For a weak acid,the incorrect statement is

The degree of dissociation of acetic acid $(0.1 \ mol \ L^{-1})$ in water ($K_a$ of acetic acid is $10^{-5}$) is

The dissociation constant of propionic acid is $1.32 \times 10^{-5}$. Calculate the degree of dissociation of the acid in a $0.05 \ M$ solution.

The ionization constant of $CH_3COOH$ is $1.7 \times 10^{-5}$. In a certain solution of acetic acid,the concentration of $H^+$ is $3.4 \times 10^{-4} \ M$. The concentration of the acetic acid solution is ............ .

$0.01 \ M \ HA_{(aq)}$ is $2\%$ ionized; $[OH^{-}]$ of solution is

At $27^{\circ} C$,the degree of dissociation of a weak acid $(HA)$ in its $0.5 \ M$ aqueous solution is $1 \%$. Its $K_{a}$ value is approximately: