Hello, this is a problem from the 2015 USNCO exam on solubility equilibrium that I'm having a bit of trouble on...
Silver chloride, AgCl (Ksp = 1.8 x 10-10), can be dissolved
in solutions containing ammonia due to the formation of
the soluble complex ion Ag(NH3)2+ (Kf = 1x108)
What is the minimum amount of NH3 that would need to
be added to dissolve 0.010 mol AgCl in 1.00 L of
(A) 0.010 mol (B) 0.020 mol
(C) 0.095 mol (D) 0.13 mol
(C) is correct answer.
I am able to combine the equations to solve for the correct answer, but my trouble is more with the concept. So, when we add the two equations, we obtain the equation of AgCl + ammonia -> complex ion + Cl-. However, how does this allow us to solve for the molar solubility of AgCl at varying concentrations of ammonia, for example? [Ag+] is absent from the equation, and from how I see people who solve these types of questions do it, they use the final concentration of the formed complex ion as the molar solubility. Does this not neglect the portion of silver ions that did not form the complex?
Thanks in advance.