A solution made by dissolving 3.46 g of an unknown compound in 85.0 g of benzene froze at 4.13 °C. What is the molar mass of the compound? The molar mass of the compound = i g mol 1 eTextbook and Media Save for Later Attempts: 0 of 15 used Submit Answer
A solution made by dissolving 3.46 g of an unknown compound in 85.0 g of benzene froze at 4.13 °C. What is the molar mass of the compound? The molar mass of the compound = i g mol 1 eTextbook and Media Save for Later Attempts: 0 of 15 used Submit Answer
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter13: Solutions And Their Behavior
Section: Chapter Questions
Problem 71GQ: An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25...
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Step 1
Given,
Mass of an unknown compound = 3.46 g
Mass of benzene = 85.0 g = 0.085 Kg
Freezing point of the solution (Tf(solution)) = 4.13°C
Molar mass of the compound = ?
Note:
Freezing point of pure benzene (Tf°(benzene)) = 5.5°C
Freezing point depression constant (Kf) for benzene = 5.12 °C/m
Assuming an unknown compound to be non-electrolyte van't Hoff factor (i) =1
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