Practice Solubility Equilibria Of Sparingly Soluble Salts (6.13)

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6 sample questions

Question 1.
Define lattice enthalpy.
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Think about energy changes during dissolution.
Question 2.
What is Ksp?
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Look for definitions related to equilibrium constants in solubility.
3Question 3.
What does Ksp represent?
- Equilibrium constant for a gas
- Solubility product constant
- Reaction quotient
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Think of what Ksp correlates with in terms of ionic concentration.
4Question 4.
The common ion effect generally results in what change in solubility?
- True
- False
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Consider Le Chatelier's principle.
Question 5.
Calculate the solubility of a sparingly soluble salt MX given Ksp = 1.0 × 10–7.
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Use the appropriate stoichiometry based on the dissolution.
Question 6.
If the solubility of Ag2CrO4 is increased in a solution containing Li+, how will Ksp be affected?
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Reference how common ions shift equilibrium.

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