38 Calculate formula mass and the molar mass of \( \mathrm{CaCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O} \).

To calculate the formula mass and molar mass of \( \mathrm{CaCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O} \), we start by identifying the atomic masses of each element involved. Calcium (Ca) has a mass of approximately 40.08 g/mol, chlorine (Cl) about 35.45 g/mol, and hydrogen (H) and oxygen (O) are about 1.01 g/mol and 16.00 g/mol, respectively. For \( \mathrm{CaCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O} \): - Calcium: 1 x 40.08 = 40.08 g/mol - Chlorine: 2 x 35.45 = 70.90 g/mol - Water (from \( 2 \mathrm{H}_{2} \mathrm{O} \)): 2 x (2 x 1.01 + 16.00) = 2 x 18.02 = 36.04 g/mol Adding these together: 40.08 + 70.90 + 36.04 = 147.02 g/mol. So, the molar mass of \( \mathrm{CaCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O} \) is 147.02 g/mol. When it comes to real-life applications, calcium chloride is widely used not just in various chemical labs but also on roads in winter to manage ice, acting as an effective de-icing agent. Additionally, its hydrated form \( \mathrm{CaCl}_{2} \cdot 2 \mathrm{H}_{2} \mathrm{O} \) is also utilized in food preservation and to keep moisture in packaged goods. Its versatility makes it a staple in many industries!