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nf_7138 nf_7138
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13 years ago
If 200.mL of a 0.00500M solution of AgNO3 were added to 400.mL of a 0.0100M solution of Na2CrO4, would Ag2CrO4 precipitate? The Ksp of Ag2CrO4 is 1.1 x 10^-12
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13 years ago
Balanced Reaction:

2 Ag+ (aq) + CrO42- (aq) Rightwards Arrow Ag2CrO4 (s)

Ksp = [Ag+]2 times [CrO4-]

If [CrO4-] = x, then [Ag+] = 2x (from the balanced equation)
then Ksp = 2x2 * x = 4x3 (substitute in for Ksp equation)

Solve for 'x'.

Max Concentration of CrO42- that is saturated in solution is: ...
Max Concentration of Ag2+ that is saturated in solution is: 2*(whatever number you get for 'x') = ...

Compare to actual concentration in solution:

Ag2+: 200 mL * ( 0.00500M / 1000 mL ) = ...
CrO42-: 400 mL * ( 0.0100M / 1000mL) = ...

If the actual amount of both ions in solution is greater than the maximum amount that will be saturated, then all the excess will precipitate out.
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