The photo above illustrates a laser beam being attenuated by soap. As the laser penetrates deeper into the sample less light is available for collection. If we apply this example to spectroscopy, the pathlength would be the physical distance between where the laser beam enters the sample and the location of the detector.

Three Examples of Pathlength Placement:

1. 1) If the detector is placed just below the surface of the liquid, a great deal of light can be collected. However very little of the sample will interact with the laser. This is not ideal because we likely will not have enough absorbance, signal, for good readings.
2. 2) If the detector is placed at the very bottom of the cylinder the opposite occurs, almost none of the laser light will reach the detector and we will have no signal. It would be difficult to distinguish between the laser being on or off.
3. 3) Ideally, the detector should be placed near the 4 mL on the cylinder. By locating the detector, a distance of approximately 10 mm under the surface of the liquid, we provide a sufficient amount of the liquid to interact with the laser, while still collecting a large number of photons.

Another example Guided Wave recommends two different pathlengths for APHA color applications.

Available Pathlength Sizes

Typical pathlength sizes are 2, 5, 10, 20, 30, 50, and 100 mm. Custom pathlengths are available. For well-established applications, we typically know what the pathlength should be. For new applications we can make educated assumptions based on its 35+ years of experience. Occasionally test samples of the analyte are required to determine the best pathlength selection.

The Math and Science of Pathlength

Using Spectroscopy to measure physical properties and chemical concentrations depends on our ability to define a mathematical equation. The equation relates the variation in the chemical composition of our sample with the changes in how light interacts with the sample. This is defined by Beer-Lambert’s Law.

Beer-Lambert Law

• The relationship between chemical concentration and spectral absorbance is defined by Beer-Lambert Law.
• The Molar Absorptivity represents how sensitive the chemical is to a specific wavelength of light.
• This is a constant/inherent property defined by physics. Pathlength and concentration are the remaining two variables that alter the absorbance levels measured by the spectrometer.
  • We cannot control the concentration, as it is the value we are attempting to measure.
  • This leaves pathlength as the variable to adjust to achieve absorbance values within the dynamic range of the detector.

Still Need Help Selecting a Pathlength?

We can select a pathlength that provides the best solution from a technical and economic standpoint. Finding the balance between the signal-to-noise of the measurement and cost to manufacture, as well as accessibility for cleaning/maintenance by the user is always our priority.