Beer-Lambert Law, also known as the Beer-Lambert-Bouguer Law, describes the relationship between the concentration of a sample and the amount of light that is absorbed by the sample. It is commonly used in analytical chemistry to determine the concentration of a solution.
According to Beer-Lambert Law, the amount of light absorbed by a solution is directly proportional to the concentration of the solution and the length of the path through which the light passes. This can be mathematically represented as:
A = εcl
Where A is the absorbance of the solution, ε is the molar extinction coefficient (a constant unique to each substance), c is the concentration of the solution, and l is the length of the path that the light passes through the solution.
By measuring the absorbance of a solution at a particular wavelength, we can determine the concentration of the solution using the Beer-Lambert Law. This is done by using a spectrophotometer, which measures the amount of light absorbed by the sample and provides a readout of the absorbance. Knowing the value of ε for the substance being measured, we can calculate the concentration of the solution.
Overall, the Beer-Lambert Law provides a simple and effective way to measure the concentration of a solution, which is useful in a wide range of applications, including medicine, environmental science, and industrial chemistry.
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