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 concentration of the conjugate acid (Hin) and base `[H^(+)] = 10^(-7) + 10^(-8) = 10^(-7)[1+0.1]` forms of the indicator by the expression
A. `log.([HIn])/([In^(-)]) = pH - pK_(In)`
B. `log.([In^(-)])/([HIn]) = pH - pK_(In)`
C. `log.([In^(-)])/([HIn]) = pK_(In) - pH`
D. `log.([HIn])/([In^(-)]) = pK_(In) - pH`
