Predict the absorbance of a solution made using 12 mL of 0.345 M [Fe2+] and 8mL

Question

Predict the absorbance of a solution made using 12 mL of 0.345 M [Fe2+] and 8mL of 0.456 M [Ligand] than diluting to 100 mL( Take into account that n which is moles of ligand/moles Fe2+ is 2.8)

Equations given: A= ELC

A= absorbance, E= epsilon (given as 12500), L= length of cell (given as 1.00cm), and C= concentration (in Molar)

I think that C needs to be found, but I really dont see how... the problem seems to be pointing to the N value as the conversion factor that helps to find C, but I'm not seeing which value going in the actual equation

Thank you for your help!!!!

Explanation / Answer

Predict the absorbance of a solution made using 12 mL of 0.345 M [Fe2+] and 8mL of 0.456 M [Ligand] than diluting to 100 mL( Take into account that n which is moles of ligand/moles Fe2+ is 2.8)

Final conc of [Fe2+]=[0.345M*12mL/100mL]=0.0414M

Final conc of Ligand=0.456M*8mL/100mL=0.03648M

since n=moles of ligand/moles of Fe2+=2.8/1

Fe2+ + 2.8 Ligand ==>product (therefore ligand is a limiting reatant) hence moles or molarity of Fe2+ consumed will be

moles of Fe2+ consumed=0.03648M/2.8=0.013M=Molarity of product

Equations given: A= ELC

A= absorbance, E= epsilon (given as 12500), L= length of cell (given as 1.00cm), and C= concentration (in Molar)

Now you can proceed

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