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

Calculate the $pH$ of a $0.08 \ M$ solution of hypochlorous acid,$HOCl$. The ionization constant of the acid is $2.5 \times 10^{-5}$. Determine the percent dissociation of $HOCl$.

The $pH$ of a monoacidic weak base is $10.9$. Calculate the percent dissociation in a $0.02 \ M$ solution. (in $\%$)

Calculate the ionisation constant of $0.08 \ mol \ dm^{-3}$ of a monobasic acid having $pH = 2$.

$A$ weak base is $5 \%$ dissociated in its $0.01 \ M$ solution. Calculate the dissociation constant.

For a $0.1 \ M$ aqueous pyridine solution,if the pyridinium ion concentration is produced such that the degree of dissociation is $0.013 \%$,calculate the concentration of the pyridinium ion.