Strontium nitrate

Strontium nitrate
Names
	IUPAC name Strontium nitrate
Identifiers
CAS Number	10042-76-9 ;
3D model (JSmol)	Interactive image;
ChemSpider	23231 ;
ECHA InfoCard	100.030.107
EC Number	233-131-9;
PubChem CID	24848;
UNII	BDG873AQZL ;
CompTox Dashboard (EPA)	DTXSID9064924 ;
	InChI InChI=1S/2NO3.Sr/c22-1(3)4;/q2-1;+2 Key: DHEQXMRUPNDRPG-UHFFFAOYSA-N ; InChI=1/2NO3.Sr/c22-1(3)4;/q2-1;+2 Key: DHEQXMRUPNDRPG-UHFFFAOYAG;
	SMILES [Sr+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O;
Properties
Chemical formula	Sr(NO3)2
Molar mass	211.630 g/mol (anhydrous); 283.69 g/mol (tetrahydrate);
Appearance	white crystalline solid
Density	2.986 g/cm3 (anhydrous); 2.20 g/cm3 (tetrahydrate)[page needed];
Melting point	570 °C (1,058 °F) (anhydrous); 100 °C (212 °F), decomposes (tetrahydrate);
Boiling point	645 °C (1,193 °F; 918 K) decomposes
Solubility in water	anhydrous: 710 g/L (18 °C (64 °F)); 660 g/L (20 °C (68 °F)); ; tetrahydrate: 604.3 g/L (0 °C (32 °F)); 2065 g/L (100 °C (212 °F)); ;
Solubility in ammonia	soluble
Solubility in ethanol	slightly soluble
Solubility in acetone	slightly soluble
Solubility in nitric acid	insoluble
Magnetic susceptibility (χ)	57.2×10−6 cm3/mol
Structure
Crystal structure	cubic (anhydrous); monoclinic (tetrahydrate);
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Irritant
NFPA 704 (fire diamond)	2 0 0 OX
Flash point	Non-flammable
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	2750 mg/kg (rat, oral)
Safety data sheet (SDS)	[1]
Related compounds
Other anions	Strontium carbonate; Strontium chloride; Strontium sulfate;
Other cations	Beryllium nitrate; Magnesium nitrate; Calcium nitrate; Barium nitrate;
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Strontium nitrate is an inorganic compound composed of the elements strontium, nitrogen and oxygen with the formula Sr(NO₃)₂. This colorless solid is used as a red colorant and oxidizer in pyrotechnics.

Preparation

Strontium nitrate is typically generated by the reaction of nitric acid with strontium carbonate.^[2]

2 HNO₃ + SrCO₃ → Sr(NO₃)₂ + H₂O + CO₂

Uses

Like many other strontium salts, strontium nitrate is used to produce a rich red flame in fireworks and road flares. Its strength as an oxidizer, which eliminates the need for large amounts of an additional chlorine-containing oxidizer, makes extremely pure colors in the orange-red to red color range attainable with simple compositions.^[3]^[4]

Strontium nitrate can aid in eliminating and lessening skin irritations. When mixed with glycolic acid, strontium nitrate reduces the sensation of skin irritation significantly better than using glycolic acid alone.^[5]

Biochemistry

As a divalent ion with an ionic radius similar to that of Ca²⁺ (1.13 Å and 0.99 Å respectively), Sr²⁺ ions mimic calcium's ability to traverse calcium-selective ion channels and trigger neurotransmitter release from nerve endings. It is thus used in electrophysiology experiments.^{[citation needed]}

References

^ Patnaik P (2003). Handbook of inorganic chemicals. New York, NY: McGraw-Hill. ISBN 0-07-049439-8.
^ Ward, R., Osterheld, R. K., Rosenstein, R. D. (1950). "Strontium Sulfide and Selenide Phosphors". Inorganic Syntheses. Inorganic Syntheses. Vol. 3. pp. 11–23. doi:10.1002/9780470132340.ch4. ISBN 978-0-470-13234-0. {{cite book}}: ISBN / Date incompatibility (help)
^ MacMillan JP, Park JW, Gerstenberg R, Wagner H, Köhler K, Wallbrecht P. ""Strontium and Strontium Compounds"". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a25_321. ISBN 978-3-527-30673-2.
^ Juknelevicius D, Mikoliunaite L, Sakirzanovas S, Kubilius R, Ramanavicius A (October 2014). "A Spectrophotometric Study of Red Pyrotechnic Flame Properties Using Three Classical Oxidizers: Ammonium Perchlorate, Potassium Perchlorate, Potassium Chlorate". Zeitschrift für anorganische und allgemeine Chemie. 640 (12–13): 2560–2565. doi:10.1002/zaac.201400299.
^ Zhai H, Hannon W, Hahn GS, Pelosi A, Harper RA, Maibach HI (2000). "Strontium nitrate suppresses chemically-induced sensory irritation in humans". Contact Dermatitis. 42 (2): 98–100. doi:10.1034/j.1600-0536.2000.042002098.x. PMID 10703633. S2CID 25910851.

[1] Patnaik P (2003). Handbook of inorganic chemicals. New York, NY: McGraw-Hill. ISBN 0-07-049439-8.

[Ward-2] Ward, R., Osterheld, R. K., Rosenstein, R. D. (1950). "Strontium Sulfide and Selenide Phosphors". Inorganic Syntheses. Inorganic Syntheses. Vol. 3. pp. 11–23. doi:10.1002/9780470132340.ch4. ISBN 978-0-470-13234-0. {{cite book}}: ISBN / Date incompatibility (help)

[3] MacMillan JP, Park JW, Gerstenberg R, Wagner H, Köhler K, Wallbrecht P. ""Strontium and Strontium Compounds"". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a25_321. ISBN 978-3-527-30673-2.

[4] Juknelevicius D, Mikoliunaite L, Sakirzanovas S, Kubilius R, Ramanavicius A (October 2014). "A Spectrophotometric Study of Red Pyrotechnic Flame Properties Using Three Classical Oxidizers: Ammonium Perchlorate, Potassium Perchlorate, Potassium Chlorate". Zeitschrift für anorganische und allgemeine Chemie. 640 (12–13): 2560–2565. doi:10.1002/zaac.201400299.

[Zhai-5] Zhai H, Hannon W, Hahn GS, Pelosi A, Harper RA, Maibach HI (2000). "Strontium nitrate suppresses chemically-induced sensory irritation in humans". Contact Dermatitis. 42 (2): 98–100. doi:10.1034/j.1600-0536.2000.042002098.x. PMID 10703633. S2CID 25910851.

[1]

[2]

[3]

[4]

[5]