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Disodium hydrogen arsenate is highly toxic. The salt is the conjugate base of arsenic acid. It is a white, water-soluble solid. [1] Being a diprotic acid, its acid-base properties is described by two equilibria: H 2 AsO − 4 + H 2 O ⇌ HAsO 2− 4 + H 3 O + (pK a2 = 6.94) HAsO 2− 4 + H 2 O ⇌ AsO 3− 4 + H 3 O + (pK a3 = 11.5)
It is a diprotic acid, the hydrogenphosphite ion, HP(O) 2 (OH) − is a weak acid: HP(O) 2 (OH) − → HPO 2− 3 + H + pK a = 6.7. The conjugate base HP(O) 2 (OH) − is called hydrogen phosphite, and the second conjugate base, HPO 2− 3, is the phosphite ion. [8] (Note that the IUPAC recommendations are hydrogen phosphonate and phosphonate ...
By definition, an acid is an ion or molecule that can donate a proton, and when introduced to a solution it will react with water molecules (H 2 O) to form a hydronium ion (H 3 O +), a conjugate acid of water. [4] For simplistic reasoning, the hydrogen ion (H +) is often used to abbreviate the hydronium ion.
The systematic IUPAC name is not always the preferred IUPAC name, for example, lactic acid is a common, and also the preferred, name for what systematic rules call 2-hydroxypropanoic acid. This list is ordered by the number of carbon atoms in a carboxylic acid.
Selenous acid is analogous to sulfurous acid, but it is more readily isolated. Selenous acid is easily formed upon the addition of selenium dioxide to water. As a crystalline solid, the compound can be seen as pyramidal molecules that are interconnected with hydrogen bonds. In solution it is a diprotic acid: [3] H 2 SeO 3 ⇌ H + + HSeO − 3 ...
The fluorinated version of malonic acid is difluoromalonic acid. Chemical structure of the malonate dianion. Malonic acid is diprotic; that is, it can donate two protons per molecule. Its first is 2.8 and the second is 5.7. [2] Thus the malonate ion can be H OOCCH 2 COO − or C H 2 (COO) 2− 2.
Squaric acid, also called quadratic acid because its four carbon atoms approximately form a square, is a diprotic organic acid with the chemical formula C 4 O 2 (OH) 2. [4]The conjugate base of squaric acid is the hydrogensquarate anion HC 4 O − 4; and the conjugate base of the hydrogensquarate anion is the divalent squarate anion C 4 O 2− 4.
The acid itself is added to foods as an antioxidant E334 and to impart its distinctive sour taste. Naturally occurring tartaric acid is a useful raw material in organic chemical synthesis. Tartaric acid, an alpha-hydroxy-carboxylic acid, is diprotic and aldaric in acid characteristics and is a dihydroxyl derivative of succinic acid.