A Reproducible and Stable Silver-Silver Oxide Electrode

Hamer, Walter J.; Craig, D. Norman

doi:10.1149/1.2428537

Cited by 41 publications

(20 citation statements)

References 9 publications

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“…The porous characteristics of the hydrous Ag(1) oxide have been postulated by many authors [12,15,211. The present data allow the estimation ofa volume 2.5 times greater than the one currently admitted for the bulk oxide [9,20,29], and show that the hydrous A&l) oxide grows developing a "freezing in" state [30] whose grade of porosity depends on the sweep rate applied.…”

Section: Discussionmentioning

confidence: 68%

Electrochemical and ellipsometric data related to the formation of soluble silver (I) during the potentiodynamic polarization of polycrystalline silver in basic solutions

Zerbino

Teijelo

Vilche

et al. 1985

Electrochimica Acta

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SolubleAg(I) species is formed in the early stages of voharnmetric silver electrooxidation in 0.1 hi NaOH and 0.1 M NaOH + 1 M NaClO, solutions at WC, as demonstrated by the rotating ring-disc technique. This result allows a reasonable interpretation of ellipsometric data obtained for the anodiition of silver under different vohammetric conditions. Correspondingly, two anodic layers of different optical constants are electroformed. The hydrous Ag(I) oxide layer behaves as a porous structure with an average thickness of about 2.5 times greater than that of the anhydrous oxide.

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Section: Discussionmentioning

confidence: 68%

Electrochemical and ellipsometric data related to the formation of soluble silver (I) during the potentiodynamic polarization of polycrystalline silver in basic solutions

Zerbino

Teijelo

Vilche

et al. 1985

Electrochimica Acta

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“…Fortunately, Ag 2 O readily decomposes on heating, and as early as 1888 Carnelly and Walker [ 27 ] showed the decomposition of Ag 2 O is complete between 300° and 430° C. Lewis [ 28 ], Keyes and Kara [ 29 ], and Benton and Drake [ 30 ] measured the decomposition of Ag 2 O over a temperature range of 173° to 500° C with the results given in table 8 . By an extrapolation of Ins data Lewis calculated the decomposition pressure of silver oxide to be 5×10 −4 atm at 25° C. In a recent electrochemical study of the Ag,Ag 2 O electrode Hamer and Craig [ 31 ] obtained 2,723 cal for the free energy of decomposition of Ag 2 O at 25° C; this value corresponds to 0.988×10 −4 atm for the decomposition pressure of Ag 2 O at 25° C.…”

Section: Materials and Purificationmentioning

confidence: 99%

Determination of the value of the faraday with a silver-perchloric acid coulometer

Craig¹,

Hoffman²,

Law³

et al. 1960

J. RES. NATL. BUR. STAN. SECT. A.

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An accurate value of t he faraday has bee n deter min ed by the e lectrolytic dissolution of metall ic silver in aq ueous solu tions of perchloric acid. Standards of electric curren t mass, a nd time a s maintained by t he National Bureau of Standards were utili zed in th~ determinatio ns. Th e electri c c l1l'rent was m easured in terms of th e standards of cle ctromotive force and electrical resistan ce. Silver of hi gh purity, freed fr om oxygen, was used.The value of t he faraday was found to be faraday = 96516.5 ± 2.4 coulombs gram -equival e nt-1 (physical scale). faraday = 96490.0 ± 2.4 coulombs gram -eq ui valent-1 (chemical scale) .These values were obtained usin g 107.9028 ± 0.001 3 and 107.8731 ± 0 .0013 for t h e atomic weigh t of silver on t h e phys ica l and ch e mical scales, resp ectively . ' The electrochemical eq uiva lent of sil ver was found to be electrochemical equivalent of s ilver = 1.117972 ± 0.000019 milligram coulomb-I.This value may be used in a n alternate meth od of defining t h e ampere in absolute value, llamely, t hat steady current which will d issolve 1.117972 milligrams of silver per seco nd a nd de pends only on t he standards of mass and t ime. The indicated un cer tainties are overa ll limi ts of error based on 95 percent co nfidence limi ts for t he mean an d a ll owan ces for t he effects of kn own sources of possible systematic errol'. I . IntroductionThe classic m ethod for the determination of the faraday involves the electrolytic deposition of silver on platinum from an aqueous solu tion of silve)' nitrate. This method h as been extensively studied and tmder closely sp ecified condi tions [1] 1 was used for many years in defining the international amper e. In the original work at th e National Bureau of Standards the national standards of electric current mass, and time were used, and great emphasis wa~ placed on the r eproducibility of the method as a ch eck on the stability of th e existing standards of electromotive for ce (Weston cell) and electrical r esistan ce (mercury ohm). In 1916 Rosa and Vinal [2] sum.-m arized th e work that h ad been done with the silver coulometer not only in yielding a value of the faraday but also in ftttaining conditions wherein reproducible r esults could be obtained. At th at time the consensus was th at tIl e silver coulome ter gave highly accurate as well ftS reproducible r esults and yielded a value of the faraday acc ura te to within 0.001 percent (10 ppm).However , 4 years earlier (in 1912) vVashburn and B ates [3 ] h ad proposed ftn improved 2 iodine coulom-1 F igures in brackets indicate the literature references at th e end of this paper. 2 T he iodine eoulometC!· bad bren studied earlier by H elTOtul [4]. D ann eel 15J, Kreider [6J , and Gallo l7J b ut tbese experimenters did not cla im higb aecm aey for t heir \vork .eter for which high reproducibility and accuracy wer e elaimed. In 1914 Vinal and B ates [8,9] made a direct comparison of the silver and iodine coulometer s in the labor atories of NBS and found that the two...

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“…HgO can appear in two different colors (yellow or red) depending on its particle size [31]. The influence of the particle size on the electrode potential was reported to be negligible [32].…”

Section: Results and Discussion Preparation Of μ-Reference Electrodesmentioning

confidence: 99%

Hydrogel-based flexible micro-reference electrodes for use in alkaline and neutral pH solutions

Schimo

Grill

Kollender

et al. 2016

J Solid State Electrochem

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Two types of nonbreakable, flexible microreference electrodes filled with gel-electrolytes were prepared for use in solutions with alkaline and neutral pH. The electrodes are intended for electrochemical measurements, in which chloride-free conditions are important. Due to the flexible, bendable construction of the electrodes, electrochemical experiments at locations difficult to access with common reference electrodes are enabled. Hg|HgO-type electrodes were prepared from amalgamated Au wires, followed by oxidation of the amalgam, which is mounted in a PTFE tube filled with 0.1M NaOH solution immobilized in a PAA-g-PEO gel. The potential of this type of electrode was found to be 0.162 ± 0.002 V (SHE) at room temperature. Cu|CuSO 4 electrodes, consisting of a Cu wire immersed in a saturated CuSO 4 solution jellied with gelatin, showed a stable open-circuit potential of 0.312 ± 0.001 V (SHE). Further characterization of the electrodes was performed in terms of electrochemical impedance spectroscopy and micro-polarization measurements. As an alternative to the flexible electrodes, rigid electrodes in glass enclosure were fabricated in analogy to the flexible-type electrodes.

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A Reproducible and Stable Silver-Silver Oxide Electrode

Cited by 41 publications

References 9 publications

Electrochemical and ellipsometric data related to the formation of soluble silver (I) during the potentiodynamic polarization of polycrystalline silver in basic solutions

Electrochemical and ellipsometric data related to the formation of soluble silver (I) during the potentiodynamic polarization of polycrystalline silver in basic solutions

Determination of the value of the faraday with a silver-perchloric acid coulometer

Hydrogel-based flexible micro-reference electrodes for use in alkaline and neutral pH solutions

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