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Proceedings of the Chemical Society, Vol. 14, No. 194 |
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Proceedings of the Chemical Society, London,
Volume 14,
Issue 194,
1898,
Page 115-128
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摘要:
Issued 12/5/1898. PROCEEDINGS OF THE CHEMICAL SOCIETY. No. 194. Session 1897-8. May 5th, 1898. Professor Dewar, F.R.S.,President, in the Chair. Messrs. E. C. Jee, W. Marshall, and T. H. Pope were formally admitted Fellows of ‘the Society. Certificates were read for the first time in favour of Messrs. Harry Brearley, Totley, Derbyshire ; Arthur 8tanley Hemmy, Government College, Lahore ;Leonard Myddleton Nash, 281, Seven Sisters’ Road; Finsbury Park, N.; Edward John Russell, Owens College, Man-Chester ;Sigmund Stein, 323, Vauxhall Road, Liverpool ;Frank Edwin Weston, 43, Larkhall Rise, Clapham, S.W. ; William Williamson, 86, Tyndall Road, Leyton, E. ; Charles Arthur Wrench, 3, Park-lands, Surbiton Hill. Of the following papers those marked * were read :-*69.“The action of hydrogen peroxide on carbohydrates in the presence of iron.” By C. F. Cross, E. J. Bevan, and Claude Smith. The results obtainod by H. J. H. Fenton (Trans., 1894,65, 899; 1895, 67,48; 1896, 69, 546) in oxidising tartaric acid by hydrogen peroxide in presence of soluble iron compounds suggested the applica- tion of the method to other hydroxy-compounds, and notably to the carbohydrates. The authors have studied the behaviour of typical hexoses and of cane-sugar, when treated in aqueous solution with hydrogen peroxide at ordinary temperatures, and, in confirmation of Fenton’s observations, have found in this group also that the presence of iron compounds is an essential condition for the production of the characteristic reactions.A convenient proportion of iron (Fe as 116 FeSO,* 7H,O) id 1/10000 of the weight of a solution containing 4grams of the carbohydrate in 100 C.C. The authors reserve for the present any statement of the limiting proportion which may be necessary, and are engaged in ascertaining whether other inorganic compounds may not be found to have similar effects. With such proportions and with hydrogen peroxide in quantities sufficient to supply 1 or 8 atoms of oxidising oxygen for each molecule of hexose, reaction takes place readily with marked rise of tempera- ture (10-20°), but in the absence of iron compounds, all other conditions remaining the same, nothing happens at ordinary tempera- tures. After reaction, the solutions are acid to the taste.The quantity of acid formed is greater from dextrose than from lsevulose. The volatile acids separated by distillation are formic and acetic acids, and represent 15-20 per cent. and 4-7 per cent. respectively of the weight of the dextrose. The non-volatile acids represent about one-half the total acidity, and contain a dicarboxylic acid which is easily isolated by precipitation as lead salt in the presenceof acetic acid, and on analysis gives numbers corresponding with those required for tartronic acid. After removal of the acids, the presence of furfuroids is identified by estimations of furfural in the distillates from hydrochloric acid (sp. gr. 1.08). The quantities obtained from dextrose or cane-sugar are 3-4 per cent., representing 7-9 per cent.of the furfuroid. The products yielding furfural are not acid in character, but there is no evidence that they are pentoses. From lzevulose, only traces of these products are formed. The solutions give a well-marked iodoform reaction, indicating that the hexose molecules undergo internal re- arrangement, and that the phenomena are not those of a simple oxidation. The characteristic products of the reaction are separated from solu- tion by the addition of alcohol and ether; on drawing off the denser aqueous layer, a solution is obtained which dries in a vacuum to a gummy solid, destitute of any appearance of crystallisation. These compounds react with phenylhydrazine acetate in the cold, forming osmones, and give evidence of the presence of highly reactive groups by reducing Fehling's solution in the cold.The yield of osazones is considerable, amounting to 30-60 per cent. of the weight of the carbo- hydrate in the case of lsvulose and of cane-sugar ;and to 12-20 per cent. in that of dextrose. Two groups of osazones have been obtained, (I) compounds melting at 185-195' and resembling the glucosazones in properties, but differing from them in composition, the nitrogen (N = 17-20 per cent.) being 2-3 per cent. higher ; (2) compounds with a low melting point (130'), and freely soluble in hot water. From these results, it might be inferred that the products are the 117 ‘6 OSOnes” or “oxyglucoses ” of Fischer, but they resist the action of zinc and acetic acid on the one hand, and of bromine on the other, and are not reduced by sodium amalgam in solutions kept slightly acid ; properties which differentiate them from the normal carbohydrates and from such of their oxy-derivatives (ketaldoses) as are at present known.The investigation of the nature of these products is complicated by the fact that no crystalline derivatives other than the osazones have been obtained. No definite acetates or benzoates have been isolated. Some evidence as to their relationship to the original hexoses, however, is obtainable from a closer study of the constants of the reaction. It appears, in the first place, that there is no simple proportion between the quantity of hydrogen peroxide employed and the amount of the characteristic products obtained.Having established this for quantities representing 3,2, and 1 atom of oxygen for each molecule of the hexose, the authors found that very considerable effects were still produced on furtherreducing the proportion of peroxide. Thus from 40grams dextrose treated with sufficient peroxide to furnish only 1/10 atom of oxygen for each molecule of hexose, the quantity of osazones formed in the cold from the product of the reaction was 8 grams, an amount as great, therefore, as that obtained when 10timesthis proportionof the peroxide was employed. Similarly, the addition of still smaller quantities of the peroxide to a dextrose solution was found to convert a considerable proportion of the hexose into compounds not fermented by yeast, though reducing Fehling’s solution and otherwise resembling the compounds just described.The authors conclude (l),that hydrogen peroxide acts primarily by determining a constitutional change in the hexose molecule, i.e., by in- ternal rearrangement, such effects bearing no direct proportion to the quantity added, and (Z), that the oxidising actions observed, e.g., the formation of dicarboxylic acids, are subordinate or secondary effects. As regards the nature of the constitutional changes in question, the reactions of the Characteristic products indicate the presence of -C(OH):C(OH)-groups. In the formation of dihydroxymaleic acid from tartaric acid, this radicle results from an actual removal of hydrogen by oxidation, and in the carbohydrates might be formed by internal rearrangement.The authors consider that such a change is the primary effect of contact with the peroxide, although -CH(OH)*CH(OH)- residues also are probably attacked and hydrogen eliminated by direct oxidation. The obvious bearings of these results upon the problem of plant physiology, from which point of view they are positive and sufficiently 118 established, induce the authors to put forward this preliminary com- munication without waiting for a definite solution of the constitutional problems, which are still under investigation. DISCUSSION. Dr. ARMSTRONGreferred to the interest of the work in connection with vegetable physiology, indicative as it was of the far-reaching character of the interactions concerned in the elaboration of the products of plant activity. Although the part played by enzymes in such processes had been generaIly recognised, their importance must be much accentuated now that Buchner’s remarkable discovery of an enzyme capable of inciting alcoholic fermentation was placed beyond doubt.It seemed quite possible, from the experiments of Mr. Cross and his colleagues, that iron, which is known to be present in most plants, may behave to some extent as an enzyme and thus possess unexpected importance from the point of view of plant chemistry; it was very noteworthy from this point of view that the formation of reduction products yielding iodoform had been observed as well as that of oxidation products.Dr. MORRELLstated that, with galactose, the disappearance of hydrogen peroxide is twice as rapid as with glucose, and that the addition of large quantities of the peroxide caused a marked rise of temperature, Ferrous iron, which could not be detected during the oxidation, reappeared when hydrogen peroxide could be recognised no longer in the solution. Mr. FENTONsaid that, since he had observed the peculiar influence of iron in the oxidation of tartaric acid, experiments had been made in other directions, and as so wide it field had been opened up for investigation the co-operation of the authors and of Dr. Morrell was most welcome. Mr. LING,referring to the possible analogy between the products of the reaction described by the authors and those formed by the oxida- tion of sugars by alkaline copper solutions, said that Kjeldahl had observed that glucose and fructose, when boiled with a solution of potassio-copper sulphate (Ost’s solution), yield mesoxalic acid.Kjeldahl had also shown that this acid, on treatment with phenyl- hydrazine acetate, is converted into a dihydrazide melting at 148’,-a derivative, therefore, of dihydroxymalonic acid. Might not the sup- posed osazone, which was formed in the cold, be a substance of this kind Z Mr. CROSS,in reply, stated that the phenylhydraeine derivatives obtained in the cold had the characteristics of osazones, although 119 neither aniline nor ammonia, which according to Fischer are simult,a- neously produced in the osazone reaction, could be detected in the fltrates.It had not escaped attention that the derivatives might possi- bly be hydrazides resulting from condensation with a -C(OH):C(OH)-group, and they were being investigated from this point of view. ‘70. 66 Note on the oxidation of certain acids in presence of iron.” By Henry J. Horstman lenton, M.A. It has been shown in several previous communications ((rrans., 1894, 65,899 ; B. A. Report, 1895, &c.) that when tartaric acid is oxidised in presence of a small quantity of ferrous iron, one molecule of the acid loses two atoms of hydrogen, giving rise to dihydroxymaleic acid. The most effective oxidising agent for the purpose is hydrogen dioxide, but the result is also brought about by chlorine, hypochlorites, bromine, &c., and by atmospheric oxygen in presence of sunlight.The presence of ferrous iron is essential, but its proportion seems to bear but little relation to the yield of acid in the ordinary course of pre- paration, the action being, in fact, what is usually termed catalytic. It is necessary that the addition of iron shall precede that of the oxidising agent. From the fact that dihydroxymaleic acid, on heating with water, yields glycollic aldehyde, and that this readily condenses to a hexose, it is evident that the change may afford information with regard to the natural formation of carbohydrates. The production of dihgdroxymaleic acid from tartaric acid is most easily represented by assuming the removal of the two non-hydroxylic hydrogen atoms : C,H,(OH),(CO,H), -H2= C,(OH),(CO,H),.It is true that dextrotartaric acid would be expected, in this manner, to yield a fumaroid instead of a maleoid acid; but it is quite possible that ‘ stereomeric’ change takes place during one of the stages of preparation, and in any case this objection can hardly be considered a serious one, bearing in mind the large number of known exceptions (Michael, J.prakt. Chern., 1892, 46, 400). While seeking for a chemical explanation of the part played by the iron, the following may be offered as a provisional suggestion. The two non-hydroxylic hydrogen atoms in tartaric acid may be supposed to possess feebly acid functions owing to the neighbourhood of the C0,H-and OE-groups, and it is possible that an atom of divalent iron may replace these two hydrogen atoms, giving the compound : CO,H*C(OH)<e>C(OH)* C0,H.On addition of the oxidising agent the iron atom assumes the trivalent state, and can therefore no longer be ‘retained.’ The result is an unsaturated acid, and the iron enters into solution as a ferric salt, e.g., ferric tartrate. Dihydroxymaleic 120 acid readily reduces ferric salts in the cold, experiment indicating that two atoms of iron are reduced by one molecule of the acid, so that the ferrous iron is regenerated at the expense of a portion of the acid. A large number of the conimoner acids have been investigated czs regards their 1)ehaviour in this respect. In addition to ,211 the now hydroxylic acids cxaminecl, lactic, rnalic, citric, and tczrtronic acitls give negative results.If,however, the above explanation be accepted, it is evident that the production of the violet coloration would only be expected in the CRS~of those acids the inolecules of which contain at least two CH(0H)-groups. Nucic and saccliaric acids might therefore be expected to yield positive results, and recent experiments have showii that this is the case, Coth these acids, when treated in the cold with i~ limited quantity of hydrogen dioxide in presence of ferrous iron, give intense violet colorations. Attempts are being ivade to isolate t’he oxidation products, which appear to be even less stable, however, than diliydroxyinaleic acid.DISCUSSION. Dr. ARMSTRONGthought a more probable explanation of the part played by iron to be that the iron salt becanie added to the carboxylic group; if changes then occurred such as he had suggested take place when optical inversion is effected by hydrolytic agents (liuns., 1896, 69, 1399), it would be easy to understand why clihydroxyinaleic acid mas obtained instead of the fumaric derivative. Mr. F~TON,referring to the suggestion he had made, said that replacement of non-hydroxylic hydrogen atonis by metals might also occur in Feliling’s and other similar solutions. In experiments with equal molecular quantities of dihydroxytartrates and tartrates, it had been found that the power of retaining copper in solution in the presence of alkali is very much greater in the latter case, although the reverse might be expected if replacement occurs in the alcoholic hydroxyl groups as is commonly supposed, *71.Properties and relationships of dihydroxytartaric acid. Part 11. Metallic Salts.” By Henry J. Horstman Fenton, M.A. The only metallic dihydroxytartrate which appears to have been prepared and studied is the sodium salt-the supposed barium salt being probably a mixture. Several other salts of the acid are now described. It is shown that the solubilities of the normal salts of sodium, potassium, rubidium, and cmium increase with the rise in atomic weight oE the metal. The lithium salt is exceptional, its solubility being greater than that of the sodium salt.The differences in solubility of these salts may perhaps be of service in separating the metals of the alkalis. Solutions of soluble dihydroxytartrates act as powerful reducing agents towards salts of silver, copper, and mercury, but are them- selves reduced to clihydroxymaloic acid by stannous and ferrous salts. *72. ‘(The affinity-constants of dihydroxymaleic, dihydroxyfumaric, dihydroxytartaric, and tartronic acids.” By S. Skinner, M.A. Tho affinity-constants have been determined from the conduc-tivity of the nqrieous solutions. The determination in the case of these acids, with the exception of tartronic acid, presents special difficulty as their solutions undergo gradual decomposition. The con- stants found are compared with those of malonic, succinic, fumaric, maleic, and tartaric acids, and it is shown that an increase in the value of the constant occurs :-(1) on the introduction of hydroxyl groups ; (2) for the lower members of the series of dibasic acids ; (3) for the unsaturated acids as compared with their saturated isologues.DISCUSSION. Dr. WALLACE objected to the explanation given OF the nature WALKER of the curves on the ground that in the production of carbon dioxide and glycollic aldehyde from dihydroxymaleic acid, the concentration of the supposed cat’alyser is decreasing at the same rate as that of the negative ion. The reaction would therefore be bimolecular, and its curve not rectilinear but one represented by an equation of the second degree.Mr. FENTONasked whether the results obtained with dihydroxy-mdeic acid could be explained by the suggestion, advanced in a previous communication, that combination with a molecular proportion of water occurs on dissolution with the production of the unstable trihydroxy- succinic acid. Mr. SKINNER,in reply, recognised that explanations of the behaviour of dihydroxymaleic acid other than that adopted in the paper were possible, but he was not prepared to say how far they would be of assistance in elucidating the results of the conductivity experiments. *73. ‘‘Note on the enolic and ketonic forms of ethylic acetoacetate.” By R. S. Morrell, M.A., Ph.D., and J. M.Crofts, B.A., B.Sc. The authors find that the purple oil obtained by the action of anhydrous ferric chloride on ethylic acetoacetate is decomposed by water in the presence of ether into ferric chloride and the ketonic 122 ethereal salt, The ether is found to contain the ketonic and not the enolic form, as would be expected.To identify the ketonic form, the method given by Schiff and Bertini (Bey., 1898, 31,207) is employed. The ethylic benzalanilineacetoacetato is found to have the composition, melting point (78O), and properties of the ketonic form. The tauto- meric change is probably due to the fact that the ferric chloride compound of ethylic acetoacetate, when decomposed by water in the presence of ether, produces hydrochloric acid, which converts the enolic into the ketonic form.The authors mentioned in a previous paper that ethylic benzaldi- acetoacetate formed a purple oil with ferric chloride in benzene solu- tion, whereas, in alcoholic solution, there was no such coloration. This oil has been obtained in the solid form and is being investigated on the lines just indicated for the ethylic acetoacetate compound. "74. ''The resolution of tetrahydropapaverine into its optically active components." By William Jackson Pope and Stanley John Peachey. Goldschmiedt has shown that papaverine is optically inactive and is, in all probability, an isoquinoline derivative of the constitution R(OMe)*CH:Q*CH:CH*fl yH:CH*fj*OMe C(OMe)*CH:C C*CH,*C=CH*C*OMe' This formula does not contain an asymmetric carbon atom and, up to the present, no optically active derivative of papaverine has been described. Amongst the derivatives of papaverine prepared by Gold- schmiedt (Mmats., 1886, '7, 495) is a tetrahydropapaverine, C,,H2,N0, to which, on the basis of the above constitution, the formula y(0Me) CH:F*CH,*CH2*rH yH:CHf*OMe C(OMe)*CH: C -CH*CH2*C=CH*C* OMe must be assigned, since, on reducing isoquinoline derivatives, hydro- genation takes place in the pyridine nucleus, On this assumption, tetrahydropapaverine contains an asymmetric carbon atom, and it should therefore be possible to separate the optically inactive compound into two enantiomorphously related isomerides, and thus obtain evidence confirming the constitution which Goldschmiedt has assigned to papaverine. In 'splitting ' an externally compensated base into its enantio-morphously related components, the dextrotartrate is almost invariably employed ;it would seem preferable, however, on various grounds, to make use in such cases of the dextrobromocamphorsulphonic acid described by Kipping and Pope (TTans.,1893, 63,584).Dextrobromo-camphorsulphonic acid is a far more powerful acid than tartaric acid, and hence might be expected to yield better characterised and more 123 easily isolated salts than the latter, with the further advantage that witha monobasic acid there is usually no tendency to form two classes of salts. Dextrobromocamphorsulphonic acid is conveniently prepared from the ammonium salt by conversion into the barium salt and careful precipitation of the solution by sulphuric acid.After filtration, the strength of the resulting solution is determined by titration. Tetrahydropapaverine is boiled with rather more than the calculated quantity of dextrobromocamphorsulphonic acid dissolved in a large quantity of water. Ultimately, the whole dissolves, and, on cooling, long needles of laevotetrahydropapaverinedextrobromocamphorsulphon-ate, C20H25N04,C10H14Br0*S03H,crystallise out. Further quantities of this salt are obtained, mixed with increasing quantities of the more soluble dextrotetrahydropapaverinedextrobromocamphorsulphonate,on concentrating the mother liquors. The two salts are readily separated by crystallisation from boiling water. Acevotetrahydropapaverine dextro6rornocamphorsuZphonate crystallises readily from water, in which it is sparingly soluble in the cold, in long, colourless, anhydrous needles melting with decomposition at 295-298'; it is somewhat more soluble in absolute alcohol, but insoluble in most other organic solvents.In a 0.3per cent. absolute alcoholic solution, it has the specific rotation of about [aID= -30'. Dextrotetvahydropapaverhae dextrobromocarnphormdphonate separates from solution as a resin which could not be obtained crystalline; when purified by repeated separation from its boiling aqueous solution and dried in the air, it forms a gritty, amorphous powder. hwotetrahydropapaverine, C20H25N04,separates on cooling a hot aqueous solution of its dextrobromocamphorsulphonateto which excess of ammonia has been added ; it crystallises from boiling dilute alcohol in colourless, minute, six-sided plates containing water which melt at 223'.The large flat face of the crystal is perpendicular to the acute bisectrix of a very small axial angle and of negative double refraction ; the material has the specific rotation [ = -149.5' in a chloroform solution containing 0,7987 grams per 25 C.C. The dextrotetrahydro-papauerine separated from itsdextrobromocamphorsulphonateresembles the laevo-isomeride in all respects, but is of opposite rotation. Inactive tetrahydropapaverine melts at 200-201°, and at ordinary temperatures is crystallographically different from its optically active components; it is, therefore, a racemic compound in the sense of Kipping and Pope's definition (Trans., 1897, 71, 989) It is formed on crystallising a mixture of equal weights of the two optically active isomerides from dilute alcohol.The salts of racemic, dextro- and lsevo-tetrahydropapaverineare being investigated, and experiments on other optically inactive alkaloids and their reduction products are in progress. 124 75. Molecular weights of permanganates, perchlorates, and periodates in solution.” By J. Murray Crofts, B.A.,B.Sc. The molecular weight of potassium permanganats in solution has been determined only by the specific conductivity method. In view of the close relationship between manganese and chlorine indicated by the periodic classification of the elements, it was thought that further investigation of the molecular weights of these substances in solution would be of interest.The method adopted was that devised by Lawenherz (Zeit.physik. Chem., lS95, 18,70), in which Glauber’s salt is the solvent employed. In this solvent sodium salts cannot undergo dissociation. The methods by which practically pure crystalline sodium permanganate and the very deliquescent sodium perchlorate were obtained are described. Determinations with both the sodium and the potassium salts of the acids were made, and the results point to the formula MMnO, for permanganates, and M’CIO, for perchlorates. For periodates (meta- periodates) the potassium salt only was used, and the constant obtained indicated KIO, as the formula, The results afford additional evidence for the inclusion of manganese with the halogens in group VII.of the periodic classification. The author is inclined to advocate Spring’s formula for perchloric acid (Bull. Acad. Belg., [ii], 39,887), and a corresponding expression for permanganic acid, the chlorine and manganese atoms being regarded as heptavalent in these compounds. 76. “The action of chlorine on pyridine.” By W. J. Sell, M.A., F.I.C.,and F. W. Dootson, M.A. In this communication the results are given of a repetition, in part, of the work of Keiser (Am. Chem. J., 1886, 8, 308), undertaken primarily with the object of comparing his dichloropyridine hydro- chloride with the trichloropyridine, melting at 7 1-72’, obtained by the authors by the action of phosphorus pentachloride on pyridine (Proc., 1898, 14,110).In consequence of the results obtained, the work was somewhat ex-tended, and it is shown that (1) an additive compound of chlorine and pyridine is formed, the constitution of which is not yet establiahed ; (2) Keiser’s dichloropyridine hydrochloride is a trichloropyridine ;(3) others of the chloropyridines seem to be formed in small amount ;(4) the compound, C,H,NCl, described by Keiser as an addition product of chlorine and pyridine, is pyridine hydrochloride. 125 77. The oxidation of paranitrotoluenesulphonio acid to dinitro- stilbenedisulphonic acid and to paranitrobenzaldehydortho-sdphonic acid.” By R.Herz and W.H. Bentley. In this paper the authors describe their experiments on the oxida- tion of sodium paranitrotoluenesulphonateby sodium hypochlorite. By using much less caustic soda than Green and Wahl (Bey., 1897, 30, 3097), they find that the product of oxidation is almost entirely sodium dinitrostilbenedisulphonate, and that sodium dinitrodibenzyl- disulphonate does not appear to be produced. The sodium, silver, barium, and lead salts, as well as the acid, have been prepared and examined. The authors are unable to accept the views of Ris and Simon (Ber., 1898, 31, 354) on the constitution of the stilbene derivative, acd from a determination of the amount of potassium permanganate required for its oxidation, maintain that it is a dinitro- and not a nitrosonitro-compound, They found, independently of Green and Wahl, that, on oxidising sodium dinitrostilbenedisulphonate in the cold with potassium permanganate, sodium paranitrobenzaldehydortho-sulphonate is formed. This substance possesses the properties of an aldehyde, and forms yellow, crystalline compounds with phenylhydr- azine and semicarbazide.78, Determination of molecular weights :-modification of Lands-berger’s boiling point method.” By James Walker and John S. Lumsden. The authors propose a modification of Landsberger’s method (Ber., 1898,31,-458)which consists essentially in measuring the volume of the solution after the boiling point has been determined, instead of ascer-taining its weight. This is effected by graduating the boiling tube, and permits of a number of successive experiments being made with the same quantity of substance.Only one weighing is necessary for fhe whole series, which occasions a considerable saving of time, making it possible to obtain four or five determinations in the course of half an hour. The accuracy is comparable with that of the Victor Meyer vapour density method in ordinary circumstances. 126 ADDITIONS TO THE LIBRARY. I. Donations. Goode, George Brown (Editor). The Smithsonian Institution, 1846-1896. The History of its First Half Century. City of Washington, 1897. Royal 8vo. Pp. x+856, with 26 full-page illustrations. Smithsonian Publication No. 1086. Howe, Jas. Lewis. Bibliography of the Metals of the Platinum Group :Platinum, Palladium, Iridium, Rhodium, Osmium, Ruthenium.City of Washington, published by the Smithsonian Institution, 1897. 8vo. Pp. 3 18. From Smithsonian Miscellaneous Collections, 38, (No. 1084). Copy of Jubilee Medal in bronze. From M. Carteighe, Esq, Neumann, Bernhard. The theory and practice of Electrolytic Methods of Analysis, translated by J. B. C. Kershaw. Pp. x+254. London 1898. From the Publishers. Bottone, 8. R. Radiography and the X-rays in practice and theory with constructional and manipulatory details. Pp. x+ 176. London 1898. From the Publishers. Obach, E. F. A. Cantor Lecture on Gutta Percha. Pp. 102. (Re-printed from the JournaZ of the Society of Arts.) London 1898. From the Author. 11. By Purchase.Paracelsus. The hermetic and alchemical writings of Aureolus Philippus Theophrastus Bombast of Hohenheim, called Paracelsus, edited by A. E. Waite. 2 vols. 4to. Pp. xvi + 394 and viii + 396. London 1894. The Hermetic Museum. The illustrations produced in facsimile. Containing translations of the following works. The Golden Treatise concerning the Philosopher’s Stone. The Golden Age come back. The Sophic Hydrolith, or Water Stone of the Wise. The Demonstration of Nature. A Philosophical Summary. The Path of the only Truth. The Glory of the World, or Table of Paradise. The Generation of Metals. The Book of Alze. Figures and Emblems concerning the Philosopher’s Stone. The Practice and Keys of Basil Valentine. The Ordinal of Alchemy.The Testament of John Cremer, sometime Abbot of Westminster, 127 The New Light of Alchemy. The Sulphur of the Philosophers. An Open Entrance to the Closed Palace of the King. A Subtle Allegory concerning the Secrets of Chemistry. The Metamorphosis of Metals. A Short Guide to the Celestial Ruby. The Fount of Chemical Truth. The Golden Calf. The All-wise Doorkeeper. 2 vols. 4to. Pp. xi + 357 : and 352. London 1893. Collectanea Chemica, being certain select treatises on Alchemy and Bermetic Medicine, by Eirenaus Philalethes, Francis Anthony, George Starkey, Sir George Ripley, etc. The Secret of the Immortal Liquor called Alkahest. Aurum Potabile. The Admirable EfEcacy of the True Oil of Sulphur Vive. The Stone of the Philosophers.The Bosom Book of Sir George Ripley. The Preparation of the Sophic Mercury. 8vo. Pp. 160. London 1893. Benedictus Figulus. A Golden and Blessed Casket of Nature’s Marvels, Concerning the blessed mystery of the Philosopher’s Stone. 8vo. Pp. xxxi + 361. London 1893. Janus Lacinius. The New Pearl of Great Price. A treatise con-cerning the treasure and most precious stone of the philosophers. Illustrated with symbolical designs. 8vo. Pp. xi +441. London 1893. Edward Kelley. The Englishman’s two excellent treatises concerning the Philosopher’s Stone, together with the Terrestrial Theatre of Astronomy. 8vo. Pp. lxvii + 153. London 1893. Basilius Valentinus. The Triumphal Chariot of Antimony, with the commentary of Theodore Kerckringius.Engraved title and plates. 8vo. Pp. xxxiii + 204. London 1893. Jones, H. C. The Freezing-Point, Boiling-Point, and Conductivity Methods. Pp. vii+64. Easton, Pa., 1897. Threlfall, Richard. On Laboratory Arts. Pp. xii + 338. London 1898. Journal of the Royal Agricultural Society. Vols. I-XXV, 1st Series, with General Index, 1840-1864. Vols. I-XXV, 2nd Series, with General Index, 1865-1889. Vols. I-VI, 3rd Series, 1890- 1895. Pamphlets. Liversidge, A. Abbreviated names for certain Crystal forms. Models to show the Axes of Crystals. -Variation in the amount of free and albuminoid Ammonia in 128 Waters, on keeping; On the Corrosion of Aluminium. -Crystallised Carbon Dioxide ; on the Internal Structure of Gold Nuggets ;Contributions to the Bibliography of Gold; Experiments on the Waterproofing of Bricks and Sandstones with Oils ;Experiments upon the Porosity of Plasters and Cements.(Reprinted from the Transactions of the Australasian Association for the Advancement of Science.) -On some New South Wales and other Minerals. Note No. 7. On the Amount of Silver and Gold in Sea Water. -The Removal of Gold and Silver from Sea Water by Muntz Metal Sheathing. (Reprinted from the Transactions of the R.S.N.S.W.) BANQUET TO PAST PRESIDENTS. It has been arranged by the Council that the Society shall entertain at a Banquet at the Hdtel MBtropole, on June 9th, the following Past Presidents who have completed a period of fifty years Fellowship of the Society :-Lord Playfair : Sir J.H.Gilbert : Sir E. Frankland : Prof. Odling : Sir F.A. Abel, Bart. : Dr. A. W. Williamson: Dr. J. H. Gladstone. The Secretaries will be glad to hear as soon as pos-sible, and in any case not Zuter thun Hay 14th) from those Fellows who intend to be present, and also if they desire to bring guests (at present limited to two). The price of tickets will be One Guinea each, including wine. They will be forwarded on receipt of a remittance for the number of tickets required, addressed to the Assistant Secretary, Chemical Society, Burlington House, W. RESEARCH FUND. A meeting of the Research Fund Committee will be held in June. Applications for grants, accompanied by full particulars, should be sent to the Secretaries on or before June 6th. At the next meeting, on Thursday, May 19th) the following papers will be communicated by the authors. The action of formaldehyde on amines of the naphthalene series,” By G. T. Morgan, B.Sc. ‘‘ On the constitution of oleic acid and its derivatives. Part I.” By F. G. Edmed, B.Sc. RICHARD CLAY AND BOW, LIMITED, LONDON AND BUNQAY.
ISSN:0369-8718
DOI:10.1039/PL8981400115
出版商:RSC
年代:1898
数据来源: RSC
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