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8/13/2019 Corrosion of Metals : Pitting
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Copyright 2012 Industrial Metallurgists, LLC and ASM International, 2012
Corrosion of Metals
Michael Pfeifer, PhD., P.E.
Industrial Metallurgists, LLC
Northbrook, IL 60062
847.528.3467
www.imetllc.com
www.materialscoursesonline.com
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Copyright 2012 Industrial Metallurgists, LLC and ASM International, 2012
Module 6: Pitting Corrosion
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Module learning objectives
1. Explain the mechanism for pitting corrosion
2. List three alloy systems that are susceptible to pitting corrosion
3. Explain the effects of chloride concentration and exposure time on pit
density and corrosion rate.
4. List four approaches for controlling pitting corrosion
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Pitting
Localized form of corrosion
Small pits form on exposed surface and penetrate into metal
Most common on passivated metals
Can be destructive if it causes perforation of equipment and structures
• Minor pitting often tolerated as long as there is no perforation and change in
appearance is acceptable
304 stainless steel exposed to aerated salt water
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Under certain environmental conditions some active metals lose their activity
• Become passive
• Form extremely thin tightly adhering oxide film on metal surface
Passive metal can revert to active state at localized areas of the surface
• Large increase in corrosion rate at these localized areas
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Reversion to active state can occur for various reasons
Changes in environment
• Change of concentration of corrosive species
• Electrolyte chemistry may vary because of a surface deposit
Metallurgical features
•
Inclusions or second phase particles, or the regions surrounding these features, may bepreferentially attacked.
• Constituents within a grain boundary, either second-phase particles or segregation of
detrimental species, can lead to pit initiation.
Surface defects
• Discontinuity such as a scratch or a gouge
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Chloride ions (Cl-) in electrolyte a common cause of pit initiation
Pitting incubation time
• Decreases as concentration of corrosive species increases
Exposed metal in pit reverts to active
Exposed active metal has lower potential than passivated metalElectrolyte within pit more corrosive than bulk electrolyte
Passive oxide
Cl-
Cl-
Cl-
Cl- Cl-
Anode
Cathode
Cl- Cl-
Cathode
Cl-
Cl-
Cl-
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Anode: M Mn+ + ne-
Cathode: O2 + 2H2O + 4e- 4OH-
Mn+
Mn+ Mn+
Mn+
Cl- Cl-
Cl-
e-e-
OH-
OH-
OH-
OH- Cl- Cl-
Cl-
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Problem 1Which graph represents the number of pits formed per unit area as the chloride ion
concentration (Cl-) in water increases? Cl-(3) > Cl-(2) > Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(1)
Cl-(3)
Time
#
p i t s / a r e a
Cl-(2)Cl-(1)
Cl-(3)
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Problem 1Which graph represents the number of pits formed per unit area as the chloride ion
concentration (Cl-) in water increases? Cl-(3) > Cl-(2) > Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(1)
Cl-(3)
Time
#
p i t s / a r e a
Cl-(2)Cl-(1)
Cl-(3)
OK
INCORRECT
Increased number of
chloride ions means
more active species to
cause corrosion
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Copyright 2012 Industrial Metallurgists, LLC and ASM International, 2012
Problem 1Which graph represents the number of pits formed per unit area as the chloride ion
concentration (Cl-) in water increases? Cl-(3) > Cl-(2) > Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(1)
Cl-(3)
Time
#
p i t s / a r e
a
Cl-(2)Cl-(1)
Cl-(3)
OK
CORRECT
Expect that the number
of pits increases with
time.
Increased number of
chloride ions means
more active species to
cause corrosion.
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Copyright 2012 Industrial Metallurgists, LLC and ASM International, 2012
Problem 1Which graph represents the number of pits formed per unit area as the chloride ion
concentration (Cl-) in water increases? Cl-(3) > Cl-(2) > Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(1)
Cl-(3)
Time
#
p i t s / a r e a
Cl-(2)Cl-(1)
Cl-(3)
OK
INCORRECT
This graph shows that a
large number of pits
quickly forms and then
the number of pits
decreases with time.
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Copyright 2012 Industrial Metallurgists, LLC and ASM International, 2012
Problem 1Which graph represents the number of pits formed per unit area as the chloride ion
concentration (Cl-) in water increases? Cl-(3) > Cl-(2) > Cl-(1)
Time
#
p i t s / a r e
a
Cl-(2)Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(3)
Cl-(1)
Time
#
p i t s / a r e a
Cl-(2)
Cl-(1)
Cl-(3)
Time
#
p i t s / a r e
a
Cl-(2)Cl-(1)
Cl-(3)
OK
INCORRECT
This graph shows that a
large number of pits
quickly forms and then
the number of pits
decreases with time.
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Copyright 2012 Industrial Metallurgists, LLC and ASM International, 2012
Effect of chloride concentration on pitting rate
Increase chloride concentration
• Decreased incubation time
• Increased # pits formed at any given time
Time
#
p i t s / a r e
aCl-(2)
Cl-(3)
Cl-(1)
Cl-(3) > Cl-(2) > Cl-(1)
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Problem 2Increasing the temperature (T) of a solution generally increases the tendency
towards pitting. Which graph best represents this? T(3) > T(2) > T(1)
Chloride concentration
T e n d e n c y t o
p i t
T(1)
T(2)
T(3)
Chloride concentration
T e n d e n c y t o
p i t
T(3)
T(2)
T(1)
Chloride concentration
T e n d
e n c y
t o
p i t
T(1) T(2)T(3)
Chloride concentration
T e n d e n c y
t o
p i t
T(3)T(2)
T(1)
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Problem 2Increasing the temperature (T) of a solution generally increases the tendency
towards pitting. Which graph best represents this? T(3) > T(2) > T(1)
Chloride concentration
T e n d e n c y
t o
p i t
T(1)T(2)
T(3)
Chloride concentration
T e n d e n c y
t o
p i t
T(3)T(2)
T(1)
Chloride concentration
T e n d e
n c y
t o
p i t
T(1) T(2)T(3)
Chloride concentration
T e n d e n c y
t o
p i t
T(3) T(2)T(1)
OK
INCORRECT
Shows that tendency to
pit increases as the
temperature decreases
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Copyright 2012 Industrial Metallurgists, LLC and ASM International, 2012
Problem 2Increasing the temperature (T) of a solution generally increases the tendency towards pitting.
Which graph best represents this? T(3) > T(2) > T(1)
Chloride concentration
T e n d e n c y t o
p i t
T(1)
T(2)
T(3)
Chloride concentration
T e n d e n c y t o
p i t T(3)
T(2)
T(1)
Chloride concentration
T e n
d e n c y
t o
p i t
T(1)T(2)
T(3)
Chloride concentration
T e n d e n
c y
t o
p i t
T(3)T(2)
T(1)
OK
CORRECT
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Problem 2Increasing the temperature (T) of a solution generally increases the tendency
towards pitting. Which graph best represents this? T(3) > T(2) > T(1)
Chloride concentration
T e n d e n c y
t o p
i t
T(1)T(2)
T(3)
Chloride concentration
T e n d e n c y
t o
p i t
T(3)T(2)
T(1)
Chloride concentration
T e n d
e n c y
t o
p i t
T(1)T(2)
T(3)
Chloride concentration
T e n d e n
c y
t o
p i t
T(3)T(2)
T(1)
OK
INCORRECT
This graph shows the
tendency to pit
decreases as the
chloride concentration
increases.
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Problem 2Increasing the temperature (T) of a solution generally increases the tendency
towards pitting. Which graph best represents this? T(3) > T(2) > T(1)
Chloride concentration
T e n d e n c y
t o
p i t
T(1)T(2)
T(3)
Chloride concentration
T e n d e n c y
t o
p i t
T(3)T(2)
T(1)
Chloride concentration T e n d e n
c y
t o
p i t
T(1)T(2)
T(3)
Chloride concentration T e n d e
n c y
t o
p i t
T(3) T(2)T(1)
OK
INCORRECT
This graph shows the
tendency to pit
decreases as thechloride concentration
increases.
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Influence of metal composition
Metals that form adherent, passive oxides most susceptible to pitting
Chromium and its alloys Aluminum and its alloys
Titanium and its alloys
Metals that contain these elements in sufficient quantities
• Stainless steels containing > 12% chromium
Within each set of alloys some have better pitting resistance than others
• Specific elements present in the alloys
• Microstructural features
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Aluminum alloys
Pitting resistance depends on purity
Purest metal most resistant
1xxx alloys (best pitting resistance)
5xxx alloys
3xxx alloys
6xxx alloys
7xxx alloys
2xxx alloys (lowest pitting resistance)
Decreasing pitting resistance
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Controlling pitting corrosion
Often unexpected
• Affects alloys selected based on their corrosion resistance
•
Susceptibility of an alloy to localized corrosion is often overlooked
1. Select a more corrosion-resistant metal for the application
• Selecting different alloy from a family of alloys
316 stainless steel instead of 304 stainless steel
• Select different family of alloys based on same major element
3xxx series of aluminum alloys instead of 5xxx series
• Select alloy based on a different major element
Titianium alloy instead of stainless steel
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Controlling pitting corrosion
2. Surface treatment to modify oxide layer
• Passivate stainless steels
• Expose steel to nitric acid solution, followed by alkaline rinse
• Removes surface iron particles
• Dissolves detrimental inclusions at the surface
• Forms a clean, slightly thicker passive oxide
• Anodize aluminum and titanium alloys
• Grow thick oxide by anodizing
• Normal oxide layer much less than 1 micrometer thick
• Thicker than 25 micrometers after anodization
3. Apply coating
• Usefulness of metal may be eliminated
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Controlling pitting corrosion
4. Adjust environment
• Reduce concentration of aggressive species
• Enhance passivity and avoid passive film breakdown• Difficult to implement in practice
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Module review
1. Metals that form a passive oxide are most susceptible to pitting.
2. Pitting mechanism involves a local breakdown of passive layer andformation of a corrosion cell in the area of the breakdown.
3. Chloride a major cause of pitting
• As chloride concentration increases, number of pits formed in a
particular period of time increases.
4. Four approaches to controlling pitting corrosion.
• Select a different alloy
• Surface treatment to modify the oxide layer
• Apply surface coating
• Modify environment
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End of Module 6