Sodium fluoride
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| Sodium fluoride | |
|---|---|
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| General | |
| Systematic name | Sodium fluoride |
| Molecular formula | NaF |
| Molar mass | 41.98817 g/mol |
| Appearance | White solid |
| CAS number | [7681-49-4] |
| Properties | |
| Density and phase | 2.558 g/cm3, solid |
| Solubility in water | 4.22 g/100mL at 18 °C |
| Other solvents | poorly sol: ethanol |
| Melting point | 993°C |
| Boiling point | 1700°C |
| Basicity (pKb) | N/A |
| Hazards | |
| MSDS | External MSDS |
| EU classification | Toxic (T) |
| R-phrases | R25, R32, R36, R38 |
| S-phrases | S22, S36, S45 |
| NFPA 704 |
0
2
0
|
| Flash point | Non-flammable. |
| Supplementary data page | |
| Structure and properties |
n, εr, etc. |
| Thermodynamic data |
Phase behaviour Solid, liquid, gas |
| Spectral data | UV, IR, NMR, MS |
| Related compounds | |
| Other anions | sodium chloride sodium bromide sodium iodide |
| Other cations | potassium fluoride calcium fluoride |
| Related bases | None listed. |
| Related compounds | None listed. |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Sodium fluoride is an ionic compound with the formula NaF. This colourless solid is the main source of the fluoride ion in diverse applications. NaF is less expensive and less hygroscopic than KF, but otherwise the potassium salt is more widely used.
Contents |
[edit] Chemical properties and structure
NaF crystallizes in the sodium chloride motif where both Na+ and F- occupy octahedral coordination sites.
It is usually as a reagent for the synthesis of fluorides. Representative substrates include electrophilic chlorides including acyl chlorides, sulfur chlorides, and phosphorus chloride.[1] Like other fluorides, NaF finds use in desilylation in organic synthesis.
[edit] Applications
Fluoride salts are used widely to enhance the strength of teeth by the formation of fluoroapatite, a naturally occurring component of tooth enamel. In the US, NaF was once used to fluoridate drinking water but its use has been displaced by hexafluorosilicic acid (H2SiF6) or its sodium salt (Na2SiF6). Toothpaste often contains sodium fluoride to prevent cavities.
Sodium fluoride was also used as an antibiotic, as rat poison, and in ceramics.
[edit] Safety considerations
Sodium fluoride is mildly toxic, LD50 = 0.18 g kg–1 in rats.
[edit] References
- ^ Halpern, D. F. “Sodium Fluoride” Encyclopedia of Reagents for Organic Synthesis, 2001, John Wiley & Sons. DOI: 10.1002/047084289X.rs071.
[edit] See also
[edit] External links
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