Strontium nitrate

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Strontium nitrate
Strontium nitrate.png
IUPAC name
Strontium nitrate
10042-76-9 YesY
ChemSpider 23231 YesY
EC number 233-131-9
Jmol-3D images Image
PubChem 24848
Molar mass 211.630 g/mol (anhydrous)
283.69 g/mol (tetrahydrate)
Appearance white granular 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
71 g/100 mL (18 °C)
66 g/100 mL (20 °C)
60.43 g/100 mL (0 °C)
206.5 g/100 mL (100 °C)
Solubility soluble in ammonia
very slightly soluble in ethanol, acetone
insoluble in nitric acid
Crystal structure cubic (anhydrous)
monoclinic (tetrahydrate)
Main hazards Irritant
EU Index Not listed
Flash point Non-flammable
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 noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Strontium nitrate is an inorganic compound with the formula Sr(NO3)2. This colourless solid is used as a colorant (red) in pyrotechnics and is also used as an oxidizer in pyrotechnics.


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



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]


As a divalent ion with an ionic radius similar to that of Ca2+ (1.13 vs. 0.99 A, 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.


  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. ^ Ward, R.; Osterheld, R. K.; Rosenstein, R. D. (1950). "Strontium Sulfide and Selenide Phosphors". Inorg. Synth. Inorganic Syntheses 3: 11–23. doi:10.1002/9780470132340.ch4. ISBN 978-0-470-13234-0 
  3. ^ J. Paul MacMillan, Jai Won Park, Rolf Gerstenberg, Heinz Wagner, Karl Köhler, Peter Wallbrecht "Strontium and Strontium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2002. doi:10.1002/14356007.a25_321
  4. ^ Zhai, H; Hannon, Hahn, Pelosi, Harper, Maibach (2000). "Strontium nitrate suppresses chemically-induced sensory irritation in humans". Contact dermatitis 11 (2): 98–100. PMID 10703633. 
Salts and the ester of the Nitrate ion
LiNO3 Be(NO3)2 B(NO3)4 RONO2 NO3
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)3 Co(NO3)2,
Ni(NO3)2 Cu(NO3)2 Zn(NO3)2 Ga(NO3)3 Ge As Se Br Kr
RbNO3 Sr(NO3)2 Y Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb Te I XeFNO3
CsNO3 Ba(NO3)2   Hf Ta W Re Os Ir Pt Au Hg2(NO3)2,
Tl(NO3)3 Pb(NO3)2 Bi(NO3)3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Uut Fl Uup Lv Uus Uuo
La Ce(NO3)x Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr