For a $10^{-3} \ M \ HCN$ solution,if the degree of dissociation $\alpha = 10\%$,find the $K_a$ and $pH$ of the solution.

Calculate the $pH$ of a $0.02 \ M$ ammonia solution that is $5\%$ ionized.

$HClO$ is a weak acid. The concentration of ${H^+}$ ions in $0.1 \ M$ solution of $HClO$ $(K_a = 5 \times 10^{-8})$ will be equal to:

The $pH$ of two equimolar weak acids are $3.0$ and $5.0$ respectively. Their relative strength is

For a diprotic organic acid in aqueous solution,the ionization constants are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. For a $0.034 \ M$ solution of this acid,select the correct statement.

$A$ weak monobasic acid is $20 \%$ dissociated in its $0.01 \ M$ solution. What is the dissociation constant of the weak acid?