The degree of dissociation of $0.1 \ M$ acid $HA$ is $5 \%$. The value of $K_c$ of $HA$ is

Calculate the value of the dissociation constant $(K_b)$ of a weak monoacidic base if it dissociates to $2 \%$ in a $0.1 \ M$ solution.

$A$ weak acid,$HA,$ has a $K_a$ of $1.00 \times 10^{-5}.$ If $0.100 \ mol$ of this acid is dissolved in one litre of water,the percentage of acid dissociated at equilibrium is closest to $...\%$

In its $0.2 \, M$ solution,an acid ionises to an extent of $60 \%$. Its hydrogen ion concentration is.....$M$

For a weak base $BOH$ at $25\,^oC$,the dissociation constant $K_b$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in its $0.01\,M$ aqueous solution will be:

The $pH$ of a $1.0 \ M$ monobasic acid $HX$ is $2$. The van't Hoff factor for the aqueous solution of the acid will be ........