(صورة توضيحية فقط)
The Beer-Lambert law relates the attenuation of light to the properties of the material through which it is traveling. It states that the absorbance ([latex]A[/latex]) of a solution is directly proportional to the concentration ([latex]c[/latex]) of the absorbing species and the path length ([latex]l[/latex]) of the light through the solution. The relationship is expressed as [latex]A = \epsilon c l[/latex], where [latex]\epsilon[/latex] is the molar absorptivity.
يُعد قانون بير-لامبرت، المعروف أيضًا باسم قانون بير-لامبرت-بوغيه، حجر الزاوية في الامتصاص الكمي التحليل الطيفي. It combines the findings of several scientists over more than a century. Pierre Bouguer (1729) and Johann Lambert (1760) established that the fraction of light absorbed is proportional to the thickness of the absorbing medium. August Beer (1852) then discovered that the absorbance is also proportional to the concentration of the absorbing substance in a solution. The law is typically written as [latex]A = \log_{10}(I_0/I) = \epsilon c l[/latex], where [latex]I_0[/latex] is the intensity of the incident light and [latex]I[/latex] is the intensity of the transmitted light. The molar absorptivity, [latex]\epsilon[/latex], is a constant that is characteristic of the absorbing substance at a specific wavelength. This means that for a given substance and path length, a plot of absorbance versus concentration will be a straight line, allowing for the creation of a calibration curve. By measuring the absorbance of an unknown sample, its concentration can be determined from this curve. The law holds true for monochromatic light and for dilute solutions where interactions between solute molecules are negligible. Deviations can occur at high concentrations due to chemical and instrumental effects.
قانون بير لامبرت
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