From the value Kf=1.2×10^9 for Ni(NH3)6^2+, calculate the concentration of NH3 required to just dissolve 0.026 mol of NiC2O4 (Ksp = 4×10^−10) in 1.00 L of solution. (Hint: You can neglect the hydrolysis of C2O4^2− because the solution will be quite basic.)
From the value Kf=1.2×10^9 for Ni(NH3)6^2+, calculate the concentration of NH3 required to just dissolve 0.026 mol of NiC2O4 (Ksp = 4×10^−10) in 1.00 L of solution. (Hint: You can neglect the hydrolysis of C2O4^2− because the solution will be quite basic.)
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter19: Transitition Metals, Coordination Chemistry And Metallurgy
Section: Chapter Questions
Problem 19.60QE
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From the value Kf=1.2×10^9 for Ni(NH3)6^2+, calculate the concentration of NH3 required to just dissolve 0.026 mol of NiC2O4 (Ksp = 4×10^−10) in 1.00 L of solution. (Hint: You can neglect the hydrolysis of C2O4^2− because the solution will be quite basic.)
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