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Ch.17 - Applications of Aqueous Equilibria
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook
All textbooksMcMurry 8th EditionCh.17 - Applications of Aqueous EquilibriaProblem 46
Chapter 17, Problem 46

The following pictures represent solutions of Ag2CrO4, which also may contain ions other than Ag+ and CrO42- that are not shown. Solution 1 is in equilibrium with solid Ag2CrO4. Will a precipitate of solid Ag2CrO4 form in solutions 2-4? Explain.
Illustration of Ag2CrO4 ions in solution, relevant to precipitation equilibrium.
(1) (2) (3) (4)

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1
Identify the ions present in each solution. In the image, the red circles represent Ag+ ions and the purple circles represent CrO4^2- ions.
Determine the concentration of Ag+ and CrO4^2- ions in each solution. Count the number of each type of ion in solutions 2, 3, and 4.
Compare the ion product (Q) of Ag+ and CrO4^2- in each solution to the solubility product constant (Ksp) of Ag2CrO4. The ion product is calculated as Q = [Ag+]^2[CrO4^2-].
If Q > Ksp, a precipitate will form because the solution is supersaturated. If Q < Ksp, no precipitate will form because the solution is unsaturated. If Q = Ksp, the solution is at equilibrium and no additional precipitate will form.
Analyze the results for each solution (2, 3, and 4) to determine if a precipitate of Ag2CrO4 will form by comparing their Q values to the Ksp value.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is a numerical value that represents the equilibrium between a solid and its ions in a saturated solution. For Ag2CrO4, Ksp can be used to determine whether a precipitate will form in a solution by comparing the product of the concentrations of the ions (Ag+ and CrO42-) to Ksp. If the product exceeds Ksp, a precipitate will form.
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Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed, the system will adjust to counteract the disturbance and restore a new equilibrium. In the context of the Ag2CrO4 solutions, adding more ions or changing conditions can shift the equilibrium, potentially leading to the formation of a precipitate if the conditions favor solid formation.
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Precipitation Reaction

A precipitation reaction occurs when two soluble salts react in solution to form an insoluble solid, known as a precipitate. In the case of Ag2CrO4, if the concentrations of Ag+ and CrO42- ions in solutions 2-4 exceed the Ksp value, a precipitate of Ag2CrO4 will form, indicating that the solution is supersaturated with respect to this compound.
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