The number of $H^{+}$ ions present in $10 \ mL$ of a solution with $pH = 12$ is ........

The $pH$ of human blood is $7.4$. The $[H^{+}]$ concentration will be:

$pH + pOH$ is equal to

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?

Ionic product of water at $310 \, K$ is $2.7 \times 10^{-14}$. What is the $pH$ of neutral water at this temperature?

Find the concentration of $(OH^-)$ in a solution with $pH = 3.3$.