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

If two acids of equimolar concentration are taken,then which option is correct?

At what concentration of $0.2 \ M$ $CH_3COOH$ will its degree of dissociation become double (in $M$)? (Given: $K_a = 1.8 \times 10^{-5}$ for $CH_3COOH$)

For a $0.1 \ M$ aqueous pyridine solution,if the pyridinium ion concentration is produced such that the degree of dissociation is $0.013 \%$,calculate the concentration of the pyridinium ion.

The percent dissociation of a weak monobasic acid is $3 \%$ in its $0.02 \ M$ solution. What is the dissociation constant of the acid?

$A$ weak acid,$HA,$ has a $K_a$ of $1.00 \times 10^{-5}.$ If $0.100 \ mol$ of this acid is dissolved in one litre of water,the percentage of acid dissociated at equilibrium is closest to $...\%$