2. Calculate the theoretical freezing point of the ice bath that you prepared in the laboratory. Assume that all 65.0gNaCl dissolved in 160.0gHH2 (some of the ice melted). Don't forget that 3. How would the freezing point from problem \#2 change if CaCl2 was used instead? (Assume that the same molality of solution is made.) Prove this by calculating the new freezing point. 65.00CaCl2160.0of12O65.00Cad2110.91mol=0.095ked0.586mol=6.16mT=(1.86)(6.16)(3)