Abstract
The iron dissolution and passivation was studied in sulphate solution containing different oxygen concentrations and within the range 3 < pH < 6. The measurements were carried out cyclic voltammetrically and under steady-state polarization conditions using a rotating disc electrode of highly pure recrystallized iron. The obtained kinetic data can be explained mainly by the iron dissolution and passivation mechanism proposed previously for oxygen free solutions. This mechanism is characterized by the formation of different oxide intermediates [Fe(OH) n ] ads, with n = 1,2,3 depending on the pH and the potential. Above a critical pH-value, the diffusion controlled oxygen reduction is the dominating cathodic process, and the anodic iron dissolution and passivation is inhibited by the time-dependent formation of three-dimensional porous oxide layers on the electrode surface. In neutral solutions the iron dissolution and passivation mechanism turns to that encountered in alkaline media.
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