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