Explain what is the freezing point

1. A solution is made by dissolving 0.586 mol of nonelecrolyte solution in 821 g of benzene. Calculate the freezing point and boiling point of the solution.

2. At -10.00 C, what is the max mass of sucralose (C12H19CI3O8) you can add to 1.50 kg of pure water and still have the solution freeze? Assume that sucralose is a molecular solid and does not ionize when it dissolves in water.

3. The boiling point of an aqueous solution is 101.36 C. What is the freezing point?

4. Imagine two solutions with the same concentration and the same boiling point, but one has benzen as the solvent and the other has carbon tetrachloride as the solvent. Determine that concetration and boiling point.

5. Biphenyl, C12H10, is a nonvolatile, nonionizing solute that is a soluble in benzene, C6H6. At 25 C, the vapor pressure of pure benzene is 100.84 torr. What is the vapor pressure of a solution made from dissolving 12.3 g of biphenyl in 26.6 g of benzene?

6. A solution is made by mixing 41.0 mL of ethanol, C2H6O, and 59.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 C?

7. When 2.66 g of a nonelectrolye solute is dissolved in 985 mL of water at 26 C, the resulting solution exerts an osmotic pressure of 973 torr.What is the molar concentration of the solution? How many moles of solute are in the solution? What is the molar mass of the solute?

8. Which has the highest freezing point? LifePO4, NH4I, Li2SO4, AO2(SO4)3?

9. Assuming 100% dissociation, calculate the freezing point and boiling point of 3.34 m K3PO4(aq).

10. If an 0.550 m aqueous solution freezes at -2.00 C, what is the van't Hoff factor, i, of the solute?

11a. In reverse osmosis, water flows out of a salt solution until the osmotic pressure of the solution equals the applied pressure. If a pressure of 65.0 car is applied to seawater, what will be the final concetration of the seawater at 20 C when reverse osmosis stops?

11b. Assuming that seawater has a total ion concentration of 1.10 Mc, calculate how many liters of seawater are needed to produe 62.0 L of fresh water at 20 C with an applied pressure of 65.0 bar.

12. For an aqueous solution of HF, determine the van't Hoff factor assuming...0% ionization and 100% ionization.A solution is made by dissolving 0.300 mol of HF in enough water to make 1.00 L of solution. At 25 C, the osmotic pressure of the solution is 0.847 atm. What is the percent ionization of the acid?

13. Given that the vapor pressure of water is 17.54 Torr at 20 C, calculate the vaor-pressure lowering of aqueous solutions that are 2.50 m in (a) sucrose, C12H22O11, and (b) calcium chloride. Assume 100% dissociation for electrolytes.