Silver chloride and silver iodide establish equilibria when they are placed in water. $\text{AgCl}(s) \rightleftharpoons \text{Ag}^+(aq) + \text{Cl}^-(aq)\qquad K_c = K_1$ $\text{AgI}(s) \rightleftharpoons \text{Ag}^+(aq) + \text{I}^-(aq)\qquad K_c = K_2$ For each case, the equilibrium position is far to the left. Silver iodide does not dissolve in aqueous ammonia. Silver chloride does dissolve in aqueous ammonia. A further equilibrium is established. $\text{Ag}^+(aq) + 2\text{NH}_3(aq) \rightleftharpoons \text{Ag(NH}_3)_2^+(aq)\qquad K_c = K_3$ This equilibrium lies to the right. What is the order of magnitude of these three equilibrium constants?
- Asmallest $K_3$ → $K_2$ → largest $K_1$
- Bsmallest $K_3$ → $K_1$ → largest $K_2$
- Csmallest $K_2$ → $K_1$ → largest $K_3$
- Dsmallest $K_1$ → $K_2$ → largest $K_3$