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       #Post#: 1174--------------------------------------------------
       Re: Properties of hydrogen peroxide
   DIR By: Shiva
       Date: November 19, 2012, 11:42 am
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       Yes, commercial sample is bit yellowish in color sometimes as it
       is contaminated with sulfur and hydrogen sulfide. So, prolong
       storage may lead to pressure build up and even sometimes
       produces explosive mixtures with air. You may perceive
       disagreeable odor as a result of this. It is better to use now
       and then haha.
       Shiva
       
       #Post#: 1175--------------------------------------------------
       Re: Properties of hydrogen peroxide
   DIR By: Michel
       Date: November 19, 2012, 1:16 pm
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       Interesting... Anyway, back to the original topic...one of the
       interesting properties of H2O2 is it's ease with which it
       participates in redox reactions. It could be difficult to
       predict if H2O2 would function as an oxidizing agent or reducing
       agent, especially with compounds of transition metals.
       #Post#: 1178--------------------------------------------------
       Re: Properties of hydrogen peroxide
   DIR By: Shiva
       Date: November 19, 2012, 3:16 pm
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       Absolutely. It normally happens when two oxidizing agents fight.
       The victory of an oxidizing agent lies in gaining electrons or
       itself reduces. These reactions are really helpful to determine
       the strength of an oxidizing agent. Hydrogen peroxide is a
       typical oxidizing agent, it is neither an aggressive oxidizing
       agent like Chlorates or Ozone nor like weaker ones like Silver
       oxide or some oxides of Nitrogen. Hydrogen peroxide is
       reasonably strong. Hence, it mostly behaves as an oxidizing
       agent. But, when competes with stronger oxidizing agents like
       Potassium permanganate, well, it has no other option. It has to
       lose.
       Shiva
       #Post#: 1187--------------------------------------------------
       Re: Properties of hydrogen peroxide
   DIR By: Michel
       Date: November 20, 2012, 1:14 pm
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       --- Quote from: Shiva link ---
       >
       > Absolutely. It normally happens when two oxidizing agents
       fight. The victory of an oxidizing agent lies in gaining
       electrons or itself reduces. These reactions are really helpful
       to determine the strength of an oxidizing agent. Hydrogen
       peroxide is a typical oxidizing agent, it is neither an
       aggressive oxidizing agent like Chlorates or Ozone nor like
       weaker ones like Silver oxide or some oxides of Nitrogen.
       Hydrogen peroxide is reasonably strong. Hence, it mostly behaves
       as an oxidizing agent. But, when competes with stronger
       oxidizing agents like Potassium permanganate, well, it has no
       other option. It has to lose.
       >
       > Shiva
       >
       --- End Quote ---
       Interesting...but then, why would H2O2 reduce CuCO3 in Cl- ?
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