Can you do a sample calculation because i still don't understand? Original Question: "A solution contains 0.01 M in both I- and Cl-. To 1.00L of this solution, 0.01 moles of AgNO3 are added (you can ignore volume changes) . Ksp for AgI is 8.3x10-17 and Ksp for AgCl is 1.8x10-10. After the solution has reached equilibrium, will anything precipitate? If yes, how much. I understand how to find IF and precipitate will form (using Q). But how do you find HOW MUCH? Will they precipitate in ratio to their Ksp values. Or the difference in Q and the base Ksp values? Thanks for your help."