🤓 Based on our data, we think this question is relevant for Professor TBA's class at MEMPHIS.

We are asked to calculate for the **percent by mass (mass %) of Fe ^{3}^{+} ion** in a sample of iron (II) oxide which is 75.01% iron by mass .

We’re going to use the **mass percent formula** shown below:

$\overline{){\mathbf{mass}}{\mathbf{}}{\mathbf{percent}}{\mathbf{}}{\mathbf{=}}\frac{\mathbf{mass}\mathbf{}\mathbf{component}}{\mathbf{total}\mathbf{}\mathbf{mass}}{\mathbf{\times}}{\mathbf{100}}}$

Despite Dalton’s laws, it is now known that many ionic compounds do not always contain atoms in small integer
ratios. For example, a sample of iron(II) oxide may, in fact, contain a significant amount of Fe^{3+} in addition to Fe^{2+}. This is an example of a *nonstoichiometric* compound. A sample of iron(II) oxide is found to be 75.01 % iron by mass.

Determine the percentage of Fe^{3+} ions in the sample.

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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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor TBA's class at MEMPHIS.