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The $P^{H}$ of a buffer solution is 5. It consists of a weak acid HA and its conjugate base $A^{-}$ . $P^{K_{a}}$ of HA is 4.699. Which of the following is correct combination of solutions present in the buffer solution?

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200 ml of 0.1M HA and 100 ml of 0.2M $A^{-}$

200 ml of 0.1M HA and 100 ml of 0.1M $A^{-}$

100 ml of 0.1M HA and 200 ml of 0.2M $A^{-}$

100 ml of 0.1M HA and 200 ml of 0.1M $A^{-}$

answer is A.

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Detailed Solution

$P^{H} = P^{K_{a}} + \log \frac{[S]}{[A]}$

$5 = 4.699 + \log \frac{[S]}{[A]}$

$0.3010 = \log 2 = \log \frac{[S]}{[A]}$

$\Rightarrow [S] : [A] = 2 : 1$

$\Rightarrow a n s w e r 1 i s c o r r e c t$

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