a) Write Bronsted acid-base equilibrium equations for the following:

b) Show the acid-base conjugated species, labeling all species

(1) HSO4- + C2O4-2
(2) HPO4-2 + NH4+

a) The Bronsted acid-base equilibrium equations for the given reactions are as follows:

(1) HSO4- + C2O4-2 ⇌ H2C2O4 + SO4-2

(2) HPO4-2 + NH4+ ⇌ NH3 + H2PO4-

b) The acid-base conjugated species for each reaction are:

(1) HSO4- is the Bronsted acid, and SO4-2 is the Bronsted base.
C2O4-2 is the Bronsted base, and H2C2O4 is the Bronsted acid.

(2) HPO4-2 is the Bronsted acid, and H2PO4- is the Bronsted base.
NH4+ is the Bronsted base, and NH3 is the Bronsted acid.

a) To write Bronsted acid-base equilibrium equations, you need to identify any acids and bases involved in the reaction and determine their respective conjugate acid-base pairs. Here are the equations for the given reactions:

(1) HSO4- + C2O4-2 ⇌ SO4-2 + HC2O4-
In this reaction, HSO4- acts as an acid by donating a proton (H+) to C2O4-2, which acts as a base. The conjugate base of HSO4- is SO4-2, and the conjugate acid of C2O4-2 is HC2O4-.

(2) HPO4-2 + NH4+ ⇌ PO4-3 + NH3
In this reaction, HPO4-2 acts as an acid by donating a proton (H+) to NH4+, which acts as a base. The conjugate base of HPO4-2 is PO4-3, and the conjugate acid of NH4+ is NH3.

b) To determine the acid-base conjugated species in a reaction, you need to identify which species gain or lose protons during the equilibrium. Here are the acid-base conjugated species labels for the given reactions:

(1) HSO4- (acid) and SO4-2 (conjugate base)
C2O4-2 (base) and HC2O4- (conjugate acid)

(2) HPO4-2 (acid) and PO4-3 (conjugate base)
NH4+ (base) and NH3 (conjugate acid)