Identify the products formed in this Brønsted-Lowry reaction.
HSO4^−+HBrO↽−−⇀acid+base
In this Brønsted-Lowry reaction, the HSO4^- ion acts as an acid, while the HBrO molecule acts as a base. When an acid and a base react, they form a conjugate acid-base pair.
To determine the products of this reaction, you need to consider how the acid and base molecules exchange protons (H+). The acid donates a proton, and the base accepts it.
Here's the step-by-step process:
1. HSO4^- (acid) donates a proton (H+) to HBrO (base).
2. The proton transfer forms the conjugate acid of the base and the conjugate base of the acid.
- HSO4^- gains a proton (H+) to become H2SO4 (conjugate acid).
- HBrO accepts the proton to become BrO^- (conjugate base).
So, the products formed in this reaction are H2SO4 (sulfuric acid) and BrO^- (hypobromite ion).
In the given Brønsted-Lowry reaction, the acid (HSO4^-) donates a proton to the base (HBrO). Let's break down the reaction step by step:
1. HSO4^- (acid) donates a proton (H+) to HBrO (base).
2. The reaction proceeds, resulting in the formation of two products:
a) The acid, HSO4^-, loses a proton (H+) and becomes SO4^2-. This is called the conjugate base of HSO4^-.
b) The base, HBrO, gains a proton (H+) and becomes H2BrO2. This is called the conjugate acid of HBrO.
So, the products formed in this Brønsted-Lowry reaction are SO4^2- (conjugate base) and H2BrO2 (conjugate acid).