Balance the following skeleton reaction and identify the oxidizing and reducing agents: Include the states of all reactants and products in your balanced equation. You do not need to include the states with the identities of the oxidizing and reducing agents.

BH4−(aq) + ClO3−(aq) → H2BO3−(aq) + Cl−(aq) [basic]

a. The oxidizing agent is:
b. The reducing agent is:

Answer :

a. The oxidizing agent is:

b. The reducing agent is:

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.

Reducing agent : It is defined as the agent which helps the other substance to reduce and itself gets oxidized. Thus, it will undergo oxidation reaction.

Oxidizing agent : It is defined as the agent which helps the other substance to oxidize and itself gets reduced. Thus, it will undergo reduction reaction.

The given chemical reaction is,

The oxidation-reduction half reaction will be :

Oxidation :

Reduction :

Now balance oxygen atom on both side.

Oxidation :

Reduction :  

Now balance hydrogen atom on both side.

Oxidation :

Reduction :

Now balance the charge.

Oxidation :

Reduction :

In order to balance the electrons, we multiply the oxidation reaction by 6 and reduction reaction by 4 and then added both equation, we get the balanced redox reaction.

Oxidation :

Reduction :

The balanced chemical equation in acidic medium will be,

In the redox reaction, act as oxidizing agent and act as an reducing agent.

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