Calculate the $pH$ of $1.36 \times 10^{-2} \ M$ solution of perchloric acid.

The concentration of $H^{+}$ ions in $0.1 \, M \, NaOH$ is .......

$75 \ mL$ of $0.2 \ M \ HCl$ is mixed with $25 \ mL$ of $1 \ M \ HCl$. To this solution, $300 \ mL$ of distilled water is added. What is the $pH$ of the resultant solution?

The $pH$ of an aqueous solution containing $[H^{+}] = 3 \times 10^{-3} \ M$ is

Equal volumes of three acid solutions of $pH$ $3$,$4$ and $5$ are mixed in a vessel. What will be the $H^{+}$ ion concentration in the mixture in terms of $\times 10^{-4} \ M$?

$L$ litres of water must be added to $1 \, L$ of an aqueous solution of $HCl$ with a $pH$ of $1$ to create an aqueous solution with $pH$ of $2$?