I would do this.
AgCl(s) ==> Ag^+ + Cl^- Ksp = 1E-10
Ag^+ + 2Cl^---> [AgCl2]^- Kf = 3E5
----------------------
AgCl(s) + Cl^- --> [AgCl2]^-
Keq = Ksp*Kf = approx 3E-5 which is not a large number which means the amount of NaCl will be relatively large.
I..0.1....0............0
add.......x..............
C...-x....-x............x
E...1E-5...0...........0.1
Where did these numbers come from? From the I line we had 0.1 M AgCl to dissolve. The others are 0 initially.
For the E line, to dissolve AgCl it will be 0.1-x. We want it to be sqrt Ksp = sqrt 1E-10 = 1E-5M so 0.1-x = 1E-5 . We want 0 NaCl left and we will have formed 0.1M - 1E-5 of the complex which is essentially 0.1M
Plug in those values into Keq expression and solve for Cl^-. Then convert from M Cl^- to grams/L and form there to g/100 mL. It will be a large number because the Kf is not all that large and the Ksp is very small.
Calculate the mass of NaCl required to cause dissolution of 0.010 moles of AgCl in 100 mL of solution. Consider that the addition of NaCl does not cause increased volume in the solution
KSP (AgCl) = 1.0 x 10 ^ -10
KF (AgCl2) = 3.0 x 10 ^ 5
1 answer
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