1 / 7

Colligative Properties

Colligative Properties. Colligative Properties properties that depend only on the number of solute particles, not on the nature of the particles. Vapor pressure Freezing point depression Boiling point elevation Osmotic pressure.

najwa
Télécharger la présentation

Colligative Properties

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Colligative Properties

  2. Colligative Propertiesproperties that depend only on the number of solute particles, not on the nature of the particles Vapor pressure Freezing point depression Boiling point elevation Osmotic pressure

  3. Vapor PressureThe pressure of the vapor over a liquid at equilibrium • Vapor pressure of pure solvent is always lowered by the addition of solute • Lowering is proportional to mole fraction of solute Raoult’s law (nonvolatile solvent) Psoln = XsolventPosolvent Psoln = observed vapor pressure Xsolvent = mole fraction of solvent Posolvent = vapor pressure of pure solvent

  4. van’t Hoff factor Number of ions/ formula unit NaCl i = 2 MgCl2i = 3 CaSO4i = 2

  5. Freezing point depression DTf = iKfm i = number of moles of particles in solution (van’t Hoff value) Kf = molal freezing point depression constant; particular to the solvent m = concentration in molality

  6. Boiling point elevation DTb = iKbm i = number of moles of particles in solution (van’t Hoff value) Kb = molal boiling point depression constant; particular to the solvent m = concentration in molality

  7. Osmotic pressureexcess pressure on solution or minimum pressure that stops osmosis p= MRT M = molarity R = gas law constant, 0.0821 atm L/mol K T = temperature, kelvins

More Related