---
title: "A student prepares a solution by dissolving \\(\\text{H}_2\\text{SO}_4\\text{(aq)}\\) in distilled water to give a final concentration of \\(0.0050 \\text{ M}\\). Assuming that both protons dissociate completely in this dilute solution, what is the pH of the solution at \\(25^\\circ\\text{C}\\)?"
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url: "https://nerd-notes.com/ubq/119311/"
date_modified: "2026-08-19T12:39:46+00:00"
---

# A student prepares a solution by dissolving \(\text{H}_2\text{SO}_4\text{(aq)}\) in distilled water to give a final concentration of \(0.0050 \text{ M}\). Assuming that both protons dissociate completely in this dilute solution, what is the pH of the solution at \(25^\circ\text{C}\)?

A student prepares a solution by dissolving \(\text{H}_2\text{SO}_4\text{(aq)}\) in distilled water to give a final concentration of \(0.0050 \text{ M}\). Assuming that both protons dissociate completely in this dilute solution, what is the pH of the solution at \(25^\circ\text{C}\)?

- **A.** 2.00
- **B.** 2.30
- **C.** 3.00
- **D.** 12.00

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119311/*