4.a. Assume you dissolve 45.0 g of camphor, CioH160, in 425 mL of ethanol, C₂H5OH. Determine the molality of camphor in the solution. The density of ethanol is 0.785 g/mL. b. A solution contains 1.00 g of an unknown nonelectrolyte dissolved in 8.01 g of lauric acid, CH3(CH₂)10COOH. The solution freezes at 39.9°C while the freezing point of pure lauric acid is 44.0°C. The freezing point depression constant of cyclohexane is -3.9°C/m. ATfp = iKpm What is the value of i for the solute? What is the value of ATfp? SHOW YOUR WORK What is the molality of the solution? SHOW YOUR WORK How many moles of solute are in the solution? SHOW YOUR WORK What is the molar mass of the solute? SHOW YOUR WORK

4.a. Assume you dissolve 45.0 g of camphor, CioH160, in 425 mL of ethanol, C₂H5OH. Determine the molality of camphor in the solution. The density of ethanol is 0.785 g/mL. b. A solution contains 1.00 g of an unknown nonelectrolyte dissolved in 8.01 g of lauric acid, CH3(CH₂)10COOH. The solution freezes at 39.9°C while the freezing point of pure lauric acid is 44.0°C. The freezing point depression constant of cyclohexane is -3.9°C/m. ATfp = iKpm What is the value of i for the solute? What is the value of ATfp? SHOW YOUR WORK What is the molality of the solution? SHOW YOUR WORK How many moles of solute are in the solution? SHOW YOUR WORK What is the molar mass of the solute? SHOW YOUR WORK

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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