Aqueous solution of $HCl$ has the $pH = 4$. Its molarity would be (in $, M$)

$NaOH_{(aq)}$,$HCl_{(aq)}$ and $NaCl_{(aq)}$ concentration of each is $10^{-3} \, M$. Their $pH$ will be respectively

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

If $0.4 \ g$ of $NaOH$ is present in $1 \ L$ of solution,then the $pH$ of the solution is .....

The $pH$ of $1 \ L$ of an aqueous solution of $HCl$ is $1$. How many liters of water must be added to make the $pH$ of this solution $2$ (in $L$)?

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)