Respuesta :
Answer : The balanced chemical equation in a acidic solution is,
[tex]3I^-(aq)+ClO^-(aq)+2H^+(aq)\rightarrow I_3^-(aq)+Cl^-(aq)+H_2O(l)[/tex]
Explanation :
Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.
Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.
Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.
Rules for the balanced chemical equation in acidic 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 less number of oxygen are present.
If the hydrogen atoms are not balanced on both the sides then adding hydrogen ion [tex](H^+)[/tex] at that side where the less number of hydrogen are present.
Now balance the charge.
The given chemical reaction is,
[tex]I^-(aq)+ClO^-(aq)\rightarrow I_3^-(aq)+Cl^-(aq)[/tex]
The oxidation-reduction half reaction will be :
Oxidation : [tex]I^-\rightarrow I_3^-[/tex]
Reduction : [tex]ClO^-\rightarrow Cl^-[/tex]
- First balance the main element in the reaction.
Oxidation : [tex]3I^-\rightarrow I_3^-[/tex]
Reduction : [tex]ClO^-\rightarrow Cl^-[/tex]
- Now balance oxygen atom on both side.
Oxidation : [tex]3I^-\rightarrow I_3^-[/tex]
Reduction : [tex]ClO^-\rightarrow Cl^-+H_2O[/tex]
- Now balance hydrogen atom on both side.
Oxidation : [tex]3I^-\rightarrow I_3^-[/tex]
Reduction : [tex]ClO^-+2H^+\rightarrow Cl^-+H_2O[/tex]
- Now balance the charge.
Oxidation : [tex]3I^-\rightarrow I_3^-+2e^-[/tex]
Reduction : [tex]ClO^-+2H^++2e^-\rightarrow Cl^-+H_2O[/tex]
The charges are balanced on both side of the reaction. Thus, added both equation, we get the balanced redox reaction.
The balanced chemical equation in acidic medium will be,
[tex]3I^-(aq)+ClO^-(aq)+2H^+(aq)\rightarrow I_3^-(aq)+Cl^-(aq)+H_2O(l)[/tex]
The balanced redox equation of the acidic solution is :
[tex]3I^{-} ( aq) + CIO ^{-} (aq) + 2H^{+} (aq) -- > I^{-} _{3} (aq) + CI^{-}(aq) + H_{2}O(l)[/tex]
Balancing the redox equation in acidic solution using half reaction method
First step : balance the main element in the oxidation-reduction half reaction
Oxidation : [tex]3I^{-} - > I_{3} ^{-}[/tex]
Reduction : [tex]CIO^{-} - > CI^{-}[/tex]
Next step : Balance the oxygen atom and hydrogen atom on both sides
Oxidation : [tex]3I^{-} - > I_{3} ^{-}[/tex]
Reduction : [tex]CIO^{-} + 2H^{+} - > CI^{-} + H_{2} O[/tex]
Next step : balance the charges
Oxidation : [tex]3I^{-} - > I_{3} ^{-} + 2e^{-}[/tex]
Reductio : [tex]CIO^{-} + 2H^{+} + 2e^{-} - > CI^{-} + H_{2} O[/tex]
Therefore the balanced chemical equation is gotten by adding both equations and we will get as
[tex]3I^{-} ( aq) + CIO ^{-} (aq) + 2H^{+} (aq) -- > I^{-} _{3} (aq) + CI^{-}(aq) + H_{2}O(l)[/tex]
Learn more about redox equation : https://brainly.com/question/1161855
