You obtained the following raw data when setting up a Bradford standard curve:BSA (mg/ml) Absorbancy595nm0.22510.3100.4200.5100.6100.72060.81070.91580.9506.0.980100.990Set up a standard curve.What would the quality of the line-fit (R2 value) be if you do not exclude experimental outliers?(Give you answer to 4 decimal places)4.

Bradford protein assay is a method which is used for determining the concentration of unknown…

You obtained the following raw data when setting up a Bradford standard curve: BSA (mg/ml) Absorbancy 595nm 0.225 1 0.310 0.420 3. 0.510 4 0.610 0.720 0.810 0.915 8 0.950 0.980 10 0.990 Set up a standard curve. What would the quality of the line-fit (R2 value) be if you do not exclude experimental outliers? (Give you answer to 4 decimal places) 5, 6, 7.

You obtained the following raw data when setting up a Bradford standard curve: BSA (mg/ml) Absorbancy 595nm 0.225 1 0.310 0.420 3. 0.510 4 0.610 0.720 0.810 0.915 8 0.950 0.980 10 0.990 Set up a standard curve. What would the quality of the line-fit (R2 value) be if you do not exclude experimental outliers? (Give you answer to 4 decimal places) 5, 6, 7.

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter9: Atomic Absorption And Atomic Fluorescence Spectrometry

Section: Chapter Questions

Problem 9.16QAP

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You obtained the following raw data when setting up a Bradford standard curve: BSA (mg/ml) Absorbancy 595nm 0.225 1 0.310 2 0.420 3 0.510 0.610 5 0.720 6 0.810 7 0.915 8 0.950 9 0.980 10 0.990 Set up a standard curve. What would the quality of the line-fit (R2 value) be if you do not exclude experimental outliers? (Give you answer to 4 decimal places) LO
3. The lead in a swab sample, lead standards, together with a blank were made up in 5.00 mL volumetric flasks using 0.2 % HNO3. 20 μL aliquots of these solutions were injected into the spectrophotometer and the absorbance measured at 217 nm. The following results were obtained. lead / ppb Absorbance 0 0.0591 10.00 0.0858 50.00 0.1926 100.0 0.3260 150.0 0.4594 200.0 0.5929 Swab sample 0.3700 (a) Determine the amount of lead in the swab sample in μg.
The absorbance of an unknown dye solution is measured to be 1.06 by a spectrometer. The calibration plot of the spectrometer is provided below. What is the molar concentration of the unknown sample (in mole L)? Absorbance vs. Molarity 18 y3 67024x-0.0343 16 14 12 1 0.8 0.6 0.4 0.2 01 0.2 0.000005 00001 0000015 Concentration of solutions, mol/L 0.00002 0.000025 000003 0 163e-5 O 2.35e-6 0 163 0 235 Absorbance
To test a spectrophotometer’s accuracy, a solution of 60.06 ppm K2Cr2O7 is prepared and analyzed. This solution has an expected absorbance of 0.641 at 350.0 nm. Several aliquots of the solution produce the following absorbance values. 0.640    0.638    0.640    0.639    0.640    0.639    0.638 is there any significant difference between the experimental mean and the expected value at a 99.9% confidence level? Question 21 options: Yes because tcal<tcritical Yes because tcal>tcritical No because tcal<tcritical No because tcal>tcritical
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.
10 Wavelength, 1. (nm) E (Red, µ.Mcm- ɛ(Yellow, µMr'cm¬1) Absorbance 500 0.0369 0.000549 0.405 430 0.00506 0.0167 0.474 An orange colored solution is prepared by mixing a red dye solution with a yellow dye solution and the absorbance was measured at the analytical wavelengths of 430 nm and 500 nm. The table provides the molar absorptivity for the red and yellow dye at each analytical wavelength. Calculate the concentration (in u.M) of the red and yellow dye in the mixture. [red] = [yellow] =
After determining the absorbance of several standards of known concentration, the trendline for a calibration curve (AKA a standard curve) plotting absorbance (y-axis) against concentration (M, x-axis) is determined to be y = 4.943x + -0.0001 The absorbance of a solution of unknown concentration is determined to be 0.48. Calculate the concentration of the unknown solution in M. Give your answer to three decimal places.
After creating her standard curve for absorption versus the concentration (M) of FD&C Red 40, a student found that her best fit linear line for FD&C Red 40 was y = 2,681x + -0.002. Her Kool-Aid sample had an absorbance of 0.337. If 0.55 grams of Kool-Aid powder was used to prepare an 8-fl oz cup of her assigned flavor, what is the percent by mass of FD&C Red 40 in her 8-fl oz cup?
A solution is prepared by diluting 2.79 mL of the blue dye stock solution to 25.00 mL. The measured absorbance for the prepared solution is: Blue dye stock solution = 0.293 M Absorbance at 630 nm = 0.00265 Calibration curve y = 0.0833x A.) What is the theoretical molar concentration? B.) What is the experimental molar concentration? C.) What is the percent error?
A liquid sample was analyzed for Fe³+. A plot of absorbance (y-axis) vs. concentration (ppm; x-axis) of the external standards produced a calibration line with an equation y = 0.2256x -0.0903 (R² = 0.9973). The absorbance of the sample was 1.25. Determine the amount of Fe³+ in the sample (in ppm).
The validation process comprises four main steps that are : hardware validation, software validation, method validation and system suitability. To evaluate a spectrophotometer’s accuracy by measuring absorbance, a solution of 60.06 mg/L K2Cr2O7 in 0.0050M H2SO4 was carefully prepared together with a 0.0050 M H2SO4 as a reagent blank. If the spectrometer’s signal is properly calibrated, it has been reported that this solution should provide an absorbance of 0.640 +- 0.010 at wavelength 350 nm. Which one of the validations mentioned above had been involved in this process? Explain your choice
A student prepared four standard solutions of (NH4)2Fe(SO4)2 and measured their absorbance at 505 nm. She created a calibration plot with the best-fit line of y = 9372 x + 0.0539. She measured the absorbance of her diluted unknown sample solution as (4.69x10^-1) nm. If she prepared her diluted sample solution by diluting 10.00 mL of the original solution to a total volume of 50.00 mL with deionized water, what is the concentration of Fe2+ in her original solution? Answer in units of M. Note: Your answer is assumed to be reduced to the highest power possible.