Calculate the pH of a centimolar solution of a monoacidic weak base which is $10 \%$ dissociated in its aqueous solution.

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.

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 $HOCl$.

In aqueous solution,the ionization constants for carbonic acid are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. Select the correct statement for a saturated $0.034 \ M$ solution of carbonic acid.

The dissociation constant of a weak monobasic acid is $3.2 \times 10^{-4}$. Calculate the degree of dissociation in its $0.04 \ M$ solution.

The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.