Use the systematic treatment of equilibrium to calculate the concentration of Ba2+ in acidic solution, if its concentration is governed by the following equilibria – BaSO4(s) → Ba2+ + SO2-4 Ksp = 1.1 x 10-10 SO2-4 +H2O → HSO-4 +OH- Kb = 9.8 x 10–13

Use the systematic treatment of equilibrium to calculate the concentration of Ba2+ in acidic solution, if its concentration is governed by the following equilibria – BaSO4(s) → Ba2+ + SO2-4 Ksp = 1.1 x 10-10 SO2-4 +H2O → HSO-4 +OH- Kb = 9.8 x 10–13

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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Question

Use the systematic treatment of equilibrium to
calculate the concentration of Ba2+ in acidic
solution, if its concentration is governed by
the following equilibria -
BaSO4(s) → Ba2+ + SO2-4
Ksp = 1.1 x 10-10
SO2-4 +H2O → HSO-4 +OH-
Kb = 9.8 x 10-13
Ba2+ + SO2-4 → BaSO4(aq)
Kf = 1.9 x 101
Hint: Since the pH is fixed at 1.89, the charge
balance is invalidated. Use the mass balance
for your calculation.

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