A student dissolved 1.50 g of solid Ni(NO3)2 in 30 mL distilled H2O and subjected it to a hot water bath for 5 minutes. After heating, a light green solution was produced which was then separated into six test tubes. To determine the relative stability of Ni2+ complexes, distilled H2O, 3.0 M 1,10-phenanthroline (phen), and 12 M NH3 were used as ligand sources. The observations are as follows (see the attached photo): Compute for the formation constant of [Ni(NH3)6]2+ in test tube 3 given the following equilibrium concentrations: [Ni(H2O)6 2+] = 2.5 x 10-2 M;[NH3] = 0.010 M; [Ni(NH3)6 2+] = 2.1 x 10-5 M.

A student dissolved 1.50 g of solid Ni(NO3)2 in 30 mL distilled H2O and subjected it to a hot water bath for 5 minutes. After heating, a light green solution was produced which was then separated into six test tubes. To determine the relative stability of Ni2+ complexes, distilled H2O, 3.0 M 1,10-phenanthroline (phen), and 12 M NH3 were used as ligand sources. The observations are as follows (see the attached photo): Compute for the formation constant of [Ni(NH3)6]2+ in test tube 3 given the following equilibrium concentrations: [Ni(H2O)6 2+] = 2.5 x 10-2 M;[NH3] = 0.010 M; [Ni(NH3)6 2+] = 2.1 x 10-5 M.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter5: Errors In Chemical Analyses

Section: Chapter Questions

Problem 5.10QAP

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