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Mixing FD&C Blue 1 and Red 40 creates a purple solution. What is/are the expected wavelength(s) of maximum absorbance?
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- What would be a reasonable guess for the wavelength of maximum absorbance for FD&C Orange 2?4. A solution containing complexes of Bi (III) and thiourea has a molar absorptivity of 9.32 x 103 L/cm.M at 470 nm. Calculate the absorbance of a 6.24 x 10-5 M solution in a 1.00 cm cell. 58.15 x 10-2 5.815 x 109 1.494 x 108 O 5.815 x 10-74. To analyze the Cu(NO3)2 unknown solution in Part 3, your group constructed a plot of absorbance vs. concentration, commonly called a calibration curve or standard curve. The absorbance at the top of the peak (i.e., at the wavelength of maximum absorbance) was chosen for these measurements. What is the potential advantage of using the wavelength of maximum absorbance, rather than some other wavelength? Can you think of a situation in which you might want to choose a different wavelength? (Hint: Scientists often do not have the luxurý of analyzing pure substances dissolved in distilled water!)
- The concentration of Fe2+ in a sample is determined by measuring the absorbance of its complex with ferroxine. The sample, measured in a 1.00 cm cuvette, has an absorbance of 0.254. The reagent blank in the same cuvette has an absorbance of 0.015. What would be the absorbance reading for each of these two solutions if measured in a 7.00 cm cuvette? Asample = Areagent blank =1) Calculate the molar extinction coefficient (molar absorptivity) of tartrazine in units of 1/(M·cm). Assume a cuvette path length of 1.00 cm. 2) If Ana determines the absorbance of an unknown tartrazine sample to be 0.662, what is the concentration of the sample in µM?1) A Chem 102 Student prepared a cobalt coordination compound. Parts "a-c" refer to this problem. a) Next, she analyzed the cobalt content of the compound by preparing a series of known concentration cobalt solutions and prepared a Beer's law graph of absorbance (Y) versus concentration(X). The equation of the line was determined using Excel to be: Y=7.50 X the coordination compound and ultimately diluted it to a total volume of 100.0 mL and measured its absorbance to be 0.310. Calculate the percent cobalt (by mass) in the compound. Where X is concentration in Molarity. She weighed 1.1050 g of
- What is the concentration of a tyrosine solution when the absorbance at 280 nm is 1.5 using a 1 cm cuvette and the molar extinction coefficient is 1405 L/mol·cm?25.0 g of an impure sample containing cobalt was dissolved in acid and diluted to1000.00 mL. 6.00 mL of this sample was removed, treated appropriately to give a coloredsolution, and then diluted to 250.00 mL. This final solution had an absorbance of 0.410.Calculate the percentage of cobalt (MW = 58.93 g/mol) in the original sample.Calculate the path length in centimetres which would give an absorbance of 0.134 of a colored dye with a molar absorptivity of 0.759 L mol-1 cm-1 at a wavelength of 645 nm if the concentration of the dye is 6.82x10-2 M. Report your answer to 3 significant figures.
- A standard iron solution was prepared by dissolving 0.0140 g of pure iron in acid then transferring to a 50.00 mL volumetric flask with orthophenanthroline as a complexing agent. At a wavelength of 540 nm, the absorbance of the standard was 0.214 in a 1.00 cm cuvette. A 0.128 g sample of an iron ore was crushed and digested in 5 mL of concentrated acid. The digested sample was then transferred to a 10.00 mL volumetric flask and diluted to the mark with water. A 1.00 mL aliquot of the sample was transferred to a 25.00 mL volumetric flask, and diluted to the mark with water. A portion of the diluted sample was then transferred to a 1.00 cm cuvette and measured at a wavelength of 540 nm. The resulting absorbance was 0.216. Determine the % w/w of Fe in the iron ore.Absorbance measurements were taken on a series of Fe standards complexed with 1,10-phenanthroline. A plot of absorbance vs. concentration yielded a linear curve with the equation y=1.008e03x + 0.0395 (where y is the absorbance and x represents the Fe concentration in moles/L). Using this information calculate the Fe concentration (in ppm) in a 40.0-mL aliquot of ground water that produced an absorbance of 0.580.A standard solution was put through appropriate dilu tions to give the concentrations of iron shown in the ac companying table. The iron(II)-1,10,phenanthroline complex was then formed in 25.0-ml aliquots of these solutions, following which each was diluted to 50.0 mL (see color plate 15). The absorbances in the table (1.00-cm cells) were recorded at 510 nm Fe(II) Concentration in Original Solution, ppm Aşie 4.00 0.160 0.390 10.0 16.0 0.630 24.0 0.950 32.0 1.260 40.0 1.580 (a) Plot a calibration curve from these data. (b) Use the method of least squares to find an equa tion relatin g absorbance and the concentration of iron(II). (c) Calculate the standard deviation of the slope and intercept.