Strontium nitrate






























































































































Strontium nitrate

Strontium nitrate.png
Names

IUPAC name
Strontium nitrate

Identifiers

CAS Number

  • 10042-76-9 ☑Y

3D model (JSmol)
  • Interactive image

ChemSpider

  • 23231 ☑Y

ECHA InfoCard
100.030.107

EC Number
 233-131-9


PubChem CID
  • 24848

UNII

  • BDG873AQZL ☑Y


CompTox Dashboard (EPA)
  • DTXSID9064924 Edit this at Wikidata




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)[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

Solubility in water
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


Magnetic susceptibility (χ)

 −57.2·10−6 cm3/mol
Structure

Crystal structure

 cubic (anhydrous)
monoclinic (tetrahydrate)
Hazards
Main hazards
 Irritant

Safety data sheet
[1]

NFPA 704


Flammability code 0: Will not burn. E.g., water
Health code 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g., chloroform
Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen
Special hazard OX: Oxidizer. E.g., potassium perchlorateNFPA 704 four-colored diamond


0


2


0

OX

Flash point
 Non-flammable
Lethal dose or concentration (LD, LC):


LD50 (median dose)

 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).


☒N verify (what is ☑Y☒N ?)

Infobox references

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




Contents






  • 1 Preparation


  • 2 Uses


  • 3 Biochemistry


  • 4 In popular culture


  • 5 References





Preparation


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


.




Uses


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]



Biochemistry


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.



In popular culture


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



References




  1. ^ Patnaik, Pradyot (2002). Handbook of Inorganic Chemicals. McGraw-Hill, .mw-parser-output cite.citation{font-style:inherit}.mw-parser-output .citation q{quotes:"""""""'""'"}.mw-parser-output .citation .cs1-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-limited a,.mw-parser-output .citation .cs1-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration{color:#555}.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration span{border-bottom:1px dotted;cursor:help}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/12px-Wikisource-logo.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output code.cs1-code{color:inherit;background:inherit;border:inherit;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;font-size:100%}.mw-parser-output .cs1-visible-error{font-size:100%}.mw-parser-output .cs1-maint{display:none;color:#33aa33;margin-left:0.3em}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-format{font-size:95%}.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-right{padding-right:0.2em}
    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. ^ 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.



























































































































































  • v

  • t

  • e


Salts and covalent derivatives of the nitrate ion


HNO3


He

LiNO3
Be(NO3)2
B(NO
3)−
4
 C
NO−
3,
NH4NO3
 O
FNO3
 Ne

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,
Fe(NO3)2
Co(NO3)2,
Co(NO3)3
Ni(NO3)2
Cu(NO3)2
Zn(NO3)2
Ga(NO3)3
 Ge
 As
 Se
 Br
 Kr

RbNO3
Sr(NO3)2
Y(NO3)3
Zr(NO3)4
 Nb
 Mo
 Tc
 Ru
 Rh
Pd(NO3)2
AgNO3
Cd(NO3)2
 In
 Sn
Sb(NO3)3
 Te
 I
Xe(NO3)2

CsNO3
Ba(NO3)2
  
 Hf
 Ta
 W
 Re
 Os
 Ir
 Pt
 Au
Hg2(NO3)2,
Hg(NO3)2
Tl(NO3)3,
TlNO3
Pb(NO3)2
Bi(NO3)3
BiO(NO3)
 Po
 At
 Rn

FrNO3
Ra(NO3)2
  
 Rf
 Db
 Sg
 Bh
 Hs
 Mt
 Ds
 Rg
 Cn
 Nh
 Fl
 Mc
 Lv
 Ts
 Og

↓


La(NO3)3
Ce(NO3)3,
Ce(NO3)4
 Pr
Nd(NO3)3
 Pm
 Sm
Eu(NO3)3
Gd(NO3)3
Tb(NO3)3
 Dy
 Ho
 Er
 Tm
 Yb
 Lu

Ac(NO3)3
Th(NO3)4
 Pa
UO2(NO3)2
 Np
 Pu
 Am
 Cm
 Bk
 Cf
 Es
 Fm
 Md
 No
 Lr







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