What is the $pH$ of acetic acid at equilibrium, given that acetic acid concentration is $0.1 \ M$ and it is $30 \%$ dissociated at equilibrium? $(\log 3=0.47)$

The dissociation constant of a weak acid $HA$ is $1.5 \times 10^{-5}$. Find the percent dissociation of a solution containing $0.2 \text{ moles}$ of $HA$ in $2 \text{ liters}$ of solution. (in $\%$)

For an aqueous solution of $H_2CO_3$,the ionization constants are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. Which statement is correct for a $0.034 \ M$ saturated solution of carbonic acid?

$A$ weak monoacidic base is $1.2 \%$ dissociated in its $0.2 \ M$ solution. What is the value of dissociation constant?

The hydrogen ion concentration in a weak acid of dissociation constant $K_a$ and concentration $c$ is nearly equal to:

$A$ weak acid is $0.1\%$ ionised in $0.1 \ M$ solution. Its $pH$ is