Respuesta :
[tex]Mn^{2+} +8OH^{-} --\ \textgreater \ MnO_{4}^{-} + 4H_{2}O +5e^{-}
\\ \\ +2-8=(-6) ----\ \textgreater \ ( -1)+5e^{-}[/tex]
Answer : The balanced oxidation half reaction in basic medium will be :
[tex]Mn^{2+}(aq)+8OH^-(aq)\rightarrow MnO_4^-(aq)+4H_2O(l)+5e^-[/tex]
Explanation :
Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.
Rules for the balanced chemical equation in basic solution are :
- First we have to write into the two half-reactions.
- Now balance the main atoms in the reaction.
- Now balance the hydrogen and oxygen atoms on both the sides of the reaction.
- If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the more number of oxygen are present.
- If the hydrogen atoms are not balanced on both the sides then adding hydroxide ion [tex](OH^-)[/tex] at that side where the less number of hydrogen are present.
- Now balance the charge.
The balanced oxidation half reaction in basic medium will be :
[tex]Mn^{2+}(aq)+8OH^-(aq)\rightarrow MnO_4^-(aq)+4H_2O(l)+5e^-[/tex]
