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 degree of dissociation of $0.1 \ M$ acid $HA$ is $5 \%$. The value of $K_c$ of $HA$ is

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?

Accumulation of lactic acid $(HC_3H_5O_3),$ a monobasic acid in tissues,leads to pain and a feeling of fatigue. In a $0.10 \ M$ aqueous solution,lactic acid is $3.7 \%$ dissociated. The value of the dissociation constant,$K_a,$ for this acid will be:

Dimethyl amine $(CH_3)_2NH$ is a weak base and its ionization constant is $5.4 \times 10^{-5}$. Calculate $[OH^{-}]$,$[H_3O^{+}]$,$pOH$ and $pH$ of its $0.2 \ M$ solution at equilibrium.

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