**Iron Ore Analysis Using Titration**A 3.41 g sample of iron ore is transformed into a solution of iron(II) sulfate, FeSO₄. This solution is titrated with 0.160 M K₂Cr₂O₇ (potassium dichromate). If it requires 42.8 mL of potassium dichromate solution to titrate the iron(II) sulfate solution, what is the percentage of iron in the ore? The chemical reaction involved is as follows:\[ 6\text{FeSO}_4(aq) + \text{K}_2\text{Cr}_2\text{O}_7(aq) + 7\text{H}_2\text{SO}_4(aq) \rightarrow 3\text{Fe}_2(\text{SO}_4)_3(aq) + \text{Cr}_2(\text{SO}_4)_3(aq) + 7\text{H}_2\text{O}(l) + \text{K}_2\text{SO}_4(aq) \]Calculate the percentage of iron in the ore using the data provided.**Percentage =** \(\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\) % **Submit Answer** **Try Another Version** *3 item attempts remaining*

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Answered: References A 3.41 g sample of iron ore…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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All I need is an answer. An explanation is not required.
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