Calcium Oxalate Precipitation (Kidney Stones)

CaCl2 + Na2C2O4 → CaC2O4↓ + 2NaCl

Overview

Calcium chloride reacts with sodium oxalate to form a white precipitate of calcium oxalate (Ksp = 2.3 × 10⁻⁹). Calcium oxalate is the primary component of approximately 80% of kidney stones. The monohydrate form (whewellite) is thermodynamically favored and forms the hardest, most painful stones.

Participants

Role Substance Coefficient State
Reactant Oxalic Acid C₂H₂O₄ 1 (aq)
Product Sodium Chloride NaCl 2 (aq)

Everyday Example

Most kidney stones are calcium oxalate crystals. Foods high in oxalate (spinach, rhubarb, almonds) can increase stone risk.

Industrial Importance

Understanding calcium oxalate precipitation is critical in nephrology, food science (oxalate content analysis), and in beer brewing (beer stone prevention).

Properties

Type
Precipitation
Reversible
No
Energy
Exothermic
ΔH
-12.0 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 Phosphate Precipitation (Bone Mineral) Calcium Sulfate Precipitation (Gypsum) Chromium(III) Hydroxide Precipitation Cobalt(II) Hydroxide Precipitation

Frequently Asked Questions

What is the equation for Calcium Oxalate Precipitation (Kidney Stones)?
The balanced equation is: CaCl₂ + Na₂C₂O₄ → CaC₂O₄↓ + 2NaCl.
What type of reaction is Calcium Oxalate Precipitation (Kidney Stones)?
Calcium Oxalate Precipitation (Kidney Stones) is a precipitation reaction.
Is Calcium Oxalate Precipitation (Kidney Stones) exothermic or endothermic?
Calcium Oxalate Precipitation (Kidney Stones) is exothermic (releases energy). The enthalpy change (ΔH) is -12.0 kJ/mol.