What is the $pH$ of a $2 \times 10^{-3} \ M$ solution of a monoacidic weak base if it ionizes to the extent of $5 \%$?

$A$ weak monobasic acid is $0.04 \%$ dissociated in $0.25 \text{ M}$ solution. What is the $pH$ of the solution?

Sulphurous acid $(H_{2}SO_{3})$ has $Ka_{1} = 1.7 \times 10^{-2}$ and $Ka_{2} = 6.4 \times 10^{-8}$. The $pH$ of $0.588 \ M \ H_{2}SO_{3}$ is ..... . (Round off to the Nearest Integer)

If the dissociation constant of an acid $HA$ is $1 \times 10^{-5}$,the $pH$ of a $0.1 \ M$ solution of the acid will be approximately

The percent dissociation of a weak monobasic acid is $3 \%$ in its $0.02 \ M$ solution. What is the dissociation constant of the acid?

The $pH$ of a $1.0 \ M$ monobasic acid $HX$ is $2$. The van't Hoff factor for the aqueous solution of the acid will be ........