摘要:

Issued 3/12/07 PROCEEDINGS OF THE CHEMICAL SOCIETY. Vol. 23. No.332. Thursday, November 21st, 1907, at 8.30 p.m., Sir WILLIAMRAMSAY, K.C.E., F.K.S., President, in the Chair. The PRESIDENTannounced that the Society has received a portrait of Farachy and Daniel1 from Professor Meldola, and a silver medal from the Socjbti: Chimiclue de France, struck in commemoration of the recent Jubilee celebration. Certificates were read For the first time in favour of Nessra. : John Arthur Ciwpenter, B.A., New College, Oxford. Cyril Dickinson, B.Sc., F.I.C., Abbotsford, Holycroft Avenue, Hampsteaii, N.W. Edward Mortimer Eagles, M, h., 5, Winsham Grove, Clapham Common, S.W. Robert Cecil Gale, 38, Scarsdale Villas, Kensington, W. George Neville Pingriff, B.A., 39, Hall Road, Handsworth, Staffs.William Bayliss Sham, Lonsdale House, WalsalL Harry Jackson Unwin, Market Place, Clay Cross, nr. Chesterfield. EIerbert Walker, Whyttington, Station Road, Wealdstone, N.W. Joseph Henry Williams, 27, Canbury Avenue, Kingston-on-Thames. Certificates have been aut.horised by the Council under Bye-lam 1 (par. 3) in favour of the following : Edward Henry Croghan, c/o Messrs. H. Eckstein & Co., P.O. Box 149, Johannesburg. Charles Thomas Foreman, Jamdpur, E.T.R.,Bengal. Of the following papers, those marked * were read :-*225. ". Emulsions." By Spencer Pickering. Paraffin oil, when churned with solutions of soap, glue, starch, albumin, &c., forms an emulsion which rises, like cream, to the sur€aceof the excess of water, and contains from 65 to 82 per cent.by volume of the oil. Close-packing of uniform globules mould give an emulsion containing 74 per cent. The percentage of oil can be increased to 99 per cent., the emulsion then being practically solid. Emulsification seems to depend on the separation from the liquid of very minute, solid particles which are attracted by, and surround, the oil globules, thus preventing them from coalescing. Any precipitated substance which is sufficiently finely divided will act as an emulsifying agent, but, after becoming agglomerated by drying, it loses this property. The basic sulphates of iron and copper are conspicuously good emulsifiers, and, when they are used instead of soap, it is possible to mix with the emulsions substances which could not be added if soap had been used; for example, sodium hydroxide.Solids which are not sufficiently fine grained to make true emulsions with oil, will sometimes made quasi-emulsions, in which the oil globules are merely entangled with the solid particles. In this case, dilution with water separates the oil from the solid, which is not the case with true emulsions. DISCUSSION. Dr. LEWKOWITSCHthought that all the phenomena mentioned by the author could be best explained by the colloidal state of the substances employed. He would therefore take exception to the explanation that the paraffin oil emulsified t,he soap solution, and would prefer to say that the soap solution emulsified the paraffin oil, Soap solutions were typical colloids, easily gelatinisable even in dilute solutions, and it was also well known how discoucerting soap solutions were once they had formed an emulsion with other substances, notably vegetable or mineral oils.The percentage (97) of paraffin oil in the emulsion shown appeared very high, and he therefore asked how much water and how much soap, presumably soft soap, were in the remaining 3 per cent. Soap solutions emulsified, not only paraffin oils, but also alcohol and notably very large amounts of water. The ferric sulphate and also the copper salt mentioned by the author were known to occur in the colloidal state, and therefore their property of forming emulsions mould exp!ain the phenomena referred to.The experiments shown with the emulsions produced by soap would fall in well with that explanation. On adding hydrochloric acid, the soap was decomposed with the formation of free fatty acids. 257 These, at any rate those formed in the given case, were not colloids, and therefore the emulsion was “broken” at once and water separated, the fatty acids remaining dissolved in the petroleum, The fact that caustic soda “ broke ” the emulsion was also easily explained, as caustic soda “salts out ” soaps, that is, precipitates them from their colloidal solution, and therefore water must separate out again. That in the experiment with lime no emulsion was formed could also be readily explained by adopting his view, for under the given conditions lime would not behave like a colloid.Mr. J. CASTELL-EVANSthought that surface-tension had a great deal, if not all, to do with the formation of emulsions, and that many finely-divided substances may be found which will induce the formation of emulsions of petroleum and water. He instanced a case, falling within his own personal observation, in an attempt at “ oil concectrn- tion ” of the metalliferous contents of some calcined tailings. These tailings consisted largely of ferric oxide and, after calcination, had been “ weathered ” for many years, On shaking up with water and mineral oil of about 0.89 sp. gr., the silicious matter, as expected, sank to the bottom of the cylinder ;so also did the coarser particles of ferric oxide, whilst the finer particles of the oxide remained in the oil, forming apparently a true emulsion. This “emulsion ” did not make the sides of the cylinder oily, and remained persistent for many months.The coarser particles of the oxide did not present a sufficiently large surface, in proportion to their mass, to be retained by the petroleum. Dr. BORNSinquired whether the author had succeeded in obtaining any emulsions of oil and pure water. K. Beck (Zeitsch.physikcd. Chem., 1907, 58, 409) had found that the viscosity of water was not affected when the water was churned with oil. When he prepared an emulsion of oil and water by rubbing the oil with some gum arabic in a mortar and adding water, however, the viscosity of the water was increased.The PRESIDENTsuggested that the suspended particles in an emulsion may be similarly electrified, and so repel each other and fail to coalesce. No doubt this phenomenon is closely connected with surface-tension phenomena. The addition of electrolytes may possibly discharge the electrified particles and cause coalescence. Mr. PICKERING,in reply, stated that the strongest emulsion which he had obtained contained only 1 per cent. of a 1 per cent. soap solution. The action of soap as an emulsifying agent was very uncertain, but that was not the case with insoluble emulsifiers. Such colloids as he had tried did not emulsify, but, on the contrary, became gelatinised. The basic sulphates were clearly not colloids ;the particles composing them could be seen under the microscope. No doubt surface-tension 258 played an important part in emulsification, but that offered no explanation of the phenomenon.Electrolytes, as such, had no effect on emulsions. "226. "Aromatic azoimides. Part 111. The naphthylazoimides and their nitro-derivatives." By Martin Onslow Forster and Hans Eduard Fierz. For the purpose OF studying further the triazo-group, and the con- ditions under which its properties are influenced by other groups, azo- imides of the naphthalene series have been examined. CloH7*N3(a),a-i~~~~~~thyZaxoipi~e7 melts at 12O, and does not yield hydrazoic acid when heated with alcoholic potash ;the 2-nitro-and 4-nitro-derivatives9 melting at 103-104" and 99" respectively, are resolved into the corresponding nitronaphthols and hydrazoic acid.The heteronucleal 5-nitro-and S-nitro-l-~ZCLphth?llaxOimides,melting at 121° and 130-131' respectively, do not furnish hydrazoic acid. P-Napl&th?llaxoimide,C1,H7~N3(P),melts at 33', and, like the heteronucleal 5-nitro-and 8-nitro-2-naphthyZaxoinaides7melting at 133.5" and 108" respectively, does not give hydrazoic acid. 1-Nitro-2-naphthyZazoimide, melting at 116-1 17O, is characterised by the readi- ness with which it loses nitrogen when heated, passing into the peroxide of /3-naphthaquinonedioxime, which is also obtained, but less readily, from the 2-nitro-1-naphthylazoimide; the 1-nitro-2-naphthyl-azoimide yields hydrazoic acid when heated with alcoholic potash.*227. The triazo-group. Part I. Triazoacetic acid and triazo- acetone (acetonylazoimide)." By Martin Onslow Forster and Hans Eduard Fierz. The interesting properties displayed by the triazo-group when -QHoN3,have led the authors to prepare occurring in the complex, -co the simplest typical compounds of this class, triazoacetic acid and triazosce tone. Triazoacetic acid, N,*CH,*CO,H, is a colourless substance, which crystallises in lustrous, transparent, hygroscopic plates, melting at 16'; it is a strong acid, has a faint odour recalling that of butyric acid, but much less pungent, and when dropped on a hot iron plate detonates with a moderate explosion, t,aking fire. The silver salt, C,H202N,Ag, crystallises from boiling water in lustrous, colourless needles, which decompose slowly when exposed to light; the ethyl 259 ester, C,H,O,N,, is a limpid, colourless oil, which boils at 45' under 2 mm.pressure, and has a very faint odour recalling chloroform rather than ethyl acetate. Triaxoacetarnide, N,*CH,*CO*NH,, crystallises from benzene in long, lustrous, colourless needles, melting at 58'. The derivatives of triazoacetic acid are much more sluggish in their reaction with concentrated sulphuric acid than is usually the case among compounds containing the triazo-grcup ; when shaken vigorously with the acid, however, nitrogen is liberated. A neutral solution of potassium triazoacetate may be boiled without undergoing change, but in presence of free alkali, two-thirds of the azidic nitrogen is eliminated in the elemental form, the remainder separating as ammonia.l'riazoncetone (ucetonylazoimide), N,*CH,*CO*CH,, is a colourless, limpid oil, which boils at 54' under 2 mm. pressure; the freshly prepared substance has a very faint odour recalling that of chloro-acetone, but much less pungent, spontaneously acquiring a suggestion of carbylamine after a few days. It is moderately soluble in water, and when shaken with dilute aqueous potash briskly liberates nitrogen, gas evolution being almost explosive when a 40 per cent. solution of alkali is used ;dropped on a hot iron plate, the substance detonates feebly, taking fire, and concentrated sulphuric acid decomposes it immediately.The semicarbaxone, C,H80N,, crystal-lises from hot water or absolute alcohol in long, lustrous needles, which melt without. evolving gas at 152'. The triazo-derivatives of acetone and acetic ester mere prepared by the action of sodium azide on the respective chloro-compounds. The authors are engaged in a study of the products obtainable from salts of hydrazoic acid and the halogen derivatives of acids, esters, ketones, aldehydes, and alcohols. DISCUSSION. Dr. KEANEasked whether Dr. Forster had examined the decomposi- tion products of the nzoimides of acetic acid and ethyl acetate when two-thirds of the total nitrogen was eliminated, and if so, whether imide derivatives of the aldehydes were obtained asin the case of the camphorylazoimide 3 Dr. FORSTERreplied that these compounds were being investigated.260 *228. “Studies of dpamic isomerism. Part VII. Note on the action of carbonyl chloride as an agent for arresting isomeric change.” By Thomas Martin Lowry and Egbert Hockey Magson. Labile solutions of nitrocamphor, in which isomeric change has been suspended, have been prepared (1) accidentally by dissolving nitro-camphor in chloroform, and (2) deliberately by adding acid to the solvent chloroform. In the latter case, the solutions acquired a powerf id odour of carbonyl chloride, and there can be no doubt that this is the efficient agent in arresting isomeric change in chloroform solutions. By means of this new agent, it is possible to arrest the isomeric change of nitrocamphor in other solvents.Thus a solution in benzene and N/lO,OOO carbonyl chloride, when stored in a quartz flask, showed n change of rotatory power of only 1.4” in twenty-five days, whilst a solution to which no carbonyl chloride had been added showed a similar change in four hours. In the same way, the velocity of isomeric change in ether was reduced to one-twentieth by the addition of N/lO,UOO carbonyl chloride, but no retardation was produced by the addition of acetic anhydride to acetic acid. *229. The electrometric determination of the hydrolysis of salts.” By Henry George Denham. The author has measured the hydrolysis of salt solutions with the hydrogen electrode. The E.M.F. of the cell, Pt,, I salt solution I saturated sol.of NH,NO, I calomel electrode, was measured, and from this the concentration of the hydrogen ion was calculated, A redetermination of the hydrolysis of solutions of aniline, chromium, and aluminium salts gave results agreeing well with those obtained by Ley (Zeitsch. physikal. Chem., 1899, 30, 193; Bruner, ibid., 1900, 32, 133; Bredig, ibid., 1894, 13, 289, and Bjerrum, ibid., 1907, 59, 336). In the case of the green chromium sulphate, the results obtained point to the conclusion that the equation given by Recoura (Ann. Chim. Phys., 1895, [vii], 4, 494) for the conversion of the blue sulphate into the green is not valid, but that the acid formed is produced through hydrolysis, and its amount depends only on the concentration and the temperature of the solution. In the case of the salts of zinc, magnesium, thorium, cobalt, and nickel, peculiar variations in the hydrogen ion concentrations have been noticed from day to day.The most probable explanation of this appears to be that the hydrolysis of these salts lead to hetero- geneous systems, in which the second phase (hydroxide or basic salt) is present in a colloidal form. 230. " The interaction of metallic sulphates and caustic alkalis." By Spencer Pickering. Alkalis, added to solntions of various nietallic sulphates, precipitate a definite basic sulphate, except in the case of manganese and mag- nesium, where the hydroxide is precipitated. After the precipita- tion is complete, the further addition of alkali converts the basic sul- phate either into another, sometimes consecutively into two other, more basic products (for example, copper and nickel), or into the hydroxide (aluminium).When one of the stronger alkalis (potash, soda) is used in excess, the product is probably always the hydroxide, but in the case of lime this does not appear to be so, at any rttte not with the sulphates of copper and nickel (see the following communi- cation). In every case examined, different alkalis have given the same results as regards the basicity of the sulphates precipitated by them in each particular case. The existence of the following eleven basic sulphates has been established in this way; the predominencc of 5 as the coefficient of equivalents of metallic oxide present is very noticeable. Those marked with an asterisk are the ones formed when the whole of the metal has been precipitated from the solution; the others are products of the action of further quantities of alkali : 6Ni0,3S03*, 6Ni0,2S02, 5A1,03,3x 2SO3*, 4Cu0,S03*, 4CoO,SO,*, 4Cd0,S03*, 5Cu0,S03, 5NiO,SO,, 5ZnO,SO,*, lOCuO,SO,, lOFeO,SO,*.231. '(The chemistry of Bordeaux mixture." By Spencer Pickering. The substances formed on the addition of lime to copper sulphate, as in the preparation of Bordeaux mixture, are dependent on the pro- portions of lime used, and may be either (1) 4CuO,S0,,0~06Ca80, ; (2) 5Cu0,S0,,0*25CaS04; (3) 10CuO,SO3,1~3CaSO,; (4) 10Cu0,S03,4Ca0,S0, ; (possibly 5) 10Cu0,S0,,10Ca0,S03, or (6) Cu0,SCaO ; that present in most cases probably being (4). The fungicidal action of Bordeaux mixture seems to depend on the liberation of normal copper sulphate by the action of carbon dioxide on the basic sulphate.The action begins only after a certain lapse of time, the basic calcium sulphate having to be decomposed before the basic copper sulphate is attacked, Ey using only sufficient lime to form 4CuO,SO,, the presence of basic calcium sulphate and the con-sequent delay in the action is avoided ; in addition to this, the amount of normal copper sulphate liberated (for a given amount of copper sulphate taken) and the insecticidal value of the mixture mill be two and a half times as great as when it consists of l@Ci10,80,,4CaO,SO,. The basic sulphates, when precipitated by lime in presence of excess of sodium sulphate, contain sodium sulphate as well as calcium sill-phate ;the formula of the most basic sulphate is lOCuO,SO,,(Na.,,Ca)SO,.When precipitated by soda, they contain no appreciable amount of sodium sulphate, unless a large excess o€ the latter is present in the liquid. Nickel sulphate with lime gives a basic sulphnte containing a very little calcium sulphste, but, if the lime is at all times in excess, the basic sulpbate is deprived of most of its acid, the precipitate consist- ing essentially of a double oxide. 232. '(The alcohols of the hydroaromatic and tcrpene series. Part I. Resolution of the alcohols into their optically active components and the preparation of the borneols." By Robert Howson Pickard and William Oswald Littlebury.An alternate method to that of the authors' (Z'TOC., 1906, 22, 71) for the resolution of racemic alcohols was described. The alcohol is combined with phthalic or succinic anhydride, and the resulting acid ester resolved by I-menthylamine or other strong optically active base. The optically active acid ester thus obtained is readily hydrolysed and yields the active alcohol in n pure state. I-Borneo1 was purified by three independent methods and found to have [a], -37.9" in toluene solution. d-Borneo1 was obtained from the reduction products of camphor by (i) treatment with zinc chloride in benzene solution, followed by (ii) conversion in the hydrogen phthalate and purification by means of the I-menthylamine salt.It then has [a], + 37.S' in toluene solution. isoBorneo1 (from camphene) was converted into the hydrogen phthzlate and resolved by means of I-menthylamino and cinchonine. The isobornyl hydrogen phthalates have [a], zk 76.8" in chloroform solution, and when hydrolysed readily yield the pure isoborneols, which have & 34.3' in ethyl-alcoholic solution. The identity of Haller's isocamphols (obtained by reduction of camphor), which had [a], 332.9" in ethyl-alcoholic solution, with the inactive isoborneol from camphene has long been assumed. The results described may be taken as proof of this, although it is probable that the product obtained from ''camphene " contains other substances besides d-and I-isoborneol.233. “The electrolytic preparation of disulphides. Part I. Dibenzyl-disulphide and diethyldisulphide.” By Thomas Slater Price and Douglas Frank Twiss. The electrolysis of the alkyl thiosulphateq (compare PTOC.,1906, 22, 260), which are used to prepare the disulphides, WRS originally per- formed in a beaker, without any diaphragm between the anode and the cathode, and the formation of disulphides was assumed to be due to the decomposition of the discharged anions, according to the equation 2R*S,O, =R,S, + 280,. Subsequent experiments, however, with divided cells, have proved the formation of disulphide to be due to the reduction of the alkyl thiosulphate anion at the cathode, according to the equation 2R*S,O,’ + 2H =R,S, + 2HS0,’.The best yield of disulphide is obtained by using a lorn current density, a concentrated solution, and current in excess of that theoretically required ;the addition of sodium carbonate or bicarbonate to the electrolyte is also advantageous. Although the piire alkyl thiosulphate compounds were used in the earlier experiments, it has been found quite satisfactory to electrolyse the mixture obtained by heating together sodium thiosulphate and the organic halide in aqueous-alcoholic solution ;a divided cell is then used. The bearing of the above results on the constitution of sodium tliiosulphate was discussed, since Gutmann, in a series of recent papers (Ber., 1905, 38, 1728 and 3276, &c.), favours the constitutional foi*mula0s>>S(ONa), in place of the usually accepted formula SO,(ON,z)(SNa).It WiiS shown that the former formula is not satis- factory, and that all Gutmann’s results are in accordance with the latter. 234. ‘‘The influence of solvents on the rotation of optically active compounds. Part XI. Ethyl tartrate in aliphatic halogen derivatives.” By Thomas Stewart Patterson and David Thomson, The rotation of ethyl tartrate has been determined in methylene chloride, carbon tetrachloride, ethylene chloride, ethylidene chloride, acetylene tetrachloride, bromoform, ethyl bromide, ethylene bromide, acetylene tetrabromide, methyl iodide, methylene iodide, and ethyl iodide at various temperatures and concentrations. The values found were compared with those for molecular solution-volume.To some extent an inverse relationship holds between these variables. In all the solvents under consideration, the rotation of the dissolved ethyl 264 tarlrate is depressed below that of the homogeneous ester, whilst, on the other hand, the molecular solution-volume becomes greater than the molecular volume. Amongst the individual dab also an inverse proportionality often obtains, but a correlation between the two variables cannot be traced through all the solvents examined, since exceptions are both numerous and important. 235. “The interaction in solution of ferrous sulphate and copper sulphate.” By Henry Russell Ellis and William Henry Collier. When ammonia is added to copper sulphate solution, the distinctive blue coloration is not obtained or is rendered indistinct if ferrous sulphate is present.If excess of ferrous sulphate is present, no coloration is produced, whilst the iron is precipitated as ferrous and ferric hydroxides ; the solution contains cuprous compounds, and a small quantity is present in the precipitate. The production of the ferric hydroxide is brought about by the oxidising action of the compound CuSO,, 5NH,OH, and the amount of oxidation is proportional to the amount of this sub- stance present. Complete oxidation is brought about when both the copper and ammonia are present in excess. The authors have been able to oxidise the whole of the iron in a few minutes in the cold by using the proportions 10NH,OH, CuSO,, and $FeSO,. Solutions of ferrous sulphate, on boiling, become hydrolysed, giving an acid solution.No action takes place between ferrous sulphate and copper sulphate solutiom in the cold, but, on boiling, the copper sulphate slowly oxidises the ferrous hydroxide produced by hydrolysis. 236. (‘Mercurous hyponitrite.” By Edward Divers. A paper with the above title, by P. C. RAy, published in the August number of the Tvansuctions, having been taken as rend, opens with the following words : ‘‘ Mercurous hyponitrite, which has already been obtained in a somewhat impure condition by the author (Tvans., 1897, 71,348), may be prepared (a)by precipitating mercurous nitrate with carefully neutralised sodium hyponitrite made according to Divers’ method (Trans., 1899, 75, 96, 119); (bj by precipitating mercuroso-mercuric nitrite (Rgy, Trans., 1902, 81, 644) with the crude alkaline hyponitrite ; or (c) by precipitating mercurous nitrate with acid potassium hyponitrite (Thum, Inaug.Dissert., 1893).” Any 265 one unacquainted with the facts referred to will hardly get a correct notion of them from this obscure sentence. These facts are (1) that Thum in an unusually brilliant inaugural dissertation on hyponitrous acid gave, in 1893, a description, accompanied by excellent analyses, of the mercurous salt among others ; (2) that, in 2897, there appeared a paper by R$y describing, as new, mercurous hyponitrite (in admixture with a mercuric salt) obtained from sodium hyponitrite by adding it to a solution of mercuroso-mercuric nitrite, a solution he had resort to (notwithstanding the complications likely to ensue consequent upon the presence in it of mercuric salt and upon its being a solution of a nitrite) because he supposed that mercurous nitrate would not serve for the purpose, in consequence of the acidity of its solution ;and (3) that., beyond this pointless substitution of a solution of one mercurous salt for another, Ray’s paper contained nothing new, nothing so good as had been already published, and yet something beneath criticism about a supposed mercuric hyponitrite (see I’rans., 1893, 75, 119). 122~’s recent paper, besides implying that mercurous hyponitrite, prepared by Riiy’s reagent, has now been obtained free from mercuric salt in some way not even alluded to (the evidence for this being some new analyses, three out of four of which are not a whit better than those of the admittedly impure preparations), contains only the state- ment that this preparation of Ray’s (possibly containing nitrite) cannot be dissolved in nitric acid without immediately yielding metallic mercury, notwithstanding the fact that Thum was able to reprecipitate the salt in a pure state from its solution in nitric acid, as his analysis and description establish, and that the writer (Trans., 1899, 75, 121) has published experience similar to Thum’s, each working with salt of high purity.237. Decomposition of mercurous and silver hyponitrites by heat.” By Edward Divers.R$y and Gaiiguli have not succeeded in giving a definite and consistent interpretation of the results which they have recorded in their recent paper on the decomposition of mercurous and silver hyponitrites by heat (Trans., 1907, 91, 1397). They have not perceived that these results are impossible as they stand, and must be corrected if they can be. The corrections called for in the case of the silver salt lie well within the limits of errors in the experimental analyses, whilst, in the case of the mercury salt, the justifiable assumption of the presence of nitrite fairly well accounts for numbers otherwise too far from what the pure salt would have given. Had the authors been aware of the imperfect nature of their results, 266 in the case of the mercury salt, they would presumably have deferred publication of them.But, even as published, these results seem capable of such revision and subsequent interpretation as may make them add materially to the knowledge of the decomposition of hypo-nitrites by heat. The two hyponitrites examined evidently decompose when heated each in three ways, which are expressed by the following equations. For the mercury salt, these are: (HgON),=2Hg+ZNO (1); (HgON), = Hg + HgO + N,O (2) ; 3(HgON), = 4Hg + (HgNO,), + 2N, (3). In Rby and Gafiguli’s mode of procedure, it would seem, on probable calculation, as tabulated below, that 2-96 out of 6.09 parts of the salt will have decomposed according to (1) ; 2-32 parts according to (2), and 0.81 part according to (3).Or, in percentage numbers, 48.6, 38, and 13.3 according to equations (1), (2), and (3) respectively. In the case of the silver salt, where we are on much surer ground, two of the equations are just like (1) and (3) for the mercury salt, whilst the otlier, which only differs from (2) as given for the mercury salt because of the instability of silver oxide, is (AgON), =2Ag + O+N,O (Y), the free oxygen of which with 2NO by equation (1) becomes first N,O,, let us say, and then nitrite, on contact. with the solution of potassium hydroxide, as R&y and Ganguli explain. Ultimately, therefore, the second equation becomes Z(AgON), = 4Ag+N20,+N,0, but, for the sake of comparison with the mercury salt, it seems better to use the equation showing free oxygen and count the nitrite nitrogen along with that as nitric oxide.The conclusion that must be come t.0, after inspecting the tables, will be that Ray and Gaiiguli had really 7.84 (=6*58+1.26) parts out of 10.15 of the silver salt decomposed according to equation (1) ; 1.26 parts according to (T),and 1-05 parts according to (3) (Ag being read for Hg). Or, 83, 13.3, and 3.7 per cent. respectively according to equations (I), (27, and (3). Reference to the authors’ paper will show that they have themselves put forward equations (1) and (a), that they reject (3), and that they suggest others which, it may here be said, could not be worked in with their results in any likely way.The interpretation, here submitted, of the effects of heating the two hyponitrites is derived from the numbers exhibited in the subjoined tables. Distribution of the Nitrogeqt and Oxygen of Mercurous Hyponitl'ite in the Products of its Decomposition by Heat. Product. N,. N,O. NO. N,O,. NO,. HgO. Total. Theory, N found ... 0.54 2'32 2.53 0.24 0.48 -6-11 6'09 0 ), ... -1-33 2.89 0.41 1.65 1.19 * 7'47 6.96 N calc. ..... 0.54 2'32 2'96 -0'27 -6.09 6-09 0 ,, . . .. . . -1'33 3.38 -0'92 1-33 6.96 6'96 Distribution of the Nitrogen and Oxygen of Silver Hyponitrite in the Products oj. its Decomposition by Heat. Prociuct. N,. N,O. NO. N,03. NO,. Total. Theory. N found ...... 1-06 1.15 6.58 1-26 0.35 10.40 10.15 0 ,, . . . ... -0'66 7-52 2-16 1'20 11.54 11'60 N calc..........0.70 1'26 6'58 1'26 0.35 10.15 10.15 0 ,, . . ....... -0'72 7'52 2.16 1'20 11.60 11-60 * See note on page 1400 in RBy and GaBguli's paper. The numbers in the first line of each table are the mean numbers of those given by the authors for the nitrogen of the several products as parts per cent. of the salt. The column headed N,O," shows the nitrogen of the nitrite in the potassium hydroxide solution t,hey made use of. The column "NO3" shows the nitrogen, obtained or calculated, as mercurous or silver nitrate. In the case of the mercurous hyponitrite, the distribution of the nitrogen as nitrite and nitrate has been assumed to have been in all three experiments as 1 :2, in agree- ment with what it was found to be in the only reported experiment in which it was determined by the authors.The numbers in the second line of each table are for the oxygen corresponding with those for the nitrogenin the first line. Their sum, in the case of the mercury salt, is much in excess of the percentage of oxygen in merciwous hyponitrite. Since the mercurous hyponitrite, which the authors made use of, had been prepared from mercuroso-mercuric nitrite, the excess of oxygen found may be attributed to the presence of nitrite in the salt as prepared. The column headed, HgO, shows the oxygen left as mercuric oxide as being necessarily equal to that in the nitrous oxide, less (in the Eecond line) by one-third of that as nitrous anhydride (1.33-0.14 = 1.19). The numbers in the third and fourth lines of each table have been calculated in accordance with the equations already given, and in such a way as to make them differ the least possible from the numbers furnished by the experiments, under the necessary condition that their respective sums shall be identical with the percentages of nitrogen and oxygen in the pure mercurous and silver hyponitrites.In the case of the mercury salt, it has been assumed that, when free 268 from nitrite? mercurous hyponitrite yields no red fumes and very little nitrate, which is in accordance with the writer’s experience, referred to by the authors. The numbers for the silver salt have been altered to make the free nitrogen equal to only twice that found as nitrate; that found as nitrous oxide to be equal to that as nitrite, and total nitrogen and oxygen to be equal respectively to the percentages of these elements in the pure salt.A noticeable point in Rby and Gaiiguli’s paper is their experience of the conversion by heat of nearly one-eighth of silver hyponitrite into silver, nitrous oxide, and oxygen. The writer did not observe the presence of any nitrous oxide in his experiments (T~ans.,1899, 75, 108). Nor has any other worker recorded the fact of having done so. On the evidence afforded by Rby and Gaiiguli’s experi- ments, the writer is prepared to admit that nitrous oxide may never be absent altogether in the products of the decomposition of silver hyponitrite by heat. As to the matter of quantity of nitrous oxide, the details of their experiments and his are sufficiently different to account for the fact of their obtaining so much of it and he so little as to pass unnoticed.The salt they used contained, they think, impurities enough to be mentioned, and began to decompose very slowly at looo, and at 140’ suffered rapid decomposition. It had been dried cold over sulphuric acid under reduced pressure, but was heated to decomposition in a tube between which and the Sprengel pump a tube of “aqueous potash” intervened. A very little moisture would have given a lower temperature of decomposi-tion, and caused free generation of nitrous oxide. In the writer’s experiments, salt of high purity, dried finally in a Sprengel vncuum at 98O, was used.Thus dried, the pure salt hardly begins to decom- pose at 140°, and is not in free decomposition much, if at all, below 160O. It would seem highly probable from the difference in the effects of heat that the generation of nitrous oxide is largely, if not wholly, a matter of hydrolysis. Another point worthy of attention in Rby and Gaiiguli’s paper is their contention that nitric peroxide is a secondary product arising out of the union of nitric oxide with the oxygen set free along with nitrous oxide. The writer thinks this to be highly probable. His position as to nitric oxide and nitric peroxide being primary products has been that for twenty years, he held, without proof, that nitric oxide was the primary product which produced red fumes by contact with air.Thum proved, in 1893, that out of contact with air the salt still gave nitric peroxide when heated. The writer then examined the matter himself for the first time and found Thum right. Having ascertained that nitric peroxide and silver gave silver nitrate and nitric oxide, he concluded, in 1899, that nitric peroxide was the primary 269 product and nitric oxide secondary. Now he returns to his first view and agrees with RAy and Gaiiguli that nitric oxide is the primary product, at the same time being certain that it is also reproduced by reduction of the nitric peroxide by silver. It is much to be desired that RAy and Gaiiguli would repeat their experiments, making use of piire mercurous hyponitrite prepared by Thum and the writer’s process, and of the driest pure silver hypo- nitrite, in their apparatus supplied with some solid potassium hydroxide in the near end of their absorption tube.238. Cupric nitrite.” By Edward Divers. A paper appeared not long ago in the Tyansuctions (1907, 91, 1405) on cupric nitrite, in which RAy sets forth his observations on what he regnrds as being the atmospheric oxidation and autoxidation of this salt. Now nitrites, as such, do not oxidise and, in the cases where they do not hydrolyse in water, they are stable in solution. (The passage of cobaltous into cobaltic nitrite is, of course, no exception to the state- ment.) What R&yhas occupied himself with is simply the oxidation of nitrous acid, not cupric nitrite, in aqueous solution.For when a cupric salt is dissolved in water, it is always hydrolysed to some extent, as is shown by its acid reaction and other facts. Nitrous acid in aqueous solution becomes nitric acid and nitric oxide, and nitric oxide oxidises in the air. When it is added that nitric acid decom- poses some of the cupric nitrite to form nitrate together with more free nitrous acid, there seems to be no more to be said. As to the oxidation of cupric nitrite, as such, we are left as we were, without any evidence whatever of its occurrence. ADDITIONS TO THE LIBRARY. I. Donations. Bunge, Gustav von. Text-book of organic chemistry for medical students. Translated, with additions, by R. 11. Aders Plimmer. pp. ix + 260. London 1907.(Recd. 8/11/07.) From the Translator. Duparc, Louis, and Monnier, AIfred. Trait6 de chimie analytique qualitative. Suivi de tables systdmatiques pour l’analyse min6rele. pp. viii+ 374. GenAve 1908: (Recd. 16/11/07.) From the Publisher : Librairie Kundig. Frankel, Sigmund. Descriptive Biochemie mit besonderer Beriick- aichtigung der chemischen Arbeitsmethoden. pp. xi + 640. Wies-baden 1907. (Recd. 16/11/07.) From the Publisher : J. F. Bergmaan. 270 Haller, Albin, and Girard, Chcwles [and others]. Memento du chimiste (ancien Agenda du chimiste). pp. xx + 758. Paris 1907. (Recd. 16/11/07.) From the Publishers : Messrs. H. Dunod and E. Pinat. Hanneke, P. Photographisches Rezept-Taschenbuch. pp. iv + 175. Berlin 1907.(Recd. 16/11/07.) From the Publisher : Gustav Schmidt. Manchester. Rivers Department. Annual Report for the year ending March 27th, 1907. (Red 1/11/07.) From the Rivers Committee. 11. By Purchase. Blyth, Alexuncler WyTzter, and Blgth, Meredith Fynter. Poisons : their effects and detection. Fourth edition. pp, xxxii + 772. London 1906. (Recd. 26/6/7.) Handbuch der anorganischen Chemie. Edited by Richard Abegg. Vol 111, part 3. pp. xiv + 876. Leipzig 1907. (Rpfererzce.) Kauffmann, Hugo. Die Auxochrome. (Ssmmlung, Vol. XII.) Stuttgart 1907. (12ecd. 9/8/7.) Le Blanc, Max. Text-book of electro-chemistry. Translated from the fourth enlarged German edition by IViZZis R. Whitney and John IV. Brown. pp. xiv + 338. ill. New York 1907.(12ecd. 26/6/7.) Nernst, TValther. Experimental and theoretical applications of thermodynamics to chemistry. pp. x + 123. ill. London 1907. (Recd. 2/7/7.) Oswald, Adolfi Lehrbuch der chemischen Pathologie. pp. vi + 6 14. Leipzig 1907. (Ziecd. 20/11/07.) Post, Julius. Chemisch-technische Analyse. Randbuch der annlytischen Untersuchungen zur Beauf sichtigung chemischer Betriebe. Edited by Bernhard Neumann. Vol. I, parts 2 and 3. Vol. 11, part 2. pp. 307, 326, 350. ill. Braunschweig 1907. (Becd. 1/10/7.) Schwalbe, Carl G. Neuere Farbetheorien. (Sammlung, Vol. XII.) Stuttgart 1907. (Becd. 9/8/7.) Stange, Albert. Die Zeitalter der Chemie in Wort und Bild. pp. xiii +528. ill. Leipzig 1907. (Recd. 20/11/07,) Thausing, Julius E. Die Theorie und Praxis der Malzbereitung und Bierfabrikation.6th edition. pp. xxviii +1280, and atlas. Leipzig 1907. (Recd. 20/11/07.) 111. Pamphlets. Albo, Giucomo. Sui principii alcaloidici dei semi di tabacco. (From Bull. Xoc. bot. ital., 1902.) Albo, Giacomo. Sul significato fisiologico della nicotina nelle piante di tabacco. 1901. Ancora sulla fisiologia della nicotina nelle piante di tabacco. (From Bull. SOC.bot. ital., 1907.) Andrews, E. C., and Mingaye, J. C. H. The geology of the New England Plateau, with special reference to the granites of Northern New England. Part IV. Petrology. (From the Records Geol. SUY. N. S. Vales, 8,1967.) Essex Education Committee. The Essex Field Experiments, 1906. Report by B. TV. Bull and V. H.Kirkham. Chelmsford 1907. Market-day Lectures, 1905-6, being report3 of addresses to farmers, delivered at Chelmsford and Colchester during the winter months. Chelmsford [1907]. Notes on agricultural analyses, 1903-1906. Compiled by V. ZI. Kirkham. Chelmsford 1119071. Herty, Clmrles H. Industrial and scientific aspects of the pine and its products. (From the Chemical Engineer, 1907.) Hooper, David. Well-waters from the Hadhramaut, Arabia. (From the J.am1 Proc., Asiatic Soc. of Bengal, 3,1907.) The fats of Gurcinia species. (From the J. and Proc., Asiutic SOC. of BengC6l, 3,1907.) Leaxher, J. Filter. The pot-culture house at the Agriculturitl Research Institute, Pusa. (From the Mem. Dept. Agric. IRdia, 1, 1907.) The composition of the oil-seeds of India.(From the &!em. Dept. Agric. Indicc, 1,1907.) Experiments on the availability of phosphates and potash in soils. (From the Menz. Dept. Ayric. Indict, 1, 1907.) Midland< Agricultural and Dairy College. Reports on expel-i-ments with crops and stock, carried out . . . in theyear 1906-1907. Mingaye, J. C. A. Notes on analyses and tests of Japanese coals. (From the Zfecords Geol. Sur. A? S. Wales, 8, 1907.) Oshima, Ki7~tnro. On the constituents of rush-pith. (From the J.Sapporo Agi-ic. Coll., Jupan, 2, 1906.) Plimmer, R.H. Aders. The work of Emil Fischer and his school on the chemistry of the proteins. (From Science Prog~ess, 1907.) Power, Prederick B., and Tutin, Prank. Chemical examination of Grindelia. (From the Proc.Amer. Pl/,urm.Assoc., 1905.) Reade, J.iVellard, and Holland, Philip. Analyses of Ludlow rocks. (From the I’roc. Liverpool Geol. Soc., 1906-1 907.) Richards, Theodore TViZliccnz, Staehler, A., Forbes, G. S., Mueller, E., and Jones, G. Further researches concerning atomic weights of potassium, silver, chlorine, bromine, nitrogen, and sulphur. Curizegie lrtstitution of FVashinyton,Publication No. 69, 1907. 272 Richards, Theodore William, Stull, W. N., Brink, F. N., and Bonnet, P. The compressibilities of the elements and their periodic relations. Carnegie Iqstitution of Washington,Publication No. 76, 1907. Waidner, C. W., and Burgess, G. K. Preliminary measurements on temperature and selective radiation of incandescent lamps.(From the Bull. Bureau of Stccndavds, Wccshington, 2, 1906.) Radiation from, and melting points of, palladium and platinum. (From the BUZZ.Bureau of Standards, Washington, 3,1907.) RESEARCH FUND. A Meeting of the Research Fund Committee mill be held in December next. Applications for Grants, to be made on forms which can be obtained from the Assistant Secretary, must be received on, or before, Monday, December 9th, 1907. All persons who received grants in December, 1906, or in December of any previous year whose accounts have not been declared closed by the Council, are reminded that reports must be in the hands of the Hon. Secretaries not later than Monday, December Znd, next. At the next Ordinary Meeting, on Thursday, December 5th, 1907, at 8.30p.m., there will be a ballot for the election of Fellows, and the following papers will be communicated : “The affinity constants of bases as determined by the aid of methyl- orange.” (Preliminary note.) By V.H. Veley. “The velocity of reduction of the oxides of lead, cadmium, and bismuth by carbon monoxide, and the existence of the suboxides of these metals.” By F. J. Brislee. “The relation between unsaturation and optical activity. Part I. The menthyl and bornyl esters of P-phenylpropionic, cinnamic, and phenylpropiolic acids.” By T. P. Hilditch. “The constituents of the essential oil of nutmeg.” By F. B. Power and A. H. Salmay.‘‘Methyl ethers of some hydroxyanthraquinones.” By A. G. Perkin. “The colouring matters of the stilbene group.Part IV. The action of caustic alkalis on paranitrotoluene and its derivatives.” ByA. G. Green, A. H. Davies, and R. S. Horsfall. “The replacement of alkyl radicles by methyl in substituted ammonium compounds.” By H. 0. Jones and J. R. Hill. 273 CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.B.-The names of those who sign from “General Knowledge ” are printed in itntics. The following Candidates have been proposed for election. A ballot will be held on Thursday, December 5th, 1907. Banks,Arthur John, 61, Lawton Road, Waterloo, Liverpool. Research Chemist. Studied Theoretical and Practical Chemistry and Microscopy in the laboratory of the late A. Korman Tate, F.I.C., F.C.S., 7-11, Hackins Hey, Liverpool (1881-2-3-4) ;have since been continuously engaged in analytical and research work ; th‘e past 44 years (1902-7) have been devoted to an enquiry into the factors governing the ‘I strength and other qualities ” of wheat. Contributions : “Note on the Liboratory Drying Oven,” Chem.brews, 58, 54 (1888). Note on “A New Chemical Test for Strength in Wheat,” Nutui-e, 75,460-1 (1907).1 ColIaborated with F. W. Fellowes in the preparation of the following papers, viz. : (1) “Some of the Micro-organisms Causing the Diseases of Beer,” Frans., North oj England Institute of Technical Brewing, 3,107-136 (1894), on p. 129 reference is made to my apparatus for cultivating anaerobic organisms by means of plate growths ;(2) “Facts, Fancies, and Fallacies,” Trarts.of the E’edernted Institutes of Brewing, 2, 247-272 (1896). Further reference to my work was made by Alf. Jorgensen in his paper “ Han-sen’s System of Pure Yeast Culture in English Top Fermentation,” Trans., Institute of Brewiqag, 7,235, 246 (1894). Horace T. Brown. W. J. Cousins. Arthur R. Ling. Frccncis €lens.y I’ute. George 2’. Holloway. . Barnett, Edward de Barry, 40, Queensborough Terrace, Hyde Park, W. Research Student, University College, London. William Kamsay. J. Norman Collie. It. W. Gray. Edward C. Cyril Baly. I;.D. Porritt. Bell, John Forbes, Craigmillar, Edinburgh. Brewer’s Chemist. Bronze Medallist and First Class Honours Certificate in Brewing, City and London Guilds Institute. Studied Chemistry under Mr.John Hunter, F.I.C., F.C.S., Analyst for County of Midlothian, &c. Member of Committee of the Scottish Section of the Institute of Brewing. John Hunter. John S. Ford. Matthew J. Cannon. John M. Guthrie. John Doull. Buckney, Frank, 51, Highbury Park, London, N. Demonstrator in Cambridge University Laboratory. Honours in Chemistry, Tripos Parts I. and IT. Cambridge. Original research : ‘‘ A New Optically Active Tetrahydroquinoline Compound,’’ delivered before Cambridge Philosophical Society. F. H. Neville. H. 0. Jones. W. J. Sell. F. E. E. Lamplough. J. Parkin. F. W. Dootson. Callan, Thomas, 22, Church Street, Egremont, Cheshire, Research Chemist. Assistant Chemist to Messrs. J. Woolley, Sons, and Co., Manchester, 1900-3.B.Sc., Victoria University of Man-Chester, with First Class Honours in Chemistry, 1906. Am now Research Assistant to Prof. J. Campbell Brown, Liverpool Univer- sity. J. Campbell Brown. D. L. Chapman. A. W. Titherley. H. B. Dixon. J. F. Thorpe. Caton, Frederic William, 6, King Street, Snow Hill, E.C. Research Chemist at Wellcome Chemical Research Laboratories. B.A. (Oxford), B.Sc. (London). Have spent one gear in Research in Mr. J. E. Marsh’s Laboratories at Oxford. Frederick B. Power. J. E. Marsh. John Watts. TV. W. Fisher. hllan F. Walden. R.de J.Fleming-Struthers. Crisp, George Hugh, 62, Gainsboro’ Road, Crewe. Chemistry Master at; the Cheshire County School, Crewe. B.A. 275 (Oxon.) ; Third Class Honours in Natural Science (main subject : Chemistry).Wishes to keep in touch with recent researches in Cb e mis try. N. V. Sidgwick. H. B. Hartley. A. F. Walden. A. Angel. D. H. Nagel. 11. Byereton Baker. Day, Edward Joseph, Darchester. Doctor of Medicine (Durham University). MedicJ Officer of Health (Rural and Urban), Dorchestor Borough and Darchester Rural Ssnitnry District. Over twenty years both app:)intments. M.D. (Durham) ; M R.C.S. (Enghnd) ; L.S.A. (London). Late Public Analyst for Boroughs of Dorchester, Eridport, and Lyme Regis. John Hunter. Fredk. Hudson-Cox. A. H. M. Muter. Edward Russell. Chay. J. Wnterfall. Dupre, Frederick Harold, Mount Edgcnmbe, Satton, Surrey. Business address : 2, Edin-biirgh Mansions, Homick Place, S.W.Analytical and Consulting Chemist. Ten years Assistant to the late Dr. A. Duprb, F.R.S. At present, jointly with my brother, P. V. Dupr6, Acting Chemical Adviser to the Explosives Department o€ the Home Office. Otto Hehner. Bernard Dyer. W. J. Dibdin. Henry E. Armstrong. Gerald T. Moody. Dupre, Percy Vivian, Mount Xdgcumbe, Sutton, Surrey. Analytical and Consulting Chemist. Associate of the City and Guilds of London Institute. Eight years’ work under the late Dr. Duprb, F.R.S. Have had two papers published in the Analyst (Aug., 1905, and July, 1906). Acting Chemical Adviser to the Explosives Depart- ment of the Home Office in conjunction with my brother. Otto Nehner. Bernard Dyer. W.J. Dibdin. Henry E. Armstrong. Gerald T.Moody. Dutton, Francis Bridger, Birch Hall, Windlesham, Snrrey. Slitdent in Chemistry, Oxford, Magdalen College. A. F. Walden. I). H. Nagel. N. V. Sidgwick. T. 8. Moore. 14. B. Hartley. 276 Fawcitt, Claude Scott, Darlington, England, and Sliimoga, S.M. Ry., India. Analytical Chemist. Undergradnate of Durham University. Seven years in laboratory of Messrs. J. and H. S. Pattinson, Newcastle-on- Tyne. Three years Chemist at Illessrs. Tho Vizisnagram Mining Coy.’s Manganese Mines, and at present Analyst to The Mysore Man- ganese Coy., Ltd. A. mT.Comber. J. T. Dunn. John Pattinson. P. Phillips Bedson. If: C. Guwett. Greenough, Thomas Rigby, Beechwood, Leigh, Lancashire. Graduate of University of Cmibridge (Natural Science TIipos, 1907).Analytical Chemist under Sir Charles Cameron, Dnblin. Worked three years in Chius College Laboratory, Cambridge, under M. M. Pattison Muir. AT. nil-. Pattison Muir. Percy Bean. W. H. Leek. Frank Scudder. Charles T. Heycock. 1-20bert Pettigrew. Hay,William, Holton IIouse, Beverley Road, Hull. Student in the Research Laboratory of the Pbarmaceuticstl Society. “Minor ” and ‘‘ Major ” examinations of the Pharmaceutical Society. Arthur W. Crossley. F. Filmer De Morgan. E. Towyn Jones. W. Palmer Wynne. M. 0.Forster. Hutchinson, William Doge, Lythmore, Tenn yson Road, Harpenden, Herts. Engaged in Research at Rothamsted Experimental Station. Second Class Honours in Chemistry at Oxford. A. D. Hall. D. H. Nagel. N.H. J. Miller. H. H. Hartley. R. T.Lattey. Ingham, Harry, 26, Hamilton St. Bury, Lanes. Lecturer at the Technical Scliool, Bury. Master of Science (Vict..). Contributed to the “Transactions of the C.S., 1907, Vol. 91,”in conjunction with Dr, J. F. Thorpe and Dr. E. F. J. Atkinson, a paper 27 7 on the ‘‘Formation and Reactions of Imino-compounds. Pt. 111.” I wish to keep in touch with the progress of Chemical Research. W. H. Perkin, jun. Norman Smith. J. F. Thorpe. J. C. Cain. William Dixon. Jones, Benjamin Owen, Boksburg, Transvaal. Chemist (M.P.S., Gt. Britain). Member of the Legislative Assembly, Transvaal. Member of the Transvaal Pharmacy Board (Government Nominee). Examiner in Pharmacy to above Eoard. Member and Vice-chairman of Rand Provisional Joint Committee (Hospitals) and Chairman of East Rand Hospitals (Witwatersrand).M. Carteighe. Peter MacEwan. J. Rymer Young. John C. Hewlett. E. J. Millard. Kaye, John, Westerfield, Perth. Research Chemist (on Glass in N.B. Glass Works, Perth). M.A., B.Sc. (Glasgow) in Piire Science. Chemistry taken both in First and Final Examinations. Acted as Demonstrator in Senior Laboratory (Glasgow University). Eighteen months’ research on “Optically Active Compounds.’’ Two papers published on ‘‘Optical Superposition,” I’ra7zs. of Chenz. Soc., 1906, Vol. 89 ; 1907, Vol. 91. T. S. Patterson. Charles E. Fawsitt. Frederick Soddy. Thomas Gray. John Ferguson. Marsden, Herbert, Bramford, Ipswich. Chemist.B.Sc., Manchester. Assisted Prof. Kipping during the past 12 months in bis work on I‘ Organic Silicon Compounds.” Chemist at Messrs. P‘ickard & Co.’s Agricultural Works, Ipswich. Harold B. Dixon. \V. H. Perkin, jnn. F. Stanley Kipping. J. L. Simonsen. R. 31. Crtven. Francis Jones. Marshall, Hubert Frederick Sankey, High Street, Burmell, Cambs. Analyst. Pupil to E. M. Chaplin, Esq., Ph.D., two years. Student Wakefield and Glo’ster Technical Schools, three years. Junior Analyst to Messrs. Stephenson’s, Ltd., Cement Works, Burwell. Now Chemist-in-Charge to Messrs. Stephenson. Edward M. Chaplin. George Embrey. Robert Stephenson. J. M. Collett. Jack V. J. Hayman. Bobert J. Caldwell. 278 Martin, Gerald Hargrave, Delce, Park Ed., Wallington, Surrey.Wholesale Optician’s Assistant. Chemicd Student, Birkbeck College. A1ex. McKenzie. George W. Clough. W. G. Tonoer. Henry Wren. H. F. C. Goltz. Moore, John Edward Langford, Walton Cottage, Loughboro’ Park, S.W. Head Dispenser to St. Bartholomew’s Hospital, E.C. Teacher of Practical Pharmacy and Demonstrator in Materin BIedica to St. Butholomew’s Hospital Medical School. Member of the Pharmaceu- tical Society. My desire for Fellowship arises from my wish to have access to the Society’s Library and Literature and to keep myself in touch with advanced chemical knowledge. P. D. Chattaway. J. A. Ormerod. W. H. Hurtley. W. L. Howie. Kenneth S. Caldwell. TIT. J. 12usseZl. Mummery, Charles Samuel, Christ’s Hospital, West Horshani.Undergraduate of Idondon University, and at present engaged in advanced experimental work in Chemistry. Is desirous of being in a position to attend the Scientific Meetings of the Society, and also of receiving the Society’s Journal and Proceedings. Henry E. Armstrong. Chas. E. Erowne. Gerald T. Moody. W. A. Davis. T. H. Boardrmn. IVilliam Bobertson. Saunders, George Joseph, School of Mines, Charters Towers, Queensland, Australia. Demonstrator and Assistnnt Lecturer in chemistry, Assaying, and Metallurgy, School of Mines, Charters Towers, Queensland. Three years Student in Chemical and Metallurgicnl Laboratories, University of Sydney, N.S. W. Graduated as B.E. (Mining and Metallurgy), 1004, Syd. Univ. Eight months Assaying and Manager of Cyanide Works, Nil Desperandum Gold Mine, Forbes, N.S.W.Nine months Assaying, Mt. Eurow Copper Mine, N.S.W. One month Assaying, North Lachlan Gold Mine, Forbes, N.S.W. J. A. Schofield. Charles Walker. Basil Turner. A. Liversidge. George Hurkw. Smith, Robert Harry, Apsley House, Priory Road, Sheffield. Undertaking private analysis aucl research. Science Teacher, holding South Kensington (Science and Art Department) Certificates in Inorganic and Organic Chemistry. Trained at the Royal College of Chemistry, London. Ft ank Clowes. G. T. W. Newsholme. W. Gowlnnd. J. ZI. Coste. TVn2. Jno. Livingsto,,. Stobie, Harold Ramsay, “Clovelly,” Craighall Gardens, Edinburgh. Analytical Chemist. Certificates in Physics and Chemistry (Part I) of the Heriot-1Vst.t College, Edinburgh.Certificate for the complete course of Chemistry and Allied Subjects of the Royal College of Science, Kensington, S.W. James C. Philip. H. E. Fierz. M. 0. Forster. G. T. Morgan. C lmpm an Jones. Thomas, Frederick, B.Sc., 29, Fairhaven Road, St. Anne’s-on-the-Sea, Lapcs. Assistant Research Chemist. Hons. in Chemistry, University of Msnchester, 1906. Research Student till March, 1907. Joint author, with Drs. Bentley, Friedl, and Weizmann, of ‘‘Derivatives of Naphthacenequinone ” (Tyans., 1907, 9 1,41 1). Siuce March, 1907, Research Assistant to Messrs. A. G. Perkin and W.P. Bloxam at Leeds University for Research on Indigo under the Government of India. H.B. Dixon.: Norman Emitb. W.$3. Perkin, jun. A. G. Green. J. F. Thorpe. A. G. Perkin. W. P. Eloxam. Tinipany, Harold Munkman, St. Winifrede’s Gardens, Shrewsbury. Principal, Technical Schools, Shrewsbury. M.Sc. (Vict.). Principal of, and Lecturer in Chemistry at, Shrewsbury Technical Schools. Author of following School Text-Books : ‘(Arithmetic of Chemistry and Physics ” (Blackie) ; ‘(Qualitative Analysis Tables with Equa-tions and Notes ” (Blackwood). H. B. Dixon. Norman Smith. G. 1%.Bailey. J. F. Thorpe. D. L. Chapman. 280 Watson, George Arthur, 7, Roseneath Villas, Cork. Chemistry Lecturer, Co. Cork Technical Instruction Committee. Consulting Chemist. Associate of Royal College of Science, Faculty of Applied Chemistry.Teacher of Chemistry, Cork Grammar School. W. N. Hartley. H. If. Atkinson. James H. Pollok. Jno. Northing. A. J. O’Farrelly. 1’. Uwtrum Roy. Wechsler, Marcus, 136, Sinclair Road, Kensington, W. Analytical Chemist. D.Sc., Grenoble (France). Contribution to ‘‘The Study of Acenaphthene ” (Dissertation, Grenoble, December, 1906). Contribution to Th. Zincke’s ‘‘ Method for Condensing Hydro- carbons mi th Benzylchloride ” (Dissertation, Grenoble, December, 1906). ‘’The Constitution of Eenzylacenaphthene ” (Bull. SOC.Cl~im., (3“) T. 31-32, p. 922). At present engaged on Analytical and Research Work at Gillman and Spencer, London. Alex. McKenzie. G. W. Clough. Henry Wren. H. B. P. Humphries. JV. G. l’onner. Wheeler, Edward, 113, Highbury Quadrant, London, N.Assistant in Chemical Dept., at Central Technical College, South Kensington. Associate of the City and Guilds Institute (A.C.G.I.) in Chemical Dept. Henry E. Armstrong. William A. Davis. William Robertson. Edward Horton. T. Martin Lowry. JOhN vUF$!C6S &??/re. WalkerJ€.Glover. Whymper, Robert, St. Clare, St. Mary’s Road, Ditton Hill, Surrey. Research Chemist. Associate of City and Guilds Institute. Salters’ Coy.’s Research Fellow. Henry E. Armstrong. Robert J. Caldwell. Wm. Robertson William A. Davis. John Vargas Eym Edward Horton. Williams, Percy, c/o The Wilhelmina Go., Pontianak, Dutch West Borneo. Chemist. B.Sc., London. “The Borides of Calcium, Strontium, and Barium,” in collaboration with H.Moissan (C.E., 1897). Two papers on ‘‘Double Carbides” (C.B., 1898). “The Transition Point of Echomt,” in collaboration with Prof. vitn’t Hoff. “ The Hydrates of 281 Manganese Chloride,” in collaboration with H. M. Dawson (Zeit.Phy. Chew,., 1899). “ A New Method for the Determination of Transition Points,” in collaboration with H. 11. Dawson (Amer. ,TOUT. Phy. Cheni., 1899). 1900-1906, Chemist to the “British Uralite ” Com-pany, Higham, Kent. 1906, Chemist to the ‘(Wilhelmina” Co., Pontianak, Dutch West Borneo. William Ramsay. J. Norman Collie. Frank Collingridge. N. T. M. Wilsmore. G. Nevi11 Huntly. Samuel Smiles. Noel Heaton. Willott, David, B.Sc., Rosedale, Thorncroft Road, Sutton, Surrey. Science Lecturer.Was a student of Chemistry at the Blanchester Technical School, and afterwards at the South-Western Polytechnic, Chelsea. Have been a lecturer in Chemistry for 15 gears at the Swa nsea Municipal Technical School, the Sutton Technical School, stc. ‘I’ook the B.Sc. Degree of the London University with Honours in Chemistry. I wish to become a Fellow of the Chemical Society that I may keep in touch with current chemical literature. F. H. Lome. J. C. Clocker. Sidney Skinner, John Il’ilsoiz. J. L. White. Wilson, TFilliam John, 28, Windmill Street, Gravesend, Kent. Analytical Chemist. Associate of the City and Guilds of London Institute. Assistant Chemist to the Associated Portland Cement . Manufacturers (1900), Ltd. Henry E. Armstrong.Edward Horton. William Robertson. W.A. Davis. Gerald T. Moody. Wootton, Hubert Arthur, B.A. (Cantab.), B.Sc. (Lond.). 20, Great College Street, Westminster. Science Master in Westminster School. Formerly Assistant Demonstrator in the University Chemical Labor‘Ltory, Cambridge. Formerly Assistant Lecturer of Clare College, Cambridge. W. J. Sell. H. J. H. Fenton. T. B, Wood. H. 0. Jones. 11. Brereton Baker. The following certificates have been authorised by the Council for presentation to Ballot, under Bye-law I (3) : Groghan, Edward Henry, c/o Messrs. H. Eckstein & Go., P.O. Box 149, Johannesburg. 282 Analytical Chemist, M atriculation and full chemical course at the South African College, Cape Town, froin 1899-1902. Also Laboratory Assistant to Professor Holm for 2 years.1903-1906, assistant Analytical Chemist to Blessrs. H. Eckstein & Co. At present, Chief Chemist to this firm, I have written two papers for the Chemical, Metallurgical, and Mining Society of South Africa, and om for the British Association at their meeting in South Africa. I wish to keep in touch with Chemical progress. James Moir. J. McCrae. Foreman, Charles Thomas, Jamalpur, E.I.R., Uengal, India. (Chief) Chemist and Metallurgist to the East Indian Railway. From M;ti.ch, 1887, to Dee., 1899, Assistant Chemist to the Consett Iron arid Steel Co., Durham. Paul Briihl. W. I?. Criper. David Hooper. lY. 1'.Grim. Schober, William Bush, Lehigh University, South Bethlehem, Pa., U.S.A. Professor of Chemistry. B.Sci., 1886; A.M., 1890, St. John's College, Annapolis, Maryland. Ph.D., Johns IZopkins University, 1893. Instructor in Chemistry, Lehigh University, 1892-1902 ; Assistant Professor, 1902-1 906 ; Professor, 1906. Ira Remsen. Chas. H. IIerty. Chas. B. Dudley. Chas. Bnskerville. Mctrston 1: Bogelat. R. CLAY AND SONS, LTD.. BHEAL, ST. HILT., R.C., AND SIUN(ihT, SLTFFOLK.

ISSN:0369-8718    

DOI:10.1039/PL9072300255

出版商:RSC    

年代:1907

数据来源: RSC