Difference between revisions of "Sodium fluoride"

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==Properties==
 
==Properties==
 
===Chemical===
 
===Chemical===
Addition of a strong acid, like [[sulfuric acid]] will release hydrofluoric acid.
+
Addition of a strong acid, like [[sulfuric acid]] will release [[hydrofluoric acid]].
  
 
: 2 NaF + H<sub>2</sub>SO<sub>4</sub> → 2 HF + Na<sub>2</sub>SO<sub>4</sub>
 
: 2 NaF + H<sub>2</sub>SO<sub>4</sub> → 2 HF + Na<sub>2</sub>SO<sub>4</sub>
  
 
===Physical===
 
===Physical===
Sodium fluoride is a white solid, poorly soluble in water.
+
Sodium fluoride is a white solid, poorly soluble in water and most solvents.
  
 
==Availability==
 
==Availability==
Sodium fluoride is sold by chemical suppliers, though it's sometimes pricey.
+
Sodium fluoride is sold by chemical suppliers, though it's sometimes pricey, depending on the seller.
  
 
It occurs in nature as the rare mineral ''villiaumite''.
 
It occurs in nature as the rare mineral ''villiaumite''.
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==Handling==
 
==Handling==
 
===Safety===
 
===Safety===
 +
Sodium fluoride is poisonous, and it's toxic if ingested, inhaled or injected.
 +
 
Avoid contact with strong acids, as it will release hydrofluoric acid.
 
Avoid contact with strong acids, as it will release hydrofluoric acid.
  
 
===Storage===
 
===Storage===
In closed plastic (PE or PP) bottles. Avoid storing it in glass containers.
+
Sodium fluoride is best kept in closed plastic (PE or PP) bottles. Avoid storing it in glass containers. Keep the bottle in a dry place.
  
 
===Disposal===
 
===Disposal===
Should be converted to the less soluble calcium fluoride and dumped in trash. Recycling is also an option.
+
Should be converted to the less soluble [[calcium fluoride]] and dumped in trash. Recycling is also an option.
  
 
==References==
 
==References==
 
<references/>
 
<references/>
 
===Relevant Sciencemadness threads===
 
===Relevant Sciencemadness threads===
*[http://www.sciencemadness.org/talk/viewthread.php?tid=72030 Fluorides from PTFE]
+
*[https://www.sciencemadness.org/whisper/viewthread.php?tid=158855 Uses for NaF]
*[http://www.sciencemadness.org/talk/viewthread.php?tid=13524 fluoride from toothpaste?]
+
*[http://www.sciencemadness.org/talk/viewthread.php?tid=155350 Sodium fluoride synthesis? [safety issues concerning HF]]
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=2424 Sodium fluoride attacks glass?]
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=2424 Sodium fluoride attacks glass?]
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=22229 sodium fluoride from calcium fluoride and sodium phosphate]
 
*[http://www.sciencemadness.org/talk/viewthread.php?tid=22229 sodium fluoride from calcium fluoride and sodium phosphate]
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=72030 Fluorides from PTFE]
 +
*[http://www.sciencemadness.org/talk/viewthread.php?tid=13524 fluoride from toothpaste?]
  
 
[[Category:Chemical compounds]]
 
[[Category:Chemical compounds]]

Latest revision as of 20:30, 16 October 2022

Sodium fluoride
Names
IUPAC name
Sodium fluoride
Other names
Florocid
Properties
NaF
Molar mass 41.988173 g/mol
Appearance White solid
Odor Odorless
Density 2.558 g/cm3
Melting point 993 °C (1,819 °F; 1,266 K)
Boiling point 1,704 °C (3,099 °F; 1,977 K)
3.64 g/100 ml (0 °C)
4.04 g/100 ml (20 °C)
5.05 g/100 ml (100 °C)
Solubility Reacts with sulfuric acid
Slightly soluble in ammonia, hydrofluoric acid
Negligible in acetone, dimethylformamide, ethanol, methanol, liq. SO2
Insoluble in halocarbons, hydrocarbons
Vapor pressure ~0 mmHg
Acidity (pKa) 7.4
Thermochemistry
51.3 J·mol−1·K−1
-573.6 kJ/mol
Hazards
Safety data sheet Sigma-Aldrich
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
52–200 mg/kg (oral in rats, mice, rabbits)
Related compounds
Related compounds
Sodium chloride
Sodium bromide
Sodium iodide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Sodium fluoride is an inorganic compound with the formula NaF, a salt of hydrofluoric acid.

Properties

Chemical

Addition of a strong acid, like sulfuric acid will release hydrofluoric acid.

2 NaF + H2SO4 → 2 HF + Na2SO4

Physical

Sodium fluoride is a white solid, poorly soluble in water and most solvents.

Availability

Sodium fluoride is sold by chemical suppliers, though it's sometimes pricey, depending on the seller.

It occurs in nature as the rare mineral villiaumite.

Preparation

Can be prepared by neutralizing hydrofluoric acid with a base, like sodium hydroxide, sodium carbonate or sodium bicarbonate.

HF + NaOH → NaF + H2O
2 HF + Na2CO3 → 2 NaF + H2O + CO2
HF + NaHCO3 → NaF + H2O + CO2

Due to its poor solubility, sodium fluoride will precipitate out of the solution.

Projects

  • Make hydrofluoric acid
  • Make fluorocarbons
  • Mineral collecting (villiaumite)

Handling

Safety

Sodium fluoride is poisonous, and it's toxic if ingested, inhaled or injected.

Avoid contact with strong acids, as it will release hydrofluoric acid.

Storage

Sodium fluoride is best kept in closed plastic (PE or PP) bottles. Avoid storing it in glass containers. Keep the bottle in a dry place.

Disposal

Should be converted to the less soluble calcium fluoride and dumped in trash. Recycling is also an option.

References

Relevant Sciencemadness threads