A sample of iron ore is dissolved in acid, and the iron is converted to Fe2+. The sample is then titrated with 47.20 mL of 0.02240 M MnO4¯ solution. The oxidation-reduction reaction that occurs during titration is as follows: MnO4(aq) + 5FE2*(aq) + 8H*(aq) 4H2O Mn2*(aq) + 5FE3+ (aq) + How many moles of MnO4 were added to the solution? Blank 1 How many moles of Fe 2+ were in the sample? Blank 2 How many grams of iron were in the sample? Blank 3 If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample? Blank 4
A sample of iron ore is dissolved in acid, and the iron is converted to Fe2+. The sample is then titrated with 47.20 mL of 0.02240 M MnO4¯ solution. The oxidation-reduction reaction that occurs during titration is as follows: MnO4(aq) + 5FE2*(aq) + 8H*(aq) 4H2O Mn2*(aq) + 5FE3+ (aq) + How many moles of MnO4 were added to the solution? Blank 1 How many moles of Fe 2+ were in the sample? Blank 2 How many grams of iron were in the sample? Blank 3 If the sample had a mass of 0.8890 g, what is the percentage of iron in the sample? Blank 4
Chapter4: Types Of Chemical Reactions And Solution Stoichiometry
Section: Chapter Questions
Problem 109AE: The blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with an...
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