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?

The molar absorptivity constant of a particular chemical is 2.31 M/cm. Determine the concentration of a solution made from this chemical that has an absorbance of 0.521 with a cell path length of 1.04 cm.

1.) Beer's Law can be used to find the concentration of a solution by measuring its absorbance. The law is given by  ?=???A=ϵbC Where A is the absorbance, ?ϵ is the molar absorptivity, b is the pathlength of the light (the width of the sample cell), and C is the concentration of the solution.  A student is analyzing a solution of a metal, and finds that the absorbance of the solution is 0.532. If ?=187 L⋅g−1⋅cm−1ϵ=187 L⋅g−1⋅cm−1 and ?=1 cmb=1 cm , what is the concentration of the metal in solution (in g/L)?    * 352 * 2.84×10−32.84×10−3 * 2.84×10−22.84×10−2 * 96.8   2.) How many significant figures does the number 0.00358 have? Group of answer choices a.1 b.2 c.3 d.5   3.) A 10.00 mL solution of a certain food dye has a concentration of 1.47 g /L. What is the total mass of food dye in the solution? Report your answer with the correct number of significant figures.

Suppose that a solution has an absorbance of 0.250 at a wavelength of 450 nm.  If the concentration of the solution is 22 μM, what is the value of the molar absorptivity?  The data were taken with a standard 1-cm cuvette. molar absorptivity in (L cm^−1 mol^-1):