---
title: "A student prepares a solution by dissolving solid barium hydroxide in distilled water to produce a solution of \\(5.0 \\times 10^{-3}\\text{ M}\\ \\text{Ba(OH)}_2\\text{(aq)}\\) at \\(25\\ ^\\circ\\text{C}\\). Assuming complete dissociation, what is the hydronium ion concentration, \\([\\text{H}_3\\text{O}^+]\\), in the solution?"
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date_modified: "2026-08-23T05:04:48+00:00"
---

# A student prepares a solution by dissolving solid barium hydroxide in distilled water to produce a solution of \(5.0 \times 10^{-3}\text{ M}\ \text{Ba(OH)}_2\text{(aq)}\) at \(25\ ^\circ\text{C}\). Assuming complete dissociation, what is the hydronium ion concentration, \([\text{H}_3\text{O}^+]\), in the solution?

A student prepares a solution by dissolving solid barium hydroxide in distilled water to produce a solution of \(5.0 \times 10^{-3}\text{ M}\ \text{Ba(OH)}_2\text{(aq)}\) at \(25\ ^\circ\text{C}\). Assuming complete dissociation, what is the hydronium ion concentration, \([\text{H}_3\text{O}^+]\), in the solution?

- **A.** \(5.0 \times 10^{-13}\text{ M}\)
- **B.** \(1.0 \times 10^{-12}\text{ M}\)
- **C.** \(2.0 \times 10^{-12}\text{ M}\)
- **D.** \(1.0 \times 10^{-2}\text{ M}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121482/*