query: give the name and formula for the acid derived from the following anion chlorite

pos: Chlorite Chlorite The chlorite ion, or chlorine dioxide anion, is . A chlorite (compound) is a compound that contains this group, with chlorine in oxidation state +3. Chlorites are also known as salts of chlorous acid. The free acid, chlorous acid HClO, is the least stable oxoacid of chlorine and has only been observed as an aqueous solution at low concentrations. Since it cannot be concentrated, it is not a commercial product. The alkali metal and alkaline earth metal compounds are all colorless or pale yellow, with sodium chlorite (NaClO) being the only commercially important chlorite. Heavy metal chlorites (Ag, Hg,

pos: Chlorous acid Chlorous acid Chlorous acid is an inorganic compound with the formula HClO. It is a weak acid. Chlorine has oxidation state +3 in this acid. The pure substance is unstable, disproportionating to hypochlorous acid (Cl oxidation state +1) and chloric acid (Cl oxidation state +5): Although the acid is difficult to obtain in pure substance, the conjugate base, chlorite, derived from this acid is stable. One example of a salt of this anion is the well-known sodium chlorite. This and related salts are sometimes used in the production of chlorine dioxide. HClO can be prepared through reaction of barium or

pos: Sodium chlorite solution in the presence of a chlorine scavenger (usually 2-methyl-2-butene). In 2005, sodium chlorite was used as an oxidizing agent to convert alkyl furans to the corresponding 4-oxo-2-alkenoic acids in a simple one pot synthesis. Mixing sodium chlorite solution with a weak food-grade acid solution (commonly citric acid), both stable, produces short-lived acidified sodium chlorite (ASC) which has potent decontaminating properties. Upon mixing the main active ingredient, chlorous acid is produced in equilibrium with chlorite anion. The proportion varies with pH, temperature, and other factors, ranging from approximately 5–35% chlorous acid with 65–95% chlorite; more acidic solutions result in a

pos: Chlorite Chlorite The chlorite ion, or chlorine dioxide anion, is . A chlorite (compound) is a compound that contains this group, with chlorine in oxidation state +3. Chlorites are also known as salts of chlorous acid. The free acid, chlorous acid HClO, is the least stable oxoacid of chlorine and has only been observed as an aqueous solution at low concentrations. Since it cannot be concentrated, it is not a commercial product. The alkali metal and alkaline earth metal compounds are all colorless or pale yellow, with sodium chlorite (NaClO) being the only commercially important chlorite. Heavy metal chlorites (Ag, Hg,

pos: Chlorite of a greater family of other chlorine oxides. Chlorite The chlorite ion, or chlorine dioxide anion, is . A chlorite (compound) is a compound that contains this group, with chlorine in oxidation state +3. Chlorites are also known as salts of chlorous acid. The free acid, chlorous acid HClO, is the least stable oxoacid of chlorine and has only been observed as an aqueous solution at low concentrations. Since it cannot be concentrated, it is not a commercial product. The alkali metal and alkaline earth metal compounds are all colorless or pale yellow, with sodium chlorite (NaClO) being the only

pos: Sodium chlorite higher proportion of chlorous acid. Chlorous acid breaks down to chlorine dioxide which in turn breaks down to chlorite anion and ultimately chloride anion. ASC is used for sanitation of the hard surfaces which come in contact with food and as a wash or rinse for a variety of foods including red meat, poultry, seafood, fruits and vegetables. Because the oxo-chlorine compounds are unstable when properly prepared, there should be no measurable residue on food if treated appropriately. ASC also is used as a teat dip for control of mastitis in dairy cattle. The U.S. Army Natick Soldier Research, Development,

pos: Chlorous acid lead chlorite and dilute sulfuric acid: Chlorous acid is a powerful oxidizing agent, although its tendency to disproportionation counteracts its oxidizing potential. Chlorine is the only halogen to form an isolable acid of formula HXO. Neither bromous acid nor iodous acid has ever been isolated. A few salts of bromous acid, bromites, are known, but no iodites. Chlorous acid Chlorous acid is an inorganic compound with the formula HClO. It is a weak acid. Chlorine has oxidation state +3 in this acid. The pure substance is unstable, disproportionating to hypochlorous acid (Cl oxidation state +1) and chloric acid (Cl oxidation

neg: Formate metal: Such fine powders are useful as hydrogenation catalysts. Formate Formate (IUPAC name: methanoate) is the anion derived from formic acid. Its formula is represented in various equivalent ways: HCOO or CHOO or HCO. It is the product of deprotonation of formic acid. It is the simplest carboxylate anion. A formate (compound) is a salt or ester of formic acid. Formate is reversibly oxidized by the enzyme formate dehydrogenase from "Desulfovibrio gigas": Formate esters have the formula ROC(O)H (alternative way of writing formula ROCH). Many form spontaneously when alcohols dissolve in formic acid. The most important formate ester is methyl

neg: Formate Formate Formate (IUPAC name: methanoate) is the anion derived from formic acid. Its formula is represented in various equivalent ways: HCOO or CHOO or HCO. It is the product of deprotonation of formic acid. It is the simplest carboxylate anion. A formate (compound) is a salt or ester of formic acid. Formate is reversibly oxidized by the enzyme formate dehydrogenase from "Desulfovibrio gigas": Formate esters have the formula ROC(O)H (alternative way of writing formula ROCH). Many form spontaneously when alcohols dissolve in formic acid. The most important formate ester is methyl formate, which is produced as an intermediate en route

neg: Acetylenedicarboxylic acid separated and the latter is treated with sulfuric acid. Acetylenedicarboxylic acid is used in the synthesis of dimethyl acetylenedicarboxylate, an important laboratory reagent. The acid is commonly traded as a laboratory chemical. It can also be reacted with sulfur tetrafluoride to produce hexafluoro-2-butyne, a powerful dienophile for use in Diels-Alder reactions. Hydrogenacetylenedicarboxylate (often abbreviated as Hadc or HADC) is a monovalent anion of acetylenedicarboxylic acid with the formula CHO or <chem>HO2C-C#C-CO2-</chem>. The anion can be derived from acetylenedicarboxylic acid by removal of a single proton or from the acetylenedicarboxylate dianion by addition of a proton. The name is also used

neg: Sulfamic acid deprotonation can be effected in ammonia solution to give the anion . With nitrous acid, sulfamic acid reacts to give nitrogen: while with nitric acid, it affords nitrous oxide: The reaction of excess hypochlorite ions with sulfamic acid or a sulfamate salt gives rise reversibly to both "N"-chlorosulfamate and "N","N"-dichlorosulfamate ions. Consequently, sulfamic acid is used as hypochlorite scavenger in the oxidation of aldehydes with chlorite such as the Pinnick oxidation. Upon heating sulfamic acid will react with alcohols to form the corresponding organosulfates. It is more expensive than other reagents for doing this, such as chlorosulfonic acid or oleum,

neg: Acetylenedicarboxylic acid potassium hydrogenacetylenedicarboxylate. Potassium hydrogenacetylenedicarboxylate is a potassium salt of HADC with chemical formula KCHO or K·HCO, often abbreviated as KHadc. It is often called potassium hydrogen acetylenedicarboxylate or monopotassium acetylenedicarboxylate. The salt can be obtained from acetylenedicarboxylic acid and is a common laboratory starting material for the synthesis of other derivatives of that acid. In the crystalline form, the hydrogenacetylenedicarboxylate anions are joined into linear chains by uncommonly short hydrogen bonds. Acetylenedicarboxylate (often abbreviated as ADC or adc) is a divalent anion with formula CO or [OC–C≡C–CO]; or any salt or ester thereof. The anion can be derived from acetylenedicarboxylic

neg: Dioxosuccinic acid Dioxosuccinic acid Dioxosuccinic acid or dioxobutanedioic acid is an organic compound with formula CHO or HO−(C=O)−OH. Removal of two protons from the molecule would yield the dioxosuccinate anion, or O−(C=O)−O. This is one of the oxocarbon anions, which consist solely of carbon and oxygen. The name is also used for salts containing that anion, and for esters with the [−O−(C=O)−O−] moiety. Removal of a single proton would result in the monovalent anion hydrogendioxosuccinate, or HO−(C=O)−O. Dioxosuccinic acid is one of the acids occurring naturally in wine, from the oxidation of tartaric acid via dihydroxyfumaric acid. The acid combines with two

neg: Tetrathionate Tetrathionate The tetrathionate anion, , is a sulfur oxoanion derived from the compound tetrathionic acid, HSO. Two of the sulfur atoms present in the ion are in oxidation state 0 and two are in oxidation state +5. Alternatively, the compound can be viewed as the adduct resulting from the binding of to SO. Tetrathionate is one of the polythionates, a family of anions with the formula [S(SO)]. Its IUPAC name is "(sulfonatodisulfanyl)sulfonate", the name of its corresponding acid is "(sulfodisulfanyl)sulfonic acid". The Chemical Abstracts Service identifies tetrathionate by the CAS Number 15536-54-6. Tetrathionate is a product of the oxidation of

neg: Hexafluorophosphoric acid Hexafluorophosphoric acid Hexafluorophosphoric acid is the inorganic compound with the chemical formula HOPF. Although the formula is often written as HPF, this compound is only available as the hydrate. This strong Brønsted acid features a non-coordinating anion, hexafluorophosphate (). It is formed from the reaction of hydrogen fluoride with phosphorus pentafluoride. Like many strong acids, hexafluorophosphoric acid is not isolable but is handled only in solution. Its aqueous solutions consist of hydronium ion, , and . Additionally, such solutions often contain products derived from hydrolysis of the P-F bonds, including , , and , and their conjugate bases. Hexafluorophosphoric acid

neg: Hexafluorophosphoric acid attacks glass. Upon heating, it decomposes to generate HF. Crystalline has been obtained as the hexahydrate, wherein is enclosed in truncated octahedral cages defined by the water and protons. NMR spectroscopy indicates that solutions derived from this hexahydrate contain significant amounts of HF. Hexafluorophosphoric acid Hexafluorophosphoric acid is the inorganic compound with the chemical formula HOPF. Although the formula is often written as HPF, this compound is only available as the hydrate. This strong Brønsted acid features a non-coordinating anion, hexafluorophosphate (). It is formed from the reaction of hydrogen fluoride with phosphorus pentafluoride. Like many strong acids, hexafluorophosphoric acid

neg: Sodium chlorite explosively with heat or shock. Sodium chlorite is derived indirectly from sodium chlorate, NaClO. First, the explosive ("only" at concentrations greater than 10% in atmosphere) chlorine dioxide, ClO is produced by reducing sodium chlorate in a strong acid solution with a suitable reducing agent (for example, sodium sulfite, sulfur dioxide, or hydrochloric acid). The chlorine dioxide is then absorbed into an alkaline solution and reduced with hydrogen peroxide (), yielding sodium chlorite. Sodium chlorite Sodium Chlorite (NaClO) is a chemical compound used in the manufacturing of paper and as a disinfectant. The main application of sodium chlorite is the generation

neg: Oxyacid phosphoric acid, HPO, has sometimes been called "orthophosphoric acid", in order to distinguish it from metaphosphoric acid, HPO. However, according to IUPAC's current rules, the prefix "ortho-" should only be used in names of orthotelluric acid and orthoperiodic acid, and their corresponding anions and salts. In the following table, the formula and the name of the anion refer to what remains of the acid when it loses "all" its hydrogen atoms as protons. Many of these acids, however, are polyprotic, and in such cases, there also exists one or more intermediate anions. In name of such anions, the prefix "hydrogen-"

neg: Formic acid Formic acid Formic acid, systematically named methanoic acid, is the simplest carboxylic acid. The chemical formula is HCOOH or HCOH. It is an important intermediate in chemical synthesis and occurs naturally, most notably in some ants. The word "formic" comes from the Latin word for ant, "formica", referring to its early isolation by the distillation of ant bodies. Esters, salts, and the anion derived from formic acid are called formates. Industrially formic acid is produced from methanol. Formic acid is a colorless liquid having a pungent, penetrating odor at room temperature, not unlike the related acetic acid. It is miscible

neg: Orthocarbonic acid Orthocarbonic acid Orthocarbonic acid (methanetetrol) is the name given to a hypothetical compound with the chemical formula HCO or C(OH). Its molecular structure consists of a single carbon atom bonded to four hydroxy groups. It would be therefore a fourfold alcohol. In theory it could lose four protons to give the hypothetical oxocarbon anion (orthocarbonate), and is therefore considered an oxoacid of carbon. Orthocarbonic acid is highly unstable. Calculations show that it decomposes spontaneously into carbonic acid and HO: Orthocarbonic acid is one of the group of carboxylic "ortho acids" that have the general structure of RC(OH).The term "ortho acid"

neg: Chlorite Tl, Pb, and also Cu and ) are unstable and decompose explosively with heat or shock. Sodium chlorite is derived indirectly from sodium chlorate, NaClO. First, the explosively unstable gas chlorine dioxide, ClO is produced by reducing sodium chlorate in a strong acid solution with a suitable reducing agent (for example, sodium chloride, sulfur dioxide, or hydrochloric acid). The chlorite ion adopts a bent molecular geometry, due to the effects of the lone pairs on the chlorine atom, with an O–Cl–O bond angle of 111° and Cl–O bond lengths of 156 pm. Chlorite is the strongest oxidiser of the chlorine

neg: Croconate blue Croconate blue Croconate blue or 1,2,3-tris(dicyanomethylene)croconate is a divalent anion with chemical formula or ((N≡C−)C=)(CO). It is one of the pseudo-oxocarbon anions, as it can be described as a derivative of the croconate oxocarbon anion through the replacement of three oxygen atoms by dicyanomethylene groups =C(−C≡N). The term Croconate Blue as a dye name specifically refers to the dipotassium salt . The anion was synthesized and characterized by A. Fatiadi in 1978, together with croconate violet. He obtained the corresponding acid, croconate acid blue by treating croconic acid with malononitrile in water solution at 80–90 °C. Croconate acid blue is

neg: Malic acid Malic acid Malic acid is an organic compound with the molecular formula . It is a dicarboxylic acid that is made by all living organisms, contributes to the sour taste of fruits, and is used as a food additive. Malic acid has two stereoisomeric forms (- and -enantiomers), though only the -isomer exists naturally. The salts and esters of malic acid are known as malates. The malate anion is an intermediate in the citric acid cycle. The name "malic" derives from Latin, "malus" meaning "apple". This derivation is also seen in the traditional German name for malic acid being Äpfelsäure

neg: Squaric acid Squaric acid Squaric acid, also called quadratic acid because its four carbon atoms approximately form a square, is a dibasic organic acid with the chemical formula . The conjugate base of squaric acid is the hydrogensquarate anion ; and the conjugate base of the hydrogensquarate anion is the divalent squarate anion . This is one of the oxocarbon anions, which consist only of carbon and oxygen. Squaric acid is a reagent for chemical synthesis, used for instance to make photosensitive squaraine dyes and inhibitors of protein tyrosine phosphatases. Squaric acid is a white crystalline powder with a thermal decomposition point

neg: Sodium tetraphenylborate strong acids, the anion undergoes protonolysis to give triphenylborane and benzene: Weakly coordinating anions often are based on tetraarylborates, with electronegative substituents. Examples include B(CF) and Brookhart's acid containing the tetrakis[3,5-bis(trifluoromethyl)phenyl]borate anion. Sodium tetraphenylborate Sodium tetraphenylborate is the organic compound with the formula NaB(CH). It is a salt, wherein the anion consists of four phenyl rings bonded to boron. This white crystalline solid is used to prepare other tetraphenylborate salts, which are often highly soluble in organic solvents. The compound is used in inorganic and organometallic chemistry as a precipitating agent for potassium, ammonium, rubidium, and cesium ions, and some

neg: Stearic acid Stearic acid Stearic acid ( , ) is a saturated fatty acid with an 18-carbon chain and has the IUPAC name octadecanoic acid. It is a waxy solid and its chemical formula is CHCOH. Its name comes from the Greek word στέαρ ""stéar"", which means tallow. The salts and esters of stearic acid are called stearates. As its ester, stearic acid is one of the most common saturated fatty acids found in nature following palmitic acid. The triglyceride derived from three molecules of stearic acid is called stearin. Stearic acid is obtained from fats and oils by the saponification of

neg: Oxocarbon anion stable 1,2-dioxetanedione CO; and the stable croconate anion corresponds to the neutral cyclopentanepentone CO, which has been detected only in trace amounts. Conversely, some oxocarbon anions can be reduced to yield other anions with the same structural formula but greater negative charge. Thus rhodizonate can be reduced to the tetrahydroxybenzoquinone (THBQ) anion and then to benzenehexolate . An oxocarbon anion can also be associated with the anhydride of the corresponding acid. The latter would be another oxocarbon with formula CO; namely, the acid minus water molecules HO. The standard example is the connection between carbonate and carbon dioxide CO. The

neg: Peroxycarbonate catalytic effect of CO on the oxidation of organic compounds by O. The potassium and rubidium salts of the monovalent hydrogenperoxocarbonate anion have also been obtained. Peroxycarbonate In chemistry, peroxycarbonate (sometimes peroxocarbonate) is a divalent anion with formula . It is an oxocarbon anion that consists solely of carbon and oxygen. It would be the anion of a hypothetical peroxocarbonic acid HO–CO–O–OH or the real hydroperoxyformic acid, HO-O-CO-OH (a.k.a. percarbonic acid, carbonoperoxoic acid). The peroxycarbonate anion is formed, together with peroxydicarbonate , at the negative electrode during electrolysis of molten lithium carbonate. Lithium peroxycarbonate can be produced also by combining

neg: Peroxycarbonate Peroxycarbonate In chemistry, peroxycarbonate (sometimes peroxocarbonate) is a divalent anion with formula . It is an oxocarbon anion that consists solely of carbon and oxygen. It would be the anion of a hypothetical peroxocarbonic acid HO–CO–O–OH or the real hydroperoxyformic acid, HO-O-CO-OH (a.k.a. percarbonic acid, carbonoperoxoic acid). The peroxycarbonate anion is formed, together with peroxydicarbonate , at the negative electrode during electrolysis of molten lithium carbonate. Lithium peroxycarbonate can be produced also by combining carbon dioxide CO with lithium hydroxide in concentrated hydrogen peroxide HO at −10 °C. The peroxycarbonate anion has been proposed as an intermediate to explain the

neg: Bistriflimide has been referred to as an amidate or imidate in an attempt to distinguish it from the acid.) The complications in naming these compounds was highlighted in an article by the IUPAC. Since then, the IUPAC has recommended (2013) that derivatives of anionic nitrogen can be named as azanides, so bis[(trifluoromethane)sulfonyl]azanide would be an acceptable and unambiguous name for bistriflimide anion. Bistriflimide Bistriflimide, systematically known as bis(trifluoromethane)sulfonimide (or 'imidate', "see below") and colloquially as TFSI, is a non-coordinating anion with the chemical formula [(CFSO)N]. The anion is widely used in ionic liquids (e.g.Trioctylmethylammonium bis(trifluoromethylsulfonyl)imide), since it is less toxic and

neg: Chlorine dioxide Traditionally, chlorine dioxide for disinfection applications has been made from sodium chlorite or the sodium chlorite – hypochlorite method: or the sodium chlorite – hydrochloric acid method: or the chlorite – sulfuric acid method: 8ClO + 4HSO → 4ClO + 2HClO + 4SO + 2HO + 2HCl All three sodium chlorite chemistries can produce chlorine dioxide with high chlorite conversion yield, but unlike the other processes the chlorite-sulfuric acid method produces completely chlorine-free chlorine dioxide, although it suffers from the requirement of 25% more chlorite to produce an equivalent amount of chlorine dioxide. Alternatively, hydrogen peroxide may be efficiently used

neg: Hyponitrous acid reversible, should not be considered as the anhydride of . The "cis" acid is not known, but its sodium salt can be obtained. Hyponitrous acid ("trans") can be prepared from silver(I) hyponitrite and anhydrous HCl in ether: Spectroscopic data indicate a "trans" configuration for the resulting acid. In enzymology, a hyponitrite reductase is an enzyme that catalyzes the chemical reaction Hyponitrous acid Hyponitrous acid is a chemical compound with formula or HON=NOH. It is an isomer of nitramide, HN−NO. Hyponitrous acid forms two series of salts, the hyponitrites containing the [ON=NO] anion, and the "acid hyponitrites" containing the [HON=NO] anion.

neg: Non-coordinating anion notable Lewis acid of this genre is tris(pentafluorophenyl)borane, B(CF), which abstracts alkyl ligands: Another large class of non-coordinating anions are derived from carborane anion . Using this anion, the first example of a three-coordinate silicon compound, the salt [(mesityl)Si][HCBMeBr] contains a non-coordinating anion derived from a carborane. Non-coordinating anion Anions that interact weakly with cations are termed non-coordinating anions, although a more accurate term is weakly coordinating anion. Non-coordinating anions are useful in studying the reactivity of electrophilic cations. They are commonly found as counterions for cationic metal complexes with an unsaturated coordination sphere. These special anions are essential components

neg: Dioxosuccinic acid molecules of water to produce dihydroxytartaric acid, CHO or HO−(C=O)−(C(OH))−(C=O)−OH. Indeed, the product traded under the name "dioxosuccinic acid hydrate" appears to be that substance. On the other hand, dihydroxytartaric acid behaves like dioxosuccinic acid in some reactions; for example, it reacts with ethanol in the presence of hydrogen chloride to yield the ester diethyl dioxosuccinate. Dioxosuccinic acid Dioxosuccinic acid or dioxobutanedioic acid is an organic compound with formula CHO or HO−(C=O)−OH. Removal of two protons from the molecule would yield the dioxosuccinate anion, or O−(C=O)−O. This is one of the oxocarbon anions, which consist solely of carbon and oxygen.

neg: Palmitic acid Palmitic acid Palmitic acid, or hexadecanoic acid in IUPAC nomenclature, is the most common saturated fatty acid found in animals, plants and microorganisms. Its chemical formula is CH(CH)COOH, and its C:D is 16:0. As its name indicates, it is a major component of the oil from the fruit of oil palms (palm oil). Palmitic acid can also be found in meats, cheeses, butter, and dairy products. Palmitates are the salts and esters of palmitic acid. The palmitate anion is the observed form of palmitic acid at physiologic pH (7.4). Aluminium salts of palmitic acid and naphthenic acid were combined during

neg: Antimony pentafluoride [SbF] is a weakly coordinating anion akin to PF. Although it is only weakly basic, [SbF] does react with additional SbF to give a centrosymmetric adduct: SbF reacts violently with many compounds, often releasing dangerous hydrogen fluoride. It is corrosive to the skin and eyes. Antimony pentafluoride Antimony pentafluoride is the inorganic compound with the formula SbF. This colourless, viscous liquid is a valuable Lewis acid and a component of the superacid fluoroantimonic acid, the strongest known acid. It is notable for its Lewis acidity and its ability to react with almost all known compounds. Antimony pentafluoride is prepared by

neg: Polyatomic ion hydrogen sulfate anion (). The removal of another hydrogen ion yields the sulfate anion (). There are two "rules" that can be used for learning the nomenclature of polyatomic anions. First, when the prefix "bi" is added to a name, a hydrogen is added to the ion's formula and its charge is increased by 1, the latter being a consequence of the hydrogen ion's +1 charge. An alternative to the "bi-" prefix is to use the word hydrogen in its place: the anion derived from + , , can be called either bicarbonate or hydrogen carbonate. Note that many of

neg: Carbenium ion fact complicates synthetic pathways to many compounds. For example, when 3-pentanol is heated with aqueous HCl, the initially formed 3-pentyl carbocation rearranges to a statistical mixture of the 3-pentyl and 2-pentyl. These cations react with chloride ion to produce about 3-chloropentane and 2-chloropentane. Carbenium ions can be prepared directly from alkanes by removing a hydride anion, , with a strong acid. For example, magic acid, a mixture of antimony pentafluoride () and fluorosulfuric acid (), turns isobutane into the cation . The tropylium ion is an aromatic species with the formula . Its name derives from the molecule tropine (itself

neg: Tellurate Tellurate In chemistry tellurate is a compound containing an oxyanion of tellurium where tellurium has an oxidation number of +6. In the naming of inorganic compounds it is a suffix that indicates a polyatomic anion with a central tellurium atom. Historically the name tellurate was only applied to oxyanions of tellurium with oxidation number +6, formally derived from telluric acid Te(OH), and the name tellurite referred to oxyanions of tellurium with oxidation number +4, formally derived from tellurous acid (HO)TeO and these names are in common use. However tellurate and tellurite are often referred to as tellurate(VI) and tellurate(IV) respectively

neg: Succinic acid Succinic acid Succinic acid () is a dicarboxylic acid with the chemical formula (CH)(COH). The name derives from Latin "succinum", meaning amber. In living organisms, succinic acid takes the form of an anion, succinate, which has multiple biological roles as a metabolic intermediate being converted into fumarate by the enzyme succinate dehydrogenase in complex 2 of the electron transport chain which is involved in making ATP, and as a signaling molecule reflecting the cellular metabolic state. It is marketed as food additive E363. Succinate is generated in mitochondria via the tricarboxylic acid cycle (TCA), an energy-yielding process shared by all

neg: 1,2-Bis(dicyanomethylene)squarate 1,2-Bis(dicyanomethylene)squarate 1,2-Bis(dicyanomethylene)squarate is a divalent anion with chemical formula or ((N≡C−)C=)(CO). It is one of the pseudo-oxocarbon anions, as it can be described as a derivative of the squarate oxocarbon anion through the replacement of two adjacent oxygen atoms by dicyanomethylene groups =C(−C≡N). The anion can be obtained by reacting squaric acid with "n"-butanol to obtain the diester 1,2-dibutyl squarate (an oily orange liquid) and treating the latter with metallic sodium and malononitrile (N≡C−)CH to give the trihydrated disodium salt 2Na··3HO, a yellow water-soluble solid. The hydrated salt loses the water below 100 °C, but the resulting anhydrous salt is

neg: 1,3-Bis(dicyanomethylene)squarate 1,3-Bis(dicyanomethylene)squarate 1,3-Bis(dicyanomethylene)squarate is a divalent anion with chemical formula or ((N≡C−)C=)(CO). It is one of the pseudo-oxocarbon anions, as it can be described as a derivative of the squarate oxocarbon anion through the replacement of two opposite oxygen atoms by dicyanomethylene groups =C(−C≡N). The anion can be obtained by reacting squaric acid with aniline to form the diester 1,3-dianiline squarate (a yellow solid), before treating the diester with malononitrile (N≡C−)CH and sodium ethoxide to give the disodium tetrahydrate salt 2Na··4HO, an orange water-soluble solid. The hydrated salt loses the water below 100 °C, but the resulting anhydrous salt is stable

neg: Palmitic acid removal of milk fat. Palmitate is attached to the alcohol form of vitamin A, retinol, to make vitamin A stable in milk. Palmitic acid Palmitic acid, or hexadecanoic acid in IUPAC nomenclature, is the most common saturated fatty acid found in animals, plants and microorganisms. Its chemical formula is CH(CH)COOH, and its C:D is 16:0. As its name indicates, it is a major component of the oil from the fruit of oil palms (palm oil). Palmitic acid can also be found in meats, cheeses, butter, and dairy products. Palmitates are the salts and esters of palmitic acid. The palmitate anion

neg: Mesoxalic acid Mesoxalic acid Mesoxalic acid, also called oxomalonic acid or ketomalonic acid, is an organic compound with formula CHO or HO-(C=O)-OH. Mesoxalic acid is both a dicarboxylic acid and a ketonic acid. It readily loses two protons to yield the divalent anion CO, called mesoxalate, oxomalonate, or ketomalonate. These terms are also used for salts containing this anion, such as sodium mesoxalate, NaCO; and for esters containing the -CO- or -O-(C=O)-O- moiety, such as diethyl mesoxalate, (CH)CO. Mesoxalate is one of the oxocarbon anions, which (like carbonate CO and oxalate CO) consist solely of carbon and oxygen. Mesoxalic acid readily absorbs

neg: Mesoxalic acid oxidation of glycerol with the help of Bi(NO). Mesoxalic acid Mesoxalic acid, also called oxomalonic acid or ketomalonic acid, is an organic compound with formula CHO or HO-(C=O)-OH. Mesoxalic acid is both a dicarboxylic acid and a ketonic acid. It readily loses two protons to yield the divalent anion CO, called mesoxalate, oxomalonate, or ketomalonate. These terms are also used for salts containing this anion, such as sodium mesoxalate, NaCO; and for esters containing the -CO- or -O-(C=O)-O- moiety, such as diethyl mesoxalate, (CH)CO. Mesoxalate is one of the oxocarbon anions, which (like carbonate CO and oxalate CO) consist solely

neg: Succinic acid injury. As of 2016 the inhibition of succinate-mediated ROS production was under investigation as a therapeutic drug target. Succinic acid Succinic acid () is a dicarboxylic acid with the chemical formula (CH)(COH). The name derives from Latin "succinum", meaning amber. In living organisms, succinic acid takes the form of an anion, succinate, which has multiple biological roles as a metabolic intermediate being converted into fumarate by the enzyme succinate dehydrogenase in complex 2 of the electron transport chain which is involved in making ATP, and as a signaling molecule reflecting the cellular metabolic state. It is marketed as food additive

neg: Hypophosphorous acid Hypophosphorous acid Hypophosphorous acid is a phosphorus oxyacid and a powerful reducing agent with molecular formula HPO. Inorganic chemists refer to the free acid by this name (also as "HPA"), or the acceptable name of phosphinic acid. It is a colorless high-melting compound, which is soluble in water, dioxane, and alcohols. The formula for blue acid is generally written HPO, but a more descriptive presentation is HOP(O)H which highlights its monoprotic character. Salts derived from this acid are called phosphinates (hypophosphites). HOP(O)H exists in equilibrium with the minor tautomer HP(OH). Sometimes the minor tautomer is called hypophosphorous acid and the

neg: Xenic acid chemistry. Salts of xenic acid are called "xenates", containing the anion. They tend to disproportionate into xenon gas and perxenates: The energy given off is sufficient to form ozone from diatomic oxygen: Salts containing the completely deprotonated anion are presently unknown. Xenic acid Xenic acid is a noble gas compound formed by the dissolution of xenon trioxide in water. Its chemical formula is HXeO. It is a very powerful oxidizing agent, and its decomposition is dangerous as it liberates a large amount of gaseous products: xenon, oxygen, and ozone. However, this feature is also what makes xenic acid practically useful

neg: Sulfate for hydrogen sulfate is 14996-02-2. Sulfate The sulfate or sulphate (see spelling differences) ion is a polyatomic anion with the empirical formula . Sulfate is the spelling recommended by IUPAC, but sulphate is used in British English. Salts, acid derivatives, and peroxides of sulfate are widely used in industry. Sulfates occur widely in everyday life. Sulfates are salts of sulfuric acid and many are prepared from that acid. The sulfate anion consists of a central sulfur atom surrounded by four equivalent oxygen atoms in a tetrahedral arrangement. The symmetry is the same as that of methane. The sulfur atom is

neg: Methanetetracarboxylate pH 10 and about 60 °C, in the presence of palladium as a catalyst. The tetraethyl ester C(COO-CH) is traded as a specialty chemical and has been used in organic synthesis. The anion can be seen as the result of removing four protons from methanetetracarboxylic acid, a hypothetical organic compound with formula CHO or C(COOH). However this acid has not been synthesised (as of 2009), and is believed to be unstable. Methanetetracarboxylate In chemistry, methanetetracarboxylate is a tetravalent anion with formula or C(COO). It has four carboxylate groups attached to a central carbon atom; so it has the same carbon

neg: High anion gap metabolic acidosis be high if it is over 12 mEq/L. High anion gap metabolic acidosis is typically caused by acid produced by the body. More rarely, it may be caused by ingesting methanol or overdosing on aspirin. The Delta Ratio is a formula that can be used to assess elevated anion gap metabolic acidosis and to evaluate whether mixed acid base disorder (metabolic acidosis) is present. The list of agents that cause high anion gap metabolic acidosis is similar to but broader than the list of agents that cause a serum osmolal gap. The most common causes of high anion gap metabolic

neg: Ester are the hydrocarbon parts of the carboxylic acid and the alcohol, respectively. For example, butyl acetate (systematically butyl ethanoate), derived from butanol and acetic acid (systematically ethanoic acid) would be written CHCOCH. Alternative presentations are common including BuOAc and CHCOOCH. Cyclic esters are called lactones, regardless of whether they are derived from an organic or an inorganic acid. One example of a (organic) lactone is γ-valerolactone. An uncommon class of organic esters are the orthoesters, which have the formula RC(OR′). Triethylorthoformate (HC(OCH)) is derived, in terms of its name (but not its synthesis) from orthoformic acid (HC(OH)) and ethanol. Esters

neg: Perrhenate Perrhenate The perrhenate ion is the anion with the formula , or a compound containing this ion. The perrhenate anion is tetrahedral, being similar in size and shape to perchlorate and the valence isoelectronic permanganate. The perrhenate anion is stable over a broad pH range and can be precipitated from solutions with the use of organic cations. At normal pH, perrhenate exists as metaperrhenate (), but at high pH mesoperrhenate () forms. Perrhenate, like its conjugate acid perrhenic acid, features rhenium in the oxidation state of +7 with a d configuration. Solid perrhenate salts takes on the color of the

neg: Dithionate electron in the radical can be detected with electron paramagnetic resonance and barium dithionate has been proposed as the basis for a radiation dosimeter. The dithionate ion can act as a bidentate ligand. The structure of the dithionate ion in the solid state is staggered in NaSO·2HO, whereas in the anhydrous potassium salt it is nearly eclipsed. Compounds containing the dithionate ion include: Dithionate The dithionate (or metabisulfate) anion, , is a sulfur oxoanion derived from dithionic acid, HSO. Its chemical formula is sometimes written in a semistructural format, as [OSSO]. The sulfur atoms of the dithionate ion are in

neg: Delta ratio Delta ratio Delta ratio is a formula that can be used to assess elevated anion gap metabolic acidosis and to evaluate whether a mixed acid base disorder (metabolic acidosis) is present. The anion gap (AG) is calculated first and if an anion gap is present, results in either a high anion gap metabolic acidosis (HAGMA) or a normal anion gap acidosis (NAGMA). A low anion gap is usually an oddity of measurement, rather than a clinical concern. The equation for calculating the Delta Ratio is:formula_1 and reflects either an increase in the anion gap or a decrease in the bicarbonate

neg: Delta ratio - base metabolic acidosis. Delta ratio Delta ratio is a formula that can be used to assess elevated anion gap metabolic acidosis and to evaluate whether a mixed acid base disorder (metabolic acidosis) is present. The anion gap (AG) is calculated first and if an anion gap is present, results in either a high anion gap metabolic acidosis (HAGMA) or a normal anion gap acidosis (NAGMA). A low anion gap is usually an oddity of measurement, rather than a clinical concern. The equation for calculating the Delta Ratio is:formula_1 and reflects either an increase in the anion gap or a

neg: Hyponitrous acid Hyponitrous acid Hyponitrous acid is a chemical compound with formula or HON=NOH. It is an isomer of nitramide, HN−NO. Hyponitrous acid forms two series of salts, the hyponitrites containing the [ON=NO] anion, and the "acid hyponitrites" containing the [HON=NO] anion. There are two possible structures of hyponitrous acid, "trans" and "cis". "Trans"-hyponitrous acid forms white crystals that are explosive when dry. In aqueous solution, it is a weak acid (p"K" = 7.21, p"K" = 11.54), and decomposes to nitrous oxide and water with a half life of 16 days at 25 °C at pH 1–3: Since this reaction is not

neg: Borinic acid some bacterial enzymes such as menaquinone methyltransferase and CcrM. This may result in development of treatments for topical application on skin. Borinic acid Borinic acid , also known as boronous acid, is an oxyacid of boron with formula . Borinate is the associated anion of boron with formula , however being a lewis acid the form in basic solution is . Borinic acid can be formed as the first step in the hydrolysis of diborane. BH+HO → HBOH + H Borinic acid itself is unstable and only lasts for a few seconds during the hydrolysis reaction. However, by using microwave

neg: Acetylenedicarboxylic acid Acetylenedicarboxylic acid Acetylenedicarboxylic acid or butynedioic acid is an organic compound (a dicarboxylic acid) with the formula CHO or <chem>HO2C-C#C-CO2H</chem>. It is a crystalline solid that is soluble in diethyl ether. The removal of two protons yields the acetylenedicarboxylate dianion CO, which consists only of carbon and oxygen, making it an oxocarbon anion. Partial ionization yields the monovalent hydrogenacetylenedicarboxylate anion HCO. The acid was first described in 1877 by Polish chemist Ernest Bandrowski. It can be obtained by treating α,β-dibromosuccinic acid with potassium hydroxide KOH in methanol or ethanol. The reaction yields potassium bromide and potassium acetylenedicarboxylate. The salts are

neg: Triflidic acid TfCH + MgBrHSOIn its anionic form, the lanthanide salts of triflidic acid ("triflides") have been shown to be more efficient Lewis acids than the corresponding triflates. The triflide anion has also been employed as the anionic component of ionic liquids. Triflidic acid Triflidic acid ("IUPAC name": tris[(trifluoromethyl)sulfonyl]methane, "abbreviated formula": TfCH) is an organic superacid. It is one of the strongest known carbon acids and is among the strongest Brønsted acids in general, with an acidity exceeded only by the carborane acids. Notably, triflidic acid is estimated to have an acidity 10 times that of triflic acid (p"K" ~ –14), as

neg: Dihydrogen complex agostic interaction that is displaced by the H. In other cases, H will displace anionic ligands, sometimes even halides. Treatment of chlorobis(dppe)iron hydride with sodium tetrafluorborate under and atmostphere of hydrogen is one example: Many metal hydrides can be protonated to give dihydrogen complexes: In such cases the acid usually is derived from a weakly coordinating anion, e.g., Brookhart's acid. In 1984, Kubas et al. discovered that the addition of H to the purple-colored species M(CO)(PR) gave a yellow precipitate of mer-trans-M(CO)(PR)(H) (M = Mo or W; R = cyclohexyl, iso-propyl). This result rapidly led to the discovery of a

neg: Benzyl cyanide Benzyl cyanide Benzyl cyanide (abbreviated BnCN) is an organic compound with the chemical formula CHCHCN. This colorless oily aromatic liquid is an important precursor to numerous compounds in organic chemistry. Benzyl cyanide can be produced via Kolbe nitrile synthesis between benzyl chloride and sodium cyanide and by oxidative decarboxylation of phenylalanine. Benzyl cyanide can be hydrolyzed to give phenylacetic acid or used in the Pinner reaction to yield phenylacetic acid esters. The compound also forms an "active methylene unit" on the carbon between the aromatic ring and the nitrile functional group. This active carbon, referred to as a nitrile anion,

neg: Sulfate Sulfate The sulfate or sulphate (see spelling differences) ion is a polyatomic anion with the empirical formula . Sulfate is the spelling recommended by IUPAC, but sulphate is used in British English. Salts, acid derivatives, and peroxides of sulfate are widely used in industry. Sulfates occur widely in everyday life. Sulfates are salts of sulfuric acid and many are prepared from that acid. The sulfate anion consists of a central sulfur atom surrounded by four equivalent oxygen atoms in a tetrahedral arrangement. The symmetry is the same as that of methane. The sulfur atom is in the +6 oxidation state

neg: Ammonium bifluoride Ammonium bifluoride Ammonium hydrogen fluoride is the inorganic compound with the formula NHHF or NHF·HF. It is produced from ammonia and hydrogen fluoride. This colourless salt is a glass-etchant and an intermediate in a once-contemplated route to hydrofluoric acid. Ammonium bifluoride, as its name indicates, contains an ammonium cation (NH) and a bifluoride, or hydrogen(difluoride), anion (HF). The centrosymmetric triatomic bifluoride anion features the strongest known hydrogen bond, with a F−H length of 114 pm. and a bond energy greater than 155 kJ mol. In solid [NH][HF], each ammonium cation is surrounded by four fluoride centers in a tetrahedron, with

neg: Borinic acid Borinic acid Borinic acid , also known as boronous acid, is an oxyacid of boron with formula . Borinate is the associated anion of boron with formula , however being a lewis acid the form in basic solution is . Borinic acid can be formed as the first step in the hydrolysis of diborane. BH+HO → HBOH + H Borinic acid itself is unstable and only lasts for a few seconds during the hydrolysis reaction. However, by using microwave spectroscopy various properties can be determined. The B-O distance is 1.352 Å, O-H distance 0.96 Å, B-H length is probably 1.2

neg: Hexanoic acid Hexanoic acid Hexanoic acid, also known as caproic acid, is the carboxylic acid derived from hexane with the chemical formula . It is a colorless oily liquid with an odor that is fatty, cheesy, waxy, and like that of goats or other barnyard animals. It is a fatty acid found naturally in various animal fats and oils, and is one of the chemicals that give the decomposing fleshy seed coat of the ginkgo its characteristic unpleasant odor. It is also one of the components of vanilla. The primary use of hexanoic acid is in the manufacture of its esters for

neg: 1,3-Bis(dicyanomethylene)squarate up to 400 °C. Reaction of the sodium salt with salts of other cations in ethanol affords the following salts: Nuclear magnetic resonance shows that the aromatic character of the squarate core is retained. 1,3-Bis(dicyanomethylene)squarate 1,3-Bis(dicyanomethylene)squarate is a divalent anion with chemical formula or ((N≡C−)C=)(CO). It is one of the pseudo-oxocarbon anions, as it can be described as a derivative of the squarate oxocarbon anion through the replacement of two opposite oxygen atoms by dicyanomethylene groups =C(−C≡N). The anion can be obtained by reacting squaric acid with aniline to form the diester 1,3-dianiline squarate (a yellow solid), before treating the

neg: 1,2-Bis(dicyanomethylene)squarate stable up to 400 °C. Reaction of the sodium salt with the chlorides of other cations in ethanol affords the following salts: Nuclear magnetic resonance shows that the aromatic character of the squarate core is retained. 1,2-Bis(dicyanomethylene)squarate 1,2-Bis(dicyanomethylene)squarate is a divalent anion with chemical formula or ((N≡C−)C=)(CO). It is one of the pseudo-oxocarbon anions, as it can be described as a derivative of the squarate oxocarbon anion through the replacement of two adjacent oxygen atoms by dicyanomethylene groups =C(−C≡N). The anion can be obtained by reacting squaric acid with "n"-butanol to obtain the diester 1,2-dibutyl squarate (an oily orange liquid)

neg: Dithionate Dithionate The dithionate (or metabisulfate) anion, , is a sulfur oxoanion derived from dithionic acid, HSO. Its chemical formula is sometimes written in a semistructural format, as [OSSO]. The sulfur atoms of the dithionate ion are in the +5 oxidation state due to the presence of the S–S bond. Generally dithionates form stable compounds that are not readily oxidised or reduced. Strong oxidants oxidise them to sulfates and strong reducing agents reduce them to sulfites and dithionites. Aqueous solutions of dithionates are quite stable and can be boiled without decomposition. The γ-irradiation of crystalline dithionates produces radical ions. The unpaired

neg: Hexamethylbenzene due to π-stacking of the aromatic systems. It is insoluble in water, but soluble in organic solvents including benzene and ethanol. Hexamethylbenzene is sometimes called mellitene, a name derived from mellite, a rare honey-coloured mineral; "meli" ( "melitos") is the Greek word for honey. Mellite is composed of a hydrated aluminium salt of benzenehexacarboxylic acid (mellitic acid), with formula . Mellitic acid itself can be derived from the mineral, and subsequent reduction yields mellitene. Conversely, mellitene can be oxidised to form mellitic acid: In 1927 Kathleen Lonsdale determined the solid structure of hexamethylbenzene from crystals provided by Christopher Kelk Ingold.

neg: Pangamic acid those claimed by the Krebses to be pangamic acid, has been scientifically verified to have the characteristics that defined the original description of the compound. The Krebses derived the term "pangamic" to describe this compound which they asserted to be ubiquitous and highly concentrated in seeds ("pan" meaning "universal" and "gamic" meaning "seed"). Pangamic acid is the name given to the chemical compound with the empirical formula CHON and a molecular weight of 281 which appeared to be an ester derived from -gluconic acid and dimethylglycine. In 1943, the Krebses applied for a patent for a process for extracting this

neg: Hydrochloride Hydrochloride In chemistry, a hydrochloride is an acid salt resulting, or regarded as resulting, from the reaction of hydrochloric acid with an organic base (e.g. an amine). An alternative name is chlorhydrate, which comes from French. An archaic alternative name is muriate, derived from hydrochloric acid's ancient name: muriatic acid. For example, reacting pyridine (CHN) with hydrochloric acid (HCl) yields its hydrochloride salt, pyridinium chloride. The molecular formula is either written as CHN·HCl or as CHNH Cl. Converting insoluble amines into hydrochlorides is a common way to make them water-soluble. This characteristic is particularly desirable for substances used in medications.

neg: Greenschist or picrite). The green is due to abundant green chlorite, actinolite and epidote minerals that dominate the rock. However, basalts may remain quite black if primary pyroxene does not revert to chlorite or actinolite. To qualify for the name a rock must also exhibit schistosity or some foliation or layering. The rock is derived from basalt, gabbro or similar rocks containing sodium-rich plagioclase feldspar, chlorite, epidote and quartz. Greenschist, as a rock type, is defined by the presence of the minerals chlorite and actinolite and may contain albite or epidote. Greenschist often has a lepidoblastic, nematoblastic or schistose texture defined

neg: Dicalcium phosphate Dicalcium phosphate Dicalcium phosphate is the calcium phosphate with the formula CaHPO and its dihydrate. The "di" prefix in the common name arises because the formation of the HPO anion involves the removal of two protons from phosphoric acid, HPO. It is also known as dibasic calcium phosphate or calcium monohydrogen phosphate. Dicalcium phosphate is used as a food additive, it is found in some toothpastes as a polishing agent and is a biomaterial. Dibasic calcium phosphate is produced by the neutralization of calcium hydroxide with phosphoric acid, which precipitates the dihydrate as a solid. At 60 °C the anhydrous

neg: Carbamic acid while others are used as insecticides, for example aldicarb. Carbamic acid Carbamic acid is the compound with the formula HNCOOH. The attachment of the acid group to a nitrogen or amine (instead of carbon) distinguishes it from carboxylic acid and an amide. Many derivatives and analogues of carbamic acid are known. They are generally unstable, reverting to the parent amine and carbon dioxide. The deprotonated anion (or conjugate base) of this functional group is a carbamate. Carbamic acid is a planar molecule. Carbamic acid is an intermediate in the production of urea, which involves the reaction of carbon dioxide and

neg: Bicarbonate on as a trivial name. The bicarbonate ion (hydrogencarbonate ion) is an anion with the empirical formula and a molecular mass of 61.01 daltons; it consists of one central carbon atom surrounded by three oxygen atoms in a trigonal planar arrangement, with a hydrogen atom attached to one of the oxygens. It is isoelectronic with nitric acid . The bicarbonate ion carries a negative one formal charge and is an amphiprotic species which has both acidic and basic properties. It is both the conjugate base of carbonic acid ; and the conjugate acid of , the carbonate ion, as shown

neg: Hypophosphoric acid p"K" = 2.2, p"K" = 2.8, p"K" = 7.3 and p"K" = 10.0. On standing the anydrous acid undergoes rearrangement and disproportionation to form a mixture of isohypophosphoric acid, HPO(OH)-O-PO(OH); pyrophosphoric acid HPO and pyrophosphorous acid. Hypophosphoric acid is unstable in hot hydrochloric acid, in 4 M HCl it hydrolyses to give HPO + HPO. Hypophosphorus acid contains oxonium ions and is best formulated [HO] [HPO]. The acid is isostructural with the diammonium salt which contains the [HOPOPOOH] anion with a P−P bond length of 219 pm. The HOPOPOOH anion in NaHPO·6HO has a symmetric,staggered ethane-like structure with a P−P

neg: Strecker amino acid synthesis reaction product was chiral alanine. The first asymmetric synthesis via a chiral catalyst was reported in 1996. Catalytic asymmetric Strecker reaction can be effected using thiourea-derived catalyst. In 2012, a BINOL-derived catalyst was employed to generate chiral cyanide anion. Strecker amino acid synthesis The Strecker amino acid synthesis, also known simply as the Strecker synthesis, was discovered by German chemist Adolph Strecker, and is a term used for a series of chemical reactions that synthesize an amino acid from an aldehyde or ketone. The aldehyde is condensed with ammonium chloride in the presence of potassium cyanide to form an α-aminonitrile,

neg: Phosphite anion Phosphite anion A phosphite anion or phosphite in inorganic chemistry usually refers to [HPO] but includes [HPO] ([HPO(OH)]). These anions are the conjugate bases of phosphorous acid (HPO). The corresponding salts, e.g. sodium phosphite (NaHPO) are reducing in character. The IUPAC recommended name for phosphorous acid is phosphonic acid. Correspondingly, the IUPAC-recommended name for the ion is phosphonate. In the US the IUPAC naming conventions for inorganic compounds are taught at high school, but not as a 'required' part of the curriculum. A well-known university-level textbook follows the IUPAC recommendations. In practice any reference to "phosphite" should be investigated to

neg: 2-Iodobenzoic acid is ejected, yielding a carbocation which is then attacked by highly nucleophilic I anion. The nitrous acid is usually generated "in situ" from sodium nitrite. 2-Iodobenzoic acid 2-Iodobenzoic acid, or "o"-iodobenzoic acid, is an organic compound with the formula ICHCOOH. The synthesis of 2-iodobenzoic acid "via" the diazotization of anthranilic acid is commonly performed in university organic chemistry labs. One of its most common uses is as a precursor for the preparation of IBX and Dess–Martin periodinane, both used as mild oxidants. 2-Iodobenzoic acid can be synthesized "via" a Sandmeyer reaction consisting of the diazotization of anthranilic acid followed by

neg: Thiophosphate monothiophosphate" refers to esters such as (CHO)POS. Dithiophosphate has the formula [POS], which has C symmetry. Sodium dithiophosphate, which is colorless, is the major product from the reaction of phosphorus pentasulfide with NaOH: Dithiophosphoric acid is obtained by treatment of barium dithiophosphate with sulfuric acid: Both NaPOS and especially HPOS are prone toward hydrolysis to their monothio derivatives. Trithiophosphate is the anion [POS], which has C symmetry. Tetrathiophosphate is the anion [PS], which has T symmetry. There are a number of these anions known. There has been interest in compounds containing these anions due to their potential application as fast

neg: Hexafluorophosphate Hexafluorophosphate Hexafluorophosphate is an anion with chemical formula of . It is an octahedral species. It imparts no color to its salts. is isoelectronic with sulfur hexafluoride, SF, and the hexafluorosilicate dianion, , and fluoroantimonate . Being poorly nucleophilic, hexafluorophosphate is classified as a non-coordinating anion. Hexafluorophosphate salts can be prepared by the reaction of phosphorus pentachloride and alkali or ammonium halide in a solution of hydrofluoric acid: Hexafluorophosphoric acid can be prepared by direct reaction of hydrogen fluoride with phosphorus pentafluoride. It is a strong Brønsted acid that is typically generated "in situ" immediately prior to its use. These

neg: Furantetracarboxylic acid Furantetracarboxylic acid In chemistry, furantetracarboxylic acid is an organic compound with formula , or (CO)(-(CO)OH), which can be viewed as deriving from furan through replacement of the four hydrogen atoms by carboxyl functional groups -(CO)OH. By removal of four protons, the acid is expected to yield the anion , furantetracarboxylate, which is one of the oxocarbon anions (consisting solely of oxygen and carbon. By loss of 1 through 3 protons it forms the anions , , and , called respectively trihydrogen-, dihydrogen-, and hydrogenfurantetracarboxylate. The same names are used for the corresponding esters. The acid can be obtained by from

neg: Triflate Triflate Triflate, also known by the systematic name trifluoromethanesulfonate, is a functional group with the formula CFSO−. The triflate group is often represented by −OTf, as opposed to −Tf (triflyl). For example, "n"-butyl triflate can be written as CHCHCHCHOTf. The corresponding triflate anion, , is an extremely stable polyatomic ion, being the conjugate base of triflic acid (CFSOH), one of the strongest acids known. It is defined as a superacid, because it is more acidic than pure sulfuric acid. A triflate group is an excellent leaving group used in certain organic reactions such as nucleophilic substitution, Suzuki couplings and Heck

neg: Ethylenetetracarboxylic acid exotic oxocarbon synthesized by pyrolysis of ethylenetetracarboxilic acid in 1981 by Patterson and others. Ethylenetetracarboxylic acid Ethylenetetracarboxylic acid is an organic compound with formula , or (HO(OC)-)C=C(-(CO)OH). By removal of four protons, the acid yields the anion , ethylenetetracarboxylate, which is one of the oxocarbon anions (consisting solely of oxygen and carbon. By loss of 1 through 3 protons it forms the anions , , and , called respectively trihydrogen-, dihydrogen-, and hydrogenethylenetetracarboxylate. The same names are used for the corresponding esters. The acid can be obtained by hydrolysis of tetraethyl ethylenetetracarboxylate, which in turn can be obtained from diethyl

neg: Shiina macrolactonization reaction of carboxyl group in the seco acid with the activated acyl carboxylate produces the corresponding MA, in the same manner as in the acidic reaction. Then, the nucleophilic catalyst acts selectively on a carbonyl group derived from the seco acid in MA to again produce activated acyl carboxylate. The hydroxyl group in the seco acid attacks its host molecule through intramolecular nucleophilic substitution, and at the same time, carboxylate anion, derived from 2-methyl-6-nitrobenzoic acid, acts as a deprotonation agent, promoting the progression of the cyclization and producing the desired lactone. To balance the reaction, each MNBA accepts the atoms

neg: Teflic acid Teflic acid Teflic acid is the chemical compound with the formula HOTeF. This strong acid is related to orthotelluric acid, Te(OH). Teflic acid has a slightly distorted octahedral geometry. Teflic acid was accidentally discovered by Engelbrecht and Sladky. Their synthesis did not yield the anticipated telluryl fluoride TeOF, but a mixture of volatile telluric compounds, "i.a." HOTeF: Teflic acid can also be prepared from fluorosulfonic acid and barium tellurate: It is also the first hydrolysis product of tellurium hexafluoride: The conjugate base of teflic acid is called the teflate anion, FTeO (not to be confused with triflate). Many teflates are

neg: Ethylenetetracarboxylic acid Ethylenetetracarboxylic acid Ethylenetetracarboxylic acid is an organic compound with formula , or (HO(OC)-)C=C(-(CO)OH). By removal of four protons, the acid yields the anion , ethylenetetracarboxylate, which is one of the oxocarbon anions (consisting solely of oxygen and carbon. By loss of 1 through 3 protons it forms the anions , , and , called respectively trihydrogen-, dihydrogen-, and hydrogenethylenetetracarboxylate. The same names are used for the corresponding esters. The acid can be obtained by hydrolysis of tetraethyl ethylenetetracarboxylate, which in turn can be obtained from diethyl dibromomalonate with sodium iodide. Ethylenetetracarboxylic dianhydride, a twofold anhydride of this compound, is an

neg: Carbamic acid Carbamic acid Carbamic acid is the compound with the formula HNCOOH. The attachment of the acid group to a nitrogen or amine (instead of carbon) distinguishes it from carboxylic acid and an amide. Many derivatives and analogues of carbamic acid are known. They are generally unstable, reverting to the parent amine and carbon dioxide. The deprotonated anion (or conjugate base) of this functional group is a carbamate. Carbamic acid is a planar molecule. Carbamic acid is an intermediate in the production of urea, which involves the reaction of carbon dioxide and ammonia. Carbamoyltransferases are transferase enzymes classified under EC number

neg: Propionic acid Propionic acid Propionic acid (from the Greek words "protos", meaning "first", and "pion", meaning "fat"; also known as propanoic acid) is a naturally occurring carboxylic acid with chemical formula CHCHCOH. It is a liquid with a pungent and unpleasant smell somewhat resembling body odor. The anion CHCHCO as well as the salts and esters of propionic acid are known as propionates or propanoates. Propionic acid was first described in 1844 by Johann Gottlieb, who found it among the degradation products of sugar. Over the next few years, other chemists produced propionic acid in various other ways, none of them realizing

neg: Levulinic acid 1850 mg/kg. Levulinic acid Levulinic acid, or 4-oxopentanoic acid, is an organic compound with the formula CHC(O)CHCHCOH. It is classified as a keto acid. This white crystalline solid is soluble in water and polar organic solvents. It is derived from degradation of cellulose and is a potential precursor to biofuels, such as ethyl levulinate. In 1840 the Dutch professor Gerardus Johannes Mulder mentioned levulinic acid for the first time. He synthesized it by heating fructose with hydrochloric acid. The former term “levulose” for fructose gave levulinic acid its name. Although levulinic acid has been well known since the 1870s, it

neg: Levulinic acid Levulinic acid Levulinic acid, or 4-oxopentanoic acid, is an organic compound with the formula CHC(O)CHCHCOH. It is classified as a keto acid. This white crystalline solid is soluble in water and polar organic solvents. It is derived from degradation of cellulose and is a potential precursor to biofuels, such as ethyl levulinate. In 1840 the Dutch professor Gerardus Johannes Mulder mentioned levulinic acid for the first time. He synthesized it by heating fructose with hydrochloric acid. The former term “levulose” for fructose gave levulinic acid its name. Although levulinic acid has been well known since the 1870s, it has never

neg: Carborane acid The carboranate anion distributes its charge by delocalizing the electrons throughout the 12 cage atoms. This was shown in a single crystal X-ray diffraction study revealing shortened bond lengths in the heterocyclic portion of the ring suggesting electronic delocalization. The chlorinated carba-"closo"-dodecaborate anion is an outstandingly stable anion with what has previously been described as “substitutionally inert” B–Cl vertices. The descriptor "closo" indicates that the molecule is formally derived (by B-to-C replacement) from a borane of stoichiometry and charge [BH""] ("n =" 12 for known carborane acids). The cagelike structure formed by the 11 boron atoms and 1 carbon atom

neg: Thioacetic acid boiling point (93 °C) and melting points are 20 and 75K lower than those for acetic acid. With a pK near 3.4, thioacetic acid is about 15x more acidic than acetic acid. The conjugate base is thioacetate: In neutral water, thioacetic acid is fully ionized. Most of the reactivity of thioacetic acid arises from the conjugate base, thioacetate. Salts of this anion, e.g. potassium thioacetate, are used to generate thioacetate esters. Thioacetate esters undergo hydrolysis to give thiols. A typical method for preparing a thiol from an alkyl halide using thioacetic acid proceeds in four discrete steps, some of which

neg: Debromoaplysiatoxin epoxide by usage of classical synthetical operations, such as introducing acetic acid or substitution reactions with tosylates. Next, a dithiane derived anion interacts to form an alcohol. The following step involves introducing an acidic sidechain on the C.9 hydroxyl group. This carboxylic, acidic side group is made of xylose and arabidose. The introduction is realized by protecting the C.29 and C.30 hydroxylgroups with respectively p-methoxybenzyl (MPM) and benzyloxymethyl (BOM), activating the sidechain with acid chloride, and subsequently replacing the C.30 protecting group with a more stable one, tert-butyldiphenylsilyl (TBDPS). Thereafter, the carboxylic acid can successfully attach to the backbone by

neg: Furantetracarboxylic acid dioxalylsuccinate. The salt rubidium trihydrogenfurantetracarboxylate crystallizes as white needles. Furantetracarboxylic acid In chemistry, furantetracarboxylic acid is an organic compound with formula , or (CO)(-(CO)OH), which can be viewed as deriving from furan through replacement of the four hydrogen atoms by carboxyl functional groups -(CO)OH. By removal of four protons, the acid is expected to yield the anion , furantetracarboxylate, which is one of the oxocarbon anions (consisting solely of oxygen and carbon. By loss of 1 through 3 protons it forms the anions , , and , called respectively trihydrogen-, dihydrogen-, and hydrogenfurantetracarboxylate. The same names are used for the

neg: Benzoquinonetetracarboxylic acid Benzoquinonetetracarboxylic acid In chemistry, 1,4-benzoquinonetetracarboxylic acid is an organic compound with formula , or (CO)(-(CO)OH), which can be viewed as deriving from "para"-benzoquinone through replacement of the four hydrogen atoms by carboxyl functional groups -(CO)OH. By removal of four protons, the acid is expected to yield the anion , benzoquinonetetracarboxylate, which is one of the oxocarbon anions (consisting solely of oxygen and carbon. By loss of 1 through 3 protons it forms the anions , , and , called respectively trihydrogen-, dihydrogen-, and hydrogenbenzoquinonetetracarboxylate. The same names are used for the corresponding esters. Removal of two water molecules gives the

neg: Perrhenate cation. Typical perrhenate salts are the alkali metal derivatives and ammonium perrhenate. These salts are prepared by oxidation of rhenium compounds with nitric acid followed by neutralization of the resulting perrhenic acid. In inorganic chemistry, perrhenate anion is also used as a weakly coordinating anion. It is a weaker base than or but stronger than or . Unlike the related permanganate, perrhenate is nonoxidising. Silver perrhenate reacts with trimethylsilyl chloride to give the silyl "ester" (CH)SiOReO. The perrhenate ion reacts with the cyanide to give "trans"-[ReO(CN)]. With sulfide sources such as hydrogen sulfide, one obtains black ReS and ReS. These

neg: Benzoquinonetetracarboxylic acid compound benzoquinonetetracarboxylic dianhydride, , one of the oxides of carbon. The acid can be obtained by from durene (1,2,4,5-tetramethylbenzene) via dinitropyromellitic and diaminopyromellitic acids. Benzoquinonetetracarboxylic acid In chemistry, 1,4-benzoquinonetetracarboxylic acid is an organic compound with formula , or (CO)(-(CO)OH), which can be viewed as deriving from "para"-benzoquinone through replacement of the four hydrogen atoms by carboxyl functional groups -(CO)OH. By removal of four protons, the acid is expected to yield the anion , benzoquinonetetracarboxylate, which is one of the oxocarbon anions (consisting solely of oxygen and carbon. By loss of 1 through 3 protons it forms the anions , ,

neg: Carbonate and carbonic acid changes constantly to the changing temperature and pressure conditions. In the case of metal ions with insoluble carbonates, e.g. CaCO, formation of insoluble compounds results. This is an explanation for the buildup of scale inside pipes caused by hard water. Systematic additive IUPAC name for carbonate anion is trioxidocarbonate(2−). Similarly, cyanide anion CN is named nitridocarbonate(1−). Following this logic, e.g. carbonate(4−) in the systematic additive nomenclature would mean carbide anion, but it is not the case. In organic chemistry a carbonate can also refer to a functional group within a larger molecule that contains a carbon atom

neg: Shiina esterification produce activated acyl carboxylate. The reaction of carboxyl group in the carboxylic acid with the activated acyl carboxylate produces the corresponding MA, in the same manner as in the acidic reaction. Then, the nucleophilic catalyst acts selectively on a carbonyl group derived from the carboxylic acid in MA to again produce activated acyl carboxylate. The hydroxyl group in alcohol attacks its host molecule through intermolecular nucleophilic substitution, and at the same time, carboxylate anion, derived from 2-methyl-6-nitrobenzoic acid, acts as a deprotonation agent, promoting the progression of the esterification and producing the desired carboxylic ester. To balance the reaction, each