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REDOX Titration

  1. Mar 13, 2010 #1
    1. The problem statement, all variables and given/known data
    Give the net ionic equation for this reaction:

    Fe(NH4)2(SO4)2.6H2O + KMnO4


    2. Relevant equations

    Reducing reaction is

    4H+ + MnO4- + 3e ---> MnO2 + 2H2O

    Oxidation

    3Fe+2 ---> 3Fe+3 + 3e


    3. The attempt at a solution

    4H+ + MnO4- + 3Fe+2 ---> MnO2 + 2H2O + 3Fe+3

    My question is is this a basic or acidic solution? I'm assuming acidic because ammonium with have a tendancy to lose it's H+. Is this the net ionic equation or do I have to include more? Can someone confirm wether or not my answer is corrent
     
  2. jcsd
  3. Mar 13, 2010 #2

    Borek

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    Staff: Mentor

  4. Mar 13, 2010 #3
    sweet so it looks like My equation was correct.
     
  5. Mar 13, 2010 #4

    Borek

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    No - MnO2 ad Mn2+ are two different things.

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  6. Mar 13, 2010 #5
    Hmmmm. The website you provided me with says Permanganate can be reduced into MnO2, Mn2+, or MnO4(-2) depending on the pH. Does this mean I have to use my molar concentrations to figure out which one it is?
     
  7. Mar 13, 2010 #6

    Borek

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    I don't remember titration methods that will not reduce permangante to Mn2+. This is the only way of being sure that the reaction can't proceed further and hence has known stoichiometry.

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  8. Mar 13, 2010 #7
    Thank You. The reaction that shoyuld take place is then.

    5Fe2+ + MnO4- + 8H+ → 5Fe3+ + Mn2+ + 4H2O
     
  9. Mar 13, 2010 #8

    Borek

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    Correct.

    --
    methods
     
  10. Apr 28, 2010 #9
    I know im going to sound like a complete moron but im lost! In my high school they offer this chemistry class. They call it pre-college chemistry. Well i am more confused than britany spears on crack. I need help with redox reaction???
     
  11. Apr 29, 2010 #10

    Borek

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    Staff: Mentor

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