The $pH$ of an acidic solution is $4.70$. Calculate the concentration of $OH^-$ ions. $(pK_w = 14)$

At $25^{\circ} C$,the ${H_3}{O^+}$ concentration of a solution is $1.0 \times 10^{-10} \ M$. What is the $pOH$ value of the solution (in $.0$)?

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?

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

On adding which of the following,the $pH$ of $20 \ mL$ of $0.1 \ N \ HCl$ will not alter?

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