The freezing point of 42.30 g of a pure solvent is measured to be 43.64 °C. When 2.84 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 40.86 °C. Answer the following questions (the freezing point depression constant of the pure solvent is 7.46 °C-kg solvent/mol solute). What is the molality of the solution? How many moles of solute are present? mol What is the molecular weight of the solute? g/mol

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 12.103QE
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The freezing point of 42.30 g of a pure solvent is measured to be 43.64 °C. When 2.84 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 40.86 °C. Answer the following
questions (the freezing point depression constant of the pure solvent is 7.46 °C-kg solvent/mol solute).
What is the molality of the solution?
How many moles of solute are present?
mol
What is the molecular weight of the solute?
g/mol
Transcribed Image Text:The freezing point of 42.30 g of a pure solvent is measured to be 43.64 °C. When 2.84 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 40.86 °C. Answer the following questions (the freezing point depression constant of the pure solvent is 7.46 °C-kg solvent/mol solute). What is the molality of the solution? How many moles of solute are present? mol What is the molecular weight of the solute? g/mol
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