I The concentration of phenol in an aqueous solution is 10 ug/mL. The absorbance is found to be 0.209 when this solution is placed in a 1.00 cm cuvette and 258 nm radiation is passed through it. a. Calculate the specific absorptivity, including units, of phenol? b. What will be the absorbance if the solution is diluted to 5 ug/mL? C. What will be the absorbance if the path length of the original solution is increased to 5.00 cm?

I The concentration of phenol in an aqueous solution is 10 ug/mL. The absorbance is found to be 0.209 when this solution is placed in a 1.00 cm cuvette and 258 nm radiation is passed through it. a. Calculate the specific absorptivity, including units, of phenol? b. What will be the absorbance if the solution is diluted to 5 ug/mL? C. What will be the absorbance if the path length of the original solution is increased to 5.00 cm?

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter27: Gas Chromatography

Section: Chapter Questions

Problem 27.5QAP

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The concentration of phenol in an aqueous solution is 10 ug/mL. The absorbance is found to be 0.209 when this solution is placed in a 1.00 cm cuvette and 258 nm radiation is passed through Calculate the specific absorptivity, including units, of phenol? What will be the absorbance if the solution is diluted to 5 ug/mL? What will be the absorbance if the path length of the original solution is increased to 5.00 cm?
A green solution containing Ni+2 ions absorbs 580 nm light. Undiluted, a sample of this solution sampled in a 1.00 cm diameter cuvette has an absorbance of 0.9765 a.u.. If the molar absorptivity coefficient for Ni+2 is 6.3 x 104 M -1 cm -1 at 580 nm, how much of the original stock Ni+2 solution (in mL) needs to be added to water to create a total dilute solution volume of 10.00 mL that measures an absorbance of 0.146 a.u. at 580 nm? Report your answer to 3 significant figures. Do not include the "mL' unit label in your response
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The measured absorbance of a solution with a pathlength of 1.00 cm is 0.544. If the concentration is 1.4010-3 M, what is the molar absorptivity for this analyte?
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a) Determine the concentration of your prepared Iron (III) Salicylate Dianion solution (pure ASA) in the 10.0. mL of 1.0 M NaOH in mg/mL (Part D) using the Beer's Law plot completed in Question 1. Hint: You need to use the measured absorbance reading of your prepared Iron (III) dianion. b) Then, calculate the mass (in mg ) of pure ASA knowing that two consecutive dilutions were done to prepare the solution. Show all of your work. given information: beer's law Standard: Concentration of ASA in Standards (mg/mL) A: 0.18 B: 0.14 C: 0.10 D: 0.070 E: 0.040 Sample: Absorbance reading standard A: 1.25 standard B: 0.96 standard C: 0.74 standard D: 0.50 standard E: 0.23 the absorbance reading for my prepared iron (III) dianion is 0.83 the volume is 25.0mL b is the path length of the cuvette (assume 1 cm) the molecular weight of Iron (III) Salicylate Dianion is 330.09g/mol (correct me if i am wrong) i do not have the molar absorptivity, but the equation is 7,1*x +0.017 for the slope-intercept…
Quinine in a 1.664 g antimalarial tablet was dissolved in sufficient 0.10 M HCl to give 500 mL of solution. A 15.00 mL aliquot was then diluted to 100.0 mL with the acid. The fluorescense intensity for the diluted sample at 347.5 nm provided a reading of 288 on an arbitrary scale. A standard 100 ppm quinine solution registered 180 when measured under conditions identical to those for the diluted sample. Calculate the mass in milligrams of quinine in the tablet.
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