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

Derive the expression for the ionization constant $(K_b)$ of a weak base.

Calculate the concentration of a weak monobasic acid if its degree of dissociation and dissociation constant are $5.0 \times 10^{-4}$ and $5.0 \times 10^{-9}$ respectively (in $M$)?

For the ionization of a weak acid $HA$ as $HA \rightleftharpoons H^{+} + A^{-}$,the $pH$ of a $1.0 \ M$ solution is $5$. The dissociation constant $K_a$ is:

If the degree of ionisation is $0.01$ for a decimolar solution of a weak acid $HA$,then the $pKa$ of the acid is:

The ionization constant of benzoic acid is $6.5 \times 10^{-5}$ at $298 \ K$ temperature. Calculate $pH$ of its $0.15 \ M$ solution. (in $.5$)