When 28.2 g of urea (CH4N₂O) are dissolved in 1150. g of a certain mystery liquid X, the freezing point of the solution is 2.4 °C lower than the freezing point of pure X. On the other hand, when 28.2 g of ammonium chloride (NH4Cl) are dissolved in the same mass of X, the freezing point of the solution is 4.8 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for ammonium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. i= 0
When 28.2 g of urea (CH4N₂O) are dissolved in 1150. g of a certain mystery liquid X, the freezing point of the solution is 2.4 °C lower than the freezing point of pure X. On the other hand, when 28.2 g of ammonium chloride (NH4Cl) are dissolved in the same mass of X, the freezing point of the solution is 4.8 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for ammonium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. i= 0
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Transcribed Image Text:When 28.2 g of urea (CH,N,O) are dissolved in 1150. g of a certain mystery liquid X, the freezing point of the solution is 2.4 °C lower than the freezing point
of pure X. On the other hand, when 28.2 g of ammonium chloride (NH4Cl) are dissolved in the same mass of X, the freezing point of the solution is 4.8 °C
lower than the freezing point of pure X.
Calculate the van't Hoff factor for ammonium chloride in X. Be sure your answer has unit symbol, if necessary, and round your answer to 2 significant digits.
i=0
X
►
00
Ar
8:
Expert Solution
Step 1: Determine the van't Hoff factor for ammonium chloride in solvent 'X' from the given data:
Given,
mass of urea ( CH4N2O ) = 28.2 g
mass of solvent 'X' = 1150. g
change in freezing point of urea solution = 2.4 oC
mass of ammonium chloride ( NH4Cl ) = 28.2 g
change in freezing point of urea solution = 4.8 oC
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