4. Using the calibration curve below, what is the concentration of a Cu2t solution which had an absorbance of 0.450? Absorbance as a Function of Concentration of Cu2+ 0.800 0.700 0.600 0.500 0.400 0.300 0.200 0.100 0.000 0.800 0.700 0.600 0.500 0.400 0.300 0.100 0.200 0.000 [Cu2] EXPERIMENT 7 121 Absorbance
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- .Q1. To determine the concentrations (mol/L) of Co(NO3)2 (A) and Cr(NO3)3(B) in an unknown sample, the following representative absorbance data wereobtained.A (mol/L) B (mol/L) 510nm 575nm5×10−1 0 0.714 0.0970 6×10−2 0.298 0.757Unknown Unknown 0.671 0.330Measurements were made in 1.0 cm glass cells.i. Calculate the four molar absorptivities: ∈A(510), ∈A(575), ∈B(510) and ∈B(575).ii. Calculate the molarities of the two salts A and B in the unknown.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) = %13. 0 0 0 5 The following curve was made by absorption spectrophotometry (2 = 500 nm) of standard protein solutions using the Lowry method you will perform in lab Exercise #4. If an unknown protein solution was analyzed using the same system and an absorbance value of 0.125 was measured, what was the protein concentration of the unknown? 1 Absorbance at 500 nm 0.8 0.6 0.4 0.2 y = 1.492E-03x + 3.513E-02 0 100 A. 107 μg/mL B. 83.7 μg/mL C. 71.4 μg/mL D. 60.2 µg/mL 200 300 400 500 600 Protein concentration, ug/mL
- A solution has an absorbance reading of 0.238 AU. Using the calibration curve below, determine the concentration of the solution. Calibration Curve 0.3 0.25 y-657.55x+ 0.017 R-0.9991 0.2 0.15 01 0.05 0.00E-005.00E-051.00E-04150E-042.00E-04250E-043.00E-O43.50E-044.00E-044. SOE-04 Concentration (M) Answer: Absorbance (AU)A colored ion solution has a concentration of 0.200 M with a measured absorbance A = 0.880. Another ion solution made of the same chemicals has an absorbance A = 0.172. What is the concentration of this unknown sample solution?A. Preparation of a Calibration Curve Initial (CrO]_O.0024M Volume of 0.0024 M K,Croq Total volume Absorbance 100 mL (00ML | 00 mL (00 mL 0.04L toso.37 0,85 13 1. 5 mL 10 mL 15 mL 2. 2.4X10"M 3.6x(0 4 3. Molar extinction coefficient for [Cro,²-] 2. 3. Average molar extinction coefficient Standard deviation (show calculations) B. Determination of the Solubility-Product Constant [Cro,?-] [Ag°] K, of Ag;CrO4 Absorbance 1. 0.80, % T=15.8 28x/0-4M 2. 0.)3,% T=14.8 24x10*M 3. 0.45 % T=l1.2 33x10 M
- Substance P has an extinction coefficient of 72.22 mM-1cm-1 at 420nm. 2 μl of Substance P was added to 998 μl water and the Absorbance at 420nm was 0.820. Calculate the mM concentration of the original Substance P solution2. What is the concentration (mM) of a solution of tryptophan if the absorbance at 280 nm is 0.850? The cell path length is 1.0 cm and the extinction coefficient is 5500 M-1 cm-14. The total absorbance of a solution is the sum of the absorbances of all different materials present. AT = Aa + Ap + Ac .. etc. At 427 nm, the molar absorbtivity of Yellow #5 is 2.73×10°M-1-cm1. At 427 nm the molar absorptivity of Red 40 is 7.49x103 M-1.cm-1. Calculate the total absorbance of a solution in which the concentration of Yellow #5 = 2.00x10-5 M and the concentration of Red 40 = 4.80x10-5 M, when measured at 427 nm in a 1.00 cm cell.
- 4. A solution containing complexes of Bi (III) and thiourea has a molar absorptivity of 9.32 x 103L cm1 mol1 at 470 nm. Calculate the absorbance of a 6.24 x 105 M solution in a 1.00 cm cell. A. 58.15 x 10² B. 5.815 x 10° C. 1.494 x 10® D. 5.815 x 10-7Solve the problems using a step-by-step process (solutions). 1. A 1.0x10-3 M solution of a dye X shows an absorbance of 0.20 at 450 nm wavelength and an absorbance of 0.05 at 620 nm wavelength. Calculate the extinction coefficient for each wavelength. (Ans. e450 = 200 ; e620 = 50)Yellow Dye Calibration Curve y = 254.78x - 0.1414 R? = 0.9792 2.5 1.5 1 0.5 0.002 0.004 0.006 0.008 0.01 0.012 Concentration(M) 3. 2. Absorbance