[Chemistry] Is it possible to have an EQUILIBRIUM where....?

Question

1. Is it possible to have an equilibrium with AgCl dissolved in water where there is more Ag ions then there are Cl ions ?

2. in the equilibrium, the Ag and Cl are forming solids at the same rate as they are dissociating into their ions

if statement 2 is correct and in statement 1 it is possible,
then how does it work? coz then when Ag and Cl form solid, there would be some Ag left over since only one Ag goes with each Cl

Answer 1

If your ONLY source of Ag+ is the AgCl, then equal numbers of Ag+ and Cl- will be present in solution. Otherwise, you would be building up charge on the remaining solid, which does happen but only to a very small extent, too small to measurably affect concentrations in solution.

But there is nothing to stop you putting solid AgCl into a solution that already contains Ag+, in which case much less AgCl will dissolve.

In any case, [Ag+] x [Cl-] = Ksp(AgCl)

Quantitatively, Ksp for AgCl is 1.8 x 10^-10. So if AgCl equlibrates with water, the solution will become 1.34 x 10-5 M in Ag+ and in Cl- (1.34 x 10^-5 x 1.34 x 10^-5 = 1.8 x10^-10). But if you equilibrate AgCl with (say) 0.1M AgNO3 solution, only 1.8 x 10^-9 can dissolve.

Answer 2

The equilibrium for the saturated solotion is
AgCl (s) <----> Ag+ (aq) + Cl- (aq)
and the equilibrium condition is given by
Ksp = [Ag+] [Cl-]
In any case it is possible to have an equilibrium with AgCl dissolved in water where there is more Ag+ and Cl-. .
The solubility of AgCl will decrease
Statement 2 is correct

Answer 3

And statement 1 is incorrect, because that would leave behind a solid that has more Cl- ions in it. Crystals are always electroneutral, because without Ag+ ions in the crystal, the negative ion-negative ion pairs would strongly repel each other.