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
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.
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