Now imagine what happens when a few crystals of NaCl are added to a saturated solution of AgCl in water.
{"Image DocumentName": "Now imagine what happens when a few crystals of NaCl are added to a saturated solution of AgCl in water.", "Image ImageDescription": "There are two sources of the chloride ion in this solution. H2O NaCl(s) \uf0e8 Na+(aq)+ Cl-(aq) AgCl(s) \uf0e8 Ag+(aq)+Cl-(aq) Once again, the ion product is larger than the solubility product. Qsp = (Ag+)(Cl-) > Ksp. This time, when the reaction comes back to equilibrium, there will be more Cl- ion in the solution than Ag+ ion. Saturated solution of AgCl to which NaCl has been added: [Ag+] < [Cl-] 3/25/2017.", "Image XResolution": "37", "Image YResolution": "37", "Image ResolutionUnit": "Pixels/Centimeter", "Image Software": "SlidePlayer", "Image YCbCrPositioning": "Centered"}