Barium Chlorate

Barium Chlorate

The barium salt of chloric acid is barium chlorate, Ba(ClO3)2. It is a white crystalline solid that is irritant and toxic, as are all soluble barium compounds. It is occasionally used in pyrotechnics to create a green color. It is also used in the manufacture of chloric acid.

Sulfuric acid solutions that have been concentrated may cause fires or explosions. When combined with ammonium salt, it may spontaneously decompose and ignite. It is used in explosives and pyrotechnics, textile dyeing, and the production of other chlorates.


It appears as a white crystalline solid. It forms very flammable mixtures with combustible materials. Mixtures may be ignited by friction and may be explosive if the combustible material is finely divided.

  • 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)


  • Synthesis

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

BaCl2 + 2 NaClO3 → Ba(ClO3)2 + 2 NaCl

When the resulting mixture is concentrated and chilled, barium chlorate precipitates. This is probably the most common preparation, taking advantage of barium chlorate’s lower solubility when compared to sodium chlorate.

The above method does result in some sodium contamination, which is undesirable for pyrotechnic purposes because sodium’s strong yellow can easily overpower barium’s green. Electrolysis can be used to produce sodium-free barium chlorate:

BaCl2 + 6 H2O → Ba(ClO3)2 + 6 H2

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

2 NH4ClO3 + BaCO3 + Q → Ba(ClO3)2 + 2 NH3 + H2O + CO2

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.

The green seen in this firework is produced by barium chlorate and barium nitrate

  • Decomposition

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

Ba(ClO3)2 → BaCl2 + 3 O2

  • Chloric acid

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:

Ba(ClO3)2 + H2SO4 → 2 HClO3 + BaSO4

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.

Commercial uses

When barium chlorate is burned with a fuel, it emits a bright green light. Because it is an oxidizer, a chlorine donor, and contains a metal, this compound produces an unrivaled green color. However, because all chlorates are unstable to sulfur, acids, and ammonium ions, they have been banned from use in class C fireworks in the United States. As a result, an increasing number of fireworks manufacturers have begun to use more stable compounds such as barium nitrate and barium carbonate.

In pyrotechnics, barium chlorate is used to create a vivid green color. If you make it by double decomposition with barium chloride and sodium chlorate, it will be difficult to remove all of the sodium ion from the product, and the yellow color that sodium gives will interfere with the desired vivid green color.

Environmental Hazard

Barium chlorate is harmful to humans and the environment. If it is leached into bodies of water, it is extremely toxic to aquatic organisms. Although chemical spills of this compound are uncommon, they can harm entire ecosystems and should be avoided. This compound must be disposed of as hazardous waste. Barium chlorate is classified as hazardous by the Environmental Protection Agency (EPA).