The $pH$ of a $0.05 \,M$ solution of a strong dibasic acid $(H_2A)$ is:

Millimoles of calcium hydroxide required to produce $100 \ mL$ of the aqueous solution of $pH$ $12$ is $x \times 10^{-1}$. The value of $x$ is $..............$. (Nearest integer). Assume complete dissociation.

What will be the resultant $pH$ when $100 \ mL$ of an aqueous solution of $HCl$ $(pH = 2)$ is mixed with $200 \ mL$ of an aqueous solution of $NaOH$ $(pH = 12)$?

The $pH$ values of $(i) \ 0.1 \ M \ HCl_{(aq)}$,$(ii) \ 0.1 \ M \ KOH$,$(iii)$ tomato juice,and $(iv)$ pure water follow the order.

The $pH$ of millimolar $HCl$ is

Calculate $pH$ and $pOH$ of $0.03 \ M$ $NaOH$ solution.