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The lead chamber process for sulfuric acid production was abandoned, partly because it could not produce sulfur trioxide or concentrated sulfuric acid directly due to corrosion of the lead, and absorption of NO 2 gas. Until this process was made obsolete by the contact process, oleum had to be obtained through indirect methods.
Sulfuric(IV) acid (United Kingdom spelling: sulphuric(IV) acid), also known as sulfurous (UK: sulphurous) acid and thionic acid, [citation needed] is the chemical compound with the formula H 2 SO 3. Raman spectra of solutions of sulfur dioxide in water show only signals due to the SO 2 molecule and the bisulfite ion, HSO − 3 . [ 2 ]
The oleum is then diluted with water to form concentrated sulfuric acid. H 2 SO 4 + SO 3 → H 2 S 2 O 7 H 2 S 2 O 7 + H 2 O → 2 H 2 SO 4. Directly dissolving SO 3 in water, called the "wet sulfuric acid process", is rarely practiced because the reaction is extremely exothermic, resulting in a hot aerosol of sulfuric acid that requires ...
Sulfuric acid: strong mineral acid; applications include its use as a dehydrating agent in many chemical reactions, sulfonation, the purification of hydrocarbons, and the production of phosphoric acid tert-Butyl hydroperoxide: used in a variety of oxidation processes; industrially, is used as a starter of radical polymerization: Tetrahydrofuran
The acid is prepared by reacting excess sulfur trioxide (SO 3) with sulfuric acid: H 2 SO 4 + SO 3 → H 2 S 2 O 7. Disulfuric acid can be seen as the sulfuric acid analog of an acid anhydride. The mutual electron-withdrawing effects of each sulfuric acid unit on its neighbour causes a marked increase in acidity. Disulfuric acid is strong ...
Concentrated sulfuric acid is a strong dehydrating agent that can strip available water molecules and water components from sugar and organic tissue. [141] The burning of coal and/or petroleum by industry and power plants generates sulfur dioxide (SO 2) that reacts with atmospheric water and oxygen to produce sulfurous acid (H 2 SO 3). [142]
Examples of strong acids are hydrochloric acid (), perchloric acid (), nitric acid and sulfuric acid (). A weak acid is only partially dissociated, or is partly ionized in water with both the undissociated acid and its dissociation products being present, in solution, in equilibrium with each other.
The decomposition products can include sulfur, sulfur dioxide, hydrogen sulfide, polysulfanes, sulfuric acid and polythionates, depending on the reaction conditions. [6] Anhydrous methods of producing the acid were developed by Max Schmidt: [6] [7] H 2 S + SO 3 → H 2 S 2 O 3 Na 2 S 2 O 3 + 2 HCl → 2 NaCl + H 2 S 2 O 3 HSO 3 Cl + H 2 S → ...