Sodium Fluoride - NaF

What is Sodium Fluoride?

Sodium fluoride is manufactured by the reaction of hydrofluoric acid with sodium carbonate or sodium hydroxide with the formula NaF. The most inexpensive chemical available for fluoridation is sodium fluorosilicate, formerly known as sodium silicofluoride. Sodium fluoride solutions are used with hard water insoluble compounds of calcium and magnesium fluoride can form. It is a dry chemical used in fluoridation of drinking water, it should be manually weighed and added to the mixing tank.

NaF

Sodium fluoride

Density

2.56 g/cm³

Molecular Weight/ Molar Mass

41.98817 g/mol

Boiling Point

1,695 °C

Melting Point

993 °C

Chemical Formula

NaF

Sodium Fluoride Structure – NaF

Sodium Flouride

Physical Properties of Sodium fluoride – NaF

Odour

Odorless

Appearance

White crystals or powder

Complexity

2

Vapour Pressure

1 mm Hg at 1971 ° F

Hydrogen Bond Acceptor

1

Solubility in water

10 to 50 mg/mL at 73° F

Chemical Properties of Sodium fluoride – NaF

  • Sodium fluoride reacts with water forms hydrogen fluoride and sodium hydroxide. The chemical equation is as below.
  • NaF + H2O → HF + NaOH

  • Sodium fluoride reacts with chlorine undergoes displacement reaction forming sodium chloride and fluorine.
  • NaF + Cl2 → NaCl + F2

Uses of Sodium fluoride – NaF

  • Sodium fluoride has bactericidal properties but it is too toxic for use as a wound antiseptic.
  • Systemic fluoride use during pregnancy has not been shown to prevent tooth decay in children
  • Sodium fluoride is used as an insecticide.
  • Used in the fluoridation of public water.
  • The monosodium salt of Sodium fluoride L-glutamic acid; used in treatment of encephalopathies associated with liver diseases.

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