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Phosphoric acid
	;
; ;	; ;
Names;
	; IUPAC name; Phosphoric acid;
	Other names; Orthophosphoric acid;
Identifiers;
; CAS Number;	; ; 7664-38-2 Y; ;
; 3D model (JSmol);	; Interactive image; ;
; ChEBI;	; ; CHEBI:26078 Y; ;
; ChEMBL;	; ; ChEMBL1187 Y; ;
; ChemSpider;	; ; 979 Y; ;
; ECHA InfoCard;	; 100.028.758;
; EC Number;	231-633-2;
; E number;	E338 (antioxidants, ...);
; KEGG;	; ; D05467 Y; ;
; ; PubChem CID; ;	; 1004; ;
; RTECS number;	TB6300000;
; UNII;	; ; E4GA8884NN Y; ;
; UN number;	1805;
	; ; InChI; ; InChI=1S/H3O4P/c1-5(2,3)4/h(H3,1,2,3,4) Y; Key: NBIIXXVUZAFLBC-UHFFFAOYSA-N Y; ; ; ; InChI=1/H3O4P/c1-5(2,3)4/h(H3,1,2,3,4); Key: NBIIXXVUZAFLBC-UHFFFAOYAI; ; ; ;
	; ; SMILES; OP(=O)(O)O; ;
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;	; 42.3 °C (anhydrous); ; 29.3 °C (hemihydrate); ; ;
; Boiling point;	158 °C (316 °F; 431 K) decomposes;
; Solubility in water;	; 392.2 g/100 g (−16.3 °C); ; 369.4 g/100 mL (0.5 °C); ; 446 g/100 mL (14.95 °C); ; ;
; Solubility;	Soluble in ethanol;
; log P;	−2.15
; Vapor pressure;	0.03 mmHg (20 °C)
; Acidity (pKa);	; pKa1 = 2.15; ; pKa2 = 7.20; ; pKa3 = 12.32; ; ;
; Conjugate base;	; Dihydrogen phosphate; Hydrogen phosphate; Phosphate;
; ; Magnetic susceptibility (χ);	−43.8·10−6 cm3/mol;
; ; Refractive index (nD);	; 1.3420 (8.8% w/w aq. soln.); ; 1.4320 (85% aq. soln) 25 °C; ; ;
; Viscosity;	2.4–9.4 cP (85% aq. soln.) ; 147 cP (100%);
Structure;
; Crystal structure;	Monoclinic;
; Molecular shape;	Tetrahedral;
Thermochemistry;
; ; Std molar; entropy (So298); ;	158 J/mol⋅K
; ; Std enthalpy of; formation (ΔfHo298); ;	−1288 kJ/mol
Hazards;
; Safety data sheet;	; ICSC 1008;
; GHS pictograms;	;
; GHS signal word;	Danger;
; GHS hazard statements;	; H290, H314
; GHS precautionary statements;	; P280, P305+351+338, P310
; NFPA 704;	; ; ; ; ; 0; ; ; 3; ; ; 0; ; ; ;
; Flash point;	Non-flammable ;
	Lethal dose or concentration (LD, LC):;
; ; LD50 (median dose);	1530 mg/kg (rat, oral)
	US health exposure limits (NIOSH):;
; ; PEL (Permissible);	TWA 1 mg/m3
; ; REL (Recommended);	TWA 1 mg/m3 ST 3 mg/m3
; ; IDLH (Immediate danger);	1000 mg/m3
Related compounds;
; Related phosphorus oxoacids; ;	; Hypophosphorous acid; ; Phosphorous acid; ; Pyrophosphoric acid; ; Triphosphoric acid; ; Peroxomonophosphoric acid; ; Peroxodiphosphoric acid; ; ;
	; 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
₂PO⁻
₄, which in turn has a conjugate base of hydrogen phosphate, HPO²⁻
₄, which has a conjugate base of phosphate, PO³⁻
₄. Phosphates are essential for life.^[8]

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.

Manufacture

Phosphoric acid is produced industrially by two general routes.^[9] In the wet process a phosphate-containing mineral such as calcium hydroxyapatite is treated with sulfuric acid.^[10]

displaystyle ce Ca5(PO4)3OH + 5H2SO4 -> 3H3PO4 + 5CaSO4v + H2O

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

Phosphoric acid speciation

Equilibrium	Disassociation constant, pK_a^[11]
H₃PO₄ ⇌ H ₂PO⁻ ₄ + H⁺	pK_a1 = 2.14^[a]
H ₂PO⁻ ₄ ⇌ HPO²⁻ ₄ + H⁺	pK_a2 = 7.20
HPO²⁻ ₄ ⇌ PO³⁻ ₄ + H⁺	pK_a3 = 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
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]

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".

^ ^a^b^c^d 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)

^ ^a^b
Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.

^ ^a^b^c 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

National pollutant inventory – Phosphoric acid fact sheet

NIOSH Pocket guide to chemical hazards

This page is only for reference, If you need detailed information, please check here

[12] Values are at 25 °C and 0 ionic strength.

[sioc-1] 
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

[chemsrc-2] 
"phosphoric acid_msds".

[PGCH-3] NIOSH Pocket Guide to Chemical Hazards. "#0506". National Institute for Occupational Safety and Health (NIOSH).

[Refractive_Index-4] 
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)

[b1-5] 
Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.

[sigma-6] Sigma-Aldrich Co., Phosphoric acid. Retrieved on 2014-05-09.

[7] "Phosphoric acid". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).

[Westheimer-8] 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.

[9] Becker, Pierre. (1988). Phosphates and phosphoric acid. New York: Marcel Dekker. ISBN 978-0824717124.

[10] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 520–522. ISBN 0-08-037941-9.

[11] 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.

[Ullmann-13] 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

[14] "Current EU approved additives and their E Numbers". Foods Standards Agency. 14 March 2012. Retrieved 22 July 2012.

[15] 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.

[Qa2014-16] 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.

[17] 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.

[18] Wet chemical etching. umd.edu.

[Wolf-19] Wolf, S.; R. N. Tauber (1986). Silicon processing for the VLSI era: Volume 1 – Process technology. p. 534. ISBN 978-0-9616721-6-4.

[20] "Ingredient dictionary: P". Cosmetic ingredient dictionary. Paula's Choice. Archived from the original on 18 January 2008. Retrieved 16 November 2007.

[21] "STAR SAN" (PDF). Five Star Chemicals. Retrieved 17 August 2015.

[:0-22] "Phosphoric Acid, 85 wt.% SDS". Sigma-Aldrich. 5 May 2016.

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Phosphoric acid

Contents

Manufacture

Acidic properties

Uses

Safety

See also

References

External links

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