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Ch.17 - Applications of Aqueous Equilibria
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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Related Practice
Textbook Question
The following pictures represent solutions at various stages in the titration of a weak diprotic acid H2A with aqueous NaOH. (Na+ ions and water molecules have been omitted for clarity.)

.(b) Which solution has the highest pH? Which has the lowest pH?
Textbook Question

The following pictures represent solutions at various stages in the titration of sulfuric acid H2A (A2- = SO4 2-) with aqueous NaOH. (Na+ ions and water molecules have been omitted for clarity.)

. (a) To which of the following stages do solutions 1–4 correspond? (i) Halfway to the first equivalence point (ii) Halfway between the first and second equivalence points (iii) At the second equivalence point (iv) Beyond the second equivalence point

Textbook Question

The following pictures represent solutions at various stages in the titration of sulfuric acid H2A (A2- = SO4 2-) with aqueous NaOH. (Na+ ions and water molecules have been omitted for clarity.)

. (b) Which solution has the highest pH? Draw a picture that represents the solution prior to addition of any NaOH.

Textbook Question
Is the pH greater than, equal to, or less than 7 after the neutralization of each of the following pairs of acids and bases?(c) HBr and aniline (C6H5NH2)
Textbook Question

Is the pH greater than, equal to, or less than 7 after the neutralization of each of the following pairs of acids and bases? (a) NaOH and benzoic acid (C6H5CO2H)