Phosphoric acid
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IUPAC name Phosphoric acid | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Other names Orthophosphoric acid | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Identifiers | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
CAS Number |
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3D model (JSmol) |
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ChEBI |
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ChemSpider |
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ECHA InfoCard | 100.028.758 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
EC Number | 231-633-2 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
E number | E338 (antioxidants, ...) | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
KEGG |
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PubChem CID |
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RTECS number | TB6300000 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
UNII |
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UN number | 1805 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
InChI
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SMILES
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Properties | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Chemical formula | H 3PO 4 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Molar mass | 7001979940000000000♠97.994 g·mol−1 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Appearance | White, deliquescent, solid viscous liquid | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Odor | Odorless | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Density | 2.030 g⋅cm−3 (25 °C) | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Melting point |
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Boiling point | 158 °C (316 °F; 431 K) decomposes | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Solubility in water |
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Solubility | Soluble in ethanol | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
log P | −2.15[2] | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Vapor pressure | 0.03 mmHg (20 °C)[3] | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Acidity (pKa) |
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Conjugate base | Dihydrogen phosphate Hydrogen phosphate Phosphate | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Magnetic susceptibility (χ) | −43.8·10−6 cm3/mol | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Refractive index (nD) |
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Viscosity | 2.4–9.4 cP (85% aq. soln.) 147 cP (100%) | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Structure | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Crystal structure | Monoclinic | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Molecular shape | Tetrahedral | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Thermochemistry | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Std molar entropy (S | 158 J/mol⋅K[5] | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Std enthalpy of formation (ΔfH | −1288 kJ/mol[5] | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
Hazards | |||||||||||||||||||||||||||||||||||||||||||||||||||||||
Safety data sheet | ICSC 1008 | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
GHS pictograms | [6] | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
GHS signal word | Danger | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
GHS hazard statements | H290, H314[6] | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
GHS precautionary statements | P280, P305+351+338, P310[6] | ||||||||||||||||||||||||||||||||||||||||||||||||||||||
NFPA 704 | Flash point Non-flammable | Lethal dose or concentration (LD, LC): | LD50 (median dose) 1530 mg/kg (rat, oral)[7] | US health exposure limits (NIOSH): | PEL (Permissible) TWA 1 mg/m3[3] | REL (Recommended) TWA 1 mg/m3 ST 3 mg/m3[3] | IDLH (Immediate danger) 1000 mg/m3[3] | Related compounds | Related phosphorus oxoacids
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references Phosphoric acid (also known as orthophosphoric acid or phosphoric(V) acid) is a weak acid with the chemical formula H3PO4. Orthophosphoric acid refers to phosphoric acid, which is the IUPAC name for this compound. The prefix ortho- is used to distinguish the acid from related phosphoric acids, called polyphosphoric acids. Orthophosphoric acid is a non-toxic acid, which, when pure, is a solid at room temperature and pressure. The conjugate base of phosphoric acid is the dihydrogen phosphate ion, H The most common source of phosphoric acid is an 85% aqueous solution; such solutions are colourless, odourless, and non-volatile. The 85% solution is a syrupy liquid, but still pourable. Although phosphoric acid does not meet the strict definition of a strong acid, the 85% solution is acidic enough to be corrosive. Contents
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Equilibrium | Disassociation constant, pKa[11] |
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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 |
^ Values are at 25 °C and 0 ionic strength.
Phosphoric acid, H3PO4, is a tribasic acid. The speciation diagram shows that, in aqueous solution, there are five main pH regions.
- There are 3 regions, centred where the pH is equal to a pK value, which are buffer regions.
- In the region centred around pH 4.7 (mid-way between the first two pK values) the dihydrogen phosphate ion, [H2PO4]−, is the only species present.
- In the region centred around pH 9.8 (mid-way between the second and third pK values) the monohydrogen phosphate ion, [HPO4]2−, is the only species present.
This means that salts of the mono- and di-phosphate ions can be selectively crystallised from aqueous solution by setting the pH value to either 4.7 or 9.8.
When phosphoric acid is dissolved in a superacid, poorly characterized products are formed. It is likely that a reaction such as
- H3PO4 + HSbF6 ⇌ [P(OH)4]+ + [SbF6]−
occurs. The ion [P(OH)4]+ is isoelectronic with silicic acid, Si(OH)4.
Uses
The dominant use of phosphoric acid is for fertilizers, consuming approximately 90% of production.[12]
Application | Demand (2006) in thousands of tons | Main phosphate derivatives |
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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[13]) is used to acidify foods and beverages such as various colas and jams. It provides a tangy or sour taste. Phosphoric acid in soft drinks has the potential to cause dental erosion.[14] Phosphoric acid also has the potential to contribute to the formation of kidney stones, especially in those who have had kidney stones previously.[15]
Specific applications of phosphoric acid include:
- In anti-rust treatment by phosphate conversion coating
- As an external standard for phosphorus-31 nuclear magnetic resonance.
- In phosphoric acid fuel cells.
- In activated carbon production.[16]
- In compound semiconductor processing, to etch Indium gallium arsenide selectively with respect to indium phosphide.[17]
- In microfabrication to etch silicon nitride selectively with respect to silicon dioxide.[18]
- As a pH adjuster in cosmetics and skin-care products.[19]
- As a sanitizing agent in the dairy, food, and brewing industries.[20]
Safety
Phosphoric acid has been implicated in the 'diet soda paradox', in which diet sodas are thought to be worse for health than sugared sodas. In order to mask the unpleasant taste of artificial sweeteners, manufacturers add more phosphoric acid to the formulation.[citation needed] At moderate concentrations phosphoric acid solutions are irritating to the skin. Contact with concentrated solutions can cause severe skin burns and permanent eye damage.[21]
See also
- Phosphate fertilizers, such as ammonium phosphate fertilizers
References
^
Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand. Retrieved 2014-06-02..mw-parser-output cite.citationfont-style:inherit.mw-parser-output .citation qquotes:"""""""'""'".mw-parser-output .citation .cs1-lock-free abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .citation .cs1-lock-limited a,.mw-parser-output .citation .cs1-lock-registration abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .citation .cs1-lock-subscription abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registrationcolor:#555.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration spanborder-bottom:1px dotted;cursor:help.mw-parser-output .cs1-ws-icon abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/12px-Wikisource-logo.svg.png")no-repeat;background-position:right .1em center.mw-parser-output code.cs1-codecolor:inherit;background:inherit;border:inherit;padding:inherit.mw-parser-output .cs1-hidden-errordisplay:none;font-size:100%.mw-parser-output .cs1-visible-errorfont-size:100%.mw-parser-output .cs1-maintdisplay:none;color:#33aa33;margin-left:0.3em.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-formatfont-size:95%.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-leftpadding-left:0.2em.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-rightpadding-right:0.2em
^
"phosphoric acid_msds".
^ abcd NIOSH Pocket Guide to Chemical Hazards. "#0506". National Institute for Occupational Safety and Health (NIOSH).
^
O. W. Edwards, R. L. Dunn, J. D. Hatfield (1964). "Refractive Index of Phosphoric Acid Solutions at 25 C.". J. Chem. Eng. Data. 9 (4): 508–509. doi:10.1021/je60023a010.CS1 maint: Multiple names: authors list (link)
^ ab
Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.
^ abc Sigma-Aldrich Co., Phosphoric acid. Retrieved on 2014-05-09.
^ "Phosphoric acid". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
^ 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.
^ Becker, Pierre. (1988). Phosphates and phosphoric acid. New York: Marcel Dekker. ISBN 978-0824717124.
^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 520–522. ISBN 0-08-037941-9.
^ 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.
^ Klaus Schrödter, Gerhard Bettermann, Thomas Staffel, Friedrich Wahl, Thomas Klein, Thomas Hofmann "Phosphoric Acid and Phosphates" in Ullmann's Encyclopedia of Industrial Chemistry 2008, Wiley-VCH, Weinheim. doi:10.1002/14356007.a19_465.pub3
^ "Current EU approved additives and their E Numbers". Foods Standards Agency. 14 March 2012. Retrieved 22 July 2012.
^ 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.
^ 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.
^ 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.
^ Wet chemical etching. umd.edu.
^ Wolf, S.; R. N. Tauber (1986). Silicon processing for the VLSI era: Volume 1 – Process technology. p. 534. ISBN 978-0-9616721-6-4.
^ "Ingredient dictionary: P". Cosmetic ingredient dictionary. Paula's Choice. Archived from the original on 18 January 2008. Retrieved 16 November 2007.
^ "STAR SAN" (PDF). Five Star Chemicals. Retrieved 17 August 2015.
^ "Phosphoric Acid, 85 wt.% SDS". Sigma-Aldrich. 5 May 2016.
External links
Wikimedia Commons has media related to phosphoric acid. |
- National pollutant inventory – Phosphoric acid fact sheet
- NIOSH Pocket guide to chemical hazards