at 542 hm 0.5 45 0.4 35 0.3 25 0.2 15 y = 15200x - 0.018. 0.1 5.00E-06 1.00E-05 1.50E-05 2.00E-05 2.50E-05 3.00E-05 3.50E-05 Concentration (M) s the molar absorptivity (in M¯1cm-1) of the unknown dye at 542 nm? nswer: correct
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- A solution of KMnO4 with a concentration of 8.25 x 10-5 M yields an absorbance value of 0.1302 when measured in a 5.60 cm cuvette, set at a wavelength of 725 nm. Compute for the Molar Absorptivity Coefficient of the sample. Choices: a. 2.8182x10-8 c. 4.8182x10-8 b. 3.8182x10-8 d. 5.8182x10-8The absorbance for a dye sample of unknown concentration is measured and the corrected absorbance is 0.666. The standard curve created is found to have this linear equation: y = 0.153x + 0.043 Calculate the concentration (ug / mL) of the dye sample. 4.54 3.33 4.07 5.17 2.07The concentration of a dilute aspirin solution is 0.000530 M 0.000530 M . Standard solutions of this compound were used to prepare a Beer's law plot which gives a slope of 1550.1 M −1 1550.1 M − 1 . What is the expected absorbance value for the aspirin solution?
- The spectrophotometer is used to measure absorbance experimentally. Briefly, explain how this is accomplished.You are measuring the concentration of an unknown protein sample, and the absorbance at 595 nm (or A595) of your unknown is greater than that of the highest-concentration standard solution. It is not advisable to simply extrapolate the line of the standard curve to calculate the concentration of the unknown In this scenario, what would be the best strategy to measure the concentration of your unknown (instead of extrapolating from the standard curve)?A Beer’s law plot is prepared by plotting absorbance vs molar concentration of the absorbing species. What are the units of the slope? What are the units of the y-intercept?
- 8. a. The value of molar absorptivity constant (e) for a colored substance is 35,000 M -1 cm-1 at 473 nm and the curvette is 1.00 cm. Determine the range of concentration possible if absorbance can be measured from 0.050 to 0.95. b. Calculate the concentration for the following values of absorbance for the colored substance above. A= 0.27 A=0.54Extinction coefficient of a dye is 7200 M-1 cm-1. Assuming a path length of the cuvette to be 1 cm, what is the concentration of solution when the absorbance is 0.300 at 500 nm.A standard 3 mL cuvette is two-thirds filled with a 1 in 5 dilution of 70 mM oxyhaemoglobin. The absorbance is measured at 580nm. A few drops of a live yeast suspension is added to the cuvette (without significantly changing the volume). The absorbance is remeasured at the same wavelength as above and is found to be 0.40, a decrease of 0.2 on the first measurement. What is the molar absorbance coefficient of the oxyhaemoglobin at 580 nm? (do not enter the units in the answer, 2 decimal places)
- Examine the given Beer's law standard curve for an unknown dye measured in a 1.0 cm cuvette. Plot of absorbance at 542 nm versus concentration. There is a best-fit line on the plot and the equation is given as y=15200x-0.018 What is the molar absorptivity (in M–1cm–1) of the unknown dye at 542 nm?Determine the concentration of a solution with an absorbance of 0.3 at 300nm measured with a light path is 2.0cm? 5.7x104M-1cm-1 is the molar absorption coefficient.Why should absorbance be less than 2? Please explain in terms of light transmittance