Calculate the $pH$ of $1.36 \times 10^{-2} \ M$ solution of perchloric acid.

Assuming complete dissociation,calculate the $pH$ of the following solutions:
$(i) \ 0.003 \ M \ HCl$
$(ii) \ 0.005 \ M \ NaOH$
$(iii) \ 0.002 \ M \ HBr$
$(iv) \ 0.002 \ M \ KOH$

Given $pH$ of a solution $A$ is $3$ and it is mixed with another solution $B$ having $pH$ $2$. If both are mixed in equal volumes,then the resultant $pH$ of the solution will be

Calculate the $pH$ of a $1.0 \times 10^{-8} \ M$ solution of $HCl$.

$1.825 \ g$ of $HCl$ is dissolved in $5 \ L$ of water. What are the concentrations of $H^+$ and $OH^-$ ions?

If $pH$ of $A$,$B$,$C$ and $D$ are $9.5$,$2.5$,$3.5$ and $5.5$ respectively,then the strongest acid is