Successfully reported this slideshow.
We use your LinkedIn profile and activity data to personalize ads and to show you more relevant ads. You can change your ad preferences anytime.

Chapter 14.2 : Colligative Properties

7,475 views

Published on

Published in: Education
  • Be the first to comment

Chapter 14.2 : Colligative Properties

  1. 1. Colligative Properties of solutions<br />Chapter 14.2<br />
  2. 2. Objectives:<br />List four colligative properties, and explain why they are classified as colligative properties.<br />Calculate freezing-point depression, boiling-point elevation, and solution molality of nonelectrolytic solutions.<br />Calculate the expected changes in freezing point and boiling point of an electrolytic solution.<br />Discuss causes of the differences between expected and experimentally observed colligative properties of electrolytic solutions.<br />
  3. 3. Colligative Properties of Solutions<br />Properties that depend on the concentration of solute particles but not on their identity.<br />Examples<br />Vapor-pressure lowering<br />Freezing-point depression<br />Boiling-point elevation<br />
  4. 4. Vapor-Pressure Lowering<br />Nonvolatile solute raises boiling point and lowers freezing point of solution<br />Nonvolatile substance : one that has little tendency to become a gas under existing conditions<br />Look at figures 14.6 and 7 on page 436 & 437<br />Solute molecules crowd surface of solution, lowering tendency of water molecules to escape to liquid phase.<br />
  5. 5. Freezing-point depression<br /> tf , is the difference between the freezing points of the pure solvent and a solution of a nonelectrolyte in that solvent, and it is directly proportional to the molal concentration of the solution.<br />Molal freezing-point constant(Kf)<br />The freezing-point depression of the solvent in a 1-molal solution of a nonvolatile, nonelectrolytic solute<br /> tf=Kfm<br />
  6. 6. Boiling-point Elevation<br />tb, is the difference between the boiling points of the pure solvent and a solution of a nonelectrolyte in that solvent, and it is directly proportional to the molal concentration of the solution.<br />Molal boiling-point constant(Kb)<br />The freezing-point depression of the solvent in a 1-molal solution of a nonvolatile, nonelectrolytic solute<br />tb=Kbm<br />
  7. 7. Osmotic Pressure<br />Semipermeable Membranes<br />Allow the movement of some particles while blocking the movement of others<br />Osmosis<br />The movement of solvent through a semipermeable membrane from the side of lower solute concentration to the side of higher solute concentration<br />Osmotic Pressure<br />External pressure that must be applied to stop osmosis<br />Life Processes<br />Cell membranes are semipermeable <br />Shrink when placed in solution of higher concentration<br />
  8. 8. Electrolytes and Colligative Properties<br />Electrolytes in solution enhance the Colligative properties.<br />Because they break up into ions<br />Example: 0.1m NaCl will double the amount the freezing point lower than a nonelectrolyte<br />0.1 m CaCl2 solution will triple the amount the boiling point elevates than a nonelectrolyte. <br />Why? More particles are produced<br />NaCl (s) Na+ (aq) + Cl- (aq)<br />CaCl2 (s) Ca2+(aq) + 2 Cl- (aq)<br />2 total moles produced<br />1 mol<br />1 mol<br />1 mol<br />3 total moles produced<br />2 mol<br />1 mol<br />1 mol<br />

×