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3. In a freezing point experiment using acetic acid as a solvent the following values were obtained: Tr (acetic acid) = 16.1°C Tr (with 1.60 g of solute in 10.00 mL of acetic acid) = -2.5°C Use this data to calculate the molecular mass of the solute. (Acetic acid: Kr=3.9 °C-kg/mol; D=1.05 g/mL)

3. In a freezing point experiment using acetic acid as a solvent the following values were obtained: Tr (acetic acid) = 16.1°C Tr (with 1.60 g of solute in 10.00 mL of acetic acid) = -2.5°C Use this data to calculate the molecular mass of the solute. (Acetic acid: Kr=3.9 °C-kg/mol; D=1.05 g/mL)

Chemistry
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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2. Calculate the expected osmotic pressure for a solution prepared from 82.0 g of KBr and 125 g of water at 20.0°C. (Density of this solution is 1.375 g/mL) 82.0 g KBv. Imolker = 0.689 moles HBr 119gKBr K: 39.10 8=79.90 1198/mal π = iMRT 200+273.15=2 3. In a freezing point experiment using acetic acid as a solvent the following values were obtained: Tr (acetic acid) = 16.1°C Tr (with 1.60 g of solute in 10.00 mL of acetic acid) = -2.5°C Use this data to calculate the molecular mass of the solute. (Acetic acid: Kr=3.9 °C-kg/mol; D=1.05 g/mL) 4. Calculate the mole fraction of solvent in a NaC₂H302 (sodium acetate) in an aqueous solution that has a freezing point of -4.40 °C. Use the theoretical van't hoff factor.
Transcribed Image Text:2. Calculate the expected osmotic pressure for a solution prepared from 82.0 g of KBr and 125 g of water at 20.0°C. (Density of this solution is 1.375 g/mL) 82.0 g KBv. Imolker = 0.689 moles HBr 119gKBr K: 39.10 8=79.90 1198/mal π = iMRT 200+273.15=2 3. In a freezing point experiment using acetic acid as a solvent the following values were obtained: Tr (acetic acid) = 16.1°C Tr (with 1.60 g of solute in 10.00 mL of acetic acid) = -2.5°C Use this data to calculate the molecular mass of the solute. (Acetic acid: Kr=3.9 °C-kg/mol; D=1.05 g/mL) 4. Calculate the mole fraction of solvent in a NaC₂H302 (sodium acetate) in an aqueous solution that has a freezing point of -4.40 °C. Use the theoretical van't hoff factor.
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