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The mole fraction of copper(II) nitrate in an aqueous copper(II) nitrate solution is

The mole fraction of copper(II) nitrate in an aqueous copper(II) nitrate solution is

Chemistry
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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**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.
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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