Redox is a reaction in which both oxidation and reduction will take place simultaneously . It is obvious that if one substance gives electron there must be another substance to accept these electrons . In some reactions, same substance is reduced as well as oxidised, these reactions are termed as disproportionation reactions.
For calculating equivalent mass in redox reaction change in oxidtaion number is realted to n-factor which is reciprocal of molar ratio.
This reaction is an example of
`Br_(2) + OH^(-) to BrO_(3)^(-) + H_(2)O + Br^(-)`

Options

A. Oxidation reaction only
B. Reduction reaction only
C. Neutralization reaction
D. Disproportionation reaction

Answer

To solve the problem regarding the reaction \( \text{Br}_2 + \text{OH}^- \rightarrow \text{BrO}_3^- + \text{H}_2\text{O} + \text{Br}^- \), we need to analyze the oxidation states of bromine in the reactants and products to determine if this reaction is a disproportionation reaction.

### Step-by-Step Solution:

1. **Identify the Reactants and Products:**
- The reactants are \( \text{Br}_2 \) and \( \text{OH}^- \).
- The products are \( \text{BrO}_3^- \), \( \text{H}_2\text{O} \), and \( \text{Br}^- \).

2. **Determine the Oxidation States:**
- For \( \text{Br}_2 \): In its elemental form, bromine has an oxidation state of 0.
- For \( \text{BrO}_3^- \): Let the oxidation state of bromine be \( x \). The oxidation state of oxygen is -2. The equation can be set up as:
\[ x + 3(-2) = -1 \quad \Rightarrow \quad x - 6 = -1 \quad \Rightarrow \quad x = +5 \]
Thus, the oxidation state of bromine in \( \text{BrO}_3^- \) is +5.
- For \( \text{Br}^- \): The oxidation state of bromine is -1.

3. **Analyze Changes in Oxidation States:**
- The oxidation state of bromine changes from 0 in \( \text{Br}_2 \) to +5 in \( \text{BrO}_3^- \) (oxidation).
- The oxidation state of bromine changes from 0 in \( \text{Br}_2 \) to -1 in \( \text{Br}^- \) (reduction).

4. **Conclusion on Reaction Type:**
- Since one species (bromine) is both oxidized (from 0 to +5) and reduced (from 0 to -1), this reaction is classified as a disproportionation reaction.

5. **Final Answer:**
- Therefore, the given reaction \( \text{Br}_2 + \text{OH}^- \rightarrow \text{BrO}_3^- + \text{H}_2\text{O} + \text{Br}^- \) is an example of a **disproportionation reaction**.