An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L. Kf for Ni(NH3)62+ is equal to 5.5 × 108. Write the expression for the dissociation constant needed to determine the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed in Part 1. Kd = [Ni2+][NH3]^6/[Ni(NH3)^2+ 6] Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed.

An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L. Kf for Ni(NH3)62+ is equal to 5.5 × 108. Write the expression for the dissociation constant needed to determine the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed in Part 1. Kd = [Ni2+][NH3]^6/[Ni(NH3)^2+ 6] Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formed.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section12.3: Determining Equilibrium Constants

Problem 12.3PSP

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