Studies in polarography. Part 1.—The rotating platinum electrode

Ferrett, D. J.; Phillips, C. S. G.

doi:10.1039/tf9555100390

Cited by 16 publications

(2 citation statements)

References 2 publications

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“…However, in the presence of metal ions, in particular T1, blank currents were sometimes obtained at voltages too low for metal deposition. The cause of this remains obscure, but what may be a similar type of behavior has previously been noted (18). If the electrodes were alternately plated and stripped several times these blank currents were nearly always entirely eliminated.…”

Section: ]~Xperiment~kl ~Roceduresupporting

confidence: 60%

Kinetics of Metal Deposition

Pavlopoulos¹,

Strickland²

1957

J. Electrochem. Soc.

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Current‐voltage curves arising from metal deposition were determined using a variety of stationary microelectrodes, mostly vertical wires, and the concentration polarization approximated that expected from convective diffusion. The Nernst diffusion equation is not valid, and current densities I , in amp/cm2, for systems containing excess inert electrolyte are given by the equation: I=1.4nFD0.8C−Ce1.2 )(12r+1δ This can be used to calculate limiting current densities during alloy formation and to characterize deposition processes as reversible or irreversible. Graphical methods can be uised to determine transfer coefficients and rate constants, for a markedly irreversible process

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Section: ]~Xperiment~kl ~Roceduresupporting

confidence: 60%

Kinetics of Metal Deposition

Pavlopoulos¹,

Strickland²

1957

J. Electrochem. Soc.

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“…For solutions of higher pH, however, their results gave slopes greater than 0.0296 v, or a < 1. According to Kolthoff and Lingane ( 16), a slope greater than the reversible value indicates a measure of Jrreversibility in the electrode process, an assumption accepted by other workers (17). In consequence, Kolthoff and Jordan concluded that the anodic oxidation of iodide ion becomes increasingly irreversible as the pH of the solution increases.…”

Section: Oxidation Of Iodide Ionmentioning

confidence: 95%

The Kinetics of the Iodine Redox Process at Platinum Electrodes

Newson

Riddiford

1961

J. Electrochem. Soc.

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Three paths for the iodine redox process at platinum electrodes are discussed with reference to stationary current/potential curves obtained for the cathodic reduction of the tri‐iodide ion in potassium iodide solutions. It is shown that the process follows the path originally proposed by Vetter, the slow stage being the transfer of an electron from the platinum to an adsorbed iodine atom, and that the degree of reversibility of the process increases as the concentration ratio of tri‐iodide to iodide is decreased. The apparent energy of activation for the over‐all process is 5.3 kcal·mole−1 for solutions containing only potassium iodide and tri‐iodide. The results, and those of other workers, indicate that the electrode surface is nonuniform.

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The oxidation potentials of phenolic and amino antioxidants

Penketh

1957

J. Appl. Chem.

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A simple and rapid polarographic method of measuring the relative oxidation potentials of organic compounds has been developed, and values for a large number of phenolic and amino compounds have been determined to find whether any relationship exists between Oxidation potential and antioxidant activity. Buffered electrolytes a t various pH levels were used and when the determined potentials are plotted against the pH of the electrolyte, most monohydric phenols give straight-line graphs which correspond closely to the theoretical equation for oxidations in which hydrogen ions are involved in the electrode processwhere E, is the standard oxidation potential.' break point ' at about pH 6 , and have different slopes above and below this value.Other phenolic compounds give graphs showing a Most of the hydroxyanisoles and amines exhibit slight curves when potential is plotted against pH. Sufficient alkylated phenols have been examined to establish definite trends in the effects of substitution; thus ortho and para substituents lower the oxidation potential by about 0.08 v while meta substituents have a much smaller effect. These effects are largely additive and the oxidation potentials of polyalkylated phenols can be predicted from a knowledge of the effects of the separate substitutents. With certain 2 : 4 : 6-compounds containing large groups, the measured oxidation potential is higher than that predicted and this is attributed to stenc hindrance.In general, as the oxidation potential decreases, the antioxidant activity increases. The relationship is not invariably close and, with certain substituted hydroxyanisoles, the antioxidant activities measured are even higher than would be anticipated from their low potentials. No compound of high antioxidant activity has been found to possess a potential higher than 0.70 v and hence the polarographic method should prove to be valuable for a rapid preliminary assessment of possible antioxidants.

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Studies in polarography. Part 1.—The rotating platinum electrode

Cited by 16 publications

References 2 publications

Kinetics of Metal Deposition

Kinetics of Metal Deposition

The Kinetics of the Iodine Redox Process at Platinum Electrodes

The oxidation potentials of phenolic and amino antioxidants

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