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Proceedings of the Chemical Society, Vol. 9, No. 128 |
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Proceedings of the Chemical Society, London,
Volume 9,
Issue 128,
1893,
Page 199-231
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摘要:
Issued 16/11/1893. PROCEEDINGS OF THE CHEMICAL SOCIETY. No. 128. Session 1893-94. The following are abstracts of papers received during the vacation, and published in the Transactions :-56. ‘‘ Peri-derivatives of naphthalene.” By R. Meldola, F.R.S.,and F. W. Streatfeild, (Trans., 1893J1054.) A description is given of the preparation of 1: 1’-,or peri-nitro-naphthylamine by nitrating a-naphthylamine in presence of sulphnric acid, and of the preparation from this compound of benzylidene-1 : 1’-nitronaphthylamine, 1: 1‘-nitrobromonaphthalene, 1: 1‘-bromonaph-thylamine, 1: 1’-bromonaphthol and 1: 1’-dibromonaphtbalene. 57. “ Note on lead tetracetate.” By A. Hutchinson, M.A,, Ph.D., and W.Pollard, B.A. (Trans., 1893, 1136.) It is shown that the compound which crystallises from a solution of red lead in glacial a.cetic acid, described by Jacquelain, in 1851, is Zead tetracetate, Pb( C2H,O2),. A corresponding propionate haR been obtained.On adding ammonium chloride to a solution of the tetr-acetate in chlorhydric acid, a, precipitate of the characteristic double salt of ammonium chloride and lead tetrachloride is produced. 58. “ Resolution of lactic acid into its optically active components.”’ By T.Purdie, Ph.D., B.Sc. (Trans.,1893, 1143.j Inactive lactic acid has already been resolved into its active com- ponents by two of the three general methods discovered by Pasteur, namely, by selective fermentation and by crystallisation of salts of the alkaloids. The author finds that the third method, that of spon-taneous resolution by crystallisation, can also be applied with success.In the course of an inrestigation on the resolution of lactic acid 200 into its active components by crystallisation of the strychnine saIts (Purdie and Walker, Trans., 2892, 754) an active zinc ammonium lactate was encountered, which possessed in a marked degree the property of forming supersaturated solutions when dissolved in a syrup of active ammonium lrtcta.te, and of separating from these solutions in comparatively large, well-defined crystals. It was also observed that a strong solution of ordinary ammonium lactate dis- solves large quantities of ordinary zinc lactate, forming a syrup from which an inactive zinc ammonium lactate does not at once crystallise.but which readily deposits zinc lactate when slightly diluted. These observations suggested the idea that possibly the active double salts might be present in such a solution in a state of supersaturation, and that they might be separately crystallised from it under suitable conditions of temperature and concentration by adding the proper crystalline nuclei. It is found that by heating a solution containing certain definite pro- portions of ammonium lactate, zinc lactate and water and then cool- ing, a snpersatumted solution is obtained, from which either of the active salts or the inactive salt cah be separated at will by adding traces of the respective salts as nuclei. By alternately dropping into such a solution dextrogymte and laevogyrate nuclei, and adding fresh inactive zinc lactate to the exhausted mother liquor, it is pos-sible to obt.ain successive crops of the oppositely active salts in quantity.By recrystallisation, products are readily obtained con-taining over 90 per cent. of the active substances. The admixture of inactive salt can be eliminated by crystallisation of the zinc lactate prepared from the double salts. Determinations of the specific rotations of the zinc lactates thus obtained gave numbers agreeing with those given by Wislicenus for zinc snrcolactate at similar con- centration. When equal quantities of 8 per cent. solutions of the oppositely active zinc ammonium salts are mixed, inactive zinc lactate is precipitated.The inactive zinc ammonium salt waLs also prepared, and was found to have the composition represented by the formula Zn(C3H503)2*NHd*C3H503*3H20,while that of the active salts is Zn(C,H503)2*NH~*C3H503*2H20.The salts also differ considerably in properties. 59. ‘‘The colouring principles of Rubia sikkimensis.” By A. G. Perkin,and J. J. Hummel. (Trans., 1893, 1157.) The authors have separated both purpurin and munjistin or pur-puroxanthincarboxylic acid from this root ; they point out that the results show that it is nearly identical as regards colouring principles with the closely allied Rzcbicc munjistin. 201 60. “The coIourin$ and other principles contained in chay root.” Bythe same. (Trans., 1893,1160.) Chay root is the root of Oldenlajtdia urnbellata, and is used as a dye-stuff in India ; a large number of distinct products were isolated by extracting it either with an aqueous solution of sulphurous acid, or with lime water, alcohol and other solvents, viz., two substances of the formula CI6Hl2O5,both of which are shown to be anthragallol- dimethyl ethers ; a, monomethyl ether of alizarin crystallising in orange needles melting at 178-179” ; a resinous yellow substance, possibly an isomeric methyl ether of alizarin in an impure form; metahydroxyanthraqninone ; a yellow substance melting at 141”, which yields alizarin when heated with sulphuric acid ; ruberythric acid ; rubichkwic acid; alizarin; a wax of the formula, (CloH,,O)e, melting at 87--8S“ ;and cane sugar.61. ‘I Phenylnaphthalenes. I. a-Phenylnaphthalene.” By F. D. Chatt-away, B.A. (Trans., 1893,1185.) It is shown that a-phehylnaphthalene can be synthesised in several ways, but that the yield in all cases is unsatisfactory. The best method is by the action of a-chloronaphthalene on benzene in the presence of anhydrous aluminium chloride. a-Phenylnaphthalone is obtained as a thick, oily liquid which solidifies 011 long standing, affording a fatty-looking mass without definite crystalline form. It boils at 324--325”, and is readily soluble in alcohol, ether and benzene, but cannot be obtained crystalline from these solutions, being deposited on evaporating them in oily drops. It volatilises with steam, and possesses a, peculiar odour resembling both naphthalene and diphenyl. 62.“The vapour pressures, molecular volumes and critical constants of ten of the lower ethereal salts of acids of the acetic series.” By Sydney Young, DSc., F.R.S., and G. L. Thomas, B.Sc. (Trans., 1893, 1191.) The authors’ chief object was to ascertain how far the generalisa- tions of Van der Waals regarding “ corresponding ” temperatures, pressures and volumes are true for the members of a group of allied compounds. It has already been shown by one of them that the generalisations hold good, with a close approximation to accuracy, in the case of the four mono-haloid derivatives of benzene, but that when componnds of different chemical character are compared much greater deviations are to be observed, more especially as regards the absolute temperatures (boiling points) at corresponding pressures.It has also been shown that among the substances so far studied the deviations are greatest in the case of acetic acid and the alcohols, and 202 it becomes, therefore, of additional interest to examine the behaviour of the salts formed by the interaction of the fatty acids and alcohols. The critical and other constants of a nxmber of these have been determined by several observers, but the results are far from con-cordant, owing, probably, to imperfect purification of the substances examined. Two samples of each ethereal salt we1.e employed : one was prepared from the acid or anhydride and the alcohol ; the other was obtained from Kahlbaum.All were carefully purified, and their purity was proved both by the constancy of their boiling points and by the agreement between the boiling points, relative densities and critical temperatures and pressures of the two samples. The investigation shows that although the results obtained with the ten compounds are in fair agreement with the generalisation af Van der Waals-in close agreement so far as the molecular volumes of liquid are concerned-yet the deviations observed are related to their composition. The ratios of the absolute temperatures to the absolute critical temperatures at any series of corresponding pressures are clearly dependent on the molecular weights, though this is apparently nut the case with the ratios of the molecular volumes of either liquid or saturated vapour to the critical volumes.The composition of the isomeric ethereal salts appears, however, to influence all the ratios, those for the formates being lowest when the absolute temperatures or volumes of saturated vapour are com- pared and highest in the case of the volumes of liquid. The ratios for the acetates, on the other hand, are highest in the case of the absolute temperatures and of the volumes of saturated vapour, and lowest for the volumes of liquid. The presence oE the iso-group in methylic isobutyrate appears to have a distinct influence on the ratios. The ratios of the actual critical densities to the theoretical densities (for a perfect gas) show a maximum variation of 2 per cent.; the mean value, 3.91, is some-what higher than that (3.76) for the majority of substances previously studied; it is, hoviever, lower than for the alcohols and for acetic acid. The ratios of the absolute temperatures and of the volumes of liquid and saturated vapour at corresponding pressures to the critical constants, also the values of PV/T at the critical points, are compared with those of the substances previously studied, and it is found that the ethereal salts form a separate group. The 22 compounds for which data are available fall into four group$, (1) the ethereal salts, (2) the alcohols-methyl alcohol being especially abnormal, (3) acetic acid, (4) ether, benzene and its haloid derivatives, carbon and tin tetrachlorides. 203 63."The fermentation of dextrose, rhamnose, and mannitol by a lsvo= lactic ferment." By George Tate, Ph.D. In studying the micro-organisms that attack ripe pears, the author has had occasion to isolate an organism that under acrobic conditions brings about levolactic fermentations of the hexoses dextrose, mannose and galactose and also of mannitol, but an inactive lactic fermentation of the methylpentose rhamnose (isodnlcite), The products of the fermentation of dextrose, mannitol and rhamnose have been quantitatively determined : 9 molecules of dextrose are found to yield 2 molecules of alcohol, 1 of succinic acid, 7 to 8 of hvolactic acid, and smaller molecular proportions of formic and acetic acids. Mannitol yields the same products, but in different proportions, there being a greater yield of alcohol and slightly greater yield of laevolactic acid.Neither alcohol nor formic acid was found among the products of the fermentation of rhamnose ; 9 molecules of this sugar afforded approximately 5 molecules of acetic acid and 4 molecules of optically inactive lactic acid. The action of the organism as a lsevolactic ferment of dextrose, was found to be unchanged after cultivating the parent cells in fluids containing rhamnose, inactive acid being formed. The organism which is referred to as a laevolactic ferment from its action upon the typical sugar dextrose belongs to the class of asco-bacteria, and can develop so as to produce two forms of growth, widely differing in macroscopic appearance-one in which rods and cocci predominate, a second in which the organism propagates as an ascobacteriurn.64. ('Derivatives of quinone containing halogens. Part 111. Derivatives of quinhydrone." By Arthur R. Ling and Julian L.Baker. (Trans., 1893, 1314.) Quinhydrone melts at 170-171". The authors have obtained a compound having the composition of a monochZoroquin7zydrone, which melts at 145O, by gently heating a solution of qninone and mono- c hloroquinol in chloro€orm ; under somewhat similar circumstances, Clark (Amer. Chem. J., 14, 574) obtained a small amount of quin-ltydrone. They have also obtained an isomeric compound melting at 132-133" by evaporating an ethereal or alcohol solution of quinol and monochloroquinone. When either of these isomerides is boiled with light petroleum they dissociate, and their constituents then interact, giving rise to dichloroquinhydrone, which is dissolved by the light petroleum, and quinhydrone, which remains undissolved.DichZoro~uinhydro~ze,C6H,C10,,C6H3C1(OH),, is obtained by mixing 204 solutions of monochloroquinone and monochloroquinol, and also by partially oxidising a solution of monochloroquinol with ferric chloride. It crystalliaes from water in dark violet needles containing one mole- cular proportion of water, melting at 70-72"; fhese are rendered anhydrous when kept over concentrated sulphuric acid and then melt at 93-9Q. Tetrachloroquinhydr~~~e,C,H,CIZO2,C6HzCl2(0H),+ 2Hz0, was de-scribed by Stadeler, in 1849.It is obtained in the form of dark violet needles by triturating paradichloroquinone and paradichloroquinol with water, and also by partially oxidising a solution of paradichloro-qninol; the authors find that it melts between 105' and l40", but has no definite melting point. They confirm Stiideler's observations that it loses its water of crystallisation when kept over concentrated sulphuric acid, becoming light yellow ; the crystalline form of the an- hydrous compound appears to be the same as that of the hydrated compound. An isomeride is obtained when metadichloroquinol and an excess of metadichloroquinone are boiled with a mixture of benzene and light petroleum ; it separates from the filtrate in long, brown, prismatic needles, and melts at 135".HexachZoroquinhydrone.-A substance of tb e composition c12H4c160, + &HzOis obtained by triturating trichloroquinone and trichloro- yuinol with water ; it melts at 115-117" and does not alter in weight when kept over concentrated sulphuric acid. The authors failed to obtain octochloroquinhydrone, and conclude, from numerous experiments which are described, that this compound is non-existent. Dibro?izoquinhyd.r.one, C6H,Broz,C6H,Br(oEi)2,crystallises from water in anhydrous, dark, bronze-coloured needles and melts at 98". Tetrabromoquinhydroize is obtained by boiling an aqueous solutioia of paradibromoquinol with an excess OP paradibronioquinone ; it aeparates, when the filtrate is rapidly cooled, in dark violet needles of the composition CsH2Br,0,,C6H2Br2(OH), + 2Hz0, rtnd melts at 145-150". It loses its water of crystallisation and becomes light- colonred when kept over concentrated sulphuric acid.DichZorodibromopuinhydrone,prepared from paradichloroquinone and paradibromoquinol, ci-ystallises from water in bluish-black needles containing two molecular proportions of water ; it melts at 130-135" and loses its water of crystallisation, becoming light -yellow coloured when kept over concentrated sulphuric acid. An isomeride is ob-tained from paradibromoquinone and paradichloroqninol ;it resembles the last-described compound and becomes pale brownish-yellow, losing its water of crystallisation, when kept over concentrated snlphnric acid.205 November 2nd, 1893. Dr. Armstrong, President, in the Chair. Messrs. Edmnnd Lamb, James A. Audley, Henry Bailey and Charles Mills were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Messrs. Frederick Edmund Bowman, Ash Leigh, Bowdon, Cheshire ; Henry Fielden Briggs, Roseneath, Toryuay ; Frank Browne, Government Civil Hospital, Hong Kong ; John Dixon Brunton, Wire Mill, Mussel-burgh ; Charles March Caines, 11, Clockhouse Road, Beckenham, Kent ; Thomafi Petson Carswell, 369, Scotswood Road, Newcastle-on- Tyne; Harry J. Chaney, 29, Chalcot Crescent, Regent’s Park, London ; Allan Thomas Cocking, 39, Lister Street, Rotherham ; John A. Craw, 2, Millgate, Cupar Fife ; Charles Sordes Ellis, 17, Blooms-bury Square, W.C.; Alexander M. Fori-ester, 22, Scotia Street, Glasgow ; Henry Garnett, 2, Bartholoniew Villas, Kentish Town, N.W. ; William Hotton Grieve, 226, Friern Road, East Dulwich ; Harry Edtvin Hadley, The School of Science, Kidderminster ; Henry Ormsby Hale, Oundle School, Northamptonshire ; Harold Harris, Denmark House, Tuffley Avenue, Gloucest,er ; William Hesketh, B.A., School House, Ferriscowles, Blackburn ; Harold B. Holthouse, 42, St. Ann’s Valley, Nottingham ; Alexander Sinclair Hughson, 12, Myrtle Crescent), South Shields ; Bertram Hunt, F.I.C., 5, Qneen’c Crescent, Glasgow ; Richard Sarory Ladell, 155,Praed Street, Hyde Park, London ; William Fred Mawer, 16, Fentiman Road, S.W.; J.R. Morgan, Leydenburgh, Port Hall Street, Brighton ; Frederick Morton, 101, Quarmby Road, Huddersfield ; George 2’. Payae, M.D., Atlanta, Georgia, U.S.A. ; Thoinas Beilby Rawlins, 2, Levan Street, Pollockshields, Glasgow ; George Percival Rees, Ely House, Basford, Stoke-on-Trent ; Thomas Anderson Reid, Lostock Gralam, North& wich ; Herbert Santer, Albion Brewery, Caledonian Road, N. ; Philip Schidrowitz, 102, Oxford Gardens, Notting Hill, W. ; W. Edgar Sims, B.Sc., Stafford House, Longsight, Manchester ; Frederick Shapley, Whittier, Fuller &-Co., San Francisco ; Frederick Spencer, Rose Villa, Uttoxeter, Staffs ; Robert Curling Styles, Knockhall, Greenhithe, Kent ; Jocelyn Field Thorpe, Gloucester House, 20, Larkhall Rise, Clapham ; William Herbert Walden, 55, Clapham Road, S.W.; Frank Emest Welchman, 16, Carlton Road, Putney Hill, S.W. ; Williani Gilchrist White, Lamb Roe, Whalley, Lancashire ;Edward Hnmphreys Winder, 37, Vincent Square, S.W. ; Stanley Wyndham, Ph.D., Judson, Florida, c/o Trenton Phosphor Co. Of the following papers those marked * were read :- “65. “The action of bromine on azobenzene-a correction.” By Henry E. Armstrong. It was pointed out by me in a recent note in these Procecdings (1892, p. 194) that a compound represented by a formula such as is assigned to azobenzene, Ph.N:N*Ph, did not come within my “colour rule ” ; at the same time I drew attention to Werigo’s colourless tetra-bromazobenzene, and stated fhat Mr. Mills, at my request, had under- taken to further study the bromo-derivatives of azobenzene, and had already confirmed Werigo’s observation.According to Werigo, tetrabromazobenzene melts at 320“ ; the product obtained by Mr. Mills charred at a high temperature with- out melting ; when boiled with tin and muriatic acid, it gave a tetra-bromobenzidine, which was readiIy purified by crystallisation from boiling xylene ; this melted at 285” (uncorr.), and proved to be identical with that prepared from benzidine, following the directions of Claus and Rislor. This benzidine derivative was converted into a tetra-bromodiphenyl melting at 18Y0(uncorr.), from which a small quantity of dimetabromobenzoic acid was obtained by oxidation. During the course of the experiments, Mr.Mills was gradually led to notice that the original product from azobenzene was very similar to tetrabromobenzidine, and he eventually satisfied himself by repeatedly crystallising it from xylene that it was, in fact, nothing but impure tetrabromobenzidine. The difference in composition between tetrabromazobenzene and tetrabromobenzidine is so small that it is practically impossible to decide by analysis which compound is under examination ; and the fhct that tetrabromobenzidine is destitute of basic properties renders its differentiation difficult. Werigo’s tetrabromazobenzene must therefore be struck off the list of known compounds ; and no argument as to the constitution of azo-beneenc can be based on its behaviour with bromine.%6. “The origin of colour. X. Coloured hydrocarbons.” By Henry E. Armstrong. Graebe, in a recent note (Ber., 1893, 2354), adduces what ap- pears to be satisfactory evidence that the acenaphthylene, CI2H8, discovered by Behr and Van Dorp, is actually a yeZEow hydrocarbon, and contends that the colour of this hydrocarbon and also that of the red hydrocarbon from fluorene (cf. these Proceedings, 1893,192) is to be regarded a.s, in the first instance, conditioned by the presence of the group >C:C<. He ascribes the non-appearance of colour in ethylene derivatives generally to a secondary influence exercised by the groups displacing the hydrogen atoms in ethylene. 207 The problem is of such importance that I will venture to point out that in the case of coloured substances generally, the type of the series is itself always coloured-the only exception which I can call to mind being iodoform (cf. these Proceedings, 1893, 62).Ace-naphthylene, no doubt, cannot well be represented otherwise than by the formula but if possessed of an etlienoid structure akin H~CH to that of anthracene, an “ explanation ” of its colour may be given similar to that which I have put forward in the case of anthracene and of certain coloured pinoline derivatives (these Proceedings, /\/\ 1893, 63). On inspecting the formula I i 11 it will be seen that\(A(’ HC=C€I the carbon atoms of the one nucleus are attached to the benzene nucleus on the left in ortho-positions and by ethenoid linkages ; in other words, the hydrocarbon is an orthoquinonoid derivative.The external coupling is, in R measure, comparable with that which occurs in compounds such as methylene blue, &c., and it is this circumstance, perhaps, which causes the colour of the hydrocarbon to be so much more intense than that of anthracene, for example. “67. “The formation of the hydrocarbon ‘truxene ’ from phenylpropi-onic acid and from hydrindone.” By F. Stanley Kipping, Ph.D., D.Sc The further study of the hydrocarbon obtained from phenyl-propionic acid (Proc., 112,107, 117, 216) has led to the following results :-The hydrocarbon is formed when hydrindone is heated either with phosphoric anhydride or with moderately concentrated sulphuric 3cid ; it is also produced when a condensation product of hydrindone of the composition CleHlpO is heated with either of these dehydrating agents.This condensation product will be described in a future paper ; the fact that it is readily converted into the hydrocarbon proves that the latter has the formula C1BH12,and not C27H18,and is also evidence in fai-our of the view that the constitution of the hydrocarbon is CsH4*C=C-YHZexpressed by the formula ICH2*b=C-I C,H; This view affords a simple explanation of the formation of the hydrocarbon from phenyl-propionic acid and of its relation to other compounds. The hydrocarbon in question is evidently identical with a com- 208 pound obtained by Hausmann (Be?..,22, 2019) by heating hydrind one with concentrated chlorhydric acid, the study of which he did not continue.It is also identical with “ truxene,” a hydrocarbon prepared by Liebermann and Bergami (Ber.,22,782) by reducing “truxone ” with iodhydric acid ; this is proved by the fact that both compounds are converted into Gabriel and Michael’s “tribenzoylene-benzene ” (Ber., 10, 1557) on oxidation with chromic acid. The author discusses the constitution of “ truxene ” and of “trux-one,” and points out that the formula assigned to them by Lieber- mann and Bergami (Bey., 23,327) do not accord with the facts of the case, and are not to be reconciled with the formation of truxone from a-truxillic acid, ClSHl6OI. It is also shown that the only evi- dence which led Liebermann and Bei-gsmi to assume that “ truxene ’’ is a “tribenzylenebenzene,” namely, its conversion into “ tribenzoyl-enebenzene ” is of little, if of any, value.The constitution of “ tribenzoylenebenzcne,” being based on its conversion into triphenylbenzene, cannot be regarded as established, as it is first fused with potash at a high temperature and the product of this treatment is distilled over lime, in order to bring abaut the change. It follows, iherefore, that the conversion of the hydro-carbon from phenylpropioaic acid into ‘’ tribenzoylenebenzene ” does not show that the former (truxene) has the molecular formula C2,H18,but that “tribenzoylenebenzeiie,” which was hitherto sup- posed to have the molecular formula C2,Hl2Os,is, in reality, Cl8HsO2 ; this view is not refuted, but is rather corroborated by a study of the methods of forming “ tribenzoylenebenzene.” The behaviour of truxene with nitric acid and with bromine and its oxidation to nitrophthalic acid [2COOH :NOz = 1 :2 :41 are described ; attentivn is also drawn to a characteristic coloration which the hydrocarbon gives with ordinary concentrated sulphuric acid, and to its very peculiar decomposition by boiling nitrobenzene.68. “The action of aluminium chloride on heptylic chloride.” ByF. Stanley Kipping, Ph.D., D.Sc. The fact that hydrindone is formed in large quantities on treating phenylpropionic chloiide with aluminium chloride (Proc., 117,216) led the author to investigate the action of the latter on heptylic chloride, as it appeared possible that methylketohexamethylene, ethylketopentamethylene or some other closed-chain compound might be formed. After many unsuccessful experiments in which almost the whole of the heptylic chloride was recovered as heptylic acid, it was found that under suitable -conditions a large proportion of the acid chloride was converted into it neutml oil which was isolated by distillation in steam, but which proved to be a mixture ; on cooling the fractions of highest boiling point collected between 290" and 310°,a consider-able quantity of colourless crystals was deposited which, when freed from oil, melted at about 41'.Analyses of this crystalline product gave results (I, C = 82.2, H = 10.2; 11, C = 82.0, H =.10*0per cent.) corresponding to the formula ClaH200= 2C6H,,*COC1 -2HC1 -H,O -H2.It yields an oily hydrosime. On analysing this (found C s: 75.4, H = 10.0, N = 6.7 ; required C = 76.i, H = 9-6,N = 6.4), the percentage of carbon found was somewhat lower than corresponds to the formula C14H20NOH,doubtless owing to the fact that the oil could not be purified. It would seem, therefore, that the crystalline substance is a Icetone, as was; in fact, to be expected. The experiments which have been carried out up to the present with the object of determining its constitution, although few in number, have already afforded results of considerable interest. Fractions of the cmde oil collected between 280" and 310",when oxidised with nitric acid, gave a mixture of several acids, one of which was characterised by sparing solubility and was, therefore, easily isolated; analyses of this acid gave results pointing to the formula, C13H1,,06 (found C = 59.4, H = 3.9; required C = 59.5, H = 39, and an analysis of its siltier saZt, C,,H,O6Ag, (found Ag = 55.1; required 55.5 per cent.) confirmed this view.Whether this acid is an oxidation product of the ketone Cl4H,,O, or whether it is produced from some other constituent of the oil has not yet been determined, but in any case its indirect formation from heptylic acid is certainly rather extraordinary, as, to judge from its coruposition, it is a closed-chain compound. The investigation. of the behaviour of acid chlorides with alnm- inium chloride is being extended, and some progress has already been made with experiments with the chlorides of butyric, benzoyl- propionic and hippuric acids."69. "The inertness of quicklime. 11. The interaction of chlorine and lime." By V. H. Veley. The author has ascertained by synthetical and analytical methods that no appreciable action takes place between dry chlorine and quicklime below 300" ; above this temperature, a partial displace- ment of oxygen is effected by the chlorine : the interaction is thus analogous to that of barsta and chlorine, not specially dried, and at ordinary temperatures. “70. “Note on hyponitrites.” By D. H. Jackson, M.A., B.Sc. The author has conducted experiments for the purpose of obtaining alkali hyponitrites, hitherto known only in solution, in a solid state.He confirms the experience of previoug observers that, contrary to the statement of Menke, hyponitrite is not formed when sodium nitrate is heated with metallic iron. Reduction of a solution of sodium nitrate with aluminium or with barium amalgam does not furnish hyponitrite. For the production of byponitrites, the author employs Divers’ method of reducing a solution of sodium nitrate with sodium amalgam. He finds that the best yield of hyponitrite results from the use of ap amalgam weak in sodium acting at a low temperature; owing to the violence of the action, no hyponitrite is obtained when sodium alone is used as the reducing agent. The origin of the metallic silver which generally contaminates silver hyponitrite produced by the usual process is traced to the reduction Qf silver hyponitrite by the hydroxylamine acetate contain, adin the solution in which precipitation is effected.In order to avoid loss Gf hyponitrite -fromthis cause, it is recommended to add mercuric oxide to the alkaline solution resulting from the reduction, This destroys the hydroxylamine, and therefore the silver hyponitrite subsequently produced does not darken in the liquid. Although an aqueow solu-tion of sodium hyponitrite quickly Ciecornposes into sodium hydroxide and nitrous oxide, it was found that in the presence of much sodium hydroxide considerably less decomposition takes place. A strongly alkaline solution of sodium hyponitrite, prepared by reducing a strong solution of sodium nitrate, when spontaneously evaporated over sulph- uric acid in a vacuum during several wecks, deposit’ed crystals of sodium hyponitrite, which conld be freed from hydroxide by washing with alcohol, in which the hyponitrite is very sparingly soluble.The crystals may also be obtained by precipitating a strong aqueous solu-$ion of the salt prepared by the interaction of silver hyponitrite and sodium chloride with alcohol. A determination of the sodium in these crystals showed that they possessed the composition of sodium h y poni trit e . Ammonium hyponitrite was obtained in groups of long needles by decomposing silver hyponitrite with an alcoholic solution of am-monium sulphide and evaporating the filtered liquid over sulphuric acid in a vacuum.Like the sodium salt, this compound is difficult to obtain in any quantity, and this circumstance prevented the author from further investigating the properties of these hyponitrites. 71. "The interaction of hydrogen chloride and potassium chlorate." By W. H. Pendlebury, M.A.,and Mrs. McKUop. The authors have determined the amount of oxidising gases (whether chlorine or its oxides) removed on passing a given volume of air at a given rate through an aqueous solution of potassium chlorate and hydrogen chloride kept at a constant temperature, and have compared the amount removed with that present in the liquid. The evolved gases were received in a solution of potassium iodide, and at the end of each half hour the amount of iodine liberated was determined.The following results were obtained at 30"with a mixture contain- ing 30 grams of potassium chlorate and 18.823 grams of hydrogen chloride in 800 C.C. ; the half-hourly determination of iodine was not performed during 41+ hours, 5.5 hours after mixing. Hey? after Mass of iodine Hour! after Mass of iodine rmxing. liberated. mixing. liberated. 2 '0 0 -0021 47 -5 0 -0028 2.5 0 -0032 48 -0 0 '0025 3 '0 0 -0038 48 -5 0 '0022 3 -5 0-0035 68 '0 0 '0012 4-0 0-0034 69 *O 0 W15 4 '5 0*0028 69 *5 0 '0016 50 0 -0025 70 -0 0 -0015 5 '5 0 -0022 71 -5 0 9016 47 -0 0-0023 72 -0 0 *0015 In a second set of observations, twice the amount of hydrogen chloride was used (KC103 :4HC1).Hours.after Mass of iodine Hours.after Mass of iodine mixing. liberated. mixing. liberated. 0 -5 0 -012 35 -0 0 -042 1 -0 0 -01'7 4Q '0 0 -048 1 -5 0 -018 44-5 0 -045 2 '0 0 -022-45 -0 0-040 2*5 0 -026 45 -5 0-040 3 -0 0 -022 50 -0 0 '039 3-5 0 -024 53 a5 0 -0301 4-0 M-0 0-033 4.5 0 -028 0 -026 65 *O 0-03010 -026 5 '0 0 -029 65 *5 0 -032 5 '5 0 '024 66 -0 0.030 6.0 0,029 66 -5 0 -031 6 -5 0 -028-70 -0 0'032 1 24 0 -042 YO -0 0 -033J 212 100 ca. portions were withdrawn at regular intervals from a solu-tion of the same strength as that used in the second set of experiments kept at SOo, and the amount of iodine liberated thereby was ascer- tained. Hovr? after Iodine liberated. Hours after Iodine liberated.mixing.mixing. 1 0-0021 2p 0-0031 2 0 '0022 28 0*0036 3 0-0024 29 0-0036 4 070022 31 0-00411 5 0-0023 32 0 -0041 6 0'0024 46 0-0055 7 0-0029 47 0*ooa 8 0-0033 96 0-0045 22 0-0032 '77 0-0045 23 0-0031 94 0-0047 A comparison of the two sets of observations shows that only a portion of the orrii€ising gases is removed by the passage of the air. Observations are referred to showing that a solution such as was used in these experiments-which after exposure during 46 hours in subdued light-liberated iodine to the extent of 0.0055 gram per 10C.C. after exposure at a window to bright sunlight during 30 minutes liberated only 0.0038 gram per 10 C.C. ; after one hour's exposure the amount liberated had fallen to 0.0023, but no further reduction took place after 34 hours' exposure.On removal into subdued light, the iodine-liberating power increased, being 0.0035after four hours, and rising to 0*0048 after 20 hours in the dark. As solutions of the oxides of chlorine lose in oxidising power on exposure to light, the change observed in the chlorate solution is probably due to their destruction. 72. "The formation of indoxazen derivatives." By Wm. A. Bone, Ph.D. The author has investigated the behaviour of orthochloronitro-benzaldoxime towards alkalis with a view to isolating nitrindoxazen, CGH4<&>N.0 Orthochlorobenzal chloride was converted by the action of fuming sulphuric acid into the corresponding aldehyde, which was then nitrated, and the nitrated aldehyde was converted into the hydroxime ; on subjecting this to the action of caustic potash at 230°, ammonia was evolved, and hydrogen chloride was split off.On acidifying the solution, a, white precipitate was thrown down, which, after recrystal- lisation, melted at 222"; it possessed acid properties, and gave a red 213 coIour with ferric chloride solution. Analysis of the silver salt showed it to be 1 :2 :5-nitrosalicylic acid. The hydroxime was then heated at 120"with a solution af sodium carbonate ; hydrogen chloride was split off, but no ammonia was evolved. On acidifXing the liquid, beautiful yellow needles appeared, melting at 189". The properties of the product (especially the facts that it gave a red colour with ferric chloride, and on heating with caustic potash yielded 1:2 :5-nitrosalicylic) pointed to the conclusion that it was I :2 :5-nitrosalicylonitri1, isomeric with nitrindoxazen, a molecnlar change having occurred during the interaction.In order to decide the question, the hitherto unknown nitriles of 1:2 :5-nitrosalicylic acid were investigated. Several attempts mere unsuccessfully made to prepare these by well-known interactions; at last, by heating salicylaldoxime with acetic anhydride, and subsequently hydrolysing with dilute caustic potash, an almost quantitative yield of salicylo-nitril was obtained. On nitrating salicylonit14e with fuming nitric acid, the 1:2 :3 :5-clinitronitril was obtained crystallised in yeIlovi- plates, melting at 175" ; unlike other members of the salicylic series, it gave no colora-tion with ferric chloride.On using ordinary nitric acid, and conducting the nitration below O", the 1:2 :5-mononitronitril was obtained. This crystnllises in long, pale yellow needles melting at 190" ; it gave a red colora- tion with ferric chloride, and was found to be identical with the product obtained from orthochloronitrobenzsldoxime and sodium carbonate. Derivatives of these nitriles were prepared and studied, notably their amidoximeu. That of the mononitronitril is a weak base ; its hydrochloride crystallises in yellow tablets melting at 21 5O. That of $he dinitronitril is a neutral substance, crystallising in orange tablets melting at 204'. The author, finally, attempted to prepare nitromethylindoxazen.Indoxazen itself is evidently exceedingly unstable, but it was thought that it methyl derivative would be more stable, and it seemed likely that orthochloronitracetophenonoximewould yield nitromethylindox- men. The hitherto unknown orthochloracctophenone was prepared by the action of orthochlorobenzoyl chloride on ethylic acetosod-acetate, and subsequently hydroIysing the product. All attempts to prepare orthochloronitracetophenone from this failed, however, owing to the fact that nitration was accompanied by simultaneous oxidation. Orthochloracetophenone is a coloui-less oil which boils at 233-240'. 214 Orthochlorouitrace tophenone was prepared by the action of ortho-chloronitrobenzoyl chloride on ethylic acetosodacetate, and subse- quently hydrolysing the product.It is a very thick syrup, becoming crystalline on standing. The author was unsuccessful in preparing the hydroxime from this, although experiments were made under various conditions (at ordinary temperature, at 1-00’, and under pressure at 130”); in all cases the ketone was unaltered, owing, probably, to the very negative character of the C6H3(N0,)C1 group. 73. “The interaction of benzylamine and phenacyl bromide. Synthesisof piazine derivatives.” By Arthur T. Mason, Ph.D., and Goodlatte Winder, Ph.D. Phenacyl bromide and benzylamine easily interact, forming mono-phenncylbenzylamine, Ph*CO*C H3*NH*CH,*Ph, and diphenacyl benzyl- amine, (Ph*CO*CH,),N.CH,*Ph.These compounds were isolated in the form of hydrobromides, as on setting the bases free, molecular changes take place ; in the case of monophenacylbenzoylamine, 2 molecules combine to form I :4-di-benzyl-2 :5-diphenylpiazine dihydride, the *condensation being ana-logous to that which takes place in the case of isoamidoaceto-C,H,’NH*CH:C(OH)*C6R5 -2H,O + C?H,WCH:CCtjH5phenone : C6H,*C(OH):CH*NH*C,H, -C6H5C:CH0NC7H7 On heating the dihydride to the boiling point toluene is eliminated -Hc’N*c*C6Hsad 2 :5-diphenylpiazine, C6H5C,N,CH , is formed, the product, being identical with that from isoamidoacetophenone (Ber., 21, 1269). When diphenacylbenzylamine is set free it is probably con-verted into an oxazine derivative. Cold alcoholic ammonia converts the hydrobromide of diphenacylbenzylamine quantitatively into an amide, (C6H5*C(0n):CH),N*C7H7, which, at loo”, loses one molecule of water, 2 :6-diphenyl-4-benzylpiazinedihydride being formed, C6H5*C:CH HN< >N*C7H7.The same condensation occurs on warming the CsH,*C:CH amide with dilute chlorhydric acid, the hydrochloride of the di- hydride being formed. When further heated, the hydride, as well as its hydrochloride, yields 2 :6-diphenylpiazine, tolnenc or benzyl chloride, as the case may be, being eliminated. CH.N(C7H,)*CC&j-HC*N*CCsHs C.H-”H-CCC6Hs -HC*N*CC6H5-k c7Ht3* 213 Aniline a.nd benzjlamine act on diphenacylbenzylamine hydrobrom- ide forming the dihydride, CH.N(C6Ha).C,C6H5)CH*N(CiH,)*C*C,Hs and 1: 4-dibenxyl-2 : 6-diphenylpiazine dihydride.On heating the latter compound with concentrated chlorhydric acid at 170", two atoms of hydrogen are eliminated ; the product is devoid of basic properties and unaltered by benzoyl chloride and acetic anhydride, and is probably 2 :6-diphenyl-3 :5-dibenzylpiazine. If, however, 1: 4-dibenzyl-2 : 6-diphenylpiazine dihydride be heated alone at 260-270", toluene is eliminated, and the remaining benzyl radicle probably " wanders " from nitrogen to carbon, 2 :6-diphenyl-3-benzylpiazine being found. These transformations are comparable wihh those occurring when tohidine and xylidine are formed by heating the hpdrochlorides of monomethyl- and dimethyl-aniline. On treating the dihydride with an alcoholic solution of ferric chloyide and chlorhydric acid, it yields 2 :6-diphenyl-4-benzylpiazine dihydride. 74.''The interaction of quinones and metanitraniline and nitroparatolu- idine : a preliminary note." By James Leicester, Ph.D. Tho relationship between quinonedianilide and azophenine has been pointed out by 0. Fischer and E. Hepp (Bey., 1888, 683) who also prepared fluorindine from the latter compound (Ber., 1890, 2789). Tn a previous paper (Ber., 1890, 2793; this Journal, Abstracts, 1890, 1445) I gave the results of an investigation of the action of orth oni traniline and metani troparatoluidin e on quinone, toluquinone and nnpbthaquinone and showed that in principle the interact,ion mas the same as in, the case of aniline and quinone; for example, orthonitraniline and quinone combine to form quinonediortho-nitranilide, C,HzOz(NHC,H4N02)2[CO :NH = 1: 2 : 4 : 51, which on reduction with ammonium sulphide yields quinonehomoflnor- indine.In addition to the quinonefluorindines certain qninonephenazine derivatives mere obtained ; these are formed from the nitro-corn- pounds corresponding to quinoneanilide, quinoneorthonitrotoluide-yieldiag quinoneorthomethylphenazine. I have now prepared a number of other quinonephenazines and quinonefluorindines ; in fact the interaction appears to be a general one in the case of para-quinones. The constitution of these compounds may be inferred partly from the manner in which they are formed and partly from their similarity in properties to the corresponding fluorindines. A 216 number of crystalline compounds have also been obtained by the re- duction of the anilides and ioluides with magnesium : the prodncts are, however, of a somewhat complex nature and their further in- ves tigation is proceeding.Quinonedimetnnitranilide is prepared by heating a solution of quinone and metanitraniline in glacial acetic acid ; it crystallises from a mixturo of methyl alcohol and benzene, and melts at 295". Qninonemetanitranilide is obtained together with the dianilide as a bronze-coloured powder melting at 13%". Ho A-N-/\=N-Quinonemetahomoflnorindine, I I/\I , is formed()&I y-;-\/ by the reduction of the dianilide with ammonium sulphide; it is A brownish-black powder melting above 360".It affords a brown colonr with acetic acid, changing to slaty green, and finally to mauve, on the gradual addition of sulphuric acid. Qninoneparanitrotoluide is obtaineti in a similar manner as a bluish-black, crystalline powder ; on reduction with ammonium sulphide it yields a slate-coloured compound which decomposes at about 300". Quinonediparanitrotolnide is ,z bronze-coloured substamcc ; on re-duction it yields a substance which melts at 320"' and dissolves in alcohol, benzene or acetic acid forming a dark, greenish-yellow colonred liquid, exhibiting a green fluorescence. Thymoquindiorthonitranilide, from thymoquinone and orthonitr- aniline, crystallises from alcohol and ether in straw-coloured needles from it, forms grey needle8 melting at about 320'.Thimoquindiparanitrotoluide is depositec! from absolute alcohol in yellowish-red plates melticg at 112";it also crystallises in needles. Thymoquinorthomethylphenazine, C&,( C3E3[,)(Me) <:> CsH3Me, is a greyish white crystalline powder which sublimes at 325",and dissolves in acetic acid and ether, forming a yellow-coloured liquid. 75. I' Preparation of a-B-diphenylindolesfrom benzoin and primary benz-enoid amines." By R. Japp, F.R.S., and T.S. Murray, D.Sc. The authors have found that a mixture of benzoin, aniline and zinc chloride yields E. Fischer's a-/3-diphenylindole according to the equation 217 By employing in place of aniline, orthotoluidinc, paratoluidine, a-naphthylamine and P-naphthylamine, they obtained respectively a-P-diphenylorthotoluindole (m.p. 136"),a-P-diphenylparatolnindole (m. p. 153"), a-/3-diphenyl-a-naphthindole(m. p. 141') and a-P-diphenyl-p-naphthindole (m. p. 166"). Their work had proceeded thus far when a paper appeared by Bischler and Fireman (Bzr., 26, 1336), in which the preparation of these indoles (with the exception of a-f3-diphenyl-a-naphthindolej by a different method was described. This method consisted in first acting on cold desyl bromide with a primary benzenoid amine so as to obtain a desylanilide, thus, C6H,*CO0CH(NHC6H5)*C6H,, and then boiling this compound with an excess of amine, when, according to Bischler and Fireman, it is converted into an indole.The authors now show :-1. That the desylanilides described as new by Bischler and Fire- man are, in reality, identical with the anilbenzoin series obtained by Voigt (J.p~.Chem. [2], 34, 2) by heating benzoin with aniline, paratoluidine and /?-naphthylamine respectively. The constitution assigned to the compounds by Bischler and Fireman, which differs from that given by Voigt, is, however, correct. 2. That these desylanilides, contrary toothe statement of Rischler and Fireman, are not converted into indoles by boiling them with amines. In order that this transformation may occur, it is necessary that the hydrochloride or hydrobromide of the amine should also be present. The desylanilides used by these authors were, from the mode of preparation, doubtless contaminated with aniline hydro-bromide.3. That the foregoing indoles, with the exception of a-P-diphenyl-/J-naphthindole can be most readily obtained by boiling benzoin with a mixture of a primary benzenoid amine and its hydrochloride. a-/3-Diphenyl-P-naphthindoleis best prepared Lby the zinc chloride method. The authors also find that all these indoles when crystallised from acetone form definite compounds with I mol. of acetone (''qcetone of crystallisation '7. In the case of a-p-diphenyl-a-naphthindole,similar compounds with ethyl methyl ketone and diethyl ketone were prepared. 21s ADDITIONS TO THE LIBRARY. I. Donations. The Nature of Things: a Didactic Poem translated from %he Latin of Titus Lucretius Carus, by J.M. Good. (With Latin text.) 2 Vols. 4to. London 1805. From Hy. Bassett, Esq. The Chemistry of Wine, by G. J. Mulder; edited by H. Bence Jones. London 1857. From W. Whitaker, Esq. On Sewage Treatment and Disposal, by T. Wardle. Manchester and London 1893. From the Author. Practical Pocket-Book of Photography, by E. Vogel : translated, from 2nd German edition, by E. C. Conrad. London 1893. From the Translator. Smithsonian Miscellaneous Collections. Vol. XXXVI. A Select Bibliography of Chemistry, 1492-1892, by H. C. Bolton. Washing-ton 1892. From the Institution. Rudiments of Chemistry, by Temple Orme. Second edition. Washington 1893. From the Author. Imperial Institute Series. Handbooks of Commercial Products. Indian Section :-No.2. Ipecacuanha, Calcutta 1892. No. 3. Podophyllum emodi. Calcutta 1892. No. 7. Resin and Turpentine from Indian Pines. Calcutta 1893. No. 8. Iron : Southern Districts, Madras Presidency. Cal-cutta 1892. No, 9. Indian Coal. Calcutta 1893. No. 10. Adhatoda vasica. Calcutta 1892. No. 11. Linseed. Calcutta 1893. No. 13. Cutch. Calcutta 1893. No. 14. Kut (The Costus). Calcutta 1893. No. 15. Turpeth, or Indian Jalap. Calcutta 1893. No. 16. Kamala Dye. Calcutta 1893. No. 18. Jalap. Calcutta 1893. No. 20. Castor Oil. Calcutta 1893. From the Imperial Institute. A Manual of Mineralogy, by R. Allan. Edinburgh 1834. A Translation of the Pharmacopoeia of the Royal College of Physi-cians of London, 1836, by It. Phillips.Fourth edition. London 1811. 219 The London Dispensntory, by A. T. Thomson. London 1815. Chemical Experiments, by G. Francis. Third edition. London 1845. A System of Chemistry, 4to. Philadelphia 1791. AnIntroduction to Practical Chemistry, by J. E. Bowman. 4th edition, edited by C. L. Bloxam. London 1861. Instructions for the use of the Blow-Pipe and Chemical Tests, with additions and observations derived from the recent publications of Professor Berzelins, by J. Mawe. Fourth edition. London 1825. From -Hart, Esq. Experiment e mit Stromen hoher Wechselzahl nnd Frequenz, zusammengestellt von E. de Fodor, revidirt und mit Anmerkungen verschen -ion N. Tesla. n’ien, Pest, Leipzig 2893. From the Publishers. 11. By Purchase.Handbuch der anorganischen Chemie, heransgegeben von 0. Dam-mer. Band 111. Stuttgart 1893. Zusammensetzung und Verdaulichkeit der Futtermittel; nach verhandenen Analysen und Untersuchungeii, zusammengestellt von T. Dietrich und J. Ronig. Zweite Auflage. 2 Bande. Berlin 1891. Kurzes Lehrbuch der organisclien Chemie, von A. Bernthsen. Vierte Auflage, bearbeitet unter Mitwirkung vor E. Buchner. Braun-schweig 1893. Hand- und Hilfsbuch zur Ausfiihrung Physikochemischer Nes-sungen, von W. Ostwald. Leipzig 1893. The Metallurgy of Lead and the Desilverization of Base Bullion by H. 0. Hofman. Second edition. New York 1893. RESEARCH FUND. A meeting of the Research Fund Committee Rill be held in December. Pellowa desiring grants are requested to make applica- tion before December 9th.At the next meeting on November 16tl1, the following papers will be read :-“ The normal butylic, heptylic and octylic salts of active glyceric acid.” By Professor Percy Frankland, F.R.S., and John MacGregor, M.A. 220 “The ethereal salts of diacetylglyceric acid in their relation to optical activity.” By Professor Percy Frankland, F.R.S., and John NacGregor, M.A. ‘‘The oxidation of paratoluidine.” By A. G. Green.(‘The products of the action of benzoyl chloride on urine in the presence of alkali,” By Dr. J. W. L. Thudichuni. CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.B.-The names of those who sign from “ General Knowledge’’ are printed in italics. The following Candidates will be balloted for on 7th December, 1893 :-Bowman, Frederic Edmund, Ash Leigh, Bowdon, Cheshire, Analytical Chemist.Was educated at Rugby, and afterward8 studied under Professor Smithells, at the Yorkshire College, heeds. Has passed his intermediate examination for B.Sc. in Chemistry. At present has charge of one of the laboratories at Messrs. Bowman, Thompson, and Co., Ld., Northwich. Fredc. H. Bowman. J. Carter Bell. Thomas Wardle. John Knowles. R. Grimshaw. Watson Smith. George H. Hurst. Arthur H. Tuer. Percy Carter Fell. Briggs, Harry Fielden, Roseneath, Torquay. Dactor of Dental Surgery ; D.D.S. TJniversity College, Mich. ; L.D.S. Faculty of Physicians and Surgeons, Glasgow; D.Sc. and B.Sc. Univ. Ohio.First Class Queen’s Prizeman in Theoretical and Practical Chemistry. Edward Smith. Jno. Wiltshire. George Cheverton. Arthur Turner. Walter H. Co$in. R.L. Taylor. Browne, Frank, Government Civil Hospital, Hong Kong. Assistant Apothecary and Assistant Analyst in the Government Civil Hospital, Hong Kong. Studied Chemistry and Practical Chemistry during one year in the School of Pharmacy of the Pharma- ceutical Society ; mas a Medallist in Chemistry. Subsequently worked 222 one year in the Research Laboratory of the Pharmaceutical Society. For the last 3&years have been Assistant Demonstrator of Practical Chemistry in the laboratories of the Pharmaceutical Socicty. Wyndham R. Dunstan. John Attfield. M. Carteighe. Thos. S.Dymond. Chap. M. Luxmoore. Brunton, John Dixon, Wire Mill, Musselburgh. Metallurgical Student. First Class Honours in Metallurgy, Assoc. S.T.S. after three years’ course at the Sheffield Technical School, including Analytical Chemistry, Mathematics, Physics, and Metal, lurgy. J. 0. Arnold. Fredk. J. Merrils. B. W. Winder. G. T. W. Newsholme. $no. C. Platts. Caines, Charles March, 11, Clockhouse Road, Beckenham, Kent. Analytical Chemist. First Class Honours Certificate in Chemistry, South Kensington Science and Art Department,. Four Sears’ expe- rience in AnalFtical Chemistry under Mr. Alfred H. Allen. Alfred H. Allen. A. Wynter Blyth. Otto Hehner. C. G. Moor. J. Kear Colwell. B. E. R. Newlands. John A. IZ. Newlands. Carswell, ThomasPetson, 369, Scotswood Road, Newcastle-on-Tyne, Analyst and Teacher at Newcastle Chemicil and Pharmaceutical Tutorial.Pharmaceutical Chemist and Memb. Pharm. SOC. Author of Papers “ On the Volumetric Estimation of Phenols by Iodine,” Pharmaceutical Conference, 1892 ; “ On a New Class of Iodine Phenol Derivatives,” Chena. News (to appear immediately in series) ; ‘‘ On Animal Charcoal,” Phamn. J., 28th January, 1893. Analyst to Borough Analyst of Bradford during summer vacancies, 1892 and 1893. Alex Crum Brown. F. M. R>immington.P.W. Richardson. Tlios. Xaberc. W. A. H. Naylo?.. Chaney, Harry J., 29: Chalcot Crescent, Regent’s Park, London. Metallurgist. Associate of the Royal School of Mines. Studied Chemistry under Professor E.Frankland, F.R.S., and Metallurgr under Professor Roberts-Austen, F.H.S., Chemist to the Mint. 223 Work carried on includes :-1. Chemistry of the various methods and products of Carbonization. 2. The Chemistry and economic application of the various lixiviation processes, more especially the Russell and allied processes. 3. The nature of the Gold Quartz deposits of the Rolad Gold Fields, India, and experimental work of all kinds in connection with Paw and Stamps Amalgamation (1889-1893). All private work. E. Frankland. W. R. Eaton Hodgkinson. G. Matthey. David Watson. W. C. Roberts-Ansten. Percy F. Franklaud. Cocking, Allan Thomas, 39, Lister Street, Rotherham. General Manager of Kynoch's Explosives and Ammu iiition Works. Three years Chemist and Works Manager, Flameless Explosives Works.Four years Chemist and Manager, Chemical Works at Ald- worke Colliery for treating products from coke ovens. Eight years Teacher of Chemistry, Rotherham School of Science and Art. Three years Lecturer on Chemistry, Rotherham College. TV Cnrleton Williams. L. T.O'Shea. George Young. J. 0. Arnold. Ralph E. Brown. Craw, John A., 2, Millgate, Cupar-Fife. Science Master, Bell-13a8xter Institute, Cupar-Fife ; also Lecturer on Chemistry, Cupar Burgh School of Science, Glasgow and West of Scotland Technical, College. Student 1886-1891. Analytical Chemist and Assayer at Parkhend Steel Works for two years. As-sistant Science Master, Harris Academy, Dundee. South Kensington Certificates in Honours, Chezistry ; Cit,y and Guilds of London in Honours, Iron and Steel Manufacture.A. Humboldt Sexton. Geo. Ritchie. Thos. A. Cheetham. Horatio Rallnntyne. ,James Robson. Ellis, Charles Sordes, 17, Bloomsbury Square, W.C. A ssistant Demonstrator of Chemistry at the Pharmaceutical Society. Late Student in the Laboratories of Owens College, Manchester, and University College, Aberystwith, Assist,ant to J. H. Lester, M.Sc., Consulting Chemist, Manchester. Harold B. Dixon. G. H. Bailey. H. Lloyd Snape. W. H. Perkin, jun. Gilbert J. Fowler. John Attfield. Harry Grimsh au-. Howard 0.#acre'. 224 Forrester, Alexander M. 22, Scotia Street, Glasgow. Technical Chemist. For over four years assistant to Mr.J. Falconer King, City Analyst of Edinburgh ; studied under Professor W. H. Perkin, jun., at Heriot-Watt College, Edinburgh ; at present Head ChemiBt with Messrs. Alex Cross and Sons, Port Dundas Chemical Works, Glasgow. J. Falconer King. John Hunter. w. H. Perkin, jun. F. Stanley Kipping James Stenhouse. W. S. Curphey. Garnett, Henry, 2, Bartholomew Villas, Kentish Town, N.W. Chemist and Analyst to the Vinolia Soap Works, Kentish Town, London. Studied Chemistry and Practical Chemistry as Bell Scholar, at the School of the Pharmaceutical Society, 1890-1891. Passed the Major Examination of the Society, 1891. Silver Medallist in Chemistry and in Practical chemistry. Percira Medallist, 1891. Afterwards worked in the Research Laboratory of the Ph,zrmnceutical Society, 1891-92, and during a part of 1893.Wyndham R. Dnnstan. John Attiield. Thomas S. Dymond. M. Carteighe. Gilbert J. Fowler. mas. P. ~i~~~t. Grieve, William Hotten, 226, Friern Road, East Dulwich, S.H. Science Demonstrator, London School Board, and Science Lecturer, Surrey County Council. Author of three works upon Mechanics. Nine years Science Demonstrator, L.S.B. Four years Lecturer upon Natural Philosophy, St. Edward’s College, Liverpool. Six years Firsk Mathematical Master, Wesley Collage, SheEeld. J. H. Gladstone. Geo. Chatloner. Harry R. Redmnn. Isaac S. Scarf. J. Howard. H. Macan. TVillinin J. I3uhhrr. Hadley, Harry Edwin, The School of Science, Kidderminster. Head-Master of Science School.Assistant Demonstrator of Physics in the Royal College of Science for one year. Demonstrator and Assistant Lecturer in Physics in the Owens College for three years. B.Sc. (Lond.) 1898. Associate of Royal College of Science. Harold B. Dixon. P. J. Hartog. Arthur Harden. Arthur W. Crossley. Gilbert J. Fowler. Gibson Dyson. 225 Hale, Henry Ormsby, Oundle School, Northamptonshire. Bachelor of Arts of Trinity College, Cambridge. Natnral Sciences Tripos, Part I, 1889. Chemistry Master, Oundle School. T. H. Easterfield. Sidney Skinner. W. J. Sell. J. T. Hewett. S. Ruhemann. Harris, Harold, Denmapk House, Toffley Avenue, Gloucester. Metallurgical Chemist. Student at Mason College during three Sessions ; passed the Senior Examinations in Theoretical and Prac- tical Metallurgy. Studied the Analysis of Explosives at Nobel’s Xxplosives Co., Glasgow. Have actcd as Engineer to Gold Mine on the Gold Coast, and as Metallurgical Chemist at Gold and Copper Mines in Bengal.Also analysed Nobel’s Explosives in India. Joint Author, with Mr. Turner, of Paper on “The Native Manufacture of Iron in India ” (Iron and Steel Institute, September, 1893). Author df Paper in course of publication, on “ The Copper Mines of Singh-boru, Bengal.” Thomas Turner. William A. Tilden. W. W. J. Nicol. Sidney Williamson. George Embrey. J. M. Collett. Hesketh, Wm., B.A., School House, Eerriscowles, Blackburn. Science Teacher. Lecturer in Chemistry to Lancashire C.C. B.A. Royal University of Ireland.Lecturer in Agricultural Chemistry to Norfolk County Council, 1881. Student in the Chemical Laboratories, Owens College, 1892, 1893. Harold B. Dixon, G. H, Bailey. Arthur Harden. W. H. Perkin, jun. Gilbert J. Fowler. Holthouse, Harold B., 42,St. Ann’s Valley, Nottingham. Senior Assistant in the Pharmaceutical Laboratory of Boot’s Pure Drug Company, Nottinghem. Have been engaged in the Manufac- ture of Pharmaceutical Preparations and Chemicals for the last 15 years, during five of which studied under John 8.Linford, F.Z.C. Also studied Theoretical and Practical Chemistry four years at the University College, Nottingham, and have been working at Analytical Chemistry generally, but more especially as applied to the examina- tion, testing, and standardising of Drugs, Chemicale, and Galenicals. Frank Clowes.J. Bernard Coleman, R. Lloyd Whiteley. Frank I’.Addyman. Edgar B. Truman. 226 Hughson, Alexander Sinclair, 12, Myrhle Crescent, South Shields. Chemist. I have been a student of Chemistry and Physics seven years, and have passed the examinations of the Pharmaceutical Society of Great Britain, and of the South Kensington Science and Art Classes. A. B. Griffiths. Hayold Follows. Alexander Hay. Thomas A. Pooley. E. C. Conrad. Hunt, Bertram, F.I.C., 5, Queen’s Crescent, Glasgow. Analytical Chemist. (1) “ Researches on Chemical Equivalence. 11, Nickelous and Cadmic Sulphates,” by E. J. Mills, D.Sc., F.R.S. and Bertram Hunt. (2) “ Estimation of Tannin,” and “ Note on the Destruction of Tannin by Boiling Solutions of Gambier,” by Bertram Hunt (J.Xoc.Chenz. Id.,4, 263). Edmund J. Mills. Richd, Reynolds. Fredk. Woodward Brown. Arthur Smithells. J. Lewkowitsch, Wm. McD. Mackey. Ladell, Richard Savory, 155, Praed Street, Hyde Park, London, W. Chemist. I have been a student of Chemistry and Physics for the past 13 years, and bave passed the examinations of the Pharmaceu- tical Society and Apothecaries’ Hall. A. B. Griffiths. H. Pollowa. Alexander Hay. Lionel Cooper. Alfred H. Allen. Thomas A. Pooley. C. T.Kingzett. E. Fightman Bell, Mawer, William Fred, 16, Fentiman Road, S.W. Chemical Demonstrator. Isanundergraddieof London University. Studied Chemistry for three years and passed the Minor and Major Examinations of the Pharmaceutical Society. Subsequently gave up the practice of Pharmacy, and has been for the last three years Assistant in the South London Public Laboratory.John Watts. W. Henry Dodd. L. de Koningh. S. I?. Burford. Lewis Ozcgh. George T.Holloway. J. West Knights. 227 Mor@Il, J. R., Leydenburgh, Port Hall Street, Brighton. Science Master at the Grammar School, Brighton. Three years Student at University College, Aberystwyth, under the late Professor J. S. Humpidge. Three years Student at University College, Cardiff, under Professor Thompson and Dr. Turpin. Passed 1st B.Sc., London University with Honours, and Final B.So. with 2nd Class (3rd place) Honours in Chemistry. Have now taken Chemistry up it8 a Profession.R.E. Hughes. G. S. Turpin. Claude I&. Thompson. E. P. Perman. J. Tudor Cundall. Morton,Frederick, 101, Quarmby Road, Huddersfield. Manufacturing Chemist and Tar Distiller. Studied' Chemisti-y at Huddersfield Technical School and Bradford Technical College nnder Mr. C. Rawson, and Porkshire College, Leeds, under Professor Smithells. Honours, Practical Chemistry, 1892. Had experience in Chemical and Tar Works of J. and E. Morton, Milnsbridge, Hudders- field, and am still in that position as Head Chemist and Tar Dis-tiller. Arthur Smithells. Herbert Ingle. J. B. Cohen. C. Rawson. H. Ellison. Payne, George F., M.D.Ph.,G., Atlanta, Georgia, U.S.A. Analyst, and as stated below. State Chemist of Georgia. Analyst of Agricultural Department.Member of Georgia Board of Pharmacy. Pharmaceutical Examiner. Professor of Materia Medica and Toxi- cology, Atlanta College of Pharmacy. Special Chcmicsl training in Columbia College School of Mines, New York City, U.S.A., 1873 and 1874. Graduated New York College of Pharmacy. Graduated Atlanta Medical College. Life Member Georgia Pharmaceutica 1 Association. Life Member Georgia State Agricultural Society. Member of the ''Association of Official Agricultural Chemists " of the United States. Elwyn Waller. Hermann T. VultB. C. I!'. Chandler. Arthur H. Elliott. Albeyt B.Prescott. Rawlins, Thomas Beilby, 2, Leven Street, Pollokshields, Glasgow. Chemist and Colour Manufacturer. 1st Class Honours Science and Art Exams.1883 or 1884. Teacher (Chemistry) Leeds Mechanics Institute 1883 and 1884. Chemist and Manager of Colour Works. Investigations on the Protection from Corrosion of Iron and Steel Structures. Edward Rawlins. Herbert Eccles. John Wm. Biggart. E. G. McBretney. Edward M. Chap&. Arthur W. Cooke. Rees, George Eercival, Ely House, Basford, Stoke-on-Trent. Assistant Blast Furnace Idanager and Analytical Chemist. Six yeacs’ experience as Metallurgical Chemist. Science and Art Depart-ment’s Certificates in Honours (lst), Inorganic (Practical), and in Advanced Organic (Theoretical and Practical), and Organic Honours, 1st Class (Practical). H. N.Brothers. Harry Silvester. Herbert Pi1kington. J. E. Stead. Xydney J.Harris. Reid, ThomasAnderson, Lostock Gralam, Northwich. Manager of Chemical Works. 15 years’ experience in Theoretical, Practical, and Manufacturing Chemistry. Special experience in the Mannfactnre of Pulp from Wood. Prize Essayist on this subject at International Forestry Exhibition, Edinburgh, 18%. Engaged during last 8 years in the development and working of the Ammonia Soda Process. At present entire charge of Chemical Department of Bowman, Thompson, and Co.’s, Limited, ammonia soda factory. Fredc. H. Bowman. John Knowles. Francis Henry Tate. J. Carter Bell. H. Grimshaw. George H. Hurst. Arthur H. Tuer. Percy Carter Bell. Santer, Herbert, Albion Brewery, Caledonian Road, N. Brewer. I have studied Chemistry for some time in the laboratory of Messrs. Gillman and Spencer, and am still continuing.I am also engaged in my own laboratory at brewery, and take a great interest in Chemistry as applied to Brewing. Alex. W. Gillman. Sam. Spencer. F. Jewon. J. Farrow Ballard. W. H. Blake. Schidrowitz, Philip, 102, Oxford Gardens, Notting Hill, W. Research Chemist (from October, 1893) to Queensferry Tar Works, Chester. Certificate of Technical Chemical School, Zurich (Federal 229 Polytcchnic) ; here stadied under Professors Lunge, Hantzsch, &c.) Degree of Ph.D. University of Bern. Publisbed Dissertation ‘‘ Beitrage zur Kenntniss der Xanthongruppe,” Bern, 1893, K. Wys about “ o-Dixanthon ” (Jouwaal of Germn?z ChemicaZ Society, 93,i, 75) ; at Bern studied under v.Kostanecki, &c. W. F. Loye, Temple Omnie. John Bairstow. WilZianl*Ramsny. -By. Forstes. 2110rl~y. Sims, W. Edgar, B.Sc. (Vict.), Stafford House, Longsight, Manchester. Late Student of the Owens College-no occupation at present. For three years Student in the Chemical Laboratories, Owens College. B.Sc. (1st class Honours in Chemistry) Victoria University. Mercer Scholar ; Le Blanc Medallist ; Dalton Prizeman. Joint Author of paper on “ Thionyl Bromido ” (Proc. Chern. Xoc.). G. H. Bailey. Arthur W. Crossley. Francis Jones. W. H. Perkin, jun. Harold €3. Dixon. Arthur Harden. Gilbert J. Fowler. P. J. Hartog. Shapley, Frederick, Whittier, Fuller & Co., San Francisco. Paint and CoIour Chemist, Learnt business under W.Urqiihart, London, W. Afterwards Chemist and Superintendent to the English Enamel Paint Company, New York. Then Chemist and Superin- tendent of Binswanger and Pollock’s Colour Factory, Philadelphia, Pa. Then Chemist and Superintendent of the Wieder Paint Com-pany’s Factory, St. Louis. And at present with Whittier, Fuller and Company, Snn Francisco; and also doing original work in A. A. Cunningham’s Laboratory, San Francisco. A. Auchie Cunningham. Arthur 3’. Price. Thos. W. Salter. Stevensow Macadam. W. Ivison Macadam. ‘Z’honaasA. Pooley. A. B. Grifiths. Spencer, Frederic, Rose Villa, Uttoxeter, Staffs. Chemist. I have passed the Examinations of the Pharmaceutical Society of Great Britain, &c. Lionel Cooper. A. B. Grifiths.Harold Follows. James D.Johnsfone. E.C‘. Conrad. Styles, Robert Curling, Knockh all, Greenhi the, Kent. At present eugaged installing Professor Roberts-Austen’s Recording Pyrometer in Ironworks. I have acted as Assistant to the late Dr. A. J. Bernays, at St. Thomas’s Hospital, correcting proofs of his last book. Studied three years at the Royal College of Science, and have obtained the Associateship in Metallurgy. Student of Inst. Chem. W. C. Roberts-Austen. T.K. Rose. Henry C. Jenkins. F. W. Bayly. Edwin J. Ball. Thorpe, Jocelyn Field, Gloucester House, 20, Larkhall Rise, Clapham. Chemist. Has passed through the Chemistry and Physics courses at the Royal College of Science. Has also studied Chemistry and Physics at King’s College, London.T. E. Thorpe. W. Palmer Wynne. John M. Thomson. G. Stillingfleet Johnson. Herbert Jackson. Wm. Tate. Walden, William Herbert, 55, Clapham Road, S.W. Chemical Expert in H.M. War Department. For 3 years engaged in Chemical Research and Practical Analysis in the Laboratory of John Woodland, Esq., F.C.S., P.L.S., &c., and still engaged in original research. 9.B. Griffiths. E. C. Conrad. Lionel Cooper. Harold Follows. E.Wightmart Be11. Richard Weacer. Thomas A.PooZey. William Crookes. Chas. A.MacMunm. Alfred H. Allen. Welchman, Frank Ernest, 16, Cai-lton Road, Putney Hill, S.W. Assistant to Dr. Hake, Westminster Hospital Medical SchooI, Caxton Street, S.W. Educated at Queenwood College, Hants (1881-86). Matriculated, London University, June, 1889.Student of the Institute of Chemistry. Pupil during 4 years in the laboratory of Dr. Hake, Westminster Hospital Medical fichool. At present assisting Dr. Hake, A. Duprk. H. Wilson Hake. Wm. Macnab. H, Sprengel. Charles E. Groves. White, William Gilchrist, Lamb Roe, Whalley, Lancashire. Print Works Chemist at Whalley Abbey Print Works (Messrs. Bryce, Smith, & Co.). I have been for the past 3 years Practical Chemist at the above Works, with 4 years’ previous training in Chemistry and the allied sciences (2 years) at the Glasgow Technical 231 College, and the following 2 years with the late Professor Dittmar. where I obtained 1st Class Certificates in the subjects I studied. Imve studied Practical Photography and its Chemistry for severad years, and have done a, little Research on the subject as a Student (see Andersonian Cham.JournaZ, November, 1889, and March, lS90), which I am at present engaged following up. Alfred M. Hanson. G. G. Henderson. James Robson. Thomas Gray. James G. Hardy. Alexander Lander. M. W. Jones. A. Humboldt Sexton. Fred Marsden. Winder, Edward Humphreys, 37, Vincent Square, London, S.W. Science Master, Westminster School. B.A. (Oxon.) : former Ex-hibitioner in Natural Science at New College, Oxford : and worked for 4 years in the University Laboratories (Chemical). John Watts. W. W. Fisher. Wm. Odling. V. H. Veley. H. Brereton Baker, Wyndham, Stanley, Ph.D., Judson, Florida, c/o Trenton Phosphor Co. Analytical Chemist.Two years’ course at Polytechnicurn, Hanover. Five years’ course at University of Freibnrg, Baden ; graduat@ed (Ph.D) in 1887; subject of original research : Thesis “Beitrage zur Kenntniss der Isophtalsiinre.” 1887-93 engaged as Analytical Chemist in America. Boverton Redwood. Thomas Tyrer. John A. R. Newlands. Bernard Dyer. B. E. R. Newlands. HARRISON AND SONS, PRINTEBS XNORDJNABY TO HER MAJESTY,ST. MABTIN’S LAXK
ISSN:0369-8718
DOI:10.1039/PL8930900199
出版商:RSC
年代:1893
数据来源: RSC
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