Al specimens were anodically oxidized in solutions of (1) 10%-H
2SO
4, (2) 2%-H
2C
2O
4⋅2H
2O and (3) 10%-H
2SO
4+2%-H
2C
2O
4⋅2H
2O by applying a constant c. d. of 9.4mA/cm
2 at 27°C, and the time-variation in the ammount of dissolved Al ions,
Wd, was measured by the oxinate extraction method. The weight and geometrical structure of the oxide were also examined at time intervals during anodization. The applied anode potentials were 12.0, 45.0 and 13.5V (vs·SCE) for solutions (1), (2) and (3), respectively. The geometrical structure (cell size, pore-wall thickness, pore-radius etc.) of the porous oxide formed in solution (3) was much more like that formed in solution (1) than to that formed in solution (2). The densities of the oxides formed in solutions (1), (2) and (3) were estimated to be 2.7, 2.8and 3.0, respectively. The dissolution rate of oxide at the pore-wall,
vs, and that at the pore base
vb, were calculated from
Wd in the manner reported previously. The result shows that
vs decreases from solution (1) through (2) to (3), whereas
vb decreases in the order, (2), (3), (1). Thus, it is advantageous to add a small amount of oxalic acid to sulfuric acid anodizing solution. The reason of this is summarized as follows: a) Current effciency for the formation of oxide considerably increases. Powdering of the oxide could be prevented because of a small value of
vs. b) Electric power does not increase very much, and it is much smaller than that consumed in the anodization in oxalic acid solutions. c) Density of oxide increases remarkably and it is even higher than that obtained by anodization in oxalic acid solutions.
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