Multiple Choice
Determine the minimum concentration of NaF required to cause precipitation of BaF₂ from a 4.0×10⁻² M Ba(NO₃)₂ solution, given that the Ksp of BaF₂ is 1.7×10⁻⁶.
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18. Aqueous Equilibrium
Precipitation: Ksp vs Q
Multiple Choice
Under what condition will a precipitate form in a solution when comparing the ion product (Q) to the solubility product constant (Ksp)?
A
Q = 0
B
Q > Ksp
C
Q < Ksp
D
Q = Ksp
Verified step by step guidance1
Understand the concept of solubility product constant (Ksp): Ksp is the equilibrium constant for the dissolution of a sparingly soluble ionic compound. It represents the maximum concentration of ions in a saturated solution.
Define the ion product (Q): Q is the product of the concentrations of the ions in the solution at any given moment, not necessarily at equilibrium.
Compare Q and Ksp to determine the formation of a precipitate: If Q > Ksp, the solution is supersaturated, and a precipitate will form as the excess ions combine to form the solid compound.
Consider the condition Q = Ksp: This indicates that the solution is at equilibrium, and no precipitate will form because the solution is saturated.
Evaluate the condition Q < Ksp: In this case, the solution is unsaturated, meaning more solute can dissolve, and no precipitate will form.
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