Slaked lime is found to be extensively used in various industrial applications to perform a variety of functions. Primarily, it serves as an alkali (base) to elevate pH levels. The process of creating hydrated lime, also known as slaked lime, involves adding water to calcium oxide (CaO), or quicklime. This action triggers an exothermic reaction called slaking, resulting in the formation of calcium hydroxide (Ca(OH)2). Initially, calcium hydroxide is generated as a fine dry powder. Upon further water addition, a mixture of calcium hydroxide, commonly referred to as milk of lime, limewater, or lime slurry, is produced.
CaO + H2O → Ca(OH)2
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A few of the most significant properties of slaked lime/calcium hydroxide can be shown below.
| Chemical Formula | Ca(OH)2 |
|---|---|
| IUPAC name | Slaked Lime/Calcium Hydroxide |
| Molecular Weight/Molar Mass | 74.093 grams per mole |
| Density | 2.211 grams per cubic centimetre |
| Appearance | White powder or colorless crystal |
| Acid Insoluble As (SiO)2 | 0.20 ± 0.60 |
| Melting Point | 853 K |
Calcium hydroxide/Slaked Lime is typically made by reactions of Calcium oxide (CaO) with water (H 2O). The chemical reaction is exothermic meaning that an enormous amount of heat is produced.
CaO + H 2O + H 2O = Ca(OH) 2
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