A student prepares two buffer solutions at 25°C using ethanoic acid (\(\text{CH}_3\text{COOH}\)) and sodium ethanoate (\(\text{CH}_3\text{COONa}\)), as shown in the table below.

Buffer Solution	Volume (mL)	\([\text{CH}_3\text{COOH}]\) (M)	\([\text{CH}_3\text{COONa}]\) (M)
Solution 1	100.0	0.10	0.10
Solution 2	100.0	0.50	0.50

The student adds drops of 1.0 M \(\text{HCl}\) to separate samples of each buffer. Which solution can neutralize a greater volume of the added \(\text{HCl}\) before its pH drops significantly, and why?