Pyrophosphoric acid.

In chemistry, a phosphoric acid, in the general sense, is a phosphorus oxoacid in which each phosphorus (P) atom is in the oxidation state +5, and is bonded to four oxygen (O) atoms, one of them through a double bond, arranged as the corners of a tetrahedron. Two or more of these PO4 tetrahedra may be connected by shared single-bonded oxygens, forming linear or branched chains, cycles, or more complex structures. The single-bonded oxygen atoms that are not shared are completed with acidic hydrogen atoms. The general formula of a phosphoric acid is Hn+2−2xPnO3n+1−x, where n is the number of phosphorus atoms and x is the number of fundamental cycles in the molecule's structure, between 0 and n + 2/2.

Pyrophosphate anion.
Trimethyl orthophosphate.

Removal of protons (H+) from k hydroxyl groups –OH leaves anions generically called phosphates (if k = n − 2x + 2) or hydrogen phosphates (if k is between 1 and n − 2x + 1), with general formula [Hn−2x+2−kPnO3n+1−x]k−. The fully dissociated anion (k = n − 2x + 2) has formula [PnO3n−x+1](n−2x+2)−. The term phosphate is also used in organic chemistry for the functional groups that result when or more of the hydrogens are replaced by bonds to other groups.

These acids, together with their salts and esters, include some of the best-known compounds of phosphorus, of high importance in biochemistry, mineralogy, agriculture, pharmacy, chemical industry, and chemical research.

Acids

Phosphoric acid

The simplest and most commonly encountered of the phosphoric acids is orthophosphoric acid, H3PO4. Indeed, the term phosphoric acid often means this compound specifically (and this is also the current IUPAC nomenclature).

Oligophosphoric and polyphosphoric acids

Polyphosphoric acid

Two or more orthophosphoric acid molecules can be joined by condensation into larger molecules by elimination of water. Condensation of a few units yields the oligophosphoric acids, while larger molecules are called polyphosphoric acids. (However, the distinction between the two terms is not well defined.)

For example, pyrophosphoric, triphosphoric and tetraphosphoric acids can be obtained by the reactions

The "backbone" of a polyphosphoric acid molecule is a chain of alternating P and O atoms. Each extra orthophosphoric unit that is condensed adds 1 extra H (hydrogen) atom, 1 extra P (phosphorus) atom, and 3 extra O (oxygen) atoms. The general formula of a polyphosphoric acid is Hn+2PnO3n+1 or HO[−P(O)(OH)−O−]nH.

Polyphosphoric acids are used in organic synthesis for cyclizations and acylations; an alternative is Eaton's reagent.[1][2][3]

Cyclic phosphoric acids

Condensation between two –OH units of the same molecule, on the other hand, eliminates two hydrogen atoms and one oxygen atom, creating a cycle, as in the formation of trimetaphosphoric acid:

H5P3O10 → H3P3O9 + H2O

The general formula of a phosphoric acid is Hn−2x+2PnO3n−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 broken to eliminate all cycles.

The limiting case of internal condensation, where all oxygen atoms are shared and there are no hydrogen atoms (x = n+2/2) would be an anhydride P2nO_{5n}, such as phosphorus pentoxide P4O10.

Phosphates

Removal of the hydrogen atoms as protons H+ turns a phosphoric acid into a phosphate anion. Partial removal yields various hydrogen phosphate anions.

Orthophosphate

The anions of orthophosphoric acid H3PO4 are orthophosphate (commonly called simply "phosphate") PO3−4, monohydrogen phosphate HPO2−4, and dihydrogen phosphate H2PO4−.

Linear oligophosphates and polyphosphates

Dissociation of pyrophosphoric acid H4P2O7 generates four anions, [H4−kP2O7]k−, where the charge k ranges from 1 to 4. The last one is pyrophosphate [P2O7]4−. The pyrophosphates are mostly water-soluble.

Likewise, tripolyphosphoric acid H5P3O10 yields at least five anions [H5−kP3O10]k−, where k ranges from 1 to 5, including tripolyphosphate [P3O10]5−. Tetrapolyphosphoric acid H6P4O13 yields at least six anions, including tetrapolyphosphate [P4O13]6−, and so on. Note that each extra phosphoric unit adds one extra P atom, three extra O atoms, and either one extra hydrogen atom or an extra negative charge.

Branched polyphosphoric acids give similarly branched polyphosphate anions. The simplest example of this is triphosphono phosphate [OP(OPO3)3]9− and its partially dissociated versions.

The general formula for such (non-cyclic) polyphosphate anions, linear or branched, is [Hn+2−kPnO3n+1]k−, where the charge k may vary from 1 to n + 2. Generally in an aqueous solution, the degree or percentage of dissociation depends on the pH of the solution.

Cyclic polyphosphates

Trimetaphosphoric acid

The phosphoric acid units can be bonded together in rings (cyclic structures) forming metaphosphoric acid molecules. The simplest such compound is trimetaphosphoric acid or cyclo-triphosphoric acid having the formula H3P3O9. Its structure is shown in the illustration. Since the ends are condensed, its formula has one less H2O (water) than tripolyphosphoric acid. What are commonly called trimetaphosphates actually have a mixture of ring sizes. A general formula for such cyclic compounds is [HPO3]x where x = number of phosphoric units in the molecule. The hypothetical monomer monometaphosphoric acid (HPO3), which would be valence isoelectronic with nitric acid, is not known to exist.

When these metaphosphoric acids lose their hydrogens as H+, cyclic anions called metaphosphates are formed. An example of a compound with such an anion is sodium hexametaphosphate (Na6P6O18), used as a sequestrant and a food additive.

Chemical properties

Solubility

These phosphoric acids series are generally water-soluble considering the polarity of the molecules. Ammonium and alkali phosphates are also quite soluble in water. The alkaline earth salts start becoming less soluble and phosphate salts of various other metals are even less soluble.

Hydrolysis and condensation

In aqueous solutions (solutions of water), water gradually (over the course of hours) hydrolyzes polyphosphates into smaller phosphates and finally into ortho-phosphate, given enough water. Higher temperature or acidic conditions can speed up the hydrolysis reactions considerably.[4]

Conversely, polyphosphoric acids or polyphosphates are often formed by dehydrating a phosphoric acid solution; in other words, removing water from it often by heating and evaporating the water off.

Uses

Ortho-, pyro-, and tripolyphosphate compounds have been commonly used in detergents (i. e. cleaners) formulations. For example, see Sodium tripolyphosphate. Sometimes pyrophosphate, tripolyphosphate, tetrapolyphosphate, etc. are called diphosphate, triphosphate, tetraphosphate, etc., especially when they are part of phosphate esters in biochemistry. They are also used for scale and corrosion control by potable water providers.[5] As a corrosion inhibitor, polyphosphates work by forming a protective film on the interior surface of pipes.[6]

Phosphate esters

General chemical structure of a monophosphate ester; here any R can be H or some organic radical.

The −OH groups in phosphoric acids can also condense with the hydroxyl groups of alcohols to form phosphate esters. Since orthophosphoric acid has three −OH groups, it can esterify with one, two, or three alcohol molecules to form a mono-, di-, or triester. See the general structure image of an ortho- (or mono-) phosphate ester below on the left, where any of the R groups can be a hydrogen or an organic radical. Di- and tripoly- (or tri-) phosphate esters, etc. are also possible. Any −OH groups on the phosphates in these ester molecules may lose H+ ions to form anions, again depending on the pH in a solution. In the biochemistry of living organisms, there are many kinds of (mono)phosphate, diphosphate, and triphosphate compounds (essentially esters), many of which play a significant role in metabolism such as adenosine diphosphate (ADP) and triphosphate (ATP).

Structure of a chiral phosphoric acid derived from BINOL.[7]

See also

References

  1. ↑ Harwood, Laurence M.; Hodgkinson, Leslie C.; Sutherland, James K.; Towers, Patrick (1984). "Synthesis of anthracyclinones. Part 1. Regioselective alkylation of 5-hydroxyquinizarin". Canadian Journal of Chemistry. 62 (10): 1922–1925. doi:10.1139/v84-329.
  2. ↑ Nakazawa, Koichi; Matsuura, Shin; Kusuda, Kosuke (1954). "Studies on the Application of Polyphosphoric Acid as a Condensing Agent. II". Yakugaku Zasshi. 74 (5): 495–497. doi:10.1248/yakushi1947.74.5_495.
  3. ↑ Eaton, P. E.; Carlson, G. R.; Lee, J. T. (1973). "Phosphorus pentoxide-methanesulfonic acid. Convenient alternative to polyphosphoric acid". J. Org. Chem. 38 (23): 4071. doi:10.1021/jo00987a028.
  4. ↑ "Phosphoric acid and phosphates". Encyclopedia of Chemical Technology. New York: The Interscience Encyclopedia, Inc. 1953. p. 421.
  5. ↑ "Polyphosphates for scale and corrosion control". Tramfloc, INC. January 2009. Retrieved December 23, 2010.
  6. ↑ "Ortho-Polyphosphate Corrosion Inhibitors" (PDF). Government Engineering:The Journal for Public Infrastructure (September–October, 2006): 48–49. Retrieved December 23, 2010.
  7. ↑ Parmar, Dixit; Sugiono, Erli; Raja, Sadiya; Rueping, Magnus (2014). "Complete Field Guide to Asymmetric BINOL-Phosphate Derived Brønsted Acid and Metal Catalysis: History and Classification by Mode of Activation; Brønsted Acidity, Hydrogen Bonding, Ion Pairing, and Metal Phosphates". Chemical Reviews. 114 (18): 9047–9153. doi:10.1021/cr5001496. PMID 25203602.

Further reading

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