Dihydrogen phosphate

Inorganic ion
Dihydrogen phosphate
Names
IUPAC name
Dihydrogenphosphate
Systematic IUPAC name
Phosphoric acid, ion(1-)
Other names
Phosphoric acid, ion(1-) Dehydrophosphoric acid (1-)
Identifiers
CAS Number
  • 14066-20-7 checkY
3D model (JSmol)
  • Interactive image
ChEBI
  • CHEBI:39745
ChemSpider
  • 978
DrugBank
  • DB02831
Gmelin Reference
 1999
PubChem CID
  • 1003
CompTox Dashboard (EPA)
  • DTXSID40930897 Edit this at Wikidata
InChI
  • InChI=1S/H3O4P/c1-5(2,3)4/h(H3,1,2,3,4)/p-1
    Key: NBIIXXVUZAFLBC-UHFFFAOYSA-M
  • OP(=O)(O)[O-]
Properties
Chemical formula
 H2O4P−1
Molar mass 96.986 g·mol−1
Conjugate acid Phosphoric Acid
Related compounds
Related compounds
 Phosphate, Monohydrogen phosphate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
Chemical compound

Dihydrogen phosphate is an inorganic ion with the formula [H2PO4]−. 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. Emulsifying agents prevent separation of two ingredients in processed foods that would separate under natural conditions while neutralizing agents make processed foods taste fresher longer and lead to an increased shelf-life of these foods.[1] Surface-activating agents prevent surface-tension formation on liquid-containing processed foods and finally, leavening agents are used in processed foods to aid in the expansion of yeast in baked goods.[1]

Dihydrogen phosphate is employed in the production of pharmaceuticals furthering their importance to medical practitioners of gastroenterology and humans in general. In this medical discipline, sodium phosphates are used as natural laxatives.[1] Other medical applications include using sodium and potassium phosphates along with other medications to increase their therapeutic effects. Inflammation, certain cancers, and ulcers can benefit from the use of combination therapy with sodium and potassium phosphates.[1]

Potassium dihydrogen phosphate, the potassium salt, is useful to human in the form of pesticides. Potassium dihydrogen phosphate is a fungicide that is used to prevent powdery mildew on many fruits.[2] Fruits that can benefit from the addition of potassium dihydrogen phosphate includes common fruits, peppers, and roses.[2]

Structure

The dihydrogen phosphate anion consists of a central phosphorus atom surrounded by 2 equivalent oxygen atoms and 2 hydroxy groups in a tetrahedral arrangement.[3] Dihydrogen phosphate can be identified as an anion, an ion with an overall negative charge, with dihydrogen phosphates being a negative 1 charge.[3] Dihydrogen phosphate contains 4 H bond acceptors and 2 H bond donors,[3] and has 0 rotatable bonds.[4]

Acid-base equilibria

Dihydrogen phosphate is an intermediate in the multi-step conversion of the polyprotic phosphoric acid to phosphate:[5]

This multistep conversion exemplifies that the dihydrogen phosphate ion is the conjugate base to phosphoric acid, while also acting as the conjugate acid to the phosphate ion.[3] This means that dihydrogen phosphate can be both a hydrogen donor and acceptor.

Equilibrium Disassociation constant, pKa[6]
H3PO4 ⇌ H
2PO−
4 + H+ 		pKa1 = 2.14[a]
H
2PO−
4 ⇌ HPO2−
4 + H+ 		pKa2 = 7.20
HPO2−
4 ⇌ PO3−
4 + H+ 		pKa3 = 12.37

Examples

Safety

Many foods including milk, eggs, poultry, and nuts contain these sodium phosphates.[1]

Notes

  1. ^ Values are at 25 °C and 0 ionic strength.

References

  1. ^ a b c d e f Tech, Noah. "Sodium Phosphates: From Food to Pharmacology | Noah Technologies". Retrieved 2021-03-23.
  2. ^ a b "Document Display | NEPIS | US EPA". nepis.epa.gov. Retrieved 2021-03-23.
  3. ^ a b c d PubChem. "Dihydrogen phosphate". pubchem.ncbi.nlm.nih.gov. Retrieved 2021-03-23.
  4. ^ "dihydrogenphosphate | H2O4P | ChemSpider". chemspider.com. Retrieved 2021-03-23.
  5. ^ "Phosphoric Acid H3PO4". aqion.de. Retrieved 2021-03-23.
  6. ^ Powell, Kipton J.; Brown, Paul L.; Byrne, Robert H.; Gajda, Tamás; Hefter, Glenn; Sjöberg, Staffan; Wanner, Hans (2005). "Chemical speciation of environmentally significant heavy metals with inorganic ligands. Part 1: The Hg2+, Cl−, OH−, CO2−
    3    , SO2−
    4    , and PO3−
    4     aqueous systems". Pure Appl. Chem. 77 (4): 739–800. doi:10.1351/pac200577040739.
  • v
  • t
  • e
H3PO4
[HPO4]2−
[H2PO4]− 		He
Li3PO4 Be BPO4
+BO3 		C (NH4)3PO4
(NH4)2HPO4
NH4H2PO4
-N 		O +F Ne
Na3PO4
Na2HPO4
NaH2PO4 		Mg3(PO4)2 AlPO4 Si P +SO4
-S 		Cl Ar
K3PO4
K2HPO4
KH2PO4 		Ca3(PO4)2 ScPO4 Ti VPO4 CrPO4 Mn3(PO4)2
MnPO4 		Fe3(PO4)2
FePO4 		Co3(PO4)2 Ni3(PO4)2 Cu3(PO4)2 Zn3(PO4)2 GaPO4 Ge As -Se Br Kr
Rb3PO4 Sr3(PO4)2 YPO4 Zr3(PO4)4 Nb Mo Tc Ru Rh Pd Ag3PO4 Cd3(PO4)2 InPO4 Sn SbPO4
-SbO4 		Te I Xe
Cs3PO4 Ba3(PO4)2 * LuPO4 Hf Ta W Re Os Ir Pt AuPO4 Hg Tl3PO4 Pb3(PO4)2 BiPO4 Po At Rn
Fr Ra ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
 
* LaPO4 CePO4 PrPO4 NdPO4 PmPO4 SmPO4 EuPO4 GdPO4 TbPO4 DyPO4 HoPO4 ErPO4 TmPO4 YbPO4
** AcPO4 Th3(PO4)4 Pa U(PO4)2 Np PuPO4 AmPO4 CmPO4 Bk Cf Es Fm Md No