If the degree of ionisation is $0.01$ for a decimolar solution of a weak acid $HA$,then the $pKa$ of the acid is:

The first and second ionization constants of $H_2X$ are $2.5 \times 10^{-8}$ and $1.0 \times 10^{-13}$ respectively. The concentration of $X^{2-}$ in $0.1 \ M$ $H_2X$ solution is . . . . . . $\times 10^{-15} \ M$. The value of $Y$ is:

$A$ monobasic weak acid dissociates $2 \%$ in its $0.002 \ M$ solution. Calculate the dissociation constant of the weak acid.

Determine the degree of ionization and $pH$ of a $0.05 \, M$ ammonia solution. The ionization constant of ammonia $(K_{b})$ is $1.77 \times 10^{-5}$. Also,calculate the ionization constant of the conjugate acid of ammonia.

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

The $pH$ of a $0.1 \ M$ solution of acetic acid will be (degree of dissociation of acetic acid is $0.0132$).