A solution is made by dissolving 23.8 g of copper (II) sulfate, CuSO4, in enough water to make exactly 250 mL of solution. Calculate the concentration (molarity) of CuSO4 in mol/L (M). M CUSO4
A solution is made by dissolving 23.8 g of copper (II) sulfate, CuSO4, in enough water to make exactly 250 mL of solution. Calculate the concentration (molarity) of CuSO4 in mol/L (M). M CUSO4
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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![### Solution Concentration Calculation
**Problem Statement:**
A solution is made by dissolving **23.8 g** of **copper(II) sulfate, CuSO₄**, in enough water to make exactly **250 mL** of solution. Calculate the concentration (molarity) of **CuSO₄** in **mol/L (M)**.
**Blank Field:**
\[ \_\_\_.\_\_\_ \text{ M CuSO₄} \]
**Buttons:**
- **Submit**
- **Show Approach**
- **Show Tutor Steps**
**Detailed Explanation:**
Copper(II) sulfate (CuSO₄) is being dissolved to determine the molarity of the resulting solution. To solve this, you'll need to follow these steps:
1. **Convert the mass of CuSO₄ to moles:**
- Find the molar mass of CuSO₄.
- Use the formula:
\[ \text{Moles of CuSO₄} = \frac{\text{Mass of CuSO₄ (g)}}{\text{Molar mass of CuSO₄ (g/mol)}} \]
2. **Convert the volume of the solution from mL to L:**
- Use the conversion:
\[ 250 \, \text{mL} = 0.250 \, \text{L} \]
3. **Calculate the molarity of the solution:**
- Use the formula:
\[ \text{Molarity (M)} = \frac{\text{Moles of solute}}{\text{Volume of solution in liters}} \]
The “Show Approach” and “Show Tutor Steps” buttons provide guidance on the intermediate steps or hint towards solving the problem.
**Note for Educators:**
Use this problem to teach students about the concepts of molarity, unit conversions, and the use of molar masses for calculation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2Fd8e35909-45fa-4076-b3cb-e36b3ab6889d%2Fo8d8ntv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Solution Concentration Calculation
**Problem Statement:**
A solution is made by dissolving **23.8 g** of **copper(II) sulfate, CuSO₄**, in enough water to make exactly **250 mL** of solution. Calculate the concentration (molarity) of **CuSO₄** in **mol/L (M)**.
**Blank Field:**
\[ \_\_\_.\_\_\_ \text{ M CuSO₄} \]
**Buttons:**
- **Submit**
- **Show Approach**
- **Show Tutor Steps**
**Detailed Explanation:**
Copper(II) sulfate (CuSO₄) is being dissolved to determine the molarity of the resulting solution. To solve this, you'll need to follow these steps:
1. **Convert the mass of CuSO₄ to moles:**
- Find the molar mass of CuSO₄.
- Use the formula:
\[ \text{Moles of CuSO₄} = \frac{\text{Mass of CuSO₄ (g)}}{\text{Molar mass of CuSO₄ (g/mol)}} \]
2. **Convert the volume of the solution from mL to L:**
- Use the conversion:
\[ 250 \, \text{mL} = 0.250 \, \text{L} \]
3. **Calculate the molarity of the solution:**
- Use the formula:
\[ \text{Molarity (M)} = \frac{\text{Moles of solute}}{\text{Volume of solution in liters}} \]
The “Show Approach” and “Show Tutor Steps” buttons provide guidance on the intermediate steps or hint towards solving the problem.
**Note for Educators:**
Use this problem to teach students about the concepts of molarity, unit conversions, and the use of molar masses for calculation.
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