摘要:

J O U R N A LH. E. AR3fSTILOSG, Ph.D., F.B.S.W. CROOKES, F.R.S.E. FRANKLASD, D.C.L., F.R.S.c. w. HEATOK, F.C.S.HCGO M~~LI.ER, Ph.D., F.R.S.WARRES DE LA Rue, D.C.L., F.R.S.OFW. H. PERKIH, F.R.S.W. J. RUSSELL, Ph.D., F.R.SR. V. Tusos, F.C.S.C. R. A. WRIGHT, D.Sc.R. \vARISGPOS, F.C.S.THE CHEMICAL SOCIETY.G. T. ATKINSOS.E. C. BABER.P. P. BEDSOP?, BSc.D. BEBDIX.F. D. BROWS.C. H. BOTHAYLEY.C. A. RVRGHARDT, Ph.D.FRASK CLOWES, D.Sc.A. J. COITSLEY.C. F. Cnoss.J. K. CROW, D.Sc.W, R. HODGKTSSOS, D.Sc.T. CARSELLEY, D.Sc.1 &I. $1. PATTISOX JIUIR.J. $1. H. XUSRO, D.Sc.E. XEISOS.E. IT. PREVOST, Ph.D.W. RANSAY, Ph.D.JOHN BOBIXSON.R. ROUTLEDGE, B.Sc.I,. T. O’SHEA.J. XILLAR THOJISOS.1 W. THOIISON.c. m. WKrTS.W. C.WILI.IAVS.WATSOS SMITH.JOHS TVATTS, D.Sc.Vol. XXXVI.1879. ABSTRACTS.L O N D O S :J. V A N VOOLZST, 1, P A T E R N O S T E R ROW.187LONDON :IIIRRISOX AND SONS, PRINTERS I N OBIJINARY TO EER JIAJESTT, ST. M4RTIK’S LAXEC O N T E N T S .ABSTRACTS OF PAPERS PUBLISHED I N OTHER JOURKALS :-General arrcl Pl~ysical Ckenzistry.PAQ ET-OGEL (H. W.). Differences in the Absorption Spectra of one and the sameSubstance . . , . . . . . . . . .LECLASCH~. An Improvement in the Peroxide of Manganese Battery. .HITTORF (W.). Proof of the Statement that ‘‘ Electroljtcs are Salts,” aT~ULLSER (A,). Relation bctween tlie Spccific Heat a t a constaiit Toiunx;CLA~SITJ (R,). The Relat,ioii between Work effected by the Diffusion ofRAOVLT (F, X), Vspour-tension and SolidifIing Point of Saline Solutions .OGIER (J,).Measurement of the Heat dereloped in the Formation ofHydrogen P1io:pliides and Srsenides . . . . . . .THOMSES (J,). Thernio-chemical Researches : Heat of Solution of Sitratcs,Sulphates, Dithionates, and some other Salts . . . . . .CIAXICIAK ((3.). Influence of Temperature and Pressure on the Spectra ofGases . . . . . . . . . . . .BURGER (H.) , .LASDA-CER (J.) . Absorption Spectra . . . . . . . .B~TTGER (R.) . PlantB’s Seconrlar~ Battery . . . . . . .BOTTGER (R,), Production of Rotatory Moi-enients in Jlercuq- . . .BGTTGE~E (R,). Production of s High Temperature hy means of dmmo-nium Sitrate . . . . . . . . . . . .XonR (F.). Naterial for Standard Weights and IIensures . . ..VOGEL (H,). Difference of the Absorpt,ion.spectra of one and the sameSubstance . . . . . . . . . . . .BRA-CS (F,), Unipolar Electrolytic Concluckon . . . . . .HERTIG (H.). On tlie Quaiiticy of Elcctricity necessai~ for the CompleteClraige of a Platinum-water Ccll, and tlie Distance between the 3IoIe-THOJISES (J,). RIoiioliJ-clrated Sodium Sniphate and Dchjclratecl SoclniniCarbonate . . . . . . . . . . . .RITTER (A,). The (‘ Temperstnre Snrfnco ’ I of Carbonic Acid . . .X.~ruar;s (A,), Density and Decomposition of Sitric doid . . .BOTTISGER (C.) . Dissociation of linmoniuni Chloride, a Lecture Experi-Reply to L. Bleekrode . . . . . . .the Temperature, and the Conductirity of GasesGases and the Second Lair of Thermodynamics . . . .Spectroscopic Inveatigation of the Constitution of LiquidsKIRXIS (31,).Transference of the Ions . . . . . .cules of Liquid Water . . . . . . . . .ment . . . . . . . . . . . . .H o ~ l ~ . i s s (A. \Ti). 3Ioclifiecl Tzponr-density Determination . . .TILDEZ (W. A,). Deterniination of Specific Grarities . . . . .SCHRODER (H.). Law of Nolecular Volumes . . . . . .SCHBODER (H.). Law of Molecular Bolunies . . . . . .ULLIS (F.). Gelatinous Silica as an Inormnic Menibrsne . . . .BOTX-E~ (-4.). Electro-chemical Actions &der Pressure . . . .CROTA (A,). Spectrometric Measurement of High Teniper~ttni*es . . .T T ~ ~ ~ ~ r : (J.). .CREJTI (L.). Gas Regulator for Air-baths . . . . . . .MEYER (T. and C.) , Determination of Vapour-densities of Substancesvhich attack JlercurJ-, or which boil above 440’ .. . . .Specific Heat and Latent Heat of Fiisioii of Psllndium .a 3111> -345610110110110110210710’1 s919319819419 J.1951951967 !I619719719819929329329.1.29429 1iv CONTESTS.VIKCEST (C.) and DELACHAXAL. Density and Coefficient of Expansion ofCLARICE (F. W.). Specific Gravity Determinations . . .BERTHBLOT. Reciprocal Displacements betaeen Oxygen, Sulpliur, anh theBERTHFLOT. Reaction between Mercury and Hydrochloric kcid Gas . .KARR (F.). Behariour of Electric Currents in Rarefied Gases . . .BEETZ iTV.). Excitation of Electricity br the Contact of Solid and GaseousLiquid Methyl Chloride . . . . . . . . .Halogens when combined with Hydrogen .. . .- -Bodies . . . . . . . .DORY (E.). Electrical’Currents produced by the flow of Liquids throughTubes . . . . . . . . . . . . .WIXKELNAKN (A). Deviation of some Gases from BoTle’s Law . , .STADEL (W.) and E. HAHN. Apparatus for Regulating the dtmospliericPressure in Boiling-point Determinations . . . . . .STEFAN. Diffusion of Carbonic Anhydride through Water and Alcohol .LEBAIQFE (E.) . Apparatus for Continual Dialpis . . . .~ m n m r a a ? ; (G.). Dissociation of Dissolred Ferric Saits . . . .OSWALD (W.). Chemical A5nity . . . .BERTHELOT. Relative Affinities and Reciprocal ‘Dispiacements of Oxygenand the Halogen Elements . . . . . . . .ME YE^ (F.) Preparation of large reg& ~ r - p t a ~ s . . . . .CONROY (Sir J.) .,LOCKYER (J. N.). Recent Researches in Solar Chemistry . . . .BROWX (J.), Theory of Voltaic Action . . . . . . .HfiR.4FD (&). New voltaic Element with Constant Current . .AYRTOX (W. E.). .GVTHRIE (F.). On Salt Solutions and Attached Water . , . .CAILLETET (L.). Compressibility of Gases . . . . . . .SCHRODER (H.). Law of Molecnlar Volumes . . . . . .SABIR’E (R.), Motions prodiiced by Dilute Acids on some Amalgam Sur-faces . . . . . . .WITZ (A,)” Therinic Effect df the’ Walis of Closed Vessels on the ContainedGases . . . . . . . . . . . .THOXSER’ (J.). Accuracy of Thermo-chemical Results . . . . .THOMSEN (J,). Heat of Forniation of Metallic Snlphides . . . .BERT~ELOT. Formation of Halo’id Ethers in the Gaseous State . . .T’OGEL (H.W.). Photogryphecl Spectra of Oxygen and Hydrogen . .RODWELL (G. F.) and H. M. Elder. Effect) of Heat on Mercury Diiodide .PFAUSDLER (L.). Vapour-density Determinations at High Teniperatnres ofBRRHL (J. W.). Limits t o the applicat,ion of t i e Mkthod of determiningENGEL (B.) and MOITESSIER. Dissociation of Chloral Hpdiate . . .SMITH (R. A,). Absorption of Gases by Charcoal. Part II. On a KewSeries of Equivalentas or Molecular Kumbers . . , . . .GREXFELL (J. G.) , Supersaturated Solutions . . . . . .CROOKES (W.) . Illumination of the ’Lines of Molecular Pressure, andNew Unirersal Stand for use with the Pociet Spectro-The Light re5ected from Potassium Permanganate .Electrical Properties of Beeswax and Lead ChiorideSXITH (A. P.).Blue Flame from Common Salt . . . . .PECKEALC (E. F.). Detern1iuat)ion of Specific Gravities . . .Substances which attack Mercury . . . .Tapour-densities in the Barometrie Vacuum . . . . .BAYLEY (T.). Catalysis . . . . . . . . .the Trajectory of Jlolecnles . . . . . . .TIOLLE (J,). Radiation from Incandescent Plat,inum . . . .LEPEL (B. I?. v,).scope . . . . . . . . . . .THOLLON (L.). Displacement of the Lines of the Spectrum by the Motiondue to the Sun’s Rotation . . . . . .MELDOLA (R.). A Cause for the Appearance of Bright Lines in the Solar ._ Spectrum . . . . . . . . . . . .. LOCIXER (J. X.). Researches on Spectra . . . . .VILLARI (E.). Tliermic and Galvanometric Laws of the Electric SparkPARR29 1.20.52962983-153453463163463473473483483513524’54254264264274284‘943043143243343343549749749549849949950050050150157357357457457457657CONTESTS. vBEILSTEIS (F.) and L.JAU-EIN. Treatment of Bunsen's Cells . . .BOUTX. Pressures produced by Galvanic Deposits . . . . .BECQUEREL (H.). AIagnetic Itotatory Power of Gases a t Ordinary Tempera-ture and Pressure . . . . . . . . . . .BICIIAT (E.). Magnetic Rotatory Power of Vapours . . . . .EXNER (F.). Electrolysis of Water : Galvanic Polarisation . . . .EXXER (F.). Galvanic Polarisation of Platinum in Water . . . .CALN (A.) . Vapour-density of Aqueous Acids. with Constant BoilingPoints . . . . . . . . . . . . .MEYER (C. and V.). Vapour-densities of some Iiiorganic Bodies.. .MOIIR (F.). Nature of Cohesion and its Cheniical Signification . . .HERYANK (R.). Specific Gravity and Atomic Volume of the Cerium MetalsGULDBERU and WAAGE. Chemical AEnity . . . . . . .STOIIMANN (F.). A Calorimetric Method . . . . . . .MITSCHERLICH. On New Phenomena shown by Gases . . . .MILLS (E. J.). Researches in Thermometry . . . . . .CARNELLEY (T.) . Relation between the Uelting Points of the Elements andRECHENBERG (V.) . Heat-absorption attending the Solution of PotassiumChloride in Water . . . . . . . . . . .CoprET (L. C. DE). Hcat developed by Contact of Water with AnhydrousSodium Sulphate . . . . . . . . . . .BERTIIELOT. Decomposition of Haloi'rl Acids by Vctals . . . .BEKETOBF (M.). Deterniination of the Atomic Heat of IIjdrogen in itsCombination with Palladium .. . . . . . . .BERTHELOT. Combination of Carbonic Oxide with the EJements . . .CIAIIIICIAN ((3.). Spectra of the Elements and their Compounds . . .CIAMICIAX (G.). Influence of Temperature d Yressuiwon the Spectra ofVapours and Gases. . . - , . . . . . .AVERBACII (F.). The Passage of the Galvanic Ctment through Iron . .PFWHL ((3.). Sketch of the Atomic Theory of Heat . . . . .DOSATII (J.). Specific Heat of Urauoso-uranic Oxide, and the AtomicWeight of t'ranium . . . . . . . . . .LECHER (E.). .HANMERL (H.). Preezlng Mixture of Calcium Chloride and Snow . . .LORIS (31.). Preliminary Study of the Action of Acids on Salts without theIntervention of a Solvent . . . . . . . . .BEKETOFF. Heat of Hydration of Sodium Oxide, and the Action of So&umI'ijdroxide and of Hydrogen on Sodium Oxide .. . 8 . .WIEBE (H. F.) . Thermo-chemical Relation between the Boiling and hlrltingPoints of Solid Elements . . . . . . . . .NAUMANN (A). Dissociation of Chloral IIgdrate . . . . .KESSLXR (F.) . Law- of Multiple Proportions . . . . . .ABT (A.). Continuous Spectrum of the Electric Spark . . . .GOLDSTEIN (M.}. Boiling Points of Normal Ethanes (Paraffins) . . .MEYER (V. and C.). Vapour-density Determinations of Inorganic J3oclies t i tHigh Temperatures . . . . . . . . . ,BERTHELOT. Heat of Formationof Cyanogen . . . . . .OGIER (J.). Thermic Formation of Silicon Hydride . . . . .OGIER (J.). Themic Researches on Silicic Ether . . .. .LOUGTJININE (W.). Influence of Substitution on the Evolution of Heatduring Format-ion of Salts . . . . . . . .SCIIILODER (H.) . Volume-constitution of the Suilpliates, Selenates, and Chro-mates of the Magnesium Metals . . . . . . . .KOPP (H.). Determination of Atomic Weights, and the Use of Isomorphisinfor the same -. . . . . . . . . . . .CORNTJ (A.). Ultra-Violet Limit of the Solar Spectrum . . . .PAALZOW (A.). The Oxygen Spectrum and Luminous Bp1)earauce of Rare-fied Gasesin Tubes with Liquid Electrodes . . . . . .BOISBATJDRAX (L. DE). Spectrum of Ytterbium . . . . . .their Coefficients of Expansion b j Heat . . * . . . .IIeat-capacit,y of Mixtures of Methgl Alcohol and WaterPAGE576576576671577578G i 951d57957958058658758858858858958959058 1685683686687G 89fX9767 '1g87698618618fjvi COSTESTS.S x I m (J.L.) and L. DE BOISBAVDRAX. .BOISBAUDRAN (L. DE). Spectrum of Erbium Nitrate . . . . .LuxassIty (S.). Stokes’s Law . . . . . . . . .BECQ~EREL (E,). On a Sote by Lamanskp on Stokes’s Law . . .Soimr (J. L,), Fluorescence of the Salts of the Eai-th-metals . . .BACDRIXONT (-4.). Influence of Coloured Light, on the Evaporation ofWater . . . . . . . . .FILEFSD (C.) . Some Gal~anic Prbpertles of Aqueous Solutions of NetallicSall,s . . . . . . . . . . . .BEETZ (W.). Electric Condnctivity of Zinc Sulphate solution . , ,BLOXDLOT (R,). Capacity of Voltaic Polarisation . . . . .DEa.iias (P.). Refraction of Invisible Heat .. . . . . .BERrHELOT. Bmnlgams of the Alkali-metalp, and the Nascent State . .SasaTiEn (P,) . Theirno-chemical Stud? of the lllialiiie Sulphitles . .SaB.uriEn (P,). Thermo-chemical Study of Dissolrd Alkaline Sulphides .Spectrum of Didymiuin SitrateBrRTrieLor. Etlieriiication . . . . . . . . . .LOLG~IXISE [W.). Thermic Effect of Substitutions . . . . .BEILTHELOT. ‘Sonie Thermo-chemical data . . . . . . .BERTIIELOT. Observations on Noble and Abel’s Xemoir on the Combustionof Gunpolviler . . . . . . . . . . .MEYER (V. and C.). Tapour-densities of some Inorganic Componntls . .PICTET (R.). Study of the Molecular Constitution of Liquicls by means of .Exsiccator for Csrbon Bisulphide, Ether, Chloroform, and Benzene . .TROOBT (L.). Distillation of a Heterogeneous Liquid .. . . .B~YIRD (A,). Viscosity, a cause of Catalpis . . . . . .MILLS (E. J.) and J. J. SYITH. .ATTESKOFER ((3.). A Simple Gasholder . . . . .DRAPER (J. C ). Presence of Dark Lines in the Solar Spectrum which COT:GERXEZ (D,). Distillation of Liquids under the Influence of Static Elec-their Coefficient of Dilation, Specific Heat, and Atomic Weight .Researrhes on Chemical E q u i d e n c e .respond closely with the Oxygen Lines . . . .tricity . . . . . . . . . . . . .The Electromotire Force produced by the Flow of Liquidsthrougli rubes . . . . . . . . . . .The Electromotire Power of a Grow’s-element in Terms ofEIJLUSD (E.).RIECKE iE ).Siemeilb- Weber Units . . . . . . . . . .PIERCE (13. 0.). Tile ElectromotiTe Power of Gas Elements .BIRCS (C.).The Thermoelectric Position and Electric Conductirity o i Steeiin tlieir Relation t o its Hardness . . . . . . . .WALTESHOFES (A. r.). Magnetic Behariour of Finely-disided Iron . .BEET2 (Jv.). Conductirit,y of Liquids for Heat . . . . . .WIEBE (H. F.). Expansion of Solid and Liquid Bodies . . . .AXIGAT (E. JI.). Compressibility of Gases a t High Pressures . . .CLARICE (F. W.). Sonio Specific Gravity Determinations . . . .KOCH (IC. R,). Changes in the Siirface of Platinum and Palladium pro-duced by Oxygen-polarisation . . . . . . . .TROOST (L.). E m p l o p e n t of Diffusion in the Study of the Phenomena ofDissociation . . . . . .BERTHELOT. Remarks on a kote bn Ciloral’Hyd;..ate dy Wurtz . . .DITTE (A.).Researches on the Decomposition of Metallic Salts, and on .IIENRICHSEN (s.). SpecifiC Heat O f Water . . . . . . .Certain Inverse Reactions which take place in Presence of Water .Inorganic Chemistry.SOLTAY (E.). Preparation of Chlorine and Hydrochloric Acid by means ofCalcium and Magnesium Chlorides , . . . . . .HOLDERXAXN (E.). On H) drochloric Acid containing Phosphoric Acid .JEREXIS. Ozone . . . . . . . . . . . .PAGE861862862863862863863F6486486 C8G b865873a7587581587687699799799 699599899910001001100210021004100410051006100610068s 5mi88CONTENTS. viiBERTHELOT. .DIETXAFAIT (31. L.). Presence of Ammoniacal Salts in Sea-water . .SNYDERS (A. J. C.). Chemicaldction of Water and Saline Solutions on ZincSNITH (J.L.). A New Earth of the Cerium Group, and on the Analysis ofOxidation of Nitrous Acid by Ozone and by Moist OxygenKatural Kiobates . . . . . .- . , . - , .On the Discorery of a New Earth, announced by J. L.SMITH (J. L.). The supposed Eew Element, Mosandrinm . . .RIARIGNAC (C.). . ,Smith . . . . * . . . . . 5 .LIST (K.). Magnetic Compounds having the formula, RN0.Fe203 . .CLERMOYT (I?. de) and J. FROXMEL. .BBTTGER (R.). Formation of Hydrogen Peroxide by the Explosiou of aMixture of Oxygen and Hrdrogen . . . . . . . .CORNE (J.). Reclurtion of Iodates by Phosphorus . . . . .VVLPIES (G.). Solubility of Sulphur and Phosphorus . . . . .HESSGE?; (C.). Action of Hrdrochloric Acid Gas on Sulph&s .. .HESSGEN (C.). Action of Hydrochloric Acid on Double Sulphrrtes . .BOTTGER (R.). Preparation of Salts in a finely-dirided'State . . .PHILIPP (G. H.). Green and Blue Ultramarine . . . . . .DELAFOVTAINE (11.). Terbium and its Compounds, and t,he prdbableExistence of a S e w Metal in the Samarskite of N. Carolina . . .DELA4pOKTAINE (M.). The AIoeandrium of J. L. Smith . . . .DELAFOSTAINE (&I.). Decipium, a New Metal from Samarskite . . .fi1ARIGSAC (C.). Ptterbinm, a Xew Metal from Gadolinite . . . .DELAFONTAINE ($1.). The Probable Compound Eature of the Didymiumfrom Cerite . . . . . . . . . . . .BOTTGER (R.). Pyrophoric Iron . . . . . . . . .J~RGENSEN (S. 11.). Cobalt-ammonium Compounds . . . , .KESSEL (F.). Double Salts of Cuprous Thiosalphate .. . , .MATTHEY (F.). Decomposition of Lead Sulphate by Sodium Chloride. ,VULPIVS (G,). Mecliauical Purification of Mercury . , . . .SEUBERT (0.). Atomic Weight of Iridium . . , , . . .SEUBERT (C.). Donble Salts of D p d Iridium . . . . . .LUNGE (G.). Preparation of Kitrous Acid . . . . . . .PICKERISG (S.). Ammonium Sitrate . . . . . . . .BECIKRTS (€1.) and R. OTTO. Sulphuric Monochloride and Dichloride .CL.4USNIZER (F.). Action of Sulphnric Monochloride on the Chlorides ofTitanium, Antimony, Tin, and Silicon . . . . . . .CLAUSKIZER (F.). Salpho-selenium Oxrtetrwhloride . . . . .ERLENMEYER (E.j. Studies of the Phosphates . . . , . .FdSSBEKDER (R.). Double Salts Of Calcium Sulphate . , . . .RICKMAEN (R.). Constitution of Ultramarine .. . . . .LEHXANN (A,). Constitution of Ultramarine . . . . . .BROWN (W. G.). Philippium . . . . . . . . .SNITH (J. L.). Remarkable Specimen of Silicon-iron . . .NORAVSKI (T.) and J. XTISGL. Potassium Permanganate and its Oxidatio;Product s . . . . . . . . . . . .THOXSEK (J.). Zinc SulphFdrate . . . . . . . .T~OXSES (J.). Composition of Precipitated Copper Snlphide . . .LOSECKE (A. v,). Formation of Ammonium Xitrite . . . . .PICHARD. Alkaline Reaction of Free, Mixed, and Combined Magnesium Car-bonates and Silicates . . . . . . . . . .SCTIULERUD (L.). On Chromates and Dichromates . . . . .DITTE (A). Action of Hydracids on 31ercuric Sulphate, and of' SulphuricAcid on the Hnlo'id Salts of Mercury . . . . . . .Dissociation of Metallic SulphidesETARD (A,).Researches on the Sulphatea . , . . . .SALZER (T.). Hypophosphoric Acid and its Salts. . . . .N (R.). Ultramnriue . . . . . . . .c ((2.). The Gadolinite Earths . . .DELAFONTAINE (M.). Philippiurn. . . . . . . .BAUBIGNY (H.). The O d e of Nickel, -Ui,04 . . . .PAGE90111212131313103 ~ .~10310410410510310:107108105113114116117117118119119119125124125125125200200200201201201L 203203204204261.20420620629529829829929viii CONTENTS.MENKE (A. E.). Reactions of Iodine and of Potassium Iodide with Sulphor-ous Acid . . . . . . . . . .LEEDS (A. R.). Action of Potassium Permanganate on Oxaiic Acid . .SCH~SE (E.).Hydrogen Peroxide . . . . . .CLAIJSNIZER (F.). Experiments on the Preparation df Sulphuric Bromideand Sulphur Oxytetrabromide . . . . . . . .TOGLER (H.). Composition of Commercial Ammonium Carbonate and ofthe Product formed on exposing it to Air . . . . . .SCHNEIDER (R.). Atomic Weight of Antimony . . . . , .LEFORT (J.). Tungstates of the Earthy and'4letallic Sesquioxides . .BERTHELOT. Ozone and the Silent Electric Discharge . . . , .OGIER. Liquefaction of Silicium Hydride . . . .HORSTNANN (A,). Relative Affinity of OxFgen for Carbonic Oxide and Hr:LETTS (E. A,). Some Bismuth Residues . . . . . .drogen. Part I1 . . I . . . . . . .BOERGEOIS (L.). Crystalline Barium Chromate . . .LOSEEASX (G.). Action of Sulphuretted HTclrogen on'dlkaiine Solutions of .-Alumina ' . . . - . . . . . . . . .HEUXAXR' (R.) , Silver Ultramarine . . . . . . .MWLLER (F, C. G.). Gases in Iron and Steel . . . . . .VORTXAXS (G,). Cobalt-ammonium Compounds. . . . . .GERRESHEIN (H.). Ammoniacal Mercury Compounds . . . .TROOST (L.). New Compounds of HFdrochlbric Acid with dnmonia .LUNQE (G.). Existence of Nitrous AnhFdride in the Gaseous StateRIBAX (J.) , Compounds of Hydrogen Phosphide with Cuprous Chlbride;and its Estimation in Gaseous Mixtures . . . . . . .SCHERISG (E.). 3fannfactui-e of Potassium Iodide . . . . .CROS (C.). dct,iou of Light of different Colours on Silver Bromide impreg-nated with various Organic; Colouring Matters . . ' . . .KONIGEL-WEISBERG (J.). Action of Chlorine on Barium Hjdrate ..WHEWELL (G.). Analysis of Bleaching Powder . . . . . .Ultramarine . . . . . . . . . . . . .BATLEY (T,). Complex Oxides of Cobalt, and Xickel . . . . .SENDTXER (R.). Some Kern- Salts of Uranyl . . . . . .BRUEL (J. W.). Purification of Mercury . . . . . . .EVXERLISG (0.). Metallic Phosphides . . . . . . .SCHIEL (J.). Formation of Ozone by Hrdrocarbons . . . . .SCHOBE (E.). HTdrogen Peroxide . . . . . . . .GUTARD (A,). Action of Oxalic Acid on Chlorates, Eromates, and Iodates .GUYARD (A,). Iodated Potassium Iodide . . . . . . .MULLER (H.) and C. PACLY. Preparation of Potassium Nitrite . . .PECHINEY (A. R.). Preparation of Anhydrous Sodium Sulphate fromGlauber Salt . . . . . . . . . .KONIGEL-WEISBERG (J.j. Action of Cilorine on Strontia .. . .BUCENER (E. W.), Ultramarine . . . . . . . . .DENIEL (W'.). Amidonitrosulphide of Iron . . . . . . .JORGESSES (S. ill.). Cobalt-ammonium Compounds . . . . .GORGEU (A). Artificial Nanganese Dioxide . . . . . .LIEPORT (J.). On Tritungstates . . . . . . . . .NILSON (F. L.). Scandium . . . . . . . . . .FLUEGQER (T.). Spitting of Silver . . . . . .SCHERISG (E.). Lead in Potassium Iodide . . . . . .SCHONE (E.). Hjdrogen Peroxide . . . . . . .ETARD (A,). Researches on the Sulphates . . . . . .NILSOS (F.). Ytterbia. . . . . . . . .OLEVE (P. T ). Chlorostannatesof the Rare'Eartiis . . . . .METER (L.),' Purification of Mercury . . , . . . . .BRUHL (J. W.). Purification of Mercury . . . . . . .XOHLER (H.). Mercuric Iodide . . . . .. . . .CLACSR'IZER (F.), Sulpho-oxychlorides , . . . . . .PAQE3-52 . . ~35335335435435435535543643643643743743743743843843850160'750350450450450550550650750750850859259259859359359559559659659759759760060060160160160260260269CONTENTS.Ra~rnrE ((I.). Sulphides of Phosphorus . . . . . . .DONATH (J.). Preparation of Barium from Barium-amalgam . . .TERREIL (A). Kew Determination of the Equiralent of Aluminium . .HECMAKN (K.). Potassium Ultramarine . . . . . . .MOISSAX (H.). Amalgams of Chromium, Iron, Manganese, Kickel, andCobalt . . . . . . . . . .MECXIER [ S . ) . Srtificial Production of' Katire Carburetted i r o n . . .ROSESFELD (M.). Cuprous Chloride .. . . . . . .NEULEK (B. %-AX DER). A Sew Copper Nitrite . . . . . .RICHE (A,). Action of Light on Silver Chloride . . . . . .FCHAER (E.), Decomposition of the HaloPd Salts of Mercury . . .POTILITZIX (a,). Action of Chlorine on Anhydrous Xetallic Bromides .LKKGE (G,). BehaTiour of the Sitrogen-acids with Sulpliuric Acid . .SmTH (J. L.). Crg-stals Extracted from Cast Iron by Ether . . .BERTHELOT. Action of Organic Solvents on Sulphur and on Metallic Sul-phides . . . . , . . . . . . . .POTILITZIX (A,). Action of Selenium on Xetallic Sulphides . . .RAMXELSBERCI (C.) . Behariour of Silicates containing Fluorine, especiallyTouaz and Mica, at Hiah Temperatuyes . . . . . . .KRAUT A(K.). Nercuric Ioaide .* . . . . . . .KESSLER (I?.).Atomic Weight of Antimony . . . . . .MATTHEY (G.). Preparation of Iridio-platinum . . . . . .THOXSOX (J. S.). .SCHONE (E.). Electrolysis of Hydrogen Peroxide . . . . .EXGEL (R.) and R~OITESSIER. Dissociation of Ammonium Sulphide . .EXQEL (R.) and MOITESSIER. Dissociation of Ammoniu~n H~drosulphide .EXGEL (R.) and AfOITESSIER. Disociation of Ammonium Hydrosulphide .ISAXBERT. 1)issociat~ioii of Ammonium Hydrosniphide . , . .ST. CLAIRE DETILLE (H.). Density of the Tapour of &monium DihJ-dro-sulpliide . . . . . . . . . . . . .COQUILLIOX (J.). Action of Aqueous Tapour on Carbonic Oxide in presenceof Red-hot Platinum . . . . . , . . .LEEDS (A. R.). Ammonium Kitrate and the Bye-products obtained in theOzonisation of Air by Noist Phosphorus .. . . . .MALLET (J. W.). Kitrogen Iodide . , . . . . . .RAXXE (G.) . Phosphorus Sulphides , . . . . . . .BERTHELOT. Chemical Constitution of l m ~ l g a m s of the 4lkali-metals .DEXIEL (W.), Zinc and Cadmiiini Arsenatcs . . . . . .UEBAIX a i d RESOEL. A Compound of Alumina rvith Carbonic Acid . .B~:CHXCR (E. W.). Red and Yellow Uitramarine . . . . .DEBRAY (H.). .MOISSAN (€1,). Iron reduced b r Hydrogen . . . . . . .HEXGSEN (C.). Sen- Double Silt o? Chromic Acid . . . . .HAaiJiERL (H.). Solution of Cartonic Oxide in an Acid Solution of CuprousChloride . . . . . . . . . . . . .SCHERTEL (A.). Grey Modification of Tin . . . . . . .ARNOLD (A. E.). Solubility of Stannic Oxide in Hydrochloric Acid ' . .SCHIFF (H.). Tungsten Oxychlorides and Chlorides .. . . .VULPIKS (G.). Formation of Mercuric from Mercurous Chloride . .KOHLER (H.) . Mercuric Iodide . . . . . . . . .JUSSIEU (P. DE). Alloys of Lead and Antimony . . . . . .BOISBlEDRAN (L. DE). Samarium, a new Metal from Saniarsltite . .DAHLL (T,). Norwegium, a Yew Metal . . . . . . .HIORTDAHL. A New Metal discovered by T. Dahll . . . . .LECHARTIER ((3.). Bction of Potassium-p!.rogaliol on Sitric Oxide . .STINGL (J.) and T. XORAWSKI. Production of Sulpliur from SulpliurousAcid and Hydrogen Sulphide . . . . . . . . .Preparation of Distilled Water free from AmmoniaTROOST (L.). Basic Hydrosulphides of Ammonia . . . .RINNE (A). Ultramarine . . . . . . . . .Peculiarity of an Experiment of Gay-Lussnc and ThBnardLIEBEN (A,). Density of Chlorine at High Temperatures .. .isPAGE69169169769269369369369369469417077077177171171277277277281887887987988088088088088088188288388388488588588588788758788788888888885988988988989089010111012101x CONTESTS.FLETCHER (J.). Preparation of Sulphurettecl Hydrogen . . . .PFIXFFER (E.). Tetrathionic and Pentathionic Acids . . , . .METER (V. and C.). Tapoiir-densities of some Metallic Chlorides . .RICIXAYS ( R ) . Constitution of Ultramarine . . . . . .VARETSE (L.). Formation of Crystallised Metnllic Osicles by means ofPotassium Cyanide . . . . ~~ ~ . . . . . . . .DEXEL (IT.). Zinc Phosphates . , . . . . . . .VSRENFE (I,,). Compoiind of Chromic Acid mitli Potassium Fluoride..ALLES (A. H.). Presence of Nitrogen in Steel . . . . . .KOELER (H.) . &lerciiric Clilorioclicle . . . . . . . .EDISON (T. A,). Action of Heat on Metals i n a VacuumJfineralogical Chemistry.KESSGOTT (A). The Fundamental Forms of C r y t s l Species . . ,BI-RGHARDT (C. A,). The Origin of some Ores o f Copper . . . .ZEPIIBROJ-ICH (1‘. T.). Yellow Doloiniie from Bleiherg . . . .REICHARDT (E.). ,!!Boron 3 h e r a l from Chili . . . . . .G c r o r (P.). Depnsits of Calcii~m Phosphate in the Tosges . . .B R ~ S H (G. J.) and E. S. DAKS. New Minerals froin Hairileld Co., C‘on-necticut . . . . . . . . . . . .IOLD (-i. E.). Thaumasite, a Sew Mineral Sprciea . . .IOLD (A. E.). Some Minerals from Laaiigban . .. .ZEPHAROTICH (V. T.). Magnetite from Monte Rlulatto, S, Tjvol. . .ZEPHAROT-ICH (V. T.). The JIirabilite from Aussee . . . . .WICHNANN (A,). TheSericite Rocks of the Taunns . . . . .BERTERTH (F.). Examiiiation of Lithia-mica froiii Paris (Maine), Rozena,MOORE (G. E.). Hetaerolite, a Kew Mineral . . . . .REI~JIARDT (E.). Uraninin Pitchblende from Joachimsthal. . . .XESSGOTT (A). PolIdymite . . . . . . . .and ZinnwaldB A ~ E R (Al,). The. . .Crvstal-Srstem of. .Potash. . . .Mica . . .LIEBISCH (T.). Occnhence of Disthene in Central Africa . . . .COLLISS (J.). Duportliite, a new dsbestiforin Mineral. . . . .G ~ U B E L (C. \V.). The Stone of the “Julius Colnmn,” the Lasez Rock in tbeUpper Bneadine, and the Sericite-gneiss in the Bundener Alp3 .KALKOTVSKY (E.).The Granite-porphyry of Bencha, near Leipzig . .LIEBISCH (T.). Aheralogical-petrographical Kotes on the Granite-porphyryof Loiver Silesia . . , . . . . . . .B ~ R G H ~ R D T (c. A.). .KESXGOTT (A). On Unghwarite, Nontronite, Gromenite, Bc. . . .PSIJKULL ( 6 . R.). Mineralogical Notices . . . . . .. .DESCLOIZEA~X and DAXOL-R. Honiilite , . . . . , .SXITH (J. L.). Dnubrhelite, the Xerv Meteoric Mineral . . . .DIEYER (R.). The Mineral Spring of “ Tenninger Bad,” Soinrimer Tobel,.Occurrence of Dioptase on Clirysocolin, from Peru. - Grisons . . . . . . . , . . .Lrjca (S. DE). Presence of Lithium in the Earth and Water of the So1f;ttara;a t Puzzuoli . . . . . . . . . . . .WROBIXTSKY (I?.). Miileral Waters of the Conban, in the Caucasus ..PLANTA-REICHES-4U (A. T.). The Mineral Snrines of Passuetr, solis, andBSLLO (31.). Mineral Waters of Buda-Pesth . . . . .& ” _-.Tiefenliasten in the Grisons, Switzerland , . . .LAGACLX (€1. v.). Breislakite . . . . . , . . .POHL (J. J.). Method of Detecting the Difference between i a t u r a l andArtiiicial Turquoise . . . . . . , . . .\vA4RTHA (T7.). Preliminal*y Note 011 the a n a l p i s of the Z d i n y 5’fe-teorite . . . . . . . . . . . . .GRIXSIIAT (H. and C.). I i i n l ~ s i s of the Water of Thirliiicre . . .G?MBEL (C. TV.). Phyllite or Sericite-Gneiss . . . * .PAGE101310131013101.410161016101610171017101814171718181919192021212323232324.24242527293031313233333312512512620620720921021COSTESTS. xiPAQEVOEL (H.) , Mineral Spring (( Marienbrunnen,” near Iserlohn, Wcst-VOHL (H.).Ofner Raddczy-Bitter water . . . . . . .H E L x (0.). illicroscopical Properties of Amber, and the amonnt of Snlpbnrcontained in it . . . . . . . . . . .H E L x (0.). Gedanite, a new Fossil Resin . . . . . . .HESSE (0.). On dsphalt,e and other Rdnalites . . . . . .THOXAS (,r. W.). Composition of the Ga3 which i:-suecl from one of t h eShafts of dbercarn Colliery . . . . . . . . .ROLTILLE (P. de). Xatural Crystals of Magneaium Sulphate (Epsomite) of1nr.e size . . . . . . . . . . . .phalia . . . . . . . . . * . .i LASAVLX (A. T.). Crystal System of Tridyinite .. . . . .FO.CQT~ (F.) and 31. L ~ Y . Production of Felspars by Fusion and by Pro-longed Maintenance a t a Temperature near that of Fusion . . .ST. 31~~-SIER. Artificial Crrstallisation of Orthose . . . . . .LTDWIG (E.). Milarite . . . . . . . . .KOCH (A). Adrilar from V&cspatak . . . . . . . .LISD (0.). .KLIEN. Chromium-Garuet in Silesia . . . . . . . .KLIES. Catlinite. . . . . . . . . . . .Cti1;J)SER (H,). The Red Gneiss of the Saxon Erzgehirge . . . .C0ss.i (A,). Serpentine froin Verrayes (dostn) . . . . . .LIEBIXII (T.). Some Syenite-porphyries of Sonth- West Norway . .LASAVLX (1. r.). An Intergrowth of two Xims from Jliddletown, Con-necticut . . . . . . . . . . . . .MEYER (0.). Twin Zircon Cr . . . . . . . .of Jloravicza, in the Banat .. . . . . . . .KORDESSKIOLD (A. E.) , Mineralouical Sotes . , . . . .LAS~ULX (A. 7.). Iodobromite. a kew Silrer Hnlo’id . . . . .~IEI-ER (0.). The Rock of the St. Gotthurd Tunnel . . . . .BVCHSER and T S C ~ E R ~ I A K . The Meteoric Iron of Hungen. . . .FRESESIVS (R.). Alkaline Constitiients of the Hunyadi Jinos Springs atBnrla-Pest . . . . . . . . . . .B.iTx€I.iTER (H,). Etch Fignres” on Quartz C r p t a l s . , . .KLOCKE (F.). The “Etch Figures” produced 011 the Alums , . .STRESG (A,). Sulphide of Iron and Silrer from Andreasberg . . .BERTRISD (E.). Ciminbar Crystals from California . . . . .SCIIROECKISQER (v.). Dietrichite, a Kern Alum from Hungaiy . . .PISAXI (F.). Wagnerite, from B a d e , in Norway. Russian Retinite ..KOCH (A,). Pseuclcbrookite and Szn.horite, neT7- Minerals . . . .BERTRASD (E.). The Crystal Form and Twin-formation of Leocophanc .DOELTER (C.). Diopsirle . . . . . . . , . .MALLARD (E.). Brarasite, a New 3fineral . . . . . . .KNOP (W,). Diabsse froin Berncck . . . . . . . .KILLISQ (K.), The Gneiss of the North Eastern Schn-artzn-ald, and its Re-DIEULAFAIT (L.). The Existence of Barium and St,rontiuin in all Rocksconstituting the Prinisry Formation . . . . . . .Examination of a Meteorite found in the XeighbonrhoodLASA~LX (A. r.). Snccharite . . . . . .Garnet, from the Erratic Gneiss of Ti’ellen, near Brenien .ZEPlI4ROT7ICH (\I-. V.). XeW ral Occurrences in the Iron-oi,e DistrictPIs.isI (F.). Double Selenides of Lead and Copper . . ..lationship to the Mineral Veins . . . . . .WIGSER (G. W.). On Cleopatra’s Needle . . . . . .HIRIAKOFF (M.).WILL?.^ (E.).CKXESQE (E.) and E. F~CIIS. The state in which the precious Xetals existin certain Minerals, Rocks, and Artificial Products . . * .KLIES. Floorite from Evigtok in Greenland . . . . . .SCHMIDT (Lk.). A Decomposition of Hornstone . . . . . .SCHmDT Quartz Diorite from Yosemite . . . . . .of Bedjansk . . . . . . .?rlineral Waters of Aurergne .21 12113003G030135;3583583583593593 x j3603613h136136136“3623633633633643633663663664394394 10‘1 4 04 104 1041 14 4 14124-2244 24434434444454454 1650951151 151sii COSTESTS.XLBKELTNE (N. S,)..TRIPPXB (P.). .TRIPPKE (P.). The T\r-in Formation of Phillipsite from Sirgwitz . .RATH (G. T.). Crystals of Amazonstone (Microline) from Pike’s Peak.lrtificinl Diopside formed in a Besserner ConverterMASKELYSB (X. S.). Eustntire from South hrriea . . . .The Enstntit,r in the Olirine Nodules of the GroditzbergColorado . . . . . . . . . . , .TACCHIYI (11.). Ferruginous Pmticles deposited by a Sirocco at certain place3 . _ . in l t a l c . . . . . , . . . . . , .REICHARDT (E.). Analysis of the Water of the J1ineral Spring at Snlil .G~rjurlv (31. A). Application of the Author’s Atomic Theory to CertainMinerals . . . . . . . . . . .GUIQNET (E.). Constitiition of Cod . . . . . ,S,rIr,L>r.is (J. 11.). Bc,riiadinite, a Resinous Xineral from California , ,PRECRT (H.).Compusition of the Uoinb&ible Gases in the Stassfurt Pot-ash Mines . . . . , . . . . . . .KLEIS (P.). Dinspore from Jordansmuhl . . . , , . .BAUER (11.). The Hydrohzeinarite of Seucnberg . . . . , .HASSEL (T.). Phosgenite from Nonte I’oni, Sardinia . . . . .KOEKIG ((3.). dnkerite from Phcenisvjlle . . . . . . .KLEIN (P.). Manganosite from Langban, Yrreden. . . . . .L A S A ~ L X (A. T.). .BROQQER (W. (3.). Occurrence of Tliomsonite at, Laven . . . .KOEYIQ ( 0 . ) . Simultaneous Occurrence of Groasular, Zoisite, Stilhite, andTscHER>f.kIi (G.). Pelagosite . . . . . . , ,Optical Properties and Crystal Form of Tridymite .Leidyite . . . . . . . . . . .R A U ~ F (H.). Chemical Composition of Sepheline, Cancrinite, and iIicro1somniite .. . . . . . . .KLIPSTEIX (r.). The ;\jepheiine Rock of Meiches in the O&nn.ald . ,SAXDBERGER (F.). Occurrence of Tin in Silicates . . . . ,BROGGER (TT. C.). The Crptal System of Mosandrite. . ~ , .K.i~r;owsr;r (E.). The Leucitophyr of Lake Arerno . . . , .MECSIER ( S . ) . Metallic Granules of dporariosidereal Xeteorites . , ,COHEX (E.). The Meteorite of Zsadhy, Temesrar . . . . .DACBRBE. A Meteorite belonging to the Eukrite Group . . , .MACRO (F.). ‘She Spinelle of Tiriolo in Calabria . . . . . .PENFIELD (S. L.) Chemical Coniposition of Triphylite . . , ,Cossa (A). Distribution of Cerium, Lanthanum, and Didgniiuin . .d u . 4 ~ ~ (F. D,). Presence of Chlorine in Scnpolites . . . . ,WILLX (E.). Presence of Xercury in the Mineral Waters of Saint; S e t -taire .. . . . . . . . . . .PAT ERN^ (E.) and G. &1azza~a. Thermal Water of Termini Imerese . .PORTER (F. B.). Mineral Water of Rosheim in Alsace . . . .BALLASD. Waters of the Ch6liff . . . . . . . . .BRCSH (G. J . ) and E. 9. 1)asa. B new and remarkable Mineral Localityin Fairfield Co., Connecticut, C.S.I. . . . . . . .SMITH (J. L.). The S a t i r e Iron of Greenland, and the Dolci-ite wliicllincloses it . . . . . . . . . . . .HELM (0.). The Sulphur in Fossil Resin . . . .RUSSELL ( J . C.). Occurrence of a Solid Hydrocarbon in the Eruptive Rock:of New Jersey, U.S.A. . . . . . . . . . .F R E x n (E,). Artificial Formation of Coal . . . . . , .SCHRA~F (A). The Tellurium Ores of Siebenburgen . .. . .STREXG (A). Sulphide of Silver from Andreasberg . . . . .ARZRUNI (A,), Crystallographical and Clieniical Examiiiation of soiiwArsenical Pyrites . . . . . . . . . . .CARNOT (A,). Mnllardite, E Nerr Katural Manganese Sulphate; and Lucltite,a Nen- Variety of Iron Su1phat.e . . . . . . . .SCHCJIACHER (E.). Growth-phenomena 011 Quartz Cryst,als from Krummin-dorf, near Strehlen . . . . . . . . . . .WEISB.XM ( A , ) , Cacochlor from Rcngersdoyf, ].ear Gorlitz . . .P IGE613513614515515515516602602G U 36036036046046046046175605605606606t;o;603608609g09609610694695695t191G D i69869869989189289689 659669789890090190190COSTESTS. xiiiSCHUXACHER (E.) .Idocrase in the Limestone Strata of Deutsoh-Tscham-niendor f . . . . . . . . . . . . .SCHUXIACHER (E.). Granular Plagioclase in the Limestone Strata of Gep-persdorf . . . . . . . . . . . . .HSRTMIAXS ($1.). Basalt$ of the duckland Islands . . . . .Cossa (A). Cinder and Lava froin Etna . . . . . . .Report on the Rcsearches of S. Meunier relative to Meteoric NickeliferousIran and the Satire Iron of Greenland . . . . . . .D’ABBAVIE. dmonnt of Sitric Acid in the Waters of tho Nile . . .JOHSSTOKE (W.). dualpis of tlie Water of St. Dnnstsn’s Well, Melrose .PHIP5OX ( T . L.). Water from the Riwr Dart . . . . . .ESTCOUBT ((2.). dnal~-ses of the Waters of Lake Tliirlruere and the RiverT y n y w . . - , . . . . . . . . . .Distribution of Copper in Primordial Rocks, and i n the DIErLlFAIT (L.).Sedinientari- Deposits derived fronq’them .. . . . .NSCIDAX (IT. J.). Composition of a Wodnle of Ozokcrite found a t King-hornness . . . . . . . . . . . . .SCHTI-ARZ (H.). Composition of Prropissite . . . . . . .MALLET (J. W.). .RCEPPER (W. T . ) . On a Pseudomorph after dnortllite, from Franklin, YewJersey . . . . . . . . . . . . .ManmmB (E.). Composition of Slate . . . . . .DAUBRBE (A,). Experiments on the Erosiw Action of Strongly CompressedHot Gases, with Reference to the History of Meteorites . . .ASDKEWS (T.) , Curious Concretion-balls derived from a Colliery MineralWater . . . . . . . . . . .Bnrcenite, a. New Antimonate from Huitzuco, Jlexico0 r g a h Chenzistry .ELTEEOFF.HESRY (L.).A Kew Unsaturated Sexvalent Hydrocarbon, Diallylene, C,WsTOXXIEB (P.). Action of Kitrous Acid on Unsaturated Hydrocarbons. .CLARKE (J. W.) . Some Seleniocyanates . . . . . . .RIBCTESE (L.). Alcohols in Potato Fusel-oil . . . . . .MIESSCHCTKIN (X.). Etherification of Primary Alcohols . . . .FLATTITZKY. Amy1 Compounds . . . . . . . . .BECPMAKX (E. 0.). Oxidation Products of Diethy1 Sulphide and AnalogousLIEBERYSKN (C.) and 0. HORXSXN. Glucoside of Buclit1;orn Berries andRhainnodulcite . , . . . , . . . . .BEREYD (L.). Isodulcite . . . . . . . . . .sCH3fIDT (E.). “ Mercurialine ” (?lethylamine) . . . . . .RFVSEFF (W.). Trimethylcarbamine . . . . . . .PISSER (1.) and I?. KLEIS Butyl Chloral I-lydrocyanke . . . .K R ~ I E K (C.).and 31. GRODZPI. The Acids of Wood-vinegar and theirconnection with the so-called Wood-oils . . . . . .3fILLER (W. Y.). Angelic Acids of Different Origin . . . . .BOTTINGER (C.). Monosulpholactic Acid . . . . . . .B~~TTINGER (C.). Action of Phosphorus Pentasulpliide on Organic Acids .CLAISEY (L.) and J. SHADXELL. Synthesis of Prroracemic Acid . .RIASCHIRSIIY (11.). Action of Zinc-methyl on the Bromides of Monobromi-nated Acid Radicles of the a-Series . . , . . . .PINKER (A,) and F. KLEIX. Conversion of Sitrils into Iniides . . .RCDXEFP (W.). Action of Iodine on Thiocarbmiides . . . . .LE BEL and GREEXE. dctioii of Zinc Chloride on Methyi Alcdhol ; Hex-methjlbenzene , . . . . . . . . . .Reactions of the Halogen Compounds of t,he OlefinesCompounds .. . . . . .RIATHEE (B.) , Snlphuretted Dicranodiamine . . . . .WALLACH (0.). Chloralide and its Deriratires . . . . .MSBERY (C. J.) and H. B. HILL. Dimethyluric Acid . . .PAGE902902903904905905906906102010201021102210231024102410249n534343 r,353636373739404040414143434.5454545464648484siv COSTENTS.PAGEA ~ S T E X (P. T.). On Dinitroparadibroinobeiizenes and their Deriratires . 50HEPP (E,), Some Addition-products of Trinitrobenzeiieancl other Sitro-com-poiinds . . . . . . . . . . . . . 50BOTTISGER ((3,). Action of Iniline on Glyoxxlic Acid . . . . 51ScHIrxIPjs (IV.). Parasylidine . . . . . 51ILES (31. \I7.) and I. R,EMSE~. Oxidation of Sulpliamidoxylke .” , .52JACOBSEX (0.). Osidatiori of Jletax~lenesul~liamide . . . . . 53FIscaEx (0.). Condensstioii-rroc?u~ts of Tekiarv droinatic Bases . . 53LAKDGRE~E (0.). Cyanogua$dine . . . . . . .HEISTZ (W,). Beiizalcliacetonamine . . . . . . . ,RATHKE (B.), rhciiSltliiocsrbaiiiic Acid . . . . . . .BESEDIKT (R.). Pentabromoresorcin . . . . . . . .PCHREDER (J,), Fluo ein-carbonic Acid . . . . . , .BESEDIKT (R.) . Trinitroso- and Trinitro-plilorogluciii. . . . .DALE (R. S.) aiid C. SCHORLEXMER. durin . . . . . . .CARO (EL) and C. G-R-AEBE. Rosoiic Acids . . . I . . ,BCCHKA (K.). Rednetion of Bcetophcnone . . . . . . .ESGLER (C.). A Sulphuretted Deriratire of Acetophenone , . .ESGLER (C,). Sulphuretted Deriratives of Benzophenone . . . .Jscousss (0.) aiid E.WEIXBERG. Dibromo-metaxjlene-sulphonic Acid .JACKSOX (C. L.) and A. W. FIELD. Parachlorobenzoyl Chloride and Bro-mide . . . . . . . . . . . . ,SOXXARCGI (E. v . ) . Tapour-density of Indigo . . . . . .SOKXARVGI (E. v.). Action of Aiminonin on Isatin, I1 . . . ,BJRTE (L.) ancl J. SCHREDER. Diphenol . . a . . . .LOSAXITCH (S. X ) . Action of Poiash 011 Tetranitrodiphenyl-cnrbamidt: .KELBE (IT.). ~al~litli~l-plioephol.uJ a i d Nnphthyl-arsenic Conipoulids .SCHGSCG (E.) and H. R o E n E R . 31ctabenzdioxyanthraquiiio11e . . .ESQLER (C.). Tetraplienglethane . . . . . . . .ZTLKOWSKT (C.). Aurin . . . . , . , .LASDGREBE (0.). Oxidation of Ditolylparabanic Acid . . .WREDEX ‘(F’.). Camphor- . . . . . . . . . .C I A X I C I . ~ ~ ((3.).Xeduction-products of Elemi-resin with Zinc.diist . .Lrca (S. DEJ. Sidittiiie ui3 of Crclamiii into Glucose and Mannite . .XESCI;; ( x j . anci N. S~EGR. Scw SFntliesis of Gilycocpuiine . . .Action of Ioclic Acid, ‘ I Snlphomoljbdic Acid,’’ and Ferric Chloride on Mar-pliine and other Substances . . . . . . . .E (0.). Remarks on Rice’s Articles on the &chona Alkalo’ids .E (0.). Substitutes for Quinine . . . . . . . .CP (Z. H.). Cinclionine and Cinchoiiidine . . . . .HESSE (0.). Iicmarlis on CinchoniIie and Cinchonidine . . ..ISCR ( P . ) , A Sen- Organic Base in tile Animal Organism . . .(0.). Lotur Bark . . . , . . . , . , .(0.). dmyriii and Icacin . . . . . . . . ,BOL-SSIXGAULT. Composition of the Milk of the Cow-tree . . ..LOSG (H,). Action of Alcoholic Potash on Bronioforin . . . ,Preparation of Etlirl Broniide . . . . . . . . -REBOTX. Iiomerisiu in the Propyl Series . . . . . . .FLIVITZPY (F.) and P. KRILOFF. Isoprop‘lacetjlene . . . . .WSLITZKY (IT.). Deriratives of Brain Cholesterin . . . , .LATSCHIXOFF (P.). Some Neutral Osidstion-products of Cliolesterin . .WITT (0.). Presence of Ethyl Alcohol in Coal-tar . . . , .SAYTZEFF (A. and P.). Preparation of Dipropyln.lly1 Carbinol . . .FLATITZI~Y (F.). Dehydration of Propylene-glycol . . . . .TOLLESS (B.). Specific Rotatory Poiver of Cane Sugar. . . . .FOUDLAKOTSKY (G.). Lactoglucose and Galactose . . . . .~IEYER (I-.). Occurrence of Furfuraldehyde in Glacial Acctic Acid . .KOHLER (H.). Decomposition of Ethyl Sulphates by G-aseous I€ydrocliloricAcid .. . . . . . . . . . . .EOHLEB (IT.). Action of lminonium Sdlphete on Barium Ethjlsnlpliate .53545455555755335961616161626263636&(i 76768686969707070717171717 273737312612712713 113513513613613613613713713713CONTESTS. SVPAGEKESSEL (F.). Bromo-derivatives of Ethyl Acetate . . . . .B~~TTIKGER (C.). Thioglycollic and Thiodiglycollic Ethers . . . .RICHTER (V. v.). .MEYER (R.). Hydroxjlation by Direct Oxidation . .SCHMIDT (E.) and R. SACHTLEBEY. Isobutxlforniio Acid (Inactive GaleriEAcid) . . . . . . . . . . . . .HECHT (0.) and J. MUXIER. Isolieptylic Acid from pHexyl Iodide . .HEITZELNAKT (R.). Dehydromucic Acid .. , . . . .REDSEFF (R7.). Trimethylcarbarnine . . . . . . . .BOTTITGER (C.). dcel~lene-carbamides . . . . . . .BITTIG (R.). Uric Acid Formula . . . . . . . .EORKER (H.). Pa~adipropylbenzene and its DeriTatires . , . .GEST.L~-SOS (G.). Broniination of Aromatic Hydrocarbons in presence ofAlumiuium Bromide . . . . . . . .BEILSTEIS (F.) anrl A. KVRBATOW. Chloranilines . . . . .BEILSTEIK (F.) and A. KERBATOW. Formation of Chloroplienylene-diamine . . . . . . . . . . . . .Malachite-green . . . . . . . . . . . ,HEISTZ (W.). Tanillo-diacetonamine . . . . . .BERSTHSEX (4.) and H. TROXPETTER.basic Organic Acids . . . . . . . . . . ,PINSER (A,) and F. KLEIN. Imido-thio-ethers . . . . . .GOLDJTEIK (11.). .GOLDSTEIX (31.). Dibenzoyl-clinitro-diphenol .. . . . .CARO (H.) and SCHRIUBE. Pherioldiazobenzeiie . . , . . .BAEXAXS (E.) . Hydrogen-Flicnyl Sulphato and similar Derivatives of t h ePhenols . . . . . . . . . . , . .GOLEBEFF. Action of Nitric Acid on DeosybenzoYn . , . . .FIT TIC.^ (F.). Nitrobenzoic Acids . . . . . , . .WIDXL~SK (E.) . Isomeric Nitro- and Amido-beuzoic Acids and Formationof Cliloranil from the latter . . . . , . . . .COLLET (T.). Sulplioparachlorobenzoic Acid . . . . . .SCHXITZ (H. J.). Substitution Products of IiIcsityleiiic Acid . . .SCHIFF (R,). Synthesis of ~Ietanitrocinnaniic .hid . , . . .METEX (R.) and J. ROSICKI. Oxypropylbenzoic kcid . . . . .BARTH (L.). Dioxybenzoic Acid . . . . . . . .BARTH (12.). Thymoloxycuminic Acid. . . . . .. .FITTIG (R.) and W. F. HILLEBIUSD. Quinic Acid . . . . .ETTI (C.). Jlalabar-kino and KinoYn . . . . . . . .JOHASSOY (E.) . Chemical Constituents of the TTillow and its PathologicalFormations j certain Reactions rrith Tannins and Allied SubstanewLA COSTE (lv.) and -4. BIICHIELIS. &lono- and Di-plien!-l Compounds ofArsenic . . . . . . . . . . , . .La COSTE (J37.) and d. 3IICH.iELIS. .L a COSTE (IT.) and A. MICIUELIS. .SCHMIDT (H.) and G. SCIITLTZ. Diphenrlbenzenes . . . . .FITTIG (R.) and A. SCHMITZ. Diphenylen~-inethane . . . . .ITZ (A). Diphenylene Iietoiie and Phenj-lbenzoic dcirl . . .IEL (J.). Diphenic Acid . . . , . . . . .NELDOLA (R.). ~aphtlinleiie-derivntires . . . . . . .FITTIG (R.) and F. GEBHARD. Fluoranthene, a new H>-clrocarbon fromCoal-tar .. . . . . . . . . . .G O L D S C H ~ U T (G.j. Idrialin . . . . , . . . .FLATITZKY (F.). Structure of Terpenes . . . . . . .FLATITZKY (F.). Dextro-gyrate Terpene from the Turpentine of Piamsy lcestris . . . . . . . . . . . .SPITZER (F. T.). Camphene from Camphor, and its Homologues. . .SPITZER (F. T,). Caniphoi* Dicliloride . . . . . . .C L A ~ S (-4.). Cinchona Alkalo'ids . . . . . . .Action of Phosphorus Pentachloride on Ethyl OxalsteAmidiues and Thiainides ofAction of Sitric Acid on Phenol and on SitrophenolTriphenylarsine and its Deriratir-esJIonotolyl Compounds of Arsenic137138138139139140141141142142142142143141.134144146147148148148148150150154155155157157157158159159160161162163163164164165165165167167168168168168 .. . . . .DRYGI;. 'A New Quinine Salt . . . . . . . . . 16svi UOSTESTS.DRYGIS. Cinchonichine, a ISew Cinchona Sllialo'id . . . . .DURASD. Bark of the Root of the Pomegranate . . , . . .TANRET ((2.). Pelletierine, aBase from the Bark of the Pomegranate . .DISQV~ (L.). Urobilin . . . . . . . . . .HOLDERXASX (E.). Iron Blhuminates , . . . . . .lline Structureof Bees'-wax . . . . .(B.). Const,itnents of Hops , . . . . . ..). Colonring Matter of Rctl Wine . . . . . .STAEDEL (T.), Halogen-deriratives of Etlisne and Ethylene . , .SAYTZEFF (A,) and SCHISOEOFF. Diethyl-all11 CaibinolSAYTZEFF (A. and P.) and A. NIXOLSKY. Action of S u i p l k c Scid 01;MESSCH'CTKIS ( Y .) . Etherification of Secondary Alcohols , . . .MESSCHTTXIN (Xu'.). Etherification of Tertiary Alroliols and Phenols . .THOVSET (L.). Action of Potassium Cyannte on Epichlorliydrin , . ,RODEFALD (H.) and R. TOLLEXS. Rec1uct)ion of Cupric Oxide by MilkAll~ldiniethylethyl- and Allyldipropyl-carbinol . . . .Sugar . . . . . . . . . . . .WOLFRAM (G.). Sitro-componnc1e of Cellnlose . . . . . .PATLEY ~ (C.) and R. OTTO. Decompoeition of Eth>-l Disulphoxide byFotash . . . . . . . . . . . , .K&ELER (H.). Formation of ELh! laniine . . . . . . .HOFXAXX (A. W,). Formation of &thy1 Aldehyde . . . . .GEFTHER (-4.). Diethylglxoxylic Ether and Diethylglroxylamide . .DEMOLE (E.). Formation of a IieLone containing four Carbon At,onis fromDibromethplene .. . . . . . . . . .KESSEL (F.). Decomposition of Ethyl Monobrom- and Dibrom-acetate .ZORS (IT-.). Diazo-compounds of the Fatty Series . , , . .SCHXITT (E.). The Volatile Acid of Croton 011 . . . . . .~ S S C H E T Z (R.). Action of Ethyl Iodide on the Silver Salts of Maleic andFumaric Acids . . . . . . . . . . .STAEDEL (W.). Racemic 4cid . . . . . . . . .Jacxsox ( 0 . R.) and H. B. HILL. Nucobromic Acid . . . . .DITTRICH (E.) . l\rethpltanrine, Methgltaurocgumine, and Tanrocyami:ie .PONOMAREFF (J.). A411nntoxaiiic Acid . . . . . . . .ADOR (E.) and d. RILLIET. Hydrocavbotis obtainei by the Action ofdliiniiniuin Chloride on Methyl Chloride and Benzene . . . .JACOBSEX (0.). Constitution uf the Prop$ Group in Cvrnene: ..BECKCRTS (H.) and R. OTTO. Mode of Action of Sulphuric H;rdroxyclilorideGERICHTEX (E. T.). P-Chlorocymene from Tlirmol , . , . .BEILSTEIN (F.) and A. KERBATOW. Action of Hydrogen Sulphide on certainKLEIX (0.). Compounds of Organic Bases with ?iIercuric Chloride . .LADEYBI-RG (A,). Experimental Determination of Position. . . .IADESB'CRG (A4.). Simple Method for preparing Sldehydincs . . .LADEXBVRR (k.) and L. RUQHEIMER. The Aldehydines . . . .LADESBURQ (4.) and T. ENGELBRECHT. Some Plienjlaldehydines . .GOLDSCHMIDT (A). The Three Isomeric Tolidines . . . . .FISCRER (E. and 0.) Certain Colouring llattere of the Rosaniline Group ,BARSYLOTSKY. Azo-hiratires of Toluene . . . . , . .BLSTLIS (A). hhtanitrophenol and its' Deriratires .. . . .STAEDEL (W.) and C. DAXM. Bromonitro- and Bronianiido-aniso'il . .PRI-SIER IL.). Quercite . . . . . . , . . .STAEDEL (W.) and E. SAUER. Dinitrobenzophenone . . . . .BECK-LRTS (H.) and R. OTTO. Spntheeis of Sromatic Sulpliones . . .OTTO (R.) and A. KSOTT. Action of Sulphuric Hgdroxrchloride 011 Sul-POSOXAREFF (J.). Some Deriratires of &lanto'in . . . .Xitro-compounds . . . . . . . . . .. .phobenzide . . . . . . . . . . . .PAVLY (C.) and R. OTTO. nisulphoxides of Benzene and Toluene . .AXXIHEIM (J.). Trtranitro-oxpsulphobenzide . , . . . ,JAXXASCH (P.) and C. EUXP. . Discovery of Vanillin in Siam Benzoin.PAGE169169170170170171171171212214214215215217217218219219213220270220221221273213224225226228225228229230230231232233233234.235236237237"sj23924224224.324324424CONTESTS. xviiGABRIET.(s.) and A. MICHAEL. Action of Dehydrating Substances onGBIESS (P.) Deriratives of Benzoic dc'id . . . . . . .JACOBSES (0.) Constitution of Oxpesitylenic Bcid . . . . .JAHK (H.). Valonia and certain other Sources of Tannin . . . .REJZSEN (I.). Oxidation of Xylene-sulphaniicles . . . . . .AROSHEIM (B.). Synthesis of the Compounds of Phenol wit,h Tin . .DIEHL (T.) and V. MERZ. Naphthopicric Acid and Some of its Derivatives,STBEDEL (W.) and KLEISSCHXIDT. Iso-inclol . . . . . ,SCHUIDT (H.) and G. SCHULTZ. Diphenyl-bases . . . . , .EWBLD (€1.). Some Coerulignone Derivatives .. . . . .GRXTZEL (.I.). Eupittone and Pittacal . . . . . . .PERGER (V.). Deriratives of Anthraquinone . . . . . .LIEBEBMISN (C.) and K. BOECK. Antliracene-disulphonic Acid and itsConreraion into dnthrarufin . . . . . . . . .GRBEBE (C.). Alizarin Blue. . . . . . . . . .LIEBERXBNN (C.). Synthesis of Bnthrarufin and Clirysazin from dnthraceneKESSEL (F.). W a s of Ficus g u m m i ~ ~ r a . , . . . . .HIRSCH (B.). Investigation of Balsomuin antarthriticuin indicuin . .RAMSAY On Picoline and its Deriratires . . . . . .MEYER (5.). Absorption-spectra of Solutions of Brucine, ;\lorphinu,Strychnine, Veratrine, and Santonin in Concentrated Acids . . .HESSE (0). Further Remarks on Alstonia const,.icta . . . . .BLFMBERQ (T.). Contribution t o a Knowledge of dlkalo'ids of Ergot ..PICCARD (J.). Cantharic Acid and it Hydrocarbon, C8HI2 . . . .LIEBERXANN (C.) and 0. HORNBXX. Formuls of Rhamnetin and Xmtho-rhamnin . . . . . . . . , . .BBRBIERI (J.). Aibundnoids of Gourd Seeds . , . . . .COQUILLON (J,). Action of Platinum Wire on Hydrocarbons , . .MERZ (V.) and W. WEITH. .NERZ (V.) and W. WEITH. .NIZTLDER (E.) and 8. J. IT. BREMER. Action of Chlorine &Ionoxide onAnhydrides . . . . . . . . . . .Action of Bromine on the Lower ParaffinsAction of Bromine on the Higher ParaffinsEthylene . . . . . . . . . . . .DESCAJWS (1.). Potasaium Cobaltocyanide . . . . . . .MEYER (G ). Action of Carbonic Anhydride on certain Cvaniiles . .SCHXITT (R.) and 0. MITTESZWEP. kction of Diazo-co&pounds on EthJ1BLEVKARD (A,).Action of Trimethylaniine on Carbon Bisulphide . .DOVILLIER (E.) and A. BUISIKE. Separation of Ethylamines . . .EELLY (0. J.). Action of Chlorocarbonic Ether on Halogen Compounds ofthe Fatty Acid Series . . . . . . . . . .KESCKI (11.) and F. SCHAFFER. Action of Chloral Hydrate on AmmoniumThiocyanate . . . . . . . . . . . .JAGI. Peonis 3loutan. . . . . . .KR~FFT (I?.). Conversion of LTndecylenic Acid iiiio Uhclecilic Bcid . .TASJIEIARI (G.). Deriratires of Amchidic Acid . . . . . .MILLER (W. v.). Dimetbrlacrylic Acid . . . . . . .OST (H,). Pyromecoriic Acid . . . . . . . . .SCHIFF (R.) and G. TASSISARI. Tu-o Monobromoppromucic Acids . .GCSTAT-SON (H.). Compouuds of Sluminium Chloride with Benzene andNercaptan .. . . . . . . . . .Toluene. . . . . . . . . . . . ,PATERK~ (E.). Constitution of Cumic Compounds and of Cpmene . .PRUNER (L.) and R. DAYID. Crystalline-products obtained from Penns,l-ranian Petroleum . . . . . . . . . .ZORS (TV.1. Action of Nitrosyl-sliver . . . . . . . .BEILSTEIN (F.) and A . KVRBATOW. Chloronitranilines . . . .MOKNET (P,), F. RETERDIN, and E. XOLTISG. llethylated Derivatives ofAniline and Toluidine, and the Colours obtained therefrom .FRIEDERICI (T.). Action of H?drogen on ~~etaiiitro-parati,ichlorace~o.to-to:luide and Z/letanitro-paravalerJl-toluide . . . . . . .VOL. XXXYI. bPAGE245246248248248249250262252253253253257259260261262262269269269270Z i l27230230230230330330330430530630630630630630730730730830530830'330930931031xyiii COSTESTS.DOEBNER (0.).Malachite Green. . . . . . . .MAGATTI (G.) . Action of Sulphnric Anhydride 011 Phenyl-thiocarbimide .WALLACH (0.). Organic Thio-compounds . . . . . . .SCHUITT (R.) . Preparation of Azobenzene from AnilineKOETIGS (W.). Action of Fuming Nitric Acid and of ?rTitro;s Acid odBenzene-sulphinic Acid . . . . . . . . . .BENDIX (J,). Derivatives of Ortho-nitrophenol . . . . . .PATERH~ (E.) and G. MAZZARA. Benzylated Cresol . . . . .HIRSCH (R,,). The so-called Dichlorazoplieriol . . . . . .GRIESS (P,). Action of some Diazosulphonic Acids on Phenols . . .ScxnrITT (R.) and R. MOHLAU. .TH~~RSER (W,) and T. BIHCKE. Pinacones and Pinacolines.Part IT .DENTSTEDT (31.). Benzyl Orthothioformato . . . . . .YRAETORITJS (H.) . Nitration of Benzophenone, Benzbydrol, and Diphenyl:Azoxy- Azo- and Hydrazo-phenetols .STAEDEL (W.). Benzophenone . . . . . .. .methane . . . . . . . . .Synthesis of ’Oxyketones by introducingAcid Rtidicles into Phenols. Part I1 . . . , . . . DOEBNER (0 ) and W. STACEYA?~N.MARTIN (G,). A Japanese Cinnamon Bark . . . . , . .ETARD (A,). Oxidation of Aromatic Compounds. . . . . .@RIESS (P.), Action of Cyanogen on Amidobenzoic and Anthranilic AcidsSCHIFF (X.). Metanitrocinnamic kcid . . . . . . . .ST~CKENIUS (0.). Phenylamidacetic Acid . . . . . . .TH~RSER (W.) and T. ZINCPE. Diphenylmethylacetic Acid. , . .CLAISEN (L.) and F. H. MORLEY. New Method of‘preparing PhenylgljosylicAci,l .. . . . . . . . . . . .GERICHTEN (E. v.) and W. ROSSLER. a-Oxyparatoluic acid. . . .GABRIEL (S,). Substituted Phthalanils . . . . . . .FRIEDERICI (T.). Kew Method of Preparing Chrpnisic Acid . . .GAIL (F.), Oxidatiou of Dioxydiphcnyimethane . . . . . .FIscHER (E. and 0.). Triphenylmethane . . . . . . .LIEBEEXASS (C.) and P. SEIDLER. Chrysarobin in I ‘ Goa Powder” . .BRECER ( A , ) and T. ZITCKE. Derioatires of the Hydrocarbon, CI,HI?, fromPhenyl Glycol . . . . . . . . . . .MOXTGOLFIER (J. DE). Derivatiyes of Terebenthene . , . . .HALLER ( A , ) . Iodocnmphor. . . . . . . . . .HALLER (A,). Cyano-derivatives of Camphor . . . . . .FORCRASD. Organic Gltramarines . . . . . . . .K ~ T z u J ~ M .~ . Inrestigation of the Seeds of Camdliajaponica . . .MARTIN (G,), Con>tituent,e of Ligustrum I b o t u . . . . . .CASTIZZARO (S.) and CARKELUTTI, Two Isomerides of Santonin . . ,CAXSI~ZARO (S.) and L. VALENFTE. Santoniii Deriostiws . . . ,HESSE (0). Cinciiotenicine . . . . . . . . .HLRXACK (E,). The Basic Constituent’of Dita Bark . . . . .MARTIN (G.). Scopotiajaponica . . . . . . . .~ I A R T I ~ (G,). Ecodia glauca . . . . . . . . .DESTREX (-1,). Cholic Acid. . . . . . . . . .FREI)ERICQ (L.), Hemocyanin from the Blood of the Octopus vu7gari.s .STAEDEL (\IT.). Halogen Derivatives of Ethane . . . . . .DEXZEL (,J.). Sonienclature and Boiling L’oints of the Clilorobromo-subst,i-tution-products of Ethane and Ethylene . . . . . ,REBOTL.Et~liylidene Chlorobroniide . . . . . . . ,LE ELL (J. A,), Dextrogyrate Amy1 Alcoliol . . . . . .DCRIS. Inversion of Cane-sugar, and Consecutive Alteration of thc Glucoseuso formed . . . . . . . . . . . .PATERS~ (E.), Propylbenzoic Acid . . . . . . .in Aqueous Solutions . . . . . . . * .FRITZSCHE (P.). Oxypheuglacetic Acid . . . . .BECK (C.). Diorpdi~henyimethane . . . . . . .HESSE (0.). Alstonia Bark . . . . . . .PAQH31 231231231331431431431531531731 7318318319319320320321521321322322322322323323324324,3253263263213283293‘9329330330330331332338333333333333333368368311936936COSTESTS. X1SPAGE37037137.'3723733 i . i37637ti3763763703763773%378379380382383383384386387387388389389390391446447447447448,149449449449450450'1514624 524 52453453453454464Mrsco~cs (F.) and J.DE XERISR. Action of Dinstase, Saliva, and Yan-WOLFRAM (G.). Nitro-derivat,ives of Celldose . . . . . .PETRI (C.). Fumaric and Maleic Acids . . . . . . .NEVER (E. v,). Some New Platinum Compounds : Fuluiinoplatinunls. .GRIMAUX (E.). Synthesis of Uric Acid Derivatix-es : Alloxan, Uraniil, M u -rexide, &c. . . . . . . . . . . .BERTHELOT. Hydrogenation of Benzene and Aromatic Compounds . .BBILSTEIS and KOCRBATOFF. Dinitrochlorobenzene . . .FITTIG (R,). Formation of Unsaturated Hydrocarbons from the Adciition:DESTREX (A.), Compounds of Metallic Salts r i t h Compound Ammoniss .VALITSKY. Action of Aniline, Toluidine, and Xaphthylamine on ClwlesterylChloride .. . . . . . . . . . . .MAILLOT (E,). Aniline-derivatives of Sebacic Acirl . . . . .POSEN (E.) . AmidohSdro-cinnamic Acid (PhenSlamido-propionic Acid) .F~TTIG (R.) and F. BISIIER. Addition-products of Cinnaniic Acid . .HEBNER (H.). Xitrosalicjlic Acids and the Isonierism of Eenzsne Deriva-tives . . . . . . . . . . . . .STAHLSCHMIDT (C.). Polyporic Acid . . . . . . . .erepitic Juice on Starcli rind Glycogen . . . . . . .REBOUL. Diallyl-acetic Acid . . . . . . . .products of Non-saturated Bcids . . . . . . . .GROTHE (A,). Metaiodonitro- and Metaiodamido-benzoic Acids . . .BITTIG (R.) and C. WCRSTER. Btropic and Isa1,ropic Acids .. .GIR~RD and PSBST. Nitroeyl-derivatives . . . . . .ROSEXSTIEHL ( A , ) . Antliraflarone and Anthraxanthic i c i d . . . .FIPCHER ( E . and 0.). Triphenylmethane and Rosaniline . . . .TILDEN (W. A,). An Examination of Distilled Essence of Lemon . .BLFJYBERQ (T.). .TAPPEISER (H.) . Action of Potassium Dichromate and Sulpliuric Acid onCholic Acid . . . . . . . . . . . .GAL (H.) and A. ETARD. Recearches on Strychnine . . . . .Contribution to a Iinowledce of the klkalo'ids of ErgotEORN ( S , ) , Decomposition-products of dlbumino'ids . . . .LOEF (0.). Oxidation of Albumin by the Oxygen of the A i r . . .RITTHIFsEN (H.). Albuminoyds from Castor o i l Seeds . . . .JONES (H. IT.). Amount of Ash and Soluble Matter in three kinds ofBuchu .. . . . . . . . . .PEBAL (L.). Action of Hypochlorous i c i d on Ethjlene . . . .FRVNIER (L.), Hydrocarbons from American Petroleum . . . .LIITXANK (E.) and J. HAWLICZEK.SAYTZEFF (A,).Eikoajlme, ra Derivative of LigniteParaffin . . . . . . . . . . . .Action of Dilute Snlphuric Acid on Allyld~methjlcar-binol . . . . . . . . . . . . .SCHIROKOFF and 8. SAITZEFF. Allyldieth~lcarbinol . . . .BERTHELOT. Influence of >Ictnllic Chlorides on Ethcrification . . .Houx.4~~ (,T. 7.). Action of HFdrocjanic Acid on Epichlorhyclrin . .HAXHIOT. On Glycide . . . . . . . . . . .IIBSIG (ill.) and M. ROSBNFELD. Sugors . . . . . . .VILLIERS (A4.). Annlysis of Honey froin Ethiopia . . . . .BOTTIXGEE (C,). 'Conversion of Aldehyde into Mel:captan .. . .SCliIFF (R.). Action of Aldehydes on Chloral-amnionis . . . .AltosaEInr (B,), On Schiitzenberger's Chlorine and Iodine Acetates . .COSRCD (N.) Identity of Ieopi*opionic Acid and Lwvulinic Acid . .DEUTSCH ( A , ) . Etheren1 Snlts of Ti.ih;tsic Formic Aciti . . . .WALLACH (0.) and 0. BIBCIIOF. Dec*oinposition of Dicliloracrylic Acid byFISCNER (E,). Hvdirazine-conipound~ of the Paraffin Series . . .FRASCHIXONT (K.). Zinc Acrtatr . . . . . . .Alkalis . . . . . . . . . . . .Acids obtained by the Saponification of Roman Chamoinile- Eorr (H,).011. . . . . . . . . . . . . .K~BIG (J.). Constituents of Roman Chamomile-oil . . . . .b - xx COSTENTS.PAGENSTECHER (A.). Angelic and Tiglic Scids . . . . . .FITTIG (R.). Constitution of Tiglic and Angelic Acids.. , . .BOURGOIN (E.). Bromocitraconic Acid . . . . . . .D E M A R ~ Y (E.). Tetric Acid and its Homologues . . . . .D E X A R ~ Y (E.). Homologues of Oxyheptic Acid . . . . .DEXAR~AY (E.). Relations of Tetric and Oxrtetric Acids and their Homo- .GRIXAVX (E.). Synthesis of Uric Acid Deriratives . . . . .PONONAREFF (J.). Compounds of the Uric Acid Group . . . .GUSTATSON (G.). Compounds of Aluminiuui Chloride with Benzene andLIPPMANS (E.) and G. ~ O R T X A N S . Componnds o i Codalt and Xickel khlor:logues to Succinyl, Malyl, and other Radides of t,he Bibasic AcidsToluene . . . . . . . .ides with Anilines . . . . . . . . . . .BECCHI (G. v.). Succinyl-compounds of Toluidine . . . . .T,iPPxANx (E.) and W. STRECKER.Amylidene-aniline . . . .KRAUSE (A,). ' Parapheiirlenediamine . " . . . . . . .WEITH (W.). Synthesis of Carbotriphengltriamine . . . . .ROSESSTIEHL (A.). Constitution of the Rostrnilines . . . . .BEILSTEIN (F.) . Perchlorophenol Chloride . . . . . . .LIPPYAKN (E.) and W. STRECKER. .NIETZXI (R.). Derivatives of Qninol (Hydroquinone) . . . . .AROSHEIN (B.). Action of Nitrous Acid on Resorcinol Ethers . . .SALKOWSKI (E. and H.). Formation of Hydrocimamic Acid by mrans ofPancreas Ferment . . . . . . . . . . .METER (R.) and J. ROSICKI. Hydi-oxypropylbenzoic Acid . . . .GRIESS (P.), Amidobenzoic Percganide . . , . . . .GKXARD (A,). Laurent's '' Carminapht,ha . , . . . , .XELBE (W.). Hydrocarbon from Rosin-oil . . . . . . ,QCHELZE (E.) and J.BARBIERI. Lupinin, a New Glucoside , . . .HOFFNAXN (E.). Narinpin . . . . , . . . . .FRAKCHIXONT (N.) and WIQXAN. Lactucone . . . . . .FRANCHIMOXT (3.) and WIQXAS. Betulin . . . . . . .The Colouring-matter of Sandal andCaliatour Woods . . . . . . . . , . .Nitrocuminol and its Derivatives .BENEDIKT (R.). Pentabromoresorcinol . . . . . . .SCHIFF (H.). Digallic Acid . . . . . . . . .STWKKEL ((3.). Daphnetin . . . . . . , . .HARZ (C. 0.). Spergulin, a R'ew Fluorescent Body . , . .FRASCHIXONT (N.) and SICEERER.FRAUDE (G.) . Aspidospermine . . . . . , . . .KRAVSE (H.) and G. SALOXOX. Formation of Xanthine Derivatives fromWEYL (T.) . Crvatinine and Creatine . . . . .PAGE45545645 745745845946046146146146146246246246346346446446 4465466465466466466467467468468469469469470470471. .Albumin .. . . . . . , . . . . ,R~TIGS (W.). Oxidation-products of Cinchonine. . , . . ,TOSXIES (P.) . Action of Nitrosrl Chloride on UnPatkrated HydrocarbonsHERZIG (J.). Two New Isomerides of Cyannric Acid . , . , .MUSCC-LUS (F.). Modifications of the Phgsical Properties of Starch . .HIORTDAHL (M.). Crystalline Form of the Stannmethyl Compounds andURECH (F.). Action of Potassium Carbonate on Isobutylaldehyde . .BRUHL (J. W.). Preparation of nivaleryl . . . . . . .BARDY (C.) and L. BORDET. Preparation of Methyl Formate and PureKAHLBAUM (8. W. A,). Physical Properties of some Methyl Compounds of3- and 4-Carbon Acids . . .. . . . . . .HELL (C.) and P. SCHOOP. DibromocRpric Acid . . . , . .WERIGO and MELIKOFF. Monochlorolactic Acid and Dichloropropionic Aridfrom Glyceric Acid . . . . . . . . . ,BOTTINGER ((3.). The Amount. of Water contained in Crrstallised CalciumGlycollate . . . . . . . . . . . .RANMARSTEX (0.). Paraglobulin . .. . . . .their Homologiies . . . . . . . .Methyl Alcohol . . . . . . . . . .47141147251751751851 852052052052152152152CONTEXTS. xxiSCEKEINER (L.). Boi!ing points of the Ethereal Salts of Hydroxy- andDU~ILLIER (E.). Derivatives of Normal Methox&utyric Acid . . .BAXDROWSKI (F.). Reaction of Dibromoanccinic Acid with TVaLer , .BOTTIXQER (C.) . Pyroracemic Acid . . . . . .BELL (C. A.) and E. LAPPER. Dry Distillation of Ammonium S i t s ofSaccharic Acid ., . . . . . . . . .BELL (C. A.). Pyrrol Derivatives . . . . . . . .WROBLEVSPY (E.). Structural Formula of Aromatic Compoutnds . .ADOR (E.) and A. RILLIET. H-drocarbons produced by the Action of.BECHI (G. T.). Succinyl Compounds of the Toluidines . . . .MICHAELIS (A,) and F. DITTLER. Reactions of Phenylphospliine . .SALKOWSKI (H.). Behaviour of Xetanitraniso’il towards Ammonia . .BECIZI (a. T.). New Mode of Formation of Ketones . , . . .JACOBSES (0.). Products of the Action of Fused Potash on PotassiuniJlesitjlene-suiphonate . . . . . . . . . .SOXKARL-GA (E. r.). Molecular Weight of Indigo . . . . .CLAISES (L.) and J. SHADWELL. Synthesis o> Isatin , . .BAEYER (A). Action of Phosphorus Pentachloride on Isatin and Allied‘Com:PAWLOW (D.). Tetramethylethylene a n i its Derivatives ..FITTIQ (R.) and H. LIPPJIANX. Constitution of Isodiphenic. Acii a n iFluoranthene . . . . . . . , . . .SMITH (W.). Vapour-densities of the three Isomeric Dinaphthyls , .LIEBERMAss (C.) . Reduction of Bnthraqninone-sulphoiiic Acids . ,LIEBERJIAXN ((3.). Anthracene Derimtives of the Chrysazin Series . .SCHKJLTZ (G.). Constitution of Phenanthrene . . . . . .ANSCHUTZ (R.) and G. SCHULTZ. Phennnthrenequinone , . . ,BALLO (If.). Action of Dehydrating Agents on Caniphoric and CemphoramicAcids . . . . . . . . . . . . .KOESIGS (W.). Svnthesis of Chinoline froin Allylaniline . . . .WEYL (T.). Decomposition of Tyroeine by Putrefaction . . . .HOOGE~-ERFF (9.) and W.A. r. UORP. Oxidation of Quinine by PotassiuniAlkyloxy-Acids . , . . . . . . . .TOLLENS (B.). Oxidation of Levnlinic Acid . . . . .Methyl Chloride on Benzene in presence of Aluminium Chloride .SCHFXCP (E.). Indigo-blue . . . . . . . . .pounds . . . . . . . . . . .XOEXIGS (\%-.). $itrochinoline . . . . . . . .Permauganate . . . . . . . . . . ,HILGER (A). Solanine and the Products of its Decomposition , . .H ~ T E T (F.) . Sarrwenia Purpurea . . . . . , . .SCHUTZEXBERGER (P.). Researches on Albnniin . . . . . .SCHROEDER (K.). Specific Gravity Determinations of Solid Organic Com-pounds . . . . . . . . .BERNHEIMER (0.). Organic’Ferr&anr&en Compounds . . . .VINCEXT ((2.). Presence of Xitrils in the Distillate obtained by the Calci-nation of Residue from Beet-root Molasses .. . . . .PIERRE (J.) and E. PZTCHOT. Products of Distillation of Akkohoh . ,CRIB (L.), An AmyloidSubstance peculiar to the “Asques” of PyrenoqcetesTHONSEN (‘J?.). Composition ot Wood. . . . . . . .JOTJSSELIN (L.). Kitrosoguanidine . . . . . . . .BYE (9.). Removal of Sulphur from Ouanidine Thiocyanate . . .LIEBEN (A.) and S. ZEISEL. Crotoii Aldehyde and its Honiologues . .EALBIANO (L.). a-Isochlorobutyric Acid and its DerivatiTes . . .HILL (H. B.). Di-substitution Derivatives of Acrylic Acid . . . .EXBETT (W. Z.) and H. B. HILL. Dichloracrylic Acid . . . .SCHXIDT (E.). Methylcrotonic and Angelic Acids. . . . . .SEMLIANI~ZIFE and A. SAYTZEFF. Oxyvaleric Acid from Allyldimethyl-carbinol ., . . . . . . . . . . .RIOBININE and A. SAYTZEFF. Diallylisopropyl carbinol . . .HARTWIG (E.). Oil of Wine. . . . . . . .PAGE5225235235 245245245255265 27527528528529529532532534535536536637537537538238539510j 4054 15415115-4154261061161261261261361361361461561561561661661761sxii COSTENTS.SCHJIDQER (M,). Isomalic Acirl , . . . . . . . .MELDER (E.). SyntheBis of Dimethylbarbituric Acid . . . . .BOTTIXQER (C.). Glyoxylic Acid. . . . . . . . .CALX (A,). Constitution of Pamdanic Acid. . ,ANDRIANOW~EY (A,). Action of Aluminium Chloride on kcetic a n i Sul-‘LOIR. Chemical Functions df Acetic Anhydride . . . . . .DE FORCRAND. Formation of Glycocine from Ethyl Nitro-acetate ..COUNCLER (C.). Boron Compounds . . . . . . . .CAEOURS (A,). Iodides of Stannopropyl . . . . . . .PREIS (K.) and B. R-~YXAXN. Action of Iodine on Aromatic Compoundswith long Side-chains . . , . . . . . . .JACOBSEN (0.). IsocTmene . . . . . . . . . .MONTET (F.), F. REGERDIN, and E. YOLTING. Presence of Metanitrotoluenein Commercial R’itrotoluene . . . . . . . . .MONSET (F.), F. REVERDIN, and E. SOLTISG. Influence of Metatolaidine inthe Preparation of Rosaniline. . . . . . . . .I’AXEBIANCO (R.). Dimorphisniof (1 : 4) 4’cetotolnide . , . .WURSTER (C.) . Methyl-derivatives of Paraphenylenediamine . . .SENDTNER (R.). Action of E t h j l Oxalate on Dimethlolparaplien~lenedis-mine . . . . . . . . . .BINDER (F.) .DimethSiparapheuflenediamine Carbamides . . . .BAOR (1.). Dimethylparaphenylenedianiine Thiocarhamide. , , .KOCH (A,), Colouring Matters containing Sulphur derived from Dimethyl-FAELBERG (C.) and I. REMSES.ORIESS (P,). Remarks on Weselsky’s and Eenedikt’s Investigation on someSCHMIDT (H.) and G. SCHULTZ. Azo-, Azoxy-, and HFdrazo-Compounds ,SPICA (P.). Proprlphenols and other Deriratires of Propylbenzene . .BARTH (L.) aiid J: SCHRFDER. Action of Fused Soda on Phenol. SynthesisBARTH (L.) and J. SCHREDER. Oxidation of Resorcinol to Pliloi.;glucinol :HESSERT (J.). Phthalyl Alcohol . . . . . . . .SCHPLTZ (E.). Specific Rotatory Power of Isochoiesterin . . . .BAEYER (A,). Diphenylphthalide and %henflphthale:n . . . .DOEBSER (0.) and W. WOLFF.Synthesis of Ozyketones . . . .FISCHLI (H.), Paratoluic and Terephtlialic Acids . . . . .GABRIEL (9.) and J. ZIIIXERZIASN. Dinitrohydrociiinamic Acid and itsDerivatives . . . . . . . . . . . .OGLIALORO (A,). Phenylcinnamic Acid . . . . . . .VCLPIVS. Salicvlates and their Application . . . . . .I(GHr.ER (H.). ‘Ethereal oils of some Ericaces . . . . . .JACOBSEN (0.). Hydroxyparaxylic Acid . . . . . . .SAARRaCH (L.) . Piienplosppropionic Acid . . . . . . .PATERSb (E.) and G. n/lAZzaRA. Cumolcarbonic Acid . . . .JACOBSEN (0.). Sulphanlinemesitglenic Acid and a New HjdrosynxsitJ-1-enic Acid . . . . . . . . . . .GRUBER (M.). .BARTR (L,). DioxSbenzoic Acids . . . . . . . .BEILSTEIN and KURBATOFF. Nitrophthalic Acid obtained by Oxicltttioii ofSitronaphthalene .. . . . . . . . . .ANSCHUTZ (R.) and L. P. KINSICUTT. Phenylgljceric Acid . . .FREDA (P.). Preparation of Digallic Acid . . . . , . .SCHIPF (H.). Digallic Acid . . . . . . . . .HRUNNER (H.). Deoxalic Acid . . . . . . . .phuric Anhydride . . . . . . . . . .DE FORCRAND. Formation of Organic Vltramarines . . . .WPRSTER (C.) . Xitrodimethylaniline . . . . . . .paraphenylenediamine . . . . . . . .Oxidation of Orthotoluene SulphamideAzo-Compounds . . . . . . . . . . .of Phloroglncinol . . . . .PREIS (R.) and B. RAYMASX. Cholesterin . . . . . .FRAEDE (G.) . OrthocresolphthaleIn * . . . .Action of Yitrouu AnhFdride on Pi-otocatechuic Acid .PAGE61861861961962062062162 1621 .~62862262362 L62.56256266266266276276286286286296306316336336346346346346366386386396406416116416426426436436446446446456 1COSTENTS. xxiiiPAGE6 476996496496506506516516516526536536546556556.55656656656657658659660660661699700700700701702703703709705705705705706706707707708710712712713713714714714C'LAISES (L.).Benzoic Cyanide and Phenylglyoxylic Acid . . . .CLAISEV (L.). Amides of Phenylglpoxylic Acid . . . . . .LENZ (W.). Fluobenzenesulphonic Acid, and the Nelting Points of Substi-tuted Benzenesulphonic Acids . . . . . . . .BERSTHSEN (A.) and H. KLIKGER. Sulphine-compounds of ThiocarbamideAROSHEIX (B.).Action of Kitrous Acid on Staniiic ihenyi Chloride . .SCHXIDT (H.) and G. SCHKLTZ. Diphenols . . . . . .SCHXIDT (H.) and G. SCHCLTZ. Diphenyl Bases . . . . . .SCH-CNCP (E.) and H. R,OEMER. a- and p-Nitroalizariu and i-Amidoalizarin.PICCARD (J.). Derivatives of Cantharadin and their Relation to the Ortho-series . . . . . . . . . . . . .Oxidation-products of Cinchona Bases . . . . .OTTO (R.). Sulphonic Acids derived From Sulphones . . . .8CHT.4RZ (H.) Formula of Hippara5n . . . . . . .LARGE (A). Diphenjlthiohydanto'fn . . . . . .SCHKLTZ (G.). Constitution of Phenanthrene . . . . . .LIEBERYAKS (C.) and 0 . HORXASN. Anthrol . . . .GRAEBE (C.). Alizarinsulphonic Acid . . . . . . . .FILETI (If.). Cinchonine . . . . . . . . .IIESSE (0.).Conquinine Sulphate . . . . . . .TEIDEL (H.). Berberine . . . . . . . . .PETIT (-1.). A New Alkalo'id . . . . . . . . .SICRBGP (H.).T-~FRET ('2.). Alkalo'ids of t.he Pomegranate . . . . . .SALKOWSKI (H.). Products of the Fermentation of Albumino'ids . .HERTR (R.). Chemical Sature of Peptones . . . . . .ZCLKOFSKY (C.) Diastase and Beet Mucilage . . . . . .LIPP~L~SS (E.) and J. HAWLICZCP. Eikosylene, a Derivatire of Brown-coalParatfin . . . . . . . . . .NIEDERIST ((3.). Action of Water on the 'Haloid Compounds of L4icohojRadicles. . . . . . . . . . . .LAUTERBACE (P.). Kitration of Derivatives of the Paraffins . . .HAITINGER (L.). Nitrobutylene . . . . . . . . .EZWEILER. Researches on Perbromination . . . . . . .Le BEL (J. A,). Limit of the Separation of Alcohol fi-om Water .. .WURTZ (A). Basea derived from Aldoi-ammonia . . . . . .QXDREASCH (R.). Decomposition of Ammonium Forniate by Heat . .HELL (C.). and 0. M ~ : H L H ~ C ~ E R . Addition-product of Acetic Acid withHELL (C.) and 0. MWHLHAESER. Acidition-product of Abetic 'Acid withBromine and Hpdrobromic a c i d . . . . . . . .HELL (C.) and 0. MUHLHAUSER. Action of Bromine on Acetic Acid . .X i j s ~ ~ t (H.). Action of Hydrocyanic aud Hjdrochloric Acids on kthpiNethplacetoacetate . . . . . . . . . . .CONRAD (31,). Substituted Malonic Acids . . . . . . .NOIUVSKI (T.). Citramalic Acid . . . . . . . . .OST (H.). Ppromeconic Acid . . . . . . . . .GKARESCHI (J.). Ethylidene-disulphurio Acid . . . . . .HOFMANN (1.W.). Aiigelylthiocarbimide . . . . . . .M ~ L Y (R.). Nitrosothiohydanto'in . . . . . . . .RCI)SEFF. Amides of Tertiary Hydrocarbon Radicles . . . . .FKIEDEL, CRAFTS, and ADOR. Durene-derivatives . . . . .K~SHART. Action of Copper on Trichlorobenzene . . . . .\\-ILLGERODT (C.). Action of Basic Compounds on Solutions of a-Dinitro-chlorobeiizene in Carbon Bisulphide . . . . . . .HasxaRT. Act,ion of Chloroform and Perchlorometlinne on Dimethpl-aniline . . . . . . . . . . . . .PETRI (R.). Chondrin . . . . . . . . . .SCH~LER (J.). Ferricyanides . . . . . . .LADENBURG (A,). Di-isobutylamine . . . . . . .Bromine and Hydrochloric Acid . . . . .DWILLIER (E.). Isomeride of Angelic Acid . . . xsiv CONTESTS.PAGEHANIXABN and HANHART. Desulphurisation of Dithiodimethgl-aniline .714LIPPUABS (E.) and W. STRZCGER. Amjlidene-aniline . . . . 714HELL (C.) and P. SCHOOP. Aniline Reeidnes . , . . . 715LADENBURG (A.) and L. RWGHEIUER. Orthotolylene-diamine-derirati~es . 716BOTTIKGER ((2.). A New Base, CISHlSK2 . . . . . . . 716HIGGIN. Dibenzanilides . . . . . . 716WILLQERODT (C.). Preparation of Ethers 01 a-Dinitrophenol anti a-Dktro-chlorobenzene. . . . . . , . , . . . 716TRWMPLER (E.). Action of Soda-solution on Picramic Acid. . . . (1,BEXEDIGT (R.).mide . . . . . . . . . . . . 717MERZ (V.) and GI.. ZETTER.r -Tribromopheno! Bromide and Tribromoresorcinol Bro-Preparation of Trinitroresorcinol a n i Trinit'ro-orcinol . . . . . . . . . . . . .SAR.4CT. Action of Bcetic anhydride and Sodium Acetate on Quinone .SOMMARUGA (32.v.). Action of Ammonia Ion Quinones . . . .WESELSKY (P.) and R. BEBEDIKT. Azophenols . . . . . .FILETI (M.). Chemical Sature of the Essence of Laurocerasus ana of BitterBlmonds . . . . . . , . . . . . .T I E ~ ~ . ~ N N (F.) and E. HELGTKBERG. Aldehydes from Orcinol and theirDerivatives . . . . . . . . . . . .Derivatives of Tropic Azid . . . . . .TIElfANN (F.) and C. L. REIMER. Umbelliferone Deriratives . . .MICHAELIS (A.). A Homologue of Phosphenyl Chloride . . . .ZETTER (H.), H. RUOFF, and MoE. Researchesin Perchlorination . .LABHARDT (E.). Nitration of Bromonaphthalene . . . . .BEILSTEIN and KCRBATOFF. Oxidation of Nitronaphthalene . . .SMITH (A. J,). Halogell Derivatives of P-Yaphthol . . . ..WIDUAKN (0.). Dichloronaphthalene-B-sulphonic Acid . . . .\ ~ I D x l X N (0.). Action of Chlorine on Saphthalene-P-sulphonic Chloride.A Xew Trichloronaphthalene . . . . . . . . .PAGLIAKI (S.). Naphthylcarbamides . . . . . . . .PERGER (v.). a-Diamidoanthraquinone . . . . . . .SCHFKCK (E.) and H. ROMER. Nitroalizarin . . . . . .HRCYLANTS. Essence of Rosemary . . . . . . . .MOSTGOLFIER (J. DE). Transformation of Caniphic Acid inio Camphor .SESTIXI (F.). The Glucoside of Liquorice . . . . . . .OGLIALORO (A.) . Preliminary Kotice on Teucriurn fruticans . . .PAT ERN^ (E.) and A. OGLIALORO. Supposed Identity oi Columbin andLimonin . . . . . . . . . . .HILGER (A.) and H. BISCHOFP. Colouring-matter of the CaryophyllaceEe .HOOGEWERF$ (S.) and TAX DORP. Oxidation of Quinoline .. . .I<OEKIQS (w.). Oxidation of Cinchonine Quinoline by Potassium Perman-FLAWITZKY (E.). Hydration of Terpenes . . . .~ ' A T E R S ~ (E.) and A. OGLIALORO. Picrotoxin . . .panate . . . . . . . . AXDGEON; (G.), Nicotine , . . . . . . . . .CAHOURS (A,) and A. ETARD. A S e w Sicotine Derivative . . . .LADENBCRG (A.). Tropidine . . . . . ' . . . .LADENBFRG ( A , ) . Artificial Atropine . . . . . . . .HOFNANN (A. W.). Piporidine and Piperine . . . . . .SELIII (F.). Poisonous AlkaloId from an Exhumed Corpse . . . .SELMI (F.). .LIEBERNAXX (L.). Gas Evolved by the Action of'Barium Hjdrale on Albu-mino'ids . . . . . . . . . . . .GUYARD (A,). Copper and Ammonium Oxyferrocyanide . . . .CLAESSON (P.). Methyl and Ethyl Sulphates .. . . . .SOEOLOFF (X.). Preparation of Kitromannite and the Conditions of itsQALKOWSGI (E.). Compounds of Grape-sugar with Cupric Hpdrate . .Formation of Poisonous Allialoi'ds in the Human Corpse .LuB.4WIN (N.). Kucle'in from cow's Milk . . . . . .Explosion . . . . . . . . .717 'ili71871871971912u7801p172112172272272'7227'37247254207267 P G1 2 ,728729730730531731131132733733733734734735135775775777778r. rC . CJSTESTS. xxvPAaEBERTHELOT. Transformation of Sugar into Alcohol by a purely ChemicalMethod . . . . . . . , . . . . .DIECK (E.) and B. TOLLENS. The Carbohydrates of the Jerusalem Arti-choke . . . . . . . . . . . .SCHMIEDEBERG (0.).A Xew Carbohydrate. . . . . . .GIRARD ( A ) . Hydrocellulose . . . . . . . . .GROSHEIKTZ (H.) . Tetrallylammonium Bromide and Triallylamine . .WURTZ (A,). Bases derived from Aldol-ammonia . . . . .LAQERMARK ((3.) and A. ELTEEOFF. Action of Sulphuric Acid on AcetyleneKOHLER (K.). Substituted Nitrogen Chlorides . . . . . .RATHKE (B.). Diguanidine . . . . . . . . . . .SCHbLFEEFF. Melissic Acid . . . . . . . . .DUVILLIER (E.). Dimethylacrylic Acid, an Isomeride of Sngelic’Acid .LAGERXLRK ((3,). Synthesis of Tetrolic Acid . . . . . .GIACOSA (P.). Fermentation of Hydroxyraleric Acid . . . . .GRIMAUX (E.) and J. TSCHERNIAE. Preparation of Slalonic L4cicl . .ZWBLIS (H.). Spthesis of Isosuccinic Acid . . . . . .SEELIG (E.). Deriratives of Mucic Acid ., . . . . .WALLACH (0.) and P. P I R I T E . Thiamides of the Oxdie Acid Series . .GRIMAEX (E.) . Pseudouric Acid. . . . . . . . .GTXTAVSOX (G.). Interpretation of Reactions occurring in Presence ofAluminium Chloride . . . . . . .GUSTATSON (G.), Compounds of Cymene with Aluminium Bromido a n iChloride . . . . . . . . . . . .BALSOHN (M.). Action of Ethylene 011 Benzene in Presence of dluminiuniChloride . . . . . . . . . . . . .BEb3fER (M.) and I?. w . CLARKE. Aniline Salts . . . . . .WALLACH (0.) and H. BLEIBTREU. Thio-derivatires . . . . .DOEIINER (0.). Homologous Tertiary Dialnines obtained in the MethvlaniiineManufacture . I . . . . . . .FISCHER (E. and 0.). Remarks onDoedner’s Communication on ‘‘ Malachite-green ’’ . . . .. . . . . . . . .FISCHER (E. and 0.). Dyes of the Rosaniline Group . . . . .BEAXER (E.) and F. W. CLARKE. Lithium Picrate . . . . .BAUMAXX (E.) and L. BRIEGEB. Formation of Cresols during Purification.BAEXANN (E.) and L. BBIEGER. Paracresol . . . . . .CLER3foKT (P. DE) and J. ~ R O M M E L . Aurin . . . . . .WaSsERlcrasn (M.). Derivatives of hfechyl-eugenol . . . . .GRAEBE (C.) and H. BUNGEXER. Synthesis of DcoxybenzoPn . . .GOLDBEFF (P.). Nitro- and Amido-derivatives of Deoxg-benzoPn . . .B~TTIKC~ER (C.). Benzal Sulphide and Thiobenzaldehyde . . . .SCHaLL (C.). .MEPER (R.). Derivatives of Hydroxypropylbenzoic Acid . . . .GIBRIEL (8.) and A. MICHAEL. Benzylmethylglycollic Acid . . .JAFFE (N.). Acids produced by the Introduction of Chloro- and Bromo-benzene into the Animal System .. . . , . . .SPIEGELBERG (L.). Sitro-, Amido-, and Bromobenzene-sulplionic Acids .HEIKZELXAKX and L. SPIEGELBERO. Pentabromobenzene-sulphonic Acid ,BAUMAXX (E.) and C. PRE~SSE. Bromophenylmercapturic Acid , . ,FAHLBERG (C.). Liquid Toluenesulphonic Chloride and Beckurts’ so-calledToluenemetasulphonic Acid . . . . . . . . .RATHER (B.). Aromatic Thiocarbaniides . . . . . . .RATHKE (B.). Action of Phenyl-thiocarbimide on Diphenyl-gusnidine .HOFMAXK (A. W.). Action of Phosphorus Pentachloride on ThiocarbimideeBA~MANN (E.) and F. TIEMANY. Constitution of Indigo . . . ,BRIEGER (L.). Aromatic Products of the Putrefaction of Albumin . ,BEILSTEIN and K~RBATOFF. Oxidation of Bromonaohthalene . . .ROSENSTIEHL.Absorption Spectrum of Alizarin and of some ColouringMatters derived from it . . . . . , . . . ,The Hydrosytoluic Acids from the Three Isomeric CresolsGRAEBE (C.) and H. BUKGENER. Spt,hesis of Chrysene . . .7787787797797797807807807817827827827827827831837847847857857851857867867877877897897891897y0790790191791795190796796802803804804r -80480580680680780780ssvi COSTESTS.I)IL SIE (G.). Actire Principle of Insect Powder . . , , .LAIBLIS (R.). Nicotine and Nicotinic Acid . . . , , , ,SKRAUP ( Z . H.). Oxidation Products of Quinine. . . , . .SXRAVP (Z. H.). Constitution of Cinchonine Bases . . , , ,IATSCHISOFF (P.). Oxidation of Cholic Acid .. . . , .EGGER (E.). Bilic Acid, an Oxidation-product of Cholic Acid . . .KOSSEL (A,). Chemical Composition of Peptones . . . , ,ZEIDLER (0. and F.). Action of Oxidising Agents 0; the Oicfilics . .ERLENMEYER (E.). TheTwo Isomeric Dibromopropanes . . . .I~RTHELOT. Direct Combiliatioil of Cpnogen with Hydrogen and theMetals . . . . . ' . . . . . . .PRBTORICS-SEIDLEB (G.). Reactions of Cyanamide . . , , .SCHYITT (R.) and GOLDBERG. Action of Bleaching Powder on EthylAlcohol . . . . . . . * . . . .EDER (J. M.). Behariour oh Gums and Carbohydrates towards ChromBitrsunder the influence of Light . . . . . . . .~IOTTEK'. Action of Heat on Sugar and Sugar Solutions . . . .GIRARD (A,). Con! ersion of Hydrocelluloae into PJ roxjlin . . .BOXGE (K.).Compoaition of Beet-root, Gum , . . .DCTILLIER (E.) and A. BUISIXE. Commercial Trirnethylamke . . .VISCXST (C.). Distillat,ion of Beet-root Residues . . . , .CUSTER (E.). Action of Ethyl Chlorocarbonate on Mono- and 11i.ainyl-amine . . . . . . . . . , . . .JOVSSELIS (L.). Salts of Guanidine . . . . . . , .~ V U I ~ T Z (A). Chloral I-IFdrate . . . . . . . . . . .LAXDOLPII (F. H.). Action of Boron Fluoride on Acetone . . . ..IDRIAXOWSKY (A,). Action of Acetic and Sulphurous AnhycIricleJ onAluminium Chloride . . . . . . . . .ALLIHN (F.). Compounds of E t h j l Monochioracetoacetate . . . .TOENNIES (P.). Conversion of Furfurangelic Acid into Azelaic Acid . .BODCHARDAT (G.). Formation of Glycollic and Pyrnvic Acids f'roun Tar-taric Acid .. . . . . . . . . . .MILLER (H. 17.). Malonic Acid . . . . . . . . ,FICINFS (0.). Preparation of Pure Tartaric Acid . . . . .BELL (C. J . ) . .COSRAD (&I.). Ethj1,Forrnrltricarbonate . . . . .TOESSIES (P,). Relation of Dibromopyromncic Acid to Mucobromic Acid :CAHOCRS (A,) and E. DEIIAR~AY. Stannopropyls and Stannisopropjls .CATIOCRS (A,) and E. DEMARCAY. Iodides of Stannohutyl and Stsnnamyl .WROBLEYSKY (E.). Separation of Orthosylene from it,s Isomeride, and aNew XTlidene . . . . . . . . . . ,ASCHEXBRASDT (H.). Paradiethylbenzene from Psradibromobenzene . .MICRLER (W.) and G. MORO. Action of Sulphochloricles on Amines . .RCDOLPH ('2.). Benzvlamine . . . . . . . , .RUDOLPH (c.1, Deriratiws of Ortlionitraniline . .F m m I jhl.) and A.PICCISI. Decomposition of Phenyleth;.lanikie I-ij dro:chloride . . . . . . . . . . . .NICHLER (W,) and G. BLATTNER. Nitration of Benzene Suiphanilide . .BERSTHSEN (A). Amidines and Thinmides of Monobasic Organic Acids .€I~:BSER (H.) and E. SIMOX. Diethyl- and Dianiyl-anhydrobenzyldianiido-benzene Compounds . . . . . . . . . .%'ILLGERoDT (C.). Ethers of Trinitrophenol . . . . . .FISCHER (G.). S e w Colonring Matter from Orthan~idophcnol . . .SCHIIITT (R,). Constitution of Dichlorophenol . . . . . .T I E x n x (P,j. Relation between the Xjlenols and some other Hjdi*osy-deriratives of Eenzene . . . . . . . . . ,DALE (R. S.) and C. SCHORLEMHER. durin . . . . , .OTTO (R,), Constitution of Sulphoto!nitle . . . . . . .BARTII (L,) and J. SCKREDER. Fusion of Aromatic Acids with Soda ..HOPPE-SEYLER (F.). Lecithin and NuclePn in Beer-yeast . . .Action of Phosphorus Pentachloride on Saccharic AcidPAGE80780880981081081081 1811907908909910910911911911912912913915 . ~.914914914915915915916917917917918918918919919920 . ~ .92092192192292292892392392492492492592692COSTESTS. ssriiPAGETIEMANN (F.) and L. LANDSIXOFF. Aldehydohydro~ybcazoic Acids fromMetahydroxybenzoic Acid . . , . . . . . .HWBNER (H.) . Iodosalicylic Acids . . . . . . . .HUBNER (H.), S. BI. BABCOCP, and H. S c n a r v a r s . NitrosnlicFlic Acidsand Dinitrophenols . . . . . . . . . . .GOLDBERG (A). Parahydrosysalicylic Acid.. . . . . .BARTH (L.) and G. GoLDscH3fIDT. Eliagic Acid . . . . . .RICHARDS (E. S.) and A. W. PILXER. Antimony Tannatc . . . .MTLLER (F. H. S.) and F . WIESIFGER, Prcparstion of S dpho-compoundsOracosa (P.). Phenolglj-collic Acid . . . . . .from Diazo-compounds . . . . . . . .EARTH (L.) and bi. 17. SCHXIDT. Deriratires of a-Phenoldisnlphonic Acid :TED CHI (V.). Resorcinolclisulphonic Acid . . . . . .MICHLER (W.) and E. EXIIERICH. Poly-substituted Carhamides. . .MICHLER (W.) and R. ZIMNERXAXS. Pola-substituted Carbamides . .LACITXANX (G.). Tolglthiocarbiniic~e . . . . . . . .BAUXAXN (E.) and F. TIEXAKN. Constitution of Indigo . . . .GIRAUD (E.). Derivatires of Indigotin . . . . . . .STIDS (W.). Isatin Derivatives . . , . . . . . .BAITER (A,).The Indigo-blue Group. . . . . . . .RIOHLAU (R.). Orthodix~iiidocliphenethol . . . . . . .GXEESE (H.). Preparation of Hexmethjlbenzene from Acrtonc . . .AUOR (E, A,) and J . $1. CRAFTS. Action of Phthalic An11~tl:i~lc 0x1 S n p l l -thalenc in presence of Aluminium Chloride . . . . . .SCHMIDT (G. A,). Kitrophenanthrene and its Deyiratives . . . .LmBERx.kxs (C.) and H. DEHNST. Constitution of Anthrarufin and Osy-anthrnrufin . . . . . . . . . .TILDE?*‘ (W. A.). Compounds of the Terpenes with Hydrochloric Acid .MoxTGoLFIER (J. DE). Terebeuthene Dih~drochloride . . . .LIEBERXAXN (C.) and S. HAJIBURGER. Formule of Quercitrin and Qucr-cetin . . . . . . . . . . .IIOOGEWERFF (S.) and IT. A. TAS DORP. Oxidaiion 01 Quininc . . .WEIDEL (H.) and &I.I-. SCHMIDT. Formation of Cinchomrronic Acid fromQuinine, and its Identity with Pyridene-carbonic Acid . . . .SKRAVP (Z. H.), Composition of Cinchonine . . . . . .SKRICP (Z. H.), Oxidation-products of Cinchoninc . . . . .SKRAUP (Z. H.) and 0. ~ O R T K 4 h - N . Cinchonidine . . . . .HUFXER (G.). Chemistry of the Bile . . . . . . . .DRECHSEL (E.). Preparation of Crystalline -4lbumin Compounds . .HOFNEISTER (F.). Regeneration of Albumin from Peptone. . . .GAMGEE (A,) and E. BLASPESHORN. Protagon . . . . . .%‘ROOST (L.). Vapour-densities of certain High-boiling Organic Compou1id~PRUNIER (L.). Unsaturated Hydrocarbons from the Decomposition ofAmerican Petroleum . . . . . . . . . .ANBDELL (G.). Physical Properties of Liquid Acetylene .. . .LESCCEUR (H.) and A. RIGAUT. Solid Cyanogen Hydridc . .LE BEL (J. A.) and GREEXE. Action of Zinc Chloride on Korninl hutsiAlcohol . . . . . . . . . . . .LE REL (J. A,). Methylpropylcarbinol prepared !& Spthesis . . .HANRIOT. Derivatives of Glycorol . . . . . , . .BOCTMY (H.). Researches on Nitroglycerol . . . . . .CLAESSON (P.). Ethereal Sulphates of Polphydric Alcohols and Carbo-3ComoN (H.). Chronology of the Isomeric Purpurins . . . .NOXTGOLFIER (J. DE). Isomeride of Borneo1 . . . . .BAEYER (A,). Syntliksis of Chinoiine . . . . . .. _hydrates . . . . . . . . . . .GOTSCHXASN (T.). Methyl- and Dimethyl-diacetonamine . .CAHOKRS (A,) and E. DEMISRCIY. Acids obtained by Distilling the CrudeAcid from the Sauonification of Fats in a Current of Steam .. .BURI (E ). Japanese‘ Wax . . . , , . . . . .9279289289289299309339339339349349359359359369379379399409409419429439 2394494494494694694794894894894995095095010251025102810281029102910291032103310351036103...XXVlll COSTEKTS.BOCRGOIX (E.). Elimination of Bromine from Bromocitraconic Scid, and aNew Organic Acid . . . . . . . , . . .ODERMATT (W.). Formation of Phenol from PutrefTina AlbuminoEd " I Matters . . . . . . . . . .MICHAEL (A). Synthesis of Phenol Giucoside and Orthoformyi Glucosideor Helicin . . . . . . . . , . . .RUSH (IT. B.). Copaibic Acid . . . . . . . . .TROOST (L.). Maximum Tension and Vapour-density of L41izariii.. .BOUCHARDAT (G.) . Identity of the HFdrates of Di-isoprene, Caoiitchene,and Terpene . , . . . . . . , . . ,KACHLER (J.) . Borneo Camphor . . . . . . . . ,H ABERKA NS (J.) . Glycyrrliizin . . . . . . . , .MIXTAPHA (I.). Active Principle uf Ammi T7isnaga . . . . .FLOKERB (H.). Lactucarium , . . . . . . . .COSTELO (D.). Gamboge . . . . . . . . . .PHIPSON (T. L.). Colouring Matter of Palmella crzcsnta . . , .DRAGENPORFF and STAHRE. Chemistry oi the Peonia peregrirza . .MASDELIX (A. F.). Quinine Citrate . . . . . . . .HESSE (0.). Paricine and Aricine . . . . . . . .OUDEXASS (A. C.). Quinamine . . . . . . . . .GREESIBH (H. G.). Bidara Law5 . . . . . . . ,ARATA (P. X.). Alkulo'id of Mio-Mio (Baccharis cordifolia) . . .Physiological Cliemistiy.DUKE CARL TKEODOR OF BATARIA.Influence of the Temperature of thesurrounding Air on the Excretion of Carbonic Acid and the Absorptionof Oxygen in the Cat . . . . . . . . . .VOIT (C.). Influence of the Temperature of the surrounding Air 011 tlieProcesses of Decomposition in the Organism of Warm-blooded dninialsCLERNONT (P. DE) and J. BROMNEL. Magnesia as an Antidote f o r d r -senious Acid . . . . . . . . . .FRIBDLAXDER (C.) and E. HERTER. Action of Carbonic Acid on tlie inimaiPICARD (P~). Researches on the Urea contained in the Organs . . .PICARD (P.). Albumino'id Compounds of the Organs, and of the Spleen inparticular . . . . . . . . . . . .SALOXOS (G.). Occurrence and Origin of Hj-poxanthine and Lactic Acid inJAFF~ (X.).Synthetic Processes in the Animal Body . . . . .JOKGE (I). DE). Secretion from the Sebaceous Glands of Birds , . .B~CHAJIP (J.) and E. BALTUS. Modification effected by the Animal Organismon Various Albuminokl Substances when Injected into the Veins . .PFEIFFER (E.). Oxalic Acid not Poisonous (?) . . . . . .PO IN CAR^ (L.). Danger of employing Methj-1 Alcohol in Certain Industries.WILCKENS @I.). Digestion in the Different Divisions of the Digestive CanalOrganism . . . . . . . . . . .the Animal Body . . . . . * . .of tlie Sheep . - . . . . . . . . , . .BERTRAM (J.). Excretion of Phosphoric Acid by Herbivora . . .POTT (R.). Researches on the Chemical Changes in the Fui~l's Egg during --Incubation . . . . . . - . . . . .SCHCLZ (H.). Action of Cacodxlic Acid on the Animal Organism ..SUHIJLZ (H.). Action of Mono- and D1-phenylarsenic Acld on Animals .SEEGEN (J.). Transformation of Glycogen by the Salivary and PancreaticFerments . . . . . . . . .QUINCKE ((3.). Formation of Emulsion, and the Influence of the Bile onDigestion . . . . . . . . . . . .B%CHAXP (J.). Xature of the Albumins in Hydrocele . . . . .SCHRODT (3.1.). Composition of Nares' Milk . . . . . .PAGE1037103810381038103910391039101,010%110411042104210431043104410441045101.674c- / o771741t51751761761763343363353913984744T647664854955056COSTESTS. sxisPAGEJOLLY (L.). Distribution of Phosphates in the Blood . . . .SALKOWSKI (E. and H.). Physiological Relations of Phenjl’acetic andPhenj-lpropionic Acids .. . . . . . . . .DISTRE. ‘i Starch Granules” and ‘‘ AmFloides” of the Egg . . . .HERTER (E,), Tension of Oxygen in Arterisl B!ood . . . , .HESSEBERG (IT.), E. KERN, and H. VITTEXBERG. .KIRCHSER (W. J.) and Du ROI. Beet-Leaves as Fodder for C o m . .SAI,KOWSKI (E.). Pancreatic Digestion . . . . . . .B O E ~ Y (A,). Digestibility of NucleZn and Lecithin . . . . ,T A K ~ C Z (1.). Oxidation in t>ho Organism . . . . .BAEMASK (E.) and C. PREUJBBE. Oxidations and Syntheses in the *4nimaiFattening of SheepOrganism . . . . . . . . . . . .EUGLING (W.). Composition of the Colostrum of the Cow . . . .BUXGE (G.). Behaviour of Potassium Salts in the Blood . . . ,B a n ~ ~ s s (E.). Behariour of Phenol in the Animal Organism .. .GIICOSA (P.). Betion of Amy1 Nitrite on Blood . . . . . .SOSNTSG (E.), &I. SCHONBERG, and H. LORESZ. Feeding Experiments withVOIT (C.) and C. THEODOR. Influence of the Surrounding Temperature ont,he Tissue Metamorphosis of Warm-blooded Animals . . , .Losw (0.). Source of Hippuric Acid in the Urine of Herbivorous AnimalsSCHXIEDEBERG (0.) and WALTER. Formation of Crea in the Animal Or-ganism . . . . . . . . . . . . .REKO~ARD (A). Analysis of Silk Cocoons . . . . . . .NENCKI (31.) and P. G~acosa. Existence of Bacteria or their Germ in theWEIK (E.). Feeding of Calves without the Corn’s Milk . . . .HILLE. Poisoning of Fowls with Pumpkin Seeds . . . . . .Sheep . . . . . . . . . . .Healthy Organs of Animals .. . . . . . .Chemistry of Vegetable Physiology and Agriculture.HECEEL (E,). Influence of Salicylic Acid, Thymol, and some Esseutid Oilson Germination . . . . . . . . . . .FITZ (A,). Fungoyd Fermentation . . . . . . . .MIKOSCH ((2,). Origin of Chlorophyll’Granules . . . . , .KELLERMSNN ((2,). Composition of the Growing Potato . . . .GAYON (V,). Inversion and Alcoholic Fermentation of Cane Sugar . .BERT (P,). Region of the Solar Spectrum which is Indispensable to VegetableLife. . . . . . . . . . . . . .M ~ S T Z (&4,). Ripening of Rye . . . . . . . . .AXDREASCH (R.), Ash of the Garden Pink and of the Rose . . .BEXMELEN (J. M.). Absorptive Porner of Soils and of Silica . . ,SOYKA J. ,J ~ G T (L.). Influence of Temperature on the Germinat,ion of Seeds .,MIQUEL (P.). Presence of an Alcoholic Ferment in the Air . . . .HEHKER (0.). The Influence of Chloroform on Gitrification . . .WARDES (C. J. H,). Composition of Poppy Petal Ash . . . .SCH~TZENBERGER (P.) and A. DESTREX. Researches on Beer-yeast . .SCH~TZEKBERGER (P.) and A. DEGTREM. Composition of Beer-yeast . .THOXSON (W.). The Ferment produced by the Morbid Growth of theBioplasm of the Yolk of Egg . . . . . . . .REICHARDT (E.I. Distribution of Fungi . . . . . . ,HAM (B.). Ripening of Grapes . . . . . . . .BARRIL (J.). Kitrates in Beet-roots . . . . . . .Influence of Soils on the Decompositiou of Organic SubstawesMIQUEL (P,). The Succinic Fermentation . . . . . .COBENWINDER IB.). On the Banana 1 . . . .. . .SCEUTZESBERGER (P ) and A. DESTREV. On Slcoholic Fermentation . . 550BOHM (J.), Formation of Starch in Chlorophjll Grains in absence of Light 5516626626628118118138148148148148158168168169519519529529521046104610461721721741741 i 433633633733733833933930339439439539547647747841947sss CONTENTS.GROSJEAN (€I.). Analysis of some Fodders, and Observations on theDamage caused to Italian Beans by the Bean Insect . . , .BEILKELEX (J. Xf. v.). Absorptire Power of Soils . . . . .BBCHAMP ( A ) . Formation of Carbonic Anhydride, Alcohol, and Acetic Acidby Yeast alone, in presence and absence of Oxygen . . . .SCHIEL (J.) . Fermentation . . . . . . . . . .RICHET ((2.).Conditions of Lactic Fermentation . . . . .FITZ (A,) Schyzomycetic Fermentation . . . . . , .GZTSKISQ (J. W.). Conditions of Life of the Lower Organisms . . .BANCEL (C.) and C. H~SSOX. Phosphorescence of Lobster’s Flesh . .BELLUCCI. Supposed Existence of Hydrogen Peroxide in the Organism ofPlants . . . . . . . . . . . .DEH~RAIN. Assim’ilation of Soda by Plants . . . . . . .ORTH (A). Constancy and Variation in the Composition of the Soil . .HBBERLtPjDT (F.). Evaporation of Water from the Ground . . .TUAER. Experimental Inquirp as to the Quantity of Nitrogen whichmuaibe supplicd to cultivated Plants to ensure their normal dereloprnent asField Crops . . . . . . , . . , . .BECHAMP (A). Influence of Oxygen on Alcoholic Fermentation . . .SCHJIOEGER ($1,).On the Possibility of Replacing the Carbonic Acid of theAir necessary for the Production of Chlorophyll in Sarcophytic and Purs-sitic Plants by Organic Substances . . . . . . . .GRETE. Formation of Xtrites in the Soil . . . . . . .HILQER (Ak.). Chemical Composition of the soils of the Trine-growing [)is.tricts of the Rhinc and Maine . . . . . , . .HEIDEN. On theSupply of Nitrogen to Plants . . . . . .MACAGNO (J.). .GT;KNIXQ. Action of Alcohol on Bacteria . . . . . . .Occurrence and Vitality of Bwteria ; Vitality of Yeast . . . .GRASDEAU (L.). Influence of Atmospheric Electricity on Plants .PELLET (H. P.). Ratio of the S u p in the Beet to the Phosphoric Acid idthe Root and Leares . . . . . . . . .GATELLIER (E.). Absorption of Atmospheric Xitrogen by Plants.. .HOPP,:-SEYLER (F.). A Simple Experiment to show the Evolution ofKELLS~R (0.).HILGER (A,). Mineral Constituents of Horseradish . . . . .PORRO (B,). Coniposition of Grapes a t diferent Stages of Ripeness . .Diseases of Cultivated Plants . . . . . . . . . .STORER (F. I€ ) arid D. S. LEWIS. .LECLERC (A). liutritire Value of Seed-bearing Beetroot . . . .PIERRE (J.). Oiling of Corn . . . . . . . . .PETERXANS (A4.). C$rmt Seeds . . . . . . . . .VIBKANS (G.). Clioice of Beehoot for Seeds . . . . . .WII.DT. Seeds of Lallemantia iberica . . . . . , . .WOLLNY (E.). Ridge Ca1t)iration . . . . . . . .DRECHSLEX. (G.). Potato CultiTation . . . . . . . .MOSER (J). Cultivation of Dhurra or Sorgho Grass . . . ..R R I x x m (C.). Action of Rain on Clorer Hay . . . . , .OTTO and 0. KSOCH. Cultivation of Grass Seeds . . . . .KSOP (W.). The Greenstone Soil of Berneck . . . . . .WOLLSY (E.). Tt mperature of Soils . . . . . . . .LAI)LTRE.4IT (A). .ULLIX (F,). Agricultural Experiments on Irrigated Land . . , .MOSER (J.). l’otassium Salts as a Manure . . . . . . .LADL-EEAU (If. A,). Nitrates in Sugar Beets . . . . . .ULLIK (F.). Absorptire Poii-ers of Soils . . . .FREYBERQ (E.). Plant Respiration . . . . .XIQUEL (P.). A New Organised Ferment . . . . . .Action of the Ferment of Sour &e on Good Wine .TSCHIPLOTITZ (F.). Absorption of Water by Leaves . . . .Oxygen by Plants in Sun Light . . * . . .Xitrogenous Constituents of Young Grass and HayAnalpis of Weeds used as Salad .Influence of the Time of lfanuring in Beet CultivationPAGE552552663663663gf14664.665665666666667667668/30736r -73773773773981781781781781881881881981981981982082082182282282282282282282382382382482482482582582682COSTESTS. sxsiPIG):8265-2893395 59569369369579579579589589599599609609619611046104610 161047104710471048104810481049104910 49105010501050105010501050I0501051CHRISTIASI (IT,), Effect of Manure on Crops .. . .DORIKQ and BOCHMANY.NENCPI (XI.).CAMERON (C. A.),Effect of Artificial Rianures on the 'Grom-th of. . .Preliminary Sotes on the Absorption of Selenium byPlants .. . . . . . . . . . .Barley and on Meadow Land . . . . . .Relation of Oxygen to t'he Life of the SlicrozoaAnalyses of Cattle iodder . . . . . . . . .STORER (F.) an6 D. S. LEWIS.STORER (F.) and D. S. LEWIS. Analysis of Share GrassHABERLASDT (F.). Cohesive Power of Soils . . . . . .LANG (C.). Hent-capacity of Soils . . . . . . . .Seed of Sorghu~n vulgnre . . . .. . . .MUTXHLER (L.) and C. KRAUCH. Composition of Candle S u t s . . ,RICWEBT (E.) dnalpes of Hops. . . . . . . . .MASSEXBACH (G. T,). Experiments with Artificial Manures . . .W r ~ s (E.) and E. EBERXASK. Jituiure Experiments with Bone-meal Supel--LIBTSER (C.), KRANDIUER, and TREIBER. Effect of Artificidly -\Innured . . . . .GERLASD (W.) ancl J.ROBERTS. Preserration of Bcet Lenres, nnd theSTORER cF. H.) and D. 8. LEWIS. Analyses of some Species of the Gonrdpliosphate and vith Potash Salts . . . . . . . .Barley on the Composition of the Wort .MOSER (J.). Cultiration and Preserration of Maize . . . . .Preparation of Brorrn Hay from 3laize . . . . . .Family . . . . . . . . . . . .PECPHAY is. F,). Composition of the Ashes of Wheat Bi~an . , .KOCH. Ilktho& of Photbgraphing Bacteria . . . . . . .C o c i i n (D,). Kon-existence of a Soluble Alcoholic Ferment . . .BERSCH (J.). Cultivation of Pure Beer Yeast . . . . . .D a v ~ (E. IT). Kitrification . . . . . . .BRIEJI (H ) . Inntieme of Light on the Yield of Sugar-beets . . ,PORTELE (R.). . . .PEDERSEN (R.). Influence of Temperature on the Erolution of CarbonicWURTZ (A,) and E.BOFCHUT. Digestire Ferment of Cnricapapya . .Gayus and MILL~RRET. On the Sacchsriiie Matter contained i n TinesInfluence of Heat on the Ripening of GrapesAnlr~ciride by Barley Seeds . . . . . . . . .W1mx.i~ (L.). Action of the Sap of Cnricn papaya . . . . .suffering from Phylloxera . . . . . . . . .Analyses of t.le Orange . . . . . . . . . . .XELLSER (0.). Nutrit,ive Value of Malt . . . . . . .COTTU (H,). Use of Sour Food for CONS . . . . . . .KLEEJIASN. Spent Hops as Fodder . . . . . . .HEIanIcii (R.) . Artificial Xanures . . . . . . . .M~SSESBA~H (T.). Esperiments with Artificial Manures . . .SCHAFFERT (F.). Experiments on Manuring . . . . .LECHIRTIER (G.). Preservation of Green Fodder in Pits .. . .LIBBSCHER, ~ J R I E U , and R. BCRGER. Exhaustion of ;he Soil by Beet-rootCiiltivation . . . . . . . . . . . .BOCHXISX. Chili Saltpetre as a Manure for Bariey . . . . .Aiicdyticd Cheinistvy.BOTTOMLEY (T.). Colorimetric Esperiments . . . . . . 77HUTCHIKSON (C. C.),tinn of Oxvgen in Water . . . . . . . . . ?7HESSE (0,). Appendix to the Estimation of Cm.bonic Acid in the Air . 78POLECK and BIEFEL.ing Gas . . . . . . . . . . . . . 78LUKGE (G,), Estimation of Nitrous and Sitric Acids . . . . . 79LALTFER (E.). Behaviour of Quartz with Nicrocosmic Salt . . . . 7!)Scliutzenberger's Process for the T'olumetric Estima-Quantitative Determiriation of Sulphnr in Illuminnt-GRETE (E. A,). Estimation of Sitric Scid as Ammonia .. . . 7xxxii CONTENTS.DATIS (T. H.). Testing and Valuing of Gas Liquor . . . . .WILSON (H. M.). Remarks on the Estimation of Calcium Sulphate inBeer . . . . . . . . . . . .CHAPUIS and LIKSOSSIER. .ORETE (E. A,). .ADAX (A). Sew and Rapid Process for the Analysis of Butter . . .LEPEL (F. v.). Adulteration of mine . . . . . . . .NECBAUER (C.). Detection of Wines Adulterated with Grape-sugar . .VOGEL (H. W.). Testing Alizarin Colouring-matters and Green AnilineColours . . . . . . . . . . . . .LTXGE (G.). Application of Witt's Tropsolins to Titration . . ,MEYER (V.). Det>ermination of Vapour-density . . . . . .DOSATH (E.). Applications of Glycerin in Analysis . , . . .BOTTGER (R.). Reagent for Detecting Nickel . . . . . .H-LGER (H.)..MAERCKER (11.). Grarimetric Estimation of Dextrose by means of an Alka-HEISRICH. Estimation of Destrose and Inrerted Sugar in presence ofSaccharose . . . . .WTRSTER (C.). Quantitative Estkmtion of 'Starcil in Paper . . .HEHSER'S Nethod of Testing Butter . . . . . . .ALLEN (A. H.). Distinctire Tests for Phenol, Cresol, and Creosote . .BOTTQER (R.).HOFMEISTER (F.) . Complete Precipitation of Albumin from Animal FluidsVIELHABER (H. C.). Application of Phenol-phthaleb . . . . .STOCK (W. F. K.). Analysis of Boiler Feed-waters . . .EDER (J. M.). Estimation of Nitric Acid in Well Water . . . ,FINKENER (R.) . Estimation of Phosphoric Acid as dinmonium Phuspho-molybdate . . . . . . . . . . , ,SMITH (E. J , ) . Electrolytic Estimation of Cadmium .. . .BEILSTEIN (F.). Separation of Zinc from Nickel . . .WEIL (I?.). Further Note on \Veil's Volumetrio Method of EstiumtingCopper . . . . . . . . . . . .JOHSSOY (0.). Test for Arsenic . . . . . . . . .MORAWSKI (T.) and J . STIFGL. Volumetric Estimation of ManganeseMORAWSKI (T.) and J. STINGL. Modification of Bunsen's Method of Man-HEXPEL (W.) . Simultaneous Determination of Carbon, Hydrogeu, andTHRESH (J. C.). Detection and Approximate Determination of MinuteREICHARDT (E,). Detection of Chloroform . . . . . , .VIELHABER (H. C.). Estimation of Hgdrocganio Acid in Bitter AlmondPresence of Lead in Bismuth Subnitrate .Estimation of Nitrogen in Nitrogenous Orgmic BodiesHAGER (H.). Butter Analysis . . . . . . . .REIKLSN. Valuation of kody Colours .. . . . .line Copper Solution . . . . . . .Estimation of Alcohol and Estractive Matter in TVine ,Detection of G,qmnn, Heavy Spars, &c., in Flourganese Determinations . . . . . . .Nitrogen in Elementary Analysis . . . . . .Quantities of Alcohol . . . . . . , .- -\Yster . . . . . . . . . . . .HESSE (0.). Test for Quinine . . . . , . . . .HESSC (0,). Test for Quinidine . . . , . . . . .HESSE (0.). Behaviour of Potassinm Thiocranate with some of the QuinineIlkalol.ds . . . . . .STOEUER (W.). Estimation of the Alialo'ids in the Bdlirian Quiiiine Barksexhibited at the Horticultural Eshibitiou in Amsterdam . . .BORSTR~QER (H.). Method for rapidly Incinerating Meal . . . ,SCHXITT (E.). Testing Bees'-wax for Rosin . .. . . .PFEIFFER (E.). Separation of the Alkaline Earths from the Alkalis . .I ( E S 3 r . m (F.). Estimation of Manganese, especially in its Alloys with Iron.WLBER (W.). Detection of Indican in Urine , . . . . .BUS (11.). Detection of Salicylic Acid in Beer . . . . . .BOKYTR~QER (H.). h New Indicator for use in dcidimetry and Alkali.metry . . . . . . . . . . . . .PSQE797980808081828283176177 ~. .178179179179180180 15018118218318327327327427521627627627727727827827928028028028128128129228334134134834239CQSTENTS. xxxiiiPAGEBECKER (a. F.). Reduction of Weighings in Air in Chemical Analysis to - -aVacuum . . . . . . . . . . .PILLITZ (W.). Analysis of the Zsad&nyer Meteorite .. . . .PFEIFFER (E.). .CASTAX (F.). Estimation of Minute Quantities of Soda in PotassiumEstimation of Nitric Acid by Potassium Dichroniate .Nitrate ' . . . . . . - . . . . . .LEEDS (A. R.). Alteration of Standard Ammonium Chloride Solution whenkept in the Dark . . . . . . . . . .STINGL (J.). Valuation of Burnt Lime . . . . . . .FRESENIUS (R.). Estimation of the available Zinc in Zinc-dust . . .KLEIN (L.). Estimation of Carbon in Cast-iron . . . . . .DONATH (E.). Detection of Chromates and of Free Chromic Acid . .BRONNER. Use of Hempel's Lamp for illustrating Silrer Assay as a LectureBISCITOF (G.). Estimation of Traces of Lead . . . . , .HGRTER (F.).LISK (1.) and R. XOCKEL. On the Delicacy of "some Reactions for Hydro:cyanic Acid .. . . . . . . . . . .LAUGIER (E.). Analysis of Raw Sugars . . . . . . .BECBAUER (C.) and E. BORGJL4Ss. .H?FSER (G.). .STETESSON (W.). .WOLFRAM (G.). Qnantitatire Dctermiuation of Theobromine in Cacao andChocolate . . . . . . . . . .LAVGIER (E,). Determination ofFree kcids in Oils . . . . ,REICHERT (E,). .DIETZELL (B. E.) and M. G. KRESSNER. Testing Butter . . . .POPPER (R,). Quantitative Determination of Precipitates without Filtering,HEHNER (0.). Determination of Phosphoric Acid as Pho&omoiybdate ,YOVSG (IT. C,). Xote on the Detection of Alum in Flour by the LogwoodTest . . . . . . . . . .DTJPR~ (A,). Detection and Estimation of Alum in Wheat Flour . .DOELTER ((2.). Estimation of Ferrous Oxide in Silicates .. . ,CAMERON (C. A.). Estimation of Lead as Lead Iodate . . . .BAYLEY (T.). ,CAMERON (C. A,). The Inconstant Composition of Well-water . . .WIGSER (G. W.). Kitrogen Compounds present in Cereals . . . .SIEBOLD (L.). Titration of Hydrocyanic Acid and Cjanides, and its relationto Ilkalimetrv . . . . . . . . . . .BARDY (C.) and i. BORDET. Estimation of Methyl dlcohol in Wood SpiritCAZENEUNE (P.). Detection and Estimation of Salicjlic Acid in AnimalSecretions . . . . . . , . . . .DWARS (B. W.). Determination df Quinine in certain of its Salts . .PRLTIER (L.). Solubility of Cinchoiiine and Estimation of Cinchona Barks .M ~ ~ R K E R (K. A. H.). Alkali-albuminatc and Sj-ntonin . . . , .CAMEROX (C. A). dniount of Solids in Milk , . . . ..WILLIAXS (G,). Substitute for Litmus . . . . . . .PUSCH. Bohr's Colorimetric Process for the Examination of Drinking-water . . . . . . . . . . .HANX~ (W.). Modifieation df Simpson's Method'for Estimating Xitrogen .SCHIFF (H.). Analysia of Organic Compounds containing Halogens orNitrogen . . . . . . . . . . . .WANKLYN (J. 1.) and W. J. COOPER. .PERRY (N. W.). Platinum dlloy Assay . . . . , , .PEXNEY (&I. D.). Alum in Flour and Bread . . . . ' . .PATY (F. W.). Volumetric Estimation of Sugar . . . . . .CAZENEIJVE (P.). Estimation of Glucose in the Blood. . . . .TOLLESS (B.). Specific Rotatory Power of Cane-sugar . . . .Experiment . . . . . . . .Estiniation of Cyanogen in Soda-IresEstimation of Glycerin in Wine .Estimation of Urea by means of Sodium Hypobromite .Estimation of Quinine in Ferri et Quinte Citras (B.P.)Simplification of Hehner's Method of Testing Butter .Washing, and Drying .. . . .STODDART (W,). The LogwFd.od Test for Alum . . . . .Analpsis of Alloys containing Copper, Zinc, and Nickel.The Xoist Combustion ProcessVOL. XXXYI. C39639739939940040040040140140240240240340 L40440340540640640640748048248348348348448 L4x54854864864874884h848948949056355365 b65665555666f153755755sxxiv CONTENTS.SIEWERT (M.). Estimation of Fatly Matters in Feeding Stuffs . , .Hnssoe (C.). Examination of Coffee, Tea, and Chicory . . . .LII~DO (D.). Analpis of Caoutchouc . . . . . , . .HILGER (A,).Detection of Ethyldiacetic Acid in Urine . . . .RUDORFF (F.). Determination of the Specific Gravity of Powdered Sub-stances . . . . . . . . . . . . .HENPEL (W.). Estimation of Hydrogen in Gaseous Xixtores .GTYARD (A,). Separation and Estimation of Chlorine, Bromine, and iodineOTTO (R.). Preparation of Sulphuretted Hydrogen for Chemico-legal Inresti-CLERNONT (P. DE.). Action of Animoniacal Salts on 3ietallic Sulphides, andWATTESBERC) (H.). Estimation of Soluble Phosphoric Acid in Superphos-BEILSTEIK (F.) and L. JAWEIS-. Estimation of Zinc . . . . .FESCA (M.). Nechanical Analpsis of Soils . . . . . . .TERREIL (A.). New Method for Determining the Melting Points of Organicgations . . . . . . . . . . .its Application to Mineral Analpis .. . . . .phates . . . . . . . . . . . .L Substances . . . . . . . . . .MALLARD and LE CHITELIER. Detection of Marsh-gas in the Air of Dlines:G~TKSECKT (H.). Diagnosis of F a t t r Alcohols . . . . . .PICARD (P.).C4ILLETET.Bernard's Method for the Estimation of Glucose in Blood .-4 Test for Tartaric Acid which distinguishes it from CitricD'ARSOXTIL. Estiination of Sugar in Blood . . . . .Acid . . . . . . . . . . . . . .IIacgR-(H.). Testing Milk for Starch Pomler . * .Xt.nr (C.), &Iarchand's Method for Determining the Butter in ililk . .BUCHSER. Adulteration of Beesx-ax . . . . . .KOSIG ((3. A). Chromometry : an Apulication of' the Biowpipe to Quantita-tire Analpis . . . . . . . . . . . .SCHONE (E.). Estimation of Hydrogen Peroxide , .. , . .REIMET (J.). The Proport,ion of Carbonic Anhydride in the Air . , .WEIY. Estiiimtioii of Soluble Phosphoric Acid in Superphosphates . .BEILSTEIS (F.) and L. JIVEIN. Estimation of Cadmium , . ~ .SKITH (E. F.). Electrolytic Estimation of Cadmium . , . . .ROSSLER (C.). Estimation of Manganese . . . . . . .I€EMPEL (W.). Friictional Conibustioii of Hydrogen and Xarsh-gas . .REQKAELD (J.). Chloi-oform as an daa.sthetic . . . . . ,P A G I J I N I (S.). Reaction of Salicylic Acid with Ferric Salts . . . ,CAZESECTE {P.). Separation and Estimation of Hippuric Acid . . .OGI,IILORO (A,). Characteristic Reactions of Picrotoxin and of some of itsDeriratires . . . . * . . . . . .SETTEGAJT (H.) . Contributions to Quantitative Spectrum Analysis ..PEKFIELD (8. L.). Volumetric Estimation of Fluorine . . , .HCHRODER (W.). Estimatioii of Xitrogen in Crine . . . . .SALKOTT-SKI (E.). Behariour of Aniiiionium Chloride in the Organism andEstimation of Chlorine in LTrine . . . . . . . .R ~ M X E L S ~ ~ R Q (c.). Detrrniinatioii of Lithium . . . . . ,GCYARD (A), Law peculiar to Xetallic Ferrocpnides. . . . .~ X I T H (W.) . Characteristic Reactions of the Aromatic Hj-drocarbons withCASAXLTOR (P.). Influence of Temperature on the Deriation of PolarisedLight bp Solutioiis of Inverted Sugar . . . . . . ,HEHKER (0.). Examiliation of Paq-'s Method of Determiniiig Glucose .DOGIEL (J,). Reactions of Albumin, and Behariour of the Albumin of theRefracting Media of the Eye . . . . . . . .H~FNER (G.).Estimation of Hremoglobin and Oxygen in the Blood . .HENXEBERG (W.). Determination of Fibrin . . . . . .L o ~ m (0.). Detection of Lecithin . . . . . . . .RUFFLE (J.). Estimation of Nitrogen . , . . . . . .II.4RCHIKD (E.). n l i k fro171 Cows of different Races . . . . .Antimony or Bismuth Tricliloricle . . . . . . .PAGE555558559560669670670671672672672673673673673674674674674675678740740744745746746746747747745748748749a2852982983083083083183283483483583583596CONTENTS. SXXVPAGE9629639639649669670689699i3973973974JOHNSON (9. W.) and E. H. JENKINS.CARXOT (A,).LEEDS (A. R.).Determination of Nitrogen in theUse of Sulphuretted Hydrogen in the Dr- Way in Anaij sis :Detection and Estimation of bitrous Acid in Potablednalpes of Agricultural Products .. . . . .BOHLIG (E.), Water Analpis . . . . . . . .Waters, Acids, &c. . . . . . . . . . .Determination of Phosphoric Acid .Estiuation of the Value of Suueruhos-JOHNSON (S. W.) and E. H. JENKINS.ALBERT (H.) and L. SIEGFRIED. I I phates . . . . . . . . . . . .Fish Guano . , . . . . .cation . . . . . . . .DIETZELL (E.) and ill. G. ~ R E S B N E R . Estimat,iou of Phosphoric Acid inCLASSEX (A.) . A Few Quantitative Analytical Method of kanifold ippli:HERTZ (J.). Estimation of Silver, Chlorine, Bromine, and 1odine'b.r Ammo:niuin Thiocyanlde . . . . . . . . . " . .WASOFICZ (31. 17.). Verrjken's Metliod of Detecting ilfetallic Poisons .PLAYFAIR (D.).Sote on the Detection of some Rare Metals in PFritesFlue-dust ' . . . . . . . . . . .- .DROKX (T. ill.). Determination of Silicon in Pig-iron and Steel . . .ROLLET (A,). Determination of Sulphur in the Ore, in the Fuel, and in theProducts of the Iron Inclustrj- . . . . . . . .CLARKE (F. V.). Electrolytic Estimation of Mercury. . , . .LECHARTIER (G.). Estimation of Organic Matter in Xatuml Waters . .PETRI (J.). .MEDICES (L.) and E. SCHWAL. Estimation of Starch in Sausages . .PROCTER (H. R.). TTeselskfs Reaction for Phloroglucin . . . .PROCTER (H. R.). Deteimication of Free Acid in Tan Liquors . . .WEIOERT (L.). Estimation of L4celio Acid in Urine I . . . .NESSLER (J.). Detection of Free Tartaric Acid, a:id on Snlpliuric Acid inUrine .. . . . . . . . .DWAR~ (B. W.). On the Todosulpl~ates of the Quini~~e'dlkaiol.ds. . .KOETTSTORFER (J.). .STEIX ((3.). Anal-sis of Turkeyred Oil . . . . . . .S!~~HV ((7,). Estimation of Urea . . . . . . . . .SCEOTT (0.) Estimation of Ioiline in Vareo . . . . . .Estimation of Phosphoric Acid in Artificial Manures . . . . ,MILLOT (A). Insoluble Phosphoric Acid in Superphosphate . . .PBECHT (€1.). Volumetric Estimation of Magnesium . . . . .3laX.v ((3.). b e m Volumetric Method for Estimating Zinc . . . .CLASSES (A,). Estimation of Cobalt, Nickel, and Zinc by Precipitation anDetection of Blighted 7Vheat in Flour by the SpectroscopeA New Method of Testing Butter for Foreign FatsOxalates .. . . . . . . . . . . .CLASS~N (A,). Separation of Jfanganese from Zinc . . . , .CLASSEX (A,). Kern Method of Separating Ferric and Aluniinium QxidesNILSON (L. F.). Criticism on Buiisen's'Older Method ;or Seiiarating ArseniEfrom Slanganese . . . . . . .from Autimoiiy . . . . . . . . " . .TORNOE (H.). .REYXOLDS (J. E.). Sugar as a Test of thc Purity of TVater . . .LEEDB (A,). Estimation of Sitrates in very Dilute Solution . . .ALLEN (A. H.) . Petroleum-spirit and Benzene . . . . . .HEXPCL (W.). Limit of Detection of Carbonic Oxide . . . . .PLUGGE (P.). Decomposition of Xercuric Cyanide bg Dilute Acid?, alonea d in Presence of Sodium Chloride . . . . . , .T 1 - a . i ~ ~ (P.). The Ebullioscopc . . . . . . . . .YTEISER (J.). The Ammoniacal Copper Test and its Application.. .ESBACH (G,). Estimation of Urea in Urine . . . . . , ,TATTERSALL (J.). Xew Test for Papaverine . . . . , ,WATSOX (W. H.). Detection of Milk Adulteration . . . . .SOXHLET (F.). Quantitatire Estiniation of Milk F a t . . . . .BLYTH (A. IT.). Composition of Deronshire Cream . . . . .R*sults of the Norwegian Expedition to the North Sca .9i4'3769769779799799y0980981982983984!!55105110521052105310541cj5d1055105310%10t1010f1210c121063106310641c16510661067106710681068106xxxvi COSTE-UTS.PAQEKOETTJTORFER (J.), .PERKINS (F. P.). Analysis of Butter Fat . . . , . . . New Method of Detecting Foreign Fats in ButterTechii,ical Chemistry.EYYDBOVEK (J.ran). Gaelighting . . . . , . . .TICHBORSE (C. R. C.). Some Pecnliarities of the Vartry Water, and theaction of that Water on Boiler-plates . . . . . . .SCHIFF (H.). Preservation of Potable Waters . . . . . .FISCHER (F.). Utilisat,ion of Suint from Wool . . . . . .STEAD (J. E.) . Phosphorus in Cleveland Ironstone and in Iron . . .STEINAE (R. and C.). .CECH (C. 0.). Preparation of Rosemary-oil . . . . , . .SAKTOS (J. R.). Analyses of Lamp-black made from the SaturaiHydrocar-SIYOXIX (L.). The Part played by Coal-dust in Proiucing Explosions inCoal Mines . . . . . . .LITACHE (A,). Abnormal Solubility of certain Bo‘dies in Soaps and A l k i n eResinates . . . . . . . . .WITTMACK (L.). Adrantages of only Paltially Remoring the Fat from Oil-Seeds , ., . . . . . . . . . .OOTTFRIEDSEX. On Tanning and Mineral Tanning . . . . .Intensifjing Photographic Xegatires by nieans of Potassium Sulphide . .Preparation of finely divided Metallic Oxides . . . . . .JOCLET (V.). C s e of Chrome Alum instead of Potassium Dichromate inBELL (I. L.). Separation of Carbon, Sulphur, and Phosphorus in OpenHearth, Puddling Furnace, and Bessemer-conrerter . . . .BOTTGER (R.). Steeling Copper-plates . . . . . . . ,BIERXAKS (E. W. L.), Manganese Alloys . . . . . . .VACCHER (G.). Ly-ch6, a New Tkckening katerial . . . . .M~~LER-JACOBS (A). Mordant for Turkey-red Dyeing . . . .TCLPICS ((3.). BehaTiour of Vulcanised Caoutchouc Kith Illumi’nating GasDEITE ((3.). Iodine Industry in France . . . . . . ,OERL.4CH (G.T.). Extraction of Sulphur by means of Superheated Steam .DIXON (1%‘. A). Metallurgy of Nickel and Cobalt . . . . .KERX (S.). Purification of Cast Iron from Phosphorus , . . .KERN (S.). Distribution of Mmganese in Ferro-Manganese Alloys . .Analyses of Clay8 . . . . . . . . . .IRELAXD (J.). Blair’s Process for Iron kmufacture . . . .Manufacture of a Red Pigment from Iron ScrapGAYOX (U.). Inactive Glucose in Crude Cane-sugars . . . .bon Gas of the Ohio Petroleum Region . . . . . .KALLAB’S Sew Bleaching Process ;or dnimal Tekile Fibres . . .WAGSER (R. T.). Kume’ite, a Kew Jewel . . . . . .m’ool-dyeing . . . . . . . . . .Preparation of Inverted Sugar . . . . . .PRTD’HONNE. Reduction of Indigo br Glycerin . . . .BOUSSIXGACLT. Chrome-Steel .. . . . . . . .KEITH’S Process for Desilrering and Refining Raw Lead by Electrolysis .DIXON (W. 4.). Extraction of Gold, Silrer, and other Metals from Pgrit,esESTCOURT ((3.). Desirability of Fixing by Analysis some Standards of Value . .Manufacture of Resorcin, Ebsin. and otherfor Beer, based on the Qualities usually sold in Large Towns.WEIGEBT (L.). Clarifying and Preserving Wine . . . .BINDSCHEDLER and BUSCH.Derivatives of Resorciii . . . . . . . . . .DEITE (C.). Testing Lubricating Oils . . . . . . . .LEWIN (L.). Spongy Iron and Animal Charcoal as Naterials for PurifyingWater . . . . . . . . . . . . .WOLFFHUQEL (a,). Carbon Monoxide in Foundrr Furnaces . . ,LAWRENCE (R.) and C . W. REILLY. Analysis of’Burton Ales and DublinPorter .. . . . . . . . . . . .10691070a5858586879097979797989999991001841841848918518518618618718818828418718728328628628628628829029029129234334434428CONTEXTS. xOn Cement . . . . . . . . . . . . .TEREEIL (A,). Analysis of Metallic Fragments obtained from PeruvianTombs at Ancon (Lima) . . , . . . . . . .Direct Preparation of Wrought Iron and Steel from Iron Ores . . .KERN (S,). Working of Mild Steel . . . . . . . .KEITH. .BERTHOLLET. Explosive Mixtures of Air with Combustible Pow&rs . .KORSCHELT (0.). Saki, the Alcoholic Drink of the Japanese . . .Aniline Blue . . , . . . . . , . . . .-4lizarin Blue . . , . . . . . . . . .GRAWITZ (S.). Sction of Chrominm Salts in presence of Chlorates ..WITZ (G.). Inactirity of Chromium Compounds in producing Aniline-blackES conipared with the Action of Vanadium Compounds . . . .L’HOTE (L.). Process for enriching Phosphatefi containing Earthy Car-bonates . . . . . . . . . . . .LOWIQ (G. and F.). Preparation of Alumina . . . . . .LOWI~ (G. and F,), Preparation of Alkaline Aluminates . . . .COCX (L. C. W,). Solubility of Lime in Water in refcrence to the prescrip-HERIXQ (C. A,). Recovery of Antimony . . . . . . .Damage done to Barley by Sprouting in the Field . . . . . .BLANKEXHORN (A,). AEration of Must . . . . . . .DREVERXABX (A). Recovery of Sugar from Calcium Saccharates . .WIGXER (G. IT,). Kitrogenous Constitnenrs of Cocoa . . . . .WIQSER (G.W,). Some experiments with Silicated Carbon and Spongy IronFilters . . . . . . . . . . . .GABBA (L.) and 0. TEXTOR. Influence of t i e Chemical Composition of theWater used in the preparation of Raw Silk . . . . . .Formation of Aniline Black by Chromates in presence ofProcess for Desilrering and Refining Raw Lead by ElectrolysisFIBCHER (F.). Wearing of Steam Boilers , . . . .tion for Aqua phagedanica . . . . . . . .Methylaniline . . . . . . . . . .GRAWITZ (S.).Chlorates . . . . . . . . . .On the Preparation of Paper ior Pigment or Carion Photo- OTT (A,).graphy . . . . . . . . . . . . .GLEQE (0.). Calcium Chloride . . . . . . . . .BENRATH (H. E.) . Nacapo’s Inrestigations on Bottle Glass . . .SI~~OBIN (L.). A New Process for the Treatment of Iron and Cower _ -Pyrites in the Dry W a r .Application of these Xetala .. . . . . . .. .FLEITXASS (T.). Preparahon of RIaileable Kickel and Cobalt. and theCoating of Metals with their Oxides to guard them against itmosphericAction . . . . . . . . . . .KERB (S.). Action of Sea-water on Iron an; Steel Plates . . . .Use of Anthracite Dust in Du Puy’s Process . . . . . . .FISCHER (F.). Iron Smelting in the Cupola Furnace . . . .DE Pry (C. &I.). . Direct Process for Making Wrought Iron and iteel .MULLEX (F. C.’G.). The Bessemer Process, . . . . . .KERX (S.). Steel Making . . . . . . . . . .KERB (S.). Manganese Steel. . . . . . . . . .KERB (S,). Preparation of Chrome Crucible Steel . . . . .MARCAXO (V.) and A. MUXTZ. Utilisation of the Banana .. . .WEIGELT (C.). The Time of F i r i Racking-off New Wines . . . .WEIQELT ((3.). Dochnahl’s New Xethod of Preparing Wine . . .SCHULTZE (W.). The Malt Test . . . . . . . . .BINDSCHEDLER and BESCH. Kew Fast Green, or kalachite Green . .Colouring Matters . . . . . . . . . . . .REIMAXX ($1,). Chrome Black on Wool . . . . . . .BEIKS (H.) , Preparation of Carbonic Anhydride under any desired PressureDELTE (C.). Ghea Butter . . . . . . . .WHEWELL (G.). Tenacity of Starch . . . . . . .xxviiPAGE40740940941041041041241341 541 942042149049049149149149249249249349349349449556056256256356356356456456456556656756756756856556956956957057157157267ssxviii CONTESTS.LUKQE (G.).Antichlor . . . . . . . . . .WALLACE (R. W.) and C. F. CLACS. Application of Gas Liquor to the Pro-duction of Potassium Carbonate and other Salts . . . . .LEXQB (G.). Soda Industry . . . . . . . . .Preparation and Use of a highly Siliceous Pig-iron . . . . .Malleable Iron a t the Paris Exhibition of 1878 . . . . . .L r c a (S. DE.). d Thread-like Subfitance found in the Excarations ofPompeii . . . . . . . . . . . . .GAWALO~~SKI. A Process for Utilising the Residue from the Manufacture ofKERNLTER (F,). On Making Red’Wine . . . . . . .KESSLER. Pressing of Red Wine , . . . . . . . .POLLACCI (E.), Plastering of Wine . , . . . . . ,WITZ (G.). Value of Certain Chemical Agents in Pyeing with Aniline-black .. . . . . . . .A Black Lac ;or Tvietal and Tqood . . . . . . . . .OTT (A,). Heliographic Printing . . , . . . . . .WEBER (R.). Composition and DurabiiitF of Class . . . . .Extraction of Silrer from the Fahl-ores of Baranca, Mexico . . . .JORDAN (P.). Preparation of Mangaiiiferous Pig-iron . . . . .HOLLWAY (J.). d Kern Application of Xapid Oxidation by which Sulphidesare Utilised for Fuel . . . . . . . . . .BODE (F.). Extraction of Copper by Wet Processes , . . . .WISICLER (C.). Fire-damp in Collieries . . . . . . .J-LILLARD. Absorbing Pomr of Wood Charcoal . . . . . .BEYRICK (C.). Process for Bleaching Vegetable Fabrics . . , .HILGER (A). Composition of “Grains” from Malt . . . . .LCSGE (G.). The Amount of Sulphuric Acid in Wines .. . .POLLACCI (E.). Plastering of Wine . . . . . . .BERTHELOT. Changes which Wine undergoes when kept . . .~ a L I x n c R r 1 (A,). A Critical Point in Making Parmesan Cieese . .OTT (A,). Photolithography . . . , . . . . .WARTHA (V.). Hectograph and Chromograph . . . . . .MROTVEC (S.). Carbon Bidphide Manufacture in Swoszomice and its ZT$eThe Ammonia Soda Process in conjunction i i t h the Manufacture of Gas .RAMDOHR (L.). Superheated Steam . . . . . . . .KLCTEAR (J,). Loss of X t r e in the Vitriol Manufacture . . . .PILTER (T.). Decomposition of Phosphatic Minerals . . . . .itioii of a Boiler Incrustation . . . . .Xethod of producing a Coating of Magnetic IronOxide on Iron Surfaces . . . . . . . . . .KOPPES (E. T.). Physical and Chemical Changes which Spiegelaisen Ironundergoes when Smelted in the Cupola Furnace .. . . .CHCRCH (J. A). Combustion in the Blast Furnace . . . . .DEBRCSNER (H. (2.). Third Form of Carbon in Steel . . . .Potassinm Ferrocpnide . . . . . . . . .BUHRIG (H,). Cerium Aniline-black . . . . . . .LCSGE (G.). Soda Industry . . . . . . .RAETZ (T.). Enamel for Casl- and Wrought-iron . . . .for the Extraction of Sulphur . . . . .Beer Analyses . . . . . . . .STUTZER (A,). Preparation of Pressed’Yeast as a Bye-Product from PotatdSpirit . . . . . . . . . . .PILTER (T.). Artificial Animal ~ i a r c o a l . . - . . . .POKORMY (F.). Purification of Beetroot S ~ u p . . . . . .STEFFESS, MAXWRY, MATEYCZEK, and DRETERXANX. Recovery of Sugarfrom Molasses . . . . . . . . .VEITZ (11,). .ABEL (F. A.). Recent Contributions to the History of Detonating Agents .MANETTI (L.) and G. MUSSO. Composition of Skimmed Wiey . . .Crystallisation of Sugar and Preparation of Sugar CandyEDER (J. M.). Examination of Chinese Tea . . . .PAGE6766776i767861968068068168168168268468475075115475575.5c- w / J D755,7571f07617617617627627637648368368378378358388398398408408418 la84284384484484484484685 185CONTESTS. xxxixEUQLIXG (W.) and v. KLESZE. Alpine Dairy Produce . . . .DUCLAEX (E.). Ripening and Decomposition of Cheese . . . .RIESSI~~LLER (L.) and H. WIESNIGER. Conrersion of Rags and Hair intoManure . . . . . . . . . . . . .HABERLAXDT (F.). Strength of Hemp. . , . . . , .JfOELLER (J ). Fibrous Materials . . . . . . . .GHo.sl\rAs (J.). Softeninc Magnesia-hard Water , . . , .l’otes i n Potable TVaters . . . .eriments with Animal Charcoal, S k a t e d Carbon,of Gas by Amnionis . . . . . .K ~ S I G (I).). Deco:nposition of Bones b>- Steam . , . . . .J o c L i E (1%). Retrogmclation of Superphosphates . . . . .DOFGLAS (T,). Grecn Pigment from Barium Chromate . . . .ILGEX (0,). Solray’s Soda used in the Preparation of LTltramarine . .Contributions to our Iinon-ledge of C l a p . . . , . . .Liquid Cpnicles and Chlorides in Blast Bnrnaces . . . . . .l ’ a ~ x n a (A). Obtaining Tanadiuru from the Eranium Ore of JoachinlsthalHi:ssG (IT.). Refining Copper . . . . . . . . .WE~ICK. (R.). 13eli:irionr of Tin and Lead A l l o ~ s with Vinegar . . .~ I I I T I I (11. A). Detection of Firedamp . . . . . . .SA~~cicic and YICLLE. .K0ur.E am1 I n i : ~ . Conibuition of G u n p o d e r . . . . . ..). Rotator- Pomv of Uecr Worts . . . . . .ONN (L) and H. IT-. UAIILES. Fermentation of Must. . .) , Resin-sizing of l’nper . . . . . , . .of the Kesitlues obtoiiied in the Manufacture of Aniline-red .AS (C.). S:nnnfnctnre of 3letlij-laniline . . , . .Q i i c b r a c h Wood . . . . . . . . . . . .1’NocTm (H. R,). Erplosi.ie Product of Solution of Phospliorus in Carbon1’s. . . . . . . . . .llecoluposition of Gun-cotton in a Closd TcsselTHO\I~ (G,), Teak II-LWC~ . . . . . . . . . .Bisulpliide . . . . . . . . . .FLECK (E.). 3Innufacture of Artificial hlother of Peari and of Imitations ofMarble from G-lne . . . . . . . . , . .HEYDEX (F. v.) and T. ECLART. Preservation of Meat . .l \ ~ r i m o (G.) nnc~ A. >fExozzI. Forwation of Fat from Case’in in the Ripen: . . ing of Cheese . . . . . . . . ,FISCIIXIL (F,). Heating Steam Boilers . . . . .GKXKIXG. Ferric Chloride as a Purifier of TT-ater . .SCII~FF (I€,). Preserration of Drinkaldo Water . . .MORGAS (T. M,). Coinposition of a Well-water a t Gronr-ilkL i s G w i s (G,),’ SouthiiiiericanYa:tpi.tre . . . . ,Clieinical Tecliiiology of Glass . . . . . . ..IRSOLD (1. E,). l’lioapliorus in Ancient Iron . . . .hoslihorisation of Pie-iron . . , , . ,CLOCET :nid RITTER lrseiric ill Grape-sugar . . , ,3faci1 ( E . ) ~ Experiinents on tlie Fiiiiiig of Wine , , ,Distilleries . ,ing . . . ,er Fermentation , .HOLZSER (G.). Reaeilrches on Beer . . . . . .. . . . .PAGE8578588598538699%9859%08698798 798798798898998Y99099099199199299399399 1995296996996996996996996 . . 1070 . . 1072 . , 1072. . l O i 2. . 10i3 . . 1074 . . 1Oi4. . 1075I . 1076. . 1076 . . l 0 T G. . l o x . . 10T7. . 1078. . 1078, . 10T8 . . 1078 . . 1073. . 1079 \ , PECKIU~I (S. F.). Explosion of thc Flour llills at IIinncnpolis, Xii-nesuta . . . . . . . . . . . . 10i9SOKOLOFF (3.). Esplosion of Xitroaiannite . . . . . . 1080BEcai. The Proper Time for Pressing Ollie8 . . . . . . 108xl COSTESTS.SMITH (W ). Extinguishing Fires in Tar Distilleries . . . .FALSKY (F,). Salicylic Acid as a Prerentative of House-fungus . .ZEREKER (H.). Method of Preventing House-fungus . . . .Pa teii fs.DUSCAY (J.), J. A. R'. NETTLANDS, and 13. E. R. XEWLANDS. Improvementsin t,he Ti-eatment of Saccharine Substances 01- Compounds . . .HOLLIDAY (J.). Improvements in Djeing and Printing Aniline-black . .MACTEAR (J.). .COTTE (E.) . Improreinents in the Manufacture of Certain ExplDsive Com-pounds . . . . . . . . . . . . .BRUXNER (H.). Improvements in the IIanufncture of Alkali . . .LAVENDER (R.). Improvements in heating Waste Sulphuric Acid that hasbeen used for Pickling Iron Plates and other Articles of Iron or Stcel .CLAUS (C. F.). Improveuients in the Manufacture of Sulpliide and otherCompounds of Zinc, and in tlie production of EFe-products resultingtherefrom . . . . . . . . . . . .Improvement in the Preparation and Treatment of SaccharineSubst,aiices and Compounds . . . . . . . , .lmpi-orements in tlie Manufacture of Snlphate of Alumina.Improvements in Purifjing or RefiningCopper . . . . . . . . . . . .Improvements in the &fanufacture of $faterials containingTannic Acid . . . . . . . , . . . .J. P.). &Innufacture of Ammonia, . . . . . , . J.). Treating Ores containing Silser and Copper . . .in the Treatment of Sugar . . . . . . . .DUNCAN (<J.), J. A. R. NERLANDS, and B. E. R. SETLANDS. ImprovementImprovements in the Manufacture of Soda and PotashPRICE (A. P.).CROLL (A. A,).WILXES (I.) and T. JOHSSOS.v E D O ~ A (F. 6.1.PIOF.10801080108042142 142242242242242542342342342349649649

ISSN:0368-1769    

DOI:10.1039/CA87936FP001

出版商:RSC    

年代:1879

数据来源: RSC

摘要:

8 ABSTRACTS O F CHEMICAL PAPERS. Inorganic C h e m i s t r y . Preparation of Chlorine and Hydrochloric Acid by means of Calcium and Magnesium Chlorides. By E. SOLVAY (Cheni. Cedr., 1818, 336) .-The above-mentioned chlorides are mixed with silica and alumina or silicate of alumina, and dried. To obtain chlorine they are intensely heated in a current of sir ; for HC1 they are heated in a current of superheated steam. Silicates and alumi- nates of lime and magnesia are formed as bye-products in this pro- cess, and may be used for making chloride of lime and precipitated silica and alumina, also for making chlorine from hydrochloric acid, and for soda manufacture by the ammonia process. J. X. T. Hydrochloric Acid containing Phosphoric Acid, By E. HOLDERMANN (Arch. Pharm. [3], 13, 100--103).-A sample of hydrochloric acid gave when tested all the reactions for purity, so that when evaporated over a bare flame in a platinum vessel it left a barely perceptible residue, but when iron was dissolved in the acid, a white precipitate was formed, which on examination was found to be due to a large quantity of phosphoric acid present.It is, therefore, advisable, when testing for phosphoric acid by volatilisation, to evaporate the liquid in a watch-glass over the water-bath. E. w. P. Ozone. By JEREYIN (Deut. Chem. Ges. Ber., 11, 988).-The author finds that ozone dissolves to a considerable extent in aqueous oxalic acid, forming n solution which keeps indefinitely. A solution which has been kept some time is a better disinfectant than whenINORGANIC CHEMISTRY.9 fresh. I n the gaseous state ozone keeps better in the light than in the dark. For washing with ozone the author constructs stoppers, stop- cocks, tubes, &., of a composition of powered pumice, paraffin, wax, and resin, which is not acted on by ozone. For experiments with sub- stances which attack paraffin he recommends a composition of gelatine and glycerin. J. R. Oxidation of Nitrous Acid by Ozone and by Moist Oxygen. By BERTHELOT (Aizn. Chim. YJiys. [ 5 ] , 13, 367--368).-1n an acid solution nitrous acid is a t once oxidised to nitric acid by ozone, which niay be exactly determined by this means. A standard solution of a nitrite is acidified and shaken with a gas containing ozone, wliicli oxidises the nitrous acid and is itself Rbsorbed.The excess of nitrite in the solution is then titrated with potassium permnnganate. 111 presence of alkalis, the ozone i s destroyed without acting on the nitrous acid. Dry *oxygen or ozone converts nitrous acid into nitrogen tetroxide, which in presence of water yields nitric acid. It is thus clear that the presence of nitrous acid and ozone simultaneously in t'he air is not possible. Presence of Amrnoniacal Salts in Sea-water. By M. L. DIEULAFAIT (Arm. Chim. Phys. [ 5 ] , 13, 374-409).-The presence of ammoniacal salts in sea-water was first pointed out by Marchand (Mem. Acad. &fed., 19, lb55), and subsequently investigated by Bous- singault (Ayroriomie. Chim. Agrie et Physiol., 208), and Forchammer (Phil. Trms., 155, 203). The author has made fresh determinations of the ammonia present in sea-water ; also of its deposits, employing Boussingault's method with slight modifications.Wrder from the JIeditewanea?z.- This water was taken south of Marseilles, 12 kilometers from the shore, and about the mericlian of Aix. 10 litres were distilled and 4 litres collected and redistilled. 800 C.C. of the second distillate are again distilled, and the ammonia determined in the first 300 C.C. which come over. In this manner the result obtained was *231 mg. NH, per litre. From water taken between hlarseilles and China a t depths varying from 1.5 to 2 metres, the following results were obtained :- mg. N I B per litre. Ismaila.. .......................................... 0-204 Red Sea, long. E. 33" 5 4 , lat. N. 24" 4' ..............0.176 Cape Gardafuy, long. E. 49" 42', lat). N. 12" 44' ........ 0.176 Socatora, north of the island ........................ 0.17C; Bay of Bengal, long. E. 87" 55', lat. N. 5" 34'. ......... 0.136 Coast of Cochin China, long. E. 107" 22', lat. N. 14" 37'.. 0.340 From these results it is seen that ammonia occurs in seas of all latitudes. The quantity of ammonia in the sea-water does not increase pro- portionally to the evaporation of the water, inasmuch as a portion of the ammonia escapes into the air. The Ammonia in the Deposits from Sen-water.-During the evapora - tion of the water in saline marshes, deposits are formed, the first con- sisting of pure cryatallised gypsum covering the surface of the pan, Moist air also slowly oxidises nitrous acid. L.T. 0's.10 ABSTRACTS OF CHEMICAL PAPERS. whilst the second is a black mud, obtained partly by the decomposition of the “ feutre,” the term applied to the “ stratum” of algae which covers the bottom of the salt-pans. There is also a greenish-yellow liquid obtained, which contains some of the refuse of the mud and a large quantity of gxpsum. Each of these contained ammonia in the following proportions :- Gypsum ........ 1.6 mg. NH, per kilo. Liquid.. ........ 3.4 ,, per litre. The water of the pool of Lavaldue contains 250 times more ammonia than the water of the Seine a t Paris, and 50 times more than that of the Bievre, on the banks of which many manufactories stand. By the evaporation of the sea-water, deposits are obtained; in the first place calcium carbonate, mixed with oxide of iron and strontium car- bonate, separates out, but the more important deposits are those of gypsum, which are two-( 1) pure gypsum, and (2 j gypsum mixed with calcium carbonate and some mud, imparting to it a grey colour.There is also a deposit of mud. These last three absorb ammonia, which fhe author has determined in twenty samples obtained from different places to the south of France. The results, of which the following are examples, show the variation in the quantity of ammonia :- Black mud ...... 8.3 ,, 7 9 Pure gypsum. Grey gypsum. Triassic. “g. mg. Simiane (Bouches du Rhone) . . 1.2 6.2 Saint Julien . . . . . . . . . . . . . . . 1.6 2.6 Castellane .................. 2.4 3% La Palud .................. 0.8 3.1 Taulanne.. ..................1.4 3.0 Solli&s (Ville) .............. 1.9 3.1 Le Beausset ................ 3.2 4.3 Le Faron (Toulon) .......... 1.8 4.8 Bandol ...................... 2.2 4.6 Black mud. mg. 15.0 12.2 14.0 11.2 12.7 14.0 11.1 12.9 14-5 The author has also examined some gypsum beds of the tertiary formation for ammonia, arid finds that they correspond with the grey gypsum above, having given the following resalts :- Bois d’dsson ............ Saint Jean de Garquier . . 2.14 ,, 7, 4.04 mg. NH, per kilo. Camoins ................ 2.87 ,, ? > The presence of ammoniacal salts in the gypsum accounts for the disengagement of ammonia in the manufacture of plaster of Paris. The boric acid emitted by the lagoons in Tuscany is often accom- panied by ammonia, which may be explained if it is admitted that the boric acid exists in the saline beds of the lagoon, which absorb ammonia, and that the part played by the volcauic agent is purely mechanical, whereas on the contrary, by assuming the boric acid to have a volcanic origin, the presence of ammonia cannot be explained.The water of Lake d’Enghien contains only 0.07 mg. NH, per litre, whilst the sulphur spring fed by the lake contains 5.06 mg. per litre.1NORGlANJ.C CHEMISTRY. 11 This is due to the fact that the water on emerging from the lake has to pass over sediments, from which it dissolves the ammoniacal salts. The author is of opinion that all saline waters obtain their mineral matter from the two salt-bearing formations, the trias and tertiary, which always contain a consid2rable quantity of ammoniacal salts, and the conclusion he draws is that all saline mineral waters ought to contain abnormal quantities of ammoniacal salts, whether they be sulphurous or not, thermal or not.L. T. 0's. Chemical Action of Water and Saline Solutions on Zinc. By A. J. C. SNYDERS (Deut. Chem. Ges. Ber., 11, 936--949).-The author has examined the action of water and of saline liquids on zinc under various conditions. 1. Zinc decomposes saline solutions, whether concentrated or dilute, without access of oxygen, evolving hydrogen and forming zinc oxide. 2. Solubility of zinc oxide in the saline liquids promotes the action. 3. Zinc oxide dissolves in solutions containing 1 per cent. or less of salt. The solubility varies with different salts, being greatest with ammonium salts.Zinc hydrate and carbonate are insoluble in carbo- nates. The solubility of zinc oxide increases with the strength of the solutions and with the temperature. 4. When a saline liquid is saturated with zinc oxide, the decom- posing action still goes on, the oxide then formed remaining undis- solved. 5. In presence of oxygen free from carbon dioxide, the zinc oxide dissolves more readily, on account of the direct oxidation of the metal. 6. In presence of the carbon dioxide of the air, the solvent action is to some extent prevented, owing to the formation of basic car- bonate. 7. The solvent action is strongest with chlorides and potassium sulphate, weaker with alkaline and barium nitrates and magnesium sulphate. 8. Solutions of alkaline carbonates and sodium phosphate do not act on zinc protected from the air.Even in presence of oxygen, solutions containing 1 per cent. of these salts dissolve but little zinc, because the carbonate or phosphate first formed protects the metal from further action. Nevertheless, traces of zinc oxide are dissolved by still weaker solutions. 9. The solrent action is greater at higher temperatures : a t 0" it is very slight. 10. Solutions of ammonium salts take up more zinc oxide than solutions of salts of fixed alkalis. The surface of the metal remains clean, and nothing is deposited from the solution, even in presence of oxygen. 11. Hard waters do not act on zinc, even when rich in chlorides and sulphates. Soft waters dissolve the more zinc the greater the preponderance of chlorides, sulphates, and ni hates over carbonates and phosphates contained in them.His results are summed up as follows : J. R.12 ABSTRACTS OF CHEMICAL PAPERS. A New Earth of the Cerium Group, and on the Analysis of Natural Niobates. By J. L. S i I I ' r H (Con@. reud., 87, 146-148). -The object of this paper is to call attention to the use the author made of concentrated hydrofluoric acid for decomposing niobates ; its action on samarskite and euxenite being as energetic as that of hydro- chloric acid on calcium carbonate. By the actiori of the acid, all the metallic acid forming oxides, together with the oxides of iron and man- ganese, are dissolved, whilst the insoluble portion contains all the earths and the uranium oxide. The presence of tantalates renders the decomposition more difficult.I n a former memoir, the author divided the earths contained in Carolina samarskite into the yttrium and cerium groups, pointing out however that the latter group might not contain cerium oxide, and that thorium could not be detected i n it x i t h certainty. Since this, he has found that the yttrium group con- tains about two-thirds of yttrium and one-third of erbium, whilst cerium is absent from the group bearing its name. He also points out that the earths of this group contain 10 per cent. of thorium, a small quantity of didymium oxide and an earth (about 3 per cent. of the mineral) which the author considers to be new, if i t is not the hypo- thetical terbium of Mosander. De la Fontaine of Chicago has con- firmed the absence of cerium, and looks upon the new earth as terbia.The author thinks, nevertheless, that he has found a new earth, and that if terbia exists among the oxides of samarskite, it is contained in the yttria group. Comparing the atomic weight of the supposed new earth with those of the oxides of cerium, lanthanum, or didymium determined by JIarignac (0 = 16) we have :- New earth.. ................ 109 (Smith). Cerium oxide .............. 110 (Marignac). Lanthanum oxide., .......... 110 ,, Didymium ,, ............ 112 ,, The new earth differs from those of the j t t h gronp in its action with potassic sulphate, from cerium oxide by its solubility in very dilute HN03, from didymium oxide by its colour, from lanthanum oxide by its colour and the ease with which its salts are decomposed by heat.The author has aIso devised a method for the separation of thorium, as follows : the freshly precipitated oxides are placed in a solution of potash or soda, and a current of chlorine is passed through the mixture when all the oxides are dissolved except those of cerium and thorium ; as the samarskite contaius no cerium, the residue consists merely of a white gelatinous precipitate of thorium oxide. J. $1. T. The supposed New Element Mosandrum. By J. L. SMiTH (Conipt. r e d . , 87, 148--131).-This paper is occupied by a claim for the priority of the discovery of the earth indicated as X by Soret in his paper to the Academy. The author maintains to have found this earth in samarskite from North Carolina, and gives a minute account cf its discovery and of his correspondence with De la FontaineIX'ORGAK'IC CHEMISTRY.13 and Marignac on the subject. Basing his remarks on his own work and tdie spectroscopic examination by Soret, he now has no hesitation i n claiming mosandruin as a new element. On the Discovery of a New Earth announced by J. L. Smith. By C. MARIGSX (Co?72pt. reid., 87, 281-5283 ).-In this paper Marignac points out the reasons leading him to the conclu- sion that Smith's " mosandrum " is identical with Mosander's " ter- bium ; " whilst the earth provisionally designated X by Soret and the author, differs from t,htl former in its absorption phenomena, althougli it shows nirt11~- points of resemblance with an earth described by De la Fontaine of Chicago. J. AT. T. J. M. T.Magnetic Compound; having the Formula RO.Fe,O,. By K. Llsr (Delcf. Clmn. Ges. Be,.., 11, 1512-1.516j.-Lime water pro- duces in a neutral solution of ferric chloride a brown precipitate, which is magnetic, and after ignition has the composition Cs0.Fe207. I n a similar manner magnetic compounds of magnesia and bnryta with ferric oxide can be obtained. The corresponding manganese, nickel, copper, and lead compouuds are formed when soda is added to a solution containing ferric chloride and copper sulphatc, &c., in their equivalent proportions. Magretic compounds are also formed when sodium or potassium carbonate is fused with ferric oxide. w. c. w. Dissociation of Metallic Sulphides. By P. DE CLERMOST and J. PROMJI EL (Co??2pt. re72d., 87, 330, 332 j .-The decomposi- tion which ensnes on boiling certain sulpliides with water is regarded by the authors as due to the dissociation of a previously formed hydrate of the sulphide.They point out that freshly precipitated sulphide of arsenic boiled with water gives rise to a more rapid evolu- tion of sulphuretted hydrogen than tlie same sulphide does when it has previously been dried at 12.5". But if this last is kept in coutact for some hours with hot water in a closed vessel, i t gives off sulphuretted hydrogen, when boiled in an opcn vessel, as rapidly a s the freshly precipitated sulphide. On boiling snlpliides with water in a vacuum, dissociation was observed to occur a t tlie following temperatures : sulphide of arsenic, 22' ; sulphide of iron, 56" ; sulphide of antimony, 95".The dissociation of arsenic sulpliide presented ccrtain pecn- liarities, which the authors believe to be due to the interference of the arsenious acid, which is one of the products of decomposition. The presence of this substance impedes the dissociation, by the formation, as they suppose, of an oxpsulphide which undergoes dissociation more Sulphide of arsenic, to which crystallised arsenious acid has been added, is dissociated more quickly than that to which arsenious acid obtained by the dissociation of tlie sulpliide has been added. As arsenic pentasulphide on dissociation yields arsenious acid and not arsenic acid, the author doubts its existence as a definite chemical compound. R. R. slowly.8 ABSTRACTS O F CHEMICAL PAPERS.Inorganic C h e m i s t r y .Preparation of Chlorine and Hydrochloric Acid by means ofCalcium and Magnesium Chlorides.By E. SOLVAY (Cheni.Cedr., 1818, 336) .-The above-mentioned chlorides are mixed withsilica and alumina or silicate of alumina, and dried. To obtainchlorine they are intensely heated in a current of sir ; for HC1 theyare heated in a current of superheated steam. Silicates and alumi-nates of lime and magnesia are formed as bye-products in this pro-cess, and may be used for making chloride of lime and precipitatedsilica and alumina, also for making chlorine from hydrochloric acid,and for soda manufacture by the ammonia process. J. X. T.Hydrochloric Acid containing Phosphoric Acid, By E.HOLDERMANN (Arch. Pharm. [3], 13, 100--103).-A sample ofhydrochloric acid gave when tested all the reactions for purity, sothat when evaporated over a bare flame in a platinum vessel it lefta barely perceptible residue, but when iron was dissolved in theacid, a white precipitate was formed, which on examination was foundto be due to a large quantity of phosphoric acid present.It is,therefore, advisable, when testing for phosphoric acid by volatilisation,to evaporate the liquid in a watch-glass over the water-bath.E. w. P.Ozone. By JEREYIN (Deut. Chem. Ges. Ber., 11, 988).-Theauthor finds that ozone dissolves to a considerable extent in aqueousoxalic acid, forming n solution which keeps indefinitely. A solutionwhich has been kept some time is a better disinfectant than wheINORGANIC CHEMISTRY. 9fresh.I n the gaseous state ozone keeps better in the light than in thedark. For washing with ozone the author constructs stoppers, stop-cocks, tubes, &., of a composition of powered pumice, paraffin, wax,and resin, which is not acted on by ozone. For experiments with sub-stances which attack paraffin he recommends a composition of gelatineand glycerin. J. R.Oxidation of Nitrous Acid by Ozone and by Moist Oxygen.By BERTHELOT (Aizn. Chim. YJiys. [ 5 ] , 13, 367--368).-1n an acidsolution nitrous acid is a t once oxidised to nitric acid by ozone, whichniay be exactly determined by this means. A standard solution of anitrite is acidified and shaken with a gas containing ozone, wliiclioxidises the nitrous acid and is itself Rbsorbed. The excess of nitritein the solution is then titrated with potassium permnnganate.111presence of alkalis, the ozone i s destroyed without acting on the nitrousacid. Dry *oxygen orozone converts nitrous acid into nitrogen tetroxide, which in presenceof water yields nitric acid. It is thus clear that the presence of nitrousacid and ozone simultaneously in t'he air is not possible.Presence of Amrnoniacal Salts in Sea-water. By M. L.DIEULAFAIT (Arm. Chim. Phys. [ 5 ] , 13, 374-409).-The presenceof ammoniacal salts in sea-water was first pointed out by Marchand(Mem. Acad. &fed., 19, lb55), and subsequently investigated by Bous-singault (Ayroriomie. Chim. Agrie et Physiol., 208), and Forchammer(Phil. Trms., 155, 203). The author has made fresh determinations ofthe ammonia present in sea-water ; also of its deposits, employingBoussingault's method with slight modifications.Wrder from the JIeditewanea?z.- This water was taken south ofMarseilles, 12 kilometers from the shore, and about the mericlian ofAix.10 litres were distilled and 4 litres collected and redistilled.800 C.C. of the second distillate are again distilled, and the ammoniadetermined in the first 300 C.C. which come over. In this manner theresult obtained was *231 mg. NH, per litre.From water taken between hlarseilles and China a t depths varyingfrom 1.5 to 2 metres, the following results were obtained :-mg. N I B per litre.Ismaila.. .......................................... 0-204Red Sea, long. E. 33" 5 4 , lat. N. 24" 4' .............. 0.176Cape Gardafuy, long.E. 49" 42', lat). N. 12" 44' ........ 0.176Socatora, north of the island ........................ 0.17C;Bay of Bengal, long. E. 87" 55', lat. N. 5" 34'. ......... 0.136Coast of Cochin China, long. E. 107" 22', lat. N. 14" 37'.. 0.340From these results it is seen that ammonia occurs in seas of alllatitudes.The quantity of ammonia in the sea-water does not increase pro-portionally to the evaporation of the water, inasmuch as a portion ofthe ammonia escapes into the air.The Ammonia in the Deposits from Sen-water.-During the evapora -tion of the water in saline marshes, deposits are formed, the first con-sisting of pure cryatallised gypsum covering the surface of the pan,Moist air also slowly oxidises nitrous acid.L. T.0's10 ABSTRACTS OF CHEMICAL PAPERS.whilst the second is a black mud, obtained partly by the decompositionof the “ feutre,” the term applied to the “ stratum” of algae whichcovers the bottom of the salt-pans. There is also a greenish-yellowliquid obtained, which contains some of the refuse of the mud and alarge quantity of gxpsum.Each of these contained ammonia in the following proportions :-Gypsum ........ 1.6 mg. NH, per kilo.Liquid.. ........ 3.4 ,, per litre.The water of the pool of Lavaldue contains 250 times more ammoniathan the water of the Seine a t Paris, and 50 times more than that ofthe Bievre, on the banks of which many manufactories stand.By the evaporation of the sea-water, deposits are obtained; in the firstplace calcium carbonate, mixed with oxide of iron and strontium car-bonate, separates out, but the more important deposits are those ofgypsum, which are two-( 1) pure gypsum, and (2 j gypsum mixed withcalcium carbonate and some mud, imparting to it a grey colour.Thereis also a deposit of mud. These last three absorb ammonia, which fheauthor has determined in twenty samples obtained from different placesto the south of France. The results, of which the following areexamples, show the variation in the quantity of ammonia :-Black mud ...... 8.3 ,, 7 9Pure gypsum. Grey gypsum.Triassic. “g. mg.Simiane (Bouches du Rhone) . . 1.2 6.2Saint Julien . . . . . . . . . . . . . . . 1.6 2.6Castellane .................. 2.4 3%La Palud ..................0.8 3.1Taulanne.. .................. 1.4 3.0Solli&s (Ville) .............. 1.9 3.1Le Beausset ................ 3.2 4.3Le Faron (Toulon) .......... 1.8 4.8Bandol ...................... 2.2 4.6Black mud.mg.15.012.214.011.212.714.011.112.914-5The author has also examined some gypsum beds of the tertiaryformation for ammonia, arid finds that they correspond with the greygypsum above, having given the following resalts :-Bois d’dsson ............Saint Jean de Garquier . . 2.14 ,, 7,4.04 mg. NH, per kilo.Camoins ................ 2.87 ,, ? >The presence of ammoniacal salts in the gypsum accounts for thedisengagement of ammonia in the manufacture of plaster of Paris.The boric acid emitted by the lagoons in Tuscany is often accom-panied by ammonia, which may be explained if it is admitted thatthe boric acid exists in the saline beds of the lagoon, which absorbammonia, and that the part played by the volcauic agent is purelymechanical, whereas on the contrary, by assuming the boric acid tohave a volcanic origin, the presence of ammonia cannot be explained.The water of Lake d’Enghien contains only 0.07 mg.NH, per litre,whilst the sulphur spring fed by the lake contains 5.06 mg. per litre1NORGlANJ.C CHEMISTRY. 11This is due to the fact that the water on emerging from the lake hasto pass over sediments, from which it dissolves the ammoniacal salts.The author is of opinion that all saline waters obtain theirmineral matter from the two salt-bearing formations, the trias andtertiary, which always contain a consid2rable quantity of ammoniacalsalts, and the conclusion he draws is that all saline mineral watersought to contain abnormal quantities of ammoniacal salts, whetherthey be sulphurous or not, thermal or not.L. T. 0's.Chemical Action of Water and Saline Solutions on Zinc.By A. J. C. SNYDERS (Deut. Chem. Ges. Ber., 11, 936--949).-Theauthor has examined the action of water and of saline liquids on zincunder various conditions.1. Zinc decomposes saline solutions, whether concentrated ordilute, without access of oxygen, evolving hydrogen and forming zincoxide.2. Solubility of zinc oxide in the saline liquids promotes theaction.3. Zinc oxide dissolves in solutions containing 1 per cent.or less ofsalt. The solubility varies with different salts, being greatest withammonium salts. Zinc hydrate and carbonate are insoluble in carbo-nates. The solubility of zinc oxide increases with the strength of thesolutions and with the temperature.4. When a saline liquid is saturated with zinc oxide, the decom-posing action still goes on, the oxide then formed remaining undis-solved.5. In presence of oxygen free from carbon dioxide, the zinc oxidedissolves more readily, on account of the direct oxidation of themetal.6. In presence of the carbon dioxide of the air, the solvent actionis to some extent prevented, owing to the formation of basic car-bonate.7. The solvent action is strongest with chlorides and potassiumsulphate, weaker with alkaline and barium nitrates and magnesiumsulphate.8. Solutions of alkaline carbonates and sodium phosphate do not acton zinc protected from the air.Even in presence of oxygen, solutionscontaining 1 per cent. of these salts dissolve but little zinc, becausethe carbonate or phosphate first formed protects the metal fromfurther action. Nevertheless, traces of zinc oxide are dissolved by stillweaker solutions.9. The solrent action is greater at higher temperatures : a t 0" it isvery slight.10. Solutions of ammonium salts take up more zinc oxide thansolutions of salts of fixed alkalis. The surface of the metal remainsclean, and nothing is deposited from the solution, even in presence ofoxygen.11. Hard waters do not act on zinc, even when rich in chloridesand sulphates.Soft waters dissolve the more zinc the greater thepreponderance of chlorides, sulphates, and ni hates over carbonatesand phosphates contained in them.His results are summed up as follows :J. R12 ABSTRACTS OF CHEMICAL PAPERS.A New Earth of the Cerium Group, and on the Analysis ofNatural Niobates. By J. L. S i I I ' r H (Con@. reud., 87, 146-148).-The object of this paper is to call attention to the use the authormade of concentrated hydrofluoric acid for decomposing niobates ; itsaction on samarskite and euxenite being as energetic as that of hydro-chloric acid on calcium carbonate. By the actiori of the acid, all themetallic acid forming oxides, together with the oxides of iron and man-ganese, are dissolved, whilst the insoluble portion contains all the earthsand the uranium oxide.The presence of tantalates renders thedecomposition more difficult. I n a former memoir, the author dividedthe earths contained in Carolina samarskite into the yttrium andcerium groups, pointing out however that the latter group might notcontain cerium oxide, and that thorium could not be detected i n itx i t h certainty. Since this, he has found that the yttrium group con-tains about two-thirds of yttrium and one-third of erbium, whilstcerium is absent from the group bearing its name. He also points outthat the earths of this group contain 10 per cent. of thorium, a smallquantity of didymium oxide and an earth (about 3 per cent. of themineral) which the author considers to be new, if i t is not the hypo-thetical terbium of Mosander.De la Fontaine of Chicago has con-firmed the absence of cerium, and looks upon the new earth as terbia.The author thinks, nevertheless, that he has found a new earth, andthat if terbia exists among the oxides of samarskite, it is containedin the yttria group.Comparing the atomic weight of the supposed new earth with thoseof the oxides of cerium, lanthanum, or didymium determined byJIarignac (0 = 16) we have :-New earth.. ................ 109 (Smith).Cerium oxide .............. 110 (Marignac).Lanthanum oxide., .......... 110 ,,Didymium ,, ............ 112 ,,The new earth differs from those of the j t t h gronp in its actionwith potassic sulphate, from cerium oxide by its solubility in verydilute HN03, from didymium oxide by its colour, from lanthanumoxide by its colour and the ease with which its salts are decomposed byheat.The author has aIso devised a method for the separation of thorium,as follows : the freshly precipitated oxides are placed in a solution ofpotash or soda, and a current of chlorine is passed through the mixturewhen all the oxides are dissolved except those of cerium and thorium ;as the samarskite contaius no cerium, the residue consists merely ofa white gelatinous precipitate of thorium oxide.J. $1. T.The supposed New Element Mosandrum. By J. L. SMiTH(Conipt. r e d . , 87, 148--131).-This paper is occupied by a claimfor the priority of the discovery of the earth indicated as X by Soretin his paper to the Academy.The author maintains to have foundthis earth in samarskite from North Carolina, and gives a minuteaccount cf its discovery and of his correspondence with De la FontainIX'ORGAK'IC CHEMISTRY. 13and Marignac on the subject. Basing his remarks on his own workand tdie spectroscopic examination by Soret, he now has no hesitationi n claiming mosandruin as a new element.On the Discovery of a New Earth announced by J. L.Smith. By C. MARIGSX (Co?72pt. reid., 87, 281-5283 ).-In thispaper Marignac points out the reasons leading him to the conclu-sion that Smith's " mosandrum " is identical with Mosander's " ter-bium ; " whilst the earth provisionally designated X by Soret and theauthor, differs from t,htl former in its absorption phenomena, althougliit shows nirt11~- points of resemblance with an earth described by De laFontaine of Chicago.J.AT. T.J. M. T.Magnetic Compound; having the Formula RO.Fe,O,. ByK. Llsr (Delcf. Clmn. Ges. Be,.., 11, 1512-1.516j.-Lime water pro-duces in a neutral solution of ferric chloride a brown precipitate,which is magnetic, and after ignition has the composition Cs0.Fe207.I n a similar manner magnetic compounds of magnesia and bnrytawith ferric oxide can be obtained. The corresponding manganese,nickel, copper, and lead compouuds are formed when soda is added toa solution containing ferric chloride and copper sulphatc, &c., in theirequivalent proportions. Magretic compounds are also formed whensodium or potassium carbonate is fused with ferric oxide. w. c. w.Dissociation of Metallic Sulphides. By P. DE CLERMOSTand J. PROMJI EL (Co??2pt. re72d., 87, 330, 332 j .-The decomposi-tion which ensnes on boiling certain sulpliides with water is regardedby the authors as due to the dissociation of a previously formedhydrate of the sulphide. They point out that freshly precipitatedsulphide of arsenic boiled with water gives rise to a more rapid evolu-tion of sulphuretted hydrogen than tlie same sulphide does when ithas previously been dried at 12.5". But if this last is kept in coutactfor some hours with hot water in a closed vessel, i t gives off sulphurettedhydrogen, when boiled in an opcn vessel, as rapidly a s the freshlyprecipitated sulphide. On boiling snlpliides with water in a vacuum,dissociation was observed to occur a t tlie following temperatures :sulphide of arsenic, 22' ; sulphide of iron, 56" ; sulphide of antimony,95". The dissociation of arsenic sulpliide presented ccrtain pecn-liarities, which the authors believe to be due to the interference of thearsenious acid, which is one of the products of decomposition. Thepresence of this substance impedes the dissociation, by the formation,as they suppose, of an oxpsulphide which undergoes dissociation moreSulphide of arsenic, to which crystallised arsenious acid has beenadded, is dissociated more quickly than that to which arsenious acidobtained by the dissociation of tlie sulpliide has been added. Asarsenic pentasulphide on dissociation yields arsenious acid and notarsenic acid, the author doubts its existence as a definite chemicalcompound. R. R.slowly

ISSN:0368-1769    

DOI:10.1039/CA8793600008

出版商:RSC    

年代:1879

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14 ABSTRACTS OF CHEMICAL PAPERS.M i n e r a1 o g i c a1 C h e m i s t r y.The Fundamental Forms of Crystal Species. By A. KEKY-GOTT (J07u-b. f. A&-, 1878, 337-349).-1t is of course an acknow-ledged rule, that in “ derivation-forms ” the axial relations of theprimary or fundamental forms are modified by means of “ derivation-coefficients,” expressed as rational numbers. This assumption thatthe “ derivation-coefficients are rational nuubers,” is open to a ques-tion, viz. : “ Is i t mathematically true that these coefficients arerational numbers ? ” C. F. Naumann, in his Lehrbuch (7e.1. ~civen zmdaugezvnndten K~ystctllogrupirie, Band I, says, “ a very remarkable butthoroughly confirmed natural law for the derivation of forms is thatthe ‘ derivation-coefficients ’ are always rational numbers.This fun-damental law must be considered as the result of all methods ofderivation.” The results of measurements of angles certainly alwayslead to rational numbers, but the above-mentioned law cannot be saidto rest upon a proved mathematical basis. A second question may beasked, viz. : “ Are the numbers expressing the lengths of the axes ofthe fiindamental forms rational or irrational ones ? ” The author con-siders that they are irrational numbers (the numbers in the regularsystem belong neither to the rational or irrational, because the axialrelations of the octohedron are expressed t,hus: 1 : 1 : 1, or by t h eformula a : a .- a, thus merely showing that t’he axes are of equallength). I n the quadratic and rhombic systems, however, the numberswhich express the axial ratios of the primary pyramids must beirrational, for this reason, viz., if the “ derivation-coefficients ” areassumed to be rational numbers, the resulting axial ratios obtainedexpressed in rational numbers, lead inevitably to the derivation of theregular octohedron from a quadratic or rhombic pyramid.A thirdquestion may be asked, viz. : “ Is the choice of a primary form alimited one, or in other Fords, do the values expressing the lengthsof the axes of non-regular primary forms lie between certain limits ? ”The choice of a primary form in all the systems except the regularsystem, is optional, falling either upon one of the forms actually 011-served, or upon one obtained by calculation from the observed forms.It is often observed that a different primary form (in the samemineral species) is chosen by different observers, and also that theaxial lengths obtained by calculation do not agree.The latter circum-stance is due, in most instances, to the varying qualities of thegoniometers used, and occasionally also to physical defects or abnor-malities on the crystals themselves. I n order to diminish the errorsarising from such differing observations, the author sugqests thatcrystallograpers should give the angles obtained by measurement orcalculation of the primary form, and the resulting axial lengkhs of theprimary forms, giving a t the same time similar observations of othercrystallographers for comparison; just as it is the rule to give theanalyses of a substance by different chemists side by side. Naumann,in his Leluhuch (already referred to), says for example in regard tothe quadratic system, that every form whose parameters have thMISERALOGICAL CHEitIISTRT.15finite relationship cc : 1 : 1, can be chosen as a geometrical primaryform ; but as normal quadratic pyramids can alone be said to fulfilthese conditions, they must therefore be chosen as primary forms. Apyramid P (of undetermined dimensions, with the parameter of thevertical axis standing to the parameter of a lateral axis in the rela-tionship of " a : 1 ") is chosen as the primary form. Opinions aredivided as to whether this relationship is a rational or irrational one ;Hauy, Weiss, and Mohs expressing " a " as a square root, whilstHreithaupt has endeavoured to show that this number is rational, andis always a multiple of the coefficient TQc, the other lateral axis, or theintermediate axis being taken as unity.It is, however, immaterial forthe independence of the quadratic sjstem whether the one or the otherof these opinions is the correct one, as the distinctive feature of thequadratic system is the contrast exhibited by one axis in regard to theother two axes, thus making a passage of quadratic forms into regular(tesseral) forms impossible.This opinion of Naumnnn is a t variance with that of the author, whohas already stated above that the numbers cannot be rational ones, asthe " derivation-coefficients " would in that case lead to the produc-tion of a regular octohedron, and not of it normal quadratic pyramid.As a proof of this opinion, the author points out that the axial rela-tion n : 1 : 1 cannot be chosen in the derivation of the primary form ofn " species," because the regular octohedron would probably occur inthe series of normal pyramids obtained, and would with equal justicebe chosen as the primary pyramid.It is impossible for a quadratic species to exhibit the axial relationa* : b2 = 2 : 1, as the faces of the primary pFramid P would intersectin a terminal edge a t an angle of 101" 32' 13", and in a lateral edge atan angle of 126" 52' 12", consequently the pyramid Px, would haveequal lateral and terminal edge angles, and be a regular octohedron.In regard to the hexagonal system, i t is evident, from its close simi-larity to the quadratic system, that the parameters of the lateral axesmust differ in length from that of the vertical axis, although as Nau-mann states in his Lehdmch, i t is theoretically possible to have nprimary hexagonal pyramid in which all the axes are of equal length.The author agrees with Naumann in considering such a form to be;L purely theoretical one, because the close analogy existing betweenthe quadratic and hexagonal systems in the characteristics of theirforms, the laws relating to their hemihedry and tetartohedry andtheir physical properties, point to a similarity in their axial relations;whence i t is safe to conclude that the length of the vertical axis of ahexagonal pyramid must differ from the lengths of its lateral axes.As;t proof of this opinion, the author gives the folIoaing examples, viz. :" a normal hexagonal pyramid with the axial relation a : b = 1 : 1,mould have an interfacial angle over a terminal edge of 135" 35' 5",;ind over a lateral edge of 98" 12' 48" ; the Corresponding ho???bohedmtwould have a terminal edge angle of 98" 12' 48", and the correspond-ing trigonuZ pyramid would have equal terminal and lateral edgeangles, vis. : 98" 12' 48". The di(fgonaZ pyramid corresponding withthis normal pyramid would have a terminal edge angle of 138" 35' 25",and a lateral edge angle of go", and the corresponding dingonaZ rhom16 ABSTRACTS OF CHEMICAL PAPERS.bohedroit would have a terminal edge angle of 104" 28' 39".Besidesthe above improbable axial relation (which would include every pos-sible rational angle-relation obtained through rational " derivationcoefficients"), the two axial relations a' : b2 = 3 : 2 and 2 : 1 are im-possible, as will readily be seen from the following, viz. : " the axialrelation a2 : b2 = 3 : 2 furnishes a normal hexagonal pyramid, havinga terminal edge angle of 131° 48' 3G", and a lateral edge angle of109" 28' 16" ; the corresponding rhombohedron is the cube, and thecorresponding normal trigonal pyramid has a terminal edge angleof 90" and a lateral edge angle of 109" 43' 16", whilst finally thediagonal hexagonal pyramid of the normal pyramid has a terminaledge angle of 134" 25' 37", and a lateral edge angle of 101" 32' 13",and the diagonal rhombohedron derived from the last-mentioned formhas a terminal edge angle of 55" 4 4 21".The axial relation a2 : 6?= 2 : 1 is equally impossible, as i t also leads to the cube as a hexagonalfoi-m. From the above, therefore, it appears that a quadratic pyramidcannot exist having the same interfacial angle on a terminal edge ason a lateral edge, because it would in that case be a regular octohe-dron ; and further, a rliombohedron cannot have the same angle on aterminal edge as on a lateral edge, because i t would then be a cube.The author also considers it impossible for a normal hexagoiial pyra-mid to have equal termirial and lateral edge angles. A normal hexa-gonal pjramid having the interfacial angle 126" 52' 12" on a terminaland lateral edge, requires the axial relation a2 : b2 = 3 : 1 ; its rhom-bohedron would have a terminal edgc angle of 78" 27' 47", its trigonalpyramid the terminal edge angle 78" 27' 47", and lateral edge angle126" 52' 12".The relative diagonal pyramid would have a terminaledge angle of 128" 40' 56", a lateral edge angle of 120°, and its rhombo-hedron (diagonal) would have a terminal edge angle of 8P 49' 9". Adiagonal hexagonal pyramid haring the same interfacial angle on itsterminal and lateral edges, viz., 126" 52' 12", and whose diagonalrhombohedron has a terminal edge angle of 78" 27' 47", requires theaxial relation a2 : b2 = 4 : 1, or n : 21 = 2 : 1. The relative normalliesagonal pxramid would have a terminal edge angle of 125" 22' 36",a11d a lateral edge angle of 133" 10' 25", its rhombohedron a terminaledge angle of 74" 44' 33", and its trigonal pyramid a terminal edgeangle of 74' 44' 33", and EL lateral edge angle of 133" 10' 25".Theaxial relation CL : I, = 2 : 1 would give the relative normal pyramid asa " derivation form " of the pyramid with the axial rclation a : b =1 : 1. If the latter form is found to be inadmissible, it follows thatits '' deiaivation forms " must also be inadniissible, and to this cate-gory belongs the pyramid 2P2, which has equal terminal and 1ater:Lledge angles. The axial relation 2 : I,2 = G : 1, is also inadmissible, aswill be seen from the following, viz. : the corresponding normal hexa-goiial pyramid would have a terminal edge angle of 123" 44' 56", anda lateral edge angle of 141" 3' 27", its I*homl)ohedron would have aterminal edge angle of 70" 31' 44", and this form combined with CtRin a pioper proportion would become a regular octohedron.Thetrigorla1 pyramid corresponding with the above-mentioned normalhexagonal pyramid would also be a regular octohedron. Fromthediagonal pyr'tmid corresponding with the above-mentioned norma3IINERALOGICAL CHEMISTRY. 17pymrnid, a diagonal rhombohedron is obiairled, which in reality is acubc. I t seems, therefore, from what has already been stated, thatallowing primary forms to have rational ’‘ derivation coefficients ”and irrational axial lengths, it still does not follow that any kind ofirrational axial relation will furnish a primary form, because certainforms mentioned above are excluded.The author concludes by statingt,hat the values of the axial relations of the possible primary formsmust oscillate between certain limits. C. A. B.Hetaerolite. A New Mineral. By G. MOORE (Jalirb. f. illin.,1878, 210--211).-This mineral occurs in botryoi’dal radio-fibrousmasses, always accompanying (dmipo?) chalkophanite in brown-ironochre, a t the Passaie zinc-mine, Sterling Hill, N. Jersey. Hetseroliteis black, has a semi-metallic lustre, a brownish-bIack streak, is infusiblebefore the blowpipe, and evolves water on being heated in a closedtube. H. = 5 . Sp. gr. = 4.933. Its chemical composition correspondswith the formula ZnO.MnO.MnO,, whence it appears to be a zinc-hausmannite.The chalkophnnite is rhombohedral, and occurs indruses in thin laminae or stnlactitic aggregates. Colour bluish-black.Jliistre metallic. H. = 2. SD. pr. 3.907. I t s chemical comDositioncorresponds with the formula, !2M\02 + (MnZn)O + 2H20. AC. A. B.The Origin of some Ores of Copper. By C . A. BURGHARDT(Chem. News, 37, 215).-hmmite. - The author considers thismineral to have had in most cases an aqueous and not an igneousorigin, o w h g to the more common occurrence of globular and stalac-titic atacamite ; the crusts of atacamite in volcanic neigh bourhoods(arising from the action of hydrochloric acid gas upon copper com-pounds) being comparatively scarce and insignificant in quantity.Natural atacemite is known to occur in three statos of hydration, t}iechemical composition of each being as follows, viz.:-(1.) Afacainite jiwn Algodon Bay, Bolivia (von Bibra, Jahesb., 1855,740)-cu. c1. 0. H20.59.25 16.1 1 12.51 12.13 = 100.00,the formula corresponding with the above being Cu40,C12 + 3H20.( 2 . ) Atacamite f r o i n Copiapo, Chili (Field, Journ. Chem. S’oc. [‘LJ, 3,193)-c u . c1. 0. HZO.56.38 14-95 10.78 17.89 = 100.00.Formula = Cu,0,C14 + 9HzO or (Cu*O,Cl,), + 9H20.(3.) Botnllnb Atacccnzite ( a ) (Church, Jouru. Chem. SOC. [2], 3,212)-Cobija Atcicai?zitc ( b ) (Berthier, Ann. cles Mines. [3], 7, 542)-c u . c1. 0. H,O.(a.) 52.90 14-76 10.4 9 22.4.5 = 100.00(b.) 53.26 14-92 9.37 22.24 = 100.00Formula = Cu,03C12 + 6H20.voL.xxxv~. 18 ABSTRACTS OF CHEMICAL P9PERS.Field (Phil. Mug. [4], 24, 1862, 124) prepared an apple-greenatacamite, corresponding with Berthier's atacamite from Cobija, byadding a solution of calcium hypochlorite to an excess of cupric sul-phate. The author obtained (in addition to cuprite and chalcotrichite)very small quantities of a green substance resemhling atacamite, byheating in one case cuprous chloride crrstals with water in a sealedtube a t a temperature ranging from 160-180"; in another case, byheating cuprous oxide with a strong solution of sodium chloride in itsealed tube a t a temperature ranging from 150-180". After numerousexperiments, it was found that large quantities of atacamite werereadily formed by simply covering cuprous oxide with a concentratedsolution of sodium chloride, and exposing this mixture to the air.Thecuprous oxide dissolves in the sodium chloride solution, forming avery concentrated solution of cuprous chloride, and the latter, onexposure to the air, rapidly decomposes, a green insoluble substanceseparating out. This substance was dried over calcium chloride untilits weight was constant, then analysed, and found to have the follow-i n g chemical composition-cu. c1. 0. H?O.56.25 14.29 10.95 18.51 = 100.00,from which it will be seen that it agrees closely with the Copiapoatacamite. The first stage of the above reaction niay be expressed bythe following equation, viz. :-3Cu2C12 + 0, = CuC1,.3CuO + 2CuC12,the cupric oxychloride thus formed becoming eventually hydrated.I n a former paper (Proc.Lit. Phil. Xoc. illmcl~ester~ 18, 27-36)the author expressed an opiiiion that most of the ores of copper arethe products of the decomposition of cuprous oxide ; and the resultsdetailed above seem to confirm this view, more especially as atacamiteis nearly always intimately associated with cuprite, chalcedony, quartz,&c., occurring in diorite and syenite. C. A. B.Uranium Pitchblende from Joachimsthal. By E. REICHARDT(Arch. Pharnz. [ 3 ] , 13, 130).-The sp. gr. of this mineral is 5.328 ; thecolour brown-black with an ochrey coating; its composition is asfollows :-Si. S. A1,03. Fe,OR. CaO. MgO. MnO. Pb.3.680 0.788 0.313 4.161 0.499 0,034 0.180 3.8880.261 0.068 0.072 0.578 83.918 trace = 98.440Polydymite.By A. KENNGOTT (Jnhrb. f. &fin., 1878, 183-185).-Laspeyres described this new mineral ( J r h b . f. X n . , 1877,206), stating its composition to be as follows, viz. :-As. Sb. p205. CUO. u203. Bi.E. w. P.Ni. CO. Fe. S. As. Sb.53.508 0.606 3.844 40.270 1.041 0,508 = 99.777,the formula corresponding with this analysis being NiS.Ki,S,, thusplacing the mineral in the same class as musenite, which containMISERALOGICrVI CHEMISTRY. 19both Ni and Co. The small amount of arsenic and antimony presentpoints to a slight intermixture of gersdorffite and ullmannite with thepolydymite. Further, Laspeyres was of opinion that the nickel-bismuth-glance (snynite, eriinauite) analysed by von Kobell, was amixture of polydymite with bismuthine, galena, and chalcopyrites(copper-pyrites), and this opinion is considered by Kenngott to bewell founded, as he obtained the formnla NiS.Ni& on deducting theseveral percentages of bisniuthine, galena, and chalcopyrites obtainedby calculation from von Kobell's analysis.Yellow Dolomite from Bleiberg.Ry V. TON ZEPHAROVICH(Juhrb. f. Ifin., 1878, 315).-This dolomite occurs fine-grained andmassive, with a sulphur-yellow to brownish-yellow colour, and oftenenclosing yellowish- brown zinc-blende. The yellow colour of the dolo-mite is most, intense in the neighbourhood of the enclosed zinc-blende,Small drusy cavities occur in the dolomite containing zinc-blende,which are filled with hemimorphite crystals, accompanied by yellowish-white calcke rhomhohedrons.A microscopical examination showedthe doloniite to be homogeneous (excluding of course the zinc-blendeenclosures). Sp.. cr. = 2.87. An analysis showed it to have thefollowing composltlon, viz. :-C. A. B.CaCO3. MgC03. ZnC03. FeC03. ZnS. CdS. FeS2. SiOP79-48 16.71 2.4'2 0-30 0-31 0.25 0.08 0.03 = 99.58.The formula correspondirig nearly with the above is 4CaC03 +MgCO,. The yellow colour is due to the presence of cadmiumsulphide. C. A. B.A Boron Mineral from Chili. By E. RErCHARDT (Arch.Plmrrn. [ 3 ] , 13, 131).--In the Chili saltpetre beds, together withcalcium borate and boronatrocalcite, a mineral is found in powderhaving the composition-Water ....................Silica. .....................Ferric oxide and alumina ....Lime ......................Sodium chloride ............Potassium chloride ..........Sodium biborate ............Sand and clay ..............Magnesium chloride ........Calcium sulphate............18.10715.0560.0 700-8400.7271.1093.7631.31032.24726.611-I99.840E. W. P.Deposits of Calcium Phosphate in the Vosges. BY P. GUYOT(Cornpt. rend., 87, 333). At Damblain and Blevaincourt, in theVosges, are found kidney-shaped masses of calcium phosphate from2 to 10 centimeters in dimeter. A sample from Damblain yielded76-99 per cent. of tribasic phosphate ; one from Blevaincourt 77.74 percent . R. R.c 20 ABSTRACTS OF CHEMICAL PAPERS.New Minerals from Fairfield Co., Connecticut. By G. J.BRUSH and E. S. DANA. First Paper (Amer.Jour. Sci. [ 3 ] , 16, 39-46).-These minerals were found in a vein of albitic granite, asso-ciated with a large number of others ; six new species were identified.Those described in the following paper occur associated in the mostintimate manner, although distinct crj-stals can be obtained.Eosphorite occurs in prismatic crystals, often of considerable size,more generally massive. Hardness = 5. .Sp. gr. (mean) = 3.134.Lustre vitreous to subresinous; of the massive mineral often greasy.Colour of the crystals pink, yellow, and grey ; of the massive mineralpale pink, greyish, bluish-, and yellowish-white and white, some-times greenish, owing to admixture of dickinsonite. Transparentto translucent. Streak nearly white. Fracture uneven to sub-conchoidal.The crystals are prismatic in habit, showing but one terminatedextremity, and belong to the orthorhombic system.The surfaces ofthe crystals are often covered with drusy quartz and with apatite ;the prismatic planes almost always, and the pyramidal planes veryoften, are finely striated, giving rise to rounded barrel-shaped crptals.The crystals are c_losely analogo_us to those of, childrenite. Observedplanes: m p m , mPm, mP, mP2, P, +@+, 2P2. Axial ratio, a': 8 : c(vert.) = 1 : 1.28732 : 0.66299. Angle, P : P (in the terminal edges)= 61" 1' 54' ; P : P (in the basal edges) = $6" 27' 45"; mP : COP= 75" 36'; ~ogijoo : mP = 52" 12' : m P : P = 49" 55'.The three axes of elasticity coincide with bhe crystalline axes ; theoptical axes lie in the macrodiagonal section or plane of cleavage.The axial angle is (approximately) 2E = 54" 30' (for red rays) andUlo 3cl' (blue rays).The dispersion of the axes is strong v>p ; thecharacter of the double refraction is negative. A parallelopiped, cutwith its edges parallel to the three crystalline axes, showed a distincttrichroism. The mean composition is as follows :-P,O,. A1,03. FeO. MnO. CnO. Na,O. H,O.31.05 22-19 7.40 23.51 0.54 0.33 15.60 = 100.62,corresponding with the formula ~A12P201,.4H20, or AI,P,O, + 2H,R02 + 2Aq. Eosphorite differs from childrenite in containiiig a largerproportion of manganese and a smaller proportion of iron. It is essen-tially a phosphate of aluminium and manganese, childrenite being ;tphosphate of aluminium and iron.In a closed tube eosphorite decrepitates, whitens, gives off water,and turns black, grey, and then brown with metallic lustre, andbecomes magnetic.Before the blowpipe, it cracks open, colours theflame pale green, and fuses to a black magnetic mass. It dissolvescompletely in the ordinary fluxes, giving iron and manganese reac-tions.TripZoidite.-This mineral occurs in crystalline aggregates, whichare parallel-fibrous to columnar or divergent, sometimes confusedlyfibrous to nearly massive. Occasionally distinct crystals are foundimbedded in quartz, from which they cannot be separated withoutbreaking into small pieces ; rarely crystals may be found projectinginto cavities in the massive mineral.It is soluble in hydrochloric and nitric acidsMISERALOGICAL CHEJIISTRY.2 1The hardness of triploidite is 4.5-5" ; sp. gr. 3.697. Lustre vitreousto greasy-adamantine ; colour yellowish- to reddish-brown ; crystalstopnz- to wine-yellow and sometinies hyacinth-red. Streak nearlywhite ; transparent to translucent ; fracture sub-conchoidal.The crystals belong to the monoclinic system and are homeomor-phous with wagnerite ; they are much striated and occasionally exhibitfalse planes. Of the two axes of elasticity which lie in the plane ofsymmetry, one nearly coincides with the vertical axis, the other isalmost normal to the orthopinacold. The mean chemical compositionis as follows:-P.,Oj. FeO. MnO. CsO. H20.32-11 14.88 48.45 0.33 4.08 = 99.85,leading to the formula R4P209.H20, or R,P,O,.H,RO,, where R =Mil : Fe = 3 : 1.Triploidite is therefore related in composition tolibethenite, olivenite, and lazulite, none of which, however, havesimilar crystalline forms. I n crystalline form it resembles wagnerite,which again is analogous to triplite in composition, thus showing arelation between triplite and triploidite. Observed planes : OP,aSm, mFm, CCP, Pm, 242. Axial ratio, u : b : c (vert.) =1 : 0.33846 : 0.80367. Angle, UP : mP m = 54° 48'; ocf 00 : cmP= 60° 27'; mPm : OP = 71" 46'; OOP: XP = 59" 6'; mP00 : OP= r l d5'.In a closed tube, triploidite gives off water, turns black, andbecomes magnetic. Fuses quietly in the naked flame, and before theblowpipe in the forceps colours the flame green.Dissolves in thefluxes, giving reactions for manganese and iron. Soluble in acids. c. w. w.c o tThe daikest specimens contain the most iron.Thaumasite, a new Mineral Species. By NORDENSKIOLD(Compt. r e d . , 87, 313).-This substance, obtained from a mine atAreskustan, has been analysed under the aut,hor's direction, withresults leadiiig to the formula CaSi03.CaS04.CaC03 + 7H20.R. R.Some Minerals from Laangban. By A. E. NORI)ENSKI~LD(Jahrb. f. N i i z . , 1878, 206--209).--Atopite T TO TO^ = unusual), a newmineral, c:rystallises in predominating regular octohedrons, in combi-nation with the cube and rhombic dodecahedron and indications ofthe trapezohedron and tetrakis- hexahedron. Yellowish- brown to resin-brown, resinous lustre, semi-transparent.Sp. gr.= 5.03. On heating it in the oxidising flame before the blowpipe,no change is observable ; i t gives a deposit on charcoal and leaves aninfusible slag-like residue after the volatilisation of all the antimony ;gives a faint trace of Mn on treating i t with carbonate of soda andnitrate of potassium. Soluble in microcosmic salt without separationof silica, the bead being yellow when hot and colourless when cold ;insoluble in acids.H. = 5.6 to 6.Chemical composition as follows, viz. :-Sb,O,. CaO. FeO. MnO. K,O. Na20.72-61 l i . 8 5 2.79 1-53 0.86 4-40 = 100.0422 ABSTRACTS OF CHEMICAL PAPERS.Formula 2R0.Sb20,. From the above i t would seem that atopiteresembles very closely nionimolite and romei te, differing howeverfrom the former in the absence of lead and a higher amount ofantimonic oxide, and from the latter in a double amount of bases, thecrystal form, and the different state of oxidation of the antimony pre-sent. Atopite occurs mostly disseminated in very fine veins anddeposits of hedyphane, which penetrates rhodonite.M o n imolite isfound a t Laangban in brown crystals and grains in calcite-drusesenclosed in rhodonite and tephroide.A'kdemite (cKErjpoS = absent, foreign), a new mineral, coarse-crys-talline, foliated, monoaxial, with a distinct basal cleavage. Lightyellow with a greenish tinge, translucent in thin splinters, resinouslustre on broken surfaces, on cleavage-planes a strong vitreous lustre.H. = 2.5-3. Sp. gr. 7.14. Brittle. Decrepitates in a closed tubeand crumbles to powder, a yellow fused mass separating out witah ease,and a t the same t'ime a sublimate of lead chloride.Heated on char-coal it furnishes a lead-bead and a deposit of lead oxide and chloride.Arsenic is also present. Soluble in nitric acid and warm hydro-chloric acid. An analysis of this mineral proved it to have the follow-ing composition, viz, :-PbO. Pb. C1. A S , ~ ~ .58.25 23.39 8.03 10.60 = 100.24.The formula corresponding with the chemical composition is 5Pb0As203,2PbC1,.HZl~~ocsrussite.-Hydrated carbonate of lead surrounding nativelead. White by transmitted light ; colourless, quadratic lamine,having a very distinct foliation. Decrepitates in the closed tubeand becomes yellowish-brown. Yields a lead-bead on charcoal.Solublein acids with eflorescence. Rather soft, The author considers itscomposition to correspond with the formula 2PbOC02,H20.Hyalotekite (3uXos = glass, and ~ ~ X E L V = melt, fuse).-A newmineral. Occurs in coarse crystalline masses, exhibiting two direc-tions of foliation which intersect each other at an angle of about !)O".H. = 5 to 5.5. Sp. gr. = 3.81. Vitreous to resinous lustre; whiteto pearl-grc7 ; semi-translucent ; brittle ; fuses easily before the blow-pipe to a clear colourless bead, which becomes black on heating it inthe reducing flame owiiig to the reduction of lead. Gives the reactionfor silica with microcosmic salt, and a lead-bead on reducing a por-tion of the mineral with sodium carbonate, also a yellow deposit whenheated aIone on charcoal.Insoluble in hydrochloric and sulphuricacids. An incomplete analysis furnished the following results, viz. : -Si02. PbO. BaO. CaO. Loss on ignition Al,03, K,O, &c.39-62 25-30 20.66 7.00 0.82HIyalotekit(e is accompanied by hedyphane and schefferite, and gener-ally resembles a greyish-white Pelspar.Occurs massive,accompanied by tephroite, which it cIosely resembles; in fact, it isoften necessary to resort to the blowpipe in order to distinguishGunonzolite (+m~pua = lustre) .-A new mineralBIISERALOGTCAL CHEMISTRY. 23between them. Cleavage indistinct. Strongly double refracting,colourless, whit'e t o greyish-white, strong resinous lustre, translucent.H. = 4. Sp. gr. 4.98. Fuses before the blowpipe to a clear bead,which become black on the surface in the reducing flame. Givesa lead-bead and a yellow deposit.Easily soluble in nitric acid, withseparation of gelatinous silica. An analysis gave the following results,viz. :-Si02. PbO. MnO. CaO. MgO. Alkalis and loss.34.55 34.89 20-01 489 3.68 1.86.Jacobsite.-This mineral which is st~ongly magnetic, has the fol-lowing chemical composition, via. :-Fe203. Mn203. MnO. MgO. CaO. PZO,. Pb. residue.58.39 6.96 29.93 1-68 0.40 0.06 1.22 2.17 = 100.81.InsolubleThe formula corresponding with the above is MnO(Fez03Mnz03).C. A. B.Magnetite from Monte Mulatto, South Tyrol. By V. VONZEPHAROVICH (Jahrb. f. Min., 1878, 310).-The crystals clothe drusyhollows in a tier-like mass of magnetite.Their size is sometimes 5 to8 mm. They exhibit the combination 000.50$. 303.0. Similar formswere observed by %-on Kokscharow, occurring on the magnetite ofAchmatowsk, and by Struve on the Albanese magnetite.C. A. B.The Mirabilite from Aussee. By V. vox ZEPHAROVICH(Jahrb. f. Nh., 1878, 314).-Some crystals of mnirabilite from the saltmines of Aussee exhibited the following forms in combination, viz. :-- i P , - 2 P ; the latter two forms being new to this mineral. Theorthopinacold generalIy predominates, whilst the faces of the clino-diagonal zone occur only in a secondary position. Most of the crystals(particularly the largest) exhibit an unusual " habit," on account of anabnormal vertical development, their height varying from 7 t o 10 cm.,and their width from 3 to 24 cm., and they are generally terminatedby OP or pyramids. Short tabular crystals through a r m are com-paratively rare.C. A. B.The Sericite Rocks of the Taunus. By A. WICHMANN (Jahd.f. Min., 1878, 264--275).-The author shows plainly that the con-clusions of K. A. Lossen (Zeits. Dezk G'eol. Ges., 1867, 1877) are erro-neous. Judging from the presence of a certain percentage of soda inthe Taunus rocks, Lossen endeavours to prove albite as a constituent ;but a microscopical examination of these rocks proved the absence ofunsymmetrical felspar. Albite is observed to occur on11 in bands orstreaks, but never as a rock-constituent, and the percentage of soda isrefcrable to a sodium-aluminium silicate, which constitutes the ground-mass of the slatey-rocks of the Taunus.Examination of Lithia-Mica from Paris (Maine), Rozena,and Zinnwald.By F. BERwEEtTH (Jahrb. .f. Mn., 1878, 316).-UP, mrm, mEm, -+l?Cr,+Pm,3?m, zm, 2.E?o@, mP, -P, P, +,P,C. A. B24 ABSTRACTS OF CHEMICAL PAPERS.The author analysed the lithia-mica from the above localities, takingperfectly pure material furnished by Tschermak for the purpose.A. Lithia-mica, from Paris (Maine) ; B. Ditto from Rozena ; C. Dittofrom Zinnwald.PpO,. F1. Si02. A1203. Fe03. FeO. MnO. I<@.A . . . . -- * 5.15 50.39 28-19 - - trace 12.34B . . . . 0.05 7.88 50.98 27.80 - 0.95 trace 10.78C . . . . 6.08 7.94 45.87 22-50 0.66 l l * G l 1.75 10.46Less oxygenNa,O. Li20. H,O. equivalent to fluorine.- 5.08 2.36 = 103.51 - 2.17 = 101.34- 5.88 0.96 = 104'35 - 3.32 = 101.060.42 3.28 0.91 = 10.5'48 - 3.34 = 109.14Rubidium and caesium were detected by the spectroscope.Thesp. gr. of the three lithia-micas A, B, C, were 2.8246, 2.834, and 2.9715respectively. C. A. B.The Crystal-System of Potash Mica. By M. BAUER (Jnhrb.f. illin., 1878, 310).-The author determined the angle which the planeof the axes forms with the basal plane, a,nd obtained values whichcoincide with those obtained by Tschermak. The results werc asfollows, riz. :-(1.) Potash mica is opt'ically monosymmetrical. (2.)The plane of the optical axes is perpendicular to the plane of symmetry,and the bisectrix is situated in the latter. (3.) The angle formed bythe apparent bisectrix with the basal plane = 87" 5') that formed by theupparent bisectrix with the normal to the basal plane = 2" 55', the trueangles being 88" 18' and 1" 42' respectively.Tho direction of thebisect>rix could not be determined. (4.) The angle of the apparentoptical axes is 64" 14', the angle of the true axes being 40" 21'. (5.) Theappare?Lt angle formed by the optical axes with the normal to the basalplane = 32" 14', the true angle being 20" 15'. C. A. B.Occurrence of Disthene in Central Africa. By T. LIEBISCH(Jahb. f. Min., 1878, 313-314).-Disthene is found in the mica-slateof the Baginsc Mountains, in East Niam-Niam-Land, enclosed in quartzcrystals, and accompanied by biotite and muscovite. The disthenecrystals are asparagus-green in colour. There are numerous biotitelamina3 interpolated in the disthene crystals, parallel to the face COP 63.The forms observed were COP 00, COP%, OCP', m'P, 00 P"2 ; the terminalplane was not observed.Some of the crystals were twins, accordingto the law " the twin axis the normal to the macropinacoi'd."C. A. B.Duporthite, a New Asbestiforin Mineral. By J. COLLIXS(Min. Mag., 7, 226).-This mineral occurs in fibrous masses, fillingclefts in serpentine. Greenish to brownish-grey ; silky lustre ; flexible ; heated in a matrass, it evolves water ; andtine fibres fuse before the blowpipe to R black glass. Insoluble inhydrochloric acid. An analysis furnished the following results, viz. :-H. = 2 ; sp. gr. = 2.78MINERALOGICAL CHEXISTRT. 25SiO,. A1203.FeO. MgO. CaO. Na,O. H,O. Hrgroscopic I1,O.49.21 27-26 6-20 11.14 0.39 0.49 3 90 0-68 = 99.27.Considering part of the water to be water of constitution, the formuladerived from the analysis is 3(A1,03Si0,)5( $Mg+Fe&H?)O + SiO,.The mineral approac-hes nearest to the neolite of Dana. The authornamed it from the place where it was found, viz., Dnporth, nearSt. Austell, Cornwall. C. A. B.The Stone of the “Julius Column,’’ the Lavez Zock inthe Upper Engadine, and the Sericite-gneiss in the Bun-dener Alps. By C. W. Gijmmr, ( J u l ~ b . f. Min., 1878, 296-300).-The Julius Column, which dates from the time of the Romans, isremarkable for the freshness of its colour and the total absence of anysigns of weathering. The author examined chemically and micro-scopically some small fragments which had probably been detachedfrom the column by the action of frost.The stone is rather soft,greasy to the touch, of a greenish colour, and a scaly granular strac-ture, which latter peculiarity arises from the occurrence of thin,cleavable, elastic laminae in isolated groups. There C R ~ be no doubtthat this rock is a “ potstone.” A considerable amount of the rock issoluble in hydrochloric acid, the soluble portion consisting of an impuremagnesite (containing calcium and iron carbonates), and a mag-nesium mineral which plays the part of a cement in the rock. Ananalysis gave the following resnlts :-SiOz Al,O,. Fe203. Cr203. MgO. CaO.Complete analysis . . . . . . 46.312 2.105 10.134 trace 36.161 0.251Portion soluble in lIC1 .. 25.15 2.09 14-90 ,, 44.59 -Portion insoluble in HCL 57.96 1-90 5.80 ,, 30.85 1.14Complete analysis . . . . . . 0.0.50 0.920 1.500 4.300 1.202 = 100.935Partion soluble in HC1 . . - - 3 36 7.48 2.09 = 99.66Portioninsoluble in HC1 0.67 2.21 - - - = 100.53K,O. NazO. CaCO,. MgC03. HzO.The iron was mostly present as ferrons oxide; there were alsotraces of titanic acid present. On examining the above results, itwould appear that a serpentine-like mineral inust be present in therock, as the amount of silica in the portion soluble in hjdrochloricacid is very low in comparison with the amount of magnesia. Mag-netic iron was also ascertained to be present in the powdered rock.The portion insoluble in the acid was principally talc, intermingledin varying amounts with chlorite, tremolite, and a sodium-felspar.Aslight trace of chromium also points to the presence of chromite.The microscopical examination of thin sections of the rock supportedthe conclusions drawn from the chemical analysis, as it was found toconsist of (1) fine-fibrous, green portions of varying intensity ofcolour; (2) of broad indented non-fibrous portions. Some of thefibrous portions exhibited distinct dichroism, and were probablychlorite and tremolite, whilst some small, non-fibrous, colourless por-$isms exhibited in polarised light the peculiar reddish shimmer whic26 ABSTRACTS OF CHEMICAL PAPERS.characterises the carbonates. Some colourless portions full of parallelrifts were also observed, pointing to the presence of talc.Betweenthe fibres, and often on the edges of the colonrless laminze, a powderhaving a metallic lustre was observed, which was no doubt magnetite.There were also here and there isolated, roundish-brown granules(putzen), which externally pass almost imperceptibly into the “ ground-mass ” surrounding them, but towards their interior exhibit the reti-culation characteristic of serpentine, so that it may be inferred thatthese granules were orginally olivine. On examining a thin sectionafter treatment with hydrochloric acid, it was found to contain isolatedcavities, thus pointing out the position of the carbonate portions. Ontreating a section witb caustic potash (after the hydrochloric acidtreatment), i t disintegrates into a mass of greenish needles andlamina From the above examination, the author considers the rockto be held together by a decomposible substance, such as serpentine,brucite, and a chloritic mineral.Potstone of Chinvema.-For comparison with the rock just described,sections were prepared of the Chiavenna potstone.This rock re-sembles closely that of the Julius Column, but the brown, roundishgranules are commoner, and consist on their external surface of ahomogeneous fibrous mass, whilst the central portmion consists of acloudy, dark-coloured substance, filled with a great quantity of veryfine black dust, and dark needles running in all directions.I n order to ascertain from whence the Romans obtained the stone ofthe Julius Column, the author examined some specimens closely re-sembling it, which he found in numerous quarries a t Pontresina inthe Upper Engadine.An analysis furnished the following results,viz. :-Si02. AI2O,. Fe20,. Cr203. MnO. CaO. MgO.Complete analysis ...... 35-90 0.89 11.30 0.23 trace 0.67 24.14Portion soluble in HC1 . . 28.77 trace 11-82 0.25 - trace 21.67Portioninsoluble in HCl . 54.80 1.50 7.52 trace - 2-33 50.50Potstone of Chiavenna(Delesse). ........... 36.57 - 5.85 - - 1.44 35.39K20. Ka20. FeC0,. CaCO,. MgCO,. H,O.Complete analysis. .... . U % 1.09 1.20 2.30 17.85 6.10=101.68Portion soluble in HCl . - - 1.70 3.23 25.07 8.42 = 100.91Portion insoluble in HC1 0.80 3.78 - - - - = 101.23Potstone of ChiaveniiaL----J(Delesse) ...........- - 14.03 4*97=100*00The excess in the complete analysis and the portion insoluble inhydrochloric acid is due to the iron being determined as ferric oxide,whereas it exists in the rock mostly in the ferrous state. The Pon-tresina rock contains a larger amount of carbonates than the rock ofthe Julius Column, but leaving this out, there is a very close analogybetween them, and the Chiavenna rock belongs also to the samegroup.A microscopical examination proved the identity of the rock of theJulius Column with that of Pontresina: hence it may be safelMIXERALOGlCAL CHEEBIISTR Y. 27inferred that the Romans used the latter rock for the erection of thecolumn. C. A. B.The Granite-porphyry of Beucha, near Leipzig. By E.KALKOWSKY (Jalwb. f. Niw., 1878, 276-286).--Zirkel was the firstto make the important discovery that the granite-porphyry fromBeucha contained " glass-enclosures " ( M i c r o s .Utxh. d. &fin. @ Gest.,Leipzig, 1873) .-This was afterwards confirmed by Rosenbusc'h(Micros. Plys., 1877, Bd. 11,s). Zirkel describes the granite-porphyryfrom Beucha and Altenberg thus :- " It is an aggregate of crystallin2minerals, amongst which quartz predominates over felspar. Themicroscopical quartz of the ground-mass is nearly always in sharplydefined crystals, which yield rhombic or hexagonal sections. Thesecrystals are so intimately intergrown with each other and the rec-tangular cloudy orthoclase crystals, that no microfelsitic suhstanceintervenes between them. The larger quartz-crystals are charac-terised further by numerous fine " glass-enclosures," often of a dihex-ahedral form, aud this is the more remarkable as the rock is of a crys-talline constitution throughout, and such enclosures are peculiar torocks in which a portion of the magma is amorphous.There are alsomovable liquid globules observed occasionally in the quartz, and theclear parts of the orthoclase crystals contain numerous rectangular'' glass-enclosures," the latter occurrence being extremely rare inquartz-porphyry, but common in granite. The rock contains alsoliornblende and chlorite, the latter mineral being in all probability asecondary product of the decomposition of the former.Baranowski considered the green substances of this rock to beaugite, and not hornblende ; and allowing the correctness of this COLI-clusion, the granite-porphyry of Beucha is most closely related to theaugitic felsite-porphyry of the neighbourhood of Leipzig described byKalkowsky (Zeits.Deut. Geol. Ges., 26, 1874). Augite-felsite-poi.-phyry is a coal-black to grey rock, having a true felsite porphyryhabit, with porphjritic quartz, felspar, and small black augite crystals.The dark colour is due to the great quantity of magnetic and titaniciron. Biotite constantly accompanies the augite, and apatite and iron-pyrites are accessory constituents ; the ground-mass is perfectlygranular, the grains diminishing sometimes to a scarcely recognisahlesize. The acid-rocks of this series " weather " easily, the felspar bs-coming more clouded and the augite fibrous. The granite-porphyryof Beucha (and the almost identical granitc-porphyry of the banks ofthe Mulden from Trebsen to Wurzen) is connected in a threefoldmanner with the above-mentioned aogite-felsite-porphyry, viz.:-(1 .) Its geological occurrence in the immediate neigh bourhood of theaugitc-felsite-porphyry. (2.) The granite-porphjry of Beucha ismostly of a reddish tint, owing t o the presence of reddish orthoclase,but there are also many degrees of colour observed, viz., from light-red to dark-red, violet, grey-violet, blackish-grey, greyish-black toblack. The porphyritic habit is caused by the occurrence of largered-orthoclase crystals and w bite plagioclase ; wliilst the large por-phyritic quartz-ciystals disappear entirely.On the northern perpen-dicular wall of the quarry, the greyish-black variety occurs, con28 ABSTRACTS OF CHEMICAL PAPERS.taining large colourless felspar crystals, which variety is scarcely dls-tiriguishable from the true augite-felsite-porphyry. There can be nodoubt that i t is the final member of a series of these rocks distin-guishable by colour alone (more compact varieties being pure black),and it gradually passes into the rock containing numerous red ortho-clase crystals. ( 3 . ) The third bond of union between the two rocksis that augite is common to both. Fresh strongly pleochroitic angitewas found by the author in two preparations only, it being generallyfibrous, as in augite-felsite-porphyry. All specimens exhibiting a red-dish tinge contained no fresh augite, but pseudomorphs of chlorite,quartz, and a mineral resembling epidote. No hornblende could bedetected.The secondary quartz in the centre of the pseudomorphsis penetrated by a mass of pores, badly formed and sometimes radi-ating. Small druses in the chlorite contain a light-yellow columnarmineral, which may be epidote. All the quartzes contain fluid enclo-sures, but not in any great number. The large porphyritic quartzcrystals contain numerous glass enclosures ; one cryst,al 0.1 mm. indiameter contained five glass enclosures, whilst another crystal con-tained a glass enclosure which was + to Q of its own bulk. The ortho-clase crystals owe their colour to. hydrated ferric oxide, which hasseparated out.All the plagioclases exhibit a polysynthetical twin-formation. Zirkel observed that orthoclase does not decompose regu-larly,. but that in the centre of the crystal a pellucid adular-like kernelremains, surrounded by clouded orthoclase. The aut,hor found thatall porphyritic orthoclase exhibits a perthite-like intergrowth of mono-symmetrical orthoclase, with a polysynthetically twinned plagioclase,most probably albite. Further, he observed that the orthoclase 6ub-stance undergoes most readily a molecular change where the smallalbite crystals occur, the adular-like portions being completely freefrom interpolated asymmetrical felspars. From the above it appearsthat an interpolation of unsymmetrical f elspars in orthoclase-crystalscauses them to be more susceptible to atmospheric action.Most ofthe porphyritic felspar-crystals are well and sharply defined, and thosehaving a roundish form are often surrounded by a row of small quartzcrystals, attached to each other like pearls in a necklace. The acces-sory minerals of the Beucha granite-porphyry are biotite, magnetite,titanic iron, apatite, and garnet. Biotite was most common in thegreyish-black variety, being rare in the reddish variety. The apatiteoccurs generally in the chlorite-pseudomorphs, but it is also found inthe ground-mass between the quartz and felspar. Red garnet occursseldom, and in small grains. The ground-mass of the Beucha granite-porphyry is a crystalline granular mixture of quartz and felspar,with secondary chlorite, oxides of iron, and some apatite, but not atrace of microfelsitic substance was detected on any of the prepara-tions.It is a curious fact that the diameters of the quartz and felsparcrystals of the ground-mass are about the same, viz., from 0.07 to0.10 mm. The author concludes from his own observations, and those ofother mineralogists, that the augite-granite-porphyry of Beucha mnsthenceforth be classed geologically with the felsite-PorphyFries, and notwith the granites. C. A. BMIXERALOGICAL CHEMISTRY. 29Mineralogical-petrographical Notes on the Granite-porphyryof Lower Silesia. By 7’. LIEBISCH (Jahrb. f. N i w . , 1878, 311-313).-The granite-porphyry of the Riesengebirge is composed ofthe following minerals : quartz, orthoclase, plagioclase, biotite, potash-mica, hornblende, augite, magnetite, apatite, and orthite.The quartzoccurs in well developed, mostly pyramidal crystals (occasionally ex-hibiting narrow prism-faces), with rouiided edves, and often enclosingmovable globules of liquid, but no microlites. nThe orthoclase crystalsoften occur colourless and transparent, exhibiting an adular-likeshimmer. They are occasionally colourless in the interior only, whilstexternally they hare a reddish colour. Some of them are white, witlia zonal structure. The crystalline fonn varies in different localities ;one form observed on orthoclase crystals from Hermsdorf was 00 P.OP.2F 00. Twins according to the Carlsbad law are very common. Thosize of these crystals varies from a few millimeters to several centi-meters in the direction of the axis c. Enclosures of biotite and quartzcrystals are very common in the orthoclase crystals, although many ofthe colonrless crystals are almost homogeneous.The orthoclase of thegranite-porphyry of the Altarstein (the southernmost rock of theGrabersteine) is penetrated by per thitic plagioclasc, that betweenKirche, Wang, and Briickenberg being enclosed by plagioclaee. In-terpolations of isolated plagioclase crystals are often observed in theorthoclase of the Riesengebirge grauites, occurring parallel with thesecond cleavage plane of both felspars. I n some localities, a consider-able decomposition of the orthoclase is observable, the product beinggreenish or yellowish mica.The plagioclase crystals vary from 1 mm.to 3 cm. in size, and are generally white or yellowish, seldom red.Double twins occur at Hermsdorf and other localities, the twin axisbeing “ the normal to the brachypinacoid ” for the twin, and the twinaxis being “ the normal to the vertical axis in the bracliydiagonal ” for.the double twin. The plagioclase of the granite-porphyry from thequarry between Erdmannsdorf and Stonsdorf exhibits a zonal struc-ture. The plagioclase “weathers” much more easily than theorthoclase, the product being a light-coloured mica. Sometimes agreenish mica occurs in radiating divergent sheaves, which exhibit inpolarlsed light a black “ interference-cross,” and also occasionally areddish-brown substance resembling pyknotrope.Kumerous veins ofquartz penetrate the granite-porphyry at all localities. The biotiteoccurs in well-defined tabular or prismatic crystals of a greenish-blackor black colour, and exhibiting in section a distinct hexagonal outline.Sections made parallel to the axis C are transparent and of a greencolour on their edges, whilst internally the colour is brown, and somesections exhibit alternately green and brown transparent laminae.Hornblende occurs but sparingly as a constituent of the granite-porphyry, the principal locality being westward between Erdmannsdorfand Stonsdorf. At Erdmannsdorf greenish-black augite occurs as anaccessory constituent, and a t the same place and a t Lomnitz orthiteoccurs as an accessory constituent in acicular crystals 4 to 1 em.inlength, with an orthodiagonal development. The ground-mass of allthe Riesengebirge granite-porphyries is massive, and seldom pre-ponderates over the crystallised rock-constituents. It is grey t o reddish30 ABSTRACTS OF CHEMICAL PAPERS.brown in colour, except in the “ sdbands,” when it is black. Quartz,orthoclase, plagioclase, mica, &c., constiti-rte the ground-mass, whichis microcrystalline and coarse-grained. The so-called “ pseudosphEro-lites” of Rosenbusch occur in great beauty, 0.2 to 0.4 mm. indiameter, in a vein between Erdmannsdorf and Stonsdorf, and in thegrani t\e-porphyry of Buschvorwerk. The difference between the con-stitution of n rock from the middle of a vein and from a salband isvery marked in a granite-porphyry vein in a quarry between Erd-mannsdorf and Stonsdorf.The granite-porphyry from the centre ofthe vein contains in the grey ground-mass large white and greenish-white orthoclase and plagioclase crystals, grey quartz crystals, andgreenish-black biotite. These crystals diminish in size as their dis-tance from the centre of the vein increases. The salband rock con-tains in the massive blackish ground-mass only very small orthoclase,plagioclase, quartz, and black biotite crystals. The orthoclase andplagioclase crystals, however, were penetrated by innumerable smallbiotite laminae, and between the latter was a double refracting crypto-crystalline mineral, which could not further be studied. On accountof the band-like arrangement of the fclspar and biotite crystals of theground-mass around the isolated crystalline const>ituents of the rock,the author considers that a fluid structure is indicated.C.A. B.Occurrence of Dioptase on Chrysocolla, from Peru. ByC. A. BURGHARDT (Cham. New?, 37, 223).-The author examinedsome specimens received from Mr. W. M. Hutchings, of Birkenhead,which the latter thought to contain dioptase. The exact locality ofthe mine is unknown; but the chrysocolla was shipped from the portof Pisco, Peru. The specimens exanlined exhibited certain cavitieshere and there, which appeared to have been eaten out of the massby the action of some powerful solvent. These cavities were dividedinto numerous cells by the intersection of thin portions of chrysocollasubstance, and upon these partition walls were attached particularlyfine sheaves and bundles of emerald-green transparent crystals.Thesecrystals were so extremely small that it was almost impossible to makeaccurate measurements, but the forms characteristic of dioptase, viz.,OCI P‘L, -2R, were well defined. No other forms were observed.Sometimes numerous fine acicular sub-individuals growing parallelto each other built up a large individual. Carefully picked crystalsgave all the blowpipe reactions for dioptase. The dioptase crystalswere associated with colourless quartz crystals, the forms +R. -R.on the latter being in equilibrium. This is the first instance observedof the occurrence of dioptase in Peru. Maskelyne (Chem.News, 24,99) mentions some specimens of dioptase in the British Museum, oneof which is said to have come from the Rosario Mine, Chili, another(associated with quartz and eisenkiesel) from the Mina del Limbo delSalado, Copiapo, Chili. Only one of these specimens is associated withchrysocolla. The author is of opinion that the dioptase describedabove has been formed from the chrysocolla by the action of water.Very fine botryoidal malachite occurs associated sometimes withchrysocolla and cuprite, in the same locality in Peru. C. A. BMISERALOGICAL CHEXISTRT. 31On Unghwarite, Nontronite, Gramenite, &c. By A. KFSN-GOTT (Jahrb. f. Min., 1878, 180-185).-A. Scrauf (Jclhrb. .f. ilI;tL.,1877, 2.56) gave the results of two analyses of chloropal from Mugran,Bohemia, which he found to agree with an analysis of .~zontrouite byBerthier ; therefore nontronite was a variety of chloropal.Kenngottobjects strongly to the name chloropal, as the minerals inclnded in theso-called " chloropal-group " of Dana (including unghwarite, nontro-nite, pinguite, bole, and gramenite) are not true opals. Schrauf'sanalyses furnished the following, viz. :-Fe,03. A1,03. CaO. MgO. Alkalis. SiO?. H,O.1. 27.50 4.16 2.97 1.77 traces 43.98 (by diff.) 19.62 = 100.002. 28.91 3.19 3.35 2.84 - 42.43 (direct) 28.32 = 99.53If the alumina be considered a vicarious constituent, replacing ferricoxide, and the magnesia a vicarious constituent replacing calciumoxide, and both calculated into the corresponding amounts of ferricoxide and calcium oxide, also if the resulting percentages are thencalculated (the percentage of ferric oxide in each analysis being madeidentical), the composition of the mineral is as follows, viz.:-Fe,03. CsO. Si02. HzO.1. 32.00 5.13 41-44 18.50 = 97.072. 32.00 6.93 40.57 17.31 = 96.81From these calculated percentages i t is evident that the relativeproportions are nearly 10H20, 1R0, 2Fez03, 7SiO?. Schrauf assignedto the mineral the formula C~trMg2A12Fe,4Si,8G84 + 40H20. Theauthor points out that. i t would probably have been more correct hadSchrauf named the mineral from Mugrau, nontronitc. Tf Berthier'sanalysis of nontronite be treated in the same way as the above, resultsare obtained which agree closely with them, with the exception of thepercentages of the RO metals.These differences arc observed in theother allied minerals, whence the author concludes that unghwarite,nontronite, gramenite, pinguite, &c., are only impure varieties of amineral species which is essentially a hydrated ferric silicate, whosetrue composition yet requires to be ascertained. C. A. B.Mineralogical Notices. By S. R. PAIJKULL (Juh~b. J'. Mh.,1878, 209-210) .-Eucrasite, a New Mineral *from Brevig.-Thismineral is found upon one of the small islands in Brevigsf'jord. Crys-talsystem, probably rhombic. H. = 4.5to 5. Blackish-brown, streak brown, uneven fracture, fuses beforethe blowpipe on the edges and becomes lighter in colonr. Borax beadi n the oxidising flame yellow, in the reducing flame violet.Microcos-mic salt dissolves it, leaving a skeleton of silica. Partially soluble inhydrochloric acid, with evolution of chlorine ; completely soluble insulphuric acid.Sp. gr. (at 15" C.) = 4.3'3.Chemical composition as follows, viz. :32 ABSTRACTS OF CHEMICAL PAPERS.SiO,. TiO?. SnOr(?) Zr0,. MnO,. Tho,. CeO,. Ce20,. La?03Di20g.16.20 1.27 1.15 0.60 2-34! 3-5-96 5.48 6.13 2.42YzOs. Er&. Fe203. A1203. CaO. MgO. K20. Na20. H20.4.33 1-62 4.25 1.77 4.00 0.95 0.11 2.48 9.15Formula corresponding with the above (3R0, + +R,O, + $RO)SiO, + 2H20. The author considers it probable that eucrasite isidentical with the polycrase (thorite) from Brevig, of Scheerer andBreithaupt, and with the polymignite of Mollcr.Picrotephyoite froin Lactngban is a light red mineral, and may be con-sidered to be tephroite in which the manganese has been replaced bymagnesium.Its chemical composition is as follows, viz. :-SiOz. MnO. CaO. MgO. Loss on ignition.33.70 51.19 0.95 12-17 0.44 = 98.45.ilIaiaga?iozcs Serpeiztine f row?. Laaizgba~~.-Colour and streak brown ;uneven fracture ; brittle. Decrepitates before the blowpipe, and isscarcely fusible even in fine splinters. Dull on broken surfaces;vitreous lustre. I s found pseudomorphous. Chemical composition asfollows, viz. :-SiO?. PbO(?). Fe203. FeO. MnO. A1203. CnO. MgO.428.40 0.30 ‘7.51 1.84 7.77 0.90 2.80 24.60K,O. Na20. P205. Loss on ignition.0.04 0.47 trace. 10.000 = 98.63.Formula corresponding with the above = 4R0.3SiO2 + 2H20.Homilite.C.A. B.By DESCLOIZEAUX and DAMOUR (Jnhrb. f. illin., 1878,204-205).-This mineral (described by Paijkull, Jahrb. f. Min.,1877, 536) is found a t Stockii, near Brevig, accompanied by melino-phane and erdmnnnite. Descloizeaux found that the mineral crystal-lises in the monosymmetrical system, and exhibits a certain similarityto the forms observed on datolite and gadolinite, the crystals beinggenerally developed irregularly. Inclination of clinoaxis to the ver-tical axis = 90” 39’. The following forms predominate, viz., OOP,$42 m, OP, 00 P 00, F m, -P. H. = 4 5 to 5.Sp. gr. = 3.34. Black vitreous lustre ; transparent in thin fragments ;grey streak. Horizontal dispersion v > p . Some crystals contain agreen double-refracting dichromatic kernel, the outer rind or shellbeing yellowish and refracting light simply.Homilite evolves wateron being heated in a closed tube, fuses easily to a black glass, anddissolves in acid with gelatinisation. An analysis by Damour showedi t to have the following composition, viz. :-Cleavage not apparent.Oxides of Ce,SiO,. Boy. FeO. MnO. CaO. La,andDi. Na,O. H,O.33.00 15.21 18-18 0.74 27.00 2.56 1.01 2.30 = 100.00.C. A. BMISERALOGICAL CHEMISTRY. 33Daubreelite, the New Meteoric Mineral. By J. 11. SJTITA( C o i ~ y f . rend., 87, 338-340).--In the resistance of daubr6elite tothe action of hydrochloric and hydroflnoric acids, the author has foundan easy method of separating i t from troiilite and other impurities.Daubr&lite tlius purified presents itself in small, black brilliant scalcs,of density 5.01. It is not magnetic, and does not fuse before theblowpipe. It gives an intense green coloiir to borax, and is com-pletely soluble in hot nitric acid. The mean of four analyses givesthe following percentage composition : S 42.69, Cr 95-91, Fe 20.10.The mineral is therefore a double sulphide corresponding with chromeiron in which the oxygen has been replaced by sulphur, thus,FeS.Cr,S,. No terrestrial mineral of this composition is known. Theauthor found daubrkelite in several meteorites in which its presencewas not previously known, and he believes that this substance, eithcrin a visible condition, or so disseminated as to be discerned only afterchemical treatment, will be found to be universallypresent in me.teori tes. R. R.The Mineral Spring of "Tenninger Bad," Somvixer Tobel,By R. MEYEII. (Dezit. CJ~enz. Ges. Rer., 11, 1521--1526).-Sp. gr. 1.002582 a t 10.5" compared10,000 parts of waterGrisons.Temperature of the spring 14.3".with distilled water a t the same temperature.contain-Na,O. KZO. (NH,),O. CaO. SrO. MgO. FcO.0.0847 0.0532 0.0273 8.3688 0.0957 1.1428 0.0016AI20, and H,P04. SO,. c1. SiO,. co?.0*0008 13.4723 0-0049 0.198 1.7182Organic matter 1.1130, and traces of MnO, Pb, Cu, Zn (?) andHN03.Although the water a t present contains mere traces of iron, a thickferruginous deposit (containing traces of arsenic) is found a t the sourceof the spring. w. c. w.Presence of Lithium in the Earths and Water of the Solfa-tara at Puzzuoli. By S. DE LUCA (Compt. rend., 87, 174).--Theaiithor allowed 10,000 litres of water, which bad been used to levigate250 cwt. of Solfatara earth, to svaporate spontaneously. From themothcr-liquors he obtained a considerable quantity of amorphousmatter by desiccation. This yielded a hydrochloride, the spectrumof which showed the brilliant lines of lithium distinctly and thesodium lines feebly, showing clearly that the earths of the Solfatar,icontain traces of lithium in the form of sulphate, which can be ex-tracted by means of rain-water. Hot water is found in abundance FLCa depth of from 10 to 12 metres below the surface about, the oldcrater of the Solfatara, containing free sulphuric acid and sever21other substances. The water is formed both by the vapours of thenumerous fumaroles, and by the rain percolating through the poroussoil and dissolving on its way the soluble matter contained in it. OnFOL. sxsv1. 34 ABSTRACTS OF CHEMICAL FM'ERS.treating this water in the manner described above, the same resultswere obtained, as far as the presence of lithium is concerned, showingthat sulphate of lithium is contained in the trachytic earth and in thehot springs of the Solfatera of Puzzuoli. J. M. T

ISSN:0368-1769    

DOI:10.1039/CA8793600014

出版商:RSC    

年代:1879

数据来源: RSC

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34 ABSTRACTS OF CHEMICAL PAPERS.Organic Chemistry.Reactions of the Halogen-compounds of Olefines. 13yELTEKOFF (Deut. Chem. Ges. Ber., 11, 989-991) .-Recent experi-ments by the author have shown that the haloid compounds ofethylene, when heated with water and lead oxide, yield glycol andaldehyde ; whilst propylene chloride and bromide, under the samecircumstances, yield propyl glycol, acetone, and propaldehyde. Simi-larly isobutylene bromide yields isobutyl glycol and the corres-ponding aldehyde, and trimethylethylene bromide yields isopropyl-methyl ketone. From these results the author conclades that thefirst product of the action in every case is a glycol, which by elimina-tion of water is partially or entirely converted into aldehyde oracetone. J.R.A New Unsaturated Hexvalent Hydrocarbon, Diallylene,C,H,. By L. HENRY (Compt. rend., 87, 171--173).-The action ofPCI, on monallyl-acetone is energetic and regular a t ordinary tempera-tures, hydrochloric acid being abundantly disengaged. The product is amixture of allylmethylchloracetol, C3H5.CH2.CC1,.CH3, and mono-chlorodiallyl, C3H5.C3H4CI, resulting from the former by eliminationof HCI. The former is a colourless liquid, with a sharp smell andtaste, boiling a t 150" with partial decomposition. It is insoluble anddenser than water. The monochlorodiallyl, which constitntcs abont +thsof the product, is a colourless mobile liquid, lighter than and insolublein water, but soluble in alcohol and ether, and possessing a sharpsmell and tsste.Its sp. gr. a t 18.2" is -9197, and it boils a t 1.50"without decomposition. The vapour-density found is 4.15, calcu-lated 4.08. This body forms a tetrabromide, (C6H,C1Br4), which theauthor has not as yet solidified. It. disengages hydrochloric acid 'whentreated with sulphuric acid, forming probably a sulphate of acetonicalcohol. Heated with potash under pressure a t 100" i t yields ahydrocarbon of the formula C6H8.The author yegards monochlorordiallgl as a mixture of two isomericbodies :-(1). C3H5.CH2.CC1=CH2 ; and (2). C,H,.CH=CCl.CH,, re-sulting from allylic dimethyl chloracetol, C3H5.CH,.CCI2.CH3, by elimi-nation of HCl.According to the author the density of diallylene a t 18.2" is -8579 ;i t boils a t 70"; its vapour-density as found is 2.79, calculated 2.76.The author has not obtained the dibromide C,H,Br,, although thORGANIC CHEMISTRY.35tetrabromide is easily formed, and by further action of bromine con-verted into the hexabroruide ; both are viscous liquids. By the actionof ammonic cuprous chloride it yields a yellow precipitate, C6H,Cu +H,O, chara.cteristic of acetylene compounds, and with an alcoholicsolution of silver nitrate it gives a precipitate corresponding withCsH7Ag + C2H,(0H) ; with an aqueous solution it gives C6H,Ag +H,O. The author considers it probable that C,H8 contains two isomeridescorresponding with the formnlm-(a) CsH,.CH,.CECH.(6.) C,H,.C-C.CH,.corresponding to the two varieties of monochlorodiallyl above men-tioned. J. M. T.Action of Nitrous Acid on Unsaturated Hydrocarbons.ByP. TOKNIES (Deict. Chem, Ges. Ber., 11, 1511--1512).-When a con-centrated solution of potassium nitrite is poured into a glacial aceticacjd solution of furfurbutylene, the crystalline compound, C8HI0.NZO3,is obtained, which yields on reduction C8HloO(OH) (NH2). This bodyforms a platinum salt having the formula [CsHl0O(OH) (NH?)HCl],PtCI4.Phenylbutylene behaves in a similar way, forming CloH12, Nz03, and[CloH,,(OH) (NH,)HCl]J’tCl,.Styrol, tolylbutylene, anethol, and amylene also form crystallineaddition products with N203. w. c. w.Some Selenocyanates. By J. W. CLARKE (Deut. C’kem. Ges.Ber., 11, 1325-1326) .-Amongst the platinum thiocyanates thepotassium salt is the best known on account of its beauty and theease with which it may be obtained.It was thought of interest toprepare the corresponding selenocyanate, but some difficulty was ex-perienced in doing so. When alcoholic solutions of potassi~m seleno-cyanate and platinic chloride are mixed, a heavy red-brown precipitateis a t once formed, which becomes darker and partly dissolves on boil-ing. Crystals of the new salt separate out from the filtrate, mixed witha reddish selenium salt; these can be purilied by recrystallising fromalcohol, although they are rather easily decomposed. The crystals areordinarily small, but can be obtained as hexagonal tables, almost blackin reflected light, and dark garnet-red by transmitted light. Sp. gr.= 3.377 a t 10“ (weighed in benzene). Analysis gives numbers indi-cating the formula K2Pt(CSeN)+ The attempt to prepare gold com-pounds was only partially successful.When an alcoholic solution ofpotassium selenocyanate is mixed with neutral gold chloride, a red prc-cipitate falls, consisting mostly of pure selenium. On gradual evapo-ration, the orange-yellow filtrate deposits a crust of small, dark redprisms, which decompose so easily that only a small quantity was ob-tained, and this not pure. Analysis gave only approximate numbers,but sufficiently near to indicate that the salt was KAu(CSeN),,considering the impurity (metallic gold) present, for this salt wasd 31; ABSTRACTS OF CHEJIICAL PAPERS.prepared by a method precisely analogous to that bz which Cleveprepared his thiocyanste.The attempt to prepare a seleniocyanatesimilar to the potassiiim chromothiocpnate, K,Cr(CSN),,.8H20, ofRoeslar was unsuccessful. Aqueous solutions of chrome alum andpotassium selenocyanate mixed together gave rise only to a precipitateof seleuium. w. s.Alcohols in Potato Fusel-oil. By L. RARUTEAU (Camp!. ye11(7.,87, 501).-The following table shows the nature, boiling-point, andquantities of the products found in 1 litre of potato fusel-oil:-Boiling points. Quantities.Degrees. c. c.Tsopropjl alcoliol ...................... 8.3 150Propyl alcohol ........................ 97 30Ordinary but$ alcohol ................. 109 50Normal butyl alcohol .................. 106.9 65Methylpropyl carbinol .................. 120 60Ordinary amyl alcohol .................128-132 275Products boiling above 132", and retaining179Water - 12.3........................ amyl alcohol -................................Aldehyde, ethyl acetatc, and e t h j l alcohol - 75TrimethylcarbinoI also appears to be present. R. R.Etherification Of Primary Alcohols. By N. MENSCHUTKrN(Deut. Chem. Ges. Be?.., 11,1507-l~ll).-The author has repeated hisexperiments on the etherification of alcohols by acetic acid at. 154"(Ber., 11, 732), and finds that his former results were not quite cor-rect. He now obtains tlie following numbers for the (I) absolute,(TI) relative initial rate, and (111) limit of etherification.Methyl alcohol ....Ethyl . . . . . .Propyl . . . . . .Normal butyl . . . . . .Octyl . . .. . .Cetyl . . . . . .Isobntjl . . . . . .Ally1 . . . . . .Benzyl . . . . . .I.53.5346.95469246.8546.5944.3635.7238.64-IT.70.5270.1869-6164-4066.6660.12G3.96--TIT.69-5966-5766.8567.3072.3480.3967-3859.4160.75From these numbers i t is seen that all the primary normal saturatedalcohols, except methyl alcohol, have the same absolute initial rate ofetherification, but the absolute initial rate of isohutyl alcohol is lessthan that of the normal alcohols. The relative initial rate decreaseswith the increase in niolecular weight. The rate of et<herification ofthe unsaturated primary alcohols is less than that of the saturated.The limits of etherification increase with the molecular weight of thORG.WlC CHEMISTRY.37alcoliol (methyl alcohol forming a n exceptionj, but the limits arelower for tlie unsaturated than for the saturated alcohols. w. c. w.Amyl-compounds. By FLAwITzKY (Deut. Cliem. Ges. Ber., 11,!W.L).--The author has o'Jtained from ethylamyl oxide an amyl iodide,having tlie specific rotatory power + 0.07. This iodide yields apentylene which boils a t 'LO.?", has the sp. gr. 0.648 a t O", and is con-verted by oxidation witlh chromic acid into acetone, acetic acid, andanother acid, probably isobutyric. The corrcsponding g i p 1 boils at2Ol", and yields by oxidation acetone, traces of an a1deh-j-de, and acids,chiefly isobutvic.Flawitzky finds that diluted sulphui-ic acid (1 part of H,SC), and1 part of H20) is the best deliydrating agent for the gl-jcols.With it,trimethylethylene and isopropylethylcnc gljcols Field tlic same pro-clucts as with 1)hosphorus pentoxide or zinc chloride, but in muchlarger quantities. J. R.Oxidation Products of Diethyl Sulphide and AnalogousCompounds. By E:. 0. BEChalAxS ( J . pr. Chem [a], 17, 439-4i7).- 'l'lie author's iwearches have added the substance phenylefligl-sdphitZs to tlie list of sulphides of alcoholic radicles. This bodx is1)roduced by heating sodium phenrlmercaptide with three times its\\eight of ethyl iodide a t 120" iii sealed tubes : the new sulpliide boils; i t 204" (barometer = i43 S mm.), has a sp. gr. of 1.0315 a t lo", andIS a strongly refractive liquid with aii exceedingly disag yeeu'uleo lour.The me1 tiiig point of clil'.rol).2lfylsir711~~~~Z~, ( C,H9B),S0, is deter-mined to be G8.5', and not 41", as stated by Saytzeff aiid Grabowskyv(,iu?~uZen, 171, 235) : this substance is but slightly soluble in hotuater, while at the ordinary temperature 2 parts of water dissolve1 part of the sulphoxide.1 he author shows that sulphoxides, as also the corresponding su!-pliides, are generally oxidised to sulphories by the action of potassinriipermanganate ; sulphones have been thus produced from sulphidwcontaining one or two alcoholic radicles derived from primary orsccondary isoalcohols.The following new sulpliones have been ob-tained by the author's method :-Diisou?iz2/ZsuZ~l/o~ie (the action of nitricitcid upoii diisoamylsulphoxide, at nloderately high temperatures, resultsi r t the formation of isoarnplsulphonic acid), t Z i i s , ~ b u t y l s u ~ ~ I ~ ~ ~ ~ i e , i s o m l y l -etlrplsulpho~~e, tli;sl)~,,.o~lllszil1Jlronc, m e t h ~ l e t l i ! l l s i L l p l ~ ~ ~ ~ ~ , ~ ) ? i e ~ ~ ? j l ~ ~ t ~ ~ l 1' ho 11 e, and e t li e I 1 rd ie f h?j Zsa Zp I1 o TI c .T lie s u 1 plio i i e s are produced byheating an aqueous solution of the corresponding sulphides with i~slight excess of potassium permangnnate also in aqueous solufioii.Details of the purification of each suiphone are given in the originalpaper.Sulphones are stable bodies which may be distilled without decom-position; they are not reduced by the action of zinc and dilute sul-phuric acid or by hyclriodic acid ; neither arc they attacked by phospho-r u s pentachloride : sulphoxitles on the other hand, arc reduced by thereagents namcd, and are readily recmverted into sulphides by theaction of phospliorus pcntachloride.Former experimeiits which werer 38 ABSTRACTS OF CHEMICAL PAPERS.said to result in the prodnction of diethyl- and dimethyl-sulphide fromthe corresponding sulphones, by reduction, were certainly erroneous :the sulphones employzd probably contained traces of sulphoxides.Sulphides which contain acid radicles are energetically attackedby potassium permanganate, and are therefore not capable of takingup oxygen without molecular decomposition ; benzo?/lethylsulpkide, forinstance, is split up by permanganate into benzoic and ethylsulphonicacids. Saytzeff (Zeitschr. f.Chem., 1868, 642) has shown that thesesulphides are also decomposed by the action of nitric acid.In connection with this behaviour of acid sulphides, the authorexamined the action of barium dioxide upon thiscetic anhydride dis-solved in absolute ether. The action is an energetic one ; the productsare barium acetate, and acetyl persulphide ( C2H302)cS2.The author's investigations do not determine wit,h certainty whethersulphones do or do not form compounds with nitric acid.Sulphoxides containing only univalent radicles form somewhatunstable compounds with nitric acid, containing the elements of onemolecule of nitric acid combined with one molecule of sulphoxide.The following are the leading properties of the new sulphones pre-pared by the author.Diisou.ni~Z.sul~hone, ( C5Hl,6),SO2, crystalljses in groups of longneedles, which are unchanged in air, odourless, but possessed of asweetish yet burning taste.A t 31" the sulphone melts to a colour-less liquid, which boils a t 295" with very slight decomposition. Water,hot or cold, and aqueous solutions of alkalis, scarcely dissolve diiso-amylsulphone, but it is largely soluble in alcohol, ether, benzene,chloroform, and carbon bisulphide ; also in concentrated nitric, sul-phuric, and acetic acids, from which solvents it is reprecipitated byxddition of water.I)iisobutlJl.~SLlyhone, (C,H,B)?SO,, is a colourless syrupy liquid re-sembling glycerin, having a faint pleasant odour ; when surroundedwith a freezing mixture the sulphone solidifies to a crystalline massmelting at 17".The sp. gr. of the sulphone a t 18" is 1.0056 : theliquid boils at 265" without material decomposition. Hot water dissolvesbut small quantities of the sulphone, although it is soluble in two partsof water at ordinary temperatures : it is readily soluble in ether, andbehaves generally towards solvents similarly to diisoamylsulphone.SO2, is a thick, colonrless liquid with-out smell, which in a freezing mixture solidifies to a crystalline mass :the solid sulphone melts at 13*5", the liquid has a sp. gr. of 1.0515 a t18", and boils at 270". The action of solvents upoii this sulphone issimilar to their action, already described, upon diisoamyl, and diiso-butylsul phone.Diisopopy Zsulphnne, ( C,H,)2~SOz, forms colourless crystals withoutodour.It melts a t 36", forming a liquid which often remains for dayswithout solidifying. This snlphone is readily soluble in cold and inhot water, as also in alcohol, ether, benzene, chloroform and carbonbisulphide : concentrated nitric, sulphui*ic, or acetic acid likewisedissolves the sulphone, which is not reprecipitated by the addition ofw at e r .Isoanz~Zetl~ybulphone, c5H'1sC2& ORGANIC CHEMISTRY. 392l~et7~ytetlryZsu~7Lone, CH3 ] SO,, crys tallises in small brilliant C2H5needles which melt at 3rio-(th; liquid often remaining for days with-out solidifying). It is devoid of odour, and very soluble in water andin alcohol. This sulphone is scarcely soluble in cold ether or in car-bon bisulphide, but is dissolved in almost all proportions by benzene,chloroform, a d acids.Nitric acid very slowly attacks the sulphone,long continued heating in sealed tubes being necessary for the com-plete decomposition of the substance.Plienylethybu~hone, C6H5 } SO,, crystallises in thick colourlesstables, devoid of odour (m.p. 42"). The solubility of the sulphone isalmost the same a6 that exhibited by diisopropylsulphone ; it is how-ever reprecipitated by water from its solution in acids.SO2, is produced by the action ofpotassium permanganate upon diethyl sulphide at the ordinary tempera-ture; it crystallises in short, hard, colourless needles. It melts a t 136.5",and distils unchanged a t a higher temperature. This sulphone is solublein hot alcohol and water ; it is scarcely dissolved by ether, benzene,chloroform, or carbon bisulphide, but is readily soluble in concen-trated nitric and sulphuric acids, less so in hydrochloric acid, and withj e t greater difficulty in acetic acid : it is decomposed by warm solutionsof the alkalis.M. M. P. M.Glucoside of Buckthorn Berries and Rhamnodulcite. By C.LIEBERMANN and 0. HORMANN (Deut. Chew. Ges. Ber., 11, 952-958).-An examination by the authors of the glucoside extracted byalcohol from the berries of buckthorn (Rhamnus infectorius) has led tosome results differing from those arrived at by previous experimenters.The glucoside was first prepared pure by Gellatly, who called itzanthorhanznin, the name adopted by the authors.It is identical withSchutzenberger's a-rhamnegin. The properties of the substance, asdescribed by these chemists, agree with the observations of theauthors.When boiled withdilute sulphuric acid it readily breaks up into rhamnetin and sugar(rhamnodulcite), the former of which is deposited in tufts of lemon-yellow needles, agreeing in composition with Schutzenberger's formula,C12H1005.Rhamnodulcite the authors find to be (contrary to the observationsof Gellatly and Schutzenberger) a crystallisable sugar. It is solublein water and absolute alcohol, and crystallises from the latter in herni-liedral tables. The aqueous solution yields holohedral crystals, whichmelt a t 92-93". Dried in the air, the sugar has the formula CSH,,O6.When heated, it melts, and at 108' gives off 1 mol.of' water: theresidual C,H,,05 solidifies on cooling to a brittle glassy mass, theaqueous solution of which again yields crystalline sugar. Rhamno-dulcite is very sweet and agreeable in taste. It does not ferment withyeast. Its action on polarised light is dextro-rotatory. It reducesh'ehling's solution on warming. Xanthorhamnin yields about 57 perccnt. of the sugar.C2H5EthyZenedL'ethyZsu2;piLone, CzH4 (C2& )2 }Xanthorhamnin does not ferment with yeast.J. R40 ABSTRACTS OF CIIEMICAL PAPERS.Isodulcite. By L. BEREND (Dcut. Chem. Ges. Bw., 11, 1353-1355).-Liebermann and Hormann obtained a beautifully crystallisedsugar, by the decomposition of the glucoside of buckthorn berries(12lmm?zus kfectorius) with acids, which was strikingly like the isodul-cite prepared by Hlasiwetz and Pfaundler from quercitrin.On accountof certain discrepancies, however, in melting point, &c., they termedi t rhamnodnlcite. On re-examining the isvdulcite of quercitrin theauthor. found that the two sugars are identical. The quercitrin employedwas prepared according to the method of Zwengler and Dronke, aridthe isodulcite therefrom according to that of Hlasiwetz and Pfaundler.Melting points (93-94”) and crystalline forms of the isodulcite andrhamnodulcite were found to be the same. Hlasiwetz and I’faundlerfound the melting point to be 10.5”. The specific rotatory power inSoleil-Scheibler’s apparatus was [aIu = 8.04. The name rhamnodul-cite can thus be dispensed with.Liebermann also points out in afootnote that Schiitzenberger’s rhamnegin-sugitr is probably only im-piire isodulcite, in spite of the difference in its properties. JV. S.‘ l Mercurialine ”. (Methylamine). By E. ScHxIDrr (L;e/,ig’s AIL-? ( d e n , 193, 73--86).-I5. Reichardt has described (Jour. J: p v k t .C‘hern., 104, i4Ol) a, volatile allraloid “ mercurialine,” whicli he ob-tained from Mem(ria1is anwua and ilfercurialis pereniks, as having thesame composition as methylamine, but differing from it in being anoily colourless liquid a t the o r d i n q temperature, and in forming tinoxalate and sulphate whose cr.ystitllisiiig characters were riot i n accord-ance with those given by JVurtz for the corresponding salts of methyl-amine.The author has separated a large quantity of the alkaloid whichexists in JIercuriczZis annua, and has compared it with pure methyl-amine prepared from caffeine.The results proye that the two alka-loids and their corresponding salts are in every respect identical, andthat Reichardt’s “ mercurialine ” is none other than an aqueous solu-tion of methylamine. I t was also found that the oxalate and sulphateof methylamine do not bclis\.c ; r i tiic manner stated by Wurtz (Atznnh,76, 324), but that they are readily crj-stallisablc from water ; in fact,agreeing with the results obtained by Reichardt with the oxalate andsulphate of “ mercurialine.”“rimethylamine in small quantity was also obtained from Illei*curialiscmuua, and its presence there, together with a considerable quantity ofthe primary base induces the supposition that diniethy lamine mayalso be present.I n many plants which the author has examined, hehas found a small quantity of trimethylamine accompanying ammo-nium salts, but has met with no species of plants other than thoseabove mentioned, which contain methylamine, although no doubtmethylamine is not confilled to them. A. J . C.Trimethylcarbarnine. By W. RUDNEFF (Deut. Chein. Ges.Ber., 11, %%).--This body was first obtained by Butlerow as a bye-product in the preparation of trimethylacetic acid. According t o theauthor’s observations, it, boils a t 45”. Its hydrochloride, CaH9NH2.HC1,crj-stallises from alcohol in small lamine. Its platinum salt forms ORGAXIC CHEMISTRY.41yellow crystalline powder. The amine combines with carbon bisul-phide to form the compound CS(NHC4N,) (SNH,C,H,), from which, b yz e a n s of mercuric chloride, tertiary butylthiocarbimide, C( CH:,j3N.CS,is obtained. This last boils a t 142", melts a t 10.5", and has an agree-able aromatic odour. J . R.Sulphuretted Dicyanodiamine. By B. RATHKE (Deut. Clzem.Ges. Ber., 11, 962--967).-The author has obtained a body to whichhe assigns the constitutional formula, NH,.CS.NH.C( NH)NH2, by theaction of thiocarbonyl chloride or phosphorus pentachloride on thio-carbamide. The reaction with phosphorus pentachlo ride is representedThe new product is a base forming transparent monoclinic crystals,which dissolve in water and sparingly in alcohol, and yield a stronglyalkaline solution.When heated above loo", it melts and is com-pletely transformed into the isomeric guanidine thiocyanate.The i ~ y d r o c l ~ l o ~ i ~ l e , C2H6N,S.H C1, forms fine transparent rhombiccrystals, which dissolve freely in water and alcohol. With platinicchloride it gives an amorphous dark-coloured precipitate. Tlie o.ca,Zate,C2H6N,S.C2H,0, -t +HLO, forms small granular crgst,als, sparinglysoluble in water. Both salts have an acid reaction.thus: 3CS(NH,), + PC1, = C?SN,H,.HCl + CS(NH,)?.HCl+ PSCI?.J. R.Butylchloral Hydrocyanide. By A. PIKNER and F. KLEIN(Deut. Chenz. G'es. Bey., 11, 1488-1499 j .-Butylchloral hydrocyanideprepsred by digesting butylchloral hydrate with aqueous hydrocyanicacid a t 100" for several days, forms crystalline plates which dissolvereadily in alcohol and in ether, sparingly in water and in benzene, butare insoluble in petroleum ether.This substance melts a t 101-102",and boils with decomposition a t 230".Action of Amrnomk-When ammonia gas is passed into a solutionof butylchloral hydrocyanide in absolute alcohol, ammonium chloride,ammonium cyanate and monochlorocrotonamide (m. p. 112") areformed, C,H5Cl3(0H)CN + INH, = C,H,ClO.NH, + 2NH,CZ +NH,CN.A good yield of chlorocrotonamide can be obtained by gently heat-ing a mixture of dry butylchloral hydrocyanide and ammonium carbo-nate in a sulphuric acid bath, until hydrocyanic acid is no longerevolved, and extracting the residue with ether.No crystalline compound is formed by the actioii of aniline on theh y d rocy anid e.Monochlorocrotouzyl carbamide, CO( NHE,)NH.C4H,C10, is obtained byheating a mixture of butylchloral hydrocyanide with urea at 105-110", until all the hydrocyanic acid is evolved, the residue being thentreated with alcohol, and tJhe ammonium chloride washed away bywater.With acetyl chloride, butylchloral hydrocyanide forms the com-pound C4H5CI3(OC,H3O)CN. It is a yellow oil, boiling with decom-position between 240" and 250".When a solution of the hydrocyanide in concentrated sulphuric acidis poured into water, tricTLloroxyvcLleramide or tril;hlorou~lerolactamide,C~H5Cl,(OH)C0.NH2 (m.p. l l 9 O ) crjstallises out. It is very solubleThis carbamide melts wit8h decomposition at 216"42 ABSTRACTS OF CHEMICAL PAPERS.in alcohol and ether, and sparingly soluble in benzme and in 1vate.r.The hydrochloride is precipitated from the alcoholic solution of theamide by gaseous hydrochloric acid.The amide prepared from acetyl-butylchloral cyanide melts at 96",and is probably a physical isomeride of the preceding compound.A mixture of trichloroxyvaleramide, and trichlor-oxyvalerimido-etheris formed by passing hydrochloric acid into an alcoholic solution ofbutylchloral hydrocyanide.Tric7~lorobz~t~Zide?zi~~tide, C4H5C13NH, obtained by heating a mixtureof dry ammonium acetate with butylctilornl hydrocyanide, and pour-ing the product into water, is a crystalline body, which melts at 164-165", and decomposes on exposure to the light, or when heated to 192".If is sparingly soluble in cold water and in cold benzene, but dissolvesreadily in alcohol, ether, glwcial acetic acid, in hot water and in hotbenzene.Trichloroxyvnleric or T?.icliZorvalel.olnctic; acid, C5HiC1303, describedby Pinner and Bischoff, forms the following salts: C,H,NaCI,O, +H20, loses its water of crystallisaLioa a t 100".The ammonium saltforms small granular crystals, and the lead salt is an amorphous pre-cipitate. The acetyl compound, C4H5Cl,(OC2H30jCOOH + H20,which crystallisps in white needles (m. p, 84"), is prepared by digest-ing the acid with acetic anhydride and pouring the product into coldwater. It is insoluble in cold water, and is slowly decomposed byboiling with water. The anhydrous compound forms a thick uncrys-tallisable syrup.Ethyl trichloroxllvcclerate, C5H6C1303.~2H5, forms long prismatic crys-tals, which melt at 40" and boil a t 255".If this ether is dissolved inalcoholic ammonia, and the solution left a t rest for several weeks, awhite crystalline crust is formed, which consists of a mixture ofammonium chloride and the amide of ~no~zochZorinaidoa~ayeZic acid,C5H,C1N,0. The amide is soluble in hot benzene, and is reprecipitatedby the addition of light petroleum to this solution. I t melts at 118"with decomposition. Platinum chloride and silver nitrate produceprecipitates in the aqueous solution. The ketone of monocldorangelac-tamide is obtained on evaporating the alcoholic solution of the smideof monochlorimidangelic acid, C5H7C1N20 + H20 = C5H6C1NO2 + NH,.When this body is heated, it decomposes without melting.Mo~~o~hZorn~zgelnctic acid, C5H7 ClO,, prepared by the reductionof trichlor-oxyvalerianic acid (Ber., 7, 589) forms the followingsalts : ( C5H,C10,),Zn, anhydrous crystals, very soluble in water ;(C5H6Clo3)2Cu, pale bliie powder insoluble in water and in alcohol:C5H9C103.Ag, deposited from a hot aqueous solution in pearly needles,is decomposed by boiling with excess of silver oxide, forming mono-chlorocrotonaldehyde or monochlorocrotonic acid.Ethyl monochlorange~actnte, C&I,C~O~.C2H5, is a heavy oil, boilingwith decomposition at 230", and is slowly decomposed by water. Theisobutyb ether boils a t 235-240', and is not decomposed by water atthe ordinary temperature.Monochloro-dibrom-oxyvaleric acid, C5H7C1Br203, is prepared by add-ing bromine to a solution of monochlorangelactic acid ia glaciaORGANIC CHEMISTRY.43acetic acid. It is soluble in ether, insoluble in benzene, and melts a t169".DichZorangeZic acid, C,H,CI,O,, is formed when t,he crude product ofthe action of phosphorus pentachloride on monochlorangehctic acid ispoured into water. It is an oily liquid, which does not form additionuroducts with bromine.MonocldorangeZic acid, C5H, ClO?, probably CH3. C ClZC H. C H?.COOH.The ether G f this acid is prepared by the action of zinc and hydro-chloric acid on the alcoholic solution of dichlorangelic acid. The freeacid obtained by saponifying the ether melts a t 103", and is soluble inhot benzene.w. c. w.Chloralide and its Derivatives. By 0. WALLACH (Liebig'sAnnalen, 193, 1-61> .-This paper consists of an historical sum-mary of the work of other chemists on chloralide, and contains also arecapitulation of the author's investigations on the subject, of whichabstracts have already appeared in this Journal.The Acids of Wood-vinegar and their connection with theso-called Wood-oils. By C. KRXMER and M. GRODZKI (Deuf.Chmz. Ges. Bey., 11, 1356--1362).-1n a previous paper on crudewood-spirit (ibid., 9, 1920), the authors indicated the possibility thatthe intermediate bodies corresponding with xylene and cymene couldbe obtained by condensation of aldehyde and acetone (methyl-ethplketone).The first opinion-that only saturated acids took part in the formx-tion of these bodies-was found untenable, and the authors weregradually led to assume that unsaturated acids must also be present inthe mother-substances, a supposition confirmed by experiment.Ander-son found that salts could be obtained from the acid fractions of wood-vinegar boiling up to above 160", which certain1.y contained propionicand bntyric acids, and probably valerianic acid ; but he did not isolatethe pure acids. The authors therefore examined certain liquors fromthe works of Kahlbaum, in Berlin, which had been obtained in thepreparation of sodium acetate or calcium acetate from wood-vinegar,and laid aside as refusing to crystallisefurther. After the greater partof the sodium acetate had been removed, the mother-liquors yielded anoil on addition of sulphuric acid, from which the following acids wcreobtained in the pure state and in considerable quantities :-A.J. C.Experiments in this direction failed.'Suturuted : Formic, acetic, propionic, bu tyric, and valeric acids.Unsaturated : Crotonic and angelic acids.The latter, however, has been recognised only by examination of itssalts.Both crotonic and isocrotonic acids were found to be present, andtheir occurrence is explained by considering them as formed by thesplitting off of two hydrogen-atoms from the normal butyric acid,CH3.CHI,.CH,.COOH, which first furnishes the unstable isocrotonicacid, CHz~CH.CH2.COOH, which becomes converted into the stablecrotonic acid, CH,.CH=CH.COOH.For this reason the occurrenc41 ABSTRACTS O F CHEMICAL PAPERS.of meth-j-1-acrylic acid, CH,=C(CH,) .COOH, would be excluded, andiiideed not a trace could be detected.1 he well-crystallising calcium salt of angelic acicl was found to havethe composition of tlie known one, (C5H802)2C:> + 2H,O. The silversalt of the acid was also obtained, and gave sufficiently good numbersfor angelic acid. It differs considerably, however, in several respects,both in behaviour and properties, from the two angelic acids known.Thus the two latter are solid, and melt a t 45' ancl 62', but this, theformer, remained fluid. Fittig has observed that by heating, thelower meltiiig acid passes over into the higher melting one, and thatthere is an intermediate stage a t which the acid remains fluid.The authors, however, did not redise this in their case.Even onheating for a clay t h e acid failed to pass from the liquid t o the solidmodification. Also on treating with bromine, a remarkable differenceis noticed. Whilst angelic acid gives a solid crystalline dibrorno-com-pound with 1 mol. of bromine, tile acid obtained by the authors re-mained liquid. Towards a l l ~ ~ . l i , hQwever, the latter brominated acidbehaves exactly like the dibromangelic acid, viz., it loses CO, andleaves behind an oil, which to all appearance is identical with crotonylbromide. Alhough i t is possible that the presence of some impurity mayoccasion the above differences, yet it is quite possible also that the acidin question may he a t,liird angelic acid analogous to isocrotonic acid.This demonstration of the occurrence of normal acids and the corre-sponding unsaturated acids iii the complex process of the splitting upof the cellulose molecule by dry distillation is interesting in severalways.Whilst in the butyric acid fermentation, only those fatty acidsare formed that have even numbers of carbon-atoms (raleric and pro-pionic acids nL)t being produced), in t h i s case the fatty acids with evenand those also with odd numbers of carbon-atoms appear, just as inalcoholic fermentation, in which, however, tlie alcohols correspondingwith these higher acids belong, not to the normal, but to the iso-series.Starting then from the same cellulose molecnle on the one handand the same sugar molecule on the other, three different kinds ofdecomposition occur :-I.By A l c o l ~ d i c ~er~~~entation.-Alcohols with even and odd numbersof carbon-atoms arise, i e . , besides ethyl and prop91 z~lcohols, also iso-butvl and isoamyl alcohols.11. By Butyric Acid ~~e,.)?zentutio,i.-Besides acetic acid, normalbutyric acid and normal caproic acid are formed, i.e., acids with evennumbers of carbon-at,oms.111. L'y Dry DistlZZation.-Acids with even and odd numbers ofcarbon-atoms : besides acetic acid, propionic, normal butyric, aiitlnormal vsleric acids were found.I n No. 111 a method of complete separation by fractional distillationwas found wholly impossible, so heterogeueous is the mixt'ure ofbodies, ancl so many boii at about the same temperature. There arethe saturated and unsaturated acids, together with bodies taken upfrom that portion of the distillate known as the " wood-oils,)) ketonesof the fatty and of the oleic scries, as well as mixed ketones of bothgroups, and also condensation-compounds, all probably present to-r igether.IV. sORGANIC CHEMISTRY. 45Angelic Acids of Different Origin. By W. V. l l I r , L m (DeJit.Chet17. Ges. Bey., 11, 1526--1,728).-By oxidising fermentation vnlc-rianic acid with potassium perriianpnate, Neubauer (A1~?iaZm, 106,63) obtained carbon dioxide, oxalic, acetic, and butyric acids, andangelic acid (m. p. 69.5-i0"), which solidified in the condenser OILdistilling the product of oxidation with sulphuric acid.A hydroxy-mid is first formed, which on distillation with sulphuric acid loseswater and forms angelic acid. This acid can be isolated, if care istaken to avoid adding an excess of sulphuric acid to the oxidation-product, and the mixture is distilled with steam. Zlydroxyialeric acidis an oily liquid, which solidifies after remaining in 'ccIc?io many daysover sulphuric acid. It is neither identical with Rohrbeck's a-methyl-15'-oxybutyric acid (ihid., 188, 229), nor with tlie a-methyl-a-oxr-butyric acid of Frankland and Duppa (ihid., 136, 9), both of whichyield a-methylcrotonic acid on dry distillation.Neubauer's acid differs from z-methylcrotonic acid in melting pointand in its barium salt. Neubauer's barium salt contains two mole-cules of water, and crystallises in the monosymmetrical system,whereas barium methyl-crotonate crystallises with four molecules ofwater in the asymmetrical system.w. c. w.Monosulpholactic Acid. By C. BOTTINGER (Dezct. Chew. Ges.Bey., 11, 1561) .-The monosulpholactic acids from pyroracemic acidand from a-chloropropionic acid are identical. Schacht's acid (Annn-l e n , 129, 1) from a-chloropropionic acid was impure : hence the appa-rent difference between the acid from the two sources. w. c. w.Synthesis of Pyroracemic Acid. By L. CLAISEN and J. SHAD-WELL (Deut. Chem. Ges. Ber., 11, 1563--1568).-The authors haveaccomplished the synthesis of pyroracemic acid by means of acetylcyanide, and have thus proved the correctness of Wichelhaus'sassumption that this acid is identical with acetyl-formic acid.When acetyl cyanide prepared by Hiibner's process (Anwrrlen, 120,334) is mixed with the theoretical quantity of hydrochloric acid,sp.gr. 1.20, acetjlformamidc separates out: C,H,O.CN + H,O =C,H,O.CO.NH,. (In this operation an excess of acid is to be avoided,and the mixture must be well cooled.) The formamide is soluble inwater, ether, alcohol, chloroform, and in benzcne. The alcoholic solu-tion deposits transparent prisms or plates, which melt a t 12&125",and begin to sublime a t lOO", forming crystals resembling benzoicacid.The amide is converted into pyroracemic acid by the action of aslight excess of dilute hydrochloric acid a t 100" : C2H,0.C0.NH2 +HCl + HZO = C2H30.COOH. + NH4Cl.The acid was identifiedby conversion into uvitic and dibromo-pyroracemic acids, and intoBy C. BoT'rIxGER (Dezct. C'hem. Ges. Be?-., 11, 135.2-1.3j3).-P?/yofa~.ta,.~~mid.-When a mixture of p j rotartaric acid and phosphorus ppntn-sulphide is distilled in small retorts, an oil is obtained coiitai;~;~ gpentabromacetone. w. c. w.Action of Phosphorus Pentasulphide on Organic Acids46 ABSTRACTS OF CHENICAL PAPERS.suspended sulphur. It is insoluble in cold water, smells slightly ofhydrogen sulphide. On long digestion with hot water it dissolves,and small quantities of hydrogen sulphide escape. The solution oncooling deposits pyrotartaric acid in yellow crystals, to which traces ofa sulphurised body adhere ; 26 grams of pyrotartaric acid furnished18-7 grams crude pyrotartaric anhydride.Pyroracemic acid.-Only a small amount of dccornposition, and smallyield of sulphurised substance.80 grams of pyroracemic acid fur-nished 27 grams of distillate. This could be separated, by fractiona-ting, into acetic acid, pyroracemic acid, and a high-boiling sulphurisedbody. With the acetic acid and the pyroracemic acid, there is also Rsmall quantity of a sulphurised body. The sulphurised body wasa red neutral oil.Lactic Acid.-This acid decomposes almost completely, on distilla-tion with phosphorus pentasulphide, into gaseous and partially sulphu-rised products. The fluid distillate is very small, and contains an oilysulphurised body. The latter was dissolved in alcohol and the solutionplaced in the exsiccator.Besides the alcohol, some volatile sulphurcompounds escaped, communicating to the sulphuric acid an intensered coloration.Action of Zinc-methyl on the Bromides of MonobrominatedAcid Radicles of the a-Series. By M. KASCIIIRSKY (Dew!. Chem.Ges. Ber., 11, 984-987).-Zinc-methyl reacts with a-bromopropionicbromide to form a hexyl alcohol boiling at 118--119", and solidifyingbelow 2.5". The chloride derived from this alcohol boils a t about 112",and solidifies at -2". The iodide boils at about 140", and solidifies a t-3". The corresponding hexylene distils between 72" and 74", andforms with bromine a solid compound melting at 169". By oxidationthe alcohol yields acetone and acetic acid. From these facts theauthor infers that the alcohol is dimethyl-isopropyl carbinol.The product of the action of zinc-methyl on a-bromisobutyric bromideis pen tamet hyle thol.Norms1 a-bromohutyric bromide reacts with zinc-methyl to form :Lheptyl alcohol boiling at 138-140", and remaining liquid a t -30".The corresponding chloride boils a t 135-138", and the iodide a t 145-147".The heptylene derived from the alcohol boils a t 92-95', andforms a liquid compound with bromine. By oxidation, the alcoholTields acetone and acetic acid. The author concludes, therefore,that the alcohol is either dimethyl-butyl carbinol or methyl-ethyl-isopropyl carbinol. J. IL.Conversion of Nitrils into Imides. By A. PINNER andF. KLEIN (Deut. Chem. Ges. Ber., 11, 1475--1487).-Action of Hydro-chloric Acid and Alcohol on Eydrocyanic Acid.-When gaseous hydro-chloric acid is passed into a well cooled solution of hydrocyanic acidin absolute alcohol, a series of explosions takes place, ammoniumchloride separates out, and the solution contains a mixture of ethylformate, ethyl chloride, diethyl - glyoxylamide, and ethylic diethyl-glyoxylate.Eth,yZcliethyl ic gZyoxy ltr te, CH( 0 C2H,)2.COOC2H5, boils a t 195-196",The neutral residue was a red mobile oily body.w. sORGANIC CHEMISTRY. 47and is lighter than water. When treated with ammonia, it yieldslarge tabular crystals of d i e t h ~ l - ~ I ~ o x y Z u n t i d e (m. p. 81-82O) and ethylalcohol, C8HI9O4 + NH3 = C6H13N03 + C2H60. If isobutyl alco-hol is substituted for ethyl alcohol in the preceding experiment, nmixture of isobutyl chloride, ammonium chloride, and isobutylicdi-isobutyl-glyoxylate is formed.IsobutyZic di-isobutyl-glyoxylate, CH(OC4Hg),.COOC4Hg, b.p. 250-252", is converted into isobutyl alcohol and di-isobutyl glgoxylamide,m. p. 42-45", by the action of alcoholic ammonia a t 100": C14H2804 + NH, = CloH2,N03 + C4H,,0. The formation of diethyl-glyoxylicacid and of di-isobutyl-glyoxylic acid from hydrocyanic and hydro-chloric acids and alcohol may be represented by the followingequations :-2HCN + 2C2HeO + 2HzO = C,HI,O, + 2NHS2HCN + 2C4H100 + 2HZO = C,&I,,O~ + 2XH3.Neither the imido-ether of formic acid, HC(NH)OC2H5, norGautier's formimido-amide, CH(NH)WHz (Con@. rend., 65, 472),were obtained by this reaction.Action of Hydrochloric Acid n?i t l Alcohol on Cyanogen.-Whencyanogen gas is passed into a solution of hydrochloric acid in ab-solute alcohol, in the proportion of 1 molecule of cj-anogen to2 molecules of hydrochloric acid, the chief product is the hydrochlorideof oximido-ether, which separates out as a white precipitate, leavingin the mother-liquor a mixture of ammonium chloride, ethyl chlo-ride, ethyl formate, and urethane, which owe their origin to a secondaryreaction.The urethane is probably formed by the decomposition ofthe oximido-ether by hydrochloric acid and water, thns : C6HI2N,O2 +2H.20 + HC1= C3H7N02 + CHOLCzH5 + NHdCl.The hydrockloi-icle of ox-i?nido-etl~er, [ C(NH)OC2H5],.2HCI, is adirect addition-product : C2N, + 2CzH60 + 2HC1 = CsH,2N202.2HCl.It is insoluble in alcohol and is decomposed by water, forming ethyloxalate.Aqueous ammonia converts it into oxamide. The free base,obtained by treating the hydrochloride with absolute ether and solidpotash, is deposited from an ethereal solution in long thick colourlessprisms (m. p. 25", b. p. 170"). If isobutyl alcohol is substituted forethyl alcohol, oximido-isobutyl ether and isobutyl urethane are ob-tained.Action qf Hydrochlo& Acid and Alroltol on Propionitri1.-The thickoil which is formed when hydrochloric acid gas is passed into a mix-ture of isobutyl alcohol and propionitril, on decomposition withalcoholic ammonia, yields long prismatic crystals of the hydyochloridrqf propionimidamide or propionanzidine, C2H,C(NH)NH2.HCl.Thehydrochloride is deliquescent', and is very soluble in water and inalcohol, but is insoluble in ether. It melts at 133", and begins to de-compose at 233". Potash solution converts this substamce into an oilyliquid, probably propionimidamide, which decomposes slowly in pw-sexice of moisture, forming ammonia and propionamide.By the action of gaseous hydrochloric acid on a well cooled mixtureof absolute alcohol and acetonitril, a crystalline compound is formed48 ABSTR-4CTS OF CHEMICAL PAPERS.which yields acetimidamide hydrocbloride, on treatment with alcoholicam mon i a.P-nccjd tli h ;llo-etll yl-ef he 1- h y71.0r7i Zwidp, C,,H7 C (N H) OC2H5. H C1, is acrystalline compound, prepared by passing hydrochloric acid gas intoa solution of two parts of @-cynnanaphtllalene in one of alcohol. Tttlecomposes when lieatecl, forming ethyl chloride and the smide of,3naphtiioic acid : C,,H7C(NH)OC2Hj.HCl = C,,H7CONH2 + C2HjCl.The free irriidc-ether is obtained by the action of aqueous ammonia onthe hydrochloride. It is an oily liquid, insoluble in water, but solublein alcoliol, ether.and benzene.Alcoholic ammonia converts the hydrochloride into ,~-nrlyhtl~iinicZo-criwb?e lycZrochZoricZe, Cl,,H,C(NH)NH2.HCl, which crystallises in pearlyneedles (ni. p. 224~--2226'). The ci-ystals are soluble in water andin alcohol, and turn red on exposure to the light.By shaking up the hydrochloride with caustic soda, the free base isobtained in the form of an oily liquid, which crjstallises in a vacuum.P-naph thimido-isoBzit~l-eth er k?yl~ocli loride, Cl,HiC (NH) 0 C,H,.HCI,prepared by passing hydrochloric acid gas into a solution of P-cyano-naphthalene in isobutyl alcohol, melts with deconiposition a t 140°,forming /%naphthamide. /3-11op?~thinlii?o-isobut2/1 ether is depositedfrom a n ethereal solution in long white needles (m. p. 38"), whichdarken on exposure to the light. On boiling with acetic anhydride,~--zic~Iitki,nido-ncetnte, Cl,H,C(NH)OC2HJ0, is formed. This substanceis deposited from a hot alcoholic solution in silky-white needles w. c. w. (m. p. 150-152O).Action of Iodine on Thiocarbamides. By W. RUDKEFF(Deut. Chern. Ges. Rer., 11, 987).-The reaction of diphenylthio-carbamide with iodine results, according to Hofmann, in the forma-tion of phenylthiocarbimide, triphenylguanidine hydriodide, and freesulphur.The author finds, however, that aniline hydriodide is alsoamongst the products of the reaction, which he represents thus :-SCS(NHC,H,), + I 2 = 2CSSCSH5 + CN3H*(CGHj)3.H1+ CGH5NHZ.HI + s.carbaniic acid is represented by Hofniann as follows :-Again, the action of iodine on the ethylamine salt of ethylthio-CS(NH.C,H,)( SNH,.C,H,) + I 2 = CSNCzH5 + C,H,NHz.HI + HI + S.But, according to the author, this equation expresses only the firstphase of the reaction, for the products include also carbon bisnlphideand diethylthiocarbamide, which are the results of secondary actions.5CS(NH.C2H,)(SNH,C2H5) + 31, = 2CSNC2H5 + 2CSz +GC2HsNH2.HI + CS(NHCzH5)Z + 3s.By C.J. MABERY and H. B. HILL (Deut.Chem. Ges. Ber., 11,1329-1352).-When dry neutral lead urate is heatedwith excess of methyl iodide, dimethyluric acid is easily formed, butthe lead salt is not completely decomposed, the product being a mix-ture of the mono- and dimethyl-compounds. A little more than thetheoretical quantity of methyl iodide, diluted with an equal weight ofether, should be used. The decomposition procecds rapidly at lGT,",r i 1 he reaction in its entirety is represented thus :-J. R.Dimethyluric AcidORGANIC CHEMISTRY. 49and is completed in 15 to 20 hours. To prevent formation of themono-compound, potassium urate containing some excess of potas-sium hydroxide, was used for precipitating the lead salt. The productof the reaction was boiled with water, the dissolved lead removed bysulphuretted hydrogen, and the crystals which separated out on cooling,were recrystallised from hot water.Di,,2eth?lZzlricacicEforms small obliqueprisms containing 1 molecule of water. From saturated solutions itsometimes separates at temperatures near 100" in thick prisms, pointedat both ends and anhydrous. The acid fuses only a t a high tempera-ture, with partial decomposition and sublimation. It dissolves in 200parts of boiling and 800 parts of cold water, scarcely at all in alcohol,ether, and glacial acetic acid. I t is easily taken up by concentratedsulpliuric and hydrochloric acids, and on dilution again cr.ystallises out.If the acid be dissolved in a little hot potash-solution arid alcohol beadded, the salt, K2C5( CH3),N4O3.4H20, precipitates in silky needles,very soluble in water, and not quite insoluble in alcohol.A similarsalt, N&C,( CH,),N40s.~H20, less soluhle in alcohol, is obtained byusing soda solution.BaC5(CH3),N4O3.3H2O, obtained by dissolving the acid in baryta-water, separates out on cooling in flat transparent prisms, soluble withdifficulty in cold water, more easily in hot.Ba[C,H(CH3)2N403]2 3H20 is obtaiced by boiling an aqueous solu-tion of the acid with barium carbonate, and precipitating with alcohol.The salts, NaC5H( CH3),N40,.2H20 and KC,H( CH:3)2N403.1+H20, mayhe prepared in a similar manner. By these salts the dimethyluric acidis well characterised as a bibasic acid. Heated a t 170" with concen-trated hydrochloric acid, the acid decomposes into carbon dioxide,ammonia, methylamine, and glycocine, according t o the equation :-CjH2(CH,)zNkO, + 5HzO = 3CO2 + NH3 + 2CHANHz + CZH5N02.The evidence thus obtained proves that the two hydrogen-atoms inthe uric acid, replaceable by metals, are directly combined with twodistiuct nitrogen-atoms.I f these two hydrogen-atoms be replaced bymethyl, then the two remaining hydrogen atoms can be exchanged formetals. This relationship finds a simple explanation only by theassumption that uric acid contains the group NH four times. Thisrequirement is expressed by two only of the various structural formuleNH.CO. C.NHproposed for uric acid, viz., by that of Medicus, I co .EH. C.NH/)I 'coyNH.C- NHN.HC-NHand by that of Fittig, CO< I >CO >CO.w. s.Action of Zinc Chloride on Methyl Alcohol. Hexmethyl-benzene. By LE REL and GREENE (Conzpt. reizd., 87, 26C).-The experiment was conducted in the same way as with butyl alcohol(Bull. Xoc. C'hinz., 1878, 29, 306). The principal products of theaction were marsh-gas, a crystalline body, water, methyl ether, andvarious oils. Traces of methaldelzyde, and of propylene, butylene, andother hydrocarbons were also formed. The crystalline body abovementioned amounts to about 0.5 per cent. of the alcohol employed.VOL. YXXVI. 50 ABSTRACTS OF CHEMICAL PAPERS.After purification from a trace of methaldehyde, oily matters, and avolatile chlorine compound, it forms laminae melting a t 150", andboiling a t 259-260" : it does not combine with bromine.I t s analysisleads to the formula c12HE16, and n comparison of the body and its com-pound with picric acid with specimens of hexmethylbenzene and itsOn Dinitroparadibromobenzenes and their Derivatives.By P. T. AUSTEN (Amer. J. Sci. [3). 16, 46). Third Paper.*--P-Dinitro~nrabromophenol, C6Hz(N 02),BrOH.-This compound is pre-pared by treating p-dinitroparadihromobenzene in dilute alcoholicsolution with potassium nitrite, and decomposing the resulting potas-sium salt with hydrochloric acid. It forms, when crystallised fromwater or alcohol, long, flat, very thin, glittering needles, melting at,71" (78" Korner), and volabilising unchanged when gently heated.Exposed to the air it turns red, probably owing to the presence ofammonia.Heated under water, it melts to a yellow oil. Heated withconcentrated sulphuric acid, it evolves nitrous acid, and forms a sul-phonic acid (?). On platinum foil, it burns with a luminous, yellow,smoky flame. When thrown on red-hot foil, it deflagrates. Heatedwith fuming nitric acid, it forms picric acid. It is difficultly solublein boiling water, still less so in boiling dilute hydrochloric andnitric acids ; easily soluble in boiling snlphuric acid ; very easily inhot alcohol, glacial acetic acid, and aniline; less so in carbon bisul-phide.Siher ,@-a initropurnbromophenate, C6H2(N02),BrOAg.-Splendid glit-tering red needles, with brilliant green reflex, difficultly soluble in hotwater, easily in alcohol.When dry, the salt deflagrates on heating ;thrown on a hot surface, it explodes. The potassium salt forms longglittering red needles, with greenish reflex. difficultly soluble in boilingwater. The barium salt, [C6H2(NOz)zBrO]2Ba, forms saffron-yellowneedles, moderately soluble in water and alcohol. Heated in a flask,it explodes, coverinq the sides with carbon. The ammonium saEtforms bright-red silky needles, soluble in boiling water and in alcohol.Volatile at 140" to a red sublimate ; above that temperature it is de-composed, partially recombining on cooling. The cnpper salt is ob-tained by treating with glacial acetic acid the product of the actionof cupric carbonate on the phenol in alcoholic solution, and dilutingwith water until the blue colour changes to brown; the salt thenseparates in short, brown glittering needles, insoluble in water andalcohol, moderately soluble in boilinc acetic acid.None of these saltscontain water of crystallisation, differing in this respect from thesalts of the isomeric dinitrobromophenol obtained by Armstrong (Ber.,6, 649). The formation of P-dinitroparabromophenol affords a con-venient method of separating ,@-dinitroparadibromobenzene from thea- and .y-compounds, which are unaffected by potassium nitrite.picrate, showed the two to be identical. c. w. w.c. w. w.Some Addition-products of Trinitrobenzene and otherNitro-compounds. By E. HEPP (Bull. SOC. Chin%. [2], 30, 4).-A* Compare this Journal, 1876, ii, 406 and 513ORGANIC CHEMISTRY.51solntion of tiinitrnbenzene in benzene deposits large prismatic crystals,which lose their benzene on exposure to the a i r ; they consist of acompound of 1 molecule of each of the constituents, C,H,(NO,), andC6H6. A similar compound with naphthalene forms long white needles,melting a t 152-153", and losing their naphthalene at the ordinarytemperature, or on recrystallisation from alrohol. Anthracene andphenanthrene appear to form similar compounds with trinitrobenzene.The compound with aniline, C,H3(NO,),.C6H,N, crystallises in redneedles melting a t 123-124", and is nearly insoluble in cold alcohol ;it might be used with advantage for the preparation of pure trinitro-benzene free from dinitrobenzene. The analogous compound withdimethylaniline melts a t 106-108".Both compounds are easily de-composed, either by exposure to the air, by washing with alcohol, orby dilute acids.By the action of aniline on an isomeric trinitrobenzene (from parw-dinitrobenzene, m. p. 171"), red needles melting a t 133" were ob-tained. Analysis led t'o the formula C6H3(N02)2NHC6H,, which is thatof a dinitrodiphenylamine. The alcoholic mother-liquors contained adiazo-amidobenzene, produced by the action of nitrous acid on theexcess of aniline.The addition-products of picramide with aniline obtained by theauthor differed from those described by Mertens, in that they lost tbewhole of t4heir base on exposure to the air. Ordinary trinitrotoluene(m. p. 82O) forms compounds exactly similar to those of t'rinitroben-zene.From this similarity between trinitrobenzene, trinitrotoluene, andpicric acid, the author supposes that the N02-groups are similarlysituated ; trinitromesitylene, however, which, according to this hypo-thesis, should form a compound with aniline, has as yet refused todo so.No componnd of aniline with a dinitro-compound has hitherto beenobtained, but compounds of these bodies with hydrocarbons are easilyformed. Ortho- and para-dinitrobenzene form crystallisable compoundswith naphthalene, the para-compound melting at 110-11 5".Action of Aniline on Glyoxylic Acid. By C. BOTTINGER(Deut. Chern. Qes. Ber., 11, 1-559-156l).-The yellow crystalline pre-cipitate, which is formed by slowly adding aniline to dilute glyoxylicacid, is an aniline salt of anilglyoxylic acid, C,aH,4N202.This bodywas also obtained by Frankland and Duppa, by adding aniline oxalateto calcium glyoxylate. It is decomposed by boiling water into aniline,carbon dioxide, and a brittle substance, which splits up on distillationc. w. w.into water, aniline, and carbanilide. w. c. w.Paraxylidine. By W. SCHAUMANN (Deut. Chem. Ges. Ber., 11,1537-1 538) .-Mononitroparaxylene (b. p. 234-237"), prepared fromparaxylene (m. p. 15", b. p. 136"), was reduced by acetic acid andiron filings, and the mixture distilled in a current of steam. Paraxp-lidine sulphate crystallised out on emporating the distillate withsalphuric acid. The free base was obtained by adding excess ofsodium carbonate to a solution of the sulphate, and distilling insteam.e 53 ABSTRACTS OF CHEMICAL PAPERS.Pai*axyZidine is a colourless liquid, which turns yellow on exposuret o the air.I t ssalts crystallise well from acid solutions, but their neutral solutionssplit up on boiling.ParaxylidiTze sukhate [ C6H3( CH3),NH2J2HZSO4, crystallises in colour-less plates. The hydrocldoride, C6H3.( CH3),NH,.HC1 + H,O, formslarge glistening plates, having a faint pink colour. It is more solublethan the sulphate. At 125-130', its water of crystallisation is ex-pelled, and the anhydrous salt sublimes.The xitrate, C6H3( CH3)2NH2.HNOJ, forms pink needle-shaped crys-tals.The ozalate forms thick prisms, having a pink colour. Onheating to 125-130", i t splits up into water and oxaZparaxyZidide[ C,H,( CH,)2NH]2C20,.This body is soluble in alcohol and in ether ;i t sublimes without melting at 125", forming slender silky-white needles.Acetoparazylidide (m. p. 138-139') separates out as a crystallinemass on boiling paraxylidine i n glacial acetic acid. It is converted into?ritracetoparazylide, CsH2( CH3),N0,NH.C2H30, by the action of fumingnitric acid. This nitro-compound is a yellow crystalline powderI t boils at 220-221", and is soluble in hot water.(m.p. 192"). IV. c. w.Oxidation of Sulphamidoxylene. By M. W. ILES and IRAREMSEN (Deut. Clienz. Ges. Ber., 11, 1326-1329).-Jacobsen (ibid.,11, 893) assumed that the authors' sulphaminetoluic acid was not apure product; but as they have obtained the acid crystallised inbeautiful long needles with constant melting point of 254.5-255'(corrwted), they consider his supposition to be unfounded.The oxy-acid obtained was also doubtless pure, and crystsllised in long lustrousneedles, m. p. 174-175", which is a little higher than Tiemann andSchotten found for their orthohomoparoxybenzoic acid. The twoacids are, however, said to be identical. Both contain half a mol. ofwater of crystallisation, both melt a t almost exactly the same tempera-ture, and neither gives any coloration with ferric chloride.If a mixture of the two sulphamidoxylenes be oxidised with thechromic acid mixture until the oil swimming on the solution hascatirely disappeared, a pure sulphaminemetatoluic acid is obtained(rn. p. 254*5-255", corrected).The product was always dissolved iiisqdinm carbonate and the solution evaporated to a small bulk. Oncooling some unaltered amide crystallised out. This was filtered o f f ,t ;ie filtrate diluted, and the acid precipitated by addition of hydro-chloric acid.It is not disputed that Jaoobsen has obtained an acid by oxidisingthe amide melting at 95-96", but the behaviour of this acid withchromic acid mixture must certainly be different from that of thesulphaminetoluic acid. That a mixture of isomeric xylene substitu-tion products can furnish a single compound on oxidation is a factIwetty well settled by other investigators.(1.) Nitroxylene, obtained by the direct action of nitric acid onxylene, yields a ni trotoluic acid.This nitrotoluic acid is ?hot oonverteii by chromic acid into a bibasicacid.After twice recrystallising it was pure.(Beilstein and Kreusler.ORGANIC CHERIISTRT.53(2.) Chlorosylene, obtained direct from xylene, yields a chlortoluicacid. (Vol lrath .)( 3 . ) Bromoxylene, obtained direct from xylene, yields a brointoluicacid. (Fittig, Ahrens, and Nattheides.)Researches are to be carried out as soon as possible to determine theconnection between the nitrotoluic acid (m. p. 203'), the bromotoluicacid (m. p. 205-206"), and the sulphaminemetatoluic acid. It isprobable that all these bodies are similarly constituted.Jncobsen contests the correctness of the conclusion that., because theamide contains a CH3-group in the ortho-position and a second in thepara-position with respect to the sulphamide- group, the productnecessarily furnishes a stable monobasic acid.However, it is wellknown that ortho-compounds behare in a peculiar manner towardschromic acid, and some observations show that they are more stablethan the isomeric compounds of the other groups.An error niade both by the authors and by Jacobsen is now corrected.The acid formed by oxidation of sulphsmiiietoluic acid with potas-sium permanganate is not sulphamineisophthalic acid, but sulpho-Oxidation of Metaxylenesulphamide. By 0. JACOBSEN (Deut.Chenz. Ges. Bey., 11, 1529--1533).--The author denies that the resultsof his experiments agree with those of Remsen (Ber., 11, 1328).Condensation-products of Tertiary Aromatic Bases. By 0.FISCHER (Deut.Chew. Ges. Bey., 11, 950-952).-1t has been shown inprevious papers that dimethylaniline reacts with benzaldehyde audwith furfural to form bodies having the respective formul~ C?,HZ6N?and Cz,Hz4N20. I n the present paper the author describes two newbodies of the same class.Dimethylaniline reacts with chloral in the manner indicatedby the equation C1,C.COH + 5C6H5N(CH3), = 3HC1 + H20 +(C,H,N(CH,)2),C.CHI(C6H,N(CH3),). The product, which must bcregarded as a substituted pentaphenylethane, crystallises in colourlessneedles. It yields by oxidation a blue colouring matter.A mixture of dimethylaniline and bemhydrol, when treated withphosphorus pentoxide, yields din?ethylnmidotri~hen~l~7~etharLe in nearlytheoretical amount. This body is a feeble base.It crystallises fromalcohol in colourless needles, which melt a t 132-133".isophthalic acid. This the authors conclusively prove. w. s.w. c. w.J. R.Cyanoguanidines. By 0. LANDGREBE (Deut. Clzem. Ges. Bey.,11, 973--978).-In a previous paper the author stated that dicyanodi-phenylguanidine reacts with aniline hydrochloride to form a basewhich he called P-clicyanotyiphenylpanidine. He has since found thatthe same base is formed also by the reactions of a-dicyanotriphenyl-guanidine with aniline and toluidine hydrochlorides. The base, unlikethe a-dic-janogiianidines, is not decomposed by boiling with alcoliolicpotash or soda, but when heated a t 100" for some hours in sealed tubes,i t is resolved into aniline, ammonia, oxalic acid, and carbon dioxide.P-Dicynnoditol?Jl~he~iylllutrnitli?2e.--This base is formed by the actionof aniline hydrochloride on dicyanoditolylguanidine. It crystallise34 ABSTRACTS OF CHEMICAL PAPERS.from alcohol and water in yellowish needles, having the formulaC2,H2,N, + $H20.The base dissolved in alcohol is converted by pro-longed boiling with hydrochloric acid into ditolylparabsnic acid. Ityields anorange-yellow amorphous platinum salt, 2(C2,H,,N5,HC1).PtC1,.p- Dicy m o t ritolylguanidin.e.-T h is s u hs tan ce is formed, together withditoly I parabanic acid, on boiling di cyan oditoly lguanidine with hydro-chloric acid. It crystallises irr pale-yellow needles, which melt at284". By prolonged boiling with alcohol and excess of hydrochloricacid it yields ditolylparabanic acid.By W.HEINTZ (Gebiq's Annalen, 193,68--77'L).-By boiling for some time a mixture of acid oxslate ofdiacetonamine, benzaldehyde and alcohol, the oxalate of benzaldi-acetonamine is formed, from which the free base can be obtained bytreatment with potash. The base separates as an oily layer, whichsolidifies on cooling. It dissolves readily in ether, crystallising there-from in large colourless prisms, and is soluble in alcohol, but withdifficulty in water. It melts a t 61*2", and boils a t 2N0, the distillateconsisting of the unaltered substance and another base, which is notvet investigated. Benzaldiacetonamine neutralises acids, forming well-&efined salts ; its formula is C,,H17N0.The nezh-a1 sulplmte, ( C1,H,,N0)2H2SO4, crystallises in small needles,which are easily soluble in hot and in cold water, but very difficultlysoluble in alcohol, and even more so in absolute alcohol.When it isagitated with ether, a portion of the base is removed and the aqueoussolution of the sulphate is rendered acid.The nitrate, CI,Hl,N0.HK03 (dried a t 105"), crystallises from waterin short prisms containing water of crystallisation, which they graduallylose on exposure to air.Neutrul oxulute, ( C,3H17NO)2C20~H2, is insoluble in alcohol and i nether, and soluble with difficulty in water, from which it crystallisesi n prisms. It dissolves more readily in water containing free oxnlicacid; from this solution it separates in crystals, which are un-distinguishable in properties from the neutral oxalate.Theliydrochloride, CrJH17N0.HC1 (dried at lOS"), and the platinum salt,( C13H17N0.HCI),.PtC14, have also been prepared. A. J. C.By B. RATHKE (Deut. C h m . Ges.Ber., 11, 958--962).-The potassium salt of this acid is formed onheating a mixture of aniline and carbon bisulphide with alcoholicpotash: CS, + NH,.C6H5 + KHO = C6H5.HN.C'S.SI( + H20.The same salt is formed, together with diphenylthiocarbamide andpotassium thiocarbonate, on heating an alcoholic solii tion of equalweights of molecule of aniline and potassium xanthate for somehours. The reactions that take place are reprebented thus :-J. R.Benzaldiacetonamine.Phenylthiocarbamic Acid.1. C,H,O.CS.SK + NH,.C,H, = C,H,.KH.CS.SK + C,H,OH.2.C,H,O.CS.SK + e(NHZ.CGH5) = (C,H5NH),CS + CZHSOH +3. CZH5O.CS.SK + KHS = (SK)ZCS + CZHSOH.KHSPotassium ph..nylthiocarbarnate, when pure, forms transparenuRQANIO CHEMISTRY. 55golden-yellow monoclinic crystals, which melt in their water ofcrystallisation below 70". I t dissolves in less than its own weight ofcold water. The solution becomes turbid when heated, owing t o theseparation of diphenylthiocal.bnmide and phenylthiocarbimide. Thisand all the other reactions of' the acid and its salts are explained bythe circumstance that the acid readily breaks up, according to theconditions, in one or other of the ways indicated by the two followingequations :-C6H5.NH.CS.SH = CSN.C6H5 + HzS;C,H,.HN.CS.SH = NH,.CtjH5 + CSZ.The phenylthiocarbimide and aniline thus produced further react toform diphenylthiocarbamide.Potassium phenylthiocarbamate undergoes decomposit,ion in theair.Its solution, when boiled with cupric sulphate, yields cupricsulphide and phenylthiocarhimide. The aqueous solution dissolves alarge quantity of aniline, forming it liquid which, when boiled, givesoff bydrogen sulphide and deposits diphenylthiocarbamide.Free p henylthiocarbamic acid cannot be obtained by acidifying thepotassium salt, because i t breaks up a t once into carbon bisulphideand aniline, as shown above. J. R.Pentabromoresorcin. By R. BENEDIKT (Bed. Chem. Ges. Ber.,11, 1559) .-Aniline acts on pentabromoresorcin, forming tribrom-aniline and tribromoresorcin, 3C,Br5H0, + 2C6H5.NH, + 3C6Br,H30, + '2C6HzBr3.NH,.Under similar conditions phenol forms tribromo-phenol.Tin and hydrochloric acid reduce pentabromoresorcin, first to tribro-moresorcin and then to resorcin. Liebcrmnnn's tribromoresorquinone isreduced to tetrabromodiresorcin, ( OH),HBr,C6.C6Br,H (OH),, whichcrystallises in pink needles. It is reduced by sodium amalgam, form-ing an amorphous body free from bromiue; this yields diphenyl ondistilhition over zinc-dust. w. c. w.Fluorescein-carbonic Acid. By J. SCHREDER (Deut. Chenz. Ges.Ber., 11, 1340-1344) .-Baeyer's beautiful method of forming con-densation-products from phthalic acid and phenols, is founded o u theproperty of phthalic acid to form an auhydride, which afterwardsenters into reaction with hydroxjbenzenes.It was to be assumed a tthe outset that acids with neighbowing carboxyl-groups would con-duct themselves similarly, and in fact this was found the case withoxyphthdic and pyromellitic acid without, in the first case, the oxg-group prejudicing the reaction. It was of interest to see if trimelliticacid, which is a 1 : 2 : 3 derivative (G. Krinos), would behave in asimilar manner. Trimelli tic acid prepared from colophony, was con-verted into the anhydride and fused with resorcin a t 'LOO", and in t h i sway a body very similar to fluorescein was obtained, dieering only byhaving an extra carboxyl-group in its composition, and hence namedtluoresce'in-carbonic acid. The product is a dry red-brown mass ofconchoidal fracture, which may be purified by boiling it with waterand solution and fractional precipitation from alcohol.When dry i56 ABSTRACTS OF CHEMICAL PAPERS.formed a light-yellow amorphous powder.boxylised fluorescein, Cz1H12O7, or C6H3( CO. OH) <Analysis showed a car-CO.(=,H3(0H) >o. ItGO. CGHs( 0 H)is very sparingly soluble in boiling water and glacial-ackc akd, butvery easily in alcohol, ether, and benzene. The barium and calciumsalts were also prepared. The intention was, by boiling it with thecarbonates of barium and calcium, to replace only the hydrogen of thecarboxyl-group by metal, but it was found that both the hydroxylhydrogens were replaced.Bwium Salt.-A blood-red solution was obtained by boiling fluo-resceh-carbonic acid with excess of barium carbonate for a long time.This solution could not be crystallised. The concentrated aqueoussolution was precipitated with alcohol, and the barium salt obtained inthe form of a beautiful orange-red amorphous powder.Calcium Salt.-Brown-red amorphous powder, prepared like thebarium salt. Both salts are very soluble in water, and on evaporationof their solutions are obtained as cantharides-green amorphous masses.The above-named remarkable behaviour of' the two hydroxyl hydro-gens caused the author to investigate Baeyer's fluoresce'in in the samedirection.Baeyer says fluorescein dissolves in lime- and baryta-waterwith a red colour. The author finds that it further decomposes thecarbonates of barium and calcium, furnishing compounds in whichboth hydroxyl-hydrogens are replaced by metal.Although apparentlystronger, fluorescein also, although containing no carhoxyl-group,furnishes these salt-like compounds much more easily than the newbody with the carboxyl-group.Barium, Salt of Fluorescein, CzoHloBaOj + 9H20, prepared like thatof the carboxylised fluorescein, is a carmine-red powder, which afterrecrystallising from water is obtained in beautiful 1eaEy crystals, con-taining 9 mols. of water.Culcium Salt, CZOH,,CaO5 + 4Hz0.-Slender needles. Prepared likethe barium salt.Acetyl-yroduct, C 2 ~ ~ 1 6 0 9 . - ~ ~ ~ o r e s c e ~ n - c c c r b ~ n ~ ~ acid was heated withacetic anhydride (5 parts) for 2-3 hours with inverted condenser,and the product treated with alcohol and left forabout 12 hours.Thesolution, poured off from the brown oily drops which had separated,was treated with water, which precipitated acetyl-products as bright-yellow flocks. No salt of this product could be prepared, fluorescein-carbonic acid being regenerated.Dibromofiworescezn - carbonic Acid.-Fluorescehcarbonic acid sus-pended in glacial acetic acid, dissolves on adding the proper quantityof bromine, and the solution soon solidifies to it crystalline paste.The product, recrystallised from glacial acetic acid, forms beautifulbrick-red needles, soluble in alkaline fluids to yellow solution.Tetrabromo$uorescein,-carbonic Acid.-Prepared like the dibromo-pro-duct, only using double the quantity of bromine. d dark-reddishsolution, showing no inclination to crystallise, was obtained.Thebromine-derivative was therefore precipitated with water. It is a darkorange-red amorphous powder, showing colour reactions with alkalisundistinguishable from those with eosin.Red-brown colour with green reflectionORGANIC CHEMISTRY. 57Potassium Salt.--Excess of the acid was treated with potash solu-tion, evaporated, and the concentrated solution treated with alcohol,whereby the salt was obtained in small needles with cantharides lustre.It is undistinguishable from eosin-potassium, and dyes like it. Thereduction of the fluorescein-carbonic acid with sodium-amalgam didnot succeed, for a yellow varnish-like mass easily soluble in alcoholmas obtained. The solution brought in contact with alkalis a t onceoxidises and regenerates the original body.This oxidation takes placepartially, even on evaporating the soliition on the water-bath. w. s.Trinitroso- and Trinitro - phloroglucin. By R. BENEDIKT(Deut. Chem. G'es. Ber., 11, 1374--1378).-The discovery of dinitroso-resorcin by Fitz, and of dinitroso-orcin by Stenhouse and Groves, madethe existence of the corresponding phloroglucin-derivative highlyprobable. On adding a concentrated well-cooled solution of potassiumnitrite to a solution of plrloroglucin in dilute acetic acid covered witha layer of ether, the mixture becomes dark-brown, and after someminutes an acid potassium salt begins to separate. On supersaturatingthe solution with potassium hydroxide, and adding alcohol, the neutralpotassium salt is thrown down in beautiful green needles amountingto about 70 per cent.of the theoretical yield. As this potassium trini-troso-phloroglucin, C,( NO),(OK),, cannot be recrystallised withoutgreat loss, it must be dissolved in water and precipitated with alcohol,to which some potassium hydroxide has been added. It is easily solublein water, with difficulty in dilute potash, quite insoluble in weakalcohol. It may be heated to above 1SO" without decomposition,but explodes a t a high temperature. A drop of sulphuric or nitricacid will also occasion violent explosion. A lead salt of trinitroeo-phloroglucin is obtained by precipitating n dilute solution of the potas-sium salt with lead acetate ; it falls as a yellolv precipitate. Whendried it forms a light cinnamon-brown powder, exploding with vio-lence when heated.Nitroso-phloroglucin can be isolated by cautiousdecomposition of the lead salt mixed with alcohol, by means of sul-phuric acid. On filtering and evaporating the alcoholic solutiongroups of needles are obtained, which are easily soluble in water andalcohol, insoluble in ether.There is a law recogriised already in relation to the number ofnitroso-groups in nitroso-derivatives of the phenols, although thenumber a t present known is so small, viz., that each hydroxyl-groupappears to render easier the admission of a nitroso-group. Into thehydrocarbons (benzene and naphthalene) NO is introduced only withdifficulty and by indirect means.The monhydric phenols, phenol, thymol, and naphthol, take upone NO-group with ease.The dihydric phenols, resorcin and orcin, give dinitroso-derivatives.The trihydric, phloroglucin phenol, yields trinitroso-phloroglucin.Trinitro-ph,ZorogZucin, C,( NOz),( OH), + HzO.-On adding powderedpotassium nitroso-phloroglucin in very small quantities at a time to amixture of nitric acid and sulphuric acid, oxidation takes place a t theordinary temperature, and finally yellow needles of trinitro-phloro-glucin separate out. The mass is then diluted with water, exhauste58 A4BSTRhCTY OF CHEMICAL PAPERS.with ether, and the product recrystallised from boiling water.Thecrystalline form is the hexagonal prisrn modified by combination withthe pyramid and prism of the second order, expressed by the formulacDP,P, OOP,.At 130" it begins tosublime; a t 158" it melts without decomposition, but explodes onfurther heating.It is easily soluble in hot water, alcohol, and ether,and is decomposed bysulphuric acid only a t a hightemperature. Likepicric acid, it possesses great tinctorial power f o r animal matters, butthe tint is richer and more beautiful. Trinitro-phloroglucin gives theisopurpuric acid reaction with potassium cyanide. On reduction withhydrogen sulphide or tin and hydrochloric acid, it appears to form thecompound analogous to picramic acid. On boiling the tin solution i tbecomes decolorised, but no triamido-phloroglucin compound could beobtained.Salts of Tr ;nitro-ph ZowgZucin.-Triaitro-phloroglucin decomposes car-bonates readily, and forms with metals three series of salts containing1, 2, and 3 equivalents of metal.The potassium salts are formed by saturating 2 molecules of thenitro-compound with 1, 2, or 3 molecules of potassium carbonate.Itis necessary to work with a solution as concentrated as possible. Thecompound C6(N02),( OK),, consists of orange-red shining needles oftenan inch long, whilst C6(N02)3(OK)20H is of a deep-yellow colour, andnot so shining as the preceding. The cornpound C6(N02)3( OK) (OH), +H2O forms long, silky, sulphur-yellow needles, losing water at loo",and becoming dull.All three potassium derivatives are sparingly soluble in cold water.The neutral ammonium derivative behaves like the correspondingpotassium compound. The barium compound formed by addingbaryta-water to an aqueous solution of trinitro-p hloroglucin, consistsof microscopically small, sulphur-yellow needles, insoluble in cold orboiling water.Lead acetate gives in an aqueous solution of the acid an amorphous,This body loses its crystalline water a t 100".All are explosive.flocculent precipitate of lead trinitro-phloroglucin. w.s.Aurin. By R. S. DALE and C. SCHORLEMMER (Dezd. Chem. Ges.Uer., 11, 1556).-Aurin is formed, together with formic acid, on heat-ing a mixture of oxalic acid and phenolsulphonic acid or bariumphenolsulphonate, or by gradually adding oxalic acid to a mixture ofsulphuric acid and excess of phenol. Srriall quantities of carbonmonoxide and carbon dioxide are evolved during the process : 3C6H60 + CzHZO, = CigHIAOA + CH2O2 + 2H20.w. c. w.Aurin. By C. ZULKOWSKP (Liebig's Annnlen, 194, 109-144).-The preparation of aurin, and several of the results described in thispaper, have already appeared in the Deut. C'hmi. GM. Ber., 10 and 11,and in this Journal in abstract. Aurin contains 70 per cent. ofpeudorosolic acid. This body separates out as an amorphous resinousmass on treating commercial aurin with sodium bisulphite and dilnt-ing the product with water. On adding strong hydrochloric acid tothe filtrate from the pseudorosolic acid, and heating the mixture tORGANIC CHEMISTRY. 5980", a crystalline precipitate is obtained, which gives off sulphur di-oxide when heated to 130". By carefully crystallising the alcoholicsolution of t h i s residue, the following substances can be obtained, viz.,two homologous rosolic acids, ClgHl1O3 and c2DIi1603 ; lencorosolicacid, C20H1803 ; and a compound having the composition C,nH1606.RosoZic acid, CZOH1603, dissolves in alcohol, forming a reddish-yellowsolution, which changes to carmine on the addition of alkalis.Thealcoholic solution deposits crystals containing 1 molecule of water,which belong to the rnonoclinic or triclinic systems. The crystalsappear dark-red by transmitted, and metallic-green by reflected light.They easily lose their water of crjstallisation a t 100". On boiling thealcoholic solution of rosolic acid with zinc-dust and acetic acid, le'zico-msolic acid, C,,H 180s, is obtained in the form of pale-yellow, anhydrousrliombic crystals.Rosolic acid, C1gH1603, crystallises in anhydrous, rhombic plates,possessing a gnraet-red colour with a bluish lustre. The leuco-pro-duct of this acid has the composition CI9Hl6O3.The compound ~ l , ~ 1 6 0 6 is a derivative of the red roscilic acid,CISHl4O3.It crystallises in violet, needle-shaped crystals, which dis-solve in alcohol, forming a brownish-yellow solution. The alcoholicsolution becomes carmine-coloured on the addition of alkalis ; whenboiled with zinc-dust and acetic acid it yields the leuco-compound cl9HI6o3, identical with the leuco-derivative of red rosolic acid. Theproperties of yseudorosozic acid have been previously described ( Uer.,loc. cit.). w. c . w.Rosolic Acids. By H. CARO and C. GRAEBE (Deut.Cliem. Ges.Ber., 11, 13~8-13jl).-Fom,aat~~t~, of DzozybHnxoi,lie?Lorie f rona Aurin.-Aurin was heated with water a.t 220-'25U0, and a colourless compoundwas thus obtained which appeared to be identical with the dioxydi-Fhrnyl-ketone of Staedel and Gail, and to which the formula co(c6H4.0H)2 is ascribed. The authors have analyscd the dioxy-compound, a i d also its acetyl- and benzoyl-ether, and found nnmbeiswhich exactly correspond with those for dioxybenzophenone and itsether. Complet,e agreement of properties was also found to existbetween the above-named colourless body and that obtained by Baeyer.and Burkhardt by the action of potassium hydrate on yhenol-phtha-lei'n, and which is also dioxybenzoplienone. Besides the coiivertibilityinto aurin, the dioxybenzophenone from either diphenylmethaiie,phthalein, or from aurin exhibits the following colour reactions.Ifsodium amalgam be added to a dilute cold aqueous solution of thedioxybenzophenone, no coloration occurs, but if the alkaline fluidpoured off fkom the sodium stmalgam be heated to boiling, a beantifulred coloration appears, which disappe:trs on cooling, and can be re-produced by again warming. The absorption spectrum of the verydilute red solution shows a strong dark band in the green. On add-ing hydrochloric acid to the colourless rednction fluid, it becomesorange-yellow, and on boiling, an orange-yellow precipitate sepa-rates, which dissolves in soda solution with violet - blue colour,and is decoloriBed by excess of the alkaline solution, This isin entire agreemeit with the observations of Baeyer and Burk60 ABSTRACTS OF CKEMICAL PAPERS.hnrdt.On heating aurin with water, besides dioxybenzophenone andcarbonised decomposi t,ion-products, phenol was formed. The reactionis explained in the following equation, and according to the new aurinformula :-,CJ&' 0(CGH,.OH),C I + H,O = CO(C,H,.OH), + CsH,.OH.Synthesis qf Auriiz from Dioxybenzop7xnone.-It was thought probablethat aurin might be formed from dioxybenzophenone and phenol. Thisdid not succeed directly, but it was successful through the mediu'm ofphosphorus trichloride. Dioxybenzophenone was heated for a shorttime with phosphorus trichloride, the excess evaporated off on thewater-bath, and, after cooling, phenol and some concentrated sulphuricacid added.An evolution of hydrochloric acid begins even in thecold, and the mass becomes yellowish-red. By heating on the water-bath or a t 140" the reaction is completed after a short time, and onadding water, aurin separates out. Chlorinated bye-products arcformed at the same time. The relations manifested by the de-composition and synthesis of aurin to dioxybenzophenone, which, ac-cording to the researches of Stadel and Beck most probably containsboth hydroxyl groups in the para-position, indicate that in aurin bothhydroxyl groups, and in rosaniline both amido groups, are also in thepara-position. That the third oxygen atom in aurin and the imidogroup in rosaniline most likely take the ortho-position, the formationof rosaniline from orthotoluidine, and a rosolic acid from salicylicaldehyde testify.The latter compound, according to the results ofLiebermann and Schwarz, is probably ident'ical with aurin. The violetbody formed from iodo-dimethaniline (Weber) is against this theory,however, as here one must assume that all three nitrogen atoms are inthe same position.Formation of it Colouring Matter from Jfonozybenzopheitone a dPhenol.-The oxybenzophenone of Dobner and Stackmann was heatedwith phosphorus trichloride, and then with phenol and sulphuricacid. On treahment with water, a resin separated out, which in appear-ance resembles crude corallin. This resin contains a colouringmatter, and its properties place it in the group of the rosolic acids.By solution in soda and precipitation with sulphurous acid, it is puri-fied, and then forms an orange-red powder which fuses under water tloa red-brown resin with green lustre.It dissolves in alkalis with aless intense violet-red than phenol-phthalein. The solutions graduallydecolorise. With alkaline hydrogen sulphites it forms colourless solu-tions, and it combines with hydrocyanic acid like rosolic acid. Theauthors believe from these observations that this compound is a rosolicC,H,acid, (C6H,)(C,H,.0H)C< I It is considered very probable that0Dobner and Stackmann had this substance in their hands when theyacted with phenol upon benzotrichloride, and that it was actually con-tained in the red-brown resin which they describe in their paper asthe product of the reaction.On repeating their experiments theORQANIO CHEMISTRY. 61authors obtained a coloaring matter on treatment with hydrogensodium sulphite, the properties of which agree with those of theReduction of Acetophenone. By K. BUCHKA (Deut. Chem Ges.Ber., 11, 1550--1551).-By the action of sodium amalgam on aceto-phenone, Emmerling and Engler obtained a pinacofie boiling a t 202",and a secondary ethyl benzene alcohol, whilst the author by the samereaction obtained only pinacone. The author considers that the lowboiling point of the pinacone is probably due to its splitting up intoequal molecules of acetophenone and the secondary alcohol.compound from oxybenzophenone. w. s.w. c. w.A Sulphuretted Derivative of Acetophenone.By C. ENGLER( D e d . Chem. Ges. Ber., 11, 930).-Acetophe1ione reacts with ammo-ninm sulphide and hydrogen sulphide in alcoholic solution to form abody which the author regards as thiacetop7~eitone or a polymeride of it.This substance crystallises from alcohol in colourless or yellowishlamina, which are insoluble in water, but soluble in ether, chloroform,and benzene. It melts a t 119.5", and sublimes in feathery crystalsexhibiting a bluish iridescence. J. R.Sulphuretted Derivatives of Benzophenone. By C. ENGLER(Deut. Chem. Ges. Ber., 11, 922-926).-1. When alcoholic solutionsof benzophenone and ammonium sulphide are mixed together andsaturated with hydrogen sulphide, the following reactions takeplace slowly: C6&.CO.C6& + H2S = C6H5.CS.C6H5 + H20; andThe product is a solid substance crystallising from alcohol in snow-white needles, which melt a t 151".It is identical with the bodywhich A. Behr (Ber., v, 970) obtained by the action of alcoholic potas-sium sulphydrate on benzophenone chloride.2. The mother-liquors of the above substance, as prepared byBehr's reaction, Field by further treatment a.nother body which crys-talliees in small white needles (m. p. 146.5"), and has the compositionof thiobenxopheizoiie, C6H5.C S .C6H5.Both these compounds, when cautiously oxidised with chromicacid, yield benzophenone and no intermediate product.3. Benzhydrol reacts with phosphorus pentasulphide to form thecrystalline compound melting a t 151" described above, and an oily body,which by treatment with mercuric oxide or chloride yields the corn-pound [ ( C6H5),CH.S]&.Dibromo-metaxylene-sulphonic Acid. B y 0. JACORSEN andE. WEINBERG (Deut. C'llem. Ges. Her., 11, 1534--1536).-~d~rorno-Inetax2/lene-sul~~~oizic acid, C6HBr2( CH,),SO,H, separates out in smallanhydrous scales when water is added to a solution of dibromo-meta-xj-lene (m. p. 72") in fuming sulphuric acid. The crystals melt a t16J", and are soluble in hot, sparingly soluble in cold water. Thebcxriim salt [ C6HBr,( CH:3)zS03]2Ba, is sparingly soluble in water.CGHBrZ( CH,),SO,PU'a + 2Hz0 forms colourless pearly scales, soluble in2(C6H,.CS.CeH5) + HZS = (C,H5),CH.Sz.CH(CtjH,)z + S.J. RG2 ABSTRACTS OF CHEMICAL PAPERS.hot, and almost insoluble in cold water.The acid chloride,C,HBr,( CH,),SO,Cl, crystallises in coloiirless rhombic plates, whichmelt a t 107". The amide, CsHBrz(CH3)zS0zNH2, forms woollyneedles, insoluble in absolute alcohol ; they melt a t 220', and begin todecompose a t 230".A mixture of 6-metaxglene-sulphamide (m. p. 96') and monobromo-8-metaxylene-sulphamide (m. p. 161") is formed by treating the pro-duct, of the action of sodium-amalgam on sodium dibromo-metn-xylene-sulphonate with phosphorus pentachloride and ammonia. Themonobromo-metaxylene-sulphamide crystallises from dilute alcohol o rfrom hot water in long flexiblc needles. The relation between dibromo-metaxylene-sulphonic acid and the allied xylene derivatives is shownby the following formulse :-B-Metaxylene-sulphonic acid.Monobromo-t9-xylene-su!phonic acid.C,H3(CH,) (SOBH) (CH3) (1 : 2 : 3). C6Hs(CH3) (S03H) (CH3\Br(l : 2 : 3 : 6).M.p. of amide.. 9 6 O . 161".Dibromo-j3-metaxplene-sulphonic mid.C,H(C&) (SOBH) (CH,) (Br2(l : 2 : 3 : 4 : 6).M.p. of amide . . 220".a-Metaxylene-sulphonic acid. Monobromo-a-xylene-sulphonic acid.C6H3(CH3)(S0,H)CH3.(1 : 3 : 4). C6H2(C&)(S0,H)(CH,)Br.(1 : 3 : 4 : 6).M.p. of amide . . 137". 194". w. c. w.Oxidation of Ditolylparabanic Acid. By 0. LANDGREBE(Deut. Chew?. Ges. Ber., 11, 978).--By the oxidation of ditolylpnrabanicacid, Nz( CO) ( Czoz) ( C~H*.CH,)Z, with potassium permanganate, theauthor has obtained an acid agreeing in composition with the formulaN2( CO) (C,O,) ( C,H,.COOH)z.The potassium salt of this acid dis-solves easily in water, sparingly in alcohol, and gives crystalline pre-cipitates with salts of the alkaline earths and heavy metals.J. R.Parachlorobenzyl Chloride and Bromide. By C. L. JACK-SON and A. W. FIELD (Deut. flhern. Ges. Ber., 11, 904).-The sub-stance described as parachlorobenzyl chloride has hitherto beenprepared from the chlorotoluene obtained by the direct action of chlo-rine 011 toluene in the cold. But this last product has been shown byHiibner and Majert ( B e y . , 6, 790) to be a mixture of ortho- and para-chlorotoluene. The authors have therefore prepared paraehlorobenzylchloride from pure parachlorotoluene, and find that it is not a liquid,as was formerly thought, but a solid substance.It crystnllises inwhite brilliant needles or prisms, having a pleasant aromatic odonr.It melts a t 29", and volatilises a t common temperatures. The vapouracts violently on the mucous membranes. Ether, benzene, carbon bi-sulphide, acetic acid, and warm alcohol dissolve i t easily. It is in-soluble in water, and when boiled therewith, it is resolved into para-chlorobenzyl alcohol and hydrogen chloride.Puracl~lorobenzyl bromide, C6&C1.CH2Br, similarly prepared, melts a t48-5", and resembles the chIoride in propcrtiea. J. RORGANIC CHEMISTRY. 63Vapour-density of Indigo. By E. v. SOMMARUGA ( n e d . Chein.Ges. Rer., 11, 1355--1356).-After his investigation on the action ofammonia on isatin, whereby he was led to the conclusion that thisbody possessed the formula C16H10N204, the author determined thevapour-density of indigo by Hnbermann's modification of Dumas'method.As a mean of nine determinations he obtained the number9.45, whilst the formula C16H10N,02 requires 9.06. Isatin is totallyAction of Ammonia on Isatin. (11.) By E. v. SOMMARUGA(Liebig's Annlrlen, 194, 85--108).-The author has proved quantita-tively that the action of ammonia on isatin under pressure may berepresented by the following equations :-decomposed before it can be vaporised. w. s.1. C16H,"N,Or + 2NH3= 2H20 + C16H12N4Oz.Isatin. isat in-diamide.2. 4'ClfiH10NzOr 4- 7NH3 7HzO + CI~H,*N~O, -+ 3C16Hi,N302.Isatin. Oxjdiimido- Desnxyimido-Derivatives of Diamido-isatin.-In addition to the salts, which havebeen previously described (Amalen, 190, 367-4384?), the author ob-tained the chromate, C16H12N40z.HzCr0d, as an orange-coloured powder,by boiling a solution of the sulphate wit'h potassium dichromate.Bythe action of sodium-amalgam on diamido-isatin, the sodium salt ofdihydro-isatinamide is obtained in long colourless crystals, which aresparingly soluble in cold water: C,6H,2N402 + HzO + H, = NH, +Cl8Hl3NJO3. The potassium salt resembles that of sodium. The freebase is deposited from an alcoholic solution in colourless needles(m. p. 2 1 3 O ) , which are sparingly soluble i n ether and in water, Di-amido-isatin is not acted on by zinc and sulphuric acid, and is withdifficulty re:?uced by tin and hydrochloric acid.Ox diimid 0- diamido-isatin, c I6H ,1N60 8.-The sul p h at e and nitrateof this base are crystalline salts. Their solutions are fluorescent. Thenitroso-compound has not yet been obtained in a state of purity.Dianaido-hydridic acid, CI6Hl"N2(OH)?( NHZ),, is obtained in granu-lar crystals by boiling the base with sodium-amalgam and neutralisingthe product with sulphuric acid. This acid melts a t 215-217", withpartial decomposition. It is oxidised by a mixture of sulphuric acidand potassium dichromate, forming diimido-hydrindin-carbonic acid,Cl6H1,N4O4, which crystallises from hot water in colourless glisteningneedles.Deoxyimido-isatin is not reduced by sodium amalgam, but is con-verted into the sodium salt of oxya?izido-7Lydr.oi.s.atin. The samechange takes place on boiling amido-isatin with alkalis, C,,HI,N,0, +HzO = Cl6HI3N,O3.On adding sulphuric acid to the sodium .salt,oxyamido-hydro-isatin sepxrates out as a yellow flocculent precipitate,which is soluble in hot water, in alkalis, and in acids.According to the author, the existence of the above compoundsshows that the molecules of isstin and of indigo contain 16 atomsof carbon. The following formuh are proposed €or these bodies andtheir derivatives :-diamido-isatin. isatin64 ABSTRACTS O F CHEMICAL PAPERS.Indigo-white.On Diphenol.Isatin. Diamido-is Itin.B.y L. BARTH and J. SCHREDER (Deut. Chew,.Ges. Ber., 11, 1332---1339).-By the action of fused potash on phenol,salicylic acid, oxybeczoic acid, and diphenol, C,,H,,02, are formed.The latter body began to crystallise after standing for some weeks,and was distilled in a vacuum : the greater portion passed over undera pressure of about 150 mm.between 310-330", and became a hardcrystalline mass, in which two different crystalline forms were easilyperceptible, viz., long thin needles and scales. This was dissolved in alarge quantity of boiling water, and the very dilute solution (whichdid not become turbid on cooling) was partly precipitated with leadacetate, the dark brown flocks removed, and the filtrate completelyprecipitated with lead acetate ; and the bulky white precipitatedecomposed with hydrogen snlphide. The solution exhausted withether yielded, after evaporation, an oil which solidified. This was care-fully crystallised from boiling water.The crystals obtained were mostclearly of two different forms. No method of separation by meansof solvents or precipitants, could be discovered, but by fractionalcrystallisation from water, a separation could be effected, althoughwith much trouble. The body crystallking in needles was thus ob-tained in some considerable quantity ; but only enough of the scalybody to enable the authors t o study its chemical characteristics. Thebulk remained behind, a, mixture defying further separation. Theneedle-shaped body was found to be the most soluble in water, butcrystallised out first owing to its preponderating quantity.The less soluble substance crystallises in small glittering scales. Bothhave the same formula, C12H1002,and are isomeric diphenols.The needle-shaped compound was designated a-diphenol, the other ,tI-diphenol.a-Diphewol, Cl,Hlo02.-Soluble in water, and easily so in alcohol,ether. chloroform, benzene, &c. Its aqueous solution gives with ferricchloride a pure cornflower-blue coloration, remaining unaltered fora week. Addition of sodium carbonate destroys the colour, andon heating, a red-brown precipitate separates, which however doesnot consist of ferric oxide. In water the diphenol melt,s below 100" ;heated alone it melts at 123". It crystallises anhydrous, and thORGANIC C€IEMISTHY. G5vnpour-density by Victor Meyer's method was found to be 6-40 ; caJ-culated 6.44. By distillation with zinc-dust it gave a very richyield of diphenyl (over 70 per cent.).Heated for some hours a tiSO", with potash and methyl iodide and some methyl alcohol insealed tubes, it yielded dianisoil.a-ni~heizol-sul~~honic acid, Cl2H8(HSO3),O,. a-Diphenol warmedwith sulphuric acid in a platinum dish until the vapours of the acidbegan to be given off , and the mass became reddish-brown, solidified oncooling to a granular crystalline mass. It dissolved very easily in coldwater. Treatment with lead or barium carbonates in the ordinaryway to remove excess of sulphuric acid is inadmissible, since thesulpho-acid itself forms almost insoluble salts with these metals. Itis best to add approximately calculated quantities of lead carbunate,and after separating the traces of dissolved lend by hydrogen sul-phide, to concentrate to a syrups consistence.I n the exsiccator thesyrupy solution solidities to a light grey crystalline mass. The acidis extremely soluble in water. At 110" it is decomposed, turningbrown, and becoming a varnish like and very hygroscopic mass. Thisdecomposition takes place in the air a t 100" after long drying.Analysis showed that the body was a disulpho-acid, C,2H8(HS03)202.The sodium salt, Cl2H,Na2S2Os + 2H,O, obtained by exactlysaturating the sulphoacid with sodium carbonate, separates in finestellate groups of needles. The water of crystallisation is driven offat 200".Sodium determinations made on crystals obtained by further con-centration of the mother-liquor gave a smaller amount of sodium. Thisobservation &as made in the case of the other salts, and indicates thata portion of the sulpho-group becomes split up on concentrating theaqueous solution. The potassium salt crystallises likewise in needleswith one molecule of water. The barium salt is obtained as a crys-talline precipitate, by decomposing the potassium or sodium salt wif hbarium chloride.The crystallisation-water could not be exactly esti-mated.Diyyrocntechin, C1?H1004.-If the potassium salt of the disulpho-acidbe heated with excess of potash, the fused mass gradually becomesyellow, and on acidifying liberates sulphurous oxide freely. Theether extract obtained in the usual way yields a brownish crystallinemass, consisting of fine interlaced needles, which easily decompose incontact with the air.It was only by sublimation in a stream ofhydrogen, that a small quantity was obtained as a colourless crystal-line sublimate ; the greater portion was, however, decomposed, remain-ing behind as a blackish-brown syrup. The melting point of tlie sub-limate was 84". I t s aqueous solution gave a bright green colourreaction with ferric chloride, which on addition of very little dilutesodium carbonate solution becomes dark blue, on further additionviolet, and finally red. This reaction is the same as that of pyro-catechin, only the first green coloration is brighter. The namedipyrocatechin was chosen in order to recall its formula and tlieanalogous colour reactions.The colour of the unsublimed product which was analysed, wasthe same (with ferric chloride and sodium carbonate), oiily theVOL.XSSVL. 66 ABSTRACTS OF CHEMICAL PAPERS.green had a shade of brown in it. The reaction is so delicate, thatmere traces can be detected. The blue and violet shades are especiallyintense.In water it israther sparingly soluble, and does not fuse therein sooner than thea-diphenol. The aqueous solution gives a bright green colour withferric chloride. After some time the clear solution becomes turbid,and green flocks separate, leaving the solution colourless. With othersolvents it behaves just like the a-diphenol. On distilling with zinc-dust, diphenyl is obtained abundantly. It melts a t 190", is anhydrous,and its vnpour-density (Victor Meyer's method) was found to be 6-39 for6.44 (calculated). Just as with a-diphenol, a dianisoil was obtainedfrom the /3-diphenol.This dianiso'il solidified in a short time after dis-tillation, forming a crystalline mass. Under the microscope octahedrawere readily distinguished. The boiling point could not be estimatedas the quantity was too small. The authors have proved qualitativelythat a number of interesting derivatives may be obtained from both thediphenols, if only a good method of separating these isomerides couldbe discovered.Dlp72en~Zbenzene.-The residue left on distilling the crude diphenolunder diminished pressure was distilled at a higher temperature. Adark yellow mass resembling rosin was obtained, whilst some carbonremained in the retort. The distillate was repeatedly boiled up withwater, whereby some a- and e-diphenol were separated.The exhaustedresidue of dark brown colour was mixed with zinc-dust and distilledin a stream of hydrogen, to ascertain if i t still contained diphcnol o rperhaps a higher condensed product. The product was a yellowish-brown semi-solid mass smelling of diphenyl, and yielding diphenyl asa sublimate on warming on the water-bath and passing a stream ofhydrogen over it : the dark residue, when distilled, furnished a yellowishoil which crystallised on cooling. This body was almost entirely solublein boiling alcohol, which deposited i t on cooling in white crystallineflocks (m. p. = 206"). Vapour density (Victor Meyer) = 7-70 ; cal-culated for Cl,H14 = 7.94. Thus the body is a diphenylbenzene, andjudging from its melting point, is the so-called paradiphenylbenzene,obtained by G.Schulz as a bye-product in the preparation of diphenylfrom benzene.Now although i t is possible that this diphenylbenzene is a secondaryproduct arising from the diphenyl, yet regarding the properties ofthe mother-substance, it seems probable that it is rather formedby reduction from a more highly condensed phenol, triphenol forexample.Of the numerous possible isomerides of diphenol four are known : (1.)That obtained by Griess from tetrazodipheuyl, later by Lincke fromphenylparasulphonic acid. (2.) That obtained by Engelhardt and Lats-chinoff from diphenyldisulphonic acid, and afterwards more closely in-vestigated by Dobner, and ( 3 ) and (4), those described by the authors.These bodies are sharply distinguished by their melting points (l),mclts a t 156-158" ; ( 2 ) 269-270" ; (3) 123", and (4) at 190".Heat-ing with zinc-dust does not decompose No. 1, whilst Nos. 2, 3, and 4yield diphenyl almost quantitatively. The colorations with ferricP-Diphenol, when pure, forms small glittex-ing scalesORGANIC CHEMISTRY. 67chloride and the lead acetate reactions are not stated in the case ofthe first-named.As regards constitution, the diphenol of Griess and Linke may bestbe named paradiphenol. As regards that investigated by Dobner (2),both hydroxyls are contained in one benzene-group, and so the namediphenol does not seem suitable, in so far as i t would express that twophenol molecules have united, with loss of H2, to form one molecule.a- and P-diphenol might perhaps be designated ortiio- and rneta-dipheid,in so far as, in their preparation, salicylic acid is formed in pre-dominating proportion, and oxybenzoic acid in smaller quantity,whilst paraoxybenzoic acid is never observed.It is by 110 means im-possible that an ortho-meta-diphenol is likewise produced. It is nott o be denied that the mechanism of the reactions in all three cases isvery similar, since by fusing phenol with potash the removal of hydro-gen at the ortho- and meta-position is effected, and by fusing thephenolparasnlphonic acid, the removal of HSO, at the para-position ;and in all cases the two phenol residues unite to form diphenols.Action of Potash on Tetranitrodiphenyl-carbamide.By S.31. LOSANITCH (Dez6t. Ciieni. Ges. Ber., 11, 1539--1542).-When asolution of diphenylguanidine or carbanilide in cold concentrated nitricacid, is heated until red fumes are no longer evolved, and the liquid isallowed to cool, tetranitrodiphenylcarbamide is deposited in paleyellow needle-shaped crystals, which are blue or green by reflectedlight. On boiling tetranitrodiphenylcarbamide with alcoholic potash,i t is slowly converted into tetranitrodiphenyl-potassium-carbamide,C0.[NKC6H3(N0,)e]?, a glistening green crystalline powder, whichexplodes on heating. This compound is converted into dinitraniline byboiling with water. CO[NKC&(N02)2]2 -I- 2H20 = 2CsH3(N0,)2.NH2+ K2COJ. Acids convert the potassium compound into tetranitrodiphe-nylcarbamide, small quantities of dinitraniline a d carbon dioxide beingalso formed.CO[NKC&&(No2)& 4- H80, = CO[NH.C~H3.(N02)2]2 + KS04.Tetrani trodiphenylcarbamide forms a yellow crystalline compoundwith calcium, and a red unstable compound with ammonium.Naphthyl-phosphorus and Napthyl-arsenic Compounds.By W. KELBE (Deut. Ghem. Ges. Be.., 11, 1499--1503).--To preparelln~7ithyZ-~hosplioroi~s acid, C,,H,.POH( OH), a mixture of mercurydinaphthyl and excess of phosphorous chloride is heated in sealedtubes a t 200" for five days; the phosphorous chloride is distilled off;and the residual oily liquid, consisting of impure naphthylphos-phorous chloride, is poured into water: PCl2CI,H, + 2H20 = 2HC1 +C,,H,.POH(OH).The liquid is boiled to expel the hydrochloricacid, and is mixed with a slight excess of sodium carbonate. Thesolution is now filtered, and the acid precipitated by the addition ofhydrochloric acid. The precipitate is washed with cold and recrys-tdlised from hot water. During this operation, oily drops of dinaphthyl-phosphinic acid remain undissolved. Naph t hyl phosphorous aci clcryatallises in small white needles, which are soluble in alcohol and inhot water, but are insoluble in hydrochloric acid, and only sparinglyw. s.w. c. w.f Cis ABSTRACTS OF CHEMICAL PAPERS.soluble in ether and in cold water. The dry acid melts a t 125--126",but when boiled in water, it melts before dissolving. Silver nitrate isreduced by this acid.Diet h y lnaph t h?y Zpl~osp7~in e, C ,H7.P ( C,H,) ?, i s prepared by tb e actionof crude naphthylphosphorous chloride diluted with benzene on nwell cooled mixture of zinc-eth3-1 and benzene. PC12C,,H7 t Zn(C2Hj)2= ZnCI, + CloH7.P(C2H5),. The benzene is distilled off from thecrude product, and the residue dissolved in hydrochloric acid. Sodais added to the solution, and the phosphine is extracted from the pre-cipitate with ether. It is a yellow oily liquid, boiling with pvrtialdecomposition above SGO", and possessing a most repulsive odour.Diethylnaphthylphosphine ah.wrbs hydrochloric acid gas, formingtirst a solid, and then a liquid compound.Trietl/ylnapkt 1yZplj osphoniznn iodide, CI0H7. P ( CZH5),I, formed bythe direct addition of ethyl iodide to diethylnaphthylphosphine,crystallises from an aqueous solution i n colourless plates (m.p. 209").Dinaphtkylphosp7inic mid, PO (OH) (C1,,Hi)2.-The formation of thisacid has been already mentioned. The oily drops solidify, forming awhite crystalline mass, m. p. 208-204", soluble in alcohol.Nqlz thy Zarsinic acid, C loHz A s 0 (OH)?.- Mercury- d i naph thy1 isreadily acted on by arsenious chloride, thus, 2AsC13 + Hg(CloH7), =HgCI, + 2C,,H2AsC12. The compound is separated from the mercuricchloride by extraction with benzene. The oily liyuid left after dis-tilling off the benzene unites with a molecule of chlorine to formC,oH7AsC14, which is decomposed by water into hydrochloric andnaphthylnrsinic acids: CloH7AsCl, + 3H20 = 4HC1+ CloH7As0. (OH),.The acid forms needle-shaped crystals (m.p. 197"). Analogous anti- w. c. w. mony compounds have not been obtained.Metabenzdioxyanthrsquinone. Ry E. SCHUNCK and H. ROE-VER (Deut. Chem. Ges. Ber., 11, 969-973).-A substance thus namedby the authors, and isomeric with alizarin, is formed, together withanthraflavic acid and a third product t o be described hereafter, by theaction of sulpburic acid on oxybenzoic acid. It crystallises fromnlcohol, in which i t is easily soluble, in yellow anhydrous needles,which melt at 291-293', and burn with a bright flame. It is solublealso in acetic acid, benzene, ether, and chloroform, but not in wateror carbon bisulphide. Sulphuric acid dissolves it, forming a brownish-yellow solutJion, which exhibits no absorption-bands. Potash, soda, andammonia dissolve i t with deep-yellow eolour. Its barium derivativecrystallises in long red needles.The calcium derivative is nearly in-soluble. The substance combines with acetic anhydride to form thecompound, C1,H6(C,H30),04, which crystallises in tufts of yellowneedles melting a t 199". Metabenzdioxyanthraquinone, when heatedwith potash, yields purpnrin.Tetraphenylethane. By C. ENGLER ( D e d . Chew. GRS. Ber.,21, 926 -93O).-'I'efraphenylethane has hitherto been prepared (1) byreducing benzophenone with zinc-dust ; (2) by the action of hydriodicacid and phosphorus on benzpinacone; (:3) by the action of hydro-ahioric and zinc on benzhydrol in acetic solution; and (4) by t h eJ. RORGANIC CHEMISTRY.6action of hydriodic acid and phosphorus on benzpinacolin. Thauthor describes the two following new methods of preparation, thcformer of which is suitable for preparing the body in large quantities.1. The sulphuretted derivative of benzophenone melling a t 1.51'described by the author in a former paper (p. 61) (which may easily beobtained in any quantity) is dissolved to saturation in boiling alcohol.and the solution is boiled for some hours with an excess of copperprecipitated from cupric sulphate by zinc. Cupric sulphide is therebyformed, and the whole ot the benzophenone-compound is convertedinto tetraphenylethane, which is deposited from the tiltered liquid, asit cools, in small acicular crystals, generally quite pure. The yield isabout 94 per cent.of the tlieoretical amount. Or the benzophenone-compound may be heated with copper in the dry state, and the result-ing tetraphenylethane sublimed in a wide-necked retort.2. Benzophenone chloride (diphenyl-chloromethane), (C,H,),CHCl,obtained by passing dry hydrogen c!iloride into benzhydroi kept cool, isdissolved in benzene and boiled for Eome hours with sodium. The liquidon cooling, or after evaporation, deposits crystals of tetraphenylethane.I t dissolvesmore freely in etber and benzene, and very easily in carbon bisulphideand chloroform, from which last it is deposited in large crystals, onslow evaporation of the solution. With benzene it forms a crystallinecompound, c26HtJI?2.c6H6, which is deposited from its solution in thatliquid in well-formed transparent tables, turning opaque in the air.A szdphonic acid of tetraphenylethane is formed on gently warmingit with eight times its weight of concentrated sulphuric acid.Thebarium salt, (C26H:16(SOJ)4Ba2, is vcry soluble. The free acid is solublein water and alcohol, but scarcely in ether or chloroform. Whenfused with potash, it yields a phenol having the composition of tetru-It !jclroxyl-tetraphenyl et hane, and crystallising in la,minz, which me1 t a t248".A nitro-con?pound, C26H18(NO,)4, crystallising from aniline in smallneedles, is obtained by treating tetraphenylethane with nitric acid inthe cold. By the action of tin and hydrochloric acid, i t yields anxmido-compound, the hydrochloride of which crystallises from water,and forms a crystallisable double salt with stannic chloride.Tetraphenylethane is but sparingly soluble in alcol~ol.J.R.Camphor. By F. WREDEN (Deut. Chem. Ges. Bey., 11, 989).-On heating ordinary camphor at 190" with hydrochloric acid of sp. gr.1-03 it is converted into an isomeric liquid modification, of sp. gr.0.913. The liquid boils a t 187-193", and does not solidify at - 17".It absorbs oxygen from the air, especially in snnshine, and gives nosilver mirror with ammoniacal silver nitrate. J. R.Reduction-products of Elerni-resin with Zinc-dust. ByG. CIAMICIAN (Deut. Cliem. Ges. Bw., 11, 1344--1348).-This is acontinuatiou of a. previous investigation, undertaken to determinewhether the different terpene-resins on reduction with zinc-dust,furnish similar products. The above resin was chosen because itcould easily be obtained quite pure and crystallised.The productsobtained were toluene, meta- and para-ethylmethyl- benzene and ethyl7 0 ABSTRACTS OF CHEMICAL PAPERS.naphthalene. Those obtained previously from abietic acid and fromcolophony were toluene, e thyl me thyl- benzene, naphthalene, met hg 1 -naphthalene, and methylanthracene. Elemi-resin and abietic acid bothyield toluene and ethylmethyl-benzene. Naphthalene and methy1-anthracene are not obtainable from elemi-resin, or a t least in scarcelyperceptible traces, and instead of the met8hylnaphthalcne of the abieticacid, ethylnaphthalene is obtained from elemi-resin. In both casestoluene, ethylmethyl-benzene, and methyl- ‘or ethyl-naphthalene, occurin far preponderating quantity, and it may therefore be inferred thatthe chemical constitution of these two substances is very similar.Splitting up of Cyclarnin into Glucose and Mannite.ByS. DE LUCA (Coiizpt. rend., 87, 297--’299).-The author shows thatcyclamin, either coagulated or in aquems solution, when left to itselffor several months, splits up into two distinct substances, namely,gIucose and crystallised mannite. Cyclamin must, therefore, be re-garded as a glucoside, from which not only glucose, but also mannite,may be obtained. R. R.New Synthesis of Glycocyamine. By M. NENCKI and N.SIEBER (J. p r . Chem. [Z], 17, 477--480).-Glycocyamine is producedby the action of glycocine upon guanidine carbonate, in accordance withthe equation 2C,H5NO2 + (CN3H6),COs = 2C3H,N302 + (NH&C03.The aqueous solution of the two substances is boiled down to a smallbulk, the glycocyamine is precipitated by addition of much water,and purified by repeating the same process three or four times.Theglycocyamine obtained is identical with that of Strecker (Conzpt. r e d . ,52, 1212). The authors find that glycocyamine is soluble in 627 partsof water at 14.5”.I n the reaction of glycocine with guanidine carbonate, a substanceis also produced which is possibly a double salt of the formulaC,H~No,.(CN,H,),CO,.H,O. This substance separates in large clearrhombic tables from the warm saturated solution obtained by boilingdown the original mixed liquids.Theauthors reserve the account of the compounds produced in this way fora future paper.Action of Iodic Acid, LLSulphomolybdic Acid,” and FerricChloride on Morphine and other Substances.(Phurm. ,I.Trans. [ 3 ] , 9, 70) .-Morphine hydrochloride dissolved in water, strikesa transitory blue with starch and iodic acid. With grape juice andstarch, iodic acid produces no blue ; but a dirty blue is observed withthe alcoholic extract of the dried juice. Orange-juice, with starch andiodic acid, gives instantly a blue colour. Saliva also produces a brightblue; but a mixture of orange juice and saliva produces a violetcolour. This reaction resembles that of morphine, but there is no alte-ration of the colour, the blue not being produced. With sulpho-molybdic acid, morphine gives a purple colour, which rapidly disap-pears, tnhe liquid becoming brown, and finally blue.With grape juiceno coloration appears for nearly half -an-hour. Fresh orange juiceremains unaltered, but with the dried juice, a faint blue is visible inw. s.Guanidine carbonate reacts with amido-acids in general.M. M. P. MORGANIC CHEMISTRY. 71ten minutes. The same result is obtained with saliva. When salivaand orange juice are mixed, coloration ensues only after the lapse ofhalf-an-hour. Ferric chloride produces a bluish-green with morphine,whereas a red is produced with dry or wet saliva; but no result isobtained with orange juice and saliva. A wine-red tint is perceptiblewith the twelve-thousandth of a grain of meconic acid in presence offerric chloride.E. w. P.Remarks on Rice’s Articles on the Cinchona Alkaloids.By 0. HESSE (Deut. Chew Ges. Ber., 11, 1549-1560).Substitutes for Quinine. BJ 0. HESSE (Dmt. Chent. Ges. Ber.,11, 1546--1549).-Dita bark (the bark of Alstonia scholtzris or Echitesschobnris) contains two alkaloids, ditamiize and echitamine. Gruppe’sextract of dita bark, ditaine, acts like curare ; this is probably due tothe echitamine.The bark of Aistonin spectabilis, which is also used as a febrifuge,contains the alkaloid alstonnmine.‘I’he bark of Crossopteryx Kotschyan,a (syn. Crossopteryx febrifiqa) con-tains 0.018 per cent. of the alkaloid crossopterine, but does not containquinine.Itis precipitated from the hydrochloric acid solution by ammonia, soda,platinum chloride, and by the double iodide of potassium and mer-Cinchonine and Cinchonidine.By Z . H. SKRAUP (Deut. Chem.Ges. Ber., 11, 1516--1519).-The results of numerous analyses of cin-chonine and its salts are given in support of the author’s view, thatthe composition of cinchonine is C19HT2N20, and not C,,H?,N,O. Cin-chonine generally contains small quantities of the compound C,,H,,N,O(the hydrocinchonine of Willm and Caventou), to which the namecinckotine is given by the author. The two bases may be separatedby fractional crystallisation of the mixed sulphates or tartrates. Cin-chotirie sulphate crystallises in prisms containing 11$-12 moleculesof water. I t is slowly attacked by potassium permanganate in thecold. Dihydrodicinchonine sulphate is easily distinguished from thepreceding compound by forming long slender crystals, containing2 molecules of water, and by being readily attacked by potassiumpermanganate.Cinchonine is oxidised by potassium permanganate, forming formicacid and cinchotenine.Cinchonidine has the same composition as cinchonine, vix., CI9H,,N2O,and is considered by the author to be probably identical with homo-cinchonidine.On oxidation, cinchonidine yield6 formic acid and alaevo-rotatory body (m. p. 25S0), which is an isomeride of cinch6tenine.Remarks on the preceding Paper. By 0. HESSE (Deut. Chem.Ges. Ber., 11, 1520--1521).-The author publishes the results ofseveral analases in favour of the formula, CmH2iN20, for cinchonine,Crossopterine is soluble in alcohol, ether, and hydrochloric acid.cury.w. c. w.I t is proposed to call this substance cinchotenidine.Tv. c. w72 ABSTRACTS OF CHEMICAL PAPERS.and gives a, test for distinguishing cinchonidine sulphate from homo-cinchonidine sulphate, viz. : 1 part of the substance is dissolved in 50parts of warm water, and left at rest for two honrs. Cinchonidinesulphate crystallises out in long brilliant prisms, whilst homocin-chonidine sulphate forms groups of delicate dull-white prisms. Thistest cannot be used in presence of appreciable quantities of quinine. w. c. w.A New Organic Base in Animal Organisms. By P.SCHREINER (Liebig's Annalen, 194, 68--84).-Charcot and Robinand numerous other observers have remarked the occurrence of apeculiar crystalline body in the secretions and in certain organsof the animal organism.The crystals, which appear to be especiallyplentiful in patients suffering from bronchial asthma, or from leuco-cythemia, were supposed by Friedrich and Huber to be tyrosine.Harting believed them to be calcium phosphate, Bottcher albumi-noid bodies, and Salkowski and Forster regarded them as mucouscompounds. The author lias shown that this body is the phos-phate of an organic base. The crystals form 5.237 per cent. of thesolid constituents of human semen, and can be easily obtained byboiling the fresh fluid with alcohol, treating the precipitate, after i lhas been dried a t 100". with warm water, containing a few drops ofammonia, and evaporating the alkaline solution.The crystals alsoseparate out on the surface of pathological preparations which arepreserved in alcohol. After purification by recrystallisat ion from hotwater containing a small quantity of ammonia, the crystals (prismsand double pyramids) are colourless and brittle. They are insolublein ether, chloroform, alcohol, and in cold water, but they dissolvereadily in dilute acids, in solutions of caustic alkalis and alkaline car-bonates.The salt contains two atoms of nitrogen to one of phosphorus ; i tloses 3 mols. of water a t loo", melts a t 170°, and decomposes at ahigher temperature, givinp off ammonia. By precipitating the phos-phoric acid with baryta-water, the free base is obtained as a colourless,inodorous crystalline mass, having a bitter taste. It is soluble inalcohol, insoluble in ether, and its solution immediately formsa crystalline compound on the addition of phosphoric acid. Thebase has been extracted from the liver, spleen, lungs, and blood ofcattle, and from the liver, spleen, blood and marrow of men who hadsuffered from leucocythEmia, by boiliiig with water containing aceticacid. Lead acetate was added to the solution, tbe excess of lead re-moved from the filtrate by means of sulphuretted hydrogen, and thebase pyecipitated by phosphotungstic acid. The free base, obtainedby boiling the phosphotungstate with baryta, forms it crystalline com-pound with hydrochloric acid, C2H5N.HCl. On the addition of platinumchloride to the hydrochloride, large prismatic crystals slowly sepa-rate out. Gold chloride precipitates the compound C2H5N.HC1.AuCl3,which crystallises in golden plates, soluble in ether, alcohol, and inwater. The characteristic odour of fresh human semen is observed,when an aqueous solution of the gold salt is treated with metallicmagnesium. w. c. wORGASIC CHENISTRY. 73Lotur Bark. By 0. HESSE (Deut. Cliem. Ges. Ber., 11, 1542-1546 j .-Lotur bark, the bark of S'ynqdocos mcemosn, contains threealkaloids, viz. : Zoturioze, 0.24 per cent. ; colloturine, 0.02 ; and lotzwidiw,0.06 per cent, The alkaloi'ds are extracted from the bark by hot alco-hol, and are converted into acetates. Loturine and colloturine areprecipitated from the neutral solution by the addition of potassiumthiocyanate, leaving the lot uridine in solution. The crystalline preci-pitate is decomposed by soda, and the alkaloids are extracted withether and recrystallised from alcohol. The efflorescent crystals ofloturine are separated mechanically from the non-efflorescent crystalsof colloturine.Lotzmhe is soluble in alcohol, ether, chloroform, and acetone, but isinsoluble in water, ammonia, and caustic soda. It gives no colora-tion with ferric chloride, strong sulphuric or nitric acids, or even onthe addition of bleaching powder and ammonia. Loturine melts a t 234',and sublimes, forming colourless prisms. The fluorescence exhibitedby a solution of loturine in dilute acids is more intense than thatof quinine sulphate. Loturine fornis well-crystallised salts. Thehydrochloride, which crystallises in white prisms soluble in alcoholand in water, fornis double salts with the chlorides of platinum, gold,and mercury. The hydriodide forms a crystalline double salt withmercuric iodide. The nitrate, thiocjanate, acetate, chromate, andpicrate arc crystalline compounds. The taunate and phosphotungstateare amorphous powders.Colloturine is deposited from alcohol in prisms terminat>ing inpyramids, which sublime a t 234". The solution of the alkaloid indilute sulphuric or hydrochloric acid is fluorescent. Gold chlo-ride produces a yellow amorphous precipitate in the solution of thehy dr oc h 1 (ride.5oturicZine.-The filtrate from the thiocjanates of loturine and collo-turine is rendered alkaline by ammonia, and the loturine extracted withether. Loturidine is a yellowish-brown amorphous body yieldingamorphous salts. It dissolves in strong nitric and sulphuric acidsforming yellow solutions. The solution iu dilute acids is fluorescent.Winckler's calyornine was not a simple substance, but a mixture ofthe acetates of these three alkaloids. w. c. w.Amyrin and Icacin. By 0. HESSE (Liebig's Anna!en, 192, 179-182).-The author compares the analyses of these two substances, andis inclined to regard icacin and amyrin as hydroxyl-compounds, viz. :CJ7H7,.0H and C,,H7s(OH)2 respectively. No new experimental dataare given. M. M. P. MI.By BOUSSINGAULT(Compt. rend., 87, 277--28l).--.The author has recently analysedthe juice of the cow-tree (Brosiwum galactodendron) which is used inSouth America as an article of diet. The results show that thisvegetable milk, in its general composition, has much resemblance tothat of the cow, inasmuch as it contains a fatty substance, saccharinematters, casein, albumin, and phosphates. The proportions of thesesubstances in the juice of Brosimum gulactodendron are, however, suchComposition of the Milk of the Cow-tree74 ABSTRACTS OF CHEMICAL PAPERS.Juice of B. Galactodendrow.Saccharine substances .... 2.8Case'in, albumin, phosphates,&c. .................. 4.0T a x and saponifiable matter 35.2Cream.Butter .............. 34.3Milk sugar .......... 4.0Casein and phosphates 3.5Water .............. 38.2Water .................. 58.0100.0 - I --100.0The fatty substances in the vegetable milk, according to C. Bernard,are capable of being split up into fatty acids and glycerin.R. R

ISSN:0368-1769    

DOI:10.1039/CA8793600034

出版商:RSC    

年代:1879

数据来源: RSC

摘要:

74 ABSTRACTS OF CHEMICAL PAPERS.P h y s i o l o g i c a1 Chemistry.Influence of the Temperature of the surrounding Atmo-sphere on the Excretion of Carbonic Acid and the Absorp-tion of Oxygen in a Cat. By the Duke CARL THEODOR of Bavaria(Zeitsck. f. BioZogie, 14, 51--56).-1n this series of experiments theauthor fed a full-grown cat on a fixed diet from December 14th, 1874,to Jan. 14th, 187.5. For the first 1 7 days the cat received daily 100grams of beef and 10 grams of pure lard, but as the animal was losingweight the diet was increased to 120 grams of meat and 15 grams oflard ; this was continued throughout the experiments. Except whenplaced in the respiration apparatus, the animal was kept in an un-heated space, and was therefore exposed to the variations in tempera-ture of the climate (Munich).The cat was weighed daily and theaverage temperature of the air noted. From December 31st to June16th the animal increased somewhat in weight; from the latter datet o March 30th (Le., during the cold season of the year) its weightremained nearly stationary (between 2,557 and 2,650 grams). Withthe advent of warm weather, however, it gradually increased in weight,until on June 14th i t weighed 3,047 grams.The author thence concludes that, for some reason less nourishmentis required during summer than in winter, for the same diet whichduring the cold weather merely maintained the animal at its originalweight, caused a considerable increase in the same during the summer.During the above-mentioned six months, 22 experiments, each last-ing from five to six hours, were made with the respiration apparatus,the absorption of oxygen, as well as the excretion of carbonic acid andwatery vapour, being estimated.The experiments were made in eachcase after the cat had fasted 17 hours.The results showed plainly that the excretion of carbonic acid andthe absorption of oxygen are increased by cold and diminished byheat. The fact that the numbers do not increase uniformly with thPHTSIOLOGICAL CHEMISTRY. [ 75lowering of the temperature, the author attributes to movements of thecat sometimes taking place, whereas the animal usually remained quietin the apparatus. The average proportion of the oxygen absorbed tothat contained in the carbonic acid excreted was as 100 : 77, being thesame as that found in the fasting dog.Influence of the Temperature of the surrounding Air on theProcesses of Decomposition in the Organism of Warm-bloodedAnimals.By C. VVIT (.Zeitsch. f. Biologie, 14, 57--160).-Thislengthy paper is divided into numerous sections, of which the firsttreats of the literature of the subject, and the others are as follows:-2. Experinzeuts with a cat.3. Ecperiwents o n man in cold and heat with exclusion of voluntarymovements.-The results obtained showed that both in the case of thecat and of man, when the temperature fell below the ordinary (14-15" C.), the excretion of carbonic acid was increased, the increaseamounting in man to 36 per cent. in a fall of 9.9". Increase oftemperature on the contrary does not show a gradual decrease, but alsoa slight increase in the carbonic acid, which amounted to 10 per cent.,when the temperature was raised 15.7".There is therefore, theauthor concludes, no doubt that it is not the voluntary movementswhich give rise to the increased excretion of carbonic acid.4. In this section, the author traces the gradual development of thetheory of the decomposition of albumin, fats, and carbo-hydrates, notby the direct action of oxygen, but by means of organised ferments.He does not consider ths temperature as the immediate cause of the de-composition, and cites the case of the diabetic (in whom, under certaincircumstances, there may be a large consumption of oxygen), tm showthat temperature and oxygen together do not suffice to bring about thedecomposition of the sugar.In diabetes, causes which normally bringabout the decomposition of sugar are absent, on which account littleoxygen is usually absorbed.5. liiftuence of the Respiratory movements on the formation of Carbonicacid.-Acoording to the author the influence of the respiratory move-ments on the formation of carbonic acid and on the decompositionstaking place in the body is due, not to the different quantities ofoxygen inhaled, but to the increased muscular activity under thesecircumstances.7. Experiments 09% the Marmot during Hibernation.- Two experimentsmade by the author in 187-4 confirm previous observations, showingthat glycogen exists in the liver in large quantihies in hibernatingmarmots. This indicates, he thinks, that glycogen is formed in the fast-ing organism, although this cannot usually be poved ; in the wakingstate there must be some cause which brings about its immediate de-composition.This cause he considers h be the musoular movemectsof the waking animal.8. Consumption of Oxygen i n Man during Sleep.-Experiments by theauthor and Pettenkofer, made in 1866, seemed to show that duringthe night considerably more oxygen is absorbed than during the day,and also that during the day considerably more oxygen is excreted inthe products of decomposition than is absorbed in the mean time. TheE. C. B76 ABSTRACTS OF CHEMICAL PhpKRS.author now detects an error in some of these experiments, owing tothe increase in weight of the bedding (due to absorption of moisturefrom the air) in 24 hours, being all attributed to the 12 hours of thenight; the excretion of water found during the day was therefore toolittle, that during the night too great, rendering the calculated amountof oxygen absorbed during the day too small, that for the night too great.9.In an experiment on a fasting dog during a sleep of 4 hours25 minutes, induced by chloral, the author found that very little car-bonic acid was given off and very little oxygen absorbed, but, whereasduring hibernation the amount of oxygen absorbed was much greaterthan that excreted, in this case the difference was abnormally small.10. An experiment made on a man suffering from paralysis, afterfracture of the eighth dorsal vertebra, gave for 12 hours an excretion ofcarbonic acid amounting to 250 grams, being 38 per cent.less carbonicacid than that excreted during the 12 hours of the day by a man in health,and 20 per cent. less than that given off during the 12 night hours.The author concludes from this arid other observations that the stimuliacting on the organs of sense exert by means of the nervous system acontinual stimulating influence on the decompositions taking place inthe organism. The nerves are not, he considers, the cause of the de-composition, but they exert a modifying influence on this cause, andare able to bring about conditions more favourable to the same.12. Decomposition, of Fut caib be increased by ReJez action.-The de-composition of albumin is dependent chiefly on the amount of albumincarried to the living cells, that of the fat, on the other hand, on thechange in relation of the particles brought about by nerve influence.Xxperimenting on dogs rendered motionless by curare, the author findsthat, as during sleep, much less carbonic acid is excreted, which heattributes not to a diminution of the amount of albumin decomposed,but to a less decomposition of fat.Prom these obserr-ations, he con-siders it probable that cold or other stimuli acting on the skin, and alsolight, when they cause in a reflex manner an increase in the excretionof' carbonic acid and absorption of oxygen, do so merely by increasingthe decomposition of the non-nitrogenous substances and not that ofalbumin, Lowering of the surrounding temperature, as long as thetemperature of the body remains constant, he finds only brings aboutan increased decomposition of fat or non-nitrogenous substances.When, however, the body-temperature is reduced, there is prcbably adiminution in the decomposition both of albuminous and of non-nitro-genous substances.Increased body-temperature artificially produced,or the result of fever, is aecompanied by an increased decomposition ofalbumin; it is doubtful whether the decomposition of fat is alsoincreased.13. The increased decomposition in the cold due to involuntaryregulation is not, the author considers, of very much importance to lifein cold climates, f o r it is assisted by other more efficient means, via.:by clothing the body with bad heat-conductors, by production of muchheat, by a great consumption of nourishment, and by muscular action.I n man and in the cat, he considers that there does not exist forhigher temperatures any appreciable reflex regulation by diminishedoxidation. E. C. BANALYTICAL CHEE?I1ISTRY. 77Magnesia as an Antidote for Arsenious Acid. By P. DECLERMONT and J. FROMMEL (Compt. rettd., 87, 332).-1n seekin?to eliminate arsenious acid in the experiments referred to on page 13of this rolume, the authors found that on adding magnesia to waterholding sulphide of arsenic in suspension, two combinations areformed : a snlph-arsenite of magnesium, R ~ ~ , ( A S S ~ ) ~ , which is solublein water, and an nrsenite, MgHAs03. insoluble. The equation repre-senting this reaction is :-2As2S3 + 5MgO + H,O = MgI(AsS3), +2M gHAs03. The soluble eulph-arsenite is dissociated when boiled,thus:-Mg2(AsS3)2 + 7H20 = MgHAs03 -t 6H2S + MgO. Ma?-riesia is an excellent antidote in cases of poisoning by arsenious mid,as the arsenite is completely insoluble ; but snpposing that a portionof the arsenious acid becomes converted into trisulphicle in the stomachor intestines, the magnesia mould render this soluble. Now, in theintestines of a person poisoned by arsenious acid, trisulpliidc in thestate of fine yellow powder has been observed (Neu. R5per. der Phariiz.,17, 386) ; and the question arises whether magnesia is as efficaciousas has been supposed, seeing that the sulphide which would otherwisenot be capable of absorption, is rendered soluble by it. R. R

ISSN:0368-1769    

DOI:10.1039/CA8793600074

出版商:RSC    

年代:1879

数据来源: RSC

摘要:

ANALYTICAL CHEE?I1ISTRY. 77 A n a1 y t i c a1 C h e m i s t r y. Colorimetric Experiments. By J. BOTTOMT~EI- ( Ch e m . News, 38, 191-193). -Experiments were made t o determine, if possible, the amount of colouring matter in a liquid by compaiison with a, standard liquid. White disks were sunk in two equal cylinders, the one containing the standard liquid, the other that to be tested, i t being thought that the dept’h of the disk would be inversely as the quantity of the colouring matter present. It appears, however, thzt the method cannot, be practically employed, owing mainly to the diffi- culty of detecting the exact shades of colour. Schutzenberger’s Process for the Volumetric Estimation of Oxygen in Water. By C. c. HUTCHINSON (Chem. News, 38, 184--187).-1n water containing sewage, oxygen is present in quan- tities below the normal, but the quantity increases as the sewage de- creases; in deep well-water, however, containing no sewage, it is stated there is an almost total absence of oxygen ; this may be owing to its having already been removed by organic matter during its passage through the strata.To settle the question whether oxygen is or is mot an indication of the purity of water, the author was anxious to employ some method more rapid than that of Bunsen’s for the de- termination of the amount of oxygm present, but it appears by the experiments that the method which he proposed to ernploy is scarcely accurate enough, although it admits of grea.t rapidity, and is morc suited for a small quantity than f o r a large quantity of water: it is also valuable as R preliminary experiment.The method consists in E. W. P.75 ABSTRACTS OF CHEMICAL PA4PERS. adding a known volume of the water to a solution capable of bein9 oxidised, accompanied by a change of colour, by the oxygen contained in the water. The extent to which this has occurred is then deter- mined by the addition of a reducing agent, which reduces it to its former condition. This last solution is standardised in terms of the oxygen it is capable of taking up ; and from the amount used in the experiment, the volume of oxygen present is calculated. The reducing agent employed is sodium hyposulphite, made by passing sulphurous anhydride to saturation into a solution of soda, sp. gr. 1.4, diluted to sp. gr. 1.34, and reducing the product with powdered zinc : milk of lime is then added, which precipitates the zinc and also renders the liquid less absorbent of free oxygen.The liquid by which the change of colour detects the completion of the process is either sodium sulphindigotat,e, or Coupier's aniline blue ; 10 grams of the indigotate are dissolved in 1 litre of water. An ammoniacal solution of copper sulphate con- taining 4.46 grams per litre is used to standardise the above solutions. The estimations must all be made in an atmosphere of hydrogen. The process for determining the oxygen present is fully described, as well as the method of standardising the solutions. Appendix to the Estimation of Carbonic Acid in the Air. By W. HESSE (Zeitschr. j'. Biologie, 14, 29--33).--Having given some additional directions with a view to avoid the introduction of carbonic acid from the outer air along with the baryta-water, the author re- commends the following method for ordinary purposes :-A solution of oxalic acid of *5727 gram to the litre is prepared, and baryta-water, of which 10 C.C.neut,ralise from 20 to 25 of this solution of oxalic acid, and volumes of air of about half a litre are used. According to whether 4 to 5 per mil. or more of carbonic acid are expected, 10 to 20 C.C. of baryta-water are added. The pipette is inserted through an india- rubber stopper with two perforations, the escape of air from the flask being regulated by the finger on the second apertrlre. The flask is rapidly closed aftler removing the pipette. The numbers are often some- what too high. E.C. B. Quantitative Determination of Sulphur in Illuminating Gas. By POLECK and BIEFEL (Chem. Centr., 1878, 331).-A measured quantity of the gas to be examined is burned in air, and the products of the combustion drawn through an alkaline solution of bromine by means of a water aspirator. The sulphur is determined as barium sulphate. The gases examined by the authors were taken from t,he works a t Breslau, the experiments being made on the same day, and as rapidly one after the other as possible. The following results were obtained :- E. W. P. Sulphur in 1,000 litres of gas, 0.600 gram I n the retort house.. .......... Before the scrubbers .......... 0.540 ,, After passing the scrubbers.. .. 0.464 ,, After passing the condensers .. 0.440 ,, I n the finished gas.. .......... 0.276 ,, In the first four determinations, H,S is included ; and when CS, isANALYTICAL CHENISTRY. 71) separately determined in the finished gas, the residual sulphur may be considered as belonging to the so-called sulphuretted hydrocarbon, the smell of which resembles phenyl mustard-oil. J. M. T. Estimation of Nitric Acid as Ammonia. By E. A. GRETE (Deut. Chem. Ges. Ber., 11, 1557-1558).-Nitrates are completely reduced to ammonia by heating to redness with soda lime and a Estimation of Nitrous and Nitric Acids. By G. LUNGE (Diwgl. polyt. J., 228, 447-4501 .-Lange has constructed an a p paratus for determining the above acids, which is a modification of Watts’ apparatus described by Davis (Chem. News, 37, 4.5), and resembles Runte’s modification of Rauch’s gas burette.This im- proved form has no trough, arid requires but little more mercury than is necessary to fill the tube (about 830 grams) ; it is easily cleaned out after every operation, and has the advantage of the mercury not coming into direct contact with the worker. Lunge calls it a “ nitro- meter. ” D. B. xant hogenat e. w. c. w. Behaviour of Quartz with Microcosmic Salt. By E. LAUFER (Deut. Chem. GRS. Ber., 11, 935).-1n a former paper, the author de- scribed a method of separating quartz from admixtures with silicates by fusion with microcosmic salt, which it was then thought decom- posed silicates without attacking quartz. But further experiment has shown that the method cannot be relied upon, inasmuch as quartz ibelf, especially when finely powdered, is acted on by the fused salt.J. R. Testing and Valuing Gas Liquor. By T. H. DAVIS (Qheliz. News, 38, 193--195).-Gas liquor, or a crude solution of ammonia salts, is generally sold on the basis of its sp. gr., or on its degree (Twaddle). This test is, however, untrustworthy, although an indica- tion of the “ strength ” of the liquor is obtained. Now, as the ammonia is that for which the manufacturer contracts, i t is recommended to titrate the ‘liquor as follows :-Into it flask of about 300 C.C. capacity 10 C.C. of the sample to be tested are run in, and into this 15 C.C. of nornial sulphuric acid. The contents of the flask are then raised to boiling, a few drops of litmus added, and titrated back with normal soda. The niimber of C.C.of soda used are deducted from the 15 C.C. of acid em- ployed, the result multiplied by 17, and divided by the specific gravity of the liquor. The result thus obtained represents the percentage of ammonia contained in the liquor. Remarks on the Estimation of Calcium Sulphate in Beer. By H. M. WLLSON (Chem.. News, 38, 197).-Organic matter appears to interfere with the complete precipitation of the sulphuric acid in beer as barium sulphate. It is advisable, therefore, in the first instance to evaporate 100 C.C. of the sample to dryness, and after the addition of 0.5 gram potassium nitrate, to ignite the residue. E. W. P. E. W. P.SO ABSTRACTS OF CHEhlICAL PAPERS. Presence of Lead in Bismuth Subnitrate. By CHAPIUS and JANNOSSIER (Conyt. rend., 87, 1G9--171).--Carnot has shown that a11 samples of bismuth subnitrate of commerce contain lead; some- times in qiiantities dangerous for public safety.The authors of the present pxper propose the followinq method for the quantitative detec- tion of the lead. The bismuth nitrate to be examined is boiled with caustic soda and n small quantity of potassium chromate, the residue, after boiling, being thrown upon a filter. To the filtered liquid, acetic acid is added until the solution is j u s t acid, when a yellow precipitate is produced, more or less pronounced, according t o the amount of lend present. For & an abundant precipitate is obtained ; for the cloudiness of the liquid is distinct, and a dcposition very soon takes place in the form of a precipitate adhering to the sides of the tube ; lead chromate is slightly soluble in the mixture of sodic acetate and acetic acid ; smaller quantities could be detected if the weight of sub- stance used was increased.After mentioning that both calcium phosphate containing silica or alumina, and also impure soda interfere with the reaction, he describes the following quantitative method similar to that described for the qualitative detection. About 10 grarns of the bismuth nitrate are used, care being taken to wash the chromate of bismuth with a mixture of potassium chromate and sodium hydrate, first by decantation, and then on the filter until the filtrate is no lbnger rendered turbid by acetic acid in excess. The filtrate is now boiled, supersaturated with acetic acid, allowed to stmd 24 hours, and filtered.The precipitate is then washed with water slightly acidulated by acetic acid, dried a t 100" and weighed. The weight, found, multiplied by 0.6408, gives the weight of lead contained in the 10 grams of substance. Estimation of Nitrogen in Organic Bodies. By E. A. GRETH (Deut. Chew,. Ges. Ber., 11, 1558).-In estimating the nitrogen in horn, leather, and wool refuse, the author advocates dissolring the substance in warm concentrated sulphuric acid before heating with soda-lime. Higher results are obtained than by the ordinary pro- cess. w. c. w. -___ ;Idoo shows only slight cloudiness, often appearing only on cooling, as J. M. T. New and Rapid Process for the Analysis of Milk. By A. ADAM (Compt. relid., 87, 290-291) .-The analysis is performed by means of an apparatus consisting essentially of a glass tube of about 40 C.C.capacity, provided with a stopper a t the top, expanded in the middle, and tapered off a t the bottom, which is closed by a glass stopcock. Into this appai-atus is introduced 10 C.C. of alcohol of 75", containing of its volume of sodic hydrate ; then 10 C.C. of milk, which must be neutral ; and finally, 12 C.C. of pure ether. The liquids are shaken together, and allowed to remain a t rest for five minutes, when they separate into two layers: the clear upper one con- tains all the butter; the lower, the lactose and case'in. The butter contained i n the former is estimated by eraporating and weighing, allowing 1 centigram for a little case'in, &c., which may be con-ANALYTICAL CHENISTRY.81 tained in the liquid, or eliminating this by re-solution in ether. In the liquid first drawn off, the lactose and casein are estimated by making up to 100 C.C. with distilled water, and adding 10 drops of acetic acid ; the casein then separates, and after having been removed by filtration, is pressed between folds of bibulous paper, dried, and weighed. The filtrate contains the salts of the milk, the acetate of sodium formed, and the lactose. The latter is estimated by means of Fehling's cupro-potassic liquid. All these operations are easily per- formed in an hour and a half; and if, a t the commencement? 10 C.C. of the milk acidulated with two drops of acetic acid are set to evapo- rate, the weights of dry residue, ash, and water may be obtained within the same time.R. R. Butter Analysis. By H. HAGER (Chew. Centr., 1878, 333-334). -1. 20.0 parts of the butter to be analysed, together with 3.0 to 4.0 parts of pure sodium chloride, are placed in a weighed glass vessel, and the whole is weighed and heated to 50-80" in a water-bath, when the fatty part forms a yellowish layer on the top, whilst the water, casei'n, and salt remain at the bottom. Two portions of 5.0 parts of the clear fat are placed in glass flasks of about 12.0 C.C. for further investiga- tion, as described in 111. 11. Estiwation of nii'disture, Casein, a d Salt.-The fat is decanted as far as possible; then 10 C.C. of warm benzene are added and gently agitated with the liquid, so as to take up the rest of the fat. The vessel is t,hen allowed to stand in a warm place for half-an-hour, when the benzene is poured off and 10 C.C.more are added to remove the last traces of fat. The liquid is allowed to stand for half-an-hour longer in a warm place to remove the last traces of benzene, and the vessel and its contents are again weighed; this, after subtracting the 3 . 0 4 . 0 NaCl added, gives the weight the total moisture, casei'n, aud salt. The residue is then treated with hot water and filtered. Thc filtrate evaporated to dryness gives, after subtracting the NaCl added, the salt in the butter. 111. Snponijication of the Butter Fat.-To the 5 grams of fat in the flask, 20 C.C. of alcohol are added, and 10 C.C. of a freshly-prepared solution of 2.0 grams of pure caustic soda in 10.0 of distilled water; the whole is then agitated and heated to 50-60°, when the flask is corked and violently shaken.The alcohol prevents frothing. After a few moments' rest, small particles of fat are observed if the saponifica- tion is not complete. When this is the case, the flask is uncorked aud again heated ; recorked, wrapped in a towel, and shaken ; it is scarcely ever necessary to repeat the operation a third time. The author says that it takes about 6-8 minutes for complete saponification. IV. The warm soap-solution is poured into a large beaker, and the flask washed out with 45 per cent. alcohol. The solution is then warmed without boiling, so as to evaporate as much as possible of the alcohol ; 3-4 C.C. do not interfere with the following reactions. A little warm water is added, and then 20.0 of previously warmed dilute sulphnric acid (1 : 5 water), and stirred; water is then poured in until the level of the liquid is about 2 c.below the mouth of the beaker. Aft,er the fat has completely separated out in the water-bath or other The casein remains on the filter. VOL. XXXVI. 9a2 ABSTRACTS OF CHEXICAL PAPERS. warm place, 5.0 of perfectly dry white wax or paraffin are added, heated to melting, and the whole placed in a cool place to solidify, leaving the glass rod in a beaker. The evaporation of t'he alcohol is necessary on account of the solubility in an alcoholic solution of the fatty acids insoluble in water. V. As the fatty acids soluble in water require a large quantity of the latter. it is better to employ 20-23 per cent.alcohol, as it dissolves them readily without acting on the insoluble acids. After cooling, the glass rod, with the cake of fat adhering to it, is carefully lifted oiit, the water poured off and replaced by the alcohol described above, and the fat again put into the beaker and gently boiled for about eight minutes. After cooling, the liquid is poured off and the whole opera- tion repeated, when all the soluble fatty bodies will have been removed. VI. The cake is now dried by means of blotting paper, and removed from the rod into a small flat-bottomed dish, previously weighed, toge- ther with the particles of fat which may have adhered to the beaker; dried at 100-120", and weighed, the weight of the wax added being subtracted. VII. It is safe to assume that butter fat contains 88 per cent.of fatty acids insoluble in water. When the amount of acid found does not exceed 88 per cent., nothing but pure butter fat is present. When it, is between 88 and 89, the butter fat may have been adulterated with other fats. When this is the case, a wick should be impregnated with the fat, lighted, and blown out. If the well-known smell of a tallow- candle is not distinctly perceived, the butter may be considered to bequite pure. When the weight exceeds 89 per cent., the butter is certainly adulterated. J. M. T. By F. v. LEPEL (Deut. Chem. Ges. Ber., 11, 1552--1556).-Beetroot juice is used in colouring wines for the purpose of concealing the presence of " magenta." The absorption- bands of " magenta " are hidden by those of the beetroot ; but if a few drops of copper sulphate solution are added to the wine, the beetroot- bands gradually vanish, and the " magenta " spectrum becomes visible.To detect " magenta " in presence of an extract of tbe flowers of the vild poppy, Pupuver Rlmas, 1 drop of iodine solution (-01 gram per c.c.) is: added to the wine, before examination with the spectro- Detection of Wines Adulterated with Grape Sugar. By C. NEUBAUEE (Dh2gZ. poZyt. J., 229, 463-466).-After decolorising the wine, which, when examined in tubes 220 mm. long with Wild's large polaristrobometer, shows a slight dextro-rotation of 0.4 to 0.6" (1" Wild = 4,6043" Soleil = 2.89005" Ventzke-Soleil), 250 to 3.50 C.C. are concentrated until the salts begin to crystallise out. The concentrated solution is, after the addition of a sufficient quan- tity of pure aqimal charcoal, diluted to 50 c.c., and filtered.The filtrate, generally of a, faint yellow colour, shows with most wines a slight dextro-rotation in tubes 220 mm. long, which varies with pure Rhine, Haardt, and Markgrafler-wines, from the years 1874 to 1876 between 0.5 and 2". The 50 C.C. are next evaporated to R Adulteration of Wine. scope. w. c. w.ANALYTICAL CHEI1IISTRT. 83 syrupy mass on the water-bath, the residue being treated gradually and with careful stirring with a quantity of 90 per cent. alcohol, large enough to throw down all precipitable matter. After having allowed the mixture to stand for 6 to 8 hours, the alcohol is either poured off or filtered off, and the residue extracted with cold water.The solution is decolorised with animal charcoal and filtered. In all natural wines the dextro-rotatory substance is chiefly in this alcoholic precipitate. The alcoholic filtrate is evaporated h one-fourth of the volume originally added, and the cold solution treated gradually with four to six times its volume of ether, shaking the mixture the whole time. After standing, a more or less thick aqueous solution separates under the ether, which in wines containing potato-sugar contains the non-fermentable substances of these preparations, soluble in alcohol (amylin), and consequently shows a strong dextro-rotation. After removing the ether, the aqueous solution is diluted with water, warmed on the water-bath, to expel all ether, decolorised with animal charcoal, and the filtrate diluted according to the size of the observation-tube to the necessary volume.With pure natural wines of medium growths, which no longer contain unfermented sugar, the dextro-rotation of this aqueous solution of the ether precipitation from 250 to 350 C.C. of wine is, after discoloration and dilution to 30 C.C. either nil, as in most cases, or a t the most, 0.2" to 0.5". The tables given in the original paper show tjhat all wines having a rotation of 0.1" t o 0.3" to the right, may be regarded as perfectly pure. If, however, the dextro- rotation is 0.5" to O*Ci", it is more satisfactory to apply the abovc- described method. D. B. Alizarin Colouring Matters, and Green Aniline Colours. By H. W. VOGEL (Deut. C'henz. Ges. Bes., 11, l371-l374).-Alizarir~- bZue.-This body dissolves in water on addition of ammonia witch indigo-blue colour, and shows a two-sided absorption of the spectrum, which appeared considerably stronger in the red than in the dark blue, and no bands could be recognised.Supersaturated with nitric acid, the solution becomes brick-red, and exhibits an absorption similar to that of red litmus tincture with a dark shadow in the green. Amy1 alcohol extracts the colouring matter quickly from the acid solutio~i, but only with difficulty from the alkaline solution. Alcohol dissolvcs the colouring matter in the completely neutral condit'ion, with violet colour. Treated with ammonia, the solution becomes blue, like cupric sulphate solution, and exhibits in the concentrated state a continuous absorption of the red end of the spectrum, and on diluting with alcohol, a highly characteristic spectrum reaction for alizarin-blue is developed.This consists of three bauds, the weakest of which is on D, the second between d and C (daylight), and the third on the extreme limit of the red, and is perceptible only with the strongest lamp-light. Potash acts differently on the alcoholic alizarin-blue solution. It becomes of a beautiful green, and then absorbs on both sides, most stronglyat the red end of the spectrum, but without bands. The aqueous solution gives the same reaction. As regards detecting the colouring matter, it is best to warm the coloured fabric with dilute 9 2S4 ABSTRACTS OF CHELWCAL PAPERS. hydrochloric acid, extract the colouring matter with amyl alcohol, and treat this with alcohol and ammonia.AZiznrin-orarzge (nitro-alizarin) in alcoholic solution shows a strong extinction of the blue, and a weaker one of the green. With certain tlegrees of concentration bwo very indistinct bands are recognised in the green. With ammonia the solution becomes coloured reddish, and then shows a stronger absorption of the green. With nitric acid it becomes bright yellow, and gims a one-sided absorption of the blue. Potassium hydroxide colours the alcoholic solution a beautiful rose colour, and gives then a continuous extinction of the green from F to D, in which two bands appear. Aqueous solutions of the colouring matter with potash become yellowish-red, and show a homogeneous shade without bands in the green.The acid aqueous solution of the “ alizarin-orange ” is easily extracted with amyl alcohol, and then gives with alcohol and potash a definite spectral reaction. From coloured textures, it is extracted just as “ alizarin-blue ’’ is. Both “ iodine-green ” and metliylrosaniline picrate show in dilute alcoholic solution an absorption-band between d and C. ‘‘ Iodine- green ” shows further a weak band on the D line, which disappears on dilution. The concentrated alcoholic solutions of both colours diluted with water turn their absorption-band somewhat towards the green (difference from “aldehyde ” and “ malachite-green ”). A drop of nitric acid added to the alcoholic solution of the “iodine-green” effects no alteration in the bands (difference from “ aldehyde-green ”).The green picrate is tlirned bluer with nitric acid, and the bands widen towards the green. A drop of ammonia colours “iodine-green ” solution violet, with formation of a band on the D line. The green picrate does not show this reaction ; it becomes yellowish. By addition of ammonia to the nitric acid solutions of the colouring matter, the original colour and the spectral bands gradually return. Jfnlnchite-green, in its optical behaviour, exhibits striking resemblance to “ aldehyde-green,” but diff’ers from it in its chemical properties. The former dissolves much more easily in alcohol, and the solution appears bluer than that of “ aldehyde-green.” Dissolved in alcohol and suitably diluted, both give exactly the same spectrum. I n highly dilute solutions, one band appears on the d line, widening itself in con- centrated solution, and besides, a continuous absorption of the blue. The only difference between the two colours is that the “ aldehyde- green” weakens the red right and left from the absorption-band somewhat more strongly than “ malachite-green ; ” with the latter, the band appears, on the other hand, considerably darker.Although so similar in optical properties, the two colours differ decidedly in their behariour with acids. A drop of hydrochloric acid or nitric acid added to the alcoholic “ aldehyde-green ” effects no apparent, alteration of colour ; on the contrary, in the nitric acid solution a striking altera- tion of position of the absoibption-band to the right is remarked, whilst the band of the “ malachite-green ’’ does not suffer the least alteration. With ammonia, “ malachite-green ” is almost immediately decolorised.“ Aldehyde-green,” on the contrary, becomes gradually blue, with ap- pearance of three faint bands, of which the last lies in the extreme red, and can be recognised only by the aid of a very bright lamp-TECHNICAL CHEMISTRY. S .'i light; the second is between d and C, and the third and weakest on D. The colours are easily extracted froin the textures with alcohol, and can be determined in the solution by the prescribed reactions. w. s,ANALYTICAL CHEE?I1ISTRY. 77A n a1 y t i c a1 C h e m i s t r y.Colorimetric Experiments. By J. BOTTOMT~EI- ( Ch e m . News,38, 191-193). -Experiments were made t o determine, if possible,the amount of colouring matter in a liquid by compaiison with a,standard liquid.White disks were sunk in two equal cylinders, theone containing the standard liquid, the other that to be tested, i tbeing thought that the dept’h of the disk would be inversely as thequantity of the colouring matter present. It appears, however, thztthe method cannot, be practically employed, owing mainly to the diffi-culty of detecting the exact shades of colour.Schutzenberger’s Process for the Volumetric Estimation ofOxygen in Water. By C. c. HUTCHINSON (Chem. News, 38,184--187).-1n water containing sewage, oxygen is present in quan-tities below the normal, but the quantity increases as the sewage de-creases; in deep well-water, however, containing no sewage, it isstated there is an almost total absence of oxygen ; this may be owingto its having already been removed by organic matter during itspassage through the strata.To settle the question whether oxygen isor is mot an indication of the purity of water, the author was anxiousto employ some method more rapid than that of Bunsen’s for the de-termination of the amount of oxygm present, but it appears by theexperiments that the method which he proposed to ernploy is scarcelyaccurate enough, although it admits of grea.t rapidity, and is morcsuited for a small quantity than f o r a large quantity of water: it isalso valuable as R preliminary experiment. The method consists inE. W. P75 ABSTRACTS OF CHEMICAL PA4PERS.adding a known volume of the water to a solution capable of bein9oxidised, accompanied by a change of colour, by the oxygen containedin the water.The extent to which this has occurred is then deter-mined by the addition of a reducing agent, which reduces it to itsformer condition. This last solution is standardised in terms of theoxygen it is capable of taking up ; and from the amount used in theexperiment, the volume of oxygen present is calculated. The reducingagent employed is sodium hyposulphite, made by passing sulphurousanhydride to saturation into a solution of soda, sp. gr. 1.4, diluted tosp. gr. 1.34, and reducing the product with powdered zinc : milk of limeis then added, which precipitates the zinc and also renders the liquidless absorbent of free oxygen. The liquid by which the change of colourdetects the completion of the process is either sodium sulphindigotat,e,or Coupier's aniline blue ; 10 grams of the indigotate are dissolved in1 litre of water.An ammoniacal solution of copper sulphate con-taining 4.46 grams per litre is used to standardise the above solutions.The estimations must all be made in an atmosphere of hydrogen. Theprocess for determining the oxygen present is fully described, as wellas the method of standardising the solutions.Appendix to the Estimation of Carbonic Acid in the Air. ByW. HESSE (Zeitschr. j'. Biologie, 14, 29--33).--Having given someadditional directions with a view to avoid the introduction of carbonicacid from the outer air along with the baryta-water, the author re-commends the following method for ordinary purposes :-A solutionof oxalic acid of *5727 gram to the litre is prepared, and baryta-water, ofwhich 10 C.C. neut,ralise from 20 to 25 of this solution of oxalic acid,and volumes of air of about half a litre are used.According to whether4 to 5 per mil. or more of carbonic acid are expected, 10 to 20 C.C. ofbaryta-water are added. The pipette is inserted through an india-rubber stopper with two perforations, the escape of air from the flaskbeing regulated by the finger on the second apertrlre. The flask israpidly closed aftler removing the pipette. The numbers are often some-what too high. E. C. B.Quantitative Determination of Sulphur in IlluminatingGas. By POLECK and BIEFEL (Chem. Centr., 1878, 331).-Ameasured quantity of the gas to be examined is burned in air, and theproducts of the combustion drawn through an alkaline solution ofbromine by means of a water aspirator.The sulphur is determinedas barium sulphate. The gases examined by the authors were takenfrom t,he works a t Breslau, the experiments being made on the sameday, and as rapidly one after the other as possible. The followingresults were obtained :-E. W. P.Sulphur in 1,000 litres of gas,0.600 gram I n the retort house.. ..........Before the scrubbers .......... 0.540 ,,After passing the scrubbers.. .. 0.464 ,,After passing the condensers . . 0.440 ,,I n the finished gas.. .......... 0.276 ,,In the first four determinations, H,S is included ; and when CS, iANALYTICAL CHENISTRY. 71)separately determined in the finished gas, the residual sulphur may beconsidered as belonging to the so-called sulphuretted hydrocarbon,the smell of which resembles phenyl mustard-oil.J. M. T.Estimation of Nitric Acid as Ammonia. By E. A. GRETE(Deut. Chem. Ges. Ber., 11, 1557-1558).-Nitrates are completelyreduced to ammonia by heating to redness with soda lime and aEstimation of Nitrous and Nitric Acids. By G. LUNGE(Diwgl. polyt. J., 228, 447-4501 .-Lange has constructed an a pparatus for determining the above acids, which is a modification ofWatts’ apparatus described by Davis (Chem. News, 37, 4.5), andresembles Runte’s modification of Rauch’s gas burette. This im-proved form has no trough, arid requires but little more mercury thanis necessary to fill the tube (about 830 grams) ; it is easily cleaned outafter every operation, and has the advantage of the mercury notcoming into direct contact with the worker.Lunge calls it a “ nitro-meter. ” D. B.xant hogenat e. w. c. w.Behaviour of Quartz with Microcosmic Salt. By E. LAUFER(Deut. Chem. GRS. Ber., 11, 935).-1n a former paper, the author de-scribed a method of separating quartz from admixtures with silicatesby fusion with microcosmic salt, which it was then thought decom-posed silicates without attacking quartz. But further experiment hasshown that the method cannot be relied upon, inasmuch as quartzibelf, especially when finely powdered, is acted on by the fused salt.J. R.Testing and Valuing Gas Liquor.By T. H. DAVIS (Qheliz.News, 38, 193--195).-Gas liquor, or a crude solution of ammoniasalts, is generally sold on the basis of its sp. gr., or on its degree(Twaddle). This test is, however, untrustworthy, although an indica-tion of the “ strength ” of the liquor is obtained. Now, as the ammoniais that for which the manufacturer contracts, i t is recommended to titratethe ‘liquor as follows :-Into it flask of about 300 C.C. capacity 10 C.C.of the sample to be tested are run in, and into this 15 C.C. of nornialsulphuric acid. The contents of the flask are then raised to boiling, afew drops of litmus added, and titrated back with normal soda. Theniimber of C.C. of soda used are deducted from the 15 C.C. of acid em-ployed, the result multiplied by 17, and divided by the specific gravityof the liquor.The result thus obtained represents the percentage ofammonia contained in the liquor.Remarks on the Estimation of Calcium Sulphate in Beer.By H. M. WLLSON (Chem.. News, 38, 197).-Organic matterappears to interfere with the complete precipitation of the sulphuricacid in beer as barium sulphate. It is advisable, therefore, in the firstinstance to evaporate 100 C.C. of the sample to dryness, and after theaddition of 0.5 gram potassium nitrate, to ignite the residue.E. W. P.E. W. PSO ABSTRACTS OF CHEhlICAL PAPERS.Presence of Lead in Bismuth Subnitrate. By CHAPIUS andJANNOSSIER (Conyt. rend., 87, 1G9--171).--Carnot has shown thata11 samples of bismuth subnitrate of commerce contain lead; some-times in qiiantities dangerous for public safety.The authors of thepresent pxper propose the followinq method for the quantitative detec-tion of the lead. The bismuth nitrate to be examined is boiled withcaustic soda and n small quantity of potassium chromate, the residue,after boiling, being thrown upon a filter. To the filtered liquid, aceticacid is added until the solution is j u s t acid, when a yellow precipitate isproduced, more or less pronounced, according t o the amount of lendpresent. For & an abundant precipitate is obtained ; for thecloudiness of the liquid is distinct, and a dcposition very soon takesplace in the form of a precipitate adhering to the sides of the tube ;lead chromate is slightly soluble in the mixture of sodic acetate andacetic acid ; smaller quantities could be detected if the weight of sub-stance used was increased.After mentioning that both calcium phosphate containing silica oralumina, and also impure soda interfere with the reaction, he describesthe following quantitative method similar to that described for thequalitative detection.About 10 grarns of the bismuth nitrate are used, care being takento wash the chromate of bismuth with a mixture of potassium chromateand sodium hydrate, first by decantation, and then on the filter until thefiltrate is no lbnger rendered turbid by acetic acid in excess.Thefiltrate is now boiled, supersaturated with acetic acid, allowed to stmd24 hours, and filtered. The precipitate is then washed with waterslightly acidulated by acetic acid, dried a t 100" and weighed.Theweight, found, multiplied by 0.6408, gives the weight of lead containedin the 10 grams of substance.Estimation of Nitrogen in Organic Bodies. By E. A. GRETH(Deut. Chew,. Ges. Ber., 11, 1558).-In estimating the nitrogen inhorn, leather, and wool refuse, the author advocates dissolring thesubstance in warm concentrated sulphuric acid before heating withsoda-lime. Higher results are obtained than by the ordinary pro-cess. w. c. w.-___ ;Idoo shows only slight cloudiness, often appearing only on cooling, asJ. M. T.New and Rapid Process for the Analysis of Milk. By A.ADAM (Compt. relid., 87, 290-291) .-The analysis is performedby means of an apparatus consisting essentially of a glass tube ofabout 40 C.C.capacity, provided with a stopper a t the top, expandedin the middle, and tapered off a t the bottom, which is closed by aglass stopcock. Into this appai-atus is introduced 10 C.C. of alcoholof 75", containing of its volume of sodic hydrate ; then 10 C.C. ofmilk, which must be neutral ; and finally, 12 C.C. of pure ether. Theliquids are shaken together, and allowed to remain a t rest for fiveminutes, when they separate into two layers: the clear upper one con-tains all the butter; the lower, the lactose and case'in. The buttercontained i n the former is estimated by eraporating and weighing,allowing 1 centigram for a little case'in, &c., which may be conANALYTICAL CHENISTRY. 81tained in the liquid, or eliminating this by re-solution in ether.Inthe liquid first drawn off, the lactose and casein are estimated bymaking up to 100 C.C. with distilled water, and adding 10 drops ofacetic acid ; the casein then separates, and after having been removedby filtration, is pressed between folds of bibulous paper, dried, andweighed. The filtrate contains the salts of the milk, the acetate ofsodium formed, and the lactose. The latter is estimated by means ofFehling's cupro-potassic liquid. All these operations are easily per-formed in an hour and a half; and if, a t the commencement? 10 C.C.of the milk acidulated with two drops of acetic acid are set to evapo-rate, the weights of dry residue, ash, and water may be obtainedwithin the same time.R. R.Butter Analysis. By H. HAGER (Chew. Centr., 1878, 333-334).-1. 20.0 parts of the butter to be analysed, together with 3.0 to 4.0parts of pure sodium chloride, are placed in a weighed glass vessel, andthe whole is weighed and heated to 50-80" in a water-bath, when thefatty part forms a yellowish layer on the top, whilst the water, casei'n,and salt remain at the bottom. Two portions of 5.0 parts of the clearfat are placed in glass flasks of about 12.0 C.C. for further investiga-tion, as described in 111.11. Estiwation of nii'disture, Casein, a d Salt.-The fat is decanted asfar as possible; then 10 C.C. of warm benzene are added and gentlyagitated with the liquid, so as to take up the rest of the fat. Thevessel is t,hen allowed to stand in a warm place for half-an-hour, whenthe benzene is poured off and 10 C.C. more are added to remove thelast traces of fat.The liquid is allowed to stand for half-an-hourlonger in a warm place to remove the last traces of benzene, and thevessel and its contents are again weighed; this, after subtracting the3 . 0 4 . 0 NaCl added, gives the weight the total moisture, casei'n, audsalt. The residue is then treated with hot water and filtered. Thcfiltrate evaporated to dryness gives, after subtracting the NaCl added,the salt in the butter.111. Snponijication of the Butter Fat.-To the 5 grams of fat in theflask, 20 C.C. of alcohol are added, and 10 C.C. of a freshly-preparedsolution of 2.0 grams of pure caustic soda in 10.0 of distilled water; thewhole is then agitated and heated to 50-60°, when the flask is corkedand violently shaken.The alcohol prevents frothing. After a fewmoments' rest, small particles of fat are observed if the saponifica-tion is not complete. When this is the case, the flask is uncorked audagain heated ; recorked, wrapped in a towel, and shaken ; it is scarcelyever necessary to repeat the operation a third time. The author saysthat it takes about 6-8 minutes for complete saponification.IV. The warm soap-solution is poured into a large beaker, andthe flask washed out with 45 per cent. alcohol. The solution is thenwarmed without boiling, so as to evaporate as much as possible of thealcohol ; 3-4 C.C. do not interfere with the following reactions. Alittle warm water is added, and then 20.0 of previously warmed dilutesulphnric acid (1 : 5 water), and stirred; water is then poured in untilthe level of the liquid is about 2 c.below the mouth of the beaker.Aft,er the fat has completely separated out in the water-bath or otherThe casein remains on the filter.VOL. XXXVI. a2 ABSTRACTS OF CHEXICAL PAPERS.warm place, 5.0 of perfectly dry white wax or paraffin are added,heated to melting, and the whole placed in a cool place to solidify,leaving the glass rod in a beaker. The evaporation of t'he alcohol isnecessary on account of the solubility in an alcoholic solution of thefatty acids insoluble in water.V. As the fatty acids soluble in water require a large quantity ofthe latter. it is better to employ 20-23 per cent.alcohol, as it dissolvesthem readily without acting on the insoluble acids. After cooling, theglass rod, with the cake of fat adhering to it, is carefully lifted oiit,the water poured off and replaced by the alcohol described above, andthe fat again put into the beaker and gently boiled for about eightminutes. After cooling, the liquid is poured off and the whole opera-tion repeated, when all the soluble fatty bodies will have been removed.VI. The cake is now dried by means of blotting paper, and removedfrom the rod into a small flat-bottomed dish, previously weighed, toge-ther with the particles of fat which may have adhered to the beaker;dried at 100-120", and weighed, the weight of the wax added beingsubtracted.VII.It is safe to assume that butter fat contains 88 per cent. offatty acids insoluble in water. When the amount of acid found doesnot exceed 88 per cent., nothing but pure butter fat is present. Whenit, is between 88 and 89, the butter fat may have been adulterated withother fats. When this is the case, a wick should be impregnated withthe fat, lighted, and blown out. If the well-known smell of a tallow-candle is not distinctly perceived, the butter may be considered tobequite pure. When the weight exceeds 89 per cent., the butter iscertainly adulterated. J. M. T.By F. v. LEPEL (Deut. Chem. Ges. Ber.,11, 1552--1556).-Beetroot juice is used in colouring wines for thepurpose of concealing the presence of " magenta." The absorption-bands of " magenta " are hidden by those of the beetroot ; but if a fewdrops of copper sulphate solution are added to the wine, the beetroot-bands gradually vanish, and the " magenta " spectrum becomes visible.To detect " magenta " in presence of an extract of tbe flowers of thevild poppy, Pupuver Rlmas, 1 drop of iodine solution (-01 gramper c.c.) is: added to the wine, before examination with the spectro-Detection of Wines Adulterated with Grape Sugar.By C.NEUBAUEE (Dh2gZ. poZyt. J., 229, 463-466).-After decolorising thewine, which, when examined in tubes 220 mm. long with Wild'slarge polaristrobometer, shows a slight dextro-rotation of 0.4 to0.6" (1" Wild = 4,6043" Soleil = 2.89005" Ventzke-Soleil), 250 to3.50 C.C. are concentrated until the salts begin to crystallise out.The concentrated solution is, after the addition of a sufficient quan-tity of pure aqimal charcoal, diluted to 50 c.c., and filtered.Thefiltrate, generally of a, faint yellow colour, shows with most winesa slight dextro-rotation in tubes 220 mm. long, which varies withpure Rhine, Haardt, and Markgrafler-wines, from the years 1874to 1876 between 0.5 and 2". The 50 C.C. are next evaporated to RAdulteration of Wine.scope. w. c. wANALYTICAL CHEI1IISTRT. 83syrupy mass on the water-bath, the residue being treated graduallyand with careful stirring with a quantity of 90 per cent. alcohol,large enough to throw down all precipitable matter. After havingallowed the mixture to stand for 6 to 8 hours, the alcohol is eitherpoured off or filtered off, and the residue extracted with cold water.The solution is decolorised with animal charcoal and filtered. In allnatural wines the dextro-rotatory substance is chiefly in this alcoholicprecipitate. The alcoholic filtrate is evaporated h one-fourth of thevolume originally added, and the cold solution treated gradually withfour to six times its volume of ether, shaking the mixture the wholetime.After standing, a more or less thick aqueous solution separatesunder the ether, which in wines containing potato-sugar contains thenon-fermentable substances of these preparations, soluble in alcohol(amylin), and consequently shows a strong dextro-rotation. Afterremoving the ether, the aqueous solution is diluted with water, warmedon the water-bath, to expel all ether, decolorised with animal charcoal,and the filtrate diluted according to the size of the observation-tube tothe necessary volume.With pure natural wines of medium growths,which no longer contain unfermented sugar, the dextro-rotation ofthis aqueous solution of the ether precipitation from 250 to 350 C.C. ofwine is, after discoloration and dilution to 30 C.C. either nil, as inmost cases, or a t the most, 0.2" to 0.5". The tables given in theoriginal paper show tjhat all wines having a rotation of 0.1" t o 0.3" tothe right, may be regarded as perfectly pure. If, however, the dextro-rotation is 0.5" to O*Ci", it is more satisfactory to apply the abovc-described method. D. B.Alizarin Colouring Matters, and Green Aniline Colours.By H.W. VOGEL (Deut. C'henz. Ges. Bes., 11, l371-l374).-Alizarir~-bZue.-This body dissolves in water on addition of ammonia witchindigo-blue colour, and shows a two-sided absorption of the spectrum,which appeared considerably stronger in the red than in the dark blue,and no bands could be recognised. Supersaturated with nitric acid,the solution becomes brick-red, and exhibits an absorption similar tothat of red litmus tincture with a dark shadow in the green. Amy1alcohol extracts the colouring matter quickly from the acid solutio~i,but only with difficulty from the alkaline solution. Alcohol dissolvcsthe colouring matter in the completely neutral condit'ion, with violetcolour. Treated with ammonia, the solution becomes blue, like cupricsulphate solution, and exhibits in the concentrated state a continuousabsorption of the red end of the spectrum, and on diluting with alcohol,a highly characteristic spectrum reaction for alizarin-blue is developed.This consists of three bauds, the weakest of which is on D, thesecond between d and C (daylight), and the third on the extreme limitof the red, and is perceptible only with the strongest lamp-light.Potash acts differently on the alcoholic alizarin-blue solution.Itbecomes of a beautiful green, and then absorbs on both sides, moststronglyat the red end of the spectrum, but without bands. Theaqueous solution gives the same reaction. As regards detecting thecolouring matter, it is best to warm the coloured fabric with dilute9 S4 ABSTRACTS OF CHELWCAL PAPERS.hydrochloric acid, extract the colouring matter with amyl alcohol,and treat this with alcohol and ammonia.AZiznrin-orarzge (nitro-alizarin) in alcoholic solution shows a strongextinction of the blue, and a weaker one of the green.With certaintlegrees of concentration bwo very indistinct bands are recognised inthe green. With ammonia the solution becomes coloured reddish, andthen shows a stronger absorption of the green. With nitric acid itbecomes bright yellow, and gims a one-sided absorption of the blue.Potassium hydroxide colours the alcoholic solution a beautiful rosecolour, and gives then a continuous extinction of the green from F toD, in which two bands appear. Aqueous solutions of the colouringmatter with potash become yellowish-red, and show a homogeneousshade without bands in the green.The acid aqueous solution of the“ alizarin-orange ” is easily extracted with amyl alcohol, and thengives with alcohol and potash a definite spectral reaction. Fromcoloured textures, it is extracted just as “ alizarin-blue ’’ is.Both “ iodine-green ” and metliylrosaniline picrate show in dilutealcoholic solution an absorption-band between d and C. ‘‘ Iodine-green ” shows further a weak band on the D line, which disappears ondilution. The concentrated alcoholic solutions of both colours dilutedwith water turn their absorption-band somewhat towards the green(difference from “aldehyde ” and “ malachite-green ”). A drop ofnitric acid added to the alcoholic solution of the “iodine-green” effectsno alteration in the bands (difference from “ aldehyde-green ”). Thegreen picrate is tlirned bluer with nitric acid, and the bands widentowards the green. A drop of ammonia colours “iodine-green ”solution violet, with formation of a band on the D line. The greenpicrate does not show this reaction ; it becomes yellowish. By additionof ammonia to the nitric acid solutions of the colouring matter, theoriginal colour and the spectral bands gradually return.Jfnlnchite-green, in its optical behaviour, exhibits striking resemblanceto “ aldehyde-green,” but diff’ers from it in its chemical properties.The former dissolves much more easily in alcohol, and the solutionappears bluer than that of “ aldehyde-green.” Dissolved in alcoholand suitably diluted, both give exactly the same spectrum. I n highlydilute solutions, one band appears on the d line, widening itself in con-centrated solution, and besides, a continuous absorption of the blue.The only difference between the two colours is that the “ aldehyde-green” weakens the red right and left from the absorption-bandsomewhat more strongly than “ malachite-green ; ” with the latter, theband appears, on the other hand, considerably darker. Although sosimilar in optical properties, the two colours differ decidedly in theirbehariour with acids. A drop of hydrochloric acid or nitric acidadded to the alcoholic “ aldehyde-green ” effects no apparent, alterationof colour ; on the contrary, in the nitric acid solution a striking altera-tion of position of the absoibption-band to the right is remarked, whilstthe band of the “ malachite-green ’’ does not suffer the least alteration.With ammonia, “ malachite-green ” is almost immediately decolorised.“ Aldehyde-green,” on the contrary, becomes gradually blue, with ap-pearance of three faint bands, of which the last lies in the extremered, and can be recognised only by the aid of a very bright lampTECHNICAL CHEMISTRY. S .'ilight; the second is between d and C, and the third and weakest onD. The colours are easily extracted froin the textures with alcohol,and can be determined in the solution by the prescribed reactions. w. s

ISSN:0368-1769    

DOI:10.1039/CA8793600077

出版商:RSC    

年代:1879

数据来源: RSC

摘要:

TECHNICAL CHEMISTRY. T e c h n i c a1 C h e m i s t r y. Gas Lighting. By J. VAN EYNDHOVEN (Dingl. polyt. J., 229, 449).-It has been supposed that the gas flame is translucent. As, however, this appeared doubtful to the author, he determined to in- vestigate the subject. The experiments were made with the aid of an excellent photometer, the results being as follows :- The first experiments were madewith a bat's-wing burlier of 160 litres' gas consumption a t 8.3 mm. pressure. The result of ten observations proved that the lighting power of the flat side was equal to 11.58, that of the narrow edge 10.04 candles. After correction for barometer and thermometer, the actual lighting power for normal consumption of gas and candle is 11.81 and 10.18 candles: English spermaceti candles with a normal consumption of 120 grains were used.For a flame consuming 100 1. of gas per hour, the actual illuminating power on the flat side was 9.03, on the narrow edge 7-42 candles, m7it.h a gas pressure of 4 mm. The difference in both cases is 1.5 candles, or 1 7 to 18 per cent., a circumstance which proves that the flame is not translucent, a bat's-wing burner giving most light on its flat side. An argand burner will from a similar cause not give all its illumina- ting power. For a good street illumination, therefore, the slits of the burners and the direction of the road must be placed perpendicularly on one another. D. B. Some Peculiarities of the Vartry Water, and the Action of that Water on Boiler-plates. B,y C. R. C. 'YICHUORNE (Cheiri,. News, 38, 191).-The water of the River Vartry consists of organic matter of a peaty nature, and mineral matter, which consists chiefly of the chlorides of the alkalis and of the alkaline earths; nitrates and nitrites are also present, which, however, cannot be detected with- out evaporation, but as concentration by heat reduces the nitrates, the water was concentrated in a vacuum.This reduction, when it takes place in high pressure boilers, is a cause of the corrosion of the boiler plates, It was found that when iron was heated with nitrates in sealed glass tubes it became oxidised. E. W. P. Preservation of Potable Water. By H. SCHIFF (Deut. Chem. Ges. Ber., 11, 1528--1529).-Water containing 3 parts of salicylic acid in 10,000 was found to be fresh after remaining in a flask for three years.Sea-water to which phenol or, preferably, carbon bisulphide (1 part to 1,000) has been added, forms a good preservative fluid for specimens of marine fauna. w. c. w.86 ABSTRACTS OF CHEJIICAL PAPERS. Utilisation of Suint from Wool. By F. FISCHER (Dim$. polyt. J., 229, 446--449).-1t is known that raw wool contains about 90 per cent. of suint soluble in cold water, consisting of the potassium compounds of oleic, stearic, and acetic acids, a small amount of valeric acid, and many other organic substances, also of potassium chloride and sulphate, ammonium salts, and especially potassium carbonate, and sodium compounds. By lixiviating wool with water, a dark brown liquid of peculiar smell is obtained, of sp. gr. 1.069; I. litre of this required, for neutrali- sation, a quantity of normal acid corresponding with 3.98 grams of potassium carbonate.By neutralising 1 litre of liquor with hydrochloric acid and shaking up with benzene, only 916 milligrams of a yellow strongly smelling fat were obtained. By evaporating 1 litre and drying at 120°, 122.16 grams of a hygroscopic mass remained, which on igni- tion swelled up considerably, and evolved a, gas burning with a bright flame. By continued heating in the air, and extracting with water and evaporating, 72.16 grams of a white saline mass, and 2.98 grams of a residue consisting of sand, alumina, lime, and phosphoric acid re- sulted. By burning the suint dried at 120" in a stream of oxygen, 3.04 per cent. of hydrogen as water and 19.92 per cent. of carbon 8s carbonic acid were obtained.The organic compounds of potassium are hereby converted into potassium carbonate. A profitable recovery of the fat and the acetic acid is impossible, but the utilisation of the evaporated mass for gas and the production of potash can be recommended. For obtaining the potash present i r i the mass, the latter is in Germany merely heated strongly in rever- beratory furnaces, the gas formed being used as fuel. Analyses of the composition of the flue gases showed that carbon monoxide is, in spitc of the sooty nature of the flame, formed very rarely, and only when the mass is at its highest heat, in which case oxygen disappears. As soon as the evaporated liquors begin to burn, the heat evolved suffices to destroy all organic matter present.Thus with 1 kilo. of Westphalian coal 12 kilos. of liquom can be evaporated and ignited. The coke formed is solid. The following is the analysis of the coal dried a t 120" :- C. H. S. 0 (and N). Ash. 76.11 4.52 1-19 10.06 8-12 The raw potash taken from the furnace gave- Salts soluble in water. Insoluble. Organic matter. 92-05 4.92 3-03 The composition of the soluble salts was as follows:- K,C03. KC1. KZSO4. NasCO3. 85.34 6-15 2.98 5.02 = 99.49 p.c. W. Graff, in Lesum, works up this raw potash from six establishments for washing wool into pure potassium carbonate, bicarbonate, chloride, and sulphate. He employs about 10 to 12 workmen, the annual sale amounting to about 120,000 marks. D. B.TECHXICAL CHEMISTRY. 87 Ingredients. Analyses of Clays. (Dingl.polyt. J., 229, 451455).--Glaze- clay.-As a very durable, perfectly impervious glaze on refractory clay, e.g., for Bunzlau vessels, water pipes, &c., a very readily fusible clay 18 often used. Seger has analysed three specimens of t'hese earthy glazes with the following results :- A. 58-99 11.73 4.16 4-77 1.83 4.83 16-19 4.80 B. 64.49 14.35 4.38 4.13 1-53 3.69 3.12 3.31 C. 62.40 15.51 5-68 4.36 1-13 3.62 2.88 4.41 A is one from Naumburg 0. Q, used in Bunzlau for the manufacture of brown kitchen utensils and water pipes ; B from Camenz i. S., used for the same purpose, and C is a glaze from the clay pipe manufactory in Dommitzsch 0. Elbe. The pyrometric investigations showed that, according to Seger's quotients of refractoriness (ibid., 228, 2M), the Naumburg glaze was the most readily fusible, that of Dommitzsch the most difficultly fusible.Stoneware-cZa$.-This clay, obtained from Hohr, and representing the raw material used for the manufacture of the fine, compact, pearl-grey vessels a t that place, had the following composition : H20 and SiO,. A1,03. Fe203. CaO. MgO. Alkalis. CO2. organic matter. Si02. Al,O,. Fe203. CaO. MgO. K20and N%O. H,O. 70.12 21.43 0.77 0.00 0.39 2-62 4.92 By sulphuric acid. Wilkins has already pointed out the important influence which a large amount of silica in clay has on the lustre and the fineness of the salt-glaze ; an observation which confirms the ready acceptation of the salt-glaze and the peculiar compactness of the above mass. Porcelain Eurth of Linzoges.-These clays are not merely distin- guished by the fineness of their forms, but the mass itself possesses a purer, more agreeable coloration, and greater fineness and strong trans- parency than the greater number of the German productions. The following is the composition of the kaolin :- i I Si02 .................... Fe203.................... CaO .................... MgO .................... K,O .................... Na.20 .................... Loss by ignition .......... A120,. ................... 58 -39 27.52 0.36 1 -52 0 '41 1 -71 2 *58 7 -19 99 -68 32 222 7.49 - 4'40 J - 26 *17 20 '03 0 -36 1 -82 7 -19 Clay sub- stance decomposible sulphuric acid. bY 47 '09 36 *04 0 '64 3 *27 12 -9488 ABSTRACTS OF CHEMICAL PAPERS. Kot decom- posible Corresponding with- Clay substance ................55.88 Quartz:. ....................... 5.95 Felspar. ....................... 38.1 7 Compared with the composition of the German and Austrian kaolins (ihid., 228, 67), this substance is distinguished by an unusually high percentage of felspar, which explains also the fact that in S h e s the mass is not mixed with felspar but merely with sand. The porcelain from Limoges had the following composition :- Decompos- ible Ingredients. SiOa .................... CaO .................... MgO .................... K20 ..................... 8 1 2 0 3 . . .................. FezO,. ................... N+O .................... Loss by ignition .......... 66 -71 21 '58 0 '47 0 -61 0 -37 2.93 1 -62 5 -54 99-83 - 47 -27 5 '93 1 3'76 - - 19 '44 15 -65' 0 -47 1 -77 5 -54 Composition of the clay substance.45 -35 36 -50 1.09 4 *13 12.92 corresponding with clay substance = 43.04, quartz 26.46, and felspar 30.50. The mass contains therefore more sodium, lime, and magnesia than, e.g., the Berlin porcelain, a circumstance which explains its ready fusibility and greater transparency. The glaze from Limoges consists of- SiOp. A1203. Fe203. CaO. Ingredients in p. c.. ............... 74.99 14.80 0.37 1.09 Not decomposible by sulphuric acid. . 70.92 12.38 - 0.20 Decomposible by sulphuric acid .... 4.07 2.42 0.37 0.89 Ingredients in p. c.. ............... 0.36 4.31 3.49 0.65 Loss by MgO. K20. NasO. ignition. Not decomposible by sulphuric acid . . 0.36 7 4 7 Decomyosible by sulphuric acid .... - 0.68 - 0.60 liurstenu?aZd-gZaxe.-This glaze adheres in the form of sand to the lignite strata, and is used in the preparation of the lead and tin enamels for the fabrication of stoves.According to Seger, the mass dried a t 120" has the following composition :-TECHNICAL CHEMISTRY s 89 H,O and carbon- Si02. A1,03. Fe,O,. MgO. E@. aceous matter. Total.. . . . . . . . . . , . . 85.96 7.30 2.26 0.25 1.97 2.11, - Not decomposible by U HZSOa ....... . .. 80.03 2.69 - 1-08 substance.. . . . . . . 5.93 4.61 2.22 1.14 2.12 Eatable-cZay.-Pattison Muir has investigated a clay-substance from Mackenzie County, in South Island, near New Zealand, which is eaten by men and sheep in large quantities. It has the following compos’ , I t’ ion :- Decomposible clay Si02. Al,03. Fe,03. CaO. MgO. NaC1. n20. Organic. 61-25 17.97 5.72 1-91 0.87 3.69 7.31 1.77 (according to R.Biedermann in Noiizb. d. Ver. fur Fuh. zo?z Ziegel?z. 1878, 229). Gross~Zme?.ode-cZay.-This clay is highly refractory and possesses great cementing power. It is coloured light bluish-grey to white, is shiny, and breaks up in water to a fine slimy mass. The following is the composition of the clay dried a t 120’ :- SiO,. r 1. - Chemically Mechanically Loss by AI203. combined. added. MgO. CaO. Fe203. K20. S. ignition. 34.52 43.38 6.53 0.73 0.76 1.66 1.51 0.26 11-04 This gives a chemical composition: 4.89(A1203, 1.65 SiO,) + RO, and the quotient of refractoriness (according to Bischof) = 2.96. D. B. Blair’s Process for Iron Manufacture. By J . IRELAND (Dingl. polyt. J., 229, 458--461).-This paper gives a detailed account of the improvements which have been recently made in the working plant, also in the method of preparing iron sponge.A brief descrip- tion of the reduction furnaces is given; these consist of a group of three vertical retorts, each retort having a diameter of 914 mm., and being 8.53 m. high. The furnace is surrounded by an outer casing of brickwork, leaving a combustion chamber between the inside of it and the outside of the retorts. The retorts were heated externally by gas jets, the air for combustion being supplied through apertures immediately above the gas jets. I n 1876 Blair discovered, that by the addition of a small quantity of alkali to the carbonaceous matter mixed with the ore, the action of reduction was facilitated to a great extent, and ore which took about thirty hours to reduce without alkali, could be per- fectly reduced in six hours with it.The existing furnaces, however, could not be altered in any way to suit the new condition of quickened reduction. Blair therefore abandoned the whole principle of heating, and adopted a system by which a stream of hot carbonic oxide was passed through the mass of ore and carbonaceous matter. The author, however, made use of the above furnace by dividing the cast-iron pipe inserted in the top of each retort into a number of smaller ones, so as90 ABSTRACTS OF CHEMICAL PAPERS. to present as small a column of materials to the action of heat as pos- sible. He used a furnace of a height of 6.4 m., the retort, being about 3.2 m. high, with four inserted tubes. A fiirnace of this description, 1.52 m.diameter and 12.92 m. high, produces from 60 to 70 tons of iron, and costs about 12,000 marks. The cost of producing iron sponge will vary according to the locality in which'the work is carried on, but with the furnaces intro- duced by Blair, the cost will be about 22 marks per ton, exclusive of the ore. Where several of the furnaces are in operation, the cost is less. Where the oye is rich and pure, iron sponge made from it can be a t once made into tool steel, the quality of which cannot be equalled by that made from the best brands of Swedish bars. I n the case of ore which is not so rich, the best way of utilising the sponge made from it is to melt i t in a cupola furnace, transferring the molten mass to a Siemens-Martin furnace, wherein the mass is converted into steel.The pig metal obtained in this manner will coiitain about 1.5 per cent. carbon and 0.19 per cent. to 0.25 per cent. silicon. D. B. Phosphorus in Cleveland Ironstone and in Iron. By J. E. STEAD (Chew,. News, 38, 14-18 ; 29-31 and 39-42).--This paper may be divided into six sections: (1.) The compound or com- pounds in which phosphoric acid exists in the Cleveland ironstone. (2.) Method of eliminating phosphoric acid from iron ores. (3.) The compound in which phosphorus exists in Cleveland metal. (4.) The effect, physically and chemically considered, which phosphorus has on pig metal. (5.) Method of removing it from pig iron. (6.) Phos- phorus in bar iron. The following are the results of the analysis of the main Cleveland ironstone bed :- Iron in the Stone Siliceous Phosphoric Loss by calcined analysed.Iron. matter. acid. Moisture. calcination. stone. Main: p. c. p. c. p. c. p. c. p. c. p. c. (1st foot 26.53 18.30 1.46 8.50 27.39 36.50 2nd ,, 29.54 10.90 1.13 9-10 29.80 42.08 3rd ,, 29.14 10.68 1-13 9.50 29.80 41.50 4th ,, 28.41 11.98 1.41 9-80 28.80 39-92 5th ,, 29.97 9.00 1.17 10.00 30.83 43.31 6th ,, 30.42 8.82 0.89 10.00 31.51 44.40 7th ,, 29.70 9-00 0.80 10.10 31.78 43-53 8th ,, 29-85 9.29 0.91 9-80 30.90 45-20 9.00 28.50 42.40 C9th ,, 30.30 12.01. 1.16 Black hard. 4 7 inches 30.56 12-90 0.44 8.50 26.80 41.75 *s {; ,, 37-87 22.20 1-12 5-50 18.00 34.00 ,, 27-26 24.70 0.81 5-00 17.00 32.85 It will be seen from these analyses that no part of the stone is free from phosphoric acid.In the " Black Hard " bed, the author found this substance very variable in quantity, reaching as much as 3 per cent. in some cases, and only 0.25 per ceut. in others. d CJTECHNICAL CBEJIISTRT. 91 1. As to the form in which phosphoric acid exists in Cleveland ironstone, the author mentions that several years ago Pattinson inves- tigated this matter and concluded, judging from the non-action of ammonium sulphide on the stone, or rather on the compound contain- ing phosphoric acid in the stone, that no iron phosphate was present, and that the phosphoric acid must be in combination with lime ; and the results obtained by other methods of investigation employed by the author has confirmed this. It is the prevailing opinion that the source of all the phosphorus in the ironstone is the remains of small phosphatic animals ; but this theory cannot be regarded as trustworthy, first, because in some parts of the “ Black Hard ” bed, where no fossil remains could be detected, the phosphoric acid has been found in large quantity, and secondly, because in all cases, on analysis, the shells and fossil remains which were taken out of the stone, were proved to con- tain much less phosphoric acid than the surrounding ironstone.The following analyses of fossil wood taken from various mines in that disirict will throw some light upon this very obscure subject. Fossilised mood found in Cleveland ironstone- OH,. C. SiO,. (20%. SO3. S. MU. d1203. 3.00 9-60 0.50 0.75 0-GO 7-56 trace 8.25 COO and NiO. Co and Ni. Fe. FeO. MgO.P,05. CaO. 3.70 1-65 5.20 10.02 1.12 20.80 27.60 Several other samples gave similar results on analysis. There can be no doubt about the fact, that these samples were at one time parts of trees, which in their natural state would not, contain more than very minute quantities of phosphoric acid. The latter must have been in solution, and has in this state passed into the substance of the wood and been there deposited in the condition in which we find it. 2. Method of Removing Phosphoric Acid from Ores.- Jacob’s method, based on the treatment of the ores with sulphurous acid produced by burning sulphur pyrites and condensing the acid fumes in coke towers, gave satisfactory results only when the stone was reduced to a very fine powder, about 90 per cent. of phosphoric acid being removed thereby.Forbes’ method, based on the action of common salt on iron phosphate when fused, also gave unsatisfactory results, as did the last method referred to by the author, the action of sodium carbonate on phosphate of lime when fused with it. From this it would seem that Cleveland ironstone cannot be freed from phosphorus by any methods as yet proposed. With regard t o the smelting of ironstone, since we know that phosphate of lime heated with carbon aud iron oxides, or metallic iron, to a very high temperature, is decomposed, the phos- phorus combining with the iron, it is to be expected that nearly all of the phosphorus introduced in the charge at the top of the blast-furnace, will be found concentrated in the pig metal. Experiments showed that fluorspar is of no value in removing the phosphoric acid or preventing its passage into the metal when employed as a flux in smelting.Iro?z a i d Phosphorus.--By direct addition of phosphorus to iron heated in a crucible, the author obtained combinations containing between 6 mid92 ABSTRACTS OF CHEMICAL PBPERS. 27 per cent. of phosphorus, although Percy has stated that iron will not take up more than 8.4 per cent. of phosphorus when the two substances are heated together in the manner described. The fusion point appears to decrease with each addition of phosphorus, until a com- pound containing from 10 to 12 per cent. of phosphorus is produced, which is the most fusible ; after which each addition makes the com- pound less and less fusible. 3. The Co~npount7s in which Phosphwus exists in Clemdand Jfeta1.- Judging from the comparative fusibility of iron, it was thought that if separate compounds of iron and phosphorus existed in pig metal, these compounds would be more fusible than the bulk.Analyses of about 1 cwt. of Cleveland iron poured into a mould were made. After the mass had become viscous, extreme pressure was applied by means of a hydraulic ram, and the portions of metal last fluid expressed. The expressed metal was found to be n combination of phosphide of iron and unaltered pig metal in the proportion of 51.5 : 48.5 or 88.05 per cent. of iron and 11.95 per cent. of phosphorus ; or, calculated into chemical equivalents, they are in the ratio 1.57 iron to 0.385 phos- phorus or 4 equivalents of iron to 1 of phosphorus, and the formula may therefore be written Fe4P.It is very clear from these results that phosphide of iron does exist in a separate state in pigmetal intimately diffused throughout the mass. On immersing bar iron in dilute acid, such as hydrochloric acid or sulphuric acid, a black residue is observed adhering to the outside of the iron. In these residues, phosphides of different constitution were found, the iron and phosphorus being pre- sent as Fe3P4 and Fe3P,. This fact proves that iron containing phos- phorus contains two or more different phosphides, and that they exist in very varying proportions in different samples of iron. 4. The Efect which Phosphorzis has on Pig metal ( a ) . Physicnl Pro- perties.--Experiments have shown that, as a considerable quantity of iron is in combination with phosphorus in Cleveland iron, there is less iron remaining capable ut taking up silicon, than is the case where no phosphorus is present: consequently less silicon w7ill be required to give to the smaller proportion of iron t,he conditions necessary for the production of glazed iron.( b . ) ChemicaZ Properties.- When sulphur is added to fluid metal-which under ordinary circum- stances would assume a grey fracture when cooled and broken-the sulphurised iron when cold will present a mottled or white fracture. I n other words, sulphur prevents the separation of carbon as graphite. I n order to ascertain if phosphorus has a similar action, experiments were made which proved that the effect of phosphorus compared with that of sulphur is very small, and would not affect materially the quality of the iron or pig in this direction, even if increased in con- siderable quantity.5 . Methods of removi?Ag Phosphorus from Pig metal.-The action of oxide of iron as a purification method is well known, but it has fre- quently been supposed that oxide of iron, without the aid of mechanical power, has very little action, and that the work a puddler gives to the metal has some important action in removing phosphorus independent of the oxide of iron. By the results obtained from numerous experi- ments it has been clearly proved that mechanical power, whether itbe in the force of the refining blast, the motion of the puddler’s bar, or the revolving of the rotary puddling machine, is simply the meaiis by which the molten iron is brought into intimate contact with the fluid or semi-fluid oxide of iron, The removal of phosphoras depends entirely on this, and not on any mechanical force.It is further illustrated experimentally that, when the puddling process is con- ducted a t a very low temperature,or when the cinder is run out of the furnace before the phosphorus is removed, the puddled bar produced is high in phosphorus. i n the first case the temperature is not high enough to liquefy the necessary amount of cinder required for the purification of the metal, and as a consequence, there is left an impure iron ; whilst in the other, when the cinder is removed from the semi- purified iron the purifying agent being taken away, the removal of phosphorus is retarded and a pliosphuretted iron is produced.On the other hand, when a high temperature is maintained, a very excellent quality of bar is produced. 6. Iron Heated with Phosphoric Acid.-It is stated that pure iron at a red heat has no power to decompose phosphoric acid ; but, if the iron be heated to its fusion point, the acid is readily decomposed. Pure iron was fused with puddler’s tap-cinder, containing above 4 per cent. of phosphoric acid, in order to determine whether or not pure iron would decompose phosphoric acid when in combination with iron oxide : the button produced contained = 2.12 per cent. Pure iron was next fused with phosphate of iron, and the metal, after fusion, was found to contain 2.68 per cent. of phosphorus. The nature of the action between oxide and phosphide of iron was proved by experiments to be not physical but chemical.The button obtained weighed about 15 per cent. more than before such treatment. 6 . Phoqhorus in Bar-iron.-From the following results i t will be seen that a considerable amount of phosphorns is removed by simply heating and rolling iron containing i t ; and that it is oxidised and removed from the iron, whereby the quality of the bar is improved considerably. No. 2 ordinary bar-iron made from Cleveland pig was twice piled and rolled. No. 4 bar, produced after the second rolling, was excellent fibrous iron, and very soft, whereas, before the treatment, it was in great part crystalline and hard:- Phosphorus combined Phosphorus in Phosphorus. with iron. cinder. Total.p. c. p. c . p. c. 2. 0.243 0.087 0.33 3. 0.130 0.110 0.24 4. 0.071 0.149 0.22 The following is an analysis of three finished bars made from Cleveland iron, puddled in the Danks’ furnaces at the Tees Side Iron Works. It would be difficult to obtain better iron thaa this:- I. 11. 111. p. c. p. c. p. c. Carbon .. .. . . .. 0.080 0.110 0.160 Silicon .... .. .. 0.092 0.046 0.040 Phosphorus . . . . 0.110 0.060 0.073 Sulphur .... .... 0.012 0.016 0.01294 ABSTRACTS OF CHEMICAL PAPERS. Pliosphorus combined Phosphorus in Phosphorus. with iron. cinder. Total. p. c. p. c. p. c. 1. 0.057 0.063 0.1 10 2. 0.023 0.037 0.069 3. 0.034 0.039 0.073 I n the third portion of his paper the author describes some of the changes which take place when air is blown through phosphuretted metal, and censiders the value of manganese oxides, chlorine, bromine, iodine, and hydrogen as agents for removing phosphorus, leaving the question of ore purification as a yet unsolved problem, and one which will not be readily solved to the satisfaction of the practical iron manufacturer. When metal containing mangnnese, silicon, carbon, and phosphorus is acted upon while in the fluid state by a stream of air, there is every reason to believe that all the elements present, probably with the ex- ception of carbon, are oxidiscd in the ratio in which they exist in the metal, and this should give a very basic cinder.Such, however. is not the case: for almost instantly after the formation of cinder, the manganese, silicon, and phosphorus still present in the fluid mass are oxidised by the oxygen of the protoxide of iron, while the reduced iron, leaving the cinder, returns to the bath and is replaced by the oxide of manganese, silicon, and phosphorus.In consequence of the rapidity with which these reactions take place, the cindey drawn off from the metal is always more or less saturated with silica, phosphoric acid, and manganese oxide. la a Bessemer converter, when the temperature is low enough, there can be no doubt that a t first all ingredients are burnt just in the proportion in which they are present. Such, however, is tlie violent agitation to which the metal is subjected, that the cinder and iron are continually in intimate con- tact, and as a consequence, the cinder is very rapidly saturated with silica and phosphoric acid.In the Bessemer converter, after the saturation point has been reached, when the silica and phosphoric acid have both in combination with them the proper chemical proportion of oxide of iron, the still unoxidised silicon in the metal will continue to reduce the oxide in the cinder, and will replace i t by silica. It is clear that when this point has been attained, viz., the removal of a base and the substitution of an acid in a compound already saturated with acid (silica), silica must be in excess, and that, as this acid is much niore powerful than phosphoric acid, i t will take away the oxide of iron a t first in combination with it, by which reaction silicic acid arid iron phosphates are transformed into phosphoric acid and iron silicate. Experiments were.undertaken which afforded proof of the theory, that manganese is capable of reducing free phosphoric acid a t a comparatively low temperature. It was further shown that the attraction of silicon for oxygen is greater than the attraction of phos- phorus for that element, and that when free phosphoric acid is exposed to the action of silicon, as i t exists in fluid metal a t low temperatures, oxygen is withdrawn from the phosphoric acid, and combines with the siiicon to form silicic acid. The results of an experiment in which fluid iron containing little or no silicon or manganese, was pouredTECHSICAL CHEMISTRY. 95 upon solid phosphoric acid placed at the bottom of a red-hot crucible, clearly showed that the acid had suffered decomposition. As the question as to the point a t which oxide of iron becomes saturated with silica is very important, several experiments were made with the view of solving it. F o r this purpose cinder containing little more than a trace of phosphoric acid wils mixed with variable propor- tions of sand, and, after fusion, was agitated with fluid iron containing phosphorus.In each case the metal was tested for phosphorus after treatment, and if no diminution was detected, it was concluded that the cinder employed contained no free iron oxide. The results were as follows :- No. 1. No. 2. No. 3. No. 4. p. c . p. c. p. c. p. c. Protoxide of iron.. ...... 73.90 64*.50 55.50 47-68 Sesquioxide of iron. ..... 11.60 10.60 8.50 6.87 Silica.. ................ 10.50 20.40 31.00 40.00 Alumina, lime, &c. ......4-00 4.50 5.00 5.45 100.00 lOO.00 100.00 100.00 No. 5. No. 6. No. 7. No. 8. p. c. p. c . p. c. p. c. Protoxide of iron ........ 42.13 43.41 38.57 29.57 Sesquioxide of iron ...... 10.71 8.13 7.86 5.00 Silica .................. 44.00 46.00 51.00 62.50 Alumina, lime, &c. ...... 3.16 2.46 2.57 2.93 100*00 100*00 100~00 100.00 Metallic iron.. .......... 65.60 57.60 49.12 41.89 Ratio of iron to silica . . . . 1 to 0.16 0.35 0.63 0.95 Before treatment ........ 1.51 1.51 1.48 1.48 After treatment.. ........ 0.13 0.04 0.2.5 0.75 Phosphorus in metal- Metallic iron.. .......... 40.27 38.34 38.50 26.50 Ratio of iron to silica .... 1 to 1-06 1.20 1.44 2.36 Before treatment ........ 091 0.91 0.91 0.91 After treatment.. ........ 0.89 0.90 0.91 0.91 Phosphorus in metal- It will be seen that when the ratio of iron to silica in the cinder is as 1 to 1.06, the compound is incapable of oxidising phosphorus from fluid iron containing it.This ratio is almost exactly the same as that of the chemical equivalents of iron and silica, viz., as 56 t o 60. It will be noticed that there has not been so much phosphorus removed in No. 1 as in No. 2, in which the cinder was dot so pure as in the first case, This, however, was due to the very sluggish nature of the cinder, which prevented its intimate admixture with the metal. It was proved by experiment that, within certain limits of tempera- ture, it is impossible to drive off from cinder its phosphoric acid by96 ABSTR.4CTS OF CHEMICAL PAPERS. the addition of silica.The analysis of the cinder made after fusion showed that it tenaciously retains phosphoric acid, confirming the theory that the whole of the phosphorus rerrioved in the various pro- cesses in which oxide of iron is used for purifying iron, is contained in the cinder, and that none is vaporised and carried iip the stack with the waste products of combustion from the furnace grate. As t o the value of manganese oxides as agents for purifying iron from phosphorus, it is mentioned that the protoxide, retaining its oxygen with much greater tenacity than the sesquioxide, and being de- composed a t very high temperatures only, in presence of reducing agents, is without any direct action on the phxphorus existing in the fluid iron ; as, however, this oxide has a much greater attraction for silica than iron oxide, it plays a part of secondary importance in the cinders of the purifying processes by taking up the silica.By forcing per- oxide of manganese under the surface of molteii iron, i t is deprived of half its oxygen, which, acting upon the oxidisable impurities in the metal, removes them. When oxide of iron acts upon phosphorus, for each part of that element oxidised, 4.5 parts of pure iron are removed from the oxide, When manganese peroxide acts upon phosphorus the oxidation is effected by free oxygen, and therefore there is no gain by the separation of metal. I t would seem, therefore, that peroxide of manganese is of much less value than iron oxides. With regard to the value of fluorspar as an agent for removing phosphorus, the fol- lowing experiment was tried. The action of a mixture of fluid oxide of iron and fluorspar upon Cleveland iron was ascertained by fusing two-thirds of mill-tap and one-third of spar, and thoroughly well mixing up with molten iron, the result being the removal of the greater part of the phosphorus.AS to the use of chlorine, bromine, and iodine, it is mentioned that since all these elements form definite compounds with phosphorus, which are all decomposed when brought into contact with red-hot iron, tthe phosphorus combining with the iron, t,here would be no advantage derived from their use. Hydrogen also is incapable of removing phosphorus from iron, as iron will with- draw phosphorus from its combination with hydrogen. Water has been advocated as an agent for removing phosphorus, it being held that the hydrogen would combine with i t and pass off as phosphoretted hydrogen. An experiment was undertaken with the following re- sults :- Pig metal.Before. After. Phosphorus.. . . . . . . 1.48 p. c. 1-48 p. c. Analysis of gases evolved from molten Cleveland iron in water :- 79.69 12.48 4.87 1.74 1.22 None = 100 H. co. CH4. H28. CO2. r205. p. c. The metal lost half its sulphur by the operation. 111 concluding this paper the author remarks, that so far as our present knowledge goes, there is nothing to surpass, in point of cost and efficiency, the process of purifying by means of oxide of iron, D. B.TECHNICAL CHEMISTRY. 97 Manufacture of a Red Pigment from Iron Scrap. By R. and C. STEINAU (Chem. Cen.fr., 1878, 336).-This pigment is formed by exposing wrought-iron shearings to the alternate action of air and water, and heating the resulting hydrated oxide to redness with access of air.Black is obtained by using reducing agents, and brown by mixing the two pigments. Preparation of Rosemary-oil. By C. 0. CECH (DingLpoZyt. J., 229, 466).-In the island Lesina, the rosemary plant attains a height of 30 to 62 cm., and, where it is carefully cultivated, 125 cm., the stems having a diameter of 2 to 3 cm. The glands filled with the ethereal oil (Oleum rosmnrini) are situated on the under side of the leaves. The manufacture of this oil in Lesina is increasing daily. Alt>hough no positive data exist as to the production of this oil, it is nevertheless known that Lesina ten years ago sent out 30,000 fl.Austr. worth of it. Every third year the biennial sprouts of the rosemary shrub are clipt in the month of May, the branches being dried for a week in the sun, and then deprived of their leaves. The distillation of the oil is made in copper stills, placed close by the sea shore, and heated over an open fire. Before charging the still, the dried leaves are moistened with water. The oil volatilising with the vapours of water passes through a worm and is collected in bottles. After separating t h e water from the oil, the latter is filled into tin vessels and sent to Trieste. Rosemary-oil is mostly used in perfumery, but is also added in small quantity to olive-oil ; the latter suffers no loss in value for technical purposes by this treatment, whilst the high duty imposed on olive-oil is avoided.From Trieste 17,000 to 20,000 kilos. of rosemary-oil are annually brought into commerce at an average price of 2 fl. per kilo. In France and Spain an alcoholic extract has for some time been prepared from this oil and other perfumes, which was known under the name of aqua regime Hungariae. This preparation had its origin in Lesina. Besides rosemary-oil, the dried leaves of this phnt are sent into commerce as spices, and for use in the smoking of meat, and for the preparation of rosemary-wine and rosemary-vinegar. Inactive Glucose in Crude Cane-sugars. By U. GAYON (Compt. rend., 87, 407).-The optically inactive glucose contained in crude cane-sugar and in molasses has been supposed to consist of a mixture of dextroglucose and levoglucose in due proportions.The paper describes experiments which confirm this opinion, and exhibit a means of transforming, by fermentation induced by pure Jlucor cir- ciqLeZZoides, the glucose of molasses into alcohol, and consequently of extracting additional quantities of crystallisable sugar from it. Analyses of Lamp-black made from the Natural Hydro- carbon Gas of the Ohio Petroleum Region. By J. R. SANTOS (Chem. News, 38, 941.-There are two wells in Knox County, Ohio, near the junction of the Kokosing and Mohican rivers, yielding very large quantities of hrdrocarbon gas, which Nee, of Gambler, has J. M. T. D. B. R. R. YOL. xsx\-1, ?Lutilised in the manufacture of a lamp-black, which he calls " diamond black." In the building used, 1,800 burners are at work, consuming about 275,000 cubic feet of gas per 24 hours, being about one-fourth of the available supply.The following is the composition of t.he gas by volume :- CHd. CpH6. N. 0. CO. CO,. 81.4 12.2 4.8 0% 0.5 0.3 = 100.0 Hydrogen, although not mentioned, is, according t o Sadtler, present in small quantity. The lamp-black is a t present manufactured to tho extent of about 16 tons per annum. It is very fine and smooth, free from coarse or gritty paiticles, and of a deep blue colour. It is sold to makers of fine printing and lithographic ink in the Unitcti States. The following analysis was made :-Sp. gr. a t 17" after corn- plete expulsion of air, equals 1.729. The air-dried lamp-black lost by exposure at ordinary temperature over sulphuric acid 2.30 per cent.of moisture, and a furt,her loss of 0.40 per cent. was experienced by lieating to 100". Continued heating at 200" and then a t 300" under atmospheric pressure gave rise to no further loss, but a miniitc: amount of water was expelled by subsequently heating in a Sprengcl 1-acuum. I. Carbon.. . . 96.041 Hydrogen.. . . 0.736 11. ), . . . . 9G.011 ,, . . . . 0.747 The occluded gases, driven out by heating to low redness in a Sprengel vacuum, represented, on calculating weight from volume :- co. CO?. N. Vapour of water. 1.378 1.386 0.776 0.682 p.c. by weight. There was also expelled and condensed on the cooler part of tile tube 0.024 of a solid light-yellow hydrocarbon, soluble i u alcohol, fusible, and volatilising rapidly under atmospheric pressure betweeii 215" and 220" (impure naphthalene ?).Hence the composition of the lamp-black may be calculatcd as- The material dried at 200" gave in two combustions :- Ash C. H. N. CO. COZ. 3320. (FZO, + CuO). 95.057" 0.665" 0.776 1.378-f 1.386-f 0.682 0.056 = 100.000. The Part played by Coal-dust in producing Explosions in Coal Mines. By L. SlnioxrN (COW@ ye?td., 87, 195-197).- I~xplosions have been known to occur in coal mines which mere l ' r c ~ from explosive gases, and this is attributed to the presence in tlic galleries of the mine of finely-divided coal-dust, which, in the event of :i very slight explosion of fire-damp or of powder when blasting tlic coal, rapidly disengages its coal-gas and increases the force of the ex- plosion. A. J. C. D. B. * Including the C and 11 of 0.024 60lid hjdrocahoii.t. These gases were doubt lcjs l)ai*tlj foriiiecl froin solid carbon and O L * L ' ~ L L ~ E ~ osjgen b j the lieat applied in tlic \ LLLCIL~III~.Abnormal Solubility of certain Bodies in Soaps and Alka- line Resinates. By A. LIVACHE (Coinpt. rend., 88, 249).- Tbc soaps known in commerce as “ petroleum soaps’’ are made by adding to ordinary soap petroleum mixed with a certaiu proportion of Carnauba wax. On heating the soap, the petroleum easily distils out, leaving the soap unaltered; these soaps are entirely solnble in water. This lattsr property is due to the Carnauba wax which they contain, or rather to the melissic alcohol contained in that body, for petroleum done is quite insoluble in soap solution, but dissolves in melissic i~lcohot. Other bodies, such as wood-spirit, amyl alcohol, &c., act in like manner, very small quantities of these solvents sufficing to dis- solve as much as 50 per cent.of petroleum in soap. Turpentine oil arid other liquids, suspended in soap-solution, dissolve on addition of coal-tar oil dissolved in the same solution. c. w. w. Kallab’s New Bleaching Process for Animal Textile Fibres. (IJijLgZ. poZyt. J., 229, 89--92).-The following method has been used with success by the author for bleaching silk, and more especially wool with the use of indigo and Schutzenberger’s hyposulphurous acid, H2S02 (Dhzgl., 225. 383). The material to be bleachcd is cleaned in the usual manner (DhgZ., 225, 389) and brought in its moist s h t e iuto a bath of clean water at the ordinary temperature, to every 100 litre of which 0.5 to 1 gram of finely-powdered reddish- blue indigo has been added.After a short treatment in this bath, tlic material is taken ont, pressed, and taken to the bleaching bath. Thc latter consists of a solutioir of freshly-prepared sodium hyposulphite o t’ 1.0069 to 1.0283 sp. gr. ; to each litre of liquid 5 to 20 C.C. of 50 pe?. cent. acetic acid are added. The latter must be free from stroil:,. mineral acids. The operation is conducted in closed vessels. Thc mechanically adhering indigo is reduced to indigo-white, and taker1 u p in a dissolved state by the fibre, whilst the sulphurous acid give11 off simultaneously bleaches the latter. After 6 to 24 hours’ exposures in the bath, a sample is taken out.If the latter is quite white and shows a slight bluish tinge, the operation is finished; the whole is taken out of the bath, allowed to drain, and finally exposed t o the air. The indigo-white is reconverted into indigo blue, producing a per- fectly fast azurage of the fibre. If concentrated bleaching baths ai-c used, a subsequent treatment with 0.5 t o 1 per cent. solution of crgs- tallised soda may be recommended. Loose wool may be bleached in :L inore concentrated bath of 1.0356 to 1.0431 sp. gr., without the addi- tion of acetic acid. For yellow shades, it is preferable to use calcium hyposulphite instead of the sodium salt, a bath of 1 to 1.0283 sp. gr. bcing the most suitable. In this ease the previous treatmect with indigo is unnecessary. If the white shows a greenish tinge, the stufl’ is drawn through a water-bath acidulated with hydrochloric or sul- phnric acid.For silk, the bleaching liquid must be much weaker tlinn for wool. This process may also be employcd for bleachiiig l’csthers, bathing sponges, lines, hemp, cotton, wood, and straw. Advantages of only Partially Removing the Fat in Oil- 13y L. W ~ ~ I R ~ A C K (IlijiyZ. p07yf. J., 229, 167).-Whcn soiuc D. B. Seeds.100 ABSTRACTS OF CHEMICAL PAPERS. time ago the idea originated of extracting the fat from oil-seeds by means of carbon bisulphide instead of by pressure, it was generally feared that the residue could not be used as fodder, becanse at that time no satisfactory method had been found of completely removing the carbon bisulphide.Since it has been found possible in practice to completely remove the carbon bisulphide from the residue, the latter has been largely used as fodder, with advantage both as to the yield of milk and also with regard to the breeding and fattening of animals. I t was, however, regretted by farmers that during the last decade the extrac- tion of fat had become so perfect, that the residue was poor in f a t compared with that obtained by pressing. It nevertheless remains to be proved whether for fattening purposes an increased quantity of fat is needed, the mast itself being very nourishing. Trials made by Wolff, Funke, and Kreuzhage in this direction gave no material dif- ference, although it is stated that an increase in the quantity of fat undoubtedly has a more nutritious action, especially with regard to the fattening of animals, from the increased utilisation of the whole fodder in the formation of fat and flesh.For this reason manu- facturers have given up the idea of completely extracting the fat from oil-seed. Moreover, by extracting merely a large proportion of the fat, they are able to operate on a much larger quantity of seeds with the same plant. D. B. On Tanning and Mineral Tanning. By GOTTFRIEDSEY (Dingl. polyt. J., 229: 180--182).-The editor of the Halle aux Cuirs in Paris obtained some time ago samples of iron-tanned leathci. (Knapp’s patent, DingE., 227, 86 and 185) from Gottfriedsen, of Braunschweig ; these were forwarded to Muntz, who, after examining them, published his results in that Journal (January 10).He con- siders that real leather always consists of a chemical combination of the tissues of the skin with tannin, every mechanical or physical union being merely a false leather without real value for application. He therefore subjected iron-tanned leather to a treatment with sulphuric: acid, and concludes from the results obtained, that the ferric oxide is not present in a combined form, and, moreover, that iron-tanned leather is not leather at all, but is perfectly useless as such. According to his views, the oxide in iron-tanned upper leather is merely a solution of ferric oxide in fat. Howevei., by comparing mineral tanned leather with ordinary leather (tanned leatlier), he does not go further than the “ evident proof’’ that, the latter is a chemical combination, without giving any explanation as to what this evidence is.The authors, therefore, undertook to complete this investigation. They found that leather made with vegetable tannin was more easily decomposable than iron-tanned leather. The same was the case with tanned or chamois leather. D. B.TECHNICAL CHEMISTRY.T e c h n i c a1 C h e m i s t r y.Gas Lighting. By J. VAN EYNDHOVEN (Dingl. polyt. J., 229,449).-It has been supposed that the gas flame is translucent. As,however, this appeared doubtful to the author, he determined to in-vestigate the subject. The experiments were made with the aid of anexcellent photometer, the results being as follows :-The first experiments were madewith a bat's-wing burlier of 160 litres'gas consumption a t 8.3 mm.pressure. The result of ten observationsproved that the lighting power of the flat side was equal to 11.58, thatof the narrow edge 10.04 candles. After correction for barometerand thermometer, the actual lighting power for normal consumptionof gas and candle is 11.81 and 10.18 candles: English spermaceticandles with a normal consumption of 120 grains were used. For aflame consuming 100 1. of gas per hour, the actual illuminatingpower on the flat side was 9.03, on the narrow edge 7-42 candles, m7it.ha gas pressure of 4 mm. The difference in both cases is 1.5 candles,or 1 7 to 18 per cent., a circumstance which proves that the flame isnot translucent, a bat's-wing burner giving most light on its flat side.An argand burner will from a similar cause not give all its illumina-ting power.For a good street illumination, therefore, the slits of theburners and the direction of the road must be placed perpendicularlyon one another. D. B.Some Peculiarities of the Vartry Water, and the Action ofthat Water on Boiler-plates. B,y C. R. C. 'YICHUORNE (Cheiri,.News, 38, 191).-The water of the River Vartry consists of organicmatter of a peaty nature, and mineral matter, which consists chieflyof the chlorides of the alkalis and of the alkaline earths; nitratesand nitrites are also present, which, however, cannot be detected with-out evaporation, but as concentration by heat reduces the nitrates, thewater was concentrated in a vacuum. This reduction, when it takes placein high pressure boilers, is a cause of the corrosion of the boilerplates, It was found that when iron was heated with nitrates insealed glass tubes it became oxidised.E. W. P.Preservation of Potable Water. By H. SCHIFF (Deut. Chem.Ges. Ber., 11, 1528--1529).-Water containing 3 parts of salicylic acidin 10,000 was found to be fresh after remaining in a flask for threeyears. Sea-water to which phenol or, preferably, carbon bisulphide(1 part to 1,000) has been added, forms a good preservative fluid forspecimens of marine fauna. w. c. w86 ABSTRACTS OF CHEJIICAL PAPERS.Utilisation of Suint from Wool. By F. FISCHER (Dim$. polyt.J., 229, 446--449).-1t is known that raw wool contains about90 per cent. of suint soluble in cold water, consisting of the potassiumcompounds of oleic, stearic, and acetic acids, a small amount of valericacid, and many other organic substances, also of potassium chlorideand sulphate, ammonium salts, and especially potassium carbonate, andsodium compounds.By lixiviating wool with water, a dark brown liquid of peculiar smellis obtained, of sp.gr. 1.069; I. litre of this required, for neutrali-sation, a quantity of normal acid corresponding with 3.98 grams ofpotassium carbonate. By neutralising 1 litre of liquor with hydrochloricacid and shaking up with benzene, only 916 milligrams of a yellowstrongly smelling fat were obtained. By evaporating 1 litre and dryingat 120°, 122.16 grams of a hygroscopic mass remained, which on igni-tion swelled up considerably, and evolved a, gas burning with a brightflame. By continued heating in the air, and extracting with water andevaporating, 72.16 grams of a white saline mass, and 2.98 grams of aresidue consisting of sand, alumina, lime, and phosphoric acid re-sulted.By burning the suint dried at 120" in a stream of oxygen,3.04 per cent. of hydrogen as water and 19.92 per cent. of carbon 8scarbonic acid were obtained. The organic compounds of potassiumare hereby converted into potassium carbonate.A profitable recovery of the fat and the acetic acid is impossible,but the utilisation of the evaporated mass for gas and the productionof potash can be recommended. For obtaining the potash present i r ithe mass, the latter is in Germany merely heated strongly in rever-beratory furnaces, the gas formed being used as fuel.Analyses of thecomposition of the flue gases showed that carbon monoxide is, in spitc ofthe sooty nature of the flame, formed very rarely, and only when themass is at its highest heat, in which case oxygen disappears. As soonas the evaporated liquors begin to burn, the heat evolved suffices todestroy all organic matter present. Thus with 1 kilo. of Westphaliancoal 12 kilos. of liquom can be evaporated and ignited. The cokeformed is solid. The following is the analysis of the coal dried a t120" :-C. H. S. 0 (and N). Ash.76.11 4.52 1-19 10.06 8-12The raw potash taken from the furnace gave-Salts soluble in water. Insoluble. Organic matter.92-05 4.92 3-03The composition of the soluble salts was as follows:-K,C03.KC1. KZSO4. NasCO3.85.34 6-15 2.98 5.02 = 99.49 p.c.W. Graff, in Lesum, works up this raw potash from six establishmentsfor washing wool into pure potassium carbonate, bicarbonate, chloride,and sulphate. He employs about 10 to 12 workmen, the annual saleamounting to about 120,000 marks. D. BTECHXICAL CHEMISTRY. 87Ingredients.Analyses of Clays. (Dingl. polyt. J., 229, 451455).--Glaze-clay.-As a very durable, perfectly impervious glaze on refractory clay,e.g., for Bunzlau vessels, water pipes, &c., a very readily fusible clay18 often used. Seger has analysed three specimens of t'hese earthyglazes with the following results :-A. 58-99 11.73 4.16 4-77 1.83 4.83 16-19 4.80B. 64.49 14.35 4.38 4.13 1-53 3.69 3.12 3.31C.62.40 15.51 5-68 4.36 1-13 3.62 2.88 4.41A is one from Naumburg 0. Q, used in Bunzlau for the manufactureof brown kitchen utensils and water pipes ; B from Camenz i. S., usedfor the same purpose, and C is a glaze from the clay pipe manufactoryin Dommitzsch 0. Elbe.The pyrometric investigations showed that, according to Seger'squotients of refractoriness (ibid., 228, 2M), the Naumburg glazewas the most readily fusible, that of Dommitzsch the most difficultlyfusible.Stoneware-cZa$.-This clay, obtained from Hohr, and representing theraw material used for the manufacture of the fine, compact, pearl-greyvessels a t that place, had the following composition :H20 andSiO,. A1,03. Fe203. CaO. MgO. Alkalis. CO2. organic matter.Si02.Al,O,. Fe203. CaO. MgO. K20and N%O. H,O.70.12 21.43 0.77 0.00 0.39 2-62 4.92By sulphuric acid.Wilkins has already pointed out the important influence which alarge amount of silica in clay has on the lustre and the fineness of thesalt-glaze ; an observation which confirms the ready acceptation of thesalt-glaze and the peculiar compactness of the above mass.Porcelain Eurth of Linzoges.-These clays are not merely distin-guished by the fineness of their forms, but the mass itself possesses apurer, more agreeable coloration, and greater fineness and strong trans-parency than the greater number of the German productions. Thefollowing is the composition of the kaolin :-i ISi02 ....................Fe203. ...................CaO ....................MgO ....................K,O ....................Na.20 ....................Loss by ignition ..........A120,.................... 58 -3927.520.361 -520 '411 -712 *587 -1999 -6832 2227.49 -4'40 J -26 *1720 '030 -361 -827 -19Clay sub-stancedecomposiblesulphuricacid.bY47 '0936 *040 '643 *2712 -988 ABSTRACTS OF CHEMICAL PAPERS.Kot decom-posibleCorresponding with-Clay substance ................ 55.88Quartz:. ....................... 5.95Felspar. ....................... 38.1 7Compared with the composition of the German and Austrian kaolins(ihid., 228, 67), this substance is distinguished by an unusuallyhigh percentage of felspar, which explains also the fact that in S h e sthe mass is not mixed with felspar but merely with sand.The porcelain from Limoges had the following composition :-Decompos-ibleIngredients.SiOa ....................CaO ....................MgO ....................K20 .....................8 1 2 0 3 .. ..................FezO,. ...................N+O ....................Loss by ignition ..........66 -7121 '580 '470 -610 -372.931 -625 -5499-83-47 -275 '93 1 3'76--19 '4415 -65'0 -471 -775 -54Compositionof theclaysubstance.45 -3536 -501.094 *1312.92corresponding with clay substance = 43.04, quartz 26.46, and felspar30.50.The mass contains therefore more sodium, lime, and magnesia than,e.g., the Berlin porcelain, a circumstance which explains its readyfusibility and greater transparency.The glaze from Limoges consists of-SiOp.A1203. Fe203. CaO.Ingredients in p. c.. ............... 74.99 14.80 0.37 1.09Not decomposible by sulphuric acid. . 70.92 12.38 - 0.20Decomposible by sulphuric acid .... 4.07 2.42 0.37 0.89Ingredients in p. c.. ............... 0.36 4.31 3.49 0.65Loss byMgO. K20. NasO. ignition.Not decomposible by sulphuric acid . . 0.36 7 4 7Decomyosible by sulphuric acid .... - 0.68 - 0.60liurstenu?aZd-gZaxe.-This glaze adheres in the form of sand to thelignite strata, and is used in the preparation of the lead and tin enamelsfor the fabrication of stoves. According to Seger, the mass dried a t120" has the following composition :TECHNICAL CHEMISTRY s 89H,O and carbon-Si02. A1,03.Fe,O,. MgO. E@. aceous matter.Total.. . . . . . . . . . , . . 85.96 7.30 2.26 0.25 1.97 2.11,- Not decomposible by UHZSOa ....... . .. 80.03 2.69 - 1-08substance.. . . . . . . 5.93 4.61 2.22 1.14 2.12Eatable-cZay.-Pattison Muir has investigated a clay-substance fromMackenzie County, in South Island, near New Zealand, which iseaten by men and sheep in large quantities. It has the followingcompos’ , I t’ ion :-Decomposible claySi02. Al,03. Fe,03. CaO. MgO. NaC1. n20. Organic.61-25 17.97 5.72 1-91 0.87 3.69 7.31 1.77(according to R. Biedermann in Noiizb. d. Ver. fur Fuh. zo?z Ziegel?z.1878, 229).Gross~Zme?.ode-cZay.-This clay is highly refractory and possessesgreat cementing power. It is coloured light bluish-grey to white, isshiny, and breaks up in water to a fine slimy mass.The followingis the composition of the clay dried a t 120’ :-SiO,.r 1. - Chemically Mechanically Loss byAI203. combined. added. MgO. CaO. Fe203. K20. S. ignition.34.52 43.38 6.53 0.73 0.76 1.66 1.51 0.26 11-04This gives a chemical composition: 4.89(A1203, 1.65 SiO,) + RO,and the quotient of refractoriness (according to Bischof) = 2.96.D. B.Blair’s Process for Iron Manufacture. By J . IRELAND (Dingl.polyt. J., 229, 458--461).-This paper gives a detailed account ofthe improvements which have been recently made in the workingplant, also in the method of preparing iron sponge. A brief descrip-tion of the reduction furnaces is given; these consist of a group ofthree vertical retorts, each retort having a diameter of 914 mm., andbeing 8.53 m.high. The furnace is surrounded by an outer casing ofbrickwork, leaving a combustion chamber between the inside of it andthe outside of the retorts. The retorts were heated externally by gasjets, the air for combustion being supplied through apertures immediatelyabove the gas jets. I n 1876 Blair discovered, that by the addition ofa small quantity of alkali to the carbonaceous matter mixed with theore, the action of reduction was facilitated to a great extent, and orewhich took about thirty hours to reduce without alkali, could be per-fectly reduced in six hours with it. The existing furnaces, however,could not be altered in any way to suit the new condition of quickenedreduction.Blair therefore abandoned the whole principle of heating,and adopted a system by which a stream of hot carbonic oxide waspassed through the mass of ore and carbonaceous matter. The author,however, made use of the above furnace by dividing the cast-iron pipeinserted in the top of each retort into a number of smaller ones, so a90 ABSTRACTS OF CHEMICAL PAPERS.to present as small a column of materials to the action of heat as pos-sible. He used a furnace of a height of 6.4 m., the retort, being about3.2 m. high, with four inserted tubes. A fiirnace of this description,1.52 m. diameter and 12.92 m. high, produces from 60 to 70 tons ofiron, and costs about 12,000 marks.The cost of producing iron sponge will vary according to thelocality in which'the work is carried on, but with the furnaces intro-duced by Blair, the cost will be about 22 marks per ton, exclusive ofthe ore.Where several of the furnaces are in operation, the cost isless. Where the oye is rich and pure, iron sponge made from it canbe a t once made into tool steel, the quality of which cannot beequalled by that made from the best brands of Swedish bars. I n thecase of ore which is not so rich, the best way of utilising the spongemade from it is to melt i t in a cupola furnace, transferring the moltenmass to a Siemens-Martin furnace, wherein the mass is converted intosteel. The pig metal obtained in this manner will coiitain about 1.5per cent. carbon and 0.19 per cent. to 0.25 per cent. silicon.D. B.Phosphorus in Cleveland Ironstone and in Iron.By J. E.STEAD (Chew,. News, 38, 14-18 ; 29-31 and 39-42).--This papermay be divided into six sections: (1.) The compound or com-pounds in which phosphoric acid exists in the Cleveland ironstone.(2.) Method of eliminating phosphoric acid from iron ores. (3.) Thecompound in which phosphorus exists in Cleveland metal. (4.) Theeffect, physically and chemically considered, which phosphorus has onpig metal. (5.) Method of removing it from pig iron. (6.) Phos-phorus in bar iron. The following are the results of the analysis ofthe main Cleveland ironstone bed :-Iron in theStone Siliceous Phosphoric Loss by calcinedanalysed. Iron. matter. acid. Moisture. calcination. stone.Main: p. c. p. c. p. c. p. c. p. c.p. c.(1st foot 26.53 18.30 1.46 8.50 27.39 36.502nd ,, 29.54 10.90 1.13 9-10 29.80 42.083rd ,, 29.14 10.68 1-13 9.50 29.80 41.504th ,, 28.41 11.98 1.41 9-80 28.80 39-925th ,, 29.97 9.00 1.17 10.00 30.83 43.316th ,, 30.42 8.82 0.89 10.00 31.51 44.407th ,, 29.70 9-00 0.80 10.10 31.78 43-538th ,, 29-85 9.29 0.91 9-80 30.90 45-209.00 28.50 42.40 C9th ,, 30.30 12.01. 1.16Black hard.4 7 inches 30.56 12-90 0.44 8.50 26.80 41.75 *s {; ,, 37-87 22.20 1-12 5-50 18.00 34.00,, 27-26 24.70 0.81 5-00 17.00 32.85It will be seen from these analyses that no part of the stone is freefrom phosphoric acid. In the " Black Hard " bed, the author foundthis substance very variable in quantity, reaching as much as 3 percent. in some cases, and only 0.25 per ceut.in others.dCTECHNICAL CBEJIISTRT. 911. As to the form in which phosphoric acid exists in Clevelandironstone, the author mentions that several years ago Pattinson inves-tigated this matter and concluded, judging from the non-action ofammonium sulphide on the stone, or rather on the compound contain-ing phosphoric acid in the stone, that no iron phosphate was present,and that the phosphoric acid must be in combination with lime ; andthe results obtained by other methods of investigation employed bythe author has confirmed this. It is the prevailing opinion that thesource of all the phosphorus in the ironstone is the remains of smallphosphatic animals ; but this theory cannot be regarded as trustworthy,first, because in some parts of the “ Black Hard ” bed, where no fossilremains could be detected, the phosphoric acid has been found in largequantity, and secondly, because in all cases, on analysis, the shells andfossil remains which were taken out of the stone, were proved to con-tain much less phosphoric acid than the surrounding ironstone.Thefollowing analyses of fossil wood taken from various mines in thatdisirict will throw some light upon this very obscure subject.Fossilised mood found in Cleveland ironstone-OH,. C. SiO,. (20%. SO3. S. MU. d1203.3.00 9-60 0.50 0.75 0-GO 7-56 trace 8.25COO and NiO. Co and Ni. Fe. FeO. MgO. P,05. CaO.3.70 1-65 5.20 10.02 1.12 20.80 27.60Several other samples gave similar results on analysis. There canbe no doubt about the fact, that these samples were at one time partsof trees, which in their natural state would not, contain more than veryminute quantities of phosphoric acid.The latter must have been insolution, and has in this state passed into the substance of the woodand been there deposited in the condition in which we find it.2. Method of Removing Phosphoric Acid from Ores.- Jacob’s method,based on the treatment of the ores with sulphurous acid produced byburning sulphur pyrites and condensing the acid fumes in coke towers,gave satisfactory results only when the stone was reduced to a veryfine powder, about 90 per cent. of phosphoric acid being removedthereby. Forbes’ method, based on the action of common salt on ironphosphate when fused, also gave unsatisfactory results, as did the lastmethod referred to by the author, the action of sodium carbonate onphosphate of lime when fused with it.From this it would seem thatCleveland ironstone cannot be freed from phosphorus by any methodsas yet proposed. With regard t o the smelting of ironstone, since weknow that phosphate of lime heated with carbon aud iron oxides, ormetallic iron, to a very high temperature, is decomposed, the phos-phorus combining with the iron, it is to be expected that nearly all of thephosphorus introduced in the charge at the top of the blast-furnace, willbe found concentrated in the pig metal. Experiments showed thatfluorspar is of no value in removing the phosphoric acid or preventingits passage into the metal when employed as a flux in smelting.Iro?z a i d Phosphorus.--By direct addition of phosphorus to iron heatedin a crucible, the author obtained combinations containing between 6 mi92 ABSTRACTS OF CHEMICAL PBPERS.27 per cent.of phosphorus, although Percy has stated that iron will nottake up more than 8.4 per cent. of phosphorus when the two substancesare heated together in the manner described. The fusion pointappears to decrease with each addition of phosphorus, until a com-pound containing from 10 to 12 per cent. of phosphorus is produced,which is the most fusible ; after which each addition makes the com-pound less and less fusible.3. The Co~npount7s in which Phosphwus exists in Clemdand Jfeta1.-Judging from the comparative fusibility of iron, it was thought thatif separate compounds of iron and phosphorus existed in pig metal,these compounds would be more fusible than the bulk.Analyses ofabout 1 cwt. of Cleveland iron poured into a mould were made. Afterthe mass had become viscous, extreme pressure was applied by meansof a hydraulic ram, and the portions of metal last fluid expressed.The expressed metal was found to be n combination of phosphide ofiron and unaltered pig metal in the proportion of 51.5 : 48.5 or 88.05per cent. of iron and 11.95 per cent. of phosphorus ; or, calculated intochemical equivalents, they are in the ratio 1.57 iron to 0.385 phos-phorus or 4 equivalents of iron to 1 of phosphorus, and the formulamay therefore be written Fe4P. It is very clear from these results thatphosphide of iron does exist in a separate state in pigmetal intimatelydiffused throughout the mass.On immersing bar iron in dilute acid,such as hydrochloric acid or sulphuric acid, a black residue is observedadhering to the outside of the iron. In these residues, phosphides ofdifferent constitution were found, the iron and phosphorus being pre-sent as Fe3P4 and Fe3P,. This fact proves that iron containing phos-phorus contains two or more different phosphides, and that they existin very varying proportions in different samples of iron.4. The Efect which Phosphorzis has on Pig metal ( a ) . Physicnl Pro-perties.--Experiments have shown that, as a considerable quantity ofiron is in combination with phosphorus in Cleveland iron, there isless iron remaining capable ut taking up silicon, than is the casewhere no phosphorus is present: consequently less silicon w7ill berequired to give to the smaller proportion of iron t,he conditionsnecessary for the production of glazed iron.( b . ) ChemicaZ Properties.-When sulphur is added to fluid metal-which under ordinary circum-stances would assume a grey fracture when cooled and broken-thesulphurised iron when cold will present a mottled or white fracture.I n other words, sulphur prevents the separation of carbon as graphite.I n order to ascertain if phosphorus has a similar action, experimentswere made which proved that the effect of phosphorus compared withthat of sulphur is very small, and would not affect materially thequality of the iron or pig in this direction, even if increased in con-siderable quantity.5 .Methods of removi?Ag Phosphorus from Pig metal.-The action ofoxide of iron as a purification method is well known, but it has fre-quently been supposed that oxide of iron, without the aid of mechanicalpower, has very little action, and that the work a puddler gives to themetal has some important action in removing phosphorus independentof the oxide of iron. By the results obtained from numerous experi-ments it has been clearly proved that mechanical power, whether ibe in the force of the refining blast, the motion of the puddler’s bar,or the revolving of the rotary puddling machine, is simply the meaiisby which the molten iron is brought into intimate contact with thefluid or semi-fluid oxide of iron, The removal of phosphoras dependsentirely on this, and not on any mechanical force.It is furtherillustrated experimentally that, when the puddling process is con-ducted a t a very low temperature,or when the cinder is run out of thefurnace before the phosphorus is removed, the puddled bar producedis high in phosphorus. i n the first case the temperature is not highenough to liquefy the necessary amount of cinder required for thepurification of the metal, and as a consequence, there is left an impureiron ; whilst in the other, when the cinder is removed from the semi-purified iron the purifying agent being taken away, the removal ofphosphorus is retarded and a pliosphuretted iron is produced. On theother hand, when a high temperature is maintained, a very excellentquality of bar is produced.6.Iron Heated with Phosphoric Acid.-It is stated that pure iron at ared heat has no power to decompose phosphoric acid ; but, if the iron beheated to its fusion point, the acid is readily decomposed. Pure ironwas fused with puddler’s tap-cinder, containing above 4 per cent. ofphosphoric acid, in order to determine whether or not pure iron woulddecompose phosphoric acid when in combination with iron oxide : thebutton produced contained = 2.12 per cent. Pure iron was nextfused with phosphate of iron, and the metal, after fusion, was found tocontain 2.68 per cent. of phosphorus. The nature of the actionbetween oxide and phosphide of iron was proved by experiments tobe not physical but chemical.The button obtained weighed about15 per cent. more than before such treatment.6 . Phoqhorus in Bar-iron.-From the following results i t will beseen that a considerable amount of phosphorns is removed by simplyheating and rolling iron containing i t ; and that it is oxidised andremoved from the iron, whereby the quality of the bar is improvedconsiderably. No. 2 ordinary bar-iron made from Cleveland pig wastwice piled and rolled. No. 4 bar, produced after the second rolling,was excellent fibrous iron, and very soft, whereas, before the treatment,it was in great part crystalline and hard:-Phosphorus combined Phosphorus in Phosphorus.with iron. cinder. Total.p. c. p. c . p. c.2. 0.243 0.087 0.333.0.130 0.110 0.244. 0.071 0.149 0.22The following is an analysis of three finished bars made fromCleveland iron, puddled in the Danks’ furnaces at the Tees Side IronWorks. It would be difficult to obtain better iron thaa this:-I. 11. 111.p. c. p. c. p. c.Carbon .. .. . . .. 0.080 0.110 0.160Silicon .... .. .. 0.092 0.046 0.040Phosphorus . . . . 0.110 0.060 0.073Sulphur .... .... 0.012 0.016 0.0194 ABSTRACTS OF CHEMICAL PAPERS.Pliosphorus combined Phosphorus in Phosphorus.with iron. cinder. Total.p. c. p. c. p. c.1. 0.057 0.063 0.1 102. 0.023 0.037 0.0693. 0.034 0.039 0.073I n the third portion of his paper the author describes some of thechanges which take place when air is blown through phosphurettedmetal, and censiders the value of manganese oxides, chlorine, bromine,iodine, and hydrogen as agents for removing phosphorus, leaving thequestion of ore purification as a yet unsolved problem, and one whichwill not be readily solved to the satisfaction of the practical ironmanufacturer.When metal containing mangnnese, silicon, carbon, and phosphorusis acted upon while in the fluid state by a stream of air, there is everyreason to believe that all the elements present, probably with the ex-ception of carbon, are oxidiscd in the ratio in which they exist in themetal, and this should give a very basic cinder. Such, however.is notthe case: for almost instantly after the formation of cinder, themanganese, silicon, and phosphorus still present in the fluid massare oxidised by the oxygen of the protoxide of iron, while the reducediron, leaving the cinder, returns to the bath and is replaced by theoxide of manganese, silicon, and phosphorus.In consequence ofthe rapidity with which these reactions take place, the cindeydrawn off from the metal is always more or less saturated with silica,phosphoric acid, and manganese oxide. la a Bessemer converter,when the temperature is low enough, there can be no doubt that a tfirst all ingredients are burnt just in the proportion in which they arepresent. Such, however, is tlie violent agitation to which the metalis subjected, that the cinder and iron are continually in intimate con-tact, and as a consequence, the cinder is very rapidly saturated withsilica and phosphoric acid.In the Bessemer converter, after thesaturation point has been reached, when the silica and phosphoric acidhave both in combination with them the proper chemical proportion ofoxide of iron, the still unoxidised silicon in the metal will continue toreduce the oxide in the cinder, and will replace i t by silica. It isclear that when this point has been attained, viz., the removal of abase and the substitution of an acid in a compound already saturatedwith acid (silica), silica must be in excess, and that, as this acid ismuch niore powerful than phosphoric acid, i t will take away the oxideof iron a t first in combination with it, by which reaction silicic acidarid iron phosphates are transformed into phosphoric acid and ironsilicate.Experiments were. undertaken which afforded proof of thetheory, that manganese is capable of reducing free phosphoric acid a ta comparatively low temperature. It was further shown that theattraction of silicon for oxygen is greater than the attraction of phos-phorus for that element, and that when free phosphoric acid is exposedto the action of silicon, as i t exists in fluid metal a t low temperatures,oxygen is withdrawn from the phosphoric acid, and combines with thesiiicon to form silicic acid. The results of an experiment in whichfluid iron containing little or no silicon or manganese, was poureTECHSICAL CHEMISTRY. 95upon solid phosphoric acid placed at the bottom of a red-hot crucible,clearly showed that the acid had suffered decomposition.As the question as to the point a t which oxide of iron becomessaturated with silica is very important, several experiments were madewith the view of solving it.F o r this purpose cinder containing littlemore than a trace of phosphoric acid wils mixed with variable propor-tions of sand, and, after fusion, was agitated with fluid iron containingphosphorus. In each case the metal was tested for phosphorus aftertreatment, and if no diminution was detected, it was concluded thatthe cinder employed contained no free iron oxide. The results wereas follows :-No. 1. No. 2. No. 3. No. 4.p. c . p. c. p. c. p. c.Protoxide of iron.. ...... 73.90 64*.50 55.50 47-68Sesquioxide of iron. ..... 11.60 10.60 8.50 6.87Silica.. ................10.50 20.40 31.00 40.00Alumina, lime, &c. ...... 4-00 4.50 5.00 5.45100.00 lOO.00 100.00 100.00No. 5. No. 6. No. 7. No. 8.p. c. p. c . p. c. p. c.Protoxide of iron ........ 42.13 43.41 38.57 29.57Sesquioxide of iron ...... 10.71 8.13 7.86 5.00Silica .................. 44.00 46.00 51.00 62.50Alumina, lime, &c. ...... 3.16 2.46 2.57 2.93100*00 100*00 100~00 100.00Metallic iron.. .......... 65.60 57.60 49.12 41.89Ratio of iron to silica . . . . 1 to 0.16 0.35 0.63 0.95Before treatment ........ 1.51 1.51 1.48 1.48After treatment.. ........ 0.13 0.04 0.2.5 0.75Phosphorus in metal-Metallic iron.. .......... 40.27 38.34 38.50 26.50Ratio of iron to silica .... 1 to 1-06 1.20 1.44 2.36Before treatment ........ 091 0.91 0.91 0.91After treatment.......... 0.89 0.90 0.91 0.91Phosphorus in metal-It will be seen that when the ratio of iron to silica in the cinder isas 1 to 1.06, the compound is incapable of oxidising phosphorus fromfluid iron containing it. This ratio is almost exactly the same as thatof the chemical equivalents of iron and silica, viz., as 56 t o 60. Itwill be noticed that there has not been so much phosphorus removedin No. 1 as in No. 2, in which the cinder was dot so pure as in the firstcase, This, however, was due to the very sluggish nature of thecinder, which prevented its intimate admixture with the metal.It was proved by experiment that, within certain limits of tempera-ture, it is impossible to drive off from cinder its phosphoric acid b96 ABSTR.4CTS OF CHEMICAL PAPERS.the addition of silica.The analysis of the cinder made after fusionshowed that it tenaciously retains phosphoric acid, confirming thetheory that the whole of the phosphorus rerrioved in the various pro-cesses in which oxide of iron is used for purifying iron, is containedin the cinder, and that none is vaporised and carried iip the stackwith the waste products of combustion from the furnace grate.As t o the value of manganese oxides as agents for purifying ironfrom phosphorus, it is mentioned that the protoxide, retaining itsoxygen with much greater tenacity than the sesquioxide, and being de-composed a t very high temperatures only, in presence of reducing agents,is without any direct action on the phxphorus existing in the fluidiron ; as, however, this oxide has a much greater attraction for silicathan iron oxide, it plays a part of secondary importance in the cindersof the purifying processes by taking up the silica.By forcing per-oxide of manganese under the surface of molteii iron, i t is deprived ofhalf its oxygen, which, acting upon the oxidisable impurities in themetal, removes them. When oxide of iron acts upon phosphorus, foreach part of that element oxidised, 4.5 parts of pure iron are removedfrom the oxide, When manganese peroxide acts upon phosphorus theoxidation is effected by free oxygen, and therefore there is no gain bythe separation of metal. I t would seem, therefore, that peroxide ofmanganese is of much less value than iron oxides.With regard tothe value of fluorspar as an agent for removing phosphorus, the fol-lowing experiment was tried. The action of a mixture of fluid oxideof iron and fluorspar upon Cleveland iron was ascertained by fusingtwo-thirds of mill-tap and one-third of spar, and thoroughly wellmixing up with molten iron, the result being the removal of thegreater part of the phosphorus. AS to the use of chlorine, bromine,and iodine, it is mentioned that since all these elements form definitecompounds with phosphorus, which are all decomposed when broughtinto contact with red-hot iron, tthe phosphorus combining with theiron, t,here would be no advantage derived from their use. Hydrogenalso is incapable of removing phosphorus from iron, as iron will with-draw phosphorus from its combination with hydrogen. Water hasbeen advocated as an agent for removing phosphorus, it being heldthat the hydrogen would combine with i t and pass off as phosphorettedhydrogen. An experiment was undertaken with the following re-sults :-Pig metal. Before.After.Phosphorus.. . . . . . . 1.48 p. c. 1-48 p. c.Analysis of gases evolved from molten Cleveland iron in water :-79.69 12.48 4.87 1.74 1.22 None = 100H. co. CH4. H28. CO2. r205. p. c.The metal lost half its sulphur by the operation.111 concluding this paper the author remarks, that so far as ourpresent knowledge goes, there is nothing to surpass, in point of costand efficiency, the process of purifying by means of oxide of iron,D. BTECHNICAL CHEMISTRY.97Manufacture of a Red Pigment from Iron Scrap. By R. andC. STEINAU (Chem. Cen.fr., 1878, 336).-This pigment is formed byexposing wrought-iron shearings to the alternate action of air andwater, and heating the resulting hydrated oxide to redness with accessof air. Black is obtained by using reducing agents, and brown bymixing the two pigments.Preparation of Rosemary-oil. By C. 0. CECH (DingLpoZyt. J.,229, 466).-In the island Lesina, the rosemary plant attains aheight of 30 to 62 cm., and, where it is carefully cultivated, 125 cm.,the stems having a diameter of 2 to 3 cm. The glands filled with theethereal oil (Oleum rosmnrini) are situated on the under side of theleaves. The manufacture of this oil in Lesina is increasing daily.Alt>hough no positive data exist as to the production of this oil, it isnevertheless known that Lesina ten years ago sent out 30,000 fl.Austr.worth of it.Every third year the biennial sprouts of the rosemary shrub areclipt in the month of May, the branches being dried for a week in thesun, and then deprived of their leaves. The distillation of the oil ismade in copper stills, placed close by the sea shore, and heated overan open fire. Before charging the still, the dried leaves are moistenedwith water. The oil volatilising with the vapours of water passesthrough a worm and is collected in bottles. After separating t h ewater from the oil, the latter is filled into tin vessels and sent to Trieste.Rosemary-oil is mostly used in perfumery, but is also added in smallquantity to olive-oil ; the latter suffers no loss in value for technicalpurposes by this treatment, whilst the high duty imposed on olive-oil isavoided.From Trieste 17,000 to 20,000 kilos. of rosemary-oil areannually brought into commerce at an average price of 2 fl. per kilo.In France and Spain an alcoholic extract has for some time beenprepared from this oil and other perfumes, which was known underthe name of aqua regime Hungariae. This preparation had its originin Lesina.Besides rosemary-oil, the dried leaves of this phnt are sent intocommerce as spices, and for use in the smoking of meat, and forthe preparation of rosemary-wine and rosemary-vinegar.Inactive Glucose in Crude Cane-sugars. By U. GAYON(Compt. rend., 87, 407).-The optically inactive glucose containedin crude cane-sugar and in molasses has been supposed to consistof a mixture of dextroglucose and levoglucose in due proportions.Thepaper describes experiments which confirm this opinion, and exhibit ameans of transforming, by fermentation induced by pure Jlucor cir-ciqLeZZoides, the glucose of molasses into alcohol, and consequently ofextracting additional quantities of crystallisable sugar from it.Analyses of Lamp-black made from the Natural Hydro-carbon Gas of the Ohio Petroleum Region. By J. R. SANTOS(Chem. News, 38, 941.-There are two wells in Knox County,Ohio, near the junction of the Kokosing and Mohican rivers, yieldingvery large quantities of hrdrocarbon gas, which Nee, of Gambler, hasJ. M.T.D. B.R. R.YOL. xsx\-1, ?utilised in the manufacture of a lamp-black, which he calls " diamondblack." In the building used, 1,800 burners are at work, consumingabout 275,000 cubic feet of gas per 24 hours, being about one-fourthof the available supply. The following is the composition of t.he gasby volume :-CHd. CpH6. N. 0. CO. CO,.81.4 12.2 4.8 0% 0.5 0.3 = 100.0Hydrogen, although not mentioned, is, according t o Sadtler, presentin small quantity. The lamp-black is a t present manufactured to thoextent of about 16 tons per annum. It is very fine and smooth, freefrom coarse or gritty paiticles, and of a deep blue colour. It issold to makers of fine printing and lithographic ink in the UnitctiStates. The following analysis was made :-Sp. gr.a t 17" after corn-plete expulsion of air, equals 1.729. The air-dried lamp-black lost byexposure at ordinary temperature over sulphuric acid 2.30 per cent. ofmoisture, and a furt,her loss of 0.40 per cent. was experienced bylieating to 100". Continued heating at 200" and then a t 300" underatmospheric pressure gave rise to no further loss, but a miniitc:amount of water was expelled by subsequently heating in a Sprengcl1-acuum.I. Carbon.. . . 96.041 Hydrogen.. . . 0.73611. ), . . . . 9G.011 ,, . . . . 0.747The occluded gases, driven out by heating to low redness in aSprengel vacuum, represented, on calculating weight from volume :-co. CO?. N. Vapour of water.1.378 1.386 0.776 0.682 p.c. by weight.There was also expelled and condensed on the cooler part of tiletube 0.024 of a solid light-yellow hydrocarbon, soluble i u alcohol,fusible, and volatilising rapidly under atmospheric pressure betweeii215" and 220" (impure naphthalene ?).Hence the composition of the lamp-black may be calculatcd as-The material dried at 200" gave in two combustions :-AshC.H. N. CO. COZ. 3320. (FZO, + CuO).95.057" 0.665" 0.776 1.378-f 1.386-f 0.682 0.056 = 100.000.The Part played by Coal-dust in producing Explosionsin Coal Mines. By L. SlnioxrN (COW@ ye?td., 87, 195-197).-I~xplosions have been known to occur in coal mines which mere l ' r c ~from explosive gases, and this is attributed to the presence in tlicgalleries of the mine of finely-divided coal-dust, which, in the event of:i very slight explosion of fire-damp or of powder when blasting tliccoal, rapidly disengages its coal-gas and increases the force of the ex-plosion.A. J. C.D. B.* Including the C and 11 of 0.024 60lid hjdrocahoii.t. These gases were doubt lcjs l)ai*tlj foriiiecl froin solid carbon and O L * L ' ~ L L ~ E ~osjgen b j the lieat applied in tlic \ LLLCIL~III~Abnormal Solubility of certain Bodies in Soaps and Alka-line Resinates. By A. LIVACHE (Coinpt. rend., 88, 249).- Tbcsoaps known in commerce as “ petroleum soaps’’ are made by adding toordinary soap petroleum mixed with a certaiu proportion of Carnaubawax. On heating the soap, the petroleum easily distils out, leavingthe soap unaltered; these soaps are entirely solnble in water.Thislattsr property is due to the Carnauba wax which they contain, orrather to the melissic alcohol contained in that body, for petroleumdone is quite insoluble in soap solution, but dissolves in melissici~lcohot. Other bodies, such as wood-spirit, amyl alcohol, &c., act inlike manner, very small quantities of these solvents sufficing to dis-solve as much as 50 per cent. of petroleum in soap. Turpentine oilarid other liquids, suspended in soap-solution, dissolve on addition ofcoal-tar oil dissolved in the same solution. c. w. w.Kallab’s New Bleaching Process for Animal Textile Fibres.(IJijLgZ. poZyt. J., 229, 89--92).-The following method has been usedwith success by the author for bleaching silk, and more especiallywool with the use of indigo and Schutzenberger’s hyposulphurousacid, H2S02 (Dhzgl., 225.383). The material to be bleachcd iscleaned in the usual manner (DhgZ., 225, 389) and brought in itsmoist s h t e iuto a bath of clean water at the ordinary temperature, toevery 100 litre of which 0.5 to 1 gram of finely-powdered reddish-blue indigo has been added. After a short treatment in this bath, tlicmaterial is taken ont, pressed, and taken to the bleaching bath. Thclatter consists of a solutioir of freshly-prepared sodium hyposulphite o t’1.0069 to 1.0283 sp. gr. ; to each litre of liquid 5 to 20 C.C. of 50 pe?.cent. acetic acid are added. The latter must be free from stroil:,.mineral acids. The operation is conducted in closed vessels. Thcmechanically adhering indigo is reduced to indigo-white, and taker1u p in a dissolved state by the fibre, whilst the sulphurous acid give11off simultaneously bleaches the latter.After 6 to 24 hours’ exposuresin the bath, a sample is taken out. If the latter is quite white andshows a slight bluish tinge, the operation is finished; the whole istaken out of the bath, allowed to drain, and finally exposed t o the air.The indigo-white is reconverted into indigo blue, producing a per-fectly fast azurage of the fibre. If concentrated bleaching baths ai-cused, a subsequent treatment with 0.5 t o 1 per cent. solution of crgs-tallised soda may be recommended. Loose wool may be bleached in :Linore concentrated bath of 1.0356 to 1.0431 sp. gr., without the addi-tion of acetic acid. For yellow shades, it is preferable to use calciumhyposulphite instead of the sodium salt, a bath of 1 to 1.0283 sp. gr.bcing the most suitable. In this ease the previous treatmect withindigo is unnecessary. If the white shows a greenish tinge, the stufl’is drawn through a water-bath acidulated with hydrochloric or sul-phnric acid. For silk, the bleaching liquid must be much weakertlinn for wool. This process may also be employcd for bleachiiigl’csthers, bathing sponges, lines, hemp, cotton, wood, and straw.Advantages of only Partially Removing the Fat in Oil-13y L. W ~ ~ I R ~ A C K (IlijiyZ. p07yf. J., 229, 167).-Whcn soiucD. B.Seeds100 ABSTRACTS OF CHEMICAL PAPERS.time ago the idea originated of extracting the fat from oil-seeds bymeans of carbon bisulphide instead of by pressure, it was generallyfeared that the residue could not be used as fodder, becanse at thattime no satisfactory method had been found of completely removingthe carbon bisulphide. Since it has been found possible in practice tocompletely remove the carbon bisulphide from the residue, the latter hasbeen largely used as fodder, with advantage both as to the yield of milkand also with regard to the breeding and fattening of animals. I t was,however, regretted by farmers that during the last decade the extrac-tion of fat had become so perfect, that the residue was poor in f a tcompared with that obtained by pressing. It nevertheless remainsto be proved whether for fattening purposes an increased quantity offat is needed, the mast itself being very nourishing. Trials made byWolff, Funke, and Kreuzhage in this direction gave no material dif-ference, although it is stated that an increase in the quantity of fatundoubtedly has a more nutritious action, especially with regard tothe fattening of animals, from the increased utilisation of the wholefodder in the formation of fat and flesh. For this reason manu-facturers have given up the idea of completely extracting the fat fromoil-seed. Moreover, by extracting merely a large proportion of thefat, they are able to operate on a much larger quantity of seeds withthe same plant. D. B.On Tanning and Mineral Tanning. By GOTTFRIEDSEY(Dingl. polyt. J., 229: 180--182).-The editor of the Halle aux Cuirsin Paris obtained some time ago samples of iron-tanned leathci.(Knapp’s patent, DingE., 227, 86 and 185) from Gottfriedsen, ofBraunschweig ; these were forwarded to Muntz, who, after examiningthem, published his results in that Journal (January 10). He con-siders that real leather always consists of a chemical combination of thetissues of the skin with tannin, every mechanical or physical unionbeing merely a false leather without real value for application. Hetherefore subjected iron-tanned leather to a treatment with sulphuric:acid, and concludes from the results obtained, that the ferric oxide isnot present in a combined form, and, moreover, that iron-tannedleather is not leather at all, but is perfectly useless as such. Accordingto his views, the oxide in iron-tanned upper leather is merely a solutionof ferric oxide in fat. Howevei., by comparing mineral tanned leatherwith ordinary leather (tanned leatlier), he does not go further than the“ evident proof’’ that, the latter is a chemical combination, withoutgiving any explanation as to what this evidence is. The authors,therefore, undertook to complete this investigation. They found thatleather made with vegetable tannin was more easily decomposablethan iron-tanned leather. The same was the case with tanned orchamois leather. D. B

ISSN:0368-1769    

DOI:10.1039/CA8793600085

出版商:RSC    

年代:1879

数据来源: RSC

摘要:

102 General a n d P h y s i c a l C h e m i s t r y . Influence ofTemperature and Pressure on the Spectra of Gases. By (3. CIAhircIm (Chem. CeTLtr., 1878, 689).-The spectra of chlorine, bromine, and iodine in the gaseous state show consider- able differences. Diluted bromine vapour gives a spectrum an alo- gons to that of chlorine ; when examined under pressure, the bromine spectrum approaches that of iodine. The spectrum of iodine vapour under considerable pressure is not comparable with that of any of the other halogens under any circumstances ; so also dilute chlorine yields a spectrum presenting little analogy to those of bromine and iodine, whilst the spectrum of compressed chlorine is closely analogous to that of diluted bromine or iodine. The spectra of those elements, which exhibit great chemical activity (H: Na, 0, C1, Br, I), are markedly altered by increase of pressure.M. M. P. M. Spectroscopic Investigation of the Constitution of Liquids. By H. BGRGER (Deut. Chenz. Ges. Ber., 11, 1876--1878).-The author describes an apparatus he has constructed for the investigation of the questions-(1.) Are the absorption-bands of mutually indifferent liquids affected by mixture? (2.) Is the absorption-spectrum of a liquid aBected by its temperature? He is engaged in investigating solutions of Co, Cu, and Na salts. C. F. C. Absorption-Spectra. By J. LANDAUER (Deut. Chem. Ges. Ber., 11, 17'72--1775.-On the addition of a concentrated acid to a safranine salt, the red colour of its solution changes to violet, indigo-blue, and finally to emerald-green. The change of colour takes place in the iseverse order, when water is added to the acid solution of safranine.The solution gives a characteristic spectrum for each colour. In a compound of picric acid with safranine or with rosaniline, picric acid can no longer be detected by means of the spectroscope. From these facts, the author concludes that absorption-spectra c m provide a clue to the composition of a compound only when the colour of the substance is characteristic of its chemical composition. w. c. w. Plant& Secondary Battery. By R. BOTTOER (Cllem.. Cent,.., 1878, 574) .-According to Plant&, if two spirals of thin sheet lead immersed in dilute sulphuric acid are connected wit,h the wires from a battery, the anode spiral becomes covered with lead peroxide, and the cathode with a grey compact film.If' the battery be disconnected when oxygen begins to be evolved a t the anode, the lead spirals are said to act as a powerful battery, and to retain their electromotive force for some days. The author finds, however, that the electromotive force diminishes rapidly, and that after 24 hours no further action is obtainable from such an arrangement,. M. M. P. M. VOL. XXXVI. i102 ABSTRACTS Ok’ CHEMICAL PAPERS. Production of Rotatory Movements in Mercury. By R. BOTTGER (Chem. Cedi-., 1878, 560).-If a drop of pure merciiry, 3 or 4 mm. in diameter, placed on a watch-glass, and covered with a dilute solution of mercuric nitrate, be touched with a rod of zinc about the size of a needle, a peculiar palpitating movement of the drop hecomes visible ; if a second rod of zinc be now brought into contact with the mercury, the drop rotates rapidly ; after a time the motion ceases. The action is no doubt caused by electric currents.M. M. P. M. Production of a High Temperature by means of Ammonium Nitrate. By R. BOTTGER (Chern. Cmtr., 1878, 560).--If ammonium nitrate be dissolved in water, the temperature falls cnnsiderably, but if zinc-dust equal in amount to the ammonium nitrate used be now thiwwn into the liquid, the temperature suddenly rises, and the liquid boils violently ; if the experiment is performed in a beaker or a flask, the vessel is generally shattered. Material for Standard Weights and Measures. By F. MOHR (Ann. Chew., 194, 40-53) .-On looking over tables of co-effi- cients of expansions, i t is found that for lo, platinum expands 9-millionths of its length; iron, 11 ; glass, 9 ; Carraramarhle, 8 ; black marble, 4$.The last-named material, the uncrystallised blwk marble, has been already used with success forthe stems of pendulums. It i s recommended now that this substance be used for constructing an unalterable standard measure. The material is to be had suitable for any dimensions, is easy to work, takes a beautiful polish, and is soft enough to yield readily to the diamond for the graduation of an enti1.e meter. For weights, rock crystal is recommended. I t is of importance thRt all weights should be made of a material of the same density, so that displacement and alteration through atmospheric conditions shall be the same in every piece. It is also important that the specific gravity of the pieces shall approximate as closely as possible to that possessed by most of the bodies separated out in analysis, and again that they hare a considerable degree of hardness to protect them against wear and tear.Instead of rock crystal, the author proposes massive glass containing a large proportion of silica. For the smaller weights lie recommends aluminium (specific gravity = 2-56), instead of platinum, or perhaps a somewhat heavier and more durable alloy with silver. All pieces to he round, and to be taken hold of in the middle, not at the edges. Except in gasometric operations, i t has so far never been thought necessary to take into account the conditions indicated by thermometer and barometer on weighing.* The influence and effect of different elevations above the sea level, with weights some of brass and some of platinum in the same set, is not noticed.A kilogram weight of rock crystal on one day, by a barometric fall of 10 mm. on the next may be reduced by 3.3 mgms. Why, then, adjust a standard kilogram to the decimal of a milligram, if atmospheric *i Abstractor’s Note.-At any rate an exception to this assertion may be men- tioned in the case of Crookes’s determination of the atomic weight of thallium, where the influence of bnrometic pressure was taken into account. M. M. P. M.INORGANIC CHEMISTRY. PO3 changes indicated by barometer and thermomeber can produce such an effect ? I n the original derivation of the kilogram, three pmctical errors were made : (1.) That water of 4" was chosen as object of com- parison.Water of any other temperature has just as definite a volume at that temperature as a t 4O, and the latter is not to be had in the greatest part of the year, and not only the water, but also balance and weight, and the whole surroundings generally, mush possess the same temperature, if a weighing lasting some considerable time is to be of value. On the contrary, i t i s easy to keep to a. mean temperature of 17.3" for any lengt,hof time. (2.) 'Yhat the weighing should have been made in ziacuo. That this could not have been correctly done arises from the facts that the weight of a litre of dry air of normal constants was not known, and finally, because the third error was com- mitted.(3.) That the specific gravity of the platinum employed had not been estimated. It is unknown if t,he temperature of the air and objects and barometric pressure were noted in the comparison. With regard to the new standard measure, i t is in t,he highest degree in- different what fraction of the earth's circumferenee it makes. w. s.102General a n d P h y s i c a l C h e m i s t r y .Influence ofTemperature and Pressure on the Spectra ofGases. By (3. CIAhircIm (Chem. CeTLtr., 1878, 689).-The spectra ofchlorine, bromine, and iodine in the gaseous state show consider-able differences. Diluted bromine vapour gives a spectrum an alo-gons to that of chlorine ; when examined under pressure, the brominespectrum approaches that of iodine.The spectrum of iodine vapourunder considerable pressure is not comparable with that of any ofthe other halogens under any circumstances ; so also dilute chlorineyields a spectrum presenting little analogy to those of bromine andiodine, whilst the spectrum of compressed chlorine is closely analogousto that of diluted bromine or iodine.The spectra of those elements, which exhibit great chemical activity(H: Na, 0, C1, Br, I), are markedly altered by increase of pressure.M. M. P. M.Spectroscopic Investigation of the Constitution of Liquids.By H. BGRGER (Deut. Chenz. Ges. Ber., 11, 1876--1878).-The authordescribes an apparatus he has constructed for the investigation of thequestions-(1.) Are the absorption-bands of mutually indifferentliquids affected by mixture? (2.) Is the absorption-spectrum of aliquid aBected by its temperature? He is engaged in investigatingsolutions of Co, Cu, and Na salts.C. F. C.Absorption-Spectra. By J. LANDAUER (Deut. Chem. Ges. Ber., 11,17'72--1775.-On the addition of a concentrated acid to a safraninesalt, the red colour of its solution changes to violet, indigo-blue, andfinally to emerald-green. The change of colour takes place in the iseverseorder, when water is added to the acid solution of safranine. Thesolution gives a characteristic spectrum for each colour.In a compound of picric acid with safranine or with rosaniline,picric acid can no longer be detected by means of the spectroscope.From these facts, the author concludes that absorption-spectra c mprovide a clue to the composition of a compound only when the colourof the substance is characteristic of its chemical composition.w. c. w.Plant& Secondary Battery. By R. BOTTOER (Cllem.. Cent,.., 1878,574) .-According to Plant&, if two spirals of thin sheet lead immersedin dilute sulphuric acid are connected wit,h the wires from a battery, theanode spiral becomes covered with lead peroxide, and the cathodewith a grey compact film. If' the battery be disconnected whenoxygen begins to be evolved a t the anode, the lead spirals are said toact as a powerful battery, and to retain their electromotive force forsome days. The author finds, however, that the electromotive forcediminishes rapidly, and that after 24 hours no further action isobtainable from such an arrangement,.M. M. P. M.VOL. XXXVI. 102 ABSTRACTS Ok’ CHEMICAL PAPERS.Production of Rotatory Movements in Mercury. By R.BOTTGER (Chem. Cedi-., 1878, 560).-If a drop of pure merciiry, 3 or4 mm. in diameter, placed on a watch-glass, and covered with a dilutesolution of mercuric nitrate, be touched with a rod of zinc aboutthe size of a needle, a peculiar palpitating movement of the drophecomes visible ; if a second rod of zinc be now brought into contactwith the mercury, the drop rotates rapidly ; after a time the motionceases. The action is no doubt caused by electric currents.M. M. P. M.Production of a High Temperature by means of AmmoniumNitrate. By R. BOTTGER (Chern. Cmtr., 1878, 560).--If ammoniumnitrate be dissolved in water, the temperature falls cnnsiderably, butif zinc-dust equal in amount to the ammonium nitrate used be nowthiwwn into the liquid, the temperature suddenly rises, and the liquidboils violently ; if the experiment is performed in a beaker or a flask,the vessel is generally shattered.Material for Standard Weights and Measures.By F. MOHR(Ann. Chew., 194, 40-53) .-On looking over tables of co-effi-cients of expansions, i t is found that for lo, platinum expands9-millionths of its length; iron, 11 ; glass, 9 ; Carraramarhle, 8 ; blackmarble, 4$. The last-named material, the uncrystallised blwk marble,has been already used with success forthe stems of pendulums. It i srecommended now that this substance be used for constructing anunalterable standard measure.The material is to be had suitable forany dimensions, is easy to work, takes a beautiful polish, and is softenough to yield readily to the diamond for the graduation of an enti1.emeter. For weights, rock crystal is recommended. I t is of importancethRt all weights should be made of a material of the same density, sothat displacement and alteration through atmospheric conditions shallbe the same in every piece. It is also important that the specificgravity of the pieces shall approximate as closely as possible to thatpossessed by most of the bodies separated out in analysis, and againthat they hare a considerable degree of hardness to protect them againstwear and tear. Instead of rock crystal, the author proposes massiveglass containing a large proportion of silica.For the smaller weightslie recommends aluminium (specific gravity = 2-56), instead ofplatinum, or perhaps a somewhat heavier and more durable alloy withsilver. All pieces to he round, and to be taken hold of in the middle,not at the edges. Except in gasometric operations, i t has so far neverbeen thought necessary to take into account the conditions indicatedby thermometer and barometer on weighing.* The influence andeffect of different elevations above the sea level, with weights someof brass and some of platinum in the same set, is not noticed. Akilogram weight of rock crystal on one day, by a barometric fall of10 mm. on the next may be reduced by 3.3 mgms. Why, then,adjust a standard kilogram to the decimal of a milligram, if atmospheric*i Abstractor’s Note.-At any rate an exception to this assertion may be men-tioned in the case of Crookes’s determination of the atomic weight of thallium,where the influence of bnrometic pressure was taken into account.M.M. P. MINORGANIC CHEMISTRY. PO3changes indicated by barometer and thermomeber can produce such aneffect ? I n the original derivation of the kilogram, three pmcticalerrors were made : (1.) That water of 4" was chosen as object of com-parison. Water of any other temperature has just as definite avolume at that temperature as a t 4O, and the latter is not to be had inthe greatest part of the year, and not only the water, but also balanceand weight, and the whole surroundings generally, mush possess thesame temperature, if a weighing lasting some considerable time is tobe of value. On the contrary, i t i s easy to keep to a. mean temperatureof 17.3" for any lengt,hof time. (2.) 'Yhat the weighing should havebeen made in ziacuo. That this could not have been correctly donearises from the facts that the weight of a litre of dry air of normalconstants was not known, and finally, because the third error was com-mitted. (3.) That the specific gravity of the platinum employed hadnot been estimated. It is unknown if t,he temperature of the air andobjects and barometric pressure were noted in the comparison. Withregard to the new standard measure, i t is in t,he highest degree in-different what fraction of the earth's circumferenee it makes. w. s

ISSN:0368-1769    

DOI:10.1039/CA8793600101

出版商:RSC    

年代:1879

数据来源: RSC

摘要:

INORGANIC CHEMISTRY. PO3I n o r g a n i c Chemistry.Formation of Hydrogen Peroxide by the Explosion of aMixture of Oxygen and Hydrogen. By R. BOTTGER (Clmn. Centr.,1878, 574).-1f two volumes of hydrogen and m e volume of oxygen beexploded in a small flask, hydrogen peroxide may be readily detectedafi,er the explosion, by adding a little starch-paste containing cadmiumiodide i n solution, followed by the addition of a crystal of ammonium-ferrous snlphate.By exploding ether vapour mixed with air, ozone is produced, butno peroxide of hydrogen ; a similar experiment with anhydrous alcoholyielded no ozone. M. M. P. M.Reduction of Iodates by Phosphorus. By J. CORNE ( J . PJmrnz.Chi))?., [4], 28, 386--389).-Moist phosphorus in presence of air,reduces iodic acid and iodates at the ordinary temperature, but if airbe excluded no reduction takes place.This reduction cannot be due tophosphorous or hypcphosphorous acid, because in the case of the former,reduction only takes place at a temperature of 80-90°, and in thelatter a t about 50'.If phosphorus is immersed in water, and the air above the waterconfined, the phosphorus becomes oxidised, and the products of oxicla-tion are dissolved in the water. This solution will immediately reducepotassium iodate. The aul hor, therefore, supposes that besides phos-phorous and hypophosphorous acids being formed, a body more greedyfor oxygen than the latter, perhaps an acid containing less oxygen, isi 104 ABSTRACTS OF CHEMICAL PAPERS.formed, and that hypophosphorous acid, H3P02, is the second of aseries of acids, in which this unknown body stands first, with aformula, H,PO.Mercury often prevents this reduction.L. T. 0's.Solubility of Sulphur and Phosphorus. By G. VULPIUS (Arch.Pharm. [3], 13, 2%9-231).-At loo", 1 part of sulphur is soluble in2,800 parts of strong formic acid, but is separated from its solutionon cooling ; the separation is less remarked if the solution is dilutedwith water of the same temperature, but i t is very evident if the wateris cold. The contrary takes place in the case of a solution of phos-phorus in acetic acid, the precipitation being greater if the liquid bediluted than if i t be cooled. Phosphorus is soluble in formic acidonly in traces. Of all the fatty acids, btearic acid is the only onewhich dissolves any appreciable quantity of phosphorus or sulphur.An alcoholic solution of the stearic acid solution of phosphorus whencooled, assumes a gelatinous form.Researches on the Sulphates.By A. ETARD (Compt. rend.,87, 602-604) .-The new compound sesquisulphates previouslydescribed by the author are not the only combinations possible.Bodies of the general form, M2(S0,),.NSO4.nSO4H? ; compound snl-phates of the formula 2( S04MS04N) .nSO,H, ; and simple or doublemore or less hydrated sulphates may be obtained.Ferrosoferric SuZphate, Pe2(SO4),.FeSO4.2H,SO4 is obtained in small,pink, hexagonal plates, by dissolving in as little water as possibleequivalent quantities of ferrous and ferric sulphates, adding a greatexcess of concentratcd sulphuric acid, and heating to about 200".Ina similar way have been also prepared, Cr2( S0,),.NiSO4.2SO4H2.3H2O,Crz( SO,),ZSO,Fe S06H2.2H20, Cr2( S0,),2S04CuS04Hz,Fe3( SO,),. S04Ni. 2 S04H2, Fez( S 0,) 3. 2 SO,Nn.3 S04H2,Al,( S04),.2S04Fe. S04Hz. Al,( S04),.2Ni S0,.S04H2.E. W. P.All these salts are insoluble in water, but are decomposed by itafter a time. The above formule, together with the author's otherobservations, show that a molecule of acid can replace a molecule ofprotosulphate in these compounds, and vice uersd, according to thenature of the metal and the temperature.The compound protosulphates are prepared by dissolving the corre-sponding salts in as little water as possible, and precipitating by alarge excess of concentrated eulphuric acid.Thus are obtained2(NiS0,ZnS04) S0,H2, 2( FeSO,ZnSO,) SOcH2, 2( CuSO,ZnSO,) S04H2,2 ( CuS0,Co S 0,) S04H2, 2 ( FeS04CoS04) SO4H2, 2 ( S04CuNiS 0,) SO,H,,and 2(NiSOaFeS0,)2S04H2. With the ferrous and cupric sul-phates, a brick-red crystallised salt is precipitated. This containsS0,CuS04Fe.2Hz0 ; it loses its water a t a higher temperature, turnsviolet, and then contains SO,Fe.SO&u, keeping its crystalline form.These salts are not oxidised by fuming nitric acid, even on boiling.S04Cu.S0,Mn.H20 and S04Cu.S0,Ni.3Hz0 are also obtained in micro-scopic crystals by the same method.By substituting the simple salts for the preceding mixtures, themono- and hi-hydrated salts are obtained in crystalline form :-S 0,Co.H20, SOpNi. 2 H,O, S 04ZnHz0, S04CuH20, S 04FeH20INORGANIC CREAMISTRY. 105The protosulphates dissolved in boiling concentrated sulphuric acidAll these bodies present to the nakedThe nickel and cobaltare deposited in crystalline form.eye a more or less shining sandy appearance.salts are gradually decomposed and dissolved by water.C. E. C.Action of Hydrochloric Acid Gas on Sulphates. By C.HENSGEN (Deut. Ciienz. Ges. Ber., 11, 1775-1 778).-Dry hydro-chloric acid has no action on anhydrous ferrous sulphate a t theordinary temperature, but a t a higher temperature ferric chloride,sulphur trioxide, and sulphur dioxide are formed. When hydrochloricacid is passed into a saturated solution of ferrous sulphate, ferrouschloride separates out,, and the mother-liquor deposits tabular crystalsof the salt FeSOa.6H20.w. c. w.Action of Hydrochloric Acid on Double Sulphates. By C.HEXSGEN (Deut. Chem. Ges. Ber., 11, 1778--1781).-When hydro-chloric acid is passed into a saturated solution of potassium-coppersulphate, green crystals separate ouh, having the compositionThe compounds K4Ye2ClG + 2H20 and (NH,),Fe2Cll0 + 2H20 wereobt'ained by the action of hydrochloric acid on concentrated solutionsK,CUCI,~H~O.of potassium and ammonium iron alums. w. c. w.Hypophosphoric Acid and its Salts. By T. SALZER (Liebig'sAiznalen, 194, 28--39).-Au abstract of the earlier part of this researchappeared in this Journal, 1877, 2, 702.Some further observations are first made on the formation of tlieabove acid.The oxidation of the phosphorus is much assisted, iflarge quantities are left to the action of the air and water in the samespace. This is effected, probably not by rise of temperature, but bythe stronger ozoriising of the air, or otherwise by the more active for-mation OE hydrogen peroxide, for the phosphorus is most corrodedwhere it dips into the liquid. It is also remarked that the formationof the hypophosphoric acid proceeds with that of the phosphorousand phosphoric acids in a certain ratio, until the liquid becomes soconcentrated that no more of the first acid can be formed : only about&th part of the phosphorus is converted into hypophosphoric acid,phosphoric acid being the chief product. With regard to his formerstatement, the autlior now says that hypophosphoric acid decomposesboth sodium chloride and sodium sulphate.The formation of crystalsof the acid sodium salt only requires more time, if the solution is notvery concentrated. The salt can be directly prepared by leavingsticks of phosphorus partially immersed in dilute solution of sodiumchloride (e.g., 1 : loo), and allowing oxidation to take place.Neutral Hypopl~ospha t P ,Xa,(POJj2 + 10H20.-If to a solution of 1 part of the acid salt in 50parts of water, a concentrated solution of 1 part of soda is added, thesolution remains clear, but if soda solution be gradually added, beauti-ful prismatic, needle-shaped crystals separate, consisting of the neutralSod imz-cu?nyourds of Hypp I q d m - i c Acid106 ABSTRACTS O F CHEMICAL PAPERS.salt, and belonging to the monoclinic system.Observed facesOP, 2Pm, cop, P, +P.The neutral salt is rather less soluble in water than the acid salt,viz., in 50 times the quantity, The cold saturated solution turnsturmeric paper brown, and concentrated soda solution precipitatesfrom i t the unaltered neutral salt. + 9 K O . - 0 h-tained by acting with less than one part by weight of crystallisedsodium carbonate on one part of the acid sodium hypophosphate insolution. The solution of this salt has an alkaline reaction. It losesits water of crystallisation a t 100". At higher temperatures i t sud-denly takes fire, and burns with a steady flame (phosphorettedhydrogen gas being liberated). The crystals belong to the mono-clinic system, and are of a glassy lustre. They are mostly of tabularform, through a predominating OP.Acid Putassium Hypophosphate, K,H,(PO,), + H20.-Pure hypo-phosphoric acid neutralised with potassium carbonate and evaporatedto syrupy consistency, gave crystalline nodules, which have not yetbeen analysed.On adding an equal quantity of acid, crystals of theabove salt were obtained. I t is soluble in double its weight of watera t the ordinary temperature, but is not soluble in alcohol. On heating,it decomposes and gives off hydrogen which burns, whilst insolublepotassium metaphosphate is left behind. It crystallises in the rhonibicsystem. The crystals are small, transparent, and colourles?, and-a corn-bination of prism GOP with pyramid 2p2 ; subordinate ooP00, Pcr, andOP.A con-centrated solution of this salt was used successfully to detect 0*00:3soda, which had been dissolved in 1 C.C. of water, and existed aschloride or sulphate.Hypophosphoric acid produces a crystalline precipitate in a solutionof lithium carbonate, soluble in water with great difficulty, but easilysoluble in excess of hypophosphoric acid.Neutral A?n?)zo?zizcm Hypophosphute, (NH,),(PO,)? + H,O.- Obtainedby heating a 5 per cent. solution of the acid with excess of ammo-nia. The crystals begin to fall or effloresce immediately after drying,and so could not be measured. They appear to consist of prismaticcolumns, with pyramidal-faced ends, and are soluble in 30 times theirweight of water, the solution reacting strongly alkaline.By evapora-tion, ammonia is driven off, the solution soon acquires an acid reaction,and a t last furnishes the acid ammonium hypophosphate. Theneutral salt loses ammonia even on standing in the air, and the clearcrystals assume a turbid or milky appearance. On warming theymelt, with strong evolution of ammonia, and a t last with combustionof the liberated hydrogen. This latter property is peculiar only tothe acid hypophosphates.Acid Arnnzo?zium Hypophosphate (NH4)2H2(P03)z.-If the solutionof the previous salt be boiled until ammonia ceases to escape, the acidanimonium salt is formed, and may be obtained in needles ; i t is isomor-phous with the acid potassium salt.Neutral Bariimt Eypophosphate, Ba2(P03)2.-This salt is thrownclown from a solution of neutral sodium hypophosphate by bariumCleavage parallel to m P a .Trisodi?Lm- h y d yog en I€ypop h osplt at e, Na3H ( P 0,)The normal potassium salt could not be obtained pureINORGANIC CHEMISTRY.107chloride as an apparently amorphous precipitate. It is very slightlysoluble iu water, also in acetic acid, more soluble in hydrochloric andhypophosphoric acids. It is anhydrous, and when heated passes overinto reddish barium pyrophosphate without any appearance of combus-tion. Even by very rapid heating of the damp neutral barium salt,it is not possible to effect the oxidation of the hypophosphoric acid bymeans of the oxygen of the air.Acid Barium Hpophosphate, BaH?( PO3), + 2H20.-Prepnred fromthe acid sodium salt by precipitation with barium chloride.On mixinghot solutions of 4 parts of acid sodium salt in 180 parts of water, and of5 parts of barium chloride in 10 parts of water, and immediately filtering,beautiful crystals were obtained on cooling. They belong to themonoclinic system, and are needles formed of OP and mPm. Theyare clear, but become turbid on heating under water. They give asolution with 1,000 parts of cold water, which reacts acid, and becomesturbid on boiling in consequence of the separation of neutral or basicbarium hypophosphate. The crystals scarcely suffer any loss inweight by heating a t loo", but a t 140" slowly lose the 2 atoms ofwater of crystallisatio~i, and at, higher temperatures pass, with combus-tion of escaping hydrogen, into barium metaphosphate, which fuses toa white bead.Neutral Cdciurn Hypophosphate, C k ( PO,), + 2H20.--In neutralcalcium solutions, neutral sodium hypophosphate even of 200,000-folddilution, gives rise to a perceptible turbidity.With greater concen-tratiou the solution assumes alkalinity, and all the calcium is preci-pitated. On the contrary, on adding calcium chloride to the sodiumsalt, the alkaline reaction disappears with completed precipitation ofthe hypophosphoric acid.After washing, the original very gelatinous precipitate quicklybecomes denser, granular, and appears under the microscope as rounded,but non-crystalline particles, and by continued washing suffers anotherchange, whereby i t becomes so finely divided as to go through thedensest double or triple filters.It is insoluble in water and almostinsoluble in acetic acid, but easily soluble in hydrochloric and hypo-phosphoric acids.The crjstallisation-water is most difficult to determine, as i t begins topass off a t loo", although the salt must be brought to 200" before all canbe driven off, and then slight decomposition (i.e., oxidation) ensues.Acid C'ulci.zm Hypoplmphate could not be obtained in the solid form,as neither the dilute nor the concentrated hypophosphoric acid woulddissolve as much neutral calcium salt as is necessary for the for-mation of the acid salt. The author finally points out that as onlyone lime compound of this acid appears to exist, it will be possible totitrate neutral calcium solutions by means of neutral sodium hypo-phosphate, after addition of red litmus tincture.Alkaline reactionsets in after completed precipitation. The same remark applies tosalts of lead and other metals. w. s.Preparation of Salts in a Finely Divided State. By R. BOT.T-GER (Chewz. Centr., 1878, .560).-Salts which are insoluble, or onlyslightly soluble, in alcohol, may be obtained in a very finely divide108 ABSTRACTS OF CHEMICAL PAPERS.state by dissolving them in boiling wat,er and pouring the concentratedsolution drop by drop into alcohol. M. M. P. &l.Green and Blue Ultramarine. By G. H. PHILIPP (Liebiy’sAnnaleii, 191, l-l2).-This paper contains the results of the furtherapplication of the author’s method (Am., 184, 132) to the compara-tive investigation of these products.It is shown that all varieties ofblue ultramwine prepared in the wet way by the action of reagents,e.g., water (in sealed tubes), zinc sulphate, ammonium chloride, bopicacid, upon the green, resemble the latter in their decomposition by acids.In the dry way green is readily converted into blue ultramarine (1) byfusion withammonium chloride. The composition of the product is essen-tially thatof theordinary bluevariety. If the access of air be prevented asmilch as possible, its composition approximates somewhat to that of thegreen. In all cases water dissolves someNaClfronithe fusedmass. (2.) Byheating in chlorine gas. This product also closely resembles the ordinaryblue varieties.The chemistry of the conversion of green into blueultramarine consists essentially in the oxidation of its sulphur (toSO2 or S202) ; this is proved by the accompanying comparative analyses,and indirectly by the change in composition of the blue varietybrought about by heating it in a current of hydrogen, when it approxi-mates closely to that of the green, the colour remaining unchanged.The author also finds that on heating blue ultramarine (Marienberg)over the blowpipe, the air being as far as possible excluded, i t is con-verted into a green mass having the composition of the ordinary greenvariety. In conclusion, he states, as the principal result of his investi-gation, that the chemical difference between these two ultramarines isUltramarine.By R. HOFFMAXN (Liebig’s AniiaZen, 194, 1-22).-In the earliest researches on ultramarine, it was observed that,on decomposing it with acids, a part of the sulphur contained inthe colour was precipitated, whilst another part escaped as hydrogensul phide, and later, that green ultyamarine furnished relatively morehydrogen sulphide and less free sulphur, than blue ultramarine ; andit was believed also that in green ultramarine there was, besides thealumino-sodium silicate, a lower, and in blue ultramarine a highersulphide of sodium, or that blue ultramarine contained more sulphurthan the green. The oldest researches made with ultraniarine poor insilica, do not harmonise with this, for they showed that these per-centages were about equal, and afterwards when ultramarines rich insilica were prepared, the blue ultramarine richer in sulphur was lookedon as the higher step of sulphurisation of the green ultramarine, andit was assumed that the green variety in the refining-roasting processwith sulphur passed, with absorption of sulphur, into the blue.Although much has been done towards clearing up this intricatesubject, the time has not yet come for a well-founded theory of thecbemical constitution of the ultramarine compouitds, or of the causeof their different colours.The author therefore intended his essaymerely as a contribution towards a true theory of the ultramarine com-pounds, to be framed a t some future time.the sodium sulphide contained i n the green variety.c. P. cINOROXNIC CHEMISTRY. 109By fusing sulphur with sodium oxide or carbonate, or by reductionof the sulphate, the following reactions take place, disregarding inter-mediate compounds, which may be formed,Na,S + 4s = Na2P,5Na,S-4Na2 = Na2Sj.If it, be assumed that there are alumino-silicates of sodium in whicha part of the oxygen in closer connection with sodium is replaceable bysulphur, and that such silico-sulphides behave similarly to the freesodium monosulphide, i.e., by absorption of sulphur or by giving upsodium, higher sulphides can arise without the whole silico-sulpliidebeing decomposed, then these assumptions suffice to explain the for-mation of the ultramarines by the known methods of preparation, theirchemical behaviour generally, and their relations to one another.Thefollowing shows this for the ultramarines poor in silica.The composition of the pure air-dried kaolin is expressed by theformula (Rammelsberg) HzA1,Si,08 + Aq, or &AI,SiZO9. If an inti-mate mixture of kaolin and sodium carbonate be ignited just as theordinary ultramarine mixture is (30 parts dry clay.to 18 of sodiumcarbonate), a complete combination of the clay with soda takes place,and the composition of the combined mass may be represented asNa2A1,Si20,, or sodium alumino-silicate. Now it is cocsidered thatthis compound may be regarded as the silicate actually contained inthe ultramarine compounds poor in silica, and that by taking upsodium, sulphur compounds it is converted into ultramarine.I n fact,very good ultramarine is obtained on treating the fused mass withan excess of soda, sulphur, and resin, and submitting to the roastingprocess as with ultramarine. If clay a t a high temperature and withproper exclusion of air be ignited with an excess of sodium sulphateand charcoal, or with soda, sulphur, and charcoal, the clay satu-rates itself with soda, and then this compound becomes united withsodium sulphide, forming the while uZtra~nari?ie of Ritter. Tbewhite u7tra)mrisie is represented as NarA1,Si20,S or N%A12Si,08 -t-Na2S. Thus one-half of the water in the air-dried clay appears to bereplaced by NhO, and the other by Na2S. White ultramarine of thispurity must contain the whole sulphur as monosulphide, and by decom-posing it with a’cids yield it as hydrogen sulphide without depositionof sulpliur.Such a pure ultramarine has never been obtained ; but$hat prepared by the author gave for tzoo of sulphur as hydrogensulphide, m e as sulpliur itself. Ritter obtained the proportion 3 : 1.From the great difficulty of obtaining white ultramarine in the purestate, the analytical numbers only approximate to those required bythe formiila-White Ultramarine.Si?. 8 1 2 . Na4. S. 08.15.4 15.0 25.4 8.9 35.3 (calculated)18.3 16.6 19.0 6.1 39.7 (Ritter)17.0 16.6 21.5 6.5 38.4 (Hoffmann)If sodium be extracted from the yvhite ultramarine, the latter passes,with continual colour-change, through yellow and green, graduallyint.0 blue ultramarine without further process or addition.Themeans employed are, oxygen in presence of free sulphur, or chlorin110 ABSTRACTS OF CHEMICAL PAPERS.alone. The extracted sodium then goes out either as sulphate or aschloride. In this removal of sodium, the mode of combination of thesulphur changes in the same way as with the free sodium monosul-phide under corresponding conditions, somewhat after the manner ofthe formula, 3Nn2S - 2Naz = Na2S3 or 5Na2S - 4Naz = Na2S,. I t ap-pears very doubtful. if the green ultram'arine is a true chemical com-pound. Theoretically, it is an intermediate body between the whiteand the blue, and probably nearer the latter than the former. Withthe object of throwing light upon the constitution of the intermediateproduct, the blue ultramarine was investigated.The iodine methodgave the proportion Sn : Sb exactly as 1 : 3, or in reference to sodiumsulphide one must assume in blue ultramarine Na2S4. If it be con-ceded that the passage of white into blue ultramarine rests on removalof sodium, then the blue ultramarine is formed by removal of 3 mole-cules of sodium from 4 molecules of the white ultramarine.Na16A18Si80J2S, - Na6 = NaloAI,S8032S4.White ultramarine. Blue ultramarine.4(Xa,il12Si20, + Na,S) 4(Xa~AlLSi20a) +, Na2SJBlue Ultramti-iue.Si,. A418. NalO. s 4 - 0 3 2 .17.0 16% 17% 9.8 39.0 (calculated)18.2 16.1 1'7.3 8.4 40.0 (found)I n the formula of blue ultramarine, the whole of the sulphur isassumed to be in the state of polysulphide, whereas i t has been longknown that decomposition with acids liberates oxysulphur-compounds.The quantity of these present, however, is very small and variable.The author believes that these oxyeulphur-compounds are most pro-bably present together with this in chemical silicate combination ; andi t appears pretty certain that these oxidised sulphur-salts arise fromultramarine previously formed, and again decomposed in the burningprocess.These oxidised products can be forrried in quantity by sub-mitting to a too excessive oxidation ; and these likewise can only bepartially removed by tvnsliing.I n concluding the series of ultramarines poor in silica, a red and ayellow compound are mentioned, but these have not been closelystudied, although the corresponding individuals in the series rich insilica are well known.Of this latter series less is known than theone just described. The white ultramarine here is quite wanting;the green is less positively known, and even the bluc, as to purity,staiids behind the one poor in silica. The large quantity of' clay-residue may especially be pointed to as a reason for this. Set-tiug out for the series rich in silica, with a silicate, H6A12Si3012, orHzA12Si3010 + 2Aq (instead of kaolin, H2A12Si208 + Aq in the preced-ing series), then with perfectly similar changes as in the latter series,the formula of the blue ultramarioe rich in silica is obtaitled. Byremoval uf the 2Aq i n the above formula, and replacement of H2 byNa2, the formula Na,A12Si20,0 is obtained, which is to be regarded asthat of the rich silicate ignited with soda. Such a silicate can bINORGANIC CHEJIISTRY.11 1obtained by igniting a mixture of kaolin with the right proportion ofsilica and soda. By adding to this formula, 2Na2S, t h o type of theoriginal silicate formula is obtained, and this transformed expression,Na6AIzSi3010Sz o r NazA1,Si,Olo + 2Na2S, must be that of the unknownwhite ultramarine of the series, Attempts to prepare this by theauthor and Ritter led to bluish or greenish-blue products, which ap-peared to stand between the white and the blue ultramarines. Byabstraction of 3Na, from 2 mols. of the hypothetical white ultramarine,the formula of the blue rich in silica is obtained :-NalzA14Si60,0S4 - Na6 = Na,A1,Si60.zoS4.2(Na.,A1,Si30,,) +.2 S a 9 2(Na,hl,Si,O,,) + Saps4White ultramarine. Blue ultramarine.Blue Ultramarijie (rich in Silicu).Si,. Al,. Na,. 0 2 0 . s4.19.5 18.5 16.0 37.1 14.9 (calculated)19.0 12.7 17.4 37.3 13.6 (blue ultramarine)17.7 15.8 17.7 38-6 12-2 (bluish-green ultramarine)Now in this series, two products are found, natmcly, a red and ayellow compound. The first has only been recently prepared in thepure state, and was a t first only designated " violet ultramarine."I b now appears that the vapours of diferent mineral acids a t a tem-perature of 150" behave quite differently towards blue ultramarinefrom the aqueous solutions of the same acids a t temperatures below100". If, for example, dry hydrochloric acid gas be passed overheated blue ultramarine, with exclusion of air, there appears to be noaction ; but in presence of air or of other oxidising agents, the blueultramarine passes gradually into a violet, and with long-continuedaction into an intensely rose-red coloured substance, without libera-tion of hydrogen sulphide or other sulphur-acids in any considerablequantity.The whole of the sulphur of the blue ultramarine appearsto pass over into tlie new compound. On washing, sodium chlorideand some alumina pass into solution. Analjsis shows that the onlydifference between tlie washed and dried substance and blue ultra-marine, is that the amount of sodium has been diminished about one-fourth, and that the manner of combination of the sulphur has beenaltered by the passage of the white ultramarine of Ritter past thegreen to the blue, ie., a-sulphur is considerably diminished, b-sulphuralmost unaltered, c-, d-, and e-sulphur somewhat increased ( c - , t l - , ande-sulphur refer to the sulphur taken a t first to be as a and il, andso determiuable by the iodine method, but by slight subsequent decom-positions in the operations, &c., converted into oxidised sulphur corn-pounds.Thus the total sulphur would be LL and b + c + d + e). Theproportion of Sa : S b is exactly 1 : 4, viz., that of tho sodium penta-sulphide, Na,S5. From marly observations on the physical behaviourof the red ultramarine, especially in the grinding and washing, also inthe chemical fact of the solution of some alumina, i t is concluded thatthe chemical process in the preparation does not go quite smoothly,and that the best product yet obtained is still farther from the condi112 ABSTRACTS OF OBEMTCAL PAPERS.tion of chemical purity than the blue ultramarine.Theoretically,the red ultramarine is obtained by abstracting 8Na2 from the 5-foldformula of the hypothetical white (rich) ultramarine. It may also bcobtairied by abstraction of Na2 from the :,-fold formula of the blue(rich) ultr&narine :-Na,30A1 1o Si,, OjoSl0 - Nitl65 (Xa2A~2si301u + ZNa28)White ultramarine (rich in silica),Na3,A120Si300~&320 - Na,5[2(Na2A12Si30,0) +. N%s41Blue ultramarine (rich in shca).SI5. Mia. Nai4. 05,.19-7 12.8 15.0 37.520.2 13.5 12.9 37.918.5 13.8 14-1 37.0- Na14AlloSiI,0MSlo.5(Na2A&Si3Ol,) i 2Na2S5Red ultramarine (rich in silica).- - Na2&~0Si3001~S202[5(Na2AlpSi30101. + .2IVaf3,]Red ultramarine (rich in sahca).SlO.15.0 (calculated)15.5 (violet, Niirnberg)16.3 (red, of Buchner)Yellow ultramarine is obtained with the red as an accidental product,but recently Griinzweig has found a sure method of preparing of itfrom the red ultramarine.A formula can be derived from that of theblue ultramarine (rich), by abstracting one-fourth of the sulphur, andadding oxygen equivalent to the total sulphur in the blue ultramarine,thus :-Na6A14Si6020S4 = 2(Na2AI2SisOI0) + Na2&Blue ultramarine (rich).Na6A14Si,0zrS3 = 2(Na2A1,Si30,,) + Na,S304.Yellow ultramarine (rich).Na6fi14Si,0zlS, = Na,A14Si6020S~ - s + 04.Yellow Ultramarine (rich in silica).Si,.Al,. Na6. Op4. s3.18.8 12.1 15.4 42.9 10.6 (calculated)18.8 13-0 13.7 42.7 11.8 (found)The iiecomposition-products were only free sulphur and sulphuricacid, so that no iodine was required. This yellow ultramarine is, asGrunzweig shows, an oxidation product of blue.The following formulae are intended to show in their arrangement,&C.-(1.) I n what series of reactions ultramarine can arisefrom alumino-silicates by the known method of preparation.(2.) In what relation the different ultramarine compounds stand toeach other.(3.) How they join themselves to those groups of the mineralsilicates, which originally stimulated the artificial preparation ofultramarineIYORGASIIC CHE3IISTRT. 113Series poor in Silica.Kaolin.. ....................HZAl2Si2O8 + HZOKaolin ignited with soda ......White ultramarine .......... Na,Al2SiZO8 + NazSBlue ultramarine ............ 4(NazA12Siz08) + Na2$Na2Al2SiZO8Nosean. ................... 2(N~AlzSiz06) + Na?SOdFresh sodalite .............. 3( NaZA1,SizO8) + 2NaC1Hauyu.. .................. 2(:} AlZSi2O8) + Ez } zSO,2Series ~ i c h in Silica.Hypothetical root silicate ....The same ignited with soda . .Mesotype (natrolite) ........Decomposed sodalite ........Hypothetical white ultramarineBlue ultramarine ............Red ultramarine ............Yellow ultramarine ..........H,AlZSi3Olo + 2Hz0Na,AlzSi 3010NazA1zSi30,0 + 2Hz0NaZAlzSi3Olo (traces of NaC1)N~AI&i3010 + 2NazS.2(NaZA1?Si3Olo) + 2N,S45(NazA1,Si3010) + 2N&S52(NazAlzSi3010) + Na2S304 w.s.The Gadolinite-Earths. By C. MARIGNAC (Ann. Chinz. Phys. [ 5 ] ,14, 2471.-Working on about 300 grams of the mixed oxides, theauthor, following out the method of separation adopted by Bahr andBunsen, succeeded in separating the oxides into eighteen differentportions, passing from pure yttria on the one hand to pure erbia onthe other. The yttria and erbia present all the properties previouslyassigned to them by Bunsen and Bahr, and by other observers. Theoriginal mixture of oxides was of a pale yellow colour, and it wasfound that, whereas yttria is white and erbia is pale rose-coloured, theintermediate portions of the oxides were of a more or less deep yellowcolour as they mere further removed from erbia on the one hand,and from yttria on the other.The most deeply-coloured portionwas examined, with the view of settling t'he question, whether t'hiscolour is due to didymium or to some other oxide of the yttriumfamily.Its solution in nitric a8cid presented the absorption-spectra oferbium and didymium. By treat,ment wit'h potassium sulphate asmall quantity of didymium was separated, after which the absorption-spectrum of didymium was no longer visible, although the colour ofthe oxide had suffered no perceptible diminution. It must thereforebe concluded that the colour of this oxide is not due to didymium,since it WRS proved by experiment that a mixture of yttria and erbianeither prevents the precipitation of didymium nor affects its absorp-tion-spectrum ; and since neither yttria nor erbia is yellow, the colourof the oxide must be due to the third gadolinite-earth, t e r b i a , origin-ally distinguished by Mosander, and the existence of which was deniedby Bunsen and Bahr, and more recently by Cleve and Hoglund.For the separation of terbia in a state fit for examination, thoseportions of the mixed oxides must be taken in which traces only o114 ABSTRACTS O F CHEMICAL PAPERS.erbia exist. The oxides are dissolved in nitric acid, and subjected toa series of fractional precipitations with oxalic acid, the first portionsof precipitate being the richest in terbia.By this treatment thewhole of the yttria is separated, and the terbia obtained mixed onlywith didymium oxide and erbia.The didymium is separated in theusual way by means of potassium sulphate ; but for the separation ofterbia from erbia no method has yet been discovered. The molecularweight of terbia (mixed with erbia) is 116, and estiniating the amountof erbia at 6-8 per cent., and taking its molecular weight a t 129, thereal molecular weight of terbia must be about 11.5, which would makethe atomic weight of terbium either 99 or 148.5, according as theoxide is considered as a monoxide or as a sesquioxide. This atomicweight was confirmed by a determination made on pure terbia obtainedfrom the forinate (see next abstract).Terbium oxide, after moderate heating, is of a pure dark orange-yellow colour ; it is decolorised by heating in a current of hydrogen, orby simple exposure to a very high temperature ; in the latter case it isnot reoxidiscd by heating in contact with oxygen.This loss of colouris accompanied by an extremely slight loss of weight, as in the case ofdidymium oxide. Terbium oxide dissolves slowly, but completely, invery dilute acids, in hydrochloric acid with disengagement of chlorine.I t s salts are colourless, and have no absorption-spectrum.Terbium sulphate, Tb,( SO,), 8H20, forms colourless crystals, iso-morphous with the sulphates of yttrium, erbium? and didymium ; thecrystals lose all their water a t a low red heat, and their sulphuric acidat a higher temperature.The yellow mixture of oxides from the decomposition of the nitrates,which contained erbia in large quantities, was submitted to fractionalprecipitation with oxnlic acid.Rp this method the whole of theyttria may be separated and an oxide obtained, whose equivalent risesgraduallyby continuation of the above treatment. but the colour of whichnever attains the intensity of pure terbia, and even seems to diminishafter a time. The oxslate from this oxide has a decided rose colour,and its solutions show the erbium absorption-bands very plainly.This and the following faets seem to point to the existence of afourth oxide of this family.Although the yellow oxide obtained in the above experiment couldnot contain more than a trace of yttria, and although it containederbia to the extent of probably half its weight, its molecular weightwas only 117, which is much lower than would be expected of amixture in equal proportions of erbia and terbia, whose respectivemolecular weights are 129 and 115.Terbium formate, as stated by Delafontaine (next abstract), ismuch less soluble than the formates of yttrium and erbium. When,however, the author attempted to separate the above mixture of oxidesby this method, he obtained only a series of products differing butslightly in their molecular weights and depths of colour.c. w. w.Terbium and its Compounds, and the probable existence ofa New Metal in the Samarskite of N. Carolina. By N. DELA-EONTAINE (,4m. Chim. Phys. [5], 14, 238).-Terbium is most adIS ORGANIC CHEJIISTRT. 115vantageously extracted from samarskite, Fhich contains but smallquantities of yttria and of Bunsen’s erhia.The oxides precipitatedby means of potassium sulphate contain but little cerium, and probablyno lanthanum, the didymium being accompanied by terbium in somequantity. The mixed oxides were dissolved in nitric acid, arid repre-cipitated by potassium sulphate. The bases contained in the mother-liquor from t,his precipitate were combined with acetic acid, theacetate thus formed crystallisi~~g in colourless crystals, easily decom-posed by heat, giving a dark-orange oxide. Treated with formic acidthis oxide gave an indistinctly crystalline crust more soluble than theformates of the cerium metals, and the mother-liquor, evaporated todryness, intumesced greatly when heated, a character not exhibited bythe formates of lanthanum and didymium.The following process is the one finally adopted for the preparationof terbia.After separation of the cerium metals by potassium sulphate,the syrupy solution of the nitrates of the yttrium metals was mixedwith a saturated solution of sodium sulphate, and crystals of the samesalt were added until no more was dissolved. The crystalline depositthus formed furnishes a dark yellow oxide, that of the soluble sulphatebeing lighter-coloured.The nitric acid solution of the dark yellow oxide was fractionallyprecipitated by oxalic acid, and the least soluble portions of the oxy-late were converted into formate. The insoluble portion of theformate thus produced furnished a dark orange-coloured oxide ; byrepeating this treatment the percentage of base in the formate maybe raised above GO per cent.The solubility of the formate is about3.3 parts in 100 parts of water.The atomic weight of terbium is fixed provisionally a t 98, themolecular weight of the oxide being 114.Terbium formate is a white powder, or forms a strongly adherentnon-crystalline crust, soluble in about 30 times its weight of viater.When heated i t burns without intumescence. The acetate crystal-lises in mall, transparent, colourless prisms, much less soluble thanacetate of didFmium. It charsbelow redness, and burns like tinder.The slight solnbility of terbium formate, and the fact that i t is ex-tracted from a double sulphate insoluble in sodium sulphate, mightconfound terbium with lanthanum and didymium.The formation, onthe other hand, of the oxalate in presence of a large excess of nitricacid, excludes the possibility of the presence of an appreciable quantityof lanthanum ; moreover, the spectroscope shows only a trace of didy-inium. The absence of colour in the salts, and the difference of solu-bility of the formates, acetates, and sulphates of terbium anddidymium, also distinguish the two metals.The terbia described in the present, paper possesses the propertiespreviously recognised in Mosander’s erbia. This is seen in its hehs-vionr to acids ; its loss of colour when heated out of contact with air,and recovery of colour when heated in contact with oxygen ; its greattendency to form sub-salts insoluble in nitric acid, acetic acid, &c.The only important difference is the slightly higher molecular weight,which is probably due to the imperfect purity of the former product.Its formula is Tb(C2H,02), + 23 Aq116 ABSTRACTS OF CHEMICAL PAPERS.On the other E u d s of Snmars1iite.-As mentioned above, sodiumsnlphate separates the oxides of the Fttrium metals of samarskite intotwo portions, one of darker, the other of lighter colour.The mixtureof oxides was treated with hot formic acid diluted with a quantity ofwater calculated to dissolve the salts produced ; a white magma was,however, formed, which was not dissolved by addition of more hotwater. The liquid from this deposit yielded on evaporation, first,brilliant, well-defined rhomhoi'dal prisms, not grouped together ; theycontained 47 to 47.5 per cent.of a bright yellow oxide ; afterwards theliquid yielded longer prisms, arranged in fan-like groups ; these last,mixed with the dried mother-liquor, gave on heating, during whichthey intumesced greatly, rz light yellow oxide, which was put aside asrich in yttria. The first formates, purified by recrystallisation, con-version into oxalate, and digestion with nitric acid, contained a basewhose equivalent (molecular weight) varied between 89 and 91 Theoxide, divided into two portions, one of which was converted intoacetate, and the other into formate, gave on mixing a slightly solublewhite powder, the molecular weight, of whose base was also about 91.The dark-yellow oxides remaining after the extraction of terbiamere subjected to a repetition of the process foil the extraction of terbia,and the portions not precipitated by oxalic acid, treated in the abovemanner, gave a white crystalline powder, the molecular weight of whosebase was also about 90.The author has also observed a number of other circumstances,which lead him to believe in the existence of a new earth in samar-skite, besides those a1 ready described.c. w. w.Philippium. By M. DELAFONTAINE (Compt. rend., 87, 559).-In aprevious paper the author indicated the probable existence of a fourthearth in samnrskite. This new earth is intermediate in colonr andmolecular weight between yttria and terbia (YO = 74.5 : TbO = 114).Assuming that philippia is a protoxide, its equivalent is between90 and 95 ; it is easily obtained free from all but a small quantity offitria, and a somewhat, largeie proportion of erbia.Philippium formate crystallises easily, either on cooling, or by spon-taneous evaporation, in small shining rhomboidal prisms, less solublethan yttrium formate, which is deposited in nodular gronps from asyrupy solution ; terbium formate is anhydrous and soluble in 30-35parts of water.Sodio-terbic sulphate is scarcely soluble in water, thecorresponding philippiurn-compound is easily soluble. Philippiurnoxalate is more soluble in nitric acid than terbium oxalate, but less so-luble than the yttrium salt. Philippiurn nitrate becomes dark pellowwhen fused ; yttrium and terbium nitrates remain colourless.Philip-pium salts are colourless when pure; the oxide is decolorised by heatingin a current of hydrogen, or simply by a strong heat, becoming yellowagain on cooling in the air. Concentrated solutions of philippinmsalts give in the indigo-blue (X = 450 nearly) a wide and very intenseabsorption-band, with its edges, more especially the right, very -Re11defined ; this band is not seen in yttrium, erbium, or terbium solutions.I n the greon there are two rays, one belonging to erbium, the otherand less refrangible, probably to philippiurn ; finally, in the red there iINORUANIC CHEMISTRY 12 7a t least one narrow band. On directing the slit of the spectroscopetowards the sun, the author observed, with solutions of terbium, amoderately dark band in the violet (X = 400405 nearly) ; itsbreadth is about half that of the band characteristic of philippiurn, andi t seems to be entirely wanting in some specimens of terbia, othershaving merely a trace. The author doubts whether it is reallycharacteristic of terbium, and considers it possible that it may indicateanother new earth, whose atomic weight would be intermediatebetween those of erbium and terbium.He intends to study this ques-tion more fully, and also promises a comparative study of philippiurnThe Mosandrium of J. L. Smith. By M. DELAFONTAINE (Compt.rend., 87, 600) .-The author considers that Lawrence Smith’s mosan-drium is identical with the terbium which he himself described in arecent memoir (Ayzn. Chirn. Phys. [5], 14, 238) (see p.115). He claimsalso the priority of discovery, since “ mosandrium ” is but a mixtureof about 75-80 per cent. terbium with 20-25 per cent. of a mixtureDecipium, a new Metal fl- 3m Samarskite. By M. DELAFON-TAINE (Compt. ret~d., 87, 632).-In his researches on the samarskite ofN. Carolina the author has discovered a new metal, which he callsdecipium (from dec$iens, deceptive). This metal, which otherwisepossesses the properties characteristic of the metals of the cerium andyttrium families, forms an oxide whose molecular weight is approxi-mately 122 for the formula DpO, or 366 for Dpz03 ; it has not j e t beensufficiently separated from didymium to be able to show its truecolour ; its salts are colourless ; the acetate crystallises easily, is lesssoluble than the didymium salt, but more so than the terbium salt;decipio-potassium sulphate is but slightly soluble in a saturatedsolution of potassium snlphate, but easily soluble in pure water.Decipium nitrate gives an absorption-spectrum containing at leastthree bands in the blue and indigo.It is necessary to usedirect solarlight. The most refrangible band is a little narrower than that ofphilippium or the band rn of didymium; i t is tolerably dark; its middlecorresponds nearly with the wave-length 416, or with No. 195 on Lecoq’sscale ; it is approximately in the middle of the space between Fraun-hofer’s lines G and H, but a little nearer to G. Neither didymiumnor terbium gives bands in this part of the spectrum; the bandcharacteristic of terbium is more to the right, and nearly out of thespectrum given by ordinary light.Under exceptional circumstancesthe author observed the violet space beyond this band, and dis-tinguished two well-defined bands, probably H and H’.The second decipium band is narrower, more intense, and less well-defined; it is situated in the less refrangible blue, and its middlecorresponds with the wave-length 478 ; it is nearly in the same placeas one of the didymium bands, but is much darker. Finally, more tothe left, and nearer the limit of blue and green, there is an ill-definedminimum of transmission, which is possibly composed of two faintbands. Samarskite therefore contains the following metals :-and terbium compounds. c. w. w.of yttrium, erbium, and philippiurn.c. w. w.VOL. XXXYI. 118 ABSTRACTS OF CHEMICAL PAPERS.Name.Yttrium . . . .Erbium . . ..Terbium . . . .Philippium..Decipium ..Thorinum . .Didymium . .Cerium . . . .Colour of oxide.White.. . , , .Rose ., .. ..Orange ....Yellow .. ..White (?) ..White.. . . . .Brownish ..Pale yellow,CharacteristicMol. weight. absorption-band in A.YO = 74.5 NoneTbO = 114-1.15 400 (about)DpO = 122 41 6Tho,= 267.5 NoneDiO = 112-114 572-577Cz03 = 324 NoneEhO = 130" 520-522PpO = 90 449 7 7The atomic weights of some of these metals present a curiousrelationship :- Yttrium - 58Philippium = 74 or 59 + 2 x 8Terbium = 98 or 58 + 5 x 8Decipium = 106? or 58 + 6 x 8Erbium = 114 or 58 + 7 x 8If these metals are taken as trivalent (YzO,,T~O,, &c.) the dif-ference would be 12 or one of its multiples, instead of 8.c. w. w.Ytterbium, a new Metal from Gadolinite. By C. MARIGNACCompt. rend., 87, 578).-1n the course of his researches on thegadolinite-earths (Ann. Chirh. Phys. [ 5 ] , 14, 247) the author obtained,by the method there described, some quantity of an earth whosephysical and chemical characters and molecular weight were those oferbia. On continuing the process of separation by fusing the nitrate,he finds, however, that a further separation takes place, resulting, onthe one hand, in a rose-coloured earth presenting the characters oferbia somewhat intensified, and on the other hand, in a colourlessearth, of molecular weight = 131 nearly.The metal contained in this new earth the author names ytterbium;it presents the following characters :-Both the oxide and the saltsare colourless; the nitrate is decomposed by heat without coloration.Solutions of ytterbia give no absorption-spectrum, either in theordinary spectrum or in the ultra-violet (Soret).The earth itself isless easily attacked by acids than the other earths of this family. Itdissolves slowly in the cold, or a t a gentle heat in slightly dilutedacids ; on boiling, it dissolves easily even in acetic and formic acids.Ytterbium sulphate resembles, and is probably isomorphous with, thesulphates of yttrium and erbium; it dissolves easily arid withoutresidue in sulphate of potassium, no precipitate being formed even onboiling. A neutral and not too concentrated solution of ytterbiumchloride is not precipitated by sodium thiosulphate ; a very concen-trated solution, containing erbium, gives a precipitate containing a,larger proportion of erbium than is contained in the residual salts.Ytterbia precipitated hy potash, and submitted to a current of chlorine,dissolves completely in presence of excess of alkali.The farmate, Yb203.SC2H203.4Aq.,t.dissolves in less than its weight of* See Marignac's paper, page 119. t (P)CH203INORGANIC CHEMISTRY. 119water, and crgstallises in small crystalline nodules, resembling theformates of yttrium and erbium ; it is decomposed with intumescenceby heat, and loses its water of crystallisation at 100". All theseproperties prove the absence of thorinum, the only metal which couldbe present and could raise the equivalent.The existence of this new metal in erbia throws doubts on thecxactness of the equivalent of the latter, as determined by Bunsen andothers ; it would lead to the sopposition that t,he molecular weight oferbia must be lower than that usually given ; in facb, in the purestspecimen of erbia prepared (which still contains ytterbia) the mole-cular weight was between 122 and 126, the true molecular weight oferbia being probably lower even than this.Taking the molecular weight of ytterbia at 131, the atomic weightof ytterbium would be either 115 or 172.5, according as we adopt theformula YbO or Yb203 for the oxide.c. w. w.The probable Compound Nature of the Didymium fromCerite. By M.DELAFONTAINE (Compt. rend., 87, 634).-Didyminmobtained from cerite shows, as is well known, in the blue towards thegreen, a group of four nearly equidistant narrow bands ; the first andfourth (-1 = 482 and y = 469, Lecoq) are much better defined anddarker than the others. Sometimes the second, third, and fourth looklike a wide minimum of transmission, in the middle of which y appearsvery distinct. Didymium from samarskite never exhibits this groupof bands under any circumstances. It seems also that the band in theindigo-blue (which Lecoq calls m), whose middle corresponds with thewave-length 444, is always less intense in samarskite didymiurn thanin cerite didyminm.It might be conceived that the presence of terbium and decipium inthe didymium from samarskite would produce the above effects ; how-ever, when a solution of terbium was placed between the solutioii ofdidymiuni and the slit of the spectroscope, no effect was producedon the spectrum of the didymium.It would seem therefore that the didymium from cerite contains anew element, characterised by the above-mentioned absorption-bands,which are wanting in the spectrum from samarskite didymium.c. w. w.Pyrophoric Iron. By R. BOTTGER (Chem. Centy., 1878, 575).-Byheating iron tartrate, a pyrophoric mixture of carbon and ferrousoxide is obtained. A pyrophoric form of ferrous oxide, free fromcarbon, may be procured by heating iron oxalate in a small glassbulb. M. M. P. M.Cobalt-ammonium Compounds.By S. M. JORGEXSEN (J. yr.Chew,. [2], 18, 209--247).-1n the present communication the authorconsiders the chZoroy~~?yz~~eo-saZts : he has also succeeded in preparinganalogous series of bromopurpureo-salts and nitrato-purpureo-salts :he regards the xantbocobalt salts of Gibbs and Genth as belonging tothe nitro-purpureo series.-4 cid Chlo rop rirpu reocobnlt Su Zphate, ((31,. CoJ ONH3)?S O4 ( S04H) 6, isprepared by intimately mixing 1 mol. of purpureo-chloride with aboutk 120 ABSTRACTS OF CHEMICAL PAPERS.12 mols. of concentrated snlphuric acid, and after some time treating themixture with40 C.C. ofwater a t 70" for every 5 grams of purpureo-chlorideused. On filtering and leaving the filtrate to cool, largedark violetprismsare deposited ; they are collected on a funnel in the lower part of whichis placed a small cone of fine platinum gauze, washed with strongalcohol, pressed between paper, and dried over snlphuric acid.Thealcohol causes the precipitation of a small amount of a new salt(probably normal sulphate ; see below), but this is washed throughthe platinum gauze and removed.The crystals are very readily decomposed on the surface by water,but dissolve in warm water, with production of an acid liquid, fromwhich cobalt,ic oxide is not precipitated on long-continued boiling.Inasmuch as in this and the following chloropurpureo-salts the chlorinecannot be detected by the ordinary tests, the author regards the chlorineas intimately combined, probably with cobalt, whereas theothernegativeradicles are in more direct combination with ammonia.The chlorinehowever in this salt is partially precipitated on boiling with silvernitrate. Anhydrous normal sulphate mixed with hydrated sulphatecrystallises from a solution of the acid sulphate in hot water.Normal Chloropurpureocobalt Sulphate. - a. Hydrated Salt,C1,. (Co210NH3)2SOa.4Hz0. Prepared in a manner very similar to thatdescribed for the foregoing salt, only 6 mols. of sulphuric acid howeverbeing employed for each mol. of purpureo-chloride ; the crystals whichseparate on filtering and partial cooling are removed (see below), andthe second filtrate on complete cooling deposits nearly pure hydratedsulphate. The crystals are washed with cold water and pressed : theypresent rhombic forms, and are of a deep purple-red colour, withbrilliant lustre.This sulphate is soluble in 133.4 parts of water a t17.3", it is readily soluble in hot water ; the solution unless very dilute,deposits the anhydrous sulphate on cooling. 011 boiling with watercobaltic oxide is precipitated. b. Anhyd?.ous Salt, C12(Co,.10NH3)2S0,.-The crystals which separate on partial cooling of the first fil-trate (see above) consist of the salts a and b mixed : on exposure toair, a alone effloresces, and b may then be mechanically separated.This salt forms black or purple-brown octohedral crystals, which aremore slowly soluble in water than the hydrated salt : the solutionreacts as that of the latter salt.Chlorop?cr~ureocobalt Nitrate, C12(Co210NH3)4N03.-This salt ap-pears to have been prepared by Gibbs (Proc.A m . Acad. 1876, 11, 3),but the formula given by him is inconsistent with his own analyticalresults. It is best prppared by mixing the purpureo-chloridewith water and a little dilute sulphuric acid, treating the mass on afilter with water a t 50°, with addition a t intervals of a few dropsof sulphuric acid, and allowing the solution to flow into an excess ofconcentrated ice-cold nitric acid ; the crystals which form are washedwith nitric acid of sp. gr. 1.2 and finally with alcohol. The salt is solublein about 80 parts of water a t 16". By slowly heating the solution, thecorresponding roseo-salt is produced : on boiling, cobaltic oxide isthrown down. At.a temperature somewhat above 110" the saltdecomposes with violence.Chloropurpzireocobalt Hydrate does not appear to exist. ThINORQANIC CHEMISTRY. 121author attempted to prepare this salt by treating of 1 mol. normalchloro-sulphate with 2 mols. of barium hydroxide and water in thecold ; the filtrate reacted however as a mixture of roseo-cobalt chlorideand hydrate. Only roseo-cobalt hydrate was obtained ou treating pur-pureo-chloride with silver oxide and water.ChZoropuryureocobnIt Bromide, CI,( c0~10NH.~)Br~, may be preparedfrom the normal sulphate, or nitrate, by precipitating with sodium bro-mide, or from the carbonate, by precipitating with concentrated hydro-bromic acid. The salt is however best prepared from purpureocobaltchloride by a process analogous to that used for the preparation of thenitrate, the liquid being allowed to flow into cold concentrated hydro-bromic acid, in place of nitric acid ; the precipitate is washed withhydrobromic acid and finally with alcohol. This salt crystallises inoctohedral forms resembling the purpureo-chloride, but of a more violet-red colour than that salt.It is soluble in 214 parts of water a t 14.3".The author regards Clandet's salt ( 10NH3.Co2)Br6 (Chern. SOC. Qu. J.,4, 361) as probably a bromide belonging to the roseo series.Clilo?.oyu,y~6reocobult Iodide, Cl,. (Co210NH,)I,, is best preparedby a method similar to that employed for the preparation of thebromide : it crystallises from hot water containing a little hydriodicacid in large dark brownish-violet octohedroris : it is soluble in 54.4parts of water a t 15.6".By treating a solution 01 this salt with iodinefor some time, or by acting on the chloronitrate with iodine dissolved inpotassic iodide, or by adding a hydriodic acid solution of iodine to anaqueous solution of the chloropurpureocobalt carbonate, brown metal-lic-like needles separate, which exert a powerful polarising action onlight. These crystals could not be obtained perfectly pure ; they aresupposed by the author to be chloro~~ulpi~reocobalt periodide.Chloropurpureocobalt. mewuric Chloride, Bromide and Iodic1e.-Bytreating purpureo-cobalt chloride with excess of mercuric chloride,Claudet, Carstanjen,and Gibbs obtained a salt with6 mols. of HgCL Thesame salt is obtained by using sodio-mercuric chloride, NaHgCl,, orNa4HgCl6: the author shows that this salt is a member of the chloro-purpureo series, and that the hydrated salt (with 4H20) prepared fromroseo-cobalt chloride is a member of the roseo series. He proposesfor the latter the formula (Co,.lOHN3)(HgCl3),'4-H:,O where HgC& =Hg=CI-ClICl- and the fcrrnula C12.( Co2.1ONH3) ( Hg3ClB)i' for theformer, where Hg3CI, = Hg< cl~cl-Hg-cl~cl- When a mode-rately warm aqueous solution of purpureo-chloride containing a littlesulphuric acid is mixed with an aqueous solution of Na2HgBr4, largeviolet-red needles slowly separate. This salt is regarded by the authoras having the complex forrula-ClZCl-Hg- C1= Cl--'C12(Co210NH3) { ~ ~ ~ ~ } (10NH3.Coz)C12.By substituting a solutionof potassium iodide, saturated a t 70" withmercuric iodide, for the double sodio-mercuric chloride, in the pre-ceding process, a salt separates immediately in brownish-yellowneedles, which, when quickly waslied with cold water in the dark, andpressed, give numbers agreeing with the formula C12.( Co210NHJ(HgI,) 122 ABSTRACTS OF CHEMICAL PAPERS.Another salt containing mercury and iodine may be prepared 13-j decom-posing a solution of the normal chlorosulphate or nitrate with potassiumiodide solution, and then adding ail aqueous solution of potassiomer-curic iodide, KaHgT4 ; after some time large brilliant brown plates sepa-rate.This salt appears to have the formula CI?.( Co?10NH,)(Hg14)2”whereHg14 = -l=I-Hg=I-.I t is alwnjs more or less mixedwith the iodide already describtd.Chl oropu rpu reoco bal t-p la tinic Bromide, C 1 ( Coal ONK,) (P t B re) ?. Thissalt, which is the analogue of the platinic chloride salt prepared byClaudet, as also by Gibbs and Genth, separates in the forin of ayellow-brown crystalline precipitate, from a moderately warm mixtureof the chlororiitrote and potassioplatinic bromide, both in aqueonssolution. I t is sparingly soluble in cold water. The crystalswhich separate from a mixed solution of the purpureo-cobalt chloride,or nitrate, and tin chloride, or tin-ammonium chloride, are shown toconsist of purpureo-chloride only, and not to be a double cobalt saltcontaining tin chloride, as supposed by Gibbs aiid Genth (Sill.Am.J. [IS], 23, 264). Similarly purpureo-cobalt bromide separates from amixed solution of the chloronitrate and potassium-zinc bromide.Chloro~?~s.pureocobaZt SiZicqfEicoritle, C1,( Co,.lONH,)( SiF6)?. Thissalt, which has been described by Gibbs (Proc. Am. Acad. 11, 9), maybe readily produced by adding a cold solution of any chloropurpureocompound,. preferably the nitrate, to excess of concentrated aqueoushydrofluosihcic acid. The crjstals are dichroic, and separate in rhom-bic plates; they are regarded by the author as without water ofcrystallisation. The formation of this salt may be used as a very delicatetest for silicic acid in presence of hydrofluoric acid. It is onlynecessary t o add 1 or 2 C.C. of a cold concentrated solution of chloro-purpureocobalt nitrate to the suspected liquid: if 1 per cent.ofsilicic acid be present, crystals of the double salt separate a t once ; withsmaller quantities of silicic acid the crystals separate only after sometime. If necessary, the crystals may be washed with alcoliol andexamined under the microscope. The author has thus detected withcertainty 1.6 mgram. of silicic acid in preseice of 305 gram of 39 percent. hydrofluoric acid.Cl~lor.opurpureocobalt Dithionate, CI,.( Co,lONH,)( S,O,),. - Thissalt separates as large, brilliant, violet prisms on mixing st cold aqueoussolution of the purpureochloride with sodium dithionate. This salt issparingly soluble in cold, more readily in hot water.ChZoro~urpureocobaZt Thiosulphcrte, C&.( Co,10NH3) (S,O.,)?, preparedby precipitating a cold solution of the pnrpureochloride with a solutionof sodium thiosulphate.The salt crystallises in rhombic €arm, OOP.ern , of a brownisl -red colour : it is insoluble in cold and only slightlysoluble in warm water.Chl,,l.op7sipzcreocol~(~lf Chyoniate, CI,(CO,~ONH~)(C~O~)~ and Dichro-n7crfe, C ~ , ( C O , ~ O N I - ~ ~ ) ( C ~ ~ O ~ ) ~ . The fornier salt is obtained in the formof a reddish or flesh-coloured crystalline powder, by mixing cold solu-tions of the normal chlorosulphate, nitrate, or purpureochloride andpotassium chromate. For the preparation of the dichromate, potassiumdichromate solution is employed, arid the temperature of the sulphateor nitrate solution is slightly raised ; if purpureo chloride be employeINOROANlC CHEMISTRY.123the solution must be cold. So soon as crystals form, the mother-liquormust be drained off, and the crystals quickly washed with cold water,and dried over oil of vitriol. If the crystals be allowed to staud for 24hours or so in contact, with a large quantity of wash-water they becomemuch altered in form and appearance, but on analysis little or nochange in composition crtn be detected. Chloropurpureocobaltdichromate crystallises in brilliant golden scales, which are somewhatsoluble in water. The author's results coucerning these chromatesalts are not in keeping with those of Braun (Gottingen, 1862).C/~Z~ro~ur~ui.cocobalt Carbomte, C12,( Co210NH3) (CO,),, crystalliseswith 9 molecules of water in large beautiful violet-red crystals, andwith 1 mol.of water in small 6 or 4-sided prisms of a darker violetcdlour. The former salt is obtained by rubbing together purpureo-chloride and excess of moist silver carbonate, filtering after a fewminutes,at once adding alcohol until a faint turbidity is produced, leavingthe solution to crystallise, and washing with alcohol of 50" (Twaddell).If the silver carbonate and purpureochloride be allowed to remain forsome time in contact, or if alcohol be not added to the filtered liquidvery shortly after filtration, roseocarbonate is produced. By dissolvingthis salt in water after efflorescence, and adding alcohol until a distinctturbidity is produced, the salt with 1 mol. of water is obtained. The%hydrated salt effloresces rapidly ; it is very soluble in water, producinga deep cherry-red liquid with alkaline reaction.C/Lloro232irpureocob,r2t Oxnlate, C1,( Co213NHL,) ( C204)2, and AcidTnrtratp, CI,( C0210NH3) ( C4H,0,),5H,0.-The former salt was ob-tained by Gibbs and Gclnth (Sill.Am. J. [ 2 ] , 23, 320). Thesechemists, however, overlooked the presence of chlorine in the salt.Krok gave the formula adopted above, which was admitted to be thetrue formula by Gibbs (Pruc. Am. dcnd., 11, 4). By using the chloro-nitrate as starting point in the preparation, the author has repeatedlyobtained crystals of the same composition. Gibbs (Zoc. cit.) says thatthe composition of different preparations varies considerably.The acid tartrate is prepared by adding a considerable excess of anaqueous solution of tartaric acid to the chlorocarbonate, followedby addition of alcohol.This salt crystallises in large brilliant violet-red needles, which are tolerably soluble in water, forming a liquid withan acid reaction.Chlo1'023ur~.ylL,.eocoBalt Pyropliosphde, C12( Co210NH3) ( P207H2)2, andC1,.(Co210NHJ) P207.zH,0.-'l'he acid salt is prepared by precipitatinga n aqueous solution of the chloronitrate with sodium pyrophosphateand a little free pyrophosphoric acid. The salt crystallises in massesof brilliant violet-red needles : i t dissolves with difficulty in water,forming an acid liquid, from which silver nitrate precipitates silverpyrophosphate, but no silver chloride.The neutral pyrophosphate is prepared by adding water just sufficientfor solution to a mixture of 1 molecule of the chloronitrate and rathermore than 1 molecule of sodium pyrophosphate, filtering a t once, andadding alcohol in small successive quantities until the greater part, ofthe salt has cryst,allised out : t h e crystals are washed with alcohol anddried in the air.This salt crystallises in long thin needles of a violet-red colour, containing from 3 to 4 molecules of water124 ABSTRACTS OP CHEMICAL PAPERS.Braun (loc. cit.) and Gibbs (Proc. Am. Acad., 11, 6) failed to obtainthe neutral chloropyrophosphate.Chloropurpureocobalt Diphosphopentamolybdate. - The acid salt,C&.( Co,10NH3) ( 5Mo03.2P04H) and the neutral ammonium salt,C12(Co210NH,) (5Mo03.2P04NH4) have both been prepared ; the formeras a rose-red crystalline powder, by precipitating a cold solution of thepurpureochloride with a solution of molybdic acid in excess of phos-phoric acid ; and the latter by using a solution of the correspondingammonium phosphomolybdate as precipitant.I n a note appended to his paper the author states that he has pre-pared a few chloropurpureo-clzyomium salts, e.g., C1,( Cr2.1C)NH3) C14, &c.,and has obtained results indicating the existence of a series ofLuteo- and also of Roseo-ohromiurn compounds.M. M. P. M.Double Salts of Cuprous Thiosulphate. By F. KESEL (Deut.Chenz. Ges. Ber., 11, 1581--1586).-The author has shown in a pre-vious paper (this Journal, 1878, 113) that the composition of theyellow salt which is formed by mixing together solutions of ctipricsulphate and sodium thiosulphate, is dependent upon the temperatureemployed.At 10" it has a composition quitie different from that of'the saltwhich had been prepared a t -10" ; and on decreasing the temperaturestill further, light yellow crystals separate, which dissolve to a colour-less solution in ice-cold water. It appears, therefore, that at a tem-perature under -lo", soluble double salts only are formed, and thesemost probably contain a larger proportion of sodium thiosulphate.Siewert's formula for the yellow salt, Na$3,03.Cu2S203.CuS, is defi-nitely confirmed. This salt can be easily prepared if the solutionsmixed a t the ordinary temperatures be kept a t 0" whilst the salt isseparating.The proportion of cupric sulphate and sodium thiosul-phate required to form the compound, Na&&03.Cu2S203.CuS, wasfound by several methods of examination to be as 2S,O3N~.CuSO4,and not in the proportion of 5S203N~.SCnS0,, as stated by Siewert.The yellow salt, when anhydrous, dissolves in concentrated hydro-chloric acid to a deep brown colonr, whereas the freshly prepared andmoist salt is couverted into a white insoluble powder, as describedin the author's previous paper. This marked distinction between thetwo compounds is ascribed to their difference in hydration. Alcoholprecipitates a light brown powder from the brown acid solution ; thesupernatant liquid contains cupric chloride. The analysis of thebrown powder (dried over sulphuric acid) showed it to be a thiosul-phate, and gave numbers corresponding with the formula,[ (S203)2CuzNa2] (GUS),. A. J. C.Decomposition of Lead Sulphate by Sodium Chloride,By F. MATTHEY (Arch. Pharnz. [ 3 ] , 13, 233--241).-A mixture oflead oxide, lead sulphate, and sodium chloride is found to react,producing lead chloride, the amount of lead chloride formed being indirect proportion to the lead oxide present, but in an inverse proportionto the sodium chloride ; the whole of the lead sulphate may, however,be removed from the mixture by repeated treatments with sodiuMINERALOGICAL CHENISTRY. 125chloride. Owing to the lengthened exposure of the above mixture tothe air, carbon dioxide was absorbed, and this caused the formation ofa chlorocarbonate, Pb,CI,CO,.Mechanical Purification of Mercury. By G. VULPIUS (Arch.Phurm. [3], 13, 231).-Mercnry is freed from dirt by causing it to passthrough a thick filter, in which several holes have been pierced by aneedle. E. W. P.E. W. P.Atomic Weight of Iridium.-By C. SEUBERT (Reut. Chem. Ges.Ber., 11, 1767--1772).-The author has determined the atomic weightof iridium (l), by estimating the amount of iridium in iridium ammo-nium chloride ; and (2) by estimating the iridium and the potassiumchloride in iridium potassium chloride. The number 192.744 wasDouble Salts of Dyad Iridium, By C. SEUBERT (Deut. Cherri.Ges. Ber., 11, 1761-1 767) .-In separating iridium from rhodium bymeans of hydrogen sodium sulphite, by Bunsen’s process, the followingdouble salts were obtained, viz., IrSO3.3N~~,SO, + 10HzO, cream-coloured scales.; IrH,( S03),.3NazS0, + 4H20, broad white needles ;and IrH2(S0,),.3Na,S03 + 10H20, in thin white needles. These saltshave an acid reaction ; they are almost insoluble in cold water, andare decomposed by hot water and by acids.When aqueous sulphurous acid is heated with iridium-ammoniumchloride to 70”, an olive-green solution is formed (reddish-brown bytmnsmitted light), which deposits a green crystalline powder on eva-poration. From the aqueous solution of this compound dark greenneedles (brown by transmitted light) separate out, having the corn-position, Ir2C16.6NH4C1 + 3H,O. On cooling down the concentratedmother-liquor to a low temperature, an acid having the composition,Ir.C12. SOsH2.4NH4CI, is obtained in orange-coloured needles. It is verysoluble in water, but is not deliquescent. It decomposes alkaline carbo-nates, forming salts. Its ammonium salt, IrCl,.SO,(NH,),.2NHrlCl + 4H20, crjstallises in rhornbic plates, and the potassium salt,,IrCI,S03Kz.2NH,C1 + 4Hz0, forms small red crystalline scales.obtained as the mean of 15 experiments. w. c . w.w. c. w

ISSN:0368-1769    

DOI:10.1039/CA8793600103

出版商:RSC    

年代:1879

数据来源: RSC

摘要:

MINERALOGICAL CHENISTRY. M i n e r a l o g i c a l C h e m i s t ry. 125 Mineral Waters of the Couban, in the Caucasus. By E. WROBLEWSKY (Bull. Xoc. Chisn. [el, 30, 436).-These waters are remarkable for the quantities of bromine, iodine, and lithium they contain. 1,000 parts left 15.75408 parts of residue, containing NaCl, 14.05290 ; MgBr,, 0.07621 ; Mg12, 0.03054 ; LiCl, 0.01433. L. T. 0’s. Mineral Waters of Buda-Pesth. By M. BALLO (Deut. Chem. Ges. Ber., 11, 1900-1904) .-This paper contains complete analyses of126 ABSTRACTS O F CHEMICAL PAPERS. certain thermal and bitter waters of Buda-Pesth, which are merely of local interest. C. F. C. The Mineral Springs of Passugg, Solis, and Tiefenkasten, in the Grisons, Switzerland. By A. v. PLAHTA-REICHENAU (Deut. Cltem. Ges.Rer., 11, 1793--1799).-The author gives the results of his analyses of the following miueral waters :-I. The alkaline Ulrjcus well. 11. The ChalybciLte Theophilus spring, both at Passugg, near Coire. 1V. The saline chalybeate, St. Peter's well, at Tiefenkasten. 111. The Donatus well (containiny iodine) a t Solis. I. 1 I. Temperature of the spring.. ........ 81 7.5 Specific gravity.. .. l * O O i 1.0036 at 11'. at 14". 19,000 parts of the water contain:- Total solids . . , , . . 60.376 29.1i8 K,SO,. ........... 1.568 1.340 NhSO, .......... 0.862 1.9iO NaN03 .......... 0.04 0.007 NaBoO,, .......... 0.067 LiCl - ............ 0.06 NaCl ............ 8.371 2.221 NaBr -- ............ 0.054 R'al ............ 0.008 0.001 Ka,C03 .......... 37.946 13.513 (NHJ)?CO~ ......0.147 0.004 CaC03 .......... 71.25 7.057 M&03 .......... 3.786 2.843 SrC03. ........... - 0.005 FeC03.. .......... 0.078 0.101 SiO, ............ 0.190 0.114 AIPO, - ............ 0.076 Free COz ........ 18.382 21.565 Bromine. ......... I trace - 111. 8.1 1.0045 at 14". 49.95'2 0-702 20.400 0.067 - - 12.037 0.024 0.013 2.089 0.003 7.750 2.509 0.004 0.137 0.149 0.068 7.36 1 IV. 10" 1.00453 a t 11". 46.270 1.150 22.862 0.023 - - 5.8 i 6 - - - 0.012 11,839 0.009 0.212 0.378 11.506 trace - - I also contains a trace of barium ; I1 contains 0.005 MnC03 ; 111, a trace of boric acid; and lV, MgSOJ, 1.150; CaSOJ, 2.145; and Al,(CO&, 0.013 parts in 10,000. w. c. w.MINERALOGICAL CHENISTRY.M i n e r a l o g i c a l C h e m i s t ry.125Mineral Waters of the Couban, in the Caucasus.By E.WROBLEWSKY (Bull. Xoc. Chisn. [el, 30, 436).-These waters areremarkable for the quantities of bromine, iodine, and lithium theycontain. 1,000 parts left 15.75408 parts of residue, containingNaCl, 14.05290 ; MgBr,, 0.07621 ; Mg12, 0.03054 ; LiCl, 0.01433.L. T. 0’s.Mineral Waters of Buda-Pesth. By M. BALLO (Deut. Chem.Ges. Ber., 11, 1900-1904) .-This paper contains complete analyses o126 ABSTRACTS O F CHEMICAL PAPERS.certain thermal and bitter waters of Buda-Pesth, which are merely oflocal interest. C. F. C.The Mineral Springs of Passugg, Solis, and Tiefenkasten, inthe Grisons, Switzerland. By A. v. PLAHTA-REICHENAU (Deut.Cltem. Ges. Rer., 11, 1793--1799).-The author gives the results of hisanalyses of the following miueral waters :-I.The alkaline Ulrjcuswell. 11. The ChalybciLte Theophilus spring, both at Passugg, nearCoire. 1V. Thesaline chalybeate, St. Peter's well, at Tiefenkasten.111. The Donatus well (containiny iodine) a t Solis.I. 1 I.Temperature of thespring.. ........ 81 7.5Specific gravity.. .. l * O O i 1.0036at 11'. at 14".19,000 parts of the water contain:-Total solids . . , , . . 60.376 29.1i8K,SO,. ........... 1.568 1.340NhSO, .......... 0.862 1.9iONaN03 .......... 0.04 0.007NaBoO,, .......... 0.067LiCl - ............ 0.06NaCl ............ 8.371 2.221NaBr -- ............ 0.054R'al ............ 0.008 0.001Ka,C03 .......... 37.946 13.513(NHJ)?CO~ ...... 0.147 0.004CaC03 .......... 71.25 7.057M&03 .......... 3.786 2.843SrC03. ........... - 0.005FeC03.. .......... 0.078 0.101SiO, ............ 0.190 0.114AIPO, - ............ 0.076Free COz ........ 18.382 21.565Bromine. ......... I trace-111.8.11.0045at 14".49.95'20-70220.4000.067 --12.0370.0240.0132.0890.0037.7502.5090.0040.1370.1490.0687.36 1IV.10"1.00453a t 11".46.2701.15022.8620.023--5.8 i 6---0.01211,8390.0090.2120.37811.506trace--I also contains a trace of barium ; I1 contains 0.005 MnC03 ; 111,a trace of boric acid; and lV, MgSOJ, 1.150; CaSOJ, 2.145; andAl,(CO&, 0.013 parts in 10,000. w. c. w

ISSN:0368-1769    

DOI:10.1039/CA8793600125

出版商:RSC    

年代:1879

数据来源: RSC