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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.
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Topics: Equilibrium
(104)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- Reaction of solid KMnO₄ ith conc.H₂SO₄ produces manganese heptoxide (Mn₂O₇) in
- A corked flask containing boiling water and its vapour is allowed
- Which of the following reaction(s) can be used for the preparation of alkyl halides?
- Oxidation number of iodine in IO₃⁻, IO₄⁻, KI and I₂ respectively are
- Which of the following is not a cheracteristic of equilibrium
Topics: Equilibrium (104)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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