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Proceedings of the Chemical Society, Vol. 18, No. 248 |
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Proceedings of the Chemical Society, London,
Volume 18,
Issue 248,
1902,
Page 51-62
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摘要:
Issued 131312 PROCEEDINGS OF THE CHEMICAL SOCIETY. EDITED BY THE XECRETARIES. Vol. 18. No. 248. March 6th, 1902. Dr. DIVERS,F.R.S., Vice-president, in the Clhair. Messrs. W. G. Black, L. V. Turner, and H. Lucas were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Messrs : Ashe, Jam es Samuel, The Adelaide Hospital, Dublin. Cook, Arthur James, 167, Richmond Road, Hackney, N.E . Dobson, Henry Arthur, Paisley Street, Orange, N.S.W. Kewley, James, King's College, Cambridge. Macknight, Alexander, Brucefield, Whitburn, N.B. Martindale, William Harrison, 10, New Cavendish Street, W. Peck, John Wicliffe, 28, West Ella Road, Harlesden, N.W. The list of names of those recommended for election as Officers and Members of Council was read.Of the following papers, those marked * were read :-"32. "The slow oxidation of methane at low temperature~." By W. A. Bone and R. V. Wheeler. The authors have studied the slow oxidation of methane at temper-atures between 300' and 400' in a supply of oxygen just sufficient to burn the carbon to carbon monoxide. The method adopted consisted in sealing mixtures of two volumes of methane and one volume of oxygen in bulbs of boro-silicate glass, which were maintained at constant temperatures of 300°, 325O, 350°, and 400' for periods of time 52 varying from 1 day to 3 weeks, The bulbs were afterwards examined and a careful analysis of the resulting mixture made. The results indicate (1) that the disappearance of the oxygen is accompanied by a proportionate diminution in the volume of the cooled products, due to formation of water.(2) That at no stage of the process is either free hydrogen or free carbon liberated. (3) That a portion only of the methane is burnt, the carbon of which appears as carbon monoxide or dioxide, and the whole of the hydrogen as water. (4) That no other products can be detected at any stage of the oxidation. Since the interaction of methane and oxygen at these temperatures is a 'surface ' phenomenon, it is impossible to measure the relative velocities of the reaction at different temperatures, but evidence was obtained that the velocity increases with rising temperature. Thus at 300°, where the velocity is just appreciable, the disappearance of oxygen and formation of water can only be detected after the lapse of one or two weeks, At 400°, on the other hand, the whole of the oxygen always disappeared within a single day, and at 350°, in some instances, in three days.Experiments have shown that similar bulbs containing electrolytic gas can be maintained at 350° for a week and at 400' for three days, without any visible formation of water occurring; at 400°, in one instance out of three, a marked formation of water took place in a week ;in the other two bulbs, however, no change could be detected. A study of the following possible secondary reactions at 326O, 350°, and 400°, namely (1)GO +H2O=CO2 +H,, and (2) 2CO +0,=2C02, (moist) indicates that no complication arising from them enters into the methaneoxygen experiments.Further, it has been proved that the following substances do not react at 350-4OOc, namely (1) methane and steam, (2) methane and carbon dioxide, (3) carbon and steam, The authors therefore conclude that the first stage of the oxidation of methane at these temperatures does not consist of a 'selective corn-ktiort' of either hydrogen or carbon, but in a aimultmowr om'htion of cmh CWUE hydrogen, as represented by the equation 2CH4+30, = 2c0 +4H20. The occurrence of carbon dioxide in the products (and in many cases as much as one-tbird to one-half of the carbon burnt appears a8 the dioxide) cannot be explained on the supposition that carbon monoxide liberated in the primary oxidation is subsequently graddZy oxidised through the agency of steam and oxygen, or steam alone.The more probable explanation is that the carbon monoxide and steam molecules which simultaneously come into being in the primary oxidation are, at the moment qf formation, in a very labite and reactive condition, and this would favour the rapid exchange of oxygen in the system, 53 CO OH, I 0,. The carbon dioxide is mainly, if not entirely, pro- I duced during this short ' labile period.' "33. ''Isomeric additive compounds of dibenzylketone and deoxy- benzoin with benzal-ptolnidine, nz-nitrobenzalaniline, and benzal-m-nitraniline. Part 111." By F. E. Francis, B.Sc., Ph.D. The additive compounds formed with dibenzylketone and deoxy- benzoin with benzal-ptoluidine were unstable and consequently unsatis- factory for confirming the existence of the so-called a-,p-, and y-modifications.In the case of dibenzylketone and m-nitrobenzalaniline the /3-modification obtained by recrystallisation of the a-form from benzene containing traces of piperidine melted 31' higher, and with dibenzylketone and benzal-m-nitraniline 43O higher than the a-additive product; in the latter case, there was also a distinct change in the solubility and appearance of the p-form. These were considered satisfactory confirmations of the individuality of the &modification, because in cases previously investigated the rise in melting point was never greater than 10--12O, and since the P-modifications were transformed into the a-by means of heat, this small difference in melt- ing point was not very satisfactory.a-Dibenzylketone benzal-m- nitraniline on recry stallisation from benzene containing traces of sodium ethoxide appears to be converted into the y-modification, and the melt- ing point rises from 134' to 182*3O,but this was the only case observed. Substances of much higher melting point and smaller solubility, and apparently belonging to neither a-,6-,or y-modifications, were obtained in the case of deoxybenzoin and benzal-p-toluidine, deoxybenzoin and benzal-m-nitraniline, and dibenzylketone and rn-nitrobenzalaniline. These are similar in molecular weight and composition to the isomerides of lower melting point, and it is interesting to note that whereas dibenzylketone and benzal-mnitraniline give a pure a-additive com-pound, deoxybenzoin with the same substance only gives the isomeride of higher melting point.DISCUSSION. Dr.:LowaY asked if it was not possible that one of the three modifica- tions described by the author as the a-,p-and y-forms might be a stable mixture of two isomerides and not a single chemical compound. In the case of the three modifications of wbromonitrocamphor, those melting at 108O and 142O were found to be the normal and pseudo-nitro-compounds respectively, whilst that melting at 126* was only a stable mixture of these two. 54 Dr. FRANCIS,in reply, said that he had been unable to obtain any evidence that any of the modifications described was a mixture, and that if they were mixed they could be again separated by fractional crystallisation. *34.G1 Mesoxalic semi-aldehyde.” By H. J. H. Fenton, F.B,S.,and J. H. Ryffel, B.A.,B.Sc. Chlorine is slowly absorbed by a solution of tartaric acid containing iron in the ferrous state, and the product, after removal of the unaltered tartaric acid, is found to have powerful reducing and other aldehyde properties. With phenylhydrazine, it yields a bright orange precipitate having the composition C15H14N402twhich is identical in every respect with the osazone obtained by Nastvogel from dibromo -pyruvic acid (Annalen, 1888, 248,85) and by Will from collodion-wool (Ber., 1891, 24,400 and 3831). A re-investigation, however, proves that the true melting point of this osazone is 222-5224’ instead of the lower number, 201-207O, ascribed to it by various authors.This osazone has the constitution CH:N2HPh*C:N2HPh*C02H and corresponds either to hydroxy-pyruvic acid, tartronic semi-aldehyde, or mesoxalic semi-aldehyde. With hydroxylamine, however, the dioxime, CHNOH*CNOH*CO,H, or dioximidopropionic acid is obtained identical with that prepared by Soderbaum from dibromopyruvic acid (Bey., 1892, 25, 904) and by oxidation with cupric hydroxide in alkaline solution mesoxalic acid results. Since the oxidation product is free from chlorine, these facts leave no room for doubt as to the nature of the substance in question, namely, that it is the semi-aldehyde of mesoxalic acid.Its formation from tartaric acid in the manner above described is due to the initial production of dihydroxymaleic acid, and it may be prepared in a pure state directly from the latter acid by the action of ferric salts. With ferric sulphate or chloride, for example, the change takes place almost quantitatively according to the equation : C,H,O, + Fe2(S04),=C,H,04 +2FeS0, +H2S04+CO,. After removal of the iron salt and free mineral acid, the product is obtained as a thick syrup, which, so far, has not been induced to crystallise. The derivatives and transformations of this aldehyde- wid are being further investigated. 55 "35. "The action of hydrogen peroxide on carbohydrates in the presence of ferrous salts.111." By R. S. Morrell and J. M.Crofts. The specific action of hydrogen peroxide in the presence of ferrous sulphate was first demonstrated by Fenton in the oxidation of tartaric acid to dihydroxymaleic acid (Trans., 1894, 65,899). Glucose, lsevulose, arabinose, and rhamnose have been shown by the authors to be transformed by this peculiar reaction into osones, which were recognised by their power to react with substituted hydrazines at the ordinary temperature (Tyans.,1899, 75,786, and 1900, 77, 1210) It has been found that mannose on oxidation gave an osone which yielded with phenylhydrazine at the ordinary temperature phenylglucosazone. The preparation of pure glucosone from both glucose and laevulose has been attempted, and a white, amorphous solid has been obtained which gave analytical results agreeing with the formuls C6H1206and C6H1006.This substance reacted readily with phenylhydrazine at the ordinary temperature and furnished a good yield of phenylglucosazone. The glucosone from glucose was feebly dextrorotatory, whilst that from laevulose was slightly laevorotatory. Glucosone obtained by E. Fischer (Ber., 1889, 22, 87) is lmorotatory. An aqueous solution of glucosone: prepared from either glucose or lsvulose on oxidation with bromine at 40' furnished a good yield of the calcium salt of a trioxybutyric acid. The barium salt of the same acid has been obtained, and both the calcium and barium salts seem to be identical with d-erythronic acid (Ruff, Ber., 1899, 32, 3678). The calcium and barium salts of this acid obtained from glucosone prepared from either dextrose or lsvulose have yielded butyric acid on reduction with hydriodic acid and phosphorus.'36. m-Nitrobenzoylcamphor." By M, 0.Forster and Miss F. M.G. Micklethwait. CBr*CO*C,H,N02a'-m-Nitrobensoyl-a-b~*omocamphor, co pre-C8Hl,< I Y pared from a'-benzoyl-a-bromocamphorand fuming nitric acid, separates from methyl alcohol in pale yellow, flat, prismatic needles melting at 93-94'; a 2 per cent. solution in chloroform has [a],= -1-87.9'. a-m-Nitro&enxoyZ-a'-bromoccjcmphor,obtained in a similar manner from the isomeric benzoylbromocamphor, crystallises in aggregates of small, pale yellow needles and melts at 101-102° ;a 2 per cent.solution in chloroform has [a],= -26.1". Enolic m-nitrobenxoylcccmphor, C8H14<&OHc*c0'C6H4N02, formed on 56 reducing the nitrobenzoylbromocauphors with alcoholic potash, crys- tallises from alcohol in long, pink, silky needles melting at 106-107°; it has not been obtained in the ketonic form, but the specific rotation of a 2 per cent. solution in chloroform, having [a],= + 209.5' when freshly prepared, falls to + 200.1' in the course of several days, indi- ca ting slight transformation into the isomerid e. m-Nit robenzoylcam- phor dissolves in aqueous alkali hydroxides and the alcoholic solution develops an intense purple coloration with ferric chloride ;oxidation with potassium permanganate gives rise to carnphoric and m-nitro- benzoic acids.The acety2 derivative crystallises from light petroleum in pale brown needles and melts at 127-128'. Enolic o-nitrobemxo?/lca~phoor crystallises from alcohol in pale brown, transparent prisms and melts at 118O ;a 2 per cent. solution in chloro-form has [.ID = +44.5' when freshly prepared, and +60.5' after an interval of several days. a'-m-Nitrobenxoyl-a-chlcrocamphor,L',H,4<~~'c6H4N02 crystal-, lises from alcohol in aggregates of pale yellow prisms and melts at '72-74O ; a 2 per cent, solution in chloroform has [a], = +40.4'. a-m-Ni~roben~o~l-u'-chZoroc~~~horseparates from alcohol in small, nearly colourless needles and melts at 110'; a 2 per cent. solution in chloroform has [a],= + 7.1". When these isomerides are heated with alcoholic potash, enolic m-nitrobenzoylcamphor is not formed ; the sole products are a-chlorocamphor and m-nitrobenzoic acid.iL*37. The Cloez reaction." By F. D. Chattaway and J. 116. Wadmore. The reaction between cyanogen chloride or bromide and an alcoholic solution of sodium ethylate appears at first sight to be inconsistent with the nitrogen halogen constitution which we have shown cyanogen chloride and bromide to possess. It becomes intelligible, however, when we consider the behaviour of the nitrogen halogen linkage towarda alcohol, Halogen attached to nitrogen reacts very readily with alcohol, the halogen being invariably replaced by hydrogen and tt hypohalogen ester formed thus : :N -X +C,H,OH =:N*H+U2H,0X.The interaction of ethyl alcohol and trichloriminocyanuric acid, when ethyl hypochlorite and cyanuric acid are produced, is a simple case. In the Cloez reaction, cyanogen chloride or bromide first reacts with the alcohol as a typical nitrogen halogen compound, forming hydrocyanic acid and ethyl hypochlorite or hypobromite, thus : C:N*C1+ C2H50H =C:N*H+C2H,0C1. 57 These then combine and form ethyl iminochlorocarbonate, the hydro- cyanic acid, or sodium cyanide, since sodium ethylate is present, behaving as an unsaturated substance : C2H,0C1+C:N*H= CHO 2 5cl,>C:K*H. The ethyl iminochlorocarbonate then reacts in various ways to form the different substances which have been isolated from the product of the action, for example, it reacts with alcohol to form diethyl imino- carbonate, with water to form urethane, whilst three molecules inter- act with elimination of hydrogen chloride to produce normal triethyl cyanurate. DISCUSSION.Professor TILDENthought Dr. Chattaway had brought forward a body of evidence which practically established his case, but he would like to inquire whether the production of a nitrile, by interaction between a common cyanide and a haloid compound, had engaged the attention of the authors, and what explanation they would give of the mechanism of the change. In such interactions, carbon appears to be directly attached to carbon, and there is no evidence of even a tem-porary formation of a compound in which the cyanide group is linked on by means of the nitrogen.gDr. CHATTAWAY,in reply, stated that the imino-structure of cyanides admitted of action occurring in three ways, addition to the nitrogen, or to both nitrogen and carbon, or to carbon, taking place thus : H*N:C+X,=HX,iN:C; or H-N:C+X,=H-NX*CX;or H*N:C+X, =H*N:C:X,, the mode of interaction in any particular case and the further secondary changes being determined by the nature of the cyanogen derivative and by that of the substance interacting with it. All reactions of these compounds could be formulated according to one or other of these types. The imino-formuls of the cyanides are capable of expressing conventionally three phases of atomic relationship, the atoms composing a single molecule can only be in one phase at any instant, but the particular phase at which it reacts is determined by a related phase of the interacting molecule, 38.The picrimidothiocarbonicesters.” By J. C. Crocker, B.A. When picryl chloride is treated with ammonium thiocyanate in alcoholic solution, a reaction readily takes place from which a well crystallised yellow substance is obtained, having the empirical formula C,,H,N7S0,,. On hydrolysis, it yields picramide. The reaction may be thus explained. Picryl thiocarbimide, Pi*N:C:S, is probably the first product. A molecule of this substance adds on another molecule of picryl chloride, the chlorine atom becoming attached to the carbon 5s atom and the picryl group to the sulphur atom. The acid chloride thus formed reacts with the alcohol to form a picrimidopicrylthio-carbonic ester with the elimination of hydrochloric acid.Thus : Pi*N:C:S + Pic1 -+ Pi.N:C<s-pic1 -+ Pi*N:C<,-+pi c1 + OEt Similar substances have also been prepared EtOH -+ PiN:C<S.pi. from methyl, propyl, and isobutyl alcohols. In the case of methyl alcohol, two ’substances have been obtained, which are stereoisomeric, corresponding to the “syn-” and “anti-” forms of the oximes CH, 0.9*S* Pi CH,*O*8*S*‘PiandK*Pi Pi*N ’ 39. “ Robinin, violaquercetin, myrticolorin and osyritrin.” By A. G. Perkin. In continuation of the research of which a preliminary account has already been given (PToc.,1901, 17, 87), the author has re-examined the properties of myrticolorin, C27H28016,a quercetin glucoside present in Eucalyptus macro~*?~ynchu,which, as described by H.G. Smith (Tram., 1898, 73, 697), differed mainly from osyritrin (Proc., 1901, 17, 87) in that the sugar derived from it appeared to be galactose. As Smith (private conimunication) finds on re-examination that this is dextrose, comparative experiments have been carried out. The results show that myrticolorin is identical with osyritrin. 40. (‘The nitration of s-trihalogen anilines.” By K. J. P. Orton. The carefully regulated action of nitric acid on the six 8-trihalogen anilines, s-tribromoaniline, 2-chloro-4 : 6-dibromoaniline,2 : 6-dichloro-4-bromoaniline, 4-chloro-2 :6-dibromoaniline, 2 :4-dichloro-6-bromoaniline, and s-trichloroaniline has been investigated.The anilines were dissolved (or suspended) in glacial acetic acid; to the solution nitric acid free from nitrous acid was added ; the mixture, which now con-tained crystalline aniline nitrate, was heated on the water-bath. From their behaviour when this mixture is heated, the anilines may be sharply divided into two classes, namely, those with a bromine atom in the para-position relative to the a-mino-group and those with a chlorine atom in the para-position. With the first, the nitrate of the aniline dissolves quickly, forming an orange solution, which becomes gradually more yellow in colour and gives off bromine ; on cooling, an aniline crystallises out, in which the p-bromine atom has been replaced by a nitro-group ; thus, from s-tribromoaniline, 2 : 6-dibromo-4-nitroaniline 59 is obtained (compare Losanitsch, Ber., 1882, 15,474) ; from 2-chloro- 4 :6-dibromoaniline7 2-chloro-6-bromo-4-nitroaniline(m.p. 177"), and from 2 :6-dichloro-4-brornoaniline,2 :6-dichloro-4-nitroaniline are ob-tained. Secondly, when a chlorine atom is in the para-position, a solu-tion is obtained, transiently of a purple colour, which quickly passes to magenta and then slowly to a deep crimson. No chlorine or bromine is evolved, nor are anilines detectable in which a bromine atom in an ortho-position or the chlorine atom in the para-position has been replaced by the nitro-group. During the period of heating there can be isolated from the solutions of both the above classes of anilines a small quantity of the corre- sponding nitroamines ; thus, from s-tribromoaniline is obtained nitvoamino-2 :4:6-tribromobenxene, slender flesh-coloured needles (from water) melting and decomposing at 143-144' ;and from s-trichloro-aniline, nitroamino-2 :4 :6-trichZorobeinxene, slender flesh-coloured needles (from water) melting and decomposing at 135'.In solution in acetic acid, in the presence of a trace of a mineral acid, the nitro- amines themselves undergo change, that from s-tribromoaniline yielding 2 :6dibromo-4-nitroaniline, whereas that from s-trichloroaniline yields a characteristic crimson solution. From the crimson solution can be isolated a small quantity of a red crystalline substance, melting and decomposing at 143'.Experiments on the preparation of this and allied substances are now in progress. 41, Some s-nitrochlorobromoanilinesand their derivatives." By IC. J. P.Orton. The following anilines, acetanilides, diacetsnilides, and chloroamino- derivatives have been prepared in connection witb the investigation described in the preceding communication. Z-Chl~o-6-bromo-d-nitroaniline,CGH,C!lBr(NO,)oNH,, prepared by chlorinating 2-bromo-4-nitroaniline7 long, yellow, prismatic needles melt- ing at 177' ;2-chloro-6-bromo-4-nitroacetaniZide,C6H2ClBr( NO,)*NHAc, slender, colourless prisms melting at 22 1-222' ; 2-chZor+6-bomo-4-.nitrodiacetmiZide,C,H,ClBr(NO,)*NAc,, colourless f our-sided prisms melting at 134' ; ucetyZchZoroamino-2-c?~bro-6-bromo-4-nitroben~ne, G,H2C1Br(N0,)*NClAc, white, lustrous prisms melting at 84-85'.2-ChZoro-Cbromo-6-nitroaniline,C,H2ClBr(N0,)~NH2, silky, yellow needles melting at 114O; 2-ch20ro-4-bromo-6-~itro~etan~Zi~ede, C,H,ClBr(N02)oNHAc, prepared by nitrating 2-chloro-4-bromoacet-anilide, white needles or prisms melting at 194' ;acetylchloroamino-Z-chlor+4-bromo-6-ltitrobenxelzen~, C,H,ClBr(NO,)*NClAc, long, pale yellow, lustrous, very soluble prisms melting at 56-57', 4-Chloro-2-bromo- 60 6-).~itroaniZine, C,H,ClBr(NO,)*NH,, silky, yellow needles melting at 114-1 15' ;4-chZoro-2-bromo-6-nit~oacetaniZide,C6H,ClBr(N0,)-NHAc, prepared by nitrating 4-chloro-2-bromoacetanilide, white prisms melting at 207'. AcetyZchloroarnino-2 :6-dibromo-bnitrobenxene, C,H,Br,(NO,)*NCIAc, small, lustrous, four-sided prisms, with domed ends, melting at 110-1 1 1'.2 : 4-Dib~*omo-6-nitrodiacetaniZide, C6H,Br,(N0,)mNAc,, prepared by boiling the aniline with excess of acetic anhydride, aggregates of prisms or rhombs melting at 96-97'. 2 :3 :4 :6-!7!etrabromoacetaniEide,C,HBr,*NHAc, prepared from tetra-bromoaniline, silky, white needles melting at 228-229O ;2 :3 :4:6-tetrabrmodiacetanilide, C,HBr,*NAc2, lustrous, four-sided prisms with domed ends, melting at 164'. 2 :3 :6-Tribromo-4-42itroaniZine, C6HBr,(NO2)*NIT,, prepared by brominating 3-bromo-4-ni troaniline, pale lemon-yellow needles melting at 155-155.5". 2 :3 :4-rribromo-6-nitroaniline, C,HBr,(NO,)*NH,, prepared from 3-bromo-6-nitroaniline, orange-yellow needles melting at 165.5-166' ;2 :3 :4-tribromo-6-nit~o-acetccnilide, C,HBr,(NO,)*NHAc, colourless, flattened needles melting at 2319 42.The resolution of pheno-a- aminoheptamethylene into its optical isomerides. Tartrates of pheno-a-aminoheptamethyleneand of hydrindamine." By F. S. Kipping and A. E. Hunter. An investigation of the salts produced by the combination of dZ-pheno-a-aminoheptamethylenewith tartaric acid has shown that this base behaves quite differently from dl-hydrindamine (pheno-a-amino- pentamethylene) in spite of the similarity in constitution of the two bases. dl-Pheno-a-amimheptameth~lene-d-tartrate,2C11Hl,N,C,H,0, +&H,O, separates from neutral and from acid solutions of the dl-base in aqueous tartaric acid, in lustrous prisms decomposing at about 235' ;in aqueous solution [a], = + 13O.1-Pherto-aaminoheptamethylenehydrogen d-tartrate, C,,H,,N,C,H,O, +3H,O, is obtained when the solution of the normal tartrate is mixed with excess of tartaric acid and fractionally crystallised; it forms slender prisms and melts at 181-182'; its aqueous solutions are feebly laevorotatory ([ a]== -1-6' approximately). 1-Rheno-a-aminoheptamethyZened-tartrate, 2C11Hl,N,C,H,0,, prepared from the &base, crystallises in transparent, triangular plates and de- composes at 215-217'. The Iq&rochZoride of the 2-base forms lustrous prisms, and in dilute aqueous solution its specific rotation is [aJD= 3-24', Benxoyl-1-pheno-a-aminoheptamethylene,C,,H,,N*COPh, crystallises in needles, melts at 175--176O, and is dextrorotatory in methyl alcoholic solution.61 d-Phano-anmiraoheptamrthylerte d-tartrate, 2C,,H15N,C,H,0,, can be isolated from the mother liquors obtained after separating the hydrogen salt of the I-base; it is anhydrousand decomposes at about 216-217'. d-P~e~o-a-arn~oh~ptamet~y~~hydrogen tartrats, Cl,Hl,N,C4H,0,, prepared by treating the normal salt with tartaric acid, decomposes at about 205-2069 dl-Bydrirzdccmine hydrogen d-tmtrate, C,HIIN,c4H606+H,O, crys-tallises in slender needles, melts at 168--169O, and is not resolved or changed in any way- by repeated crystallisation from water. The normal d-tartrate of the dI-base forms plates melting at about 200° and dissociates hydrolytically in aqueous solution.1-Pho-a-aminohptamethyZmd-bromocamphholrsdphnate, C,,Hl,N,Cl0H,BrO*SO,H, crystallises in prisms melting at 216-217O; in dilute aqueous solution [,,I, = +47.84 ADDITIONS TO THE LIBRARY. Landauer, John. Blowpipe analysis. Pp.173. London 1901. From the Publishers. Remsen, Ira. A college text-book of chemistry. Pp. 689. London 1901. From the Publishers. Soderbaum, Henrik (xustav. Jac. Berzelius. Sjalf biografiska anteckeningar. Utgifna af Kongl. Svenska Vetenskapsakademien genom H. G. S. Pp. 246. Stockholm 1901. From C. P. Sandberg. Travers? Morris William. The experimental study of gases. An account of the experimental methods involved in the determination of the properties of gases, and of the more important researches connected with the subject.Pp. 323. London 1901. From the Publishers. 11.Pu?*ch$e. Elbs, Karl. Ubungsbeispiele fiir die elektrolytische Darstellung chemischer miparate. Zum Cebrauch in Laboratorium fur Chemiker und Elektrochemiker. Pp. 100. Ill. Halle-a-5. 1902. Encomium Argenti Vivi. A treatise upon the use and properties of quicksilver, or, the natural, chemical, and physical history of that surprising mineral, extracted from the writings of the best ndiuralists, chemists, and physicians. Wherein its various operations are accounted 62 for, and the use of it recommended : with some remarks upon the animadversions of Dr. Turner upon belloste. London. ANNUAL GENERAL MEETINU. The Annual General Meeting of the Society, for the election of Officers and Council, and for other business, will be held on Wednesday, March 26th, at half-past four o’clock in the afternoon.RAOULT MEMORIAL LECTURE. The Raoult Memorial Lecture will be delivered by Professor van’t Hoff, on Wednesday, March 26th, at 9 p.m. This Lecture will be delivered, by kigd permission of the Managers, in the Theatre of the Royal Institution, Albemarle Street, W. Admission will be by ticket only. Each Fellow of the Society will be entitled to two tickets, which may be obtained on application to the Assistant Secretary, Chemical Society, Burlington House. At the next meeting, on Wednesday, March 19th, at 5.30 p.m., the following papers will be communicated : *I The absorption spectra of metallic nitrates. Part I.” By W. N, Hartley. ‘‘A method of determining the ratio of distribution of a base between two acids.” By H. M. Dawson and F. E. Grant. On the molecular complexity of acetic acid in chloroform solution,” By H. M. Dawson. 6‘ On the existence of polyiodides in nitrobenzene solution.” ByI€.M. Dawson and R. Gawler. ‘‘Nitrogen chlorides containing the propionyl groups,” By F. D. Chtrttaway. Derivatives of a-aminocamphoroxime.” By A. Lapworth and A. W. Harvey.‘;Preparation of sulphamide from ammonium amidosulphite.” ByE. Divers and M.Ogawa.‘(Hypoiodous acid.” By R. L. Taylor. RICEABD CLAY AND SONS. LIWITED, LONDON AND BUNOhY
ISSN:0369-8718
DOI:10.1039/PL9021800051
出版商:RSC
年代:1902
数据来源: RSC
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