Solubility Of Silver Research Articles

Solutions of soaps in organic solvents

The solubilities of silver and chromium soaps in nonaqueous solvents have been determined by a radiotracer technique. The metal soaps are sparingly soluble in nonaqueous solvents but more soluble in alcohols. The solubility data at different temperatures in benzene, toluene, and m-xylene has been used to determine the critical micelle concentration (c.m.c) of these soaps. Small amounts of methanol enhance the solubility of the metal soaps in benzene and the viscosity of soap solutions in methanol–benzene (15% methanol) showed the existence of micelles at high soap concentrations. The solubility of silver laurate in aqueous solutions of dioctyl sodium sulphosuccinate and Nonidet-P40 has been determined and the data was used to calculate the c.m.c. of aqueous surfactants.

The Solubility of Silver (II) Oxide in Alkaline Solutions

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A Chronopotentiometric Study of the Silver‐Silver Chloride and Silver‐Silver Bromide Systems

The dissolution of silver in its molten chloride and bromide was studied using a chronopotentiometric technique. The solubility of silver in molten and was evaluated by adding small amounts of silver to the salts until saturation was reached, as measured in situ, by anodic chronopotentiometry. The solubility of silver in its chloride at 520°C was 0.0123 mole % and in its bromide, 0.0118 mole % at 500°C. Analyses of the anodic chronopotentiogram wave shapes indicated that the oxidation of the soluble silver species in the chloride and bromide was a reversible one‐electron process. Diffusion coefficients for this species were determined to be in at 520°C and in at 500°C.

Melting and structural correlations of some thorium-rich eutectics

Thorium-rich alloys in the binary systems with copper, silver, gold, iron, cobalt and nickel have been examined. Eutectics not previously reported have been detected between thorium and Th 2Ag at 30 ± 1 at % silver and 1012 ± 12° C, thorium and Th 2Au at 20 ± 1 at % gold and 1100 ± 12° C, and thorium and Th 7Co 3 at 20 ± 1 at % cobalt and 1100 ± 12° C. Th 7Co 3 crystallised directly from the melt at 1188 ± 12° C. The solid solubility of silver, gold, iron and cobalt in thorium was found to be significantly lower than 2 % at the eutectic or peritectic temperatures. The peritectic formation of Th 7Fe 3 has been confirmed and the peritectic temperature was found to be 962 ± 12° C. The compositions of the eutectics previously reported between thorium and Th 2Cu and between thorium and Th 7Ni 3 have been confirmed but the present eutectic temperatures of 1037 ± 12° C and 1062 ± 12° C are significantly higher than those given in the literature. Experimental evidence is presented which suggests that this might be due to the impure nature of the material on which the earlier results were obtained. Information on thorium-rich eutectics in nineteen systems in which intermetallic compounds occur has been surveyed and it has been shown that, in general, the eutectic temperatures increase and the eutectic compositions become richer in thorium as the melting points of the compounds increase. Correlations between the melting points of the eutectics, electron concentration in the liquid, the crystal structure of the intermetallic compounds and the group in the periodic table to which the alloying elements belong have also been pointed out.

Diffusion and solid solubility of silver in single-crystal bismuth telluride

The anisotropic diffusion and the solid solubility of silver in single-crystal bismuth telluride have been measured by radioactive tracer techniques employing silver-110 and silver-111. The diffusion coefficient perpendicular to the cleavage planes is given by D tT = 5.1 +2.1 −1.6×10 −3exp( −0.92eV kT ) and that parallel to the cleavage planes by D t∥ = 5.4 +2.6 −1.7×10 −3exp( −0.45eV kT ) The solid solubility has a maximum of 1.5 × 10 20 atoms/cm 3 (2.5 atom per cent) and the variation of solid solubility with temperature is shown to be consistent with the existing knowledge of the silver-bismuth-tellurium system.

Silver/Silver Oxide Electrodes for Fuel Cells

MANY laboratories active in the field of fuel cell research have adopted the silver/silver oxide electrode as the oxygen electrode in conjunction with strong alkali (generally 20–40 per cent potassium hydroxide) electrolyte. There have been many investigations of the fundamental operating characteristics of such an electrode under current drain conditions, and various theories have been advanced to account for its behaviour. Although various polarization mechanisms have been considered, as in the work of Dirkse1, it is remarkable that the significant solubility of silver in strong potassium hydroxide has been systematically ignored. This solubility is adequately recorded in the work of Mathur and Dahr2, and of Johnston, Cuta and Garrett3 for room-temperature operation under quiescent conditions and a synopsis of these authors' results is given in Table 1.

On the mechanism of sulphurization of copper

The sulphidation of two copper–silver alloys containing 5 and 10 wt.% silver (Cu–5Ag and Cu–10Ag, respectively) was investigated over the temperature range 550–750°C in H2/H2S mixtures under sulphur pressures below the dissociation of Ag2S. External scales, composed mainly of cuprous sulphide, often containing some (Cu,Ag)2−xS islands, formed on both alloys. The corrosion kinetics were significantly affected by the detachment of the outer scales at temperature, as a consequence of the significant volume increase due to sulphidation. After scale detachment, sulphidation proceeded through a dissociative transport of sulphur in voids between the outer sulphide layer and the alloy substrate, yielding an abrupt decrease of the corrosion rate in all cases and modifying the composition of the reaction products in the case of Cu–10Ag. An increase of the volume fraction of the silver-rich solid solution in the subscale region with respect to the original alloy was observed in all cases. The silver islands coalesced to a continuous subscale layer only in the sulphidation of Cu–5Ag at 650 and 750° whereas, in all the other cases, they remained as particles in a Cu2S matrix. The peculiar corrosion behaviour of these alloys is attributed to the low solubility of silver in copper.

Ti-Ag系状態図について

The phase diagram of the titanium-silver system has been investigated in the whole range mainly by metallographic examination, X-ray analysis and the thermal analysis method. Only an intermediate compound TiAg was found to exist in this system by X-ray analysis and metallographic examination. The crystal structure of this compound was nearly similar to the report by R. J. Van Thyne et al. and a=4.078 Å, c=4.065 Å and c⁄a=0.996 were determined, A peritectic reaction beta-Ti+Liq.\ ightleftharpoonsTiAg occurs at 1045°C and beta-Ti decomposes into alpha-Ti and TiAg by eutectoid reaction: beta-Ti\ ightleftharpoonsalpha-Ti+TiAg. The eutectoid point was about 23 wt% silver and its temperature lies between 860° and 890°C. The solubility of silver in beta-Ti is about 53 wt% at peritectic temperature and the solubility in alpha-Ti is less than 12 wt% at room temperature but more than 13 wt% at eutectoid temperature. The intermediate compound TiAg extends from 68 wt% to 73 wt% silver at room temperature and its hardness was about 130 kg/mm2 VPN, but the compound was brittle to give any reduction by rolling and could work easily neither at room temperature nor higher temperature. On the silver-rich side, a eutectic reaction Liq.\ ightleftharpoonsTiAg+Ag was observed at 890°C and its composition was about 96 wt% silver. The whole phase diagram which was obtained by these experimental results as shown in Fig. 6.

On the Solid Solubility of Silver in Aluminium

Heating the specimens of aluminium-silver alloy which are in thermal equilibrium, from the room temperature to above the two phase boundary, the changes of specific heat and electrical resistance have been examined: from the characteristic changes of them due to the resolution of precipitated phase, the solid solubility curve or “solvus” of silver in aluminium has been determined. A remarkable change in the direction of the solvus at about 20 atomic percentage of silver and at 526°C which was for the first time observed by Raynor and Wakeman through their micrographic examination, has been reconfirmed. Besides, the energy of solid solution and accompanied entropy change have been determined and shown plotted against silver content from 1.3 to 50 atomic %. Both curves show a bending which is probably attributable to the effect of the electronic band structure of pure aluminium metal. The energy of valence electrons in the solid solutions has been calculated by means of the state density curve due to Matyas...

The Solubility of Silver in Mercury. II.

ADVERTISEMENT RETURN TO ISSUEArticleNEXTThe Solubility of Silver in Mercury. II.Robert E. DeRightRobert E. DeRightMore by Robert E. DeRightCite this: J. Phys. Chem. 1933, 37, 4, 405–416Publication Date (Print):April 1, 1933Publication History Published online1 May 2002Published inissue 1 April 1933https://doi.org/10.1021/j150346a001RIGHTS & PERMISSIONSArticle Views79Altmetric-Citations9LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (647 KB) Get e-Alerts