Freezing point depression can be used to experimentallydetermine the van't Hoff factor of a solute in solution. Given thedata in the table, please answer the questions below and determinethe \"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 (Kf) ofwater | 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,ΔTf, of the solution?
c. What is the colligative molality,mc, of the solution?
d. How many moles of soluteparticles 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 thatexperimentally, i does not have to be an integer!)
