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1. What is the value of the temperature to be used to solve for the osmotic pressure of the solution?  2. What is the osmotic pressure of solution?  3. At the same temperature, what will be the molar concentration of glycerol considering the computed osmotic pressure of the solution and the normal osmotic pressure inside a yeast cell of 7.3 atmospheres?

1. What is the value of the temperature to be used to solve for the osmotic pressure of the solution?  2. What is the osmotic pressure of solution?  3. At the same temperature, what will be the molar concentration of glycerol considering the computed osmotic pressure of the solution and the normal osmotic pressure inside a yeast cell of 7.3 atmospheres?

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
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Questions: 

1. What is the value of the temperature to be used to solve for the osmotic pressure of the solution? 

2. What is the osmotic pressure of solution? 

3. At the same temperature, what will be the molar concentration of glycerol considering the computed osmotic pressure of the solution and the normal osmotic pressure inside a yeast cell of 7.3 atmospheres? 

Yeasts are able to produce high internal concentrations of glycerol to counteract the osmotic pressure of the surrounding media. Suppose that a sample of yeast cells were placed in a 4% sodium chloride solution by weight. Density of solution at 25 °C = 1.02 g/mL MW of solute = 58.44 g/mol i of glycerol = 1 R = 0.08205 L-atm/mol·K %3D
Transcribed Image Text:Yeasts are able to produce high internal concentrations of glycerol to counteract the osmotic pressure of the surrounding media. Suppose that a sample of yeast cells were placed in a 4% sodium chloride solution by weight. Density of solution at 25 °C = 1.02 g/mL MW of solute = 58.44 g/mol i of glycerol = 1 R = 0.08205 L-atm/mol·K %3D
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