Science
CHEM110L Stevenson University Spectrometric Analysis of Cobalt Lab Report

CHEM110L

Stevenson University

Question Description

please read the attachments before writing the report.

Read the instructions that we followed for lab experiment to know the tools we used and the chemicals.

Also read the attached slides which is also about separation of a mixture of solid, it will help.

Report sheet are attached which include all the data that we collected for this lab report.

Report Style:

1-Cover Page (50 points)

2-Introduction (50 points) (should include what is the lab about, how the report will cover the experiment. General information about the topic)

3- Typed data and observations (400 points) (should include all the data attached as report sheet with further information like what you think of the reaction and how we got these numbers. Also, pictures while doing the experiment will be attached)

4- What's Up (200 points) (how can we involve this experiment in our daily life in engineering) ( a real life example in engineering)

5-Conclusion (100 points) (explanation of the experiment and what you learn from this experiment and what you think) (explosions of how you thing the data are, and explain what error occurred in the experiment)

(More pictures will be attached for during the experiment)

(Example of the complete work will be attached

(There will be a plagiarism check)

CHEM110L Stevenson University Spectrometric Analysis of Cobalt Lab Report
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CHEM110L Stevenson University Spectrometric Analysis of Cobalt Lab Report
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CHEM110L Stevenson University Spectrometric Analysis of Cobalt Lab Report
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CHEM110L Stevenson University Spectrometric Analysis of Cobalt Lab Report
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CHEM110L Stevenson University Spectrometric Analysis of Cobalt Lab Report
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CHEM110L Stevenson University Spectrometric Analysis of Cobalt Lab Report
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Unformatted Attachment Preview

Spectrometric Analysis of Cobalt(II) Chloride by Me & ? Get the Following: 1. 8 small test tubes 2. 1 water bottle 3. 25 mL 0.150 M CoCl2 in a 50 mL beaker 4. 50 mL water in a medium size beaker 5. 2 disposable pipets 6. 10 mL graduated cylinder 7. 1 spectrometer 8. 1 calculator 9. 25 mL of unknown after approval 10. Make sure your Spec 20 is turned on Fill each test tube with the following Calculate the concentration of CoCl2 in each test tube , and record your results in the table Tube #1 #2 #3 #4 #5 #6 #7 mL of 0.150 M CoCl2 mL of distilled water V 1 = 5.0 0.0 V 2 = 4.0 1.0 V 3 = 3.0 2.0 2.5 V 4 = 2.5 V 5 = 2.0 3.0 V 6 = 1.5 3.5 V 7 = 1.0 4.0 Concentration C 1= V1(0.030 M/mL) C 2= V2(0.030 M/mL) C 3= V3(0.030 M/mL) C 4= V4(0.030 M/mL) C 5= V5(0.030 M/mL) C 6= V6(0.030 M/mL) C 7= V7(0.030 M/mL) MaVa = MbVb Vb = V(H20) + V(CoCl2) Va = V(CoCl2) Ma = Concentration of CoCl2 = 0.150 M Ma/ Vb = 0.030 M/mL Mb = Concentration of diluted CoCl2 1. 2. 3. 4. 5. 6. 7. 8. Adjust your wavelength to 512 nm Adjust your dark current to zero percent transmission using the zero adjust Insert your test tube 8 with pure distilled water into the sample holder Adjust your light control to 100% transmission Remove you test tube 8, and insert your test tube 1 Change your mode from transmission to absorbance Record your absorbance for sample # 1 on your table next to its concentration Repeat for samples #2 - #7 1. Plot your concentration versus absorbance on the computer, and record the slope under the table which had the data that generated it. 2. Your slope should equal something like k = 5.1 1/M 3. Pick up you unknown, and remake it as you did the standard solution Use the table in your lab manual (or use your calculation page) to record your unknown data and pick the best four for your report Tube #1 #2 #3 #4 #5 #6 #7 mL of unknown CoCl2 V 1 = 5.0 V 2 = 4.0 V 3 = 3.0 V 4 = 2.5 V 5 = 2.0 V 6 = 1.5 V 7 = 1.0 mL of distilled water 0.0 1.0 2.0 2.5 3.0 3.5 4.0 Unknown Concentration of Absorbance diluted unknown A1 C 1 = A 1 /k A2 C 2 = A 2 /k A3 C 3 = A 3 /k A4 C 4 = A 4 /k A5 C 5 = A 5 /k A6 C 6 = A 6 /k A7 C 7 = A 7 /k Concentration of unknown before dilution C 1(5.0 mL)/V1 = M1 C 2(5.0 mL)/V2 = M2 C 3(5.0 mL)/V3 = M3 C 4(5.0 mL)/V4 = M4 C 5(5.0 mL)/V5 = M5 C 6(5.0 mL)/V6 = M6 C 7(5.0 mL)/V7 = M7 1. Complete the chart for your unknown concentration by using the best four results 2. Show your calculations for your best four on your report page as well as your calculation page 3. Find the average concentration 4. For extra credit you can do standard deviation Find the deviation from the mean = di = i - Add all four deviation together after squaring them = Divide by n-1 = 4 – 1 = 3. This will give you the variance To find the standard deviation, take + or – the square root of the variance Graph from http://www.comfsm.fm/~dleeling/statistics/text5.html ...
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Final Answer

Here it is. I used the report you sent as a template. It should be good. I have already done the cover, I included it. I did not modify any data or calculations you made. Let me know if you need anything else.

CHEM 110L-002

General Engineering Chemistry I
Fall, 2019
(SPECTROMETRIC ANALYSIS OF COBALT (II) CHLORIDE)

Student Name: Omar Salman

Date: 20/11/2019

Introduction
The measurement of UV-Vis radiation absorption gives a reliable and easy method to analyze
several organic and inorganic compounds. Radiation in this region of the electromagnetic spectrum
has enough energy to induce electronic transitions of the valence electrons of several compounds.
In this quantitative technique a solution is irradiated with a beam, being able to measure how much
radiation was absorbed (absorbance) in a spectrometer. The absorbance is directly related to the
concentration of the analyte and therefore we can determine the concentration of unknown
solutions by using the Beer-Lambert’s Law.

𝐼

log 𝐼 𝑇 = 𝐴𝑏𝑠 = 𝜀 × 𝑏 × 𝑐 Beer’s Law
𝑂

The Beer’s Law states that the absorbance is directly proportional to the concentration of the
solution and the thickness of the container. Since in the experiment the cell used will be the same
all along and the constant ε does not change since it’s the same compound, the term 𝜀 × 𝑏 can de
considered a constant and the equation can be rewritten as:
𝑨𝒃𝒔 = 𝑲 × 𝒄
Experimentally, a series of solutions with known concentration will be prepared and their
absorbances measured in a spectrometer (Spectronic 20), then the concentration vs. the absorbance

will be plotted in what is commonly referred to as a calibration curve. Calculating the slope of the
straight, if the Beer’s law applies, we can determine the constant K by comparing the equations:

𝑨𝒃𝒔 = 𝑲 × 𝒄 𝑖𝑠 𝑒𝑞𝑢𝑖𝑣𝑎𝑙𝑒𝑛𝑡 𝑡𝑜

𝒚 = 𝒎𝒙 + 𝒃

𝑤ℎ𝑒𝑟𝑒 𝑚 = 𝑘 = 𝑠𝑙𝑜𝑝𝑒

...

jlco88 (806)
Rice University

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