Oxides on the Silver Electrode

Wales, Charles P.; Burbank, Jeanne

doi:10.1149/1.2427169

Cited by 57 publications

(49 citation statements)

References 4 publications

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“…8 are not linear (Fig. [2], takes over (13). The ratio is comparatively large initially at the lower charging currents and then it decreases; at high charge currents the ratio increases.…”

Section: Oxidation Of the Electrodesmentioning

confidence: 92%

The Silver-Silver Oxide Electrode

Wales

1961

J. Electrochem. Soc.

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Silver electrodes were oxidized anodically at 25~ in 35 or 50% KOH at constant charge currents that ranged from the 1/2 to 40 hr rates. The electrodes were given both partial and complete charges. Except at a low charging rate the capacity was higher in 35% KOH than at 50% KOH. Oxidation was highly efficient at the first two potential plateaus. During a charge at the Ag=O/AgO plateau initially Ag~O oxidizes to AgO and then the prevailing reaction is Ag oxidizing to AgO. Simultaneously some AgO reacts with Ag to give Ag=O. Under certain discharge conditions AgO may reduce directly to Ag, with Ag20 forming as a secondary product.) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 130.56.64.29 Downloaded on 2015-03-13 to IP ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 130.56.64.29 Downloaded on 2015-03-13 to IP

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“…8 are not linear (Fig. [2], takes over (13). The ratio is comparatively large initially at the lower charging currents and then it decreases; at high charge currents the ratio increases.…”

Section: Oxidation Of the Electrodesmentioning

confidence: 92%

The Silver-Silver Oxide Electrode

Wales

1961

J. Electrochem. Soc.

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“…Some cufi-uaiin in investigations of the silver electrode has beo, cau sed by the report of Jones and Thirsk (6) of what they believed was the x -ray diffracti-n patern of AgO. The pattern reported has since been shown to be that of the so-called silver peroxysulfate Ag 7 OSO 4 and not AgO (7). Bi iggs, Dugdale, and Wynne-Jones (2) confirmed that the final product of anodizing Ag in H 2 SO 4 was mainly the peroxysulfate and not AgO.…”

Section: Application Of This Cell To the Silver Electrode In Koh Solumentioning

confidence: 99%

“…In earlier work at this Laboratory, a silver electrode was removed from a cell-following various amounts of charge or discharge and then examined by x-ray diffraction after rinsing the electrode in water and blotting dry (7). In alkaline electrolyte, the only materials identified were Ag, Ag 2 0, and AgO.…”

Section: Application Of This Cell To the Silver Electrode In Koh Solumentioning

confidence: 99%

Electrolytic Cell for X-Ray Diffraction Studies of Electrode Phenomena

Wales¹,

Burbank²

1964

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“…Much research work was conducted to better understand the charge-discharge behaviour of AgO as an active material for alkaline storage and primary batteries containing silver electrodes [10][11][12][13][14]. Many research works revealed that there are different types of silver oxides and that the behaviour of silver electrode in alkaline electrolyte is fairly complicated.…”

Section: Introductionmentioning

confidence: 99%

Separation of Silver by Ozone Oxidation of Silver Nitrate Solution

Nishimura¹,

Hoshoda²

2008

Canadian Metallurgical Quarterly

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The oxidative precipitation of silver(I) species with ozone has been studied for the separation of silver ion from aqueous nitrate solutions in the range of pH 2 to 12 at temperatures up to 80°C. The X-ray diffraction analysis showed that silver oxysalt, Ag 7 O 8 NO 3 , from acidic solutions and silver oxide, AgO, from neutral or alkaline solutions were produced as the final solids, respectively. Their particles were assessed by a scanning electron microscope (SEM). The progress of the reaction was continuously monitored by measuring the oxidation reduction potential (ORP) and the amount of NaOH added to maintain solution pH. A rise in pH of solution and ozone partial pressure promotes the reaction. A rising reaction temperature, however, results in a considerably suppressed reaction.Résumé -On a étudié la précipitation par oxydation de l'espèce argent(I) par l'ozone pour la séparation de l'ion argent provenant de solutions aqueuses de nitrate, dans la gamme de pH de 2 à 12 à des températures allant jusqu'à 80°C. L'analyse cristallographique par diffraction a montré que l'on produisait, comme solides finaux, l'oxysel d'argent, Ag 7 O 8 NO 3 , à partir de solutions acides et l'oxyde d'argent, AgO, à partir de solutions neutres ou alcalines, respectivement. On a évalué leurs particules au moyen d'un microscope électronique à balayage (SEM). On a surveillé continuellement le progrès de la réaction en mesurant le potentiel d'oxydoréduction (ORP) et la quantité de NaOH ajoutée pour maintenir le pH de la solution. Une élévation du pH de la solution et de la pression partielle de l'ozone favorise la réaction. Cependant, une remontée de la température de réaction a pour conséquence une réaction considérablement supprimée.

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Oxides on the Silver Electrode

Cited by 57 publications

References 4 publications

The Silver-Silver Oxide Electrode

The Silver-Silver Oxide Electrode

Electrolytic Cell for X-Ray Diffraction Studies of Electrode Phenomena

Separation of Silver by Ozone Oxidation of Silver Nitrate Solution

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