The $pH$ of neutral water at room temperature is nearly:

Calculate $[OH^{-}]$ and $pH$ of a solution containing $[H^{+}] = 0.001 \ M$.

At $25 \, ^\circ C$,the $pH$ value of a solution is $6$. The solution is:

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?

When $NaCl$ is dissolved in water,the sodium ion undergoes ......... .

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