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Properties of Solutions

Properties of Solutions. Essential Questions. What factors affect the solubility of solutions?. Review. Solute: Solvent: Solution. Review. Solute: one being dissolved Solvent: one doing the dissolving Solution: the solute and the solvent put together. Factors Affecting Solubility.

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Properties of Solutions

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  1. Properties of Solutions

  2. Essential Questions • What factors affect the solubility of solutions?

  3. Review • Solute: • Solvent: • Solution

  4. Review • Solute: one being dissolved • Solvent: one doing the dissolving • Solution: the solute and the solvent put together

  5. Factors Affecting Solubility • Nature of the Solvent • Polarity: “like dissolves like” • Polar with polar, Nonpolar with nonpolar • Pressure • Gas solutes only: increasing pressure will increase solubility • Carbonated beverages

  6. Factors Affecting Solubility Cont. • Temperature • Solids & Liquids: increasing temp. will almost always increase solubility • Gases: increased temp will decrease solubility

  7. Rate of Solution • Make a hypothesis as to which will dissolve faster, a sugar cube or granulated sugar. The amount of sugar is equivalent in each. Provide an explanation for your hypothesis.

  8. Factors Affecting Rate of Solution • Size of Particle • Increased surface area (smaller particles) allows greater contact with solvent • Amount of solute already dissolved • higher conc. slower rate

  9. Factors Affecting Rate of Solution Cont. • Temperature • Solids and Liquids: Increased temp. increases rate of solution • For Gases: Increased temp. decreases rate of solution • Stirring

  10. Types of solutions • Unsaturated: • Saturated: • Supersaturated:

  11. Types of solutions • Unsaturated: solute has not reached the saturation point yet (More solute can be added) • Saturated: saturation point has been reached, but no excess solute appears. • Supersaturated: Too much solute is present than can be dissolved. Excess solute is present.

  12. Think! • What would happen if you added more solute to a saturated solution?

  13. Solubility Curve

  14. Practice Problems • Use the solubility chart on the slide above to answer the following. • What amount of NaCl is needed to make a saturated solution at 80oC? 2. What type of solution exists when 90g KNO3 is dissolved at 40oC?

  15. Think: • What would happen if you added more solute to a saturated solution?

  16. Solute Types • Electrolytes • Non-electrolytes

  17. Types of Solutes • Electrolytes • Break apart into ions in solution • Number of ions = Subscript total • Conduct electricity • Example: NaCl in solution

  18. Types of Solutes Cont. • Non-electrolytes • Stay whole in solution • Do not conduct electricity • Example: CO2

  19. Types of Solutes Cont. • Type of solute affects the total # of solute particles in solution • Ex: If one had equal concentrations of KBr, an electrolyte and C6H12O6, a nonelectrolyte in solution, there would be more particles in the KBr solution.

  20. Examples • Determine the number of particles in the following: • NaCl, an electrolyte • NO2, a non-electrolyte • CH4, a non-electrolyte • CaCl2, an electrolyte

  21. ESSENTIAL QUESTION • How “strong” is that solution? • Think-ink-share…. • What is this lesson about? What do we mean by a solution being strong? • Give me a synonym for the word “strong” as it is meant in the EQ.

  22. Concentration • Measured in molarity • Think…. How is concentration measured? http://www.youtube.com/watch?v=tXG0PACMUOo The more you add… the more concentrated. The less volume you have, the more concentrated.

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