Sodium fluoride
Sodium fluoride is an inorganic compound with formula NaF.
- 1Names
- 2Formulae and structures
- 3Properties
- 4Constituents
- 5Thermodynamic properties
- 6Solubility
- 7Hazards
- 8Preparations
- 9Chemical reactions
- 10References
- 11Related substances
- 12Related categories
Names
List of substance names
- Typical name
- Sodium fluoride
- Compositional nomenclature
- Sodium fluoride
Formulae and structures
List of formulae
- Typical formula
- NaF
- Compositional formula
- NaF
- Structural formula
- Lewis structure
- Colored Lewis structure
Properties
List of substance properties
Constituents
Constituent ions
Ion | Name | Charge number | Number |
---|---|---|---|
Na+ | Sodium ion | 1 | 1 |
F− | Fluoride ion | -1 | 1 |
Constituent atoms
Atom | Name | Oxidation state | Number |
---|---|---|---|
Na | Sodium | +1 | 1 |
F | Fluorine | −1 | 1 |
Ratio of atoms
Atom | Atomic weight | Number | Atomic ratio | Weight ratio |
---|---|---|---|---|
Na | 22.990 | 1 | 50.00% | 54.75% |
F | 18.998 | 1 | 50.00% | 45.25% |
Thermodynamic properties
Phase transition properties
Standard thermodynamic properties
State | Standard enthalpy of formation ΔfH° kJ · mol−1 | Standard Gibbs energy of formation ΔfG° kJ · mol−1 | Standard molar entropy S° J · K−1 · mol−1 | Standard molar heat capacity at constant pressure Cp° J · K−1 · mol−1 |
---|---|---|---|---|
Crystalline solid | −573.647[3] | −543.494[3] | 51.46[3] | 46.86[3] |
Gas | −291.2[3] | −310.5[3] | 217.59[3] | 34.221[3] |
Ionized aqueous solution | −572.75[3] | −540.68[3] | 45.2[3] | −60.2[3] |
Solubility
Qualitative solubility
Solubility in water (g/100 g)[1]
0°C | 20°C | 30°C | 40°C | 60°C | 80°C | 100°C |
---|---|---|---|---|---|---|
3.66 | 4.06 | 4.22 | 4.4 | 4.68 | 4.89 | 5.08 |
Solubility curve (g/100 g)
Hazards
GHS label[4]
- Hazard pictograms
GHS06: Skull and crossbones GHS07: Exclamation mark GHS05: Corrosion GHS08: Health hazard
- Signal word
- Danger
- Hazard statements
- H301: Toxic if swallowed
- H315: Causes skin irritation
- H318: Causes serious eye damage
- H370: Causes damage to organs
- H370: Causes damage to nervous system
- H370: Causes damage to heart
- H370: Causes damage to kidney
- H372: Causes damage to organs through prolonged or repeated exposure
- H372: Causes damage to tooth through prolonged or repeated exposure
- H372: Causes damage to bone through prolonged or repeated exposure
- H373: May cause damage to organs through prolonged or repeated exposure
- H373: May cause damage to heart through prolonged or repeated exposure
- H373: May cause damage to liver through prolonged or repeated exposure
- H373: May cause damage to kidney through prolonged or repeated exposure
- H373: May cause damage to male reproductive organs through prolonged or repeated exposure
- H402: Harmful to aquatic life
Physical hazards[4]
Health hazards[4]
Environmental hazards[4]
Preparations
Reaction of metal and nonmetal
The reaction of and yields sodium fluoride.
Reaction of acid and base
The reaction of hydrogen fluoride and sodium hydroxide yields sodium fluoride and water.
Reaction of basic oxide and acid
The reaction of sodium oxide and hydrogen fluoride yields sodium fluoride and water.
Reaction of salt of weak base and strong base
The reaction of salt of weak base and strong base can yield sodium fluoride.
Reaction of active metal and acid
The reaction of and hydrogen fluoride yields sodium fluoride and .
Chemical reactions
Electrolytic dissociation
Electrolytic dissociation of sodium fluoride yields sodium ion and fluoride ion.
Reaction with strong acid
The reaction of sodium fluoride and strong acid yields salt of strong acid and hydrogen fluoride.
Reaction with nonvolatile acid
The reaction of sodium fluoride and nonvolatile acid yields salt of non volatile acid and hydrogen fluoride.
Precipitation reaction
When a certain chemical species is present in aqueous solution, it reacts with sodium fluoride to form a precipitate.
Electrolysis of aqueous solution
Electrolysis of aqueous sodium fluoride yields a variety of products.
Molten salt electrolysis
Molten salt electrolysis of sodium fluoride yields and .
References
List of references
- 1James G. Speight (2017)Lange's Handbook of Chemistry, 17th editionMcGraw Hill Education
- ^ Density, 2.78 g/cm3 - p.64
- ^ Melting point, 996 °C - p.64
- ^ Boiling point, 1704 °C - p.64
- ^ Enthalpy of fusion, 33.35 kJ · mol−1 - p.310
- ^ Enthalpy of vaporization, 176.1 kJ · mol−1 - p.310
- ^ Enthalpy of vaporization at 25°C, 284.9 kJ · mol−1 - p.310
- ^ Qualitative solubility, Very soluble in water
- ^ Qualitative solubility, Insoluble in ethanol - p.64
- ^ Solubility in Water (g/100 g), See the table - p.343
- 2John R. Rumble Jr, David R. Lide, Thomas J. Bruno (2019)CRC Handbook of Chemistry and Physics 100th EditionCRC Press
- ^ Density, 2.78 g/cm3 - p.4-49
- ^ Melting point, 996 °C - p.4-49
- ^ Boiling point, 1704 °C - p.4-49
- ^ Enthalpy of fusion, 33.35 kJ · mol−1 - p.6-160
- 3Janiel J. Reed (1989)The NBS Tables of Chemical Thermodynamic Properties: Selected Values for Inorganic and C1 and C2 Organic Substances in SI UnitsNational Institute of Standards and Technology (NIST)
- ^ ΔfH°, -573.647 kJ · mol−1
- ^ ΔfG°, -543.494 kJ · mol−1
- ^ S°, 51.46 J · K−1 · mol−1
- ^ Cp°, 46.86 J · K−1 · mol−1
- ^ ΔfH°, -291.2 kJ · mol−1
- ^ ΔfG°, -310.5 kJ · mol−1
- ^ S°, 217.59 J · K−1 · mol−1
- ^ Cp°, 34.221 J · K−1 · mol−1
- ^ ΔfH°, -572.75 kJ · mol−1
- ^ ΔfG°, -540.68 kJ · mol−1
- ^ S°, 45.2 J · K−1 · mol−1
- ^ Cp°, -60.2 J · K−1 · mol−1
- 4Chemical Management CenterGHS Classification ResultsNational Institute of Technology and Evaluation