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Abstracts of the Proceedings of the Chemical Society, Vol. 3, No. 42 |
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Proceedings of the Chemical Society, London,
Volume 3,
Issue 42,
1887,
Page 105-116
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ABSTRACTS OF THE PROCEEDINGS OF THE CHEMICAL SOCIETY. No. 42. Session 1888-89. November 3rd, 1887. Mr. William Crookes, F.R.S., President, in the Chair. Sir Benjamin V. S. Brodie, Bast., and Messrs. L. 0. Simmons, William Bott and Edward D. Gravill were formally admitted Fellows of the Society. Certificates were read for the first time in favour of Messrs. Horace Woodward Crowther, Hope Street, West Bromwich ; Frank Cdder, University College, Bristol ; T. Arthur Dickson, 28, Cross Street, Manchester ; Charles A. Fawsitt, 4, Maule Terrace, Partick, Glasgow ; David Ranken S. Galbraith, Auckland, New Zealand ; Joseph C. August Hall, Grosvenor House, Swansea ; Casimir James Head, Landore Steel Company, Swansea ; James Garnett Heywood, 68, Sutherland Avenue, Maida, Vale, N.W.; Walter Hogben, Mon- ville, Seine Infkrieure, France ; Samuel Lees, Jun., Park Bridge, Ashton-under-Lyne; David Lennox, M.D., 144, Xethergate, Dundee ; Eberhard Luttgen, 1814, Mervine Street, Philadelphia, Penna. ; Angus Mackay, Sydney, New South Wales ; Sidney Martinean, South Road, Clapham Park, S.W.; William Edward Matthews, Kosferd Place, Albert Park, Melbourne; John A. Miller, B.Sc., 16, North Pearl Street, Buffalo, U.S. ; John McArthur, 5, Glen Avon Terrace, Partick, Glasgow ; John C. H. Mingays, Taylor Street, Garramatta, Sydney ; Archibald R. Ormiston, Heathland, Uddingston ; Julius Ostersetzer, Goulding’s Chemical Manura Works, Dublin ; Andrew William Taylor, Truman Street, Nottingham ; Arthur Twivey, 151, Broad Street, Birmingham ; Jose Maria Vargas, 397, Eennington Road, S.E.; John Septibo Ward, 36, Oxford Street, Liverpool Bartlett W.Winder, Sandoa Terrace, Sheffield, The following papers were read :- 106 73. “Note on the Atomic Weight of Gold.” By T. E. Thorpe, F.R.S., and A. P. Laurie. In a former paper (Trans., 1887, 565) the authors gave as their final result of 25 determinations of the atomic weight of gold the number 196.85, which differs by 0.21 from the value determined by Kruss. Kriiss has sought to show, however, that this difference is probably due to the presence of free gold in the bromoamate of potassium employed by the authors (Berichte, 1887,2365). The authors reply that they were unable to detect any free gold in the salt used by them, and that they therefore altogether dissent from Kriiss’s conclusion that the lower value of 196.64 is to be preferred.DISCUSSION. The PRESIDENTinquired whether the authors had ever attempted t’o purify the gold by distillation. Stas had stated that it could be volatilised by means of the oxyhydrogen flame, and he had occasion to confirm this observation-in fact, gold boiled violently when heated in a lime crucible by means of the oxyhydrogen blowpipe. Professor THORPEreplied that no doubt the method suggested might be employed to purify gold. They had obtained their material from the mint : the only impurity which might have been present was platinum, but it was improbable that it was, as a quantity which might escape detection by qualitative chemical tests appeared to be capable of rendering the gold brittle.74. “The Interaction of Zinc and Sulphuric Acid.” By M. M. Pattison Muir and R. H. Adie. The experiments described are altogether qualitative. The authors have examined the interaction bet,ween sulphuric acid of varying concentration and zinc of different degrees of purity. If pure or nearly pure zinc and moderately dilute sulphuric acid inter- act at moderate temperatures, they give zinc sulphate and hydrogen only ; as temperature and concentration increase the quantity of hydrogen produced decreases, and sulphur dioxide and sulphur- etted hydrogen begin to appear. With concentrated acid and nearly pure zinc the chief gaseous product is sulphur dioxide. When commercial zinc is used, sulphur dioxide and sulphuretted hydrogen are produced at almost all temperatures and even with acids as dilute as H2SO~*100H20.Zinc sulphate is the only solid product of the interaction at any temperature or concentration of acid.The reaction with platinised zinc-foil resembles that with commercial zinc ; is both cafies sulphur is formed at moderately high temperatures when 107 fairly concentrated acids are employed. Variations in the relative mass of zinc employed are without regular influence on the nature of the products of the change. The possible sources of the sulphur and the sulphur comp0und.s are discussed in the light of the tabulated experimental results. The general conclusion is that the interaction between nearly pure zinc and sulphuric acid of different degrees of concentration is chiefly a direct chemical reaction; but that when less pure zinc is employed the reaction is largely electrolytic.The marked influence of concentration and temperature, in every case, makes it probable that the reactions are many and complex, and that they occur between zinc and various molecular aggregates of H,SOa and HzO,or of H,SO,, SO, and H,O. DISCUSSION. In answer to Mr. Groves, Mia. MU~Rsaid that they had not ascer-tained whether the sulphur which was produced was the soluble or the insoluble modification. Replying to Mr. Harcourt he said that they bad not attempted to take into direct account the influence of varying amounts of zinc sulphate ; he thought, however, that if it had exercised any particular influence this would have been noticed in the course of the experi- ments, as the conditions had been very greatly varied.Dr. A~~MSTRONGexpressed his surprise that the authors should have made in the beginning of their paper a halting confession that inter- actions such as that between sulphuric acid and zinc were to some extent at least electrolyt,ic ; and still more that they should state the opinion that their experiments afforded evidence that in the case of approximately pure zinc “ chiefly direct chemical interaction ” takes place. It was very remarkable that chemists did not recognise, as physicists had done, that the chemical and electrical phenomena were in such cases absolutely interdependent.The authors had brought forward a large amourrc of valuable information in their paper, but he could not conceive how any of their evidence could be interpreted as proof of direct chemical interaction-whatever that expression might mean. In reply to Dr. Armstrong, Mr. MUIR stated that by the ex-pression “ direct chemical interaction,” as compared with the expres- sion used when speaking of the action between sulphuric acid and commercial zinc, viz., “ a reaction partly chemical, and also to a large extent electrolytic,” the authors meant that in one case zinc, sulphuric acid and water interact in the manner usually called chemical, and that the products are either hydrogen and zinc sulphate, or, with a different concentration of the acid and a different temperature, hydro- gen, zinc sulphate and sulphur dioxide; while in the other case, 108 besides this change, another occurs, viz., the decomposition of the acid by the electric current produced in the chemical reaction occurring between the acid, the zinc and the other metal or metals in the specimen of zinc used.The first change might be, and probably was, electrical as well as chemical; but, if so, the generally used term, “chemical interaction,” is here employed to include the electrical as well as the chemical part of the whole occurrence. 75. “Note on Safety Taps.” By W. A. Shenstone. The author has previously pointed out (“ Methods of Glass Working,’’ pp.646) that the safety taps recently introduced are open to the rather serious objection that they offer no special resistance to the passage of air in the direction in which leakage is most likely to occur, and that therefore such taps are only trustworthy when em-ployed in conjunction with suitable mercury traps. But it had hitherto escaped his notice, and probably that of others also, that even when so protected these taps are still of unsatisfactory construction, as when the properly lubricated plug of the tap is brought into position the space below the plug remains full of air. If the tap be well made, nearly all this air will remain there during the exhaustion of any vessel that may be attached to either arm of the tap ; but after- wards, especially if the lubrication of the tap becomes imperfect, air will gradually find its way from below the plug into any apparatus that may be attached to the tap.To remove this imperfection a very simple alteration only is required, viz., that the plug shall be drilled so that when the tap is open there is free communication between the space below the plug and the contents of any apparatus of which the tap maj form a part. DISCUSSION. The PRESIDENTexhibited and described two safety taps, the one sealed in one, the other in two directions, by mercury, which were not open to the objection raised by Mr. Shenstone. Mr. SHENSTONEsubsequently pointed out that the chance of leakage was very much reduced by placing the two arms of the tap at different levels and bringing them into communication by drilling a hole diagonally through the plug ; aid he particularly insisted on the importance of this modification of the ordinary method of con-struction. 76.“Note on Guthrie’s Compound of Amylene with Nitrogen Peroxide.” By A. K. Miller, Ph.D. In the examination of the products of the inanufncture of oil-gas 109 (Armstrong and Miller, Trans., 18136, 74) the want of a method of identifying different unsaturated hydrocarbons was keenly felt, and experiments in more than one direction are in progress which it is hoped may lead to a satisfactory solution of the difficuIt<y of analysing complicated hydrocarbon mixtures of a similar nature. It appeareti to be not improbable that nitrogen peroxide might prove a valuable reagent for the recognition of some of the constituents, as it was known to combine with certain unsaturated hydrocarbons to form well-defined crystalline derivatives ; and it was further hoped that perhaps a reagent might be discovered which would characterise NzOa,and might be of service in studying the vexed question of the existence of gaseous I$pU',O,.It was conceirable that the formation of crystalline compounds depends on a particular molecular grouping of the carbon and hydrogen atoms, and that they will be producible from a homologous series of like constituted hydrocarbons only and not from their isomerides. A few preliminary experiments only have as yet been made, the work having been postponed from last winter owing to the great difficulty of working with such very volatile hydrocarbons and such comparatively unstable substances in hot weather.The reason for already bringing the subject before the Chemical Society is the recent publication of a paper by Wallacli (Annalen, 241, 288), who has to some extent anticipated the author's line of work. Many years ago, Guthrie (Annalen, 119, 83) showed that when commercial amylene and nitrogen peroxide were brought together, combination took place, the products being a definite crystalline sub- stance, C,H,,N,Oa, which decomposed sharply at 95", and an oil. Although commercial amylene is known to consist chiefly of tri-rnethylethylene, no proof had been given that Guthrie's compound is derived solely from this hydrocarbon, and not from some other constituent.This being a point of importance in connection with the research as indicated above, pure trimethylethylene was pre-pared from commercial amylene by agitation with sulphuric acid, &c., according to Wischnegradsky's method (AnnnZen, 190, 328). The action of pure nitrogen peroxide on trimethylethylene and on the residual amylene was then separately examined. The trimethylethyl- ene, dissolved in either carbon bisulphide or glacial acetic acid and cooled by iced water, was converted almost entirely into Guthrie's crystalline compound; some green oil was also produced, but this crystallised for the most part on standing. On crystallising the product from benzene, prismatic crystals were obtained which decom- posed sharply at 99". No signs of the needles described by Tl'allach (loc.cit.) were observed. On submitting a small portion of the residual amylene to the 110 same treatment, no crystals were produced, and on pouring the pro- duct into water a separation into three layers was observed. The lowest layer consisted of a heavy oil which coixld not be made to crystallise by cooling to -lOo, or by exposure to air. The upper- most layer was very volatile and consisted in all probability of pentane originally present in the amylene. Experiments were also made with normal amylene and normal hexylene ; these both yielded oily products heavier than water, and which also refused to crystnllise. From these results it would appear bhat trimethylethylene is the only constituent of commercial amylene which yields a crystalline derivative with nitrogen peroxide.It remains to be seen how the remaining isomerides behave. DISCUSSION. Professor DUNSTANasked whether Dr. Miller had examined the action of reducing agents on Guthrie's compound. He suggested this as a test of tho correctness of the formula proposed by Wallach, which represented the compound as a nitrosyl iiit,rate, a view Victor Meyer had previously rejected, because he obtained all the nitrogen in the form of ammonia by redncing with sodium amalga,m. The act ion of ferrous hydroxide might decide the question, hince nitrosyl, if present, would probably yield hyponitrite, while the nitroxyl would be unattacked by the weak reducing agent, and would form amyl nitrate.Dr. MILLERreplied that b had not. 77. " The Dehydration of Metallic Hydroxides by Heat, with Special Reference to the Polymerisation of the Oxides and to the Periodic Law." By Professor Carnelley, D.Sc., and Dr. James Walker, University College, Dundee. The object of this investigation was--First, to ascertain whether some light could be thrown on the question of the polpmerisation of the metallic oxides (cf. Henry, Pltil. Mag. [5], 20,81) by heating certain hydrates at regularly increasing temperatures, and deter-minirig the degree of dehydration tllus produced. In this way it seemed probable that data coula be obtained for the construction of curves which would indicate whether any compounds were formed intermediate between the normal hydrates and the corresponding oxides, and thus give some information in regard to the general phenomena occurring during the dehydration, whilst the composition of those compounds if formed might also afford some clue to the true 111 molecular Keights of the oxides.Second, to determine the minimum temperature of complete dehydration of the metallic hydroxides with a view of ascertaining whether this temperature was a periodic function of the atomic weight of the positive element. In the paper the methods of working and the full results are given, together with diagrams of curves in which these results are represented graphically.The general conclusions arrived at are as follows :-1. Precipitated antimony trioxide is anhydrous. On heating it underwent the following changes : Sb203or Sb20030stable up to 360" ; then rapid absorption of oxygen with formation of Sb2,0n (?); the latter comparatively stable to 415-440" ; then further absorption of oxygen with formation of Sb2,03,(?); the latter comparatively stable to 500-565" ; third absorption of oxygen with formation of Sb204or Sb,,O,, ; the latter stable from 590" to above 775". 2. The following definite stable hydrates appear to exist :-(a.) Ag(OH), stable up to about loo", then Papid loss of waker with formation of Ag.0 ; the lat,ter stable to 180-270", then reduc- tion to metallic silver ; this reduction complete at 300-340".(b.) Hg(OH),, stable up to about 100"; complete dehydration to HgO at about 175", when incipient decomposition into Hg and O2commences, followed by full decomposition at about 415" to 440". (c.) Ce02*2H20or Ce(OH)4 = ortho-ceric hydrate. This hydrate was formed on heating precipitated hydrate of cerium dioxide to about 385". It remained stable from about 385" to 600". It was of a light-yellow colour. On heating to over 600°, it underwent dehydration to Ce02, and became salmon- coloured. This is the only definite stable hydrate of the oxides RO, of the silicon-titanium-group obtained. In other respects cerium hydrate on dehydration behaved like the hydrates referred to in § 5. (d.) 5Coz03.8H20.--This was the composition of air-dried cobaltic hydrate, and was perfectly stable up to 75".3. The following data in regard to the action of heat on the hydrate of Pb,O will possibly be of interest in the manufacture of red lead :-Hydrate dried in air = 3PbO2.H2O; complete dehydration about 230"; PbOz stable up to about 280"; loss of oxygen with formation of Pbz03 at 280-290" ; Pb20s stable at 290-360" ;loss of oxygen with formation of Pb@* at 360-415" ; Pb304 stable at 415- 530" ;loss of oxygen with formation of PbO at 530-530" ;PbO stable from 580" to above 815" ;PbO fused somewhere between 585" and 630". 4. Air,dried thallic hydrate = T1203-H20,but unstable on heating; 112 complete dehydration to TL0, at about 230"; T1,0, perfectly stable at 230-360" ; reduction to 3T120,j.T120 at 360--440° ; 3TI2O3.T1,0 per-fectly stable at 440-565" ; rapid loss of oxygen and volatilisation of T1,O formed at 585-815" ; the rate of loss gradually diminishing after fusion at 630" ; remaining T1,0, constant from 815" upwards.5. An examination of all the results shows that, with the excep- tions referred to in 9 2, there was no certain indication of the forma- tion of definite hydrates which were stable through any but possibly a very small range of temperature. From this we must conclude, either that there are no definite hydrates formed on heating at gradually increasing temperatures, or that a very large number of guch hydrates are produced under these conditions but are SO unstable that a further rise in temperature is sufficient to convert a higher into a lower hydrahe.Of these, the second alternative is, for reasons given, by far the more probable. The results accord entirely with Professor Henry's theory that the known metallic oxides are polymers n(R0,) of the unknown simple oxides (RO,). The results also show that in most cases, especially those of SiOz, TiOz, SnO?, 81203, &C., the cofficient n of polymerisation must be very large, as might be expected from the infusible character of these oxides. Minimum values for this coefficient are indicated in some cases. 6. The retention of water by many oxides at comparatively high temperatures, at and above a red heat, is notewort'hy. This is espe-cially interesting in the case of the hydrate Ce(OH)4, which is stable to so high a temperature as 600".The retention of' water at such high temperatures illustrates the great importance in quan- titative analysis of the thorough ignition of hydrates before weighing. 7. The minimum temperature of complete dehydration is a periodic. function of the atomic weight, as follows :-(a.) For normal oxides of odd members of the same group, the mini-waum temperature of complete dehydration diminishes as tJAe atomic weight of the positive element increases. (b.) For even members of the same group it increases as the atomic weight of the positive element increases. (c.) For normal oxides of elements belonging to the same period the minimum temperature of complete dehydration diminishes fronc the beginning to the middle, and then increases to the end of the period.These results accord with the heats of combination of the normal oxides with water in the formation of hydrates, 8. Of two oxides belonging to the same group, the one which requires the highest temperature for complete dehydration will 113 usually combine at any other lower temperature with it greater quan- tity of water per molecule of oxide, though this is not always the case, the pairs SiO,,SnO, and A1203,1n203 being marked exceptions. Prom this we may conclude that the order of affinity of the oxides for water is usually the same both in intension and in extension, though not always so. 9. Changes of colour on dehydration which are permanent 0.n coolilzg usually indicate the formation of a definite hydrate, or that the dehydration is complete, or that some other definite chemical change has occurred.78. “The Bromination of Naphthalene p-Sulphonic Acid.” By(3. Stallard. The author has revised and extended the work of Darmstadter and Wichelhaus (Annalen, 152, 303) and Jolin (Nova Acta Soc. Upsal., 187’7). He finds that when a strong solution of C,H,*SO,K(P) is acted upon by 1mol. prop. of bromine, a mixture of mono-and di- bromo-salt is precipitated, consisting chiefly of the former. Their separat’ion is best effected by fractional crystallisation of the copper salts : the mono-salt separates out first in the form of very small pale- green rhombic plates, while the dibromo-salt remains in the mother- liquor, and eventually comes down from a sufficiently concentlrated solution in the form of long, eage-green, seaweed-like filaments.The mono-salts examined are the potassium (anhydrous), barium (+H20), calcium (+ H,O), sodium (+H,O)-which all crystallise in colour- less needles-and the copper salt (+ 8H,O). The dibromo-salts examined are the potassium (+ +H,O), barium (+ 3iH20),calcium (+ 2B20),and sodium (+ H,O)-which were all obtained in colour-less needles-and the zinc salt (+ 9&H,O), which separated from solution in the form of a slightly opalescent, almost translucent jelly, and the copper salt (+ 7H,O). The constitution of these bodies is shown by the fact that the monobromo-salts yield on hydrolysis a-bromonaphthalene, while the dibromo-salts give the so-called p-dibromonaphthalene, which is the a’a4 modification.Hence the tribromonaphthalene (m. p. 86.5”) which Jolin prepared from the dibromo-sodium salt by the action of PBr,, is either the a’P2a4or the a’P2’a4modification. The first of these forrnuh, however, is inadmissible, since it has been already assigned with good reason to Meldola’s tribromonaphthalene of m. p. 114” (Chem. SOC.Tyafis., 1883,4) from dibromo-a-naphthylamine,and hence the constitution of the mono- and di-bromo-sulplionic acids ’ above-mentioned must be Br : S0,H = 1 -2‘ and Br : Br : SOsH = 1:4 -2’. 114 Purther experiments to test the correctness of this conclusion are in progress.The monobrom-acid appears to correspond to the chloro- sulphonic acid which Cleve has recently (Berichte, 1887, 72) obtained from nitronaphthalene-p-sulphonicacid. 79. “ The Constitution of the three Isomeric Pyrocresols.” ByW. Bott, Ph.D. By reducing a-pyrocresol by means of hydrogen iodide, the author has obtained, among other products, a hydrocarbon having the pro- perties of a paraffin and approximately of the composition CI5Hs2; zinc-dust appears to reduce pyrocresol in a similar manner-but with difficulty. Attempts to displace the oxygen in pyrocresol by chlorine by means of phosphorus pentachloride were attended with little success-all attempts to purify the product having failed. Prom these results and those previously obtained by Schwsrz and himself, the author draws the conclusion that the pyrocresols are compounds of the type of phenyl ether. DISCUSSION.In reply to Dr. Armstrong, who asked why so peculiarly unfortunate a name as “pyrocresols ” had been assigned to compounds which were neutral substances and not “ols,” i.e., phenols, and could not possibly bear any simple relation to the cresols, Dr. BOTTsaid that he was not responsible for the name ; it was selected by Schwnrz because they were bye-products of the manufacture of cresols and their homologues, a,nd were obtained when the retorts in which distillation was effected became overheated. 80. ‘‘Preliminary Note on certain Products from Teak.” By R. Romanis. The author finds that alcohol extracts a soft resin from teak, but no oil or varnish. On distilling the resin he obtained a crystalline sub-stance which he also found to be present in considerable quantity in the tar resulting from the destructive distillation of teak.The analyses which he has made for the crystals point to the empirical formula CsH80; on oxidation with nitric acid they yield what appears to be a quinone of the formula ClsHl6O2. 115 ADDITIONS TO THE LIBRARY. I. Donations. Twenty-third Annual Report on Alkali Works, 1886 : by the Chief Inspector : London, 1887 : from Dhe Chief Inspector. The Norwegian North Atlantic Expedition, 1876-1878 : XVIII a and p. The North Atlantic Ocean. Its Depths, Temperature and Circulation : by H. Mohn : Christiania, 1887 : from the Editorial Committee.Smithsonian Miscellaneous Collections : XXVIII : Meteorological and Physical Tables : by A. Guyot : XXIX : Catalogue of Scientific Periodicals : by H. Carrington Bolton : XXX : Scientific Writings of Joseph Henry : Washington, 1887 : from the Smithsonian Institution. Mason Science College, Birmingham : Calendar for the Session, 1887-1888 : from the College. Memoranda of Field and other Experiments at Rothamsted : June, 1887 : from Sir J. B. Lawes. Transactions of the Wagner Free Institute of Science of Phila-delphia: vol. i, 1887 : from the Institute. Hampshire Field Club: Papers and Proceedings, No. 1, 1887 : Southampton, 1887 : from the Club. Exercises in Prmtical Chemistry : vol. i : Elementary Exercises : by A.G. Vernon Harconrt and H. G. Madan : 4th ed. : Revised by H. G. Madan: Oxford, 1887 : from the Editor. Reports of the Royal College of Chemistry and Researches con-ducted in the Laboratories, 1845-6-7 : London, 1849 : from Dr. Hodgkinson. Timhcri: The Journal of the Royal Agricultural and Commercial Society of British Guiana : vol. i ; part 1: from t,he Society. Mineral. Physiology and Physiography : by T. Sterry Hunt : Boston, 1886 : from the Author. A New Basis for Chemistry : by T. Sterry Hunt : Boston, 1887 : from the Author. Practical Organic Chemistry : by J. B. Cohen : London, 1887 : from the Author. Qualitative Chemical Analysis : by C. R. Fresenius : Tenth Edition, translated from the fifteenth German edition: and edited by C.E. Groves : London, 1887: from the Publishers. Ueber die raumliche Aiiordnung der Atome in organischen Mole-kulen : (Pamphlet) : J. Widicenus : Leipzig, 1887 : from the Author. Calendar of the City of London College : For the years 1887-88 : from the College. Handbook of Modern Chemistry, Inorganic and Organic : by C. M, Tidy : 2nd ed. : London, 1887: from the Author, Elementary Chemistry: by M. M. Pattison Muir and C. Slater: Cambridge, 1887. from the Authors. Practical Chemistry : by M. M. Pattison Muir and D. Carnegie : Cambridge, 1887 : from the Authors. Notes on the Ancient Iron Industry of Scotland: by W. Ivison Macadam : (Pamphlet) : from tho Author, 11. By Purchase. Die Berechnungen fiir Entwurf und Betrieb von Eisenhochofen : von H.Wedding : Braunschweig, 1887. Manual of Bacteriology: by E. M. Crookshank : 2nd ed. : London, 1887. Photograpby of Bacteria : by E. M. Crookshank : London, 1887. Untersuchung iiber Kakao und dessen Praparate : von P. Zipperer : Hamburg and Leipzig, 1887. Noveau Dictionnaire de Chimie: par E. Bouant. Fas. I, A-Chaleur : Pas. 11,Chalumeau-Goudron : Paris, 1887 (cont.). Lehrbuch der Zuckerfalbrikation: von K. Stammer : 2 Auf: Braunschweig, 1887. Die Fortschritto in der metallurgischen Probirkunst in den Jahren 1882-1887 : von Bruno Kerl : Leipzig, 1887. Exercises in Quantitative Chemical Analysis with a short Treatise on Gas Analysis : by W. Dittmar : London and Glasgow, 1887. Heilquellen Anallysen fur normale Verhaltnisse und zur Mineral-wasserfabrikation berechnet auf Zehntausend Theile : yoii F. Raspe ; Dresden. At the next meeting, on November 17th, there will be a ballot for the eZection of Fellows, and the following paper will be read:- "Experiments on Zinc-copper and Tin-coppcr Alloys." By A. P. Laurie. HABRISON AND SONS, PRINTERS i~ ORDINAEY TO HEX MAJESTY, ST.XARTIN'S LANE.
ISSN:0369-8718
DOI:10.1039/PL8870300105
出版商:RSC
年代:1887
数据来源: RSC
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