Solutions of BaCl2 and NaOH were mixed until a certain amount of precipitate was formed. The equilibrium concentration of Ba2+ in the combined solution above the precipitate was found to be 0.50 M. What is the concentration of the OH– ions in that solution? The solubility product constant of Ba(OH)2 is Ksp = 5.0 × 10–3. A. 0.20 M B. 0.10 M C. 0.020 M D. 0.14 M E. 0.050 M
Solutions of BaCl2 and NaOH were mixed until a certain amount of precipitate was formed. The equilibrium concentration of Ba2+ in the combined solution above the precipitate was found to be 0.50 M. What is the concentration of the OH– ions in that solution? The solubility product constant of Ba(OH)2 is Ksp = 5.0 × 10–3. A. 0.20 M B. 0.10 M C. 0.020 M D. 0.14 M E. 0.050 M
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 70QAP: . The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method...
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Solutions of BaCl2 and NaOH were mixed until a certain amount of precipitate was formed. The equilibrium concentration of Ba2+ in the combined solution above the precipitate was found to be 0.50 M. What is the concentration of the OH– ions in that solution? The solubility product constant of Ba(OH)2 is Ksp = 5.0 × 10–3.
- A. 0.20 M
- B. 0.10 M
- C. 0.020 M
- D. 0.14 M
- E. 0.050 M
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