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Standard XII

Chemistry

Basic Buffer Action

The concentra...

Question

The concentration of $H C N$ and $N a C N$ in a solution is $0.01 M$ each. Calculate the concentrations of hydrogen and hydroxyl ions if the dissociation constant of $H C N$ is $7.2 \times 10^{- 10}$ .

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Solution

$p H = l o g \frac{[S a l t]}{[A c i d]} - log K_{a} = - l o g (7.2 \times 10^{- 10}) = - log [H^{+}]$
$[H^{+}] = 7.2 \times 10^{- 10} M$
$[H^{+}] [O H^{-}] = 10^{- 14}$
So, $[{O H}^{-}] = 1.4 \times 10^{- 7} M$

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Q. The concentration of

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0.01 M

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7.2 \times 10^{- 10}

The concentration of $H C N$ and $N a C N$ in a solution is $0.01 M$ each. Calculate the concentration of hydroxyl ions if the dissociation constant of $H C N$ is $7.2 \times 10^{- 10}$ .

Q. Determine the hydrogen ion concentration in

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aqueous solution of the base would be:

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The concentration of HCN and NaCN in a solution is 0.01M each. Calculate the concentrations of hydrogen and hydroxyl ions if the dissociation constant of HCN is 7.2×10−10.

pH=log[Salt][Acid]−logKa=−log(7.2×10−10)=−log[H+][H+]=7.2×10−10M[H+][OH−]=10−14So,[OH−]=1.4×10−7M

The concentration of $H C N$ and $N a C N$ in a solution is $0.01 M$ each. Calculate the concentrations of hydrogen and hydroxyl ions if the dissociation constant of $H C N$ is $7.2 \times 10^{- 10}$ .

$p H = l o g \frac{[S a l t]}{[A c i d]} - log K_{a} = - l o g (7.2 \times 10^{- 10}) = - log [H^{+}]$
$[H^{+}] = 7.2 \times 10^{- 10} M$
$[H^{+}] [O H^{-}] = 10^{- 14}$
So, $[{O H}^{-}] = 1.4 \times 10^{- 7} M$