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The rapid change of pH near the stoichio...

The rapid change of `pH` near the stoichiometric point of an acid-base titration is the basic of indicator detection. `pH` of the solution is related to the ratio of the concentration of conjugate acid `(Hin)` and base `(In^(-))` forms of the indicator by the expression

A

`log.([In^(-)])/([In^(-)])= pK_(In) -pH`

B

`log.([HIn^(-)])/([In^(-)])= pK_(In) -pH`

C

`log.([HIn^(-)])/([In^(-)])= pH_(In) -pK_(In)`

D

`log.([In^(-)])/([ H In^(-)])= pH_(In) -pK_(In)`

Text Solution

Verified by Experts

The correct Answer is:
D
`pH = pK_(a)+log. (["Conjugate base"])/(["Acid"])`
`:. pH - pK_(In)=log. ([In^(-)])/([H In])`
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