An unknown chemical has an absorbance of 0.265 in a 1.0cm cuvette at a concentration of 0.703 M. What is the chemical's absorptivity constant in M cm1? Report your answer to three decimals.
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- Suppose that a solution has an absorbance of 0.250 at a wavelength of 450 nm. If the concentration of the solution is 22 μM, what is the value of the molar absorptivity? The data were taken with a standard 1-cm cuvette. molar absorptivity in (L cm^−1 mol^-1):The nitrite in a series of standard solutions (mg/L, n = 5) are converted to azo dye and the slope of the calibration curve is 2.0 ppm. A 10.00-mL mineral water sample is treated in the same way as standards and diluted to a final volume of 100.00-mL It gives an absorbance of 0.80. The absorbance of blank solution under the same conditions is 0.10. Calculate ppm (mg/L) of NO2 (46 g/mol) and the molarity of NaNO2 (69 g/mol) in the original sampleThe nitrite in a series of standard solutions (mg/L, n = 5) are converted to azo dye and the slope of the calibration curve is 2.0 ppm1. A 10.00-mL mineral water sample is treated in the same way as standards and diluted to a final volume of 100.00-mL. It gives an absorbance of 0.80. The absorbance of blank solution under the same conditions is 0.10. Calculate ppm (mg/L) of NO2 (46 g/mol) and the molarity of NANO2 (69 g/mol) in the original sample
- an absorbance of a solution with a pathlength of 1.00 cm is 0.544 and concentration is 1.40x10^ ^ -3 M , what is its molar absorptivity?The molar absorptivity constant of a particular chemical is 2.31 M/cm. Determine the concentration of a solution made from this chemical that has an absorbance of 0.408 with a cell path length of 1.12 cm.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 = 4.586x + -0.0010 %3D The absorbance of a solution of unknown concentration is determined to be 0.68. Calculate the concentration of the unknown solution in M. Give your answer to thrėe decimal places.
- 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.Caffeine, C8H10O2N4 H2O (MW = 212.2 g/mol) has been shown to have an average absorbance of 0.644 for a concentration of 1.783 mg per 100 mL at 272 nm. A sample of 3.658 g of a soluble coffee product was mixed with water to a volume of 500 mL and a 25 mL aliquot was transferred to a flask containing 25 mL of 0.1 M H2SO4. This was subjected to the prescribed clarification treatment and made up to 500 mL. A portion of this treated solution showed an absorbance of 0.666 at 272 nm. Assumbe b = 1.0 cm. Calculate the % caffeine (w/w) in the sample.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.
- 6. Blue Blue dye stock solution 0.293 M Absorbance at 630 nm 0.00265 Calibration curve y = 0.0833x 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 listed in the data table. (a) What is the theoretical molar concentration? [Blue]theoretical x 10 |M (b) What is the experimental molar concentration? [Blue]experimental x 10 M (c) What is the percent error? Percent error (blue) = %Suppose that a solution has an absorbance of 0.226 at a wavelength of 450 nm. If the concentration of the solution is 24 μM, what is the value of the molar absorptivity? The data were taken with a standard 1-cm cuvette.A solution of a specific vitamin has a åmax of 245 nm and a concentration of 4.15 x 10-M. The absorbance of the solution at 245 nm is A = 0.145. What is the molar absorptivity of the vitamin at 245 nm ? A sample path length is 1.00 cm. molar absorptivity: L mol-'cm-!