Answer
The pH at the equivalence point is equal to 7.
Work Step by Step
For a titration between a strong acid and a strong base ($HBr$ and $KOH$), the pH at the equivalence point will be equal to 7.
This is the neutralization reaction:
$HBr(aq) + KOH(aq) -- \gt KBr(aq) + H_2O(l)$
At the equivalence point, the $HBr$ is completely neutralized by the $KOH$. Therefore, the remaining compounds in the solution are $KBr$, which is a neutral salt, and $H_2O$, which is also neutral.
So, the pH at that point is equal to the pH of a neutral water solution, which is equal to 7.
