$A$ centimolar solution of a weak acid is $1.3 \%$ dissociated at $298 \ K$. What is its dissociation constant?

$0.02 \, M$ monobasic acid dissociates $2 \%$,hence,$pH$ of the solution is

What is the $pH$ of a $2 \times 10^{-3} \ M$ solution of a monoacidic weak base if it ionizes to the extent of $5 \%$?

The $pK_a$ of a weak acid is $5.85$. The concentrations of the acid and its conjugate base are equal at a $pH$ of (in $.85$)

The dissociation constants of monobasic acids $A$,$B$,$C$ and $D$ are $6 \times 10^{-4}$,$5 \times 10^{-5}$,$3.6 \times 10^{-6}$ and $7 \times 10^{-10}$ respectively. The $pH$ values of their $0.1 \ M$ aqueous solutions are in the order

Ionisation constant of $CH_3COOH$ is $1.7 \times 10^{-5}$ and concentration of $H^{+}$ ions is $3.4 \times 10^{-4} \ M$. Find the initial concentration of $CH_3COOH$ molecules.