Balance the following skeleton reaction and identify the oxidizing and reducing agents: Include the states of all reactants and

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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:________

Chemistry

1 answer:

Alekssandra [3K] · Answer 1 · 2026-02-27T06:26:22+03:00

Answer:

a. The oxidizing agent is: $BH_4^-$

b. The reducing agent is: $ClO_3^-$

Explanation:

Redox reaction, or oxidation-reduction reaction: It refers to a reaction where oxidation and reduction occur at the same time.

Oxidation reaction: It defines a reaction where a substance loses electrons, resulting in an increase in the oxidation state of that element. In essence, oxidation denotes the loss of electrons.

Reduction reaction: This describes a reaction where a substance acquires electrons, with the oxidation state of the element decreasing. Thus, reduction is characterized by the gain of electrons.

Reducing agent: This is the agent that facilitates the reduction of another substance while itself undergoing oxidation. Hence, it partakes in the oxidation reaction.

Oxidizing agent: This agent assists another substance in oxidation while experiencing reduction itself, participating in the reduction reaction.

The provided chemical reaction is,

$BH_4^-(aq)+ClO_3^-(aq)\rightarrow H_2BO_3^-(aq)+Cl^-(aq)$

Half-reactions for oxidation and reduction are as follows:

Oxidation: $BH_4^-\rightarrow H_2BO_3^-$

Reduction: $ClO_3^-\rightarrow Cl^-$

Next, balance the oxygen atoms on each side.

Oxidation: $BH_4^-\rightarrow H_2BO_3^-+3H_2O$

Reduction: $ClO_3^-+3H_2O\rightarrow Cl^-$

Next, balance hydrogen atoms on both sides.

Oxidation: $BH_4^-+4OH^-\rightarrow H_2BO_3^-+3H_2O$

Reduction: $ClO_3^-+3H_2O\rightarrow Cl^-+6OH^-$

Then balance the charges.

Oxidation: $BH_4^-+4OH^-\rightarrow H_2BO_3^-+3H_2O+4e^-$

Reduction: $ClO_3^-+3H_2O+6e^-\rightarrow Cl^-+6OH^-$

To balance the electrons, multiply the oxidation reaction by 6 and the reduction reaction by 4, and then sum both equations to acquire the balanced redox reaction.

Oxidation: $6BH_4^-+24OH^-\rightarrow 6H_2BO_3^-+18H_2O+24e^-$

Reduction: $4ClO_3^-+12H_2O+24e^-\rightarrow 4Cl^-+24OH^-$

The balanced chemical reaction in an acidic environment is,

$6BH_4^-+4ClO_3^-\rightarrow 6H_2BO_3^-+6H_2O+4Cl^-$

$3BH_4^-+2ClO_3^-\rightarrow 3H_2BO_3^-+3H_2O+2Cl^-$

In the redox reaction, $ClO_3^-$ functions as the oxidizing agent and $BH_4^-$ serves as the reducing agent.