A 0.1783 g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as Fe²⁺(aq). The iron solution was titrated with Ce⁴⁺ solution according to the balanced chemical reaction shown below. After calculation, it was found that 0.0286 g of iron from the ore reacted with the cerium solution.\[ \text{Ce}^{4+}(aq) + \text{Fe}^{2+}(aq) \rightarrow \text{Ce}^{3+}(aq) + \text{Fe}^{3+}(aq) \]Calculate the mass percent of iron in the original ore sample. Please round your answer to the tenths place.\[ \text{Your Answer:} \]\[ \_\_\_\_\_\_\_\ \]Answer \hspace{4cm} units

Given: Mass of iron ore sample =0.1783 g Mass of iron that reacted with the cerium solution = 0.0285…

A 0.1783 g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as Fe (aq). The iron solution was titrated with Ce solution according to the balanced chemical reaction shown below. After calculation, it was found that 0.0285 g of iron from the ore reacted with the cerium solution. ,4+ Ce*lag) + Fe2"(aq) - Ce(aq) + Fe (aq) Calculate the mass percent of iron in the original ore sample. Please round your answer to the tenths place. Your Answer:

A 0.1783 g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as Fe (aq). The iron solution was titrated with Ce solution according to the balanced chemical reaction shown below. After calculation, it was found that 0.0285 g of iron from the ore reacted with the cerium solution. ,4+ Ce*lag) + Fe2"(aq) - Ce(aq) + Fe (aq) Calculate the mass percent of iron in the original ore sample. Please round your answer to the tenths place. Your Answer:

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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