In theory, electrolysis of hot calcium chloride solution will produce the chlorate salt,[citation needed] analogous to the process used for the manufacture of sodium chlorate. In practice, electrolysis is complicated by calcium hydroxide depositing on the cathode, preventing the flow of current.
Reactions
When concentrated solutions of calcium chlorate and potassium chloride are combined, potassium chlorate precipitates:[1][2]
Ca(ClO3)2 + 2 KCl → 2 KClO3 + CaCl2
This is the second step of the Liebig process for the manufacture of potassium chlorate.[2]
Solutions of calcium chlorate react with solutions of alkali carbonates to give a precipitate of calcium carbonate and the alkali chlorate in solution:
Ca(ClO3)2 + Na2CO3 → 2 NaClO3 + CaCO3
On strong heating, calcium chlorate decomposes to give oxygen and calcium chloride:
Contact with strong sulfuric acid can result in explosions[4] due to the instability of concentrated chloric acid. Contact with ammonium compounds can also cause violent decomposition due to the formation of unstable ammonium chlorate.[4]
Calcium chlorate is occasionally used in pyrotechnics,[citation needed] as an oxidizer and pink flame colorant. Its hygroscopic nature and incompatibility with other common pyrotechnic materials (such as sulfur) limit its utility in these applications.
^Ira Remsen, Charles August Rouillu (1883). "American Chemical Journal". 4: 309. Solution of pure calcium chlorate, treated by sulphuric acid, would of course give a solution of chloric acid{{cite journal}}: Cite journal requires |journal= (help)