Sodium fluoride: Difference between revisions
Content deleted Content added
0.36 pounds changed to easier to parse 36 pence |
Erin.marie17 (talk | contribs) m i deleted it Tag: blanking |
||
| Line 1: | Line 1: | ||
{{Chembox |
|||
| Verifiedfields = changed |
|||
| Watchedfields = changed |
|||
| verifiedrevid = 464362396 |
|||
| Name = Sodium fluoride |
|||
| ImageFile = Sodium-fluoride-3D-ionic.png |
|||
| ImageName = Sodium fluoride |
|||
| pronounce ={{IPAc-en|ˌ|s|oʊ|d|i|ə|m|_|ˈ|f|l|ʊər|aɪ|d}}<ref>{{citation|last=Wells|first=John C.|year=2008|title=Longman Pronunciation Dictionary|edition=3rd|publisher=Longman|pages=313 and 755|isbn=9781405881180}}. According to this source, an alternative pronunciation of the second word is {{IPAc-en|ˈ|f|l|ɔr|aɪ|d}} and, in the UK, also {{IPAc-en|ˈ|f|l|uː|.|ə|r|aɪ|d}}.</ref> |
|||
| IUPACName = Sodium fluoride |
|||
| OtherNames = Florocid |
|||
|Section1={{Chembox Identifiers |
|||
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
|||
| ChemSpiderID = 5045 |
|||
| UNII_Ref = {{fdacite|correct|FDA}} |
|||
| UNII = 8ZYQ1474W7 |
|||
| InChI = 1/FH.Na/h1H;/q;+1/p-1 |
|||
| InChIKey = PUZPDOWCWNUUKD-REWHXWOFAH |
|||
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
|||
| StdInChIKey = PUZPDOWCWNUUKD-UHFFFAOYSA-M |
|||
| ChEMBL_Ref = {{ebicite|correct|EBI}} |
|||
| ChEMBL = 1528 |
|||
| CASNo = 7681-49-4 |
|||
| CASNo_Ref = {{cascite|correct|CAS}} |
|||
| RTECS = WB0350000 |
|||
| EINECS = 231-667-8 |
|||
| UNNumber = 1690 |
|||
| ChEBI_Ref = {{ebicite|correct|EBI}} |
|||
| ChEBI = 28741 |
|||
| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
|||
| StdInChI = 1S/FH.Na/h1H;/q;+1/p-1 |
|||
| PubChem = 5235 |
|||
| KEGG_Ref = {{keggcite|changed|kegg}} |
|||
| KEGG = C08142 |
|||
}} |
|||
|Section2={{Chembox Properties |
|||
| Formula = NaF |
|||
| MolarMass = 41.988173 g/mol |
|||
| Appearance = White to greenish solid |
|||
| Odor = odorless |
|||
| Density = 2.558 g/cm<sup>3</sup> |
|||
| Solubility = 36.4 g/L (0 °C);<BR /> 40.4 g/L (20 °C);<BR /> 50.5 g/L (100 °C)<ref>{{cite book | editor= Haynes, William M. | year = 2011 | title = [[CRC Handbook of Chemistry and Physics]] | edition = 92nd |
|||
| publisher = [[CRC Press]] | isbn = 1439855110|page=5.194}}</ref> |
|||
| SolubleOther = slightly soluble in [[hydrofluoric acid|HF]], [[ammonia]] <br> negligible in [[alcohol]], [[acetone]], [[sulfur dioxide|SO<sub>2</sub>]], [[dimethylformamide]] |
|||
| MeltingPtC = 993 |
|||
| BoilingPtC = 1704 |
|||
| VaporPressure = 1 mmHg @ 1077 C°<ref>Lewis, R.J. Sax's Dangerous Properties of Industrial Materials. 10th ed. Volumes 1–3 New York, NY: John Wiley & Sons Inc., 1999., p. 3248</ref> |
|||
| RefractIndex = 1.3252 |
|||
| MagSus = −16.4·10<sup>−6</sup> cm<sup>3</sup>/mol |
|||
}} |
|||
|Section3={{Chembox Structure |
|||
| MolShape = Octahedral |
|||
| CrystalStruct = Cubic |
|||
| LattConst_a = 462 pm |
|||
}} |
|||
|Section5={{Chembox Thermochemistry |
|||
| DeltaHf = -573.6 kJ/mol |
|||
| DeltaGf = -543.3 kJ/mol |
|||
| Entropy = 51.3 J/mol K |
|||
| HeatCapacity = 46.82 J/mol K |
|||
}} |
|||
|Section6={{Chembox Pharmacology |
|||
| ATCCode_prefix = A01 |
|||
| ATCCode_suffix = AA01 |
|||
| ATC_Supplemental = {{ATC|A12|CD01}},<br />{{ATC|V09|IX06}} ([[Fluorine-18|<sup>18</sup>F]]) |
|||
}} |
|||
|Section7={{Chembox Hazards |
|||
| ExternalSDS = <ref name="sigma">{{Sigma-Aldrich|id=450022|name=Sodium Fluoride|accessdate=2015-03-17}}</ref> |
|||
| HPhrases = {{H-phrases|301|315|319}}<ref name="sigma" /> |
|||
| NFPA-H = 3 |
|||
| NFPA-F = 0 |
|||
| NFPA-R = 0 |
|||
| FlashPt = Non-flammable |
|||
| LD50 = 52–200 mg/kg (oral in rats, mice, rabbits)<ref>{{Citation |author1=Martel, B. |author2=Cassidy, K. |title=Chemical Risk Analysis: A Practical Handbook |publisher=Butterworth–Heinemann |year=2004 |isbn=1-903996-65-1 |page=363}}</ref> |
|||
| PEL = TWA 2.5 mg/m<sup>3</sup><ref name=PGCH>{{PGCH|0563}}</ref> |
|||
| IDLH = 250 mg/m<sup>3</sup> (as F)<ref name=PGCH/> |
|||
| REL = TWA 2.5 mg/m<sup>3</sup><ref name=PGCH/> |
|||
}} |
|||
|Section8={{Chembox Related |
|||
| OtherAnions = [[Sodium chloride]]<br/>[[Sodium bromide]]<br/>[[Sodium iodide]]<br/>[[Sodium astatide]] |
|||
| OtherCations = [[Lithium fluoride]]<br/>[[Potassium fluoride]]<br/>[[Rubidium fluoride]]<br/>[[Caesium fluoride]]<br/>[[Francium fluoride]] |
|||
| OtherCompounds = [[TASF reagent]] |
|||
}} |
|||
}} |
|||
<!-- Definition and medical uses --> |
|||
'''Sodium fluoride''' ('''NaF''') is a [[chemical compound]] and medication.<ref name=Sp2008/><ref name=WHO2008/> As a medication it is primarily used to prevent [[tooth decay]] in children older than 6 months in areas where the [[drinking water]] is low in [[fluoride]].<ref name=WHO2008>{{cite book|title=WHO Model Formulary 2008|date=2009|publisher=World Health Organization|isbn=9789241547659|page=501-502|url=http://apps.who.int/medicinedocs/documents/s16879e/s16879e.pdf|accessdate= 8 January 2017}}</ref> Sodium fluoride is used as a liquid, pill, or paste by mouth with this use being known as [[fluoride therapy]].<ref name=BNF69/><ref>{{cite book|last1=Saha|first1=Ashok Kumar|title=Otology & Middle Ear Surgery|publisher=JP Medical Ltd|isbn=9789352501229|url=https://books.google.com/books?id=uVGqDAAAQBAJ&pg=PA194|language=en|year=2016}}</ref> |
|||
<!-- Side effects and mechanisms --> |
|||
Normal doses may occasionally result in [[dental fluorosis|white marks]] on the [[teeth]].<!-- <ref name=BNF69/> --> Excessive doses can result in brown or yellow coloring of the teeth.<ref name=BNF69>{{cite book|title=British national formulary : BNF 69|date=2015|publisher=British Medical Association|isbn=9780857111562|page=699-700|edition=69}}</ref> It is believed to work mostly through direct contact with the teeth.<ref name=WHO2008/> Sodium fluoride is a colorless solid.<!-- <ref name=Sp2008/> --> It is most often made by mixing [[fluorosilicic acid]] with [[sodium hydroxide]].<ref name=Sp2008/> |
|||
<!-- History and culture --> |
|||
Sodium fluoride came into use to prevent tooth decay in the 1940s.<ref>{{cite book|last1=Murray|first1=John J.|last2=Nunn|first2=June H.|last3=Steele|first3=James G.|title=The Prevention of Oral Disease|date=2003|publisher=OUP Oxford|isbn=9780192632791|page=53|url=https://books.google.com/books?id=3hG4UCQDr60C&pg=PA53|language=en}}</ref> It is on the [[World Health Organization's List of Essential Medicines]], the most important medications needed in a basic [[health system]].<ref name=WHO19th>{{cite web|title=WHO Model List of Essential Medicines (19th List)|url=http://www.who.int/medicines/publications/essentialmedicines/EML_2015_FINAL_amended_NOV2015.pdf?ua=1|work=World Health Organization|accessdate=8 December 2016|date=April 2015}}</ref> In the United Kingdom a typical month supply costs the [[NHS]] about 36 pence.<ref name=BNF69/> It is also commonly used for [[water fluoridation]] and added to [[toothpaste]].<ref name=Sp2008>{{cite book|last1=Spellman|first1=Frank R.|title=Handbook of Water and Wastewater Treatment Plant Operations, Second Edition|date=2008|publisher=CRC Press|isbn=9781420075304|page=131|edition=2|url=https://books.google.com/books?id=Ja28hvTxVpwC&pg=PA131|language=en}}</ref><ref name=BNF69/> An estimated 90 percent of toothpastes in the [[United States]] contains some type of fluoride.<ref>{{Cite book|url=https://books.google.com/books?id=-6RelfsQzr8C&pg=PA12|title=Review Of Fluoride: Benefits And Risks. Report Of The Ad Hoc Subcommittee On Fluoride|last=Company|first=DIANE Publishing|date=1992-09-30|publisher=DIANE Publishing|year=|isbn=9780788107290|location=|pages=12|language=en}}</ref> |
|||
==Uses== |
|||
[[Image:Sodium fluoride tablets.jpg|thumb|left|Sodium fluoride is sold in tablets for cavity prevention]] |
|||
===Dental caries=== |
|||
{{See also|Fluoride therapy|Water fluoridation}} |
|||
Fluoride salts are often added to municipal drinking water (as well as certain food products in some countries) for the purposes of maintaining dental health. The fluoride enhances the strength of teeth by the formation of [[fluorapatite]], a naturally occurring component of [[tooth enamel]].<ref>{{cite book|last1=Bourne|first1=volume editor, Geoffrey H.|title=Dietary research and guidance in health and disease|date=1986|publisher=Karger|location=Basel|isbn=3-8055-4341-7|page=153}}</ref><ref>{{cite book|last1=Jr|first1=Cornelis Klein, Cornelius S. Hurlbut,|title=Manual of mineralogy : (after James D. Dana)|date=1999|publisher=J. Wiley|location=New York|isbn=0-471-31266-5|edition=21st ed., rev.}}</ref><ref>{{cite journal|last1=Selwitz|first1=Robert H|last2=Ismail|first2=Amid I|last3=Pitts|first3=Nigel B|title=Dental caries|journal=The Lancet|date=January 2007|volume=369|issue=9555|pages=51–59|doi=10.1016/S0140-6736(07)60031-2|pmid=17208642}}</ref> Although sodium fluoride is used to [[Water fluoridation|fluoridate water]] and, indeed, is the standard by which other water-fluoridation compounds are gauged, [[hexafluorosilicic acid]] (H<sub>2</sub>SiF<sub>6</sub>) and its salt sodium hexafluorosilicate (Na<sub>2</sub>SiF<sub>6</sub>) are more commonly used additives in the U.S.<ref>{{Citation |url=http://cdc.gov/fluoridation/pdf/statistics/1992.pdf |format=PDF |title= Fluoridation census 1992 |author= Division of Oral Health, National Center for Prevention Services, CDC |year=1993 |accessdate=2008-12-29 |postscript=.}}</ref> [[Toothpaste]] often contains sodium fluoride to prevent [[dental caries|cavities]], although [[tin(II) fluoride]] is generally considered superior for this application.{{citation needed|reason=Source needed for the claim that tin(II) fluoride and sodium monofluorophosphate are superior for the prevention of cavities|date=October 2015}} |
|||
===Osteoporosis=== |
|||
Fluoride supplementation has been extensively studied for the treatment of postmenopausal [[osteoporosis]]. This supplementation does not appear to be effective; even though sodium fluoride increases bone density, it does not decrease the risk of fractures.<ref>{{cite journal|last1=Haguenauer|first1=D|last2=Welch|first2=V|last3=Shea|first3=B|last4=Tugwell|first4=P|last5=Wells|first5=G|title=Fluoride for treating postmenopausal osteoporosis.|journal=The Cochrane database of systematic reviews|date=2000|issue=4|pages=CD002825|pmid=11034769|doi=10.1002/14651858.CD002825}}</ref><ref>{{cite journal|last1=Vestergaard|first1=P|last2=Jorgensen|first2=NR|last3=Schwarz|first3=P|last4=Mosekilde|first4=L|title=Effects of treatment with fluoride on bone mineral density and fracture risk—a meta-analysis.|journal=Osteoporosis international : a journal established as result of cooperation between the European Foundation for Osteoporosis and the National Osteoporosis Foundation of the USA|date=March 2008|volume=19|issue=3|pages=257–68|pmid=17701094|doi=10.1007/s00198-007-0437-6}}</ref> |
|||
===Medical imaging=== |
|||
In medical imaging, [[fluorine-18]]-labelled sodium fluoride ([[United States Pharmacopeia|USP]], sodium fluoride F18) is one of the oldest tracers used in [[positron emission tomography]] (PET), having been in use since the 1960s.<ref>{{cite journal|last1=Blau|first1=Monte|last2=Ganatra|first2=Ramanik|last3=Bender|first3=Merrill A.|title=18F-fluoride for bone imaging|journal=Seminars in Nuclear Medicine|date=January 1972|volume=2|issue=1|pages=31–37|doi=10.1016/S0001-2998(72)80005-9}}</ref> Relative to conventional bone [[scintigraphy]] carried out with [[gamma camera]]s or [[SPECT]] systems, PET offers more sensitivity and spatial resolution. Fluorine-18 has a [[half-life]] of 110 min, which requires it to be used promptly once produced; this logistical limitation hampered its adoption in the face of the more convenient [[technetium-99m]]-labelled [[radiopharmaceutical]]s. However fluorine-18 is generally considered to be a superior radiopharmaceutical for skeletal imaging. In particular it has a high and rapid bone uptake accompanied by very rapid blood clearance, which results in a high bone-to-background ratio in a short time.<ref>{{cite journal|last1=Ordonez|first1=A. A.|last2=DeMarco|first2=V. P.|last3=Klunk|first3=M. H.|last4=Pokkali|first4=S.|last5=Jain|first5=S.K.|title=Imaging Chronic Tuberculous Lesions Using Sodium [18F]Fluoride Positron Emission Tomography in Mice.|journal=Molecular Imaging and Biology|date=October 2015|volume=17|issue=5|pages=609–614|doi=10.1007/s11307-015-0836-6}}</ref> Additionally the annihilation photons produced by decay of <sup>18</sup>F have a high energy of 511-keV compared to 140-keV photons of <sup>99m</sup>Tc.<ref>{{cite journal|last1=Grant|first1=F. D.|last2=Fahey|first2=F. H.|last3=Packard|first3=A. B.|last4=Davis|first4=R. T.|last5=Alavi|first5=A.|last6=Treves|first6=S. T.|title=Skeletal PET with 18F-Fluoride: Applying New Technology to an Old Tracer|journal=Journal of Nuclear Medicine|date=12 December 2007|volume=49|issue=1|pages=68–78|doi=10.2967/jnumed.106.037200|pmid=18077529}}</ref> |
|||
===Chemistry=== |
|||
Sodium fluoride has a variety of specialty chemical applications in synthesis and extractive [[metallurgy]]. It reacts with electrophilic chlorides including [[acyl chloride]]s, sulfur chlorides, and phosphorus chloride.<ref name=halpern>{{citation | last = Halpern | first = D.F. | contribution = Sodium Fluoride | title = Encyclopedia of Reagents for Organic Synthesis | year = 2001 | publisher = [[John Wiley & Sons]] | doi = 10.1002/047084289X.rs071| isbn = 0471936235 }}</ref> Like other fluorides, sodium fluoride finds use in [[desilylation]] in [[organic synthesis]]. Sodium fluoride can be used to produce [[fluorocarbon]]s via the [[Finkelstein reaction]]; this process has the advantage of being simple to perform on a small scale but is rarely used on an industrial scale due the existence of more effective techniques (e.g. [[Electrofluorination]], [[Fowler process]]). |
|||
===Other uses=== |
|||
Sodium fluoride is used as a cleaning agent (e.g., as a "laundry sour").<ref name=Aigueperse/> |
|||
Sodium fluoride is used as a stomach poison for plant-feeding insects. Inorganic fluorides such as [[fluorosilicates]] and sodium fluoride complex magnesium ions as [[magnesium fluorophosphate]]. They inhibit enzymes such as [[enolase]] that require Mg<sup>2+</sup> as a prosthetic group. Thus, fluoride poisoning prevents phosphate transfer in [[oxidative metabolism]].<ref>{{citation | author=Metcalf, Robert L. | contribution=Insect Control | title=[[Ullmann's Encyclopedia of Industrial Chemistry]] | edition=7th | publisher=Wiley | year=2007 | page=9}}</ref> |
|||
==Safety== |
|||
{{See also|Fluoride poisoning}} |
|||
Fluorides, particularly aqueous solutions of sodium fluoride, are rapidly and quite extensively absorbed.<ref name="fluorine">{{citation | author=Kapp, Robert | contribution=Fluorine | title=Encyclopedia of Toxicology | edition=2nd | volume=2 | publisher=Elsevier | year=2005 | pages=343–346}}</ref> |
|||
Fluorides interfere with electron transport and calcium metabolism. Calcium is essential for maintaining cardiac membrane potentials and in regulating coagulation. Large ingestion of fluoride salts or hydrofluoric acid may result in fatal [[arrhythmia]]s due to profound [[hypocalcemia]]. Chronic over-absorption can cause hardening of bones, calcification of ligaments, and buildup on teeth. Fluoride can cause irritation or corrosion to eyes, skin, and nasal membranes.<ref name="fluoride">{{citation | author=Greene Shepherd | contribution=Fluoride | title=Encyclopedia of Toxicology | edition=2nd | volume=2 | publisher=Elsevier | year=2005 | pages=342–343}}</ref> |
|||
The lethal dose for a 70 kg (154 lb) human is estimated at 5–10 g.<ref name=Aigueperse/> Sodium fluoride is classed as toxic by both [[inhalation]] (of dusts or aerosols) and [[ingestion]].<ref>[http://hazard.com/msds/mf/baker/baker/files/s3722.htm NaF MSDS]. hazard.com</ref> In high enough doses, it has been shown to affect the heart and circulatory system. For occupational exposures, the [[Occupational Safety and Health Administration]] and the [[National Institute for Occupational Safety and Health]] have established occupational exposure limits at 2.5 mg/m<sup>3</sup> over an eight-hour time-weighted average.<ref>[https://www.cdc.gov/niosh/npg/npgd0563.html CDC – NIOSH Pocket Guide to Chemical Hazards]</ref> |
|||
In the higher doses used to treat [[osteoporosis]], plain sodium fluoride can cause pain in the legs and incomplete stress fractures when the doses are too high; it also irritates the stomach, sometimes so severely as to cause ulcers. Slow-release and [[Enteric coating|enteric-coated]] versions of sodium fluoride do not have gastric side effects in any significant way, and have milder and less frequent complications in the bones.<ref>{{vcite journal |author=Murray TM, Ste-Marie LG |title=Prevention and management of osteoporosis: consensus statements from the Scientific Advisory Board of the Osteoporosis Society of Canada. 7. Fluoride therapy for osteoporosis |journal=CMAJ |volume=155 |issue=7 |pages=949–54 |year=1996 |pmid=8837545 |pmc=1335460 }}</ref> In the lower doses used for water fluoridation, the only clear adverse effect is [[dental fluorosis]], which can alter the appearance of children's teeth during [[tooth development]]; this is mostly mild and is unlikely to represent any real effect on aesthetic appearance or on public health.<ref>{{vcite book |url=http://nhmrc.gov.au/_files_nhmrc/file/publications/synopses/Eh41_Flouridation_PART_A.pdf |format=PDF |year=2007 |title=A systematic review of the efficacy and safety of fluoridation |author=National Health and Medical Research Council (Australia) |isbn=1-86496-415-4 }} Summary: {{vcite journal |author= Yeung CA |title= A systematic review of the efficacy and safety of fluoridation |journal= Evid Based Dent |volume=9 |issue=2 |pages=39–43 |year=2008 |pmid=18584000 |doi=10.1038/sj.ebd.6400578 |laysummary=http://nhmrc.gov.au/_files_nhmrc/file/media/media/rel07/Fluoride_Flyer.pdf |laydate=2007 |laysource=NHMRC }}</ref> A chronic fluoride ingestion of 1 ppm of fluoride in drinking water can cause [[mottling]] of the teeth (fluorosis) and an exposure of 1.7 ppm will produce mottling in 30–50 % of patients.<ref name="fluorine" /> |
|||
==Chemical structure== |
|||
Sodium fluoride is an [[ionic compound]], dissolving to give separated Na<sup>+</sup> and F<sup>−</sup> ions. Like [[sodium chloride]], it crystallizes in a cubic motif where both Na<sup>+</sup> and F<sup>−</sup> occupy [[Octahedral molecular geometry|octahedral coordination sites]];<ref name=wells>{{Citation | last = Wells | first = A.F. | year = 1984 | title = Structural Inorganic Chemistry | place = Oxford | publisher = [[Clarendon Press]] | isbn = 0-19-855370-6}}</ref><ref name=tp>{{citation | url = http://www.atsdr.cdc.gov/toxprofiles/tp11.pdf | format = PDF | contribution = Chemical and physical information | title = Toxicological profile for fluorides, hydrogen fluoride, and fluorine | pages = 187 | publisher = Agency for Toxic Substances and Disease Registry (ATDSR) | date = September 2003 | accessdate = 2008-11-01}}</ref> its lattice spacing, approximately 462 pm, is somewhat smaller than that of sodium chloride. |
|||
==Occurrence== |
|||
The [[mineral]] form of NaF, [[villiaumite]], is moderately rare. It is known from plutonic [[nepheline syenite]] rocks.<ref name=minhandbook>{{Citation | url = http://rruff.geo.arizona.edu/doclib/hom/villiaumite.pdf | format = PDF | title = Mineral Handbook |
|||
| year = 2005 | publisher = Mineral Data Publishing | issue = version 1 | postscript = .}}</ref> |
|||
==Production== |
|||
NaF is prepared by neutralizing [[hydrofluoric acid]] or [[hexafluorosilicic acid]] (H<sub>2</sub>SiF<sub>6</sub>), byproducts of the reaction of fluorapatite (Ca<sub>5</sub>(PO<sub>4</sub>)<sub>3</sub>F) from [[phosphate rock]] during the production of [[superphosphate]] fertilizer. Neutralizing agents include [[sodium hydroxide]] and [[sodium carbonate]]. Alcohols are sometimes used to precipitate the NaF: |
|||
:HF + NaOH → NaF + H<sub>2</sub>O |
|||
From solutions containing HF, sodium fluoride precipitates as the [[bifluoride]] salt NaHF<sub>2</sub>. Heating the latter releases HF and gives NaF. |
|||
:HF + NaF ⇌ NaHF<sub>2</sub> |
|||
In a 1986 report, the annual worldwide consumption of NaF was estimated to be several million tonnes.<ref name=Aigueperse>{{citation | first1 = Jean | last1 = Aigueperse | first2 = Paul | last2 = Mollard | first3 = Didier | last3 = Devilliers | first4= Marius | last4 = Chemla | first5 = Robert | last5 = Faron | first6 = Renée | last6 = Romano | first7 = Jean Pierre | last7 = Cuer | contribution = Fluorine Compounds, Inorganic | editor-last = Ullmann | title = Encyclopedia of Industrial Chemistry | year = 2005 | publisher = Wiley-VCH | place = Weinheim|doi = 10.1002/14356007.a11_307| isbn = 3527306730 }}</ref> |
|||
== See also == |
|||
{{Commons category}} |
|||
* [[Cryolite]] |
|||
==References== |
|||
{{reflist|30em}} |
|||
{{Sodium compounds}} |
|||
{{Stomatological preparations}} |
|||
{{Mineral supplements}} |
|||
{{fluorine compounds}} |
|||
{{Authority control}} |
|||
{{DEFAULTSORT:Sodium Fluoride}} |
|||
[[Category:Fluorides]] |
|||
[[Category:Metal halides]] |
|||
[[Category:Alkali metal fluorides]] |
|||
[[Category:Sodium compounds]] |
|||
[[Category:Dental drugs]] |
|||