Consider the following equilibrium: HC2O4- + HSO4- <—> H2C2O4 + SO42-
The order of Bronsted-Lowry acids and bases in the reaction is .

See explanation

Explanation:

According to Bronsted-Lowry definition of acids/bases, an acid is a proton donor while a base is a proton acceptor.

Hence, in a reaction, the species that donate protons are strong acids while the species that accept protons are strong bases.

Hence, HSO4- is a stronger acid than H2C2O4 and SO42- is a weaker base than HC2O4-

Note that the conjugate base of a strong acid is a weak base and vice versa.

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