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Beer Lambert Law Calculator With Solution

Beer-Lambert Law:

\[ A = \epsilon \times c \times l \]

L·mol⁻¹·cm⁻¹
mol/L
cm

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1. What is the Beer-Lambert Law?

The Beer-Lambert Law relates the absorption of light to the properties of the material through which the light is traveling. It states that the absorbance (A) is directly proportional to the concentration (c) of the absorbing species and the path length (l) of the sample.

2. How Does the Calculator Work?

The calculator uses the Beer-Lambert Law equation:

\[ A = \epsilon \times c \times l \]

Where:

Explanation: The law shows that absorbance is proportional to concentration when the path length and molar absorptivity are constant.

3. Importance of Beer-Lambert Law

Details: This law is fundamental in spectrophotometry and is used to determine the concentration of solutions, study chemical kinetics, and analyze various substances in chemistry and biochemistry.

4. Using the Calculator

Tips: Select which variable you want to solve for, then enter the other three known values. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What are the limitations of Beer-Lambert Law?
A: The law assumes monochromatic light, dilute solutions, and non-interacting particles. It may not hold at high concentrations.

Q2: What is typical molar absorptivity range?
A: Typically 0-10⁵ L·mol⁻¹·cm⁻¹. Values >10⁴ are considered strong absorbers.

Q3: What is the practical absorbance range?
A: For accurate measurements, absorbance should generally be between 0.1 and 1.0.

Q4: Can I use any units for concentration?
A: The calculator uses mol/L. For other units, you'll need to convert them first.

Q5: Does temperature affect absorbance?
A: Temperature can affect the equilibrium position of some reactions, which may change absorbance, but the Beer-Lambert law itself is temperature-independent.

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