The ionic product of water $(K_w)$ increases if:

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

Statement-$I$ :- $pH$ of pure water increases with increase in temperature.
Statement-$II$ :- Degree of ionisation increases with increase in temperature.

Find the concentration of hydrogen ions in a solution with $pH = 5.4$ in $mol/L$.

The value of the ion product constant for water,$(K_w)$ at $60\,^{\circ}C$ is $9.6 \times 10^{-14} \,M^2$. What are the $[H_3O^{+}]$ of a neutral aqueous solution at $60\,^{\circ}C$ and the nature of an aqueous solution with a $pH = 7.0$ at $60\,^{\circ}C$,respectively?

What is the dissociation constant of water at $25^{\circ}C$?