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Proceedings of the Chemical Society, Vol. 8, No. 115 |
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Proceedings of the Chemical Society, London,
Volume 8,
Issue 115,
1892,
Page 141-184
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摘要:
Issued 29/11/1892. PROCEEDINGS OF THE CHEMICAL SOCIETY. -No. 115. Session 1892-93. The following are abstracts of papers received during the vacation and published in the Transactions :-44. “ Some homonudeal tri-derivatives of naphthalene (Peri-dibromonaphthniene).” By R. Meldola, F.R.S., and C. H. Desch (Trans., 1892, 765). It is shown that Prager’s statement (Bey., 1885, 2163) that the NH, group in 2-nitro-4-bromo-1-amidonaphthalenecannot be dis- placed by bromine by Sandmeyer’s method is incorrect; and a description is given of the 1: 4-dibromo-%nitronaphthalene,and also of the corresponding chlorobromo- and iodobromo-naphthalenes ; all three substances are described as crystallising in small, ochreous needles melting at 117”. On reduction, they yield amiries almost destitute of basic properties, which readily oxidise in air; their acet.yl derivatives crystallise in white needles, bromiodo-p-acetnaph- thalid melting at 235”,the chloriodo-compound at 218”. A lengthy footnote is appended to the paper, in which the con-clusion arrived at by Armstrong and Rossiter (these Proceedings, No.104,7,I%),that when a mixture of ortho- and para-nitracet- naphthalid is brominated, the ortho-compound is alone attacked, is corroborated ; and in which the interestiug statement is made that one of the authors and F. W. Streatfeild have prepared peridibromo- naphthalene from 1: 1’-nitrobromonaphthalene : this new dibromo- naphthalene meits at about 109”. 45. “ A method of measuring the vapour pressures of solutions.” By Thomas Bwan, B.Sc., Ph.D., aud W.R. Ormandy (Trans., 1892, 769). A condensation hygrometer for determining vapour pressures of solutions at ordinary temperatures is described and figured. The 142 hygrometer consists of a thin polished silver cup soldered to R stronger ring of brass, which in its turn is cemented into a glass tnbe by means of tinfoil and sulphur ; the upper end of the tube is closed with a cork, through which pass a tbermometer and an open tube carried down below the surface of the ether placed in the silver bulb, a side tube near the top being connected with an aspirator in such a way that the amount of air passing through the ether is under the control of the observer. The hygrometer is suspended in a glass regsel containing the solution under examinntion ; this consists of a cylindrical bulb with a long narrow neck, a narrow side tube through which the rod of a stirrer passes being sealed into the shoulder of the bulb.The temperature is determined at which dew first becomes visible on the silver bulb. Results obtained with solutions of sodium and cupric chloride are given in the paper. 46. “ The hydrazines of qninoline.” By S. F. Dufton, B.A., D.Sc. (Trans., 1892, 782). A description is given of an improved method of nitrating quin- oline, and of a variety of derivatives prepared from the ana-corn- pound. To nitrate quinoline, the nitrate prepared from 50 grams is added in about five portions to 50 C.C.of strong sulphuric acid contained in it litre flask, 10 C.C. of fuming salphuric acid (d = 2.0) being poured in after each introduction of nitrate, the mixture being kept cool. The yield is very good, 200 grams of ana- and 150 grams of ortbo-nitroquinoline haviug been obtained from 300 grams of quinoline in one operation. A small quantity (equal to about 3 per cent. of the quinoline taken) of a dinitrohydroxyquinoline is formed ; this sub- stance very closely resembles trinitrophenol. The compounds described are the ana-amine and hydrazine, the semicarbazide, pyruvic hydrazone, acetone-hydrazone, benzaldehyde- hydrazone and anaquinolineme thylpyrazolone prepared from the hydr- nzine and anaquinindole-a-carboxylicacid. It is pointed out that in the case of both ortho-and ana-derivatives, one remarkable feature common to both is the intense red colour of the mon-acid salts of the amine and hydrazine.The pgruvic hydrazone separates from an aqueous solution as a bright red, crystal- line precipitate differing from the corresponding ortho-compound by being soluble in water, and by its vivid colour; this, however, changes to yellow, on drying, with loss of water of crystallisation. 143 47. “ The origin of colour (IV). Note on tbe appearance of colour in quinoline derivatives and of fluorescence in quinine salts.” By Henry E. Ai-mstrong (Trans., 1892, 789). Attention is directed to the fact that it could scarcely have been lwedicted that the anaquinoline derivatives such as are described by Dr.Dufton would manifest colour, and it is argued that they arc probably qcinnnoid compounds : that the appearance of colour, in fact. if,conditioned bv the occurrence of an isodynamic change in -volvinc the passage from the “centric” structure of quinoline to the “ethenoid” structure of a qninone. Further, it is suqgested that it may eventunllv prove to be possible to explain the fluorescence of certain salts of quinine by the application of a similar principle. [Correction and dddendun~.-Tt. is stated in t,he foregoing note that “ The ortho-derivatives described hy Dr. Dufton, excepting the pvru& hydrazone, apparently are colourless substances.” This, as Dr. Dufton has pointed out to the writer, is not the case.The mistake-an en tirely inexcuw blP one-appears to hsve been made owing to the absence from Dr. Dufton’s paper describiny the ortho- compounds of any reference to the colour of the acid salts of the nrnine and hydrazine; it is only incidentally. in the paper on the ana-derivatives, thrit he mentions that the intense red colour of the mon-acid salts of the anline and hydrazine is a, remarkable feabure conimon to both ortho- and ana-series : although an entry of this fact was originally made when my attention was first called to the work* in writing out the “note,” the descriptions of the individual compoulcls were apparently alone consulted, and the incidental reference to the coloixr of the ortho-compound was consequentlv overlooked. Alt,hough at present deprived of the forcible arpument which t.he non-appearance ‘of colour in the ortho-series would afford, I see no reason to abandon my contention that the colonred aua-compounds are of peculiar structure.Dr. Dufton’s tliscoveries have, in fact, added greatly to the interest attaching to the study of quinoline derivaAives, and it is necessary that the ortho-derivatives should he examined with special cme. So many cases are now known in which substances long regarded as uniform, definite compounds have proved to be composite that it is justifiable, in my opinion, to recard the ortho-derivatives with suspicion until their homogeneity has been placed beyond question.-H. E. A.] 48. “Dicarboxyglutaconic acid ,’’ By S. Ruhemann, Ph.D., and R.S. Morrell (Trans., 1892, 791). The action of phen ylhydrazine on ethylic d icarboxyglut nconic acid and its benzyl derivative is shown to resemble that of ammonia, the 144 final products being a pyrazolone derivative and ethylic nialonate or benzylmalonat.e, the pjrazolone derivative being formed by con-densation from the substituted Rmidoethylenedicarboxylate first produced. Phenylpyrazolone a,nd several of its derivatives are clescribecl. 43. “ Action of nitric acid on anthracene (II).” By A. G. Perkin and J. FJ. Mackenzie (Trans., 1892, 865). One of the aut,hors has previously shown that compounds of anthracene with either ethylic or metbFlic nitrates are formed when solutions of anthracene in ethylic or niethylic alcohol are treated with nitric acid.It is now shown that the corresponding propylic, isobutylic and benzylic compounds niay be prepared by using the appropriate alcohcls ; no corresponding product coidd be obtained from triinethylcarbinol, the action of nitric acid on the solution of nnthracene in this alcohol giving rise to nitrosoailthrone. Under slightly modified conditions, the action of nitric acid on nnthracene dissolved in isobutylic alcohol is found to give rise to a compound which the authors regard as nitroanthroiie, this is converted into the isomeric nitroanthrol by treatment with ;tl(wliolic potash. On treating anthracene dissolve3 in acetone (Kahlbaum’s pure) with nitric acid, the compound of nnthracene wit11 methylic iiiti-ate mas produced in such quantity as to negative the assump- ticn that it was derired froni methylic alcohol present in the acet- (,lie: it would therefore seem probable that the acid acts on the acetone forming methylic nitrate and acetic acid.Using methyl- ated ether carefully freed froni alcohol, the compounds of anthr-:-1 wne with both ethylic and nieth-j-lic nitrate were obtained. 59. (‘ The behnvioixr of ethylene on explosion with less than its own volume of oxxgen.” By B. Lean, B.A., B.Sc., and W. A. Bone 13.8~.(Trans., 1892, 873). After giving a brief account of previous observations, the authors describe a series of experiments in which mixtures of ethylene with it,s own or a less volume of oxygen were fired in a leaden coil.Their results are in agreement with those of Dalton, Kersten and E. von %!eyer, and show that, when fired with about its own volume of oxygen, ethylene eventually yields mainly carboiiic oxide and 145 hydrogen ; but they have also observed that metliane, acetylene and carbon are prod uced. The following are the tabulated results 08 the analjsea :-Composition of mixture. c. D. E F. a. Etbjlene ........... 56.03 5418 49.771’ 48.64 49.41 Oxygen ............ 39.46 41.52 45-83’45.84 47.69 Nitrogen ........... 4-51 4.30 4.42 5.52 2.90 Composition of product. C. D. E. P. G. Unsaturated hydro-carbons .......... 5.53 3.77 2.78 2-14 -Methane ........... 5.96 3.77 2.32 25.5 1.01 Carbon dioxide ...... 1-63 2.80 1.24 0.194 0.33 ,, monoxide.... 38.!35 44-84 47.i9 46.53 49-11 Hydrogen. .......... 43.30 41.72 43.32 45.35 48.78 Nitrogen.. .......... 5.16 3s.10 2.35 2.49 1.01 Incidentally it is shown that mygen is-appreciably absorbed by fuming sulplinric acid, but that neither strong potash nor alkaline pyrogallol solution appreciably affecbs ebhylene. 51. “The lowering of the freenuing points of cadmiumj bismuth and lead when alloyed with otheri metals.” By C. T.’ Heycock, M.A., and F.H. Neville, M.A. (Trans,, 1892,888). The authors have considerably extended the inquiry of which they have previously given a short account (these Proceedings, No. 88). A very large number of data are recorded in tbe paper. From the>e it is apparent that the “atomic fall,” i.e., the rat’io of the fall in freezing point of the alloy below that of the pure solvent to the number of foreign atoms present per 100 of solvent, is independent of the concentration when the solution is dilute.As the concentra- tion increases, a gradual change takes place, however, in the atomic fall value. In a few cases, such as that of gold in cadmium or tin, and of mercury in cadminm, there is an increase in the atomic fall as the concentration increases, bat in most cases the reverse is true. The various possible causes of change in atomic fall with increasing concentration are considered, and, after calling attention to the fact that Van’t Hoff’s formula is strictly true only of infinitely dilute solutions, a formula applicable to finite concentrations is suggested ; on the assumption that the molecule of the substance in solution contains 1 atom, the different atomic fall values ccrresponding to different numbers of atoms of foreign metal per 100 of solvent 146 are calculated, and it is then pointed out that on taking a general survey of the atomic falls given in the tables in the paper and comparing them with the molecular falls predicted by the theory of osmotic pressure, it is apparent, not only that the experimental nutn- bers are identical in a great many cases with the theoretical fall piv- duced by a monatomic molecule, but that the experimental numbers, while often lower, aye nevey higher than the theoretical number.This is an important point in favour of the osmotic theory of solution, for this theory, whilst, readily explaining a low atomic fall by the hypothesis of the dissolved molecule containing more than 1 atom, assigns a, superior limit, corresponding to the state in which the molecules in solution contain each 1 atom of ihe dissolved substance.In presence of these numbers, it seems impossible to resist the conclusion that the process of dissolution consists essentially in the disintegration of the dissolved substance and its uniform diffusion through the solvent as a gas; in other words, hhat the “physical theory of solution ” is correct. In some cases, however, for instance that of gold dissolved in cadmium and a few others, the aiithors have n.o doubt that the molecule in solution contains atoms of both metals.52. “Isolation of a compound of gold and cadmium.” By C. T. Hepock, M.A., and F. H. Neville, M.A. (Trans., 1898, 914). The compound has the composition represented by AuCd, and is of A greyish, silvery-wh ite appearance, like cadmium. It was prepare. I Iiy alloying gold with cadmium and moderately heating in a VRCUUIU so long as cadmium distilled away. The immediate interest of thc compound is that it corifirms the supposition advanced by the authors to account for the remarkable behaviour of gold and cadmium when dissolved in tin. 53. ‘(The resins of Ficus rzcbiginosa and F. mmrophylla.” By E. H. Rennie, D.Sc., and G. Goyder, Jun. (‘l’rans., 1892, 916). An account is given of the results of an examination of the resin of F.rubilqinosa by De la Rue arid Miiller, contained in a paper pub- lished in the Phil. Trans. of 1860, and the somewhat different rcsults of the authors are then recorded. They have separated a crystalline substance from both resins externally closely resembling De la Rue and Muiler’s product, but giving numbers for carbon about 3 per cent., and for hydrogen about 1 per cent. higher ; the nnrnbers are most in accordance with the formula C,iH,,02. This substance is resolved hy alkaline hydrolpis into acetic acid and a crystalline sub-stance melting at 114”, of the formula C32H510,very closely re- sembling the substance described by De la Rue and Muller, which they obtaiiied in a similar way. 54. “The hydrolytic functions of yeast.Part 11.” By James O’Sullivan (Trans., 1892, 926). A further series of experiments on the hydroljtic activity of healthy yeast cells are described, the following being a summary of the con-clusions arrived at :-1. The hydrolytic action of yeast at ordinary temperatures (12” to 20” C.) follows the same course as that of a simple chemical inter- change, and is not influenced by either air or carbon dioxide. 2. A time curve representing the action would correspond with that given for invertase under the most suitable conditions of acidity by O’Sullivan and Tompson (0. 8. Trans., 1890, 57, 878). The rate, thertfore, differa from that at which the alcoholic fermentation of yeast takes place, which would be represented by a straight line (Dumas, An?),.Chirn.Phys. L3], 1874, 81; and A. J. Brown, C. S. Trans., 1892, 384). 3. Any interference involving either an increase or a diminution of the natnr.it1 acidity of the yeast cell diminishes its action. This is it vcry important matter, and should always be considered when dealing with organisms or cellular membranes possessing the power of hydro-lysing cane sagar. Dumas observed that both acids and alkalis interfered with alcoholic feymentat’ion, and that in the case of alkalis the yeast possessed the power of overeoming the alkalinity, the liquid again becoming acid and fermentation recommencing. It is found that a quantity of potassium hydrate which completely arrested the hydrolytic action of yeast for thi=ee to six hours was neutralised by the yeast in about 24 hours, the solutions eventually becoming acid and hydrolysid recomm.encing. 4.It is inferred trom experimenba on the effect of rupturing the cell on the velociiy of the hydrolytic action, and also from the rate at which the chaiige pmceeds, thah the whole of the invertnse of the yeast cell comes into action rn soon as the cane sugar is added to the yeast, and that it continues to act during the progress of the hydro- lytic action. 5. The power which yeast possesses of producing alcoholic fermenta- tion is not influenced by the yeast having first hydrolysed cane sugar, this being the case whether the hydrolytic action is brought about in the first instance in the presence of air or carbon dioxide.55. “ Iniidosulphonates.” By E. Divers aud T. Haga (Trans., 1892, 943). The authors have obtained sodium imidosulphonate for t.he first 148 time and from sodium nitrite by a modification of Fremy's mdhod of preparing the corresponding potassium salt (sulphnniid~tc). The potassium salt is nearly insoluble in water, but the sodium salt is exceedingly soluble ; and whereas the direct preparation of t,he former has provnd to be uncertain and the yield unsatisfactory, the latter can be obtained from the nitrite almost without loss. Probably the potassium salt could be much more easily prepared than it has been were the here-described modified process adapted to its production ; but the sodium salt is a much more useful agent because of its solu- bility, and the potassium salt can at once be prepmed from it by precipitating with potassium chloride.Sodium nitrite and sodium carbonate (crptals) in tlie proportions shown by the equation 2NaN02 + 3Na&03 + 850, = 2N(S03Na)3 + Na2S20,+ 3C02 are placed in a flask together with a little water and a rapid stream of sulphur dioxide is passed into the magma. The flask needs to be agitatcd, and during the latter part of the process to be kept cool. When neutrality is approached, the gas is to be passed in more slowly, and is to be stopped just when lacmoid paper is first permanently reddened. Two salts are now present in the liquor, sodium nitrilosulphonate and mstasulphite, but in a fcw minutes hydrolysis of the nitrilosulphonate sets in, giving disodium imido- sulphonate and acid sulphate, and the latter acts on the metasulphite, forming sulphurous acid and disodium sulphate.By thus taking up the sulphuric acid, tbe metasulphite entirely prevents subsequent hydrolysis of the imidosulphonate into amidosulphonate. After expelling sulphur dioxide by a rapid current of air, a little sodinni carbonate is added to make the liquor slightly alkaline, and enough of the water is evaporated off at a gentle heat. On cooling to near O", most of the sulphate crystallises and can be removed. The con- centrated mother liquor affords hard, brilliant crystals of almost pure imidosulphonate ; from its mother liquor more sulphate and imido- salphonnte can be alternately separated.The imidosulphonate can be safely recrystallised from slightly alkaline warm vrater or by cold evaporation. It forms large, rhombic prisms of the composition HN(S03Na),,(OH2),, feebly acid to litmm, which only very slowly lose water in a vacuum. Like the potassium salt, disodium imidosulphonate is not precipi- tated by many of the ordinary agents, because nearly all other imidosulphonates corresponding to it are soluble. It, however, affords precipitates with sodium hydroxide, potassium chloride or nitrate, bariiim hydroxide, strong ammonia-water, basic lead acetate, 149 and mercuric and mercurous nitrates ; most of these act also on the dipotassium salt. Sodium hydroxide precipitates trisodium imido- sulphonate ; and the same salt is formed by evaporating Lhe disodium salt with sodium carbonate, or with sodium acetate if the evaporation is repeated.Potassium chloride precipitates the dipotassinm salt. Ammonia precipitates a sodium ammonium salt, and also when the solutioiis are very concentrated triammonium irnidosulphonate ; but in presence of other sodium salts, nitrate or chloride, ammonia pre- cipitates pure t#risodium imidosulphonate, leaving ammonium nitrate or chloride in solution. Baryta-water gives a barium sodium imido- sulphonate. T’risodium imidosulphonate, NaN(S0,Na),,(OH,)12, crystallises in thin plate9, sparingly soluble in cold water, freely soluble in hot water. It is a very stable salt, easy to prepare and to preserve for uiilimited periods.Tt is an alkaline salt, and when neutralised with sulphuric acid furnishes a solution from which the disodium salt can be crystallised out. In a vacuum the crystals lose only 11 mols. of water ; t>he other one can be expelled by heat, almost completely. A number of other imidosulphonates of corresponding composition, often double salts, can be prepared from the trisodium salt by precipi- tation ; ammonium imidosulphonates can be also prepared from it, through the intermediation of the barium hydrogen salt, or the basic lead salt, or the silver salt. Berglund, 18 years ago, established the fact that diammonium imidnsulphonate is Rose’s parasulphatammon, still described in the latest English text books (Ramsay, Mendel4eff) as ammonium aniido- sulphonate. The authors find that dry diammsnium imidosulphonate, an anhydrous salt’, combines with dry ammonia to form anhj-drous triammonium imidosulphoriate, and that this is Rose’s aulpbatammon.They have +so prepared in the wet way a triammonium imidosulph- onate with 1 mol. of water, isomorphous with tripotassium imido- aulphonate. Barium imidosulphonate is precipitated as a voluminous matted mass of microscopic, fibrous crystals, in appearance like an organic salt. Barium hydrogen, barium ammonium, barium sodium, barium potassium imidosulphonates are all crystalline salts. Of the double calcium salts, the sodium compound may be mentioned as forming stellate groups of thick, often very brilliant, prisms. Besides a very soluble, unstable lead hydrogen salt, a prismatic tri-hemihydroxy-lead salt’, (HOPb),N(S0,)2, and a tetra-lead salt, HO(HOPb)4N(SO,),, which are both insoluble, may be obtained No double lead salts can be prepared; the hydrogen salt is known only in solution.The interaction of trisodium imidosulphonate and silver nitrate is 150 specially remarkable for giving in succession three strikingly different precipitates :-AgNiizN( SO,),, in the form of fibrous, pale yellow crystals ; Ag2NaN(S03)?,a sparkling, white " sand " of microscopic, hexagonal crptals, all detached ; and Ag3N(S03),, a white precipitate, drying on the tile to chalk-like masses. The relation in composition of these three silver salts IS also interesting for its rare, if not excep-tional, character. The following double mercury salts are well-defined compounds which have been examined in detail because of their interest as being at the same time sulphonic and nitrogen salts of mercury :-Neither a single mercupy imidosulphonate nor any mercurous salts can be prepared.Berglund's belief in the existlence of a specially stable mercury iinidosnlphonic acid is not confirmed by the authors' observations, for although mercury dipotassium imidosulphonate readily exchanges its potassium for barium and other metals, it keeps its potassium and exohaiiges its mercury for hydrogen when treated with nitric acid ; and, besides, mercury hydrogen imidosulph- onate is apparently less stable than imidosulphonie acid itself.Diammonium imidosulphonate forms a double salt with sodium nitrate, and so does the dipotassium salt. The existenee of these compounds and of tho pentahydroxytetm-lead salt and the retention of 1 mol. of water by the trisodium salt left in a vacuum-desiccator seem to show that imidosulphonntes preserve some of the power of ammonia to unite with acids md milts, the nitrogen becoming quin- quevalent, thus :-H (SO,PbOH),' Ho"K(PbOH), The effect of beating ammonium and potassium imidosulphonates has been examined by previous workers, but their observations are defective. Diammonium imidosulphonate melts and boils near 357", and flows back almost unchanged. Violent ebullition for an hour has little effect, if moisture he rigorously excluded.But the salt decom- poses to a small extent like the potassium salt. Dipotassium imido- sulphonate is decomposed only at the softening point of good soft lime glass into potassium sulphate, atnrnonia, sulphur dioxide and nitrogen. The carefully dried disodium salt behaves similarly. The trisodium salt at the same high temperature gives sodium sulphate, sulphur and nitrogen. Lead, silver and mercury salts are some-what more easily affected by heat : in their case, besides products such as are above enumerated, mercury and even its sulphide, silver and silver sulphide, lead sulphide and sulphite are among the products. The barium salt decomposes explosively. Anhydrous imidosulphonates of potassium or sodium, alone or with otlier metals, when heated to about 130” and upwards in ordinary air slowly increase in weight and become acid, being hydrolysed by the atmospheric moisture.This fact is the more interesting in that at about the same temperature amidosulphonates, heated in dry air or in a vacuum, give off ammonia and become imidosulphonates, as was first observe11 by Berglnnd. Soon after the appearance ofAuDEN1)U~~.-oxyan~i~~os,~phonates. the authors’ last paper (J. Chem. Soc., 55, i65), which treated of oc~.ya?ni~’~sulphonates,Dr. Rnschig wrote to request them to state on his behalf that he agreed with their account of the decom-position of these salts by causfic alkali, and wished to withdraw his own statement which had been based 011 qualitative observations only.56. “ Modification of Beckmann’s boiling point method of deter-mining UAOlecUhr wei-ghts of substances in solution.” By Joji Sak urai, The great experimental diGulty afEecting Becbniann’s well-known method is the exact determinstion of the boiling points. A thermo-meter dipped into a boiling liquid always gives irregular readings, but this difficulty may be completely overcome by the nietliod already described by $he author in his paper on “ The determination of the temperature of steam arising from boiling salt wlutious ” (C.S. Tram., lS91), which consists in passing a current of the vapour of the solvent into the boiling liquid, tlie amount of the vapour 1,huspassed in being regulated by the height of the lamp. The dqgree of con-stancy of $he temperature attained in this manner by the boiling liquid is really astonishing, a most delicate thermometer capable of showing 1/10Gutls of a degree rernairiiiig almost stationary.The apparatus used is of the simplest construction and can be set up by any one with materials commonly found in all chemical laboratories. Another advantage is that the boiling point of the solution is ascertained just before its con~positionis determined, the connection between these properties being, therefore, rendered more certain than in the case of Beckmann’s method. The following table (p. 152j gives an example of the results ob-taiiied. The author confirms the statement, first made by Beckmann, that t8he difference in dour of iodine when dissolved in ether and in carbm bisulphide is not due to a difference in the state of its molecular aggregation, the numbers obtained for the molecular weight of iodine, Solvent : Etkyt Ether.0*02T2Lat. Ht. Vap. = 90.1 (Regnault, 1862) ; b.p. = 34O.9 C. 7= 21.0. g substance Observed Diff.Substance. I 7 solution r subst.ance. g solvent. per 1009 molecular per 100.3olvent. lolution Rise. solvent. weight. --~-------------------c--------Salicylic acid, C,H,OH.COPH= 138 .. 1*013 1'397 0 *384 6 -9880 0 '1733 6 -8147 2 -543 139-1 +o 8 .. 1 '337 1-661 0 -324 7 -2700 0,1591 7 *I109 2 *237 145'0 +5-1$9 .. 0 -986 1*236 0 *250 7 *1384 0 -1174 '7 '0210 1'672 140.4 +1.7 +)) crr w Naphthalene, CloH, = 128 ...........0 -739 1'464 0 '725 7 -2743 0 *3128 6.9615 4 -493 130-1 +1*7 ........... 1*038 1-541 0.503 7 -0014 0 -2143 6 '78'71 3 *la 131.9 + 3 *o3) ........... 1275 1*542 0 -267 7.0232 0 -1112 6-9120 1*609 126'6 -1 -19) Iodine, 12 = 254.. .................. 1*295 1'615 0 '320 7 -1600 0 -2678 6 -8922 3 -886 255 '0 + 0.4 ................... 1*098 1* 302 0 7204 7.2938 0 -1796 7 -1042 2 $28 260 -2 + 2 *4 9, ................... 1-174 1-856 0 481 6 * 9250 0 *0692 6 '8538 1.009 261'6 +3*09, - 153 when dissclved in carbon bisulphide (247.1-261.9) agreeing with those contained in the table (255.0-261.6). Beckmann’s view that the molecular magnitude of sulphur in carbon bisulphide solution is yepresented by the formula S, has also received a striking confirma- tion in t,he author’s hands, the numbers he obtained varying only between 252.3 and 254.9 (S, = 256).57. “Anhydro-derivatives of citric and aconitic acids.” By T.H. Nasterfield mid W. J. Sell. CHZ-CO Acetanhydrocitric acid, probably b(0Ac)CO” prepared from bH,*COOH ’ anhydrous citric acid and acetic chloride, crystallises from ether in groups of short prisms melting at 115”; it decomposes at higher tem- peratures yielding citraconic anhjdride if distilled under ordinary pvessure, and itacoiiic anhydride when distilled under reduced pressure (30 mm.). It yields acetylcit.ric acid on hydrolysis ; aniline converts it into citrodianilic acid ; when hydrolysed by alcoholic potash it affords aconitic acid, the method being probably t’he best yet; devised for the preparation of this acid.Ammonia converts acetanhydrocitric acid into citrazinic acid. Aconitic anhydride may be prepared by boiling aconitic acid with excess of acetyl chloride; it cryfitallises out in colourless, deli-quescent octahedra. On treatment with ammonia it affords citr- azinic acid. The authors were unable to obtain citrazinic acid from tricnrballylic anhydride and ammonia., arid point out that the formation of this acid from citric ethereal salts ie probably largely dependent on the easy formation of an ethenoid union, 58. “ Disubstituted semithiocarbazides.” By Augustus E. Dixon, D/I.D. In two former papers (Trans., 1889, 302, and 1890, 257) the autlior gave a short account of some members of the class of semit,hiocarb-azides, principally with reference to the isomerism there shown to exist amongst the disubstitution derivatives.The study has siuce been continued, but the publication of a paper dealing with such compounds was deferred until further investigation should be made regarding a phenomenon which was frequently observed, viz., the apparent existence, for a given semithiocarbazide, of two different melting points. A cc:mmunication has, however, just appeued in the Berichts (1892, 30%) in which tLis 12tter subject is specially dealt 154 with ; thc aut;ior, therefore, desires to record, without further delay, the experimental results which he has already obtained. Pa?-ntolylphen?ibe,izithiora,.bazi(le(from pToNCS and PhNH-NH,) occurs as a colourless, crystalline mass, siiitering at 149"; or in vitreous prisms, meltine at 173-174" (uncorr.).P7zenylpa.l.atolylssmithiocal.hnzide (from PhNCS and pToNH-NH,) occurs as n crystalline mass, sintering at 117", and convertible, by repeated crystallihation from boiling alcohol, into feathery needles, hecoming electrical on friction and melting at 172" (uncorr.). This and the precedinq pair are doubtless identical with componnds de- scribed (lot cit.1 by Marckwald. Ort~zotol~lpni-utol~jlsemit~iocnrbazide,when prepared at a moderate temperatnre from oToNCS and pTnNH*NH,, melts at 130-131 ", im-mediately resolidifying ; on furtber heating, it again melts at 162-163". The compound of m. p.162-163" is direct,ly obtained by combining the constituents in boiling (alcoholic) solution. Pnratot~lorthofoZyls~~~ith~o~~r~az~~e,prepared from pToNCS and oToNH*NH,, forms vitreous prisms melting at 141-142" (uncorr.). The formation of a compound having a lower melting point was not observed. Diorfl~nfolyZs~mifhiocnrbazide.-Brilliant,colourless octahedra, melt- ing at 148-149" (uncorr.). Dipnr~,tolr/lsen~it2iiocarhazid~.-Tfprepared in gently-warmed al-coholic solution, forms aggregates of flattened crystals, melting at about 125",but at once resolidif.ying and then melting at or near 153". By mixing >ding alcoholic solutions of the constitiients, the sub-stance is obtained in pointed prisms melting at 153-154" (un-coi-r.). Alphannphthylphesz?/lsemithioca,rbazine (from a-7Trt-pNCS and PhNH-NH,) .-Brilliant, vitreous needles, melting at 183" (iincorr,). Isomeric with Freund's (Ber., 24, 4190) pheriyl-a-naph thy1 deriva- tive melking at 195".Plien.~lb~fana~hthylsemithiocarbazide,prepared from Ph NCS and P-NapNH-NH,, forms pearly needles, melting at 184-184.5" (un-corr.). According to Freund (Zoc. cit.) this substance melts at 202". Betltnaphth?lZyhen?ilsemithiocarbazir7e,prepared from p-NapNCS and PhNHoNH,, crystallises in silvery needles, melting at 190-191" (uncorr.). Reizzylphenylsemithiocarbazide-White, flexible prisms ; m. p. 115-116" (uncorr.). On heating in alcoholic solution with a trace of cblorhydric acid the m. p. rises to 163". BenzyZpnratolyIsemit~Lliocarbi~zide.-Shining,flattened prisms ; m.p. 120-121" (uncorr.). 59. “Studies on the interaction of bromine and toluene. Pre-paration and properties of ortho- znd para-bromotoluene, and of the dibromotoluenes derivable therefrom. Ortho- and para-bromotoluene- sulphonic acids.” By A. K. Miller, Ph.D. It is shown that, parabromotoluene atiFords two dibromotoluenes, viz., orthoparadibromo-and metaparad i bromo- toluene, the latter being the major product ; orthobromotoluene yielding orthoparadi- bromotoluene as minor product, together with the orthometa-deriva- tive containing the bromine atoms relatively in the para-position. Parabromotoluene also yields some 1: 2 :4 : 5-tribromotoluene (Me = l), which appears to be derived from the 1: 2 :4-di-deriva-tive.60. “Note an the const’itution of Nede and Winther’s ortho- toluidinesulphonic acid, and on the acids formed by sulphonating orthochloro- and bromo-toluene.” By W. P. Wynne, D.Sc. A comparison of the chloro- and bromo-acids obtained by Sand- meyer’s method from Nevile and Winther’s orthotoluidinemeta-sulphonic acid with tbose formed from orthochloro- and orthobromo- toluene by sulphonation has established their identity. Nevile and Winther gave reasons for assigning to their acid the coustitu- tion [Me : NH, : S03H= 1: 2 : 51, but further evidence seemed desirable in view of the nature of their proof. The metabromortho- toluidinemetasulphonic acid formed from Nevile and Winther’a acid by careful byomination was converted by Sandmeyer’s method into the corresponding dibromotoluenesulphonic acid, and the sulphonic radicle was eliminated from the acid by hydrdysis with phosphoric acid in a current of superheated steam ; the resulting dibromotolnene was identified as the 1 : 2 : 3-derivative, since it melted at 30--31”, and its nitro-derivative at 59”.It hence follows that the bromotolu- idinesulphonic acid has the constitution [Me : NH, :Br : SO,H = 1 :2 :3 :51, and Nevile and Winther’s acid that assigned to it by them. 61. “The action of iodine on a mixture of sulphite and thio- sulphate.” By Arthur Colefax, M.A., Ph.D. This paper has reference to Spring’s contention, advanced in his recent note in the Proceedings (1892, 91), that although it, is true, as the author had asserted, t’hat no trithionate is formed by the action of iodine on a mixture of sodium sulphite and thiosulphate, frithionate is produced if potassium salts are used in place of sodium salts.It is shown that trithionate is not produced by the action of iodine either on the pobassium or sodium salts, and that the formation of trithionate is due to the occurrence of a secondary interaction of 156 tetrathionate and sulphite, which takes place when the iodine acts slowly, as it does, especially wheii used in the solid stabe. It is also shown that when iodine acts on a solution containing both sulphite and t,hiosulphate of potassium or sodium, present in molecular pro-portions, it oxidises the sulphite only slightly more quickly than it converts the thiosulphate into tetrathionate.62. "The methylic salts of camphoric acid." By James Walker, Ph.D., D.8c. The author has prepared the dimethyl and the two methyl hydro-gen salts of camphoric acid, and finds their properties to be in the ninin the same as those of the compounds described by Bruhl and Rraonschweig and by Haller. Orthomethylic sodic camphorate may be obtained by adding 1 mol. prop. of powdered carnphoric anhydr- ide to a cold solutiou of 1 at. prop. of sodium (1 mol. prop. sodium methoxide) in methyl alcohol ; the corresponding hydrogen salt may be prepared by acidifying the sodium salt. If 1mol. prop. of methyl iodide be added in addit'ion, and the mixture be heated for 24 hours at lOO", dimethylic camphorate is formed.The author succeeded in obtaining the allomethylic hydrogeii camphorate in a measurable form by crystallisation from metaxylene. The " dissociation " coii-staiit of the ortho-compound is 0.00108,of the allo-compound 0.000975, which are nearly equal and not far removed from half of that of cnniphoric acid, viz., 0.00225. These values correspond with the assumption that caniphoric acid is a dicarboxFlic acid, and are at variance with the formula proposed by Friedel. 157 November 17, 1892. Sir Henry Roscoe, M.P., F.R.S., Vice-president, in the Chair. On taking the Chair, Sir HENRY congratulated the Pelldws ROSCOE on the verj great improvement effected in the Society's rooms, espe-cially in the meeting room, during the recess.The Treasurer, Professor THORPE,agreed with the Chairman in thinking that the Fellows present had good reason to congratulate themselves on the changed conditions under which they met. The meeting room had undergone, as they saw, what was practically com- plete rec:onstruction, the position of the table and of the seats having been altered, with the result that not only had a very considerable air-space been gained, which would tend to the better ventilation of the room, but also additional accommodation, both in actual seating space and in the means of entrance and exit, had been secured. Pro-vision liad been made for a larger supply of fresh air and for the removal of that which passed into the rooms.Moreover, it would be noticed that the electric light had been substituted for gas as at1 illiiminant throughout the building ; this, it was hoped, would pro- mote the comfort of Fellows attending the meetings, not only in its effect on the nature of the air within the rooms, on the cleanliness o€ the apartments, and on the preservation of their decoi-ative cbaracter, but also by affording greater facilities for the exhibition of speciinens, diagrams and lantern projections. It would be under- stood that the structural and other alterations required by these changes necessarily occupied a considerable time, and, although every effort had been made to complete the changes within the recess, it had been considered desirable to postpone the date of the opening mLeting to a week or so later than the usual time, in order to secure everyhhiug being in proper working order when t'he Society met.The structural alterations had been planned and their executioii super- intended by &. Martin L. Saunders, to whom the thanks of the Society were due for the care and assiduity with which he had charged the duty he undertook. These alterations had been made by Messrs. Colls and Son, who had also carried out the redecoration of t'he whole of the apartments to the entire satisfac- tion of the Committee. The installation of the electric lighting was planned by Professor Ayrlon, to whom the Society was under a very special cbligation for the great amount of time, thought and energy he had expended on the work.The business of wiring the building and of aExing the fittings was entrusted to Messrs. Spagnoletti and Crookes, with the result that all present were able to enjoy. The fittings, that is, brackets and pendants, were supplied by Messrs. Faraday and Sons, and do credit to the reputation of that firm for 158 artistic work. Experience could alone show how these various altera- tions would work in practice, but enough had been seen already to indicate that they were undoubtedly great improvemelit s, aiid would conduce to the health and comfort of the Fellows. On the motion of the Chairman, seconded by the Treasurer, it was resolved, that Ihe best thanks of the Fellows be tendered to Mr. Martin L. Saunders and Professor Ayrton for their valuable services.Certificates were read for $lie first time in favour of Messrs Robert Samuel Adcock, Rio Tinto Mines, Huelva, Spain ; William Sniellie Anderson, Marine Station, Granton ; David Avery, Queeii’s College, Melbourne University, Australia ; Arthur John Bensnsan, 13, Lansdown Road, Kensingtou Park, W., and Darling Point, Sydney ; Horace Viucent Buttfield, 16, Thistlewaite Road, Clapton, N.E. ; Frederick Walter Carlton, Marlow House, Swindon ; Ernest Victor Clark, 5, Tisbury Road, West Brighton; Arthur James Cooper, The Schoolhouse, Bromyard, Herefordshire ; Andrew William Craig, 77, Peel Street, North Melbourne ; Joseph R. Denison, 1,Park View Terrace, Manningham, Bradford ; Thomas Duxbury, Richmond Terrace, Darweii ; Martin Onslow Forster, 32, Binfield Road, Clapham Road, S.W.; William French, 74, Walmersley Road, Bury, Lanca- shire ; Walter Goodall, Alma House, Pudsey, near Leeds ; John Goodfellow, F.R.M.S., 2, Rutland Terrace, High Road, Leyton, Essex ; Thomas Gray, 16, Craigrnore Terrace, Dowanhill, Glasg.ow ; William Thomas Gronow, Port Pirie Smelting Works, Port Pirie, South Australia ; Wdter S. Haines, Chicago, U.S.A. ; James G. Hardy, 1, Keir Teimce, Pollokshields, Glasgow ; Samuel C. Hooker, Philadelphia, U.S.A . ; John Horsfall, 88, Scar Terrace, Bacup, Lanca- shire; Edgar Edward C. Horwill, 104, Ferndale Road, Clapham, S.W.; W. H. Ince, Ph.U., 12, Cowley Street, Dean’s Yard, West- minster ; John F. V. Isaac, 18, Montserrat Road, Putney, S.W.; John Jackson, Rhyniney ; Samuel Jackson, Nether Thong, Hudders- field ; William George Johnston, 4, Hilgrove Road, Fincliley Road, Hampstead, N.W. ; K. K. Kacker, Ilelhi, India; Thomas Torrens Knowles, School House, Lwnoaster ; G. Krause, Cothen, Anhalt, Germany ; Thornton Charles Lamb, Polygon, Ardwick, Manchester ; William Howard Lloyd, 5, Belmont Villas, New Walk, Leicester ; Arnold G. Maddox, 15, Fleetwood Street, Clissold Park, N:; Colin Francis hloorwood, 260, Bnrnsley R,oad, Sheffield ; J. B. Nickolls, 8, College Terrace, Grange, Guernsey ; Hugh Ramage, Royal College of Science, Dublin; James Wyllie Rodger, 76, Anerley Park, S.E. ; Norman Scott Rudolf, Sewan Sarun, Bengal, India ; Satyaprasad Sarbadhicary, 53,Wellington Street, Calcutta ; Aagustus Schloesser, Ph.D., M.Sc., 7, Victoria Crescent, Busby, near Glasgow ; William James Sell, 1,Bene’t Place, Cambridge ; George Arthur Shaw, 112, Hramhall Lane, Stockport ; Reginald des Foyes Shepherd, 6, Colt-man Street, Hull ; Charles Spackman, Sileby, Longhborough ; Ernst Speiclel, B.S., 17, Quincy Street, Chicago, Illinois; A. H.Turton Ashley, Cai*lisle Road, Edgbaston ; Frederick William Westaway, 1,Aytoun Road, Stockwell, S.W. ; John Lowe Whiteside, 51, Canon Street, Bolton ; Frederick Henry Wigham, 85, Pinderfield Road, Wa kefield ; William Williams, Smithfield Street, Dolgelly, N. Wales ; N. T. XI.Wilsmore, Altona, Orrony Road, Elsternwick, Melbourne. The Chairman announced that the following address had been forwarded to the sister society in Berlin :-Address to the Deutsche chemische Gesellschaft.The Chemical Society of London desires to offer its warmest con- gratulations to the Deutache chernische Gesellschaft on the occasion of the celeblation of its Twenty-fifth Anniversary, while, at the same time, it joins with the sister Society in deploring most deeply the rwent irreparable loss of one who was Iong so intimately associated with both bodies, who exercised so important an influence on their development, arid who took so large a share in the guidance of the affairs, first of the one and then of the other. The Chemical Society of London is proud to think that it may properly regard the German Society as its direct lineal descendant through Hofmann.No offspring could possibly have done greater credit to its parent ; indeed, the rapidity of growth and youthful rigour of the offshoot is beyond all precedent. A true mirror of the progress of chemical science, the stately series of volumes issued by the Society during the first quarter-century of its existence, will ever serve as the priceless historical record of the marvellous ad-vance of chemistry during the period ; and that advancc would appear to be in no small degree due to the incitement afforded to experi- mental inquiry by the regular and frequent issue of the now far-famed Berichte. But probably it will in the future come to be regarded as thc greatest service of the Deutsche cheniische Gesellschaft that it has clorie SO much to render possible the ultimate denationalisation of chemical science.Chemists of all nations record their results in the pages of its publication, which has become a meeting grmnd where international jealousies disappear and the spirit of utmost toleration prevails. No one more clearly recognised the greatness of such a service than Hofmann. In 1863, when President of the Chemical Society of Lolidoil, speaking at the Twenty-second Anniversary 160 Meeting of the delivery OE lectures to the Society by distinguished foreign chemists, he said : " The Chemical Society has loudly pro- claimed the cosmopolitan character of science, and that henceforth it will look upon the several nations engaged in scientific pursuits as upon so many federal members of a great Republic united by the love of science, and pledged by contributions to a coinmm treasury, as it were, to uphold its cause and raise its dignity." The cosmopolitan influence of the great moving spirit of its councils during the first 25 years of the existence of the Deutsche chemischc Gesellschaft will ever be regarded as a priceless service rendered to chemical science by Hofmann.The following resolution was passed at the meeting of the Council in the afternoon:-''The Council learns with deep rcgret tha.t, through the death of Dr. Longstaff, on the 23rd September last, the Society has lost its senior Fellow and one of its founders. " The deep interest which Dr. Longstaff took in the Society and in the promotion of the interests of cbemical science having been evinced by the munificent gift which secured the establish- ment of the Research Fund, his name will ever remain associuted with the history of the Society arid will be retained fresh in the memory of the Fellows through the triennial award, to those who have distinguished themselves in chemical research, of the Medal bearing his name." The following papers were read :-63.''Fluosulphonic acid." By T. E. Thorpe, F.R.S., and Walter Kirman. The authors have prepared this compound by distilling a slight excess of hydrogen fluoride into a weighed platinum flask contain- ing s known amount of sulphuric anhydride, both the condensing tube and the receiver being surrounded with a mixture of ice and calcium chloride ; the excess of hydrogen fluoride was subsequently removed by passing a current of dry carbon dioxide through the liquid product at a temperature between 25" and 35".The interac- tion is attended with the development of much heat. Fluosulphonic acid, SO,HF, is a thin, colourless liquid boiling with slight decomposition (apparently into S02F2and S0,H2) at 162*6",which, it is noteworthy, is a higher temperature than that at which chlorosulphonic acid boils (155.3"). It has but lit'tle action on the dry skin, feeling greasy to the touch, and being -with- out the intense blistering action of hydrogen fluoride. 161 DISCUSSIOS. Professor RAMSATexpressed the opinion that the name fluoro- bulphonic acid was preferable to fluosulphonic acid.and also Sir HENRY asked whether the isolatioii Mi-. PAGE ROSCOE of fluorine had been confirmed by any independent observer since the announcement of Moissan’s discovery. Dr. ARNSTROXGsaid the fact that fluosulphonic acid had R higher boiling point than chlorosulphonic was of special interest, as in the case of come spondiiig “atomic ” compounds the fluorine compound, as a rule, had a lower boiling point than the chlorine compound ; he thought that on the whole the evidence favoured the view that chlor osulphonic acid was a so-called molecular compound, and, per- haps, an explanation was to be found in this direction. He suggested also that probably the flnor-and chlor-acids would be found to yield the “ pyrofluoride ” and the pyrochloride, and not the sulphuryl compounds on distillation.Professor THORPE,in replF, said that he had no special Fiews with regard to the use of the syllable fluor-instead of fluo-. He had spent considerable time in attempting to repeat I\loissan’s work, without obtaining definite resnlts ; but possibly he had not had the good fortune to hit on the precise experimental conditioiis requisite for smces. He had, however, given Moissan a long account of his trials witliout obtaining any specific information from him in reply. 64. “ Note on the interaction of iodine and potassium chlorate.” By T. E. Thorpe, F.R.S., and George H. Perry. The interaction is mually represented by the equation 3KC103 + I?= KC10, + KC1 + KIO, + IC1 + O2; the authors find, however, that it primarily and in the main involves a simple interchange of iodine and chlorine: 2KC10, + I2= 2KI0, + Cl,.When care is taken in heating the mixture, it is possible to convert practically the whole of the iodine present into potassium iodate, the equivalent amount of gaseous chlorine being liberated. 65. “ The magnetic rotation of sulphuric and nitric acids, and of their aqueous solutioiis; also of solutions of sodium sulphate aid lithium nitrate.” By W. H. Perkin, Ph.D., F.R.S. The author has previoizsly shown that, although the molecular rotations of the fatty acids and their amnionium salts are not appre- ciably influenced by the presence of water, yet that of sulphuric acid is to a considerable extent, the rotation rapidly falling for small dilutions, but diminishing as the amount of water is increased ; in these experiments the examination was only extended to a mixture corresponding to HzS04+ SOH,.Nitric acid was also found to behave in a similar manner. On account of remarks by Professor Ostwald on these results, and the interest which is taken in the subject of solutions, a more ex- tended series of observations has been undertaken. The results are given in the paper in a tabular form, and are also represented graphically. In the case of sulphuric acid and sodium sulphate, it is shown that there is no apparent connection between the value for the rotation and extent to which dissociation is supposed to take place down to solutions containing about 9 per cent.of acid or 12 per cent. of sodium sulphate. The same conclusion was come to from the examination of solusions of these substances at temperatures of about 90°, when tlie rotation increased instead of diminishing, as it should have done, according to the dissociation hypothesis. The results, however, are not inconsistent with the assumption that com- bination takes place with the forniation of (HO),SO. The results obtained with uitric acid give a different kind of curve to that afforded by sulphuric acid, viz., one consisting of a practically straight line down to solutions containing about 33 per cent, of HN03, after which it appears to curve somewhat downwards ; and, although it does not deviate SO niiich as sulphnric acid from tbnf representing the dissociation, yet it does not correspond at all closely with it.It is considered that these results may inclicate the forma- tion of a compound resulting from the union of the acid with water, e.g., (HO),NO. Lithium nitrate reseiiibler nitric acid in its behaviour. The rota- tions of the haloid hydricles in aqueous solution are also referred to, showing that as those of the concentrated solutions at first change very rapidly with small dilutions, but more slowly with large dilu- tions, at last becoming nearly stationary, they are not in agreernel;t with their clissocintion, vv-hicli increases with dilution. 66. ‘‘Note on tlie refractive indices and magnetic i~otatioiis of sulphuric acid solutions.” By S.U. Pickering. The values for the refractive indices of these solutions obtained by van der Willingerr when plotted out and esamined by a flexible lath, show the existence of a well-marked “break ’’ as well as a maximum at 84.5 per cent. (the monohydrate), another “break ” at 57.7 per cent. (the tetrahydrate), and another at 24-30 per cent. The first two of these agree with the breaks shown by the magnetic rotations, and all three of them agree with breaks found in tlie examination o€ 163 other properties. The experimental points available were not sufficiently numerous to indicate more than the most prominent “breaks,” and it was found that the densities when treated so as to lead to the indications of the most prominent “ breaks ” only, in- dicated thesc same three.For this purpose the molecular volumes were calculated from the densities of solutions of the same strength as those used by Dr. Pei=kin, and when plotted out they showed “breaks ” at 83.5, 60 and about 30 per cent. When the same number of values, but for solutions of different strengths, were taken, the same “breaks ” were still indicated. DlscnssIos. Professor RAMSAYdrew attention to a work by van der Waals, 011 t’he Co~~tinuityof the liquid and gaseous states, the fundamental equation underlying all the calculations in which is-RT a p=-(v -6) -_v2 This expression, graphically iiitc!rprstzd, gives a cu-1 e of double flexure, with very abrupt changes of curvatures, proT-ided numbers be appropriately chosen.(The curve was drawn on the black board.) He entirely dissented from Mr. Pickei-ing’s conclusions as regards “breaks,” and denied tlie existence of anything but continuous transitions from one stfate to another; and he maintained that it was no more sensible to attempt to detect “breaks” with a bent lath than to assume that all curves were parabolas or circles. Dr. ’CVALKEEdrew attention to the circumsta,nce that in calculating the aniount of electrolytic dissociation from the electrical conductivity of mixtures of sulphuric acid and watw Dr. Perkin had neglected to take account of one of the factors which cletermine the con-ductivity, namely the speed of the ions, which is intimately connected with the viscosity of the solutions.His “dissociation ” curves, therefore, did not represent at all the actual degree of dissociation in the strong solutions studied by him, for in them the viscogity is com-paratively great. The same objection applied to the temperature experiments. The great increase of condnctirity caused by elevation of temperature is due almost exclusively to the increased speed of the ions, and not to any change in the dissociation. In his opinion, therefore, tlie conclusions drawn by DL’.Perkin as to the want of con-cordance between his results and the theory of electrolytic dissocia- tion were from this cause invalid. Mi*. PICKERIKG,in repiy to ProEessor Ramsay, said that, as he had long ago pointed out,, there were, of course, many classes of curves which were not amenable to ireatment with a flexible lath ;the 164 fact that Professor Ramsay wa8 able to instaiice one of these neither proved nor disproved anything .67. " The hydrate theory of solutions. Some componnds of the dkylamines with water." By S. U. Pickering. In making a series of determinations of the freezing points of solu-tions of these ainines it was fonnd that most of them formed one or more definite crj-stalline hydrates. Sixteen rtmines were examined, of which two were entirely and two very sparingly soluble, and 24 hydrates in all mere isolated. Hydrates with the sanie iinmber of water molecules occur in many different cases, but no con- nection could be traced lset8weeii the degree of hydration and the natjure of the amine.Indications of hydrates were also obtained by "breaks " in the curves representing the freezing points, and in every instance butl one a hydrate of the composition thus indicated in the case of one amiiie was actually isolated in the crystalline con- dition in the cabe of some other aniine. The lowest hydrate isolated (in four cases) contained $H20,and the higllest 11H,O. The freezing points of the hydrates ranged from +5" to -71". 111the case of the amines themselves, as well as of such hydrates as contain the same number of water molecules, the freezing points seem to fall as the number of carbon atoms present in the alkyl radicle increase, and to rise as the niimber of radicles in the amine increases.The follow-ing is a list of analysed hjdrates isolated as crystals :-EtNH,,5.5H,O BNH,(iso-), iH,O I\le,NH, SH,O P~~NH~(~so-),8H,O PrNH,,SH20 Et2NH,8H,O Me3N,11H,O Professor THORPE,after referring to the fact t.hat the late Professor Gnthrie had investigated the relationship of certain of the alkyl-ainines to water as far back as 1884 (P7aiZ.lllag. ;Plays. SOC.Proceed-ings, 1884, 169), said that among other things Guthrie had pointed out that while a mixture of triethylamine and water containing fi.oiil 15 to 50 per cent. of the alkylamine was clear and transparent at ordinary temperature, on warming it became suddenly turbid, om-ing, apparently, to the triethylamine being thrown ont of solution.On 165 cooling the liquid it again became clear, but could again be rendered turbid on warming. The tempersture at which this change occurs is remarkable constant, viz., aboutl 18.4”. In this behariour a solu-tion of triethylamine in water resembles an aqueous solution of am-monia. It occurred to the speaker to try whether the effect of pres-sure on the solution would be to increase the apparent solubility of the alkylamine in water by observing whether the turbidity would dis- appear under pressure, the temperature being maintained above 18O.4. Experiments showed that this was the case. By enclosing a quantity of the solution in a Cizilletei tube to which pressure could he applied in the ordinary waj bx the Ducretet, pump, it was found that on rendering the liquid turbid by surrounding the tube with tepid water the turbidity almost iristantlyidisappeared when the pres- sure was increased a few atmospheres, and as quickly reappeared on releasing the pressure.Professor Thorpe proceeded to demonstrate this phcuonienon with the aid of t,he electric light by throwing an image of the tube on the screen. On gently aayming the tube the soJut.ion became so turbid as to practically stop the passage of the light. On applying pressure, the solution was seen to clarify, but on re- leasing the pressure it again became milky, and, in fact, nearly opaque. 65. “The atomic weight of boron.” By Emily Aston, B.Sc. (Lond.), and William Ramsay, Ph.D., F.R.S. An account is given of the redetermination of the atomic weight of boron by two methods-by hlie cletermiiiation of the water of crystal-lisation in borax, and by the conversion of ailhydrous sodium borate into sodium chloride by distillation of the borax with chlorhydric acid and methyl alcohol, and $5 eigliing the resulting sodium chloride.The aggregate of seven experiments in which 42 grams of borax were deprived of water gave as atomic weight 10.921, with a probable error of 0.01. Two series of experiments were made in which borax was converted into eodium chloride. The first series, in which over 20 grams were employed, gave as atomic weight 10.942 ; the second series, in which more than 23 grams were converted, gave as atomic weight 10.966.The result of the second series is regarded as more probably correct. The authors discuss the discrepnucy between their results and Abrahnll’s (0. S. Trans., 1892, 650) and give reasons why they regard the value deduced by this observer (10.825) as too low ; they think that his boron bromide may have been contaminated with hydrogen bromide present as BBr,*HBr. 166 69. "Methoxyamido-1 : 3-dimethylbenzene and some of its cieriva-tives." By W. R. Hodgkinson and Leonhard Limpach. Having devisecl a method of separating 1 : 2 : 4-metnxylidine from paraxylidine, &c., with which it is mixed in commercial xylidine, the authors have had the opportunity of preparing 1 : 2 :4-metaxylenol in large qiiantit.y. An almost theoretical yield of this phenol was obtained by diazotising a solution containing only 5 per cent.of the xylidine sulphate and then steam distilling; the product did not solidify even at -20"; but a' considerable quantity was caused to crystallise by adding solid obtained by cooling a small portion by nieaiis of carbon dioxide and ether. The presence of a trace of water was found to prevent cqstallisation. On nitration, metaxylenol yields almost the theoretical amount of 5t iiitroxylenol in which the NO2 group is contiguous to the hydroxyl. The authors have prepared tho corresponding amido- and hydroxy-xylenols and their methylated derivatives (dimethylanisoils) ; they also describe a quinaldine cleri- vative, formed by condensation from the methoxyamidoxzlene and ethylic ace toace hate.167 ADDITIONS TO THE LIBRARY. I. Donations. A collectioii of Pamphlets on Chemical and other subjects in 70 VOlP. From Sir H. E. Roscoe, F.R.S. The Threshold of Science, a variety of simple and amusing experi- ments illustrating soma of the chief physical and chemical propertics of surrounding objects, and the effects upon them of light and heat, by C. R. Alder Wright. London, 1892. From the Publishcrs. A Systematic Course of Qnnlitntire Chemical Analysis of Inorganic Substances, by C. F. Juritz. Capetown a.nd Johanriesbui*g, 1890. From the Author. Transactions of the Sanitary Institute, Vol. XII, 1891. London, 1892. From the Institut#e. Agricultural Chemistry, by A. Sibson : Revised by the Auhhor and A.E. Sibson. London 1892. From the Authors. On the History and Growing Utilisations of Tussur Silk, by T. Wardle. London 1891. From the Author. Royal College of Physicians, Edinburgh : Reports from the Labo- ratory. Vol. IV. Edinburgh and London 1892. From the Council of the College. On the Chemistry and Therapcixtics of Uric Acid Gravel and Gout, by VF. Roberts. London 1892. From the Author. Matriculation Chemistry : Chemistlay of the Non-Metallic Elements and their Compounds, by T. Orme. London 1892. From the Author. The Year Book of the Imperial Institute of the United Kingdom, the Colonies, and India. First Issue. 189.2. London 1892. From the Institute. Commercial Organic Analysis, by A. H. Allen. 2nd Edition. Vol.IIT. Part 11. London 1892. From the Author. Six Lectures on the Int-estigations at Rothamsted Experimental Station, delivered under the Provisions of the Lawes Agricultural Trust, by R. Warington. Washington 1892. From the Author. Chemical Theory for Beginners, by L. Dobbin and J. Walker. .London 1892. From the Authors. A General System of Chemical Knowledge and its Application to the Phenomena of Nature and Art, by A. F. Fourcroy. Translated by W. Nicholson. Eleven volumes. London 1804. From G.B. Buckton, Esq., F.R.S. TI. By Puwhnse. Garungstechnisches Jahrbuch, hersusgegeben von A. Schrolie. Erster Jahrgang 1891. Berlin 1892. Lecons de Chimie a l’usage des eleres de mathematiques speciales, par H. Gaut’hier et G. Charpy. Paris 1892.Ueber die Theorie der Losungen, 1-011 A. Ilorstmann. Eeidclberg 1892. (Pamphlet.) Der Indigo vom practischen uncl theoretisclten Scandpunkt, darges-tsllt, von G. v. Georgievics. Leipzig u. Wien 1892. Hanclbuch der Anorganischeii Chemie, lierausgegeben von 0. Dammer. Drei Biinde : Band I. Stut,tgart lS92. Stereochemie, nach J. H. Vm’t HOE’S Dix aiinkes ‘clans l’histoire d’une theorie ; unter Mitwirkung des vcrfassers neu bearbeitet von W. Meyerhoffer. Leipzig und Wien 189‘2. Trstite de Chemie agricole, par P. P. Delierain. Paris 1892. Extra Meeting, December 13th. An extra meeting of the Society will be held on Tuesday, Decem- ber 13th, at 8 P.M., the anniversary of thc death of Stas. A paper, specially prepared for the occasion by Professor J.W. Mallett, F.R,.S., entitled “ Jean Semais Stas, niicl the measurement of the re-lative masses of tlie atoms of t1;e cheniicnl elements,” will be read and discussed. At the next meeting, on December lst, the following papers will be read:- “Isolation of two predicted hydrat.es of nitric acid.” By 8. U. Pickering.‘‘ Notes on anhydrous oxalic acid.” By W. W. Fisher. “ The formation of orcinol arid other coiidensation products from dehydracetic acid.” By J. Norman Collie. ‘‘ Observations on the origin of colour and of fluorescence.” ByW. N. Hartley. “ The origin of colour. (V.) Azobenzene.” By Henry E. Arni-strong. “ The reduction products of ad-dimethyl-&a’-diacetylpentnne. ByF. S. Kipping. 169 ‘(The products of the action of sulphuric: acid on camphor.” By H.E. Armstrong and P.S. Kipping. “Methods of showing the spectra of easily volatile metals and their salts and of separating their spectra from those of the alkaline earths.” By W. N. Hartley. CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.n.-The names of those who sign from “ General Knowledge ” are pinted in itulics. The following Candidates will be balloted for on December 15th, 1892 :-Adcock, Samuel Robert, Rio Tinto Mines, Huelva, Spain. Analytical Chemist. I have been 4years in the Laboratory of the Rio Tinto Company, Spain. 1year 8 months Assistant, and 2 years 4 months Chief Assistant, Chemist. Science and Art Certificates. Honours 1st Practical Inorganic Chemistry, Honours 2nd Practical and Theoretical Metallurgy, &c.Member of the Mineralogical Society. Frank Johnson. E. Godm-in Clayton. William H. Martin. Matthew Cannon. W. H. Cannon. J. Parry Laws. P. Coulson Bunn. Willium Newton. Anderson,William Smellie, Marine Station, Granton. Analytical Chemist. Studied Theoretical, Analytical, and Agri-cultural Chemistry under Dr. Stevenson Macadam and Mr. Ivison Macadam ; Organic Chemistry uiider Professor Crum Brown ; Agriculture under Professor Wallace. Have been Chemist. at Granton Marine Station for last 3i years, under Dr. John Murray, of the “ Challenger ” Commission, and Mr. Irvine, F.C.S. Robert Irvine. Slevenson Macadam. W. Ivison Macadam. George Young. G. G.Henderson. Avery, David, Queen’s College, Melbourne University. Student. Bachelor of Science, Melbourne University. Kernot and Wgsilaskie Scholar in Chemistry, and Final Honour Scholar in Chemistry, Meltmurne University. Scholar of Queen’s College. Orme Masbon. J. B. Kirkland. C. R. Blackett. George Poosd. Robert Barton. Franc& H.Pmr. 171 Bensusan, Arthur John, 13, Lansdown Road, Kensington Park, W., and Darling Point, Sydney, N.S.W. Associate of the Royal School of Mines, South Keneington. '1SIIet.d-lurgist. Was placed second in the First Class Division in the Final Examination in Metallurgy at the Royal College of Science. Has studied Chemistry at the Royal College of Science, and under Pro-fessor Dixon, Sydney, N.S.W.T. E. Thorpe. W. C. Roberts-Austen. Eclwin J. Ball. Henry C. Jenkins. Bennett H. Rrough. Chaprnsn Jones. Buttfield. Horace Vincent, 16, Thistlewaite Road, Clapton, N.R. Overseer and Analyst at Messrs. Vincent Brooks, Day, and Son, Tithographers. Member of the Society of Cliernical Tndustrv ; 3 years a Student of Chemistry and Physics in the City of London College ; Holder of 10 Certificates and Prizes awarded by the Science and Art Department in Tnorqanic Chemistry, Theoretical and Prac-tical Organic Chemistry, Theoretical and Practical Experimental Physics, &c. J. Howard. TSR~CS. Scarf. James Scorgie. A. E. Carey. 7ivimB. Lewes. 9.Wood1att d To11 is. Carlton, Frederick Walter, Marlow House, Swindon, Student (Chemical and Metallurgical).StmudiedChemistry at the Edinburgh High School and obtained 1st Class Certificates. En-gaged in practical work at own private Laboratory. H. Joshua Phillips. F. M. Mercer. J. Jas. Morgan. C. A. Serre. Bertram Blount. Clark, Ernest Victor, 5, Tishury Road, West Brighton. Metallurgical Chemist. Associate of Royal College of Science (Chemistry, 1st Class). Associate of Royal School of Mines (Metal- lurgu).W. C. Roberts-Austen. T. E. Thorpe. A. E. Tutton. Chapman Jones. Edwin J. Ball. Cooper, Arthur James, The School House, Bromyard, Herefordshire. Head Master of Bromyard School. B.Sc. (Lond.), First in the First Class in Honours in Chemistry. Senior Prize for General and 172 Theoretiml Chemistry, Mason College, 13irmingham.Senior Prize for Practical Chemistry, Mason College, Birmingham. Head Master of Bromyerd Grammar School and Lecturer on Chemistry to the Here- fordshire County Council, William A. Tilden. W. W. J. Nicol. Thomas Turner. Sidney Willianason. Henry E. Armstrong. Cooper, Lionel, 173, Marylebone Road, London, N.W. Teacher of Chemistry and Physics. For four years engaged in Chemical Research, and now Partner and Teacher of Chemistry and Physics in the Central School of Chemistry, 173, Marylebone Road, N.W. A. W. Oxford. Lewis Ough. John Woodland. Richard A. Hoyle. C.R. Alder Wright. Craig, Andrew William, 77, Peel Street, North Melbourne. Master of Arts, Melbourne Universitr. Junior Demonstrator in Chemistry, Melbourne University.Lecturer in Chemistry, Melbourne University Extension Scheme. Orme Masson. J. 3. Kirkland. C. R. Blackett. George Food Rob& Barton. Francis R.Power. Denison, Joseph R., 1,Park View Terrace, Manningham, Bradford. Analyst and Dyer's Chemist. Student) three years at the Bradford Technical College, in the Chemistry and Dyeing Department. First Class Certificates in Theoretical and Practical Inorganic Chemistry. First Prize in Honours, Wool Dyeing, in 1889, City and Guilds Ex-amination. For short time Demonstrator in Dyeing and Chemist'ry Department, Bradford Technical College. Now assistant to Thorp Whitaker, F.C.S., in tbe Chemical Department at Bowling Dye Works. Engaged in the manufacture of sulphuric acid, soap, indigo products, iron liquor, tin solutions and crystals, aluminium acetate, Glauber's salts, &c., and dyewood and tannin extracts.Thorp Whitaker. Walter Leach. G. W. Slatter. C. Rawson. F. W. Richardson. Duxbury, Thomas, Richmond Terrace, Darwen. Engineer and Manager, Corporation Gas Works, Drrrwem, Lanca- shire. Have been Engineer and Manager of these Gas and Water Works for 15 years, and previous to this occupied similar position under the Accrirgton Gas and Water Works Company. Many years ago I taught a private evening chemical class. Attended evening chemical classes at the Owens College, Manchester, €or two sessions. Latterly have paid particular attention to Cooper’s coal lining process and Bunsen process of gas making, sulphate making, tar distilling, &c~.Am also Chemical Adviser to a Paper Mill Company here. Am Uernber of the Nanchester Chemical Club, &c. William Foster. Percy F. Pranklanu. B. E. R. Newlands. W.J.Dibdin. R.Grimwood. J.A. Formoy. Forster, Martin Onslow, 32, Binfield Road, Clapham Road, London, S.W. Research Assistant to Professor Dr. Tilden, Mason College, Bir-mingham. In conjunctioo with Professor Meldola, I contributed “ Researches on the Triazines ” (Chem. SOC.Truns., lr9l). I have been for three years a Student at, Finsbury Technical College, and then studied for one year at Wurzburg, of which University I am a Ph.D. I am working at present under Professor Tilclen, of Birming-ham. R. Meldola. Henry E. Armstrong.William A. Tilden. W. W. J. Nicol. Sidney Williamson. French, William, 74, Walmersley Road, Bury, Lnncashire. 1st Class Nat. Science Tripos, 189G, Cambridge. A.I.C. by ex-amination, 1889. Many years Assistant to Professor Liveing, F.R.S., at the University Chemical Laboratory, Cambridge. Note on “Estimation of Gold, Tin, and Cadmium” (Chem. News,March 18, 1892). Investigaticns on the separation of Platinum Metals with Professor Liveing (unpublished). G. D. Liveing. W. C. Roberts-Austen. H. J. H. Fenton. Alexander Scott. James Dewar. S. Ruhemann. M. 31.Pattison Muir. Goodall, Walter, Alma House, Pudsey, near Leeds. Analyst. Associate of the Institute of Chemistry. Student €or three years at Yorkshire College, Leeds.Arthur Smithells. Herbert Iqle. Charles H. Bothamley. C. Rawson. Frederic Win. Richardson. Goodfellow, John, F.R.M.S., 2, Rutland Termce, High Road, Leyton, Essex. Lecturer on Physiological Chemistry at the Bow and Bromley Insti- tute, and Analytical Chemist. 1. Late Senior Demonsbrator at; tlle 174 Chemical Laboratory, ChnrterhouBe. 2. Lmtnrer on Phj-siologicrtl Chemistry and Food Analysis at the Bow and Bromley Institute, London. 3. Author of The Dietetic Vahe qf Bread (Macrnilla,n), con- taining many original Researches on the Cliemisti-y of Bread. Also co-author of Physiological Chernistyy (Gill and Son). H. E. Roscoe. Hugh Gordon. David Howard. David Salomons. Edwd. Rider Cook. Gray, Thomas, 16, Craigmore Terrace, Doaanhill, Glasgom.Assistant to Professor of Chemistry, Glasgow and West of Scot-land Technical College. Bachelor of Science, University of London. I have conducted courses of Lectures in Organic and Inorganic Cliemistry, and am at present Assistant to Professor Henderson, M.A., D.Sc., in tlie above College. G. G. Henderson. Edmand J. Mills. Chas. A. Fawsitt. Alex. Crum Brown. John McArthur. Gronow, William Thomas, Port Pirie Smelting Works, Port Pirie, South Australia. Metallurgist. Graduate of the Ballarat School of Mines in Chemistry, Metallurgy, Assaying, Mineralogy, &.c.; Chemistry Scliolar of Ormond College at University of hlelbourne ; Demonstrator of Chemistry, Metallurgy, and dssaying, and Lecturer in Elementary Science at the School of Mines, Ballarat; Analyst and Assayer to the Pinnacle Group Silver Mining Company, the Conimodore Van- derbilt Gold and Silver Mining Company, and the Broken Rill Pre-prietary Company, Australia ; Met,allurgist to the Australian Smelt- ing and Refining Company (Limited), slid to the Broken Hil' Proprietary and Block 14 Companies at Port Pirie Smelting W orks.Gregory Board. Frank Mousley. Thomas J. G reenway. Geoyge Food. lildward H. Bennie. Haines, Walter S., Chicago, U.S.A. I'rofessor of Chemistry in Rush Medical College, Chicago, U.S.A. ; has been the Professor of Chemistry in Rush Medical College for the past 14 years ; is the Consulting Chemist, to the Health Department of the City of Chicago ; is Toxicologist to the Presbyterian Hospital, Chicago ; has contributed numerous articles on Medical Chemistry to Medical Journals, &c.John A. Miller. Edw. Gudeman. Theodore S. Wormley. C. F. Chandler. Elwyn Waller. 175 Hardy, James G., 1,Keir Terrace, Pollokshields, Glasgow. Assistant to Professor Sexton, Metallurgical Department, An-derson’s College. For 3&years a Student under the late Professor Dittmar, and now Chief Assistant to Professor Sexton in teaching, and in private analytical work. A. Humboldt Sexton. G. G. Henderson. R. R. Tatlock. T. A. Cheetham. Chas. A. Fawsitt. Hooker, Samuel C., Philadelphia, U.S.A. Chemist to the Franklin Sugar Refining Company, 701, South Front. Street. Ph.D. (Munich) ; Author of Papers on “Action of Aldebydes and Ammonia on Benzil” (with Professor Japp) ;“Retene ” (Liebig’sAnnalen, with Professor Bamberger) ; “Lapachic Acid,” and numerous other subjects.P. R.Japp. Henry E. Armstrong. W. P. Wynne. Chapman Jones. T.E. [rhorpe. W. Ramsay. Horsfall, John, 88, Scar Terrace, Bacup, Lancashire. Science Master. dtudied Chemistry at the Royal College of Science, London ; Cbemistry and Mathematical Master at the Grammar School, Newchuroh-in-Rossendale, Lancashire. Jos. Hill Heywood. W. W. Haldane Gee. William Jago. J. Hart. W.P. Wynne. Wrn. rate. Horwill, Edgar Edward C., 104?Ferndale Road, Clapham, S.W. Schoolmaster. (1) Lecturer in Theoretical and Practical Chem-istry at St. John’s Middle Class Schools, Kennington, S.E., to the London School Board, and Queen’s Park Institute, Harrow Road, W.; (2) seven years’ experience in laboratory work, &c., as Student and .Lecturer ; (3) the following South Kensington Science Certificates (all First Classes) : (a, b) Inorganic Theoretical Advanced, 1885 and 2888, (c, d) Inorganic Practical Advanced, 1885 and 1888, (e) Org-anic Theoretical Advanced, 1886, ( f) Organic Practical Advanced, 1886. Alonzo John Rider. Wm. B. Hards. E.W. De Velling. George Collar. James HaU. 176 Ince, Walter Hollinshed, Ph.D. (Wurzburg), 12, Cowley Street, Dean’s Yard, Westminster. Demonstrator of Chemistry at St. Thomas’s Hospital, lately De- monstrator of Chemistry at University College, Liverpool. Studied for 3+ years at the University of Wiireburg, and then for 1+years at the Polytechnicnm of Zurich.Author of the following contribu- tiopa :-“ On the formation of Phenyl-indoles by Isomeric Change ” (C. J. Proc. and Annalen, 253,35) ; “Action of Amines on Diketo-pentamethylene ” (Rer., 23, 1478, C. +J. Abstr.) ; with Professor Dunstan, “ Contributions to our Knowledge of the Aconite Alkalo’ids ” (C. J. Trans., 1891, 271). Wyndham R. Dunstan. J. Campbell Brown. Charles A. Kohn. W. Collingwood Williams. Thomas S. Dymond. Isaac, John F. V., 18, Montserrat Road, Pntney, S.W. Engaged in Chemical Research. Student at Owens College for a year, 1886-1887 ; four years, 1887-1891, at Oxford, Second Class Honours Chemiswy, B.A. ; engaged in research work in laboratory of Messrs.Cross and Bevan during the last six months. W. W. Fisher. John Watts. V. H. Veley. Chas. Fred. Cross. Edward Bevan. J. E. Marsh. Jackson, John, Rhymney. Analytical Chemist. Seven years as Analytical Chemist under the Rhymney Iron Company, during which time have studied the manu- facture of iron and steel, passing in Honours in Science and Arb Department. Fred. R. Stone. G. T. Evans. J. Jas. Morgan. H. Joshua Phillips. J. M. Collett. C. A. Berre. W. B. h!oberts. Jackson, Samuel, Nether Thong, Hnddersfield. Analyst and Assistant in Dyehouse. 3 years Student at Royal College of Science, London ; 14 years Student at Yorkshire College (Dyeing .Dept.) ; Associate (in Chemistry) of the Royal College of Science, London : Associate of the Institute of Chemistry (Elected October, 1890); 19 years Analyst at Meltham Mills, Huddersfield.T. E. Thorpe. J. J. Hummel. Arthur Smithells. Herbert Ingle. J. B. Cohen. 177 Johnston, William George, 4,Hilgrove Road, Pinchley Road, South Hampstead, N.W. Analytical Chemist. Demonstrator in Chemistry, Ahderson’s College, Glasgow, 1878-80 ; during this time was engaged on research and analytical work in general, and in particular assisted the late Professor W. Dittmar, LL.D., F.R.S., &c., in his “ Investigation on the Composition of Ocean Water,” “ Challenger ” Reports, Phys. and Chem., vol. 1,Pt. I ; for last five years private Assistant to Dr. Albert R. Leeds, Stevens Institute of Technology, Hoboken, N.J., United States, and co-operated with him in Investigations on Methods of Water and Food Analyses, which are embodied in the Journals and Transactions of the American Chemical Society, the Franklin In..stitute, &c. W. S. Curphey. R. R. Tatlock. R. T. Plimpton. Watson Smith. Alfred H. Allen. M. F. Roberts. Kacker, Kunwar Rishor, Delhi, India (London address, 3, Burton Crescent, W.C.). Student of Chemistry. 1. Passed Matriculation Examination of Calcutta and Allahabad Universities. 2. Student at Lahore Medical College, 1887-89 ; Studies passed : Chemistry, Physics, Materia Medica, and Pharmacy. 3. Student at Grant Medical College, Bombay, 1889-91 ; same subjects as above, with Mechanics of Solids and Fluids. 4. Private Student of Chemistry in London since July, 1891.5. As an Indian returning to India, I wish to retain a scientific connection with England, and intend diffusing chemical knowledge in India, where its widening influence is much needed. Otto Hehner. Bernard Dyer. E. G. Clayton. John M. Thomson. Alfred Hy. Alleia. Robert H. Davies. Knowles,Thomas Torrens, School House, Lancaster. Schoolmaster. M.A. (Cambridge), M.A. (Royal University, Ire- land ; Science and Mathematical Master, Lancaster Grammar School ; experience in the Laboratories of Cambridge University and Queen’s College, Belfast ; Cambridge University Extension Lecturer in Chem-istry, &c. T. H. Easterfield. A. Hutchinson. G. S. Turpin. H. J. H. Fenton. Sydney Lupton. 178 Krause, G., Cothen, Anhalt, Germany.Redacteur of the Chemilcer Zeitung. Victor Meyer. E. Erlenmeyer. Otto N. Witt. R. Meldola. Henry E.Armstrong. Lamb, Thornton Charles, Polygon, Ardwick, Mancheeter. Research Student at Owens College. Four years Assistant Chemist in Tar Distillery. Three years Student in Chemical Laboratories, Owencr College ; Science Exhibitioner for 1892 (1851 Exhibition). Has published, with Dr. Bailey, “A Redetermination of the Atomic Weight of Palladium,” J. Chem. SOC.,1892. Harold R. nixon. W. H. Perkin, Junr. Arthur Harden. Gilbert J. Fowler. G. H. Bailey. Lloyd, William Howard, 5: Belmvnt Villas, New Walk, Leicester. Wholesale Manufacturing Chemist. Educated at the Wyggeston Hospital School or Leicester Grammar School.For two years Head Assistant in the Manufacturing Laboratory of Messrs. Richardson and Go., of this town, and since then four years’ experience in Manu-facturing Pharmaceutical and Analytical Work ; holder of the Assistant’s Certificate of Apothecaries’ Society and Associate of Pharmaceutical Society, and now of the firm of J. Howard Lloyd and Co., Manufacturing Chemists, Leicester. Wm. Harkness, Samuel Francis Burford. John Hodgkin. J. Bell. H. J.Helm. C. Proctor. J. Woodward. Maddox, Arnold G., 15, Pleetwood Street, Clissold Park, London, N. A.C.Y., 1st Honours, &c. Head Master, holding nearly thirty diplomas, including Advanced Chemistry, Physics, Mathematics, &c. Science Lecturer (Chemistry, he.), Highbury Institute, N., and just appointed as same to the Bucks County Council (Slough-Windsor centre).Science Writer (Agricultural Chemistry, Hygiene, &c.) to the Teacher’s Aid. A-Section Editor of Science, Ayt, aiLd I‘echnical Bducation. Author of “ Solutions to Chemistry Questions, May, 1892.” Ten years’ work as a Science Lecturer (Hygiene, Physiology, Chemistry, Physiography, &c.). J. Howard (Islington). Robt. Steele. J. Hughes. Issaac S. Scarf. John J. Pilley. Edwa?. Ri1ey . R, H. garland. Vivian B. Lewes. -Walter N. Edwards. A. J. de Hailes. E. J. Coa. 179 Moorwood, Colin Francis, 260, Barnsley Road, Sheffield. Analytical Chemist. For fii7e years Assistant to James Taylor, Esq., B.Sc., Metallurgist ; afterwards connected with the Basic Bessemer process, and at present acting as Chemist to a firm of Steel Manufacturers.James Taylor. W. B. Bottomley. W. H. Greenwood. Fredk. J. Merrils. J. Hall Worrall. Nickolls, John Bate, 8, Grange, Guernsey. Analyst and Natural Science Lecturer. Pnblic Analyst for Guernsey. Nat. Science Lecturer at Highgate College, Guernsey. Member Society Public Analysts, Mem. SOC.Chemical Industry, Men;. Pharmaceutical Society. John Muter. G. Rult Francis. W. A. H. Naylor. A. E. Barclap. L. de Koningh. Matthew A. Adams. Ramage, Hugh, Royal College of !Science, Dublin. Assistant; Chemist. Associate of the R40gal College of Science. Associate of the Institute of Chemistry. Assistant Examiner in Chemistry, Science and A rt J-)epartment.W. N. Hartley. W. E. Adeney. Jos. Reddrop. M. H. Foye. Thus. A. Shegog. Robson, James, 1,Maxwell Street, Paisley. Chemist. Studied in Anderson College for three years. Six years and a half Assistant to the late Professor Dittmar, three of which Senior Assistant. Reappointed by Professor Henderson, D.Sc. G. G. Henderson. Edmund J. Mills. Alex. Crum Brown. Chas. A. Fawsitt. John McArthur. Rodger, James Wyllie, 76, Anerley Park, S.E. Assistant Lecturer in Chemistry, Royal College of Science, South Kensington. Associate of the Royal College of Science. First Royal Scholar in Session 1884-85 : joint author with Professor Thorpe of papers on "Potilizin's Law of Mutual Displacement of Chlorine and 180 Bromine ” (Proc., 1888, p.20) and on “ Thiophosphoryl Fluoride ” (Trans., 1883, p. 306). T. E. Thorpe. Percy I?. Frankland. F. R. Japp. W. P. Wynn e. Chapman Jones. A. E. Tutton. Rudolf,Norman Scott, Sewan, Sarun, Bengal, India. Analytical and Consulting Chemist, Bachelor of Science with Honours in Chemistry of Victoria University. Passed examination for Associateship of Institute of Chemistry. First Silver Medal from City and Guilds of London Institute for proficiency in the Chemistry of Fuel ; also passed the examination of above Institute with Honours in Alkali. Certificate for proficiency in Technology from University College, Liverpool. J. Campbell Brown. Charles A. Kohn. Herbert B. Stocks. S. G. Rawson. W. Uollingwood Williams.Sarbadhicary, Satyaprasad, 53, Wellington Street, Calcutta. Manager, Oriental Apothecaries’ Hall, 1,College Street, Calcutta Was brought up in the Calcutta Medical College. Is now the Mmu-facturing and Analytical Chemist to the Oriental Apothecaries’ Hall, an old established and respectable firm of Pharmaceutical aid Analy- tical Chemists. Kanny Loll Dey. Preo La11 Dey. Taraprasauna Koy. Ramchandra Dutta. G. C. Bose. F. h’. Macnamui-a. J. Bell. Schloesser, Augustus, Ph.D., M.Sc., 7, Victoria Crescent, Busby, near Glasgow. Lecturer on Chemistry. Dissertation, .‘Condensation von Benzoyl- essigester mit bernsteinsaurern Natrium.” With W. H. Perkin, Ph.D., F.R.S., “ Diphenylfurfuran ” (Jouwz. Chern. SOC.,57,944). W. H.Perkin, jun. A. G. Perkin. James Stenhouse. A. Hnmboldt Sexon. G. G. Henderson. F. Bl, Perkin. Sell, William James, 1,Bene’t Place, Cambridge. Demonstrator of Chemistry. First Class (Chemistry) Natural Sciences Tripos, 1876. For many years Senior Deliionstrator at the 181 UniversitT Laboratory, Cambridge. Papers : (1) “On the Volu- metric ICstimnt4ion of Chromium ” (Chem. SOC.Trans., 1879, 292) ; (2) “ On a Series of Salts of a Base containing Chromium and Urea.” Part I (Proc. Roy. Soc., No. 218, 1682) ; (3) “ On a Series of Salts of a Base containing Chromium and Urea.” Part I1 (Proc. Eoy. ~S’OC.,45, 321) ; (4) ’‘Volumetric Determination of Chromium ” (Chena. News, 54, 299). G. D. Liveing. H. J. H. Fenton. James Dewar. Alexander Scott.T. H. Easterfield. Shaw, George Arthur, 112, Bramhall Lane, Stockport. Manufacturing Chemist (Kay Brothers, Limited). Pharmaceutical Chemist. Have passed Major and Minor Examinations of the Phar- rnaceut.ica1 Society. Two years Student in Chemistry at the Stockport Technical School (1889-91). One year Student of Chemistry and Practical Chemis try in the School of the Pharmaceutical Society, where I was awarded the Silver Medal in Practical Chemistry, and two Certificates of Honour in Chemistry. M. Crtrteighe. Wyndham R. Dunstan. Thomas S. Dymond. John Attfield. R. J. Brown. Shepherd, Reginald des Forges, 6, Coltman Street: Hull. Three years in the Chemical Laboratories o€ the Owens College ; B.Sc., with Honours in Chemistry, Victoria University.Harold B. Dixon; Arthrir Harden. P. J. Hartog. G. J. Fowler. G. H. Bailey. James Grant. Spackman, Charles, Sile by, Loughboroa gh. Chemical Engineer. From 1873 to 1878, working under the late Gen. Scott, F.R.S., at experiments on sewage treatment, and on limes and cements. From 1879 to 1882, Chemist to the Folkestone Cement Company. During 1883,Engineer for the erection of Barrow Cement Works, near Loughboroagh. Since then, and at the present time, Resident Engineer and Chemist at these works. Full students’ lecture course and laboratory work at University College, Notting- ham. Communicated two chemical papers to the Jozw. SOC.Chem. Ind. R. Lloyd Whiteley. Frank CIowes. L. Archbutt. J. B. Coleman.Frank T. Addyman. M. J. R.Dunstara. 182 Speidel, Emst, B.S., Nos. 17, 19, 21, Quincy Street, Chicago, Illinois. Analytical and Consulting Chemist. One year as Assistant in Chemical Manufactory. Six years as Chemist in Testing Labora- tories of the C., B., and Q.R.R. and C. and N.W. Railroad. One year Chemist in chargs Opaque Cloth Works. Expert in colours and oils. John A. Miller. Edw. Gudeman. H. A. Wetzel. Oh. I?. Chandler. Elwyn Waller. Turton, Albert Hy., Ashleigh, Carlyle Road, Edgbaston, Birmingham, and Launces- ton, Tasmania. Pharmaceutical Chemist, Assayer, and Metallurgical Chemist. Certificated Chemist of Tasmania, and Member of its Pliarmaceutical Society also. Member of South Australian Pharmaceutical Societ,y.Student in the Metallurgical Laboratory, Mason College. Thomas Turner. Alfred Hill. Chas. Hunt. W. P.Haydon. Geo. S. Albright. Warry, John King, 15, Grafton Street, Mile End. Doctor of Medicine. Deputy Medical Officer of Health and Public Analyst for Hackney. Frederic Jas. M. Page. J. Hugh Bicket. E. Francis Smith. Theodore Maxwell. George Robertson. Westaway, Frederic William, 1, Aytoun Road, Stockwell, S.W. Lecturer at Stockwell Pupil Teachers’ School, S.W. B.A. (London). Holder of 12 Advanced Science Certificates from the Science and Art Department, including Theoretical and Practical Chemistry. Student aud Teacher of Chemistry and Natural Science since 1884. Just appointed Director of Technical Instruction under the Dalton-in- Furness School Board.George Collar. Wm. B. Hards. James Hall. J,H. Gladstone. H. R. Hind. Whiteside, Jno. Lowe, 51, Cannon Street, Bolton. Chemical Lecturer. Teacher of Chemistry (Organic and Inorganic) from 1879at the Bolton Church Institute4o prevent time (31 benches). 183 Teacher of Metallurgy, and Head of the Bleaching, Dyeing, and Printing Department at Bolton Technical School. George H. Hurst. W. B. Mason. H. E. Roscoe. Ernest Bentz. R. W. WaIker. Wigham, Frederick Henry, 25, Pinderficld Road, Wakefield. Analyst and Metallui*gical Chemist. Four years Assistant with Messrs. Pattinson and Stead, of Middlesbrough. Three years Aoa-lyst with Messrs. G. Cradock and Co., Wakefield. J. E. Stead. H. Frankland.E. H. Saniter. C. H. Ridsdale. John Pattinson. Williams, William, Smithfield Street, Dolgelly, N. Wales. Medical Practitioner and Lecturer in Hygiene to the University College of Wales, Aberystwitb. Late Assistant M.O. of Health to Shropshire. M.A. (Oxon.), with First Class Honours in Natural Science (Chemistry) ; late Demonstrator of Chemistry in the Chemical Laboratory, Oxford; M.B., B.Ch., and D.P.H. (Oxon.); M.R.C.S. (Eng.) ; L.S.A. (Lond.). William Odling. W. W. Fisher. John Watts. V. H. Veley. D.H. Nagel. Wilsmore, N. T. M., Altona, Orrong Road, Elsternwick, Melbourne. Student. Bachelor of Science in Chemistry, University of Me]-bourne ; " Researches on the Organo-Metallic Compounds," con- tributed to the Third Meeting of the Australasian Science Association and to the Chemical Society.Orme Masson. J. B. Kirkland. C. R. Blnckett. George Foord. BoLert Burton. Francis 3.Power. The following Candidates are recommended by the CounciI for ballot under Bye-law I (para. 3) :-Campbell, Andrew, c/o Burmah Oil Co., Rangoon. Analytical Chemist. Four years Assistant to J. Fa.lconer Kcnp, Esq., F.I.C., City Analjst,, Edinburgh. Chemist to Linlithgow Oil CO., Limited. Nnnaging Chemist to the Burmah Oil Go., Limited, Rangoon. J. Falconer King. John Hnnter. James C. Hamilton. Williams, Jno., Georgetown, Demerara. Private Assistant to Government Analytical Chemist, British Guiana. Five years’ study in Chemistry under the late Professor Francis, F.C.S., F.I.C., Government Analyst, and two years under Professor J.B. Harrison, F.C.S., F.I.C., Government Chemist. Acted as Assistant Government Chemist during the absence on leave of the Government Chemist from September 1891, to April, 1892. J. B. Harrison. William Douglas, H. Arnzody. Francis Watts. John R.Bovell. HARRISON AND SONS, PRINTERS IR ORDINARY TO HER MAJESTY, ST. MARTIN’S LANE.
ISSN:0369-8718
DOI:10.1039/PL8920800141
出版商:RSC
年代:1892
数据来源: RSC
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