Solutions of naphthalene in ethanol absorb at λ=312 nm . A 2.50 ×10^-3 mol dm^-3 solution gives

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Solutions of naphthalene in ethanol absorb at λ=312 nm . A...

Solutions of naphthalene in ethanol absorb at $\lambda=312 \mathrm{nm} .$ A $2.50 \times 10^{-3} \mathrm{mol} \mathrm{dm}^{-3}$ solution gives an absorbance of 0.72. Determine the concentration of a solution for which the absorbance is $1.00 .$ The same solution cell was used for both readings.

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Key Concepts

Direct Proportionality Between Absorbance and Concentration

In a fixed-path-length cell with a constant molar absorptivity, the absorbance of a solution is directly proportional to its concentration. This principle means that any change in absorbance is directly associated with a proportional change in concentration, which is critical for quantitative analysis in spectroscopy.

Calibration Using Standard Solutions

Calibration using standard solutions involves determining the instrument's response (absorbance) for a known concentration, which can then be used to infer the concentration of unknown samples. This technique is essential for ensuring accuracy in measurements and is widely applied in analytical methods to establish a reliable concentration-absorbance relationship.

Beer-Lambert Law

The Beer-Lambert Law is a fundamental principle in spectroscopy that relates the absorbance of a solution to the concentration of the absorbing species, the path length of the light through the solution, and the molar absorptivity coefficient. This linear relationship, expressed as A = ?lc, allows one to calculate unknown concentrations based on measured absorbance values.

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