$NaOH$ is a strong base. What will be the $pH$ of a $5.0 \times 10^{-2} \ M$ $NaOH$ solution? (Given: $\log \ 2 = 0.3$)

What is the pH of $10^{-8} \ M \ HCl$ solution?

$0.837 \ g$ of $Ba(OH)_2$ is dissolved in $100 \ mL$ of solution. Calculate the $pH$ of the solution. (Atomic masses: $Ba = 137, O = 16, H = 1$)

The $pH$ of $0.01 \ M \ NaOH_{(aq)}$ solution will be

What will be the $pH$ of a $10^{-8} \ M \ HCl$ 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)