Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute...

Freezing point depression can be used to experimentally determine the van't Hoff factor of a solute in solution. Given the data in the table, please answer the questions below and determine the "real" van't Hoff factor of the solute.

Experimental Results

Mass of solvent (water)	5.267 g
Freezing point of water	0.00°C
Freezing point depression constant (K_f) of water	1.86°C/m
Mass of solution	6.121 g
Freezing point of solution	-3.73°C

a. What mass of solute was used?

b. What is the freezing point depression, ΔT_f, of the solution?

c. What is the colligative molality, m_c, of the solution?

d. How many moles of solute particles are present in solution?

e. If the solute has a molar mass of 235.28, what is the van't Hoff factor, i, for the solute? (Remember that experimentally, i does not have to be an integer!)

Solutions

Expert Solution

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queen_honey_blossom answered 2 months ago

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