A solution contains 6.81 x 10^{-3} M barium nitrate and 1.30 x 10^{-2} M silver acetate. Solid...


A solution contains {eq}6.81 \times 10^{-3} {/eq} M barium nitrate and {eq}1.30 \times 10^{-2} {/eq} M silver acetate. Solid ammonium sulfate is added slowly to this mixture.

A. What is the formula of the substance that precipitates first?

B. What is the concentration of sulfate ion when this precipitation first begins?

Selective Precipitation:

In soluble salts typically precipitate out of solution when their respective Qsp Ion-Product Constant Values become greater than or equal to the Ksp Solubility-Product Constant. A technique that utilizes the differences in the Solubility-Product Constant values to precipitate one of the dissolved cations is known as selective precipitation. With this method, the cation with a lower Ksp associated with its precipitation will form at a much lower concentration of precipitating agent added.

Answer and Explanation: 1

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The Solubility Product Constants associated with the formation of the sulfate salts are:

{eq}\rm BaSO_4 ~K_{sp} = 1.07\times10^{-10} \\ Ag_2SO_4...

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Learn more about this topic:

The Common Ion Effect and Selective Precipitation


Chapter 11 / Lesson 6

Learn about the common ion effect on solubility. Learn what a common ion is, examine a common ion chart, and work through examples of the common ion effect.

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