QuestionIonic equilibrium / indicators
In acid base titration the color change of an indicator is expressed by:
\(pH = pK'_{In} + \log\frac{[In_B]}{[In_A]}\)
(Where \(In_B\) = Indicator in the basic form, \(In_A\) = indicator in acid form)
The basic color of the indicator would be visible when:
- (a) \([In_B]/[In_A] > 10\)
- (b) \([In_B]/[In_A] < 10\)
- (c) \([In_A]/[In_B] > 10\)
- (d) \([In_B] = [In_A]\)
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