In an acid-base titration,the rapid change in | vedclass

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(D) The dissociation of an acid-base indicator $(HIn)$ can be represented as: $HIn \rightleftharpoons H^+ + In^-$. Applying the law of mass action,the

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$\log \frac{[In^-]}{[HIn]} = pH - pK_{In}$

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(D) The dissociation of an acid-base indicator $(HIn)$ can be represented as: $HIn \rightleftharpoons H^+ + In^-$. Applying the law of mass action,the dissociation constant $K_{In}$ is given by: $K_{In} = \frac{[H^+][In^-]}{[HIn]}$. Taking the negative logarithm on both sides: $-\log K_{In} = -\log [H^+] - \log \frac{[In^-]}{[HIn]}$. This simplifies to: $pK_{In} = pH - \log \frac{[In^-]}{[HIn]}$. Rearranging the terms gives: $\log \frac{[In^-]}{[HIn]} = pH - pK_{In}$.

In an acid-base titration,the rapid change in $pH$ near the equivalence point depends on the indicator used. The $pH$ of the solution is related to the ratio of the concentrations of the conjugate acid $(HIn)$ and base $(In^-)$ forms of the indicator by which equation?

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