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.
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.
$c=0.1 \,M$
$pH =2.34$
$-\log \left[ H ^{+}\right]= pH$
$-\log \left[ H ^{+}\right]=2.34$
$\left[ H ^{+}\right]=4.5 \times 10^{-3}$
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
$K_{a}=c \alpha^{2}$
$=0.1 \times\left(45 \times 10^{-3}\right)^{2}$
$=202.5 \times 10^{-6}$
$=2.02 \times 10^{-4}$
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