Why Does the Common Ion Effect Increase Ksp for AgCl in the Presence of Cl-?

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SUMMARY

The discussion centers on the common ion effect and its impact on the solubility product constant (Ksp) of silver chloride (AgCl) in the presence of chloride ions (Cl-). The Ksp of AgCl in pure water is established at 1.77x10^-10, while the presence of 0.01M Cl- raises the concentration of Ag+ to 1.77x10^-8. This indicates that the solubility of AgCl increases in the presence of Cl-, which is counterintuitive since Ksp remains constant under unchanged temperature conditions. The increase in Ag+ concentration does not imply greater dissociation of AgCl but rather reflects the equilibrium shift due to the common ion effect.

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I'm working Ksp problems comparing pure water solutions w/ those with an ion already present in solution. Example: AgCl and NaCl both in solution.

The pure water Ksp for AgCl is given as 1.77x10^-10. The question is what the Ksp would be with .01M of Cl- already present. After working the problem, I get an answer (verified as correct) as: 1.77x10^-8. This makes mathematic sense, but it doesn't intuitively make sense to me. The Ksp is larger (10^-8) with the extra ion than for pure water (10^-10)? Doesn't this indicate that AgCl dissociates MORE with .01M Cl- already present? How?
 
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1.77x10-8 is not Ksp, but concentration of Ag+ in the solution. Ksp is constant (as long as temperature doesn't change).
 
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