Answer:
The absorbance of the solution is 0.21168.
Explanation:
Given that,
Wavelength = 500 nm
Molar absorptivity = 252 M⁻¹ cm⁻¹
Number of moles = 0.00140
Volume of solution = 500.0 mL
Length = 3.00 mm
We need to calculate the molar concentration
Using formula of the molar concentration
[tex]C=\dfrac{N}{V}[/tex]
Where, N = number of moles
V = volume
Put the value into the formula
[tex]C=\dfrac{0.00140}{0.5000}[/tex]
[tex]C=0.0028\ M[/tex]
We need to calculate the absorbance of the solution
Using formula of absorbance
[tex]A=\epsilon C l[/tex]
Put the value into the formula
[tex]A=252\times0.0028\times0.300[/tex]
[tex]A=0.21168[/tex]
Hence, The absorbance of the solution is 0.21168.
The absorbance of a compound, with a molar absorptivity at 500 nm wavelength of 252 M⁻¹ cm⁻¹, prepared by dissolving 0.00140 moles of a solute in enough water to make a 500.0 mL solution, measured in a 3 .00 mm pathlength cell, is 0.212.
First, we will calculate the molarity of the compound, which is equal to the moles of solute divided by the liters of solution.
[tex]M = \frac{0.00140mol}{0.5000L} = 0.00280 M[/tex]
Then, we will convert 3.00 mm to cm using the conversion factor 1 cm = 10 mm.
[tex]3.00 mm \times \frac{1cm}{10mm} = 0.300 cm[/tex]
Finally, we will calculate the absorbance of the compound using the Beer–Lambert equation.
[tex]A = \epsilon \times b \times C[/tex]
where,
[tex]A = \epsilon \times b \times C = \frac{252}{M.cm} \times 0.300 cm \times 0.00280 M = 0.212[/tex]
The absorbance of a compound, with a molar absorptivity at 500 nm wavelength of 252 M⁻¹ cm⁻¹, prepared by dissolving 0.00140 moles of a solute in enough water to make a 500.0 mL solution, measured in a 3 .00 mm pathlength cell, is 0.212.
You can learn more about the Beer–Lambert law here: https://brainly.com/question/24571070?referrer=searchResults
