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Balancing Redox Equations | Chemistry Class 11 - NEET PDF Download

Balancing of Redox Chemical Equations

Every chemical equation must be balanced according to the law of conservation of mass. In a balanced chemical equation, the atoms of various species involved in the reactants and products must be equal in number. 

Redox reaction can be balanced through 

  1. Oxidation number method
  2. Half Reaction method

Difference between Oxidation Number Method & Half Reaction MethodDifference between Oxidation Number Method & Half Reaction Method

Oxidation Number Method

When writing equations for oxidation-reduction reactions, similar to other reactions, you need to know the compositions and formulas of the substances involved in the reaction and those that are produced.

Steps for balancing Redox Equations by Oxidation Number method

  • Step 1: Begin by writing the unbalanced (skeletal) redox equation, including all known reactants and products.
  • Step 2: Assign oxidation numbers to all atoms in the equation, placing them above each element's symbol.
  • Step 3: Identify which elements have undergone a change in oxidation number. Generally, two elements are involved: one with an increase in oxidation number (reducing agent) and one with a decrease (oxidizing agent).
  • Step 4: Determine the total increase or decrease in oxidation number for each element. If multiple atoms of the same element are involved, calculate the total oxidation change, then multiply this by the number of atoms that experienced the change.
  • Step 5: To maintain balance, equate the total increase in oxidation numbers with the total decrease by adjusting the coefficients of the oxidizing and reducing agents on the reactant side.
  • Step 6: Balance the remaining atoms in the equation, except for hydrogen and oxygen.
  • Step 7: Balance hydrogen and oxygen:
    Acidic Solution: If the reaction occurs in an acidic solution, add H⁺ ions to the side lacking hydrogen.
    Basic solution: Add H₂O molecules to the side deficient in hydrogen and, at the same time, add an equal number of OH⁻ ions to the opposite side.
  • Step 8: Simplify the final equation by canceling out any identical species that appear on both sides of the equation.

Balancing Redox Equations | Chemistry Class 11 - NEET

Let's understand it by the following example 

Zn + HCl →  ZnCl2 + H2

It involves the following steps.

Step I: Write the skeleton equation (if not given).

Zn + HCl →  ZnCl2 + H2

Step II: Assign the oxidation number of each atom.Balancing Redox Equations | Chemistry Class 11 - NEET

Step III:  The oxidation number of zinc increases from 0 to +2, while hydrogen’s oxidation number decreases from +1 to 0. The oxidation number of chlorine, however, stays the same on both sides of the reaction. Thus, zinc acts as the reducing agent, and HCl serves as the oxidizing agent, as shown in the changes below.

Balancing Redox Equations | Chemistry Class 11 - NEETStep IV: The increase and decrease in oxidation number per atom can be indicated as: Balancing Redox Equations | Chemistry Class 11 - NEET

Step V: The increase in oxidation number of 2 per atom can be balanced with decrease in oxidation number of 1 per atom if Zn atoms are multiplied by 1 and HCl by 2. Consequently the equation will be:

Zn + 2HCl →  ZnCl2 + H2

Step VI: Balance all other atoms on both sides of the equation.

Zn + 2HCl →  ZnCl2 + H2

Question for Balancing Redox Equations
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Which method can be used to balance redox chemical equations?
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Half Reaction Method

In this approach, you balance each half of the equation separately and then combine them to create a balanced overall equation. This method of balancing was developed by Jette and Lamer in 1927.

Balancing Redox Equations | Chemistry Class 11 - NEET

Steps for balancing a chemical equation using the ion-electron method (half-reaction method):

Step 1: Identify elements that have changed oxidation numbers, and select the oxidizing and reducing agents.

Step 2: Split the equation into two half-reactions: one for the oxidizing agent’s change and one for the reducing agent’s change.

Step 3: Balance each half-reaction by:

(i) Balancing all atoms except H and O.

(ii) Adjusting oxidation numbers by adding electrons to the necessary side.

(iii) Ensuring both sides have the same charge.

(iv) Adding water molecules to finalize the balance.

Step 4: Combine the two balanced half-reactions, multiplying as needed to equalize electrons between them.

Redox reactions can occur in acidic, basic, or neutral media. In acidic media, H⁺ ions appear in the equation; in basic media, OH⁻ ions are present; and in neutral media, neither H⁺ nor OH⁻ ions appear. Adjustments may be needed depending on the medium.

Let's understand this with an example:

Cu + HNO3 → Cu(NO3)2 + NO + H2O

It involves the following steps:

Step I: Write the redox reaction in ionic form.

Cu + H+ + NO3 → Cu2+ + NO + H2O

Step II: Split the redox reaction into its oxidation half and reduction half-reaction.

Balancing Redox Equations | Chemistry Class 11 - NEET

Step III: Balance atoms of each half-reaction (except H and O) by using simple multiples.

Cu → Cu2+ and NO3 → NO

(Except for H and O, all atoms are balanced)

Step IV: Balance H and O as

(i) For acidic and neutral solutions- Add the H2O molecule to the side deficient in oxygen and H+ to the side deficient in hydrogen.Balancing Redox Equations | Chemistry Class 11 - NEET(ii) For alkaline solutions- For each excess of oxygen, add one water molecule to the same side and OH ion to the other side to balance H.

Step V: Add electrons to the side deficient in electrons.

Balancing Redox Equations | Chemistry Class 11 - NEETStep VI: Equalize the number of electrons in both reactions by multiplying a suitable number.

Balancing Redox Equations | Chemistry Class 11 - NEETStep VII: Add the two balanced half-reactions and cancel common terms of opposite sides.

Balancing Redox Equations | Chemistry Class 11 - NEETStep VIII: Convert the ionic reaction into molecular form by adding spectator ions.

Balancing Redox Equations | Chemistry Class 11 - NEET

(Ions that are present in solution but do not take part in the redox reaction are omitted while writing the net ionic equation of a reaction and are known as spectator ions.)

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Solved Examples

Example: Balance the following Reaction
VO2+ + MnO4¯ ---> V(OH)4+ + Mn
2+

Solution:

1) Half reactions:

VO2+ ---> V(OH)4+
MnO4¯ ---> Mn2+

2) Balance:

3H2O + VO2+ ---> V(OH)4+ + 2H+ + e¯
5e¯ + 8H+ + MnO4¯ ---> Mn2+ + 4H2O

3) Equalize electrons:

15H2O + 5VO2+ ---> 5V(OH)4+ + 10H+ + 5e¯
5e¯ + 8H+ + MnO4¯ ---> Mn2+ + 4H2O

4) Add:

11H2O + 5VO2+ + MnO4¯ ---> 5V(OH)4+ + Mn2+ + 2H+

Example: Balance the equation for the reaction of a stannous ion with pertechnetate in an acidic solution. Products are stannic ions, Sn4+, and technetium(IV), and Tc4+ ions.

Solution:

1) Net ionic:

TcO4¯ + Sn2+ ---> Tc4+ + Sn4+

2) Half-reactions:

TcO4¯ ---> Tc4+
Sn2+ ---> Sn4+

3) Balance:

3e¯ + 8H+ + TcO4¯ ---> Tc4+ + 4H2O
Sn2+ ---> Sn4++ 2e¯

4) Equalize electrons:

6e¯ + 16H+ + 2TcO4¯ ---> 2Tc4+ + 8H2O
3Sn2+ ---> 3Sn4++ 6e¯

5) Add:

16H+ + 2TcO4¯ + 3Sn2+ ---> 2Tc4+ + 3Sn4+ + 8H2O

Example: Solve the net ionic equation where potassium dichromate(VI) (K2Cr2O7) reacts with sodium sulphite (Na2SO3) in an acidic medium to form sulphate ion and chromium(III) ion.

Solution:

Step 1-

The basic equation or the skeletal form of the reaction is

Balancing Redox Equations | Chemistry Class 11 - NEET

Step 2-

Correctly assign oxidation numbers to Cr and S

Balancing Redox Equations | Chemistry Class 11 - NEET

Therefore, from the reaction we can decipher that dichromate ion is the oxidant in the reaction and the sulphite ion is the reductant in the reaction

Step 3-

Calculation of the increase and the decrease in the oxidation number for making each side of the equation equal

Balancing Redox Equations | Chemistry Class 11 - NEET

Step 4-

We know from the equation, the reaction occurs in the acidic medium. Moreover, we can see that the ionic charges in both the sides of the equation are not same. Therefore, we will add 8H+ I order to make the ionic charges equal.

Balancing Redox Equations | Chemistry Class 11 - NEET

Step 5-

In the final step, we will calculate the required amount of water molecules and add it on the right side of the equation to make the equation a balanced redox reaction. In the given equation, we will need to add 4 water molecules on the right side to balance the equation.

Balancing Redox Equations | Chemistry Class 11 - NEET

Example: Write the balanced redox equation by half-reaction method when Permanganate(VII) ion (MnO4) produces iodine molecule (I2)  and manganese (IV) oxide (MnO2) in a basic medium.

Solution:

Step 1-

Firstly, we will write the base form of the equation

Balancing Redox Equations | Chemistry Class 11 - NEET

Step 2-

In this step, we will find the two half-reactions and write them

Oxidation Half

Balancing Redox Equations | Chemistry Class 11 - NEET

Reduction Half

Balancing Redox Equations | Chemistry Class 11 - NEET

Step 3-

We will balance the iodine atoms present in the oxidation half of the reaction. Therefore, the equation will become

Balancing Redox Equations | Chemistry Class 11 - NEET

Step 4-

We will balance the oxygen atoms in the reduction half of the reaction by the addition of two water molecules. Refer to the equation below

Balancing Redox Equations | Chemistry Class 11 - NEET

Now, we will balance the H atoms by the addition of four H+ ions on the left half of the reduction half-reaction.

Balancing Redox Equations | Chemistry Class 11 - NEET

We know that the reaction occurs in a basic medium. Thus, to balance four H+ ions, we need to add four OH ions to each side of the equation.

Balancing Redox Equations | Chemistry Class 11 - NEET

Finally, we will interchange the H+ ions and OH– ions with the water molecule. The final equation of the fourth step will be

Balancing Redox Equations | Chemistry Class 11 - NEET

Step 5-

The charges on the two half-reactions are balanced

Balancing Redox Equations | Chemistry Class 11 - NEET

Balancing Redox Equations | Chemistry Class 11 - NEET

Finally, we have to equalize the electrons in the above reactions. Thus, we will multiply the oxidation half of the equation by 3 and the reduction half of the reaction by 2.

Balancing Redox Equations | Chemistry Class 11 - NEET

Balancing Redox Equations | Chemistry Class 11 - NEET

Step 6-

We have to determine the net reaction by the addition of two halves of the reaction and by the cancellation of electrons on each side.Balancing Redox Equations | Chemistry Class 11 - NEET

Step 7-

Finally, we have to verify the equation in terms of the number of atoms and charges on both sides. Additionally, verification needs to be done about the equations written on both sides.

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FAQs on Balancing Redox Equations - Chemistry Class 11 - NEET

1. What is the oxidation number method for balancing redox equations?
Ans. The oxidation number method involves assigning oxidation numbers to all elements in the reaction. By comparing the oxidation numbers of the reactants and products, one can identify which elements are oxidized (increase in oxidation number) and which are reduced (decrease in oxidation number). Balancing involves ensuring that the total increase in oxidation numbers equals the total decrease, often by adding electrons to the half-reactions.
2. How do you use the half-reaction method to balance redox equations?
Ans. The half-reaction method involves separating the oxidation and reduction processes into two half-reactions. Each half-reaction is balanced for mass and charge, typically by adding electrons. After balancing both half-reactions, they are combined back into one equation, ensuring that the electrons cancel out. This method is particularly useful in acidic or basic solutions.
3. What are some common mistakes to avoid when balancing redox equations?
Ans. Common mistakes include failing to assign oxidation numbers correctly, not balancing all atoms in the half-reactions, overlooking the need for electrons, and neglecting to account for the medium (acidic or basic) in which the reaction occurs. It’s also important to ensure that the number of electrons lost in oxidation equals the number gained in reduction.
4. Can you provide an example of a redox reaction and how to balance it using both methods?
Ans. Consider the reaction between zinc and copper(II) sulfate: Zn + CuSO4 → ZnSO4 + Cu. Using the oxidation number method, we assign oxidation numbers: Zn goes from 0 to +2 (oxidized), and Cu goes from +2 to 0 (reduced). The balanced equation would be Zn + Cu²⁺ → Zn²⁺ + Cu. Using the half-reaction method, we write Zn → Zn²⁺ + 2e⁻ (oxidation) and Cu²⁺ + 2e⁻ → Cu (reduction), then combine both half-reactions.
5. How are redox reactions relevant for NEET and other competitive exams?
Ans. Redox reactions are fundamental in chemistry and are frequently included in the NEET syllabus, particularly in sections related to inorganic chemistry and electrochemistry. Understanding how to balance these equations is crucial for solving problems related to reaction mechanisms, stoichiometry, and real-world applications such as batteries and metabolic processes. Mastery of these concepts can significantly improve performance in exams.
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