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| {{for|the Front Line Assembly album|Corrosion (album)}}
| | It is very common to have a dental emergency -- a fractured tooth, an abscess, or severe pain when chewing. Over-the-counter pain medication is just masking the problem. Seeing an emergency dentist is critical to getting the source of the problem diagnosed and corrected as soon as possible.<br><br>Here are some common dental emergencies:<br>Toothache: The most common dental emergency. This generally means a badly decayed tooth. As the pain affects the tooth's nerve, treatment involves gently removing any debris lodged in the cavity being careful not to poke deep as this will cause severe pain if the nerve is touched. Next rinse vigorously with warm water. Then soak a small piece of cotton in oil of cloves and insert it in the cavity. This will give temporary relief until a dentist can be reached.<br><br>At times the pain may have a more obscure location such as decay under an old filling. As this can be only corrected by a dentist there are two things you can do to help the pain. Administer a pain pill (aspirin or some other analgesic) internally or dissolve a tablet in a half glass (4 oz) of warm water holding it in the mouth for several minutes before spitting it out. DO NOT PLACE A WHOLE TABLET OR ANY PART OF IT IN THE TOOTH OR AGAINST THE SOFT GUM TISSUE AS IT WILL RESULT IN A NASTY BURN.<br><br>Swollen Jaw: This may be caused by several conditions the most probable being an abscessed tooth. In any case the treatment should be to reduce pain and swelling. An ice pack held on the outside of the jaw, (ten minutes on and ten minutes off) will take care of both. If this does not control the pain, an analgesic tablet can be given every four hours.<br><br>Other Oral Injuries: Broken teeth, cut lips, bitten tongue or lips if severe means a trip to a dentist as soon as possible. In the mean time rinse the mouth with warm water and place cold compression the face opposite the injury. If there is a lot of bleeding, apply direct pressure to the bleeding area. If bleeding does not stop get patient to the emergency room of a hospital as stitches may be necessary.<br><br>Prolonged Bleeding Following Extraction: Place a gauze pad or better still a moistened tea bag over the socket and have the patient bite down gently on it for 30 to 45 minutes. The tannic acid in the tea seeps into the tissues and often helps stop the bleeding. If bleeding continues after two hours, call the dentist or take patient to the emergency room of the nearest hospital.<br><br>Broken Jaw: If you suspect the patient's jaw is broken, bring the upper and lower teeth together. Put a necktie, handkerchief or towel under the chin, tying it over the head to immobilize the jaw until you can get the patient to a dentist or the emergency room of a hospital.<br><br>Painful Erupting Tooth: In young children teething pain can come from a loose baby tooth or from an erupting permanent tooth. Some relief can be given by crushing a little ice and wrapping it in gauze or a clean piece of cloth and putting it directly on the tooth or gum tissue where it hurts. The numbing effect of the cold, along with an appropriate dose of aspirin, usually provides temporary relief.<br><br>In young adults, an erupting 3rd molar (Wisdom tooth), especially if it is impacted, can cause the jaw to swell and be quite painful. Often the gum around the tooth will show signs of infection. Temporary relief can be had by giving aspirin or some other painkiller and by dissolving an aspirin in half a glass of warm water and holding this solution in the mouth over the sore gum. AGAIN DO NOT PLACE A TABLET DIRECTLY OVER THE GUM OR CHEEK OR USE THE ASPIRIN SOLUTION ANY STRONGER THAN RECOMMENDED TO PREVENT BURNING THE TISSUE. The swelling of the jaw can be reduced by using an ice pack on the outside of the face at intervals of ten minutes on and ten minutes off.<br><br>In the event you beloved this post as well as you wish to receive more details with regards to [http://www.youtube.com/watch?v=90z1mmiwNS8 dentist DC] kindly visit our web site. |
| {{Mechanical failure modes}}
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| '''Corrosion''' is the gradual destruction of materials, (usually [[metal]]s), by chemical reaction with its environment.
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| In the most common use of the word, this means electrochemical [[oxidation]] of metals in reaction with an oxidant such as [[oxygen]]. [[Rusting]], the formation of [[iron]] oxides, is a well-known example of electrochemical corrosion. This type of damage typically produces [[oxide]](s) or [[salt (chemistry)|salt]](s) of the original metal. Corrosion can also occur in materials other than metals, such as [[ceramic materials|ceramics]] or [[polymers]], although in this context, the term degradation is more common. Corrosion degrades the useful properties of materials and structures including strength, appearance and permeability to liquids and gases.
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| Many structural [[alloy]]s corrode merely from exposure to moisture in air, but the process can be strongly affected by exposure to certain substances. Corrosion can be concentrated locally to form a [[Corrosion#Pitting corrosion|pit]] or crack, or it can extend across a wide area more or less uniformly corroding the surface. Because corrosion is a diffusion-controlled process, it occurs on exposed surfaces. As a result, methods to reduce the activity of the exposed surface, such as [[Passivation (chemistry)|passivation]] and [[Chromate conversion coating|chromate conversion]], can increase a material's corrosion resistance. However, some corrosion mechanisms are less visible and less predictable.
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| [[File:Rust and dirt.jpg|thumb|right|Rust, the most familiar example of corrosion.]]
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| [[File:Corroding machinery at old White Island sulphur mine.JPG|thumb|right|[[Volcanic gas]]es have accelerated the corrosion of this abandoned mining machinery.]]
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| [[File:Rust Bolt.JPG|thumb|right|Corrosion on exposed metal.]]
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| == Galvanic corrosion ==
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| {{Main|Galvanic corrosion}}
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| [[File:Galvanic corrosion of aluminum and steel in seawater.jpg|thumb|Galvanic corrosion of aluminium. A 5-mm-thick Al alloy plate is physically (and hence, electrically) connected to a 10-mm-thick mild steel structural support. Galvanic corrosion occurred on the Al plate along the joint with the steel. Perforation of Al plate occurred within 2 years.<ref>[http://www.corrosionclinic.com/types_of_corrosion/galvanic_corrosion.htm Galvanic Corrosion]. Corrosionclinic.com. Retrieved on 2012-07-15.</ref>]]
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| Galvanic corrosion occurs when two different metals have physical or electrical contact with each other and are immersed in a common [[electrolyte]], or when the same metal is exposed to electrolyte with different concentrations. In a [[galvanic cell|galvanic couple]], the more active metal (the anode) corrodes at an accelerated rate and the more [[noble metal]] (the cathode) corrodes at a retarded rate. When immersed separately, each metal corrodes at its own rate. What type of metal(s) to use is readily determined by following the [[galvanic series]]. For example, zinc is often used as a sacrificial anode for steel structures. Galvanic corrosion is of major interest to the marine industry and also anywhere water (containing salts) contacts pipes or metal structures.
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| Factors such as relative size of [[anode]], types of metal, and operating conditions ([[temperature]], [[humidity]], [[salinity]], etc.) affect galvanic corrosion. The surface area ratio of the anode and [[cathode]] directly affects the corrosion rates of the materials. Galvanic corrosion is often prevented by the use of [[sacrificial anode]]s.
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| === Galvanic series ===
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| {{Main|Galvanic series}}
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| In a given environment (one standard medium is aerated, room-temperature [[seawater]]), one metal will be either more ''noble'' or more ''active'' than others, based on how strongly its ions are bound to the surface. Two metals in electrical contact share the same electrons, so that the "tug-of-war" at each surface is analogous to competition for free electrons between the two materials. Using the electrolyte as a host for the flow of ions in the same direction, the noble metal will take electrons from the active one. The resulting mass flow or electrical current can be measured to establish a hierarchy of materials in the medium of interest. This hierarchy is called a ''galvanic series'' and is useful in predicting and understanding corrosion. This method is expensive but offers maximum protection against corrosion.
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| == Corrosion removal ==
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| Often it is possible to chemically remove the products of corrosion. For example [[phosphoric acid]] in the form of [[naval jelly]] is often applied to ferrous tools or surfaces to remove rust. Corrosion removal should not be confused with [[electropolishing]], which removes some layers of the underlying metal to make a smooth surface. For example, phosphoric acid may also be used to electropolish copper but it does this by removing copper, not the products of copper corrosion.
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| == Resistance to corrosion ==
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| Some metals are more intrinsically resistant to corrosion than others (for some examples, see [[galvanic series]]). There are various ways of protecting metals from corrosion (oxidation) including painting, [[hot dip galvanizing]], and combinations of these.<ref>[http://www.pipingtech.com/technical/bulletins/corrosion_protection.htm Methods of Protecting Against Corrosion] Piping Technology & Products, (retrieved January 2012)</ref>
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| === Intrinsic chemistry ===
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| [[File:GoldNuggetUSGOV.jpg|thumb|Gold nuggets do not naturally corrode, even on a geological time scale.]]
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| The materials most resistant to corrosion are those for which corrosion is [[thermodynamics|thermodynamically]] unfavorable. Any corrosion products of [[gold]] or [[platinum]] tend to decompose spontaneously into pure metal, which is why these elements can be found in metallic form on Earth and have long been valued. More common "base" metals can only be protected by more temporary means.
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| Some metals have naturally slow [[chemical kinetics|reaction kinetics]], even though their corrosion is thermodynamically favorable. These include such metals as [[zinc]], [[magnesium]], and [[cadmium]]. While corrosion of these metals is continuous and ongoing, it happens at an acceptably slow rate. An extreme example is [[graphite]], which releases large amounts of energy upon [[oxidation]], but has such slow kinetics that it is effectively immune to electrochemical corrosion under normal conditions.
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| === Passivation ===
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| {{Main|Passivation (chemistry)}}
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| Passivation refers to the spontaneous formation of an ultrathin film of corrosion products known as passive film, on the metal's surface that act as a barrier to further oxidation. The chemical composition and microstructure of a passive film are different from the underlying metal. Typical passive film thickness on aluminium, stainless steels and alloys is within 10 nanometers. The passive film is different from oxide layers that are formed upon heating and are in the micrometer thickness range – the passive film recovers if removed or damaged whereas the oxide layer does not. Passivation in natural environments such as air, water and soil at moderate [[pH]] is seen in such materials as [[aluminium]], [[stainless steel]], [[titanium]], and [[silicon]].
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| Passivation is primarily determined by metallurgical and environmental factors. The effect of pH is summarized using [[Pourbaix diagram]]s, but many other factors are influential. Some conditions that inhibit passivation include high pH for aluminium and zinc, low pH or the presence of [[chloride]] ions for stainless steel, high temperature for titanium (in which case the oxide dissolves into the metal, rather than the electrolyte) and [[fluoride]] ions for silicon. On the other hand, unusual conditions may result in passivation of materials that are normally unprotected, as the alkaline environment of [[concrete]] does for [[steel]] [[rebar]]. Exposure to a liquid metal such as [[mercury (element)|mercury]] or hot [[solder]] can often circumvent passivation mechanisms.
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| Passivation is primarily determined by metallurgical and environmental factors.
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| == Corrosion in passivated materials ==
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| Passivation is extremely useful in mitigating corrosion damage, however even a high-quality alloy will corrode if its ability to form a passivating film is hindered. Proper selection of the right grade of material for the specific environment is important for the long-lasting performance of this group of materials. If breakdown occurs in the passive film due to chemical or mechanical factors, the resulting major modes of corrosion may include [[pitting corrosion]], [[crevice corrosion]] and [[stress corrosion cracking]].
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| === Pitting corrosion ===
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| {{Main|Pitting corrosion}}
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| [[File:Pitting corrosion-scheme.png|thumb|upright|The scheme of pitting corrosion]]
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| Certain conditions, such as low concentrations of oxygen or high concentrations of species such as chloride which complete as [[anion]]s, can interfere with a given alloy's ability to re-form a passivating film. In the worst case, almost all of the surface will remain protected, but tiny local fluctuations will degrade the oxide film in a few critical points. Corrosion at these points will be greatly amplified, and can cause ''corrosion pits'' of several types, depending upon conditions. While the corrosion pits only [[nucleation|nucleate]] under fairly extreme circumstances, they can continue to grow even when conditions return to normal, since the interior of a pit is naturally deprived of oxygen and locally the pH decreases to very low values and the corrosion rate increases due to an autocatalytic process. In extreme cases, the sharp tips of extremely long and narrow corrosion pits can cause [[stress concentration]] to the point that otherwise tough alloys can shatter; a thin film pierced by an invisibly small hole can hide a thumb sized pit from view. These problems are especially dangerous because they are difficult to detect before a part or structure [[structural failure|fails]]. Pitting remains among the most common and damaging forms of corrosion in passivated alloys{{Citation needed|date=May 2010}}, but it can be prevented by control of the alloy's environment.
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| === Weld decay and knifeline attack ===
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| [[File:Unsensitised structure of type 304 stainless steel.jpg|thumb|Normal microstructure]][[File:Sensitized structure of 304 stainless steel.jpg|thumb|Sensitized microstructure]]
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| {{Main|Intergranular corrosion}}
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| Stainless steel can pose special corrosion challenges, since its passivating behavior relies on the presence of a major alloying component ([[chromium]], at least 11.5%). Because of the elevated temperatures of [[welding]] and heat treatment, chromium [[carbide]]s can form in the [[crystallite|grain boundaries]] of stainless alloys. This chemical reaction robs the material of chromium in the zone near the grain boundary, making those areas much less resistant to corrosion. This creates a [[electrochemistry|galvanic couple]] with the well-protected alloy nearby, which leads to ''weld decay'' (corrosion of the grain boundaries in the heat affected zones) in highly corrosive environments.
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| A stainless steel is said to be sensitized if [[chromium carbide]]s are formed in the microstructure. A typical microstructure of a normalized type-304 stainless steel shows no signs of sensitization while a heavily sensitized steel shows the presence of grain boundary precipitates. The dark lines in the sensitized microstructure are networks of chromium carbides formed along the grain boundaries.<ref>[http://www.corrosionclinic.com/types_of_corrosion/intergranular_corrosion_cracking.htm Intergranular Corrosion]. Corrosionclinic.com. Retrieved on 2012-07-15.</ref>
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| Special alloys, either with low carbon content or with added carbon "[[getter]]s" such as titanium and [[niobium]] (in types 321 and 347, respectively), can prevent this effect, but the latter require special heat treatment after welding to prevent the similar phenomenon of ''knifeline attack''. As its name implies, corrosion is limited to a very narrow zone adjacent to the weld, often only a few micrometers across, making it even less noticeable.
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| === Crevice corrosion ===
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| {{Main|Crevice corrosion}}
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| [[File:Crevice corrosion of 316 stainless steel in desalination.jpg|thumb|Corrosion in the crevice between the tube and tube sheet (both made of type-316 stainless steel) of a heat exchanger in a seawater desalination plant.<ref>[http://www.corrosionclinic.com/types_of_corrosion/crevice_corrosion.htm Crevice Corrosion]. Corrosionclinic.com. Retrieved on 2012-07-15.</ref>]]
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| [[Crevice corrosion]] is a localized form of corrosion occurring in confined spaces (crevices), to which the access of the working fluid from the environment is limited. Formation of a differential aeration cell leads to corrosion inside the crevices. Examples of crevices are gaps and contact areas between parts, under gaskets or seals, inside cracks and seams, spaces filled with deposits and under sludge piles.
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| Crevice corrosion is influenced by the crevice type (metal-metal, metal-nonmetal), crevice geometry (size, surface finish), and metallurgical and environmental factors. The susceptibility to crevice corrosion can be evaluated with ASTM standard procedures. A critical crevice corrosion temperature is commonly used to rank a material's resistance to crevice corrosion.
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| == Microbial corrosion ==
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| {{Main|Microbial corrosion}}
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| [[Microbial corrosion]], or commonly known as microbiologically influenced corrosion (MIC), is a corrosion caused or promoted by [[microorganism]]s, usually [[chemoautotroph]]s. It can apply to both metallic and non-metallic materials, in the presence or absence of oxygen. [[Sulfate-reducing bacteria]] are active in the absence of oxygen (anaerobic); they produce [[hydrogen sulfide]], causing [[sulfide stress cracking]]. In the presence of oxygen (aerobic), some bacteria may directly oxidize iron to iron oxides and hydroxides, other bacteria oxidize sulfur and produce sulfuric acid causing [[biogenic sulfide corrosion]]. [[Concentration cell]]s can form in the deposits of corrosion products, leading to localized corrosion.
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| Accelerated low-water corrosion (ALWC) is a particularly aggressive form of MIC that affects steel piles in seawater near the low water tide mark. It is characterized by an orange sludge, which smells of hydrogen sulfide when treated with acid. Corrosion rates can be very high and design corrosion allowances can soon be exceeded leading to premature failure of the steel pile.<ref>JE Breakell, M Siegwart, K Foster, D Marshall, M Hodgson, R Cottis, S Lyon. ''Management of Accelerated Low Water Corrosion in Steel Maritime Structures'', Volume 634 of CIRIA Series, 2005, ISBN 0-86017-634-7</ref> Piles that have been coating and have cathodic protection installed at the time of construction are not susceptible to ALWC. For unprotected piles, sacrificial anodes can be installed local to the affected areas to inhibit the corrosion or a complete retrofitted sacrificial anode system can be installed. Affected areas can also be treated electrochemically by using an electrode to first produce chlorine to kill the bacteria, and then to produced a calcareous deposit, which will help shield the metal from further attack.
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| == High-temperature corrosion ==
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| High-temperature corrosion is chemical deterioration of a material (typically a metal) as a result of heating. This non-galvanic form of corrosion can occur when a metal is subjected to a hot atmosphere containing oxygen, sulfur or other compounds capable of oxidizing (or assisting the oxidation of) the material concerned. For example, materials used in aerospace, power generation and even in car engines have to resist sustained periods at high temperature in which they may be exposed to an atmosphere containing potentially highly corrosive products of combustion.
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| The products of high-temperature corrosion can potentially be turned to the advantage of the engineer. The formation of oxides on stainless steels, for example, can provide a protective layer preventing further atmospheric attack, allowing for a material to be used for sustained periods at both room and high temperatures in hostile conditions. Such high-temperature corrosion products, in the form of [[compacted oxide layer glaze]]s, prevent or reduce wear during high-temperature sliding contact of metallic (or metallic and ceramic) surfaces.
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| == Metal Dusting ==
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| {{Main|Metal dusting}}
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| [[Metal dusting]] is a catastrophic form of corrosion that occurs when susceptible materials are exposed to environments with high carbon activities, such as synthesis gas and other high-CO environments. The corrosion manifests itself as a break-up of bulk metal to metal powder. The suspected mechanism is firstly the deposition of a graphite layer on the surface of the metal, usually from carbon monoxide (CO) in the vapour phase. This graphite layer is then thought to form metastable M<sub>3</sub>C species (where M is the metal), which migrate away from the metal surface. However, in some regimes no M<sub>3</sub>C species is observed indicating a direct transfer of metal atoms into the graphite layer.
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| == Protection from corrosion ==
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| [[File:Corrosion protection.jpg|thumbnail|US Army [[shrink wrap]]s equipment such as helicopters to protect it from corrosion and thus save millions of dollars.]]
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| === Surface treatments ===
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| ==== Applied coatings ====
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| {{Main|Galvanization}}
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| [[File:Galvanized surface.jpg|thumb|[[Galvanization|Galvanized]] surface]]
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| [[Plating]], [[paint]]ing, and the application of [[vitreous enamel|enamel]] are the most common [[anti-corrosion]] treatments. They work by providing a barrier of corrosion-resistant material between the damaging environment and the structural material. Aside from cosmetic and manufacturing issues, there may be tradeoffs in mechanical flexibility versus resistance to abrasion and high temperature. Platings usually fail only in small sections, but if the plating is more noble than the substrate (for example, chromium on steel), a [[galvanic couple]] will cause any exposed area to corrode much more rapidly than an unplated surface would. For this reason, it is often wise to plate with active metal such as zinc or cadmium.
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| Painting either by roller or brush is more desirable for tight spaces; spray would be better for larger coating areas such as steel decks and waterfront applications. Flexible polyurethane coatings, like Durabak-M26 for example, can provide an anti-corrosive seal with a highly durable slip resistant membrane. Painted coatings are relatively easy to apply and have fast drying times although temperature and humidity may cause dry times to vary.
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| ==== Reactive coatings ====
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| If the environment is controlled (especially in recirculating systems), [[corrosion inhibitor]]s can often be added to it. These chemicals form an electrically insulating or chemically impermeable coating on exposed metal surfaces, to suppress electrochemical reactions. Such methods make the system less sensitive to scratches or defects in the coating, since extra inhibitors can be made available wherever metal becomes exposed. Chemicals that inhibit corrosion include some of the salts in [[hard water]] (Roman water systems are famous for their [[Eifel Aqueduct#The aqueduct as a stone quarry|mineral deposits]]), [[chromate]]s, [[phosphate]]s, [[polyaniline]], other [[conducting polymers]] and a wide range of specially-designed chemicals that resemble [[surfactant]]s (i.e. long-chain organic molecules with ionic end groups).
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| ==== Anodization ====
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| {{Main|Anodizing}}
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| [[File:Belaying8.jpg|thumb|right|This [[Belay device|climbing descender]] is anodized with a yellow finish.]]
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| Aluminium alloys often undergo a surface treatment. Electrochemical conditions in the bath are carefully adjusted so that uniform pores, several [[nanometer]]s wide, appear in the metal's oxide film. These pores allow the oxide to grow much thicker than passivating conditions would allow. At the end of the treatment, the pores are allowed to seal, forming a harder-than-usual surface layer. If this coating is scratched, normal passivation processes take over to protect the damaged area.
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| Anodizing is very resilient to weathering and corrosion, so it is commonly used for building facades and other areas that the surface will come into regular contact with the elements. Whilst being resilient, it must be cleaned frequently. If left without cleaning, [[panel edge staining]] will naturally occur.
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| ====Biofilm coatings====
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| A new form of protection has been developed by applying certain species of bacterial films to the surface of metals in highly corrosive environments. This process increases the corrosion resistance substantially. Alternatively, antimicrobial-producing [[biofilms]] can be used to inhibit mild steel corrosion from [[sulfate-reducing bacteria]].<ref>{{cite journal|author=R. Zuo, D. Örnek, B.C. Syrett, R.M. Green, C.-H. Hsu, F.B. Mansfeld and T.K. Wood|title= Inhibiting mild steel corrosion from sulfate-reducing bacteria using antimicrobial-producing biofilms in Three-Mile-Island process water|journal= Appl. Microbiol. Biotechnol. |year=2004|volume= 64|pages=275–283|doi=10.1007/s00253-003-1403-7}}</ref>
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| === Controlled permeability formwork ===
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| {{Main|Controlled permeability formwork}}
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| Controlled permeability formwork (CPF) is a method of preventing the corrosion of [[reinforcement]] by naturally enhancing the durability of the [[Concrete cover|cover]] during concrete placement. CPF has been used in environments to combat the effects of [[carbonation]], chlorides, [[frost]] and abrasion.
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| === Cathodic protection ===
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| {{Main|Cathodic protection}}
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| Cathodic protection (CP) is a technique to control the corrosion of a metal surface by making that surface the cathode of an [[electrochemical cell]]. Cathodic protection systems are most commonly used to protect steel, water, and fuel [[pipeline transport|pipelines]] and tanks; steel pier [[Deep foundation|piles]], ships, and offshore [[oil platform]]s.
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| ==== Sacrificial anode protection ====
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| [[File:Sacrificial anode.jpg|thumb|Sacrificial anode on the hull of a ship.]]
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| For effective CP, the potential of the steel surface is polarized (pushed) more negative until the metal surface has a uniform potential. With a uniform potential, the driving force for the corrosion reaction is halted. For galvanic CP systems, the anode material corrodes under the influence of the steel, and eventually it must be replaced. The [[polarization (corrosion)|polarization]] is caused by the current flow from the anode to the cathode, driven by the difference in electrochemical potential between the anode and the cathode.
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| ==== Impressed current cathodic protection ====
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| For larger structures, galvanic anodes cannot economically deliver enough current to provide complete protection. [[Cathodic protection#Impressed current CP|Impressed current cathodic protection]] (ICCP) systems use anodes connected to a [[direct current|DC]] power source (such as a [[cathodic protection rectifier]]). Anodes for ICCP systems are tubular and solid rod shapes of various specialized materials. These include high silicon [[cast iron]], graphite, mixed metal oxide or platinum coated titanium or niobium coated rod and wires.
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| === Anodic protection ===
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| {{Main|Anodic protection}}
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| Anodic protection impresses anodic current on the structure to be protected (opposite to the cathodic protection). It is appropriate for metals that exhibit passivity (e.g., stainless steel) and suitably small passive current over a wide range of potentials. It is used in aggressive environments, e.g., solutions of sulfuric acid.
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| ===Rate of corrosion===
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| A simple test for measuring corrosion is the weight loss method.{{citation needed|date=July 2012}} The method involves exposing a clean weighed piece of the metal or alloy to the corrosive environment for a specified time followed by cleaning to remove corrosion products and weighing the piece to determine the loss of weight. The rate of corrosion (R) is calculated as
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| :<big>''R = KW/(ρAt)''</big>
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| where ''k'' is a constant,
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| ''W'' is the weight loss of the metal in time ''t'', ''A'' is the surface area of the metal exposed, and ''ρ'' is the density of the metal (in g/cm³).
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| == Economic impact ==
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| [[File:Silver Bridge collapsed, Ohio side.jpg|thumb|The collapsed Silver Bridge, as seen from the Ohio side]]
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| In 2002, the US [[Federal Highway Administration]] released a study titled ''Corrosion Costs and Preventive Strategies in the United States'' on the direct costs associated with metallic corrosion in the U.S. industry. In 1998, the total annual direct cost of corrosion in the U.S. was ca. $276 billion (ca. 3.2% of the US [[gross domestic product]]).<ref>Gerhardus H. Koch, Michiel P.H.Brongers, Neil G. Thompson, Y. Paul Virmani and Joe H. Payer. [http://web.archive.org/web/20110708193325/http://www.corrosioncost.com/summary.htm CORROSION COSTS AND PREVENTIVE STRATEGIES IN THE UNITED STATES] – report by CC Technologies Laboratories, Inc. to Federal Highway Administration (FHWA), September 2001.</ref>
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| Rust is one of the most common causes of bridge accidents. As rust has a much higher volume than the originating mass of iron, its build-up can also cause failure by forcing apart adjacent parts. It was the cause of the collapse of the [[Mianus river bridge]] in 1983, when the bearings rusted internally and pushed one corner of the road slab off its support. Three drivers on the roadway at the time died as the slab fell into the river below. The following [[NTSB]] investigation showed that a drain in the road had been blocked for road re-surfacing, and had not been unblocked; as a result, runoff water penetrated the support hangers. Rust was also an important factor in the [[Silver Bridge]] disaster of 1967 in [[West Virginia]], when a steel [[suspension bridge]] collapsed within a minute, killing 46 drivers and passengers on the bridge at the time.
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| Similarly, corrosion of concrete-covered steel and iron can cause the concrete to [[spall]], creating severe structural problems. It is one of the most common failure modes of [[reinforced concrete]] [[bridge]]s. Measuring instruments based on the [[Half-cell potential field measurement of concrete|half-cell potential]] can detect the potential corrosion spots before total failure of the concrete structure is reached.
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| Until 20–30 years ago; galvanized steel pipe was used extensively in the potable water systems for single and multi-family residents as well as commercial and public construction. Today, these systems have long ago consumed the protective zinc and are corroding internally resulting in poor water quality and pipe failures.<ref>{{cite web|last=Robles, PE|first=Daniel|title=Potable Water Pipe Condition Assessment For a High Rise Condominium in The Pacific Northwest|url=http://crmanage.com/potable-water-pipe-condition-assessment-for-a-high-rise-structure-in-the-pacific-northwest/|publisher=GSG Group, Inc. Dan Robles, PE|accessdate=10 December 2012}}</ref> The economic impact on homeowners, condo dwellers, and the public infrastructure is estimated at 22 billion dollars as insurance industry braces for a wave of claims due to pipe failures.
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| == Corrosion in nonmetals ==
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| Most [[ceramic]] materials are almost entirely immune to corrosion. The strong [[chemical bond]]s that hold them together leave very little free chemical energy in the structure; they can be thought of as already corroded. When corrosion does occur, it is almost always a simple dissolution of the material or chemical reaction, rather than an electrochemical process. A common example of corrosion protection in ceramics is the [[Calcium oxide|lime]] added to soda-lime [[glass]] to reduce its solubility in water; though it is not nearly as soluble as pure [[sodium silicate]], normal glass does form sub-microscopic flaws when exposed to moisture. Due to its [[brittle]]ness, such flaws cause a dramatic reduction in the strength of a glass object during its first few hours at room temperature.
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| === Corrosion of polymers ===
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| [[File:Ozone cracks in tube1.jpg|thumb|[[Ozone cracking]] in [[natural rubber]] tubing]]
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| [[Polymer degradation]] involves several complex and often poorly understood physiochemical processes. These are strikingly different from the other processes discussed here, and so the term "corrosion" is only applied to them in a loose sense of the word. Because of their large molecular weight, very little [[entropy]] can be gained by mixing a given mass of polymer with another substance, making them generally quite difficult to dissolve. While dissolution is a problem in some polymer applications, it is relatively simple to design against. A more common and related problem is ''swelling'', where small molecules infiltrate the structure, reducing strength and stiffness and causing a volume change. Conversely, many polymers (notably flexible [[polyvinyl chloride|vinyl]]) are intentionally swelled with [[plasticizer]]s, which can be leached out of the structure, causing brittleness or other undesirable changes. The most common form of degradation, however, is a decrease in polymer chain length. Mechanisms which break polymer chains are familiar to biologists because of their effect on [[DNA]]: [[ionizing radiation]] (most commonly [[ultraviolet]] light), [[Radical (chemistry)|free radical]]s, and [[redox|oxidizer]]s such as oxygen, [[ozone]], and [[chlorine]]. [[Ozone cracking]] is a well-known problem affecting [[natural rubber]] for example. [[Plastic additive|Additive]]s can slow these process very effectively, and can be as simple as a UV-absorbing [[pigment]] (i.e., [[titanium dioxide]] or [[carbon black]]). [[Plastic shopping bag]]s often do not include these additives so that they break down more easily as [[litter]].
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| === Corrosion of glasses ===
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| [[File:Glaskorrosion.jpg|thumb|Glass corrosion]]
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| [[Glass disease]] is the corrosion of silicate glasses in [[aqueous]] solutions. It is governed by two mechanisms: [[diffusion]]-controlled leaching (ion exchange) and hydrolytic dissolution of the glass network.<ref>A.K. Varshneya. [http://books.google.com/books?id=P8g_Mm-VayYC&printsec=frontcover ''Fundamentals of inorganic glasses'']. Gulf Professional Publishing, 1994 ISBN 0127149708.</ref> Both mechanisms strongly depend on the pH of contacting solution: the rate of ion exchange decreases with pH as 10<sup>−0.5pH</sup> whereas the rate of hydrolytic dissolution increases with pH as 10<sup>0.5pH</sup>.<ref>M.I. Ojovan, W.E. Lee. [http://books.google.com/books?id=rAL-7GU0ec8C&printsec=frontcover ''New Developments in Glassy Nuclear Wasteforms'']. Nova Science Publishers, New York (2007) ISBN 1600217834 pp. 100 ff.</ref>
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| Mathematically, corrosion rates of glasses are characterized by normalized corrosion rates of elements NR<sub>i</sub> (g/cm<sup>2</sup>·d) which are determined as the ratio of total amount of released species into the water M<sub>i</sub> (g) to the water-contacting surface area S (cm<sup>2</sup>), time of contact t (days) and weight fraction content of the element in the glass f<sub>i</sub>:
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| :<math>NR_i = \frac{M_i}{Sf_it}</math>.
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| The overall corrosion rate is a sum of contributions from both mechanisms (leaching + dissolution) NR<sub>i</sub>=Nrx<sub>i</sub>+NRh.
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| Diffusion-controlled leaching (ion exchange) is characteristic of the initial phase of corrosion and involves replacement of alkali ions in the glass by a hydronium (H<sub>3</sub>O<sup>+</sup>) ion from the solution. It causes an ion-selective depletion of near surface layers of glasses and gives an inverse square root dependence of corrosion rate with exposure time. The diffusion-controlled normalized leaching rate of cations from glasses (g/cm<sup>2</sup>·d) is given by:
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| :<math>NRx_i = 2\rho \sqrt{\frac{D_i}{\pi t}}</math>,
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| where t is time, D<sub>i</sub> is the i-th cation effective diffusion coefficient (cm<sup>2</sup>/d), which depends on pH of contacting water as D<sub>i</sub> = D<sub>i0</sub>·10<sup>–pH</sup>, and ρ is the density of the glass (g/cm<sup>3</sup>).
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|
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| Glass network dissolution is characteristic of the later phases of corrosion and causes a congruent release of ions into the water solution at a time-independent rate in dilute solutions (g/cm<sup>2</sup>·d):
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| :<math> NRh = \rho r_h </math>,
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| where r<sub>h</sub> is the stationary [[hydrolysis]] (dissolution) rate of the glass (cm/d).
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| In closed systems the consumption of protons from the aqueous phase increases the pH and causes a fast transition to hydrolysis.<ref>[http://books.google.com/books?id=xBkP6wVu_VgC&printsec=frontcover ''Corrosion of Glass, Ceramics and Ceramic Superconductors'']. D.E. Clark, B.K. Zoitos (eds.), William Andrew Publishing/Noyes (1992) ISBN 081551283X.</ref> However, a further saturation of solution with silica impedes hydrolysis and causes the glass to return to an ion-exchange, e.g. diffusion-controlled regime of corrosion.
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| In typical natural conditions normalized corrosion rates of silicate glasses are very low and are of the order of 10<sup>−7</sup>–10<sup>−5</sup> g/(cm<sup>2</sup>·d). The very high durability of silicate glasses in water makes them suitable for hazardous and nuclear waste immobilisation.
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| ==== Glass corrosion tests ====
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| [[File:Spidergraph ChemDurab.png|thumb|Effect of addition of a certain glass component on the chemical durability against water corrosion of a specific base glass (corrosion test ISO 719).<ref>[http://glassproperties.com/chemical_durability/ Calculation of the Chemical Durability (Hydrolytic Class) of Glasses]. Glassproperties.com. Retrieved on 2012-07-15.</ref>]]
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| There exist numerous standardized procedures for measuring the corrosion (also called '''chemical durability''') of glasses in neutral, basic, and acidic environments, under simulated environmental conditions, in simulated body fluid, at high temperature and pressure,<ref>[http://www.vscht.cz/sil/english/chemtech_ag/vht.htm Vapor Hydration Testing (VHT)]. Vscht.cz. Retrieved on 2012-07-15.</ref> and under other conditions.
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| The standard procedure ISO 719<ref>[http://www.iso.org/iso/iso_catalogue/catalogue_tc/catalogue_detail.htm?csnumber=4948 International Organization for Standardization, Procedure 719 (1985)]. Iso.org (2011-01-21). Retrieved on 2012-07-15.</ref> describes a test of the extraction of water-soluble basic compounds under neutral conditions: 2 g of glass, particle size 300–500 μm, is kept for 60 min in 50 ml de-ionized water of grade 2 at 98 °C; 25 ml of the obtained solution is titrated against 0.01 mol/l [[Hydrochloric acid|HCl]] solution. The volume of HCl required for neutralization is classified according to the table below.
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| {| class="wikitable"
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| |-
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| ! Amount of 0.01M HCl needed to neutralize extracted basic oxides, ml
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| ! Extracted [[Sodium oxide|Na<sub>2</sub>O]]<br>equivalent, μg
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| ! Hydrolytic<br>class
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| |-
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| | < 0.1
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| | < 31
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| | 1
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| |-
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| | 0.1-0.2
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| | 31-62
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| | 2
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| |-
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| | 0.2-0.85
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| | 62-264
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| | 3
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| |-
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| | 0.85-2.0
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| | 264-620
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| | 4
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| |-
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| | 2.0-3.5
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| | 620-1085
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| | 5
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| |-
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| | > 3.5
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| | > 1085
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| | > 5
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| |}
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| == See also ==
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| {{colbegin|3}}
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| * [[Anaerobic corrosion]]
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| * [[Chemical hazard label]]
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| * [[Copper band]] corrosion.
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| * [[Corrosion in space]]
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| * [[Electronegativity]]
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| * [[Electrical resistivity measurement of concrete]]
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| * [[Environmental stress fracture]]
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| * [[Forensic engineering]]
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| * [[FRP tanks and vessels]]
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| * [[Hydrogen analyzer]]
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| * [[Hydrogen embrittlement]]
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| * [[Kelvin probe force microscope]]
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| * [[Oxidation potential]]
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| *[[Pitting Resistance Equivalent Number]]
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| * [[Redox]]
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| * [[Reduction potential]]
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| * [[Periodic table]]
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| * [[Rouging]]
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| * [[Salt spray test]]
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| * [[Stress corrosion cracking]]
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| * [[Tribocorrosion]]
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| * [[Zinc pest]]
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| * [http://isalama.wordpress.com/article/corrosion-inhibitors-in-the-oilfield-3uf3kbfllnswt-4/ Corrosion Inhibitors in the Oilfield]
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| {{colend}}
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| == References ==
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| {{Reflist|35em}}
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| ==Further reading==
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| * {{cite book
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| | title = Principles and Prevention of Corrosion
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| | edition = 2nd edition
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| | last = Jones
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| | first = Denny | publisher = [[Prentice Hall]]
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| | location = [[Upper Saddle River, New Jersey]]
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| | year = 1996
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| | isbn = 0-13-359993-0 }}
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| == External links ==
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| {{Commons category|Corrosion}}
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| * [http://www.corrosionprevention.org.uk/ Corrosion Prevention Association]
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| *[http://www.nace.org/ NACE International] -Professional society for corrosion engineers ( [[NACE International|NACE]] )
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| * [http://www.llnl.gov/es_and_h/hsm/doc_14.08/doc14-08.html Working Safely with Corrosive Chemicals]
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| *[http://www.efcweb.org/Member_Societies.html efcweb.org] – European Federation of Corrosion
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| *[http://www.corrosionist.com/Corrosion_Fundamental.htm Metal Corrosion] – Corrosion Theory
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| *[http://electrochem.cwru.edu/encycl/art-c02-corrosion.htm Electrochemistry of corrosion]
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| * A 3.4-Mb pdf handbook [http://ammtiac.alionscience.com/pdf/Corrosion_Hdbk_S2.pdf "Corrosion Prevention and Control"], 2006, 296 pages, US DoD
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| *[http://www.emergometal.com/_EmergoMetal/files/bf/bf0c3008-68d2-4d64-9fcf-eb00859e32ca.pdf How do you remove and prevent flash rust on stainless steel?] Article about the preventions of flash rust
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| *[http://www.doitpoms.ac.uk/tlplib/aqueous_corrosion/index.php DoITPoMS Teaching and Learning Package- "Kinetics of Aqueous Corrosion"]
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| [[Category:Corrosion| ]]
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| [[Category:Glass chemistry]]
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