A solution of 0.278 m (molal) of CaCl2 in water freezes at -1.33 oC. (a) What is the expected freezing point of the solution if CaCl2 dissociates completely in solution?                                (b) What is the apparent van’t Hoff factor i of CaCl2 at this concentration? (Water has Kf = 1.86 oC/m)

Calculate the vapor pressure at 85.0°C of a solution prepared by dissolving 0.450 mol of liquid dibromoethane (C2H4B12, P° = 127 torr) in 1.80 mol of liquid dibromopropane (C3H6Br2, p° = 173 torr). %3D torr

A chemist is studying small organic compounds for theirpotential use as an antifreeze. When 0.243 g of a compound isdissolved in 25.0 mL of water, the freezing point of the solutionis -0.201°C. (a) Calculate the molar mass of the compound (dof water 1.00 g/mL). (b) Analysis shows that the compoundis 53.31 mass % C and 11.18 mass % H, the remainder being O.Calculate the empirical and molecular formulas of the com-pound. (c) Draw a Lewis structure for a compound with this for-mula that forms H bonds and another for one that does not.

The Henry's Law constant of methyl bromide, CH3Br, is k = 0.159 mol/(L atm) at 25°C. What is the solubility of this compound in water at 25°C and at a partial pressure of 406 mmHg?