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2. Calculate the normal freezing point of a 0.7439 mol aqueous solution of C12H22O11 that has a density of 1.35 g/ml. (C12H2½O11 is a non-volatile non-dissociating solute.) The molal freezing point depression constant of water is 1.86°C kg/mole. 3. When 0.279 g of a molecular compound, benzoic acid, was dissolved in 43.0 g of benzene, the freezing point of the solution was lowered to 5.15 °C. What is the molecular weight of the benzoic acid? (Note: Kf for benzene = 5.12°C/m; Freezing point of benzene= 5.5°C)

2. Calculate the normal freezing point of a 0.7439 mol aqueous solution of C12H22O11 that has a density of 1.35 g/ml. (C12H2½O11 is a non-volatile non-dissociating solute.) The molal freezing point depression constant of water is 1.86°C kg/mole. 3. When 0.279 g of a molecular compound, benzoic acid, was dissolved in 43.0 g of benzene, the freezing point of the solution was lowered to 5.15 °C. What is the molecular weight of the benzoic acid? (Note: Kf for benzene = 5.12°C/m; Freezing point of benzene= 5.5°C)

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter12: Solutions
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Problem 12.108QP: Analysis of a compound gave 39.50% C, 2.21% H, and 58.30% Cl. When 0.855 g of this solid was...
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Number 2 and 3 only.

TASK 1: SOLVE MY PROBLEMS! Let us further deepen our understanding by solving the following problems: 1. Calculate the boiling point of a solution containing 12g glucose C,H12O6 dissolved in 200g of water H2O. (0.5120C – Kp of H2O) 2. Calculate the normal freezing point of a 0.7439 mol aqueous solution of C12H22O11 that has a density of 1.35 g/ml. (C12H22O11 is a non-volatile non-dissociating solute.) The molal freezing point depression constant of water is 1.86°C kg/mole. 3. When 0.279 g of a molecular compound, benzoic acid, was dissolved in 43.0 g of benzene, the freezing point of the solution was lowered to 5.15 °C. What is the molecular weight of the benzoic acid? (Note: K; for benzene = 5.12°C/m; Freezing point of benzene= 5.5°C)
Transcribed Image Text:TASK 1: SOLVE MY PROBLEMS! Let us further deepen our understanding by solving the following problems: 1. Calculate the boiling point of a solution containing 12g glucose C,H12O6 dissolved in 200g of water H2O. (0.5120C – Kp of H2O) 2. Calculate the normal freezing point of a 0.7439 mol aqueous solution of C12H22O11 that has a density of 1.35 g/ml. (C12H22O11 is a non-volatile non-dissociating solute.) The molal freezing point depression constant of water is 1.86°C kg/mole. 3. When 0.279 g of a molecular compound, benzoic acid, was dissolved in 43.0 g of benzene, the freezing point of the solution was lowered to 5.15 °C. What is the molecular weight of the benzoic acid? (Note: K; for benzene = 5.12°C/m; Freezing point of benzene= 5.5°C)
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