$A$ weak base is $5 \%$ dissociated in its $0.01 \ M$ solution. Calculate the dissociation constant.

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:

At $25 \, ^\circ C$,the dissociation constant of a base $BOH$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in $0.01 \, M$ aqueous solution of the base would be:

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

$A$ weak base $MOH$ of $0.1 \ N$ concentration shows a $pH$ value of $9$. What is the percentage degree of ionization of the base ? $.......\%$

$A$ 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 $...\%$