Consider a solution made by massing 8.3 g of a nonvolatile solute (molar mass = 68.51 g/mol) and then adding water to the 100-mL mark on a volumetric flask. The solution density is 1.03 g/mL at a temperature of 30.8°C. The vapor pressure o water at this temperature is 33.3 torr. The freeing point depression constant fo water is 1.86 K/molal. Part 1- Answer ALL of these. (a) Compute the mole fraction of solute in the solution. (b) Compute the mole fraction of water in the solution. (c) Compute the molarity of the solution. (d) Compute the molality of the solution.
Consider a solution made by massing 8.3 g of a nonvolatile solute (molar mass = 68.51 g/mol) and then adding water to the 100-mL mark on a volumetric flask. The solution density is 1.03 g/mL at a temperature of 30.8°C. The vapor pressure o water at this temperature is 33.3 torr. The freeing point depression constant fo water is 1.86 K/molal. Part 1- Answer ALL of these. (a) Compute the mole fraction of solute in the solution. (b) Compute the mole fraction of water in the solution. (c) Compute the molarity of the solution. (d) Compute the molality of the solution.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.95QE
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Transcribed Image Text:2. Consider a solution made by massing 8.3 g of a nonvolatile solute (molar mass =
68.51 g/mol) and then adding water to the 100-mL mark on a volumetric flask. The
solution density is 1.03 g/mL at a temperature of 30.8°C. The vapor pressure of
water at this temperature is 33.3 torr. The freeing point depression constant for
water is 1.86 K/molal.
Part 1- Answer ALL of these.
(a) Compute the mole fraction of solute in the solution.
(b) Compute the mole fraction of water in the solution.
(c) Compute the molarity of the solution.
(d) Compute the molality of the solution.
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