The reaction Co(H2O)6^+2 + 4Cl- <==> CoCl^-2 + 6H2O is at equilibrium. The right side is pink and the left side is blue. 1. What would happen if you added AgNO3? Would nothing happen? Or would the Ag+ react with the Cl- and shift the reaction left? 2. What would happen if acetone was added? would the solution become blue or pink at the top and why?

To determine the effect of adding AgNO3 to the reaction Co(H2O)6^+2 + 4Cl- <==> CoCl^-2 + 6H2O, we need to consider the solubility rules and the possibility of the formation of a precipitate.

1. When AgNO3 is added, Ag+ ions are introduced into the system. According to the solubility rules, AgCl is insoluble and forms a precipitate. The reaction can be represented as follows:

Ag+(aq) + Cl-(aq) → AgCl(s)

The formation of AgCl reduces the concentration of Cl- ions in the solution. According to Le Chatelier's principle, when the concentration of one reactant (Cl-) decreases, the equilibrium position shifts in the direction that produces more of the reactant, i.e., to the left side. Therefore, the addition of AgNO3 will cause the reaction to shift the equilibrium to the left, resulting in a decrease in the concentration of the pink CoCl^-2 complex and an increase in the concentration of the blue Co(H2O)6^+2 complex.

2. Acetone (CH3COCH3) is a nonpolar solvent and typically does not react with the ions or complexes in the given reaction. Acetone will primarily act as a solvent and not affect the equilibrium of the reaction. As a result, the addition of acetone is unlikely to cause a color change in the solution. The solution will likely remain blue as the dominant species in equilibrium, Co(H2O)6^+2, is present on the left side of the reaction and is blue in color.