Answer
Acid in the left side: $HBrO(aq)$
Base in the left side: $H_2O(l)$
Conjugate Acid: $H_3O^+(aq)$
Conjugate Base: $BrO^-(aq)$
Work Step by Step
$HBrO(aq) + H_2O(l) BrO^-(aq) + H_3O^+(aq)$
Since $HBrO$ donates a proton, it is the Bronsted-Lowry Acid.
Since $H_2O$ receives a proton, it is the Bronsted-Lowry Base.
$BrO^-$ is the conjugate base because it derives from the acid ($HBrO$)
$H_3O^+$ is the conjugate acid because it derives from the base ($H_2O$)
