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Solid NaI is slowly added to a solution that is 0.010 M in Cu+ and 0.010 M in Ag+.

Solid NaI is slowly added to a solution that is 0.010 M in Cu+ and 0.010 M in Ag+.

(a) Which compound will begin to precipitate first?

(b) Calculate [Ag+] when CuI just begins to precipitate.

(c) What percent of Ag+ remains in solution at this point?
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Answer #1

Ksp for CuI is 1 x 10^-12
Ksp for AgI is 8.3 x 10^-17

These two salts would both dissociate in the same way, so we can say that because AgI has a smaller Ksp value, the AgI should precipitate first.

[Cu+][I-] = 1 x 10^-12
[0.01][I-] = 1 x 10^-12
[I-] = 1 x 10^-10 M

[Ag+][I-] = 8.3 x 10^-17
[Ag+][1 x 10^-10] = 8.3 x 10^-17
[Ag+] = 8.3 x 10^-7 M

(8.3 x 10^-7 M) divided by (0.01 M) x 100%

0.0083% of Ag+ remains in solution

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