- CAS No.
- Chemical Name:
- Hydrogen fluoride
- HF;HYDROFLUORIC ACID;Anhydrous hydrofluoric acid;hydrofluoric;Urea Hydrofluoride;HydrofL;Fluoric acid;Hydrofluoride;Hydrofluoric acid(HF);Hydrofluoric Acid, TraceGrade
- Molecular Formula:
- Molecular Weight:
- MDL Number:
- MOL File:
- MSDS File:
|Density||1.15 g/mL at 25 °C(lit.)|
|vapor density||1.27 (vs air)|
|vapor pressure||25 mm Hg ( 20 °C)|
|storage temp.||Store at +5°C to +30°C.|
|form||Liquid, Double Sub-Boiling Quartz Distillation|
|Odor||Acrid, irritating odor|
|PH||3.27(1 mM solution);2.65(10 mM solution);2.12(100 mM solution)|
|Exposure limits||Ceiling limit 3 ppm (～2.5 mg/m3) as F (ACGIH); TWA 3 ppm (MSHA and OSHA).|
|Stability||Stable. Hygroscopic. Incompatible with glass, alkali metals, light metals, alkaline earth metals|
|LogP||0.1 at 20℃|
|Indirect Additives used in Food Contact Substances||HYDROFLUORIC ACID|
|FDA 21 CFR||175.105|
|CAS DataBase Reference||7664-39-3(CAS DataBase Reference)|
|EWG's Food Scores||3-6|
|NIST Chemistry Reference||Hydrogen fluoride(7664-39-3)|
|EPA Substance Registry System||Hydrofluoric acid (7664-39-3)|
Risk and Safety Statements
|RIDADR||UN 1790 8/PG 2|
|DOT Classification||8, Hazard Zone C (Corrosive material)|
|Toxicity||LC50 (15 min.) in rats, guinea pigs: 2689, 4327 ppm (Rosenholtz)|
Hydrogen fluoride price More Price(44)
|Manufacturer||Product number||Product description||CAS number||Packaging||Price||Updated||Buy|
|Sigma-Aldrich||30103||Hydrofluoric acid puriss. p.a., reag. ISO, reag. Ph. Eur., ≥40%||7664-39-3||1l||$89.8||2023-06-20||Buy|
|Sigma-Aldrich||HX0628||Hydrofluoric Acid OmniTrace Ultra||7664-39-3||250ML||$918||2022-05-15||Buy|
|Sigma-Aldrich||HX0628||Hydrofluoric Acid OmniTrace Ultra||7664-39-3||500ML||$1310||2022-05-15||Buy|
|Sigma-Aldrich||HX0628||Hydrofluoric Acid OmniTrace Ultra||7664-39-3||1L||$1500||2022-05-15||Buy|
|Sigma-Aldrich||HX0627||Hydrofluoric Acid OmniTrace||7664-39-3||500ML||$272||2022-05-15||Buy|
Hydrogen fluoride Chemical Properties,Uses,Production
Hydrofluoric acid (HF) is an aqueous solution of hydrogen fluoride gas. At room temperature, it appears as colorless transparent to light yellow smoke liquid with pungent odor. It has a specific gravity of 0.98 which is slightly lighter than water. It has a boiling point of 19.4 °C, being highly volatile. It can release white smoke once placed in air. The aqueous solution containing less than 60% hydrogen fluoride appears as a colorless clear fuming liquid. Industrial products are usually aqueous solution containing 40 to 45% HF. It has pungent odor. It can react with sulfur trioxide or chlorosulfonic acid to generate fluoride sulfonic acid, and can react with halogenated aromatic hydrocarbons, alcohols, olefins, hydrocarbons to generate fluorine-containing organic compound. When being dissolved in water, it can produce highly corrosive acid, being medium-intensity acid. It is extremely smelly, being very toxic and is prone to cause ulceration when get touch with the skin with a severe extent being larger than any acids. If inhaled of its vapor, it can have fatal effects, thus strict attention should paid during usage.
1. Hydrofluoric acid can also react with general metals, metal oxides, and hydroxide, generating a variety of metal fluoride salts, but the effect is not as dramatic as hydrochloric acid. Gold, platinum, lead, paraffin and some plastics (polyethylene, etc.) does not react with it and thus being able to be used as containers.
2. Strong corrosiveness: it can erode glass and silicate to produce gaseous silicon tetrafluoride. The reaction is as follows: SiO2 + 4HF → H2O + SiF4 ↑, glass is a silicon compound so the hydrofluoric acid can’t be put into glass containers.
Hydrofluoric acid can form acid salt, hydrofluoric acid is a monobasic acid, but can produce a series of acid salts such as NaHF2, KHF2, NH4HF2, which are the other three kinds of halogen acid.
4. The weak acidity of hydrofluoric acid; because of the strong binding capability of hydrogen atom with fluorine atom, hydrofluoric acid can’t be completely dissociated in the water. In the hydrohalic acid, only hydrofluoric acid is weak acid (its ionization constant is 3.5 × 10 ^-4; its apparent ionization degree is about 10% at a concentration of 0.1mo1.L^-1, therefore, HF can reluctantly taken as a kind of strong acid. The ionization degree at high concentration is higher than that at low concentration. This property is different from other kinds of general weak electrolytes).
It appears as colorless fuming liquid. It is intensively exothermic when being dissolved in water and further become hydrofluoric acid.
Hydrogen fluoride is the most important compound of fluorine. Anhydrous hydrogen fluoride is used in the production of most fluorine-containing chemicals. It is used in the production of refrigerants, herbicides, pharmaceuticals, high-octane gasoline, aluminum, plastics, electrical components, and fluorescent light bulbs. Aqueous hydrofluoric acid is used in stainless steel pickling, glass etching, metalcoatings, exotic metal extraction, and quartz purification(Hance et al. 1997).The most important use of hydrogen fluoride is in the production of fluorocarbon chemicals, including hydrofluorocarbons, hydrofluorochlorocarbons, and fluoropolymers; 60% of production is used for this purpose. Demand for hydrogen fluoride for fluorocarbons, broadly used as refrigerants, is increasing as a nonchlorinated alternative to ozone-depleting chlorofluorocarbons.(Production of fluorocarbons uses more hydrogen fluoride than production of chlorofluorocarbons.) The next most important uses of hydrogen fluoride are:chemical derivatives,18%; aluminum manufacturing,6%; stainless steel pickling,5%; petroleum alkylation catalysts, 4%; and uranium chemicals production,3%.Miscellaneous other uses include glassetching, herbicides, and rare metals(CMR 2002).Generally, the aluminum industry consumes 10-40 kg of fluoride per metric ton of aluminum produced.The AlF, used in aluminum reduction cells may be produced directly from acid-grade fluorspar or byproduct fluorosilicic acid, rather than from hydrogen fluoride. Anhydrous hydrogen fluoride is used as a catalyst in the petroleum alkylation, a process that increases the octane rating of petroleum. In uranium chemicals production, hydrogen fluoride is used to convert uranium oxide(yellow cake,U3O8) to UF4. before further fluorination to UF6.
Hydrofluoric acid has irritating smell and acute toxicity, belonging to the medium strength & slightly weak acid. It is corrosive. It is commonly used in the manufacture of fluorocarbon, sodium fluoride, aluminum fluoride, uranium hexafluoride and cryolite and other organic or inorganic fluorine compounds. It can be applied to the pickling of stainless steel and non-ferrous metal. The semiconductor industry take it as a cleaning agent; glass etching industry as its etchant; the steel industry take it as a surface rust removing agent; the petrochemical industry take it as a catalyst; the cleaning services take it as a dirt cleaning agent or as an external wall cleaning agent.
For professionals that are exposure to hydrofluoric acid in the daily work, improper use may cause non-negligible harm to the human body. Its exposure approaches include the skin and mucous membranes contact, respiratory inhalation and gastrointestinal uptake. Skin, if in contact with a over 50% concentrations of hydrofluoric acid, will immediately get painful feeling, whitening, swelling reaction. Blister can occur in 1 to 2 hours and the necrosis and ulceration can occur within 6 to 24 hours. People exposure to lower concentration (below 10%) will get pain and other symptoms in 6 hours or more. This may be overlooked by the parties, leading to extremely delayed treatment and finally permanent injury. Generally, the most common part of the injury is the finger.
In addition, if exposed from other approaches such as the respiratory tract and gastrointestinal tract, it will produce cough, burning and breathing difficulties and other symptoms, or causing abdominal pain, nausea, vomiting blood, intestinal perforation and other symptoms. The harm of hydrofluoric acid on the human body, in addition to acid corrosion damage, fluoride ions entering into the body may bind to calcium and magnesium ions, resulting in hypocalcemia, hypomagnesemia and hyperkalemia, further affecting the nervous and cardiovascular system.
Daily administration of hydrofluoric acid should avoid contact with the body, including skin, eyes and respiratory tract. In prevention of the contact with the skin, we should wear gloves of fluorinated polyethylene (PVDF) and natural rubber. Do not use cloth and cotton gloves and should do systemic protection in occasion easy to splash. We can wear the coverall protecting cloth and work boots of rubber material with the eye should wear goggles or full-face mask. If accidentally corroded by the hydrofluoric acid, immediately use large amount of water to rinse the affected area for at least 30 minutes until there is not any attached solid or liquid that can be observed in the body. Meanwhile, send the patients immediately to hospital for medical treatment as soon as possible. During the medical treatment, we should be brought the chemicals in contact to enable the timely and correct medical treatment by the medical staffs.
See also hydrofluoric acid.
Hydrofluoric acid is highly corrosive, being able to corrode glass and nail with its vapor being extremely poisonous. The maximum allowable concentration is 1 mg/m3 (LD501.276 × 10-3). Skin contact will cause swelling and burning sensation and the eyes will get blurred vision. After inhalation, people can get sore throat, cough and have difficulty in breathing. After entering into the digestive tract, people can get abdominal pain, diarrhea, and vomiting. For protection, people should pay attention to ventilation. The operator must wear protective equipment, preventing its contact with the skin. Upon inadvertently contacting the skin, immediately rinse with plenty of water; after rinse away the acid, you can generally use mercurochrome solution or gentian violet for coating the affected area. Upon serious case, the patients should be sent to hospital for treatment.
It has irritating and toxic effect with strong corrosive effect on the skin and eyes, being able to produce serious burns; burns do not immediately appear, and the treatment is relatively slow. Access to it must be conducted in a well-ventilated place or in a fume hood. The staff should wear fluoride resistant gloves of suitable size, boots and protective aprons and face shields. In case of contact or suspected contact with this product, rinse with plenty of water and seek for medical treatment immediately.
Sulfuric acid method: mix the dried fluorite powder and sulfuric acid in the ratio of 1: (1.2~1.3), send into the rotary reaction furnace for reaction. The temperature of the furnace gas phase is controlled at 280 °C ± 10 °C. The post-reaction gas enters into the crude distillation tower for removal of most of the sulfuric acid, water and fluorite powder. The temperature of the tower kettle is controlled at 100 to 110 °C and the top temperature is 35 to 40 °C. The crude hydrogen fluoride gas is further condensed into a liquid state through a degassing tower with the temperature of the tower kettle being controlled at 20 to 23 °C and the top temperature of the tower being controlled at-8 °C ± 1 °C and then enters into the rectification tower for rectification with the temperature of the tower kettle being controlled at 30 to 40 °C and the temperature of the top of the column being controlled at 19.6 ° C ± 0.5 °C. The purified hydrogen fluoride is absorbed by water so the hydrofluoric acid product is obtained. The reaction formula is:
CaF2 + H2SO4 → 2HF + CaSO4
Sulfuric acid method: the hydrogen fluoride generated through sulfuric acid decomposition of fluorite is subject to the crude distillation, degassing and then be distilled to produce anhydrous hydrofluoric acid. And the reaction formula is:
CaF2 + H2SO4 → 2HF + CaSO4
Refining purification technology: the industrial grade hydrofluoric acid is purified by distillation with condensation to remove impurities, and filtered through a microporous membrane to remove dust particles, producing colorless and transparent electronic grade hydrofluoric acid.
Hydrofluoric acid is a solution of hydrogen fluoride in water. Hydrofluoric acid is highly corrosive inorganic acid. It is utilized widely in the manufacture of ceramics and graphite, in the electropolishing and pickling of metals, in the etching and frosting of glass, in the semiconductor industry as etchant and cleaning agent, in the chemical and oil-refining industries, and in cleaning solutions, laundry powder and pesticides. Hydrofluoric acid is also widely used in the preparation of many useful fluorine compounds, such as Teflon, Freon, fluorocarbons, and many medications such as fluoxetine (Prozac).
colourless gas with a pungent odour
Hydrofluoric Acid (HF) is a solution of hydrogen fluoride in water.
While this acid is extremely corrosive and difficult to
handle, it is technically a weak acid. Hydrogen fluoride,
often in the aqueous form as hydrofluoric acid,
is a valued source of fluorine, being the precursor to
numerous pharmaceuticals such as fluoxetine (Prozac),
diverse polymers such as polytetrafluoroethylene
(Teflon), and most other synthetic materials that
contain fluorine. Hydrofluoric acid is best known to
the public for its ability to dissolve glass by reacting
with SiO2 (silicon dioxide), the major component of
most glass, to form silicon tetrafluoride gas and hexafluorosilicic acid. This property has been known
since the seventeenth century, even before hydrofluoric
acid had been prepared in large quantities by
Scheele in 1771. Because of its high reactivity toward glass, hydrofluoric acid must be stored (in small quantities) in polyethylene or Teflon containers. It is also unique in its ability to dissolve many metal and semimetal oxides. Hydrofluoric acid attacks glass by reaction with silicon dioxide to form gaseous or water-soluble silicon fluorides.
Hydrofluoric acid is very dangerous to handle, because the human skin becomes easily saturated with the acid. Even though skin absorption of small areas of only 25 square inches (160 cm2) may be relatively painless, yet the exposure may be ultimately fatal. High concentrations of hydrofluoric acid and hydrogen fluoride gas will also quickly destroy the corneas of the eyes.
Anhydrous hydrogen fluoride was first prepared by Fremy in 1856. It mayhave been made earlier in 1670 by Schwankhard in the process of etchingglass using fluorspar and acid.
Hydrogen fluoride is the most important fluorine compound, in terms ofamounts produced and the vast number of uses. The largest application of thiscompound is in the manufacture of aluminum fluoride and sodium aluminumfluoride (cryolite) for electrolytic production of aluminum. Another majorapplication is in the manufacture of chlorofluorocarbons, which are used asrefrigerants and foaming agents; for making polymers; and for pressurizinggases. Another important application is in the processing of uranium whereHF converts uranium dioxide to uranium tetrafluoride and hexafluoride,respectively. Uranium hexafluoride is used to separate isotopes of uraniumby diffusion.
Hydrogen fluoride also is used as a catalyst in alkylation of aromatic com-pounds and for dimerization of isobutene. Other catalytic applications are inisomerization, polymerization, and dehydration reactions. Other uses are in366HYDROGEN FLUORIDEpp-03-25-new dots.qxd 10/23/02 2:38 PM Page 366 etching and polishing glasses for manufacturing light bulbs and TV tubes; inextraction of ores; in pickling stainless steel; in acidizing oil-wells; to removelaundry stains; for sample digestion in metal analysis; for removal of sandduring metal castings; as a stabilizer for rocket propellant oxidizers; and inpreparation of a number of fluoride alts of metals.
Diluted hydrofluoric acid (1-3 %wt) is used in the "Oil Patch" in a mixture with other acids (HCl or organic acids) in order to stimulate the production of water, oil and gas wells specifically where sandstone is involved. HF is also used in oil refining. In a standard oil-refinery process known as Alkylation, isobutane is alkylated with low-molecular weight alkenes (primarily a mixture of propylene and butylene) in the presence of a strong acid catalyst, hydrofluoric acid. The catalyst is able to protonate the alkenes (propylene, butylene) to produce reactive carbo-cations , which cause alkylation of isobutane. The phases separate spontaneously, so the acid phase is vigorously mixed with the hydrocarbon phase to create sufficient contact surface. Hydrofluoric acid (HF) is used principally in organofluorine chemistry. Additionally, most high-volume inorganic fluoride compounds are prepared from hydrofluoric acid. Foremost are Na3AlF6, (Cryolite), and AlF3(aluminum trifluoride). A molten mixture of these solids serves as a high-temperature solvent for the production of metallic aluminum. Concerns about fluorides in the environment have led to a search for alternative technologies. Other inorganic fluorides prepared from hydrofluoric acid include NaF and UF6.
The ability of hydrofluoric acid to dissolve metal oxides is the basis of several applications. It removes oxide impurities from stainless steel in a process called pickling. Surface oxides are removed from silicon with hydrofluoric acid in the Semiconductor Industry. For this purpose, dilute hydrofluoric acid is sold as a household rust stain remover. Recently, it has even been used in “Car-Wash” facilities in “wheel cleaner” compounds. Due to its ability to dissolve oxides, hydrofluoric acid is useful for dissolving rock samples (usually powdered) prior to analysis. Similarly, this acid has been used to extract organic fossils from silicate rocks. Fossiliferous rock may be immersed directly into the acid, or a cellulose nitrate film may be applied (dissolved in amyl acetate), which adheres to the organic component and allows the rock to be dissolved around it.
Cleaning cast iron, copper, brass; removing efflorescence from brick and stone, or sand particles from metallic castings; working over too heavily weighted silks; frosting, etching glass and enamel; polishing crystal glass; decomposing cellulose; enameling and galvanizing iron; increasing porosity of ceramics. Its salts are used as insecticides and to arrest undesirable fermentation in brewing. Also used in analytical work to determine SiO2, etc.
Hydrofluoric acid is used as a fluorinatingagent, as a catalyst, and in uranium refining.It is also used for etching glass and forpickling stainless steel. Hydrogen fluoridegas is produced when an inorganic fluoride is distilled with concentrated sulfuricacid.
A colorless liquid produced by dissolving hydrogen fluoride in water. It is a weak acid, but will dissolve most silicates and hence can be used to etch glass. As the interatomic distance in HF is relatively small, the H–F bond energy is very high and hydrogen fluoride is not a good proton donor. It does, however, form hydrogen bonds.
ChEBI: A diatomic molecule containing covalently bonded hydrogen and fluorine atoms.
Anhydrous hydrogen fluoride is manufactured by the action of sulfuric on calcium fluoride. Powdered acid-grade fluorspar (≥97% CaF2) is distilled with concentrated sulfuric acid; the gaseous hydrogen fluoride that leaves the reactor is condensed and purified by distillation.
Anhydrous hydrogen fluoride is manufactured by treating fluorspar (fluorite, CaF2) with concentrated sulfuric acid in heated kilns. The gaseous HF evolved is purified by distillation, condensed as liquid anhydrous HF, and stored in steel tanks and cylinders.
Although anhydrous hydrogen fluoride is a very strong acid, its aqueous solution, hydrofluoric acid, is weakly acidic, particularly when dilute. The Ka value of aqueous acid at 25°C is 6.46x10–4 mol/L. It is an excellent solvent for many inorganic fluorides, forming bifluoride anion:
HF + NaF → Na+ + HF2¯ At lower temperatures (below 200°C), HF forms molecular aggregates that are held by hydrogen bonding containing linear chains of –F—H—-F—H—- F—H—-. However, above this temperature the weak hydrogen bond breaks producing monomolecular HF. Thermal dissociation of HF into elements probably occurs only at very high temperatures. Forty to 50% HF probably dissociates around 4,000°C, indicating that it is one of the most stable diatomic molecules. The most important reactions of HF involve formation of inorganic fluoridesalts. HF gas or hydrofluoric acid reacts with oxides, hydroxides, carbonates, chlorides and other metal salts forming the corresponding fluorides. Some examples are:
Bi2O3 + 6HF → 2BiF3 + 3H2O
LiOH + HF → LiF + H2O
CaCO3 + 2HF → CaF2 +CO2 + H2O
FeCl3 + 3HF → FeF3 + 3HCl
CoCl2 + 2HF → CoF2 + 2HCl Reaction with potassium dichromate yields chromyl fluoride:
K2Cr2O7 + 6HF → 2CrO2F2 + 2KF + 3H2O When ammonia gas is bubbled through a 40% ice-cold solution of hydrofluoric acid, the product is ammonium fluoride:
NH3 + HF → NH4F The addition of equimolar amount of NaOH or Na2CO3 to 40% HF instantaneously precipitates NaF:
NaOH + HF → NaF + H2O Excess HF, however, yields sodium bifluoride, NaHF2:
NaOH + 2HF → NaHF2 + H2O Reaction with phosphorus trichloride yields phosphorus trifluoride; and with phosphoryl fluoride and sulfur trioxide, the product is phosphorus pentafluoride:
PCl3 + 3HF → PF3 + HCl
POF3 + 2HF + SO3 → PF5 + H2SO4
HF is a colorless inorganic acid. Hydrogen fluoride may be formed by reacting calcium fluoride and sulfuric acid at 200oC. The fluoride in the acid has very high affinity to silicon, making it useful in etching or removal of silicon.
Air & Water Reactions
Fumes in air. Fumes are highly irritating, corrosive, and poisonous. Generates much heat on dissolution [Merck, 11th ed., 1989]. Heat can cause spattering, fuming, etc.
Hydrofluoric acid attacks glass and any other silica containing material. May react with common metals (iron, steel) to generate flammable hydrogen gas if diluted below 65% with water. Reacts exothermically with chemical bases (examples: amines, amides, inorganic hydroxides). Can initiate polymerization in certain alkenes. Reacts with cyanide salts and compounds to release gaseous hydrogen cyanide. May generate flammable and/or toxic gases with dithiocarbamates, isocyanates, mercaptans, nitrides, nitriles, sulfides. Additional gas-generating reactions may occur with sulfites, nitrites, thiosulfates (to give H2S and SO3), dithionites (SO2), and carbonates. Can catalyze (increase the rate of) chemical reactions. Reacts explosively with cyanogen fluoride, methanesulfonic acid or glycerol mixed with nitric acid. Reacts violently with arsenic trioxide, phosphorus pentachloride, acetic anhydride, alkali metals, ammonium hydroxide, chlorosulfonic acid, ethylenediamine, fluorine, potassium permanganate, oleum, propylene oxide, vinyl acetate, mercury(II) oxide. Emits highly corrosive fumes of hydrogen fluoride gas when heated [Sax, 9th ed., 1996, p. 1839]. Contact with many silicon compounds and metal silicides causes violent evolution of gaseous silicon tetrafluoride [Mellor, 1956, Vol. 2, suppl. 1, p. 121].
Toxic by ingestion and inhalation, highly corrosive to skin and mucous membranes.
Hydrofluoric acid and hydrogen fluoride gasare extremely corrosive to body tissues, causing severe burns. The acid can penetrate theskin and destroy the tissues beneath and evenaffect the bones. Contact with dilute acid cancause burns, which may be perceptible hoursafter the exposure. The healing is slow. Contact with the eyes can result in impairment ofvision.
Prolonged exposure to 10–15 ppm concentrations of the gas may cause redness ofskin and irritation of the nose and eyes inhumans. Inhalation of high concentrations ofHF may produce fluorosis and pulmonaryedema. In animals, repeated exposure toHF gas within the range 20–25 ppm hasproduced injury to the lungs, liver, andkidneys.
LC50 value, inhalation (mice): 342 ppm/h.
When heated, Hydrofluoric acid emits highly corrosive fumes of fluorides. Its corrosive action on metals can result in formation of hydrogen in containers and piping to create fire hazard. Toxic and irritating vapors are generated when heated. Will attack glass, concrete, and certain metals, especially those containing silica, such as cast iron. Will attack natural rubber, leather, and many organic materials. May generate flammable hydrogen gas in contact with some metals.
Flammability and Explosibility
Hydrogen fluoride is not a combustible substance
Hydrofluoric acid (HF) is a colorless liquid with a characteristic odor. It releases fumes
when in contact with moist air. Hydrofluoric acid is manufactured from fluorite containing
96–97% CaF2 by reacting it with concentrated sulfuric acid:
CaF2+H2SO4 = 2HF+CaSO4 The acid is sold as a 40% solution. The hydrofluoric acid is used as an activator and depressant, mostly during flotation of industrial minerals (i.e. columbite, tantalite, silica, feldspars).
Carbon steel (without nonmetallic inclusions) is acceptable for handling hydrogen fluoride up to approximately 150°F (65.6°C). Aluminum- silicon-bronze, stainless steel, or nickel are suitable for cylinder valves. For higher temperatures, Monel, Inconel, nickel, or copper should be used. Cast iron or malleable fittings should be avoided. Polyethylene, lead, soft copper, Kel-F, and Teflon are acceptable gasket materials. Polyethylene, Kel-F, and Teflon are acceptable packing materials.
Hydrogen fluoride is highly corrosive to all living tissue. Contact with liquid anhydrous hydrogen fluoride, its vapor, or hydrogen fluoride solutions can cause severe bums to skin, eyes, or respiratory tract. ACGIH recommends a Threshold Limit Value-Ceiling (TLV-C) of 3 ppm (2.3 mg/m3 ) fi)r hydrogen fluoride (as F). The TLV-C is the concentration that should not be exceeded during any part of the working exposure .
NTP conducted two chronic oral bioassays of fluoride administered as sodium fluoride (0, 25, 100, or 175 ppm) in drinking water for 103 weeks in rats and mice.The first study was compromised, so it was used to determine doses for the second study. NTP concluded that there was no evidence that fluoride was carcinogenic at doses up to 4.73 mg/kg/day in female rats or at doses up to 17.8 and 19.9 mg/kg/day in male and female mice, respectively.
Hydrogen fluoride is a colorless, fuming liquid with a strong,
irritating odor. The density is 1.002 at 0 ℃ and the boiling
point is 19.51 ℃. Hydrogen Fluoride is naturally released into
the environment, primarily from volcanoes, ranging from 0.6
to 6 million metric tons per year. The majority of artificial
pollutants come from electrical utilities.
Hydrogen fluoride is removed from air by wet deposition as fluoride salts with an atmospheric lifetime of 1–5 days.
All work with HF should be conducted in a fume hood to prevent exposure by inhalation, and splash goggles and neoprene gloves should be worn at all times to prevent eye and skin contact. Containers of HF should be stored in secondary containers made of polyethylene in areas separate from incompatible materials. Work with anhydrous HF should be undertaken using special equipment and only by well-trained personnel familiar with first aid procedures.
It can be purified by trap-to-trap distillation, followed by drying over CoF2 at room temperature and further distillation. Alternatively, it can be absorbed on NaF to form NaHF2 which is then heated under vacuum at 150o to remove volatile impurities. The HF is regenerated by heating at 300o and is stored with CoF3 in a nickel vessel, being distilled as required. (Water content should be ca 0.01%.) To avoid contact with base metal, use can be made of nickel, polychlorotrifluoroethylene and gold-lined fittings [Hyman et al. J Am Chem Soc 79 3668 1957]. An aqueous solution is hydrofluoric acid (see above). It is HIGHLY TOXIC and attacks glass.
HFA is toxic by ingestion, inhalation, and (most commonly) by dermal exposure. It is highly corrosive to the skin and mucous membranes with very short (5 s or less) exposure concentrations of 0.003% and above, acting by protonation of tissues. It causes a liquefying necrosis at the site of contact. Absorption of fluoride ions leads to systemic fluoride poisoning, in turn leading to hypokalemia and hypomagnesemia potentially resulting in neuromuscular paralysis and cardiac arrhythmias.
HF reacts with glass, ceramics, and some metals. Reactions with metals may generate potentially explosive hydrogen gas.
Excess hydrogen fluoride and waste material containing this substance should be placed in an appropriate container, clearly labeled, and handled according to your institution's waste disposal guidelines. For more information on disposal procedures, see Chapter 7 of this volume.
 David J. Monk, and David S. Soane, A review of the chemical reaction mechanism and kinetics for hydrofluoric acid etching of silicon dioxide for surface micromachining applications, Thin Solid Films, 1993, vol. 232, 1-12
 P. Sanz-Gallen, S. Nogue, P. Munne and A. Faraldo, Hybocalcaemia and hypomagnesaemia due to hydrofluoric acid, Occup Med (Lond), 2001, vol. 51, 294-295
Anhydrous hydrogen fluoride is available from a number of suppliers with grades ranging from 99.0 percent to 99.96 percent. The major impurities are water (H20) and sulfur dioxide (S02).
Hydrogen fluoride Preparation Products And Raw materials
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