Phosphoric acid
Chemical compound (PO(OH)3) From Wikipedia, the free encyclopedia
Chemical compound (PO(OH)3) From Wikipedia, the free encyclopedia
Phosphoric acid (orthophosphoric acid, monophosphoric acid or phosphoric(V) acid) is a colorless, odorless phosphorus-containing solid, and inorganic compound with the chemical formula H3PO4. It is commonly encountered as an 85% aqueous solution, which is a colourless, odourless, and non-volatile syrupy liquid. It is a major industrial chemical, being a component of many fertilizers.
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| Names | |||
|---|---|---|---|
| IUPAC name
Phosphoric acid | |||
| Other names
Orthophosphoric acid | |||
| Identifiers | |||
3D model (JSmol) |
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| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| ECHA InfoCard | 100.028.758 | ||
| EC Number |
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| E number | E338 (antioxidants, ...) | ||
| KEGG | |||
PubChem CID |
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| RTECS number |
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| UNII | |||
| UN number | 1805 | ||
CompTox Dashboard (EPA) |
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| Properties | |||
| H3PO4 | |||
| Molar mass | 97.994 g·mol−1 | ||
| Appearance | Colorless solid | ||
| Odor | Odorless | ||
| Density | 1.6845 g/cm3 (25 °C, 85%),[1] 1.834 g/cm3 (solid)[2] | ||
| Melting point | 42.35 °C (108.23 °F; 315.50 K) anhydrous[3] 29.32 °C (84.78 °F; 302.47 K) hemihydrate[4] | ||
| Boiling point | |||
| Solubility | Soluble in ethanol | ||
| log P | −2.15[9] | ||
| Vapor pressure | 0.03 mmHg (20 °C)[10] | ||
| Conjugate base | Dihydrogen phosphate | ||
| −43.8·10−6 cm3/mol[11] | |||
Refractive index (nD) |
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| Viscosity | 2.4–9.4 cP (85% aq. soln.) 147 cP (100%) | ||
| Structure | |||
| Monoclinic | |||
| Tetrahedral | |||
| Thermochemistry[13] | |||
Heat capacity (C) |
145.0 J/(mol⋅K) | ||
Std molar entropy (S⦵298) |
150.8 J/(mol⋅K) | ||
Std enthalpy of formation (ΔfH⦵298) |
−1271.7 kJ/mol | ||
Gibbs free energy (ΔfG⦵) |
−1123.6 kJ/mol | ||
| Hazards | |||
| GHS labelling: | |||
 [14] | |||
| Danger | |||
| H290, H314[14] | |||
| P280, P305+P351+P338, P310[14] | |||
| NFPA 704 (fire diamond) | |||
| Flash point | Non-flammable | ||
| Lethal dose or concentration (LD, LC): | |||
LD50 (median dose) |
1530 mg/kg (rat, oral)[15] | ||
| NIOSH (US health exposure limits): | |||
PEL (Permissible) |
TWA 1 mg/m3[10] | ||
REL (Recommended) |
TWA 1 mg/m3 ST 3 mg/m3[10] | ||
IDLH (Immediate danger) |
1000 mg/m3[10] | ||
| Safety data sheet (SDS) | ICSC 1008 | ||
| Related compounds | |||
Related phosphorus oxoacids |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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The compound is an acid. Removal of all three H+ ions gives the phosphate ion PO3−4. Removal of one or two protons gives dihydrogen phosphate ion H2PO−4, and the hydrogen phosphate ion HPO2−4, respectively. Phosphoric acid forms esters, called organophosphates.[16]
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.
Phosphoric acid is produced industrially by one of two routes, wet processes and dry.[17][18][19]
In the wet process, a phosphate-containing mineral such as calcium hydroxyapatite and fluorapatite are treated with sulfuric acid.[20]
Calcium sulfate (gypsum, CaSO4) is a by-product, which is removed as phosphogypsum. The hydrogen fluoride (HF) gas is streamed into a wet (water) scrubber producing hydrofluoric acid. In both cases 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). The phosphoric acid from both processes may be further purified by removing compounds of arsenic and other potentially toxic impurities.
To produce food-grade phosphoric acid, phosphate ore is first reduced with coke in an electric arc furnace, to give elemental phosphorus. This process is also known as the thermal process or the electric furnace process. 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.[21] The thermal process produces phosphoric acid with a very high concentration of P2O5 (about 85%) and a low level of impurities.
However, this process is more expensive and energy-intensive than the wet process, which produces phosphoric acid with a lower concentration of P2O5 (about 26-52%) and a higher level of impurities. The wet process is the most common method of producing phosphoric acid for fertilizer use.[22]
Phosphoric acids produced from phosphate rock or thermal processes often requires purification. A common purification methods is liquid-liquid extraction, which involves the separation of phosphoric acids from water and other impurities using organic solvents, such as tributyl phosphate (TBP), methyl isobutyl ketone (MIBK), or n-octanol. Nanofiltration involves the use of a premodified nanofiltration membrane, which is functionalized by a deposit of a high molecular weight polycationic polymer of polyethyleneimines. Nanofiltration has been shown to significantly reduce the concentrations of various impurities, including cadmium, aluminum, iron, and rare earth elements. The laboratory and industrial pilot scale results showed that this process allows the production of food-grade phosphoric acid.[23]
Fractional crystallization can achieve highest purities typically used for semiconductor applications. Usually a static crystallizer is used. A static crystallizer uses vertical plates, which are suspended in the molten feed and which are alternatingly cooled and heated by a heat transfer medium. The process begins with the slow cooling of the heat transfer medium below the freezing point of the stagnant melt. This cooling causes a layer of crystals to grow on the plates. Impurities are rejected from the growing crystals and are concentrated in the remaining melt. After the desired fraction has been crystallized, the remaining melt is drained from the crystallizer. The purer crystalline layer remains adhered to the plates. In a subsequent step, the plates are heated again to liquify the crystals and the purified phosphoric acid drained into the product vessel. The crystallizer is filled with feed again and the next cooling cycle is started.[24]
In aqueous solution phosphoric acid behaves as a triprotic acid.
The difference between successive pKa values is sufficiently large so that salts of either monohydrogen phosphate, HPO2−4 or dihydrogen phosphate, H2PO−4, can be prepared from a solution of phosphoric acid by adjusting the pH to be mid-way between the respective pKa values.
Aqueous solutions up to 62.5% H3PO4 are eutectic, exhibiting freezing-point depression as low as -85°C. When the concentration of acid rises above 62.5% the freezing-point increases, reaching 21°C by 85% H3PO4 (w/w; the monohydrate). Beyond this the phase diagram becomes complicated, with significant local maxima and minima. For this reason phosphoric acid is rarely sold above 85%, as beyond this adding or removing small amounts moisture risks the entire mass freezing solid, which would be a major problem on a large scale. A local maximum at 91.6% which corresponds to the hemihydrate 2H3PO4•H2O, freezing at 29.32°C.[25][26] There is a second smaller eutectic depression at a concentration of 94.75% with a freezing point of 23.5°C. At higher concentrations the freezing point rapidly increases. Concentrated phosphoric acid tends to supercool before crystallization occurs, and may be relatively resistant to crystallisation even when stored below the freezing point.[4]
Phosphoric acid is commercially available as aqueous solutions of various concentrations, not usually exceeding 85%. If concentrated further it undergoes slow self-condensation, forming an equilibrium with pyrophosphoric acid:
Even at 90% concentration the amount of pyrophosphoric acid present is negligible, but beyond 95% it starts to increase, reaching 15% at what would have otherwise been 100% orthophosphoric acid.[27]
As the concentration is increased higher acids are formed, culminating in the formation of polyphosphoric acids.[28] It is not possible to fully dehydrate phosphoric acid to phosphorus pentoxide, instead the polyphosphoric acid becomes increasingly polymeric and viscous. Due to the self-condensation, pure orthophosphoric acid can only be obtained by a careful fractional freezing/melting process.[4][3]
The dominant use of phosphoric acid is for fertilizers, consuming approximately 90% of production.[29]
| 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[30]) is used to acidify foods and beverages such as various colas and jams, providing a tangy or sour taste. The phosphoric acid also serves as a preservative.[31] 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.[32] Phosphoric acid also has the potential to contribute to the formation of kidney stones, especially in those who have had kidney stones previously.[33]
Specific applications of phosphoric acid include:
Phosphoric acid may also be used for chemical polishing (etching) of metals like aluminium or for passivation of steel products in a process called phosphatization.[39]
Phosphoric acid is not a strong acid. However, at moderate concentrations phosphoric acid solutions are irritating to the skin. Contact with concentrated solutions can cause severe skin burns and permanent eye damage.[40]
A link has been shown between long-term regular cola intake and osteoporosis in later middle age in women (but not men).[41]
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