Chapter 3 – Section 1 Quiz by dffhrtcv3


									 Book L
 Chapter 3
 Section 2
             The Universal Solvent
   Water is often described as the “Universal
    Solvent” because it can dissolve so many
    different solutes
       Solutions where water is the solvent are called
                  Why Water???
   Water is the “Universal Solvent” because of
    the polar covalent bonds that holds it
       Creates a “+” and a “-” end
        Water and Ionic Compounds
   When an ionic compound is placed in
    water, the water molecules are attracted to
    the “+” and “–” ions of the compound.
       “+” ends of water molecule surround “–” ions and
        vice versa. Compound “breaks up”
    Water and Covalent Compounds
   When a substance with covalent bonds is
    placed into water, water “gets between” the
       The substance stay together but is attracted to
        the water molecule.
               Rules of Solubility
   “Like dissolves like”
       Polar dissolves polar (sugar-water)
       Non polar dissolves non polar
   Polar and Non polar substances will not
    dissolve in one another.
       Oil / Water
   Solubility is a measure of the amount of
    solute that will dissolve in a given amount
    of solvent.
       Measured as:
        _?_ g of _(solute)_ in 100g of _(solvent)_ at 25º

       Potassium Chromate (high – 63g)
       Barium Sulfate (low - .00025g)
              Temperature Effects
   An increase in temperature:
       Causes more of a solid to dissolve in a liquid
       Causes less of a gas to dissolve in a liquid
                Saturation Point
   When a solution is holding as much solute
    as it possibly can, it is saturated
       Also: Saturation Point
       Changes with temperature
   Concentration is usually measured as a
    percent per unit volume.
       15g / 100mL(15%) OR 25g / 200mL (12.5%)
       Read as solute per solvent

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