Barium Carbonate Precipitation

BaCl₂ + Na₂CO₃ → BaCO₃↓ + 2NaCl

Overview

Barium chloride reacts with sodium carbonate to form a white precipitate of barium carbonate (Ksp = 2.6 × 10⁻⁹). BaCO₃ occurs naturally as the mineral witherite. It dissolves in dilute acids with effervescence, releasing CO₂.

Participants

Role	Substance	Coefficient	State
Reactant	Sodium Carbonate Na₂CO₃	1	(aq)
Product	Sodium Chloride NaCl	2	(aq)

Everyday Example

Barium carbonate is used in rat poison because its acid-solubility allows it to dissolve in stomach acid, releasing toxic barium ions.

Industrial Importance

BaCO₃ is used in brick and tile manufacturing to prevent white scum (efflorescence), in ceramic glazes, and as a precursor for other barium compounds.

Properties

Type: Precipitation
Reversible: No
Energy: Exothermic
ΔH: -17.0 kJ/mol

Related Reactions

Aluminum Hydroxide Precipitation Barium Sulfate Precipitation Cadmium Sulfide Precipitation (Yellow) Calcium Carbonate Precipitation Calcium Fluoride Precipitation (Fluorite) Calcium Oxalate Precipitation (Kidney Stones) Calcium Phosphate Precipitation (Bone Mineral) Calcium Sulfate Precipitation (Gypsum) Chromium(III) Hydroxide Precipitation Cobalt(II) Hydroxide Precipitation

Frequently Asked Questions

What is the equation for Barium Carbonate Precipitation?

The balanced equation is: BaCl₂ + Na₂CO₃ → BaCO₃↓ + 2NaCl.

What type of reaction is Barium Carbonate Precipitation?

Barium Carbonate Precipitation is a precipitation reaction.

Is Barium Carbonate Precipitation exothermic or endothermic?

Barium Carbonate Precipitation is exothermic (releases energy). The enthalpy change (ΔH) is -17.0 kJ/mol.