Slideshare uses cookies to improve functionality and performance, and to provide you with relevant advertising. If you continue browsing the site, you agree to the use of cookies on this website. See our User Agreement and Privacy Policy.

Slideshare uses cookies to improve functionality and performance, and to provide you with relevant advertising. If you continue browsing the site, you agree to the use of cookies on this website. See our Privacy Policy and User Agreement for details.

Like this presentation? Why not share!

- Colligative properties by dirksr 2839 views
- Solutions and colligative properties by Jill Dodson 1630 views
- colligative property ,made by-chin... by CHINMAY JAGADEV 2069 views
- Chapter 14.2 : Colligative Properties by Chris Foltz 6474 views
- 3- Solutions & It's Colligative Pro... by Rawa M. Ahmed 940 views
- Chapter 13 Lecture on Solutions & C... by Mary Beth Smith 15704 views

20,647 views

Published on

No Downloads

Total views

20,647

On SlideShare

0

From Embeds

0

Number of Embeds

62

Shares

0

Downloads

377

Comments

1

Likes

12

No embeds

No notes for slide

- 1. Colligative Properties of Solutions<br />
- 2. The presence of solutes affects the properties of solutions.<br />Some of these properties are not dependant on what dissolved substance but only on how much.<br />Colligative properties are those that depend on the concentration of solute particles but not on their identity.<br />Colligative Properties? What the…<br />
- 3. Vapor pressure is the pressure caused by molecules that have escaped from the liquid phase to the gaseous phase.<br />Experiments show that the vapor pressure of a solvent containing a nonvolatile* solute is lower than the vapor pressure of the pure solvent at the same temp.<br />This lowers the freezing point and raises the boiling point.<br />*a substance with little tendency to become a gas<br />Vapor Pressure<br />
- 4. Phase Diagram<br />
- 5. Pure Solvent v. Solution<br />
- 6. Freezing Point Depression<br />The freezing point of a 1-molal solution of a nonelectrolyte solute in water is found by experiment to be 1.86°C lower than the freezing point of water.<br />When the solution is 2-molal the freezing point is lowered by 3.72°C.<br />In fact, for any concentration of a nonelectrolyte solute in water, the decrease in freezing point can be determined using the value of -1.86°C/m.<br />This value is called the molal freezing-point, Δtf<br />
- 7. Freezing-point depression can be calculated by using the following equation.<br />Δtf= Kfm<br />Kfis the freezing-point depression constant.<br />m is the molality.<br />Each solvent has its own characteristic molal freezing-point constant. See Table 14-2 on page 438.<br />
- 8. What is the freezing-point depression of water in a solution of 17.1 g of sucrose, C12H22O11, and 200. g of water? What is the actual freezing point of this solution?<br />Sample Problem 14-3<br />
- 9. A water solution containing an unknown quantity of a nonelectrolyte solute is found to have a freezing point of -0.23°C. What is the molal concentration of the solution?<br />Sample Problem 14-4<br />
- 10. Page 449 Questions 19-24<br />Assignment <br />

No public clipboards found for this slide

×
### Save the most important slides with Clipping

Clipping is a handy way to collect and organize the most important slides from a presentation. You can keep your great finds in clipboards organized around topics.

0.465 :)