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Factors Affecting Alpha

A buffer solu...

Question

A buffer solution that has a pH of $4.72$ is prepared by mixing of $1 M NaOH$ and $1 M HCN$ . What is the ratio of volumes of the acid to the base? $(p K_{b} {of CN}^{-} = 9.28)$

1 : 1

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1 : 2

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2 : 1

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3 : 1

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Solution

The correct option is C 2 : 1
Let the volume of NaOH be $V_{1}$ and volume of $H C N$ be $V_{2}$
M eq of $H C N = V_{2} - V_{1}$
M eq of $N a C N = V_{1}$ Now this will form acidic buffer whose pH is given by
$p H = p K_{a} + l o g \frac{[N a C N]}{[H C N]}$ Now given
$p K_{b} {of CN}^{-} = 9.28$
$∴ p K_{a} o f H C N = 4.72$ , putting these values in above equation
$4.72 = 4.72 + l o g \frac{V_{1}}{V_{2} - V_{1}}$
so $\frac{V_{1}}{V_{2} - V_{1}} = 1$
Hence $V_{2} = 2 V_{1}$

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A buffer solution that has a pH of 4.72 is prepared by mixing of 1 M NaOH and 1M HCN. What is the ratio of volumes of the acid to the base? (pKb of CN−=9.28)

A buffer solution that has a pH of $4.72$ is prepared by mixing of $1 M NaOH$ and $1 M HCN$ . What is the ratio of volumes of the acid to the base? $(p K_{b} {of CN}^{-} = 9.28)$