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Proceedings of the Chemical Society, Vol. 29, No. 410 |
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Proceedings of the Chemical Society, London,
Volume 29,
Issue 410,
1913,
Page 21-48
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[288Wd 15/2/13 P RO C E ED I N G S OF TER CHEMICAL SOCIETY. VOl. 29 No.410. Thursday, February 6th, 1913, at 8.30 p.m., Prof. A. SMITHELLS, F.R.S., in the Chair. Messrs. H. E. Annett, M. P. Applebey, E. Jobling, and A. K. Menon were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Messrs.: Edward Cahen, 32, Queen’s Road, Bayswater, W. Alexander Caruth, 101, Singleton Avenue, Prenton, Birkenhead. Harold Edward Pollock Hodsoll, 22, Pembridge Mansions, Bays- water, W. Douglas Rayment Keller, B.Sc., 48, Weymouth Street, Watford. Arthur George Abraham Miller, B.Sc., 1, Pretoria Terrace, Waltham Cross. Sosde Garalapury Sastry, B.A., Kavitha Vilas, Mysore, India. Thomas Harrison Winstanley, 45, Dicconson Street West, Wigan.Clifton Wyver, 37, Boulton Street, Wolstanton, Stoke-on-Trent. Of the following papers, those marked * were read: *20. “The presence of helium in the gas from the interior of an X-ray bulb.” By Sir William Ramsay, K.C.B. Helium containing a trace of neon was found after absorbing the condensable gases by .cooled charcoal from the gases obtained on heating the broken pieces of three X-ray bulbs, which use had coloured deep violet. In a second set of experiments, the bulbs 22 were not broken, but attached to a Topler pump by an air-tight connexion. The bulbs were heated to 350°, connexion was made between the interior of the bulb and the pump, and the gases were similarly tested. Again helium was found, containing, as before, a trace of neon.The bulbs were then broken, and the glass was examined for the same gas. Not a trace was found; it had all been expelled during the previous operation. *21. “The presence of neon in hydrogen after the passage of the electric discharge through the latter at low pressures.” (Preliminary note.) By John Norman Collie and Herbert Sutton Patterson. In a letter to Xature last July (89, 502) Sir William Rarnsay mentioned that one of the authors (J. N. C.) had noticed that calcium fluoride under the action of cathode rays emitted a gas, and that the gas contained traces of neon. Since then many more experiments have been made, both with and without calcium fluoride, it being found that so long as there were traces of hydrogen in the tube, neon could always be detected in the gas that had been submitted to the passage of the electric discharge at low pressures.In the meantime the other author (H. S. P.) had been engaged on the same research, but had approached it from another point of view. Neither of the authors was aware of the work of the other until the end of November, when, as they had both obtained the same results, it seemed best to publish the results in a joint paper. The experiments were carried out in an X-ray bulb or in an ordinary large-sized Pflucker tube, the hydrogen being obtained either from sodium amalgam and boiled water, or by the electrolysis of barium hydroxide solution. After the hydrogen had been submitted tcl the electric discharge for several hours, at varying pressures from 1mm.down to an X-ray vacuum and the pump being kept working most of the time, the collected hydrogen was mixed with excess of pure oxygen, prepared by heating potassium per- manganate, and exploded. The residual oxygen was then intre duced into an apparatus (invented by Sir W. Ramsay), where the oxygen could be absorbed by charcoal immersed in liquid air (and the authors take the opportunity of calling attention to this invalu- able discovery of Sir J. Dewar, without which the neon in the gas could never have been detected) ;the residual gas was then driven up into a narrow capillary bore tube with a platinum wire sealed into the top. By ireezing the mercury in the capillary tube, and then allowing a spark .tQ pass through the gas from the mercury to the platinum wire, the spectrum of neon was always noticed.Great care was always taken to be sure that no air leaked into the apparatus during the experiment; also caseful testa were made to see that there was no air either in the hydrogen or the oxygen used, and blank experiments were always made by exploding large quantities of the oxygen and hydrogen employed, and unless the hydrogen had been submitted to the electric discharge, neon was always absent in the residual oxygen. The amount of air necessary to produce the quantity of neon usually found would be about 1 to 2 C.C. In one experiment, where enough neon had been found to give the ordinary flams-coloured appearance when sparked, the oxygen absorbed by the charcoal and liquid air was carefully pumped off and absorbed by phosphorus; a small bubble of gas the size of a large pin’s head remained.This gas, however, when examined in a spectrum tube was found to be not residual nitrogen from an air leak, but hydrogen. The neon therefore found in hydrogen that has been sparked at low pressures in an X-ray vacuum is not due to air leaking into the apparittus during the experiment. Addendum.-Since the above communication was submitted to the Chemical Society some fresh facts have been obtained by oils of the authors (J. N. C.). In order to be certain that the neon had not leaked in from the outside air, through the glass, when the glass wm under the influence of the cathode discharge, a tube was made in which that end of the apparatus was inside another tube.The outside tube was then filled, first with neon, and secondly helium, the inner tube containing the hydrogen. In both cao3es neon was found in the hydrogen as before, and not a trace of helium leaked in. A final experiment was made with an entirely fresh apparatus, in which the whole inner tube was encased in an outer one. Again neon was found in the hydrogen that was sparked in the inner tube. The vacuum in the outer tube was below that of an X-ray bulb for the spark would not pass through it. It wit8 thought worth while to wash out this outer tube after the experiment with 1 C.C. of pure oxygen. The oxygen was then absorbed by charcoal cooled with liquid air, and a residue remained at least fifts times as great as the residue from the gas in the inner tube.It was a mixture of helium and neon, the helium being in excees. This result has been confirmed by the other author (H. S. P.), who has also found that if the outer tube is filled with oxygen under 10 cm. pressure, the residual gas in the outer tube, instead of being mostly helium, is mostly neon. 24 "22. ''Vaubel's supposed phenyldi-imine. 'I By Martin Onslow Forster and John Charles Withers, Proceeding in the manner described by Vaubel (Ber., 1900, 33, 1711), the authors failed to produce phenyldi-imine, obtaining instead a constant boiling mixture of phenylazoimide and aniline.The percentage composition of a mixture, C,H,*N, +C,H,*NH,, is identical with that of the supposed phenyldi-imine, C6H,*N:NH, and the properties ascribed by Vaubel to this individual accord with those of the mixture in question. "23. '(The latent heat of vapours." (Preliminary note.) By Malcolm Percival Applebey and David Leonard Chapman. On the assumption that the characteristic equation of a liquid and its vapour can be expressed by the equation: p(v -b)=Rt, in which p is the total pressure (the sum of the external and internal pressures), b a function of the temperature only, R the gas constant, and t the absolute temperature, the authors have deduced thermodynamically that the molecular latent heat of a vapour is given by the equation : 1 dbL=Btloge-v2-b +Rt ---) t-v1-b (v,L 9,-b dt' L being the molecular latent heat, and v2 and v1 the molecular volumes of the liquid and vapour respectively.With the aid of S. Young's determination of the latent heat of n-pentane vapour (Sci. Proc. Roy. Dubl. SOC.,1910, 12, 414), it dbhas been shown that -is probably almost constant between 30°dt and 180°, and equal to 0.0892. The value of b at the critical point is a little greater than a third of the critical volume. In the following table the observed latent heats of n-pentane are compared with those calculated from the above formula. Latent Heats of n-Pentane between 30' and 190°. b =120.30 at the critical point; 6' =0.0892.dt Temperature. 30" L (ob-served). 85-76 L (calculated).86.02 Temperature. 130" L(ob-served). 60.85 L (calculated). 60 '60 40 84-31 83'22 140 56-58 56'57 50 82-13 82-03 150 52.39 52-34 60 80.07 79.98 160 47-42 47'46 70 80 90 100 77-77 75.33 72.73 69-94 77.73 75'34 72-73 69-93 . 170 180 190 197'15 42-06 35.01 24.68 0.0 42.09 35'30 24'51 0.0 110 120 67'31 64-48 67.16 64'06 (critical temp. ) 25 The validity of the formula can be tested with the aid of the discovery of J. E. Mills (J. Physical Chem., 1905, 9, 402) that *=E at the critical point. For, writing the above equation dt v in the form: it will be seen that at a temperature just below the critical point, when v2-q is small, it reduces to: L 1 +-t 1 db-=Rt(--}, v2-91 v1 -6 (vl-bj2 dt and L --t-.dP ~2 -vl dt 1 dbIntroducing the values 120.30 and OS0892for b and -respec-dt tively, and putting v1 equal to 309.95, the value given by Young for the critical volume, one obtains : and this is in close agreement with the formula discovered by Mills.This investigation furnishes evidence for the view that b increases at a uniform rate from the absolute zero to the critical point, and that it does not diminish as Roth found for ethylene (Ann. Phys. Chem., 1880, [iii], 11, I). The discrepancy between Roth’s con- clusion and the authors’ is probably accounted for by the fact that Roth made the same assumption as van der Waals, namely, that the internal pressure is at all temperatures proportional to the square of the density, whereas the authors’ speculations are inde- pendent of any assumption as to the value of this magnitude.It is obvious that, on the assumption that * is constant,dt values of b can be calculated from Mills’ relation and the law of rectilinear diameter quite independently of the latent heats, and that these values can be used to calculate the latent heats. DIscusSION. Mr. MERRIMANpointed out that Professor Young’s values for the latent heats of vapours could not strictly be called “observed” values, as they were calculated from the thermodynamical formula : 26 the quantities vl, v2, 9being read from smoothed curves. Thisdt Fact should be borne in mind when considering the validity of the conclusions drawn by the authors from the comparison of their new expression with Professor Young’s values, as these values must include any assumptions made in deducing the thermodynamicai formula.24. *‘Derivatives of 0-xylem.” (Preliminary note.)By John Lionel Simonsen. With the view of devising a new method for the preparation of 3-nitro-o-xylene7 the author has investigated the nitration of o-xylene-4sulphonic acid. The three isomeric nitro-o-xylene-4-sulphonic acids have been isolated, and yield amides melting at 158O, MOO, and 214O respectively. The acid which yields the amide melting at 158O has been shown to be 4-nitro-o-xylene-5-sulphonicacid. Experiments are in progress with a view to orientating the other two nitro-sulphonic acids. The sulphonation of o-3-xylidine and 04-xylidine is also under investigation.26. 86 ‘Phe alkaloid8 of Xanthoxylum braehyacanthum.” By Hooper Albert Diokinson Jowett and Prank Lee Pgman. The bark of Xanthoxylum brachyacanthzcm was shown to contain 0.06per cent. of y-homochelidonine, and a quaternary base, which was isolated in the form of its chloride, C2,H2p04NC1,H20, in a yield of 1-85per cent. The properties of this salt suggested that it was one of the methochlorides of 1-canadine. A quantity of the latter alkaloid was therefore methylated, and the a-and b-metho-chlorides were sepaxated, when it was found that the former was identical with the dt from X. brac?igacanthu,m. The physiological examination of I-canedine a-and 0-metho-chlorides, which was carried out by Dr. P.P. Lnidlaw, showed that both possessed a curare-like action, and that the relative activity in this respect was as 1 to 12 on the frog. 26. “The absorption spectra of nimgle aliphatic substances in aolutions and 811 vaponrs. Part 11. Unsaturated aldehydes and ketones.” By John Edward Purvis and Nial Patrick XcCleland. The chief results obtained in the examination of the absorption spectra of certain unsaturated aldehydes and ketones were (I) the 27 considerable number of narrow bands found in the vapours of acrolein and crotonaldehyde, and which are absent from their solutions; and (2) the absence of similar narrow bands from the vapours of other unsaturated aldehydes, ketones, alcohol, and acid, and the close similarity of their specific absorption with those of the solutions.These results were discussed from a consideration of the ethenoid linking and the carboxyl group acting as primary oscillation centres. 27. ‘‘Phytin and phytic acid.” (Preliminary note.) By George Clarke. Phytin was extracted from finely ground, oil-free seeds of the ordinary Indian field mustards, a mixture of Brassica junceu (Hf and T) and Brassica campestris (Linn.), by 4 per cent. acetic acid or 0.2 per cent. hydrochloric acid, and separated from the dark brown acid extract by neutralisation with ammonia. The crude substance wits purified by further extraction, and precipita- tion from dilute acetic acid, and finally by extracting with ice-cold 8 per cent.acetic acid, from which it separated on boiling as an amorphous, white powder, completely redissolving if allowed to cool. The yield was 0*3-0*4 per cent. of the seeds. The phytin thus prepared resembled in properties the substance described by Schulze and Winterstein (Zeitsch. physiol. Chem., 1896, 22,90). It was completely soluble in cold, very sparingly so in hot, dilute acetic acid. It was decomposed by heating under pressure at 130-150° with 30 per cent. sulphuric acid into phos- phoric acid and inositol (hexa-acetyl derivative, m. p. 211O). The free acid was obtained from the pure phytin described above by precipitating the lead salt from cold dilute acetic acid, decom- posing the latter with hydrogen sulphide, and repeating ths treat- ment until the acid residue was completely soluble in 95 per cent.ethyl alcohol. This substance consisted of a mixture of approxi-mately equal proportions of phosphoric acid and an acid corre-sponding with the formula C,H40(HP04). The strychnine salt of the above acid, corresponding with the empirical formula, C&H270,N,P,2H20or csH40 (HP04) ,C2,H,2O2N2,2H20 crystallised from boiling water, in which it was sparingly soluble, in long needles melting and decomposing at 202-203O (uncorr.). It was very easily separated in a pure condition from strychnine dihydrogen phosphate [m. p. 252-253O (uncorr.)], with which it was mixed, by fractional crystallisation from water, the latter salt being very readily soluble in the cold. 28.‘‘ The constituents of the oil of Cydnus Indicus.” By Edwin Roy Watson. The strong and unpleasant odour of the insect Cydnus Zndicus is due to an oil which it secretes. The oil has been found to contain a large percentage of a non-volatile oil of the same general character as other animal oils. It also contains about 1.5 per cent. of an oil which is volatile with steam. This consists of an acid, C,H,,O, probably cycloheptanecarboxylic acid, and a small quantity of a non-acid substance (C,,H2,0, a). The acid has a strong, rancid odour, and the non-acid volatile substance has a still stronger odour. 29. ‘‘Vapour density of ammonium nitrate.” (Preliminary note.) By Prafulla Chandra Rly and Sarst Chandra Jana. In continuation of the determination of the vapour density of ammonium nitrite, the authors have extended their work to other decomposable substances under diminished pressure.Ammonium nitrate was selected for the present experiment, and the determina- tion of the vapour density was effected in a modified form of Victor Meyer’s zpparatus suitable for diminished pressure. It has been found that a part of the salt decomposes into nitrogen monoxide and water, and the rest sublimes. When the tube becomes cold after completion of the experiment, white crystals of the salt were deposited in the neck of the tube. The vapour density was found to be approximately 20. It thus seems probable that the undecom- posed part completely dissociates into ammonia and nitric acid in the gaseous state.30. ‘‘The solubility of sulphanilio acid and its hydrates.” By James Charles Philip. The solubility of sulphanilic acid has been determined at tem- peratures between Oo and 55O, and the resulting curve exhibits two breaks, corresponding with changes in the character of the solid which is in equilibrium with the saturated solution. The solids which are successively stable in contact with the saturated solution are dihydrate, monohydrate, and anhydrous acid respectively, and the temperatures at which the transitions occur are 21° and 40°. The dihydrate of sulphanilic acid is an efflorescent substance which loges all its water rapidly and regularly under conditions in which the monohydrate is unchanged, or is dehydrated with extreme slowness.This observation indicates that the water molecules in the dihydrate and in the monohydrate are attached in different ways. 29 31. (‘Hexahydropyrimidine and its benroyl derivatives.” By Arthur Waleh Titherley and Oerald Eyre Kirkwood Branch. By the action of aqueous formaldehyde on ay-diaminopropane monohydrochloride, a mixture of the hydrochlorides of meihylene- ay-diaminopropane (I) and hexahydropyrimidine (11) results, in which the former greatly predominates. On adding alkali the two bases form a tautomeric equilibrium mixture, in which the cyclic form (11)predominates: NH CH, CH,:N.[CH,],*NH, ZCH /-\CH, 2\-/ NH CH, * (1.) (11.) On fractionation the cyclic base distils at about 150°, leaving a polymerised form of the open-chain base, but owing to rapid tauto- meric change in the distillate, on refractionation it leaves behind a considerable portion it9 the non-volatile open-chain base.An aqueous solution of the mixture of bases on titration with acid requires rather more tkan one equivalent to reach the neutral point, but owing to isomerisation to the cyclic form (and partly to hydro- lysis, yielding ay-diaminopropane) further gradual addition of acid gives a second neutral point corresponding with two equivalents. Hydrolysis prevents pure crystalline salts being isolated. The monobenzoyl derivative, CH,:N-[CH&.NHBz, obtained by the action of formaldehyde on monobenzoyl-ay-diaminopropane (T., 1912, 101, 2350) is an amorphous $-base of neutral reaction, which with hydrochloric acid rearranges, giving the crystalline hydro- chloride of monobenzoylhexahydropyrimidine, but the free base cannot be obtained, since it immediately rearranges to the open- chain, amorphous methylene derivative.1:3-Dibenzoylhexahydropyrimidineis a stable, crystalline solid (m. p. 95O) obtained in quantitative yield by the moist benzoylation of methylene-ay-diaminopropaneZhexahydropyrimidine, and also by the slow action of formaldehyde on dibenzoyl-ay-diaminopropane id the presence of concentrated hydrochloric acid. 32. Condensation of ketones with phenols.” By Remendra Kumar Sen-Glnpta. Methyl ethyl ketone condenses with a-naphthol in glacial acetic acid solution in the presence of fuming hydrochloric acid, yielding the anhydride of 1:1-dihydroxymethylethyl-aa-dinaphthyhethane, CHCMeEt<C10H6>0 (m.p. 154-155O); in common with the 10 6 30 members of this type, it crystallises from glacial acetic acid in transparent, rhonibic plates. A bromo-derivative melts at 250°, and a nitro-compound at 265O. Methyl propyl ketone and diethyl ketone condense under the same conditions, giving respectively the anhydrides CMePra<CIOHd>O (m. p. 162O) and CEt2<CIOH6>0 CH CH 10 0 10 R (m. p. 166’5O). Acetophenone and a-naphthol, when dissolved in a minimum quantity of glacial acetic acid and saturated with dry hydrogen chloride, condense in the course of five to seven hours at 10looo, and the compound CMePh< CH6>0 melts at 167O.Benzo-CIOE-T,phenone does not appreciably condense in presence of hydrogen chloride alone ;phosphoryl chloride, however, brings about the con- densation very readily, and the compound CPb,<~lO~R>O melts 10 6 at 273O. With an excess of the agent, the product is probably identical with that described by Clough (T., 1906, 89, 771). The condensation of acetone and phenol which has been described by Dianiu (J. Russ. Phys. Chem. SOC.,1892, 23,488) requires about twenty-four hours’ heating to give a yield of 60-65 per cent. It has been found in this connexion that by the use of stannic chloride diluted with one and a-half to two times its volume of chloroform, a 50 per cent. yield can be obtained in the course of a few hours at 40-50°.33. rL The reaction between ferrio salts and thiosulphates.” By John Theodore Hewitt and Gladys Ruby Mann. The authors have studied the reduction of solutions of ammonia ferric alum by sodium thiosulphate and of other ferric solutions made up with the alum and potassium thiocyanate, phenol, or aceto- acetic ester. The rate at which ammonium ferrisulphate reacts is slower than that shown by ferric chloride; the iron probably forms part of a negative complex. The reactions measured proved to be all of the fourth order. 34. Influence of acetylacetone on ionic reactions.” By John Theodore Hewitt and Gladys Ruby Mann. The action of acetylacetone in hindering the precipitation of ferric phosphate from solutions of ammonia iron alum led to a general examination of the action of this substance on solutions of metallic salts, since other metals besides iron furnish volatile acetylacetonates. Approximately N / 20-solutions of various metallic salts were prepared, also solutions containing 12’5 and 31 17.5 grams of metylacetone per litre.One volume of salt solution mixed with an equal volume of the solution of the acetylacetone would give a solution in which for 1 atom of metal about 24 molecules or 34 molecules of acetylacetone were present according to whether the weaker or the stronger solution were used. The weaker solution was used for salh of bivalent metals, the stronger for the tervalent metals. Ordinary reagents were then added to see whether or not the presence of acetylacetone inhibited their action.Silver Nitrate.-Slight cloudiness on adding the acetylacetone : sodium chloride precipitates silver chloride. Mercurous Nitrate.-Acetylacetone reduces to metal. Mercuric Chloride.-No visible change on adding acebyhetone : hydrogen sulphide precipitates mercuric sulphide. Lead LVitrate.-No apparent change : hydrogen sulphide, sodium chloride, p.otassium chromate, sodium carbonate, and potassium sulphate give the usual precipitates. Copper Su1phate.-Colour changes from blue to green : hydrogen sulphate, pchassium thiocyanate, and sodium hydroxide gave the usual reactions. Cadmium Su1pAate.--No visible change : hydrogen sulphide pre- cipitates cadmium sulphide.Potash Alum.-No apparent change : sodium hydroxide, sodium hydrogen phosphate, and ammonium hydrogen phosphate give the usual precipitates. Chromium Sulphate.-No visible change. With ammonia and sodium hydrogen phosphate precipitates are formed on keeping. Ammonium hydrogen phosphate gives no precipitate ; the precipi- tate with sodium hydroxide is soluble in excess of the reagent. Ferric Alum.-Colour changes to deep red (deeper than thio- cyanate) on adding acetylacetone. Ammonia produces a precipitate on keeping for some time. Sodium hydrogen phosphate gives no precipitate in the cold, but the solution is considerably lightened in colour, and a precipitate is produced on boiling. Precipitates are obtained with sodium hydroxide and ammonium hydrogen phosphate.Zinc Sdphate aad Manganese Sdphate.-No visible change : usual reactions with sodium hydrogen phosphate, sodium carbonate, hydrogen sulphide, and sodium hydroxide. Nickel SulpJbate.-No visible change : usual reactions with sodium hydroxide and hydrogen sulphide (after adding ammonia). Cobalt SuZphate.-No visible change : hydrogen sulphide precipi- tates cobalt sulphide after adding ammonia. Sodium hydroxide gives a blue precipitate, which turns brown on keeping. 35. “Viscosity and association. Part IV. The viscosity of the aromatic amines.” By Ferdinand Bernard Thole. This work was undertaken with the primary object of finding whether substitution in the benzene ring a$ects the viscosity of the aromatic amines in the same way as in the case of the phenols.At the same time the range of amines previously studied by Mussell, Thole, and Dunstan has been increased considerably. A large number of arnines, substituted both in the amino-group and in the benzene nucleus by different groups, have been examined in the pure state at 55O and in amyl acetate solution. The results show a number of interesting parallels with the corresponding phenolic derivatives, especially as regards the influ- ence of the carbethoxyl and nitro-groups, but frequently the analogies are hidden by the influence of other factors, the impor- tant effects of which are shown much more clearly in this series than in the other types of compounds hitherto examined. 36. (‘The influence of the constitution of tertiary bases on the rate of formation of quaternary ammonium salts.Part I.” By Ebenezer Rees Thomas. The author has measured the reaction-velocities of certain aromatic tertiary bases with ally1 bromide, and, in some cases, benzyl bromide, at 40° in 1\T/10-absolute alcoholic solution. Twenty-one bases have, been examined, and certain general con- clusions as to the influence of the nature and position of substituents were indicated. 37. Some blue iron cyanogen compounds.” By Herbert Ernest Williams. The precipitation of a blue ferric ferrocyanide from a ferro-cyanide of an alkali metal always contains some alkali metal in combination which cannot be removed by washing. Several blue compounds were prepared under different conditions from the alkali metal ferrocyanides, and analysed after being thoroughly washed and dried.In all cases the alkali metal was found to be present in definite ratio to the ferrocyanogen, and blue iron cyanogen compounds of complex formulz were obtained. Mangarnommganic ferrocyanide is produced by the action of concentrated nitric acid on the white manganous ferrocyanide; it forms a dark brown, granular powder. 33 38. Some properties of carbon monoxide.” By Richard William Merriman. Three hundred litres of carbon monoxide were prepared by slowly delivering pure formic acid below the surface of concentrated sulphuric acid kept at 60°. The gas was passed through four Drechsel flasks containing 30 per cent. sodium hydroxide, and was collected over water in a large gas-holder.Although always described as an odourless and tasteless gas, this specimen had a perfectly definite metallic odour and taste. The idea occurred to the author that it might contain a small quantity of the unknown formic anhydride. This substance would have the properties of an aldehyde, so the following experiment was performed. The gas was bubbled through a series of Drechsel flasks containing the following solutions : sodium hydroxide, decolorised rosaniline, sodium hydroxide (Z), Fehling’s solution, and ammoniacal silver nitrate. The decolorised rosaniline wa not altered, but the silver nitrate and Fehling’s solution were at once reduced. Carbon monoxide prepaxed in the following ways also possessed similar pr opr ties.(a) Prom Oxalic Acid.-Two hundred and thirty C.C. of pure sulphuric acid were added to 100 grams of crystallised oxalic acid. The temperature rose to 45O. Effervescence commenced at 65O, and slow evolution at 90°. A regular stream of gas was evolved by keeping the temperature at llOo. The gas was washed with four portions of 30 per cent. sodium hydroxide and passed through four soda-lime towers. It was passed through three Drechsel flasks containing Fehling’s solution and three containing ammoniacal silver nibrate. All showed reduction. (6) From Potassium Cyanide.-Pure sulphuric acid was dropped on to 200 grams of potawium cyanide in lumps, The cyanide turned brown, and rapidly evolved gas.The gas wi~spassed through four Drechsel flasks containing 30 per cent. sodium hydroxide, four soda-lime towers, and two Drechsel flasks containing 20 per cent. silver nitrate. The first two portions of sodium hydroxide turned reddish- brown and finally black. The last silver nitrate Bhowed no precipi-tate of silver cyanide. The gas possessed the same odour, taste, and reducing properties ae the other specimens. (c) From Pure Sdphuric Acid and Sodium Formate.-External heat was unnecessary except at the end of the preparation. The gas was washed as before, and had the same properties. (d) From 70 per Cent. Sulphuric Acid ad Sodium Formte.-The formate dissolved at 70°; slow evolution of gas commenced at 34 85O, but did not become rapid below 115O; the final temperature was 135O.The gas, treated as before, possessed the same properties. (e) Smaller quantities of gas were prepared from lactic acid and malic acid with similar results. (f) From Carbon, Dioxide and Cadon.-As a final test, 40 litres of carbon monoxide were prepared by slowly passing pure carbon dioxide through a tube 80 cm. long packed with charcoal heated to bright rednegs. In this experiment formic aahydride could not have been produced. The carbon dioxide from a Kipp’s apparatus was passed through two wash-bottles containing sodium carbonate solution and two containing pure sulphuric acid. The resulting gas was washed as before, and possessed the same properties. It follows that pure carbon monoxide possesses a perfectly char- acteristic odour and taste, and readily reduces Fehling’s solution and ammoniacal silver nitxate solution.It has no action on decolorised rosaniline. ADDITIONS TO THE LIBRARY. I. Donatiam. Barnett, l3dwmd de Bawy. The preparation of organic compounds. London 1912. pp. xvi +310. ill. 88. 6d. net. (Recd. 14/1/13,) From the Author. Cram, Char268 Fredarkk, and Bevan, &hard John. Researches on cellulose. 111 (1905-1910). London 1912. pp. x+173. 78. 6d. net. (Reed. 7/1/13.) From the Authors. 11. By Purchass. aiohter, Victor wn. Chemie der Kohlenstoffverbindungen oder o.rgmische Chemie. VoL 11. Carbocyclische und heterocyclische Verbindungen. Edited by R. Anwhutz and a.Meerweia 11th edition. Bonn 1913.pp. xxii+ 1048. M.26.-. (Reference.) 35 ANNIVERSARY DINNER. It has been arranged that the Fellows of the Society and their friends shall dine together at the Whitehall Rooms, Hotel Metro- pole, at 7 for 7.30 o’clock, on Friday, March 14th, 1913 (the day fixed for the Annual General Meeting). The Council has decided to invite Fellows to become Stewards for this Dinner, the additional liability of each Steward not to exceed 10s. 6d. The price of the tickets will be One Guinea each, including wine, and half a guinea each, not including wine. All applications for tickets must be received not later than Friday, Mmch 7th, next. Tickets will be forwarded to Fellows on receipt of a remittance for the number required, made payable to Mr.S. E. Carr, and addressed to the Assistant Secretary, Chemical Society, Burlington House, W. At the next Ordinary Scientific Meeting on Thursday, February 20th, 1913, at 8.30 p.m., there will be a ballot for the election of Fellows, and the following papers will be communicated : “The mode of combustion of carbon.” By T. F. E. Rhead and R. V. Wheeler. “The nomenclature of the rhamnose group aad of other substances related to the aldohexoses.” By H. Marshall. “ Some green iron cyanogen compounds.” By H. E. Williams. “Catalytic decomposition of hydrogen peroxide.” By Gwen Dyer and Alice B. Dde. 36 CERTIFICATES 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 ZOth, 1913. Acland, Theodore William Gull, 19, Bryanston Sq., W., and King’s College, Cambridge. Student. I have been working as a Science Student for some years. Last year I took Natural Sciences Tripos, Part I. This year I am study- ing Chemistry only, doing the work for Part 11. in that subject. W. J. Sell. W. H. Mills. J. G. M. Dunlop. C. T.Heycock. W. J. Pope. Sydney Lupton. Adam, Neil Kensington, 21, Barton Road, Cambridge. Scholar of Trinity College, Cambridge. Student of Chemistry in the University Laboratory, Cambridge : 1st Class Natural Sciences Tripos, Part I. W. J. Pope. C. T. Heycock.F. G. Hopkins. H. J. H. Fenton. W. J. Sell. W. €I.Mills. Beath, William, 152, St. George’s Road, Hull. Teacher of Chemistry at the Boulevard Secondary School, Hull. Intermediate B.Sc. Exam., Lond. Univ. I am desirous of keeping in touch with all the recent work in connexion with the study of Chemistry, in order to fit me for my post of “ Teacher of Chemistry.” F. W. I)e Velling. Harry Thompson, T. Luxton. R.. J. Porter. T. A. Nightscales. 37 Bissett, Crellyn Colgrave, 10, Claremont Place, Sheffield. Student. B.Sc. (Lmdon), Chemistry being one of the subjects. B.Met. (Sheffield), with Honours. At present Honours Student in Chemistry at Sheffield University. W. Palmer Wynne. J. Kenner. W. E. S. Turner. W. J. Jarrard.C. R. Young. Brier, Albert, 19, Alexander Road, Ulverston, Lanes. M.Sc. (Chemistry), Leeds University, B.Sc. (Chemistry and Physics), Victoria University. Senior Science Master, Ulverston Victoria Grammar School, and Lecturer in Chemistry, Ulverston Evening School. Arthur Smithells. H. M. Dawson. J. B. Cohen. G. H. Daniel. W. Meredith, Burr, Percy Charles, Essex Lodge, Ravensbourne Park, Catford, S.E. Teacher of Science. Obtained First Class Honours in Chemistry at London B.Sc., 1912. Has studied Chemistry during the last three years at the Goldsmiths’ College, New Cross; desires to undertake Chemical Resekch. Arthur Lapworth. R. W. L. Clarke. George Barger. Geo. Jas. Woods. Arthur J. Ewins. Christie, John Hugh, c/o Dr.Bean, Crossgates, Near Leeds. Pupil of the Leeds City Analyst. B.Sc. (Loud.), Honours in Chemistry (2nd Class). Formerly a schoolmaster (taught mathematics and science). At present a pupil of T. Fairley, Esq., Public Analyst, Leeds. Arthur Smithells. B. A. Burrell. J. B. Cohen. Thomas Fairley. H. M. Dawson, F. G. Haymer. Clotworthy, Harold Reginald Septimus, 39, Trinity College, Dublin, Ireland. Research Assistant to W. H. Thompson, Sc.D., Professor of Physiology, Trinity College, Dublin, I received my training in the Chemical Laboratories of the Royal College of Science for Ireland and 38 Trinity College, Dublin, and I have the following degrees: B.A. (T.C.D.), B.Sc. (Lond.), A.R.C.Sc.1. Emil A. Werner. Wm. Caldwell.Hans Krall. Arthur Wallace. Sydney Young. Cockshutt, John Albert, M.Sc., Senior Science Master, Queen’s College, Taunton, Somerset. B.Sc. with Honours in Chemistry, Manchester University, 1911 ;M.Sc. by Research, 1912. Harold E. Dixon. Ch. Weizmann. Gilbert J. Fowler, E. C. Edgar. W. H. Perkin. Cutbush, Charles George, 59, Byne Road, Spdenham, Kent, Chief Assistant of Testing at the City of London Electric Light Co.’s Power Works, Bankside. For 8 years past in charge of Chemical Laboratory at above works; 16 years with Company as Testing Assistant. Student at Regent Street Polytechnic (2 years Evening Courses) ; student at Borough Polytechnic (3 years Evening Courses). F.Mollwo Perkin. H. Burrows. Charles A. Keane. M.aC. Lamb, Walter Hibbert.Davies, Daniel Jmes, 177, Le Marchant Road, St. John’s, Newfoundland. Vice-Principal, Methodist College, St. John’s. Analyst to the Depart. of Agriculture and Mines, Newfoundland. B.Sc. (Wales) in Chemistry, Metallurgy and Assaying, Geology. July, 1904--May, 1805, Assistant Analyst and Assayer to Messrs. Edwd. Riley & Co., 14A, Finsbury Square, London, E.C. Taught Chemistry, Sept., 1903--July, 1904, Whitland County School. May, 1905-Sept., 1905, Demonstrator in Chemistry, Swindon Education Committee. Sept., 1905-July, 1911, taught Chemistry, Llandyssul Intermediate School. A. A. Read. Claude M. Thompson. E. P. Perman. Edwd. Riley. Robt. D.AbeZZ. Doumin, Roland, 76, Tannsfeld Road, Sydenham, S.E. After receiving a general classical and scientific education at school, I was for some time in the laboratories of Messrs.Jeancrtrd Fils, and under M. Satie, where I received a thorough training in the Chemistry and Technology of Essential Oils. I am desirous of 39 keeping in touch with modern research on the subject, and am anxious to have the benefit; of the Sxiety’s publications. John C. Umney. Edgar Neumann. Edwin Harrison. Hubert E. Burgess. Ernest J. Parry. Edmondson,James Henry, 93, Manchester Road, Bolton. Chief Assistant to the Manager and Chemist, Bolton Corporation Sewage Works. Passed through a course of Evening Lectures and Laboratory Work in Pure and Applied Chemistry, Physics, &c. (period 5 years), at Manchester Technical School.Engaged in varied analytical work, and research on the Purification of Sewage, under Dr. Fowler, F.I.C., at the Manchester Sewage Works, for a period of seven years. Edmund Kn echt. Ja8. Grant, F. 8. Sinnatt. F. G. Richards. W. E. Speight. 8. J. Peachey. Elliott, Thomas Lenton, Lincoln House, Heckmondwike, Yorks. Technical Chemist (Textile Industries). Formerly Senior A &stant to Messrs. Cannon and Newton, Analysts and Assayers, and Consult- ing Chemists of Mincing Lane and Love Lane, London, E.C. (Business now discontinued). The Candidate is well known amongst Naturalists’ Societies in the West Riding of Yorks as a lecturer on biological chemistry and on applications of chemical science to questions of Natural History in general.The Candidate chiefly desires election to regularly receive the publications of the Society, R. S. Cahill. R. T. Marshall. C. E. Womersley. A. G. Green. H.B. Cooper, Evans,Ulick Richardson, The Keir, The Common, Wimbledon. Consulting Electrochemist at 28 Victoria Street, Westminster. Cam-bridge University Natural Science Tripos, Part I,First Class Honours ; Part II., Second Class. Samuel Rideal. C. T. Heycock. W. J.Pope. W. H. Mills. F. W. Dootson. 40 Garrett, Albert Edward, Yaverland,” Clarence Road, St. Albsns, Herts. Analyst and Scientific Adviser to the Dr. Jaeger Sanitary Woollen System Go., Ltd., 95, Milton Street, E.C. B.Sc. (by Research) Lond. Author of : Periodic Lnw,:International Scientific Series ; Advance of Photography, Kegan Paul & Co.; Fibres for Fabrics, Hodder and Stoughton.Original papers read at Physical Society of London : (1) ‘‘Chemical Decomposition and Electricsl Conductivity ” ; (2) “ Electrical Conductivity Produced by Heating Salts ” ; (3) “ Effect of Radiations on the Brush Discharge ” ; (4) ‘‘Positive Electricity Produced by Heating Salts.” Isaac Sydney Scarf. George W. Neal. E. J, Jackman. J. Lewkowitsch. Edward Gardner. Ghose, Tin Kari, 23/1 Baniatola Street, Hatkhola P.O., Calcutta. Assistant Analyst, Calcutta Corporation. (1) B.A. (Calcutta University) ; (2) L.M.S. (Calcutta Medical College) ; (3) Assistant Analyst, Calcutta Corporation-Analysis of water, food and drugs is done here; (4) Consulting Chemist to B.K. Paul & Co.’s Research Lahorstory, where preparations of indigenous drugs are manufactured. T. N. Majumdar. D hirendanat h Mitra. S. N. De. David Hoopr. G. D. Hope. Gilmour, Robert,B.Sc., Ph.D., Scores Villa West, St. Andrews. Carnegie Research Fellow, Graduated B.Sc., 1908, St. Andrews University. Papers with Prof, J. C. Irvine : “Constitution of Glucose Derivatives,” Parts I and II.,J.C.S., 19OS, 93,1429, and 1909, 95, 1545. 1909-1 1, studied at Wiirzhurg ; 1912, Ph.D. Wuraburg. Thomas Pnrdie. William S. Denham. J. C. Irvine. W. N. Haworth. J. L. A. Macdonald. Gray, George Watson, 8, Inner Temple, Liverpool. Analytical and Consulting Chemist. Fellow of the Institute of Chemistry. Author of papers relating to Chemical Analysis.J. E. Stead. P. W. Harbord. Boverton Redwood. H. A. Auden. Itobert Redwood. James Smith. 41 Henville, Douglas, 67, Glencoe Street, Newington, Hull, Yorks. Analyst. Associate of the Institute of Chemistry. Lecturer in Technical Chemistry at the Hull Municipal Technical College. Two years in the laboratory of R. A. Cripps, Esq., F.I.C., Brighton. Two years and a-half at University College, Nottiogham. Three months as locum tenens, to lecture in Dairy Chemistry and carry out agricultural analyses, at the Midland Agricultural and Dairy College, Kingston, Derby. Three years and a-half as assistant analyst and bacteriologist at the City Laboratories, Hull. Arnold R. Tankard Geo. H. Appleyard. John Evans G.E. Scott-Xmith. Jccs. I: Stevenson. Hewitt, James Arthur, B.Sc. (St. Andrews), 3, South Bridge Street, St. Andrews, Fife. Assistant to the Professor of Physiology, the University, St. Andrews, Fife. As my teaching and research work include physio- logical chemistry, I am desirous of keeping in touch with the Society’s work and publications. J. C. Irvine. Thomas Purdie. William S. Denham. G. Druce Lander. W. N.Haworth. Holt,William Joseph, 31, Spruce Hills Road, Walthamstow. Teiching. Interested in chemistry,and desire to keep up to date in the subject. J. T. Hewitt. W. H. Ratcliffe. Clarence Smith. A. D. Mitchell. Frank G. Pope. Arthur E. Pitt. Howells, Alfred Leslie, “Bank Field,” New Mill Road, Holmfirth, West Riding, Yorkshire.Assistant Schoolmaster. B.Sc. (London), First Class Honours in Chemistry at Final (October, 1910) ;South Kensington Honoursman in Chemistry (1910) ; Drapers’ Science Scholar, East London College (University of London), September, 1907, to July, 1910. Science Master in the Secondary School, Holmfirth, Yorksbire. Lecturer on Chemistry in the Holmfirth Technical Institute (September, 1911, to the present time). J. T. Hewitt. Clarence Smith. Frank G. Pope. J.J. Fox. ArtAur E. Pitt. 42 Kirkland, Thomas James, B.Sc., Hereward Hall, Ely, Cambridgeshire. First Science Master, King’s School, Ely. Educated at West minster School and King’s College, London. Since January, 1906, have been First Science Master at King’s School, Ely.In addition to teaching work have been engaged in Analytical work connected with the Printing Industry. John M. Thomson. Herbert Jackson. Patrick H. Kirkaldy. B. Middleditch. Henry L.Smith. Leitch, Peter Thomas, c/o John Edgar, Esq.,176, West George Street, Glasgow. Assistant to R. R. Tatlock & Thomson, Public Analysts, Glasgow, from August, 1905, to February, 1911. Student at the West of Scotland Technical College, Glasgow, for Iron and Steel, Assaying nud General Chemistry. Sometime Assistant to the Canada Cement Co., Limited, at Plant No. 2, Montreal, Qua, and Plant No. 12, Exshan, Alberta. At present, Chief Chemist at Plant No. 12, Exshan, Alberta. It. R. Tatlock. Harry Dunlop. R. T. Thornson. G. G. Henderson.Thomas Gray. Lloyd, Daniel William, The Manse, Ormonde Road, Kilkenny. Senior Instructor in Science and Mathematics, City Technical School, Kilkenny. B.Sc., University of London. Senior Demonstrator in Chemistry and Physics, etc., Technical School, Kilkenny. Consult-ing Analyst for the St. Francis’ Abbey Brewery, Kilkenny. Analyst for the Woollen Mills, Kilkenny, in 1909. Analyst for Motor Factory, Patrick Street, Kilkenny, 1910. J. Wood ward. Beresford Ingram. E. Towyn Jones. J. H. Robbins. Robt. D. Abell. J. W. Shepherd. John Evans. A. E. Middleton. Lopes, Walter Cyril, Eastfield, Comberton Road, Kidderminster. Analytical Chemist to Messrs. J. P. Harvey & Go., Ltd., Chemical Manure Manufacturers, etc., and Assistant to Joseph Lo~es, F.I.C., F.C.S.I have had five years’ experience in analytical work in metallurgy, fertilisers and feeding stuffs, and for the last two and a-half years in food and drugs in the Laboratory of the Public Analyst for 43 Smethwick. Of late years I have devoted considerable time to the study of electricity in its relation to chemical science. I have also had a great deal of experience in the analysis of waters and sewage. Cecil Duncan. Ernest J. Panay. J. Stewart Remington. Chas. J. Waterfcdl. Arthur Adams. Fredk.O’Brien. Macbeth,Alexander Killen, M.A., B.Sc., 3, Victoria Terrace, Cregagh, Belfast. Demonstrator in Chemistry. Senior Scholar in Chemistry, 1911-22. Andrews Student, 1912. First Class Honours in M.A. (Q.U.B); First Class B.Sc.(gold medal), Q.U.B. Appointed Senior Demonstrator in Chemistry, Queen’s University, Belfast, 191 2. Has contributed to Proceedings and Transactions of the Society. E. A. Letts. C. R. Cryrublo. Samuel Smiles. A. W. Stewart. R. Wright. Martin, Henry Staphen, 64, Dyke Road, Brighton, Sussex. Pharmacist, M.P.S. I received my early training as a student iu an analytical laboratory; engaged for the pa& thirty-five years in the manuFacturing and dispensing of all kinds of pharmaceutical com-pounds. Greatly interested, and have conducted investigationst in the manufacturing of mineral and aerated waters. For knowledge, have been awarded Gold, Silver, and Bronze Medals, also three Diplomas, and three Certificates of Honour and Merit, and still continue my researches as a chemist.Chas. Umney. C. T. Bennett. John C. Umney. WiZliana Xtevenson. Arlhur W. Crossley. MaudeJAylmer Henry, Great Baddow, nr. Chelmsford. Chemist. I studied Chemistry at Pinsbury Technical College, obtained their Certificate, studied an additional two years and obtained the Associateship of the Institute of Chemistry. I have worked as Assistant Chemist to Mr. M.J. Cannon and to Messrs. S. Courtauld & 00. Matthew J. Cannon. Arthur J. Hale. Sidney S. Napper. G. Francis Morrell. R. Meldola. 44 May, Joseph Horsnell, 21, Donovan Avenue, Muswell Hill, N. Electro-chemical Engineer. Member Institution Electrical Engin- eers. Chief Chemist and Laboratory Superintendent from 1893 to 1910; Chief Chemist and Works Superintendent, 1910 ; Chief Engineer (with control of all chemical and technical work), 1911-Electrical Power Storage Company, Ltd., Storage Battery Manu-facturers, Consulting Chemical Engineer, 1912-1 3.Walter A. Voss. John J. Pilley. E. R. Buggd. Xpencey Pickeying. Arthur P. Strohmenger. Mumford, Ernest Joseph, 67, Hatherley Road, Walthamstow, N. €3. Teacher. Made a special study of Chemistry. I wish to keep up to date in the subject. J. T. Hewitt. Clarence Smith. Frank G. Pope. A. D. Mitchell. Arthur E. Pitt. Murphy, Paul, Burnside, Sidcup, Kent. Analyst. Studied Chemistry at the City and Guilds Technical College, Finsbury, under Professor MeIdola for four years, taking full course and obtaining the Diploma on leaving.Fellow of the Institute of Chemistry. Asaistt.int to Dr. Bernard Dyer, of 17, Great Tower Street, E.C. Raphael Meldola. J. F. H. Qilbard. Bernard Dyer. Frank W. G. King.B. H. Buttle. Naylor, Jonathan Harold, 73, Castle Street, Bolton, Lancashire. Senior Chemistry Master, Secondary School, Widnes, 1912. First Assistant, Chemistry Department, Mining and Technical College, Wigan, 1907-1912. Have passed through the 3 years’ course in the Honours School of Chemistry, at Manchester University, and one year’s research work. Obtained the degrees of B.Sc. (Honours in Chemistry) and M.Sc. Obtained the Associateship of the Institute of Chemistry, 1912. Harold B. Dixon. Ch. Weizmann.W. H. Perkin. Norman Smith. E. B. Naylor. 45 Nolan, Thomas Joseph, 32, Newmarket, Dublin. Research Student. M.Sc. with First Class Honours, National University ;Travelling Student in Chemistry of the National Uni-versity. Demonstrator in Chemistry at University College, Dublin, and joint author of papers published in the Proceedings of the Royal Irish Academy and in the Proceedings of the Chemical Society. William Ramsay. Samuel Smiles. J. Norman Collie. N. T. M. Wilsmore. W. C. McC. Lewis. Pollard, Cornelius Theodore, 21, Wharncliffe Road, Broomhall Park, Sheffield. Student. B.Sc. (Sheffield), Chemistry being one of the subje:ts. At present, student for M.Sc. (Chemistry) at Sheffield University. W. Palmer Wynne.J. Kenner. W. E. S. Turner. W. J. Jarrard. C. R. Young. Rae, William Norman, Colombo, Ceylon. Lecturer in Science, Royal College, Colombo. Corpus Christi College, Cambridge, 1905-8 ; Second Class Honours, Part I., Nat. Science Tripoe, Camb., 1908. Science Master, Cranbrook School, Kent, 1908-11. Scienc~ Lecturer, Royal College, Colombo, 191 1. A. F. Joseph. E. C. Browning. Thomas Cockerill. M. Kelway Bamber. A. Bruce. Roskin, Hermann Horace, 11, Newlands Road, Middlesbrough. Assistant Science Master, Middlesbroagh High School ; Lecturer in Chemistry, Middlesbrough Evening Technical School. B.Sc. (Wales) : subjects-the Metallurgical group (Inorganic Chemistry, Metallurgy, and Geology). Distinctions in Advanced Chemistry at the Central Welsh Board Senior Examination.Seven years’ experience as Teacher and Lecturer of Theoretical and Practical Chemistry (appointments other than above being : Assistant Science Master, County School, Ebbw Vale, Mon., and Senior Science Master at the Grammar SchQal, Wotton-under-Edge, Glos.). R. B. Wight. H. Frankland. J. E. Stead, Ernest W.Jackson. C. H. Ridsdale. Simpson, William Slessor, Dynamite Factory, Somerset West, South Africa. Analytical aod Research Chemist, C rpe Ezplosives Works, Somerset West, South Africa. M.A. (Abdn.); B.Sc. (Abdn.), with special distinction in Chemistry ant1 Geology. For eight yews (1904-12) an Assistant Research Chemist in the Research Department, Royal Arsenal, Woolwich. F. R.Japp. Robert Robertson. William Ramsay. Alfred C. G. Egerton. W. H. Gibson. Smith,Jobn Walter, 48(a), Hurstbourne Road, Forest Hill, S.E. Teacher in London County Council service. Obtained 2nd Class Honours in Chemistry at London B.Sc., 1912 ; has worked for the last four years at Goldsmiths’ College, New Cross, and now desires to undertake chemical research, Arthur Lapworth. R. W. L. Clarke. George Barger. Geo. Jas. Woods. Arthur J. Ewins. Taylor,Harold Victor, Royal College of Science, London. At present Student (adv. work) ; Chemistry Lecturer (1907-1910) at Hurst Grammar Schoal, ‘L’aunton ;Chemistry Student (1910-19 12) at R.C.S. (London) ;Degree in Chemistry, A.R.C.S. Research work (1912) : “Enzymes of the Pitcher fluid of the Nepenthes plant.” H.F. Harwood. M.0. Forster. James C. Philip. H. Brereton Baker. Chapm sn Joned. Thompson,Percy James, The Avenue, Clytha Square, Newport, Mon. Student of Agricultural Chemistry ;sometime Lecturer in Analyti-cal Chemistq. 1906-7, Student of Pharmaceutical Chemistry at Metropolitan College of Pharmacy, Lmdon ; 1907-8, Student at Bath and West of England College of Chemistry and Pharmacy; 1908-1 1, Lecturer at the latter college-engaged with D. J. Willinme, F.C.S., Ph.C., in analysis of foodstuffs, sewage, etc. ; 1912, specialising in Agricultural Chemistry; Student at the Summer School of the Royal Agricultural College, Cirencester (passing the examination in Agricultural Chemistry) ;Silver Medaltist in Chemistry and Pharmacy ; Qualified as Pharmacist and Member oE the Pharmaceutical Society.Desirous of keeping abreast of modern research. David J. Williams. D. 4. Chpfmaln. John M. H. Munro. B. Lambert. J. Griffin. M. P. Applebey. Turner, Bertrand, 55, Golden Hillock Road, Birmingham. Research Student, University of Birmingham. Passed final examinations for B.Sc. (Birmingham). Chemistry Principal. Percy F. Frankland. Edward P. Frankland. Hamilton McCombie. C. I(.Tiukler. J. E. Coates. Frederick Challenger. Turnill, Thomas Wiloughby, Stibbington, Wansford, Northamptonshire. Chemist and Works’ Manager. Pupil of W. Elborne, M.A., Public Analyst, Peterboro’ ;then Assistant Chemist, Hull Stearine Co. ; Chemist and Departmental Manager at Messrs. Major, Tar Distillers, Hull; Manager and Chemist at Works at Stoke Ferry, Norfolk, manuf.sulphate of ammonia from peat. Two years Chief Assistant to J. A. Foster, F.I.C., Public Analyst, E.R. Yorks., etc., and at present am Chemist and Works Manager at Atlas Preservit- tive Co., Deptford, S.E. Thos. Luxton. Ambat Kesava Menon. Edwin B. Atkinson. T. P. Parkes. C. E. Cooke. Webb, Edward, Berwyn, Totteridge, Herts. Lecturer (Chemistry), Islington L.C.C. Training College, Offord Road, Barnsbury, N. B.Sc. (London). Chemistry Lecturer (6 years) Islington Training College (L.C. C.). Formerly Science Master Fins- bury (L.C.C.) Pupil Teachers’ Centre (9 years). George W. Neal. Jos. S. Bridges. James Swain. Prank E. Weston. H. R.Ellis.Wilson, Siddons Siddons, 154, Burges Road, East Ham. Analytical Chemist to The British Oil and Cake Mills, Ltd., 29, Great St. Helens, E.C. Assistant Chemist in The British Oil and Cake Mills laboratory for ten years. J. Lewkowitsch. A. E. Dunstan. F. 33. Thole, R. W. Wilson. A. J. Harvey. 48 Wood, Hubert Rogers, c/o Messrs. Fenner & Alder & Co., Ltd., Millwall, E. Works Chemist. Three years pupil to Mr. Harry Thompson, F.C.S., Hull. Two years Chief Assistant Chemist at the Hull Stearine and Warehousing Co., Ltd., Hull. One and a-half years Assistant Chemist at Blundell Spence & Co., Ltd., Hull. Four years (and present situation) Chief Chemist at Fenner & Alder & Co., Ltd., Paint Manufacturers, London. Desire to be admitted as a Fellow of the Society for the use of Journal and Library as a great help in my study and general analytical and chemical work.Karry Thompson. Arnold R. Tankard. Geo. H. Appleyard. T. Luxton. T~os.A. flight8CC6kS. The following Certificate has been rruthorised by the Council for presentation to ballot under Bye-law 1(3) : Parker, Jonathan, c/o The Wattle Extract Go., 42, Anglo-African Home, Durban, S. Africa. Analytical Chemist. Junior Assistant to Dr. Hellon, Public Analyst, Whitehaven. Chemirt to the St. Helens Colliery Co. Workington, and in charge of the Chemical Department of the Bye-Products Recovery Plant. Held similar post with the Moresby Coal Go. Chemist to the Wattle Extract Co., Durban, Natal. Robert Hellon. W. H. Watson. Henry R. Proder. J. Tcherniac. &. C1,AY AND SONS, LTD., BRUNSWICI ST., STAMFORD ST., S.E., AND BUNGAY. SUFFOLB.
ISSN:0369-8718
DOI:10.1039/PL9132900021
出版商:RSC
年代:1913
数据来源: RSC
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