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 concentration of a substance is directly proportional to the absorbance of the solution.

2. How Does the Calculator Work?

The calculator uses the Beer-Lambert Law equation:

Where:

• \( C \) — Concentration (Molarity, M)
• \( A \) — Absorbance (unitless)
• \( \varepsilon \) — Molar extinction coefficient (M^-1cm^-1)
• \( l \) — Path length (cm)

Explanation: The equation shows that concentration is directly proportional to absorbance and inversely proportional to both the molar extinction coefficient and path length.

3. Importance of Concentration Calculation

Details: Accurate concentration determination is essential in chemistry, biochemistry, and molecular biology for preparing solutions, conducting experiments, and analyzing results.

4. Using the Calculator

Tips: Enter absorbance (typically between 0.1-1.0 for best accuracy), molar extinction coefficient (specific to your compound), and path length (usually 1 cm for standard cuvettes).

5. Frequently Asked Questions (FAQ)

Q1: What is the ideal absorbance range?
A: 0.1-1.0 absorbance units is optimal. Below 0.1 may lack precision, above 1.0 may deviate from linearity.

Q2: Where do I find the extinction coefficient?
A: Check literature or product specifications for your compound. It's wavelength-dependent.

Q3: What if my path length isn't 1 cm?
A: Measure your cuvette's actual path length or adjust the value in the calculator accordingly.

Q4: Does this work for mixtures?
A: Only for single compounds or when using the weighted average extinction coefficient for mixtures.

Q5: What are common sources of error?
A: Dirty cuvettes, air bubbles, incorrect wavelength, or exceeding the linear range of absorbance.