Given that `K_(w)` for water is `10^(-13)` `M^(2)` at `62^(@)`C, compute the sum of pOH and pH for a neutral aqueous solution at `62^(@)`C:

The sum of pH and pOH in aqueous solution is equal to

what is the value of PH + POH for any aqueous solution at 25^@C .?

The pH and pOH of 0.1 M aqueous solution of HNO_3 , are

The value of the ion product constant for water, (K_(w)) at 60^(@) C is 9.6xx10^(-14) M^(2) what is the [H_(3)O^(+)] of a neutral aqueous solutoin at 60^(@) C and an aqueous solution with a pH=7.0 at 60 ^(@) C are respectively?