8. Precipitation calculations with Ni2+ and Pb²+ a. Use the solubility product for Ni(OH), (s) to calculate the pH at which Ni(OH), begins to precipitate from a 0.18 M Ni²+ solution (K, Ni(OH), = 5.5x10-1) sp ? (The Kp b. Will Pb(OH), (s) precipitate at the above pH from a 0.18 M Pb2* solution for Pb(OH), = 1.2x10-15)
8. Precipitation calculations with Ni2+ and Pb²+ a. Use the solubility product for Ni(OH), (s) to calculate the pH at which Ni(OH), begins to precipitate from a 0.18 M Ni²+ solution (K, Ni(OH), = 5.5x10-1) sp ? (The Kp b. Will Pb(OH), (s) precipitate at the above pH from a 0.18 M Pb2* solution for Pb(OH), = 1.2x10-15)
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 17.86QP
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