Calculate the $pH$ of $0.0035 \ M \ Ba(OH)_2$ solution.

What is the $pH$ of $10^{-9} \ M$ aqueous $HCl$ solution?

$10^{-6} \ M \ NaOH$ is diluted $100$ times. The $pH$ of the diluted base is

The ratio of $pH$ of $0.1 \, M \, H_2SO_4$ and that of $0.1 \, N \, H_2SO_4$ is

$pH$ of $10^{-8} \ M$ $Ba(OH)_2$ solution will be

Given below are two statements:
Statement-$I$: $pH$ of a $1.0 \times 10^{-8} \ M$ solution of $HCl$ is $8$ at $25^{\circ} C$.
Statement-$II$: $HCl$ is a strong acid and negative log of $H^{+}$ concentration is called $pH$.
In the light of the above statements,choose the most appropriate answer from the options given below: