A student intends to prepare a buffer solution with a target \(\text{pH} = 4.80\) by reacting a weak monoprotic acid, \(\text{HA}\) (\(\text{p}K_a = 4.80\)), with a strong base according to the following equation:

\[ \text{HA(aq)} + \text{OH}^-\text{(aq)} \rightarrow \text{A}^-\text{(aq)} + \text{H}_2\text{O(l)} \]

The procedure directs the student to use a volumetric pipet to deliver \(50.0 \text{ mL}\) of \(0.20 \text{ M HA}\) into a flask, followed by the addition of \(25.0 \text{ mL}\) of \(0.20 \text{ M NaOH(aq)}\) from a buret. However, the student rinsed the volumetric pipet with distilled water immediately before use and did not condition it with the \(0.20 \text{ M HA}\) solution, leaving residual water droplets inside the pipet barrel. Assuming all other measurements are carried out correctly and \(\text{HA}\) remains in stoichiometric excess over \(\text{OH}^-\), how will the initial \(\text{pH}\) of the prepared buffer compare to the target \(\text{pH}\) of \(4.80\), and what is the correct justification?