The pH of a solution with concentration 10-3 M of an indicator with Kb = 1.0 x 10-10 will change colour at

The pH of a solution with concentration 10^-3 M of an indicator with K_b = 1.0 x 10^-10 will change colour at

For weak base indicator, at equivalence point

$[In OH] = [{In}^{+}] InOH ⇌ {In}^{+} + {OH}^{-} ∴ pOH = {pK}_{b} + \log \frac{[{In}^{+}]}{[InOH]} = {pK}_{b} = 10 ∴ pH = 14 - 10 = 4$

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