Question

1. What is the freezing point of a solution prepared by dissolving 7.40 g of K2SO4 in 110 g of water? (4) 2. A solution of 5.00 g of sodium chloride in 1.00 kg of water has a freezing point of -0.299 °C. What is the actual van't Hoff factor for this salt at this concentration compared to the ideal one of 2? (4) 3. The osmotic pressure of blood is 7.65 atm at 37°C. What mass of glucose (C6H12O6) is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood. (5) 4. Pure benzene freezes at 5.50°C. A solution prepared by dissolving 0.450 g of an unknown substance in 27.3 g of benzene is found to freeze at 4.18 °C. Determine the molecular weight of the unknown substance. The freezing point constant for benzene is 5.12°C.kg.mol-1. Note the assumption that the solute is nonvolatile. (6) 5. A KCl solution is prepared by dissolving 40.0 g KCl in 250.0 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg? (6) Constants: Kf (H2O) = 1.86°C. kg. mol-1 Kb(H2O) = 0.51°C. kg. mol-1 R = 0.08206 L. atm. mol-1.K-1 R = 8.314 J.K-1.mol-1 Solubility = k.P

          1. What is the freezing point of a solution prepared by dissolving 7.40 g of K2SO4 in 110 g of water? (4)
2. A solution of 5.00 g of sodium chloride in 1.00 kg of water has a freezing point of -0.299 °C. What is the actual van't Hoff factor for this salt at this concentration compared to the ideal one of 2? (4)
3. The osmotic pressure of blood is 7.65 atm at 37°C. What mass of glucose (C6H12O6) is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood. (5)
4. Pure benzene freezes at 5.50°C. A solution prepared by dissolving 0.450 g of an unknown substance in 27.3 g of benzene is found to freeze at 4.18 °C. Determine the molecular weight of the unknown substance. The freezing point constant for benzene is 5.12°C.kg.mol-1. Note the assumption that the solute is nonvolatile. (6)
5. A KCl solution is prepared by dissolving 40.0 g KCl in 250.0 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg? (6)

Constants:
Kf (H2O) = 1.86°C. kg. mol-1
Kb(H2O) = 0.51°C. kg. mol-1
R = 0.08206 L. atm. mol-1.K-1
R = 8.314 J.K-1.mol-1
Solubility = k.P

1. What is the freezing point of a solution prepared by dissolving 7.40 g of K2SO4 in 110 g of water? (4)
2. A solution of 5.00 g of sodium chloride in 1.00 kg of water has a freezing point of -0.299 °C. What is the actual van't Hoff factor for this salt at this concentration compared to the ideal one of 2? (4)
3. The osmotic pressure of blood is 7.65 atm at 37°C. What mass of glucose (C6H12O6) is needed to prepare 2.25 L of solution for intravenous injection? The osmotic pressure of the glucose solution must equal the osmotic pressure of blood. (5)
4. Pure benzene freezes at 5.50°C. A solution prepared by dissolving 0.450 g of an unknown substance in 27.3 g of benzene is found to freeze at 4.18 °C. Determine the molecular weight of the unknown substance. The freezing point constant for benzene is 5.12°C.kg.mol-1. Note the assumption that the solute is nonvolatile. (6)
5. A KCl solution is prepared by dissolving 40.0 g KCl in 250.0 g of water at 25°C. What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg? (6)

Constants:
Kf (H2O) = 1.86°C. kg. mol-1
Kb(H2O) = 0.51°C. kg. mol-1
R = 0.08206 L. atm. mol-1.K-1
R = 8.314 J.K-1.mol-1
Solubility = k.P

Added by Leslie B.

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