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13.3 solubility
 

13.3 solubility

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    13.3 solubility 13.3 solubility Presentation Transcript

    • SOLUBILITY 13.3
    • 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
    • Dissociation
      • This occurs because ions have charged particles.
        • water is polar
        • it has a + and - pole
      + -
    • POLARITY
      • Water is polar because it has a positive and a negative side.
      • Some substances are nonpolar.
        • no charges or poles
        • example: oil
    • LIKES DISSOLVE LIKES POLAR DISSOLVES IN POLAR NONPOLAR DISSOLVES IN NONPOLAR
    • 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.
    • 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.
    • 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
    • Reading a Solubility Curve: Above line = supersaturated On the line = saturated Below the line = unsaturated
    • KCl To make a saturated solution of KCl at 60ºC, how much would I add to 100 ml of water? 46g
    • KNO 3 At what temperature will 80g of KNO 3 dissolve in 100ml of water to make a saturated solution? 48ºC
    • 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