When AgNO3 is added drop wise to the solution, the one with Qsp greater than Ksp will ppt first. You're correct, that is AgI. More drops of AgNO3 results in AgI continuing to ppt until Ksp for AgCl is met. What is (Ag^+) then?
Ksp = (Ag^+)(Cl^-). You know Ksp and you know Cl^-, solve for Ag^+. At that point with Ag^+ that value, what is I^-?
Ksp = (Ag^+)(I^-). You know Ksp and (Ag^+), solve for I^-. That is I^- at that point.
An aqueous solution that 2.00 M in AgNO3 is slowly added from a buret to an aqueous solution that is 1.00×10−2 M in Cl− and 0.260 M in I−. When the second ion begins to precipitate, what is the remaining concentration of the first ion?
I know that the first ion to ppt is I- , however I can't figure out the remaining concentration.
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