If the osmotic pressure of a 8.88×10-2-M aqueous solution of CaCl2 was found to be 5.77 atm at 20°C, what would be the "observed" van't Hoff factor? 2.70 . Use the above van't Hoff factor to predict the freezing point of this solution. Note that the corresponding molality would be 9.00×10-2 m, given that the density of the solution is 0.997 g/cm3. -4.52×10-1 °C question is Use the above van't Hoff factor to predict by how many degrees the boiling point of this solution will be elevated above that for pure water.
If the osmotic pressure of a 8.88×10-2-M aqueous solution of CaCl2 was found to be 5.77 atm at 20°C, what would be the "observed" van't Hoff factor? 2.70 . Use the above van't Hoff factor to predict the freezing point of this solution. Note that the corresponding molality would be 9.00×10-2 m, given that the density of the solution is 0.997 g/cm3. -4.52×10-1 °C question is Use the above van't Hoff factor to predict by how many degrees the boiling point of this solution will be elevated above that for pure water.
Chemistry
10th Edition
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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If the osmotic pressure of a 8.88×10-2-M aqueous solution of CaCl2 was found to be 5.77 atm at 20°C, what would be the "observed" van't Hoff factor? 2.70 . Use the above van't Hoff factor to predict the freezing point of this solution. Note that the corresponding molality would be 9.00×10-2 m, given that the density of the solution is 0.997 g/cm3. -4.52×10-1 °C
question is Use the above van't Hoff factor to predict by how many degrees the boiling point of this solution will be elevated above that for pure water.
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