Question

Silver chloride is not very soluble. The reaction by which it goes into solution is:

AgCl(s) <==> Ag^+ (aq) + Cl^- (aq)

A.) suppose a saturated solution of silver chloride were present. What would happen if you added a few ml of Jack solution and why?

B.) What would happen if you added a few ml of Silver Nitrate solution and why?

C.) If this reaction is known to be endothermic, what would happen if the solution were heated? What if it were cooled?

Answer 1

According to Lechatlier's principle,

(A) Addition of stock solution will precipitate the AgCl.

(B) Addition silver nitrate increases the concentration of Ag⁺ ions, but at a fixed temperature the solubility porduct of AgCl is constant. SO, to maintain constant Ksp, certain amount of Ag⁺ ions gets precipitated as AgCl.

(C) If thereaction is endothermic, increase in temperature favours endothermic reaction. It means more amount of salt can be soluble.

But decrease in temperature favours the exothermic reaction. SO, it makes the precipitation of AgCl on cooling.