Pre-lab 5 - Beer's law
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Quantitative General Chemistry Lab Manual
Lab 5: Pre-Lab Assignment
Name:
Section:
1. Assuming Allura Red, molar mass 496.42 g/mol, has a molar absorptivity of about 25,000
cm
−
1
M
−
1
at 500 nm, what mass of it will you need to create 100. mL of a solution that
has an absorbance of 1.0 in a 1.0 cm cuvette?
2. Will you be able to accurately measure that mass using a top-loading balance? Why or
why not?
3. What about with an analytical balance? Why or why not?
Lab 5: Quantitative Analysis Using Beer’s Law
·
75
4. Considering this amount you would have to weigh out for a dilution to 100 mL in volu-
metric glassware, propose another volume to dilute to that might be easier to execute. Is
this volume practical considering you only need
∼
1 mL of the final solution to check its
absorbance at 500 nm?
5. If you think the molar absorptivity of this food dye is representative of most dyes at their
respective
λ
max
, do you think most dyes can be accurately weighed as a dry powder and
diluted in a single step using common volumetric glassware to achieve an absorbance value
in the linear range of a spectrophotometer? Would your answer be different if you were
aiming for an absorbance value of 0.1 instead of 1.0?
As part of your notebook preparation, create a diagram similar to Figure 5.4 for creating
the absorbance 1.0 solution of Allura Red based on your answers to the pre-lab assignment.
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Related Questions
A. Copper sulfate pentahydrate is often used to teach students about Beer’s Law by making a standard curve (linear regression). The bright blue color of the solution has a peak absorbance in the red range of the electromagnetic spectrum. The absorbance value is proportional to concentration. How many grams of CuSO4 5H2O to make up 250 mL of a 0.2 M stock of this solution?
B. Using M1V1 = M2V2 how many mL would a student need to measure out in graduated cylinder to make up a 50 mL (V2) solution of 0.1M, 0.05 M, 0.025M 0.0125M solutions for a standard curve at the peak wavelenth for this compound?
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A. Copper sulfate pentahydrate is often used to teach students about Beer’s Law by making a standard curve (linear regression). The bright blue color of the solution has a peak absorbance in the red range of the electromagnetic spectrum. The absorbance value is proportional to concentration. How many grams of CuSO4 5H2O to make up 250 mL of a 0.2 M stock of this solution?
B. Using M1V1 = M2V2 how many mL would a student need to measure out in graduated cylinder to make up a 50 mL (V2) solution of 0.1M, 0.05 M, 0.025M 0.0125M solutions for a standard curve at the peak wavelenth for this compound?
I need help with part B of this question.
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A direct ELISA experiment was done to determine the amount of protein present in a sample. A standard curve was prepared by plotting log Absorbance versus log concentration of protein in (ng/mL). The equation of the line is Y= 0.895 X -1.25. If an unknown protein shows an absorbance of 1.23. Calculate the concentration of this protein in the sample in (ng/mL).
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GMU QUESTION 7
An ethanol solution of 3.5 mg/100 ml of compound Y (150.0 g/mol) in a 1.00 cm quartz cell has an absorbance (A) of 0.972 at Amax-235
nm. What is its molar extinction coefficient? Report your answer to the correct number of significant figures. Do not include units in your
answer.OGMU 2020
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Table II
Cuvette #
Concentration
Absorbance
0.50 M
1
1.049
2
0.40 M
0.926
3
0.20 M
0.740
0.298
4
0.10 M
5
0.05 M
0.202
Unknown # 9
0.427
Unknown # 10
7
0.646
Blank (DI water)
0
1. If Beer's Law is valid, the value of "E" should be constant. Use A = E*C*L or E=
A/(E*L) and the data from Table II to calculate values of E for the five solutions below
The value of L is normally 1 cm so E = A/C in this experiment.
Table III
Solution #
Calculated Values of E
1
2
3
4
5
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AP Questions // Questions 10 - 11) A student creates four solutions with varying
concentration of FeSCN2 and gathers the following data at 298 K using a spectrophotometer
calibrated to 460 nm:
[FESCN]
Absorbance
1.1 x 10-4 M
0.076
1.6 x 10-4 M
0.112
2.2 x 10-4 M
0.167
2.5 x 10-4 M
0.199
On the axis below, create a Beer's Law calibration plot for [FESCN2*]. Draw a best-fit line
through your data points.
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PLEASE Answer within 20-30 minutes. Thank you!
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Conclusion 5: You are tasked with analyzing a suspiciously pink sample of drinking water to establish if it has unsavory levels of MnO4-contamination. It has an absorbance of 0.83 at 544 nm when measured in a cuvette that is 1 cm across.
Using the equation of your trend line from Plot 4, determine the concentration of KMnO4 in moles/liter.
Convert this concentration to grams of manganese/liter and compare it to the EPA guideline above.
Trandline is Absorbtion = 2000(Concentration KMnO4) (Y=Mx)
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So
Please don't provide the handwriting solution
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Absorbance
1.40
Beer's Law Plot
1.20
1.00
0.80
0.60
0.40
0.20
0.00
0
10
20
30
40
50
Concentration (M x 105)
D
The slope for the line is 80.23. Use the Beer's Law plot provided to determine the
concentration for a solution with absorbance = 0.5786.
M
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given the following results " create a “standard curve” (a graph) that shows the concentration on the x-axis and the absorbance on the y-axis" and "a solution of copper(II) sulphate with an unknown concentration was found to have an absorbance of 0.09. Use your standard curve to determine its concentration"
ample Number
Concentration of Copper(II) Sulphate (mM)
Measured Absorbance
1
0
0
2
50
0.12
3
100
0.24
4
150
0.35
5
200
0.47
Unknown
40
0.09
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The following Absorbance vs concentration of nitrite graph is obtained for a set of data:
Absorbance Vs Concentration y = 1.6628x+0.0373
R? = 0.9893
1.8
1.6
1.4
1.2
1
0.8
0.6
0.4
0.2
0.2
0.4
0.6
0.8
1
Concentration of nitrite (mg/L)
Determine the concentration of unknown solution for which the absorbance is determined
as 0.69
A. More data is required
В. 0.69
С. 0.65
D. 0.39
Absorbance
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How do I find Concentration?
flask
Calculate solution Concentration (M)
Volume stock of 0.40 M CuSO4 (ml)
Volume of flask (ml)
Absorbance at 635 nm(a.u.)
1
2.0
10
.185
2
4.0
10
.362
3
6.0
10
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4
8.0
10
.674
5
10.0
10
.843
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line of best fit. y=0.001x + 0.1987, absorbance is 1.29.
Calculate the concentration of your sample. units must be ug/mL
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[CV] / M A
1.0 × 10–6 M 0.250
3.0 × 10–6 M 0.750
Question 12 options:
4.5 × 10–6 M
5.0 × 10–6 M
5.5 × 10–6 M
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