#K_"sp"# #AgCl(s)-=1.77xx10^-10#....and this equilibrium constant (which WILL be given you) addresses the following equilibrium...
#AgCl(s) rightleftharpoonsAg^+ + Cl^(-)#..
And so #K_"sp"# #AgCl(s)# #=[Ag^+][Cl^-]# #-=1.77xx10^-10#
Now it is a fact that #[Ag^+]=S_"solubility of AgCl"# for this problem....but we artificially raised #[Cl^-]#, i.e. we have #"salted out"# the stuff....
And so #Sxx(0.216*mol*L^-1+S)=1.77xx10^-10#
And if we make the reasonable approx. that #0.108*mol*L^-1">>"S#, then....
#S_1=(1.77xx10^-10)/(0.216*mol*L^-1)=8.19xx10^-10*mol*L^-1#
...the value is indeed small compared to #0.216*mol*L^-1#...so our approx. was justified. In pure water, would silver chloride be more soluble? Why or why not?
Thanx to Truong-Son who pointed out an error on my part...
