1. Center for Advanced Energy Studies
Corrosion and Its control
Dr Harikrishna Erothu
Associate Professor
Center for Advanced Energy Studies
K L University

2. Natural Abundance of Metals
In the form of oxides, carbonates, chlorides, silicates etc.
Dr Harikrishna Erothu

3. Corrosion: The destructive and unintentional degradation of metallic material, through an unwanted chemical or electrochemical attack by its environment
Introduction, why to study corrosion, cause of corrosion
Dry or Chemical Corrosion
Wet or Electrochemical Corrosion
Types:
Dr Harikrishna Erothu

4. Dry or Chemical Corrosion
Oxidation Corrosion
Corrosion by other gases
Liquid Metal Corrosion
Dr Harikrishna Erothu

5. Oxidation Corrosion
Oxygen present in the atmosphere attacks the metal surface
– formation of oxide layers
Mechanism:
Nature of the Oxide: When oxidation starts, a thin layer of oxide film will be formed on the surface and the nature of the film decides the further action!
i.e. Porous film or non-porous film
Dr Harikrishna Erothu

6. Pilling – Bedworth rule
If the volume of the metallic oxide is equal or greater in volume to the metal surface
- The metal surface is compact, non-porous - protective
Eg. Cu, In, Al, Ni, Cr forms oxides whose volume is greater than the volume of the metal
If the volume of the metallic oxide is less than the volume of the metal surface
- The oxide layer is porous, non-protective
Eg. Alkali and alkaline earth metals – Li, Na, K, Mg
Dr Harikrishna Erothu

7. The oxide films are classified as
Stable oxide layer
A fine-grain of oxide which forms a compact surface adhered tightly to the parent metal surface
Eg. Oxides of Al, Sn, Cu, etc.
Impervious in nature (which cuts of the penetration of O2)
Such a films behaves like a protective Coating
2. Unstable oxide layer
Oxides of noble metals such as platinum, silver, Au etc.
Dr Harikrishna Erothu

8. Oxide layers volatilize as soon as they are formed Excessive corrosion
3. Volatile layer
Oxide layers volatilize as soon as they are formed
Excessive corrosion
Molybdenum oxide (MoO3)
4. Porous Oxide layer
Oxide layers with minute pores
Volume of the oxide layer is ……….. than metal
Corrosion ……………..
Dr Harikrishna Erothu

9. Corrosion by other gases
(other than oxygen in the absence of moisture)
SO2, CO2, Cl2, H2S, F2 etc.
The extent of corrosive effect depends mainly on the chemical affinity between the metal and gas
It can form Protective layer (AgCl) Eg: 2 Ag + Cl2→ 2AgCl
Non-protective (SnCl4)
Liquid Metal Corrosion
Chemical action of flowing liquid metal at high temperatures on solid metal or alloy
a. dissolution of solid metal by liquid metal
b. internal penetration of the liquid metal in to the solid metal
H2 Embrittlement: Formation of cracks and blisters on metal surface due to high pressure of H2 gas, Fe + H2S → FeS + H2
Dr Harikrishna Erothu

10. Wet or Electrochemical Corrosion
When a conducting liquid is in contact with the metal
When two dissimilar metals or alloys either immersed or partially dipped in a solution
Existence of separate “anodic” and “cathodic” areas/parts, between which current flows through the conducting solution
At Anode (oxidation)
Corrosion Always occurs at anode
Eg: Fe + O2  + H2O → Fe(OH)2
Dissolves in solution
The formation of anodic and cathodic areas should have a contact with each other
Presence of conducting medium
Corrosion occurs only at anodic area
Formation of corrosion product is somewhere between anodic and cathodic areas
Forms compounds like oxides
At Cathode (Reduction) - Gain of electrons
Cathodic reactions do not affect the cathode – Most of the metals can’t be reduced
Dr Harikrishna Erothu

11. The principle of electrochemical corrosion is involved in the following types of corrosion
Hydrogen Evolution Corrosion
Oxygen absorption corrosion
Acidic environment:
Hydrogen evolution: All metals above H2 in electrochemical series undergo this type of corrosion
Example: Iron metal in contact with HCl, 2H+ + 2e-→ H2
Dr Harikrishna Erothu

12. Oxygen absorption corrosion
Neutral or basic environment:
Absorption of oxygen: Formation of hydroxide ion type corrosion.
½ O2 + 2e- + H2O→ 2OH-
Example: Iron metal in contact with a neutral solution.
Net Corrosion is Fe2+ + 2OH- →Fe(OH)2
Eg. Rusting of iron in neutral medium in the presence of oxygen,
Copper fitting on a steel pipe carrying water. Steel pipe acts as the anode and copper fitting, the cathode. Water acts as electrolyte, allowing for migration of the ions, and completion of the circuit.
Dr Harikrishna Erothu

13. Types of Wet Corrosion (a) Galvanic Corrosion (b) Pitting Corrosion
There are different types of corrosions based on the reactions and physical states.
(a) Galvanic Corrosion
(b) Pitting Corrosion
(c) Stress Corrosion
(d) Water-line Corrosion
(e) Differential aeration Corrosion
(f) Inter granular corrosion
(g) Crevice Corrosion
Dr Harikrishna Erothu

14. Galvanic Corrosion (bimetallic corrosion)
When 2 dissimilar metals (different potentials) are connected and exposed to an electrolyte, they form a galvanic cell. The anodic metal is oxidized and it undergoes corrosion.
Zinc and copper metals connected with each other in an electrolyte medium form galvanic cell. Zinc acts as anode, undergoes corrosion while cathode is unaffected.
Eg. Steel pipe connected to Cu
Dr Harikrishna Erothu

15. Pitting Corrosion
Due to crack on the surface of a metal, local straining of metal, sliding under load, chemical attack, there is formation of a local galvanic cell. The crack portion acts as anode and rest of the metal surface acts as cathode. It is the anodic area which is corroded and the formation of a pit is observed.
Presence of external impurities such as sand, dust, scale embedded on the surface of metals lead to pitting.
Eg. Stainless steel and Aluminum show pitting in chloride solution.
Dr Harikrishna Erothu

16. Stress Corrosion
In a metallic structure, if there is a portion under stress, it acts as anode and rest part of the structure acts as cathode. It is now a galvanic system and hence anodic part which is small in area would corrode more.
Eg. Caustic embrittlement is a type of stress corrosion occurring in steel tank (Boiler) at high temperature and in alkaline medium. Boiler water has Na2CO3; it is hydrolyzed at high temperature to give NaOH. It flows into hair cracks and crevices, reacts with iron and forms Na2FeO2 which decomposes to give Fe3O4 and NaOH. NaOH thus formed further reacts with iron to cause corrosion. It is called caustic embrittlement.
Fe +2NaOH → Na2FeO2 (sodium ferroate) + H2
3Na2FeO2 + 3H2O→ Fe3O4 (ferric oxide) + H2 + 6NaOH
Dr Harikrishna Erothu

17. Water-line Corrosion
It’s observed in the case of an iron tank containing water, that the portion of iron tank just below the water level undergoes corrosion. It is due to the difference in oxygen concentration.
Corroding portion is poor in oxygen and acts as anode.
At Anode: Fe → Fe2+ + 2e-
At cathode: ½ O2 + 2e- + H2O→ 2OH-
Net Reaction: Fe2+ + 2OH- →Fe(OH)2
Dr Harikrishna Erothu

18. Differential aeration Corrosion
When a metal rod is dipped in an electrolyte, the portion dipped in water is poor in oxygen concentration and works as anode which gets corroded and the portion above water acts as cathode which is protected.
The system acts as a concentration cell and the chemical reactions for zinc dipped in water are given as:
At Anode: Zn→ Zn e-
At Cathode: ½ O2 + 2e- + H2O→ 2OH-
Net Reaction: Zn + H2O + ½ O2 → Zn(OH)2
Dr Harikrishna Erothu

19. Inter granular corrosion
This corrosion is observed in case of alloys. The corrosion product is observed at the boundaries of grains. Externally not visible and There is a sudden failure of material due to this Corrosion.
Eg. During the welding of stainless steel (an alloy of Fe, C, Cr), chromium carbide is precipitated at the grain boundaries and the region adjacent to grain boundaries becomes depleted of chromium composition and is made anodic with respect to solid solution within the grains richer in chromium. Rapid quenching after heat treatment of a metal is the remedy of inter-granular corrosion.
Dr Harikrishna Erothu

20. Crevice Corrosion
Crevice corrosion occurs when two components are joined close together to form a crevice.
Corrosion occurs as the crevice accumulates water. If the crevice is small enough a differential oxygen concentration in the water can form. When this happens the base of the crevice becomes anodic to the upper region.
Crevice corrosion often occurs under bolts and rivet heads as well as in shielded areas and under dirt or sand deposits.
Dr Harikrishna Erothu

21. Galvanic Series: A metal having higher position can reduce other metals that have lower position in the series
Dr Harikrishna Erothu
Decreasing order of activity of a series of metals

22. Electrochemical Series
Dr Harikrishna Erothu

23. Factors Influencing Corrosion
Nature of the Metal
Effect of Environment
Position of metal in galvanic series
Temperature
Humidity
Purity of the metal
Impurities in the atmosphere
Relative areas of anode and cathode
pH value
Physical state of the metal
O2 concentration and Formation of O2 concentration cell
Nature of the oxide film
Volatility and Solubility of
Corrosion products
Dr Harikrishna Erothu

24. Corrosion Control 1. Proper Designing
Avoid contact of dissimilar metals
Anodic material should be large
Dissimilar metals should be as close as possible in galvanic series
Insulating fitting between dissimilar metals
Anodic material should not be painted
Prevent inhomogenities
No sharp edges or corners & crevices in joints
Free circulation of air
Uniform flow of liquids
Prevent some areas of structure to stress
Dr Harikrishna Erothu

25. Corrosion Control 2. Using pure metal (impurity causes corrosion)
3. Using metal alloys (should be homogeneous)
4. Modifying the environment
i. De-aeration (removes O2)
ii. Deactivation (Na2SO3, N2H4 absorb oxygen)
iii. Dehumidification (adding alumina or silica gel)
iv. Alkaline neutralization (CO2, H2S, SO2 & HCl give acidic medium responsible for corrosion and are neutralised by NH3 or NaOH or lime)
Dr Harikrishna Erothu

26. Corrosion Control
5. Corrosion Inhibitors – Reduce the rate of corrosion
Two types - anodic and cathodic Inhibitors
Anodic Inhibitors - form sparingly soluble products which are adsorbed on the surface of metal, protect from corrosion
Eg. Phosphate, chromate and tungstate protect anode
Cathodic Inhibitors - organic amines, mercaptans, thiourea and substituted urea, delay reduction reaction occurs at cathode
6. Cathodic protection (Electrochemical method)
Sacrificial anodic protection
Impressed current cathodic protection
Dr Harikrishna Erothu

27. Sacrificial anodic protection
Underground steel pipes are protected from corrosion by this method
A magnesium rod is fixed near the metal under protection and both are connected with a conducting wire. Magnesium is more positive than iron (electrochemical cell) Mg acts as anode and iron (Fe) acts as cathode.
According to the principle of galvanic cell, it is anode that undergoes oxidation and hence, corrosion occurs at anode saving cathode (iron) from corrosion. Thus, magnesium sacrifice itself for saving the iron. Mg Fe
Dr Harikrishna Erothu

28. Impressed current cathodic protection
The object to be protected is made as cathode and it is connected to the negative terminal of a DC (direct current) source. The positive terminal of the source is connected to the other electrode made of graphite or platinum, lead or nickel
The impressed current opposes the galvanic current (corrosion current) and, hence, protection from corrosion takes place
Eg. Recent paints that automatically fill the gap if any scratches are there and protect the metal from corrosion
Dr Harikrishna Erothu

29. Electroplating - organic surface coatings
An electrochemical process in which a base metal is coated by Zn, Ag, Cr, Au, Sn etc. to protect it from corrosion and also to make it shine and decorative. The base metal is made cathode, dipped in a suitable electrolyte, and the metal to be deposited is made an anode.
They not only protect from corrosion but also give a good look to the metal.
Organic coats must have chemical inertness, good surface adhesiveness and non-effectiveness towards inorganic chemicals and water.
Dr Harikrishna Erothu

30. Electroplating - Purification
Before subjecting to electroplating process, it is essential to clean the surface of object. The following methods are used to clean the metal surface.
Solvent cleaning: Organic solvents such as Trichloro ethylene and methylene chloride are used to remove organic matter and grease on the surface of cathode. Trichloro ethylene is used to remove paint varnishes, films, resins and Per chloro ethylene is used to remove high melt waxes and cleaning printed circuit board (PCB).
Alkali cleaning: After solvent cleaning, the metal is cleaned with alkali  solutions such as soaps, detergents, sodium carbonate,  sodium hydroxide, sodium phosphate etc.
Mechanical cleaning: The object is subjected for mechanical cleaning to remove oxide scales, rust and other impurities on the metal surface. This method involves cleaning with bristle brushes, mechanical polishing, grinding using polishing machines and sand blasting.
Pickling: In this method the oxides scales are removed by dipping the base metal in a dilute acids. Pickling of steel involves dipping in dilute HCl or dilute H2SO4 to remove rust and other oxide scales.
Rinsing with water: After surface cleaning process, the metallic surface is thoroughly rinsed with water, dried and subjected for electroplating process.
Dr Harikrishna Erothu

31. Electroplating of Copper
Procedure: Cathode - the cleaned article is made as cathode.
Anode: the anode is the coating metal itself or an inert material of good electrical conductivity like graphite.
Electrolyte: the electrolyte is a solution of a soluble salt of the coating metal. The anode and cathode are dipped in the electrolyte. When direct current is passed, coating metal ions migrate to the cathode and get deposited there. A thin layer of coating metal is obtained on the article made as cathode.
For brighter and smooth deposits, low temperature, medium current density, low metal-ion concentration
Dr Harikrishna Erothu

32. Electroplating of Copper
Process in steps:
Step 1: The metal to be electroplated is first treated with organic solvents like CCl4 (carbon tetra chloride) to remove oils, greases etc.,
Step 2: The metal to be coated i.e. the base metal after step-1 is cleaned with dil. HCl to remove scales or the oxide layer.
Step 3: Anode - pure copper, Cathode - base metal
Electrolyte is CuSO4 solution taken in an electrolytic tank. Anode and Cathode are immersed in the electrolyte.
At anode: Cu (s) Cu2+ (aq) + 2e- (Oxidation) Copper is dissolved
At cathode: Cu2+ (aq) + 2e Cu (s) (Reduction) Copper is deposited
Reactions:
Dr Harikrishna Erothu

33. Electroplating of Copper
Sulphate bath
Cyanide bath
Plating bath solution
g CuSO4,
50-75 g H2SO4, per L of bath solution
40-50 g CuCN, g
KCN, 10 g K2CO3 per L
Operating temperature C C
Current density
20-50 mA/cm2
10-40 mA/cm2
Addition agents
Gelatin, dextrin, sulphur containing brighteners, sulphonic acids
Sodium thiosulphate
Current efficiency (%)
95-99
60-90
Dr Harikrishna Erothu