$\text{AgNO}_3(aq)$ is introduced into a solution containing a halide ion, $\text{X}^-(aq)$, and then aqueous ammonia is added. The ionic equations for the two reactions that take place are shown. $\text{Ag}^+(aq) + \text{X}^-(aq) \rightleftharpoons \text{AgX}(s)$ (equilibrium 1) $\text{Ag}^+(aq) + 2\text{NH}_3(aq) \rightleftharpoons \text{Ag(NH}_3)_2^+(aq)$ (equilibrium 2) Which statement is correct?
- AThe position of equilibrium 1 lies to the left when $\text{X}^- = \text{I}^-$.
- BIncreasing the concentration of ammonia causes the position of equilibrium 1 to move to the left.
- C$K_c$ for equilibrium 2 is larger when $\text{X}^- = \text{Cl}^-$ than when $\text{X}^- = \text{I}^-$.
- DEquilibrium 2 is a redox reaction.