A sample of iron ore weighing 0.2812 g was dissolved in an excess of a dilute acid solution. All the iron was first converted to Fe(II) ions. The solution then required 21.70 mL of 0.0184 M KMnO4 for oxidation to Fe(III) ions. Calculate the percent by mass of iron in the ore. _____% by mass of Fe
A sample of iron ore weighing 0.2812 g was dissolved in an excess of a dilute acid solution. All the iron was first converted to Fe(II) ions. The solution then required 21.70 mL of 0.0184 M KMnO4 for oxidation to Fe(III) ions. Calculate the percent by mass of iron in the ore. _____% by mass of Fe
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
Chapter4: Types Of Chemical Reactions And Solution Stoichiometry
Section: Chapter Questions
Problem 158IP: The vanadium in a sample of ore is converted to VO2+. The VO2+ ion is subsequently titrated with...
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A sample of iron ore weighing 0.2812 g was dissolved in an excess of a dilute acid solution. All the iron was first converted to Fe(II) ions. The solution then required 21.70 mL of 0.0184 M KMnO4 for oxidation to Fe(III) ions. Calculate the percent by mass of iron in the ore.
_____% by mass of Fe
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