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It is a conjugate acid of phosphate [PO 4] 3-and a conjugate base of dihydrogen phosphate [H 2 PO 4] −. It is formed when a pyrophosphate anion [P 2 O 7] 4− reacts with water H 2 O by hydrolysis, which can give hydrogenphosphate: [P 2 O 7] 4− + H 2 O ⇌ 2 [HPO 4] 2−
Acid Conjugate base H 2 F + Fluoronium ion HF Hydrogen fluoride: HCl Hydrochloric acid: Cl − Chloride ion H 2 SO 4 Sulfuric acid: HSO − 4 Hydrogen sulfate ion (bisulfate ion) HNO 3 Nitric acid: NO − 3 Nitrate ion H 3 O + Hydronium ion H 2 O Water: HSO − 4 Hydrogen sulfate ion SO 2− 4 Sulfate ion H 3 PO 4 Phosphoric acid: H 2 PO − 4 ...
Dihydrogen phosphate is an inorganic ion with the formula [H 2 PO 4] −.Phosphates occur widely in natural systems. [1]These sodium phosphates are artificially used in food processing and packaging as emulsifying agents, neutralizing agents, surface-activating agents, and leavening agents providing humans with benefits.
The last one is pyrophosphate [P 2 O 7] 4−. The pyrophosphates are mostly water-soluble. Likewise, tripolyphosphoric acid H 5 P 3 O 10 yields at least five anions [H 5−k P 3 O 10] k−, where k ranges from 1 to 5, including tripolyphosphate [P 3 O 10] 5−. Tetrapolyphosphoric acid H 6 P 4 O 13 yields at least six anions, including ...
4] 2−, is the only species present. At pH 13 or higher, the acid is completely dissociated as the phosphate ion, (PO 4) 3−. This means that salts of the mono- and di-phosphate ions can be selectively crystallised from aqueous solution by setting the pH value to either 4.7 or 9.8. In effect, H 3 PO 4, H 2 (PO 4) − and H(PO 4) 2−
A phosphite anion or phosphite in inorganic chemistry usually refers to [HPO 3] 2− but includes [H 2 PO 3] − ([HPO 2 (OH)] −). These anions are the conjugate bases of phosphorous acid (H 3 PO 3). The corresponding salts, e.g. sodium phosphite (Na 2 HPO 3) are reducing in character.
Monohydrogen phosphate, inorganic ion with the formula [HPO 4] 2− Dihydrogen phosphate , inorganic ion with the formula [H 2 PO 4 ] − Potassium hydrogen phosphate
The second and third pK a 's of phosphoric acid, pK a2 and pK a3, are 7.2 and 12.37, respectively. It follows that HPO 2− 4 and PO 3− 4 are sufficiently basic to serve as ligands. The examples below confirm this expectation. Molecular metal phosphate complexes have no or few applications.