equilibrium constant = [cl]/[I] not sure where the original equilibrium lies. Ag

Question

equilibrium constant = [cl]/[I]

not sure where the original equilibrium lies.

AgI will precipitate bcs it will be adding more I ions to a saturated solution of AgCl causing the equilibrium to shift right and create more AgI.

what can be added to my answer to make it more correct? Thanks

8) What is the equilibrium constant for the following reaction? AgCl (s) + r (aq) Agl( s) + cr (aq) Does the equilibri ion, r, is added on, I, is added to a saturated solution of silver chloride, Agci? (11 points) um lie to the right or to the left? Will Agl precipitate if a salt containing iodide to a saturated solution of silver chloride, AgCI? (11 points)

Explanation / Answer

KSp of AgCl- = [Ag+][Cl-]

Ksp of AgI = [Ag+][I-]

then

Kexpression = Ksp AgCl / Ksp AgI

Kexpression = [Cl-]/[I-]

note that

Ksp AgCl >> KSp AgI, then

Kexpression > 1; meaning it favours Ag and Cl-

that is

[Cl-] >>> [I-]

the shift is actually to the right

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