freezing point of 57.08 g of a pure solvent is measured to be 50.83 ºC. When 2.86 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 48.78 ºC. Answer the following questions ( the freezing point depression constant of the pure solvent is 7.33 ºC·kg solvent/mol solute). What is the molality of the solution? How many moles of solute are present? What is the molecular weight of the solute?
The freezing point of 57.08 g of a pure solvent is measured to be 50.83 ºC. When 2.86 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 48.78 ºC. Answer the following questions ( the freezing point depression constant of the pure solvent is 7.33 ºC·kg solvent/mol solute).
What is the molality of the solution?
How many moles of solute are present?
What is the molecular weight of the solute?
Given ->
Weight of solvent= 57.08 gm = 0.05708 kg (1kg=1000g)
Freezing point of pure solvent = 50.83°C
Weight of solute = 2.86 gm
Van't Hoff factor = 1.0000
Freezing point of solution= 48.78°C
Freezing point depression constant= 7.33°C.kg/mole
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