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.

(1) (2) (3) (4)

Verified step by step guidance

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.
2. 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.
3. 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-].
4. 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.
5. 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.