Freezing point depression can be used to experimentally determine the van \'t Ho

Question

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.

Mass of solvent (water) 7.973 g Freezing point of water 0.00 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. What mass of solute was used? What is the freezing point depression ?Tf of the solution? What is the colligative molality mc of the solution? How many moles of solute particles are present in solution? If the solute has a molar mass of 137.37, what is the van 't Hoff factor i for the solute? (Remember that experimentally, i does not have to be an integer.)

Explanation / Answer

a) mass of solute = Mass of solution - Mass of solvent (water) = 8.757 g - 7.973g = 0.784 g

b)the freezing point depression ?Tf of the solution = Freezing point of water - Freezing point of solution= 0.00

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.