The $pH$ of $0.1 \ M$ acetic acid is $3$. The dissociation constant of the acid will be:

In aqueous solution,the ionization constants for carbonic acid are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. Select the correct statement for a saturated $0.034 \ M$ solution of carbonic acid.

$A$ monoprotic acid in a $0.1 \ M$ solution ionizes to $0.001 \%$. Its ionisation constant is

The ionization constant of benzoic acid is $6.5 \times 10^{-5}$ at $298 \ K$ temperature. Calculate $pH$ of its $0.15 \ M$ solution. (in $.5$)

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 $0.1 \ N$ solution of $CH_3COOH$ is $1.3\%$ ionized,what will be the $pH$ of the solution? (Given: $\log 1.3 = 0.11$)