$0.01 \, M$ acetic acid solution is $1 \%$ ionised,then $pH$ of this acetic acid solution is :

The $pH$ of a $0.1 \ M$ solution of acetic acid will be (degree of dissociation of acetic acid is $0.0132$).

The ionization constant of $HF$ is $3.2 \times 10^{-4}$. Calculate the degree of dissociation of $HF$ in its $0.02 \ M$ solution. Calculate the concentration of all species present ($H_{3}O^{+}$,$F^{-}$ and $HF$) in the solution and its $pH$.

At $25 \, ^\circ C$,the equilibrium constant for a base $BOH$ is $1.0 \times 10^{-12}$. What will be the concentration of hydroxide ions in a $0.01 \, M$ aqueous solution of the base?

At $298 \ K$ temperature,calculate the $pH$ of a $0.25 \ M$ solution of $(CH_3)_2NH$ given that its $K_b$ is $5.4 \times 10^{-4}$.

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: