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A solution contains three anions with the following concentrations: 0.20 M CrO42-, 0.10 M CO32 - , and 0.010 M Cl-. If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4 (Ksp = 1.2 × 10-12), Ag2CO3 (Ksp = 8.1 × 10-12), or AgCl (Ksp = 1.8 × 10-10)?

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Hubert Koch
Hubert KochLv2
25 May 2020

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Related questions

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

second anion begins to precipitate, in part (b). 99.5+% removed indicates good separation!]

0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 x 10-12 and respectively.

Solid, soluble silver nitrate is added slowly to a solution forwhich the initial concentrations of Cl-1 andCrO4-2 were [Cl-1 ]0 = 0.10 molL-1 and [CrO42- ]0 = 0.025 molL-1.

(a) Calculate [Ag+] when a precipitate first appears andidentify the precipitate. The Ksp values for AgCl(s) andAg2CrO4(s) are 1.8x10-10 and1.1x10-12, respectively.

(b) Calculate [Cl-1] and[CrO42-] just before the second precipitateis formed. What is the % efficiency of the separation? (i.e. If Xrepresents the anion that precipitates first, then what fraction ofX was precipitated from the solution at the instant the secondprecipitate starts to form?)

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