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Proceedings of the Chemical Society, Vol. 18, No. 256 |
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Proceedings of the Chemical Society, London,
Volume 18,
Issue 256,
1902,
Page 207-234
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摘要:
Zsssued 26111/O2 P 13 0 C l.C l.C D 1 N (3 S OF THR CHEMICAL SOCIETY. EDITED BY THE SECRETARIES. Vol. 18. No. 256. Wednesday, November 19th, 1902. Professor EMERSONREYNOLDS, SC.~).,V.P.R.S., President, in the Chair. Certificates mere read for the first time in favour of Messrs. : Gilbert John Alderton, Eglinton Road, Plumstead, S.E. Harry Percy Lewis, Swansea Hematite Works, Landore. Thomas Samuel, School of Science and Art, Liscard, Cheshire. John Mello Wadmore, B.A., Meriden, Exmouth. Albert Wilmore, 158, Skipton Road, Colne. William Wade Yeomans, Middlewich, Cheshire. The PRESIDENTannounced that the Council that afternoon had appointed Dr. G. T. Morgan to be Editor of the publications of the Society from January 1st next. Of the following papers: those marked * were read : *160.(‘The dynamic isomerism ’ of thiourea and ammonium thio- cyanate.” By J. E. Reynolds, D.Sc.,F.R.S.,and E. A. Werner, F.I.C. The method of producing thiourea for use in the arts is still essentially that by which one of the authors succeeded in isolating the substance in 1868 (Twms., 7, 1). This consists in carefully 208 heating fused ammonium thiocyanate so as to seciire as far as possible the molecular rearrangement represented by NH,CNS =CSN,H,. The proportion of thiourea actually formed at any single operation of this kind is known to be small, Volhard and others have variously estimated the yield at 15 to 22 per cent. of %he thiocyanats taken for conversion. It is also well known that pure thiourea, when melted, slowly reverts to ammonium thiocyanate ; but the estimates of the extent of this reversion also vary considerably.Viewed as a L6 balanced action ” conditioned by heat alone, these changes are cited by Lowry as examples of “dynamic isomerism.” In view of these discrepancies which they considered were probably due to the use of small quantities of impure or moist materials, the authors have systeinatically studied on a comparatively large scale the effects of temperature and time on the course of these changes, and give *the results of their experiments in curves. They show that : 1. Ammonium thiocyanate fused and then raised to, and maintained at, a steady temperature of 170°, underwent gradual change into thiourea until a maximum of 24.7 per cent.was reached after 45 minutes. Continued heating for 25 minutes longer led to slight loss of thiourea by decomposition. 2. In another series of experiments, the .mean temperature being 182O, similar results were obtained, but the change was more rapid in the earlier stages, although the time required for the maximum effect was substantially the same as before. 3. Pure thiourea fused, and then maintained at a steady temperature of 170°, gradually reverted to ammonium thiocyanate, and after 40 minutes only 25.8 per cent. of thiourea remained. That proportion was not materially diminished by continued heating. Therefore equilibrium is reached from either side when the isomerides are present in the melt in proportions which are substantially 25 per cent.of thiourea and 75 per cent. of ammonium thiocyanate, which is the composition of a definite compound having the formula CSN,H,,(NH,CNS),. The authors conclude that the arrest of change is due to the pro- duction of this compound which appears to be more stable at high temperatures than either of its constituents. In confirmation of this view, they find that crystalline aggregates of nearly the above composition can be separated from the centre of a slowly cooled mass, produced by heating about a kilogram of ammonium thiocyanate to 170” for 40 minutes. Further, having noted that the material which contained about 25 per cent. of thiourea remained liquid down to 106O, they determined the points of complete liquefaction of a number of very intimate mixtures of pure thiourea and thiocyanate.They found that there was a regular decrease in melting point from 148' (that of pure thiocyanate) to 1060, at which latter temperature a mixture containing 25 per cent. of thiourea fused, but with still higher percentages of thiourea there was a regular rise in melting point, as shown on a curve of eutectic form having its minor point at 106'. Finally, it was pointed out that the dissociation of the high tempera- ture cornpound by solvents is by no means complete unless the latter are used in comparatively large proportions. Thus, when the melt was treated with insufficient warm acetone to dissolve it wholly, the solution afforded a compound which afteryards separated in feathery groups of crystals.This substance. proved on analysis to be CSN2H4,NH4CNS. With alcohol and water, the process of breaking down proceeds farther, but even warm water, if used in small pro- portion, does not cause complete separation, as fine, long crystals mere easily obtained from such a solution which consisted of (CSN2H,),,NH4CNS. This compound is obviously complementary in composition to that which is formed in the Fused mass at 170". Re-solution of the crystals in water leads to complete separation. Generally, the authors conclude that the state of equilibrium reached when either isomeride is heated to 170" for 40 minutes is conditioned as much by perfectly definite' chemical attraction as by heat."161. Isomeric partially racemic salts containing quinquevalent nitrogen. Part VIII. Resolution of the hydrindamine bromo-camphorsulphonates." By F. S. Kipping. In previous communications (Trans., 1900,77, 861 ;1901, 79, 430), the author has described several cases of a new type of isomerism observed in the study of salts of dZ-hydrindamine (and of dl-benzyl-hydrindamine) with bromo- and chloro-camphorsul phonic acids and with cis-r-camphanic acid; in order to account for the existence of these isomerides, it was assumed that each of the optically active bases gives rise to two salts, and that the four compounds thus formed unite in pairs to produce the two partially rncemic isomerides. Further investigation, which so far has been restricted to the iso- meric hydrindamine bromocamphorsulphonates (distinguished as the 'a '-and p'-salts), seems to show that this view of their nat,ure is substantially correct. IZesol?i,tion of the a-XaZt.-When the a-salt (m.p. 150°),which separ- ates unchanged from most ordinary solvents, is heated with a little ethyl acetate under suitable conditions, it is resolved into two com- 210 ponents, one of which is deposited from the hot solution, whilst the other can be isolated from the mother liquors. The former, provision- ally called the aA-salt, crgstallises in needles melting at about 223'; the latter, the aB-salt, crystalli-es in needles melting at about 130'. These two salts have practically the same specific rotation in dilute aqueous solution, namely, [a],, = +60" ;the molecular rotation, there- fore, in both cases is +266O, a value identical with that of bromo-camphorsulphonic acid.The two compounds represent, nevertheless, salts of the enantiomorphously related hydrindamines, the bases having such low molecular rotations that they show no appreciable activity, even in moderately concentrated solutions of their hydro- chlorides. The hydrochlorides, prepared from the aA-and aB-salts, are identical in ordinary properties, but the salts obtained by com- bining the bases from aA and aB with opticnlly active acids are diff erent ; it follows, therefore, that the enantiomorphously related bases do not undergo rxcemisntion when liberated from their salts.Besolution of the p-Scdt.-The partially racemic p-salt (m. p. 130') is also resolved into different components when it is crystallised from hot ethyl acetate under suitable conditions. The salt, which separates from the hot solution, crystallises in needles which appear homogeneous and which resemble aA very closely in outward and in optical properties ;when, however, this compound is system-atically crystallised from water, after some 30-40 operations, it is further resolved into a salt identical with UAand a new isomeride PA ; the latter is very similar to aA, but melts at a lower temperature (about 215"), and has a lower specific rotation ([a],,= +56') in aqueous solution; it is possible that this salt may not have been obtained quite free from aA.The ethyl acetate mother liquors, from which aA and PA have been deposited, contain unchanged p-salt together with two isomerides; one of these is identical with aB, but the other, PB, although very similar to aB in some properties, can be separated from it by fractional crystallisation from water. This fourth isomeride, PB, melts at about 130' and has a specific rotation [a],,= +39.5"in aqueous solution. Synthesis of the a-and p-S'cc~ts.-when equal quantities of aA and aB are dissolved together in hot water, the solution deposits the partially racemic a-salt, and fractional crystallisation fails to reveal the presence of any p-salt in the product. When aA and UB are separately decomposed with baryta and the liberated bases are neutralised with the bromo-acid, the salts obtained appear to be identical with aA and aB respectively, but they are not so; for if now mixed in equal quantities and crystallised from water they give a product which consists of a mixture of the a-and p-partially racemic salts.This is because, on uniting with the acid, the 211 one base gives ail. and PA, the other aB and /3B ; the salt produced by combining the base from aB with the acid may, in fact,, be resolved into aB and PB by fractional crystallisation. When equal quantities of PA and PB are dissolved together in water, there results a salt which crystallises in hydrated prisms, in- distinguishable in appearance from those of the partially racemic ,%salt (m.p. 130°), but which, when dehydrated, melts at about 165’; this fact, and- the constant occurrence of four compounds in the pro-ducts of the resolution of s:amples of the @-salt which have been Yepeatedly crystallised to free them from a-salt, show that the p-salt is composed of four isomerides. The salt composed oE equal quantities of PA and PB seems to represent a new isomeride, in which case there woulcl be three pnrtially racemic salts. “162. ‘61someric compounds of the type NR,R,H,.” By F. S. Ripping. From the results summarisecl in the preceding note, it will be seen that six isomeric salts have now been isolated from the mixture pro- duced by the combination of d-hydrindarnine and d-bromocamphor- sulphonic acid. Four of these salts, aA, aB, PA, and BB contain one molecule of one of the enantiomorphously related bases combined with one molecule of the acid, that is to say, each of the bases gives rise to two isomerides which may be represented by the symbols : /\ /\HH HH Such compounds, containing only three different radicles united with quinquevalent nitrogen, afford an example of a type of isomerism hitherto unknown ; it is possible, however, that the isomerism of the optically inactive compounds of the type NRIR2R3R4R5,de-scribed by Wedekind, may be of an analogous character.The existence of these new isomorides has no doubt an important bearing on the question of the arrangement in space of the groups around a quinquevalent atom, and would seem to exclude the double tetrahedron configuration ;also the view, very generally held, that the negative ion in an ammonium salt takes up one particular valency.The fact that, in the case examined, the two radicles It, and R, are enantiomorphous does not of course preclude the possibility of the existence of isomerides in which the three different radicles are all optically inactive, and it may even be possible that an apparently 212 simple salt, such as ammonium chloride, is in reality a mixture of two isomerides. One particularly striking fact in connection with the isomeric hydrindamine salts is their stability ;all the four simple isomerides have been repeatedly crystallised from boiling water and other solvents, and hitherto the conversion of one into the other has never been observed.It is also interesting to note the highly abnormal molecular rotation of the PB-isomeride ;in 2 per cent. aqueous solution, [MI, = +175", whereas that of the acid is [MIu = +270". Since the ordinary base ion, although enantiomorphous, has only an extremely low molecular rota- tion, it might be inferred that the PB-isomeride is only very partially dissociated, and that there are two distinct types of ammonium salts. *163 "The oxime of mesoxamide and some allied compounds. Part 11, Disubstituted derivatives." By Miss M. A. Whiteley, D.Sc. The following mono-and di-substituted derivatives of the oxime of mesoxamide have been prepared : isonitrosomacloizdirnethylccnzide, m. p. 157O, the potussizm and ferrous salts ;isonitrosoiiicclonanilide, m.p. 141", the potassizcm, ferrous, and silver salts ;isonilosonzalondi-p-tolyl-amide, m. p. 170-171": the potccssium and silver salts ;isonitrosomalon-m.mono-p-tolylamide, m. p. 183" ;iso?zitrosonia~o?zdi-o-toZl/lami~~, p. 11lo, the potccssium salt ; ethyl iso?zitrosonaaZon-o-toZylanLa;cte, m. p. 140-141' ;isonitrosotizaZondi-a-nap~t?~~Za~i~~de,m. p. 184O, the potass-iunz salt ,isonitroso~~~cclondi-~-nap~~thy~unz~de,m. p. 22lo,the cccetyl derivative, m. p. 179", a chlorinated derivative, m. p. 202". All these compounds possess the characteristic salt-forming properties exhibited by the original oxime, the alkali salts being yellow and the ferrous. salts purple or blue. An interesting tautornerism is exhibited by some of them, the two isomerides differing from one another in colour (one being yellow and the other colourless), crystalline form, and solubility.The most probable explanation of this tautomerism is the assumption that the colourless isomeride has the isooximino-structure, whilst the yellow isomeride and the yellow salts correspond to the oxi mi no-comp oun d , The examination of a fairly extensive series of a-oximino-ketones has shown that in addition to the well kuown characteristic yellow coloration with alkalis, almost all give a deep purple or blue colour on the further addition of ferrous sulphate. This latter characteristic, how- ever, appears to be influenced by the isomerism of the oxiinino-group, for a-benzil monoxime gives the reaction, whilst the P-isomeride does not.Again, among the dioximes, a considerable number, including a-benzil 213 dioxime, were found to give a deep purple or brown coloration with ferrous sulphate and an alkali, whilst p-and y-benzil dioxime gave no coloration under these conditions, *164. ''Interaction of ketones and aldehydes with acid chlorides -the formation of benzoxyolefines and 1-benzosycamphene." ByF. H. Lees. The author hiis found that methyl wnonylketone and benzoyl chloride readily interact when boiled together, forming P-beiazoxy- undecyletae (a or p), CH,:C(OBz)-C9H1, or CH3-C(OBz):CH*C,H17. It is an oil, b. p. 233-235' (50 mm.), and is iegarded RS being formed according to the scheae : This formation oP P-benzoxyundecylene represents the first instance of the direct trmsformcttion of a mono-oxygenated ketone into a derivative of its enolic form.The author has extended this reaction to other ketones, an aldehyde, and an aliphatic acid chloride, the following substsauces resulting : P-ber~zoxyiao~zyleiae(a or PI, CH,:C(OBZ).C~K,~or CH,*C~OBz):CH*C',Hl3,from methyl n-h*ptyl- ketone and benzoyl chloride, b. p. 210-211° (50 mm); P-bei?,-irxo,Eg-y-methylheptgbne (a or p), CH,:C(OBz).CH(CH,)*C,H, or CH3*C(OBz):C(CH,)*C,Hg,from methyl sec.-hexylketone and benzoyl chloride, b. p. 197-200' (50 mm.); P-benxoxyhezylene (a or p), CH,:C(ORz).C4H9 or CH3*C(OBz):CH*C,H7, from methyl vb-butyl- ketone and benxoyl chloride, b. p. 170-175' (50 mm.) ; a-benzoxy-a-phenylethylene, C6H5*C(~Bz):CH2, from acetophenone and benzoyl CHchloride, b.p. 227-230' (50 mm.) ;l-benxoxycmnp4ene, C,H,,<I IC-OBz' from camphor and benzoyl chloride, b. p. 215-220' (50 mm.) ; a-benxoxy-a-~~e~tglne,C,H,,* CkKCH(0 Bz), f roru cmanthaldehyde and benzoyl chloride, b. p. 195' (50 inm.) ; p-valeyoxyundecylene (a or p), CH,: C(O* CO*C,H,).C, H, or CH,*C(O*CO*C,H9):CH*C,Hl7, from methyl w-nonylketone and valeryl chloride, b p. 185-190' (50 mm.). Acetone with benzoyl chloride, and methyl nonylketone with acetyl chloride, did not interact ; me thy1 n-propylketone and benzoyl chloride interacted only slightly. All the substances prepared are nearly colourless and odourless oils, and in their chemical properties ex- actly resemble each other.They all readily absorb bromine, form- 214 ing dibromo-addition products, and are unstable to potassium per-manganate. The possibility of benzoxycamphene having a structure analogous to hydroxycampheiie (Forster, T'rcw,~.,1902, 81, 264) was considered, but the fact that benzoxycamphene is readily hydrolysed by alcoholic hydroxylatnine, yielding I-rotatory camphoroxime, and that its dibromo-addition product readily splits up into a-bromo-camphor and benzoyl bromide; definitely proves the correctness of the CHstructure c,H,~<IcI OBZ' 65. 6c The synthesis of aa-dimethylglutaric acid, of P-hydroxy-aa-dirnethglglutaric acid, and of the cis-and tmm-modifications of aa-dimethylglwtaconic acid." By W.H.Perkin, jun., and Miss A. E. Smith. When a mixture of ethyl dimethylmalonate anti ethyl acetate is tre.ited with sodium, condensation readily takes place tvith the formation of ethyl aa-dimethylacetonediciirboxylate, CO,Et*CMe,*CO*CH,*CO,Et, which distils at 185-190" (100 inm.) and gives, in alcoholic solution with ferric chloride, a red-violet coloration. When this ester is redaced with sodium amalgam and then with hydriodic acid, it yields the following acids : /3-flpl~oxy-aa-climethylgZu taric acicl, CO,H CAI<>.,G'H(0H) CH,CO,H, which crystallisss from water in prisms and melts at 158-160". aa-Dimethylglutaric acid, CO, H*CMe2*CH,*C1H,*C02H,which melts at 90' and is identical with the acid of this constitution obtdined from isolauronolic acid by oxidation with nitric acid.cis-aal-Dinzet?~yZgZutaconic acid, CO,H*GMe,*CH:CH C0,H. This acid is readily soluble in water and melts at 134O; it combines with bromine yielding cis-al/3-dibro~~?zo-aa-din~et~~~ZgZutcLricacid (m. p. 1SO'). When hydroxydimethylglutaric acid is distilled, it is, in part, con-verted into the sparingly soluble trans-aa,-dimethylglutaconic acid which melts at 172" and was first obtained (Perkin, Frans., 1902, 81, 253) by the hydrolysis of ethyl al-bromo-ua-dimethylglutar,zte, CO,Et.CMe,.CH,*CHBr*CO,Et, with alcoholic potash. This same acid is obtained almost quantitatively from the above hydroxy-acid by treatment with phosphorus pentachloride, then with alcohol, and finally with alcoholic potash, C'O,Et.CMe,~CHCI*CH,*CO,Et, giving CO,H*CiMe,~~H:CH~CO,H. The trans-acid is acted on only with difficulty by bromine with formation of tra~zs-alP-dibromo-aa-dimethyl-glutaric acid (rr~p.217"). It appears, therefore, that the cis-and trans-modifications of aa-dimethylglutaconic acid melt respectively at 134' and 17%". The bearing of this on the work of Conrad and of Henrich on this subject was discussed. 215 166. '(Areaction of some phenolic colouring matters. 11." ByA.G. Perkin and C,R. Wilson. By means of alcoholic potassium acetate, gallacetophenone gives the salts (a) C,H,O,K,H,O, and (b) C24H23012K.The former, pale yellow needles, identical with the compound which Nencki and Sieber (Journ. pact.Chent., ["I7 23, 23, 546) prepared with alcoholic potash, is anhydrous at 160°, and gives the salt Cl,Hl,OsBa, yellow needles. Sodium acetate gives the salt CsH70,Na,H,0. With methyl iodide this gives gallnceto~l~e~zonenethylether, CsHp03(OCH,), needles, m. p. 132--133O, the diucetyl derivative of which melts at 146-14s'; and on methylation gallacetophenonedimethyl ether, m. p. 77-78", (T?*ans 1S95, 67, 997) is formed. It is thus ft para- or meta-methoxy- compound. The sdt (b), colourless needles, is also formed from gallace- tophenone and potassium acetate in aqueous solution and from this the compound C,sH,,O,,Ba can be obtained. The following salts have been prepared with alcoholic potassium acetate. Ellagic acid gives C,,H,O,K .and C14H40SK2,daphnetiu, C9H,0,,KC2H,0,, galangin, C,,H ,O, K ,H,O, kampheride, Ci,Hi,OGK,H20, dihydroxybenzalcumaranone (OH :OH = 6 : 7), C,,H,,O,,KC,H,O,, carminic acid, C,iHi,OGK and C22H22012Ba, styro- gdlol, C,, H70,K, .napht hazarine, (CloH60,)2,KC,H,0,?, and curcumin, (321131906K.By means of alcoholic potash, daphnetin gives the salts C,,H,,O,K and 'C,H,O,K, and carminic acid the salt C22H23012K. From acetyl rhamnetin, the compound Cl,Hl,07K was obtained.Di.l1.zatl~ozyccizhy/clrogZycogalZoZ,C,,H,,O,, yellow needles, m. p. 122', gives with pi otocatechuic alclehy de clinzet~oxydihyclroxybenzcc1cunzus.-uno?~e,C17H1406, orange-coloured needles, which with potassium acetate gives the salt Cl7H1,O,IL Yyrogallolnzoszo,netliyZ etlbep-, incidentally prepared, melts at 102-104", and not at 95' as given by Benedikt (Ber., 1877, 9, 125).167. ''Note on mixtures of constant boiling point." By S. Young,D.Sc.,F.R.S. It mas noticed by Thorpe (Trans., 1879, 35, 544) that when a mixture of equal volumes of carbon tetrachloride and methyl alcohol is distilled a mixture of minimum boiling point, 55.6-55-9", comes over first. The vaporxr density of this distillate was found to be 41.82, and the composition was therefore Carbon tetrachloride .................. 78.1 Methyl alcohol ........................ 21.9 100.0 216 At Dr. Thorpe’s suggestion, the author has determined the composi- tion of the mixture of minimum boiling point by the distillation method, and also from the specific gravity of the mixture after re-distilla tion.The results are as follows : Distillation Met?bod. From excess From excess From specificof CH,OH. of CC4. gravity. CCI, ............... 79-99 79.35 79-44 CH,OH ......... 20.01 20-65 20.56 100~00 100~00 100~00 The separation of the mixture of minimum boiling point from methyl alcohol is very much more difficult than from carbon tetra- chloride, and it is in all probability for this reason that the percentage of alcohol in Thorpe’s distillate was too high, whilst that calculated from the results of the distillation of a mixture containing excess of alcohol was too lorn. The most accurate value is probably that deduced from the speci6c gravity of the redistilled mixture of constant boiling point.Determinations by Thayer (J0ur.n. Phys. Chem., 1898, 2, 382), Ryland (Amer. Chem. Jourm., 1899, 22, 384), and Carveth (Journ. Yhys. Chem., 1902, 6, 248) of the boiling points and composition of mixtures of benzene with ethyl and methyl alcohol were compared with those of Miss Fortey and the author (Trams., 1902, 81,739). 168. ‘‘ The Vapodr pressures and boiling points of mixed liquids. Part 11.” By S. Young, D.Sc., F.R.S.,and Miss E. C.Fortey, B.Sc, In a previous paper (TYL~s.,1902, 81,753) it was shown that, so far as mixtures of chlorobenzene and bromobenzene are concerned, the conclusion of van der Waals is true that if the criticd pressures of the two liquids are equal and if the relation suggested by Galitzine and by Berthelot, CC~,~.= Jzholds good, the relation between vxpour pressure and molecular composition should be represented by a straight line, or the vapour pressures of mixtures may be expressed by the formula P=-ppAf(lOO-pP)PB,where P,PA,and P,, are the vapour 100 pressures of the mixture and of the two components A arid B at the same temperature, and p is the molecular percentage of A.It does not, however, follow tlint it’ is only when the critical 217 pressures are equal thLtt the vapour pressures agree with the formula; indeed Speyers goes so far as to state that it is always applicable to mixtures of liquids of norrual molecular weight. As the statement of Speyers is certainly too general, it seemed desirable to determine the boiling points of mixtures of a number of closely related compounds the critical pressures of which are not equal.Four pairs of such liquids were examined, (I) ethyl acetate and ethyl propionate, (2) toluene aud ethyl betizene, (3) n-hexane and n-octane, (4) beuzetie and toluene, and, in addition, carbon tetra-chloride and benzene. The investigation resulted in the following conclusions :-1. The volume and temperature changes on mixing closely related substances are in all the observed cases very small, but it is only with chlorobenzene and brouiobenzene that they can certainly be said to be within the limits of experimental error. With the two eaters, these limits are very closely 'i pproached, whilst with benzene and toluene, which are somewhat less closely related, the changes are distinctly larger, and for mixtures of benzene with mhexane and with carbon tetrachloride they are very much larger.is nearly, if not quite, true 2. The formula P=pr~+(loo-~)p~100 for closely related liquids, even when the critical pressures are widely different;it is not true, however, asa rule, for mixtures of liquids of norrual molecular weight such as benzeue and n-hexane, or for benzene and carbon tetrachloride, which are not closely related. Of the five pairs of clojely related liquids exsmined, it is only chlorobenzene and brviuobeuzene which &ow absolutely no tempera- ture fir volLme change on mixing, and for mixtures of which the vapour pressures are accurately given by the above formula, and it is only this pair of liquids which h;.Lve the same critical presaure.The deviations in the other cases are, however, so small that it remains an open question whether equality of critical pressure is a necessary criterion for absolute agreement with the formula. It appears, at any rate, that equality of critical pressure without closeness of chemical relationship is not a suflicient criterion. It may be stated definitely that in the case of closely related sub- stances, whatever their critical pressures, the deviations ara, as a rule at any rate, exceedingly small. Lastly, it is shown that there ib strong evidence for the existence of mixtures of minimum boiling point in the case of carbon tetrachloride and berizene, and also of 72-hexane and beiizene, although the boiling points of the mixtures could hardly be distinguished from those of 218 carbon tetrachloride and rt-hexane respectively by ordinary thermo- metric methods.169. "The vapour pressures and boiling points of mixed liquids. Part 111." By S. Young, D.Sc., F.R.S. If the vapour pressures of mixtures of two liquids, A and B, are accurately expressed by the formula P =PpA +(loo-p)pB(where P,100 PA,and PBare the vapour pressures of the mixture and of the two components respectively at the same temperature, and p is the mole- cular percentage of A), and if the difference between PAand P, is small, the relation between the boiling points of the mixtures at con- stant, pressure and their molecular composition is represented by a nearly straight line, and the temperature may with small error be loo( -tB).The greater the calculated by means of the formula t = t, +-!? t, difference between PAand P,, the greater is the deviation of the boil- ing point-composition curve from a straight line, and the higher is the molecular percentage of A in that mixture which shows the maximum deviation, D.This percentage is given with fair accuracy by the formula pD=50 +0.18A (where A is the difference between the boil- ing points of A and &'),and the maximum deviation may be calculated with very slight error from the formula I) --0-00015SA2 .c",~ -__ c' .T' CB dtwhere c, and c, are the values of -. -1 for the two components dp 1' c' = (50+0.18A)cA +(50-Oo18A)c, and -____---100 -~(50 + O*lSA)Y', + (50 -O.ISA)/I,p= 100 The values of D,,calculated from the above formula, and of D,, deduced from the actual vapour pressures (ITrccns., 1902, 81, 752) for nineteen pairs of closely related compounds, were shown in a table.The greatest difference between L), and D,is 0*16*,although the actual value of D,is in one case -32.8'. The boiling point curves have been determined experimentally in five cases, and the maximum devia- tion, D,,read from the curves; the greatest difference between D, and D,is 0.27". For mixtures of liquids which are not closely related, the formula p=ppA+(loo-p)pB is not, as a rule, applicable, but if the ratio ?A_-______-100 CB 219 lies between 0.95 and 1.05 (probably between 0.9 and I-l),D,agrees well with D,,and in other cases the difference rarely amounts to one degree. The observed boiling points of mixtures differ, however, as a rule, from those deduced from the vapour pressures, more especially when the molecules of one or both liquids are associated.Whether a mixture of constant boiling point can be formed or not depends chiefly on the relative values of A and D,-Dl.If A is very small, such a mixture may be formed even when the difference be- tween D,and D,is less than lo,as in the case of carbon tetrachloride and benzene (A = 3-44’, D,-D,= -0.S9’). On the other hand, methyl alcohol and water do not form such a mixture, although D,-D,= -4-95’, A having in this case the high value 35-11”.170. “Note on the condensation points of the thorium and radium emanations.” By E. Rutherford and F. Soddy. It was shown (Trans., 1902,81, 342) that the radioactive emanation from thorium compotlnds passed in unchanged amount through a tube cooled to -78” with solid carbon dioxide and ether. The acquisition of a liquid air plant has enabled the authors to repeat the experiment at a lower temperature, with the result that they have now succeeded in condensing both the thorium and the radium emanations. A current of hydrogen (or of air) was passed through the thorium or radium compound, and thence throngh a copper spiral cooled in liquid air. No trace of emanation escaped in theissuing gas either in the case of radium or OF thorium.At the temperature of liquid air the emanations are therefore either condensed or lose their activity. The radium (or thorium) compound was then removed, and the gas current sent directly through the spiral tube, which was quickly taken out of the liquid air and placed in cotton cool. Nothing happened for two or three minutes as the temperature of the spiral slowly rose, until suddenly the presence of the emanation was observed in large amount in the escaping gas. The result therefore cannot be explained by supposing that the emanations lose their ionising power at the temperature of liquid air. It is clear that they are condensed and again volatilised. From the sharpness and suddenness of the phenomena there appeared to exist for each emanation a definite temperature of volatilisation.This temperature is very nearly the same in the two cases and considerably above the boiling point of liquid air. By measuring the temperature of the copper spiral at the instant of volatilisation, it was found that successive determinations agreed 220 amongst themselves to within a degree. The exact temperatures cannot yet be given, but as a first approximation it may be said that for the radium emanation the volat,ilisation point lies in the neighbourhood of -130’ and for the thorium emanation about five degrees lower. This experiment furnishes an additional proof-if such were needed -that radioactivity is accompanied by the continuous production of special kinds of active matter, which possess distinct and sharply defined chemical and physical properties. 171.‘‘Note on the action of barium hydroxide on dimethylvioluric acid.” By Miss M. A. Whiteley, D.Sc. When dimethylvioluric acid is decomposed by boiling with barium hydroxide, the chief product is isonit,rosom;tlondimethylamide, which crystallises in well developed prisms belonging to the monosymmetric system (a :b :c = 1.53394 : 1;0.88680 ; = 68’43’) ; it melts at 157’, and yields a yellow potasGtim salt and a purple ferrous Palt,both of which are crystalline. In addition to this compoiind, six other decomposition product-s can be isolated, one, melting at 23!3-240’, has not been identified, the other five are carbon dioxide, oxdic acid (a4 barium salts), monomethyloxamide, methylamine, and methylamine oxamate.An-dreasch (Monntsh , 1895, 16, 17), who first examined this reaction, obtained only three products, nnmely, carbon dioxide, methylamine, and a crystalline compound melt,ing at 228’ which he identified as iso-nitrosomnlondimethylamide ;this investigation. however, indicates that it was probably an impure specimen of monomethyloxamide. 172. ‘‘The determination of strychnine and brucine in nux vomica.” By E. Dowzard. In order to determine the strychnine, the pure mixed alkaloids are dissolved in 50 C.C. of 2 per cent. sulphuric acid, 5 C.C.of nitric acid are added, and the mixture allowed to stand for 15 minutes; the solution is transferred to a separator containing 15C.C.of ammonia (sp. gr.0.S90) and 10 C.C. of chloroform, the mixture is shaken for 5 minutes, the solvent separated,and the alkaline liquid again shaken with 10c c. of chloroform. The mixed chloroform washings are now shaken with 15 C.C.of dilute ammonia (1 C.C. of above mentioned strength, diluted to 45 c.c.), this is repeated twice, the chloroform evaporated off, and the residue dried at 100’ until constant. To determine the brucine, a standard briicine solution is required, which is made by dissolving 0.16 gram of anhydrous brucine and 0.16 227 gram of strychnine in 2 per cent. sulphuric acid and the soliltion made up to 100 C.C. Then 0.10 gram of the pure mixed alkaloids is dissolved in 50 C.C.of 2 per cent sulphuric acid, this solution and 50 C.C. of the standard are placed in two small beakers, 5 c.c. of nitric acid (sp. gr. 1.42) are added simultaneously to the contents of each beaker; the solutions are then transferred to the comparison troughs of a Gallenkamp colorirneter. Five minutes after adding the nitric acid, six readings are taken; from the average of these, the brucine is calculated. Results were given which proved the accuracy of the determination made by both these methods. RESEARCH FUND. A meeting of the Research Fund Committee will be held in December. Applications for grants, to be made on forms which can be obtained from the Assistant Secretary, must be received on or before December 8th. At the next meeting, on Thursday, December 4th, at 8 pm., when there will be a Ballot for the Election of Fellows, the following papers will be communicated : “The absorption spectra of metallic nitrates.Part IT.’’ By W. N. Hartley, D.Sc, F.R.S. ‘‘The specific heats of liquids.” By H. Crompton. “ The constitution of enolic benzoylcamphor.” By M. 0. Forster. “Isomeric benzoyl derivatives from isonitrosocamphor.” By M. 0. Forster. ‘‘The constitution of the products of the nitration of m-acetoluidide,” By J. B. Cohen and H. D, Dakin, CER,TIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.B.-The Eames of those who sign from ‘(General Knowledge ” are printed in italics. The following Candidates have been proposed for election. A ballot will be held on December 4th, 1902.Alder, John Frederick, 13, Priestwood Mansions, Highgate, N. Headmaster of the Higher School, East Finchley, N. 1nter.B.Sc. (Lond.), Qualified Science Teacher under Science and Art Depart- ment ; two years Demonstrator at High School, Mitldlesbrough, three years Science Master, East Finchley Science School ; Lecturer in Chemistry to the Middiesex County Council (Finchley Centre). J. Archyll Jones. John Geo. Taylor. Frederick Doyle. Geoiage Dean. A. Greeees. Beams, Alfred Edward, Moatlands, Paddock Wood, Kent. Analytical and General Chemist at Falcon Works, Wallis Road, Hackney Wick. Formerly Chemical Student at King’s College, London, under Professor J. A%. Thomson. R. L. Barnes. T’. A. Lawson. W.S. Simpson. F. Evershed. R.MeZdok~6. 223 Blair, Herbert, No. 3, General Hospital, Kroonstad, O.R. Colony, or c/oRobert Blair, Solicitor, Harton Lodge, Harton, South Shields, England. Compounder of Medicines, Analytical Chemist and Assayer ;Student in Chemistry and Assaying at the Durham Ccllege of Science, Newcastle-upon-Tyne. John C. Hewlett. P. Phillips Bedson. Charles Nills. F. C. Garrett. S. Hoare Collins. Brincker, John Augustus Herman, 7, St. Mary’s Terrace, Paddington, London, W. Medical Officer to the Croydon Borough Fever Hospital, and Bacteriologist to the Croydon Borough. B.A. (CaKlti3,b ; First Class Natural Science Tripos), 1896 ;‘B.A. (Univ. Cape of Good Hope-Honours in Mathematics and Science), M.B., B.C.(Cantab) ; M.R.C.S. (Erg.), L.R.C.P. (Lond.) ;D.P.H. (Cantab),D.P.H.,R.C.P.S. England, Late Assistant to the Prof. of Chemistry, U.C.G.H. ; Government Scholar in Cliemistry, Univ. .C.G. H. ; Porter Student and Univ. Scholar, U.C.G.H. ; Foundation Scholar St. John’s College, Cantab. and Univ. Exhibitioner in Natural Science, Stx Mary’s Hospital. James Moir. Edward A. A udrews. Henry Kenwood. Aithur P. Luff. Chris topher Child s. J:3’.Byaga. W. H. Corfield. 8anzueZ Rideal. Bryant, Vernon Seymour, Camborne, Cornwall, England. Chief Chemist to the Egyptian Salt and Soda Company, Natural Soda Works, Bir Hooker, Wadi Natron Estate, Lower Egypt. Senior Minor, and Foundation Scholar and Natural Science Prizeman of Downing College, Cambridge.13.8. Nat. Sci. Tripos, 1899. W. J. Sell. John J. Geringer. Ayerst Henham Hooker. Henry Jackson. W. H. Lewis. Carmichael, Thomas 3urnel1, Parton, Whitehaven, at present living at 415, Walton Breck Road, Anfield, Li verpool, Student with Nessrs. A, Norman Tate & Co., Hackins Hey, Liver- pool, Analytical Chemists. Previous to the above was a student in the 224 Laboratory of the Mossbay Hematite Iron and Steel Go.. Workington, Cumberland, with Mr. G. Valentine, Chief Chemist. J. W. Clayton. T. Armistead Ward. Wm. Hall Jowett. Wi1liam Barrington. Archd. Kitchin. Cockle, Charles, Peter Symonds’ School, Winchester. Science Master. Two years’ training at the Royal College of Science, South Kensington ; 1893-1895. 1st Class Honours, 1896, Practical Inorgan.Chem. Seven years’ experience in teaching Chemistry in Secondary Schools : Dorchester Grammar School ;Camberwell Gram- mar School ; Peter Syrnonds’ School, Winchester. My chief reason for beiug admitted is to secure the best literature ou Chemistry. AE. 0. Forster. H. Burrows. G. T. Norgan. J. W.Hiuchley. W. Palmer Wqnne. Drought, James J ustinian, P.O. Box 4058, Johannesburg. Present address, Woodlands, Slackrock, Co. Dublin. Assayer and Consulting Chemist. Member of the Chemical aud XetL Society of South Africa. Chief Assayer, the Lnncaster Gold Mining Co., Krngersdorp. Cyanide Manager and Acting General Manager, the Nooitgedi-tcht E. and G.M. Co., Lydenburg. Consulting Chemist to the Lsnglaagte Etecovery Works, Ltd.Johannesburg. W. N. Hartley. George T.Holloway. J. Holrns Pollok. w.F. Cousins. 1% E. Adeney. Edlin, Edgar Leeder, B.A., Marsh Parade, Newcastle, Staffs. Senior Science Master, the High School, Newcastle, Staffs. For-merly Science Exhibitioner at Merton College, Oxford, 1st Class in Honours Chemistry, Natural Science School, in June, 1900 ;now Senior Science Master, .NemcastJe, Staffs. John Watts. J. E. Marsh, W. W. Fisher. H. A. hliers. V. 11, Veley. H. L, Bowman, 225 Edwards, Walter Henry, The Grammar f3cli001, Wellingborough, Northants. School Master. Science Master, Wellingborough Grammar School since 1895. H. Brereton Baker. R. H. Aders Plimmer. Frank Clowes. R. T. Lattey. Arthur H. Coote.Green, George Felix Dudbridge, Rosslea, 9 Ross Road, South Norwood, S.E. Analytical Chemist. At present Assistant to Xr. Matthew J. Cannon, E.C.S. General and Scientific Education, Dulwich College, S.E., and Lyde Jansan, Paris. First year of Diploma Course at City and Guilds tinder Professor Henry Armstrong. Two years under Professor J. M. Thornson, King's College, W.C. Course of Bacteriology under Professor Cruickshank. Passed the Intermediate for A.I.C., July 1901. Now Assistant to bfr. M. J. Cannon, F.C.S. John M. Thonison. D. Northall-L:iurie. Herbert Jackson. Natthew J. Cannon. Patrick H. Kirkddy. Robert Yates. C. T. Kingzett. Grimwade, Wilfred Russell, Melbourne, Australia. Manufacturing Chemist. Bdielor of Science of the Melbourne Uuiversity.Orme Nasson. Robert iu. Leunox. Thomas Tyrer. N. H. Hartin. J. Le wkowitsch. Il'cdter 3'. Reid. J. Campbell Byown. Gumersall, Edward, Atbara, Sidcup, Kent. Sub-Inspector Eoard of Education. Certificate for Associateship Course' in Chemistry of Royal College of Science, London. Have been engaged in promoting the teaching of the subject under the Board of Education for the past eight years, T. E. Thorpe. R. MeIdola. \Y. Pjlmer Wynne. A. E. Tutton, Ohapman Jones. 226 Hollingworth, David Vincent, Aldred House, Crescent, Sdford. Analytical Chemist. .Have had four year&’ traiuing in Inorganic and Organic Chemistry, Cod Tar Products, &c., &c., at Royal Technical Institute, Sitlford. I have position as chief chemist at Stretford Gas Works, and desire to keep myself well informed, in Modem Chemistry by perusal of the literature of the Chemical Society.Jas. R. Appleyard. Ernest Clark. J. R. Denison. Jccrnes IVaZker. John S.L~msde~2. Holt,Alfred, jun., B.A.(Camb.), Crofton, Aigburth, Liverpool. Research Student in the Owens College, Mqchester. Studied Chemistry at Cambridge, and worked with Professor Moissan at the Sorbonne, and has published two papers in conjunction with M. Moissan on the preparation of two silicides of vanadium. Harold B. Dixon. W. H. Perkin, jun. Norman Smith. J. F. Thorpe. D. L, Chapman. Framis V. Darbishire. Hosking, Arthur Francis, Roskear Villas, Cstinbome, Cornwall, England. Chief Chemist of the Cyanide Works, and Reduction Plant of the Arubs Gold Concession, Limited, Aruba Island, D.W.I.1891-1 SO3 private student assistant to John J. Beringer, Esq., A.R.S.M., F.I.C., F.C.S.,obtaining Honours in Chemistry and Metallui*gy, South Kensing- ton Exams. First position in Cornwall both years, and highest council prizes. 1893 to 1896(three years), Demonstrator in Honours Chemistry, Metallurgy, and Assaying at the Camborne Mining Schools, Coruwall. During this period I made the complete analyses of rock formations for the Geological Surveys made by the President of the Cornmall Geological Society. T received the highest award of the Royal Corn- wall Polytechnic Society for complete analyses with microscopic sec- tions and diagrams of various strata from the bottom of the Dolcoath Tin MZne in Cornwall. Also, for a period of over a year I made the assays of white tin and arsenic productions of the Drakewail Tin, Copper, and Arsenic Mines in North Cornwall, to the thorough satis-faction of the mine and the arsenic refiners who mere the buyers.July 1896 to end of 1898. Engaged as assistant manager and tech-nical expert to the Cassingrt Concession’s Prospecting Expedition in Angola, South-west Africa. 1899 to April 1900. Special studies 2.27 and research work on working potass cyanide liquors, &c., at the Camborne Mining School Laboratory. During this period I was awarded the silver medal of the Mining Association and Institute of Cornwall and Devon for chemistry, metallurgy, and allied subjects.April 1900 to date. Chief chemist of the Cyanide Works and reduc- tion Piarit of $he Aruba Gold Concession, Aruba Island, Dutch West Indies. Thomas Blackburn. J. J. Beringer. H. R. Beringer. H. W. Hutchin. John Gill. Jackson, Clements Frederick.Vivian, Bris bane. Assistant Government Geologist of Queeneland. Bachelor of Min-ing and Metallurgy (Sydney University, 1900); Student for three years in the Chemical and Metallurgical Laboratories, University of Sydney, under Prof. Liversidge and Mr. J. A. Schofield. First Class honours Quantitative and Qualitative Analysis ; First Class honours General Chemistry ; Second Class honours Metallurgy and Assaying ; First Class honours. Physics ; Slade Prize for Practical Physics ; Bachelor of Civil Engineering (Sydney University, 1895) ; Associate Member of the Institution of Civil Engineers (London).A. Liversidge. Chas. Watkin. J. A. Schofield. J. Brownlie Henderson. Basil Turner. Jardine, Douglas Kennedy, B.Sc., 20, Doune Terrace, Kelvinside, Glasgow, N. Analytical Chemist. Studied at Owens College for five years, 1884-1898, and later at the Laboratory of the City Analysts, Messrs. R. R. Tatlock and Thomson, 1899 till date. Work consisted of analyses of every class, Scientificsand Commercial. Holds Degree of Bachelor of Science. R. R. Tatlock. W. H. Perkin, jun. H. B. Dixon. G. H. Bailey. D. L. Chapman. Leather, John Petty, 17, Carlton Road, Burnley. Gas Engineer and Manager of Burnley Corporation Gas Works.Studied Chemistry under Profs. Roscoe and Schorlemmer, 1876-1879. Since then Assistant Manager and Chemist, and for last twelve years Engineer and Manager of Burnley Corporation Gas Works. Joint 228 author of paper (Soc. Chem. Ind.) on the Constitution of Gas Oils. At present engaged with Mr, Itoss in a research on Bvrneo oil. Raymond Ross. George Ernbiey. Wilfred Irwin. Chas. J, Waterfall. James Bertram Russel I. Lidbury, Frank Austin, M.Sc., Omens College, Nanches ter. Demonstrator and Assistant Lecturer in Chemisiry in the Owens College. Studied Chemistry at the Oweris College (B.Sc., 1898), Research work with Prof. Rsmsay and Prof. Ostwald. Has pub-lished, in the JoumaZ Chertz. Xoc., Iwo papers, and one paper in ZeiL.Phys. Chew&. Harold B. Dixon. J. F. Thorpe. W. H. Perkin, jm. 1).L. Chapman. Norman Smith. Francis V. Darbishire. Liotard, Ernest, 2, Rue de France, Nice, France. Pharmacien de premiere classe, Rlembre de la Socidte chimiyue de Paris, de la Socikte de pharmacie de MOSCOU, de Medecine de Nice. Auteur du trait4 d’analyse des urines, des huiles essentielles des essences antiseptiques, du rnanuel de pharmacologie, et de notes de chimie. Alfred H. Allen. G. E. Scott-Smith. Arnold R. Tankard, G. T.W. Neu)shoZnze. L.l’roost. Logan, Thomas Stratford, 52, Kirkgute, Leeds. Physician. Studied Chemistry and allied subjects at Queen’s College, Belfast, and at Yorkshire College, Leeds ; Experience of Public Health Chemistrj , in the Sanitary Department of Leeds Cor-porittion.H. M.Dawson. H. D. Dakin. A. Turnbull. J. K. S. Dixon. B. A. Bzcr~ell. 229 MacCallum, Douglas A., 10, Midlothian Drive, Shawlands, Glasgow. Manufacturing, Analytical, and Consulting Chemist. Office address : Central Chambers, 93, Hope Street, Glasgow. (1) Technical College, Student and Assistant to Chemical Professor there, 3 years. (2) Iron and Steel Works Chemist, and latterly Assistant Manager ;analyti-cal work ;research and investigations in connection with practical working, &c., 13 years. (3) Manufacturing and consulting privately, 2 years. (4)Member Society of Chemical Industry and West of Scot-land Iron and Steel Institute. A. Humboldt Sexton.James &Cracken. R. R. Tatlock. Joh7a Clccrk. R. T. Thomsm. G. G. Hmdersoia. Mann, William, B.Sc. (Lond.), Fonnoreau Villa, Dartford. Science Lecturer ; Lecturer in Organic Chemistry and Mathematics, Technical Schools, Southend-on-Sea. Two years Teacher of Physics, Boulevard Science School, Hull, Bachelor of Science (London). Am desirous of keeping in touch with all branches of Chemical Science. Alf. 5.Parker. Jas. Baynes. F. \V, De Velliog, Thomas Luxton. W. H. Templeman. Marsh, John, 29 High St., Naidstone. Assistant Chemist to the Associated Portland Cement Manu-facturers, Ltd. I have taken the 3 years’ Diploma Course in Chemistry at the Central Technical College, Exliibition Rd., S.W. Henry E. Armstrong. T. M. Lowry.Gerald T. Moody. William A. Davis. Edward W. Lewis. Mellor, Joseph William, 62 Bland Street, Moss Side, ,Manchester. Doctor of Science, (N.Z. University) ; First Class Honours (chem- istry); 3 years 1851 Exhibition Scholar; late Senior Scholar (N.Z. University) ; engaged in Research work, as Research Fellow, at the Owens College from 1899 up to present time ;published papers in Trans-actions Chemicul Society ‘‘ On Union of H and Cl,” &c. ; and papers in other Scientific Journals. Author of ‘‘Higher Mathematics for Students of Chemistry,” &c. (Lougmans, Green and Co., London). H. B. Dixon. W. H. Perkin, jun. J. F’. Thorpe. Francis V. Darbishire. R. S. Hutton. 230 Millington, John Price, Christ’s College, Cambridge.Student. Junior Demonstrator in the Camb. University Chemical Laboratory, Scholar of Christ’s College, Cambridge. First Class in Natural Sciences Tripos Part I., B.A. (Camb.), B.Sc. (Wales). G. D. Liveing. H. J. El. Fenton. W. J. Sell. H. 0.Jones. T.I3. Wood. Phelps, John, Trinity College, Oxford. Student of Chemistry, B.A. (Oxon), Millard Sc?iol,zr, Trinity College, Oxford. Honours in Chemistry, 1st Class, Natural Science Final Schools, Oxford 1902. H. Brereton Baker. Arthur J. Webb. D. H. Nagel. J. E. Marsh. Henry A. Miers. N. V. Siclgwick. Ricketts, Guy Dunstan, Sir John Cass Teclinicttl Institute, Jt3wry Sk’reet, E.C. Lecturer on Metallurgy-at the above Institute. B4.A. (Citntah.), NaturiLl Sciences Tripos, Part I., 1898; Associ;tteship Examiliation in Metallurgy, Royal School of Nines, 1900; Assistant in Sir W.C. Roberts-Austen’s Research Laboratory, 1901. W. C. Roberts-Austen. Charles T. Heycoclr. T. K. Rose. Charles A. Kohn. W. 13. Merrett. ROBS,George Archibald Park, 20, Westliall Gardens, Edinburgh. Medical Practitioner (M.B., Cl1.6. Edin.). Graduated M.B. Ch.B. at Edinburgh in 1901. D.P.H. of the Ropzl Colleges Ediu. in 2902. Intend taking up Public Health work in the Colonies and am desirous of keeping in touch with Chemical progress. G. H, Gernmell. J. Falconer Icing. Hugh Marshall. Alex Crum Erowu. William C. Ross. Thos. Darling. Leonard Dobbi~. Sampson,John William, Helpringham, Heckington, Lincs. Analytical Chemist. For two years engaged in Organic and Analytical Chemistry under Mr.F. Eedford, B.Sc. (Lond.). For some 231 time demonstrator in Practical Chemistry at Metropolitan College of Pharmacy. Have passed Major Exam. of Pharmaceutical Society. Desirous of increasing my knowledge of Chemistry. F. Stanley Kipping. R. M. Caven. G. Druce Lander. Fred Bedford. W. Watson Will. Harry Lucas. I?. Filmer De Morgan. Sindall, Robert Walter, 80, Manor Rd., Brockleg, London, S.E. Analyst, Chemical Engineer, Paper Trade Expert. Student under Professor Armstrong at the City and Guilds Institute, South Kensington. For some years Analyst and Chemical Engineer to Messra. Edward Lloyd, Ltd. Pitpermakers, England, Norway, Canada. Now Consulting Chemist and Expert to the Pulp and Paper Trades.Henry €4. Armstrong. W. Palmer Wynne. H. F. C. Goltz. William J. Pope. Stanley J. Peacheg. Clayton Beadle. Simpson, Duncan, 10, Brynmill Crepcent, Swansea. Assayer. Having had 18 months’ study of Analytical Chemistry uncier the late W. Terrill, Esq.: 3 months’ practice in the Cape Copper Co.’s Laboratory ; 3 years at t4heSwansea Hsmatite Iron and Steel Works under F. B. Last, Esq.; 13’ months in Emu Spelter Works, research and analytical work under Messrs. Sulman and Picnrd on their patent process for treatment of sulphide ores of lead and zinc, and having in connection with this last invented and pro-tected a process for the treatment OF the furnace residues, and having since been engaged at J. S. Merry and Co.’s Lab.in work on Au, Ag, Cu, and Pb ores, &c., and having during the whole of the last seven years attended South Kensington night classes in Chemistry, Metallurgy, and Physics, Hons. Certificate. E. Howard Tripp. Godf rey Millard. Christopher James. Frank B. Last. L. Ludlow. John JV. Bevan. Ckc-vence A. Seyler. Smith, Leonard, 14, West Hill, Highgate, London, N.. Student of City and Guilds of London Central Technical College. I have been a student in the Chemical Department of the above College for three years and am now engaged in research. Henry E. Armstrong. William A. Davis. Gerald T. Moody. T. Martin Lowry. Edward W. Lewis. 232 Smythe, John Seabury, BSc., Ph.D., 143, Smithdown Lane, Liverpool. Analytical Chemist.B.Sc. (Vict.) Honours Chemistry 1897 ;Ph.D. (Wiirzburg) 1899. Chemist with Meesrs. W. Meadowcroft and Son, Ltd., Blackburn, Eqsence Distillers and Manufacturing Chemists, since January, 1900. J. Campbell Brown. Herbert B. Stocks. W. Collingwood Williams. Prosper H. Jfarsden. F. H. Tate. Stansfield, Edgar, B.Sc., Technical College, Sunderland. Assistant Lecturer and Demonstrator in Chemistry, the Technical College, Sunderland. Student at Omens College 1897-1 901, elected a Research Student October 1901. Obtained degree of B.Sc. (Vict.) Honours School of Chemistry, June 1900. Original Research : ‘‘Pre-1iminaryNote on the Preparation of Barium” read before the Manchester Lit. and Phil. Society October 29, 1901. H. B. Dixon.J. F. Thorpe. W. H. Perkin, jun. R. S. Hutton. E. Clark. Sutherst, Walter Frederick, Cheshire Agricultural College, Holmes Chapel. Lecturer in Chemistry and Analyst. Diploma of Federal Poly- technic, Zurich. Ph.D. (Geneva). A.I.C. Published following in-vestigations : “The Solubility of Phosphatic Manures in some Organic Acids” (Chem. News, 2187) ; ‘‘ the Freezing Point of Vegetable Saps and Juices ” (Chem.ilJews, 2190) ; Influence of Manilring on Chemical Composition of Potatoes ’’ (Chenz. News, 2192) ; “ Effect of Lime on the Insoluble Phosphates in Soils ” (Chem. News, 2210) ; (‘the Com-position of Colostrum ” (Chm. News, 2223) ; <‘the Reversion of Superphosphate in Soils ” (Agriculturcd Gazette, Sept. 1st, 1902) ; ‘‘Chemical Changes in the Ripening of Cheshire Cheese ” (Xoc.Chem. Ind., Feb. 28th, 1902). Thesis : ‘(Derivatives of Naphthazonium.” Edric Druce. Bernard Dyer. J. Carter Bell. Walter 15.Gardner A. B. Knaggs. Thomson, George Sutherland, Government Offices, Adelaide, South Australia. Scientific Dairy Expert to the Government of South Australia. Author of ‘; Preservatives in Dairy Produce, with Analyses ” ; “Causes 233 of Variation in the Water Percentage of Butter (with analyses) ” ; ‘LCheese Experiments and Analyses’’ ;‘‘Cattle-feeding Experiments and Analyses,” and ‘‘Stsle Butter and Anzlgses,” issued by the Government of South Australia. Instructorin Dairy Science at Government School of Mines ; College of Agriculture ; School of Agriculture ; Agricultural Bureaus, and to the Dairy Factory Managers in South Anstralin.Thomas 8. Goodwin. James Hendrick. J. F. Blackshtw. FrederickJ.Lloyd. C. M. Aikman. James McCutcheon. Jas. McCv*eath. Tidy, Henry Letheby, New College, Oxford. Medical Student. Graduate in Chemistry of Oxford University. William Odling. James Dewar. William Crookes. Harold Hartley. D. H. Nagel. Wallis, Thomas Edward, 78, Essex Road, Islington, N. Assistant Lesturer in Chemistry in the School of Pharmacy of the Pharmaceutical Society. B.Sc. (Lond.). Have published several papers dealing with the anatomy of drugs ; 1899 to 1900 Junior Demonstrator in Practical Chemistry ; 1900 to 1901 Demonstrator in Pharmaceutics in the School of Pharmacy. J.Norman Collie. IT.Carteighe. A. Lapworth. Walter Hills. D. North all-Laurie. White, William Carter, 113, Gower Street, W.C. Analyst to Messrs. Geo. Curling, Wyman & Go., 58,.Bunhill Row, E.C. Joint author of Removal of Fat from Nux Vomica Prepara- tions,” C. & D.,lxi., p. 87. Author of ‘‘ Cobalt Nitrate as a Reagent.” Ph. J.,4th series, 1674, p. 68. William Fowler. Peter RlacEwan. W. L. Howie. Thomas Tyrer. A. R. Huntington. Wilson, Lyndon, 66, Castle Gate, Newark-on-Trent. Analytical Chemist to Messrs. J. Richardson & Son, Newark-on- 234 Trent. Analytical Chemistry under J. Heron, Esq. Practical and Scientific Brewer and Maltster. John Heron. Arthur R. Ling. Leonard Temple Thorne. E.Haynes Jefers. Wm. G. Johnstone.F. Jewsorb. The following Certificates were authorised by Council under Bye-law I.(3) : Edminson, Sidney Robert, Maritzburg College, Natal. Schoolmaster. B.Sc. (London) in Chemistry, &c., for some years a chemical student at Firth College, Sheffield. Teacher of Chemistry at Maritzburg College, Natal, S. Africa. For five years Science Master at Wesley College, Sheffield. Percy John Vinter. Mukergee, Beni Madhav, Roorkee, India. Science Demonstrator, Thomason College, Roorkee, India. Graduate (science course) of the A llahabad University, formerly Science De- monstrator for four years in the Muir Central College, Allahabad. Since 1899, Demonstrator in the Thomason College, Roorkee, in which capacity he has to lecture to the Engineer Classes on Chemistry and also do the commercial analysis undertaken by the College. Abbyacharan Sanyal. PEbram, Richard,Ph.D. The University, Czernowitz, Austria. Professor of Chemistry in the University of Czernowitz. Hans Meyer. William Rcmsccy. RIOEARD IILAY AND SONB, LIMITED, LONDON AND BUNGAY.
ISSN:0369-8718
DOI:10.1039/PL9021800207
出版商:RSC
年代:1902
数据来源: RSC
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