Strontium nitrate

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.

Strontium nitrate
Strontium nitrate.png
Names
IUPAC name
Strontium nitrate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.107 Edit this at Wikidata
EC Number
  • 233-131-9
UNII
Properties
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)[1]
Melting point 570 °C (1,058 °F; 843 K) (anhydrous)
100 °C, decomposes (tetrahydrate)
Boiling point 645 °C (1,193 °F; 918 K) decomposes
anhydrous:
710 g/L (18 °C)
660 g/L (20 °C)
tetrahydrate:
604.3 g/L (0 °C)
2065 g/L (100 °C)
Solubility soluble in ammonia
very slightly soluble in ethanol, acetone
insoluble in nitric acid
−57.2·10−6 cm3/mol
Structure
cubic (anhydrous)
monoclinic (tetrahydrate)
Hazards
Main hazards Irritant
Safety data sheet [1]
NFPA 704 (fire diamond)
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
2750 mg/kg (rat, oral)
Related compounds
Other anions
Strontium sulfate
Strontium chloride
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).
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Infobox references

PreparationEdit

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

2 HNO3 + SrCO3 → Sr(NO3)2 + H2O + CO2
 
The reaction of nitric acid and strontium carbonate to form strontium nitrate

UsesEdit

Like many other strontium salts, strontium nitrate is used to produce a rich red flame in fireworks and road flares. The oxidizing properties of this salt are advantageous in such applications.[3]

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.[4]

BiochemistryEdit

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

In popular cultureEdit

In his short story "A Germ-Destroyer", Rudyard Kipling refers to strontium nitrate as the main ingredient of the titular fumigant. Sr

ReferencesEdit

  1. ^ Patnaik, Pradyot (2002). Handbook of Inorganic Chemicals. McGraw-Hill, ISBN 0-07-049439-8
  2. ^ Ward, R.; Osterheld, R. K.; Rosenstein, R. D. (1950). Strontium Sulfide and Selenide Phosphors. Inorganic Syntheses. 3. pp. 11–23. doi:10.1002/9780470132340.ch4. ISBN 978-0-470-13234-0.
  3. ^ MacMillan, J. Paul; Park, Jai Won; Gerstenberg, Rolf; Wagner, Heinz; Köhler, Karl and Wallbrecht, Peter (2002) "Strontium and Strontium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. doi:10.1002/14356007.a25_321
  4. ^ 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.