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Calculate molar absorptivity with our easy online calculator. Enter absorbance, concentration, and path length to get fast, accurate results.
| Term | Meaning |
|---|---|
| A = εcl | Beer-Lambert Law: absorbance equals molar absorptivity × concentration × path length |
| ε = A ÷ (c × l) | Molar absorptivity, rearranged from the Beer-Lambert Law |
| L·mol⁻¹·cm⁻¹ | Standard unit for molar absorptivity (also written L/(mol·cm)) |
A molar absorptivity calculator helps you find how well a sample absorbs light. It uses the Beer-Lambert law. We developed this calculator so users can find molar absorptivity with ease. You enter absorbance, concentration, and path length. The tool then gives the result fast.
Molar absorptivity shows how well a substance absorbs light. A high value means strong light absorbance. A low value means weaker absorbance.
Think of it like a light filter. A strong filter blocks more light than a weak one. In lab work, this value can help compare samples at a set wavelength.
Molar absorptivity is also called the molar absorption coefficient. It is often used with UV-Vis data and the Beer-Lambert law.
The main Beer-Lambert law is:
A = ε × c × l
To find molar absorptivity, use:
ε = A ÷ (c × l)
Here, A means absorbance. It has no unit. ε means molar absorptivity. c means concentration in mol/L. l means path length in cm.
The common unit for molar absorptivity is:
L mol⁻¹ cm⁻¹
This formula is the core of the calculator.
Keep your units correct. This step matters. If needed, convert concentration to mol/L first.
Suppose the absorbance is 0.500. The concentration is 0.000020 mol/L. The path length is 1 cm.
Use the formula:
ε = A ÷ (c × l)
ε = 0.500 ÷ (0.000020 × 1)
ε = 0.500 ÷ 0.000020
ε = 25,000 L mol⁻¹ cm⁻¹
So, the molar absorptivity is 25,000 L mol⁻¹ cm⁻¹.
A molar absorptivity calculator saves time and cuts down math work. It uses the Beer-Lambert law to find ε from absorbance, concentration, and path length.
Just enter valid values and keep the units right. The calculator does the rest.
The formula is:
ε = A ÷ (c × l)
The common unit is L mol⁻¹ cm⁻¹.
It means the sample absorbs light more strongly at the chosen wavelength.
Yes. Absorbance has no unit.
Enter the actual path length of the cell or cuvette. A common value is 1 cm.
The standard formula gives molar absorptivity in L mol⁻¹ cm⁻¹ when concentration is in mol/L and path length is in cm.