Question

The next 11 questions are related to the titration of 35.00 mL of a 0.0950 M acetic acid solution with 0.1000 M KOH. Assume that the temperature is 25 oC. What is the initial pH of the analyte solution? 2.89 (figured this one out) What volume of KOH is required to reach the equivalence point of the titration? 33.25 mL ( figured this one out) How many mmol of acetate are present at the equivalence point? Report the analytical amount, not the equilibrium amount of acetate at the equivalence point. The mmoles of acetate present at the equivalence point must be equal to the initial number of mmoles of acetic acid. What is the total volume of the solution at the equivalence point? 68.25 mL (I figured this one out) What is the analytical concentration of acetate ions at the equivalence point? What is the pOH at the equivalence point? What is the pH at the equivalence point? What volume of KOH has been added at the half-equivalence point? What is the pH at the half-equivalence point? What is the pH when 14.00 mL of the KOH solution have been added? What is the pH when 40.00 mL of the KOH solution have been added?