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{{other}}
{{Chembox {{Chembox
| Verifiedfields = changed
⚫ | verifiedrevid = 401800846
| Watchedfields = changed
⚫ | verifiedrevid = 428203184
| ImageFile = Ammonium phosphate.png | ImageFile = Ammonium phosphate.png
| ImageSize = 200px
| ImageFile1 = Triammonium-phosphate-3D-balls.png | ImageFile1 = Triammonium-phosphate-3D-balls.png
| ImageSize1 = 240px | ImageSize1 = 240px
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| Reference = <ref name="hand"> | Reference = <ref name="hand">
{{cite book | last = Lide | first = David R. | year = 1998 {{cite book | last = Lide | first = David R. | year = 1998
| title = Handbook of Chemistry and Physics | title = Handbook of Chemistry and Physics
| edition = 87 | volume = | edition = 87 | volume =
| location = Boca Raton, FL | location = Boca Raton, Florida
| publisher = CRC Press | publisher = CRC Press
| isbn = 0-8493-0594-2 | pages = 4–42, 5–19}}</ref> | isbn = 978-0-8493-0594-8 | pages = 4–42, 5–19}}</ref>
| IUPACName = ammonium phosphate | IUPACName = ammonium phosphate
| OtherNames = triammonium phosphate | OtherNames = triammonium phosphate
| Section1 = {{Chembox Identifiers |Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 140090 | ChemSpiderID = 140090
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = ZRIUUUJAJJNDSS-UHFFFAOYSA-N | StdInChIKey = ZRIUUUJAJJNDSS-UHFFFAOYSA-N
| CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Comment = {{cascite|correct|CAS}}
| CASNo = 10361-65-6 | CASNo = 10361-65-6
| PubChem = | EC_number = 269-789-9
| UNII_Ref = {{fdacite|changed|FDA}}
| UNII = 2ZJF06M0I9
| PubChem = 159282
| SMILES = P()()=O... | SMILES = P()()=O...
}} }}
| Section2 = {{Chembox Properties |Section2={{Chembox Properties
| Formula = (NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub>
| N=3|H=12|O=4|P=1
| Appearance = | Appearance = White, ] crystals
| Density = | Density =
| MeltingPt = | MeltingPt =
| BoilingPt = | BoilingPt =
| Solubility = 58.0 g/100 mL (25°C)}} | Solubility = 58.0&nbsp;g/100&nbsp;mL (25&nbsp;°C)
| SolubleOther = Insoluble in ]<ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1138561632 |pages=4–41|edition=99th |language=English}}</ref>
⚫ | Section3 = {{Chembox Hazards
| MolarMass<!-- MolecularWeight -->=149.09 g/mol}}
⚫ | MainHazards =
⚫ |Section3={{Chembox Hazards
⚫ | FlashPt =
| Autoignition = }} | GHSPictograms = {{GHS07}}
| GHSSignalWord = Warning
⚫ | Section4 = {{Chembox Thermochemistry
| HPhrases = {{H-phrases|302|319}}
⚫ | DeltaHf = -1671.9 kJ/mol
| PPhrases = {{P-phrases|264|270|280|301+312|305+351+338|330|337+313|501}}
⚫ | DeltaHc =
| Entropy = | NFPA-H = 2
| NFPA-F = 0
| NFPA-R = 0
⚫ | MainHazards =
⚫ | FlashPt =
| AutoignitionPt = }}
⚫ |Section4={{Chembox Thermochemistry
⚫ | DeltaHf = −1671.9&nbsp;kJ/mol
⚫ | DeltaHc =
| Entropy =
| HeatCapacity = }} | HeatCapacity = }}
| Section8 = {{Chembox Related |Section8={{Chembox Related
| OtherAnions = ]<br/>] | OtherCations = ]<br/>]
| OtherCations = ]<br/>] | OtherCompounds = ]<br/>]
| OtherFunctn =
| Function =
| OtherCpds =
}} }}
}} }}


'''Ammonium phosphate''' is the ] of ] and ]. It has the ] (NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub> and consists of ] ]s and ] ]. It is obtained as a crystalline powder upon mixing concentrated solutions of ammonia and phosphoric acid, or on the addition of excess of ammonia to the acid phosphate ]. It is soluble in water, and the aqueous solution on boiling loses ammonia and the acid phosphate ] is formed. '''Ammonium phosphate''' is the ] with the ] (NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub>. It is the ammonium ] of orthophosphoric acid. A related "double salt", (NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub><sup>.</sup>(NH<sub>4</sub>)<sub>2</sub>HPO<sub>4</sub> is also recognized but is impractical to use. Both triammonium salts evolve ammonia. In contrast to the unstable nature of the triammonium salts, the ] (NH<sub>4</sub>)<sub>2</sub>HPO<sub>4</sub> and ] (NH<sub>4</sub>)H<sub>2</sub>PO<sub>4</sub> are stable materials that are commonly used as fertilizers to provide plants with fixed nitrogen and phosphorus.<ref name=Ullmann>{{Ullmann|first1=Klaus|last1=Schrödter|first2=Gerhard|last2=Bettermann|first3=Thomas |last3=Staffel|first4=Friedrich|last4=Wahl|first5=Thomas|last5=Klein||first6=Thomas|last6=Hofmann|title=Phosphoric Acid and Phosphates|year=2008|doi=10.1002/14356007.a19_465.pub3}}</ref>


==Preparation of triammonium phosphate==
Ammonium phosphate is used as an ingredient in some ]s as a high source of elemental ]. It is also used as a ] in thermoplastic compositions. It is also used in bread making to promote the growth of the yeast.<ref>http://www.freshpatents.com/Flame-retardant-composition-dt20051229ptan20050288402.php</ref>
Triammonium phosphate can be prepared in the laboratory by treating 85% phosphoric acid with 30% ammonia solution:{{cn|date=April 2019}}

:H<sub>3</sub>PO<sub>4</sub> + 3 NH<sub>3</sub> → (NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub>

(NH<sub>4</sub>)<sub>3</sub>PO<sub>4</sub> is a colorless, crystalline solid. The solid, which has the odor of ammonia, is readily soluble in water. The salt converts to diammonium hydrogen phosphate (NH<sub>4</sub>)<sub>2</sub>HPO<sub>4</sub>.


==See also== ==See also==
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==References== ==References==
{{Reflist}} {{Reflist}}

{{Ammonium salts}}
{{Phosphates}}


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{{inorganic-compound-stub}} {{inorganic-compound-stub}}

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