aqueous solution of a purine triphosphate at a concentration of J. sodium dehydrate (molar mass 586 g/mol), give an absorbance of 1.014 with a light th of 1cm. Calculate the molar absorption coefficient. What would be the absorbance fa 10 uM solution, and what would be the percentage of light transmittance?

aqueous solution of a purine triphosphate at a concentration of J. sodium dehydrate (molar mass 586 g/mol), give an absorbance of 1.014 with a light th of 1cm. Calculate the molar absorption coefficient. What would be the absorbance fa 10 uM solution, and what would be the percentage of light transmittance?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

UV Visible Spectroscopy

Spectroscopy refers to the absorption or emission of light or other radiations by matter. When a substance or chemical absorbs light or radiation, they reach an excited state followed by de-excitation or emission of the light or radiation forming distinct spectra. UV-visible spectroscopy or ultraviolet-visible refers to the absorption and emission in the ultraviolet and visible regions of the electromagnetic spectrum.

Question

An aqueous solution of a purine triphosphate at a concentration of 57.8 mg/dm of its.
trisodium dehydrate (molar mass 586 g/mol), give an absorbance of 1.014 with a light
path of lcm. Calculate the molar absorption coefficient. What would be the absorbance
of a 10 uM solution, and what would be the percentage of light transmittance?
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