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Standard XII

Chemistry

Liquids in Liquids

The ionisatio...

Question

The ionisation constant of $H C N$ is $4 \times 10^{- 10}$ . Calculate the concentration of hydrogen ions in $0.2 M$ solution if $H C N$ containing $1 m o l L^{- 1}$ of $K C N$ .

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Solution

$H C N ⇌ H^{+} {+ C N}^{-}$
It is given that $K_{a} = 4 \times 10^{- 10}$ , $[H C N] = 0.2 M$ and $[{C N}^{-}] = 1 M$
According to law of mass action,
$K_{a} = \frac{[H^{+}] [{C N}^{-}]}{[H C N]}$
From above equation we get $[H^{+}] = 8 \times 10^{- 11} M$

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The ionisation constant of HCN is 4×10−10. Calculate the concentration of hydrogen ions in 0.2M solution if HCN containing 1mol L−1 of KCN.

HCN⇌H++CN−It is given that Ka=4×10−10, [HCN]=0.2M and [CN−]=1MAccording to law of mass action,Ka=[H+][CN−][HCN]From above equation we get [H+]=8×10−11M

The ionisation constant of $H C N$ is $4 \times 10^{- 10}$ . Calculate the concentration of hydrogen ions in $0.2 M$ solution if $H C N$ containing $1 m o l L^{- 1}$ of $K C N$ .

$H C N ⇌ H^{+} {+ C N}^{-}$
It is given that $K_{a} = 4 \times 10^{- 10}$ , $[H C N] = 0.2 M$ and $[{C N}^{-}] = 1 M$
According to law of mass action,
$K_{a} = \frac{[H^{+}] [{C N}^{-}]}{[H C N]}$
From above equation we get $[H^{+}] = 8 \times 10^{- 11} M$