It is of interest to decide if an analytical separation of the metal ions can be effected by selective precipitation of carbonates from a solution that is 0.110 M in Fe2+ and 0.105 M in Ba2+, FeCO3 Ksp = 3.50x10-11 BaCO3 Ksp = 8.10x109 To analyze this problem, answer the following questions. (1) What carbonate concentration is needed to precipitate 99.9% of the metal that forms the least soluble carbonate? (2) When 99.9% of the least soluble carbonate has precipitated, will all of the metal that forms the more soluble carbonate still remain in solution? O (3) What is the upper limit on the carbonate ion concentration if the more soluble compound is not to precipitate? M M

It is of interest to decide if an analytical separation of the metal ions can be effected by selective precipitation of carbonates from a solution that is 0.110 M in Fe2+ and 0.105 M in Ba2+, FeCO3 Ksp = 3.50x10-11 BaCO3 Ksp = 8.10x109 To analyze this problem, answer the following questions. (1) What carbonate concentration is needed to precipitate 99.9% of the metal that forms the least soluble carbonate? (2) When 99.9% of the least soluble carbonate has precipitated, will all of the metal that forms the more soluble carbonate still remain in solution? O (3) What is the upper limit on the carbonate ion concentration if the more soluble compound is not to precipitate? M M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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