Beers Law lab report - Introduction The Beer-Lambert Law is used to show the relationship between absorbance and concentration The Beer-Lambert Law

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Introduction: The Beer-Lambert Law is used to show the relationship between absorbance and concentration. The Beer-Lambert Law can be quantitavely expressed by the following equation: A= ε bc The “A” in this equation is used to signify the measured absorbance, the “c” is used to denote the concentration, the “b” is the path length or the width of the cuvet, and the “ ε is a constant called the molar absorptivity. The molar absorptivity is constant for a particular chemical compound at a specific wavelength. Usually, there is one wavelength that corresponds to the maximum epsilon value. The molar absorptivity value can be derived from a graph that has the concentration values on the x-axis and the absorbance values on the y-axis. This graph has a linear relationship between these two values and can be written in the form y=mx+b (where b, the intercept, is zero). The slope of this line is equivalent to εb. Typically there are two types of dilutions that are commonly employed. A serial dilution involves a series of solutions where each of the solutions that are made becomes the source solution for the following solution in the series. One advantage behind conducting a serial dilution is that a number of concentrations can be accomodated if this approach is used. A parallel dilution is where a series of solutions are made from the original solution. The advantage behind conducting a serial dilution is that there are fewer
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This note was uploaded on 04/11/2008 for the course MUS 334 taught by Professor Shaheen during the Spring '08 term at University of Arizona- Tucson.

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Beers Law lab report - Introduction The Beer-Lambert Law is used to show the relationship between absorbance and concentration The Beer-Lambert Law

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