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Degger [83]
3 years ago
15

A 3.96x10^-24 M solution of compound A exhibited an absorbance of 0.624 at 238 nm in a 1.000-cm cuvet; a blank solution containi

ng only solvent had an absorbance of 0.029 at the same wavelength. Find the molar absorptivity of compound A.
Chemistry
1 answer:
viktelen [127]3 years ago
4 0

Actual question from source:-

A 3.96x10-4 M solution of compound A exhibited an absorbance of 0.624 at 238 nm in a 1.000 cm cuvette.  A blank had an absorbance of 0.029.  The absorbance of an unknown solution of compound A was 0.375.  Find the concentration of A in the unknown.

Answer:

Molar absorptivity of compound A = 1502.53\ {Ms}^{-1}

Explanation:

According to the Lambert's Beer law:-

A=\epsilon l c

Where, A is the absorbance

 l is the path length  

\epsilon is the molar absorptivity

c is the concentration.  

Given that:-

c = 3.96\times 10^{-4}\ M

Path length = 1.000 cm

Absorbance observed = 0.624

Absorbance blank = 0.029

A = 0.624 - 0.029 = 0.595

So, applying the values in the Lambert Beer's law as shown below:-

0.595=\epsilon\times 1.000\ cm\times 3.96\times 10^{-4}\ M

\epsilon=\frac{0.595}{3.96\times 10^{-4}}\ {Ms}^{-1}=1502.53\ {Ms}^{-1}

<u>Molar absorptivity of compound A = 1502.53\ {Ms}^{-1}</u>

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