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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.80QE
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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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