Sodium+Fluoride

__Sodium Flouride(NaF)__
NaF is prepared by neutralizing [|hydrofluoric acid] or [|hexafluorosilicic acid] (H 2 SiF 6 ), byproducts of the production of [|superphosphate] fertilizer. Neutralizing agents include [|sodium hydroxide] and [|sodium carbonate]. Alcohols are sometimes used to precipitate the NaF:


 * Sodium fluoride** is an inorganic chemical compound. It's 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].

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].

__Uses:__ TOOTHPASTE A source of inorganic fluoride which is used topically to prevent dental caries.

__HOW?__ Fluoride salts are used to enhance the strength of teeth by the formation of [|fluorapatite], a naturally occurring component of [|tooth enamel]. Although sodium fluoride is also used to [|fluoridate water] and, indeed, is the standard by which other water-fluoridation compounds are gauged, [|hexafluorosilicic acid] (H2SiF6) and its salt sodium hexafluorosilicate (Na 2 SiF 6 ) are more commonly used additives in the U.S. [|Toothpaste] often contains sodium fluoride to prevent [|cavities].Alternatively, sodium fluoride is used as a cleaning agent, e.g. as a "laundry sour". A variety of specialty chemical applications exist in synthesis and extractive [|metallurgy]. It reacts with electrophilic chlorides including [|acyl chlorides], sulfur chlorides, and phosphorus chloride. Like other fluorides, sodium fluoride finds use in [|desilylation] in [|organic synthesis]. The fluoride is the reagent for the synthesis of [|fluorocarbons].

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