State True or False
Rusting of `Fe` is quicker in saline water than in ordinary water.

Explanation

**Step-by-Step Solution:**

1. **Understanding Rusting**: Rusting of iron (Fe) is a chemical process where iron reacts with moisture and oxygen in the environment, resulting in the formation of a reddish-brown layer known as rust, which is primarily composed of iron(III) oxide (Fe2O3·xH2O).

2. **Rusting in Different Environments**: Rusting can occur in both ordinary water and saline (saltwater) environments. The presence of moisture and oxygen is essential for rusting to take place.

3. **Effect of Salts on Rusting**: Saline water contains dissolved salts, primarily sodium chloride (NaCl). The presence of these salts introduces additional ions (Na⁺ and Cl⁻) into the water.

4. **Conductivity and Electrochemical Reactions**: The presence of ions in saline water increases its electrical conductivity. Higher conductivity facilitates electrochemical reactions, which are integral to the rusting process. In this scenario, iron acts as the anode, where it gets oxidized to Fe²⁺ ions.

5. **Comparison of Rusting Rates**: Due to the increased mobility of ions and higher conductivity in saline water, the rusting process occurs more rapidly compared to ordinary water, which lacks significant amounts of salts and thus has lower conductivity.

6. **Conclusion**: Therefore, the statement "Rusting of Fe is quicker in saline water than in ordinary water" is **True**.

---