08-29-2021-2145 - Phosphoric acid weak acid acetic orthophosphoric acid or phosphoric(V) acid H3PO4 acidic H+ ion proton protons PO4,3- dihydrogen phosphate H2PO4,- ester organophosphate pyrophosphoric acid phosphoric acid

Phosphoric acid, also known as orthophosphoric acid or phosphoric(V) acid, is a weak acid with the chemical formula H
3PO
4. The pure compound is a colorless solid.

All three hydrogens are acidic to varying degrees and can be lost from the molecule as H⁺ ions (protons). When all three H⁺ ions are removed, the result is an orthophosphate ion PO₄³⁻, commonly called "phosphate". Removal of one or two protons gives dihydrogen phosphate ion H
2PO−
4, and the hydrogen phosphate ion HPO2−
4, respectively. Orthophosphoric acid also forms esters, called organophosphates.^[15]

Phosphoric acid is commonly encountered in chemical laboratories as an 85% aqueous solution, which is a colourless, odourless, and non-volatile syrupy liquid. Although phosphoric acid does not meet the strict definition of a strong acid, the 85% solution can still severely irritate the skin and damage the eyes.

The name "orthophosphoric acid" can be used to distinguish this specific acid from other "phosphoric acids", such as pyrophosphoric acid. Nevertheless, the term "phosphoric acid" often means this specific compound; and that is the current IUPAC nomenclature. 

Manufacture[edit]

Phosphoric acid is produced industrially by two general routes.^[16] In the wet process a phosphate-containing mineral such as calcium hydroxyapatite is treated with sulfuric acid.^[17]

Fluoroapatite is an alternative feedstock, in which case fluoride is removed as the insoluble compound Na₂SiF₆. The phosphoric acid solution usually contains 23–33% P₂O₅ (32–46% H₃PO₄). It may be concentrated to produce commercial- or merchant-grade phosphoric acid, which contains about 54–62% P₂O₅ (75–85% H₃PO₄). Further removal of water yields superphosphoric acid with a P₂O₅ concentration above 70% (corresponding to nearly 100% H₃PO₄). Calcium sulfate (gypsum) is produced as a by-product and is removed as phosphogypsum.

To produce food-grade phosphoric acid, phosphate ore is first reduced with coke in an electric arc furnace, to make elemental phosphorus. Silica is also added, resulting in the production of calcium silicate slag. Elemental phosphorus is distilled out of the furnace and burned with air to produce high-purity phosphorus pentoxide, which is dissolved in water to make phosphoric acid.

The phosphoric acid from both processes may be further purified by removing compounds of arsenic and other potentially toxic impurities.

Acidic properties[edit]

All three hydrogens are acidic, with dissociation constants pK_a1 = 2.14, pK_a2 = 7.20, and pK_a3 = 12.37. It follows that, in water solutions, phosphoric acid is mostly dissociated into some combination of its three anions, except at very low pH. The equilibrium equations are:

H₃PO₄   + H₂O ⇌ H₃O⁺ + H₂PO₄⁻      K_a1= 7.25×10⁻³ [pK_a1 = 2.14]

H₂PO₄⁻+ H₂O ⇌ H₃O⁺ + HPO₄²⁻       K_a2= 6.31×10⁻⁸ [pK_a2 = 7.20]

HPO₄²⁻+ H₂O ⇌ H₃O⁺ +  PO₄³⁻        K_a3= 3.98×10⁻¹³ [pK_a3 = 12.37]

Uses[edit]

The dominant use of phosphoric acid is for fertilizers, consuming approximately 90% of production.^[18]

Application	Demand (2006) in thousands of tons	Main phosphate derivatives
Soaps and detergents	1836	STPP
Food industry	309	STPP (Na5P3O10), SHMP, TSP, SAPP, SAlP, MCP, DSP(Na2HPO4), H3PO4
Water treatment	164	SHMP, STPP, TSPP, MSP (NaH2PO4), DSP
Toothpastes	68	DCP (CaHPO4), IMP, SMFP
Other applications	287	STPP (Na3P3O9), TCP, APP, DAP, zinc phosphate (Zn3(PO4)2), aluminium phosphate (AlPO4, H3PO4)

Food-grade phosphoric acid (additive E338^[19]) is used to acidify foods and beverages such as various colasand jams, providing a tangy or sour taste. Soft drinks containing phosphoric acid, which would include Coca-Cola, are sometimes called phosphate sodas or phosphates. Phosphoric acid in soft drinks has the potential to cause dental erosion.^[20] Phosphoric acid also has the potential to contribute to the formation of kidney stones, especially in those who have had kidney stones previously.^[21]

Specific applications of phosphoric acid include:

• in anti-rust treatment by phosphate conversion coating or passivation
  • to prevent iron oxidation by means of the Parkerization process
• as an external standard for phosphorus-31 nuclear magnetic resonance
• in phosphoric acid fuel cells
• in activated carbon production^[22]
• in compound semiconductor processing, to etch Indium gallium arsenide selectively with respect to indium phosphide^[23]
• in microfabrication to etch silicon nitride selectively with respect to silicon dioxide^[24]
• as a pH adjuster in cosmetics and skin-care products^[25]
• as a sanitizing agent in the dairy, food, and brewing industries^[26]

• Phosphate fertilizers, such as ammonium phosphate fertilizers

References[edit]

1. ^ Christensen, J. H. & Reed, R. B. (1955). "Design and Analysis Data—Density of Aqueous Solutions of Phosphoric Acid Measurements at 25 °C". Ind. Eng. Chem. 47 (6): 1277–1280. doi:10.1021/ie50546a061.
2. ^ "CAMEO Chemicals Datasheet - Phosphoric Acid".
3. ^ http://www.chemspider.com/Chemical-Structure.979.html
4. ^ Brown, Earl H.; Whitt, Carlton D. (1952). "Vapor Pressure of Phosphoric Acids". Industrial & Engineering Chemistry. 44 (3): 615–618. doi:10.1021/ie50507a050.
5. ^ Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand. Retrieved 2 June 2014.
6. ^ Jump up to: ^a b Haynes, p. 4.80
7. ^ "phosphoric acid_msds".
8. ^ Jump up to: ^a b c d NIOSH Pocket Guide to Chemical Hazards. "#0506". National Institute for Occupational Safety and Health (NIOSH).
9. ^ Haynes, p. 5.92
10. ^ Haynes, p. 4.134
11. ^ Edwards, O. W.; Dunn, R. L. & Hatfield, J. D. (1964). "Refractive Index of Phosphoric Acid Solutions at 25 C.". J. Chem. Eng. Data. 9 (4): 508–509. doi:10.1021/je60023a010.
12. ^ Haynes, p. 5.13
13. ^ Jump up to: ^a b c Sigma-Aldrich Co., Phosphoric acid. Retrieved on 9 May 2014.
14. ^ "Phosphoric acid". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
15. ^ Westheimer, F.H. (6 June 1987). "Why nature chose phosphates". Science. 235 (4793): 1173–1178 (see pp. 1175–1176). Bibcode:1987Sci...235.1173W. CiteSeerX 10.1.1.462.3441. doi:10.1126/science.2434996. PMID 2434996.
16. ^ Becker, Pierre (1988). Phosphates and phosphoric acid. New York: Marcel Dekker. ISBN 978-0824717124.
17. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 520–522. ISBN 978-0-08-037941-8.
18. ^ Schrödter, Klaus; Bettermann, Gerhard; Staffel, Thomas; Wahl, Friedrich; Klein, Thomas; Hofmann, Thomas (2008). "Phosphoric Acid and Phosphates". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_465.pub3.
19. ^ "Current EU approved additives and their E Numbers". Foods Standards Agency. 14 March 2012. Retrieved 22 July 2012.
20. ^ Moynihan, P. J. (23 November 2002). "Dietary advice in dental practice". British Dental Journal. 193 (10): 563–568. doi:10.1038/sj.bdj.4801628. PMID 12481178.
21. ^ Qaseem, A; Dallas, P; Forciea, MA; Starkey, M; et al. (4 November 2014). "Dietary and pharmacologic management to prevent recurrent nephrolithiasis in adults: A clinical practice guideline from the American College of Physicians". Annals of Internal Medicine. 161 (9): 659–67. doi:10.7326/M13-2908. PMID 25364887.
22. ^ Toles, C.; Rimmer, S.; Hower, J. C. (1996). "Production of activated carbons from a washington lignite using phosphoric acid activation". Carbon. 34 (11): 1419. doi:10.1016/S0008-6223(96)00093-0.
23. ^ Wet chemical etching. umd.edu.
24. ^ Wolf, S.; R. N. Tauber (1986). Silicon processing for the VLSI era: Volume 1 – Process technology. p. 534. ISBN 978-0-9616721-6-4.
25. ^ "Ingredient dictionary: P". Cosmetic ingredient dictionary. Paula's Choice. Archived from the original on 18 January 2008. Retrieved 16 November 2007.
26. ^ "STAR SAN" (PDF). Five Star Chemicals. Retrieved 17 August 2015.
27. ^ Tucker KL, Morita K, Qiao N, Hannan MT, Cupples LA, Kiel DP (1 October 2006). "Colas, but not other carbonated beverages, are associated with low bone mineral density in older women: The Framingham Osteoporosis Study". American Journal of Clinical Nutrition. 84 (4): 936–942. doi:10.1093/ajcn/84.4.936. PMID 17023723.
28. ^ "Phosphoric Acid, 85 wt.% SDS". Sigma-Aldrich. 5 May 2016.

Cited sources[edit]

• Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. ISBN 978-1439855119.

External links[edit]

Wikimedia Commons has media related to phosphoric acid.

• National pollutant inventory – Phosphoric acid fact sheet
• NIOSH Pocket guide to chemical hazards

Categories: 

• Mineral acids
• Flavors
• Food acidity regulators
• Glassforming liquids and melts
• Phosphates
• Phosphorus oxoacids
• Hydrogen compounds
• Acid catalysts
• E-number additives
• Phosphorus(V) compounds

https://en.wikipedia.org/wiki/Phosphoric_acid

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