Calculate the concentration in ppm of a K2CrO4 solution that has a %T of 77.17 in a 4.50cm cell at 372nm, the molar absorptivity is 4,459.0 L mol-1 cm-1. [Report the result to two decimal places]
There are two equations
A = 2 - log10 (%T) ........(1)
A = e c L ........(2)
A = absorption
e = molar absorptivity
c = concentration
L = path length
%T = transmission
Using
A = 2 - log10 (%T)
= 2 - log (77.17)
= 0.11255
Putting this value in equation (2)
A = e c L
c = A/eL
= 0.11255/(4459.0x4.50)
= 5.609 x 10-6 moles/Litre
Molecular mass of K2CrO4 = 194.2 g/mol
so, c = 5.609 x 10-6 mol/L x 194.2 g/mol
= 1.089 x 10-3 g/L
= 1.089 x 10-3 x 103 mg/L
= 1.09 ppm [1 ppm = 1 mg/L]
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