A mixture of solution contains 0.060M Ca2+ and 0.040M Ag+. Which one precipitates first by adding...

A mixture of solution contains 0.060M Ca2+ and 0.040M Ag+. Which one precipitates first by adding SO4 2- (sulfate). Can 99% of Ca2+ be precipitated by sulfate without precipitating Ag+?. (given Ksp values for CaSO4 = 4.93 x 10^-5 and Ag2SO4= 1.2 x 10^-5). The Ksp values in this question are hypothetical values.

Expert Solution

The salt with lower K_sp value will precipitate first.
K_sp = [Ag⁺]² [SO₄^2-] , once this ion product concentration value crosses K_sp then it
precipitates immediately
K_sp = [Ca⁺²] [SO₄^2-]
4.93*10^-5 = 0.060 * [SO₄^2-]
[SO₄^2-] = 8.2167*10^-4 M
Now calculate the product of [Ag⁺]² [SO₄^2-]
[Ag⁺]² [SO₄^2-] = 0.040² * 8.2167*10^-4 = 1.3146*10^-6
Since this ion product concentration did not exceed K_sp it will not precipitate first
Hence CaSO₄ will precipitate first.
Ca⁺² will be precipitated completely by sulfate before the Ag⁺ precipitation begins
So, Yes 99% of Ca²⁺ be precipitated by sulfate without precipitating Ag⁺

queen_honey_blossom answered 2 years ago

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