The ionic product of water with increase in temperature.

Calculate the $pOH$ of a solution at $25 \, ^\circ C$ that contains $1 \times 10^{-10} \, M$ of hydronium ions,i.e.,$H_3O^{+}$.

For the reaction $B^{-} + H_2O \rightleftharpoons HA + OH^{-}$,the value of the hydrolysis constant at equilibrium is equal to $K_a^{-1} = \dots \dots$

Number of hydrogen ions present in $10$ millionth part of $1.33 \ cm^{3}$ of pure water at $25^{\circ} C$ is

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 hydrogen ion concentration in a given solution is $6 \times 10^{-4} \ M$. Its $pH$ will be