The indicator constant of an indicator is 10−4. If pH of solution in which this indicator is present is 3.5, which of the following facts will be correct?

A
Ionized indicator is present in the larger amount
B
Unionized indicator is present in the larger amount
C
Both ionized and unionized indicator are present in equal amounts
D
Percentage of indicator present in ionized form cannot be predicted

Solution:

$HIn ⇌ H^{+} +$ + In; Since $pH < p K_{Hin}^{\circ},$ the solution contains larger $H^{+}$ than that obtained from ionization of $HIn$ alone. Hence, the above equilibrium is shift to left, thus more of unionized indicator is present.

The indicator constant of an indicator is $10^{- 4}$ . If pH of solution in which this indicator is present is 3.5, which of the following facts will be correct?

Solution:

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