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Proceedings of the Chemical Society, Vol. 11, No. 155 |
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Proceedings of the Chemical Society, London,
Volume 11,
Issue 155,
1895,
Page 159-198
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摘要:
PROCEEDINGS OF THE CHEMICAL SOCIETY. EDITED BY THE SECRETARIES. No. 155. Session 1895-96. The following are the abstracts of papers received during the vacation, and published in the Transactions :-104. I' Homonucleal tri-derivatives of naphthalene." By Raphael Meldola F.R.B., and Frederick William Streatfeild. Dibromonitronaphthalene, C,,H,Br*NO,.Br (1 : 2 : 4), m. p. 117", has been prepared by the authors and submitted to further study. The corresponding dibromo-/3-naphthjlamine consists of white, silky needles melting at 106-107"; the acetyl derivative melts at 220--'221". When this dibromo-/3-naphthyla.mine is diazotised in the presence or" an excess of mineral acid and the diazo-salt solution boiled with water, the NH2-groupis not replaced by hydroxyl, as in the normal Griess reaction, but bromine is displaced, and a diazoxide formed in accordance with the scheme The diazoxide has the constitution b : N2: Br = 1: 2 : 4.It con-sists of ochreous needles, soluble in boiling water, and decomposing at 146-151". It is reduced by tin and hydrochloric acid to p-amido-a-naphthol, and bromine and glacial acetic acid converts it into dibromo-a-naphthaquinone, ni. p. 216". Chlorobromo-/3-naphthylamine, CloH5Cl*NH2*Br(1 : 2 : 4), wag ob-tained in the form of white, silky needles melting at 102-103" ; the acetyl derivative at 218O, the benzoyl derivative at 185-186O. By nitrous acid this chlorobromo-/3-naphthylamine is converted into the diazoxide, above described, in the presence of excess of mineral acid ; in its abseuce the diazoamide, CloHjC1Br*N?*NH*CloH~C1Br,is formed.160 This compound is very stable for a diazoamido-compound, and crys- tallises from toluene in yellowish needles melting at 205-210", with decomposition. The authors also show that iodine chloride is an ex- cellent reagent for preparing iodine derivatives of the acetnsphthalides, both a: and p. They give the melting points of the following com- pounds :-C,,H,I.NHAc (4 : l), 197"; CloHa*NOz*I*NHAc(2 :4 :1) ; CloH5.N02*I*OH(2 :4 : l), 150"(shrinking at 147') ;C,,H5*N02.1*OC2H, (2 : 4), 104--105". The potassium salt of the nitroiodonaphthol has also been prepared and analysed. 105. '' The ethereal salts of the optically active lactic, chloropropionic, and bromopropionic acids." By J.Wallace Walker, M.A. The methylic, etbylic, and propylic etherea,l salts of active lactic acid were prepared by the action of the alkyl iodides on the an-hydrous silver 'salt. From the ethereal lactates the corresponding bromopropionic salts were prepared by the action of phosphorus penta- bromide. For both series of salts there is a, constant difference in rotatory power, in the first case of 5.5", in the second of 14*2O, between two adjacent members. The ethereal chloropropionates were prepared by the action of phosphorus pentachloride on lactic acid. These bodies possess a high degree of optical activity, and the values given in this paper are much higher than those found by Le Bel, Walden, and Frankland and Henderson for such of the substances as they have examined.The observed results do not agree with Guye's hypothesis. 106. "Some new azo-compounds." By Charles Mills. By the action of nitrosobenzene on aniline dissolved in acetic acid azobenzene is produced (Baeyer, Ber., 7, 1638). The author has extended this reaction, and has prepared the following siibstances :--m-AcetyZarnidoaxobenxene, m. p. 130-131" C. On hydrolysis wirh caustic soda it gives m-amidoazobenzene, crystallising from light petroleum spirit in long, silky, orange needles, m. p. 56--57°C. Readily soluble in alcohol, acetic acid, ethyl acetate, acetone, chloro- form, benzene and ether. c6H,*N2*C6*H4*~,*c6H~,dipradiphenyz-disazophenylene, prepared by the action of nitrosobenzene on p-amido-azobenzene.p-Benzeneazotoluene formed by the action of nitrosobenzene on p-toluidine, also by the action of p-nitrosotoluene on aniline. The following compounds are also described :--p-Benzeneazotolzcenesui$hoi& chloride. p-Benzeneazo-o-acettoluide, C6H3*CH3*NHAc*N:N.C6H6(1 :2 :4). m-Arnido-p-benzeneazotoluene. C6H4*NHAc,CH3*N:N*C6H6neizsene-o-nzo-o-acettoluide, (1:2 :3). m-Amidobenzene-o-azotoluene, C6H4*NH2*CH3*Nz*C6H5(1 :2 :3). 107. “Some derivatives of Maclurin.” By C. S. Bedford, and A. G. Perkin. When an aqueous extract of old fustic (MOTUStinctoria) is treated with a solution of diazobenzene sulphate, a colouring matter is pro-duced. The chief constituents of old fustic are, morin, ClJ31007, and maclurin, C,,H,,O,, only the latter reacts readily with diazo-benzene.Benzeneazomaclurin, cl3H,o6(CJ&,*NZ)z,0-and p-toluene- nzomaclurin, p-nitrobenzeneazomaclurin, and maclurinazobenzene-p- sulphonate of sodium have also been prepared. These substances dye wool and silk orange-coloured to deep brown shades. Maclurin, by tthe‘ action of reducing agents, yields phloroglucin and proto- catechuic acid, and is considered to be a pentahydroxybenzophenone? C,H,( OH),*CO*C6H2*(OH),. Phloroglucin combines with ‘2 mol. props. of diazobenzene, while no reaction t,akes place between this latter and protocatechuic acid. The constitution of benzeneazomaclurin should therefore be thus represented, OH C6H3(OH)?*co/\N:N*C,& OH(.!,,, C685.R:N 108. “ The constituents of ‘Artocarpus integrifolia,‘ ” By A.G.Perkin and F.Cope. Artocarpus integr(foZia is the well known Jack Fruit, cultivated in India, Burmah, and Ceylon, It is much esteemed for carpentry, and is used in conjunction with alum as a yellow dye. It contaiiis a yellow colouring matter of the formula, C15H,,O7, identical with morilz, and a substance of the formula C&1$&, to which the name cyanomachrin has been given. With diazobenzene it yields a corn-pound, C,5H,006(C)6H6N2)2,crystalljsing in scarlet needles, which dyes unmordanted wool and silk orange to orange-red shades, but which does not dye with mordants. When boiled with dilute acids, cyanomaclurin yields red-brown products, resembling in character the so-called “ anhydrides ” of catechin, which can be produced from this latter substance in a similar may.That first formed dissolves in hot water and dilute alkalis, but by longer treatment becomes more sparingly soluble, and the final product obtained is insoluble in dilute alkalis and the usual solvents. No glucose is produced during- this reaction, so that cyanomaclurin is not a glucoside. The study of this substance will be continued. 162 189. ‘‘ Optically active methoxy- and propoxy-succinic acids.” By T, Purdie, F.R.S., and H.W.Bolam, B.Sc. The authors have resolved inactive methoxy- and propoxy-succinic acids into their active components, the cinchonine and strychnine salts being made use of in the case of methoxysnccinic acid, the strychnine salts in the case of the propoxysuccinic acid.Rotations of the acids in water and different organic solvents are given, with the rotations of salts of both acids in aqueous solution. 110. “ Ethereal salts of active methoxy- and ethoxysuccinic acids.” By T. Purdie, F.R.S., and S. Williamson, Ph.D. Inactive methoxp- and ethoxy-succinic acids were resolved into their active components by means of their strychnine salts. Obser-vations on the activity of the various strychnine salts in aqueous solu-tion were made, and results obtained in accordance with the law of Oudemans. Methyl-, ethyl-, propyl-, and butyl-, rnethoxy- and ethoxy-succi- cates, and the isopropyl and isobutyl salts of ethoxysuccinic acid, were prepared by the action of their respective iodides upon the silver salts of the acids, and their rotations observed. The specific rotations of the active acids in water and various organic solrents were also taken.A discussion of the results obtained is contained in the paper. 111. (‘Note on the production of potassium platinichloride.” ByE. Sonstadt. Dry potassium platinichloride, when heated with mcrcury, is decomposed according to the proportion of mercury used. (1.) 2KC1,PtClp + 4Hg = 2KC1 + Pt + 4HgC1. (2.) 3KCI,PtCI, + 2Hg = 2KC1 + Pt + 2HgC1,. The decomposition begins even below 100’ C., and is complete at a lower temperature than is required to expel from the containing vessel the mercurous or mercuric chloride produced.In treating small quantities of the platinichloride, the mercury is placed in a porcelain crucible, and covered with platinichloride, in the proportion of about two parts of mercury to one of salt. Heat is applied very gently, to avoid loss through boiling, till the raaction is complete, when the heat is raised to expel the mercurous chloride. When larger quantities are decomposed, the salt is preferably tritxrated with the mercury, and gently heated, so as to avoid a too sudden or Fiolent reaction. ADDITIONALNOTE; BY Ar; rHoIt.-Dry silver chloride is not clecom- 163 posed by mercury, even at a red heat ; nor when mixed or combined with a platinum salt. 112. ‘I Orthobenzoic sulphinide.” By William J. Pope. The author finds that pure orthobenzoic sulphinide in large well- defined crystals may be obtained from t,he commercial mixture known as “ saccharill ” by crystallisation from acetone.Crystallographical measurements are given. 113. ” Derivatives of P-resorcylic acid.” By A. G,Perkin. The principal product of the action of methylic iodide up011 P-resorcylic acid is a substance crystallising in needles melting :it 76-77’, and having the constitution C6H2.Me(O~~e)*OH*C00~fe. It appears probable that the hydroxyl group in &resorcylic acid, which resists methylation, is in the o-position to the carboxyl group. The principal product of the action of ethylic iodide upon /3-resor-cylic acid is insoluble in alkalis, and contains but two ethoxy-groups. It has the formula, C6H3(OEt) (OH).COOEt.The action of methylic iodide upon resacetophsnone has been studied, but the results have been anticipated by Gregor (rMoVzatsh. 1894, 15, 437). The principal product is a substance having the constitution C6H,(O&!e)* (OH)*n/Ie*C0CH3, insoluble in alkalis, and resembling the results of the action of methylic iodide upon p-resor- cylic acid. It appears probable that the insolubility of the methyl and etbyl ethers of P-resorcylic acid and resace tophenone, which apparently contain a free hydroxyl group, is due to the fact that the oxygen of this latter has assumed the ketonic form. The constitution of the two former substances would therefore be Preliminary experiments on the methylation of gallacetophenon e have yieldeci a substance melting at 76-77’, apparently a dimethyl-. ether, C6H,(OMe),*OH*CO*CH3.Gallacetophenone oxime, C6H,(OH)3wC:NOH*CH3,and quhzacetophe-nofie oxirne, C6H3( OH),*C:NOH*CH3, were also obtained. 114. “ Note on the gravimetric estimation of maltose by FehIing’ssolution.” By T. A. Glendinning. The specific cupric-reducing power of maltose possesses a different value according to whet.her potash or soda is t’he alkali employed in 164 the preparation of Fehling’s solution. Undcr the conditions of experiment given, the reducing powers to be attributed to maltose, are :-Soda, K3.86= 61. Potash, K(3.96= 64. On making comparative analyses of starch-transformation pro-ducts with the two kinds of Fehling’s solntion, identical results were obtained, provided the respective values of K were used.No such difference occurs in the case of dextrose or of invert sugar. 115. “ Studies in the malonic acid series.” By S. Ruhemann, Ph.D., M.A., and K. J. P. Orton, B.A. The authors have investigated the action of ammonia, hydrazine, aud phenplhydrazine on dibromomalonamide. Ammonia yields di- aminonialonamide, C (NH,),(CONH,), ; and hydraxine and phanyl- hydrazine give the hydrazone and phenylhydrazone respectively of I adonamide. Fuming nitric acid acts on malonamide forming nitromalonamide. Aniline, when heated with nitromalonamide until ammonia ceases to come off, yields diphenylurea. On reduction of nitromalonamide with sodium amalgam, amino- Inalonic acid is obtained.By permission of Professor C1aisen, the authors have investigated the action of hydrazine hydrate on ethyl ethoxymethylenemalonate. They obtain a result which does not agree with that of V. Rothenberg. 116. ‘‘Mercury perchlorates.” By M. Chikashigb. Mercuric perchlorate is not anhydrous, its cornposition being Hg(C104),,GH20. It slowly loses, in a desiccator, acid and water, and effloresces. In the air it is very deliquescent (Serullas). When heated, it melts completely at 34’ (in dry air) ; as the temperature rises to 150°, it very slowly decomposes, giving off water and per- chloric acid, while a white, basic perchlorate, Hg302(ClO,),, is left, permanent at that temperature. If the salt is heated in a long narrow tube, it may be kept in a bath at 400°, for any time, without permanent decomposition, boiling freely and retaining its trans- parency? and, when cooled, solidifying unchanged.Whilst heated it is, however, continuously decomposing into basic salt and acid and water, but as the acid and water vapours condense and flow back, the salt is continuously reformed, and presents only the phenomena of ebullition. Mercurous perchlorate has the composition (HgC10,),,4H,O, ac-cording to the author ; Roscoe found 6H,O. In a vacuum desiccator it loses in two weeks 2H20and a very little acid, and then ceases to 165 lose weight. It is slowly decomposed by heat, even at 100' or less, in dry air, first losing water and perchloric acid, then gradually, from 150' upwards, becoming mercuric salt, and yielding chlorides and a, little chlorate.It resembles mercuric perchlorate in its decom- position, but does not show the phenomena of fusion and ebullition. According to Roscoe, mercurous perchlorate does not lose weight in a vacuum over sulphuric acid, or at 100". 117. '' a-Ethylene dihydroxylamine dihydrobromide." By C. M. Lux-moore, D.Sc. When ethylene bromide is heated with a solution of hydroxylamine in methyl alcohol to loo', two mols. of the latter combine with one of the former to form the dihydrobromide of ethylene dihydroxyl- amine, a white, crystalline subst'ance, soluble in water and alcohol, insoluble in ether. When reduced with hydriodic acid? all the nitro- gen is obtained as ammonia.The constitution of the substance is-therefore CH,*O.NH,*HBr ,and its formation lends some support to the ICH2*O*NH2*HBr view that free hydroxylamine has the structure O=NH,. -Ethylene oxide also reacts with hydroxylamine, forming apparently the base corresponding with lhe hydrobromide described above. 118. '' The alleged isomerism of potassium nitrososulphate." By C. M.Luxmoore, D.Sc. Potassium nitrososulphate, whether prepared by the absorption of nitric oxide, by potassium sulphite, or by the absorption of a mixture of sulphur dioxide and nitric oxide by potassium hydroxide, has always the same properties. Hantzsch's silver salt, (KAgSN205), has been obtained from specimens prepared in these different ways, and showed the characteristic behavioui- described by him.Potassium nitrososulphate reaches a temperature of about 134" (as indicated by a thermometer embedded in the salt) before it explodes, the gradual and quiescent decomposition into potassium sulphate and nitrous oxide that precedes the explosion furnishing the heat that raises the temperature of the substance above that of the bath in which it is heated. Pelouze's account of the properties of this substance can be com- pletely reconciled with the recent observations of Hantzsch and of Divers and Hap, with the exception of the statement that it loses no weight when heated to 110", which is evidently a mistake. Five minutes' heating below 105' causes a loss of weight of 2+ per cent.There is no eridence to warrant, the suggestion of Hantxsch that Raschig's first salt is isomeric with potassium nitrososulphate, nor 166 can it be regarded as identical with the salt prepared by Davy and Pelouze. 119. “On the freezing points of silver and gold.” By C. T. Heycock,F.R.S.,and F. H. Neville. The authors draw attention to the close agreement between the determination of the freezing point of gold, by Callendar, in 1E92, and their own determinations in 1894. The platinum temperatures differ by a few degrees, but, when reduced to the scale of the air thermometer by the same method, the two results do not difier by more than one degree. The authors further consider the icfluence of various gases on the freezing point of silver.They find that the highest and steadiest freezing points are obtained in the presence of free hydrogen or of coal gas, and that nitrogen or carbon dioxide produce little or no depression. They find that the well-known effect of oxygen on the freezing point of silver may amount, in extreme cases to a depression of 20” C., but that the oxygen can be removed by the action of nitrogen or hydrogen. November 7th, 1895. Mr. A. G. Vernon Harcourt, President, in the Chair. Messrs. A. F. Fuerst, T. F. H. Gilbard, E. T. Read, and A. Stans-field were formally admitted Fellows of the Society. Certificates were read for the first time in favour of the Earl of Berkeley, Boars Hill, Abingdon ; Messrs. Arthur Jenner Chapman, Burleigh House, Yerbury Road, Upper Holloway ; George Bertram Cockburn, B.A., St. George’s Hospital, S.W.; Charles Crocker, St. Peter’s Road, Cockett, Swansea ; Gurney Cuthbertson, 69, Shoreharn Street, SheGeld ; William Dixon, 102, Spring Street, Bury, Lanes. : Patrick Joseph D. Fielding, 8, St. Joseph’s Place, Cork; James Gardner, 80, Heaton Terrace, Middleton, near Manchester ; Edward Graham, B.Sc., Dalton Hall, Manchester ; Edgar Septimus Hanes, 108, Alexandra Road, St. John’s Wood, N.W.; Thomas Hawkins Percy Heriot, 23, Wolseley Road, Crouch End, N. ; Frederick Arthur Hillard, B.A., 1, Upper Tichboriie Street, Leicester ; Arthur Edward Holme, MA., 3, Ash Terrace, Savile Town, Dewsbury ; Alfred James, 18, St. Andrews Drive, Pollokshields, N.B. ; Frederick Edward Johnson, 16, Stanley Terrace, West Park, Hull ; Leonard P.Kinni-cutt, Yh.D., &c., Worcester, Mass., U.S.A. ; Walter Mansfield, Trafalgar House, Rroughton, lmics. ; Cecil Massey, Lyniion House, lG7 Lenton Boulevard, Nottiagham ; James l\ilcCreath, 4, Lombard Court, E.C. ; David James Morgan, 10, Northampton Place, Swansea ; Herbert Peck, Wigan Road, Ormskirk ; William Round, 45, St. Peter's Road, Handsworth, Birmingham ; Clarence Arthur Seyler, B.Sc., 31, Windsor Terrace, Swansea ; Matthew Smith, B.A., Aston Hall, Preston Brook, Cheshire ; Frank Robert Stephens, Idris & Co., Camden Town, N.W. ; George Stone, Sydney, N.S.W ; Albertl Thorpe, Charnwood House, Sleaford Road, Preston ; John Williams, B.A., Wesley College, Sheffield ; Thomas Rowland Wingfield, 43, Dorset Street, Rolton ; William Chattaway, Apothecaries Hall, Blackfriars, E.C.;Martin Priest, Apothecaries Hall, Blackfriars, E.C.; William Oakes Kibble, Norbon Villa, Buckhurst Hill, Essex. The PREPTDERTannounced that the following telegram had been sent to Madame Pasteur on the death of her husband, M. Louis Pasteur, in October last -" Madame Pasteur, Institut Pasteur, Rue Dutot, Pttris. " The Chemical Society of London, in common with the entire scientific vorld, mourns the loss of its illustrious Fmeign Member and begs to express to you its deepest sympathy, " VERSON HARCOUI~T, president. " T. E. THORPE,Tyenszwer. '' Joas M. THOJ~SOS, 1 " WY-sDH-4M R. DL-SSTAK,S:ccretnries,'' (' R. MELDOLA, 1 and that the following Address had been presented on behalf of the Society by Dr.Frankland to the Institute of France on the occasion of its Hundredth Anniversary :-" The leading men of the Freiich nation in Literature, Science, .and Art celebrate to-day the hundredth anniversary of a great event. There had perished in the throes of ths revolution a group of Academies which for more than a hundred Fears had shed lustre upon France, and had contributed among the foremost to the general advance of mankind. It was an eclipse of which the darkness could not last long. Two years later, on the 25th of October, 1795, the law was passed which revived the Academies and combined them in the Institute. " The Chemical Society of London, born half a century later and representing one of the sciences which are united under the Acadkmie des Sciences Mathb;matiques et Physiques desire on this occasion to record their sense of the splendid additions to chemical knowledge and thought which have been made by members of the French Academy. They respectfully offer to the Institute their congratulations on what has been achieved, to which they must now add their sympathy and regret for those who have passed away, t,hiiiking especially of the recent loss which science and humanity have sustained by the death of the illustrious Pasteur." Presidmt. A. VERNONHARCOLTRT. '' Treaszwei-. T. E. THORPE.c[I:: " Honorary Secretaries. { .TOHN M. THOMSOK. W YNDHAM R.DUKSTAN. " Fo~eiyiiSecretary. RAPHAELMELDOLA." October 25th, 1895, Of the following papers those marked * were read :-*120.'' On flame temperatures and the acetylene theory of 1~minosity.'~'By Arthur Smithells, B.Sc. The author has submitted to experimental and critical examination the acetylene theory of luminous hydrocarbon flames advocated by Lewes (Trans., 1895, 61,322 ; Pmc. Roy. SOC.,1895, 57, 450); and concludes that it is untenable. Details of the measurement of the temperatures of different parts of hydrocarbon flames by means of the Le Chatelier thermo-couple are given. It is shown that to obtain readings of any value the wires constituting the couple must be bent so as to fit the particular region of the flame in which the measurement is desired, and that if the sheet of flame he thin, even this precaution is insufficient.The exploration of an ordinary flat coal-gas flame gives evidence of no sudden change of temperature in a vertical plane. Sudden changes. are found, however, when the couple is moved from the middle of the flame outwards in a horizontal plane, and the mantle has a tem-perature higher than the melting point of platinum. The author considers Lewes's description of the distribution of zones in flames to be based on erroneous temperature measure-ments, and finds no evidence of such a local condition of temperature as would point to the decomposition of acetylene. The conclusion in, favour of the acetylene theory, based on the comparative luminosity of the ethylene and acetylene flames, is attributed to neglect of the consideration that in the latter there is a higher temperature and a, greater relative amount of carbon.The indirect evidence derived fi-om the behaviour of cyanogen is stated to arise from the yellow ammonia flame having been mistaken for one containing solid carbon. The theoretical arguments based on thermo-chemical con- siderations are adversely criticised. The author maintains that, the luminosity of hydrocarbon flames, including t’he flame of acetylene, can be adequately explained on the older theory of their structure confirmed and extended by his earlier experiments (Trans., 1892, 61, 217). According to this view, a luminous flame is invested by a sheath of gas in non-luminous com- bustion.This sheath, which is double at the lower part, corresponds to the two cones of a Bunsen flame, and produces an exceedingly high temperature. The gas within this sheath is intensely heated as it ascends, and is gradually decomposed so as to furnish a sheet of carbon particles, becoming more and more numerous. These glow partly by heat and partly by combustion ; the higher the tempera- ture of the non-luminous sheath, and the greater the relative number cf particles, the brighter will be the flame. This is well seen in the case of acetylene. The author believes that the precise steps in the decomposition of a hydrocarbon by which carbon is deposited are at present unascertainable by any direct means, but as the glow of the carbon particles in a hydrocarbon flame is in no case greater than that acquired by a platinum wire immersed in the same region, he considers that there is no ground for supposing that the endothermic decomposition of acetylene (of which substance only a very small quantity has been found in the flame gases) plays any appreciable part in the phenomenon.*121. “A new series of liydrazines.” By Frederick D. Chattaway, B.A., and Harry Ingle, B.Sc. Primary and secondary hydrazines have proved such important substances that other substituted derivatives of hydrasine have scarcely been studied. Theoretically, hydrazine should yield five series of substituted deri- vatives, of which only three are known, the primary, the secondary symmetrical, and the secondary unsymmetrical.No simple method of obtaining members of the other series has hitherto been described, and the authors have undertaken their investigation. The quaternary hydrazines, which are dealt with in the paper, can be obtained by a simple general reaction from the secondary amin es . The secondary amine is treated with sodium or sodium ethylate, whereby the hydrogen atom is replaced by sodium, R,NH + Na = R,NNa + H. The equivalent quantity of iodine is then allowed to act upon the sodium compoiind, when the sodium atoms are with- drawn, and the two Eubstihted amido-groups unite to form the qua- ternary hydrazine, R,N*Na + I, + Na*NR, = R2N*NR2+ 2NaI. The aromatic quaternary hydrazines which have been so far more 170 especially studied are stable, well-crystallised compounds, which are not easily oxidised and are scarcely if at all basic.Their percentage composition and the molecular weights obtained by Raoult’s method, using benzene as a solvent, agree well with the theoretical. Tetrapheszyl hydmzine, (CsH5),N.N( C6H5),,obtaired by the above reaction from diphenylamine, crystallises in long, orthorhotubic prisms, m, p. 147’. It is easily soluble in benzene, chloroform, and acetone, and dissolves in cold concentrated sulphuric acid, giving a deep purple solutioi:. Tetra-P-toZyZ hydmzine, (C6&CH,),N*N(C6H4CH3)2, prepared from di-p-tolylamine, cryatallises in large, pale yellow monoclinic prisms or tables, m. p.138’. It is easily soluble in benzene, acetone, and chloroform, and dissolves in cold concentrated sulphuric acid, giving a brilliant, azure blue solution. 122. “The action of certain acidic oxides on salts of hydroxy-acids. Part 11.” By G. G. Henderson, D.Sc., M.A., and David Prentice. The action of antiinonious and arsenious oxides upon salts of citric, malic, lactic, and mucic acids has been studied, and several new salts have been prepared, the oxide being heated with solutions of salts of those acids for varying periods, and the compounds formed precipi- tated by alcohol or separated by crystallisation. With citrates of potassium, sodium and ammonium, antimonious oxide gave compounds of the general formula sboM’3(C6H60,)2.xH?0, which are all crystalline and readily soluble in water.A sparingly soluble barium salt, SbOBa3(C6H60,),.10H20, was obtained by pre- cipitation, and from it a very soluble crystalline compound of the probable formula 0H.Sb:(C6H707), was prepared. Arsenious oxide gave similar compounds with citrates of the alkalis. They have the general formula ASOM’,(C6H60,)2*zH20,are crystalline, and dissolve freely in water. Bosh antimonious and arsenious oxides dissolve in boiling aqueous solutions of alkaline malates. A well cryst,allised antimony com-pound, whose simplest formula is (XbU),K,H( C4H,O6),*3H,O, was prepared, but no corresponding arsenic compounds have yet been obtained, owing to their instability. Boiling solutions of 1actat.e~ of the alkalis and of barium readily dissolve both antimonious and arsenious oxides, and alcohol precipi- tates colourless syrups, containing large quantities of unaltered lactates. Compouncls of the oxides with rnucates were also prepared, though with some difficulty.Two antimony compounds of tLe formuh ~SbOKCsH80,.KC6H30,.6H,0and SbOKCtiH,0,*4H,0 were obtained 171 in the form of sparingly soluble cryst8alline powders. An arsenic compound corresponding to the second of these was likewise ob- tained. These substances might be regarded as double citrates, malates, &c., containing the radicles (SbO)’ and (AsO)’, but, if so, then in all probability those radicles replace the hydrogen of alcoholic hydroxy 1 groups, and not the hydrogen of carboxyl groups as in the formation of selts, for otherwise it is difficult to understand why hydroxy-acids alone seem to have the power of forming such compounds.On the other hand, they might be regarded as salts of acids derived from antimonious or arsenious acids by replacement of two of the hydroxyl groups of those acids by organic acid radicles, as is the case with the antimonio- and arsenio-tartrates. The formulm of such acids would be, for antimonio-citric acid OH~Sb:(CsH,07)a, for antimonio- malic acid OH*Sb:(C4H505)2, for antimonio-mucic acid, OH-Sb:C6H80,; the formula of the arsenious acid derivatives would be similar to these. In the case of some at least of the new compounds this view appears preferable. 123. Sodium nitrososulphate.” By E.Divers, F.R.S., and T.Haga. Sodium nitrososulphate, being a very soluble salt, does not crystallise out when even the strongest solution of sodium sulphite is treated with nitric oxide. But if the solution, after this treatment has been continued long enough, be deprived of most of its sodium sulphate by freezing out, and be then evaporated in a vacuum to a very small volume, sodium nitrososulphate is deposited in crystals. It is an anhjdrons salt, forming very minute crystals, which in tlte solution adherr! together in opaque crusts. The salt is slightly alkaline to litmus, and tastes much like common sslt. It is exceed- ingly soluble in water and very unstable, wet or dry. In the dry state, in which it can be obtained in a desiccator, and at the common temperature, it rapidly decomposes on exposure to (damp) air, becomes nearly as hot as slaking lime, and gives off llirge quantities of nitrous and nitric oxides.The residue consists of sodium sulphate and sulphite. It thus behaves at the common temperature as potas- sium nitrososulphate only does when heated to about 100”. In solution in water it continnously decomposes, like the potassium ,salt, into sulphate and nitrous oxide. A little sodium hydroxide greatly ret,arda this decomposition in water, but if a solution of the salt containing sodium hydroxide is heated to boiling, the salf dccoinposes freely into nitric oxide and sulphite. This behaviour is unlike that of the potassium salt. Its composition, which was indirectly determined quantitatively, is Na*ON:NO.SO,Na.172 124. “ The constitution of nitrososulphates.” By E. Divers, F.R.S., and T. Haga. Potassium nitrososulphate in aqueous solution becomes strongly alkaline when mixed with a little alcohol. This is due to the salt and the alcohol partly decomposing into potassium ethyl sulphate, nitrous oxide, and potassium hydroxide. The primary reaction is, beyond a doubt, one in which potassium hydrogen hyponitrit,e is produced, along with the potassium ethyl sulphate, although none can be detected; but then its formation proceeds here very slowly, and certainly not faster than it is known to decompose of itself into potassium hydroxide and nitrous oxide. This reaction is peculiarly interesting, for in it alcohol decom- poses a sulphate in alkaline solution, and liberates potassium hydroxide, though indirectly.The occurrence of this reaction, taken with other properties, solves the problem of the constitution of the ni trososulphates. They are anhydro-double salts of hyponitrous and sulphuric. acids, which hydrolyse into the acid salts of these acids, the the acid salts simultaneously changing into normal sulphate, nitrous oxide, and water. They are analogous to the thiosnlphates, the hyponitrite radicle acting as sulphur does in them. Thus we see calcium thiosulphate and sodium nitrososulphate forming themselves from the sulphite of their metal and decomposing into it again, under precisely similar conditions.Nitrososulphates are, however, true sulphates, as their reactions with alcohol and with acidified barinm chloride show, their nitrogen being united to their dphuy only though an atom of oxygen, KON,*0.S03K. 125. “ Normal hexane from light petroleum (petroleum ether).” By G. L. Thomas, B.Sc., and Sydney Young, D.Sc., F.R.S. Having devised an improved form of dephlegmator (Chenz. News, 71,177) we determined to attempt the separation of a pure paraffin from “petroleum ether” in the same way that ethyl acetate was separated from a mixture of methyl, ethyl, and propyl acetates (Phil. Nag., 1894, 8). Each fraction was weighed, and its temperature range noted and corrected for the thermometric error and for the difference between the barometric reading and 760 mm.The ratio of the weight of any fraction (Aw) to its temperature range (At) gives, AS a rule, a mea-sure of the pnrity of the liquid, though in the early fractionations of a complex mixture this cannot be relied on. Thus, in the 4th fyactionation the fraction coming over between 65.0” and 66.0’ had the highest value of Aw/At, whereas in the 16th fractionation the corresponding fraction (65.0’ to 66.85”) had the 173 lowest value. At an early stage of the work it appeared, therefore, as though a single substance boiling at about 65" or 66' was being separated from liquids boiling at much higher and lower temperatures (above 90' and below 40') ; but the later fractionations showed that instead of a single substance boiling at about 65' or 66", there were really two liquids-one boiling at 69", and the other at about 61" (normal and iso-hexane) .As the number of fractions was very large, it was decided after the 16th fractionation to proceed only with the separation of normal hexane, and after 31 preliminary fractionations it was considered that the separation had proceeded far enough for the final series of fractiona- tions to be undertaken, as in the case of ethyl acetate (Zoc. cit.). The hexane obtained by the final fractionation of the fractions boiling at and above 69-05', when distilled from phosphorus pentoxide, boiled at 69.1°, or only 0.1" higher than the hexane prepared from propyl- iodide, but its sp. gr. at 0" (0.68478) was 1.15 per cent.higher. 'I'he hexaae was then treated with a mixture of concentrated sulphuric and nitric acids, when considerable heat was evolved, and the acid became yellow, and was found to contain some m-dinitrobenzene in solution. The impurity present was therefore benzene or possibly hexanaphthene, or both. The remaining high boiling fractions were treated with the mixed acids and were refractionated; the low bding fractions also were treated in the same manner before their final fractionation, and in every case it was fouiid that m-dinitrobenzene was formed. By further long continued treatment of the two specimens of hexane with the mixed acids and subsequent distillation, a quantity was finally obtained boiling at 69.05' and with the sp. gr. 0.67813 at 0", or only 0.17 per cent.higher than that of pure hexane. The vapour pressares and specific vohmes-as liquid and as satu- rated vapour-were determined at a few temperatures, and the critical temperature and pressure were also observed ; the results differed but slightly from those obtained with the hexane from propyl iodide. The critical constants of both specimens are given below. Critical Critical temperature. pressure. Hexane from petroleum ether.. .. 235.15' 22560 Hexane from prop91 iodide ...... 234.8 22510 The hexaiie was evidently very nearly pure, but the separation of this paraffin from petroleum ether is only possible by long continued fractional distillation with an efficient dephlegmator, and by removal of benzene or hexanaphthene with nitric and snlphuric acids.174 .26. "The vapour pressures, specific volumes, and critical constants of normal hexane." By G. L. Thomas, B.Sc., and Sydney Young, D.Sc., F.R.S. The normal hexazle employed was obtained from Kahlbaum and prepared by the action of sodium on propyl iodide. It was purified by treatment with concentrated nitric and sulphuric acids and subse- quent fractional distillation. The boiling point at 760 mm. is 69*0",and the specific gravity at Oo is 0,67696. The critical coristnnts are, Critical temperature. .... .. 234.8" Critical pressure.. ... . .... 22510 mm. Critical volume of a gram .. 4.268 C.C. The vapour pressures and the volumes of a gram-as liquid and as saturated vapour-were determined, and a limited number of observa-t>ionsof presslire and volume of unsaturated vapour were made at a series of temperatures with the object of finding whether the isochors showed any indic:htion of curvature.As in the case of isopentane (in about the same volume region) the isochors were found to be very slightly curved, the values of @/dt diminishing with rise of tempera- ture. The deviations from constancy become smaller as the volume increases. The absolute temperatures and molecular volumes of liquid and saturated vapour were read from the curves at a series of pressures " correspmding " to those given in previous papers, and the ratios of the absolute temperatures mid of the volumes to the critical constants werc calculated.These ratios agree with those of isopentane and benzene ; nornial hexane therefore belongs to Group 1in the classifi- cation of substances previously adopted (Trans., 63,1257 ; Phil. Mag., 1894, l), and the molecules of the liquid are probably simple like those of the gas. The absolute temperature ratios at corresponding pressurcs are higher for hexane than for isopentane ; in this respect the paraffins been1 to resemble the esters (Trans., 63, 1252), for which the ratios increase without exception with rise of molecular weight. In the case of the esters, the volume ratios appear to be independent of molecular weight, but-for isomeric compounds-to depend to some extent on the constitution. It seems probable that this may also be the case for the two paraffins studied, but an investigation of other parafins will be necessary before these points can be decided.The ratio of the actual to the theoretical density at the critical point is 3.83, the mean value for the other members of Group I, including carbon dioxide (Amagat) and isopentane being 3.75. 175 127. ‘‘ Acidylthiocarbimide;.” By Augustus E.Dixon, M .D. This paper gives an account of further experiments (see Dixon aid Doran, Trans., 1895, 67, 565) on the production of thiocarbimides containing acidic radicles. By heating the chloride of valerianic or of cinnamic acid with lead thiocyanate in presence of anhydrous ben- zene, valeryl or cinnarnoyl thiocarbimide is formed, and passes into solntion. Both these thiocarbimides have a slightly pungent odour, and attack the eyes, causing a flow of tears, the former being especially active.They are readily desulphurised by lead or silver salts, but decompose in presence of water, yielrling thiocyanic acid, together with tbe acid characteristic of the thiocarbimide, Ph*CH:CH*CO*NCS + H,O = HSCN + PhCH:CH*COOH. By bringing the solutions into contact with ammonia, amines, or ethyl alcohol, the correspond- ing thioureas, thiocarbamides, or thiourethanes, respectively, are pro-duced. The following compounds are described : ab-’CTaZeryZphhenylthiocaI.ba?nide,BuCO*NH*CS*NHPh; sym. valeryl-pheny lurea, BuCO*NH*CO-KHPh; ab-valerylort7~otoZylthiocar~a~nid~, BnCO-NH*CS.NH-o-To; sym. waZerylorthotolylurea; ab-vaZerylpara-tolylthiocarbamide, BuC0-NH.CS-KH-p-To; valsryl-x-naphthylthio-cnrbamide, BuCO*NH*CS.NH*aNapt; n-~aZeryZ-v-benzylphenlJZfhiolcl.ea, PhCH,*N(Ph) *C(SH)1N.COBu ; t-alery 1thiourea, CSN,H,.C 0Bu ; Taleryl-p-thiourethane, BuCO*NH.CS*OC,H,; ab-cin?aamoyl~henylthi~-ca;.bamide, PhCH:CH*CO*NH*CSsNKPh ; ab-cinnamoylorthotollJZthio-carburnide, PhCH:CH*CO*NH*CS.NH-o-To;a,b-cinnamoyZ~aratoZllZlhio-carbaazide, PhCl3:C H*C0.NH.C S-NH-p-To ; ab-cinnarnoy Zcclphunaph-thylthiocarbamide, PhCHICH*C O*NH*CS*N HaNapt ; cinnanaoyZthio-urea, CSM,H,.COCH:CHPPh ;PhCH:CH.CO*NHCS *OC2H5,cinnamoyl-0-tliiourethane.All the thioureas above-named, with the exception of the valerylbenzoylphenyl compound, are desulphurised by heating wihh alkaline lead tartrate.It is proposed to extend these experiments with lead thiocyanate, in the hope of obtaining thiocarbamides derived from other acids than those only containing the group CO-Cl; for example, picric, phenylsulphonic, and ethylsulphuric acids. 128. ‘‘ Some constituents of the root of ‘Polygonum Cuspidaturn.’ ’’ By A. G. Perkin. Polygonunz cuspidatum is a native of China and Japan, and flourishes in parts of India and Russia. The freshly gathered roots consist of a thick, succulent bark of an orange-red colour, and a central, woody portion of‘a light yellow tint. The principal constituent of the root bark was found to be a glu- coside, C21HZ0010,crystallising in lustrous, yeIIow needles melting at 202-203”. On hydrolysis, this yielded 61.82 per cent.of a product which was recognised as emodin, tlie reaction C,,H,,,O,,, + H,O = C,5H,o0,+ C,H,,O, requiring G2.5 per cent. of emoilin. This glucoside, lor which the name cuspiduti?z is proposed, di-ff’ers considerably in properties from frangulin, C21H2009,the glucoside of emodin which is contained in the bark of the Rhunznzcs jyangula. A second glucoside was also isolated, but in too small quantity for malysis. On hydrolysis, it yielded a crystalline substance melting at 199O, which by treatment with sulphuric acid at 160’ was con-verted into emodin. It was found to be identical with the errlodin monomethyl ether previously isolated from the root bark of VentiZngo machaspatamce (Trans., 1894, 923). The other substances found were a sniall amount of free emodin and a wax which crystallised in colourless leaflets melting at 134-135’.This latter was found to be identical with the wax C18H2,0,present in the root bark of the Mos-inda umbelluta (Trans., 1894, 854). An examination is being carried out of the constituents of the root3 of the Polggonurrz bistorta and Runzex nepalensis, which are closely allied to this plant. 129. “Note on tlic action of hydrofluoric acid upon crystallised silicon.” By G. S. Newth. It is generally stated that hydrofluoric acid is without action upon crystallised silicon -tliat while amorphous silicon is attacked by it, this acid is incapable of acting upon the cr-j-stallised element. This statement, however, requires to be made with some reserva-tion, for although it is doubtless true of the aqueous acid, and possibly of the liquid acid, it is not true of the gas.If acid potassium fluoride be heated in a platinum retort, and the pure gaseous hydrofluoric acid so produced be allowed whilst hot to blow upor, a little heap of crystallised silicon supported on a porcelain crucible lid, the silicon at once takes fire and burns brillia~tly in the gas, forming silicon fluoride and hydrogen. If the neck of the retort be more than an inch or two in lengtli, it is necessary to heat it in order to keep the gas sufficiently hot, but if it be quite short, the temperature of the gas as it is disengaged from its compound is sufficiently high to enable it to attack the silicoii.The importance of this observation lies in the facc tliat the spon-taneous ignition of crystallised silicon is generally regarded as in all cases a sufficient test for free fluorine; but it is evident that unjess the temperature of the gas is below a certain point the conibustiori of silicon is not a safe criterion. 130. “Note on the periodides of theobromine.” By G. E. Shaw. Apparently only one periodide of theobromine has been previously described, viz., that having the formula C7H8N4Oz*HI*I3,prepared by Jorgensen by exposing a solu lion of theobromine hydrochloride, mixed with potassium iodide, to the air. By varying the amounts of hydrochloric and hydriodic acids present, the author has obtained compounds having the formulz (C,H,N40,),HI~HCl*I,and (C7H,N402)3H~(HC1)2T3, and by recyystallisation of a mixture of the three froni weak alcohol containing hydriodic acid and iodine, a substance of the Composition (C7H,N40,HI)12 + H,O was obtained. A solution of theobromine in saturated hydriodic acid deposited on standing crystals having the composition (C7H,N40,HI),T3.131. A synthesis of diphenyloxytriazoline.” By George Young, Ph.D. The reaction between benzaldehyde and phenylsemicarbaside de-scribed in a previous notice (Proc., 1894,95, 124), and represented by the equation CiHl,N30+ C,H,O + 0 = ClaH,,N30 + 2Hz0, is shown in the present paper to take place in the following two stages. I. C7HJY,O + 0 = C,H;N.30 + HZO; 11. C;H,N,O + CiHeO = C~~H~IN~O+ H,O.The intermediate product, CTH7N30,is phenyl- azocarbonamide, C,H,N:N*CO*NH,. It is formed immediately by the action of ferric chloride in aqueous solut,ion, or Fota’ssiuin permanga- nate in dilute sulphuric acid. It is also formed, but very slowly, by the action of moist air on phenylsemicarbazide. It forms red needle- shaped crystals, m. p. 114”. The second stage of the above reaction does not take place so easily when the intermediate product is isolated as when the benzaldehyde is added to the phenylsemi-carbazide before oxidation. In the latter case, the whole reaction takes place in boiling alcohol ; in the former, the azo-derivative and the benzaldehyde require to be heated in alcohol in a sealed tube at, 120” C. The benzoyl derivative, ClrH,,N30(CiH5O), has been pre- pared, in addition to those previoiisly mentioned, by the action of benzoyl chloride on diphenyloxyt,riazoline and its silver salt. It forms flat needles, m.p. 133.5’. 132. “ Note on piperovatine.” By Wyndham R. Dunstan, F.R.S.,and Francis H. Can. The method previously used (Trans., 1895) for extracting pipero-vatiiie from Pipel-ocatum being exceedingly tedious, the authors experimented with the view of finding a better method. The following process is a considerable improvement, and with its aid the active constituent can now be extracted and crystallised in the course of a few hours. The method consists in percolating with ether; the dark- coloured extract fhus obtained is freed from ether, and the adhering volatile oil, and then extracted with hot dilute alcohol (15 per cent,.) ; on cooling this extract, crystals separate, which may be recrystallised from 40 per cent.alcohol. Further experiments have been made on tfhe hydrolysis of pipero-vatine with the small remaining quantity of material. A small quantity was heated with water in a sealed tube to 160°, with the result that a volatile base, probably a pyridine derivative, a substance smelling like anisol and giving phenol, on treatment with sodium hydroxide, and also an acid were produced. 133. "Dibenzaconine and tetracetylaconine." By Wyndham R. Dunstan, F.R.S.,and Francis H. Cam. The authors having failed so far to produce aconitine by the acetylation of benzaconine have tried to form benzaconine by intro- duciiig a benzoyl group into aconine; this, however, has not yet been contrived, but new aconine derivatives have been obtained, When equimolecular proportions of aconine and benzoic anhydride are dissolved together in chloroform and allowed to &and at the ordinary temperature, reaction occurs with production of dibenz-aconine.Dibenzaconine, C,,H3,(Bz),NO,, is unlike aconine in being insoluble in water and soluble in ether ; it crystallises from ether in rosettes of needles, m. p. 265", Dibenzaconine hydrobromide crystallises well from a mixture of alcohol and ether, m. p 261". Dibenzacouine aurichloride is precipitate cl by adding a sohtion of gold chloride to a solution of the hydrochloride of the base, and may be crys- tallised in yellow tables from a mixture of alcohol, ether, and petroleum, m.p. 212'. This salt contained 18.2 per cent. of gold; calculated for C,,H,,(Bz),N O,,HAUC~~,18.71per cent. Hydrolysis of the base furnished 33.3 per cent. of benzoic acid; the calculated quantity for C,,H37(Bz)2N0,0is 34.4per cent. By the action of a large excess of benzoic anhydride, a crptalline base, m. p. 190", soluble in ether and insoluble in water, is formed, which has not been f urt'hey examined. Benzoyl chloride dissolved in chloroform does not react with aconine even when heated with the base. Tetracetyl-aconine is formed when a solution of aconine hydro- chloride and acetyl chloride in chloroform is allowed to stand for 36 hours at the ordiiinry temperature.It is insoluble in water, but 179 readily soluble in ether and in alcohol, from either of which solvents it crystallises in small prisms, m. p. 196". On hydrolysis, aconine and 35.2 per cent. of acetic acid areformed, the formula C24H35(A~)4NOI,) demands 35% per cent. of acetic acid. 134. " Molecular volume change during the formation of dilute solu-tions in organic liquids." By A. Wentworth Jones, M.A. The author has determined the volume changes during the forma- tion of several solutions in benzene and carbon disulphide, and calculated the molecular volume change as v x m x W/V x M x w --2. Where w = observed volume change, V = volume of solution, n?.= molecular weight of substance, zu = weight of substance taken, W = ,, solvent ,, 31 = molecular weight of solvent, and x = ,, expansion or contraction. The values for molecular weights of several "non-associating " liquids are very different, and sometimes change their sign, and if the phenomena, of these solutions in organic liquids are comparable with those of aqueous sollitions of organic compounds, it is impossible to admit that these volume changes are measurements of the attraction csf substance for solvent and equal for molecular weights of different substances, as is stated by Traube (Bey., 2895, 28, 410).The following values have been obtained by the use of the specific gravity method. Cadon Disulphide Polutions Benzene Solutions cct 15' C. at 15' C.Molecular Molecular expansion.expansion. Methyl formate.. .... 0.0156Mt.thj1 formate ...... 0.0797 Ethyl acetate ....... 0.0076Ethyl acetate ........ 0.0809 Ethyl acetoacetate ... 0.0120Ethyl acetoacetate .... 0.1072 Paraldehyde ........ 0.0141Paraldehyde ......... 0.0972 Nitrobenzene .......-0.0040Nitrobenzene ........ 0.0549 Benzaldehyde ......-0.0042Benzaldehyde ........ 0.0305 Aniline ............-0*(I'067Aniline ............. 0.0310 Carbon disulphide ... 0.0188Benzene ............ 0.0320 Piperidine .......... 0.0020Ethyl iodide ...... -0.0632 Phosphom s trichloride O.OC41 Phosphorus trichloride. -0.0913 A contraction occurs in the A contraction occLirs in the 5th, 6th, and 7th cases. last two. 110 The author suggests that these volume changes occurring cn solution are of the same nature as the smaller changes occurring when a moderately strong solution is diluted, and that both are analogous to the deviations from Boyle’s lam observed in the case of gases.ADDITIONS TO THE LIBRARY. I. Donations. Notes on the Chemistry of Iron. By Magrius Troilius, E.M. Svo. Pp. vi+ 98. New York 1886. From B. H. Brough, Esq. Notes on the Nebular Theory in relation to Stellar, Solar, Plaue- harp, Cometary, and Geological Phenomena. By W. Ford Stanley, F.R.A.S., F.G.S., &c. 8vo. Pp. xv+259. London 1895. From the Author. An Introduction to the Study of Rocks. Mineral Department, British Museum (Natural History). Printed by Order of the Trustees. Prom the Trustees.The Glasgow TJniversity Calendar, for the year 1895-96. From the University. Principles of Chemistry. By D. Mendel6eff. 6th Edition. Svo. Pp. ixf i80. From Prof. D. Mendelkeff. Poisons: Their Effects and Detection. A Manual for the use of Analytical Chemists and Experts. By Alexander Wynter Blyth. 3rd Edition. Revised and Enlarged. 8vo. Pp. xxxii3.724. London 1895. From the Author. University College, Bristol. Calendar for the Session 1S95 96. dristol 1895. From the Council of the College. 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Notes of Courses of Lectures delivered at the Royal Institu- t'ion during the years 1833-37 by Faraday, Brande, and others, with some later notes.4to. Pp. 542 +8 pp. index. Presented by Mr. E. Ivens Moon. 11. By Purchase. h Dictionary of Explosives (Second Edition). By Lient.-Col. J, P. Cundill, R.A. Entirely Re-arranged and brought up to date by Captain J. H. Thomson, R.A. 8vo. Pp. xliv+ 183. London 1895. Die neueren Arzneimittel in ihrer Anwendung und Wirkung dar- geetellt. Ton Dr. W. P. Loebisch. 8vo. Pp. viii+416. Wien und Leipzig 1895. Die Methoden der Bakterien-Forschung. Handbuch der gesamm- ten Methoden der Nikrobiologie. Von Dr. Ferdinand Hueppe, Svo. Pp. viii $495. Wiesbaden 1891. Geschichte der Explosivstoffe. I. Geschichte der SprengstofT-chemie, der Sprengtechnik und des Torpedowesens bis zum Beginn der Neuesten Zeit.S. J. von Roinocki. 8vo. Pp. viii+395. Berlin 1895. A Guide to Stereochemistry, based on Lectures delivered at Cornel, University, with an Index to the Literature and an Appendix, Models for use in Teaching Organic Chemistry. By Arnold Eiloart, Ph.D., R.Sc. Reprinted with additions from Scientitific Periodicals. Illus- 183 trated with 50 Woodcuts and five Plates. 8vo. Pp. ii+ 96f 6. New York and Halle. An Introduction to the Study of Metallurgy. By W. C. Roherts- Austen, C.B., F.R.S. Third edition. Revised and Enlarged. 8vo. Pp. xvi+379. London 1894. Lehrbuch der Gerichtlichen Chemie mit Beriichsichtigung Sani- tatspolieeilicher und hledicinisch-Chemischer untersuchungon Zuni Gebrauche bei Vorlesungen und iru Laboratinm. Bearbeitet von 111..Gevrg Baumert. 8vo. Pp. xx +422. Braunschweig 1889-1893 . An Introduction to Chemical Crystallography. By Andreas Pock, Ph.D. (Berlin). Translated and Edited by Wm. J. Pope, with a Preface by N. Story-Maskelyne, MA., F.R.S. 8170. Pp. xvi+lS9. Oxford 1895. Ausfuhrliches Lehrbuch der Pharmaceutischen Chemie. Bearbeitet von Dr. Ernst Schmidt. Erster Band. Anorganische Chemie. Dritte vermehrte Auflage mit zahlreichen Holzstichen und einer fabrigen Spectraltafel. 8vo. Pp. xxiii +1106. Braunschweig 1893. Ostwald’s Klassiker der exakten Wissenschaften, Nr. 66. Die Anfange des Naturlichen Systemes der Chemischen Elemente. Ab-handlungen von J. W. Docbereinel. (1829) und Max.Pettenkofer (1850). 8170. Pp. 34. Leipzig 1895. A Manual of Microchemical Analysis. By Professor H. Behrens, with an Introductory Chapter by Professor J. W. Judd, P.R.S., wikh 84 Illustrations drawn by the Author. 8170. Pp. xxv+246. Londoii 1894. Kurzes Handbuch der Kohlenhydrate. Von Dr. B. Tollens. Zweiter Band. 8vo. Pp. xvi+407. Breslau 1895. Jahrbuch der Organischen Chemie : herausgegeben von Gaetano Jfinunni, Palermo. Erster Jahrgang 1893 mit einem Vorwort von Ernst von Meyer. Leipzig 1895. Svo. Pp. xiv+881. Two copies. M6moire sur la liqukfaction de l’oxyghne, la liqukfaction et la solidification de l’hydrogdne et sur les theories des changements des corps. Par M. Raoul Pictet. Genhe 1878. 8170. Pp. 108. Three plates. Die Industrie des Steinkohlentheers nnd Ammoniaks.Von Dr. Georg Lunge. Dritte Auflage. Braunschweig 1888. 8vo. Pp. xvi +657. A Text-book of the Science and Art of Bretid-making, including the Chemistry and Analytic and Practical Testing of Wheat, Flour, and other materials employed in Baking. By W. Jago. London 1895. 8vo. Pp. xii+648. Chemical Analysis of Oils, Fats, and Waxes, and of the Commercial Products derived therefrom. From the German of Professor Dr. R. Benedikt. Revised and enlarged by Dr. J. Lewkowitsch. London 1895. 8vo. Pp. xviii+683. Solution and Electrolysis. By W. C. D. Whetham, JL4. Cani-bridge, 1895. 8vo. Pp. viii +296. (Cambridge Natural Science Manuals. Physical Se~ies.) COLLECTIVE INDEX OF THE TRANSACTIONS, ABSTRACTS, AND PROCEEDINGS OF THE CHEMICAL SOCIETY.Volume 11,187:3 to 1882. Volume 111,1883 to 1892. The Council, having determined to publish a Collective Index of their publications from 1875 to 1892 inclusive, will issue copies to Fellows who may notify their wish to receive them. Both volumes will be sent to those who have been Members of the Society since the end of 1882. Volume I11will be sent to Fellows who have joined the Society between 1st January, 1883 and 31st December, 1892. Fellows who are ineligible to receive gratis copies, and those who may have neglected to apply for them within the prescribed period, may obtain them by purchase at a price to be hereafter fixed. Fellows who desire the Index should notify their wish by letter, enclosing 1s.for cost of distribution, &c., to the Assistant-Secretary, Mr. Robert Steele, Chemical Society, Burlington House, W., before 31st December, 1895. For Fellows resident abroad, who should remit %.,which may be paid along with their annual contribution, the time will be ex- tended to 1st Narcb, 1896. RESEARCH FUND. A meeting of the Research Fund Committee will be held in December. Applications for grants, accompanied by full particulars, should be sent to the Secretaries before December 11th. At the next meeting on Thursdaj, November 21st, the following papers will be read :-“ The evolution 01carboil monoxide by alkaline pyrognllol solutions during absorption of oxygen.” By Professor Clomes. “ The composition of the limiting explosive mixtures of various combubtible gases with air.” By Professor Clowes.“ Barium butyiate and the estiniation of butyric acid.” By W. H. Wilcox, B.Sc. “ On some derivatives of antbraquinone.” By Dr. E. Schunck, F.R.S., and Dr. L. Marchlemski. CERTIFICATES OF CANDIDATES FOB 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 Thursday, December 5th, 1895:-Bailey, George Percy, 7, Mount Pleasant Square, Dublin. Chemical Demonstrator. Senior Moderator, E.A. in Experimental Science of Dublin University ; now engaged in chemical investiga- tion at above University, and also as extra assistant to Professor of Chemistry ; late Science Master at Lucton School, Herefordshire.J. Emerson Reynolds. Emil A. Werner. W. E. Adeney. William A. Tilden. Charles A. Kohn. Berkeley, the Earl of, Boars Hill, A4bingdon, Oxfordshire. Occupied in scientific research. Has studied Chemistry and @ology at the Royal College of Science, and is working especially on the density and crystalline forms of related salts in the labora- t,ory, Christ Church, Oxford. A. Veriion Harcourt. T. E. Thorpe. W. Palmer Wynne. Wpdham R. Dunstan. John M. ThomsoiL. Chapman, Arthur Jenner, Burleigh House, Yerburg Road, Upper Holloway, N. Analytical Chemist. Four years at Finsbury Technical College, and now engaged as Chemical Assistant in the Laboratory of the London County Council.R. illeldola. W. J. Dibdin. R. Grimwood. E. J. Parry. J. H. Coste. 186 Chattaway, Wm., Apothecaries’ Hall, Lonclon, E.C. Chemist and Superintendent of the Society of Apothecaries. Public Analyst for the Borough of Colchester and the Parish of Hammersmith. Fellow of the Institute of Chemistry, Member of the Society of Public Analysts. Frank L. Teed. Ed ward Bevan. Clias. Fred. Cross. Leonard Temple Thorne. C. G. Moor. Alfred H. Allen. Cockburn, George Bertram, St. George’s Hospital, Hyde Park Corner, S.W. Demonstrator of Chemistry. Studied Chemistry at New College, Oxford, and graduated in Chemistry, taking Honours in the Final School of Natural Science. At present, Demonstrator in the Chemical Laboratories at St.George’s Hospital. W. W. Fisher. John Watts. J. Addyman Garclner. J. E. Marsh. V. H. Veley. Chas. Slater. Crocker, Charles, St. Peter’s Road, Cockett, Swansea. Analytical Chemist and Assayer. Analytical Chemist and Assayer, Gas Analyst to the County Borough of Swansea ; Science Teacher (Honours) under the South Kensington Science and Art Department. For 16 years chief Assistant to the late Dr. W. ;Ilorgan, F.I.C., F.C.S., and at present chief Assistant to Messrs. W. Morgzn, Son, and Seyler, Technical Institute, Swansea. Christopher James. Geo. L. Thompson. W. Terrill. Williain Crookes. William Ramsay. Cuthbertson, Gurney, 69, Shoreham Street, Sheffield. Superintendent of (for Messrs. Lewis, Berger, and Sons, Limited) the Lead Works, Sheffield. Matriculated London Universit,y, Janu- ary, 1890.Studied at University College of Wales, Aberystwyth, and in the laboratories of Messrs. Wren and Gurney. For three years Assistant in the Laboratory of Messrs. Lewis, Berger, and Sons, Limited, Manufacturers of colours, paints, &c., axid at, present engaged in their Sheffield Works as above. William Thorp. Bernard Dyer. John Spiller. Frederic Jas. $1. Page. Frank Clowes. 187 Dixon, William, 102, Spring Street, Bury, Lancashire. Science Master. Head of Chemistdry and Physical Departments, Municipal Technical School, Bury. Member of the Society of Chemical Industry. Sixteen years’ experience as Lecturer and Demonstrator in Chemistry and Physics.Educated at the Royal College of Science, South Kensington, London, during 1877-8-9, and for several years at Owens College, Manchester. E. Frankland. T. E. Tliorpc. G. S. Newth. W. Palmer Wynne. H. E. R,oscoe. H. B. Dixon. Jas. Graszt. Farr, Edward Henry, Uckfield. Pharmaceutical Chemist. Teacher of Chemistry at Uckfield Grammar School (Organised Science School). Pharmaceutical Councils’ Silver Medal for Practical Chemistry, 1885 ; 1885-1887 Chemist to Messrs. Wright, Idayman, and Umuey, Wholesale and Manufacturing Chemists, London. 1886-1894. Original Work On “ Daphnidinm Cubeba ;” in 1886 Joint Paper (see Yeay-Book of Pharmacy), Braithwaite and Pam ; 15 Original Papers (Farr and Wright) on Alkaloidal Drugs, their Standardisation and Esti- mation by Gravimetric and Volumetric Methods (see Phamt.Jownal, Chemist and Druggist, and Year-Book of Pharnzucy, 1890 to 1894). Wyndham R. Dunstan. John Attfield. M. Carteighe. Alfred H. Allen. Chas. Uniney. W. A. H. ATayloy. Fauvel, Charles James, The Laboratory, Cranford, Middlesex. Mining and Metallurgical Engineer and Assayer. Formerly of the Cape University. Ten years engaged in Metallurgical and Minera- logical Research in connection with the recovery of Gold from its ores, and in the application of Chemistry to Mining and Metallurgy. Member of the Institute of Mining and Metallurgy, &c. P. Gerald Sanford. H. Bailey. D. A. Louis. Arnold Philip. W. C. Roberts Austen. Frederic Jas. JI. Page.X.Heybert Cox.Fielding, Patrick Joseph D., S, St. Joseph’s Place, Cork. Pharruaceu tical Chemist. Member of the Pharmaceu tics1 Society. Fifteen years with the firm of Messrs. Harrington, Cork. Member of Society of Arts. Chemical educafion at Queen’s College, Cork, under Professor Maxwell Simpson. William B. Harrington. Henry V. Alford, M.D., Lond. Thoinas Farrington. Eugene MacSwiney. Chas. Rl. C. Tichhorne. Eldmard Whitley Allson. Patk. T. O’Sullivan, MS., B.Ch. Daniel J. 0. Mahony. Maxwell Simpson. A. E. Dixon. R. E. Dornn. H. N. B. Richardson, B.A. J. Emerson Reyitolds. Foakes, Jervis E., Medical School, Caxton Street, Westminster. Analytical Chemist. Chief Assistant to nr. DuprB, F.R.S. In Chemistry .-Has worked nearly 8 years with Dr.Duprt5, F.R.S., latterly Chief Assistant. Has been employed by the Medical Depart- ment of the Local Government Board to assist Dr. Duprb: in a research on Micro-organisms. Previously studied Chemistry at King’s College, London, under Professor Bloxam and Professor Thomson. In Engineering : Has studied Mechanical and Electrical Engineering for 6 months with Professor Ayrton, F.R.S., and Pro- fessor Perry, P.R.S. Has served a 3 years’ apprenticeship in Mechanical and Electrical Engineering at Messrs. Henleyv’s Tele- graph Works, North Woolwich. Has worked with Mr. D. K. Clark, M.I.C.E., 1year, experimenting on Sewage, with machinery of which Jlr. Clark and he were joint inventors and patentees. A. DuprB. X. Sprengel. John M. Thomson.H. Wilsoii Hake. Otto Hehner. ?V.J. Dibdin. Fox, Stanley, 23, Soutli Road, Faversham, Kent. Chemical Analyst to the Cotton Powder Company, Limited, Faver- sham. Two years studied Chemistry and Practical Chemistry in the School of the Pharmaceutical Society, and afterwards worked during one session in the Research Laboratory of the Pharmaceutical Society. Wyndham R. Dunstan. John Attfield. 31. Carteighe. G. French. P. Gerald Sanford. E. F. Harrison. Gardner, James, 80, Heaton Terrace, Middleton, near Manchester. Manufacturing Chemist. Three years Assistant Chemist to Messrs. S. Schwabe &-Co., Calico Printers, &c., Rhodes, near Man- 189 chestsr. Articles (three years). Served under Mr.Estcourt, P.C.S., F.I.C., City Analyst for Manchester, and Analyst for Lancaster, Oldham, &c. Three years Chemist to Messrs.J. F. Hill & Co., Calico Printers, &c., Bowker Eank Print Woi-ks, Dlwnchester. Charles Estcourt. T. H averson Estcourt. C. Harq-Bowes. C. Francis Young. George H. I€wst. Wm. T. TlLompsou. Graham, Edward, D a1 ton Hall, Man ches ter. Research Student in Chemistcry. Four years in Chemical Labora-totbies of the Owens College. B.Sc. with Honours in Chemisbry, Victoria University. During past session has conducted a research ‘‘ On the Duration of the Flame of Explosions ” under Professor llixon. Harold B. Dixon. Arthur Harden. W. El. Perkin, jun. Gilbert J. Fowler. P. J. Hartog. Grossmann, Edward Henry, 12, Alfred Place West, S.W. Assistant to Dr.Hake at the Westminster Hospital Medical School. Associate of the Royal Cclllege of Science, London. One year and 8 months with Dr. Hake as above. H. Wilson Hake. A. DuprB. Wm. Macnab. Chapman Jones. William Tate. Otto Hehner. William.A. Tilden. Hall, Henry Arthur (The Rev.) M.A., The Schoolhouse, Totnes. Teacher in Science, under the Technical Committee of the Devon County Council, and Head Master of Totnes Grammar School. Student at the Chemical Laboratory, Oxford. Science Master, St. Edward’s School, Oxford. Local Lecturer in Theoretical and Practi- cal Chemistry, undev the auspices of the Devon County Council. Science Master at Totnes School. V. H. Veley. W. W. Fisher. John Watts. H. T. Gerrans. J. E.Marsh.Hanes, Edgar Septimus, 108, Alexandra Road, St. John’s Wood. Lecture Demonstrator, Clifton College, Clifton, Brist,ol. Associate of the Institute of Chemistry. Joint author of paper on “ Azo-com-pounds of the Ortho-series.” Part I11 (Tram. of Chem. Soc., 1894). R. Meldoln. W. A. Shenstone. Charles R. Beck. R. C. T. Evans. Gerald T. Moody. Martin 0. Forster. William J. Pope. Harrison, C. E., 53, Lansdowne Road, W. Analytical Chemist. Passed special examination in Chemistry for degree of B.A., 1st class, 1892, having attended lectures and practical classes at Caius College, and University Laboratories, Cantbridge, 1889-92. Articled pupil to Dr. A. DuprB, P.R.S., January, 1892-January, 1895. A. Dupr6. H. Wilson Hake. Wm.Macnab. TV. Kell?zer, Otto Heliner.. Wiiliam A. Tildeii. Chapmun Jones. Henderson, James, 193, Blackness Road, Dundee. Research Student, University College, Dundee. B.Sc., St. Sndrew’s University. Author of the following papers :-In con-junction with Professor Walker, D.Sc., Ph.L>., &c. (a.) “ Halo-gen Estimation in Organic Compounds” (Chem. ATews7 1895, 71, No. 1840). (b.) “ Electrolysis of Potassium Allo-ethyllc Cam-phorate ” (J. Chem. Soc., 1895, 40, 337) ; also in conjunction with Professor Frankland, F.R.S., B.Sc., Ph.D. (c.) “ Some Ethereal Derivatives of Sarcolactic acid ” (Proceedings of the Chemica’l Society, 1895, KO. 150, 54 ; Forster Research Scholar, University College, Dundee, 1893-94. James Wa1 ker. Thomas Purdie.Percy F. Frankland. Fred. J. Hambly. Frank W. Young. James R. Appleyard. Heriot, Thomas Iiawkins Percy, 23, Wolseley Road, Crouch End, N. Analytical Chemist. Two years articled pupil to Mr. R. H. Harland, 37, Lombard Street, and subsequently for 6 years his assist- ant. At present engaged as analjst to Messrs. Welford and Sons, Limitsd. R. H. Harlanci. Otto Hebner. Fredl;. J. Lloyd. J. Parry Laws. Bet rm-d Dyer. 191 Hillard, Frederick Arthur, 1, Upper Tichborne Street, Leicester. Schoolmaster, B.A., Oxford (2nd class Nat. Sc. Honour Schools, 1894), Int. B.Sc. Loiidon, 1893. Head Master of Scieiice Depart- ment Wpggeston Schools, Leicester. Lecturer in Chemistry, Wool- Ilyeing, and General Biology in the Leicester Technical Schools.V. H. Veleg. W. W. Fisher. John Watts. J. E. Marsh. J. A. Gardner. Holme, Arthur Edward, M.A., Oxon, 3, Ash Terrace, Saville Town, Dewsbury. Schoolmaster. Educated at Blanchester Grammar School, Open Scholar, Wadham College, 1877. Graduated B.A. First Class Honours Mathematics, 1880; First Class Honours Natural Science, 1882. Proxime Accessit Junior Gniversity Mathematical Scholar- ship 1879. Mathemetical and Science Master, Manchester Grammar School, 1882-87. Chief Physics Master, 1888-89. Head Master Dewsbury Grammar School, and G hie€ Teacher of Chemistry therein. 1880-95. Francis Jones. R. L. Taylor. C. L. Barnes. Julius R. Cohen. Arthur Smithells. James, Alfred, 18, St. Andrew’s Drive, Pollockshields, N.B. Metallurgical Chemist.For some years Chief Chemistl, and now Technical Manager to the Cassel G. L. Go. Limited. Has been engaged on the Electrolysis of Chloride Solutions, the exploitation of the Cyanide process for dissolving Gold from Ores, and on the manu-facture of Cyanides by fixation of Atmospheric Nitrogen. A. K, Huntington. Walter G. McMillan. James Mactear. John J. Beringer. John S. MacArthur. George Beilby. Cornelius Beyingel.. R. R.Tatlock. Edrnund J. 2clills. Johnson,Frederick Edward, 16, Stanley Terrace, West Park, Hull. Director of and Chemist to E. and H. Allison, Limited, Manu-facturing Chemists, Hull, student with James Baynes, Esq., and G. Carr Robinson, Esq., of Hull, and of Professors Attfield, Bentley, Dunstan, and Redwood, in Londan.Associate of the Pharmaceutical Society, and Member of the Pharmaceutical Society of N.S.W. John Attfield. G. Garr Robinson. Jas. Baynes. Wyndham R. Dunstan. Thos. Tyrer. 192 Kibble, William Oakes, A.I.C., Norton Villa, Buckhurst Hill, Essex. Chemist. Certificated student (3 years’ course) Finsbury Teclmical College. Chemist to Messrs. W. J. Fraser and Co., Chemical Engi-neers ; New Explosives Company, Stowmarket ; Messrs. Fowler Brothers, Limited, Sugar Refiners. R. Meldola. Bernard Dyer. B. E. R. Newlands. Arthur B. Ling. Julian L. Baker. P. Gerald Sanford. Johm A. R. Newlands. Kinnicutt, Leonard P., Worcester, Mass., U.S.A. Professor of Chemistry, Worcester Polytechnic Institute, Wor-cester, U.S.A.S. B. (M. I. T.) 1875. V. S. D. (HAIE). 1875.--“ An-thracene Pressings.” [Graduating Thesis.] Abstract in Prest’s Bep., 1875, 142. 1878.--(With B. Anscbutz.) “Ein Verswh zur Da,r-stellung der Phenylglycerinsaure ’’ (Ber. d. Chem. Gesell, 1878, 1219). (With same.) “Addition von Bromwasserstoff mitteist einer Losung von Bromwasserstoff in Eisessig ” (Id., 1878, 1221). 1879.-(With same.) “Synthese der Phenylglycerinsaure oder Stycerin- saure ” (Id., 1879, 537). 1881.-“ An Indirect Determination of Chlorine and Bromine by Electrolysis ” (Proo. Am. Acad., 17, 91-93). 1882.-“ The Decomposition of Phenyltribrompropionic Acid by Water” (Anzer. C7zem. J., 4, 25). 1883.-“ Modification of Noack’s Method of Preparing Carbonic Oxide ” (Id., 5, 43).(With 5. U. Nef.) “ The Volumetric Determination of Combiced Nitrous Acid” (PTOC.An?. Acad., 18, 275-276). (With G. M. Palmer.) “The p-Phenyltribrompropioiiic Acid ” (Id., 18, 277--281; Arner. Ckevn. J., 5, 383). “ Rex Magnns ” (Science, 2, 345). Determi-‘a nation of Combined Nitrous Acid” (Amer. Chenz. J., 5, 388). 1884.-“ Report on the Meteoric Iron from the Altar Mounds in the Little Miami Valley, Ohio ” (Seventee& 3ep. Peabody iiaseurn, 381-384). 1885.-(With R. C. Sweetser.) “ Remarks on Schulze’s Process for the Quantitative Determination of the Halogens in Aro-matic Compounds ” (Anler. Chenz. J., 6, 415--416). 1887.-“ Dis-posal of the Sewage of the City of Worcester” (City Engineer’s Beport). Reprinted. Pph. ~vo.,pp. 9. P.Philips Bedson. E’. R. Japp. Wolcott Gibbs. Charles E. Munroe. Henry E. Roscoe. Prederic P. Dewey. Saville Shaw. 193 Mansfield, Walter, Trafalgar House, Brougliton, Manchester. Experimental Chemist and Gas and Chemical Engineer. Studied Chemistry at Manchester Grammar School, Owens College, and in Berlin, Moscow, and Vienna. At present engaged as Research Chemist and partner in the firm of Edwin Mansfield & Sons, Gas Engineers, of Manchester, London, Madras, and Calcutta. Inventor of Plant for making Gas from sawdust, nut shells, sunflower seed shells and all kinds of mineral, animal, and vegetable matter. Designer of apparatus for use in Indian Government Colleges of Science. George J. Allen. Arthur H. Green. H.Follows. A. B. Griffiths. Rowland Williams. Massey, Cecil, Lyndon House, Lenton Boulevard, Nottingham. Analytical and Agricultural Chemist. Author of papers “ On the Composition of certain Soils of South India ” (Chem. News, 71,26l), and other papers in coui*se of publication. Joint author, with Dr. A. B. Griffiths, of a paper, ‘‘ Sur une Leucomaine extraite des Urines dam l’Angina pectoris ” (Cornptes Rendus de l’dcade’mie des Sciences, Paris, Tome 120; and Chem. News: 71, 282). At present time engaged in research work. H. Follows. A. B. Griffiths. Alexander Hay. Robert H. Wilson. Frank Clovies. J. B. Coleman. William Crookes. James Dewar. E. PranklaixL PI ayfair. McCreath, James, Agricultural Laboratory, 4,Lombard Court, E.C. Analytical Chemist.Studied Chemistry in Glasgow with Messrs. Tatlock, Readman, and Thomson. Assistant to Mr. F. J. Lloyd, carrying out for him the Investigations into the Chemistry and Bacteriology of Cheddar Cheese-making. Obtained Scholarship, Royal Agricultural Society, and holds 1st Class Certificate Highland and Sgricultural Society. Fredk. J. Lloyd. R. R. Tatlock. Horatio Ballantyne. C. M. Aikman. J. Augustus Voelcker. Alexander Cameron. Morgan, David James, 10, Northampton Place, Swansea. Undergraduate of St, John’s College, Cambridge. First Open Natural Science Scholar (Chemistry and Physica), 1892, of St. John’s College, Cambridgc. Have worked in the laboratory of Dr. Wm. Morgan, Ph.D., F.C.S., F.I.C., for some time. Otto Hehner. S.Rnhemann. W. Tirrill. William Crookes. William Xanzsny. Peck, Herbert, L.R.C.P., L.R.C.S. Edinburgh, D.P.H. Cam-bridge, Wigan Road, Ormskirk. Medical Officer of Health. Possesses qualifications in Medicine, Surgery, and Public Health, and analyzes Water for the District Councils of Ormskirk and Sefton. Wm. Jas. Orsman. W. Naylor. Edward Sergeant. Alfred Hi11. E.F?.anklancl. Pennington, William Henry, Field House, Rochdale. Manager. Head-Manager of the Dyeiiig and Bleachiq and Silk Departments, John Bright and Bros., Limited, Fieldhouse Mills, Roch-dale. Lecturer on Chemisty, Rochdale Co-operative Society’s Science Classes, 1883-86. Formerly Student of 0wens College and the Manchester Techiiical Schools. Passed 1st Class in applied Chemistry, Owens College, 1893.Arthur G. Green. C. Rawson. William Marshall. Thomas Stenhouse. Robt. W. Oddy. Ernest Bentz. R.Lloyd Whiteley. Wm. A. IGaiqht. Priest, Martin, Apothecaries’ Hall, Blackfriars, Analyst. Three years under Professor Meldola, FinEbury Techni- cal College, 1888-91. Assistant to W. A. Shenstone, Esq., F.I.C,, Clifton College, 1891, May, 1893. Assistant to Wni. Chatfaway, Esq., Public Analyst for Hammersmith and Borough of Colchester, May 1893--February, 1894, since which time I have held the ap-pointment of Assistant Analyst to the Society of Apothecaries, London. I was associated 7:ith ?V. A. Shenstone, Esq., in a, paper read before the Cheniical Societ,y, in May, 1893: “ Studies on the formation of Ozone.” R. Meldola.W. A. Shenstone. Frank. L. Teed. Edward Bevan. C. G. Moor. Arthur B. Ling. Julian T. Baker. 195 Ridge, W. T. B., 2, Ashwood Terrace, Longton, Staffs. Teacher, Higher Grade School, Hanley. As student : Studied inorganic and organic chemistry (practical and theory), together with other sciences for 9 years. Honoursman in Chemistry, &c., Science and Art Department. As teacher : Assistant Demonstrator in Cheniistry at the Hanley Municipal Science Schools, 1893-94. TeacEer in Science at the Stoke (1893-4-5) and Tunstdl Science and Techniological Classes, and at the Higher Grade evening classes, Hanley, 1894-95. James A. Audley. Wm. Ha,mpton. R. Hornby. G. G. Quinn. St. J. Gover. Round, William, 45, St.Peter’s Road, Handsworth, Birmingham. Analytical Chemist. Seven years with A. E. Tucker, F.I.C., Analytical Chemist, 35, Paradise Street, Birmingham, four years of wliich time as chief assistant. 1st Class Honours Iron and Steel City and Guilds. 1st Honours Metallurgy Science and Art. 2nd Honoiirs Practical ditto Science and Art. Seven years’ training in Chemistry and Metallurgy and Metallurgical Chemistry. Harry Silvester. Joseph Lones. Arthur Adams. Herbert McLeod. F. E.Matthews. Thomas Turner. Rugginz, William Augustus, 114, Upton Lane, Forest Gate, E. Lecturer and Demonstrator of Chemistry to the Worshipful Com- pany of Carpenters’ Technical Institute and Organized Science School, StratfoTd. Student of Finsbury Technical College, 1886-7-8.Appointed Special Lecturer in Chemistry, 1889-90, to Londun School Board. R. Meldola. Thos. Tyrer. A. P. Laurie. W. Palmer Wynne. Wm. Tate. Seyler, Clarence Arthur, 31, Windsor Terrace, Swansea. Analytical and Consulting Chemist. B.Sc. (Lond.) in Chemistry (Honours), Physics and Mathematics, F.I.C. ;assistant successively to Dr. C. M. Tidy, to Mr. W.Crooizes, F.R.S., and to Dr. W. Morgan, M.D., F.I.C. Interim Public Analyst for the County of Gla-morgan and Borough of Swansea, &c. Author of series of articles 196 on “ Water Analyis,” Chem. Nezos, 70, pp. 82, 104, 112, 140, 151, &c. Otto I-Iehner. William Crookes. William Ramsay. W. Terrill. S. RNhemun.TL. Smith, Mathew, B.A., Aston Hall, Preston Brook, Cheshire.Second Master, and Science Master at Aston Hall. Three years training in laboratory of W.P.K. Stock., F.C.S., F.I.C., County Analyst for Durham; three years training at Cambridge, in Chemistry, for Science Tripos under M. M. Patterson Muir, M.A., F.C.S., &c., and two terms teaching under Science and Art Rules at Knutsford Grammar School, and now Science Master at Aston Hall since September, 1894. Studied science also at Heidelberg, and at Edinburgh University, 1893. W. F. Keating Stock. M. M. Pattison Muir. A. Sheridan Len. Alfred Hutchinson. E. I). Walrond. A. Hutchinson. Stephens, Frank R., (Idris and Co.), Carnden Town. Analytical Chemist. I have been under Dr. Muter for two sessions, also one course at the School of Pharmacy’s Laboratory under ProfeFsor Attfield, and Chemical Lecture under Professor Dunstan.Since August, 1893, exclusively engaged in chemical work in the Laboratory of Messrs. Idris and Co. Special studies :-Bacteriology and Water Analysis. Passed the Major Examination, Ju!~,1893. W. H. Symons. M. Carteighe. C. M. Luxmoore. T. A. W. Idris. J. Hughes. Stone, George, Sydney, New South Wales. Brewer. Chief brewer and chemist to 5. T. & J. Toohey, Sydney, for the last 12years ; five years in conjunction with IJ.C. Daniell, F.C.S., for the same firm. Lahe Assistant to Messrs. Shanell and Sons, Birmingham. Appointed by the Jersey Milk Company, N.S.W., to analyse and report on the crystallisation of sugar and other changes occurring in and after the manufacture of condensed ndk.Selected to analjse and report bacteriologically of ale irnForted to Australia. I urgently wish to avail myself of the reports and periodicals of the Society. L. C. Daniell. Lawrence Briant. Gwilym Evans. wpa.A. Dixon. Henry H. IVhiteheccd, 197 Thorpe, Albert, Charnwood House, Sleaford Road, Boston. Analytical Chemist. Author of papers on “ Monazite, a mineral containing Helium ” (Chenz. News, 72,33) ; “ Recent Analyses of Leucite Basalt from Vesuvius ” (Chew News,72,53) ; “A New Bacterial Pigment ” (Chem. News,72,82), &c. Silver Medallist in Chemistry and Physics. A. B. GrifEths. H. J. Mousley. R. Savory Ladell. W. Herbert Walden. TV. B. Bottornley.Junzes Dewnr. William Cq-ookes. C. T. Kingzett. Tibbals, W. J., 76, Lafayette Avenue, Detrait, Mich., U.X.A. Chemist to the City of Detroit, Michigan, U.S.A. Graduate iii Pharmacy, University of Michigan. Assistant for 15 months at the State Agricultural Experiment Station, Geneva, N.Y. Post Graduate Chemical Studies, University of Michigan, from 1891-1892. Assistant for 2+ years to Professor John A. Miller, Niagara Univer- sity, Buffalo, N.Y. John A. Miller. Albert B. Prescott. Charles Platt. Ernest A 00ngdon. TValter 8. Eaines. Williams, John, Wesley College, Sheffield, Schoolmaster. Second Class Natural Science Tripos, Cambridge. Senior Soier:ce Mast,er at Wesley College. W. Carleton Williams. Charles T. Heycock. Douglas Berridge. Walter El.Joseland. Art hu~Harden. Wingfield, Thomas Rowland, 43, Dorset Street, Bolton. Scientific Brewer. Studied chemistry for the last seven years, three of which were spent at the Manchester Technical School. During the above period the following examinations have been passed: Honours stage in brewing of ths City Guilds ; inorganic and organic theoretical chemistry, in practical inorganic chemistry, first class honours, South Kensington. In addition, I am a member of the Insti- tutes of Brewing of London, and the North of England at Man-Chester, also of Society of Chemical Industry, Manchester Section. William L. Hiepe. Alex. K. Miller. M. 0. L. Whiteside. Thomas Cockerill. Jas. Grant. Goorye H. Hurst. 198 Wright, Harold E., Springhurst, Hartburn, Stockton- on-Tees? Metallurgical Chemist.Head Assistant Chemist under Mr. C. H. Ridsdale, F.I.C.,F.C S.,&c., at the North Eastern Steel Works, Middlesborough, having occupied the position five Sears, entailing the conduct of the whole analytical work during that period, a,nd Assistant for altogether over 11years. First Class in Honours Grade, Iron and Steel Manufacturing, 1888 (City and Guilds). Have conducted investigations on the presence and estimation of arsenic in pig iron, steel, &c.,the composit,ion of various lubricants, &c. More recently, a series of experiments on the consti- tution and “citrnte solubility ” of basic slag in connection with a paper read by MI.. C. H. Itidsdale on the “ Solubility of Basic Slag ” (Cleveland Institute Engineers, January, 1895). Edwd. Riley. J. E. Stead. H. Franklurid. C. H. Ridsdale. A. C. Wilson. X.H. Saniter. Jno. A~chy11 Jams. IXARRISON AND SONS,PRINTERS IN OEDINABY TO HER MAJESTY, ST. MARTIN’S LANE.
ISSN:0369-8718
DOI:10.1039/PL8951100159
出版商:RSC
年代:1895
数据来源: RSC
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