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Redox Titrations?

  1. May 21, 2008 #1
    1. What volume of a 0.0200 M KMnO4 solution is required to oxidize 40.0 mL of 0.100 M FeSO4 in sulfuric acid solution?



    2. MnO4-1 + H+ + Fe+2 --> Fe+3 + Mn+2 + H2O



    3. I honestly have no idea how to tackle this, I failed the titration portion of the AP Exam. I Think is maybe M1V1=M2V2 though

    1. A 20.00 mL sample of Na2SO3 was titrated with 36.0 mL of 0.0513O M K2Cr2O7 solution in the presence of H2SO4. Calculate the molarity of the Na2SO3 solution.



    2. SO3-2 + Cr2O7 + H+ --> SO4-2 + Cr+3 + H2O



    3. No idea.

    As a note, I didn't know how to do superscripts and subscripts, so the tiny ones are the amount of that element is in that cmpd, and the big italicized numbers are the charge of the ion or element.
     
  2. jcsd
  3. May 21, 2008 #2
    I would calculate how many moles of [tex]FeSO_{4}[/tex] and from that calculate how many moles of [tex]KMNO_{4}[/tex] would be needed to oxidize the compound.
     
  4. May 22, 2008 #3

    Borek

    User Avatar

    Staff: Mentor

    Most important thing: you have to balance reaction equations. Without that you won't move ahead.

    Superscripts and subscripts are done with [ sub][ /sub] and [ sup][ /sup] tags (no spaces after opening square bracket)
     
    Last edited: May 22, 2008
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