Mass % Iron:

$\mathbf{\%}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{Fe}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{Fe}\mathbf{}\mathbf{in}\mathbf{}\mathbf{hemoglobin}}{\mathbf{molar}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{hemoglobin}}\mathbf{\times}\mathbf{100}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\mathbf{molar}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{hemoglobin}\mathbf{=}\frac{\mathbf{mass}\mathbf{}\mathbf{Fe}\mathbf{}\mathbf{in}\mathbf{}\mathbf{hemoglobin}}{{\displaystyle \frac{\mathbf{\%}\mathbf{}\mathbf{mass}\mathbf{}\mathbf{Fe}}{\mathbf{100}}}}$

- MW of Fe = 55.85 g/mol

Hemoglobin, the oxygen-carrying protein in red blood cells, has four iron atoms per molecule and contains 0.340% iron by mass. Calculate the molar mass of hemoglobin. Express your answer using three significant figures.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Mass Percent Formula concept. You can view video lessons to learn Mass Percent Formula. Or if you need more Mass Percent Formula practice, you can also practice Mass Percent Formula practice problems.