How do you identify the conjugate pairs in this acid-base reaction?

The reactant that loses an H+ is acting as an acid. Since HSO4- becomes SO4-2, the HSO4- is acting as an acid. That makes SO4-2 its conjugate base. Likewise, HSO3- has gained an H+ to become H2SO3, meaning HSO3- is acting as a base. That makes H2SO3 its conjugate acid.

The acid reactant is the one that donates a H+ to the other reactant. Here, HSO4- donates a H+ to HSO3- to form H2SO3 and SO4 2-. So HSO4- is the acid reactant. Its conjugate base is what is left after removing the H+ (SO4 2-). The conjugate acid of the base HSO3- is what was formed when H+ was added to it (H2SO3).

HSO3- is the base, HSO4- acid. H2SO4 is the conjugate acid, SO3^2- the conjugate base. You can easily identify the acid, because it always donates a hydrogen, which is always accepted by the base. The conjugate acid of a base has 1 more hydrogen and 1 less negative charge than the original base. The conjugate base of an acid always has 1 less hydrogen and one more negative charge.

The reactant that loses an H+ is acting as an acid. Since HSO4- becomes SO4-2, the HSO4- is acting as an acid. That makes SO4-2 its conjugate base. Likewise, HSO3- has gained an H+ to become H2SO3, meaning HSO3- is acting as a base. That makes H2SO3 its conjugate acid.

The acid reactant is the one that donates a H+ to the other reactant. Here, HSO4- donates a H+ to HSO3- to form H2SO3 and SO4 2-. So HSO4- is the acid reactant. Its conjugate base is what is left after removing the H+ (SO4 2-). The conjugate acid of the base HSO3- is what was formed when H+ was added to it (H2SO3).

challenging aspect. query on google. this could help!