You have a solution with a concentration of 0.50 mM, and you put it in a cuvette with a 1.0cm pathlength. You read an absorbance of 0.600. What is the extinction coefficient of your analyte? Question 4 options: 1.2 mM cm 1.2 mmole/L/cm 1.2 L/mmole/cm 1.2 mmol/L (cm)-1
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- You have a solution with a concentration of 0.80 mM, and you put it in a cuvette with a 1.0cm pathlength. You read an absorbance of 0.400. What is the extinction coefficient of your analyte? Question 4 options: 0.50 mmole/L/cm 0.50 mmol/L (cm)-1 0.50 L/mmole/cm 0.50 mM cm45.0 mL of an unknown FeCl3 solution is diluted to a total volume of 230.0 mL. The diluted FeCl3 solution measured an absorbance of 0.223. Calculate the molarity of the undiluted unknown FeCl3 solution if the molar extinction coefficient is 230.0 M-1⋅cm-1 and a path length of 1.00 cm. Group of answer choices 0.000190 M 0.00496 M 0.00593 M 10.0 M 0.00399 M3. An indicator is a dye whose spectrum changes with pH. Consider the following data for the absorption spectrum of an indicator (pK = 4) in its ionized and nonionized form. InH+ → In + H* Molar absorptivity, ɛ (M1.cm1) InH+ (nm) In 400 10,000 420 15,000 2,000 440 8,000 8,000 460 12,000 480 3,000 The absorbance of the indicator solution is increased in a 1-cm cell and found to be 400 420 440 460 480 (nm) A 0.250 0.425 0.400 0.300 0.075 a. Calculate the pH of the solution. [4.0] b. Calculate the absorbance of the solution at 440 nm and pH 6.37 for the same total indicator concentration. [0.400] c. If you want to measure the quantum yield of fluorescence of In and H* independently, what wavelength would you choose for exciting In H+? For exciting In? Why?
- How would I do 2? the concentration iron is 1.85mg/vitamin tablet, and the absorbance at 508nm is 0.37A solution containing a mixture of the compounds X and Y had an absorbance of 0.814 at 443 nm and an absorbance of 0.699 at 520 nm when measured with a 1.00 cm cell. The molar absorptivities (e) of X and Y at each wavelength are shown in the table. [X] = Wavelength (2, nm) [Y] = 443 Incorrect 520 2.13 x10-5 1.23 x10-4 Incorrect Molar Absorptivity (c. M-¹cm-¹) X What are the concentrations of X and Y in this mixture? 16180 3936 Y 3817 6333 4 M Mcan you explain how I can get 1.596 mg/L of concentration of Fe3+ in dilutes sample and can you also make the calibration curve.
- Q1So Please don't provide the handwriting solutionPlease answer the question correctly is all I want and explain why its thats answer for the final and please answer as quickly as possible, thanks! You graph the calibration curve of a solution of an unknown metal (we will call it M+) at 400 nm. The graph is shown below. What is the concentration the solution with an absorbance of 0.500 at 400 nm?
- The absorbance values at 250nm of 5 standard solutions, and sample solution of a drug are given below: Conc. (ug/ml) A 250 nm10 0.16820. 0.32930 0.50840. 0.66050 0.846Sample. 0.661Calculate the concentration of the sampleA solution of a specific vitamin has a 4max of 271 nm and a concentration of 2.73 x 10-"M. The absorbance of the solution at 271 nm is A = 0.155. What is the molar absorptivity of the vitamin at 271 nm? A sample path length is 1.00 cm. molar absorptivity: L mol-'cm-!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 cm? Report your answer to three decimals.