You note that the Ksp of Ba3(PO4)2 is much smaller than that of Ba(OH)2. Therefore, you wonder if adding a phosphate species, such as H3PO4, can precipitate out more of the barium ions (Ba²+) from the solution (and then you could filter out the solid to have a smaller waste volume!). Therefore, you look up another equilibrium constant, shown for equation below: H3PO4 (aq)=3 H+ (aq) + PO¾-¯ (aq) K₁ = 2.0 x 10-22 15. If you were to add H3PO4 to your waste solution to attempt to precipitate Ba3(PO4)2, what would be the equilibrium constant for the net reaction (shown below)? 3 Ba(OH)2 (s) + 2 H3PO4 (aq) = 6 H2O (l) + Ba3(PO4)2 (5)

You note that the Ksp of Ba3(PO4)2 is much smaller than that of Ba(OH)2. Therefore, you wonder if adding a phosphate species, such as H3PO4, can precipitate out more of the barium ions (Ba²+) from the solution (and then you could filter out the solid to have a smaller waste volume!). Therefore, you look up another equilibrium constant, shown for equation below: H3PO4 (aq)=3 H+ (aq) + PO¾-¯ (aq) K₁ = 2.0 x 10-22 15. If you were to add H3PO4 to your waste solution to attempt to precipitate Ba3(PO4)2, what would be the equilibrium constant for the net reaction (shown below)? 3 Ba(OH)2 (s) + 2 H3PO4 (aq) = 6 H2O (l) + Ba3(PO4)2 (5)

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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