If 40.0 g of  MgSO4⋅7H2O
  is thoroughly heated, what mass of anhydrous magnesium sulfate will remain?

When heating magnesium sulfate heptahydrate (MgSO₄·7H₂O), all the water of hydration (7 moles of water per mole of MgSO₄) will be removed, leaving behind anhydrous magnesium sulfate (MgSO₄).

### Step-by-step calculation:
1. **Molar mass of MgSO₄·7H₂O**:
   - Mg: \( 24.31 \, \text{g/mol} \)
   - S: \( 32.07 \, \text{g/mol} \)
   - O₄: \( 4 \times 16.00 \, \text{g/mol} = 64.00 \, \text{g/mol} \)
   - 7H₂O: \( 7 \times (2 \times 1.01 + 16.00) = 126.14 \, \text{g/mol} \)

   So, the molar mass of MgSO₄·7H₂O is:
   \[
   24.31 + 32.07 + 64.00 + 126.14 = 246.52 \, \text{g/mol}
   \]

2. **Molar mass of anhydrous MgSO₄**:
   - Mg: \( 24.31 \, \text{g/mol} \)
   - S: \( 32.07 \, \text{g/mol} \)
   - O₄: \( 4 \times 16.00 = 64.00 \, \text{g/mol} \)

   So, the molar mass of MgSO₄ is:
   \[
   24.31 + 32.07 + 64.00 = 120.38 \, \text{g/mol}
   \]

3. **Mass ratio** of anhydrous MgSO₄ to hydrated MgSO₄·7H₂O:
   \[
   \frac{120.38 \, \text{g/mol}}{246.52 \, \text{g/mol}} = 0.4885
   \]

4. **Mass of anhydrous MgSO₄ remaining** after heating 40.0 g of MgSO₄·7H₂O:
   \[
   40.0 \, \text{g} \times 0.4885 = 19.54 \, \text{g}
   \]

So, after thorough heating, **19.54 g** of anhydrous magnesium sulfate (MgSO₄) will remain.

Would you like more details on any step or have other questions?

Here are 5 related questions:
1. How much water is lost during the heating process?
2. What is the percent composition of water in MgSO₄·7H₂O?
3. What is the significance of heating hydrates in chemical reactions?
4. How would this process differ for other hydrates, like CuSO₄·5H₂O?
5. How can you experimentally verify the loss of water during heating?

**Tip:** Always ensure accurate molar masses when dealing with hydrates to avoid calculation errors.

If 40.0 g of MgSO₄·7H₂O is thoroughly heated, what mass of anhydrous magnesium sulfate will remain?

Learn how to calculate the mass of anhydrous magnesium sulfate (MgSO₄) after thoroughly heating 40.0 g of MgSO₄·7H₂O. This problem involves stoichiometry, molar mass calculations, and mass ratios. Ideal for high school chemistry students.

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