The absorbance of a sample of erioglaucine was measured to be 0.525 through a 10mm cuvette. The concentration of the sample was also determined to be 7.85 x 106M. Determine the molar absorptivity of erioglaucine. (Report answer to the ones place regardless of sig figs.) *"Only use numeric values in your answer. Do not use words, spaces, or symbols (ie. %).**
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- An unknown amount of a compound with a molecular mass of 270.57 g/mol is dissolved in a 10 mL volumetric flask. A 1.00 mL aliquot of this solution is transferred to a 25 mL volumetric flask, and enough water is added to dilute to the mark. The absorbance of this diluted solution at 355 nm is 0.495 in a 1.000 cm cuvette. The molar absorptivity for this compound at 355 nm is €355 = 6149 M-¹cm-¹. What is the concentration of the compound in the cuvette? concentration: What is the concentration of the compound in the 10 ml flask? concentration: How many milligrams of compound were used to make the 10 mL solution? mass: M M mgThree compounds (A, B and C) are mixed together ( they are present in the same container). Molar absorptivity coefficients of these compounds at 575nm -1 -1 are: 2500, 3750 and 5250Lcm mol, respectively. Concentrations are: 2 × 10M for A, 5× 105 M for B and -6 1.5×10 M for C. What is the absorbance measured at 575mm, in 1.0cm cuvette of the solution containing all three compounds? Show your calculations.Calculate the concentration of a solution of peptide AWSME, in mM if the absorbance at 280 nm for the solution is 0.6 absorbance units, and a 0.2-cm cuvette is used. For the extinction coefficient, take into account that e280(Trp) = 5690 M-1 cm-1 and e280(Tyr) = 1280 M-1 cm-1. Round your answer to two decimals.
- The absorption coefficient of rhodopsin at 496 nm is 40,000 M-1cm-1. If you have a 1M solution of rhodopsin, how many times will you dilute the solution so that the diluted solution will give you an absorption reading at 496 nm that is in the range of 0.1-1.0. And what will be the absorption by the diluted solution?3) A compound, X, with a molecular weight of 292.16 g/mol was dissolved in a 5.00 mL volumetric flask and diluted to the mark. A 1.00 mL aliquot of this was withdrawn, placed into a 10.00 mL volumetric flask and diluted to the mark. The absorbance at 340 nm was 0.427 in a 1.000 cm cuvette. The molar absorptivity of X at 340 nm is 6130 M-¹ cm-¹ a) Using Beer's Law, what is the [X] (concentration in molarity) for the diluted solution in the cuvet ? mmmmm b) Use the dilution equation (McVc = MdVa) to calculate [X] in the original 5.00 mL flask. c) How many milligrams of X was used in the original solution ? (Find total moles X using original concentration and original volume - and then use the molar mass to go from moles to grams and then milligrams)A reaction was carried out with Fe3+ and SCN- to produce FeSCN2+. Two best-fit lines for Absorbance vs [FeSCN-] were obtained. The first line produced: y = 200x + 0.005, r2=0.951 and the second line produced: y= 10,000x + 0.005, r2 = 0.993. Determine the best-fit line of two, and then use the line equation to determine the equilibrium concentration of FeSCN2+ if the absorbance = 0.863.
- 13. A 9.50 μM standard solution of X yields an absorbance of 0.657 at 630 nm using a 1.00-cm cuvette. The molar absorptivity for X at 630 nm is a) 40,700 M-¹cm-1 b) 614,000 M-¹cm-¹ c) 1010 M-¹cm-1 d) 69,200 M¹¹cm ¹ e) 138,700 M¹¹cm¹ 14. The molar absorptivity for ferricyanide ion (FW = 211.95 g/mol) at 420 nm is 1010 M-¹cm¹. What is the concentration of ferricyanide in a solution that yields an absorbance of 0.354 in a 1.00-cm cuvette? a) 30 ppm b) 45 ppm c) 60 ppm d) 75 ppm e) 90 ppm 15. Deviations from Beer's law are observed when measurements are made a) with highly concentrated solutions b) using polychromatic light sources c) in the presence of stray light d) all of these e) none of these 16. Photometric assays typically involve measuring absorbance at an analyte's "Amax" in order to a) maximize sensitivity b) maximize selectivity c) maximize accuracy d) maximize precision e) maximize detection limit 17. The calibration curves shown at the right indicate the photometric…When measured in a 1.00 cm cuvette, a 4.1x10M solution of species X exhibited absorbances of 0.1025 and 0.533 at 530 nm and 325 nm, respectively. A8.20x10 M solution of species Y gave absorbances of 0.230 and 0.508 at 530 nm and 325 nm, respectively. Both species were dissolved in the same solvent, and the solvent's absorbance was 0.000 and 0.000 at 530 nm and 325 nm, respectively, in a 1 cm cuvette. Calculate the concentrations of X and Y in an unknown solution that yielded absorbance data of 0.683 at 530 nm and 1.351 at 325 nm in a 1.0 em cuvete O A.X-4.20 x10 M Y=3.20 x104 M OBX-1.25 X10M Y420 x10-SM OCX-3.75x1oM Y-1 A10M OD.X-3.80 x 10M Y=2.10x10MWhen measured in a 1.00 cm cuvette, a 4.1x10M solution of species X exhibited absorbances of 0.1025 and 0.533 at 530 nm and 325 nm, respectively. A 8.20x10 M solution of species Y gave absorbances of 0.230 and 0.508 at 530 nm and 325 nm, respectively. Both species were dissolved in the same solvent, and the solvent's absorbance was 0.000 and 0.000 at 530 nm and 325 nm, respectively, in a 1 cm cuvette. Calculate the concentrations of X and Y in an unknown solution that yielded absorbance data of 0,683 at 530 nm and 1.351 at 325 nm in a 1.0 cm cuvette A. X= 4.20 X10M Y=3.20 x10+M O B. X1.25 X10M Y= 4.20 x10-5M OCX-3.75X10M Y-1 4x10M OD.X-3.80 x 10 M Y 2.10K10M
- A 1.0x10 -3 M solution of a dye X shows an absorbance of 0.20 at 450 nm wavelength and anabsorbance of 0.05 at 620 nm wavelength. Calculate the extinction coefficient for each wavelength.(Ans. e 450 = 200 ; e 620 = 50)What is the molar absorptivity of a 2.50 x 10-4 M solution if its absorbance at 550 nm is 0.500? The sample is placed in the standard 1-cm quartz cuvette. 2.00 x 10-3 M-1cm-1 5.00 x 10-4 M-1cm-1 2.00 x 103 M-1cm-1 1.25 x 10-4 M-1cm-1Unrounded Rounded ε∗,L/μmol 0.0259825 0.0260 Heres the data if needed: TZ # Concentration Absorbance at 430 nmnm 1 33.6480 0.931 2 25.2360 0.757 3 16.8420 0.210 4 8.41200 0.137 5 4.20600 0.122