Chapter 17, Problem 17.103QP

Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia.

$\text{AgCl}(s)+2{\text{NH}}_3(aq)\rightleftharpoons \text{Ag}{({\text{NH}}_3)}_2{}^{+}(aq)+{\text{Cl}}^{-}(aq)$

1. a What is the equilibrium constant for this dissolving process?
2. b Ammonia is added to a solution containing excess AgCl(s). The final volume is 1.00 L and the resulting equilibrium concentration of NH₃ is 0.80 M. Calculate the number of moles of AgCl dissolved, the molar concentration of Ag(NH₃)₂⁺, and the number of moles of NH₃ added to the original solution.