Which statement best describes the acid–base behavior of sodium bromide, $NaBr$, when dissolved in water?

• A. $NaBr$ is a weak base because $B{r}^{-}$ is the conjugate base of a weak acid.
• B. $NaBr$ is an acidic salt because $N^a$ hydrolyzes to produce $H^{+}$ in water.
• C. $NaBr$ is a strong base because $B{r}^{-}$ accepts $H^{+}$ strongly from water.
• D. $NaBr$ is a neutral salt (neither acidic nor basic) because it is formed from a strong base and a strong acid.

Answer: (D)