---
title: "A student prepares a buffer solution by mixing \\(100. \\, \\text{mL}\\) of a \\(1.0 \\, \\text{M}\\) solution of a weak acid, \\(\\text{HA}\\) (\\(K_a = 1.0 \\times 10^{-4}\\)), with \\(100. \\, \\text{mL}\\) of a \\(0.10 \\, \\text{M}\\) solution of \\(\\text{NaA}\\). What is the pH of the resulting buffer solution at \\(25^\\circ\\text{C}\\)?"
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url: "https://nerd-notes.com/ubq/119301/"
date_modified: "2026-08-21T18:09:02+00:00"
---

# A student prepares a buffer solution by mixing \(100. \, \text{mL}\) of a \(1.0 \, \text{M}\) solution of a weak acid, \(\text{HA}\) (\(K_a = 1.0 \times 10^{-4}\)), with \(100. \, \text{mL}\) of a \(0.10 \, \text{M}\) solution of \(\text{NaA}\). What is the pH of the resulting buffer solution at \(25^\circ\text{C}\)?

A student prepares a buffer solution by mixing \(100. \, \text{mL}\) of a \(1.0 \, \text{M}\) solution of a weak acid, \(\text{HA}\) (\(K_a = 1.0 \times 10^{-4}\)), with \(100. \, \text{mL}\) of a \(0.10 \, \text{M}\) solution of \(\text{NaA}\). What is the pH of the resulting buffer solution at \(25^\circ\text{C}\)?

- **A.** \(3.00\)
- **B.** \(4.00\)
- **C.** \(5.00\)
- **D.** \(11.00\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119301/*