When 3.56 g of a nonelectrolyte solute is dissolved in water to make 925 mL of solution at 21 °C, the solution exerts an osmotic pressure of 849 torr. What is the molar concentration of the solution? concentration: How many moles of solute are in the solution? moles of solute: mol What is the molar mass of the solute? molar mass: g/mol
When 3.56 g of a nonelectrolyte solute is dissolved in water to make 925 mL of solution at 21 °C, the solution exerts an osmotic pressure of 849 torr. What is the molar concentration of the solution? concentration: How many moles of solute are in the solution? moles of solute: mol What is the molar mass of the solute? molar mass: g/mol
Chemistry
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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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:When 3.56 g of a nonelectrolyte solute is dissolved in water to make 925 mL of solution at 21 °C, the solution exerts an osmotic
pressure of 849 torr.
What is the molar concentration of the solution?
concentration:
M
How many moles of solute are in the solution?
moles of solute:
mol
What is the molar mass of the solute?
molar mass:
g/mol
Expert Solution
Step 1
Given,
mass of nonelectrolyte solute (m) = 3.56 g
Note: 1000 mL = 1 L
Volume of solution (V) = 925 mL = 0.925 L
Temperature (T) = 21°C = (21 + 273.15) K = 294.15 K
Note: 760 torr = 1 atm
Osmotic pressure (π) = 849 torr = 1.117 atm
van't Hoff factor (i) for nonelectrolyte solute = 1
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