PbCl2 ==> Pb^++ + 2Cl^-
AgCl --> Ag^+ + Cl^-
Using Ksp for PbCl2, calculate what the (Cl^-) must be to ppt PbCl2. You know (Pb^++) and Ksp, solve for (Cl^-).
Do the same for AgCl. You know Ag^+ and Ksp, solve for (Cl^-). The one with the lower Cl^- will appear first so that answers the first two questions. Do that and perhaps the third question will be easier than it is now.
HCl is slowly added to a solution that is .250 M in Pb^2+ and .00150 M in Ag+. Which precipitate forms first, PbCl2 or AGCl? At what Cl- ion concentration will the precipitate first appear? Ksp for PbCl2= 1.6*10^-5, Ksp for AgCl= 1.7*10^-10
Seriously don't understand Ksp and solubility. How do I even approach this problem?
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