Question

Hey everyone!
I am solving some organic chemistry excercises. They are about acid-base equilibrium and Keq calculating.
The first thing I'd like to know is how acetic acid in this reaction acts as a Bronsted acid (electron donor):
CH3CO2H + CO3- --> CH3CO2- + HCO3-
I know the equilibrium goes right, because acetic acid donates a proton to CO3-, so it becomes carbonic acid. But, what's the mechanism?
Thank you!

Answer 1

\[\color{green}{CH_3COOH \rightarrow CH_3COO^- + H^+}\]
Then,\[\color{green}{H^+ + CO_3^{2-} \rightarrow HCO_3{^-}}\]
Bronsted-Lowry acids are proton donors. You are confusing this with Lewis acids.

Answer 2

That's right! thank you :D