Answer:
[tex]\rm Br^{-}[/tex] would be the conjugate base in this reaction according to the Bronsted-Lowry acid-and-base theory.
Explanation:
Among the reactants, the Bronsted-Lowry acid is the species that supplies protons [tex]\rm H^+[/tex]. The Bronsted-Lowry base would be the species that accept the protons.
On the product side of the equation, the BL-acid donates a proton [tex]\rm H^+[/tex] to produce the conjugate base. The BL-base accepts a proton [tex]\rm H^+[/tex] to produce the conjugate acid.
In this case, each [tex]\rm HBr[/tex] molecule donates a proton to form one [tex]\rm Br^{-}[/tex] ion. Hence,
Each [tex]\rm H_2O[/tex] molecule would accept a proton to produce an [tex]\rm H_3O^{+}[/tex] ion. Hence,
