The degree of dissociation of $0.1 \, M \, HCN$ solution is $0.01 \%$. Its ionisation constant would be

$A$ monoprotic acid in a $0.1 \ M$ solution ionizes to $0.001 \%$. Its ionisation constant is

Calculate $\alpha$ for $0.1 \ M$ acetic acid $(K_{a} = 1.0 \times 10^{-5})$.

The degree of ionization of a $0.1 \, M$ bromoacetic acid solution is $0.132$. Calculate the $pH$ of the solution and the $pK_{a}$ of bromoacetic acid.

$K_{a}$ for butyric acid $(C_{3}H_{7}COOH)$ is $2 \times 10^{-5}$. The $pH$ of $0.2 \ M$ solution of butyric acid is $........... \times 10^{-1}$. (Nearest integer) [Given $\log 2 = 0.30$]

What is the percent dissociation of acetic acid in its $0.01 \ M$ solution if the dissociation constant of the acid is $1.34 \times 10^{-6}$ (in $\%$)?