CHEM 211 1st Edition Lecture 7Outline of Last Lecture I. Solutions and ColloidsII. Solutions and SolubilityIII. Solutions and Intermolecular ForcesIV. Dual Polarity and Effects on SolubilityV. Heats of Solution and Solution CyclesVI. Heat of SolutionVII. Solvation and HydrationOutline of Current Lecture I. Solutions and EntropyII. Solubility and EquilibriumIII. Factors that Affect SolubilityIV. Henry’s LawCurrent LectureI. Solutions and EntropyA. The entropy of a system is related to the number of ways a system can disperse its energy and therefore to the freedom of motion of the particles.B. Gases have the highest entropy of the three states of matter.C. A solution usually has higher entropy than the pure solute and pure solvent.D. An increase in entropy is favored in both physical and chemical processes.E. For octane, ∆Hsoln is very small, but the entropyincrease due to mixing is large, so octane dissolves.II. Solubility and EquilibriumA. A saturated solution contains the maximumamount of dissolved solute at a given temperaturein the presence of undissolved solute.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.B. Undissolved solute is in equilibrium with dissolved soluteC. Solute (undissolved)> solute (dissolved)D. An unsaturated solution contains less than the equilibrium concentration of dissolved solute. If more solute is added, it will dissolve.III. Factors that affect SolubilityA. Temperature affects solubility.B. Most solids are more soluble at higher temperatures.C. Gases become less soluble as temperature increases.D. Pressure affects the solubility of gases – they become more soluble at higher pressure.IV. Henry’s LawA. The solubility of a gas (Sgas) is directly proportional to the partial pressure of the gas (Pgas) above the solution.a) Sgas = kHX
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