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1.0 INTRODUCTION.
1.1 CORROSION.
Vast range of constructional materials such as; metals and alloys, plastics, rubber,
ceramics, composites, wood, etc, serves as the backbone for modern day technological
processes. Since metals are involved in most cases, mechanical, physical and chemical
properties must be considered, and in this connection it should be observed that whereas
mechanical and physical properties can be expressed in terms of constants, the chemical
properties of a given metal are dependent entirely on the precise environmental
conditions prevailing during service (Shreir, 1994). The interaction of a metal or alloy (or
a non-metallic material) with its environment is clearly of vital importance in the
performance of materials of construction. While a metal or alloy may be selected largely
on the basis of its mechanical or physical properties, the fact is that there are very few
applications where the effect of the interaction of a metal with its environment can be
completely ignored, although the importance of this interaction will be of varying
significance depending on the situation (Shreir, 1994).
Corrosion (Latin Corrode – to gnaw away), is the gradual deterioration of a material
caused by the chemical (or) electrochemical reaction with its environment. Corrosion has
been defined as the undesirable deterioration of a metal or alloy, i.e. an interaction of the
metal with its environment that adversely affects those properties of the metal that are to
be preserved. This definition- referred to as the deterioration definition - is also
applicable to non-metallic materials such as glass, concrete, etc. and embodies the
concept that corrosion is always deleterious (Uhlig, 1948).
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The word Corrosion stands for material or metal deterioration or surface damage in an
aggressive environment. Corrosion is a chemical or electrochemical oxidation process, in
which the metal transfers electrons to the environment and undergoes a valence change
from zero to a positive value (Perez, 2004). The environment may be a liquid, gas or
hybrid soil-liquid. These environments are called electrolytes since they have their own
conductivity for electron transfer. Though the materials undergo deterioration in very
many ways, the term “corrosion” is presently restricted to surface degradation due to the
chemical attack. Corrosion occurs when protective mechanisms have been overlooked,
broken down, or have been exhausted, leaving the metal vulnerable to attack.
The corrosion of metals can be regarded in some ways as reverse extractive metallurgy.
Most metals exist in nature in the combined state, for example, as oxides, sulphides,
carbonates, or silicates. In these combined states the energies of the metals are lower. In
the metallic state the energies of metals are higher, and thus there is a spontaneous
tendency for metals to react chemically to form compounds. For example, iron oxides
exist commonly in nature and are reduced by thermal energy to iron, which is in a higher
energy state. There is, therefore, a tendency for the metallic iron to spontaneously return
to iron oxide by corroding (rusting) so that it can exist in a lower energy state.
The scope of the term ‘corrosion’ is continually being extended; Fontana and Staehle
(1990) have stated that corrosion will include the reaction of metals, glasses, ionic solids,
polymeric solids and composites with environments that embrace liquid metals, gases,
non-aqueous electrolytes and other non-aqueous solutions .
Vermilyea,(1962) defined corrosion as a process in which atoms or molecules are
removed one at a time, this includes evaporation of a metal into vacuum, since atomically
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it is similar to other corrosion processes. Evans, (1960) considers that corrosion may be
regarded as a branch of chemical thermodynamics or kinetics, as the outcome of electron
affinities of metals and non-metals, as short-circuited electrochemical cells, or as the
demolition of the crystal structure of a metal. These considerations lead to the conclusion
that there is probably a need for two definitions of corrosion, which depend upon the
approach adopted (Uhlig, 1971; Shreir, 1994):
1. Definition of corrosion in the context of Corrosion Science: the reaction of a solid with
its environment.
2. Definition of corrosion in the context of Corrosion Engineering: the reaction of an
engineering/constructional material with its environment with a consequent deterioration
in properties of the material.
1.2 Effect of corrosion
The effects of corrosion are many and varied. Effects on the safe, reliable and efficient
operation of equipments or structures are often more serious than the simple loss of a
mass of metal. Failures of various types and the consequent expensive replacements may
occur, even though the amount of metal destroyed is quite small. The first area of
significance of corrosion studies is the economical aspect including the objective of
reducing material losses resulting from the corrosion of pipes, tanks, metal components
of machines, ships, bridges, marine structures etc. The second is the safety of operating
equipments from resulting catastrophic consequences due to corrosion. Examples are
metallic containers for radioactive materials, turbine blades and rotors, pressure vessels,
boilers, bridge cables, aeroplane components, automotive steering mechanisms. The third
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dimension of corrosion studies is conservation of materials as applied primarily to metal
resources.
It is very well known that the supply of metals is limited and their wastage include
corresponding losses of energy and water reserves associated with the production and
fabrication of metal structures. The human efforts required for the design and repair of
corroded equipments can well be utilized for other socially useful purposes.
Currently, research in corrosion is primarily motivated by the economic factors. Losses
incurred by industry, military and municipalities amount to many billions of dollars
annually. Loss due to corrosion is approximately estimated to be 3-5% of the Gross
National Product (GNP) (Jones, 1996). 15% or more could be saved by the application of
existing technologies to mitigate corrosion. The existing technologies include the
methodologies like proper design, selection of materials, coatings and linings, cathodic
protection and inhibitors (Shreir, 1994).
Economic losses due to corrosion are classified as direct losses and indirect losses. The
direct losses are the cost of replacing the corroded structures and machines or their
components such as condenser tubes, mufflers, pipelines and metal roofing including
labour cost. Direct losses also include an extra cost of using corrosion resistance metals
and alloys instead of carbon steel where the latter does have adequate mechanical
properties but not sufficient corrosion resistance. The cost of galvanizing, nickel plating
of steel, use of corrosion inhibitors, or dehumidification of storage rooms for metal
equipments also accounts for direct losses.
Indirect losses, which are more difficult to assess, may either be economical or social.
These may include contamination of the product, loss of valuable product from a
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corroded container, damage of adjacent equipment, decreased safety and production (e.g.
sudden failure of equipment may cause fire, explosion or release of toxic products) and
change of appearance.
Obviously, indirect losses are a substantial part of the economic overhead imposed due to
corrosion, although it is difficult to arrive at an accurate estimate of total losses of an
industry. The indirect losses are in fact very difficult to assess in the event of loss of
health or life through explosions, unpredictable failure of chemical equipment or
wreckage of aeroplanes, trains or automobiles through sudden failure by corrosion of
critical parts. To sum up, it can be stated that corrosion is a potent force which incurs
economic loss, depletes resources and causes irreversible and untimely failures of
industrial plants, equipments and their components.
1.3. Corrosion and its mechanism
As a first approach to the principles which govern the behaviour of metals in specific
environments it is preferable for simplicity to disregard the detailed structure of the metal
and to consider corrosion as a heterogeneous chemical reaction which occurs at a
metal/non-metal interface and involves the metal itself as one of the reactants. Therefore,
corrosion can be expressed by electrochemical reaction comprising of both anodic and
cathodic reactions.
For mild steel, the anodic reaction involves the dissolution of the metal according to
equation (1.1)
Fe Fe2+ + 2e (1.1)
At the cathode, the electrons released are utilized in the reduction of species depending
on the nature of the environment. This could involve hydrogen reduction according to
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equation (1.2) in acidic environments, reduction of oxygen in near neutral or alkaline
environments according to equation (1.3), or reduction of sulphate ions in the absence of
oxygen following equation (1.4).
2H+ + 2e H2 (1.2)
O2 + 2H2O + 4e 4OH- (1.3)
4H2 + SO42- S2- + 4H2O (1.4)
The driving force for the corrosion is the thermodynamic instability of the metal in its
surrounding environment. The electron potential of a metal is a measure of its tendency
to corrode. The metals corrode faster when dissolution potential is negative. In the
absence of any surface active compound, the oxidation of iron is the primary anodic
reaction. The possibility for the oxidation of iron in aqueous solution can best be
demonstrated by various oxide formation reactions along with their electrode potential
values (E°).
Fe + 2OH- FeO + H2O + 2e- E° = -0.422V (1.5)
3Fe + 8OH- Fe3O4 + 4H2O + 8e- E° = -0.473V (1.6)
2Fe + 6OH- Fe2O3 + 3H2O + 6e- E° = -0.431V (1.7)
Fe + H2O FeO + 2H+ +2e- E° = -0.450V (1.8)
3Fe + 4H2O Fe3O4 + 8H+ + 8e- E° = -0.421V (1.9)
2Fe + 3H2O Fe2O3 + 6H+ + 6e- E° = -0.463V (1.10)
From the values of oxide formation potentials, it is seen that iron oxidizes readily in
water and the occurrence of the above reactions depends on the potentials established on
the electrode surface. In general the chemical stability of a metal exposed to a solution is
a function of the potential of the metal with respect to the solution, and the pH of the
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solution. The regions where the various species are stable can be plotted on a map of
potential against pH, know as an E-pH or Pourbaix diagram (Pourbaix, 1974).
There are three regions in the Pourbaix diagram:
1. When the metal is in the thermodynamically stable state, the metal is immune from
corrosion.
2. When the stable species is a soluble corrosion product, the metal is said to be active,
and will corrode relatively rapidly.
3. When the stable species is an insoluble corrosion product, then the metal is said to be
passive, and will corrode relatively slowly.
The oxide formation potentials are pH dependent and the relationship between the pH
and the potential is demonstrated by Pourbaix diagram.
Fig.1.1 illustrates the Pourbaix diagram for iron in water at 250C. It shows all possible
equilibra between various anions and cations of iron (or its compound) and water
together with their nature and activities. For example, parallel lines of curve (x)
represents the equilibrium between Fe(OH)3 and Fe2+ (aq) at various activities of the latter
ranging from 100 to 10-6. The arbitrary value of 10-6 has been selected and used to
classify various regions as show in Fig.1.1.
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Fig.1.1. The Pourbaix diagram for Fe-H2O system at 250C.
(Source: www.corrosion-doctors.org)
From the diagram, three different regions of interest exists, and are discussed as follows;
Immunity zone, where the metal is in equilibrium with Fe2+(aq) or FeO2H- (aq) at an
activity less than 10-6.
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Corrosion zone, in which the activity of Fe2+, Fe3+(aq) or FeO2-(aq) is greater than 10-6
Passivation zone: in this region Fe(OH)2, Fe3O4 or Fe(OH)3 are in equilibrium with metal
ions at an activity less than 10-6. However, due to the lack of kinetic information, the
Pourbaix diagram can not be used to predict the rate of metallic corrosion.
1.4. Forms of corrosion.
Corrosion can affect the metal in a variety of ways which depend on its nature and the
precise environmental conditions prevailing, leading to the various forms of corrosion
identified below;
1.4.1. Pitting Corrosion.
This form of corrosion is extremely localized and shows itself as holes on a metal
surface. The initial formation of pits is difficult to detect due to the small size, but it
requires a prolong time for visual detection. Pitting corrosion may occur due to
breakdown of a protective film (passive oxide film or organic coating). This form of
corrosion can be found on aluminum and its alloys and automobile chromium-plated
bumpers or body coated (painted) parts due to film breakdown at isolated surface sites.
Pits vary in shape, but are very small surface holes due to the extremely localized anodic
reaction sites (Schreir, 1979).
The appearance of pits on a metal surface is not very appealing, but they can be harmless
if perforation does not occur. The initiation of pits occurs at localized sites on a metal
surface defects, which may be due to coating failure, mechanical discontinuities or
microstructural phase heterogeneities such as secondary phases (Vereecken, 1994.).
Besides the prolong time needed for pit formation or its growth, it is assumed that many
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anodic and cathodic reactions take place at localized sites. Both rates of anodic and
cathodic reactions are slow; however, the reactions continue inward in the direction of
gravity in most cases. This suggests that the bottoms of pits are rich in metal ions due to
the large number of anodic reactions.
1.4.2. Crevice Corrosion.
Crevice corrosion is similar to pitting corrosion after its initiation stage in a stagnant
electrolyte. This form of corrosion initiates due to changes in local chemistry such as
depletion of oxygen in the crevice, increase in pH with increasing hydrogen
concentration [H+], and increase of chlorine Cl- ions. Oxygen depletion implies that
cathodic reaction for oxygen reduction cannot be sustained within the crevice area and
consequently, metal dissolution occurs. The problem of crevice corrosion can be
eliminated or reduced using proper sealants and protective coatings. The mechanism of
crevice corrosion is electrochemical in nature. It requires a prolong time to start the metal
oxidation process, but it may be accelerated afterwards (Fontana, 1986).
1.4.3. Stress-Corrosion Cracking
Structural parts subjected to a combination of a tensile stress and a corrosive environment
may prematurely fail at a stress below the yield strength. This phenomenon is known as
environmentally induced cracking (EIC), which is divided into the following categories:
stress-corrosion cracking (SCC), hydrogen-induced cracking (HIC) and corrosion-fatigue
cracking (CFC) (Vereecken, 1994). These three categories can develop under the
influence of an applied potential. It is known that SCC occurs under slow strain-rate
(SSR) ) only if the tensile strain rate or the applied potential is within a narrow and yet,
critical range; otherwise metals and alloys would appear to be immune to SCC either due
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to film repair at low strain rates or mechanical failure at high strain rates. The primary
characteristic of HIC is the brittle mechanical fracture caused by diffusion of atomic
hydrogen into the material because hydrogen is very small and has the capability of
migrating through the crystal lattice (Vereecken, 1994). The detrimental effect of atomic
hydrogen diffusion on mechanical properties is a continuous decrease in ductility (as well
as in strength). This particular mechanism is also known in the literature as hydrogen
embrittlement (HE) and it is a form of irreversible hydrogen damage. If hydrogen atoms
within the lattice defects, such as voids, react to form molecular hydrogen, and these
molecules form babbles, then the metallurgical damage is called blistering.
1.4.4. Underground Corrosion.
Factors affecting the corrosivity of a given soil include porosity, electrical conductivity,
dissolved salts, moisture, acidity and alkalinity. In poor aerated soils, an observed
corrosion is in the form of pitting. Localized corrosion of this kind is obviously more
deleterious to a pipeline than a higher overall corrosion rate occurring more uniformly
(Mikhailovskii, et al., 1997).
1.5. Factors influencing corrosion
Corrosion rate and extent depend mainly on the environment and nature of the metal.
1.5.1. Nature of the Environment
The nature of the environment affects the rate of corrosion due to various reasons. Such
factors like pH of the solution, temperature, velocity and concentration of solution play a
vital role.
(a) Concentration of Solution
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Corrosion rate is not linear with concentration even at a wide range. In equipments such
as distillation column, reactors and evaporators, concentration changes continuously,
making prediction of corrosion rate rather difficult.
(b) pH of the solution
Metals such as iron are soluble in acid. Rate of corrosion in the middle pH range is
controlled by the rate of transport of an oxidizer (usually dissolve O2) to metal surface.
Noble metals such as gold, platinum are not affected by pH changes. Oxidizing that
accelerate the corrosion of some materials may also retard corrosion of others through
deformation of their oxides on the surface.
(c) Velocity
An increase in the velocity of relative movement between a corrosive solution and
metallic surface frequently tends to accelerate corrosion. This type of corrosion occurs
frequently in smaller diameter tubes or pipes through which corrosive liquid may be
circulated at high velocities (e.g. heat exchangers and evaporator tubes) (Schreir, 1979).
(d) Temperature
The rate of corrosion increases with an increase in temperature. Suitability of a metal for
high temperature service is dependent upon the properties inherent in the metals
composition and the condition of their application. A large number of metal failures
occur due to the development of excessive thermal stress at high temperatures.
1.5.2. Nature of the metal
The extent of corrosion depends upon the position of the metal in the galvanic series.
When two metals are in electrical contact in the presence of electrolyte the metal higher
up in the galvanic series becomes anodic and suffers corrosion. Greater the difference
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between the two metals in the galvanic series, faster will be the corrosion of the anodic
metal. Further, the reduction in the over voltage also plays an important role in
accelerating corrosion. The relative areas of the anode and cathode also contribute to the
corrosion.
Corrosion rate is also influenced by the orientation of the crystal at the metal surface and
by the size of the grains of the metal / alloys. The presence of impurities in the metal also
influences the rate of corrosion (Roberge, 1984).
The solubility of the corrosion product formed is an important factor in electrochemical
corrosion. If the corrosion product is soluble, corrosion rate will be higher. If the
corrosion leads to the formation of insoluble product, then a protective film may be found
over the metal/alloy which may suppress corrosion (Roberge). The nature of the oxide
film formed influences the rate of corrosion. If the oxide film formed is porous, the
diffusion of oxygen can easily occur and consequently corrosion rate is enhanced. On the
other hand, aluminium and heavy metals form impervious oxide film which protects the
metal from further oxidation. Only fission or a crack in this film can trigger corrosion.
1.5.3. Biological effects.
Macro and microscopic organisms influence corrosion in two principal forms.
(i.) By creating obstructions on the surface of the metal, thereby producing differential
aeration cells, or
(ii). By adsorbing hydrogen from the metal surface and thus eliminating the hydrogen as
a resistance factor in the corrosion cell. Most sulphate reducing bacteria operate in this
form, creating sulphuric acid in the vicinity of the cathodic areas of the metal,
consequently accelerating corrosion (Brasunas, 1984).
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1.6. Corrosion Monitoring
Corrosion measurement involves the application of various techniques to determine the
corrosiveness of the environment and the rate of metal loss. Corrosion measurement is
usually a quantitative method of evaluating the performance and effectiveness of
corrosion control and prevention techniques. After evaluation is completed, the result
obtained is used to improve and enhance the techniques.
The methods for corrosion measurement can be broadly divided into four categories.
They are [Roberge, 1984]
1. Weight loss methods, where the corrosion is directly measured by the loss in weight of
a sample. This is appropriate for all systems but may require a long exposure time if the
corrosion rate is low (Roberge, 1984).
2. Electrochemical corrosion rate methods such as linear polarization, ac impedance and
electrochemical noise. These require a conducting solution and so are not appropriate for
gases or for non-aqueous systems, such as almost dry hydrocarbons (Wiston, 2000).
3. Electrical resistance measurement, where the loss of metal is followed by the increase
in electrical resistance as the metal films. This is appropriate for all systems.
4. Fluid analysis, for example the measurement of the increase in dissolved iron levels as
a fluid passes through a pipeline (Wiston, 2000).
It is important that the monitoring is representative, so location of corrosion probes
should reflect the worst expected corrosion, for example at high flow rates or at areas
where water may separate.
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Similar methods can be used for testing in the laboratory. Here it is important to
reproduce the actual exposure conditions as far as possible.
1.7. Corrosion Prevention
The corrosion process can be retarded by using different methods as the following:
i- Methods based on modification of the environment:
a- By de-aeration or adjusting the pH of the environment.
b- By de-humidification of air.
c- By addition of inhibitors.
ii- Methods based on modification of the metal:
a- By addition of alloying elements.
b- By heat treatment
iii- Methods based on protective coating:
a- Coating by a reaction product (chemical or electrochemical treatment of metal
surface).
b- Organic coating (paints, resins).
c- Inorganic coating (enamels, cement).
d- Metal coating.
e- Temporary protective.
1.7.1.1. Metal Coatings
Coating a substrate metal with a metallic material may be carried out to provide
decorative effect or prevent corrosion. In both cases the corrosion behaviour of the
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substrate/coating system must be considered as a whole. Ideally, a protective coating will
provide a complete barrier and exclude the corrosion environment from the substrate
metal which it is desired to protect; however, no coating is ever perfect. In reality all
coatings contain discontinuities which will lead to contact between the substrate and
corrosion environment. These discontinuities may occur during application or
subsequently due to mechanical damage. Consideration of the corrosion behaviour of the
substrate, the coating and the bimetallic system produced is therefore required.
Metallic coatings can be classified as either anodic or cathodic to the substrate depending
on their position in the electrochemical series and the interaction between the two metals
in the specific environment.
Anodic coatings: Anodic coating is used to describe a coating material, which has a more
negative electrochemical potential than the substrate. In this situation, it is possible for
the coating to sacrificially protect the substrate corroding preferentially at any location
where the two metals are in contact within an electrolyte. Corrosion of the more anodic
metal provides electrons to support the cathodic reaction at the cathodic material hence,
the anodic reaction for the steel, i.e. dissolution, will be reduced or may even be
completely stopped. This type of corrosion protection is referred to as cathodic protection
or sacrificial protection. Zinc coatings on steel (galvanizing) are examples of anodic
coatings. At breaks or pores in the coating, or at cut edges, the coating corrodes
preferentially and provides sacrificial protection (galvanic protection) to the underlying
steel substrate.
Cathodic coatings: They behave in the opposite way to anodic coatings in that the coating
is more electropositive than the substrate. Nickel or copper coatings on steel are examples
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of cathodic coatings. These coatings can provide excellent corrosion protection.
However, an outstanding limitation of such coatings is that they must provide a complete
barrier to the substrate from the environment. If the substrate is exposed to the corrosion
environment through breaks, pores or cut edges, the underlying steel will become the
anode and corrosion will be dramatically accelerated because the anodes is small while
the cathode area is much larger, severe pitting in the substrate may result causing the
coating to flake away from the substrate.
1.7.1.2. Materials Selection and design against corrosion
Most corrosion resistant materials are protected by a passive corrosion product film.
Common corrosion resistant materials are:
• Stainless steel: these are iron-based alloys with the passive film being formed by
chromium. Several classes of a stainless steel are available: ferritic steels are basically
iron-chromium alloys, with about 13% Cr; austenitic steels contain nickel to stabilize the
austenitic structure, a common composition is 18% Cr, 8% Ni; martensitic steels can be
hardened by precipitation of iron carbide in the same way as carbon steels.
• Aluminium and its alloys are protected by a film of alumina, Al2O3, which is very
insoluble and protective. Many of the alloys are, however, susceptible to pitting
associated with copper or iron containing precipitates.
• Nickel base alloys are similar to stainless steels, but tend to be more corrosion resistant
because nickel is a somewhat more noble metal (it is also much more expensive).
• Titanium is protected by a passive film of TiO2. This is one of the most resistant alloys
to localized corrosion, and it is also relatively light but strong. It is relatively expensive.
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Design features can have an important influence on corrosion behaviour. Favorable
designs should encompass the following considerations:
The ideal design will have smooth surfaces, with no crevices or regions where liquid will
accumulate, or from which liquid cannot be drained.
It will not normally use mixtures of different metals (in order to avoid galvanic
corrosion), and
It will avoid highly stressed regions (to prevent stress corrosion cracking).
1.7.1.3. Environment Modification and Inhibitors.
The simplest modification to the environment is the removal of oxygen. In neutral
solution this reduces the rate of corrosion of iron and steel to a very low value. Increasing
the pH to above about 10 will also reduce the corrosion rate of iron and steel, as the iron
will passivate. If these methods are not applicable, then chemicals may be added to the
environment to interfere with the corrosion process, usually by forming a film of some
kind. These chemicals called corrosion inhibitors are substances which, when added in
small quantities to a normally corrosive environment, reduces the corrosion rate of the
metal, without significantly changing the concentration of corrosive species.
Broadly, there are only two ways in which inhibitors can exert their action:
• By forming an adsorbed layer on the metal surface, or,
• By forming a three-dimensional film, either a passive film or a precipitated film.
1.7.2. TYPES OF INHIBITORS.
Numerous classes of inhibitors exist. However, to narrow this down, classification shall be done
by considering certain criteria.
1.7.2.1. Classification based on electrode process
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1.7.2.1.1. Anodic inhibitors.
They form or facilitate the formation of passivating films that inhibits the anodic metal
dissolution reaction. Anodic inhibitors are usually used in near-neutral solutions where sparingly
soluble corrosion products, such as oxides, hydroxides, or salt are formed.
Addition of these inhibitors causes the corrosion potential to shift in a cathodic direction (more
positive potential). Anodic inhibitors are often called passivating inhibitors when they cause large
shifts in the corrosion potential. Passivation may be oxidizing, or nonoxidizing. The oxidizing
anions such as chromate, nitrate, etc do not require the presence of oxygen, while the
nonoxidizing anions like tungstate and phosphate, (Shibli and Saji, 2005) do not require the
presence of oxygen.
When the concentration of an anodic inhibitor is not sufficient, corrosion may be accelerated,
rather than inhibited, hence they are called dangerous inhibitors. The critical concentration above
which inhibitors are effective depends on the nature and concentration of the aggressive ions.
1.7.2.1.2. Cathodic inhibitors.
Cathodic inhibitors either slow the cathodic reaction itself, or they selectively precipitate on
cathodic areas to increase circuit resistance and restrict diffusion of reducible species towards the
cathode (Ref.). Here, cations migrate towards the cathode surfaces where they are precipitated
chemically or electrochemically and thus block these surfaces. Action of As3+ and Sb3+ on
dissolution of Fe in acids is an example.
Some cathodic inhibitors make the discharge of hydrogen gas more difficult, and they are said to
increase the hydrogen overvoltage. Other cathodic inhibitors utilize the increase in alkalinity at
cathodic sites to precipitate insoluble compounds on the metal surface. The cathodic reaction,
hydrogen ion and/or oxygen reduction causes the environment immediately adjacent to the
cathodes to become alkaline; therefore, ions such as calcium or zinc may be precipitated as oxides
to form a protective layer on the metal (Speller, 1951).
1.7.2.1.3. Mixed inhibitors.
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About 80% of inhibitors that cannot be designated specially as anodic or cathodic and are known
as mixed inhibitors. Such type of inhibitors retards both the anodic and cathodic processes. The
shift in the potential is smaller and the direction is determined by the relative size of the anodic
and cathodic sites. Such inhibitors will have the advantage over other inhibitors in that they
control both the cathodic and anodic corrosion reactions and hence are very safe to apply.
1.7.2.1.4. Vapour phase inhibitors.
Temporary protection against atmospheric corrosion, particularly in close environments can be
achieved using vapour-phase inhibitors (VPI). Substances having low significant pressure of
vapour with inhibiting properties are effective. The vapour-phase inhibitors are used by
impregnating wrapping paper or by placing them loosely inside a closed container slow
vaporization of the inhibitor protects against air and moisture. Vapour phase inhibitors (VPI), are
also called volatile corrosion inhibitors (VCI).
The VCIs contain anticorrosive chemicals, which extend their corrosion inhibiting properties to a
metal surface by volatilization within an enclosed space. In spite of the fact that VCIs have been
used for a long time for inhibiting atmospheric corrosion, the action mechanism of these
compounds is not completely clear. It is believed that the major parameters responsible for their
efficiency are vapor pressures and the interactions with the metal surface. In general, when
mechanisms are discussed as to how VCIs function to prevent corrosion, very simplified
explanations are often presented. These explanations contain the assumption that the outer surface
of a metal is composed of a well-behaved metal oxide of fairly uniform thickness (Da-quan
Zhang et al., 2006). The VCI then attaches itself to oxide through weak chemical bonding and
forms an adsorbed monolayer to shield this interface from penetration by corrosive agents such as
water, erosive ions (Cl- or SO42-), etc. The adsorbed monolayer may change the rate of
electrochemical reactions like the dissolution of metal or the reduction of oxygen.
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Desirably, it is necessary for a VPI to provide inhibition rapidly and to have also a lasting effect.
Hence, the compound should have a high volatility to saturate all of the accessible vapour space
as quickly as possible, but at the same time, it should not be too volatile, because it would be lost
rapidly through any leaks in the package or container in which it is used. The optimum vapour
pressure of a VPI should then be just sufficient to maintain an inhibiting concentration on all
exposed metal surface.
1.7.2.1.5. .Inorganic inhibitors (Wiston, 2000),
The common inorganic inhibitors used are crystalline salts, for instance, sodium
chromate and molybdate. The only active groups of these compounds that functions to
reduce corrosion are the negative anions they carry.
1.7.2.1.6. Organic inhibitors
Organic corrosion inhibitor can be anodic, cathodic and mixed type depending on its size, carbon
chain length, aromaticity, conjugation and nature of bonding atoms.
The effectiveness of organic inhibitors is related to the extent to which they adsorb and cover the
metal surface. Adsorption depends on the structure of the inhibitor, surface charge of the metal
and the type of electrolyte. Mixed inhibitors protect the metal in three possible ways viz.,
physical adsorption, chemisoption and film formation. Physical (or electrolyte) adsorption is a
result of electrostatic attraction between the inhibitor and the metal surface. When the metal
surface is positively charged, adsorption of negatively charged (anionic) inhibitors is facilitated.
Positively charged molecules acting in combination with a negatively charged intermediate can
inhibit a positively charged metal. Anions, such as halide ions, in solution adsorb on the
positively charged metal surface, and organic cations subsequently adsorb on the dipole.
Corrosion of iron in sulphuric acid containing chloride ions is inhibited by quaternary ammonium
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cations through this synergistic effect. Physically adsorb inhibitors interact rapidly, but they are
also easily removed from the surface. Increase in temperature generally facilitates desorption of
physically adsorbed inhibitor molecules.
Most effective inhibitors are those that chemically adsorb (chemisorbs), a process that involves
charge sharing or charge transfer between the inhibitor molecules and metal surface.
Chemisorptions take place more slowly than physical adsorption. As temperature increases,
adsorption and inhibition also increase. Chemisorption is specific and is not completely
reversible. Adsorbed inhibitor molecules may undergo surface reactions, producing polymeric
films. Corrosion protection increases markedly as the films grow from nearly two-dimensional
adsorbed layers to three-dimensional films up to several hundred angstroms thick and inhibition
is effective only when the films are adherent, and insoluble, preventing the excess of the solution
to the metal.
1.7.2.1.7 ‘Green’ Corrosion Inhibitors.
Inorganic compounds including chromates, dichromates, phosphates, arsenates, phosphates,
nitrates, nitrites, and sulphides of alkali metals have been in use widely as corrosion inhibitors.
However, due to strict environmental regulations, their continued use has faced relentless
condemnation. Consequently, organic compounds, which function as adsorption inhibitors are
now replacing the inorganic corrosion inhibitors.
In line with this, large numbers of organic compounds, principally those containing
heteroatoms like oxygen, nitrogen or sulphur groups in a conjugated system are now
known to serve as corrosion inhibitors for different metals in various aggressive media.
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1.8. Objective of Study
It is obvious that plant extracts show corrosion inhibition potential in different
aggressive media. Plant materials are the richest source of heterocyclic compounds and
high molecular aromatic contents, and adsorption of these compounds play a key role in
corrosion inhibition of metals (Zucchi and Omar, 1986; Khamis, et al., 2005; Oguzie,
2008b).
Recent development in the area of corrosion control has been on the screening of various
plant extracts for anticorrosive properties. But there does not seem to be any approach for
the detection of active ingredients responsible for the corrosion inhibition effect.
Pertinently, study of the corrosion inhibition of mild steel in acid medium in presence of
green inhibitors is undertaken in this study.
The present work is geared towards the determination of anticorrosion effect of the
following plants which have been chosen based on the literature survey.
a) Moringa oliferia
b) Mimosa pudica
c) Dacryodes edulis
d) Euphorbia hirta.
This study includes,
a) Weight loss measurement at different temperatures and calculation of various
kinetic parameters.
b) Potentiostatic polarization at room temperature and calculation of corrosion
current density and corrosion potential.
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c) Impedance measurements at room temperature and calculation of series
resistance, charge transfer resistance and double layer capacitance.
d) Surface characterization by scanning electron microscope (SEM) to get the
quantitative analysis of the absorbed layers of inhibition.
e) Quantum chemical calculations in order to get useful quantitative and semi-quantitative
information.
CHAPTER TWO: LITERATURE REVIEW.
Usually the corrosion of metals and alloys in acid solution is very severe and this kind of attack
can be inhibited by a large number of organic substances. In general, nitrogen, oxygen and
sulphur containing compounds with a hydrocarbon part attached to the polar group are used as
inhibitors (Oguzie, 2005a). Many nitro and nitroso compounds have been tried as corrosion
inhibitors. Certain azo compounds such as methyl orange and methyl red have been found to be
effective inhibitors (ref). The inhibitive capabilities of some organic dyes namely; Safranine-O,
Thymol blue and Fluorescein-Na on the electrochemical corrosion of mild steel in sulphuric acid
solution using the gasometric technique have been studied, (Oguzie and Ebenso, 2005). The
inhibitory properties of indigo dye during corrosion of mild steel in aerated sulphuric acid
solutions at 30–50 °C have been assessed (Oguzie, et al., 2004). Also, (Oguzie, et al., 2005),
investigated the inhibitory mechanism of methylene blue dye on the corrosion of mild steel in 2
M H2SO4 solutions. (Oguzie, 2005b), again investigated the inhibitory mechanism of methylene
blue dye on the corrosion of mild steel in hydrochloric acid solution using the gravimetric
method. Tang and co-workers (2003) researched on the corrosion inhibiting effect of neutral red
on the corrosion of cold rolled steel in 1.0 M hydrochloric acid (HCl) using weight loss method
and potentiodynamic polarization technique.
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Congo red dye has been assessed for its inhibitive properties on mild steel corrosion in sulphuric
acid solution by Oguzie, (Oguzie, 2004).
The corrosion behaviour of AA2024-T3 pre-treated with bis-[triethoxysilylpropyl]tetrasulphide
have been studied by Cabral and co-workers (Cabral et al., 2005). Imidazolines and amidic
precursors were evaluated as corrosion inhibitors in an aqueous solution of 1.0 M HCl (Olivares-
Xometl et al., 2006). The adsorption behavior of dodecylamine on a copper–nickel alloy in 0.2M
NaCl solutions was studied using electrochemical methods and atomic force microscopy (Qu et
al., 2005). Inhibitive action of a non-ionic surfactant of tween-40 on the corrosion of cold rolled
steel in 0.5–7.0 M sulphuric acid was studied by Xianghong and Guannan, (Xianghong and
Guannan, 2005). Abdallah et al (2006) has studied the effect of some aminopyrimidine
derivatives on the corrosion of 1018 carbon steel in 0.05 M HNO3 solution (Abdallah et al.,
2006). Inhibiting action of 2,2I-Dithiobis(3-cyano-4,6-dimethylpyridine) on the corrosion of mild
steel in 1–5 M H2SO4 solutions at 35–50 0C was investigated by Morad and Kamal, (2006).
Corrosion inhibition of steel in hydrochloric acid by decylamides of α-amino acids derivatives
was studied using gravimetric and electrochemical techniques (Olivares et al., 2006). Benzyl
triphenyl phosphonium bromide has been evaluated as a corrosion inhibitor for mild steel in
aerated 0.5 M sulfuric acid solution (Bhrara and Singh, 2006). Abdallah (2003) studied the
inhibitive effect of some substituted pyrazolones on the corrosion of 304stainless steel in
sulphuric acid. The inhibition effect of halide ions such as iodide, bromide and chloride ions on
the corrosion of iron in 0.5 mol L-1 H2SO4 and the adsorption behaviour of these ions on the
electrode surface have been studied (Venkatachari, et al., 2006). The influence of pH and
concentration of potassium ethyl xanthate (KEtX) on the spontaneous dissolution of copper in
acidic chloride solutions containing oxygen has been studied ( Scendo, 2005). Studies on the
corrosion inhibition of iron in 0.5 M H2SO4 solutions by alkyl quaternary ammonium halides
inhibitors have been carried out (Lin Niu, et al., 2005). Reports on the corrosion inhibition of
mild steel in 0.5 M H2SO4 in the temperature range 30–60 °C using sodium naphthalene
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disulphonic acid (NDSA) as an inhibitor has been documented (Bayoumi and Ghanem, 2005).
The inhibiting efficiency of non-toxic imidazole derivatives on copper corrosion in sulphuric acid
have been investigated (Stupnisˇek-Lisac, et al., 2002). 1, 12-bis (1, 2, 4-triazolyl) dodecane
(dTC12) have been reported to be an excellent corrosion inhibitor for carbon steel in deaerated 1
M HCl solution (Ait Chikh, et al., 2005). The effect of 2,5-bis(4-pyridyl)-1,3,4-thiadiazole (4-
PTH) on the corrosion of mild steel in acidic media (1 M HCl, 0.5 M H 2SO4, 1M HClO4) has
been investigated (Lebrini, et al., 2006). Eight diazoles namely, Benzimidazole, 2-
Methylbenzimidazole, 2-Hydroxymethylbenzimidazole, 2-Aminobenzimidazole, 2-
Mercaptobenzimidazole, 5(6)-Nitrobenzimidazole, 5(6)-Carboxybenzimidazole and 2-
Benzimidazolylacetonitrile, have been investigated as corrosion inhibitors of mild steel in 1 M
hydrochloric acid (Popova, et al., 2004). (Bentiss, et al., 2006) evaluated the inhibitive effect of
the new pyridazine derivative, namely 1,4-bis(2-pyridyl)-5H-pyridazino[4,5-b]indole (PPI)
against mild steel corrosion in 1 M HCl solutions. Adsorption and corrosion inhibitive properties
of three different organic molecules: 2- naphthalenesulfonic acid, 2,7-naphthalenedisulfonic acid
and 2-naphthol-3,6-disulfonic acid were investigated on Armco-iron electrode cathodically
polarized, in 0.5mol dm-3 H2SO4 solution (Vracar and Drazie, 2002). (Frignani, et al., 2005),
investigated the influence exerted by phenylthiourea (PTU) towards the corrosion of Fe79B16Si5
metallic glass in deaerated 0.1 N H2SO4. The effect of propargylic alcohol on the corrosion
inhibition of low alloy steel in sulphuric acid has been studied (Gojic, 2001). Several new
isoxazolidines namely, 1-methylamino-3-pentadecanol, 2-tert-butyl-5-dodecylisoxazolidine, 2-
isopropyl-5-dodecylisoxazolidine, 2-methyl-5-dodecylisoxazolidine, 2-methyl-5-
hexylisoxazolidine, having varying degree of steric environment and hydrophobic chain length,
were tested for corrosion inhibition of mild steel in 1M and 5M HCl at 50–70 °C (Ali, et al.,
2005). (Harek and Larabi, 2004) studied the Corrosion Inhibition of Mild Steel in 1 mol dm–3 HCl
by Oxalic N-Phenylhydrazide N'-Phenylthiosemicarbazide. Also, N-Phenyl oxalic dihydrazide
(PODH) and oxalic N-phenylhydrazide N'-phenylthiosemicarbazide (OPHPT), were tested as
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inhibitors for the corrosion of mild steel in molar HCl (Larabi, et al., 2005). The inhibition
effect of some PEGs on carbon steel corrosion at 25oC in 0.5 N HCl as corroding solution was
evaluated (Ashassi-Sorkhabi, et al., 2006). 2-amino-5-mercapto-1,3,4-thiadiazole and 2-methyl-
5-mercapto-1,3,4-thiadiazole have been reported as copper corrosion inhibitors in neutral chloride
environments (Orlin and Annick, 2004). The performance of poly(diphenylamine) as corrosion
inhibitor for iron in 0.5 M H2SO4 has also been evaluated (Jeyaprabha, et al., 2005). Zinc
corrosion in sulphuric acid containing different m-substituted aniline-N-salicylidenes has been
studied with respect to inhibitor and acid concentration, period of exposure and temperature
(Talati, et al., 2005). Five heterocyclic compounds, having a five atom ring, fused with the
benzene ring (indole, benzimidazole, benzotriazole, benzothiazole and benzothiadiazole) were
investigated as corrosion inhibitors of mild steel in 1 N HCl (Popova and Christov, 2006) using
impedance and polarisation resistance methods. (Emregul, et al., 2006) has studied the effect of
three Schiff base compounds namely, (E)-2-(1-(2-(2-hydroxyethylamino)ethylimino)
ethyl)phenol, 2,2'-(1E,1'E)-1,1'-(2,2'-azanediylbis(ethane-2,1-diyl)bis(azan-1-yl-1-ylidene))
bis(ethan-1-yl-1-ylidene)diphenol and 2,2'-((2E,12E)-3,6,9,12-tetraazatetradeca-2,12-diene-2,13-
diyl)diphenol on the corrosion behavior of steel in 2 M HCl at 298 K by weight loss
measurements, potentiodynamic polarization and electrochemical impedance spectroscopy (EIS)
methods. The effectiveness of the cationic surfactant; 1-dodecyl-4-methoxy pyridinium bromide
as corrosion inhibitor for mild steel in 2M HCl solution has been reported (Migahed, 2005). The
effects of methylthiourea (MTU), phenylthiourea (PTU) and thiobenzamide (TBA) on the
corrosion of mild steel in 0.1 M H2SO4 solution at temperatures of 30 ◦C, 40 ◦C and 50 ◦C have
been studied (Dehri and Ozcan, 2006). The corrosion inhibition of mild steel in 0.5 M
hydrochloric acid solutions by some new hydrazine carbodithioic acid derivatives namely N'-
furan-2-yl-methylene-hydrazine carbodithioic acid , N'-(4-dimethylamino-benzylidene)-hydrazine
carbodithioic acid and N'-(3-nitro-benzylidene)-hydrazine carbodithioic have been studied
(Khaled, 2006) using chemical and electrochemical (potentiodynamic and electrochemical
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impedance spectroscopy, EIS) measurements. (Mounim, et al., 2005) reported on the inhibiting
effects of some oxadiazole derivatives on the corrosion of mild steel in perchloric acid solution.
The inhibitor effect of N,N'-bis(salicylidene)-2-hydroxy-1,3-propanediamine (LOH) and N,N'-
bis(2-hydroxyacetophenylidene)-2-hydroxy- 1,3-propanediamine (LACOH) in 2 mol dm−3 HCl
medium on mild steel has been investigated at 303 K (Emregul, et al., 2005). The anti-corrosive
properties of 2-aminomethylbenzimidazole (AMB) and bis(benzimidazol-2-ylethyl)sulfide
(BBES) has been analyzed using electrochemical techniques like polarization curves and
electrochemical impedance spectroscopy (EIS) (Cruz, et al., 2005). The results showed that AMB
behaved as a cathodic inhibitor, while BBES functioned as mixture inhibitor. The effect of some
mercapto-triazole derivatives on the corrosion and hydrogen permeation of mild steel in 1.0 M
HCl has been investigated (Hui-Long, et al., 2004). (Giacomelli, et al., 2004) studied the inhibitor
effect of succinic acid on the corrosion resistance of mild steel in sulfuric acid solutions using
potentiodynamic polarization, electrochemical impedance spectroscopy, weight loss and optical
microscopic analysis. Three macrocyclic compounds, namely 2,3,9,10-tetramethyl-6,13-dithia-
1,4,5,7,8,11,12,14-octaaza-cyclotetradeca 1,3,6,8,10,13- hexaene (MTAT), 3,4,9,10-tetramethyl-
7,12-dithia-1,2,5,6,8,11-hexaazacyclododecane-2,4,7,8,10,12-hexaene (MTAD), 3,4,9,10-
tetramethyl- 7,12-dioxa-1,2,5,6,8,11-hexaazacyclododecane-2,4,7,8,10,12-hexaene(MOAD)were
synthesized and studied for their corrosion inhibitive effect in 5N HCl by weight loss and
potentiodynamic polarization studies (Quraishi and Rawat, 2002). (Azhar, et al., 2001) studied
the inhibitive effect of [2,5-bis(n-pyridyl)-1,3,4-thiadiazoles]on mild steel in 1 M HCl and 0.5 M
H2SO4. Studies on the influence of [(2-pyridin-4-ylethyl)thio]acetic acid (P1) and pyridine (P2)
on the corrosion inhibition of steel in sulphuric acid solution has been reported (Bouklah, 2005).
The effect of benzimidazole derivatives on mild steel corrosion in 1 M HCl at five different
temperatures has been studied (Popova, et al., 2003). The influence of l-ascorbic acid (AA) on
mild steel corrosion in pH = 2–6 solutions has been investigated using electrochemical and
weight loss techniques (Ferreira, et al., 2004). Electrochemical measurements have been
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performed to investigate the effectiveness of cationic surfactants of the N-alkyl quaternary
ammonium salt type, namely, myristyltrimethylammonium chloride (MTACl),
cetyldimethylbenzylammonium chloride (CDBACl), and trioctylmethylammonium chloride
(TOMACl), as corrosion inhibitors for type X4Cr13 ferritic stainless steel in 2MH2SO4 solution
(Fuchs-Godec, 2006). (Khaled, 2003) studied the inhibitive action of some benzimidazole
derivatives namely 2-aminobenzimidazole (AB), 2-(2-pyridyl)benzimidazole (PB), 2-
aminomethylbenzimidazole (MB), 2-hydroxybenzimidazole (HB) and benzimidazole (B), against
the corrosion of iron (99.9999%) in solutions of hydrochloric acid using potentiodynamic
polarization and electrochemical impedance spectroscopy (EIS). 1,2,4-triazole, 3-amino-1,2,4-
triazole, benzotriazole and 2-mercaptobenzothiazole were evaluated as corrosion inhibitors for
protection of the 2024 aluminium alloy in neutral chloride solutions (Zheludkevich, et al., 2005).
The inhibition effect of three amino acids against steel corrosion in HCl solutions has been
investigated by potentiodynamic polarization method (Ashassi-Sorkhabi, et al., 2004).
Tryptophan has been tested as a copper corrosion inhibitor in 0.5 M aerated sulfuric acid in the
20–50 °C temperature range (Moretti and Guidi, 2002). (Larabi, et al., 2006), investigated the
inhibition of corrosion of copper in hydrochloric acid by 2-mercapto-1-methylimidazole by dc
polarization, ac impedance and weight loss techniques. The co-inhibition characteristic of sodium
tungstate has been evaluated along with potassium iodate on mild steel corrosion (Shibli and Saji,
2005). The inhibitive effect of thiourea (TU) on the corrosion behaviors of bulk nanocrystallized
and coarse grain industrial pure iron (BNIPI & CGIPI) were investigated in 1 mol L -1 HCl at
room temperature by means of electrochemical impedance spectroscopy (EIS) and
potentiodynamic polarization curve (Shen, et al., 2006). Reports on the study of the conditions
and mechanism of copper corrosion inhibition by linear sodium heptanoate (Rocca, et al., 2001),
with a formula of CH3(CH2)5COONa has been documented. The inhibition effect of some amino
acids towards the corrosion of aluminum in 1 M HCl + 1 M H2SO4 solution was investigated
(Ashassi-Sorkhabi, et al., 2005), using weight loss measurement, linear polarization and SEM
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techniques. The corrosion inhibition of Cu–Ni alloys was investigated in aqueous chloride
solutions using amino acids (Badawy, et al., 2006). The effect of cysteine (cys) on the anodic
dissolution of copper in sulfuric acid media has been studied at room temperature using
electrochemical methods (Matos, et al., 2004).
Electrochemical investigation of ascorbic acid adsorption on low-carbon steel in 0.50 M Na2SO4
solutions have been carried out (Goncalves and Mello, 2001). It was observed that the incidence
of monochromatic light may affect the electrochemical behavior of the electrode in this medium
as well as the interaction between the electrode and ascorbic acid. The action of light was
attributed to the complex interaction of several photosensitive phenomena. The effect of some
thiophene derivatives on the electrochemical behavior of AISI 316 austenitic stainless steel in
acidic solutions containing chloride ions has been investigated (Galal,et al., 2005). Evidence of
the formation of the surface layer was confirmed from surface reflectance infrared spectroscopy
measurements. The elemental composition of the surface as indicated from energy dispersive X-
ray analysis and X-ray photoelectron spectroscopy (XPS) proved that the application of the
inhibitor increases the concentration of Cr at the surface of the specimen. The efficiency of 2-
amino-5-mercapto-1,3,4-thiadiazole and 2-methyl-5-mercapto-1,3,4-thiadiazole as copper
corrosion inhibitors in neutral chloride environments has been investigated (Blajiev and Hubin,
2004). The study was carried out by means of a density-functional quantum-chemical approach
and by impedance spectroscopy. Obtained estimates of the total dc path resistance showed that
the studied thiadiazole derivatives were excellent copper corrosion inhibitors. The molecular
behavior of some aniline derivatives as corrosion inhibitors of iron and copper in acidic media
(HCl and H2SO4) were investigated quantum-electrochemically by some recently developed
models based on density functional theory and cluster/ polarized continuum approaches. The
adsorption of aniline molecules on iron seemed to have chemical properties, while that on copper
has a more physical nature. Moreover, in both cases, adsorptions were almost parallel with the
corroding surfaces and took place through an sp3 nitrogen lone pair (Lashgari, et al., 2007).
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Fundamental study of corrosion inhibition behavior of selected organic anions on low-carbon
steel in saturated Ca(OH)2 solution containing chlorides have been carried out. The compounds
studied include eight amino acids, two carboxylic acids, ascorbic acid and a mimosa tannin
extract (Martinez, et al., 2007). All the inhibitors suppressed the reduction of O2, a process that is
known to be strongly catalyzed on passive iron. The highest degree of inhibition was observed for
ascorbic acid. Corrosion Inhibition of Aluminum Alloy 2024-T3 by Aqueous Vanadium Species
has been studied (Ralston, et al., 2008). Potentiodynamic polarization measurements were carried
out on Al alloy 2024-T3 in 50 mM NaCl solutions in which pH and vanadate concentration were
systematically varied. Results showed that inhibition by vanadates occurred mainly in alkaline
solutions where tetrahedrally coordinated vanadates, metavanadate and pyrovanadate, were
abundant. Inhibition was not observed in solutions where octahedrally coordinated decavanadates
predominated. Effects of 1,5-naphthalenediol (ND) on corrosion inhibition of aluminum have
been investigated in 0.50 M NaCl using potentiodynamic polarization, potentiostatic current-time,
air-exposed potential, and electrochemical impedance spectroscopy measurements. The study was
also complemented by the quartz crystal analysis (QCA), cyclic voltammetery, scanning electron
microscopy (SEM), energy dispersive X-ray analysis (EDX), and Fourier transform infrared
(FTIR) spectroscopy. The addition of ND to the electrolyte decreased both general and pitting
corrosion of aluminum in 0.50 M NaCl to a great extent due to its adsorption on the aluminum
electrode surface (Sherif and Park, 2005). The adsorption of ND passivated or blocked the flawed
areas of the aluminum oxide film, and pits formed on the aluminum metal surface from the severe
chloride attack. (Gasparac, et al., 2000a) investigated the efficiency of imidazole derivatives for
corrosion inhibition of copper in 0.5 M hydrochloric acid. Corrosion inhibition was studied using
impedance spectroscopy. Imidazole and its derivatives 4-methylimidazole, 4-methyl-5-
hydroxymethylimidazole, 1-phenyl-4-methylimidazole, 1-(p-tolyl)-4-methylimidazole were
investigated. This study showed that 1-(p-tolyl)-4-methylimidazole is the best inhibitor in this
series and that it acts as mixed inhibitor. Similar studies using potentiodynamic methods have
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shown that 1-(p-tolyl)-4- methylimidazole has the best inhibitory efficiency (Gasparac, et al.,
2000b). The corrosion inhibition of copper in aerated 0.5 M H2SO4 solution in presence of two
classes of heterocyclic compounds, namely phenylazo-pyrazolones (PAP) or hydroxyl quinoline
and bromobenzyl-carboxy-1,2,3 triazole (BCT) derivatives has been studied. The inhibition effect
was attributed to the adsorption of the dye molecules, the precipitation of Cu chelates and/or
formation of p-complexes at the electrode surface (Elmorsi and Hassanein, 1999). The properties
of organic coatings containing Polyaniline (PANI) and PANI in combination with other anti-
corrosive pigments have been studied (Kalendova, et al., 2008). The adhesion, barrier, and
anticorrosion properties of the coatings containing PANI and selected chemically active pigments
were studied as well as the combination of PANI with zinc dust. The comparison of the results of
corrosion tests completed in the atmosphere of SO2 and of NaCl revealed that the PANI +
Zn3(PO4)2·2H2O combination increased the anti-corrosion efficiency of organic-coatings.
3-mercaptopropyltrimethoxysilane (MPS) has been used as a copper corrosion inhibitor in 0.100
mol L-1 KCl solution. The inhibition was studied as a function of the MPS pretreatment
concentration in ethanol. From the polarization resistance, the inhibition efficiency improved with
increase in MPS concentration during the pretreatment. Polarization studies suggested that MPS
is an anodic as well as a cathodic inhibitor, in the presence of dissolved oxygen (Tremont, et al.,
2000). Abdel Rehim and co-workers studied the influence of the concentration of adenine (AD),
as a safe inhibitor, on the corrosion of low carbon steel (LCS) in aerated 4.0 M H 2SO4 solutions
(Abdel Rehim, et al., 2008). The investigations involved weight loss, potentiodynamic
polarization, impedance and electrochemical frequency modulation (EFM) methods. Results
obtained revealed that together with iodide ion, AD is an effective corrosion inhibitor for LCS
corrosion in H2SO4 solutions. Potentiodynamic polarization studies showed that AD alone and the
mixture of AD and iodide ions acted as mixed-type inhibitors for the corrosion of LCS in 4.0 M
H2SO4 solution. Variation of carbon steel corrosion rate with flow conditions in the presence of
an inhibitive formulation (Fatty amines associated with phosphonocarboxylic acid salts) used for
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the treatment of water in cooling circuits was assessed (Srisuwan, et al., 2008). Two distinct
surface areas were visualized on the metal surface and the ratio between the two zones was
dependent on the flow conditions. A non-monotonic variation of the corrosion current densities
was also observed and explained by the variation of the ratio between the two layers, which each
have different intrinsic protective properties. The inhibitive effect of four oleo chemicals
(namely; 2-Pentadecyl-1,3-imidazoline (PDI), 2-Undecyl-1,3-imidazoline (UDI), 2-Heptadecyl-
1,3-imidazoline (HDI), 2-Nonyl-1,3-imidazoline (NI)), regarded as green inhibitors, has been
studied for the corrosion protection of mild steel in 0.5 M H2SO4. The methods employed were
weight loss, potentiodynamic polarization and electrochemical impedance techniques. The
inhibition efficiency increased with increase in inhibitor concentration, immersion time and
decreased with increase in solution temperature (Rafiquee, et al, 2009). The corrosive behaviour
of mild steel in 1M HCl solutions containing selected imidazolines of fatty acids with C7-C17 was
investigated using weight-loss method, potentiodynamic polarization technique and scanning
electron microscopy (Quaraishi, et al., 2008). The results obtained revealed that all the studied
imidazolines are effective in reducing corrosion of mild steel in HCl media. Potentiodynamic
polarization data showed that the compounds studied are mixed type inhibitors in the acid
solution. (Eddy, et al., 2009) has studied the inhibition efficiency of some antibiotics against mild
steel corrosion using weight loss and quantum chemical techniques. 3,5-Diamino-1,2,4-triazole
Schiff base derivatives and their inhibition efficiency, based on the effect of changing functional
groups, has been reported to establish a relationship between inhibitor efficiency and molecular
structure using weight loss method, electrochemical and Fourier transform infrared spectral
techniques. It was also found that the molecules containing more electron donating groups have
higher inhibition efficiency than the corresponding compounds with low electron donating groups
(Gopi, et al., 2010). The inhibiting action of 4-amino-antipyrine (AAP) and its schiff bases 4-
[(benzylidene)-amino]-antipyrine (BAAP), 4-[(4-hydroxy benzylidene)-amino]-antipyrine
(SAAP) and 4-[(4-methoxy benzylidene)-amino]-antipyrine (AAAP) which are derived from 4-
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amino-antipyrine with benzaldehyde, salicylaldehyde and anisaldehyde, toward the corrosion
behaviour of mild steel in 1 M HCl solution has also been studied (Govindaraju, et al., 2009)
using weight loss, potentiodynamic polarization, electrochemical impedance and FT-IR
spectroscopic techniques. Although AAP was found to retard the corrosion rate of mild steel, the
synthesized schiff base compounds were also seen to retard the corrosion rate very effectively.
Ssanbhag and co-workers has investigated the corrosion inhibition characteristics of N′-[(1E)-(4-
hydroxy phenyl) methylene] isonicotinohydrazide (HIH) and N′-[(1E)-(4-hydroxyl-3-methoxy
phenyl) methylene] isonicotinohydrazide (HMIH) on mild steel corrosion in 1 M hydrochloric
acid by weight loss, potentiodynamic polarization and impedance techniques. The inhibition
efficiency was found to increase with increase in inhibitor concentration but decreased with
increase in temperature (Shanbhag, et al., 2007). Tramadol[2-[(dimethylamino)methyl]-1-(3-
methoxyphenyl)cyclohexanol hydrate], a drug, has been tested as a corrosion inhibitor for mild
steel in 0.5 M HCl and 0.25 M H2SO4 separately at 300, 310 and 320 K using mass loss and
galvanostatic polarization techniques (Prabha, et al., 2006). The protection efficiency increased
with increase in inhibitor concentration and decreased with increase in temperature in both the
acid solutions. Galvanostatic polarization studies showed that the inhibitor is of mixed type with a
slight predominance of cathodic character. (Granero, et al., 2009) carried out a study of the
behaviour of a mixture of amines and amides, commercially known as Dodigen 213-N (D-
213 N), as a corrosion inhibitor for ASTM 1010 mild steel in 10% w/w HCl solution. The weight
loss and electrochemical techniques used were corrosion potential measurement, anodic and
cathodic polarization curves, and electrochemical impedance spectroscopy (EIS). The corrosion
potential values shifted to slightly more positive values, thus indicating mixed inhibitor
behaviour. The anodic and cathodic polarization curves showed D-213 N as an effective
corrosion inhibitor, since both the anodic and the cathodic reactions were polarized in comparison
with those obtained without inhibitor. The effect of betanin (2,6-pyridinedicarboxylic acid, 4-(2-
(2-carboxy-5-(beta-D-glucopyr-anosyloxy)-2,3-dihydro-6-hydroxy-1H-indol-1-yl)ethenyl)-2,3-
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dihydro-(S-(R*,R*))) on the corrosion inhibition of mild steel has been investigated in 1 M HCl
solution (Ashassi-Sorkhabi and Es’haghi, 2008). Weight loss method, potentiodynamic
polarization, and electrochemical impedance spectroscopy techniques were applied to study the
mild steel corrosion behaviour in the absence and presence of different concentrations of betanin
under the influence of various experimental conditions. Polarization curves showed that betanin
behaves mainly as a mixed-type inhibitor. The inhibiting behaviour of Nile blue and Indigo
Carmine organic dyes on mild steel corrosion has been evaluated in 1 M HCl solution, separately,
by weight loss, potentiodynamic polarization, and electrochemical impedance spectroscopy
techniques. Polarization curves indicate that the inhibition of the both inhibitors is of a mixed
anodic–cathodic nature, and Langmuir isotherm was found to be an accurate isotherm describing
the adsorption behaviour (Abdeli and Ahmadi, 2009). (Eddy, et al., 2009) investigated the
corrosion inhibition of ampicillin (AMP) and its synergistic combination with halides (KI, KCl
and KBr) for the corrosion of mild steel in H2SO4 using gravimetric, gasometric, thermometric
and infrared (IR) methods. The adsorption of AMP on the mild steel surface was found to obey
the Langmuir adsorption isotherm model and combination of AMP with the halides (KI, KBr and
KCl) enhanced the inhibition efficiency and adsorption behaviour of the inhibitor indicating
synergism. The corrosion inhibition properties of these compounds; 2-Pentadecyl-1,3-imidazoline
(PDI), 2-Undecyl-1,3-imidazoline (UDI), 2-Heptadecyl-1,3-imidazoline (HDI), 2-Nonyl-1,3-
imidazoline (NI) on aluminium in 1 M HCl and 0.5 M H2SO4 were investigated (Quraishi, et al.,
2007) by weight loss, potentiodynamic polarization, electrochemical impedance and scanning
electron microscopic techniques. Weight loss studies showed that the inhibition efficiency
increased with increase in the concentration of the inhibitor and was found to be inversely related
to time and temperature while it showed no significant change with increase in acid
concentration. The adsorption of these compounds on aluminium surface followed the Langmuir
adsorption isotherm and potentiodynamic polarization data showed that the compounds studied
were mixed type inhibitors. The inhibition performance of Basic yellow 13 dye on mild-steel
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corrosion in hydrochloric acid solution was studied at 25 °C using weight loss and
electrochemical techniques (Ashassi-Sorkabi, et al., 2009). Inhibition efficiency increased with
increase of basic yellow 13 concentrations. ΔGads was calculated and its negative value indicated
spontaneous adsorption of the Basic yellow 13 molecules on the mild-steel surface and strong
interaction between inhibitor molecules and metal surface. The corrosion inhibition of mild steel
in 0.5 M sulfuric acid by two newly synthesized Schiff bases namely, 4-X-2-{[2-(2-pyridin-2-yl-
ethylsulfanyl) ethylimino] methyl}-phenol [X = –NO2 (S 1) and –OMe (S 2)] has been investigated
in the temperature range 298–318 K using Tafel polarization and electrochemical impedance
spectroscopy (EIS) methods ( Hosseini, et al., 2009). The Temkin isotherm was found to provide
an accurate description of the adsorption behavior of the Schiff bases.
Two triazole derivatives, 3,4-dichloro-acetophenone-O-1′-(1′,3′,4′-triazolyl)-methaneoxime (4-
DTM) and 2,5-dichloro-acetophenone-O-1′-(1′,3′,4′-triazolyl)-methaneoxime (5-DTM) have been
tested for inhibition effects for mild steel corrosion in 1 M HCl solutions by weight loss
measurements, electrochemical tests and scanning electronic microscopy (SEM). The
potentiodynamic polarization experiment revealed that the triazole derivatives are inhibitors of
mixed-type and electrochemical impedance spectroscopy (EIS) confirmed that changes in the
impedance parameters (R ct and C dl) are due to surface adsorption (Li, et al., 2007).
(Singh and Quraishi, 2010) studied the inhibition effect of all the three Mannich bases against the
corrosion of mild steel in 1 M HCl solution by weight loss, electrochemical impedance
spectroscopy (EIS), potentiodynamic polarization, and atomic force microscopy techniques. The
adsorption of Mannich bases obeyed Langmuir adsorption isotherm. Polarization curves indicated
a mixed nature of inhibition. All the Mannich bases were observed to be adsorbed physically at
lower concentration, whereas chemisorption was favoured at higher concentration.
The corrosion inhibition of C38 steel in molar HCl by N,N-bis[2-(3,5-dimethyl-1H-pyrazol-1-
yl)ethyl]buthylamine and 5-{N,N-bis[2-(3,5-dimethyl-1H-pyrazol-1-yl)ethyl] amino} pentanol
has been investigated at 308 K using electrochemical and weight loss measurements (Zerga, et
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al., 2010). Measurements showed that these compounds acted as good inhibitors without
changing the mechanism of the corrosion process. Moreover, the inhibiting efficiency increased
with the increase in concentration of the studied inhibitors.
(Gopi, et al., 2007) studied the corrosion inhibition of mild steel by means of newly synthesized
triazole phosphonates 3-Vanilidene amino 1,2,4-triazole phosphonate (VATP), 3-Anisalidene
amino 1,2,4-triazole phosphonate (AATP) and 3-paranitro benzylidene amino 1,2,4-triazole
phosphonate (PBATP) along with cetyl trimethyl ammonium bromide (CTAB) in natural aqueous
environment using weight loss measurement, potentiodynamic polarisation and ac impedance
measurement. Addition of molybdate was noticed to increase the inhibition efficiency of triazole
in a synergistic manner. Results from experimental observation indicated VATP as a better
corrosion inhibitor for mild steel in aqueous solution. Additionally the formulation consisting of
VATP, sodium molybdate and CTAB offered good corrosion inhibition efficiency.
The effect of seven amphiphilic compounds, on steel API 5L X52 corrosion in sulphuric acid 1 M
solution was studied by (Pérez-Navarrete, et al., 2010) using potentiodynamic polarization
curves, and electrochemical impedance spectroscopy (EIS). Potentiodynamic polarization curves
indicated that these compounds acted mainly as cathodic type inhibitors.
Even with the broad spectrum of organic compounds available for use, the final choice of an
appropriate inhibitor for a particular application is restricted by several factors, ranging from
increased environmental awareness and the need to promote environmentally friendly processes,
to the vast variety of possible corrosion systems available.
Accordingly, the need exists for the development of new class of corrosion inhibitions that are of
low toxicity and good efficiency.
2.2. Natural products as corrosion inhibitors.
The investigation of natural products which are of plant origin as inexpensive and eco-friendly
corrosion inhibitors has gained interest recently. Plant extracts have become important as an
environmentally acceptable, readily available and renewable source for wide range of inhibitors.
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They are the rich sources of ingredients which have very high inhibition efficiency. In addition to
being environmentally friendly and ecologically acceptable, plant products are of low-cost and
renewable sources of materials (Sharma, et al., 2008, Khamis, et al., 2005, Quraishi, 2004,
Zucchi and Omar, 1985). Extracts from their leaves, barks, seeds, fruits and roots comprise of
organic compounds containing nitrogen, sulphur and oxygen atoms and some have been reported
to function as effective inhibitors of metal corrosion in different aggressive environments.
The inhibition effect of Zenthoxylum alatum plant extract on the corrosion of mild steel in 5%
and 15% aqueous hydrochloric acid solution has been investigated (Chauhan and Gunasekaran,
2007) by weight loss and electrochemical impedance spectroscopy (EIS). Plant extract was able
to reduce the corrosion of steel more effectively in 5% HCl than in 15% HCl. The adsorption of
this plant extract on the mild steel surface was observed to obey the Langmuir adsorption
isotherm.
The inhibitive effect of the extract of khillah (Ammi visnaga) seeds, on the corrosion of SX 316
steel in HCl solution was determined (El-Etre, 2006) using weight loss measurements as well as
potentiostatic technique. It was found that the presence of the extract reduces markedly the
corrosion rate of steel in the acid solution. Also noticed was the increase in inhibition efficiency
as the extract concentration was increased.
(Oguzie, 2005a) investigated the efficacy of Telfaria occidentalis extract as a corrosion inhibitor
for mild steel in 2M HCl and 1M H2SO4 solutions. Telfaria occidentalis extract was found to
inhibit mild steel corrosion in 2M HCl and 1M H2SO4 solutions. Inhibition efficiency increased
with extract concentration but decreased with rise in temperature.
The inhibition effect of Zenthoxylum alatum plant extract on the corrosion of mild steel in 20, 50
and 88% aqueous orthophosphoric acid was investigated (Gunasekaran and Chauhan, 2004) by
weight loss and electrochemical impedance spectroscopy (EIS). Observation showed that plant
extract was able to reduce the corrosion of steel more effectively in 88% phosphoric acid than in
20% phosphoric acid.
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The aqueous extract of the leaves of henna (lawsonia) was tested as corrosion inhibitor of C steel,
nickel and zinc in acidic, neutral and alkaline solutions, using the polarization technique (El-Etre,
et al., 2005). It was found that the extract acts as a good corrosion inhibitor via mixed inhibition
mechanism for the three tested electrodes in all tested media.
Comparison of steel anticorrosive protection formulated with natural tannins extracted from
acacia and from pine bark have been carried out (Matamalaa, et al., 2000). The results indicated
that pine tannins present better reactivity than acacia tannins, with better corrosion inhibition and
better adherence to metallic substrates.
Inhibition of aluminium corrosion in 2M sodium hydroxide solution in the presence and absence
of 0.5M NaCl using damsissa (Ambrosia maritime, L.) extract has been studied (Abdel-Gaber, et
al., 2008) employing different chemical and electrochemical techniques. Chemical gasometric
technique showed that addition of chloride ions or damsissa extract to sodium hydroxide solution
decreased the volume of the hydrogen gas evolved while potentiodynamic results manifested that
chloride ion retard the anodic dissolution of aluminium, below the pitting potential, in sodium
hydroxide solution. Damsissa extract, in presence or absence of chloride ion, influenced both the
anodic dissolution of aluminium and the generated hydrogen gas at the cathode indicating that the
extract behaved as mixed-type inhibitor.
Ocimum basilicum extract has been established to inhibit aluminium corrosion in the acidic and
alkaline environments (Oguzie, et al., 2006a). Inhibition efficiency was found to increase with
extract concentration but decreased with rise in temperature, suggesting physical adsorption of
the organic matter on the metal surface.
(Oguzie, 2006a) also studied the corrosion inhibition of mild steel in 2M HCl and 1M H2SO4 by
leaf extracts of Occimum viridis via the gasometric technique.
The inhibitive behaviour on steel of flavanoid monomers that constitute mangrove tannins
namely catechin, epicatechin, epigallocatechin and epicatechingallate has been investigated
(Rahim, et al., 2006) in an aerated HCl solution via electrochemical methods. The monomers
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were found to be mainly cathodic inhibitors and the inhibition efficiency was dependent on
concentration.
Wild strain of Bacillus mycoides has been investigated for possible corrosion inhibition potential
(Eimutis, et al., 2006). Aluminium, zinc and mild steel were subjected to influence of wild strain
Bacillus mycoides for 2 years under laboratory conditions at controlled temperature and humidity.
Results obtained from the electrochemical impedance measurements performed for both biotic
and abiotic samples indicated microbially influenced corrosion inhibition for aluminium,
corrosion acceleration for zinc and indifference for steel.
The inhibitive action of the acid extracts of seeds, leaves and bark from the Ficus virens plant
towards hydrochloric and sulfuric acid corrosion of aluminium has been tested using mass loss
and thermometric techniques. It was found that the extract acts as a good corrosion inhibitor for
aluminium corrosion in all concentration of hydrochloric and sulfuric acid solution. It was also
found that the Ficus virens extract provides a good protection against pitting corrosion in chloride
ion containing solution (Jain, et al., 2006).
(Oguzie, et al., 2007) studied the effectiveness of Gongronema latifolium extract as an
environmentally friendly corrosion inhibitor for aluminium in strong acid (2M HCl) and alkaline
(2M KOH) environments. The results showed that the extract was well adsorbed on the metal
surface and significantly repressed aluminium corrosion in both environments.
The effectiveness of guar gum as an inhibitor for carbon steel corrosion in sulphuric acid
environments has been studied (Abdallah, 2004). Rosmarinus officinalis L. has been reported to
inhibit the corrosion of Al-Mg in chloride solution (Kliskic, et al., 2000).
The effect of extracts of Chamomile (Chamaemelum mixtum L.), Halfabar (Cymbopogon
proximus), Black cumin (Nigella sativa L.), and Kidney bean (Phaseolus vulgaris L.) plants on
the corrosion of steel in aqueous 1M sulphuric acid has been investigated using electrochemical
impedance spectroscopy (EIS) and potentiodynamic polarization techniques. Potentiodynamic
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polarization curves indicated that the plant extracts behave as mixed-type inhibitors (Abdel-
Gaber, et al., 2006).
The protective effect and adsorption behaviour of Azadirachta indica extract in controlling mild
steel corrosion in 1M H2SO4 and 2M HCl has been assessed (Oguzie, 2006b). Azadirachta indica
extract effectively inhibited steel corrosion in the acid media studied by virtue of adsorption. The
inhibitor adsorption characteristics were approximated by Langmuir isotherm. (Sharma, et al.,
2009) also investigated the effect of this same plant on the corrosion of zinc in sulphuric acid
solutions.
Seed extract of Garcinia kola (Oguzie, et al., 2006b) was investigated as a corrosion inhibitor for
mild steel in 2M HCl and 1M H2SO4 solutions using the gasometric technique. Results indicated
that the extract inhibited the metal corrosion in the acidic environments and inhibition efficiency
increased with concentration. Temperature studies revealed a decrease in efficiency with rise in
temperature while corrosion activation energies increased in the presence of the extract. (Okafor,
et al., 2007) also investigated ethanol extract of Gracinia kola for inhibition of mild steel
corrosion in H2SO4 solutions.
Effect of berberine abstracted from Coptis chinensis and its inhibition efficiency on corrosion of
mild steel in 1 M H2SO4 was investigated (Li, et al., 2005).The weight loss results showed that
berberine is an excellent corrosion inhibitor for mild steel immersed in1 M
H2SO4.Potentiodynamic curves suggested that berberine suppressed both cathodic and anodic
processes.
Two different aerobic bacteria, viz. Pseudomonas alcaligenes and Pseudomonas cichorii have
been reported (Chongdar, et al., 2005) to influence the corrosion of mild steel electrodes
incubated in phosphate-buffered basal salt solution (BSS). In the medium containing P. cichorii,
significant reduction in the corrosion rate was observed due to the surface reaction leading to the
formation of corrosion inhibiting bacterial biofilm.
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The inhibitive action of leaf extracts of Sansevieria trifasciata on aluminium corrosion in 2 M
HCl and 2 M KOH solutions has also been studied (Oguzie, 2007) using the gasometric
technique. The results indicate that the extract functioned as a good inhibitor in both
environments via a mechanism of physical adsorption. The adsorption characteristics of the
inhibitor were approximated by Freundlich isotherm.
Four siderophores isolated from bacteria have been studied as possible corrosion inhibitors for
iron in deaerated 1 N HCl. The compounds were aerobactin, enterobactin, parabactin, and
rhodotorulic acid. Polarization measurements showed all four compounds as good inhibitors
(McCafferty and McArdle, 1995).
(Okakor, et al., 2008) studied the inhibitive action of leaves (LV), seeds (SD) and a combination
of leaves and seeds (LVSD) extracts of Phyllanthus amarus on mild steel corrosion in HCl and
H2SO4 solutions using weight loss and gasometric techniques. The results indicate that the
extracts functioned as a good inhibitor in both environments and temperature studies revealed an
increase in inhibition efficiency with rise in temperature while activation energies decreased in
the presence of the extract. A mechanism of chemical adsorption of the plants components on the
surface of the metal was proposed for the inhibition behaviour.
The inhibiting action of the calyx extract of Hibiscus sabdariffa on mild steel corrosion in 2 M
HCl and 1 M H2SO4 solutions has been assessed using the gasometric technique. The results
demonstrated that Hibiscus sabdariffa extract suppressed the corrosion reaction in both acid
media. The inhibition mechanisms, estimated from the temperature dependence of inhibition
efficiency as well from kinetic and activation parameters showed that the extract functioned via
mixed inhibition mechanism (Oguzie, 2008).
The influence of natural honey (chestnut and acacia) and natural honey with black radish juice, on
corrosion of tin in aqueous and sodium chloride solutions was studied (Radojcic, et al., 2008)
using weight loss and polarization techniques. Results showed that the inhibition efficiency of
acacia honey was lower than that of chestnut honey, while the addition of black radish juice
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increased the inhibition efficiency of both honey varieties. The process of inhibition was
attributed to the formation of multilayer adsorbed film on the tin surface. The adsorption of
natural honey and honey with black radish on tin was found to follow the Langmuir adsorption
isotherm.
(Oguzie, 2008b) investigated the Corrosion inhibition of selected plants on mild steel corrosion in
2 M HCl and 1 M H2SO4 using a gasometric technique. The studied plants materials include leaf
extracts Occimum viridis, Telferia occidentalis, Azadirachta indica and Hibiscus sabdariffa as
well as extracts from the seeds of Garcinia kola. The results indicated that all the extracts
inhibited the corrosion process in both acid media by virtue of adsorption and inhibition
efficiency improved with concentration of the extracts studied.
The corrosion inhibitive effect of the extract of black pepper on mild steel in 1 M H 2SO4 media
was evaluated by conventional weight loss studies, electrochemical studies viz., Tafel
polarization, ac impedance and scanning electron microscope (SEM) studies (Raja and
Sethuraman, 2008). Results from weight loss study revealed that black pepper extract acts as a
good inhibitor even at high temperatures. The inhibition is through adsorption which is found to
follow Temkin adsorption isotherm. Tafel polarization revealed the mixed mode inhibition of
black pepper extract.
Inhibition of the corrosion of mild steel by ethanol extract of Musa species peel has been studied
(Eddy, et al., 2009) using hydrogen evolution and thermometric methods of monitoring
corrosion. The result of the study revealed that different concentration of ethanol extract of Musa
species peel inhibit mild steel corrosion. Inhibition efficiency of the extract was found to vary
with concentration, temperature, period of immersion, pH and electrode potentials.
A study of rosemary oil as a green corrosion inhibitor for steel in 2 M H3PO4 has been carried out
(Bendahou, et al., 2006).The oil was found to be a good inhibitor for steel corrosion, but, its
efficiency decreased with temperature. Polarisation measurements showed that rosemary oil acted
essentially as a cathodic inhibitor.
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The inhibitive effect of Jasminum nudiflorum Lindl leaves extract on the corrosion of cold rolled
steel (CRS) in 1.0 M hydrochloric acid (HCl) was investigated (Li, et al., 2010) by weight loss,
potentiodynamic polarization, and electrochemical impedance spectroscopy (EIS) methods. The
results showed the extract as a very good inhibitor, and the inhibition efficiency increases with
concentration. The adsorption of the extract obeyed Langmuir adsorption isotherm.
The corrosion behaviour of mild steel and aluminium exposed to H2SO4 solution and their
inhibition in H2SO4 containing Gum Arabic (GA) used as inhibitor has been assessed using
weight loss and thermometric techniques. Corrosion rate increased both in the absence and
presence of inhibitor with increase in temperature. Corrosion rate was also recorded to decrease
in the presence of inhibitor compared to the free acid solution. He proposed the phenomenon of
chemical adsorption for mild steel corrosion, while physical adsorption mechanism was proposed
for aluminium corrosion (Umoren, 2008).
2.3. Ethnobotanical details of the plants.
The botanical details of the plant and the major constituents present in the plants which were
screened for corrosion inhibition studies are discussed as follows.
2.3.1. Moringa oleifera.
Moringa oleifera Lam. belonging to the single genus family Moringaceae is a small fast-growing
ornamental tree originally belonging to India. Root, bark, pods and leaves of this tree are used in
traditional medicine for the treatment of human diseases, the leaves are enriched in vitamins A
and C. Pods and young leaves of the plant are primarily used for vegetative purpose (Mughal, et
al., 1999). M. oleifera seed oil is also high in tocopherols (Tsaknis, et al., 1999). The seeds of this
plant are also employed for water purification (Okuda, et al., 2001). Anti-cancer (Guevara et al.,
1999), anti-inflammatory and hepatoprotective (Kurma and Mishra, 1998a, 1998b) activities in
various tissues have also been reported. Detailed information on the nutritional value and
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chemical composition of M. oleifera seed oil is available (Ching and Mohamed, 2001; Lalas and
Tsakins, 2002; Ryynanen, et al., 2004). Number of phytochemicals from various parts of
Moringa oleifera have also been isolated (Bennett et al., 2003; Faizi et al., 1994a, 1994b; Francis,
et al., 2004; Lakshminarayana, et al, 2005) except the saponins which are commonly found in
trees (Wina, et al, 2005). An immunoenhancing polysaccharide (Mondal, et al, 2004) and
niaziminin, having structural requirement to inhibit tumorpromoter induced Epstein Barr virus
activation have been reported from the leaves (Murakami, et al., 1998).
2.3.2. Mimosa pudica.
Mimosa pudica Linn belonging to the family Mimisoideae is commonly known as sensitive plant.
The plant has very sensitive leaves which fold on touching and has reddish roots. The plant is
widely distributed through tropical and subtropical parts of India, common in waste place where
the climate is moist and warm. The useful parts of this plant are roots, leaves and flower heads.
The whole plant is used medicinally in ayurvedic folk medicine and its photochemical studies
revealed the presence of minosine, orientin, isoorientin, β- sterol, D-pinitol, norepinepherine,
crocetin, tannins and turgorins. Mimosa pudica is an important plant which is used for various
ailments in ayurvedic system of medicine (Nadkarani, 1982, 2001; Chopra, et al., 1996; Rastogi,
et al., 2005).
In previous studies, it was found that the decoction of Mimosa pudica leaves has anticonvulsant
properties (NgoBum, et al., 2002). Both the ethanolic and aqueous extracts of the leaves of
Mimosa pudica possess hyperglycemic and antidepressant activities in mice and rats respectively
(Amalraj and Ignacimuthu, 2002; Molina, et al., 1999).
2.3.3. Dacryodes edulis.
Dacryodes edulis is a dioecious shade loving species of non-flooded forests in the humid tropical
zone (Adebayo-Tayo and Ajibesin, 2008; Hutchison and Daiziel, 1958). Dacryodes edulis is a
versatile plant in African ethnomedicine, as its various parts are employed to treat several
diseases. The bark of the plant has long been used to cicatrize wound in Gabon. It is also used as
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gargle and mouth-wash to treat tonsillitis. The leaf decoction is prepared to produce vapour that
treats fever and headache, while the stems are employed as chewing sticks for oral hygiene
(Ajibesin, et al., 2008). Β-caryophyllene has been reported to occur as the main constituent of the
leaf essential oil of D. edulis (Onocha, et al., 1999). Ajibesin (2005) had identified phenolics such
as ethylgallate and quercitrin in the plant leaves.
In a study conducted in Cameroon, the extracts of 42 medicinal plants used for anaemia, diabetes,
AIDS, malaria and obesity were investigated for phytochemical substances and antioxidant
properties. The leaves of Dacryodes edulis elicited very high antioxidant effect when analyzed
against three assay methods: Folin (Folin Ciocalteu Reagent), FRAP (Ferric Reducing
Antioxidant Power) and DPPH (1, 1-diphenyl-2-picryhydrazyl), ranking second behind
Alchornea cordifolia (Agbor, et al., 2007). This antioxidant property was attributed to the
presence of flavonoids in the plant extract.
2.3.4. Euphorbia hirta.
Euphorbia hirta is well known and used by the major tribes in Nigeria. In Nigeria, the name in
Yoruba is Emi-ile. The plant E. hirta is commonly called asthma plant because of its alleged
efficacy in East and West Africa in the treatment of asthma and various respiratory ailments
(Odugbemi, 2008; Brown, 1995; Oliver, 1959). The plant is used as a diuretic, febrifuge,
galactogogue, purgative and vermifuge. It is reported as medication for intestinal amoebic
dysentery (Ogbulie et al., 2007; Stuart, 1979). Traditionally, the plant is squeezed in water and
the extract taken orally as a remedy for asthma. The phytochemicals in E. hirta include volatile
oil, alkaloids, tannins, saponins and steroids (Hashemi et al., 2008). The analgesic, antipyretic
and anti-inflammatory properties of the plant have been reported (Lanhers et al., 1991). The
ethanolic extracts of the plant have been found to demonstrate antibacterial activity and
toxicological potential (Ogbulie et al., 2007). In vitro antifungal and antibacterial properties as
well as ulcer-protective effect and hepatoprotective activity of the plant extract in rats have also
been demonstrated (Somchit et al., 2001; Rao et al., 2003; Edwin et al., 2007). Bioassay-guided
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fractionation of the methanol extracts of Euphorbia hirta Linn (Euphorbiaceae) aerial parts led to
the isolation of flavonol glycosides; afzelin, quercitrin, and myricitrin (Liu, et al., 2007).
2.3.5 PIPER GUINENSIS (AFRICAN BUSH PEPPER)
Piper guinensis (African bush pepper) or commonly called uziza in Igbo are climbing glabrous
creeper cultivated in various part of India, Malaya Island, Nigerian and other West African
countries. There is considerable local use of this species as a condiment and it is widely found in
almost all Nigerian market. The roots, fruits and leaves of this plant are widely used in the
treatment of asthma, bronchitis, fever and pain in the abdomen, as stimulant and in haemorrhoidal
infection. The fresh fruits of piper guinensis are often eaten raw for their spicy taste. The fruits
are also dried and then pounded and sieved; this powder is added to tea or coffee or used for
seasoning vegetables (Ebenso et al 2008). Piper guinensis is a plant among the candidate with
enormous potential for use as a bio insecticide, it is a member of the piperraceae family. It is
used in small quantities for flavour in foods and medicinal purposes, the excess post harvest is
usually wasted, since new stock come to meet the previous season stock.
2.3.6 MISTLETOE (Viscum album)
Natural tannins are complex mixtures extracted from plant materials that are either being
investigated or are in use as corrosion inhibitors in aqueous solutions (Oguzie et al,
2004).Tannins acts as corrosion inhibitors on bare steel in acid or neutral solution due to their
ability to form chelate compounds with ferrous and ferric ions that are released in the course of
steel corrosion process(Roberge,1994).
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Viscum album growing on a populous species has the following scientific classification: Kingdom: Plantae,
Division: magnoliophyta , Class: magnoliopsida, Order: santalales, Family: santalsceae, Genus: Viscum, Specie: V. album
It is a hemi-parasitic shrub which grows on the stem of other trees. It has stems 30-100cm
(12-39in)long with dichotomous branching. The leaves are in opposite pairs, strapped shaped
entirely leather textured, 2.8cm (0.79-3.1in) long and 0.8-2.5cm broad.
Yellowish-green in color. The specie is deciduous and the flowers are inconspicuous
yellowish-green in 2-3mm diameter. The fruit is a white/yellow berry containing one (very
rarely several) seed embedded in the very sticky, glutinous fruit pulp (Morgenstern, 1996).
V. album has an added appearance; a yellowish ball hanging high up on the tree, visible only
when the host plant have lost its leaves. V. album is ever green and sustains its greenish
yellow leaves throughout the winter. It’s growing habit is distinctly round; it’s twigs branch
frequently and its elongated, oral leaves always grow in opposite pairs. The tiny
inconspicuous yellowish flowers appear in May. The berries are distinctly sticky, hence, the
latin name Viscum album-(white sticky stuff) and easily cling to branches and soon send out a
sucker rootlet that penetrate the back of the host three and tap its sap for nutrient and water.
Though, V. Album is a parasite and as such dependent on the host plant for nutrient and
water. It does not rely on host for CO2. or kill the host plant and thus is not really harmful to
the host. While birds feed on the berries without apparent harm, they are toxic to humans
(Morgenstern, 1996)
The toxic lectin viscumin has been isolated from v. album. Viscumin is a cyto-toxic protein
that binds to galactose residues ofcell surface glycoproteins and may be internalized by
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endocytosis. Viscum strongly inhibits protein synthesis by inactivating the 60 S-ribosomal
sub units.
V. album is chiefly used to lower blood pressure and heart rate, ease anxiety and promote
sleep. In low doses it can also relieve panic attacks and headaces and also improves the
ability to concentrate. There is no doubt that certain constituents of the plants, especially the
viscotoxins exhibits anti-cancer activities (Morgenstern, 1996) .
They are antispasmodic, cardiac, cytostatic, diuretic, hypotensive, narcotic, nervine,
stimulant, tonic and vasodilator. V. album has a reputation for curing epilepsy and other
convulsive nervous activities that causes the spams, but larger dosages can produce the
problem. V. album has also been employed in checking internal hemorrhages, in treating high
blood pressure and in treating cancer of the stomach, lungs and ovaries (Morgenstern, 1996).
Externally, the plant has been used to treat arthritis, rheumantism, chilblains, leg ulcer and
varicose veins. A homeopathic remedy is made from equal quantities of the berries and
leaves. It is difficult to make because of the viscidity of the sap. (Morgenstern, 1996)
Oguzie et al(2004a) worked on the influence of halide ion on the inhibition effect of Congo
red dye on the corrosion of mild steel in sulphuric acid solution and he formed out that Congo
red dye inhibits mild steel corrosion in sulphuric acid solution. The inhibition efficiency
increased with concentration but decreased with rise in temperature. The adsorption process
followed Flory Huggins isotherm. Also Oguzie et al , (2004b) worked on the corrosion
inhibition and adsorption behavior of bismark brown dye on aluminium in sodium hydroxide
solution and they found out that Bismark Brown dye inhibited aluminium corrosion in 0.1M
NaOH solution, the inhibition efficiency increasing with concentration. Furthermore, Oguzie
et al, worked on inhibition of mild steel corrosion in acid in media by aqueous extracts from
Garcinia Kola seed and they discovered that the extracts from seeds of Garcinia Kola inhibits
mild steel corrosion in 2 M HCl and 1M H2SO4 solutions by physical adsorption onto the
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metal surface. Also inhibition efficiency increased with increase in concentration but
decreased with rise in temperature.
Finally, Oguzie et al also studied the inhibitive effect of occinum vividis extract on the acid
corrosion of mild steel and he discovered that O. Vividis inhibited mild steel in 2 M HCl and
1 M H2SO4 at the temperature studies. Inhibition efficiency increased with an increase in
extract concentration and synergistically increased in the presence of halide ions. Temperature
studies recorded a decrease in efficiency with rise in temperature
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CHAPTER THREE
3.0 EXPERIMENTAL
3.1 Material Preparation
3.1.1 Metal Specimen
This study was carried out on mild steel metal procured from the Materials and
Metallurgical Engineering Department of Federal University of Technology, Owerri. The
mild steel has the following compositions: C; 0.05%, Mn; 0.60%, P; 0.36%, Si; 0.03%. It
was pressed–cut mechanically using the guillotine machine into coupons of uniform
dimensions 3cm x 3cm and a hole drilled at the centre of the coupon with radius 2.5mm.
Its thickness was 1mm. The coupons were used without further polishing. However, they
were degreased in absolute ethanol, dried in acetone and stored in moisture–free
desiccator containing silica gel prior to use.
3.1.1 REAGENTS
All reagents used were of BDH analytical grades purchased and used without further
purification. They included acetone, ethanol, conc. HCl, conc. H2SO4 and potassium
iodide. The blank corrodents were 1M HCl and 0.5M H2SO4 and were prepared from
their stock solutions. Potassium iodide used for corrosion experiment has molarity of
0.0005M. All gravimetric measurements were carried out using a FAJA weighting
balance of model FA 2004A and weighing capacity 0.0001-200g.
3.1.6 Extraction Process
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Each leaf (Dacryodis edulis, Viscuum ablum, Euphobeace hirtha linn, Piper guinesis
Moringa olifera and Mimosa pudica) extract solutions were prepared by boiling a
weighed amount of the ground leaves (20g) in 800ml of the acid using a reflux condenser
and 1000ml round-bottomed flask for three hours. This was carried out at low heating
temperature. The experiments were carried out separately for each of the acids (1M HCl
and 0.5M H2SO4). The solutions were allowed to cool to room temperature, filtered and
then stored in an air-tight glass container. The stock concentrations were determined by
carefully drying the residues and weighing to obtain the amount of the extracts infused in
the solutions.
GRAVIMETRIC MEASUREMENTS:
Blank Experiment;
250ml volumetric flask was filled with the stock acid solutions and then transferred to a
measuring cylinder and 200ml was measured and poured into a beaker and covered. Two
mild steel coupons labeled A and B for the two acids (two for each acid) were weighed
and suspended in the acid solution with the aid of a wooden cross bar and a polyester
rope at room temperature and also at 400C, 500C and 600C. The set up was allowed to
stand for six hours after which the coupons were retrieved, scrubbed with bristle brush
under running water, dried with acetone and warm air and then weighted. The final
weights of the coupons were less than the initial indicating that the mild coupons have
undergone corrosion leading to the dissolution of some parts.
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Gravimetric Measurements in the Presence of these Extracts
A micro syringe was used to aspirate the calculated volumes of extract stock solutions
into 250ml volumetric flasks and topped with the stock acid under investigation. The
contents were shaken vigorously to facilitate better dissolution of the extracts in the acid
solution. The 200ml of the mixture was transferred into a beaker and then covered. Two
mild steel coupons for each extract concentration were weighed and same procedure
carried out as in blank experiment.
The total surface area of mild steel coupon is given as
. . . . . . . . . . . . . . . . . . 3.1.9a
Where total surface area of immersed coupon
Length of coupon
width of coupon
thickness of coupon
radius of hole drilled on coupon.
Corrosion rates of mild steel in the different test solutions were determined using the
formular;
. . . . . . . . . . . . . . . 3.1.9b
Where corrosion rate in mg/dm2/day
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weight loss (mg).
time of retrieval in days
total surface area of mild steel coupon in dm2
From the value of corrosion rates in the presence and absence of the inhibitor, the
inhibition efficiencies were calculated using;
. . . . . . . . . . . . . . 3.1.9c
50mg/l exhibited lowest inhibition efficiency in both acid solutions while 800 mg/l and
1000 mg/l showed highest inhibition efficiency in 1M HCl and 0.5M H2SO4 respectively.
3.2.0 Experiment with a Halide (KI)
The effect of halide additives was studied by introducing 5.0mM of the halide ion
(potassium iodide) with each plant extracts to enhance the inhibiting performance of the
extract components. Ion-pair interactions between the organic cations and the halide ion
will result in increased surface coverage. Protonated or molecular species in the extract
components will be responsible for synergistic increase in inhibition efficiency.
3.3.0 Effect of Temperature on Corrosion and Corrosion Inhibition
This was carried out using the extract concentrations that inhibited least and the ones that
showed highest inhibition efficiency. Corrosion rates, inhibition efficiency and activation
energy were then calculated.
2.3. Electrochemical measurements
Metal samples for electrochemical experiments were machined into cylindrical
specimens and fixed in polytetrafluoroethylene (PTFE) rods by epoxy resin in such a way
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that only one circular surface of area 0.64 cm2 was left uncovered. The round surface was
necessary in order to avoid edge effects. The exposed surface was ground with silicon
carbide abrasive paper (from grade #200 to #1000), degreased in acetone, rinsed with
distilled water and dried in warm air. Electrochemical experiments were conducted in a
Model K0047 corrosion cell using a VERSASTAT 400 Complete DC Voltammetry and
Corrosion System, with V3 Studio software. Two graphite rods were used as counter
electrode and a saturated calomel electrode (SCE) as reference electrode. The latter was
connected via a Luggin’s capillary. Electrochemical corrosion tests were performed at the
end of 1 h of immersion at 303 K. Impedance measurements were made at corrosion
potentials (Ecorr) over a frequency range of 100 kHz – 10 mHz, with a signal amplitude
perturbation of 5 mV. Potentiodynamic polarization studies were carried out in the
potential range 250 mV versus corrosion potential (in 1 M HCl, which did not show
any evidence of passivation) and from -700 to 1600 mV (in 0.5 M H2SO4). The scan rate
in either case was 0.333 mV s-1. Each test was run in triplicate to verify the
reproducibility of the systems.
SURFACE ELECTRON-MICROSCOPY (SEM)
1cm×1cm coupons were dipped in blank solution and in best inhibitor concentration for
1-2 days. The coupons were retrieved after 1-2 hours, washed lightly with bristle brush
under running water, and then dried thoroughly in acetone and warm air. After which
they are packaged and tagged.
FTIR
Plant materials were obtained dried and grounded to fine powder. This powdered
sample was further divided into two with one subjected to analysis. The second part
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of the dried sample was extracted using 1M HCl and 0.5M H2SO4 solution. 20ml of
the extract was collected sun-dried and the powdered residue collected for analysis.
Two coupons were dipped seperately into 200ml of the highest inhibition
concentration from the two acid solutions for 2-3 days to form an adsorbed layer.
After which they were retrieved, dried scrape with sharp blade and the scrapings
collected for analysis.
Evaporate extract solution to dryness (no heat), collect powered residue
Dip 3-4 coupons in extract solution for 2-3 days to form extract adsorbed layer.
Retrieved, dry, scrape with sharp blade and collect the scrapping.
Three different samples for FTIR
Appendix
3.1.4 Preparation of Stock Solution for 1M HCl
Basis = 100g. Average assay = = 36.5
Volume of HCl = . . . . . . . . . . . . . . 3.1.4a
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cm3
84.75cm3of stock contains 36.5g HCl
1000cm3 will contain 430.68g
Therefore, mass concentration of HCl is g/dm3
Molarity (mol/dm3) = . . . . . . . . . . . . . . . 3.1.4b
11.81 mol/dm3
This indicates that the stock concentration of HCl is 11.81M.
To obtain the volume of 1M HCl needed for the experiment. The dilution formular was
used thereafter;
. . . . . . . . . . . . . . . . . . . . . . . 4.1.4c
Where
C1 = stock concentration (11.81 mol/dm3)
V1 = volume of stock acid required.
C2 = Concentration of acid required (1M)
V2 = Volume of flask used for dilution (2dm3)
ml
3.1.5 Preparation of Stock Solution for 0.5M H2SO4
Volume of HCl = . . . . . . . . . . . . . . . . . . . . 3.1.5a
= 54.35cm3
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Therefore, 54.35cm3 of the stock contains g H2S04
1000cm3 will contain g
Molar concentration (mol/dm3) = =18.40 mol/dm3
To obtain the volume of 0.5M H2SO4 needed, the dilution formular was also used
. . . . . . . . . . . . . . . . . . . . . . . . . 3.1.5b
Where all parameters used are as applied to HCl.
. . . . . . . . . . . . . . . . . . . . . . . . . . . . . 3.1.5c
Given that C1 = 0.5M, V2 = 2 dm3 and C1= 18.40 mol/dm3
Hence, V1 0.054347 mol/dm3 = 54.35ml.
54. 35ml of stock H2SO4 was therefore used to prepare a 2dm3 solution of 0.5M H2SO4.
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