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2 cards from this section. Quick, good the night before a test.
What does Ksp represent for a sparingly soluble salt?
Think about how Ksp relates to solubility.
Define common ion effect.
Consider what happens to equilibrium when more of a specific ion is present.
What is the solubility product constant?
Remember the context of saturated solutions.
True or False: Increasing the concentration of a common ion decreases the solubility of a sparingly soluble salt.
Consider how equilibrium shifts with added ions.
If Ksp for AgBr is 5.0 × 10–13, calculate the solubility of AgBr in water.
Remember to define the Ksp expression first.
Assess how adding NaCl affects the solubility of AgCl, given Ksp = 1.77 × 10–10.
Utilize Le Chatelier’s principle in your response.
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