Question

BALANCE THE FOLLOWING E QUATION IN BASIC SOLUTION ClO- + I- Cl- + I2

Answer 1

Cl in ClO- has oxidation state of +1
Cl in Cl- has oxidation state of -1
So, Cl in ClO- is reduced to Cl-

I in I- has oxidation state of -1
I in I2 has oxidation state of 0
So, I in I- is oxidised to I2





Reduction half cell:
ClO- + 2e- --> Cl-
Oxidation half cell:
2 I- --> I2 + 2e-
Number of electrons is same in both half reactions.
So, balancing of electrons is not required. It's already balanced

Lets combine both the reactions.
ClO- + 2 I- --> Cl- + I2
Balance Oxygen by adding water

ClO- + 2 I- --> Cl- + I2 + H2O

Balance Hydrogen by adding H+
ClO- + 2 I- + 2 H+ --> Cl- + I2 + H2O

Add equal number of OH- on both sides as the number of H+
ClO- + 2 I- + 2 H+ + 2 OH- --> Cl- + I2 + H2O + 2 OH-

Combine H+ and OH- to form water
ClO- + 2 I- + 2 H2O --> Cl- + I2 + H2O + 2 OH-

Remove common H2O from both sides
Balanced Eqn is
ClO- + 2 I- + H2O --> Cl- + I2 + 2 OH-
This is balanced chemical equation in basic medium
Answer:

ClO^- + 2 I^- + H₂O --> Cl^- + I₂ + 2 OH^-