Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:**Problem Statement:**
The mole fraction of copper(II) nitrate in an aqueous copper(II) nitrate solution is 0.126. What is the molality of the copper(II) nitrate solution?
**Calculation:**
To find the molality (\( m \)) of the solution, we can use the relationship between mole fraction and molality. However, additional details such as molecular weights and density of water might be required for detailed calculation in a practical scenario. Here is how you can approach the calculation:
1. **Understand the Mole Fraction:**
- The mole fraction of copper(II) nitrate (\( \chi_{\text{Cu(NO}_3)_2} \)) = 0.126.
- The mole fraction of water (\( \chi_{\text{H}_2\text{O}} \)) = 1 - 0.126 = 0.874.
2. **Approach:**
- Assuming 1 mole of solution, calculate the moles of solute and solvent:
- Moles of copper(II) nitrate (solute): 0.126 moles.
- Moles of water (solvent): 0.874 moles.
- Convert moles of water to kilograms:
- Since 1 mole of water is approximately 18.015 g, 0.874 moles of water is approximately 15.74 grams or 0.01574 kilograms.
- Molality (\( m \)) = moles of solute / kilograms of solvent.
- \( m = \frac{0.126}{0.01574} \approx 8.01 \, \text{mol/kg} \).
**Conclusion:**
The molality of the copper(II) nitrate solution is approximately 8.01 mol/kg.
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