Phosphates

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Phosphate deposits can contain significant amounts of naturally occurring heavy metals. Mining operations processing phosphate rock can leave tailings piles containing elevated levels of <a href="http://en.wikipedia.org/wiki/Cadmium" title="Cadmium" >cadmium</a>, <a href="http://en.wikipedia.org/wiki/Lead" title="Lead" >lead</a>, <a href="http://en.wikipedia.org/wiki/Nickel" title="Nickel" >nickel</a>, <a href="http://en.wikipedia.org/wiki/Copper" title="Copper" >copper</a>, <a href="http://en.wikipedia.org/wiki/Chromium" title="Chromium" >chromium</a>, and <a href="http://en.wikipedia.org/wiki/Uranium" title="Uranium" >uranium</a>. Unless carefully managed, these waste products can leach heavy metals into groundwater or nearby estuaries. Uptake of these substances by plants and marine life can lead to concentration of toxic heavy metals in food products.<sup id="cite_ref-9" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-9" >[10]</a></sup><sup id="cite_ref-9" class="reference" ></sup>

<h1 id="firstHeading" class="firstHeading" >Phosphate</h1>

<div id="siteSub" >From Wikipedia, the free encyclopedia</div>

<div id="contentSub" >  (Redirected from <a href="http://en.wikipedia.org/w/index.php?title=Phosphates&redirect=no" title="Phosphates" >Phosphates</a>)</div>

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<th colspan="2" >Phosphate</th>

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<div class="NavHead" ><a href="http://en.wikipedia.org/wiki/IUPAC_nomenclature" title="IUPAC nomenclature" class="mw-redirect" >Systematic name</a><a class="NavToggle" id="NavToggle1" href="javascript:toggleNavigationBar(1);" >[hide]</a></div>

<p >Phosphate<sup id="cite_ref-0" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-0" >[1]</a></sup></p>

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<th colspan="2" >Identifiers</th>

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<td ><a href="http://en.wikipedia.org/wiki/CAS_registry_number" title="CAS registry number" >CAS number</a></td>

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<td ><a href="http://en.wikipedia.org/wiki/PubChem" title="PubChem" >PubChem</a></td>

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<td ><a href="http://en.wikipedia.org/wiki/ChemSpider" title="ChemSpider" >ChemSpider</a></td>

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<td ><a rel="nofollow" class="external text" href="http://www.nlm.nih.gov/cgi/mesh/2007/MB_cgi?mode=&term=Phosphates" >Phosphates</a></td>

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<td ><a href="http://en.wikipedia.org/wiki/ChEBI" title="ChEBI" >ChEBI</a></td>

<td ><a rel="nofollow" class="external text" href="https://www.ebi.ac.uk/chebi/searchId.do?chebiId=18367" >CHEBI:18367</a><sup > <img src="/a5f46370-c15b-5c78-b6b1-5c584c6f5137.png"/></sup></td>

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<td ><a href="http://en.wikipedia.org/wiki/ChEMBL" title="ChEMBL" >ChEMBL</a></td>

<td ><a rel="nofollow" class="external text" href="https://www.ebi.ac.uk/chembldb/index.php/compound/inspect/CHEMBL289287" >CHEMBL289287</a><sup > <img src="/495d6c9e-54fe-5016-96dc-1f275c550a5d.png"/></sup></td>

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<td ><a href="http://en.wikipedia.org/wiki/Beilstein_database" title="Beilstein database" >Beilstein Reference</a></td>

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<td ><a href="http://en.wikipedia.org/wiki/Gmelin_database" title="Gmelin database" >Gmelin Reference</a></td>

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<td ><a href="http://en.wikipedia.org/wiki/Jmol" title="Jmol" >Jmol</a>-3D images</td>

<td ><a rel="nofollow" class="external text" href="http://chemapps.stolaf.edu/jmol/jmol.php?model=%5BO-%5DP%28%5BO-%5D%29%28%5BO-%5D%29%3DO" >Image 1</a>

<a rel="nofollow" class="external text" href="http://chemapps.stolaf.edu/jmol/jmol.php?model=%5BO-%5DP%28%3DO%29%28%5BO-%5D%29%5BO-%5D" >Image 2</a>

<a rel="nofollow" class="external text" href="http://chemapps.stolaf.edu/jmol/jmol.php?model=O%3DP%28%5BO-%5D%29%28%5BO-%5D%29%5BO-%5D" >Image 3</a></td>

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<div align="center"><a href="http://en.wikipedia.org/wiki/Simplified_molecular_input_line_entry_specification" title="Simplified molecular input line entry specification" class="mw-redirect" >SMILES</a></div>

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<div align="center"><a href="http://en.wikipedia.org/wiki/International_Chemical_Identifier" title="International Chemical Identifier" >InChI</a></div>

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<th colspan="2" >Properties</th>

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<td ><a href="http://en.wikipedia.org/wiki/Chemical_formula" title="Chemical formula" >Molecular formula</a></td>

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<td ><a href="http://en.wikipedia.org/wiki/Molar_mass" title="Molar mass" >Molar mass</a></td>

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<td ><a href="http://en.wikipedia.org/wiki/Exact_mass" title="Exact mass" class="mw-redirect" >Exact mass</a></td>

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<td colspan="2" > <img src="/209ce532-9dd9-5fa2-a350-f7c92e79d764.png"/> <a class="external text" href="http://en.wikipedia.org/w/index.php?title=Special:ComparePages&rev1=458267616&page2=Phosphate" >(verify)</a> <a href="http://en.wikipedia.org/wiki/Wikipedia:WikiProject_Chemicals/Chembox_validation" title="Wikipedia:WikiProject Chemicals/Chembox validation" >(what is:</a> <img src="/8cf6139c-39ce-5d41-9399-48e62cd77a05.png"/>/<img src="/f94dfbee-041a-5a4d-a857-1ed2a8991819.png"/>?)

Except where noted otherwise, data are given for materials in their <a href="http://en.wikipedia.org/wiki/Standard_state" title="Standard state" >standard state (at 25 °C, 100 kPa)</a></td>

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<td colspan="2" ><a href="http://en.wikipedia.org/wiki/Wikipedia:Chemical_infobox#References" title="Wikipedia:Chemical infobox" >Infobox references</a></td>

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<p >A <b>phosphate</b>, an <a href="http://en.wikipedia.org/wiki/Inorganic_chemical" title="Inorganic chemical" class="mw-redirect" >inorganic chemical</a>, is a <a href="http://en.wikipedia.org/wiki/Salt_(chemistry)" title="Salt (chemistry)" >salt</a> of <a href="http://en.wikipedia.org/wiki/Phosphoric_acid" title="Phosphoric acid" >phosphoric acid</a>. In <a href="http://en.wikipedia.org/wiki/Organic_chemistry" title="Organic chemistry" >organic chemistry</a>, a phosphate, or <a href="http://en.wikipedia.org/wiki/Organophosphate" title="Organophosphate" >organophosphate</a>, is an <a href="http://en.wikipedia.org/wiki/Ester" title="Ester" >ester</a> of phosphoric acid. Organic phosphates are important in <a href="http://en.wikipedia.org/wiki/Biochemistry" title="Biochemistry" >biochemistry</a> and <a href="http://en.wikipedia.org/wiki/Biogeochemistry" title="Biogeochemistry" >biogeochemistry</a> or <a href="http://en.wikipedia.org/wiki/Ecology" title="Ecology" >ecology</a>. Inorganic phosphates are <a href="http://en.wikipedia.org/wiki/Mining" title="Mining" >mined</a> to obtain<a href="http://en.wikipedia.org/wiki/Phosphorus" title="Phosphorus" >phosphorus</a> for use in agriculture and industry.<sup id="cite_ref-PhosphatePrimer_1-0" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-PhosphatePrimer-1" >[2]</a></sup><sup id="cite_ref-Kuntz1_2-0" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-Kuntz1-2" >[3]</a></sup><sup id="cite_ref-Kuntz2_3-0" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-Kuntz2-3" >[4]</a></sup> At elevated temperatures in the solid state, phosphates can <a href="http://en.wikipedia.org/wiki/Condensation_reaction" title="Condensation reaction" >condense</a> to form <a href="http://en.wikipedia.org/wiki/Pyrophosphate" title="Pyrophosphate" >pyrophosphates</a>.</p>

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<h2 >Contents</h2>

  [<a href="http://en.wikipedia.org/wiki/Phosphates#" class="internal" id="togglelink" >hide</a>] </div>

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<li class="toclevel-1 tocsection-1" ><a href="http://en.wikipedia.org/wiki/Phosphates#Chemical_properties" >1 Chemical properties</a>

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<li class="toclevel-2 tocsection-2" ><a href="http://en.wikipedia.org/wiki/Phosphates#Biochemistry_of_phosphates" >1.1 Biochemistry of phosphates</a></li>

<li class="toclevel-2 tocsection-3" ><a href="http://en.wikipedia.org/wiki/Phosphates#Geochemistry_of_phosphates" >1.2 Geochemistry of phosphates</a></li>

<li class="toclevel-2 tocsection-4" ><a href="http://en.wikipedia.org/wiki/Phosphates#Ecology_of_phosphates" >1.3 Ecology of phosphates</a></li>

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<li class="toclevel-1 tocsection-6" ><a href="http://en.wikipedia.org/wiki/Phosphates#References" >3 References</a></li>

<li class="toclevel-1 tocsection-7" ><a href="http://en.wikipedia.org/wiki/Phosphates#External_links" >4 External links</a></li>

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<h2 >[<a href="http://en.wikipedia.org/w/index.php?title=Phosphate&action=edit&section=1" title="Edit section: Chemical properties" >edit</a>]Chemical properties</h2>

The general chemical structure of an organophosphate.</div>

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This is the <a href="http://en.wikipedia.org/wiki/Structural_formula" title="Structural formula" >structural formula</a> of the phosphoric acid <a href="http://en.wikipedia.org/wiki/Functional_group" title="Functional group" >functional group</a> as found in a weakly <a href="http://en.wikipedia.org/wiki/Acidic" title="Acidic" class="mw-redirect" >acidic</a><a href="http://en.wikipedia.org/wiki/Aqueous_solution" title="Aqueous solution" >aqueous solution</a>. In more <a href="http://en.wikipedia.org/wiki/Basic_(chemistry)" title="Basic (chemistry)" class="mw-redirect" >basic</a>aqueous solutions, the group donates the two <a href="http://en.wikipedia.org/wiki/Hydrogen" title="Hydrogen" >hydrogen</a> <a href="http://en.wikipedia.org/wiki/Atom" title="Atom" >atoms</a>and <a href="http://en.wikipedia.org/wiki/Ion" title="Ion" >ionizes</a> as a phosphate group with a negative charge of 2. <sup id="cite_ref-4" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-4" >[5]</a></sup></div>

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<p >The phosphate ion is a <a href="http://en.wikipedia.org/wiki/Polyatomic_ion" title="Polyatomic ion" >polyatomic ion</a> with the <a href="http://en.wikipedia.org/wiki/Empirical_formula" title="Empirical formula" >empirical formula</a> PO3−<br />

4 and a <a href="http://en.wikipedia.org/wiki/Molar_mass" title="Molar mass" >molar mass</a> of 94.97 g/mol. It consists of one central <a href="http://en.wikipedia.org/wiki/Phosphorus" title="Phosphorus" >phosphorus</a> atom surrounded by four oxygen atoms in a<a href="http://en.wikipedia.org/wiki/Tetrahedron" title="Tetrahedron" >tetrahedral</a> arrangement. The phosphate ion carries a negative three formal charge and is the<a href="http://en.wikipedia.org/wiki/Conjugate_acid" title="Conjugate acid" >conjugate base</a> of the hydrogen phosphate ion, HPO2−<br />

4, which is the conjugate base of H<sub >2</sub>PO−<br />

4, the dihydrogen phosphate ion, which in turn is the conjugate base of H<sub >3</sub>PO<sub >4</sub>, <a href="http://en.wikipedia.org/wiki/Phosphoric_acid" title="Phosphoric acid" >phosphoric acid</a>. The phosphate ion is a <a href="http://en.wikipedia.org/wiki/Hypervalent_molecule" title="Hypervalent molecule" >hypervalent molecule</a> (the phosphorus atom has 10 electrons in its <a href="http://en.wikipedia.org/wiki/Valence_shell" title="Valence shell" class="mw-redirect" >valence shell</a>). A phosphate salt forms when a positively charged ion attaches to the negatively charged oxygen atoms of the ion, forming an ionic <a href="http://en.wikipedia.org/wiki/Chemical_compound" title="Chemical compound" >compound</a>. Many phosphates are not <a href="http://en.wikipedia.org/wiki/Solubility" title="Solubility" >soluble</a> in <a href="http://en.wikipedia.org/wiki/Water" title="Water" >water</a> at<a href="http://en.wikipedia.org/wiki/Standard_temperature_and_pressure" title="Standard temperature and pressure" class="mw-redirect" >standard temperature and pressure</a>. The sodium, potassium, rubidium, caesium and ammonium phosphates are all water soluble. Most other phosphates are only slightly soluble or are insoluble in water. As a rule, the hydrogen and dihydrogen phosphates are slightly more soluble than the corresponding phosphates. The <a href="http://en.wikipedia.org/wiki/Pyrophosphate" title="Pyrophosphate" >pyrophosphates</a> are mostly water soluble.

Aqueous phosphate exists in four forms. In strongly basic conditions, the phosphate ion (PO3−<br />

4) predominates, whereas in weakly basic conditions, the hydrogen phosphate ion (HPO2−<br />

4) is prevalent. In weakly acid conditions, the dihydrogen phosphate ion (H<sub >2</sub>PO−<br />

4) is most common. In strongly acidic conditions, trihydrogen phosphate (H<sub >3</sub>PO<sub >4</sub>) is the main form.</p>

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4</center>

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4</center>

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4</center>

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<p >More precisely, considering the following three equilibrium reactions:</p>

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4</dd>

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4 <img src="/b98f08f1-4726-5c09-8fad-63592472ae16.png"/> H<sup >+</sup> + HPO2−<br />

4</dd>

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4 <img src="/01a42719-da1b-5c54-86fa-aadc0508db62.png"/> H<sup >+</sup> + PO3−<br />

4</dd>

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<p >the corresponding constants at 25°C (in mol/L) are (see <a href="http://en.wikipedia.org/wiki/Phosphoric_acid" title="Phosphoric acid" >phosphoric acid</a>):</p>

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<p >The <a href="http://en.wikipedia.org/wiki/Determination_of_equilibrium_constants#Speciation_calculations" title="Determination of equilibrium constants" >speciation diagram</a> obtained using these p<i>K</i> values shows three distinct regions. In effectH<sub >3</sub>PO<sub >4</sub>, H<sub >2</sub>PO−<br />

4 and HPO2−<br />

4 behave as separate <a href="http://en.wikipedia.org/wiki/Weak_acid" title="Weak acid" >weak acids</a>. This is because the successive <a href="http://en.wikipedia.org/wiki/Acid_dissociation_constant" title="Acid dissociation constant" >p<i>K</i>values</a> differ by more than 4. For each acid the pH at half-neutralization is equal to the p<i>K</i> value of the acid. The region in which the acid is in equilibrium with its conjugate base is defined by pH ≈ p<i>K</i>± 2. Thus the three pH regions are approximately 0–4, 5–9 and 10–14. This is idealized as it assumes constant <a href="http://en.wikipedia.org/wiki/Ionic_strength" title="Ionic strength" >ionic strength</a>, which will not hold in reality at very low and very high pH values.

For a neutral pH as in the cytosol, pH=7.0</p>

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4 and HPO2−<br />

4 ions are present in significant amounts (62% H<sub >2</sub>PO−<br />

4, 38% HPO2−<br />

4Note that in the extracellular fluid (pH=7.4), this proportion is inverted (61% HPO2−<br />

4, 39% H<sub >2</sub>PO−<br />

4).

Phosphate can form many polymeric ions such as <a href="http://en.wikipedia.org/wiki/Diphosphate" title="Diphosphate" class="mw-redirect" >diphosphate</a> (also known as <a href="http://en.wikipedia.org/wiki/Pyrophosphate" title="Pyrophosphate" >pyrophosphate</a>),P<sub >2</sub>O4−<br />

7, and <a href="http://en.wikipedia.org/wiki/Sodium_triphosphate" title="Sodium triphosphate" >triphosphate</a>, P<sub >3</sub>O5−<br />

The various <a href="http://en.wikipedia.org/wiki/Metaphosphate" title="Metaphosphate" >metaphosphate</a> ions (which are usually long linear polymers) have an empirical formula of PO−<br />

3 and are found in many compounds.</p>

<h3 >[<a href="http://en.wikipedia.org/w/index.php?title=Phosphate&action=edit&section=2" title="Edit section: Biochemistry of phosphates" >edit</a>]Biochemistry of phosphates</h3>

<p >In <a href="http://en.wikipedia.org/wiki/Biological_system" title="Biological system" >biological systems</a>, phosphorus is found as a free phosphate ion in solution and is called <b>inorganic phosphate</b>, to distinguish it from phosphates bound in various phosphate esters. Inorganic phosphate is generally denoted <b>P<sub >i</sub></b> and at physiological (neutral) <a href="http://en.wikipedia.org/wiki/PH" title="PH" >pH</a> primarily consists of a mixture of HPO2−<br />

4 and H<sub >2</sub>PO−<br />

4 ions.

Inorganic phosphate can be created by the <a href="http://en.wikipedia.org/wiki/Hydrolysis" title="Hydrolysis" >hydrolysis</a> of <a href="http://en.wikipedia.org/wiki/Pyrophosphate" title="Pyrophosphate" >pyrophosphate</a>, which is denoted <b>PP<sub >i</sub></b>:</p>

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7 + H<sub >2</sub>O <img src="/a29e6b13-dfac-5d54-b604-f815ff96eff3.png"/> 2 HPO2−<br />

4</dd>

</dl>

<p >However, phosphates are most commonly found in the form of adenosine phosphates, (<a href="http://en.wikipedia.org/wiki/Adenosine_monophosphate" title="Adenosine monophosphate" >AMP</a>, <a href="http://en.wikipedia.org/wiki/Adenosine_diphosphate" title="Adenosine diphosphate" >ADP</a> and <a href="http://en.wikipedia.org/wiki/Adenosine_triphosphate" title="Adenosine triphosphate" >ATP</a>) and in <a href="http://en.wikipedia.org/wiki/DNA" title="DNA" >DNA</a> and <a href="http://en.wikipedia.org/wiki/RNA" title="RNA" >RNA</a> and can be released by the hydrolysis of ATP or ADP. Similar reactions exist for the other <a href="http://en.wikipedia.org/wiki/Nucleotide" title="Nucleotide" >nucleoside diphosphates</a> and <a href="http://en.wikipedia.org/wiki/Nucleotide" title="Nucleotide" >triphosphates</a>. Phosphoanhydride bonds in ADP and ATP, or other nucleoside diphosphates and triphosphates, contain high amounts of energy which give them their vital role in all living organisms. They are generally referred to as <a href="http://en.wikipedia.org/wiki/High_energy_phosphate" title="High energy phosphate" class="mw-redirect" >high energy phosphate</a>, as are the <a href="http://en.wikipedia.org/wiki/Phosphagen" title="Phosphagen" >phosphagens</a> in muscle tissue. Compounds such as substituted <a href="http://en.wikipedia.org/wiki/Phosphine" title="Phosphine" >phosphines</a> have uses in organic chemistry but do not seem to have any natural counterparts.

The addition and removal of phosphate from proteins in all cells is a pivotal strategy in the regulation of <a href="http://en.wikipedia.org/wiki/Metabolism" title="Metabolism" >metabolic</a> processes.</p>

<a href="http://en.wikipedia.org/wiki/Reference_ranges_for_blood_tests" title="Reference ranges for blood tests" >Reference ranges for blood tests</a>, showing <i>inorganic phosphorus</i> in purple at right, being almost identical to the molar concentration of phosphate.</div>

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<p >Phosphate is useful in animal <a href="http://en.wikipedia.org/wiki/Cell_(biology)" title="Cell (biology)" >cells</a> as a <a href="http://en.wikipedia.org/wiki/Buffering_agent" title="Buffering agent" >buffering agent</a>. Phosphate salts that are commonly used for preparing <a href="http://en.wikipedia.org/wiki/Buffer_solution#Useful_buffer_mixtures" title="Buffer solution" >buffer solutions</a> at cell p<i>H</i>s include Na<sub >2</sub>HPO<sub >4</sub>, NaH<sub >2</sub>PO<sub >4</sub>, and the corresponding potassium salts.

An important occurrence of phosphates in biological systems is as the structural material of bone and teeth. These structures are made of crystalline <a href="http://en.wikipedia.org/wiki/Calcium_phosphate" title="Calcium phosphate" >calcium phosphate</a> in the form of <a href="http://en.wikipedia.org/wiki/Hydroxylapatite" title="Hydroxylapatite" >hydroxyapatite</a>. The hard dense enamel of mammalian teeth consists of <a href="http://en.wikipedia.org/wiki/Fluoroapatite" title="Fluoroapatite" class="mw-redirect" >fluoroapatite</a>, an hydroxy calcium phosphate where some of the <a href="http://en.wikipedia.org/wiki/Hydroxyl" title="Hydroxyl" >hydroxyl</a> groups have been replaced by <a href="http://en.wikipedia.org/wiki/Fluoride" title="Fluoride" >fluoride</a> ions.

Insect exoskeleta are constructed of <a href="http://en.wikipedia.org/wiki/Chitin" title="Chitin" >chitin</a> containing crystalline calcium phosphate as a strengthening material.</p>

<h3 >[<a href="http://en.wikipedia.org/w/index.php?title=Phosphate&action=edit&section=3" title="Edit section: Geochemistry of phosphates" >edit</a>]Geochemistry of phosphates</h3>

<p >Phosphates are the naturally occurring form of the element <a href="http://en.wikipedia.org/wiki/Phosphorus" title="Phosphorus" >phosphorus</a>, found in many <a href="http://en.wikipedia.org/wiki/Phosphate_mineral" title="Phosphate mineral" class="mw-redirect" >phosphate minerals</a>. In mineralogy and geology, phosphate refers to a rock or ore containing phosphate ions. Inorganic phosphates are <a href="http://en.wikipedia.org/wiki/Mining" title="Mining" >mined</a> to obtain phosphorus for use in agriculture and industry.<sup id="cite_ref-PhosphatePrimer_1-1" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-PhosphatePrimer-1" >[2]</a></sup><sup id="cite_ref-Kuntz1_2-1" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-Kuntz1-2" >[3]</a></sup><sup id="cite_ref-Kuntz2_3-1" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-Kuntz2-3" >[4]</a></sup>

The largest <a href="http://en.wikipedia.org/wiki/Phosphorite" title="Phosphorite" >phosphorite</a> or <i>rock phosphate</i> deposits in <a href="http://en.wikipedia.org/wiki/North_America" title="North America" >North America</a> lie in the <a href="http://en.wikipedia.org/wiki/Bone_Valley" title="Bone Valley" >Bone Valley</a> region of central <a href="http://en.wikipedia.org/wiki/Florida" title="Florida" >Florida</a>, <a href="http://en.wikipedia.org/wiki/United_States" title="United States" >United States</a>, the Soda Springs region of Idaho, and the coast of North Carolina. Smaller deposits are located in Montana, Tennessee, Georgia and South Carolina near Charleston along Ashley Phosphate road. The small island nation of <a href="http://en.wikipedia.org/wiki/Nauru" title="Nauru" >Nauru</a> and its neighbor <a href="http://en.wikipedia.org/wiki/Banaba_Island" title="Banaba Island" >Banaba Island</a>, which used to have massive phosphate deposits of the best quality, have been mined excessively. Rock phosphate can also be found in Egypt, Israel, Morocco, Navassa Island, Tunisia, Togo and Jordan, countries that have large phosphate mining industries.

Phosphorite mines are primarily found in:</p>

<ul >

<li ><b>North America</b>: <a href="http://en.wikipedia.org/wiki/United_States_of_America" title="United States of America" class="mw-redirect" >United States of America</a>, especially <a href="http://en.wikipedia.org/wiki/North_Carolina" title="North Carolina" >North Carolina</a>, with lesser deposits in <a href="http://en.wikipedia.org/wiki/Florida" title="Florida" >Florida</a>, <a href="http://en.wikipedia.org/wiki/Idaho" title="Idaho" >Idaho</a> and <a href="http://en.wikipedia.org/wiki/Tennessee" title="Tennessee" >Tennessee</a>.</li>

<li ><b>Africa</b>: <a href="http://en.wikipedia.org/wiki/Morocco" title="Morocco" >Morocco</a>, mainly near <a href="http://en.wikipedia.org/wiki/Khouribga" title="Khouribga" >Khouribga</a> and <a href="http://en.wikipedia.org/wiki/Youssoufia" title="Youssoufia" >Youssoufia</a>; <a href="http://en.wikipedia.org/wiki/Senegal" title="Senegal" >Senegal</a>, <a href="http://en.wikipedia.org/wiki/Togo" title="Togo" >Togo</a>, <a href="http://en.wikipedia.org/wiki/Tunisia" title="Tunisia" >Tunisia</a> and <a href="http://en.wikipedia.org/wiki/Western_Sahara" title="Western Sahara" >Western Sahara</a>.</li>

<li ><b>Middle East</b>: <a href="http://en.wikipedia.org/wiki/Israel" title="Israel" >Israel</a>, <a href="http://en.wikipedia.org/wiki/Saudi_Arabia" title="Saudi Arabia" >Saudi Arabia</a>, <a href="http://en.wikipedia.org/wiki/Jordan" title="Jordan" >Jordan</a>, <a href="http://en.wikipedia.org/wiki/Iraq" title="Iraq" >Iraq</a>, at the town of <a href="http://en.wikipedia.org/wiki/Akashat" title="Akashat" >Akashat</a>, near to the Jordanian borders.</li>

<li ><b>Oceania</b>: <a href="http://en.wikipedia.org/wiki/Australia" title="Australia" >Australia</a>, <a href="http://en.wikipedia.org/wiki/Makatea" title="Makatea" >Makatea</a>, <a href="http://en.wikipedia.org/wiki/Nauru" title="Nauru" >Nauru</a>, <a href="http://en.wikipedia.org/wiki/Banaba_Island" title="Banaba Island" >Banaba Island</a>.</li>

</ul>

<p >In 2007, at the current rate of consumption, the supply of phosphorus was estimated to run out in 345 years.<sup id="cite_ref-5" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-5" >[6]</a></sup> However, some scientists now believe that a "<a href="http://en.wikipedia.org/wiki/Hubbert_peak_theory#Phosphorus" title="Hubbert peak theory" >Peak phosphorus</a>" will occur in 30 years and that "At current rates, reserves will be depleted in the next 50 to 100 years."<sup id="cite_ref-Lewis_6-0" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-Lewis-6" >[7]</a></sup>

Some phosphate rock deposits are notable for their inclusion of significant quantities of radioactive uranium isotopes. This syndrome is noteworthy because radioactivity can be released into surface waters<sup id="cite_ref-7" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-7" >[8]</a></sup> in the process of application of the resultant phosphate fertilizer (e.g. in many tobacco farming operations in the southeast USA).</p>

<h3 >[<a href="http://en.wikipedia.org/w/index.php?title=Phosphate&action=edit&section=4" title="Edit section: Ecology of phosphates" >edit</a>]Ecology of phosphates</h3>

<p >In ecological terms, because of its important role in biological systems, phosphate is a highly sought after resource. Once used, it is often a limiting nutrient in <a href="http://en.wikipedia.org/wiki/Environment_(biophysical)" title="Environment (biophysical)" >environments</a>, and its availability may govern the rate of growth of organisms. This is generally true of freshwater environments, whereas nitrogen is more often the limiting nutrient in marine (seawater) environments. Addition of high levels of phosphate to environments and to micro-environments in which it is typically rare can have significant ecological consequences. For example, blooms in the populations of some organisms at the expense of others, and the collapse of populations deprived of resources such as oxygen (see<a href="http://en.wikipedia.org/wiki/Eutrophication" title="Eutrophication" >eutrophication</a>) can occur. In the context of pollution, phosphates are one component of <a href="http://en.wikipedia.org/wiki/Total_dissolved_solids" title="Total dissolved solids" >total dissolved solids</a>, a major indicator of water quality.

Calcium hydroxyapatite and calcite precipitates can be found around bacteria in alluvial topsoil.<sup id="cite_ref-Schmittner_8-0" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-Schmittner-8" >[9]</a></sup> As clay minerals promote biomineralization, the presence of bacteria and clay minerals resulted in calcium hydroxyapatite and calcite precipitates.<sup id="cite_ref-Schmittner_8-1" class="reference" ><a href="http://en.wikipedia.org/wiki/Phosphates#cite_note-Schmittner-8" >[9]</a></sup>

<tr>

<td class="mbox-text" >Wikimedia Commons has media related to: <i><b><a class="external text" href="http://commons.wikimedia.org/wiki/Category:Phosphates" >Phosphates</a></b></i></td>

</tr>

</tbody></table>

<ul >

<li ><a href="http://en.wikipedia.org/wiki/Hypophosphite" title="Hypophosphite" >Hypophosphite</a> – H<sub >2</sub>PO<sub >2</sub><sup >-</sup></li>

<li ><a href="http://en.wikipedia.org/wiki/Organophosphorus" title="Organophosphorus" >Organophosphorus</a> compounds</li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphate_conversion_coating" title="Phosphate conversion coating" >Phosphate conversion coating</a></li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphine" title="Phosphine" >Phosphine</a> – PR<sub >3</sub></li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphine_oxide" title="Phosphine oxide" >Phosphine oxide</a> – OPR<sub >3</sub></li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphinite" title="Phosphinite" >Phosphinite</a> – P(OR)R<sub >2</sub></li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphonite" title="Phosphonite" >Phosphonite</a> – P(OR)<sub >2</sub>R</li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphite" title="Phosphite" >Phosphite</a> – P(OR)<sub >3</sub></li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphinate" title="Phosphinate" >Phosphinate</a> – OP(OR)R<sub >2</sub></li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphonate" title="Phosphonate" >Phosphonate</a> – OP(OR)<sub >2</sub>R</li>

<li >Phosphate — OP(OR)<sub >3</sub>, such as <a href="http://en.wikipedia.org/wiki/Triphenyl_phosphate" title="Triphenyl phosphate" >triphenyl phosphate</a></li>

<li ><a href="http://en.wikipedia.org/wiki/Polyphosphate" title="Polyphosphate" >Polyphosphate</a> – P<sub >n</sub>O<sub >3n+1</sub><sup >(n+2)-</sup></li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphorylation" title="Phosphorylation" >Phosphorylation</a></li>

<li ><a href="http://en.wikipedia.org/wiki/Pyrophosphate" title="Pyrophosphate" >Pyrophosphate</a> – P<sub >2</sub>O<sub >7</sub><sup >4-</sup></li>

<li ><a href="http://en.wikipedia.org/w/index.php?title=Phosphorus_oxoacids&action=edit&redlink=1" class="new" title="Phosphorus oxoacids (page does not exist)" >Phosphorus oxoacids</a></li>

<li ><a href="http://en.wikipedia.org/w/index.php?title=Phosphate_homeostasis&action=edit&redlink=1" class="new" title="Phosphate homeostasis (page does not exist)" >Phosphate homeostasis</a></li>

<li ><a href="http://en.wikipedia.org/wiki/Phosphogypsum" title="Phosphogypsum" >Phosphogypsum</a></li>

<li ><a href="http://en.wikipedia.org/wiki/Fertilizer" title="Fertilizer" >Fertilizer</a></li>

</ul>

</div>

<h2 >[<a href="http://en.wikipedia.org/w/index.php?title=Phosphate&action=edit&section=6" title="Edit section: References" >edit</a>]References</h2>

<li id="cite_note-0" ><b><a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-0" >^{</a></b> }<a rel="nofollow" class="external text" href="http://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=1061&loc=ec_rcs" >"Phosphates – PubChem Public Chemical Database"</a>. <i>The PubChem Project</i>. USA: National Center of Biotechnology Information.</li>

<li id="cite_note-PhosphatePrimer-1" >^ <a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-PhosphatePrimer_1-0" ><sup ><i><b>a</b></i></sup></a> <a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-PhosphatePrimer_1-1" ><sup ><i><b>b</b></i></sup></a> <a rel="nofollow" class="external text" href="http://fipr1.state.fl.us/PhosphatePrimer" >"Phosphate Primer"</a>.</li>

<li id="cite_note-Kuntz1-2" >^ <a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-Kuntz1_2-0" ><sup ><i><b>a</b></i></sup></a> <a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-Kuntz1_2-1" ><sup ><i><b>b</b></i></sup></a> Lynn A. Kuntz (June 2006). <a rel="nofollow" class="external text" href="http://www.foodproductdesign.com/articles/661ingredient2.html" >"Figuring Out Phosphates"</a>.</li>

<li id="cite_note-Kuntz2-3" >^ <a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-Kuntz2_3-0" ><sup ><i><b>a</b></i></sup></a> <a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-Kuntz2_3-1" ><sup ><i><b>b</b></i></sup></a> Lynn A. Kuntz (June 2006). <a rel="nofollow" class="external text" href="http://www.foodproductdesign.com/articles/661ingredient2.html" >"Food Product Design"</a>.</li>

<li id="cite_note-4" ><b><a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-4" >^{</a></b> }<a href="http://en.wikipedia.org/wiki/Neil_Campbell" title="Neil Campbell" >Campbell, Neil A.</a>; Reece, Jane B. (2005). <i>Biology</i> (Seventh ed.). San Francisco, California: Benjamin Cummings. pp. 65. <a href="http://en.wikipedia.org/wiki/International_Standard_Book_Number" title="International Standard Book Number" >ISBN</a> <a href="http://en.wikipedia.org/wiki/Special:BookSources/0-8053-7171-0" title="Special:BookSources/0-8053-7171-0" >0-8053-7171-0</a>.</li>

<li id="cite_note-5" ><b><a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-5" >^{</a></b> }"How Long Will it Last?". <i>New Scientist</i> <b>194</b> (2605): 38–9. May 26, 2007. <a href="http://en.wikipedia.org/wiki/Digital_object_identifier" title="Digital object identifier" >doi</a>:<a rel="nofollow" class="external text" href="http://dx.doi.org/10.1016%2FS0262-4079%2807%2961508-5" >10.1016/S0262-4079(07)61508-5</a>. <a href="http://en.wikipedia.org/wiki/International_Standard_Serial_Number" title="International Standard Serial Number" >ISSN</a> <a rel="nofollow" class="external text" href="http://www.worldcat.org/issn/0262" >4079 0262 4079</a>.</li>

<li id="cite_note-Lewis-6" ><b><a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-Lewis_6-0" >^{</a></b>&nbsp};Leo Lewis (2008-06-23). <a rel="nofollow" class="external text" href="http://business.timesonline.co.uk/tol/business/industry_sectors/natural_resources/article4193017.ece" >"Scientists warn of lack of vital phosphorus as biofuels raise demand"</a>. <a href="http://en.wikipedia.org/wiki/The_Times" title="The Times" >The Times</a>.</li>

<li id="cite_note-7" ><b><a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-7" >^{</a></b> C}.Michael Hogan. 2010. <a rel="nofollow" class="external text" href="http://www.eoearth.org/article/Water_pollution" ><i>Water pollution</i>. Encyclopedia of Earth</a>. eds. Mark McGinley and C. Cleveland. National Council for Science and the Environment. Washington DC.</li>

<li id="cite_note-Schmittner-8" >^ <a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-Schmittner_8-0" ><sup ><i><b>a</b></i></sup></a> <a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-Schmittner_8-1" ><sup ><i><b>b</b></i></sup></a> Schmittner KE, Giresse P (1999). "Micro-environmental controls on biomineralization: superficial processes of apatite and calcite precipitation in Quaternary soils, Roussillon, France".<i>Sedimentology</i> <b>46</b> (3): 463–76. <a href="http://en.wikipedia.org/wiki/Digital_object_identifier" title="Digital object identifier" >doi</a>:<a rel="nofollow" class="external text" href="http://dx.doi.org/10.1046%2Fj.1365-3091.1999.00224.x" >10.1046/j.1365-3091.1999.00224.x</a>.</li>

<li id="cite_note-9" ><b><a href="http://en.wikipedia.org/wiki/Phosphates#cite_ref-9" >^{</a></b> Gnandil}, K.; Tchangbedjil, G.; Killil, K.; Babal, G.; Abbel, E. (March). "The Impact of Phosphate Mine Tailings on the Bioaccumulation of Heavy Metals in Marine Fish and Crustaceans from the Coastal Zone of Togo". <i>Mine Water and the Environment</i> <b>25</b> (1): 56–62.<a href="http://en.wikipedia.org/wiki/Digital_object_identifier" title="Digital object identifier" >doi</a>:<a rel="nofollow" class="external text" href="http://dx.doi.org/10.1007%2Fs10230-006-0108-4" >10.1007/s10230-006-0108-4</a>.</li>

</ol>

</div>

<h2 >[<a href="http://en.wikipedia.org/w/index.php?title=Phosphate&action=edit&section=7" title="Edit section: External links" >edit</a>]External links</h2>

<ul >

<li ><a rel="nofollow" class="external text" href="http://mazamascience.com/Minerals/USGS" >US Minerals Databrowser</a> provides data graphics covering consumption, production, imports, exports and price for phosphate and 86 other minerals</li>

<li ><a rel="nofollow" class="external text" href="http://seekingalpha.com/article/182522-taking-stock-of-phosphorus-and-biofuels" >Taking Stock of Phosphorus and Biofuels</a>, global phosphate mining, use and shortages.</li>

</ul>

</div>