Use the systematic treatment of equilibrium to calculate the concentrationof Ba2+ in acidic solution, if its concentration is governed by the followingequilibria –BaSO4 (s) → Ba2+ + SoKsp = 1.1 x 10-10so, +H2O HSO, +OHK, = 9.8 x 10-13Bat + So,BaSO4 (aq)K = 1.9 x 10Hint: Since the pH is fixed at 1.89, the charge balance is invalidated. Usethe mass balance for your calculation.

1.BaSO4(s)→Ba2+ + SO42- Ksp=[Ba2+][SO42-] 2. SO42- +H2O→HSO4-+OH- Kb=HSO4-OH-SO42- 3. Ba2+ +…

Use the systematic treatment of equilibrium to calculate the concent of Ba2+ in acidic solution, if its concentration is governed by the following equilibria - BasO4 (s) Ba2+ + so?- Ksp = 1.1 x 10-10 %3D so, +H2O HSO, +OH K, = 9.8 x 10-13 %3D so K = 1.9 x 10! Ba+ + 2+ - BaSO4 (aq) Hint: Since the pH is fixed at 1.89, the charge balance is invalidated. Use the mass balance for your calculation.

Use the systematic treatment of equilibrium to calculate the concent of Ba2+ in acidic solution, if its concentration is governed by the following equilibria - BasO4 (s) Ba2+ + so?- Ksp = 1.1 x 10-10 %3D so, +H2O HSO, +OH K, = 9.8 x 10-13 %3D so K = 1.9 x 10! Ba+ + 2+ - BaSO4 (aq) Hint: Since the pH is fixed at 1.89, the charge balance is invalidated. Use the mass balance for your calculation.

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

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

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

Chapter17: Equilibrium

Section: Chapter Questions

Problem 38A

See similar textbooks

Similar questions

In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the concentrations of the species at equilibrium are [N2] = 0.0013, [O2] = 0.0024, and [NO2] = 0.00065.
5.49. Consider the following equilibrium: What is the effect on the equilibrium of each of the following changes? (You may need to calculate some standard enthalpy or Gibbs energy changes to answer these.) (a) The pressure is increased by decreasing the volume. (b) The temperature is decreased. (c) The pressure is increased by the addition of nitrogen gas, .
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
Write an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a product
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?