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!)

Expert Solution

Dear student,

Please give a positive rating if satisfied with the answer.

queen_honey_blossom answered 3 months ago

Calculate the van't Hoff factor for an aqueous acetic acid solution that has a concentration of...

Calculate the van't Hoff factor for an aqueous acetic acid solution that has a concentration of 0.400 percent by mass and a freezing point of -0.200oC?

If 100 percent of the NaCL molecules dissociated, the Van't Hoff Factor, I, would be equal...

If 100 percent of the NaCL molecules dissociated, the Van't Hoff Factor, I, would be equal to 2 for NaCI. We assumed I=2 when we calculated the Kf of the NaCl solution. a Now calculate the opposite. Experimentally determine the Van't Hoff factor ( I ) for each NaCl trial, using kf=1.86 C/m and the calculated molality of your NaCl solution and the change in temperature for that trial. Calculate the average "I" value. i = (deltaTf) / (kf x...

In order to determine the molar mass of an unknown solute by measuring the freezing point...

In order to determine the molar mass of an unknown solute by measuring the freezing point depression of a solution of this unknown solute in a solvent as compared to the freezing point of the pure solvent (distilled water), we immersed a test tube with ~20ml of solute + distilled water in a ice-salt water bath, in addition to a test tube of ~20ml of pure distilled water (in a different ice-salt water bath) and recorded the temperature every 30...

Please help explain how to obtain the (i) in the van't Hoff factor. My text states...

Please help explain how to obtain the (i) in the van't Hoff factor. My text states that it is a ratio of the experimentally measured value of a colligative property to the value expected if the solute did not dissocite into ions when it dissoloved. (I don't understand that definition) Also the text provided a few examples: the value for "i" for NaCl is 2, MgSO4 is 2, CaCl2 is 3 and 4 for Na3PO4. (I don't understand how to...

A)What is the van't hoff factor for Mg3(PO4)2 in an ideal solution? B)What is the vapor...

A)What is the van't hoff factor for Mg3(PO4)2 in an ideal solution? B)What is the vapor pressure in atm of a solution at 25 oC produced by dissolving 115.4 g of dextrose (C6H12O6) in 357.4 g of water? Vapor pressure of water at 25 oC = 0.0313 atm

Molar Mass Determination by Depression of the Freezing Point A student determines the freezing point of...

Molar Mass Determination by Depression of the Freezing Point A student determines the freezing point of a solution of 0.630 g of mandelic acid in 20.78 g of tbutanol. He obtains the following temperature-time readings: Time (min) Temp (C) Time (min) Temp (C) Time (min) Temp (C) 0.0 34.9 3.0 22.3 6.0 21.8 0.5 33.3 3.5 21.4 6.5 21.7 1.0 29.7 4.0 22.3 7.0 21.6 1.5 27.1 4.5 22.2 7.5 21.5 2.0 25.2 5.0 22.1 8.0 21.3 2.5 23.6 5.5...

The formula that governs the depression of freezing point and elevation of boiling point for a...

The formula that governs the depression of freezing point and elevation of boiling point for a solution consisting of a solute dissolved in a solvent is: ΔT = i × kb × m where: ΔT = the temperature change between a pure solvent and its solution i = the number of species per mole of solute that are dissolved in the solvent (e.g., i = 1 for a non-ionic solute that does not break apart into ions; i = 2...

Describe in general terms an experiment to determine the molal freezing point depression constant of water....

Describe in general terms an experiment to determine the molal freezing point depression constant of water. assume the availablity of deionized water and solid NaNO3

How is a solution freezing point and boiling point affected by addition of a dissolved solute?

Determination of a Molar Mass by Freezing Point Depression: This experiment used Stearic Acid Experiments done...

Determination of a Molar Mass by Freezing Point Depression: This experiment used Stearic Acid Experiments done in many first-year chemistry courses. They often use cyclohexane as the solvent and compounds such as p-dichlorobenzene, biphenyl, and naphthalene as the unknown solutes. Describe the advantages of this experiment over those.

Question