Barium chlorate

Barium chlorate

Names
IUPAC name Barium dichlorate
Other names Chloric acid, barium salt
Identifiers
CAS Number	13477-00-4 Y
3D model (Jmol)	Interactive image
ChemSpider	24273 Y
ECHA InfoCard	100.033.404
PubChem CID	26059
RTECS number	FN9770000
InChI InChI=1S/Ba.2ClHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2 Y Key: ISFLYIRWQDJPDR-UHFFFAOYSA-L Y InChI=1/Ba.2ClHO3/c;2*2-1(3)4/h;2*(H,2,3,4)/q+2;;/p-2 Key: ISFLYIRWQDJPDR-NUQVWONBAT
SMILES [Ba+2].[O-]Cl(=O)=O.[O-]Cl(=O)=O
Properties
Chemical formula	Ba(ClO3)2
Molar mass	304.23 g/mol
Appearance	white solid
Density	3.18 g/cm3, solid
Melting point	413.9 °C (777.0 °F; 687.0 K) (decomposes)
Solubility in water	27.5 g/100 ml (20 °C)
Magnetic susceptibility (χ)	-87.5·10−6 cm3/mol
Hazards
Safety data sheet	Barium Chlorate MSDS
EU classification (DSD) (outdated)	Oxidant (O) Harmful (Xn)
R-phrases (outdated)	R9, R20/22
S-phrases (outdated)	S13, S27
NFPA 704	0 3 3 OX
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Y  (what is YN ?)
Infobox references

Barium chlorate, Ba(ClO₃)₂, is a white crystalline solid, the barium salt of chloric acid. It is an irritant and toxic, as are all soluble barium compounds. It is sometimes used in pyrotechnics to produce a green color. It also finds use in the production of chloric acid.

Barium chlorate can be produced through a double replacement reaction between solutions of barium chloride and sodium chlorate:

On concentrating and chilling the resulting mixture, barium chlorate precipitates. This is perhaps the most common preparation, exploiting the lower solubility of barium chlorate compared to sodium chlorate.

The above method does result in some sodium contamination, which is undesirable for pyrotechnic purposes, where the strong yellow of sodium can easily overpower the green of barium. Sodium-free barium chlorate can be produced directly through electrolysis:

It can also be produced by the reaction of barium carbonate with boiling ammonium chlorate solution:

The reaction initially produces barium chlorate and ammonium carbonate; boiling the solution decomposes the ammonium carbonate and drives off the resulting ammonia and carbon dioxide, leaving only barium chlorate in solution.

When exposed to heat, barium chlorate alone will decompose to barium chloride and oxygen:

Barium chlorate is used to produce chloric acid, the formal precursor to all chlorate salts, through its reaction with dilute sulfuric acid, which results in a solution of chloric acid and insoluble barium sulfate precipitate:

Both the chlorate and the acid should be prepared as dilute solutions before mixing, such that the chloric acid produced is dilute, as concentrated solutions of chloric acid (above 30%) are unstable and prone to decompose, sometimes explosively.