Question

Given the equation
Ag^+(aq) + 2NH3 (aq) -> [Ag(NH3)2]^+ (aq) kf= 2 x 10^7
determine the concentration of NH3(aq) that is required to dissolve 415 mg of AgCl(s) in 100.0 mL of solution. The Ksp of AgCl is 1.77× 10–10.

Answer 1

AgCl ==> Ag^+ + Cl^- Ksp = (Ag^+)(Cl^-)
Ag^+ + 2NH3 ==> [Ag(NH3)2]^+ Kf = ---
Add the equations to get this:
AgCl(s) + 2NH3 ==> Cl^- + [Ag(NH3)2]^+
So Keq = Ksp*Kf
Set up an ICE chart and solve for (NH3). I think a quadratic will be necessary. Post your work if you get stuck.

Answer 2

AgCl(s) + 2NH3 ==> Cl^- + [Ag(NH3)2]^+
I 0........4.21M.......0

C -2x.......+x..........+x

E -2x.......4.21-x......x

3.54x10^-3=(x)(4.21-x)/(-2x)^2

???

Please help

Answer 3

Can you help here please

Answer 4

You don't start with 0 AgCl.

Answer 5

AgCl is solid, it is not included in an ice table