Determine mass percent of a solution of sucrose (C12H01) prepared by dissolving 3.245 g of C12H,O in 73.5 g of water.

Chemistry
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Chapter1: Chemical Foundations
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**Determine the mass percent of a solution of sucrose (C₁₂H₂₂O₁₁) prepared by dissolving 3.245 g of C₁₂H₂₂O₁₁ in 73.5 g of water.**

### Explanation:

To calculate the mass percent of a solution:

1. **Determine the total mass of the solution:**
   - Mass of sucrose = 3.245 g
   - Mass of water = 73.5 g
   - Total mass of solution = 3.245 g + 73.5 g = 76.745 g

2. **Use the formula for mass percent:**

   \[
   \text{Mass percent} = \left( \frac{\text{Mass of solute}}{\text{Total mass of solution}} \right) \times 100
   \]

3. **Substitute the values:**

   \[
   \text{Mass percent} = \left( \frac{3.245}{76.745} \right) \times 100
   \]

4. **Calculate the mass percent:**

   \[
   \text{Mass percent} \approx 4.23\%
   \]

Therefore, the mass percent of sucrose in the solution is approximately 4.23%.
Transcribed Image Text:**Determine the mass percent of a solution of sucrose (C₁₂H₂₂O₁₁) prepared by dissolving 3.245 g of C₁₂H₂₂O₁₁ in 73.5 g of water.** ### Explanation: To calculate the mass percent of a solution: 1. **Determine the total mass of the solution:** - Mass of sucrose = 3.245 g - Mass of water = 73.5 g - Total mass of solution = 3.245 g + 73.5 g = 76.745 g 2. **Use the formula for mass percent:** \[ \text{Mass percent} = \left( \frac{\text{Mass of solute}}{\text{Total mass of solution}} \right) \times 100 \] 3. **Substitute the values:** \[ \text{Mass percent} = \left( \frac{3.245}{76.745} \right) \times 100 \] 4. **Calculate the mass percent:** \[ \text{Mass percent} \approx 4.23\% \] Therefore, the mass percent of sucrose in the solution is approximately 4.23%.
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