Complete these Bronsted-Lowry reactions.

Question

Complete these Bronsted-Lowry reactions.

Reaction 1: HPO^2-/4 +H⁺ ⇌ ?

Reaction 2: HPO^2-/4 +OH^- ⇌?

Answer 1

Reaction 1: HPO₄^2- + H⁺ ⇌ H₂PO₄^-

In reaction 1, H⁺ is a Bronsted-Lowry acid (proton donor) and HPO₄^2- is a B-L base (proton acceptor). To HPO₄^2-, you are adding 1 hydrogen with a charge of +1. Therefore, in the chemical formula of the product, the # of hydrogens increases by 1 (H₂) and the overall charge is obtained by adding (-2) + 1 = -1.

Reaction 2: HPO₄^2- + OH^- ⇌ PO₄^3- + H₂O

In reaction 2, HPO₄^2- is a Bronsted-Lowry acid (proton donor) and OH^- is a B-L base (proton acceptor). On the product side, PO₄^3- is the conjugate base of HPO₄^2-, and H₂O is the conjugate acid of OH^-.

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