$1 \ L$ of $0.02 \ M$ aqueous $HCl$ is mixed with $1 \ L$ of $0.01 \ M$ aqueous $H_2SO_4$ solution. Assuming complete dissociation and no change in the volume upon mixing,the $pH$ of the resultant solution is $(\log_{10} 2 = 0.3)$.

The number of moles of $Ca(OH)_2$ required to prepare $250 \ mL$ of solution with $pH$ $14$ (assuming complete ionization) is :-

Given a $0.1 \ M$ solution of each of the following. Which solution has the lowest $pH$?

$pH$ values of $HCl$ and $NaOH$ solutions each of strength $\frac{N}{100}$ will be respectively:

The $pH$ value of which one of the following is not equal to $1$?

Calculate the $pH$ of the following solutions:
$(a)$ $2 \,g$ of $TlOH$ dissolved in water to give $2 \,L$ of solution.
$(b)$ $0.3 \,g$ of $Ca(OH)_2$ dissolved in water to give $500 \,mL$ of solution.
$(c)$ $0.3 \,g$ of $NaOH$ dissolved in water to give $200 \,mL$ of solution.
$(d)$ $1 \,mL$ of $13.6 \,M \,HCl$ is diluted with water to give $1 \,L$ of solution.