In the second part of this experiment, a student makes a solution with initial concentrations of iron(III) and thiocyanate ions of 0.000900 M and 0.000600 M respectively. Using the Beer's Law plot produced in the first part of the lab, the student determines the equilibrium concentration of the thiocyanatoiron(III) complex (Fe(SCN)2+) to be 2.00 × 10−5 M. What are the equilibrium concentrations of the two starting ions, and what is the value of the equilibrium constant? [Fe3+] = [SCN−] = Kc =
In the second part of this experiment, a student makes a solution with initial concentrations of iron(III) and thiocyanate ions of 0.000900 M and 0.000600 M respectively. Using the Beer's Law plot produced in the first part of the lab, the student determines the equilibrium concentration of the thiocyanatoiron(III) complex (Fe(SCN)2+) to be 2.00 × 10−5 M. What are the equilibrium concentrations of the two starting ions, and what is the value of the equilibrium constant? [Fe3+] = [SCN−] = Kc =
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter20: Chemistry Of Selected Transition Elements And Coordination Compounds
Section: Chapter Questions
Problem 44QRT
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In the second part of this experiment, a student makes a solution with initial concentrations of iron(III) and thiocyanate ions of 0.000900 M and 0.000600 M respectively. Using the Beer's Law plot produced in the first part of the lab, the student determines the equilibrium concentration of the thiocyanatoiron(III) complex (Fe(SCN)2+) to be 2.00 × 10−5 M.
What are the equilibrium concentrations of the two starting ions, and what is the value of the equilibrium constant?
[Fe3+] =
[SCN−] =
Kc =
Kc =
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