The concentration of hydrogen ion $[H^{+}]$ in $0.01 \, M$ $HCl$ is

$pH$ of a $10 \ M$ solution of $HCl$ is

Assuming complete ionisation,the $pH$ of $0.1\,M\,HCl$ is $1$. The molarity of $H_2SO_4$ with the same $pH$ is (in $,M$)

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

$600 \, mL$ of $0.01 \, M \, HCl$ is mixed with $400 \, mL$ of $0.01 \, M \, H_2SO_4$. The $pH$ of the mixture is $....... \times 10^{-2}$. (Nearest integer) [Given $\log 2 = 0.30, \quad \log 3 = 0.48, \quad \log 5 = 0.69, \quad \log 7 = 0.84, \quad \log 11 = 1.04$]

$NaOH$ is a strong base. What will be the $pH$ of a $5.0 \times 10^{-2} \ M$ $NaOH$ solution? (Given: $\log \ 2 = 0.3$)