---
title: "A student mixes \\(50.0\\text{ mL}\\) of \\(1.6 \\times 10^{-5}\\text{ M }\\text{Ba(NO}_3\\text{)}_2\\text{(aq)}\\) with \\(50.0\\text{ mL}\\) of \\(1.0 \\times 10^{-5}\\text{ M }\\text{Na}_2\\text{SO}_4\\text{(aq)}\\) at \\(25\\text{ }^\\circ\\text{C}\\). The dissolution equilibrium for barium sulfate is represented by the following equation.  \\[\\text{BaSO}_4\\text{(s)} \\rightleftharpoons \\text{Ba}^{2+}\\text{(aq)} + \\text{SO}_4^{2-}\\text{(aq)} \\quad\\quad K_{sp} = 1.0 \\times 10^{-10} \\text{ at } 25\\text{ }^\\circ\\text{C}\\]  Which of the following correctly predicts whether a precipitate of \\(\\text{BaSO}_4\\text{(s)}\\) will form and provides the correct justification?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/119745/"
date_modified: "2026-08-21T08:12:12+00:00"
---

# A student mixes \(50.0\text{ mL}\) of \(1.6 \times 10^{-5}\text{ M }\text{Ba(NO}_3\text{)}_2\text{(aq)}\) with \(50.0\text{ mL}\) of \(1.0 \times 10^{-5}\text{ M }\text{Na}_2\text{SO}_4\text{(aq)}\) at \(25\text{ }^\circ\text{C}\). The dissolution equilibrium for barium sulfate is represented by the following equation.

\[\text{BaSO}_4\text{(s)} \rightleftharpoons \text{Ba}^{2+}\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} \quad\quad K_{sp} = 1.0 \times 10^{-10} \text{ at } 25\text{ }^\circ\text{C}\]

Which of the following correctly predicts whether a precipitate of \(\text{BaSO}_4\text{(s)}\) will form and provides the correct justification?

A student mixes \(50.0\text{ mL}\) of \(1.6 \times 10^{-5}\text{ M }\text{Ba(NO}_3\text{)}_2\text{(aq)}\) with \(50.0\text{ mL}\) of \(1.0 \times 10^{-5}\text{ M }\text{Na}_2\text{SO}_4\text{(aq)}\) at \(25\text{ }^\circ\text{C}\). The dissolution equilibrium for barium sulfate is represented by the following equation.

\[\text{BaSO}_4\text{(s)} \rightleftharpoons \text{Ba}^{2+}\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} \quad\quad K_{sp} = 1.0 \times 10^{-10} \text{ at } 25\text{ }^\circ\text{C}\]

Which of the following correctly predicts whether a precipitate of \(\text{BaSO}_4\text{(s)}\) will form and provides the correct justification?

- **A.** No precipitate will form, because \(Q = 4.0 \times 10^{-11}\), which is less than \(K_{sp}\).
- **B.** A precipitate will form, because \(Q = 1.6 \times 10^{-10}\), which is greater than \(K_{sp}\).
- **C.** A precipitate will form, because \(Q = 4.0 \times 10^{-11}\), which is less than \(K_{sp}\).
- **D.** No precipitate will form, because \(Q = 1.6 \times 10^{-10}\), which is greater than \(K_{sp}\).

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119745/*