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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.

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

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manish

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