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The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to the ratio of the concentrations of the conjugate acid ($HIn$) and base ($In^–$) forms of the indicator, as per the expression:

1.	$\log \frac{[HIn]}{[{In}^{-}]} = {pK}_{In} - pH$	2.	$\log \frac{[HIn]}{[{In}^{-}]} = pH - {pK}_{In}$
3.	$\log \frac{[{In}^{-}]}{[HIn]} = pH + {pK}_{In}$	4.	None of the above

Subtopic: Buffer |

Level 3: 35%-60%

AIPMT - 2004

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