In Part I of the experiment, you will prepare 5 solutions according to the chart below. Notice that the final volume of each solution is 50 mL. 0.200 M Fe(NO3)3 0.0020 M SCN™ H20 Beaker number (mL) (mL) (mL) 1 (blank) 5.0 0.0 45.0 2 5.0 5.0 40.0 3 5.0 4.0 41.0 4 5.0 3.0 42.0 5 5.0 2.0 43.0 For the solutions that you will prepare in Part I, calculate the [FeSCN²]. Assume that all of the SCN ions react. In Part I of the experiment, mol of SCN=mol of FeSCN2+. Thus, the calculation of [FeSCN2] is: mol FeSCN2 + L of total solution. Or, you can use M₁V₁= M₂V₂. Show at least one sample calculation.
In Part I of the experiment, you will prepare 5 solutions according to the chart below. Notice that the final volume of each solution is 50 mL. 0.200 M Fe(NO3)3 0.0020 M SCN™ H20 Beaker number (mL) (mL) (mL) 1 (blank) 5.0 0.0 45.0 2 5.0 5.0 40.0 3 5.0 4.0 41.0 4 5.0 3.0 42.0 5 5.0 2.0 43.0 For the solutions that you will prepare in Part I, calculate the [FeSCN²]. Assume that all of the SCN ions react. In Part I of the experiment, mol of SCN=mol of FeSCN2+. Thus, the calculation of [FeSCN2] is: mol FeSCN2 + L of total solution. Or, you can use M₁V₁= M₂V₂. Show at least one sample calculation.
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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![Prelab - Experiment 4: The Determination of
an Equilibrium Constant
Prelab Assignment
In Part I of the experiment, you will prepare 5 solutions according to the chart below. Notice
that the final volume of each solution is 50 mL.
0.200 M Fe(NO3)3
0.0020 M SCN™
H20
Beaker
number
(mL)
(mL)
(mL)
1 (blank)
5.0
0.0
45.0
2
5.0
5.0
40.0
3
5.0
4.0
41.0
4
5.0
3.0
42.0
5
5.0
2.0
43.0
For the solutions that you will prepare in Part I, calculate the [FeSCN²*].
Assume that all of the SCN ions react. In Part I of the experiment, mol of SCN = mol of
FeSCN2+. Thus, the calculation of [FeSCN2+] is: mol FeSCN²+ + L of total solution.
Or, you can use M₁ V₁ = M₂V₂. Show at least one sample calculation.
Beaker number
[FeSCN²] = [SCN]
1 (blank)
0.00 M
2
3
4
5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3ece18ee-616a-4a89-836b-a67bbe1fad5e%2Fc6e1c03e-8cce-45c6-8a6f-e77f7abadaf8%2Flf65s7d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Prelab - Experiment 4: The Determination of
an Equilibrium Constant
Prelab Assignment
In Part I of the experiment, you will prepare 5 solutions according to the chart below. Notice
that the final volume of each solution is 50 mL.
0.200 M Fe(NO3)3
0.0020 M SCN™
H20
Beaker
number
(mL)
(mL)
(mL)
1 (blank)
5.0
0.0
45.0
2
5.0
5.0
40.0
3
5.0
4.0
41.0
4
5.0
3.0
42.0
5
5.0
2.0
43.0
For the solutions that you will prepare in Part I, calculate the [FeSCN²*].
Assume that all of the SCN ions react. In Part I of the experiment, mol of SCN = mol of
FeSCN2+. Thus, the calculation of [FeSCN2+] is: mol FeSCN²+ + L of total solution.
Or, you can use M₁ V₁ = M₂V₂. Show at least one sample calculation.
Beaker number
[FeSCN²] = [SCN]
1 (blank)
0.00 M
2
3
4
5
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