Degree of dissociation is $10\%$ for $10^{-3} \ M$ solution of $H_2CO_3$. Then,the $pH$ of the solution is:

$A$ monobasic acid is $5 \%$ dissociated in its $0.02 \ M$ solution. Calculate the dissociation constant of the acid.

Which of the following compounds has the maximum $K_{a}$ value?

What is the molar concentration of a weak monobasic acid if its dissociation constant is $5 \times 10^{-8}$ and it undergoes $0.5 \%$ dissociation (in $M$)?

Consider the dissociation equilibrium of the following weak acid $HA \rightleftharpoons H^{+}_{(aq)} + A^{-}_{(aq)}$. If the $pK_{a}$ of the acid is $4$, then the $pH$ of $10 \ mM$ $HA$ solution is . . . . . . . (Nearest integer)
[Given : The degree of dissociation can be neglected with respect to unity]

At $25 \, ^\circ C$,the dissociation constant of a base $BOH$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in $0.01 \, M$ aqueous solution of the base would be: