"dioxide reacts with OH to form nitric acid: When clouds are present, the loss rate of SO is faster than can be explained by gas phase chemistry alone. This is due to reactions in the liquid water droplets. sulphur dioxide dissolves in water and then, like carbon dioxide, hydrolyses in a series of equilibrium reactions: There are a large number of aqueous reactions that oxidize sulphur from S(IV) to S(VI), leading to the formation of sulphuric acid. The most important oxidation reactions are with ozone, hydrogen peroxide and oxygen (reactions with oxygen are catalyzed by iron and manganese in the"
"organic compounds and metal particles. This method is preferred over the more traditional chromic acid bath for cleaning NMR tubes, because no traces of paramagnetic chromium can remain to spoil spectra. While chromic acid baths are discouraged because of the high toxicity of chromium and the potential for explosions, aqua regia is itself very corrosive and has been implicated in several explosions due to mishandling. Due to the reaction between its components resulting in its decomposition, aqua regia quickly loses its effectiveness (yet remains a strong acid), so its components are usually only mixed immediately before use. While local regulations"
"Adamkiewicz reaction The Adamkiewicz reaction is part of a biochemical test used to detect the presence of the amino acid tryptophan in proteins. When concentrated sulfuric acid is combined with a solution of protein and glyoxylic acid, a red/purple colour is produced. It was named after its discoverer, Albert Wojciech Adamkiewicz. Pure sulphuric acid and formaldehyde yields the reaction in addition to an oxidation-reduction reactionand also an avoidance of excess formaldehyde. This oxidizing agentcan be sodium amalgam to reduce oxalic acidwhile the reducing agentis nitric acid which oxidizes an alcohol. Reduction of the oxalic acid in done in a sulphuric"
"but the optic nerves may show demyelination, loss of axons and gliosis. International commerce of sulfuric acid is controlled under the United Nations Convention Against Illicit Traffic in Narcotic Drugs and Psychotropic Substances, 1988, which lists sulfuric acid under Table II of the convention as a chemical frequently used in the illicit manufacture of narcotic drugs or psychotropic substances. Sulfuric acid Sulfuric acid (alternative spelling sulphuric acid), also known as vitriol, is a mineral acid composed of the elements sulfur, oxygen and hydrogen, with molecular formula HSO. It is a colorless, odorless, and syrupy liquid that is soluble in water,"
"Sulfuric acid Sulfuric acid (alternative spelling sulphuric acid), also known as vitriol, is a mineral acid composed of the elements sulfur, oxygen and hydrogen, with molecular formula HSO. It is a colorless, odorless, and syrupy liquid that is soluble in water, in a reaction that is highly exothermic. Its corrosiveness can be mainly ascribed to its strong acidic nature, and, if at a high concentration, its dehydrating and oxidizing properties. It is also hygroscopic, readily absorbing water vapor from the air. Upon contact, sulfuric acid can cause severe chemical burns and even secondary thermal burns; it is very dangerous even"
"zero have been measured in ARD produced by this process. ARD can also produce sulfuric acid at a slower rate, so that the acid neutralizing capacity (ANC) of the aquifer can neutralize the produced acid. In such cases, the total dissolved solids (TDS) concentration of the water can be increased from the dissolution of minerals from the acid-neutralization reaction with the minerals. Sulfuric acid is used as a defense by certain marine species, for example, the phaeophyte alga ""Desmarestia munda"" (order Desmarestiales) concentrates sulfuric acid in cell vacuoles. In the stratosphere, the atmosphere's second layer that is generally between 10"
"with strong bases to form silicate salts, but not with water: Silicon dioxide is the anhydride of silicic acid: Si(OH) –> 2HO + SiO Phosphorus(III) oxide reacts to form phosphorous acid in water: Phosphorus(V) oxide reacts with water to give phosphoric (v) acid: Phosphorus pentoxide is the anhydride of phosphoric acid: 2HPO –> 3HO + PO. Sulfur dioxide reacts with water to form the weak acid, sulfurous acid: Sulfur trioxide forms the strong sulfuric acid with water (so, sulfur trioxide is the anhydride of sulfuric acid): This reaction is important in the manufacture of the acid. Chlorine(I) oxide reacts with"
"reactions result in the volatile products nitrosyl chloride and chlorine as evidenced by the fuming nature and characteristic yellow color of aqua regia. As the volatile products escape from solution, the aqua regia loses its potency. Nitrosyl chloride can further decompose into nitric oxide and chlorine. This dissociation is equilibrium-limited. Therefore, in addition to nitrosyl chloride and chlorine, the fumes over aqua regia contain nitric oxide. Because nitric oxide reacts readily with atmospheric oxygen, the gases produced also contain nitrogen dioxide, NO. Aqua regia was first mentioned in a work of Pseudo-Geber dated to ca. 1300. The third of Basil"
"Sulfurous acid Sulfurous acid (also sulphurous acid) is the chemical compound with the formula HSO. There is no evidence that sulfurous acid exists in solution, but the molecule has been detected in the gas phase. The conjugate bases of this elusive acid are, however, common anions, bisulfite (or hydrogen sulfite) and sulfite. Sulfurous acid is an intermediate species in the formation of acid rain from sulfur dioxide. Raman spectra of solutions of sulfur dioxide in water show only signals due to the SO molecule and the bisulfite ion, . The intensities of the signals are consistent with the following equilibrium:"
"Angeli–Rimini reaction The Angeli–Rimini reaction is an organic reaction between an aldehyde and the sulfonamide ""N-hydroxybenzenesulfonamide"" in presence of base forming an hydroxamic acid. The other reaction product is a sulfinic acid. The reaction was discovered by the two Italian chemists Angelo Angeli and Enrico Rimini (1874–1917), and was published in 1896. The reaction is used in a chemical test for the detection of aldehydes in combination with ferric chloride. In this test a few drops of aldehyde containing specimen is dissolved in ethanol, the sulfonamide is added together with some sodium hydroxide solution and then the solution is acidified"
"by accepting another oxygen atom. Sulfurous acid Sulfurous acid (also sulphurous acid) is the chemical compound with the formula HSO. There is no evidence that sulfurous acid exists in solution, but the molecule has been detected in the gas phase. The conjugate bases of this elusive acid are, however, common anions, bisulfite (or hydrogen sulfite) and sulfite. Sulfurous acid is an intermediate species in the formation of acid rain from sulfur dioxide. Raman spectra of solutions of sulfur dioxide in water show only signals due to the SO molecule and the bisulfite ion, . The intensities of the signals are"
"as a liquid medium for organisms with a chemistry based on silicon, oxygen, and other elements such as aluminium. Other solvents sometimes proposed: Sulfuric acid in liquid form is strongly polar. It remains liquid at higher temperatures than water, its liquid range being 10 °C to 337 °C at a pressure of 1 atm, although above 300 °C it will slowly decompose. Sulfuric acid is known to be abundant in the clouds of Venus, in the form of aerosol droplets. In a biochemistry that used sulfuric acid as a solvent, the alkene group (C=C), with two carbon atoms joined by"
"increase the hydrogen ion concentration of water. For instance, carbon dioxide increases the hydrogen ion concentration of rain water (pH = 5.6) by a factor of 25 compared to pure water (pH = 7). They are also Lewis acids, because they accept electron pairs from some Lewis bases, most notably base anhydrides. The oxides of period three elements demonstrate periodicity with respect to acidity. As you move across the period, the oxides become more acidic. Sodium and magnesium oxides are alkaline. Aluminium oxides are amphoteric (reacting both as a base or acid). Silicon, phosphorus, sulfur, and chlorine oxides are acidic."
"combining aromatic compounds and sulfur sources. The most important member of the class is Sulfur Black 1. It is produced by the reaction of 2,4-dinitrophenol and sodium sulfide in hot water. Like many sulfur dyes, details on the chemical reactions are poorly understood. It is accepted that the sulfide reduces the nitro groups to aniline derivatives, which are thought to form indophenol-containing intermediates that are further crosslinked by reaction with sulfur. The result are insoluble, high molecular weight species. Sulfur Black 1 is imperfectly understood, and the material is probably heterogeneous. It is speculated to be a polymer consisting of"
"presence of sulfuric acid and water. The recent patent literature describes batch and continuous processes that produce AMPS in high purity (to 99.7%) and improved yield (up to 89%, based on isobutene) with the addition of liquid isobutene to an acrylonitrile / sulfuric acid / phosphoric acid mixture at 40°C. 2-Acrylamido-2-methylpropane sulfonic acid 2-Acrylamido-2-methylpropane sulfonic acid (AMPS) was a Trademark name by The Lubrizol Corporation. It is a reactive, hydrophilic, sulfonic acid acrylic monomer used to alter the chemical properties of wide variety of anionic polymers. In the 1970s, the earliest patents using this monomer were filed for acrylic fiber"
"explains the old name of the acid ('oil of vitriol'). Commercial sulfuric acid is sold in several different purity grades. Technical grade is impure and often colored, but is suitable for making fertilizer. Pure grades, such as United States Pharmacopeia (USP) grade, are used for making pharmaceuticals and dyestuffs. Analytical grades are also available. Nine hydrates are known, but three of them were confirmed to be tetrahydrate (HSO·4HO), hemihexahydrate (HSO·HO) and octahydrate (HSO·8HO). Anhydrous is a very polar liquid, having a dielectric constant of around 100. It has a high electrical conductivity, caused by dissociation through protonating itself, a process"
"the Atlantic Ocean typically has a pH of 5.0–5.6; rain that comes across the continental from the west has a pH of 3.8–4.8; and local thunderstorms can have a pH as low as 2.0. Rain becomes acidic primarily due to the presence of two strong acids, sulfuric acid (HSO) and nitric acid (HNO). Sulfuric acid is derived from natural sources such as volcanoes, and wetlands (sulfate reducing bacteria); and anthropogenic sources such as the combustion of fossil fuels, and mining where HS is present. Nitric acid is produced by natural sources such as lightning, soil bacteria, and natural fires; while"
"forms the end=product. The formation of the nitrene intermediate 10 is ruled out given the lack of reactivity of the chemical mixture towards simple alkenes. The Angeli–Rimini reaction has recently been applied in solid-phase synthesis with the sulfonamide covelently linked to a polystyrene solid support. Angeli–Rimini reaction The Angeli–Rimini reaction is an organic reaction between an aldehyde and the sulfonamide ""N-hydroxybenzenesulfonamide"" in presence of base forming an hydroxamic acid. The other reaction product is a sulfinic acid. The reaction was discovered by the two Italian chemists Angelo Angeli and Enrico Rimini (1874–1917), and was published in 1896. The reaction is"
"acids belonging to this group of compounds are the products of the reaction between sulphurous and nitrous acids, the base being essential only in so far as it protects the products of the reaction against hydrolysis, and that, contrary to the statements of previous workers, normal sulfites and nitrites have no action on each other. Divers and Haga further showed that the primary product of the reaction between sulphurous and nitrous acids is always hydroxylaminedisulfonic acid and nothing else. Divers was pre-eminently an experimental chemist and rarely occupied with the theoretical study of chemical questions. He greatly encouraged the spirit"
"sulfuric acid (HSO) in water is accompanied by hydrolysis to give hydronium and bisulfate, the sulfuric acid's conjugate base. For a more technical discussion of what occurs during such a hydrolysis, see Brønsted–Lowry acid–base theory. Acid–base-catalysed hydrolyses are very common; one example is the hydrolysis of amides or esters. Their hydrolysis occurs when the nucleophile (a nucleus-seeking agent, e.g., water or hydroxyl ion) attacks the carbon of the carbonyl group of the ester or amide. In an aqueous base, hydroxyl ions are better nucleophiles than polar molecules such as water. In acids, the carbonyl group becomes protonated, and this leads"
", Bulgarian: солна киселина, Russian: соляная кислота, , Korean: 염산, and Taiwanese: iâm-sng. Gaseous HCl was called ""marine acid air"". The old (pre-systematic) name ""muriatic acid"" has the same origin (""muriatic"" means ""pertaining to brine or salt"", hence ""muriate"" means hydrochloride), and this name is still sometimes used. The name ""hydrochloric acid"" was coined by the French chemist Joseph Louis Gay-Lussac in 1814. Hydrochloric acid has been an important and frequently used chemical from early history and was discovered by the alchemist Jabir ibn Hayyan around the year 800 AD. Aqua regia, a mixture consisting of hydrochloric and nitric acids,"
"known that can be crystallised. It is a strong acid and concentrated solutions are strong oxidising agents, though gold, platinum, rhodium, and iridium are immune to attack. A 3:1 mixture of concentrated hydrochloric acid and nitric acid, called ""aqua regia"", is still stronger and successfully dissolves gold and platinum, because free chlorine and nitrosyl chloride are formed and chloride anions can form strong complexes. In concentrated sulfuric acid, nitric acid is protonated to form nitronium, which can act as an electrophile for aromatic nitration: The thermal stabilities of nitrates (involving the trigonal planar anion) depends on the basicity of the"
"hydroxides of the other alkali metals are also strong bases. Beryllium hydroxide Be(OH) is amphoteric. The hydroxide itself is insoluble in water, with a solubility product log ""K""* of −11.7. Addition of acid gives soluble hydrolysis products, including the trimeric ion [Be(OH)(HO)], which has OH groups bridging between pairs of beryllium ions making a 6-membered ring. At very low pH the aqua ion [Be(HO)] is formed. Addition of hydroxide to Be(OH) gives the soluble tetrahydroxoberyllate/tetrahydroxidoberyllate anion, [Be(OH)]. The solubility in water of the other hydroxides in this group increases with increasing atomic number. Magnesium hydroxide Mg(OH) is a strong base"
"Arsenic trisulfide Arsenic trisulfide is the inorganic compound with the formula AsS. It is a bright yellow solid that is insoluble in water. It also occurs as the mineral orpiment (Latin: auripigment), which has been used as a pigment called King's yellow. It is produced in the analysis of arsenic compounds. It is a group V/VI, intrinsic p-type semiconductor and exhibits photo-induced phase-change properties. The other principal arsenic sulfide is AsS, a red-orange solid known as the mineral realgar. AsS occurs both in crystalline and amorphous forms. Both forms feature polymeric structures consisting of trigonal pyramidal As(III) centres linked by"
"use for hydrosilylation, the main drawback is the deliquescent properties of the catalyst. It is generally agreed that chloroplatinic acid is a precursor to the actual catalyst. A possible role for colloidal platinum or zero-valent complexes has also been considered. Chloroplatinic acid prepared from aqua regia is proposed to contain nitrosonium hexachloroplatinate, (NO)PtCl. Nitrosonium hexachloroplatinate is obtained by the reaction of nitrosyl chloride (NOCl) and platinum metal. Nitrosonium hexachloroplatinate has been found to react vigorously with water and hydrochloric acid, making contamination of chloroplatinic acid prepared with aqua regia with nitrosonium hexachloroplatinate unlikely. Chloroplatinic acid Chloroplatinic acid or hexachloroplatinic acid"
"Sulfenic acid A sulfenic acid is an organosulfur compound and oxoacid with the general formula RSOH. It is the first member of the family of organosulfur oxoacids, which also include sulfinic acids and sulfonic acids, RSOH and RSOH, respectively. The base member of the sulfenic acid series with R = H is hydrogen thioperoxide. In contrast to sulfinic and sulfonic acids, simple sulfenic acids, such as methanesulfenic acid, CHSOH, are highly reactive and cannot be isolated in solution. In the gas phase the lifetime of methanesulfenic acid is about one minute. The gas phase structure of methanesulfenic acid was found"
"O NMR spectroscopy provided evidence that solutions of sulfurous acid and protonated sulfites contains a mixture of isomers, which is in equilibrium: When trying to concentrate the solution by evaporation to produce waterless sulfurous acid it will decompose (reversing the forming reaction). In cooling down a clathrate SO·HO will crystallise which decomposes again at 7 °C. Thus sulfurous acid HSO cannot be isolated. Aqueous solutions of sulfur dioxide, which sometimes are referred to as sulfurous acid, are used as reducing agents and as disinfectants, as are solutions of bisulfite and sulfite salts. They are oxidised to sulfuric acid or sulfate"
"acid, also known as oleum—sulfuric acid containing excess sulfur trioxide—and azeotropic nitric acid (consisting of about 70% nitric acid, with the rest being water). The sulfuric acid produces protonated nitric acid species, which are attacked by glycerol's nucleophilic oxygen atoms. The nitro group is thus added as an ester C−O−NO and water is produced. This is different from an electrophilic aromatic substitution reaction in which nitronium ions are the electrophile. The addition of glycerol results in an exothermic reaction (i.e., heat is produced), as usual for mixed-acid nitrations. If the mixture becomes too hot, it results in a runaway reaction,"
"with nitrosylsulfuric acid) and tower acid being the acid recovered from the bottom of the Glover tower. They are now obsolete as commercial concentrations of sulfuric acid, although they may be prepared in the laboratory from concentrated sulfuric acid if needed. In particular, ""10M"" sulfuric acid (the modern equivalent of chamber acid, used in many titrations) is prepared by slowly adding 98% sulfuric acid to an equal volume of water, with good stirring: the temperature of the mixture can rise to 80 °C (176 °F) or higher. Sulfuric acid reacts with its anhydride, , to form , called ""pyrosulfuric acid"","
"with hydrofluoric, hydrochloric, hydrobromic, hydriodic, sulfuric, or nitric acid. It does react with selenic acid, and is dissolved by aqua regia, a 1:3 mixture of nitric acid and hydrochloric acid. Nitric acid oxidizes the metal to +3 ions, but only in minute amounts, typically undetectable in the pure acid because of the chemical equilibrium of the reaction. However, the ions are removed from the equilibrium by hydrochloric acid, forming AuCl ions, or chloroauric acid, thereby enabling further oxidation. Gold is similarly unaffected by most bases. It does not react with aqueous, solid, or molten sodium or potassium hydroxide. It does"
"NOCl also arises from the combination of hydrochloric and nitric acids according to the following reaction: In nitric acid, NOCl is readily oxidized into nitrogen dioxide. The presence of NOCl in aqua regia was described by Edmund Davy in 1831. NOCl behaves as an electrophile and an oxidant in most of its reactions. With halide acceptors, for example antimony pentachloride, converts to nitrosonium salts: In a related reaction, sulfuric acid gives nitrosylsulfuric acid, the mixed acid anhydride of nitrous and sulfuric acid: NOCl reacts with silver thiocyanate to give silver chloride and the pseudohalogen nitrosyl thiocyanate: Nitrosyl chloride is used"
"Sulfamic acid Sulfamic acid, also known as amidosulfonic acid, amidosulfuric acid, aminosulfonic acid, and sulfamidic acid, is a molecular compound with the formula HNSO. This colorless, water-soluble compound finds many applications. Sulfamic acid melts at 205 °C before decomposing at higher temperatures to water, sulfur trioxide, sulfur dioxide and nitrogen. Sulfamic acid (HNSO) may be considered an intermediate compound between sulfuric acid (HSO), and sulfamide (HNSO), effectively replacing a hydroxyl (–OH) group with an amine (–NH) group at each step. This pattern can extend no further in either direction without breaking down the sulfonyl (–SO–) moiety. Sulfamates are derivatives of"
"be prepared by the reaction of red phosphorus with sodium chlorite at room temperature. A mixture of hypophosphoric acid, phosphorous acid (HPO) and phosphoric acid (HPO) is produced when white phosphorus oxidises in air when partially immersed in water. The tetrasodium salt NaPO·10HO crystallises at pH 10 and the disodium salt, NaHPO·6HO at pH 5.2. The disodium salt can be passed through an ion exchange column to form the acid dihydrate, HPO·2HO. The anhydrous acid can be formed by vacuum dehydration over PO or by the reaction of HS on lead hypophosphate, PbPO. Hypophosphoric acid is tetraprotic with dissociation constants"