Answer
The pH at the equivalence point of that titration is above 7.
Work Step by Step
$NaHCO_3$ is a strong electrolyte, therefore, it is completely dissociated in: $Na^+$ and $HCO_3^-$. That last one can act as an acid if $NaOH$ is added to the solution. That reaction can be described by the equation:
$NaHCO_3 (aq) + NaOH(aq) -- \gt Na_2CO_3(aq) + H_2O(l)$
At the equivalence point, all the $NaHCO_3$ and $NaOH$ is consumed, and the only remaining compounds are $Na_2CO_3$ and $H_2O$.
Since $Na_2CO_3$ is also a strong electrolyte, the $CO_3^{2-}$ ion will be present in the solution.
$CO_3^{2-}$ acts as a base in water, therefore, the pH at the equivalence point is basic. pH $\gt$ 7.
The $Na^+$ ions and the water will not affect the pH of the solution.
