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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
- How many coulombs of electricity are required for the reduction of 1 mol
- CH₃CH₂OH converts into CH₃CHO in the presence of
- Concentrated sulphuric acid is always dilute by adding
- Which of the following will be most stable diazonium salt RN₂⁺ X⁻
- Which of the following pairs of substance on reaction will not evolve H₂ gas
Topics: Equilibrium (104)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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