The $pH$ of $10^{-7} \ N \ HCl$ is

Calculate the $pH$ of a mixture obtained by mixing equal volumes of $0.01 \ M \ HCl$ and $0.1 \ M \ NaOH$.

$50 \ mL$ of water is added to $50 \ mL$ of $0.01 \ M$ $Ba(OH)_2$ solution. Calculate the $pH$ of the resulting solution.

Assuming that $Ba(OH)_{2}$ is completely ionised in aqueous solution under the given conditions,the concentration of $H_{3}O^{+}$ ions in $0.005 \, M$ aqueous solution of $Ba(OH)_{2}$ at $298 \, K$ is $..... \times 10^{-12} \, mol \, L^{-1}$. (Nearest integer)

Calculate the volume of $0.1 \ M \ NaOH$ required to complete the neutralization of $300 \ mL$ of $HCl$ solution having $pH = 2.25$. (in $mL$)

The concentration of $NaOH$ solution is $10^{-8} \ M$. Find out the $[OH^{-}]$ concentration.