The dilute aqueous solution of `H_(2)O_(2)` turns blue litmus red. True/False

Answer

To determine whether the statement "The dilute aqueous solution of H₂O₂ turns blue litmus red" is true or false, we can analyze the properties of hydrogen peroxide (H₂O₂) in a dilute solution.

### Step-by-Step Solution:

1. **Understanding Hydrogen Peroxide (H₂O₂):**
- Hydrogen peroxide is a chemical compound that can act as a weak acid in aqueous solution.

2. **Ionization of H₂O₂:**
- When dissolved in water, H₂O₂ partially ionizes to produce hydrogen ions (H⁺) and peroxide ions (O₂²⁻).
- The ionization can be represented as:
\[ H₂O₂ \rightleftharpoons H⁺ + O₂²⁻ \]
- However, this ionization is not complete; it is only partial.

3. **Acidic Nature:**
- Since H₂O₂ can release H⁺ ions, it exhibits weak acidic behavior.
- Acids typically turn blue litmus paper red because they increase the concentration of H⁺ ions in the solution.

4. **Sufficient H⁺ Ion Concentration:**
- In the case of dilute H₂O₂, the concentration of H⁺ ions produced is not sufficient to significantly change the color of blue litmus paper.
- Therefore, while it is weakly acidic, it does not produce enough H⁺ ions to turn blue litmus red.

5. **Conclusion:**
- Since the dilute aqueous solution of H₂O₂ does not produce enough H⁺ ions to turn blue litmus red, the statement is **False**.

### Final Answer:
The statement "The dilute aqueous solution of H₂O₂ turns blue litmus red" is **False**.

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