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- In an analytical laboratory a chemical compound namely Paracetamol (151.163 g/mol) is determined in a sample. A sample weighing 0.0295 g was dissolved in a solvent and diluted the solution to 1 L. The solution has λ max at 243 nm (ε=2.6×104 cm-1 mol-1 L). The solution exhibits an absorbance of 0.638 in a 2 cm cell. Calculate the percentage paracetamol in the 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?A solution prepared by dissolving 25.8 mg of benzene (78.11 g/mol) in hexane (86.16 g/mol) and diluting to 250 mL had an absorption peak at 256 nm and an absorbance of 0.266 in a 1.000-cm cell. What is the concentration of benzene solution? O 1.20x10-3 M O 1.32x10-3 M O 1.32 M O 1.20 M
- Caffeine (C8H10O2N4 • H2O) has an absorbance of 0.510 at 272 nm and 1 cm optical path in1 mg / 100 mL concentration solutions. A 2.5 g sample of soluble coffee is diluted withwater to 500 mL. Take 250 mL, add 25.0 mL of 0.1 N H2SO4 and dilute it to 500 mL. Theabsorbance at 272 nm resulting in 0.415. A) Calculate the grams of caffeine per kg of soluble coffee in the sample. Themolar mass of caffeine is 212 g / mol.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.A never circulated 1975 penny with a mass of 3.00 g was dissolved in concentrated nitric acid, the resulting solution was then diluted to 50.0 mL with water. The weight percent copper in the penny was determined to be 94.7%. If the best-fit line for the Beer’s law plot was y=1.5x + 0.02, what is the absorbance of the penny solution?
- What is the absorbance of a theoretical compound in a 5.26x10-5 M solution, a path length of 1.5cm, and a molar absorptivity of 37.4 mol / L cm?Q3) A solution of Tryptophan has an absorbance at 280 nm of 0.25 in a 0.5 cm length cuvette. Given the absorbance coefficient of Tryptophan is 6.4 × 103 L Mol-1 cm-1. What is the concentration of solution?Q)A histidine solution with a concentration of C = 60.5 mg/L has an absorbance of 0.794 when the light path length is 1.0 cm. Note that the molecular mass of tryptophan is 155.15 g/mol. 1-Calculate the molar absorbance of a histidine solution expressed as L.mol 1.cm-1. 2-Description of the preparation of 100 mL of a 15.0 ppm histidine solution mentioned above
- 22. To test a spectrophotometer's accuracy, a solution of 60.06 ppm K2Cr2O7 is prepared and analyzed. This solution has an expected absorbance of 0.641 at 350.0 nm. Several aliquots of the solution produce the following absorbance values. 0.640 0.638 0.640 0.639 0.640 0.639 0.638 is there any significant difference between the experimental mean and the expected value at a 99.9% confidence level? Yes because tcal>tcritical Yes because tcaltcritical No because tcalA. Copper sulfate pentahydrate is often used to teach students about Beer’s Law by making a standard curve (linear regression). The bright blue color of the solution has a peak absorbance in the red range of the electromagnetic spectrum. The absorbance value is proportional to concentration. How many grams of CuSO4 5H2O to make up 250 mL of a 0.2 M stock of this solution? B. Using M1V1 = M2V2 how many mL would a student need to measure out in graduated cylinder to make up a 50 mL (V2) solution of 0.1M, 0.05 M, 0.025M 0.0125M solutions for a standard curve at the peak wavelenth for this compound? I need help with part B of this question.The absorbance of an unknown dye solution is measured to be 1.06 by a spectrometer. The calibration plot of the spectrometer is provided below. What is the molar concentration of the unknown sample (in mole L)? Absorbance vs. Molarity 18 y3 67024x-0.0343 16 14 12 1 0.8 0.6 0.4 0.2 01 0.2 0.000005 00001 0000015 Concentration of solutions, mol/L 0.00002 0.000025 000003 0 163e-5 O 2.35e-6 0 163 0 235 AbsorbanceSEE MORE QUESTIONS