Sodium nitrate

Sodium nitrate ;
Names:	sodium nitrate; nitrate of soda; chile saltpeter; Peru saltpeter; soda niter; cubic niter; Е251 food additive;
Formula:	NaNO3;
Molar mass:	84.994 g/mol;
Density:	2.257 g/cm3;
Crystal system:	hexagonal; a=5.0665 Å, b=5.0665 Å, c=16.577 Åα=90°, β=90°, γ=120°;
Shapes:	https://en.crystalls.info/w/uploads/media/3/36/Oblique_rhombic_prism.json Oblique rhombic prism https://en.crystalls.info/w/uploads/media/b/bc/Rhombic_prism.json Rhombic prism https://en.crystalls.info/w/uploads/media/3/37/Octahedron.json Octahedron ;
Color:	colorless; white;
Melting point:	308 °C581.15 K <br />586.4 °F <br />1,046.07 °R <br />;
Decomposition point:	380 °C653.15 K <br />716 °F <br />1,175.67 °R <br />;
Refractive index:	1.336 (orthorhombic); 1.587 (rhombohedral);
Optical properties:	birefringence;
Magnetic properties:	diamagnetic; χ=-2.56 · 10-5cm³/mol;
Stability:	stable;
Hardness:	relatively strong; (2 on Moh's scale);
Toxicity:	non-toxic; LD50=3236mg/kg

Description

Inorganic compound, salt of alkaline metal sodium and inorganic nitric acid. Doesn't form water hydrates.

Precursors

Reaction between sodium hydroxide or carbonate and nitric acid

Chemical equation:

NaOH + HNO₃ = NaNO₃ + H₂O

Na₂CO₃ + 2HNO₃ = 2NaNO₃ + 2H₂O + CO₂↑

For preparation of 100.00g of sodium nitrate а 47.06g of sodium hydroxide or 62.35g of carbonate and 114.06g of 65%65% acid is required.

Add acid to the flask, then add small parts of sodium compound with stirring until it will totally dissolve or, if you use carbonate, until carbon dioxide emission will stop. After reaction will stop, filter the solution and use it for crystal growing.

Reaction between excess of sodium hydroxide or carbonate and ammonium nitrate

Chemical equation:

NH₄NO₃ + NaOH = NaNO₃ + H₂O + NH₃↑

2NH₄NO₃ + Na₂CO₃ = 2NaNO₃ + 2H₂O + 2NH₃↑ + CO₂↑

For preparation of 100.00g of sodium nitrate а 47.06g of sodium hydroxide or 62.35g of carbonate and 94.17g of ammonium nitrate is required.

Add to the flask saturated solution of sodium compounds and then add small parts of hot nitrate ammonium solution with heating and stirring. Emission of large amount of ammonia will begin.Attention, exuding ammonia irritates eyes and lungs! The synthesis should be carried out only in a fume hood or outdoors!

Reaction between sodium chloride and ammonium nitrate

Chemical equation:

NH₄NO₃ + NaCl = NaNO₃↓ + NH₄Cl

For preparation of 100.00g of sodium nitrate а 68.76g of sodium chloride and 94.17g of ammonium nitrate is required.

Add to the flask with hot nitrate ammonium solution a chloride sodium solution with stirring. Cooling this mixture will cause forming a large amount of crystalline precipitate. Filter precipitate and wash it wish small amount of cold water, then filter the solution and use it for crystal growing.

Reaction between calcium or lead(II) nitrate and sodium hydroxide, carbonate or sulfate

You can use sodium chloride instead of sulfate in reaction with lead salt.
Chemical equation:

Ca(NO₃)₂ + 2NaOH = Ca(OH)₂↓ + 2NaNO₃

Pb(NO₃)₂ + 2NaOH = Pb(OH)₂↓ + 2NaNO₃

Ca(NO₃)₂ + Na₂CO₃ = CaCO₃↓ + 2NaNO₃

Pb(NO₃)₂ + Na₂CO₃ = PbCO₃↓ + 2NaNO₃

Ca(NO₃)₂ + Na₂SO₄ = CaSO₄↓ + 2NaNO₃

Pb(NO₃)₂ + Na₂SO₄ = PbSO₄↓ + 2NaNO₃

Pb(NO₃)₂ + 2NaCl = PbCl₂↓ + 2NaNO₃

For preparation of 100.00g of sodium nitrate а 47.06g of sodium hydroxide or 62.35g of carbonate or 83.56g of sulfate or 68.76g of chloride and 194.84g of lead(II) nitrate or 138.92g of calcium nitrate

tetrahydratetetrahydrate
anhydrous

is required.

Add to the flask with calcium or lead nitrate solution small parts of sodium salt solution and stir. The large amount of poorly soluble precipitate will form. Settle it out and discard, then filter the solution carefully.

Notes

Dissolving is endothermic, solution cools much, so use hot water or using heat.

Storage conditions

Keep in its original form or under several layers of varnish at average humidity and room temperature. Do not keep crystals near heaters.

Solubility

TableGraph

Temperature	g/`100,00` g water	g/`100,00` g ethanol 50%	g/`100,00` g ethanol	g/`100,00` g methanol	g/`100,00` g diethyl ether	g/`100,00` g pyridine	g/`100,00` g nitric acid	g/`100,00` g acetic acid	g/`100,00` g ammonia	g/`100,00` g hydrazine	g/`100,00` g hydroxylamine	g/`100,00` g dimethylformamide	g/`100,00` g ethylenediamine
0°C273.15 K <br />32 °F <br />491.67 °R <br />	`72.7`								`127`
10°C283.15 K <br />50 °F <br />509.67 °R <br />	`79.9`
20°C293.15 K <br />68 °F <br />527.67 °R <br />	`87.6`				`0.0196`		`1.5`			`100`	`13.1`
25°C298.15 K <br />77 °F <br />536.67 °R <br />	`91.6`	`19.4`	`0.036`	`0.41`		`0.35`		`0.173`				`15.4`	`33.5`
30°C303.15 K <br />86 °F <br />545.67 °R <br />	`96.1`							`0.197`
40°C313.15 K <br />104 °F <br />563.67 °R <br />	`104.9`							`0.246`
50°C323.15 K <br />122 °F <br />581.67 °R <br />	`114.1`
60°C333.15 K <br />140 °F <br />599.67 °R <br />	`124.7`
80°C353.15 K <br />176 °F <br />635.67 °R <br />	`149`
100°C373.15 K <br />212 °F <br />671.67 °R <br />	`176`							`1.22`

Soluble in ethanol. Slightly soluble in pyridine. Insoluble in acetone.

Gallery

Video

Sources

Nitrates
Salts	Ammonium nitrate (NH₄NO₃) • Barium nitrate (Ba(NO₃)₂) • Bismuth(III) nitrate (BI(NO₃)₃) • Calcium nitrate (Ca(NO₃)₂) • Cesium nitrate (CsNO₃) • Cobalt(II) nitrate (Co(NO₃)₂) • Copper(II) nitrate (Cu(NO₃)₂) • Iron(II) nitrate (Fe(NO₃)₂) • Lead(II) nitrate (Pb(NO₃)₂) • Neodymium nitrate (Nd(NO₃)₃) • Nickel nitrate (Ni(NO₃)₂) • Potassium nitrate (KNO₃) • Silver(I) nitrate (AgNO₃) • Sodium nitrate (NaNO₃) • Strontium nitrate (Sr(NO₃)₂) • Uranyl nitrate (UO₂(NO₃)₂) • Zirconyl nitrate (ZrO(NO₃)₂)
Double salts	Calcium-ammonium nitrate (5Ca(NO₃)₂ · NH₄NO₃) • Cerium(IV)-ammomium nitrate (2NH₄NO₃ · Ce(NO₃)₄) • Cerium(III)-cobalt nitrate (3Co(NO₃)₂ · 2Ce(NO₃)₃) • Cerium(III)-cobalt-manganese nitrate (3(Co,Mn)(NO₃)₂ · 2Ce(NO₃)₃) • Cerium(III)-manganese nitrate (3Mn(NO₃)₂ · 2Ce(NO₃)₃)
Complexes	Bis-thetramethylethylenediaminecopper(II) nitrate ([Cu((H₃CNCH₃)₂C₄H₈)](NO₃)₂) • Nitratopentakis-karbamatbismuth(III) nitrate ([Bi(NO₃)(CO(NH₂)₂)₅](NO₃)₂) • Nitratopentakis-tiokarbamatbismuth(III) nitrate ([Bi(NO₃)(CS(NH₂)₂)₅](NO₃)₂)

Sodium compounds
Salts	Sodium acetate (NaCH₃COO) • Sodium bromide (NaBr) • Sodium citrate (Na₃C₃H₅O(COO)₃) • Sodium chlorate (NaClO₃) • Sodium chloride (NaCl) • Sodium cyclamate (C₆H₁₂NNaO₃S) • Sodium decavanadate (Na₆V₁₀O₂₈) • Sodium ethilate (NaC₂H₅O) • Sodium glutamate (NaC₅H₈NO₄) • Sodium hydrocarbonate (NaHCO₃) • Sodium hydrosulfate (NaHSO₄) • Sodium iodide (NaI) • Sodium metavanadate (NaVO₃) • Sodium niobate (NaNbO₃) • Sodium nitrate (NaNO₃) • Sodium oxalate (Na₂C₂O₄) • Sodium para-aminosalicylate (C₇H₆NNaO₃) • Sodium perchlorate (NaClO₄) • Sodium saccharinate (C₇H₄NaNO₃S) • Sodium sulfate (Na₂SO₄) • Sodium sulfide (Na₂S) • Sodium tetraborate (Na₂B₄O₇) • Sodium thiosulfate (Na₂S₂O₃) • Sodium trichloroacetate (NaCCl₃COO) • Sodium trioxalatoaluminate (Na₃[Al(C₂O₄)₃]) • Sodium tungstate (Na₂WO₄)
Double salts	Potassium-sodium tartrate (KNaC₄H₄O₆) • Sodium-ammonium sulfate (NaNH₄SO₄) • Uranyl-sodium acetate (NaUО2(CH₃COO)₃) • Uranyl-zinc-sodium acetate (NaZn(UO₂)₃(CH₃COO)₉) • Zinc-sodium sulfate (Na₂Zn(SO₄)₂)
Adducts	Glucose and sodium bromide adduct (2C₆H₁₂O₆ · NaBr) • Glucose and sodium chloride adduct (2C₆H₁₂O₆ · NaCl) • Urea and sodium chloride adduct (CO(NH₄)₂ · NaCl)
Complex compounds	Sodium dicarbonatocuprate(II) (Na₂[Cu(CO₃)₂]) • Sodium dioxalatocuprate(II) (Na₂[Cu(C₂O₄)₂]) • Sodium ethylenediaminetetraacetate-ferrate(III) (Na[Fe((OOCCH₂)₂N(CH₂)₂N(CH₂COO)₂)]) • Sodium hexacyanoferrate(II) (Na₄[Fe(CN)₆]) • Tripotassium-sodium hexacyanoferrate(II) (K₃Na[Fe(CN)₆]) • Sodium hexafluorosilicate (Na₂[SiF₆]) • Sodium nitroprusside (Na₂[Fe(CN)₅NO]) • Sodium trioxalatochromate(III) (Ns₃[Cr(C₂O₄)₃]) • Dipotassium-sodium trioxalatoferrate(III) (K₂Na[Fe(C₂O₄)₃]) • Potassium-sodium trioxalatoferrate(III) (K₅Na[Fe(C₂O₄)₃]₂) • Sodium trioxalatoferrate(III) (Na₃[Fe(C₂O₄)₃])

Sodium nitrate
Names:	sodium nitrate nitrate of soda chile saltpeter Peru saltpeter soda niter cubic niter Е251 food additive
Formula:	NaNO₃
Molar mass:	84.994 g/mol
Density:	2.257 g/cm³
Crystal system:	hexagonal a=5.0665 Å, b=5.0665 Å, c=16.577 Åα=90°, β=90°, γ=120°
Shapes:	Oblique rhombic prism Rhombic prism Octahedron
Color:	colorless white
Melting point:	308 °C581.15 K <br />586.4 °F <br />1,046.07 °R <br />
Decomposition point:	380 °C653.15 K <br />716 °F <br />1,175.67 °R <br />
Refractive index:	1.336 (orthorhombic) 1.587 (rhombohedral)
Optical properties:	birefringence
Magnetic properties:	diamagnetic χ=-2.56 · 10^-5cm³/mol
Stability:	stable
Hardness:	relatively strong (2 on Moh's scale)
Toxicity:	non-toxic LD₅₀=3236mg/kg

Sodium nitrate

Description

Minerals

Precursors

Reaction between sodium hydroxide or carbonate and nitric acid

Reaction between excess of sodium hydroxide or carbonate and ammonium nitrate

Reaction between sodium chloride and ammonium nitrate

Reaction between calcium or lead(II) nitrate and sodium hydroxide, carbonate or sulfate

Notes

Storage conditions

Solubility

Gallery

Video

Sources

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