Corrosion: Understanding the Basics by J. R. Davis

By J. R. Davis

Provides sensible discussions on thermodynamic and electrochemical ideas of corrosion, acceptance and prevention of assorted sorts of corrosion, varieties of corrosive environments more often than not encountered. DLC: Corrosion and anti-corrosives.

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Extra resources for Corrosion: Understanding the Basics

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With the third behavior, the metal corrodes but a state of passive behavior is observed. On immersion of the metal in the solution there is a reaction, and the metal does corrode; however, an insoluble, protective corrosion-product film is formed. This thin (~30Å) protective film, also referred to as a passive film, slows the reaction rate to very low levels. The corrosion resistance when dealing with passive behavior depends on the integrity of the protective film. If the passive film is broken or dissolves, then the metal can revert to active behavior and rapid dissolution can occur.

These compounds also produce a large number of hydrogen ions (hydrochloric acid) and hydroxyl ions (potassium hydroxide) in solution. Boric acid and ammonium hydrogen, on the other hand, are a weak acid and a weak base, respectively, because there are only a few hydrogen ions and hydroxyl ions in their solutions. The chemicals that are acids generate hydrogen ions when they dissociate. The chemicals that are bases produce hydroxyl ions when they dissociate. Salts are chemicals that produce neither hydrogen ions nor hydroxyl ions when they dissociate.

The position of metals in the emf series tells, in general, of the reactivity of the metal with deaerated acids, that is, acids containing no dissolved oxygen. Metals more negative than the hydrogen potential react with deaerated acids. Metals more positive than the hydrogen electrode are not attacked by deaerated acids. This only applies to acids in the absence of oxygen. The emf series provides an indication of the potential difference between two metals coupled together in a galvanic corrosion cell.

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