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Proceedings of the Chemical Society, Vol. 30, No. 424 |
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Proceedings of the Chemical Society, London,
Volume 30,
Issue 424,
1914,
Page 21-52
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摘要:
[Issued 16/2/14 PROCEEDINGS OF THE CHEMICAL SOCIETY. Vol. 30 No.424. Thursday, February 5th, 1914, at 8.30 p.m., Professor W. H. PERKIN,LLD., F.R.S., President, in the Chair. The PRESIDENTreferred to the loss sustained by the Society, through death, of: Elected. Died. Frsiilr Baker........................ Feb. 21st, 1907. Jan. 21st, 1914. Frederick George Bicharcls...... Feb. 15th, 1905 Jan. 21st, 1914. Certificates were read for the first time in favour of Messrs.: Abdel Hameed Ahmad, B.Sc., The University, Edgbaston, Birmingham. Charles Wesley Bayley, 63, Caxton Road, Wood Green, N. Robert Bsrclay Craig, 50, North Albion Street, Glasgow. Jaroslav Heyrovskf, B.Sc., 24, Agincourt Road, N.W. Lawson John Hudleston, B. Sc., 68, Parliament Hill, Hamp-stead, N.W.Arthur Ulysses Newton, B.Sc., 37, Netherhall Gardens, Hamp- stead, N.W. La11 Behary Seal, Third Assistant Chemical Examiner, Rangoon, Burma. Norman Cecil White, B.A., B.Sc., 35, Spencer Park, Wands- worth, S.W. Of the following papers, those marked * were read: 22 *25. Existence of racemic compounds in the liquid state.’’ By Clarence Smith. The investigation, by the Ramsay-Shields’ method, of the exist- ence of racemic compounds in the liquid state (Mitchell and Smith, T., 1913, 103, 489) has been extended to include substances which contain a hydroxyl group. Not infrequently such substances are associated in the liquid state. The dissociation produced by rise of temperature is manifested by an abnormally large rate of decrease of the molecular surface energy, so that the value of k increases with rise of temperature, and does not remain constant (or decrease slightly), SLS is the case with unassociated liquids.If, therefore, the optically active modifications of a liquid are associated and the inactive form is an equal molecular mixture of the active forms, the expectation is legitimate that the k values of all the modifica,- tions will increase at the same rate with rise of temperature, whereas if the inactive form is a racemic compound (associated or not), material differences will be observed in the k values of the inactive and the’ active liquids. Unfortunately, all the liquids, the active forms of which are at present at the author’s command, have proved to be unassociated between Oo and 90°, so that the preceding method of proof is unavailable.However, the practkally constant and not materially different k values of the active and the inactive modifications of each of the substances examined prove, as in the case of the pinenes and the limonenes (Zoc. cit.), that the inactive modifi~at~ions are not liquid racemates. The following values of k (mean of four values between loo and 80°) have been calculated : methyl-fl-phenylethylcarbinol, dl-form 2.185, d-form 2.015, I-form 2-15; methylhexylcarbinol, dl-form 2.045, d-form 1.975, E-form 1-91;phenylethylcarbinol, dl-form 2.02, ,?-form 1.96 ; methyl P-hydroxy-P-phenylpropionate,61-form 2.33, d-form 2.395. DIscusSION.Dr. DUNSTANpointed out that Mr. Thole had already shown bhat the inactive carbinols prepared by Dr. Pickard were dl-mixtures and not racemic compounds. He further stated that, even when racemic compounds had been found to exist in solution, the quanlity present in equilibrium with the active components was always very small. “26. (‘The water gas equilibrium in hydrocarbon flames.” By George William Andrew. The author has examined the equilibrium conditions as regards the reversible system CO +OH2 CO,+ H, in hydrocarbon flames 23 by exploding ati varying initial pressures homogeneous mixtures of such hydrocarbons as methane, ethane, and ethylene with quanti- ties of oxygen insufficient for complete combustion, but sufficient to prevent any depositioii of carbon on explosion (for example, CH, +O,, 2CH4+ 30,, 2C,H6 + 30,, 2C2H, + So,, C,H, +20,, etc.).The results prove that, notwithstanding the very different maximum flame temperatures in the various experiments, the equilibrium ratios ‘Ox OH2 in the cooled products were nearlyUO, x H2 constant t’hroughout the series, and practically identical with the value found by H. B. Dixon in his well-known experiments on the division of oxygen between CO and H, in flames, thus: Mixtwc. CH,+ 0, .................... 3’98 2CH, + 302 ..................... 3-98 2C,B, + 30,. .................... 4’1 2 2C,H, +50, ..................... 3’63 2C,H4+-30, ................... 3-33-Mean ... 3.83 It would thus appear that the experimentally determined equili- brium constant “ K ” does not correspond with the maximum flame temperature, but with some lower temperature in the “ cooling curve” when the gases cease to react rapidly.This temperature is identified as lying somewhere between 1500O and 1600O. It was further shown that so. rapidly does the equilibrium in the system CO + OH, CO, i-H2 adjust itself to the falling temperature, during the cooling period down to the said temperature, that even the deposition of carbon or the recurrence of considerable quanti- ties of methane in the products has little or no influence on the said equilibrium. 27. “The absorption spectra of the vaponrs and solutions of various substances containing two benzene nuclei.” By John Edward Purvis.The observations prove that all the various vapour bands of benzene are obliterated in such compounds as diphenyl, diphenyl- methane, diphenylamine, diphenyl ether, etc., and all the various vapour bands of aniline in such compounds as azobenzene, azoxy- benzene, benzidine, etc. In every instance the vapour bands and the solution bands are similar. 28. “The oxidation of some benzyl compounds of sulphur. Part 11. Benzyl tetrasulphoxide.” By John Armstrong Smythe. When benzyl tetrasulphide is oxidised with hydrogen peroxide, benzyl tetrasulphoxide is formed in quantitative yield. Benzyl trisulphide, on oxidation, gives the same compound, in addition to benzaldehyde, sulphuric acid, and benzylsulphonic acid.Bensyl tetrasulphoxide is a somewhat unstable compound, melt- ing at 134-139O and decomposing at its melting point into benzyl disul phide and sulphur dioxide. When heated in solution, or treated with a variety of reagents, it decomposes into benzyl disulphoxide, sulphur, and sulphur dioxide, and the subsequent reaction of these products gives the clue to a number of changes which the compound undergoes. Excess of hydrogen peroxide oxidises the tetrasulphoxide to sulphuric and benzylsulphonic acids ; some benzaldehyde is also formed, as is the case with all the polysulphidic compounds of benzyl on oxidation. Other reactions, which serve to bring out the relationship of the tetrasulphoxide with other sulphur compounds, were described.29. The reaction between iodine and aliphatic aldehydes.” By Harry Medforth Dawson and Joseph Marshall. According to C’hautard (Ann. Chim. Phps., 1889, [vi], 16, 145), iodine reacts with the aliphatic aldehydes in alcoholic solution in the presence of iodic acid, and monoiodo-substitution products are formed. In some cases the substances obtained are supposed to be a-derivativm, whilst in others it is claimed that &substitution products are produced. In view of the fact that evidence has been obtained that halogen substitution in the aldehydes is preceded by isomeric change, and that p-substitution products cannot be accounted for, if this is the mechanism of the reaction, it was considered advisable to repeat some of Chautard’s experiments.The authors find that there is no evidence of the formation of 0-iodopropaldehyde, the properties of the substance obtained being in entire agreement with the supposition that it is the a-iodo- derivative. The statement that alkyl esters are formed when the iodoalde- hydes are acted on by silver acetate is also not confirmed by the authors’ observations. In the case of iodoacetaldehyde, no trace of ethyl acetah was found, and the product appears to be acetyl- glycollaldehyde. 25 30. The erosion of lead.”L‘ By John Franois Liverseege and Arthur William Knapp. The authors have examined the action of a slightly alkaline natural water on strips of sheet lead under the conditions of the test proposed by Houston (area of 6-45 sq.cm. of lead exposed to 10 C.C. of water in a test-tube), save that a duration of one day was preferred to the seven or fourteen days suggested by Houston. It was found that erosion was due to the action of oxygen in the presence of water. Carbon dioxide in an amount up to 1 per cent. by volume produced little effect on the amount of erosion; when 2 or more per cent. of carbon dioxide was present, erosion no longer occurred, for the liquid remained clear, and lead was dissolved (in amount less than that removed by erosion). The amount and kind of erosion was chiefly dependent on the alkalinity of the water. With alkalinity expressed as parts of calcium carbonate per 100,000 of water, (a) lime giving 3--9 parts of alkalinity reduced the erosion, but larger and smaller quantities slightly increased it; (b) calcium carbonate giving 4 parts of alkalinity greatly reduced erosion ; (c) calcium carbonate giving only 2 parts of alkalinity practically prevented it.Variations in the amount of organic matter did not influence the erosion. Exposure to glass lowered the erosive quality of the water, but filtration through sand did not. The amount of lead eroded was less the greater the distance from the lead to the water surface, and was generally proportional to tohe area of the surface of the lead exposed, and independent of the volume of tlhe water. 31. “Beylation as influenced by steric hindrance: the action of acid anhydrides on 3 :5-dinitro-paminophenol.” By Eaphael Meldola and William Francis Hollely.The known N-acetyl derivative of the above dinitroaminophenol is best prepared by starting from the diacetyl derivative and hydrolysing the latter by cold dilute sodium hydroxide solution. The authors find that this dinitro-p-aminophenol has the remark- able property of becoming acylated at the hydroxyl group with extreme facility, the 0-aoetyl derivative being formed by simply boiling the dinitro-compound with a little acetic anhydride diluted with acetic acid for half-an-hour or less. In these circumstances the amino-group is unattacked, and the isomeric N-acetyl and 0-acetyl deriyatives can accordiiigly be preparea by regulating the conditiom, The authors attribute this property to the extreme 26 protection of the amino-group by the ortho-nitro-groups, aided probably by an ortho-quinonoid structure due to the existence of an “inner salt ” structure : OAc /\II O”\/:I1 No\/O’ NH,---Reasons were given, based chiefly on the marked difference in colour between the isomerides and the character of their absorption spectra (photographed by Dr.J. T. Hewitt), for assigning the above formula to the 0-acetyl derivative, The’ authors conclude that all the nitro-derivatives of the aminophenols in which there is a nitro-group adjacent tlo an amir,o-group are best represented as “ inner salts ” of the above type. 32. “The constitution of carbamide. Part I. The preparation of isocarbamides by the action of methyl snlphate on carbamides.” By Emil Alphonse Werner.It was pointed out that hitherto carbamide has not been known to yield by any direct reaction derivatives of the type HN:C(OR) *NH,, in contrast to thiocarbamide, which readily affords the sulphur analogues HN:C(SR)-NH, by the direct reaction with the alkyl haloids. So far, isocaxbamides of the types HN:C(OR)-NH,, RN:C(OR)NH,, and RN:C(OR)-NHR have been obtained by the union of cyanamides and alcohols in t%e presence of hydrogen chloride or sodium ethoxide (Stieglitz and McKee, Ber., 1900, 33, 1618; and Bruce, J. Amer. C’hem. SOC.,1904, 26, 419, 449). It was shown t’hat methylisocarbamide and its substituted deriv- atives may be readily prepared from carbamide and substituted carbamides by the aid of methyl sulphate; the change takes place quantitatively in accordance with the equation : NH + (cH,),s~,= HN:c<~.~~HN:c<~~~~ N H,,CH,-HSO, 3 Whilst in the case of carbamide the reaction is liable to bacoirie very violent unless the temperature is carefully controlled, the chige proceeds quite smoothly with the substituted derivatives.The free bases may be isolated by treating the product with sodiuni hydroxide solution, and extracting with ether or alcohol. The decomposition of methylisocarbamide methyl hydrogen sulphate, and the substituted derivatives has been examined, and the results have furnished interesting confirmatory evidence in support of the author’s views regarding the constitution of carb-amide and substituted carbamides ;thus, whilst the methylisocarb- NRamide salt and the derivatives of the types HN:C<0.C2H, and HN:C<g!EL, afforded cyanuric acid and mono-N-methylcyanuric acid as part of the decomposition products, neither of these acids NHwas obtained from the derivatives of the type RN:C<O.Cb, prepared from the mono-substituted carbamides.The interaction of carbamide and methyl sulphate carried on slowly to the stage of the decomposition of the isocarbamide salt may be used as a quick and simple method for the preparation of pure methylamine. If the reaction is allowed to become very violent some dimethylamine is formed. 33. “A new formula for the latent heat of vapours.” By Malcolm Percival Applebey and David Leonard Chapman.A new formula for the heat of vaporisation of liquids, of which a preliminary account has already been published (P., 1913, 29, 24) was deduced from the thermodynamic principles and van der Waals’ equa&ion. The latent heats of the vapour of some common non-associated and associated compounds were calculated with the aid of the formula, and the values obtained were compared with those experimentally determined by S. Young (Sci. Proc. Roy. Uubl. Soc., 1910, 12, 414). 34. The electro-deposition of zinc at high current densities.” By John Norman Pring and Urlyn Clifton Tainton. At certain very high-current densities the electro-deposition of zinc can be effected in presence of a high concentration of free acid. Under these conditions the ratio of zinc to hydrogen liber- ated actually increases with the acid concentration up to a certain value, and also increases with the current density.In this way, with a concentration of sulphuric acid of about 15 grams per 100 C.C. and a current density of between 20 and 50 amperes per sq. dcm. the metal can be deposited with an efficiency of about 95 per cent. With lead anodes this electrolysis is achieved with a potential difference about 5 volk and with zinc anodes 3 volts. The presence of small quantities of colloidal matter exerk a marked effect on this reaction, and enables the production of bright, 28 adherent deposits. The presence of the colloid also enables the application of a higher current density, and in this way raises the current efficiency.In these solutions a very strong retardation was observed in the deposition of iron present in the electrolyte. On account of this, considerable quantities of this metal in the electrolyte caused very little contamination of €he zinc. The results obtained could not be entirely ascribed to effects of over-voltage, or surface tension, or viscosity of the electrolyte, and are probably mainly determined by influences which control the rate of the reactions involved in the change from the ionised to the free element. Thet results obtained in this work indicate the most favourable conditions under which zinc can be obtained from commercial solutions, either with a view to the recovery of the metal or to its application for the purpose of electro-plating.35. The ageing of alloys of silver and tin.” By William Arthur Knight, The author has investigated the ageing of filings of alloys of silver and tin, and the densities of unaged and aged filings of the alloy Ag,Sn. The ageing of filings of the alloy AgsSn is not accom- panied by a detectable change of weight, and this applies whether the ageing is carried out in coal gas or in air. Ozone and hydrogen peroxide did not oxidise these filings at room temperature, and, further, after treatment with these oxidising agents, the filings were still unaged. From these experiments, in conjunction with others previously published, the hypothesis that the ageing of these filings is due to superficial oxidation was shown to be untenable.It was found that hydrogen sulphide at room temperature had no effect on the state of ageing of the filings. The phenomenon of ageing becomes less pronounced when the content of silver in the alloy exceeds 75 atoms per cent., solid solutions of silver in the compound Ag,Sn thus having the same effect as the free tin ;.n those alloys which contain less than 75 atoms per cent. of silver. Density determinations showed that the density of aged filings of the alloy Ag3Sn is greater than that of unaged filiqs; thus, as there IS no increase in weight, there must be a contraction in volume on ageing. Dilatometer measure-ments confirmed this contraction, although bhe results did not agree accurately with those deduced from density determinations.36. "The action of phosphorus pentachloride on the esters of glyceric acid ; optically active ap-dichloropropionates." By Percy Faraday Frankland and Andrew Turnbull. From lzevorotatory methyl, ethyl, isobutyl, and heptyl glycerate respectively the authors have obtained the corresponding aB-di-chloropropiopates, of which the methyl compound was dextro- and the others lmo-rotatory. The dextrorotation of methyl aj3-di-chloropropionate increasee with rise of temperature, whilst the lzvorotation of the others diminishes in the same circumstances. There would appear, therefore, to be no doubt that all of these dichloropropionates have the same configuration. A more highly chlorinated inactive compound was in each case also obtained, having the molecular formula C3H2C1,0R, of which the probable constitution is CH2C1*CCl,*CC12*ORor CHCI,.C'HCl*CCl,*OR, in which R stands for methyl, ethyl, isobutyl, and heptyl respec- tively (see also T., 1913, 103,718). 37. '' A criticism of Holmes' method of determining the molecular complexity of liquids.? By William Ernest Stephen Turner. In a recent paper (T., 1913, 103, 2147), and in continuation of previous work (T., 1906, 89, 781; Holmes and Sageman, ibid., 1907, 91, 1608; 1909, 95, 1919), Holmes sets out the results of a method which he employs for the determination of the molecular complexity in the liquid state. As a new method of attacking an old problem it deserves a welcome, but the results are so much different from those deduced on the basis of other and well-known metliods that they call for examination.The, view adopted by the author of the theory is that in most cases the only forces which are brought into action when two liquids mix are of a physical character, and that the miscibility of liquids depends on the true relative molecular volumes, or what comes to the same thing, the relative radii, of the constituents. The method employed to obtain the relative complexities is, there- fore, to determine the molecular composition, referred to the gaseous state, of the liquid mixture in which the maximum devia- tion occurs between the calculated and observed proportions by volume of the constituent with the larger molecular volume. The ratio of the molecular proportions so obtained is considered as that of the relative molecular complexities, water, for example, from its mixture with ethyl tartrate being considered to have a molecule, (H20)4,relative to the ester; and by similar processes, molecular 30 (c4H1~o)4~(CBC1,)&p(cGH6)8, (cGH14)8, and (cs2)1G are assigned.In practice, however, the method is not so simple as it appears; thus, the mixtures of maximum deviation in the case of water with ethyl and propyl alcohols are C2H60,1$H,0 and C3H,0,14H20 respectively, and of water and n-butyric acid, 4C4H,02,7H,0 ;yet the aIcohols and butyric acid are nevertheless held to be of a similar complexity to water in order to agree with the author's theory that molecular radii must have certain values to permit of miscibility.Nor are substances of approximately equal molecular volume, like aniline and ethyl acetate, soluble in water to anything like the same extent, and to explain this dis- crepancy, speculations are introduced concerning the quasi-electri- cal forces which are presumed to act, causing disturbances in the molecular volume or co-volume. Without dea.ling further with these speculations, however, it may be said that the results themselves are sufficient evidence of the antagonism Eetween this method and those based on current physico-chemical doctrines. The main points to be noted about the values of the degree of complexity given by Holmes are that (1) they appear to vary from substance to substance by the factor 2, being 1, 2, 4, 8, or 16; (2) they are represented by integral numbers ; (3) the substances which all other methods demonstrate to be normal are often the most associated of all.Now the occurrence of whole numbers as association factors must have a definite meaning. In a gas the molecules of which are capable of association there is at any temperature a condition of equilibrium between two sets, the more and the less complex molecules, this equilibrium being readjusted at each alteration of temperature. With sulphur vapour, according to the conditions of temperature and pressure, molecules S,, S,, S,, and S, exist, three forms often ceexisting (Preuner and Schupp, Zeitsclr . physikal. Chem., 1909, 68, 129).There is no a priori reason to suppose that in the liquid state an associated substance can have but one degree of complexity independent of temperature ;indeed, it would be surprising if the general effect of temperature and pressure wsls entirely different for different states of matter. The case of nitrogen peroxide may be quoted against such a possibility; for as liquid nitrogen peroxide becomes coloured with rise of tem- perature, it must of necessity indicate that a different molecule is being produced, almost certainly NO,, since the substance of this formula has a brown colour in the state of vapour; thus, without any assumption either as to the distribution of kinetic energy added to a substance, or of the actual molecular complexity, the behaviour of nitrogen peroxide clearly shows that the degree of 31 aggregation of a liquid is certainly affected by temperature varia- tion.If Holmes’ theory is correct, however, then it is most improb- able that temperature has such an effect. Holmes himself admits this (T., 1913, 103,2164), for if the degree of complexity can be represented as a whole number in every one of the twenty-seven examples given, then it is highly improbable that either of the constituenk of a liquid can have present within it molecules of two or more degrees of complexity, such as one must presume to exist on the consideration of the non-integral values derived by the Ramsay and Shields’ method and its numerous modifications, or Traube’s or Guye’s or any other method depending on the study of properties very varied in character; and the improbability is all the greater when it is remembered that Holmes’ numbers are derived from measurements made at purely arbitrary temperatures at which the liquids are far from being at corresponding states.Again, the degree of complexity deduced by the method appears to be independent of the nature of the second component of the mixture, for the value arrived at is the same; for example, when ethyl alcohol is mixed with water, or with ethyl ether, methyl iodide, or carbon disulphide, results wholly at variance from those obtained by freezing-point and boiling-point measurements, which indicate that the nature of the solvent is a powerful factor in modifying molecular state (compare Auwers, Zeitsch.physikaE. Chem., 1899, 30, 300; Meldrum and Turner, T., 1908, 93,876; 1910, 97,1605; Turner, ibid., 1911, 99,880). The third point mentioned above is equally important. Against the probability that n-hexane, benzene, and carbon disulphide are associated in the way Holmes believes, there is much evidence from a consideration of several properties. It would, for example, not be easy to reconcile the great complexity of (C&JI6, of molecular weight 1216, with a boiling point as low as 46O. There are, how- ever, more fundamental objections. Consider the substances ethyl ether, ethyl acetate, benzene, n-hexane, chloroform, and carbon disulphide, all of which Holmes considers so complex.In the state of vapour they each occupy a volume corresponding with the simplest possible molecular formula, and if, therefore, any altera- tion of complexity occurs, it must be presumed to take place when the vapour condenses. If, therefore, the temperature of the mixture of liquid and vapour be raised towards the critical point, either the molecular complexity of the liquid must decrease (which on Holmes’ view is improbable, as shown above) or that of the vapour must increase, since liquid and vapour become identical at the critical point. Now when vapour and liquid are of different degrees of complexity, it has been found (Young, Phil. Mag., 1892, [v], 34, 503; Young and Thomas, T., 1893, 63, 1191; Young, “ Stoichiometry,” Longmans, 1908 ; compare Ramsay, Yroc.Roy. Soc., 1894, 56, 171) that the various critical relationships are abnormal. Water, the alcohols and acetic acid, all of which Holmes agrees a;e associated, are’ abnormal ;but benzene, n-hexane, ether, ethyl acetate, and alkyl iodides are not, and one may conclude that the complexity of the liquid and vapour undergoes little or no change. Similarly, it is possible from the value of the surface tension of a liquid at the ordinary temperature (Ramsay and Shields, T., 1893, 63, 1089) or from the viscosity (Batschinski, Zeitsc?b. physikul. Clhem., 1911, 75,665) to calculate with a fair degree of accuracy the critical temperatures of benzene, ether, ethyl iodide, ethyl acetate, and carbon disulphide, whereas with the unquedionably associated substances this is quite an impossible matter.In conclusion, it may be pointed out that Holmes’ results are deduced from solutions, and not from the pure liquid itself, in which case, despite the strength of solution used, there should be at least some measure of comparison between his results and those derived from methods based on osmotic-pressure determination. Actually, results of an opposite character are found, hydrocarbons and their halogen derivatives, ethyl acetate, carbon disulphide, etc., to which Holmes assigns a high degree of complexity, being quite unassociated by freezing-point and similar tests. It theref ore follows from what has been said, that if Holmes’ method is correct, temperature has no’ effect on the degree of complexity of a liquid; and present interpretations of critical data, as also van’t Hoff’s laws of solution, are untenable.If, on the other hand, they are correct, H~lme~’ deductions cannot be. In the author’s opinion, Holmes’ numbers cannot represent the molecular complexities of liquids, either actual or relative. 38. ‘(Phytin and phytic acid.” By George Clarke. A detailed description of work of which a preliminary account has already appeared (P., 1913, 29, 27). 39. ‘‘ Sulphonyl and carbonyl derivatives of alanine. Resolution of externally compensated p-toluenesulphonylalanine into its optically active components.” (Preliminary note.) By Charles Stanley Gibson. In continuation of the work of Pope and Gibson (T.,1912, 101, 939), a comprehensive stereochemical study of derivatives of aIanine and other amino-acids is being undertaken.The met.hod of preparation of externally-compensated ptoluene- 33 sulphonylalanine has been conveniently modified, and the com-pound has been resolved into its optically active components by the method of Pope and Gibson (Zoc. tit.). One equivalent of p-toluenesulphonylalanine was treated in boiling aqueous solution with half an equivalent each of strychnine and sodium hydroxide, and after allowing the clear solution to remain, an almost theoretical quantity of the strychnine salt of d-p-toluenesulphonylalanine separated. This was recrystallised from very dilute alcohol, and obtained in clusters of colourless needles, melting at 188--189O.The acid remaining in the mother liquor from the separation of the strychnine salt was then isolated, and treated with the corresponding quantities of brucine and sodium hydroxide in boiling water. After some time a good quantity of the brucine salt of I-ptoluenesulphonylalaninesepar-ated. This was recrystallised from a large quantity of boiling water, and obtained in long, colourless prisms, melting at 148-1 49 d-p-2’01uenesulp?~oriylalair/ie, CH,*CH(C0,H) NH SO,*C,H,*CH,, was obtained in the usual manner from the strychnine salt, and after one recrystallisation from aqueous alcohol it was found to be pure, and separated in long, colourless needles, melting at 131-132O.Its rotation was determined in alcoholic solution at 25O: 0.5894, made up to 25 C.C. and observed in a 2-dcm. tube, gave a, +0.37O, [a], +7.7l0. In a similar way l-p-toluenesulp?~onylalanirzewas isolated from the brucine salt, and this was obtained pure after two recrystallisa- tions from aqueous alcohol. It separated in well-defined, colourless crystals, melting at 131-132O. The melting point of the racemic compound is 138-139O (Zoc. cit.). The rotation of the lmo-com- pound was determined under the Bame conditions as the above: 0.5472 gave a, -0’35O, [a], -7.62O. The completion of this and other investigations is being delayed so that the final observations may be made under better and more accurate conditions. 40. The ‘azeotropic’ mixtures of ethyl acetate and water.” By Robert Tabor Lattey.Although its derivation signifies ‘‘unchanged by boiling,” Wade defined an azeotropic mixture as one of maximum (or minimum) boiling point. The mixtures of ethyl acetate and water described by Merriman (T.?1913, 103, 1798) do not strictly fall under this 34 definition. The points representing their composition and pressure on a P/x diagram are three-two for liquid phases and one for vapour phase. None of these is a maximum point; that represent- ing the vapour phase is the intersection of two curves. This was pointed out in the case of triethylamine and water, where similar conditions prevail (T., 1907, 91,1959). It is not possible to construct the complete P/y curve (y =molecular fraction of water in vapour) from Merriman's data, but its correct form at 37.55O is shown in the accompanying figure.The right-hand branch cannot have the form assigned to it by Merriman, since %=yP by defini- mm 20( 16( x=o x=1 y=O y=l Vapour presstires of ethyl ncctate and utnter at 37'55". tiori and p2 is very nearly constant for the water-vapour in contact with its solutions in ethyl acetate at each of the temperatures investigated. For a true bzeotrope, ?=O. In the cme of ethyl acetate and d9 wdter, dy has two values for the vapour in contact with mutually dY saturated solutions. At 37~55~these are given by the two values of -namely, 0.231 -0.269 and 0.231 -0.986 = 70+Y-SP,Y(1 -?/! 0.231 x 0.769 0.231 x 0-769 -850,using Merriman's data.There is a hypothetical azeotrope in this case having the, composi- tion x=y =0.25 (approximately). This cannot be realised, since the liquid separates into two layers. The horizontal line in the figure indicates the composition at A and B of the saturated liquid phases, and at C of Merriman’s so-called ‘‘ azeotrope.” Liquid and vapour cannot co-exist under conditions indicated by points above the line ACB. For, suppose a solution were prepared having x> that corresponding with the point A, for example, x=O*18, the vapour corresponding with this liquid would have a composition between y=0*23 and y=0*25, and exert a pressure of about 205 mm. Such a vapour is saturated at about 194 mm., and would, theref ore, undergo partial condensation. Distillation would therefore go on until two liquids, A and B, had formed.The second (hypolhetical) maximum at about x=0’85 does not indicate an azeotrope. It is true that gp and clx’ are all *2 dl; dP dc shall also be zero, and dc zero. It is, however, not necessary that -hence y=x . does not change signs here, since both dP and dydY change signs. If the following forms of the equation deduced by Duhem, Margules, and Lehfeldt are examined : it is seen that (i) if y=x the total and partial pressure curves all have maxima or minima, that is, an azeotrope is formed; (ii) it dPdoes not follow that because cf=O, either -=O or y=x.dx On page 1799 (Zoc. cit.) Marshall’s equation has been misinter- preted: II: represents the composition of the liquid.As Merriman poinix out, x has two values (corresponding with the two layers) in the case considered, and neither of these is the same its y for the vapour. Marshall’s equation is another way of writing y=x dPwhen -=0, and since, as has been shown above, this condition is dY not fulfilled, the equation is not applicable. The calculation carried out by Merriman is simply an application of Dalton’s law of partial pressures. 41. 4L Direct combination of nitrous acid with primary, secondary, and tertiary amines.” By Paiichaiian Neogi. Ha\-ing isolated the nitrites of the primary, secondary, and tertiary amines from mixtures of their hydrochlorides and alkali 36 nitrites (Neogi, :I?., 1911, 27, 242; T.,1912, 101, 1610; Gizem.News, 1913, 108, 53, 62), the author advanced the theory that an amine nitrate is formed as an intermediate compound in the inter- action of nitrous acid and the aniines (excepting purely aromatic aminos). In continuation of the same subject, the direct action of free nitrous acid and free amine at a low temperature has been studied. It has been found that with suitable precautions pure amine nitrites are obtained by the combination of ice-cold solutions of free nitrous acid with the amines. In this way, ammonium, methylammonium, diethylammonium, trimethylammonium, benzyl- ammonium, and piperidinium nitrites have been obtained. 42. ''The mechanism of nitrification." (Preliminary note.) By Ernest Moore Mumford.Investigation wae directed to the bacterial oxidation of aqueous solutions of ammonium salts on suitably inoculated experimental filters with a view to identify intermediate products of oxidation and determine the internal mechanism of the change. The filters were inoculated from actively nitrifying sewage filters, the organisin being checked by the customary methods. As a resuIt of the work, it ha been found that the oxidation proceeds in a series of stages compatible with the hypothesis that bacterial oxidation is attained by successive hydroxylation of hydrogen atoms, and subsequent elimination of water. Intermediate compounds were identified in hydroxylamine salts and salts of hyponitrous and nitrous acids, and it waa found that the loss of nitrogen, which invariably takes place to a certain extent on such filters, is due in part to complex interactions between these various intermediate compounds ;and, a8 the relative concen- tration of these compounds is det'ermined by the degree of aeration of the filter, this hypothesis is in correlation with the observed difference in the loss of nitrogen between a percolating filter and a contact bed.The hydroxylamine was identified by the sodium nitroprusside reaction, and estimated by titration with iodine solution in presence of sodium hydrogen carbonate, and the hyponitrous acid was detected by the formation of the insoluble silver salt; the nitrous and nitric acids were determined by the customary methods employed in wafer analysis.37 43. (( U-and P-Trimethyl cobalticyanide.” By Emald George Justinian Hartley. Silver cobalticyanide and methyl iodide react at a temperature of about 45O to form silver iodide and two isomeric trimethyl cobalticyanides, together with some decomposition products. The two isomerides differ both in physical and chemical properties. One of them, which it is proposed to call the a-compound, is less soluble than its isomeride in water and the lower alcohols. It crystallises from hot water in very fine, hair-like fibres somewhat resembling glass-woo!. It forms double salts with silver cobalticyanide and with silver nitrate. The P-variety crystallises in minute needles from any of the above solvents.It also forms double salts with silver cobalti-cyanide and silver nitrate respectively, but of different composition from the corresponding a-compounds. 44. ‘(The preparation of dithiobenzoic acid.” By (jierald Noel White. The following simple method of preparing dithiobenzoic acid, C,H,*CS,H, directly from benzaldehyde in one operation has been found to give satisfactory results. A solution of 18 grams of benzaldehyde in 300 C.C. of alcohol and 150 C.C. of ammonia (D 0.880) is mixed with powdered sulphur (10 grams), and the mixture then saturated with hydrogen sulphide, first at the ordinary temperature, and finally, with frequent shaking, on the water-bath. The treatment with hydrogen sulphide is continued until all the sulphur has dissolved, and on dilution of a sample kith water, no appreciable precipitate of benzaldehyde is obtained.The deep red liquid, after being diluted and shaken with benzene to remove a small quantity of unchanged aldehyde, is acidified with hydrochloric acid. The precipitate is collected and washed with ether, which is also employed to extract the dithiobenzoic acid from the acidified liquid. The substance is readily obtained as a purple oil by treating the concentrated ethereal solution with methyl alcohol. 38 45. ''Condensation of ethyl a-chloroacetoacetate with phenols." By Biman Bihari Dey. On condensing a-naphthol with ethyl a-chloroacetoacetate under suitable conditions in the presence of concentrated sulphuric acid at Oo, 3-chloro-4-methyl-1:2-a-naphthalryrone, co I I I \/\/is obtained in 70-75 per cent.yield. It crystallises from glacial acetic acid in clusters of hard, colourless needles, melting at 227O. On boiling it for several hours with excess of 30 per cent. alcoholic potassium hydroxide, crystals of the sodium salt of a-naphtha-coumarilic acid slowly separate out, which, on acidification, is converted info the free 2-methyl-a-naphthafuran-1-carboxylicacid, prepared by Hantzsch and Pfeiffer (Ber., 1886, 19,1303). It melts at 248O, about 6O higher than that given by Hantzsch and Pfeiffer. ni-Cresol condenses with ethyl chloroacetoacetate to give an almost quantitative yield of 3 -chloro -4 :7 -dimethylcoumarin, C,,H,O,Cl, crystallising from alcohol in long needles melting at 135O.On boiling with alcoholic potassium hydroxide, it is con-verted into 2 :5-dimethylcoumarilic acid, melting at 218O; Fries and Fickewirth (Annalen, 1908, 362, 51), who obtained it from the product of bromination of 4 :7-dimethylcoumarin, gave 212O as the melting point. p-Cresol under similar conditions forms 3-chloro-4 :6-dimethyl-coumarin, crystallising from acetic acid in colourless needles melting at 160O; boiling alcoholic potassium hydroxide converts it into 2 :4-dimethylcoumarilic acid, prepared by Hantzsch and Lang (Ber., 1886, 19, 1299). o-4-Xylenol under the same treatment gives an 80 per cent. yield of 3-chloro-4 :6 :7-trimeth ylcoumarz'n, C,,H,,O,Cl, crystallising from alcohol in needles melting at 170O.It is converted by alcoholic potassium' hydroxide into 2 :4:5-trimethylcoumclri'lic acid, C12H1203, crystallising from ethyl acetate in colourless needles melting at 249O. On distilling the acid with excws of dry lime, the corre-sponding trintethylcoumarone, C1,H120, passes over as an oil, which solidifies on cooling in ice; it crystallises from acetone in snowy flakes melting at 39--40°. Phloroglucinol gives a good yield of 3-chloro-5:7-dihydroxy-4-met hylcoumarin, C,,H70,C1, crystallising in yellow needles melting 39 at 308”. The dirnethyi! ether, C,,H,,O,Cl, forms aggregates of short needles melting at 170° ;the diacetyl derivative, C,4H,,0,Cl, forms needles melting at 154O, and the dibenaoyl derivative, C2,H,,06Cl, crystallisw in rhombic plates melting at 186O.Hydroxyquinol gives a rather poor yield of 3-chZoro-6 :7-di-hydrozy-4-methylcoumarin, C1,E,0,Cl, crystallising in nearly colourless needles, and melting at 259-260O. The diacetyl (C,,H,,O,Cl) and the dibe~uoyl(C2,Hl,0,C1) derivatives melt at 172O and 192O respectively. 46. The action of phosphoric oxide on dibenzylmalonic acid.” By Hubert Cyril Cutts. As 1-hydrindone may be prepared by the intramolecular con-densation of phenylpropionyl chloride (Kipping T., 1894, 65,480), it seemed probable that dibenzylmalonic acid might be converted CHinto a compound of ths constitution C,B4<CO~C<Co~C,H,.CH Attempts to bring about this change by means of phosphoric oxide redted in the isolation of two products, melting at 145O and 78O respectively.The investigation of these compounds and of their derivatives was jilst on the point of completion (last July) when further experiments were rendered superfluous by the publication of a paper by Leuchs, Wutke. and Gieseler (Ber., 1913, 46, 2200). The results of these investigators, who, however, employed thionyl chloride, and the facts established by the author, showed that the compound melting at 145O was the 0-dibenzylacetyl derivative of l-hydroxy-2-benzylindene, and the compound melting at 78O, di-benzylacetic anhydride. 47. (‘The relation between the absorption spectra of acids and their salts. Part 11.” By Robert Wright. The examination of a number of acids and salts, with reference to their light absorbing power, seems to point to the following con- clusions: (1) The absorption spectra of strong acids are identical with those of their sodium salts; (2) Moderately strong acids, such as acetic, etc., are more absorbent than their sodium salts, but the difference between the spectrum of an acid and its salt diminishes with the weaker homologues; (3) Very feeble acids, such as hydr- ogen sulphide or arsenious acid, are less absorptive than their salts.The generalisations given do not, of course, apply to those cases, where the acid and salt are of different structure. 40 ADDITIONS TO TRE LIBRARY. I. Donations. Bayliss, ViZZiam Maddock. The nature of enzyme action.3rd edition. London 1914. pp. vi + 180. 5s. net. (Recd. 8/1/14.) From the Publishers : Messrs. Longmans, Green and Co. GCerber, Armand. Zur Kenntniss des Orthotolidins. Basel 1889. pp. 76. (R9fwenc.r.) From Geh. Rat Prof. Otto N. Witt. Loeb, Morris. The scientific work of Morris Loeb. Edited by Theodore W. Richards. Cambridge 1913. pp. xxiii + 349. ill. $2 net. (Recd. 27/1/14.) From the Publishers : Harvard University Press. Smiles, Samuel. Chemische Konsti tution und physikalische Eigeoschafteo. Translated by P. Krassa and edited by R.0. Herzog. Leipzig 1914. pp. xiif676. M. 21.-. (Recd. 2/2/14.) From the Author. 11. By Purchas~. Abderhalden, Emi2. [Editor.J Biocbemisches Handlexikor . Vol. VIII. Berlin 1914. pp. 507. M. 36.50.-. (Red 11/1/14.) Allen, Ayred Henry.Commercial organic analysis. Kol. VIII. 4th edition. Edited by W. A. Davis and Samuel S. Sadtler. London 1914. pp. x + 696. ill. 218. net,. (Recd. 2/2/14.) Kauffmann, Hugo. Die Valenzlehre. Stuttgart 1911. pp. ix + 558. M. 15.-. (Recd. 23/1/14.) Wiley, Harvey Wmhington. Principles and practice of agricultural analysis. Vol. 111. Agricultural products. 2nd edition. Easton, Pa., 1914. pp. xv +846. ill. 26s. net. (Recd. 5/2/14.) 41 At the next Ordinary Scientific Meeting on Thursday, February 19th,1914, at 8.30 p.m., there will be a ballot for the election of Fellows, and the following papers will be communicated : “ Condensations of cyanohydrins. Part 11. The condensation of chloralcyanohydrin with chloral hydrate and with bromal hydrate.” By H.L. Crowther, H. McCombie, and T. H. Reade. “ The system : ethyl ether-water-potaasium iodidemercuric iodide. Part 11. Saturated solutions in the four-component system.” By A. C. Dunningham. “The connexion between the dielectric constant and the solvent power of a liquid.” By W. E. S. Turner and C. C. Bissett. “ The viscosities of some binary liquid mixtures containing formamide.” By E. W. Merry and W. E. S. Turner. ERRATUM. PROCEEDINUS, 1914. Page 6, line 1, for “ Part XXI.”?and “ Part XXII.” 42 CERTIFlCATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N,B.-The names of those who sign from ‘(General Knowledge ” are printed in italics. The following Candidates have been proposed for election.A ballot will be held on Thursday, February 19th, 1914. Blair, Ethelbert William, 70,Fountayne Road, Stoke Newington, N. Student. B.Sc. London (2nd Class Hons. Chemistry). Neil Arnott Scholar in Chemistry, 1913. Intend following Chemistry as a profession. J. T. Hewitt. Arthur E. Pitt. Clarence Smith. R. W. Merriman. Frank G. Pope. A. D. BXitchell. Calvert, Albert Frederick,‘‘ Royston,” Eton Avenue, N.W. Author of Technical and Statistical books relating to Mining and Chemical Industries. Engaged on new books dealing with “The Chemistry of Salt ” and ‘‘The Manufacture of Salt,” and am anxious to keep up to date in the latest developments of Chemical Research. Kenneth S. Low. E. 0. Courtman. W. H. Merrett.V.Gowland. J. c. Philip. Clifford, Sydney George, 3, Norman Villas, East Dulmich, S.E. Analytical Chemist. Certificate Dept. of Chemistry, Finsbury Technical College. For it period Junior Assistant to Professor Meldola, and now Chemist with hfesers. Waterlow and Sons, Ltd. Raphael Meldola. R. H. Buttle. Arthur J. Hale. C. Melville Clark. Reginald F. Eastoa. Dhs, Behari L&I, 107/2/1, Manaharpukur Road, Kalighah, Calcutta. Vaccination Inspector, Health Dept.., Calcutta Corporation. Passed the final examination of the Campbell Medical School, Calcutta ;then Iwas Student for 3 years in Chemistry. Late Resident Medical Officer, Government Emigration Agency and Burmah Military Police. Reason is to improve in science. B. B.Dutta. Dhirendransth Mitra. M. Sinha. Kunjo Behary Seal. J. Chakrabwty. Davenport, Sydney Edward, Fernbank;” York Road, Windsor. Analytical Chemist, For three years articled to Mr. Leo Taylor, F.T.C., Public Analyst for the Metropolitan Borough of Hackney. At present chief assistant at Ms. Taylor’s Lzboratories, 31 Moorgate Street. Percy Edgerton. R. P. Hodges. B. C. Smith. Charles A. Keane. G. Francis Morrell. Davidson, Thomas Alexander, 57, Strathyre Avenue, Norbury, London, S.W. Works Manager. Analptical and Research Chemist ; Speciality : Shellac, Drying Oils and Varnishes. Lecturer on ‘(Painters’ Oils, Colours and Varnishes ” at Regent St. Polytechnic. Original work published: ‘‘Action of Driers on Linseed Oil,” Proc. Paint and Famish Society, Nov., 1908 ;Feb., 1909 ;June, 1910.Frank E.Weston. J. Cruickshank Smith, William Hy. Collier. Walter F. Reid. H. hCtanZey Xedgrove. Davies, Thomas Eynon. 25, Trevor Street, Aberdare, Glam. Assistant Master, and Lecturer in Mining Chemistry. B.Sc., Hons. in Chemistry ;Post Graduate Diploma in Metallurgy, Univ. of Wales; Ten years’ experience as Science Master ;Lecturer in Mining Chemistry, Glam. Clounty Council. At present engaged in work upon the “Detection and Estimation of Mine Gases,” and desire to avail myself of the facilities offered by the Society to carry out this work. Claude M. Thompson, William G. Tonner. E. P. Perman. T. Campbell James. A. A. Read. B. Perrott. Denington,Richard Charles. 69, Dover Road, S.Wanstead, Essex. Research Chemist to Messrs. Bastol, Ltd. Trained, East London 44 Technical College and Royal College of Science. Research Assistant to A. R. Ling, Esq.; Works Chemist, Messrs. A. Boake Roberts; Research Chemist, British Alcohol Syndicate and Bastol, Ltd. J. T. Hewitt. Arthur R.. Ling. Frank G. Pope. Lewis Eynon. E. W. Brown. Fernie, Charles George. I‘ Holmleigh,” Northwood, Middlesex. Science Tutor, B.Sc. (London University), Engaged in advanced work preparatory for proposed research work at the Imperial College of Science. H. B. Baker. J. W. Hinchley. James C. Philip. C. E. Sladden. A. 5”. King. Finch, George Ingle, 41, Ladbroke Road, W. Demonstrator in the Department of Chemical Technology, Imperial College of Science and Technology, South Kensington.Obtained the Diploma of the Swiss Federal Polytechnic in March, 1911. April, 1911, to Oct., 1911, Assistant Lecturer in Electro-and Physical Chemistry, and from Oct., 1911, to March, 1912, Assistant in Technical Chemical Analysis and Chemistry at the Swiss Federal Polytechnic, March to September, 1912, studied at the University of Geneva. November, 1912, to Jan. (inclusive), 1913, as Assistant Chemist in the Research Depnrtment, Roynl Arsenal, Woolwich. 1have occupied the present post since Feb., 191 3. I have published four papers, viz. : three in the Zeitsc?hrift fiir das ges. Schiess- und Sprengstofwesen, May, 1910; April, 1912 ;August, 1912. In the Chemikeer Zeitung, 1912, page 782.William A Bone. P. W. Robertson. H. Brereton Baker. Arthur A. Eldridge. James C. Pbilip. A. T. King. H. V. A. Briscoe. Furness, Reginald, 90, Woodlands Road, Ansdell, Lyt ham, Lance. Research Chemist to Hydrogenators, Ltd. B.Sc. Victoria, 191 2. Mercer Scholar ; Leblanc Medallist ; Schunck Research Assistant ; M.S. (Vict.) 1913. 1912-1914, Private Research Assistant to Prof. W. H. Perkin, F.R.S., in the Universities of Manchester and Oxford. Joint author of papers (in the course of writing, to be 45 published in the J.C.X.) with Prof. A. Lapworth and Prof. W. H. Perkin and others. Harold B. Dixon. W. H. Perkin. Arthur Lapworth. B. Lambert. F. R. Lankshear. A. F. Walden. Uarth, John, 170, St. Thomas’s Road, Preston.Physician. Medical Officer of Health, Analyst, and Bacteriologist for Fulwood. Former Student of Dr. Muter, Publi; Analyst, South London. Former Student of Dr. Campbell Brown, Public Analyst for Lancashire. Former Student of Professor DelBpine, Bacterio-logist, Victoria University. John Hargreaves. John W. Towers. William Naylor. Charles Dreyfics. James Hargreaves. G. Fitx-Brown. B’rnncis Henry ?’ate. Gibbs, Ivan Riohard, University Hall, 3 Moor’s Gardens, Chelsea. Assistant Demonstrator, Imperial College of Science and Technology. B. A. Oxford, 2nd Class Honours Chemistry. H. B. Baker. James C. Philip. B. Mouat Jones. A. T. King. P. W. Robertson. Hale, James Stanley, Principe 4, Bilbao, Spain. Analytical Chemist. Studied chemistry at the Central Technical School, Liverpool, and was assistant to G.Watson Gray, Esq., F.I.C., of Liverpool, for over ten years. G. Watson Gray. James Smith. W. H. Pearson. C. Durham Garbutt. John Hanley. Harper, Theophilus, 39, Camden St., Belfast. Pharmaceutical Chemist,. Lecturer on Pharmacy, Materia Medica, and Botany, Municipal Technical Institute, Belfast. Member of the Pharmaceutical Societies of Great Britain and Ireland ;Member of the British Pharmaceutical Conference ;formerly Demonstrator of Chem- istry, School of Applied Chemistry, Belfast, and Lecturer on General 46 and Pharm. Chemistry, Schools of Science and Technology, Belfast, and Municipal Technical Institute, Belfast. Henry Wren. A. JV. Stewart.John Hawthorne. A. K. Macbeth. Ellis Clayton. C. R. Crymble. Thomas Maben. R.Gilmoui-, John C. Umney. A. Percy Hoskins. C. T.Bennett. Harrap, Eric Russell, Maisemore, Ebury Road, Rickmans wor th, Her ts. Works Chemist. Two years Assistant to George T. Holloway Esq., Consulting Chemist, etc. (Sept., 1908, to Oct., 1910). Three years Works Chemist to Messrs. Bells United Asbestos Co., Ltd. (Oct., 1910, to Oct., 1913). George T. Holloway. Charles A. Keane. William G. Wagner. H. Burrows. J. G. Baxter. Horwood, Oswald Ryle (Clerk in Holy Orders), Tunstall Rectory, Suffolk. Physician and Surgeon. M.A,, 2nd Class Science, Corpus Christi College, Cantab. ;M.R.O.S., England ; L.R.C.P., London. Anderson Prizeman, London Hospital.Chief Master, Keswick Laboratory (Chemical, 1905--1906). 1907-1910, sent out by Board of Education tobuild Simla Chemical Laboratory. Manufactured reagents, chemicals, etc., for this laboratory, as we found it better to manufacture our own on the spot-we acquired the necessary apparatus. 1910-19 12, studied Physiological Organic Chemistry (with a view to medicine and surgery). W. G. Gledhill. Harold Rogerson. Herbert Marsden. Chc~s.W. Moore. E. Herbert Fison. Prank Tutin. Iyer, Manappadam Rrtmaswami Viswanatha, 50, Prem Chand Bural Street, Bow-Bazar, Calcutta. Assistant Chemist, Indian Tea Association, Indian Museum, Calcutta. Formerly a student of Technical Chemistry in the Victoria Jubilee Technical Institute, Bombay, for three years.At present an Afisistant Chemist in the Scientific Department of the Indian Tea Association. P. H. Carpenter. Kali Prosonuo Rai. David Hooper. Dhirendranath Mitra. Tin Kc6ri Ghose. 47 James, Dan Ivor ,‘(Frondeg,” Llandilo, S. Wales. 13.S~. (Wales), Hons. in Chemistry; M.A. Cmtab., 1st Class Nat. Sci. Tripos, Parts I. and 11.(Chemistry); Late Lecturer in Chemistry, School of Mines and Technology, Johannesburg ; Joint Author, “Racemisation of a-Hydroxy-acids,” J.C.S:, 1912 ; ‘‘Action of Alkalis on Phenolphthalein,” Journ. Chern. itfin.and Met. Soc., S.A., 1912. W. J. Sell. F. W. Dootson. H. J. H. Fenton. J. G. M. Dunlop. W. J. Pope. Kolhatker, Gopal Balkrishn, Ferguson College, Poons, India. Professor of Chemistry, Ferguson College. M.A.(with Honours) of the Bombay University. A research student in the Indian Institute of Science, Bangalore. At present engaged in determining velocity of alcoholysis with different catalysers by physico-chemical methods. M. W. Travers. H. E. Watson. J. J. Sudborough. N. S. Rudolf. D. D. Kanga, Leigh, Alfred John, Duff House, Banff, N.B. Analytical Chemist, at Duff House Sanatorium, Banff. Associate of Royal College of Science, South Kensington (student from 1909-1913). Graduate of London University (B.Sc., 1st Class Hons. Chemistry, 191 2-Internal). Henry F. Harwood. H. B. Baker. Chapman Jones. James C. Philip, M. 0. Forster. Leighton, Frederic William, Lydiard Tregoze, Wootton Bassett, Wilts. Mining Engineer and Metallurgist.Certificate of Manchester University in Applied Chemistry. Diploma of the School of Technology, Manchester. Associate of the School of Technology (Metallurgy). E. L. Rhead. F. S. Sinnatt. E. Knecht. Jas. Grant. 8.J. Peachey. Makin, Fredk.Arthur,‘‘The Nest,” Taunton Road, Ashton-under-Lyne. ManageI* and Chemist. Engaged as Manager and Chemist t( 48 Messrs. R. F. Barrett & Go., Soda Water Mfcra, having served with them for 25 years. For the past three years have attended the Technological Chemistry Classes in the School of Technology, Manchester. Passed all examinations during that period, and obtained First Class Honours, City and Guilds. Am desirous of becoming a member so as to keep up to date with chemical progress.Jas. Grant. F. G. Richards. F. S. Sinnatt. 3.L. Mead. S. J. Peachey. E. Kmcht. McLaren, Alexander Williamson, 3, Hayfield Tce., Langside, Glaegow. Analytical Chemist. Assistant to R. R. ‘lhtlock and Thomson, City Analysts of Glasgow for 13 yeam, and Student at Royal Technical College, Glasgow, for eleven years. R. R. Tatlock. Thomas Gray. R. T. Thomson. G. G. Henderson. Harry Dunlop. Macpherson, Archibald, 51, Keir Street, Glasgow. Chemist. 15 years’ practical experience in Manufacturing and Agricultural Chemistry. Being engaged in scientific work with Messrs. Manley & James, Ltd., Manufacturing Chemists, London, J desire to extend my opportunities for keeping in touch with advancements in scientific chemical science, and to enjoy the privilege of attending the meetings of the Chemical Society, also to receive the Journal. F.W. Crossley-Holland. G. Mason Williams. Carter White. J. Stuart Lawson. John Wm. Patterson. Morris, Thorn-, 53, Poolstock, Wigan. Brewer and Chemist. Engaged for the past twelve years as Brewer and Chemist to Messrs. Airey’s Brewery, Ltd., Wigan. During the last three years have attended the Technological Chemistry Classes at the School of Technology, Mancheatar. Passed all School and the Honours City and Guilds examinations during that period. Am desirous of becomiag a member so as to keep up with advances in chemical knowledge. Jas. Grant. S. J. Peachey. F. S. Sinnatt. F. G. Richards. If, Knecht. 49 Nichols, Raymond William, Central Experimental Farm, Ottawa, Canada.Assistant for Milling and Baking to the Cerealist of the Dominion of Canada. Assistant in the Scientific Department of Messrs. Guinness’s Brewery, Dublin, for 10 years, including 3 years assistant in the Guinness Research Laboratory. A. J. Banks. J. H. Millar. Thomas B. Case. Horace T. Brown. Adrian J. Browra, Odlum, William Julian, Ardmore, Bray, Go. Wicklow. Flour Milling Chemist. B. A,, Trinity College, Dublin. Interested in all Analysis Work and especially that connected with Flour Milling. Studied at Aynsome Technical Laboratories. J. Stewart Remington. Sydney Young. C. Smith. Wm. C. Ramsden. Emil A. Werner, Oldroyd, Rowland Ernest, 90, Park Road, Rochdale.Chemist (Works). At present Chemist to Measrs. John Bright & Bros. ;at present Member of the Committee for the Standardisation of Indigo (Cotton and Wool), Textile Institute. Late Lecturer in DyeiDg at Halifax Technical College. Clothworkers’ Scholar and Chemistry Prizetuan, Yorkshire College. C. A. Crook. E. W. Smith. W. J. Stanafield. J. H. Dyson. Reginald B. Brown. Pickworth, Frederick Alfred, 70, Highfield Road, Dartford. Pharmaceutical and Analytical Chemist. Assistant Analyst to Messrs. Burroughs Wellcome & Co., Dartford. Major Examination of Pharmaceutical Society. Intermediate B.Sc., Ronours in Chemistry (Lond.). H. A. D. Jowett. Harold King. Frederic H. Lees. W. P. Hayworth. Frank Lee Pyman. Francis IT. Carr.Pick,William Henry, 141, Mare Street Hackney, London, N.E. Science Master, Queen Mary’s School, Basingstoke, Hampshire. 50 B.Sc. (London), 191I. G radliated from University College, London ; London University Teacher’s Diploma, 1912. Licentiate and Member, College of Preceptors. Samuel Smiles. R. Whytlaw-G-ray. Percy May. J. N. Collie. V.Lefebure. Riley, Cody Hunter, Anchorage, Clay ton-le-Moors, Accring ton. Chemical Manufacturer. Student of Chemistry in the Blackburn Technical School and the University of Mancheater ;member of the firm of James Riley & Co., Chemical Manufacturers, Openshaw, Accrington. Harold B. Dixon. F. Y.Burt. Arthur Lapworth. E. C. Edgar. F. R. Lankshear. Ch. Weizmann. Robson, William Pawson 78, Rolland Street, Cape Town,S.Africa. Chemist. Honours, B.A., Cape of Good Hope University (1910); Assistant Govt. Analyst, Cape Town (191 1) ;Ph.D., Hallo University, Germany (1913) ;Research Student, University College, London, 1913. J. Norman Collie. W. B. Tuck. Samuel Smiles. H, T. Clarke. C. R.Crymble. Roy, Ghandra Bhusan, Moradpore P.O., Bankipore. Demonstrator of Chemistry, Pzttna College. M.A. (Chemistry), Calcutta University ;Demonstrator in Chemistry, Patna College. P. C. RAy. Jyoti Bhushan Bhaduri. K. 8.Caldwell. Hem Ch. D. Guyta. Jatindranath Sen. Smith, Joseph de Carl (Junior), Oak House, Newmarkot Road, Norwich. Student. Bachelor of Science of London Univeraity. Proceeding with the study of Chemistry. Hugh Ramage.Richard Hornby. Walter W. Reed. Frank Clomes. Thos. Tyrer. Stamp, Charles Alfred, Passey’s House, Eltham, Kent. Food and General Analyst, Institute of Hygiene, 34 Devonshire Street, Harley Street, W. 3 Years with Leo Taylor, F.I.C., C.C. Public 51 Analyst for Hackney ; Assistant Analyst, Messrs. Liebig’s & Co., Ltd., Southwark Street, S.E.; First Assistant at Kent County Laboratories, Maidstone (under late Dr. Adams). Frank E. Weston. W, M. Seaber. C. T.Bennett. M. 8. Salamon. B. C. Smith. Stone, Horace Gilbert, 24, High Street, High Wycombe, Bucks. Schoolmaster [Science Master at Spring Gardens School, High Wycombe]. (1) 3 Years’ course of Study at Birkbeck College for the l3.S~.degree of London University ; (2) 2 Years’ course at St..Paul’s Coll., Cheltenham, for Int. B.Sc. under W. Boone, Esq., B.A. B.Sc. F.C.S. ; (3) A Bachelor of Science of Lond. Univ. ; (4) Science Master at the above school. Alex. McKenzie. Geoffrey Martin. G. W. Clougb. Fred Barrow, G. H. Martin. Temple, Harold Edwin, 239, Cashel St., Christchurch, N.Z. Assistant Engineer to the Christchurch Gas, Coal and Coke Co., Ltd. Certificates : Dept. of Education ; Practical and Theoretical Adv. Inorganic and Organic Chemistry ; Honours in Inorganic. Special courses of study in Examination of Foods, Identification of Poisons and Preparation of Dyes, fine Tar products and Alkaloids. In charge of all Analyses and research for the Windsor Street and Adderley Street Works of B’ham Corp.Gas Dept. from 1899-1905 ; also had control of erection and working of Cyanogen Plant ; Assistant Engineer, Windsor Street Works, Feb., 1905-0ct., 1906 ; Nechells Works, Oct., 1906-April, 1910 ; Assistant Engineer, Christchurch, N.Z., May, 19 10;Control of anhydrous ammonia manufacture. Robert English. W. B. Davidson. Harold G. Colman. A. M. Wright. Douglas 3’.Twiss. Turner,Eustace Ebenezer, 5, Queen’s Gate Villas, S. Hackney, N.E. Research Student. Research Student at East London College. B.Sc., London (First Class Honours Chemistry), J. T. Hewitt. R. W. Merriman. Frank G. Pope. A. D. Mitchell. Clarence Smith. 52 Wright, Robert James, c/o R. Burnett Esq., 336, Pollokshaws Road, Glasgow. Assistant Science Master, Hillhead High School, Glasgow.M.A. (Glasgow). Is engaged in teaching Chemistry, and is desirous of keeping in touch with current Chemical literature. G. G. Henderson. I. M. Heilbron. F. J. Wilson. Jas. A. Russell Benderson. Thomas Gvay. The following Certificate has been authorised by the Council for presentation to ballot under Bye-lam 1 (3) : Cohen, Lionel, Stock Dept. Laboratory, Caeino, N.S.W. Analyst, Stock Branch Dept. of Agriculture. Eleven years Assis- tant in the Chemical Laboratory, Dept. of Agriculture, N.S.W. Two years in charge of this laboratory (Casino). Reprints of contributions to scientific work dealing with Chemical matters sent to you 2nd August,, 1913. Loxley Meggit t. RICHARD CLAY AND SONS, LIMITED, BREAD ST. HILL, R.C., AXD BUNQAY, SUFFOLK.
ISSN:0369-8718
DOI:10.1039/PL9143000021
出版商:RSC
年代:1914
数据来源: RSC
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