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13.3 solubility
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  • 1. SOLUBILITY 13.3
  • 2. IONIC COMPOUNDS
    • When ionic compounds dissolve in water they:
      • Break down into single molecules.
      • Break down into their ions.
    Na Cl water Na Cl + - this is called dissociation
  • 3. Dissociation
    • This occurs because ions have charged particles.
      • water is polar
      • it has a + and - pole
    + -
  • 4. POLARITY
    • Water is polar because it has a positive and a negative side.
    • Some substances are nonpolar.
      • no charges or poles
      • example: oil
  • 5. LIKES DISSOLVE LIKES POLAR DISSOLVES IN POLAR NONPOLAR DISSOLVES IN NONPOLAR
  • 6. Solubility
    • How much of a substance will dissolve in a given amount of water.
    • Will it dissolve?
    • SOLUBLE: substance will dissolve .
    • INSOLUBLE: substance will not dissolve.
  • 7. States of Solubility
      • Unsaturated: When a solvent holds less solute than it normally could at a given temperature.
      • Saturated: When a solvent holds as much solute as it normally could at a given temperature.
      • Supersaturated: When a solvent is holding more solute than it would at a given temperature.
  • 8. SOLIDS VS. GASES
    • Solids
      • solubility increases as temp. increases
      • solubility decreases as temp. decreases
    • Gases
      • solubility increases as temp. decreases
      • solubility decreases as temp. increases
  • 9. Reading a Solubility Curve: Above line = supersaturated On the line = saturated Below the line = unsaturated
  • 10. KCl To make a saturated solution of KCl at 60ºC, how much would I add to 100 ml of water? 46g
  • 11. KNO 3 At what temperature will 80g of KNO 3 dissolve in 100ml of water to make a saturated solution? 48ºC
  • 12. NH 4 Cl What kind of a solution would 75g of NH 4 Cl dissolved in 100 ml of water at 55ºC be? Point falls above the line supersaturated