Question

AgCl(s) (Ksp = 1.8 ×10-10 ) is dissolved in water until a saturated solution is formed. NH3 (g) is then bubbled into the solution. Knowing that Ag(NH3)2+ has a Kf = 1.7 × 107, what should you expect happens to the solution of AgCl ?

Answer 1

The solution of AgCl will get more dissociated

Step-by-step explanation:

When AgCl is dissolved in water until it attains saturated solution then at this condition the solubility product will be equal to the ionic product

When NH3 is added to the solution as the equilibrium constant for the formation of the complex Ag(NH3)2+ is higher, the Ag+ present in the solution will get consumed in this reaction

So by Le chatelier's principle as the Ag+ is consumed in the reaction which involves the solubility of AgCl, the reaction will move in the forward direction

∵ As more forward reaction takes place, AgCl will get more dissociated