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Proceedings of the Chemical Society, Vol. 26, Nos. 372 and 373 |
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Proceedings of the Chemical Society, London,
Volume 26,
Issue 372,
1910,
Page 121-160
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摘要:
Issued 10/6/10 PROCEEDINGS OF THE CHEMICAL SOCIETY. VOl. 26. Nos. 372 and 373. Thursday, May 26th, 1910, at 8.30 I)."., Professor HAROLDB. DIXON,M.A., Ph.D., F.R.S., President, in the Chair. Messrs. 0. L. Brady, T. W. Dickson, E. Hinks, W. E. S. Tiirner, and J. Young were formally admitted Fellows of the Society. The President stated that the Council, at their Meeting held that afternoon, had sealed the following respectful Address of Condolence and Congratulation for presentation to his Majesty King George V. He moved that the Fellows of the Society should join with the Council in paying respect to the memory of the late illustrious King Edward VII and in offering homage to his Majesty King George V. This motion was seconded by Mr. C. E.Groves, and carried unanimously, the Fellows present al! standing. TO HIS MOST GRACIOUS MAJESTY KING GEORGE V, MAYIT PLEASE YOUR MAJESTY We, the President, Council and Fellows o€ The Chemical Society, most respectfully beg leave to approach your Majesty with an expression of our deepest sympathy in the great loss which your Majesty and the Empire have sustained in the death of His Most Gracious Majesty our late Sovereign Lord King Edward VII. The Chemical Society will always bear in grateful remembrance the fact that a Royal Charter was granted to us by Queen Victoria, 122 whose illustrious Consort took the deepest interest in the promotion of Science, and specially fostered the growth of Chemical Science in this country by the foundation of the Royal College of Chemistry.We recall with gratitude the Royal welcome accorded last year by your Majesty, and her Majesty Queen Mary, to the Chemists of all Nations assembled in your Capital at the International Congress of Applied Chemistry. We venture to hope that your Majesty’s reign may see discoveries in Chemical Science no less brilliant and contributing no less to the welfare of your people than those which marked the reigns of your August Father and of Queen Victoria. We beg leave to be permitted to offer to your Majesty this expression of our sincere congratulation on your accession to the Throne, and to assure yonr Dliijesty of our loyal devotion and of our earnest wish and prayer. th:it your MajesLy’s reign may be long, happy and benc ficent.Signed on behalf of the Chemical Society, (Signed) HAROLD DIXON, PRESIDENT, ,, ALEXANDER SCOTT, TREASURER, I,. s. ARTHUR W. CROSSLEY, G. T. MORGAN, HONORARY1SECRETARIES, ,, HORACE T. BROWN, (s~~~~~~&. Dated this Twenty-sixth Day of May, One Thousand Nine Hundred and Ten. The Yresident made the following announcements : (1) That owing to the death of his Most Gracious Majesty King Edward VII, the Banquet to Past Presidents had been postponed by the Council from May 26th to November llth, 1910. (2) That,the following Resolution of Council had been communicated to Signor Cannizzaro, son of the late Honorary and Foreign Member, Professor Stanislso Cmnizzaro : The President, Oficers, and Council of the Chemical Society have heard with deep regret of the death of Professor Stanislao Cannizzaro, the senior amotig their distinguished Honorary and Foreign Members.All Chemists look back to the work of Professor Cannizzaro as one of the turning points in the progress of theoretical chemistry ; and the 123 Fellows will ever bear in grateful memory the mastorfiil exposition of his views given to the Society by the Faraday Lecturer of 1872. The Council desire to express to the family of their late colleague the deepest sympathy in their loss. (Signed) HORACET. BROWN, Fomign Secretary May 12th. 1910. (3) That a fund was being collected to found a memorial to the late Professor Richard Abegg, the memorial to take the form of bursaries for students of Chemistry and Metallurgy at the University of Breslau.Subscriptions to the fund would be received by the President or Sir William Ramsay. (4) That the Council had invited Prof. Theodore W. Richards to deliver the Faraday Lecture during the next Session. The invitation had been accepted, and an announcement of the date of the Lecture would be made later. Certificates were read for the first time in favour of Messrs.: Ward Allen Batley, M.Sc., 197, Eccles New Road, Salford. Ronald Leslie Collett, B.A., Little Dawley, Hayes, Middlesex. Charles Frederick Guhlmann, Grantwood, Bergen Co., New Jersey, U.S.A. Lionel Leslie Jacobs, Shelford, Beckenham, Kent. William Ernest Martin, 111,Bellevue Road, Berea, Durban, Natal.Benjamin Mason Narbeth, B.Sc., Durban Technical Institute, Durban, Natal. Robert O'Field Oakley, 54, Sydney Road, Hornsey, N. John Alexander Reddie, 3, Spring Gardens, Bradford, Yorks. Ernest Stedman, B.Sc., 6, Breakwater Road, Bude, Cornwall. Certificates of Candidates have been authorised by the Council for presentation to Ballot under Bye-lam I (3) in favour of Messrs,: Kaikhushroo Bamanji Sorabji, Secunderabad, Deccan, India, John Williams, B.Sc., 122, Liddell Street, Invercargill, New Zealand. 124 Of the following papers, those marked * were read: *128. “The constituents of the leaves of Prunus serbtina.” By Frederick Belding Power and Charles Watson Moore. The material employed, consisting of the air-dried leaves of Prunus serotina, Ehrhart, yielded, on maceration with water, an amount of hydrogen cyanide equivalent to 0.0056 per cent.of its weight. The leaves contain a relatively sinall amount of I-mandelonitrile glucoside, together with an enzyme which hydrolyses /3-glucosides. An alcoholic extract of the leaves, on distillation in a current of steam, yielded a very small amount of an essential oil, but no hydrogen cyanide. The non-volatile constituents of the leaves consisted of a green resin, insoluble in either hot or cold water, and material which remained dissolved in the aqueous liquid. The green resin, amounting to about 5.5 per cent. of the weight of the leaves, yielded hentri-acontane, pentatriacontane, ceryl alcohol, palmitic, stearic, linolic and isolinolenic acids, a little ipuranol, C,,H,,O,(OH),, and a new crystalline substance, C,1H,,0(OH)2,melting at 275-277’, which has been designated prunol.The portion of the alcoholic extract which was soluble in water contained benzoic acid, quercetin, a new glucoside of quercetin, C,,H,,0,,,3H20 (m. p. 245O), which has been designated serotrirt, and I-mandelonitrile glucoside, together with a quantity of sugar and tannin. The aqueous liquid, after heating with dilute sulphuric acid, yielded, furthermore, I-mandelic acid, which had evidently been formed by the hydrolysis of the Z-mandelo- nitrile glucoside. “129. ‘‘The action of potassium chlorate on concentrated sulphuric acid.” (Preliminary note.) By Stanley Smith.The author has observed that at 338’ the action of potassium chlorate on concentrated sulphuric acid is entirely unattended by explosive violence, the addition of the powdered salt to the boiling acid merely resulting in a brisk effervescence, with the production of chlorine, oxygen, and perchloric acid. The volume of oxygen evolved corresponds with about 90 per cent. of the total oxygen contained in the potassium chlorate, whilst the amount of perchloric acid formed appears to be very small. This reaction was studied at various temperatures, and it was found that from 338O to ZOOo no crackling or detonation is produced. At 1709 however, the addition of potassium chlorate to sulphuric acid results in a number of small detonations, which increase in violence as the sulphuric acid is cooled and reach m maximum between 130° and 125 130°,when a sharp explosion results.Below 120' the violence of the action diminishes, until, at 60°,chlorine peroxide is quietly evolved without crackling or detonation. DISCUSSION. SIR WILLIAM suggested that the first action of sulphuricRAMSAY acid on potassium chlorate is the potential formation of chloric anhydride, CI,O,. This decomposes into C1, and 50, and the oxygen is partly used in oxidising chlorine to perchloric acid. The usual equation, therefore, 3KC10, = KC10, + 2C10, + K,O must be indeterminate. The PRESIDENTasked whether Mr. Smith had ever obtaioed pure chlorine peroxide from a chlorate and sulphuric acid, as in his own experience he had always found that oxygen was given off in varying quantity as the change went on, and some free chlorine was liberated."130. Mechanism of tautomeric change."LL By Henry Thomas Tizard. Jn all cases of tautomeric change where one form is more highly ionised than the other (including pseudo-acids and bases, besides substances like ammonium cyanate), the question arises, Ts the change primarily due to the undissociated molecules or to the products of its dissociation ? Both views have found support. Walker and Hambly thought that they had proved that the change of ammonium cyanate into carbamide was brought about by the interaction of the two ions NH, and CNO. Dimroth (Annalsn, 1904,335,l), on the other hand, held that in the case of his trinzole derivatives only the undissociated part changed.Goldschmidt (Zeitsch. EZektrochem., 1905, 11,5) showed that either hypothesis was tenable in all cases, for if the rate of change is proportional to the concentration OF the undissociated part, it is also proportional to the product of the concentrations OF the ions, and vice versa. Thus, if in the change of the ionisable XOH into HXO we find that we also have KGOH = CX*CO€i, and therefore Hence determination of rates of change affords no direct evidence in favour of either hypothesis. Indirect evidence of a kind can be obtained by changing the solvent. For instance, the degree bf dissociation and rate of change of ammonium cyanate in water and in 90 per cent.alcohol have been determined ; from the results it can be shown that if the change is due to the undissociated part, it is about eight times as fast in alcohol as in water ; if to the ions, it is nearly me hundred times as fast. The former seems much more probable, Similar conclusions follow from Dimroth’s work on the rate of change of the triaaoles in various solvents. So, too, instead of changing the solvent, we can substitute a similar tautomeride of a different degree of dissociation. This method has been adopted by Sidgwick and Rivett (Truntt., 1909, 95, 899). This argument, however, is not conclusive, and, indeed, there are many substances which change more rapidly the greater the ionising power of the solvent. It is then usual to assume that the change takes place by the interaction of the ions.Before we accept this view it might be as well to consider rather more closely what it involves. Such a change must take place in three stages : I I6-OH (!I-0 + H’ CO + H’ C=O --L I cbH -C! GH’ CH, I I I I(1.1 (11.1 (111.) Of these, (I)and (111) are strictly ionic reactions, and therefore must be instantaneous. The slow change on which the whole velocity depends must therefore be (IK), that is, the rearrangement of the anion. This must depend only on the concentration of the anion. The tautomeric change must thus be proportional, not to the product of the concentrations of the two ions, but to the concentration of the anion alone. If a mineral acid were added, the concentration of the anion, and therefore the rate of reaction, would diminish.In no single case investigated has this behaviour been found. Addition of hydrochloric acid invariably has an accelerating effect, and this is proportional to the increase in the product of the concentration of the two ions. The only way in which this difficulty can be overcome is by supposing that the second ion has a catalytic effect. The rate of change will then be proportional to the concentration of both ions. This is of course in agreement with facts, but it may well be doubted whether it offers a satisfactory or even a plausible explanation. If in all the reactions examined, the second ion were hydrogen, we might be compelled to admit the possibility of this peculiar catalytic action of one ion on another, but the phenomenon seems to be quite general, and entirely unconfined to one particular ionic species. Pseudo-bases, where the second ion is fiydroxyl, behave exactly like pseudo-acids, and so do even such substances as ammonium cyanate and its analogues, where the second ion is ammonium or a substituted ammonium.127 These considerations seem to show thAt in no case of tautomerism is it probable that the change is brought about directly through the ions, although the rate may of course be influenced by a factor which also influences the ionisation. The changing substance must always be the undissociated molecule. DISCUSSION. Dr. FLURSCHEIMsuggested that the tautomeric ohanges in the triphenylmethyl series might throw some light on the problem.The reactivity of some para-substituents in compounds, such as the tri- phenglmethyl halogenides, necessitated the assumption of a reversible change from the benzonoid to the quinonoid form. If this change occurred in the undissociated molecule, then, hydrogen being more mobile than halogen, tautomeric change of the quinonoid form (I)of unsubstituted triphenylmethyl bromide would produce p-bromo-triphenylmethane. If, however, the change occurred in the ion, then, an electric charge being more mobile than hydrogen, tautomeric change of the quinonoid form (11) would give the original triphenyl- methyl bromide. (1.) (11.) Since the latter alternative corresponded with experimental observ- ation, the taubmeric change, in this case at least, must take place in the ion.Dr. SIDGWICHasked, with reference to Dr. Lnpworth's remarks, how the catalytic effect of bases could be attributed to the formation of salts. The fact that in the case of nitrocamphor the effect of piperidine was so enormously greater than that of alkali seemed to Show that some other factors were concerned. "131. ''A new sulphide of nitrogen." By Frank Playfair Burt. When yellow nitrogen sulphide, N4S4,is sublimed in a vacuum over silver gauze heated to loo', a small quantity of a blue substance is formed, although most of the nitrogen sulphide is deposited un-altered. The blue substance has been shown by analysis to have the same percentage composition as the yellow sulphide.DISCUSSION. The PSESIDENTinquired what was the temperature of the tube at the point where the blue sulphide was first formed, and whether the 128 yield of the new sulphide was increased in the absence of the silver gauze. Mr. BURTstated that the temperature of the tube where the blue sulphide first began to deposit was approximately that of the room. In the absence of silver gauze, no blue sulphide at all was formed. *132. *‘ The molecular complexity, in the liquid state, of amines, nitriles, and amides.” (Preliminary note.) By William Ernest Stephen Turner and Ernest Wyndham Merry. An investigation has beon carried out, based on Ramsay and Shields’s method, of the molecular complexities in the liquid state of thirteen amides and anilides, eleven nitriles and eleven amines.In view of the quickened interest taken in the problem of solution, largely through the investigation, by Walden, of the solvent powers of organic media, including formamide, it was considered desirable to state that formamide exists, as a liquid, in a state of high molecular association. The association is, in fact, greater than in the case of water, and the authors suggest that the solvent action of formamide on salts, so similar to that of water, can be ascribed to the similar molecular complexity of the two substances. All the amides investigated exist in an associated state; of the nitriles, only those of the aliphatic series show association.Primary amines are slightly associated. Substituted amines show a remarkable and interesting behaviour. The value of Rnmsay and Shields’s constant rises both with the number of hydrogen atoms substituted and with the weight of the substituting group. With tribenzylamine, the value of k is 3.50-3.60. “133. Lk A third active principle in ergot extracts.” (Preliminary note.) By George Bnrger and Henry Hallett Dale. In addition to the active principles previously described by the authors as present in ergot and its extracts, namely, ergotoxine (Z’rccns., 1907, 91, 337; Biochem. J., 1907, 2, 286) and p-hydroxy- phenylethylamine (J. Physiol., 1909, 38, lxsvii ;Trans,, 1909, 95, 1 123), there remained for identification the substance responsible for the intense activity exhibited by some ergot extracts in producing contraction of the isolated, non-pregnant uterus of the cat (compare Kehrer, A~ch,exp.Path. Piharm., 1908, 58, 366). As Kehrer found, this action is specially characteristic of Wernich’s Ergotinum dialysatum. The relative abundance of this principle in dialysed extracts suggested that it was wholly or partly produced by micro-organisms, and this supposition was confirmed by physio- 129 logical experiment. It was also found that commercial extracts of meat and of yeast have a similar activity in smalleridegree. Applying Kutscher’s method (Zeitsch. Nahr. Genussm., 1905, 10,528 ; 1906, 11, 582) for separating bases from meat-extract, the authors obtained the active principle from ergotinum dialysatum as a silver compound by adding silver nitrate in excess and then baryta.Tho hydrochloride of the physiologically active base, obtained from this silver precipitate, is readily soluble in cold methyl alcohol, less so in hot ethyl alcohol, and very sparingly so in cold ethyl alcohol. After suitable purification, a minute quantity of a crystalline picrate, melting at 220--230°, and a picrolonate, very sparingly soluble in boiling water and melting at about 250°, were obtained. The base regenerated from either salt had an intense action on the uterus, and gave Pauly’s reaction with p-diazobenzenesulphonic acid. This, together with the conditions under which the base was precipitated by baryta in the presence of silver nitrate, suggested that it was a derivative of histidine.Histidine itself was found to be inactive, but acquired a trace of activity on heating, and became markedly so when exposed to putrefaction. It therefore seemed probsblo that the active base was p-iminazolylethylarnine, produced from histidine EH*NH>CH +CO,C--N’ I6H,-CH(NH,)-CO,H CH,*CH,*NH, by loss of carbon dioxide in the same way that p-hydroxyphenyl- ethylamine in ergot extracts is produced from tyrosine. This provisional identification is supported by the fact that the properties of the hydrochloride, picrate, and picrolonate above described correspond closely with those of the salts of @-iminazolyl-ethylamine synthesised by Windaus and Vogt (Ber., 1907, 40, 360), and quite recently obtained by Ackermann (Zeitscla. physiol.Chem., 1910, 65, 504)by the putrefaction of histidine.* 134. ‘‘ Volumetric estimation of manganese in manganese ores.” By H. V. Krishnayya. The process consists of a combination of two well known methods, namely, the basic acetate separation of iron and the permaupanate titration for manganese. The hydrochloric acid solution containing * Dr. Ackermann’s kindness, which the anthors gratcfull y acknowledge, has since enabled them to complete the identification by direct comparison of the base from ergot with that which he obtained by the pntrefaction of histidine. In the crystalline form of their picratee, and particularly in their action on the uterus, the two bases were found to be identical.130 0.2 gram of the ore is carefully neutralised with sodium carbonate, diluted to 400c.c., and precipitated with 0.5 gram of sodium acetate. The boiling solution, without filtering off the iron precipitate, is then titrated with itr/10-permanganate solution. 135. (6 Indirect estimation of copper.” By Tarak Nath Das. Roth copper and cupric sulphide dissolve in dilute sulphuric acid on boiling with excess of potassium ohlorate. A volumetric estimation of copper based on this reaction (as regards cupric sulphide) was suggested. 136, Synthesis of 6-carboxy-3 :4-dimethoxypheoylglyoxylicacid.” By Victor John Harding and Charles Weizmann. By the condensation of acetyl chloride and homocatechol dimethyl ether, the authors have obtained 4 : 5-dimethoxy-o-me1hyZaceto-phenone (I).On oxidation with warm alkaline potassium per-OMe/\Me OMe/\CO,H OMe OMe!\)COMe OMA\/ICO*CO,H ONe()~$CO,€€ (1.) (11-1 (111.) manganate this ketone gives 6-carboxy- 3 :4-dimethoxyphenylglyoxylic acid (11) (Trans.,1902, 81, 1022). The intermediate oxidation product (111) has also been isolated. When acted on by nitric acid, 4 : 5-dimethoxy-o-methylaceto-phenone gives nitrohomocatechol dimethyl ether, a direct’displacement of the acetyl by the nitro-group occurring : OMe/\Me OMe/\MeOMJ\/Jcol\le -+ OM~~~NO, 137. “Note on the paper of Dr. A. Slator and Dr. H. J. S. Sand on ‘the r61e of diffusion in fermentation by yeast-cells.’ ” ByHorace T. Brown.In the course of the discussion which followed tho reading of the above paper (this vol., p. 85), the author expressed an opinion that provided the gradient of concentration of the sugar at the immediate surface of the yeast-cell is known, and also the amount of sugar fermented by a cell in unit of time, it should be possible to determine the minimal concentration requisite to supply the cell with its require-ments by diffusion only by means of a simple mathematical treatment I31 wbich renders it unnecessary to take into account the particular mode of diffusion within the cell itself. On further oonsideration, and after discussing this point with Dr. Slator, the author has arrivedat the conclusion that such a simplifica-tion of the problem would only be applicable if, at the limiting value of the concentration, the cell functions as a perfect absorber, that is to say, if the transformation of the sugar takes place at its immediate surface, which is almost certainly not the case.Under all other conditions, internal diffusion becomes a factor which has to be taken into account. The authors of the paper are therefore correct in their statement that for the determination of the minimid concentration of a sugar solution which will just supply the cell with its requirements by diffusion only, it is necessary to make certain initial assumptions with regard to the distribution of enzyme within the cell. 138. The resolution of gnoscopine (dl-narcotine)." (Preliminary note.) By William Henry Perkin, jun., and Robert Robinson.The authors have succeeded in resolving gnoscopine by the fractional crystallisation of its d-bromocamphorsulphonate from ethyl acetate. The first fraction consisted mainly of I-narcotim d-bromocamphor- sulphonate, which, after recrystallisation, melted and decomposed at 110-120' and had [.ID + 97.2' in chloroform. The second fraction consisted also mainly of this salt, and the mother-liquors, when left in the ice chest, deposited a large crop of crystals of d-narcotine d-bromocamphorsulphonate mixed with a quantity of the gnoscopine salt. The latter mas removed by treat- ment with ethyl acetate, in which the d-narcotine salt is sparingly soluble, and, after crystallisation, the residue mas found to be d-narcotine d-bromocamphorsulphonate,which melted at 170-1 85O and had [alp -29.0' in chloroform.When liberated from their salts by treatment with alcoholic ammonia, the alkaloids exhibited the following properties in chloroform solution : I-Narcotine from gnoscopine : [a], -199.P. 9,d-Narcotine ,, ,, + 199.9'. I-Narcotine from opium ,, -199.9O. All these specimens melted at 174-1 75' (uncorr.). On mixing hot alcoholic solutions oE d-and I-narcotine, crystals of gnoscopine, melting at 230°, separated at once. d-Narcotine had not previously been described, and the authors propose to submit it to physiological examination. A short time since (this vol., p. 46), the authors described a synthesis of gnoscopine from cotarnine and meconine, and as Salway (ibid,,98) has lately synthesised the former 132 substance, the synthesis of the inactive and active modifications of narcotine is now complete.The resolution of gnoscopine was rendered possible by the generosityof Messrs. T.and H. Smith, of Edinburgh, who placed 100 grams of this rare opium alkaloid at the authors’ disposal. The authors are also indebted to Prof. W. J. Pope for the d-bromocamphorsulphonic acid required for this research. 139. The products of diszotisation of the trinitro-p-anisidines.” By Raphael Meldola and Fr6dQric Reverdin. The two isomerides, 2 :3 :5-and 2 :3 :6-trinitro-p-anisidine, both lose the 3-nitro-group on diazotisation, and give rise to the quinone- diazides : O*CH, 0 CH, ANO, NO2( \NO, \/:O%? N, A description was given of these compounds and of their azo-p-naphthol derivatives.The results of the diazotisation of these trinitro- anisidines, taken in conjunction with those of former researches, bring out very clearly the extreme mobility of the 3-nitro-group as compared with the methoxy-group under comparable conditions of displaceability . 140. (( m-Hemipinic and asaronic acids.” By Bernard Dunstan Wilkinson Luff, William Henry Perkin, jun., and Robert Robinson. Although m-hemipinic acid is an acid of considerable importance, especially in connexion with researches on natural products, it is diflticult to obtain in quantity, and the following experiments were instituted with the object of discovering a convenient method for its preparation.Creosol methyl ether is nitrated, and the resulting nitrocreosol methyl ether reduced by tin and hydrochloric acid to 4 :5-dimethox~-o-toZzcidirte(I),which melts at 109”. This amino-derivative is then converted by Sandmeyer’s reaction into dirnethoxy-o-tohonitrile(11),which melts at 81” and, on hydrolysis with barium hydroxide, yields dimethoxy-o-toluic acid (III), which has already been prepared by Perkin and Weizmann (Tra~s.,1906, 99, 1651). This acid is oxidised by ?alkaline permanganate quantitatively to m-hemipinic acid (IV). MeO/\Me M~o/\M~ M~o/\M~ MeOAC0,H M~o!,)NH, nled\/JCN M~O()CO,H M ~ O I \//CO,H~ (1.1 (11.1 (111.) (IV. 1 133 Considerable quantities of m-hemipinio acid have been prepared in this way, and the following observations were also made during the course of this research.Aminocreosol methyl ether (I)is readily oxidised by ferric chloride to 4methoxy-2 :5-toluquinone (V), which crystallises in golden spangles, melts and decomposes at 170-172’, and is reduced by sulphurous acid to the corresponding quinol (m. p. 123”; VI). The latter is converted by methyl sulphate into 2 :4 :5-trimethoxytoluene (VII), which melts at 55O and, on oxidation with permanganate, yields asaronic acid (VIII). O:’\Me HO/\Me MeO/‘*Me MeO/\C02H Me01 I’O Med,/OH Me01\/IOMe MeO!,)UMe\/-(V. 1 (VI. 1 (VII.) (VIII.) When eugenol methyl ether is treated with acetyl chloride in the presence of aluminium chloride, a substance is produced which melts at 114’, and is evidently 6 :7-dimethoxy-1 -methylnaphthalene. MeO/\ MeO/\C0.CH3M~O!,,/CH~*CH:OEI, -+ M~OI \/ICH,-CH:CH, -+ Me 141.“The influence of radium emanation on equilibrium in a gaseous system : a correction.” By Francis Lawry Usher. The velocity-constant for the decomposition of ammonia by emanation has been recalculated from data already published (Trans.,1910, 97, 389). 142. ‘‘The intramolecular rearrangement of the halides of phenazo-thionium.” By Harold James Page and Samuel Smiles. It was shown that the chlorides of the simpler derivatives of phenazothionium are converted by the action of warm hydrochloric acid into the corresponding chloro-compounds of thiodiphenylamine. Displacement o€ hydrogen in the benzenoid systems of tbiodiphenyl-amine by the nitro- and similar groups seems to hinder this reaction.The complete process of chlorination of thiodiphenylamine has thus been accomplished, the two intermediate products-the sulphoxide and phenazothionium salt-having now been isolated. The exhaustive chlorination of thiodipheny lamihe may be carried out without isolating these intermediate compounds ; hydrogen dioxide and hydrochloric acid furnish tetrachlorothiodiphenylamine. 134 143. (( A study of the Landsberger-Sakurai boiling-point method of determining molecular weights.” By William Ernest Stephen Turner. The author criticised the Landsberger-Sakurai method and its modifications, and described the nature and vitlue of the corrections needed to make the method available for the determination of series of molecular weights at different dilutions.A simple form of apparatus whereby such determinations can be carried out was described. The revised value, 39.0, of the molecular elevation of the boiling point of chloroform, recently given by Beckmann, has been confirmed. 144. (‘The salts of 8-hydroxyquinoline.” By John Jacob Fox. The salts of 8-hydroxyquinoline have been prepared and found to dissolve appreciably in benzene and chloroform. The copper, cadmium, and nickel salts are greenish-yellow, the remaining salts being yellow- or buff-coloured. The degree of hydrolysis of the sodium salt of 8-hydroxyquinoline and of the hydrochloride was determined by Farmer and Warth’s method (Trans., 1901, 79, 863).It was found that in a O*lN-solution the sodium salt was hydrolysed to the extent of 11.6 per cent., and the hydrochloride to the extent of 4.2 per cent. 8-Hydroxyquinoline and its salts, 8-ethoxyquinoline and its hydrochloride, 5 :7-dibromo-8-hydroxyquinoline, and 8 -hydroxy-1:2 :3 :4-tetrahydroquinoline and its hydrochloride were examined spectrographically in alcoholic solution. The yellow colour of the salts was shown to be due to the extension of the bands of the original substances into the visible region, the general form of the curves for absorption being similar in the derivatives of S-hydroxy-quinoline and its salts. The curves obtained from hydroxytetrahydro- quinoline and its hydrochloride, were of a different character from that of hydroxyquinoline, and resembled those obtained from alkylated anilines.145. (( Apparatus for demonstrating the volumetric compositions of gases.’’ By Alaric Vincent Colpoys Fenby. The apparatus described was devised for the rapid demonstration of the combining volumes of gases and of the compositions OE compound gases. The volumes of gases introduced are simple multiples of a unit volume (15 c.c.) equal to one division on the burette, which is divided into six parts, The pressure is adjusted to atmospheric 135 pressure at each measurement, and no corrections for temperature or pressure are required. The apparatus consists of four parts, namely, (1) the gas burette, of special design ; (2) the levelling tube ; (3) a reservoir for filling the burette, and (4)a special form of gas generator and holder, by which fixed volumes of a gas can be passed into the burette.The whole is conveniently supported on a single retort stand. The use of the apparatus for the following experiments was described : Composition of ammonia by the chlorine method ; com-bination of hydrogen and chlorine in equal volumes ; combining volumes of hydrogen and oxygen ;the composition of carbon monoxide and hydrocarbon gases, and the decomposition of hydrogen chloride by sodium amalgam. Special features of the apparatus include the generation of chlorine in the burette; the method of introducing fixed volumes of gas into the burette from the generator, and the construction of the generator itself and the burette.146. (‘Some reactions of benzgl mercaptan. Benzyl tri- and tetra- sulphides.” By John Armstrong Smythe and Aquila Forster. When a solution of benzyl mercaptan in glacial acetic acid is saturated with sulphur dioxide and hydrogen chloride, a quantitative reaction takes place according to the equation : 4C,H,*CH2*SH+SO, = (C,H,*CH,),S, +(C,H,*CH,),S, + 2H,O. Benzyl tiisulpilicle melts at 49O, and possesses considerable crystal- lising powers. It forms a sparingly soluble additive product, (C6HS*CH2)2S3, AgNo3(m. p. 96O), with silver nitrate. The action of sulphur dioxide on benzyl mercaptan thus resembles that of thionyl chloride on mercaptans (Holmberg, Annalen, 1907, 359,Sl), and the results throw some light on Jones and Tssker’s work (Trans., 1909, 95, 1910).Benzyl mercaptan and benzyl disulphoxide condense in the p-* Iesence of glacial acetic acid and a current of dry hydrogen chloride, water being formed, the disulphoxide reduced to disulphide, and the mercaptan oxidised to disulphide : =3(C6H5*(C,H,~CH,),X,O, +4C6H,*CH2*SH CH,),S, + 2H20. Similarly, benzyl disulphoxide in the presence of glacial acetic acid and dry hydrogen chloride condenses with hydrogen sulphide, forming benzyl disulphide, water, and sulphur : (C,H,*CH,),S,O, 3. 2H,S =(C6H,*CH,)2S2+ 2H,O +S,. These condensations are quantitative. 136 Benzyl sulphoxide does not condense in this way when sodium ethoxide or acetic anhydride are used as condensing agents. Benzyl tetmsulphide, together with hydrogen chloride, is formed by the interaction of benzyl mercaptan and sulphur chloride, thus : 2C,H,*CH2*SH+S,CI, =(C6H5*CH2),S4+ 2HC1.The new sulphide is a white, crystalline powder, soluble in alcohol, benzene, etc., insoluble in water, and melting at 49-50’, It forms no additive products with methyl iodide or with silver nitrate. Nascent hydrogen reduces it, giving benzyl mercaptan and hydrogen sulphide, and chlorine attacks it in the cold with the formation of sulphur chloride and benzyl chloride, In glacial acetic acid solution it is oxidised by hydrogen peroxide. 147. “The action of sodium or potassium hydroxides on sodium alkyl thiosulphates and on disulphides.” By Thomas Slater Price and Douglas Frank Twiss.The authors referred to the criticism by Fromm and Erfurt (Ber., 1909, 42,3816) of their explanation of the course of the reaction between alkalis and the sodium dkyl thiosulphates, and pointed out that there is no satisfactory experimental evidence for the formation of intermediate compounds of the type R-S-QH, postulated by Gutmann (Bey., 19OS, 41, 1650) and favoured by Fromm and Erfurt. In connexion with the action of alcoholic potassium hydroxide on benzyl disulphide, it was shown that if benzyl chloride is added to the mixture after the reaction has taken place, and the mixture again heated, the main products are benzyl sulphide and benzoic acid, whereas if benzyl chloride is present from the commencement, a considerable quantity of the benzylmercaptal o€ benznldehyde is also formed From these results it was deduced that the primary result of the action of alkali on benzyl disulphide is the formation of benzyl mercaptan and benzoic acid.148. Carboxylic acids of cyclohexanone and some of its derivatives.” (Preliminary note.) By Henry Dent Oardner, William Eenry Perkin, jun,, and Hubert Watson. These acids are obtained when the cyclic ketones are treated, in ethereal solution, with sodamide and carbon dioxide. 137 cycloHexanone-2-carboxylicacid softens at 79", melts and decomposes at 81--8Z0, and, on reduction with sodium amalgam, yields cycZo- hexanol-2-carboxylic acid (hexahydrosalicylic acid), which melts at 111'.1-Methylcyclohexan-2-orte-3-carboxylicacid is a syrup. d-1-kfethylcyclohexan -3 -one -2(?)-carboxylic acid, prepared from 1-methylcyclohexan-3-onefrom pulegone, melts at 103", and has [.II, + 97-2O. dl-1-Methylcyclohexnn-3-onecarboxylic acid, prepared from dl-1-methylcyclohexanone, melts at looo. 1 Methylcyc1oh~xa~~-4-one-3-carboxyZicacid melts at 1Ol", and, on reduction with sodium amalgam, yields l-methyZcyclohexan-4-oZ-3-carhoxylic acid, which melts at 114" and, when heated, yields a methyl-cyclohemlzecarboxyZic acid, which distils at 153"/25 mm. and crystallises. This acid is being investigated with the object of determining the position of the double linking. Menthonecarboxylic acid melts at 154", and thymomenthone-carBoxylic acid at 150-15 1".All thoso acids which contain the grouping *CO*CH*CO,R give intense colorations when ferric chloride is added to their alcoholic solutions. Thursday, June and, 1910, at S.30 p.m., Professor HAROLDB. DIXON,M.A., Ph.D., F.R.S., President, in the Chair. Messrs. W. P. Bloxam and Hubert L. Lucking were formally admitted Fellows of the Society. Of the following papers, those marked * were read: "149. '' The interaction of nickel carbonyl and carbon disulphide." By Sir James Dewar and Humphrey Owen Jones. Nickel carbonyl and carbon disulphide vapours interact readily at the ordinary temperature to form carbon monoxide and a bronze-coloured deposit containing nickel, sulphur, and carbon ;the liquids, on the other hand, interact only to a very slight extent.An examination of the volume changes when the two vapours are allowed to react in a specially devised apparatus shows that the reaction is probably represented by the equation (11)rather than (I): SNi(CO), + CS, = 2NiS + 8CO + C . . . (11) Ni(CO),+CS,= NiS+4CO+CS . . . (I). 138 The reaction, however, is incomplete, proceeds more extensively at low pressures than at higher pressures, and is completely inhibited by the pre.sence of carbon monoxide of a sufficient concentration. Thus, for example, there is no change in a mixture containing nickel carbonyl vapour under 37.5 mm., carbon disulphide vapour under 32.5 mm., and carbon monoxide under 68.5 mm. pressure.In order to account for the influence of carbon monoxide on the reaction, and for the fact that the reaction, although not reversible, is incomplete, it is suggested that the actual reaction takes place, not between molecules of nickel carbonyl and carbon disulphide, but between free nickel produced by the dissociation of nickel carbonyl and carbon disulphide. The initial concentration of free nickel in the vapour of nickel carbonyl would be small, and would be much reduced by the presence of carbon monoxide, to which the dissociation of nickel carbonyl is very sensitive. Consequently, the presence of carbon monoxide would tend to inhibit the reaction until it mould finally come to standstill. DISCUSSION. The PRESIDENTasked whether it was not nascent nickel that reacted with the carbon disulphide vapaur.Had the authors observed whether the vapour of nickel carbonyl showed appreciable dissociation through- out its mass when admitted to a vacuous bulb, or whether the dissociation only took place in contact with the glass surface ? Dr. JONESreplied that the behaviour of nickel carbonyl vapour at low pressures indicated that dissociation takes place in contact with the glass surface, and the interaction with carbon disulphide appeared to take place similarly. *150. ‘‘ Synthesis of cotarnine.” By Arthur Henry Salway. The author described in detail an investigation, of which a pre-liminary account has recently been given (this vol., 98). DISCUSSION. In reply to Dr. Barger, Dr.SALWAYpointed out that the synthesis of cotarnine is complete, since myristicinnldehyde has been prepared by the author from rnyristicinic acid, which in turn is readily obtained from cotarnic acid (Roser, Annaclen, 1889, 254, 348). The synthesis of cotarnic acid has already been accomplished (Perkin, Robinson, and Thomas, Trans.,1909, 95, 1977). 139 *151. ‘‘The accuracy of the gold bullion assay.” By John Phelps. The author has examined a number of results obtained in the assay of gold bullion from the point of view of the probable error. The following points were considered : 1. Gold assays made in the course of routine work in the assay department of the Royal Mint. 2. (a;) Assays of “trial plates” and comparisons of samples of ‘‘ proof ” gold ; (b) Comparison of proof gold made in the Mint laboratory with that produced by the Utrecht Mint.3. Comparison of the results of assays made at the Royal Mint with the results of other assayers working on the same material. 4. Discussion on the same lines of results recorded in a paper by F. P. Dewey (“The Assay and Valuation of Gold Bullion,” Trans. Amer. East. Mining Engineers, 1909). The author finds that ordinary gold assays weighed to 0.05 per 1000 are subject to a probable error of +0*043per 1000, while in the case of special assays weighed to 0.01 per 1000, the probable error of a single assay may be reduced to f.0.032 per 1000. From this it is concluded that the error in the mean of 20 assays made with the greatest care should not exceed 0.01 per 1000. “152.“Morphological studies of benzene derivatives. Part I. Introductory.” By Henry E. Armstrong. The studies referred to were instituted with the object of ascertain-ing the general and particular effect of alterations in molecular structure-especially of alterations in the orientation in the molecule of similar radicles-on crystalline form in the case of the extensive series of isomeric tri-derivatives obtained on introducing two like or unlike halogen atoms and the sulphonic Iladicle in its various forms into benzene. The plan of the work was explained and a general account was given of the course it has taken. The inquiry has been prosecuted in the author’s laboratory during the past fifteen years but the significance of the results arrived at has been apparent only since the development of the Barlow-Pope theory of the interconnexion of external crystalline form and internal molecular structure : the results appear to afford singular confirmation of the theory. “153.Morphological studies of benzene derivatives. Part 11. Sulphonic derivatives of the 1 :4-di-derivatives of benzene containing halogens.” By Reginald Thomas Colgate and Ernest Harry Rodd. Twenty-seven compounds of the 1:4-series have been measured : the results were fully reported and discuseed. The sulphonic 140 chlorides and bromides fall into the one or the other of two crystallo- graphic series ; one or two cases of dimorphism have been observed, however, which connect the two series; the connexion is further established by the fact that in some cases the sulphonic chloride crystallises in the one series whilst the corresponding bromide crystallises in the other, although, as a rule, there is very close resemblance between corresponding sulphonic chlorides and bromides.The sulphonanilides and the ortho-, meta- and para-toluidides also form an isodimorphous group; in most cases they are obtainable in a labile as well as in a stable form. It was shown that all the compounds described can be arranged in one or the other of two series, one derived from the hexagonal, the other from the cubic mode of packing equal spheres-the two alternative modes which Barlow and Pope have shown to be possible in the case of benzene units.The results afford most striking evidence of the maintenance of a benzene framework in the molecules, *154. “Behaviour of two salts with a common ion, when dissolved in an organic solvent.” By James Charles Philip and Harold Reuben Courtman, The conductivity of solutions of tetraethylammonium iodide and potassium iodide, separately and together, in methjl and ethyl alcohols, methyl ethyl ketone, acetonitrile, and nitromethane has been deter- mined at 25’. The examination of the separate salts has shown that between v=50 and v=2000 the equivalent conductivity is a linear function of the cube root of the concentration ;that is, the empirical rule, A= A, -a vK formulated by Kohlrausch for binary salts in aqueous solution, may be taken as valid also for these salts in organic solvents.On the basis of this rule it is possible by Barmwater’s method to calculate the conductivity of a solution containing two salts with a common ion, on the assumption that in the mixture each salt behaves as if it were present alone at cz concentration equal to the sum of the concentrations of the two salts. The agreement between the observed and calculatted values is such as to suggest that the relation of two salts with a common ion in an ionising organic solvent is closely similar to the relation existing between them when dissolved in water. DISCUSSION. Dr. PHILIP,in reply to a question, said that the differences between the observed and calculated values for the conductivity of the mixed iodides were greater than the experimental errors.Formamide had not been tried as a solvent. Like water, it was characterised by 141 a high dissociative power, and for such solvents the differences between the values for the conductivity of the mixed salts calculated by Barmwater’s method and those calculated on an additive basis were considerably less than in solvents of weaker ionising power. 165. “The effect of contiguous unsaturated groups on optical activity. Part VI. The influence of molecular symmetry. Application to the relative rotatory powers of position-isomerides.” By Thomas Percy Hilditch. It was ahown that, in an optically active compound completely symmetrical with respect to the geometrical centre of its molecule and containing at the same time adjacent unsaturated radicles, there usually exists a very anomalous degree of rotatory power.The direction of the anomaly (positive or negative) is not always the same, and, in particular, negative effects frequently occur when two or more unsaturated groups are in spacial proximity, Similar, but less pronounced, phenomena accompany the presence of partial molecular symmetry coupled with unsaturation. This effect, together with that due to the conjunction in space of two unsaturated groups (Trans., 1909, 95,1577), appears in some measure to explain the deviations frequently observed from Guye’s hypothesis (in its simplest qualitative form) in the rotatory powers of optically-active position-isomerides.By utilising derivatives of trisubstituted benzene compounds (such as the phenolic camphor-/3- sulphonates) it has been possible to differentiate between the maximum effects due respectively to symmetry (1 :3 :5-isomeride) and to the influence of mass (1 :3 :4-isomeride), both of which are concentrated in the para-derivative in disubstitu ted compounds. 156. “The aotion of Grignard reagent on camphoric and SO-camphoric esters.” By Yiiji Shibata. The author has recently shown (Trans., 1909, 95, 1449) that the action of the Grignard reagent on phthalic esters results in the formation of derivatives of phthalide or those of phthalan, whilst glycols are produced from succinic and terephthnlic esters, and the conclusion was drawn that the two CO,R groups in phthalic esters are in the cis-position, whilst those in succinic and terephthalic esters are in the trans-position.In order to obtain further confirmation of this view, the author has now examined the action of the Grignard reagent on camphoric and isocamphoric esters, these being definitely known to be cis-trrans-isomerides. In accordance with the anticipation, dimethyl 142 camphorate, an ester of the cis-acid, gave campholides, whilst dimethyl iaocamphorate, an ester of the trans-acid, gave the non-condensed ester of diphenylhydroxyisocampholic acid. By the action of magnesium isopropyl iodide on dimethyl camphorate, a substance, CI4H2*OS, probably methyl 1 : 2 : 2-trimethyl-3-isobutyrylcyclopentane-1-carb-oxylate, was obtained.The author also discussed the constitution of dimethylcampholide obtained by G. Komppa (Ber., 1908, 41, 1039). 157. ‘‘ Some aromatic antimony compounds.” (Preliminary note.) By Percy May. By the action of boi, fuming nitric acid on triphenylstibine, Michaelis and Reese (Annalen, 1886, 233, 52) obtained triphenyl- stibine nitrate, (C6H5),Sb(NOJ2,melting at 156O. The author has, however, succeeded in nitrating the benzene nuclei of triphenylstibine, and has obtained a well pytallised trinikro-derivative melting at 191’. This, on reduction with zinc dust and glacial acetic acid, yields the corresponding amino-compound, which can. be recognised by the usual tests, but has not yet been isolated in the pure condition.A very small quantity of tri-p-aminophen?/lstibine has, however, been obtained by the action of sodium on a solution of antimony trichloride and p-chloroaniline in benzene solution. The extreme smallness of the yield is not surprising, a8 an insoluble compound is formed when a benzene solution of antimony chloride is added to a solution of p-chloroaniline in the same solvent, the formation of which tends to prevent the reaction from proceeding. Analysis indicates that this compound is formed by the union of one molecule of antimony chloride with one of chloroaniline. Antimony chloride does not appear to form similar compounds with aniline or with p-chloro- phenol. An attempt has been made to sulphonate triphenylstibine, and althoggh it was evident that sulphonation had taken place, no pure compound has, as yet, been isolated from the reaction product.It is proposed to prepare other substituted derivatives of triphenyl- stibine by the method indicated above, and also to study the derivatives of the amino-compound. 158. ‘‘Note on the cobaltinitrites.” By Mary Cunningham and Frederick Hollwo Perkin. In a recent paper (Tmns., 1909, 95, 1562), the authors gave a method for the preparation of sodium cobaltinitrite which was found to furnish the best results. Prof. E. Biilmann points out that an almost 143 identical method has been previously described by him. The authors regret that, in searching the literature, the communication of Prof.Biilmann had escaped their attention. 159. Acetone derivatives of &fructose." By James Colquhoun Irvine and Charles Scott Garrett. The condensation of fructose with acetone gives three fructose-monoacetones, two of which, on continued action, condense with a second molecule of the ketone, giving rise to the a-and p-fructose- diacetones previously described by Fischer. The formation of these three isomerides was explained on stereochemical grounds, and necessi- tates an extension of the nomenclature of sugar derivatives. a-Pructosemonoacetone was obtained by the partial hydrolysis of a-fructosediacetone by the action of 0.1 per cent. of hydrogen chloride at 30". Under these conditions only the non-glucosidic acetone residue is removed.The compound melts at 120-121°, and gave [a]? -158.9" in aqueous solution. /3-Fructoaemonoacetone was obtained as a syrup, and was identified by analysis and by the formation from it of P-fructosediacetone. The third monoacetone compound is incapable of further condensation, and was characterised by conversion into trimethyl fructosemonoacetone(b. p. 120°/15 mm.) by the silver oxide reaction. The a-and p-fructosediacetones have been further examined. The compouods show a remarkable difference in their behnviour towards hydrolytic agents. In each case the non-glucosidic group is the first to be removed, and this takes place with the a-compound under conditions towards which the p-isomeride is perfectly stable. 160. The absorption spectra of 1 :4-dihydronaphthalene and 1 :2 :3 :4-tetrahydronaphthalene." By Alfred Godfrey Gordon Leonard.Bamberger has shown that when reduction is confined to one of the nuclei in the naphthalene molecule, the properties of the compounds r;o produced are in close agreement with those of analogous benzene derivatives. These substances have been examined to ascertain if there might be any similar relationship between their respective absorption spectra, and the following conclusions are drawn : (1)The curves of 1 :4-dihydronaphthalene and 1:2 :3 :4-dihydronaphthalene are similar, and occupy a position intermediate between the curves of naphthalene and o-xylene. (2) The spectra are those of a benzenoid nucleus as modified by the presence of an aliphatic ring.144 (3) Such spectra are in close agreement with the observed chemical properties of the two hydrides. 161. “The determination of malonic acid by potassium perman- ganate.” By Alexander Thomas Cameron and Basil Charles McEwan. In order to extend the observations of Marshall and Cameron on the succinates (Trans., 1907, 91, 1519) to the corresponding maIouates, it was necessary to find a conveniently simple method for the quantitative estimation of malonic acid. Durand (Ann. Chim. anal., 1903, 8, 330) states that malonic acid can be estimated with potassium permanganate in acid solution at SOo, the formic acid, which is one of the products, reacting with the permanganate so slowly that a definite end point can be obtained.He writes the reaction as : C,H,O, + 30 =H,O + H,CO, + 2C0,. . . . (1>. Concentrated solutions of malonic acid and malonates decompose on boiling, with rapid evolution of carbon dioxide and production of acetic acid. Lamoureux (Compt. rend., 1899, 128, 998) states that this reaction commences at 68’. Any method requiring a temperature of 80” can evidently only be applied to dilute solutions. Using Durand’s original method, the authors have never obtained a definite end-point; this is due presumably to the slow but steady oxidation of the formic acid. On the other hand, the truth of the above equation can be easily shown qualitatively. When a dilute solution of malonic acid is distilled with acid permanganate, carbon dioxide is evolved, and the distillate contains formic acid, An attempt was made to reduce the oxidation of the formic acid to a minimum by heating the malonic acid with excess of permanganate for a few minutes, reducing the permanganate remaining with oxalic acid, and titrating the excess of oxalic acid with more permanganate. According to equation (l),1 gram of malonic acid is oxidised by 1.823 grams of potassium permanganste.In nine titrations the corresponding figure varied from 1.933 to 2.205 grams, showing no regularity. If complete oxidation of the malonic acid took place, as expressed by the equation : C,H,0,+20,=2H,0+3C02 . . . . (2)* 1gram of malonic acid would require 2.431 grams of permanganate. The actual results lie between the two figures, and it is evident that the method is inapplicable owing to the oxidation of an indeterminate amount of formic acid.Formic acid is immediately oxidised by hot alkaline permanganate, whilst under the same conditions malonic acid is very slowly attacked ; hence complete oxidation of the malonic acid can be brought about by first heating with excess of acid permanganate, and then rendering the whole alkaline with excess of alkali. This method was tested in the following manner. Eithera weighed quantity of solid or (where the weight is given in brackets) a measured volume of standard solution of malonic acid was added to approximately 2N-sulphuric acid, excess of permanganate solution added, and the whole heated to 80-90" for ten minutes (or longer with the more dilute solutions) ;the solution was then rendered alkaline with strong aqueous potassium or sodium hydroxide, and the heating continued for some minutes'; finally, excess of sulphuric acid was added, then for convenience excess of oxalic acid, and this excess determined with more permanganate. The results are given below : Grams Grams Grams Grams Weight malonic KMnO, Weight malonic KMnO, No.of of acid per gram No. Of of acid per gram experi-malonic per litre 111 alonic experi-inalonic per litre malonic ment. acid. solution. acid. ment. acid. soliltion. acid. 1 (0.2004) 2.85 2.382 6 0.1682 1'12 2.419 2 (0'2000) 1'42 2'431 7 0-1544 1'03 2.430 3 0.1942 1.30 2'449 8 (0.2100) 0'66 2.453 4 (0'2000) 1*25 2.451 9 (0,2048) 0'43 2-125 5 0.1850 1.23 2.449 10 (0.2048) 0'40 2.481 Theory 2'431 The figures show that the explanation given is the correct one.At the same time they indicate the limits of dilution (calculated on the concentration at the commencement of the reaction) within which the method can be employed quantitatively. In the first experiment some decomposition of the malonate through heat has already taken place, whilst in the last two the results are uncertain. Further experiments on similar lines have indicated that to obtain accurate results it is essential to work below 90' (the reaction commences at about 70",and proceeds rapidly between 80' and 85") and to avoid great excess of sulphuric acid. Mestrezat (Ann.Chim. anal., 1907, 12,173) states that tartaric and malic acids react with potassium permanganate in the same manner, with the production of formic acid and carbon dioxide, He suggests a similar method for their estimation.The case of citric acid (Wohlk, Zeitsch. anal. Chern., 1902, 41, 77) is more complex, but the reaction proceeds on corresponding lines, the chief products being acetone and carbon dioxide. It is evident that the permanganate reacts with all this series of acids in a parallel manner, and can therefore be used to estimate any one of them only in the proved absence of the others. 146 162. “The direct union of carbon and hydrogen. Synthesis of methane.” Part 11. By William Arthur Bone and Hubert Frank Coward. In continuation of their previous experiments (Trnns., 1908, 93, 1975), the authors are now able to report a not less than 95 per cent. yield of methane from less than 0.03 gram of highly purified sugar charcoal (containing not more than 0.06 per cent, of ash and less than 0.1 per cent. of hydrogen) by maintaining it in a steady current of pure dry hydrogen at 1150’ for from seventeen to twenty-five hours continuously, thus completing the proof of the direct synthesis of methane from its elements at this temperature. 163.(‘The existence of racemic compounds in solution.” By Albert Ernest Dunstan and Ferdinand Bernard Thole. In continuation of their previous work (Trans., 1908, 93,1815) the authors have investigated the viscosity-concentration relationships for various solutions of active and racemic compounds. The eec.-octyl hydrogen phthalates (d-, I-, and inactive forms) were examined in benzene solution, and were found to give identical curves.Hence the inactive ester does not exist in solution as a racemic compound. The d-, I-, and r-mandelic acids have the same viscosity in aqueous and in pyridine solutions, but when the viscosities were determined in a non-dissociating solvent, such as amyl acetate, a clear difference between the active and inactive forms was apparent. Adriani (Zeitsch. physikcd. Chem., 1900, 33,413) has already proved by Roozeboom’s method that r-mandelic acid exists in the fused state. In further support of the previous work on the tartaric acids, it was shown that a solution of racemic acid mixed with d-tartaric acid has a viscosity different from that of a solution of the pure d-acid of identical concentration.164. Note on the occurrence of oeyritrin (violaquercitrin) in Osyris abyssinica.” By Samuel James Manson Auld. In an examination of ‘‘ Pruimbast ” or ‘‘Cape Sumach,” Osyris compesea (Colpom mpe88urn), A. G. Perkin (Trarte.,1897, 71,1132) separated a glucoside, osyritvin, which he later showed to be identical with violaquercitrin, isolated previously by Mandelin (Jahresber, 1883, 1369) from Viola tricolor. Samples of Cape sumach have been examined at the Imperial Institute from time to time, and no difficulty has been experienced in separating the osyritrin from them. Recently a considerable consignment of the leaves and stalks of Osyris abyssinica, Hochst, has been received for examination from the Transvaal.The material as received gave a much deeper coloured extract than Cape sumach, and produced a darker leather of rather poor quality. The aqueous extract, on keeping, deposited a certain amount of solid matter, but this did not appear at all similar to the crystalline deposits previously obtained from Osyris compressa. The new material was therefore examined more closely. The Tamnilwr.-Analysis showed that the leaves contained about 23 per cent. of tannin. The leaves were extracted with water and the extract evaporated to a small bulk, when there separated a quantity of solid matter consisting of colouring principle and the phlobaphen of the tannin.The aqueous solution was fractionally precipitated with lead acetate, and the last fraction washed and decomposed with hydrogen sulphide. After removal of the lead sulphide and the excess of hydrogen sulphide, the solution was evaporated to dryness. It yielded a reddish-brown tannin of the catechol series. This tannin is much darker than that previously obtained from Osyris compressa, and it also shows more readiness to lose water and form the phlobaphen. Extraction of the Colouring Matter.-The coarsely-ground leaves were thoroughly extracted in a Soxhlet apparatus with 90 per cent. alcohol, and the residue, after removing the spirit, was poured into water. The green mass which separated was filtered off, and, after drying, was extracted separately with light petroleum and alcohol.The alcoholic extract set to a viscid, semi-solid mass on concentration. By pouring into excess of boiling water it was possible to separate a large quantity of dark brown insoluble matter of a phlobaphen nature, and on cooling the aqueous solution, a dirty brown solid deposit was obtained, which, after repeated precipitation with water from alcoholic solution, yielded a mass of small crystals. These were purified by several crystallisations from dilute alcohol and finally from boiling water. A further quantity of the same substance was obtained by deposition from the main filtrate containing the tannin. The substance formed small, greenish-yellow needles, melting at 189-190', after softening at 185-186' (osyritrin melts at 186').After being dried at 160°, it gave on analysis : C =53.17; H =4.51. C27H,801,requires C =53.28 ;H = 4.60 per cent. After being dried at 160' : Found, H,O =7.90. ~27H2801,,3H,0requires H,O =8-15 per cent. 148 On hydrolysis with dilute acid the substance gives an insoluble colouring matter and a sugar. The latter is dextrorotatory, and gives an osazone melting at 204-205’. Estimation of the colouring matter gave C,,Hlo07 = 45.45. The equation C27H2sO16+3H20 = C,,H,,07 + 2C,H1,06 requires C,,H1,,07=45.61 per cent, The colouring matter has all the properties of quercetin, and the penta-acetyl compound, prepared in the usual manner, melted at 190” and gave on analysis : C =58.48; H =3.93.Calc. C =58.59 ; H =3.90 per cent. The glucoside is therefore identical with osyritrin. 165. “The relative influence of the ketonic and ethenoid linkings on refractive power.” By Ida Smedley. The molecular refractions of the following unsaturated ketones were determined in chloroform solution : Ma. MP. MY. Eenzylidenescetone ..................... 48 -52 51-33 53-79 Heiizylideneacetophenone ............ 70’48 75‘30 80.2 Ciniiamylideneacetone .................. 64-19 70-76 -Dibenzylideneacetone ................. 84 -04 92-17 -Cinnamylideneacetophenone ......... 87 -59 98.17 -Cinnamylidenebenzylideneacetone ... 102.69 ---Dicinnaniylideueacetone ............... 121 -5 -The conclusion is drawn that, placed at one end of a chain of conjugated ethenoid linkings, the ketonic and ethenoid linkings have apparently the same effect in exalting refractive power.When interposed in a chain of ethenoid linkings, the effect of the carbonyl group diminishes the exaltation. Its effect is probably then com-parable with that of an ethenoid linking contained in a side-chain. 166. (‘The constitution of the /3-diketonks.” By Ida Smedley. The evidence from the physical properties of the P-diketones was shown to be in harmony with a hydroxy-ketonic structure, and it is found unnecessary to assume the existence of the di-enolic form. Dibenzoyldimethylmethane (m. p. 99.) was prepared, and the molecular refractions of the following substances were determined in chloroform solutions. Ma.Mg-Ma. Benzoylacetone ........................ 50-3 3-2 Dibenzoylmethane .................. 74’6 6-9 Dibenzoyleth ylmethane ............ 75-0 3.4 Dibenzoyldimethylmethane ...... 76 ‘0 2’3 Ethoxybenzylideneacetophenone.. 79.6 5.2 Tetraphenylallene ................. 117.7 6 *7 Tetraphenylacetone .................. 115-3 4-0 In the preparation of tetraphenylallene (Vorliinder, Ber., 1906, 39, 1024), tetraphenylacetone, m. p. 2S0, was isolated. The action of the Grignard reagent on dibenzoylmethane and benzoyldimethylmethane was also studied. 167. ‘(An apparatus for the distillation of fats and fatty acids in the vacuum of the cathode light.” By [the late] JamesCampbell Brown. 4r& ::QM 771 mn+<RVI In the course of an investigation of the constitution of various naturally-occurring fats, it became desirable to subject the fats them- selves, and also the acids derived from them, to fractional distillation in a high vacuum, with a view to effecting, if possible, a separation into their constituents.Distillations in the vacuum of the cathode light have been previously carried out, notably by Krafft (Ber., 1896, 29, 1316), but it was thought that the apparatus used might be considerably improved, more particularly in the case of the receiver. A series of experiments was therefore entered upon with this object in view, and the apparatus described below is the outcome. It consists essentially of a desiccator, made with a broad flange, on to which the lid was very carefully ground by means of carborundurri powder.Inside the lower portion of the desiccator a circular iron plate was fitted on glass bearings in such a way that it could revolve very freely. The best method of doing this was found to be as follows. A cork, or, as was afterwards used, a block of lead carrying a pointed glass rod, was cemented to the bottom of the vessel in an exactly central position. The plate was fitted by means of a cork cemented firmly to it with a glsss tube which would pass freely over the rod, and the sealed end of which rested on the point of the latter. The plate was pierced near its rim with eight holes, each of which carried a test-tube, and each of these tubes could be brought in turn beneath the delivery-tube by means of a magnet worked on the outside of the vessel.The lid of the desiccator was fitted with a tightly fitting rubber cork, through which passed the delivery-tube and the exit-tube, and also two thick brass -rods, the use of which will be explained later. In the earlier experiments this cork was fitted with a mercury tube, but it was found that this was unnecessary, and that the same end could be obtained by lubricating the stopper with a small amount of glycerol. The delivery-tube was sealed to the flask which con-tained the substance to be distilled, whilst the exit-tube was sealed to a Topler pump. On the exit-tube was sealed a vacuum tube, through 150 which the passage of an electric discharge was used to determine the vacuum. On testing the apparatus it was found to hold a vacuum, in which the green fluorescence mas visible for at least two hours, and as it was intended to keep the pump at work throughout each experiment, this was considered quite satisfactory.In the distillation of acids the melting point of which was in the neighbourhood of 70°,a difficulty was met with. The acid solidified in the delivery-tube in- side the desiccator, and thus brought the distil- lation to an abrupt close. This difficulty was sur-mounted by wrapping the delivery-tube with resistance wire both in- side and outside the receiver, and keeping the tube hot by passing a current through the wire. In order to pre- vent the acid from solidifying in the por- tion of the tube which passed through the stopper, the tube was heated for about twenty minutes before the ex-periment was started, and the difficulty was in this way overcome.The brass rods previously mentioned were used to convey the current through the stopper. The working of the apparatus will be better understood by reference to tbe figure, which shows an elevation of the receiver, and a plan of the evolving plate. Many experiments were carried out with it, and in all these it worked extremely well. Its advantages are that it occupies an extremely small space, and that a distillate can readily be divided into any number of fractions, it is very easy to manipulate, while at the same time very high vacua indeed can be maintained in it over a comparatively extended period.151 168. The p-tolyl-1 :2-naphthylenediazoimines(3-p-tolyl-p-naphtha-isotriazoles).” (Preliminary note.) By G). T. Morgan and Arthur Bramley. The authors have prepared 2-p-tolylnaphthylene-1 -diazo-2-i,mine (3-p- tol?/Z-P-napl~thaisotriazole)(I), m. p. 165-1 66O, by the action of nitrous acid on 2-p-tolyl-1 :2-naphthylenediamine, and its isameride, 2-p-tolyl-1 :2-naphthatriazole (11), m. p. 149’ ; the latter substance was obtained by oxidising p-tolueneazo-P-naphthylamine(m. p. 113O) with chromic acid, and corresponds in properties with the product recently isolated by G. Charrier on heating the foregoing azo-p naphthylamine at 300’ (Atti R.Accccd.Sci. Torino, 1910, 45, 131).H/y*’ lo 6\N*C7H, a . /3 N C H / I \i.c;H7’ a . Plo 6\r[J/ ..... (1.1 (11.) The authors propose to examine the physical and chemical properties of other members of the two series of triazenes indicated by the above formulae. 169. (( A note on the aromatic derivatives of antimony.” By G.T. Morgan, F.M.Gc. Micklethwait, and Gi.. S. Whitby. In pursuing the investigation of certain derivatives of triphenyl-stibine oxide recently described (Trans., 1910, 97, 34), the authors have found that the nitration of triphenylstibine leads to the formation of a nitro-derivative, melting at 190°, from which, by reduction, a diazotisable arnine can be obtained. Some of the acyl derivatives of this base have been prepared.By the nitration of triphenylstibine hydroxynitrate, a trinitro-compound is produced, which on reduction yields a crystallisable triamine, furnishing a crystalline hydrochloride. This base has also given acetyl and om-P-naphthol derivatives, together with platini- and stanmi-chlorides. The sulphonation of triphenylstibine and triphenylstibine hydroxy- sulphate has been undertaken, and a soluble trisulphonic acid obtained, yielding very soluble alkali salts. The authors are at present engaged in the further study of these and other derivatives of triphenylstibine. 152 LIST OF FELLOWS, 1910. The List of Fellows for 1910 is now in active preparation, and changes of address received after 30th June cannot be included in it.In order that the new list may be as complete as possible, those Fellows whose degrees and Christian names do riot appear in full are requested to communicate them to the Assistant Secretary, At the next Ordinary Scientific Meeting on Thursday,June 16th, 1910, at 8.30 pm., there will be a ballot for the election of Fellowp, and the following papers will be communicated : “Studies of dynamic isomerism. Part XII. The equations for two consecutive unimolecular changes.” By T. M. Lowry and W. T. John. ‘(Studies of dynamic isomerism. Part XIII. Camphorcarboxy-amide and camphorcarboxypiperidide.” By W. H. Glover and T. M. Lowry. “The constitution of orthodiazoirnines. Part I. The naphthylene-diazoimines and their benzenesulphonyl derivative^.'^ By G.T. Morgan and W. Godden. ‘‘ The colour and constitution of diazonium salts. Part 11. Diazo- derivatives of as-benzylethyl-1 :4-naphthylenediamine.” By G. T. Morgan and E. G. Couzens. “The action of alkalis on certain derivatives of coumarin.” ByA. Clayton. The colour and constitution of the amino-coumsrins.” By A. Clayton.‘‘The relation between absorption spectra and chemical constitution. Part XV. The nitrated azo-compounds.” By E. C. C. Baly, W. B. Tuck, and Miss E. G. Mnrsden. ‘‘ Indirubin. Part I.” By W. P. Bloxam and A. G. Perkin. “Estimatiori of sodiiim aud cesium as bismuth nitrites. Part I. Estimation of sodium.” By W. C. Ball. “ The by-products of alcoholic fermentation.” By Miss C.E. Ashdown and J. T. Howitt. ‘‘A simple method of preparing tetranitromethane.” By F. D. Chat taway. “ Dimethoxy-p-tolylphenylmethane.” By J. E. Mackenzie. 153 CERTIFICATES OF CANDIDATES FOR ELECTJON AT THE NEXT BATJLOT. N.B.-The names of those who sign from ‘‘ General K.nowledge ” are printed in italics. The following Csndidates have been proposed for election. A ballot will be held on Thursday, June 16th, 1910. Batley, Ward Allen, 197, Eccles New Hoad, Salford, Manchester. Science Lecturer, B.Sc, (Chemistry and Physics) hlanehester University, 1908. M.Sc. (Chemistry) 1909. Wishful to keep abreast with chemical research. Harold B. Dixon. Alfred Holt, jun. W. H. Perkin. Ch. Weizmann. Norman Smith. Aythur LapuJorth.Bracewell, Geoffrey Alfred, 20, Heaton Grove, Bradford. Analytical and Consulting Chemist. For one year at Leeds University (Science Dept.). For three years with F. W. Richardson, Esq., F.T.C. Joint Author with F. W. Richardson, Esq. : ‘‘ Factors in the Analysis of Beeswax, Woolgrease,” etc., Soc. Chem. Industry. Fellow of the Royal Microscopical Society. F. W. Richardson. F. W. Branson. A. Jaffk. B. A. Burrell. George H. Martin. Collett, Ronald Leslie, Little Dawley, Hayes, Middlesex. Analytical Chemist. B.A. (Cantab.) Natural Science Tripos. Associate of the Institute of Chemistry. Bernard Dyer. Herbert Jackson. John M. Thomson. Patrick H. Kirkaldy. Alf. Chaston Chapman. 154 Dand,Middleton Henry, Steyning, Sussex.Brewer. Have spent many years in the study and practice of Chemistry as applied to the brewing industry, and am the inventor of the “Dand Forcing Tray Flask ” and the (‘Lawrence-Dand Refri- gerators,” Basil Wm. Valentin. F. G. Adair Roberts. Francis Davidson. B. A’. R. Newlunds. A. J. Murphy. John Joseph Eastick. Dodd,Alexander Scott, 173, Brun tsfield Place, Edinburgh. Analytical Chemist. (1) Six and a half years’ experience in Analytical Chemistry under J. Falconer King, Esq., F.I.C., City Analyst of Edinburgh. (2) Associate of the Institute of Chemistry. (3) B.Sc. Final in Chemistry on the Higher Standard at Edinburgh University. J. Falconer King. Leonard Dobbin. John E. Mackenzie. J. P. Longstaff. James Walker. Alex. C.Gumming. Grieve, James, 127, Buchanan Street, Glasgow. Chemist. Pharmaceutical Chemist ; Member of the Pharma- ceutical Society; Lecturer on Pharmacy and Materia Medica at the Glasgow and West of Scotland Technical College; a Director of Brazer and Green, Ltd., Manufacturing Chemists, Glasgow. Martin Dechan. Arthw JK Crossley. W. H. Martindale. Chus. Hor ne Warner. Alex. Gunn. Charles Alex. Hill. W. L. Horvie. Charles Gilling. C. R. Hennings. Thomas Cockburn. Guhlmann, Charles Frederick, Grantwood, Bergen Co., New Jersey, U.S.A. Chief Chemist, General Chemical Company of New York, (‘Hud-son River Works,” US.A. University of Pennsylvania, Mining Engineering and Chemistry Class, 1896. From 1896 to 1906, Chief Chemist, Harrison Bros.& Co., Chemical Wks., Philadelphia. From 1906 up to and including present time, Chief Chemist, Gen. Chem. Co., 155 Hudson River Works. Inorganic and Organic Research in Manu- facturing and Analytical Chemistry. T. Lynton Briggs. Hardee Chambliss. G. T.Bruckmann. Clmrtes F. Chcmdley-Marston T.Boge9.i. Hackford, John Edward, 15, Burford Road, Nottingham. Chemist to the Russian Steam Oilmill Co., St. Petersburg. B.Sc. 2nd Class Honours (Lond.). A.T.C. Joint author of : (1) ‘(The Electrolytical Estimation of Minute Qiiantities of Arsenic,” Sand & Hackford, (J.C.S., 1904, p. lOlS), and (2) “The Preparation of Silicols from Silicones, and their Spon baneous Transformation into Oxides,” Kipping & Hackford (to be published shortly).R. M. Caven. F. Stanley Kipping. Henry J. S. Sand. Arthur Slator. G. Druce Lander. Haycock, John, Great Glen, near Leicester. Analytical Chemist. Pharmaceutical Chemist. Chief Chemist to Messrs. T. H. Lloyd & Go., Leiceriter At present engaged on elaborating a new method for the separation and estimation of Cinchona alkaloids. Wishes to keep in contact with current chemical knowledge. Edward Masters. S. F. Burford. C. T. Bennett. Ernest J. Parry. r1. D. ,cUw. Huck, John, The Foundation, St. Bees School, Cumberland. Schoolmaster. Senior Science Master St. Bees School. AT. A. Cantab. 1st Class Natural Science Tripos, Pt. I., 1904. Scholar and Prizeman, Selwyn College, Cambridge. Science Master and Lecturer : Berkhamsted School, Herts (2 years) ;St.Bees School, Cumberland (4years). George Dixon. C. T.Heycock. John Parkin. R. H. Adie. L. A. Borradaile. C. H. H. Walker. Robert HeElon. Jacobs,Lionel Leslie, Sbelford, Becken ham, Kent. Assistant Manager. Dominion Tar and Chemical Co.’s Works, Sault Ste. Marie, Ont. Student of Chemistry studying for degree. 156 Some knowledge and technical experience of Coal Tar Products. Shortly to assist in research work in Coal Tar Products. George Barger. Geo. Jas. Woods. Reginald W. L. Clarke. Elkan Wech sler. Isaac S. Scarf. Joshi, Govind Laxman, 5, Argyle Avenue, Victoria Park, Manchester. Govt. of India State Technical Scholar. L. T.M. (Bombay), the course of study being Textile Chemistry, Physics, Mathematics and Fhgineering.Studied Applied Chemistry at the Muncipal School of Technology and I am desirous of keeping in touch with the latest researches in Chemistry. Jas. Grant. F, S. Sinnatt. F. G. Richards. S. J. Peachey. E. I,. Rhead. Long, Frank Stevenson,‘‘Hadley,” 80, Tylney Road, Forest Gate, Demonstrator, Chemical Dept., East London College. B.Sc. (Lond.). At present engaged in research. J. T. Hewitt. S. H. Woolhouse. F. G. Pope. Clarence Smith. J. J. Fox. Martin, William Ernest, 111, Bellevue Rd., Beres, Durban, Natal. Explosives Chemist. Chief Chemist, Kynoch Ltd., Umboyuturin, Durban. Seven years Assistant, Government Laboratory, Walt ham Abbey, Essex. Four years Chemist in charge of Guncotton Factory, Kynoch, Ltd.Seven years Chief Chemist, Kynoch, Ltd., Arklow. Walter H. Pay. J. S.Jamieson. H. H. C. Puntan. E. Nevill. A. B. Tonkin. Narbeth, Benjamin Mason, Durban Technical Institute. Principal of the Durban Technical Institute. Bachelor of Science in the University of Wales. Formerly Lecturer at the Swindon and North Wilts Technical Institute. Studied Chemistry at St. John’s College, Battersea, and at University College, Cardiff. J. S. Jamieson. A. €3. Tonkin. E. Nevill. H. H. C. Puntan. Walter H. Pay. 157 Oakley,Robert O’Field, 54, Sydney Rd., Hornsey, N. Student of Gray’s Inn ; Civil Servant. London Matriculation, 1903, 1st class; Int. B.Sc., 1904, 1st class; National Scholarship in Chemistry, 1905 ;parts I.and 11. in Chemistry at the Royal College of Science, 1905-7, 1st class; took B.Sc. Honours course with Dr. W. H. Mills at the Northern Polytechnic, 1908-9. M. 0. Forster. James C. Philip. G. T. Morgan. E. G. Couzens. William A. Tilden. A. Clayton. Paris, Edward Talbot, 15, Montpellier Villas, Cheltenham. Lecturer in Chemistry, Cheltenham Technical Schools. Lecturer to Science and Technical Students and Teachers ;holds advance certifi- cates in Chemistry; Hon. Assist. Sec. to the Cotteswold Nat. F. C.; Author of several palsontological communications ; engaged in Chemico-geological research work. J. M. Collett. Gerald T. Moody. G. W. Headley. Frank Dixon. AEfred C. Youngs. Reddie, John Alexander, 3, Spring Gardens, Bradford, Yorks.Chemical-Bacteriological Assistant to the Sewage Committee of the Bradford Corporation. for the last 7 years. Constantly engaged in research work at the Bradford Sewage Works, and have recently isolated the Anthrax bacillus, and other specific organisms, from the Sewage of Bradford. F. W. Richardson. Walter M. Gardner. A. Jaff6. Barker North. George H. Martin. Reed, Walter William, M.Sc. (Wales),A.I.C., 28, South Parade, Huddersfield. Assistant Lecturer in Chemistry, Technical College, Huddersfield. First Class Hons. in Chemistry B.Sc. (Wales), June, 1906. Isaac Roberts Research Scholar, University College of North Wales, Bangoc, 1906-8. M.Sc. (Wales), June, 1908. Associate of the Institute of Chemistry, April, 1908. Joint Author with Prof. K.J. P. Orton, of “The Wagdering of Bromine in the Chlorination of Bromoanilines ” (Trans., 1907, 91,1543), and “Isomeric Change in Benzene Deriv- 158 atives. Replacement of Halogen by Hydroxyl in Chlorobromodiazo- benzenes ” (Trans., 1907, 91,1554). Kennedy J. P. Orton. Alexander Lauder. James J. Dobbie. James Bruce. Allan Baguley. Rose, John George, Government Analytical Laboratory, Cape Town, Cape Colony. Government Analyst. Has occiipied his present position of Analyst in the Government Analytical Laboratory, Department of Agriculture, Cape Colony, for the last thirteen years, i.e., since March 14th, 289’7 ; vide ‘‘ Official Chemical Appointmonts,” 3rd edition. J. Muller. George N. Blackshaw. E. V.Flack. Walter D. Severn. Arthi-Stead. Sinclair, St. Clair Overbeck, M.A., Government Analytical Laboratory, Graharnstown, Cape Colony. Government Analyst. Has occupied his present position of Analyst in the Government Analytical Laboratory, Department of Agriculture, Cape Colony, for the last thirteen years, i.e., since August 5th, 1897 ; vide “Official Chemical Appointments,” 3rd edition. J. Muller. George N . Blackshaw. E. V. Flack. Walter D. Severn. Arthur Stead. Slade, Roland Edgar, Muspratt Laboratory, The University, Liverpool. Assistant Lecturer and Demonstrator in Physical Chemistry. B.Sc. Honours in Chemistry (Victoria), 1906, Mercer Scholar. M.Sc. (Victoria), 1907. 190’7-8, Assistant Chemist to British Aluminium Go., Ltd.1908, Gartside Scholar. 1909, Assistant Lecturer in Physical Chemistry at Liverpool University. Publica-tions : ‘‘ The Reducibility of Magnesium Oxide by Carbon ’’ (Tram., 1908, 94, 327). F. G. Donnan. Ch. Weizmann. V. J. Harding. R. Robinson. W. H. Perkin. Smith, James Harry, 5, Turks Road, Radcliffe, Lancs. Chemist. Conduct Analyses. Member of the Pharmaceutical Society. Desirous of keeping in touch with recent developments of Chemistry. J. Rymer Young. James S. Broome. George Clay ton. Wm. Scholes. F. Smith, James Ashton. 159 Smith, Thomas May,‘‘ Walla Crag,” Osborne Road, Romford. Trade Manager, A. Boake Roberts Cpr; Co., Ltd.; Stratford, E. Has been engaged in Practical Brewing for upwards of twenty years; has had a large number of pupils through his hands; has contributed largely to the brewing literature and obtained first prize for the best Article on ‘‘Practical Brewing,” in the Technical Journal, Feb., 1905.Basil P. Wigan. A. Leonard H. Gccrside. Alex. I(.Miller. Basil Wm. Valentin. A. Boake. J. Ross Nackenzie. Stedman, Ernest, 6, Breakwater Road, Bude, Cornwall. Science Master. Victoria University, B.Sc. with Second Class Honours in Chemistry, 1908. Teacher of Science in Bude County School. Am desirous of keeping in touch with chemical publications. Harold 16. Dixon. Ch. Weizmann. W. H. Perkin. Robert Robinson. Norman Smith. V. J. Harding. Thole, Ferdinand Bernard, 23, Cowper Avenue, East Ham, Essex. Assistant Lecturer, East Ham Technical College.B.Sc. (Lond.), 1st Class Honours Chemistry. Published research with Prof. Hewitt OR “Colour and Constitution of Azo-Compounds,” and with Mr. Dunstan on “The Relation between Viscosity and Chemical Con-stitution. ” W. H. Barker. J. T. Hewitt. F. G. Pope. Albert E. Dunstan. W. T. Clough. Williams, Frederick George, 5, Mayhill Road, Charlton, S.E. Metallurgist. For seven years First Assistant to the Metallurgist, Royal Gun Factories, Royal Arsenal, Woolwich. Training in Chemistry and Metallurgy at the Birkbeck College, Chancery Lane, London. Wesley Lambert. R. J. Redding. A. H. Mundey. H. Russell Pitt. H. Heron Smith. 160 The following Certificates have been authorised for presentation to Ballot by the Council, under Eye-law I (3) : Sorabji, Kaikhushroo Bamanji, Secunderabad, Deccan, India.Graduate in Medicine and Surgery of the Bombay University. Engaged in Chemical Analysis. The object is to be always well- informed of the latest researches in Chemical Science. E. M. Modi. Williams, John, 122, Liddell Street, Invercargill, New Zealand. Trained Teacher. Chemistry Master, Southland Boys’ High School, Invercargill, and Technical School, Invercargill, since Sept. 1907. (1) Bachelor of Science, London, in Chemistry, Physics and Mathe- matics. Bachelor of Science, New Zealand. (2) Triple Honours in Chemistry, Board of Education. (3) Teacher of Theoretical and Practical Chemistry in the Technical School, Brierley Hill. Wm. Whitehouse. Frank E. Thompson. ~~ K. CIAY AND SONb, LTD., BREAD ST. HILL, E.C. AND BUNGAY, SUFFOLK.
ISSN:0369-8718
DOI:10.1039/PL9102600121
出版商:RSC
年代:1910
数据来源: RSC
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