Beer-Lambert Law:
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The Beer-Lambert Law (or Beer's Law) relates the absorption of light to the properties of the material through which the light is traveling. It states that there is a linear relationship between the absorbance and the concentration of an absorbing species.
The calculator uses the Beer-Lambert Law equation:
Where:
Explanation: The law states that absorbance is directly proportional to the concentration of the absorbing species in the solution and the path length of the light through the solution.
Details: This calculation is fundamental in analytical chemistry, particularly in spectrophotometry, for determining the concentration of substances in solution. It's widely used in biochemistry, molecular biology, and pharmaceutical analysis.
Tips:
Q1: What is the valid range for absorbance measurements?
A: For most accurate results, keep absorbance between 0.1 and 1.0. Values below 0.1 have poor signal-to-noise ratio, while values above 1.0 may deviate from linearity.
Q2: Where can I find molar extinction coefficients?
A: Literature values are available for common compounds. They are wavelength-specific and should be determined experimentally for new compounds.
Q3: Why is path length important?
A: Absorbance is directly proportional to path length. Using the correct path length (usually 1 cm) is crucial for accurate calculations.
Q4: What are limitations of Beer's Law?
A: The law assumes monochromatic light, dilute solutions, and no scattering or fluorescence. Deviations occur at high concentrations or with chemical associations.
Q5: Can I use this for mixtures?
A: For mixtures, you need absorbance measurements at multiple wavelengths and knowledge of all components' extinction coefficients at those wavelengths.