$A$ monobasic weak acid dissociates $2 \%$ in its $0.002 \ M$ solution. Calculate the dissociation constant of the weak acid.

$A$ weak monobasic acid is $3.0 \%$ dissociated in its $0.04 \ M$ solution. What is the dissociation constant of the acid?

$A$ weak base is $1.42 \%$ dissociated in its $0.05 \ M$ solution. Calculate its dissociation constant.

The dissociation constant of acetic acid is $10^{-6}$ and the dissociation constant of formic acid is $10^{-5}$. What is the value of $pK_a(\text{acetic acid}) - pK_a(\text{formic acid})$?

The first and second ionization constants of $H_2X$ are $2.5 \times 10^{-8}$ and $1.0 \times 10^{-13}$ respectively. The concentration of $X^{2-}$ in $0.1 \ M$ $H_2X$ solution is . . . . . . $\times 10^{-15} \ M$. The value of $Y$ is:

$A$ weak monoprotic acid of $0.1 \ M$ ionizes to $1\%$ in solution. What will be the $pH$ of the solution?