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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
Options
(a) log [In⁻] / [HIn] = pKIn – pH
(b) log [HIn] / [In⁻] = pKIn – pH
(c) log [HIn] / [In⁻] = pH – pKIn
(d) log [In⁻] / [HIn] = pH – pKIn
Correct Answer:
log [In⁻] / [HIn] = pH – pKIn
Explanation:
No explanation available. Be the first to write the explanation for this question by commenting below.
Related Questions: - 8.2 L of an ideal gas weight 9.0 gm at 300 K and 1 atm pressure
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Topics: Equilibrium
(104)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- 8.2 L of an ideal gas weight 9.0 gm at 300 K and 1 atm pressure
- The correct order of ionization energy of C, N, O, F is
- Which of the following is not a cheracteristic of equilibrium
- Amino acids,Which build up proteins, have both the carboxylic and amino groups
- Glass is soluble in
Topics: Equilibrium (104)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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