|
1. |
Proceedings of the Chemical Society, Vol. 14, No. 191 |
|
Proceedings of the Chemical Society, London,
Volume 14,
Issue 191,
1898,
Page 61-88
Preview
|
PDF (1642KB)
|
|
摘要:
Issued 23/3/1898. PROCEEDINGS OF THE CHEMICAL SOCIETY. EDITED BY THE SECRETARIES. No. 191. Session 1897-8. March 17th, 1898. Professor Dewar, F.R.S., President, in the Chair, Messrs. A. J. Buller Cooper, J. Murray Crofts, R. S. Morrell, T. Cunningham Porter, F. F. Renwick, and Harold C. Sayer were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Messrs. Oscar Julian Steinhart, Ph.D., 4, Palace St. Mansions, S.W.; Samuel A. Tuiker, Ph.D., Columbia University, New York ; Ernest Withnm, The Grammar School, Rotherham. ANNOUNCEMENT BY THE COUNCIL. The PRESIDENTannounced that notice of the following resolutions to be proposed at the Annual General Meeting by Messrs. Hartog and Harden had been received :-RESOLUTIONI.''That in order to carry out the suggestion of Mr. Cozens-Hardy, Q.C., communicated by the Council to the Society at the meeting held on February 17th, 1898 (Proc., 1898, 14,38) the following steps shall be taken to ascertain the wishes of the whole Society with regard to the desirability of obtaining a Supplemental Charter for the purpose of enabling Fellows to record their votes at the Annual election of the Officers and other members of the Council by proxy or post. 62 (1) ''The following papers shall be printed and distributed to the Fellows of the Society not later than April 14th :-(4 (( THECHEMICALSOCIETY, BURLINGTONHOUSE, PICCADILLY, W.LONDON, '(DEARSIR,-In accordance with the resolution passed at the General Meeting of the Chemical Society held on March 31st, 1898, we are instructed to request you to be good enough to- " (i) Answer the question printed below, by writing 'Yes ' or ;No ' in the space marked for the purpose.(( (ii) Fold this paper with the blank side outermost, place it in the envelope A ' provided, close the envelope, and write your signature legibly outside. '' (iii) Enclose the envelope 'A ' in the stamped envelope 'B,' and return this by post to the Secretaries on or before May 14th next. "We are, faithfully yours, ('(Signatures of Secretaries). " Are you in favour of the proposal that a Supplemental Charter should be applied for to the Privy Council so as to enable Fellows to vote at the annual election of the Officers by post or proxy .Z '((Here write 'Yes ' or 'No ')." An envelope marked thus :-'ITHECHEMICALSOCIETY.Re CHARTEB. A. ''Voting Paper. ''Please sign legibly here......... . .,. . .,. . . ..,.,. . . . . . . .. . .,........ . . . . . . . . . . (4 ''An envelope stamped with a penny stamp, and marked thus :-B. ''Re Application for Xupplemental Charter. THE SECRETARIESOF THE CHEMICALSOCIETY, BURLINGTONHOUSE, LONDON,W. 'I (2) At the next meeting held after May 14th the envelopes shall be opened and the voting papers placed, without being unfolded, in a balloting-box, and they shaIl be counted by a sufficient number of scrutators, to be appointed by the presiding officer. The signatures on the envelopes shall be at the same time checked against an official list of Fellows of the Society, and shall be preserved for a year.RESOLUTIONXI. If a majority of the votes recorded in accordance with the method prescribed by the foregoing resolution be in favour of an application being made for a Supplementary Charter for the purpose named, the Council shall be, and are hereby instructed, without any further pro- ceedings, to make the necessary application without delay.” To this notice of Resolutions the following reply had been sent :-CHEMICALSOCIETY, BURLINGTONHOUSE,W. March 17th, 1898. DEARSIRs,-The Council have carefully considered the proposed resolutions which you have forwarded to the Secretaries, notifying them that you intend to move them at the Annual General Meeting.We are, in the first place, to point out that the efEect of passing such resolutions would be precisely the same as passing a bye-law to enable Fellows to vote by proxy or through the post on this question, and that Mr. Cozens-Hardy, Q.C., has already advised that any such bye-law would be repugnant to the Charter. We are directed to say that this of itself would be sufficient to make the proposed resolutions out of order, but there are other grounds on which the Council are advised that such resoIutions cannot be submitted to a General Meeting. The Council are advised that in view of the opinions of Mr. Cozens-Hardy, such resolutions would not be in order, because they propose to deal with a question which is outside the scope of matters which can be decided at a General Meeting of the Society. They are also advised that even if such resolutions were passed they would have no power to act upon them, because in considering whether the Fellows really desire the change proposed, regard must not be had only to those who are present in person at a meeting (and still less t,o a bare majorit7 of Fellows voting, as you propose), but to the wishes of the whole body of the Fellows. You will remember that Mr.Cozens-Hardy thinks that an application for a Supplemental Charter would probably not be listened to unless it represented the practically unanimous view of the Fellows, and that any active opposition by even a small minority would probably be fatal.64 The Council are further advised that it would be ultra vires to expend any part of the fuds of the Society in giving effect to the pro- posed resolutions or in applying for a Supplemental Charter. In these circumstances, we are directed to inform you that it would be the President’s duty to refuse to put such resolutions to the meeting. We are also to point out that it would be open to any Fellows of the Society, at their own expense, to send out the circulars referred to in the resolutions, and that if it should be found that the Fellows were practically unanimous in desiring that application should be made for a Supplemental Charter, this could he applied for by them at the like expense, and that in the event of there being no opposition Her Majesty might be pleased to direct that such expenses should eventually be paid out of the funds of the Society.We are, dear Sirs, Your obedient Servants, M, THOMSON, rJOHN R. DUNSTAN, Xecretaries.WYNDHAM Honorary ARTHUR ESQ.HARDEN, P. J. HAILTOG,ESQ. 01 the following papers those marked * were read :-“34. (I The reduction of bromic acid and the law of mass action.” By Winifred Judson, B.Sc., and J. Wallace Walker, M.A., Ph.D. The authors have investigated the velocity of the reduction of bromic acid by hydrobromic acid, and find that, in the presence of a large quantity of sulphuric acid, the reaction is bimolecular, whereas in the absence of sulphuric acid it is tetramolecular. The results are in agreement with the conclusions drawn by Noyes (Zeit.Phys. Chem., 1896, 19,599) from the experiments of himself and others on the re- duction of bromic acid by hydriodic acid. The explanation put forward is that the stage of the reaction, which requires a measurable time for +--its completion, is expressed by the equation 2H + Br + BrO, = HBrO + HBr02, and that the bromous and hypobromous acids are instantly decomposed by the hydrobromic acid present. A further result ob-tained is that the reduction of bromic acid by hydriodic acid takes place 58.5 times faster than by hydrobromic acid, and that, therefore, although the latter is produced from bromic by hydriodic acid, its pre- sence in no way vitiates the conclusions drawn by Noyes from that reaction.65 *35. '' The action of ferric chloride on the ethereal salts of ketone acids," By R. S. Horrell, M.A.,Ph,D.,and J. M.Crofts, B.A.B.Sc. When anhydrous ferric chloride dissolved in absolute ether is added to an ethereal solution of ethylic ketophenylparaconate, a red oil separates. This, when washed with absolute ether, becomes solid, and is, most probably, represented by the formula, EeC12(Cl,H,105). Water decomposes the compound with formation of the basic ferric salt of ethj lic ketophenylparaconate, Fe(OH)(C,,H,,O,),, and ferric chloride. The ethylic salt of the lactone of oxalcitric acid yields with ferric chloride in absolute ether solution a red oil, which does not solidify, and is most probably an addition product, represented by the formula FeCI,,Cl,H1,O,. It loses hydrochloric acid slowly in a vacuiim.On treatment with water, it yields the ferric salt of the lactone of ethylic oxalcitrate, Fe(CI4HIPOJ3, and ferric chloride. In the case OF ethylic acetoacetate and ethylic beozaldincetoacetate purple oils are obtained by the action of anhydrous ferric chloride. The purple substances have not as yet been prepared in a sufficiently pure state to justify the authors in assigning formulz to them. *36. Note on the volatility of sulphur." By T,C. Porter, M.A., &c.6i During the analysis of some pumice rock from Tenerife, the author was led to the conclusion that sulphur is volatile at 100'. Several glass tubes were carefully cleaned, into which specimens of sulphur of varying physical condition and purity were placed.Some of the tubes were exposed to the air, others mere exhausted. After being exposed to a temperature of 100' for some minutes, it was oh-served that, as was to be expected, the better the vacuum, the more rapid is the sublimation of the sulphur. The sublimate consists at first of very pale yellow drops, which possess little viscosity, and remain unchanged in some cases even at 10" for days. Rhombic octahedra and prismatic sulphur are occasionally formed together, the former crystals sometimes grow at the expense of the drops. Sulphur does not yield a. perceptible sublimate at ordinary temperatures, in a ''good vacuum," even after a year. The two forms S, and 5, therefore have their transition point between 90" and 100".DISCUSSION. Professor MCLEODsaid that about 1870 Mr. Douglas Herman had experimented on the volatility of various substances in vacuous tubes, although he believed the results have never been published. Mr. Herman found that sulphur could be volatilised in a vacuum when heated to the temperature of boiling water, and that the vapour con- densed in drops on the cool parts of the tube, and remained liquid for many days. Octahedral crystals were formed at the expense of .the drops in the neighbourhood of the crystals, the drops gradually evaporating whilst the crystals increased in size ;prismatic crystals were very rarely seen, When phosphorus is heated in vacuo by the warmth of the hand, its vapour also is deposited in drops, although, RS in the case of sulphur, the vapour had not been heated to the melting point of the solid.Iodine at onc0 forms crystals under similar con- ditions, no liquid being deposited. The PRESIDENTsaid that, in a lecture on liquid atmospheric air in 1893 (Proc. Roy. Inst., 14, 7), he had described the use of sulphur in the construction of vacuum vessels for the storage of liquid air, and had shown that in such vacua cooling with liquid air or oxygen was sufficient to produce a visible distillation of sulphur at ordinary temperatures. The vapour tension of sulphur at 100" amounts to 0.06 mm.,so that the tension is comparatively high in Mr. Porter's experiments, considering that mercury distils rapidly under a pressure of one-millionth of an atmosphere, as shown by the application of liquid air.He also remarked that phosphorus distils practically instantaneously. "37. '' Cannabinol." By T. B. Wood, M.A.;W. T,N. Spivey, N.A.; and T. H. Easterfield, M.A., Ph.D. The authors have continued their examination of cannabinol, the toxic resinous constituent of Indian hemp (Fyans., 1896, 69, 539). The substance boils with slight decomposition at about 400", its absorption spectrum shows no characteristic bands, its vapour-density at the temperature of boiling sulphur corresponds with the formula C,,H,,O,, already assigned to the compound. An account is given of the reaction of cannabinol with acetic anhydride, Fenzoyl chloride, and phosphoric anhydride ; the results indicate that one hydroxyl group is present. In the case of acetic anhydride or acetyl chloride, however, a crystalline compound melting at 75" is one of the products of the reaction.The authors assign the formula C,,H1,O, to this compound. The same compound has recently been described by Dunstan and Henry (Proc., 1898, 14, 44,Feb. 17j who ascribe the formula C,,T-I,,OA.c to it. Fuming hydriodic acid gives no methyl or ethyl iodide when boiled with cannabinol. Reduction with hydriodic acid in sealed tubes produces a hydrocarbon, CloH2-,. By long-continued boiling with or without dehydrating agents, a hydrocarbon, ClOHl6,is formed. 67 Oxidation with aqueous chromic acid, alkaline, or acid permanganate, or dilute nitric acid is accompanied by the production of a caproic acid, lower fatty acids being probably produced at the same time.The action of fuming nitric acid upon cannabinol dissolved in cold glacial acetic acid removes one carbon atom as carbonic anhydride, and pro- duces a red, amorphous substance which gives numbers on analysis agreeing with the formula C17H2,N,0,. This substance, when boiled with nitric acid, yields a light red substance, C17H20N208, which upon further oxidation yields, amongst other substances, a yellow acid crystalline compound, C1,Hl,N2O5 which forms sparingly soluble crystalline sodium, ammonium, and silver salts and is probably a di-nitrophenol, and a compound, C1,Hl,NO,, the properties of which agree closely with those of the ‘‘oxycannabin ” of Bolas and Francis (Chem.News, 1871., 24, 77). This compound has the properties of a nitro-lactone, as has been already shown by Dunstan and Henry (Proc., Zoc. cit.). Corresponding crystalline potassium and silver salts have been prepared and analysed. The name cannabinic acid is proposed for the unnitrated parent oxy-acid. Amido-cannabinolactone, C,1H1102NH2, is obtained in colourless crystals melting at 119”, when the nitro-lactone is reduced either by hydriodic acid or by tin and hydrochloric acid. The base is readily rwrystallised from hot water, its salts cannot be recrystallised from water without decomposition ;the hydriodide and platinochloride have been analysed.“38. ‘(Contributions to the chemistry of thorium.” By Bohuslav Brauner, Ph.D. As there are few direct methods of separating the elements of the rare earths, the author investigated the reaction of Bahr (1864), who showed that thorium oxalate is easily soluble in a solution of ammo-nium oxalate. Bunsen (1876), though he found that the oxalates of the other rare earths are only slightly soluble in that reagent, had to repeat the process of solution many times to obtain a product which did not show in its spark spectrum the lines of other elements. The reaction is due to the formation of a double thorium-ammonium oxalate, decomposed by water, and existing in solution only in the presence of free ammonium oxalate. After numerous crystallisations, a salt was obtained having the formula Th(C204)2+ B(NH4)C204-I-+ H20.Finding,4H,O, with one-third to one-half of free (NH4)2C204 however, that the solution readily becomes supersaturated, a compound having the formula Th(C204), +2(NH,)C204+ 7H,O, was obtained in such a high state of purity that from its analysis the atomic weight of thorium, Th =232.59, could be calculated. 68 This “ complex ” salt is ammoniuin thoroxalate. It is decomposed by water, but a definite quantity of the soluble product of decomposi- tion dissolves the insoluble constituent, so that one part of water keeps one part of ammonium thoroxalate in solution if an additional half-molecule of free ammonium oxalate is present, The salt forms two hydrates, in accordance with Potilizin’s law that a compound forming supersaturated solutions exists in several hydrate forms, one with 7H,O, the other with 4H20.The former loses water in air of average humidity, passing into the latter form, which becomes anhydrous in perfectly dry air, or more readily at looo,without loss of ammonia. On heating at higher temperatures, large quantities of cyanogen gas are evolved. The amount of the decomposition of the salt caused by increasing the quantity of water was determined, together with the proportion of ammonium oxalate required to prevent decomposition. Three mols. of ammonium oxalate form, with one mol. of thorium oxalate, a clear solution in 300 mols. of water. This solution is, however, supersatu- rated with thorium oxalate, the latter separating until their relative proportions become 3.3 :1.A convenient method for the purification OF thorium may be based on these results, as the author has determined quantitatively the great difference in solubility between the oxalate of the feebly basic tetravalent thoria and those of the other trivalent rare earths in ammoniutn oxalate. The rule was thus established : “ the tendency to form complex oxalates is inversely proportional to the basicity of an earth.” This, and another property OF oxalates, that their stability under the oxidising action of nitric acid decreases considerably with an increasing basicity of the earth, was utilised for the purification of thorium. On precipitating a solution of ammonium thoroxalate with oxalic acid, an acid thorium oxalate-thoroxalate of thorium and hydrogen- is formed, having the formula H2Th2(C20,)5+ 9H,O.On using mineral acids (Glaser, Zeit.Anal. Chem., 1897, 36,216 ;1898,37,25), a different result is observed. “39. On the atomic weight of thorium.” By Bohuslav Brauner, Ph.D. The author determined the purity of the material, obtained as described above, by the spark spectrum, and by atomic weight deter- minations. He determined in the air-dry oxalate (a) the thorium tetroxide by heating, and (b) the percentage of C20, by means of a solution of potassium permanganate. The first series of experiments gave concordant results, leading to the value Th =233.3, a value not in agreement with that previously obtained by him, Th =232.59.Purther study showed that the oxalate used was contaminated with basic salt, and a normal oxalate being prepared, the following values mere obtained as a result of five series of experiments made with different preparations. Th = 232.50, 232.46, 232.45, 232.31, 232.33, 232.50, 232.44, and 232.35 ; average, Th = 232.42. This number agrees with that obtained by Kruss and Nilson, Th = 232.45. The author then investigates the conditions which led him to obtain the high value in the first series, approaching the value of Cleve, Th = 234.5. The work of other investigators is vitiated by untrustworthy methods and impure material. *40. “On the compound nature of cerium.” By Bohuslav Brauner, Ph.D. The author showed in 1882 (Tkacns.,41, 68 ; Monnts., 3, 486) that cerium from cerite is associated with an element whose higher oxide forms yellow and lower white salts, though the higher oxide is far less stable than cerium tetroxide. The substance is found with lanthanum and didymium when separating cerium by Bunsen’s method.In 1885,the author showed (T~ccrts.,47,879)that the substance remains in the mother liquor after the bulk of the cerium sulphate has crystal- lised, and may be precipitated froin it by alcohol. Schutzenberger has repeated the author’s experiments without mentioning his name. After applying Debray’s method of separating cerium to these fractions and again fractionating, the author obtained substances with the following values for the atomic weights.The method employed was the analysis of the oxalate, and the determination of ‘active ’ ozonic oxygen by Bunsen’s method in the oxide obtained by calcination, the latter number being given in parenthesis : R”’= 140.25 (4.64), 140.22 (4*65), 140.12 (4*81), 140.00 (4*65), 140.01 (4.59), 139.65 (4*61), 139.16 (4 01), 138.72 (4.51), 136.50 (3*31), 135-43 (3*93), 132.07 (3-73), 130.70 (3.21). As the value of the atomic weight decreases, the colour changes from white to a reddish-brown orange. The quantity of ‘active ’ oxygen, therefore, decreases almost in proportion to the decrease in value of the atomic weight. If we assume that the ‘active’ oxygen is due entirely to the cerium present, the value of the atomic weight of the other element may be calculated at about 110.The author has thoroughly investigated the spark spectrum of the lower fractions, but has found no characteristic line, other than those of cerium. In one case only were traces found of the two characteristic groups of lines in the red belonging to yttrium. No appreciable amount of yttria could be found, however, in the solution, even when a large quantity of the material in question was treated with potassium sulphate. As terbium forms a higher 70 oxide of an orange colour, the colour of the lower fractions of cerium may be due to its presence, but as its atomic weight is higher than that of cerium, another earth of lower atomic weight must still be present, and it is not improbable that, like gadolinum, this element may give no characteristic spectrum.The recent controversy between Wyruboff and Boudouard (Compt. rend., 1897, 125,pass.) has led the author to publish the result of this research, which has occupied him many years. *41 ‘‘On praseodidymium and neodidymium.” By Bohuslav Brauner, Ph.D. Applying Mendelhef’s method of cry stallisation of the double nitrates with a.mmonium nitrate to a mixture of lanthanum and didy- mium, Auer von Welsbach (1885) succeeded in splitting up the old didymium into praseodym ” and ‘‘neodym.” Praseodidymium, according to him, has an atomic weight Pr = 143.6, and forms two oxides, Pr20, and Pr,O,. The higher oxide is black-brown, the lower forms green salts with a characteristic spectrum, Neodidgmium Nd = 140.8 gives only one oxide, Nd,O, with pink salts possessing eleven absorption bands.Nothing of importance has been added to our knowledge on the subject during the last 11 years. The author spent several years in repeating Welsbach’s work, but last year he obtained from Dr. Waldron Shapleigh, in Gloucester, N.J., a quantity of highly purified research material. From this mixture (40 grams of praseodidymium oxide with 20 grams of lanthanum oxide) the latter was removed, the former being converted by fusion with nitre into the oxide Pr,O,. This was puri- fied by fractionating with ammonium nitrate solution, ammonia, and oxalic acid. A preliminary determination of the atomic weight gave the value Pr = 140% The analysis of the oxalate and the synthesis of the sul- phate gave thirteen numbers, varying between 140.84 and 141.19, the average being Pi-= 140.95.The lower oxide, Pr203,is of a beautiful pale green colour, and the spectrum of its green salts contains the absorption bands X = 5968, 5895, 4812, 4693 and 1447 (Rowl.) Praseodidymium trichloride gives a characteristic spark spectrum. Salts of the trioxide having the following formulae have been pre- pared and analysed by the author :-Pr2(S04)3, Pr,(SO,), +6H,O, Pr,(SO,), + 8H,O, Pr(N0J3 + 2NH4N0, + iH,O, PrAc, + H,O, Pr,(C,O,), + 1OH,O. According to Professor Vrba’s measurements, the salt Pr2(S04), +8H,O is isomorphous with Y,(SO,), +8H,O and other sulphates of this type. This fact, and the slight solubility of the oxalate in ammonium oxalate, 71 prove that the formula of the lower oxide is Pr203,and not Pr204or Pr,O,, in which cases the atomic weight would be 188 or 235.The tetroxide, Pr204,obtained from the nitrate on heating to a tempera-ture of 440°, or by fusion with nitre:at 400°, is jet-black, but it becomes dark brown in a state of fine division. Up to the present, only its basic salts have been obtained; the sulphate, 2Pr20,*S0,+ 29H,O, and the basic acetate in acetic acid solution, having a formula which may be represented by either Ac3-Pr'JO-Pr1V-(OH)3, or Ac,-Prlr',O,-OH Ac + H,O. The double fluorides are being investigated. It is of the greatest importance to know whether the tetroxide is (a) a true oxide of the water type, with ozonic oxygen (like lead tetr- oxide, PbO,), in which case the praseodidymium would be tetravalent, or (b) a true peroxide of the hydrogen peroxide type, with ant-ozonic oxygen (like barium peroxide, BaO,), in which case the metal would be trivalent.With regard to the first view, it yields, with dilute acids, free oxygen, and the solution does not reduce potas- sium permanganate (negative test for hydrogen peroxide). On treat- ment with concentrated nitric and sulphuric acids, oxygen containing much ozone is evolved, and with hydrochloric acid chlorine is set free, arising probably from the decomposition of the unstable perchloride, PrCl, (3). Like other ozonic oxides of the water type, it presents with hydrogen peroxide the phenomenon of catalysis in the presence of dilute sulphuric acid, a quantity of the hydrogen peroxide being oxidised, strictly equivalent to the 'active ' oxygen lost by praseo- didymium tetroxide according to the equation : Pr20,+ H,O, + 3H280, + Aq =Pr,(SO,), + 0,+ 4H,o + Aq.On the other hand, praseodidymium tetroxide gives with ether, water, sulphuric acid, and potassium bichromate an intensely blue coloration (Baresville's reaction) according to the equation Pr,0, + 3H,S04+Aq =Pr,(SO,), + H,O, + 2H,O + Aq. In the treatment, there- fore, of the tetroxide with dilute sulphuric acid both reactions take place simultaneously, and the result is the evolution of oxygen, 2Pr20, + 6H,SO, + Aq =2Pr,(SO,), + 0,+ 6H,O -I-Aq.Praseodidymium tetroxide is, therefore, an oxide of a new kind, belonging simultaneously to the ozonic oxides of the water type, and to the antozonic oxides of the hydrogen peroxide type; it is, in fact, the missing link between these two hithertcj entirely different types of peroxides, its active oxygen being at the same time both entirely ozonic and entirely antozonic. The basic acetate of the tetroxide, which is nearly white, and in the spectrum of which the blue absorption bands are invisible when seen by reflected light, though the yellow band remains unchanged (an indication of the complex nature of praseodidymium), is the salt of an oxide belonging to the hydrogen peroxide type, for it reduces potas- sium permanganate quantitatively and gives Baresville’s reaction for hydrogen peroxide. It is, however, so remarkably stable that it does not part with all its active oxygen even after being boiled for an hour with concentrated caustic potash solution.As regards the author’s neodidymium, its absorption spectrum con- tains the bands A= 7283, 7080, 6905, 6368, 6279, 6247, 57SS, 5323, 5211, 5097, 5063 and 4280. It contains, in addition to these, a strong, sharp band of wave-length X =4694 which differs in character and position from the praseodidgmium band X=4693. There were also traces of Pr 4812 and Pr 4447, Dg 4752 and 4605 (Sm. series a). The value of the atomic weight of neodidymium found after the first purification of the material by treatment with oxalicacidwas Nd = 143.4, after another purification, Nd = 143.63.Its lower oxide, having the formula Nd,O,, is of a beautiful pink colour with an amethyst tint, whereas the higher oxide contains a little more oxygen than corresponds to the formula Nd,O, (the author’s old Di,O,). Neodidymium also gives two series of salts, the acetate of the higher oxide being nearly white. According to a quantitative analysis, by comparing the intensity of the bands the author’s neodidymium con1 ained 2.9percent. praseodidy- mium, whereas the old didymium from cerite contained in 100 parts of the oxide 78.8 parts Nd,O, and only 21.2 per cent, Pr,O,. With regard to the position of these elements in the periodic system, the author concludes from the tendency of them both to become more highly oxidised than would correspond to the formul~ Pr,O, and Nd,O,, that praseodidymium and neodidyrnium may be further split up. This is regarded as very probable by all rare earth chemists.The pure oxides will probably be found to have the formuls Pr,05and Nd,O,, so that the eighth series of the periodic system would assume the following form :-I I1 111 1v V VI cs. Ba. La. Ce. Pr. Nd. 133 137.4 138.2 139.7 141 143.6 DISCUSSION. The PRESIDENTcongratulated Professor Brauner on the valuable scientific results he had presented to the Society, and on behalf of the members expressed their appreciation of the motives which had induced the author to come all the way from Prague to communicate four papers of such great importance to the Chemical Society.He wished him success in the continuation of such laborious and intricate inves- tigation. 73 42. Action of ammonia and substituted ammonias on acetyl-urethane." By George Young, Ph.D., and Ernest Clark. Acetylurethane has been subjected to the action of ammonia and of substit'uted ammonias under varying conditions as to solvent, temperature, and pressure. The general results of the invest'igation show that action takes place principally according to the equation, MeCONHC0,Et + NH,R =MeCO *NH= CO-NHR +EtOH. Under cer- tain conditions, the products point to the action having resulted in the formation of acetamidine urethanes, MeCO,NHCO,Et +NH,R =Me(XHR)C:N* C0,Et +H,O.These acetamidines have not been isolated, but in their place the products of hydrolysis, acetamide and substituted acetamides, have been obtained, Me(NHR)C:N* CO,E t + 2H,O =Me*CO*NHR+NH, +CO, +EtQH. Ammonia and methyl- amine enter into action most easily, piperidine, aniline, the naphthyl- amines and phea ylurea less so. Acety lurea, acetanilide, and diphenyl- amine appear to be without action. '(43. Formation of oxytriazoles from semicarbazides." By George Young,Ph.D., and Benjamin Mitchell Stockwell, B.Sc. This paper contains an account of the formation of oxytriazoles according to the equation R*NH-NH*CO *NH,+C,H,*CHO +0 = R(C,H,)*C,N,OH + 2H,O where R is an aromatic radicle. The follow-ing substances are described. Pai.~toZyZsernical.ba~ide,m.p. 187-1 88". Acetylparcetolylsemicccrba~i~~e, p. 212.5". Benxo ylparatolylsemicarb- m. uaide, m. p. 218". Pai.atoZyZccxocal.bamide,M.p. 142". 5-Phenyl-I-para-m.tolyl-3 oxytriaxole, m. p. 242". Acetylp~~eny~cercctol~loxytriaxole,p. 112-113". Benxoy~~heny~ar~toZyZoxytricc~oZe,m. p. 132". Phenylpa?*a-tolylethoxytriaxole, m. p. 51-52". P-NcciuhtiLylse~~icarbccxide,m. p. 225". Pl~enyZ-~~apht~yZoxytri~xoZe,m. p. 274-276". Acetylphenyl-,B-napI~thyl-oxytriaxole, m. p. 142-143'. Benxoyl~l~enyl-,B-n~pl~t?~?!Zo~ytriaxoZe,m. p, 141-1 42". Metanitrophenylsemicarbaxide, m. p. 195". BenxoyZmeta-nitroplenylsemiccr~axi~e,m. p. 188-1 89". JIetanitrophenyZaxocurbamide, m. p. 168-169'. 5-Phenyl-l-metunit~ophenyl-3-oxytriaxoZe,m.p. 235". AcetyZphenyZrnetaniti~ophen~lox?/ll., m. p. 130-1 32". Benxolymeta-m. p. 168". Ariti.ocliphenybtloxyt~.~a~o~e,nitrodip~~enyZo~ytriaxoZe, m. p. 96". 44. '' Formation of aa'-dihydroxypy ridine." By S. Ruhemann, Ph.D., M.A. Ethylic aa'-dihydroxydinicotinate (Proc., 1898, 14, 47) when boiled with concentrated hydrochloric acid, yields the hydrochloride of aa'-di-hydroxypyridine, from which ammonia sets free the ba8e (m. p. 74 192-193'). The same substance is obtained from Guthzeit and Dressel's monethylic athoxypyridonedicarboxylate (Afinulen, 1891, 262,113) by boiling hydrochloric acid. 45. ''Position-isomerism and optical activity ; the comparative rotatory powers of diethylic mono-benzoyl and mono-toluyl tartrates." By Percy Frankland, F.R.S., and J. McCrae, Ph.D.The authors review the present state of knowledge concerning the relative rotatory powers of the phenyl and three toluyl derivatives of optically active compounds, and point out that whilst of the three isomeric toluyl groups, the ortho- has almost invariably the least, and the para- the greatest, rotatory influence, the rotatory influence of the phenyl-group is in some series greater, and in some less, than that of any one or of all of the toluyl groups. As a contribution to this study, theauthors have prepared the com- pounds mentioned above, and have determined their rotations in a fused state over a wide range of temperature, whilst they have also determined the molecular weight and rotation of each in glacial acetic acid solution, with a view of ascertaining the relative rotations of the compounds in the monomolecular condition.The following are the specific rotations at 100" for each of the com- pounds, as well as of diethylic tartrate, from which they may be regarded as derived. Diethylic tartrate...... . .. .... . . . . . [a]":= + 7.66" [a]l:OO = + 15-77" ,, monobenzoyltartrate .. [a]? = + 20-71" [aIgg5"= + 17.69" ,, mono-o-toluyltartrate. [a]': = + 11.82" [a]'F = + 10-88O 99 77 -m-9, [a]*:= + 13.59' [a]'y= + 12.57' 79 7) 3,-P-[u]'F == + 25.85" Thus the dextrorotation of diethylic tartrate increases with rise of temperature, whilst that of the above monacidyl tartrates diminishes. In glacial acetic acid solution, the benzoyltartrate has a lower rotation than the para-toluyltartrate, but otherwise the above order of the rotations is unchanged. In all cases the rotation in glacial acetic acid solution was considerably lower than that of the pure substance, but this difference is not attributable to the pure substance in the fused state being associated, for the rotation of the diethylic monobenzoyltartrate in benzene solu- tion was even lower still, and yet in benzene solution it is more probable that there would be association than in glacial acetic acid.Thus from the results in benzene it would appear that association of the benzoyl compound is attended with diminution in the rotation, so that the higher rotation of the liquid benzoyl compound itself cannot 7.5 be due to association also.Neither do the molecular volumes of these compounds point to association when interpreted by Traube’s formula. Diethylic monobenzoyltartrate has been previously prepared by Guye and Fayollat (Bull. Xoc. Chim., 1895, [iii], 13,20l), their pre- paration was admittedly impure, and yielded a very much lower rota- tion and melting point. It was first prepared by Perkin (Trccm.,1867, 20, 138), but without determining the rotation, the melting point which he obtained was almost exactly the same as that found by the authors. 46. ‘‘ The action of di-isocyanates upon amido-compounds. ” By H. Lloyd Snape, D.Sc., Ph.D. By the action of diphenylenedi-isocyanate upon pheny1-hydrazine in ethereal solution, dip~enylenedi-phenylsemicarbaxide, Ph-NH-NH.CO *KH*C,H,* C,H,*NH* CO *NH*NH*Ph,was obtained.The product was a white powder which was insoluble in the more common organic solvents, It gave with copper sulphate a chocolate-brown colour, which was changed to green on the addition of ammonia. ToZuyZenedi-phenyZsern&arbaxide, Me* C,H,(NH* CO *NH*NH*Ph),, (1 : 2 : 4) mas prepared by acting with 1:2 : 4-toluylenedi-isocyanate on an ethereal solution of phenyl-hydrazine. The product, after recrys- tallisation from alcohol, consisted of colourless crystals which decom- posed and rose in a capillary tube at 203’. This carbazide also was insoluble in the more common organic solvents, with the exception of alcohol, in which it was difficultly soluble.With copper sulphate, it gave a wine-red coloration which changed to green on the addition of ammonia. 1:2 :4-Biphenyl-toZuyZene-diu~ea,Me- C,H,(NH* CO *NH*Ph),, was obtained on mixing ethereal solutions of aniline and toluylenedi- isocyanate. The product was recrystallised from alcohol ; it formed microscopic needles which melted at 261’ with accompanying decom- position. It was difficultly soluble in methyl, ethyl, and amyl alcohol. 1 : 2 :4-ToZuyZene-diurea, Me*C,H,(NH*CO*NH,),, was prepared by treating an ethereal solution of toluylenedi-isocyanate with ammonia and crystallising the product from water. Minute crystals, which melted with accompanying decomposition at about 252’. It was sparingly soluble in alcohol.Lussy had previously described this reaction, but states that the product melts at 220”. 47. “The action of alkyl iodides on silver malate and on silver lactate.” By Thomas Purdie, F.B.S.,and Gc, Druce Lander, B.Sc. The object of this research was to discover the cause of the abnor- mally high optical activity of the ethereal malates and lactates pre- 76 pared by the silver salt method. An abstract of the first part of the paper treating of the action of isopropylic iodide and ethylic iodide on silver malate has already been published as a preliminary note (Proc., 1896, 12, 219). The high activity of the malates, thus prepared, is due to the simultaneous production of ethereal salts of the much more active alkyloxysuccinic acids.The silver salt of inactive lactic acid acts in a similar manner. With isopropylic iodide, the ethereal salt of (n-or iso-) propoxypro- pionic acid is produced in considerable quantity. By reactions similar to those employed in the case of silver malate, the substance was separated from the ethereal lactate with which it is mixed, and identi- fied by the analysis of several salts obtained from it. Evidence was also obtained that with ethylic iodide the ethylic salt of ethoxypro-pionic acid is produced, though in this case, as in the corresponding reaction with silver malate, it was not possible to isolate the salts in the pure state owing to the small quantity of the alkyloxy-acid formed. The authors have recently effected the resolution of several alkyloxy- propionic acids by means of alkaIoids, and find that these acids are highly active as compared with lactic acid.Their production in the reaction above referred to accounts therefore for the abnormal activity of the ethereal lactates prepared from silver lactate, The reaction seems to be a general one for the silver salts of hydroxy- acids (see following paper), and cannot therefore be relied on for the preparation of the ethereal salts of these acids in the pure state. With the permission of Mr. Brame, the authors have recently extended his experiments on the action of alkyl iodides on silver tartrate. The results already obtained point to the formation of dialkyloxysuccinates being the cause of the abnormally high activity of the ethereal tar-trates thus prepared.The authors are carrying on the research with the view of throwing light on the reaction by which the alkyloxy-acids are produced, and of adapting it, if possible, for the direct preparation of optically active acids of this kind from the corresponding active hydroxy-acids. 48. ‘‘ On the optical rotations of methyl and ethyl tartrates.’’ By J. W. Rodger and J. S. S. Brame. The authors, in attempting to prepare the alkyl tartrates in a high state of purity, find that when prepared by saturating an alcoholic solution of the acid with hydrochloric acid, or heating the acid or mono-substituted ester with alcohol in sealed tubes, the rotation of the pro- duct is much lower than that obtained for esters prepared by the action of an alkyl iodide on silver tartrate, Differences of the same nature have been observed by J.Wallace 77 Walker (Trans., 1895, 67,914) in the case of the lactates, and by Purdie and Williamson (Trccns.,1896,69, 818) for malates and lactates. With alkyl tartrates, however, the difference in activity is much greater than with lactates or malates. Further, the rotation for different specimens of tartrates prepared by the silver method is by no means constant, although every precaution was taken to ensure similar treatment during preparation. In order to determine any other differences in the esters prepared by these different methods, samples of methyl tartrate giving these different optical activities were hydrolysed with excess of sodium hydrate, when the products of hydrolysis gave practically the same rotations.Secondly, no difference in the refractive indices was found ; and on combustion of methyl and ethyl tartrates prepared by different methods and varying widely in rotation, no real difference in the per- centage of carbon could be detected. These abnormal results for the rotations may be explained on three hypotheses. The low rotation of the ethereal salts prepared by hydro- chloric acid saturation or by the sealed tube method may be due to racemisation. Second, the esters from the silver salts may be isomeric with and more active than those prepared by other methods ; or third, the esters prepared from silver salts may be contaminated with some much more optically active substance. The first hypothesis is precluded by the constancy of the rotations obtained by the authors for specimens prepared by three different methods and the agreement with the rotations observed by others with these substances. The second is improbable, but receives some support from the result of hydrolysis. With regard to the third hypothesis, Purdie and Lander in a preliminary note on the action of alkyl iodides on silver malate (PYoc.,1896, 12,221)ascribe the higher rotation given by the malates so obtained to the presence of (‘small quantities of the ethereal salts of the highly active alkyloxy-acids.” The same explanation may hold with the tartrates, in which case these derivatives must be highly active, for they can only be present in small amount, since there is no appreciable rise in the percentage of carbon found. If the high rotation for tartrates prepared from silver salts is due to this cause, then the agreement of results obtained on hydrolysis is only a coincidence. 78 ANNIVERSAR,Y MEETING.The Anniversary Meeting will be held on Thursday, March 31st, at 3 o’clock in the afternoon. At the next Ordinary Meeting, on Thursday, April 21st, there will be a ballot for the election of Fellows. 79 CERTIFICATES OF CANDIDATES FOR ELECTION. N.B.-The names of those who sign from ‘‘General Knowledge ” are printed in italics. The following Candidates have been proposed for election. A ballot will be held on Thursday, April 21st.Coupe-Annable, Henry William, University College, Sheffield. Chemical Assistant. For six years Chemical Assistant to Prof. Williams, University College, Sheffield. Author (jointly with Dr. G. Young) of paper, ‘‘Formation of substituted Oxytriazoles from Semi- carbazides,” P~oc.,1897, also paper ‘‘Benzoylphenylsemicarbazide,” Tram., 1897. W. Carleton Williams. L. T. O’Shea. George Young. Fred Ibbotson. William H. Oates. Abbott, Albert, Church Street, Adlingtou, Chorley, Lancashire. Schoolmaster. B.A., Oxford. First Class in Chemistry in Final Honour School. Formerly Science Master at the Marling School, Stroud ; for last 2& years Science Master at the Grammar School, Doncaster. J. Mitchell Wilson. John Watts.V. H. Veley. J. E. Marsh. W. W. Fisher. John William Young. Baskerville, Charles, B.S., Ph.D. University of North Carolina, Chapel Hill, N.C. Assistant Professor of Chemistry Univ. of North Carolina, Assist. Chemist to North Carolina Geolog. Survey. Grad. in Chem. Univ. of Va, P.G.Student Vanderbilts University. Studied in 1893 under Dr. Emil Fischsr, Univ. of Berlin. Ph.D., Univ. N.C. 1894. Instructor in, then Assist. Prof. of Chem. Univ. of N.C., Secy. Section C. Am. Assist. of Adv. Science. Author “Separation of Zirconium by SO2,” “ Rapid Method Determination P. in Titaniferous Iron Ores,” ‘‘Re-actions between Copper and H,SO,,” ‘‘Reaction between Mercury and H,SO,,” and others. Co-author with Dr. F. P. Venable, (‘Sulphites of Zirconium,” (‘Zirconium Oxalates,” &c.J.W. Mallet. W. L. Dudley. F. P. Venable. Marcus Benjamin. F. P. Dunnington. Jas. Lewis Howe. Brierley, Joseph, Ashton Road, Failswort 11, Manehester. Assistant Lecturer in Chemistry at the Technical College, Hudders- field. B.Sc. (Victoria) Associate of The Owens College. Harold B. Dixon. G. H, Bailey. J. H. Wolfenden. S. G. Rawson. W. H. Perkin, junv. Campion, Alfred, 637, Alexandra Parade, Dennistoun, Glasgow. Chemist to Steel Co. of Scotland, Ltd., Blochairn Works, Glasgow. Three years’ training at Pinsbury Technical College, London. Chemical Lecture Assistant for 34 years at R.I.E. College, Cooper’s Hill, Staines. At present Chemist at Blochairn Steel Works. Associate of the Institute of Chemistry.R. Meldola. Herbert McLeod. J. E. Stead. F. E. Matthews. F. W. Harbord. Caven, Robert Martin, University College, Nottingham (private address-The Tower House, Park Row, Nottingham). Lecturer and Demonstrator in Chemistry. B.Sc. Lond., E.1.C‘. For upwards of two years Assistant in the Laboratory of the City Analyst, Birmingham. Since September, 1895, Lecturer and Demon- strator in Chemistry, Nottingham. Author of the following papers : January, 1896, J.X.C.I., (‘On some Properties of Ferric Phosphate.” 81 January, 1897, J.X.C.I., Some Properties of Certain Metallic Phos- phates,” in conjunction with A. Hill. November, 1897, Proc., “The Action of Magnesium on Cupric Sulphate Solution,” in conjunction with F.Clowes, D.Sc. December, 1897, J.8.C.I. “The Estimation of Cuprous Oxide by means of Standard Potassium Permanganate Solution,” in conjunction with A. Hill. Frank Clowes. F. Stanley Kipping. Alfred Hill. J. J. Sudborough. William A. Tilden. L. Archbutt. Hudson-Cox, Fredk., 67, Surrey Street, Sheffield. Analytical Chemist. For three years a Htudent of Chemistry at the School of the Pharmaceutical Society, and for one year a Student of Physics at University College, London. Associate of the Institute of Chemistry, Assistant to Mr. A. H. Allen. Wyndham R. Dunstan. Arthur P. Luff. Thos. Stevenson. Alfred H. Allen. G. E. Scott-Smith. Dudley, Charles Benjamin, Drawer 334, httoona, Penn., U.S.A. Chemist, Pennsylvania Railroad Company. Ph.D.from Sheffield Scientific School of Yale College, 1874. Instructor Univ. of Penn., 1875. Chemist Penna., R.R.Co., 1875 to date. Published investiga- tions on the Chemistry and Wear of Steel Rails, 1875-82. Also a series of articles on “Chemistry applied to Railroads,” in 1889-1897. Many isolated papers on various Metallurgical and Chemical subjects, Prest. Am, Chemical Society, 1896 and 1897. Charles F. Chandler. S. A. Goldschmidt. H. T. VultB. Jas.S. C. Wells. Arthur H. Elliott. EZwp Walley. Fleming, John Arnold, Britannia Pottery, Glasgow. Potter. Practical Manager of a Pottery. Studied Analytical Chemistry under Dr. Readman, Edinburgh. Attended Dr. Stevenson Macadam’s Lectures in Edinburgh, taking the First Class Medal of the year, and have continuously made chemical investigations in connection with my work.Stevenson Macadam. John Clurk. G. H. Gemmell. A. Humboldt Sexton. R. R. Tatlock. G. G. Hende~son. Edw. C. C. Stanford. 82 Garside, Arthur Leonard Harry, C/o Messrs. Lawes and Co., Ltd., Barking Creek, Essex. Analytical Chemist. Formerly Student in Chemistry, Physics, &c., at the Vivian Institute, Torquay, under C. W. Priestley, Esq., B.Sc., A.R.C.S. (Lond.) and at other Institutions. From 1895-97 Demon-strator in Chemistry, &c., at the Science and Art Schools of Torquay and Paignton. Since March, 1897, Assistant Chemist to the Lawes’ Chemical Manure Co., Ltd., and Lawes’ Chemical Go., Ltd. Otto C. J. G. L. Overbeck.C. W. Priestley. Vincent Edwards. J. Theo. Hewitt. Walter D. Severn. Frank Dixon. F. Napier Xutton. Gidden, William Thomas, 108, Vicarage Road, Langley, Birmingham. Chemist to the British Cyanides Company, Oldbury. Five years Student of Chemistry at Central Technical College ; Diploma of Associate of City Guilds Institute in Department of Chemistry. Assistant Demonstrator in Chemistry, East London Technical College, Session 1896-1897. Now Chemist to British Cyanides Company. Henry E. Armstrong. Gerald T. Moody. William H. Davis. Sidney Williamson. James C. Philip. William J. Pope. Guthrie, Alexander, B.Sc., Rocking, Braintree, Essex. Manager of Saml. Courtauld & Co.’s (Ltd.) Crape-finishing Works. For over four years studied Chemistry practically in Glasgow and Leipzic.For two years Chemist and Sub-Manager in Fish-Products Factory. Over two years Sub-Manager in Chemical Manufacturing Works. For two years Manager of White-Lead Works. Four years in charge of Silk Dyeing and Finishing. John Ferguson. James J. Dobbie. G. G. Henderson, C. M. Aikman. Edmund J. Mills. Heaton, John, 81, Garmoyle Road, Liverpool. Brewer and Brewers’ Chemist. Two years and a half Student of Chemistry under Mr. P. J. Beveridge, M.A., B.Sc., Laboratories Cowley Schools. A course of lectures on Organic Chemistry and Physics Owens College. Honours Technical Brewing, May, 1897, City Guilds Institute. John Heron. Arthur R. Ling. Walter J. Sykes. Prosper H.Marsden. Leonard Temple Thorne.Chas. E. Eastick. Bernurd Dyer. 83 Hislop, Lawrence, Gas Works, Uddingston. Engineer and Manager to Bothwell and Uddingston Gas Company, Ltd. Received my training in Chemistry (both Inorganic and Organic) in Glasgow and West of Scotland Technical College under T. A. Cheetham, Esq., F.C.S.; then for a short time in Messrs. Tatlock’s Laboratory, Glasgow. For last five years (in present situation) have been engaged in Analytical work, such as Coal Analysis, Gas Analysis, &c., &c. Thos. A. Cheetham. Archd. R. Ormiston. James Knight. J. Watson Napier. William E. Kay. Hodgson, Harry Pearson, Caldew Bank, Cummersdale, Carlisle. Works Chemist. Completed a three years’ course of Chemistry at Owens College.Assisted Professor Perkin and Dr. Thorpe in their work on i-Camphoronic Acid. In Leopold Cassella’s Dye Works at Frankfurt-a-M. Harold B. Dixon. D. Lawrence. W. H. Perkin, jun. G. H. Bailey. A. William Gilbody. Hyland, John Shearson, Ph.D., M.A., F.G.S. 11, Powis Square, Bayswater, London, W. Mining Engineer and Metallurgist. Studied Chemistry at the University of Leipzig, taking his degree in Chemistry, Physics, and Mineralogy. Author of original investigations on the Chemical Con- stitution of Minerals, vide Tschermak’s Mittheil, 10,88, and Scientific Proceedings of the Royal Dublin Society, 6. W. N. Hartley. Edward Davies. Henry A. Miers. Lazarus Fletcher. William Crookes. Jee, Edwin Charles, 45, Pepys Road, New Cross, S.E. Engaged in Chemical Research at the Central Technical College. B.Sc.(London). Late Assistant Master and Science Teacher at Orms-kirk Grammar School, South Lancashire. Chas. E. Browne. Henry E. Armstrong. Gerald T. Moody. William J. Pope. Sidney Williamson Arthur Lapworth. W. Palmer Wynne. 84 Jessop, Samuel Morton, 12, Hanson Terrace, Wakefield. Laboratory Assistant, County Council Laboratory, County Hall, Wakefield. Engaged during past five years on the systematic in- vestigations instituted by the West Riding of Yorkshire County Council into (a) Purification of Rivers, and (b) Plumbo-solvent Action of Moorland Water Supplies. Holds eight Certificates for the Science and Art Department’s Examinations in Chemistry, including First Class Honours.E. Frankland. B. A. Burrell. Alfred H. Allen. Thomas Faidey. Edward N.Chaplin. Frank Clowes. Jones, Edward, Vine Cottage, Tudor Road, Kingston-on-Thames. Analyst. Bachelor of Science, London University. Fellow of the Institute of Chemistry. For sixteen years Analyst in the Government Laboratory, London. T. E. Thorpe. C. Proctor. R. Bannister. J. Woodward. H. J. Helm. E. Grant Hooper. Jones, William, 29, High Street, Wavertree, Liverpool. Chemist and Dentist. Pharmaceutical 1874, Dental 1878. desire admission to Chemical Society in order to read the publications of the Society, and so keep in touch with the latest discoveries of Chemical Science. Arthur W. Wnrrington. John W. Towers. Jos. P.Burnett. James Grant.Herbert W. Seely. I? C. Hurtmann. John Hcvgreaues. Lowry, Thomas Martin, 28, St. Lawrence Road, W. Kensington, W. Assistant in the Chemical Department of the Central Technical College, London, S.W. Diploma of the City and Guilds of London Institute, London University, B.Sc., with First Class Honours in Chemistry and Second Class Honours in Physics. Work on Chlor- bromcamphor and on Nitrocamphor (Proc., 1897, 13,159). Henry E. Armstrong. W. J. Pope. Gerald T. Moody. Sidney Williamson, F. Stanley Ripping. 85 Masson, George Henry, 22, Lauriston Place, Edinburgh. Doctor of Medicine, Master of Surgery, Edinburgh ; Bachelor of Science in the Department of Public Health, Edinburgh. Late Govern- ment Analyst under Food and Drugs Act, and Assistant to the Govern- ment Analyst, Port of Spain, Trinidad, B.W.I.Late Student Public Health Laboratory, Edinburgh University. Senior Medallist, Class of Practical Chemistry, Edinburgh University, Session 1891-1892. Alex. Crum Brown. Leonard Dobbin. John Hunter. John S. Ford. Hugh Marshall. G. H. Gemmell. Mitchell, Albert Henry, Martin’s Lane, Tiverton, Devon. Science Master. Have been engaged in teaching Chemistry since 1890, and for the last three years as Chemistry Master at the Tiverton Technical School. B.Sc. (London) and Honours South Kensington Organic and Inorganic Chemistry. Author of Quantitutive Exercises for Beginners, Parts I. and 11. Student at the Owens College (Even- ing Classes) 1891 and 1892.Arthur Harden. F. Gossling. G. H. Bailey. Geo. Stubbs. J. Woodward. H. B. Bixon. Parker, Alfred James, 21, East Hill, Dartford, Kent. Analytical Chemist. Three years’ training Finsbury Technical College, 1st Prizeman in Inorganic and Analytical Chemistry and Organic Chemistry. Honoursman in Practical Inorganic Chemistry, South Kensington. Six years Messrs. Burroughs, Wellcome and Co., Manufacturing Chemists, Dartford, Kent, Analytical Laboratory, and Chemist to the Physiological Department. One and a-half ,years Messrs. Parke, Davis and Co., Manufacturing Chemists, North Audley Street, W., and Detroit, U.S.A., Consulting Chemist and Superintendent of Laboratory. 3. H. Robbins. 12. Bufinister. R. Meldola. H. J. Helm. F. Harwood Lescher.J. Voodwccrd. Paters, Walter Charles Cross, 14, Trinity Square, S.E. Demonstrator of Public Health at Guy’s Hospital, Thos. Stevenson. John Wade. Charles E. Groves. Arthur R. Ling. William J. Pope. Ratcliffe, Walter, 21, Mawdsley Street, Bolton. Analytical and Consulting Chemist, Assayer, &c. Chemist to the Bolton Corporation. Late Chemist to the Dominion Cotton Mills Co., Montreal. George J. Allen. Charles A. Fogg. William B. Mason. Harold Rostron. Jno. L. TVhiteside. Smith, Francis Pitt, 77, Woodland Avenue, New Rochelle, N.Y., U.S.A. Bachelor of Philosophy in the course of Analytical and Applied Chemistry, School of Mines, Colurnbizt University, 1888. Tutor in Chemistry, Columbia University, 1897-98.Analyst, New York City Board of Health, 1890-91. Chemist, U.S. Navy Department, 1892-95. Papers : Editor, Anthonp’s Photographic Bulletin, 1893, ‘‘ Paint 2s a Protection for Iron,” the Engineers’ Club of Philadelphia. Nov. 16th, 1895. Charles F. Chandler. Arthur H. Elliott. Jas. 8. C. Wells. Hermann T. Vultb. Elwyn Waller. 8. A. GoZdsclmidt . Smith, Thomas De, Eastbourne College, Eastbourne. Natural Science Master. B.A., late Scholar of Jesus College, Cam- bridge. 1st Class Natural Science Tripos. 1st and 2nd M.B. Exami- nations, including Pharmaceutical Chemistry. Natural Science and Mathematical Master, Eastbourne College, M. 11.Pattison Muir. G. S. Turpin. S. Ruhemann. R. S. Morrell. Charles T. Heycock. J. E. S. Tuckett. Somerville, Henry, 33, Vincent Square, S.W.Lecturer on Chemical Physics at Westminster Hospital Medical School. Senior Lecturer on Chemistry United Westminster School. B.Sc. (London)-[Chemistry and Physics]. A. Dupr6. Jervis E. Foakes. C. F. Cross. Edward Bevan. H. Wilson Hake. 87 Spivey, William Thomas Newton, 5, Trumpington Street, Cambridge. M.A. Trinity College, Cambridge. Demonstrat.or to the Jacksonian Professor of Natural Philosophy, Cambridge. James Dewar. W. J. Sell. G. D. Liveing. H. J. H. Fenton. Thomas H. Easterfield. St.John, Harry, Thornfield, Sunderland. Wine and Spirit Merchant, Brewer and Analytical Chemist. Two years’ Certificate of attendance at Durham College of Science in Chemistry, Physics, and Mathematics.Two years’ pupilage at two Breweries in Practical Brewing. Two years’ pupilage in Analytical Chemistry applied to Brewing. Two years’ pupilage in Analytical Chemistry under London Analyst. Certificates from South Kensington in Organic and Inorganic Analysis, Advanced. Member of the Society of Chemical Industry. General Manager, Head Brewer, and Analyst to firm of William St. John for past six years. W. Dixon. W. H. Blake. C. Ranken. H. 0. Hale. William Fowler. Chas. Wm. Xutton. Walker, Samuel, 126, Gilmore Place, Edinburgh. M.A., B.Sc., Edin. Teacher of Chemistry in George Heriot’s Hospital School, Edinburgh. For seven years Teacher in Perth Academy, and in Sharp’s Institute, Perth, and Lecturer to Science and Art Classes in Chemistry, &c.For twelve years Chemistry Master in Heriot’s School, Edinburgh. Assisted the late Prof. Carnelly in his investigations on some Derivatives of Diphenyl. Alex. Crum Brown. Leonard Dobbin. Andrew Thomson. J. Gibson. W. H. Perkin, jun. Hugh Marshall. Williamson, John Alexander, 81, Cheverton Road, Upper Holloway, N. Analytical Chemist. Student at Glasgow University two years under Prof, J. Ferguson, M.A., and Prof. G. G. Henderson, M.A., D.Sc., F.I.C. ; five years under R. R. Tatlock, F.R.S.E., P.I.C., F.C.S., Glasgow ; one year as Chemist in Askam-in-Furness Iron Works, Lancashire ;two and a half years Laboratory Chemist, and Chemist in charge of manufacture to the British Explosives Synd., Pitsea, Essex. 88 At present Analyst to Messrs.Baird and Tatlock, London. Publication in J.S.C.Z. 1894, p. 1098. R. R. Tatlock. John Ferguson. G. G. Henderson. Wrn. Rintoul. W. R. Lang. Horatio Ballantyne. W. Msckean. Wood, Thomas Barlow, Caius College, Cambridge. Lecturer on Agricultural Chemistry. M.A. Caius College, Cam- bridge. James Dewar. W. J. Sell. G. D. Liveing. H. J. H. Fenton. Thomas H. Easterfield. Woodhead, Samuel Allinson, Agricultural College, Uckfield, Sussex. Science Lecturer and Analyst for the County of East Sussex. Lecturer in Chemistry (General and Agricultural) at the Agricultural College, Uckfield. Science Master at the Uckfield Grammar School. Bachelor of Science (Durham). Prizeman in Practical Chemistry. Public Analyst for the County of East Sussex and Town of Hove. Author of paper on Agricultural Chemistry. P. Phillips Bedson. F. C. Garrett. Saville Shaw. E. H. Farr. It. Greig Smith. John,M. Thornson. RICHARD CLAY AND SONS, LIMITED, LONDON AND BUNCAY.
ISSN:0369-8718
DOI:10.1039/PL8981400061
出版商:RSC
年代:1898
数据来源: RSC
|
|