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Ch.7 Energy, Rate and EquilibriumWorksheetSee all chapters
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Nature of Energy
First Law of Thermodynamics
Endothermic & Exothermic Reactions
Bond Energy
Thermochemical Equations
Heat Capacity
Thermal Equilibrium (Simplified)
Hess's Law
Rate of Reaction
Energy Diagrams
Chemical Equilibrium
The Equilibrium Constant
Le Chatelier's Principle
Solubility Product Constant (Ksp)
Spontaneous Reaction
Entropy (Simplified)
Gibbs Free Energy (Simplified)

Solubility Product Constant (Ksp) is associated with any ionic compound, which measures how soluble the compound will be in a solvent.


Concept #1: Solubility Product Constant (Ksp)

Example #1: Which substance is the most soluble? 

a) AgCl Ksp = 1.6 x 10-10

b) MgCO3 Ksp = 3.5 x 10-8

c) CaSO4 Ksp = 7.1 x 10-5

d) CuS  Ksp = 8.5 x 10-45

Concept #2: Equilibrium Expressions

Example #2: Provide the equilibrium expression for calcium nitrate, Ca(NO3)2.

Concept #3: Calculating Ksp from Solubility

Concept #4: Calculating Solubility from Ksp

Practice: Determine the equilibrium expression of the barium nitride solid.

Practice: Manganese (V) hydroxide has a measured solubility of 3.4×10–5 M at 25ºC. Calculate its Ksp value.

Practice: The Ksp value for strontium fluoride, SrF2, is 7.9×10–10 at 25ºC. Calculate its solubility in g/L.