$A$ base dissolved in water yields a solution with a hydroxyl ion concentration of $0.05 \ mol \ L^{-1}$. The solution is

The $pH$ of $10^{-8} \ M$ aqueous solution of $HCl$ is

Equal volumes of two solutions $A$ and $B$ of a strong acid having $pH=6.0$ and $pH=4.0$ respectively are mixed together to form a new solution. The $pH$ of the new solution will be in the range

Calculate the $pH$ of a $4 \times 10^{-3} \ M \ Y(OH)_2$ solution. Assume $100\%$ dissociation for the first step and $50\%$ dissociation for the second step.

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

What is the $pH$ of $0.005 \ M \ NaOH$ solution?