Question

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 ratio of the concentrations of the conjugate acid (HIn) and base (In⁻) forms of the indicator by the expression
(a) $\log\frac{[ln^-]}{[Hln]} = pK_{ln} - pH$
(b) $\log\frac{[Hln]}{[ln^-]} = pK_{ln} - pH$
(c) $\log\frac{[Hln]}{[ln^-]} = pH - pK_{ln}$
(d) $\log\frac{[ln^-]}{[Hln]} = pH - pK_{ln}$

Answer 1

$<b>$
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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 ratio of the concentrations of the conjugate acid (HIn) and base (In⁻) forms of the indicator by the expression
(a) $\log\frac{[ln^-]}{[Hln]} = pK_{ln} - pH$
(b) $\log\frac{[Hln]}{[ln^-]} = pK_{ln} - pH$
(c) $\log\frac{[Hln]}{[ln^-]} = pH - pK_{ln}$
(d) $\log\frac{[ln^-]}{[Hln]} = pH - pK_{ln}$

→ [B]


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Answer 2

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➡️Option -: B✔️✔️

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