If the Ksp of BaF2 = 1.8 × 10-7 at 25 0C, calculate the molar solubility of BaF2 at 25 0C in: i. Pure water ii. A 0.015 M solution of NaF iii. A 0.02 M solution of Ba(NO3)2 iv. Briefly account for the difference in the molar solubility of BaF2 whenever a “common ion” is present in the solution.
If the Ksp of BaF2 = 1.8 × 10-7 at 25 0C, calculate the molar solubility of BaF2 at 25 0C in: i. Pure water ii. A 0.015 M solution of NaF iii. A 0.02 M solution of Ba(NO3)2 iv. Briefly account for the difference in the molar solubility of BaF2 whenever a “common ion” is present in the solution.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter17: Solubility And Complex-ion Equilibria
Section: Chapter Questions
Problem 17.98QP: A saturated solution of lead iodate in pure water has an iodate-ion concentration of 8.0 105 M. a...
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If the Ksp of BaF2 = 1.8 × 10-7 at 25 0C, calculate the molar solubility of BaF2 at 25 0C in: i. Pure water ii. A 0.015 M solution of NaF iii. A 0.02 M solution of Ba(NO3)2 iv. Briefly account for the difference in the molar solubility of BaF2 whenever a “common ion” is present in the solution.
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