---
title: "A student prepares a solution by mixing equal volumes of solution containing equal concentrations of standard aqueous solutions, specifically mixing equal volumes of stoichiometric equivalents of a weak monoprotic acid,  \\(\\text{HC}_2\\text{H}_3\\text{O}_2\\text{(aq)}\\), and a strong base, \\(\\text{NaOH(aq)}\\), at \\(25^\\circ\\text{C}\\). Which of the following correctly predicts whether the resulting solution is acidic, neutral, or basic, and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/119211/"
date_modified: "2026-08-19T12:39:23+00:00"
---

# A student prepares a solution by mixing equal volumes of solution containing equal concentrations of standard aqueous solutions, specifically mixing equal volumes of stoichiometric equivalents of a weak monoprotic acid, 
\(\text{HC}_2\text{H}_3\text{O}_2\text{(aq)}\), and a strong base, \(\text{NaOH(aq)}\), at \(25^\circ\text{C}\). Which of the following correctly predicts whether the resulting solution is acidic, neutral, or basic, and provides the correct justification?

A student prepares a solution by mixing equal volumes of solution containing equal concentrations of standard aqueous solutions, specifically mixing equal volumes of stoichiometric equivalents of a weak monoprotic acid, 
\(\text{HC}_2\text{H}_3\text{O}_2\text{(aq)}\), and a strong base, \(\text{NaOH(aq)}\), at \(25^\circ\text{C}\). Which of the following correctly predicts whether the resulting solution is acidic, neutral, or basic, and provides the correct justification?

- **A.** The solution is neutral (\(\text{pH} = 7.0\)) because equal moles of acid and base react completely to form a neutral salt and water.
- **B.** The solution is acidic (\(\text{pH} < 7.0\)) because \(\text{HC}_2\text{H}_3\text{O}_2\text{(aq)}\) is a weak acid that does not react completely with \(\text{NaOH(aq)}\), leaving excess \(\text{H}^+\text{(aq)}\) in solution.
- **C.** The solution is basic (\(\text{pH} > 7.0\)) because the conjugate base reacts with water according to \(\text{C}_2\text{H}_3\text{O}_2^-\text{(aq)} + \text{H}_2\text{O(l)} \rightleftharpoons \text{HC}_2\text{H}_3\text{O}_2\text{(aq)} + \text{OH}^-\text{(aq)}\).
- **D.** The solution is basic (\(\text{pH} > 7.0\)) because \(\text{NaOH(aq)}\) is a strong base that dissociates completely, leaving unreacted \(\text{OH}^-\text{(aq)}\) in excess.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119211/*