Question

1. When 0.3163 g of benzoic acid (C7H6O2) was dissolved in 15.563 g cyclohexanol, the freezing point of the mixture was 8.19°C lower than that of the pure cyclohexanol. What is the molal freezing point constant of the cyclohexanol? (?T = m · Kf · i) 2. Since the freezing point of a solution depends on the number of particles, what would you expect for the freezing point of 0.1 m solutions of aqueous NaCl and BaCl2? If the actual freezing points of these solutions were -0.348°C and -0.470°C respectively, what are the van't Hoff factors (i) for these two solids? Fill in the table below with your responses. Ideal van't Hoff | Predicted Freezing Point | Actual Freezing Point | Calculated van't Hoff NaCl | 2 | | -0.348°C | BaCl2 | 3 | | -0.470°C | Do your calculations here: 3. How many grams of ethylene glycol (C2H6O2) per kilogram of water are needed to give protection up to 120°C in a car radiator? (Show your math setup.) How would your response change if you used methyl alcohol (CH3OH) instead of ethylene glycol? Use the back of this page for additional calculation space if necessary.

          1. When 0.3163 g of benzoic acid (C7H6O2) was dissolved in 15.563 g cyclohexanol, the freezing point of the mixture was 8.19°C lower than that of the pure cyclohexanol. What is the molal freezing point constant of the cyclohexanol? (?T = m · Kf · i)

2. Since the freezing point of a solution depends on the number of particles, what would you expect for the freezing point of 0.1 m solutions of aqueous NaCl and BaCl2? If the actual freezing points of these solutions were -0.348°C and -0.470°C respectively, what are the van't Hoff factors (i) for these two solids? Fill in the table below with your responses.

Ideal van't Hoff | Predicted Freezing Point | Actual Freezing Point | Calculated van't Hoff
NaCl | 2 | | -0.348°C |
BaCl2 | 3 | | -0.470°C |

Do your calculations here:

3. How many grams of ethylene glycol (C2H6O2) per kilogram of water are needed to give protection up to 120°C in a car radiator? (Show your math setup.) How would your response change if you used methyl alcohol (CH3OH) instead of ethylene glycol? Use the back of this page for additional calculation space if necessary.

1. When 0.3163 g of benzoic acid (C7H6O2) was dissolved in 15.563 g cyclohexanol, the freezing point of the mixture was 8.19°C lower than that of the pure cyclohexanol. What is the molal freezing point constant of the cyclohexanol? (?T = m · Kf · i)

2. Since the freezing point of a solution depends on the number of particles, what would you expect for the freezing point of 0.1 m solutions of aqueous NaCl and BaCl2? If the actual freezing points of these solutions were -0.348°C and -0.470°C respectively, what are the van't Hoff factors (i) for these two solids? Fill in the table below with your responses.

Ideal van't Hoff | Predicted Freezing Point | Actual Freezing Point | Calculated van't Hoff
NaCl | 2 | | -0.348°C |
BaCl2 | 3 | | -0.470°C |

Do your calculations here:

3. How many grams of ethylene glycol (C2H6O2) per kilogram of water are needed to give protection up to 120°C in a car radiator? (Show your math setup.) How would your response change if you used methyl alcohol (CH3OH) instead of ethylene glycol? Use the back of this page for additional calculation space if necessary.

Added by Phillip B.

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