---
title: "A student dissolves a \\(12.0 \\text{ g}\\) sample of \\(\\text{XCl}\\) (molar mass \\(= 60.0 \\text{ g/mol}\\)) in enough distilled water to make \\(500. \\text{ mL}\\) of solution. In a separate container, the student dissolves a \\(12.0 \\text{ g}\\) sample of \\(\\text{YCl}_2\\) (molar mass \\(= 90.0 \\text{ g/mol}\\)) in enough distilled water to make \\(500. \\text{ mL}\\) of solution. Assuming both salts dissociate completely in water, what is the value of the ratio \\(\\dfrac{[\\text{Cl}^-]_{\\text{YCl}_2}}{[\\text{Cl}^-]_{\\text{XCl}}}\\)?"
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url: "https://nerd-notes.com/ubq/123529/"
date_modified: "2026-09-28T12:00:03+00:00"
---

# A student dissolves a \(12.0 \text{ g}\) sample of \(\text{XCl}\) (molar mass \(= 60.0 \text{ g/mol}\)) in enough distilled water to make \(500. \text{ mL}\) of solution. In a separate container, the student dissolves a \(12.0 \text{ g}\) sample of \(\text{YCl}_2\) (molar mass \(= 90.0 \text{ g/mol}\)) in enough distilled water to make \(500. \text{ mL}\) of solution. Assuming both salts dissociate completely in water, what is the value of the ratio \(\dfrac{[\text{Cl}^-]_{\text{YCl}_2}}{[\text{Cl}^-]_{\text{XCl}}}\)?

A student dissolves a \(12.0 \text{ g}\) sample of \(\text{XCl}\) (molar mass \(= 60.0 \text{ g/mol}\)) in enough distilled water to make \(500. \text{ mL}\) of solution. In a separate container, the student dissolves a \(12.0 \text{ g}\) sample of \(\text{YCl}_2\) (molar mass \(= 90.0 \text{ g/mol}\)) in enough distilled water to make \(500. \text{ mL}\) of solution. Assuming both salts dissociate completely in water, what is the value of the ratio \(\dfrac{[\text{Cl}^-]_{\text{YCl}_2}}{[\text{Cl}^-]_{\text{XCl}}}\)?

- **A.** \(0.67\)
- **B.** \(0.75\)
- **C.** \(1.33\)
- **D.** \(3.00\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123529/*