Use the Bronsted-Lowry definitions to identify the two conjugate acid-base pairs in the following acid-base reaction:
HCO3^- + S^2- <-> HS^- + CO3^2-
I got it.
HCO3^- is the base in the pair with CO3^2-.
S^2- is the acid in the pair with HS^-.
Would you believe you have it backwards.
The HCO3^- is the acid because it has the proton and can donate it; the CO3^-2 is the base of the pair. Same reasoning for HS^- for the acid and S^-2 as the base. The one that HAS the H is the acid and the one to which the H can go is the base.