Q4 :[a] 5.00 x 10M solution of an analyte is placed in a sample cell that has a path lengthof 1.00 cm. When measured at a wavelength of 490 nm, the absorbance of thesolution is found to be 0.338. What is the analyst's molar absorptivity at thiswavelength

Given: The concentration (c) of the solution is 5.00 x 10-4 M The path length (b) is 1.00 cm The…

Answered: Q4 :[a] 5.00 x 10 M solution of an…

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

Chapter13: An Introduction To Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 13.24QAP

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3.) The accuracy of a spectrophotometer is evaluated by preparing a solution of 60.06 ppm K2Cr2O7 and measuring its absorbance at a wavelength of 350 nm in a cell with a pathlength of 1.00 cm. The expected absorbance is 0.640. What is the expected molar absorptivity of K2Cr2O7 at this wavelength?
The ultraviolet spectrum of aspirin shows a secondary absorption band at 271 nm. If a solution of aspirin in water, with a concentration of 1×10-4 molar solution is examined at 271 nm, what will be the absorbance reading (ℇ = 1000) and what will be the intensity ratio, IO/I, respectively?
The molar absorptivity for the FD&C dye “Red No. 3” (Erythrosine) 8.25104 M‒1·cm‒1 at 526 nm. Calculate the expected absorbance of solution of Red No. 3 with a concentration of 4.00×10–6M when measured at 629 nm in a 2.00 cm cell.
To determine the concentration of these analyte ions in a mixture, the mixture absorbance is analyzed in a cell with a pathlength of 1.00 cm at 396 nm and at 550 nm, yielding values of 0.109 and 0.0.183, respectively. What is the molar concentrations of X3+ in the sample? What are the molar concentrations of Y2+ in the sample?
The molar absorptivity for Blue #1 dye is 1.30105 M‒1 ·cm‒1 at 629 nm. Calculate the expected absorbance of solution of Blue #1 with a concentration of 4.50×10–6M when measured at 629 nm in a 1.50 cm cell.
A 5.00×10−4 M solution of analyte is placed in a sample cell that has a pathlength of 1.00 cm. At a wavelength of 490 nm, the solution’s absorbance is 0.338. What is the analyte’s molar absorptivity at this wavelength?
Calculate the molar extinction coefficient of a biomolecule with a MW of 300 if a 5.0 mM solution in a 1.2 cm cuvette has an absorbance of 0.50 at 340 nm.
The absorbance of a 1.05x10-5 M Fe+3 determined at 580 nm using a 2.50-cm cell was said to be 0.200. What is the molar absorptivity of this solution in liters/mole cm?
Fe+3 (aq) + SCN – (aq) FeSCN +2 (aq) She mixes 4.00 mL of 2.00 mM SCN– and 5.00 mL of 2.00 mM Fe+3 ions, then diluting with 1.00mL of water to give a total volume of 10.00mL. She measures the absorbance of the solution asbeing 0.210. If she has previously calculated the molar absorbtivity constant (ε) of the product tobe 2583 cm–1 M–1, what is her best estimate for the K value for this reaction?
A 7.21 x 10−5 M solution of potassium permanganate has a transmittance of 52.1% whenmeasured in a 3.81-cm cell at a wavelength of 550 nm. Calculate (a) the absorbance of thissolution and (b) the molar absorptivity of KMnO4
.A 8 × 10-5 M solution of potassium permanganate has a transmittance of 45% when measured in 2.0 cm cell at wavelength of 526 nm. Calculate (a) the absorbance of this solution and (b) the molar absorptivity of KMnO4.
A solution containing 3.75mg/100 ml of analyte (X) 220 g/mol has a transmittance of 39.6% in a 1.00 cm cell at 480 nm. Calculate a) The molar absorbtivity of X. b) The fraction of light transmitted from a solution three times the mentioned concentration.

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Q4 :[a] 5.00 x 10 M solution of an analyte is placed in a sample cell that has a path length of 1.00 cm. When measured at a wavelength of 490 nm, the absorbance of the solution is found to be 0.338. What is the analyst's molar absorptivity at this wavelength