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

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

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

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 HA is 4.9 xx 10^(-8) . Calculate for a decimolar solution of acid:. OH^(-) concentration

The dissociation constant of a weak acid HA is 4.9 xx 10^(-8) . Calculate for a decimolar solution of acid:. OH^(-) concentration