Lab 4 REPORT Gregory Chekerdjian

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Purdue University *

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11500

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Chemistry

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Feb 20, 2024

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Lab 4: How Can Absorption of Light be Used to Determine Concentration of a Compound in Solution? REPORT FORM Answer the following discussion questions. Support your claim using evidence, i.e., experimental data and/or observations that support the claim. Cite specific quantitative results. Connect your evidence (data and/or observations) to your claim using reasoning that explains why your evidence supports your claim. Reasoning should be based on a scientific rule, law, principle or definition. Question #0. Insert a table or a photo of your data sheet from lab below. My groups data: Other two groups data: Question #1. Write the equation of the chemical reaction used to convert Fe 2+ to a colored species. Include states of matter in your equation. Fe ( aq ) 2 + ¿ + 3 Phen ( aq ) ¿¿ λmax = 508 m
Question #2. Insert a screenshot of your absorption spectrum and label the wavelength of maximum absorbance you used for your experiments. You can label λ max on the graph with a stylus or a text-box if needed. Question #3. Provide a sample calculation for the concentration of Fe(phen) 3 2+ in standard solution 1. Include work, units, molar ratio and appropriate significant figures. You will receive no credit if you use M 1 V 1 = M 2 V 2 unless you specifically state the molar ratio of components. For the molar ratio, consider that the reagent you used for the standard solutions was prepared from (NH 4 ) 2 Fe(SO 4 ) 2 , and the compound for which you measured the absorbance was Fe(phen) 3 2+ . In other words, what is the molar ratio of (NH 4 ) 2 Fe(SO 4 ) 2 to Fe 2+ to Fe(phen) 3 2+ ? For full credit, you must state or include the molar ratio(s) in your sample calculation. Question #4. Insert a screenshot of your calibration plot (standard curve) with the best-fit line. Include a title, axis labels and R 2 value. These components can be written on the graph with a stylus or a text-box if needed. Question #5 Use your calibration plot (not the line equation) to estimate the concentration of a solution if the absorbance value was 0.500. Show or explain how you estimated the concentration, and what your reasoning was behind your method. One option is to draw lines and/or mark on your calibration plot as part of your explanation. Title: How does the change in concentration (mol/L) influence the absorbance (nm) at its maximum height R 2 = 0.978 Although I would have liked to use an iPad to draw on the calibration plot I couldn’t because I did not have access to one however, I was still able to get a estimate of the concentration of a solution. If the chosen solution had a absorbance value of 0.500 then the concentration would be around 2.4 * 10 -4 . I understand that this number seems off but as I mentioned before I made a mistake when calculating the concentration of each standard.
Question #6. Using the absorbance value for unknown solution A and your line equation, calculate the concentration of Fe 2+ in your diluted sample solution of unknown A. Then, calculate the concentration of Fe 2+ in the original solution of unknown A (i.e. the undiluted solution from the reagent bottle). Include work, units, molar ratio and appropriate significant figures. For the molar ratio, remember that you measured the absorbance of Fe(phen) 3 2+ , but you are asked to solve for the concentration of Fe 2+ . In other words, what is the molar ratio of Fe(phen) 3 2+ to Fe 2+ ? For full credit, you must state or include the molar ratio in your sample calculation. Question #7. Compare the experimental concentration of Fe 2+ you determined to the actual value provided by your instructor. Show a calculation to support your answer. (Hint: Which formula from Lab 1 is appropriate for this comparison?) Explain what might have contributed to a difference between your value and the actual value. Molar ratio is 1:1 Using the equation of y = mx + b we plugged in all the known values from our graph and the absorbance of unknown A and B to get the x value which is the concentration. Solution A ¿ 1.95 10 4 3.36 10 4 3.36 10 4 ¿ 0.41 100 = 41% Solution B ¿ 4.14 10 4 6.85 10 4 6.85 10 4 ¿ 0.39 100 = 39% The reason why there was such a large percent error was because I made a mistake with the calculations of my concentration. The other issue that caused such a large percent error was human error as we might have poured more of unknown A. In order to get the most reliable average value of the Fe 2+ concentration of the unknown we should find the average of each groups slope intercept equation. It would help us get the most accurate values since we might have all done little errors with our graphs and we did not all choose the maximum wavelength. We also know that finding the average of several trials is much better then only using one trial. Although not necessary I think having a new calibration plot with the averages of everything would be better since all our values would have slightly changed.
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Question #8. Which values in the Fe 2+ concentration results from your group and other groups would you use to calculate a reliable average value of the Fe 2+ concentrations of the unknown solutions? Explain the criterion you used to decide which values could/could not be used to calculate a reliable average. Would you need to construct a new calibration plot to use absorbance data from other groups to calculate Fe 2+ concentration? Question #9. In this analysis, you made inferences about the concentration of Fe 2+ using absorbance measurements of Fe(phen) 3 2+ solutions. What assumption(s) about the reaction between Fe 2+ and “phen” did you make for this analysis? (Hint: the assumption is provided in the lab instructions). Question #10. Why should you measure the absorbance of the solution with the lowest concentration first? What error or errors could occur if you started from the most concentrated solution? “The intensity of the color of the solutions is directly related to the concentration of Fe(phen)32+ in the solutions. Using the concentration of Fe(phen)32+ in the solution, you can calculate the concentration of Fe2+ in the original sample since the molar ratio of Fe2+ to Fe(phen)32+ is 1:1.” The assumption is that we would have to use a 1 to 1 ratio and it will let us make the inferences about the unknown solutions. We would measure the solution of the lowest concentration first since it has the lowest maximum wavelength compared to the other solutions. By measure the lowest concentration we would be able to minimize the error. If we started with the most concentrated solution the maximum wavelength would be higher thus causing the percent error to be larger.