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Solutions

Learn about factors influencing solubility, types of solutions, dissolution rates, and the impact of temperature and pressure on solubility equilibrium. Explore solute-solvent interactions and the heat of solution concept.

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Solutions

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  1. Solutions The Solution Process

  2. Objectives • Describe the factors that affect solubility and the rate at which the solute dissolves. • Distinguish between saturated, unsaturated, and supersaturated solutions.

  3. Factors Affecting the Rate of Dissolution • Surface area • Stirring • temperature

  4. Solubility

  5. Solubility Solution equilibrium – state in which dissolution and crystallization of a solute occur at equal rates Saturated solution – a solution that contains the maximum amount of dissolved solute Unsaturated solution – a solution that contains less solute than the maximum that can be dissolved under the existing conditions. Supersaturated solution – a solution that contains more dissolved solute than a saturated solution under the same conditions.

  6. Solubility Values Solubility – amount of a solute that forms a saturated solution in a given amount of solvent at a specific temperature • Pressure must be specified for gases Examples: solubility in 100 g of H2O at 20oC NaCl: 35.9 g O2: 0.00537 g at 1 atm

  7. Objectives • Describe the factors that affect solubility. • Describe the interactions that contribute to the heat of solution.

  8. Solute-Solvent Interactions “Like dissolves Like”

  9. Ionic Compounds in Aqueous Solutions Hydration – process in which water molecules are attracted to ions in solution.

  10. Liquid Solutes and Solvents Immiscible – when liquid solutes and solvents are not soluble in each other Miscible – when liquids dissolve freely in one another.

  11. Effects of Pressure Gas + solvent ↔ solution

  12. Henry’s Law • The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid

  13. Effect of Temperature on Solubility

  14. Heat of Solution • The net amount of energy released or absorbed when a specific amount of solute dissolves in a solvent. -can be exothermic or endothermic

  15. Heat of Solution The heat of solution is the sum of the following energy changes. • Solute particles must be separated. Energy is required (lattice energy) • Solvent particles must be separated. Energy is required (intermolecular forces) • Solute particles are attracted to solvent particles (solvation) Energy is released.

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