Question

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)

Work:
Ksp = x^2 /(2x+10)^2 = 1.8 x 10^-10
Now I am confused.......
At first I got 0.557 an now.. I don't think this is correct... :(

I used the ICE chart to calculate, but it seems that I am doing this incorrectly...

Answers

DrBob222
The first thing wrong is you are using Ksp. You still haven't answered my question about the Kf. Kf is the formation constant for the complex.
Ag^+ + 2NH3 ==> [Ag(NH3)2]^+
The literature shows that as about 1.7E7 and your question gives it as 0.0031. I think that 0.0031 is the equilibrium constant for the reaction
AgCl(s) + 2 NH3(aq) → Ag(NH3)2+(aq) + Cl-(aq) and that is NOT Kf.

In addition, if I calculate the value of Keq for that reaction it is Keq = Kf*Ksp = 0.0031 which adds some credibility to what I've said above. Here is the way I would set up the ICE chart.
.AgCl + 2NH3 =>[Ag(NH3)2]^+ + Cl^-
I..solid..10.....0.............0
C....s....-2x....x.............x
E..s....10-2x....x.............x

K = 0.0031 = (x)(x)/(10-2x)^2
Solve for x.

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