Chemical Equilibrium
1
Solubility Product Principle
• Another equilibrium situation is slightly soluble
products
• Ksp is the solubility product constant
• Ksp can be found on a chart at a specific
temperature
• Since the product is solid on the left side, only
the products (ions) are involved in the Ksp
expression
2
Solubility Product Principle
3
Solubility Product Principle
• Example: Find the concentration of ions present in
calcium fluoride (in water) and the molar solubility.
CaF2(s) --> Ca+2 + 2 FKsp = [Ca+2] [F-]2 = 2 X 10 -10
If x = [Ca+2 ], then [F-] = 2x
[x] [2x]2 = 2 X 10 -10
4x3 = 2 X 10 -10
x3 = 5 X 10 -11
x = 3.68 X 10 -4
[Ca+2 ] = x = 3.68 X 10 -4
[F-] = 2x = 7.37 X 10 -4
Solubility of CaF2 = 3.68 X 10 -4
4
Solubility Product Principle
• Example: Find the molar solubility of silver
chloride (in water).
AgCl (s) --> Ag+ + Cl -
5
Predicting Precipitate Reactions
• When 25 ml of 0.010 mol/L silver nitrate is
mixed with 25.0 mL of 0.0050 mol/L of
potassium chloride, will a precipitate form.
6
Le Chatalier’s Principle and Solubility
• How does the solubility
of ionic compounds
change when the
temperature increases?
• How does Ksp change?
7
Common Ion Effect.
• How does the addition of NaCl effect the
solubility of Lead Chloride?
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Questions
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Q 1-4 p 486
Q 5-6 p 489
Q 7-12 p 492
Q 1-13 p 493
• Review Titration Techniques
• Prepare Self Design Lab Investigation 7.6.2
To Determine the Ksp of calcium hydroxide.
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