.H0 series; the limit of ally1 alcohol, forexample, being 7.5 per cent.less than that of propyl alcohol.Acetic Eth ens of the SecorLdnry McohoZs.-The author’s mean resultsmay be exhibited briefly in the following table, similar to that for tlheprimary alcohols :-1 per cent.from the mean ; for the latter,Alcohol. Initial rate.Dimethylcarbinol (isopropyl alcohol) . 26.53E thylmethylcarbinol (secondary butylalcohol) ........................ 22.56Isopropylmethylcarbinol.. .......... 18.95Ethyl vinyl carbinol .............. 14-85Diethylcarbinol .................... 16-93Hexylmethylcarbinol (cnpryl alcohol). 21.19Diallycarbinol .................... 10.31Limit.60.5250.2859.3158.66630352-2550.138 ABSTRACTS OF CHEMTCAL PAPERS.Both the initial rate and the limit of etherification are thus muchlower for secondary than for primary alcohols. Comparing the formeramongst themselves, the highest initial rate is that of dimethylcar-binol ; whilst the two other alcohols of similar structure, ethylmethyl-carbinol and hexylmethylcnrbinol, have a lower rate almost identicalin the two cases.The influence of isomerism in lowering the rate isshown by comparing isopropylmethylcarbinol (18.95) with diethyl-carbinol (16.93). The relative initial rate is lowered by increase ofmolecular weight and by isomerism, as the following numbers show :-Dimethylcarbinol, 43.85 ; ethylmethylcarbinol, 38.10 ; hexylmethyl-carbinol, 34.16 ; isopropylmethylcarbinol, 31.95 ; diethylcarbinol, 28-86,The absolute and relative rates are also lower for alcohols containingunsaturated radicles than for those containing only CnB2n+l radicles,but this difference is not so great as it is with the primary alcohols.The limit of etherification of secondary alcohols does not show anincrease with increase of molecular weight, but is considerably lower€or the non-saturated than for the saturated series.Acetic Ethers of Tertiary AZcohoZs.-The reaction of tertiary alcoholswith acetic acid differs from that of primary and secondary alcohols,being generally complicated by dissociation of the compound etherinto olefine and acid, and the re-formation of the tertiary alcohol bycombination of the olefine with water in presence of acid ; and perhapscombination of the olefine with acid to form the ethereal salt.AHthese reactions are limited. After heating the mixture for a certaintime, equilibrium is established, which, as the formation of the olefineis a; case of dissociation, depends on the temperature.1.Formation of the Cornpound Ether with Elimination of Wafer.-On account of the partial dissociation of the ethereal salt into hydro-carbon and acid, the limit of etherification cannot be ascertained withaccuracy; but it is very much lower than in the case of pyimary orsecondary alcohols, and is attained in a comparatively short time.The quantity of acid etherified a t the end of 24 hours, compared withthe mean limit and the initial rate (absolute) of etherification, havealready been given (Zoc. cit., p. 216).2. Decomposition of the Ethereal Salt by the Water formed in theReaction.-In consequence of the relatively larger quantity of waterformed during the etherification of tertiary alcohols, this reactionproceeds to a much greater extent than in the case of primary andsecondary alcohols.3.Dissociation of the Compound Ether into Olefine und Acid.-Thisreaction occurs in all the cases studied, and reaches a limit dependenton the temperature employed. Equations representing the equilibriumof the system formed by a molecular mixture of trimethylcarbinol andacetic acid a t 155" have been given (Zoc. cit., p. 216).The author gives in detail the analytical data from which theseequations are deduced. The polymerisation of the olefines under theinfluence of sulphuric acid is explained by the author as the dissocia-tion of sulphovinic ethers of the tertiary alcohols, which it is knownare produced from these hydrocarbons by fixation of water.Acetic Ethers of PhenoEs.-The results of experiments with phenol,paracresol, thymol, and a-naphthol have been given (Zoc.cit., p. 217)ORGANIC CHEMISTRY. 39They show a striking resemblance in this respect t o tertiary alCohol6,with which the author suggests they should be classed ; their similarityin structure is shown by the position of the hydroxyl group, this beingin both cases attached to a carbon atom, whose remaining affinitiesare satisfied by carbon atoms. The continuity between the aromaticand other series is again shown by these experiments. No dissociationof the acetic ethers of this class was observed a t the temperature(155") employed. The general conclusions to be deduced from thewhole of the anthor's experiments have been pointed out in theremarks on each class.J. M. H. M.Influence of Isomerism of Monobasic Saturated Acids onEtherification. Ey N. MENSCHUTKIN (Bull. SOC. Chim. [3], 34, 87-388).-The relative initial velocity (at the end of one hour a t 155" C.)and limit of etherification of primary, secondary, and tertiary mono-basic fatty acids are compared :-Primary acids. Initial velocity. Limit.Formic acid.. .......... 61-69 64.23 (at 100" C.)Normal butyric acid.. ... 33.25 69.52 ,,Normal caproic acid.. ... 33.08 69.81 ,.Acetic acid ............ 44.36 67.38 (at 155 C.)Propionic acid ......... 41.18 68.70 ,,Normal caprylic acid .... 30.86 70.87 ,,Isobutyric acid ......... 29.03 69.51 ,,Trimethyl-acetic acid.. .. 8.25 72.65 ,,Secondary acids.Methylethyl acetic acid. . 21.50 73.71 ,,Tertiary acids.Dimethylethyl-acetic acid 3.45 74.15 ,,V.H. V.Oxidation-products of Dimethyluric Acid. By C. F. MABERYand H. B. HILL (Ber., 13, 73'3-740) .-Methylalloxan and methylcar-bamide are formed by the oxidation of dimethyluric acid with nitricacid or with hydrochloric acid and potassium chlorate. In the lattercase a small quantity of a compound having the composition C6H,NzOsis produced. This substance crystallises i n prisms (m. p. 160') whichare sparingly soluble in cold water.Methylparabanic acid (m. p. 149") is formed from dimethyluricConversion of Terebenthene into Cymene. By BRU$RE(Conzpt. rend., 90,1428-14-29).-When terebenthene is dropped slowlyinto boiling sulphuric acid mixed with 2 mols. of water, a mixture ofcymene with unaltered terebenthene and water distils over.This an-altered terebenthene is polymerised by agitation with concentratedsulphuric acid and the cymene purified bey a final distillation. Thewater is separated out from the product, the sulphurous acid neutralisedwith sodium carbonate, and the remaining liquid dried and fraction-It appears to act as an acid.acid by long-continued boiling with nitric acid. w. c. w40 ABSTRACTS OF CHEMICAL PAPERS.ally distilled. Unsuccessful attempts were made to substitute otherbodies for sulphuric acid, which is very violent in its action, but onheating 1 mol. of terebenthene with 1 mol. of ethyl sulphate a t 120"for 10-15 hours, the mixture assumes a violet colour, and containscymene, et,her, and sulphurous acid.By allowing terebenthene andethyl sulphate to remain in contact for some time at loo', the mixturegradually becomes homogeneous. The liquid produced is heavier thanwater, is stable at the ordinary temperature, of a lemon-yellow colour,and peculiar odour. When cooled to -20" the mixture separates intotwo layers, one of terebenthene, the other of ethyl sulphate. The homo-geneous solution appears to be a very unstable combination of tereben-thene and ethyl sulphate, ~loH16.S04(C2H5)2, which readily splits upinto cymene and ether-Remarks on Kelbe's Discovery of a New Cymene in LightResin Oil (Resin Spirit). By H. E. ARMSTRONG and W. A. TILDEN( B e y . , 13, 1548--1549).-The authors draw attention to the fact thatthey have been engaged for some time in the investigation of "resinspirit'," and have already published some account of their results (thisJournal, Trans., 1879, 275, and Ber., 12, 176).Whilst acknowledgingthe right of Kelbe to continue the investigation of the new hydrocarbon,the authors wish to reserve the further study of resin spirit.P. P. B.Synthesis of Hexmethylbenzene and of Mellitic Acid. ByC. FRIEDNL and J. M. CRAFTS ( C o q ~ t . rend., 91, 257-260).-1n aprevious paper (Compt. reid., 84, 1394), the authors announced theformation of tetramethylbenzene by passing a current of methyl chlo-ride through a warm mixture of benzene with aluminium chloride ; at,the same time they suspected the presence of pentamethylbenzene andhexmethylbenzene amongst the products.By operating with tolueneinstead of benzene they have succeeded in preparing these two com-pounds in considerable quantity.On purification by fractional distillation and pressure of the solidproduct, three distinct compounds are obtained, boiling constantly at190", 225", and 264", and melting a t 110", 50", and 164' respectively.The first of these bodies is tetramethylbenzene, the second penta-methylbenzene, and the third hexmethylbenzene. The vapour-den-sities of the two latter are 5.27, 5.73 (experiment), correspondingwith 5.12 and 5.61 (theory). Attempts were also made to purifythese substances by fractional crystallisation from alcohol and by theaction of strong sulphuric acid, which attacks the less methylatedbenzene hydrocarbon first.Neit'her of these methods was successful.By oxidising hexmethylbenzene with dilute nitric acid or with nitricacid and potassium permanganate, a mixture of acids was obtained,amongst which there appenred to be a small quantity of mellitic acid.When potassium permanganate alone was used for the oxidation, andthe action allowed to spread over several months, a much larger quan-tity of meilitic acid (as potassium mellitate) was obtained, whicORGANIC CHEMISTRY. 41was identified by its reactions with salts of barium, calcium, zinc,copper, silver, and magnesium, and by analysis of the silver salt.J. M. H. M.Paraditolylnitrosarnine. By A. LEHNE (Ber., 13,1544--1545) .-Gerber (Dissertation, Zurich, 1874) and J. Cosack (Bey., 13,1092) havealready obtained this body.The author prepares it by heating dito-lylamine in alcohol with hydrochloric acid and then adding a solutionof sodium nitrite. It is insoluble in water, but soluble in ether, ben-zene, and light petroleum, and sparingly so in alcohol. I t crystal-lises from light petroleum in golden-yellow rhombic crystals. Bro-mine acts on this nitrosamine, forming tetrabromditolylamine,(C7H5Brz),NH, which me1t.s at 162". It has been described by Gerber(Zoc. cit.).Heznit~-oditoZyZainine, Cl4H8(NOZ),NH, is prepared by the carefulnitration of paraditolylnitrosamine, it may also be obtained from para-ditolylamine. It crystallises from glacial acetic acid in yellow crys-tals, which melt a t 258O, and is sparingly soluble in the ordinarysolvents.Its acetic acid solution on reduction with zinc-dust gives adeep-red coloration. Hexnitroditolylamine corresponds with thenitro-derivative of diphenylamine, used as n dye under the name of" tiurantia." P. P. B.It may also be obtained directly from ditolylamine.Paraditolylhydrazine. By A. LEHNE (Ber., 13, 1546-1 547).-This compound is prepared by the reduction of ditolylnitrosaminewith zinc and acetic acid in a mariner analogous to Fischer's prepara-tion of diphenylhydrazine (Hydrazinverbiiidungen ; Miinchen).Fai.aditoZyZhydrazine, (C,H,),N,H,, crystallises from benzene incolourless leaflets, melting at 171-172". It is easily soluble in alco-hol and benzene, sparingly in ether, and almost -insoluble in lightpetroleum.When dry it does not change on exposure to the air, itschloroform solution, however, becomes blue under these circumstances.T h e hydrocldoride, ( C7H7),N2H2.HC1, is an unstable salt ; it crystal-lises in slender colourless needles. It is easily soluble in water, and itssolution on cooling decomposes into basic salt and free acid, on warm-ing the salt is again formed.dfonob enzoy ZdituZ y Zhydrazine, ( C7H,) ,N,H. C,H,CO, is obtained byacting on a solution of the base in benzene with benzoic chloride. Itcrjstallises in slender colourless needles, melting at 186.5". Its solutionin benzene becomes dark green on exposure to the air. Nitrous acidconverts ditolylhydrazine into ditolylnitrosamine. Ditolylhydrazineis converted by bromine into tetrabromoditolylamine, and by nitricacid into hexnitroditolylamine.Oxidising agents, such as ferricchloride or mercuric oxide, convert it into ditolylamine.P. P. B.Azo-derivatives. By J. H. STKBRINS (Ber., 13, 715-718).-Azobenzenehydroxybenzo~c acid, PhN,.CsH3(OH) .COOH, is deposited inorange-coloured needles from an alkaline mixture of diazobenzenenitrate and salicylic acid. The crystals are soluble in alcohol andinsoluble in water. A sulphonic acid is obtained by the action ofsulphuric acid42 ABSTRACTS OF CHEMICAL PAPERS.Phloroglucin~arazobeizzen esuZp3hoiiic mid, CRH4( HSO,) .N2. C6H2( OH),,crystallises in yellow plates, having a metallic lustre. The sodiumsalt is prepared by mixing sodium paradiazobenzenesulphonnte withan alkaline solution of phloroglncin. The precipitated salt is purifiedby solution in hot water and rep~ecipitntion by sodium chloride.Axobeizze,iediu?n.idotoluene, C6H5.B2.C6H2Me(NH2)2, is obtained inyellow needles soluble in alcohol, by treating with ammonia the pro-duct of the action of a-toluylenediamine on diazobenzene.This baseforms a hydrochloride, crystallising in orange-coloured needles, whichdissolve freely in water. With an excess of hydrochloric acid, anunstable scarlet coloured crystalline compound is produced. Thehydrochloride also forms crystalline double salts with metallic chlo-rides.Uinm.):doazonc7phthaZene, CloH7.N2.CloH5(NH2)2, prepared from diazo-naphthalene nitrate and diamidonaphthalene, unites with acids to formbrown coloured salts.A mbenmnecresoZsuZp honk acid, CsH5.N2.CeH2Me (H SO,). OH, obtainedby the action of diazobenzene nitrate on an alkaline solution of cresol-sulphonic acid, forms brown, needle-shaped crystals, having a strongmetallic lustre. It dissolves in alcohol, forming a solution whichdyes silk or wool yellow. w. c. w.Action of Hydrochloric Acid on Organic Amides (Preli-minary). By L. SCHULERUD (J. pr. Chem. [el, 22, 288-290).-When amidobenzoic acid is heated in a stream of dry hydrochloric acidgas, ammonium chloride sublimes, and a solid amorphous residueremains in the retort. This body is nnactled on by the ordinarysolvents, but is soluble in concentrated sulphuric acid, and is preci-It does not melt when[eated, but chars and decomposes. Analysis gave no satisfactoryresult.When heaked with hydrochloric acid gas, salicylamide splits upinto disalicylamide and ammonia.A part of the amide sublimesunaltered, water and phenol are also evolved. Disalicylamide is ayellowish-white, asbestos-like body, consisting of small, woolly needles,insoluble in water, but tolerably soluble in hot alcohol and acetic acid.The alcoholic solution gives a yellowish-red to blood-red precipitatewith ferric chloride. The diamide (m. p. 197-199") dissolves inalkalis with a yellow colour, and forms compounds with metals. Thesilver compound, (C,H,( OH). CO),NAg, is crystalline, and of a yellowcolour.Salicylamide absorbs hydrochloric acid slowly at ordinary tempera-tures, with formation of a compound, from which a stream of dry airgradually expels the gas in the cold.The gas is also expelled bywarming the compound either alone or with water or alcohol. Whenhydrochloric acid is passed into a solution of salicylamide in dry ether,brilliant acicular crjstals are formed, consisting of 2C6H4( OH).CONB, + HCl. Hjdroxybenzamide is obtained by leaving the ether ofhydroxybenzoic acid in contact with strong ammonia. It forms colour-less thin plates (m. p. 167" uncorr.), which dissolve readily in hotwater and in alcohol. G. T. Aitated from the solution unchanged by waterORGANIC CHEMISTRY. 43Alphatoluylamide. By C. L. REIXER (Bey., 13, 741).-In thepreparation of benzyl cyanide by the action of potassium cyanide onbenzyl chloride, a-toluylamide is obtained as a bye-product.Thetoluylamide is found in the retort,, after the benzyl cyanide has beendistilled over i n a current of steam. w. c. w.Phenyl- and Tolyl-thiocarbimide Glycollide. By M. VOLTZKOW(Rer., 13, 1579--1580).-The author describes some homologues ofphenylt8hiocarbimide-glycollide (this Journal, 38, 659), which havebeen obtained in a similar manner.>CO, obtainedfrom paratolplthiocarbimide and monochloracetic acid ; it crystallisesfrom hot wat>er in small leaflets or needles (m. p. 162"), easily solublein the ordinary solvents. It is decomposed by boiling with baryta-water in a manner analogous to the phenyl-derivative, yielding para-toluidine, barium carbonate, and barium thioglycollate.Orthotolylthiocarbimide-glyco~licle is prepared in a manner similar tothe para-compound ; it crystallises in white, shining needles (m.p. 120°),and is easily soluble in the ordinary solvent's. b y boiling with baryta-water, it is resolved into orthotohidine, carbonic anhydride and thio-glycollic acid.When phenyl- or tolyl-thiocarbimide is heated with monochloraceticacid alone, then compounds are formed having the formule CsHsNOC1and C9HIoNOCl. The former is obtained from phenylthiocarbimide, thelatter from to 1 y 1 thiocarbimid e.PnratoZylthiocarbimide-glycollide, C,H,.N C<--,- S.CH,P. P. B.Guanylthiocarbamide and some Guanylguanidines. By E.RAMBERGER (Bey., 13,1580-1384) .-The author regards Rathke's thio-dicyandiamine (Ber., 11, %7), guanylthiocarbamide, and the compounddescribed by the same author (this Journal, 34, 804)) having theformula NHPti.CS.NPh.C(NH,) : NHPh, as a triphenylated panyl-thiocarbamide. The following derivatives of this guanylthiocarbamidehave been obtained :-GuaiLyl~he,L2llthiocarbamida, CsSN,H,,, prepared by acting upon guani-dine carbonate with phenylthi ocarbimide, crystallises in white, shining,strongly refractive, monoclinic crystals (m.p. 175-1 76"). It dissolvesin alcohol, yielding an alkaline solution. It is a base, and is easilysoluble in acids. Its hydrochloride, C,SN,H,,.HCl, cryst>allises in long3silky needles, and is more easily soluble in alcohol than water; onwarming, its aqueous solution evolves sulphuretted hydrogen. Thissolution gives a yellow precipitate with platinum chloride, and a dirtyviolet precipitate with copper sulpiiate, becoming black on boiling,owing to its conversion into sulphide.The picrute, C,SN,H,,.C,H,(NO,),OH, crystallises in yellow needles.The oauZl_rte crystallises in white, shining scales.The mdphate cryvs-tallises in shining leaflets ; its aqueous solution decomposes whenwarmed, forming a yellow powder, which is soluble in alcohol. Byheating with hydrochloric acid a t 185", the base is resolved intocarbonic anhydride, sulphuretted hydrogen, aniline, and perhap44 ABSTRACTS OF CHEMICAL PAPERS.guanidine, and may therefore be represented by either of the twofollowing formulae :-NHPh NHPh"<NH.C(NH,) : NH Or "<N: C(NH,)iPhenyZguanyZguanidine, NH C(NHPh).NH.C(NH,) : NH.Thenitrat.e of this base is obtained by treating guanylphenylthiocarbamidewith ammoniacal silver nitrate ; it has the composition C9H6H1203, andmelts at 208-209". It is easilysoluble in alcohol and water, and thebase is precipitated from its aqueous solutions in a flocculent state bysoda, but becomes crystalline on standing.When guanylphenylthiocarbamide is treated with an alcoholic solutionof mercuric chloride, the hydrochloride C,N5Hi.HC1 is obtained ; andthe sulphate is obtained by treatment with silver sulphate. Whentreated with moist silver oxide, the hydrochloride yields the free baseCsH,H,,, which crystallises in white leaflets ; it is easily soluble in alco-hol and in water, and is precipitated from its aqueous solutions by soda.DipiLenylguamylgunnid~ne, N Ph C(NHPh).NH.C(NH,) : NH.Thenitmte of this base is obtained by treating guanylphenylthiocarbamidewith silver nitrate in presence of aniline. It crystallises from water inshining white needles united in groups (m. p. 231'). The free baseis precipitable on adding soda to the aqueous solution of the nitrate.The base is unchanged by exposure to the air, and is more easily solublein alcohol than water, forming an alkaline solution. P. P. €3.Constitution of the Thiourethanes. By C. LIEBERMANN (Bsr., 13, '682-689) .-The acid nature of phenyllhiouretlzane, PhN : C (SH) .OEt,is shown by the fact that this substance dissolves in dilute solutions ofpotash, soda, or baryta, and is reprecipitated from these solutions onthe addition of an acid.Phenylthiourethane forms metallic compounds,which are obtained as crystalline precipitates when certain metallicsalts are added to its alcoholic solution, e.g., PhNC (Spb).OEt +H20; PhN : C(SAg).OEt, and PhN : C(SHgCl.HCI).OEt. By theaction of methyl and ethyl iodides on the silver salt at loo', methyl andethylderivatives have been prepared. PhN : C(SMe).OEt is an oilyliquid (b. p. 260-265'), soluble in strong hydrochloric axid, but repre-cipitated on dilution with water. The hydrochloric acid solution giveswith platinum chloride an orange-coloured crystalline precipitate,which is sparingly soluble in cold alcohol.EtZiy~7~enylthiourethal.Le, PhN : C( SEt).OEt, when freshly prepared,is an oily liquid (b. p. 275"), which slowly solidifies to a crystallinemass (m.p. 30"). The platinochloride resembles that of the precedingcompound.The ethyl compound is decomposed by the action of dilute sulphuricacid at 200" into aniline and ethyl thiocarbonate, according to the fol-lowing equation :-PhN:C(SEt).OEt + H,O = Ph.NH2 + EtO.CO.SEt.When phenylthiourethane is heated with dilute sulphuric acid, itsplits up into aniline, alcohol, carbonic oxide, and sulphuretted hydro-gen.PhN:C(SH).OEt f 2H20 = Ph.NH, + CO, + HZS + EtHOORGANIC CHEBIlSTRY. 45On boiling a mixture of methylphenyl thiourethane, aniline, andalcohol in a flask connected with an upright condenser, methylmer-captan and diphenylcarbamide are produced.PhN: C(SMe).OEt + PhNH, + H20 = EtHO $- MeHS +I f alcoholic ammonia is substitmuted for aniline in the precedingexperiment, miline and monophenylguanidine will be produced.From the preceding reactions the author concludes that thioure-thanes have the constitution R.N : C<oE.The formation of phenyl-thiocarbamidoglycollide by the action of monochloracetic acid onphenylthiourethane, must be represented as follows :-NHPh.CO.NHPh.SMPhN: C(SH).OEt + ClCH,.COOH = HCl + EtHO +PhN: C < s * ~ ~ > C O . -w. c. w.Para- and Ortho-tolylthiourethanes. By C. LIEBERNANNand S. NATANSON (Ber., 13, 1575--1579).-1n favour of the viewsalready advanced by one of the authors (Bey., 13, 682), as to the con-stitution of phenylthiourethane, the formation of phenylurethanesulphide, NPh : C(OEt).S2.C(OEt) : NPh, is cited.This compoundis obtained by decomposing silver phenylthiourethane,with iodine. It crystallises from alcohol in colourless rhombic prisms,and melts at 102".ParatoZylthioz.crethane, C,H,N C (OEt) .SH, is prepared in a, mannersimilar to the plienyl derivative, viz., by heating paratolylthiocarba-mide with alcohol a t 130". It forms colourless transparent crystals,melting at 87".Ortlzotoly Ithiourethane is prepared from the orthotolylthiocarbamide.It is an oil.Both the tolylthiourethanes are soluble in dilute alkalis, and are re-precipit'ated by acids. Ammoniacal silver nitrate precipitates the silversalts from alcoholic solutions of the tolylthiaurethanes. The methyl andethyl derivatives of these tolylthiourethanes have been obtained by de-composing the silver salts with methyl and ethyl iodides respectively,These derivatives may also be obtained by boiling solutions of thetolylthiourethanes in caustic alkalis with methyl or ethyl iodide.The methyl and ethyl salts are oils, which distil above 250" withoutdecomposition.The ethyl derivative of paratolylthiourethane yields mercaptanwhen heated with ammonia ak 150"; with dilute sulphuric acid a tPhN : C(OEt).SAg,200", paratoluidine sulphate and ethyl.thiocarbonate are formed.P. P. B.Introduction of the Hydroxyl Group by Direct Oxidation,By R. MEYER and A. BAUR (Ber., 13, 1495--1500).--In continuingtheir investigatsions (Ber., 11, 1283, 1787, 1790, 2172; and 12, 1071,2238), the authors have submitted the potassium cymenesulphonat46 ABSTRACTS OF CHEhITCAL PAPERS.(cymene from camphor) to the action of potassium permanganafe. Inthis way potassium hydroxypropylsulphobeiizoate is formed, thus :-C6H,MePr.So3H + 0 4 = CooH.C,H,(Hso,).C,H,(OH).The potassium sult, CloHl,,S06Kz + 2H,O, crystallises from absolutealcohol in beautiful shining needles, but is deposited in rhombic tableson slow evaporation of the alcoholic solution; and from its aqueous so-lution in large rhombic crystals: By evaporation with hydrochloricacid, the potassium salt is converted into an acid which combinesdirectly with bromine, and probably has the formulaCOO H.C6H3 ( S O,H) . C3H5.That the hydroxypropylsnlphobenzoic acid does not contain thehydroxyl in the ‘‘nucleus’’ is shown by its solution yielding nocoloration with ferric chloride.The introduction of a hydroxyl groupin this cymene is contrary to the experience that such action takesplace only in presence of the tertiary group (CH). The authorthinks this is explained by the inter-molecular changes which haveoften been observed in cymene derivatives, a change resultirig in theconversion of normal propyl into isopropyl. This oxidation of themethyl group is similar to what takes place in the animal organism(Gerichten, Rer., 11, 369), and also to the oxidat’ion of chlorocymene(Claus and Wimmel, Ber., 13, 9@2), and dibromocymene.Cymenesulphonic acid when oxidised by nitric acid yields para-tolylsulphonic acid, C6H&fe(SO,H).COOH + 2H&, crystallising inneedles, which are not hygroscopic.The results from the study ofthe salts of this acid agree with those of Fischli (Ber., 12, 615), savethat the authors find the following formulze for the barium and leadsalts, viz., C8H6S05Ba + 4Hz0 and CsH&305Pb + 3+H20. The melt-ing point of the amide was found to be 218’.Oxidation of cinnamic acid by potassium permanganate yieldschiefly henzaldehy de and benzoic acid, whilst mandelic acid yieldsbenzoylformic acid, C6H5.C0.COOH. Hunaeus and Zincke (Bey., 10,1489) obtained the same result by oxidising mandelic acid with nitricacid. P. P. B.A Fourth Mononitrophenol. By F. FITTICA (Bey., 13, 711-715) .-Liquid mononitrophenol is best prepared by slowly droppingstrong sulphuric acid into a mixture of phenol, 10 grams ; alcohol, 10 ;ether, 10 ; and 8 grams of nitric acid (sp.gr. 1.4). As soon as theliquid begins to boil, it is poured into water. A current of air isblown through the layer of liquid floating on the water, in order toexpel the ether, and t,he heavy oil which separates out is well washedwith water and distilled in a current of steam. Ether first passesover, and then an oily liquid, the greater portion of which solidifiesafter being in contact with calcium chloride for some days. Thefraction which still remains liquid consists of a mixture of orthonitro-phenol and the new nitro-phenol. The orthonitrophenol is partly re-moved by distillation in steam; the portion which does not solidifyi y dissolved in dilute soda, and the sparingly soluble orthonitrophenolsalt separated from the new nitrophenate by crystallisation.ThORGANIC CHEMISTRY. 47fourth mononitrophenol is liquid at the ordinary temperature, but it,solidifies at 0" to a pale yellow crystalline mass (m. p. 34"). It yieldsan amidophenol crystallising in needles (m. p. 150°), which dissolvereadily in water. w. c. w.New Nitrophenols. By F. FITTICA (Ber., 13, 153.5-1538).-The boiling point of the fourth nitrophenol, already described by theauthor (preceding abstract), cannot be determined, as it is changed atthis temperature into orthonitrophenol. By reducing the compound ofnitrophenol and phmol (Zoc. &.) with tin and hydrochloric acid, orby reducing the fourih nit'rophenol under special conditions with tinand hydrochloric acid, a fourth amidophenol is obtained.I t crystal-lises from alcohol in needles (m. p. 151"). The hydrochloride ofthis amidophenol crystallises in greyish-white needles, which sublimeat 230" with partial decomposition. The sulphate is a white powder,consisting of small crystalline needles, soluble in water.A fifth nitrophenol is obtained by treating the tarry residue obtainedafter separation of orthonitrophenol from the para-compound withsoda, By this means a solid sodium salt is-obtained, which is pressedand treated with acid, and the oil obtained submitted to the action ofalkali and acid again. The oil obtained solidifies partially, and bycrystallisation from ether the new nitrophenol is obtained in yellowneedles (m.p. 105-106"). It yields an amidophenol, melting at150".In concluding, the author replies to the criticism of Claus (Ser.,13, 891) on the author's former communication (Zoc. cit.).P. P. B.Action of Bromine on Benzyl Cyanide and on PhenylaceticAcid at High Temperatures. By C. L. REIMER (Ber., 13, 742-748) .--DicyanostiZberbe, CN.PhC CPh.CN, is formed, together with asmall quantity of benzoic acid, when bromine is allowed to dropslowly into a flask containing benzyl cyanide at a temperatnre of 170".The product, after purification by washing with water, and solationin a mixture of alcohol and chloroform, is moistened with ether, andpressed between bibulous p p e r to remove resinous impurities. Thesolution of the residue in warm benzene deposits on cooling glisteningcrystalline plates (m.p. 1 5 8 O ) , which are soluble in chloroform, ben-zene, carbon bisulphide, glacial acetic acid, and in hot, alcohol.Dicyanostilbene is decomposed by alcoholic potash, with evolution ofammonia. If hvdrochloric acid is added to the solution after thealcohol has bein expelled by boiling, diphenylfurnaric anhydride,PhC : CPh/ \ is precipitated. This substance is deposited from alcohol oc . o . co'in pale yellow needles, and from carbon bisulphide in prisms. Itmelts at 155", and sublimes without decomposition. The free acidcorresponding to the anhydride cannot be isolated, but several of itssalts hare been prepared. The potassium salt forms colourless needles,which dissolve freely in water; the barium salt is crystalline, andsparingly soluble.Neutral silver diphenylf umarate, C16H,,Ag20a, i48 ABSTRACTS OF CHEMICAL PAPERS.amorphous ; the acid salt, C16H11Ag04, is crystalline. Both are verysparingly soluble.Bthyl diphenylfumarate crystallises in prisms (m. p. 54")) whichdissolve freely in chloroform and carbon bisulphide.By the action of ammonia on diphenylfumaric anhydride at 180",diphenylfunzarimide, C16H1002.NH2, is obtained in yellow needle-shapedcrystals, insoluble in water, but soluble in alcohol. This substancemelts a t 213", and sublimes without decomposition a t a higher tem-perature. On reduction with zinc and hydrochloric acid, dicyano-stil-bene yields a crystalline compound (m. p. 208"), having the composi-tion CI6H14N2.Diphenylfumaric anhydride and benzoic acid are also producedwhen the product of the action of bromine on phenylncetic acid a t230' is treat)ed with alcoholic potash. w.c. w.Action of Ethyl Chlorocarbonate on Phenols. By G. BENDER(Ber.? 13, 696--703).-The author has examined the products of theaction of ethyl chlorocarbonate on potassium salts of the differentphenols.Under these conditions quinol yields diethylic phenyldiox ycarbonate,C,H,(O.COOEt),. This compound is deposited from an alcoholicsolution in colourless needles (m. p. lolo), soluble in ether, but in-soluble in water.ResorcinoL-When ethyl chlorocarbonate acts on resorcinol, carbonicoxide escapes, and mono- and diethyl-resorcinol are formed.Catechol (pyrocatechin) gives a crystalline compound (m.p. 1 IS"),haying the composition C7Hi03, which yields diorthotolylcarbamidewhen boiled with orthotoluidine.From pyrogallol an ethyl salt having the composition c6H3 (O),iC.OEtis obtained. This substance melts a t 105", and distils between 250"and 280" with partial decomposition. It is deposited from an alcoholicsolution in pearly scales. Ortho-, meta-, and para-cresol yield threeliquid isomeric ethylic tolylcarbonates, CJ&.MeO.COOEt, which boilrespectively a t 236", 246") and 245".From orcinol, the compound C16H120a is obtained in yellow needles,which are sparingly soluble in alcohol, and melt with decompositionat 195".P-Napht7mZ yields a white amorphous mass, having the composition(CloH70)2C(OEt),.It boils at 298-301".a-NaphthoZ forms ethyl-naphthol carbonate, CloH70.COOEt, whichcrystallises in colourless rhombic plates (m. p. 31'). This body is de-composed by boiling ; alcohol distils over, carbonic anhydride escapes,and yellow needle-shaped crystals are deposited (m. p. 240°), of the w. c. IT.Methylenecaffeic and Methylenehomocaffeic Acids and theirBy C. LORENZ (Rer., 13, 756- 761).-Met7~ylenecaffeiccomposition ( CloH6)2C02.Derivatives.acid or ~ e t ~ y l e l z e d i o x ~ p h s n y l a c r y l i c acid,is prepared by boiling a mixture of piperonal, sodium acetate, andacetic anhydride for six hours in a flask fitted with an upright con-CH2 : 0 2 : C,HS.CH : CH.COOHORGANIC CHEMISTRY. 49denser. The aqueous solution of the product is extracted with ether,and the ethereal extract treated with soda.On the addition of hydro-chloric acid to the sodium salt, the methylenecaffeic acid (m. p. 232")is precipitated. It is insoluble in water, but dissolves freely inalcohol and ether. The copper, Iead, and zinc salts of this acid aresparingly soluble in water. On reduction with sodium amalgam, theacid takes up 2 atoms of hydrogen, forming methylenehydrocaffeic ormethylenedioxyphenylpropionic acid, CH, : 0, C6H3. (CH,),.COOH,which crystallises in colourless needles (m. p. 84"). The lead andzinc salts which form needle-shaped crystals, and the silver salt whichcrystallises in glistening scales, are sparingly soluble in water.Meth y leize-a- Izom,ocafeic or methyl e.l;r ed ioa~~henylmethacrlllic a cid,CH, : 0, : C,H3.CH CMe.COOH, obtained by the action of sodiumacetate and propionic anhydride on piperonal, is deposited from dilutealcohol in colourless prisms (m.p. 193"), soluble in alcohol and ether.The copper and lead salts of this acid are insoluble in water, the zincsalt is sparingly solnble.By the action of water and sodium amalgam, this acid is convertediilto m e t l ~ ? / l e n , e - a - h o n z o ~ ~ ~ a r ~ c ~ ~ ~ e ~ c or methylenedioxyphenylisobutyricacid, CHI? : 0, C6H3.CH2.CHMe.COOH, which crystallises in prisms(m. p. 77") of a yellow colour. It is soluble in alcohol and ether.Methylenecaff eic and methylene-a-homocaff eic acids occupy an inter-mediate position between piperonylic acid, C8H604, and hydropipericacid, Cl2HI2O4.w. c. w.Nitrometaxylenesulphonic Acid. By W. HARMSEN (Ber., 13,1558-1568) .-ParanitrometaxyZene, C6H$fe.Me.NO2 [ 1 . 3 . 41, is0btaine.d by nitrating metaxylene ; it is a liquid which boils at 243-244" (corr.), and remains liquid at - 2 O O . Its constitution was shownt o be the above by converting it into a xylidine, which yields Jacob-sen's metaxylenol, C6H3.Me.Me.0H [l . 3 . 41, by means of the diazo-reaction.Nitroxylenesulphonic acid, C6H,(Me),(NOz).S03H, was obtained byheating the above nitro-derivative with sulphuric acid and convertingthe product into calcium salt, which gave the free acid when decom-posed by sulphuric acid. It crystallises from water in small hygro-scopic needles, and from dilute nitric acid in long colourless needles(m.p. 1 2 2 O ) .The ctr1cizl.m salt, [C,H,Me,(NO,).SO,],Ca 4- 6H,O, c r y s t a l h a inslender pale-yellow prisms, having a vitreous lustre ; it effloresces onexposure to the air ; at 18.5" it dissolves in 16 parts of water.The magnesium salt, [ C6H2Me2(N02).S03],Mg + 9H20, formsoctaq-onal plates, which are sparingly soluble in water.The sodium salt, CGH2Mez(NO2) .S03Na + H,O, crystallises inshining needles.The same acid is obtahed by nitrating a-metaxylene sulphonic acid?the constitution of which is C6H3Me.Me.S03H [l . 3 . 41 ; thereforethe constitution of the nitrometaxylenesulphonic acid is-C6H3.Me.Me.So3H.NO2. [l . 3 . 4. 61. P. P. B.VOL. XL. 50 ABSTRACTS OF CHEMICAL PAPERS.cdsophthalosulphonic Acid.By 0. JACOBSEE and H. L~SNIES(Bey., 13, 1556-1 558) .-When sodium a-metasylenesulphonateis oxidised by potassium permanganate and the manganese dioxideremoved by treatment with hydrochloric acid it yields an acid potas-sium a-isophth,alosuZphonate, C6H3( COO),( S03)H2K + 2H20. It crys-tallises in colourless brittle needles, having a vitreous lustre, and issparingly soluble in cold water.a- I s o ~ ~ h ~ t h a Z o s u ~ h o n i c acid, C6H3(COOH)2.S0,H + H20, is obtainedby decomposing the insoluble lead salt with snlphuretted hydrogen ; itcrystallises in colourless flat needles. It resembles the 7- isophthalo-sulphonic acid (Ber., 13, 704), and is more easily crystallised from sul-phuric acid than from water. Fused with potash, it yields a-hydroxy-isophthalic acid.It melts between 235-240", and is more easilysoluble in water than the anhydrosulphonamine-isophthalic acid.Barium iso~htl~nZosu.~horLnte, C6H3( COO)z(SO,)HBa + 3H,O, is ob-tained as a white crystalline precipitate by adding barium chloride tothe solution of the free acid or its acid potassium salt. Bariumchloride produces a precipitate only after some time in a solution ofthe acid in ammonia ; under the same conditions sulpf~onamineiso-phthalic acid gives a precipitate also, the anhydro-acid does not, how-ever, give a precipitate with barium chloride.Isophthalosulphonic and anhydrosulphonamine-iscphthalic acids be-have differeiitIy with silver nitrat'e. In the case of the former, neitherthe free .acid nor its potassium salt gives a precipitate with silvernitrate, whilst the latter, either as free acid or potassium salt, gives avoluminous precipitate, which becomes crystalline on standing.el- Isophthalosulphonic Acid and 7-Hydroxyisophthalic Acid.By H.LONNIES (Ber., €3, 703-707).-y-lsophthalosulplionic acid,C6H3(SOJH)(COOH)2 [I : 3 : 51, is prepared by heating isophthnlicacid with fuming sulphuric acid a t 200" for six hours. The liquid isthen diluted with twice its volume of water which precipitates theunaltered isophthalic acid : the sulphonic acid is deposited as a crys-talline mass on cooling. The sulphonic acid is deposited from dilutesulphuric acid in colourless prisms containing 2 niols. H,O. Thecrystals are deliquescent a t the ordinary temperature, but begin toeffloresce a t 60".The anhydrous acid melts a t 257" with decomposi-tion.The barium salt, [C,H,(SO,) (C00)2]2Ba3 + 8H20, crystallking insilky needles, and the calcium salt crystallking in transparent prisms,are freely soluble in water. A solution of the sodium salt yieldsprecipitates with mercuric nitrate, ferric chloride, copper acetate, andlead acetate.The preparation and properties of yhydroxyisophthalic acid havebeen described by Heine (Ber., 13,491). The anhydrous acid nielts a t288", and requires 3,280 times its weight of water at 5" for completesolution. A solution of the potassium salt is precipitated by ferricchloride, barium chloride, copper sulphate, silver nitrate, and leadacetate. Zinc sulphate does not, yield an immediate precipitate, butafter some time small prismatic crystals are deposited which areP.P. B.sparingly soluble in water. w. c. wORGANIC CHEMISTRY. 51Anhydrosulphonamine-isophthalic Acid. By 0. JACOB SE N(Ber., 13, 1554--1555).-A further examination of the body formedby the oxidation of sulphonamine-metatoluic acid, has confirmed theviews of Remsen (this Journal, 38, 258), viz., tl& anhydrosulphon-amine-isophthalic acid is obtained.Amarine and Lophine. By E. FISCHER and H. TROSCHKE (Ber.,13, 706-711) .-Amarine dichromate, ( C21H18Nz)2H2Cr207, is throwndown as a yellow precipibate when chromic acid is added to a solutionof amarine in dilute acetic acid. The solution of this salt in glacialacetic acid is converted into Zophhze by boiling.A solution of lophinein glacial acetic acid is oxidised by chromic acid a t 100" with theformation of benzamide and dibenzamide.Lophine dissolves in strong sulphuric acid at 170", forming a disul-phonic acid, which is sparingly soluble in water and alcohol. It isnot attacked by strong hydrochloric acid, but is reduced to lophine bysodium-amalgam.The mono-sodium salt, Cz,H14N2( S03)2X'aH + 2Hz0, crystallises inwhite needles, sparingly soluble in alcohol and in water.An unstable crystalline compound, C21H16N2Br6.HBr, is produced bythe action of bromine on lophine hydrobromide.The authors believe that amarine and lophine contain the group>C.C6€€,. The formula for lophine, C2,HI6N2, was con-P. P. B.C6H5-C. NCcH5--6.NIfirmed by the vaponr-density determination. w. c. w.Indoline. By E. GIRAUD (Compt. reml., 90, 1429-1430 j .-Flavindin dissolved in dilute soda is treated with sodium-amalgam(3 per cent.), when a dirty yellow powder is precipitated; this iswashed, dissolved in alcohol, and the solution diluted with water,when the indoline is precipitated, and may be purified by sublimation.It is probably formed according to the equation, C32H,*N*05 + 14H =2(C16H14N,) + 5H20. It gives the same reaction with picric acid asthe indoline described by Schiitzenberger. When dissolved in chloro-form and treated with chlorine, it yields a chlorinated derivative,C,,H,,N,CI,. An orange-yellow dinitro-compound, C16H12N2(N02)2, isobtained by treating indoline with nitric acid ; it is soluble in alcohol,but insoluble in water.By treating indoline with fuming sulphuricacid a t 180°, and saturating the product with sodium carbonate,CiGHJJ,( S03Na)2 is obtained.Derivatives of Anthraquinonesulphonic Acid. By D. A.MCHUUL (Ber., 13, 692-694). - A~thrapuinonesul2r,honic chloride,ClaH,O2.SO2C1, is prepared by heating equivalent quantities of an-thraquinonesulphonic acid and phosphorus pentachloride at 180" forfour hours. The residue which remains after the phosphorus oxychlo-ride is distilled off is extracted with hot water and recrystallised fromboiling benzene. The chloride crystallises in pale-yellow plates(m. p. 193") which dissolve in benzene, toluene, and glacial aceticacid. By the action of water at 160°, it is converted into anthra-quinonesulphonic acid.L.T. 0's.e 52 ABSTRACTS OF CHEMICAL PAPERS.Anthrapuinonesulphaamide, ClaH7O2. S02NH2, formed by heating thesulphonic chloride with alcoholic ammonia at 140", is deposited froma solution in glacial acetic acid in long yellow crystals (m. p. 2 6 1 O )which are insoluble in alcohol, toluene, chloroform, and carbon bisul-phide.,4nthraquinonesuZphaniZide, C14H702.NHPh, obtained by heating thesulphonic chloride with a solution of aniline in toluene at 180", formslong brown prisms (m. p. 1 9 3 O ) soluble in alcohol and glacial aceticacid.AnthraqzLinonedimethyZarnidoplienylsulphone, CI4H,O,.SO.,C,H4.NMez(m. p. 17l0), is obtained by the process described by Michler andSalathe (Ber., 12, 1789 ; this Journal, 38, 108) for preparinga-~a~~htl~yldimethyZamidopkeiiyZ~.ulpphone.The reduction of the sulphonic chloride by sodium-amalgam yieldssodium anthracenesulphonate, sodium anthracenehydridesulphonate, w.c. w.Gum Resin from Arizona and California. By J. M. STILL-NANN (Ber., 13, 754--756).-The resinous substance found on thetwigs of the Larrea ilfexicana and Acacia gyeggii in Arizona andCalifornia, appears to be identical with Indian shellac. I t is composedof resin, &c., soluble in alcohol, 61.7; colouring matter soluble inwater, 1.4 ; soluble in soda, 26.3 ; insoluble residue, 6.0 ; colouring w. c. w.and a small quantity of anthraquinone.matter soluble in soda and loss, 4.6 per cent.A Substance Extracted from Thalictrum Macrocarpum.ByM. HANRIOT and E. DOASSANS (BuJZ. Xoc. Chiin. [2], 34, 83-84).-In a former communication the authors described a yellow crystallinesubstance from the Thalictrum macrocarpurn, which was named bythem "thalictrin." They propose t o change the name to macro-carpin. In order to obtain this substance, the roots of the thalictrumare exhausted with alcohol, the excess of which is distilled off in avacuum ; it is then purified from a resin by ether, and finally precipi-tated with distilled water. Macrocarpin is a yellow substance, crys-tallising in needles, soluble in water and alcohol, but insoluble inether ; its best solvent is amyl alcohol. It is neutral, precipitated byacids, but soluble in ammonia. The analyses gave : C = 58-25 ; H =5.67 ; 0 = 86.08.Owing to the small quantity at the authors' disposal,they were unable to study the products of decomposition and assigna formula. V. H. V.Thalictrine. By E. DOASSANS (BUZZ. Xoc. Chim. [el, 34, 84).-By exhausting crude macrocarpin with ether, an alkaloid, thalictrine,is obtained ; a colourless crysialline substance, insoluble in cold andwarm water, soluble in ether and in alcohol. With hydrogen nitrate,it gives crystals of thalictrine nitrate. In its properties and reac-tions it resembles most nearly aconitine.Catechin. By C. LIEBERMANN and TAUCHERT (Ber., 13, 694-696).The catechin used in these experiments was prepared from catechu byLoewe's process (Zeits. Anal. Chem., 1874, 113), but it was recrystal-V. H. VORGANlC CHEMISTRY.53lised twice from hot water before it was treated with ethyl acetate.It is deposited from an aqueous solution in minute needie-shapedcrystal!, having the composition C2,H,0g + 5H20. Dincetic cntechin,C21H1SAc209, obt'ained by the action of acetic anhydride and sodiumacetate on catechin, crystallises in yellow needles and prisms (m. p.130°), which are insoluble in water and ligroin, but dissolve freely inother solvents.Dichloracetic catechin, C21H16C12&09 (m. p. 16!1°), is prepared bypassing chlorine through a concentrated solution of diacetic catechinin glacial acet,ic acid: the substance is precipitated on the additionof water. Muizobromncetiecatechin, Cz1H,,BrAc2Og, is deposited from an alcoholic solution inwhite needles (m.p. 120").The existence of these compounds shows that catechin has the corn-It is sol-uble in alcohol and ethyl acetate.position C21H200,. W. c. w.Alkannin. By G. CARNELUTTI and R. NASINI (Bey., 13,1514-1516) .-This body was obtained by extracting commercial colouringmatter with dilute potash solution ; this extract mas shaken with etherto remove a reddish-brown acid, an impurity present in the alkanninobtained by Pelletier, Bolley, and Weydler. The solution in potashwhen saturated with carbonic anhydride gives a precipitate of alkan-nin, which was further purified by solution in ether. It is obtainedas a dark reddish-brown mass, with metallic lustre, and is sparinglysoluble in the ordinary solvents ; it is most easily soluble in chloro-form and glacial acetic acid.Its alcoholic solution is not changed byexposure to light or by continued boiling. The analytical results showits formula to be C15Hld04, whilst Pelletier obtained Cl,Hlo04, andBolley and Weydler C,,H,O8 from their analyses.Acetic and benzoic-chlorides have no action on alkannin ; a diacetylderivative, Cl,Hl,04Ac2, is obtained by heating it with acetic anhy-dride and sodium acetate: it is a brown powder which crystallisesfrom glacial acetic acid in dirty yellow crystalline grains.A barium salt containing 2 atoms of barium t,o 3 molecules ofalkannin is obtained by precipitating the alcoholic solution withammonincal barium chloride.Nitric acid or bromine in alkaline solution oxidises alkannin tooxalic and succinic acids. Bromine acts on solid alkannin, but noton its solutions.Alkannin appears to be related to santalin.P. P. B.Derivatives of Santonin. By S. CANNIZZARO and J. CARNELUTTI(Bey., 13,1516 -1517).-By the fusion of santonous and isosantonousacids with barium hydrate (Bey., 12, 15i4) the authors obtained abody having the formula C12Hc,20. Since this body when distilledwith zinc-dust yields a hydrocarbon, C12H12, whose physical properties,and the properties of its picric acid compound, and of its tribromo-derivative, show it to be dimethylnaphthalene, the authors conclude thatthe compound C12H120 is dimethylnaphthol. The dimethylnaphthalenecontains the methyl groups in the same relative position that the bro-mine atoms occupy in Glaser's dibrornonaphthelene (m.p. 80.5 -81")54 ABSTRACTS OF CHEMICAL PAPERS.Santonous acid distilled over zinc-dust yields some dimethyl-A small quan-P. P. B.naphthol, also dimethylnaphthalene and propylene.tits of xylene appears to be formed.Cyanethine, and New Bases derived from it. By E. V. MEYER(J. pr. Chem. [el, 22,261-288).-Cyanethine was discovered 33 yearsago by Kolbe and Frankland (Annden, 65, 'LG9), and its homologuecyanmethine has been since described by Bayer (this Journal, 1871,Cyanethine is prepared by acting on tolerably large pieces of cleansodium with ethyl cyanide in a retort provided with an upright con-denser, the upper end of which is air-tight, and has a bent glasstube fitted to it which dips into mercury.The apparatus is filledwith carbonic anhydride ; one-third of the ethyl cyanide is added atfirst, and the rest gradually as the reaction becomes less violent. Theexcess of cyanide is removed by distillation, and the yellow-colouredproduct powdered and washed with water. It is then dried on porousplates and crystallised from alcohol (of 90 per cent.). The chief pro-cesses of the reaction are shown by the following equations :-397).Na + C,H,CN = NaCN + CzH5Na + C,EI,CN = C,H,NnCN + HCZH, + H = C2HG.Cyanethine melts at 189". One part dissolves in 1,365 to 1,380 partsof water at 17", but it is tolerably soluble in alcohol.* A concentrated solution of cyanethine in hydrochloric acid crystal-lises in large transparent striated prisms, which, when dried overquicklime and sulphnric acid, contain about 1 mol.of water. Thesecrystals dried at 110", have the composition C9H,,N3.HC1.Cyanethine forms a double salt, (C9H15N3)2.AgN03, with silvernitrate. It is also shown by the action of ethyl iodide to belong tothe tertiary bases. Nitrous acid has no marked action on it, but it isoxidised by permanganate with formation of formic acid as the chiefproduct; carbonic anhydride is evolved at the same time, while anammonium salt is found in the solution together with a second acid,probably propionic.When c-j-anethine is heated with tolerably concentrated mineralacid, it yields a monncid base containing oxygen, CgH140N2. Thisbase crystallises from hot water in fine tufts of brilliant needles: fromalcohol in long striated prisms ; when precipitated by ammonia fromone of its salts, it forms intricate, sometimes dendritic, aaicular masses ;carefully heated, it sublimes in small needles far below its meltingpoint, which lies between 156" and 157".One part of this base re-quires 133 parts of water for solution, but it does not impart anyalkaline reaction to the water. It is most soluble in chloroform andbenzene. The salts are soluble in water, to which they give an acidreaction, and for the most part crystallise well.The hydrochloride, C9H,,0N2.HC1, is obtained by evaporation of thehydrochloric acid solution and drying at 110" as a white flocculentcrystalline powder, small quantities of which sublime in minute prismsORGAXIC CHEDIISTRY.55The pZatknoc7~Zoride, (C,HlrON2.HC1)z.PtClr, forms yellow rhombicplates which dissolve easily in water, but sparingly in alcohol.The nitrate, CgHIION2.HN03, cry stallises in fine (probably mono-clinic) prisms which undergo decomposition a t 1 0 0 O . The acid oxalate,CgHl4ONz,CZO4Hz, is anhydrous.The body which has act'ed as a base in the above salts can alsoexchange an atom of hydrogen for one of silver. The siher salt,C,H,,AgON,, is precipitated as a white, bulky, microscopic crystallinepowder which is readily soluble in ammonia and in dilute nitric acid.Similar compounds could not, however, be obtained with copper, lead,&c. The ready solubility of the base, C9€1140N2, in alkalis, seems t oindicate that it forms compounds with them, but it is separated fromthem again by carbonic anhydride. The reaction with ethyl iodideshows that it belongs to the tertiary bases.It unites with aceticchloride t o form the compound CgHl,ONz.CH,COC1. As this base is notaltered by heating with acetic anhydride at 180", the oxygen wouldseem to be united with hydrogen as hydroxyl. Heating with excessof hydriodic acid a t 200" decomposes a small part of the base withformation of ammonia and probably propionic acid.Potassium permanganate in acid solution oxidises it, the nitrogenbeing evolved in the form of ammonia ; in alkaline solutions propionicacid (and probably a little acetic acid) is also formed. When treatedwith phosphorus pentachloride, a new base is produced of the formulaC9H,,C1N2.This base is a bright yellow oil with an unpleasant odour,and cannot be distilled a t the ordinary pressure without decomposi-tion. I t is insoluble in water. On heati=g with ammonia and alcohol, *cyanethine is re-formed, which shows that cyanethine contains a mole-cule of amidogen. When alcoholic potash acts on the compoundCgH,,C1N2 a new base, CgH13(OEt)N2, is formed ; it is a faintly-colouredoil with a cabbage-like smell. It can be distilled without change at269" to 231". Strong hydrochloric acid converts it into the baseCgH140N2 or C9Hl,(OH)N,. When the base C9HI4C1N2 is acted on byzinc and hydrochloric acid a double zinc salt, ( CgHl~Nz.HC1),.ZnCl2, isformed, but it is not improbable that this salt contains also ananalogous base, C9H16Nz.On continued agitation, the base, C9H14Nz, dissolves in water in con-siderable quantities, and imparts to it an alkaline reaction ; when thesolution is heated, the base separates in oily drops.It is a clear liquidwith high refractive power and an unpleasant narcotic smell ; whenthe rapour is inhaled, it produces a heavy feeling in the head, so thatgreat care is necessary in working with it. It boils at 204--205", andis easily volatilised in steam. It does not reduce Pehling's solution ;an ammoniacal solution of a silver salt is only reduced on continuedheating. Powerful oxidising agents such as chromic acid, &c., actenergetically on it. Crystalline salts of the base have not been ob-tained. The above properties of the base strongly resemble those ofconine, and its physiological action is similar, but more violent thanthat of conine.It may perhaps be cyanoconine for C,H14(CN)N =CgHI4N,. If this is the case, the bases described in the paper may beexpressed as follows :56 ABSTRACTS OF CHEMICAL PAPER§.CgH,Nz = CsH14( CN)N, cyanoconine.CgHIaClNz = C,H&l (CN) N, chlorocyanoconine.C9HdOH)N2 = CsHI3( OH) (CN)N, oxycyanoconine.CgH13(0C2H5)N2 = C,Hl,(OCzH5) (CN)N, oxyethylcyanoconine.C9H13(NH,)N2 = C8Hu(NHz) (CN)N, amidocyanoconine =cyanethine. G. T. A.Bases of the Pyridine Series. By 0. DE CONINCK (Compt. rend.,91, 296--297).-The bases of this series formed in the distillation ofcinchonine with potash have been separated and purified by theauthor. They are isomeric with the bases of the same name found incoal-tar napht,ha, and in Dippel's oil. After separating them as faras possible by fractional distillation, the different fractions are treatedwith excess of hydrochloric acid, agitated two or three t,imes withether, the ether separated, and excess of potash solution added.Theseparated bases are taken up by ether; the ethereal solution dried overpotash and distilled.Lutidine, C7HgN, is a colourless, mobile, strongly refracting liquid,with peculiar odour and burning taste. It is very hygroscopic, andalmost insoluble in water. Boiling point, 155" ; vapour-density, 3.8(found) ; 3.71 (calculated) ; sp. gr. at O", 0.9593.Lutiiiine hydnxhloride, C7HgN.HC1, forms white, deliquescent,lamellar crystals.The hydrobromide is similar. The plntinochloridecrystallises in fine orange-red needles ; treated with boiling water, itloses 2 mols. HCI, and crystallises in yellow needles. The auro-chloride is a shining yellow powder.Collidiite, C8Hl1N, boils a t 195", and is similar in appearance andVapour-density, 4.25 (found) ; 4.19 (calcu-Lted) ; sp. gr., 0.9656 at 0". The platinochloride is an orange-redpowder, transformed by boiling water into minute yellow needles.Parvolzne has not yet been obtained quite pure; it boils at about220".roperties to lutidine.The platinochloride forms a, brownish-yellow powder.Lutidine from Dippel's oil is of sp. gr. 0.946 i;nd b. p. 155.5".Collidine 9 7 9 ) ,, 0.944 180.Parvoline 9 ) 9, 7 9 bo& at 188.J.M. H. M.Crystalline Quinoidine Borate. By J. JOBST (Ber., 750-751).-The substance described by Pavesi (Za Farmncia, 1879, 26) as aquinoidine borate is merely a mixture of boric acid and qninoidine,from which the base is completely removed by recrystallisation. w. c. w.Hyoscine. By A. LADENBTJRG (Ber., 13, 1549--1554).-1n aformer communication (Ber., 13,910), the author stated, that an alka-lo'id accompanies hyoscyamine, which is known as " amorphoushyoscyamine." To this the author gives the name hyoscine ; it is ob-tained in commerce as a syrup, from which, by conversion into theaurochloride and recrystallisation of the latter, it may be obtained ina tolerably pure state. When the hyoscine obtained from the auro-chloride is decomposed by barytn, it yields tropic acid and a baseisomeric with tropine, which is styled pseudotropineORGANIC CHEMISTRY, 57Pseudotropine forms a white crystalline mass ; it boils at 241-243"(tropine boils a t 229').Its platilzochZoride ( C,H,,NOHC1),.PtjCl4, hasbeen obtained in well-defined crystals, belonging to the rhombicsystem, a complete description of which is given. The auwrhlnride,CsH,NO.HCl.AuC1,, has a solubility similar to that of tropineaurochloride ; the appearance of the crystals is, however, different.The picrate and double salt with meycuric chloride have been obtained inwell- defined crystals.The aurochloride of hyoscyine may be obtained pure by first boilinghyoscyine hydrochloride with animal charcoal. The aurochlorideprepared from the hydrochloride so purified crystallises well, and meltsat 198".The reactions of hyoscyine are similar to those of hyoscyamine.Potassio-mercuric iodide gives a light yellow amorphous precipitate,with acid solution of hyoscyine, and mercuric chloride, an amorphousprecipitate ; in some cases an oil is obtained.Iodine solution gives ablack oily periodide, and potassium ferrocyanide a white amorphousprecipitate.The physiological action of hyoscyine resembles that of atropine.Atropine, hyoscyamine, and hyoscyine are isomerides, whi 1st homa-fropine is a homologne containing CH, less than these alkaloids.Ptomaines considered in Relation to Judicial Chemistryand Toxicology. By T. HUSENANN (Arch. Pharm. [3], 16, 169-181).-The name "ptomaines" has been given by Selmi to bodieswhich have been detected in exhumed corpses, and resemble the vege-table alkalo'ids in their chemical reactions and physiological effects.The author gives a summary of the observations already published onthis class of bodies, and considers the very important bearing they haveon the study of poisons and on forensic medicine.It becomes ex-tremely important to discover, if possible, reactions which will distin-guish between these poisonoiis bodies, which are the result of putre-factive processes, and those very similar vegetable principles which,when administered, may produce death. Bodies of the " ptomaine "class seem to have different physiological actions. Some appear toact as poisons, others are inactive : whilst others again counteract theeffects of poisonous substances.The study of these bodies embraces also the poisonous effects pro-duced by food in certain conditions of putrefaction or ferruentation.Panum showed that albuminous substances by putrefaction yielded apoisonous body, acting like a ferment, soluble in water, insoluble inalcohol, and capable of withstanding a temperature of 100".This hasbeen confirmed by Bergmann, who describes a compound calledsepsin, generated by putrefaction.It appears from the researcbes of Panum and of Schweninger, thatcompounds having different physiological actions are produced a t dif-ferent stages of decay.Sonnenschein and Zuelzer found in an anatomical maceration fluidan alkaloid which resembled atropine in its action, and poisonoussausages produced a similar effect; the existerice of a product ofdecay which caused tetanic symptoms was also noticed.Aebi andP. P. B58 ABSTRACTS OF CHEBIICAL PBPERS.Schwazenbach detected a compound allied to an ethereal salt inextract from dead bodies. Substances derived from putrefaction ofmaize certainly produce tetanic symptoms, as was first proved byLombroso and Erba ; and this action has been traced to the presenceof basic substances. It appears probable, however, that drowsiness,loss of sensation, and. weakening of the action of the heart may bedue to the presence of acid bodies in the extract of putrefied maize,since lactic acid and sodium lactate produce effects similar to those ofmorphine.Lombroso thinks that the tetanic and narcotic action ofextract of putrefied maize, and its beneficial effect on several skinaffections, indicate the possible origin of pellagra in diseased or putridmaize. This mould explain the prevalence of pellagra in the SouthEuropean maize-growing countries, and in other countries it mayoriginat'e from the putrefaction of albumino'id * substances of othercereals. This kind of putrefaction cannot be caused by artificial heat,aIthough it occurs only in hot summer weather, and probably thereforerequires the presence of special microscopic organisms. A similar ex-planation may be applied to tetanic symptoms caused by wounds andprevented by the Lister treatment. Frequently the tetanising principlein the maize extract has its action marked by it narcotic substance ;just as Ranke showed that the physiological action of strychnine inbodies long buried may be masked by ptomaines.Lombroso's siiggestion that skin complaints may be due to putre-factive products of maize has its known analogues in erysipelas causedby wound poisoning, and in skin eruptions caused by eating bad fishand other putrefying substances.Such poisonous effects ape: however,often produced by parts of living organisms, as for instance by thebeard of the mussel; and they are not produced on all individuals,since dogs accustomed to eat decomposing substances are not affectedby putrefactive principles.The relation of these products of putrefaction to certain diseases isevident from tbe fact, that Sonnenschein's alkalo'id is found in thebodies of patients dying from typhus fever, a.nd many individualspoisoned by decomposing food show marked typhus symptoms.I n many cases of poisoning by cheese, it was found that the badeffect was not due to vegetable growths or to microscopic organisms5and the clieese was frequently fresh.It appears from the study of the literature concerning ptoma'ines,that they are usually produced in bodies which, after brief exposure,have been excluded from air, as in buried bodies, sausages, and tinnedfoods; and further, in these cases, the production chiefly occurs in theinternal portions. Cases, however, are known where similar principleshave been present in comparatively fresh substances which have beenconstantly exposed to the air : hence under the name " ptomaines "must be included all alkalojidal products of decay, whether formed inPapain. By A. WURTZ (Covnpt. rend., 90,1379--1385).-The sapof the Carica papaya contains a soluble ferment, which the author andRouchut have described (this Journal, 1879, Abst., 1048). The fer-ment is obtained by making incisions in the bark of the tree and in thethe presence or absence of air. F. cVEGETABLE PHYSIOLOGY AND AGRICULTURE. 59unripe fruit, when a milky sap exudes, which coagulates on exposureto the air. By expressing the liquid from the coagnlum, and addingalcohol to it, a precipitate of papain is obtained. Papain is also ob-tained from the coagulum by triturating it with water several times,concentrating the solutions, and adding alcohol. Prepared in this wayit differs slightly in composition from that obtained from the liquidportion of the sap. Papain of another composition is also obtainedby mixing the sap obtained from the fruit with water to form apulp, filtering, concentrating the solution, and adding alcohol. Bywashing the residue and concentrating the filtrate, a further quantityof papain is obtained. It appears, therefore, that the solubleferment of Carica papaya is not of constant composition. All thepreparations contain from 4 to 10 per cent. of ash, whilst afterdeducting the ash the percentage of carbon varies from 46 to 53, andthat of nitrogen from 14 to 18 ; it also contains about 2.2 per cent. ofsulphur. Those preparations giving the greatest percentage of carbonwere obtained either by dialping the precipitate obtained withalcohol, or by precipitating adhering albumin, &c., with subacetate oflead, and separating the excess of lead with sulphuretted hydrogen,and precipitating the papain with alcohol. The ferment thus obtainedacts energetically on fibrin, and its composition resembles that of thealbuminoids. It is very soluble in water, dissolving in less than itsown weight like gum. The solution when boiled or allowed t o standfor some time becomes turbid, but the papain does not coagulate likealbumin. Hydrochloric and nitric acids precipitate papain, but theprecipitates are soluble in excess. Orthophosphoric and acetic acidsdo not give precipitates with papain, but with metaphosphoric acid aprecipitate is formed. Subacetate of lead produces st turbidity inpapain solutions; on adding potash and boiling, it becomes black.Millon’s reagent gives a yellowish-white precipitate, which on boilingbecomes brick-red. Papain does not act so energetically on fibrineas the t r y p i n e of Kiihne.The author has also obtained a saponifiable fat, and a nitrogenousbody from the juice of the Ca~icapapnya. L. T. 0’s

ISSN:0368-1769    

DOI:10.1039/CA8814000032

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

VEGETABLE PHYSIOLOGY AND AGRICULTURE. 59Chemistry of Vegetable Physiology and Agriculture.Artificial Generation of Spleen-Fungus. By H. BUCHNER(Ried. Cewtr,, 1880, 594--598).-The fungus which causes inflam-mation of the spleen in animals can be slowly transformed into haybacteria by contiuuous cultivation in a solution of extract of meat forsome mont,hs, and the comerse of this change of form may be effectedby the growth of hay bacteria in blood,The Function of Fat in Germination. By A. LADUREAU (Bied.Centr., 1880, 628).-When seeds are brought in contact with water,J. I(. C60 ABSTRACTS OF CHEMICAL PAPERS.decomposition and acidification of the contained fatty matter is pro-duced, whereby heat is evolved and germination is hastened.J. K. C.Growth of Sprouts on Potatoes.By K. KRAES (Bied. Cerh-.,1880, 602--606).-The sprouts on potatoes flourish in proportion totheir nearness to the apex of the tuber. Treatment with water insunlight iocreases the growth forty or fifty times, although this is notthe case in the dark. For the growth of the young tubers, absence oflight is necessary. J. K. C.Vegetation of Oil-producing Plants. By MAQUENNE (Bied.Centr., 1880, 630).-The formation of highly-reduced oils is notaccompanied by a loss of oxygen in the whole plant. In all oil-pro-ducing plants there exists an easily oxidisable substance, similar in itsproperties to tannin. J. K. C.Distribution of Sugar in Sorghum. By P. MEUNIER (Bied.Centr., 1880, 629) .-The amount of cane-sugar gradually decreasesfrom the lowest part t o the summit of the cane, whilst the middle isrichest in glucose.Pressure in Plant-stems.By J. BOHM (Bied. Centr., 1880,629).-This pressure the author attributes to the evolution of gases inthe stem, and not to osmotic forces.J. K. C.J. I(. C.Successful Growth of Flax in Saxony. By OEHME andothers (Bied. Centr., 1880, 598--60G).-In the case of one field, aprofit of 80 per cent. was obtained on the total outlay connected withthe culture and cleaning of the flax.Cultivation of Beet. By E. WOLLNY (Bied. Centr., 1880, 606-613).-The author shows that a certain amount of room, varying withthe sort of plant, is necessary to obtain the maximum yield. With regardto ridging of the plants, transplanting, &c., the author's results agreewith those of former investigators.J.K. C.J. K. C.Experiments with Various Kinds of Beet. By C. BRTER andL. JEHLE (Bied. Cenntr., 1880, 624-626) .-Further experiments arenecessary to determine which of the 13 kinds of beet under investiga,-tion are best for the soil where the experiments were carried out', asthe results were very irregular.Cultivation of Beetroot. By A. PAGNOUL ( B i d Centr., 1880,629) .-These researches are merely of local interest.J. K. C.J. K. C.Influence of Trenching on the Temperature and Moistureof Soil. By E. WOLLNY (Bied. Centr., 1880, 563--567).-Experi-ments with five different kinds of soil showed that the temperaturewas raised in the day and lowered a t night by trenching the earth,the mean temperature being, however, greater than on level soil.Theamount of moisture was less in the trenches than on the flat. ThesVEGETABLE PIISSJOLOGY AND AGRICULTURE. 6 1observations are explained by the fact that there is a greater sur-face exposed in the trenches, and consequently radiat,ion is greater atnight: also, that the sun’s rays fall more perpendicularly on parts ofthe trenches than on level ground. J. K. C.Descent of Rain-water down Tree Stems. By W. RIEGLER(Ried. Centr., 1880, 561-563) .-The quantity of rain-water whichtrickles down the trunks of trees to the earth varies with the upwardor downward extension of the branches and the force of the rainfall.In the case of firs, it is much less than in beech and oak.J.K. C.Worthlessness of Phosphates as Manure for Certain Soils.By P. P. DEHORAIN and MEYER (Bied. Centr., 1890, 567--570).--Inthe case of a field at Grignon, phosphate, when used as manure,wsts found to produce no effect, although the soil was not rich inphosphates. J. K. C.Curacao Guano. By F. HUL~-A (Bied. Centr., 1880, 626-627).-This gmno is of very uniform quality, containing about 88 per cent. ofcalcium triphosphate, and is easily soluble in acid. J. I(. C.Manuring Experiments on Arable Land. By A. SCHUMACHER(Bied. Cent?.., 1880, 580-5859 .-The manure used was superphos-phate and Chili saltpetre. The results were, however, not successful,as the quantity employed was insufficient. J. K. C.Manuring Experiments with Mangold Wurzel and Beet.By H. POGGE-ROGGOW (Bied. CeuLtr., 1880, 572-575).-The mangoldswere manured with Chili saltpetre and superphosphate, which inevery case more than paid f o r itself, whereas the 24 experimentswith beet were all, with one exception, unsuccessful in a pecuniarypoint of view.Analysis of Pond Slime. By HOLDEFLEISS (Bied. Centr., 1880,627).-The percentage of nitrogen varied from 0.78 to 0.07; ofphosphoric acid, 0.15 to 0.02; of potash, from 0.15 t o 0.10; and oflime, from 0.75 to 0.26 in the upper and lower layers of slime.J. K. C.J. K. C.Best Method of Manuring Potatoes.. By PXTOW-LALEBDORF(Bied. Centr., 1880, 575--577).-The most successful method seems tobe to partially dig the manure into the soil.Manuring of Beetroot. By A. DUDOUY ( B i d Centr., 1880,570-571) .-The author concludes from his experiments that potashhas an injurious action on the amount of sugar in the root; thisinference, however, can hardly be considered as established by the re-sults obtained. J. K. C.J. K. C

ISSN:0368-1769    

DOI:10.1039/CA8814000059

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

62 ABSTRACTS OF CHF,MICAL PAPERS. A n a1 y t i c a 1 C h e m i s t r y. Apparatus for the Volumetric Estimation of Nitrogen. By H. SCHWARZ (Ber., 13, 7’71--773).-This is a convenient moclification of Zulkowsky’s apparatus for collecting the nitrogen evolved in organic analyses of nitrogenous compounds by Dumas’s method. w. c. w. Action of Organic Acids on Minerals. By H. C. BOLTON (Bey., 13, 726--734).-l’The author points out that a large number of minerals are decomposed, either by a hot concentrated solution of citric acid, or by the combined action of citric acid and sodium nitrate, potassium iodide or ammonium fluoride, and he suggests that this acid would, on account of its safe portability, prove a valuable reagent during mineralogical excursions. Tables are given of this reaction with a large number of minerals.w. c. w. Estimation of Retrograde Phosphoric Acid. By A. GRUPE and others (Bied. Centr., 1880, 582--584).-The solvent action of ammonium citrate is greater a t 35” C. than at the ordinary tempera- ture, and in using this as a reagent for the estimation of retrograde phosphate, care must be taken to first remove by washing soluble salts of magnesia, which have the effect of rendering bicalcium phosphate insoluble in ammonium citrate ; the presence of calcium carbonate also has the same effect. J. K. C. Retrograde Phosphoric Acid. By M. A. MILLOT (Biecl. Centr., 1880, 577--580).-The author finds that when mineral superphos- phates contain a considerable quantity of ferric oxide, a part of the phosphoric acid combines with the iron, forming a compound insoluble in ammonium citrate, even when a sufficient quantity of sui- phuric acid has been used in the decomposition of the phosphate.Calcium monophosphate also after a time becomes converted into &phosphate, but not into triphosphate. The presence of alumina also gives rise to the formation of phosphates soluble in ammonium citrate. When calcium carbonate is mixed with superphosphate in sufficient quantity, tricalcium phosphate is formed, insoluble in ammonium citrate ; if, however, a neutral solution of potassium citrate is employed, instead of ammoniacal potassium citrate, the retrograding of the phosphoric acid appears to be much greater than it really is. J. K. C. Alkanet Red, a Test for Magnesium Salts. By F. v. LEPEL (Ber., 13, 763-766).-Alkanet red, the colouring matter obtained from the roots of the false alkanet, Anchusa tinctoria, dissolved in a mixture of alcohol (2 parts), and ether (1 part), and diluted with water, exhibits an ahsorption spectrum composed of three bands.The violet-coloured solution produced by the addition of ammonium car- bonate to this mixture, is changed to blue by a minute quantity of aANALYTICAL CHEMISTRY. 63 magnesium salt, and a characteristic fourth absorption band is formed. By this test, 0.05 mgrm. in 1 C.C. of liquid can be detected. w. c. w. Vegetable Colouring Matters as Tests for Magnesium Salts. By I?. v. LEEPEL (Ber., 13, 766-’768).-Magnesium salts alter the absorption spectra of the colouring matters derived from (I) the roots of Aizchusa tiizcforicc and common beet (Beta uzdgaaris) ; (2) the flowers of the dahlia, dragon’s mouth (Antirrhiimm majm), horse chestnut, hyacinth, violet, rhododendron, the purple aster, and PhzuZa fnrinosa ; Chromium Sesquioxide.By T. WILM (BUZZ. XOC. Chirr~. [2], 34. 86) .-By reducing potassium dichromate or chrome alum with alcohol and hydrochloric acid, and then precipitating the sesquioxide by ammonia, a weight of the oxide is obtained greater than that required by theory. This is attributed to a partial oxidation and formation of chromic acid. (3) the juice of elderberries. w. c. w. V. H. V. The Officinal Test of Quinine and Water of Crystallisation of Quinine Sulphate. By 0. HESSE (Bey., 13, 1517--1520).-The method of testing quinine for cinchonidine adopted in Germany is that described in this Journal, 34, 434.The auth0.r points out that when cinchonidine sulphate is not added as an adulterant, but is mixed by crystallisation, it then takes a form which allows some to escape detection by the above method. The author has discovered an optical method of testing quinine, by which small amounts of cinchonidine n a y be detected. As cinchonidine sulphate crystallises with 6 mols. H20, or 13.7 per cent., and pure quinine sulphate with 8 mols. HzO, or 16-17 per cent., so the presence of cinchonidine may be detected by its influence on the percentage of water of crystallisation of a specimen. The purer the quinine sulphate, if perfectly dry and unweathered, the nearer is the percentage of water of crystallisation to 16-17.Korner states that he has obtained pure, unweathered crystals of quinine sul- phate, with only 14.4 per cent. of water. The author’s experience is contradictory to this statement, and he would regard such a low per- centage of water as presumptive evidence of the presence of cinchoni- dine sulphate. P. P. B. Testing Commercial Sulphate of Quinine for Foreign Alkaloids. By G. KERNER (Arch. Pharm. [ 3 ] , 16, 186--205).-The author described in 1862 the ‘‘ ammonia-method ’’ for testing the purity of commercial sulphate of quinine: the method has been adopted very widely. A fuller account of his process is here given, together with criticisms on a method proposed by Hesse. Hessc’s process resembles the author’s in not detecting less than 1 per cent. of cinchonidine sulphate, but from published results it appears to yield only an approximate estimation, whereas the ammonia- method as now described yields numbers of almost absolute accuracy.After stating his reasons for considering Hesse’s process unsatisfactory, the author describes the ammonia-method with recent improvements. The “ammonia-method” depends on the facts that a cold satu-64 ABSTRACTS OF CHEMICAL PAPERS. rated sclution of quinine sulphate contains an invariable quantity of the alkalo?d, and that the quantity of ammonia required to precipitate this as hydrate is constant, and that the excess of ammonia required to re-dissolve this precipitate is also constant. If the quantity of ammonia necessary to form the precipitate, and then re-dissolve it in a known volume of pure quinine sulphate solution a t normal or known temperatures has been determined, the excess of ammonia required for the same quantity of a saturated solution of commercial quinine sulphate gives the means of calculating the quantity of associated alkaloids, of which cinchonidine alone is usually preseut.Since quinine solution readily alters by becoming mouldy, and ammonia solution also alters in strength by keeping,. it is best to prepare a solution of pure quinine snlphate for each estimation, and titrate with it the ammonia to be used. Pure Quiniiae Xul@hate.-It is often necessary to recrystallise from three to six times, with addition of several drops of sulphuric acid in excess, in order t o get rid of the last traces of cinchonidine.The purity can be tested by treating portions with different proportions of cold water and titrating the solutions with ammonia: solutions of commercial samples require different amounts of ammonia when the proportion of solvent to solid has been varied ; but when pure, varia- tions of solid to solvent between 1 : 10 and 1 : '700 produce no altera- tion in the quantity of ammonia required, and the excess of solid remaining undissolved in making the solutions yields also solutions of precisely the same ammonia titre. Preparation, of Solutions and Process of Titratiort.-The pure quinine sulphate prepared as above is rubbed into a homogeneous paste with water in a mortar and rinsed into a stoppered vessel, in which it is frequently agitated during from twelve to eighteen hours : the pro- portion of quinine to water used being about 1 : 100.To prepare the solution of the sample to be tested, 5 grams are similarly treated with 50 C.C. of water. The vessels containing the quinine solutions and the vessel containing the ammonia solution (of 0.92 sp. gr.) are placed in cold water, and as soon as their contents have reached the same temperature, the quinine solutions are filtered through dry filter-papers. The temperature need not be normal, provided both quinine solutions are prepared a t the same temperature. The undissolved pure quinine is dried and kept, for future use. 10 C.C. of* each of the quinine solutions are then measured off into t,est-tubes, and each is titrated with the ammonia solution. 5 C.C. of ammonia solution are run in, and the test-tube is closed with the finger, and its contents are mixed by several times inverting without shaking it.The quinine is thus precipitated and almost entirely redis- solved, the liquid remaining but slightly turbid ; by gradually dropping in ammonia, mixing, and waiting several seconds after each addition, the moment when the liquid becomes perfectly clear is easily noted. The excess of ammonia required gives the quantity of cinchonidine sulphate present; on an average 0.288 c.c., or roughly 0.3 C.C. of ammonia solution of 0.92 sp. gr. were found to correspond to 1 mgrm. of crystallised cinchonidine sulphate. The error in the process cannot exceed 0.05 per cent.ANALYTICAL CHEMISTRY. 65 It must be understood that this process is only directly applicable to samples which answer t o the qualitative ammonia test, and which contain not more than 1.5 per cent.of cinchonidine sulphate ; if more than 2 per cent. is present, the final reaction cannot be obtained, since either insoluble flocks appear or the solution gelatinises when near the clarifying point : if from a preliminary qualitative test the nature or intensity of the turbidity renders it probable that 2 per cent. or more is present, the solution to be titrated may be prepared as directed above, and then be diluted with known quantities of the pure quinine solution, or larger proportions of water to quinine may be employed in making the solution : in the latter case, it is better to warm during the process of solution. It is nofed that chemically pure quinine hydrate crystallises out from the titrnted solution on standing. Afz approximate estimation of the cinchonidine sulphate can be made by introducing 5 C.C.of the water extract (1 : 10, prepared at 15" C.) into a 10 C.C. cylinder graduated to tenths of a c.c., and adding 3 C.C. of ammonia of 0.92 sp. gr. On mixing by inversion, the liquid Kill usually remain very turbid ; ammonia is then gradually added with constant mixing until the liquid becomes perfectly clear, and the total volume of ammonia added is read off. Assuming that 5 C.C. of ammonia indicate 1 per cent. of cinchonidine sulphate, and 3 C.C. indicate none, the percentage can be ascertained. This method gives with great accuracy relative values for quinine samples examined under similar conditions. This method is suaciently accurate for practical purposes, the former more exact method being resorted to for disputed cases and for scientific purposes only.Quinidine is seldom present, except as an aclulterant purposely added ; it dissolves somewhat more readily in excess of ammonia than cinchonidine does. The percentage of water, present as water of cry stallisation or other- wise, is of considepable importance, both for commercial reasons and to ensure the correctness of quantities of the alkalo'id used as doses. The presence of a small quantityof sulphuric acid tends to promote crumbling of the crystals with loss of their water of crystallisation, whilst a small amount of uncombined water tends to prevent this change. Uncombined water is estimated by the difference bet ween the quantities of water found on drying a portion of the original sample and another portion which has been pressed between soft blotting-paper. The author, after a long experience in estimating wa$er in quinine, considers that in the crystalline condition its formula is 2CzoHz4N,O,.H,SO4 -+ 7H,O: when dried at 115" C.it loses 14.45 per cent. of water: in practice the loss varies between 14.38 and 14.8. A good sample will usually not lose more than 13.8 to 14.4 per cent. by drying, but no sample should lose more than 14.6 per cent. without exciting suspicion. If left for some time in a dry and moderately warm situation, the crystallised sulphate loses nearly 5H20 (= 10.32 per cent.), leaving 2CzoH,4N,0z.H2S04 + 2Hz0, which contains 4.60 per cent.of water. In this form, the salt is less presentable in appearance, but is per- manent at temperatures below 100" C.: the sulphate would be well VOL. XL. f66 ABSTRACTS OF CHEMICAL PAPERS. suited for pharmaceutical purposes in this condition, since it is not liable to loss or absorption of moisture, and contains a maximum amount of 5 per cent. of water : it would also be impossible to moisten it without altering its appearance. Another means of avoiding the inconvenience arising from the variation in composition which is noticed in the ordinary commercial sulphate, would be to replace it by the hydrochloride, which is a far less variable salt, and is also more easily assimilated. As long as the crystallised sulphate is used, it is necessary to estimate the percentage of water in every sample in determining its value.The percentage of water is estimated either by finding the quantity of anhydrous alkaloid, and then calculating from the formula the quantity of water as recommended by Dwars (Arch. Phamz., 11, 149), or better, by directly estimating the loss of water, when from 1 to 2 grams are dried by heating very gradually to 115” C. 1’. c. Butter Analysis. By L. MEDICUS and others (Bied. Cerztr., 1880, 615-617). -The authors have examined Reichert’s method of esti- mating adulteration in butter, and confirm the results already obtained by him. Donny recommends as an easy method of detecting adultera- tion to heat a sample of butter in a test-tube at 160” ; if the butter is pure it foams very much, and becomes of a uniform brown colour ; if impurities are present there is very littlle swelling, but the liquid bumps violently, and casein separates out on the sides of the tube in brown masses, whilst the rest of the butter retaius its original colour.J. I(. C.62 ABSTRACTS OF CHF,MICAL PAPERS.A n a1 y t i c a 1 C h e m i s t r y.Apparatus for the Volumetric Estimation of Nitrogen. ByH. SCHWARZ (Ber., 13, 7’71--773).-This is a convenient moclificationof Zulkowsky’s apparatus for collecting the nitrogen evolved inorganic analyses of nitrogenous compounds by Dumas’s method. w. c. w.Action of Organic Acids on Minerals. By H. C. BOLTON (Bey.,13, 726--734).-l’The author points out that a large number ofminerals are decomposed, either by a hot concentrated solution ofcitric acid, or by the combined action of citric acid and sodium nitrate,potassium iodide or ammonium fluoride, and he suggests that this acidwould, on account of its safe portability, prove a valuable reagentduring mineralogical excursions.Tables are given of this reactionwith a large number of minerals. w. c. w.Estimation of Retrograde Phosphoric Acid. By A. GRUPEand others (Bied. Centr., 1880, 582--584).-The solvent action ofammonium citrate is greater a t 35” C. than at the ordinary tempera-ture, and in using this as a reagent for the estimation of retrogradephosphate, care must be taken to first remove by washing soluble saltsof magnesia, which have the effect of rendering bicalcium phosphateinsoluble in ammonium citrate ; the presence of calcium carbonate alsohas the same effect.J. K. C.Retrograde Phosphoric Acid. By M. A. MILLOT (Biecl. Centr.,1880, 577--580).-The author finds that when mineral superphos-phates contain a considerable quantity of ferric oxide, a part ofthe phosphoric acid combines with the iron, forming a compoundinsoluble in ammonium citrate, even when a sufficient quantity of sui-phuric acid has been used in the decomposition of the phosphate.Calcium monophosphate also after a time becomes converted into&phosphate, but not into triphosphate. The presence of alumina alsogives rise to the formation of phosphates soluble in ammonium citrate.When calcium carbonate is mixed with superphosphate in sufficientquantity, tricalcium phosphate is formed, insoluble in ammoniumcitrate ; if, however, a neutral solution of potassium citrate is employed,instead of ammoniacal potassium citrate, the retrograding of thephosphoric acid appears to be much greater than it really is.J.K. C.Alkanet Red, a Test for Magnesium Salts. By F. v. LEPEL(Ber., 13, 763-766).-Alkanet red, the colouring matter obtainedfrom the roots of the false alkanet, Anchusa tinctoria, dissolved in amixture of alcohol (2 parts), and ether (1 part), and diluted withwater, exhibits an ahsorption spectrum composed of three bands. Theviolet-coloured solution produced by the addition of ammonium car-bonate to this mixture, is changed to blue by a minute quantity of ANALYTICAL CHEMISTRY. 63magnesium salt, and a characteristic fourth absorption band is formed.By this test, 0.05 mgrm.in 1 C.C. of liquid can be detected. w. c. w.Vegetable Colouring Matters as Tests for Magnesium Salts.By I?. v. LEEPEL (Ber., 13, 766-’768).-Magnesium salts alter theabsorption spectra of the colouring matters derived from (I) the rootsof Aizchusa tiizcforicc and common beet (Beta uzdgaaris) ; (2) the flowersof the dahlia, dragon’s mouth (Antirrhiimm majm), horse chestnut,hyacinth, violet, rhododendron, the purple aster, and PhzuZa fnrinosa ;Chromium Sesquioxide. By T. WILM (BUZZ. XOC. Chirr~. [2], 34.86) .-By reducing potassium dichromate or chrome alum with alcoholand hydrochloric acid, and then precipitating the sesquioxide byammonia, a weight of the oxide is obtained greater than that requiredby theory.This is attributed to a partial oxidation and formationof chromic acid.(3) the juice of elderberries. w. c. w.V. H. V.The Officinal Test of Quinine and Water of Crystallisationof Quinine Sulphate. By 0. HESSE (Bey., 13, 1517--1520).-Themethod of testing quinine for cinchonidine adopted in Germany isthat described in this Journal, 34, 434. The auth0.r points out thatwhen cinchonidine sulphate is not added as an adulterant, but is mixedby crystallisation, it then takes a form which allows some to escapedetection by the above method. The author has discovered an opticalmethod of testing quinine, by which small amounts of cinchonidinen a y be detected. As cinchonidine sulphate crystallises with 6 mols.H20, or 13.7 per cent., and pure quinine sulphate with 8 mols.HzO, or16-17 per cent., so the presence of cinchonidine may be detected by itsinfluence on the percentage of water of crystallisation of a specimen.The purer the quinine sulphate, if perfectly dry and unweathered, thenearer is the percentage of water of crystallisation to 16-17. Kornerstates that he has obtained pure, unweathered crystals of quinine sul-phate, with only 14.4 per cent. of water. The author’s experience iscontradictory to this statement, and he would regard such a low per-centage of water as presumptive evidence of the presence of cinchoni-dine sulphate. P. P. B.Testing Commercial Sulphate of Quinine for ForeignAlkaloids. By G. KERNER (Arch. Pharm. [ 3 ] , 16, 186--205).-Theauthor described in 1862 the ‘‘ ammonia-method ’’ for testing thepurity of commercial sulphate of quinine: the method has beenadopted very widely.A fuller account of his process is here given,together with criticisms on a method proposed by Hesse.Hessc’s process resembles the author’s in not detecting less than1 per cent. of cinchonidine sulphate, but from published results itappears to yield only an approximate estimation, whereas the ammonia-method as now described yields numbers of almost absolute accuracy.After stating his reasons for considering Hesse’s process unsatisfactory,the author describes the ammonia-method with recent improvements.The “ammonia-method” depends on the facts that a cold satu64 ABSTRACTS OF CHEMICAL PAPERS.rated sclution of quinine sulphate contains an invariable quantity ofthe alkalo?d, and that the quantity of ammonia required to precipitatethis as hydrate is constant, and that the excess of ammonia requiredto re-dissolve this precipitate is also constant.If the quantity ofammonia necessary to form the precipitate, and then re-dissolve it ina known volume of pure quinine sulphate solution a t normal or knowntemperatures has been determined, the excess of ammonia requiredfor the same quantity of a saturated solution of commercial quininesulphate gives the means of calculating the quantity of associatedalkaloids, of which cinchonidine alone is usually preseut. Sincequinine solution readily alters by becoming mouldy, and ammoniasolution also alters in strength by keeping,.it is best to prepare asolution of pure quinine snlphate for each estimation, and titrate withit the ammonia to be used.Pure Quiniiae Xul@hate.-It is often necessary to recrystallise fromthree to six times, with addition of several drops of sulphuric acidin excess, in order t o get rid of the last traces of cinchonidine. Thepurity can be tested by treating portions with different proportions ofcold water and titrating the solutions with ammonia: solutions ofcommercial samples require different amounts of ammonia when theproportion of solvent to solid has been varied ; but when pure, varia-tions of solid to solvent between 1 : 10 and 1 : '700 produce no altera-tion in the quantity of ammonia required, and the excess of solidremaining undissolved in making the solutions yields also solutions ofprecisely the same ammonia titre.Preparation, of Solutions and Process of Titratiort.-The pure quininesulphate prepared as above is rubbed into a homogeneous paste withwater in a mortar and rinsed into a stoppered vessel, in which it isfrequently agitated during from twelve to eighteen hours : the pro-portion of quinine to water used being about 1 : 100.To prepare thesolution of the sample to be tested, 5 grams are similarly treated with50 C.C. of water. The vessels containing the quinine solutions andthe vessel containing the ammonia solution (of 0.92 sp. gr.) are placedin cold water, and as soon as their contents have reached the sametemperature, the quinine solutions are filtered through dry filter-papers.The temperature need not be normal, provided both quinine solutionsare prepared a t the same temperature.The undissolved pure quinineis dried and kept, for future use.10 C.C. of* each of the quinine solutions are then measured off intot,est-tubes, and each is titrated with the ammonia solution. 5 C.C. ofammonia solution are run in, and the test-tube is closed with thefinger, and its contents are mixed by several times inverting withoutshaking it. The quinine is thus precipitated and almost entirely redis-solved, the liquid remaining but slightly turbid ; by gradually droppingin ammonia, mixing, and waiting several seconds after each addition,the moment when the liquid becomes perfectly clear is easily noted.The excess of ammonia required gives the quantity of cinchonidinesulphate present; on an average 0.288 c.c., or roughly 0.3 C.C.ofammonia solution of 0.92 sp. gr. were found to correspond to 1 mgrm.of crystallised cinchonidine sulphate. The error in the process cannotexceed 0.05 per centANALYTICAL CHEMISTRY. 65It must be understood that this process is only directly applicableto samples which answer t o the qualitative ammonia test, and whichcontain not more than 1.5 per cent. of cinchonidine sulphate ; if morethan 2 per cent. is present, the final reaction cannot be obtained, sinceeither insoluble flocks appear or the solution gelatinises when nearthe clarifying point : if from a preliminary qualitative test the nature orintensity of the turbidity renders it probable that 2 per cent.or moreis present, the solution to be titrated may be prepared as directedabove, and then be diluted with known quantities of the pure quininesolution, or larger proportions of water to quinine may be employedin making the solution : in the latter case, it is better to warm duringthe process of solution.It is nofed that chemically pure quinine hydrate crystallises outfrom the titrnted solution on standing.Afz approximate estimation of the cinchonidine sulphate can be madeby introducing 5 C.C. of the water extract (1 : 10, prepared at 15" C.)into a 10 C.C. cylinder graduated to tenths of a c.c., and adding 3 C.C.of ammonia of 0.92 sp. gr. On mixing by inversion, the liquid Killusually remain very turbid ; ammonia is then gradually added withconstant mixing until the liquid becomes perfectly clear, and thetotal volume of ammonia added is read off.Assuming that 5 C.C. ofammonia indicate 1 per cent. of cinchonidine sulphate, and 3 C.C.indicate none, the percentage can be ascertained. This method giveswith great accuracy relative values for quinine samples examinedunder similar conditions. This method is suaciently accurate forpractical purposes, the former more exact method being resorted tofor disputed cases and for scientific purposes only.Quinidine is seldom present, except as an aclulterant purposelyadded ; it dissolves somewhat more readily in excess of ammonia thancinchonidine does.The percentage of water, present as water of cry stallisation or other-wise, is of considepable importance, both for commercial reasons andto ensure the correctness of quantities of the alkalo'id used as doses.The presence of a small quantityof sulphuric acid tends to promotecrumbling of the crystals with loss of their water of crystallisation,whilst a small amount of uncombined water tends to prevent thischange.Uncombined water is estimated by the difference bet weenthe quantities of water found on drying a portion of the originalsample and another portion which has been pressed between softblotting-paper. The author, after a long experience in estimatingwa$er in quinine, considers that in the crystalline condition its formulais 2CzoHz4N,O,.H,SO4 -+ 7H,O: when dried at 115" C.it loses 14.45per cent. of water: in practice the loss varies between 14.38 and14.8. A good sample will usually not lose more than 13.8 to 14.4 percent. by drying, but no sample should lose more than 14.6 per cent.without exciting suspicion.If left for some time in a dry and moderately warm situation, thecrystallised sulphate loses nearly 5H20 (= 10.32 per cent.), leaving2CzoH,4N,0z.H2S04 + 2Hz0, which contains 4.60 per cent. of water.In this form, the salt is less presentable in appearance, but is per-manent at temperatures below 100" C.: the sulphate would be wellVOL. XL. 66 ABSTRACTS OF CHEMICAL PAPERS.suited for pharmaceutical purposes in this condition, since it is notliable to loss or absorption of moisture, and contains a maximumamount of 5 per cent. of water : it would also be impossible to moistenit without altering its appearance. Another means of avoiding theinconvenience arising from the variation in composition which isnoticed in the ordinary commercial sulphate, would be to replace itby the hydrochloride, which is a far less variable salt, and is also moreeasily assimilated. As long as the crystallised sulphate is used, it isnecessary to estimate the percentage of water in every sample indetermining its value.The percentage of water is estimated either by finding the quantityof anhydrous alkaloid, and then calculating from the formula thequantity of water as recommended by Dwars (Arch. Phamz., 11, 149),or better, by directly estimating the loss of water, when from 1 to 2grams are dried by heating very gradually to 115” C. 1’. c.Butter Analysis. By L. MEDICUS and others (Bied. Cerztr., 1880,615-617). -The authors have examined Reichert’s method of esti-mating adulteration in butter, and confirm the results already obtainedby him. Donny recommends as an easy method of detecting adultera-tion to heat a sample of butter in a test-tube at 160” ; if the butter ispure it foams very much, and becomes of a uniform brown colour ; ifimpurities are present there is very littlle swelling, but the liquidbumps violently, and casein separates out on the sides of the tube inbrown masses, whilst the rest of the butter retaius its original colour.J. I(. C

ISSN:0368-1769    

DOI:10.1039/CA8814000062

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

66 ABSTRACTS OF CHEMICAL PAPERS. T e c h n i c a1 Chemistry. The Changes Undergone by Meat in the Process of Pick- ling. By VOIT ( Z e i t s , Biologie, 15,492-495).-Rubner (Zeits. BLoZogie, 1877, 13, 513) found that meat, when pickled, lost no albumino'ids arid only 11 per cent. of its phosphoric acid. The author treated 926 grams of meat with a brine containing 60 grams of common salt for 14 days. The meat originally contained 702.8 grams of water, and 223.2 grams of solid residue ; the residue yielded 211.1 grams of organic matter and 12.04 grams of ash, with 4.12 grams of phosphoric acid. After 14 days, the brine contained 23.48 grams of dry residue with the compo- sition :-TECHNICAL CHEMISTRY. 67 Meat lost Total. Per cent. per cent. Organic matters. ....... 4.4 7 19.88 2.1 Albumin.............. 2.18 9-68 1.1 Extractives .......... 2.29 10.19 13.5 Ash.. 80.12 I ................ 18.01 NaCl 71.50 - ................ 16.08 Phosphoric acid. ....... 0.35 1.56 8-5 The meat when taken out weighed 892.3 grams, indicating a loss of 33.7 grams ; the dry residue of the meat weighed 270.5 grams, i.e., the salt meat contained 30.31 per cent. solid and 69.69 per cent. of water. 1,000 parts of fresh meat would from these results be affected by salting as follows :- It would take up 43 grams salt. It would lose 19.7 grams water = 10.4 per cent. 9 , 4-8 ,, organic matter = 2.1 ,, 9’ 2.4 ,, albumin = 1.1 ,, 9 , 2.5 ,, extractives = 13.5 ,, ’ 9 0.4 ,, phosphoric acid= 8.5 ,, The author is of opinion that meat is by no means so seriously deteriorated as a food by salting as is generally supposed.W. N. Analyses of Gluten Bread. By I(. BIRNBAUM ( B e d . Centr., 1880, 370-311) .-The preparation of bread from the gluten of wheat for the use of persons suffering from diabetes is of considerable im- portance. Boussingault examined some samples and declared them unsuitable, but the author’s investigations show that he must have examined inferior qualities, and that his condemnation should not extend to all kinds. The German preparations show a large propor- tion of proteh substance and a small one of carbohydrates. J. F. Hair-dyes. By J. F. BRAGA (Chem. News, 42, 8).-A solution of silver nitrate (10 grams per litre) when used f o r some time as a hair- dye produces a dull reddish-brown tint. This is particularly noticeable when the light falls veryobliquely.This defect is avoided by adding zt small quantity of copper solution to the silver nitrate; 36 grams of silver nitrate and 2.5 grams of copper sulphate are dissolved in 250 C.C. of water, sufficient ammonia to redissolve the precipitate, and the whole made up to 1 litre with water. An “ instantaneous dye” is obtained by treating the hair first with a solution of pyrogallic acid, made strongly acid with acetic acid, and when it is almost dry, the silver and copper solution of the above strength is added. All shades from brown to black may be obtained by varying the strength of the pyrogallic acid from 1 to 50 grams per litre. L. T. 0’s. Composition of Ink. By W. THOMPSON (Ckem. News, 42, 32- 33).-Thc author finds that in the testing of inks, the following re-68 ABSTRACTS OF CHEMICAL PAPERS.agents are the best :-Dilute sulphnric acid, strong hydrochloric acid, dilute nitric acid., sulphurous acid, caustic soda, oxalic acid, bleaching powder, stannous and stannic chlorides. Ink, prepared by the same maker at different Limes, gives different results. Black inks, when treated with dilute sulphuric acid, behave very differently, some giving shades from a bright crimson to a deep red, whilst others give a blue-green, violet, or grey. The reactions given by the same ink with the same reagent vary according to the length of time which has elapsed since the ink was used. The length of time that an ink is exposed to sunlight also in- fluences the character of the reaction, as does the use of steel pens.L. T. 0’s. Combustibility of Tobacco. By E. QUAJAT ( B i d Ce7rtr., 1880, 345-347) .-The author examined 14 specimeiis of tobacco, con- sisting of common and fine sorts. The percentage of ash to dry sub- stance varied from 31.05 in a Ra,ssano sample down to 17.11 in Vir- ginian and 16-78 in a sample of Turkish. The author rules that the finer the quality the smaller is the amount of ash. (Nessler, however, says that there is no relation between the two.) The composition of the ash is of the most variable character, and in the most easily combustible, potassium salts seem to pre- dominate over ofher mineral salts. Some samples, which burned with difficulty, were improved by steeping in a solution o f potassium salts and organic acids, but others were not so improved.The author re- commends the study of this point to tobacco manufacturers. He agrees with Nessler that the amount of nicotine present has no effect on the combustibility. Compositiozt of the Ash of 5 Samples of Tobacco. Silicic acid ........ Lime ............ Magnesia.. ........ Phosphoric acid .... Sulphuric anhydride Carbonic ,, Ferric oxide ...... Chlorine .......... Potash.. .......... Soda.. ............ Virginia cigars. 2 *55 26 ‘64 47 *69 2 -97 4 -21 20.82 3 ‘27 6 *55 20 *01 5 *77 -- Sella cigars. 2 *99 6 *93 3 -61 3.80 -~ 28.70 i 9 . m 2 -79 3 *’is 21 -27 ’7 *03 Benerent,on leaves. 0 ‘00 27.99 1.74 5 .28 4 *83 20 -09 4.71 7 *14 24 -15 3 .89 Virginia leaves. Bot. Gar., Padua. 0 *95 37 *49 4 -96 6 9 1 3 *63 25 -26 1 ‘27 1 *Of3 11 -75 5 -33 J.F.66 ABSTRACTS OF CHEMICAL PAPERS.T e c h n i c a1 Chemistry.The Changes Undergone by Meat in the Process of Pick-ling. By VOIT ( Z e i t s , Biologie, 15,492-495).-Rubner (Zeits. BLoZogie,1877, 13, 513) found that meat, when pickled, lost no albumino'idsarid only 11 per cent. of its phosphoric acid.The author treated 926 grams of meat with a brine containing60 grams of common salt for 14 days.The meat originally contained 702.8 grams of water, and 223.2 gramsof solid residue ; the residue yielded 211.1 grams of organic matter and12.04 grams of ash, with 4.12 grams of phosphoric acid. After 14days, the brine contained 23.48 grams of dry residue with the compo-sition :TECHNICAL CHEMISTRY. 67Meat lostTotal.Per cent. per cent.Organic matters. ....... 4.4 7 19.88 2.1Albumin.. ............ 2.18 9-68 1.1Extractives .......... 2.29 10.19 13.5Ash.. 80.12 I ................ 18.01NaCl 71.50 - ................ 16.08Phosphoric acid. ....... 0.35 1.56 8-5The meat when taken out weighed 892.3 grams, indicating a lossof 33.7 grams ; the dry residue of the meat weighed 270.5 grams, i.e.,the salt meat contained 30.31 per cent. solid and 69.69 per cent. ofwater.1,000 parts of fresh meat would from these results be affected bysalting as follows :-It would take up 43 grams salt.It would lose 19.7 grams water = 10.4 per cent.9 , 4-8 ,, organic matter = 2.1 ,,9’ 2.4 ,, albumin = 1.1 ,,9 , 2.5 ,, extractives = 13.5 ,,’ 9 0.4 ,, phosphoric acid= 8.5 ,,The author is of opinion that meat is by no means so seriouslydeteriorated as a food by salting as is generally supposed.W. N.Analyses of Gluten Bread.By I(. BIRNBAUM ( B e d . Centr.,1880, 370-311) .-The preparation of bread from the gluten of wheatfor the use of persons suffering from diabetes is of considerable im-portance. Boussingault examined some samples and declared themunsuitable, but the author’s investigations show that he must haveexamined inferior qualities, and that his condemnation should notextend to all kinds. The German preparations show a large propor-tion of proteh substance and a small one of carbohydrates.J. F.Hair-dyes. By J. F. BRAGA (Chem. News, 42, 8).-A solution ofsilver nitrate (10 grams per litre) when used f o r some time as a hair-dye produces a dull reddish-brown tint.This is particularly noticeablewhen the light falls veryobliquely. This defect is avoided by adding ztsmall quantity of copper solution to the silver nitrate; 36 grams ofsilver nitrate and 2.5 grams of copper sulphate are dissolved in 250 C.C.of water, sufficient ammonia to redissolve the precipitate, and the wholemade up to 1 litre with water.An “ instantaneous dye” is obtained by treating the hair first witha solution of pyrogallic acid, made strongly acid with acetic acid, andwhen it is almost dry, the silver and copper solution of the abovestrength is added. All shades from brown to black may be obtainedby varying the strength of the pyrogallic acid from 1 to 50 grams perlitre.L. T. 0’s.Composition of Ink. By W. THOMPSON (Ckem. News, 42, 32-33).-Thc author finds that in the testing of inks, the following re68 ABSTRACTS OF CHEMICAL PAPERS.agents are the best :-Dilute sulphnric acid, strong hydrochloric acid,dilute nitric acid., sulphurous acid, caustic soda, oxalic acid, bleachingpowder, stannous and stannic chlorides.Ink, prepared by the same maker at different Limes, gives differentresults. Black inks, when treated with dilute sulphuric acid, behavevery differently, some giving shades from a bright crimson to a deepred, whilst others give a blue-green, violet, or grey.The reactions given by the same ink with the same reagent varyaccording to the length of time which has elapsed since the ink wasused.The length of time that an ink is exposed to sunlight also in-fluences the character of the reaction, as does the use of steel pens.L. T. 0’s.Combustibility of Tobacco. By E. QUAJAT ( B i d Ce7rtr., 1880,345-347) .-The author examined 14 specimeiis of tobacco, con-sisting of common and fine sorts. The percentage of ash to dry sub-stance varied from 31.05 in a Ra,ssano sample down to 17.11 in Vir-ginian and 16-78 in a sample of Turkish. The author rules that thefiner the quality the smaller is the amount of ash. (Nessler, however,says that there is no relation between the two.)The composition of the ash is of the most variable character,and in the most easily combustible, potassium salts seem to pre-dominate over ofher mineral salts. Some samples, which burned withdifficulty, were improved by steeping in a solution o f potassium saltsand organic acids, but others were not so improved. The author re-commends the study of this point to tobacco manufacturers. Heagrees with Nessler that the amount of nicotine present has no effecton the combustibility.Compositiozt of the Ash of 5 Samples of Tobacco.Silicic acid ........Lime ............Magnesia.. ........Phosphoric acid ....Sulphuric anhydrideCarbonic ,,Ferric oxide ......Chlorine ..........Potash.. ..........Soda.. ............Virginiacigars.2 *5526 ‘6447 *692 -974 -2120.823 ‘276 *5520 *015 *77--Sellacigars.2 *996 *933 -613.80-~28.70i 9 . m2 -793 *’is21 -27’7 *03Benerent,onleaves.0 ‘0027.991.745 .284 *8320 -094.717 *1424 -153 .89Virginialeaves.Bot. Gar.,Padua.0 *9537 *494 -966 9 13 *6325 -261 ‘271 *Of311 -755 -33J. F

ISSN:0368-1769    

DOI:10.1039/CA8814000066

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

69 General and P h y s i c a l Chemistry. Relative Intensity of the Spectral Lines of Hydrogen and Nitrogen; its Bearing on the Conqtitution of Nebulae. By C. FIEVEZ (Anrt. Chim. Phys. [5], 20, 179-1 85).-Observations by Huggins have shown that in the spectra of certain nebulte there exists only one nitrogen line and one hydrogen line, and further researches by the same physicist have proved that the complex spectrum of nitrogen .can be readily simplified by merely diminishing its intensity, so that it is possible to extinguish a portion of the luminous rays, and to leave visible only those which are observable in the nebular spectrum. Adopting a method similar to that originally devised by Huggins, the author has also succeeded in showing that if the hydrogen spectrum be reduced in intensity, the line F, which corresponds with that of the nebuh, will alone remain visible after the C and other more refrangible lines have become too weak t o affect the eye.The method employed consisted in projecting by means of a lens a real image of the luminous body on the slit of the,spectroscope, and after- wards altering the intensity of this image, either by diminishing the aperture of the lens used for projection, or by placing a diaphragm with a circular opening between the lens and the image. The hydrogen tube was one of Plucker's, entirely covered with lamp-black: with the exception of a small portion of the contracted part, and was placed vertically before the projection lens. The dis- kames from the tube to the lens arid from the latter to the slit were arranged in such a manner that the projected image was narrower than the length of the slit, so that the luminous pencil, after it had passed through the slit, was received in its entirety upon the objective of the spectroscope. This arrangement, which is due to Lockyer, enables the observer to distinguish between long and short lines.With a powerful induction coil and condenser arranged for tension, and with a six-prism spectroscope, the hydrogen lines C, F, and H, are perfectly visible ; the hminous pencil was then narrowed gradually by means of a diaphragm of Of!07 meter aperture, by withdrawing the diaphragm from the slit and bringing it nearer to the lens. The length of the lines was seen to diminish, and the H line finally became invisible, whilst the other two lines still remained brilliant.With a diaphragm of 0.002 meter aperture the C line also disappeared, leaving the F line alone visible. With a small induction coil without a con- denser, and a two-prism spectroscope, the same results may be obtained, but less rapidly than with more powerful instruments. The line spectrum of nitrogen, called also a spectrum of the second order, is formed of several groups of lines indicated by Plucker by the numerals 1, 2, 3, 4, and 5. With the large coil and spectroscope, and a 0.007 meter diaphragm as before, the groups 1, 3, 5, 2, successively g VOL. XL.70 ABSTRACTS OF CHEMICAL PAPERS. disappear, and group 4 is extinguished, with the exception of the double line coinciding with that of the nebuh.If, while the experiment is proceeding, and when a line or group of lines have just been rendered invisible, the width of the slit of the spectroscope be slightly increased, the extinguished line immediately reappears, thus showing plainly that the disappearance is due, as was anticipated, to the weakening of the luminous iutcnsity of the ray. We are therefore at liberty to consider with Huggins that certain nebula do contain nitrogen and hydrogen among their constituent elements, referring the relative invisibility of the other rays to the absorptive action of space. J. W. Fluorescence. By 0. LUBARSCH (Aim. Phys. Chem. [2], 11, 46-69) .-The paper describes the author’s researches ou fluorescencei in which he has repeated the experiments of Eagenbach with certain modifications in the spectroscopic apparatus, whereby light of greater homogeneity is obtained.From the numerous experiments and observations adduced in the paper, the author’s conclusion is that Stokes’s law can no longer be maintained as a universally valid prin- ciple. R. R. Thermia Theory of Electricity. By J. L. HOORWEG (Ann. Phys. Chem. [2], 11, 133--155).-1n tbis paper, the author continues to adduce experiments and reasonings in support of the view which regards the molecular motion of heat as the source of electrical energy. He conceives that when any disturbance of the motions of the mole- cules occasions a loss of their vis viva, an equivalent quantity of elec- tricity appears. Among the propositions discussed are the following :- The division of bodies into classes, according as their conductivity is distinguished as metallic or electrolytic, is artificial. A current arises when a t least one of the substances in a closed circuit has its con- ductivity increased by rise of temperature.The electricity of friction and pressure arises from the contact of heterogeneous substances, by which the loss of molecular vis viva is occasioned. Friction simply increases the intimacy of the contact by multiplying the points at which the bodies touch, and it unequally raises the temperature of both substances, thus producing conditions which co-operate in aug- menting the effect. The electricity of friction and pressure has the same origin as that of the pile, viz., a disturbance of the molecules occasioning a loss of their vis viva.The theory is applied to pyro- electricity, thermo-electricity, and the electrical phenomena observed in evaporation, solidification, solution, cleavage, division, osmose, and capillary acttion. R. R. Discharge of Electricity in Gases and High Vacua. By F. NARR (Ann. Phys. Ohem., 11, 155--163).-The paper describes experiments in continuation of a former research on the passage of electricity through the vacua obtained by the Sprengel mercury pump. Glass tubes were not employed on account of their uncertain and changeable electrical properties, the vessel used being a hollow brass sphere. The resnlts appear to shorn that electricity traversesQENERAL AND PHYSICAL CHEMISTRY. 71 C E = - . I) Condensa- tion. 1 *49 1 ‘36 1 .17 1 -76 1 -34 0 9 7 1.38 1.05 --- the gas-vacuum, but the author remits their full discussion to a forth- coming communication.R. R. A. 1 sp. gr. Observer. - --_- 2.20 Clarke 2 .78 do. 1.998 Kremer 3-10 Clarke 3-49 do. 3 -94 Knight 5 .98 Fullerton 3.02 do. Electrical Conductivity of Saline Solutions. By J. H. LONG (Ann. Phys. Chem. [Z], 11, 37--46).-The author has continued the investigations of Rohlrausch on the conductivity of saline solutions at different temperatures and states of concentration. The salts exa- mined were the chlorides of manganese and zinc, and the nitrates of copper, strontium, and lead. The results, of which tables and graphic representations are given, are discussed in relation to the observations of other experimenters. R. R. Vapour-tensions of Homologous Series and Kopp’s Law of ‘Constant Difference of Boiling Points. By A.W~NKELMAN By U. D~HRING (Ann. Phys. Chem. [ Z ] , 11, 163--170).-The correctness of a law brought forward by the author having been questioned by A. Winkel- man (ibid. [Z], 9, 391), the present paper is devoted to its defence. The law in dispute maybe represented (Annalen, 204, 251-264). The Law of Corresponding Boiling Points. the equation- B. weight. 120.9 165 ‘4 42 ‘5 87.0 134.0 183 ‘0 366 .O ~ 0 1 . - 212.4 t’,) - t’, - qr tp’ - tp 4 - - where tp and 4’ are the boiling points of a liquid under the pressures p and p’ respectively, and t;l and t;l’ those of another liquid under the same pressures, while q and 4’ are constants depending upon the two liquids. R. R. Volume Relations of some HaloYd Salts.By W. MGLLXR ERZBACH (Ber., 13, 1658-1660) .-The author has previously pointed out that the contraction taking place when chlorine, bromine, and iodine combine with metals is most considerable in t’he case of chlorine, and least with iodine. He now confirms his prerious observations by cal- culating the contraction from a number of new data obtained by various observers. These are given in the following table :- Name of salt. RbCl . . . RbBr.. RbI . . . . LiC1.. . . LiBr . . . LiI.. . . . CdI,. . . . CdC12. # . - C. Calc. volume. 81 -7 81 .7 81 *’7 37’4 37 *4 37 -4 64 *2 64 *2 - B D = -. A Volnme found. 55 .o 59 ‘8 70 ‘0 21 ‘2 28 -1 38 *5 46 -5 61 -0 C-D C Contrac- tion. 0 9 2 0.27 0 -14 0 -4.3 0 -25 - 0 ‘03 0.27 0 *05 F =-. --- 0. H. 9 269General and P h y s i c a l Chemistry.Relative Intensity of the Spectral Lines of Hydrogen andNitrogen; its Bearing on the Conqtitution of Nebulae.ByC. FIEVEZ (Anrt. Chim. Phys. [5], 20, 179-1 85).-Observations byHuggins have shown that in the spectra of certain nebulte thereexists only one nitrogen line and one hydrogen line, and furtherresearches by the same physicist have proved that the complexspectrum of nitrogen .can be readily simplified by merely diminishingits intensity, so that it is possible to extinguish a portion of theluminous rays, and to leave visible only those which are observable inthe nebular spectrum.Adopting a method similar to that originally devised by Huggins,the author has also succeeded in showing that if the hydrogenspectrum be reduced in intensity, the line F, which corresponds withthat of the nebuh, will alone remain visible after the C and othermore refrangible lines have become too weak t o affect the eye.Themethod employed consisted in projecting by means of a lens a realimage of the luminous body on the slit of the,spectroscope, and after-wards altering the intensity of this image, either by diminishing theaperture of the lens used for projection, or by placing a diaphragmwith a circular opening between the lens and the image.The hydrogen tube was one of Plucker's, entirely covered withlamp-black: with the exception of a small portion of the contractedpart, and was placed vertically before the projection lens. The dis-kames from the tube to the lens arid from the latter to the slit werearranged in such a manner that the projected image was narrowerthan the length of the slit, so that the luminous pencil, after it hadpassed through the slit, was received in its entirety upon the objectiveof the spectroscope.This arrangement, which is due to Lockyer,enables the observer to distinguish between long and short lines.With a powerful induction coil and condenser arranged for tension,and with a six-prism spectroscope, the hydrogen lines C, F, and H,are perfectly visible ; the hminous pencil was then narrowed graduallyby means of a diaphragm of Of!07 meter aperture, by withdrawing thediaphragm from the slit and bringing it nearer to the lens. Thelength of the lines was seen to diminish, and the H line finally becameinvisible, whilst the other two lines still remained brilliant. With adiaphragm of 0.002 meter aperture the C line also disappeared, leavingthe F line alone visible.With a small induction coil without a con-denser, and a two-prism spectroscope, the same results may be obtained,but less rapidly than with more powerful instruments.The line spectrum of nitrogen, called also a spectrum of the secondorder, is formed of several groups of lines indicated by Plucker by thenumerals 1, 2, 3, 4, and 5. With the large coil and spectroscope, anda 0.007 meter diaphragm as before, the groups 1, 3, 5, 2, successivelyg VOL. XL70 ABSTRACTS OF CHEMICAL PAPERS.disappear, and group 4 is extinguished, with the exception of the doubleline coinciding with that of the nebuh.If, while the experiment isproceeding, and when a line or group of lines have just been renderedinvisible, the width of the slit of the spectroscope be slightly increased,the extinguished line immediately reappears, thus showing plainlythat the disappearance is due, as was anticipated, to the weakening ofthe luminous iutcnsity of the ray. We are therefore at liberty toconsider with Huggins that certain nebula do contain nitrogen andhydrogen among their constituent elements, referring the relativeinvisibility of the other rays to the absorptive action of space.J. W.Fluorescence. By 0. LUBARSCH (Aim. Phys. Chem. [2], 11,46-69) .-The paper describes the author’s researches ou fluorescenceiin which he has repeated the experiments of Eagenbach with certainmodifications in the spectroscopic apparatus, whereby light of greaterhomogeneity is obtained.From the numerous experiments andobservations adduced in the paper, the author’s conclusion is thatStokes’s law can no longer be maintained as a universally valid prin-ciple. R. R.Thermia Theory of Electricity. By J. L. HOORWEG (Ann. Phys.Chem. [2], 11, 133--155).-1n tbis paper, the author continues toadduce experiments and reasonings in support of the view whichregards the molecular motion of heat as the source of electrical energy.He conceives that when any disturbance of the motions of the mole-cules occasions a loss of their vis viva, an equivalent quantity of elec-tricity appears. Among the propositions discussed are the following :-The division of bodies into classes, according as their conductivity isdistinguished as metallic or electrolytic, is artificial.A current ariseswhen a t least one of the substances in a closed circuit has its con-ductivity increased by rise of temperature. The electricity of frictionand pressure arises from the contact of heterogeneous substances,by which the loss of molecular vis viva is occasioned. Friction simplyincreases the intimacy of the contact by multiplying the points atwhich the bodies touch, and it unequally raises the temperature ofboth substances, thus producing conditions which co-operate in aug-menting the effect. The electricity of friction and pressure has thesame origin as that of the pile, viz., a disturbance of the moleculesoccasioning a loss of their vis viva.The theory is applied to pyro-electricity, thermo-electricity, and the electrical phenomena observedin evaporation, solidification, solution, cleavage, division, osmose, andcapillary acttion. R. R.Discharge of Electricity in Gases and High Vacua. ByF. NARR (Ann. Phys. Ohem., 11, 155--163).-The paper describesexperiments in continuation of a former research on the passage ofelectricity through the vacua obtained by the Sprengel mercury pump.Glass tubes were not employed on account of their uncertain andchangeable electrical properties, the vessel used being a hollowbrass sphere. The resnlts appear to shorn that electricity traverseQENERAL AND PHYSICAL CHEMISTRY.71C E = - .I)Condensa-tion.1 *491 ‘361 .171 -761 -340 9 71.381.05---the gas-vacuum, but the author remits their full discussion to a forth-coming communication. R. R.A. 1sp. gr. Observer.- --_-2.20 Clarke2 .78 do.1.998 Kremer3-10 Clarke3-49 do.3 -94 Knight5 .98 Fullerton3.02 do.Electrical Conductivity of Saline Solutions. By J. H. LONG(Ann. Phys. Chem. [Z], 11, 37--46).-The author has continued theinvestigations of Rohlrausch on the conductivity of saline solutions atdifferent temperatures and states of concentration. The salts exa-mined were the chlorides of manganese and zinc, and the nitrates ofcopper, strontium, and lead. The results, of which tables and graphicrepresentations are given, are discussed in relation to the observationsof other experimenters.R. R.Vapour-tensions of Homologous Series and Kopp’s Law of‘Constant Difference of Boiling Points. By A. W~NKELMANBy U. D~HRING(Ann. Phys. Chem. [ Z ] , 11, 163--170).-The correctness of a lawbrought forward by the author having been questioned by A. Winkel-man (ibid. [Z], 9, 391), the present paper is devoted to its defence.The law in dispute maybe represented(Annalen, 204, 251-264).The Law of Corresponding Boiling Points.the equation-B.weight.120.9165 ‘442 ‘587.0134.0183 ‘0366 .O~ 0 1 .-212.4t’,) - t’, - qrtp’ - tp 4- -where tp and 4’ are the boiling points of a liquid under the pressuresp and p’ respectively, and t;l and t;l’ those of another liquid under thesame pressures, while q and 4’ are constants depending upon the twoliquids. R. R.Volume Relations of some HaloYd Salts. By W. MGLLXRERZBACH (Ber., 13, 1658-1660) .-The author has previously pointedout that the contraction taking place when chlorine, bromine, and iodinecombine with metals is most considerable in t’he case of chlorine, andleast with iodine. He now confirms his prerious observations by cal-culating the contraction from a number of new data obtained byvarious observers. These are given in the following table :-Name ofsalt.RbCl . . .RbBr..RbI . . . .LiC1.. . .LiBr . . .LiI.. . . .CdI,. . . . CdC12. # . -C.Calc.volume.81 -781 .781 *’737’437 *437 -464 *264 *2 -B D = -. AVolnmefound.55 .o59 ‘870 ‘021 ‘228 -138 *546 -561 -0C-DCContrac-tion.0 9 20.270 -140 -4.30 -25- 0 ‘030.270 *05F =-.---0. H.9

ISSN:0368-1769    

DOI:10.1039/CA8814000069

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

72 ABSTRACTS OF CHEMICAL PAPERS. I n o r g a n i c C h e mi s t r y. A Source of Atmospheric Carbonic Anhydride. By M. S . MEUNIER (Bied. Centr., 1880, 633-634) .-According to Cloez, iron which contains carbon and manganese yields carbonic anhydride on treatment with hot water ; this reaction may be assumed to go on in the neighbourhood of hot springs in metnlliferous districts, and thus to be a source of atmospheric carbonic anhydride. J. K. C. Id Liquid Sulphur Phosphide. By H. SCHULZE (J.pr. Chem. [2 22, 113-130) .-After referring to the experiments of Berzelius &n Rumme (Ber., 12, 1350), the latter of whom observed that there was no rise of temperature when phosphorus and sulphur were combined under warm water, and that on distilling the liquid product with steam, phosphorus passes over, leaving sulphur with a smaller propor- tion of phosphorus behind.The aiithor says he has repented the experiments and can confirm these observations, for not only was there no rise, but there was a slight fall of temperature on bringing sulphur and phosphorus together under water at 20". On cooling the liquid of the composition PIS, it was found to deposit crystals of phosphorus which redissolved when the temperature rose to 15", but separated out on again cooling. Liquid P,S deposited sulphur crystals. Wicke (Ann. Chenz. Pharm., 86, 115) had found that sulphur dissolved in P,S is deposited again on long standing in a cool place. Contrary to what is stated by Berzelius, the author finds that phosphorus rolatilises, when heated at 100" in a stream of hydrogen, whilst the hydrogen is partly converted into phosphine.The author did not succeed in effecting complete separation in this manner, as sometimes below and sometimes above lOO", a reaction took place in the liquid, causing an explosion. After a less violent reaction he has, however, occasionally succeeded, by very gradually heating small quantities in the paraffin-bath, in removing phosphorus, far below its boiling point, in a current of carbonic anhydride, and obtaining a residue of solid sulphur phosphide. The author finds, contrary to Gmelin-Kraut's notice, that carbon bisulphide is incapable of dissolving out the phosphorus from the sulphur ; but he succeeded in effecting a partial separation by dissolv- ing in carbon bisulphide, and then agitating the concentrated solution with alcohol, ether, chloroform, light petroleum, or other liquids, miscible with carbon bisulphide, but of slight solvent power for sul- phur, when most of the sulphur is separat.ed, and a liquid produced containing more or less sulphur in solution, according t o the amount of carbon bisulphide present.Phosphorus is also precipitated from its solution in carbon bisulphide by these reagents, so that it is only at first that pure sulphur is deposited. R. Bottger (J. pr. Chem., 12, 358) found that by shaking trans- parent phosphorus with potassium pdysulphide, and nllo wing it to stand for four days in a dark place, transparent sulphurphosphide wasINORGANIC CHEMISTRY. 73 produced. This the author can confirm, as also the decomposition of hydrogen persulphide by transparent phosphorus.In reviewing the facts as thus presented, it would seem that these sulphur phosphides are not chemical compounds, as there is no evolu- tion of heat on their formation, moreover they are readily decomposed by lowering the temperature, by solvents, and by heating in a current of gas. The decomposition of the potassium polysulphides and of hydro- gen persulphide by phosphorus seems to point the other way, but simi- lar actions are seen in crystalline salts giving up their water of crys- tallisation to the air, and the fact observed by Schone (Gmelin-Kraut, 2, 38), that alcohol precipitates potassium t'etrasulphide from a con- centrated solution of the pentasulphide, dissolving sulphur (and poly- sulphide).Since neither phosphorus nor sulphur by itself can decompose water, it seems remarkable that, a simple mixture of the two should have the power. But there are several examples which show that two bodies acting in common on a third, need by no means be combined. The action of chlorine and carbon on alumina is a case in point. The lique- faction of solid salts soluble in water, by contact with ice, is perfectly analogous to the formation of the liquid sulphur phosphide from its elements. F. L. T. The Earths of Samarskite. By C. MARIGNAC (Ann. Chim. Phys. [ S ] , 20, 535--557).-1n this memoir, the author describes only those oxides which form nitrates of relative high stability, and have been separated from those oxides, such as erbia, ytterbia, &c., which form nitrates easily decomposed by heat.They have been separated one from another by taking advantage of the different solubilities uf their double sulphates with potassium in a saturated solution of potassium sdphate. Details of this and other methods of separation employed, are given. The earths present in samarskite (from North America,) were thus divided into four groups :- I . Double Sulphates Soluble in less than 100 vob. of K,S04 Solution. Molecdar weight rises to 119.-Ytt.ria and terbia, with traces of the oxides of decipium and didymium, and probably traces of the oxide of Y a found in Group 11. The terbia, even after strong ignition, had a faint chamois tint, which disappeared on heating in a current of hydrogen, and reappeared when the oxide was again heated in the presence of air.These changes of colour were accompanied by very alight rariations in weight. 11. Double Subhates soluble in 100-200 ~01.9. of K,S04 Solution. Molecula?. weight varies between 119 and 120.-This portion consisted mainly of the oxide of a metal which the author provisionally desig- nates Ya. I t s molecular weight is about 120.5, a maximum between the molecular weights of those earths which most nearly approach it in their behaviour with potassium.sulphate solution. It forms colour- less salts, the solutions of which show no absorption spectrum. It is distinguished from all tbe metals of this class except yttrium and ytterbium by the very faint orange-yellow colour of its oxide, and by the fact that its salts show no absorption spectrum: from yttrium by the sparing solubility of its formate, and of its double potassium74 ABSTRACTS OF CHEMICAL PAPERS. sulphate ; from ytterbium by the much greater stability of its nitrate, and the ease with which the ignited oxide dissolves in dilute acids.Yr, is probably identical with that base, the'existence of which has been indicated by Delafontaine (Compt. rend., 90). Mole- culur weight falls from 119 to 115 as the Solubility decreases.-This group contains the oxide of Ya, a small quantity of the oxide of didymium which cannot be completely separated, and the oxide of a metal of Yp, which forms a nitrate readily decomposed by heat, but is included in this group, because its double potassium sulphate is very sparingly soluble in K,S04 solution.The molecular weight of the oxide of Y/3 is probably somewhat lower than 115.6. Its sulphate forms small, short, crystals similar to those of the sulphates of yttrium and didymium, but of a sulphur-yellow colour ; they have the constitution- 111. Dozd2.e Xulphates very slightly soluble in K,S04 Solution. 3(YP0.S03) + 8H,O. Solutions of the salts of this base give a well-defined absorption spectrum which closely resembles that ascribed by Delafontaine to decipium, or, still more closely, that described by Boisbaudran as peculiar to the new element samarium. Since these three bodies were obtained from samarskite by the same methods, it is probable that they are essentially one and the same substance. The molecular weight of the oxide of decipium is, howeber, according to Delafontaine, 130, whilst that of the oxide of YB is below 115.6.Further, the salts of decipium are colourless, those of Y have a yellow colour, the intensity of which increases the further the purification is carried. Probably either the substance obtained by Delafontaine is mixed with a considerable pro- portion of some other base having a high molecnlar weight, or that, obtained by the author contains a base forming yellow salts, a d having a much lower molecular weight. Further investigations are necessary to decide this point. IV. Double Sulphates irmlu hle in K2S04 Solution.-This group con- tained only didymium, which, however, could not be completely puri- fied from traces of other metals. Some of the products, pa,rticularly those most soluble in R,SO, solu- tion, contained traces of a substance which formed a yellowish oxide and is probably identical with the philippium of Delafontaine.The author has attempted to determine the relative solubilities of the formates of the metals present in samarskite and similar minerals, but without success. The solubility of these salts varies very greatly with the mechanical treatment to which they are subjected, and their solutions readily assume a state of supersaturation which they retain for a considerable length of time, even when in contact with the solid salt. C. H. B. metallic Oxides of the Iron Group. By H. MOISSAN (AWL. Chim. Phya. [ 51, 21, 199-255).--lron.-The black pyrophoric powder obtained by heating ferrous oxalate, or ferric oxide in a current of hydrogen or carbonic oxide, consists of ferrous oxide, a d contains TLO nietallic iron, or only traces.INORGANIC CHEMISTRY.75 The reduction of ferric oxide in a current of hydrogen commences a little above 330" ; between this temperature and the boiling point of sulphur, 440", the product is triferric tetroxide, Fe304. The same oxide is obtained when hydrated or anhydrous ferric oxide is heated to the melting point of zinc, 420°, in a current of pure and dry car- bonic oxide. If the carbonic oxide contains carbonic anhydride, a small quantity of ferruginous carbon is deposited. Between 500" and 600" ferrous oxide FeO, pyrophoric a t ordinary temperatures, is ob- tained. The results are the same even if the ferric oxide be mixed with a considerable proportion of alumina. By heating ferrous oxide to the softening point of glass in a current of hydrogen, metallic iron is obtained, but it is more or less agglutinated and is not pyrophoric.It is evident that the reduction of ferric oxide to metallic iron takes place in well-defined stages. When ferric oxide is heated to dull red- ness in a current of carbonic oxide, a more or less agglutinated powder is obtained, which is not pyrdphoric, and dissolves in dilute sulphuric acid with evolution of hydrogen, leaving a residue of carbon. Pyro- phoric metallic iron may, however, be obtained by heating ferric oxide in a current of perfectly dry hydrogen at 440" for a very long time, i e . , several days ; or by distilling iron amalgam at the lowest possible temperature. In all these cases of reduction, it is necessary, in order to obtain good results, that the reducing gas should be as pure and as dry as possible, and the current should be somewhat rapid.In addition to the methods above dcscribed, ferrous oxide may be prepared by heating ferrous oxalate out of contact with the air. That the pyrophoric black powders obtained in these experiments and shown by analysis to correspond in composition with FeO were really ferrous oxide, and not mixtures of triferric tetroxide with metallic iron was proved by the fact that they gave no hydrogen when treated with dilute acids, and did not decolorise an aqueous solution of iodine. When ferrous carbonate is heated out of contact with air, triferric tetroxide, Fe,04, is formed. Now, when carbonic anhydride is passed over heated ferrous oxide, carbonic oxide and triferric tetroxide are produced. It is probable therefore that the ferrous carbonate first splits up into ferrous oxide and carbonic anhydride, which react on each other in accordance with the equation 3Fe0 + CO, = Fe304 + CO.If the ferrous carbonate be heated slowly in a current of nitrogen, ferric oxide is formed: if rapidly heated, a small quantity of pyro- pboric ferrous oxide is produced. Allotropic ModiJicution of Triferric Tetyoxide.-In addition to the methods described above, triferric tetroxide may be obtained by heat- ing ferric oxide, or metallic iron reduced by hydrogen, to redness in a current of hydrogen saturated with aqueous rapour a t 90" ; by heating ferrous carbonate to dull redness in a currertt of carbonic anhydride; and by heating reduced iron in a current of carbonic anhydride at 440".As thus prepared a t low temperatures, it is a black magnetic powder, density 4.86, is readily attacked by concen- trated nitric acid, and when heated becomes incandescent, forming Fea03. This is one modification of triferric tetroxide. When the ferric oxide produced by heating this modification is exposed to a high tempcratnre, about 1500c, it gives off oxygen, and is reconverted into76 ABSTRAOTS OF CHEMICAL PAPERS. triferric tetroxide, a black magnetic substance, sp. gr. 5 to 5.09, almost unattacked by boiling concentrated nitric acid, and not forming ferric oxide when heated ; it is, in fact, the most stable oxide of iron. When the first modification of the triferric tetroxide is heated to whiteness in a current of nitrogen, it agglomerates, increases in deiisity, no longer forms Fe,O, when heated, and has all the properties of the second modification.It is evident that there are two well-defined allotropic forms of triferric tetroxide, one formed a t low, the other at high temperatures. The author explains the fact that the modifica- tion ,8 formed at high temperatures does not give ferric oxide when heated, by assumifig that when the modification a, formed a t low tem- peratures, is converted into ferric oxide, the heat evolved is less than that evolved when the modification a is converted into the modifica- tion 6, and therefore the formation of ferric oxide from the latter would be an endothermic reaction.Allotropic Modijicatiow of -Ferrous Oxide.-When prepared a t tem- peratures below GOO", ferrous oxide is a pulverulent, ivory-black sub- stance, which readily burns in the air, forming Fe203, the temperature of the combustion being sufficiently high to convert a portion of the Fe,O, into Fe304. It is oxidised with incandescence by nitric acid, burns, when gently heated in nitrogen monoxide or dioxide, displaces ammonia from its combinations, and decomposes water slowly a t ordinary temperatures, more rapidly a t 100". If, however, it be ob- tained a t a high temperature, as for example, by heating reduced iron in a current of carbonic anhydride, it is not pyrophoric a t ordinary temperatures, and is converted into triferric tetroxide when burnt. When pyrophoric ferrous oxide is heated in an atmosphere of nitrogen to the melting point of silver, it loses its pyrophoric properties, is not attacked by dilute acetic acid, and when heated burns like tinder, forming Fe304.Further, when the modification of ferrous oxide formed a t low temperatures is heated in a current of carbonic anhy- dride, it is converted into the low temperature modificat'ion of triferric tetroxide, but the high temperature modification of ferrous oxide, when heated, gives the k3 or high temperature modification of triferric tetroxide. 1Cfmgal.~ese.-When manganese dioxide, obtained by calcining man- ganous nitrate, is heated at 280" in a current of hydrogen, it becomes incandescent, and is reduced to the monoxide MnO. The reduction of the dioxide commences at 230", and if the temperature is kept constant at this point, manganese sesquioxide, Mn203, having a deep maroon colour: is obtained.At a somewhat higher temperature trimanganic tetroxide, Mn,04, is formed, and this, when carefully heated in the presence of air, is converted into the sesquioxide which, when strongly heated, gives trimanganic tetroxide, unalterable by heating in contact with air. When the trimanganic tetroxide obtained at a low tempera- ture is heated a t 260" in a current of pure and dry hydrogen, it is rapidly reduced with formation of the monoxide, a green powder which oxidises rapidly, and if previously heated to 140" takes fire when thrown into the air. Out of contact with air, this oxide is but slightly acted on by water, but in presence of air it quickly oxidises.A non- pyrophoric variety of the monoxide has been obtained by Deville inINORGANIC CREMISTRY. 77 regular octohedra of a beautiful green tint, by reducing a higher oxide a t a red heat in a current of hydrogen containing hydrochloric acid. When the crystalline amalgam of manganese obtained by electro- lysis, is distilled a t 440" in a current of pure hydrogen, a light, porous, blackish grey mass of metallic manganese is left. It is oxidised with incandescence by nitric acid, and portions of it take fire when thrown into the air. Nickel.-Hydrated or anhydrous nickel sesquioxide, Ni203, heated a t 190" in a current of hydrogen, is reduced to the grey magnetic oxide, Ni,O,. At ZL somewhat higher temperature the yellowish-green monoxide is obtained.This undergoes no further change at 200", but at 230-240" is reduced to metallic nickel, in the form of a black powder, which is pyrophoric at ordinary temperatures, but does not burn so brilliantly a s metallic iron reduced at 440". That the tem- perature of combustion is not very high is shown by the fact that the product consists mainly of the sesquioxide, whereas the only oxide stable a t a high temperature is the monoxide. When nickel amalgam is distilled in a current of hydrogen a t the lowest possible temperature, the nickel obtained is not pyrophoric. Nickel monoxide obtained by reduction is green when cold, yellow when hot. It readily absorbs oxygen even a t ordinary temperatures, and is partially converted by nitric acid, with elevation of tempera- ture, into the sesquioxide, which dissolves in acids with evolution of oxygen.The monoxide when heated in air or oxygen to 350-440", forms a blackish powder, the composition of which depends on the temperature ; at 600" this black powder is reconverted into the mon- oxide, showing that the higher oxides of nickel can only exist below a certain temperature. Nickel monoxide dissolves in hydrochloric and sulphuric acids, with rise of temperature ; it forms a beautiful violet solution with ammonia, and displaces ammonia from its salts. Cob&.-The sesquioxide is reduced a t the same temperature as nickel sesquioxide, viz., 190-200". A t 250" metallic cobalt is ob- tained in the form of a black powder, which takes fire a t ordinary temperatures, forming mainly the oxide Co304.If the reduction takes place a t 700°, the metallic cobalt is never pyrophoric ; and the metal obtained by distilling the amalgam in hydrogen at the lowest possible temperature behaves in the same way Cobalt monoxide obtained by reduction is a dark colonred, readily oxidisable powder, which when slightly heated in presence of air, becomes incandescent, and is converted into the sesquioxide. The sesquioxide at a higher temperature forms the magnetic oxide, Cos04, and this when still further heated gives the monoxide, COO, the oxide stable a t high temperatures. Chromium.-The sesquioxide is not reduced by hydrogen at any known temperature. When strongly heated, it becomes incandescent', and is rendered almost insoluble in acids.The ignited oxide when heated a t 440" in a current of hydrogen sulphide, dry chlorine, oxygen, or bromine vapour, undergoes no change whatever. When the non-ignited oxide is heated at 440" in a current of hydro- gen sulphide, it forms chromium sesquisulphide, the properties of which have been previously described by the author (this Journal,78 ABSTRACTS OF CHEMICAL PAPERS. Abstr., 1880, 527). Heated in a current of oxygen, the sesquioxide is oxidised to the dioxide, CrOz, as already pointed out by Kriiger. This dioxide has a deep grey colour, and when calcined evolves oxygen and is reconverted into the sesquioxide. When heated with hydrochloric acid or a mixture of snlphuric acid and sodium chloride, chlorine is given off. Fused with potash, out of contact with air, it gives potas- sium chromate and chromium sesquioxide.When the hydrated sesquioxide is gradually heated in a current of chlorine, it first loses water, and at 440" is converted into chromyl dichloride. The dehydrated but not ignited sesquioxide is partially converted into chromic chloride, but no chromyl dichloride is formed ; if, however, the chlorine be saturated with aqueous vapour a t 8- lo", the latter compound is formed in considerable quantity. I f the chlorine be saturat,ed with aqueous vnpour at 20°, but little chromyl dichloride is produced. Chromyl dichloride is also formed when a current of moist chlorine is passed over chromic chloride heated a t 440°, but a moist inert gas, such as carbonic anhydride, does not pro- duce this change. Further, it is found that the hydrated sesquioxide when dried at 440" contains 5-10 per cent.of water. Probably in all these cases chromic chloride i s first formed, and then decomposed with production of chromyl dichloride, by the excess of chlorine, and the water present either in the gas or in the oxide. By arresting the action of moist chlorine on the chromium sesqui- oxide a t the moment when the red vapours of Cr02Clz are given off, a brown powder is obtained, which approaches in composition the oxy- chlorides described by Moberg. Bromine vapour, under the same conditions, also attacks the non- ignited chromium sesquioxide. Chromium amalgam may be obtained by the action of sodium amal- gam on the chloride, bromide, or iodide of chromium. Like the amalgams of all the metals of this gronp, it oxidises readily.When distilled in a current of hydrogen a t the lowest possible temperature, metallic chromium is left in the form of a black, amorphous, very slightly agglutinated substance, which takes fire when exposed to the air. If distilled at temperatures above 355", the residual chromium is not, pyrophoric. The chromium thus obtained is more readily oxidised, and is more soluble in acids than that obtained by Deville by reducing the sesquioxide with carbon. When heated to dull redness in a carrent of dry carbonic anhydride, it is converted into the sesquioxide. If this family of elements be arranged in the order, chromium, manganese, iron, cobalt, nickel, their affinity for oxygen and the heats of formation of the oxides, chlorides, bromides, iodides, and sulphides decrease as the atomic weight increases.Atomic Weight of Antimony. By R. SCHNEIDER (J. pr. Chem [: 21, 22,131-147).-A controversial paper in reply to strictures passed by Kessler on the author's results. The ant'hor, together with Cooke, finds 120 as the atomic weight; Ressler, in common with Dexter and Dumas, obtains 122. The author's method is by reduction of a pure specimen of antimony C. H. B.INORQANIC CHEMISTRY. 79 glance by hydrogen, and in 1856 (Pogg. AWL., 98,293-308) obtained 120.3 by this means. The author gives three recent determinations made on the same plan, and with an antimony glance containing- Insoluble residue Antimony sulphide. (quartz). Calcium carbonate. Ferrous sulphide. 99-81 1 0-108 0-048 0.033 As on heating it in a current of hydrogen or carbonic anhydride it decrepitated, giving out a slight empyreumatic odour, it was heated before reduction in hydrogen to 290-320” until decrepitation had ceased and thg issuing gas was odourless.Antimony sulphide itself undergoea no reduction at this temperature. The mean result from the three experiments is 120.182, which com- pares well with 120.3, the one previously obtained. Dexter, like Berzelius, determined the atomic weight by oxidation of the metal with nitric acid and ignition of the residue. The suppo- sition that the residue on ignition is a thoroughly stable body of the composition of antimony tetroxide is incorrect, as Bunsen has shown (Annalem, 192, 317). Kessler’s method (Pogg. Anw,., 95,204 (1855), and 113,134 (1861)) is to oxidise antimonious chloride in concentrated hydrochloric acid b-y a volumet,ric solution of potassium dichromate in excess, and to add, after dilution of the solution, an excess of ferrous chloride and then titrate back the excess of ferrobs chloride by chromium solution.I n 1855 he obtained the atomic weight, 123.7, and in 1861 one experi- ment with antimony, one with antimony trioxide, and a third with antimonious chloride, gave 122.29. The author criticises Kessler’s method, and infers that no reliance is to be placed on it. Products of Decomposition and Metamorphosis of Uranyl Sulphide. By C. Z~MMERMANN (AnnuZen, 204-2’24) .-Uranium does not exhibit a great affinity f o r sulphur, since uranyl sulphide is con- verted into uranyl hydroxide by washing with warm water.It has been noticed by Reme16 (Pogg. Ann., 124, 120) that when uranyl sul- phide is left in contact with ammonium sulphide the liquid becomes of a brown to deep black colour. The author shows that this is due to the solubility of the uranyl sulphide i n ammonium carbonate con- tained in the ammonium sulphide. When precipitated uranyl sulphide is left for a long time in contact with ammonium sulphide in the cold, two bodies are obtained, one red the other black. The author shows that when the ammonium sulphide contains a considerable amount of thiosulphate the red body is formed, but that in absence of thio- sulphate the black body is obtained. The thiosulphate is formed by the action of atmospheric oxygen on the ammonium snlphide.The formula assigned to uranium-black is Ur,O,< O>Ur + 2Ur,0,. Uranium-red seems to consist of an oxygen-compound which contains, besides sulphur, a second base (potassium, sodium, ammonium, 01’ barium), and some uranium, probably as uranyl sulphide. Anhydrous F. L. T. 080 ABSTRACTS OF CHEMICAL PAPERS. uranium-red, on the assumption that it is perfectly free from admixture, OK may be formulated thus : U6SK209 = 2Ur203 + UrzOz< SK. G. T, A.72 ABSTRACTS OF CHEMICAL PAPERS.I n o r g a n i c C h e mi s t r y.A Source of Atmospheric Carbonic Anhydride. By M. S .MEUNIER (Bied. Centr., 1880, 633-634) .-According to Cloez, ironwhich contains carbon and manganese yields carbonic anhydride ontreatment with hot water ; this reaction may be assumed to go on inthe neighbourhood of hot springs in metnlliferous districts, and thus tobe a source of atmospheric carbonic anhydride. J.K. C.Id Liquid Sulphur Phosphide. By H. SCHULZE (J.pr. Chem. [222, 113-130) .-After referring to the experiments of Berzelius &nRumme (Ber., 12, 1350), the latter of whom observed that there wasno rise of temperature when phosphorus and sulphur were combinedunder warm water, and that on distilling the liquid product withsteam, phosphorus passes over, leaving sulphur with a smaller propor-tion of phosphorus behind. The aiithor says he has repented theexperiments and can confirm these observations, for not only was thereno rise, but there was a slight fall of temperature on bringing sulphurand phosphorus together under water at 20".On cooling the liquidof the composition PIS, it was found to deposit crystals of phosphoruswhich redissolved when the temperature rose to 15", but separated outon again cooling. Liquid P,S deposited sulphur crystals. Wicke(Ann. Chenz. Pharm., 86, 115) had found that sulphur dissolved inP,S is deposited again on long standing in a cool place.Contrary to what is stated by Berzelius, the author finds thatphosphorus rolatilises, when heated at 100" in a stream of hydrogen,whilst the hydrogen is partly converted into phosphine. The authordid not succeed in effecting complete separation in this manner, assometimes below and sometimes above lOO", a reaction took place inthe liquid, causing an explosion. After a less violent reaction he has,however, occasionally succeeded, by very gradually heating smallquantities in the paraffin-bath, in removing phosphorus, far below itsboiling point, in a current of carbonic anhydride, and obtaining aresidue of solid sulphur phosphide.The author finds, contrary to Gmelin-Kraut's notice, that carbonbisulphide is incapable of dissolving out the phosphorus from thesulphur ; but he succeeded in effecting a partial separation by dissolv-ing in carbon bisulphide, and then agitating the concentrated solutionwith alcohol, ether, chloroform, light petroleum, or other liquids,miscible with carbon bisulphide, but of slight solvent power for sul-phur, when most of the sulphur is separat.ed, and a liquid producedcontaining more or less sulphur in solution, according t o the amountof carbon bisulphide present. Phosphorus is also precipitated from itssolution in carbon bisulphide by these reagents, so that it is only atfirst that pure sulphur is deposited.R. Bottger (J.pr. Chem., 12, 358) found that by shaking trans-parent phosphorus with potassium pdysulphide, and nllo wing it tostand for four days in a dark place, transparent sulphurphosphide waINORGANIC CHEMISTRY. 73produced. This the author can confirm, as also the decomposition ofhydrogen persulphide by transparent phosphorus.In reviewing the facts as thus presented, it would seem that thesesulphur phosphides are not chemical compounds, as there is no evolu-tion of heat on their formation, moreover they are readily decomposedby lowering the temperature, by solvents, and by heating in a currentof gas.The decomposition of the potassium polysulphides and of hydro-gen persulphide by phosphorus seems to point the other way, but simi-lar actions are seen in crystalline salts giving up their water of crys-tallisation to the air, and the fact observed by Schone (Gmelin-Kraut,2, 38), that alcohol precipitates potassium t'etrasulphide from a con-centrated solution of the pentasulphide, dissolving sulphur (and poly-sulphide).Since neither phosphorus nor sulphur by itself can decompose water,it seems remarkable that, a simple mixture of the two should have thepower. But there are several examples which show that two bodiesacting in common on a third, need by no means be combined.Theaction of chlorine and carbon on alumina is a case in point. The lique-faction of solid salts soluble in water, by contact with ice, is perfectlyanalogous to the formation of the liquid sulphur phosphide from itselements. F. L. T.The Earths of Samarskite. By C. MARIGNAC (Ann. Chim. Phys.[ S ] , 20, 535--557).-1n this memoir, the author describes only thoseoxides which form nitrates of relative high stability, and have beenseparated from those oxides, such as erbia, ytterbia, &c., which formnitrates easily decomposed by heat. They have been separated onefrom another by taking advantage of the different solubilities uf theirdouble sulphates with potassium in a saturated solution of potassiumsdphate.Details of this and other methods of separation employed,are given. The earths present in samarskite (from North America,)were thus divided into four groups :-I . Double Sulphates Soluble in less than 100 vob. of K,S04 Solution.Molecdar weight rises to 119.-Ytt.ria and terbia, with traces of theoxides of decipium and didymium, and probably traces of the oxide ofY a found in Group 11. The terbia, even after strong ignition, had afaint chamois tint, which disappeared on heating in a current ofhydrogen, and reappeared when the oxide was again heated in thepresence of air. These changes of colour were accompanied by veryalight rariations in weight.11. Double Subhates soluble in 100-200 ~01.9. of K,S04 Solution.Molecula?. weight varies between 119 and 120.-This portion consistedmainly of the oxide of a metal which the author provisionally desig-nates Ya. I t s molecular weight is about 120.5, a maximum betweenthe molecular weights of those earths which most nearly approach itin their behaviour with potassium.sulphate solution.It forms colour-less salts, the solutions of which show no absorption spectrum. It isdistinguished from all tbe metals of this class except yttrium andytterbium by the very faint orange-yellow colour of its oxide, and bythe fact that its salts show no absorption spectrum: from yttrium bythe sparing solubility of its formate, and of its double potassiu74 ABSTRACTS OF CHEMICAL PAPERS.sulphate ; from ytterbium by the much greater stability of its nitrate,and the ease with which the ignited oxide dissolves in dilute acids.Yr, is probably identical with that base, the'existence of which hasbeen indicated by Delafontaine (Compt.rend., 90).Mole-culur weight falls from 119 to 115 as the Solubility decreases.-Thisgroup contains the oxide of Ya, a small quantity of the oxide ofdidymium which cannot be completely separated, and the oxide of ametal of Yp, which forms a nitrate readily decomposed by heat, but isincluded in this group, because its double potassium sulphate is verysparingly soluble in K,S04 solution. The molecular weight of the oxideof Y/3 is probably somewhat lower than 115.6. Its sulphate formssmall, short, crystals similar to those of the sulphates of yttrium anddidymium, but of a sulphur-yellow colour ; they have the constitution-111. Dozd2.e Xulphates very slightly soluble in K,S04 Solution.3(YP0.S03) + 8H,O.Solutions of the salts of this base give a well-defined absorptionspectrum which closely resembles that ascribed by Delafontaine todecipium, or, still more closely, that described by Boisbaudran aspeculiar to the new element samarium.Since these three bodies wereobtained from samarskite by the same methods, it is probable that theyare essentially one and the same substance. The molecular weight ofthe oxide of decipium is, howeber, according to Delafontaine, 130, whilstthat of the oxide of YB is below 115.6. Further, the salts of decipiumare colourless, those of Y have a yellow colour, the intensity of whichincreases the further the purification is carried.Probably either thesubstance obtained by Delafontaine is mixed with a considerable pro-portion of some other base having a high molecnlar weight, or that,obtained by the author contains a base forming yellow salts, a dhaving a much lower molecular weight. Further investigations arenecessary to decide this point.IV. Double Sulphates irmlu hle in K2S04 Solution.-This group con-tained only didymium, which, however, could not be completely puri-fied from traces of other metals.Some of the products, pa,rticularly those most soluble in R,SO, solu-tion, contained traces of a substance which formed a yellowish oxideand is probably identical with the philippium of Delafontaine.The author has attempted to determine the relative solubilities ofthe formates of the metals present in samarskite and similar minerals,but without success.The solubility of these salts varies very greatlywith the mechanical treatment to which they are subjected, and theirsolutions readily assume a state of supersaturation which they retainfor a considerable length of time, even when in contact with the solidsalt. C. H. B.metallic Oxides of the Iron Group. By H. MOISSAN (AWL.Chim. Phya. [ 51, 21, 199-255).--lron.-The black pyrophoric powderobtained by heating ferrous oxalate, or ferric oxide in a current ofhydrogen or carbonic oxide, consists of ferrous oxide, a d contains TLOnietallic iron, or only tracesINORGANIC CHEMISTRY. 75The reduction of ferric oxide in a current of hydrogen commences alittle above 330" ; between this temperature and the boiling point ofsulphur, 440", the product is triferric tetroxide, Fe304.The sameoxide is obtained when hydrated or anhydrous ferric oxide is heatedto the melting point of zinc, 420°, in a current of pure and dry car-bonic oxide. If the carbonic oxide contains carbonic anhydride, asmall quantity of ferruginous carbon is deposited. Between 500" and600" ferrous oxide FeO, pyrophoric a t ordinary temperatures, is ob-tained. The results are the same even if the ferric oxide be mixedwith a considerable proportion of alumina. By heating ferrous oxideto the softening point of glass in a current of hydrogen, metallic ironis obtained, but it is more or less agglutinated and is not pyrophoric.It is evident that the reduction of ferric oxide to metallic iron takesplace in well-defined stages.When ferric oxide is heated to dull red-ness in a current of carbonic oxide, a more or less agglutinated powderis obtained, which is not pyrdphoric, and dissolves in dilute sulphuricacid with evolution of hydrogen, leaving a residue of carbon. Pyro-phoric metallic iron may, however, be obtained by heating ferric oxidein a current of perfectly dry hydrogen at 440" for a very long time,i e . , several days ; or by distilling iron amalgam at the lowest possibletemperature. In all these cases of reduction, it is necessary, in orderto obtain good results, that the reducing gas should be as pure and asdry as possible, and the current should be somewhat rapid.In addition to the methods above dcscribed, ferrous oxide may beprepared by heating ferrous oxalate out of contact with the air.Thatthe pyrophoric black powders obtained in these experiments andshown by analysis to correspond in composition with FeO were reallyferrous oxide, and not mixtures of triferric tetroxide with metallic ironwas proved by the fact that they gave no hydrogen when treated withdilute acids, and did not decolorise an aqueous solution of iodine.When ferrous carbonate is heated out of contact with air, triferrictetroxide, Fe,04, is formed. Now, when carbonic anhydride is passedover heated ferrous oxide, carbonic oxide and triferric tetroxide areproduced. It is probable therefore that the ferrous carbonate firstsplits up into ferrous oxide and carbonic anhydride, which react oneach other in accordance with the equation 3Fe0 + CO, = Fe304 + CO.If the ferrous carbonate be heated slowly in a current of nitrogen,ferric oxide is formed: if rapidly heated, a small quantity of pyro-pboric ferrous oxide is produced.Allotropic ModiJicution of Triferric Tetyoxide.-In addition to themethods described above, triferric tetroxide may be obtained by heat-ing ferric oxide, or metallic iron reduced by hydrogen, to rednessin a current of hydrogen saturated with aqueous rapour a t 90" ; byheating ferrous carbonate to dull redness in a currertt of carbonicanhydride; and by heating reduced iron in a current of carbonicanhydride at 440".As thus prepared a t low temperatures, it is ablack magnetic powder, density 4.86, is readily attacked by concen-trated nitric acid, and when heated becomes incandescent, formingFea03. This is one modification of triferric tetroxide.When the ferricoxide produced by heating this modification is exposed to a hightempcratnre, about 1500c, it gives off oxygen, and is reconverted int76 ABSTRAOTS OF CHEMICAL PAPERS.triferric tetroxide, a black magnetic substance, sp. gr. 5 to 5.09, almostunattacked by boiling concentrated nitric acid, and not forming ferricoxide when heated ; it is, in fact, the most stable oxide of iron. Whenthe first modification of the triferric tetroxide is heated to whitenessin a current of nitrogen, it agglomerates, increases in deiisity, nolonger forms Fe,O, when heated, and has all the properties of thesecond modification.It is evident that there are two well-definedallotropic forms of triferric tetroxide, one formed a t low, the other athigh temperatures. The author explains the fact that the modifica-tion ,8 formed at high temperatures does not give ferric oxide whenheated, by assumifig that when the modification a, formed a t low tem-peratures, is converted into ferric oxide, the heat evolved is less thanthat evolved when the modification a is converted into the modifica-tion 6, and therefore the formation of ferric oxide from the latterwould be an endothermic reaction.Allotropic Modijicatiow of -Ferrous Oxide.-When prepared a t tem-peratures below GOO", ferrous oxide is a pulverulent, ivory-black sub-stance, which readily burns in the air, forming Fe203, the temperatureof the combustion being sufficiently high to convert a portion of theFe,O, into Fe304.It is oxidised with incandescence by nitric acid,burns, when gently heated in nitrogen monoxide or dioxide, displacesammonia from its combinations, and decomposes water slowly a tordinary temperatures, more rapidly a t 100". If, however, it be ob-tained a t a high temperature, as for example, by heating reduced ironin a current of carbonic anhydride, it is not pyrophoric a t ordinarytemperatures, and is converted into triferric tetroxide when burnt.When pyrophoric ferrous oxide is heated in an atmosphere of nitrogento the melting point of silver, it loses its pyrophoric properties, is notattacked by dilute acetic acid, and when heated burns like tinder,forming Fe304.Further, when the modification of ferrous oxideformed a t low temperatures is heated in a current of carbonic anhy-dride, it is converted into the low temperature modificat'ion of triferrictetroxide, but the high temperature modification of ferrous oxide,when heated, gives the k3 or high temperature modification of triferrictetroxide.1Cfmgal.~ese.-When manganese dioxide, obtained by calcining man-ganous nitrate, is heated at 280" in a current of hydrogen, it becomesincandescent, and is reduced to the monoxide MnO. The reduction ofthe dioxide commences at 230", and if the temperature is kept constantat this point, manganese sesquioxide, Mn203, having a deep marooncolour: is obtained.At a somewhat higher temperature trimanganictetroxide, Mn,04, is formed, and this, when carefully heated in thepresence of air, is converted into the sesquioxide which, when stronglyheated, gives trimanganic tetroxide, unalterable by heating in contactwith air. When the trimanganic tetroxide obtained at a low tempera-ture is heated a t 260" in a current of pure and dry hydrogen, it israpidly reduced with formation of the monoxide, a green powder whichoxidises rapidly, and if previously heated to 140" takes fire whenthrown into the air. Out of contact with air, this oxide is but slightlyacted on by water, but in presence of air it quickly oxidises. A non-pyrophoric variety of the monoxide has been obtained by Deville iINORGANIC CREMISTRY.77regular octohedra of a beautiful green tint, by reducing a higher oxidea t a red heat in a current of hydrogen containing hydrochloric acid.When the crystalline amalgam of manganese obtained by electro-lysis, is distilled a t 440" in a current of pure hydrogen, a light, porous,blackish grey mass of metallic manganese is left. It is oxidised withincandescence by nitric acid, and portions of it take fire when throwninto the air.Nickel.-Hydrated or anhydrous nickel sesquioxide, Ni203, heateda t 190" in a current of hydrogen, is reduced to the grey magneticoxide, Ni,O,. At ZL somewhat higher temperature the yellowish-greenmonoxide is obtained. This undergoes no further change at 200", butat 230-240" is reduced to metallic nickel, in the form of a blackpowder, which is pyrophoric at ordinary temperatures, but does notburn so brilliantly a s metallic iron reduced at 440".That the tem-perature of combustion is not very high is shown by the fact that theproduct consists mainly of the sesquioxide, whereas the only oxidestable a t a high temperature is the monoxide.When nickel amalgam is distilled in a current of hydrogen a t thelowest possible temperature, the nickel obtained is not pyrophoric.Nickel monoxide obtained by reduction is green when cold, yellowwhen hot. It readily absorbs oxygen even a t ordinary temperatures,and is partially converted by nitric acid, with elevation of tempera-ture, into the sesquioxide, which dissolves in acids with evolution ofoxygen.The monoxide when heated in air or oxygen to 350-440",forms a blackish powder, the composition of which depends on thetemperature ; at 600" this black powder is reconverted into the mon-oxide, showing that the higher oxides of nickel can only exist below acertain temperature. Nickel monoxide dissolves in hydrochloric andsulphuric acids, with rise of temperature ; it forms a beautiful violetsolution with ammonia, and displaces ammonia from its salts.Cob&.-The sesquioxide is reduced a t the same temperature asnickel sesquioxide, viz., 190-200". A t 250" metallic cobalt is ob-tained in the form of a black powder, which takes fire a t ordinarytemperatures, forming mainly the oxide Co304. If the reduction takesplace a t 700°, the metallic cobalt is never pyrophoric ; and the metalobtained by distilling the amalgam in hydrogen at the lowestpossible temperature behaves in the same wayCobalt monoxide obtained by reduction is a dark colonred, readilyoxidisable powder, which when slightly heated in presence of air,becomes incandescent, and is converted into the sesquioxide. Thesesquioxide at a higher temperature forms the magnetic oxide, Cos04,and this when still further heated gives the monoxide, COO, the oxidestable a t high temperatures.Chromium.-The sesquioxide is not reduced by hydrogen at anyknown temperature.When strongly heated, it becomes incandescent',and is rendered almost insoluble in acids. The ignited oxide whenheated a t 440" in a current of hydrogen sulphide, dry chlorine, oxygen,or bromine vapour, undergoes no change whatever.When the non-ignited oxide is heated at 440" in a current of hydro-gen sulphide, it forms chromium sesquisulphide, the properties ofwhich have been previously described by the author (this Journal78 ABSTRACTS OF CHEMICAL PAPERS.Abstr., 1880, 527).Heated in a current of oxygen, the sesquioxide isoxidised to the dioxide, CrOz, as already pointed out by Kriiger. Thisdioxide has a deep grey colour, and when calcined evolves oxygen andis reconverted into the sesquioxide. When heated with hydrochloricacid or a mixture of snlphuric acid and sodium chloride, chlorine isgiven off. Fused with potash, out of contact with air, it gives potas-sium chromate and chromium sesquioxide.When the hydrated sesquioxide is gradually heated in a current ofchlorine, it first loses water, and at 440" is converted into chromyldichloride.The dehydrated but not ignited sesquioxide is partiallyconverted into chromic chloride, but no chromyl dichloride is formed ;if, however, the chlorine be saturated with aqueous vapour a t 8- lo",the latter compound is formed in considerable quantity. I f thechlorine be saturat,ed with aqueous vnpour at 20°, but little chromyldichloride is produced. Chromyl dichloride is also formed when acurrent of moist chlorine is passed over chromic chloride heated a t440°, but a moist inert gas, such as carbonic anhydride, does not pro-duce this change. Further, it is found that the hydrated sesquioxidewhen dried at 440" contains 5-10 per cent.of water. Probably inall these cases chromic chloride i s first formed, and then decomposedwith production of chromyl dichloride, by the excess of chlorine, andthe water present either in the gas or in the oxide.By arresting the action of moist chlorine on the chromium sesqui-oxide a t the moment when the red vapours of Cr02Clz are given off, abrown powder is obtained, which approaches in composition the oxy-chlorides described by Moberg.Bromine vapour, under the same conditions, also attacks the non-ignited chromium sesquioxide.Chromium amalgam may be obtained by the action of sodium amal-gam on the chloride, bromide, or iodide of chromium. Like theamalgams of all the metals of this gronp, it oxidises readily.Whendistilled in a current of hydrogen a t the lowest possible temperature,metallic chromium is left in the form of a black, amorphous, veryslightly agglutinated substance, which takes fire when exposed tothe air. If distilled at temperatures above 355", the residualchromium is not, pyrophoric. The chromium thus obtained is morereadily oxidised, and is more soluble in acids than that obtained byDeville by reducing the sesquioxide with carbon. When heated todull redness in a carrent of dry carbonic anhydride, it is convertedinto the sesquioxide.If this family of elements be arranged in the order, chromium,manganese, iron, cobalt, nickel, their affinity for oxygen and the heatsof formation of the oxides, chlorides, bromides, iodides, and sulphidesdecrease as the atomic weight increases.Atomic Weight of Antimony.By R. SCHNEIDER (J. pr. Chem[: 21, 22,131-147).-A controversial paper in reply to strictures passedby Kessler on the author's results.The ant'hor, together with Cooke, finds 120 as the atomic weight;Ressler, in common with Dexter and Dumas, obtains 122.The author's method is by reduction of a pure specimen of antimonyC. H. BINORQANIC CHEMISTRY. 79glance by hydrogen, and in 1856 (Pogg. AWL., 98,293-308) obtained120.3 by this means.The author gives three recent determinations made on the sameplan, and with an antimony glance containing-Insoluble residueAntimony sulphide. (quartz). Calcium carbonate. Ferrous sulphide.99-81 1 0-108 0-048 0.033As on heating it in a current of hydrogen or carbonic anhydride itdecrepitated, giving out a slight empyreumatic odour, it was heatedbefore reduction in hydrogen to 290-320” until decrepitation hadceased and thg issuing gas was odourless. Antimony sulphide itselfundergoea no reduction at this temperature.The mean result from the three experiments is 120.182, which com-pares well with 120.3, the one previously obtained.Dexter, like Berzelius, determined the atomic weight by oxidationof the metal with nitric acid and ignition of the residue.The suppo-sition that the residue on ignition is a thoroughly stable body of thecomposition of antimony tetroxide is incorrect, as Bunsen has shown(Annalem, 192, 317).Kessler’s method (Pogg. Anw,., 95,204 (1855), and 113,134 (1861))is to oxidise antimonious chloride in concentrated hydrochloric acidb-y a volumet,ric solution of potassium dichromate in excess, and toadd, after dilution of the solution, an excess of ferrous chloride andthen titrate back the excess of ferrobs chloride by chromium solution.I n 1855 he obtained the atomic weight, 123.7, and in 1861 one experi-ment with antimony, one with antimony trioxide, and a third withantimonious chloride, gave 122.29.The author criticises Kessler’s method, and infers that no relianceis to be placed on it.Products of Decomposition and Metamorphosis of UranylSulphide. By C. Z~MMERMANN (AnnuZen, 204-2’24) .-Uranium doesnot exhibit a great affinity f o r sulphur, since uranyl sulphide is con-verted into uranyl hydroxide by washing with warm water. It hasbeen noticed by Reme16 (Pogg. Ann., 124, 120) that when uranyl sul-phide is left in contact with ammonium sulphide the liquid becomes ofa brown to deep black colour. The author shows that this is due tothe solubility of the uranyl sulphide i n ammonium carbonate con-tained in the ammonium sulphide. When precipitated uranyl sulphideis left for a long time in contact with ammonium sulphide in the cold,two bodies are obtained, one red the other black. The author showsthat when the ammonium sulphide contains a considerable amount ofthiosulphate the red body is formed, but that in absence of thio-sulphate the black body is obtained. The thiosulphate is formed bythe action of atmospheric oxygen on the ammonium snlphide. Theformula assigned to uranium-black is Ur,O,< O>Ur + 2Ur,0,.Uranium-red seems to consist of an oxygen-compound which contains,besides sulphur, a second base (potassium, sodium, ammonium, 01’barium), and some uranium, probably as uranyl sulphide. AnhydrousF. L. T.80 ABSTRACTS OF CHEMICAL PAPERS.uranium-red, on the assumption that it is perfectly free from admixture,OK may be formulated thus : U6SK209 = 2Ur203 + UrzOz< SK.G. T, A

ISSN:0368-1769    

DOI:10.1039/CA8814000072

出版商:RSC    

年代:1881

数据来源: RSC

摘要:

80 ABSTRACTS OF CHEMICAL PAPERS. M i n e r a1 o g i c a1 C h e mi s t r y. Analysis of the Mineral Water of Niederbronn in Unter- Elsass. By E. BURI (J.yr. Chem. [2], 22, 388--395).-The water as it runs into a large basin from the spring appears deep green, occasional bubbles of gas escape; it is perfectly clear at first, bub appears turbid when removed. The sample was collected on 5th June, 1880 ; its temperature then was 17*9", that of the air being ll*6°. Its sp. gr. a t 16.4" was 1.0036, taste saline and somewhat inky ; no smell was noticeable. With test- paper the reaction for carbonic acid was given. In 10,000 parts by weight, of t.he water there were contained:- Strontium sulphate ........ Calcium sulphate ........ Potassium chloride ........ Sodium chloride .......... Lithium chloride ..........Amnionium chloride ...... Calciiim chloride .......... Magnesium chloride ...... Calcium bicarbonate ...... Magnesium bicarbonate .... Ferrous bicarbonate. ....... Silica. ................... 0250 0.697 2.187 30.748 0.274 0.088 6.621 2-456 3.900 0.049 0.104 0.135 47.509 Free carbonic anhydride.. .. 0.794 Nitrogen ................ 0.328 There were also present traces of phosphoric acid, bromine, man- ganese, alumina, and organic matter. The bubbles of gas rising from the water in the basin contained 5-34 per cent. of carbonic anhydride and 94.65 per cent. of nitrogen by volume. The mud collected from the sides of the basin into which the water flowed was thoroughly washed and then dried. It contained the fol- lowing percentages :-1*533 of arsenious acid, 0.005 of lead sulphate, and 55.534 of ferric oxide, together with traces of antimony, copper, zinc, and manganese.Supposing the arsenious acid to bear the same proportion to the ferric oxide in the water as it does in the mud, 10,000 parks of the water would contain 0.0013 part of arsenious acid.MINERALOGICAL CHEBIISTRY. 81 The analysis was conducted according to Bunsen’s method, and the actual weights of the precipitates obtained are given : the arsenic Wacs The Hot Spring.at Bagnoles de I’Orne, and the Deposits Formed in the Conduits. By DELACHANAL ( A m . Chi~n. Phys. [ 5 ] , estimated by Bunsen’s new method as pentasulphide. P. c. 21, 275-278). A m l y s i s of the Water (per litre). 0.0182 0.0040 0,0151 0.0127 0.0035 0.0003 0*00lt Si02.K,S04. Na,S04. NaC1. CsSO+ Ca,P,O,. 8 1 2 0 3 + Fe203. The total residue per litre was 0.0628, the organic matter and loss being 0.0073. There were traces of lithium, magnesium, zinc, and lead present. The water had a perfectly neutral reaction; iodine and arsenic could not be detected. The numbers obtained by the author differ from those obtained by Henry in 1868, the total solid residue a t that time, for example, being 0.1309 per litre. The composition of the water has evidently changed. Analysis of Deposit. Si02. PbO. ZnO. Fe,O,. P?05. SiiO,. 10.7 14.1 1.3 53.3 17.6 2.3 = 99.3 C. H. B. Results of the Norwegian North Sea Expedition. By L. SCHMELCK) J. pr. Chem. [2], 22, 165-188).-1. Solid constituents of sea-water. The Northern Arctic Ocean has a mean sp.gr. of 1.0265, and con- tains per cent.- CaO. MgO. K20. c1. so,. 0.05 78 0.2203 0.047% 1.9320 0.2214. The average amounts of salts occurring in the sea and the composi- tion of the sea-salt are :- I n sea-water. In sea-salt. per cent. per cent. Calcium cnrbonnt e .......... 0.0 02 0 0.05 7 Calcium sulphate .......... 0.1395 4.00 Magnesium sulphnte ........ 0.2070 5.93 Magnesium chloride ........ 0.3562 10.20 Potassium chloride. ......... 0.0747 2.14 Hydrogen sodium carbonate. . 0.0166 0.476 Sodium chloride ............ 2.682 76-86 F. L. T.80 ABSTRACTS OF CHEMICAL PAPERS.M i n e r a1 o g i c a1 C h e mi s t r y.Analysis of the Mineral Water of Niederbronn in Unter-Elsass. By E. BURI (J.yr. Chem. [2], 22, 388--395).-The wateras it runs into a large basin from the spring appears deep green,occasional bubbles of gas escape; it is perfectly clear at first, bubappears turbid when removed.The sample was collected on 5th June, 1880 ; its temperature thenwas 17*9", that of the air being ll*6°.Its sp. gr. a t 16.4" was 1.0036,taste saline and somewhat inky ; no smell was noticeable. With test-paper the reaction for carbonic acid was given.In 10,000 parts by weight, of t.he water there were contained:-Strontium sulphate ........Calcium sulphate ........Potassium chloride ........Sodium chloride ..........Lithium chloride ..........Amnionium chloride ......Calciiim chloride ..........Magnesium chloride ......Calcium bicarbonate ......Magnesium bicarbonate ....Ferrous bicarbonate........Silica. ...................02500.6972.18730.7480.2740.0886.6212-4563.9000.0490.1040.13547.509Free carbonic anhydride.. .. 0.794Nitrogen ................ 0.328There were also present traces of phosphoric acid, bromine, man-ganese, alumina, and organic matter.The bubbles of gas rising from the water in the basin contained5-34 per cent. of carbonic anhydride and 94.65 per cent. of nitrogenby volume.The mud collected from the sides of the basin into which the waterflowed was thoroughly washed and then dried. It contained the fol-lowing percentages :-1*533 of arsenious acid, 0.005 of lead sulphate,and 55.534 of ferric oxide, together with traces of antimony, copper,zinc, and manganese. Supposing the arsenious acid to bear the sameproportion to the ferric oxide in the water as it does in the mud,10,000 parks of the water would contain 0.0013 part of arseniousacidMINERALOGICAL CHEBIISTRY.81The analysis was conducted according to Bunsen’s method, and theactual weights of the precipitates obtained are given : the arsenic WacsThe Hot Spring.at Bagnoles de I’Orne, and the DepositsFormed in the Conduits. By DELACHANAL ( A m . Chi~n. Phys. [ 5 ] ,estimated by Bunsen’s new method as pentasulphide. P. c.21, 275-278).A m l y s i s of the Water (per litre).0.0182 0.0040 0,0151 0.0127 0.0035 0.0003 0*00ltSi02. K,S04. Na,S04. NaC1. CsSO+ Ca,P,O,. 8 1 2 0 3 + Fe203.The total residue per litre was 0.0628, the organic matter and lossbeing 0.0073. There were traces of lithium, magnesium, zinc, andlead present.The water had a perfectly neutral reaction; iodine and arseniccould not be detected.The numbers obtained by the author differfrom those obtained by Henry in 1868, the total solid residue a t thattime, for example, being 0.1309 per litre. The composition of thewater has evidently changed.Analysis of Deposit.Si02. PbO. ZnO. Fe,O,. P?05. SiiO,.10.7 14.1 1.3 53.3 17.6 2.3 = 99.3C. H. B.Results of the Norwegian North Sea Expedition. By L.SCHMELCK) J. pr. Chem. [2], 22, 165-188).-1. Solid constituents ofsea-water.The Northern Arctic Ocean has a mean sp. gr. of 1.0265, and con-tains per cent.-CaO. MgO. K20. c1. so,.0.05 78 0.2203 0.047% 1.9320 0.2214.The average amounts of salts occurring in the sea and the composi-tion of the sea-salt are :-I n sea-water. In sea-salt.per cent. per cent.Calcium cnrbonnt e .......... 0.0 02 0 0.05 7Calcium sulphate .......... 0.1395 4.00Magnesium sulphnte ........ 0.2070 5.93Magnesium chloride ........ 0.3562 10.20Potassium chloride. ......... 0.0747 2.14Hydrogen sodium carbonate. . 0.0166 0.476Sodium chloride ............ 2.682 76-86F. L. T

ISSN:0368-1769    

DOI:10.1039/CA8814000080

出版商:RSC    

年代:1881

数据来源: RSC