---
title: "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?"
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url: "https://nerd-notes.com/ubq/119317/"
date_modified: "2026-08-19T12:39:47+00:00"
---

# 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?

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?

- **A.** Solution 1, because lower solute concentrations minimize repulsions between ions, allowing the weak base to react more rapidly with added \(\text{H}_3\text{O}^+\).
- **B.** Solution 1, because its initial pH is lower, making it better suited to absorb additional acidic species.
- **C.** Solution 2, because it contains a greater concentration of \(\text{CH}_3\text{COO}^-\)
- **D.** Solution 2, because its initial pH is higher than that of Solution 1, allowing more acid to be added before the solution becomes acidic.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119317/*