Sodium+Flouride

Sodium fluoride is an [|ionic compound], dissolving to give separated Na+ and F− ions. Like [|sodium chloride], it crystallizes in a cubic motif where both Na+and F− occupy [|octahedral coordination sites]. [|[3]][|[4]] One of the uses of Sodium Fluoride, in __tablet__ form, is cavity prevention. Sodium Fluoride is toxic when inhaled or ingested, in high doses it has been shown to effect the circulatory system.
 * Sodium fluoride** is an [|inorganic chemical compound] with the [|formula] **NaF.** A colorless solid, it is a source of the fluoride ion in diverse __applications__. [|Sodium] [|fluoride] is less expensive and less [|hygroscopic] than the related salt [|potassium fluoride].

Production:
NaF is prepared by neutralizing hydrofluoric acid or hexafluorosilicic acid (H2SiF6), byproducts 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.[6]



fluoride salts are used to enhance the strength of teeth by the formation of fluorapatite, a naturally occurring component of tooth enamel. Although this is used to fluoridate water and is the standard by which other water fluoridation compounds are gauged, other acids are used as additives in the U.S.