Pyrophosphoric acid

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Pyrophosphoric acid
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Names
IUPAC names
Diphosphoric acid
μ-oxido-bis(dihydroxidooxidophosphorus)
Other names
Pyrophosphoric acid
Phosphonophosphoric acid
Phosphono dihydrogenphosphate
Identifiers
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3D model (JSmol)
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EC Number Page Template:Plainlist/styles.css has no content.
82619
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  • InChI=1S/H4O7P2/c1-8(2,3)7-9(4,5)6/h(H2,1,2,3)(H2,4,5,6) checkY
    Key: XPPKVPWEQAFLFU-UHFFFAOYSA-N checkY
  • InChI=1/H4O7P2/c1-8(2,3)7-9(4,5)6/h(H2,1,2,3)(H2,4,5,6)
    Key: XPPKVPWEQAFLFU-UHFFFAOYAX
  • O=P(O)(O)OP(=O)(O)O
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
Hazards
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Template:Chembox Footer/trackingTemplate:Short description

Script error: No such module "Redirect-distinguish". 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.

Preparation

It can be prepared by reaction of phosphoric acid with phosphoryl chloride:[2]

Page Module:Chem2/styles.css has no content.5 H3PO4 + POCl3 → Page Module:Chem2/styles.css has no content.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]

Page Module:Chem2/styles.css has no content.H4P2O7 ⇌ [H3P2O7]− + H+, pKa = 0.85
Page Module:Chem2/styles.css has no content.[H3P2O7]− ⇌ [H2P2O7]2− + H+, pKa = 1.96
Page Module:Chem2/styles.css has no content.[H2P2O7]2− ⇌ [HP2O7]3− + H+, pKa = 6.60
Page Module:Chem2/styles.css has no content.[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]

Page Module:Chem2/styles.css has no content.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]

See also

References

  1. ^ a b Page Module:Citation/CS1/styles.css has no content.Havelange, Sébastien; Lierde, Nicolas; Germeau, Alain; Martins, Emmanuel; Theys, Tibaut; Sonveaux, Marc; Toussaint, Claudia; Schrödter, Klaus; Bettermann, Gerhard; Staffel, Thomas; Wahl, Friedrich; Klein, Thomas; Hofmann, Thomas (2022). "Phosphoric Acid and Phosphates". Ullmann's Encyclopedia of Industrial Chemistry. pp. 1–55. doi:10.1002/14356007.a19_465.pub4. ISBN 9783527303854. S2CID 246266565.
  2. ^ Page Module:Citation/CS1/styles.css has no content.R. Klement (1963). "Condensed Orthophosphates". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 546.
  3. ^ Page Module:Citation/CS1/styles.css has no content.Korte, Carsten; Conti, Fosca; Wackerl, Jürgen; Lehnert, Werner (2016), Li, Qingfeng; Aili, David; Hjuler, Hans Aage; Jensen, Jens Oluf (eds.), "Phosphoric Acid and its Interactions with Polybenzimidazole-Type Polymers", High Temperature Polymer Electrolyte Membrane Fuel Cells, Cham: Springer International Publishing, pp. 169–194, doi:10.1007/978-3-319-17082-4_8, ISBN 978-3-319-17081-7, retrieved 2023-02-11{{citation}}: CS1 maint: work parameter with ISBN (link)
  4. ^ Page Module:Citation/CS1/styles.css has no content.Wakefield, Zachary T.; Egan, Edward P., Jr. (1962), "Fertilizer Materials, Melting Points in Orthophosphoric Acid -- Pyrophosphoric Acid System", Journal of Agricultural and Food Chemistry, vol. 10, no. 4, ACS Publications, pp. 344–346, doi:10.1021/jf60122a023{{citation}}: CS1 maint: multiple names: authors list (link)
  5. ^ Page Module:Citation/CS1/styles.css has no content.Shen, Chung Y (1975), "Production of Crystalline Pyrophosphoric Acid and its Salts", Industrial & Engineering Chemistry Process Design and Development, vol. 14, no. 1, ACS Publications, pp. 80–85, doi:10.1021/i260053a014
  6. ^ Page Module:Citation/CS1/styles.css has no content.Yadav, Prerna; Blacque, Olivier; Roodt, Andreas; Zelder, Felix (2021). "Induced fit activity-based sensing: A mechanistic study of pyrophosphate detection with a "flexible" Fe-salen complex". Inorganic Chemistry Frontiers. 8 (19): 4313–4323. doi:10.1039/d1qi00209k. PMC 8477187. PMID 34603734.
  7. ^ Page Module:Citation/CS1/styles.css has no content.Corbridge, D. (1995). "Chapter 3: Phosphates". Studies in inorganic Chemistry vol. 20. Elsevier Science B.V. pp. 169–305. doi:10.1016/B978-0-444-89307-9.50008-8. ISBN 0-444-89307-5.
  8. ^ Material Safety Data Sheet: Pyrophosphoric acid MSDS www.sciencelab.com
  9. ^ Page Module:Citation/CS1/styles.css has no content.Beck, Lewis Caleb (1834). A Manual of Chemistry: Containing a Condensed View of the Present State of the Science, with Copious References to More Extensive Treatises, Original Papers, Etc. E.W & C Skinner. p. 160. Retrieved January 30, 2015.

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