A solution contains 0.010 M Ba2+ and 0.010 M Ag+. Can 99.91% of either ion be precipitated by

chromate (CrO42-) without precipitating the other metal ion? The Ksp for BaCrO4 is 2.1 x 10-10 and

the Ksp for Ag2CrO4 is 1.2 x 10-12

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Nelly StrackeLv2

29 Sep 2019

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Silver chloride has Ksp = 1.6 x 10-10 and silver chromate has Ksp = 9.0 x 10-12. We have 1.00 liter of a

solution which contains both NaCl (0.10 M) and Na2CrO4 (0.10 M). Solid AgNO3 is added slowly and the solution is stirred well.

a) Which salt precipitates first, AgCl or Ag2CrO4? (Show your work!)

b) What are the concentrations of [Ag+], [Cl-], and [CrO42-] at the point when the second salt just begins to

precipitate?

c) Is this method of selective precipitation a good one for separating the anions in the solution? [Hint: Calculate the percent of the first ion (to precipitate) remaining in solution at the point the

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