The dissociation constant of a weak monobasic acid in `0.01 M` solution is `10^(-8)`. What is its `[OH^(-)]` concentration?

The dissociation constant of a weak monoprotic acid, which is 0.01 % ioniosed in 1 .00M solution , is

The dissociation constant of a weak monoprotic acid, which is 0.01 % ioniosed in 1 .00M solution , is

The dissociation constant of a weak monobasic acid is 3.5 xx 10^(-8) . Calculate its degree of dissociation in 0.05 M solution.

The dissociation constant of a monobasic acid is 1.0xx10^(-9) . The pH of its 0.1 M aqueus solution is:

The dissociation constant of a weak acid is 10^(-6) . Then the P^(H) of 0.01 Nof that acid is

The dissociation constant of a weak acid is 10^(-6) . Then the P^(H) of 0.01 Nof that acid is

The dissociation constant of a weak monobasic acid K_a is 1 xx 10^-5 . The pH of 0.1 M of that acid would be

pH of a weak monobasic acid is 3.2 in its 0.02 M solution. Calculate its dissociation constant.