French
DeutschMonocalcium phosphate
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| Names | |
|---|---|
| IUPAC name Calcium bis(dihydrogen phosphate) | |
| Other names Acid calcium phosphate Calcium acid phosphate Calcium diorthophosphate Calcium biphosphate Calcium superphosphate Monobasic calcium phosphate Monocalcium orthophosphate Phosphoric acid, calcium salt (2:1) | |
| Identifiers | |
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3D model (JSmol) | |
| ChemSpider | |
| ECHA InfoCard | 100.028.943 |
| E number | E341(i) (antioxidants, ...) |
PubChem CID | |
| UNII |
|
CompTox Dashboard (EPA) | |
| |
| |
| Properties | |
| CaH4P2O8 | |
| Molar mass | 234.05 g/mol |
| Appearance | White powder |
| Density | 2.220 g/cm3 |
| Melting point | 109 °C (228 °F; 382 K) |
| Boiling point | 203 °C (397 °F; 476 K) (decomposes) |
| 2 g/100 mL | |
Refractive index (nD) | 1.5176 |
| Structure | |
| Triclinic | |
| Hazards | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Related compounds | |
Other anions | Calcium pyrophosphate |
Other cations | Magnesium phosphate Dicalcium phosphate Tricalcium phosphate Strontium phosphate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
Monocalcium phosphate is an inorganic compound with the chemical formula Ca(H2PO4)2 ("AMCP" or "CMP-A" for anhydrous monocalcium phosphate). It is commonly found as the monohydrate ("MCP" or "MCP-M"), Ca(H2PO4)2·H2O. Both salts are colourless solids. They are used mainly as superphosphate fertilizers and are also popular leavening agents.[1]
Preparation
[edit]Material of relatively high purity, as required for baking, is produced by treating calcium hydroxide with phosphoric acid:
Samples of Ca(H2PO4)2 tend to convert to dicalcium phosphate:
Applications
[edit]Use in fertilizers
[edit]Superphosphate fertilizers are produced by treatment of phosphorite with acids ("acidulation"). Using phosphoric acid, fluorapatite is converted to Ca(H2PO4)2:
This solid is called triple superphosphate. Several million tons are produced annually for use as fertilizers. Using sulfuric acid, fluorapatite is converted to a mixture of Ca(H2PO4)2 and CaSO4. This solid is called single superphosphate.
Residual HF typically reacts with silicate minerals co-mingled with the phosphate ores to produce hexafluorosilicic acid (H2SiF6). The majority of the hexafluorosilicic acid is converted to aluminium fluoride and cryolite for the processing of aluminium.[1] These materials are central to the conversion of aluminium ore into aluminium metal.
When sulfuric acid is used, the product contains phosphogypsum (CaSO4·2H2O) and is called single superphosphate. [2]
Use as leavening agent
[edit]Calcium dihydrogen phosphate is used in the food industry as a leavening agent, i.e., to cause baked goods to rise. Because it is acidic, when combined with an alkali carbonate ingredient, commonly sodium bicarbonate (baking soda) or potassium bicarbonate, it reacts to produce carbon dioxide and a salt. Outward pressure of the carbon dioxide gas causes the rising effect. When combined in a ready-made baking powder, the acid and alkali ingredients are included in the right proportions such that they will exactly neutralize each other and not significantly affect the overall pH of the product. AMCP and MCP are fast acting, releasing most carbon dioxide within minutes of mixing. It is popularly used in pancake mixes. In double-acting baking powders, MCP is often combined with the slow-acting acid sodium acid pyrophosphate (SAPP).[3]
See also
[edit]References
[edit]- ^ a b 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. ISBN 978-3527306732.
- ^ Kongshaug, Gunnar; Brentnall, Bernard A.; Chaney, Keith; Gregersen, Jan-Helge; Stokka, Per; Persson, Bjørn; Kolmeijer, Nick W.; Conradsen, Arne; Legard, Torbjørn; Munk, Harald; Skauli, Øyvind; Kiiski, Harri; Solheim, Kai Roger; Legard, Torbjörn; Brentnall, Bernard A.; Rauman-Aalto, Paulina (2014). "Phosphate Fertilizers". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. pp. 1–49. doi:10.1002/14356007.a19_421.pub2. ISBN 978-3527306732.
- ^ John Brodie, John Godber "Bakery Processes, Chemical Leavening Agents" in Kirk-Othmer Encyclopedia of Chemical Technology 2001, John Wiley & Sons. doi:10.1002/0471238961.0308051303082114.a01.pub2
Further reading
[edit]- Havlin, J.L., J.D. Beaton, S.L. Tisdale, and W.L. Nelson. 2005. Soil Fertility and Fertilizers. 7th edn. Pearson Prentice Hall, N.J., ISBN 0130278246