What is the approximate concentration of free Fe³⁺ ion in a solution prepared by mixing equal volumes of 0.06 M Fe³⁺ and 4.0 M F- solutions? [The net formation constant for FeF₅(H₂O)₂^- is 2.0 × 10¹⁵.]

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Quizplus · Accepted Answer

The formation of FeF5(H2O)2- complex ion decreases the free Fe3+ ion concentration. The equilibrium constant expression for the formation of the complex ion is:Kf = [FeF5(H2O)2-] / [Fe3+][F-]5Substituting the given values into the expression, we get:2.0 × 10^15 = [FeF5(H2O)2-] / [Fe3+][4.0]^5Assuming that the initial concentration of Fe3+ is 0.03 M (since equal volumes of 0.06 M Fe3+ and 4.0 M F- solutions are mixed), we can solve for the concentration of free Fe3+ ion:[Fe3+] = [FeF5(H2O)2-] / (2.0 × 10^15 * [4.0]^5)[Fe3+] = 6.9 × 10^-19 M

What Is the Approximate Concentration of Free Fe3+ Ion in a Solution

What Is the Approximate Concentration of Free Fe³⁺ Ion in a Solution