Pyrophosphoric acid
Chemical compound
From Wikipedia, the free encyclopedia
Pyrophosphoric acid, also known as diphosphoric acid, is the inorganic compound with the formula H4P2O7 or, more descriptively, [(HO)2P(O)]2O. Colorless and odorless, it is soluble in water, diethyl ether, and ethyl alcohol. The anhydrous acid crystallizes in two polymorphs, which melt at 54.3 and 71.5 °C. The compound is a component of polyphosphoric acid, an important source of phosphoric acid.[1] Anions, salts, and esters of pyrophosphoric acid are called pyrophosphates.
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| Names | |
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| IUPAC names
Diphosphoric acid μ-oxido-bis(dihydroxidooxidophosphorus) | |
| Other names
Pyrophosphoric acid Phosphonophosphoric acid Phosphono dihydrogenphosphate | |
| Identifiers | |
3D model (JSmol) |
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| ChEBI | |
| ChEMBL | |
| ChemSpider | |
| DrugBank | |
| ECHA InfoCard | 100.017.795 |
| EC Number |
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| 82619 | |
| KEGG | |
PubChem CID |
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| UNII | |
CompTox Dashboard (EPA) |
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| Properties | |
| H4P2O7 | |
| Molar mass | 177.97 g/mol |
| Melting point | 71.5 °C (160.7 °F; 344.6 K) |
| Extremely soluble | |
| Solubility | Very soluble in alcohol, ether |
| Conjugate base | Pyrophosphate |
| Hazards | |
| GHS labelling: | |
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| Danger | |
| H302, H314 | |
| P260, P264, P264+P265, P270, P280, P301+P317, P301+P330+P331, P302+P361+P354, P304+P340, P305+P354+P338, P316, P317, P321, P330, P363, P405, P501 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Preparation
It can be prepared by reaction of phosphoric acid with phosphoryl chloride:[2]
- 5 H3PO4 + POCl3 → 3 H4P2O7 + 3 HCl
It can also be prepared by ion exchange from sodium pyrophosphate or by treating lead pyrophosphate with hydrogen sulfide.[1]
Boiling the water from orthophosphoric acid will not dehydrate it to pure pyrophosphoric acid, instead a mixture of ortho, pyro, and polyphosphoric acids are produced, the maximum pyrophosphoric acid concentration remains below 50% and occurs slightly before what would otherwise be pure pyrophosphoric acid.[3] This is because the equilibrium in the liquid phase favors the disproportionation of pyrophosphoric acid. Pyrophosphoric acid may be obtained from mixed phosphoric acids by careful crystallization or by the addition of seed crystals.[4][5]
Reactions
Pyrophosphoric acid is a tetraprotic acid, with four distinct pKa's:[6]
- H4P2O7 ⇌ [H3P2O7]− + H+, pKa = 0.85
- [H3P2O7]− ⇌ [H2P2O7]2− + H+, pKa = 1.96
- [H2P2O7]2− ⇌ [HP2O7]3− + H+, pKa = 6.60
- [HP2O7]3− ⇌ [P2O7]4− + H+, pKa = 9.41
The pKa's occur in two distinct ranges because deprotonations occur on separate phosphate groups. For comparison with the pKa'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.
When molten, pyrophosphoric acid rapidly converts to an equilibrium mixture of phosphoric acid, pyrophosphoric acid and polyphosphoric acids. The percentage by weight of pyrophosphoric acid is around 40% and it is difficult to recrystallise from the melt.
Even in cold water, pyrophosphoric acid hydrolyses to phosphoric acid. All polyphosphoric acids behave similarly.[7]
- H4P2O7 + H2O → 2 H3PO4
Safety
While pyrophosphoric acid is corrosive, it is not known to be otherwise toxic.[8]
History
The name pyrophosphoric acid was given by a "Mr. Clarke of Glasgow" in 1827 who is credited with its discovery following the heating to red heat of a sodium phosphate salt. It was found that phosphoric acid when heated to red heat formed pyrophosphoric acid that was readily converted to phosphoric acid by hot water.[9]