What is the $pH$ of a solution having $H^{+}$ ion concentration $3.981 \times 10^{-7} \ M$? $(\log 3.981 = 0.6000)$

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 concentration of $H_3O^{+}$ ions in a solution having $pOH$ value $9$?

Hydrogen ion concentration in $mol/L$ in a solution of $pH = 5.4$ will be

Which of the following does not make any change in $pH$ when added to $10 \ mL$ of dilute $HCl$?

Pure water does not conduct electricity because ....