Bradford protein assay. The tubes contained the following amounts of the BSA solution: 0, 20, 40, 60, 80, 100 μL. Each sample then had water added to make the final volume 100 μL. The corresponding absorbencies after adding Bradford reagent were the following: 0, 0.05, 0.09, 0.14, 0.19, and 0.22. If you took 20 μL of an unknown and added 80 μL of water, mixed, took 10 μL of the mixture and 90 μL of water and added the Bradford reagent and saw an absorbance of 0.08, what was the protein concentration of the undiluted unknown to one decimal place?

Bradford protein assay. The tubes contained the following amounts of the BSA solution: 0, 20, 40, 60, 80, 100 μL. Each sample then had water added to make the final volume 100 μL. The corresponding absorbencies after adding Bradford reagent were the following: 0, 0.05, 0.09, 0.14, 0.19, and 0.22. If you took 20 μL of an unknown and added 80 μL of water, mixed, took 10 μL of the mixture and 90 μL of water and added the Bradford reagent and saw an absorbance of 0.08, what was the protein concentration of the undiluted unknown to one decimal place?

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter9: Complexometric And Precipitation Titrations

Section: Chapter Questions

Problem 17P

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You obtained the following raw data when setting up a Bradford standard curve: BSA (mg/ml) Absorbancy 595nm 0 0.225 1 0.310 2 0.420 3 0.510 4 0.610 5 0.720 6 0.810 7 0.915 8 0.950 9 0.980 10 0.990 After blanking against a bradford-dH2O sample, the protein concentration of an unknown sample was determined using the same method and an absorbancy of 0.523 was obtained. Set up a standard curve, excluding outliers (experimental and statistical) and determine the protein concentration in the unknown sample in mg / ml (up to 3 significant figures).
Biuret Assay accurately quantify protein concentration within the range of 5-150 mg/mL. JUSTIFY THE STATEMENT.
You obtained the following raw data when setting up a Biuret standard curve: BSA (mg/ml) Absorbancy 540nm 0 0.158 1 0.210 2 0.260 3 0.305 4 0.360 5 0.410 6 0.455 7 0.510 8 0.530 9 0.550 10 0.554 After blanking against a biuret-dH2O sample, the protein concentration of an unknown sample was determined using the same method and an absorbancy of 0.251 was obtained. Set up a standard curve, excluding outliers (experimental and statistical) and determine the protein concentration in the unknown sample in mg / ml (up to 3 significant figures).
A 50.0 mL juice extract is colorimetrically assayed using Nelson’s test. One milliliter (1.00 mL) of the solution and the standard glucose solution (concentration: 1mg/mL) were treated with freshly prepared Nelson’s reagent and arsenomolybdate reagent and then diluted to 10.0 mL separately in properly labeled test tubes. Absorbance at 480 nm for the standard is 1.702 and for the sample, 0.926. A. What is the principle behind the assay? B. Calculate the concentration of the reducing sugar in the 50.0 mL sample in mg/mL. Apply Beer-Lambert’s law.
A 50.0 mL juice extract is colorimetrically assayed using Nelson’s test. One milliliter (1.00 mL) of the solution and the standard glucose solution (concentration: 1mg/mL) were treated with freshly prepared Nelson’s reagent and arsenomolybdate reagent and then diluted to 10.0 mL separately in properly labeled test tubes. Absorbance at 480 nm for the standard is 1.702 and for the sample, 0.926. A. What is the principle behind the assay? B. Calculate the concentration of the reducing sugar in the 50.0 mL sample in mg/mL. Apply Beer-Lambert’s law: A=bc
A 50.0 mL juice extract is colorimetrically assayed using Nelson’s test. One milliliter (1.00 mL) of the solution and the standard glucose solution (concentration: 1mg/mL) were treated with freshly prepared Nelson’s reagent and arsenomolybdate reagent and then diluted to 10.0 mL separately in properly labeled test tubes. Absorbance at 480 nm for the standard is 1.702 and for the sample, 0.926. A. What is the principle behind the assay?
Briefly explain how cation exchange chromatography can used in protein separation?
The molar absorptivities of compounds X and Y were measured with pure samples of each: ε (M-1 cm-1) λ (nm) X Y 272 16,440 3,870 327 3,990 6,420 A mixture of compounds X and Y in a 1.00-cm cell had an absorbance of 0.957 at 272 nm and 0.559 at 327 nm. Find the concentrations of Y in the mixture. 4.43 x 10-5 M 3.03 x 10-6 M 5.95 x 10-5 M 3.56 x 10-4 M
60 ml of standard hardness containing 1 mg of pure CaCO3 per ml consumed 22 ml of EDTA. 40 ml of water sample consumed 20 ml of EDTA solution using EBT indicator. 40 ml of water sample after boiling, filtering consumed 15 ml of EDTA. Calculate the temporary and permanent hardness of water sample.
A spectrophotometric method for the quantitative determination of the concentration ofPb2+ in blood yields an Ssamp of 0.133 for a 1 mL sample of blood that has been diluted to 6 mL. A second sample is spiked with 1 µL of a 1467 ppb Pb2+ standard and diluted to 6 mL, yielding an Sspike of 0.491. Determine the concentration of Pb2+ in the original sample of blood.
A 10 ml of ascorbic acid (MW=176.1) injection was transferred to a 100 ml volumetric flask and made up to volume with deionized water. A 20 ml of the diluted injection was transferred to a conical flask and titrated with Iodine VS using starch mucilage as the indicator. The iodine solution was standardized against a solution of sodium thiosulfate primary standard (MW=248.2). Results: Weight of sodium thiosulfate used to prepare 100 mL primary standard solution = 2.501 g Volume of thiosulfate solution required to titrate 25 mL of Iodine solution = 24.83 mL Volume of iodine solution required to titrate 20 mL of the diluted ascorbic acid injection = 21.55 mL Stated content of the injection = 10% w/v Calculate the % of the stated content in the injection. (Round-off your answer to 2-decimal places) Answer = ____%
A 10 ml of ascorbic acid (MW=176.1) injection was transferred to a 100 ml volumetric flask and made up to volume with deionized water. A 20 ml of the diluted injection was transferred to a conical flask and titrated with Iodine VS using starch mucilage as the indicator. The iodine solution was standardized against a solution of sodium thiosulfate primary standard (MW=248.2). Results: Weight of sodium thiosulfate used to prepare 100 mL primary standard solution = 2.501 g Volume of thiosulfate solution required to titrate 25 mL of Iodine solution = 24.83 mL Volume of iodine solution required to titrate 20 mL of the diluted ascorbic acid injection = 21.55 mL Stated content of the injection = 10% w/v Calculate the % of the stated content in the injection.