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Chemistry / Chemistry 11 / Chapter 12 / Problem 77P

Chemistry | 11th Edition | ISBN: 9780073402680 | Authors: Raymond Chang

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Solved: The osmotic pressure of 0.010 M solutions of CaCl2

Chapter 12, Problem 77P

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QUESTION:

The osmotic pressure of 0.010 M solutions of \(\mathrm{CaCl}_{2}\) and urea at 25°C are 0.605 atm and 0.245 atm, respectively. Calculate the van’t Hoff factor for the \(\mathrm{CaCl}_{2}\) solution.

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QUESTION:

The osmotic pressure of 0.010 M solutions of \(\mathrm{CaCl}_{2}\) and urea at 25°C are 0.605 atm and 0.245 atm, respectively. Calculate the van’t Hoff factor for the \(\mathrm{CaCl}_{2}\) solution.

ANSWER:

Step 1 of 2

The van't Hoff factor (i) is a measure of the degree of dissociation of a compound in solution, and is defined as the ratio of the number of particles in solution to the number of entities (such as molecules) in the original substance.

The osmotic pressure of a solution is the pressure required to stop osmosis.

The osmotic pressure of a solution is given by

where is the molarity of solution, is the gas constant . atm/ , and is the absolute temperature.

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