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

If the $pH$ of $0.10 \ M$ monoacidic base at $298 \ K$ is $9.0$,the value of $K_{b}$ and $pK_{b}$ at the same temperature are respectively:

Nicotinic acid $(K_a = 10^{-5})$ is represented by the formula $HNiC$. Calculate the percentage of dissociation in a solution containing $0.1 \ mol$ of nicotinic acid in $2 \ L$ of solution.

The $K_a$ of a weak acid $HA$ is $1.00 \times 10^{-5}$. If $0.100 \ mol$ of this acid is dissolved in $1 \ L$ of water,what is the percentage dissociation of the acid at equilibrium?

If a metal hydroxide with the molecular formula $M(OH)_4$ is $50\%$ ionized,then the $pH$ of its $0.0025 \ M$ solution will be:

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