Strontium nitrate

Last updated
Strontium nitrate
Strontium nitrate.png
Names
IUPAC name
Strontium nitrate
Identifiers
  • 10042-76-9 Yes check.svgY
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.107 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 233-131-9
PubChem CID
UNII
  • InChI=1S/2NO3.Sr/c2*2-1(3)4;/q2*-1;+2 Yes check.svgY
    Key: DHEQXMRUPNDRPG-UHFFFAOYSA-N Yes check.svgY
  • 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)
Appearancewhite 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
NFPA 704 (fire diamond)
2
0
0
OX
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).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)
Infobox references

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.

Contents

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 Strontium Carbonate and Nitric acid.jpg
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 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 his short story "A Germ-Destroyer", Rudyard Kipling refers to strontium nitrate as the main ingredient of the titular fumigant.

Related Research Articles

Barium Chemical element, symbol Ba and atomic number 56

Barium is a chemical element with the symbol Ba and atomic number 56. It is the fifth element in group 2 and is a soft, silvery alkaline earth metal. Because of its high chemical reactivity, barium is never found in nature as a free element.

In chemistry, a salt is a chemical compound consisting of an ionic assembly of cations and anions. Salts are composed of related numbers of cations and anions so that the product is electrically neutral. These component ions can be inorganic, such as chloride (Cl), or organic, such as acetate ; and can be monatomic, such as fluoride (F), or polyatomic, such as sulfate.

Alkaline earth metal Group of chemical elements

The alkaline earth metals are six chemical elements in group 2 of the periodic table. They are beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra). The elements have very similar properties: they are all shiny, silvery-white, somewhat reactive metals at standard temperature and pressure.

Calcium fluoride is the inorganic compound of the elements calcium and fluorine with the formula CaF2. It is a white insoluble solid. It occurs as the mineral fluorite (also called fluorspar), which is often deeply coloured owing to impurities.

Hypochlorite Ion

In chemistry, hypochlorite is an anion with the chemical formula ClO. It combines with a number of cations to form hypochlorite salts. Common examples include sodium hypochlorite and calcium hypochlorite. The Cl-O distance in ClO is 210 pm.

Lithium nitrate Chemical compound

Lithium nitrate is an inorganic compound with the formula LiNO3. It is the lithium salt of nitric acid (an alkali metal nitrate). The salt is deliquescent, absorbing water to form the hydrated form, lithium nitrate trihydrate. Its eutectics are of interest for heat transfer fluids.

Barium nitrate Chemical compound

Barium nitrate is the inorganic compound with the chemical formula Ba(NO3)2. It, like most barium salts, is colorless, toxic, and water-soluble. It burns with a green flame and is an oxidizer; the compound is commonly used in pyrotechnics.

Sodium azide Chemical compound

Sodium azide is the inorganic compound with the formula NaN3. This colorless salt is the gas-forming component in legacy car airbag systems. It is used for the preparation of other azide compounds. It is an ionic substance, is highly soluble in water and is very acutely poisonous.

Strontium chloride Chemical compound

Strontium chloride (SrCl2) is a salt of strontium and chloride.

Sulfamic acid Chemical compound

Sulfamic acid, also known as amidosulfonic acid, amidosulfuric acid, aminosulfonic acid, and sulfamidic acid, is a molecular compound with the formula H3NSO3. This colourless, water-soluble compound finds many applications. Sulfamic acid melts at 205 °C before decomposing at higher temperatures to water, sulfur trioxide, sulfur dioxide and nitrogen.

Uranyl nitrate Chemical compound

Uranyl nitrate is a water soluble yellow powder with the formula UO2(NO3)2 • nH2O. The hexa-, tri-, and dihydrates are known. The compound is mainly of interest because it is an intermediate in the preparation of nuclear fuels.

An inorganic nonaqueous solvent is a solvent other than water, that is not an organic compound. These solvents are used in chemical research and industry for reactions that cannot occur in aqueous solutions or require a special environment. Inorganic nonaqueous solvents can be classified into two groups, protic solvents and aprotic solvents. Early studies on inorganic nonaqueous solvents evaluated ammonia, hydrogen fluoride, sulfuric acid, as well as more specialized solvents, hydrazine, and selenium oxychloride.

Aluminium nitrate Chemical compound

Aluminium nitrate is a white, water-soluble salt of aluminium and nitric acid, most commonly existing as the crystalline hydrate, aluminium nitrate nonahydrate, Al(NO3)3·9H2O.

α-Hydroxy acids, or alpha hydroxy acids (AHAs), are a class of chemical compounds that consist of a carboxylic acid substituted with a hydroxyl group on the adjacent carbon. They may be naturally occurring or synthetic. AHAs are well known for their use in the cosmetics industry. They are often found in products that aid in the reduction of wrinkles, that soften strong, defining lines, and that improve the overall look and feel of the skin. They are also used as chemical peels. AHAs have effective results through continuous treatment in the cosmeceutical industry.

Mercury(II) nitrate Chemical compound

Mercury(II) nitrate is a toxic colorless or white soluble crystalline mercury(II) salt of nitric acid. It was used to treat fur to make felt in a process called 'carroting'. The phrase 'mad as a hatter' is associated with psychological illness brought on by excessive exposure to mercury(II) nitrate. The practice continued in the United States until it was banned in December 1941 by the United States Public Health Service. The ban freed mercury(II) nitrate to be used in the manufacture of detonators in the then ongoing war.

Lead(IV) acetate Chemical compound

Lead(IV) acetate or lead tetraacetate is a chemical compound with chemical formula Pb(C2H3O2)4. It is a colorless solid that is soluble in nonpolar organic solvents, indicating that it is not a salt. It is degraded by moisture and is typically stored with additional acetic acid. The compound is used in organic synthesis.

Strontium sulfate Chemical compound

Strontium sulfate (SrSO4) is the sulfate salt of strontium. It is a white crystalline powder and occurs in nature as the mineral celestine. It is poorly soluble in water to the extent of 1 part in 8,800. It is more soluble in dilute HCl and nitric acid and appreciably soluble in alkali chloride solutions (e.g. sodium chloride).

Cobalt(II) nitrate Chemical compound

Cobalt nitrate is the inorganic compound with the formula Co(NO3)2.xH2O. It is cobalt(II)'s salt. The most common form is the hexahydrate Co(NO3)2·6H2O, which is a red-brown deliquescent salt that is soluble in water and other polar solvents.

Gallium nitrate Chemical compound

Gallium nitrate (brand name Ganite) is the gallium salt of nitric acid with the chemical formula Ga(NO3)3. It is a drug used to treat symptomatic hypercalcemia secondary to cancer. It works by preventing the breakdown of bone through the inhibition of osteoclast activity, thus lowering the amount of free calcium in the blood. Gallium nitrate is also used to synthesize other gallium compounds.

Calcium perchlorate Chemical compound

Calcium perchlorate is classified as a metal perchlorate salt with the molecular formula Ca(ClO4)2. It is an inorganic compound that is a yellow-white crystalline solid in appearance. As a strong oxidizing agent, it reacts with reducing agents when heated to generate heat and products that may be gaseous (which will cause pressurization in closed containers). Calcium perchlorate has been categorized as having explosive reactivity. Ca(ClO4)2 is a common chemical on the soil of planet Mars, counting for almost 1% of the Martian dust, by weight.

References

  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.