$$ \begin{array}{c c c}
\text{Solution} & \text{Acid} & K_a \\ \hline
1 & \ce{CH3CO2H} & 1.75\times 10^{-5} \\
2 & \ce{CF3CO2H} & 1.0\times 10^0 \\
\end{array} $$
Acid-dissociation constants of two acids are listed in the table above. A 20. mL sample of a \(0.10 M\) solution of each acid is titrated to the equivalence point with 20. mL of \(0.10 M \ce{NaOH}\). Which of the following is a true statement about the pH of the solutions at the equivalence point?