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Henderson Hassleback Equation

The pK b of c...

Question

The $p K_{b}$ of cyanide ion is 4.7 The pH of a solution prepared by mixing 2.5 moles of KCN and 2.5 moles of HCN in water and making total volume upto 500 ml is :

9.3

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7.3

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10.3

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8.3

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Solution

The correct option is A 9.3
Above solution is an acidic buffer solution
Since, number of moles and volume is same; $[s a l t] = [A c i d]$
thereore, from Henderson equation $p H = p K_{a} + log \frac{[s a l t]}{[a c i d]} . . . . .1$
or $p H = p K_{a} from eq. 1$ $p K_{a} o f H C N = 14 - p K_{b}$
$p K_{a} o f H C N = 14 - 4.7 = 9.3$

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Henderson Hassleback Equation

Standard XII Chemistry

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The pKb of cyanide ion is 4.7 The pH of a solution prepared by mixing 2.5 moles of KCN and 2.5 moles of HCN in water and making total volume upto 500 ml is :

The correct option is A 9.3Above solution is an acidic buffer solution Since, number of moles and volume is same; [salt]=[Acid] thereore, from Henderson equation pH=pKa+log[salt][acid] .....1 or pH=pKa from eq. 1pKa of HCN=14−pKb pKa of HCN=14−4.7=9.3

The $p K_{b}$ of cyanide ion is 4.7 The pH of a solution prepared by mixing 2.5 moles of KCN and 2.5 moles of HCN in water and making total volume upto 500 ml is :