Answer:
The question is incomplete. Searching in google I found: 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 solution containing only solvent had an absorbance of 0.029 at the same wavelength. Find the molar absorptivity of compound A.
The molar absorptivity of compound A is 1502.5 M⁻¹cm⁻¹.
Explanation:
The question is incomplete. Searching in google I found: 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 solution containing only solvent had an absorbance of 0.029 at the same wavelength. Find the molar absorptivity of compound A.
The absorbance (A) is given by:
[tex] A = \epsilon cl [/tex]
Where:
c: is the concentration of compound A = 3.96x10⁻⁴ M
ε: is the molar absorptivity of compound A =?
l: is the pathlength = 1 cm
[tex]A_{s}[/tex]: is the absorbance of the solution= 0.624
[tex]A_{b}[/tex]: is the absorbance of the blank solution= 0.029
First, we need to find the absorbance of compound A:
[tex] A = A_{s} - A_{b} = 0.624 - 0.029 = 0.595 [/tex]
Now, we can calculate the molar absorptivity of compound A:
[tex] \epsilon = \frac{A}{cl} = \frac{0.595}{3.96 \cdot 10^{-4} M*1 cm} = 1502.5 M^{-1}cm^{-1} [/tex]
Therefore, the molar absorptivity of compound A is 1502.5 M⁻¹cm⁻¹.
I hope it helps you!
