Homework Answers
The calibration graph is drawn.
The equation of best fit line is y = 7877.1x + 0.01
where y represents absorbance and x represents concentration
![Chart Tools Home Page Layout Formulas Data Rview Vew Design Layout Format Chart 1 1 [Fe(NCS12t] (M Absorbance 20.0000179 3 0.0000358 4 0.0000537 S 0.0000716 0.15 0.3 0.42 0.58 Calibration graph: Absorbance vs Concentration 0.7 0.6 0.5 12 13 0.4 15 17 0.3 Best fit line 19 y-7877.1x+0.01 21 0.2 0.1 27 0.00001 0.00002 0.00003 0.00004 0.00005 0.00006 0.00007 0.00008 concentration of [FeINCS)2+] (M) 31 32 4 She Ready Recovered Sheet2 Sheet3 Average: 0.181272375 Count: 10 Sum: 1.450179 Em 100%](http://img.homeworklib.com/questions/14fd8330-1c13-11ec-afd6-65edc916c50a.png?x-oss-process=image/resize,w_560)
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4. Having prepared all of your solutions, take all five of them to the spectrophotometer which...
How can the colouration (or lack thereof) of the solutions be explained? How would you expect...
How can the colouration (or
lack thereof) of the solutions be explained?
How would you expect DELTAO to change as the number of L ligands
about the metal increases or decreases, and why?
UJUS ML PULUUPIUIUMLILI There are several types of spectrophotometers. Be sure to ask the instructor if you are unsure how to use the one you are assigned. You will be measuring absorbances at different wavelengths so it is essential to know how to quickly adjust the settings...
Take three cuvettes from the Containers shelf and place them onto the workbench. Take an Erlenmeyer...
Take three cuvettes from the Containers shelf and place them onto the workbench. Take an Erlenmeyer flask from the Containers shelf and place it onto the workbench. There is a solution on the Materials shelf labeled 2% starch. This has a starch concentration of 1 mg/ml. In the Erlenmeyer flask, you should create 100 mL of a new starch solution that is 1/400th of the stock solution using water as the filler. How much starch and water should you add?...
I had clearer images. Part 1 - Making Standard solutions. 1. Into a clean, dry beaker...
I had clearer images.
Part 1 - Making Standard solutions. 1. Into a clean, dry beaker combine the solutions from the table for each calibration solution using the appropriate pipettes. Pour the contents of the beaker into a provided cuvettes (do not fill the cuvettes to the top). Pour any excess from the sample beaker into a waste beaker, rinse the sample beaker, and continue making solutions until you have the blank and four solutions for the calibration. Calibration Solution...
Beer’s Law Objective : We will explore an application of absorption spectroscopy using calibration curves and...
Beer’s Law Objective : We will explore an application of absorption spectroscopy using calibration curves and Beer’s Law. Use the “LAB : HOW TO…” link from the class website if you need help with how to use balance, Bunsen burner… and such. Introduction: You may write this information in your lab notebook for your own reference. It can’t be cut and pasted. Different solutions have different spectral properties. In this portion of the experiment those properties will be utilized to...
I am stuck on how to find concentration for standards and unknowns. Any kind of help would be appreciated. The correct...
I am stuck on how to find concentration for standards and
unknowns. Any kind of help would be appreciated.
The corrected absorbance is = Blank - absorbance
1. Prepare the BCA working reagent. Use a graduated cylinder and add 30 ml of the BCA reagent into a 50 ml Erlenmeyer flask. Use the appropriate micropipette to add 600 uL of the CuSO4 solution into the flask and mix by swirling the flask. Record the exact mass of albumin and the...
7. The Absorption Spectrum of Cobalt(II) Chloride Procedure Getting Started 1. Your laboratory instructor may ask...
7. The Absorption Spectrum of Cobalt(II) Chloride Procedure Getting Started 1. Your laboratory instructor may ask that you work in groups rather than alone. 2. Obtain directions from your laboratory instructor for discarding the solutions that you will use in'! this experiment. 3. Obtain instructions for using your spectrophotometer. 4. Obtain your unknown. Making the Measurements 1. Mark each of 7 dry 18 x 150-mm test tubes with one of a series of identification numbers running from 1 to 7....
Calculate initial concentration of Fe+3 for tubes 1-3. Show your work. Procedure A. Determination of B...
Calculate initial concentration of Fe+3 for tubes 1-3. Show your
work.
Procedure A. Determination of B for Beer's Law 1. Using a buret, add 4.00 mL of 0.0025 M Fe(NO3)s (which is in 0.1 M HNOs) to a 100- mL volumetric flask. Add enough deionized water to bring the total volume to the mark on the neck of the flask. Stopper and shake the flask. Label this flask “Diluted Fe.” spectrophotometer tubes (cuvettes), they are too small to use at...
Part C. Quantitative Spectroscopy Wavelength(A) Absorbance Amax-10 Amax 10 Wavelength used for Analysis in Part C:...
Part C. Quantitative Spectroscopy Wavelength(A) Absorbance Amax-10 Amax 10 Wavelength used for Analysis in Part C: Solution Concentration Absorbance % Transmittance Standard 1 Standard 2 Standard 3 Standard 4 Unknown 0.20 M Show an example calculation obtaining the molarity of the standards. a. Copper Standard 2: Obtain additional 0.20 M CuSO4 solution from the tray. Pipet 10 mL of 0.20 M CuSO4 solution into a 50 mL Erlenmeyer flask. Pipet 10 mL of DI water into the same tube and...
PROCEDURE A. ABSORBANCE SPECTRA 1. Obtain three cuvettes. Add-2mL of the following samples to them: red...
PROCEDURE A. ABSORBANCE SPECTRA 1. Obtain three cuvettes. Add-2mL of the following samples to them: red dye, blue dye, yellow dye. 2. Obtain a spectrum for each dye according to the provided directions (water is the blank). 3. For each of the three dyes (red, yellow, and blue) record the wavelength for the largest peak in the visible range (380 nm to 750 nm), Record this in the data table below. Save the red dye for part B. 4. Identify...
all questions EXPERIMENT 8 Spectrophotometric Study of an Equilibrium Reaction Since known amounts of iron(III) and...
all questions
EXPERIMENT 8 Spectrophotometric Study of an Equilibrium Reaction Since known amounts of iron(III) and thiocyanate will be mixed, and the concentration of the iron-thiocyanate complex determined spectrophotometrically, it will be possible to cal- culate the equilibrium constant for each of the three possible equilibrium reactions above. The reaction which gives a constant value of K, for all the solutions prepared will be the correct one under the experimental conditions. AGRERERERLER . 1 Procedure 1. Clean and dry five...
How can the colouration (or
lack thereof) of the solutions be explained?
How would you expect DELTAO to change as the number of L ligands
about the metal increases or decreases, and why?
UJUS ML PULUUPIUIUMLILI There are several types of spectrophotometers. Be sure to ask the instructor if you are unsure how to use the one you are assigned. You will be measuring absorbances at different wavelengths so it is essential to know how to quickly adjust the settings...
I had clearer images.
Part 1 - Making Standard solutions. 1. Into a clean, dry beaker combine the solutions from the table for each calibration solution using the appropriate pipettes. Pour the contents of the beaker into a provided cuvettes (do not fill the cuvettes to the top). Pour any excess from the sample beaker into a waste beaker, rinse the sample beaker, and continue making solutions until you have the blank and four solutions for the calibration. Calibration Solution...
I am stuck on how to find concentration for standards and
unknowns. Any kind of help would be appreciated.
The corrected absorbance is = Blank - absorbance
1. Prepare the BCA working reagent. Use a graduated cylinder and add 30 ml of the BCA reagent into a 50 ml Erlenmeyer flask. Use the appropriate micropipette to add 600 uL of the CuSO4 solution into the flask and mix by swirling the flask. Record the exact mass of albumin and the...
7. The Absorption Spectrum of Cobalt(II) Chloride Procedure Getting Started 1. Your laboratory instructor may ask that you work in groups rather than alone. 2. Obtain directions from your laboratory instructor for discarding the solutions that you will use in'! this experiment. 3. Obtain instructions for using your spectrophotometer. 4. Obtain your unknown. Making the Measurements 1. Mark each of 7 dry 18 x 150-mm test tubes with one of a series of identification numbers running from 1 to 7....
Calculate initial concentration of Fe+3 for tubes 1-3. Show your
work.
Procedure A. Determination of B for Beer's Law 1. Using a buret, add 4.00 mL of 0.0025 M Fe(NO3)s (which is in 0.1 M HNOs) to a 100- mL volumetric flask. Add enough deionized water to bring the total volume to the mark on the neck of the flask. Stopper and shake the flask. Label this flask “Diluted Fe.” spectrophotometer tubes (cuvettes), they are too small to use at...
Part C. Quantitative Spectroscopy Wavelength(A) Absorbance Amax-10 Amax 10 Wavelength used for Analysis in Part C: Solution Concentration Absorbance % Transmittance Standard 1 Standard 2 Standard 3 Standard 4 Unknown 0.20 M Show an example calculation obtaining the molarity of the standards. a. Copper Standard 2: Obtain additional 0.20 M CuSO4 solution from the tray. Pipet 10 mL of 0.20 M CuSO4 solution into a 50 mL Erlenmeyer flask. Pipet 10 mL of DI water into the same tube and...
PROCEDURE A. ABSORBANCE SPECTRA 1. Obtain three cuvettes. Add-2mL of the following samples to them: red dye, blue dye, yellow dye. 2. Obtain a spectrum for each dye according to the provided directions (water is the blank). 3. For each of the three dyes (red, yellow, and blue) record the wavelength for the largest peak in the visible range (380 nm to 750 nm), Record this in the data table below. Save the red dye for part B. 4. Identify...
all questions
EXPERIMENT 8 Spectrophotometric Study of an Equilibrium Reaction Since known amounts of iron(III) and thiocyanate will be mixed, and the concentration of the iron-thiocyanate complex determined spectrophotometrically, it will be possible to cal- culate the equilibrium constant for each of the three possible equilibrium reactions above. The reaction which gives a constant value of K, for all the solutions prepared will be the correct one under the experimental conditions. AGRERERERLER . 1 Procedure 1. Clean and dry five...
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