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                                            [CBSE PMT 2004]

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

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

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

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