The $K_a$ of propanoic acid is $1.4 \times 10^{-5}$. Calculate the $pH$ of a $0.1 \ M$ solution.

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

For a $10 \ M \ CH_3COOH$ solution,if $K_a = 10^{-5}$,what will be the values of $[H^{+}]$ and $pH$ respectively?

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?

Degree of dissociation is $10\%$ for $10^{-3} \ M$ solution of $H_2CO_3$. Then,the $pH$ of the solution is:

The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$,is (in $M$)