# Problem: Calculate the solubility of silver chloride in a solution that is 0.160 M in NH3 (initial concentration).

###### FREE Expert Solution

We’re being asked to calculate the solubility of Silver Chloride (AgCl) in 0.160 M NH3. The presence of NH3 would increase the solubility of AgCl because Ag+ would be consumed to form Ag(NH3)2+(aq)

There are two reactions involved:

Reaction 1:

AgCl (s) ⇌  Ag+(aq)  +   Cl- (aq)

Ksp = [Ag+][Cl-]  =  1.6x10-10   (you can get the Ksp value in books or the internet)

Reaction 2:

Ag+(aq)  +  2  NH(aq)  ⇌   Ag(NH3)2+ (aq)        A coefficient of 2 is added to NHto balance the reaction.

${\mathrm{K}}_{\mathrm{f}}=\frac{\left[\mathrm{Ag}{\left({\mathrm{NH}}_{3}\right)}_{2}\right]}{\left[{\mathrm{Ag}}^{+}\right]{\left[{\mathrm{NH}}_{3}\right]}^{2}}=\mathbf{1}\mathbf{.}\mathbf{7}\mathbf{×}{\mathbf{10}}^{\mathbf{7}}$  (you can get the Kvalue in books or the internet) ###### Problem Details

Calculate the solubility of silver chloride in a solution that is 0.160 M in NH3 (initial concentration).