---
title: "A student tests a barium hydroxide solution used to neutralize acidic wastewater. At \\(25^\\circ\\text{C}\\), the analytical concentration of \\(\\text{Ba(OH)}_2\\) is \\(5.0 \\times 10^{-3}\\text{ M}\\). Assume that the solute dissociates completely according to the equation  \\(\\text{Ba(OH)}_2\\text{(aq)} \\rightarrow \\text{Ba}^{2+}\\text{(aq)} + 2\\text{OH}^{-}\\text{(aq)}\\)  What are the \\(\\text{pOH}\\) and \\(\\text{pH}\\) of the solution?"
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url: "https://nerd-notes.com/ubq/119324/"
date_modified: "2026-08-19T12:39:49+00:00"
---

# A student tests a barium hydroxide solution used to neutralize acidic wastewater. At \(25^\circ\text{C}\), the analytical concentration of \(\text{Ba(OH)}_2\) is \(5.0 \times 10^{-3}\text{ M}\). Assume that the solute dissociates completely according to the equation

\(\text{Ba(OH)}_2\text{(aq)} \rightarrow \text{Ba}^{2+}\text{(aq)} + 2\text{OH}^{-}\text{(aq)}\)

What are the \(\text{pOH}\) and \(\text{pH}\) of the solution?

A student tests a barium hydroxide solution used to neutralize acidic wastewater. At \(25^\circ\text{C}\), the analytical concentration of \(\text{Ba(OH)}_2\) is \(5.0 \times 10^{-3}\text{ M}\). Assume that the solute dissociates completely according to the equation

\(\text{Ba(OH)}_2\text{(aq)} \rightarrow \text{Ba}^{2+}\text{(aq)} + 2\text{OH}^{-}\text{(aq)}\)

What are the \(\text{pOH}\) and \(\text{pH}\) of the solution?

- **A.** \(\text{pOH}=1.70\) and \(\text{pH}=12.30\)
- **B.** \(\text{pOH}=2.00\) and \(\text{pH}=12.00\)
- **C.** \(\text{pOH}=2.30\) and \(\text{pH}=11.70\)
- **D.** \(\text{pOH}=12.00\) and \(\text{pH}=2.00\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119324/*