| IUPAC name
| Other names
|Molar mass||41.988173 g/mol|
|Melting point||993 °C (1,819 °F; 1,266 K)|
|Boiling point||1,704 °C (3,099 °F; 1,977 K)|
| 3.64 g/100 ml (0 °C)|
4.04 g/100 ml (20 °C)
5.05 g/100 ml (100 °C)
|Solubility|| Reacts with sulfuric acid|
Slightly soluble in ammonia, hydrofluoric acid
Negligible in acetone, dimethylformamide, ethanol, methanol, liq. SO2
Insoluble in halocarbons, hydrocarbons
|Vapor pressure||~0 mmHg|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
|Lethal dose or concentration (LD, LC):|
LD50 (Median dose)
|52–200 mg/kg (oral in rats, mice, rabbits)|
| Sodium chloride|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Sodium fluoride is an inorganic compound with the formula NaF, a salt of hydrofluoric acid.
Addition of a strong acid, like sulfuric acid will release hydrofluoric acid.
- 2 NaF + H2SO4 → 2 HF + Na2SO4
Sodium fluoride is a white solid, poorly soluble in water and most solvents.
Sodium fluoride is sold by chemical suppliers, though it's sometimes pricey.
It occurs in nature as the rare mineral villiaumite.
- HF + NaOH → NaF + H2O
- 2 HF + Na2CO3 → 2 NaF + H2O + CO2
- HF + NaHCO3 → NaF + H2O + CO2
Due to its poor solubility, sodium fluoride will precipitate out of the solution.
- Make hydrofluoric acid
- Make fluorocarbons
- Mineral collecting (villiaumite)
Avoid contact with strong acids, as it will release hydrofluoric acid.
Sodium fluoride is best kept in closed plastic (PE or PP) bottles. Avoid storing it in glass containers. Keep the bottle in a dry place.
Should be converted to the less soluble calcium fluoride and dumped in trash. Recycling is also an option.