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

Vedclass pdf generator app on play store
Vedclass iOS app on app store

$\left[\mathrm{H}^{+}\right]=3.12 \times 10^{-3} \mathrm{M}, \mathrm{pH}=2.5$

Similar Questions

A solution of weak acid $HA$ containing $0.01$ moles of acid per litre of solutions has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.

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

$pH$ of $0.1\,\, M$ $N{H_3}$ aqueous solution is $({K_b} = 1.8 \times {10^{ - 5}})$

A weak acid is $ 0.1\% $ ionised in $0.1\, M $ solution. Its $pH$  is

Ionisation constant of $CH_3COOH$ is $1.7 \times 10^{-5}$ and concentration of $H^+$ ions is $3.4 \times 10^{-4}$. Then find out initial concentration of $CH_3COOH$ Molecules