Consider the reaction of acetic acid in water CH3CO2H(aq) + H2O(l) CH3CO2-(aq) + H3O+(aq) where Ka

Question:

Consider the reaction of acetic acid in water
CH3CO2H(aq) + H2O(l) ⇌ CH3CO2-(aq) + H3O+(aq) where Ka = 1.8 × 10-5.
a. Which two bases are competing for the proton?
b. Which is the stronger base?
c. In light of your answer to part b, why do we classify the acetate ion (CH3CO2-) as a weak base? Use an appropriate reaction to justify your answer.