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REDOX Titration

  • Thread starter Hockeystar
  • Start date
  • #1
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Homework Statement


Give the net ionic equation for this reaction:

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


Homework Equations



Reducing reaction is

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

Oxidation

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


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
 

Answers and Replies

  • #2
Borek
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  • #3
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sweet so it looks like My equation was correct.
 
  • #4
Borek
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No - MnO2 ad Mn2+ are two different things.

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  • #5
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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?
 
  • #6
Borek
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All these reactions are used in analytical chemistry, but the most popular is the use of permanganate in low pH solutions.
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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  • #7
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Thank You. The reaction that shoyuld take place is then.

5Fe2+ + MnO4- + 8H+ → 5Fe3+ + Mn2+ + 4H2O
 
  • #8
Borek
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Correct.

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methods
 
  • #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???
 
  • #10
Borek
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