Weak acid $HX$ has dissociation constant $1 \times 10^{-5}$. Calculate the percent dissociation in its $0.1 \ M$ solution. (in $\%$)

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.

When a $1$ deci-normal solution of acetic acid is $1.3\%$ ionized,what is the value of the ionization constant $(K_a)$?

$A$ solution of weak acid $HA$ containing $0.01 \ mol/L$ of acid has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.

The $pH$ of a $0.1 \ M$ solution of $NH_{4}OH$ (having $K_{b} = 1.0 \times 10^{-5}$) is equal to

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