Barium chlorate

Structural formula
General
Surname	Barium chlorate
other names	Barium chlorate Chlorate of barite
Molecular formula	Ba (ClO 3 ) 2
Brief description	colorless, odorless crystals or powder
External identifiers / databases
CAS number 13477-00-4 (anhydrous) 10294-38-9 (monohydrate) EC number 236-760-7 ECHA InfoCard 100.033.404 PubChem 26059 ChemSpider 24273 Wikidata Q412492
properties
Molar mass	304.24 g mol −1
Physical state	firmly
density	3.18 g cm −3
Melting point	Decomposition from 250 ° C
solubility	good in water (256 g l −1 at 20 ° C)
safety instructions
GHS hazard labeling from  Regulation (EC) No. 1272/2008 (CLP) , expanded if necessary danger H and P phrases H: 271-332-302-411 P: 210-220-221-261-264-270-271-273-280-283-301 + 312-304 + 340-306 + 360-312-330-370 + 378-371 + 380 + 375-391-501
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Barium chlorate is a barium salt of chloric acid . It has the formula Ba (ClO ₃ ) ₂ and belongs to the group of chlorates .

Extraction and presentation

It can be produced in the laboratory by electrolysis of a barium chloride solution . Part of the product crystallizes out due to its lower solubility.

It can also be obtained by reacting calcium chlorate or sodium chlorate with barium chloride.

${\displaystyle \mathrm {BaCl_{2}+2\ NaClO_{3}\longrightarrow Ba(ClO_{3})_{2}+2\ NaCl} }$

It is also possible to display it by reacting ammonium chlorate with barium carbonate

${\displaystyle \mathrm {2\ NH_{4}ClO_{3}+BaCO_{3}\longrightarrow Ba(ClO_{3})_{2}+2\ NH_{3}+H_{2}O+CO_{2}} }$

or by a Liebig process through the reaction of barium hydroxide with chlorine gas .

${\displaystyle \mathrm {6\ Ba(OH)_{2}+6\ Cl_{2}\longrightarrow 5\ BaCl_{2}+Ba(ClO_{3})_{2}+6\ H_{2}O} }$

The monohydrate is formed from solutions.

properties

Barium chlorate is a colorless powder that decomposes above 250 ° C.

${\displaystyle \mathrm {Ba(ClO_{3})_{2}\longrightarrow BaCl_{2}+3\ O_{2}} }$

It is a powerful oxidizer . Like all chlorates, this compound must be handled with care. The monohydrate releases its water of crystallization at 120 ° C, with release starting at 85 ° C.

The monohydrate has a monoclinic crystal structure with the space group C 2 / c (space group no. 15) . The anhydrate has an orthorhombic crystal structure which probably belongs to the space group Fd 2 d (No. 43, position 3) .

use

In the pyrotechnics barium chlorate is rarely used. Nowadays, barium nitrate is used to color the flame green , as preparations with barium chlorate can react violently to impact, impact and friction.

Barium chlorate is used relatively seldom today and is only produced in smaller quantities compared to potassium chlorate and sodium chlorate .

It is also used on a laboratory scale for the production of chloric acid and is also sometimes used for black printing.

Individual evidence

1. ↑ ^{a b c d e f} Entry on barium chlorate in the GESTIS substance database of the IFA , accessed on February 21, 2017(JavaScript required) .
2. ↑ Entry on barium chlorate in the Classification and Labeling Inventory of the European Chemicals Agency (ECHA), accessed on February 1, 2016. Manufacturers or distributors can expand the harmonized classification and labeling .
3. ↑ European regulations regarding Barium chlorate  ( page no longer available , search in web archives )  Info: The link was automatically marked as defective. Please check the link according to the instructions and then remove this notice.  
4. ↑ F. Haber: Grundriss der Technischen Elektrochemie On Theoretical Basis . 2016, ISBN 978-4-88695-269-1 , pp. 441 ( limited preview in Google Book search).
5. ↑ ^{a b c d} Heinrich Böttger, RJ Meyer: Chlor . Springer-Verlag, 2013, ISBN 978-3-662-11321-9 , pp. 337 ( limited preview in Google Book search).
6. ↑ ^{a b c} Richard C. Ropp: Encyclopedia of the Alkaline Earth Compounds . Newnes, 2012, ISBN 978-0-444-59553-9 , pp. 81 ( limited preview in Google Book search).
7. ↑ Michael S. Russell: The Chemistry of Fireworks . Royal Society of Chemistry, 2009, ISBN 978-0-85404-127-5 , pp. 110 ( limited preview in Google Book search).
8. ^ Takeo Shimizu: Selected Pyrotechnic Publications of Dr. Takeo Shimizu Part 3 Studies on Fireworks Colored Flame Compositions . Journal of Pyrotechnics, 1997, ISBN 1-889526-11-8 , pp. 78 ( limited preview in Google Book search).
9. ^ Egon Wiberg: Textbook of Inorganic Chemistry With an appendix: History of chemistry . Walter de Gruyter, 2011, ISBN 978-3-11-023832-7 , p. 124 ( limited preview in Google Book search).
10. ^ Rudolf Nietzki: Chemistry of organic dyes . Springer-Verlag, 2013, ISBN 978-3-662-36672-1 , pp. 170 ( limited preview in Google Book search).