The $pH$ of a $0.1 \ M$ solution of the acid $HA$ is $3$. The value of the ionization constant,$K_a$ of this acid is

At $T$ $(K)$,if the ionisation constant of ammonia in solution is $2.5 \times 10^{-5}$,the $pH$ of $0.01 \ M$ ammonia solution and the ionisation constant of its conjugate acid respectively at that temperature are $(\log 2 = 0.30)$

The degree of dissociation of $0.1 \, N \, CH_3COOH$ is (Dissociation constant $K_a = 1 \times 10^{-5}$)

The $pH$ of $0.1 \, M$ acetic acid solution is closest to $.....$ [Dissociation constant of the acid,$K_{a} = 1.8 \times 10^{-5}$]

The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.

Derive the equation for the ionization constant $K_a$ of a weak acid $HX$.