Strontium nitrate

Chemical compound From Wikipedia, the free encyclopedia

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.

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Strontium nitrate
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
  • InChI=1S/2NO3.Sr/c2*2-1(3)4;/q2*-1;+2 checkY
    Key: DHEQXMRUPNDRPG-UHFFFAOYSA-N checkY
  • InChI=1/2NO3.Sr/c2*2-1(3)4;/q2*-1;+2
    Key: DHEQXMRUPNDRPG-UHFFFAOYAG
  • [Sr+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O
Properties
Sr(NO3)2
Molar mass
  • 211.630 g/mol (anhydrous)
  • 283.69 g/mol (tetrahydrate)
Appearance white crystalline solid
Density
Melting point
  • 570 °C (1,058 °F; 843 K) (anhydrous)[2]
  • 100 °C (212 °F; 373 K), decomposes (tetrahydrate)
Boiling point 645 °C (1,193 °F; 918 K)[2] decomposes
  • anhydrous:
    • 660–709 g/L (20 °C (68 °F; 293 K))[2][3]
  • tetrahydrate:
    • 604.3 g/L (0 °C (32 °F; 273 K))
    • 2065 g/L (100 °C (212 °F; 373 K))
Solubility in ammonia soluble
Solubility in ethanol slightly soluble
Solubility in acetone slightly soluble
log P 0.19[2]
57.2×10−6 cm3/mol
Structure
  • cubic (anhydrous)
  • monoclinic (tetrahydrate)
Hazards
GHS labelling:[2]
GHS03: OxidizingGHS05: Corrosive
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)
[3]
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
2
0
2
OX
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
2750 mg/kg (rat, oral)[3]
>4.5 mg/L (rat, 4h, inhalation)[3]
Related compounds
Other anions
Other cations
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Preparation

Strontium nitrate is typically generated by the reaction of nitric acid with strontium carbonate.[4]

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

Uses

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 nitrate (along with other strontium compounds) emit light in almost the same range from their hydroxides and oxides as their chlorides, with the chlorides emitting a slightly deeper red.[6] 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.[7][8]

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.[9]

Biochemistry

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

  1. [a]
    See copper in particular, which can produce any of red, green, or blue / blue-violet depending on the active emitter in a flame.[5]

References

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