In Lab Experiment 2, you studied the following equilibrium: Fe3+(aq) + SCN–(aq) ⇌ Fe(SCN)2+(aq) If you knew the equilibrium constant K and the initial concentrations of Fe3+(aq) and SCN–(aq), what would be the simplest way to determine the equilibrium concentration of Fe(SCN)2+(aq)? A. By writing the equilibrium constant equation and solving it for [Fe(SCN)2+]equ.
In Lab Experiment 2, you studied the following equilibrium: Fe3+(aq) + SCN–(aq) ⇌ Fe(SCN)2+(aq) If you knew the equilibrium constant K and the initial concentrations of Fe3+(aq) and SCN–(aq), what would be the simplest way to determine the equilibrium concentration of Fe(SCN)2+(aq)? A. By writing the equilibrium constant equation and solving it for [Fe(SCN)2+]equ.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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 Lab Experiment 2, you studied the following equilibrium:
Fe3+(aq) + SCN–(aq) ⇌ Fe(SCN)2+(aq)
If you knew the equilibrium constant K and the initial concentrations of Fe3+(aq) and SCN–(aq), what would be the simplest way to determine the equilibrium concentration of Fe(SCN)2+(aq)?
-
A.
By writing the equilibrium constant equation and solving it for [Fe(SCN)2+]equ.
-
B.
By measuring the absorbance of the equilibrium samples and using the Beer–Lambert law.
-
C.
By ensuring that SCN– is not in excess relative to Fe3+(aq).
-
D.
[Fe(SCN)2+]equ is always equal to the initial concentration of SCN–.
-
E.
By plotting the absorbance of Fe(SCN)2+(aq) versus concentration and determining the slope.
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