Final Answer:
The concentration of the solution at an absorbance of 1.5 can be determined by finding the corresponding point on the calibration curve or using the Beer-Lambert law.
Step-by-step explanation:
In UV-Visible spectroscopy, the Beer-Lambert law relates absorbance to concentration and path length. The calibration curve, generated by measuring absorbance at various known concentrations, helps correlate absorbance values to concentrations.
To find the concentration at an absorbance of 1.5, reference the calibration curve at that absorbance value and determine the corresponding concentration. This involves identifying the point on the curve where the absorbance is 1.5 and reading off the concentration axis.
The Beer-Lambert law states that absorbance (A) is directly proportional to the concentration (c) and path length (l) of the sample. It's mathematically represented as A = εcl, where ε is the molar absorptivity or extinction coefficient, c is the concentration, and l is the path length. By rearranging the equation to solve for concentration, you can use A = εcl to find concentration (c) when absorbance (A) and ε (the molar absorptivity) are known.