An acid-base indicator which is a weak acid has a ${pK}_{in}$ value = 5.45. At what concentration ratio of sodium acetate to acetic acid would the indicator show a colour half-way between those of its acid and conjugate base forms?
[ ${pK}_{a}$ of acetic acid = 4. 75, log 2 = 0.3]

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3 : 1

6 : 1

5 : 1

4 : 1

answer is C.

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Detailed Solution

$\begin{array}{l} pH = p K_{I n} = 5.45 \\ 5.45 = 4.75 + \log \{\frac{[{AcO}^{-}]}{[AcOH]}\} \Rightarrow \frac{[{AcO}^{-}]}{[AcOH]} = \frac{5}{1} \end{array}$

Correct option is C.

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