Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water by calculating the freezing point depression of solutions containing 220. g of each salt in 1.00 kg of water. (An advantage of is that it acts more quickly because it is hygroscopic, that is, it absorbs moisture from the air to create a solution and begin the process. A disadvantage is that this compound is more costly.) Assume full dissociation of ionic compounds. Kfp(H2O)= -1.86 °C/m. ΔTfp= °C for NaCl
ΔTfp= °C for CaCl2