A sample of iron ore is dissolved in acid, and the iron isconverted to Fe2*. The sample is then titrated with 47.20mL of 0.02240 M MnO4 solution. The oxidation-reductionreaction that occurs during titration is as follows:MnO4(aq) + 5FE2*(aq) + 8H*(aq) → Mn²*(aq) + 5FE3* (aq) +4H2OHow many moles of MnO4¯ were added to the solution?Blank 12+How many moles of Fewere in the sample? Blank 2How many grams of iron were in the sample? Blank 3If the sample had a mass of 0.8890 g, what is thepercentage of iron in the sample? Blank 4Blank 1Add your answerBlank 2Add your answerBlank 3Add your answerBlank 4Add your answer

Given Volume of MnO4- =47 .20 ml Molarity =0.02240 M

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

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...

See similar textbooks

Similar questions

For a product to be legally called "vinegar", it must contain at lest 5.0% by mass of acetic acid, HAc(a weak monoprotic acid with molar mass 60.05 g/mol). A 10.00 g sample of "Cartman's Yummy Vinegar" is titrated with 0.1250 M KOH (aq). It takes 56.14 mL of the KOH (aq) to completely neutralize the HAc in the sample. The percentage by mass of HAc in the sample is?
To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a 46.0g sample in strong acid and titrates it to the endpoint with 130.mL of 0.1900M potassium permanganate KMnO4 solution. The balanced chemical equation for the reaction is: 8H+(aq) + 5Fe2+(aq) + MnO−4(aq) -> 5Fe3+(aq) + Mn2+(aq) 4H2O(l) What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Fe in the sample. Be sure your answer has the correct number of significant digits.
Consider the net ionic equation: Cr2O72- + 6Fe2+ + 14H+ = 2Cr3+ + 6Fe3+ + 7H2O. If it takes 26.0 mL of 0.0250 M Cr2O72-(aq) to titrate 25.0 mL of a solution containing Fe2+, what is the molar concentration of Fe2+?
To measure the amount of calcium carbonate (CaCo,) in a seashell, an analytical chemist crushes a 4.800 g sample of the shell to a fine powder and titrates it to the endpoint with 190. ml. of 0.4000 Mhydrogen chloride (HCI) solution. The balanced chemical equation for the reaction is: 2HCI(ag) + Co, (aq) - H,CO,(aq) + 2C1 (ag) O precipitation What kind of reaction is this? O acid-base O redox If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of CaCO, in the sample. Be sure your answer has 0% the correct number of significant digits.
Redox Reactions
The following reaction occurs when two aqueous solutions are mixed: Cr(NO3)3(aq) + 3NaOH(aq) → Cr(OH)3(s) + 2NaNO3(aq) Identify the spectator ion OR ions in the solution. SELECT ALL SPECTATOR IONS!
Write the net ionic equation for this reaction.
Balance the "molecular" equation for the above reaction: Cu (s) + HNO3 (aq) → Cu(NO3)2 (aq) + NO2 (g) + H20 (1)
The amount of I3−(aq) in a solution can be determined by titration with a solution containing a known concentration of S2O32−(aq) (thiosulfate ion). The determination is based on the net ionic equation 2S2O32−(aq)+I3−(aq)⟶S4O62−(aq)+3I−(aq) Given that it requires L44.0 mL of 0.240 M Na2S2O3(aq) to titrate a 30.0 mL sample of I3−(aq), calculate the molarity of I3−(aq) in the solution.
SIMPLE REACTIONS Writing nebionic equations The following chemical reaction takes place in aqueous solution: 2 Fe(NO;),(aq)+3 Na,S(aq) →Fe,S;(s)+6 NaNO,(aq) Write the net ionic equation for this reaction.
In the reaction 2 HCl(aq) + Zn(s) ⟶ZnCl2(aq) + H2(g), what is the reducing agent and what is the oxidizing agent.
The following reaction is a precipitation reaction. NaCl (aq) + AgNO3 (aq) → NaNO3 (aq) + AgCl (s) a metal displacement a decomposition an acid-base neutralization