A student titrates separate \(25.00 \text{ mL}\) samples of a \(0.100 \text{ M}\) weak monoprotic acid, \(\text{HA}\) (\(K_a = 1.0 \times 10^{-5}\) at \(25^\circ\text{C}\)), with \(0.100 \text{ M NaOH(aq)}\). In each trial, a different acid-base indicator is used to identify the endpoint of the titration. The results and the pH transition ranges of the indicators are recorded in the table below.

Indicator	pH transition range	Titrant volume at endpoint (mL)	Apparent calculated \([\text{HA}]\) (M)
Methyl red	\(4.4 - 6.2\)	\(18.50\)	\(0.0740\)
Bromothymol blue	\(6.0 - 7.6\)	\(24.60\)	\(0.0984\)
Phenolphthalein	\(8.2 - 10.0\)	\(25.00\)	\(0.100\)
Alizarin yellow R	\(10.2 - 12.0\)	\(28.20\)	\(0.113\)

Based on the data and the principles of acid-base equilibria, which of the following claims and justifications best explains why phenolphthalein accurately determines \([\text{HA}]\) whereas methyl red results in a substantial systematic error?