1. The problem statement, all variables and given/known data Consider a titration in which 50.00 mL of .450 M benzoic acid, C6H5COOH, is reacted with 0.2000 M Ca(OH)2. What will the pH be when 60.00 mL of Ca(OH)2 has been added? 2. Relevant equations 2C6H5COOH + Ca(OH)2 -> 2 H2O + Ca(C6H5COO)2 3. The attempt at a solution I have determined that the equivalence point is at 56.25 mL, so this is past that. The thing that is throwing me off is the mol ratio of acid:base. I try doing an ICF chart and keep getting that there is still acid left and no base. I thought that after the equiv. point, there is no acid left and you determine the pH based on the remaining base. Can anyone help me fill in the ICF chart so that I can find the pH? I need moles of acid and base to do this.