The degree of dissociation of acetic acid $(0.1 \ mol \ L^{-1})$ in water ($K_a$ of acetic acid is $10^{-5}$) is

$A$ weak base is $1.42 \%$ dissociated in its $0.05 \ M$ solution. Calculate its dissociation constant.

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:

The $pH$ of a $0.1 \ M$ solution of $NH_{4}OH$ (having $K_{b} = 1.0 \times 10^{-5}$) is equal to

Weak acid $HX$ has dissociation constant $1 \times 10^{-5}$. Calculate the percent dissociation in its $0.1 \ M$ solution. (in $\%$)

What will be the hydrogen ion concentration of $0.006 \ M$ benzoic acid? $(K_a = 6 \times 10^{-5})$