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, answer the questions below and determine the "real" van 't Hoff factor of the solute.Experimental ResultsMass of solvent (water)8.413 gFreezing point of water0.00°CFreezing point depression constant (Kf) of water 1.86°C/mMass of solution9.226 gFreezing point of solution−4.73°C(a) What mass of solute was used? g(b) What is the freezing point depression ΔTf of the solution? °C(c) What is the colligative molality mc of the solution? m(d) How many moles of solute particles are present in solution? mol(e) If the solute has a molar mass of 144.02, what is the van 't Hoff factor i for the solute? (Remember that experimentally, i does not have to be an integer.)

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Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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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, answer the questions below and determine the "real" van 't Hoff factor of the solute.

Experimental Results

Mass of solvent (water)	8.413 g
Freezing point of water	0.00°C
Freezing point depression constant (K_f) of water	1.86°C/m
Mass of solution	9.226 g
Freezing point of solution	−4.73°C

(a) What mass of solute was used?
  g

(b) What is the freezing point depression ΔT_f of the solution?
  °C

(c) What is the colligative molality m_c of the solution?
  m

(d) How many moles of solute particles are present in solution?
  mol

(e) If the solute has a molar mass of 144.02, what is the van 't Hoff factor i for the solute? (Remember that experimentally, i does not have to be an integer.)

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“Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts for you. To get the remaining sub-part solved please repost the complete question and mention the sub-parts to be solved.”

According to the question,

Mass of solvent (water) = 8.413 g

The Freezing point of water= is 0.00°C

The Freezing point depression constant (K_f) of water =1.86°C/m

The Mass of solution= 9.226 g

The Freezing point of solution = −4.73°C

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