Food acidity regulators

Source: Wikipedia. Pages: 26. Chapters: Acidity regulator, Adipic acid, Ammonium bicarbonate, Ammonium hydroxide, Citric acid, Fumaric acid, Glucono delta-lactone, Lactic acid, Malic acid, Phosphoric acid, Potassium adipate, Potassium citrate, Potassium sodium tartrate, Potassium tartrate, Sodium adipate, Tartaric acid, Trisodium citrate. Excerpt: Phosphoric acid (also known as orthophosphoric acid or phosphoric(V) acid) is a mineral (inorganic) acid having the chemical formula H3PO4. Orthophosphoric acid molecules can combine with themselves to form a variety of compounds which are also referred to as phosphoric acids, but in a more general way. The term phosphoric acid can also refer to a chemical or reagent consisting of phosphoric acids, such as pyrophosphoric acid or triphosphoric acid, but usually orthophosphoric acid. In addition to being a chemical reagent, phosphoric acid has a wide variety of uses, including as a rust inhibitor, food additive, dental and orthop(a)edic etchant, electrolyte, flux, dispersing agent, industrial etchant, fertilizer feedstock, and component of home cleaning products. Pure anhydrous phosphoric acid is a white solid that melts at 42.35 °C to form a colorless, viscous liquid. Most people and even chemists refer to orthophosphoric acid as phosphoric acid, which is the IUPAC name for this compound. The prefix ortho is used to distinguish the acid from other phosphoric acids, called polyphosphoric acids. Orthophosphoric acid is a non-toxic, inorganic, rather weak triprotic acid, which, when pure, is a solid at room temperature and pressure. The chemical structure of orthophosphoric acid is shown above in the data table. Orthophosphoric acid is a very polar molecule; therefore it is highly soluble in water. The oxidation state of phosphorus (P) in ortho- and other phosphoric acids is +5; the oxidation state of all the oxygen atoms (O) is -2 and all the hydrogen atoms (H) is +1. Triprotic means that an orthophosphoric acid molecule can dissociate up to three times, giving up an H each time, which typically combines with a water molecule, H2O, as shown in these reactions: H3PO4(s) + H2O(l) H3O(aq) + H2PO4(aq) Ka1= 7.25×10H2PO4(aq)+ H2O(l) H3O(aq) + HPO4(aq) Ka2= 6.31×10HPO4(aq)+ H2O(l) H3O(aq) + PO4(aq) Ka3= 4.80×10The anion after the first dissociation, H2PO4, is the dihydrogen p