Equal numbers of moles of two soluble, substances, substance A and substance B, are placed into separate 1.0-L samples of water.

a. The water samples are cooled. Sample A freezes at -0.50°C, and Sample B freezes at -1.00°C. Explain how the solutions can have different freezing points.
b. You pour 500 mL of the solution containing substance B into a different beaker. How would the freezing point of this SOO-mL portion of solution B compare to the freezing point of the 1.0-L sample of solution A?
c. Calculate the molarity of the solutions of A and B. Assume that i = 1 for substance A.
d. If you were to add an additional 1.0 kg of water to solution B, What would be the new freezing point of the solution? Try to write an answer to this question Without using a mathematical formula.
e. What concentration (molality) of substances A and B would result in both solutions having a freezing point of -0.25°C?
f. Compare the boiling points, vapor pressure and osmotic pressure of the original solutions of A and B. Don’t perform the calculations; just state which is the greater in each ease.