What is the value of $pH$ of a $NaOH$ solution that dissociates $2 \%$ in its $0.01 \ M$ solution?

$A$ weak monobasic acid is $2 \%$ dissociated in its $0.1 \ M$ solution. What is 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 $pK_a(\text{acetic acid}) - pK_a(\text{formic acid})$?

$A$ $0.1 \ M$ solution of $HF$ is $1 \%$ ionized. What is the $K_a$?

The $pH$ of a monoacidic base is $10$. Calculate its percentage dissociation in $0.01 \ M$ solution at $298 \ K$. (in $\%$)

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