PRODUCTS

SODIUM FLUORIDE

Sodium fluoride is also used in metallurgy and in medical imaging.
Sodium fluoride is used as a cleaning agent (e.g., as a "laundry sour").
Sodium fluoride can be used in a nuclear molten-salt reactor, which sodium fluoride is used as the reactor's coolant.

CAS Number: 7681-49-4
EC (EINECS) Number: 231-667-8
Molecular Formula: NaF
Molecular Weight: 41.99 g/mol

SYNONYMS:
Sodium fluoride, Florocid, sodium fluoride, 7681-49-4, Fluoride, sodium, Sodium fluoride (NaF), Florocid, Pergantene, Zymafluor, Pediaflor, Ossin, Sodium flouride, Fluonatril, Fluorident, Sodium monofluoride, Villiaumite, Antibulit, Floridine, Fluoraday, Fluorol, Flursol, Karidium, Koreberon, Liquiflur, Ossalin, Xaridium, Flura, Luride, Roach salt, Flura Drops, T-Fluoride, Fungol B, Sodium hydrofluoride, Chemifluor, Flozenges, Fluorigard, Fluorineed, Fluorinse, Fluoritab, Fluorocid, Flurcare, Gelution, Iradicav, Lemoflur, Pedident, Pennwhite, Studafluor, Karigel, Nafeen, Nufluor, Predent, Rafluor, Credo, Gleem, Fluorid sodny, Sodium fluorure, Rescue squad, Alcoa sodium fluoride, NaFpak, Cavi-trol, Flura-gel, Flura-loz, Kari-rinse, Na frinse, Natrium fluoride, Point two, Super-dent, Thera-flur, Neutra Care, Minute-Gel, Luride lozi-tabs, Phos-Flur, Stay-Flo, Fluor-O-kote, Luride SF, Luride-SF, Thera-flur-N, Lea-Cov, Fluorure de sodium, SO-Flo, Trisodium trifluoride, Dentalfluoro, Sodium fluoride (Na2F2), F1-Tabs, Zooby, Sodium fluoride cyclic dimer, Natrum fluoratum, GEL II, NCI-C55221, FDA 0101, Sodium fluoride, solid (DOT), Natrii fluoridum, Fluor-A-day, NSC-77385, DTXSID2020630, Fluoride (as sodium), Neutral Sodium Fluoride, 8ZYQ1474W7, Fluoride (as sodium fluoride), CHEBI:28741, NSC77385, Fluoristats, SODIUM FLUORIDE [WHO-DD], SODIUM FLUORIDE [WHO-IP], HY-B1766, SODIUM FLUORIDE [ORANGE BOOK], AKOS024438093, FLUORIDE (AS SODIUM) [VANDF], SODIUM FLUORIDE [EP MONOGRAPH], CS-5131, DB09325, SODIUM FLUORIDE [USP MONOGRAPH], NATRII FLUORIDUM [WHO-IP LATIN], Sodium fluoride [UN1690] [Poison], Sodium fluoride, 99.995% (metals basis), NS00076215, COLGATE TOTAL COMPONENT SODIUM FLUORIDE, FLUORIDE (AS SODIUM FLUORIDE) [VANDF], C08142, D00943, P00019, Sodium Fluoride, Trace metals grade, 99.99%, A838842, Q407520, Sodium fluoride, NaF, Sodium monofluoride, Natrium fluoride, Florocid, Floridine, Fluorident, Fluorigard, Villiaumite, Disodium difluoride, Sodium hydrofluoride, Trisodium trifluoride, Cavi-trol, Chemifluor, Credo, Alcoa sodium fluoride

Sodium fluoride is a colorless crystalline solid or white powder, or the solid dissolved in a liquid.
Sodium fluoride is soluble in water.
Sodium fluoride is noncombustible.

Sodium fluoride is corrosive to aluminum.
Sodium fluoride solution appears as an aqueous solution.
Sodium fluoride is odorless.

The maximum solubility of sodium fluoride in water at room temperature is 4.2 g per 100 g of water.
Sodium fluoride is a metal fluoride salt with a Na(+) counterion.
Sodium fluoride has a role as a mutagen.

Sodium fluoride (NaF) is an inorganic, white crystalline salt widely used in dentistry to prevent tooth decay by strengthening enamel, and in water fluoridation.
Sodium fluoride is also used as an insecticide, in wood preservatives, and in metallurgical processes.

While beneficial for dental health, high exposure can lead to toxicity, and Sodium fluoride should be handled with caution.
Sodium fluoride is an inorganic ionic compound composed of sodium (Na⁺) and fluoride (F⁻) ions.
Sodium fluoride is commonly found as a white crystalline solid and is widely used in dental care products, water fluoridation, metallurgy, pesticides, and chemical synthesis due to its ability to supply fluoride ions.

Sodium fluoride (NaF) is an inorganic compound with the formula NaF.
Sodium fluoride is a colorless or white solid that is readily soluble in water.
In 2023, Sodium fluoride was the 264th most commonly prescribed medication in the United States, with more than 1 million prescriptions.

Sodium fluoride, NaF, is a white, odourless powder (or crystals), supplied in 25 kg bags.
Sodium fluoride is easily soluble in water, and the solubility varies little with temperature.
Sodium fluoride has a specific gravity of 2.78 at 20°C.

The typical commercial grade of sodium fluoride is 97% purity, with about 44% fluorine.
Sodium fluoride has a bulk density of 1040–1440 kg/m³.
The pH of a 1% solution is 6.5; that of a 4% solution is 7.6.

Suitable materials for handling sodium fluoride include iron, steel, fibreglass-reinforced plastic and polyethylene.
Sodium fluoride is an inorganic chemical compound that is a source of the fluoride ion in many applications, including dental care and radiographic imaging when it is used as [Fluoride ion F-18].

Sodium fluoride's benefits on dental health were first observed in the 1930s, when individuals in communities with fluoridated drinking water showed less tooth decay than those without fluoridated water.
The use of fluoride in dental practice began in the 1940s.

Now, sodium fluoride may be found in a variety of gels, varnishes, rinses, toothpaste products, and fluoride treatments provided in dental care.
According to the American Dental Association (ADA), thorough evidence reviews have indicated that the use of fluoride to prevent and control dental caries is safe when used correctly and is highly effective in reducing the prevalence of caries.

Sodium Fluoride is an inorganic salt of fluoride used topically or in municipal water fluoridation systems to prevent dental caries.
Fluoride appears to bind to calcium ions in the hydroxyapatite of surface tooth enamel, preventing corrosion of tooth enamel by acids.
This agent may also inhibit acid production by commensal oral bacteria.

Sodium fluoride is a source of inorganic fluoride which is used topically to prevent dental caries.
Sodium Fluoride is a naturally occurring mineral that serves to protect teeth from dental caries.
Sodium fluoride is scientifically proven that the correct amount of fluoride in water and use of fluoride-containing toothpastes and mouth rinses have a significant benefit on oral health and help to reduce tooth decay.

Fluoride helps promote remineralisation of the tooth surface.
Fluoride ions are taken up into the enamel and form fluoroapatite which is harder than hydroxyapatite.
Thus, fluoride strengthens the enamel which is then more resistant to acid attacks and the incidence of dental caries is reduced.

USES and APPLICATIONS of SODIUM FLUORIDE:
Sodium fluoride is used as an insecticide.
Sodium fluoride is also used to fluorinate water supplies, as a wood preservative, in cleaning compounds, manufacture of glass, and for many other uses.

In addition to its electrolytic use in electroplating baths, Sodium fluoride is also used in the leather industry as a pest control and insecticide.
Sodium fluoride has applications in the textile industry, polymerization, and the cosmetics industry.

Sodium hydrogen difluoride is used in anatomical and zoological specimens, metal plating, and many other applications.
Sodium fluoride is used in the following products: textile processing products and dyes, and cosmetics and personal care products.

Metal, wood and plastic building and building materials, flooring, furniture, toys, building materials, curtains, shoes, leather products, paper and cardboard products, electronic equipment, machine washes/detergents, automotive care products, paints, coatings or adhesives.
Sodium fluoride is used in fragrances and air fresheners.

Sodium fluoride is a medication used in a variety of dental products to support strong teeth and help prevent cavities.
Sodium fluoride is an inorganic chemical compound that is a source of the fluoride ion in many applications, including dental care and radiographic imaging when it is used as Fluoride ion F-18.

Sodium fluoride is an inorganic chemical compound that, when used as Fluoride ion F-18, is a source of fluoride ions in many applications, including dental care and radiographic imaging.
Public Health Applications of Sodium fluoride: Drinking water fluoridation programs to reduce tooth decay.

Industrial Uses of Sodium fluoride: Aluminum production, Metallurgical flux, Glass etching and frosting, Ceramics manufacturing, Chemical intermediate for fluorine compounds.
Agricultural Uses of Sodium fluoride: Insecticides, Rodenticides, Wood preservatives (historically).

Laboratory Uses of Sodium fluoride: Analytical reagent, Source of fluoride ions in chemical synthesis, Biochemistry studies as enzyme inhibitor.
Sodium fluoride is used in trace amounts in the fluoridation of drinking water to prevent tooth decay, and in toothpastes and topical pharmaceuticals for the same purpose.

Sodium fluoride prevents and treats low fluoride levels in your body.
Sodium fluoride may also be used to prevent tooth decay or cavities.
Sodium fluoride works by making your teeth stronger.

Fluoride is a mineral that plays an important role in the health of your teeth and bones.
Sodium fluoride may be used for other purposes; ask your health care provider or pharmacist if you have questions.

Sodium fluoride is widely used as fluxing and opacifying agent in the manufacture of colours, frites and enamels, for wood preservation, mineral flotation processes, metal surface treatments in the aluminium industry, the manufacture of glue and adhesives, glass glazing, water fluoridation, chemical synthesis, and the manufacture of sodium monophosphate.

Beyond its dental applications, sodium fluoride also has industrial uses, such as in the production of aluminum, glass, and other materials.
However, Sodium fluoride's widespread use in water fluoridation has been a topic of extensive research and debate.
The addition of sodium fluoride to public water supplies aims to reduce the prevalence of dental caries at the population level.

In conclusion, the mechanism of sodium fluoride involves the transformation of hydroxyapatite into fluorapatite, enhancing remineralization, and exerting antimicrobial effects.
These actions collectively contribute to Sodium fluoride's effectiveness in preventing dental caries and maintaining oral health.

Understanding these mechanisms allows for informed decisions regarding the use and implications of sodium fluoride in various applications.
Sodium fluoride can be used in solution feed systems at a strength of 1–2%, or in a saturator system where water is passed through a bed of sodium fluoride crystals, thus producing a saturated solution.

The water used for dissolving sodium fluoride should not have a hardness greater than 75 mg/L (as calcium carbonate, CaCO3), because the presence of calcium and magnesium causes the formation of insoluble fluorides which may cause clogging problems.
When using sodium fluoride, it is good practice to add the chemical after drinking water has been treated, because fluoride ions may be adsorbed onto the surfaces of suspended matter in water.

-Typical use in Australian drinking water treatment:
Sodium fluoride is used to artificially fluoridate water, to reduce the occurrence of dental caries.
In each State and Territory, except for South Australia, the fluoridation of drinking water is regulated by an Act of Parliament; New South Wales and Queensland also have regulations in force.

-Osteoporosis uses of Sodium fluoride:
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.

-Medical imaging uses of Sodium fluoride:
In medical imaging, fluorine-18-labelled sodium fluoride (USP, sodium fluoride Na18F) is one of the oldest tracers used in positron emission tomography (PET), having been in use since the 1960s.
Relative to conventional bone scintigraphy carried out with gamma cameras 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 radiopharmaceuticals.
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.
Additionally the annihilation photons produced by decay of 18F have a high energy of 511 keV compared to the 140 keV photons of 99mTc.

-Chemistry uses of Sodium fluoride:
Sodium fluoride has a variety of specialty chemical applications in synthesis and extractive metallurgy.
Sodium fluoride reacts with electrophilic chlorides including acyl chlorides, sulfur chlorides, and phosphorus chloride.
Like other fluorides, sodium fluoride finds use in desilylation in organic synthesis.

Sodium fluoride can be used to produce fluorocarbons 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 to the existence of more effective techniques (e.g. Electrofluorination, Fowler process).

-Biology uses of Sodium fluoride:
Sodium fluoride is sometimes added at relatively high concentrations (~20 mM) to protein lysis buffers in order to inhibit endogenous phosphatases and thereby protect phosphorylated protein sites.
Sodium pyrophosphate and Sodium orthovanadate are also used for this purpose.

-Insecticide uses of Sodium fluoride:
Inorganic fluorides such as fluorosilicates and sodium fluoride complex magnesium ions as magnesium fluorophosphate.
They inhibit enzymes that require Mg2+ as a prosthetic group.

In cases of fluoride poisoning, phosphate transfer in oxidative metabolism is prevented.
Sodium fluoride, patented as an insecticide in 1896, was commonly used through the 1970s on ants and other domestic pests, and as a stomach poison for plant-feeding insects.

-Dental caries uses of Sodium fluoride:
Fluoride salts are often added to municipal drinking water (as well as to certain food products in some countries) for the purpose of maintaining dental health.

The fluoride enhances the strength of teeth by the formation of fluorapatite, a naturally occurring component of tooth enamel.
Although sodium fluoride is used to fluoridate water and is the standard by which other water-fluoridation compounds are gauged, hexafluorosilicic acid (H2SiF6) and its salt sodium hexafluorosilicate (Na2SiF6) are more commonly used additives in the United States.

-Common Uses of Sodium fluoride:
Oral Hygiene: Toothpastes and rinses.
Water Treatment: Municipal water fluoridation.
Industrial: Glass manufacturing, cleaning compounds, and insecticides.

-Uses / Applications of Sodium fluoride:
*Dental and Medical Uses:
Toothpaste formulations.
Mouth rinses.
Professional dental treatments.
Prevention of dental caries (tooth decay).
Fluoride ions help strengthen tooth enamel and increase resistance to acid attack from bacteria.

KEY ASPECTS OF SODIUM FLUORIDE:
*Health Benefits:
Sodium fluoride promotes remineralization of tooth enamel and inhibits acid production by oral bacteria, effectively preventing dental caries.
Sodium fluoride is used in toothpaste, varnishes, and drinking water.

*Medical Use:
Besides dental care, Sodium fluoride has been investigated for treating osteoporosis, as it can stimulate new bone formation, although it is not standard, approved therapy for this in the U.S.

*Safety Precautions:
Sodium fluoride is corrosive to aluminum.

*Environmental/Industrial Usage:
Sodium fluoride is used as a wood preservative and in manufacturing, as well as an insecticide.

BENEFITS of SODIUM FLUORIDE:
*Dental Health Benefits:
Strengthens tooth enamel.
Prevents dental caries.
Promotes remineralization of teeth.
Reduces bacterial acid damage.

*Industrial Benefits:
Improves metal processing efficiency.
Enhances glass etching processes.
Useful reagent in fluorination chemistry.

*Public Health Benefits:
Cost-effective prevention of tooth decay.
Reduced dental disease in populations with fluoridated water.

CHEMICAL STRUCTURE of SODIUM FLUORIDE:
Sodium fluoride is an inorganic ionic compound, dissolving in water to give separated Na+ and F− ions.
Like sodium chloride, Sodium fluoride crystallizes in a cubic motif where both Na+ and F− occupy octahedral coordination sites; its lattice spacing, approximately 462 pm, is smaller than that of sodium chloride (564 pm).

OCCURRENCE of SODIUM FLUORIDE:
The mineral form of Sodium fluoride, villiaumite, is moderately rare.
Sodium fluoride is known from plutonic nepheline syenite rocks.

PRODUCTION of SODIUM FLUORIDE:
Sodium fluoride is prepared by neutralizing hydrofluoric acid or hexafluorosilicic acid (H2SiF6), both byproducts of the reaction of fluorapatite (Ca5(PO4)3F) 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 + H2O
From solutions containing HF, sodium fluoride precipitates as the bifluoride salt sodium bifluoride (NaHF2).
Heating the latter releases HF and gives Sodium fluoride.

HF + NaF ⇌ NaHF2
In a 1986 report, the annual worldwide consumption of Sodium fluoride was estimated to be several million tonnes.

RELATED COMPOUNDS of SODIUM FLUORIDE:
***Other anions
Sodium chloride
Sodium bromide
Sodium iodide
Sodium astatide

***Other cations
Lithium fluoride
Potassium fluoride
Rubidium fluoride
Caesium fluoride
Francium fluoride

***Related compounds
TASF reagent

WHAT DOES SODIUM FLUORIDE DO?
Sodium fluoride in toothpaste and mouthwash safely and effectively helps to prevent tooth decay, when formulated correctly and used as directed.
Fluoride helps diminish demineralization of tooth enamel and enhances the remineralization of potential weak spots, strengthening the enamel.

PHYSICAL AND CHEMICAL PROPERTIES of SODIUM FLUORIDE:
Sodium fluoride is a colorless crystalline solid, a white powder, or a solid dissolved in a liquid.
Sodium fluoride is odorless and has a salty taste.
Sodium fluoride, or fluoride, is a naturally occurring mineral.
However, it's not as harmless a chemical as we might think.

The higher the amount of fluoride, the greater the harm.
Fluoride is added to drinking water in some countries.
Although fluoride is not added to drinking water in our country, it is naturally present in some tap water supplies.

High doses of sodium fluoride can cause conditions such as intellectual disability and cancer in children.
Fluoride is the most potent known rat poison.
It's undeniable that fluoride is a poison.

Sodium fluoride, most commonly used in toothpaste, is unfortunately also found in children's toothpaste despite its never-approved formula.
Sodium fluoride is now present in everything we eat, drink, creams, shampoos, and even our clothing.
Normally, fluoride is an important element in its natural state; man-made fluoride is sodium fluoride.

Sodium fluoride is highly absorbed from the intestines.
Sodium fluoride negatively affects the biological development of children.
There is no definitive evidence that sodium fluoride, which we use most often through toothpaste, prevents tooth decay.

Sodium fluoride weakens the immune system and reduces the body's resistance to infections.
Sodium fluoride seriously damages the reproductive system, delaying the eruption of permanent teeth.
25% of tranquilizers contain sodium fluoride.

CHEMICAL CHARACTERISTICS of SODIUM FLUORIDE:
*Simple inorganic salt.
*Strong electrolyte in aqueous solution.
*Provides fluoride ions in solution.
*High thermal stability.
*Crystallizes in face-centered cubic structure similar to sodium chloride.
*Slightly alkaline in water.
*Stable under normal environmental conditions.

FUNCTIONAL PROPERTIES of SODIUM FLUORIDE:
*Sodium fluoride acts as:
Fluoride ion source.
Enamel strengthening agent.
Anticaries agent.
Flux in metallurgical processes.
Chemical reagent in synthesis.
Enzyme inhibitor in biochemical studies.

WHAT IS THE MECHANISM OF SODIUM FLUORIDE?
Sodium fluoride (NaF) is a compound that has garnered significant attention due to its widespread use in dental care products, water fluoridation, and various industrial applications.

Understanding the mechanism of sodium fluoride is essential for appreciating its effectiveness and potential impacts on health and the environment.
Sodium fluoride works primarily through its interaction with the mineral components of teeth, predominantly hydroxyapatite, which is a crystalline structure composed of calcium and phosphate.

When sodium fluoride is applied topically through toothpaste, mouth rinses, or professional treatments, it undergoes a series of exchanges with the enamel surface.
One of the key mechanisms is the conversion of hydroxyapatite into fluorapatite.
Fluorapatite is more resistant to acid dissolution than hydroxyapatite.

This transformation occurs as fluoride ions from sodium fluoride replace hydroxyl groups in the hydroxyapatite structure, forming a more stable and less soluble fluorapatite.
This process reduces the enamel’s susceptibility to acid attacks from bacterial metabolism, a primary cause of dental caries.

Furthermore, sodium fluoride enhances remineralization, which is the natural process of replenishing minerals in enamel that have been lost due to acid erosion.
When fluoride is present in the oral environment, Sodium fluoride facilitates the uptake of calcium and phosphate ions into the demineralized areas of enamel, effectively repairing and strengthening the tooth structure.

This remineralization process not only arrests the progression of early carious lesions but also reinforces the enamel against future acid challenges.
In addition to its direct benefits on enamel, sodium fluoride also exerts antimicrobial effects.

Fluoride ions can inhibit the enzymatic activity of bacteria, particularly Streptococcus mutans, which is a major contributor to tooth decay.
By disrupting bacterial glycolysis, fluoride reduces the production of acidic byproducts that demineralize enamel.
This antimicrobial action further contributes to the overall caries-preventive effect of sodium fluoride.

CHEMISTRY of SODIUM FLUORIDE:
Sodium fluoride is produced by neutralising hydrofluoric acid with either sodium carbonate or sodium hydroxide.
The dissolution of sodium fluoride in water forms fluoride ions (F−) and sodium ions (Na+) as follows:
NaF↔Na+ + F−

WHAT'S THE DIFFERENCE BETWEEN STANNOUS FLUORIDE AND SODIUM FLUORIDE?
Stannous fluoride is an anti-bacterial agent that's clinically proven to protect against gingivitis, plaque and tooth sensitivity, while still providing the trusted cavity protection you expect from Crest.
Although sodium fluoride protects against cavities, it doesn't provide protection from these other conditions.

PHYSICAL and CHEMICAL PROPERTIES of SODIUM FLUORIDE:
Chemical Name: Sodium Fluoride
CAS Number: 7681-49-4
EC (EINECS) Number: 231-667-8
Molecular Formula: NaF
Molecular Weight: 41.99 g/mol
Chemical Classification: Inorganic fluoride salt
Chemical Family: Alkali metal fluoride
Appearance: White crystalline powder or colorless crystals
Physical State: Solid
Odor: Odorless
Color: White to off-white
Molecular Weight: 41.99 g/mol

Density: 2.55–2.78 g/cm³
Specific Gravity: ~2.558
Melting Point: 993 °C
Boiling Point: ~1700–1704 °C
Refractive Index: 1.336
Vapor Pressure: 1.4 mm Hg (0 °C)
Crystal Structure: Cubic (NaCl-type structure)
Hygroscopicity: Slightly hygroscopic
Flash Point: Not considered flammable
Storage Temperature: Room temperature or 2–8 °C recommended
Physical Form: Crystalline powder or granules

Partition Coefficient: No significant data
Chemical Formula: NaF
Ionic Composition: Sodium cation (Na⁺) and fluoride anion (F⁻)
Bond Type: Ionic bonding
Water Solubility: About 4 g / 100 mL at 25 °C
Solubility in Organic Solvents: Poorly soluble
pH (aqueous solution): Approximately 7.0 – 10.0
Stability: Stable under normal conditions
Reactivity:
Reacts with strong acids to produce hydrogen fluoride (HF) gas
Incompatible with strong acids and glass under certain conditions

Hydrolysis: Slight hydrolysis in aqueous solution
Decomposition: May produce toxic fluoride fumes when heated strongly
Chemical formula: NaF
Molar mass: 41.988173 g/mol
Appearance: White to greenish solid
Odor: odorless
Density: 2.558 g/cm3
Melting point: 993 °C (1,819 °F; 1,266 K)
Boiling point: 1,704 °C (3,099 °F; 1,977 K)
Solubility in water: 36.4 g/L (0 °C)
40.4 g/L (20 °C)
50.5 g/L (100 °C)

Solubility: slightly soluble in HF, ammonia
negligible in alcohol, acetone, SO2, dimethylformamide
Vapor pressure: 1 mmHg @ 1077 °C
Acidity (pKa): 3,20 (weak base, see HF)
Magnetic susceptibility (χ): −16.4·10−6 cm3/mol
Refractive index (nD): 1.3252
Structure
Crystal structure: Cubic
Lattice constant: a = 462 pm
Molecular shape: Octahedral

Thermochemistry
Heat capacity (C): 46.82 J/(mol K)
Std molar entropy (S⦵298): 51.3 J/(mol K)
Std enthalpy of formation (ΔfH⦵298): −573.6 kJ/mol
Gibbs free energy (ΔfG⦵): −543.3 kJ/mol
CAS number: 7681-49-4
EC index number: 009-004-00-7
EC number: 231-667-8
Grade: ACS, ISO, Reag. Ph Eur
Hill Formula: FNa
Chemical formula: NaF
Molar Mass: 41.98 g/mol

HS Code: 2826 19 10
Density: 2.8 g/cm3 (20 °C)
Melting Point: 996 °C
pH value: 10.2 (40 g/l, H₂O, 20 °C)
Vapor pressure: 1 hPa (1077 °C)
Solubility: 42 g/l soluble
Physical state: crystalline
Color: white
Odor: No data available
Melting point/ range: 993 °C
Initial boiling point and boiling range: 1.704 °C
Flammability (solid, gas): No data available

Upper/lower flammability or explosive limits: No data available
Flash point: Not applicable
Autoignition temperature: No data available
Decomposition temperature: No data available
pH: No data available
Viscosity, kinematic: No data available
Viscosity, dynamic: No data available
Water solubility: No data available
Partition coefficient: Not applicable for inorganic substances
Vapor pressure: 1,9 hPa
Density: 2,780 g/cm3

Relative density: No data available
Relative vapor density: No data available
Particle characteristics: No data available
Explosive properties: Not classified as explosive
Oxidizing properties: none
Other safety information: No data available
Molecular Weight: 41.9881724 g/mol
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 1
Rotatable Bond Count: 0
Exact Mass: 41.98817244 Da

Monoisotopic Mass: 41.98817244 Da
Topological Polar Surface Area: 0 Å²
Heavy Atom Count: 2
Formal Charge: 0
Complexity: 2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes

FIRST AID MEASURES of SODIUM FLUORIDE:
-Description of first-aid measures
*General advice:
Show this material safety data sheet to the doctor in attendance.
*If inhaled:
After inhalation:
Fresh air.
*In case of skin contact:
Take off immediately all contaminated clothing.
Rinse skin with
water/ shower.
*In case of eye contact:
After eye contact:
Rinse out with plenty of water.
Call in ophthalmologist.
Remove contact lenses.
*If swallowed:
After swallowing:
Immediately make victim drink water (two glasses at most).
Consult a physician.
-Indication of any immediate medical attention and special treatment needed.
No data available

ACCIDENTAL RELEASE MEASURES of SODIUM FLUORIDE:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Cover drains.
Collect, bind, and pump off spills.
Observe possible material restrictions.
Take up dry.
Dispose of properly.
Clean up affected area.

FIRE FIGHTING MEASURES of SODIUM FLUORIDE:
-Extinguishing media:
*Suitable extinguishing media:
Carbon dioxide (CO2)
Foam
Dry powder
*Unsuitable extinguishing media:
For this substance/mixture no limitations of extinguishing agents are given.
-Further information:
Prevent fire extinguishing water from contaminating surface water or the ground water system.

EXPOSURE CONTROLS/PERSONAL PROTECTION of SODIUM FLUORIDE:
-Control parameters:
--Ingredients with workplace control parameters:
-Exposure controls:
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
Safety glasses
*Body Protection:
protective clothing
*Respiratory protection:
Recommended Filter type: Filter A
-Control of environmental exposure:
Do not let product enter drains.

HANDLING and STORAGE of SODIUM FLUORIDE:
-Conditions for safe storage, including any incompatibilities:
*Storage conditions:
Tightly closed.
Dry.

STABILITY and REACTIVITY of SODIUM FLUORIDE:
-Chemical stability:
The product is chemically stable under standard ambient conditions (room temperature).
-Possibility of hazardous reactions:
No data available