Basically I said the definition for Kf is for
Ag^+ + 2NH3 ==> [Ag(NH3)2]^+ and that is something like 1.7E7. I don't think your Kf you quoted of 0.0031 is Kf; I think it is for
AgCl + 2NH3 ==> [Ag(NH3)2]^+ + Cl^- and that makes it Keq for that reaction and that is not the same as Kf which I showed above. The way you calculate Keq is Ksp*Kf (unless of course it is given in the problem) and if you use 1.8E-10 for Ksp and 1.7E7 for Kf you get 0.0031. As for showing my work, I'll be happy to check yours. If you had shown your work before I could have told you hours ago where the error is.
I do not quiet understand what you said. Could you show your work.
What is the solubility of AgCl in 10 M NH3? The Kf of Ag(NH3)2+ from AgCl(s) in aqueous NH3 is 0.0031, which is for the balanced reaction shown below.
AgCl(s) + 2 NH3(aq) → Ag(NH3)2+(aq) + Cl-(aq)
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