That is right, use a = A/bc. A = –log(T), not –log(%T), so A = –log(0.396). The path length is "b" in the equation, normally in cm units, so 1.50 cm is correct. You do not need the wavelength for the calculation, but since absorptivity depends on the wavelength, the wavelength is given as a formality. The concentration c can be in any units. However, since the question asks for the molar absorptivity, the concentration needs to be converted to moles per liter. That's why the molar mass was given, 220 g/mol.
4. A solution concentration 3.75 mg/ml of a sample 220 g/mol has a transmittance of 39.6% in a 1.50-cm cell at 480 nm. Calculate the molar absorptivity of sample.
I know I use Beers Law:
A=abc
solve for a = A/bc
I know A is equal to -log (39.6)
b, I am unsure of but I think it is 1.50 cm, I am confused on the wavelength value of 480nm.
c, I think should be 3.75 mg/ml, but what us the 220 g/mol for?
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