Q

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

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

Views

We have,
Concentration of cyanic acid = 0.1 M
$p^H=-\log [H^+]$ $= 2.34$

Therefore, the concentration of $[H^+]$ = antilog (-2.34)
= $4.5 \times 10^{-3}$

It is known that,
$[H^+]$ $=C.\alpha$  = $4.5 \times 10^{-3}$
$\alpha = \frac{4.5\times 10^{-3}}{0.1} = 4.5\times 10^{-2}$

Then Ionization constant ($K_a$) $=C.\alpha^2$ =
$=(0.1)(4.5\times10^{-2})^2$
$=2.02\times 10^{-4}$

Exams
Articles
Questions