1. Calculate the boiling point of a solution containing 12g glucose C6H12O6 dissolved in 200g of water H2O. (0.5120C – Kb 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 1.86OC 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 = 5.120C/m; Freezing point of benzene= 5.50C)
1. Calculate the boiling point of a solution containing 12g glucose C6H12O6 dissolved in 200g of water H2O. (0.5120C – Kb 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 1.86OC 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 = 5.120C/m; Freezing point of benzene= 5.50C)
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter13: Solutions And Their Behavior
Section: Chapter Questions
Problem 71GQ: An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25...
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1. Calculate the boiling point of a solution containing 12g glucose
C6H12O6 dissolved in 200g of water H2O. (0.5120C – Kb 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 1.86OC 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 = 5.120C/m; Freezing point of benzene= 5.50C)
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