posted by .

The amount of iron in a meteorite was determined by a redox titration using KMnO4 as the titrant. A 0.4408 g sample was dissolved in acid and the liberated Fe3+ quantitatively reduced to Fe2+. Titrating with 0.0220 M KMnO4 requires 41.38 ml to reach the end point.

Unbalance reaction: Fe2+ + MnO4- → Fe3+ + Mn2+.

Determine the % w/w Fe2O3.

  • chem -

    Balance the equation.
    mols MnO4^- = M x L = ?
    Convert mols MnO4^- to mols Fe using the coefficients in the balanced equation.
    g Fe = mols Fe x molar mass Fe
    %Fe = (g Fe/mass sample)*100 = ?
    Post your work if you get stuck.

  • chem -

    im confused on how to balance

  • chem -

    Mn goes from +7 in MnO4- to +2 in Mn.
    Fe goes from +2 to +3.
    Here is a site all about redox and balancing redox equations.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    If I am titrating KMnO4 against a sample of Fe2+, but there is also I- in the sample which of the iron and iodine will be oxidised first?
  2. Chemistry

    In a previous experiment, 0.800 g of the green complex iron salt was placed in an Erlenmeyer flask and heated with concentrated sulfuric acid until all oxalate ion was destroyed (CO2, SO2 and H2O are formed). Ferric ion (Fe3+) remained …
  3. Redox Titration questions!

    Oh goodness, I'm such a pain! I need some help with these! How do I calculate the percentage?
  4. chemistry

    A 49.45 mL sample of solution containing Fe2+ ions is titrated with a 0.0103 M KMnO4 solution. It required 23.76 mL of KMnO4 solution to oxidize all the Fe2+ ions to Fe3+ by the following reaction. MnO4-(aq) + Fe2+(aq) Mn2+(aq) + Fe3+(aq) …
  5. Chemistry

    when 25.0 mL of a solution containing both Fe2+ and Fe3+ ions is titrated with 23.0 mL of 0.0200 M KMnO4 (in dilute sulfuric acid). As a result, all of the Fe2+ ions are oxidized to Fe3+ ions. Next, the solution is treated with Zn …
  6. chemistry.

    a quantity of 25 ml of a solution containing both Fe2+ and Fe3+ ions is titrated with 23 ml of .02 M KMnO4 solution. as a result all the Fe2+ ions are oxidised to Fe3+ ions. Next the solution is treated with Zn metal to convert all …
  7. Redox Titration questions!

    Calculate the percent of iron in a 50.0 gram sample containing iron if 45.6 mL of 2.5 M KMnO4 titrant was used. can you solve this?
  8. Chem

    The Fe2 (55.845 g/mol) content of a 2.271 g steel sample dissolved in 50.00 mL was determined by tiration with a standardized 0.100 M potassium permanganate (KMnO4, 158.034 g/mol) solution. The titration required 28.05 mL to reach …
  9. Chemistry

    A 0.020 M KMnO4 solution was used to determine the percent iron in a sample containing iron(II). MnO− 4 + 5 Fe2+ + 8 H+ → Mn+2 + 5 Fe3+ + 4 H2O It took 25.0 mL of the KMnO4 to completely react with all the iron(II) in the …
  10. Science

    When 25.0 ml of a solution containing both Fe2+and Fe3 +ions is titrated with 23.0 ml of 0.0200M KMnO4(in dilute sulphuric acid), all the Fe2+ are oxidised to Fe3+ ions. Next, the solution is treated with Zinc metal to convert all …

More Similar Questions