CHEM 122 11th Edition Lecture 12 Outline of Last LectureI. Solubilitya. Saturated solutionb. Supersaturated solutionII. Solubility of two liquidsIII. Solubility of Gases in LiquidsOutline of Current Lecture I. Temperature Effects on Gas SolubilityII. Colligative Properties of Solutionsa. Lower vapor pressureb. Higher boiling pointCurrent LectureTemperature effects on gas solubility:- Solubility of a gas in a liquid decreases with increasing temperature.- Why is gas solubility reduced with increasing temperature?o As temperature increases, average kinetic energy increases, more dissolved gas molecules can overcome intermolecular forces of the liquid molecules, therefore increasing their chance to escape the liquid.Colligative Properties of Solutions: physical properties of solutions that depend only on the concentration of solute particles; not on the chemical identity of the particles.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best Used as a supplement to your own notes, not as a substitute.- Vapor Pressure: pressure exerted by the vapor when the liquid and vapor state is in equilibrium, only happened in a closed container.o Nonvolatile: Particle that doesn’t have a vapor pressure, all ions are nonvolatile.o What happens to vapor pressure in a solution? Molecules must be at the surface to vaporize. For a solution only the solvent can vaporize and some of the solute particles are at the surface. This reduces the number of solvent molecules at the surface and therefore reduces the rate of evaporation. Solute particles interfere with evaporation but the rate of condensation isn’t affected.o Raoult’s Law: Gives the vapor pressure of a solution containing nonvolatile solute.oPsoln=XsolventPsolventoPsoln: Vapor pressure of the solutionXsolvent: Mole fraction of the solventPsolvento: Vapor pressure of pure solvento Vapor Pressure lowering Equation:o∆ P= XsolutePsolvento=PsolventoPsolution o Total vapor pressure of the solution:oPtotal=XAPAo+ XBPBo- Boiling Point Elevation: the boiling point of solution with nonvolatile solutes is higher than that of the pure solvent.o Equation for boiling-point-elevation: ∆ Tb=Kb∗m o∆ Tb: Boiling point increase (∆ C❑o)oKb: Boiling-point-elevation constant (C❑o/ m ¿om: molality of the solute
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