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12 Dec 2019
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!]
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!]
Nelly StrackeLv2
13 Dec 2019