A student prepares two separate \(1.0 \text{ L}\) buffer solutions using a weak monoprotic acid, \(\text{HA}\) (\(\text{p}K_a = 5.00\)), and its conjugate base salt, \(\text{NaA}\). Buffer 1 contains \(0.40 \text{ mol}\) of \(\text{HA}\) and \(0.40 \text{ mol}\) of \(\text{NaA}\). Buffer 2 contains \(0.20 \text{ mol}\) of \(\text{HA}\) and \(0.20 \text{ mol}\) of \(\text{NaA}\).

A \(0.10 \text{ mol}\) sample of \(\text{HCl}(g)\) is dissolved into each buffer solution with negligible change in total volume. Which of the following correctly gives the final ratio \(\dfrac{[\text{A}^-]}{[\text{HA}]}\) for each buffer and compares the magnitudes of the \(\text{pH}\) changes (\(\Delta\text{pH} = |\text{pH}_{\text{final}} - \text{pH}_{\text{initial}}|\))?