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Colligative Properties

Colligative properties are vital in chemistry, depending solely on the number of solute particles rather than their identity. This overview covers vapor pressure, freezing point depression, boiling point elevation, and osmotic pressure. Vapor pressure decreases with solute addition, in line with Raoult's law. Freezing and boiling point changes are calculated using the van't Hoff factor and specific constants. Additionally, osmotic pressure describes the minimum force needed to prevent osmosis. This knowledge aids in numerous scientific and industrial applications.

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Colligative Properties

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  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

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