Answer
A $NaBr$ solution is going to be neutral.
Work Step by Step
1. Identify the strength of each ion in the salt:
$Na^+$: Insignificant acidity.
- Since $Na^+$ is the conjugate acid of a strong base $NaOH$, it has a negligible acidity.
$Br^-$: Insignificant basicity:
- Since $Br^-$ is the conjugate base of a strong acid: $HBr$, it has a negligible basicity.
Therefore, since none of the ions are significant electrolytes, the solution of this salt will be neutral.
