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Since the ends are condensed, its formula has one less H 2 O (water) than tripolyphosphoric acid. The general formula of a phosphoric acid is H n−2x+2 P n O 3n−x+1, where n is the number of phosphorus atoms and x is the number of fundamental cycles in the molecule's structure; that is, the minimum number of bonds that would have to be ...
Tetrasodium pyrophosphate is produced by the reaction of furnace-grade phosphoric acid with sodium carbonate to form disodium phosphate, which is then heated to 450 °C to form tetrasodium pyrophosphate: [5] 2 Na 2 HPO 4 → Na 4 P 2 O 7 + H 2 O
K3PO4. Tripotassium phosphate has few industrial applications, however it is commonly used as a base in laboratory-scale organic chemistry. Being insoluble in organic solvents, it is an easily removed proton acceptor in organic synthesis.
Trisodium phosphate is produced by neutralization of phosphoric acid using sodium carbonate, which produces disodium hydrogen phosphate. The disodium hydrogen phosphate is reacted with sodium hydroxide to form trisodium phosphate and water. Na 2 CO 3 + H 3 PO 4 → Na 2 HPO 4 + CO 2 + H 2 O Na 2 HPO 4 + NaOH → Na 3 PO 4 + H 2 O
Phosphoric acid (orthophosphoric acid, monophosphoric acid or phosphoric(V) acid) is a colorless, odorless phosphorus-containing solid, and inorganic compound with the chemical formula H 3 P O 4. It is commonly encountered as an 85% aqueous solution , which is a colourless, odourless, and non- volatile syrupy liquid.
The pKa's occur in two distinct ranges because deprotonations occur on separate phosphate groups. For comparison with the pK a 's for phosphoric acid are 2.14, 7.20, and 12.37. At physiological pH's, pyrophosphate exists as a mixture of doubly and singly protonated forms.
Sodium phosphates are popular in commerce in part because they are inexpensive and because they are nontoxic at normal levels of consumption. [4] However, oral sodium phosphates when taken at high doses for bowel preparation for colonoscopy may in some individuals carry a risk of kidney injury under the form of phosphate nephropathy.
It can be oxidised by nitric acid to phosphoric acid. Violet phosphorus ignites upon impact in air. [20] [better source needed] If it is heated in an atmosphere of inert gas, for example nitrogen or carbon dioxide, it sublimes and the vapour condenses as white phosphorus.