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sodium fluoride

 
Dictionary: sodium fluoride

n.
A colorless crystalline salt, NaF, used in fluoridation of water, in treatment of tooth decay, and as an insecticide and a disinfectant.


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Chemistry Dictionary: sodium fluoride
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A crystalline compound, NaF, soluble in water and very slightly soluble in ethanol; cubic; r.d. 2.56; m.p. 993°C; b.p. 1695°C. It occurs naturally as villiaumite and may be prepared by the reaction of sodium hydroxide or of sodium carbonate with hydrogen fluoride. The reaction of sodium fluoride with concentrated sulphuric acid may be used as a source of hydrogen fluoride. The compound is used in ceramic enamels and as a preservative agent for fermentation. It is highly toxic but in very dilute solution (less than 1 part per million) it is used in the fluoridation of water for the prevention of tooth decay on account of its ability to replace OH groups with F groups in the material of dental enamel.



Dental Dictionary: sodium fluoride
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n
NaF

A white, odorless powder used in 2% aqueous solution and applied topically to teeth as a caries-preventing agent; used as 33% NaF in kaolin and glycerin as a desensitizing agent for hypersensitive dentin. In drinking water, one part per million of NaF is used as a caries-prophylactic substance.

Drug Info: Sodium Fluoride
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Brand names: Flourigard®, Fluorinse®, Fluoritab®, Fluorodex®, Flura-Drops®, Flura-Tab®, Karidium®, Luride®, Pediaflor®, PreviDent®



Sodium Fluoride oral solution

What is sodium fluoride oral solution?

SODIUM FLUORIDE (Pediaflor®, Luride®, Fluoritab®, Flura-Drops®, Karidium®) is a mineral that strengthens tooth enamel and helps to prevent dental decay. Fluoride also helps to decrease sensitivity of the teeth. Fluoride, in small amounts, also helps maintain healthy bones. Most natural water supplies contain some fluoride and fluoride may be added to the water. Additional fluoride may be necessary in some cases. Generic sodium fluoride dental rinse is not available. Generic sodium fluoride oral solution is available.

What should I tell my health care provider before I take this medicine?

They need to know if you have any of these conditions:
• arthritic joints
• stomach or intestinal disease
• kidney disease
• stained, mottled, or pitted teeth
• an unusual or allergic reaction to fluoride, other medicines, foods, dyes, or preservatives
• pregnant or trying to get pregnant
• breast-feeding

How should I take this medicine?

Sodium fluoride oral solution is taken by mouth. Follow the directions on the prescription label. Drop the solution directly into the mouth using the dropper provided, or add to fruit juice or food that does not contain calcium. Do not take your medicine more often than directed.

Contact your pediatrician or health care professional regarding the use of this medicine in children. Special care may be needed.

What if I miss a dose?

If you miss a dose, take it as soon as you can. If it is almost time for your next dose, take only that dose. Do not take double or extra doses.

What drug(s) may interact with sodium fluoride?

• aluminum salts
• calcium salts
• magnesium salts

Tell your prescriber or health care professional about all other medicines you are taking, including non-prescription medicines, nutritional supplements, or herbal products. Also tell your prescriber or health care professional if you are a frequent user of drinks with caffeine or alcohol, if you smoke, or if you use illegal drugs. These may affect the way your medicine works. Check with your health care professional before stopping or starting any of your medicines.

What should I watch for while taking sodium fluoride?

Do not take this solution unless you are sure you need extra fluoride. Ask your dentist or health care professional for advice, especially if you move to a new area where the amount of fluoride in the water may be different.

Do not take calcium supplements, or antacids containing calcium, aluminum, or magnesium, at the same time as sodium fluoride. There should be an interval of at least 2 hours to make sure the sodium fluoride works properly.

Do not use glass containers for fluoride solutions; fluoride can etch the glass.

If more than the recommended amount of the oral solution is accidently swallowed, contact a Poison Control Center immediately. Also, prolonged daily ingestion can cause abnormal tooth enamel. Enamel is the hard part on the outside of the tooth. Immediately report any signs of abnormal tooth color or staining or spotting of the teeth.

What side effects may I notice from taking sodium fluoride?

Recommended doses of sodium fluoride produce few side effects. Serious side effects can occur with overuse of sodium fluoride and include:
• aches and pains in the bones or joints
• black, tarry stools
• blood in vomit
• mottled or discolored teeth
• nausea, vomiting
• skin rash, itching
• sores in the mouth or on the lips
• stomach pain
• unusual weakness
Call your prescriber or health care professional for advice if you get any of these side effects.

Where can I keep my medicine?

Keep out of the reach of children in a container that small children cannot open.

Store at room temperature between 15 and 30 degrees C (59 and 86 degrees F). Keep container tightly closed. Throw away any unused medicine after the expiration date.


Last updated: 3/12/2004 6:16:00 PM

Important Disclaimer: The drug information provided here is for educational purposes only. It is intended to supplement, not substitute for, the diagnosis, treatment and advice of a medical professional. This drug information does not cover all possible uses, precautions, side effects and interactions. It should not be construed to indicate that this or any drug is safe for you. Consult your medical professional for guidance before using any prescription or over the counter drugs.

Wikipedia: Sodium fluoride
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Sodium fluoride
Sodium fluoride
IUPAC name
Other names Florocid
Identifiers
CAS number 7681-49-4 Yes check.svgY
PubChem 5235
EC number 231-667-8
UN number 1690
RTECS number WB0350000
Properties
Molecular formula NaF
Molar mass 41.988713 g/mol
Appearance White solid
Odor odorless
Density 2.558 g/cm3
Melting point

993 °C

Boiling point

1695 °C

Solubility in water 4.13 g/100 g (25 °C)
Solubility soluble in HF
insoluble in ethanol
Hazards
MSDS Sodium fluoride MSDS
EU Index 009-004-00-7
EU classification Toxic (T)
Irritant (Xi)
R-phrases R25, R32, R36/38
S-phrases (S1/2), S22, S36, S45
NFPA 704
NFPA 704.svg
0
3
0
 
Flash point Non-flammable
LD50 52–200 mg/kg (oral in rats, mice, rabbits)[1]
Related compounds
Other anions Sodium chloride
Sodium bromide
Sodium iodide
Other cations Lithium fluoride
Potassium fluoride
Rubidium fluoride
Caesium fluoride
Related compounds TASF reagent
 Yes check.svgY (what is this?)  (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Sodium fluoride is the inorganic compound with the formula NaF. This colorless solid is a source of the fluoride ion in diverse applications. Sodium fluoride is less expensive and less hygroscopic than the related salt potassium fluoride.

Contents

Structure, general properties, occurrence

Sodium fluoride is an ionic compound, dissolving to give separated Na+ and F ions. It crystallizes in the cubic (sodium chloride) motif where both Na+ and F occupy octahedral coordination sites.[2][3]

The mineral form of NaF, villiaumite, is moderately rare. It is known from plutonic nepheline syenite rocks.[4]

Production

NaF is prepared by neutralizing hydrofluoric acid or hexafluorosilicic acid (H2SiF6), coproducts of the production of superphosphate fertilizer. Neutralizing agents include sodium hydroxide and sodium carbonate. Alcohols are sometimes used to precipitate the NaF:

HF + NaOH → NaF + H2O

From solutions containing HF, sodium fluoride precipitates as the bifluoride salt NaHF2. Heating the latter releases HF and gives NaF.

HF + NaF NaHF2

In a 1986 report, the annual, worldwide consumption of NaF was estimated to be several million tonnes.[5]

Applications

Sodium fluoride is sold in tablets for cavity prevention.

Fluoride salts are used to enhance the strength of teeth by the formation of fluorapatite, a naturally occurring component of tooth enamel. Originally, sodium fluoride was used to fluoridate water; however, hexafluorosilicic acid (H2SiF6) and its salt sodium hexafluorosilicate (Na2SiF6) are more commonly used additives, especially in the United States.[citation needed] Toothpaste often contains sodium fluoride to prevent cavities.[6]

Alternatively, sodium fluoride is used as a cleaning agent, e.g. as a "laundry sour."[5] A variety of specialty chemical applications exist in synthesis and extractive metallurgy. The fluoride is the reagent for the synthesis of fluorocarbons. Representative substrates include electrophilic chlorides including acyl chlorides, sulfur chlorides, and phosphorus chloride.[7] Like other fluorides, sodium fluoride finds use in desilylation in organic synthesis.

In medical imaging, fluorine-18-labelled sodium fluoride is used in positron emission tomography (PET). Relative to conventional bone scintigraphy carried out with gamma cameras or SPECT systems, PET offers more sensitivity and spatial resolution. A disadvantage of PET is that fluorine-18 labelled sodium fluoride is less widely available than conventional technetium-99m-labelled radiopharmaceuticals.

Sodium fluoride is used to conserve tissue samples in biochemistry and medicinal testing as fluoride ions stop glycolysis by inhibiting the enzyme enolase[citation needed]. Sodium fluoride is often used together with iodoacetic acid, which inhibits the enzyme aldolase[citation needed]. It also is used in RIPA lysis buffer as phosphatase inhibitor along with Na3VO4.

Safety

Sodium fluoride is classed as toxic by both inhalation (of dusts or aerosols) and ingestion.[8] In high enough doses, it has been shown to affect the heart and circulatory system, and the lethal dose for a 70 kg human is estimated at 5–10 g.[5]

See also

References

  1. ^ Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. p. 363. ISBN 1903996651. 
  2. ^ Wells, A.F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press. ISBN 0-19-855370-6. 
  3. ^ "Chemical and physical information" (PDF), Toxicological profile for fluorides, hydrogen fluoride, and fluorine, Agency for Toxic Substances and Disease Registry (ATDSR), September 2003, pp. 187, http://www.atsdr.cdc.gov/toxprofiles/tp11.pdf, retrieved 2008-11-01 
  4. ^ "Mineral Handbook" (PDF). Mineral Data Publishing. 2005. http://rruff.geo.arizona.edu/doclib/hom/villiaumite.pdf. 
  5. ^ a b c Aigueperse, Jean; Paul Mollard, Didier Devilliers, Marius Chemla, Robert Faron, Renée Romano, Jean Pierre Cuer (2005), "Fluorine Compounds, Inorganic", in Ullmann, Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a11_307 
  6. ^ "Sodium fluoride, Molecule of the week". American Chemical Society. 2008-02-19. http://portal.acs.org/portal/acs/corg/content?_nfpb=true&_pageLabel=PP_ARTICLEMAIN&node_id=841&content_id=WPCP_008239&use_sec=true&sec_url_var=region1. Retrieved 2008-11-01. 
  7. ^ Halpern, D.F. (2001), "Sodium Fluoride", Encyclopedia of Reagents for Organic Synthesis, John Wiley & Sons, doi:10.1002/047084289X.rs071 
  8. ^ http://www.jtbaker.com/msds/englishhtml/S3722.htm NaF MSDS

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Dictionary. The American Heritage® Dictionary of the English Language, Fourth Edition Copyright © 2007, 2000 by Houghton Mifflin Company. Updated in 2009. Published by Houghton Mifflin Company. All rights reserved.  Read more
Chemistry Dictionary. A Dictionary of Chemistry. Sixth Edition. Copyright © Market House Books Ltd, 2008. All rights reserved.  Read more
Dental Dictionary. Mosby's Dental Dictionary. Copyright © 2004 by Elsevier, Inc. All rights reserved.  Read more
Drug Info. Gold Standard. Copyright © 2008 by Gold Standard. All rights reserved.  Read more
Wikipedia. This article is licensed under the Creative Commons Attribution/Share-Alike License. It uses material from the Wikipedia article "Sodium fluoride" Read more