37 Calculate formula mass and the molar mass of \( \mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O} \).

To calculate the formula mass and the molar mass of \( \mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O} \), we first break it down into its components. The formula consists of copper (Cu), sulfur (S), oxygen (O), and water (H₂O). 1. **Cu**: 1 × 63.55 g/mol = 63.55 g/mol 2. **S**: 1 × 32.07 g/mol = 32.07 g/mol 3. **O** in \( \mathrm{CuSO}_{4} \): 4 × 16.00 g/mol = 64.00 g/mol 4. **H₂O**: Each H₂O contributes 18.02 g/mol, and for 5 H₂O: 5 × 18.02 g/mol = 90.10 g/mol Now, add them all together: \[ \text{Total} = 63.55 + 32.07 + 64.00 + 90.10 = 249.72 \text{ g/mol} \] Thus, the formula and molar mass of \( \mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O} \) is approximately 249.72 g/mol. To dive a little deeper, did you know that copper sulfate pentahydrate has both practical and artistic uses? It’s often employed in agriculture as a fungicide and algicide, and it can be found in chemistry labs for experiments. Even artists love it for creating vibrant blue pigments! Just make sure to handle it with care; safety first!