Properties of Solutions

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Properties of Solutions

• Chapter 16.1

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Learning Objectives?

• What solubility is and how it is determined
• Recognize various levels of saturation and its
  relationship to solutions
• Miscible vs Immiscible
• Factors that affect solubility, with special
  attention to temp.
• Henrys Law

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What is solubility?

• Solubility refers to how much of a solute can be
  dissolved in solvent
• Solubility is often expressed in grams of solute
  per 100 g of solvent (usually data tables are at
  temp. 25oC)

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Types of Solutions
A saturated solution contains the maximum amount
of a solute that will dissolve in a given solvent
at a specific temperature. (i.e. 36.2 grams of
NaCl dissolved in a 100 g water)
An unsaturated solution contains less solute than
the solvent has the capacity to dissolve at a
specific temperature.
An heterogeneous mixture is where you add so much
solute to the solvent that it crashes out. You
can visibly see solvent.
A supersaturated solution contains more solute
than is present in a saturated solution at a
specific temperature.
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Miscible vs. Immiscible

• Two liquids are miscible if they dissolve in each
  other in all proportions (antifreeze)
• Two liquids are immiscible if they separate into
  two phases (oil and water)
• Liquids that are slightly soluble in each other
  partially miscible (ether and H2O)

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What affects solubility?

• Factors that affect solubility
• Surface Area of solute
• Agitation
• Temperature
• Pressure (for gases in aqueous solutions)

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How does temperature affect solubility?

• Increased kinetic energy causes an increase in
  particle collisions
• Solubility of most solids increases with increase
  in solvent temperature
• Solubility of gases decreases with an increase in
  solvent temperature

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How does pressure affect gas solubility?

• Gas solubility increases as the pressure of the
  gas increases
• Henrys Law

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Homework for 16.1
Page 477 3, 6 Page 499 42, 43, 44, 48, 49
Page 500 71, 79