Chromatography Lab Report

Graph ? ?  the table and find X1 valeu.

can you explain how I can get 1.596 mg/L of concentration of Fe3+ in dilutes sample and can you also make the calibration curve.

3.

Please complete Table 2 and show the calculations for protein concentration and the concentration of the undiluted sample.  a). Using Excel software, enter data from Table 1 to plot a standard curve (corrected average absorbance on Y-axis and protein concentrations on X-axis). The standard curve must contain correct labels on both axes. b). From the standard curve, obtain a best fit line and equation. c). Use the best fit equation and data from Table 2 to find the concentrations of proteins in sample A2-D2 and E1.  [onto your plotted standard curve, indicate where A595 of A2-D2 and E1 are located]  d). Calculate the concentrations of proteins in undiluted samples A to E. Thank you very much.

SPECTROPHOTOMETRY Two groups in a BIO 120 lab extracted a blue-violet pigment from mayana plant which was to be used as a natural dye for Philippine textiles. To determine the concentration of the pigment isolated, each group made a standard curve using commercially available indigo dye in dimethylsulfoxide (DMSO). The following data were obtained by the two groups: Table 4. Absorbance readings of standard solutions of varying concentrations of indigo dye in DMSO. Pure DMSO 0.115 Standard solutions (ppm) Group 1 Data Group 2 Data 0.2 0.398 0.224 0.4 0.563 0.437 0.6 0.732 0.603 0.8 0.833 0.811 1.0 1.008 0.966 1. Show the constructed standard curves of the two groups with proper figure titles. 2. Which of the two groups generated a better standard curve? Justify your answer by providing the R? value for each data set. 3. The extracted pigment has an absorbance of 0.983. When a 0.2 mL-aliquot of the extract was diluted to 1.0 mL, the absorbance of the diluted solution was found to be…

A student weighed out 0.150 g of protein powder and dissolved it in 100 mL of water (Solution 1). The student then diluted this solution by transferring 1 mL into a 25 mL flask and diluting with water (Solution 2). Finally, 1 mL of that solution was transferred to a test tube and combined with 4 mL Bradford reagent. The absorbance of the solution in the test tube was 0.11. Assuming that the best fit linear line of the standard curve was y = 0.04144 x + 0.01521 (μ g mL), calculate the percent protein by mass in the original protein powder.

use the following chromatogram and table as your data.       What is the %composition of the Vitamin A peak in the sample?     78.43%        77.73%     7.867%       72.74%

A sample is going to be analyzed for trace amounts of ibuprofen using gas chromatography. Which of the following detectors would work best for the detection of ibuprofen? ibuprofen.png Group of answer choices alkali flame detector thermal conductivity detector flame ionization detector flame photometric detector sulfur chemiluminescence detector electron capture detector

Compare and contrast the amount of caffeine obtained from the single vs multipleextractions with Red Bull and Coca-Cola beverages. Explain why this has occured. Single Extractions:       TEST SOLUTION NAME      ABSORBANCE READING          [CAFFEINE]mg/100ml 5ml Red Bull                         2.412                  57.9mg/100ml 5ml Coca-Cola                         0.716                  16.2mg/100ml   Multiple Extractions:      TEST SOLUTION NAME        ABSORBANCE READING           [CAFFEINE]mg/100ml 10ml Red Bull                    3.253                 78.453mg/100ml 10ml Coca-Cola                     0.785                 17.844mg/100ml

Which one of the following techniques cannot be used to measure the amount of Ni in a sample? O gas chromatography visible light spectrometry voltammetry ICP-MS O atomic absorption spectrometry

Here is the protocol for a UV-Vis spectrophotometer to detect water and chlorine-carbon. 1.Dissolve the water and chlorine-carbon compounds in a solvent, such as water. 2.Prepare a standard solution of known concentration that is similar to the sample being measured. 3.Calibrate the spectrophotometer using the standard solution. 4.Measure the absorbance of the sample using the spectrophotometer. 5.Calculate the concentration of the compounds in the sample using the calibration curve obtained from the standard solution. How is the spectrophotometer calibrated with standard solutions? When is the blank solution placed in the spectrophotmeter?

A student weighed out 0.150 g of protein powder and dissolved it in 100 mL of water (Solution 1). The student then diluted this solution by transferring 1 mL into a 25 mL flask and diluting with water (Solution 2). Finally, 1 mL of that solution was transferred to a test tube and combined with 4 mL Bradford reagent. The absorbance of the solution in the test tube was 0.144. Assuming that the best fit linear line of the standard curve was y=0.04144x+0.01521 (μgmL), calculate the percent protein by mass in the original protein powder.

Record your absorbance data for the YELLOW and RED dyes below. Calculate the dye concentration in mM for each cuvette using M1V2 = M2v2 . Remember the concentration of stock solutions (100^ % dye) is 0.020 mM(mM= millimolar =mm /L). Data for YELLOW: peak absorbance used on spectrophotometer =420nm Cuvette 1 - 100% dye = 0.680 absorption Cuvette 2 - 75% dye = 0.510 absorption Cuvette 3 - 50% dye = 0.340 absorption Cuvette 4 - 25% dye = 0.170 absorption Data for RED - peak absorption used on spectrophotometer = 500nm Cuvette 1 - 100% dye: 0.621 absorption Cuvette 2 - 75%: 0.466 absorption Cuvette 3 - 50% dye: 0.311 absorption Cuvette 4 - 25% dye: 0.1555 absorption

Based on the data, calculate the concentration of analyte in the ORIGINAL sample in ppm. Report to 1 decimal place Sample: A 10.00 mL aliquot of the unknown was placed in a 100.0 mL volumetric flask and made up to the mark will distilled water. The absorbance of this solution is 0.185. Sample + Spike: A 10.00 mL aliquot of the unknown and a 13.00 mL aliquot of the 46.00 ppm stock were both placed in the same 100.0 mL volumetric flask and diluted to the mark with water. The absorbance of this solution is 0.326.   ( Please type answer note write by hend)

If the stationary phase and the compound being tested are both polar, will the retention factor (Rf) likely be smaller or larger than if a nonpolar compound was tested? Why? 1) The retention factor will likely be smaller as it has a smaller interaction with the stationary phase O 2) The retention factor will likely be greater as it has a smaller interaction with the stationary phase O3) The retention factor will likely be smaller as it has a greater interaction with the stationary phase 4) The retention factor will likely be greater as it has a greater interaction with the stationary phase

The concentration of methylene blue in the sample is estimated through (select the correct)   options:   refractive index measurement (refractometry).   turbidity measurement (turbidimetry).   absorbance measurement (spectrophotometry).   titration with 2% HCl solution.

The aspirin we made in lab gad 125-133 melting point and I attached the IR. Base on this information, does it mean we made aspirin? The percent yield was also less than 50. Is that acceptable? Is this aspirin pure or not? please explain your answer.