Answer
That statement is true.
Work Step by Step
There is a significant difference between the pH at the equivalence point, when titrating a weak and a strong acid, which makes a neutral solution.
$HNO_3:$
$HNO_3(aq) + NaOH(aq) -- \gt N{O_3}^-(aq) + Na^+(aq) + H_2O(l)$
- As we can see, at the end of the reaction, there are no significant electrolytes.
$CH_3COOH:$
$CH_3COOH(aq) + NaOH(aq) -- \gt CH_3COO^-(aq) + Na^+(aq) + H_2O(l)$
But, in this case, there are $CH_3COO^-$ ions at the end, making the solution basic.
Neutrals solutions have lower pH than basic ones.
