The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows:
HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l)
Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH.
A. What is the pH at the beginning of the titration, Vbase = 0.00 mL?
B. What is the pH at the equivalence point?
C. What is the pH of the titration when 5.00 mL of base have been added?
D. What is the pH when the volume of base added equals half the volume of the equivalence point?
E. What is the pH of the titration when 20.00 mL of base have been added?
F. What is the pH of the titration when 30.00 mL of base have been added?
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