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Proceedings of the Chemical Society, Vol. 19, No. 271 |
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Proceedings of the Chemical Society, London,
Volume 19,
Issue 271,
1903,
Page 235-270
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Issued S8/11/03 PROCEEDINGS OF THE CHEMICAL SOCIETY. VOl. 19. No. 271. Wednesday, November 18th, 1903. Professor W. A. TILDEN,D.Sc., F.R.S., President, in the Chair. Cert,ificates were read for the first time in favour of Messrs. Allan Baguley, B.Sc., University College, Bangor. James Rocheid Forrest, D.P.H., Kirkee, near Poona, India. Harry James Glover, 33, Albert Road, Stroud Green, N. John Augustus Goodson, 19, Darnley Road, Hackney, N.E. Alfred Henry Hoit, 4,Montgomerie Road, Southsea. Bernard Middleditch, B.A., Woodcroft, Harrow-on-the-Hill. Bertram Prentice, Ph.D., D.Sc., Royal Technical Institute, Salford. Frederick Henry Streatfeild, 9, Crescent Road, South Tottenham, N, William Wood Underhill, 10, Hartham Road, Holloway, N. Francis Langston ?Vatt, 111,Lauderdale M.ansions, Maida Vale, W.The PRESIDENTannounced that the Librarian had reported that the following books were missing from the Library : Lunge, G. A treatise on the distillation of coal-tar and ammoniacal liquor and the separation from them of valuable products. London 1882. Ganot, A. Elementary treatise on physics. Trans. by E. Atkinson. 6th edition. London 1873. Muir, M. If.P. The alchemical essence and the chemical element. An episode in the quest of the unchanging. London 1894. Pamphlets, Vol. 6. Centralblatt fur Bakteriologie. Bd. 23. He would be glad if Fellows would do what they could to assist the Librarian in recovering these missing volumes. 236 Of the following papers, those marked * were read : *149.The union of carbon monoxide and oxygen and the drying of gases by cooling.’’ By A. F. Oirvan. The following experiments were made in order to investigate whether the drying of an explosive mixture of carbon monoxide and oxygen by exposure to low temperatures was sufficient to prevent chemical union taking place when the gas was sparked after it had regained the ordinary temperature. A small glass gas-holder containing the explosive mixture was sealed to the following apparatus arranged in series: (1) a small bubbler containing water, (2) a stopcock, (3) a vertical glass spiral, (4) a glass tube, one centimetre in diameter, furnished with platinum terminals with a spark gap of about 4 mm., (5) a stopcock, (6) a Topler pump. Stopcocks were sealed as side-tubes between (2) and (3) and between (5) and (6).The carbon monoxide was prepared by the interaction of ‘(pure ” sulphuric and formic acids, the oxygen being obtained by heating potassium permanganate ;the gases were collected and stored over water and the proportion was correct to within 1per cent. A slow current of air was aspirated through the apparatus by means of the side-taps, while the whole apparatus between them was thoroughly heated. The spiral was then surrounded by a freezing mixture and the tube between it and the pump was heated to the softening point of the glass. After some time, the current of air was stopped and the heating discontinued, The apparatus was then completely exhausted as far as the bubbler by means of the Tapler pump and the explosive mixture slowly admitted at the rate of one bubble per second.When the gas in the apparatus was under atmospheric pressure, the tap of the gas-holder was closed and sparks from an induction coil were passed through the explosion tuba in which the gas was now at the temperature of the atmosphere. In the first experiments, where liquid air was used, care had to be taken that this cooling agent was not too fresh, as it WAS then sufficiently cold to liquefy the explosive mixture. No explosion took place on passing sparks from an induction coil which, at the same time, was giving 12 rnm. sparks in the air, although the sparks in the gaseous mixture were usually surrounded with a little ball of blue flame.When the glass spiral was allowed to regain the ordinary tem- perature, the moisture which had been condensed in the spiral slowly diffused into the explosion-tube and a single spark exploded the mixture with a sharp report. 257 On sparking the mixed gases which had been cooled in a mixture of solid carbon dioxide and alcohol ( -SO'), there was no explosion, and the littIe ball of flame round the sparks had much the same appearance as when the gases bad been dried at -180°, but when the glass spiral had acquired the ordinary temperature, a single spark produced a sharp explosion. When the gaseous mixture had been cooled to -15" and allowed to regain the ordinary temperature, the first spark always caused an explosion, but this did not occur after cooling below -50'.When dried between -50" and -35', faint sparks did not, as a rule, cause the mixture to explode, although powerful sparks always produced this effect. The freezing mixture employed was either liquid air or solid carbon dioxide in alcohol, and when kept in a vacuum-vessel its temperature rose only about half a degree per minute, even when a current of air was passing through the spiral. A single powerful spark, when passed through the mixture (after drying between -50" and -35O), frequently produced no effect, whereas an explosion always occurred on passing the second or third spark. The explosion produced by powerful sparks in the gases dried between -50° and -35O is of a very different character from that obtained with the wet gases; the latter is very quick and violent and gives a metallic click, but the former takes place quietly, and the explosive wave often travels quite slowly along the tube (compare Dixon, Phi,?.Tmns., 1884, 175, 11,630).The wave pro- ceeding from these feeble explosions always stopped directly it reached the cold part of the spiral, and the gas in this part of the apparatus was found to be unaltered, but when the gas was moist and the spiral at the ordinary temperature, the explosion passed to the furthest part of the apparatus. The platinum terminals were now replaced by (1) a silver wire, (2) a gold wire : each of these was heated to redness and then fused by an electric current, without causing any visible union in the explosive mixture, which had been dried at about -80°.In order to find out whether platinum mould act catalytically on the dried or partly dried gases (compare Dixon, Zoc. cit.), a tube, in which the platinum terminals mere replaced by a coil of platinum wire, was sealed in place of the sparking-tube and the apparatus dried as before. The explosive mixture was then allowed to enter through the spiral, which was kept at various temperatures. With a mixture dried at about -35", the platinum acted catalytic- ally, and in becoming heated to redness brought about a quiet and feeble explosion. When, however, the mixture was dried at temperatures between -SOo and -180°, the platinum still acted 235 catalytically and glowed for several seconds, but there was no other sign of chemical action.After the glowing had ceased, the coil was kept at a white beat for several minutes by means of an electric current, and the gas was then pumped off and collected. About one- eighth of the gaseous mixture was absorbed in caustic potash solution and the residue was still explosive, showing that combination was far from complete. At Sir William Ramsay's suggestion, the author calculated the amount of moisture present in the mixture after cooling (compare Trans, 1886, 49, 46), the following data being employed : Temperatures ......... -61" -56.5' -51' -45' -36' Pressures in mm. ....,. 0.008 0.01 50.039 0.052 0.160 When the vapour pressure of the water is less than about 0.03 mm., as is the case with the mixture after cooling at -5O', the gases will not explode.When the vapour pressure is less than about 0.16 mm., the explosion is very feeble. In the first case, the amount of water vapour present is about one part in twenty-four thousand by volume, and in the second, one part in five thousand. At -6l0, the amount of water vapour would be about one part in a hundred t,housand of gas. It would appear then that the mixture will not explode when sparked at the ordinary temperature if there is less than one mol. of water vapour to twenty-four thousand mols. of the gas. These figures must, however, be taken as being only approximate, since below -50° the vapour pressure of ice falls to half its value for a decrease of about 'I",and, moreover, it is not known whether the glass of the apparatus exerts any drying effect on the contained gas.DISCUSSION. Sir W. RAMSAYpointed out the interest of Mr. Girvan's experiments in connection with surface-layers on glass. The water-vapour in contact with the water-layer on the glass must have a vapour-pressure comparable with, or less than, the vapour-pressure in contact with ice at -185". This film is removed on heating the glass in a current of dry air, and is not removed when the mixed gases, dried at -60°, are allowed to enter the dried tube. Such questions are of very great interest from the standpoint of molecular physics, and -Mr. Girvan, he knew, hoped to attack these and similar problems at an early opportunity.Dr. SCOTT suggested that the water which adhered to the glass might be there not as a gaseous layer but either as a hydrated silicate or in combination with alkali. 239 WO. ‘(Simplification of Zeisel’s method of methoxyl and ethoxyl determinations.” By W. R. Perkin. In this process, a long-necked distilling flask was employed without any other condensing arrangement, the tube for the current of carbon dioxide being passed down the neck to within a short difjtance of the hydriodic acid. It was eventually found that as long as the tempera- ture of the glycerin bath was so adjusted that actual distillation of the acid into the delivery tube did not take place, no appreciable quantity of hydrogen iodide passed rforward into the silver nitrate flasks, The acid used boiled at 126O and had a sp.gr. oE 1.68 ap-proximately. The following arrangement has been found to prevent the silver nitrate eolution from being sucked back into the distilling flask after a sudden ebullition of hydriodic acid. Two small flasks are used as usual, but the tube conducting the carbon dioxide and methyl iodide vapour, instead of passing into the silver solution, is kept some distance above its surface. The flasks are then connected with a siphon tube, one arm of which reaches to within a short distance of the solution in the first flask, whilst the other arm dips a little below the surface in the second. By this arrangement, the methyl iodide is chiefly absorbed by the surface of the silver solution, but any escaping is caught as it bubbles through the second quantity, then, if any such drawing back takes place, some of the solution passes into the first flask, and as soon as the pressure increases is forced back again into the second.This method of determining the methoxyl group gave very good numbers and can be used equally well for determining the ethoxyl group, but in this case the numbers are not usually so accurate, being generally a little less than the calculated quantity, ”151. “The rusting of iron. Part 11.” By G,T.Moody. The author has further investigated the causes of the rusting of iron, more particularly with reference to the influence of soluble substances, and finds that the salts of strong acids, such as sodium chloride and sulphate, potassium sulphate, ammonium sulphate, magnesium chloride and sulphate, calcium chloride and sulphate, and potassium chlorate have no retarding influence on rusting. These salts do not combine with and are not decomposed by carbonic acid.Com-pounds which inhibit rusting may be divided into two classes. The first contains substances having an alkaline reaction, such as sodium carbonate, hydroxide, phosphate and borate, ammonium carbonate, and 240 barium and calcium hydroxides, all of which directly absorb and com- bine with carbonic acid. The second class includes salts of weak acids, such as potassium and sodium nitrites, sodium formate, sodium acetate, potassium ferrocyanide and chromate.These salts are all decomposed by carbonic acid. Sodium nitrite solution, for example, after exposure to air becomes alkaline and contains sodium carbonate. A solution of 10 grams of the nitrite, through which a slow stream of carbon dioxide was passed for 9 days, contained 1.585 grams of sodium car5onate. Similarly, potassium ferrocyanide solution, when exposed to air, slowly evolves hydrogen cyanide and becomes alkaline. This change occurs more rapidly when carbon dioxide is passed through the solution, the escaping gas having the odour of hydrogen cyanide and precipitating silver cyanide from a solution of silver nitrate. Potassium ferri- cyanide is a salt of a weak acid which exceptionally does not appear to retard rusting.This substance is, however, reduced by iron whether its solution be exposed to air or not, the metal becoming covered in either case with a mass of insoluble, greenish-blue cyanide, It may therefore be concluded that the influence of any particular compound on the atmospheric rusting of iron depends on its behaviour towards carbonic acid, and that only those substanoes which combine with or are decomposed by carbonic acid inhibit rusting. Dunstan has stated (Proceedings of the Royal Artillery Institution, 1899, 5,26, and this vol., p. 150) that the metals which rust in air are oxidised by hydrogen peroxide, whilst those which are not oxidised by this reagent do not rust in air. Iron, zinc, and lead are cited as examples of the first class, and copper, silver, and nickel as types of the second.It is noteworthy that iron and zinc rapidly decompose aqueous carbonic acid, whilst copper, silver, and nickel are indifferent to the acid. Having regard to this, and also to the fact that Giorgis (Guxxettcc, 1891,21,510)has shown that hydrogen peroxide, when carefully freed from carbon dioxide, is practically without action on magnesium, it appeared probable that iron would not be oxidised by pure hydrogen peroxide. The author has investigated this question by leaving a specimen of distilled hydrogen peroxide in contact with iron for four- teen days. No oxidation of the iron was observed, but on adding to a further portion of the pure peroxide containing iron a drop of hydro- chloric acid or a solution of carbon dioxide, hydrated ferric oxide was formed.In the light of the experiments described, the aerial rusting of iron cannot be attributed to hydrogen peroxide, but must be regarded as a change involving the interaction of iron and acid and subsequent formation of rust by the oxidation of ferrous salt. 241 DISCUS#10N. Dr. RIDEALremarked that Muntz had shown (Compt. rend., 1891, 112, 1142) that calcium nitrite in-sterilised soil gave off nitrous acid rapidly in presence of carbonic acid, and that he had noticed this re- action in bacterial sewage filters. Mr. W. A. DAVISpointed out that the decomposition brought about in aqueous solutions of sodium nitrite and potassium ferro- cyanide, although at first sight surprising, was a neuessary consequence of the principle of mass action.As both nitrous and hydrocyanic acids are volatile, the conversion of their salts into carbonates by an excess of carbonic acid should be complete after a sufficient interval of time. Dr. MOODY,in reply, said that the sodium nitrite used, which was a well-crystallised specimen, having a high degree of purity and quite free from carbonate, mas so sensitive to carbon dioxide that the gas, after passing through the solution, immediately reacted with potassium iodide and starch solution, 152. '' Constitution of ethyl cyanoacetate. Condensation of ethyl cyanoacetate with its sodium derivative." By F. G.P. Remfry and J. F. Thorpe. When ethyl sodiocyanoacetate is heated in alcoholic solution for 2 hours at 100" with a molecular proportion of ethyl cyanoacetate, a '70 per cent.yield of the compound, CN*CH,*HC(OEt)*O*CH(CN)*C0,E b, is produced, which crystallises from dilute alcohol in long needles, melts at 53",and distils with partial decomposition at 235" under 20 mm. pressure. On boiling with sodium carbonate solution, this substance dissolves, and, on acidifying the solution, the acid, CN*CH,*HC(OEt)*O*CH(CN)*CO,II, separates; it crystal lises from water in large prisms and melts at 142O with evolution of carbon diox- ide, being converted into a substunce having the formula (C7H1002N2)z, which crystallises from glacial acid in small, yellow needles having no definite melting point; on distillation, it gives rise to the cornpound CN*CH,*HC(OEt)*O*CH2*CN,separating from absolute alcohol in large prisms melting at 181O and boiling at 208O under 25 mm.pressure. The same substance is produced quantitativeIy if fhe ammonium salt of the acid melting at 142" is distilled under diminished pressure. Concentrated aqueous potash hydrolyses the substances melting at 53" and 142O, forming malonic acid ;the compound melting at 181', when similarly treated, yields malonic and acetic acids. 242 When the sodium compound of the condensation product is heated directly with methyl iodide, the methyl compound, CNmCHMe*HC(OEt)*O*CH(CN)*CO,Et, is produced; it crystallises from dilute alcohol in small prisms, melts at 63O, and boils without decomposition at 220' under 20 mm.pressure. With sodium carbonate, the acid, CN*CHMe*HC(OE t)*O* CH(CN)*CO,H, is produced ;it crystallises from water in glistening plates, melts at 145' with evolution of carbon dioxide, and becomes converted into a compound, (C,H,,O,N,),, having no definite melting point, but which, on distillation, is converted into the substance, CN*CHMe*HC( OEt) *O.CH,.CN, crgstallising from absolute alcohol in small prisms and melting at 121'. The same substance is produced when the acid melting at 145' is boiled for some time with sodium carbonate solution, or when its ammonium salt is distilled. The substances melting at 63' and at 145' give, on hydrolysis with aqueous caustic potash, malonic and methyl- malonic acids ;the compound melting at 121° yields methglmalonic and acetic acids.When the sodium compound of the condensation product is treated directly with ethyl iodide, it is converted into the ethyl compound, CN*CHEt*HC(OE t) O*CH(CN)*C02Et, which crystalli ses from dilute alcohol in prisms, melts at 68O, and boils without decomposition at 215' under 20 mm. pressure. With sodium carbonate, it yields the ad, CN*CHEt*HC(OEt)*O*CH(CN)*CO,H,which crystallises from water and melts at 153O with evolution of carbon dioxide and becomes converted into an infusible substance having the formula (CSH1402N2)2. The latter compound, on distillation, gives rise to the aubstance CN-CHE t *HC(OE t)*O*CH,*CN, which crystallises from absolute alcohol in small plates melting at 115'.Complete hydrolysis of the above-mentioned substances melting at 68O and at 153O gives rise to malonic and ethylmalonic acids; the compound melting at 115O yields ethylmalonic and acetic acids. When the substance melting at 53' is treated with excess of sodium ethoxide and methyliodide, it is converted into the trimethyl corn-pound, CN*C( Me),*HC(OE t)*O*CMe(CN)*CO,E t, which crystallises from dilute alcohol in small needles and melts at 120'. Complete hydrolysis of this substance with aqueous potash gives rise to methyl- malonic and dimethylmalonic acids. The action of acidic hydrolytic agents on these substances, and the condition governing the formation of similar Condensation products from substituted ethyl cyanoacetntes, is under investigation.243 153. “The action of water and dilute caustic soda solutions on crystalline and amorphous arsenic,” By W. T. Cooke. Engel (Conzpt. rend., 1883, 96,1314) states that amorphous arsenic is unaltered in moist air, whilst the crystalline modification oxidises rapidIy. The author’s experiments were made with the view of ascertaining: (1) whether water alone had any action on either variety, (2) whether the action, if any, was increased by the presence of caustic soda, (3) and whether, in the presence of air, the crystalline variety dissolved to a greater extent in caustic soda solution than in water. Asnorphous Ars:nic.--The operations were carried out entirely in an inert atmosphere, the gas employed being either carbon dioxide or hydrogen, according as water or caustic soda solution was used.The main part of the apparatus consisted of two boiling tubes provided with condensers and also with tubes for the introduction of the gas. Hydrogen arsenide mas passed into one carefully dried boiling tube, so that arsenic was deposited on warming, The water or caustic soda solution contained in the other tube was freed from air by boiling and by passing through it a current of hydrogen or carbon dioxide. The pressure of the gas in the apparatus was then used to force over the solution into the tube containing the arsenic, after any remaining hydrogen arsenide had been expelled, The solution could then be boiled in contact with the arsenic for any desired time, and finally drawn off through an asbestos filter.The arsenic in the filtrate was usually estimated by titrating with iodine solution. The following results were obtained using 125 C.C. of distilled water : Time of boiling in hours ....... . ,.... . . 2‘5 1.5 2.5 8 4 Weight of dissolved arsenic in grams.,. 0.0020 0.0009 0’0004 0’0034 0’0013 0’0016 In the absence of air, the actionof water on amorphous arsenic is thus seen to be very slight. When air was aspirated through the boiling water for 65 hours in contact with the amorphous arsenic, only 0.0010 gram of the element was dissolved, hence the presence of air has no effect. In the absence of air, the effect of dilute caustic soda solutions was slightly greater than that of water, and the action increases with the 244 concentration of the alkali.Moreover, the action is not influenced bg the presence of air. In the absence of air. I In the presence of air. Weight of Weight of Concentra-Tilne of disiolved Coacentra-Time of dissolved tion. arsoiiicin 'lours* in grams. tion. boiling, arsenicin hours. in grams. N/100 1-5 0'0022 N/100 2.75 0'0014 5-3 0'0026 6-0 0'0014 N/50 3 '5 0.0021 N/50 2'5 0,0038 6'0 0 '0020 6-0 0'0010 "25 6-0 0.0038 A725 6-0 0.0046 6.0 0.0014 Crystalline Arsenic.-In this case, the boiling tube was provided with a side tubulure, through which the crystalline arsenic could be introduced, The arsenic was powdered and introduced into the apparatus as quickly as possible on account of the readiness with which the finely divided element undergoes oxidation. The volume of liquid used was 50 C.C.When distilled water was used and air excluded, about 0.0025 gram of arsenic dissolved in la to 1; hours. With distilled water in presence of air, about 0.0233 gram of arsenic dissolved in 14 hours. Hence the presence of air greatly increases the action in the case of the crystalline modification of the element, The following results obtained with caustic soda shorn that the alkali does not materially increase the action. In the absence of air. In the presence of air. Weight of Time of Weight of Coiicentra. Time of dissolved Concentra-boiling, dissolved tion. boiling, arsenic tion.arsenicin hours. in grams. in hours. in grams, N/lOO 6 0.0025 ~7001~ 6 0.0712 N/50 6 0'0016 h/50 6 0.0797 N/25 6 0'0030 N/25 6 0.0267 6 0.0017 By estimating the dissolved arsenic by the iodometric and gravimetria methods, it was found to be entirely in the form of arsenioas acid, The results seem to show that water either alone or in the presence of caustic soda has practically no action on arsenic. In the presence of air, however, direct oxidation takes place, If water is concerned in the oxidation, the formation of hydrogen arsenide might be anticipated: 2As+3H20 * As20,+6H, 2As+6H = 2AsH,; but this gas was never found in the foregoing experiments. Th. Panzer (Chern. Centr., 1903,ii, 821), has also shown that the oxida- tion of arsenic in moist air is due not to the decomposition of water, but to the intervention of free oxygen.154. LL Note on a double chloride of molybdenum and potassium.” By G. G. Henderson. According to Berzelius (Poggsndorf’s Annalen, 1826,6, 331, 339 ; 7,261), a chloride of molybdenum and potassium is obtained when the black liquid produced by the action of ;potassium amalgam on a solution of molybdenum pentachloride is evaporated to the crystal- lising point, and is described as a black, efflorescent salt, which, when redissolved in water, leaves a black powder, probably a basic salt. A definite duzcbZe chduride of molybdenum and potassium, having the formula 3KC1,MoC1,,2H20, has been prepared in the following manner : potassium amalgam was added, in small quantities at a time, to a solution of molybdic acid in excess of hydrochloric acid until the liquid had acquired a purple-black colour.The solution was concentrated and saturated with gaseous hydrochloric acid, when successive crops of crystals were obtained ;the first was composed of potassium chloride alone, the second of a mixture of potassium chloride with red crystals of the double salt, and the third of the double salt alone, The red crystals were collected, washed with fuming hydrochloric acid, dried by pressure between folds of filter paper, and analysed with the follow- ing result : Found : Mo = 21.39 ; C1= 45-46 ; K20= 7.47. 3KCl,MoC1,,2H2O requires Mo= 20.92 j Cl= 45.80 ;H20=7.80 per cent. The new salt, which crystallises in garnet-red prisms, is fairly easily soluble in cold water, without any apparent decomposition, giving a deep red solution. In the dry state, the salt is quite stable, but it decomposes in aqueous solution, slowly in the cold, but quickly on boiling ; this decomposition is prevented by the presence of hydro-chloric acid.The salt is dissolved, to a small extent, by concentrated hydrochloric acid, which then acquires a deep red colour. When a solution of molybdic acid in hydrochloric acid was reduced in a similar manner by sodium amalgam, a few red crystals were 246 obtained, very similar in appearance to those of the potassium salt ; they probably consisted of the corresponding double chloride of molybdenum and sodium, but were not analysed on account of the difficulty of freeing them from admixed sodium chloride.An attempt was made to prepare the potassium salt by adding potassium chloride to a concentrated solution of molybdic hydroxide, Mo(OH),, in hydrochloric acid, and subsequent saturation of the liquid with gaseous hydrochloric acid, but in this case the brilliant, green crystals of the compound 2KC1,MoOCl,,2H20, which has been prepsred previously, but in a different manner, by Nordenskjold (Bey., 1901, 34, 1572), were produced instead of the expected double chloride. It was found that the same green crystals could be prepared by the action of potassium amalgam on a solution of molybdic acid in hydrochloric acid, if the potassium was added in smaller quantity than is necessary for the production of the red double chloride, and also that the green salt could be converted into the red salt by reducing its hydrochloric acid solution with potassium amalgam.155. '' The action of benzamidine on olefinic P-diketenes," By S. Ruhemann. The author showed that hydrogen chloride reacts with a mixture of m-nitrobenzaldehyde and a &diketone to form a m-nitrobenzylidenedi-ketone, instead of giving rise to the additive product. Thus, m-nitrobenzaldehyde and acetylacetone furnish nz-nitrobenzylidene-acetylacetone, UAc,:CH*C,H,*NO,, melting at 101-102°. The yield of m-nitrobenzylidenebenzoylacetone, PhCO*CAc:CH*C6H;N02 (m. p. 11 1-1 12"), is very small owing to the ease with which it is decomposed by acids.One of the products of the decomposition which has been isolated is m-nitrobenzylideneacetophenone,COSh*CH:CH*C,H,*NO, (m. p. 145"). m-Nitrobenzylidene-@diketones are also produced by the action of piperidine on the dry mixture of the aldehyde and the diketone. But in alcoholic soluiion, the saturated tetraketone is formed, such as m-nitrobenzylidenebisbenzoylacetone, NO,*C,H;CH(CAc*COPh), (m. p. 229-230"). Benzamidine reacts with benzylidenebenzoylacetone, PhCO* CAc:CH*Ph, at the ordinary temperature to form an additive compound (m. p. 132"), the constitution of which is NH:CPh*NH*CPh(OH)*CAc:CEtPh,be-cause the compound is decomposed by dilute hydrochloric acid, giving rise to dibenzamide. Similar additive products with benzamidine are formed from the other olefinic P-diketones ;these, however, are changed when their alcoholic solutions are heated on the water-bath.Thus, 247 sodium ethoxide and benzylideneacetylacetone react with benzamidine at 100' as follows : CAc,:CHPh +CPh(NH,): NH + C,H,O =C17H,,N, + MeC0,Et + H,O. The compound, C17Hl,N,(m. p. 149-150'), is most probably dihydro- diphenylmethylpyrimidine, CHMe<~~~~~>NH. Benzamidine and m-nitro benzylideneacety lace tone interact differ en tly , since m-nitrophenylphenylmethylpyrimidine, (m. p. 137-138'), is formed, instead of the corresponding dihydro- pyrimidine. The olefinic [ monoketone, benzylidenedesoxy benzoin, COPh*CPh:CHPh, does not condense with benzamidine, and the action of hydrogen chloride on the iuixture of m-nitrobenzaldehyde and desoxybenzoin proceeds in the same way as when benzaldehyde is used, and yields COPh.CHPh*CHCl*C,H,~NO~(m. p.166-167O). 156. '(Dissociation constants of trimethylenecarboxylic acids." ByW. A. Bone and C. H.G. Sprankling. In connection with the work on methylenedimethylsuccinic acid, it became necessary to determine the dissociation constants of some trimethylenedicarboxylic acids, since no data with respect to them were available, The following numbers were obtained : &5*. K 25% Trimethylenecar box ylic cis-Trime thylene- 1:2-di-acid ... ... 0.00171 carboxylic acid ... 0,042 Trimethylene-1 : 1 -di-trans-Tri me th ylene -carboxylic acid ... 2.08 1:2-dicarboxylic acid 000215 A comparison of these values with those of the corresponding open chain saturated acids containing two additional hydrogen atoms indicates that the formation of a trimethylene ring increases the constant, this effect being particularly noticeable in the succinic series.157. (( The elimination of hydrogen bromide from bromo-gem-di-methylsuccinic acid and from ,bromotrimethylsuccinic anhy- dride." By W,A. Bone and H,Henstock. Bromo-gem-dimethybszcccinicacid (m. p. 140') is readily prepared by heating gena-dimet hylsuccinic acid with the calculated quantity of dry bromine in sealed tubes at 130-140' ;when heated with redistilled diethy1 aniline at 130°, carbon dioxide is freely evolved, hydrogen bromide is eliminsted, and aaulal-tetramethyZdihydromuconicacid is 248 formed in the following manner : 2C02H*CMe,*CHBr*C02H= C0,H*CMe,*CH:CH*CMe,*C02H+ 2HBr + 2C0,.The new acid is obtained in well-defined, transparent, prismatic forms melting at 70‘ ;it is extremely soluble in the ordinary organic aolvents with the exception of light petroleum ; its aqueous solutions immediately decolorise alkaline permanganate with formation of the dihydroxy-acid, CO,H*CMe,*CH(OH)~CH(OH).CMe,*CO,H,which melts at 129-130’. The dissociation constant of the tetrahydromuconic acid is K,, = 0*001684. The acid distils unchanged under the ordinary pressure, but when boiled with acetic anhydride it yields its own liquid anhydride. In view of Paolini’s observation (Gaxxetta, 1900, 30, ii, 497) that ethyl dimethyltrimethylenedicarboxylateis the product of the action of phosphorus pentachloride upon ethyl h ydroxytrimethylsuccinate, the authors have repeated the work of Bone and Sprankling on the action of diethylaniline on bromotrimethylsuccinic anhydride (Trans., 1902, 81,SO), and by a study of the physical properties of the resultant acid, C7HI0O4,have fully confirmed the previous conclusion that it is methylenedinzethyluccinic cicid, CH2:C(C0,H)*CMe,*C02H. This acid melts at 142O, has a dissociation constant, K,, =0.01597, and gives an insoluble calcium salt.Determinations of the refractive power and magnetic rotation of die thy1 methylenedimethylsuccinate, made by Dr. W. H. Perkin, sen., fully support the argument in favour of the unsaturated character as against the triinethylene ” configuration of the foregoing acid.ADDITIONS TO THE LIBRARY. I. Donations. Hellot, Jean. Fiirbekunst oder Unterricht, Wolle und wollene Zeuge zu fiirben; nebst Vorschriften wegen der Prufungen durch Absieden. Aus dem franzosischen iibersetzt von Abraham Gotthelf Kastner. Zwente Auflsge, welcher eine Nachricht von der Seiden-fiirberen. Altenburg 1765. From Major-General J. Waterhouse, I.S.C. Holleman, A. F. Textbook of Organic Chemistry, translated from the second Dutch edition by A. J. Walker, assisted by 0. E. Mott. New York 1903. From the Publishers, 249 Meyer, Dr. H. Determination of Radicles in Carbon Compounds. Authorised translation by J.Bishop Tingle. 2nd edition. ill. New York 1903. From the Translator. 11. By Purchase. A begg, R. Die Theorie der elektrolytischen Dissociation. Stutt-gart 1903. Aschan, Ossian. Die Konstitution des Kamphers und seiner wichtigsten Derivate. Braunschweig 1903. Baccioni, G. B. Dall ’Alahimia alla Chimiza. Torino 1903. Crookes, W. On the manufacture of beetroot sugar in England and Ireland. ill. London 1870. Deutschen Land wirtschaf ts-Gesellschaf t Arbeiten. Heft 80. Die Dungung mit schwefelsaurem Ammoniak und organischen Stickstoff dungern im Vergleich zum Chilisalpeter. Berlin 1903. -Heft 81. Untersuchungen iiber den Wert des neuen 40 pro-zent.Kalidungesa1zes gegenuber dem Kainit. Berlin 1903. Ferchland, P. Gruodriss der reinen und angewandten Elektro-chemie.ill. Halle 1903. Fischer, E. Synthesen in der Purin- und Zuckergruppe. Braun-schweig 1903. Garola, C. V. Engrais. Paris 1903. Gauss, Carl Friederich. A llgemeine Grundlsgen einer Theorie der Gestalt von Flussigkeiten im Zustand des Gleichgewichts. Ueebersetzt von R. H. Weber. Hrsg. von H. Weber (Gstwald’s Klccssiker, No. 135.) Leipzig 1903. Grandeau, Louis. Valeur et r81e alimentaires du sucre chez l’homme et chez les animaux. Paris 1903. Guldberg, C. M. Thermodynamische Abhandlungen uber Molekular- theorie und chemische Gleichgewichte 1867-1872. Ubersetzt und hrsg. von R. Abegg. (Ostwald’s Klassiker, No. 139.) Leipzig 1903. Haller, Albin. Les industries chimiques et pharmaceutiques. 2 Tome. ill. Paris 1903.Hassack, P. Garungs-Essig. ill. Wien 1904. Horstmann, A. Abhandlungen zur Thermodynamik chemischer Vorgiinge. Hrsg. von J. H. van’t Hoff (Ostwald’s Klassikev, No. 137.) Leipzig 1903. Junemann, Friedrich. Die Brike tt-Industrie und die Brennmateri- alien. Wien 1903. Konig, J. Chemie der menschlichen Nahrungs-und Genussmittel. Val. I, Chemische Zusammensetzung der menschlichen Nahrungs-und Q50 Genussmittel. Naoh vorhandenen Analysen mit Angabe der Quellen ausammengestellt. 4 Aufl. Hrsg. von A. Bomer. Berlin 1903. Labonne, Henry. Formulaire pratique des parfums et des fsrds. ill. Paris 1903. Lodge, Oliver. Modern Views on Matter. (Romanes Lecture 1903.) Oxford 1903. Mahler, P. gtudes sur les aombustibles solides, liquides et gazeux.ill. Paris 1903. Meunier, Louis, and Vaney, Clement. La tannerie. Etude, pr6- paration et essai des matibres premieres, thhorie et pratique des diff Orentes methodes actuelles de tannage, examen des produits fabriquhs, publie sous la direction de LBOVignon. ill. Paris 1903. Ostwald, W. Scientific foundations of analytical chemistry, treated in an elementary manner. Translated by George M’Gowan. London 1900. Pairault, E. A. Le rhum et sa fabrication. ill. Paris 1903. Seubert, Karl. Internationale Atomgewichte von 1903. Leipzig 1903. Whetham, William Cecil Dampier. A treatise on the theory of solution, including the phenomena of electrolysis. Cambridge 1902. Wiener, F. Die Weissgerberei, Samischgerberei und Pergament- Fabrikation, ill, Wien 1904.Winteler, F. Die Aluminium-Industrie. Erauaschweig 1903. Wohltmann, Dr. F. Chilisalpeter oder Arnmoniak ? Berlin 1903. 111. Pamphlets. Dyer, Bernard, and Shrivell, F. W. E. The manuring of market garden crops. (From the Journal of the Royal Horticultural Society, 27, 1903.) Fairley, T. On writing and printing inks. (From the Journal of the Society of Dyers and Calourists, July, 1903.) Golding, John. Experiments on peas in water culture. (From the Centralblatt f. Bahteriologie Abt. II., XI.) Liversidge, A. The Boogaldi, Barratta Nos. 2 and 3, Gilgoin Nos. 1 and 2, and Eli Elwah or Hay Meteorites, New South Wales. (From the Journal and Pyoceedings of the Royal Society of X.S. Wcdes, Vol. 36.) Taylor, R.L. I, On a higher oxide of cobalt. 11, A method for the volumetric determination of cobalt. (From tlhe Xenzoirs and Proceedings of the Manchester Literary and PhiZosophicccZ Society, 47, 1902-1 903.) Thwaite, B. H. The eifect of flue dust upon the thermal efficiency 251 of hot-blast stoves. (From the Journal of the Iron and Steel Institute, 1903, I.) Vines, 5. H. Proteolytic enzymes in plants (11). (Fmm the Annals of Botany, XVII, 1903.) RESEARCH FUND. A Meeting of the Eesearch Fund Committee will be held in December. Applications for grants, to be made on forms which can be obtained from the Assistant Secretary, must be received on or before December 7th. At the next meeting, on Thursday, December 3rd, 1903, at 8 p.m., there will be a ballot for the election of Fellows, and the following papers will be communicated :-(‘On the molecular formuls of some fused salts as determined by their molecular surface energy.” By J.F. Bottomley.‘‘Acid salts of monobasic acids.’’ By R. C. Farmer. &‘ The atmospheric corrosion of zinc.” By G. T, Moody. “The solubilities of the hydrates of nickel sulphate.” By B. D. Steele and F. M. G. Johnson. 252 CERTIFICATES OF CANDIDATES FOR ELECTION AT THE NEXT BALLOT. N.B.-The names of those who sign fram ‘l General Knowledge ” we printed in italics. The following Candidates have been proposed for election, A ballot will be held on Thursday, December 3rd, 1903. Abell, Robert Duncombe, Bradwall, Sandbach, Cheshire, Assistant Lecturer and Demonstrator in Chemistry in the University College of North Wales, Bangor. Studied in Bangor.‘‘Diploma in Agriculture,” 1894 ; ‘(Diploma in Agricultural Chemistry,” 1895 ; B.Sc. (Wales) with First Class Honours in Chemistry, 1899 ; Associate of Institute of Chemistry, 1899 ; 1851Exhibition Scholar, 1899-1902 ; Ph.D. (Leipzig) and D.Sc. (Wales), 1902 ; F.I.C.,1903. “The Con-densation of Phenyl ethyl ketone and Benzaldehyde,” Trans.,1901, 79,928. ‘‘ The Condensetion of Phenyl ethyl ketone with Benzyl- ideneacetophenone and of Acetophenone with Benzylidenepropio-phenone,” Trans., 1903, 83,360. ‘‘ A Synthesis of 1:3 : 5-triphonyl-2 :4-dimethylcyclopentane and of 1 :3 :5-triphenyl-2-methylcydo- penfane,” Trans., 83,367.James J. Dobbie. William A. Bone. H. B. Dixon. D. L. Chapman. W. H. Perkin, jun. Kennedy J. P. Orton. Alexander Lauder. Appleyard, Percy, Albany, Western Australia. Pharmaceutical Chemist. Chemist. Interested in Assay work, and desiroiis of keeping in touch with Chemical Investigation. F. W. Richardson. T. Donald Watson. E. J. Millard. B. E.I?. iVewlands. John C. Hewlett. Peler MacEwan, ?has. Tyrev? 253 Armstrong, Edward Frankland, 55, Granville Park, Lewisham, S.E. Salters’ Research Fellow, Central Technical College. Ph.D. Berlin. Author of papers in the I‘ Sitzungsberichte der Akademie der Wissen- schaft zu Berlin ” and the ‘‘Berichte der Deutschen Chemischen Gesellschaft,” in conjunction with either Prof.van ’t Hoff or Prof. E. Fischer. Henry E. Armstrong. Percy F. Frankland. Emil Fischer. W. Palmer Wynne. J. H. van ’t Hoff. Gerald T. Moody. Ashdown, Herbert Henry, 3, Genesta Road, Plumstead. Analytical Chemist and Metallurgist. Eleven years Assistant in the Laboratory of H. H. Smith, Esq., F.I.C., Royal Laboratory Department, Royal Arsenal, Woolwich. Four years Demonstrator to R. J. Redding, Esq., in Chemistry and Metallurgy at the Royal Arsenal Mechanics Institute. Honours in Chemistry, Metallurgy, and Iron and Steel Manufacture. R. J. Redding. F. Mollwo Perkin. A. Lapworth. Lionel M. Jones. Chas. R. Darling. Attwell, Herbert Moore, Hill House, Limpley Stoke, Bath. Student of Royal College of Science (Lond.). Student for three years at above College, and Associate of the Royal College of Science (A.R.C.S.). James C. Philip. William A. Tilden. Chapman Jones. G. T. Morgan. 111. 0. Forster. M. White Stevens. Badoock, William Cornish, The Grammar School, Crediton, Devon. Science Master in the above school. Studied Chemistry for 3 years at Cambridge, B.A. 1st Class Nat. Sci. Tripos Pt. I. 1900. Desires admission to the Society in order that he may keep in touch with recent work in Chemistry. M. M. Pattison Rluir. R. S. Morrell. S, Ruhemann. E. K. Hanson. H. J. H. Fenton, 254 Bailey, Harold James, 40, The Avenue, Pontypridd, South Wales, Chemist to the Great Western Coll. Co. Coke Works and Bye- product Plant. 42~years Chemistry Student University College, Sheffiold.2 years Chief Assistant to F. G. Treharne, Esq., F.C.S., Consulting and Analytical Chemist, Cardiff. Chemist at present to Bye-product Recovery Plant at Coke Works (above). F. Gmlyn Treharne. William H. Oates. George Young. Henry Annable. W. Carleton Williams. Barker, Thomas Vipond, Exeter College, Oxford. Undergraduate ;will take Chemistry Schools in June, 1904. Done research work in Chemical Crystallograpby for nine months under Prof. Groth in Munich; part of the results already published in the current I‘ Zeit. fur. Kryst.” s. 275. Henry A. Miers. H. L. Bowman. W. W. Fisher. J. E. Marsh. John Tt‘cctts. Beadnell, Charles Marsh, H.M.S. Bccrracoutcc, Capetown and West Coast. Staff Surgeon, Royal Navy.Anxious to obtain the Proceedings of the Society and use of Library. Chas. E. Beadnell. Thos. Stevenson. Charles E. Groves. II. C. 11. Carpenter. E. A. 2bZer. Bayly, Harold Goodenough, ‘‘Moatside,” Bedford. Analytical Chemist. Associate of the Institute of Chemistry. Student in the Laboratory of Alfred Jorgensen of Copenhagen, Oct-December, 1902. Now Chemist to Messrs. Batey & Co., Mineral Water Manufacturers. John M. Thomson. D. Nortball Laurie. Herbert Jackson. alfrecl H. Allen. Patrick H. Kirkaldy. Fredk. J. Lloyd. GiE6el.t J. Alderton. 255 Beam,William, M.A., M.D., Pension Sima, Cairo, Egypt. Chief Chemist to the Egyptian Salt S: Soda Co. Formerly Chief Chemist to the Baltimore and Ohio Railway in America, Joint Author, with Dr.Henry Leffmann, of the following works : (1) Progressive Exercises in Practical Chemistry ; (2) Examination of Water for Sanitary and Technical Purposes; (3) Analysis of Milk and Milk Products; (4) Select Methods in Food Analysis (No. 4 Published by Rebman, London), Blakeston, Philadelphia. Otto Hehner. John GoZding . Wm. Chattaway. Aythur R.Ling. H. Droop Richmond. Edward Bevan. Bliss, Henry James Wheeler, Balliol College, Oxford. Student.. Studied under Rev. T. C. Porter, Eton College, and 3 years at Balliol College. T. C. Porter, H. B. Hartley. R. Tabor Lattey. HenTy E. Roscoe. D. H. Nagel. TVilZiarn Crookes. Bluman, Nicholas John, 10, Amersham Road, New Cross, S.E. Works Chemist. Day student for 3 years under Dr.F. Mollwo Perkin in the Borough Polytechnic Laboratories, and assistant in Practical Chemistry Classes during the session 1902-3. F. Mollmo Perkin. John E. Mackenzie. Edwin C. Jee. J. T.Hewitt. Bertram Blount. 0. J. Steinhart. Bruhl, Paul, Engineering College, Sibpur, near Calcutta. Professor of Physics, Mineralogy, and Geology, Engineering College, Sibpur. Lecturer on Chemistry, "najshahye College, 1882-1 887. Professor of Physics and Chemistry, Engineering College, Sibpur, 1887-1895. Professor of Physics, Geology and Mineralogy, 1896 to the present time. William Tate. Prafulla Chandra Ray. David Hooper. Walter T. Grice. H. E. Stapleton. 256 Bugg6, Erasmue Robert, 327, Grove Green Road, Leytonstone.Chemist.. Student in Chemistry 1895 and 1896 under Dr. Hewitt. Holder of various certificates from the Science and Art Dept., S.K. Engaged at the Chemical Works of Messrs. Walter Voss & Co., Millwall, for 9 years, and has there done a considerable amount of analytical and research work, and is now desirous of being privileged to attend the meetings of the Society and to enjoy the benefit of the Society's Literature and Library. Alfred C. Young. Isaac S. Scarf. Walter A. Voss. J. T. Hewitt. Charles E. Sohn. Clacker, William, Bryantwood, Auckland Road, Ilford. Analytical Chemist. From 1892 to present time. Chemist with Henry Tate and Sons, Ltd., Silvertown, Sugar Refiners. Studied Chemistry under Dr. Hewitt at the East London Technical College, and obtained 1st Class at the London Matriculation.J. Woodward. Hugh Main. J. T. Hewitt. D. Bendix. Albert Harrison. B. E. E. Newlcmds. Desks, William Thomas, High St., Shanklin, I. of W. Pharmaceutical Chemist. Interested in the Bacteriology of Fer-mentation. Frank Oram. J. Brierley. Harry Wilson. Robert Wright. Walter S. Crocker. Derwent, Ernest, 36, Sixth and Railroad, Ironton, Ohio, U.S.A. Analytical Chemist. 12 years' experience in Analysis of Iron and Steel, Refractory Material, etc. Chief Chemist to Union Iron and Steel Co., Ironton, Ohio, U.S.A. J. E. Stead. C. f1. Ridsdale. H-.Frankland. John Pattinson. E. H. Saniter. J. 2'. Dunn. Ellis, Henry Russel, 177, Warwick Road, W. Science Teacher. Inter, B,Sc.London [Working for Honours 257 Chemistry at Final B.Sc.1. Teacher of Chemistry at Regent Street Polytechnic. Wishes to become aMember to obtain the advantages of the meetings and the Journal, and to keep in touch with modern chemical advances. Frank E. Weston. J. Bernard Coleman. J. C. Crocker. 0. LoewenthaI. R. w.Xicndcdl. Fawsitt, Charles Edward, 9, Foremount Ter., Glasgow, W. Demonstrator in Chemistry, University of Edinburgh. Am engaged in original research in physical chemistry. Published work in Zeitschrqt fur Physikal. Chemie, 1902. Member of the Society of Chemical Industry, the Faraday Society, the German Chemical Society, ex-1851 Exhibition Scholar, Ph.D., B.Sc., author of ‘‘ Tables for Students of Quantitative Chemical Analysis ” (Clay, 1903).Alex. Crum Brown. Leonard Dobbin. James J. Dobbie, Morris W. Travers. James Walker. Alexander Lauder , Forster, William, 6, North Railway Street, Seaham Harbour. Pharmaceutical Chemist, Formerly a student under Mr. Wm. Fowler, F.C.S., Sunderland, and Mr. Wm. Duncan, F.C.S., Royal Dispensary, Edinburgh ; and at the Pharmaceutical Society’s School, Bloomsbury Square. William Fowler. J. Norman Collie, William Duncan, Arthur Lapworth. T. E. Wallis. Friend, John Albert Newton, 2, Francis Road, Watford, Herts. Science Master at Watford Grammar School. B.Sc. (Honours Chemistry) Birmingham University, 1902. M.Sc. (for Research on the Reaction between Caro’s acid and H,O,) Birmingham University, 1903.Priestley Research Scholar at Birmingham University (from 1902-3). Late Assistant Demonstrator at University, Birmingham (1901-42). Percy F. Frankland. Alex. Findlay. Alex. McIienzie. T. Slater Price. l’homccs Turner. 258 Gardiner, Ernest Alexander, Bretherton, Nr. Preston Lancs. Teacher, B.A. Keble College, Oxford. 1st Class in Final Honour School of Chemistry (June 1903). Senior Science Master at the Plymouth and Mannamead College. Engaged in Research Work on Inorganic Chemistry. W. W. Fisher. J. E. Marsh. John Watts. Allan F. Walden. H. L.Bowman. Gatehouse, Frank Brooks, 56, Windmill Street, Gravesend, Kent. Demonstrator in Chemistry and Metallurgy. Assistant analytical chemist. Two years in laboratory under J.W. Gatehouse, F.I.C., Public Analyst for Bath, &c. Four and a half years as student-demonstrator at the Merchant Ven turcrs’ Technical Coll. Bristol, under Prof. J. Wertheimer, B.Sc., F.I.C., F.C.S. ;Associate of the Merchant Venturers’ Technical Coll., Bri~tol, and Assistant Chemist to the ‘(Associated Portland Cement Manufacturers, Ltd., Gravesend and London.” Author of “Process for estimation of Cyanide in the presence of a Chloride” (Chem,. News, Ocf. 25, 1901). Has passed .Honours Part 11. inorganic and organic Chemistry, and Hons. Pt,I.Metallurgy, Brd. of Ed. practical examinations. 9. Wertheimer. Arnold Philip, G. P. Darnel1 Smith. p. Fcdis &oddcc?*t. A. E. Thomas. Ernest 19: Cook. Gent, Percy William, 7924, Ridge Street, Newark, N.J.,U.S.A. Metallurgical Chemist. Student for three years at University College, London, under Sir William Ramsay, K.C.B., F.R.S. ;also at Royal College of Science, S. Kensington. Assistant Chemist with Dr. Paul Jeserich, Gerichts-Chemicker of Charlottenburg, Berlin, and afterwards with Messrs. Morris dz GO., Metal Extractors, Doncaster, Now metallurgical chemist with the Balbach Smelting and Refining Go., Newark, N. J.,U.S,A. William Ramsay. Otto Hehner. Edward C, Cyril Baly. Allan T. Hall. Thomas Gough, Morris W. Traverg, Grundy, Frank Barnes, Red Lodge, King’s Road, Richmond, S.W. Technical Chemist. Three years’ Chernical Training, University 259 College, Victoria University. Assistant to Professor Lewes four years.Eight years Assistant Chemist Welsbach Incandescent Co. ; now Manager and Chemist, Ramie Co., Bredbury, Stockport. Vivian B. Lewes. James Swinburne. J. S. S. Brame. W. R. Cooper. Charles A. Kohn. W. Mackean. Horatio Ballantyne. Hall, John T., West View, StanwelI, Staines. Manager and Analyst for the Staines Sewage Works, Stanwell. am a Member of the Sanitary Institute (by Exam.); I am the author of a paper on Sewage Works Management and Analytical Chemistry for Sewage Works Managers, read before a Meeting of the Sewage Works Managers Assoc., July 18th, 1903. James Ashton. v.TVatson Will. Samuel Rideal. A. Wynter Blyth. Henry Ken wood. A. JY. Ge.r*rad. Heasman, Harold Montague, 1, Carlisle Road, Finsbury Park, N. Analytical Chemist.Studied Science at University College under Sir William Ramsay and Prof. Carey-Foster. Studied Metallurgy under C. J. Head, Esq., F.C.S., F.I.C., and at King’s Collegs and the Birkbeck Institution. Have been acting as Assistant Chemist for the past four years to Messrs. Stanger and Blount, 2, Broadway, West- minster, where I am still engaged. S. Dickson. C. J. Head. Bertram Blount. A. M. Kellas. John E,Mackenzie. Hendrickson, Arthur V., The Gasworks, Lower Sydenha,m, ELE, Analytical and Gasworks Chemist. Chemist to the Crystal Palace District Gas Company, TAower Sydenham, for past 2 years, Robert English. Vivian B. Lewes. Samuel Rideal, v.w.Du$eZd. H. F. Hills. Fb LvGpieT sutton. Rowayth, John George,‘‘ Danes Dyke,” Capstone Road, Bournemouth.Senior Science Master, Bournemouth School. Teacher of Chernistpy and Physics (Registered under the Board of Education), for the last 260 eight years, at the Crypt Grammar School, Gloucester, and the Bournemouth School (School oE Science). George Embrey. B. 8. Gott. W. H. Edwards. J. M. ColZett. J.8.8. Brame. Hughes, Edwin Reginald, 106, Queen Victoria St., London, E.C. Analytical and Metallurgical Chemist. Formerly five years assistant to Mr. Edward Riley. 15 years Chemist to South Wales Steel Works, Llanelly, now practising at above address. George H. Hughes. B. E. R. Newlande, John Hughes. E. W. Voelcker. Bernard Dyer. Thos. Howard. Hymans,Herbert, 13 and 14, Trinity Sq., E.C. Manufacturing Chemist (Pharmaceutical and Technical Chemicals and Drugs).Formerly student in the Laboratories of the City of London College under Mr. I. S. Scarf, F.C.S. Pupil Assistant (18 months) in Laboratory of Samuel Rideal, Esq., D.Sc., F.I.C., F.C.S. Assistant (3; years) in Analytical Laboratory of Messrs. Wright, La.yman and Umney, Manufacturing Chemists, London. Notes, etc,, published :-“ New Method for Estimation OF Phenols ” (Pharma-ceutical Journal) ; ‘‘The Occurrence of %odium Sulphate in Nature ” (Pharmaceutical Journal, 1900). Samuel Rideal. Henry Durham, Ernest J. Parry. Isaac S. Scarf. J. Wicliffe Peck. Ibbotson, Edward Charles, 3, Ashgate Road, Sheffield. Works Manager, Sybry, Searls, & Co., Ltd., Sheffleld. Mappin Medallist (Metallurgy).Associate Sheffield University. (4 years) Managing Chemist, The Aruba Island Gold Mining Co., Ltd., Dutch West Indies. Fredk. J. Merrils. Alfred H, Allen. Lawrence Duf ty. G. T,W. Newsholme. Harry Brewley. Jackson, William Henry, 73, Chiirch Street, West Hartlepool. Analytical Chemist. Three years as Articled Pupil and thr6e years as Assistant to Mr. A. C. Wilson, F.R.S.E., District Agricultural 261 Analyst to the Co. of Durham. Two years as Chemist to the West Yorkshire Iron and Coal Co., Ltd., &c., and during the last four years have been engaged in private practice as Analytical and Con-sulting Chemist, A. C. Wilson. Thomas Pairley. J. Falconer King. George Siddle. I? W. Richardson. Jennings, Walter Ernest, 8, Rawdon Terrace, Ashby-de-la-Zouch.Schoolmaster. Certificated in Honours in Chemistry by the Board of Education. Teacher of Chemistry at Ald. Newton’s School, Leicester, for 9 years. Headmasterof the English Department of the Grammar Foundation, Ashby-de-la-Zouch. W. W. Tunnicliffe. W, Ball. Fredk. Cowling. 8. I. Crookes. C. 0’Xullivu.n. Kent, Thomas Oliver, 89, Loughboro’ Park, Brixton, S.W. Analytical and Research Chemist. Managing Chemist of the Research Laboratories of Messrs. Oppenheimer, Son, Co., Ltd. Original work done on the physiological action of the Iron Salts. Am desirous of possessing the literature of the Chemical Society, and keeping in touch with chemical progress, W. Shepperson. Alan Fletcher. H.Helbing. A. Searl. J. T. Ainslie Walker. C. P. Cross. Edward Bevan. Kielty, John J., 71, Cairo Road, Walthamstow, Teacher of Chemistry in the Walthamstow Technical School, Science School A. (1) Teacher of Chemistry for 16 years; (2) 1st Class Honours Practical Chemistry ; 1st Class Advanced Theory of Chemistry ;1st Class Advanced Organic Theory ; 1st C1as.s Advanced Practical Organic, S.K. ;(3) Certificated Teacher and qualified Teacher of Physics and Mathematics. Jos. S. Bridges. Chapman Jones. C. A. Buckmaster. James C. Philip. Isacic 8.Scarf. 262 Knight, Harley Fancutt, ‘‘Ledbury,” 64,Amhurst Park, Stamford Hill, N. Analytical Chemist, Assistant to Bertram Blount, Esq. Certificated student of the Chem. Depart., City of London Guilds Technical College, Finsbury, E.C.R. Meldola. F. Southerden. John Castell-Evans. Chas. R. Darling. Bertram Blount. Laing, John, F.I.C., Everlie, Skelmorlie, N.B. Analytical Chemist. Papers on Destructive and Conservative Distillations of Mineral Oils and their molecular condition. Keith Medal, Royal Scottish Society of Arts, Edinburgh (printed in their transactions). Oil Gas before Society of Chemical Industry (printed in their transactions). Late Chemist and Works Manager, Midlothian Oil Company, Ltd., Straiton, Midlothian. Late General and Commercial Manager, Boson Oil Company, Ltd., near Frhjus, Var. France. Stevenson Macadam. George Beil by. John Hunter. J. Falconer King. J.Xtanley Muir. Lamplough, Francis Edward Everard, Trinity College, Cambridge.Student. 1st Class Eat. Sci. Tripos, 1902. Major Scholar of Trinity College. Exhibitioner in Chemistry, London Intermediate Science, 1903. G. 3.Liveing, H. J. H. Fenton. W. J. Sell. H. 0. Jones. J. P. Millington. Lawrence, Henry William, Wellington, New Zealand. Analytical Chemist. Chief Assistant, Chemical Laboratory-Agri- cultural Department, Wellington, N.Z. Formerly assistant to Dr. Voelcker, Royal Agricultural Society’s Laboratory, and to Sir Henry Gilbert, Rothamsted Laboratory (10 years). Now with Mr. B. C. Aston, Chemist of Agric. Dept. Wellington, N.Z. J. Augustus Voelcker. Harry M. Freear. Thos. Howard, E. W. Voelcker. Bernard Dyer. 263 Leadbetter, Harold Duff, 95, Cape1 Road, Forest Gate, London,tE. Assistant Demonstrator at the Royal College of Science, London.Associate of the Royal College of Science, London. Assistant Chemist €or 3 years at Messrs. A. Boake, Roberts and Go., Ltd., London, E. William A. Tilden. G. T. Morgan. M. 0. Forster. H. Burrows. J. C. Philip. Le Bas,Gervaise, Baymont House, St. Aubin’s, Jersey. Science Teacher. B.Sc. London University. Received Chemical Training University College, London. Formerly Science Master, Kingswood School, Bath. At present Science Master, County Inter- mediate School, Llanelly. William Ramsay. Edward C. Cyril Baly. Morris W. Travers. W. Lester Alton. A. Vincent Elsden. Macdonald, David Baird, 18, Kimberley Road, Leicester. Chemist and Laboratory Manager.Studied Chemistry under Dr. David Lees, Glasgow ; passed the Pharmaceutical Society’s Minor Exam. 1896 ;gained Kinninmont Gold Medal (Electricity, Magnetism and Botany, 1896) ;spent 4 years in Pharmaceutical Laboratory, J. F-Macfarlan and Go., Edinburgh, under D. B. Dott, Esq., F.I.C., F.R.S.E., &c. ;Studied Essential Oils under W. Watson Will, Esq., Metropolitan Coll. Pharmacy, London ; late Chemist to Messrs. Dabin Brothers, Middlesex Street, London, E.C. ;now Chemist and Manager to E. H. Butler and Sons, Manufacturing Chemists, New Haymarket, Leicester. W. Watson Will. Harold E. Burgess. F. Filmer De Morgan. Peter MacEwan. Ernest J. Parry. Thos. Tyrer. McMahon, Frederick William, 61, Brockley Rise, Forest Hill, S.E.Works Chemist. I received my training as an analytical chemist at ShThomas’sHospital. First as a student (three years) and then as lecture assistant (four years) under Professor Wyndham R. Dungtan, At present engaged as works chemist to Oxychlorides, Ltd., doing research work, Wyndham R. Dunstan, Hamilton Wingate. Arthur W. Crossley, W. Caw& Anderson, H. R. Le Sueur, Jaws Roberts, h. 264 Mann, Ernest William, ’‘ Lynton,” Willow Avenue, Edgbast on, Birmingham. Analyst and Chemist to Messrs. Southall Bros. and Barclay, Manuf. Chemists, Birmingham. Apprenticed to the above firm in analytical laboratory for 4 years, assistant chemist 7 years, now chief. Pharmaceutical Chemist. Co-author with the late John Barclay, B.Sc., in a paper on the investigation of Benzoin and allied drugs (Pharma-ceuticat Journal, Mar, 15, 1902).Contributed a paper on the adulterations and methods of detection of Copaiba (Pharmaceutical JournaZ, Mar. 21, 1903). Alfred Southall. C. G. Moor. Frank H. Alcock. Geo. E.Perry. Robert H. Pickard. A. F. Gerrard, Monier-Williams, Gordon Wickham, The Lammas, Esher, Surrey. B.A. Oxon. First Class, Honour School of Natural Science, Oxford, 1903. Now a Student in the University of Freiburg. V.H. Veley. W. W. Fisher. H. E. Roscoe. J. E. Marsh. Wm. Odling. James Dewar. William Ramsay. Nairne, Urban Orlando Scotchburn, 7, Hawthorne Terrace, Ripple Road, Barking, Essex. Analytical Chemist, Have been for the last five years Assistant to H.Leicester Greville, J?.I,C,, F.C.S., Chemist to the Commercial Gas Company, and am a First Class Matriculated Student of the London University, and Chemist to the Wandsworth and Putney Gas Co. H. Leicester Greville. W..J. Dibdin. D. A. Sutherland, Robt. G. Grimwood. H. F. Hills. W.J. A. Buttev$eEd. Nevin, James Victor, Bristol Dispensary, Bristol. Pharmacist. I have been engaged in Analytical work for over two years in the Chemical Laboratory, Swindon. Since 1898 have been Pharmacist in charge of the Bristol Dispensary ;during Ghat t,ime have had a considerable amount of Analytical work to do. Ernest H. Cook, Wm. Berry. Frederic R. Ellis. G. P. Darnetl-Smith. John c. Umney. 365 Parry,William, 23, Mount Pleasant, Waterloo, Liverpool.Schoolmaster. E.Sc. (London University, Nathematics and Chemistry). Teacher of Chemistry in Merchant Taylors’ School, Crosby. W. Ross Innes. Prosper H. Marsden. Henry C. Bond. J. W. Shepherd. Prancis Jones. Pike, Henry George, Downton, Salk bury, Wilts, Demonstrator in Practical Chemistry at the College of Agriculture, Downton. For 20 years Assistant to Dr. Munro. Professor of Chemistry at the College of Agriculture, Downton, Wilts. For 10 years, Demonstrator of Practical Chemistry, Qualitative Analyses, and Quantitative Analyses of Fertilisers, Feeding Stuffs, Waters, Soils, Milk and other Dairy products, &c., at the College of Agriculture. John N.H. Munro. John Wright son. +4lfred J. Wilcox. C.€?.Corbett. F, 0. Solomon. Bes.na;?.d Dyer. Plymen, George Horace Gladstone, 2, Melton Road, Leicester. Science teacher in Organised Science School. Government re-cognised and registered teacher of mience (including chemistry) in secondary schools. Six years’ experience as student in chemical laboratories ; the experience includes work in Honours Stage (South Kensington), and the work laid down in the B.Sc. (Lond.) syllabus, Inter. B.Sc. London University (1900). William Ball. F. w.Tow. Edward Masters. A. D. Hall, W. W. Tunnicliffe. E. J. Russell. William T. Boone. Albert Howard. Lewis Ough. M. J. R. Bunstam, Pollard, William Branch, 68, Finnart Street, Greenock, N.B. Analytical Chemist B.A. (Cantab.). Second Class Natural Science Tripos, 1901.Technical research on the cause of frothing in boiling sugar solutions. W. J. Sell. H. J. H. Fenton. Sidney Skinner. William C. T. Beasley. E.0.Jones. 266 Redfern, Herbert Stanley,B.So., U.M.F.C. College, Ningpo, China, Principal and Lecturer in Science. Took the course prescribed for the Victoria B.Sc. degree in the Honours School of Chemistry at Owens College, Manchester (1899-1 900), and Yorkshire College, Leeds (1900-1902). Graduated June, 1902 ;since which has taken a post-graduate course at Yorkshire College in General and Technical Organic Analysis. Has recently been appointed Principal of the U.M.F.C. College at Ningpo, China, and his duties will include the teaching of Chemistry and Physics. Desirous of having the Society's publications in order to keep himself informed of current investigations.H. B. Dixon. Norman Smith. D. L. Chapman. Julius B. Cohen. Wm. A. Bone. Ip. H. Perkin,jun. Rich, Stiles William George, Stanley Street, South Brisbane, Queensland. Pharmaceutical Chemist. Ten years' experience as Pharma-ceutical Chemist, during which time was four years Assistant to A. B. Chater, Esq, F.C.S. (present Public Analyst for Brisbane), and two years as Lecturer at College of Pharmacy, Rrisbane. J. Brownlie Henderson. Horat io Ballan ty ne. Arthur B, Chater. J. West Knights. T.H. W.Idrk Richardson, Harold Ernest, 63, Lansdowne Road, Seven Kings, Ilford. Science Master at Coopers' Company's School. Bachelor of Arts and Bachelor of Science (London University).J. T. Hewitt. W. H. C. Jemmett. J. McCrae. A. E. Dunstan. Harold A, Aden. Rogers, William David, 36,Grange Road, Smethwick. Assistant in the Chemical Laboratory, Clifton College, Bristol. Associate of the Royal College of Science for Chemistry. Been engaged in teaching Chemistry for several years under W. A. Shenstone and F. T. S, Houghton, King Edward's School, Five Ways, Birmingham. W. A. Shenstone. M. 0. Forster. William A. Tilden. G. T. Morgan. G. M. Norman. 267 Senter, George, 37, Ronalds Road, Highbury, London, N. Teacher of Chemistry. Sir John Cass Technical Institute, Aldgate, London, E.C. Ph.D. (Leipzig). B.Sc. (Lond.). Pharmaceutical Chemist. Studied Chemistry at Pharm.Society’s School ; University College, London ; Universities of Leipzig and Gottingen ;late 1851 Exhibition Research Scholar. Published Papers : ‘‘Das H,O,-Zerset- zende Enzym des Blutes ” (Zeit. Phys. Cliem., 1903, 44,257) ; 1903 ‘‘ Density of Colloidal Solutions ” (with Sir W. Ramsay, K.C.B.), B. A. Report, 1901 ;‘6 Measurement of Temperature” (with Dr. Travers and Dr. Jacquerod), (PAXTrans.,1902, A., p. 105). William Ramsay. Edward C. Cyril Baly. Charles A. Kohn. Samuel Smiles. Morris W. Travers. J. Norman C~lli~. Slator, Arthur, The Priory, Burton-on-Trent. Demonstrator and Lecturer at University College, Nottingham, having the following degrees : Ph.D. (Leipzig), M.Sc. (Birmingham), B.Sc. (London), and having contributed a paper on “The Chemical Dynamics of the Reactions between Chlorine and Benzene ” to the J.Chem. Soc., 1903, 83,729. F. Stanley Kipping. T Slater Price. Percy F. Frankland R. M. Caven. Henry J. 5. Sand. Smith, Frank Gurney, 7, Luxemburg Gardens, Brook Green, W. Chemical Student. Diploma of Associate of City and Guilds Insti-tute (1902). Since October, 1902, have been engaged in Research work under the direction of Dr. Armstrong at the Central Technical College. Henry E. Armstrong. William A. Davis. Gerald T. Moody. William Robertson. T. Martin Lowry. Edward W. Lewis. Smith, William Veysey, 7, Grove Road, Ipsmich Road, Norwich. One of His Majesty’s Inspectors of Factories under the Home Office, Formerly Postmaster in Natural Science (Chemistry) at Merton College, Oxford. Second Class Final Honour School of Chemistry, 268 Oxford.B.A. I have held a Science Mastership at Clranbrook School, Kent, and Blundell’s School, Tiverton. W. W. Fisher. V,H. Veley. John Watts. Allan F. Waldelt. J. E. Marsh. H. L. Bowman. Stewart, Alfred Walter: 18, Annfield Terrace, Partick Hill, Glasgow. Student. Bachelor of Science, Glasgow University, 1902 ; was appointed Research Student in Chemistry, 1901 ; spent a winter semester in Germany on Besearch work, 1902-3 ; was appointed to nn 1851 Exhibition Scholarship (1 903). John Ferguson. James Roberts, jun. W. Carrick Anderson. Matthew A. Parker, D. R,Boyd. Tighe, Arthur, 20, Marlborough Place, St. John’s Wood. Chemical Student.Student under Basil Turner, Esq., Assayer of Sydney, N.S.Wales (eighteen months), Lecturer, Sydney University. Student under A. C. Chapman, Esq,, F.I.C., of Duke St.,Aldgate, E.C. (twelve months). Also at Finsbury College for one course. Alfred C. Chapman. F. Southerden. R. Meldoln. F. Guy Stirling Baker. Fredk. J. Harry. Turner,Arnold, 316, Entwisle Rd., Rochdale. Brewer and Chemist. A Student in the Brewing Section of Chemical Department, Manchester School of Technology for three years. Obtained first plaoe in Honours and the Silver Medal in Brewing, of City and Guilds, London, 1903. Desirous of obtaining the Society’s Journal for purposes of study. William J. Pope. S. J. Peachey. Jas. Grant. L. G. Radcliffe. F. S. Sinnatt.Turner, William Ernest Stephen, 52, Cheshire Road, Smethwick. Science Teacher. Science Instructor to the Oldbury Higher Education Committee. Birmingham University Research Scholar, B,Sc. (London). Percy F. Frankland. Alex. Findlay. Alex. McKeazie. T. Slater Price, R. Lloyd Whiteley. 269 Walker-Pole, Miles, 71, De Korle Street, Braamfontein, Johannesburg. Analytical and General Chemist. Registered as a Chemist and Druggist under the Pharmaceutical Society of Great Britain, October 7, 1893. Granted Diploma by the ‘‘ Raad van Examinatoren,” Pretoria, March 17, 1896, for special mining analytical report. Chemical work under Stevenson Macadam, Edin., 1891. Eight years’ practical experience Gold Assay and General Mining Chemistry.Assay work under Dr. Muter, Kennington, 1894. Experiments in Amalgama- tion, resulting in the production of a metal for mining pumps which stands the action of the Rand water better than that in use before. John Muter. John C. Hewlett. E. J. Millard. Petey MacEwau. R. L. Jenks. Weiss, Carl Friederich Richard, 37, Binfield Road, Clapham, London, S.W. Formerly Analytical Chemist (Assistant of Prof. Dr. Migula, Karls- ruhe, Bad.), now Pharmaceutical Chemist. Studied Chemistry at Berlin University, 2 years ; Bacteriology at Karlsruhe Polytechnic, 1 year; Bacteriology and Chemistry at Bale University, 7 year. Ph.D., M.A., BMe University. Diploma as German Apotheker, Berlin University ; M.Ph.S., London. Author OF “ Ueber die Bac- terienflora der sauren Gahrung einiger Nahrungs und Genussmittel,” 1899.Otto Hehner. H. Helbing. Oscar Guttmann. Admr R. Ling. B. B. €2. ilewlands. Wright, Fred, Terry Street, Balmain, N.S.W. Chemist. Lecturer in Pharmacy, Materia Medica, and Pharma-ceutical Chemistry, Technical College, Sydney, 1882-1 902. Pharma-ceutical Chemist to Elliott Bros. (Limited), Manufacturing Chemists, Ealmain, Sydney, N.S.W. Henry G. Smith. Will. A. Dixon. William &I. Hamlet. TV. M. DoheTty. Anchew J.Dixon. 270 The following were recommended by the Council for presentation to ballot under Bye-Law I. (3) : Kin, Thein, Rangoon. Assistant to the Chemical Examiner, Burma. Studied Chemistry in the Rangoon College. B.A., Calcutta University, 1895. First Assistant to the Lecturer in Chemistry and Physical Science, Rangoon College, 1896-1901.Assistant to the Chemical Examiner, Burma, from April, 1901. 11.Hunter. Andrew Camnp6elZ. Prasad, Mata, Beni lal’s Katra, Benares City. Merchant and Honorary Lecturer in Chemistry. M.A. First Class Allahabad University, late Professor Physical Science Barellg College, at present Honorary Professor and Lecturer of Chemistry Central Hindu College, Benares. Arthur Richardson. Sydney Young. Abhayacharan Sanyal. Fyalzcis G. Fvancis. Robertson,Philip Wilfred, 20, Talavera Terrace, Wellington, New Zealand. Student. Author of “Atomic and Molecular Heats of Fusion,” T., 1233, P., 1902, 131. Sir George Grey Scholar in Physics and Chemistry at Victoria College. At present engaged in research in Organic and Physical Chemistry under Professor Easterfield.Thomas H. Easterfield. J. S. Maclaurin. R. CLIT ASD SOX< LTD., BREAD ST. IIILL, E.C., AiiD RUSGAY SUFFOLK.
ISSN:0369-8718
DOI:10.1039/PL9031900235
出版商:RSC
年代:1903
数据来源: RSC
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