Calcium Hydroxide

Calcium Hydroxide

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  • Calcium dihydroxide
  • 2522.20.00
  • Ca(OH)2
  • White granules/powder
  • 1305-62-0
  • Slaked lime; Hydrated lime; Calcium dihydroxide; Calcium (II) hydroxide
  • 5KGS/BAG
    20-26TONS / 20' GP
Grade Origin Download


Brief Overview


Calcium oxide does not occur naturally since it reacts readily with water (to form hydrated lime) and carbon dioxide to form limestone. This is an exothermic reaction which releases a lot of heat and thus caution must be taken. Calcium oxide vary in the degree of crystallization and cohesion of the crystalline mass and the homogeneity of the matrix.


Manufacturing Process


Method 1: Calcium carbonate is reacted with hydrochloric acid to generate calcium chloride. After which, ammonia is added for neutralization and left to stand for precipitation to occur. The solution is then filtered and lastly, sodium bicarbonate is added to generate calcium carbonate precipitate.


Method 2: Calcium carbonate is heated to higher temperature to undergo thermal decomposition to form calcium oxide or burnt lime. Calcium oxide is then treated or slaked with water to produce calcium hydroxide on a commercial scale: CaO + H2O → Ca(OH)2. The calcium oxide is broken down into fine particles of calcium hydroxide in this hydration reaction and this occurs in a continuous hydrator. The particle sizes can be modified through milling to ensure consistent particle size.

Food Industry: Used to produce beverages like alcohol and soft drinks. And it’s also applied in preparation a traditional Swedish food called Lutefisk. Ca(OH)2 prevents fruits from ripening before they are shipped to grocery store.


Sewage treatment Industry: Used as a flocculant in water and sewage treatment.


Other Applications:


  • Used to produce ammonia gas by reacting it with ammonium chloride.


  • Used as an intermediate to produce sodium hydroxide in the paper industry.

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