The $pH$ of $0.1$ $M$ solution of cyanic acid $(HCNO)$ is $2.34$. Calculate the ionization constant of the acid and its degree of ionization in the solution.

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

$c=0.1 \,M$

$pH =2.34$

$-\log \left[ H ^{+}\right]= pH$

$-\log \left[ H ^{+}\right]=2.34$

$\left[ H ^{+}\right]=4.5 \times 10^{-3}$

Also.

$\left[ H ^{+}\right]=c \alpha$

$4.5 \times 10^{-3}=0.1 \times \alpha$

$\frac{4.5 \times 10^{-3}}{0.1}=\alpha$

$\alpha=45 \times 10^{-3}=.045$

Then

$K_{a}=c \alpha^{2}$

$=0.1 \times\left(45 \times 10^{-3}\right)^{2}$

$=202.5 \times 10^{-6}$

$=2.02 \times 10^{-4}$

Similar Questions

Which of the following base is weakest

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 $3.7\%$ dissociates. The value of dissociation constant, $K_a,$ for this acid will be

  • [NEET 2013]

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 ? .......$\%$

The hydrogen ion concentration of a $0.006\,M$ benzoic acid solution is $({K_a} = 6 \times {10^{ - 5}})$

The dissociation constant of an acid $HA$  is $1 \times {10^{ - 5}}$. The $pH$ of $0.1$ molar solution of the acid will be