When silver chloride and silver iodide are added to water, equilibria are set up. $\text{AgCl}(s) \rightleftharpoons \text{Ag}^+(aq) + \text{Cl}^-(aq) \quad K_c = K_1$ $\text{AgI}(s) \rightleftharpoons \text{Ag}^+(aq) + \text{I}^-(aq) \quad K_c = K_2$ The equilibrium position for each of these lies far to the left. Silver iodide does not dissolve in aqueous ammonia, but silver chloride does dissolve in aqueous ammonia. A further equilibrium is established. $\text{Ag}^+(aq) + 2\text{NH}_3(aq) \rightleftharpoons \text{Ag(NH}_3\text{)}_2^+(aq) \quad K_c = K_3$ This equilibrium position lies to the right. What order of magnitude do these three equilibrium constants have?
- A$K_1 > K_2 > K_3$
- B$K_2 > K_1 > K_3$
- C$K_3 > K_1 > K_2$
- D$K_3 > K_2 > K_1$