Sodium nitrate

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Sodium nitrate
Sodium nitrate.jpg
Crystals of NaNO3 obtained via evaporation
IUPAC name
Sodium nitrate
Other names
Chilean saltpeter
Cubic niter
Peru saltpeter
Soda niter
Molar mass 84.9947 g/mol
Appearance White solid
Odor Odorless
Density 2.257 g/cm3
Melting point 308 °C (586 °F; 581 K) (decomposition begins)
Boiling point Decomposes
73 g/100 ml (0 °C)
91.2 g/100 ml (25 °C)
180 g/100 ml (100 °C)
Solubility Very soluble in ammonia, hydrazine
Soluble in ethanol, methanol
Slightly soluble in pyridine
Insoluble in acetone
Vapor pressure ~0 mmHg
116 J·mol-1·K-1
−467 kJ/mol
Safety data sheet Sigma-Aldrich
Lethal dose or concentration (LD, LC):
3,236 mg/kg
Related compounds
Related compounds
Lithium nitrate
Potassium nitrate
Rubidium nitrate
Caesium nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Sodium nitrate (also known as Chilean saltpeter) is a sodium salt with the chemical formula NaNO3.



Sodium nitrate decomposes in the presence of a metal to yield sodium nitrite:

2 NaNO3 → 2 NaNO2 + O2

Reaction with sulfuric acid produces nitric acid:

NaNO3 + H2SO4 → HNO3 + NaHSO4
2 NaNO3 + H2SO4 → 2 HNO3 + Na2SO4

Potassium nitrate, typically more desired as an oxidizer than sodium nitrate, can be produced in a somewhat impure form by cooling a hot saturated solution containing the proper molar amounts of both sodium nitrate and potassium sulfate. Because sodium sulfate is much less soluble than potassium nitrate, most of it will crystallize out of solution fairly quickly.


Sodium nitrate is a white solid which is very soluble in water. Unlike its potassium counterpart, sodium nitrate is hygroscopic. It's soluble in methanol, ethanol, ammonia, and hydrazine, but not in acetone.


Sodium nitrate is sold as a meat curing salt and food additive, sometimes in pharmacies. It can also be bought in larger quantities as fertilizers, which are often impure. Sodium nitrate is cheaper to produce than buy in places with easy access to ammonium nitrate.


Sodium nitrate is prepared industrially by neutralizing nitric acid with sodium carbonate or sodium bicarbonate.

2 HNO3 + Na2CO3 → 2 NaNO3 + H2O + CO2
HNO3 + NaHCO3 → NaNO3 + H2O + CO2

An easier route involves mixing a solution of sodium hydroxide and ammonium nitrate, which can be made even easier with the use of sodium bicarbonate or carbonate:

NH4NO3 + NaOH → NaNO3 + NH4OH
NH4NO3 + NaHCO3 → NaNO3 + NH3 + H2O + CO2 (Requires heating in solution to complete)
2 NH4NO3 + Na2CO3 → 2 NaNO3 + 2 NH3 + H2O + CO2 (Requires heating in solution to complete)

Since ammonium hydroxide will quickly decompose in the basic conditions to release ammonia, the solution will contain fairly pure sodium nitrate, though heating may be required to finish decomposing it:

NH4OH → NH3 + H2O

This reaction should be performed outside or in a fume hood. The reaction is self-sustaining and proceeds very quickly with wet sodium hydroxide and more slowly in dry conditions, but with the carbonate or bicarbonate is easily controlled and requires a long period of boiling of the solution.




Sodium nitrate is not very toxic, and as long as it is not consumed it's safe to handle. Medical studies indicate that long-term consumption increases the risk of several illnesses, such as stomach cancer, diabetes mellitus and Alzheimer.

Because it's hygroscopic, sodium nitrate is a poor oxidizer unless kept completely dry, through much effort, until it is used.


Sodium nitrate should be stored in closed containers, due to its hygroscopicity.


Sodium nitrate doesn't require special disposal, although it's best to avoid releasing it in the environment due to its sodium ions.



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