The `[H+]` of a solution is `10^(-8)`. Its `pOH` is

The [OH^-] in a solution is 1xx10^(-8) . The pH of the solution is

The P^(H ) of a solution is 6. Its [H_(3)O^(+)] is decreased by 1000 times. Its P^(H) will be

The P^(H) of a solution is 3.602. Its H^(+) ion concentration is

The pH value of solution is 2. If its pH value is to be doubled then the H+ ion concentration of the original solution has to be decreased by :

At 298 K, the [H_(3),O^(+)] of a solution is 2 xx 10^(-9) M. The nature of the solution is

The H ion concentration of a solution is 4.75 xx 10^(-5) M. Then the OH ion concentration of the same solution is

Calculate the pH of solution that contains [H^(+)]=10^(-8)M is -

The pH of a solution increased from 3 to 6 . Its [H^(o+)] will be

The pH of a solution is 5. to this solution acid was added so that its pH value bcomes 2.0. The increase in H^(+) concentration is :

At 25^(@) C dissociation constants of acid HA and base BOH in aqueous solution are same. The pH of 0.01 M solution of HA is 5. The pOH of 10^(-4) M solution of BOH at the same temperature is :