Strontium Sulfate Precipitation

SrCl2 + Na2SO4 → SrSO4↓ + 2NaCl

Overview

Strontium chloride reacts with sodium sulfate to form a white precipitate of strontium sulfate (Ksp = 3.4 × 10⁻⁷). SrSO₄ is moderately insoluble, less so than BaSO₄ but more than CaSO₄. The mineral form is celestine, the primary source of strontium.

Participants

Role Substance Coefficient State
Reactant Sodium Sulfate Na₂SO₄ 1 (aq)
Product Sodium Chloride NaCl 2 (aq)

Everyday Example

Strontium compounds give fireworks their characteristic red color. The element is named after Strontian, a village in Scotland.

Industrial Importance

Strontium sulfate (celestine) is mined as the primary source of strontium for fireworks, ceramic ferrite magnets, and zinc refining.

Properties

Type
Precipitation
Reversible
No
Energy
Exothermic
ΔH
-9.5 kJ/mol

Related Reactions

Aluminum Hydroxide Precipitation Barium Carbonate 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

Frequently Asked Questions

What is the equation for Strontium Sulfate Precipitation?
The balanced equation is: SrCl₂ + Na₂SO₄ → SrSO₄↓ + 2NaCl.
What type of reaction is Strontium Sulfate Precipitation?
Strontium Sulfate Precipitation is a precipitation reaction.
Is Strontium Sulfate Precipitation exothermic or endothermic?
Strontium Sulfate Precipitation is exothermic (releases energy). The enthalpy change (ΔH) is -9.5 kJ/mol.