World Library  
Flag as Inappropriate
Email this Article

Strontium carbonate

Article Id: WHEBN0008324182
Reproduction Date:

Title: Strontium carbonate  
Author: World Heritage Encyclopedia
Language: English
Subject: Strontium iodide, Strontium, Strontium ruthenate, Strontium bromide, Calcium carbonate
Collection:
Publisher: World Heritage Encyclopedia
Publication
Date:
 

Strontium carbonate

Strontium carbonate
Identifiers
CAS number  YesY
PubChem
ChemSpider  YesY
UNII  YesY
EC number
RTECS number WK8305000
Jmol-3D images Image 1
Properties
Molecular formula SrCO3
Molar mass 147.63 g/mol
Appearance White or grey powder
hygroscopic
Odor Odorless
Density 3.74 g/cm3
Melting point 1494 ºC (decomp.)
Solubility in water 0.0011 g/100 mL (18 ºC)
0.065 g/100 mL (100 °C)
Refractive index (nD) 1.518
Structure
Crystal structure rhombic
Hazards
MSDS External MSDS data
EU Index Not listed
NFPA 704
0
1
0
Flash point Non-flammable
Related compounds
Other cations Magnesium carbonate
Calcium carbonate
Barium carbonate
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
 YesY   YesY/N?)

Strontium carbonate (SrCO3) is the carbonate salt of strontium that has the appearance of a white or grey powder. It occurs in nature as the mineral strontianite.

Chemical properties

Strontium carbonate is a white, odorless, tasteless powder. Being a carbonate, it is a weak base and therefore is reactive with acids. It is otherwise stable and safe to work with. It is practically insoluble in water (1 part in 100,000). The solubility is increased significantly if the water is saturated with carbon dioxide, to 1 part in 1,000. It is soluble in dilute acids.

Preparation

Other than the natural occurrence as a mineral, strontium carbonate is prepared synthetically in one of two manners. First of which is from naturally occurring celestine also known as strontium sulfate (SrSO4) or by using soluble strontium salts by the reaction in solution with a soluble carbonate salt (usually sodium or ammonium carbonates). For example if sodium carbonate was used in solution with strontium nitrate:

Sr(NO3)2 (aq) + Na2CO3 (aq) → SrCO3 (s) + 2 NaNO3 (aq).

Uses

Nitric acid reacts with strontium carbonate to form strontium nitrate.

The most common use is as an inexpensive colorant in fireworks. Strontium and its salts emit a brilliant red color in flame. Unlike other strontium salts, the carbonate salt is generally preferred because of its cost and the fact that it is not hygroscopic. Its ability to neutralize acid is also very helpful in pyrotechnics. Another similar application is in road flares.

Strontium carbonate is used for electronic applications. It is used for manufacturing CTV to absorb electrons resulting from the cathode.

It is used in the preparation of iridescent glass, luminous paints, strontium oxide or strontium salts and in refining sugar and certain drugs.

It is widely used in the ceramics industry as an ingredient in glazes. It acts as a flux and also modifies the color of certain metallic oxides. It has some properties similar to barium carbonate.

It is also used in the manufacturing of strontium ferrites for permanent magnets which are used in Loudspeakers and door magnets.

Strontium carbonate is also used for making some superconductors such as BSCCO and also for electroluminescent materials where it is first calcined into SrO and then mixed with sulphur to make SrS:x where x is typically europium. This is the famous "blue/green" phosphor which is sensitive to frequency and changes from lime green to blue when run from 200Hz up to 1400Hz. Other dopants can also be used such as gallium, or yttrium to get a yellow/orange glow instead.

Because of its status as a weak Lewis base, strontium carbonate can be used to produce many different strontium compounds by simple use of the corresponding acid.

Microbial precipitation

The cyanobacteria, Calothrix, Synechococcus and Gloeocapsa, can precipitate strontian calcite in groundwater. The strontium exists as strontianite in solid solution within the host calcite with the strontium content of up to one percent.[1]

References

  1. ^ Henry Lutz Ehrlich; Dianne K Newman (2009). Geomicrobiology, Fifth Edition. CRC Press. p. 177. 

External links

  • [1] Reference page at CeramicMaterials.Info
  • International Chemical Safety Card 1695
This article was sourced from Creative Commons Attribution-ShareAlike License; additional terms may apply. World Heritage Encyclopedia content is assembled from numerous content providers, Open Access Publishing, and in compliance with The Fair Access to Science and Technology Research Act (FASTR), Wikimedia Foundation, Inc., Public Library of Science, The Encyclopedia of Life, Open Book Publishers (OBP), PubMed, U.S. National Library of Medicine, National Center for Biotechnology Information, U.S. National Library of Medicine, National Institutes of Health (NIH), U.S. Department of Health & Human Services, and USA.gov, which sources content from all federal, state, local, tribal, and territorial government publication portals (.gov, .mil, .edu). Funding for USA.gov and content contributors is made possible from the U.S. Congress, E-Government Act of 2002.
 
Crowd sourced content that is contributed to World Heritage Encyclopedia is peer reviewed and edited by our editorial staff to ensure quality scholarly research articles.
 
By using this site, you agree to the Terms of Use and Privacy Policy. World Heritage Encyclopedia™ is a registered trademark of the World Public Library Association, a non-profit organization.
 



Copyright © World Library Foundation. All rights reserved. eBooks from Hawaii eBook Library are sponsored by the World Library Foundation,
a 501c(4) Member's Support Non-Profit Organization, and is NOT affiliated with any governmental agency or department.