Barium carbonate: Difference between revisions
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In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts ([[calcium sulfate]] and [[magnesium sulfate]]) that cause [[efflorescence]]. |
In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts ([[calcium sulfate]] and [[magnesium sulfate]]) that cause [[efflorescence]]. |
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Barium carbonate is also used to demonstrate the ([[Meissner Effect]]). Here's a step by step process: |
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1. The Meissner effect may be used in this hypothetical situation ([[Ray Romano]]) where barium carbonate is a [[source]] --> check out my sauce <https://www.woolworths.com.au/shop/productdetails/608712/masterfoods-reduced-salt-sugar-tomato-sauce> |
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2. You know how barium carbonate is used in D/C motors ye? It's the [[photoelectric effect]] |
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3. Finally, a [[magnetic field]] is expelled inside the other below [[critical temperature]] causing it to [[levitate]] <https://bayernstrikes.com/2017/10/03/bayern-munich-time-kingsley-coman-step/> |
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Got Him |
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==References== |
==References== |
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Revision as of 10:15, 29 May 2018
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| Names | |
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| Other names | |
| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.007.426 |
| EC Number |
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PubChem CID
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| RTECS number |
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| UNII | |
| UN number | 1564 |
CompTox Dashboard (EPA)
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| Properties | |
| BaCO3 | |
| Molar mass | 197.34 g/mol |
| Appearance | white crystals |
| Odor | odorless |
| Density | 4.286 g/cm3 |
| Melting point | 811 °C (1,492 °F; 1,084 K) polymorphic transformation |
| Boiling point | 1,450 °C (2,640 °F; 1,720 K) decomposes[1] from 1360 °C |
| 16 mg/L (8.8°C) 22 mg/L (18 °C) 24 mg/L (20 °C) 24 mg/L (24.2 °C)[1] | |
Solubility product (Ksp)
|
2.58·10−9 |
| Solubility | decomposes in acid insoluble in ethanol |
| -58.9·10−6 cm3/mol | |
Refractive index (nD)
|
1.676 |
| Thermochemistry | |
Heat capacity (C)
|
85.35 J/mol·K[1] |
Std molar
entropy (S⦵298) |
112 J/mol·K[2] |
Std enthalpy of
formation (ΔfH⦵298) |
-1219 kJ/mol[2] |
Gibbs free energy (ΔfG⦵)
|
-1139 kJ/mol[1] |
| Hazards | |
| GHS labelling: | |
 [3]
| |
| Warning | |
| H302[3] | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
|
418 mg/kg, oral (rat) |
| Safety data sheet (SDS) | ICSC 0777 |
| Related compounds | |
Other cations
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Magnesium carbonate Calcium carbonate Strontium carbonate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Barium carbonate (BaCO3), also known as witherite, is a chemical compound used in rat poison, bricks, ceramic glazes and cement.
Witherite
Witherite crystallizes in the orthorhombic system. The crystals are invariably twinned together in groups of three, giving rise to pseudo-hexagonal forms somewhat resembling bipyramidal crystals of quartz, the faces are usually rough and striated horizontally.[4] It transforms into an hexagonal phase at 1084 K that changes into a cubic phase at 1254 K.
The mineral is named after William Withering, who in 1784 recognized it to be chemically distinct from barytes.[5] It occurs in veins of lead ore at Hexham in Northumberland, Alston in Cumbria, Anglezarke, near Chorley in Lancashire and a few other localities. Witherite is readily altered to barium sulfate by the action of water containing calcium sulfate in solution and crystals are therefore frequently encrusted with barytes. It is the chief source of barium salts and is mined in considerable amounts in Northumberland. It is used for the preparation of rat poison, in the manufacture of glass and porcelain, and formerly for refining sugar.[4] It is also used for controlling the chromate to sulfate ratio in chromium electroplating baths.[6]
Preparation
Barium carbonate is made commercially from barium sulfide either by treatment with sodium carbonate at 60 to 70 °C (soda ash method) or by passing carbon dioxide at 40 to 90 °C.
In the soda ash process, solid or dissolved sodium carbonate is added to barium sulfide solution, and the barium carbonate precipitate is filtered, washed and dried.[7]
Reactions
Barium carbonate reacts with acids such as hydrochloric acid to form soluble barium salts, such as barium chloride:
- BaCO
3(s) + 2 HCl(aq) → BaCl
2(aq) + CO
2(g) + H
2O(l)
However, the reaction with sulfuric acid is poor, because barium sulfate is highly insoluble.
Uses
Barium carbonate is widely used in the ceramics industry as an ingredient in glazes. It acts as a flux, a matting and crystallizing agent and combines with certain colouring oxides to produce unique colours not easily attainable by other means. Its use is somewhat controversial since some claim that it can leach from glazes into food and drink. To provide a safe means of use, BaO is often used in fritted form.
In the brick, tile, earthenware and pottery industries barium carbonate is added to clays to precipitate soluble salts (calcium sulfate and magnesium sulfate) that cause efflorescence.
Barium carbonate is also used to demonstrate the (Meissner Effect). Here's a step by step process:
1. The Meissner effect may be used in this hypothetical situation (Ray Romano) where barium carbonate is a source --> check out my sauce <https://www.woolworths.com.au/shop/productdetails/608712/masterfoods-reduced-salt-sugar-tomato-sauce>
2. You know how barium carbonate is used in D/C motors ye? It's the photoelectric effect
3. Finally, a magnetic field is expelled inside the other below critical temperature causing it to levitate <https://bayernstrikes.com/2017/10/03/bayern-munich-time-kingsley-coman-step/>
Got Him
References
- ^ a b c d http://chemister.ru/Database/properties-en.php?dbid=1&id=377
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. ISBN 0-618-94690-X.
- ^ a b Sigma-Aldrich Co., Barium carbonate. Retrieved on 2014-05-06.
- ^ a b One or more of the preceding sentences incorporates text from a publication now in the public domain: Chisholm, Hugh, ed. (1911). "Witherite". Encyclopædia Britannica. Vol. 28 (11th ed.). Cambridge University Press. p. 759.
- ^ Withering, William (1784). "Experiments and Observations on Terra Poderosa". Philosophical Transactions of the Royal Society of London. 74: 293–311. doi:10.1098/rstl.1784.0024.
- ^ Whitelaw, G.P. (2003-10-25). "Standard Chrome Bath Control". finishing.com. Archived from the original on 13 December 2006. Retrieved 2006-11-29.
{{cite web}}: Cite has empty unknown parameter:|coauthors=(help); Unknown parameter|deadurl=ignored (|url-status=suggested) (help) - ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
External links
- ^ "Preparation and Characterization of Barium Carbonate Nanoparticles - Volume 2 Number 4 (Aug. 2011) - IJCEA". www.ijcea.org. Retrieved 2017-12-13.