When $NaCl$ is dissolved in water,the sodium ion becomes

Given that $K_w$ for water is $10^{-13} \ M^2$ at $62 \ ^\circ C$,compute the sum of $pOH$ and $pH$ for a neutral aqueous solution at $62 \ ^\circ C$.

What is the $pH$ of the solution containing $1.342 \times 10^{-3} \ M \ H^{+}$ ions?
$(\log 1.342 = 0.1277)$

The $pH$ of a solution is $5.0$. To this solution,sufficient acid is added to decrease the $pH$ to $2.0$. The increase in hydrogen ion concentration is $...$ times.

Calculate the $[H_3O^+]$ concentration if the $pH$ of the solution is $4.25$.

The $pH$ of a solution in which the $[H^{+}] = 0.01 \, M$ is