1. The problem statement, all variables and given/known data COCL4 + 6H2 <=> Co(H20) +4CL blue <=> pink Question: Add a very small amount of AgNO3 to test tube #6. Stopper the test tube and shake. The solution in test tube turned pink, so I interpreted that as a shift to the products. Also, a precipitate (proper term? a solid was present...) formed. 3. The attempt at a solution Now I have to offer an explanation for why this occurred. It seems as though the Ag+ is slightly soluble in Cl-, and the Cl is found on the product side, so was the Cl consumed somehow and thus produced CoCl42-? To me that doesn't seem reasonable. EDIT: I somehow thought myself into a circle, because CoCl42- wouldn't have been produced, for if it had the solution should have turned blue right? I'm fairly sure my explanation should hinge on the fact that Ag+is only slightly soluble with Cl-, but I don't want to go off on a tangent either, so if I'm horribly misguided please advise.