Following the experimental procedure described in the lab manual, a student combined 5.00 mL of 0.0020 M Fe3+ and 1.00 mL of 0.0020 M SCN¯ with 4.00 mL of water to create their Trial 1 solution. The student used their spectrophotometer to measure the absorbance of the reaction mixture and recorded an absorbance of 0.095. Given these experimental conditions and results, please calculate the following (be sure to save your work in case you need help from your instructor): a. The initial concentration of Fe3+: M (give to nearest 0.0001 M) b. The initial concentration of SCN": M (give to nearest 0.0001 M) c. The equilibrium concentration of FeSCN2+: (give as decimal to nearest 0.000 001)

Following the experimental procedure described in the lab manual, a student combined 5.00 mL of 0.0020 M Fe3+ and 1.00 mL of 0.0020 M SCN¯ with 4.00 mL of water to create their Trial 1 solution. The student used their spectrophotometer to measure the absorbance of the reaction mixture and recorded an absorbance of 0.095. Given these experimental conditions and results, please calculate the following (be sure to save your work in case you need help from your instructor): a. The initial concentration of Fe3+: M (give to nearest 0.0001 M) b. The initial concentration of SCN": M (give to nearest 0.0001 M) c. The equilibrium concentration of FeSCN2+: (give as decimal to nearest 0.000 001)

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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Question

Following the experimental procedure described in the lab manual, a student combined 5.00 mL of
0.0020 M Fe3+ and 1.00 mL of 0.0020 M SCN with 4.00 mL of water to create their Trial 1 solution.
The student used their spectrophotometer to measure the absorbance of the reaction mixture and
recorded an absorbance of 0.095.
Given these experimental conditions and results, please calculate the following (be sure to save your
work in case you need help from your instructor):
a. The initial concentration of Fe3+:
M (give to nearest 0.0001 M)
b. The initial concentration of SCN:
M (give to nearest 0.0001 M)
c. The equilibrium concentration of FeSCN2*:
(give as decimal to nearest 0.000
001)
Hint: The extinction coefficient of FeSCN2+ is 4,630 M-1°cm 1 and the cuvettes we use have a path
length of 1.0 cm.
d. The equilibrium concentration of Fe3+:
M (give as decimal to nearest 0.000
001 M)
e. The equilibrium concentration of SCN:
M (give as decimal to nearest 0.000
001 M)
f. The equilibrium constant K:
(give to nearest tens place)

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