$A$ is an aqueous acid; $B$ is an aqueous base. They are diluted separately,then:

The $H^{+}$ ion concentration is $1.0 \times 10^{-6} \ mol/L$ in a solution. Its $pH$ value will be

At a certain temperature $T$,if the conductivity of pure water is $5.5 \times 10^{-7} \ S \ cm^{-1}$,calculate the $pH$ of water at the given temperature. Given: $\lambda_{H^{+}}^\infty = 350 \ S \ cm^2 \ eq^{-1}$ and $\lambda_{OH^{-}}^\infty = 200 \ S \ cm^2 \ eq^{-1}$.

The standard Gibbs energy change in the reaction $H_2O \rightleftharpoons H^{+} + OH^{-}$ at $25\ ^oC$ is.....$kJ/mol$.

The $pH$ of pure water or neutral solution at $50\,^{\circ}C$ is .... ($pK_w = 13.26$ at $50\,^{\circ}C$)

$pH$ of a solution is $5$. Its hydroxyl ion concentration is