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Τι (ποιος) είναι sulphuric acid - ορισμός
![Acidic [[drain cleaner]]s usually contain sulfuric acid at a high concentration which turns a piece of [[pH paper]] red and chars it instantly, demonstrating both the strong acidic nature and dehydrating property.](https://commons.wikimedia.org/wiki/Special:FilePath/Acidic drain cleaner containing sulfuric acid (sulphuric acid).jpg?width=200 "Acidic [[drain cleaner]]s usually contain sulfuric acid at a high concentration which turns a piece of [[pH paper]] red and chars it instantly, demonstrating both the strong acidic nature and dehydrating property.")
![An acidic [[drain cleaner]] can be used to dissolve grease, hair and even tissue paper inside water pipes.](https://commons.wikimedia.org/wiki/Special:FilePath/Acidic drain opener.JPG?width=200 "An acidic [[drain cleaner]] can be used to dissolve grease, hair and even tissue paper inside water pipes.")
![[[John Dalton]]'s 1808 sulfuric acid molecule shows a central [[sulfur]] atom bonded to three oxygen atoms, or [[sulfur trioxide]], the [[anhydride]] of sulfuric acid.](https://commons.wikimedia.org/wiki/Special:FilePath/Dalton's-sulphuric-acid.jpg?width=200 "[[John Dalton]]'s 1808 sulfuric acid molecule shows a central [[sulfur]] atom bonded to three oxygen atoms, or [[sulfur trioxide]], the [[anhydride]] of sulfuric acid.")
![Rio Tinto]] with its highly acidic water](https://commons.wikimedia.org/wiki/Special:FilePath/Rio tinto river CarolStoker NASA Ames Research Center.jpg?width=200 "Rio Tinto]] with its highly acidic water")
![D]]F in place of HF. (see text)](https://commons.wikimedia.org/wiki/Special:FilePath/Structure of protonated sulfuric acid.png?width=200 "D]]F in place of HF. (see text)")
Βικιπαίδεια
Sulfuric acid (American spelling and the preferred IUPAC name) or sulphuric acid (Commonwealth spelling), known in antiquity as oil of vitriol, is a mineral acid composed of the elements sulfur, oxygen, and hydrogen, with the molecular formula H2SO4. It is a colorless, odorless, and viscous liquid that is miscible with water.
Pure sulfuric acid does not occur naturally due to its strong affinity to water vapor; it is hygroscopic and readily absorbs water vapor from the air. Concentrated sulfuric acid is highly corrosive towards other materials, from rocks to metals, since it is an oxidant with powerful dehydrating properties. Phosphorus pentoxide is a notable exception in that it is not dehydrated by sulfuric acid but, to the contrary, dehydrates sulfuric acid to sulfur trioxide. Upon addition of sulfuric acid to water, a considerable amount of heat is released; thus, the reverse procedure of adding water to the acid should not be performed since the heat released may boil the solution, spraying droplets of hot acid during the process. Upon contact with body tissue, sulfuric acid can cause severe acidic chemical burns and even secondary thermal burns due to dehydration. Dilute sulfuric acid is substantially less hazardous without the oxidative and dehydrating properties; however, it should still be handled with care for its acidity.
Sulfuric acid is a very important commodity chemical; a country's sulfuric acid production is a good indicator of its industrial strength. It is widely produced with different methods, such as contact process, wet sulfuric acid process, lead chamber process, and some other methods. Sulfuric acid is also a key substance in the chemical industry. It is most commonly used in fertilizer manufacture but is also important in mineral processing, oil refining, wastewater processing, and chemical synthesis. It has a wide range of end applications, including in domestic acidic drain cleaners, as an electrolyte in lead-acid batteries, in dehydrating a compound, and in various cleaning agents. Sulfuric acid can be obtained by dissolving sulfur trioxide in water.
