What is the molar mass of a fictitious, non-electrolyte, unknown when 4.1055 g are dissolved to make 225.0 mL of solution with an osmotic pressure of 2.257 atm at 40.1 oC? Assume the theoretical Van't Hoff factor.
What is the molar mass of a fictitious, non-electrolyte, unknown when 4.1055 g are dissolved to make 225.0 mL of solution with an osmotic pressure of 2.257 atm at 40.1 oC? Assume the theoretical Van't Hoff factor.
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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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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What is the molar mass of a fictitious, non-electrolyte, unknown when 4.1055 g are dissolved to make 225.0 mL of solution with an osmotic pressure of 2.257 atm at 40.1 oC? Assume the theoretical Van't Hoff factor.
Expert Solution
Step 1
Given,
The mass of unknown electrolyte= 4.1055g
Volume of solution= 225.0mL
Osmotic pressure= 2.257 atm
Temperature= 40.10C
We have to find the molar mass of the unknown electrolyte
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