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Proceedings of the Chemical Society, Vol. 10, No. 139 |
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Proceedings of the Chemical Society, London,
Volume 10,
Issue 139,
1894,
Page 111-129
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摘要:
PROCEEDINGS OF THE CHEMICAL SOCIETY. No. 139. Session 1893-94. May 17th, 1894. Dr. Armstrong, President, in the Chair. Professor D. MendelBef, of S t. Petersburg, Foreign Member of the Society, being present signed the RolI of Fellows. Certificates were read for the first time in favour of Messrs. Cecil Cooke Duncan, Royd Agricuitural College, Cirencester ; Bhirkaji Edalji Ghasvda, Tardes, Bombay ; Donald Gordon Forbes, Shilling- stone, near Blandford, Dorset; Richard s, Ladell, 21, Lower Gros-venor PIace, S.W. Of the following papers those marked * were read:- “17. “The influence of moisture on chemical action.” ByH. Brereton Baker, M.A. Since the publication of a note in the Procekdings (May 4th, 1893) further inrestiptions of the actions there menfioned have been made.Sulphur trioxide does not combine with highly purified lime; but a trace of moisture brings about vivid incmdescence. Dry copper oxide is also without action on sulphur trioxide. Purified and dried lime does not decompose dried ammonium chloride, which may be sublimed from the mixture without evolving any ammonia. Purified and dried nitric oxide gives no brown fumes with dried oxygen, but a trace of moist air cauYes them to appear at once. A mixture of purified and dried hydrogen and chlorine can be exposed to daylight for fom days without more than three-fourths of the gases combining. Ammonium chloride, heated in a vacuum in a soft glass tube, leaves a residue of ammonia gars; but when dried and heated in a hard glass tube, no gaseous residue is obtained.This led to the investigation of the vapour density of dry ammoninrn chloride, which was shown to be 112 normal, 28.7 being the mean result of six experiments. With regard to the theory of the subject, the author believes that an electro-chemical hypothesis is applicable. Separation of dried ammonia and hydrogeri chloride gases takes place when plates with opposite electrical charges are introduced into the mixture though the action cannot be electrolytic, since discharge is, under the circumstances, impossible. Similar separation was noticed with air and with a mixture of dried hydrogen and oxygen. Electric discharge, when not of high tension, will not pass in dried gases; but the high- tension discharge does pass, and renders it possible for the low- tension discharge to pzss afterwards.With regard to the influence of moisture, it, appears that a-hat holds for chemical combination holds also for electrical discharge, and that there is great significance in the apparent similarity in the two cases. DI sc USSION. The PRESIDENTspoke of Mr. Baker’s results as of great value and as calcnlated to convince all of the important influence exercised by moisture in promoting very many chemical changes; he had long been satisfied that the presence of an electrolyte was essential to every chemical change, and that water was of service bwsuse it gave rise to an electrolyte. It was now important to ascertain whether other substances besides water could condition the formation of electro-lytes and thus co-operate in producing change, and to determine what their nature was ; probably water was one of very few substances able to act in tlhis manner, if indeed it were not the only one.In the case of hydrogen and chlorine, there was reason to think, as Mr. Shenstone had indicated, that some substance other than water was also essential to the occurrence of change. He was glad to hear Mi-. Shenstone say that he was not yet satisfied fhst pure oxygen can be ozonised ; his statement that more ozone was obtained from dried oxygen mightdbe regarded as evidence that water influenced its formation ; the amount of ozone finally obtained de- pended on the amount destroyed as well as on the amount originally formed, and if both its formation and destmction were influenced by moisture, it might well be that one action was more directly influenced than the other when but very little moisture was present.If the destruction took place the less rapidly the less water present, the amount finally obtained would be the greater the more carefully the oxygen was dried. Regarding the decomposition of ammonium chloride by heat, a1though moisture would promote its decomposition, the absence of moisture would not have the effect of making it a stable substance at all temperatures ; it might be expected that, if dry, it would decom- 113 pose when heated sufflciently, but would not dissociate; in other worc?~ there woiild be no re-formation of ammonium chloride under such cotidi tions.Mr. SHENSTONEwasglad to find that Mr. Baker's resnlts had confirmed his own earlier experiments on the production of ozone from oxygen and on the action of ozone on mercury. At the same time he was not yet himself convinced that really dry oxygen would ozonise, and he was at present studying the influence of moisture on the forma- tion of ozone from oxygen qnantitatively. He expected the character of the curve obtained would settle the question. He could also, from the results of many experiments, confirm Mr. Baker's statements as to the persistent activity of highly dried chlorine towards certain subtnnces. Its action on mercury, for example, was often apparently independent of dryness.In fact, the results obtained pointed to the presence of some other substance than water, as being able to influence the action of these two sub- stqnces. This had led him to search for a more satisfactory source of chlorine. *18."New voIatiIe compounds of lead sdphide." By J. B. Hannay. Early experimenters, notably Pattinson, Regnault, and Jordaii, have noticed the volatilisation of lead sulphide in water vapour and its subsequent crystallisation, but their results in other respects seem to be irreconcilable. An investigation showed that all the phenomena described are easily ucderstood, on the supposition that both water and sulphur dioxide tombine at high temperatures with lead sulphide, forming gaseous compounds.When difference of temperature is taken into account, it is found that water vapour reacts with lead sulphide in the following manner. 1. About 750".., ..... PbS .tH20 = PbO*H2S 2. ,, 90V........ 2Pb0 + 2PbS = 3Pb + PbS,O, 3. ,, 1400" ........ PbS + HZO = PbS*H,O Neither of the first two changes is complete, but in each the sulphide is decomposed. In the third rea'ction, however, there is no decomposition, and the sulphide is redeposited on cooling. Reasons are adduced for the conclasion that a definite molecular compound PbS*H,O exists. Similar indirect evidence is given to demonstrate the existence of the compound PbS,S02, or PbS& Both these compoiinds are colourless gases at a rsd heat, but when the temperature falls decorn-position occurs.This remarkable fact is explained by the observation 114 trhat the oxygen of sulphur dioxide and of water displaces the sulphrir of the lead sulphide temperatures near 800°, whilst at higher tempe- 1-atures, such as 1400°, both sulphur dioxide and water combine wit.h lead sulphide, and redeposit it on cooling. DISCUSSION. after remarking that the subject brought forward by Mr. Hannay evidently gave abundant opportunitg for discussion, the PRESIDENT said that, assuming that a volatile compound of the formula PbS-SO, existed at high temperatures, the properties assigned to it by Mr. Hannay were not of the unique character he appeared to suggest ; numerous cases were recorded of compounds which underwent change as the temperature fell, but probably this was due, not to their intrinsic instability, but to the tendency of such molecules to interact among themselves.At high temperatures lead sulphide might consist of simple (di-atomic) molecules capable of combining with those of other substances, while at lower temperatures such molecnles might associate, forming galena, which probably was a polymeride of the compound PbS. The extrusion of oxygen from molten silver and of carbon dioxide on freezing soda water, might be regarded as cases comparable with those brought forward by Mr. Hannay, and such an explanation would apply to them. Professor ROBERTS-AUSTENsaid that the metallurgy of lead pre- sented many peculiarities. One of these is the necessit,y of condens-ing volatile products of the reactions which had led smelters of lead ores to construct condensing flues which might, reach a mile in length.The author of the paper would, therefore, be doing good service if he added to our knowledge of the condensible products formed during lead smelting. Rut the question arose, Had the author of the paper established the fact that water vapour and sulphurous anhydride really carry away sulphide of lead in molecular propor-tions ? There are, as the President had said, many instances of com-pounds which are stable at a high, and unstable at a low, temperature, and this is a point in ivh. Hnnnay’s favour, but the extyeme solvent action of Iit,harge itself must, not be forgotten, and litharge, more- over, absorbs oxygen when fluid, and evolves it Rgain on solidifica-tion ;the effects observed by Mr.Hannay may, therefore, be in some way connected with the solvent action of litharge. It appeared to the speaker that the evidence given by the author of the paper as to the existence of volatile compounds of sulphide of lead and sulphurous anhydride were of the most slender description. If it were possible to obtain evidence as to the vapour density of the yolatile products, that would, of course, settle the question, but the author’s main evi- dence appeared to rest on observations made by looking along a red- 115 hot tube, and recording whether certain vapours did or did not form as the temperature is varied. It appeared that Mr, Hannay had .not even satisfied himself that when the alleged com-pounds are cooled down and become unstable they yield their constituents in exactly the proportions demanded by his theory.The evidence afforded by the composition of the “lead fume” which accumulates in the condensing dues is not without import- ance, but, upon this point, Mr. Gowland would state the results of his expeiience. Professor Austen gathered that Mr. Hannay objected to the accepted equation PbS04 + PbS = ZSO, + 2Pb, on the ground of the comparative infusibility of the sulphide and sulphate of lead, but it, must be remembered that many sub-stances interacted by “ fritting ” at temperatures well below their melting point. Percy’s statement as to the separation of lead, under the conditions represented by the equation, was very definite, and Dr. Percy was very careful, and did not make such statements except on the clearest experimental evidence.The action is, however, an endothermic one, aud it would certainly be well to re-examine the conditions with great care. Assuming that the accuracy of the accepted equation PbS + BPbU = 3Pb + SO, (which is less endo- thermic than the first) can be maintained, surely the fact that lead is the result of the reaction, points to the instability at a red heat of Jfr. Hannay’s compound of sulphide and oxide of lead. Lead sulph- ide and lead oxide had long been known to be volatile at moderate furnace temperatures, and chemists must certainly have more evidence than that now presented to them before they could accept Mr.Bannay’s conciusions. Mr. GOWLANDdid not think that Mr. Hannny had given us suffi-cient proof that a substance of the formula PbS,O, exists ; he does not appear to have isolated it, neither has he shown adequate grounds for regarding it as a product of the smelting of lead sulphide. The conditions of Mr. Hannay’s experiment are not similar to those which occur in the reverberatory furnace in actually smelting lead snlphide. It is generally admitted that the two compounds formed in this operation, viz., lead oxide and sulphate, are volatile in a current of air (see Percy’s Metallurgy of Lead, pp. 15-42), and that these substances are the chief constituents of the volatile products condensed in the flues of the smelting furnace.Again, if the lead lost by volatilisation is volatilised as PbS,O,, the volatile products which are condensed in the flues as “ lead fume ” should consist mainly of it, or of the product of its decomposition-lead sulphide. This is, however, not borne out by analyses of “ lead. fume.” In a tlpical specimen, analysed in Percy’s laboratory, the lead, sulphur, and oxygen existed in the following proportions : Pb, 68.47 per cent. ; S, 11.25 per cent. ; 0, 20.28 per cent., whereas, if the fume had consisted of PbS20,, or its products of decomposition, these propGrtions should have been Pb, 68.32; S, 21-12; 0, 10.56, or Pb, 86.61 ; S, 13.39, or some intwmediate proportion. Until further proof of the existence of FbS2CI, has been obtained, we have not sufficient grounds for setting aside the old explanation of the chemistry of lead smelting as set forth by Percy and other distinguished metallurgists.Mr. A. G. BLOXAMstated that some recent experiments at the Goldsmiths’ Institute had shown that galena could be volatilised in both hydrogen and nitrogen. The mineral was heated in a porcelain tube situated in a furnace very similar to that depicted by Mr. Hannay, so that it seemed fair to conclude that the temperature attained was approximately the same as that at which Mr. Hannay worked. The gases were purified by passage through (1) silver nitrate solution, (3) alkaline permanganate solution, (3) red-hot copper, and (4)columns of quicklime and of phosphorous pentoxide.The text-book statement that galena could be volatiiised in hydrogen, forming some hydrogen snlphide, was confirmed. In the case of heating in nitrogen, large crystals of galena weie afterwards found in the cooler part of the tube, and a sublimation of sulphur was notded. Mr. HANNAYsaid, in reply to Professor Roberts-Ansten, that the discussion showed how much this difficult subject required to be con- sidered before a true appreciation of the evidence could be arrived at. The last experimental work on the subject was done in 1830. As to the evidence establishing the existence of the compounds being in- sufficient, a study of the paper would show that all the reactions are quite definite, and that the analysed CO agree with the composition given.The paper did not deal with lead smelting, and some of the dia- grams exhibited merely showed the part played by the new volatile compound in certain reactions. In reply to Mi*. Gowland, Mr. Hannay pointed out that lead sulphate is not volatile at the temperature of the smelting furnace, and t,hat the flue-dust, to which reference was made, was simply the product of oxidation (or partial oxidation) of the volatile compound PbS202,which is formed in the furnace. As PbS20zdecomposes on cooling, it is useless to look for it in the flue-dust ; we only find its products of decomposition. It would be very difficult to determine its vapour density. The speakers in the discussion seemed inclined to adhere to the old equation PbS + Oo= Pb + SO,; but this equation seemed to 117 be only hypothetical, and unsupported by experimental proof.As the subject evidently required Eurther elucidation, Mr. Hannay promised to prepare a paper dealing minutely with this part of the metallurgy of lead. In reply to M-r. Bloxam, Mr. Hannay stated that it is quite true that minute quantities of lead sulphide are volatilised by all gases, but the action of water and sulphur dioxide brought about a, sudden and copious evolution of fumes, and the composition of these fumes could be represented by a definite molecular proportion. 19. ‘I Notes on the cupellation of bismuth-silver alloys.” ByErnest A. Smith, Assoc. R.S.M. The loss of silver in the cupellation of lead-silver alloys has been the subject of a large number of experiments at various times, but comparatively few results have been published on the loss of silver in the cupellation of bismuth-silver alloys.A series of experiments was made some years ago by Mr. Hambly (Chem. Gaz., 1836, pp. 185-6) on the cupellation of lead-silver alloys, which prove that, according to the decrease of weight of the silver cupelled, so the loss of that metal very slightly increases, provided the ratio of lead employed be constant. His results also confirm the fact that an increasing ratio of lead produces an increasing loss of silver. The present experiments were made to ascertain whether the loss of silver by cupellation was the same when varying quantities were employed with a constant ratio of bismuth in the place of lead, and also to find the loss of silver when cupelled with a gradually in- creasing ratio of bismuth.The bismuth and the silver employed were specially purified. The temperature was slightly lower than that usually adopted in the cupellation of lead-silver alloys. Mr. Hambly concluded that, provided a constant ratio of lead and silver be employed, the loss of silver very slightly increases accord- ing to the decrease in the weight of the silver cupelled. The author finds that a very much greater loss takes place under the same conditions when bismuth is present instead of lead, although the ratio of the loss appears to be about the same. The results confirm the fact, already known, that an increasing ratio of lead or bismuth produces an increasing loss of silver, the loss, however, being very much greater in the case of bismuth.As the loss of silver by volatilisation during cupellation is altogethey inconsiderable, unless the temperature at which the operation has been conducted has been much too high, the loss is evidently due to the fact that silver is absorbed by the cupel. 118 20. ''Azo-p-cresol derivatives." By R. Meldola, F.R.S.,and F. Southerden. The reduction of the acetyl-derivatives of oxyazo-compounds of the ortho-series has been shown to give ambiguous results so far as concerns the question of the constitution of these compounds (Meldola, Hawkins arid Burls, Trans., 1893, 923).An attempt was therefore made to solve the problem by the more direct method of decomposing the acetyl-derivatives by means of nitric acid or bromine. In the case of the alkyl-derivatives of benzeneazo-/3-naphthol, the nitric acid method gave a definite indication that the alkyl group is hydroxylic and not amidic (Meldola and. Morgan, Trans., 1889, 608). In the case of the acetyl-derivative of benzeneazo-P-naphthol, nitric acid appears to act simply as a nitrating agent (ibid., 609). We have applied the same method to some ortho-azo-derivatives of p-cresol, and the results are submitted in the present note. Paratalueneazo-p-cresol was prepared and acetylated (Nolting and Cohn, Ber., 1684, 354). The acetyl-derivative, on reduction with zinc dust on acetic acid, gave, as the only definite product, acetopara- toluide.Acetamido-p-cresol may have been formed, but lost by oxidation during the treatment necessary for the isolation of the acetoparatoluide. Resinous colouring matters are formed during the evaporation of the solution by the oxidation of some unstable com- pound resulting from the reduction. The original compound (para- tolueneazo-y-cresyl acetate) is brominated by the action of bromine, but the nzo-group is not split off and no separation of the molecule takes place, as, e.g., in the case of benzeneazo-P-naphthylamine. Benzeneazo-p-cresol was acetylated (Nolting and Cohn, Bz~~T.,1884, 953) and the product, dissolved in glacial acetic acid, was allowed to stand for two or three days with an excess of bromine.A crystalline substance slowly formed, which, after repeated crystallisation from glacial acetic acid and finally from alcohol, formed golden-brown needles with st silky lustre, melting at 168". hnalysis proved the compound to be a dibromo-derivative of beimeneazo-p-cresol. Calcu-lated for C,,H,,Br,N,O ; Br:43.24 per cent., N, 7.57 per cent. Found, Br, 43-50 and N, 7-64per cent. The acetyl-group thus splits off under the influence of bromine; the azo-compound simply becomes brominated, and, as no separation of the molecule takes place, the products were not further investi- gated. Parachlorobenzeneazo-p-cresolwas prepared in the usual way by mixing a solution of diazotised parachloraniline with an alkaline solution of paracresol.The prodnct, when purified by crystallisation from alcohol and benzene in successiofi, forms flat, golden-orange 119 needles, melting at 155”. The compound appears to exist also in another crystalline form, as the rapid evaporation of the benzene solution gives rise to a deposit of small, opaque, ochreous needles, having the same melting point. The purity of the compound was ascertained by analysis. Calculated for (p)Cl*C,H4*N2*C6H3(CK,)*OH [N, : CH, : OH = 6 : 4 : 11; C1, 14.43 and N, 11.36 per cent. Found, C1, 14-46 and N, 11.45 per cenf. The ace tlyl-derivatire was prepared by boiling the foregoing com- pound with excess of acetic anhydride for about 20 hours. After crystaljisation from alcohol, it forms orange needles, melting at 120”.Calculated, C1, 12.51 and N,9.61 per cent. Found, C1, 12.46 and IS,9.78 per cenc. As bromine had acted on these compounds merely as a bromin-ating agent, the substance was acted upon by nitric acid of various strengths and under various conditions. Nothing of the nature of a nitrated aniline, acet anilide, amido- or acetamido- cresol was, how -ever, obtained Nitric acid appears to nitrate the azo-compound as a whole, forming a yellow, uncrystallisable product, apparently of the same nature as that resulting from the nitration of benzeneazo-P-naphthyl acetate (Trans., 18~9,609). 21. ‘I Effect of heat on iodates and bromates.” By Ernest H. Cook, D.Sc. This paper is the first instalment of an account of the experiments made upon the effect of heat upon iodates and bromates.It deals with potassic iodate and bromate. Details are first given of the methods of purification of the reagenh used. Exceptional difficulties were experienccd witb potassium iodide, and the ordinary methods of purification adopted were shown not to yield a sufficiently pure product. The paper of Robineau and Rollin (J. €‘harm. [5], 26, 485-490), in which they state that “all acids, even carbonic anhydride in presence of air and moisture, decompose potassic iodide,” is quoted, and a series of experiments to test the truth of this state- ment are detailed. The results obtained show that the statement is only partly true. The methods adopted for the analysis of the oxy-salts are then given.These were of t.hree kinds :-(1) Digestion with potassic iodide and hydrochloric acid ; (2) reduction by sulphurous acid ; and (3) reduction by the copper-zinc couple. These methods are com-pared and the precautions necessary for success are stated. In the first it is shown that accurate results can only be obtained when a blank experiment, with potassium iodide and hydrogen chloride is cctrried on side by side with the principal one. Potassic iodate is difficult to purify ; repeated crystallisations from 120 water fails to give a reliable product. The method adopted was, therefore, to crystallise from water once or twice, then to precipitate the solution by means of alcohol, collect the precipitate and recrystal- lise from water.The first effect of heat on the iodate is to cause the substance to become brown. This brown substance has the same com- position as the original iodate, and it is formed without any alteration taking place in weight. When the heating of the iodate is continued up to the time of its ceasing to lose weight, the following changes are observed : the brown substance fuses and becomes a colourless liquid, during the fusion, iodine is evolved ; after continued and regulated heating, the liquid becomes a white solid, and when thoroughly solid, ceases to lose weight ; the residue is potassium iodide. The next point, studied was the partial decomposition of the iodate. The salt was heated for varying periods, the amount of loss ascer- tained, and the residue analysed.The results showed that no other oxy-compounds were formed at any stage of the process. Potassium bromate was next experimented with, the total decompo- sition of the salt by heat as well as the partial decomposition being studied. No change of colour occurs with the bromate, but the salt decrepitates at about 180" C. During the decrepitation bromine is evolved, but at no other stage of the process. The salt fuses to a colonrless liquid, from which oxygen is steadily evolved ; the residue consists of potassium bromide. The partial decomposition indicated the presence of breaks in t'he rate of evolution of the oxygen ; these were shown to be due to the mode of heating, and not to definite chemical reactions.The residue consists of a mixture of bromate and bromide. These experiments having failed to produce any oxy-compounds, it was thought that these compounds might be formed if the heatiug were effected under reduced pressure ; but at a pressure of 30 mm. the results were preaiseiy the same as under normal conditions. Finally, in order to discover at what stage the chlorine known to be evolved when chlorate is heated is produced, experiments were made with that substance. It was found that the chlorine was evolved just at the same period as the iodine from the iodate, viz., during the melting of the salt. The amount formed is 0.03per cent. It mould, therefore, appear that the halogen is liberated early, but that it is not actually set free until the structure of the salt is broken down-in the case of the iodate by fusion, and in that of the bromate by decreoitation.121 ADDITIONS TO THE LIBRARY. I. Donations. Engineering Chemistry ; compyising Methods of Analysis and Valuation of the Principal M-aterials used in Engineering Work. By H. J. Phillips. London 1894. From the Author. Transactions of the Sanitary Institute. Vol. XIV, 1893. London 1893. From the Institute. Rothamsted Jubilee Fund. Report of the Executive Committee ; with an Account of the Proceedings at the Commemoration of the Jubilee of the Rothamsted Experiments, July 29th, 1893. London 1894. From the Committee. Pamphlets from the Authors. Ueber colloidales Gold, von P.Schottlander (Verh. Gesells. deut. Natnrforscher u. Aertzte). Niirnberg 1893. De 1’Emploi du Sulfate de Magn6sie cornme Engrais. Par E. Silz. Paris 1890. RESEARCH FUND. A meeting of the Research Fund Committee will be held in June. Fellows who desire grants are requested to send in their applications to the Secretaries at Burlington House, not later than Tuesday, June 5th. At the next meeting of the Society, on Thursday, June 7th, 1894, there will be a ballot for the election of Fellows, and the following papers will be rend :-“ The nature of phospborescence.” By Herbert Jackson, B.Sc. “ The crystallography of the normal sulphate of potassium, ru-bidium, and caesium.” By A. E. Tutton. “The boiling poiuts of homologous compounds. Part II.” By Dr.James Walker. CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. JUNEith, 1894. N.D.-The names of those who sign from “ General Knowledge ” are printed in italics. Dixon, George, Trinity College, Cambridge. Research Student. B.A. Trinity College, Cambridge. Honours in Natural Sciences, Tripos, 1893. Assisting Messrs. Easterfield and Sell in investigations upon the derivatives of pyridine. W. J. dell. T. H. Easterfield. J. T. Hewitt. Alexander Scott. H. J. H. Fenton. Donald, George, Arnold Printworks, North Adams, Mass., U.A. Printworks’ Chemist. Three years a bnrssr in the Young Laboratory, Glasgow; nine months Chemist in Loch Katrine Dis-t’llery, Glasgow ; four years Chemist in Lennoxmill Priniworks, by Gliisgow ; eight years Chemist in Arnold Printworks.Joint author (with Professor Mills) of a paper “ On the Action of Oxides 0x1 Salts ” (Chern. Xoc. J., 41, 1882, 18). Edmund J. Mills. A. G. Perkin. Wm. McD. Mackey. Archibald Walker. A. Humboldt Sexton. Eumorfopoulos, Nicholas, 1, Kensington Park Gardens, W. Student. Student in University College. B.Sc. University of Loiidon. William Rnmsay. J. Norman Collie. James Walker. John Shields. Temple Orme. Morris W. ‘l’ravers. Flintoff, Robert John, Haxhy. Crumpsall Lane, Crumpsall, Manchester. Printworks’ Chemist. Educated at t,he Manchester Grammar School and Owens College, worked in Professor Dixon’s Laboratory, 123 and with Mr. Ernest Bentz, Lecturer on Technical Chemistry.On leaving college was appointed Chemist to Messrs. T. and D. Southern, Manufacturers of sulphuric, hydrochloric, and nitric acids. After-wards became Chemist to Messrs. Grimshaw and Bros., Limited, and in that capacity wwked on the purification of sewage and waste efflu- ents, also on the manufacture of the basic per. salts of iron. Am now Chemist at Messrs F. Scott and Uo., Calico Printers, Littleboro’, and am engaged at present upon the production of “ azo ” colours directly upon the fibre. Harold B. Dixon. Harry Grimshaw. Francis Jones. G. H. Bailey. Arhhur Harden. P. J. Hartog. Gilbert J. Fowler. W.H, Perkin, jun. Hadley, Arthur, 226, Monument Road, Edgbaston, Birmingham. Brewer &nd Brewer’s Chemist, at Mitchell’s Brewery, Cape Hill, Birmingham.Honours in Chemistry, Science and Art Examination, and other passes. Honours in Brewing, City and Guilds Examina- tion, 1892 and 1893. Student at Mason’s Science College, Birming- ham, and Institute ; also Birmingham Municipal Technical School for some years. William W. Butler Jno. W. Alcock. Geo. E. Perry. Thomas Edwards. W. Duncan, F.I.C. H. J. Mousley. Awred Xenthall. G. T.Evans. Harris, Sydney Walters, 15, Lansdowne Terrace, Walters Road, Swansea. Analytical Chemist. Six months studying the analysis of steel in the Laboratory of the Forest Steel Works (Messrs. Wm. Williams & Co.). Subsequently four years with Dr. Wm. Morgan, a Fellow of your Society, and Public Analyst of Swansea, &c., undergoing a course of Analytical Chemistry in all it branches.Am now, and have been for the last two years, engaged as Analytical Chemist and Assayer with Messrs. Richardson & Co., Mineral Importers of this town. Wm. Morgan. W. Terrill. Rhys. P. Charles. Arthur Luty. Otto Hehner. Frank B. Last. Kitchens, J. H., North Devon Lodge, Cheltenham. M.A. Oxon., Senior Science Master at Cheltenham College, late 124 Scholar of Queen’s College, Oxford; Honours in final Art Science School, Burdett-Coutts Scholar, late Science Master at St. Peter’s College, Radley. W. A Shenstone. W.W. Fisher. J. A. Gardner. n. H. Nagel. J. E. Marsh. Bolt, Wilmot, jun., The Park, Didshury, Manchester. Research Student in the Owens College.For four years Student, of Chemistry at the Owens College, having completed course for De-gree in the Honours School of Chemistry. Recently published “ Behavionr of the Alkali Metals under Oxidation ” (jointly with W. E. Sims). Harold B. Uixon. W. H. Perkin, jun. Arthur Harden. G. H. Bailey. Arthur W. Crossley, Gilbert J. Fowler. Hope,Arthur Peach, Salisbury Road, Leicester. Analytical Chemist. Member by examination of the Pbarmacenti- cal Society. Has devoted special attention to the purification of sewage and kindred subjects, particularly the analytical and bacterio-logical examination of water in its relation to sewage contamination. Author and patentee of Hope’s Bacilli Sewage Purification Process now running at Kettering and other towns.Percy F. Frankland. J. W. Slater. Edward D. Gravill. Wallace C. Nickels. T.A. Ellwood. McLeod, James, 2, Gladslone Terrace, Paisley. Chemist’s Assistant. Four years Lecture Assistant to Mr. Charles Manners, jun., F.I.C. ; Analytical Chemist, Lecturer on Chemistry, &c., Paisley. Five years nine months Assistant in Laboratory of Messrs. J. and P. Coats, Limited, Thread Manufacturers, Paisley. G. G. Kenderson. James Robson. Aug. Schloesaer. Thomas Gray. A. Humboldt Sexton. Newth, G. S., 29, iMonnt Park Road, Ealing, W. Demonstrator Royal College of Science, South Kensington. Late Lecturer on Chemistry, New College, Rampstead, and Princess 125 Helena College, Ealing. Author ‘‘ Newth’s Chemical Lecture Ex- periments.” T.E. Thorpe. Chapman Jones. Henry .E. Armstrong. W. Palmer Wynne. Wyndham R. Dunstan. John 31.Thomaon. Nixon, Alfred, 14, Eniwistle Street, Moss Side, Manchester. Principal of the Central Commercial Evening School, University and Special Classes. Lecturer to Teacbers’ Classes and Higher Grade Schools (Science Departments). Lechres arid Practical Work in Mr. Rot’nwell’s Classes, under Sir H. Roscoe at Owens College, and in Materia Medica and Pharmacy at Owens College. Passed the 1st M.B. examination (equivalent to 1st B.Sc.) of the Victoria University in Chemistry, Biology, and Physics. Written and practical work in all subjects. C. F. Seymour Rothwell. Robt. R. Rothwell. R. L. Taylor. George H.Hurst. Joseph Morris. Parker, G. L., The Paddocks, Eccleston, Chester. Mining Engineer and Assayer. Pupil in Laboratory of W. F. Lowe, Assay Office, Chester ; also studied at the Camboriie School of Mines, Cornwall. Assayer and Engineer to the Mashonaland Gold and Land Company. W. F. Lowe. John Rairstow. G. Watney Webster. Edward Kinch. A. J. Greenaway. J.Curter Bell. Pike, E. Brooke, 6, Lathom Road, East Ham. Chemical Assistant at the Northern Outfall Precipitation Works, Beckton, E. For two years a pupil of Dr. DnprB, F.R.S. For four and a half years an Assistant in the Chemical Department of the London County Council under Mr. Dibdin, F.I.C., F.C.S. A. DuprB. W. J. Dibdin. H. Wilson Hake. Prederic Jas. M. Page. Alfred G. Pike. John M.Thornson. Robjohns,Herbert Harold, King’s School, Pont,efract, Yorks. Science Master King’s School, and Science Mmter Town Technical School, Pontefract, 1887-90. Student in Chemical Laboratories, University C3llege of Wales, Aberystwyth, 1891. Lecture Assistant 126 to Professor of Chemiqtry, U.C.W., 1892 onwards, as above. Science Master at King’s School, &c. B.Sc. London. H. Lloyd Snnpe. Arthur W. Warrington. Leonard T. Thorne. E’rank Woodward Branson. W.J.Russell. F.D. Chattaway. Rolfe, John F., Homewood, Leytonstone, Essex. Analytical Chemist. Studied in the Laboratory at University College under Professor Graham, during the Session 1888-89, and during the same year attended courses of lectures, Worked for three years since as a student, and during the last two years as Assistant under Dr.Graham and Mr. Chapman. Have had consider- able experience in chemical work of all kinds. Charles Graham. Alfred C. Chapman. Charles J. Wilson. William Ramsay. John Norman Collie. James Walker. Ryce, George, Rathmore Place, Cork. B.A. Royal University, Ireland. Analytical Chemist. Has studied Chemistry at Queen’s College, Cork, under Professor Maxwell Simpson. Senior Scholar in Experimental Science, Queen’s College, Cork. A 1851 Commission Exhibitioner. At present studying Chemistry at the Royal College of Science, South Kensington. T. E. Thorpe. W. Palmer Wynne. William Tate. Chapman Jones. A. E. Tutton. J. W. Rodger. Shorthouse, Herbert Stephen, 47, Pershore Road, Birmingham.Chemist and Laboratory Manager for Messrs. P. Harris and Co., Manufacturing and Analytical Chemists, Birminghtzm. Have for seveu years been engaged daily in the manufacture of inorganic and organic chemicals and pharmaceutical preparations, and in analysis of commercial articles. Have passed Iron and Steel Manufacture Examination (City and Guilds). Advanced Practical and Theory Chemistry (South Kensington), Scholarship. Honours Practical Chemistry (Inorganic) 1st Class. Harry Silvester. Arthur Adams. William W. Butler. Jno. W. Alcock. Charles Bayliss. Shuttleworth, Professor Edward B., Lecturer on Materia Nedica, Trinity Medical College, Toronto. 127 Formerly a pupil of Professor Sullivan and Sir Robert Kane, Dublin.Doctor of Pharmacy, Trinity College, Toronto. Lately Professor of Chemistry and Dean in the Ontario College of Pharmacy. Was for 10 years Chairman of the Board of Examiners, Ontario College of Pharmacy. Have been Editor of the Canadian Pharmaceutical Journal for 25 years. Aathor of “Preparation of Dialysed Iron” (18767, Canadian Pharmaceutical Journal and Year Book. Lithiumti Benzoate ” (1875), Canadian Pharmaceutical Journal and Year Book. “ New Mode of Preparing Ferric Salts ” (1879)’ Canadian Pharma- ceutical Journal and Yeai- Book ;etc. John Attfield. W. H. Ellis. W. H. Pike. J. Bemrose. WyndhanaR. Dunstan. G. P.Qirdwood. J. Baker Edwards. Smith, Ernest Alfred, 17, Oval Road, Regent’s Park, N.W. Met,allurgist. Assistant Instructor in Assaying, Royal School of Mines, London.Associate of Royal School of Mines. London Honours Medallist, Science and Art Department. Late Chief Assistant to B. Kitto, Esq., F.G.S., F.I.C., Analyst, 30-31, St. Swithin’s Lane. Late Lecturer on Metallurgy and Instructor in Assay- ing, Royal College of Science, Dublin. Member of Society of Chemical Industry. Author of paper on“‘ Presence and Estimation of Gold and Silver in Antimony and Bismuth.” T. E. Thorpe. N. C. Roberts-Austen. W. Palmer Wynne. Bennett H. Brougb. William Tate. Spenzer, John George, M.D.,Ph.D., Cleveland, O., U.S.A., 370, Central Avenue. From 1880-1884 and 1886-1887 Assistant in Chemistry to the Medical Department ; from 1884-1887 Assistant in Chemistry to Literary Department (Adelbert College) of Western Reserve Univer- sity, at Cleveland, Ohio ; from 1887-1891 practising Physician ; from 1891 to the present, Student of Chemistry at the Strassburg University ; from 1881-1891 contributions of Chemical, Pharma- ceutical, or Medical interest, read before and publisheci in the Pro-ceedings of the American A.A.Sciense Amer. Pharm. Assoc. ; Ohio State Pharm. Assoc. ; and Ohio State Microscopical Society. D. R. Fitdig. C. F. Baker. Dr. H. C. Myers. Robert Hellon. Archibald Kitchin. Herbert Ingle. J. B. Cohen. 128 Steel, Robert W., Wedd erburn, Paisley. Chemist. Four years’ College training in Anderson’s College, Glasgow, under the late Professor Dittmar, and latterly Professor Henderson. Over one year and six months with Messrs.J. and P. Coats, Limited, Thread Manufacturers, Paisley. G. G. Henderson. James Robson. Aug. Schloesser. Thomas Gray. A. Humboldt Seaton. Taylor,Herbert John, Fern Villa, 33, Russell Street, Eccles, near Manchesber. Teacher of Chemistry. Two years Laboratory Assistant and Teacher of Chemistry at the Central Hr. Gd. Bd, School, Man- Chester. Student at the Manchester Technical School and Owens College (Evening Classes). Two years Teacher of Chemistry at the Astley Institute, Dnkinfield (Evening Classes). Two years Student in Chemistry at the Normal School of Science, South Kensington. At present, and during the last four years, Assistant Science Master at the Central Higher Grade Board School, Manchester. T.E. Thorpe. R. L. Taylor. Francis Jones. William Burton. S. Parrish. Thompson, Edward Cumming, 5, Gubyon Avenue, Heme Hill, S.E. Manufacturing Chemist. Chemist at Messrs. F. C. Hill and Com- pany’s Chemical Works, Deptford. Associate of the Royal College of Science, London, in Chemistry (1st Class). Engaged in research work under Professor Thorpe, F.R.S., for six months. 1st Class Honours in Chemistry at Intermediate Science Examination, London University. T. E. Thorpe. W. Palmer Wynne J. W. Rodger. A. E. Tutton. William Tate. W. A. S. Calder. Thudichum, George Dupr6, Montrose, Dorset Road, Merton Park, Assistant in the Chemical and Gas Department of the London County Council. For ten years engaged in experimental work in connection with sewage treatment and allied subjects, under the direction of the Chemist to the Metropolitan Board of Works and the London County Council. Formerly assistant with Dr.DuprB. J. L. W. Thudichum, M.D. Dibdin, W. J. A. Dnpr6. Frederic Jsts. M. Page. R. Grimwood. Wm. Jno. Livingston. 129 Walker, Charles H.H., Prospect Place, Cainscross Rd., Stroud, Glos. Master. B.A. Oxford. 1st Class Natural Science School (Chern-istry) 1893. Science Master at Marling School, Stroud. Late Lecture Assistant, Chemical Department, Oxford. Author of "Pro-ducts of the Action of Nitric Acid on Tin," Chem. SOC.J., 1893. W. W. Fisher. W. H. Veley. J. A. Gardner. J. E. Marsh. John Watts. R. E. Hughes. Waterfield, Arthur Swainson, The Grammar School, Beverley.Science Teacher. M.A. Oxon. Honours in Chemistry. Formerly Science Teacher at Guildford, and Assistant to County Council Lecturer. Now empl oyed by the E. Riding C.C. John Watts. W. W. Fisher. J. E. Marsh. V. H. Veley. D.H. Nagel. M'illiam Esson. Wright, Robert, 11,Eagle Parade, Buxton. Pharmaceutical Chemist. As a student in the laboratory of the Pharmaceutical Society, took Medal for Practical Chemistry and Certificate of Honour in General Chemistry, and have since pub-lished twenty-eight notes and papers on subjects connected with Chemical Science. John C. Thresh. John Attfield. 111. Carteighe. W. A. H. Naylor. Wm. Martindale. A. C. Abraham. 31. Conroy. Edward Davies.
ISSN:0369-8718
DOI:10.1039/PL8941000111
出版商:RSC
年代:1894
数据来源: RSC
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