question_answer

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 \[(I{{n}^{-}})\]forms of the indicator by the expression :-

A)  \[\log \,\frac{[HIn]}{[I{{n}^{-}}]}=p{{K}_{In}}+pH\]

B)  \[\log \,\frac{[HIn]}{[I{{n}^{-}}]}=pH-p{{K}_{In}}\]

C)  \[\log \,\frac{[I{{n}^{--}}]}{[HIn]}=pH-p{{K}_{In}}\]

D)  \[\log \,\frac{[I{{n}^{--}}]}{[HIn]}=p{{K}_{In}}-pH\]