What is the minimum concentration of Cl- necessary to begin precipitation of AgCl(s) (Ksp = 1.77×10-1) in a solution of 5.0×10-5M Ag+?
Ag+ + Cl- = AgCl
Ksp (AgCl) = [Ag+] [Cl-]
given Ksp (AgCl) = 1.77×10-1
[Ag+] = 5.0×10-5 M
[Cl-] = Ksp / [Ag+]
[Cl-] = 1.77×10-1 / 5.0×10-5
[Cl-] = 3540 M or 3.5 x 103 M
What is the minimum concentration of Cl- necessary to begin precipitation of AgCl(s) (Ksp = 1.77×10-1)...
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