The reaction Co(H2O)6^+2 + 4Cl- <==> CoCl^-2 + 6H2O is at equilibrium. The left side is pink and the right 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?

The A part is the latter; i.e., Ag^+ will combine with Cl^- to form AgCl which will shift the equilibrium to the left. Is the equilibrium you cite in acetone to begin with, in water, or in some other solvent?

To DrBob222 - it starts as an aqueous solution, with acetone then added.

To determine the effect of adding AgNO3 and acetone on the given equilibrium reaction, we need to consider the potential reactions that could occur.

1. AgNO3:
When AgNO3 is added, it dissociates into Ag+ and NO3-. The Ag+ ions have the potential to react with Cl- ions in solution, forming AgCl precipitate according to the equation: Ag+ + Cl- → AgCl. This reaction consumes Cl- ions and reduces their concentration in the solution. As a result, the equilibrium will shift to the left to compensate for the decrease in Cl- concentration. Since the left side of the equilibrium reaction is pink, shifting the reaction left would favor the formation of more pink Co(H2O)6^+2 ions.

2. Acetone:
Acetone is a polar organic solvent that can potentially solvate ions. However, since the equilibrium reaction involves aqueous species, the addition of acetone would not have a direct effect on the reaction itself. Acetone is immiscible with water, so it would form a separate layer on top of the aqueous solution. Since it does not directly participate in the equilibrium reaction, it will not shift the reaction left or right.

Therefore, the addition of AgNO3 would shift the equilibrium reaction to the left, favoring the formation of more pink Co(H2O)6^+2 ions. On the other hand, the addition of acetone would not cause any noticeable changes in the color or composition of the solution, as it would remain separate from the aqueous solution.