What does Beer's law state about the relationship between absorbance and concentration?

Beer's law, also known as the Beer-Lambert law, articulates that absorbance is directly proportional to the concentration of a solute in a solution. This means that as the concentration of the solute increases, the absorbance measured at a specific wavelength also increases. This relationship allows for quantitative analysis of substances by measuring their absorbance and determining their concentration through calibration curves.

The law can be mathematically expressed as A = εlc, where A is the absorbance, ε is the molar absorptivity, l is the path length of the light through the solution, and c is the concentration of the solute. This direct proportionality makes it possible for chemists to use absorbance readings to deduce concentrations in various analytical applications, including clinical chemistry tests.

The incorrect options focus on relationships that do not align with the principles outlined by Beer's law, either suggesting that absorbance decreases with increasing concentration, is independent of concentration, or varies with factors like temperature, which are not defined in the law itself.