Strontium nitrate
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| Names | |
|---|---|
| IUPAC name
Strontium nitrate | |
| Identifiers | |
3D model (JSmol) |
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| ChemSpider | |
| ECHA InfoCard | 100.030.107 |
| EC Number |
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PubChem CID |
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| UNII | |
CompTox Dashboard (EPA) |
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| Properties | |
| Sr(NO3)2 | |
| Molar mass |
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| Appearance | white crystalline solid |
| Density |
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| Melting point |
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| Boiling point | 645 °C (1,193 °F; 918 K)[2] decomposes |
| Solubility in ammonia | soluble |
| Solubility in ethanol | slightly soluble |
| Solubility in acetone | slightly soluble |
| log P | 0.19[2] |
| Band gap | 3.71 eV[4] |
| 57.2×10−6 cm3/mol[5] | |
| Structure (anhydrous)[4] | |
| Cubic | |
| Pa3 | |
| m3 | |
a = 7.76 Å, b = 7.76 Å, c = 7.76 Å α = 90°, β = 90°, γ = 90° | |
Lattice volume (V) |
466.47 Å3 |
Formula units (Z) |
4 |
| Structure (tetrahydrate)[citation needed] | |
| Monoclinic | |
| Thermochemistry (anhydrous)[5] | |
Heat capacity (C) |
149.9 J⋅mol−1·K-1 |
Std molar entropy (S⦵298) |
194.6 J⋅mol−1·K-1 |
Std enthalpy of formation (ΔfH⦵298) |
−978.2 kJ⋅mol−1 |
Gibbs free energy (ΔfG⦵) |
−780.0 kJ⋅mol−1 |
Enthalpy of fusion (ΔfH⦵fus) |
44.6 kJ⋅mol−1 |
| Hazards | |
| GHS labelling:[2] | |
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| Danger | |
| H271, H318, H402 | |
| P210, P220, P221, P273, P280, P283, P305+P351+P338+P310, P306+P360, P370+P378, P371+P380+P375, P501 | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) |
2750 mg/kg (rat, oral)[3] |
LC50 (median concentration) |
>4.5 mg/L (rat, 4h, inhalation)[3] |
| Related compounds | |
Other anions |
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Other cations |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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
[edit]Strontium nitrate is typically generated by the reaction of nitric acid with strontium carbonate.[6]
- 2 HNO3 + SrCO3 → Sr(NO3)2 + H2O + CO2
Uses
[edit]Pyrotechnics
[edit]Like many other strontium salts, strontium nitrate is used to produce a rich red flame in fireworks and road flares. Unlike most other commonly used color-producing compounds,[a] strontium emits light in almost the same range from their hydroxides and oxides as their chlorides, with the chlorides emitting a slightly deeper red. Oxidizers break down into their oxides and hydroxides upon combustion of a pyrotechnic mixture, generally speaking.[8] Combined with strontium nitrate's high strength as an oxidizer, extremely pure colors in the orange-red to red color range are attainable with simple compositions using it as both oxidizer and colorant and without chlorine donors.[9][10]
Experimental medicine
[edit]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.[11]
Biochemistry
[edit]As a divalent ion with an ionic radius similar to that of Ca2+ (1.13 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]
Notes
[edit]References
[edit]- ↑ Patnaik P (2003). Handbook of inorganic chemicals. New York, NY: McGraw-Hill. ISBN 0-07-049439-8.
- 1 2 3 4 5 Sigma-Aldrich Co., Strontium Nitrate. Retrieved on 1 January 2026.
- 1 2 3 4 "Strontium Nitrate Anhydrous (Crystalline/Certified ACS), Fisher Chemical 100 g | Fisher Scientific". www.fishersci.com. ThermoFisher Scientific. 18 December 2025. Retrieved 2 January 2026.
- 1 2 "Strontium nitrate - Materials Explorer". next-gen.materialsproject.org. The Materials Project. mp-4157. Retrieved 3 May 2026.
- 1 2 Haynes WM, ed. (2016). CRC Handbook of Chemistry and Physics (97th ed.). Boca Raton, Florida: CRC Press. pp. 4–130, 5–36, 6–161. ISBN 9781498754293.
- ↑ Ward, R., Osterheld, R. K., Rosenstein, R. D. "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.
- ↑ Meyerriecks W, Kosanke K (2003). "Color Values and Spectra of the Principal Emitters in Colored Flames" (PDF). Journal of Pyrotechnics (18): 15. Retrieved 2 January 2026.
- ↑ Ding D, Tabata D, Yoshida T (19 October 2009). "Characteristics of the Red Colored Flame of Firework Compositions" (PDF). Journal of Pyrotechnics (28): 51–60. 0079. Retrieved 2 January 2026.
- ↑ 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.
