Lime

A versatile chemical derived from limestone. It exists as Quicklime (CaO) and Slaked Lime (Ca(OH)2).

Description of what it is like

• Quicklime: White, caustic lumps.
• Slaked Lime: White powder or putty.

Origin and where to find it

• Source: Limestone (Calcium Carbonate), chalk, or seashells.
• Process: Produced by heating limestone to high temperatures (~900°C).

Minimum processing required

1. Quarrying: Extract limestone.
2. Calcination: Burn in a kiln (Lime Kiln) to release CO2, creating Quicklime (CaO).
3. Slaking: Add water to Quicklime to create Slaked Lime (Ca(OH)2). DANGER: This reaction releases intense heat.

Tools needed to work on it

• Kiln: To reach high temperatures.
• Protective Gear: To prevent burns.
• Containers: For slaking and storage.

Common forms of use

• Mortar/Plaster: Mixed with sand and water.
• Agriculture: To neutralize acidic soil.
• Tanning: To remove hair from hides.
• Whitewash: Cheap paint/sealant.

Possible substitutes

• Cement: Modern alternative.
• Clay: For simple mortar (adobe).
• Gypsum: For plaster.

Limitations and common failures

• Carbonation: Slaked lime hardens by absorbing CO2 from air (slow process).
• Water: Quicklime reacts violently with water; must be stored dry.

Risks and safety

• Burns: Quicklime can cause severe thermal and chemical burns.
• Blindness: Contact with eyes is extremely dangerous.
• Explosion: If water hits stored quicklime in a confined space.

Related materials

• Limestone: The raw material.
• Chalk: Softer form of limestone.
• Mortar: The product.

Related inventions

• Kiln: Needed for calcination.
• Firing: The process of creating lime.