Please help I am completely confused, I included the 2
graphs needed for this post lab. Thank you!
Postlab Assignments . (a) Using your own standard curve, the line equation you generated and Beer’s law equation Equation 1) calculate the molar absorpivity (e) of blue dye. For all your measurem cuvette used is 1.00 cm. Use this as the value of b in Equation 1 ents, the size of (b) Using Beer’s law equation again, what does a high value of molar absorptivity tell you in relation to on and absorbance of species in solution? What does a very low molar absorptivity tell you? 2. The absorbance (A) of light is related to the amount of light transmitted through the equation: AlogT or T 10 A The standard curve below is generated after analyzing a series of standard solutions of FD&C Yellow dye at a certain wavelength. (a) If a commercial “vitamin” water sample containing yellow dye has a percent transmittance, % T, of 43, what is the molar concentration of the yellow dye in the vitamin water? (Hint: You have to use equation 4 first, then Beer’s law (equation 1)] (b) If another commercial drink has a transmittance of 73% at the same wavelength, how much yellow dye does it contain? Show one sample calculation below: Blue Dye Calibration Curve Enter data into the table below and a plot will be generated Conc 2.00E-06 4.00E-06 6.00E-06 1.00E-05 Abs 195 0. 0.366 0.536 0.849 2 Standard Calibration Curve 0.9 0.8 0.7 0.6 2 0.5 R2 0.994 O 0.4 0.3 0.2 0.1 0.00E+00 5.00E-06 1.00E-05 1.50E-05 Concentration, M Print page and turn in with laboratory Standard Curve for Yellow Dye 1.200 1.000 0.800 2 0.600 0.400 0.200 0.000 y 25600x z = 0.9947 0.00E+00 1.00E-05 2.00E-05 3.00E-05 4.00E-05 5.00E-05 Molarity of Yellow Dye, mol/L
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