An acid `HA` ionizes as `HAhArrH^(+)+A^(-)` The `pH` of `1.0 M` solution is `5`. Its dissociation constant would be

An acid HA ionises as HA hArr H^(+)+A^(-) The pH of 1.0 M solution is 5. Its dissociation constant would be :

An acid HA ionises as, HAiffH^(+)+A^- The pH of 1.0 M solution is 5. its dissociation constant would be

An acid HA ionises as HA overset(rightarrow)(leftarrow) H^+ + A^- . The pH of 1M solution of this acid is 6.The dissociation constant of this acid would be

The pH of 0.1 M solution of an organic acid is 4.0. Calculate its dissociation constant.

The degree of dissociation of an acid HA in 0.1 M solution is 0.1%. Its dissociation constant is

The ph of 1 M aqueous solution of the weak acid HA is 6.0.Find its dissociation constant.