Join 60,000+ competitive exam aspirants
Which of the following is the most effective method to prevent the corrosion of iron structures in highly saline coastal environments?
Painting the iron surface
Galvanization
Simple oiling
Storing in a humid chamber
Galvanization
Galvanization coats iron with a layer of zinc, which acts as a sacrificial anode and protects the underlying iron from corrosion.
Galvanization coats iron with a layer of zinc, which acts as a sacrificial anode and protects the underlying iron from corrosion.
It is like assigning a bodyguard (zinc) who takes all the attacks so the VIP (iron) stays safe.
Zinc Saves Iron (ZSI).
Zn→Zn2++2e− — oxidation of zinc (sacrificial)
Fe→Fe2++2e− — corrosion of iron
Zinc, being more electro‑positive than iron, preferentially oxidises (Zn→Zn2++2e−). The released electrons flow to the iron surface, preventing its oxidation (Fe→Fe2++2e−) and thus inhibiting rust formation, especially in chloride‑rich sea‑air.
Zinc has a more negative electrode potential than iron.
The zinc coating provides both barrier protection and sacrificial protection.
Long‑lasting protection (10–20 years).
Effective in highly corrosive, salty environments.
Initial cost higher than simple painting.
If the coating is damaged, corrosion can start at the exposed spot.
Marine structures, ship hulls, offshore platforms.
Bridges, steel water pipelines, automobile chassis.
| Feature | Painting | Galvanization |
|---|---|---|
Protection Mechanism | Physical barrier (paint) | Sacrificial anode (zinc coating) |
Standard hot‑dip galvanizing uses ~0.5 mm zinc coating.
Option A (painting) merely slows corrosion and can fail quickly in salty spray.
B is correct — galvanization provides sacrificial protection that outperforms painting in saline conditions.
Remember that the metal with the lower (more negative) standard electrode potential acts as the sacrificial anode, so zinc protects iron.