A solution containing a mixture of the compounds X and Y had an absorbance of 0.

Question

A solution containing a mixture of the compounds X and Y had an absorbance of 0.585 at 443 nm and an absorbance of 0.502 at 520 nm when measured with a 1.00 cm cell. The molar absorptivities (?) of X and Y at each wavelength are shown in the table below.

A solution containing a mixture of the compounds X and Y had an absorbance of 0.585 at 443 nm and an absorbance of 0.502 at 520 nm when measured with a 1.00 cm cell. The molar absorptivities (epsilon) of X and Y at each wavelength are shown in the table below. What are the concentrations of X and Y in this mixture?

Explanation / Answer

we will use lambert beer's law which is

A = eCl

A= absorbance

e = extinction coefficient

C = conc

l = pathh length

so for a mixture A at 443nm = (e x Cx x l) + (e x Cy x l)

0.585 = (16430 x Cx x 1) + (3877 x Cy x 1) ................(1)

similarly at 520 nm, 0.502 =(3997 x Cx x 1) + (6431 x Cy x 1).....................(2)

So, solving 2 simulataneous equations,

Cx = [X] = 2.01E-5M

Cy = [Y] = 6.55E-5

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